Chemistry (9701) | A2 Level ONLY Not AS | Full-Scale Course
This Full-Scale course offers a complete online class for both the covering of the syllabus and the preparation for the examination. The Full-Scale Course is a tentative 2-4 months course, where the prime goal is to train a student from scratch …
Overview
This Full-Scale course offers a complete online class for both the covering of the syllabus and the preparation for the examination. The Full-Scale Course is a tentative 2-4 months course, where the prime goal is to train a student from scratch to learn everything that they need to know for the examination. We incorporate a sophisticated strategy to target all the subject areas that are required to get the best grade possible. The A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) covers the complete syllabus of Chemistry (9701)- For A2 Level Only NOT AS. The course has been designed to help any student, no matter how much they have prepared for the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online). Students at all levels can benefit from the course. You are not required to buy any book to complement the course as it covers all that is required for a successful attempt at the subject. Also, being a A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online), the curriculum follows periodic content availability, just like a real classroom. However, the timing of the class does not matter: each student can take the class as per their own feasibility. Whenever new content is uploaded or is available, an announcement is made both on the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) page, and communicated via e-mail to the students so that they may stay informed. Also, you may join later as the course allows for backward compatibility. Thus, a student joining in week 3 has access to the materials of week 1 and week 2, as well as limited ability to submit the assignments of these weeks. The curriculum shall be updated as the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) progresses.
Ideally, the course contains:
- Complete lectures of Each Topic in A Unique Way
- Notes and Presentations
- Periodic Assignments with Proper Grading and Feedback
- Past Paper Based Quizzes
- Forum Access To Ask Any Question
- Complete availability of the Teacher.
- Best Resources and Guidelines
- Tip and Tricks for Paper Solution
- Paper Attempting Methodology for Best Grades
Join the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) now and get the best grades in upcoming examination.
What Educate A Change Expects From The Student For This Course?
Full Scale Courses on Educate A Change are designed specifically to study the syllabus in-depth and solve as many past papers as possible. Our expectation with such courses are as follows:
- The student may or may not be aware of the basic contents of the syllabus. Thus, these courses suit the students who are studying a syllabus for the first time.
- The student may or may not understand the basic paper solution pattern.
- The student’s expectation regarding A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) is to learn the complete syllabus, learn paper solving techniques and practice as many past papers as possible for the upcoming examination.
- The student needs a complete and in-depth understanding of the entire syllabus content.
- A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) is the student’s preferred method to get the best grade in their exams.
How Will The Course Progress?
The A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) has been designed to provide maximum flexibility to our students. Here is a breakup of how the course will progress in general. This division is subject to change based on the progression of the course:
- Once your A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) has been activated, a timer starts to run on each of the content areas reflected in the curriculum section. Mobile users may access this section by clicking on the cube shape above this description.
- The timer remains unique to each student. It defines the exact time when you will receive a new content.
- Generally, the Full Scale Courses have a weekly progression. This aspect means you will get new contents at different times during the week. Again, the timer shows you the exact time for the content to arrive in your portal.
- If there are any significant changes, you will be informed in the announcements section. Remember, the announcements section is listed above this description. Additionally, you may locate the announcements in your e-mail as well. Do not forget to check the junk/ spam folder regularly.
- We use the Facebook Group of Educate A Change to communicate different course related updates as well. You can join the group using the following link https://www.facebook.com/groups/AYLOTIEducation
- The timings for live classes, if any, are also coordinated using the announcements section and emails.
- There are specific classes in the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) called quizzes. These quizzes can be attempted at any point as you wish. There is no restriction as to when you have to attempt them. However, there is a restriction on the number of times you can access any quiz. Make sure you remain aware of those restrictions. They are mentioned at the start of the quiz.
- Additionally, there are assignments in the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) as well. These assignments are designed using the past paper contents mostly. Remember, the assignment will be marked exactly one week after your first submission by the instructor. In some assignments, you have more than 1 submission as well. In such cases, you have to make sure that we receive your second submission before 1 week passes since your first submission. Also, only one submission is marked by the instructor.
- You may attempt the assignment directly on the portal or you may attempt it on a piece of paper and attach pictures or PDF here on the portal. Both ways are completely acceptable. Emailing the assignment is not allowed. Similarly, you may not use social media to submit an assignment.
- The past paper discussion classes of AA Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) will focus on providing the detailed solution methods of past papers. Additionally, video discussion using recorded videos will be provided for the most important questions. Detailed points, techniques and information for each question are also included.
- The official course discussion board or FORUM is accessible to all the enrolled students. You may ask any question related to any class, quiz, past paper discussion or assignment etc. both in public and private on this forum. This forum is the official method to ask questions and get answers by your instructor. You can ask using written, audio, video or image questions. Additionally, you can quote different answers on the forum for further clarification as well.
What may NOT be expected from the course?
A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online) is a formal course, which makes it impossible for Educate A Change to make any adjustments for any specific students. Students must not expect the course to:
- Give the material before the time on your timer.
- Give all the material at once.
- Give more time for the material to be accessed than the course’s time.
- Give the material in any other form than mentioned in the course
- The course does NOT register or pay your fee for the official Cambridge examination
Additionally, you may NOT except the instructor
- To give you any personal mentoring outside the course in the same price.
- Answer questions and other issues you may have regarding the course on personal social media.
- Collaborate with you in any shape or form outside the mentioned methods of the A Level Chemistry Complete Course online / Full-Scale Course Online (A Level Chemistry 9701 Full Scale Course online / Complete Course online)
A reply or support in any of the above mentioned issues may NOT be expected.
Curriculum
- 21 Sections
- 926 Lessons
- 32 Weeks
Expand all sectionsCollapse all sections
- Sample ContentSample Notes, Videos, Quizzes, Cheat Sheets, Assignments and Much More For Pre-Purchase Consideration.4
- Course Related InformationImportant Information Related To The Courses, Live Classes, Zoom Links etc.3
- Notes + Written Material For Contents of The SyllabusNotes for Chapters + Written Resources Regarding The Content153
- 3.1Chemical Energetics: Lattice Energy And Born-haber Cycles: Define And Use The Terms: (A) Enthalpy Change Of Atomisation, Δhat (B) Lattice Energy, Δhlatt (The Change From Gas Phase Ions To Solid Lattice)
- 3.2Chemical Energetics: Lattice Energy And Born-haber Cycles: (A) Define And Use The Term First Electron Affinity, Ea (B) Explain The Factors Affecting The Electron Affinities Of Elements (C) Describe And Explain The Trends In The Electron Affinities Of The Group 16 And Group 17 Elements
- 3.3Chemical Energetics: Lattice Energy And Born-haber Cycles: Construct And Use Born–haber Cycles For Ionic Solids (Limited To +1 And +2 Cations, –1 And –2 Anions)
- 3.4Chemical Energetics: Lattice Energy And Born-haber Cycles: Carry Out Calculations Involving Born–haber Cycles
- 3.5Chemical Energetics: Lattice Energy And Born-haber Cycles: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of A Lattice Energy
- 3.6Chemical Energetics: Enthalpies Of Solution And Hydration: Define And Use The Term Enthalpy Change With Reference To Hydration, Δhhyd, And Solution, Δhsol
- 3.7Chemical Energetics: Enthalpies Of Solution And Hydration: Construct And Use An Energy Cycle Involving Enthalpy Change Of Solution, Lattice Energy And Enthalpy Change Of Hydration
- 3.8Chemical Energetics: Enthalpies Of Solution And Hydration: Carry Out Calculations Involving The Energy Cycles In 23.2.2
- 3.9Chemical Energetics: Enthalpies Of Solution And Hydration: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of An Enthalpy Change Of Hydration
- 3.10Chemical Energetics: Entropy Change, Δs: Define The Term Entropy, S, As The Number Of Possible Arrangements Of The Particles And Their Energy In A Given System
- 3.11Chemical Energetics: Entropy Change, Δs: Predict And Explain The Sign Of The Entropy Changes That Occur: (A) During A Change In State, E.g. Melting, Boiling And Dissolving (And Their Reverse) (B) During A Temperature Change (C) During A Reaction In Which There Is A Change In The Number Of Gaseous Molecules
- 3.12Chemical Energetics: Entropy Change, Δs: Calculate The Entropy Change For A Reaction, Δs, Given The Standard Entropies, S⦵ , Of The Reactants And Products, Δs⦵ = Σs⦵ (Products) – Σs⦵ (Reactants) (Use Of Δs⦵ = Δssurr + Δssys Is Not Required)
- 3.13Chemical Energetics: Gibbs Free Energy Change, Δg: State And Use The Gibbs Equation Δg⦵ = Δh⦵ – Tδs⦵
- 3.14Chemical Energetics: Gibbs Free Energy Change, Δg: Perform Calculations Using The Equation Δg⦵ = Δh⦵ – Tδs⦵
- 3.15Chemical Energetics: Gibbs Free Energy Change, Δg: State Whether A Reaction Or Process Will Be Feasible By Using The Sign Of Δg
- 3.16Chemical Energetics: Gibbs Free Energy Change, Δg: Predict The Effect Of Temperature Change On The Feasibility Of A Reaction, Given Standard Enthalpy And Entropy Changes
- 3.17Electrochemistry: Electrolysis: Predict The Identities Of Substances Liberated During Electrolysis From The State Of Electrolyte (Molten Or Aqueous), Position In The Redox Series (Electrode Potential) And Concentration
- 3.18Electrochemistry: Electrolysis: State And Apply The Relationship F = Le Between The Faraday Constant, F, The Avogadro Constant, L, And The Charge On The Electron, E
- 3.19Electrochemistry: Electrolysis: Calculate: (A) The Quantity Of Charge Passed During Electrolysis, Using Q = It (B) The Mass And/or Volume Of Substance Liberated During Electrolysis
- 3.20Electrochemistry: Electrolysis: Describe The Determination Of A Value Of The Avogadro Constant By An Electrolytic Method
- 3.21Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Define The Terms: (A) Standard Electrode (Reduction) Potential (B) Standard Cell Potential
- 3.22Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe The Standard Hydrogen Electrode
- 3.23Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe Methods Used To Measure The Standard Electrode Potentials Of: (A) Metals Or Non-metals In Contact With Their Ions In Aqueous Solution (B) Ions Of The Same Element In Different Oxidation States
- 3.24Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Calculate A Standard Cell Potential By Combining Two Standard Electrode Potentials
- 3.25Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use Standard Cell Potentials To: (A) Deduce The Polarity Of Each Electrode And Hence Explain/deduce The Direction Of Electron Flow In The External Circuit Of A Simple Cell (B) Predict The Feasibility Of A Reaction
- 3.26Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Deduce From E ⦵ Values The Relative Reactivity Of Elements, Compounds And Ions As Oxidising Agents Or As Reducing Agents
- 3.27Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Construct Redox Equations Using The Relevant Half-equations
- 3.28Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Predict Qualitatively How The Value Of An Electrode Potential, E, Varies With The Concentrations Of The Aqueous Ions
- 3.29Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use The Nernst Equation, E.g. E = E ⦵ + (0.059/z) Log [oxidised Species] [reduced Species] , To Predict Quantitatively How The Value Of An Electrode Potential Varies With The Concentrations Of The Aqueous Ions; Examples Include Cu2+(Aq) + 2e– ⇌ Cu(S), Fe3+(Aq) + E– ⇌ Fe2+(Aq)
- 3.30Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Understand And Use The Equation Δg⦵ = –ne ⦵ Cell F
- 3.31Equilibria: Acids And Bases: Understand And Use The Terms Conjugate Acid And Conjugate Base
- 3.32Equilibria: Acids And Bases: Define Conjugate Acid–base Pairs, Identifying Such Pairs In Reactions
- 3.33Equilibria: Acids And Bases: Define Mathematically The Terms Ph, Ka, Pka And Kw And Use Them In Calculations (Kb And The Equation Kw = Ka × Kb Will Not Be Tested)
- 3.34Equilibria: Acids And Bases: Calculate [h+ (Aq)] And Ph Values For: (A) Strong Acids (B) Strong Alkalis (C) Weak Acids
- 3.35Equilibria: Acids And Bases: (A) Define A Buffer Solution (B) Explain How A Buffer Solution Can Be Made (C) Explain How Buffer Solutions Control Ph; Use Chemical Equations In These Explanations (D) Describe And Explain The Uses Of Buffer Solutions, Including The Role Of Hco3 – In Controlling Ph In Blood
- 3.36Equilibria: Acids And Bases: Calculate The Ph Of Buffer Solutions, Given Appropriate Data
- 3.37Equilibria: Acids And Bases: Understand And Use The Term Solubility Product, Ksp
- 3.38Equilibria: Acids And Bases: Write An Expression For Ksp
- 3.39Equilibria: Acids And Bases: Calculate Ksp From Concentrations And Vice Versa
- 3.40Equilibria: Acids And Bases: (A) Understand And Use The Common Ion Effect To Explain The Different Solubility Of A Compound In A Solution Containing A Common Ion (B) Perform Calculations Using Ksp Values And Concentration Of A Common Ion
- 3.41Equilibria: Partition Coefficients: State What Is Meant By The Term Partition Coefficient, Kpc
- 3.42Equilibria: Partition Coefficients: Calculate And Use A Partition Coefficient For A System In Which The Solute Is In The Same Physical State In The Two Solvents
- 3.43Equilibria: Partition Coefficients: Understand The Factors Affecting The Numerical Value Of A Partition Coefficient In Terms Of The Polarities Of The Solute And The Solvents Used
- 3.44Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Explain And Use The Terms Rate Equation, Order Of Reaction, Overall Order Of Reaction, Rate Constant, Half-life, Rate-determining Step And Intermediate
- 3.45Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Understand And Use Rate Equations Of The Form Rate = K [a]m[b]n (For Which M And N Are 0, 1 Or 2) (B) Deduce The Order Of A Reaction From Concentration–time Graphs Or From Experimental Data Relating To The Initial Rates Method And Half-life Method (C) Interpret Experimental Data In Graphical Form, Including Concentration–time And Rate–concentration Graphs (D) Calculate An Initial Rate Using Concentration Data (E) Construct A Rate Equation
- 3.46Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Show Understanding That The Half-life Of A First-order Reaction Is Independent Of Concentration (B) Use The Half-life Of A First-order Reaction In Calculations
- 3.47Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Calculate The Numerical Value Of A Rate Constant, For Example By: (A) Using The Initial Rates And The Rate Equation (B) Using The Half-life, T ½ , And The Equation K = 0.693/t ½
- 3.48Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: For A Multi-step Reaction: (A) Suggest A Reaction Mechanism That Is Consistent With The Rate Equation And The Equation For The Overall Reaction (B) Predict The Order That Would Result From A Given Reaction Mechanism And Rate-determining Step (C) Deduce A Rate Equation Using A Given Reaction Mechanism And Rate-determining Step For A Given Reaction (D) Identify An Intermediate Or Catalyst From A Given Reaction Mechanism (E) Identify The Rate Determining Step From A Rate Equation And A Given Reaction Mechanism
- 3.49Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Describe Qualitatively The Effect Of Temperature Change On The Rate Constant And Hence The Rate Of A Reaction
- 3.50Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain That Catalysts Can Be Homogeneous Or Heterogeneous
- 3.51Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Heterogeneous Catalyst To Include Adsorption Of Reactants, Bond Weakening And Desorption Of Products, For Example: (A) Iron In The Haber Process (B) Palladium, Platinum And Rhodium In The Catalytic Removal Of Oxides Of Nitrogen From The Exhaust Gases Of Car Engines
- 3.52Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Homogeneous Catalyst By Being Used In One Step And Reformed In A Later Step, For Example: (A) Atmospheric Oxides Of Nitrogen In The Oxidation Of Atmospheric Sulfur Dioxide (B) Fe2+ Or Fe3+ In The I – /s2o8 2– Reaction
- 3.53Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Trend In The Thermal Stability Of The Nitrates And Carbonates Including The Effect Of Ionic Radius On The Polarisation Of The Large Anion
- 3.54Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Variation In Solubility And Of Enthalpy Change Of Solution, Δh⦵ Sol, Of The Hydroxides And Sulfates In Terms Of Relative Magnitudes Of The Enthalpy Change Of Hydration And The Lattice Energy
- 3.55Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Define A Transition Element As A D-block Element Which Forms One Or More Stable Ions With Incomplete D Orbitals
- 3.56Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Sketch The Shape Of A 3dxy Orbital And 3dz² Orbital
- 3.57Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Understand That Transition Elements Have The Following Properties: (A) They Have Variable Oxidation States (B) They Behave As Catalysts (C) They Form Complex Ions (D) They Form Coloured Compounds
- 3.58Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Have Variable Oxidation States In Terms Of The Similarity In Energy Of The 3d And The 4s Sub-shells
- 3.59Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Behave As Catalysts In Terms Of Having More Than One Stable Oxidation State, And Vacant D Orbitals That Are Energetically Accessible And Can Form Dative Bonds With Ligands
- 3.60Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Form Complex Ions In Terms Of Vacant D Orbitals That Are Energetically Accessible
- 3.61Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe And Explain The Reactions Of Transition Elements With Ligands To Form Complexes, Including The Complexes Of Copper(Ii) And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 3.62Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Ligand As A Species That Contains A Lone Pair Of Electrons That Forms A Dative Covalent Bond To A Central Metal Atom/ion
- 3.63Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Understand And Use The Terms: (A) Monodentate Ligand Including As Examples H2o, Nh3, Cl   – And Cn– (B) Bidentate Ligand Including As Examples 1,2-diaminoethane, En, H2nch2ch2nh2 And The Ethanedioate Ion, C2o4 2– (C) Polydentate Ligand Including As An Example Edta4–
- 3.64Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Complex As A Molecule Or Ion Formed By A Central Metal Atom/ion Surrounded By One Or More Ligands
- 3.65Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Geometry (Shape And Bond Angles) Of Transition Element Complexes Which Are Linear, Square Planar, Tetrahedral Or Octahedral
- 3.66Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Explain Qualitatively That Ligand Exchange Can Occur, Including The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 3.67Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Predict, Using E ⦵ Values, The Feasibility Of Redox Reactions Involving Transition Elements And Their Ions
- 3.68Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Reactions Of, And Perform Calculations Involving: (A) Mno4 – /c2o4 2– In Acid Solution Given Suitable Data (B) Mno4 – /fe2+ In Acid Solution Given Suitable Data (C) Cu2+ / I – Given Suitable Data
- 3.69Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Perform Calculations Involving Other Redox Systems Given Suitable Data
- 3.70Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Define And Use The Terms Degenerate And Non-degenerate D Orbitals
- 3.71Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe The Splitting Of Degenerate D Orbitals Into Two Non-degenerate Sets Of D Orbitals Of Higher Energy, And Use Of Δe In: (A) Octahedral Complexes, Two Higher And Three Lower D Orbitals (B) Tetrahedral Complexes, Three Higher And Two Lower D Orbitals
- 3.72Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Explain Why Transition Elements Form Coloured Compounds In Terms Of The Frequency Of Light Absorbed As An Electron Is Promoted Between Two Non-degenerate D Orbitals
- 3.73Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe, In Qualitative Terms, The Effects Of Different Ligands On Δe, Frequency Of Light Absorbed, And Hence The Complementary Colour That Is Observed
- 3.74Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Use The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions As Examples Of Ligand Exchange Affecting The Colour Observed
- 3.75Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Describe The Types Of Stereoisomerism Shown By Complexes, Including Those Associated With Bidentate Ligands: (A) Geometrical (Cis/trans) Isomerism, E.g. Square Planar Such As [pt(Nh₃)₂cl₂] And Octahedral Such As [co(Nh3) 4(H2o)2] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+ (B) Optical Isomerism, E.g. [ni(H2nch2ch2nh2) 3] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+
- 3.76Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Deduce The Overall Polarity Of Complexes Such As Those Described In 28.4.1(A) And 28.4.1(B)
- 3.77Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Define The Stability Constant, Kstab, Of A Complex As The Equilibrium Constant For The Formation Of The Complex Ion In A Solvent (From Its Constituent Ions Or Molecules)
- 3.78Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Write An Expression For A Kstab Of A Complex ([hâ‚‚o] Should Not Be Included)
- 3.79Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Use Kstab Expressions To Perform Calculations
- 3.80Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Describe And Explain Ligand Exchanges In Terms Of Kstab Values And Understand That A Large Kstab Is Due To The Formation Of A Stable Complex Ion
- 3.81Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Page 47 Contain A Functional Group Which Dictates Their Physical And Chemical Properties
- 3.82Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound
- 3.83Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules (Including Cyclic Compounds Containing A Single Ring Of Up To Six Carbon Atoms) With Functional Groups Detailed In The Table On Page 47, Up To Six Carbon Atoms (Six Plus Six For Esters And Amides, Straight Chains Only For Esters And Nitriles)
- 3.84Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aromatic Molecules With One Benzene Ring And One Or More Simple Substituents, For Example 3-nitrobenzoic Acid Or 2,4,6-tribromophenol
- 3.85Organic Chemistry: An Introduction To Organic Chemistry of A Level: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Electrophilic Substitution (B) Addition–elimination
- 3.86Organic Chemistry: An Introduction To Organic Chemistry of A Level: Shapes Of Aromatic Organic Molecules; Σ And ΠBonds: Describe And Explain The Shape Of Benzene And Other Aromatic Molecules, Including Sp² Hybridisation, In Terms Of Σ Bonds And A Delocalised ΠSystem
- 3.87Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand That Enantiomers Have Identical Physical And Chemical Properties Apart From Their Ability To Rotate Plane Polarised Light And Their Potential Biological Activity
- 3.88Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand And Use The Terms Optically Active And Racemic Mixture
- 3.89Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Describe The Effect On Plane Polarised Light Of The Two Optical Isomers Of A Single Substance
- 3.90Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Explain The Relevance Of Chirality To The Synthetic Preparation Of Drug Molecules Including: (A) The Potential Different Biological Activity Of The Two Enantiomers (B) The Need To Separate A Racemic Mixture Into Two Pure Enantiomers (C) The Use Of Chiral Catalysts To Produce A Single Pure Optical Isomer (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds And Nomenclature Such As Diastereoisomers Is Not Required.)
- 3.91Organic Chemistry: Hydrocarbons: Arenes: Describe The Chemistry Of Arenes As Exemplified By The Following Reactions Of Benzene And Methylbenzene: (A) Substitution Reactions With Cl₂ And With Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃, To Form Halogenoarenes (Aryl Halides) (B) Nitration With A Mixture Of Concentrated Hno₃ And Concentrated H₂so₄ At A Temperature Between 25°c And 60°c (C) Friedel–crafts Alkylation By Ch₃cl And Alcl₃ And Heat (D) Friedel–crafts Acylation By Ch₃cocl And Alcl₃ And Heat (E) Complete Oxidation Of The Side-chain Using Hot Alkaline Kmno₄ And Then Dilute Acid To Give A Benzoic Acid (F) Hydrogenation Of The Benzene Ring Using H₂ And Pt/ni Catalyst And Heat To Form A Cyclohexane Ring
- 3.92Organic Chemistry: Hydrocarbons: Arenes: Describe The Mechanism Of Electrophilic Substitution In Arenes: (A) As Exemplified By The Formation Of Nitrobenzene And Bromobenzene (B) With Regards To The Effect Of Delocalisation (Aromatic Stabilisation) Of Electrons In Arenes To Explain The Predomination Of Substitution Over Addition
- 3.93Organic Chemistry: Hydrocarbons: Arenes: Predict Whether Halogenation Will Occur In The Side-chain Or In The Aromatic Ring In Arenes Depending On Reaction Conditions
- 3.94Organic Chemistry: Hydrocarbons: Arenes: Describe That In The Electrophilic Substitution Of Arenes, Different Substituents Direct To Different Ring Positions (Limited To The Directing Effects Of –nh₂, –oh, –r, –no₂, –cooh And –cor)
- 3.95Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Recall The Reactions By Which Halogenoarenes Can Be Produced: Substitution Of An Arene With Cl₂ Or Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃ To Form A Halogenoarene, Exemplified By Benzene To Form Chlorobenzene And Methylbenzene To Form 2-chloromethylbenzene And 4-chloromethylbenzene
- 3.96Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Explain The Difference In Reactivity Between A Halogenoalkane And A Halogenoarene As Exemplified By Chloroethane And Chlorobenzene
- 3.97Organic Chemistry: Hydroxy Compounds: Alcohols: Describe The Reaction With Acyl Chlorides To Form Esters Using Ethyl Ethanoate
- 3.98Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Reactions (Reagents And Conditions) By Which Phenol Can Be Produced: (A) Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 3.99Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol:
- 3.100Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Chemistry Of Phenol, As Exemplified By The Following Reactions: (A) With Bases, For Example Naoh(Aq) To Produce Sodium Phenoxide (B) With Na(S) To Produce Sodium Phenoxide And H2(G) (C) In Naoh(Aq) With Diazonium Salts, To Give Azo Compounds (D) Nitration Of The Aromatic Ring With Dilute Hno₃(Aq) At Room Temperature To Give A Mixture Of 2-nitrophenol And 4-nitrophenol (E) Bromination Of The Aromatic Ring With Br₂(Aq) To Form 2,4,6-tribromophenol
- 3.101Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain The Acidity Of Phenol
- 3.102Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Describe And Explain The Relative Acidities Of Water, Phenol And Ethanol
- 3.103Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain Why The Reagents And Conditions For The Nitration And Bromination Of Phenol Are Different From Those For Benzene
- 3.104Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall That The Hydroxyl Group Of A Phenol Directs To The 2-, 4- And 6-positions
- 3.105Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Apply Knowledge Of The Reactions Of Phenol To Those Of Other Phenolic Compounds, E.g. Naphthol
- 3.106Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reaction By Which Benzoic Acid Can Be Produced: (A) Reaction Of An Alkylbenzene With Hot Alkaline Kmnoâ‚„ And Then Dilute Acid, Exemplified By Methylbenzene
- 3.107Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe The Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂ To Form Acyl Chlorides
- 3.108Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recognise That Some Carboxylic Acids Can Be Further Oxidised: (A) The Oxidation Of Methanoic Acid, Hcooh, With Fehling’s Reagent Or Tollens’ Reagent Or Acidified Kmno₄ Or Acidified K₂cr₂o₇ To Carbon Dioxide And Water (B) The Oxidation Of Ethanedioic Acid, Hooccooh, With Warm Acidified Kmno₄ To Carbon Dioxide
- 3.109Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Carboxylic Acids, Phenols And Alcohols
- 3.110Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Chlorine-substituted Carboxylic Acids
- 3.111Organic Chemistry: Carboxylic Acids And Derivatives: Esters: Recall The Reaction By Which Esters Can Be Produced: (A) Reaction Of Alcohols With Acyl Chlorides Using The Formation Of Ethyl Ethanoate And Phenyl Benzoate As Examples
- 3.112Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Recall The Reactions (Reagents And Conditions) By Which Acyl Chlorides Can Be Produced: (A) Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂
- 3.113Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Following Reactions Of Acyl Chlorides: (A) Hydrolysis On Addition Of Water At Room Temperature To Give The Carboxylic Acid And Hcl (B) Reaction With An Alcohol At Room Temperature To Produce An Ester And Hcl (C) Reaction With Phenol At Room Temperature To Produce An Ester And Hcl (D) Reaction With Ammonia At Room Temperature To Produce An Amide And Hcl (E) Reaction With A Primary Or Secondary Amine At Room Temperature To Produce An Amide And Hcl
- 3.114Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Addition–elimination Mechanism Of Acyl Chlorides In Reactions In 33.3.2(A)–(E)
- 3.115Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Explain The Relative Ease Of Hydrolysis Of Acyl Chlorides, Alkyl Chlorides And Halogenoarenes (Aryl Chlorides)
- 3.116Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Recall The Reactions (Reagents And Conditions) By Which Primary And Secondary Amines Are Produced: (A) Reaction Of Halogenoalkanes With Nh₃ In Ethanol Heated Under Pressure (B) Reaction Of Halogenoalkanes With Primary Amines In Ethanol, Heated In A Sealed Tube/under Pressure (C) The Reduction Of Amides With Lialh₄ (D) The Reduction Of Nitriles With Lialh₄ Or H₂/ni
- 3.117Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe The Condensation Reaction Of Ammonia Or An Amine With An Acyl Chloride At Room Temperature To Give An Amide
- 3.118Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe And Explain The Basicity Of Aqueous Solutions Of Amines
- 3.119Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe The Preparation Of Phenylamine Via The Nitration Of Benzene To Form Nitrobenzene Followed By Reduction With Hot Sn/concentrated Hcl Followed By Naoh(Aq)
- 3.120Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe: (A) The Reaction Of Phenylamine With Br₂(Aq) At Room Temperature (B) The Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 3.121Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe And Explain The Relative Basicities Of Aqueous Ammonia, Ethylamine And Phenylamine
- 3.122Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Recall The Following About Azo Compounds: (A) Describe The Coupling Of Benzenediazonium Chloride With Phenol In Naoh(Aq) To Form An Azo Compound (B) Identify The Azo Group (C) State That Azo Compounds Are Often Used As Dyes (D) That Other Azo Dyes Can Be Formed Via A Similar Route
- 3.123Organic Chemistry: Nitrogen Compounds: Amides: Recall The Reactions (Reagents And Conditions) By Which Amides Are Produced: (A) The Reaction Between Ammonia And An Acyl Chloride At Room Temperature (B) The Reaction Between A Primary Amine And An Acyl Chloride At Room Temperature
- 3.124Organic Chemistry: Nitrogen Compounds: Amides: Describe The Reactions Of Amides: (A) Hydrolysis With Aqueous Alkali Or Aqueous Acid (B) The Reduction Of The Co Group In Amides With Lialhâ‚„ To Form An Amine
- 3.125Organic Chemistry: Nitrogen Compounds: Amides: State And Explain Why Amides Are Much Weaker Bases Than Amines
- 3.126Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Acid/base Properties Of Amino Acids And The Formation Of Zwitterions, To Include The Isoelectric Point
- 3.127Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Formation Of Amide (Peptide) Bonds Between Amino Acids To Give Di- And Tripeptides
- 3.128Organic Chemistry: Nitrogen Compounds: Amino Acids: Interpret And Predict The Results Of Electrophoresis On Mixtures Of Amino Acids And Dipeptides At Varying Phs (The Assembling Of The Apparatus Will Not Be Tested)
- 3.129Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyesters: (A) The Reaction Between A Diol And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of A Hydroxycarboxylic Acid
- 3.130Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyamides: (A) The Reaction Between A Diamine And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of An Aminocarboxylic Acid (C) The Reaction Between Amino Acids
- 3.131Organic Chemistry: Polymerisation: Condensation Polymerisation: Deduce The Repeat Unit Of A Condensation Polymer Obtained From A Given Monomer Or Pair Of Monomers
- 3.132Organic Chemistry: Polymerisation: Condensation Polymerisation: Identify The Monomer(S) Present In A Given Section Of A Condensation Polymer Molecule
- 3.133Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Predict The Type Of Polymerisation Reaction For A Given Monomer Or Pair Of Monomers
- 3.134Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Deduce The Type Of Polymerisation Reaction Which Produces A Given Section Of A Polymer Molecule
- 3.135Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Poly(Alkenes) Are Chemically Inert And Can Therefore Be Difficult To Biodegrade
- 3.136Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Some Polymers Can Be Degraded By The Action Of Light
- 3.137Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Polyesters And Polyamides Are Biodegradable By Acidic And Alkaline Hydrolysis
- 3.138Organic Chemistry: Organic Synthesis: Organic Synthesis: For An Organic Molecule Containing Several Functional Groups: (A) Identify Organic Functional Groups Using The Reactions In The Syllabus (B) Predict Properties And Reactions
- 3.139Organic Chemistry: Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus
- 3.140Organic Chemistry: Organic Synthesis: Organic Synthesis: Analyse A Given Synthetic Route In Terms Of Type Of Reaction And Reagents Used For Each Step Of It, And Possible By-products Analysis
- 3.141Analytical Techniques: Thin-layer Chromatography: Describe And Understand The Terms (A) Stationary Phase, For Example Aluminium Oxide (On A Solid Support) (B) Mobile Phase; A Polar Or Non-polar Solvent (C) Rf Value (D) Solvent Front And Baseline
- 3.142Analytical Techniques: Thin-layer Chromatography: Interpret Rf Values
- 3.143Analytical Techniques: Thin-layer Chromatography: Explain The Differences In Rf Values In Terms Of Interaction With The Stationary Phase And Of Relative Solubility In The Mobile Phase
- 3.144Analytical Techniques: Gas/liquid Chromatography: Describe And Understand The Terms (A) Stationary Phase; A High Boiling Point Non-polar Liquid (On A Solid Support) (B) Mobile Phase; An Unreactive Gas (C) Retention Time
- 3.145Analytical Techniques: Gas/liquid Chromatography: Interpret Gas /liquid Chromatograms In Terms Of The Percentage Composition Of A Mixture
- 3.146Analytical Techniques: Gas/liquid Chromatography: Explain Retention Times In Terms Of Interaction With The Stationary Phase
- 3.147Analytical Techniques: Carbon-13 Nmr Spectroscopy: Analyse And Interpret A Carbon-13 Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of The Carbon Atoms Present (B) The Possible Structures For The Molecule
- 3.148Analytical Techniques: Carbon-13 Nmr Spectroscopy: Predict Or Explain The Number Of Peaks In A Carbon-13 Nmr Spectrum For A Given Molecule
- 3.149Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Analyse And Interpret A Proton (1 H) Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of Proton Present Using Chemical Shift Values (B) The Relative Numbers Of Each Type Of Proton Present From Relative Peak Areas (C) The Number Of Equivalent Protons On The Carbon Atom Adjacent To The One To Which The Given Proton Is Attached From The Splitting Pattern, Using The N + 1 Rule (Limited To Singlet, Doublet, Triplet, Quartet And Multiplet) (D) The Possible Structures For The Molecule
- 3.150Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Predict The Chemical Shifts And Splitting Patterns Of The Protons In A Given Molecule
- 3.151Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Use Of Tetramethylsilane, Tms, As The Standard For Chemical Shift Measurements
- 3.152Analytical Techniques: Proton (1 H) Nmr Spectroscopy: State The Need For Deuterated Solvents, E.g. Cdcl₃, When Obtaining A Proton Nmr Spectrum
- 3.153Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Identification Of O–h And N–h Protons By Proton Exchange Using D₂o
- Video Lectures For The ContentVideo Lectures Covering Course Content In Detail15
- 4.1Chemical Energetics
- 4.2Electrochemistry
- 4.3Equilibria
- 4.4Reaction Kinetics
- 4.5Group 2
- 4.6Chemistry of Transition Elements
- 4.7An Introduction To A Level Organic Chemistry
- 4.8Hydrocarbons
- 4.9Halogen Compounds
- 4.10Hydroxy Compounds
- 4.11Carboxylic Acids And Derivatives
- 4.12Nitrogen Compounds
- 4.13Polymerisation
- 4.14Organic Synthesis
- 4.15Analytical Techniques
- QuizzesShort Quizzes To Auto-Test Your Knowledge of The Syllabus15
- 5.1Chemical Energetics10 Minutes0 Questions
- 5.2Electrochemistry10 Minutes0 Questions
- 5.3Equilibria10 Minutes0 Questions
- 5.4Reaction Kinetics10 Minutes0 Questions
- 5.5Group 210 Minutes0 Questions
- 5.6Chemistry of Transition Elements10 Minutes0 Questions
- 5.7An Introduction To A Level Organic Chemistry10 Minutes0 Questions
- 5.8Hydrocarbons10 Minutes0 Questions
- 5.9Halogen Compounds10 Minutes0 Questions
- 5.10Hydroxy Compounds10 Minutes0 Questions
- 5.11Carboxylic Acids And Derivatives10 Minutes0 Questions
- 5.12Nitrogen Compounds10 Minutes0 Questions
- 5.13Polymerisation10 Minutes0 Questions
- 5.14Organic Synthesis10 Minutes0 Questions
- 5.15Analytical Techniques10 Minutes0 Questions
- Quizzes For PreparationQuizzes With Detailed Explained Answers And Common Mistakes Discussed In Detail152
- 6.1Chemical Energetics: Lattice Energy And Born-haber Cycles: Define And Use The Terms: (A) Enthalpy Change Of Atomisation, Δhat (B) Lattice Energy, Δhlatt (The Change From Gas Phase Ions To Solid Lattice)
- 6.2Chemical Energetics: Lattice Energy And Born-haber Cycles: (A) Define And Use The Term First Electron Affinity, Ea (B) Explain The Factors Affecting The Electron Affinities Of Elements (C) Describe And Explain The Trends In The Electron Affinities Of The Group 16 And Group 17 Elements
- 6.3Chemical Energetics: Lattice Energy And Born-haber Cycles: Construct And Use Born–haber Cycles For Ionic Solids (Limited To +1 And +2 Cations, –1 And –2 Anions)
- 6.4Chemical Energetics: Lattice Energy And Born-haber Cycles: Carry Out Calculations Involving Born–haber Cycles
- 6.5Chemical Energetics: Lattice Energy And Born-haber Cycles: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of A Lattice Energy
- 6.6Chemical Energetics: Enthalpies Of Solution And Hydration: Define And Use The Term Enthalpy Change With Reference To Hydration, Δhhyd, And Solution, Δhsol
- 6.7Chemical Energetics: Enthalpies Of Solution And Hydration: Construct And Use An Energy Cycle Involving Enthalpy Change Of Solution, Lattice Energy And Enthalpy Change Of Hydration
- 6.8Chemical Energetics: Enthalpies Of Solution And Hydration: Carry Out Calculations Involving The Energy Cycles In 23.2.2
- 6.9Chemical Energetics: Enthalpies Of Solution And Hydration: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of An Enthalpy Change Of Hydration
- 6.10Chemical Energetics: Entropy Change, Δs: Define The Term Entropy, S, As The Number Of Possible Arrangements Of The Particles And Their Energy In A Given System
- 6.11Chemical Energetics: Entropy Change, Δs: Predict And Explain The Sign Of The Entropy Changes That Occur: (A) During A Change In State, E.g. Melting, Boiling And Dissolving (And Their Reverse) (B) During A Temperature Change (C) During A Reaction In Which There Is A Change In The Number Of Gaseous Molecules
- 6.12Chemical Energetics: Entropy Change, Δs: Calculate The Entropy Change For A Reaction, Δs, Given The Standard Entropies, S⦵ , Of The Reactants And Products, Δs⦵ = Σs⦵ (Products) – Σs⦵ (Reactants) (Use Of Δs⦵ = Δssurr + Δssys Is Not Required)
- 6.13Chemical Energetics: Gibbs Free Energy Change, Δg: State And Use The Gibbs Equation Δg⦵ = Δh⦵ – Tδs⦵
- 6.14Chemical Energetics: Gibbs Free Energy Change, Δg: Perform Calculations Using The Equation Δg⦵ = Δh⦵ – Tδs⦵
- 6.15Chemical Energetics: Gibbs Free Energy Change, Δg: State Whether A Reaction Or Process Will Be Feasible By Using The Sign Of Δg
- 6.16Chemical Energetics: Gibbs Free Energy Change, Δg: Predict The Effect Of Temperature Change On The Feasibility Of A Reaction, Given Standard Enthalpy And Entropy Changes
- 6.17Electrochemistry: Electrolysis: Predict The Identities Of Substances Liberated During Electrolysis From The State Of Electrolyte (Molten Or Aqueous), Position In The Redox Series (Electrode Potential) And Concentration
- 6.18Electrochemistry: Electrolysis: State And Apply The Relationship F = Le Between The Faraday Constant, F, The Avogadro Constant, L, And The Charge On The Electron, E
- 6.19Electrochemistry: Electrolysis: Calculate: (A) The Quantity Of Charge Passed During Electrolysis, Using Q = It (B) The Mass And/or Volume Of Substance Liberated During Electrolysis
- 6.20Electrochemistry: Electrolysis: Describe The Determination Of A Value Of The Avogadro Constant By An Electrolytic Method
- 6.21Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Define The Terms: (A) Standard Electrode (Reduction) Potential (B) Standard Cell Potential
- 6.22Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe The Standard Hydrogen Electrode
- 6.23Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe Methods Used To Measure The Standard Electrode Potentials Of: (A) Metals Or Non-metals In Contact With Their Ions In Aqueous Solution (B) Ions Of The Same Element In Different Oxidation States
- 6.24Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Calculate A Standard Cell Potential By Combining Two Standard Electrode Potentials
- 6.25Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use Standard Cell Potentials To: (A) Deduce The Polarity Of Each Electrode And Hence Explain/deduce The Direction Of Electron Flow In The External Circuit Of A Simple Cell (B) Predict The Feasibility Of A Reaction
- 6.26Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Deduce From E ⦵ Values The Relative Reactivity Of Elements, Compounds And Ions As Oxidising Agents Or As Reducing Agents
- 6.27Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Construct Redox Equations Using The Relevant Half-equations
- 6.28Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Predict Qualitatively How The Value Of An Electrode Potential, E, Varies With The Concentrations Of The Aqueous Ions
- 6.29Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use The Nernst Equation, E.g. E = E ⦵ + (0.059/z) Log [oxidised Species] [reduced Species] , To Predict Quantitatively How The Value Of An Electrode Potential Varies With The Concentrations Of The Aqueous Ions; Examples Include Cu2+(Aq) + 2e– ⇌ Cu(S), Fe3+(Aq) + E– ⇌ Fe2+(Aq)
- 6.30Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Understand And Use The Equation Δg⦵ = –ne ⦵ Cell F
- 6.31Equilibria: Acids And Bases: Understand And Use The Terms Conjugate Acid And Conjugate Base
- 6.32Equilibria: Acids And Bases: Define Conjugate Acid–base Pairs, Identifying Such Pairs In Reactions
- 6.33Equilibria: Acids And Bases: Define Mathematically The Terms Ph, Ka, Pka And Kw And Use Them In Calculations (Kb And The Equation Kw = Ka × Kb Will Not Be Tested)
- 6.34Equilibria: Acids And Bases: Calculate [h+ (Aq)] And Ph Values For: (A) Strong Acids (B) Strong Alkalis (C) Weak Acids
- 6.35Equilibria: Acids And Bases: (A) Define A Buffer Solution (B) Explain How A Buffer Solution Can Be Made (C) Explain How Buffer Solutions Control Ph; Use Chemical Equations In These Explanations (D) Describe And Explain The Uses Of Buffer Solutions, Including The Role Of Hco3 – In Controlling Ph In Blood
- 6.36Equilibria: Acids And Bases: Calculate The Ph Of Buffer Solutions, Given Appropriate Data
- 6.37Equilibria: Acids And Bases: Understand And Use The Term Solubility Product, Ksp
- 6.38Equilibria: Acids And Bases: Write An Expression For Ksp
- 6.39Equilibria: Acids And Bases: Calculate Ksp From Concentrations And Vice Versa
- 6.40Equilibria: Acids And Bases: (A) Understand And Use The Common Ion Effect To Explain The Different Solubility Of A Compound In A Solution Containing A Common Ion (B) Perform Calculations Using Ksp Values And Concentration Of A Common Ion
- 6.41Equilibria: Partition Coefficients: State What Is Meant By The Term Partition Coefficient, Kpc
- 6.42Equilibria: Partition Coefficients: Calculate And Use A Partition Coefficient For A System In Which The Solute Is In The Same Physical State In The Two Solvents
- 6.43Equilibria: Partition Coefficients: Understand The Factors Affecting The Numerical Value Of A Partition Coefficient In Terms Of The Polarities Of The Solute And The Solvents Used
- 6.44Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Explain And Use The Terms Rate Equation, Order Of Reaction, Overall Order Of Reaction, Rate Constant, Half-life, Rate-determining Step And Intermediate
- 6.45Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Understand And Use Rate Equations Of The Form Rate = K [a]m[b]n (For Which M And N Are 0, 1 Or 2) (B) Deduce The Order Of A Reaction From Concentration–time Graphs Or From Experimental Data Relating To The Initial Rates Method And Half-life Method (C) Interpret Experimental Data In Graphical Form, Including Concentration–time And Rate–concentration Graphs (D) Calculate An Initial Rate Using Concentration Data (E) Construct A Rate Equation
- 6.46Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Show Understanding That The Half-life Of A First-order Reaction Is Independent Of Concentration (B) Use The Half-life Of A First-order Reaction In Calculations
- 6.47Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Calculate The Numerical Value Of A Rate Constant, For Example By: (A) Using The Initial Rates And The Rate Equation (B) Using The Half-life, T ½ , And The Equation K = 0.693/t ½
- 6.48Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: For A Multi-step Reaction: (A) Suggest A Reaction Mechanism That Is Consistent With The Rate Equation And The Equation For The Overall Reaction (B) Predict The Order That Would Result From A Given Reaction Mechanism And Rate-determining Step (C) Deduce A Rate Equation Using A Given Reaction Mechanism And Rate-determining Step For A Given Reaction (D) Identify An Intermediate Or Catalyst From A Given Reaction Mechanism (E) Identify The Rate Determining Step From A Rate Equation And A Given Reaction Mechanism
- 6.49Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Describe Qualitatively The Effect Of Temperature Change On The Rate Constant And Hence The Rate Of A Reaction
- 6.50Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain That Catalysts Can Be Homogeneous Or Heterogeneous
- 6.51Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Heterogeneous Catalyst To Include Adsorption Of Reactants, Bond Weakening And Desorption Of Products, For Example: (A) Iron In The Haber Process (B) Palladium, Platinum And Rhodium In The Catalytic Removal Of Oxides Of Nitrogen From The Exhaust Gases Of Car Engines
- 6.52Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Homogeneous Catalyst By Being Used In One Step And Reformed In A Later Step, For Example: (A) Atmospheric Oxides Of Nitrogen In The Oxidation Of Atmospheric Sulfur Dioxide (B) Fe2+ Or Fe3+ In The I – /s2o8 2– Reaction
- 6.53Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Trend In The Thermal Stability Of The Nitrates And Carbonates Including The Effect Of Ionic Radius On The Polarisation Of The Large Anion
- 6.54Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Variation In Solubility And Of Enthalpy Change Of Solution, Δh⦵ Sol, Of The Hydroxides And Sulfates In Terms Of Relative Magnitudes Of The Enthalpy Change Of Hydration And The Lattice Energy
- 6.55Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Define A Transition Element As A D-block Element Which Forms One Or More Stable Ions With Incomplete D Orbitals
- 6.56Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Sketch The Shape Of A 3dxy Orbital And 3dz² Orbital
- 6.57Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Understand That Transition Elements Have The Following Properties: (A) They Have Variable Oxidation States (B) They Behave As Catalysts (C) They Form Complex Ions (D) They Form Coloured Compounds
- 6.58Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Have Variable Oxidation States In Terms Of The Similarity In Energy Of The 3d And The 4s Sub-shells
- 6.59Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Behave As Catalysts In Terms Of Having More Than One Stable Oxidation State, And Vacant D Orbitals That Are Energetically Accessible And Can Form Dative Bonds With Ligands
- 6.60Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Form Complex Ions In Terms Of Vacant D Orbitals That Are Energetically Accessible
- 6.61Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe And Explain The Reactions Of Transition Elements With Ligands To Form Complexes, Including The Complexes Of Copper(Ii) And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 6.62Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Ligand As A Species That Contains A Lone Pair Of Electrons That Forms A Dative Covalent Bond To A Central Metal Atom/ion
- 6.63Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Understand And Use The Terms: (A) Monodentate Ligand Including As Examples H2o, Nh3, Cl   – And Cn– (B) Bidentate Ligand Including As Examples 1,2-diaminoethane, En, H2nch2ch2nh2 And The Ethanedioate Ion, C2o4 2– (C) Polydentate Ligand Including As An Example Edta4–
- 6.64Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Complex As A Molecule Or Ion Formed By A Central Metal Atom/ion Surrounded By One Or More Ligands
- 6.65Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Geometry (Shape And Bond Angles) Of Transition Element Complexes Which Are Linear, Square Planar, Tetrahedral Or Octahedral
- 6.66Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Explain Qualitatively That Ligand Exchange Can Occur, Including The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 6.67Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Predict, Using E ⦵ Values, The Feasibility Of Redox Reactions Involving Transition Elements And Their Ions
- 6.68Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Reactions Of, And Perform Calculations Involving: (A) Mno4 – /c2o4 2– In Acid Solution Given Suitable Data (B) Mno4 – /fe2+ In Acid Solution Given Suitable Data (C) Cu2+ / I – Given Suitable Data
- 6.69Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Perform Calculations Involving Other Redox Systems Given Suitable Data
- 6.70Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Define And Use The Terms Degenerate And Non-degenerate D Orbitals
- 6.71Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe The Splitting Of Degenerate D Orbitals Into Two Non-degenerate Sets Of D Orbitals Of Higher Energy, And Use Of Δe In: (A) Octahedral Complexes, Two Higher And Three Lower D Orbitals (B) Tetrahedral Complexes, Three Higher And Two Lower D Orbitals
- 6.72Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Explain Why Transition Elements Form Coloured Compounds In Terms Of The Frequency Of Light Absorbed As An Electron Is Promoted Between Two Non-degenerate D Orbitals
- 6.73Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe, In Qualitative Terms, The Effects Of Different Ligands On Δe, Frequency Of Light Absorbed, And Hence The Complementary Colour That Is Observed
- 6.74Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Use The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions As Examples Of Ligand Exchange Affecting The Colour Observed
- 6.75Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Describe The Types Of Stereoisomerism Shown By Complexes, Including Those Associated With Bidentate Ligands: (A) Geometrical (Cis/trans) Isomerism, E.g. Square Planar Such As [pt(Nh₃)₂cl₂] And Octahedral Such As [co(Nh3) 4(H2o)2] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+ (B) Optical Isomerism, E.g. [ni(H2nch2ch2nh2) 3] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+
- 6.76Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Deduce The Overall Polarity Of Complexes Such As Those Described In 28.4.1(A) And 28.4.1(B)
- 6.77Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Define The Stability Constant, Kstab, Of A Complex As The Equilibrium Constant For The Formation Of The Complex Ion In A Solvent (From Its Constituent Ions Or Molecules)
- 6.78Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Write An Expression For A Kstab Of A Complex ([hâ‚‚o] Should Not Be Included)
- 6.79Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Use Kstab Expressions To Perform Calculations
- 6.80Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Describe And Explain Ligand Exchanges In Terms Of Kstab Values And Understand That A Large Kstab Is Due To The Formation Of A Stable Complex Ion
- 6.81Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Page 47 Contain A Functional Group Which Dictates Their Physical And Chemical Properties
- 6.82Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound
- 6.83Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules (Including Cyclic Compounds Containing A Single Ring Of Up To Six Carbon Atoms) With Functional Groups Detailed In The Table On Page 47, Up To Six Carbon Atoms (Six Plus Six For Esters And Amides, Straight Chains Only For Esters And Nitriles)
- 6.84Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aromatic Molecules With One Benzene Ring And One Or More Simple Substituents, For Example 3-nitrobenzoic Acid Or 2,4,6-tribromophenol
- 6.85Organic Chemistry: An Introduction To Organic Chemistry of A Level: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Electrophilic Substitution (B) Addition–elimination
- 6.86Organic Chemistry: An Introduction To Organic Chemistry of A Level: Shapes Of Aromatic Organic Molecules; Σ And ΠBonds: Describe And Explain The Shape Of Benzene And Other Aromatic Molecules, Including Sp² Hybridisation, In Terms Of Σ Bonds And A Delocalised ΠSystem
- 6.87Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand That Enantiomers Have Identical Physical And Chemical Properties Apart From Their Ability To Rotate Plane Polarised Light And Their Potential Biological Activity
- 6.88Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand And Use The Terms Optically Active And Racemic Mixture
- 6.89Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Describe The Effect On Plane Polarised Light Of The Two Optical Isomers Of A Single Substance
- 6.90Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Explain The Relevance Of Chirality To The Synthetic Preparation Of Drug Molecules Including: (A) The Potential Different Biological Activity Of The Two Enantiomers (B) The Need To Separate A Racemic Mixture Into Two Pure Enantiomers (C) The Use Of Chiral Catalysts To Produce A Single Pure Optical Isomer (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds And Nomenclature Such As Diastereoisomers Is Not Required.)
- 6.91Organic Chemistry: Hydrocarbons: Arenes: Describe The Chemistry Of Arenes As Exemplified By The Following Reactions Of Benzene And Methylbenzene: (A) Substitution Reactions With Cl₂ And With Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃, To Form Halogenoarenes (Aryl Halides) (B) Nitration With A Mixture Of Concentrated Hno₃ And Concentrated H₂so₄ At A Temperature Between 25°c And 60°c (C) Friedel–crafts Alkylation By Ch₃cl And Alcl₃ And Heat (D) Friedel–crafts Acylation By Ch₃cocl And Alcl₃ And Heat (E) Complete Oxidation Of The Side-chain Using Hot Alkaline Kmno₄ And Then Dilute Acid To Give A Benzoic Acid (F) Hydrogenation Of The Benzene Ring Using H₂ And Pt/ni Catalyst And Heat To Form A Cyclohexane Ring
- 6.92Organic Chemistry: Hydrocarbons: Arenes: Describe The Mechanism Of Electrophilic Substitution In Arenes: (A) As Exemplified By The Formation Of Nitrobenzene And Bromobenzene (B) With Regards To The Effect Of Delocalisation (Aromatic Stabilisation) Of Electrons In Arenes To Explain The Predomination Of Substitution Over Addition
- 6.93Organic Chemistry: Hydrocarbons: Arenes: Predict Whether Halogenation Will Occur In The Side-chain Or In The Aromatic Ring In Arenes Depending On Reaction Conditions
- 6.94Organic Chemistry: Hydrocarbons: Arenes: Describe That In The Electrophilic Substitution Of Arenes, Different Substituents Direct To Different Ring Positions (Limited To The Directing Effects Of –nh₂, –oh, –r, –no₂, –cooh And –cor)
- 6.95Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Recall The Reactions By Which Halogenoarenes Can Be Produced: Substitution Of An Arene With Cl₂ Or Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃ To Form A Halogenoarene, Exemplified By Benzene To Form Chlorobenzene And Methylbenzene To Form 2-chloromethylbenzene And 4-chloromethylbenzene
- 6.96Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Explain The Difference In Reactivity Between A Halogenoalkane And A Halogenoarene As Exemplified By Chloroethane And Chlorobenzene
- 6.97Organic Chemistry: Hydroxy Compounds: Alcohols: Describe The Reaction With Acyl Chlorides To Form Esters Using Ethyl Ethanoate
- 6.98Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Reactions (Reagents And Conditions) By Which Phenol Can Be Produced: (A) Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 6.99Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol:
- 6.100Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Chemistry Of Phenol, As Exemplified By The Following Reactions: (A) With Bases, For Example Naoh(Aq) To Produce Sodium Phenoxide (B) With Na(S) To Produce Sodium Phenoxide And H2(G) (C) In Naoh(Aq) With Diazonium Salts, To Give Azo Compounds (D) Nitration Of The Aromatic Ring With Dilute Hno₃(Aq) At Room Temperature To Give A Mixture Of 2-nitrophenol And 4-nitrophenol (E) Bromination Of The Aromatic Ring With Br₂(Aq) To Form 2,4,6-tribromophenol
- 6.101Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain The Acidity Of Phenol
- 6.102Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Describe And Explain The Relative Acidities Of Water, Phenol And Ethanol
- 6.103Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain Why The Reagents And Conditions For The Nitration And Bromination Of Phenol Are Different From Those For Benzene
- 6.104Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall That The Hydroxyl Group Of A Phenol Directs To The 2-, 4- And 6-positions
- 6.105Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Apply Knowledge Of The Reactions Of Phenol To Those Of Other Phenolic Compounds, E.g. Naphthol
- 6.106Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reaction By Which Benzoic Acid Can Be Produced: (A) Reaction Of An Alkylbenzene With Hot Alkaline Kmnoâ‚„ And Then Dilute Acid, Exemplified By Methylbenzene
- 6.107Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe The Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂ To Form Acyl Chlorides
- 6.108Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recognise That Some Carboxylic Acids Can Be Further Oxidised: (A) The Oxidation Of Methanoic Acid, Hcooh, With Fehling’s Reagent Or Tollens’ Reagent Or Acidified Kmno₄ Or Acidified K₂cr₂o₇ To Carbon Dioxide And Water (B) The Oxidation Of Ethanedioic Acid, Hooccooh, With Warm Acidified Kmno₄ To Carbon Dioxide
- 6.109Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Carboxylic Acids, Phenols And Alcohols
- 6.110Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Chlorine-substituted Carboxylic Acids
- 6.111Organic Chemistry: Carboxylic Acids And Derivatives: Esters: Recall The Reaction By Which Esters Can Be Produced: (A) Reaction Of Alcohols With Acyl Chlorides Using The Formation Of Ethyl Ethanoate And Phenyl Benzoate As Examples
- 6.112Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Recall The Reactions (Reagents And Conditions) By Which Acyl Chlorides Can Be Produced: (A) Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂
- 6.113Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Following Reactions Of Acyl Chlorides: (A) Hydrolysis On Addition Of Water At Room Temperature To Give The Carboxylic Acid And Hcl (B) Reaction With An Alcohol At Room Temperature To Produce An Ester And Hcl (C) Reaction With Phenol At Room Temperature To Produce An Ester And Hcl (D) Reaction With Ammonia At Room Temperature To Produce An Amide And Hcl (E) Reaction With A Primary Or Secondary Amine At Room Temperature To Produce An Amide And Hcl
- 6.114Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Addition–elimination Mechanism Of Acyl Chlorides In Reactions In 33.3.2(A)–(E)
- 6.115Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Explain The Relative Ease Of Hydrolysis Of Acyl Chlorides, Alkyl Chlorides And Halogenoarenes (Aryl Chlorides)
- 6.116Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Recall The Reactions (Reagents And Conditions) By Which Primary And Secondary Amines Are Produced: (A) Reaction Of Halogenoalkanes With Nh₃ In Ethanol Heated Under Pressure (B) Reaction Of Halogenoalkanes With Primary Amines In Ethanol, Heated In A Sealed Tube/under Pressure (C) The Reduction Of Amides With Lialh₄ (D) The Reduction Of Nitriles With Lialh₄ Or H₂/ni
- 6.117Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe The Condensation Reaction Of Ammonia Or An Amine With An Acyl Chloride At Room Temperature To Give An Amide
- 6.118Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe And Explain The Basicity Of Aqueous Solutions Of Amines
- 6.119Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe The Preparation Of Phenylamine Via The Nitration Of Benzene To Form Nitrobenzene Followed By Reduction With Hot Sn/concentrated Hcl Followed By Naoh(Aq)
- 6.120Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe: (A) The Reaction Of Phenylamine With Br₂(Aq) At Room Temperature (B) The Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 6.121Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe And Explain The Relative Basicities Of Aqueous Ammonia, Ethylamine And Phenylamine
- 6.122Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Recall The Following About Azo Compounds: (A) Describe The Coupling Of Benzenediazonium Chloride With Phenol In Naoh(Aq) To Form An Azo Compound (B) Identify The Azo Group (C) State That Azo Compounds Are Often Used As Dyes (D) That Other Azo Dyes Can Be Formed Via A Similar Route
- 6.123Organic Chemistry: Nitrogen Compounds: Amides: Recall The Reactions (Reagents And Conditions) By Which Amides Are Produced: (A) The Reaction Between Ammonia And An Acyl Chloride At Room Temperature (B) The Reaction Between A Primary Amine And An Acyl Chloride At Room Temperature
- 6.124Organic Chemistry: Nitrogen Compounds: Amides: Describe The Reactions Of Amides: (A) Hydrolysis With Aqueous Alkali Or Aqueous Acid (B) The Reduction Of The Co Group In Amides With Lialhâ‚„ To Form An Amine
- 6.125Organic Chemistry: Nitrogen Compounds: Amides: State And Explain Why Amides Are Much Weaker Bases Than Amines
- 6.126Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Acid/base Properties Of Amino Acids And The Formation Of Zwitterions, To Include The Isoelectric Point
- 6.127Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Formation Of Amide (Peptide) Bonds Between Amino Acids To Give Di- And Tripeptides
- 6.128Organic Chemistry: Nitrogen Compounds: Amino Acids: Interpret And Predict The Results Of Electrophoresis On Mixtures Of Amino Acids And Dipeptides At Varying Phs (The Assembling Of The Apparatus Will Not Be Tested)
- 6.129Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyesters: (A) The Reaction Between A Diol And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of A Hydroxycarboxylic Acid
- 6.130Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyamides: (A) The Reaction Between A Diamine And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of An Aminocarboxylic Acid (C) The Reaction Between Amino Acids
- 6.131Organic Chemistry: Polymerisation: Condensation Polymerisation: Deduce The Repeat Unit Of A Condensation Polymer Obtained From A Given Monomer Or Pair Of Monomers
- 6.132Organic Chemistry: Polymerisation: Condensation Polymerisation: Identify The Monomer(S) Present In A Given Section Of A Condensation Polymer Molecule
- 6.133Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Predict The Type Of Polymerisation Reaction For A Given Monomer Or Pair Of Monomers
- 6.134Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Deduce The Type Of Polymerisation Reaction Which Produces A Given Section Of A Polymer Molecule
- 6.135Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Poly(Alkenes) Are Chemically Inert And Can Therefore Be Difficult To Biodegrade
- 6.136Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Some Polymers Can Be Degraded By The Action Of Light
- 6.137Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Polyesters And Polyamides Are Biodegradable By Acidic And Alkaline Hydrolysis
- 6.138Organic Chemistry: Organic Synthesis: Organic Synthesis: For An Organic Molecule Containing Several Functional Groups: (A) Identify Organic Functional Groups Using The Reactions In The Syllabus (B) Predict Properties And Reactions
- 6.139Organic Chemistry: Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus
- 6.140Organic Chemistry: Organic Synthesis: Organic Synthesis: Analyse A Given Synthetic Route In Terms Of Type Of Reaction And Reagents Used For Each Step Of It, And Possible By-products Analysis
- 6.141Analytical Techniques: Thin-layer Chromatography: Describe And Understand The Terms (A) Stationary Phase, For Example Aluminium Oxide (On A Solid Support) (B) Mobile Phase; A Polar Or Non-polar Solvent (C) Rf Value (D) Solvent Front And Baseline
- 6.142Analytical Techniques: Thin-layer Chromatography: Interpret Rf Values
- 6.143Analytical Techniques: Thin-layer Chromatography: Explain The Differences In Rf Values In Terms Of Interaction With The Stationary Phase And Of Relative Solubility In The Mobile Phase
- 6.144Analytical Techniques: Gas/liquid Chromatography: Describe And Understand The Terms (A) Stationary Phase; A High Boiling Point Non-polar Liquid (On A Solid Support) (B) Mobile Phase; An Unreactive Gas (C) Retention Time
- 6.145Analytical Techniques: Gas/liquid Chromatography: Interpret Gas /liquid Chromatograms In Terms Of The Percentage Composition Of A Mixture
- 6.146Analytical Techniques: Gas/liquid Chromatography: Explain Retention Times In Terms Of Interaction With The Stationary Phase
- 6.147Analytical Techniques: Carbon-13 Nmr Spectroscopy: Analyse And Interpret A Carbon-13 Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of The Carbon Atoms Present (B) The Possible Structures For The Molecule
- 6.148Analytical Techniques: Carbon-13 Nmr Spectroscopy: Predict Or Explain The Number Of Peaks In A Carbon-13 Nmr Spectrum For A Given Molecule
- 6.149Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Analyse And Interpret A Proton (1 H) Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of Proton Present Using Chemical Shift Values (B) The Relative Numbers Of Each Type Of Proton Present From Relative Peak Areas (C) The Number Of Equivalent Protons On The Carbon Atom Adjacent To The One To Which The Given Proton Is Attached From The Splitting Pattern, Using The N + 1 Rule (Limited To Singlet, Doublet, Triplet, Quartet And Multiplet) (D) The Possible Structures For The Molecule
- 6.150Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Use Of Tetramethylsilane, Tms, As The Standard For Chemical Shift Measurements
- 6.151Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Identification Of O–h And N–h Protons By Proton Exchange Using D₂o
- 6.152Analytical Techniques: Proton (1 H) Nmr Spectroscopy: State The Need For Deuterated Solvents, E.g. Cdcl₃, When Obtaining A Proton Nmr Spectrum
- AssignmentsDetailed Assignments For Syllabus Preparation (Including Past Paper Questions)14
- 7.1Chemical Energetics3 Days
- 7.2Electrochemistry3 Days
- 7.3Equilibria3 Days
- 7.4Reaction Kinetics3 Days
- 7.5Group 23 Days
- 7.6An Introduction To A Level Organic Chemistry3 Days
- 7.7Hydrocarbons3 Days
- 7.8Halogen Compounds3 Days
- 7.9Hydroxy Compounds3 Days
- 7.10Carboxylic Acids And Derivatives3 Days
- 7.11Nitrogen Compounds3 Days
- 7.12Polymerisation3 Days
- 7.13Organic Synthesis3 Days
- 7.14Analytical Techniques3 Days
- Paper Pattern/ Paper Preparation/ Techniques To Attempt The Paper/ Common Mistakes To AvoidDetailed Information Including Written + Video Material Regarding Paper Attempt / Preparation/ Techniques/ Common Mistakes To Avoid0
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- 10.54May June 2024 Paper 41
- 10.55May June 2024 Paper 42
- 10.56May June 2024 Paper 43
- 10.57May June 2024 Paper 51
- 10.58May June 2024 Paper 53
- 10.59Feb March 2024 Paper 52
- 10.60May June 2024 Paper 52
- 10.61Feb March 2024 Paper 42
- 10.62October November 2024 Paper 41
- 10.63October November 2024 Paper 42
- 10.64October November 2024 Paper 43
- 10.65October November 2024 Paper 51
- 10.66October November 2024 Paper 52
- 10.67October November 2024 Paper 53
- 10.68May June 2025 Paper 41
- 10.69May June 2025 Paper 42
- 10.70May June 2025 Paper 43
- 10.71May June 2025 Paper 51
- 10.72May June 2025 Paper 52
- 10.73May June 2025 Paper 53
- 10.74Feb March 2025 Paper 42
- 10.75Feb March 2025 Paper 52
- 10.76October November 2025 Paper 41
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- 10.79October November 2025 Paper 51
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- Notes (Rearranged Version)Notes Arranged In A Different Style For Preparation Ease14
- 11.1Chemical Energetics
- 11.2Electrochemistry
- 11.3Equilibria
- 11.4Reaction Kinetics
- 11.5Group 2
- 11.6Chemistry of Transition Elements
- 11.7Hydrocarbons
- 11.8Halogen Compounds
- 11.9Hydroxy Compounds
- 11.10Carboxylic Acids And Derivatives
- 11.11Nitrogen Compounds
- 11.12Polymerisation
- 11.13Organic Syntheis
- 11.14Analytical Techniques
- Videos Lectures (Pre-Recorded)Videos Recorded In A Different Style For Preparation Ease0
- PracticalContent For Practical/ Alternative To Practical Paper In Detail0
- Cheat SheetsShort, Quick Revision Cheat Sheets152
- 14.1Chemical Energetics: Lattice Energy And Born-haber Cycles: Define And Use The Terms: (A) Enthalpy Change Of Atomisation, Δhat (B) Lattice Energy, Δhlatt (The Change From Gas Phase Ions To Solid Lattice)0 Questions
- 14.2Chemical Energetics: Lattice Energy And Born-haber Cycles: (A) Define And Use The Term First Electron Affinity, Ea (B) Explain The Factors Affecting The Electron Affinities Of Elements (C) Describe And Explain The Trends In The Electron Affinities Of The Group 16 And Group 17 Elements
- 14.3Chemical Energetics: Lattice Energy And Born-haber Cycles: Construct And Use Born–haber Cycles For Ionic Solids (Limited To +1 And +2 Cations, –1 And –2 Anions)
- 14.4Chemical Energetics: Lattice Energy And Born-haber Cycles: Carry Out Calculations Involving Born–haber Cycles
- 14.5Chemical Energetics: Lattice Energy And Born-haber Cycles: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of A Lattice Energy
- 14.6Chemical Energetics: Enthalpies Of Solution And Hydration: Define And Use The Term Enthalpy Change With Reference To Hydration, Δhhyd, And Solution, Δhsol
- 14.7Chemical Energetics: Enthalpies Of Solution And Hydration: Construct And Use An Energy Cycle Involving Enthalpy Change Of Solution, Lattice Energy And Enthalpy Change Of Hydration
- 14.8Chemical Energetics: Enthalpies Of Solution And Hydration: Carry Out Calculations Involving The Energy Cycles In 23.2.2
- 14.9Chemical Energetics: Enthalpies Of Solution And Hydration: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of An Enthalpy Change Of Hydration
- 14.10Chemical Energetics: Entropy Change, Δs: Define The Term Entropy, S, As The Number Of Possible Arrangements Of The Particles And Their Energy In A Given System
- 14.11Chemical Energetics: Entropy Change, Δs: Predict And Explain The Sign Of The Entropy Changes That Occur: (A) During A Change In State, E.g. Melting, Boiling And Dissolving (And Their Reverse) (B) During A Temperature Change (C) During A Reaction In Which There Is A Change In The Number Of Gaseous Molecules
- 14.12Chemical Energetics: Entropy Change, Δs: Calculate The Entropy Change For A Reaction, Δs, Given The Standard Entropies, S⦵ , Of The Reactants And Products, Δs⦵ = Σs⦵ (Products) – Σs⦵ (Reactants) (Use Of Δs⦵ = Δssurr + Δssys Is Not Required)
- 14.13Chemical Energetics: Gibbs Free Energy Change, Δg: State And Use The Gibbs Equation Δg⦵ = Δh⦵ – Tδs⦵
- 14.14Chemical Energetics: Gibbs Free Energy Change, Δg: Perform Calculations Using The Equation Δg⦵ = Δh⦵ – Tδs⦵
- 14.15Chemical Energetics: Gibbs Free Energy Change, Δg: State Whether A Reaction Or Process Will Be Feasible By Using The Sign Of Δg
- 14.16Chemical Energetics: Gibbs Free Energy Change, Δg: Predict The Effect Of Temperature Change On The Feasibility Of A Reaction, Given Standard Enthalpy And Entropy Changes
- 14.17Electrochemistry: Electrolysis: Predict The Identities Of Substances Liberated During Electrolysis From The State Of Electrolyte (Molten Or Aqueous), Position In The Redox Series (Electrode Potential) And Concentration
- 14.18Electrochemistry: Electrolysis: State And Apply The Relationship F = Le Between The Faraday Constant, F, The Avogadro Constant, L, And The Charge On The Electron, E
- 14.19Electrochemistry: Electrolysis: Calculate: (A) The Quantity Of Charge Passed During Electrolysis, Using Q = It (B) The Mass And/or Volume Of Substance Liberated During Electrolysis
- 14.20Electrochemistry: Electrolysis: Describe The Determination Of A Value Of The Avogadro Constant By An Electrolytic Method
- 14.21Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Define The Terms: (A) Standard Electrode (Reduction) Potential (B) Standard Cell Potential
- 14.22Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe The Standard Hydrogen Electrode
- 14.23Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe Methods Used To Measure The Standard Electrode Potentials Of: (A) Metals Or Non-metals In Contact With Their Ions In Aqueous Solution (B) Ions Of The Same Element In Different Oxidation States
- 14.24Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Calculate A Standard Cell Potential By Combining Two Standard Electrode Potentials
- 14.25Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use Standard Cell Potentials To: (A) Deduce The Polarity Of Each Electrode And Hence Explain/deduce The Direction Of Electron Flow In The External Circuit Of A Simple Cell (B) Predict The Feasibility Of A Reaction
- 14.26Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Deduce From E ⦵ Values The Relative Reactivity Of Elements, Compounds And Ions As Oxidising Agents Or As Reducing Agents
- 14.27Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Construct Redox Equations Using The Relevant Half-equations
- 14.28Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Predict Qualitatively How The Value Of An Electrode Potential, E, Varies With The Concentrations Of The Aqueous Ions
- 14.29Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use The Nernst Equation, E.g. E = E ⦵ + (0.059/z) Log [oxidised Species] [reduced Species] , To Predict Quantitatively How The Value Of An Electrode Potential Varies With The Concentrations Of The Aqueous Ions; Examples Include Cu2+(Aq) + 2e– ⇌ Cu(S), Fe3+(Aq) + E– ⇌ Fe2+(Aq)
- 14.30Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Understand And Use The Equation Δg⦵ = –ne ⦵ Cell F
- 14.31Equilibria: Acids And Bases: Understand And Use The Terms Conjugate Acid And Conjugate Base
- 14.32Equilibria: Acids And Bases: Define Conjugate Acid–base Pairs, Identifying Such Pairs In Reactions
- 14.33Equilibria: Acids And Bases: Define Mathematically The Terms Ph, Ka, Pka And Kw And Use Them In Calculations (Kb And The Equation Kw = Ka × Kb Will Not Be Tested)
- 14.34Equilibria: Acids And Bases: Calculate [h+ (Aq)] And Ph Values For: (A) Strong Acids (B) Strong Alkalis (C) Weak Acids
- 14.35Equilibria: Acids And Bases: (A) Define A Buffer Solution (B) Explain How A Buffer Solution Can Be Made (C) Explain How Buffer Solutions Control Ph; Use Chemical Equations In These Explanations (D) Describe And Explain The Uses Of Buffer Solutions, Including The Role Of Hco3 – In Controlling Ph In Blood
- 14.36Equilibria: Acids And Bases: Calculate The Ph Of Buffer Solutions, Given Appropriate Data
- 14.37Equilibria: Acids And Bases: Understand And Use The Term Solubility Product, Ksp
- 14.38Equilibria: Acids And Bases: Write An Expression For Ksp
- 14.39Equilibria: Acids And Bases: Calculate Ksp From Concentrations And Vice Versa
- 14.40Equilibria: Acids And Bases: (A) Understand And Use The Common Ion Effect To Explain The Different Solubility Of A Compound In A Solution Containing A Common Ion (B) Perform Calculations Using Ksp Values And Concentration Of A Common Ion
- 14.41Equilibria: Partition Coefficients: State What Is Meant By The Term Partition Coefficient, Kpc
- 14.42Equilibria: Partition Coefficients: Calculate And Use A Partition Coefficient For A System In Which The Solute Is In The Same Physical State In The Two Solvents
- 14.43Equilibria: Partition Coefficients: Understand The Factors Affecting The Numerical Value Of A Partition Coefficient In Terms Of The Polarities Of The Solute And The Solvents Used
- 14.44Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Explain And Use The Terms Rate Equation, Order Of Reaction, Overall Order Of Reaction, Rate Constant, Half-life, Rate-determining Step And Intermediate
- 14.45Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Understand And Use Rate Equations Of The Form Rate = K [a]m[b]n (For Which M And N Are 0, 1 Or 2) (B) Deduce The Order Of A Reaction From Concentration–time Graphs Or From Experimental Data Relating To The Initial Rates Method And Half-life Method (C) Interpret Experimental Data In Graphical Form, Including Concentration–time And Rate–concentration Graphs (D) Calculate An Initial Rate Using Concentration Data (E) Construct A Rate Equation
- 14.46Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Show Understanding That The Half-life Of A First-order Reaction Is Independent Of Concentration (B) Use The Half-life Of A First-order Reaction In Calculations
- 14.47Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Calculate The Numerical Value Of A Rate Constant, For Example By: (A) Using The Initial Rates And The Rate Equation (B) Using The Half-life, T ½ , And The Equation K = 0.693/t ½
- 14.48Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: For A Multi-step Reaction: (A) Suggest A Reaction Mechanism That Is Consistent With The Rate Equation And The Equation For The Overall Reaction (B) Predict The Order That Would Result From A Given Reaction Mechanism And Rate-determining Step (C) Deduce A Rate Equation Using A Given Reaction Mechanism And Rate-determining Step For A Given Reaction (D) Identify An Intermediate Or Catalyst From A Given Reaction Mechanism (E) Identify The Rate Determining Step From A Rate Equation And A Given Reaction Mechanism
- 14.49Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Describe Qualitatively The Effect Of Temperature Change On The Rate Constant And Hence The Rate Of A Reaction
- 14.50Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain That Catalysts Can Be Homogeneous Or Heterogeneous
- 14.51Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Heterogeneous Catalyst To Include Adsorption Of Reactants, Bond Weakening And Desorption Of Products, For Example: (A) Iron In The Haber Process (B) Palladium, Platinum And Rhodium In The Catalytic Removal Of Oxides Of Nitrogen From The Exhaust Gases Of Car Engines
- 14.52Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Homogeneous Catalyst By Being Used In One Step And Reformed In A Later Step, For Example: (A) Atmospheric Oxides Of Nitrogen In The Oxidation Of Atmospheric Sulfur Dioxide (B) Fe2+ Or Fe3+ In The I – /s2o8 2– Reaction
- 14.53Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Trend In The Thermal Stability Of The Nitrates And Carbonates Including The Effect Of Ionic Radius On The Polarisation Of The Large Anion
- 14.54Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Variation In Solubility And Of Enthalpy Change Of Solution, Δh⦵ Sol, Of The Hydroxides And Sulfates In Terms Of Relative Magnitudes Of The Enthalpy Change Of Hydration And The Lattice Energy
- 14.55Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Define A Transition Element As A D-block Element Which Forms One Or More Stable Ions With Incomplete D Orbitals
- 14.56Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Sketch The Shape Of A 3dxy Orbital And 3dz² Orbital
- 14.57Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Understand That Transition Elements Have The Following Properties: (A) They Have Variable Oxidation States (B) They Behave As Catalysts (C) They Form Complex Ions (D) They Form Coloured Compounds
- 14.58Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Have Variable Oxidation States In Terms Of The Similarity In Energy Of The 3d And The 4s Sub-shells
- 14.59Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Behave As Catalysts In Terms Of Having More Than One Stable Oxidation State, And Vacant D Orbitals That Are Energetically Accessible And Can Form Dative Bonds With Ligands
- 14.60Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Form Complex Ions In Terms Of Vacant D Orbitals That Are Energetically Accessible
- 14.61Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe And Explain The Reactions Of Transition Elements With Ligands To Form Complexes, Including The Complexes Of Copper(Ii) And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 14.62Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Ligand As A Species That Contains A Lone Pair Of Electrons That Forms A Dative Covalent Bond To A Central Metal Atom/ion
- 14.63Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Understand And Use The Terms: (A) Monodentate Ligand Including As Examples H2o, Nh3, Cl   – And Cn– (B) Bidentate Ligand Including As Examples 1,2-diaminoethane, En, H2nch2ch2nh2 And The Ethanedioate Ion, C2o4 2– (C) Polydentate Ligand Including As An Example Edta4–
- 14.64Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Complex As A Molecule Or Ion Formed By A Central Metal Atom/ion Surrounded By One Or More Ligands
- 14.65Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Geometry (Shape And Bond Angles) Of Transition Element Complexes Which Are Linear, Square Planar, Tetrahedral Or Octahedral
- 14.66Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Explain Qualitatively That Ligand Exchange Can Occur, Including The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 14.67Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Predict, Using E ⦵ Values, The Feasibility Of Redox Reactions Involving Transition Elements And Their Ions
- 14.68Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Reactions Of, And Perform Calculations Involving: (A) Mno4 – /c2o4 2– In Acid Solution Given Suitable Data (B) Mno4 – /fe2+ In Acid Solution Given Suitable Data (C) Cu2+ / I – Given Suitable Data
- 14.69Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Perform Calculations Involving Other Redox Systems Given Suitable Data
- 14.70Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Define And Use The Terms Degenerate And Non-degenerate D Orbitals
- 14.71Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe The Splitting Of Degenerate D Orbitals Into Two Non-degenerate Sets Of D Orbitals Of Higher Energy, And Use Of Δe In: (A) Octahedral Complexes, Two Higher And Three Lower D Orbitals (B) Tetrahedral Complexes, Three Higher And Two Lower D Orbitals
- 14.72Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Explain Why Transition Elements Form Coloured Compounds In Terms Of The Frequency Of Light Absorbed As An Electron Is Promoted Between Two Non-degenerate D Orbitals
- 14.73Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe, In Qualitative Terms, The Effects Of Different Ligands On Δe, Frequency Of Light Absorbed, And Hence The Complementary Colour That Is Observed
- 14.74Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Use The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions As Examples Of Ligand Exchange Affecting The Colour Observed
- 14.75Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Describe The Types Of Stereoisomerism Shown By Complexes, Including Those Associated With Bidentate Ligands: (A) Geometrical (Cis/trans) Isomerism, E.g. Square Planar Such As [pt(Nh₃)₂cl₂] And Octahedral Such As [co(Nh3) 4(H2o)2] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+ (B) Optical Isomerism, E.g. [ni(H2nch2ch2nh2) 3] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+
- 14.76Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Deduce The Overall Polarity Of Complexes Such As Those Described In 28.4.1(A) And 28.4.1(B)
- 14.77Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Define The Stability Constant, Kstab, Of A Complex As The Equilibrium Constant For The Formation Of The Complex Ion In A Solvent (From Its Constituent Ions Or Molecules)
- 14.78Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Write An Expression For A Kstab Of A Complex ([hâ‚‚o] Should Not Be Included)
- 14.79Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Use Kstab Expressions To Perform Calculations
- 14.80Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Describe And Explain Ligand Exchanges In Terms Of Kstab Values And Understand That A Large Kstab Is Due To The Formation Of A Stable Complex Ion
- 14.81Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Page 47 Contain A Functional Group Which Dictates Their Physical And Chemical Properties
- 14.82Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound
- 14.83Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules (Including Cyclic Compounds Containing A Single Ring Of Up To Six Carbon Atoms) With Functional Groups Detailed In The Table On Page 47, Up To Six Carbon Atoms (Six Plus Six For Esters And Amides, Straight Chains Only For Esters And Nitriles)
- 14.84Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aromatic Molecules With One Benzene Ring And One Or More Simple Substituents, For Example 3-nitrobenzoic Acid Or 2,4,6-tribromophenol
- 14.85Organic Chemistry: An Introduction To Organic Chemistry of A Level: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Electrophilic Substitution (B) Addition–elimination
- 14.86Organic Chemistry: An Introduction To Organic Chemistry of A Level: Shapes Of Aromatic Organic Molecules; Σ And ΠBonds: Describe And Explain The Shape Of Benzene And Other Aromatic Molecules, Including Sp² Hybridisation, In Terms Of Σ Bonds And A Delocalised ΠSystem
- 14.87Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand That Enantiomers Have Identical Physical And Chemical Properties Apart From Their Ability To Rotate Plane Polarised Light And Their Potential Biological Activity
- 14.88Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand And Use The Terms Optically Active And Racemic Mixture
- 14.89Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Describe The Effect On Plane Polarised Light Of The Two Optical Isomers Of A Single Substance
- 14.90Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Explain The Relevance Of Chirality To The Synthetic Preparation Of Drug Molecules Including: (A) The Potential Different Biological Activity Of The Two Enantiomers (B) The Need To Separate A Racemic Mixture Into Two Pure Enantiomers (C) The Use Of Chiral Catalysts To Produce A Single Pure Optical Isomer (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds And Nomenclature Such As Diastereoisomers Is Not Required.)
- 14.91Organic Chemistry: Hydrocarbons: Arenes: Describe The Chemistry Of Arenes As Exemplified By The Following Reactions Of Benzene And Methylbenzene: (A) Substitution Reactions With Cl₂ And With Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃, To Form Halogenoarenes (Aryl Halides) (B) Nitration With A Mixture Of Concentrated Hno₃ And Concentrated H₂so₄ At A Temperature Between 25°c And 60°c (C) Friedel–crafts Alkylation By Ch₃cl And Alcl₃ And Heat (D) Friedel–crafts Acylation By Ch₃cocl And Alcl₃ And Heat (E) Complete Oxidation Of The Side-chain Using Hot Alkaline Kmno₄ And Then Dilute Acid To Give A Benzoic Acid (F) Hydrogenation Of The Benzene Ring Using H₂ And Pt/ni Catalyst And Heat To Form A Cyclohexane Ring
- 14.92Organic Chemistry: Hydrocarbons: Arenes: Describe The Mechanism Of Electrophilic Substitution In Arenes: (A) As Exemplified By The Formation Of Nitrobenzene And Bromobenzene (B) With Regards To The Effect Of Delocalisation (Aromatic Stabilisation) Of Electrons In Arenes To Explain The Predomination Of Substitution Over Addition
- 14.93Organic Chemistry: Hydrocarbons: Arenes: Predict Whether Halogenation Will Occur In The Side-chain Or In The Aromatic Ring In Arenes Depending On Reaction Conditions
- 14.94Organic Chemistry: Hydrocarbons: Arenes: Describe That In The Electrophilic Substitution Of Arenes, Different Substituents Direct To Different Ring Positions (Limited To The Directing Effects Of –nh₂, –oh, –r, –no₂, –cooh And –cor)
- 14.95Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Recall The Reactions By Which Halogenoarenes Can Be Produced: Substitution Of An Arene With Cl₂ Or Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃ To Form A Halogenoarene, Exemplified By Benzene To Form Chlorobenzene And Methylbenzene To Form 2-chloromethylbenzene And 4-chloromethylbenzene
- 14.96Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Explain The Difference In Reactivity Between A Halogenoalkane And A Halogenoarene As Exemplified By Chloroethane And Chlorobenzene
- 14.97Organic Chemistry: Hydroxy Compounds: Alcohols: Describe The Reaction With Acyl Chlorides To Form Esters Using Ethyl Ethanoate
- 14.98Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Reactions (Reagents And Conditions) By Which Phenol Can Be Produced: (A) Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 14.99Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol:
- 14.100Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Chemistry Of Phenol, As Exemplified By The Following Reactions: (A) With Bases, For Example Naoh(Aq) To Produce Sodium Phenoxide (B) With Na(S) To Produce Sodium Phenoxide And H2(G) (C) In Naoh(Aq) With Diazonium Salts, To Give Azo Compounds (D) Nitration Of The Aromatic Ring With Dilute Hno₃(Aq) At Room Temperature To Give A Mixture Of 2-nitrophenol And 4-nitrophenol (E) Bromination Of The Aromatic Ring With Br₂(Aq) To Form 2,4,6-tribromophenol
- 14.101Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain The Acidity Of Phenol
- 14.102Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Describe And Explain The Relative Acidities Of Water, Phenol And Ethanol
- 14.103Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain Why The Reagents And Conditions For The Nitration And Bromination Of Phenol Are Different From Those For Benzene
- 14.104Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall That The Hydroxyl Group Of A Phenol Directs To The 2-, 4- And 6-positions
- 14.105Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Apply Knowledge Of The Reactions Of Phenol To Those Of Other Phenolic Compounds, E.g. Naphthol
- 14.106Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reaction By Which Benzoic Acid Can Be Produced: (A) Reaction Of An Alkylbenzene With Hot Alkaline Kmnoâ‚„ And Then Dilute Acid, Exemplified By Methylbenzene
- 14.107Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe The Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂ To Form Acyl Chlorides
- 14.108Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recognise That Some Carboxylic Acids Can Be Further Oxidised: (A) The Oxidation Of Methanoic Acid, Hcooh, With Fehling’s Reagent Or Tollens’ Reagent Or Acidified Kmno₄ Or Acidified K₂cr₂o₇ To Carbon Dioxide And Water (B) The Oxidation Of Ethanedioic Acid, Hooccooh, With Warm Acidified Kmno₄ To Carbon Dioxide
- 14.109Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Carboxylic Acids, Phenols And Alcohols
- 14.110Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Chlorine-substituted Carboxylic Acids
- 14.111Organic Chemistry: Carboxylic Acids And Derivatives: Esters: Recall The Reaction By Which Esters Can Be Produced: (A) Reaction Of Alcohols With Acyl Chlorides Using The Formation Of Ethyl Ethanoate And Phenyl Benzoate As Examples
- 14.112Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Recall The Reactions (Reagents And Conditions) By Which Acyl Chlorides Can Be Produced: (A) Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂
- 14.113Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Following Reactions Of Acyl Chlorides: (A) Hydrolysis On Addition Of Water At Room Temperature To Give The Carboxylic Acid And Hcl (B) Reaction With An Alcohol At Room Temperature To Produce An Ester And Hcl (C) Reaction With Phenol At Room Temperature To Produce An Ester And Hcl (D) Reaction With Ammonia At Room Temperature To Produce An Amide And Hcl (E) Reaction With A Primary Or Secondary Amine At Room Temperature To Produce An Amide And Hcl
- 14.114Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Addition–elimination Mechanism Of Acyl Chlorides In Reactions In 33.3.2(A)–(E)
- 14.115Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Explain The Relative Ease Of Hydrolysis Of Acyl Chlorides, Alkyl Chlorides And Halogenoarenes (Aryl Chlorides)
- 14.116Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Recall The Reactions (Reagents And Conditions) By Which Primary And Secondary Amines Are Produced: (A) Reaction Of Halogenoalkanes With Nh₃ In Ethanol Heated Under Pressure (B) Reaction Of Halogenoalkanes With Primary Amines In Ethanol, Heated In A Sealed Tube/under Pressure (C) The Reduction Of Amides With Lialh₄ (D) The Reduction Of Nitriles With Lialh₄ Or H₂/ni
- 14.117Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe The Condensation Reaction Of Ammonia Or An Amine With An Acyl Chloride At Room Temperature To Give An Amide
- 14.118Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe And Explain The Basicity Of Aqueous Solutions Of Amines
- 14.119Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe The Preparation Of Phenylamine Via The Nitration Of Benzene To Form Nitrobenzene Followed By Reduction With Hot Sn/concentrated Hcl Followed By Naoh(Aq)
- 14.120Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe: (A) The Reaction Of Phenylamine With Br₂(Aq) At Room Temperature (B) The Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 14.121Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe And Explain The Relative Basicities Of Aqueous Ammonia, Ethylamine And Phenylamine
- 14.122Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Recall The Following About Azo Compounds: (A) Describe The Coupling Of Benzenediazonium Chloride With Phenol In Naoh(Aq) To Form An Azo Compound (B) Identify The Azo Group (C) State That Azo Compounds Are Often Used As Dyes (D) That Other Azo Dyes Can Be Formed Via A Similar Route
- 14.123Organic Chemistry: Nitrogen Compounds: Amides: Recall The Reactions (Reagents And Conditions) By Which Amides Are Produced: (A) The Reaction Between Ammonia And An Acyl Chloride At Room Temperature (B) The Reaction Between A Primary Amine And An Acyl Chloride At Room Temperature
- 14.124Organic Chemistry: Nitrogen Compounds: Amides: Describe The Reactions Of Amides: (A) Hydrolysis With Aqueous Alkali Or Aqueous Acid (B) The Reduction Of The Co Group In Amides With Lialhâ‚„ To Form An Amine
- 14.125Organic Chemistry: Nitrogen Compounds: Amides: State And Explain Why Amides Are Much Weaker Bases Than Amines
- 14.126Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Acid/base Properties Of Amino Acids And The Formation Of Zwitterions, To Include The Isoelectric Point
- 14.127Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Formation Of Amide (Peptide) Bonds Between Amino Acids To Give Di- And Tripeptides
- 14.128Organic Chemistry: Nitrogen Compounds: Amino Acids: Interpret And Predict The Results Of Electrophoresis On Mixtures Of Amino Acids And Dipeptides At Varying Phs (The Assembling Of The Apparatus Will Not Be Tested)
- 14.129Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyesters: (A) The Reaction Between A Diol And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of A Hydroxycarboxylic Acid
- 14.130Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyamides: (A) The Reaction Between A Diamine And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of An Aminocarboxylic Acid (C) The Reaction Between Amino Acids
- 14.131Organic Chemistry: Polymerisation: Condensation Polymerisation: Deduce The Repeat Unit Of A Condensation Polymer Obtained From A Given Monomer Or Pair Of Monomers
- 14.132Organic Chemistry: Polymerisation: Condensation Polymerisation: Identify The Monomer(S) Present In A Given Section Of A Condensation Polymer Molecule
- 14.133Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Predict The Type Of Polymerisation Reaction For A Given Monomer Or Pair Of Monomers
- 14.134Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Deduce The Type Of Polymerisation Reaction Which Produces A Given Section Of A Polymer Molecule
- 14.135Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Poly(Alkenes) Are Chemically Inert And Can Therefore Be Difficult To Biodegrade
- 14.136Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Some Polymers Can Be Degraded By The Action Of Light
- 14.137Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Polyesters And Polyamides Are Biodegradable By Acidic And Alkaline Hydrolysis
- 14.138Organic Chemistry: Organic Synthesis: Organic Synthesis: For An Organic Molecule Containing Several Functional Groups: (A) Identify Organic Functional Groups Using The Reactions In The Syllabus (B) Predict Properties And Reactions
- 14.139Organic Chemistry: Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus
- 14.140Organic Chemistry: Organic Synthesis: Organic Synthesis: Analyse A Given Synthetic Route In Terms Of Type Of Reaction And Reagents Used For Each Step Of It, And Possible By-products Analysis
- 14.141Analytical Techniques: Thin-layer Chromatography: Describe And Understand The Terms (A) Stationary Phase, For Example Aluminium Oxide (On A Solid Support) (B) Mobile Phase; A Polar Or Non-polar Solvent (C) Rf Value (D) Solvent Front And Baseline
- 14.142Analytical Techniques: Thin-layer Chromatography: Interpret Rf Values
- 14.143Analytical Techniques: Thin-layer Chromatography: Explain The Differences In Rf Values In Terms Of Interaction With The Stationary Phase And Of Relative Solubility In The Mobile Phase
- 14.144Analytical Techniques: Gas/liquid Chromatography: Describe And Understand The Terms (A) Stationary Phase; A High Boiling Point Non-polar Liquid (On A Solid Support) (B) Mobile Phase; An Unreactive Gas (C) Retention Time
- 14.145Analytical Techniques: Gas/liquid Chromatography: Interpret Gas /liquid Chromatograms In Terms Of The Percentage Composition Of A Mixture
- 14.146Analytical Techniques: Gas/liquid Chromatography: Explain Retention Times In Terms Of Interaction With The Stationary Phase
- 14.147Analytical Techniques: Carbon-13 Nmr Spectroscopy: Analyse And Interpret A Carbon-13 Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of The Carbon Atoms Present (B) The Possible Structures For The Molecule
- 14.148Analytical Techniques: Carbon-13 Nmr Spectroscopy: Predict Or Explain The Number Of Peaks In A Carbon-13 Nmr Spectrum For A Given Molecule
- 14.149Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Analyse And Interpret A Proton (1 H) Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of Proton Present Using Chemical Shift Values (B) The Relative Numbers Of Each Type Of Proton Present From Relative Peak Areas (C) The Number Of Equivalent Protons On The Carbon Atom Adjacent To The One To Which The Given Proton Is Attached From The Splitting Pattern, Using The N + 1 Rule (Limited To Singlet, Doublet, Triplet, Quartet And Multiplet) (D) The Possible Structures For The Molecule
- 14.150Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Use Of Tetramethylsilane, Tms, As The Standard For Chemical Shift Measurements
- 14.151Analytical Techniques: Proton (1 H) Nmr Spectroscopy: State The Need For Deuterated Solvents, E.g. Cdcl₃, When Obtaining A Proton Nmr Spectrum
- 14.152Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Identification Of O–h And N–h Protons By Proton Exchange Using D₂o
- Practice Questions/ Practice ExamsPractice Questions/ Exams Based Both On Actual Exam Pattern And On Topical Content To Boost Preparation And Improve Performance152
- 15.1Practice Questions: Chemical Energetics: Lattice Energy And Born-haber Cycles: Define And Use The Terms: (A) Enthalpy Change Of Atomisation, Δhat (B) Lattice Energy, Δhlatt (The Change From Gas Phase Ions To Solid Lattice)
- 15.2Practice Questions: Chemical Energetics: Lattice Energy And Born-haber Cycles: (A) Define And Use The Term First Electron Affinity, Ea (B) Explain The Factors Affecting The Electron Affinities Of Elements (C) Describe And Explain The Trends In The Electron Affinities Of The Group 16 And Group 17 Elements
- 15.3Practice Questions: Chemical Energetics: Lattice Energy And Born-haber Cycles: Construct And Use Born–haber Cycles For Ionic Solids (Limited To +1 And +2 Cations, –1 And –2 Anions)
- 15.4Practice Questions: Chemical Energetics: Lattice Energy And Born-haber Cycles: Carry Out Calculations Involving Born–haber Cycles
- 15.5Practice Questions: Chemical Energetics: Lattice Energy And Born-haber Cycles: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of A Lattice Energy
- 15.6Practice Questions: Chemical Energetics: Enthalpies Of Solution And Hydration: Define And Use The Term Enthalpy Change With Reference To Hydration, Δhhyd, And Solution, Δhsol
- 15.7Practice Questions: Chemical Energetics: Enthalpies Of Solution And Hydration: Construct And Use An Energy Cycle Involving Enthalpy Change Of Solution, Lattice Energy And Enthalpy Change Of Hydration
- 15.8Practice Questions: Chemical Energetics: Enthalpies Of Solution And Hydration: Carry Out Calculations Involving The Energy Cycles In 23.2.2
- 15.9Practice Questions: Chemical Energetics: Enthalpies Of Solution And Hydration: Explain, In Qualitative Terms, The Effect Of Ionic Charge And Of Ionic Radius On The Numerical Magnitude Of An Enthalpy Change Of Hydration
- 15.10Practice Questions: Chemical Energetics: Entropy Change, Δs: Define The Term Entropy, S, As The Number Of Possible Arrangements Of The Particles And Their Energy In A Given System
- 15.11Practice Questions: Chemical Energetics: Entropy Change, Δs: Predict And Explain The Sign Of The Entropy Changes That Occur: (A) During A Change In State, E.g. Melting, Boiling And Dissolving (And Their Reverse) (B) During A Temperature Change (C) During A Reaction In Which There Is A Change In The Number Of Gaseous Molecules
- 15.12Practice Questions: Chemical Energetics: Entropy Change, Δs: Calculate The Entropy Change For A Reaction, Δs, Given The Standard Entropies, S⦵ , Of The Reactants And Products, Δs⦵ = Σs⦵ (Products) – Σs⦵ (Reactants) (Use Of Δs⦵ = Δssurr + Δssys Is Not Required)
- 15.13Practice Questions: Chemical Energetics: Gibbs Free Energy Change, Δg: State And Use The Gibbs Equation Δg⦵ = Δh⦵ – Tδs⦵
- 15.14Practice Questions: Chemical Energetics: Gibbs Free Energy Change, Δg: Perform Calculations Using The Equation Δg⦵ = Δh⦵ – Tδs⦵
- 15.15Practice Questions: Chemical Energetics: Gibbs Free Energy Change, Δg: State Whether A Reaction Or Process Will Be Feasible By Using The Sign Of Δg
- 15.16Practice Questions: Chemical Energetics: Gibbs Free Energy Change, Δg: Predict The Effect Of Temperature Change On The Feasibility Of A Reaction, Given Standard Enthalpy And Entropy Changes
- 15.17Practice Questions: Electrochemistry: Electrolysis: Predict The Identities Of Substances Liberated During Electrolysis From The State Of Electrolyte (Molten Or Aqueous), Position In The Redox Series (Electrode Potential) And Concentration
- 15.18Practice Questions: Electrochemistry: Electrolysis: State And Apply The Relationship F = Le Between The Faraday Constant, F, The Avogadro Constant, L, And The Charge On The Electron, E
- 15.19Practice Questions: Electrochemistry: Electrolysis: Calculate: (A) The Quantity Of Charge Passed During Electrolysis, Using Q = It (B) The Mass And/or Volume Of Substance Liberated During Electrolysis
- 15.20Practice Questions: Electrochemistry: Electrolysis: Describe The Determination Of A Value Of The Avogadro Constant By An Electrolytic Method
- 15.21Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Define The Terms: (A) Standard Electrode (Reduction) Potential (B) Standard Cell Potential
- 15.22Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe The Standard Hydrogen Electrode
- 15.23Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Describe Methods Used To Measure The Standard Electrode Potentials Of: (A) Metals Or Non-metals In Contact With Their Ions In Aqueous Solution (B) Ions Of The Same Element In Different Oxidation States
- 15.24Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Calculate A Standard Cell Potential By Combining Two Standard Electrode Potentials
- 15.25Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use Standard Cell Potentials To: (A) Deduce The Polarity Of Each Electrode And Hence Explain/deduce The Direction Of Electron Flow In The External Circuit Of A Simple Cell (B) Predict The Feasibility Of A Reaction
- 15.26Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Deduce From E ⦵ Values The Relative Reactivity Of Elements, Compounds And Ions As Oxidising Agents Or As Reducing Agents
- 15.27Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Construct Redox Equations Using The Relevant Half-equations
- 15.28Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Predict Qualitatively How The Value Of An Electrode Potential, E, Varies With The Concentrations Of The Aqueous Ions
- 15.29Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Use The Nernst Equation, E.g. E = E ⦵ + (0.059/z) Log [oxidised Species] [reduced Species] , To Predict Quantitatively How The Value Of An Electrode Potential Varies With The Concentrations Of The Aqueous Ions; Examples Include Cu2+(Aq) + 2e– ⇌ Cu(S), Fe3+(Aq) + E– ⇌ Fe2+(Aq)
- 15.30Practice Questions: Electrochemistry: Standard Electrode Potentials E⦵ , Standard Cell Potentials E⦵ Cell And The Nernst Equation: Understand And Use The Equation Δg⦵ = –ne ⦵ Cell F
- 15.31Practice Questions: Equilibria: Acids And Bases: Understand And Use The Terms Conjugate Acid And Conjugate Base
- 15.32Practice Questions: Equilibria: Acids And Bases: Define Conjugate Acid–base Pairs, Identifying Such Pairs In Reactions
- 15.33Practice Questions: Equilibria: Acids And Bases: Define Mathematically The Terms Ph, Ka, Pka And Kw And Use Them In Calculations (Kb And The Equation Kw = Ka × Kb Will Not Be Tested)
- 15.34Practice Questions: Equilibria: Acids And Bases: Calculate [h+ (Aq)] And Ph Values For: (A) Strong Acids (B) Strong Alkalis (C) Weak Acids
- 15.35Practice Questions: Equilibria: Acids And Bases: (A) Define A Buffer Solution (B) Explain How A Buffer Solution Can Be Made (C) Explain How Buffer Solutions Control Ph; Use Chemical Equations In These Explanations (D) Describe And Explain The Uses Of Buffer Solutions, Including The Role Of Hco3 – In Controlling Ph In Blood
- 15.36Practice Questions: Equilibria: Acids And Bases: Calculate The Ph Of Buffer Solutions, Given Appropriate Data
- 15.37Practice Questions: Equilibria: Acids And Bases: Understand And Use The Term Solubility Product, Ksp
- 15.38Practice Questions: Equilibria: Acids And Bases: Write An Expression For Ksp
- 15.39Practice Questions: Equilibria: Acids And Bases: Calculate Ksp From Concentrations And Vice Versa
- 15.40Practice Questions: Equilibria: Acids And Bases: (A) Understand And Use The Common Ion Effect To Explain The Different Solubility Of A Compound In A Solution Containing A Common Ion (B) Perform Calculations Using Ksp Values And Concentration Of A Common Ion
- 15.41Practice Questions: Equilibria: Partition Coefficients: State What Is Meant By The Term Partition Coefficient, Kpc
- 15.42Practice Questions: Equilibria: Partition Coefficients: Calculate And Use A Partition Coefficient For A System In Which The Solute Is In The Same Physical State In The Two Solvents
- 15.43Practice Questions: Equilibria: Partition Coefficients: Understand The Factors Affecting The Numerical Value Of A Partition Coefficient In Terms Of The Polarities Of The Solute And The Solvents Used
- 15.44Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Explain And Use The Terms Rate Equation, Order Of Reaction, Overall Order Of Reaction, Rate Constant, Half-life, Rate-determining Step And Intermediate
- 15.45Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Understand And Use Rate Equations Of The Form Rate = K [a]m[b]n (For Which M And N Are 0, 1 Or 2) (B) Deduce The Order Of A Reaction From Concentration–time Graphs Or From Experimental Data Relating To The Initial Rates Method And Half-life Method (C) Interpret Experimental Data In Graphical Form, Including Concentration–time And Rate–concentration Graphs (D) Calculate An Initial Rate Using Concentration Data (E) Construct A Rate Equation
- 15.46Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: (A) Show Understanding That The Half-life Of A First-order Reaction Is Independent Of Concentration (B) Use The Half-life Of A First-order Reaction In Calculations
- 15.47Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Calculate The Numerical Value Of A Rate Constant, For Example By: (A) Using The Initial Rates And The Rate Equation (B) Using The Half-life, T ½ , And The Equation K = 0.693/t ½
- 15.48Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: For A Multi-step Reaction: (A) Suggest A Reaction Mechanism That Is Consistent With The Rate Equation And The Equation For The Overall Reaction (B) Predict The Order That Would Result From A Given Reaction Mechanism And Rate-determining Step (C) Deduce A Rate Equation Using A Given Reaction Mechanism And Rate-determining Step For A Given Reaction (D) Identify An Intermediate Or Catalyst From A Given Reaction Mechanism (E) Identify The Rate Determining Step From A Rate Equation And A Given Reaction Mechanism
- 15.49Practice Questions: Reaction Kinetics: Simple Rate Equations, Orders Of Reaction And Rate Constants: Describe Qualitatively The Effect Of Temperature Change On The Rate Constant And Hence The Rate Of A Reaction
- 15.50Practice Questions: Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain That Catalysts Can Be Homogeneous Or Heterogeneous
- 15.51Practice Questions: Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Heterogeneous Catalyst To Include Adsorption Of Reactants, Bond Weakening And Desorption Of Products, For Example: (A) Iron In The Haber Process (B) Palladium, Platinum And Rhodium In The Catalytic Removal Of Oxides Of Nitrogen From The Exhaust Gases Of Car Engines
- 15.52Practice Questions: Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Describe The Mode Of Action Of A Homogeneous Catalyst By Being Used In One Step And Reformed In A Later Step, For Example: (A) Atmospheric Oxides Of Nitrogen In The Oxidation Of Atmospheric Sulfur Dioxide (B) Fe2+ Or Fe3+ In The I – /s2o8 2– Reaction
- 15.53Practice Questions: Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Trend In The Thermal Stability Of The Nitrates And Carbonates Including The Effect Of Ionic Radius On The Polarisation Of The Large Anion
- 15.54Practice Questions: Inorganic Chemistry: Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe And Explain Qualitatively The Variation In Solubility And Of Enthalpy Change Of Solution, Δh⦵ Sol, Of The Hydroxides And Sulfates In Terms Of Relative Magnitudes Of The Enthalpy Change Of Hydration And The Lattice Energy
- 15.55Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Define A Transition Element As A D-block Element Which Forms One Or More Stable Ions With Incomplete D Orbitals
- 15.56Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Sketch The Shape Of A 3dxy Orbital And 3dz² Orbital
- 15.57Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Understand That Transition Elements Have The Following Properties: (A) They Have Variable Oxidation States (B) They Behave As Catalysts (C) They Form Complex Ions (D) They Form Coloured Compounds
- 15.58Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Have Variable Oxidation States In Terms Of The Similarity In Energy Of The 3d And The 4s Sub-shells
- 15.59Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Behave As Catalysts In Terms Of Having More Than One Stable Oxidation State, And Vacant D Orbitals That Are Energetically Accessible And Can Form Dative Bonds With Ligands
- 15.60Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Physical And Chemical Properties Of The First Row Of Transition Elements, Titanium To Copper: Explain Why Transition Elements Form Complex Ions In Terms Of Vacant D Orbitals That Are Energetically Accessible
- 15.61Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe And Explain The Reactions Of Transition Elements With Ligands To Form Complexes, Including The Complexes Of Copper(Ii) And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 15.62Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Ligand As A Species That Contains A Lone Pair Of Electrons That Forms A Dative Covalent Bond To A Central Metal Atom/ion
- 15.63Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Understand And Use The Terms: (A) Monodentate Ligand Including As Examples H2o, Nh3, Cl   – And Cn– (B) Bidentate Ligand Including As Examples 1,2-diaminoethane, En, H2nch2ch2nh2 And The Ethanedioate Ion, C2o4 2– (C) Polydentate Ligand Including As An Example Edta4–
- 15.64Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Define The Term Complex As A Molecule Or Ion Formed By A Central Metal Atom/ion Surrounded By One Or More Ligands
- 15.65Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Geometry (Shape And Bond Angles) Of Transition Element Complexes Which Are Linear, Square Planar, Tetrahedral Or Octahedral
- 15.66Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Explain Qualitatively That Ligand Exchange Can Occur, Including The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions
- 15.67Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Predict, Using E ⦵ Values, The Feasibility Of Redox Reactions Involving Transition Elements And Their Ions
- 15.68Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Describe The Reactions Of, And Perform Calculations Involving: (A) Mno4 – /c2o4 2– In Acid Solution Given Suitable Data (B) Mno4 – /fe2+ In Acid Solution Given Suitable Data (C) Cu2+ / I – Given Suitable Data
- 15.69Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: General Characteristic Chemical Properties Of The First Set Of Transition Elements, Titanium To Copper: Perform Calculations Involving Other Redox Systems Given Suitable Data
- 15.70Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Define And Use The Terms Degenerate And Non-degenerate D Orbitals
- 15.71Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe The Splitting Of Degenerate D Orbitals Into Two Non-degenerate Sets Of D Orbitals Of Higher Energy, And Use Of Δe In: (A) Octahedral Complexes, Two Higher And Three Lower D Orbitals (B) Tetrahedral Complexes, Three Higher And Two Lower D Orbitals
- 15.72Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Explain Why Transition Elements Form Coloured Compounds In Terms Of The Frequency Of Light Absorbed As An Electron Is Promoted Between Two Non-degenerate D Orbitals
- 15.73Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Describe, In Qualitative Terms, The Effects Of Different Ligands On Δe, Frequency Of Light Absorbed, And Hence The Complementary Colour That Is Observed
- 15.74Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Colour Of Complexes: Use The Complexes Of Copper(Ii) Ions And Cobalt(Ii) Ions With Water And Ammonia Molecules And Hydroxide And Chloride Ions As Examples Of Ligand Exchange Affecting The Colour Observed
- 15.75Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Describe The Types Of Stereoisomerism Shown By Complexes, Including Those Associated With Bidentate Ligands: (A) Geometrical (Cis/trans) Isomerism, E.g. Square Planar Such As [pt(Nh₃)₂cl₂] And Octahedral Such As [co(Nh3) 4(H2o)2] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+ (B) Optical Isomerism, E.g. [ni(H2nch2ch2nh2) 3] 2+ And [ni(H2nch2ch2nh2) 2(H2o)2] 2+
- 15.76Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stereoisomerism In Transition Element Complexes: Deduce The Overall Polarity Of Complexes Such As Those Described In 28.4.1(A) And 28.4.1(B)
- 15.77Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Define The Stability Constant, Kstab, Of A Complex As The Equilibrium Constant For The Formation Of The Complex Ion In A Solvent (From Its Constituent Ions Or Molecules)
- 15.78Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Write An Expression For A Kstab Of A Complex ([hâ‚‚o] Should Not Be Included)
- 15.79Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Use Kstab Expressions To Perform Calculations
- 15.80Practice Questions: Inorganic Chemistry: Chemistry Of Transition Elements: Stability Constants, Kstab: Describe And Explain Ligand Exchanges In Terms Of Kstab Values And Understand That A Large Kstab Is Due To The Formation Of A Stable Complex Ion
- 15.81Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Page 47 Contain A Functional Group Which Dictates Their Physical And Chemical Properties
- 15.82Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound
- 15.83Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules (Including Cyclic Compounds Containing A Single Ring Of Up To Six Carbon Atoms) With Functional Groups Detailed In The Table On Page 47, Up To Six Carbon Atoms (Six Plus Six For Esters And Amides, Straight Chains Only For Esters And Nitriles)
- 15.84Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aromatic Molecules With One Benzene Ring And One Or More Simple Substituents, For Example 3-nitrobenzoic Acid Or 2,4,6-tribromophenol
- 15.85Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Electrophilic Substitution (B) Addition–elimination
- 15.86Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Shapes Of Aromatic Organic Molecules; Σ And ΠBonds: Describe And Explain The Shape Of Benzene And Other Aromatic Molecules, Including Sp² Hybridisation, In Terms Of Σ Bonds And A Delocalised ΠSystem
- 15.87Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand That Enantiomers Have Identical Physical And Chemical Properties Apart From Their Ability To Rotate Plane Polarised Light And Their Potential Biological Activity
- 15.88Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Understand And Use The Terms Optically Active And Racemic Mixture
- 15.89Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Describe The Effect On Plane Polarised Light Of The Two Optical Isomers Of A Single Substance
- 15.90Practice Questions: Organic Chemistry: An Introduction To Organic Chemistry of A Level: Isomerism: Optical: Explain The Relevance Of Chirality To The Synthetic Preparation Of Drug Molecules Including: (A) The Potential Different Biological Activity Of The Two Enantiomers (B) The Need To Separate A Racemic Mixture Into Two Pure Enantiomers (C) The Use Of Chiral Catalysts To Produce A Single Pure Optical Isomer (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds And Nomenclature Such As Diastereoisomers Is Not Required.)
- 15.91Practice Questions: Organic Chemistry: Hydrocarbons: Arenes: Describe The Chemistry Of Arenes As Exemplified By The Following Reactions Of Benzene And Methylbenzene: (A) Substitution Reactions With Cl₂ And With Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃, To Form Halogenoarenes (Aryl Halides) (B) Nitration With A Mixture Of Concentrated Hno₃ And Concentrated H₂so₄ At A Temperature Between 25°c And 60°c (C) Friedel–crafts Alkylation By Ch₃cl And Alcl₃ And Heat (D) Friedel–crafts Acylation By Ch₃cocl And Alcl₃ And Heat (E) Complete Oxidation Of The Side-chain Using Hot Alkaline Kmno₄ And Then Dilute Acid To Give A Benzoic Acid (F) Hydrogenation Of The Benzene Ring Using H₂ And Pt/ni Catalyst And Heat To Form A Cyclohexane Ring
- 15.92Practice Questions: Organic Chemistry: Hydrocarbons: Arenes: Describe The Mechanism Of Electrophilic Substitution In Arenes: (A) As Exemplified By The Formation Of Nitrobenzene And Bromobenzene (B) With Regards To The Effect Of Delocalisation (Aromatic Stabilisation) Of Electrons In Arenes To Explain The Predomination Of Substitution Over Addition
- 15.93Practice Questions: Organic Chemistry: Hydrocarbons: Arenes: Predict Whether Halogenation Will Occur In The Side-chain Or In The Aromatic Ring In Arenes Depending On Reaction Conditions
- 15.94Practice Questions: Organic Chemistry: Hydrocarbons: Arenes: Describe That In The Electrophilic Substitution Of Arenes, Different Substituents Direct To Different Ring Positions (Limited To The Directing Effects Of –nh₂, –oh, –r, –no₂, –cooh And –cor)
- 15.95Practice Questions: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Recall The Reactions By Which Halogenoarenes Can Be Produced: Substitution Of An Arene With Cl₂ Or Br₂ In The Presence Of A Catalyst, Alcl₃ Or Albr₃ To Form A Halogenoarene, Exemplified By Benzene To Form Chlorobenzene And Methylbenzene To Form 2-chloromethylbenzene And 4-chloromethylbenzene
- 15.96Practice Questions: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Organic Chemistry: Halogen Compounds: Halogen Compounds: Explain The Difference In Reactivity Between A Halogenoalkane And A Halogenoarene As Exemplified By Chloroethane And Chlorobenzene
- 15.97Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Describe The Reaction With Acyl Chlorides To Form Esters Using Ethyl Ethanoate
- 15.98Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Reactions (Reagents And Conditions) By Which Phenol Can Be Produced: (A) Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 15.99Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol:
- 15.100Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall The Chemistry Of Phenol, As Exemplified By The Following Reactions: (A) With Bases, For Example Naoh(Aq) To Produce Sodium Phenoxide (B) With Na(S) To Produce Sodium Phenoxide And H2(G) (C) In Naoh(Aq) With Diazonium Salts, To Give Azo Compounds (D) Nitration Of The Aromatic Ring With Dilute Hno₃(Aq) At Room Temperature To Give A Mixture Of 2-nitrophenol And 4-nitrophenol (E) Bromination Of The Aromatic Ring With Br₂(Aq) To Form 2,4,6-tribromophenol
- 15.101Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain The Acidity Of Phenol
- 15.102Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Describe And Explain The Relative Acidities Of Water, Phenol And Ethanol
- 15.103Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Explain Why The Reagents And Conditions For The Nitration And Bromination Of Phenol Are Different From Those For Benzene
- 15.104Practice Questions:Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Recall That The Hydroxyl Group Of A Phenol Directs To The 2-, 4- And 6-positions
- 15.105Practice Questions: Organic Chemistry: Hydroxy Compounds: Alcohols: Phenol: Apply Knowledge Of The Reactions Of Phenol To Those Of Other Phenolic Compounds, E.g. Naphthol
- 15.106Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reaction By Which Benzoic Acid Can Be Produced: (A) Reaction Of An Alkylbenzene With Hot Alkaline Kmnoâ‚„ And Then Dilute Acid, Exemplified By Methylbenzene
- 15.107Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe The Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂ To Form Acyl Chlorides
- 15.108Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Recognise That Some Carboxylic Acids Can Be Further Oxidised: (A) The Oxidation Of Methanoic Acid, Hcooh, With Fehling’s Reagent Or Tollens’ Reagent Or Acidified Kmno₄ Or Acidified K₂cr₂o₇ To Carbon Dioxide And Water (B) The Oxidation Of Ethanedioic Acid, Hooccooh, With Warm Acidified Kmno₄ To Carbon Dioxide
- 15.109Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Carboxylic Acids, Phenols And Alcohols
- 15.110Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Carboxylic Acids: Describe And Explain The Relative Acidities Of Chlorine-substituted Carboxylic Acids
- 15.111Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Esters: Recall The Reaction By Which Esters Can Be Produced: (A) Reaction Of Alcohols With Acyl Chlorides Using The Formation Of Ethyl Ethanoate And Phenyl Benzoate As Examples
- 15.112Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Recall The Reactions (Reagents And Conditions) By Which Acyl Chlorides Can Be Produced: (A) Reaction Of Carboxylic Acids With Pcl₃ And Heat, Pcl₅ Or Socl₂
- 15.113Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Following Reactions Of Acyl Chlorides: (A) Hydrolysis On Addition Of Water At Room Temperature To Give The Carboxylic Acid And Hcl (B) Reaction With An Alcohol At Room Temperature To Produce An Ester And Hcl (C) Reaction With Phenol At Room Temperature To Produce An Ester And Hcl (D) Reaction With Ammonia At Room Temperature To Produce An Amide And Hcl (E) Reaction With A Primary Or Secondary Amine At Room Temperature To Produce An Amide And Hcl
- 15.114Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Describe The Addition–elimination Mechanism Of Acyl Chlorides In Reactions In 33.3.2(A)–(E)
- 15.115Practice Questions: Organic Chemistry: Carboxylic Acids And Derivatives: Acyl Chlorides: Explain The Relative Ease Of Hydrolysis Of Acyl Chlorides, Alkyl Chlorides And Halogenoarenes (Aryl Chlorides)
- 15.116Practice Questions: Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Recall The Reactions (Reagents And Conditions) By Which Primary And Secondary Amines Are Produced: (A) Reaction Of Halogenoalkanes With Nh₃ In Ethanol Heated Under Pressure (B) Reaction Of Halogenoalkanes With Primary Amines In Ethanol, Heated In A Sealed Tube/under Pressure (C) The Reduction Of Amides With Lialh₄ (D) The Reduction Of Nitriles With Lialh₄ Or H₂/ni
- 15.117Practice Questions: Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe The Condensation Reaction Of Ammonia Or An Amine With An Acyl Chloride At Room Temperature To Give An Amide
- 15.118Practice Questions: Organic Chemistry: Nitrogen Compounds: Primary And Secondary Amines: Describe And Explain The Basicity Of Aqueous Solutions Of Amines
- 15.119Practice Questions: Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe The Preparation Of Phenylamine Via The Nitration Of Benzene To Form Nitrobenzene Followed By Reduction With Hot Sn/concentrated Hcl Followed By Naoh(Aq)
- 15.120Practice Questions: Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe: (A) The Reaction Of Phenylamine With Br₂(Aq) At Room Temperature (B) The Reaction Of Phenylamine With Hno₂ Or Nano₂ And Dilute Acid Below 10°c To Produce The Diazonium Salt; Further Warming Of The Diazonium Salt With H₂o To Give Phenol
- 15.121Practice Questions: Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Describe And Explain The Relative Basicities Of Aqueous Ammonia, Ethylamine And Phenylamine
- 15.122Practice Questions: Organic Chemistry: Nitrogen Compounds: Phenylamine And Azo Compounds: Recall The Following About Azo Compounds: (A) Describe The Coupling Of Benzenediazonium Chloride With Phenol In Naoh(Aq) To Form An Azo Compound (B) Identify The Azo Group (C) State That Azo Compounds Are Often Used As Dyes (D) That Other Azo Dyes Can Be Formed Via A Similar Route
- 15.123Practice Questions: Organic Chemistry: Nitrogen Compounds: Amides: Recall The Reactions (Reagents And Conditions) By Which Amides Are Produced: (A) The Reaction Between Ammonia And An Acyl Chloride At Room Temperature (B) The Reaction Between A Primary Amine And An Acyl Chloride At Room Temperature
- 15.124Practice Questions: Organic Chemistry: Nitrogen Compounds: Amides: Describe The Reactions Of Amides: (A) Hydrolysis With Aqueous Alkali Or Aqueous Acid (B) The Reduction Of The Co Group In Amides With Lialhâ‚„ To Form An Amine
- 15.125Practice Questions: Organic Chemistry: Nitrogen Compounds: Amides: State And Explain Why Amides Are Much Weaker Bases Than Amines
- 15.126Practice Questions: Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Acid/base Properties Of Amino Acids And The Formation Of Zwitterions, To Include The Isoelectric Point
- 15.127Practice Questions: Organic Chemistry: Nitrogen Compounds: Amino Acids: Describe The Formation Of Amide (Peptide) Bonds Between Amino Acids To Give Di- And Tripeptides
- 15.128Practice Questions: Organic Chemistry: Nitrogen Compounds: Amino Acids: Interpret And Predict The Results Of Electrophoresis On Mixtures Of Amino Acids And Dipeptides At Varying Phs (The Assembling Of The Apparatus Will Not Be Tested)
- 15.129Practice Questions: Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyesters: (A) The Reaction Between A Diol And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of A Hydroxycarboxylic Acid
- 15.130Practice Questions: Organic Chemistry: Polymerisation: Condensation Polymerisation: Describe The Formation Of Polyamides: (A) The Reaction Between A Diamine And A Dicarboxylic Acid Or Dioyl Chloride (B) The Reaction Of An Aminocarboxylic Acid (C) The Reaction Between Amino Acids
- 15.131Practice Questions: Organic Chemistry: Polymerisation: Condensation Polymerisation: Deduce The Repeat Unit Of A Condensation Polymer Obtained From A Given Monomer Or Pair Of Monomers
- 15.132Practice Questions: Organic Chemistry: Polymerisation: Condensation Polymerisation: Identify The Monomer(S) Present In A Given Section Of A Condensation Polymer Molecule
- 15.133Practice Questions: Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Predict The Type Of Polymerisation Reaction For A Given Monomer Or Pair Of Monomers
- 15.134Practice Questions: Organic Chemistry: Polymerisation: Predicting The Type Of Polymerisation: Deduce The Type Of Polymerisation Reaction Which Produces A Given Section Of A Polymer Molecule
- 15.135Practice Questions: Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Poly(Alkenes) Are Chemically Inert And Can Therefore Be Difficult To Biodegrade
- 15.136Practice Questions: Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Some Polymers Can Be Degraded By The Action Of Light
- 15.137Practice Questions: Organic Chemistry: Polymerisation: Degradable Polymers: Recognise That Polyesters And Polyamides Are Biodegradable By Acidic And Alkaline Hydrolysis
- 15.138Practice Questions: Organic Chemistry: Organic Synthesis: Organic Synthesis: For An Organic Molecule Containing Several Functional Groups: (A) Identify Organic Functional Groups Using The Reactions In The Syllabus (B) Predict Properties And Reactions
- 15.139Practice Questions: Organic Chemistry: Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus
- 15.140Practice Questions: Organic Chemistry: Organic Synthesis: Organic Synthesis: Analyse A Given Synthetic Route In Terms Of Type Of Reaction And Reagents Used For Each Step Of It, And Possible By-products Analysis
- 15.141Practice Questions: Analytical Techniques: Thin-layer Chromatography: Describe And Understand The Terms (A) Stationary Phase, For Example Aluminium Oxide (On A Solid Support) (B) Mobile Phase; A Polar Or Non-polar Solvent (C) Rf Value (D) Solvent Front And Baseline
- 15.142Practice Questions: Analytical Techniques: Thin-layer Chromatography: Interpret Rf Values
- 15.143Practice Questions: Analytical Techniques: Thin-layer Chromatography: Explain The Differences In Rf Values In Terms Of Interaction With The Stationary Phase And Of Relative Solubility In The Mobile Phase
- 15.144Practice Questions: Analytical Techniques: Gas/liquid Chromatography: Describe And Understand The Terms (A) Stationary Phase; A High Boiling Point Non-polar Liquid (On A Solid Support) (B) Mobile Phase; An Unreactive Gas (C) Retention Time
- 15.145Practice Questions: Analytical Techniques: Gas/liquid Chromatography: Interpret Gas /liquid Chromatograms In Terms Of The Percentage Composition Of A Mixture
- 15.146Practice Questions: Analytical Techniques: Gas/liquid Chromatography: Explain Retention Times In Terms Of Interaction With The Stationary Phase
- 15.147Practice Questions: Analytical Techniques: Carbon-13 Nmr Spectroscopy: Analyse And Interpret A Carbon-13 Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of The Carbon Atoms Present (B) The Possible Structures For The Molecule
- 15.148Practice Questions: Analytical Techniques: Carbon-13 Nmr Spectroscopy: Predict Or Explain The Number Of Peaks In A Carbon-13 Nmr Spectrum For A Given Molecule
- 15.149Practice Questions: Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Analyse And Interpret A Proton (1 H) Nmr Spectrum Of A Simple Molecule To Deduce: (A) The Different Environments Of Proton Present Using Chemical Shift Values (B) The Relative Numbers Of Each Type Of Proton Present From Relative Peak Areas (C) The Number Of Equivalent Protons On The Carbon Atom Adjacent To The One To Which The Given Proton Is Attached From The Splitting Pattern, Using The N + 1 Rule (Limited To Singlet, Doublet, Triplet, Quartet And Multiplet) (D) The Possible Structures For The Molecule
- 15.150Practice Questions: Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Use Of Tetramethylsilane, Tms, As The Standard For Chemical Shift Measurements
- 15.151Practice Questions: Analytical Techniques: Proton (1 H) Nmr Spectroscopy: State The Need For Deuterated Solvents, E.g. Cdcl₃, When Obtaining A Proton Nmr Spectrum
- 15.152Practice Questions: Analytical Techniques: Proton (1 H) Nmr Spectroscopy: Describe The Identification Of O–h And N–h Protons By Proton Exchange Using D₂o
- Mock Tests/ Mock ExamsMock Exams For Final Preparation0
- Class RecordingsClass Recordings From Previous Sessions/ Current Session For Content0
- Other MaterialOther Useful Material For Exams0
- Notes + Written Material For Contents of The Syllabus Version 2Notes for Chapters + Written Resources Regarding The Content Version 240
- 20.1Lattice Energy and Born-Haber Cycles
- 20.2Enthalpies of Solution and Hydration
- 20.3Entropy Change, ΔS
- 20.4Gibbs Free Energy Change, ΔG
- 20.5Electrolysis
- 20.6Standard Electrode Potentials E⦵, Standard Cell Potentials E⦵ cell And The Nernst Equation
- 20.7Acid and Bases
- 20.8Partition Coefficient
- 20.9Sample Rate Equations, Orders of Reaction And Rate Constants
- 20.10Homogeneous and Heterogeneous Catalysts
- 20.11Similarities And Trends In The Properties of The Group 2 Metals, Magnesium to Barium, and Their Compounds
- 20.12Genera’ Physical and Chemical Properties of the First Row of Transition Elements, Titanium to Copper
- 20.13General Characteristics Chemical Properties of the First Set of Transition Elements, Titanium to Copper
- 20.14Color of Complexes
- 20.15Stereoisomerism in Transition Element Complexes
- 20.16Stability Constants, Kstab
- 20.17An Introduction To A Level Organic Chemistry
- 20.18Formulas, Functional Groups and The Naming of Organic Compounds
- 20.19Characteristic Organic Reactions
- 20.20Shapes of Aromatic Organic Molecules; σ and π Bonds
- 20.21Isomerism Optical
- 20.22Arenes
- 20.23Halogen Compounds
- 20.24Alcohols
- 20.25Phenol
- 20.26Carboxylic Acids
- 20.27Esters
- 20.28Acyl Chlorides
- 20.29Primary And Secondary Amines
- 20.30Phenylamine and Azo Compounds
- 20.31Amides
- 20.32Amino Acids
- 20.33Condensation Polymerisation
- 20.34Predicting The Type of Polymerisation
- 20.35Degrade Polymers
- 20.36Organic Synthesis
- 20.37Thin-Layer Chromatography
- 20.38Gas/ Liquid Chromatography
- 20.39Carbon-13 NMR Spectroscopy
- 20.40Proton (1 H) NMR Spectroscopy
- Quizzes For Preparation Version 2Quizzes With Detailed Explained Answers And Common Mistakes Discussed In Detail Version 240
- 21.1Lattice Energy and Born-Haber Cycles
- 21.2Enthalpies of Solution and Hydration
- 21.3Entropy Change, ΔS
- 21.4Gibbs Free Energy Change, ΔG
- 21.5Electrolysis
- 21.6Standard Electrode Potentials E⦵, Standard Cell Potentials E⦵ cell And The Nernst Equation
- 21.7Acid and Bases
- 21.8Partition Coefficient
- 21.9Sample Rate Equations, Orders of Reaction And Rate Constants
- 21.10Homogeneous and Heterogeneous Catalysts
- 21.11Similarities And Trends In The Properties of The Group 2 Metals, Magnesium to Barium, and Their Compounds
- 21.12Genera’ Physical and Chemical Properties of the First Row of Transition Elements, Titanium to Copper
- 21.13General Characteristics Chemical Properties of the First Set of Transition Elements, Titanium to Copper
- 21.14Color of Complexes
- 21.15Stereoisomerism in Transition Element Complexes
- 21.16Stability Constants, Kstab
- 21.17An Introduction To A Level Organic Chemistry
- 21.18Formulas, Functional Groups and The Naming of Organic Compounds
- 21.19Characteristic Organic Reactions
- 21.20Shapes of Aromatic Organic Molecules; σ and π Bonds
- 21.21Isomerism Optical
- 21.22Arenes
- 21.23Alcohols
- 21.24Halogen Compounds
- 21.25Phenol
- 21.26Carboxylic Acids
- 21.27Esters
- 21.28Acyl Chlorides
- 21.29Primary And Secondary Amines
- 21.30Phenylamine and Azo Compounds
- 21.31Amides
- 21.32Amino Acids
- 21.33Condensation Polymerisation
- 21.34Predicting The Type of Polymerisation
- 21.35Degrade Polymers
- 21.36Organic Synthesis
- 21.37Thin-Layer Chromatography
- 21.38Gas/ Liquid Chromatography
- 21.39Carbon-13 NMR Spectroscopy
- 21.40Proton (1 H) NMR Spectroscopy
- Cheat Sheets Version 2Short, Quick Revision Cheat Sheets Version 240
- 22.1Lattice Energy and Born-Haber Cycles
- 22.2Enthalpies of Solution and Hydration
- 22.3Entropy Change, ΔS
- 22.4Gibbs Free Energy Change, ΔG
- 22.5Electrolysis
- 22.6Standard Electrode Potentials E⦵, Standard Cell Potentials E⦵ cell And The Nernst Equation
- 22.7Acid and Bases
- 22.8Partition Coefficient
- 22.9Sample Rate Equations, Orders of Reaction And Rate Constants
- 22.10Homogeneous and Heterogeneous Catalysts
- 22.11Similarities And Trends In The Properties of The Group 2 Metals, Magnesium to Barium, and Their Compounds
- 22.12Genera’ Physical and Chemical Properties of the First Row of Transition Elements, Titanium to Copper
- 22.13General Characteristics Chemical Properties of the First Set of Transition Elements, Titanium to Copper
- 22.14Color of Complexes
- 22.15Stereoisomerism in Transition Element Complexes
- 22.16Stability Constants, Kstab
- 22.17An Introduction To A Level Organic Chemistry
- 22.18Formulas, Functional Groups and The Naming of Organic Compounds
- 22.19Characteristic Organic Reactions
- 22.20Shapes of Aromatic Organic Molecules; σ and π Bonds
- 22.21Isomerism Optical
- 22.22Arenes
- 22.23Halogen Compounds
- 22.24Alcohols
- 22.25Phenol
- 22.26Carboxylic Acids
- 22.27Esters
- 22.28Acyl Chlorides
- 22.29Primary And Secondary Amines
- 22.30Phenylamine and Azo Compounds
- 22.31Amides
- 22.32Amino Acids
- 22.33Condensation Polymerisation
- 22.34Predicting The Type of Polymerisation
- 22.35Degrade Polymers
- 22.36Organic Synthesis
- 22.37Thin-Layer Chromatography
- 22.38Gas/ Liquid Chromatography
- 22.39Carbon-13 NMR Spectroscopy
- 22.40Proton (1 H) NMR Spectroscopy
Instructor
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Once you receive access to the course, use notes from Section 3 and attempt the Quizzes for Preparation Section 6. These quizzes serve 2 purposes. First, they allow your instructor to judge exactly where you stand and devise the best strategy moving forward. Second, they allow you to get a glimpse of the entire syllabus quickly, helping you follow the material easily later on. Please note, passing these quizzes or scoring a high mark is NOT A REQUIREMENT. Attempting them is mandatory.
Use the course forum to submit ONLY the questions you attempted WRONG in each quiz. For example, if you attempted Question 5.18, 25 wrong from Quiz Number 6.7, on the forum just write Quiz 6.7 Question 5, 18, 25. That's all.
In each quiz for preparation, you are offered the answers and explanations for each question, including why a certain answer is correct, at the end of the quiz. Use them to check which answers you attempted wrong.
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2. Section 2 is Course Related Information
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The items inside each section are numbered with decimals. For example, 3.12 is part of Notes + Written Material For Contents of The Syllabus.
This method makes it easier to find relevant quizzes, cheat sheets and practice questions etc. of each set of notes/ topics."
1. Section 1 is Sample Content
2. Section 2 is Course Related Information
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The items inside each section are numbered with decimals. For example, 3.12 is part of Notes + Written Material For Contents of The Syllabus.
This method makes it easier to find relevant quizzes, cheat sheets and practice questions etc. of each set of notes/ topics."
We make sure that our courses are extremely useful for the students. For each course, we offer multiple types of notes. Section 3 contains notes divided exactly per syllabus division and in complete detail. As such, these notes are extremely useful for a first-time learner learning from scratch. Notes in Section 11 are rearranged in a more learning friendly way and makes them easier for students to follow. In some courses, other Notes sections appear at the end, offering even more variations of notes for students to benefit from.
Section 5 Quizzes are to be completed DURING the course. Section 6 Quizzes For Preparation Are Preliminary quizzes to be completed at the start of the course.
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This Full-Scale course / Complete Course offers a complete online coverage for both the syllabus and the preparation for the examination. The AS Level Islamic...
Further Mathematics (FP1 and FM1) (9231) | AS LEVEL | Full-Scale Course
This Full-Scale course / Complete Course offers a complete online coverage for both the syllabus and the preparation for the examination. The AS Level Further...
Information Technology (9626) | AS LEVEL | Full Scale Course
This Full-Scale course / Complete Course offers a complete online coverage for both the syllabus and the preparation for the examination. The AS Level Information...
English Language (9093) | AS LEVEL | Full Scale Course
This Full-Scale course / Complete Course offers a complete online coverage for both the syllabus and the preparation for the examination. The AS Level English...
₨123,123.00
Course Features
- Lectures 926
- Quizzes 16
- Duration 6-8 Months
- Skill level All levels
- Language English-Urdu
- Students 5
- Assessments Yes