Sample Notes: Atomic Structure

Sample Notes: Nitrogen Compounds

Sample Quizzes For Preparation: Atomic Structure

Sample Quizzes For Preparation: Nitrogen Compounds

Schedule For Live Classes

Zoom Details

Course Breakup

Atomic Structure: Particles In The Atom And Atomic Radius: Understand That Atoms Are Mostly Empty Space Surrounding A Very Small, Dense Nucleus That Contains Protons And Neutrons; Electrons Are Found In Shells In The Empty Space Around The Nucleus

Atomic Structure: Particles In The Atom And Atomic Radius: Identify And Describe Protons, Neutrons And Electrons In Terms Of Their Relative Charges And Relative Masses

Atomic Structure: Particles In The Atom And Atomic Radius: Understand The Terms Atomic And Proton Number; Mass And Nucleon Number

Atomic Structure: Particles In The Atom And Atomic Radius: Describe The Distribution Of Mass And Charge Within An Atom

Atomic Structure: Particles In The Atom And Atomic Radius: Describe The Behaviour Of Beams Of Protons, Neutrons And Electrons Moving At The Same Velocity In An Electric Field

Atomic Structure: Particles In The Atom And Atomic Radius: Determine The Numbers Of Protons, Neutrons And Electrons Present In Both Atoms And Ions Given Atomic Or Proton Number, Mass Or Nucleon Number And Charge

Atomic Structure: Particles In The Atom And Atomic Radius: State And Explain Qualitatively The Variations In Atomic Radius And Ionic Radius Across A Period And Down A Group

Atomic Structure: Isotopes: Define The Term Isotope In Terms Of Numbers Of Protons And Neutrons

Atomic Structure: Isotopes: Understand The Notation X Ya For Isotopes, Where X Is The Mass Or Nucleon Number And Y Is The Atomic Or Proton Number

Atomic Structure: Isotopes: State That And Explain Why Isotopes Of The Same Element Have The Same Chemical Properties

Atomic Structure: Isotopes: State That And Explain Why Isotopes Of The Same Element Have Different Physical Properties, Limited To Mass And Density

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Understand The Terms: • Shells, Sub-shells And Orbitals • Principal Quantum Number (N) • Ground State, Limited To Electronic Configuration

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe The Number Of Orbitals Making Up S, P And D Sub-shells, And The Number Of Electrons That Can Fill S, P And D Sub-shells

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe The Order Of Increasing Energy Of The Sub-shells Within The First Three Shells And The 4s And 4p Sub-shells

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe The Electronic Configurations To Include The Number Of Electrons In Each Shell, Sub-shell And Orbital

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Explain The Electronic Configurations In Terms Of Energy Of The Electrons And Inter-electron Repulsion

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Determine The Electronic Configuration Of Atoms And Ions Given The Atomic Or Proton Number And Charge, Using Either Of The Following Conventions: E.g. For Fe: 1s2 2s2 2p6 3s2 3p6 3d6 4s2 (Full Electronic Configuration) Or [ar] 3d6 4s2 (Shorthand Electronic Configuration)

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Understand And Use The Electrons In Boxes Notation E.g. For Fe: [ar]

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe And Sketch The Shapes Of S And P Orbitals

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe A Free Radical As A Species With One Or More Unpaired Electrons

Atomic Structure: Ionisation Energy: Define And Use The Term First Ionisation Energy, Ie

Atomic Structure: Ionisation Energy: Construct Equations To Represent First, Second And Subsequent Ionisation Energies

Atomic Structure: Ionisation Energy: Identify And Explain The Trends In Ionisation Energies Across A Period And Down A Group Of The Periodic Table

Atomic Structure: Ionisation Energy: Identify And Explain The Variation In Successive Ionisation Energies Of An Element

Atomic Structure: Ionisation Energy: Understand That Ionisation Energies Are Due To The Attraction Between The Nucleus And The Outer Electron

Atomic Structure: Ionisation Energy: Explain The Factors Influencing The Ionisation Energies Of Elements In Terms Of Nuclear Charge, Atomic/ionic Radius, Shielding By Inner Shells And Sub-shells And Spin-pair Repulsion

Atomic Structure: Ionisation Energy: Deduce The Electronic Configurations Of Elements Using Successive Ionisation Energy Data

Atomic Structure: Ionisation Energy: Deduce The Position Of An Element In The Periodic Table Using Successive Ionisation Energy Data

Atoms, Molecules And Stoichiometry: Relative Masses Of Atoms And Molecules: Define The Unified Atomic Mass Unit As One Twelfth Of The Mass Of A Carbon-12 Atom

Atoms, Molecules And Stoichiometry: Relative Masses Of Atoms And Molecules: Define Relative Atomic Mass, Ar , Relative Isotopic Mass, Relative Molecular Mass, Mr , And Relative Formula Mass In Terms Of The Unified Atomic Mass Unit

Atoms, Molecules And Stoichiometry: The Mole And The Avogadro Constant: Define And Use The Term Mole In Terms Of The Avogadro Constant

Atoms, Molecules And Stoichiometry: Formulas: Write Formulas Of Ionic Compounds From Ionic Charges And Oxidation Numbers (Shown By A Roman Numeral), Including: (A) The Prediction Of Ionic Charge From The Position Of An Element In The Periodic Table (B) Recall Of The Names And Formulas For The Following Ions: No3 – , Co3 2–, So4 2–, Oh– , Nh4 + , Zn2+, Ag+ , Hco3 – , Po4 3–

Atoms, Molecules And Stoichiometry: Formulas: (A) Write And Construct Equations (Which Should Be Balanced), Including Ionic Equations (Which Should Not Include Spectator Ions) (B) Use Appropriate State Symbols In Equations

Atoms, Molecules And Stoichiometry: Formulas: Define And Use The Terms Empirical And Molecular Formula

Atoms, Molecules And Stoichiometry: Formulas: Understand And Use The Terms Anhydrous, Hydrated And Water Of Crystallisation

Atoms, Molecules And Stoichiometry: Formulas: Calculate Empirical And Molecular Formulas, Using Given Data

Atoms, Molecules And Stoichiometry: Reacting Masses And Volumes (Of Solutions And Gases): Perform Calculations Including Use Of The Mole Concept, Involving: (A) Reacting Masses (From Formulas And Equations) Including Percentage Yield Calculations (B) Volumes Of Gases (E.g. In The Burning Of Hydrocarbons) (C) Volumes And Concentrations Of Solutions (D) Limiting Reagent And Excess Reagent (When Performing Calculations, Candidates’ Answers Should Reflect The Number Of Significant Figures Given Or Asked For In The Question. When Rounding Up Or Down, Candidates Should Ensure That Significant Figures Are Neither Lost Unnecessarily Nor Used Beyond What Is Justified (See Also Mathematical Requirements Section).) (E) Deduce Stoichiometric Relationships From Calculations Such As Those In 2.4.1(A)–(D)

Chemical Bonding: Electronegativity And Bonding: Define Electronegativity As The Power Of An Atom To Attract Electrons To Itself

Chemical Bonding: Electronegativity And Bonding: Explain The Factors Influencing The Electronegativities Of The Elements In Terms Of Nuclear Charge, Atomic Radius And Shielding By Inner Shells And Sub-shells

Chemical Bonding: Electronegativity And Bonding: State And Explain The Trends In Electronegativity Across A Period And Down A Group Of The Periodic Table

Chemical Bonding: Electronegativity And Bonding: Use The Differences In Pauling Electronegativity Values To Predict The Formation Of Ionic And Covalent Bonds (The Presence Of Covalent Character In Some Ionic Compounds Will Not Be Assessed) (Pauling Electronegativity Values Will Be Given Where Necessary)

Chemical Bonding: Ionic Bonding: Define Ionic Bonding As The Electrostatic Attraction Between Oppositely Charged Ions (Positively Charged Cations And Negatively Charged Anions)

Chemical Bonding: Ionic Bonding: Describe Ionic Bonding Including The Examples Of Sodium Chloride, Magnesium Oxide And Calcium Fluoride

Chemical Bonding: Metallic Bonding: Define Metallic Bonding As The Electrostatic Attraction Between Positive Metal Ions And Delocalised Electrons

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: Define Covalent Bonding As Electrostatic Attraction Between The Nuclei Of Two Atoms And A Shared Pair Of Electrons (A) Describe Covalent Bonding In Molecules Including: • Hydrogen, H2 • Oxygen, O2 • Nitrogen, N2 • Chlorine, Cl 2 • Hydrogen Chloride, Hcl • Carbon Dioxide, Co2 • Ammonia, Nh3 • Methane, Ch4 • Ethane, C2h6 • Ethene, C2h4 (B) Understand That Elements In Period 3 Can Expand Their Octet Including In The Compounds Sulfur Dioxide, So2, Phosphorus Pentachloride, Pcl 5 , And Sulfur Hexafluoride, Sf6 (C) Describe Coordinate (Dative Covalent) Bonding, Including In The Reaction Between Ammonia And Hydrogen Chloride Gases To Form The Ammonium Ion, Nh4 + , And In The Al 2cl 6 Molecule

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: (A) Describe Covalent Bonds In Terms Of Orbital Overlap Giving Σ And Π Bonds: • Σ Bonds Are Formed By Direct Overlap Of Orbitals Between The Bonding Atoms • Π Bonds Are Formed By The Sideways Overlap Of Adjacent P Orbitals Above And Below The Σ Bond (B) Describe How The Σ And Π Bonds Form In Molecules Including H₂, C₂h₆, C₂h₄, Hcn And N₂ (C) Use The Concept Of Hybridisation To Describe Sp, Sp² And Sp³ Orbitals

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: A) Define The Terms: • Bond Energy As The Energy Required To Break One Mole Of A Particular Covalent Bond In The Gaseous State • Bond Length As The Internuclear Distance Of Two Covalently Bonded Atoms (B) Use Bond Energy Values And The Concept Of Bond Length To Compare The Reactivity Of Covalent Molecules

Chemical Bonding: Shapes Of Molecules: State And Explain The Shapes Of, And Bond Angles In, Molecules By Using Vsepr Theory, Including As Simple Examples: • Bf3 (Trigonal Planar, 120°) • Co2 (Linear, 180°) • Ch4 (Tetrahedral, 109.5°) • Nh3 (Pyramidal, 107°) • H2o (Non-linear, 104.5°) • Sf6 (Octahedral, 90°) • Pf5 (Trigonal Bipyramidal, 120° And 90°)

Chemical Bonding: Shapes Of Molecules: Predict The Shapes Of, And Bond Angles In, Molecules And Ions Analogous To Those Specified In 3.5.1

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: (A) Describe Hydrogen Bonding, Limited To Molecules Containing N–h And O–h Groups, Including Ammonia And Water As Simple Examples (B) Use The Concept Of Hydrogen Bonding To Explain The Anomalous Properties Of H₂o (Ice And Water): • Its Relatively High Melting And Boiling Points • Its Relatively High Surface Tension • The Density Of The Solid Ice Compared With The Liquid Water

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: Use The Concept Of Electronegativity To Explain Bond Polarity And Dipole Moments Of Molecules

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: (A) Describe Van Der Waals’ Forces As The Intermolecular Forces Between Molecular Entities Other Than Those Due To Bond Formation, And Use The Term Van Der Waals’ Forces As A Generic Term To Describe All Intermolecular Forces (B) Describe The Types Of Van Der Waals’ Forces: • Instantaneous Dipole–induced Dipole (Id-id) Forces, Also Called London Dispersion Forces • Permanent Dipole–permanent Dipole (Pd-pd) Forces, Including Hydrogen Bonding (C) Describe Hydrogen Bonding And Understand That Hydrogen Bonding Is A Special Case Of Permanent Dipole–permanent Dipole Forces Between Molecules Where Hydrogen Is Bonded To A Highly Electronegative Atom

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: State That, In General, Ionic, Covalent And Metallic Bonding Are Stronger Than Intermolecular Forces

Chemical Bonding: Dot-and-cross Diagrams: Use Dot-and-cross Diagrams To Illustrate Ionic, Covalent And Coordinate Bonding Including The Representation Of Any Compounds Stated In 3.4 And 3.5 (Dot-and-cross Diagrams May Include Species With Atoms Which Have An Expanded Octet Or Species With An Odd Number Of Electrons)

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: Explain The Origin Of Pressure In A Gas In Terms Of Collisions Between Gas Molecules And The Wall Of The Container

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: Understand That Ideal Gases Have Zero Particle Volume And No Intermolecular Forces Of Attraction

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: State And Use The Ideal Gas Equation Pv = Nrt In Calculations, Including In The Determination Of Mr

States Of Matter: Bonding And Structure: Describe, In Simple Terms, The Lattice Structure Of A Crystalline Solid Which Is: (A) Giant Ionic, Including Sodium Chloride And Magnesium Oxide (B) Simple Molecular, Including Iodine, Buckminsterfullerene C60 And Ice (C) Giant Molecular, Including Silicon(Iv) Oxide, Graphite And Diamond (D) Giant Metallic, Including Copper

States Of Matter: Bonding And Structure: Describe, Interpret And Predict The Effect Of Different Types Of Structure And Bonding On The Physical Properties Of Substances, Including Melting Point, Boiling Point, Electrical Conductivity And Solubility

States Of Matter: Bonding And Structure: Deduce The Type Of Structure And Bonding Present In A Substance From Given Information

Chemical Energetics: Enthalpy Change, Δh: Understand That Chemical Reactions Are Accompanied By Enthalpy Changes And These Changes Can Be Exothermic (δh Is Negative) Or Endothermic (δh Is Positive)

Chemical Energetics: Enthalpy Change, Δh: Construct And Interpret A Reaction Pathway Diagram, In Terms Of The Enthalpy Change Of The Reaction And Of The Activation Energy

Chemical Energetics: Enthalpy Change, Δh: Define And Use The Terms: (A) Standard Conditions (This Syllabus Assumes That These Are 298k And 101kpa) Shown By ⦵ . (B) Enthalpy Change With Particular Reference To: Reaction, Δhr , Formation, Δhf , Combustion, Δhc , Neutralisation, Δhneut

Chemical Energetics: Enthalpy Change, Δh: Understand That Energy Transfers Occur During Chemical Reactions Because Of The Breaking And Making Of Chemical Bonds

Chemical Energetics: Enthalpy Change, Δh: Use Bond Energies (δh Positive, I.e. Bond Breaking) To Calculate Enthalpy Change Of Reaction, Δhr

Chemical Energetics: Enthalpy Change, Δh: Understand That Some Bond Energies Are Exact And Some Bond Energies Are Averages

Chemical Energetics: Enthalpy Change, Δh: Calculate Enthalpy Changes From Appropriate Experimental Results, Including The Use Of The Relationships Q = Mcδt And Δh = –mcδt/ N

Chemical Energetics: Hess’s Law: Apply Hess’s Law To Construct Simple Energy Cycles

Chemical Energetics: Hess’s Law: Carry Out Calculations Using Cycles And Relevant Energy Terms, Including: (A) Determining Enthalpy Changes That Cannot Be Found By Direct Experiment (B) Use Of Bond Energy Data

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Calculate Oxidation Numbers Of Elements In Compounds And Ions

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Use Changes In Oxidation Numbers To Help Balance Chemical Equations

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Explain And Use The Terms Redox, Oxidation, Reduction And Disproportionation In Terms Of Electron Transfer And Changes In Oxidation Number

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Explain And Use The Terms Oxidising Agent And Reducing Agent

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Use A Roman Numeral To Indicate The Magnitude Of The Oxidation Number Of An Element

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: (A) Understand What Is Meant By A Reversible Reaction (B) Understand What Is Meant By Dynamic Equilibrium In Terms Of The Rate Of Forward And Reverse Reactions Being Equal And The Concentration Of Reactants And Products Remaining Constant (C) Understand The Need For A Closed System In Order To Establish Dynamic Equilibrium

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Define Le Chatelier’s Principle As: If A Change Is Made To A System At Dynamic Equilibrium, The Position Of Equilibrium Moves To Minimise This Change

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use Le Chatelier’s Principle To Deduce Qualitatively (From Appropriate Information) The Effects Of Changes In Temperature, Concentration, Pressure Or Presence Of A Catalyst On A System At Equilibrium

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Deduce Expressions For Equilibrium Constants In Terms Of Concentrations, Kc

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use The Terms Mole Fraction And Partial Pressure

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Deduce Expressions For Equilibrium Constants In Terms Of Partial Pressures, Kp (Use Of The Relationship Between Kp And Kc Is Not Required)

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use The Kc And Kp Expressions To Carry Out Calculations (Such Calculations Will Not Require The Solving Of Quadratic Equations)

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Calculate The Quantities Present At Equilibrium, Given Appropriate Data

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: State Whether Changes In Temperature, Concentration Or Pressure Or The Presence Of A Catalyst Affect The Value Of The Equilibrium Constant For A Reaction

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Describe And Explain The Conditions Used In The Haber Process And The Contact Process, As Examples Of The Importance Of An Understanding Of Dynamic Equilibrium In The Chemical Industry And The Application Of Le Chatelier’s Principle

Brønsted–lowry Theory Of Acids And Bases: State The Names And Formulas Of The Common Acids, Limited To Hydrochloric Acid, Hcl, Sulfuric Acid, H2so4, Nitric Acid, Hno3, Ethanoic Acid, Ch3cooh

Brønsted–lowry Theory Of Acids And Bases: State The Names And Formulas Of The Common Alkalis, Limited To Sodium Hydroxide, Naoh, Potassium Hydroxide, Koh, Ammonia, Nh3

Brønsted–lowry Theory Of Acids And Bases: Describe The Brønsted–lowry Theory Of Acids And Bases

Brønsted–lowry Theory Of Acids And Bases: Describe Strong Acids And Strong Bases As Fully Dissociated In Aqueous Solution And Weak Acids And Weak Bases As Partially Dissociated In Aqueous Solution

Brønsted–lowry Theory Of Acids And Bases: Appreciate That Water Has Ph Of 7, Acid Solutions Ph Of Below 7 And Alkaline Solutions Ph Of Above 7

Brønsted–lowry Theory Of Acids And Bases: Explain Qualitatively The Differences In Behaviour Between Strong And Weak Acids Including The Reaction With A Reactive Metal And Difference In Ph Values By Use Of A Ph Meter, Universal Indicator Or Conductivity

Brønsted–lowry Theory Of Acids And Bases: Understand That Neutralisation Reactions Occur When H+ (Aq) And Oh– (Aq) Form H2o(L)

Brønsted–lowry Theory Of Acids And Bases: Understand That Salts Are Formed In Neutralisation Reactions

Brønsted–lowry Theory Of Acids And Bases: Sketch The Ph Titration Curves Of Titrations Using Combinations Of Strong And Weak Acids With Strong And Weak Alkalis

Brønsted–lowry Theory Of Acids And Bases: Select Suitable Indicators For Acid-alkali Titrations, Given Appropriate Data (Pka Values Will Not Be Used)

Reaction Kinetics: Rate Of Reaction: Explain And Use The Term Rate Of Reaction, Frequency Of Collisions, Effective Collisions And Non-effective Collisions

Reaction Kinetics: Rate Of Reaction: Explain Qualitatively, In Terms Of Frequency Of Effective Collisions, The Effect Of Concentration And Pressure Changes On The Rate Of A Reaction

Reaction Kinetics: Rate Of Reaction: Use Experimental Data To Calculate The Rate Of A Reaction

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Define Activation Energy, Ea, As The Minimum Energy Required For A Collision To Be Effective

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Sketch And Use The Boltzmann Distribution To Explain The Significance Of Activation Energy

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Explain Qualitatively, In Terms Both Of The Boltzmann Distribution And Of Frequency Of Effective Collisions, The Effect Of Temperature Change On The Rate Of A Reaction

Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain And Use The Terms Catalyst And Catalysis: (A) Explain That, In The Presence Of A Catalyst, A Reaction Has A Different Mechanism, I.e. One Of Lower Activation Energy (B) Explain This Catalytic Effect In Terms Of The Boltzmann Distribution (C) Construct And Interpret A Reaction Pathway Diagram, For A Reaction In The Presence And Absence Of An Effective Catalyst

The Periodic Table: Chemical Periodicity: Periodicity Of Physical Properties Of The Elements In Period 3: Describe Qualitatively (And Indicate The Periodicity In) The Variations In Atomic Radius, Ionic Radius, Melting Point And Electrical Conductivity Of The Elements

The Periodic Table: Chemical Periodicity: Periodicity Of Physical Properties Of The Elements In Period 3: Explain The Variation In Melting Point And Electrical Conductivity In Terms Of The Structure And Bonding Of The Elements

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, And Write Equations For, The Reactions Of The Elements With Oxygen (To Give Na2o, Mgo, Al 2o3, P4o10, So2), Chlorine (To Give Nacl, Mgcl 2, Alcl 3, Sicl 4, Pcl 5) And Water (Na And Mg Only)

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: State And Explain The Variation In The Oxidation Number Of The Oxides (Na2o, Mgo, Al 2o3, P4o10, So2 And So3 Only) And Chlorides (Nacl, Mgcl 2, Alcl 3, Sicl 4, Pcl 5 Only) In Terms Of Their Outer Shell (Valence Shell) Electrons

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, And Write Equations For, The Reactions, If Any, Of The Oxides Na2o, Mgo, Al 2o3, Sio2, P4o10, So2 And So3 With Water Including The Likely Phs Of The Solutions Obtained

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, Explain, And Write Equations For, The Acid/base Behaviour Of The Oxides Na2o, Mgo, Al 2o3, P4o10, So2 And So3 And The Hydroxides Naoh, Mg(Oh)2 And Al(Oh)3 Including, Where Relevant, Amphoteric Behaviour In Reactions With Acids And Bases (Sodium Hydroxide Only)

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, Explain, And Write Equations For, The Reactions Of The Chlorides Nacl, Mgcl 2, Al Cl 3, Sicl 4, Pcl 5 With Water Including The Likely Phs Of The Solutions Obtained

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Explain The Variations And Trends In 9.2.2, 9.2.3, 9.2.4 And 9.2.5 In Terms Of Bonding And Electronegativity

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Suggest The Types Of Chemical Bonding Present In The Chlorides And Oxides From Observations Of Their Chemical And Physical Properties

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Write Equations For, The Reactions Of The Elements With Oxygen, Water And Dilute Hydrochloric And Sulfuric Acids

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Write Equations For, The Thermal Decomposition Of The Nitrates And Carbonates, To Include The Trend In Thermal Stabilities

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Make Predictions From, The Trends In Physical And Chemical Properties Of The Elements Involved In The Reactions In 10.1.1 And The Compounds Involved In 10.1.2, 10.1.3 And 10.1.5

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: State The Variation In The Solubilities Of The Hydroxides And Sulfates

Group 17: Physical Properties Of The Group 17 Elements: Describe The Colours And The Trend In Volatility Of Chlorine, Bromine And Iodine

Group 17: Physical Properties Of The Group 17 Elements: Describe And Explain The Trend In The Bond Strength Of The Halogen Molecules

Group 17: Physical Properties Of The Group 17 Elements: Interpret The Volatility Of The Elements In Terms Of Instantaneous Dipole–induced Dipole Forces

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Relative Reactivity Of The Elements As Oxidising Agents

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Reactions Of The Elements With Hydrogen And Explain Their Relative Reactivity In These Reactions

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Relative Thermal Stabilities Of The Hydrogen Halides And Explain These In Terms Of Bond Strengths

Group 17: Some Reactions Of The Halide Ions: Describe The Relative Reactivity Of Halide Ions As Reducing Agents

Group 17: Some Reactions Of The Halide Ions: Describe And Explain The Reactions Of Halide Ions With: (A) Aqueous Silver Ions Followed By Aqueous Ammonia (The Formation And Formula Of The [ag(Nh3) 2] + Complex Is Not Required) (B) Concentrated Sulfuric Acid, To Include Balanced Chemical Equations

Group 17: The Reactions Of Chlorine: Describe And Interpret, In Terms Of Changes In Oxidation Number, The Reaction Of Chlorine With Cold And With Hot Aqueous Sodium Hydroxide And Recognise These As Disproportionation Reactions

Group 17: The Reactions Of Chlorine: Explain, Including By Use Of An Equation, The Use Of Chlorine In Water Purification To Include The Production Of The Active Species Hocl And Clo– Which Kill Bacteria

Nitrogen And Sulfur: Nitrogen And Sulfur: Explain The Lack Of Reactivity Of Nitrogen, With Reference To Triple Bond Strength And Lack Of Polarity

Nitrogen And Sulfur: Nitrogen And Sulfur: Describe And Explain: (A) The Basicity Of Ammonia, Using The Brønsted–lowry Theory (B) The Structure Of The Ammonium Ion And Its Formation By An Acid–base Reaction (C) The Displacement Of Ammonia From Ammonium Salts By An Acid–base Reaction

Nitrogen And Sulfur: Nitrogen And Sulfur: State And Explain The Natural And Man-made Occurrences Of Oxides Of Nitrogen And Their Catalytic Removal From The Exhaust Gases Of Internal Combustion Engines

Nitrogen And Sulfur: Nitrogen And Sulfur: Understand That Atmospheric Oxides Of Nitrogen (No And No2) Can React With Unburned Hydrocarbons To Form Peroxyacetyl Nitrate, Pan, Which Is A Component Of Photochemical Smog

Nitrogen And Sulfur: Nitrogen And Sulfur: Describe The Role Of No And No2 In The Formation Of Acid Rain Both Directly And In Their Catalytic Role In The Oxidation Of Atmospheric Sulfur Dioxide

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Define The Term Hydrocarbon As A Compound Made Up Of C And H Atoms Only

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That Alkanes Are Simple Hydrocarbons With No Functional Group

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Pages 29 And 30 Contain A Functional Group Which Dictates Their Physical And Chemical Properties

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound Stated In The Table On Pages 29 And 30

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules With Functional Groups Detailed In The Table On Pages 29 And 30, Up To Six Carbon Atoms (Six Plus Six For Esters, Straight Chains Only For Esters And Nitriles)

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Deduce The Molecular And/or Empirical Formula Of A Compound, Given Its Structural, Displayed Or Skeletal Formula

An Introduction To As Level Organic Chemistry: Characteristic Organic Reactions: Interpret And Use The Following Terminology Associated With Types Of Organic Compounds And Reactions: (A) Homologous Series (B) Saturated And Unsaturated (C) Homolytic And Heterolytic Fission (D) Free Radical, Initiation, Propagation, Termination (E) Nucleophile, Electrophile, Nucleophilic, Electrophilic (F) Addition, Substitution, Elimination, Hydrolysis, Condensation (G) Oxidation And Reduction (In Equations For Organic Redox Reactions, The Symbol [o] Can Be Used To Represent One Atom Of Oxygen From An Oxidising Agent And The Symbol [h] To Represent One Atom Of Hydrogen From A Reducing Agent)

An Introduction To As Level Organic Chemistry: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Free-radical Substitution (B) Electrophilic Addition (C) Nucleophilic Substitution (D) Nucleophilic Addition (In Organic Reaction Mechanisms, The Use Of Curly Arrows To Represent Movement Of Electron Pairs Is Expected; The Arrow Should Begin At A Bond Or A Lone Pair Of Electrons)

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe Organic Molecules As Either Straight-chained, Branched Or Cyclic

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe And Explain The Shape Of, And Bond Angles In, Molecules Containing Sp, Sp2 And Sp3 Hybridised Atoms

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe The Arrangement Of Σ And Π Bonds In Molecules Containing Sp, Sp2 And Sp3 Hybridised Atoms

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Understand And Use The Term Planar When Describing The Arrangement Of Atoms In Organic Molecules, For Example Ethene

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Structural Isomerism And Its Division Into Chain, Positional And Functional Group Isomerism

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Stereoisomerism And Its Division Into Geometrical (Cis/trans) And Optical Isomerism (Use Of E/z Nomenclature Is Acceptable But Is Not Required)

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Geometrical (Cis/trans) Isomerism In Alkenes, And Explain Its Origin In Terms Of Restricted Rotation Due To The Presence Of Π Bonds

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Explain What Is Meant By A Chiral Centre And That Such A Centre Gives Rise To Two Optical Isomers (Enantiomers) (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds, Or Nomenclature Such As Diastereoisomers Is Not Required.)

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Identify Chiral Centres And Geometrical (Cis/trans) Isomerism In A Molecule Of Given Structural Formula Including Cyclic Compounds

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Deduce The Possible Isomers For An Organic Molecule Of Known Molecular Formula

Hydrocarbons: Alkanes: Recall The Reactions (Reagents And Conditions) By Which Alkanes Can Be Produced: (A) Addition Of Hydrogen To An Alkene In A Hydrogenation Reaction, H2(G) And Pt/ni Catalyst And Heat (B) Cracking Of A Longer Chain Alkane, Heat With Al 2o3

Hydrocarbons: Alkanes: Describe: (A) The Complete And Incomplete Combustion Of Alkanes (B) The Free-radical Substitution Of Alkanes By Cl 2 Or Br2 In The Presence Of Ultraviolet Light, As Exemplified By The Reactions Of Ethane

Hydrocarbons: Alkanes: Describe The Mechanism Of Free-radical Substitution With Reference To The Initiation, Propagation And Termination Steps

Hydrocarbons: Alkanes: Suggest How Cracking Can Be Used To Obtain More Useful Alkanes And Alkenes Of Lower Mr From Heavier Crude Oil Fractions

Hydrocarbons: Alkanes: Understand The General Unreactivity Of Alkanes, Including Towards Polar Reagents In Terms Of The Strength Of The C–h Bonds And Their Relative Lack Of Polarity

Hydrocarbons: Alkanes: Recognise The Environmental Consequences Of Carbon Monoxide, Oxides Of Nitrogen And Unburnt Hydrocarbons Arising From The Combustion Of Alkanes In The Internal Combustion Engine And Of Their Catalytic Removal

Hydrocarbons: Alkenes: Recall The Reactions (Including Reagents And Conditions) By Which Alkenes Can Be Produced: (A) Elimination Of Hx From A Halogenoalkane By Ethanolic Naoh And Heat (B) Dehydration Of An Alcohol, By Using A Heated Catalyst (E.g. Al 2o3) Or A Concentrated Acid (E.g. Concentrated H2so4) (C) Cracking Of A Longer Chain Alkane

Hydrocarbons: Alkenes: Describe The Following Reactions Of Alkenes: (A) The Electrophilic Addition Of (I) Hydrogen In A Hydrogenation Reaction, H2(G) And Pt/ni Catalyst And Heat (Ii) Steam, H2o(G) And H3po4 Catalyst (Iii) A Hydrogen Halide, Hx(G), At Room Temperature (Iv) A Halogen, X2 (B) The Oxidation By Cold Dilute Acidified Kmno4 To Form The Diol (C) The Oxidation By Hot Concentrated Acidified Kmno4 Leading To The Rupture Of The Carbon–carbon Double Bond And The Identities Of The Subsequent Products To Determine The Position Of Alkene Linkages In Larger Molecules (D) Addition Polymerisation Exemplified By The Reactions Of Ethene And Propene

Hydrocarbons: Alkenes: Describe The Use Of Aqueous Bromine To Show The Presence Of A C=c Bond

Hydrocarbons: Alkenes: Describe The Mechanism Of Electrophilic Addition In Alkenes, Using Bromine/ethene And Hydrogen Bromide/propene As Examples

Hydrocarbons: Alkenes: Describe And Explain The Inductive Effects Of Alkyl Groups On The Stability Of Primary, Secondary And Tertiary Cations Formed During Electrophilic Addition (This Should Be Used To Explain Markovnikov Addition)

Halogen Compounds: Halogenoalkanes: Recall The Reactions (Reagents And Conditions) By Which Halogenoalkanes Can Be Produced: (A) The Free-radical Substitution Of Alkanes By Cl 2 Or Br2 In The Presence Of Ultraviolet Light, As Exemplified By The Reactions Of Ethane (B) Electrophilic Addition Of An Alkene With A Halogen, X2, Or Hydrogen Halide, Hx(G), At Room Temperature (C) Substitution Of An Alcohol, E.g. By Reaction With Hx(G); Or With Kcl And Concentrated H2so4 Or Concentrated H3po4; Or With Pcl 3 And Heat; Or With Pcl 5; Or With Socl 2

Halogen Compounds: Halogenoalkanes: Classify Halogenoalkanes Into Primary, Secondary And Tertiary

Halogen Compounds: Halogenoalkanes: Describe The Following Nucleophilic Substitution Reactions: (A) The Reaction With Naoh(Aq) And Heat To Produce An Alcohol (B) The Reaction With Kcn In Ethanol And Heat To Produce A Nitrile (C) The Reaction With Nh3 In Ethanol Heated Under Pressure To Produce An Amine (D)  The Reaction With Aqueous Silver Nitrate In Ethanol As A Method Of Identifying The Halogen Present As Exemplified By Bromoethane

Halogen Compounds: Halogenoalkanes: Describe The Elimination Reaction With Naoh In Ethanol And Heat To Produce An Alkene As Exemplified By Bromoethane

Halogen Compounds: Halogenoalkanes: Describe The Sn1 And Sn2 Mechanisms Of Nucleophilic Substitution In Halogenoalkanes Including The Inductive Effects Of Alkyl Groups

Halogen Compounds: Halogenoalkanes: Recall That Primary Halogenoalkanes Tend To React Via The Sn2 Mechanism; Tertiary Halogenoalkanes Via The Sn1 Mechanism; And Secondary Halogenoalkanes By A Mixture Of The Two, Depending On Structure

Halogen Compounds: Halogenoalkanes: Describe And Explain The Different Reactivities Of Halogenoalkanes (With Particular Reference To The Relative Strengths Of The C–x Bonds As Exemplified By The Reactions Of Halogenoalkanes With Aqueous Silver Nitrates)

Hydroxy Compounds: Alcohols: Recall The Reactions (Reagents And Conditions) By Which Alcohols Can Be Produced: (A) Electrophilic Addition Of Steam To An Alkene, H2o(G) And H3po4 Catalyst (B) Reaction Of Alkenes With Cold Dilute Acidified Potassium Manganate(Vii) To Form A Diol (C) Substitution Of A Halogenoalkane Using Naoh(Aq) And Heat (D) Reduction Of An Aldehyde Or Ketone Using Nabh4 Or Lialh4 (E) Reduction Of A Carboxylic Acid Using Lialh4 (F) Hydrolysis Of An Ester Using Dilute Acid Or Dilute Alkali And Heat

Hydroxy Compounds: Alcohols: Describe: (A) The Reaction With Oxygen (Combustion) (B) Substitution To Form Halogenoalkanes, E.g. By Reaction With Hx(G); Or With Kcl And Concentrated H2so4 Or Concentrated H3po4; Or With Pcl 3 And Heat; Or With Pcl 5; Or With Socl 2 (C) The Reaction With Na(S) (D) Oxidation With Acidified K2cr2o7 Or Acidified Kmno4 To: (I) Carbonyl Compounds By Distillation (Ii) Carboxylic Acids By Refluxing (Primary Alcohols Give Aldehydes Which Can Be Further Oxidised To Carboxylic Acids, Secondary Alcohols Give Ketones, Tertiary Alcohols Cannot Be Oxidised) (E) Dehydration To An Alkene, By Using A Heated Catalyst, E.g. Al 2o3 Or A Concentrated Acid (F) Formation Of Esters By Reaction With Carboxylic Acids And Concentrated H2so4 As Catalyst As Exemplified By Ethanol

Hydroxy Compounds: Alcohols: (A) Classify Alcohols As Primary, Secondary And Tertiary Alcohols, To Include Examples With More Than One Alcohol Group (B) State Characteristic Distinguishing Reactions, E.g. Mild Oxidation With Acidified K2cr2o7 , Colour Change From Orange To Green

Hydroxy Compounds: Alcohols: Deduce The Presence Of A Ch3ch(Oh)– Group In An Alcohol, Ch3ch(Oh)–r, From Its Reaction With Alkaline I2(Aq) To Form A Yellow Precipitate Of Tri-iodomethane And An Ion, Rco2 –

Hydroxy Compounds: Alcohols: Explain The Acidity Of Alcohols Compared With Water

Carbonyl Compounds: Aldehydes And Ketones: Recall The Reactions (Reagents And Conditions) By Which Aldehydes And Ketones Can Be Produced: (A) The Oxidation Of Primary Alcohols Using Acidified K2cr2o7 Or Acidified Kmno4 And Distillation To Produce Aldehydes (B) The Oxidation Of Secondary Alcohols Using Acidified K2cr2o7 Or Acidified Kmno4 And Distillation To Produce Ketones

Carbonyl Compounds: Aldehydes And Ketones: Describe: (A) The Reduction Of Aldehydes And Ketones Using Nabh4 Or Lialh4 To Produce Alcohols (B) The Reaction Of Aldehydes And Ketones With Hcn, Kcn As Catalyst, And Heat To Produce Hydroxynitriles As Exemplified By Ethanal And Propanone

Carbonyl Compounds: Aldehydes And Ketones: Describe The Mechanism Of The Nucleophilic Addition Reactions Of Hydrogen Cyanide With Aldehydes And Ketones In 17.1.2(B)

Carbonyl Compounds: Aldehydes And Ketones: Describe The Use Of 2,4-dinitrophenylhydrazine (2,4-dnph Reagent) To Detect The Presence Of Carbonyl Compounds

Carbonyl Compounds: Aldehydes And Ketones: Deduce The Nature (Aldehyde Or Ketone) Of An Unknown Carbonyl Compound From The Results Of Simple Tests (Fehling’s And Tollens’ Reagents; Ease Of Oxidation)

Carbonyl Compounds: Aldehydes And Ketones: Deduce The Presence Of A Ch3co– Group In An Aldehyde Or Ketone, Ch3co–r, From Its Reaction With Alkaline I2(Aq) To Form A Yellow Precipitate Of Tri-iodomethane And An Ion, Rco2 –

Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reactions By Which Carboxylic Acids Can Be Produced: (A) Oxidation Of Primary Alcohols And Aldehydes With Acidified K2cr2o7 Or Acidified Kmno4 And Refluxing (B) Hydrolysis Of Nitriles With Dilute Acid Or Dilute Alkali Followed By Acidification (C) Hydrolysis Of Esters With Dilute Acid Or Dilute Alkali And Heat Followed By Acidification

Carboxylic Acids And Derivatives: Carboxylic Acids: Describe: (A) The Redox Reaction With Reactive Metals To Produce A Salt And H2(G) (B) The Neutralisation Reaction With Alkalis To Produce A Salt And H2o(L ) (C) The Acid–base Reaction With Carbonates To Produce A Salt And H2o(L) And Co2(G) (D) Esterification With Alcohols With Concentrated H2so4 As Catalyst (E) Reduction By Lialh4 To Form A Primary Alcohol

Carboxylic Acids And Derivatives: Esters: Recall The Reaction (Reagents And Conditions) By Which Esters Can Be Produced: (A) The Condensation Reaction Between An Alcohol And A Carboxylic Acid With Concentrated H₂so₄ As Catalyst

Carboxylic Acids And Derivatives: Esters: Describe The Hydrolysis Of Esters By Dilute Acid And By Dilute Alkali And Heat

Nitrogen Compounds: Primary Amines: Recall The Reactions By Which Amines Can Be Produced: (A) Reaction Of A Halogenoalkane With Nh₃ In Ethanol Heated Under Pressure Classification Of Amines Will Not Be Tested At As Level.

Nitrogen Compounds: Nitriles And Hydroxynitriles: Recall The Reactions By Which Nitriles Can Be Produced: (A) Reaction Of A Halogenoalkane With Kcn In Ethanol And Heat

Nitrogen Compounds: Nitriles And Hydroxynitriles: Recall The Reactions By Which Hydroxynitriles Can Be Produced: (A) The Reaction Of Aldehydes And Ketones With Hcn, Kcn As Catalyst, And Heat

Nitrogen Compounds: Nitriles And Hydroxynitriles: Describe The Hydrolysis Of Nitriles With Dilute Acid Or Dilute Alkali Followed By Acidification To Produce A Carboxylic Acid

Polymerisation: Addition Polymerisation: Describe Addition Polymerisation As Exemplified By Poly(Ethene) And Poly(Chloroethene), Pvc

Polymerisation: Addition Polymerisation: Deduce The Repeat Unit Of An Addition Polymer Obtained From A Given Monomer

Polymerisation: Addition Polymerisation: Identify The Monomer(S) Present In A Given Section Of An Addition Polymer Molecule

Polymerisation: Addition Polymerisation: Recognise The Difficulty Of The Disposal Of Poly(Alkene)s, I.e. Non-biodegradability And Harmful Combustion Products

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

Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus

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

Analytical Techniques: Infrared Spectroscopy: Analyse An Infrared Spectrum Of A Simple Molecule To Identify Functional Groups (See The Data Section For The Functional Groups Required)

Analytical Techniques: Mass Spectrometry: Analyse Mass Spectra In Terms Of M/e Values And Isotopic Abundances (Knowledge Of The Working Of The Mass Spectrometer Is Not Required)

Analytical Techniques: Mass Spectrometry: Calculate The Relative Atomic Mass Of An Element Given The Relative Abundances Of Its Isotopes, Or Its Mass Spectrum

Analytical Techniques: Mass Spectrometry: Deduce The Molecular Mass Of An Organic Molecule From The Molecular Ion Peak In A Mass Spectrum

Analytical Techniques: Mass Spectrometry: Suggest The Identity Of Molecules Formed By Simple Fragmentation In A Given Mass Spectrum

Analytical Techniques: Mass Spectrometry: Deduce The Number Of Carbon Atoms, N, In A Compound Using The [m + 1]+ Peak And The Formula N = 100 × Abundance Of [m + 1]+ Ion 1.1 × Abundance Of M+ Ion

Analytical Techniques: Mass Spectrometry: Deduce The Presence Of Bromine And Chlorine Atoms In A Compound Using The [m + 2]+ Peak

Atomic Structure

Atoms, Molecules And Stoichiometry

Chemical Bonding

States of Matter

Chemical Energetics

Electrochemistry

Equilibria

Reaction Kinetics

The Periodic Table: Chemical Periodicity

Group 2

Group 17

Nitrogen And Sulfur

An Introduction To AS Level Organic Chemistry

Hydrocarbons

Halogen Compounds

Hydroxy Compounds

Carbonyl Compounds

Carboxylic Acids And Derivatives

Nitrogen Compounds

Polymerisation

Organic Synthesis

Analytical Techniques

Atomic Structure

Atoms, Molecules And Stoichiometry

Chemical Bonding

States of Matter

Chemical Energetics

Electrochemistry

Equilibria

Reaction Kinetics

The Periodic Table: Chemical Periodicity

Group 2

Group 17

Nitrogen And Sulfur

Hydrocarbons

Halogen Compounds

Hydroxy Compounds

Carbonyl Compounds

Carboxylic Acids And Derivatives

Nitrogen Compounds

Polymerisation

Organic Synthesis

Analytical Techniques

Quiz Atomic Structure

Atomic Structure: Particles In The Atom And Atomic Radius: Understand That Atoms Are Mostly Empty Space Surrounding A Very Small, Dense Nucleus That Contains Protons And Neutrons; Electrons Are Found In Shells In The Empty Space Around The Nucleus

Atomic Structure: Particles In The Atom And Atomic Radius: Identify And Describe Protons, Neutrons And Electrons In Terms Of Their Relative Charges And Relative Masses

Atomic Structure: Particles In The Atom And Atomic Radius: Understand The Terms Atomic And Proton Number; Mass And Nucleon Number

Atomic Structure: Particles In The Atom And Atomic Radius: Describe The Distribution Of Mass And Charge Within An Atom

Atomic Structure: Particles In The Atom And Atomic Radius: Describe The Behaviour Of Beams Of Protons, Neutrons And Electrons Moving At The Same Velocity In An Electric Field

Atomic Structure: Particles In The Atom And Atomic Radius: Determine The Numbers Of Protons, Neutrons And Electrons Present In Both Atoms And Ions Given Atomic Or Proton Number, Mass Or Nucleon Number And Charge

Atomic Structure: Particles In The Atom And Atomic Radius: State And Explain Qualitatively The Variations In Atomic Radius And Ionic Radius Across A Period And Down A Group

Atomic Structure: Isotopes: Define The Term Isotope In Terms Of Numbers Of Protons And Neutrons

Atomic Structure: Isotopes: Understand The Notation X Ya For Isotopes, Where X Is The Mass Or Nucleon Number And Y Is The Atomic Or Proton Number

Atomic Structure: Isotopes: State That And Explain Why Isotopes Of The Same Element Have The Same Chemical Properties

Atomic Structure: Isotopes: State That And Explain Why Isotopes Of The Same Element Have Different Physical Properties, Limited To Mass And Density

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Understand The Terms: • Shells, Sub-shells And Orbitals • Principal Quantum Number (N) • Ground State, Limited To Electronic Configuration

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe The Order Of Increasing Energy Of The Sub-shells Within The First Three Shells And The 4s And 4p Sub-shells

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe The Electronic Configurations To Include The Number Of Electrons In Each Shell, Sub-shell And Orbital

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Explain The Electronic Configurations In Terms Of Energy Of The Electrons And Inter-electron Repulsion

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Determine The Electronic Configuration Of Atoms And Ions Given The Atomic Or Proton Number And Charge, Using Either Of The Following Conventions: E.g. For Fe: 1s2 2s2 2p6 3s2 3p6 3d6 4s2 (Full Electronic Configuration) Or [ar] 3d6 4s2 (Shorthand Electronic Configuration)

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Understand And Use The Electrons In Boxes Notation E.g. For Fe: [ar]

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe And Sketch The Shapes Of S And P Orbitals

Atomic Structure: Electrons, Energy Levels And Atomic Orbitals: Describe A Free Radical As A Species With One Or More Unpaired Electrons

Atomic Structure: Ionisation Energy: Define And Use The Term First Ionisation Energy, Ie

Atomic Structure: Ionisation Energy: Construct Equations To Represent First, Second And Subsequent Ionisation Energies

Atomic Structure: Ionisation Energy: Identify And Explain The Trends In Ionisation Energies Across A Period And Down A Group Of The Periodic Table

Atomic Structure: Ionisation Energy: Identify And Explain The Variation In Successive Ionisation Energies Of An Element

Atomic Structure: Ionisation Energy: Understand That Ionisation Energies Are Due To The Attraction Between The Nucleus And The Outer Electron

Atomic Structure: Ionisation Energy: Explain The Factors Influencing The Ionisation Energies Of Elements In Terms Of Nuclear Charge, Atomic/ionic Radius, Shielding By Inner Shells And Sub-shells And Spin-pair Repulsion

Atomic Structure: Ionisation Energy: Deduce The Electronic Configurations Of Elements Using Successive Ionisation Energy Data

Atomic Structure: Ionisation Energy: Deduce The Position Of An Element In The Periodic Table Using Successive Ionisation Energy Data

Atoms, Molecules And Stoichiometry: Relative Masses Of Atoms And Molecules: Define The Unified Atomic Mass Unit As One Twelfth Of The Mass Of A Carbon-12 Atom

Atoms, Molecules And Stoichiometry: Relative Masses Of Atoms And Molecules: Define Relative Atomic Mass, Ar , Relative Isotopic Mass, Relative Molecular Mass, Mr , And Relative Formula Mass In Terms Of The Unified Atomic Mass Unit

Atoms, Molecules And Stoichiometry: The Mole And The Avogadro Constant: Define And Use The Term Mole In Terms Of The Avogadro Constant

Atoms, Molecules And Stoichiometry: Formulas: Write Formulas Of Ionic Compounds From Ionic Charges And Oxidation Numbers (Shown By A Roman Numeral), Including: (A) The Prediction Of Ionic Charge From The Position Of An Element In The Periodic Table (B) Recall Of The Names And Formulas For The Following Ions: No3 – , Co3 2–, So4 2–, Oh– , Nh4 + , Zn2+, Ag+ , Hco3 – , Po4 3–

Atoms, Molecules And Stoichiometry: Formulas: (A) Write And Construct Equations (Which Should Be Balanced), Including Ionic Equations (Which Should Not Include Spectator Ions) (B) Use Appropriate State Symbols In Equations

Atoms, Molecules And Stoichiometry: Formulas: Define And Use The Terms Empirical And Molecular Formula

Atoms, Molecules And Stoichiometry: Formulas: Understand And Use The Terms Anhydrous, Hydrated And Water Of Crystallisation

Atoms, Molecules And Stoichiometry: Formulas: Calculate Empirical And Molecular Formulas, Using Given Data

Atoms, Molecules And Stoichiometry: Reacting Masses And Volumes (Of Solutions And Gases): Perform Calculations Including Use Of The Mole Concept, Involving: (A) Reacting Masses (From Formulas And Equations) Including Percentage Yield Calculations (B) Volumes Of Gases (E.g. In The Burning Of Hydrocarbons) (C) Volumes And Concentrations Of Solutions (D) Limiting Reagent And Excess Reagent (When Performing Calculations, Candidates’ Answers Should Reflect The Number Of Significant Figures Given Or Asked For In The Question. When Rounding Up Or Down, Candidates Should Ensure That Significant Figures Are Neither Lost Unnecessarily Nor Used Beyond What Is Justified (See Also Mathematical Requirements Section).) (E) Deduce Stoichiometric Relationships From Calculations Such As Those In 2.4.1(A)–(D)

Chemical Bonding: Electronegativity And Bonding: Define Electronegativity As The Power Of An Atom To Attract Electrons To Itself

Chemical Bonding: Electronegativity And Bonding: Define Electronegativity As The Power Of An Atom To Attract Electrons To Itself

Chemical Bonding: Electronegativity And Bonding: Explain The Factors Influencing The Electronegativities Of The Elements In Terms Of Nuclear Charge, Atomic Radius And Shielding By Inner Shells And Sub-shells

Chemical Bonding: Electronegativity And Bonding: State And Explain The Trends In Electronegativity Across A Period And Down A Group Of The Periodic Table

Chemical Bonding: Electronegativity And Bonding: Use The Differences In Pauling Electronegativity Values To Predict The Formation Of Ionic And Covalent Bonds (The Presence Of Covalent Character In Some Ionic Compounds Will Not Be Assessed) (Pauling Electronegativity Values Will Be Given Where Necessary)

Chemical Bonding: Ionic Bonding: Define Ionic Bonding As The Electrostatic Attraction Between Oppositely Charged Ions (Positively Charged Cations And Negatively Charged Anions)

Chemical Bonding: Ionic Bonding: Describe Ionic Bonding Including The Examples Of Sodium Chloride, Magnesium Oxide And Calcium Fluoride

Chemical Bonding: Metallic Bonding: Define Metallic Bonding As The Electrostatic Attraction Between Positive Metal Ions And Delocalised Electrons

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: Define Covalent Bonding As Electrostatic Attraction Between The Nuclei Of Two Atoms And A Shared Pair Of Electrons (A) Describe Covalent Bonding In Molecules Including: • Hydrogen, H2 • Oxygen, O2 • Nitrogen, N2 • Chlorine, Cl 2 • Hydrogen Chloride, Hcl • Carbon Dioxide, Co2 • Ammonia, Nh3 • Methane, Ch4 • Ethane, C2h6 • Ethene, C2h4 (B) Understand That Elements In Period 3 Can Expand Their Octet Including In The Compounds Sulfur Dioxide, So2, Phosphorus Pentachloride, Pcl 5 , And Sulfur Hexafluoride, Sf6 (C) Describe Coordinate (Dative Covalent) Bonding, Including In The Reaction Between Ammonia And Hydrogen Chloride Gases To Form The Ammonium Ion, Nh4 + , And In The Al 2cl 6 Molecule

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: (A) Describe Covalent Bonds In Terms Of Orbital Overlap Giving Σ And Π Bonds: • Σ Bonds Are Formed By Direct Overlap Of Orbitals Between The Bonding Atoms • Π Bonds Are Formed By The Sideways Overlap Of Adjacent P Orbitals Above And Below The Σ Bond (B) Describe How The Σ And Π Bonds Form In Molecules Including H₂, C₂h₆, C₂h₄, Hcn And N₂ (C) Use The Concept Of Hybridisation To Describe Sp, Sp² And Sp³ Orbitals

Chemical Bonding: Covalent Bonding And Coordinate (Dative Covalent) Bonding: A) Define The Terms: • Bond Energy As The Energy Required To Break One Mole Of A Particular Covalent Bond In The Gaseous State • Bond Length As The Internuclear Distance Of Two Covalently Bonded Atoms (B) Use Bond Energy Values And The Concept Of Bond Length To Compare The Reactivity Of Covalent Molecules

Chemical Bonding: Shapes Of Molecules: State And Explain The Shapes Of, And Bond Angles In, Molecules By Using Vsepr Theory, Including As Simple Examples: • Bf3 (Trigonal Planar, 120°) • Co2 (Linear, 180°) • Ch4 (Tetrahedral, 109.5°) • Nh3 (Pyramidal, 107°) • H2o (Non-linear, 104.5°) • Sf6 (Octahedral, 90°) • Pf5 (Trigonal Bipyramidal, 120° And 90°)

Chemical Bonding: Shapes Of Molecules: Predict The Shapes Of, And Bond Angles In, Molecules And Ions Analogous To Those Specified In 3.5.1

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: (A) Describe Hydrogen Bonding, Limited To Molecules Containing N–h And O–h Groups, Including Ammonia And Water As Simple Examples (B) Use The Concept Of Hydrogen Bonding To Explain The Anomalous Properties Of H₂o (Ice And Water): • Its Relatively High Melting And Boiling Points • Its Relatively High Surface Tension • The Density Of The Solid Ice Compared With The Liquid Water

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: Use The Concept Of Electronegativity To Explain Bond Polarity And Dipole Moments Of Molecules

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: (A) Describe Van Der Waals’ Forces As The Intermolecular Forces Between Molecular Entities Other Than Those Due To Bond Formation, And Use The Term Van Der Waals’ Forces As A Generic Term To Describe All Intermolecular Forces (B) Describe The Types Of Van Der Waals’ Forces: • Instantaneous Dipole–induced Dipole (Id-id) Forces, Also Called London Dispersion Forces • Permanent Dipole–permanent Dipole (Pd-pd) Forces, Including Hydrogen Bonding (C) Describe Hydrogen Bonding And Understand That Hydrogen Bonding Is A Special Case Of Permanent Dipole–permanent Dipole Forces Between Molecules Where Hydrogen Is Bonded To A Highly Electronegative Atom

Chemical Bonding: Intermolecular Forces, Electronegativity And Bond Properties: State That, In General, Ionic, Covalent And Metallic Bonding Are Stronger Than Intermolecular Forces

Chemical Bonding: Dot-and-cross Diagrams: Use Dot-and-cross Diagrams To Illustrate Ionic, Covalent And Coordinate Bonding Including The Representation Of Any Compounds Stated In 3.4 And 3.5 (Dot-and-cross Diagrams May Include Species With Atoms Which Have An Expanded Octet Or Species With An Odd Number Of Electrons)

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: Explain The Origin Of Pressure In A Gas In Terms Of Collisions Between Gas Molecules And The Wall Of The Container

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: Understand That Ideal Gases Have Zero Particle Volume And No Intermolecular Forces Of Attraction

States Of Matter: The Gaseous State: Ideal And Real Gases And Pv = Nrt: State And Use The Ideal Gas Equation Pv = Nrt In Calculations, Including In The Determination Of Mr

States Of Matter: Bonding And Structure: Describe, In Simple Terms, The Lattice Structure Of A Crystalline Solid Which Is: (A) Giant Ionic, Including Sodium Chloride And Magnesium Oxide (B) Simple Molecular, Including Iodine, Buckminsterfullerene C60 And Ice (C) Giant Molecular, Including Silicon(Iv) Oxide, Graphite And Diamond (D) Giant Metallic, Including Copper

States Of Matter: Bonding And Structure: Describe, Interpret And Predict The Effect Of Different Types Of Structure And Bonding On The Physical Properties Of Substances, Including Melting Point, Boiling Point, Electrical Conductivity And Solubility

States Of Matter: Bonding And Structure: Deduce The Type Of Structure And Bonding Present In A Substance From Given Information

Chemical Energetics: Enthalpy Change, Δh: Understand That Chemical Reactions Are Accompanied By Enthalpy Changes And These Changes Can Be Exothermic (δh Is Negative) Or Endothermic (δh Is Positive)

Chemical Energetics: Enthalpy Change, Δh: Construct And Interpret A Reaction Pathway Diagram, In Terms Of The Enthalpy Change Of The Reaction And Of The Activation Energy

Chemical Energetics: Enthalpy Change, Δh: Define And Use The Terms: (A) Standard Conditions (This Syllabus Assumes That These Are 298k And 101kpa) Shown By ⦵ . (B) Enthalpy Change With Particular Reference To: Reaction, Δhr , Formation, Δhf , Combustion, Δhc , Neutralisation, Δhneut

Chemical Energetics: Enthalpy Change, Δh: Understand That Energy Transfers Occur During Chemical Reactions Because Of The Breaking And Making Of Chemical Bonds

Chemical Energetics: Enthalpy Change, Δh: Use Bond Energies (δh Positive, I.e. Bond Breaking) To Calculate Enthalpy Change Of Reaction, Δhr

Chemical Energetics: Enthalpy Change, Δh: Understand That Some Bond Energies Are Exact And Some Bond Energies Are Averages

Chemical Energetics: Enthalpy Change, Δh: Calculate Enthalpy Changes From Appropriate Experimental Results, Including The Use Of The Relationships Q = Mcδt And Δh = –mcδt/ N

Chemical Energetics: Hess’s Law: Apply Hess’s Law To Construct Simple Energy Cycles

Chemical Energetics: Hess’s Law: Carry Out Calculations Using Cycles And Relevant Energy Terms, Including: (A) Determining Enthalpy Changes That Cannot Be Found By Direct Experiment (B) Use Of Bond Energy Data

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Calculate Oxidation Numbers Of Elements In Compounds And Ions

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Use Changes In Oxidation Numbers To Help Balance Chemical Equations

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Explain And Use The Terms Redox, Oxidation, Reduction And Disproportionation In Terms Of Electron Transfer And Changes In Oxidation Number

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Explain And Use The Terms Oxidising Agent And Reducing Agent

Electrochemistry: Redox Processes: Electron Transfer And Changes In Oxidation Number (Oxidation State): Use A Roman Numeral To Indicate The Magnitude Of The Oxidation Number Of An Element

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: (A) Understand What Is Meant By A Reversible Reaction (B) Understand What Is Meant By Dynamic Equilibrium In Terms Of The Rate Of Forward And Reverse Reactions Being Equal And The Concentration Of Reactants And Products Remaining Constant (C) Understand The Need For A Closed System In Order To Establish Dynamic Equilibrium

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Define Le Chatelier’s Principle As: If A Change Is Made To A System At Dynamic Equilibrium, The Position Of Equilibrium Moves To Minimise This Change

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use Le Chatelier’s Principle To Deduce Qualitatively (From Appropriate Information) The Effects Of Changes In Temperature, Concentration, Pressure Or Presence Of A Catalyst On A System At Equilibrium

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Deduce Expressions For Equilibrium Constants In Terms Of Concentrations, Kc

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use The Terms Mole Fraction And Partial Pressure

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Deduce Expressions For Equilibrium Constants In Terms Of Partial Pressures, Kp (Use Of The Relationship Between Kp And Kc Is Not Required)

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Use The Kc And Kp Expressions To Carry Out Calculations (Such Calculations Will Not Require The Solving Of Quadratic Equations)

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Calculate The Quantities Present At Equilibrium, Given Appropriate Data

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: State Whether Changes In Temperature, Concentration Or Pressure Or The Presence Of A Catalyst Affect The Value Of The Equilibrium Constant For A Reaction

Equilibria: Chemical Equilibria: Reversible Reactions, Dynamic Equilibrium: Describe And Explain The Conditions Used In The Haber Process And The Contact Process, As Examples Of The Importance Of An Understanding Of Dynamic Equilibrium In The Chemical Industry And The Application Of Le Chatelier’s Principle

Brønsted–lowry Theory Of Acids And Bases: State The Names And Formulas Of The Common Acids, Limited To Hydrochloric Acid, Hcl, Sulfuric Acid, H2so4, Nitric Acid, Hno3, Ethanoic Acid, Ch3cooh

Brønsted–lowry Theory Of Acids And Bases: State The Names And Formulas Of The Common Alkalis, Limited To Sodium Hydroxide, Naoh, Potassium Hydroxide, Koh, Ammonia, Nh3

Brønsted–lowry Theory Of Acids And Bases: Describe The Brønsted–lowry Theory Of Acids And Bases

Brønsted–lowry Theory Of Acids And Bases: Describe Strong Acids And Strong Bases As Fully Dissociated In Aqueous Solution And Weak Acids And Weak Bases As Partially Dissociated In Aqueous Solution

Brønsted–lowry Theory Of Acids And Bases: Appreciate That Water Has Ph Of 7, Acid Solutions Ph Of Below 7 And Alkaline Solutions Ph Of Above 7

Brønsted–lowry Theory Of Acids And Bases: Explain Qualitatively The Differences In Behaviour Between Strong And Weak Acids Including The Reaction With A Reactive Metal And Difference In Ph Values By Use Of A Ph Meter, Universal Indicator Or Conductivity

Brønsted–lowry Theory Of Acids And Bases: Understand That Neutralisation Reactions Occur When H+ (Aq) And Oh– (Aq) Form H2o(L)

Brønsted–lowry Theory Of Acids And Bases: Understand That Salts Are Formed In Neutralisation Reactions

Brønsted–lowry Theory Of Acids And Bases: Sketch The Ph Titration Curves Of Titrations Using Combinations Of Strong And Weak Acids With Strong And Weak Alkalis

Brønsted–lowry Theory Of Acids And Bases: Select Suitable Indicators For Acid-alkali Titrations, Given Appropriate Data (Pka Values Will Not Be Used)

Reaction Kinetics: Rate Of Reaction: Explain And Use The Term Rate Of Reaction, Frequency Of Collisions, Effective Collisions And Non-effective Collisions

Reaction Kinetics: Rate Of Reaction: Explain Qualitatively, In Terms Of Frequency Of Effective Collisions, The Effect Of Concentration And Pressure Changes On The Rate Of A Reaction

Reaction Kinetics: Rate Of Reaction: Use Experimental Data To Calculate The Rate Of A Reaction

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Define Activation Energy, Ea, As The Minimum Energy Required For A Collision To Be Effective

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Sketch And Use The Boltzmann Distribution To Explain The Significance Of Activation Energy

Reaction Kinetics: Effect Of Temperature On Reaction Rates And The Concept Of Activation Energy: Explain Qualitatively, In Terms Both Of The Boltzmann Distribution And Of Frequency Of Effective Collisions, The Effect Of Temperature Change On The Rate Of A Reaction

Reaction Kinetics: Homogeneous And Heterogeneous Catalysts: Explain And Use The Terms Catalyst And Catalysis: (A) Explain That, In The Presence Of A Catalyst, A Reaction Has A Different Mechanism, I.e. One Of Lower Activation Energy (B) Explain This Catalytic Effect In Terms Of The Boltzmann Distribution (C) Construct And Interpret A Reaction Pathway Diagram, For A Reaction In The Presence And Absence Of An Effective Catalyst

The Periodic Table: Chemical Periodicity: Periodicity Of Physical Properties Of The Elements In Period 3: Describe Qualitatively (And Indicate The Periodicity In) The Variations In Atomic Radius, Ionic Radius, Melting Point And Electrical Conductivity Of The Elements

The Periodic Table: Chemical Periodicity: Periodicity Of Physical Properties Of The Elements In Period 3: Explain The Variation In Melting Point And Electrical Conductivity In Terms Of The Structure And Bonding Of The Elements

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, And Write Equations For, The Reactions Of The Elements With Oxygen (To Give Na2o, Mgo, Al 2o3, P4o10, So2), Chlorine (To Give Nacl, Mgcl 2, Alcl 3, Sicl 4, Pcl 5) And Water (Na And Mg Only)

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: State And Explain The Variation In The Oxidation Number Of The Oxides (Na2o, Mgo, Al 2o3, P4o10, So2 And So3 Only) And Chlorides (Nacl, Mgcl 2, Alcl 3, Sicl 4, Pcl 5 Only) In Terms Of Their Outer Shell (Valence Shell) Electrons

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, And Write Equations For, The Reactions, If Any, Of The Oxides Na2o, Mgo, Al 2o3, Sio2, P4o10, So2 And So3 With Water Including The Likely Phs Of The Solutions Obtained

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, Explain, And Write Equations For, The Acid/base Behaviour Of The Oxides Na2o, Mgo, Al 2o3, P4o10, So2 And So3 And The Hydroxides Naoh, Mg(Oh)2 And Al(Oh)3 Including, Where Relevant, Amphoteric Behaviour In Reactions With Acids And Bases (Sodium Hydroxide Only)

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Describe, Explain, And Write Equations For, The Reactions Of The Chlorides Nacl, Mgcl 2, Al Cl 3, Sicl 4, Pcl 5 With Water Including The Likely Phs Of The Solutions Obtained

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Explain The Variations And Trends In 9.2.2, 9.2.3, 9.2.4 And 9.2.5 In Terms Of Bonding And Electronegativity

The Periodic Table: Periodicity Of Chemical Properties Of The Elements In Period 3: Suggest The Types Of Chemical Bonding Present In The Chlorides And Oxides From Observations Of Their Chemical And Physical Properties

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Write Equations For, The Reactions Of The Elements With Oxygen, Water And Dilute Hydrochloric And Sulfuric Acids

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Write Equations For, The Thermal Decomposition Of The Nitrates And Carbonates, To Include The Trend In Thermal Stabilities

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: Describe, And Make Predictions From, The Trends In Physical And Chemical Properties Of The Elements Involved In The Reactions In 10.1.1 And The Compounds Involved In 10.1.2, 10.1.3 And 10.1.5

Group 2: Similarities And Trends In The Properties Of The Group 2 Metals, Magnesium To Barium, And Their Compounds: State The Variation In The Solubilities Of The Hydroxides And Sulfates

Group 17: Physical Properties Of The Group 17 Elements: Describe The Colours And The Trend In Volatility Of Chlorine, Bromine And Iodine

Group 17: Physical Properties Of The Group 17 Elements: Describe And Explain The Trend In The Bond Strength Of The Halogen Molecules

Group 17: Physical Properties Of The Group 17 Elements: Interpret The Volatility Of The Elements In Terms Of Instantaneous Dipole–induced Dipole Forces

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Relative Reactivity Of The Elements As Oxidising Agents

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Reactions Of The Elements With Hydrogen And Explain Their Relative Reactivity In These Reactions

Group 17: The Chemical Properties Of The Halogen Elements And The Hydrogen Halides: Describe The Relative Thermal Stabilities Of The Hydrogen Halides And Explain These In Terms Of Bond Strengths

Group 17: Some Reactions Of The Halide Ions: Describe The Relative Reactivity Of Halide Ions As Reducing Agents

Group 17: Some Reactions Of The Halide Ions: Describe And Explain The Reactions Of Halide Ions With: (A) Aqueous Silver Ions Followed By Aqueous Ammonia (The Formation And Formula Of The [ag(Nh3) 2] + Complex Is Not Required) (B) Concentrated Sulfuric Acid, To Include Balanced Chemical Equations

Group 17: The Reactions Of Chlorine: Describe And Interpret, In Terms Of Changes In Oxidation Number, The Reaction Of Chlorine With Cold And With Hot Aqueous Sodium Hydroxide And Recognise These As Disproportionation Reactions

Group 17: The Reactions Of Chlorine: Explain, Including By Use Of An Equation, The Use Of Chlorine In Water Purification To Include The Production Of The Active Species Hocl And Clo– Which Kill Bacteria

Nitrogen And Sulfur: Nitrogen And Sulfur: Explain The Lack Of Reactivity Of Nitrogen, With Reference To Triple Bond Strength And Lack Of Polarity

Nitrogen And Sulfur: Nitrogen And Sulfur: Describe And Explain: (A) The Basicity Of Ammonia, Using The Brønsted–lowry Theory (B) The Structure Of The Ammonium Ion And Its Formation By An Acid–base Reaction (C) The Displacement Of Ammonia From Ammonium Salts By An Acid–base Reaction

Nitrogen And Sulfur: Nitrogen And Sulfur: State And Explain The Natural And Man-made Occurrences Of Oxides Of Nitrogen And Their Catalytic Removal From The Exhaust Gases Of Internal Combustion Engines

Nitrogen And Sulfur: Nitrogen And Sulfur: Understand That Atmospheric Oxides Of Nitrogen (No And No2) Can React With Unburned Hydrocarbons To Form Peroxyacetyl Nitrate, Pan, Which Is A Component Of Photochemical Smog

Nitrogen And Sulfur: Nitrogen And Sulfur: Describe The Role Of No And No2 In The Formation Of Acid Rain Both Directly And In Their Catalytic Role In The Oxidation Of Atmospheric Sulfur Dioxide

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Define The Term Hydrocarbon As A Compound Made Up Of C And H Atoms Only

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That Alkanes Are Simple Hydrocarbons With No Functional Group

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand That The Compounds In The Table On Pages 29 And 30 Contain A Functional Group Which Dictates Their Physical And Chemical Properties

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Interpret And Use The General, Structural, Displayed And Skeletal Formulas Of The Classes Of Compound Stated In The Table On Pages 29 And 30

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Understand And Use Systematic Nomenclature Of Simple Aliphatic Organic Molecules With Functional Groups Detailed In The Table On Pages 29 And 30, Up To Six Carbon Atoms (Six Plus Six For Esters, Straight Chains Only For Esters And Nitriles)

An Introduction To As Level Organic Chemistry: Formulas, Functional Groups And The Naming Of Organic Compounds: Deduce The Molecular And/or Empirical Formula Of A Compound, Given Its Structural, Displayed Or Skeletal Formula

An Introduction To As Level Organic Chemistry: Characteristic Organic Reactions: Interpret And Use The Following Terminology Associated With Types Of Organic Compounds And Reactions: (A) Homologous Series (B) Saturated And Unsaturated (C) Homolytic And Heterolytic Fission (D) Free Radical, Initiation, Propagation, Termination (E) Nucleophile, Electrophile, Nucleophilic, Electrophilic (F) Addition, Substitution, Elimination, Hydrolysis, Condensation (G) Oxidation And Reduction (In Equations For Organic Redox Reactions, The Symbol [o] Can Be Used To Represent One Atom Of Oxygen From An Oxidising Agent And The Symbol [h] To Represent One Atom Of Hydrogen From A Reducing Agent)

An Introduction To As Level Organic Chemistry: Characteristic Organic Reactions: Understand And Use The Following Terminology Associated With Types Of Organic Mechanisms: (A) Free-radical Substitution (B) Electrophilic Addition (C) Nucleophilic Substitution (D) Nucleophilic Addition (In Organic Reaction Mechanisms, The Use Of Curly Arrows To Represent Movement Of Electron Pairs Is Expected; The Arrow Should Begin At A Bond Or A Lone Pair Of Electrons)

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe Organic Molecules As Either Straight-chained, Branched Or Cyclic

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe And Explain The Shape Of, And Bond Angles In, Molecules Containing Sp, Sp2 And Sp3 Hybridised Atoms

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Describe The Arrangement Of Σ And Π Bonds In Molecules Containing Sp, Sp2 And Sp3 Hybridised Atoms

An Introduction To As Level Organic Chemistry: Shapes Of Organic Molecules; Σ And Π Bonds: Understand And Use The Term Planar When Describing The Arrangement Of Atoms In Organic Molecules, For Example Ethene

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Structural Isomerism And Its Division Into Chain, Positional And Functional Group Isomerism

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Stereoisomerism And Its Division Into Geometrical (Cis/trans) And Optical Isomerism (Use Of E/z Nomenclature Is Acceptable But Is Not Required)

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Describe Geometrical (Cis/trans) Isomerism In Alkenes, And Explain Its Origin In Terms Of Restricted Rotation Due To The Presence Of Π Bonds

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Explain What Is Meant By A Chiral Centre And That Such A Centre Gives Rise To Two Optical Isomers (Enantiomers) (Candidates Should Appreciate That Compounds Can Contain More Than One Chiral Centre, But Knowledge Of Meso Compounds, Or Nomenclature Such As Diastereoisomers Is Not Required.)

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Identify Chiral Centres And Geometrical (Cis/trans) Isomerism In A Molecule Of Given Structural Formula Including Cyclic Compounds

An Introduction To As Level Organic Chemistry: Isomerism: Structural Isomerism And Stereoisomerism: Deduce The Possible Isomers For An Organic Molecule Of Known Molecular Formula

Hydrocarbons: Alkanes: Recall The Reactions (Reagents And Conditions) By Which Alkanes Can Be Produced: (A) Addition Of Hydrogen To An Alkene In A Hydrogenation Reaction, H2(G) And Pt/ni Catalyst And Heat (B) Cracking Of A Longer Chain Alkane, Heat With Al 2o3

Hydrocarbons: Alkanes: Describe: (A) The Complete And Incomplete Combustion Of Alkanes (B) The Free-radical Substitution Of Alkanes By Cl 2 Or Br2 In The Presence Of Ultraviolet Light, As Exemplified By The Reactions Of Ethane

Hydrocarbons: Alkanes: Describe The Mechanism Of Free-radical Substitution With Reference To The Initiation, Propagation And Termination Steps

Hydrocarbons: Alkanes: Suggest How Cracking Can Be Used To Obtain More Useful Alkanes And Alkenes Of Lower Mr From Heavier Crude Oil Fractions

Hydrocarbons: Alkanes: Understand The General Unreactivity Of Alkanes, Including Towards Polar Reagents In Terms Of The Strength Of The C–h Bonds And Their Relative Lack Of Polarity

Hydrocarbons: Alkanes: Recognise The Environmental Consequences Of Carbon Monoxide, Oxides Of Nitrogen And Unburnt Hydrocarbons Arising From The Combustion Of Alkanes In The Internal Combustion Engine And Of Their Catalytic Removal

Hydrocarbons: Alkenes: Recall The Reactions (Including Reagents And Conditions) By Which Alkenes Can Be Produced: (A) Elimination Of Hx From A Halogenoalkane By Ethanolic Naoh And Heat (B) Dehydration Of An Alcohol, By Using A Heated Catalyst (E.g. Al 2o3) Or A Concentrated Acid (E.g. Concentrated H2so4) (C) Cracking Of A Longer Chain Alkane

Hydrocarbons: Alkenes: Describe The Following Reactions Of Alkenes: (A) The Electrophilic Addition Of (I) Hydrogen In A Hydrogenation Reaction, H2(G) And Pt/ni Catalyst And Heat (Ii) Steam, H2o(G) And H3po4 Catalyst (Iii) A Hydrogen Halide, Hx(G), At Room Temperature (Iv) A Halogen, X2 (B) The Oxidation By Cold Dilute Acidified Kmno4 To Form The Diol (C) The Oxidation By Hot Concentrated Acidified Kmno4 Leading To The Rupture Of The Carbon–carbon Double Bond And The Identities Of The Subsequent Products To Determine The Position Of Alkene Linkages In Larger Molecules (D) Addition Polymerisation Exemplified By The Reactions Of Ethene And Propene

Hydrocarbons: Alkenes: Describe The Use Of Aqueous Bromine To Show The Presence Of A C=c Bond

Hydrocarbons: Alkenes: Describe The Mechanism Of Electrophilic Addition In Alkenes, Using Bromine/ethene And Hydrogen Bromide/propene As Examples

Hydrocarbons: Alkenes: Describe And Explain The Inductive Effects Of Alkyl Groups On The Stability Of Primary, Secondary And Tertiary Cations Formed During Electrophilic Addition (This Should Be Used To Explain Markovnikov Addition)

Halogen Compounds: Halogenoalkanes: Recall The Reactions (Reagents And Conditions) By Which Halogenoalkanes Can Be Produced: (A) The Free-radical Substitution Of Alkanes By Cl 2 Or Br2 In The Presence Of Ultraviolet Light, As Exemplified By The Reactions Of Ethane (B) Electrophilic Addition Of An Alkene With A Halogen, X2, Or Hydrogen Halide, Hx(G), At Room Temperature (C) Substitution Of An Alcohol, E.g. By Reaction With Hx(G); Or With Kcl And Concentrated H2so4 Or Concentrated H3po4; Or With Pcl 3 And Heat; Or With Pcl 5; Or With Socl 2

Halogen Compounds: Halogenoalkanes: Classify Halogenoalkanes Into Primary, Secondary And Tertiary

Halogen Compounds: Halogenoalkanes: Describe The Following Nucleophilic Substitution Reactions: (A) The Reaction With Naoh(Aq) And Heat To Produce An Alcohol (B) The Reaction With Kcn In Ethanol And Heat To Produce A Nitrile (C) The Reaction With Nh3 In Ethanol Heated Under Pressure To Produce An Amine (D)  The Reaction With Aqueous Silver Nitrate In Ethanol As A Method Of Identifying The Halogen Present As Exemplified By Bromoethane

Halogen Compounds: Halogenoalkanes: Describe The Elimination Reaction With Naoh In Ethanol And Heat To Produce An Alkene As Exemplified By Bromoethane

Halogen Compounds: Halogenoalkanes: Describe The Sn1 And Sn2 Mechanisms Of Nucleophilic Substitution In Halogenoalkanes Including The Inductive Effects Of Alkyl Groups

Halogen Compounds: Halogenoalkanes: Recall That Primary Halogenoalkanes Tend To React Via The Sn2 Mechanism; Tertiary Halogenoalkanes Via The Sn1 Mechanism; And Secondary Halogenoalkanes By A Mixture Of The Two, Depending On Structure

Halogen Compounds: Halogenoalkanes: Describe And Explain The Different Reactivities Of Halogenoalkanes (With Particular Reference To The Relative Strengths Of The C–x Bonds As Exemplified By The Reactions Of Halogenoalkanes With Aqueous Silver Nitrates)

Hydroxy Compounds: Alcohols: Recall The Reactions (Reagents And Conditions) By Which Alcohols Can Be Produced: (A) Electrophilic Addition Of Steam To An Alkene, H2o(G) And H3po4 Catalyst (B) Reaction Of Alkenes With Cold Dilute Acidified Potassium Manganate(Vii) To Form A Diol (C) Substitution Of A Halogenoalkane Using Naoh(Aq) And Heat (D) Reduction Of An Aldehyde Or Ketone Using Nabh4 Or Lialh4 (E) Reduction Of A Carboxylic Acid Using Lialh4 (F) Hydrolysis Of An Ester Using Dilute Acid Or Dilute Alkali And Heat

Hydroxy Compounds: Alcohols: Describe: (A) The Reaction With Oxygen (Combustion) (B) Substitution To Form Halogenoalkanes, E.g. By Reaction With Hx(G); Or With Kcl And Concentrated H2so4 Or Concentrated H3po4; Or With Pcl 3 And Heat; Or With Pcl 5; Or With Socl 2 (C) The Reaction With Na(S) (D) Oxidation With Acidified K2cr2o7 Or Acidified Kmno4 To: (I) Carbonyl Compounds By Distillation (Ii) Carboxylic Acids By Refluxing (Primary Alcohols Give Aldehydes Which Can Be Further Oxidised To Carboxylic Acids, Secondary Alcohols Give Ketones, Tertiary Alcohols Cannot Be Oxidised) (E) Dehydration To An Alkene, By Using A Heated Catalyst, E.g. Al 2o3 Or A Concentrated Acid (F) Formation Of Esters By Reaction With Carboxylic Acids And Concentrated H2so4 As Catalyst As Exemplified By Ethanol

Hydroxy Compounds: Alcohols: (A) Classify Alcohols As Primary, Secondary And Tertiary Alcohols, To Include Examples With More Than One Alcohol Group (B) State Characteristic Distinguishing Reactions, E.g. Mild Oxidation With Acidified K2cr2o7 , Colour Change From Orange To Green

Hydroxy Compounds: Alcohols: Deduce The Presence Of A Ch3ch(Oh)– Group In An Alcohol, Ch3ch(Oh)–r, From Its Reaction With Alkaline I2(Aq) To Form A Yellow Precipitate Of Tri-iodomethane And An Ion, Rco2 –

Hydroxy Compounds: Alcohols: Explain The Acidity Of Alcohols Compared With Water

Carbonyl Compounds: Aldehydes And Ketones: Recall The Reactions (Reagents And Conditions) By Which Aldehydes And Ketones Can Be Produced: (A) The Oxidation Of Primary Alcohols Using Acidified K2cr2o7 Or Acidified Kmno4 And Distillation To Produce Aldehydes (B) The Oxidation Of Secondary Alcohols Using Acidified K2cr2o7 Or Acidified Kmno4 And Distillation To Produce Ketones

Carbonyl Compounds: Aldehydes And Ketones: Describe: (A) The Reduction Of Aldehydes And Ketones Using Nabh4 Or Lialh4 To Produce Alcohols (B) The Reaction Of Aldehydes And Ketones With Hcn, Kcn As Catalyst, And Heat To Produce Hydroxynitriles As Exemplified By Ethanal And Propanone

Carbonyl Compounds: Aldehydes And Ketones: Describe The Mechanism Of The Nucleophilic Addition Reactions Of Hydrogen Cyanide With Aldehydes And Ketones In 17.1.2(B)

Carbonyl Compounds: Aldehydes And Ketones: Describe The Use Of 2,4-dinitrophenylhydrazine (2,4-dnph Reagent) To Detect The Presence Of Carbonyl Compounds

Carbonyl Compounds: Aldehydes And Ketones: Deduce The Nature (Aldehyde Or Ketone) Of An Unknown Carbonyl Compound From The Results Of Simple Tests (Fehling’s And Tollens’ Reagents; Ease Of Oxidation)

Carbonyl Compounds: Aldehydes And Ketones: Deduce The Presence Of A Ch3co– Group In An Aldehyde Or Ketone, Ch3co–r, From Its Reaction With Alkaline I2(Aq) To Form A Yellow Precipitate Of Tri-iodomethane And An Ion, Rco2 –

Carboxylic Acids And Derivatives: Carboxylic Acids: Recall The Reactions By Which Carboxylic Acids Can Be Produced: (A) Oxidation Of Primary Alcohols And Aldehydes With Acidified K2cr2o7 Or Acidified Kmno4 And Refluxing (B) Hydrolysis Of Nitriles With Dilute Acid Or Dilute Alkali Followed By Acidification (C) Hydrolysis Of Esters With Dilute Acid Or Dilute Alkali And Heat Followed By Acidification

Carboxylic Acids And Derivatives: Carboxylic Acids: Describe: (A) The Redox Reaction With Reactive Metals To Produce A Salt And H2(G) (B) The Neutralisation Reaction With Alkalis To Produce A Salt And H2o(L ) (C) The Acid–base Reaction With Carbonates To Produce A Salt And H2o(L) And Co2(G) (D) Esterification With Alcohols With Concentrated H2so4 As Catalyst (E) Reduction By Lialh4 To Form A Primary Alcohol

Carboxylic Acids And Derivatives: Esters: Recall The Reaction (Reagents And Conditions) By Which Esters Can Be Produced: (A) The Condensation Reaction Between An Alcohol And A Carboxylic Acid With Concentrated H₂so₄ As Catalyst

Carboxylic Acids And Derivatives: Esters: Describe The Hydrolysis Of Esters By Dilute Acid And By Dilute Alkali And Heat

Nitrogen Compounds: Primary Amines: Recall The Reactions By Which Amines Can Be Produced: (A) Reaction Of A Halogenoalkane With Nh₃ In Ethanol Heated Under Pressure Classification Of Amines Will Not Be Tested At As Level.

Nitrogen Compounds: Nitriles And Hydroxynitriles: Recall The Reactions By Which Nitriles Can Be Produced: (A) Reaction Of A Halogenoalkane With Kcn In Ethanol And Heat

Nitrogen Compounds: Nitriles And Hydroxynitriles: Recall The Reactions By Which Hydroxynitriles Can Be Produced: (A) The Reaction Of Aldehydes And Ketones With Hcn, Kcn As Catalyst, And Heat

Nitrogen Compounds: Nitriles And Hydroxynitriles: Describe The Hydrolysis Of Nitriles With Dilute Acid Or Dilute Alkali Followed By Acidification To Produce A Carboxylic Acid

Polymerisation: Addition Polymerisation: Describe Addition Polymerisation As Exemplified By Poly(Ethene) And Poly(Chloroethene), Pvc

Polymerisation: Addition Polymerisation: Deduce The Repeat Unit Of An Addition Polymer Obtained From A Given Monomer

Polymerisation: Addition Polymerisation: Identify The Monomer(S) Present In A Given Section Of An Addition Polymer Molecule

Polymerisation: Addition Polymerisation: Recognise The Difficulty Of The Disposal Of Poly(Alkene)s, I.e. Non-biodegradability And Harmful Combustion Products

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

Organic Synthesis: Organic Synthesis: Devise Multi-step Synthetic Routes For Preparing Organic Molecules Using The Reactions In The Syllabus

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

Analytical Techniques: Infrared Spectroscopy: Analyse An Infrared Spectrum Of A Simple Molecule To Identify Functional Groups (See The Data Section For The Functional Groups Required)

Analytical Techniques: Mass Spectrometry: Analyse Mass Spectra In Terms Of M/e Values And Isotopic Abundances (Knowledge Of The Working Of The Mass Spectrometer Is Not Required)

Analytical Techniques: Mass Spectrometry: Calculate The Relative Atomic Mass Of An Element Given The Relative Abundances Of Its Isotopes, Or Its Mass Spectrum

Analytical Techniques: Mass Spectrometry: Deduce The Molecular Mass Of An Organic Molecule From The Molecular Ion Peak In A Mass Spectrum

Analytical Techniques: Mass Spectrometry: Suggest The Identity Of Molecules Formed By Simple Fragmentation In A Given Mass Spectrum

Analytical Techniques: Mass Spectrometry: Deduce The Number Of Carbon Atoms, N, In A Compound Using The [m + 1]+ Peak And The Formula N = 100 × Abundance Of [m + 1]+ Ion 1.1 × Abundance Of M+ Ion

Analytical Techniques: Mass Spectrometry: Deduce The Presence Of Bromine And Chlorine Atoms In A Compound Using The [m + 2]+ Peak

Atomic Structure

Atoms, Molecules And Stoichiometry

Chemical Bonding

States of Matter

Chemical Energetics

Electrochemistry

Equilibria

Reaction Kinetics

The Periodic Table: Chemistry Periodicity

Group 2

Group 17

Nitrogen And Sulfur

An Introduction To AS Level Organic Chemistry

Hydrocarbons

Halogen Compounds

Hydroxy Compounds

Carbonyl Compounds

Carboxylic Acids And Derivatives

Nitrogen Compounds

Polymerisation

Organic Synthesis

Analytical Techniques

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Complete Breakdown Of AS Level Chemistry Papers (Paper 1, Paper 2, Paper 3)

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Marks Distribution And Weightage Across Papers (AO1, AO2, AO3 Focus)

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Time Allocation Strategy For Each Paper

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): How Cambridge Designs Questions From Learning Outcomes

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Understanding Command Words And What Examiners Actually Want

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Difference Between Knowledge Marks And Application Marks

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): Examiner Language Vs Student Language (Why Answers Get Capped)

Understanding The AS Level Chemistry Paper Structure (Paper Intelligence): How Mark Schemes Are Applied Positively (Not Deductively)

Paper 1 (MCQs) — Pattern, Strategy & Traps: Paper 1 Question Styles And Recurring MCQ Patterns

Paper 1 (MCQs) — Pattern, Strategy & Traps: Elimination Technique For Difficult MCQs

Paper 1 (MCQs) — Pattern, Strategy & Traps: Common Calculation Traps In MCQs (Units, Ratios, Logs, pH)

Paper 1 (MCQs) — Pattern, Strategy & Traps: Misleading Options: How Cambridge Designs Wrong Answers

Paper 1 (MCQs) — Pattern, Strategy & Traps: Data Booklet Usage Strategy In MCQs

Paper 1 (MCQs) — Pattern, Strategy & Traps: Handling Organic Reaction MCQs Without Full Working

Paper 1 (MCQs) — Pattern, Strategy & Traps: Speed Vs Accuracy: The Ideal MCQ Attempt Order

Paper 1 (MCQs) — Pattern, Strategy & Traps: Most Common MCQ Mistakes Reported By Examiners

Paper 2 (Structured Questions) — High-Scoring Techniques: How Structured Questions Are Layered (Easy → Trap → Discriminator)

Paper 2 (Structured Questions) — High-Scoring Techniques: Writing Chemical Equations The Examiner Accepts

Paper 2 (Structured Questions) — High-Scoring Techniques: Calculation Layout That Secures Full Working Marks

Paper 2 (Structured Questions) — High-Scoring Techniques: Significant Figures, Units And Penalty Errors

Paper 2 (Structured Questions) — High-Scoring Techniques: Explaining Trends Using Correct Chemical Language

Paper 2 (Structured Questions) — High-Scoring Techniques: Organic Mechanism Diagrams: What Loses Marks Instantly

Paper 2 (Structured Questions) — High-Scoring Techniques: Data Interpretation Questions: Graphs, Tables, Unknowns

Paper 2 (Structured Questions) — High-Scoring Techniques: How To Answer “Explain” Vs “Describe” Vs “Deduce”

Paper 2 (Structured Questions) — High-Scoring Techniques: Common Paper 2 Mistakes That Drop Students One Grade

Paper 3 (Practical Skills) — Reality Vs Myth: Actual Structure Of Paper 3 (Not What Students Assume)

Paper 3 (Practical Skills) — Reality Vs Myth: Planning Questions: What Must Be Written Vs What Is Wasted

Paper 3 (Practical Skills) — Reality Vs Myth: Recording Observations The Cambridge Way

Paper 3 (Practical Skills) — Reality Vs Myth: Processing Data And Graph Drawing Rules

Paper 3 (Practical Skills) — Reality Vs Myth: Error, Uncertainty And Improvement Questions Demystified

Paper 3 (Practical Skills) — Reality Vs Myth: Why “Human Error” Is Penalised

Paper 3 (Practical Skills) — Reality Vs Myth: Evaluation Questions That Look Easy But Destroy Marks

Paper 3 (Practical Skills) — Reality Vs Myth: Most Repeated Practical Mistakes From Examiner Reports

Calculation Mastery & Mathematical Technique: Mole Calculations That Cause Maximum Failure

Calculation Mastery & Mathematical Technique: pH, Ka, Kc, Kp And Log Errors Students Repeat Every Year

Calculation Mastery & Mathematical Technique: Thermochemistry Calculations: Where Marks Are Actually Lost

Calculation Mastery & Mathematical Technique: Electrochemistry Calculations And Sign Convention Errors

Calculation Mastery & Mathematical Technique: Rate Equations And Half-Life Traps

Calculation Mastery & Mathematical Technique: When Rounding Costs You Marks (And When It Doesn’t)

Organic Chemistry Answering Strategy: Writing Organic Reactions Without Over-Writing

Organic Chemistry Answering Strategy: Mechanisms: How Much Detail Is Enough

Organic Chemistry Answering Strategy: Multi-Step Organic Synthesis: Planning Before Writing

Organic Chemistry Answering Strategy: Functional Group Tests: Precision Vs Guessing

Organic Chemistry Answering Strategy: Common Organic Misconceptions Examiners Flag

Exam-Day Intelligence & Final Preparation: Order Of Attempting Questions For Maximum Score

Exam-Day Intelligence & Final Preparation: When To Skip, When To Return, When To Commit

Exam-Day Intelligence & Final Preparation: How To Use The Last 10 Minutes Effectively

Exam-Day Intelligence & Final Preparation: Presentation, Cross-Outs, Extra Booklets — What’s Allowed

Exam-Day Intelligence & Final Preparation: Examiner Red Flags That Instantly Cap Marks

Exam-Day Intelligence & Final Preparation: Final 7-Day Revision Strategy Based On Past Paper Trends

Atomic Structure

Atoms, Molecules And Stoichiometry

Chemical Bonding

States of Matter

Chemical Energetics

Electrochemistry

Equilibria

Reaction Kinetics

The Periodic Table: Chemical Periodicity

Group 2

Group 17

Nitrogen And Sulfur

An Introduction To AS Level Organic Chemistry

Hydrocarbons

Halogen Compounds

Hydroxy Compounds

Carbonyl Compounds

Carboxylic Acids And Derivatives

Nitrogen Compounds

Polymerisation

Organic Synthesis

Analytical Techniques

Formulae Sheet: Fundamental Quantities & Constants: SI Units, Prefixes And Powers Of Ten Used In Chemistry

Formulae Sheet: Fundamental Quantities & Constants: Avogadro Constant And Its Applications

Formulae Sheet: Fundamental Quantities & Constants: Relative Atomic Mass (Aᵣ) And Relative Molecular Mass (Mᵣ)

Formulae Sheet: Fundamental Quantities & Constants: Molar Mass, Moles And Amount Of Substance

Formulae Sheet: Fundamental Quantities & Constants: Density Formula And Rearrangements

Formulae Sheet: Fundamental Quantities & Constants: Percentage Composition By Mass

Formulae Sheet: Empirical Formula And Molecular Formula Relationships

Formulae Sheet: Stoichiometry & Chemical Calculations: Mole Ratio Calculations From Balanced Equations

Formulae Sheet: Stoichiometry & Chemical Calculations: Limiting Reagent Calculations

Formulae Sheet: Stoichiometry & Chemical Calculations: Percentage Yield Formula

Formulae Sheet: Stoichiometry & Chemical Calculations: Percentage Purity Formula

Formulae Sheet: Stoichiometry & Chemical Calculations: Concentration In mol dm⁻³

Formulae Sheet: Stoichiometry & Chemical Calculations: Conversion Between Mass, Moles And Concentration

Formulae Sheet: Stoichiometry & Chemical Calculations: Dilution Formula (C₁V₁ = C₂V₂)

Formulae Sheet: Stoichiometry & Chemical Calculations: Gas Volume Calculations At r.t.p. (24.0 dm³ mol⁻¹)

Formulae Sheet: Atomic Structure & Periodicity Formulae: Proton, Neutron And Electron Relationships

Formulae Sheet: Atomic Structure & Periodicity Formulae: Isotopic Abundance And Weighted Mean Formula

Formulae Sheet: Atomic Structure & Periodicity Formulae: Mass Spectrometry Calculations

Formulae Sheet: Atomic Structure & Periodicity Formulae: Ionisation Energy Calculations (Conceptual + Numerical Links)

Formulae Sheet: Chemical Bonding & Structure (Quantitative Parts): Enthalpy And Bond Energy Relationships

Formulae Sheet: Chemical Bonding & Structure (Quantitative Parts): Bond Enthalpy Calculations

Formulae Sheet: Chemical Bonding & Structure (Quantitative Parts): Enthalpy Change Of Reaction From Bond Energies

Formulae Sheet: Chemical Bonding & Structure (Quantitative Parts): Lattice Energy (Conceptual Formula Links Only – AS Level)

Formulae Sheet: States Of Matter & Gas Laws: Ideal Gas Equation: pV = nRT

Formulae Sheet: States Of Matter & Gas Laws: Rearrangements Of The Ideal Gas Equation

Formulae Sheet: States Of Matter & Gas Laws: Unit Conversions For Pressure, Volume And Temperature

Formulae Sheet: States Of Matter & Gas Laws: Gas Density Formula Derived From pV = nRT

Formulae Sheet: Chemical Energetics: Enthalpy Change Definition Formula (ΔH)

Formulae Sheet: Chemical Energetics: Enthalpy Change From Temperature Change (q = mcΔT)

Formulae Sheet: Chemical Energetics: Hess’s Law Cycle Calculations

Formulae Sheet: Chemical Energetics: Enthalpy Of Formation Calculations

Formulae Sheet: Chemical Energetics: Enthalpy Of Combustion Calculations

Formulae Sheet: Chemical Energetics: Enthalpy Of Neutralisation Calculations

Formulae Sheet: Kinetics (Rates Of Reaction): Rate Of Reaction Formula

Formulae Sheet: Kinetics (Rates Of Reaction): Rate From Concentration–Time Graphs

Formulae Sheet: Kinetics (Rates Of Reaction): Rate From Tangents And Gradients

Formulae Sheet: Kinetics (Rates Of Reaction): Activation Energy Concepts Linked To Maxwell–Boltzmann

Formulae Sheet: Kinetics (Rates Of Reaction): Effect Of Concentration And Temperature (Quantitative Reasoning)

Formulae Sheet: Chemical Equilibria: Dynamic Equilibrium Expression

Formulae Sheet: Chemical Equilibria: Equilibrium Constant Kc Formula

Formulae Sheet: Chemical Equilibria: Writing Kc Expressions Correctly

Formulae Sheet: Chemical Equilibria: Calculating Kc From Equilibrium Concentrations

Formulae Sheet: Chemical Equilibria: Predicting Equilibrium Shifts (Le Chatelier — formula-linked logic)

Formulae Sheet: Acids, Bases & pH Calculations: pH Formula (pH = −log[H⁺])

Formulae Sheet: Acids, Bases & pH Calculations: Rearranging pH Formula To Find [H⁺]

Formulae Sheet: Acids, Bases & pH Calculations: Strong Acid pH Calculations

Formulae Sheet: Acids, Bases & pH Calculations: Strong Base pH Calculations

Formulae Sheet: Acids, Bases & pH Calculations: Relationship Between pH And Concentration

Formulae Sheet: Acids, Bases & pH Calculations: Ka Expression For Weak Acids

Formulae Sheet: Acids, Bases & pH Calculations: Calculating Ka From pH And Concentration

Formulae Sheet: Acids, Bases & pH Calculations: pKa And Its Relationship To Ka

Formulae Sheet: Acids, Bases & pH Calculations: Using Ka To Compare Acid Strength

Formulae Sheet: Redox & Electrochemistry: Oxidation Number Rules

Formulae Sheet: Redox & Electrochemistry: Redox Half-Equation Method

Formulae Sheet: Redox & Electrochemistry: Electron Transfer Calculations

Formulae Sheet: Redox & Electrochemistry: Electrolysis Charge Formula (Q = It)

Formulae Sheet: Redox & Electrochemistry: Faraday Constant Applications

Formulae Sheet: Redox & Electrochemistry: Mass And Mole Calculations In Electrolysis

Formulae Sheet: Organic Chemistry Quantitative Formulae: General Formulae Of Homologous Series

Formulae Sheet: Organic Chemistry Quantitative Formulae: Molecular Formula Determination From Percentage Composition

Formulae Sheet: Organic Chemistry Quantitative Formulae: Combustion Analysis Calculations

Formulae Sheet: Organic Chemistry Quantitative Formulae: Yield Calculations In Organic Reactions

Formulae Sheet: Organic Chemistry Quantitative Formulae: Atom Economy Formula

Formulae Sheet: Practical & Data Handling Formulae: Uncertainty And Percentage Uncertainty Formula

Formulae Sheet: Practical & Data Handling Formulae: Combining Uncertainties

Formulae Sheet: Practical & Data Handling Formulae: Gradient Formula For Graphs

Formulae Sheet: Practical & Data Handling Formulae: Mean, Range And Trend Interpretation (Data Skills)

Practical Skills: Understanding Paper 3 Structure & Assessment: Structure Of AS Level Chemistry Paper 3

Practical Skills: Understanding Paper 3 Structure & Assessment: Skill Weighting: Planning, Observation, Processing, Evaluation

Practical Skills: Understanding Paper 3 Structure & Assessment: How Marks Are Awarded In Practical Questions

Practical Skills: Understanding Paper 3 Structure & Assessment: Difference Between Method Marks And Accuracy Marks

Practical Skills: Understanding Paper 3 Structure & Assessment: Common Examiner Expectations In Paper 3

Practical Skills: Experimental Planning Skills: Writing A Complete Experimental Plan (Variables, Controls, Steps)

Practical Skills: Experimental Planning Skills: Independent, Dependent And Controlled Variables

Practical Skills: Experimental Planning Skills: Choosing Appropriate Apparatus (Size, Accuracy, Precision)

Practical Skills: Experimental Planning Skills: Designing Fair Tests

Practical Skills: Experimental Planning Skills: Repeats, Averages And Reliability

Practical Skills: Experimental Planning Skills: Safety Considerations And Hazards

Practical Skills: Experimental Planning Skills: Planning Questions That Involve Titration

Practical Skills: Experimental Planning Skills: Planning Questions Involving Rates Of Reaction

Practical Skills: Experimental Planning Skills: Planning Questions Using Calorimetry

Practical Skills: Experimental Planning Skills: Planning Questions Using Gas Collection

Practical Skills: Measurement & Apparatus Handling: Correct Use Of Burettes, Pipettes And Measuring Cylinders

Practical Skills: Measurement & Apparatus Handling: Reading Scales Correctly (Meniscus Rules)

Practical Skills: Measurement & Apparatus Handling: Choice Between Measuring Cylinder Vs Pipette (Exam Logic)

Practical Skills: Measurement & Apparatus Handling: Use Of Thermometers And Temperature Control

Practical Skills: Measurement & Apparatus Handling: Use Of Stopwatches And Timing Reactions

Practical Skills: Measurement & Apparatus Handling: Balances: Mass Measurement And Significant Figures

Practical Skills: Recording Results & Observations: Recording Qualitative Observations (Colour, Precipitate, Gas)

Practical Skills: Recording Results & Observations: Writing Observations Vs Explanations

Practical Skills: Recording Results & Observations: Correct Use Of Tables (Headings, Units, Consistency)

Practical Skills: Recording Results & Observations: Decimal Places And Significant Figures In Tables

Practical Skills: Recording Results & Observations: Avoiding Subjective Language In Observations

Practical Skills: Recording Results & Observations: Common Observation Errors Examiners Penalise

Practical Skills: Data Processing & Calculations: Calculations From Raw Practical Data

Practical Skills: Data Processing & Calculations: Titration Calculations From Experimental Readings

Practical Skills: Data Processing & Calculations: Rate Calculations From Time Measurements

Practical Skills: Data Processing & Calculations: Energy Change Calculations From Calorimetry Data

Practical Skills: Data Processing & Calculations: Percentage Yield And Purity In Practical Contexts

Practical Skills: Data Processing & Calculations: Error Carried Forward In Practical Calculations

Practical Skills: Graph Skills (High-Frequency Area): Choosing Correct Axes And Scales

Practical Skills: Graph Skills (High-Frequency Area): Plotting Points Accurately

Practical Skills: Graph Skills (High-Frequency Area): Drawing Best-Fit Lines Or Curves

Practical Skills: Graph Skills (High-Frequency Area): Determining Gradients And Tangents

Practical Skills: Graph Skills (High-Frequency Area): Extracting Quantitative Information From Graphs

Practical Skills: Graph Skills (High-Frequency Area): Common Graph Drawing Mistakes

Practical Skills: Uncertainty, Errors & Evaluation: Types Of Error: Random Vs Systematic

Practical Skills: Uncertainty, Errors & Evaluation: Sources Of Error In Practical Experiments

Practical Skills: Uncertainty, Errors & Evaluation: Absolute And Percentage Uncertainty

Practical Skills: Uncertainty, Errors & Evaluation: Combining Uncertainties

Practical Skills: Uncertainty, Errors & Evaluation: Meaningful Evaluation Statements (Not Vague Ones)

Practical Skills: Uncertainty, Errors & Evaluation: Improvements That Actually Score Marks

Practical Skills: Uncertainty, Errors & Evaluation: Why “Human Error” Is Penalised

Practical Skills: Uncertainty, Errors & Evaluation: Limitations Vs Improvements (Exam Distinction)

Practical Skills: Qualitative Analysis Skills: Identifying Gases From Tests And Observations

Practical Skills: Qualitative Analysis Skills: Flame Tests And Their Limitations

Practical Skills: Qualitative Analysis Skills: Test For Cations And Anions (Observation-Focused)

Practical Skills: Qualitative Analysis Skills: Organic Functional Group Tests In Practical Contexts

Practical Skills: Qualitative Analysis Skills: Writing Balanced Chemical Equations For Tests

Practical Skills: Examiner Traps & Final Practical Intelligence: Most Repeated Paper 3 Mistakes From Examiner Reports

Practical Skills: Examiner Traps & Final Practical Intelligence: Words That Instantly Lose Marks In Evaluation

Practical Skills: Examiner Traps & Final Practical Intelligence: How Over-Detail Loses Planning Marks

Practical Skills: Examiner Traps & Final Practical Intelligence: When Diagrams Help And When They Waste Time

Practical Skills: Examiner Traps & Final Practical Intelligence: Using Data Booklet In Practical Questions

Practical Skills: Examiner Traps & Final Practical Intelligence: Final Checklist Before Submitting Paper 3