Solids, Liquids And Gases: State The Distinguishing Properties Of Solids, Liquids And Gases

Solids, Liquids And Gases: Describe The Structures Of Solids, Liquids And Gases In Terms Of Particle Separation, Arrangement And Motion

Solids, Liquids And Gases: Describe And Explain Changes Of State (Melting, Boiling, Evaporating, Freezing And Condensing) In Terms Of Kinetic Particle Theory

Solids, Liquids And Gases: Interpret And Explain Heating And Cooling Curves In Terms Of Kinetic Particle Theory

Solids, Liquids And Gases: Describe And Explain, In Terms Of Kinetic Particle Theory, The Effects Of Temperature And Pressure On The Volume Of A Gas

Diffusion: Describe And Explain Diffusion In Terms Of Kinetic Particle Theory

Diffusion: Describe And Explain The Effect Of Relative Molecular Mass On The Rate Of Diffusion Of Gases

Elements, Compounds And Mixtures: Describe The Differences Between Elements, Compounds And Mixtures

Atomic Structure And The Periodic Table: Describe The Structure Of The Atom As A Central Nucleus Containing Neutrons And Protons Surrounded By Electrons In Shells

Atomic Structure And The Periodic Table: State The Relative Charges And Relative Masses Of A Proton, A Neutron And An Electron

Atomic Structure And The Periodic Table: Define Proton Number/atomic Number As The Number Of Protons In The Nucleus Of An Atom

Atomic Structure And The Periodic Table: Define Mass Number/nucleon Number As The Total Number Of Protons And Neutrons In The Nucleus Of An Atom

Atomic Structure And The Periodic Table: Determine The Electronic Configuration Of Elements And Their Ions With Proton Number 1 To 20, E.g. 2,8,3

Atomic Structure And The Periodic Table: State That

Isotopes: Define Isotopes As Different Atoms Of The Same Element That Have The Same Number Of Protons But Different Numbers Of Neutrons

Isotopes: State That Isotopes Of The Same Element Have The Same Chemical Properties Because They Have The Same Number Of Electrons And Therefore The Same Electronic Configuration

Isotopes: Interpret And Use Symbols For Atoms, E.g. 12 6c, And Ions, E.g. 35 17cl  –

Isotopes: Calculate The Relative Atomic Mass Of An Element From The Relative Masses And Abundances Of Its Isotopes

Ion And Ionic Bonds: Describe The Formation Of Positive Ions, Known As Cations, And Negative Ions, Known As Anions

Ion And Ionic Bonds: Describe The Giant Lattice Structure Of Ionic Compounds As A Regular Arrangement Of Alternating Positive And Negative Ions

Ion And Ionic Bonds: State That An Ionic Bond Is A Strong Electrostatic Attraction Between Oppositely Charged Ions

Ion And Ionic Bonds: Describe The Formation Of Ionic Bonds Between Ions Of Metallic And Non-metallic Elements, Including The Use Of Dot-and-cross Diagrams

Ion And Ionic Bonds: Describe And Explain In Terms Of Structure And Bonding The Properties Of Ionic Compounds

Simple Molecules And Covalent Bonds: State That A Covalent Bond Is Formed When A Pair Of Electrons Is Shared Between Two Atoms Leading To Noble Gas Electronic Configurations

Simple Molecules And Covalent Bonds: Describe The Formation Of Covalent Bonds In Simple Molecules, Including H2, Cl 2, H2o, Ch4, Nh3, Hcl, Ch3oh, C2h4, O2, Co2 And N2. Use Dot-and-cross Diagrams To Show The Electronic Configurations In These And Similar Molecules

Simple Molecules And Covalent Bonds: Describe And Explain In Terms Of Structure And Bonding The Properties Of Simple Molecular Compounds

Giant Covalent Structures: Describe The Giant Covalent Structures Of Graphite, Diamond And Silicon(Iv) Oxide, Sio2

Giant Covalent Structures: Relate The Structures And Bonding Of Graphite And Diamond To Their Uses

Giant Covalent Structures: Describe The Similarity In Properties Between Diamond And Silicon(Iv) Oxide, Related To Their Structures

Metallic bonding: Describe metallic bonding as the electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electrons

Metallic bonding: Explain In Terms Of Structure And Bonding The Properties Of Metals

Formulae: State The Formulae Of The Elements And Compounds Named In The Subject Content

Formulae: Define The Molecular Formula Of A Compound As The Number And Type Of Different Atoms In One Molecule

Formulae: Define The Empirical Formula Of A Compound As The Simplest Whole Number Ratio Of The Different Atoms Or Ions In A Compound

Formulae: Deduce The Formula Of A Simple Compound From The Relative Numbers Of Atoms Or Ions Present In A Model Or A Diagrammatic Representation

Formulae: Deduce The Formula Of An Ionic Compound From The Charges On The Ions

Formulae: Construct Word Equations, Symbol Equations And Ionic Equations To Show How Reactants Form Products, Including State Symbols

Formulae: Deduce The Symbol Equation With State Symbols For A Chemical Reaction, Given Relevant Information

Relative Masses Of Atoms And Molecules: Describe Relative Atomic Mass, Ar , As The Average Mass Of The Isotopes Of An Element Compared To 1/12th Of The Mass Of An Atom Of 12c

Relative Masses Of Atoms And Molecules: Define Relative Molecular Mass, Mr , As The Sum Of The Relative Atomic Masses. Relative Formula Mass, Mr , Will Be Used For Ionic Compounds

The Mole And The Avogadro Constant: State That The Mole, Mol, Is The Unit Of Amount Of Substance And That One Mole Contains 6.02×1023 Particles, E.g. Atoms, Ions, Molecules; This Number Is The Avogadro Constant

The Mole And The Avogadro Constant: Use The Relationship Amount Of Substance (Mol) = Mass (G) Molar Mass (G/mol) To Calculate

The Mole And The Avogadro Constant: Use The Molar Gas Volume, Taken As 24dm3 At Room Temperature And Pressure, R.t.p., In Calculations Involving Gases

The Mole And The Avogadro Constant: State That Concentration Can Be Measured In G/dm3 Or Mol/dm3

The Mole And The Avogadro Constant: Calculate Stoichiometric Reacting Masses, Limiting Reactants, Volumes Of Gases At R.t.p., Volumes Of Solutions And Concentrations Of Solutions Expressed In G/dm3 And Mol/dm3 , Including Conversion Between Cm3 And Dm3

The Mole And The Avogadro Constant: Use Experimental Data To Calculate The Concentration Of A Solution In A Titration

The Mole And The Avogadro Constant: Calculate Empirical Formulae And Molecular Formulae, Given Appropriate Data

The Mole And The Avogadro Constant: Calculate Percentage Yield, Percentage Composition By Mass And Percentage Purity, Given Appropriate Data

Electrolysis: Define Electrolysis As The Decomposition Of An Ionic Compound, When Molten Or In Aqueous Solution, By The Passage Of An Electric Current

Electrolysis: Identify In Simple Electrolytic Cells

Electrolysis: Describe The Transfer Of Charge During Electrolysis

Electrolysis: Identify The Products Formed At The Electrodes And Describe The Observations Made During The Electrolysis

Electrolysis: Identify The Products Formed At The Electrodes And Describe The Observations Made During The Electrolysis Of Aqueous Copper(Ii) Sulfate Using Inert Carbon/graphite Electrodes And When Using Copper Electrodes

Electrolysis: State That Metals Or Hydrogen Are Formed At The Cathode And That Non-metals (Other Than Hydrogen) Are Formed At The Anode

Electrolysis: Predict The Identity Of The Products At Each Electrode For The Electrolysis Of A Binary Compound In The Molten State

Electrolysis: Predict The Identity Of The Products At Each Electrode For The Electrolysis Of A Halide Compound In Dilute Or Concentrated Aqueous Solution

Electrolysis: Construct Ionic Half-equations For Reactions At The Anode (To Show Oxidation) And At The Cathode (To Show Reduction)

Electrolysis: State That Metal Objects Are Electroplated To Improve Their Appearance And Resistance To Corrosion

Electrolysis: Describe How Metals Are Electroplated

Hydrogen–oxygen Fuel Cells: State That A Hydrogen–oxygen Fuel Cell Uses Hydrogen And Oxygen To Produce Electricity With Water As The Only Chemical Product

Hydrogen–oxygen Fuel Cells: Describe The Advantages And Disadvantages Of Using Hydrogen–oxygen Fuel Cells In Comparison With Gasoline/petrol Engines In Vehicles

Exothermic And Endothermic Reactions: State That An Exothermic Reaction Transfers Thermal Energy To The Surroundings Leading To An Increase In The Temperature Of The Surroundings

Exothermic And Endothermic Reactions: State That An Endothermic Reaction Takes In Thermal Energy From The Surroundings Leading To A Decrease In The Temperature Of The Surroundings

Exothermic And Endothermic Reactions: State That The Transfer Of Thermal Energy During A Reaction Is Called The Enthalpy Change, Δh, Of The Reaction. Δh Is Negative For Exothermic Reactions And Positive For Endothermic Reactions

Exothermic And Endothermic Reactions: Define Activation Energy, Ea, As The Minimum Energy That Colliding Particles Must Have To React

Exothermic And Endothermic Reactions: Draw, Label And Interpret Reaction Pathway Diagrams For Exothermic And Endothermic Reactions Using Information Provided

Exothermic And Endothermic Reactions: State That Bond Breaking Is An Endothermic Process And Bond Making Is An Exothermic Process And Explain The Enthalpy Change Of A Reaction In Terms Of Bond Breaking And Bond Making

Exothermic And Endothermic Reactions: Calculate The Enthalpy Change Of A Reaction Using Bond Energies

Physical And Chemical Changes: Identify Physical And Chemical Changes, And Describe The Differences Between Them

Rate Of Reaction: Describe Collision Theory

Rate Of Reaction: State That A Catalyst Increases The Rate Of A Reaction, Decreases The Activation Energy, Ea, Of A Reaction And Is Unchanged At The End Of A Reaction

Rate Of Reaction: Describe And Explain The Effect On The Rate Of Reactions

Rate Of Reaction: Describe And Evaluate Practical Methods For Investigating The Rate Of A Reaction, Including Change In Mass Of A Reactant Or A Product And The Formation Of A Gas

Rate Of Reaction: Interpret Data, Including Graphs, From Rate Of Reaction Experiments

Reversible Reactions And Equilibrium: State That Some Chemical Reactions Are Reversible As Shown By The Symbol ⇌

Reversible Reactions And Equilibrium: Describe How Changing The Conditions Can Change The Direction Of A Reversible Reaction

Reversible Reactions And Equilibrium: State That A Reversible Reaction In A Closed System Is At Equilibrium

Reversible Reactions And Equilibrium: Predict And Explain, For A Reversible Reaction, How The Position Of Equilibrium Is Affected

Reversible Reactions And Equilibrium: State The Symbol Equation For The Production Of Ammonia In The Haber Process, N2(G) + 3h2(G) ⇌ 2nh3(G)

Reversible Reactions And Equilibrium: State The Sources Of The Hydrogen (Methane) And Nitrogen (Air) In The Haber Process

Reversible Reactions And Equilibrium: State The Typical Conditions In The Haber Process As 450°c, 20000kpa/200 Atm And An Iron Catalyst

Reversible Reactions And Equilibrium: State The Symbol Equation For The Conversion Of Sulfur Dioxide To Sulfur Trioxide In The Contact Process, 2so2(G) + O2(G) ⇌ 2so3(G)

Reversible Reactions And Equilibrium: State The Sources Of The Sulfur Dioxide (Burning Sulfur Or Roasting Sulfide Ores) And Oxygen (Air) In The Contact Process

Reversible Reactions And Equilibrium: State The Typical Conditions For The Conversion Of Sulfur Dioxide To Sulfur Trioxide In The Contact Process As 450°c, 200kpa/2 Atm And A Vanadium(V) Oxide Catalyst

Reversible Reactions And Equilibrium: Explain, In Terms Of Rate Of Reaction And Position Of Equilibrium, Why The Typical Conditions Stated Are Used In The Haber Process And In The Contact Process, Including Safety Considerations And Economics

Redox: Use A Roman Numeral To Indicate The Oxidation Number Of An Element In A Compound

Redox: Define Redox Reactions As Involving Simultaneous Reduction And Oxidation

Redox: Define Oxidation In Terms

Redox: Define Reduction In Terms

Redox: Identify Redox Reactions As Reactions Involving Gain And Loss Of Oxygen, Or Gain And Loss Of Electrons

Redox: Identify Redox Reactions By Changes In Oxidation Number

Redox: Identify Redox Reactions By The Colour Changes Involved When Using Acidified Aqueous Potassium Manganate(Vii) Or Aqueous Potassium Iodide

Redox: Define An Oxidising Agent As A Substance That Oxidises Another Substance And Is Itself Reduced

Redox: Define A Reducing Agent As A Substance That Reduces Another Substance And Is Itself Oxidised

Redox: Identify Oxidation, Oxidising Agents, Reduction And Reducing Agents In Redox Reactions

The Characteristic Properties Of Acids And Bases: State That Aqueous Solutions Of Acids Contain H+ Ions And Aqueous Solutions Of Alkalis Contain Oh– Ions

The Characteristic Properties Of Acids And Bases: Define Acids As Proton Donors And Bases As Proton Acceptors

The Characteristic Properties Of Acids And Bases: State That Bases Are Oxides Or Hydroxides Of Metals And That Alkalis Are Soluble Bases

The Characteristic Properties Of Acids And Bases: Describe The Characteristic Properties Of Acids In Terms Of Their Reactions

The Characteristic Properties Of Acids And Bases: Describe The Characteristic Properties Of Acids In Terms Of Their Reactions

The Characteristic Properties Of Acids And Bases: Describe The Neutralisation Reaction Between An Acid And An Alkali To Produce Water, H+

The Characteristic Properties Of Acids And Bases: Describe Acids And Alkalis In Terms Of Their Effects

The Characteristic Properties Of Acids And Bases: Define A Strong Acid As An Acid That Is Completely Dissociated In Aqueous Solution And A Weak Acid As An Acid That Is Partially Dissociated In Aqueous Solution

The Characteristic Properties Of Acids And Bases: State Examples Of Strong Acids, Including Hydrochloric Acid, Nitric Acid And Sulfuric Acid And Construct The Symbol Equations To Show Their Complete Dissociation, E.g. Hcl(Aq) → H+ (Aq) + Cl   – (Aq)

The Characteristic Properties Of Acids And Bases: State Examples Of Weak Acids, Including Carboxylic Acids And Construct The Symbol Equations To Show Their Partial Dissociation, E.g. For Ethanoic Acid, Ch3cooh(Aq) ⇌ H+ (Aq) + Ch3coo– (Aq)

The Characteristic Properties Of Acids And Bases: Describe How To Compare Hydrogen Ion Concentration, Neutrality, Relative Acidity And Relative Alkalinity In Terms Of Colour And Ph Using Universal Indicator Paper

Oxides: Describe Amphoteric Oxides As Oxides That React With Acids And Bases To Produce A Salt And Water

Oxides: Classify Oxides As Acidic, Including So2 And Co2, Basic, Including Cuo And Cao, Or Amphoteric, Limited To Al 2o3 And Zno, Related To Metallic And Non-metallic Character

Preparation Of Salts: Describe The Preparation, Separation And Purification Of Soluble Salts By Reaction Of An Acid

Preparation Of Salts: Describe The Preparation, Separation And Purification Of Soluble Salts By Reaction Of An Acid

Preparation Of Salts: Describe The General Solubility Rule For Salts

Preparation Of Salts: Define A Hydrated Substance As A Substance That Is Chemically Combined With Water And An Anhydrous Substance As A Substance Containing No Water

Preparation Of Salts: Define The Term Water Of Crystallisation As The Water Molecules Present In Hydrated Crystals, Including Cuso4•5h2o And Cocl 2•6h2o

Arrangement Of Elements: Describe The Periodic Table As An Arrangement Of Elements In Periods And Groups And In Order Of Increasing Proton Number/atomic Number

Arrangement Of Elements: Describe The Change From Metallic To Non-metallic Character Across A Period

Arrangement Of Elements: Describe The Relationship Between Group Number And The Charge Of The Ions Formed From Elements In That Group

Arrangement Of Elements: Explain Similarities In The Chemical Properties Of Elements In The Same Group Of The Periodic Table In Terms Of Their Electronic Configuration

Arrangement Of Elements: Explain How The Position Of An Element In The Periodic Table Can Be Used To Predict Its Properties

Arrangement Of Elements: Identify Trends In Groups, Given Information About The Elements

Group I Properties: Describe The Group I Alkali Metals, Lithium, Sodium And Potassium, As Relatively Soft Metals With General Trends Down The Group

Group I Properties: Predict The Properties Of Other Elements In Group I, Given Information About The Elements

Group VII properties: Describe the Group VII halogens, chlorine, bromine and iodine, as diatomic non-metals with general trends down the group

Group VII properties: State The Appearance Of The Halogens At R.t.p.

Group VII properties: Describe And Explain The Displacement Reactions Of Halogens With Other Halide Ions

Group VII properties: Predict The Properties Of Other Elements In Group Vii, Given Information About The Elements

Transition Elements: Describe The Transition Elements As Metals

Noble Gases: Describe The Group Viii Noble Gases As Unreactive, Monatomic Gases And Explain This In Terms Of Electronic Configuration

Properties Of Metals: Compare The General Physical Properties Of Metals And Non-metals

Properties Of Metals: Describe The General Chemical Properties Of Metals, Limited To Their Reactions

Uses Of Metals: Describe The Uses Of Metals In Terms Of Their Physical Properties

Alloys And Their Properties: Describe An Alloy As A Mixture Of A Metal With Other Elements

Alloys And Their Properties: Explain In Terms Of Structure How Alloys Can Be Harder And Stronger Than The Pure Metals Because The Different Sized Atoms Or Ions In Alloys Mean The Layers Can No Longer Slide Over Each Other

Alloys And Their Properties: Identify Representations Of Alloys From Diagrams Of Structure

Reactivity Series: State The Order Of The Reactivity Series As: Potassium, Sodium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Hydrogen, Copper, Silver, Gold

Reactivity Series: Describe The Relative Reactivities Of Metals In Terms Of Their Tendency To Form Positive Ions, By Displacement Reactions, If Any, With The Aqueous Ions Of Magnesium, Zinc, Iron, Copper And Silver 3 Describe The Reactions

Reactivity Series: Describe The Reactions

Reactivity Series: Explain The Apparent Unreactivity Of Aluminium In Terms Of Its Oxide Layer

Reactivity Series: Deduce An Order Of Reactivity From A Given Set Of Experimental Results

Corrosion Of Metals: State The Conditions Required For The Rusting Of Iron And Steel To Form Hydrated Iron(Iii) Oxide

Corrosion Of Metals: Describe How Barrier Methods Prevent Rusting By Excluding Oxygen Or Water

Corrosion Of Metals: State Some Common Barrier Methods, Including Painting, Greasing And Coating With Plastic

Corrosion Of Metals: Explain Sacrificial Protection In Terms Of The Reactivity Series And In Terms Of Electron Loss

Corrosion Of Metals: Describe The Use Of Zinc In Galvanising As An Example Of A Barrier Method And Sacrificial Protection

Extraction Of Metals: Describe The Ease Of Obtaining Metals From Their Ores, Related To The Position Of The Metal In The Reactivity Series

Extraction Of Metals: Describe The Extraction Of Iron From Hematite In The Blast Furnace, Including Symbol Equations For Each Step

Extraction Of Metals: Describe The Extraction Of Aluminium From Purified Bauxite/aluminium Oxide

Water: Describe Chemical Tests For The Presence Of Water Using Anhydrous Cobalt(Ii) Chloride And Anhydrous Copper(Ii) Sulfate

Water: Describe How To Test For The Purity Of Water Using Melting Point And Boiling Point

Water: Explain That Distilled Water Is Used In Practical Chemistry Rather Than Tap Water Because It Contains Fewer Chemical Impurities

Water: State That Water From Natural Sources May Contain Substances

Water: State That Some Of These Substances Are Beneficial

Water: State That Some Of These Substances Are Potentially Harmful

Water: Describe The Treatment Of The Domestic Water Supply

Fertilisers: State That Ammonium Salts And Nitrates Are Used As Fertilisers

Fertilisers: Describe The Use Of Npk Fertilisers To Provide The Elements Nitrogen, Phosphorus And Potassium For Improved Plant Growth

Air Quality And Climate: State The Composition Of Clean, Dry Air As Approximately 78% Nitrogen, N2, 21% Oxygen, O2, And The Remainder As A Mixture Of Noble Gases And Carbon Dioxide, Co2

Air Quality And Climate: State The Source Of Each Of These Air Pollutants

Air Quality And Climate: State The Adverse Effects Of These Air Pollutants

Air Quality And Climate: Describe How The Greenhouse Gases Carbon Dioxide And Methane Cause Global Warming

Air Quality And Climate: State And Explain Strategies To Reduce The Effects Of These Environmental Issues

Air Quality And Climate: Explain How Oxides Of Nitrogen Form In Car Engines And Describe Their Removal By Catalytic Converters, E.g. 2co + 2no → 2co2 + N2

Air Quality And Climate: Describe Photosynthesis As The Reaction Between Carbon Dioxide And Water To Produce Glucose And Oxygen In The Presence Of Chlorophyll And Using Energy From Light

Air Quality And Climate: State The Word Equation And Symbol Equation For Photosynthesis