States of matter - Solids, liquids and gases - State the distinguishing properties of solids, liquids and gases

States of matter - Solids, liquids and gases - Describe the structures of solids, liquids and gases in terms of particle separation, arrangement and motion

States of matter - Solids, liquids and gases - Describe changes of state in terms of melting, boiling, evaporating, freezing and condensing

States of matter - Solids, liquids and gases - Describe the effects of temperature and pressure on the volume of a gas

States of matter - Solids, liquids and gases - Explain changes of state in terms of kinetic particle theory, including the interpretation of heating and cooling curves

States of matter - Solids, liquids and gases - Explain, in terms of kinetic particle theory, the effects of temperature and pressure on the volume of a gas

States of matter - Diffusion - Describe and explain diffusion in terms of kinetic particle theory

States of matter - Diffusion - Describe and explain the effect of relative molecular mass on the rate of diffusion of gases

Atoms, elements and compounds - Elements, compounds and mixtures - Describe the differences between elements, compounds and mixtures

Atoms, elements and compounds - 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

Atoms, elements and compounds - Atomic structure and the Periodic Table - State the relative charges and relative masses of a proton, a neutron and an electron

Atoms, elements and compounds - Atomic structure and the Periodic Table - Define proton number/atomic number as the number of protons in the nucleus of an atom

Atoms, elements and compounds - 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

Atoms, elements and compounds - 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

Atoms, elements and compounds - Atomic structure and the Periodic Table - State that: (a) Group VIII noble gases have a full outer shell (b) the number of outer shell electrons is equal to the group number in Groups I to VII (c) the number of occupied electron shells is equal to the period number

Atoms, elements and compounds - Isotopes - Define isotopes as different atoms of the same element that have the same number of protons but different numbers of neutrons

Atoms, elements and compounds - Isotopes - Interpret and use symbols for atoms, e.g. ${}_6^{12} mathrm{C}$, and ions, e.g. ${}_{17}^{35} mathrm{Cl}^{-}$

Atoms, elements and compounds - 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

Atoms, elements and compounds - Isotopes - Calculate the relative atomic mass of an element from the relative masses and abundances of its isotopes

Atoms, elements and compounds - Ions and ionic bonds - Describe the formation of positive ions, known as cations, and negative ions, known as anions

Atoms, elements and compounds - Ions and ionic bonds - State that an ionic bond is a strong electrostatic attraction between oppositely charged ions

Atoms, elements and compounds - Ions and ionic bonds - Describe the formation of ionic bonds between elements from Group I and Group VII, including the use of dot-and-cross diagrams

Atoms, elements and compounds - Ions and ionic bonds - Describe the properties of ionic compounds: (a) high melting points and boiling points (b) good electrical conductivity when aqueous or molten and poor when solid

Atoms, elements and 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

Atoms, elements and compounds - Giant covalent structures - Describe the giant covalent structures of graphite and diamond

Atoms, elements and compounds - Giant covalent structures - Relate the structures and bonding of graphite and diamond to their uses, limited to: (a) graphite as a lubricant and as an electrode (b) diamond in cutting tools

Atoms, elements and compounds - Giant covalent structures - Describe the giant covalent structure of silicon(IV) oxide, $mathrm{SiO}_2$

Atoms, elements and compounds - Giant covalent structures - Describe the similarity in properties between diamond and silicon(IV) oxide, related to their structures

Atoms, elements and compounds - Metallic bonding - Describe metallic bonding as the electrostatic attraction between the positive ions in a giant metallic lattice and a 'sea' of delocalised electrons

Atoms, elements and compounds - Metallic bonding - Explain in terms of structure and bonding the properties of metals: (a) good electrical conductivity (b) malleability and ductility

Stoichiometry - Formulae - State the formulae of the elements and compounds named in the subject content

Stoichiometry - Formulae - Define the molecular formula of a compound as the number and type of different atoms in one molecule

Stoichiometry - Formulae - Deduce the formula of a simple compound from the relative numbers of atoms present in a model or a diagrammatic representation

Stoichiometry - Formulae - Construct word equations and symbol equations to show how reactants form products, including state symbols

Stoichiometry - Formulae - Define the empirical formula of a compound as the simplest whole number ratio of atoms or ions in a compound

Stoichiometry - Formulae - Deduce the formula of an ionic compound from the relative numbers of the ions present in a model or a diagrammatic representation or from the charges on the ions

Stoichiometry - Formulae - Construct symbol equations with state symbols, including ionic equations

Stoichiometry - Formulae - Deduce the symbol equation with state symbols for a chemical reaction, given relevant information

Stoichiometry - Relative masses of atoms and molecules - Describe relative atomic mass, $A_r$ as the average mass of the isotopes of an element compared to $1 / 12$ th of the mass of an atom of ${ }^{12} mathrm{C}$

Stoichiometry - Relative masses of atoms and molecules - Define relative molecular mass, $M_r$ as the sum of the relative atomic masses. Relative formula mass, $M_r$ will be used for ionic compounds

Stoichiometry - Relative masses of atoms and molecules - Calculate reacting masses in simple proportions. Calculations will not involve the mole concept

Stoichiometry - The mole and the Avogadro constant - State that concentration can be measured in $mathrm{g} / mathrm{dm}^3$ or $mathrm{mol} / mathrm{dm}^3$

Stoichiometry - The mole and the Avogadro constant - State that the mole, mol, is the unit of amount of substance and that one mole contains $6.02 imes 10^{23}$ particles, e.g. atoms, ions, molecules; this number is the Avogadro constant

Stoichiometry - The mole and the Avogadro constant - Use the relationship amount of substance $(mathrm{mol})=frac{ ext { mass }(mathrm{g})}{ ext { molar mass } (mathrm{g} / mathrm{mol})}$

Stoichiometry - The mole and the Avogadro constant - Use experimental data from a titration to calculate the moles of solute, or the concentration or volume of a solution

Stoichiometry - The mole and the Avogadro constant - Calculate empirical formulae and molecular formulae, given appropriate data

Stoichiometry - The mole and the Avogadro constant - Calculate percentage yield, percentage composition by mass and percentage purity, given appropriate data

Electrochemistry - Electrolysis - Define electrolysis as the decomposition of an ionic compound, when molten or in aqueous solution, by the passage of an electric current

Electrochemistry - Electrolysis - Identify in simple electrolytic cells: (a) the anode as the positive electrode (b) the cathode as the negative electrode (c) the electrolyte as the molten or aqueous substance that undergoes electrolysis

Electrochemistry - Electrolysis - State that metals or hydrogen are formed at the cathode and that non-metals (other than hydrogen) are formed at the anode

Electrochemistry - Electrolysis - Predict the identity of the products at each electrode for the electrolysis of a binary compound in the molten state

Electrochemistry - Electrolysis - State that metal objects are electroplated to improve their appearance and resistance to corrosion

Electrochemistry - Electrolysis - Describe how metals are electroplated

Electrochemistry - Electrolysis - Describe the transfer of charge during electrolysis to include: (a) the movement of electrons in the external circuit (b) the loss or gain of electrons at the electrodes (c) the movement of ions in the electrolyte

Electrochemistry - 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

Electrochemistry - Electrolysis - Predict the identity of the products at each electrode for the electrolysis of a halide compound in dilute or concentrated aqueous solution

Electrochemistry - Electrolysis - Construct ionic half-equations for reactions at the anode (to show oxidation) and at the cathode (to show reduction)

Electrochemistry - 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

Electrochemistry - Hydrogen-oxygen fuel cells - Describe the advantages and disadvantages of using hydrogen-oxygen fuel cells in comparison with gasoline/petrol engines in vehicles

Chemical energetics - 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

Chemical energetics - 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

Chemical energetics - Exothermic and endothermic reactions - Interpret reaction pathway diagrams showing exothermic and endothermic reactions

Chemical energetics - Exothermic and endothermic reactions - State that the transfer of thermal energy during a reaction is called the enthalpy change, $Delta H$, of the reaction. $Delta H$ is negative for exothermic reactions and positive for endothermic reactions

Chemical energetics - Exothermic and endothermic reactions - Define activation energy, $E_{a}$, as the minimum energy that colliding particles must have to react

Chemical energetics - Exothermic and endothermic reactions - Draw and label reaction pathway diagrams for exothermic and endothermic reactions using information provided, to include: (a) reactants (b) products (c) enthalpy change of the reaction, $Delta H$ (d) activation energy, $E_{mathrm{a}}$

Chemical energetics - 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

Chemical energetics - Exothermic and endothermic reactions - Calculate the enthalpy change of a reaction using bond energies

Chemical reactions - Physical and chemical changes - Identify physical and chemical changes, and describe the differences between them

Chemical reactions - Rate of reaction - Describe the effect on the rate of reaction of: (a) changing the concentration of solutions (b) changing the pressure of gases (c) changing the surface area of solids (d) changing the temperature (e) adding or removing a catalyst, including enzymes

Chemical reactions - Rate of reaction - State that a catalyst increases the rate of a reaction and is unchanged at the end of a reaction

Chemical reactions - Rate of reaction - Describe 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

Chemical reactions - Rate of reaction - Interpret data, including graphs, from rate of reaction experiments

Chemical reactions - Rate of reaction - Describe collision theory in terms of: (a) number of particles per unit volume (b) frequency of collisions between particles (c) kinetic energy of particles (d) activation energy, $E_{mathrm{a}}$

Chemical reactions - Rate of reaction - State that a catalyst decreases the activation energy, $E_a$, of a reaction

Chemical reactions - Rate of reaction - 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

Chemical reactions - Reversible reactions and equilibrium - State that some chemical reactions are reversible as shown by the symbol $ ightleftharpoons$

Chemical reactions - Reversible reactions and equilibrium - Describe how changing the conditions can change the direction of a reversible reaction for: (a) the effect of heat on hydrated compounds (b) the addition of water to anhydrous compounds limited to copper(II) sulfate and cobalt(II) chloride

Chemical reactions - Reversible reactions and equilibrium - State that a reversible reaction in a closed system is at equilibrium when: (a) the rate of the forward reaction is equal to the rate of the reverse reaction (b) the concentrations of reactants and products are no longer changing

Chemical reactions - Reversible reactions and equilibrium - Predict and explain, for a reversible reaction, how the position of equilibrium is affected by: (a) changing temperature (b) changing pressure (c) changing concentration (d) using a catalyst using information provided

Chemical reactions - Reversible reactions and equilibrium - State the typical conditions in the Haber process as $450^{circ} mathrm{C}, 20000 mathrm{kPa} / 200 mathrm{~atm}$ and an iron catalyst

Chemical reactions - Reversible reactions and equilibrium - State the symbol equation for the conversion of sulfur dioxide to sulfur trioxide in the Contact process, $2 mathrm{SO}_2(mathrm{~g})+mathrm{O}_2(mathrm{~g}) ightleftharpoons 2 mathrm{SO}_3(mathrm{~g})$

Chemical reactions - Reversible reactions and equilibrium - State the sources of the sulfur dioxide (burning sulfur or roasting sulfide ores) and oxygen (air) in the Contact process

Chemical reactions - Reversible reactions and equilibrium - State the typical conditions for the conversion of sulfur dioxide to sulfur trioxide in the Contact process as $450^{circ} mathrm{C}, 200 mathrm{kPa} / 2 mathrm{~atm}$ and a vanadium(V) oxide catalyst

Chemical reactions - 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

Chemical reactions - Redox - Use a Roman numeral to indicate the oxidation number of an element in a compound

Chemical reactions - Redox - Define redox reactions as involving simultaneous oxidation and reduction

Chemical reactions - Redox - Define oxidation as gain of oxygen and reduction as loss of oxygen

Chemical reactions - Redox - Identify redox reactions as reactions involving gain and loss of oxygen

Chemical reactions - Redox - Identify oxidation and reduction in redox reactions

Chemical reactions - Redox - Define oxidation in terms of: (a) loss of electrons (b) an increase in oxidation number

Chemical reactions - Redox - Define reduction in terms of: (a) gain of electrons (b) a decrease in oxidation number

Chemical reactions - Redox - Identify redox reactions as reactions involving gain and loss of electrons

Chemical reactions - Redox - Identify redox reactions by the colour changes involved when using acidified aqueous potassium manganate(VII) or aqueous potassium iodide

Chemical reactions - Redox - Define an oxidising agent as a substance that oxidises another substance and is itself reduced

Chemical reactions - Redox - Define a reducing agent as a substance that reduces another substance and is itself oxidised

Chemical reactions - Redox - Identify oxidising agents and reducing agents in redox reactions

Acids, bases and salts - The characteristic properties of acids and bases - Describe the characteristic properties of acids in terms of their reactions with: (a) metals (b) bases (c) carbonates

Acids, bases and salts - The characteristic properties of acids and bases - Describe acids in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange

Acids, bases and salts - The characteristic properties of acids and bases - State that bases are oxides or hydroxides of metals and that alkalis are soluble bases

Acids, bases and salts - The characteristic properties of acids and bases - Describe the characteristic properties of bases in terms of their reactions with: (a) acids (b) ammonium salts

Acids, bases and salts - The characteristic properties of acids and bases - Describe alkalis in terms of their effect on: (a) litmus (b) thymolphthalein (c) methyl orange

Acids, bases and salts - The characteristic properties of acids and bases - State that aqueous solutions of acids contain $mathrm{H}^{+}$ ions and aqueous solutions of alkalis contain $mathrm{OH}^{-}$ ions

Acids, bases and salts - 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 $mathrm{pH}$ using universal indicator paper

Acids, bases and salts - The characteristic properties of acids and bases - Describe the neutralisation reaction between an acid and an alkali to produce water, $mathrm{H}^{+}(mathrm{aq})+mathrm{OH}^{-}(mathrm{aq}) ightarrow mathrm{H}_2 mathrm{O}(l)$

Acids, bases and salts - Oxides - Classify oxides as acidic, including $mathrm{SO}_2$ and $mathrm{CO}_2$, or basic, including $mathrm{CuO}$ and $mathrm{CaO}$, related to metallic and non-metallic character

Acids, bases and salts - Oxides - Describe amphoteric oxides as oxides that react with acids and with bases to produce a salt and water

Acids, bases and salts - Oxides - Classify $mathrm{Al}_2 mathrm{O}_3$ and $mathrm{ZnO}$ as amphoteric oxides

Acids, bases and salts - Preparation of salts - Describe the preparation, separation and purification of soluble salts by reaction of an acid with: (a) an alkali by titration (b) excess metal (c) excess insoluble base (d) excess insoluble carbonate

Acids, bases and 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

Acids, bases and salts - Preparation of salts - Describe the preparation of insoluble salts by precipitation

Acids, bases and salts - Preparation of salts - Define the term water of crystallisation as the water molecules present in hydrated crystals, including $mathrm{CuSO}_4 cdot 5 mathrm{H}_2 mathrm{O}$ and $mathrm{CoCl}_2 cdot 6 mathrm{H}_2 mathrm{O}$

The Periodic Table - 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

The Periodic Table - Arrangement of elements - Describe the change from metallic to non-metallic character across a period

The Periodic Table - Arrangement of elements - Describe the relationship between group number and the charge of the ions formed from elements in that group

The Periodic Table - 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

The Periodic Table - Arrangement of elements - Explain how the position of an element in the Periodic Table can be used to predict its properties

The Periodic Table - Arrangement of elements - Identify trends in groups, given information about the elements

The Periodic Table - Group I properties - Describe the Group I alkali metals, lithium, sodium and potassium, as relatively soft metals with general trends down the group, limited to: (a) decreasing melting point (b) increasing density (c) increasing reactivity

The Periodic Table - Group I properties - Predict the properties of other elements in Group I, given information about the elements

The Periodic Table - Group VII properties - Describe the Group VII halogens, chlorine, bromine and iodine, as diatomic non-metals with general trends down the group, limited to: (a) increasing density (b) decreasing reactivity

The Periodic Table - Group VII properties - State the appearance of the halogens at r.t.p. as: (a) chlorine, a pale yellow-green gas (b) bromine, a red-brown liquid (c) iodine, a grey-black solid

The Periodic Table - Group VII properties - Describe and explain the displacement reactions of halogens with other halide ions

The Periodic Table - Group VII properties - Predict the properties of other elements in Group VII, given information about the elements

The Periodic Table - Transition elements - Describe the transition elements as metals that: (a) have high density (b) have high melting points (c) form coloured compounds (d) often act as catalysts as elements and in compounds

The Periodic Table - Transition elements - Describe transition elements as having ions with variable oxidation numbers, including iron(II) and iron(III)

The Periodic Table - Noble gases - Describe the Group VIII noble gases as unreactive, monatomic gases and explain this in terms of electronic configuration

Metals - Properties of metals - Compare the general physical properties of metals and non-metals, including: (a) thermal conductivity (b) electrical conductivity (c) malleability and ductility (d) melting points and boiling points

Metals - Properties of metals - Describe the general chemical properties of metals, limited to their reactions with: (a) dilute acids (b) cold water and steam (c) oxygen

Metals - Alloys and their properties - Describe an alloy as a mixture of a metal with other elements, including: (a) brass as a mixture of copper and zinc (b) stainless steel as a mixture of iron and other elements such as chromium, nickel and carbon

Metals - Alloys and their properties - State that alloys can be harder and stronger than the pure metals and are more useful

Metals - Alloys and their properties - Describe the uses of alloys in terms of their physical properties, including stainless steel in cutlery because of its hardness and resistance to rusting

Metals - Alloys and their properties - Identify representations of alloys from diagrams of structure

Metals - 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 in alloys mean the layers can no longer slide over each other

Metals - Reactivity series - State the order of the reactivity series as: potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold

Metals - Reactivity series - Deduce an order of reactivity from a given set of experimental results

Metals - 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

Metals - Reactivity series - Explain the apparent unreactivity of aluminium in terms of its oxide layer

Metals - Corrosion of metals - State the conditions required for the rusting of iron and steel to form hydrated iron(III) oxide

Metals - Corrosion of metals - State some common barrier methods, including painting, greasing and coating with plastic

Metals - Corrosion of metals - Describe how barrier methods prevent rusting by excluding oxygen or water

Metals - Corrosion of metals - Describe the use of zinc in galvanising as an example of a barrier method and sacrificial protection

Metals - Corrosion of metals - Explain sacrificial protection in terms of the reactivity series and in terms of electron loss

Metals - Extraction of metals - Describe the ease in obtaining metals from their ores, related to the position of the metal in the reactivity series

Metals - Extraction of metals - State that the main ore of aluminium is bauxite and that aluminium is extracted by electrolysis

Metals - Extraction of metals - Describe the extraction of aluminium from purified bauxite/aluminium oxide, including: (a) the role of cryolite (b) why the carbon anodes need to be regularly replaced (c) the reactions at the electrodes, including ionic half-equations

Chemistry of the environment - Water - Describe chemical tests for the presence of water using anhydrous cobalt(II) chloride and anhydrous copper(II) sulfate

Chemistry of the environment - Water - Describe how to test for the purity of water using melting point and boiling point

Chemistry of the environment - Water - Explain that distilled water is used in practical chemistry rather than tap water because it contains fewer chemical impurities

Chemistry of the environment - Water - State that water from natural sources may contain substances, including: (a) dissolved oxygen (b) metal compounds (c) plastics (d) sewage (e) harmful microbes (f) nitrates from fertilisers (g) phosphates from fertilisers and detergents

Chemistry of the environment - Water - State that some of these substances are beneficial, including: (a) dissolved oxygen for aquatic life (b) some metal compounds provide essential minerals for life

Chemistry of the environment - Water - Describe the treatment of the domestic water supply in terms of: (a) sedimentation and filtration to remove solids (b) use of carbon to remove tastes and odours (c) chlorination to kill microbes

Chemistry of the environment - Fertilisers - State that ammonium salts and nitrates are used as fertilisers

Chemistry of the environment - Fertilisers - Describe the use of NPK fertilisers to provide the elements nitrogen, phosphorus and potassium for improved plant growth

Chemistry of the environment - Air quality and climate - State the composition of clean, dry air as approximately $78 \%$ nitrogen, $mathrm{N}_2, 21 \%$ oxygen, $mathrm{O}_2$ and the remainder as a mixture of noble gases and carbon dioxide, $mathrm{CO}_2$

Chemistry of the environment - 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

Chemistry of the environment - Air quality and climate - State the word equation for photosynthesis, carbon dioxide + water $ ightarrow$ glucose + oxygen

Chemistry of the environment - Air quality and climate - Describe how the greenhouse gases carbon dioxide and methane cause global warming, limited to: (a) the absorption, reflection and emission of thermal energy (b) reducing thermal energy loss to space

Chemistry of the environment - Air quality and climate - Describe the role of oxides of nitrogen in the formation of photochemical smog and their removal by catalytic converters, e.g. $2 mathrm{CO}+2 mathrm{NO} ightarrow 2 mathrm{CO}_2+mathrm{N}_2$

Chemistry of the environment - Air quality and climate - State the symbol equation for photosynthesis, $6 mathrm{CO}_2+6 mathrm{H}_2 mathrm{O} ightarrow mathrm{C}_6 mathrm{H}_{12} mathrm{O}_6+6 mathrm{O}_2$

Organic chemistry - Formulae, functional groups and terminology - Draw and interpret the displayed formula of a molecule to show all the atoms and all the bonds

Organic chemistry - Formulae, functional groups and terminology - State that a homologous series is a family of similar compounds with similar chemical properties due to the presence of the same functional group

Organic chemistry - Formulae, functional groups and terminology - State that a saturated compound has molecules in which all carbon-carbon bonds are single bonds

Organic chemistry - Formulae, functional groups and terminology - State that an unsaturated compound has molecules in which one or more carbon-carbon bonds are not single bonds

Organic chemistry - Formulae, functional groups and terminology - State that a structural formula is an unambiguous description of the way the atoms in a molecule are arranged, including $mathrm{CH}_2=mathrm{CH}_2$, $mathrm{CH}_3 mathrm{CH}_2 mathrm{OH}, mathrm{CH}_3 mathrm{COOCH}_3$

Organic chemistry - Naming organic compounds - Name and draw the displayed formulae of: (a) methane and ethane (b) ethene (c) ethanol (d) ethanoic acid (e) the products of the reactions stated in sections 11.4-11.7

Organic chemistry - Naming organic compounds - State the type of compound present, given a chemical name ending in -ane, -ene, -ol, or -oic acid or from a molecular formula or displayed formula

Organic chemistry - Naming organic compounds - Name and draw the displayed formulae of the unbranched esters which can be made from unbranched alcohols and carboxylic acids, each containing up to four carbon atoms

Organic chemistry - Fuels - Name the fossil fuels: coal, natural gas and petroleum

Organic chemistry - Fuels - Name methane as the main constituent of natural gas

Organic chemistry - Fuels - State that hydrocarbons are compounds that contain hydrogen and carbon only

Organic chemistry - Fuels - State that petroleum is a mixture of hydrocarbons

Organic chemistry - Fuels - Describe the separation of petroleum into useful fractions by fractional distillation

Organic chemistry - Fuels - Describe how the properties of fractions obtained from petroleum change from the bottom to the top of the fractionating column, limited to: (a) decreasing chain length (b) higher volatility (c) lower boiling points (d) lower viscosity

Organic chemistry - Alkanes - State that the bonding in alkanes is single covalent and that alkanes are saturated hydrocarbons

Organic chemistry - Alkanes - Describe the properties of alkanes as being generally unreactive, except in terms of combustion and substitution by chlorine

Organic chemistry - Alkanes - State that in a substitution reaction one atom or group of atoms is replaced by another atom or group of atoms

Organic chemistry - Alkenes - State that the bonding in alkenes includes a double carbon-carbon covalent bond and that alkenes are unsaturated hydrocarbons

Organic chemistry - Alkenes - Describe the manufacture of alkenes and hydrogen by the cracking of larger alkane molecules using a high temperature and a catalyst

Organic chemistry - Alkenes - Describe the reasons for the cracking of larger alkane molecules

Organic chemistry - Alkenes - Describe the test to distinguish between saturated and unsaturated hydrocarbons by their reaction with aqueous bromine

Organic chemistry - Alkenes - State that in an addition reaction only one product is formed

Organic chemistry - Alcohols - Describe the combustion of ethanol

Organic chemistry - Alcohols - State the uses of ethanol as: (a) a solvent (b) a fuel

Organic chemistry - Alcohols - Describe the advantages and disadvantages of the manufacture of ethanol by: (a) fermentation (b) catalytic addition of steam to ethene

Organic chemistry - Carboxylic acids - Describe the reaction of ethanoic acid with: (a) metals (b) bases (c) carbonates including names and formulae of the salts produced

Organic chemistry - Carboxylic acids - Describe the formation of ethanoic acid by the oxidation of ethanol: (a) with acidified aqueous potassium manganate(VII) (b) by bacterial oxidation during vinegar production

Organic chemistry - Carboxylic acids - Describe the reaction of a carboxylic acid with an alcohol using an acid catalyst to form an ester

Organic chemistry - Polymers - Define polymers as large molecules built up from many smaller molecules called monomers

Organic chemistry - Polymers - Describe the formation of poly(ethene) as an example of addition polymerisation using ethene monomers

Organic chemistry - Polymers - State that plastics are made from polymers

Organic chemistry - Polymers - Describe how the properties of plastics have implications for their disposal

Organic chemistry - Polymers - Describe the environmental challenges caused by plastics, limited to: (a) disposal in land fill sites (b) accumulation in oceans (c) formation of toxic gases from burning

Organic chemistry - Polymers - Identify the repeat units and/or linkages in addition polymers and in condensation polymers

Organic chemistry - Polymers - Deduce the structure or repeat unit of an addition polymer from a given alkene and vice versa

Organic chemistry - Polymers - Deduce the structure or repeat unit of a condensation polymer from given monomers and vice versa, limited to: (a) polyamides from a dicarboxylic acid and a diamine (b) polyesters from a dicarboxylic acid and a diol

Organic chemistry - Polymers - Describe the differences between addition and condensation polymerisation

Organic chemistry - Polymers - Describe and draw the structure of: (a) nylon, a polyamide (b) PET, a polyester

Organic chemistry - Polymers - State that PET can be converted back into monomers and re-polymerised

Organic chemistry - Polymers - Describe proteins as natural polyamides and that they are formed from amino acid monomers with the general structure

Organic chemistry - Polymers - Describe and draw the structure of proteins as

Experimental techniques and chemical analysis - Experimental design - Name appropriate apparatus for the measurement of time, temperature, mass and volume, including: (a) stopwatches (b) thermometers (c) balances (d) burettes (e) volumetric pipettes (f) measuring cylinders (g) gas syringes

Experimental techniques and chemical analysis - Experimental design - Suggest advantages and disadvantages of experimental methods and apparatus

Experimental techniques and chemical analysis - Acid-base titrations - Describe an acid-base titration to include the use of a: (a) burette (b) volumetric pipette (c) suitable indicator

Experimental techniques and chemical analysis - Acid-base titrations - Describe how to identify the end-point of a titration using an indicator

Experimental techniques and chemical analysis - Chromatography - Describe how paper chromatography is used to separate mixtures of soluble coloured substances, using a suitable solvent

Experimental techniques and chemical analysis - Chromatography - Interpret simple chromatograms to identify: (a) unknown substances by comparison with known substances (b) pure and impure substances

Experimental techniques and chemical analysis - Chromatography - Describe how paper chromatography is used to separate mixtures of soluble colourless substances, using a suitable solvent and a locating agent

Experimental techniques and chemical analysis - Chromatography - State and use the equation for $R_{mathrm{f}}$ : $R_{mathrm{f}}=frac{ ext { distance travelled by substance }}{ ext { distance travelled by solvent }}$

Experimental techniques and chemical analysis - Separation and purification - Describe and explain methods of separation and purification using: (a) a suitable solvent (b) filtration (c) crystallisation (d) simple distillation (e) fractional distillation

Experimental techniques and chemical analysis - Separation and purification - Suggest suitable separation and purification techniques, given information about the substances involved

Experimental techniques and chemical analysis - Separation and purification - Identify substances and assess their purity using melting point and boiling point information

Experimental techniques and chemical analysis - Identification of ions and gases - Describe the use of a flame test to identify the cations: (a) lithium, $mathrm{Li}^{+}$ (b) sodium, $mathrm{Na}^{+}$ (c) potassium, $mathrm{K}^{+}$ (d) calcium, $mathrm{Ca}^{2+}$ (e) barium, $mathrm{Ba}^{2+}$ (f) copper(II), $mathrm{Cu}^{2+}$