Science (Double Award) — Chemistry

Science 4SD0 — specification explorer

All 131 specification statements from the official Pearson Edexcel specification, as printed — filter by paper, unit or tier exactly as Pearson Edexcel assesses them.

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131 spec points

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Assessment homes come from the parsed Pearson specification (content summaries & assessment overviews). Hover a chip for the printed rule. Filters appear only where the qualification has that structure — a linear IGCSE has no unit scope, and only Maths A splits Foundation / Higher tiers.

1. Principles of chemistry

1. States of matter

C1.1understand the three states of matter in terms of the arrangement, movement and energy of the particlesPaper 1Paper 2Also in Double Award
C1.2
understand the interconversions between the three states of matter in terms of:
- the names of the interconversions
- how they are achieved
- the changes in arrangement, movement and energy of the particles
Paper 1Paper 2Also in Double Award
C1.3understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explainedPaper 1Paper 2Also in Double Award
C1.4
know what is meant by the terms:
- solvent
- solute
- solution
- saturated solution
Paper 1Paper 2Also in Double Award

2. Elements, compounds and mixtures

C1.8understand how to classify a substance as an element, compound or mixturePaper 1Paper 2Also in Double Award
C1.9understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperaturesPaper 1Paper 2Also in Double Award
C1.10
describe these experimental techniques for the separation of mixtures:
- simple distillation
- fractional distillation
- filtration
- crystallisation
- paper chromatography
Paper 1Paper 2Also in Double Award
C1.11understand how a chromatogram provides information about the composition of a mixturePaper 1Paper 2Also in Double Award
C1.12understand how to use the calculation of R f values to identify the components of a mixturePaper 1Paper 2Also in Double Award
C1.13practical: investigate paper chromatography using inks/food colouringsPaper 1Paper 2Also in Double Award

3. Atomic structure

C1.14know what is meant by the terms ‘atom’ and ‘molecule’Paper 1Paper 2Also in Double Award
C1.15know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particlesPaper 1Paper 2Also in Double Award
C1.16know what is meant by the terms: atomic number, mass number, isotopes and relative atomic mass (Ar)Paper 1Paper 2Also in Double Award
C1.17be able to calculate the relative atomic mass of an element (Ar) from isotopic abundancesPaper 1Paper 2Also in Double Award

4. The Periodic Table

C1.18
understand how elements are arranged in the Periodic Table:
- in order of atomic number
- in groups and periods
Paper 1Paper 2Also in Double Award
C1.19understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic TablePaper 1Paper 2Also in Double Award
C1.20understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metalsPaper 1Paper 2Also in Double Award
C1.21identify an element as a metal or a non-metal according to its position in the Periodic TablePaper 1Paper 2Also in Double Award
C1.22understand how the electronic configuration of a main group element is related to its position in the Periodic TablePaper 1Paper 2Also in Double Award
C1.23understand why elements in the same group of the Periodic Table have similar chemical propertiesPaper 1Paper 2Also in Double Award
C1.24understand why the noble gases (Group 0) do not readily reactPaper 1Paper 2Also in Double Award

5. Chemical formulae, equations and calculations

C1.25
write word equations and balanced chemical equations (including state symbols):
- for reactions studied in this specification
- for unfamiliar reactions where suitable information is provided
Paper 1Paper 2Also in Double Award
C1.26calculate relative formula masses (including relative molecular masses) (Mr) from relative atomic masses (Ar)Paper 1Paper 2Also in Double Award
C1.27know that the mole (mol) is the unit for the amount of a substancePaper 1Paper 2Also in Double Award
C1.28understand how to carry out calculations involving amount of substance, relative atomic mass (Ar) and relative formula mass (Mr)Paper 1Paper 2Also in Double Award
C1.29calculate reacting masses using experimental data and chemical equationsPaper 1Paper 2Also in Double Award
C1.30calculate percentage yieldPaper 1Paper 2Also in Double Award
C1.31understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisationPaper 1Paper 2Also in Double Award
C1.32know what is meant by the terms ‘empirical formula’ and ‘molecular formula’Paper 1Paper 2Also in Double Award
C1.33calculate empirical and molecular formulae from experimental dataPaper 1Paper 2Also in Double Award
C1.36practical: know how to determine the formula of a metal oxide by combustion (e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)Paper 1Paper 2Also in Double Award

6. Ionic bonding

C1.37understand how ions are formed by electron loss or gainPaper 1Paper 2Also in Double Award
C1.38
know the charges of these ions:
- metals in Groups 1, 2 and 3
- non-metals in Groups 5, 6 and 7
- Ag + , Cu 2+ , Fe 2+ , Fe 3+ , Pb 2+ , Zn 2+
- hydrogen (H + ), hydroxide (OH – ), ammonium (NH 4 + ), carbonate (CO 3 2– ), nitrate (NO 3 - ), sulfate (SO 4 2– )
Paper 1Paper 2Also in Double Award
C1.39write formulae for compounds formed between the ions listed abovePaper 1Paper 2Also in Double Award
C1.40draw dot-and-cross diagrams to show the formation of ionic compounds by electron transfer, limited to combinations of elements from Groups 1, 2, 3 and 5, 6, 7 only outer electrons need to be shownPaper 1Paper 2Also in Double Award
C1.41understand ionic bonding in terms of electrostatic attractionsPaper 1Paper 2Also in Double Award
C1.42understand why compounds with giant ionic lattices have high melting and boiling pointsPaper 1Paper 2Also in Double Award
C1.43know that ionic compounds do not conduct electricity when solid, but do conduct electricity when molten and in aqueous solutionPaper 1Paper 2Also in Double Award

7. Covalent bonding

C1.44know that a covalent bond is formed between atoms by the sharing of a pair of electronsPaper 1Paper 2Also in Double Award
C1.45understand covalent bonds in terms of electrostatic attractionsPaper 1Paper 2Also in Double Award
C1.46
understand how to use dot-and-cross diagrams to represent covalent bonds in:
- diatomic molecules, including hydrogen, oxygen, nitrogen, halogens and hydrogen halides
- inorganic molecules including water, ammonia and carbon dioxide
- organic molecules containing up to two carbon atoms, including methane, ethane, ethene and those containing halogen atoms
Paper 1Paper 2Also in Double Award
C1.47explain why substances with a simple molecular structures are gases or liquids, or solids with low melting and boiling points the term ‘intermolecular’ forces of attraction can be used to represent all forces between moleculesPaper 1Paper 2Also in Double Award
C1.48explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular massPaper 1Paper 2Also in Double Award
C1.49explain why substances with giant covalent structures are solids with high melting and boiling pointsPaper 1Paper 2Also in Double Award
C1.50explain how the structures of diamond, graphite and C 60 fullerene influence their physical properties, including electrical conductivity and hardnessPaper 1Paper 2Also in Double Award
C1.51know that covalent compounds do not usually conduct electricityPaper 1Paper 2Also in Double Award

2. Inorganic chemistry

1. Group 1 (alkali metals) – lithium, sodium and potassium

C2.1understand how the similarities in the reactions of these elements with water provide evidence for their recognition as a family of elementsPaper 1Paper 2Also in Double Award
C2.2understand how the differences between the reactions of these elements with air and water provide evidence for the trend in reactivity in Group 1Paper 1Paper 2Also in Double Award
C2.3use knowledge of trends in Group 1 to predict the properties of other alkali metalsPaper 1Paper 2Also in Double Award

2. Group 7 (halogens) – chlorine, bromine and iodine

C2.5know the colours, physical states (at room temperature) and trends in physical properties of these elementsPaper 1Paper 2Also in Double Award
C2.6use knowledge of trends in Group 7 to predict the properties of other halogensPaper 1Paper 2Also in Double Award
C2.7understand how displacement reactions involving halogens and halides provide evidence for the trend in reactivity in Group 7Paper 1Paper 2Also in Double Award

3. Gases in the atmosphere

C2.9know the approximate percentages by volume of the four most abundant gases in dry airPaper 1Paper 2Also in Double Award
C2.10understand how to determine the percentage by volume of oxygen in air using experiments involving the reactions of metals (e.g. iron) and non-metals (e.g. phosphorus) with airPaper 1Paper 2Also in Double Award
C2.11describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfurPaper 1Paper 2Also in Double Award
C2.12describe the formation of carbon dioxide from the thermal decomposition of metal carbonates, including copper(II) carbonatePaper 1Paper 2Also in Double Award
C2.13know that carbon dioxide is a greenhouse gas and that increasing amounts in the atmosphere may contribute to climate changePaper 1Paper 2Also in Double Award
C2.14practical: determine the approximate percentage by volume of oxygen in air using a metal or a non-metalPaper 1Paper 2Also in Double Award

4. Reactivity series

C2.15
understand how metals can be arranged in a reactivity series based on their reactions with:
- water
- dilute hydrochloric or sulfuric acid
Paper 1Paper 2Also in Double Award
C2.16
understand how metals can be arranged in a reactivity series based on their displacement reactions between:
- metals and metal oxides
- metals and aqueous solutions of metal salts
Paper 1Paper 2Also in Double Award
C2.17know the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, goldPaper 1Paper 2Also in Double Award
C2.18know the conditions under which iron rustsPaper 1Paper 2Also in Double Award
C2.19
understand how the rusting of iron may be prevented by:
- barrier methods
- galvanising
- sacrificial protection
Paper 1Paper 2Also in Double Award
C2.20
understand the terms:
- oxidation
- reduction
- redox
- oxidising agent
- reducing agent in terms of gain or loss of oxygen and loss or gain of electrons
Paper 1Paper 2Also in Double Award
C2.21practical: investigate reactions between dilute hydrochloric and sulfuric acids, and metals (e.g. magnesium, zinc and iron)Paper 1Paper 2Also in Double Award

5. Acids, alkalis and titrations

C2.28describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutionsPaper 1Paper 2Also in Double Award
C2.29understand how to use the pH scale, from 0–14, can be used to classify solutions as strongly acidic (0–3), weakly acidic (4–6), neutral (7), weakly alkaline (8–10) and strongly alkaline (11–14)Paper 1Paper 2Also in Double Award
C2.30describe the use of universal indicator to measure the approximate pH value of an aqueous solutionPaper 1Paper 2Also in Double Award
C2.31know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ionsPaper 1Paper 2Also in Double Award
C2.32know that alkalis can neutralise acidsPaper 1Paper 2Also in Double Award
C2.34
know the general rules for predicting the solubility of ionic compounds in water:
- common sodium, potassium and ammonium compounds are soluble
- all nitrates are soluble
- common chlorides are soluble, except those of silver and lead(II)
- common sulfates are soluble, except for those of barium, calcium and lead(II)
- common carbonates are insoluble, except for those of sodium, potassium and ammonium
- common hydroxides are insoluble except for those of sodium, potassium and calcium (calcium hydroxide is slightly soluble)
Paper 1Paper 2Also in Double Award
C2.35understand acids and bases in terms of proton transferPaper 1Paper 2Also in Double Award
C2.36understand that an acid is a proton donor and a base is a proton acceptorPaper 1Paper 2Also in Double Award
C2.37describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, bases and metal carbonates (excluding the reactions between nitric acid and metals) to form saltsPaper 1Paper 2Also in Double Award
C2.38know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in waterPaper 1Paper 2Also in Double Award
C2.39describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactantPaper 1Paper 2Also in Double Award
C2.42practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxidePaper 1Paper 2Also in Double Award

6. Chemical tests

C2.44
describe tests for these gases:
- hydrogen
- oxygen
- carbon dioxide
- ammonia
- chlorine
Paper 1Paper 2Also in Double Award
C2.45describe how to carry out a flame testPaper 1Paper 2Also in Double Award
C2.46
know the colours formed in flame tests for these cations:
- Li + is red
- Na + is yellow
- K + is lilac
- Ca 2+ is orange-red
- Cu 2+ is blue-green
Paper 1Paper 2Also in Double Award
C2.47
describe tests for these cations:
- NH 4 + using sodium hydroxide solution and identifying the gas evolved
- Cu 2+ , Fe 2+ and Fe 3+ using sodium hydroxide solution
Paper 1Paper 2Also in Double Award
C2.48
describe tests for these anions:
- Cl – , Br – and I – using acidified silver nitrate solution
- SO 4 2– using acidified barium chloride solution
- CO 3 2– using hydrochloric acid and identifying the gas evolved
Paper 1Paper 2Also in Double Award
C2.49describe a test for the presence of water using anhydrous copper(II) sulfatePaper 1Paper 2Also in Double Award
C2.50describe a physical test to show whether a sample of water is purePaper 1Paper 2Also in Double Award

3. Physical chemistry

1. Energetics

C3.1know that chemical reactions in which heat energy is given out are described as exothermic and those in which heat energy is taken in are described as endothermicPaper 1Paper 2Also in Double Award
C3.2describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisationPaper 1Paper 2Also in Double Award
C3.3calculate the heat energy change from a measured temperature change using the expression Q = m c Δ TPaper 1Paper 2Also in Double Award
C3.4calculate the molar enthalpy change (ΔH) from the heat energy change QPaper 1Paper 2Also in Double Award
C3.8
practical: investigate temperature changes accompanying some of the following types of change:
- salts dissolving in water
- neutralisation reactions
- displacement reactions
- combustion reactions
Paper 1Paper 2Also in Double Award

2. Rates of reaction

C3.9describe experiments to investigate the effects of changes in surface area of a solid, concentration of a solution, temperature and the use of a catalyst on the rate of a reactionPaper 1Paper 2Also in Double Award
C3.10describe the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas, temperature and the use of a catalyst on the rate of a reactionPaper 1Paper 2Also in Double Award
C3.11explain the effects of changes in surface area of a solid, concentration of a solution, pressure of a gas and temperature on the rate of a reaction in terms of particle collision theoryPaper 1Paper 2Also in Double Award
C3.12know that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reactionPaper 1Paper 2Also in Double Award
C3.13know that a catalyst works by providing an alternative pathway with lower activation energyPaper 1Paper 2Also in Double Award
C3.15practical: investigate the effect of changing the surface area of marble chips and of changing the concentration of hydrochloric acid on the rate of reaction between marble chips and dilute hydrochloric acidPaper 1Paper 2Also in Double Award
C3.16practical: investigate the effect of different solids on the catalytic decomposition of hydrogen peroxide solutionPaper 1Paper 2Also in Double Award

3. Reversible reactions and equilibria

C3.17know that some reactions are reversible and that this is indicated by the symbol ⇌ in equationsPaper 1Paper 2Also in Double Award
C3.18describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloridePaper 1Paper 2Also in Double Award

4. Organic chemistry

1. Introduction

C4.1know that a hydrocarbon is a compound of hydrogen and carbon onlyPaper 1Paper 2Also in Double Award
C4.2understand how to represent organic molecules using empirical formulae, molecular formulae, general formulae, structural formulae and displayed formulaePaper 1Paper 2Also in Double Award
C4.3know what is meant by the terms: homologous series, functional group and isomerismPaper 1Paper 2Also in Double Award
C4.4understand how to name compounds relevant to this specification using the rules of International Union of Pure and Applied Chemistry (IUPAC) nomenclature students will be expected to name compounds containing up to six carbon atomsPaper 1Paper 2Also in Double Award
C4.5understand how to write the possible structural and displayed formulae of an organic molecule given its molecular formulaPaper 1Paper 2Also in Double Award
C4.6understand how to classify reactions of organic compounds as substitution, addition and combustion knowledge of reaction mechanisms is not requiredPaper 1Paper 2Also in Double Award

2. Crude oil

C4.7know that crude oil is a mixture of hydrocarbonsPaper 1Paper 2Also in Double Award
C4.8describe how the industrial process of fractional distillation separates crude oil into fractionsPaper 1Paper 2Also in Double Award
C4.9know the names and uses of the main fractions obtained from crude oil: refinery gases, gasoline, kerosene, diesel, fuel oil and bitumenPaper 1Paper 2Also in Double Award
C4.10know the trend in colour, boiling point and viscosity of the main fractionsPaper 1Paper 2Also in Double Award
C4.11know that a fuel is a substance that, when burned, releases heat energyPaper 1Paper 2Also in Double Award
C4.12know the possible products of complete and incomplete combustion of hydrocarbons with oxygen in the airPaper 1Paper 2Also in Double Award
C4.13understand why carbon monoxide is poisonous, in terms of its effect on the capacity of blood to transport oxygen references to haemoglobin are not requiredPaper 1Paper 2Also in Double Award
C4.14know that, in car engines, the temperature reached is high enough to allow nitrogen and oxygen from air to react, forming oxides of nitrogenPaper 1Paper 2Also in Double Award
C4.15explain how the combustion of some impurities in hydrocarbon fuels results in the formation of sulfur dioxidePaper 1Paper 2Also in Double Award
C4.16understand how sulfur dioxide and oxides of nitrogen contribute to acid rainPaper 1Paper 2Also in Double Award
C4.17describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by catalytic cracking (using silica or alumina as the catalyst and a temperature in the range of 600–700 ºC)Paper 1Paper 2Also in Double Award
C4.18explain why cracking is necessary, in terms of the balance between supply and demand for different fractionsPaper 1Paper 2Also in Double Award

3. Alkanes

C4.19know the general formula for alkanesPaper 1Paper 2Also in Double Award
C4.20explain why alkanes are classified as saturated hydrocarbonsPaper 1Paper 2Also in Double Award
C4.21understand how to draw the structural and displayed formulae for alkanes with up to five carbon atoms in the molecule, and to name the unbranched-chain isomersPaper 1Paper 2Also in Double Award
C4.22describe the reactions of alkanes with halogens in the presence of ultraviolet radiation, limited to mono-substitution knowledge of reaction mechanisms is not requiredPaper 1Paper 2Also in Double Award

4. Alkenes

C4.23know that alkenes contain the functional group >C=C<Paper 1Paper 2Also in Double Award
C4.24know the general formula for alkenesPaper 1Paper 2Also in Double Award
C4.25explain why alkenes are classified as unsaturated hydrocarbonsPaper 1Paper 2Also in Double Award
C4.26understand how to draw the structural and displayed formulae for alkenes with up to four carbon atoms in the molecule, and name the unbranched-chain isomers knowledge of cis/trans or E/Z notation is not requiredPaper 1Paper 2Also in Double Award
C4.27describe the reactions of alkenes with bromine to produce dibromoalkanesPaper 1Paper 2Also in Double Award
C4.28describe how bromine water can be used to distinguish between an alkane and an alkenePaper 1Paper 2Also in Double Award
C4.41, 4.42, 4.43 are in the Pearson Edexcel International GCSE in Chemistry only.Paper 1Paper 2Also in Double Award

5. Synthetic polymers

C4.44know that an addition polymer is formed by joining up many small molecules called monomersPaper 1Paper 2Also in Double Award
C4.45understand how to draw the repeat unit of an addition polymer, including poly(ethene), poly(propene), poly(chloroethene) and (poly)tetrafluoroethenePaper 1Paper 2Also in Double Award
C4.46understand how to deduce the structure of a monomer from the repeat unit of an addition polymer and vice versaPaper 1Paper 2Also in Double Award
C4.47
explain problems in the disposal of addition polymers, including:
- their inertness and inability to biodegrade
- the production of toxic gases when they are burned
Paper 1Paper 2Also in Double Award