GCSE Chemistry Full Spec Points (single only)

1:01 understand the three states of matter in terms of the arrangement, movement and energy of the particles

1:02 understand the interconversions between the three states of matter in terms of: the names of the interconversions, how they are achieved and the changes in arrangement, movement and energy of the particles

1:03 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained

1:08 understand how to classify a substance as an element, a compound or a mixture

1:09 understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperatures

1:10 describe these experimental techniques for the separation of mixtures: simple distillation, fractional distillation, filtration, crystallisation, paper chromatography

1:11 understand how a chromatogram provides information about the composition of a mixture

1:12 understand how to use the calculation of Rf values to identify the components of a mixture

1:13 practical: investigate paper chromatography using inks/food colourings

1:14 know what is meant by the terms atom and molecule

1:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles

1:16 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Aᵣ)

1:17 be able to calculate the relative atomic mass of an element (Aᵣ) from isotopic abundances

1:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods

1:21 identify an element as a metal or a non-metal according to its position in the Periodic Table

1:25 write word equations and balanced chemical equations (including state symbols): for reactions studied in this specification and for unfamiliar reactions where suitable information is provided

1:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ)

1:37 understand how ions are formed by electron loss or gain

1:38b know the charges of these ions: metals in Groups 1, 2 and 3, non-metals in Groups 5, 6 and 7, hydrogen (H⁺), hydroxide (OH⁻), ammonium (NH₄⁺), carbonate (CO₃²⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻)

1:39 write formulae for compounds formed between the ions listed in 1:38

1:41 understand ionic bonding in terms of electrostatic attractions

1:42 understand why compounds with giant ionic lattices have high melting and boiling points

1:44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons

1:47 explain 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 molecules

1:49 explain why substances with giant covalent structures are solids with high melting and boiling points

2:01 understand how the similarities in the reactions of lithium, sodium and potassium with water provide evidence for their recognition as a family of elements

2:02 understand how the differences between the reactions of lithium, sodium and potassium with air and water provide evidence for the trend in reactivity in Group 1

2:03 use knowledge of trends in Group 1 to predict the properties of other alkali metals

2:05 know the colours, physical states (at room temperature) and trends in physical properties of chlorine, bromine and iodine

2:06 use knowledge of trends in Group 7 to predict the properties of other halogens

2:09 know the approximate percentages by volume of the four most abundant gases in dry air

2:10 understand 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 air

2:11 describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfur

2:13 know that carbon dioxide is a greenhouse gas and that increasing amounts in the atmosphere may contribute to climate change

2:14 Practical: determine the approximate percentage by volume of oxygen in air using a metal or a non-metal

2:15 understand how metals can be arranged in a reactivity series based on their reactions with: water and dilute hydrochloric or sulfuric acid

2:17 know the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, gold

2:18 know the conditions under which iron rusts

2:19a understand how the rusting of iron may be prevented by: barrier methods, galvanising

2:28a describe the use of litmus to distinguish between acidic and alkaline solutions

2:29 understand 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)

2:30 describe the use of Universal Indicator to measure the approximate pH value of an aqueous solution

2:31 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ions

2:32 know that bases can neutralise acids

2:44 describe tests for these gases: hydrogen, oxygen, carbon dioxide, ammonia, chlorine

2:45 describe how to carry out a flame test

2:46 know the colours formed in flame tests for these cations: Li⁺ is red, Na⁺ is yellow, K⁺ is lilac, Ca²⁺ is orange-red, Cu²⁺ is blue-green

2:48a describe a test for CO₃²⁻ using hydrochloric acid and identifying the gas evolved

2:49 describe a test for the presence of water using anhydrous copper(II) sulfate

3:01 know 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 endothermic

3:02 describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisation

3:03 calculate the heat energy change from a measured temperature change using the expression Q = mcΔT

3:08 practical: investigate temperature changes accompanying some of the following types of change: salts dissolving in water, neutralisation reactions, displacement reactions and combustion reactions

3:10 describe 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 reaction

3:12 know that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reaction

3:15 practical: 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 acid

4:01 know that a hydrocarbon is a compound of hydrogen and carbon only

4:02a understand how to represent organic molecules using molecular formulae, general formulae, structural formulae and displayed formulae

4:07 know that crude oil is a mixture of hydrocarbons

4:09 know the names and uses of the main fractions obtained from crude oil: refinery gases, gasoline, kerosene, diesel, fuel oil and bitumen

4:10 know the trend in colour, boiling point and viscosity of the main fractions

4:11 know that a fuel is a substance that, when burned, releases heat energy

4:12 know the possible products of complete and incomplete combustion of hydrocarbons with oxygen in the air

4:13 understand why carbon monoxide is poisonous, in terms of its effect on the capacity of blood to transport oxygen references to haemoglobin are not required

4:14 know that, in car engines, the temperature reached is high enough to allow nitrogen and oxygen from air to react, forming oxides of nitrogen

4:15 explain how the combustion of some impurities in hydrocarbon fuels results in the formation of sulfur dioxide

4:16 understand how sulfur dioxide and oxides of nitrogen oxides contribute to acid rain

4:19 know the general formula for alkanes

4:20 explain why alkanes are classified as saturated hydrocarbons

4:21 understand 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 isomers

4:23 know that alkenes contain the functional group >C=C<

4:24 know the general formula for alkenes

4:25 explain why alkenes are classified as unsaturated hydrocarbons

4:26 understand 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 required

4:28 describe how bromine water can be used to distinguish between an alkane and an alkene

4:44 know that an addition polymer is formed by joining up many small molecules called monomers

4:45a understand how to draw the repeat unit of an addition polymer poly(ethene)

4:46 understand how to deduce the structure of a monomer from the repeat unit of an addition polymer and vice versa

4:47 explain problems in the disposal of addition polymers, including: their inertness and inability to biodegrade, the production of toxic gases when they are burned