stuart2022-11-29T13:49:09+00:001:01 understand the three states of matter in terms of the arrangement, movement and energy of the particles
stuart2022-11-30T13:57:13+00:001:02 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
stuart2023-09-18T10:54:46+00:001:03 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained
stuart2023-09-18T10:58:41+00:001:04 know what is meant by the terms: solvent, solute, solution, saturated solution
stuart2022-11-30T13:57:56+00:001:08 understand how to classify a substance as an element, a compound or a mixture
stuart2023-05-11T16:37:43+00:001:09 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
stuart2023-09-18T11:04:24+00:001:10 describe these experimental techniques for the separation of mixtures: simple distillation, fractional distillation, filtration, crystallisation, paper chromatography
stuart2023-09-18T11:02:13+00:001:11 understand how a chromatogram provides information about the composition of a mixture
stuart2023-09-18T11:02:34+00:001:12 understand how to use the calculation of Rf values to identify the components of a mixture
stuart2023-09-18T11:03:01+00:001:13 practical: investigate paper chromatography using inks/food colourings
stuart2022-11-30T14:11:04+00:001:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles
stuart2022-11-30T14:11:18+00:001:16 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Aᵣ)
stuart2022-11-30T14:11:27+00:001:17 be able to calculate the relative atomic mass of an element (Aᵣ) from isotopic abundances
stuart2023-01-10T12:19:15+00:001:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods
stuart2023-01-10T12:19:42+00:001:19 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table
stuart2023-01-10T12:25:58+00:001:20 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals
stuart2023-01-10T12:26:21+00:001:21 identify an element as a metal or a non-metal according to its position in the Periodic Table
stuart2023-01-10T12:26:36+00:001:22 understand how the electronic configuration of a main group element is related to its position in the Periodic Table
stuart2023-01-10T12:26:46+00:001:23 Understand why elements in the same group of the Periodic Table have similar chemical properties
stuart2023-09-18T11:05:10+00:001:25 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
stuart2022-11-30T14:12:46+00:001:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ)
stuart2018-04-25T21:37:27+00:001:27 know that the mole (mol) is the unit for the amount of a substance
stuart2018-04-25T21:37:27+00:001:28 understand how to carry out calculations involving amount of substance, relative atomic mass (Aᵣ) and relative formula mass (Mᵣ)
stuart2018-04-25T21:37:27+00:001:29 calculate reacting masses using experimental data and chemical equations
stuart2023-01-10T11:36:41+00:001:31 understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisation
stuart2023-01-10T08:29:26+00:001:32 know what is meant by the terms empirical formula and molecular formula
stuart2023-01-10T08:30:04+00:001:33 calculate empirical and molecular formulae from experimental data
stuart2019-03-16T10:58:55+00:001:36 practical: know how to determine the formula of a metal oxide by combustion (e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)
stuart2023-01-10T11:37:49+00:001:38 know the charges of these ions: metals in Groups 1, 2 and 3, non-metals in Groups 5, 6 and 7, Ag⁺, Cu²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Zn²⁺, hydrogen (H⁺), hydroxide (OH⁻), ammonium (NH₄⁺), carbonate (CO₃²⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻)
stuart2022-11-30T14:13:29+00:001:39 write formulae for compounds formed between the ions listed in 1:38
stuart2023-01-10T11:24:32+00:001:40 draw 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 be shown
stuart2023-01-10T11:24:55+00:001:42 understand why compounds with giant ionic lattices have high melting and boiling points
stuart2023-01-10T11:25:05+00:001:43 Know that ionic compounds do not conduct electricity when solid, but do conduct electricity when molten and in aqueous solution
stuart2023-01-10T11:26:44+00:001:44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons
stuart2023-01-10T11:28:29+00:001:46 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
stuart2023-01-10T11:29:01+00:001:47 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
stuart2023-01-10T11:29:19+00:001:48 explain why the melting and boiling points of substances with simple molecular structures increase, in general, with increasing relative molecular mass
stuart2023-01-10T11:30:25+00:001:49 explain why substances with giant covalent structures are solids with high melting and boiling points
stuart2023-01-10T11:30:51+00:001:50 explain how the structures of diamond, graphite and C60 fullerene influence their physical properties, including electrical conductivity and hardness
stuart2023-01-10T12:29:10+00:002:01 understand how the similarities in the reactions of lithium, sodium and potassium with water provide evidence for their recognition as a family of elements
stuart2023-01-10T12:29:20+00:002:02 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
stuart2023-01-10T12:29:32+00:002:03 use knowledge of trends in Group 1 to predict the properties of other alkali metals
stuart2023-01-10T11:50:40+00:002:05 know the colours, physical states (at room temperature) and trends in physical properties of chlorine, bromine and iodine
stuart2023-01-10T11:51:01+00:002:06 use knowledge of trends in Group 7 to predict the properties of other halogens
stuart2023-01-10T11:51:13+00:002:07 understand how displacement reactions involving halogens and halides provide evidence for the trend in reactivity in Group 7
stuart2023-09-18T11:05:32+00:002:09 know the approximate percentages by volume of the four most abundant gases in dry air
stuart2023-09-18T11:06:04+00:002:10 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
stuart2022-11-30T14:20:27+00:002:11 describe the combustion of elements in oxygen, including magnesium, hydrogen and sulfur
stuart2022-11-28T13:09:36+00:002:12 describe the formation of carbon dioxide from the thermal decomposition of metal carbonates, including copper(II) carbonate
stuart2022-11-30T14:20:45+00:002:13 know that carbon dioxide is a greenhouse gas and that increasing amounts in the atmosphere may contribute to climate change
stuart2023-09-18T11:06:27+00:002:14 Practical: determine the approximate percentage by volume of oxygen in air using a metal or a non-metal
stuart2023-01-10T12:30:26+00:002:15 understand how metals can be arranged in a reactivity series based on their reactions with: water and dilute hydrochloric or sulfuric acid
stuart2023-01-10T12:30:47+00:002:16 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
stuart2023-01-10T12:31:04+00:002:17 know the order of reactivity of these metals: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver, gold
stuart2023-01-10T12:31:29+00:002:19 understand how the rusting of iron may be prevented by: barrier methods, galvanising and sacrificial protection
stuart2023-04-19T10:58:30+00:002:20 in terms of gain or loss of oxygen and loss or gain of electrons, understand the terms: oxidation, reduction, redox, oxidising agent, reducing agent, in terms of gain or loss of oxygen and loss or gain of electrons
stuart2023-01-10T12:32:04+00:002:21 practical: investigate reactions between dilute hydrochloric and sulfuric acids and metals (e.g. magnesium, zinc and iron)
stuart2023-01-13T22:06:03+00:002:28 describe the use of litmus, phenolphthalein and methyl orange to distinguish between acidic and alkaline solutions
stuart2023-01-10T11:38:25+00:002:29 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)
stuart2023-01-10T11:39:19+00:002:30 describe the use of Universal Indicator to measure the approximate pH value of an aqueous solution
stuart2023-01-10T11:39:28+00:002:31 know that acids in aqueous solution are a source of hydrogen ions and alkalis in a aqueous solution are a source of hydroxide ions
stuart2023-01-10T11:40:19+00:002:34 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)
stuart2023-01-10T11:41:38+00:002:36 understand that an acid is a proton donor and a base is a proton acceptor
stuart2023-01-10T11:41:49+00:002:37 describe 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 salts
stuart2023-01-10T11:42:29+00:002:38 know that metal oxides, metal hydroxides and ammonia can act as bases, and that alkalis are bases that are soluble in water
stuart2023-01-10T11:42:40+00:002:39 describe an experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reactant
stuart2023-09-18T11:07:48+00:002:42 practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting from copper(II) oxide
stuart2023-01-10T11:43:33+00:002:44 describe tests for these gases: hydrogen, oxygen, carbon dioxide, ammonia, chlorine
stuart2023-01-10T11:44:14+00:002:46 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
stuart2023-01-10T11:44:30+00:002:47 describe tests for these cations: NH₄⁺ using sodium hydroxide solution and identifying the gas evolved, Cu²⁺, Fe²⁺ and Fe³⁺ using sodium hydroxide solution
stuart2022-12-12T11:10:04+00:002:48a describe a test for CO₃²⁻ using hydrochloric acid and identifying the gas evolved
stuart2023-01-10T11:44:43+00:002:48 describe tests for these anions: Cl⁻, Br⁻ and I⁻ using acidified silver nitrate solution, SO₄²⁻ using acidified barium chloride solution, CO₃²⁻ using hydrochloric acid and identifying the gas evolved
stuart2023-01-10T11:15:29+00:002:49 describe a test for the presence of water using anhydrous copper(II) sulfate
stuart2023-09-18T11:08:18+00:002:50 describe a physical test to show whether a sample of water is pure
stuart2023-01-10T11:58:37+00:003:01 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
stuart2023-01-10T11:58:51+00:003:02 describe simple calorimetry experiments for reactions such as combustion, displacement, dissolving and neutralisation
stuart2023-03-06T17:22:19+00:003:03 calculate the heat energy change from a measured temperature change using the expression Q = mcΔT
stuart2023-01-10T11:59:12+00:003:04 calculate the molar enthalpy change (ΔH) from the heat energy change, Q
stuart2023-01-10T11:59:24+00:003:08 practical: investigate temperature changes accompanying some of the following types of change: salts dissolving in water, neutralisation reactions, displacement reactions and combustion reactions
stuart2022-11-02T20:24:20+00:003:09 describe 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 reaction
stuart2022-11-30T14:30:11+00:003:10 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
stuart2023-01-10T11:19:55+00:003:11 explain 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 theory
stuart2023-01-10T11:20:08+00:003:12 know that a catalyst is a substance that increases the rate of a reaction, but is chemically unchanged at the end of the reaction
stuart2022-10-19T07:44:49+00:003:13 know that a catalyst works by providing an alternative pathway with lower activation energy
stuart2022-11-30T14:30:40+00:003:15 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
stuart2019-10-25T11:26:46+00:003:16 practical: investigate the effect of different solids on the catalytic decomposition of hydrogen peroxide solution
stuart2023-01-10T11:20:32+00:003:17 know that some reactions are reversible and this is indicated by the symbol ⇌ in equations
stuart2023-01-10T11:20:40+00:003:18 describe reversible reactions such as the dehydration of hydrated copper(II) sulfate and the effect of heat on ammonium chloride
stuart2023-01-10T08:33:05+00:004:01 know that a hydrocarbon is a compound of hydrogen and carbon only
stuart2023-01-10T08:33:16+00:004:02 understand how to represent organic molecules using empirical formulae, molecular formulae, general formulae, structural formulae and displayed formulae
stuart2023-01-10T08:33:27+00:004:03 know what is meant by the terms homologous series, functional group and isomerism
stuart2023-01-10T08:33:38+00:004:04 understand 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 atoms
stuart2023-01-10T08:33:53+00:004:05 understand how to write the possible structural and displayed formulae of an organic molecule given its molecular formula
stuart2023-01-10T08:34:04+00:004:06 understand how to classify reactions of organic compounds as substitution, addition and combustion. Knowledge of reaction mechanisms is not required
stuart2023-01-10T08:34:25+00:004:08 describe how the industrial process of fractional distillation separates crude oil into fractions
stuart2023-01-10T08:34:49+00:004:09 know the names and uses of the main fractions obtained from crude oil: refinery gases, gasoline, kerosene, diesel, fuel oil and bitumen
stuart2023-01-10T08:35:37+00:004:10 know the trend in colour, boiling point and viscosity of the main fractions
stuart2023-01-10T08:35:44+00:004:11 know that a fuel is a substance that, when burned, releases heat energy
stuart2023-01-10T08:35:55+00:004:12 know the possible products of complete and incomplete combustion of hydrocarbons with oxygen in the air
stuart2023-01-10T08:36:04+00:004:13 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
stuart2023-01-10T08:36:12+00:004:14 know that, in car engines, the temperature reached is high enough to allow nitrogen and oxygen from air to react, forming oxides of nitrogen
stuart2023-01-10T08:36:20+00:004:15 explain how the combustion of some impurities in hydrocarbon fuels results in the formation of sulfur dioxide
stuart2023-01-10T08:36:29+00:004:16 understand how sulfur dioxide and oxides of nitrogen oxides contribute to acid rain
stuart2023-01-10T08:36:43+00:004:17 describe 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 600–700⁰C)
stuart2023-01-10T08:36:51+00:004:18 explain why cracking is necessary, in terms of the balance between supply and demand for different fractions
stuart2023-01-10T11:04:20+00:004:21 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
stuart2018-04-25T21:51:10+00:004:22 describe the reactions of alkanes with halogens in the presence of ultraviolet radiation, limited to mono-substitution knowledge of reaction mechanisms is not required
stuart2023-01-10T11:05:17+00:004:26 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
stuart2018-04-25T21:51:58+00:004:27 describe the reactions of alkenes with bromine, to produce dibromoalkanes
stuart2022-11-30T14:58:16+00:004:28 describe how bromine water can be used to distinguish between an alkane and an alkene
stuart2023-01-10T11:05:50+00:004:44 know that an addition polymer is formed by joining up many small molecules called monomers
stuart2023-01-10T11:06:01+00:004:45 understand how to draw the repeat unit of an addition polymer, including poly(ethene), poly(propene), poly(chloroethene) and (poly)tetrafluroethene
stuart2023-01-10T11:06:29+00:004:46 understand how to deduce the structure of a monomer from the repeat unit of an addition polymer and vice versa
stuart2022-11-30T14:59:29+00:004:47 explain problems in the disposal of addition polymers, including: their inertness and inability to biodegrade, the production of toxic gases when they are burned
