4.1Atomic structure and the periodic table
4.1.3Properties of transition metals (chemistry only)
4.1.3.2 Typical properties
07.7 — Identifying where in the periodic table catalytic converter elements are most likely found
10.5 — Identifying which metal ion could form a coloured equilibrium mixture with thiocyanate ions
07.5 — Identifying the most likely metal in a metal oxide catalyst, using the periodic table
4.2Bonding, structure, and the properties of matter
4.2.2How bonding and structure are related to the properties of substances
4.2.2.2 State symbols
05.1 — Explaining why a reaction mixture becomes cloudy, using a given equation
03.1 — Identifying which state symbol does not represent one of the three states of matter
10.1 — Naming the solvent used to dissolve ions in a reaction
4.3Quantitative chemistry
4.3.1Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
4.3.1.1 Conservation of mass and balanced chemical equations
07.5 — Completing and balancing the equation for nitrogen dioxide decomposition
10.7 — Writing a balanced equation for the complete combustion of an alcohol (4.7.2.3 — alcohols context noted)
04.3 — Completing and balancing the equation for the complete combustion of a hydrocarbon (4.7.1.3 — hydrocarbon context noted)
05.1 — Completing and balancing the equation for an ore reacting with oxygen
08.4 — Writing a balanced equation for the complete combustion of a compound
09.1 — Completing and balancing the equation for calcium carbonate reacting with hydrochloric acid
4.3.1.2 Relative formula mass
06.4 — Calculating the percentage by mass of an element in a compound, from relative atomic and formula masses
05.2 — Calculating the percentage by mass of an element in a compound (MS 1c)
08.5 — Calculating the relative formula mass of part of an amino acid molecule
4.3.1.3 Mass changes when a reactant or product is a gas
08.1 — Explaining why the contents of a conical flask lose mass during a reaction
07.3 — Explaining what happens to the mass of a flask during an acid-carbonate reaction
02.2 — Explaining why the mass of a test tube and contents decreased on heating
07.2 — Explaining why the mass of a flask and contents decreased during a reaction
08.1 — Explaining why a conical flask and contents lost mass during a reaction
4.3.1.4 Chemical measurements
02.1 — Determining the mass of an empty test tube from experimental measurement data
02.3 — Suggesting why heating continued until mass no longer changed (WS 2.6/3.7 — measurement validity)
4.3.2Use of amount of substance in relation to masses of pure substances
4.3.2.1 Moles (HT only)
09.2 — Identifying the number of moles of hydrogen from given data
4.3.2.2 Amounts of substances in equations (HT only)
09.1 — Calculating the maximum mass of water produced from a hydrated compound, using the reacting mole ratio
09.2 — Calculating a related stoichiometric mass value for a hydrated compound reaction
4.3.3Yield and atom economy of chemical reactions (chemistry only)
4.3.3.2 Atom economy
10.1 — Calculating the atom economy of a reaction from relative atomic masses
07.2 — Explaining how an equation shows a reaction has 100% atom economy
4.3.5Use of amount of substance in relation to volumes of gases (chemistry only) (HT only)
4.3.5 Use of amount of substance in relation to volumes of gases
05.4 — Calculating the volume of a gas at room temperature and pressure from reaction data
05.4 — Calculating the volume of air needed to supply oxygen for a given volume of hydrogen
05.7 — Calculating the volume of a gas at room temperature and pressure from its mass
4.4Chemical changes
4.4.2Reactions of acids
4.4.2.6 Strong and weak acids (HT only)
07.2 — Explaining how an ionisation equation shows that ethanoic acid is a weak acid — general weak-acid ionisation content, not carboxylic-acid-specific
4.5Energy changes
4.5.1Exothermic and endothermic reactions
4.5.1.1 Energy transfer during exothermic and endothermic reactions
02.4 — Calculating energy taken in during an endothermic reaction, to 3 significant figures (MS 3c, MS 2a)
4.6The rate and extent of chemical change
4.6.1Rate of reaction
4.6.1.1 Calculating rates of reactions
08.2 — Plotting mass-loss data on a graph [Figure — print if needed] (MS 4c — plotting experimental data)
08.3 — Calculating the rate of reaction from a tangent to a graph, to 2 significant figures (MS 4e — tangent to a curve; MS 2a — significant figures)
03.2 — Identifying two pieces of apparatus to measure the rate of gas production (AT — apparatus for measuring gas volume and time)
03.3 — Plotting rate data and drawing a line of best fit [Figure — print if needed] (MS 4c / WS 3.2)
03.4 — Giving three conclusions about reaction rate from graph and table data
09.3 — Calculating the mean rate of reaction to 2 significant figures, using graph data (MS 2b — mean; MS 2a — significant figures)
08.1 — Plotting reaction rate data and drawing a line of best fit [Figure — print if needed] (MS 4c / WS 3.2)
08.2 — Determining the mean rate of reaction between two time points, with units (MS 3c)
08.3 — Explaining how results show a reaction rate conclusion is correct (WS 3.5)
09.2 — Explaining why lines of best fit on a rate graph become horizontal
09.3 — Explaining how a graph shows one reaction is slower than another
09.4 — Determining the rate of reaction at a given time from a tangent, to 2 significant figures (MS 4e — tangent to a curve; MS 2a)
08.2 — Determining the rate of reaction in mol/s at a given time, using a tangent (MS 4e, MS 3c)
08.4 — Explaining why a reaction stopped, shown by a horizontal line of best fit, because the limiting reactant was used up (4.3.2.4 noted)
01.1 — Suggesting why a stopper must be added quickly in a gas-collection method (WS 2.6/3.7 — reducing gas loss and measurement error)
01.2 — Determining a mean time from repeated trial data, excluding an anomalous result (MS 2b, WS 3.7)
07.3 — Determining the rate of reaction at a given time from a tangent to a graph (MS 4e)
09.2 — Calculating the number of moles of hydrogen collected between two time points (4.3.5 noted)
09.3 — Reading rate-of-reaction data from a graph for a repeated investigation
08.3 — Determining a rate of reaction in standard form from a graph (MS 4e / MS 1b)
09.3 — Labelling a predicted result line for smaller marble chips on a graph [Figure — print if needed]
09.5 — Calculating the mean rate of reaction to 3 significant figures
09.6 — Calculating a rate of reaction in standard form, showing working on a graph
4.6.1.2 Factors which affect the rates of chemical reactions
05.2 — Planning an investigation into how concentration affects reaction rate, giving valid results — RP5: investigate how changes in concentration affect the rates of reactions by a method involving measuring the volume of a gas produced and a method involving a change in colour or turbidity (WS 2.1/2.2)
03.5 — Identifying which two statements are correct about a reaction repeated at higher temperature
09.2 — Identifying two method improvements needed for valid rate-of-reaction results — RP5 context (WS 3.7 — improving a method)
09.4 — Sketching a comparison curve for a lower-concentration repeat of an investigation [Figure — print if needed] (WS 1.2/3.2)
09.1 — Identifying an apparatus setup error in a rate investigation (WS 3.7 — identifying a method error)
08.1 — Explaining why a reaction mixture becomes cloudy as a solid product forms
08.3 — Explaining a change in reaction rate over time, in terms of concentration
08.5 — Sketching a predicted results line for a different concentration [Figure — print if needed] (WS 1.2/3.2)
08.6 — Identifying a method improvement to control light reaching a sensor (WS 2.2/3.7)
08.7 — Naming the concept shown when similar results are obtained on different days under the same conditions (WS 3.6 — reproducibility)
08.8 — Identifying the mathematical relationship between two variables shown on a graph (MS 3a)
08.9 — Determining a simplest whole number ratio of reacting volumes from a graph (MS 1c)
01.3 — Identifying two changes that would decrease the rate of a gas-producing reaction
07.4 — Comparing results for a repeated investigation using a different concentration (WS 3.5)
09.1 — Explaining why the volume of gas collected is less than the volume actually produced
09.4 — Comparing results between two concentrations of acid, using graph data (WS 3.5)
09.2 — Plotting volume-of-gas data on a graph [Figure — print if needed] (MS 4c / WS 3.2)
4.6.1.3 Collision theory and activation energy
09.5 — Explaining, in terms of collision theory, why powdered reactant reacts faster than lumps
07.4 — Explaining, in terms of collision theory, why one weak acid reacts faster than another
08.4 — Calculating the surface area to volume ratio of a cube as a whole number ratio (MS 5c / MS 1c)
08.5 — Describing how the surface area to volume ratio differs for a larger cube
09.5 — Explaining how increasing temperature would affect a reaction rate, in terms of collision theory
06.6 — Explaining why a reaction is slower using a weak acid than a strong acid, in terms of collision theory
08.4 — Explaining how the rate of a decomposition reaction depends on temperature
09.4 — Explaining, in terms of collision theory, the effect of particle size on reaction rate
4.6.1.4 Catalysts
09.1 — Identifying the type of substance that acts as a catalyst in the process
09.5 — Explaining how a catalyst increases the rate of a reaction
09.6 — Suggesting why a catalyst is used in the industrial process, not in terms of rate
09.5 — Identifying the most likely formula of metal ions that lower activation energy as a catalyst (4.1.3.2 — transition metal properties noted)
07.1 — Explaining how a catalyst increases the rate of a decomposition reaction
02.4 — Completing a reaction profile: labelling activation energy, reactants and products [Figure — print if needed]
02.5 — Identifying how a reaction profile would differ without a catalyst
08.2 — Explaining a difference between two catalysts' reaction profiles
4.6.2Reversible reactions and dynamic equilibrium (chemistry only)
4.6.2.1 Simple equilibria
02.5 — Identifying the type of reaction taking place when a hydrated compound is heated, forming the anhydrous compound and water
03.1 — Identifying two words that describe a reversible reaction
4.6.2.3 Equilibrium
09.8 — Explaining why concentrations of substances do not change at dynamic equilibrium
03.2 — Identifying the correct description of a reaction at dynamic equilibrium
4.6.2.4 The effect of changing conditions on equilibrium
09.7 — Suggesting the effect of the catalyst on the equilibrium yield of methanol — equilibrium position content, not rate/catalyst content
09.6 — Suggesting the effect of adding a catalyst on an equilibrium position — a catalyst changes the rate of reaching equilibrium, not the position
09.3 — Identifying the effect of a catalyst on an equilibrium position
4.6.2.5 The effect of changing concentration
10.2 — Explaining a colour change when concentration of an ion is increased in an equilibrium mixture (WS 3.5)
09.7 — Identifying how to shift an equilibrium position by changing concentration
4.6.2.6 The effect of changing temperature
09.3 — Explaining the effect on methanol yield of using a higher temperature
10.6 — Explaining how data shows the forward reaction is exothermic
10.3 — Explaining what a colour change shows about the energy change of the forward reaction (WS 3.5)
10.3 — Explaining an equilibrium effect for an exothermic reversible reaction
09.3 — Identifying the effect of increasing temperature on an equilibrium position
07.2 — Identifying the correct statement about temperature and yield for an exothermic equilibrium reaction
09.1 — Explaining why a high temperature is used in an industrial equilibrium reaction
10.2 — Using Le Chatelier's principle to predict the effect of increasing temperature on an equilibrium yield
4.6.2.7 The effect of changing pressure
09.4 — Explaining why higher pressure gives both greater yield and increased rate
10.2 — Explaining why a low pressure is used in a Haber-process-type stage, in terms of equilibrium
10.3 — Determining the effect of increasing pressure on the position of an equilibrium
10.4 — Explaining why a change in pressure does not affect the colour of an equilibrium mixture
09.4 — Interpreting an equilibrium demonstration apparatus involving a change in volume
09.5 — Explaining the effect of increasing pressure on an equilibrium position
07.3 — Explaining why higher pressure increases the percentage yield of an industrial reaction
07.4 — Suggesting two reasons why a higher pressure is not used industrially
09.2 — Explaining why as low a pressure as possible is used in an industrial equilibrium reaction
10.3 — Explaining how increasing pressure affects an equilibrium yield
4.7Organic chemistry
4.7.1Carbon compounds as fuels and feedstock
4.7.1.1 Alkanes
01.4 — Identifying an alkane from a list of hydrocarbon formulae
02.5 — Completing the formula of a named alkane
02.5 — Writing the molecular formula of a hydrocarbon from a model
02.6 — Naming a hydrocarbon from a model
4.7.1.2 Fractional distillation of crude oil
01.1 — Suggesting a suitable furnace temperature for fractional distillation
01.2 — Explaining why diesel oil collects between two other fractions in a fractionating column
02.6 — Explaining why a larger hydrocarbon condenses lower in a fractionating column
04.1 — Identifying a crude oil fraction from a boiling point range table
04.2 — Identifying two useful materials produced from petrochemical feedstock
05.5 — Describing the fractional distillation process used to produce kerosene from crude oil
02.1 — Naming the process shown in a fractional distillation diagram
02.2 — Naming the changes of state occurring at two labelled points in fractional distillation
02.3 — Identifying a fuel obtained at a given point in a fractionating column, using data
4.7.1.3 Properties of hydrocarbons
01.3 — Suggesting two reasons why bitumen is not used as a fuel
02.1 — Plotting boiling point data on a graph [Figure — print if needed] (MS 4c)
02.2 — Predicting a boiling point from a graph and table (MS 1d / MS 4a — estimating from a plotted trend)
02.3 — Suggesting why a graph is unsuitable for a value outside its plotted range (WS 3.4 — limitations of extrapolation)
02.4 — Identifying the physical state of an alkane at a given temperature, using melting/boiling point data (4.2.2.1 — states of matter noted)
04.5 — Identifying a fraction using a table of carbon-number ranges
02.4 — Ordering fuels by increasing flammability, using boiling point range data
02.7 — Balancing the equation for the complete combustion of a hydrocarbon
05.1 — Estimating a boiling point from a table of unsaturated hydrocarbon data
05.6 — Explaining why an unsaturated hydrocarbon burns with a smoky flame, a feature of incomplete combustion
01.2 — Comparing boiling point, flammability and viscosity across hydrocarbons of different sizes
4.7.1.4 Cracking and alkenes
01.5 — Describing the conditions needed to crack a hydrocarbon fraction
01.6 — Explaining why large hydrocarbon molecules are cracked into smaller ones
01.7 — Completing an equation for the cracking of a given hydrocarbon
03.2 — Identifying observations when bromine water is added to an alkane and an alkene
10.1 — Naming the process used to produce ethene from large hydrocarbon molecules
10.2 — Describing the conditions used to produce ethene from large hydrocarbon molecules
04.6 — Naming a process and its conditions that produce smaller hydrocarbons from a larger fraction
01.1 — Identifying which product of a cracking reaction is an alkane
4.7.2Reactions of alkenes and alcohols (chemistry only)
4.7.2.1 Alkenes
03.1 — Matching hydrocarbons to their formulae [Figure — print if needed]
06.2 — Determining the general formula for a homologous series from given examples
04.7 — Identifying a pair of hydrocarbons that would both decolourise bromine water
08.1 — Circling an alkene functional group on a diagram [Figure — print if needed]
08.2 — Describing the observation when a compound is shaken with bromine water, the specified test for an alkene
05.5 — Naming an unsaturated hydrocarbon from its formula
4.7.2.2 Reactions of alkenes
08.3 — Describing a test to show a compound is an unsaturated hydrocarbon and its result
03.3 — Comparing an alkane and an alkene in terms of structure, reactivity and combustion (drawing on 4.7.1.1/4.7.1.3 and 4.9.3.1)
06.1 — Describing a test for a carbon-carbon double bond and its result
06.3 — Completing the displayed structural formula of an addition product [Figure — print if needed]
05.2 — Naming the compound produced when an alkene reacts with water vapour
05.4 — Identifying the displayed formula of the product of an alkene and chlorine reaction
10.1 — Explaining why a mixture from a separator contains both ethanol and water, since fermentation produces an aqueous solution
4.7.2.3 Alcohols
02.4 — Suggesting a use of methylated spirit
02.5 — Describing how ethanol is produced from sugar solution and naming the process
02.6 — Completing the displayed formula for ethanol [Figure — print if needed]
02.7 — Naming the gas produced when sodium is added to ethanol
02.8 — Identifying the type of substance that reacts with methanol to produce methanoic acid
04.5 — Circling an alcohol functional group on a diagram [Figure — print if needed]
10.4 — Naming the process used to produce ethanol from sugar solution using yeast
10.5 — Suggesting reaction conditions to produce an alcohol from sugar solution using bacteria
10.6 — Calculating the number of moles of ethanol needed for a given journey, using energy data (4.3.2.1 — moles; MS 3c)
02.1 — Calculating the mass of one alcohol needed to release the same energy as burning a given mass of another (MS 3c)
02.2 — Plotting energy-released data against carbon number [Figure — print if needed] (MS 4c)
02.3 — Estimating the energy released when a given mass of an alcohol is burned, using a graph (MS 4a / MS 1d)
02.6 — Identifying what reacts with an alcohol to produce a carboxylic acid
01.5 — Identifying which alcohol is oxidised to produce propanoic acid
4.7.2.4 Carboxylic acids
07.1 — Completing a table about carboxylic acid reactions
07.5 — Naming the ester produced when ethanoic acid reacts with ethanol
07.6 — Identifying the displayed structural formula of an ester product
02.7 — Completing the displayed structural formula of the carboxylic acid functional group [Figure — print if needed]
02.8 — Matching compounds to the product formed when each reacts with a carboxylic acid [Figure — print if needed]
08.3 — Circling an ester functional group on a diagram [Figure — print if needed]
01.4 — Identifying the structure of propanoic acid
4.7.3Synthetic and naturally occurring polymers (chemistry only)
4.7.3.1 Addition polymerisation
06.2 — Completing the structure of poly(propene) in an equation [Figure — print if needed]
06.1 — Completing the displayed structural formula of a monomer [Figure — print if needed]
04.1 — Completing the displayed structural formula equation for poly(ethene) production [Figure — print if needed]
01.1 — Completing the displayed structural formula of a monomer [Figure — print if needed]
08.1 — Circling the functional group that allows a monomer to form an addition polymer [Figure — print if needed]
08.2 — Completing the equation for producing an addition polymer from its monomer [Figure — print if needed]
08.6 — Circling the repeating unit in a polymer diagram [Figure — print if needed]
08.5 — Completing a displayed formula equation for an addition polymerisation reaction [Figure — print if needed]
08.6 — Identifying the type of polymer formed in an addition polymerisation reaction
07.7 — Completing the equation for the production of an addition polymer from its monomer [Figure — print if needed]
06.1 — Completing the displayed formulae of ethene and poly(ethene) in an equation [Figure — print if needed]
4.7.3.2 Condensation polymerisation (HT only)
06.1 — Naming the small molecule lost in a condensation polymerisation reaction
06.4 — Explaining given information comparing carpet fibre materials
06.2 — Naming a substance formed when two monomers join to produce a polyester — condensation polymerisation content, not the carboxylic acid precursor
06.3 — Naming the small molecule lost when a polyester forms
04.6 — Completing a table showing the small molecule formed when monomers join by condensation
07.1 — Naming two monomers that react to form a polyester
07.2 — Naming the type of condensation polymer produced from two named monomers
07.3 — Naming the small molecule lost when a condensation polymer forms
06.2 — Comparing addition and condensation polymerisation using a named example of each
4.7.3.3 Amino acids (HT only)
09.3 — Identifying the number of functional groups in a given molecule
09.4 — Naming the other substance produced in a condensation polymerisation reaction
08.4 — Naming the small molecule produced when an amino acid polymerises
07.4 — Naming the type of condensation polymer produced when an amino acid polymerises
07.5 — Completing the displayed structural formula of an amino acid [Figure — print if needed]
07.6 — Identifying the polymer formed when different amino acids combine in one chain
4.7.3.4 DNA and other naturally-occurring polymers
09.2 — Naming two naturally occurring polymers produced from glucose
09.6 — Describing the shape and structure of a naturally occurring polymer
08.7 — Suggesting the identity of a naturally occurring polymer from its structure
08.8 — Giving the general name for the monomers making up a naturally occurring polymer
08.9 — Naming the shape of a naturally occurring polymer's structure
4.8Chemical analysis
4.8.1Purity, formulations and chromatography
4.8.1.1 Pure substances
05.5 — Suggesting what a company means by describing treated water as 'pure', against the scientific meaning
02.4 — Describing a test to show water is pure and its expected result
4.8.1.2 Formulations
02.1 — Naming the type of useful product a mixture such as methylated spirit is called
02.2 — Calculating the percentage by mass of methanol in methylated spirit (MS 1c — percentage by mass within a formulation)
02.3 — Suggesting why pyridine and methyl violet are added to ethanol to make methylated spirit — a formulation question, not alcohol content
02.2 — Naming the type of mixture a tablet with fixed-amount components is called
02.3 — Calculating the percentage by mass of an active ingredient in a tablet (MS 1c — percentage by mass)
04.4 — Suggesting why manufacturers always use the same proportions of dyes in a formulation
03.3 — Identifying the correct description of a paint's formulation
4.8.1.3 Chromatography
04.1 — Giving the problem caused by each of two chromatography method mistakes — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances
04.2 — Giving two conclusions from a chromatography results diagram — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances
04.3 — Calculating the distance moved by the solvent, using an Rf value — RP6 context (MS 3c — rearranging the Rf relationship)
04.1 — Calculating the distance moved by the solvent, using an Rf value — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances (MS 3c)
04.2 — Suggesting why only two spots are seen for a mixture of more than two compounds — RP6 context
04.3 — Identifying two ways to increase the distance between chromatogram spots — RP6 context
04.5 — Identifying which change would definitely produce a smaller Rf value — RP6 context
03.1 — Planning an investigation to determine the Rf value of a dye — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values (WS 2.1/2.2, MS 3c)
03.2 — Identifying how two investigations differed, given different Rf results for the same dye — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values
03.3 — Identifying the stationary phase in paper chromatography — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values
06.1 — Identifying two apparatus-setup mistakes in a chromatography investigation — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values (WS 3.7)
06.2 — Determining a distance value from chromatography data — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values (MS 3c)
06.3 — Explaining why Rf values differ using two types of chromatography paper — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values
06.4 — Identifying another change that could result in a different Rf value — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances and calculate Rf values
04.1 — Explaining why two dyes travel different distances, referring to forces of attraction with the paper
04.2 — Explaining why a dye is in different positions in two repeated chromatography experiments
04.3 — Comparing the purity of two dyes, using chromatography evidence (4.8.1.1 — purity noted)
04.4 — Calculating the distance moved by the solvent front, given an Rf value (MS 3c)
04.5 — Explaining why the Rf value of a dye is not affected by how far the solvent travels
07.1 — Suggesting problems caused by chromatography method mistakes — RP6: investigate how paper chromatography can be used to separate and distinguish between coloured substances (WS 3.7)
07.2 — Calculating an Rf value to 2 significant figures — RP6 context (MS 3c, MS 2a)
07.3 — Calculating a distance moved on chromatography paper, given an Rf value
07.4 — Explaining how different dyes are separated by paper chromatography
4.8.2Identification of common gases
4.8.2.1 Test for hydrogen
01.4 — Describing the test for hydrogen gas and its result
4.8.2.2 Test for oxygen
09.1 — Describing a test to identify a collected gas and its result
09.1 — Describing a test to identify a collected gas and its result
02.3 — Describing the test for oxygen gas and its result
4.8.2.3 Test for carbon dioxide
02.4 — Identifying the chemical name of limewater
02.5 — Giving the result of the carbon dioxide test using limewater
4.8.2.4 Test for chlorine
05.6 — Describing a test for chlorine gas and its result
05.3 — Describing the test for chlorine gas and its result
4.8.3Identification of ions by chemical and spectroscopic means (chemistry only)
4.8.3.1 Flame tests
01.1 — Identifying the flame colour produced by sodium ions
01.2 — Naming a metal ion that would produce a green flame
01.3 — Explaining why it is difficult to identify metal ions from a mixed-ion flame colour
01.1 — Identifying the flame colour produced by copper sulfate solution
01.2 — Explaining why a flame test method did not produce a distinct colour, due to a missed step
07.1 — Describing a test to identify a Group 1 metal ion and its result — RP7: use of chemical tests to identify the ions in unknown compounds
01.1 — Describing a test to identify sodium ions and its result — RP7: use of chemical tests to identify the ions in unknown compounds
06.3 — Identifying a metal ion from a flame test result
07.6 — Explaining why a flame test could not identify two metal ions in a mixture
4.8.3.2 Metal hydroxides
07.1 — Describing a test for a metal ion using sodium hydroxide solution and its result — RP7: use of chemical tests to identify the ions in unknown compounds
01.3 — Giving the results of sodium hydroxide tests on two solutions
07.3 — Giving the result of a sodium hydroxide test for a metal ion — RP7: use of chemical tests to identify the ions in unknown compounds
07.4 — Identifying an additional step and result needed to distinguish between two metal ions — RP7: use of chemical tests to identify the ions in unknown compounds
01.5 — Naming a solution and result that shows the presence of copper(II) ions — RP7: use of chemical tests to identify the ions in unknown compounds
05.3 — Describing a test for copper(II) ions in solution and its result — RP7: use of chemical tests to identify the ions in unknown compounds
06.1 — Naming another metal ion that produces a white precipitate with sodium hydroxide — RP7: use of chemical tests to identify the ions in unknown compounds
06.2 — Describing a test to confirm aluminium ions in solution and its result — RP7: use of chemical tests to identify the ions in unknown compounds
4.8.3.3 Carbonates
02.1 — Planning an investigation to show the presence of lithium ions and carbonate ions in a tablet — RP7: use of chemical tests to identify the ions in unknown compounds (drawing on 4.8.3.1 Flame tests and 4.8.3.3 Carbonates)
06.5 — Describing a test on gas bubbles that confirms carbonate ions and its result
07.7 — Identifying an unknown compound from a sequence of test results, including a carbonate test
4.8.3.4 Halides
01.5 — Identifying the ion shown to be present by a cream precipitate
01.5 — Naming the solution that would show the presence of iodide ions, and the test result
03.1 — Planning a method to show the presence of two named ions in a medicine sample, drawing on the specific ion tests — RP7: use of chemical tests to identify the ions in unknown compounds
01.2 — Describing a test to identify chloride ions and its result — RP7 context
06.4 — Identifying a non-metal ion from a silver nitrate precipitate test
4.8.3.5 Sulfates
01.6 — Describing a test for sulfate ions and its result
07.2 — Describing a test to show water contains sulfate ions and its result — RP7: use of chemical tests to identify the ions in unknown compounds
01.4 — Naming the solution that would show the presence of sulfate ions
07.5 — Describing a test to identify sulfate ions in a solution and its result — RP7: use of chemical tests to identify the ions in unknown compounds
01.6 — Describing a test for sulfate ions and its result — RP7: use of chemical tests to identify the ions in unknown compounds
07.1 — Describing a test for sulfate ions and its result
4.8.3.6 Instrumental methods
03.3 — Giving an advantage of an instrumental method over a chemical test
04.6 — Suggesting an advantage of using gas chromatography as an instrumental method
4.8.3.7 Flame emission spectroscopy
01.4 — Identifying two metal ions present in a mixture from flame emission spectra
07.2 — Naming an instrumental method that could identify and quantify a metal ion
03.2 — Identifying an instrumental method (flame emission spectroscopy) to identify and quantify a metal ion
07.5 — Using flame emission spectra to identify two metal ions present in a mixture
4.9Chemistry of the atmosphere
4.9.1The composition and evolution of the Earth's atmosphere
4.9.1.2 How oxygen increased
03.5 — Explaining why scientists are not certain about early-atmosphere gas percentages (WS 1.3 — limitations of evidence)
09.5 — Identifying two gases from Earth's early atmosphere used by algae to produce a named molecule
04.1 — Explaining how the percentage of nitrogen changed in the Earth's early atmosphere
04.2 — Reading early-atmosphere carbon dioxide percentage data from a table
04.3 — Plotting early-atmosphere carbon dioxide data and drawing a line of best fit [Figure — print if needed] (MS 4c / WS 3.2)
4.9.1.3 How carbon dioxide decreased
08.1 — Explaining why organisms could not have evolved the same way on another moon as on Earth
06.1 — Explaining a change in the percentage of oxygen in an early-atmosphere graph region, due to photosynthesis
4.9.1.4 Composition of the atmosphere today
03.4 — Explaining the processes that changed the Earth's early atmosphere to today's atmosphere
06.2 — Explaining a change in the percentage of carbon dioxide in an early-atmosphere graph region
06.3 — Comparing changes in the percentages of two gases in a later atmospheric graph region
06.4 — Identifying the process that caused the atmospheric gas changes shown
06.5 — Describing how deposits of a fossil fuel were formed
04.4 — Explaining changes in atmospheric carbon dioxide and oxygen percentages over time, using data
4.9.2Global climate change
4.9.2.1 Greenhouse gases
08.2 — Explaining how a greenhouse gas keeps a moon's atmosphere warmer
04.1 — Identifying a greenhouse gas from a list of gases
05.2 — Describing how carbon dioxide helps maintain temperatures on Earth
4.9.2.2 Human activities which contribute to increased greenhouse gases
04.2 — Explaining why increased world population may have increased atmospheric carbon dioxide
04.3 — Explaining why increased world population may have increased atmospheric methane
04.5 — Evaluating the evidence linking greenhouse gas increase to rising mean surface temperature (WS 1.6/3.5 — correlation, uncertainty, alternative explanations)
05.1 — Giving a reason why it is difficult to produce models for future climate change
05.3 — Explaining how human activities have contributed to a temperature trend, linking activities to greenhouse gases
4.9.2.3 Global climate change
04.4 — Describing two potential effects of an increase in mean surface temperature
4.9.2.4 The carbon footprint and its reduction
05.2 — Explaining a positive environmental impact of burning hydrogen rather than natural gas, using emissions data
4.9.3Atmospheric pollutants from fuels
4.9.3.1 Combustion of fuels
07.1 — Explaining how carbon monoxide is produced when petrol is burned in car engines
07.4 — Describing how oxides of nitrogen are produced when petrol is burned in car engines
05.2 — Naming the gases produced when methane is burned, in terms of complete/incomplete combustion
05.3 — Balancing the equation for the incomplete combustion of methane (4.3.1.1 — balancing a symbol equation)
06.1 — Explaining why soot is formed when some fossil fuels are burned
06.3 — Explaining why oxides of nitrogen are formed in car engines
05.1 — Explaining how oxides of nitrogen are produced when fuels are burned
01.3 — Identifying the equation representing incomplete combustion of a hydrocarbon
4.9.3.2 Properties and effects of atmospheric pollutants
07.2 — Suggesting two reasons why the maximum allowed carbon monoxide percentage has decreased for newer cars
07.3 — Giving a reason for a maximum allowed percentage of unburned hydrocarbons in exhaust fumes
07.6 — Naming two other pollutants reduced by catalytic converters
06.2 — Explaining how reducing sulfur in fossil fuels reduces limestone erosion
01.2 — Explaining the environmental effects of combustion products released into the atmosphere
04.4 — Explaining why sulfur impurities are removed from petrol before it is burned
05.3 — Explaining a negative environmental impact of burning hydrogen rather than natural gas, using data
4.10Using resources
4.10.1Using the Earth's resources and obtaining potable water
4.10.1.1 Using the Earth's resources and sustainable development
06.3 — Suggesting why a fibre-blend carpet is more sustainable than a single-material carpet
05.1 — Suggesting two reasons why wood is more sustainable than natural gas as a heating fuel
01.1 — Describing changes in the percentage of electricity generated from two sources over a decade, using graph data (MS 4a / WS 3.2 — interpreting and describing graph trends)
01.3 — Suggesting why solar energy is a more sustainable way of generating electricity than burning oil
01.4 — Suggesting two reasons why solar energy may not fully replace fossil fuel electricity generation
4.10.1.2 Potable water
07.3 — Planning an investigation to find the total mass of dissolved solids in a water sample, giving valid results — RP8: analyse and purify water samples from different sources, including pH and dissolved solids
02.1 — Explaining how potable water is produced from fresh water
02.2 — Suggesting a process to obtain potable water for a country with limited rainfall
05.2 — Identifying a plausible ion concentration pair for desalinated water
05.3 — Explaining why certain ion concentrations are unchanged by a water treatment process
05.4 — Explaining why a water sample requires further treatment before being safe to drink
01.3 — Explaining why heating continued until mass no longer changed (WS 2.6 — ensuring a complete, reliable measurement)
01.4 — Identifying how the mass of a dried solid was calculated from raw measurements
01.5 — Calculating a mean concentration of an ion from repeated trial data (MS 2b; 4.3.2.5 noted)
01.1 — Explaining why a burette rather than a measuring cylinder was used to measure a sample volume (AT 8)
01.2 — Identifying the dependent variable in a water-sample investigation (WS 2.2)
01.3 — Describing how to ensure all water had evaporated in an evaporation step
01.4 — Identifying how the mass of dissolved solids in a sample was calculated
01.5 — Calculating the mean concentration of dissolved solids in g/dm³ from repeated sample data (4.3.2.5, MS 2b, MS 3c)
01.6 — Suggesting why different sea water samples contain different masses of dissolved solids
02.1 — Identifying the two main steps used to treat lake water, with reasons
02.3 — Completing and labelling a distillation diagram for desalination [Figure — print if needed] (AT 4 — distillation apparatus)
02.5 — Explaining why producing drinking water from sea water is expensive
4.10.1.3 Waste water treatment
02.3 — Matching waste water substances to their treatment process [Figure — print if needed]
02.4 — Calculating the percentage of sewage sludge processed by a given method, to 3 significant figures (MS 1c / MS 2a)
02.5 — Suggesting a reason why the total mass of processed sewage sludge increased over time
02.6 — Suggesting two reasons why more sewage sludge was used as fertiliser over time
05.1 — Describing how sewage is treated to remove organic matter
03.3 — Explaining what happens to water in two named water-treatment processes
02.2 — Explaining why producing drinking water from waste water is more difficult than from lake water
4.10.1.4 Alternative methods of extracting metals
08.4 — Describing how a metal is extracted from low-grade ore by phytomining
08.5 — Suggesting two reasons why phytomining has not been widely adopted
05.4 — Describing what is meant by bioleaching
4.10.2Life cycle assessment and recycling
4.10.2.1 Life cycle assessment
10.1 — Evaluating the use of coated paper compared with poly(styrene) for disposable cups, using LCA features
10.2 — Calculating the energy needed to produce a given mass of coated paper cups, in standard form (MS 1b — standard form)
05.1 — Suggesting two pieces of energy-usage information needed for a complete LCA
05.2 — Evaluating the use of different materials for food plates, using LCA features (WS 1.4/3.5)
03.1 — Evaluating two materials for making a product, using life cycle assessment data (WS 1.4/3.5)
03.2 — Calculating the mass of a material using density and volume data (MS 3c, MS 5c)
4.10.2.2 Ways of reducing the use of resources
08.3 — Suggesting three reasons why recycling scrap metal is more sustainable than extracting it from ore
01.2 — Suggesting why polymer insulation must be removed from scrap wire before recycling
01.3 — Describing how scrap metal wire can be recycled to make new pipes
01.4 — Suggesting two reasons why recycling a metal is more sustainable than extracting it from ore
03.1 — Evaluating aluminium and wood as materials for doors, using comparison data (WS 1.4)
4.10.3Using materials
4.10.3.1 Corrosion and its prevention
04.1 — Explaining what would happen to nails in different rust-test conditions
04.2 — Explaining how a coating prevents steel from rusting
04.3 — Explaining why aluminium window frames do not corrode after manufacture
06.2 — Explaining why aluminium alloy bicycle frames do not need protection from corrosion
06.3 — Suggesting a method other than paint to protect iron bicycle chains from rusting
03.2 — Explaining how an oxide coating protects aluminium from corrosion
03.1 — Identifying the resolution of a balance used in a rusting investigation (AT 1 / WS 2.6)
03.2 — Calculating a difference in percentage mass increase between two samples, to 3 significant figures (MS 1c, MS 2a)
03.3 — Drawing conclusions about factors affecting rusting and evaluating coatings, using investigation results (WS 3.5/3.7)
03.4 — Completing the word equation for the formation of rust
4.10.3.2 Alloys as useful materials
08.1 — Suggesting a health-related reason why certain alloys are now preferred over others
08.2 — Suggesting a reason why two alloys have different melting points, using data
06.1 — Evaluating aluminium alloy and bamboo as materials for bicycle frames, using comparison data (WS 1.4)
4.10.3.3 Ceramics, polymers and composites
10.3 — Explaining why melamine does not melt when heated
06.4 — Explaining why a type of polyester melts when heated
06.5 — Matching composite material terms to their descriptions [Figure — print if needed]
06.6 — Suggesting two reasons why an outer skin is added to a composite material core
05.3 — Describing how ceramic food plates are produced from clay
04.2 — Suggesting why a thermosoftening polymer is easier to recycle than a thermosetting polymer
04.3 — Explaining how different forms of a polymer can be produced from the same monomer
04.4 — Comparing the structures of two different-density forms of a polymer
08.3 — Giving the general name for a material made of reinforcement fibres in a polymer matrix
06.4 — Identifying the roles of the two components of a composite material
08.7 — Naming the word used to describe polymers that melt when heated
08.8 — Explaining why some polymers do not melt when heated
07.8 — Describing the structure of a thermosetting polymer
04.1 — Explaining a trend in the percentage of milk bottles made from a polymer rather than glass
04.2 — Justifying a material choice for milk bottles, using given information
4.10.4The Haber process and the use of NPK fertilisers (chemistry only)
4.10.4.1 The Haber process
03.1 — Naming a gas used in the Haber process, obtained from methane
03.2 — Giving the approximate temperature and pressure used in the Haber process reactor
03.3 — Suggesting why ammonia condenses but the other gases do not (4.2.2.4 — boiling point/condensation of small molecules noted)
10.4 — Determining how many times greater a percentage yield is under different conditions (MS 1c)
10.5 — Giving a reason why higher pressure conditions are not used industrially
07.1 — Giving the raw material sources for the Haber process
07.3 — Explaining how ammonia is separated from unreacted gases in the Haber process
07.4 — Plotting remaining data and drawing a line of best fit on a partially-completed graph [Figure — print if needed] (MS 4c / WS 3.2)
07.5 — Determining a percentage yield from a graph, showing working (MS 4a, MS 1c)
07.6 — Explaining why specific temperature, pressure and catalyst conditions are chosen for economical ammonia production (4.6.1.4 catalysts, 4.6.2.6 temperature, 4.6.2.7 pressure noted)
02.1 — Explaining why a condenser is linked to the reactor in the Haber process
02.2 — Identifying the metal used as a catalyst in an industrial reaction
09.4 — Calculating the volume of air required to obtain a given volume of nitrogen for the Haber process
09.5 — Explaining how ammonia is separated from unreacted gases in the Haber process
4.10.4.2 Production and uses of NPK fertilisers
10.7 — Suggesting why demand for ammonia has increased over time
05.1 — Identifying two compounds that each contain two named NPK elements
05.2 — Naming the soluble salts produced when a phosphate rock reacts with two named acids
05.3 — Describing the industrial steps used to produce ammonium sulfate for fertiliser
10.1 — Evaluating which fertiliser compound would best address a soil nutrient deficiency (WS 1.4/3.5)
10.2 — Identifying how a named fertiliser raw material is obtained from the Earth
10.3 — Naming another compound that could give a similar agricultural productivity improvement
10.4 — Naming a compound needed to produce nitric acid for fertiliser production
10.5 — Suggesting why phosphate rock cannot be used directly as a fertiliser
10.6 — Naming the salts produced by treating phosphate rock with two named acids
02.6 — Suggesting a use of ammonium nitrate
09.6 — Explaining an environmental consequence of nitrogen released when fertiliser and plant matter break down
08.1 — Naming the two compounds used to manufacture ammonium nitrate
08.2 — Explaining why an NPK value is useful information on a fertiliser label (4.8.1.2 — formulation context noted)
08.3 — Explaining the relationship between ammonia production and world population, using graph data
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