5.1Atomic structure and the periodic table
5.1.1A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes
5.1.1.1 Atoms, elements and compounds (not assessed in these 8 papers)
5.1.1.2 Mixtures
08.2 — Choosing filtration to remove unreacted iron
5.1.1.3 The development of the model of the atom
06.1 — Drawing conclusions from the alpha-scattering experiment
01.2 — Identifying the plum pudding model
01.3 — Identifying the model from Chadwick's work
04.1 — Ordering the discovery of the three subatomic particles
03.1 — Identifying two conclusions from the alpha-scattering experiment
5.1.1.4 Relative electrical charges of subatomic particles (not assessed in these 8 papers)
5.1.1.5 Size and mass of atoms
04.3 — Working out total electrons in F₂ from atomic notation
01.1 — Finding electrons and neutrons in an aluminium atom
06.2 — Calculating a gold atom's diameter
01.4 — Explaining what isotopes are
04.2 — Calculating how many times heavier a proton is than an electron
04.3 — Finding neutrons in a given bromine atom
04.4 — Finding electrons in a bromide ion
03.2 — Explaining why particle X isn't an atom
03.3 — Identifying the correct notation for particle X
5.1.1.6 Relative atomic mass
01.5 — Calculating Ar from isotope abundances
04.5 — Calculating Ar from isotope abundances
5.1.1.7 Electronic structure
02.1 — Comparing Na and Cl electron shell arrangements
5.1.2The periodic table
5.1.2.1 The periodic table
01.4 — Predicting beryllium's reactivity vs magnesium using periodic position
5.1.2.2 Development of the periodic table
04.1 — Stating the ordering principle of early periodic tables
04.2 — Explaining how Mendeleev corrected misplaced elements
07.3 — Explaining the iodine/tellurium placement issue
01.1 — Identifying the undiscovered group in Mendeleev's table
5.1.2.3 Metals and non-metals (not assessed in these 8 papers)
5.1.2.4 Group 0
04.5 — Explaining neon's unreactivity via electronic structure
5.1.2.5 Group 1
06.3 — Explaining why sodium is less reactive than potassium
07.2 — Explaining why caesium is more reactive than sodium
03.3 — Giving two observations as sodium burns in oxygen
03.4 — Describing two differences if potassium were used instead
5.1.2.6 Group 7
04.5 — Explaining the halogen displacement reactivity trend
04.4 — Explaining the boiling-point trend down Group 7
04.1 — Naming the Group 7 elements collectively
04.2 — Explaining why Group 7 elements react similarly
04.4 — Completing a melting-point bar chart [Figure — print if needed]
07.2 — Explaining why chlorine is more reactive than bromine
07.3 — Describing the boiling-point trend vs. relative formula mass
03.6 — Completing a word equation for a halogen displacement
03.7 — Explaining decreasing reactivity down Group 7
5.2Bonding, structure, and the properties of matter
5.2.1Chemical bonds, ionic, covalent and metallic
5.2.1.1 Chemical bonds
03.5 — Identifying the bonding type in ClF₃
5.2.1.2 Ionic bonding
02.2 — Describing electron transfer forming NaCl
06.2 — Describing observations as sodium reacts with chlorine
07.1 — Explaining caesium + oxygen electron transfer
03.2 — Describing electron behaviour forming sodium oxide
07.1 — Explaining calcium and chlorine atoms in electron terms
5.2.1.3 Ionic compounds
07.1 — Giving two limitations of a 2D ionic model vs. a 3D one
5.2.1.4 Covalent bonding
04.2 — Completing a dot-and-cross diagram for F₂ [Figure — print if needed]
03.3 — Completing a dot-and-cross diagram for O₂ [Figure — print if needed]
02.1 — Giving a limitation of a ball-and-stick water molecule model
02.3 — Giving a molecular formula from a structure diagram
04.3 — Giving a molecular formula from a structure diagram
06.1 — Completing a dot-and-cross diagram for hydrogen chloride [Figure — print if needed]
04.6 — Completing a dot-and-cross diagram for Cl₂ [Figure — print if needed]
05.1 — Completing a dot-and-cross diagram for ammonia [Figure — print if needed]
05.3 — Completing a dot-and-cross diagram for HOCl [Figure — print if needed]
5.2.1.5 Metallic bonding (not assessed in these 8 papers)
5.2.2How bonding and structure are related to the properties of substances
5.2.2.1 The three states of matter
04.7 — Naming a surface process at boiling point besides evaporation/boiling
5.2.2.2 State symbols
04.1 — Giving chlorine's state symbol (requires knowing halogen states)
02.1 — Giving the state symbol for ammonium nitrate solution
02.3 — Giving nitric acid's state symbol
04.6 — Giving bromine's state symbol at a given temperature
01.5 — Giving the missing state symbol in an equation
05.1 — Giving state symbols for three substances
5.2.2.3 Properties of ionic compounds
05.2 — Explaining conditions needed for NaCl to conduct
07.6 — Explaining how sodium chloride can conduct electricity
05.1 — Explaining why solid NaCl doesn't conduct
07.3 — Explaining why copper oxide has a high melting point
5.2.2.4 Properties of small molecules
04.3 — Explaining why halogens have low boiling points
06.4 — Comparing structure and bonding of NaCl and HCl
02.2 — Completing a sentence about ice's intermolecular forces
04.5 — Explaining the melting-point trend down Group 7
07.4 — Explaining why water has a low melting point
03 — Comparing the structure and bonding of sodium chloride and oxygen
03.4 — Explaining the boiling-point increase down Group 7
5.2.2.5 Polymers
05.4 — Comparing intra-chain bonding with inter-chain forces
5.2.2.6 Giant covalent structures
02.6 — Naming two other giant covalent structures
07.4 — Comparing silicon dioxide and poly(ethene)
5.2.2.7 Properties of metals and alloys
04.3 — Explaining why steel is harder than iron
04.4 — Calculating an unknown element mass in an alloy
05.3 — Explaining why other metals are added to aluminium
01.1 — Giving two conclusions from a copper-production graph
01.2 — Explaining why the copper-zinc alloy is harder than pure copper
01.3 — Calculating copper's mass from a given percentage composition
04.7 — Explaining why alloys are harder than pure metals
5.2.2.8 Metals as conductors
05.3 — Describing how sodium conducts thermal energy
07.5 — Describing how sodium metal conducts electricity
07.2 — Explaining why copper's structure allows thermal conduction
07.3 — Explaining why aluminium conducts better than sodium
5.2.3Structure and bonding of carbon
5.2.3.1 Diamond
05.1 — Explaining diamond's high melting point
02.4 — Stating the number of bonds per carbon atom in diamond
02.5 — Giving two physical properties of diamond
5.2.3.2 Graphite
04.2 — Explaining why graphite conducts electricity
5.2.3.3 Graphene and fullerenes
04.1 — Identifying buckminsterfullerene's formula
05.1 — Identifying a carbon structure from a diagram
05.2 — Suggesting a nanotechnology-relevant property
07.1 — Identifying the pair of substances with hexagonal rings
08.1 — Describing carbon atom arrangement in a nanotube
08.2 — Giving another use of nanotubes
08.4 — Explaining why nanotubes conduct electricity
5.3Quantitative chemistry
5.3.1Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
5.3.1.1 Conservation of mass and balanced chemical equations
04.4 — Completing a balanced equation for Al + Br₂
06.1 — Selecting the correctly balanced equation for Na + Cl₂
03.1 — Balancing an equation for sodium and oxygen
5.3.1.2 Relative formula mass
06.2 — Calculating a metal's Ar from the Mr of a compound of the metal
02.5 — Calculating percentage mass of oxygen in NH₄NO₃
02.2 — Calculating the Mr of sulfuric acid
02.3 — Calculating percentage mass of oxygen in lithium sulfate
02.2 — Calculating percentage mass of oxygen in calcium hydroxide
5.3.1.3 Mass changes when a reactant or product is a gas
06.1 — Giving formulae for carbonate decomposition products
06.3 — Finding the gradient of a gas-volume-vs-time graph
02.4 — Plotting data and drawing a line of best fit [Figure — print if needed]
02.5 — Explaining the mass decrease on thermal decomposition
06.1 — Explaining why a Bunsen burner was used instead of a water bath
06.2 — Explaining two mass-change trends for magnesium and magnesium carbonate
06.4 — Explaining why a "solid escaped" conclusion is incorrect
5.3.1.4 Chemical measurements
02.4 — Identifying the measure of uncertainty from repeat readings
5.3.2Use of amount of substance in relation to masses of pure substances
5.3.2.1 Moles (HT only)
06.4 — Determining Mr using the 24 dm³/mole gas rule
04.6 — Using the Avogadro constant to find atoms in 1g of argon
08.3 — Calculating moles of carbon using the Avogadro constant
5.3.2.2 Amounts of substances in equations (HT only)
08.3 — Calculating iron's mass via mole ratios
06.3 — Calculating mass of chlorine from a mole ratio
06.1 — Calculating moles of oxygen gas reacted
06.3 — Calculating copper oxide mass produced
06.3 — Calculating MgCl₂ concentration via a multi-step mole calculation
04.5 — Identifying the mole ratio from a given equation
05.2 — Calculating hydrogen's mass from a mole ratio
06.3 — Explaining why the final mass is the same for both reactions
5.3.2.3 Using moles to balance equations (HT only)
06.4 — Determining an iron oxide's formula and equation
06.5 — Determining a mole ratio, formula, and balanced equation
5.3.2.4 Limiting reactants (HT only)
07.4 — Determining the limiting reactant and maximum product mass
5.3.2.5 Concentration of solutions
01.5 — Converting g/dm³ concentration to a mass
01.5 — Calculating HCl concentration in g/dm³
05.7 — Calculating mass of CuSO₄ in a given volume
02.5 — Calculating mass needed to make a given volume of solution
01.3 — Identifying the solubility trend from a graph
02.4 — Calculating concentration in g/dm³
01.4 — Calculating concentration in g/dm³
5.4Chemical changes
5.4.1Reactivity of metals
5.4.1.1 Metal oxides
06.2 — Explaining a mass difference without a lid
5.4.1.2 The reactivity series
01.1 — Ranking four metals by reactivity from acid reactions
01.2 — Naming two variables to keep constant
01.3 — Identifying the variable that is changed
03 — Planning an investigation to find the reactivity order of three metals
07.2 — Completing and balancing an equation
5.4.1.3 Extraction of metals and reduction
01.2 — Explaining the meaning of "reduction"
06.1 — Naming a metal found natively as the element
06.2 — Suggesting the most economical extraction method
04.1 — Explaining why iron can be extracted by carbon reduction
04.4 — Identifying the reduced substance
5.4.1.4 Oxidation and reduction in terms of electrons (HT only)
08.4 — Identifying the reduced species, writing its half-equation
05.1 — Identifying the reaction type at the negative electrode
05.2 — Completing a half equation for chlorine production
07.3 — Writing a half-equation showing sodium's oxidation
06.2 — Explaining what happens to the magnesium atoms
5.4.2Reactions of acids
5.4.2.1 Reactions of acids with metals
08.1 — Naming the gas from iron + acid
5.4.2.2 Neutralisation of acids and salt production
02.2 — Identifying the correct formula for nitric acid
03 — Planning a method to test a hypothesis about carbonate decomposition
04.2 — Suggesting a way to speed up the reaction
04.7 — Completing and balancing an equation for sodium hydroxide + sulfuric acid
02.5 — Deducing zinc nitrate's formula from given ion formulae
02.1 — Deducing potassium sulfate's formula from given ion formulae
01.6 — Describing a method to investigate gas volume vs. carbonate mass
02.1 — Naming the reaction type
02.1 — Identifying the acid used to prepare copper sulfate
07.2 — Deducing aluminium sulfate's formula
5.4.2.3 Soluble salts
03 — Correcting method errors in preparing copper sulfate crystals
04.1 — Completing state symbols for a zinc oxide + acid equation
04.3 — Recognising when all acid has reacted
04.4 — Describing how to obtain the salt solution from the mixture
04.5 — Describing how crystals are produced from solution
02.4 — Giving two observations as zinc carbonate is added in excess
02.6 — Planning a method to prepare pure copper chloride
01.1 — Giving three observations as copper carbonate is added to sulfuric acid
01.2 — Describing how to remove the excess solid
01.5 — Determining crystallised mass from a solubility curve
06.1 — Describing how solid MgCl₂ is obtained from the mixture
02.2 — Explaining why excess copper carbonate is used
02.3 — Describing how to produce crystals from the solution
5.4.2.4 The pH scale and neutralisation
07.1 — Identifying four unknown solids from pH/solubility data
02.3 — Stating indicator colours in acid and alkali
02.4 — Identifying the pH pattern as acid is added in excess
04.6 — Suggesting pH values before and after excess acid is added
04.8 — Calculating new H⁺ concentration after a pH increase
02.1 — Giving the colour change with nitric acid
02.2 — Stating the pH change
01.3 — Stating the pH at the end of the reaction
01.4 — Naming the reaction type
01.1 — Identifying the ion that makes CO₂ solution acidic
01.2 — Naming an indicator and its result for an acidic test
01.4 — Identifying the pH trend from the same graph
04.4 — Writing the ionic equation for acid + alkali
04.6 — Identifying indicator colour with excess acid present
5.4.2.5 Strong and weak acids (HT only)
07.2 — Calculating pH after a 100× dilution
06.2 — Explaining the term "strong acid"
06.3 — Describing how magnesium distinguishes a strong from a weak acid
06.4 — Determining pH change from a 100× concentration increase
04.1 — Explaining the term "strong acid"
04.2 — Explaining "dilute aqueous solution"
04.3 — Identifying the H⁺ concentration change from pH 1 to pH 3
05.2 — Calculating H⁺ concentration at a given pH
05.4 — Explaining why a weak acid has a higher pH than a strong acid
5.4.3Electrolysis
5.4.3.1 The process of electrolysis
05.2 — Completing a sentence about when NaCl also conducts
01.3 — Explaining how the results disprove a constant-rate hypothesis
5.4.3.2 Electrolysis of molten ionic compounds (not assessed in these 8 papers)
5.4.3.3 Using electrolysis to extract metals
05.1 — Explaining why electrolysis is used for reactive metals
05.2 — Naming the two substances in aluminium's molten electrolyte
01.3 — Explaining why carbon anodes need replacing
01.4 — Identifying charge carriers in three conductors within the aluminium extraction process
07.1 — Giving the method and conditions to extract metal Y
06.3 — Naming a substance in the aluminium extraction diagram
06.4 — Explaining what happens to the positive carbon electrodes
06.5 — Writing the half equation at the negative electrode
04.2 — Explaining why cryolite is mixed with aluminium oxide
04.3 — Writing the half equation for oxygen production
04.5 — Explaining the cost difference between extracting aluminium and iron
04.6 — Explaining the cost difference between extracting aluminium and chromium
5.4.3.4 Electrolysis of aqueous solutions
01.1 — Identifying the gas released at the anode
01.2 — Inferring copper's reactivity from cathode deposit
01.3 — Making an estimate from a pattern in tabulated repeat data
01.4 — Finding a repeat value using the arithmetic mean, with rearrangement
05.5 — Extrapolating expected copper mass after 24 hours from a graph
05.6 — Reading a starting mass from a graph's y-intercept
05.7 — Calculating the gradient of a mass-vs-time graph
05.3 — Explaining oxygen production in sodium sulfate electrolysis
02.2 — Reading gas volumes from the apparatus diagram
02.3 — Explaining how the volumes support a given hypothesis
05.3 — Suggesting a suitable inert electrode material
05.5 — Explaining a pH increase during electrolysis
01.1 — Suggesting a way to reduce risk from poisonous chlorine gas
01.2 — Plotting data and drawing a line of best fit [Figure — print if needed]
01.5 — Explaining why hydrogen was given off instead of potassium
5.4.3.5 Representation of reactions at electrodes as half equations (HT only)
05.3 — Completing half equations for molten copper chloride electrolysis
05.4 — Suggesting reasons for a mass discrepancy in an experiment
05.4 — Completing a half equation for chlorine production
5.5Energy changes
5.5.1Exothermic and endothermic reactions
5.5.1.1 Energy transfer during exothermic and endothermic reactions
02.6 — Describing a method to test temperature change vs. mass dissolved
05.1 — Identifying the dependent variable
05.2 — Explaining a 4-minute wait before adding magnesium
05.3 — Drawing a line of best fit [Figure — print if needed]
05.4 — Determining temperature change from a graph
05.5 — Explaining a temperature decrease after 7 minutes
05.6 — Identifying an unknown metal from a smaller temperature change
03.1 — Identifying the dependent variable
03.2 — Suggesting three accuracy improvements
03.3 — Explaining a temperature-time pattern
04.7 — Giving two improvements for more accurate results
02.1 — Explaining the term "exothermic"
02.3 — Planning a method to investigate temperature change vs. mass
5.5.1.2 Reaction profiles
02.3 — Completing an exothermic reaction profile [Figure — print if needed]
03.1 — Labelling activation energy on a reaction profile [Figure — print if needed]
03.2 — Reading overall energy change from a reaction profile
03.4 — Drawing a labelled exothermic reaction profile
05.4 — Completing and labelling a reaction profile [Figure — print if needed]
5.5.1.3 The energy change of reactions (HT only)
03.4 — Calculating energy change from given bond energies
07.1 — Explaining why methane and oxygen don't react at room temperature
07.2 — Predicting energy released from a data pattern
07.3 — Calculating a bond energy from given data
06.5 — Calculating a bond energy from given data
05.3 — Calculating a bond energy from given data
05.5 — Calculating overall energy change from bond energies
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