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GCSE Chemistry (AQA) MCQs with answers

Practise GCSE Chemistry (AQA) (AQA 8462) with 313 exam-style MCQs, each with the answer and a short explanation. Every test is marked the moment you finish and shows your score chapter by chapter, so you know what to revise next. It is free and needs no sign-up.

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GCSE Chemistry (AQA) MCQs with answers

Practise GCSE Chemistry (AQA) (AQA 8462) with 313 exam-style MCQs, each with the answer and a short explanation. Every test is marked the moment you finish and shows your score chapter by chapter, so you know what to revise next. It is free and needs no sign-up.

313 questions · 10 chapters

What each chapter covers 10 chapters

The questions follow the syllabus chapter by chapter. You can test the whole subject or one chapter at a time.

  1. Atomic structure and the periodic table 39 questions4.1.1 Atoms, elements, compounds and mixtures, 4.1.1 Atomic models, subatomic particles, isotopes and electronic structure, 4.1.2 The periodic table: development, Group 0, Group 1 and Group 7, 4.1.3 Properties of transition metals
  2. Bonding, structure, and the properties of matter 29 questions4.2.1 Ionic, covalent and metallic bonding, 4.2.2 How bonding and structure are related to properties, 4.2.3-4.2.4 Structure and bonding of carbon; nanoparticles
  3. Quantitative chemistry 38 questions4.3.1 Conservation of mass and relative formula mass, 4.3.2 Moles, reacting masses and limiting reactants (HT), 4.3.3 Yield and atom economy, 4.3.2.5, 4.3.4-4.3.5 Concentrations of solutions and volumes of gases
  4. Chemical changes 29 questions4.4.1 Reactivity of metals, 4.4.2 Reactions of acids, 4.4.3 Electrolysis
  5. Energy changes 19 questions4.5.1 Exothermic and endothermic reactions, 4.5.2 Chemical cells and fuel cells
  6. The rate and extent of chemical change 36 questions4.6.1 Calculating and measuring rates of reaction, 4.6.1 Factors affecting rate, collision theory and catalysts, 4.6.2 Reversible reactions and dynamic equilibrium
  7. Organic chemistry 37 questions4.7.1 Crude oil, alkanes, fractional distillation and cracking, 4.7.2 Alkenes, alcohols and carboxylic acids, 4.7.3 Synthetic and naturally occurring polymers
  8. Chemical analysis 23 questions4.8.1 Purity, formulations and chromatography, 4.8.2-4.8.3 Tests for gases and ions; instrumental methods
  9. Chemistry of the atmosphere 22 questions4.9.1 Composition and evolution of the Earth's atmosphere, 4.9.2-4.9.3 Greenhouse gases, climate change and atmospheric pollutants
  10. Using resources 41 questions4.10.1 Using the Earth's resources and obtaining potable water, 4.10.2 Life cycle assessment and recycling, 4.10.3 Using materials, 4.10.4 The Haber process and NPK fertilisers
Sample GCSE Chemistry (AQA) MCQs with answers 12 questions

12 questions from the test, one or two from each chapter. Try each one, then open the answer.

1. Why are the noble gases unreactive?

  1. A
    they are gases, and gases cannot take part in reactions
  2. B
    their atoms have only one electron in the outer shell
  3. C
    their atoms already have full outer shells of electrons
  4. D
    their atoms are joined in molecules by strong covalent bonds
Show answer

Answer: C. A full outer shell is a stable arrangement, so noble gas atoms do not easily gain, lose or share electrons. They exist as single atoms.

2. Magnesium oxide has a much higher melting point than sodium chloride. What is the best explanation?

  1. A
    the ions in MgO have larger charges, so they attract each other more strongly
  2. B
    magnesium oxide has stronger intermolecular forces between its molecules
  3. C
    magnesium atoms are heavier than sodium atoms, so they are harder to move
  4. D
    magnesium oxide has covalent bonds that are much stronger than ionic bonds
Show answer

Answer: A. Mg2+ and O2− attract more strongly than Na+ and Cl−, so more energy is needed to break the lattice. Both are ionic, with no intermolecular forces.

3. What is the relative formula mass of calcium carbonate, CaCO3?

  1. A
    68
  2. B
    84
  3. C
    100
  4. D
    116
Show answer

Answer: C. Mr = 40 + 12 + (3 × 16) = 100. 68 comes from counting only one oxygen.

4. A strong acid has a pH of 2. It is diluted so that the concentration of H+ ions falls by a factor of 100. What is the new pH?

  1. A
    1
  2. B
    3
  3. C
    4
  4. D
    6
Show answer

Answer: C. Each decrease of 1 in pH means ten times more H+ ions, so a factor of 100 (10 × 10) changes the pH by 2: from 2 up to 4.

5. Which reaction is endothermic?

  1. A
    respiration in living cells
  2. B
    the neutralisation of an acid by an alkali
  3. C
    the combustion of methane in a Bunsen burner
  4. D
    the thermal decomposition of limestone
Show answer

Answer: D. Thermal decomposition needs a continuous input of energy, so it is endothermic. Combustion, neutralisation and respiration all release energy.

6. H2(g) + I2(g) ⇌ 2HI(g). What is the effect of increasing the pressure on the equilibrium amount of HI?

  1. A
    it increases, because the higher pressure favours the forward reaction
  2. B
    it doubles, because the pressure has doubled
  3. C
    it decreases, because the higher pressure pushes the reaction back to the reactants
  4. D
    it is unchanged, because both sides have the same number of gas molecules
Show answer

Answer: D. There are 2 gas molecules on each side, so pressure does not favour either direction. The rate still increases.

7. Which conditions are used to make ethanol by fermentation?

  1. A
    sugar and yeast heated to 100 °C with plenty of air passing through
  2. B
    sugar solution and yeast kept warm, at about 30 °C, in the absence of air
  3. C
    ethene and steam passed over a phosphoric acid catalyst at about 300 °C
  4. D
    glucose solution heated with a nickel catalyst at high pressure
Show answer

Answer: B. Yeast enzymes work best when warm, are denatured at high temperatures, and without air the ethanol is not oxidised to ethanoic acid. The ethene and steam route is a different method.

8. Why is the start line on chromatography paper drawn in pencil rather than ink?

  1. A
    pencil helps the solvent to rise faster up the paper
  2. B
    pencil is insoluble, so it does not dissolve and move up the paper
  3. C
    ink would react with the paper and change the colours
  4. D
    pencil is easier to see than ink against the paper
Show answer

Answer: B. Graphite is insoluble, so the line stays put. An ink line would dissolve and give its own spots, spoiling the result.

9. How is carbon monoxide produced when fuels burn?

  1. A
    the fuel burns in a limited supply of oxygen
  2. B
    sulfur impurities in the fuel burn in plenty of oxygen
  3. C
    nitrogen from the air reacts with oxygen at a high temperature
  4. D
    hydrocarbons burn completely in a plentiful supply of air
Show answer

Answer: A. With too little oxygen, carbon is only partly oxidised, giving carbon monoxide and soot. Complete combustion gives carbon dioxide.

10. Which is a synthetic material made from crude oil that is used to replace a natural material?

  1. A
    silk, used instead of natural cotton
  2. B
    wood, used instead of natural rubber
  3. C
    polyester, used instead of natural wool
  4. D
    cotton, used instead of synthetic nylon
Show answer

Answer: C. Polyester is a synthetic polymer made from crude oil. Cotton, wood and silk are all natural materials, so none of them is synthetic.

11. How many protons, neutrons and electrons are in the ion 27Al3+? (atomic number of aluminium = 13)

  1. A
    13 protons, 14 neutrons, 13 electrons
  2. B
    13 protons, 27 neutrons, 10 electrons
  3. C
    13 protons, 14 neutrons, 10 electrons
  4. D
    14 protons, 13 neutrons, 10 electrons
Show answer

Answer: C. Neutrons = 27 − 13 = 14. The 3+ charge means 3 electrons have been lost, so 13 − 3 = 10 electrons.

12. Carbon nanotubes are used to reinforce materials such as tennis rackets. Which properties make them suitable?

  1. A
    a high length to diameter ratio and high tensile strength
  2. B
    solubility in water, so they spread through it
  3. C
    a low melting point and a soft, slippery feel
  4. D
    ionic bonding, which makes them very hard and brittle
Show answer

Answer: A. Nanotubes are cylindrical fullerenes that are very long compared with their width and very strong when pulled, so they strengthen composites.

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The 313 MCQs are our own, written to the syllabus in the style of the exam.

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