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Exam Practice
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AQA GCSE Chemistry Smart practice A mixed round aimed at your weak spots
Unit 1
Atomic structure and the periodic table
A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes
Atoms, elements and compounds
0%
Mixtures
0%
The development of the model of the atom
0%
Relative electrical charges of subatomic particles
0%
Size and mass of atoms
0%
Relative atomic mass
0%
Electronic structure
0%
The periodic table
The periodic table
0%
Development of the periodic table
0%
Metals and non-metals
0%
Group 0
0%
Group 1
0%
Group 7
0%
Properties of transition metals (chemistry only)
Comparison with Group 1 elements (chemistry only)
0%
Typical properties (chemistry only)
0%
Unit 2
Bonding, structure, and the properties of matter
Chemical bonds, ionic, covalent and metallic
Chemical bonds
0%
Ionic bonding
0%
Ionic compounds
0%
Covalent bonding
0%
Metallic bonding
0%
How bonding and structure are related to the properties of substances
The three states of matter
0%
State symbols
0%
Properties of ionic compounds
0%
Properties of small molecules
0%
Polymers
0%
Giant covalent structures
0%
Properties of metals and alloys
0%
Metals as conductors
0%
Structure and bonding of carbon
Diamond
0%
Graphite
0%
Graphene and fullerenes
0%
Bulk and surface properties of matter including nanoparticles (chemistry only)
Sizes of particles and their properties (chemistry only)
0%
Uses of nanoparticles (chemistry only)
0%
Unit 3
Quantitative chemistry
Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
Conservation of mass and balanced chemical equations
0%
Relative formula mass
0%
Mass changes when a reactant or product is a gas
0%
Chemical measurements
0%
Use of amount of substance in relation to masses of pure substances
Moles (HT only)
0%
Amounts of substances in equations (HT only)
0%
Using moles to balance equations (HT only)
0%
Limiting reactants (HT only)
0%
Concentration of solutions
0%
Yield and atom economy of chemical reactions (chemistry only)
Percentage yield (chemistry only)
0%
Atom economy (chemistry only)
0%
Using concentrations of solutions in mol/dm³ (chemistry only) (HT only)
0%
Use of amount of substance in relation to volumes of gases (chemistry only) (HT only)
0%
Unit 4
Chemical changes
Reactivity of metals
Metal oxides
0%
The reactivity series
0%
Extraction of metals and reduction
0%
Oxidation and reduction in terms of electrons (HT only)
0%
Reactions of acids
Reactions of acids with metals
0%
Neutralisation of acids and salt production
0%
Soluble salts
0%
The pH scale and neutralisation
0%
Titrations (chemistry only)
0%
Strong and weak acids (HT only)
0%
Electrolysis
The process of electrolysis
0%
Electrolysis of molten ionic compounds
0%
Using electrolysis to extract metals
0%
Electrolysis of aqueous solutions
0%
Representation of reactions at electrodes as half equations (HT only)
0%
Unit 5
Energy changes
Exothermic and endothermic reactions
Energy transfer during exothermic and endothermic reactions
0%
Reaction profiles
0%
The energy change of reactions (HT only)
0%
Chemical cells and fuel cells (chemistry only)
Cells and batteries (chemistry only)
0%
Fuel cells (chemistry only)
0%
Unit 6
The rate and extent of chemical change
Rate of reaction
Calculating rates of reactions
0%
Factors which affect the rates of chemical reactions
0%
Collision theory and activation energy
0%
Catalysts
0%
Reversible reactions and dynamic equilibrium
Reversible reactions
0%
Energy changes and reversible reactions
0%
Equilibrium
0%
The effect of changing conditions on equilibrium (HT only)
0%
The effect of changing concentration (HT only)
0%
The effect of temperature changes on equilibrium (HT only)
0%
The effect of pressure changes on equilibrium (HT only)
0%
Unit 7
Organic chemistry
Carbon compounds as fuels and feedstock
Crude oil, hydrocarbons and alkanes
0%
Fractional distillation and petrochemicals
0%
Properties of hydrocarbons
0%
Cracking and alkenes
0%
Reactions of alkenes and alcohols (chemistry only)
Structure and formulae of alkenes (chemistry only)
0%
Reactions of alkenes (chemistry only)
0%
Alcohols (chemistry only)
0%
Carboxylic acids (chemistry only)
0%
Synthetic and naturally occurring polymers (chemistry only)
Addition polymerisation (chemistry only)
0%
Condensation polymerisation (HT only) (chemistry only)
0%
Amino acids (HT only) (chemistry only)
0%
DNA (deoxyribonucleic acid) and other naturally occurring polymers (chemistry only)
0%
Unit 8
Chemical analysis
Purity, formulations and chromatography
Pure substances
0%
Formulations
0%
Chromatography
0%
Identification of common gases
Test for hydrogen
0%
Test for oxygen
0%
Test for carbon dioxide
0%
Test for chlorine
0%
Identification of ions by chemical and spectroscopic means (chemistry only)
Flame tests (chemistry only)
0%
Metal hydroxides (chemistry only)
0%
Carbonates (chemistry only)
0%
Halides (chemistry only)
0%
Sulfates (chemistry only)
0%
Instrumental methods (chemistry only)
0%
Flame emission spectroscopy (chemistry only)
0%
Unit 9
Chemistry of the atmosphere
The composition and evolution of the Earth's atmosphere
The proportions of different gases in the atmosphere
0%
The Earth's early atmosphere
0%
How oxygen increased
0%
How carbon dioxide decreased
0%
Carbon dioxide and methane as greenhouse gases
Greenhouse gases
0%
Human activities which contribute to an increase in greenhouse gases in the atmosphere
0%
Global climate change
0%
The carbon footprint and its reduction
0%
Common atmospheric pollutants and their sources
Atmospheric pollutants from fuels
0%
Properties and effects of atmospheric pollutants
0%
Unit 10
Using resources
Using the Earth's resources and obtaining potable water
Using the Earth's resources and sustainable development
0%
Potable water
0%
Waste water treatment
0%
Alternative methods of extracting metals (HT only)
0%
Life cycle assessment and recycling
Life cycle assessment
0%
Ways of reducing the use of resources
0%
Using materials (chemistry only)
Corrosion and its prevention (chemistry only)
0%
Alloys as useful materials (chemistry only)
0%
Ceramics, polymers and composites (chemistry only)
0%
The Haber process and the use of NPK fertilisers (chemistry only)
The Haber process (chemistry only)
0%
Production and uses of NPK fertilisers (chemistry only)
0%
Avg
score:
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Topics
done:
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Diamond

Practise 15 exam-style questions on Diamond for AQA GCSE Chemistry. Write your answer as you would in the exam and get it marked in seconds against the mark scheme, point by point, with an AI tutor on hand if you get stuck.

  • 15 questions
  • 1–6 marks each
  • Instant marking
  • No sign-up needed
15 questions, marked as you go

Sample questions with model answers

Here are 4 of the questions in this topic, each with a model answer, an explanation of why it earns the marks and the mark scheme an examiner would use.

Question 1

1 mark

What type of structure does diamond have?

Model answer

A giant covalent structure.

Explanation

Diamond has no separate molecules: every carbon atom is joined to others by covalent bonds throughout the whole crystal. Both words are needed, because giant ionic and giant metallic structures also exist.

Mark scheme
  1. 1 mark

    giant covalent (structure)

    allow macromolecular / giant covalent lattice; do not accept 'giant' or 'covalent' alone, giant ionic or metallic

Question 2

2 marks

A student says: 'Diamond does not conduct electricity because it has no electrons.'

Explain why the student is wrong.

Model answer

Diamond does contain electrons: every carbon atom has six. However, each carbon atom uses all four of its outer electrons to form covalent bonds, so none of the electrons are delocalised and free to move and carry charge.

Explanation

Every substance contains electrons. What matters for conduction is whether any charged particles are free to move. In diamond all the outer electrons are fixed in bonds between pairs of atoms.

Mark scheme
  1. 1 mark

    diamond does contain electrons (each carbon atom has six electrons)

  2. 1 mark

    but all the outer electrons are used in covalent bonds, so none are delocalised / free to move

Question 3

3 marks

Carbon is in Group 4 of the periodic table.

Explain why each carbon atom in diamond forms four covalent bonds.

Model answer

A carbon atom has four electrons in its outer shell, so it needs four more to have a full outer shell of eight. In diamond, each carbon atom shares a pair of electrons with each of four neighbouring carbon atoms, forming four covalent bonds.

Explanation

The group number gives the number of outer electrons. Because diamond uses all four outer electrons in bonding, none are left over to be delocalised, which is also why diamond does not conduct electricity.

Mark scheme
  1. 1 mark

    a carbon atom has four electrons in its outer shell

  2. 1 mark

    it needs four more electrons to have a full outer shell (of eight)

    allow to gain a stable electronic structure like a noble gas

  3. 1 mark

    it shares one pair of electrons with each of four other carbon atoms

Question 4

5 marks

Diamonds are used on the tips of drills for drilling through rock. The tips become very hot during drilling.

Explain why diamond is suitable for this use, in terms of its structure and bonding.

Model answer

In diamond, each carbon atom forms four strong covalent bonds with other carbon atoms, making a rigid giant covalent structure. This makes diamond very hard, so it can cut through rock without wearing away quickly. Diamond also has a very high melting point because a lot of energy is needed to break its many strong covalent bonds, so the drill tip does not melt when it becomes hot from friction.

Explanation

Two properties matter here: hardness, to cut the rock, and a very high melting point, to cope with the heat. Both come from the same rigid network of strong covalent bonds.

Mark scheme
  1. 1 mark

    each carbon atom forms four covalent bonds with other carbon atoms

    max 5

  2. 1 mark

    the covalent bonds are strong

  3. 1 mark

    giant rigid (three-dimensional) structure, so diamond is very hard and can cut through rock

  4. 1 mark

    very high melting point, so the tip will not melt when it gets hot

  5. 1 mark

    because a lot of energy is needed to break the many strong covalent bonds

  6. 1 mark

    the tip does not wear away quickly / is not scratched by the rock

Ready to try the rest? Every answer you write is marked against the mark scheme, so you can see exactly where the marks are.

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