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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
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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
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Graphite
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Graphene and fullerenes
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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
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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
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Extraction of metals and reduction
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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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Group 0

Practise 21 exam-style questions on Group 0 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.

  • 21 questions
  • 1–6 marks each
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20 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

2 marks

The elements in Group 0 of the periodic table are called the noble gases.

Explain, in terms of electrons, why the noble gases are unreactive.

Model answer

The atoms of the noble gases have a full outer shell of electrons, which is a stable arrangement. This means they do not need to lose, gain or share electrons, so they do not easily react to form compounds or molecules.

Explanation

Reactions involve atoms losing, gaining or sharing electrons to reach a stable electronic structure. Noble gas atoms already have a full outer shell (8 electrons, or 2 for helium), so there is nothing to be gained by reacting. Say 'full outer shell', not just 'full shells'.

Mark scheme
  1. 1 mark

    (their atoms have) a full outer shell (of electrons) / a stable arrangement of electrons

    allow 8 electrons in the outer shell (2 for helium); allow stable electronic structure

  2. 1 mark

    so they do not (easily) lose, gain or share electrons

    allow do not need to lose, gain or share electrons / do not easily form bonds

Question 2

2 marks

When Mendeleev published his periodic table in 1869, it did not include any of the noble gases.

Suggest why the noble gases were not included.

Model answer

The noble gases had not yet been discovered. They are very unreactive and do not form compounds, so chemists had not detected them in any substances. When they were discovered later, they fitted into a new group at the end of the table.

Explanation

Most elements were found because they formed compounds that chemists could study. The noble gases do not react, are colourless and make up only a small part of the air, so they went unnoticed until the 1890s.

Mark scheme
  1. 1 mark

    the noble gases had not been discovered

    allow scientists did not know they existed

  2. 1 mark

    because they are unreactive / do not form compounds (so they were hard to detect)

    allow they are colourless gases present in only small amounts in air

Question 3

3 marks

Krypton is the element between argon and xenon in Group 0.

Predict three properties of krypton.

Model answer

Krypton will be a colourless gas at room temperature. It will be very unreactive because it has a full outer shell, and it will exist as single atoms. Its boiling point will be higher than argon's but lower than xenon's.

Explanation

An element's properties can be predicted from its group and its position in the group. As a noble gas, krypton shares the group properties (unreactive, monatomic gas); because it is between argon and xenon, values such as boiling point and density lie between theirs.

Mark scheme
  1. 1 mark

    (very) unreactive / does not easily form compounds

    max 3; any three from the list

  2. 1 mark

    gas at room temperature

    allow colourless gas

  3. 1 mark

    boiling point higher than argon's but lower than xenon's

    allow boiling point between −186 °C and −108 °C if values are quoted

  4. 1 mark

    exists as single atoms / does not form molecules

    allow monatomic

  5. 1 mark

    density higher than argon's but lower than xenon's

  6. 1 mark

    8 electrons in its outer shell / full outer shell

Question 4

4 marks

Argon (atomic number 18) is unreactive. Chlorine (atomic number 17) and potassium (atomic number 19) are both very reactive.

Explain these differences in terms of the electronic structures of the atoms.

Model answer

Argon has the electronic structure 2,8,8. Its outer shell is full, which is stable, so it does not need to lose, gain or share electrons and it is unreactive. Chlorine is 2,8,7, so it readily gains one electron (or shares one) to complete its outer shell. Potassium is 2,8,8,1, so it readily loses its single outer electron to leave a full outer shell. Because chlorine and potassium can reach a stable full outer shell by gaining or losing one electron, they react easily.

Explanation

Reactivity depends on the outer shell. Elements just before or after a noble gas react to reach the same stable structure as that noble gas: chlorine gains an electron and potassium loses one. Argon already has that structure, so it does not react.

Mark scheme
  1. 1 mark

    argon is 2,8,8 / has a full outer shell

    allow 8 electrons in outer shell

  2. 1 mark

    so argon is stable and does not need to lose, gain or share electrons

  3. 1 mark

    chlorine is 2,8,7 so it gains one electron (or shares an electron) to get a full outer shell

    allow chlorine needs one more electron

  4. 1 mark

    potassium is 2,8,8,1 so it loses one electron to get a full outer shell

    allow potassium loses its outer electron easily

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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