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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
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Graphite
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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
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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
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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:
0/124

Group 1

Practise 20 exam-style questions on Group 1 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.

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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

A small piece of lithium is added to a trough of water.

Describe two things you would observe.

Model answer

The lithium floats on the water and fizzes steadily as bubbles of gas are given off. It moves slowly around the surface and gradually gets smaller until it disappears.

Explanation

Observations are what you can see, not what you know is produced: 'fizzes' is an observation, 'hydrogen is made' is not. Lithium is the least reactive of the first three alkali metals, so it does not melt or catch fire.

Mark scheme
  1. 1 mark

    floats

    max 2; any two from the list

  2. 1 mark

    fizzes / bubbles / effervescence

    ignore 'gas given off' or naming hydrogen without an observation

  3. 1 mark

    moves (slowly) on the surface

  4. 1 mark

    gets smaller / disappears

    ignore dissolves

Question 2

2 marks

Sodium is added to water. After the reaction, a few drops of universal indicator are added to the solution.

Give the colour of the indicator and explain your answer.

Model answer

The indicator turns purple. Sodium reacts with water to form sodium hydroxide, which is a strong alkali, so the solution has a high pH.

Explanation

All Group 1 metals react with water to form metal hydroxides, which are alkalis containing OH⁻ ions. Universal indicator is purple in a strongly alkaline solution (pH 12-14).

Mark scheme
  1. 1 mark

    purple

    allow blue / violet; do not accept green or red

  2. 1 mark

    the solution contains sodium hydroxide, which is an alkali

    allow the solution is alkaline / has a high pH / contains hydroxide ions (OH⁻)

Question 3

3 marks

Lithium, sodium and potassium have similar chemical reactions.

Explain why, in terms of their electronic structures.

Model answer

Lithium (2,1), sodium (2,8,1) and potassium (2,8,8,1) all have one electron in their outer shell. When they react, each atom loses this one electron to form an ion with a 1+ charge and a full outer shell, so they all react in the same way.

Explanation

Chemical reactions involve the outer electrons, so elements with the same number of outer electrons react in similar ways. Every Group 1 element forms 1+ ions, which is why their compounds have similar formulae, such as LiCl, NaCl and KCl.

Mark scheme
  1. 1 mark

    they all have one electron in their outer shell

    allow electronic structures 2,1 / 2,8,1 / 2,8,8,1

  2. 1 mark

    they lose this (one) electron when they react

  3. 1 mark

    forming ions with a 1+ charge / ions with a full outer shell

    allow forming ions with the electronic structure of a noble gas

Question 4

4 marks

A small piece of sodium is heated until it starts to burn and then lowered into a gas jar of chlorine.

Describe what you would observe and write a balanced symbol equation for the reaction.

Model answer

The sodium burns vigorously with a bright yellow flame and a white solid (sodium chloride) forms on the sides of the jar. The green colour of the chlorine fades.
2Na + Cl₂ → 2NaCl

Explanation

Alkali metals react vigorously with chlorine to form white, ionic metal chlorides. Chlorine is diatomic (Cl₂), so two sodium atoms are needed for each chlorine molecule.

Mark scheme
  1. 1 mark

    sodium burns (vigorously) with a bright yellow / orange flame

    allow bright flame / glows brightly

  2. 1 mark

    a white solid / white powder / white smoke is formed

    allow the green colour of the chlorine fades as an alternative observation for this mark

  3. 1 mark

    correct formulae: Na + Cl₂ → NaCl

  4. 1 mark

    balanced: 2Na + Cl₂ → 2NaCl

    allow multiples; ignore state symbols

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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