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100+ Free GCSE Chemistry Practice Questions

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What change in pH occurs if the H⁺ concentration of a solution decreases by a factor of 100?

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Key Facts: GCSE Chemistry Exam

9-1

Grading scale

Ofqual

May-June

Exam series

AQA, Edexcel, OCR timetable

3 boards

Specifications available

AQA, Edexcel, OCR

100

Free practice questions here

OpenExamPrep

AQA, Edexcel, OCR GCSE Chemistry is assessed through linear end-of-course exam papers (Key Stage 4). Coverage spans atomic structure, bonding structure and matter, quantitative chemistry, and grading uses the 9-1 scale on 2026 specifications.

Sample GCSE Chemistry Practice Questions

Try these sample questions to test your GCSE Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1What is the relative mass of a proton?
A.1/1836
B.1
C.0
D.2
Explanation: Protons have a relative mass of 1 (the same as a neutron). The mass of an atom is concentrated in the nucleus, which contains protons and neutrons.
2An atom of magnesium can be represented as ²⁴₁₂Mg. How many neutrons does this atom contain?
A.12
B.24
C.36
D.10
Explanation: Number of neutrons = mass number − atomic number = 24 − 12 = 12. The mass number (top) is the total of protons and neutrons; the atomic number (bottom) is the number of protons.
3What is the electronic configuration of a chlorine atom (atomic number 17)?
A.2,8,8
B.2,7
C.2,8,7
D.2,8,5
Explanation: Chlorine has 17 electrons. They fill shells in order: 2 in the first shell, 8 in the second, leaving 7 in the third — giving 2,8,7. The 7 outer electrons place chlorine in Group 7.
4Which statement about isotopes is correct?
A.They have the same number of neutrons but a different number of protons.
B.They have the same number of protons but a different number of neutrons.
C.They have a different number of protons and electrons.
D.They have different chemical properties because they have different proton numbers.
Explanation: Isotopes are atoms of the same element (so the same number of protons) with different numbers of neutrons. They have the same chemical properties because chemistry is determined by the electron configuration, but they have different physical properties (e.g. density).
5Chlorine has two stable isotopes: ³⁵Cl (75%) and ³⁷Cl (25%). Calculate the relative atomic mass of chlorine.
A.35.0
B.35.5
C.36.0
D.37.0
Explanation: Relative atomic mass = (35 × 75 + 37 × 25) / 100 = (2625 + 925) / 100 = 3550 / 100 = 35.5. This is the weighted mean of the isotope masses, weighted by their abundances.
6Which scientist is credited with discovering the nucleus through the gold-foil (alpha-scattering) experiment?
A.John Dalton
B.J. J. Thomson
C.Ernest Rutherford
D.Niels Bohr
Explanation: Rutherford's team (Geiger and Marsden, 1909) fired alpha particles at thin gold foil. Most passed straight through, but a few deflected sharply — leading Rutherford to conclude that atoms contain a tiny, dense, positively charged nucleus.
7In which group of the periodic table is potassium (atomic number 19) found?
A.Group 0
B.Group 1
C.Group 2
D.Group 7
Explanation: Potassium has the electronic configuration 2,8,8,1. Having one electron in its outer shell places it in Group 1, the alkali metals. It reacts with water to form potassium hydroxide and hydrogen.
8Why does reactivity increase going down Group 1 (the alkali metals)?
A.The atoms get smaller, so the outer electron is held more tightly.
B.The outer electron is in a shell further from the nucleus and is more easily lost.
C.There are more outer electrons to lose.
D.The atoms have more neutrons, which makes them more reactive.
Explanation: Going down Group 1, the atomic radius increases and the outer electron is in a shell further from the nucleus, shielded by inner shells. The attraction between the nucleus and the outer electron is therefore weaker, so the electron is lost more easily and reactivity increases.
9Which of the following is the correct trend in reactivity for the Group 7 halogens, from most to least reactive?
A.Iodine, bromine, chlorine, fluorine
B.Fluorine, chlorine, bromine, iodine
C.Chlorine, fluorine, bromine, iodine
D.Bromine, chlorine, fluorine, iodine
Explanation: Halogens become less reactive down the group because they gain an electron to react. As atoms get larger, the outer shell is further from the nucleus, so the attracting force on the incoming electron is weaker. Fluorine is the most reactive halogen and iodine is the least reactive of the four.
10Which row of the periodic table is correctly described as a 'period'?
A.A vertical column
B.A horizontal row
C.Only the noble gases
D.The transition metals only
Explanation: A period is a horizontal row of the periodic table. Elements in the same period have the same number of occupied electron shells. A group is a vertical column.

About the GCSE Chemistry Exam

GCSE Chemistry is offered by AQA, Edexcel, OCR as part of the UK General Certificate of Secondary Education qualification framework. The course covers atomic structure, bonding structure and matter, quantitative chemistry, chemical changes and is assessed primarily through written exam papers at the end of the two-year course.

Questions

100 scored questions

Time Limit

3-5 hours total across multiple papers

Passing Score

Grade 4 is the standard pass, Grade 5 is the strong pass (1-9 scale)

Exam Fee

£40-£80 per subject (school-set entry fee) (AQA, Edexcel, OCR)

GCSE Chemistry Exam Content Outline

Core

Atomic Structure and Periodic Table

Atoms, ions, isotopes, electronic structure, periodic table development

Core

Bonding, Structure and Properties of Matter

Ionic, covalent, metallic bonding; states of matter; nanoparticles

Core

Quantitative Chemistry

Relative formula mass, the mole, percentage yield, atom economy

Core

Chemical Changes

Acids, bases, salts, electrolysis, reactivity series

Core

Energy Changes

Exothermic and endothermic reactions, reaction profiles, bond energies

Core

Rate and Extent of Chemical Change

Rates of reaction, collision theory, catalysts, reversible reactions, equilibrium

Core

Organic Chemistry

Crude oil, alkanes, alkenes, alcohols, carboxylic acids, polymers

Core

Chemical Analysis

Purity, separation, flame tests, identifying ions and gases

Core

Atmosphere

Composition, evolution, greenhouse gases, climate change, atmospheric pollutants

Core

Using Earth's Resources

Finite vs renewable, life-cycle assessment, alloys, ceramics, composites, polymers

How to Pass the GCSE Chemistry Exam

What You Need to Know

  • Passing score: Grade 4 is the standard pass, Grade 5 is the strong pass (1-9 scale)
  • Exam length: 100 questions
  • Time limit: 3-5 hours total across multiple papers
  • Exam fee: £40-£80 per subject (school-set entry fee)

Keys to Passing

  • Complete 500+ practice questions
  • Score 80%+ consistently before scheduling
  • Focus on highest-weighted sections
  • Use our AI tutor for tough concepts

GCSE Chemistry Study Tips from Top Performers

1Use past papers from your specific exam board — questions follow the same style year on year
2Time yourself on full papers to build pacing for the long extended-response questions
3Build a clear understanding of mark schemes — examiners reward specific assessment objectives
4Review examiner reports each summer; common errors repeat

Frequently Asked Questions

What exam boards offer GCSE Chemistry?

GCSE Chemistry is offered by AQA, Edexcel, OCR. All boards follow Ofqual subject content but vary in the choice of set texts, optional topics, and paper structure.

When is the GCSE Chemistry exam taken?

Exams are written in the May-June series at the end of the two-year Key Stage 4 course. Most students sit the papers in Year 11.

How is GCSE Chemistry graded?

GCSEs are graded on the 9-1 scale, where 9 is the highest grade. A grade 4 is a standard pass, and grade 5 is a strong pass. Grade 7 is broadly equivalent to the old A grade.

How many papers does GCSE Chemistry have?

Most GCSE subjects have 2-3 written papers. The exact number, timing, and weighting depend on the chosen exam board. Some subjects also include a non-examined assessment (NEA) coursework component.