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100+ Free A-Level Chemistry Practice Questions

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When chlorine is bubbled through potassium bromide solution, what is observed?

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Key Facts: A-Level Chemistry Exam

A*-E

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 A-Level Chemistry is assessed through linear end-of-course exam papers (Year 13). Coverage spans physical chemistry, inorganic chemistry, organic chemistry, and grading uses the A*-E scale on 2026 specifications.

Sample A-Level Chemistry Practice Questions

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

1Which subatomic particle has a relative mass of approximately 1/1836 compared to a proton?
A.Neutron
B.Electron
C.Proton
D.Alpha particle
Explanation: An electron has a relative mass of approximately 1/1836 (or 0.0005) compared to a proton, which is taken as 1. Neutrons have a relative mass of 1, equal to protons. This very small electron mass is why atomic mass calculations focus on protons and neutrons.
2What is the full electron configuration of a chromium atom (Z = 24) in its ground state?
A.1s2 2s2 2p6 3s2 3p6 3d4 4s2
B.1s2 2s2 2p6 3s2 3p6 3d5 4s1
C.1s2 2s2 2p6 3s2 3p6 3d6
D.1s2 2s2 2p6 3s2 3p6 4s2 3d4
Explanation: Chromium is one of the two notable exceptions to standard Aufbau filling (along with copper). A half-filled 3d5 4s1 configuration is more stable than 3d4 4s2 due to the exchange energy associated with half-filled d-subshells. This gives an additional measure of stability through symmetrical electron distribution.
3There is a small dip in first ionisation energy between Group 2 and Group 13 (e.g., Mg to Al). What is the main reason?
A.Al has a larger nuclear charge so electrons are held more tightly
B.The outermost electron in Al is in a 3p orbital, which is at slightly higher energy than the 3s orbital in Mg
C.Al has paired electrons in 3s which repel each other
D.Mg has a smaller atomic radius than Al
Explanation: Aluminium's outermost electron occupies a 3p orbital, which is at a slightly higher energy (and further from the nucleus on average) than the 3s orbital in magnesium. Less energy is therefore needed to remove it, even though Al has a higher nuclear charge. This dip is characteristic of crossing from an s-block to p-block.
4Successive ionisation energies of an element are 786, 1577, 3232, 4356, 16091, 19805 kJ mol⁻¹. In which group of the Periodic Table is the element?
A.Group 2
B.Group 13
C.Group 14
D.Group 15
Explanation: The large jump occurs between the 4th and 5th ionisation energies (4356 to 16091), showing that the first four electrons are removed from the outer shell and the fifth comes from an inner shell. Four outer electrons means the element is in Group 14 (e.g., silicon). The pattern of successive ionisation energies is a key A-Level skill for identifying group membership.
5Which bond type involves the donation of a lone pair from one atom to form a shared pair, with both electrons coming from the same atom?
A.Ionic bond
B.Standard covalent bond
C.Dative covalent (coordinate) bond
D.Metallic bond
Explanation: A dative covalent (coordinate) bond forms when one atom donates both electrons of the shared pair, while the other atom contributes none. Once formed, a dative bond is chemically identical to a standard covalent bond. Examples include the bond from N to H in NH4+ and from O to B in H3N→BF3 adducts.
6Using VSEPR theory, what is the shape and bond angle of a sulfur hexafluoride (SF6) molecule?
A.Tetrahedral, 109.5°
B.Trigonal bipyramidal, 90° and 120°
C.Octahedral, 90°
D.Square planar, 90°
Explanation: Sulfur in SF6 has six bonding pairs and no lone pairs. Six electron pairs around the central atom adopt an octahedral geometry, with all F–S–F bond angles of 90°. SF6 is a classic example of an expanded octet at A-Level.
7Why does water (H2O) have a much higher boiling point than hydrogen sulfide (H2S), despite H2S having a greater molecular mass?
A.H2O molecules form hydrogen bonds because O is small and highly electronegative with lone pairs
B.H2S is a non-polar molecule
C.H2O has stronger covalent O–H bonds than H2S has S–H bonds
D.H2S has a linear shape while H2O is bent
Explanation: Water exhibits hydrogen bonding between molecules because oxygen is small, highly electronegative, and has two lone pairs. These are unusually strong intermolecular forces and require more energy to overcome during boiling. H2S only experiences weaker dipole-dipole and London forces because S is too large and not electronegative enough for hydrogen bonding.
8What is the shape and approximate bond angle of an ammonia (NH3) molecule?
A.Tetrahedral, 109.5°
B.Trigonal pyramidal, 107°
C.Trigonal planar, 120°
D.Bent (V-shaped), 104.5°
Explanation: Nitrogen in NH3 has three bonding pairs and one lone pair, giving four pairs of electrons. Lone pairs repel more strongly than bonding pairs, so the H–N–H angle is compressed from the tetrahedral 109.5° to about 107°. The resulting molecular shape is trigonal pyramidal.
9Which of the following molecules is polar overall (has a non-zero net dipole moment)?
A.CO2
B.CCl4
C.BF3
D.CHCl3
Explanation: CHCl3 (trichloromethane) is tetrahedral but its four bonds are not identical: three C–Cl polar bonds and one C–H bond. The individual bond dipoles do not cancel, leaving a net dipole moment. CO2, CCl4 and BF3 all have symmetrical shapes (linear, tetrahedral, trigonal planar respectively) where bond dipoles cancel exactly.
10Metallic bonding can be described as which of the following?
A.Electrostatic attraction between oppositely charged ions in a giant lattice
B.Sharing of electron pairs between adjacent atoms
C.Electrostatic attraction between positive metal ions and a sea of delocalised electrons
D.Weak induced-dipole forces between metal atoms
Explanation: In a metallic lattice, outer-shell electrons become delocalised and can move freely. This 'sea' of electrons is attracted electrostatically to the regularly arranged positive metal cations. This model explains electrical conductivity, malleability, ductility, and the high melting points of most metals.

About the A-Level Chemistry Exam

A-Level Chemistry is offered by AQA, Edexcel, OCR as part of the UK A-Level qualification framework. The course covers physical chemistry, inorganic chemistry, organic chemistry, analytical techniques and is assessed primarily through written exam papers at the end of the two-year course.

Questions

100 scored questions

Time Limit

5-7 hours total across multiple papers

Passing Score

Grade E is the minimum pass, Grades A*-E count as a pass (A*-A-B-C-D-E)

Exam Fee

£75-£130 per subject (school-set entry fee) (AQA, Edexcel, OCR)

A-Level Chemistry Exam Content Outline

Core

Physical: Atomic Structure and Bonding

Subatomic particles, electron configuration, ionic/covalent/metallic bonding, shapes of molecules, intermolecular forces

Core

Physical: Energetics, Kinetics, Equilibrium

Enthalpy, Hess's law, rates of reaction, Maxwell-Boltzmann, equilibria (Kc, Kp), Le Chatelier

Core

Physical: Redox, Acids and Electrochemistry

Oxidation numbers, electrochemical cells, Brønsted-Lowry acids/bases, pH, Ka, buffers

Core

Inorganic Chemistry

Periodicity, Group 2, Group 7 (halogens), Period 3 oxides, transition metals (complexes, colour, catalysis)

Core

Organic Chemistry

Alkanes, alkenes, halogenoalkanes, alcohols, aldehydes, ketones, carboxylic acids, esters, amines, aromatic chemistry, polymers, amino acids, proteins, DNA

Core

Analytical Techniques

Mass spectrometry, infrared spectroscopy, NMR (proton and carbon), chromatography

How to Pass the A-Level Chemistry Exam

What You Need to Know

  • Passing score: Grade E is the minimum pass, Grades A*-E count as a pass (A*-A-B-C-D-E)
  • Exam length: 100 questions
  • Time limit: 5-7 hours total across multiple papers
  • Exam fee: £75-£130 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

A-Level 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 A-Level Chemistry?

A-Level 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 A-Level Chemistry exam taken?

Exams are written in the May-June series at the end of the two-year linear A-Level course. Most students sit the papers in Year 13.

How is A-Level Chemistry graded?

A-Levels are graded A*-E. A* is the highest grade and E is the minimum pass. UCAS tariff points are awarded for A-Level grades on most university applications.

How many papers does A-Level Chemistry have?

Most A-Level subjects have 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.