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100+ Free IGCSE Chemistry Practice Questions

Pass your Cambridge IGCSE Chemistry (0620) exam on the first try — instant access, no signup required.

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Which gas is given off when ammonium chloride is warmed with aqueous sodium hydroxide?

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Key Facts: IGCSE Chemistry Exam

0620

Cambridge IGCSE Chemistry syllabus code

Cambridge International

3 papers

MCQ + theory + practical/ATP

Cambridge 0620 syllabus 2026-2028

A*-E

Extended grading scale

Cambridge International

100

Free practice questions here

OpenExamPrep

Cambridge IGCSE Chemistry 0620 (2026-2028) is assessed by three papers: a 40-mark multiple-choice paper (Paper 1 Core or Paper 2 Extended), an 80-mark short-answer and structured theory paper (Paper 3 Core or Paper 4 Extended), and a 40-mark practical (Paper 5) or alternative to practical (Paper 6). Weighting is 30% MCQ, 50% theory, 20% practical.

Sample IGCSE Chemistry Practice Questions

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

1Which statement correctly describes the particles in a solid?
A.Far apart, moving randomly in all directions
B.Close together in a regular pattern, vibrating about fixed positions
C.Close together but able to slide past each other
D.Touching and moving in straight lines until they collide
Explanation: In a solid the particles are packed closely in a fixed, regular arrangement (lattice) and can only vibrate about their fixed positions. This explains why solids have a fixed shape and fixed volume.
2What is the name of the change of state from a gas directly to a solid?
A.Condensation
B.Sublimation
C.Deposition
D.Freezing
Explanation: Deposition is the change of state directly from gas to solid without passing through the liquid state. Cambridge 0620 treats it as the reverse of sublimation; both terms 'sublimation' and its reverse appear in mark schemes.
3Two gases, hydrogen (Mr = 2) and oxygen (Mr = 32), are released at the same point. Which statement is correct?
A.Oxygen diffuses faster than hydrogen because it is heavier
B.Hydrogen diffuses faster than oxygen because lighter particles move faster at the same temperature
C.Both diffuse at the same rate because the temperature is identical
D.Neither gas diffuses at room temperature
Explanation: At a given temperature lighter molecules have greater average speeds, so they diffuse faster. Graham's law states the rate of diffusion is inversely proportional to the square root of relative molecular mass, so hydrogen (Mr 2) diffuses faster than oxygen (Mr 32).
4What happens to the kinetic energy of particles in a substance as it is heated from solid to gas?
A.It decreases
B.It stays the same
C.It increases
D.It only changes at the melting point
Explanation: Heating supplies energy that is stored as kinetic energy of the particles, increasing their average speed and the rate at which they move or vibrate. At phase changes the energy goes into breaking forces between particles rather than raising the temperature, but overall kinetic energy still rises across the heating process.
5Why does a gas exert pressure on the walls of its container?
A.Because the particles attract the walls
B.Because the particles collide with the walls and exert a force
C.Because gravity pulls the particles downwards
D.Because the particles dissolve into the container walls
Explanation: Gas particles move randomly at high speed. When they collide with the container walls they exert a force; the total force per unit area is the pressure.
6A liquid is heated in a sealed container. What happens to its boiling point compared with boiling in an open beaker?
A.It is lower because pressure decreases
B.It is the same as in an open beaker
C.It is higher because pressure increases
D.It cannot boil at all
Explanation: In a sealed container, vapour cannot escape so the gas pressure above the liquid rises. A liquid boils when its vapour pressure equals the surrounding pressure, so a higher external pressure raises the boiling point.
7Bromine vapour and air are placed in two connected gas jars. After a few minutes the brown bromine colour is seen throughout both jars. Which process explains this observation?
A.Convection
B.Diffusion of particles from areas of higher to lower concentration
C.Chemical reaction between bromine and air
D.Condensation of bromine onto the glass
Explanation: Diffusion is the random movement of particles from a region of higher concentration to a region of lower concentration. Bromine molecules and air molecules spread until evenly mixed throughout both jars.
8Which arrangement best describes a liquid?
A.Particles widely spaced in random positions, moving at high speed
B.Particles close together but with no fixed positions, free to move past each other
C.Particles in a rigid lattice, only vibrating
D.Particles arranged in flat layers that slide easily over each other
Explanation: In a liquid the particles are close together (similar to a solid) but they are not in fixed positions and can move past one another. This is why liquids have a fixed volume but take the shape of their container.
9Which factor would NOT increase the rate of diffusion of a gas through air?
A.Increasing the temperature
B.Decreasing the relative molecular mass of the gas
C.Increasing the pressure of the surrounding air
D.Using a gas with smaller molecules
Explanation: Diffusion is faster when particles move faster (higher temperature) or are lighter (smaller Mr). Increasing the pressure of the surrounding air makes diffusion slower because gas particles have to push through more collisions per second.
10During melting, the temperature of a pure substance stays constant. Why?
A.No energy is being supplied
B.Energy is used to weaken the forces between particles rather than to raise the temperature
C.The thermometer is faulty during a state change
D.The kinetic energy of the particles decreases
Explanation: At the melting point, energy supplied is absorbed as latent heat to break or weaken the forces of attraction between particles in the solid lattice, allowing the substance to change to a liquid. Until all of the solid has melted, the temperature does not rise.

About the IGCSE Chemistry Exam

Cambridge IGCSE Chemistry (0620) is awarded by Cambridge Assessment International Education and can be taken at Core (grades C-G) or Extended tier (grades A*-E). The 2026-2028 syllabus covers the particulate nature of matter, atomic structure and bonding, stoichiometry, electrochemistry, energetics, rates and equilibria, acids and bases, the periodic table, metals, air and water, and organic chemistry, assessed via a multiple-choice paper, a theory paper, and a practical or alternative to practical paper.

Questions

100 scored questions

Time Limit

Approx. 3 hours 15 minutes total: MCQ 45 min + theory 1 h 15 min + practical/ATP 1 h 15 min

Passing Score

Grade C is the standard pass (Extended A*-E); Core graded C-G

Exam Fee

£40-£90 per subject (school-set entry fee) (Cambridge Assessment International Education (CAIE))

IGCSE Chemistry Exam Content Outline

~10%

States of Matter

Kinetic particle theory for solids, liquids and gases; changes of state including melting, freezing, boiling, condensing and sublimation; diffusion and the effect of relative molecular mass on diffusion rate (Graham's law)

~10%

Atoms, Elements and Compounds

Protons, neutrons and electrons; atomic number Z and mass number A; isotopes and calculation of relative atomic mass from abundance; electron shells (2,8,8); ionic, covalent and metallic bonding; simple and giant covalent structures (diamond, graphite, silicon dioxide, fullerenes); properties from structure

~10%

Stoichiometry

Relative formula mass Mr, mole = mass/Mr, Avogadro's constant, moles from equations, percentage yield and percentage atom economy, gas volumes at RTP (24 dm3/mol), concentration in mol/dm3 and g/dm3, titration calculations

~10%

Electrochemistry

Electrolysis of molten lead bromide; aqueous solutions and H+ vs metal-ion preference; chlor-alkali (concentrated NaCl) producing H2, Cl2 and NaOH; electroplating; dilute sulfuric acid; copper purification; aluminium extraction from Al2O3 in molten cryolite; hydrogen-oxygen fuel cells

~10%

Chemical Energetics

Exothermic vs endothermic reactions and energy level diagrams; activation energy; bond breaking is endothermic and bond making is exothermic; calculation of enthalpy change from bond energies; calorimetry using q = mcDeltaT

~10%

Chemical Reactions

Physical vs chemical changes; rate factors (temperature, concentration/pressure, surface area, catalyst); collision theory; reversible reactions and dynamic equilibrium; Haber process (450 C, 200 atm, Fe); contact process for sulfuric acid; redox in terms of electrons and oxygen; oxidising and reducing agent tests

~15%

Acids, Bases and Salts

pH scale and indicators (litmus, methyl orange, phenolphthalein, universal); strong vs weak acids; acids with metals, bases and carbonates; preparation of soluble and insoluble salts; titration to find unknown concentration; solubility rules; cation and anion tests; flame tests for Li, Na, K, Ca, Cu

~10%

The Periodic Table

Group 1 alkali metals (reactivity increases down group); Group 7 halogens (reactivity decreases down); transition metals (variable oxidation states, coloured compounds, catalytic activity); noble gases inert; period 3 trends

~10%

Metals

Reactivity series K Na Ca Mg Al (C) Zn Fe Sn Pb (H) Cu Ag Au; displacement reactions; extraction methods linked to reactivity (electrolysis for Al, blast furnace for Fe, none for Au); rust prevention (galvanising, sacrificial protection, painting); alloys (brass, bronze, steel, stainless, duralumin, solder)

~10%

Air and Water

Composition of clean air (78% N2, 21% O2, 1% Ar, 0.04% CO2); pollutants (SO2, NOx, CO, particulates, CH4); ozone depletion by CFCs; catalytic converters; water treatment (sedimentation, filtration, chlorination); water tests (cobalt chloride blue-pink, anhydrous CuSO4 white-blue, b.p. 100 C)

~15%

Organic Chemistry

Alkanes CnH2n+2 (combustion, substitution); alkenes CnH2n (bromine water, addition with H2/Ni, steam/H3PO4 300 C, HBr); addition polymers (polythene, PVC, polypropene); alcohols (fermentation, hydration of ethene); carboxylic acids and esterification; condensation polymers (nylon, Terylene); proteins, fats, soaps; fractional distillation fractions and cracking

How to Pass the IGCSE Chemistry Exam

What You Need to Know

  • Passing score: Grade C is the standard pass (Extended A*-E); Core graded C-G
  • Exam length: 100 questions
  • Time limit: Approx. 3 hours 15 minutes total: MCQ 45 min + theory 1 h 15 min + practical/ATP 1 h 15 min
  • Exam fee: £40-£90 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

IGCSE Chemistry Study Tips from Top Performers

1Use Cambridge 0620 past papers from cambridgeinternational.org — Paper 2 (Extended MCQ) and Paper 4 are the highest-yield practice
2Memorise key tests: cations with NaOH, anions with HCl/BaCl2 or AgNO3, gas tests (limewater for CO2, glowing splint for O2, pop for H2), flame colours
3Show working in mole calculations (n = m/Mr, n = cV, n at RTP = V/24) — method marks reward correct setup
4Learn the reactivity series and the rules that follow from it (extraction method, displacement, electrolysis preference)

Frequently Asked Questions

What is Cambridge IGCSE Chemistry (0620)?

Cambridge IGCSE Chemistry (0620) is the international General Certificate of Secondary Education in Chemistry, awarded by Cambridge Assessment International Education. It can be taken at Core tier (grades C-G) or Extended tier (grades A*-E) and is examined through three papers covering theory and practical skills.

How many papers does IGCSE Chemistry 0620 have?

Candidates take three papers. Core students sit Paper 1 (multiple choice, 45 minutes, 40 marks) and Paper 3 (theory, 1 hour 15 minutes, 80 marks). Extended students sit Paper 2 (multiple choice, 45 minutes, 40 marks) and Paper 4 (theory, 1 hour 15 minutes, 80 marks). All candidates also take Paper 5 (practical) or Paper 6 (alternative to practical).

When are the IGCSE Chemistry exams taken?

Cambridge IGCSE exams run in three series each year: February-March (selected regions), May-June, and October-November. Most candidates sit Chemistry 0620 in the May-June series at the end of their two-year programme.

What is the difference between Core and Extended IGCSE Chemistry?

Core covers the foundational subject content and is graded C to G. Extended covers the Core content plus the Supplement (harder topics such as calculation of relative atomic mass from isotopic abundance, electrolysis of aqueous solutions in detail, enthalpy calculations from bond energies, and the contact process), and is graded A* to E. Students aiming for top grades take Extended.