IGCSE Chemistry Full-length Online Test 1 (Cambridge Paper 2 style MCQs)

1ExtendedCh 1 States of Matter

Ice is heated at a constant rate. As the temperature rises from 0 °C to 100 °C (the sloping section after melting), what is the energy supplied mainly used for?

(a) overcoming the forces of attraction between the particles(b) breaking the bonds between the hydrogen and oxygen atoms(c) making the particles expand(d) increasing the kinetic energy of the particles

2Ch 1 States of Matter

Which describes the particles in a solid?

(a) close together, in a regular pattern, vibrating about fixed positions(b) far apart, random, moving quickly(c) close together, random, sliding past each other(d) far apart, regular, not moving

3Ch 2 Atoms, Elements and Isotopes

What is the relative charge of a neutron?

(a) +1(b) −1(c) 1/1836(d) 0

4Ch 2 Atoms, Elements and Isotopes

Which particle contains 12 protons, 12 neutrons and 10 electrons?

(a) a magnesium-24 atom(b) a sodium-24 ion, Na⁺(c) a magnesium-24 ion, Mg²⁺(d) a neon-22 atom

5Ch 3 Bonding and Structure

Why does diamond not conduct electricity?

(a) it contains ions that cannot move(b) its layers cannot slide over each other(c) its covalent bonds are weak(d) all four outer electrons of each carbon atom are used in covalent bonds

6ExtendedCh 3 Bonding and Structure

Why are metals malleable?

(a) the electrons are fixed in place(b) layers of positive ions can slide over each other(c) the metal atoms share electrons(d) the ions repel each other

7ExtendedCh 4 Formulae, Equations and Relative Masses

Aqueous barium chloride is added to aqueous sodium sulfate, and a white precipitate of barium sulfate forms. Which ions are spectator ions?

(a) Na⁺ and Cl⁻(b) Ba²⁺ and SO₄²⁻(c) Ba²⁺ and Cl⁻(d) Na⁺ and SO₄²⁻

8ExtendedCh 4 Formulae, Equations and Relative Masses

Aqueous lead(II) nitrate reacts with aqueous potassium iodide to form a yellow precipitate of lead(II) iodide. What is the ionic equation?

(a) Pb²⁺(aq) + I⁻(aq) → PbI(s)(b) K⁺(aq) + NO₃⁻(aq) → KNO₃(s)(c) Pb(NO₃)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO₃(aq)(d) Pb²⁺(aq) + 2I⁻(aq) → PbI₂(s)

9Ch 5 The Mole and Calculations

Thymolphthalein is added to aqueous sodium hydroxide in a conical flask, and dilute acid is added from a burette. What is the colour change at the end-point?

(a) blue to colourless(b) colourless to blue(c) yellow to red(d) red to yellow

10ExtendedCh 5 The Mole and Calculations

25.0 cm³ of aqueous sodium hydroxide is exactly neutralised by 20.0 cm³ of 0.150 mol/dm³ hydrochloric acid: NaOH + HCl → NaCl + H₂O. What is the concentration of the sodium hydroxide?

(a) 0.120 mol/dm³(b) 0.188 mol/dm³(c) 0.0600 mol/dm³(d) 0.240 mol/dm³

11Ch 6 Electrolysis and Fuel Cells

Molten potassium chloride is electrolysed. What are the products?

(a) hydrogen at the cathode, chlorine at the anode(b) potassium at the cathode, chlorine at the anode(c) chlorine at the cathode, potassium at the anode(d) potassium at the cathode, oxygen at the anode

12Ch 6 Electrolysis and Fuel Cells

Dilute sulfuric acid is electrolysed with inert electrodes. What forms at the cathode?

(a) oxygen(b) hydrogen(c) sulfur(d) sulfur dioxide

13Ch 7 Chemical Energetics

On a reaction pathway diagram for an exothermic reaction, what does the vertical distance between the reactant level and the product level show?

(a) the energy given out to the surroundings(b) the activation energy(c) the temperature of the reaction(d) the energy of the products only

14Ch 7 Chemical Energetics

Hand warmers use which type of reaction?

(a) endothermic(b) exothermic(c) electrolysis(d) photosynthesis

15Ch 8 Chemical Changes and Rates of Reaction

Why is cotton wool placed in the neck of the flask in the mass-loss method?

(a) to stop gas escaping(b) to keep the flask warm(c) to catalyse the reaction(d) to let gas escape but stop acid spray escaping

16Ch 8 Chemical Changes and Rates of Reaction

Which is a chemical change?

(a) burning wood(b) melting ice(c) dissolving sugar(d) boiling water

17Ch 9 Reversible Reactions and Equilibrium

Which symbol shows a reversible reaction?

(a) ⇌(b) →(c) =(d) ↑

18Ch 9 Reversible Reactions and Equilibrium

Removing water from a hydrated salt by heating is

(a) exothermic(b) a combustion(c) endothermic(d) a neutralisation

19Ch 10 Redox

In the thermite reaction, 2Al + Fe₂O₃ → Al₂O₃ + 2Fe, which statement is correct?

(a) aluminium is reduced and iron(III) oxide is oxidised(b) aluminium is oxidised and iron(III) oxide is reduced(c) iron(III) oxide is oxidised and aluminium oxide is reduced(d) iron is oxidised and aluminium oxide is reduced

20Ch 10 Redox

Rusting of iron is

(a) a reduction of iron(b) an oxidation of iron(c) a neutralisation(d) a decomposition

21ExtendedCh 11 Acids, Bases and Oxides

Which oxide is amphoteric?

(a) Na₂O(b) CO₂(c) ZnO(d) SO₂

22Ch 11 Acids, Bases and Oxides

Which oxide is acidic?

(a) SO₂(b) CaO(c) CuO(d) MgO

23Ch 12 Preparation of Salts

Which chloride is insoluble?

(a) sodium chloride(b) zinc chloride(c) copper(II) chloride(d) lead(II) chloride

24Ch 12 Preparation of Salts

How do you know that excess magnesium carbonate has been added to an acid?

(a) the solution turns blue(b) the solution gets hot(c) fizzing stops and solid remains(d) a precipitate forms

25Ch 13 The Periodic Table

An element forms an ion with a charge of 3−. In which group of the Periodic Table is it?

(a) Group III(b) Group VI(c) Group VII(d) Group V

26Ch 13 The Periodic Table

Why do elements in the same group have similar chemical properties?

(a) same number of shells(b) same mass(c) same number of neutrons(d) same number of outer-shell electrons

27ExtendedCh 14 Metals, Alloys and Reactivity

Why are alloys harder than pure metals?

(a) the atoms are joined by covalent bonds(b) different-sized atoms stop the layers sliding over each other(c) they contain more electrons(d) they are compounds

28ExtendedCh 14 Metals, Alloys and Reactivity

In terms of ions, why is magnesium more reactive than copper?

(a) magnesium has a greater tendency to form positive ions(b) magnesium forms negative ions(c) copper loses electrons more easily(d) magnesium has more protons

29ExtendedCh 15 Corrosion and Extraction of Metals

Which half-equation shows the reaction that protects galvanised iron at a scratch?

(a) Fe → Fe²⁺ + 2e⁻(b) Zn²⁺ + 2e⁻ → Zn(c) Zn → Zn²⁺ + 2e⁻(d) Fe³⁺ + 3e⁻ → Fe

30Ch 15 Corrosion and Extraction of Metals

In a rusting experiment, anhydrous calcium chloride is put in a stoppered tube with an iron nail. What is its purpose?

(a) to absorb water vapour from the air in the tube(b) to absorb oxygen from the air in the tube(c) to speed up rusting(d) to coat the nail with a protective layer

31Ch 16 Water and Fertilisers

Which elements do NPK fertilisers supply?

(a) nitrogen, phosphate, potash(b) nitrogen, phosphorus, potassium(c) sodium, phosphorus, potassium(d) nitrogen, potassium, krypton

32ExtendedCh 16 Water and Fertilisers

What is the percentage by mass of nitrogen in ammonium sulfate, (NH₄)₂SO₄ (Mᵣ = 132)?

(a) 10.6%(b) 28.0%(c) 21.2%(d) 35.0%

33Ch 17 Air Quality and Climate

What is the approximate percentage of oxygen in clean, dry air?

(a) 21%(b) 78%(c) 1%(d) 50%

34Ch 17 Air Quality and Climate

What is needed for photosynthesis besides CO₂ and water?

(a) oxygen and heat(b) a platinum catalyst(c) light and chlorophyll(d) nitrogen

35Ch 18 Organic Chemistry: Fuels and Alkanes

How is petroleum separated into fractions?

(a) fractional distillation(b) cracking(c) filtration(d) chromatography

36Ch 18 Organic Chemistry: Fuels and Alkanes

What is a saturated compound?

(a) it contains a C=C bond(b) all carbon–carbon bonds are single(c) it contains oxygen(d) it is dissolved in water

37Ch 19 Alkenes, Alcohols and Carboxylic Acids

Hexane, an alkane, is shaken with bromine water. What is seen?

(a) orange to colourless(b) colourless to orange(c) a white precipitate forms(d) the bromine water stays orange

38Ch 20 Polymers

In the biodegradability experiment, which must be kept the same for all the samples?

(a) the size of the samples, the type of soil and the temperature(b) the type of plastic(c) the mass lost by each sample(d) the time taken to break down

39Ch 21 Experimental Techniques and Separation

How many spots does a pure substance give on a chromatogram?

(a) one(b) none(c) two(d) several

40Ch 22 Identification of Ions and Gases

Which gas turns damp red litmus blue?

(a) chlorine(b) sulfur dioxide(c) carbon dioxide(d) ammonia

IGCSE Chemistry Full Test 1

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