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Practice paper written from an analysis of every
O-Level Chemistry paper, 2009–2026

CHEMISTRY

Specimen 2026

Paper 1 Multiple Choice

FORECAST PAPER · SET 10 Hard

For practice before the 2026 examination

1 hour

Additional Materials: Paper for your answers, numbered 1 to 40

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.

There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.

Choose the one you consider correct and record your choice on a separate sheet of paper, numbered 1 to 40.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.

Any rough working should be done in this booklet.

A copy of the Periodic Table is printed on page 18.

The use of an approved scientific calculator is expected, where appropriate.

This document consists of 17 printed pages and 1 blank page.

NOT AN OFFICIAL EXAMINATION PAPER
Written for classroom practice from the topic frequencies in the chermistry theory-paper analysis. It follows the layout, wording and mark scheme conventions of the O-Level Chemistry papers but is not set, endorsed or marked by any examination board.

1Hard

A gas is dried by passing it through a tube of calcium oxide.

The dry gas is then collected in a gas jar, as shown.

Which gas can be dried and collected in this way?

[average M_r of air, 29]

Aammonia

Bcarbon dioxide

Chydrogen

Dpropane

2Hard

A pure sample of compound Y melts at 80 °C and boils at 200 °C.

A research student heats a sample of Y steadily and records its temperature, as shown.

Which row describes the sample at 10 minutes and the purity of the sample?

	state of the sample at 10 minutes	the sample is
A	solid	impure
B	liquid	impure
C	liquid	pure
D	solid	pure

3Hard

A research team analyses a sample of steel and detects the particles shown in nuclide notation.

15828Ni²⁺

25426Fe

35626Fe³⁺

45525Mn²⁺

Which two particles have the same number of electrons but different numbers of neutrons?

A1 and 2

B1 and 3

C2 and 4

D3 and 4

4Hard

An ion of element Z has the electron arrangement 2,8,8 and a charge of 2−. The ion has a nucleon number of 34.

Another isotope of Z has a nucleon number of 32.

The letter Z is not the chemical symbol.

Which row describes an atom of this other isotope?

	protons	neutrons	electrons
A	16	16	16
B	16	16	18
C	18	14	18
D	20	12	20

5Medium

A crystal of an ionic compound breaks into pieces when it is hit sharply with a hammer.

The diagram shows what happens to a layer of ions in the crystal when a force is applied.

Which statement explains why the crystal breaks?

AThe force breaks the covalent bonds between the ions.

BThe force pulls the ions apart so that delocalised electrons escape from the crystal.

CThe force slides a layer of ions so that ions of the same charge are next to each other and repel.

DThe force makes the ions free to move, as they are when the compound is molten.

6Hard

The diagram shows the outer shell electrons in a molecule formed by two elements, X and Y.

The dots are electrons from atoms of X and the crosses are electrons from atoms of Y. The letters are not the chemical symbols.

Which row gives the Groups of the Periodic Table in which X and Y are found?

	Group of X	Group of Y
A	14	16
B	16	16
C	16	14
D	14	14

7Easy

Which material is an alloy?

Acopper(II) oxide

Bsodium chloride

Cstainless steel

Dzinc oxide

8Hard

Iodine, silicon(IV) oxide and poly(ethene) are each heated until they melt or soften.

Which row shows what is overcome when each substance melts or softens?

	iodine	silicon(IV) oxide	poly(ethene)
A	covalent bonds	covalent bonds	covalent bonds
B	covalent bonds	covalent bonds	forces between molecules
C	forces between molecules	covalent bonds	covalent bonds
D	forces between molecules	covalent bonds	forces between molecules

9Hard

The table shows some properties of four solids, P, Q, R and S.

solid	melting point / °C	conducts electricity when solid	conducts electricity when molten
P	770	no	yes
Q	1,540	yes	yes
R	1,710	no	no
S	−7	no	no

The letters are not the chemical symbols.

Which statements are correct?

1R has a high melting point because it has a giant structure of atoms joined by strong covalent bonds.

2S has a low melting point because the covalent bonds within its molecules are weak.

3P conducts electricity when molten because its ions are free to move.

4Q conducts electricity when solid because it contains delocalised electrons.

A1, 2 and 3

B1, 2 and 4

C1, 3 and 4

D2, 3 and 4

10Hard

Cobalt oxide, Co₃O₄, is used in rechargeable batteries.

Each formula unit contains oxide ions, O²⁻, and cobalt ions that are either Co²⁺ or Co³⁺.

How many cobalt ions of each charge are there in one formula unit of Co₃O₄?

	number of Co²⁺ ions	number of Co³⁺ ions
A	0	3
B	1	2
C	2	1
D	3	0

11Hard

A geologist compares four iron ores.

Which ore has the highest percentage by mass of iron?

[A_r: C, 12; O, 16; S, 32; Fe, 56]

AFe₂O₃

BFe₃O₄

CFeCO₃

DFeS₂

12Hard

Copper(II) hydroxide is made by mixing aqueous copper(II) sulfate with aqueous sodium hydroxide. The equation for the reaction is shown.

CuSO₄(aq) + 2NaOH(aq) → Cu(OH)₂(s) + Na₂SO₄(aq)

A research student mixes 24.0 g of copper(II) sulfate with 8.0 g of sodium hydroxide, both dissolved in water. The student collects 6.86 g of dry copper(II) hydroxide.

What is the percentage yield of copper(II) hydroxide?

[A_r: H, 1; O, 16; Na, 23; S, 32; Cu, 64]

A21%

B35%

C47%

D70%

13Easy

Universal Indicator is added to an aqueous solution of an alkali.

Which row describes the ion that the alkali produces in water and the colour of the indicator?

	ion produced by the alkali	colour of Universal Indicator
A	H⁺	purple
B	H⁺	red
C	OH⁻	red
D	OH⁻	purple

14Medium

A research group adds excess dilute hydrochloric acid separately to four magnesium-containing substances.

Which row shows the product, other than magnesium chloride, that forms?

	substance added to the acid	other product or products
A	magnesium oxide	water
B	magnesium carbonate	carbon dioxide only
C	magnesium hydroxide	hydrogen
D	magnesium	water

15Medium

Lead(II) sulfate is insoluble in water.

A technician mixes aqueous lead(II) nitrate with aqueous sodium sulfate and a precipitate forms.

Which procedure gives a pure, dry sample of lead(II) sulfate?

AFilter the mixture, then evaporate the filtrate to dryness.

BEvaporate the mixture until crystals form, leave it to cool, then filter off the crystals and dry them.

CFilter the mixture, wash the residue with distilled water, then dry the residue.

DFilter the mixture, then dry the residue without washing it.

16Hard

Methanol is made by a reversible reaction between carbon monoxide and hydrogen.

A research team tests four sets of conditions. The table shows the results.

conditions	temperature / °C	pressure / atm	catalyst	yield at equilibrium / %	time to reach equilibrium / min
P	300	100	present	42	45
Q	300	100	absent	42	2,400
R	450	100	present	14	5
S	300	200	present	55	30

Which statement about the results is correct?

AUsing a catalyst increases the yield and shortens the time to reach equilibrium.

BRaising the temperature from 300 °C to 450 °C increases the yield and shortens the time to reach equilibrium.

CRaising the pressure from 100 atm to 200 atm increases the yield and shortens the time to reach equilibrium.

DRaising the pressure from 100 atm to 200 atm increases the yield but lengthens the time to reach equilibrium.

17Easy

A gas is bubbled through acidified potassium manganate(VII). The purple solution turns colourless.

Which gas is it?

Aammonia

Bcarbon dioxide

Chydrogen

Dsulfur dioxide

18Medium

Chlorine is added separately to aqueous potassium iodide and to acidified potassium manganate(VII).

Which row describes the colour changes and what chlorine acts as?

	aqueous potassium iodide	acidified potassium manganate(VII)	chlorine acts as
A	colourless to brown	no change	an oxidising agent
B	colourless to brown	purple to colourless	both an oxidising and a reducing agent
C	no change	purple to colourless	a reducing agent
D	no change	no change	neither an oxidising nor a reducing agent

19Hard

Molten lithium chloride is electrolysed using inert electrodes.

1.4 g of lithium forms at the negative electrode.

What is the volume of gas formed at the positive electrode, measured at r.t.p.?

[A_r: Li, 7]

A1.2 dm³

B2.4 dm³

C4.8 dm³

D9.6 dm³

20Hard

Three aqueous solutions are electrolysed using inert electrodes. The products are listed.

•aqueous Q nitrate: Q at the negative electrode, oxygen at the positive electrode

•aqueous R sulfate: hydrogen at the negative electrode, oxygen at the positive electrode

•concentrated aqueous sodium chloride: hydrogen at the negative electrode, chlorine at the positive electrode

The letters Q and R are not the chemical symbols.

Which row shows the products when concentrated aqueous R chloride and aqueous Q sulfate are each electrolysed using inert electrodes?

	concentrated aqueous R chloride		aqueous Q sulfate
	negative electrode	positive electrode	negative electrode	positive electrode
A	hydrogen	chlorine	Q	oxygen
B	hydrogen	oxygen	Q	oxygen
C	R	chlorine	Q	oxygen
D	hydrogen	chlorine	hydrogen	oxygen

21Hard

A steel strip is copper-plated in two set-ups, X and Y. Each uses aqueous copper(II) sulfate as the electrolyte.

Four statements about the set-ups are listed.

1In set-up X, the copper anode increases in mass.

2In set-up X, the blue colour of the electrolyte stays the same.

3In set-up Y, a gas forms at the anode.

4In both set-ups, the steel strip is coated with copper.

Which statements are correct?

A1, 2 and 3

B1, 2 and 4

C1, 3 and 4

D2, 3 and 4

22Medium

Elements P, Q and R are in the same period of the Periodic Table. Their proton numbers increase from P to R.

The oxide of each element is added to dilute hydrochloric acid and to aqueous sodium hydroxide.

•The oxide of P reacts with the acid but not with the alkali.

•The oxide of Q reacts with both the acid and the alkali.

•The oxide of R reacts with the alkali but not with the acid.

Which row is correct?

	most metallic element	least metallic element
A	P	R
B	P	Q
C	Q	R
D	R	P

23Hard

Lithium is above sodium in Group 1. Fluorine is above chlorine in Group 17.

Four predictions about lithium and fluorine, made from their positions in the Periodic Table, are listed.

1Lithium reacts more vigorously with cold water than sodium does.

2Lithium has a higher melting point than sodium.

3Fluorine is a gas at room temperature.

4Fluorine is less reactive than chlorine.

Which predictions are correct?

A1 and 4

B2 and 3

C2 and 4

D3 and 4

24Medium

Potassium chlorate(V) decomposes slowly when it is heated, forming potassium chloride and oxygen.

A small amount of a different powdered oxide is mixed with separate samples of potassium chlorate(V), and each sample is heated at the same temperature. The time taken to collect 30 cm³ of oxygen is measured.

•no oxide added: 640 s

•iron(III) oxide: 150 s

•copper(II) oxide: 90 s

•calcium oxide: 630 s

•magnesium oxide: 625 s

Which two oxides are most likely to be oxides of transition elements?

Airon(III) oxide and copper(II) oxide

Biron(III) oxide and calcium oxide

Ccopper(II) oxide and magnesium oxide

Dcalcium oxide and magnesium oxide

25Hard

A workshop that recycles electronic waste has a waste solution that contains aqueous silver nitrate, aqueous copper(II) nitrate and aqueous zinc nitrate.

Excess iron powder is added to the solution, which is stirred until no further change occurs. The mixture is then filtered.

Which row shows the solids in the filter paper and the metal ions in the filtrate?

	solids in the filter paper	metal ions in the filtrate
A	silver and copper	iron(II) ions and zinc ions
B	silver and copper	zinc ions only
C	silver, copper, iron and zinc	iron(II) ions only
D	silver, copper and iron	iron(II) ions and zinc ions

26Medium

The steel roof of a factory is covered with sheets coated with zinc or with tin. Zinc is more reactive than iron, and tin is less reactive than iron.

The coating on each type of sheet is scratched through to the steel and the sheets are left in damp air.

Which row is correct?

	steel under the scratch in the zinc coating	steel under the scratch in the tin coating
A	rusts	rusts
B	rusts	does not rust
C	does not rust	rusts
D	does not rust	does not rust

27Medium

The energy released when 1 mol of H–Br bonds forms from separate hydrogen atoms and bromine atoms is 366 kJ.

What is the enthalpy change when 0.50 mol of hydrogen bromide molecules, HBr, is broken up into separate hydrogen atoms and bromine atoms?

A−183 kJ

B+183 kJ

C+366 kJ

D+732 kJ

28Hard

When 1 mol of hydrogen reacts with 1 mol of iodine, 587 kJ is taken in to break the bonds in the reactants and 598 kJ is released when the bonds in the product form.

H₂(g) + I₂(g) → 2HI(g)

Hydrogen iodide decomposes when it is heated.

2HI(g) → H₂(g) + I₂(g)

Which row describes the decomposition of 2 mol of hydrogen iodide?

	energy taken in to break the bonds / kJ	overall energy change
A	587	11 kJ released
B	587	11 kJ taken in
C	598	11 kJ released
D	598	11 kJ taken in

29Hard

A chemist wants to increase the rate of a reaction.

Four changes are listed.

1adding a catalyst

2raising the temperature

3increasing the concentration of a reactant

4increasing the surface area of a solid reactant

In which changes does a larger proportion of the collisions between particles have enough energy to react?

A1 and 2

B1 and 3

C2 and 4

D3 and 4

30Hard

A student adds 0.12 g of magnesium ribbon to an excess of dilute hydrochloric acid at different temperatures and measures the time for all of the magnesium to disappear.

•at 20 °C: 96 s

•at 30 °C: 48 s

•at 40 °C: 24 s

•at 50 °C: 12 s

The same pattern continues at higher temperatures.

What is the average rate of reaction at 60 °C, in g of magnesium per second?

A0.0050

B0.010

C0.020

D0.040

31Medium

An alkane burns completely in oxygen.

When 0.10 mol of the alkane burns, 0.40 mol of carbon dioxide and 0.50 mol of water are formed.

What is the molecular formula of the alkane?

AC₄H₈

BC₄H₁₀

CC₅H₁₀

DC₅H₁₂

32Medium

A gas from a cracking experiment is a mixture of ethane, C₂H₆, and ethene, C₂H₄.

A 100 cm³ sample of the mixture is bubbled through excess aqueous bromine. The volume of gas that leaves the aqueous bromine is 40 cm³, measured at the same temperature and pressure.

What is the volume of ethene in the 100 cm³ sample?

A20 cm³

B40 cm³

C50 cm³

D60 cm³

33Hard

Fatty acids are carboxylic acids with long, unbranched carbon chains that contain only C–C single bonds and C=C double bonds.

Stearic acid, C₁₇H₃₅COOH, has no C=C bonds in its molecules.

Which fatty acid is polyunsaturated?

AC₁₅H₃₁COOH

BC₁₆H₃₁COOH

CC₁₇H₃₁COOH

DC₁₇H₃₃COOH

34Hard

An unbranched alcohol, X, is completely oxidised to a carboxylic acid, Y, by warming with acidified potassium manganate(VII).

The relative molecular mass of Y is 74.

What is the name of X?

[A_r: H, 1; C, 12; O, 16]

Abutan-1-ol

Bethanol

Cmethanol

Dpropan-1-ol

35Easy

Which equation represents the formation of ethanoic acid from ethanol by atmospheric oxygen?

AC₂H₅OH + O₂ → CH₃COOH + H₂O

BC₂H₅OH + 3O₂ → 2CO₂ + 3H₂O

CC₆H₁₂O₆ → 2C₂H₅OH + 2CO₂

DCH₃COOH + C₂H₅OH → CH₃COOC₂H₅ + H₂O

36Hard

Methyl propanoate is an ester that is used in some flavourings.

A student warms 7.4 g of propanoic acid with an excess of methanol and a few drops of concentrated sulfuric acid. The student obtains 5.28 g of methyl propanoate.

What is the percentage yield of methyl propanoate?

[M_r: CH₃CH₂COOH, 74; CH₃OH, 32; H₂O, 18]

A40%

B50%

C60%

D71%

37Hard

Part of a molecule of an addition polymer that is used in sealants is shown.

One molecule of the polymer has a relative molecular mass of 8400.

Which row shows the monomer and the number of monomer molecules that joined to make this molecule of the polymer?

[A_r: H, 1; C, 12]

	monomer	number of monomer molecules
A	(CH₃)₂C=CH₂	150
B	(CH₃)₂C=CH₂	75
C	CH₃CH=CHCH₃	150
D	CH₃CH=CH₂	200

38Medium

Three statements about the disposal of waste plastics are listed.

1Burning waste plastics can release toxic gases such as carbon monoxide.

2Non-biodegradable plastics stay in landfill sites for many years because bacteria do not break them down.

3The carbon dioxide formed when plastics burn is not a pollutant because it is already present in air.

Which statements are correct?

A1, 2 and 3

B1 and 2 only

C1 and 3 only

D2 and 3 only

39Medium

The diagram shows part of the carbon cycle.

Which row identifies the processes P, Q, R and S?

	P	Q	R	S
A	photosynthesis	respiration	combustion	respiration
B	photosynthesis	respiration	respiration	combustion
C	photosynthesis	photosynthesis	respiration	combustion
D	respiration	photosynthesis	respiration	combustion

40Hard

The table shows the concentrations of carbon dioxide and methane in the air in 1850 and in 2020, in parts per million (ppm) by volume.

gas	concentration in 1850 / ppm	concentration in 2020 / ppm
carbon dioxide	280	410
methane	0.80	1.92

Which statement is correct?

ACarbon dioxide has increased by the greater percentage; both gases contribute to global warming.

BCarbon dioxide has increased by the greater percentage; only methane contributes to global warming.

CMethane has increased by the greater percentage; both gases contribute to global warming.

DMethane has increased by the greater percentage; only carbon dioxide contributes to global warming.

The Periodic Table of Elements

Group

Key

hydrogen

helium

lithium

beryllium

proton (atomic) number

atomic symbol

name

relative atomic mass

boron

carbon

nitrogen

oxygen

fluorine

neon

sodium

magnesium

aluminium

silicon

phosphorus

sulfur

chlorine

35.5

argon

potassium

calcium

scandium

titanium

vanadium

chromium

manganese

iron

cobalt

nickel

copper

zinc

gallium

germanium

arsenic

selenium

bromine

krypton

rubidium

strontium

yttrium

zirconium

niobium

molybdenum

technetium

–

ruthenium

101

rhodium

103

palladium

106

silver

108

cadmium

112

indium

115

tin

119

antimony

122

tellurium

128

iodine

127

xenon

131

caesium

133

barium

137

57–71

lanthanoids

hafnium

178

tantalum

181

tungsten

184

rhenium

186

osmium

190

iridium

192

platinum

195

gold

197

mercury

201

thallium

204

lead

207

bismuth

209

polonium

–

astatine

–

radon

–

francium

–

radium

–

89–103

actinoids

104

rutherfordium

–

105

dubnium

–

106

seaborgium

–

107

bohrium

–

108

hassium

–

109

meitnerium

–

110

darmstadtium

–

111

roentgenium

–

112

copernicium

–

113

nihonium

–

114

flerovium

–

115

moscovium

–

116

livermorium

–

117

tennessine

–

118

oganesson

–

lanthanoids

lanthanum

139

cerium

140

praseodymium

141

neodymium

144

promethium

–

samarium

150

europium

152

gadolinium

157

terbium

159

dysprosium

163

holmium

165

erbium

167

thulium

169

ytterbium

173

lutetium

175

actinoids

actinium

–

thorium

232

protactinium

231

uranium

238

neptunium

–

plutonium

–

americium

–

curium

–

berkelium

–

californium

–

einsteinium

–

100

fermium

–

101

mendelevium

–

102

nobelium

–

103

lawrencium

–

The volume of one mole of any gas is 24 dm³ at room temperature and pressure (r.t.p.).

The Avogadro constant, L = 6.02 × 10²³ mol^-1