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1

The diagram shows the result of dropping a purple crystal into water. water purple crystal after five hours purple solution Which processes take place in this experiment?

7. Acids, bases and salts  →  7.3. Preparation of salts

12. Experimental techniques and chemical analysis  →  12.1. Experimental design

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2

Which row about elements, mixtures and compounds is correct?

9. Metals  →  9.3. Alloys and their properties

2. Atoms, elements and compounds  →  2.1. Elements, compounds and mixtures

8. The Periodic Table  →  8.1. Arrangement of elements

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3

The atomic structures of four particles, W, X, Y and Z, are shown...

2. Atoms, elements and compounds  →  2.3. Isotopes

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

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4

Which statement explains why isotopes of the same element have the same chemical properties?

2. Atoms, elements and compounds  →  2.3. Isotopes

8. The Periodic Table  →  8.1. Arrangement of elements

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5

Nitrogen forms a nitride ion with the formula N3–. Which particle does not have the same electronic configuration as the nitride ion?

8. The Periodic Table  →  8.1. Arrangement of elements

2. Atoms, elements and compounds  →  2.2. Atomic structure and the Periodic Table

8. The Periodic Table  →  8.5. Noble gases

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6

Which row describes the formation of single covalent bonds in methane?

2. Atoms, elements and compounds  →  2.5. Simple molecules and covalent bonds

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7

Which formula is an empirical formula?

3. Stoichiometry  →  3.1. Formulae

3. Stoichiometry  →  3.3. The mole and the Avogadro constant

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8

Heating iron sulfide, FeS2, in air produces sulfur dioxide. 4FeS2 + 11O2 → 2Fe2O3 + 8SO2 What is the maximum mass of sulfur dioxide produced from 120 kg of iron sulfide?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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9

Which substance produces hydrogen and bromine when electrolysed?

4. Electrochemistry  →  4.1. Electrolysis

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10

Which statements about hydrogen fuel cells are correct?

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

4. Electrochemistry  →  4.1. Electrolysis

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11

Ethene gas, C2H4, is completely burned in excess oxygen to form carbon dioxide and water. The equation for this exothermic reaction is shown...

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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12

Which row describes the effect on the activation energy and the frequency of particle collisions when the temperature of a chemical reaction is increased?

6. Chemical reactions  →  6.2. Rate of reaction

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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13

Solid copper(sulfate exists in two different forms, anhydrous and hydrated. One of these forms is blue and the other is white. The change between these two forms is reversible. blue form white form What is the blue form and how is the change from the blue form to the white form brought about?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

10. Chemistry of the environment  →  10.1. Water

4. Electrochemistry  →  4.1. Electrolysis

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14

Sodium ions, Na+, and oxygen ions, O2–, combine with chromium ions to form a salt. The salt sodium dichromate has the formula Na2Cr2O7. What is the oxidation state of chromium in this salt?

6. Chemical reactions  →  6.4. Redox

9. Metals  →  9.4. Reactivity series

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15

The concentration of hydrogen ions in 100 cm3 of 0.1 mol / dm3 hydrochloric acid is higher than the concentration of hydrogen ions in 100 cm3 of 0.1 mol / dm3 ethanoic acid. Which statement explains the difference in hydrogen ion concentration?

7. Acids, bases and salts  →  7.1. The characteristic properties of acids and bases

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16

Which oxide is classified as an amphoteric oxide?

7. Acids, bases and salts  →  7.2. Oxides

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17

Which method produces the salt copper(carbonate?

7. Acids, bases and salts  →  7.3. Preparation of salts

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

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18

Which statements about the trends across a period of the Periodic Table are correct?

8. The Periodic Table  →  8.1. Arrangement of elements

9. Metals  →  9.3. Alloys and their properties

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19

Some information about elements in Group II of the Periodic Table is shown...

8. The Periodic Table  →  8.2. Group I properties

8. The Periodic Table  →  8.1. Arrangement of elements

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20

A new element oxfordium, Ox, was discovered with the following properties. solubility electrical conduction formula of element bonding in a molecule of Ox2 insoluble in water does not conduct Ox2 Ox Ox In which group of the Periodic Table should the new element be placed?

8. The Periodic Table  →  8.1. Arrangement of elements

8. The Periodic Table  →  8.3. Group VII properties

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21

Which row describes a similarity and a difference between chlorine and bromine?

8. The Periodic Table  →  8.3. Group VII properties

11. Organic chemistry  →  11.5. Alkenes

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22

Which statement describes transition elements?

8. The Periodic Table  →  8.4. Transition elements

1. States of matter  →  1.1. Solids, liquids and gases

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23

Which gas is made when powdered zinc is added to dilute hydrochloric acid?

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

9. Metals  →  9.4. Reactivity series

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24

The diagram represents the structure of a solid. Which solids does the diagram represent?

9. Metals  →  9.3. Alloys and their properties

11. Organic chemistry  →  11.8. Polymers

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25

Steel is an alloy of iron. Which statement explains why steel is stronger than iron?

9. Metals  →  9.3. Alloys and their properties

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26

Three students, X, Y and Z, are told that solid P reacts with dilute acids and also conducts electricity. The table shows the students’ suggestions about the identity of P. X Y Z copper iron graphite Which students are correct?

4. Electrochemistry  →  4.1. Electrolysis

9. Metals  →  9.4. Reactivity series

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27

Which statement explains why aluminium appears to be unreactive?

9. Metals  →  9.4. Reactivity series

9. Metals  →  9.3. Alloys and their properties

9. Metals  →  9.2. Uses of metals

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28

During the electrolysis of aluminium oxide, the mass of the carbon anode changes. Which row describes the change and gives a reason for this change?

4. Electrochemistry  →  4.1. Electrolysis

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29

Several processes are used to treat domestic water. Which row identifies a reason for the given process?

10. Chemistry of the environment  →  10.1. Water

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30

What is the equation for photosynthesis?

10. Chemistry of the environment  →  10.3. Air quality and climate

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31

Which statement describes how the C–H bonds in methane gas in the atmosphere contribute to global warming?

10. Chemistry of the environment  →  10.3. Air quality and climate

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32

The structural formulae of two hydrocarbons are shown...

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.1. Formulae, functional groups and terminology

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33

The structural formula of compound Q is given. CH3CH2CH2COOCH2CH2CH3 What is compound Q?

3. Stoichiometry  →  3.1. Formulae

11. Organic chemistry  →  11.1. Formulae, functional groups and terminology

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34

The fractional distillation of petroleum is shown...

11. Organic chemistry  →  11.3. Fuels

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35

Which equation represents the cracking of an alkane?

11. Organic chemistry  →  11.5. Alkenes

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36

What is the structure of the product of the reaction of propene with bromine?

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.2. Naming organic compounds

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37

In reaction R, 2000 molecules of CH2=CH2 react to form a single molecule X only. 2000 CH2=CH2 → X Which terms describe reaction R, CH2=CH2 and X?

11. Organic chemistry  →  11.4. Alkanes

11. Organic chemistry  →  11.5. Alkenes

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38

Part of the structure of a polymer is shown...

11. Organic chemistry  →  11.8. Polymers

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39

The concentration of acids and alkalis can be determined by titration. Which pieces of equipment are needed to perform a titration?

12. Experimental techniques and chemical analysis  →  12.2. Acid-base titrations

12. Experimental techniques and chemical analysis  →  12.5. Identification of ions and gases

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40

Which chromatogram shows how the Rf value of a substance is calculated?

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

3. Stoichiometry  →  3.3. The mole and the Avogadro constant

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