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1

Which statement about solids, liquids or gases is correct?

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

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2

Which substance is a mixture?

11. Organic chemistry  →  11.3. Fuels

10. Chemistry of the environment  →  10.1. Water

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3

The structure of an atom of element X is shown...

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

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4

Sodium reacts with chlorine to form sodium chloride. Which statements describe what happens to the sodium atoms in this reaction?

2. Atoms, elements and compounds  →  2.4. Ions and ionic bonds

6. Chemical reactions  →  6.4. Redox

9. Metals  →  9.4. Reactivity series

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5

Which statement about ammonia is correct?

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

2. Atoms, elements and compounds  →  2.4. Ions and ionic bonds

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6

Which row describes the structure and a use of graphite?

2. Atoms, elements and compounds  →  2.6. Giant covalent structures

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

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7

The equation represents the reaction between solid magnesium oxide and dilute hydrochloric acid to form magnesium chloride and water. MgO + 2HCl  MgCl 2 + H2O Which row shows the state symbols for hydrochloric acid, magnesium chloride and water?

3. Stoichiometry  →  3.1. Formulae

9. Metals  →  9.4. Reactivity series

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8

What is the equation for the reaction between calcium and chlorine?

11. Organic chemistry  →  11.4. Alkanes

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

9. Metals  →  9.4. Reactivity series

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9

Calcium nitrate has the formula Ca(NO3)2. What is the relative formula mass, Mr, of calcium nitrate?

3. Stoichiometry  →  3.2. Relative masses of atoms and molecules

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

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10

Dilute sulfuric acid is electrolysed using platinum electrodes. The gases produced at each electrode are collected. The gases are mixed together and ignited with a lighted splint. What is formed during this reaction?

4. Electrochemistry  →  4.1. Electrolysis

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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11

Electricity is passed through molten sodium chloride using inert electrodes. What is observed at the electrodes?

4. Electrochemistry  →  4.1. Electrolysis

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12

Fuel cells are used as energy sources in cars. Which row gives a fuel used in a fuel cell and the products formed?

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

11. Organic chemistry  →  11.3. Fuels

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13

When water is added to anhydrous iron(chloride, FeCl 3, hydrated iron(chloride, FeCl 3•6H2O, is formed and energy is given out. FeCl 3 + 6H2O FeCl 3•6H2O Which reaction pathway diagram represents the formation of anhydrous iron(chloride in the reverse reaction?

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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14

Which process is a chemical change?

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

6. Chemical reactions  →  6.1. Physical and chemical changes

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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15

Anhydrous cobalt(chloride is blue and turns pink when water is added. How is this reaction reversed?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

10. Chemistry of the environment  →  10.1. Water

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16

Ethanol can be turned into ethanoic acid by passing it over hot copper(oxide. CH3CH2OH + 2CuO  CH3COOH + H2O + 2Cu What is this type of reaction?

11. Organic chemistry  →  11.7. Carboxylic acids

11. Organic chemistry  →  11.6. Alcohols

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17

When heated strongly, silicon(oxide reacts with carbon. SiO2 + 2C  Si + 2CO Which term describes what happens to silicon(oxide?

2. Atoms, elements and compounds  →  2.6. Giant covalent structures

6. Chemical reactions  →  6.4. Redox

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18

Information about four solutions, P, Q, R and S, is listed. Solution P reacts with ammonium chloride to form ammonia. Solution Q reacts with sodium carbonate to form carbon dioxide. Solution R contains a high concentration of OH– ions. Solution S turns litmus red. Which solutions are alkaline?

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

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

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19

Which oxides are basic?

7. Acids, bases and salts  →  7.2. Oxides

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20

Which row describes the changes across a period of the Periodic Table, from left to right?

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

8. The Periodic Table  →  8.1. Arrangement of elements

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21

Which row shows properties of an element that is in the same group of the Periodic Table as lithium?

8. The Periodic Table  →  8.1. Arrangement of elements

8. The Periodic Table  →  8.2. Group I properties

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22

Which row describes how the properties of Group I elements change as the group is descended?

8. The Periodic Table  →  8.2. Group I properties

8. The Periodic Table  →  8.1. Arrangement of elements

8. The Periodic Table  →  8.3. Group VII properties

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23

The elements in Group VII include chlorine, bromine and iodine. Which statements are correct?

8. The Periodic Table  →  8.3. Group VII properties

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24

Cobalt is a transition element. What is a property of cobalt?

8. The Periodic Table  →  8.4. Transition elements

9. Metals  →  9.1. Properties of metals

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25

Which statements about brass are correct?

9. Metals  →  9.3. Alloys and their properties

9. Metals  →  9.1. Properties of metals

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26

Aluminium is used to make containers for storing food. Which property makes it suitable for this use?

9. Metals  →  9.2. Uses of metals

9. Metals  →  9.3. Alloys and their properties

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27

Which pair of diagrams represents both a pure metal and an alloy?

9. Metals  →  9.3. Alloys and their properties

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28

A metal M is between sodium and magnesium in the reactivity series. Which reactions occur with M and its oxide?

9. Metals  →  9.4. Reactivity series

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29

The diagrams show experiments to investigate rusting of iron nails. boiled water salt water tap water layer of oil In which test-tubes do the nails rust?

9. Metals  →  9.5. Corrosion of metals

9. Metals  →  9.1. Properties of metals

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30

Some uses of water are listed. for drinking in chemical reactions in swimming pools in washing For which uses is it necessary to chlorinate the water?

10. Chemistry of the environment  →  10.1. Water

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31

Two tests are done on an NPK fertiliser. test 1 flame test test 2 heat with aqueous sodium hydroxide and aluminium foil Which observations are made?

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

11. Organic chemistry  →  11.5. Alkenes

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32

The gases from the engine of a car contain oxides of nitrogen. How are these oxides formed?

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

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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33

Which statements explain why plastics should be recycled?

11. Organic chemistry  →  11.8. Polymers

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34

Unwanted vegetation is sometimes placed in a bin where it decomposes. The compost formed is used to fertilise soils. Which gas is likely to be present in a higher percentage inside the bin than in the air outside the bin?

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

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35

Ethene reacts with steam and with bromine in two separate reactions. What are the products of these two reactions?

11. Organic chemistry  →  11.2. Naming organic compounds

11. Organic chemistry  →  11.5. Alkenes

11. Organic chemistry  →  11.6. Alcohols

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36

Four types of reactions are listed. substitution combustion polymerisation addition Which reactions will ethane undergo?

11. Organic chemistry  →  11.2. Naming organic compounds

11. Organic chemistry  →  11.4. Alkanes

11. Organic chemistry  →  11.6. Alcohols

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37

The flow diagram shows how polymay be made from petroleum. petroleum fuel oil ethene poly1 What are stages 1, 2 and 3?

11. Organic chemistry  →  11.8. Polymers

11. Organic chemistry  →  11.3. Fuels

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38

Magnesium reacts with dilute hydrochloric acid to produce hydrogen gas. Which pieces of apparatus are needed to determine the rate of this reaction?

6. Chemical reactions  →  6.2. Rate of reaction

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39

The chromatograms of four different dyes are shown...

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

6. Chemical reactions  →  6.4. Redox

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40

The results of some tests on an aqueous solution of substance X are listed. A cream precipitate is produced when adding aqueous silver nitrate. Adding aqueous sodium hydroxide produces a green precipitate which dissolves in excess alkali. Adding aqueous ammonia produces a green precipitate which is insoluble in excess ammonia. What is substance X?

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

10. Chemistry of the environment  →  10.1. Water

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