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1

Oxygen was prepared from hydrogen peroxide and collected as shown...

4. Electrochemistry  →  4.2. Hydrogen–oxygen fuel cells

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

9. Metals  →  9.5. Corrosion of metals

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2

The table gives the properties of four substances. Which substance is a solid metal at room temperature?

9. Metals  →  9.1. Properties of metals

2. Atoms, elements and compounds  →  2.7. Metallic bonding

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

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3

Nitrogen dioxide is a dark brown gas and is more dense than air. A gas jar containing nitrogen dioxide is sealed with a glass plate and is then inverted on top of a gas jar containing air. nitrogen dioxide air glass plate The glass plate is removed. Which one of the following correctly describes the colours inside the gas jars after a long period of time?

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

8. The Periodic Table  →  8.3. Group VII properties

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4

A student tested a solution by adding aqueous sodium hydroxide. A precipitate was not seen because the reagent was added too quickly. What could not have been present in the solution?

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

10. Chemistry of the environment  →  10.1. Water

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

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5

Which substance has a giant molecular structure at room temperature?

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

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

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

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6

When a covalent liquid boils its molecules become more widely spaced. Which property of the molecules has the most influence on the energy required to boil a covalent liquid?

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

11. Organic chemistry  →  11.5. Alkenes

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7

The diagram shows the chromatogram obtained by analysis of a single dye. Three measurements are shown...

12. Experimental techniques and chemical analysis  →  12.3. Chromatography

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8

The atoms Cu and Zn have the same A nucleon number. B number of electrons. C number of neutrons. D proton number.

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

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9

Why does molten sodium chloride conduct electricity?

4. Electrochemistry  →  4.1. Electrolysis

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

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10

Which equation describes the most suitable reaction for making lead sulphate?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

4. Electrochemistry  →  4.1. Electrolysis

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11

In which oxide does X have the same oxidation state as in the chloride, XCl3?

6. Chemical reactions  →  6.4. Redox

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12

A sample of copper contains a metal impurity which is below copper in the reactivity series. The diagram shows the apparatus used for refining the sample. aqueous copper(sulphate pure copper cathode impure copper anode The loss in mass of the anode (positive electrode) is 50 g and the gain in mass of the cathode (negative electrode) is 45 g. What is the percentage purity of this sample of copper?

9. Metals  →  9.4. Reactivity series

4. Electrochemistry  →  4.1. Electrolysis

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13

One mole of a sample of hydrated sodium sulphide contains 162 g of water of crystallisation. What is the correct formula of this compound?

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

3. Stoichiometry  →  3.1. Formulae

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14

The diagram shows the electrolytic production of aluminium. waste gases cathode carbon anodes What are the products at the electrodes?

4. Electrochemistry  →  4.1. Electrolysis

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15

When dilute sulphuric acid is electrolysed between platinum electrodes, which statements are correct?

4. Electrochemistry  →  4.1. Electrolysis

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16

Which of the following is an endothermic reaction?

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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17

At 400 °C the reaction between hydrogen and iodine reaches an equilibrium. H2+ I22HI∆H = –13 kJ Which change in conditions would increase the percentage of hydrogen iodide in the equilibrium mixture?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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18

The diagram shows the reaction pathway for a reaction without a catalyst. energy reaction pathway Which diagram shows the addition of a catalyst which speeds up the reaction?

6. Chemical reactions  →  6.2. Rate of reaction

5. Chemical energetics  →  5.1. Exothermic and endothermic reactions

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19

Sulphur dioxide reacts with aqueous bromine according to the following equation. SO2+ Br2+ 2H2O→ H2SO4+ 2HBrWhich element has been oxidised?

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

11. Organic chemistry  →  11.5. Alkenes

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20

When 20 cm3 of a 2 mol/dm3 solution of potassium hydroxide is mixed with 20 cm3 of a 1 mol/dm3 solution of sulphuric acid, the temperature of the mixture rises. What best explains this?

9. Metals  →  9.4. Reactivity series

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

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21

A colourless gas is passed into each of three different solutions. The results for each solution are shown...

6. Chemical reactions  →  6.4. Redox

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

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22

Which observation is typical of a solid non-metal element?

9. Metals  →  9.1. Properties of metals

8. The Periodic Table  →  8.4. Transition elements

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23

Which equation represents the reaction between hydrochloric acid and sodium hydroxide?

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

9. Metals  →  9.4. Reactivity series

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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24

The following statements about dilute sulphuric acid are all correct. A white precipitate is formed when aqueous barium chloride is added. The solution turns anhydrous copper(sulphate from white to blue. Addition of Universal Indicator shows that the solution has a pH value of less than 7.0. The solution reacts with copper(oxide, forming a blue solution. Which two statements confirm the acidic nature of the solution?

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

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25

Ammonia gas is produced when solid ammonium chloride is heated with A calcium hydroxide. B calcium sulphate. C hydrochloric acid. D magnesium nitrate.

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

9. Metals  →  9.4. Reactivity series

6. Chemical reactions  →  6.3. Reversible reactions and equilibrium

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26

Sulphur and selenium (Se) are in the same group of the Periodic Table. From this, we would expect selenium to form compounds having the formulae A SeO, Na2Se and NaSeO4. B SeO2, Na2Se and NaSeO4. C SeO2, Na2Se and Na2SeO4. D SeO3, NaSe and NaSeO4.

8. The Periodic Table  →  8.1. Arrangement of elements

3. Stoichiometry  →  3.1. Formulae

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

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27

X and Y are diatomic elements. X is less reactive than Y. What are elements X and Y?

8. The Periodic Table  →  8.3. Group VII properties

8. The Periodic Table  →  8.1. Arrangement of elements

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28

A metal X, in Group I of the Periodic Table, would be expected to A form a nitrate of formula X(NO3)2. B form an acidic oxide. C form an insoluble chloride. D produce hydrogen from cold water.

8. The Periodic Table  →  8.1. Arrangement of elements

8. The Periodic Table  →  8.2. Group I properties

8. The Periodic Table  →  8.4. Transition elements

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29

Four test-tubes were set up as shown...

9. Metals  →  9.5. Corrosion of metals

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30

Three types of steel have different properties. steel 1 easily shaped steel 2 brittle steel 3 resistant to corrosion What are the names of these three types of steel?

9. Metals  →  9.3. Alloys and their properties

9. Metals  →  9.5. Corrosion of metals

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31

Aluminium is used to make saucepans because of its apparent lack of reactivity. Which property of aluminium explains its unreactivity?

9. Metals  →  9.4. Reactivity series

9. Metals  →  9.2. Uses of metals

9. Metals  →  9.1. Properties of metals

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32

The diagram shows the apparatus used in an experiment to reduce substance Q with the gas generated in the flask. dilute hydrochloric acid P heat Q What are substances P and Q?

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

9. Metals  →  9.4. Reactivity series

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33

The flow chart shows how impure water can be treated to produce drinkable water. impure water drinkable water pass through large-sized gravel pass through small-sized gravel pass through carbon pass chlorine through it What is not removed from the water by this process?

10. Chemistry of the environment  →  10.1. Water

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34

A solid substance Z burns in air to form a product that is gaseous at 20 °C. What is Z?

11. Organic chemistry  →  11.3. Fuels

11. Organic chemistry  →  11.6. Alcohols

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

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35

A section of a polymer is shown...

11. Organic chemistry  →  11.8. Polymers

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36

Carboxylic acids react with alcohols to form esters. Which acid and alcohol react together to form the following ester?

11. Organic chemistry  →  11.7. Carboxylic acids

11. Organic chemistry  →  11.2. Naming organic compounds

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37

Which two compounds are members of the same homologous series?

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

11. Organic chemistry  →  11.2. Naming organic compounds

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38

The diagram shows the structure of the compound 1,3-butadiene. H C H C C C H H H H How many molecules of hydrogen are needed to saturate one molecule of 1,3-butadiene?

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

3. Stoichiometry  →  3.1. Formulae

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39

Which compound has more than two carbon atoms per molecule?

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

11. Organic chemistry  →  11.3. Fuels

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40

Alkanes are a homologous series of organic compounds. Which statement about alkanes is correct?

11. Organic chemistry  →  11.4. Alkanes

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

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