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1

The first four ionisation energies for element X are shown...

1. Atomic structure  →  1.4. Ionisation energy

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2

What is a basic assumption of the kinetic theory, as applied to an ideal gas?

4. States of matter  →  4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

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3

A sample of the hydrocarbon C6H12 is completely burned in dry oxygen and the product gases are collected as shown...

2. Atoms, molecules and stoichiometry  →  2.4. Reacting masses and volumes (of solutions and gases)

11. Group 17  →  11.4. The reactions of chlorine

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4

5.0 g samples of the carbonates of barium, copper, lithium and magnesium are decomposed to the metal oxides and carbon dioxide. For which compound is there the greatest loss in mass?

10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

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5

In this question you should assume methane behaves as an ideal gas. The gas laws can be summarised in the ideal gas equation below. pV = nRT The volume of a sample of methane is measured at a temperature of 60 °C and a pressure of 103 kPa. The volume measured is 5.37 × 10–3 m3. What is the mass of the sample of methane, given to two significant figures?

4. States of matter  →  4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

2. Atoms, molecules and stoichiometry  →  2.4. Reacting masses and volumes (of solutions and gases)

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6

A butane burner is used to heat water. The Mr of butane is 58. ● of butane is –2877 kJ mol–1. ● 250 g of water is heated from 12 °C to 100 °C. ● The burner transfers 47% of the heat released from the burning fuel to the water. Assume that the butane undergoes complete combustion and none of the water evaporates. What is the minimum mass of butane that must be burnt?

2. Atoms, molecules and stoichiometry  →  2.4. Reacting masses and volumes (of solutions and gases)

5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)

14. Hydrocarbons  →  14.1. Alkanes

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7

Nitric acid is known to take part in the oxidation of atmospheric sulfur dioxide. One possible reaction is shown...

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

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8

A transition metal ion, M2+, reacts with acidified dichromate(ions to form M4+ ions, Cr3+ ions, and H2O. Which equation correctly represents this reaction?

2. Atoms, molecules and stoichiometry  →  2.3. Formulas

11. Group 17  →  11.3. Some reactions of the halide ions

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9

In this question you should assume that all gases behave ideally. Hydrogen and iodine react reversibly in the following reaction. The system reaches dynamic equilibrium. H2+ I22HI∆H = –9.5 kJ mol–1 Which statement must be true for the Kp of this equilibrium to be constant?

7. Equilibria  →  7.1. Chemical equilibria: reversible reactions, dynamic equilibrium

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10

0.200 mol of sulfur dioxide and 0.200 mol of oxygen are placed in a 1.00 dm3 sealed container. The gases are allowed to react until equilibrium is reached. 2SO2 + O2 2SO3 At equilibrium there is 0.100 mol of SO3 in the container. What is the value of Kc?

7. Equilibria  →  7.1. Chemical equilibria: reversible reactions, dynamic equilibrium

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11

Two reactions are shown...

8. Reaction kinetics  →  8.3. Homogeneous and heterogeneous catalysts

18. Carboxylic acids and derivatives  →  18.2. Esters

15. Halogen compounds  →  15.1. Halogenoalkanes

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12

Sodium and sulfur are burned separately in oxygen. Each reaction has a distinctive coloured flame. Which row is correct?

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

11. Group 17  →  11.4. The reactions of chlorine

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13

X and Y are elements in Period 3 of the Periodic Table. ● The oxide of X is a solid at room temperature. This oxide has a giant structure. ● The chloride of X does not react with water. ● Argon is the only element in Period 3 with a lower melting point than Y. What could be the formula of a compound formed between elements X and Y?

9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3

4. States of matter  →  4.2. Bonding and structure

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14

Which row describes the structure and bonding of SiO2 and SiCl 4?

4. States of matter  →  4.2. Bonding and structure

3. Chemical bonding  →  3.4. Covalent bonding and coordinate (dative covalent) bonding

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15

A sample of anhydrous calcium nitrate is placed in a test-tube and heated in a roaring Bunsen flame until it decomposes. The description of the gas in the test-tube is then noted. A glowing splint is then put into the test-tube and any changes are noted. Which observations are correct?

4. States of matter  →  4.1. The gaseous state: ideal and real gases and \( pV = nRT \)

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

14. Hydrocarbons  →  14.1. Alkanes

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16

Which row correctly describes the properties of the halogens as Group 17 is descended from chlorine to iodine?

11. Group 17  →  11.1. Physical properties of the Group 17 elements

11. Group 17  →  11.2. The chemical properties of the halogen elements and the hydrogen halides

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17

Reaction 1: chlorine reacts with cold aqueous sodium hydroxide to form solution Z. Reaction 2: solution Z is heated and forms Cl O3 –and Cl –. Which equations represent reaction 1 and reaction 2?

11. Group 17  →  11.4. The reactions of chlorine

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

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18

Which statement explains the observation that magnesium hydroxide dissolves in aqueous ammonium chloride, but not in aqueous sodium chloride?

3. Chemical bonding  →  3.2. Ionic bonding

11. Group 17  →  11.3. Some reactions of the halide ions

10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

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19

Transition elements and their compounds are widely used as catalysts. What is the identity and what is the oxidation number of the element present in the catalyst used in the Contact process?

6. Electrochemistry  →  6.1. Redox processes: electron transfer and changes in oxidation number (oxidation state)

9. The Periodic Table: chemical periodicity  →  9.2. Periodicity of chemical properties of the elements in Period 3

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20

What is true of every nucleophile?

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21

X has the molecular formula C5H12O. X has a branched carbon skeleton and a secondary alcohol functional group. How many structural isomers fit this description of X?

13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds

13. An introduction to AS Level organic chemistry  →  13.4. Isomerism: structural isomerism and stereoisomerism

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22

A new jet fuel has been produced that is a mixture of different structural isomers of compound Q. Q Which skeletal formula represents a structural isomer of Q?

13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds

13. An introduction to AS Level organic chemistry  →  13.4. Isomerism: structural isomerism and stereoisomerism

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23

The conversion of propene to propan-2-ol can be carried out in two stages represented by the equations shown...

13. An introduction to AS Level organic chemistry  →  13.2. Characteristic organic reactions

14. Hydrocarbons  →  14.2. Alkenes

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24

An organic molecule W contains 3 carbon atoms. It requires 4.5 molecules of oxygen for complete combustion. What could W be?

13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds

14. Hydrocarbons  →  14.1. Alkanes

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25

Compound J, C15H23Br2Cl, is reacted with an excess of a hot concentrated solution of sodium hydroxide in ethanol. One of the products is X. X excess NaOH in ethanol compound J Cl Br Br What could be the skeletal formula of X?

15. Halogen compounds  →  15.1. Halogenoalkanes

13. An introduction to AS Level organic chemistry  →  13.1. Formulas, functional groups and the naming of organic compounds

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26

Sodium reacts with 1 mol of compound Y to produce 1 mol of H2. Which compound could Y be?

11. Group 17  →  11.4. The reactions of chlorine

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

19. Nitrogen compounds  →  19.2. Nitriles and hydroxynitriles

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27

Which compound shows optical isomerism and gives a positive test with alkaline aqueous iodine?

13. An introduction to AS Level organic chemistry  →  13.4. Isomerism: structural isomerism and stereoisomerism

16. Hydroxy compounds  →  16.1. Alcohols

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28

Ethanedioic acid, HO2CCO2H, is reduced using an excess of lithium aluminium hydride, LiAl H4. What is the organic product of the reaction?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

15. Halogen compounds  →  15.1. Halogenoalkanes

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29

The diester shown...

16. Hydroxy compounds  →  16.1. Alcohols

11. Group 17  →  11.4. The reactions of chlorine

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30

J is a branched-chain alcohol, C5H12O. J is heated under reflux with an excess of Cr2O7 2– / H+ until no further reaction occurs. An organic compound K is formed in good yield. The infra-red spectrum of K is shown...

16. Hydroxy compounds  →  16.1. Alcohols

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31

Which ions contain one or more unpaired electrons?

1. Atomic structure  →  1.3. Electrons, energy levels and atomic orbitals

2. Atoms, molecules and stoichiometry  →  2.3. Formulas

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32

Which molecules and ions have a bond angle of 120°?

3. Chemical bonding  →  3.5. Shapes of molecules

13. An introduction to AS Level organic chemistry  →  13.3. Shapes of organic molecules; σ and π bonds

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33

Which statements are correct for all exothermic reactions?

5. Chemical energetics  →  5.1. Enthalpy change, \(\Delta H\)

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34

The factors affecting the rate of reaction between aqueous sodium thiosulfate and hydrochloric acid can be investigated. The ionic equation for the reaction is shown...

8. Reaction kinetics  →  8.1. Rate of reaction

11. Group 17  →  11.4. The reactions of chlorine

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35

Which reaction routes can be used to make a pure sample of barium sulfate?

10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

18. Carboxylic acids and derivatives  →  18.2. Esters

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36

Which properties increase from magnesium to barium?

10. Group 2  →  10.1. Similarities and trends in the properties of the Group 2 metals, magnesium to barium, and their compounds

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37

2-methylpropene can react in more than one way with chlorine. One of the reactions follows the pathway shown...

13. An introduction to AS Level organic chemistry  →  13.2. Characteristic organic reactions

14. Hydrocarbons  →  14.1. Alkanes

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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38

The halogenoalkanes listed below all react with NaOH. Which reactions proceed mainly by an SN1 mechanism?

15. Halogen compounds  →  15.1. Halogenoalkanes

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39

3-oxobutanoic acid can be synthesised in a two-step process. X Y 3-oxobutanoic acid O O OH What could be the structure of X?

21. Organic synthesis  →  21.1. Organic synthesis

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

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40

Ethanal reacts with HCN in the presence of KCN. Which changes in bonding occur during this reaction?

14. Hydrocarbons  →  14.2. Alkenes

19. Nitrogen compounds  →  19.2. Nitriles and hydroxynitriles

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