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1

What are the shapes of the molecules of water and boron trifluoride?

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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2

The electronic configuration of the two outermost shells of an atom is 3s23p63d54s2. What is this atom?

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

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3

Drinking water may contain dissolved calcium hydrogencarbonate, Ca(HCO3)2. How many electrons are present in a hydrogencarbonate anion?

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

1. Atomic structure  →  1.1. Particles in the atom and atomic radius

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4

Which molecule contains a nitrogen atom with sp hybridised orbitals?

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

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

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5

Which mass of solid residue is obtained from the thermal decomposition of 4.10 g of anhydrous calcium nitrate?

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

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

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6

Sodium hydroxide neutralises acid. H+ + OH– → H2O In a 11 000 dm3 sample of an aqueous solution, the concentration of acid, [H+], is 1.26 × 10– 3 mol dm–3. Which mass of solid sodium hydroxide neutralises the acid?

7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases

11. Group 17  →  11.4. The reactions of chlorine

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7

The gas laws can be summarised in the ideal gas equation. pV = nRT 0.960 g of oxygen gas is contained in a vessel of volume 7.00 × 10–3 m3 at a temperature of 30 °C. Assume that the gas behaves as an ideal gas. What is the pressure in the vessel?

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

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8

Which equation represents the standard enthalpy change of formation of water?

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

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9

Hess’ Law and bond energy data can be used to calculate the enthalpy change of a reaction. Bromoethane, CH3CH2Br, can be made by reacting ethene with hydrogen bromide. CH2=CH2 + HBr → CH3CH2Br What is the enthalpy change for this reaction?

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

5. Chemical energetics  →  5.2. Hess’s law

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10

Which reaction is not a redox reaction?

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

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11

The reaction between sulfur dioxide and oxygen is reversible. 2SO2 + O2 2SO3 ∆H o = –196 kJ mol–1 Which conditions of pressure and temperature favour the reverse reaction?

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

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12

Which statement about the effect of a catalyst on a reversible reaction is correct?

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

8. Reaction kinetics  →  8.3. Homogeneous and heterogeneous catalysts

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13

Which oxide is insoluble in aqueous sodium hydroxide?

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

7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases

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14

X, Y and Z are three elements in the third period. ● X reacts with chlorine to give a liquid product. ● Y reacts with chlorine to give a solid product that dissolves in water to give a solution of pH 7. ● Z reacts with chlorine to give a solid product that dissolves in water to give a solution of pH 6. Which elements are good conductors of electricity?

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

9. The Periodic Table: chemical periodicity  →  9.1. Periodicity of physical properties of the elements in Period 3

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15

A solution contains both Mg2+and Sr2+at the same concentration. The solution is divided into two equal portions. Aqueous sodium hydroxide is added dropwise to one portion. Dilute sulfuric acid is added dropwise to the other portion. Which row is correct?

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

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

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16

The volatility of the Group 17 elements, chlorine, bromine and iodine, decreases down the group. What is responsible for this?

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

Bromine is extracted from sea-water. In the final stages of the process two redox reactions take place. Br2+ SO2+ 2H2O→ 2HBr+ H2SO42HBr+ Cl 2→ Br2+ 2HCl Which row is correct?

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

11. Group 17  →  11.4. The reactions of chlorine

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18

When burned, sulfur forms a gaseous product X which can be oxidised to produce a gas Y. Gas Y reacts with water to produce a product Z. Which row correctly shows the oxidation states of sulfur in X, Y and Z?

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

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

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19

One molecule of ammonia reacts with one molecule of ethyl methanoate, HCO2C2H5, to produce one molecule of methanamide, HCONH2, and only one other molecule, X. One molecule of methanamide decomposes on heating strongly to produce one molecule of ammonia and only one other molecule, Y. What could be the identities of X and Y?

15. Halogen compounds  →  15.1. Halogenoalkanes

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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20

Which types of stereoisomerism are shown...

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

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21

An organic ion containing a carbon atom with a negative charge is called a carbanion. An organic ion containing a carbon atom with a positive charge is called a carbocation. The reaction between aqueous sodium hydroxide and 1-bromobutane proceeds by an SN2 mechanism. What is the first step in the mechanism?

15. Halogen compounds  →  15.1. Halogenoalkanes

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

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22

Compound X can be converted into compound Y in a single step. O O OH X Y What could be the identity of X?

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

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23

Which compound reacts with 2,4-dinitrophenylhydrazine reagent but does not react with Tollens’ reagent?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

15. Halogen compounds  →  15.1. Halogenoalkanes

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24

Structural isomerism and stereoisomerism should be considered when answering this question. The molecular formula of compound X is C5H12O. Compound X: ● reacts with alkaline aqueous iodine ● can be dehydrated to form two alkenes only. What could be the identity of compound X?

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

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

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25

Which volume of hydrogen, measured under room conditions, is produced when 0.160 g of methanol reacts with an excess of sodium?

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

14. Hydrocarbons  →  14.1. Alkanes

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

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26

Compound X produces a carboxylic acid when heated under reflux with acidified potassium dichromate(. Compound X does not react with sodium metal. What could be the identity of compound X?

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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27

A reaction occurs when a sample of 1-chloropropane is heated under reflux with sodium hydroxide dissolved in ethanol. Which row is correct?

15. Halogen compounds  →  15.1. Halogenoalkanes

11. Group 17  →  11.4. The reactions of chlorine

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28

Ethanedioic acid has the formula HO2CCO2H. What is the formula of aluminium ethanedioate?

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

7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases

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29

Alcohols, aldehydes and nitriles can each be converted into carboxylic acids. Which descriptions of their conversions into carboxylic acids are correct?

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

19. Nitrogen compounds  →  19.2. Nitriles and hydroxynitriles

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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30

How many structural isomers with the molecular formula C4H10O give infra-red absorptions both at approximately 1200 cm–1 and at approximately 3400 cm–1?

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

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

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31

Compound Q contains 40% carbon by mass. What could Q be?

22. Analytical techniques  →  22.2. Mass spectrometry

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

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32

A container is partially filled with hot water, sealed and left to cool. Which statements are correct?

8. Reaction kinetics  →  8.2. Effect of temperature on reaction rates and the concept of activation energy

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

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33

Ammonia and chlorine react together in the gas phase. 8NH3 + 3Cl 2 → N2 + 6NH4Cl Which statements are correct?

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

11. Group 17  →  11.4. The reactions of chlorine

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

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34

In which reactions does NH3 behave as a Brønsted-Lowry acid?

7. Equilibria  →  7.2. Brønsted–Lowry theory of acids and bases

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35

Chlorine reacts with hot aqueous sodium hydroxide. Which oxidation states does chlorine show in the products of this reaction?

11. Group 17  →  11.4. The reactions of chlorine

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

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36

In which different forms does nitrogen exist in compounds?

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

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

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37

Polyand PVC are examples of addition polymers. Which statements are correct?

20. Polymerisation  →  20.1. Addition polymerisation

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38

Organic compound X gives a precipitate when warmed with aqueous silver nitrate. This precipitate dissolves when concentrated aqueous ammonia is added. What could X be?

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

15. Halogen compounds  →  15.1. Halogenoalkanes

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39

Propanal reacts with hydrogen cyanide to form 2-hydroxybutanenitrile. A suitable catalyst for this reaction is sodium cyanide. NaCN CH3CH2CHO + HCN CH3CH2CH(OH)CN Which statements about the reaction of propanal with hydrogen cyanide are correct?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

19. Nitrogen compounds  →  19.2. Nitriles and hydroxynitriles

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40

To avoid the issue of disclosure of answer-related information to candidates, all copyright acknowledgements are reproduced online in the Cambridge International Examinations Copyright Acknowledgements Booklet. This is produced for each series of examinations and is freely available to download at www.cie.org.uk after the live examination series. 40 The structure of lactic acid is shown...

18. Carboxylic acids and derivatives  →  18.2. Esters

16. Hydroxy compounds  →  16.1. Alcohols

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