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1

A pure hydrocarbon is used in bottled gas for cooking and heating. When 10 cm3 of the hydrocarbon is burned in 70 cm3 of oxygen (an excess), the final gaseous mixture contains 30 cm3 of carbon dioxide and 20 cm3 of unreacted oxygen. All gaseous volumes were measured under identical conditions. What is the formula of the hydrocarbon?

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

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

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

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2

On collision, airbags in cars inflate rapidly due to the production of nitrogen. The nitrogen is formed according to the following equations. 2NaN3 → 2Na + 3N2 10Na + 2KNO3 → K2O + 5Na2O + N2 How many moles of nitrogen gas are produced from 1 mol of sodium azide, NaN3?

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

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

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3

The first six ionisation energies of four elements, A to D, are given. Which element is most likely to be in Group IV of the Periodic Table?

1. Atomic structure  →  1.4. Ionisation energy

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4

In which species are the numbers of electrons and neutrons equal?

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

1. Atomic structure  →  1.2. Isotopes

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

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5

The diagram shows the variation of the boiling points of the hydrogen halides. b.p. HF HCl HBr HI What explains the higher boiling point of hydrogen fluoride?

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

3. Chemical bonding  →  3.6. Intermolecular forces, electronegativity and bond properties

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6

Three substances, R, S, T, have physical properties as shown...

4. States of matter  →  4.2. Bonding and structure

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

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7

Iodine trichloride, ICl3, is made by reacting iodine with chlorine. I2+ Cl2→ 2ICl; ∆H o = +14 kJ mol–1 ICl+ Cl2→ ICl3; ∆H o = –88 kJ mol–1 By using the data above, what is the enthalpy change of the formation for solid iodine trichloride?

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

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8

In the extraction of aluminium by electrolysis, why is it necessary to dissolve aluminium oxide in molten cryolite?

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

4. States of matter  →  4.2. Bonding and structure

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9

A cheap carbon monoxide detector for a gas heater consists of a patch containing palladium chloride crystals. When carbon monoxide is present, the crystals turn from orange to black as the following reaction takes place. CO+ PdCl2+ H2O→ CO2+ Pd+ 2HClorange black Which is the element whose oxidation number decreases in this reaction?

11. Group 17  →  11.4. The reactions of chlorine

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

2. Atoms, molecules and stoichiometry  →  2.3. Formulas

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10

The dissociation of dinitrogen tetraoxide into nitrogen dioxide is represented by the equation below. N2O42NO2; ∆H o = +57 kJ mol –1 If the temperature of an equilibrium mixture of the gases is increased at constant pressure, will the volume of the mixture increase or decrease and why?

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

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11

The reaction represented by the following equation was carried out. HCO2CH3+ NaOH→ HCO2Na+ CH3OHWhich graph best shows the relationship between [CH3OH] and t, the time from mixing of the reactants?

8. Reaction kinetics  →  8.1. Rate of reaction

11. Group 17  →  11.4. The reactions of chlorine

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12

The following species contain the same number of electrons. In which order do their radii increase?

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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13

Use of the Data Booklet is relevant to this question. Which element is likely to have an electronegativity similar to that of aluminium?

3. Chemical bonding  →  3.1. Electronegativity and bonding

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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14

Use of the Data Booklet is relevant to this question. Which is true for calcium or its compounds compared with the corresponding statements for magnesium?

1. Atomic structure  →  1.4. Ionisation energy

3. Chemical bonding  →  3.2. Ionic bonding

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15

Concentrated sulphuric acid is added to separate solid samples of sodium chloride, sodium bromide or sodium iodide. With which sampledoes sulphuric acid act as an oxidising agent?

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

11. Group 17  →  11.4. The reactions of chlorine

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16

Which graph correctly describes a trend found in the halogen group?

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

3. Chemical bonding  →  3.6. Intermolecular forces, electronegativity and bond properties

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17

Limestone, CaCO3, has been used as a building material for thousands of years, and was used on the Pyramids in Egypt. In the past hundred years many limestone buildings have begun to suffer damage. What is the cause of this damage?

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18

In an historically famous experiment Wöhler heated “inorganic” ammonium cyanate in the absence of air. The only product of the reaction was “organic” urea, CO(NH2)2. No other products were formed in the reaction. What is the formula of the cyanate ion present in ammonium cyanate?

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

2. Atoms, molecules and stoichiometry  →  2.3. Formulas

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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19

Bromomethane, CH3Br, is used as a fumigant to destroy insect pests in grain that is to be stored. It can be made by reacting methanol with hydrogen bromide. CH3OH + HBr → CH3Br + H2O What type of reaction is this?

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

15. Halogen compounds  →  15.1. Halogenoalkanes

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20

Prop-2-en-1-ol (allyl alcohol) has the following structure. H H H H C H C C OH Which reagent would react with prop-2-en-1-ol to form a product that could exist as optical isomers?

15. Halogen compounds  →  15.1. Halogenoalkanes

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

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21

Under the Montreal Protocol the use of chlorofluorocarbons is to be phased out. Fluorocarbons are often used to replace them. One chlorofluorocarbon which was widely used as a solvent is CCl2FCCl F2 and large stocks of it remain. One process to use up these stocks is to convert it into the fluorocarbon CH2FCF3 by the following route. CCl2FCCl F2 step 1 CCl3CF3 step 2 CH2FCF3 CCl2FCF3 step 3 What type of reaction is step 1?

21. Organic synthesis  →  21.1. Organic synthesis

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

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22

When bromine reacts with propene in an organic solvent at room temperature, what is the mechanism by which the bromine attacks the propene?

14. Hydrocarbons  →  14.2. Alkenes

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

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23

Dichlorodifluoromethane, CCl2F2, has been used in aerosol propellants and as a refrigerant. Which statement helps to explain why dichlorodifluoromethane is chemically inert?

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

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

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24

Under identical conditions, even though it proceeds by the same mechanism, reaction 1 is faster than reaction 2. reaction 1 CH3CHBrCH3 + NaCN → CH3CH(CN)CH3 + NaBr reaction 2 CH3CHBrCH3 + NaI → CH3CHICH3 + NaBr What factor will explain this result?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

15. Halogen compounds  →  15.1. Halogenoalkanes

8. Reaction kinetics  →  8.1. Rate of reaction

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25

Ethyl ethanoate is a very important solvent in industry. Currently, researchers are investigating ways of producing the ester from cheap, low grade ethanol by the following process. CH3CH2OH step 1 step 2 step 3 CH3CHO CH3CH2OCHCH3 CH3CH2OCOCH3 OH What types of reaction are steps 1 and 3?

18. Carboxylic acids and derivatives  →  18.2. Esters

16. Hydroxy compounds  →  16.1. Alcohols

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26

Malic acid occurs in apples. C OH CO2H CH2CO2H H malic acid Which substance will react with all three –OH groups present in the malic acid molecule?

18. Carboxylic acids and derivatives  →  18.1. Carboxylic acids

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

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27

Which compound reacts with its own oxidation product (an oxidation which involves no loss of carbon) to give a sweet-smelling liquid?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

14. Hydrocarbons  →  14.2. Alkenes

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28

Which reagent could be used to distinguish between CH3CH(OH)CH2CHO and CH3COCH2CH2OH ?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

16. Hydroxy compounds  →  16.1. Alcohols

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29

Ibuprofen is an anti-inflammatory drug. (CH3)2CHCH2 CH(CH3)CO2H ibuprofen What reaction would lead to its formation?

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

16. Hydroxy compounds  →  16.1. Alcohols

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30

In many countries plastic waste is collected separately and sorted. Some of this is incinerated to provide heat for power stations. Why is pvc, polyvinylchloride, removed from any waste that is to be incinerated?

20. Polymerisation  →  20.1. Addition polymerisation

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31

+ 31 Which of the following molecules and ions have a regular trigonal planar shape?

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

3. Chemical bonding  →  3.5. Shapes of molecules

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32

A quantity of solid Y was placed in a previously evacuated vessel and the apparatus was then held at a series of different temperatures. At each temperature, the mass of Y in the vapour state was calculated from pressure measurements. The results are shown...

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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33

Which of the enthalpy changes of the following reactions can only be obtained by application of Hess’ Law?

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

5. Chemical energetics  →  5.2. Hess’s law

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34

The stoichiometry of a catalysed 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

Use of the Data Booklet is relevant to this question. Which properties would be expected from radium, 88Ra, or its compounds?

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

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36

The number of moles of chlorine that react with 1 mol of X is twice the number of moles of chlorine that react with 1 mol of Y. Which of these pairs could be X and Y?

11. Group 17  →  11.4. The reactions of chlorine

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

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37

Which statements are true about the Haber process for the manufacture of ammonia?

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

12. Nitrogen and sulfur  →  12.1. Nitrogen and sulfur

14. Hydrocarbons  →  14.1. Alkanes

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38

Which compounds can be obtained from ethene in a single reaction?

14. Hydrocarbons  →  14.2. Alkenes

14. Hydrocarbons  →  14.1. Alkanes

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39

The steroid shown...

15. Halogen compounds  →  15.1. Halogenoalkanes

17. Carbonyl compounds  →  17.1. Aldehydes and ketones

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40

A sun protection cream contains the following ester as its active ingredient. CH3O CH CHCO2CH2CH CH2CH2 CH2CH2CH2CH3 What are the products of its partial or total hydrolysis by aqueous sodium hydroxide?

18. Carboxylic acids and derivatives  →  18.2. Esters

16. Hydroxy compounds  →  16.1. Alcohols

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