Suggested answers to in-text activities and unit-end exercises Topic 3 Unit 11

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1 Suggested answers to in-text activities and unit-end exercises In-text activities Checkpoint (page 37) 1 a) iron + dilute hydrochloric acid iron(ii) chloride + hydrogen b) zinc + dilute sulphuric acid zinc sulphate + hydrogen 2 a) calcium + water calcium hydroxide + hydrogen b) 3 a) No reaction. b) Magnesium burns to give magnesium oxide. c) No reaction. Discussion (page 40) Mg(s) + H 2 O(g) MgO(s) + H 2 (g) N 2 (g) + 3H 2 (g) 2NH 3 (g) The reactant(s) involved Magnesium and water (steam) Nitrogen and hydrogen The product(s) formed Magnesium oxide and hydrogen Ammonia The states of substances involved Magnesium and magnesium oxide are solids. Steam and hydrogen are All the substances are gases. The number of particles of each type of substance involved Does the reaction go one way only? gases. 1 magnesium atom reacts with 1 water molecule to give 1 formula unit of magnesium oxide and 1 hydrogen molecule. Yes. 1 nitrogen molecule reacts with 3 hydrogen molecules to give 2 ammonia molecules. No, the reaction is reversible. Checkpoint (page 43) 1 a) CaCO 3 (s) CaO(s) + CO 2 (g) b) 2PbO(s) + C(s) 2Pb(s) + CO 2 (g) 2 a) 4Fe(s) + 3O 2 (g) 2Fe 2 O 3 (s) b) Mg(s) + H 2 O(g) MgO(s) + H 2 (g) c) Zn(s) + 2HCl(aq) ZnCl 2 (aq) + H 2 (g) Suggested answers to in-text activities and unit-end exercises 1 Jing Kung. All rights reserved.

2 d) 2ZnO(s) + C(s) 2Zn(s) + CO 2 (g) e) HgS(s) + O 2 (g) Hg(l) + SO 2 (g) 3 a) CO 2 (g) + CaCO 3 (s) + H 2 O(l) Ca(HCO 3 ) 2 (aq) b) Fe 2 O 3 (s) + 3CO(g) 2Fe(s) + 3CO 2 (g) Problem Solving (page 47) Study the reactions of each metal with solutions of compounds of other metals. The more reactive the metal is, the more solutions the metal can react with. Checkpoint (page 49) 1 a) Ca(s) + 2H + (aq) Ca 2+ (aq) + H 2 (g) b) Mg(s) + 2Ag + (aq) Mg 2+ (aq) + 2Ag(s) 2 a) The nail becomes coated with a brown layer of copper. The solution turns pale green. b) Fe(s) + CuSO 4 (aq) FeSO 4 (aq) + Cu(s) c) Fe(s) + Cu 2+ (aq) Fe 2+ (aq) + Cu(s) 3 a) i) A reaction takes place. ii) Zn(s) + Pb(NO 3 ) 2 (aq) Zn(NO 3 ) 2 (aq) + Pb(s) Zn(s) + Pb 2+ (aq) Zn 2+ (aq) + Pb(s) b) i) A reaction takes place. ii) Mg(s) + Fe(NO 3 ) 2 (aq) Mg(NO 3 ) 2 (aq) + Fe(s) Mg(s) + Fe 2+ (aq) Mg 2+ (aq) + Fe(s) Checkpoint (page 56) 1 a) True. Barium is more reactive than sodium. Sodium reacts with cold water vigorously. Hence barium can react with cold water. b) False. Iron displaces copper from copper(ii) sulphate solution. Hence copper(ii) sulphate solution cannot be stored in an iron container. Suggested answers to in-text activities and unit-end exercises 2 Jing Kung. All rights reserved.

3 2 a) Magnesium b) i) Gas bubbles are given off. ii) Mg(s) + 2HCl(aq) MgCl 2 (aq) + H 2 (g) iii) Mg(s) + 2H + (aq) Mg 2+ (aq) + H 2 (g) c) d) Reactivity: Y < Z < X Y is the least reactive as it can be extracted from its oxide by heating alone but the other two metals cannot. X is more reactive than Z as it reacts with dilute hydrochloric acid but Z does not. Unit-end exercises (pages 62-69) Answers for the HKCEE and HKALE questions are not provided. Suggested answers to in-text activities and unit-end exercises 3 Jing Kung. All rights reserved.

4 1 2 a) Platinum b) Sodium c) Sodium, calcium d) Magnesium / zinc / iron e) Hydrogen f) Dilute hydrochloric acid or sulphuric acid 3 a) 2Pb(s) + O 2 (g) 2PbO(s) b) 2K(s) + 2H 2 O(l) 2KOH(aq) + H 2 (g) c) Mg(s) + H 2 O(g) MgO(s) + H 2 (g) d) Fe(s) + H 2 SO 4 (aq) FeSO 4 (aq) + H 2 (g) e) Cu(s) + 2AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2Ag(s) f) 2ZnS(s) + 3O 2 (g) 2ZnO(s) + 2SO 2 (g) 4 a) Mg(s) + 2H + (aq) Mg 2+ (aq) + H 2 (g) b) 2Al(s) + 6H + (aq) 2Al 3+ (aq) + 3H 2 (g) c) Zn(s) + Fe 2+ (aq) Zn 2+ (aq) + Fe(s) d) Fe(s) + 2Ag + (aq) Fe 2+ (aq) + 2Ag(s) 5 a) Metal Ore Main metallic Extraction method Suggested answers to in-text activities and unit-end exercises 4 Jing Kung. All rights reserved.

5 compound in the ore Copper copper pyrite copper(ii) iron(ii) sulphide heating the ore in air Zinc zinc blende zinc sulphide roasting the ore in air to obtain the oxide, then heating the oxide with carbon Magnesium magnesite magnesium carbonate electrolysis of molten ore b) Metals at the top of the reactivity series are extracted by electrolysis. Metals in the middle are extracted by reduction of their oxides with carbon. Metals near to the bottom are extracted from their ores by heating in air. 6 C Element X is calcium. Option A X is in Period 4 of the periodic table. Option B X sinks in water. 7 C Copper, lead and platinum do not react with steam. 8 A 9 D 10 A 11 B 12 D (1) sodium + water sodium hydroxide + hydrogen (2) calcium + dilute hydrochloric acid calcium chloride + hydrogen (3) iron + steam iron(ii,iii) oxide + hydrogen 13 D 14 D (1) Both the oxides of iron and lead can be reduced by carbon. Nickel is in between iron and lead in the reactivity series. Hence nickel(ii) oxide can be reduced by carbon as well. 15 A As the reactivity of Group I elements increases down the group, thus rubidium is more reactive than potassium. (3) Potassium cannot be extracted from its oxide by reduction with carbon. Hence rubidium Suggested answers to in-text activities and unit-end exercises 5 Jing Kung. All rights reserved.

6 cannot be extracted from its oxide by reduction with carbon as well. 16 a) i) Iron dissolved. Gas bubbles were given off. Fe(s) + 2HCl(aq) FeCl 2 (aq) + H 2 (g) ii) A golden yellow flame was observed. A white smoke was formed. 4Na(s) + O 2 (g) 2Na 2 O(s) iii) The yellow solid turned orange. A solid with metallic lustre was formed. 2PbO(s) + C(s) 2Pb(s) + CO 2 (g) iv) Zinc dissolved. A brown solid deposited. The blue colour of the solution faded gradually. Zn(s) + CuSO 4 (aq) Cu(s) + ZnSO 4 (aq) v) A brown solid with metallic lustre was formed. CuO(s) + Mg(s) Cu(s) + MgO(s) b) i) Calcium oxide is very stable. It cannot be reduced by carbon. ii) Copper is less reactive than magnesium. It cannot displace magnesium from magnesium nitrate solution a) Group II b) i) X burned with a very bright light. ii) 2Mg(s) + O 2 (g) 2MgO(s) c) i) X dissolved. / Gas bubbles were given off. ii) Mg(s) + H 2 SO 4 (aq) MgSO 4 (aq) + H 2 (g) d) i) Y burned with a lilac flame. ii) 4K(s) + O 2 (g) 2K 2 O(s) e) i) Z might be iron. ii) Fe(s) + H 2 SO 4 (aq) FeSO 4 (aq) + H 2 (g) a) i) Caesium hydroxide ii) 2Cs(s) + 2H 2 O(l) 2CsOH(aq) + H 2 (g) iii) Difference Caesium reacts more vigorously. Similiarity Similar products (hydroxide + hydrogen) are formed. Suggested answers to in-text activities and unit-end exercises 6 Jing Kung. All rights reserved.

7 b) Caesium is a soft metal. Caesium has a low melting point The method of extraction of a metal depends on how reactive the metal is. Metals in the middle of the reactivity series such as zinc, iron and lead can be extracted by removing oxygen from their oxides using carbon. Take iron as an example. The common ore of iron is haematite. It consists mainly of iron(iii) oxide. In industry, the ore of iron is converted to iron in a blast furnace. During the extraction, a mixture of iron ore, coke and limestone is added at the top of the furnace. At the same time, hot air is blown into the bottom of the furnace. A chain of chemical reactions then occurs. Carbon monoxide is produced in the process. The carbon monoxide reacts with iron(iii) oxide in the ore, producing iron. Fe 2 O 3 (s) + 3CO(g) 2Fe(l) + 3CO 2 (g) Reactive metals such as potassium, sodium, magnesium and aluminium cannot be extracted with carbon. These metals are extracted by electrolysis of their molten ores. Take aluminium as an example. The common ore of aluminium is bauxite. It consists of aluminium oxide mainly. The electrolysis is carried out in a large steel tank. The electrodes are made of graphite. During the process, aluminium forms at the negative electrode while oxygen gas bubbles off from the positive electrodes. Suggested answers to in-text activities and unit-end exercises 7 Jing Kung. All rights reserved.

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