Chemistry_QB

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 109 8. Which of the following ions are coloured? (1) Cu 2+ (aq) (2) Cr 2 O 7 2  (aq) (3) K + (aq) A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 9. The charge of sulphate ion is A. 1+ B. 2+ C. 1  D. 2  □ 10. Which of the following ions has 1  charge? A. Ammonium ion B. Hydrogencarbonate ion C. Sulphite ion D. Chromate ion □ 11. Which of the following ions does NOT have 1+ charge? A. Dichromate ion B. Hydrogen ion C. Silver ion D. Potassium ion □ 12. Which of the following formulae does NOT stand for an ion? A. H + B. NCl 3 C. NH 4 + D. OH  □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 112 23. The table below gives atomic numbers of four atoms. Atom Atomic number P 17 Q 18 R 19 S 20 Which of the following atoms can form an ion with a charge of 1+? A. P B. Q C. R D. S □ 24. The diagrams below show the electronic diagrams of four atoms. A. B. C. D. Which of the following atoms can form an ion with a charge of +1? A. P B. Q C. R D. S □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 115 32. An atom X forms a X − ion. X and X − have the same (1) chemical properties. (2) number of electrons. (3) number of neutrons. (4) number of protons. Which of the above is/are correct? A. (1) only B. (2) only C. (3) and (4) only D. (1), (3) and (4) only □ 33. Which of the following pairs has an UNEQUAL number of electrons? A. Ne, F − B. Li + , Be 2+ C. Cl − , Ar D. Na + , Cl − □ 34. Which of the following is the electron diagram (showing electrons in the outermost shell only) of sodium chloride? A. B. C. D. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 118 41. Which of the following statements about ionic bonds are correct? (1) They are formed by the transfer of one or more protons from one atom (or group of atoms) to another. (2) They are non-directional. (3) Ionic bonds are strong. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 42. Which of the following pairs of elements can react together to form an ionic compound? A. Bromine and nitrogen B. Bromine and sodium C. Nitrogen and argon D. Sodium and argon □ 43. Which of the following compounds is NOT an ionic compound? A. NH 4 Cl B. CaO C. NaOH D. SiO 2 □ 44. Which of the following pairs of elements is likely to form an ionic compound? A. Carbon and sulphur B. Calcium and iodine C. Copper and zinc D. Phosphorus and chlorine □ 45. Which of the following substances has a giant ionic structure? A. Calcium carbonate B. Calcium ion C. Carbon dioxide D. Calcium atom □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 121 56. Elements X and Y react to form an ionic compound with formula Y 3 X . If Y has the electronic arrangement of 2,8,8,1, which group does X belong to in the Periodic Table? A. Group III B. Group V C. Group VI D. Group VII □ 57. The formula for the oxide of caesium metal is Cs 2 O. Which of the following would most likely be the formula for caesium hydrogencarbonate? A. CsHCO 3 B. Cs 2 HCO 3 C. Cs(HCO 3 ) 2 D. HCO 3 Cs □ 58. An ionic compound has the formula X 2 Y 3 . The ions present in the compound are A. X 2+ ions and Y 3− ions. B. X 3+ ions and Y 2− ions. C. Y 3+ ions and X 2− ions. D. Y 2+ ions and X 3− ions. □ 59. Elements X and Y react to form an ionic compound with formula XY . If Y belongs to Group VI of the Periodic Table, to which group does X belong? A. I B. II C. III D. VI □ 60. Elements X and Y have atomic numbers 12 and 7 respectively. The formula for the compound formed between X and Y would be A. X 2 Y 5 . B. X 5 Y 2 . C. X 2 Y 3 . D. X 3 Y 2 . □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 131 5. Which of the following molecules has an atomicity of 2? A. Hydrogen chloride B. Oxygen C. Ozone D. Neon □ 6. Which of the following compounds consists of covalent bond only? A. NH 4 Cl B. CO 2 C. NaOH D. K 2 CO 3 □ 7. Which of the following compounds consists of double covalent bond? A. CS 2 B. H 2 O C. HCl D. N 2 □ 8. Number of pairs of shared electrons in a methane molecule (CH 4 ) is A. 1 B. 2 C. 4 D. 8 □ 9. Which of the following statements about an oxygen molecule is INCORRECT? A. An oxygen molecule consists of a double bond. B. An oxygen molecule consists of 2 oxygen atoms. C. An oxygen molecule is formed by electron transfer. D. An oxygen molecule is formed by sharing of electrons. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 134 Element X Element Y A. Group IV Group VII B. Group V Group VII C. Group I Group VI D. Group IV Group VI □ 15. Which of the following combinations can give a covalent compound? A. Group II element + Group VII element B. Group VI element + Group VII element C. Group I element + Group 0 element D. Group VI element + Group 0 element □ 16. Which of the following groups of elements combines to form covalent compounds only? A. Na, S, O B. N, H, C, O C. Ca, C D. H, Cl, O □ 17. Which of the following statements about covalent bond are correct? (1) It is formed by the sharing of electrons between the bonded atoms. (2) It is non-directional. (3) It is a type of electrostatic attraction. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 18. Which of the following molecules does NOT contain lone pair? A. N 2 B. CO 2 C. NH 3 D. CH 4 □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 135 19. Which of the following substances contains at least one triple covalent bond? A. NH 3 B. N 2 C. Al 2 O 3 D. O 2 □ 20. Which of the following substances would have the same number of electrons as a water molecule? A. Neon B. Fluorine C. Lithium oxide D. Sodium chloride □ 21. Which of the following would have the same number of electrons as a molecule of water? (1) A neon atom (Ne) (2) An oxide ion (O 2− ) (3) A sodium ion (Na + ) (4) A methane molecule (CH 4 ) A. (1) and (2) only B. (3) and (4) only C. (1), (2) and (3) only D. (1), (2), (3) and (4) □ 22. Which of the following molecules has the greatest number of lone pairs of electrons? A. HCl B. Cl 2 C. NH 3 D. H 2 O □ 23. Which of the following statements is true? A. Krypton (a noble gas) consists of Kr 2 molecules. B. A fluorine atom cannot exist by itself at room conditions. C. Sodium chloride consists of Cl + and Na − ions. D. Magnesium metal consists of Mg 2 molecules. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 136 24. Which of the following diagrams represents chlorine gas? (Different circles represent atoms of different elements.) A. B. C. D. □ 25. Which of the following pairs of elements can react together to form a covalent compound? A. Magnesium and nitrogen B. Magnesium and potassium C. Nitrogen and chlorine D. Chlorine and potassium □ 26. Which of the following formulae represents a molecule? A. NH 3 B. NaCl C. Cr 2 O 7 2  D. Mg □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 137 27. Which of the following formulae is unlikely to exist? A. CH 4 B. Cl 3 C. F 2 O D. NCl 3 □ 28. A compound, M x N y , is formed from elements M and N . M has an atomic number of 6 and N has an atomic number of 8. Which of the following combinations is correct? x y Nature of bonding A. 1 2 Ionic B. 1 2 Covalent C. 2 1 Ionic D. 2 1 Covalent □ 29. Element X and Y belong to Group V and VII respectively in the Periodic Table. Which of the following combinations about the compound they form is correct? Chemical formula Bonding type A. X 3 Y Ionic B. XY 3 Covalent C. X 3 Y Covalent D. XY 3 Ionic □ 30. The atomic numbers of elements X and Y are 15 and 17 respectively. They combine to form a compound Z . Which of the following statements about compound Z is/are correct? (1) Z has a giant covalent structure. (2) Z has a chemical formula of XY 3 . (3) Z cannot conduct electricity. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 138 31. What is the relative molecular mass of carbon dioxide? A. 28.0 B. 44.0 C. 60.0 D. 74.0 □ 32. What is the formula mass of calcium sulphate? A. 232.3 B. 136.2 C. 120.2 D. 88.2 □ 33. What is the formula mass of copper(II) nitrate-3-water, Cu(NO 3 ) 2 ∙ 3H 2 O? A. 241.5 B. 227.5 C. 209.5 D. 187.5 □ 34. HCl is an ionic compound. HCl consists of H + and Cl  ions. □ 35. When forming a covalent compound, each fluorine atom tends to gain 1 electron. Each fluorine atom has 7 outermost shell electrons and could attain an octet by gaining one more electron. □ 36. Oxygen gas consists of discrete molecules at room conditions. Each oxygen atom can gain 2 electrons to form an O 2− ion. □ 37. Covalent bonds bind atoms together in a molecule. Molecules are held together by intermolecular forces. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 144 Chemistry: Chapter 9 Structures and properties of substances Combined Science (Chemistry Part): Chapter 9 Structures and properties of substances 1. Chlorine exists as a gas at room temperature and pressure because A. chlorine is reactive. B. the intermolecular forces among chlorine molecules are weak. C. the intermolecular forces between chlorine atoms are weak. D. chlorine molecules are diatomic. □ 2. Which of the following statements about simple molecular substances are correct? (1) They have low melting points and boiling points. (2) Most of them are insoluble in water but soluble in non-aqueous solvents. (3) They must be gases at room temperature. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 3. Which of the following statements concerning the structure of solid carbon dioxide is/are correct? (1) It has a simple molecular structure. (2) Carbon and oxygen atoms within the molecules are held together by ionic bond. (3) Carbon dioxide molecules are held together by intermolecular forces. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 145 4. Consider the following information: Substances Attraction between the particles in the substance (1) Iodine Intermolecular forces (2) Silicon(IV) oxide Ionic bond (3) Calcium chloride Covalent bond Which of the above information is/are correct? A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 5. Which of the following statements about molecules is correct? A. It consists of atoms of the same kind. B. Atoms within the molecules are bonded by weak intermolecular forces. C. It is formed a positive and negative ions. D. It is the smallest part of an element or a compound which can exist on its own under ordinary conditions. □ 6. Which of the following substances do NOT have a molecular structure? (1) Silicon(IV) oxide (2) Hydrochloric acid (3) Polyethene A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 7. Which of the following pure substances CANNOT conduct electricity in the liquid state? A. Mercury B. Sodium chloride C. Bromine D. Lead(II) bromide

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 146 8. Which of the following substances is an electrolyte? A. Magnesium sulphate B. Copper C. Distilled water D. Sugar □ 9. Molten sodium chloride conducts electricity because A. it contains metallic sodium. B. it contains mobile ions. C. it contains free chlorine. D. it contains free electrons. □ 10. Which of the following involves a chemical change? A. Melting of wax. B. Electrolysis of molten lead(II) bromide. C. Conducting electricity by iron. D. Dissolving sodium bromide in water. □ 11. Which of the following substances can conduct electricity in molten state or in aqueous solution? A. Methylbenzene (a compound formed by C and H) B. Sulphur C. Pure ethanoic acid (a compound formed by C, H and O) D. Sodium chloride □ 12. Which of the following temperatures would be most probably the melting point of an ionic compound? A. 209 o C B. 32 o C C. 150 o C D. 1030 o C □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 147 13. Which of the following diagrams represents the structure of sodium chloride (only the cross section is shown) at room conditions? A. B. C. D. □ 14. Which of the following statements concerning the structure of sodium chloride are correct? (1) Sodium ions are smaller than chloride ions. (2) Each sodium ion is surrounded by four chloride ions. (3) Each chloride ion is surrounded by six sodium ions. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 15. Which of the following substances has a giant ionic structure? A. Common salt B. Steel C. Methane D. Diamond □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 148 16. Which of the following statements are correct? (1) Almost all ionic compounds are solids under room conditions. (2) Ionic compounds usually have high melting points and boiling points. (3) Sodium hydroxide has a giant ionic structure. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 17. Which of the following statements about ionic compounds are correct? (1) They are solids which conduct electricity. (2) They are usually soluble in water but insoluble in non-aqueous solvents. (3) They are malleable and ductile. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 18. Sodium and oxygen react to form sodium oxide. Which of the following statements about sodium oxide is correct? A. The chemical formula of sodium oxide is NaO 2 . B. It is a gas at room temperature. C. It is soluble in methylbenzene. D. It conducts electricity in molten state. □ 19. Which of the following is NOT an ionic substance? A. KMnO 4 B. KOH C. Li 2 O D. PCl 5 □ 20. Which of the following statements about potassium iodide is INCORRECT? A. Potassium iodide is a solid at room temperature. B. I atom and I − ion have different chemical properties. C. Potassium iodide is insoluble in methylbenzene. D. Potassium iodide becomes ionic when dissolved in water.

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 149 21. Elements X and Y react to form a compound with a chemical formula of XY 2 . This compound has a giant covalent structure If element X belongs to Group IV in the Periodic Table, element Y would belong to Group A. II. B. III. C. VI. D. VII. □ 22. Which of the following statements is correct for both solid carbon dioxide and silicon(IV) oxide? A. Both have simple molecular structures. B. Both have high melting point. C. Both are covalent compounds. D. Both are soluble in water. □ 23. Which of the following statements about graphite and diamond is correct? A. They have the same chemical properties as they are the same element. B. Diamond is hard as it has extremely strong intermolecular force. C. Graphite can conduct electricity, as it is not in a giant covalent structure. D. They have the same boiling and melting points. □ 24. The atomic numbers of elements X and Y are 6 and 8 respectively. The compound formed between X and Y (1) has a simple molecular structure. (2) is a gas at room temperature. (3) is a non-conductor of electricity. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 150 25. Nitrogen dioxide has a A. giant ionic structure. B. simple molecular structure. C. macromolecular structure. D. giant covalent structure. □ 26. Which of the following statements are INCORRECT? (1) Covalent substances are all gases, liquids or low-melting solids. (2) Covalent bonds are weak forces of attraction. (3) Molecules within a giant covalent structure are attracted by weak intermolecular forces. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 27. Which of the following statements about giant covalent structures are correct? (1) All of them have similar physical properties. (2) All of them are insoluble in any solvents. (3) All of them have high melting points and boiling points. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 28. Which of the following does NOT have a giant covalent structure? A. Gold B. Silicon(IV) oxide C. Diamond D. Graphite □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 151 29. Which of the following about substances having giant covalent structures are INCORRECT? (1) All of them are non-conductors of electricity. (2) All of them are extremely hard. (3) All of them are compounds of two or more elements. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 30. Which of the following substances could have a giant covalent structure? Substance State at room temperature Solubility in water A. Solid Soluble B. Solid Insoluble C. Gas Insoluble D. Liquid Insoluble □ 31. Which of the following properties about silicon(IV) oxide and nitrogen dioxide are correct? (1) Both of their constituent elements are joined together by covalent bonds. (2) Both of them are insoluble in methylbenzene. (3) Both of them do not conduct electricity under any conditions. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 32. Substance X melts at 3  C and boils at 44  C. X (1) is a solid at room temperature. (2) has weak intermolecular forces between molecules. (3) has a giant covalent structure. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 152 33. Which of the following statements about iodine is correct? A. At room temperature and pressure, iodine exists as a solid. B. Iodine has a giant covalent structure. C. Iodine molecules are held together by strong covalent bonds to form a solid. D. Weak intermolecular forces hold the two iodine atoms together to form an iodine molecule in the solid. □ 34. Which of the following combinations is INCORRECT? Substances Attraction between the particles in the substance A. Diamond Giant covalent bond B. Quartz Covalent bond C. Potassium chloride Ionic bond D. Carbon dioxide Intermolecular forces between its molecules □ 35. Which of the following pairs of elements react to give a compound having a giant covalent structure? A. Silicon and oxygen B. Calcium and silicon C. Magnesium and bromine D. Carbon and sulphur □ 36. Which of the following is NOT a covalent substance? A. NH 3 B. NH 4 Cl C. I 2 D. SiO 2 □ 37. Which of the following combinations indicates the correct type of constituent particles exists in that substance at room conditions? Substance Constituent particles A. Hydrogen Atoms B. Magnesium oxide Ions C. Silicon(IV) oxide Molecules D. Iron Ions

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 153 38. Which of the following explanations about the thermal conductivity of metal is correct? A. Heat energy makes metal atoms collide with each other and the collisions produce heat. B. Free electrons near the energy source gain energy. They run throughout the metal and transfer energy to all parts of the metal. C. The free electrons move faster when they have gained energy and hit other electrons more frequently. Then energy is transferred along the metal. D. The metal ions near the energy source gain energy. They move and carry heat energy throughout the metal. □ 39. Which of the following statements about metallic bond are correct? (1) The lower position of the metal in the Periodic Table, the weaker is the metallic bond. (2) The strength of metallic bond increases with increasing number of outermost shell electrons of the metal atoms. (3) Metal is ductile and malleable because metallic bond is a very weak attraction. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 40. Metals are good electrical conductors because A. the metal ions in the metal lattice are free to move to conduct electricity. B. the metal atoms in the metal lattice are free to move to conduct electricity. C. the outermost shell electrons of metal atoms are free to move to conduct electricity. D. all the electrons in the metal lattice are free to move to conduct electricity. □ 41. The number of delocalized electron(s) per atom in potassium metal is A. 1 B. 2 C. 4 D. 5 □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 154 42. Which of the following is correct for both iron and iron(III) oxide? A. They have giant metallic structure. B. They conduct electricity in liquid state. C. They are electrolytes. D. They are malleable. □ 43. Which of the following metals has the highest melting point? A. Sodium B. Magnesium C. Aluminium D. Potassium □ 44. When a metal conducts electricity, A. half of the electrons move towards the positive pole. B. all electrons move towards the positive pole. C. delocalized electrons move in the same direction. D. electrons move from the positive pole to the negative pole. □ 45. The melting point and boiling point of copper are 1083 o C and 2595 o C respectively. Which of the following diagrams best shows the structure of copper at 2000 o C? A. B. C.

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 155 D. □ 46. The table below lists the melting points and boiling points of five metals. Metal Melting point (  C) Boiling Point /(  C) Aluminium 660 2470 Copper 1083 2595 Iron 1535 3000 Lead 327 1744 Platinum 1769 4530 At 2500 o C, which of the following combinations about the states of metals is correct? Aluminium Copper Iron Lead Platinum A. Gas Liquid Liquid Gas Liquid B. Gas Gas Gas Liquid Liquid C. Liquid Gas Gas Liquid Gas D. Liquid Liquid Liquid Gas Gas □ 47. The table below shows properties of three substances. Substance Property X Conducts electricity only in aqueous state. Y Conducts electricity when molten and in aqueous solution. Z Conducts electricity when molten and in solid state. Which of the following combinations is correct? X Y Z A. H 2 SO 4 NaBr P B. NaBr P H 2 SO 4 C. H 2 SO 4 NaBr Pb D. NaBr Pb P □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 156 48. Substance Y has high melting and boiling point, and it can conduct electricity when molten or in aqueous solution and at the same time decomposed by electricity. Substance Y is likely to be A. silicon dioxide. B. graphite. C. gold. D. lead(II) bromide. □ 49. Potassium atoms in nature are joined to one another by A. covalent bonds. B. ionic bonds. C. metallic bonds. D. intermolecular forces. □ 50. Which of the following statements are correct? (1) Metallic bonds are non-directional. (2) A giant metallic structure consists of positive and negative ions bonded together. (3) Delocalized electrons can move freely within a giant metallic structure. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 51. Which of the following statements is correct? A. Metals are positively charged. B. Metallic bonds are weak. C. Metallic bonds in a metal are the same in all directions. D. Metal ions could move freely within a giant metallic structure. □ 52. When both ends of an iron nail are connected to a battery, its delocalized electrons (1) would move in the same direction. (2) would return to their electron shells. (3) would move towards the negative pole of the battery. A. (1) only

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 157 B. (2) only C. (1) and (3) only D. (2) and (3) only □ 53. Which of the following statements are INCORRECT? (1) Molten metal compounds conduct electricity because there are delocalized electrons. (2) There are chemical changes when metals conduct electricity. (3) If a metal piece is connected to a battery, the atoms in the metal would lose electrons. A (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 54. When a current passes through a piece of sodium, which of the following statements are INCORRECT? (1) Sodium atoms would lose electrons to form sodium compounds. (2) The sodium sample conducts electricity only if it is in molten state. (3) The sodium sample conducts electricity when its delocalized electrons collide with neighbouring electrons. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 55. Most metals have high melting points and boiling points because A. metals are good conductors of heat. B. most of them are solids at room temperatures. C. metallic bonds are usually strong and not easily broken. D. metallic bonds are non-directional. □ 56. Which of the following solids consists of discrete molecules? A. Carbon dioxide B. Diamond

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 158 C. Sodium chloride D. Iron □ 57. Which of the following statements are INCORRECT? (1) An ionic compound is formed between metal and non-metal ions. (2) Ionic bonds and covalent bonds are both strong and non-directional. (3) Ionic bonds and metallic bonds both are formed between different elements. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 58. Consider the information listed in the table below: Substance Melting point (°C) Solubility in water Electrical conductivity at room temperature W 1610 Insoluble Poor X 872 Soluble Good when in aqueous solution Y 45 Insoluble Poor Z 1769 Insoluble Good Which of the following substances would probably have a giant covalent structure at room temperature? A. W B. X C. Y D. Z □ 59. Which of the following substances has a giant ionic structure? Substance State at room temperature Does it conduct electricity? Solid state Molten state A. Solid No Yes B. Solid Yes Yes C. Solid Yes No D. Liquid No Yes □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 159 60. X, Y and Z are three elements and the properties of their chlorides are given below: Melting point(°C) Electrical conductivity in molten state Chloride of X 4 Poor Chloride of Y 873 Good Chloride of Z 677 Poor Which of the following statements are INCORRECT? (1) The chlorides of Y and Z have giant ionic structures. (2) The chloride of X is a solid at room temperature. (3) X is probably a metal. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 61. If Y has a very high melting point and conducts electricity only when molten or in aqueous solution, Y most probably has a A. giant covalent structure. B. simple molecular structure. C. giant ionic structure. D. giant metallic structure. □ 62. If X has a high melting point and is insoluble in water, X most probably has a A. giant covalent structure. B. simple molecular structure. C. giant ionic structure. D. giant metallic structure. □ 63. A substance X melts at 714°C. It does not conduct electricity in solid state, but conducts in molten state. X probably has A. a metallic structure. B. an ionic structure. C. a giant covalent structure. D. a simple molecular structure. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 160 64. The melting points of some chlorides are given below: Chloride Melting point(°C) Chloride Melting point(°C) NaCl 808°C MgCl 2 714°C SiCl 4 − 70°C PCl 3 − 92°C What can be deduced from the above data? (1) NaCl can conduct electricity at 800°C. (2) MgCl 2 is a liquid at 720°C. (3) SiCl 4 is a covalent compound with a simple molecular structure. (4) PCl 3 is a covalent compound with a giant covalent structure. A. (1) and (3) only B. (1) and (4) only C. (2) and (3) only D. (2), (3) and (4) only □ 65. The melting point and boiling point of substance X are 321°C and 765°C respectively. In its molten state, X conducts electricity without decomposition. X probably has A. an giant ionic structure. B. a giant metallic structure. C. a simple molecular structure. D. a covalent network structure. □ 66. The atomic numbers of two elements A and B are 11 and 16 respectively. The compound formed between A and B A. is a gas at room temperature. B. is a not an electrolyte. C. has a chemical formula of A 2 B . D. is insoluble in water. □ 67. Two elements X and Y have 4 and 7 outermost shell electrons respectively. Which of the following statements about the compound formed between X and Y is correct? A. It is an ionic compound. B. It has a very high melting point. C. It has a chemical formula of XY 4 . D. It can conduct electricity. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 161 68. Which of the following compounds has the lowest melting point? A. Carbon dioxide B. Quartz C. Sodium iodide D. Carbon tetrachloride □ 69. Which of the following sequences indicates the correct ascending order of melting points of the substances? A. HCl < NaCl < CCl 4 B. NaCl < CCl 4 < HCl C. HCl < CCl 4 < NaCl D. CCl 4 < HCl < NaCl □ 70. The electronic arrangement of atoms X and Y are 2,8,1 and 2,8,7 respectively. Which of the following statements about the compound formed between X and Y is INCORRECT? A. It has a giant structure. B. It has a high melting point. C. It is insoluble in water. D. It conducts electricity in molten state. □ 71. Which of the following substances dissolve in water? (1) Potassium chloride (2) Sugar (3) Quartz A. (1) and (2) only B. (2) and (3) only C. (1) and (3) only D. (1), (2) and (3) □ 72. Strontium (Sr) is just below calcium in the Periodic Table and it reacts with chlorine to form a compound. Which of the following statements about the chloride of strontium is INCORRECT? A. It has a giant structure. B. It has a high melting point.

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 162 C. It is a white solid. D. It is a good electrical conductor at room temperature. □ 73. The table below shows the melting points of two chlorides. Melting point (°C) Chloride of X – 50 Chloride of Y 1000 Which of the following statements about these two chlorides is correct? A. Both X and Y are metals. B. The chloride of X can conduct electricity in molten state. C. The chloride of X has a giant covalent structure. D. The chloride of Y can conduct electricity at 1000°C. □ 74. The atomic numbers of two elements X and Y are 19 and 16 respectively. The compound formed between X and Y A. has a formula X 2 Y . B. conducts electricity at room conditions. C. is a liquid at room conditions. D. is insoluble in water. □ 75. Substances which conduct electricity must A. have a regular packing of constituent particles. B. be ionic compounds. C. contain freely moving charged particles. D. be soluble in water. □ 76. Neon exists as a gas at room temperature and pressure. Neon molecules are monoatomic. □ 77. Iodine solid sublimes on heating. Iodine atoms within a molecule are joined together by strong covalent bond. □ 78. Ammonium chloride is not an electrolyte. Ammonium chloride is made up of non-metals only. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 163 79. Aluminium cannot conduct electricity. Aluminium is not an electrolyte. □ 80. Aqueous solutions of sodium compounds conduct electricity. Aqueous solutions of sodium compounds contain mobile ions. □ 81. Solid magnesium chloride conducts electricity. Magnesium chloride is an electrolyte. □ 82. All ionic compounds are soluble in water. All ionic compounds are electrolytes. □ 83. Solid ammonium nitrate conducts electricity. Ammonium nitrate is an electrolyte. □ 84. Silicon(IV) oxide has a high melting point. Silicon is a semi-metal. □ 85. The melting point of carbon dioxide is higher than that of silicon(IV) oxide. Carbon dioxide molecule has two strong C=O bond. □ 86. Both dry ice and quartz have a giant covalent structure. Carbon and silicon atoms have the same number of outermost shell electrons. □ 87. Iodine has a giant covalent structure. Iodine is a solid at room conditions. □ 88. Silicon(IV) oxide has a simple molecular structure. It is a compound formed between two non-metals. □

HKDSE Chemistry – A Modern View Part II Microscopic World I © Aristo Educational Press Ltd. 2009 164 89. Metals are good conductors of electricity. Metals conduct electricity by delocalized electrons. □ 90. Magnesium cannot be cut as easily as sodium. Metallic bond strength is greater in magnesium than sodium. □ 91. Metals could not be re-shaped. Metallic bonds are strong and could not be easily broken. □ 92. Iron is a good conductor of heat. There are mobile electrons in iron. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 262 Multiple Choice Questions Chemistry: Chapter 10 Occurrence and extraction of metals Combined Science (Chemistry Part): Chapter 10 Occurrence and extraction of metals 1. Which of the following properties is NOT true for copper? A. Malleable B. Excellent conductor of heat C. Magnetic D. Corrosion resistant □ 2. Which of the following is NOT a usual use of aluminium? A. Coins B. Overhead power cables C. Kitchen foil D. Windows frames □ 3. Which of the following properties of metals would NOT be considered for making soft drink cans? A. Toxicity B. Density C. Malleability D. Electrical conductivity □ 4. Which of the following combinations is correct? Metal Recycled from A. Iron Drink cans B. Copper Electrical wires C. Aluminium Jewellery D. Calcium Window frames □ 5. Which of the following is a common application of copper? A. Magnet B. Supersonic aircraft C. Soft drink cans D. Electrical wire □ 6. Which of the following is NOT a property of aluminium? A. Magnetic B. Corrosion resistant C. Good conductor of heat D. Good conductor of electricity □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 263 7. Which of the following substances is used to make thermometers? A. Silver B. Mercury C. Bromine D. Aluminium □ 8. Copper can conduct electricity because A. it is an electrolyte. B. it contains mobile Cu 2+ ions. C. its atoms are held together by ionic bonds. D. it has delocalized electrons. □ 9. Which of the following metals is most suitable for making steam boiler tubes? A. Magnesium B. Iron C. Platinum D. Copper □ 10. Which of the following metals occurs in free state in nature? A. Copper B. Zinc C. Gold D. Iron □ 11. Which of the following combinations is correct? Metal ore Metal can be extracted A. Bauxite Silver B. Haematite Iron C. Galena Gold D. Calcite Copper □ 12. Which of the following is the main composition of haematite? A. Iron(II) oxide B. Iron(III) oxide C. Iron D. Iron(II) sulphide □ 13. Gold can be found in free state in nature because of A. its high density. B. its closely packed structure. C. its stability. D. its attractive appearance. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 264 14. Which of the following compounds upon being heated can produce a gas that relights a glowing splint? A. Copper(II) oxide B. Mercury(II) oxide C. Calcium oxide D. Iron(III) oxide □ 15. Which of the following word equations about metal extraction is INCORRECT? A. lead(II) oxide + carbon  lead + carbon dioxide B. aluminium oxide + carbon  aluminium + carbon dioxide C. iron(III) oxide + carbon  iron + carbon dioxide D. copper(II) oxide + carbon  copper + carbon dioxide □ 16. Which of the following should be the most probable year of discovery of aluminium? A. 2027 B.C. B. 1027 B.C. C. 1027 A.D. D. 1827 A.D. □ 17. Three metals were discovered at different times. Metal Year of Discovery M 50 B.C. N 1800 A.D. O 1000 A.D. The ascending order of their reactivity is A. M , N , O B. M , O , N C. N , O , M D. N , M , O □ 18. Which of the following metals can be obtained by direct heating of its oxide? A. Sodium B. Magnesium C. Aluminium D. Silver □ 19. When copper(II) carbonate is heated in air with Bunsen flame, A. a white solid forms. B. a black solid forms. C. hydrogen gas evolved. D. a white fume forms. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 265 20. Aluminium is obtained by A. carbon reduction of aluminium oxide. B. heating aluminium oxide alone. C. passing hydrogen gas over aluminium ores. D. electrolysis of its molten ores. □ 21. X , Y , and Z are three metals. X can be extracted from its oxides by carbon reduction and Y can be extracted by direct heating of its oxide; while Z cannot be extracted by such methods. Which of the following statements must be true? A. Z is the least reactive one. B. Y is more reactive than X . C. Y should be discovered before Z . D. X is probably calcium. □ 22. For metals which are low in the reactivity series, their compounds can be reduced to metals easily because A. these compounds are not useful. B. these metals have few compounds. C. these compounds have lower stability. D. these compounds are easily reduced. □ 23. Which of the following statements about metal extraction is correct? A. Sodium oxide can be reduced to sodium by carbon. B. Coke is usually used for carbon reduction. C. Carbon dioxide can reduce zinc oxide to zinc. D. Even electrolysis cannot extract potassium from potassium oxide. □ 24. It is more difficult to reduce sodium oxide than copper(II) oxide because A. copper(II) oxide is heavier than sodium oxide. B. sodium oxide is more reactive than copper(II) oxide. C. sodium is more reactive than copper. D. copper is more reactive than sodium. □ 25. Which of the following statements about heating silver oxide strongly in air is correct? A. A gas evolved in the reaction can relight a glowing splint. B. A white solid forms. C. The solid product reacts with air readily to form silver oxide again. D. There is no observable change. □ 26. Which of the following methods used to extract sodium metal is correct? A. Electrolysis of aqueous sodium chloride solution. B. Heating sodium chloride under 1700°C with carbon monoxide. C. Electrolysis of molten sodium chloride. D. Heating sodium chloride directly.

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 266 27. Which of the following gases would be produced from the extraction of lead from lead(II) sulphide? (1) Carbon dioxide (2) Oxygen (3) Sulphur dioxide A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 28. Which of the following are possible ways to extract silver from its ore? (1) Direct heating (2) Electrolysis (3) Heating with carbon A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 29. Three metals are commonly extracted by the following ways. Metal Common extraction method X Electrolysis Y Direct heating Z Heating with carbon The descending order of their reactivity is A. X, Z, Y B. Y , Z , X C. X , Y , Z D. Z , Y , X □ 30. Which of the following statements are correct? (1) Iron could be extracted from iron(III) oxide by direct heating. (2) In the electrolysis of molten aluminium oxide, molten aluminium could be obtained at the negative electrode. (3) Zinc could be obtained from its ore by heating with carbon. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 31. Which of the following metal oxides can be reduced by heating alone? (1) Silver oxide (2) Mercury(II) oxide (3) Calcium oxide A. (1) only

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 267 B. (1) and (2) only C. (2) and (3) only D. (1), (2) and (3) □ 32. What is the method used to obtain aluminium from its ore? A. Heating the aluminium ore alone B. Heating the aluminium ore with carbon C. Heating the aluminium ore with hydrogen D. Electrolysis of molten aluminium ore □ 33. Which of the following oxides would be reduced to metals when heated on a charcoal block with a Bunsen flame in school laboratory? (1) Iron(III) oxide (2) Lead(II) oxide (3) Copper(II) oxide A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 34. Which of the following methods would be used to extract caesium, a Group I metal with an atomic number of 55, from its ore? A. Heating the ores with carbon. B. Electrolysis of its molten ore. C. Heating the ores with sodium at very high temperature. D. Heating the ores with carbon monoxide in the absence of oxygen. □ 35. Which of the following metal oxides could be reduced by copper? A. Iron(II) oxide B. Lead(II) oxide C. Magnesium oxide D. Mercury(II) oxide □ 36. An oxide of metal X could be reduced by zinc. Which of the following statements about X are probably INCORRECT? (1) X is more reactive than zinc. (2) X reacts with hot water to give hydrogen. (3) The reaction between X and dilute hydrochloric acid is explosive. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 37. Which of the following substances could reduce lead(II) oxide under strong heating? A. Hydrogen

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 268 B. Copper C. Mercury D. Carbon □ 38. Which of the following substances CANNOT reduce hot copper(II) oxide to copper? A. Iron B. Magnesium C. Carbon dioxide D. Carbon □ 39. Which of the following represents the ascending order of prices of the metals? A. Lead < Silver < Aluminium < Iron B. Iron < Lead < Aluminium < Silver C. Aluminium < Iron < Silver < Lead D. Silver < Aluminium < Lead < Iron □ 40. Which of the following metals is the most abundant i n the Earth’s crust? A. Iron B. Aluminium C. Steel D. Titanium □ 41. The high price of silver is probably due to (1) the high capital input for detecting the locations of ores. (2) the high cost and difficulty in extracting silver from its ores. (3) the low abundance of silver i n the Earth’s crust. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 42. The ease of metal extraction depends on A. the abundance of the metal in the Earth’s crust. B. the position of the metal in the reactivity series. C. how many types of ore the metal has. D. the number of uses of the metal. □ 43. Metals X and Y can be extracted by carbon reduction. X was found earlier and its oxide is black in colour. Which of the following combinations is correct? Metal X Metal Y A. Iron Copper B. Copper Zinc C. Copper Gold D. Aluminium Lead

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 269 44. Which of the following metals are obtained mainly from its oxide ores? (1) Calcium (2) Aluminium (3) Iron A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 45. Which of the following is the correct colour of collection bin for collecting waste aluminium cans? A. Brown B. Blue C. Red D. Yellow □ 46. Which of the following methods help(s) to reserve metals? (1) Recycling soft drink cans. (2) Replacing aluminium with steels in making window frames. (3) Reuse aluminium foil in the kitchen. A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 47. Which of the following are the consequences of metal recycling? (1) Fuels are saved. (2) Metals will run out at a later time in future. (3) Metals will be stronger to resist corrosion. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 48. Which of the following is NOT necessarily an advantage of metal recycling? A. Less pollution because fewer scrap metals is left for disposal. B. Saving other resources like water and fuels. C. Price sliding of metals as it ensures constant supply of metals. D. Extend the reserve of metals. □ 49. Which of the following materials is commonly used to replace copper for making water pipes? A. Iron B. Plastic C. Glass

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 270 D. Clay □ 50. Which of the following are possible ways to conserve metals? (1) Reusing metal articles (2) Recycling used metals (3) Replacing metals by other materials A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 51. Which of the following metals is more expensive than copper? A. Iron B. Lead C. Zinc D. Tin □ 52. Which of the following is NOT a possible way to conserve metals? A. Reusing metal articles B. Increase the quantity of mining C. Recycling used materials D. Replacing metals by other materials □ 53. What is the correct sequence for recycling of metal? A. Collecting  Sorting  Storing  Purifying B. Sorting  Collecting  Storing  Purifying C. Purifying  Collecting  Sorting  Storing D. Storing  Purifying  Collecting  Sorting □ 54. Iron(steel) is used to build Tsing Yi – Ma Wan Bridge. Iron(steel) is hard and strong. □ 55. Titanium is used to make water pipes. Titanium is very corrosion resistant. □ 56. Copper is used to make cooking pans. Copper is an excellent conductor of electricity. □ 57. Titanium is often used in making cooking utensils. Titanium has an excellent thermal conductivity. □ 58. Aluminium is mainly obtained from haematite. The composition of haematite is mainly aluminium oxide. □ 59. Mercury is obtained by heating mercury(II) oxide. Mercury is an unreactive metal.

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 271 60. Aluminium oxide is extracted by electrolysis. Aluminium oxide has a high melting point. □ 61. Gold was discovered in about 5000 B.C. Gold has a shiny golden yellow colour. □ 62. Aluminium is the cheapest metal on the Earth. Aluminium is the most abundant metal i n the Earth’s crust. □ 63. In the view of conservation of metals, aluminium should be recycled. Aluminium is light but strong. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 277 Chemistry: Chapter 11 Reactivity of metals Combined Science (Chemistry Part): Chapter 11 Reactivity of metals 1. Which of the following factors is/are used to compare reactivity of metals? (1) The rate of reaction (2) The lowest temperature at which the reaction finishes (3) The amount of heat energy given out during reaction A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 2. Which of the following chemical reactions is correct? A. Silver reacts with water to form silver hydroxide. B. Copper reacts with dilute sulphuric acid to give hydrogen gas. C. Iron reacts with oxygen to form iron(II) iron(III) oxide. D. Aluminium reacts with steam to form aluminium hydroxide. □ 3. Metal X reacts with water readily while metal Y and metal Z do not. Metal Y reacts with dilute hydrochloric acid but metal Z does not. Which of the following combinations is correct? Metal X Metal Y Metal Z A. Sodium Calcium Zinc B. Sodium Zinc Iron C. Magnesium Lead Iron D. Calcium Iron Copper □ 4. Which of the following is INCORRECT when some calcium granules are put into cold water? A. The metal sinks. B. An alkaline solution is formed. C. Some colourless gas bubbles are evolved. D. The metal burns with a brick-red flame. □ 5. When a metal with an atomic number of 20 reacts with water, which of the following products will be formed? (1) Metal hydroxide (2) Metal oxide (3) Hydrogen gas A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 278 6. Calcium sinks when placed in water because A. calcium is denser than water. B. the reaction between calcium and water is too vigorous that the water surface cannot withstand. C. the gas bubbles formed in the reaction push the metal down. D. attraction between water molecules and calcium atoms are greater than tension at water surface. □ 7. Which of the following combinations describing the reaction between sodium and water is correct? Resultant solution Gas evolved A. Acidic Oxygen B. Alkaline Oxygen C. Acidic Hydrogen D. Alkaline Hydrogen □ 8. Which of the following flame colours does NOT match correctly? Metal Flame colour A. Magnesium White B. Calcium Brick-red C. Potassium Lilac D. Sodium Blue □ 9. Which of the following colours does NOT match the corresponding metal oxide? Metal Oxide Colour (when cold) A. Magnesium oxide White B. Copper(II) oxide Blue C. Zinc oxide White D. Lead(II) oxide Yellow □ 10. Sodium and calcium can react with water. Which of the following observations is INCORRECT for both reactions? A. The metals move quickly on the water surface with a hissing sound. B. Colourless gas is produced during their reactions with water. C. The solutions become hot after the reactions. D. The resultant solutions are alkaline. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 279 11. Consider the following experimental set-up. Metal X is most probably A. Fe B. Cu C. Hg D. Ag □ 12. Which of the following metals gives a white solid oxide when heated in air? A. Aluminium B. Lead C. Iron D. Copper □ 13. Which of the following sets of state symbols is correct for the following reaction? Mg + H 2 O  MgO + H 2 A. (s), (l), (s), (g) B. (s), (g), (s), (g) C. (s), (l), (aq), (g) D. (s), (g), (aq), (g) □ 14. Which of the following equations represents the reaction between sodium and water? A. Na + H 2 O  NaO + H 2 B. 4Na + 2H 2 O  4NaH + O 2 C. 2Na + H 2 O  Na 2 O + H 2 D. 2Na + 2H 2 O  2NaOH + H 2 □ 15. Refer to the following three metals A , B and C . Property Metal A Metal B Metal C Heating in air No observable change Gives a lilac flame A white powder is produced Reaction with cold water No observable change Hydrogen gas is produced No observable change Reaction with dilute hydrochloric acid No observable change — Hydrogen gas is produced Which of the following is the correct order of decreasing reactivity of the metals? A. A > B > C B. C > A > B trough metal X heat wet sand hydrogen water delivery tube

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 280 C. B > A > C D. B > C > A □ 16. Refer to the following three metals A , B and C . Property Metal A Metal B Metal C Heating in air No observable change Gives a lilac flame A white powder is produced Reaction with cold water No observable change Hydrogen gas is produced No observable change Reaction with dilute hydrochloric acid No observable change — Hydrogen gas is produced A could be A. potassium. B. magnesium. C. copper. D. platinum. □ 17. Refer to the following three metals A , B and C . Property Metal A Metal B Metal C Heating in air No observable change Gives a lilac flame A white powder is produced Reaction with cold water No observable change Hydrogen gas is produced No observable change Reaction with dilute hydrochloric acid No observable change — Hydrogen gas is produced B could be A. aluminium. B. calcium. C. potassium. D. sodium. □ 18. Refer to the following three metals A , B and C . Property Metal A Metal B Metal C Heating in air No observable change Gives a lilac flame A white powder is produced Reaction with cold water No observable change Hydrogen gas is produced No observable change Reaction with dilute hydrochloric acid No observable change — Hydrogen gas is produced C could be A. calcium. B. potassium. C. magnesium. D. lead.

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 281 19. Which of the following chemical equations is correct? A. 2Al(s) + 3H 2 O(g)  Al 2 O 3 (s) + 3H 2 (g) B. 2Al(s) + 6H 2 O(g)  2Al(OH) 3 (s) + 3H 2 (g) C. Al(s) + H 2 O(g)  AlO(s) + H 2 (g) D. 3Al(s) + 2H 2 O(g)  Al 3 O 2 (s) + 2H 2 (g) □ 20. In school laboratory, hydrogen gas can be safely produced by adding dilute sulphuric acid to A. copper. B. lead. C. potassium. D. zinc. □ 21. Which of the following reactions does NOT give hydrogen? A. Adding calcium to cold water. B. Adding zinc to dilute hydrochloric acid. C. Passing steam over hot magnesium. D. Adding iron to cold water. □ 22. Which of the following metals will NOT form oxide(s) when heated strongly in air? (1) Copper (2) Platinum (3) Mercury A. (1) only B. (2) only C. (1) and (3) only D. (2) and (3) only □ 23. Which of the following statements are INCORRECT? (1) Gold burns in air with a golden yellow flame under strong heating. (2) Iron reacts with steam to give iron(III) oxide and hydrogen. (3) Calcium burns under strong heating to give oxygen. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 24. Which of the following metals react with steam under room conditions? (1) Calcium (2) Magnesium (3) Zinc A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 282 D. (1), (2) and (3) □ 25. Which of the following metals would NOT react with dilute sulphuric acid under room conditions? (1) Sodium (2) Copper (3) Silver A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 26. Which of the following statements concerning the reactions of zinc are INCORRECT? (1) Zinc reacts with hot water to give zinc oxide and hydrogen. (2) Zinc reacts with dilute sulphuric acid to give hydrogen. (3) Zinc burns in air to give oxygen under very strong heating. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 27. Which of the following metals do NOT burn on strong heating? (1) Lead (2) Silver (3) Platinum A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 28. Which of the following sets of state symbols is correct for the following reaction? potassium + water  potassium hydroxide + hydrogen A. (s), (aq), (aq), (g) B. (s), (l), (l), (g) C. (s), (l), (aq), (g) D. (s), (l), (aq), (aq) □ 29. Given three metals, X , Y and Z . The table below lists the results of their reactions with different substances. X Y Z Reaction with dilute hydrochloric acid explosive reaction slow reaction steady reaction Reaction with steam vigorous reaction ? no reaction

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 283 Reaction with cold water steady reaction no reaction no reaction Arrange the reactivity of X , Y , and Z in descending order. A. X , Z , Y B. Y , Z , X C. X , Y , Z D. Z , Y , X □ 30. Given three metals, X , Y and Z . The table below lists the results of their reactions with different substances. X Y Z Reaction with dilute hydrochloric acid explosive reaction slow reaction steady reaction Reaction with steam vigorous reaction ? no reaction Reaction with cold water steady reaction no reaction no reaction Which of the following is the probable result when Y reacts with steam? A. No reaction B. Slow reaction C. Steady reaction D. Explosive reaction □ 31. Arrange the following metals in descending order of reactivity: calcium, lead, copper, magnesium A. copper, lead, magnesium, calcium B. calcium, magnesium, lead, copper C. magnesium, calcium, lead, copper D copper, lead, calcium, magnesium □ 32. Which of the following statements about the reactivity series is correct? A. Density of metals decreases down the reactivity series. B. Metals in the reactivity series are in the same group of the Periodic Table. C. Reactivity of metals decreases down the series. D. The number of outermost shell electrons of metals decreases down the series. □ 33. Metals X and Y are extracted by electrolysis from their ores. Metal X reacts with cold water while metal Y does not. Metal Z is low in the reactivity series and forms a yellow oxide when cold. Which of the following combinations about metals X , Y and Z is correct? Metal X Metal Y Metal Z A. Sodium Aluminium Lead B. Potassium Calcium Zinc C. Calcium Zinc Iron D. Zinc Iron Copper

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 284 34. Both magnesium and carbon can reduce iron(III) oxide to iron, but carbon is used to extract iron instead of magnesium. Which of the following explanations are correct? (1) Carbon is much cheaper than magnesium. (2) Magnesium is more expensive than iron. (3) Carbon dioxide formed will escape and will not mix with iron. A. (1) and (2) only B. (1) and (3) only C. (2) and (3) only D. (1), (2) and (3) □ 35. Chromium reacts with lead(II) sulphate to give lead. It also reacts with dilute sulphuric acid but does not react with cold water. The position of chromium in the metal reactivity series is probably placed A. above magnesium. B. between magnesium and lead. C. between lead and mercury. D. below mercury. □ 36. Which of the following substances CANNOT reduce hot lead(II) oxide to lead? A. Carbon monoxide B. Magnesium C. Coke D. Copper □ 37. Which of the following statements about reactivity of metals is correct? A. The more reactive a metal is, the easier it loses electron(s) to form anions. B. The reactivity of metal decreases when moving down the group in the Periodic Table. C. The reactivity of metal increases rightward across a period in Periodic Table. D. The more reactive a metal is, the more stable compounds it forms. □ 38. Which of the following explanations about the fact that potassium is more reactive than sodium is correct? A. Potassium is heavier than sodium. B. Potassium atom is larger than sodium atom. C. The outermost shell electron of potassium is easier to be lose than that of sodium. D. Potassium has one more proton in the nucleus than that of sodium. □ 39. When copper forms copper(II) oxide, it A. gains electrons and is oxidized. B. gains electrons and is reduced. C. loses electrons and is oxidized. D. loses electrons and is reduced.

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 285 40. When a piece of magnesium is immersed into a beaker of copper(II) sulphate solution, which of the following will happen? A. Magnesium dissolves because copper(II) sulphate solution is corrosive. B. A black solid forms. C. The solution becomes paler in colour. D. Gas bubbles evolved. □ 41. Metal Y can displace the ions of metal Z from the aqueous solution of a compound of metal Z . It can be concluded that A. Metal Y is more reactive than metal Z . B. Metal Y is less reactive than metal Z . C. Metal Y is heavier than metal Z . D. Metal Y is more soluble than metal Z . □ 42. Which of the following reactions is expected to take place? A. Pb(s) + H 2 SO 4 (aq)  Pb(OH) 2 (aq) + SO 2 (g) B. Fe(s) + 2NaNO 3 (aq)  Fe(NO 3 ) 2 (aq) + 2Na(s) C. Cu(s) + H 2 O(l)  CuO(aq) + H 2 (g) D. 2Rb(s) + 2H 2 O(g)  2RbOH(aq) + H 2 (g) (given: Rb is an element in the same group with K and Na) □ 43. Consider the diagrams shown below. Which of the following combinations is correct? rod of metal Z Metal W displaced aqueous metal W salt solution rod of metal W Metal X displaced aqueous metal X salt solution rod of metal X Metal Y displaced aqueous metal Y salt solution

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 286 W X Y Z A. Lead Copper Zinc Iron B. Copper Zinc Iron Lead C. Zinc Iron Lead Copper D. Iron Lead Copper Zinc □ 44. A piece of zinc is placed in a silver nitrate solution. Which of the following about the colour change of the solution is correct? A. Blue colour disappears slowly. B. It turns to pale blue quickly. C. It turns to milky. D. There is no colour change. □ 45. Which of the following statements is INCORRECT? A. Magnesium reacts with dilute hydrochloric acid to release chlorine. B. Aluminium was discovered later than zinc. C. Iron does not displace magnesium because it is less reactive than magnesium. D. Lead(II) oxide is orange when hot and yellow when cold. □ 46. Metal A reacts with cold water to give hydrogen, but metals B and C do not. Metal B can displace the ions of metal C in aqueous solution. Which of the following gives the correct order of increasing reactivity of the three metals? A. B < C < A B. C < B < A C. C < A < B D. A < B < C □ 47. In which of the following test tubes will a reaction take place? A. iron(III) nitrate solution copper B. potassium nitrate solution zinc C. magnesium nitrate solution copper D. silver nitrate solution lead □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 287 48. Consider the results of displacement reactions of four metals, A , B , C and D . Metal Solution of nitrate of A B C D A — No Yes No B Yes — Yes Yes C No No — No D Yes No Yes — The decreasing order of reactivity of the metals is A. D > A > C > B . B. B > D > A > C . C. C > A > D > B . D. B > A > D > C . □ 49. X , Y and Z are metals. Carbon at red hot will remove oxygen from the oxides of X and Y , but not from that of Z . X displaces Y from a solution of the nitrate of Y . In which of the following are the metals arranged in the correct order of decreasing reactivity? A. Z , X , Y B. Z , Y , X C. X , Y , Z D. Y , X , Z □ 50. Which of the following ionic equations can be used to represent the reaction between calcium and zinc sulphate solution? A. Zn(s) + Ca 2+ (aq)  Zn 2+ (aq) + Ca(s) B. Ca(s) + Zn 2+ (aq)  Ca 2+ (aq) + Zn(s) C. Ca(s) + SO 4 2− (aq)  CaSO 4 (aq) D. Zn(s) + SO 4 2− (aq)  ZnSO 4 (aq) □ 51. Which of the following represents the ionic equation for the reaction between magnesium and silver nitrate solution? A. Mg(s) + 2Ag + (aq)  Mg 2+ (aq) + 2Ag(s) B. Mg(s) + Ag + (aq)  Mg + (aq) + Ag(s) C. 2Mg(s) + Ag 2+ (aq)  2Mg + (aq) + Ag(s) D. Mg(s) + Ag 2+ (aq)  Mg 2+ (aq) + Ag(s) □ 52. Which of the following equations represents a displacement reaction that is NOT possible at room conditions? A. Ca(s) + Mg 2+ (aq)  Ca 2+ (aq) + Mg(s) B. Mg(s) + Fe 2+ (aq)  Mg 2+ (aq) + Fe(s) C. Cu(s) + Zn 2+ (aq)  Cu 2+ (aq) + Zn(s) D. Pb(s) + 2Ag + (aq)  Pb 2+ (aq) + 2Ag(s) □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 288 53. A small amount of calcium oxide is heated in a test tube. The masses of the content and the test tube are recorded at several time intervals, and the data are sketched. Which of the following graphs best represents the data recorded? A. B. C. D. □ 54. Which of the following statements about the metal reactivity series is INCORRECT? A. Metals at the top of the series are the most reactive. B. Metals at a higher position in the series can displace ions of metals at a lower position from their aqueous solution. C. Metals at a position higher than copper in the series can react with dilute hydrochloric acid to give hydrogen. D. Metals at the top of the series are easier to extract from their ores. □ 55. Gold is golden yellow in colour. Gold is an unreactive metal. □ 56. Sodium burns with a golden yellow flame in air. Sodium is a very reactive metal. □ 57. Calcium is stored in paraffin oil. Calcium reacts with oxygen in air. □ 58. Magnesium can reduce copper(II) oxide on heating. Magnesium is more reactive than copper. □ 59. Copper can dissolve in silver nitrate solution. Copper displaces the silver metal from the silver nitrate solution. □ Mass of CaO Time Mass of CaO Time Mass of CaO Time Mass of CaO Time

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 289 60. A metal lower in the reactivity series can displace the metal higher in the series from its aqueous solution. A more reactive metal loses electrons more easily. □ 61. Silver will displace copper from copper(II) sulphate solution. Silver is an unreactive metal. □ 62. Silver oxide is decomposed on strong heating. Silver is an unreactive metal. □ 63. The lower the position of a metal in the reactivity series, the latest it was first discovered. The less reactive the metal, the more stable compounds it forms. □ 64. Silver was discovered much earlier than sodium. Silver is less reactive than sodium. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 295 Chemistry: Chapter 12 Reacting masses Combined Science (Chemistry Part): Chapter 12 Reacting masses 1. 1 mole of calcium chloride contains A. 1 mole of calcium chloride molecules. B. 6.02  10 23 calcium atoms and 2 × 6.02  10 23 chlorine atoms. C. 2 1  6.02  10 23 calcium ions and 6.02  10 23 chloride ions. D. 6.02  10 23 calcium ions and 2  6.02  10 23 chloride ions. □ 2. Which of the following is the unit for formula mass? A. Gram B. Mole C. No unit D. Mass unit □ 3. What is the molar mass of tetrachloromethane, CCl 4 ? A. 1.0 mol B. 1.0 g mol C. 154.0 mol D. 154.0 g mol □ 4. Which of the following substances contains the least number of ions? A. 0.7 mole of Na 2 O B. 0.9 mole of CaO C. 0.5 mole of Al 2 O 3 D. 0.8 mole of MgCl 2 □ 5. Which of the following statements is correct about 0.4 mole of aluminium oxide? A. There are 0.4 mole of Al 2+ ions and 0.4 mole of O 2 − ions. B. There are 0.8 mole of Al + ions and 0.4 mole of O 2 − ions. C. There are 0.8 mole of Al 3+ ions and 1.2 moles of O 2 − ions. D. There are 1.2 moles of Al 3+ ions and 0.8 mole of O 2 − ions. □ 6. A mixture of copper(II) sulphate and copper(II) bromide contains 0.3 mole of sulphate ions and 0.6 mole of bromide ions. How many moles of copper(II) ions are in the mixture? A. 0.6 mol B. 0.8 mol C. 0.9 mol D. 1.1 mol □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 296 7. Which of the following statements is correct? A. One mole of oxygen gas contains the same number of atoms as there are in one mole of neon gas at room conditions. B. One mole of magnesium contains the same number of atoms as there are in one mole of iodine at room conditions. C. One mole of chlorine gas and one mole of bromine gas have the same number of molecules and atoms. D. One mole of sodium has the same mass as there are in one mole of potassium. □ 8. What is the mass of 2.3 moles of aluminium oxide? A. 124.8 g B. 234.6 g C. 367.5 g D. 417.4 g □ 9. M is a metal in Group I. 0.5 mole of the metal sulphate weighs 71.05 g. Find the relative atomic mass of M . A. 19.0 B. 23.0 C. 27.0 D. 31.0 □ 10. Which of the following substances has the smallest mass? A. 0.8 mole of CaBr 2 B. 1 mole of C 4 H 10 C. 1.5 moles of Fe 2 O 3 D. 1.9 moles of K □ 11. How many shared electrons in 35.5 g of chlorine gas at room conditions? A. 1.51  10 23 B. 3.01  10 23 C. 6.02  10 23 D. 1.20  10 24 □ 12. How many moles of aluminium ions are present in 17.12 g of aluminium sulphate? A. 0.005 mol B. 0.01 mol C. 0.05 mol D. 0.1 mol □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 297 13. Calculate the mass of sulphur which contains the same number of atoms as 8.1 g of magnesium does? A. 5.3 g B. 10.7 g C. 16.0 g D. 21.4 g □ 14. Which of the following substances contains the same number of ions as 2.34 g of sodium chloride does? A. 2.984 g of potassium chloride B. 3.125 g of zinc chloride C. 3.598 g of calcium sulphate D. 5.529 g of magnesium bromide □ 15. If 2.4 g of oxygen contains x atoms at room conditions, then how many atoms are present in 12.0 g of helium? A. 5 x B. 10 x C. 20 x D. 30 x □ 16. If 1 mole of X O 3 contains the same number of atoms as 72 g of X H 4 , What is the relative atomic mass of X ? A. 72.0 B. 86.0 C. 90.0 D. 102.0 □ 17. If two moles of ozone, O 3 contain y atoms, how many atoms are present in one mole of oxygen gas? A. 3 2 y B. 3 y C. 2 y D. 6 y □ 18. Which of the following statements are about one mole of propane, C 3 H 8 , and one mole of propene, C 3 H 6 , is correct? A. They have equal masses. B. They have the same number of molecules. C. They have the same number of atoms. D. They have the same boiling point.

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 298 19. Which of the following statements is INCORRECT? A. One mole of carbon has a mass of 12.0 g. B. The mass of one mole of chlorine gas equals to the relative atomic mass of chlorine in grams. C. One mole of sodium chloride contains two moles of ions. D. 1 dm 3 of a 1.0 mol dm − 3 bromine liquid has one mole of bromine molecules. □ 20. What is the mass of two moles of chlorine molecules? A. 70.0 g B. 71.0 g C. 84.0 g D. 142.0 g □ 21. What is the number of moles of carbon atoms in 4.7 g of ethane, C 2 H 6 ? A. 0.182 mol B. 0.283 mol C. 0.278 mol D. 0.314 mol □ 22. What is the formula mass of iron(II) sulphate-7-water, FeSO 4 ∙ 7H 2 O? A. 151.9 B. 169.9 C. 229.9 D. 277.9 □ 23. What is the number of moles of 160.0 g sodium hydroxide? A. 0.25 mol B. 1 mol C. 4 mol D. 40 mol □ 24. How many moles of calcium ions are present in 200.2 g of calcium carbonate? A. 0.5 mol B. 1 mol C. 2 mol D. 4 mol □ 25. One mole of a substance A. has the same relative atomic mass as carbon-12. B. is the amount containing the Avogadro constant of formula units. C. contains 6.02 × 10 23 atoms. D. is the smallest amount of a substance which could exist on its own under room conditions. □

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 299 26. One mole of sodium oxide contains A. 1 mole of molecules. B. 2 moles of anions. C. 2 moles of cations. D. 4 moles of ions. □ 27. The formula mass of a compound A. is measured in grams. B. has a unit of g mol − 1 . C. is always a whole number. D. is the mass of one formula unit of the compound on the 12 C = 12.000 00 scale. □ 28. A mixture of magnesium chloride and magnesium sulphate contains 0.6 mole of chloride ions and 0.2 mole of sulphate ions. The number of moles of magnesium ions present is A. 0.4 mol. B. 0.5 mol. C. 0.8 mol. D. 1.0 mol. □ 29. Which of the following represents the mass of an oxygen molecule? A. 16.0 g B. 16.0 × 2 g C. 23 10 6.02 16.0  g D. 23 10 6.02 2 16.0   g □ 30. What is the percentage by mass of chlorine in 11.8 g of aluminium chloride? A. 20.2% B. 56.8% C. 72.4% D. 79.8% □ 31. What is the percentage by mass of C in C 6 H 12 O 6 ? A. 37.5% B. 40.0% C. 50.0% D. 67.5% □ 32. What is the mass of iron in 15 g of iron(II) sulphate-7-water, FeSO 4 ∙ 7H 2 O? A. 0.2 g B. 3.0 g C. 6.2 g D. 20.0 g

HKDSE Chemistry – A Modern View Part III Metals © Aristo Educational Press Ltd. 2009 300 33. The chloride of a metal X has the formula X Cl 3 and contains 65.6% by mass of chloride. Find the relative atomic mass of X . A. 12.2 B. 18.6 C. 34.4 D. 55.8 □ 34. Given that the relative atomic mass of X is 48.0. What is the percentage by mass of X in Ca X 2 O 7 ? A. 33.31% B. 38.69% C. 46.11% D. 47.98% □ 35. An element forms a compound X 2 Cl 3 which contains 25% by mass of chlorine. What is the relative atomic mass of the element X ? A. 39.9 B. 79.9 C. 106.5 D. 159.8 □ 36. An ore sample contained 60% Al 2 O 3 by mass. The other ingredients did not contain aluminium. Which of the following was the percentage by mass of aluminium in the sample? A. 24.0% B. 31.8% C. 52.9% D. 60.0% □ 37. An element X forms an oxide X 2 O which contains 11.2% of oxygen by mass. The relative atomic mass of X is A. 14.0. B. 23.0. C. 63.4. D. 108.0. □ 38. Which of the following is a molecular formula? A. Mg B. CH 4 C. NaCl D. NH 4 Cl □ 39. Which of the following is the structural formula of a molecule? A. K + Cl − B. O=C=O C. CH 2 O