1. Properties of Metals

2. Compare the general physical properties of metals and non-metals, including:
3. (a) thermal conductivity
4. (b) electrical conductivity
5. (c) malleability and ductility
6. (d) melting points and boiling points
7. Describe the general chemical properties of metals, limited to their reactions with:
8. (a) dilute acids
9. (b) cold water and steam
10. (c) oxygen

11. Uses of Metals

12. Describe the uses of metals in terms of their physical properties, including:
13. (a) aluminium in the manufacture of aircraft because of its low density
14. (b) aluminium in the manufacture of overhead electrical cables because of its low density and good electrical conductivity
15. (c) aluminium in food containers because of its resistance to corrosion
16. (d) copper in electrical wiring because of its good electrical conductivity and ductility

17. Alloys and Their Properties

18. Describe an alloy as a mixture of a metal with other elements, including:
19. (a) brass as a mixture of copper and zinc
20. (b) stainless steel as a mixture of iron and other elements such as chromium, nickel, and carbon
21. State that alloys can be harder and stronger than the pure metals and are more useful
22. Explain in terms of structure how alloys can be harder and stronger than the pure metals because the different sized atoms in alloys mean the layers can no longer slide over each other
23. Describe the uses of alloys in terms of their physical properties, including stainless steel in cutlery because of its hardness and resistance to rusting
24. Identify representations of alloys from diagrams of structure

25. Reactivity Series

26. State the order of the reactivity series as: potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold
27. Describe the relative reactivities of metals in terms of their tendency to form positive ions, by displacement reactions, if any, with the aqueous ions of magnesium, zinc, iron, copper, and silver
28. Describe the reactions, if any, of:
29. (a) potassium, sodium, and calcium with cold water
30. (b) magnesium with steam
31. (c) magnesium, zinc, iron, copper, silver, and gold with dilute hydrochloric acid
32. and explain these reactions in terms of the position of the metals in the reactivity series
33. Explain the apparent unreactivity of aluminium in terms of its oxide layer
34. Deduce an order of reactivity from a given set of experimental results

35. Extraction of Metals

36. Describe the ease in obtaining metals from their ores, related to the position of the metal in the reactivity series
37. Describe the extraction of iron from hematite in the blast furnace, limited to:
38. (a) the burning of carbon (coke) to provide heat and produce carbon dioxide
39. (b) the reduction of carbon dioxide to carbon monoxide
40. (c) the reduction of iron(III) oxide by carbon monoxide
41. (d) the thermal decomposition of calcium carbonate / limestone to produce calcium oxide
42. (e) the formation of slag
43. State the symbol equations for the extraction of iron from hematite:
44. (a) C + O2 → CO2
45. (b) C + CO2 → 2CO
46. (c) Fe2O3 + 3CO → 2Fe + 3CO2
47. (d) CaCO3 → CaO + CO2
48. (e) CaO + SiO2 → CaSiO3
49. State that the main ore of aluminium is bauxite and that aluminium is extracted by electrolysis
50. Describe the extraction of aluminium from purified bauxite / aluminium oxide, including:
51. (a) the role of cryolite
52. (b) why the carbon anodes need to be regularly replaced
53. (c) the reactions at the electrodes, including ionic half-equations
54. Details of the purification of bauxite are not required