1. Non-Metals Prepared December 2007 Alrick Moodie

2. What are non-metals ? Non-metals are those substances which are not metals i.e. they do not ionize by electron loss and do not show the characteristics of metals

3. Properties of Non-Metals Poor conductors of heat and electricity Brittle, not malleable and ductile Dull in colour Low in sonority

4. Chemical Properties React with air/oxygen to give covalent acidic oxides ( although a few give neutral oxides e.g. CO ) React with metals to form ionic compounds Do not react with dilute acids Do not react with water except chlorine Tend to be oxidizing agents

5. Common Non-metals We will be looking at : Hydrogen Chlorine Oxygen Carbon Sulphur Nitrogen

6. Hydrogen It is a diatomic gas H 2 It is colourless and odourless. It is almost insoluble in water and is the lightest known substance.

7. Chemical Properties of Hydrogen It has a neutral pH It burns in air/oxygen It combines with reactive metals to give hydrides : Mg + H 2  MgH 2 It can act as a reducing agents e.g. in the extraction of metals CuO + H 2  Cu + H 2 O

8. Uses of Hydrogen Manufacture of ammonia, nitric acid and nylon Manufacture of margarine and other hydrogenated oils In welding As fuel

9. Laboratory Preparation Hydrogen can be prepared by reacting an acid with a metal Zn + 2HCl  ZnCl 2 + H 2

10. Diagram of the Laboratory Preparation of Hydrogen

11. The Water Cycle

13. Water vapour in the atmosphere condenses and form water droplets and precipitation occurs. If temperature is low we will get snow or hail ( ice ). The water on the ground : percolates and go underground runs off into rivers and the seas evaporates

14. Plants absorb water and loses it through a process called transpiration Animals also intake water and lose through excretion ( sweat, urine or breathing )

15. Uses of water Domestic purposes e.g. drinking, washing, cooking, cleaning Irrigation of crops Generation of electricity Industrial processes Recreational activities

17. Chlorine

18. It is a diatomic gas Cl 2 It is a greenish-yellow gas with a choking odour. It is more dense than air and is slightly soluble in water.

19. Chemical Properties of Chlorine Readily combines with metals to form chlorides : Mg + Cl 2  MgCl 2 It is a powerful oxidizing agent It bleaches substances ( in the presence of moisture )

20. Uses of Chlorine Manufacture of plastics e.g. PVC Sterilize water e.g. drinking supplies, swimming pools Preparation of cleaning fluids and bleaching agents Manufacture of hydrochloric acid

21. Laboratory Preparation Chlorine can be the oxidation of conc. Hydrochloric acid by potassium manganate VII HCl (l) + KMnO 4 (s)  KCl (aq) + MnCl 2 (aq) + H 2 O (l) + Cl 2 (g)

23. Oxygen

24. Oxygen is the most abundant element on Earth. Approximately 50% of the earth’s crust is composed of oxygen containing compounds, while 20% of the atmosphere is free oxygen gas.

25. Oxygen is a diatomic gas O 2 although in the upper atmosphere it exists in the allotrope form as ozone O 3. It is a colourless odourless gas which is slightly soluble in water and has the same density as air.

26. Chemical Properties It has a neutral pH of 7 Supports combustion Combines with most elements to form oxides It is involved in biological processes of respiration.

27. Uses of Oxygen In welding apparatus Rocket fuels Steel manufacture Breathing equipment

28. Laboratory Preparation Oxygen is prepared by the catalytic decomposition of hydrogen peroxide. 2H 2 O 2 (aq)  2H 2 O (l) + O 2 (g) MnO 2 is the catalyst used

30. Carbon

31. Carbon exists as many natural occurring allotropes ; diamond, graphite, charcoal and coke.

33. Chemical Properties of Carbon Readily burns in oxygen to form carbon dioxide. In limited supply of air carbon monoxide is formed. It is a powerful reducing agent at high temperatures.

34. Carbon Dioxide Carbon dioxide is a colourless, odourless gas which is slightly soluble in water. It is more dense than air and is slightly acidic. The presence of carbon dioxide can be determined by the formation of a precipitate with calcium hydroxide.

35. Preparation Carbon dioxide is prepared by the reaction of a carbonate and a dilute acid.

37. Uses of Carbon dioxide As a refrigerant As a fire suppressant In sodas

38. Carbon cycle

39. Sulphur

40. Sulphur is found in the earth’s crust as a free element and as sulphides and sulphates. The free sulphur occurs as two allotropes, monoclinic and rhombic.

41. Chemical Properties Burns in air to form sulphur dioxide Combines with most metals to form sulphides.

42. Uses Manufacture of sulphuric acid Manufacture of gunpowder and matches Manufacture of fungicides and pesticides Vulcanization of rubber

43. Sulphur is obtained by the Frasch process where the sulphur is mined directly from the earth in its elemental form.

44. Sulphuric acid

45. Concentrated sulphuric acid is a colourless, odourless, oily liquid. It is a powerful dehydrating liquid. Diluting conc. sulphuric acid is a very exothermic reaction and must be done cautiously.

46. Uses Manufacture of fertilizers Manufacture of white paint Manufacture of soaps and detergents Refining of petroleum Vulcanization

47. Manufacture Sulphuric acid is manufactured by the Contact process which has three stages. 1.Sulphur is burned in air to form sulphur dioxide S (s) + O 2 (g)  SO 2 (g) 2.The sulphur dioxide is oxidized to sulphur trioxide 2SO 2 (g) + O 2 (g)  2SO 3 (g)

48. 3.The sulphur trioxide is dissolved in concentrated sulphuric acid to form oleum which is diluted to form sulphuric acid. H 2 SO 4 (aq) + SO 3 (g)  H 2 S 2 O 7 (l) H 2 S 2 O 7 (l) + H 2 O (l)  2H 2 SO 4 (aq)

50. Nitrogen

51. Nitrogen forms 78% of the air by volume. It is a colourless, odourless gas which is insoluble in water and has the same density as air.

52. Nitrogen is notoriously inert. However it will combine with oxygen at high temperatures to form nitrous oxides. This occurs during lightning discharges and in the engines of vehicles. It will also combine with hydrogen under certain conditions of temperature and pressure to form ammonia.

53. Uses & Manufacture As a refrigerant As an inert atmosphere in packaging Manufacture of ammonia Nitrogen is obtained by fractional distillation of air.

56. Ammonia Ammonia is a colourless gas with a pungent, choking smell. It is less dense than air and is very soluble in water. Chemical formula NH 3 Dissolved ammonia is called aqueous ammonia NH 3 (aq) or ammonium hydroxide NH 4 OH

57. Chemical properties Dissolves in water to give a weakly alkali solution. It is the only common alkali gas. Combines directly with acids to form ammonium salts Acts as a reducing agent

58. Laboratory Preparation Ammonia can be prepared by heating an ammonium salt with an alkali. 2NH 4 Cl (s) + Ca(OH) 2 (s)  2NH 3 (g) + CaCl 2 (aq) + 2H 2 O (l)

60. Industrial Preparation Ammonia is prepared by the Haber Process. Purified Nitrogen and Hydrogen gases are passed over a finely divided iron catalyst at 350 – 400 o C and a pressure of 250 to 300 atmospheres. N 2 (g) + 3H 2 (g)  2NH 3 (g)

63. Uses of Ammonia Water purification Cleaning agent Refrigerant Manufacture of fertilizers Manufacture of nitric acid Manufacture of nylon

64. GasColourOdourTest HydrogenNone Gives a pop with a lighted splint. No effect on litmus OxygenNone Relights a glowing splint. No effect on litmus Carbon dioxideNone Turns lime water cloudy then colourless AmmoniaNonePungentDense white fumes formed when in contact with hydrogen chloride. Turns moist red litmus blue. Sulphur dioxideNoneChokingReduces potassium dichromate and manganate VII Turns moist blue litmus red. Hydrogen chloride NoneIrritatingDense white fumes formed when in contact with ammonia. Turns moist blue litmus red. ChlorineYellow-greenIrritatingMoist blue litmus turns red and then bleached. Nitrogen dioxide BrownIrritatingMoist blue litmus turns red. Water vapourNone Cobalt chloride paper turns from blue to pink.