1. Metal and Non-metal Oxides

2. An oxide is a compound of oxygen and one or more other elements.

3. Examples of oxides are carbon dioxide, CO 2,

4. An oxide is a compound of oxygen and one or more other elements. Examples of oxides are carbon dioxide, CO 2, sulfur trioxide, SO 3,

5. An oxide is a compound of oxygen and one or more other elements. Examples of oxides are carbon dioxide, CO 2, sulfur trioxide, SO 3, and sodium oxide, Na 2 O.

6. In Science 10, you are given this Periodic Table: METALSNON-METALS

7. An oxide formed by a metal and oxygen is called a metal oxide.

8. Some examples are:

9. An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O

10. An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O MgO

11. An oxide formed by a metal and oxygen is called a metal oxide. Some examples are: Li 2 O MgO CaO

12. An oxide formed by a non-metal and oxygen is called a non-metal oxide.

13. Some examples are:

14. An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2

15. An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2 NO 2

16. An oxide formed by a non-metal and oxygen is called a non-metal oxide. Some examples are: CO 2 NO 2 Cl 2 O

17. Metal oxides, and non-metal oxides have quite different properties.

18. One very important difference is what they produce when they are dissolved in water.

19. Metal oxides dissolve in water to form BASIC solutions.

20. Non-metal oxides dissolve in water to form ACIDIC solutions.

21. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l) 

22. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq)

23. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq) sodium hydroxide

24. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Na 2 O (s) + H 2 O (l)  2NaOH (aq) sodium hydroxide (a base)

25. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l) 

26. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

27. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

28. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq)

29. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq) magnesium hydroxide

30. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. MgO (s) + H 2 O (l)  Mg(OH) 2(aq) magnesium hydroxide (a base)

31. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l) 

32. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq)

33. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid

34. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l) 

35. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l)  H 2 SO 3(aq)

36. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Sulfurous acid

37. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l) 

38. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l)  H 2 SO 4(aq)

39. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. SO 3(g) + H 2 O (l)  H 2 SO 4(aq) Sulfuric acid

40. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l) 

41. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq)

42. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) Nitrous acid

43. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq)

44. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid

45. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid Nitrous Acid

46. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2

47. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq)

48. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq) Hypochlorous Acid

49. Metal oxides dissolve in water to form BASIC solutions. Non-metal oxides dissolve in water to form ACIDIC solutions. Cl 2 O (g) + H 2 O (l)  2HOCl (aq)

50. Non-metal oxides dissolve in water to form ACIDIC solutions.

52. Acid Precipitation Non-metal oxides dissolve in water to form ACIDIC solutions.

53. CO 2(g) Naturally occurs in Earth’s atmosphere

54. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq)

55. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid

56. Non-metal oxides dissolve in water to form ACIDIC solutions. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Carbonic acid A weak acid

57. Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6

58. Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6

59. Carbon dioxide dissolves in rainwater to form weak carbonic acid. CO 2(g) + H 2 O (l)  H 2 CO 3(aq) Natural rainwater has a pH of about 5.6 Rainwater with a pH of 5.6 and above is NOT called Acid Rain

60. Natural rainwater has a pH of about 5.6 Rainwater is a pH lower than 5.6 is called Acid Rain Non-metal oxides dissolve in water to form ACIDIC solutions.

61. Thermal power generating plants burn large amounts of coal.

62. Non-metal oxides dissolve in water to form ACIDIC solutions. Thermal power generating plants burn large amounts of coal. Coal and other fossil fuels contain small amounts of sulfur.

63. S (s) + O 2(g) 

64. S (s) + O 2(g)  SO 2(g)

65. SO 2 is a non-metal oxide S (s) + O 2(g)  SO 2(g)

66. SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Sulfurous acid

67. S (s) + O 2(g)  SO 2(g) SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Dissolved sulfurous acid causes Acid Precipitation

68. SO 2(g) + H 2 O (l)  H 2 SO 3(aq) SO 3(g) + H 2 O (l)  H 2 SO 4(aq) Many industrial processes release SO 2 and SO 3 into the atmosphere

69. SO 2(g) + H 2 O (l)  H 2 SO 3(aq) Aqueous sulfurous acid and sulfuric acid cause Acid Precipitation SO 3(g) + H 2 O (l)  H 2 SO 4(aq)

70. Non-metal oxides dissolve in water to form ACIDIC solutions. Vehicle exhaust releases nitrogen oxides like NO 2 to the atomosphere.

71. 2NO 2(g) + H 2 O (l)  HNO 2(aq) + HNO 3(aq) Nitric acid Nitrous Acid

72. Acid precipitation can have serious effects on freshwater organisms, crops, and forests.

73. Acid precipitation can also damage buildings and statues made of limestone or marble.

74. Limestone and marble are made up of calcium carbonate, CaCO 3(s).

75. Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs:

76. CaCO 3(s) + H 2 SO 4(aq) 

77. Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s)

78. Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l)

79. Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l) + CO 2(g)

80. Limestone and marble are made up of calcium carbonate, CaCO 3(s). When calcium carbonate is exposed to sulfuric acid (H 2 SO 4(aq) ), the following reaction occurs: CaCO 3(s) + H 2 SO 4(aq)  CaSO 4(s) + H 2 O (l) + CO 2(g) This slowly dissolves the CaCO 3 which makes up limestone or marble.