1. Lewis acid-base theory

2. Very different from Brønsted-Lowrey acid-base.

3. Lewis acid-base theory Very different from Brønsted-Lowrey acid-base. Not dependent on protons or pH.

4. Lewis acid-base theory An acid is a lone-pair acceptor. Definitions:

5. Lewis acid-base theory An acid is a lone-pair acceptor. H + no electrons – by accepting 2 electrons it attains noble gas configuration. Definitions:

6. Lewis acid-base theory An acid is a lone-pair acceptor. H + no electrons – by accepting 2 electrons it attains noble gas configuration. BF 3 electron deficient compound - B needs 2 electrons for noble gas configuration.

7. B Group III 3 valence electrons

8. F Group VII 7 valence electrons

9. B Group III 3 valence electrons F Group VII 7 valence electrons

11. 6 electrons for boron rather than 8 Lewis Acid

12. Lewis acid-base theory Lewis base: lone-pair donor Definitions:

13. Lewis acid-base theory Lewis base: lone-pair donor NH 3 N has lone pair Definitions:

14. Group V Group I

16. Lewis Base

17. Lewis acid-base theory Lewis base: lone-pair donor NH 3 - N has lone pair H 2 O - O has 2 lone pairs

18. Lewis acid-base theory H 3 N : + BF 3 H 3 N : BF 3

19. Lewis acid-base theory H 3 N : + BF 3 H 3 N : BF 3 Lewis base

20. Lewis acid-base theory H 3 N : + BF 3 H 3 N : BF 3 Lewis base Lewis acid

21. Lewis acid-base theory H 3 N : + BF 3 H 3 N : BF 3 Lewis base Lewis acid Both electrons in this bond come from nitrogen.

22. Lewis acid-base theory H 3 N : + BF 3 H 3 N : BF 3 Lewis base Lewis acid Coordinate covalent bond

23. (CH 3 ) 3 N BCl 3 (CH 3 ) 3 N : + BCl 3 (CH 3 ) 3 N : BCl 3

24. (CH 3 ) 3 N BCl 3 (CH 3 ) 3 N : + BCl 3 (CH 3 ) 3 N : BCl 3 This compound may be referred to as an adduct.

25. CH 3 COOH (aq) + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq)

26. CH 3 COOH (aq) + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq) NH 3 Lewis base

27. CH 3 COOH (aq) + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq) NH 3 Lewis base CH 3 COOH is not a Lewis acid.

28. H + + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq) NH 3 Lewis base CH 3 COOH is not a Lewis acid. CH 3 COOH(aq) + H 2 O H 3 O + + CH 3 COO -

29. H + + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq) NH 3 Lewis base CH 3 COOH is not a Lewis acid. CH 3 COOH(aq) + H 2 O H 3 O + + CH 3 COO - H 3 O + H + + H 2 O

30. CH 3 COOH (aq) + NH 3(aq) NH 4 + (aq) + CH 3 COO - (aq) NH 3 Lewis base CH 3 COOH is not a Lewis acid. H + is the Lewis acid.

31. Al(OC 2 H 5 ) 3

32. Tri-ethoxy aluminum

33. Al(OC 2 H 5 ) 3 Al is Group III - electron deficient like BF 3.

34. Al(OC 2 H 5 ) 3 Al is Group III - electron deficient like boron.

35. Al(OC 2 H 5 ) 3 Al is Group III - electron deficient like boron. This molecule is a Lewis acid.

36. Al(OC 2 H 5 ) 3 Al is Group III - electron deficient like boron. This molecule is a Lewis acid. O has lone pairs, it is a Lewis base

37. Al(OC 2 H 5 ) 3 Al is Group III - electron deficient like boron. This molecule is a Lewis acid. O has lone pairs, it is a Lewis base The molecule is both a Lewis acid and base.

38. x3 Al...

39. Al(OC 2 H 5 ) 3

40. Covalent bonds

41. Al(OC 2 H 5 ) 3 Electron deficient

42. Al(OC 2 H 5 ) 3 Empirical formula

43. [Al(OC 2 H 5 ) 3 ] 2 Al(OC 2 H 5 ) 3 Empirical formula Molecular formula

44. [Al(OC 2 H 5 ) 3 ] 2 dimer

45. [Al(OC 2 H 5 ) 3 ] 2 dimer Covalent bonds

46. [Al(OC 2 H 5 ) 3 ] 2 dimer Covalent bonds Coordinate covalent bonds

47. [Al(OC 2 H 5 ) 3 ] 2 dimer

48. AlCl 3

49. Empirical formula

50. AlCl 3 Empirical formula [AlCl 3 ] 2 Molecular formula

51. [AlCl 3 ] 2

53. s block

54. p block

55. s block p block Main Group Elements

56. Oxides of s and p block elements are acid and base anhydrides, with definite trends in respect to the elements’ location in the periodic table.

57. Oxides of non-metals tend to be acid anhydrides Oxides of metals tend to be base anhydrides

58. Structure and bonding in s and p block oxides From: N. C. Norman Chapter 5

59. Norman: Chapter 6 should be read for acid and base information.

60. Structure and bonding in s and p block oxides From: N. C. Norman Group numbers are changed in Norman.

61. Groups 1 - 18 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

62. Structure and bonding in s and p block oxides Increasing electronegativity

63. Binary ionic compounds form from elements having very different electronegativities.

64. Binary ionic compounds form from elements having very different electronegativities.

65. Oxygen is high on the electronegativity scale, Rb and Ba have the lowest electronegativities of the metals on the Norman chart.

66. K 2 O : ionic material

67. K 2 O(s) + H 2 O(l) 2 K + (aq) + O 2- (aq)

68. K 2 O : ionic material K 2 O(s) + H 2 O(l) 2 K + (aq) + O 2- (aq) O 2- (aq) + H 2 O(l) 2 OH - (aq)

69. K 2 O : ionic material K 2 O(s) + H 2 O(l) 2 K + (aq) + 2 OH - (aq) Strong base

70. K 2 O : ionic material K 2 O(s) + H 2 O(l) 2 K + (aq) + 2 OH - (aq) Strong base Base anhydride

72. Small differences in electronegativities lead to covalent bonds.

73. Small differences in electronegativities lead to covalent bonds.

74. SO 3 : covalent molecule

75. SO 3 (g) + H 2 O(l) H 2 SO 4 (aq) Strong acid

76. SO 3 : covalent molecule SO 3 (g) + H 2 O(l) H 2 SO 4 (aq) Strong acid Acid anhydride

79. Some of the polymeric oxides will be amphoteric.

80. Some of the polymeric oxides will be amphoteric. They will act as acids or bases depending on how acidic or basic the environment is.

81. Some of the polymeric oxides will be amphoteric. Al 2 O 3 (aq) + 6 H + (aq) 2 Al 3+ (aq) + 3 H 2 O(l)

82. Some of the polymeric oxides will be amphoteric. Al 2 O 3 (aq) + 6 H + (aq) 2 Al 3+ (aq) + 3 H 2 O(l) Al 2 O 3 reduces H + = basic

83. Some of the polymeric oxides will be amphoteric. Al 2 O 3 (aq) + 6 H + (aq) 2 Al 3+ (aq) + 3 H 2 O(l) Al 2 O 3 reduces H + = basic Al 2 O 3 (aq) + 2 OH - (aq) + 3 H 2 O(l) 2 [Al(OH) 4 ] - (aq)

84. Some of the polymeric oxides will be amphoteric. Al 2 O 3 (aq) + 2 OH - (aq) + 3 H 2 O(l) 2 [Al(OH) 4 ] - (aq) Al 2 O 3 reduces OH - : acidic

85. Structures of polymeric oxides

86. quartz SiO 4 Empirical formula

87. quartz SiO 4 Empirical formula

88. quartz SiO 4 Empirical formula

89. quartz Tetrahedra share all corners Each share = 1/2 O/Si

90. quartz Tetrahedra share all corners Each share = 1/2 O/Si

91. quartz Tetrahedra share all corners Each share = 1/2 O/Si

92. Binary compounds with halogens

93. chlorides

94. NaCl : ionic salt

95. chlorides NaCl : ionic salt CCl 4 : dense liquid

96. chlorides NaCl : ionic salt CCl 4 : dense liquid BCl 3 : gas covalent

97. chlorides AlCl 3 : dimer

98. chlorides AlCl 3 : dimer GaCl 3 : dimer

99. chlorides AlCl 3 : dimer GaCl 3 : dimer

100. chlorides BeCl 2 : infinite chain