2. Acids & Bases

3. Water and acid combine in an exothermic reaction - releasing large amounts of heat.

4. Water and acid combine in an exothermic reaction - releasing large amounts of heat.

5. Acid - Base Theories Lavoisier Arrhenius Bronsted-Lowry Lewis Lavoisier Arrhenius Bronsted-Lowry Lewis

6. Antoine Lavoisier

7. Acidity is caused by the presence of oxygen in the compound. Lavoisier - 1777

8. He even created the word oxygen - from the Greek oxys, "sour" and genes, "born" Lavoisier - 1777

9. Oxygen means "acid maker". Lavoisier - 1777

10. Lavoisier's idea about acids turned out to be wrong... Lavoisier - 1777

11. but it is historically important since it is the first scientific attempt to chemically characterize acids and bases. Lavoisier - 1777

12. Arrhenius Bronsted-Lowry Lewis

13. Svante August Arrhenius

14. Arrhenius Acid Any substance that produces hydrogen ions, H +, in water solution.

15. Any substance that produces hydroxide ions, OH -, in water solution. Arrhenius Base

16. In a formula, such as HCl, the positive part of a Arrhenius acid will ALWAYS be hydrogen.

17. In a formula, such as NaOH, the negative part of a Arrhenius base will ALWAYS be hydroxide.

18. Arrhenius acids and bases, and soluble salts, are called electrolytes.

19. When each dissolves, ions are released that conduct electricity.

20. If a solution has NO ions, it cannot conduct electricity.

21. Johannes Nicolaus Bronsted Bronsted-Lowry Theory

22. Thomas Martin Lowry Bronsted-Lowry Theory

23. Any substance that acts as a proton donor. Bronsted-Lowry Acid

24. A B-L acid MUST have hydrogen somewhere in its formula. Bronsted-Lowry Acid

25. When an electron is removed from a hydrogen atom... + - Bronsted-Lowry Acid

26. a hydrogen ion is produced - a proton. + Bronsted-Lowry Acid

27. Bronsted-Lowry Base Any substance that acts as a proton acceptor.

28. Bronsted-Lowry Base Most negative ions can acts as B-L bases.

29. The acid/base definitions are broadened because no specific ion must be formed, although hydrogen is the only source of protons. Bronsted-Lowry Theory

30. What is the formula for the hydronium ion?

31. H3O+H3O+

32. The hydronium ion is formed by combining a hydrogen ion and a water molecule. H 2 O + H + H 3 O + Bronsted-Lowry Theory

33. conjugate base Bronsted-Lowry Theory

34. A conjugate base is the particle that remains AFTER an acid gives up a proton. Bronsted-Lowry Theory

35. conjugate acid Bronsted-Lowry Theory

36. A conjugate acid is the particle formed when a base accepts a proton. Bronsted-Lowry Theory

37. HCl + H 2 O Cl - + H 3 O + Identify the B-L acid in this equation. What gives up a proton from the left side to the right?

38. HCl + H 2 O Cl - + H 3 O + HCl donates a proton, it is the B-L acid.

39. Identify the B-L base in this equation. What gains a proton from the left side to the right? HCl + H 2 O Cl - + H 3 O +

40. H 2 O accepts a proton, it is the B-L base.

41. HCl + H 2 O Cl - + H 3 O + Identify the conjugate base in this equation. What is left when the acid gives up a proton?

42. HCl + H 2 O Cl - + H 3 O + Cl - is left when HCl gives up a proton, it is the conjugate base.

43. HCl + H 2 O Cl - + H 3 O + Identify the conjugate acid in this equation. What is formed when the base accepts a proton?

44. HCl + H 2 O Cl - + H 3 O + H 3 O + is formed when water accepts a proton, it is the conjugate acid.

45. HCl + H 2 O Cl - + H 3 O + acids have conjugate bases

46. HCl + H 2 O Cl - + H 3 O + bases have conjugate acids

47. Remove a proton from an acid to get its conjugate base. H 2 SO 4 HI H 2 O

48. Remove a proton from an acid to get its conjugate base. HSO 4 - H 2 SO 4 HI H 2 O

49. Remove a proton from an acid to get its conjugate base. HSO 4 - I - H 2 SO 4 HI H 2 O

50. Remove a proton from an acid to get its conjugate base. HSO 4 - I - OH - H 2 SO 4 HI H 2 O

51. Add a proton to a base to get its conjugate acid. Cl - H 2 O NO 3 -

52. Add a proton to a base to get its conjugate acid. HClCl - H 2 O NO 3 -

53. Add a proton to a base to get its conjugate acid. HCl H 3 O + Cl - H 2 O NO 3 -

54. Add a proton to a base to get its conjugate acid. HCl H 3 O + HNO 3 Cl - H 2 O NO 3 -

55. Gilbert Newton Lewis The Lewis Theory

56. Lewis Acid Any substance that acts as an electron-pair acceptor.

57. Lewis Base Any substance that acts as an electron-pair donor.

58. The Lewis Theory This theory is the broadest of all.

59. The Lewis Theory Any reaction that involves the exchange of electrons WILL have a Lewis acid and Lewis base.

60. The Lewis Theory In an equation, the Lewis acid gets MORE NEGATIVE from the left side to the right side - it gains e -.

61. The Lewis Theory In an equation, the Lewis base gets MORE POSITIVE from the left side to the right side - it loses e -.

62. Cl 2 + I - Cl - + I 2 Identify the Lewis acid in this equation. What gets more negative?

63. Cl 2 gets more negative from the left side to the right, it is the Lewis acid. Cl 2 + I - Cl - + I 2

64. Identify the Lewis base in this equation. What gets more positive? Cl 2 + I - Cl - + I 2

65. I - gets more positive from the left side to the right, it is the Lewis base. Cl 2 + I - Cl - + I 2

66. End Acid - Base Theories

67. Binary Acids Acids composed of two elements: hydrogen and a halogen

68. First: Determine the stem word. The stem word comes from the negative element. Naming Binary Acids

69. First: Determine the stem word. Example - HCl chlorine is the negative element - CHLOR is the stem. Naming Binary Acids

70. Second: Add the prefix hydro to the stem. Naming Binary Acids

71. Second: Add the prefix hydro to the stem. Example - hydro + chlor Naming Binary Acids

72. Third: Change the ending of the stem to ic. Naming Binary Acids

73. Third: Change the ending of the stem to ic. Example - hydro + chlor + ic Naming Binary Acids

74. Final name: hydrochloric acid Naming Binary Acids

75. HCl HF HBr HI Naming Binary Acids

76. HCl hydro chlor ic acid HF HBr HI Naming Binary Acids

77. HCl hydro chlor ic acid HF hydro fluor ic acid HBr HI Naming Binary Acids

78. HCl hydro chlor ic acid HF hydro fluor ic acid HBr hydro brom ic acid HI Naming Binary Acids

79. HCl hydro chlor ic acid HF hydro fluor ic acid HBr hydro brom ic acid HI hydro iod ic acid Naming Binary Acids

80. Ternary acids composed of three elements: hydrogen, oxygen, and a nonmetal Naming Ternary Acids

81. First: Determine the stem part of the name of the third element Naming Ternary Acids

82. First: Determine the stem Example - H 2 SO 4 sulfur is the third element, SULFUR is the stem. Naming Ternary Acids

83. Second: The most common form of the acid is given the suffix ic. Naming Ternary Acids

84. Second: The most common form of the acid is given the suffix ic. Example - sulfur + ic acid Naming Ternary Acids

85. Third: If the acid is NOT in its most common form, do the following: Naming Ternary Acids

86. Add the prefix per if the acid has one more oxygen than the most common form.

87. Add the prefix per if the acid has one more oxygen than the most common form. Example - H 2 SO 5 per + sulfuric acid Naming Ternary Acids

88. Add the suffix ous if the acid has one less oxygen than the most common form.

89. Add the suffix ous if the acid has one less oxygen than the most common form. Example - H 2 SO 3 sulfur + ous acid Naming Ternary Acids

90. Add the prefix hypo if the acid has two less oxygen atoms than the most common form.

91. Add the prefix hypo if the acid has two less oxygen atoms than the most common form. Example - H 2 SO 2 hypo + sulfur + ous acid Naming Ternary Acids

92. HClO 3 Chloric Acid Naming Ternary Acids

93. HClO 4 HClO 3 Chloric Acid Naming Ternary Acids

94. HClO 4 Perchloric Acid HClO 3 Chloric Acid Naming Ternary Acids

95. HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Naming Ternary Acids

96. HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid Naming Ternary Acids

97. HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid HClO Naming Ternary Acids

98. HClO 4 Perchloric Acid HClO 3 Chloric Acid HClO 2 Chlorous Acid HClO Hypochlorous Acid Naming Ternary Acids

99. Strong or Weak

100. Strong acids and bases ionize completely in water solution.

101. Strong or Weak HCl, HBr, and HI are the only Strong binary acids.

102. Strong or Weak In Strong ternary acids, the number of oxygen atoms exceeds the number of...

103. Strong or Weak hydrogen atoms by two or more. H 2 SO 4 and HNO 3 are strong. H 3 PO 4 is weak.

104. Strong or Weak Hydroxides of groups 1 and 2, except Be, are Strong bases.

105. Amphoteric A substance that acts as either an acid or base, depending on what it reacts with.

106. Water is the most common amphoteric substance. HOH

107. Anhydrous - Without H 2 O

108. Acid Anhydride - an oxide that produces an acid in water.

109. SO 2 + H 2 O H 2 SO 3 Acid Anhydride - oxides of nonmetals

110. Basic Anhydride - an oxide that produces a base in water.

111. Na 2 O + H 2 O 2NaOH Basic Anhydride - oxides of metals

112. Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 2. H 2 C 2 O 4 3. H 3 PO 4 4. H 4 C 2 O 2

113. Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 3. H 3 PO 4 4. H 4 C 2 O 2

114. Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 4. H 4 C 2 O 2

115. Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 HPO 3 4. H 4 C 2 O 2

116. Anhydrous - Without H 2 O Write the anhydrous form of: 1. H 2 SO 3 SO 2 2. H 2 C 2 O 4 C 2 O 3 3. H 3 PO 4 HPO 3 4. H 4 C 2 O 2 C 2