1. Electrochemistry Lesson 1 Introduction

2. Electrochemistry Is the study of reactions that gain or lose electrons.

3. Electrochemistry Is the study of reactions that gain or lose electrons. In this unit we will study:

4. Battery Reactions

5. Corrosion

6. Preventing Corrosion

7. Combustion

8. Electroplating

9. Refining Metals

10. Oxidation means loss of electrons LEO

11. Oxidation means loss of electrons LEOLossElectronsOxidation

12. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions

13. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons

14. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Na

15. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Na metalion

16. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Na Na + metalion Balance charge Add electron to most positive side

17. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Na Na + metalion Balance charge Add electron to most positive side

18. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons 0+1 Na Na + metalion Balance charge Add electron to most positive side

19. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons0 Na Na + +1e - metalion Balance charge Add electron to most positive side Oxidation- electrons are on the right

20. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Al

21. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Al metalion

22. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Al Al 3+ metalion Balance charge Add electrons to most positive side

23. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons Al Al 3+ metalion Balance charge Add electrons to most positive side

24. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons 0+3 Al Al 3+ metalion Balance charge Add electrons to most positive side

25. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons0 Al Al 3+ +3e - metalion Balance charge Add electrons to most positive side Oxidation- electrons are on the right

26. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons O 2-

27. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons O 2- anionatom

28. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons O 2- O 2 anionatom

29. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons O 2- O 2 anionatom Balance for numbers

30. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons 2O 2- O 2 anionatom Balance for numbers

31. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons 2O 2- O 2 anionatom Balance for numbers Balance charge Add electrons to most positive side

32. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons -40 2O 2- O 2 anionatom Balance for numbers Balance charge Add electrons to most positive side

33. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons-4 2O 2- O 2 +4e - anionatom Balance for numbers Balance charge Add electrons to most positive side

34. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons 2O 2- O 2 +4e - anionatom Balance for numbers Oxidation- electrons are on the right Balance charge Add electrons to most positive side

35. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons Ga 3+

36. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons Ga 3+ cation atom

37. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons Ga 3+ Ga cation atom

38. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons +30 Ga 3+ Ga cationatomBalance charge Add electrons to most positive side

39. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons0 Ga 3+ + 3e - Ga cationatomBalance charge Add electrons to most positive side Reduction- electrons are on the left

40. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2

41. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2

42. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2 N 3-

43. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2 2N 3-

44. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2 + 6e - 2N 3-

45. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N 2 + 6e - 2N 3- Reduction- electrons are on the left

46. Balance each simple half reaction 1.Ca 2.F 2 3.O 2 4.Ga 5.Br - 6.Li +

47. Balance each simple half reaction 1.Ca Ca 2+ +2e - 2.F 2 + 2e - 2F - 3.O 2 + 4e - 2O 2- 4.Ga 5.Br - 6.Li +

48. Balance each simple half reaction 1.Ca Ca 2+ +2e - 2.F 2 + 2e - 2F - 3.O 2 + 4e - 2O 2- 4.Ga Ga 3+ +3e - 5.2Br - Br 2 + 2e - 6.Li + +e - Li

49. Balance each simple half reaction 1.Ca Ca 2+ +2e - oxidation 2.F 2 + 2e - 2F - reduction 3.O 2 + 4e - 2O 2- reduction 4.Ga Ga 3+ +3e - oxidation 5.2Br - Br 2 + 2e - oxidation 6.Li + +e - Lireduction

50. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 3

51. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 Al Al 3+ +3e - oxidation

52. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 Al Al 3+ +3e - oxidation Zn 2+ Use metals/cations

53. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 Al Al 3+ +3e - oxidation Zn 2+ +2e - Znreduction

54. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction Balance electrons

55. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ + 6e - 2Al 3+ + 3Zn + 6e - redox

56. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ + 6e - 2Al 3+ + 3Zn + 6e - redox

57. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ 2Al 3+ + 3Zn redox

58. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ 2Al 3+ + 3Zn redox Check charge

59. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ 2Al 3+ + 3Zn redox+6 Check charge

60. Redox Reactions Both oxidation and reduction must occur. The number of electrons gained must be equal to the number of electrons lost. It is simpler to write the net ionic equation. 1.Al+Zn(NO 3 ) 2 2(Al Al 3+ +3e - )oxidation 3(Zn 2+ +2e - Zn)reduction 2Al + 3Zn 2+ 2Al 3+ + 3Zn redox+6 Check chargeSame!

61. 2.Cl 2 +Na

62. Cl 2 +2e - 2Cl - reduction

63. 2.Cl 2 +Na Cl 2 +2e - 2Cl - reduction Na Na + +1e - oxidation

64. 2.Cl 2 +Na Cl 2 +2e - 2Cl - reduction 2(Na Na + +1e - )oxidation

65. 2.Cl 2 +Na Cl 2 +2e - 2Cl - reduction 2(Na Na + +1e - )oxidation Cl 2 + 2Na 2Cl - + 2Na + redox0

66. Oxidizing Agents

67. Oxidizing Agents cause oxidation by undergoing reduction.

68. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons.

69. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons.

70. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2

71. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+

72. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2

73. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na +

74. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na + Cl 2 +2e -2Cl -

75. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na + Cl 2 +2e -2Cl - Ca 2+ +2e -Ca

76. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na + Cl 2 +2e -2Cl - Ca 2+ +2e -Ca Both can gain electrons

77. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na + Cl 2 +2e -2Cl - Ca 2+ +2e -Ca Both can gain electrons

78. Oxidizing Agents cause oxidation by undergoing reduction. They gain electrons. Nonmetals and cations are oxidizing agents because they gain electrons. Cl 2 Ca 2+ F 2 Na + Cl 2 +2e -2Cl - Ca 2+ +2e -Ca Both can gain electrons

79. Reducing Agents

80. Reducing Agents cause reduction by undergoing oxidation.

81. Reducing Agents cause reduction by undergoing oxidation. They lose electrons.

82. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons.

83. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3-

84. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- Al

85. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2-

86. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2- Li

87. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2- Li 2N 3-N 2 +6e - AlAl 3+ +3e -

88. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2- Li 2N 3-N 2 +6e - AlAl 3+ +3e - Both can lose electrons

89. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2- Li 2N 3-N 2 +6e - AlAl 3+ +3e - Both can lose electrons

90. Reducing Agents cause reduction by undergoing oxidation. They lose electrons. Metals and anions are reducing agents because they lose electrons. N 3- AlO 2- Li 2N 3-N 2 +6e - AlAl 3+ +3e - Both can lose electrons

91. You need to be able to tell an oxidizing agent from a reducing agent.

92. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent.

93. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons

94. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

95. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

96. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

97. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

98. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

99. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

100. You need to be able to tell an oxidizing agent from a reducing agent. Circle each oxidizing agent. They can reduce or gain electrons GaRb + I - P 4 FeCo 2+ SI 2 CuPb 2+ LiBr -

101. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb2Ag +Pb 2+

102. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb2Ag +Pb 2+ Reduction

103. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb2Ag +Pb 2+ ReductionOxidation

104. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb2Ag +Pb 2+ ReductionOxidation Ox Agent

105. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb2Ag +Pb 2+ ReductionOxidation Ox AgentRed Agent

106. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ 3I 2 +Al

107. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ 3I 2 +Al Oxidation

108. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ 3I 2 +Al OxidationReduction

109. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ 3I 2 +Al OxidationReduction Red Agent

110. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ 3I 2 +Al OxidationReduction Red AgentOx Agent