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- oxidation and reduction

5. Corrosion- oxidation

6. Preventing Corrosion

7. Oxidation

8. Electroplating- reduction

9. Refining Metals- reduction

10. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons metalion Balance charge Add electron to most positive side Oxidation- electrons are on the right Na→ 0+1 +1e - Na +

11. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons metalion Balance charge Add electrons to most positive side Oxidation- electrons are on the right Al→ 0+3 Al 3+ +3e -

12. Oxidation means loss of electrons LEOLossElectronsOxidation Oxidation Half Reactions show how Metals or Anions lose electrons O 2- → anionatom Balance for numbers Oxidation- electrons are on the right Balance charge Add electrons to most positive side O2O2 2+4e -

13. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons cationatom Balance charge Add electrons to most positive side Reduction- electrons are on the left 3+ 0 →Ga+ 3e - Ga 3+

14. Reduction means gain of electrons GERGainElectronsReduction Reduction Half Reactions show how Nonmetals or Cations gain electrons N2N2 N 3- 2+ 6e - → Reduction- electrons are on the left

15. Balance each simple half reaction 1. → Ca 2+ +2e - Caoxidation 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

16. Redox Reactions Both oxidation and reduction must occur. The electrons gained equals the electrons lost. 1.Al+Zn(NO 3 ) 2 Al →Al 3+ +3e - ( )oxidation Zn 2+ ( ) reduction 2 3 2Al + 3Zn 2+ → 2Al 3+ + 3Zn redox +2e - →Zn

17. 2.Cl 2 +Na Cl 2 +2e - →2Cl - reduction 2(Na →Na + +1e - )oxidation Cl 2 + 2Na → 2Cl - + 2Na + redox

18. 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

19. 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 - Al→Al 3+ +3e - Both can lose electrons

20. 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 -

21. Label each reactant as an oxidizing or reducing agent. 2Ag + +Pb→2Ag +Pb 2+ Gaining electrons ReductionOxidation Losing electrons Ox AgentRed Agent

22. Label each reactant as an oxidizing or reducing agent. 6I - + 2Al 3+ →3I 2 +2Al Gaining electronsLosing electrons Oxidation Red Agent Reduction Ox Agent