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2. Chapter Menu Electrochemistry Section 20.1 Voltaic Cells Section 20.2 Batteries Section 20.3 Electrolysis Exit Click a hyperlink or folder tab to view the corresponding slides. 3. Section 20-1 Section 20.1Voltaic Cells
oxidation:the loss of electrons from the atoms of a substance; increases an atoms oxidation number
reduction:the gain of electrons by the atoms of a substance; decreases the atoms oxidation number 4. Section 20-1 Section 20.1Voltaic Cells(cont.) salt bridge electrochemical cell voltaic cell half-cell In voltaic cells, oxidation takes place at the anode, yielding electrons that flow to the cathode, where reduction occurs. anode cathode reduction potential standard hydrogen electrode 5. Section 20-1 Redox in Electrochemistry
6. Section 20-1 Redox in Electrochemistry(cont.) 7. Section 20-1 Redox in Electrochemistry(cont.)
8. Section 20-1 Redox in Electrochemistry(cont.)
9. Section 20-1 Chemistry of Voltaic Cells
10. Section 20-1 Chemistry of Voltaic Cells(cont.)
11. Section 20-1 Calculating Electrochemical Cell Potentials
12. Section 20-1 Calculating Electrochemical Cell Potentials(cont.)
13. Section 20-1 Calculating Electrochemical Cell Potentials(cont.)
14. Section 20-1 Calculating Electrochemical Cell Potentials(cont.) 15. Section 20-1 Calculating Electrochemical Cell Potentials(cont.)
16. Section 20-1 Use Standard Reduction Potentials
17.
Section 20-1 Section 20.1 Assessment In electrochemistry, the site where oxidation occurs is called ____.A. electrode B. anode C. cathode D. ion 18.
Section 20-1 Section 20.1 Assessment The standard potential of a voltaic cell is the difference between the:A. electrode voltage B. standard reduction potentialof the cell and hydrogen C. standard reduction potentialsof the half-cell reactions D. half-cell reactions and thesalt bridge 19. End of Section 20-1 20. Section 20-2 Section 20.2Batteries
reversible reaction:a reaction that can take place in both the forward and reverse directions
21. Section 20-2 Section 20.2Batteries(cont.) battery dry cell primary battery secondary battery Batteries are voltaic cells that use spontaneous reactions to provide energy for a variety of purposes. fuel cell corrosion galvanization 22. Section 20-2 Dry Cells
23. Section 20-2 Dry Cells(cont.)
24. Section 20-2 Dry Cells(cont.)
25. Section 20-2 Dry Cells(cont.)
26. Section 20-2 Dry Cells(cont.)
27. Section 20-2 Lead-Acid Storage Battery
28. Section 20-2 Lithium Batteries
29. Section 20-2 Fuel Cells
30. Section 20-2 Fuel Cells(cont.)
31. Section 20-2 Corrosion
32. Section 20-2 Corrosion(cont.)
33. Section 20-2 Corrosion(cont.) 34. Section 20-2 Corrosion(cont.)
35. Section 20-2 Corrosion(cont.)
36.
Section 20-2 Section 20.2 Assessment Which type of battery has a reversible spontaneous reaction? A. alkaline battery B. secondary battery C. primary battery D. zinc-carbon battery 37.
Section 20-2 Section 20.2 Assessment Which is NOT a method of preventing corrosion?A. painting B. galvanization C. coating with electrolytes D. sacrificial anode 38. End of Section 20-2 39. Section 20-3 Section 20.3Electrolysis
redox reaction:an oxidation-reduction reaction electrolysis electrolytic cell
In electrolysis, a power source causes nonspontaneous reactions to occur in electrochemical cells. 40. Section 20-3 Reversing Redox Reactions
41. Section 20-3 Applications of Electrolysis
42. Section 20-3 Applications of Electrolysis(cont.)
43. Section 20-3 Applications of Electrolysis(cont.)
44. Section 20-3 Applications of Electrolysis(cont.)
45. Section 20-3 Applications of Electrolysis(cont.)
46.
Section 20-3 Section 20.3 Assessment Which of the following is NOT a product of electrolysis of brine?A. Chlorine gas B. Hydrogen gas C. Sodium hydroxide solution D. Sodium metal 47.
Section 20-3 Section 20.3 Assessment What is required to drive a nonspontaneous reaction in an electrolytic cell?A. electrodes B. additional ions C. an energy source D. an electrolyte 48. End of Section 20-3 49. Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion 50. Study Guide 1 Section 20.1Voltaic Cells Key Concepts
51. Study Guide 1 Section 20.1Voltaic Cells(cont.) Key Concepts
52. Study Guide 2 Section 20.2Batteries Key Concepts
53. Study Guide 3 Section 20.3Electrolysis Key Concepts
54.
Chapter Assessment 1 A salt bridge is used for what? A. electrolysis B. allowing ions to move fromone half-cell to the other C. increasing the reductionpotential D. linking multiple voltaic cellstogether 55.
Chapter Assessment 2 Batteries that can be used more than once are also called ____. A. primary batteries B. secondary batteries C. tertiary batteries D. fuel cells 56.
Chapter Assessment 3 Corrosion is loss of metal by what mechanism? A. electrolysis B. galvanization C. oxidation-reduction reaction D. salt bridge 57.
Chapter Assessment 4 Electrolysis of H 2 O results in what products? A. H +and OH B. H 2 O 2and O 2 C. NaOH and H 2 D. H 2and O 2 58.
Chapter Assessment 5 Which of the following is NOT a dry-cell?A. a car battery B. a silver battery C. a zinc-carbon battery D. an alkaline battery 59.
STP 1 Which is NOT a characteristic of an acid? A. sour taste B. conduct electricity in solution C. reactivity with some metals D. slippery feel 60.
STP 2 Which metal has the lowest standard reduction potential? A. Sodium B. Magnesium C. Lithium D. Silver 61.
STP 3 Which statement is NOT true about batteries? A. Batteries are composed of twohalf-cells. B. Secondary batteries are alsoknown as storage batteries. C. Redox reactions in zinc-carbonbatteries are easily reversible. D. Batteries are compact forms ofvoltaic cells. 62.
STP 4 Which of the following is the equation used to calculate a cell potential? A. E 0 cell=E 0 oxidation E 0 reduction B. E 0 cell=E 0 reduction E 0 oxidation C. E 0 cell=E 0 reduction+ E 0 oxidation D. E 0 cell=E 0 reduction xE 0 oxidation 63.
STP 5 Which is NOT an example of a sacrificial anode?A. magnesium B. aluminum C. iron D. titanium 64. IB Menu Click on an image to enlarge. 65. IB 1 66. IB 2 67. IB 3 68. IB 4 69. IB 5 70. IB 6 71. IB 7 72. IB 8 73. IB 9 74. IB 10 75. IB 11 76. IB 12 77. IB 13 78. IB 14 79. IB 15 80. IB 16 81. IB 17 82. IB 18 83. IB 19 84. CIM Figure 20.2Voltaic Cells 85. Help Click any of the background top tabs to display the respective folder. Within the Chapter Outline, clicking a section tab on the right side of the screen will bring you to the first slide in each respective section. Simple navigation buttons will allow you to progress to the next slide or the previous slide. The Return button will allow you to return to the slide that you were viewing when you clicked either the Resources or Help tab. The Chapter Resources Menu will allow you to access chapter specific resources from the Chapter Menu or any Chapter Outline slide. From within any feature, click the Resources tab to return to this slide. To exit the presentation, click the Exit button on the Chapter Menu slide or hit Escape [Esc] on your keyboards while viewing any Chapter Outline slide. 86. End of Custom Shows This slide is intentionally blank.