1. © 2015 Pearson Education, Inc. Clicker Questions Chapter 20 Barbara Mowery York College

2. © 2015 Pearson Education, Inc. The oxidation state of nitrogen in the ammonium ion (NH 4 1+ ) is _______. a.+1 b.0 c.−1 d.−3

3. © 2015 Pearson Education, Inc. The oxidation state of nitrogen in the ammonium ion (NH 4 1+ ) is _______. a.+1 b.0 c.−1 d.−3

4. © 2015 Pearson Education, Inc. The oxidation state of manganese in the permanganate ion (MnO 4 1− ) is _______. a.−1 b.+2 c.+4 d.+7

5. © 2015 Pearson Education, Inc. The oxidation state of manganese in the permanganate ion (MnO 4 1− ) is _______. a.−1 b.+2 c.+4 d.+7

6. © 2015 Pearson Education, Inc. Zn + Cu 2+  Zn 2+ + Cu The reducing agent in the reaction above is _______. a.Zn b.Cu 2+ c.Zn 2+ d.Cu

7. © 2015 Pearson Education, Inc. Zn + Cu 2+  Zn 2+ + Cu The reducing agent in the reaction above is _______. a.Zn b.Cu 2+ c.Zn 2+ d.Cu

8. © 2015 Pearson Education, Inc. Zn + Cu 2+  Zn 2+ + Cu The oxidizing agent in the reaction above is _______. a.Zn b.Cu 2+ c.Zn 2+ d.Cu

9. © 2015 Pearson Education, Inc. Zn + Cu 2+  Zn 2+ + Cu The oxidizing agent in the reaction above is _______. a.Zn b.Cu 2+ c.Zn 2+ d.Cu

10. © 2015 Pearson Education, Inc. To balance the half-reaction MnO 4 −  Mn 2+ in acidic solution, ___ electrons must be added on the ___ side. a.5; product b.2; product c.7; reactant d.5; reactant

11. © 2015 Pearson Education, Inc. To balance the half-reaction MnO 4 −  Mn 2+ in acidic solution, ___ electrons must be added on the ___ side. a.5; product b.2; product c.7; reactant d.5; reactant

12. © 2015 Pearson Education, Inc. MnO 4 −  Mn 2+ To balance this reaction in acidic solution, ___ H + must be added on the ___ side. a.8; product b.4; product c.8; reactant d.4; reactant

13. © 2015 Pearson Education, Inc. MnO 4 −  Mn 2+ To balance this reaction in acidic solution, ___ H + must be added on the ___ side. a.8; product b.4; product c.8; reactant d.4; reactant

14. © 2015 Pearson Education, Inc. If the value of the standard cell potential for a reaction is large and positive, then the reaction is a.at equilibrium. b.spontaneous. c.nonspontaneous. d.very fast.

15. © 2015 Pearson Education, Inc. If the value of the standard cell potential for a reaction is large and positive, then the reaction is a.at equilibrium. b.spontaneous. c.nonspontaneous. d.very fast.

16. © 2015 Pearson Education, Inc. The purpose of the salt bridge in a voltaic cell is to a.provide H + ions needed to balance charges. b.maintain neutrality by allowing the flow of ions. c.serve as the site for oxidation to occur. d.serve as the site for reduction to occur.

17. © 2015 Pearson Education, Inc. The purpose of the salt bridge in a voltaic cell is to a.provide H + ions needed to balance charges. b.maintain neutrality by allowing the flow of ions. c.serve as the site for oxidation to occur. d.serve as the site for reduction to occur.

18. © 2015 Pearson Education, Inc. Which of the following is the strongest oxidizing agent? (If necessary, consult a table of standard reduction potentials.) a.F 2 b.Cl 2 c.Br 2 d.I 2

19. © 2015 Pearson Education, Inc. Which of the following is the strongest oxidizing agent? (If necessary, consult a table of standard reduction potentials.) a.F 2 b.Cl 2 c.Br 2 d.I 2

20. © 2015 Pearson Education, Inc. Which of the following is the strongest reducing agent? (If necessary, consult a table of standard reduction potentials.) a.Zn b.Al c.Na d.Li

21. © 2015 Pearson Education, Inc. Which of the following is the strongest reducing agent? (If necessary, consult a table of standard reduction potentials.) a.Zn b.Al c.Na d.Li

22. © 2015 Pearson Education, Inc. Cl 2  2 Cl − ε red = + 1.36 V I 2  2 I − ε red = + 0.54 V Select the true statement. a.Cl 2 will reduce I − to I 2. b.Cl 2 will oxidize I − to I 2. c.I 2 will reduce Cl − to Cl 2. d.I 2 will oxidize Cl 2 to Cl −.

23. © 2015 Pearson Education, Inc. Cl 2  2 Cl − ε red = + 1.36 V I 2  2 I − ε red = + 0.54 V Select the true statement. a.Cl 2 will reduce I − to I 2. b.Cl 2 will oxidize I − to I 2. c.I 2 will reduce Cl − to Cl 2. d.I 2 will oxidize Cl 2 to Cl −.

24. © 2015 Pearson Education, Inc. G = Gibbs free energy. n = moles of electrons. F = Faraday constant. E = cell potential. Change in G = ? a.F + nE b.F − nE c.−nFE d.nF − E

25. © 2015 Pearson Education, Inc. G = Gibbs free energy. n = moles of electrons. F = Faraday constant. E = cell potential. Change in G = ? a.F + nE b.F − nE c.−nFE d.nF − E

26. © 2015 Pearson Education, Inc. The Nernst Equation is most useful for determining cell potentials when _______ are nonstandard. a.oxidizing agents b.reducing agents c.ion concentrations d.temperatures

27. © 2015 Pearson Education, Inc. The Nernst Equation is most useful for determining cell potentials when _______ are nonstandard. a.oxidizing agents b.reducing agents c.ion concentrations d.temperatures

28. © 2015 Pearson Education, Inc. In a concentration cell, the half-reactions are a.the same. b.at equilibrium. c.acid–base reactions. d.different colors.

29. © 2015 Pearson Education, Inc. In a concentration cell, the half-reactions are a.the same. b.at equilibrium. c.acid–base reactions. d.different colors.

30. © 2015 Pearson Education, Inc. The electrolyte in a lead-acid automobile battery is _______. a.Pb b.PbO 2 c.PbSO 4 d.H 2 SO 4

31. © 2015 Pearson Education, Inc. The electrolyte in a lead-acid automobile battery is _______. a.Pb b.PbO 2 c.PbSO 4 d.H 2 SO 4

32. © 2015 Pearson Education, Inc. A cell that uses external energy to produce an oxidation–reduction reaction is called _______ cell. a.a galvanic b.a voltaic c.an electrolytic d.a prison

33. © 2015 Pearson Education, Inc. A cell that uses external energy to produce an oxidation–reduction reaction is called _______ cell. a.a galvanic b.a voltaic c.an electrolytic d.a prison

34. © 2015 Pearson Education, Inc. Reduction occurs at the a.anode, in both galvanic and electrolytic cells. b.cathode, in both galvanic and electrolytic cells. c.anode in galvanic cells and cathode in electrolytic cells. d.cathode in galvanic cells and anode in electrolytic cells.

35. © 2015 Pearson Education, Inc. Reduction occurs at the a.anode, in both galvanic and electrolytic cells. b.cathode, in both galvanic and electrolytic cells. c.anode in galvanic cells and cathode in electrolytic cells. d.cathode in galvanic cells and anode in electrolytic cells.

36. © 2015 Pearson Education, Inc. Oxidation occurs at the a.anode, in both galvanic and electrolytic cells. b.cathode, in both galvanic and electrolytic cells. c.anode in galvanic cells and cathode in electrolytic cells. d.cathode in galvanic cells and anode in electrolytic cells.

37. © 2015 Pearson Education, Inc. Oxidation occurs at the a.anode, in both galvanic and electrolytic cells. b.cathode, in both galvanic and electrolytic cells. c.anode in galvanic cells and cathode in electrolytic cells. d.cathode in galvanic cells and anode in electrolytic cells.

38. © 2015 Pearson Education, Inc. Q = charge in coulombs I = current in amperes t = time in seconds Which is true? a.Q = I + t b.Q = I − t c.Q = It d.Q = I / t

39. © 2015 Pearson Education, Inc. Q = charge in coulombs I = current in amperes t = time in seconds Which is true? a.Q = I + t b.Q = I − t c.Q = It d.Q = I / t

40. © 2015 Pearson Education, Inc. Corrosion of metals can be prevented by all of the following methods except a.a sacrificial anode. b.a salt bridge. c.formation of an oxide coating. d.paint.

41. © 2015 Pearson Education, Inc. Corrosion of metals can be prevented by all of the following methods except a.a sacrificial anode. b.a salt bridge. c.formation of an oxide coating. d.paint.