Basic Chemistry 4e Chapter 15 Oxidation and Reduction
Basic Chemistry, 4/e Chapter 15: Oxidation and Reduction Karen Timberlake © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 1. The oxidation number for chlorine in Cl. O 3– is A. B. C. D. +7. +6. +5. – 5. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 1. The oxidation number for chlorine in Cl. O 3– is A. B. C. D. +7. +6. +5. – 5. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 2. All of the following can have an oxidation number of +4 except A. B. C. D. carbon. iron. lead. tin. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 2. All of the following can have an oxidation number of +4 except A. B. C. D. carbon. iron. lead. tin. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 3. The oxidation number of an element in the free or uncombined state is always A. B. C. D. 0. +1. – 1. the same as its ionic charge. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 3. The oxidation number of an element in the free or uncombined state is always A. B. C. D. 0. +1. – 1. the same as its ionic charge. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 4. A substance is oxidized if it A. B. C. D. gains oxygen atoms. gains hydrogen atoms. gains electrons. None of these © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 4. A substance is oxidized if it A. B. C. D. gains oxygen atoms. gains hydrogen atoms. gains electrons. None of these © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 5. In the reaction C 2 H 4 + H 20 C 2 H 6 O, carbon is A. oxidized. B. reduced. C. neither oxidized nor reduced. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 5. In the reaction C 2 H 4 + H 20 C 2 H 6 O, carbon is A. oxidized. B. reduced. C. neither oxidized nor reduced. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 6. In the reaction N 2 + 2 H 2 O NH 4+ + NO 2–, nitrogen is A. B. C. D. oxidized. reduced. neither oxidized nor reduced. both oxidized and reduced. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 6. In the reaction N 2 + 2 H 2 O NH 4+ + NO 2–, nitrogen is A. B. C. D. oxidized. reduced. neither oxidized nor reduced. both oxidized and reduced. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 7. What element is oxidized in the following equation, and what element is reduced? I 2 + 2 Br – 2 I – + Br 2 A. Iodine, I, is oxidized, while the bromine ion, Br–, is reduced. B. Iodine, I, is reduced, while the bromine ion, Br–, is oxidized. C. Both the iodine, I, and the bromine ion, Br–, are reduced. D. Both the iodine, I, and the bromine ion, Br–, are oxidized. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 7. What element is oxidized in the following equation, and what element is reduced? I 2 + 2 Br – 2 I – + Br 2 A. Iodine, I, is oxidized, while the bromine ion, Br–, is reduced. B. Iodine, I, is reduced, while the bromine ion, Br –, is oxidized. C. Both the iodine, I, and the bromine ion, Br–, are reduced. D. Both the iodine, I, and the bromine ion, Br–, are oxidized. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 8. What element behaves as the oxidizing agent in the following equation, and what element behaves as the reducing agent? I 2 + 2 Br – 2 I – + Br 2 A. The I 2 is the oxidizing agent, while the Br– is the reducing agent. B. The I 2 is the reducing agent, while the Br– is the oxidizing agent. C. The I– is the oxidizing agent, while the Br 2 is the reducing agent. D. The I– is the reducing agent, while the Br 2 is the oxidizing agent. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 8. What element behaves as the oxidizing agent in the following equation, and what element behaves as the reducing agent? I 2 + 2 Br – 2 I – + Br 2 A. The I 2 is the oxidizing agent, while the Br– is the reducing agent. B. The I 2 is the reducing agent, while the Br– is the oxidizing agent. C. The I– is the oxidizing agent, while the Br 2 is the reducing agent. D. The I– is the reducing agent, while the Br 2 is the oxidizing agent. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 9. Which compound can be either an oxidizing agent or a reducing agent? A. B. C. D. H 2 O 2 KMn. O 4 Na 2 Cr 2 O 7 HNO 3 © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 9. Which compound can be either an oxidizing agent or a reducing agent? A. B. C. D. H 2 O 2 KMn. O 4 Na 2 Cr 2 O 7 HNO 3 © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 10. Hydrogen peroxide used as an oxidizing agent is reduced to A. B. C. D. O 2. H 2 O 2. H 2. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 10. Hydrogen peroxide used as an oxidizing agent is reduced to A. B. C. D. O 2. H 2 O 2. H 2. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 11. In a lead storage battery (car battery), the electrolyte is A. B. C. D. lead. hydrogen. lead (IV) oxide. sulfuric acid. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 11. In a lead storage battery (car battery), the electrolyte is A. B. C. D. lead. hydrogen. lead (IV) oxide. sulfuric acid. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 12. Which of the following uses spontaneous oxidation-reduction reactions to produce electrical energy? A. B. C. D. Voltaic cell Electroplating Electrolytic cell Electrolysis © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 12. Which of the following uses spontaneous oxidation-reduction reactions to produce electrical energy? A. B. C. D. Voltaic cell Electroplating Electrolytic cell Electrolysis © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 13. What set of coefficients is necessary to balance the following chemical equation? __Ce 4+ + __Cl– __Ce 3+ + __Cl 2 A. 2, 2, 2, 1 B. 1, 4, 1, 2 C. 1, 2, 1, 1 D. 3, 4, 3, 2 © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 13. What set of coefficients is necessary to balance the following chemical equation? __Ce 4+ + __Cl– __Ce 3+ + __Cl 2 A. 2, 2, 2, 1 B. 1, 4, 1, 2 C. 1, 2, 1, 1 D. 3, 4, 3, 2 © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 14. Describe the following reaction in a battery. Zn(s) + 2 OH–(aq) Zn. O(s) + H 2 O(l) + 2 e– A. Zinc is oxidized at the anode. B. Zinc is oxidized at the cathode. C. Zinc is reduced at the anode. D. Zinc is reduced at the cathode. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 14. Describe the following reaction in a battery. Zn(s) + 2 OH–(aq) Zn. O(s) + H 2 O(l) + 2 e– A. Zinc is oxidized at the anode. B. Zinc is oxidized at the cathode. C. Zinc is reduced at the anode. D. Zinc is reduced at the cathode. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 15. Describe the following reaction in a battery. 2 Mn. O 2(s) +H 2 O(l) + 2 e– Mn 2 O 3(s) + 2 H 2 O(aq) A. Mn. O 2 is oxidized at the anode. B. Mn. O 2 is oxidized at the cathode. C. Mn. O 2 is reduced at the anode. D. Mn. O 2 is reduced at the cathode. © 2014 Pearson Education, Inc.
Chapter 15 – Oxidation and Reduction 15. Describe the following reaction in a battery. 2 Mn. O 2(s) +H 2 O(l) + 2 e– Mn 2 O 3(s) + 2 H 2 O(aq) A. Mn. O 2 is oxidized at the anode. B. Mn. O 2 is oxidized at the cathode. C. Mn. O 2 is reduced at the anode. D. Mn. O 2 is reduced at the cathode. © 2014 Pearson Education, Inc.
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