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Basic Chemistry, 4/e Chapter 15: Oxidation and Reduction

This chapter delves into the fundamentals of oxidation and reduction reactions, including determining oxidation numbers and identifying oxidizing and reducing agents. Explore key concepts in redox chemistry.

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Basic Chemistry, 4/e Chapter 15: Oxidation and Reduction

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  1. Basic Chemistry, 4/eChapter 15: Oxidation and Reduction Karen Timberlake

  2. Chapter 15 – Oxidation and Reduction 1. The oxidation number for chlorine in ClO3– is A. +7. B. +6. C. +5. D. –5.

  3. Chapter 15 – Oxidation and Reduction 1. The oxidation number for chlorine in ClO3– is A. +7. B. +6. C. +5. D. –5.

  4. Chapter 15 – Oxidation and Reduction 2. All of the following can have an oxidation number of +4 except A. carbon. B. iron. C. lead. D. tin.

  5. Chapter 15 – Oxidation and Reduction 2. All of the following can have an oxidation number of +4 except A. carbon. B. iron. C. lead. D. tin.

  6. Chapter 15 – Oxidation and Reduction 3. The oxidation number of an element in the free or uncombined state is always A. 0. B. +1. C. –1. D. the same as its ionic charge.

  7. Chapter 15 – Oxidation and Reduction 3. The oxidation number of an element in the free or uncombined state is always A. 0. B. +1. C. –1. D. the same as its ionic charge.

  8. Chapter 15 – Oxidation and Reduction 4. A substance is oxidized if it A. gains oxygen atoms. B. gains hydrogen atoms. C. gains electrons. D. None of these

  9. Chapter 15 – Oxidation and Reduction 4. A substance is oxidized if it A. gains oxygen atoms. B. gains hydrogen atoms. C. gains electrons. D. None of these

  10. Chapter 15 – Oxidation and Reduction 5. In the reaction C2H4 + H20  C2H6O, carbon is A. oxidized. B. reduced. C. neither oxidized nor reduced.

  11. Chapter 15 – Oxidation and Reduction 5. In the reaction C2H4 + H20  C2H6O, carbon is A. oxidized. B. reduced. C. neither oxidized nor reduced.

  12. Chapter 15 – Oxidation and Reduction 6. In the reaction N2 + 2 H2O  NH4+ + NO2–, nitrogen is A. oxidized. B. reduced. C. neither oxidized nor reduced. D. both oxidized and reduced.

  13. Chapter 15 – Oxidation and Reduction 6. In the reaction N2 + 2 H2O  NH4+ + NO2–, nitrogen is A. oxidized. B. reduced. C. neither oxidized nor reduced. D. both oxidized and reduced.

  14. Chapter 15 – Oxidation and Reduction 7. What element is oxidized in the following equation, and what element is reduced? I2 + 2 Br – 2 I – + Br2 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.

  15. Chapter 15 – Oxidation and Reduction 7. What element is oxidized in the following equation, and what element is reduced? I2 + 2 Br – 2 I – + Br2 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.

  16. 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? I2 + 2 Br – 2 I – + Br2 A. The I2 is the oxidizing agent, while the Br– is the reducing agent. B. The I2 is the reducing agent, while the Br– is the oxidizing agent. C. The I– is the oxidizing agent, while the Br2 is the reducing agent. D. The I– is the reducing agent, while the Br2 is the oxidizing agent.

  17. 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? I2 + 2 Br – 2 I – + Br2 A. The I2 is the oxidizing agent, while the Br– is the reducing agent. B. The I2 is the reducing agent, while the Br– is the oxidizing agent. C. The I– is the oxidizing agent, while the Br2 is the reducing agent. D. The I– is the reducing agent, while the Br2 is the oxidizing agent.

  18. Chapter 15 – Oxidation and Reduction 9. Which compound can be either an oxidizing agent or a reducing agent? A. H2O2 B. KMnO4 C. Na2Cr2O7 D. HNO3

  19. Chapter 15 – Oxidation and Reduction 9. Which compound can be either an oxidizing agent or a reducing agent? A. H2O2 B. KMnO4 C. Na2Cr2O7 D. HNO3

  20. Chapter 15 – Oxidation and Reduction 10. Hydrogen peroxide used as an oxidizing agent is reduced to A. O2. B. H2O. C. H2O2. D. H2.

  21. Chapter 15 – Oxidation and Reduction 10. Hydrogen peroxide used as an oxidizing agent is reduced to A. O2. B. H2O. C. H2O2. D. H2.

  22. Chapter 15 – Oxidation and Reduction 11. In a lead storage battery (car battery), the electrolyte is A. lead. B. hydrogen. C. lead (IV) oxide. D. sulfuric acid.

  23. Chapter 15 – Oxidation and Reduction 11. In a lead storage battery (car battery), the electrolyte is A. lead. B. hydrogen. C. lead (IV) oxide. D. sulfuric acid.

  24. Chapter 15 – Oxidation and Reduction 12. Which of the following uses spontaneous oxidation-reduction reactions to produce electrical energy? A. Voltaic cell B. Electroplating C. Electrolytic cell D. Electrolysis

  25. Chapter 15 – Oxidation and Reduction 12. Which of the following uses spontaneous oxidation-reduction reactions to produce electrical energy? A. Voltaic cell B. Electroplating C. Electrolytic cell D. Electrolysis

  26. Chapter 15 – Oxidation and Reduction • What set of coefficients is necessary to balance the following chemical equation? __Ce4+ + __Cl– __Ce3+ + __Cl2 A. 2, 2, 2, 1 B. 1, 4, 1, 2 C. 1, 2, 1, 1 D. 3, 4, 3, 2

  27. Chapter 15 – Oxidation and Reduction • What set of coefficients is necessary to balance the following chemical equation? __Ce4+ + __Cl– __Ce3+ + __Cl2 A. 2, 2, 2, 1 B. 1, 4, 1, 2 C. 1, 2, 1, 1 D. 3, 4, 3, 2

  28. Chapter 15 – Oxidation and Reduction 14. Describe the following reaction in a battery. Zn(s) + 2 OH–(aq)  ZnO(s) + H2O(l) + 2e– 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.

  29. Chapter 15 – Oxidation and Reduction 14. Describe the following reaction in a battery. Zn(s) + 2 OH–(aq)  ZnO(s) + H2O(l) + 2e– 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.

  30. Chapter 15 – Oxidation and Reduction 15. Describe the following reaction in a battery. 2 MnO2(s) +H2O(l) + 2e– Mn2O3(s) + 2 H2O(aq) A. MnO2 is oxidized at the anode. B. MnO2 is oxidized at the cathode. C. MnO2 is reduced at the anode. D. MnO2 is reduced at the cathode.

  31. Chapter 15 – Oxidation and Reduction 15. Describe the following reaction in a battery. 2 MnO2(s) +H2O(l) + 2e– Mn2O3(s) + 2 H2O(aq) A. MnO2 is oxidized at the anode. B. MnO2 is oxidized at the cathode. C. MnO2 is reduced at the anode. D. MnO2 is reduced at the cathode.

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