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2. Standardized Test Prep
Resources
Chapter Presentation
Lesson Starters
Transparencies
Sample Problems
Visual Concepts
Standardized Test Prep

3. Chapter 19 Table of Contents Section 1 Oxidation and Reduction
Oxidation-Reduction Reactions
Chapter 19
Table of Contents
Section 1 Oxidation and Reduction
Section 2 Balancing Redox Equations
Section 3 Oxidizing and Reducing Agents

4. Section 1 Oxidation and Reduction
Chapter 19
Objectives
Assign oxidation numbers to reactant and product species.
Define oxidation and reduction.
Explain what an oxidation-reduction reaction (redox reaction) is.

5. Chapter 19 Oxidation States
Section 1 Oxidation and Reduction
Chapter 19
Oxidation States
The oxidation number assigned to an element in a molecule is based on the distribution of electrons in that molecule.
The rules by which oxidation numbers are assigned are summarized on the next slide.

6. Rules for Assigning Oxidation Numbers
Section 1 Oxidation and Reduction
Chapter 19
Rules for Assigning Oxidation Numbers

7. Assigning Oxidation Numbers
Section 1 Oxidation and Reduction
Chapter 19
Assigning Oxidation Numbers

8. Rules for Assigning Oxidation Numbers
Visual Concepts
Chapter 19
Rules for Assigning Oxidation Numbers
Click below to watch the Visual Concept.
Visual Concept

9. Section 1 Oxidation and Reduction
Chapter 19
Oxidation
Reactions in which the atoms or ions of an element experience an increase in oxidation state are oxidation processes.
A species whose oxidation number increases is oxidized.

10. Chapter 19 Oxidation Visual Concepts
Click below to watch the Visual Concept.
Visual Concept

11. Section 1 Oxidation and Reduction
Chapter 19
Reduction
Reactions in which the oxidation state of an element decreases are reduction processes.
A species that undergoes a decrease in oxidation state is reduced.

12. Chapter 19 Reduction Visual Concepts
Click below to watch the Visual Concept.
Visual Concept

13. Oxidation and Reduction as a Process
Section 1 Oxidation and Reduction
Chapter 19
Oxidation and Reduction as a Process
Any chemical process in which elements undergo changes in oxidation number is an oxidation-reduction reaction.
This name is often shortened to redox reaction.
The part of the reaction involving oxidation or reduction alone can be written as a half-reaction.

14. Oxidation and Reduction as a Process, continued
Section 1 Oxidation and Reduction
Chapter 19
Oxidation and Reduction as a Process, continued
Equations for the reaction between nitric acid and copper illustrate the relationship between half-reactions and the overall redox reaction.
(oxidation half-reaction)
(reduction half-reaction)
(redox reaction)

15. Section 1 Oxidation and Reduction
Chapter 19
Oxidation and Reduction as a Process, continued Redox Reactions and Covalent Bonds
When hydrogen burns in chlorine, a covalent bond forms from the sharing of two electrons.
The pair of electrons is more strongly attracted to the chlorine atom because of its higher electronegativity.

16. Section 1 Oxidation and Reduction
Chapter 19
Oxidation and Reduction as a Process, continued Redox Reactions and Covalent Bonds, continued
Neither atom has totally lost or totally gained any electrons.
Hydrogen has donated a share of its bonding electron to the chlorine but has not completely transferred that electron.

17. Particle Model for a Redox Reaction
Section 1 Oxidation and Reduction
Chapter 19
Particle Model for a Redox Reaction

18. Half-Reaction Equation
Visual Concepts
Chapter 19
Half-Reaction Equation
Click below to watch the Visual Concept.
Visual Concept

19. Section 2 Balancing Redox Equations
Chapter 19
Objectives
Explain what must be conserved in redox equations.
Balance redox equations by using the half-reaction method.

20. Chapter 19 Half-Reaction Method
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method
The half-reaction method for balancing redox equations consists of seven steps:
1. Write the formula equation if it is not given in the problem. Then write the ionic equation.
2. Assign oxidation numbers. Delete substances containing only elements that do not change oxidation state.

21. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
3. Write the half-reaction for oxidation.
Balance the atoms.
Balance the charge.
4. Write the half-reaction for reduction.

22. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
5. Conserve charge by adjusting the coefficients in front of the electrons so that the number lost in oxidation equals the number gained in reduction.
6. Combine the half-reactions, and cancel out anything common to both sides of the equation.
7. Combine ions to form the compounds shown in the original formula equation. Check to ensure that all other ions balance.

23. Balancing Redox Equations Using the Half-Reaction Method
Section 2 Balancing Redox Equations
Chapter 19
Balancing Redox Equations Using the Half-Reaction Method

24. Balancing Redox Equations Using the Half-Reaction Method
Section 2 Balancing Redox Equations
Chapter 19
Balancing Redox Equations Using the Half-Reaction Method

25. Rules for the Half-Reaction Method
Visual Concepts
Chapter 19
Rules for the Half-Reaction Method
Click below to watch the Visual Concept.
Visual Concept

26. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A
A deep purple solution of potassium permanganate is titrated with a colorless solution of iron(II) sulfate and sulfuric acid. The products are iron(III) sulfate, manganese(II) sulfate, potassium sulfate, and water—all of which are colorless. Write a balanced equation for this reaction.

27. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution
1. Write the formula equation if it is not given in the problem. Then write the ionic equation.

28. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
2. Assign oxidation numbers to each element and ion. Delete substances containing an element that does not change oxidation state.
Only ions or molecules whose oxidation numbers change are retained.

29. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
3. Write the half-reaction for oxidation. The iron shows the increase in oxidation number. Therefore, it is oxidized.
Balance the mass.
The mass is already balanced.
Balance the charge.

30. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
4. Write the half-reaction for reduction. Manganese is reduced.
Balance the mass.
Water and hydrogen ions must be added to balance the oxygen atoms in the permanganate ion.
Balance the charge.

31. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
5. Adjust the coefficients to conserve charge.

32. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
6. Combine the half-reactions and cancel.

33. Half-Reaction Method, continued
Section 2 Balancing Redox Equations
Chapter 19
Half-Reaction Method, continued
Sample Problem A Solution, continued
7. Combine ions to form compounds from the original equation.

34. Chapter 19 Lesson Starter
Section 3 Oxidizing and Reducing Agents
Chapter 19
Lesson Starter
Label a small object (such as an empty box) “electrons.”
Ask another student to take the electrons from you.
The other student was the agent of your losing the electrons and you were the agent of the other student’s gaining the electrons.

35. Lesson Starter, continued
Section 3 Oxidizing and Reducing Agents
Chapter 19
Lesson Starter, continued
By causing you to lose your electrons, the other student is the oxidizing agent.
You are the reducing agent because you caused the student to gain electrons.
The student is reduced by you, and you are oxidized by the other student.

36. Section 3 Oxidizing and Reducing Agents
Chapter 19
Objectives
Relate chemical activity to oxidizing and reducing strength.
Explain the concept of disproportionation.

37. Section 3 Oxidizing and Reducing Agents
Chapter 19
A reducing agent is a substance that has the potential to cause another substance to be reduced.
An oxidizing agent is a substance that has the potential to cause another substance to be oxidized.

38. Strengths of Oxidizing and Reducing Agents, continued
Section 3 Oxidizing and Reducing Agents
Chapter 19
Strengths of Oxidizing and Reducing Agents, continued

39. Strengths of Oxidizing and Reducing Agents, continued
Section 3 Oxidizing and Reducing Agents
Chapter 19
Strengths of Oxidizing and Reducing Agents, continued
Different substances can be compared and rated by their relative potential as reducing and oxidizing agents.
The negative ion of a strong oxidizing agent is a weak reducing agent.
The positive ion of a strong reducing agent is a weak oxidizing agent.

40. Chapter 19 Disproportionation
Section 3 Oxidizing and Reducing Agents
Chapter 19
Disproportionation
A process in which a substance acts as both an oxidizing agent and a reducing agent is called disproportionation.
A substance that undergoes disproportionation is both self-oxidizing and self-reducing.
example: Hydrogen peroxide is both oxidized and reduced

41. End of Chapter 19 Show

42. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
1. In the following reaction, which species is reduced?
A. K
B. Br2
C. All of the above
D. None of the above

43. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
1. In the following reaction, which species is reduced?
A. K
B. Br2
C. All of the above
D. None of the above

44. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
2. The oxidation number of the sulfur atom in the
A. +2.
B. 2.
C. +6.
D. +4.

45. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
2. The oxidation number of the sulfur atom in the
A. +2.
B. 2.
C. +6.
D. +4.

46. Chapter 19 Multiple Choice 3. A half-reaction
Standardized Test Preparation
Chapter 19
Multiple Choice
3. A half-reaction
A. involves a change in the oxidation state of an element.
B. always contains H2O molecules.
C. always contains H+ ions.
D. All of the above

47. Chapter 19 Multiple Choice 3. A half-reaction
Standardized Test Preparation
Chapter 19
Multiple Choice
3. A half-reaction
A. involves a change in the oxidation state of an element.
B. always contains H2O molecules.
C. always contains H+ ions.
D. All of the above

48. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
4. In the following reaction, which is the oxidizing agent?
A. AgNO2
B. Cl2
C. KOH
D. KCl

49. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
4. In the following reaction, which is the oxidizing agent?
A. AgNO2
B. Cl2
C. KOH
D. KCl

50. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
5. What are the oxidation states (in increasing order) of the element that undergoes disproportionation in the following reaction:
A. 1, 0, +2
B. 1, 0, +1
C. 2, 1, 0
D. None of the above

51. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
5. What are the oxidation states (in increasing order) of the element that undergoes disproportionation in the following reaction:
A. 1, 0, +2
B. 1, 0, +1
C. 2, 1, 0
D. None of the above

52. Chapter 19 Multiple Choice 6. Which reaction is a redox reaction? A.
Standardized Test Preparation
Chapter 19
Multiple Choice
6. Which reaction is a redox reaction? A. B. C. D.

53. Chapter 19 Multiple Choice 6. Which reaction is a redox reaction? A.
Standardized Test Preparation
Chapter 19
Multiple Choice
6. Which reaction is a redox reaction? A. B. C. D.

54. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
7. Arrange the following in order of increasing oxidation number of the sulfur atom: A. B. C. D.

55. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
7. Arrange the following in order of increasing oxidation number of the sulfur atom: A. B. C. D.

56. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
8. Which answer contains the correct information about the following reaction:
A. This reaction is a decomposition reaction and not a redox reaction.
B. This reaction is a redox reaction in which the lead is reduced and the oxygen is oxidized.
C. This reaction is a disproportionation reaction.
D. This reaction is a redox reaction in which the nitrogen is reduced and the oxygen is oxidized.

57. Chapter 19 Multiple Choice
Standardized Test Preparation
Chapter 19
Multiple Choice
8. Which answer contains the correct information about the following reaction:
A. This reaction is a decomposition reaction and not a redox reaction.
B. This reaction is a redox reaction in which the lead is reduced and the oxygen is oxidized.
C. This reaction is a disproportionation reaction.
D. This reaction is a redox reaction in which the nitrogen is reduced and the oxygen is oxidized.

58. Standardized Test Preparation
Chapter 19
Short Answer
9. Determine the oxidation numbers for Cu in the superconductor YBa2Cu3O7.Yttrium (Y) has an oxidation number of +3. (Cu does not have oxidation numbers greater than +3.) Give only integer oxidation numbers.

59. Standardized Test Preparation
Chapter 19
Short Answer
9. Determine the oxidation numbers for Cu in the superconductor YBa2Cu3O7.Yttrium (Y) has an oxidation number of +3. (Cu does not have oxidation numbers greater than +3.) Give only integer oxidation numbers.
Answer: The oxidation numbers for Y, Ba, and O are +3, +2, and 2, respectively. Therefore, the sum of the oxidation numbers for the three Cu atoms must be +7. Two Cu atoms must have +2 oxidation states, and one Cu atom must have a +3 oxidation state.

60. Chapter 19 Short Answer 10. What is an oxidizing agent?
Standardized Test Preparation
Chapter 19
Short Answer
10. What is an oxidizing agent?

61. Chapter 19 Short Answer 10. What is an oxidizing agent?
Standardized Test Preparation
Chapter 19
Short Answer
10. What is an oxidizing agent?
Answer: An oxidizing agent is a species that causes another species to be oxidized in a redox reaction. An oxidizing agent is therefore reduced in a redox reaction.

62. Chapter 19 Extended Response
Standardized Test Preparation
Chapter 19
Extended Response
11. B, F, K, and L are four unknown reducing agents that oxidize to singly charged cations. Using the following information, construct a table showing the relative strengths of the oxidizing and reducing agents. Data: F reduces K+, B+, and L+. B+ oxidizes K and F, but not L.

63. Chapter 19 Extended Response Answer: Reducing agents Oxidizing F K B L
Standardized Test Preparation
Chapter 19
Extended Response
11. B, F, K, and L are four unknown reducing agents that oxidize to singly charged cations. Using the following information, construct a table showing the relative strengths of the oxidizing and reducing agents. Data: F reduces K+, B+, and L+. B+ oxidizes K and F, but not L.
Answer:
Reducing
agents
Oxidizing F K B L F+ K+ B+ L+

64. Chapter 19 Extended Response
Standardized Test Preparation
Chapter 19
Extended Response
12. Balance the equation for the following reaction in basic solution:
Give the balanced equation for each half-reaction and for the overall reaction. Give the oxidizing agent and the reducing agent.

65. Chapter 19 Extended Response Standardized Test Preparation
12. Balance the equation for the following reaction in basic solution:
Give the balanced equation for each half-reaction and for the overall reaction. Give the oxidizing agent and the reducing agent.
Answer:
Oxidation half-reaction:
Reduction half-reaction:
Overall reaction:
This reaction is a disproportionation reaction; therefore, ClO2 is
both the reducing agent and the oxidizing agent.