Oxidation and Reduction Reactions Workbook

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Worksheets Quiz

1. Oxidation, Reduction, Agents, & Reactions. WS 1

2. Lab: The Strength of Oxidizing Agents.

3. Oxidation Numbers Spontaneous Reactions WS 2 1

4. Oxidation Numbers, Application to Reactions. WS 3

5. Balancing Redox Half Reactions Acid/Base. WS 4 2

6. Balancing Redox Reactions in Acid/Base. WS 5

7. Standard Potentials Using Chart. WS 6 3

8. Electrochemical Cells. WS 7

9. Electrochemical Cells Lab.

10. Electrolytic Cells. WS 8 4

11. Electrolytic Cells Lab.

12. Application of Electrolytic Cells. WS 9 5

13. Application of Electrochemical Cells: Bat & Cor. WS 10 6

14. Breathalyzer and review. Internet Review Quizmebc

15. Review Practice Test # 1

16. Review Practice Test # 2

17. Test.

Text book Hebden Read Unit V

If you want an A in this class you need to do this!!

Redox Half Reactions and Reactions WS #1

Define each

1. Oxidation - loss of electrons

2. Reduction - gain of electrons

3. Oxidizing agent - causes oxidation by undergoing reduction

4. Reducing agent - causes reduction by undergoing oxidation

Write half reactions for each of the following atoms or ions. Label each as oxidation or reduction.

5. Al -----------> Al³⁺ + 3e^- oxidation

6. S + 2e^- ---------> S^2- reduction

7. 2O^2- ----------> O₂ + 4e^- oxidation

8. Ba²⁺ + 2e^- -----------> Ba reduction

9. 2N^3- ----------> N₂ + 6e^- oxidation

10. Br₂ + 2e^- ---------> 2Br^- reduction

11. P + 3e^- ----------> P^3- reduction

12. Ca -----------> Ca²⁺ + 2e^- oxidation

13 Ga³⁺ + 3e^- -----------> Ga reduction

14. S + 2e^- ---------> S^2- reduction

15. H₂ ---------> 2H⁺ + 2e^- oxidation

16. 2H⁺ + 2e^- ---------> H₂ reduction

17. 2F^- ----------> F₂ + 2e^- oxidation

18. P^3- ----------> P + 3e^- oxidation

Balance each spontaneous redox equation. Identify the entities reduced and oxidized. State the reducing agent and the oxidizing agent.

19. Al & Zn²⁺

2Al + 3Zn²⁺ → 2Al³⁺ + 3Zn

oxidized reduced

reducing agent oxidizing agent

20. F₂ & O^2-

2F₂ + 2O^2- → 4F^- + O₂

reduced oxidized

oxidizing agent reducing agent

21. O₂ & Ca

2Ca + O₂ → 2Ca²⁺ + 2O^2-

oxidized reduced

reducing agent oxidizing agent

22. Al³⁺ & Li

Al³⁺ + 3Li → Al + 3Li⁺

reduced oxidized

oxidizing agent reducing agent

Label the species that is reduced, that is oxidized, the reducing agent and the oxidizing agent.

23. Fe²⁺ + Co → Co²⁺ + Fe

Co → Co²⁺ + 2e^- oxidation Fe²⁺ + 2e- → Fe reduction

24. 3 Ag⁺ + Ni → Ni³⁺ + 3 Ag

Ni → Ni²⁺ + 2e^- oxidation Ag⁺ + 1e- → Ag reduction

25. Cu²⁺ + Pb → Pb²⁺ + Cu

Pb → Pb²⁺ + 2e^- oxidation Cu²⁺ + 2e- → Cu reduction

26. O₂ + 2 Sn → O^2- + 2 Sn²⁺

Sn → Sn²⁺ + 2e^- oxidation O₂ + 4e- → 2O^2- reduction

27. Co²⁺ + 2 F^- → Co + F₂

2F^- → F₂ + 2e^- oxidation Co²⁺ + 2e- → Co reduction

28. List the species (formulas from above) that lose electrons:

Co Ni Pb Sn F^-

29. List the species (formulas from above) that gain electrons:

Fe²⁺ Ag⁺ Cu²⁺ O₂ Co²⁺

For each of the following reactions, identify:

-The Oxidizing Agent.

-The Reducing Agent.

-The Substance Oxidized.

-The Substance Reduced.

30. I^- + Cl₂ ----------> Cl^- + I₂

Substance oxidized I^- Reducing agent I^-

Oxidizing agent Cl₂ Substance reduced Cl₂

31. Co + Fe³⁺ -----------> Co²⁺ + Fe²⁺

Substance oxidized Co Reducing agent Co

Oxidizing agent Fe³⁺ Substance reduced Fe³⁺

32. Cr⁶⁺ + Fe²⁺ -----------> Cr³⁺ + Fe³⁺

Substance oxidized Fe²⁺ Reducing agent Fe²⁺

Oxidizing agent Cr⁶⁺ Substance reduced Cr⁶⁺

Redox Half Reactions and Reactions WS #2

1. State the Oxidation Number of each of the elements that is underlined.

a) NH₃ -3 b) H₂SO₄ 6

c) ZnSO₃ 4 d) Al(OH)₃ 3

e) Na 0 f) Cl₂ 0

g) AgNO₃ 5 h) ClO₄^- 7

i) SO₂ 4 j) K₂Cr₂O₄ 3

k) Ca(ClO₃)₂ 5 l) K₂Cr₂O₇ 6

m) HPO₃^2- 3 n) HClO 1

o) MnO₂ 4 p) KClO₃ 5

q) PbO₂ 4 r) PbSO₄ 2

s) K₂SO₄ 6 t) NH₄⁺ -3

u) Na₂O₂ -1 v) FeO 2

w) Fe₂O₃ 3 x) SiO₄^4- -2

y) NaIO₃ 5 z) ClO₃^- 5

aa) NO₃^- 5 bb) Cr(OH)₄ 4

cc) CaH₂ -1 dd) Pt(H₂0)₅(0H)²⁺ +3

ee) Fe(H₂O)₆³⁺ +3 ff) CH₃COOH 0

2. What is the oxidation number of carbon in each of the following substances?

a) CO 2 b) C 0

c) CO₂ 4 d) CO₃^2- 4

e) C₂H₆ -3 f) CH₃OH -2

3. For each of the following reactions, identify: the oxidizing agent, the reducing agent, the substance oxidized and the substance reduced.

a) Cu²⁺ _(aq) + Zn _(s) --------> Cu _(s) + Zn²⁺ _(aq)

Substance oxidized Zn Substance reduced Cu²⁺

Oxidizing agent Cu²⁺ Reducing agent Zn

b) Cl_{2 (g)} + 2 Na _(s) --------> 2 Na+ _(aq) + 2 Cl^- _(aq)

Substance oxidized Na Substance reduced Cl₂

Oxidizing agent Cl₂ Reducing agent Na

WS # 3 Spontaneous and Non-spontaneous Redox Reactions

Describe each reaction as spontaneous or non-spontaneous.

1. Au⁺³ + Fe⁺³ -----> Fe⁺² + Au nonspontaneous (two oxidizing agents)

2. Pb + Fe⁺³ ------> Fe⁺² + Pb⁺² spontaneous

3. Cl₂ + F^- ------> F₂ + 2Cl^- nonspontaneous

4. S₂O₈^-2 + Pb ------> 2SO₄^-2 + Pb⁺² spontaneous

5.Cu⁺² + 2Br^- ------> Cu + Br₂ nonspontaneous

6. Sn⁺² + Br₂ ------> Sn⁺⁴ + 2Br^- spontaneous

7. Pb⁺² + Fe⁺² ------> Fe⁺³ + Pb nonspontaneous

8. Can you keep 1 M HCl in an iron container. If the answer is no, write a balanced equation for the reaction that would occur. No

Fe + 2H⁺ --------> Fe²⁺ + H₂

9. Can you keep 1 M HCl in an Ag container. If the answer is no, write a balanced equation for the reaction that would occur.

Yes. There is no reaction.

10. Can you keep 1 M HNO₃ in an Ag container. If the answer is no, write a balanced equation for the reaction that would occur. (remember HNO₃ consists of two ions H⁺ and NO₃^-)

No 3Ag + NO₃^- + 4H⁺ --------> 3Ag⁺ + NO + 2H₂O

11. Can you keep 1 M HNO₃ in an Au container. If the answer is no, write a balanced equation for the reaction that would occur. (Remember, HNO₃ consists of two ions H⁺ and NO₃^-)

Yes. There is no reaction.