1. Relative Strengths of Oxidizing and Reducing Agents

2. non-metals: gain electrons and are good oxidizing agents. metals: lose electrons and are good reducing agents.

3. Brief Activity Series

4. Strong Reducing Agent.

5. Strong Oxidizing Agent

6. Li + (aq) + e - ↔ Li(s) E o = -3.04 V (non-spontaneous as written) Li + (aq) + e - → Li(s) E o = -3.04 V (non-spontaneous) Li + is acting as a oxidizing agent (gaining an electron), but the negative sign shows this to be a non-spontaneous reaction. Li(s) → Li + (aq) + e - E o = +3.04 V (spontaneous) Li(s) is acting as a reducing agent (losing an electron) and the positive sign shows this to be a spontaneous reaction. So Li(s) makes a much better reducing agent than Li + (aq) makes as an oxidizing agent.

7. Li + (aq) + e - ↔ Li(s) E o = -3.04 V (non-spontaneous as written) Li + (aq) + e - → Li(s) E o = -3.04 V (non-spontaneous) Li + is acting as a oxidizing agent (gaining an electron), but the negative sign shows this to be a non-spontaneous reaction. Li(s) → Li + (aq) + e - E o = +3.04 V (spontaneous) Li(s) is acting as a reducing agent (losing an electron) and the positive sign shows this to be a spontaneous reaction. Zn 2+ (aq) + 2e - ↔ Zn(s) E o = -0.76 V (non-spontaneous as written Zn 2+ (aq) + 2e - → Zn(s) E o = -0.76 V Zn 2+ is acting as an oxidizing agent. Is it a stronger or weaker oxidizing agent than Li + ? stronger,less negative Zn(s) → Zn 2+ (aq) + 2e - E o = +0.76 V Zn(s) is acting as a reducing agent. Is it a stronger or weaker reducing agent than Li(s)? Weaker, +3.04 > +0.76

8. Li(s) can reduce Zn 2+ (aq) or Zn 2+ (aq) can oxidize Li(s) 2Li(s) + Zn 2+ (aq) → 2Li + (aq) + Zn(s) E o cell = +3.04 + -0.76 = +2.28 V What can be said about Mg(s) and Al 3+ (aq)? What about Al 3+ (aq) and Zn 2+ (aq)? Mg(s) can reduce Al 3+ (aq) or Al 3+ (aq) can oxidize Mg(s). Nothing will happen, they are both fully oxidized.

10. Cr(s) can give electrons (reduce) any of the ions below it.

11. Cd 2+ can (oxidize) gain electrons from the elements above.