1 / 12

Relative Strengths of Oxidizing and Reducing Agents

Relative Strengths of Oxidizing and Reducing Agents. metals: lose electrons and are good reducing agents. non-metals: gain electrons and are good oxidizing agents. Brief Activity Series . Strong Reducing Agent. Strong Oxidizing Agent.

arleen
Download Presentation

Relative Strengths of Oxidizing and Reducing Agents

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Relative Strengths of Oxidizing and Reducing Agents

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

  3. Brief Activity Series

  4. Strong Reducing Agent.

  5. Strong Oxidizing Agent

  6. Li+(aq) + e-↔ Li(s) Eo = -3.04 V (non-spontaneous as written) Li+(aq) + e-→ Li(s) Eo = -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- Eo = +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) Eo = -3.04 V (non-spontaneous as written) Zn2+(aq) + 2e-↔ Zn(s) Eo = -0.76 V (non-spontaneous as written Li+(aq) + e-→ Li(s) Eo = -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- Eo = +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. Zn2+(aq) + 2e-→ Zn(s) Eo = -0.76 V Zn2+ is acting as an oxidizing agent. Is it a stronger or weaker oxidizing agent than Li+? stronger,less negative Zn(s) → Zn2+(aq) + 2e- Eo = +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 Zn2+(aq) or Zn2+(aq) can oxidize Li(s) 2Li(s) + Zn2+(aq) → 2Li+(aq) + Zn(s) Eocell= +3.04 + -0.76 = +2.28 V What can be said about Mg(s) and Al3+(aq)? Mg(s) can reduce Al3+(aq) or Al3+(aq) can oxidize Mg(s). What about Al3+(aq) and Zn2+(aq)? Nothing will happen, they are both fully oxidized.

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

  10. Cd2+ can (oxidize) gain electrons from the elements above.

More Related