Relative Strengths of Oxidizing and Reducing Agents
This presentation is the property of its rightful owner.
Sponsored Links
1 / 12

Relative Strengths of Oxidizing and Reducing Agents PowerPoint PPT Presentation


  • 57 Views
  • Uploaded on
  • Presentation posted in: General

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.

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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


Relative strengths of oxidizing and reducing agents

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.


Relative strengths of oxidizing and reducing agents

Brief Activity Series


Relative strengths of oxidizing and reducing agents

Strong Reducing Agent.


Relative strengths of oxidizing and reducing agents

Strong Oxidizing Agent


Relative strengths of oxidizing and reducing agents

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.


Relative strengths of oxidizing and reducing agents

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


Relative strengths of oxidizing and reducing agents

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.


Relative strengths of oxidizing and reducing agents

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


Relative strengths of oxidizing and reducing agents

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


  • Login