Relative Strengths of Oxidizing and Reducing Agents
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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.

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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

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

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