Question

Which of the following metal cations is the strongest oxidizing agent?

a) Cu2+; EoCu2+/Cu = + 0.34 V

b) Al3+; EoAl3+/Al = -1.66 V

c) Sn2+; EoSn2+/Sn = -0.14 V

d) Ag+; EoAg+/Ag = + 0.80 V

e) Mn2+; EoMn2+/Mn = -1.18 V

Answer 1

The strongest oxidizing agent from the options given is Ag+, which has the highest standard reduction potential (+0.80 V) among the metals listed.

Step-by-step explanation:

The question asks which metal cation listed is the strongest oxidizing agent. An oxidizing agent gains electrons and is reduced in a chemical reaction, meaning it has a greater tendency to take on electrons. The strength of an oxidizing agent is directly related to its standard electrode potential value (Eo), with higher values indicating a stronger oxidizing agent.

Comparing the Eo values provided:

• Cu2+; EoCu2+/Cu = +0.34 V
• Al3+; EoAl3+/Al = -1.66 V
• Sn2+; EoSn2+/Sn = -0.14 V
• Ag+; EoAg+/Ag = +0.80 V
• Mn2+; EoMn2+/Mn = -1.18 V

Out of these, Ag+ has the highest standard reduction potential of +0.80 V. Therefore, Ag+ is the strongest oxidizing agent from the options given.

Answer 2

Answer: Option (d) is the correct answer.

Step-by-step explanation:

An oxidizing agent is defined as the substance that itself gains an electron and helps in oxidation of another substance.

For example,
`Ag^(+) + 1e^(-) \rightarrow Ag`

Here,
`Ag^(+)` is the oxidizing agent.

Also, a substance with more positive value of electrode potential will be the strongest oxidizing agent. Whereas a substance with more negative value of electrode potential will be the strongest reducing agent.

Therefore, out of the given options
`Ag^(+)` has the highest positive value of electrode potential so,
`Ag^(+)` is the strongest oxidizing agent.