Question

Among $L{i}^{+}$, $K^{+}$, $N{a}^{+}$ and $A{l}^{3+}$ which will get oxidized first?

• A. $A{l}^{3+}$
• B. $K^{+}$
• C. $N{a}^{+}$
• D. $L{i}^{+}$

Answer 1

The correct option is D $L{i}^{+}$

According to the electrochemical series, metals which are at the top of the series have high negative standard electrode potential values and are good reducing agents, and thus they easily give away electrons.
Metals which are at the bottom of the series have positive standard electrode potential values and are good oxidizing agents, and thus easily accept electrons.
In the electrochemical series, $L{i}^{+}$ is placed just at the top of the series. It has the highest negative electrode potential value. It gives away electrons very easily. Thus $L{i}^{+}$ is the best reducing agent and it gets oxidized most easily.
All other metals are placed below Lithium in this series and thus they are poor reducing agents than Lithium and are not oxidized that easily either.
Thus $L{i}^{+}$ is the best reducing agent and it gets oxidized most easily.