Problem

Lithium's exceptional reducing power in water hinges on the standard reduction potential — specifically, how easily it loses electrons. Even though Li has a very high ionization energy, its $E°$ value is the most negative of all metals, meaning it's thermodynamically most eager to be oxidized. The key insight is that in aqueous solution, the large hydration energy released when $\text{Li}^+$ forms compensates for the energy cost of ionization, making the overall process highly favorable and giving Li unmatched reducing ability.

Lithium's exceptional reducing power in water hinges on the standard reduction potential — specifically, how easily it loses electrons. Even though Li has a very high ionization energy, its $E°$ value is the most negative of all metals, meaning it's thermodynamically most eager to be oxidized. The key insight is that in aqueous solution, the large hydration energy released when $\text{Li}^+$ forms compensates for the energy cost of ionization, making the overall process highly favorable and giving Li unmatched reducing ability.