Why Lithium Is Strongest Reducing Agent?

Lithium ion is small in size and has high ionization enthalpy. ... Thus, Li has a greater tendency to lose electrons in solution than other alkali metals. The Large amount of hydration energy makes it the strongest reducing agent in spite of its highest ionisation enthalpy.

What makes lithium the strongest reducing agent among the alkali metals?

Among all the alkali metals, $Li$ have the highest oxidation potential therefore, it has the highest reducing property. Moreover, due to its small size $Li$ has very high hydration enthalpy. So, $Li$ has a high tendency to lose electrons in solution. Hence, $Li$ is the strongest reducing agent.

Why is lithium a better reducing agent than sodium?

The greater reducing character of Li than Na is due to its greater hydration energy. Lithium being small in size has high ionization energy. On the other hand because of its small size it is easily hydrated with very high hydration enthalpy.