How do you account for the strong reducing power of lithium in aqueous solution?

Answers (1)

Li ions, due to small size, have high enthalpy of ionization and hydration. In aqueous solution, high hydration enthalpy predominates, and Li loses electrons and has strong reducing power.

Li (s) \rightarrow Li (g) (Sublimation enthalpy )

Li(g) \rightarrow Li^{+}(g)+1e^{-}(Enthalpy of Ionization )

Li^{+}(g)+H_{2}O \rightarrow Li^{+} (aq) (Enthalpy ofhydration)

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