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

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

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Li ions, due to small size, have high enthalpy of ionisation 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 Ionisation)

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

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