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(C) The reducing power of a metal in an aqueous solution is determined by the standard electrode potential $(E^{\circ})$,which depends on the sum of s

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Hydration enthalpy

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(C) The reducing power of a metal in an aqueous solution is determined by the standard electrode potential $(E^{\circ})$,which depends on the sum of sublimation enthalpy,ionization enthalpy,and hydration enthalpy. Due to the very small size of the $Li^{+}$ ion,it has the highest hydration enthalpy among alkali metal ions. This high negative value of hydration enthalpy compensates for the high ionization enthalpy of $Li$,making its standard reduction potential $(E^{\circ} = -3.04 \ V)$ the most negative. Therefore,$Li$ acts as the strongest reducing agent in aqueous solution.

$I. Na_3N$	$II. Na_2O$
$III. NaO_2$	$IV. Na_2O_2$

The reducing power of a metal depends on various factors. Suggest the factor which makes $Li$ metal the strongest reducing agent in aqueous solution.

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