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

1.	How do you account for the strong reducing power of lithium in aqueous solution ?
Answer» Solution :Electrode potential is a measure of the tendency of an element to lose electrons in the aqueous solution . It mainly depends upon the FOLLOWING three factors , i.e., (i) `Li (s) overset("Sublimation enthalpy")(to) Li (G) , (ii) Li (g) overset("Ionization enthalpy")(to) Li^(+) (g)` (iii) `Li^(+) (g) + aq to Li^(+) (aq) + ` enthalpy of HYDRATION The sublimation enthalpy of alkali metals are almost SIMILAR . since Li has the smallest size , its enthalpy of hydration is the highest among alkali metals . Although ionization enthalpy of Li is the highest among alkali metals , it is more than compensated by the high enthalpy of hydration . Thus , Li has the most negative standard electrode potential `(-3*04 V)` and hence Li is the strongest REDUCING agent in aqueous solution mainly because of its high enthalpy of hydration .

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