The strongest reducing agent among the alkali | vedclass

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(A) The reducing power of an element in an aqueous solution is determined by its standard electrode potential $(E^\circ)$.$Li$ has the most negative s

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$Li$

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(A) The reducing power of an element in an aqueous solution is determined by its standard electrode potential $(E^\circ)$.$Li$ has the most negative standard electrode potential $(E^\circ = -3.04 \ V)$ among alkali metals,which is due to its very high hydration energy.Therefore,$Li$ is the strongest reducing agent in an aqueous solution.

The strongest reducing agent among the alkali metals is

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