Which of the following is the weakest reducin | vedclass

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(D) The reducing power of an element is determined by its standard electrode potential $(E^\circ)$.For alkali metals,the reducing power in aqueous sol

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$Rb$

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(D) The reducing power of an element is determined by its standard electrode potential $(E^\circ)$.For alkali metals,the reducing power in aqueous solution depends on the sum of sublimation energy,ionization energy,and hydration energy.Although $Li$ has the highest ionization energy,it has the highest hydration energy due to its small size,which makes its standard electrode potential $(E^\circ = -3.04 \ V)$ the most negative.Therefore,$Li$ is the strongest reducing agent in aqueous solution.Among the given options,as we move down the group from $Li$ to $Rb$,the standard electrode potential becomes less negative.Thus,$Rb$ is the weakest reducing agent among the given alkali metals.

Which of the following is the weakest reducing agent?

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