Which of the following is the strongest reduc | vedclass

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(B) The reducing power of alkali metals depends on their standard oxidation potential,which is related to the ease of losing an electron (low ionizati

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$Cs$

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(B) The reducing power of alkali metals depends on their standard oxidation potential,which is related to the ease of losing an electron (low ionization enthalpy) and high hydration energy.In the gas phase,ionization enthalpy decreases down the group $(Li > Na > K > Rb > Cs)$.However,in aqueous solution,the standard electrode potential $(E^\circ)$ is determined by the sum of sublimation,ionization,and hydration energies.Lithium $(Li)$ is the strongest reducing agent in aqueous solution due to its very high hydration energy.Among the given options $(Na, K, Rb, Cs)$,the reducing power increases as we go down the group because the ionization enthalpy decreases significantly.Therefore,$Cs$ (Cesium) is the strongest reducing agent among the given options.

Which of the following is the strongest reducing agent?

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