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(A) The ease of reduction of a metal oxide depends on the thermodynamic stability of the oxide,which is related to the standard Gibbs free energy of f

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$Cs$

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(A) The ease of reduction of a metal oxide depends on the thermodynamic stability of the oxide,which is related to the standard Gibbs free energy of formation $(\Delta G_f^\circ)$.Metals with higher negative values of $\Delta G_f^\circ$ form more stable oxides,making them harder to reduce.According to the Ellingham diagram,alkali and alkaline earth metals like $Cs$ and $Mg$ have very stable oxides compared to transition metals like $Zn$ or $Ag$.Among the given options,$Cs$ (Cesium) is an alkali metal with a very high affinity for oxygen,making its oxide the most stable and thus the most difficult to reduce to the metal.

Which metal is most difficult to be extracted from its oxide?

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