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(C) The ionization energy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion.Successive ionization energies increase signi

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$Ca^+(g) 	o Ca^{2+}(g) + e^-$

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(C) The ionization energy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion.Successive ionization energies increase significantly because it becomes harder to remove an electron from an increasingly positive ion.Option $A$ and $B$ represent the first ionization energy $(IE_1)$ of $Ba$ and $Ca$ respectively.Option $C$ represents the second ionization energy $(IE_2)$ of $Ca$,which is significantly higher than $IE_1$.Option $D$ represents the total energy for the removal of two electrons $(IE_1 + IE_2)$ from $Mg$.Comparing the processes,the removal of the second electron from a cation (as in option $C$) or the cumulative energy for two electrons (as in option $D$) involves higher energy values than a single first ionization.However,the second ionization energy of $Ca$ $(IE_2)$ is a specific high-energy step compared to the first ionization of larger atoms like $Ba$ or $Ca$. Given the standard comparison of $IE$ values,the process $Ca^+(g) 	o Ca^{2+}(g) + e^-$ requires the most energy among the single-step processes listed.

Which of the following processes represents the highest ionization energy?

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