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(A) The hydration enthalpy of an ion depends on its charge density,which is directly proportional to the charge and inversely proportional to the ioni

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$C > E > A > B > D$

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(A) The hydration enthalpy of an ion depends on its charge density,which is directly proportional to the charge and inversely proportional to the ionic radius $(H_{hyd} \propto \frac{q}{r})$.$1$. Comparing charges: Ions with higher charge $(Mg^{2+}, Ca^{2+})$ have significantly higher hydration enthalpies than monovalent ions $(K^{+}, Rb^{+}, Cs^{+})$.$2$. Within the same group,hydration enthalpy decreases as the ionic radius increases.$3$. For group $2$ ions: $Mg^{2+} > Ca^{2+}$ $(C > E)$.$4$. For group $1$ ions: $K^{+} > Rb^{+} > Cs^{+}$ $(A > B > D)$.Combining these,the overall order is $Mg^{2+} > Ca^{2+} > K^{+} > Rb^{+} > Cs^{+}$,which corresponds to $C > E > A > B > D$.

The correct order of hydration enthalpies is
$A. K^{+}$; $B. Rb^{+}$; $C. Mg^{2+}$; $D. Cs^{+}$; $E. Ca^{2+}$
Choose the correct answer from the options given below:

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The correct order of hydration enthalpies is$A. K^{+}$; $B. Rb^{+}$; $C. Mg^{2+}$; $D. Cs^{+}$; $E. Ca^{2+}$Choose the correct answer from the options given below: