Hydration enthalpy of which of the following | vedclass

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(A) Hydration enthalpy is the amount of energy released when one mole of ions is dissolved in excess of water.It is directly proportional to the charg

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$Mg^{2+}$

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(A) Hydration enthalpy is the amount of energy released when one mole of ions is dissolved in excess of water.It is directly proportional to the charge density of the ion.Hydration enthalpy increases as the ionic size decreases and the ionic charge increases.Comparing the given ions: $Na^{+}$ and $Mg^{2+}$ belong to the $3^{rd}$ period,while $K^{+}$ and $Ca^{2+}$ belong to the $4^{th}$ period.Ions with smaller size ($Na^{+}$ and $Mg^{2+}$) have higher hydration enthalpy than those with larger size ($K^{+}$ and $Ca^{2+}$).Between $Na^{+}$ and $Mg^{2+}$,$Mg^{2+}$ has a smaller ionic radius and a higher charge ($+2$ vs $+1$).Therefore,$Mg^{2+}$ has the highest charge density and the highest hydration enthalpy.

Hydration enthalpy of which of the following ions is highest?

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