Which of the following ions has a lower entha | vedclass

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(B) The enthalpy of hydration is directly proportional to the charge density of the ion,which is defined as the ratio of charge to size $(q/r)$.For th

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$Na^{+}$

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(B) The enthalpy of hydration is directly proportional to the charge density of the ion,which is defined as the ratio of charge to size $(q/r)$.For the given ions,the charge density follows the order: $Be^{2+} > Mg^{2+} > Na^{+}$.Since $Na^{+}$ has a lower charge $(+1)$ and a larger ionic radius compared to $Mg^{2+}$ $(+2)$,its charge density is lower.Therefore,the enthalpy of hydration of $Na^{+}$ is lower than that of $Mg^{2+}$.

Which of the following ions has a lower enthalpy of hydration than the $Mg^{2+}$ ion?

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