Question:
Hydration enthalpy of which of the following ions is highest?
Hydration enthalpy of which of the following ions is highest?
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Hydration enthalpy \(\propto \frac{\text{charge}^2}{\text{ionic radius}}\). Small, highly charged ions have the highest values.
Updated On: Jun 26, 2026
- Mg\(^{2+}\)
- Na\(^{+}\)
- Ca\(^{2+}\)
- K\(^{+}\)
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The Correct Option is A
Solution and Explanation
Step 1: Understand hydration enthalpy.
Hydration enthalpy increases with higher charge and smaller ionic radius because the ion attracts water molecules more strongly.
Step 2: Compare given ions.
- Mg\(^{2+}\) has a small radius and +2 charge → very high hydration enthalpy.
- Na\(^{+}\), Ca\(^{2+}\), and K\(^{+}\) are larger or less charged.
Step 3: Conclusion.
The ion with the highest hydration enthalpy is \[ \boxed{\text{Mg}^{2+}} \]
Hydration enthalpy increases with higher charge and smaller ionic radius because the ion attracts water molecules more strongly.
Step 2: Compare given ions.
- Mg\(^{2+}\) has a small radius and +2 charge → very high hydration enthalpy.
- Na\(^{+}\), Ca\(^{2+}\), and K\(^{+}\) are larger or less charged.
Step 3: Conclusion.
The ion with the highest hydration enthalpy is \[ \boxed{\text{Mg}^{2+}} \]
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