Question:
The correct order of hydration enthalpy of ions of Li, Na, Mg, Ca is
The correct order of hydration enthalpy of ions of Li, Na, Mg, Ca is
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Hydration enthalpy:
\[
\propto \frac{\text{Charge}}{\text{Radius}}
\]
Higher charge and smaller radius lead to greater hydration enthalpy.
Updated On: Jun 17, 2026
- $Ca > Mg > Na > Li$
- $Li > Na > Mg > Ca$
- $Na > Li > Ca > Mg$
- $Mg > Ca > Li > Na$
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The Correct Option is D
Solution and Explanation
Concept:
Hydration enthalpy increases with increasing charge density.
Smaller ions and higher charge produce larger hydration enthalpy.
Step 1: Compare charge densities.
\[ Mg^{2+} \] has highest charge density. \[ Ca^{2+} \] has lower charge density than magnesium. Among alkali ions, \[ Li^+ > Na^+ \]
Step 2: Arrange the ions.
\[ Mg^{2+}>Ca^{2+}>Li^+>Na^+ \] \[ \boxed{Mg>Ca>Li>Na} \]
Step 1: Compare charge densities.
\[ Mg^{2+} \] has highest charge density. \[ Ca^{2+} \] has lower charge density than magnesium. Among alkali ions, \[ Li^+ > Na^+ \]
Step 2: Arrange the ions.
\[ Mg^{2+}>Ca^{2+}>Li^+>Na^+ \] \[ \boxed{Mg>Ca>Li>Na} \]
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