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(B) The hydration energy of alkaline earth metal ions decreases as the size of the ion increases $(Mg^{2+} > Ca^{2+} > Sr^{2+} > Ba^{2+})$. $MgCl_2$ f

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$MgCl_2$

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(B) The hydration energy of alkaline earth metal ions decreases as the size of the ion increases $(Mg^{2+} > Ca^{2+} > Sr^{2+} > Ba^{2+})$. $MgCl_2$ forms a hexahydrate $(MgCl_2 \cdot 6H_2O)$,whereas $CaCl_2$ forms a hexahydrate,$SrCl_2$ forms a hexahydrate,and $BaCl_2$ forms a dihydrate $(BaCl_2 \cdot 2H_2O)$. Among the given options,$MgCl_2$ has the highest tendency to coordinate water molecules due to its small ionic radius and high charge density,allowing it to form stable hexahydrates.

$A$. $Be$	$I$. $1.74$
$B$. $Mg$	$II$. $1.84$
$C$. $Ca$	$III$. $2.63$
$D$. $Sr$	$IV$. $1.55$

Which of the following salts can accommodate the largest number of $H_2O$ molecules per molecule in their halide hydrates?

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Match the following alkaline earth metals with their respective densities $(g/cm^3)$:
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$CaCO_3$ $\xrightarrow[excess \ H_2O]{in \ CO_2} A$ $\xrightarrow{\Delta} B$
Identify $A$ and $B$.

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