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In which of the following the hydration energy is higher than the lattice energy?
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Verified Answer
The correct answer is:
$\mathrm{MgSO}_4$
The solubility of sulphates of alkaline earth metals decreases with group from $\mathrm{Be}$ to $\mathrm{Ba}$ due to the ionic size increases down the group.
$\mathrm{BeSO}_4 > \mathrm{MgSO}_4 > \mathrm{CaSO}_4 > \mathrm{SrSO}_4 > \mathrm{BaSO}_4$
Related Theory
The greater the lattice enthalpy, the stronger the forces between ions. Those forces are only completely broken when the ions are present as gaseous ions, scattered so far apart that there is negligible attraction between them.
I Caution
$\rightarrow$ The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference.
$\mathrm{BeSO}_4 > \mathrm{MgSO}_4 > \mathrm{CaSO}_4 > \mathrm{SrSO}_4 > \mathrm{BaSO}_4$
Related Theory
The greater the lattice enthalpy, the stronger the forces between ions. Those forces are only completely broken when the ions are present as gaseous ions, scattered so far apart that there is negligible attraction between them.
I Caution
$\rightarrow$ The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference.
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