Why is $LiF$ almost insoluble in water whereas $LiCl$ soluble not only in water but also in acetone?
(N/A) $LiF$ is almost insoluble in water due to its very high lattice energy,which arises from the small size of both $Li^+$ and $F^-$ ions.
In contrast,$LiCl$ has a lower lattice energy and possesses significant covalent character due to the polarization of the $Cl^-$ ion by the small $Li^+$ ion (Fajans' rule).
This covalent character makes $LiCl$ soluble in organic solvents like acetone,while its lower lattice energy compared to $LiF$ allows it to dissolve more readily in water.
In contrast,$LiCl$ has a lower lattice energy and possesses significant covalent character due to the polarization of the $Cl^-$ ion by the small $Li^+$ ion (Fajans' rule).
This covalent character makes $LiCl$ soluble in organic solvents like acetone,while its lower lattice energy compared to $LiF$ allows it to dissolve more readily in water.
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