Comparison of melting points of ionic compounds is generally done by considering the following two factors:
Charge of the cation/anion : More the charge of cation or anion, stronger will be the forces of attraction between the ions and higher will be the melting point.
Ionic radii: More the distance between ions, lesser will be the strength of the bond giving rise to lesser melting point.
Going by the above rules, the order should have been: LiCl>NaCl>KCl>RbCl
(Since charges of the ions are same for each molecule and cationic radius increases down the group.)
But LiCl, due to excessive polarization , exhibits high covalent character and is placed last in the order. Hence, the new order would be:
NaCl>KCl>RbCl>LiCl
The other ions, being similar in size to chloride ions, do not undergo much polarization.