Fajan’s rule :
i. Smaller the size of the cation and larger the size of the anion, greater is the covalent character of the ionic bond.
For example,
Li+ Cl- is more covalent than Na+ Cl.
Similarly,
Li+I- is more covalent than Li+Cl-.
ii. Greater the charge on cation, more is covalent character of the ionic bond.
For example,
Covalent character of AlCl3, MgCl2 and NaCl decreases in the following order
Al3+(Cl-)3 > Mg2+(Cl-)2 > Na+ Cl-
iii. A cation with the outer electronic configuration of the s2p6d10 type possesses greater polarising power compared to the cation having the same size and same charge but having outer electronic configuration of s2p6 type.
This is because d electrons of the s2p6d10 shell screen nuclear charge less effectively compared to s and p electrons of s2p6 shell.
Hence,
The effective nuclear charge in a cation having s2p6d10 configuration is greater than that of the one having s p configuration.
For example :
Cu+ Cl- is more covalent than Na+ Cl-.
Here,
(Cu+ = 1s2 2s2 2p6 3s2 3p6 3d10; Na+ = 1s2 2s2 2p6)