How does the covalent character vary in LiCl, | vedclass

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Question

(C) According to Fajan's rule,the covalent character of an ionic bond increases with an increase in the polarizing power of the cation.Polarizing powe

Vedclass · Accepted Answer

$LiCl < BeCl_2 < BCl_3 < CCl_4$

Vedclass · Answer

(C) According to Fajan's rule,the covalent character of an ionic bond increases with an increase in the polarizing power of the cation.Polarizing power is directly proportional to the charge density of the cation (charge/size ratio).As we move from $Li^+$ to $Be^{2+}$ to $B^{3+}$ to $C^{4+}$,the positive charge on the cation increases and the ionic size decreases.Therefore,the polarizing power increases in the order: $Li^+ Consequently,the covalent character increases in the order: $LiCl < BeCl_2 < BCl_3 < CCl_4$.

How does the covalent character vary in $LiCl, BeCl_2, BCl_3$ and $CCl_4$?

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