How does the covalent character vary in LiCl, | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

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 $CCl_4$?

Similar Questions

Amongst $LiCl$,$RbCl$,$BeCl_2$,and $MgCl_2$,the maximum and minimum ionic character will be shown by the compounds:

The combination of which of the following gives an ionic compound with maximum covalent character?

The order of solubility of lithium halides in non-polar solvents follows the order:

Which ion exhibits the maximum Lewis acid character?

Which of the following has the lowest melting point?

Vedclass Test Series

Exam Paper Generator

Online Exam Module