The correct order of covalent bond character | vedclass

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

Question

(A) According to Fajan's rule,the covalent character of an ionic bond increases with:$1$. Smaller size of the cation.$2$. Higher charge on the cation.

Vedclass · Accepted Answer

$LiCl < BeCl_2 < BCl_3 < CCl_4$

Vedclass · Answer

(A) According to Fajan's rule,the covalent character of an ionic bond increases with:$1$. Smaller size of the cation.$2$. Higher charge on the cation.Comparing the cations $Li^{+}$,$Be^{2+}$,$B^{3+}$,and $C^{4+}$:- The charge increases in the order: $Li^{+} - The ionic radius decreases in the order: $Li^{+} > Be^{2+} > B^{3+} > C^{4+}$.Both factors favor increased polarization of the anion by the cation as we move from $LiCl$ to $CCl_4$.Therefore,the covalent character increases in the order: $LiCl < BeCl_2 < BCl_3 < CCl_4$.

The correct order of covalent bond character of $BCl_3, CCl_4, BeCl_2, LiCl$ is

Similar Questions

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

The most polarisable ion among the following is

Assertion : $LiCl$ is predominantly a covalent compound.
Reason : Electronegativity difference between $Li$ and $Cl$ is too small.

Maximum covalent character is associated with the compound:

Polarization is the distortion of the shape of an anion by an adjacently placed cation. Which of the following statements is correct?

Vedclass Test Series

Exam Paper Generator

Online Exam Module