Question:
The correct order of covalent bond character of \( BCl_3, CCl_4, BeCl_2, LiCl \) is:
The correct order of covalent bond character of \( BCl_3, CCl_4, BeCl_2, LiCl \) is:
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Smaller cations and larger anions increase covalent character due to higher polarization.
Updated On: Mar 24, 2025
- \( LiCl<BeCl_2<BCl_3<CCl_4 \)
- \( CCl_4<BeCl_2<BCl_3<LiCl \)
- \( CCl_4<BCl_3<BeCl_2<LiCl \)
- \( LiCl<BCl_3<BeCl_2<CCl_4 \)
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Verified By Collegedunia
The Correct Option is A
Solution and Explanation
Step 1: Apply Fajan’s Rule
Covalent character increases with:
- Higher cation charge density.
- Larger anion size.
Step 2: Arrange Based on Covalent Character
\[
LiCl<BeCl_2<BCl_3<CCl_4
\]
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