Question:
The Lewis acid character of boron tri halides follows the order :
The Lewis acid character of boron tri halides follows the order :
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The strength of Lewis acids can be compared based on the extent of back bonding and the electronegativity of halides.
Updated On: Apr 1, 2026
- $BCl _3> BF _3> BBr _3> BI _3$
- $BI _3> BBr _3> BCl _3> BF _3$
- $BBr _3> BI _3> BCl _3> BF _3$
- $BF _3> BCl _3> BBr _3> BI _3$
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The Correct Option is B
Approach Solution - 1
Extent of back bonding, reduces down the group leading to more Lewis acidic strength
So, the correct option is (B).
So, the correct option is (B).
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Approach Solution -2
Extent of back bonding reduces down the group leading to more Lewis acidic strength.
For example, \( \text{BF}_3 \) has the most extent of back bonding due to the \( 2p - 2p \) interaction, whereas \( \text{BCl}_3 \) and \( \text{BBr}_3 \) show less back bonding.
Therefore, the Lewis acid strength increases from \( \text{BF}_3 \) to \( \text{BCl}_3 \), \( \text{BBr}_3 \), and finally \( \text{B}_1 \).
Thus, the correct order is \( \text{B}_1 > \text{BBr}_3 > \text{BCl}_3 > \text{BF}_3 \).
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Concepts Used:
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- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
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