The correct Lewis acidity order of BX_3 is: | vedclass

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(A) $(I)$ The Lewis acidity of boron trihalides $(BX_3)$ is governed by the extent of $p\pi-p\pi$ back-bonding between the lone pair of the halogen at

Vedclass · Accepted Answer

$BF_3 < BCl_3 < BBr_3 < BI_3$

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(A) $(I)$ The Lewis acidity of boron trihalides $(BX_3)$ is governed by the extent of $p\pi-p\pi$ back-bonding between the lone pair of the halogen atom and the vacant $p$-orbital of the boron atom.$(II)$ As the size of the halogen atom increases from $F$ to $I$,the effectiveness of the $p\pi-p\pi$ back-bonding decreases because the overlap between the $2p$ orbital of boron and the $np$ orbital of the halogen becomes less efficient.$(III)$ Consequently,$BF_3$ has the strongest back-bonding,making it the weakest Lewis acid,while $BI_3$ has the weakest back-bonding,making it the strongest Lewis acid.$(IV)$ Therefore,the correct order of Lewis acidity is $BF_3 < BCl_3 < BBr_3 < BI_3$.

The correct Lewis acidity order of $BX_3$ is:

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