The Lewis acid nature of BX_3 follows the ord | vedclass

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(B) The Lewis acid strength of boron trihalides $(BX_3)$ is determined by the extent of $p\pi-p\pi$ back-bonding between the halogen atom and the boro

Vedclass · Accepted Answer

$BF_3 < BCl_3 < BBr_3 < BI_3$

Vedclass · Answer

(B) The Lewis acid strength of boron trihalides $(BX_3)$ is determined by the extent of $p\pi-p\pi$ back-bonding between the halogen atom and the boron atom. In $BF_3$,the fluorine atom has a small size and its $2p$ orbitals effectively overlap with the empty $2p$ orbital of boron,leading to strong back-bonding. This reduces the electron deficiency of boron,making $BF_3$ the weakest Lewis acid. As the size of the halogen increases from $F$ to $I$,the effectiveness of $p\pi-p\pi$ back-bonding decreases $(F > Cl > Br > I)$. Therefore,the electron deficiency of boron increases,and the Lewis acid strength increases in the order: $BF_3 < BCl_3 < BBr_3 < BI_3$.

The Lewis acid nature of $BX_3$ follows the order:

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