The Lewis acid strength of BBr_3,BCl_3,and BF | vedclass

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Question

(C) The given boron trihalides are electron-deficient molecules that act as Lewis acids by accepting an electron pair.The Lewis acid strength is deter

Vedclass · Accepted Answer

$BF_3 < BCl_3 < BBr_3$

Vedclass · Answer

(C) The given boron trihalides are electron-deficient molecules that act as Lewis acids by accepting an electron pair.The Lewis acid strength is determined by the extent of $ppi-ppi$ back-bonding between the halogen atom and the boron atom.In $BF_3$,the $2p-2p$ back-bonding is most effective due to the similar size of the orbitals,which reduces the electron deficiency of the boron atom significantly.As the size of the halogen increases from $F$ to $Cl$ to $Br$,the effectiveness of back-bonding decreases $(2p-2p > 2p-3p > 2p-4p)$.Therefore,the electron deficiency on boron increases in the order $BF_3 < BCl_3 < BBr_3$,making $BBr_3$ the strongest Lewis acid.

The Lewis acid strength of $BBr_3$,$BCl_3$,and $BF_3$ is in the order:

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