Me_3B,BH_3,and BF_3 are three Lewis acids. Wh | vedclass

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Question

(B) The Lewis acidity of boron trihalides and alkyl boranes depends on the electron-withdrawing or electron-donating nature of the substituents attach

Vedclass · Accepted Answer

$Me_3B < BF_3 < BH_3$

Vedclass · Answer

(B) The Lewis acidity of boron trihalides and alkyl boranes depends on the electron-withdrawing or electron-donating nature of the substituents attached to the boron atom. $1$. In $BF_3$,the fluorine atoms have lone pairs that participate in $p\pi-p\pi$ back-bonding with the empty $p$-orbital of boron,which reduces its Lewis acidity. $2$. In $BH_3$,there is no back-bonding,making it a stronger Lewis acid than $BF_3$. $3$. In $Me_3B$,the methyl groups are electron-donating due to the $+I$ effect,which increases the electron density on the boron atom and significantly reduces its Lewis acidity. Therefore,the order of increasing Lewis acid strength is $Me_3B < BF_3 < BH_3$.

$Me_3B$,$BH_3$,and $BF_3$ are three Lewis acids. Which one of the following is the correct sequence of these acids in order of their increasing acid strength?

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