The Lewis acid strength of BBr3, BCl3 and BF3 is in the order

Question

The Lewis acid strength of BBr3, BCl3 and BF3 is in the order (A) BBr3 < BCl3 < BF3 (B) BCl3 < BF3 < BBr3 (C) BF3 < BCl3 < BBr3 (D) BBr3 < BF3 < BCl3

Tardigrade Admin · Accepted Answer

Given compounds of boron are electron deficient molecule, which have tendency to accept a pair of electrons to achieve stable electronic configuration and thus behave as Lewis acids. Lewis acid strength of

BB r_{3}, BC l_{3}

and

B F_{3}

increases in the order

B F_{3} < BC l_{3} < BB r_{3}

.

B F_{3}

has least acidity due to effective back bonding between

2 p

-orbital of

B

and

2 p

-orbital of

F

. Whereas, no such back bonding is observed in

BB r_{3}

and thus has maximum acidity.

Q. The Lewis acid strength of $BB r_{3}, BC l_{3}$ and $B F_{3}$ is in the order

$BB r_{3} < BC l_{3} < B F_{3}$

$BC l_{3} < B F_{3} < BB r_{3}$

$B F_{3} < BC l_{3} < BB r_{3}$

$BB r_{3} < B F_{3} < BC l_{3}$

Q. The Lewis acid strength of BBr3​,BCl3​ and BF3​ is in the order

BBr3​<BCl3​<BF3​

BCl3​<BF3​<BBr3​

BF3​<BCl3​<BBr3​

BBr3​<BF3​<BCl3​

Q. The Lewis acid strength of $BB r_{3}, BC l_{3}$ and $B F_{3}$ is in the order

$BB r_{3} < BC l_{3} < B F_{3}$

$BC l_{3} < B F_{3} < BB r_{3}$

$B F_{3} < BC l_{3} < BB r_{3}$

$BB r_{3} < B F_{3} < BC l_{3}$