A) \[B{{F}_{3}}\]
B) \[BC{{l}_{3}}\]
C) \[BB{{r}_{3}}\]
D) \[B{{I}_{3}}\]
Correct Answer: D
Solution :
As the size of the halogen atom increases from \[F\] to\[I\], the extent of overlapping (\[ie,\] \[p\pi -p\pi \] back bonding) between \[2p\] orbital of \[B\] and a \[p-\]orbitals of halogens (\[2p\] in\[F\], \[3p\] in \[Cl\], \[4p\] in \[Br\] and \[5p\] in \[I\]) decreases and consequently the electron deficiency of \[B\] increases and thus the Lewis acid character increases. Thus, the acidic strength of boron trihalide is as \[B{{F}_{3}}<BC{{l}_{3}}<BB{{r}_{3}}<B{{I}_{3}}\]
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