A) \[BB{{r}_{3}}\]
B) \[BC{{l}_{3}}\]
C) \[B{{I}_{3}}\]
D) \[B{{F}_{3}}\]
Correct Answer: C
Solution :
Generally, as the electronegativity increases, acidic character increases but in case of boron halides, \[B{{I}_{3}}\] is most acidic, ie, strongest Lewis acid. This is because there is back donation of electrons from F atom to boron in case of \[B{{F}_{3}}\]. This makes the \[B{{F}_{3}}\] less electron deficient. The tendency of back donation decreases as the size of halogen atom increases (due to large energy difference). Hence, \[B{{I}_{3}}\] is most electron deficient and thus, the strongest Lewis acid.
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