Consider the following boron halides:
I. $B F_{3}$
II. $B C l_{3}$
III. $B B r_{3}$
IV. $B I_{3}$
The Lewis acid characters of these halides are such that:

I < I I < I I I < I V

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I < I I I < I I < I V

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I V < I I I < I I < I

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I V < I I < I I I < I

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Solution

The correct option is A $I < I I < I I I < I V$
The trend is due to $π$ back bonding. All halides have lone pairs, they donate one lone pair to boron by overlapping with the p orbitals of Boron. Effective overlap between orbitals decreases due to large size of p orbitals of halides. Hence electron deficiency of boron atom in its halides follow the trend $B I_{3} > B B r_{3} > B C l_{3} > B F_{3}$ and so is the lewis acidity order.

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