Which of the following is least likely to behave as Lewis base?

N H_{3}

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B F_{3}

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O H^{-}

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H_{2} O

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Solution

The correct option is C $B F_{3}$
Boron trifluoride $B F_{3}$ is least likely to behave as Lewis base.

On the contrary, it is a Lewis acid.

In $B F_{3}$ , the central $B$ atom has six electrons and can easily accept an electron pair from a suitable base.

Thus, it acts as Lewis acid. It cannot act as Lewis base as it cannot donate an electron pair.

Option B is correct.

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