A reaction between ammonia and boron trifluoride is given below:

BF_{3}+:NH_{3}\rightarrow BF_{3}:NH_{3}

Identify the acid and base in this reaction. Which theory explains it? What is the hybridisation of B and N in the reactants?

Answers (1)

As per the information given in the question,NH_{3} + BF_{3}\rightarrow H_{3}N: BF_{3}

NH_{3} (N=1s^{2}2s^{2}2p^{1}) is the Lewis acid in this reaction because it has a lone pair of e- to donate in its p-orbital. Moreover, the Lewis base in this case is BF3 as p-orbital of Boron is empty(B=1s^{2}2s^{2}2p^{1}). As such, it will be accepting lone pair from N to form a dative bond, as is clear from the lewis electronic theory. Thus, the Hybridisation of N is sp3 and B is sp2.

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