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Question
A reaction between ammonia and boron trifluoride is given below: \[\ce{NH3 + BF3 -> H3N : BF3}\] Identify the acid and base in this reaction. Which theory explains it? What is the hybridisation of B and N in the reactants?
Solution
Although \[\ce{BF3}\] does not have a proton but acts as Lewis acid as it is an electron-deficient compound. It reacts with \[\ce{NH3}\] by accepting the lone pair of electrons from \[\ce{NH3}\] and completes its octet. The reaction can be represented by \[\ce{BF3 + :NH3 -> BF3 <- : NH3}\]
Lewis electronic theory of acids and bases can explain it. Boron in \[\ce{BF3}\] is sp2 hybridised, whereas N in \[\ce{NH3}\] is sp3 hybridised.
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