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प्रश्न
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?
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उत्तर
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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\[\ce{BF3}\] does not have proton but still acts as an acid and reacts with \[\ce{NH3}\]. Why is it so? What type of bond is formed between the two?
Match the following species with the corresponding conjugate acid:
| Species | Conjugate acid |
| (i) \[\ce{NH3}\] | (a) \[\ce{CO^{2-}3}\] |
| (ii) \[\ce{HCO^{-}3}\] | (b) \[\ce{NH^{+}4}\] |
| iii) \[\ce{H2O}\] | (c) \[\ce{H3O+}\] |
| (iv) \[\ce{HSO^{-}4}\] | (d) \[\ce{H2SO4}\] |
| (e) \[\ce{H2CO3}\] |
Acidity of BF3 can be explained on the basis of which of the following concepts?
