A reaction between ammonia and boron trifluoride is given below: :NH3 + BF3 →H3N : BF3. Identify the acid and base in this reaction. Which theory explains it? What is the hybridization of B and N in the reactants?

In the given reaction:

NH3+BF3→H3N:BF3NH3+BF3→H3N:BF3

Ammonia (NH3NH3) acts as the base, while boron trifluoride (BF3BF3) acts as the acid. This reaction involves the formation of a coordinate covalent bond between the lone pair of electrons on the nitrogen atom in ammonia and the empty orbital on the boron atom in boron trifluoride.

This reaction is best explained by Lewis acid-base theory. According to this theory, an acid is defined as a substance that can accept an electron pair, while a base is a substance that can donate an electron pair. In the given reaction, boron trifluoride acts as the Lewis acid by accepting the lone pair of electrons from ammonia, which acts as the Lewis base.

The hybridization of boron (BB) and nitrogen (NN) in the reactants can be determined by considering the electron configuration and bonding in the molecules:

1. In boron trifluoride (BF3BF3), boron has an electron configuration of 1s22s22p11s22s22p1. Boron forms three bonds with fluorine atoms, resulting in sp^2 hybridization for boron. The three hybridized orbitals on boron overlap with the p orbitals of the three fluorine atoms to form three sigma bonds.

2. In ammonia (NH3NH3), nitrogen has an electron configuration of 1s22s22p31s22s22p3. Nitrogen forms three bonds with hydrogen atoms, resulting in sp^3 hybridization for nitrogen. The three hybridized orbitals on nitrogen overlap with the s orbitals of the three hydrogen atoms to form three sigma bonds.

Therefore, in the reactants, the hybridization of boron is sp^2 and the hybridization of nitrogen is sp^3.