Hybridization is a concept of mixing or merging of orbitals of same atom with slight differences in energies to redistribute their energies and give new orbitals of equivalent energy called 'Hybrid Orbitals'. Hybridisation is a hypothetical concept and never actually exists.
One should not be confused by a common misconception that hybridization is responsible for particular geometry. Geometry of a molecule is decided by energy factor not by hybridization. It is the orbital (which may be half filled, completely filled or empty) that undergoes hybridization and not the electron. The bond angles in hybridised orbitals are influenced by presence of lone pair, presence of multiple bonds, presence of one electron and electronegativity of atom.
An increase in s-character of hybridised orbitals results in decrease in size of orbitals. This results in decrease in bond length and increase in energy.
Which of the following statements is true?

Options

A. The state of hybridization of boron and oxygen atoms in boric acid are `sp^(3)` and `sp^(2)` respectively.
B. `NH_(3)` and `[BF_(4)^(-)]` have same bond angles of `109^(@)28'`
C. `SF_(6)` and `PF_(6)^(-)` both have undistorted octahedral structures.
D. The hybridization of P in `P_(4)` molecules is the same as in S in `SO_(3)` molecule.

Answer

C

Explanation

(a) `{:(" "O-H),(" |"),(H-O-underset(sp^(2))B-underset(sp^(2))O-H):}`
(b) `BF_(4)^(-)` is tetrahedral with B.A. = `109^(@)28'`
`P_(4)rarrsp^(3),SO_(3)rarrsp^(2)`