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One hybridization of one s and one p orb...

One hybridization of one `s` and one `p` orbital we get

A

Two mutually perpendicular hybrid orbitals

B

Two equivalent hybrid orbitals at `180^(@)`

C

Four hybrid orbitals directed tetrahedrally

D

Three hybrid orbitals in the plane

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The correct Answer is:
B
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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. Among the following which have the same molecular geometry? (P) I_(3)^(-) (Q) XeF_(4) (R) BrF_(4)^(-) (S) XeO_(2)F_(2)

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