The approximate shape of a molecule can often be predicted by using what is called the valence-shell electron-pair repulsion (VSEPR) model. Electrons in bonds and in lone pairs can be thought of a ''charge cloud'' that repel one another nad stay as far apart as possible, thus causing molecules to assume specific shapes.
The repulsive interactions of electron pairs decrease in the order:
Lone pair - Lone pair gt Lone pair - Bond pair gt Bond pair - Bond pair
These repulsive effects result in deviations from idealised shapes and alteration in bond angles in molecules.
Which among the following molecules have `sp^(3)d` hybridization with one lone pair of electron on the central atom?
(P) `SF_(4)`
(Q) `[PCl_(4)]^(+)`
(R) `XeO_(2)F_(2)`
(S) `ClOF_(3)`

Options

A. P, Q and R only
B. P, R and S only
C. P and Q only
D. Q and R only

Answer

B

Explanation

`PCl_(4)^(+)` has zero l.p. on C.A.