Question

Match the species in
Column I with the type of hybrid orbitals in Column II.

	Column-I		Column-II
A	$S{F}_4$	$\left(i\right)$	$s{p}^3{d}^2$
B	$I{F}_5$	$\left(ii\right)$	$d^{2}s{p}^3$
C	$N{O}_2^{+}$	$\left(iii\right)$	$s{p}^{3}d$
D	$N{H}_4^{+}$	$\left(iv\right)$	$s{p}^3$
		$\left(v\right)$	$sp$

Answer 1

Definition of hybridisation.

Hybridization is the process of intermixing of the orbitals of slightly different energies to redistribute their energies, which results in the formation of new set of orbitals of equivalent energies and shape.
Hybridization helps in deciding the structure of the molecules.

Total number of hybrid orbitals = No. of sigma bonds made by central atom + No. of lone pairs of electrons on central atom.

Molecules	Bond pairs	lone pairs	Total no.of hybrid orbitals	Hybridisation
$S{F}_4$	4	5	4+1=5	$s{p}^{3}d$
$I{F}_5$	5	6	5+1=6	$s{p}^3{d}^2$
$N{O}_2^{+}$	2	2	2+0=2	$sp$
$N{H}_4^{+}$	4	0	4+0=4	$s{p}^3$

	Column-I		Column-II
A	$S{F}_4$	$\left(iii\right)$	$s{p}^{3}d$
B	$I{F}_5$	$\left(i\right)$	$s{p}^3{d}^2$
C	$N{O}_2^{+}$	$\left(v\right)$	$sp$
D	$N{H}_4^{+}$	$\left(iv\right)$	$s{p}^3$