Question

What is the hybridization of the underlined nitrogen atom in each of the following molecules or ions?

a. ${\mathrm{NO}}^{+}$

b. $N_2{O}_3\left(O_{2}N\underline{N}O\right)$

c. $\underline{N}{O}_2^{-}$

d.${\underline{N}}_2$

Short answer

(a) The hybridization of underlined nitrogen atom in${\mathrm{NO}}^{+}$ is sp hybridization.

(b) The hybridization of underlined nitrogen atom in$N_2{O}_3\left(O_{2}N\underline{N}O\right)$ is${\mathrm{Sp}}^2$ hybridization.

(c) The hybridization of underlined nitrogen atom in$\underline{N}{O}_2^{-}$ is hybridization.

(d) The hybridization of underlined nitrogen atom in ${\underline{N}}_2$is sp hybridization.

Step-by-step solution

Concept Introduction

In chemistry, hybridization is the idea of combining two atomic orbitals to create a brand-new category of hybridised orbitals. Typically, this mixing creates hybrid orbitals with completely distinct energies, morphologies, etc.

Hybridization of N in NO+

(a)

Marked atom is sp hybridized because it has lone electron pair and one$\mathrm{\sigma }$bond that are sp hybridized and one$\mathrm{\pi }$bond that is formed by overlapping p orbitals.

The structure is as follows –

Therefore, nitrogen has sp hybridization.

Hybridization of N in N2O3 (O2NNO)

(b)

Marked nitrogen atom is ${\mathrm{Sp}}^2$ hybridized because two $\sigma$ bonds were formed from these hybridized orbitals as well as lone electron pair is ${\mathrm{Sp}}^2$hybridized.

The structure is as follows –

Therefore, nitrogen has ${\mathrm{Sp}}^2$hybridization.

Hybridization of N in NO2-

(c)

Marked nitrogen atom is ${\mathrm{Sp}}^2$hybridized because two bonds were formed between central nitrogen and two oxygen atoms from these hybridized orbitals as well as lone electron pair is ${\mathrm{Sp}}^2$hybridized.

The structure is as follows –

Therefore, nitrogen has hybridization.