Hybridization of central atom in  ${\mathrm{NO}}_2^{-},{\mathrm{NH}}_2^{-},{\mathrm{NO}}_2^{+}$  respectively

The concept of hybridization is crucial in understanding the bonding and molecular structure of compounds. Below is the detailed hybridization analysis for the given species: NO₂⁻, NH₂⁻, and NO₂⁺.

1. Hybridization in NO₂⁻

The nitrate ion (NO₂⁻) consists of a nitrogen atom as the central atom. The bonding and hybridization can be analyzed as follows:

• Bond pairs (bp): 2
• Lone pairs (lp): 1

The steric number (sum of bond pairs and lone pairs) is 3, which corresponds to sp² hybridization. This allows the central nitrogen to form a planar structure with bond angles close to 120°.

2. Hybridization in NH₂⁻

For the amide ion (NH₂⁻), the nitrogen atom is the central atom, and its hybridization can be determined as follows:

• Bond pairs (bp): 2
• Lone pairs (lp): 2

Here, the steric number is 4, which corresponds to sp³ hybridization. This hybridisation of NH₂⁻ results in a tetrahedral electronic geometry, though the molecular shape is bent due to the lone pairs repelling the bond pairs.

3. Hybridization in NO₂⁺

In the nitronium ion (NO₂⁺), nitrogen acts as the central atom, and its hybridization is analyzed as follows:

• Bond pairs (bp): 2
• Lone pairs (lp): 0

The steric number is 2, which corresponds to sp hybridization. This hybridization leads to a linear structure with a bond angle of 180°.

Summary

The hybridization of the central atoms in the given species is summarized below:

Understanding the hybridisation of NH₂⁻, NO₂⁻, and NO₂⁺ is essential for predicting their geometry and reactivity in various chemical reactions.