The bonding in diatomic (nitrogen) N 2 is to be explained using hybrid orbitals and the valence bond theory . Concept introduction: According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms. To understand bonding, write the electronic configuration of the central atom in the ground state and draw the valence orbitals. Determine the number of orbitals that are singly occupied and can form the bonds. Hybrid orbitals are formed by the mixing of atomic orbitals. To explain bonding by hybrid orbitals, examine the Lewis dot structure of the molecule Find the number of electron domains present around the central atom. Draw the orbital diagram of the central atom in its ground state. Promote electrons to higher orbitals to get the highest number of unpaired electrons. Combine the required number of atomic orbitals to get the hybrid orbitals.

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Chapter 9.6, Problem 1PPB

Interpretation Introduction

Interpretation: The bonding in diatomic (nitrogen) N2 is to be explained using hybrid orbitals and the valence bond theory.

Concept introduction: According to the valence bond approach, a bond is formed by the overlapping of singly occupied orbitals present on two atoms.

To understand bonding, write the electronic configuration of the central atom in the ground state and draw the valence orbitals.

Determine the number of orbitals that are singly occupied and can form the bonds.

Hybrid orbitals are formed by the mixing of atomic orbitals.

To explain bonding by hybrid orbitals, examine the Lewis dot structure of the molecule

Find the number of electron domains present around the central atom.

Draw the orbital diagram of the central atom in its ground state.

Promote electrons to higher orbitals to get the highest number of unpaired electrons.

Combine the required number of atomic orbitals to get the hybrid orbitals.

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