It should be checked that can hybrid orbital be used to explain how a central atom can form more bonds than the number of unpaired electrons in its ground state configuration. Concept introduction: According to valence bond theory , The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms. The each overlapping atomic orbital must be contained with a single unpaired. Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis. Pi (π) bonds: the bonds in which shared un-hybridized orbital’s (p, d, etc.) electron density are concentrated in above and below of the plane of the molecule. Double bonds: One sigma bond and one pi bond are together known as a double bond.

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Chapter 7.8, Problem 7.8.3SR

Interpretation Introduction

Interpretation:

It should be checked that can hybrid orbital be used to explain how a central atom can form more bonds than the number of unpaired electrons in its ground state configuration.

Concept introduction:

According to valence bond theory,

The bonds between atoms are formed by sharing their electrons through the overlap of atomic orbitals between other atoms.

The each overlapping atomic orbital must be contained with a single unpaired.

Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy.
Sigma (σ) bonds: The bonds in which shared hybrid orbital’s electron density are concentrated along the inter-nuclear axis.

Pi (π) bonds: the bonds in which shared un-hybridized orbital’s (p, d, etc.) electron density are concentrated in above and below of the plane of the molecule.

Double bonds: One sigma bond and one pi bond are together known as a double bond.

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