Question

Describe the bonding in ${\mathbf{\text{SO}}}_{\mathbf{\text{2}}}$and ${\mathbf{\text{SO}}}_{\mathbf{\text{3}}}$ using the localized electron model (hybrid orbital theory). How would the molecular orbital model describe the bonding in these two compounds?

Short answer

The creation of $\sigma$and $\mathrm{\pi }$ localised bonds is explained by the localised electron hypothesis in the sulphur compounds. The creation of a molecular orbital that comprises delocalized electrons across the molecule is suggested by the molecular orbital model.

Step-by-step solution

Concept Introduction

Pi ($\mathbf{\pi }$ ) bonds are covalent chemical connections that entail the lateral overlapping of two lobes of one atomic orbital with two lobes of another atomic orbital from a different atom.

π bonding in sulphur compounds

Molecule${\text{SO}}_{\text{2}}$will form two$\sigma$and two$\mathrm{\pi }$bonds between the sulphur atom and two oxygen atoms.$\sigma$bonds will be createdin the line between each oxygen atom and the sulphur atom. In the molecular plane will be placed lone electron pair as wellas two$\sigma$bonds.$\mathrm{\pi }$bonds will be formed by overlappingorbitals. And they will be placed above or below the molecularplane.

The similar situation occurs in${\text{SO}}_3$molecule. The only difference will be the additional$\sigma$and$\mathrm{\pi }$bond with the thirdoxygen atom.$\sigma$bonds will lie in the molecular plane and$\mathrm{\pi }$bonds will be placed above or below that plane.

The molecular orbital model explains the delocalization of$\mathrm{\pi }$bonds electrons. Therefore, molecular orbital will be formedand there will be placed delocalized electrons. The difference between these two models regarding$\mathrm{\pi }$bonds will be inlocalization and delocalization of$\mathrm{\pi }$bonds electrons.

Therefore, localized electron model explains the formation of $\sigma$ and $\mathrm{\pi }$bonds that are localized. Molecular orbital model suggestsformation of molecular orbital that contains delocalized electrons across the molecule.