Chapter 9, Problem 55IL

Interpretation Introduction

Interpretation:

The two possible structures of acetate ion have to be drawn. The hybridization of the carbon atoms of $-C{O}_2{}^{-}$ has to be identified. The orbitals that overlap to form bonds between carbon and the three elements attached to it have to be identified.

Concept Introduction

• Sometimes the chemical bonding of a molecule cannot be represented using a single Lewis structure. In these cases, the chemical bonding are described by delocalization of electrons and is known as resonance.
• All the possible resonance structures are imaginary whereas the resonance hybrid is real.
• These structures will differ only in the arrangement of the electrons not in the relative position of the atomic nuclei.
• Hybridization is the mixing of valence atomic orbitals to get equivalent hybridized orbitals that having similar characteristics and energy. Geometry of a molecule can be predicted by knowing its hybridization.
• ${\text{sp}}^{\text{3}}$ hybrid orbitals is produced by hybridization of single s-orbital and three p-orbital.
• ${\text{sp}}^2$ hybrid orbitals is produced by hybridization between one s-orbital and two p-orbitals.
• $\text{sp }$ hybrid orbitals is produced by hybridization of single s-orbital and single p-orbital.
• Sigma (σ) bonds are the bonds in which shared hybrid orbital’s electron density are concentrated along the internuclear axis.
• Pi (π) bonds are the bonds in which shared unhybridized orbital’s (p, d, etc) electron density are concentrated in above and below of the plane of the molecule.