Draw the two resonance structures that describe the bonding...

Draw the two resonance structures that describe the bonding in the acetate ion. What is the hybridization of the carbon atom of the $-\mathrm{CO}_{2}^{-}$ group? Select one of the two resonance structures and identify the orbitals that overlap to form the bonds between carbon and the three elements attached to it.

Key Concepts

Hybridization

Hybridization involves the mixing of an atom’s orbitals to form new, degenerate orbitals suited for bonding with other atoms. In the acetate ion, the carbon atom of the -CO2? group is sp² hybridized, resulting in a trigonal planar geometry around the carbon with bond angles close to 120 degrees, which allows for effective overlapping with neighboring atoms.

Orbital Overlap

Orbital overlap is the interaction where atomic orbitals combine to form molecular orbitals, leading to stable sigma and pi bonds. In one of the acetate ion's resonance structures, the sp² hybrid orbitals of the carbon overlap with the orbitals of the adjoining atoms to form sigma bonds, while the unhybridized p orbital on the carbon overlaps with the appropriate p orbitals on the oxygen atoms to form a pi bond, contributing to the delocalized electron system.

Resonance Structures

Resonance refers to the representation of a molecule by two or more Lewis structures that contribute to the overall hybrid structure, indicating the delocalization of electrons within the molecule. In the acetate ion, resonance is depicted by two structures illustrating the shifting position of the double bond between the carbon and the oxygen atoms, which accounts for the equivalent bond characteristics observed in the ion.

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