For each of the following molecules, indicate the hybridization requested and whether or not the electrons will be delocalized: (a) ozone (\({{\rm{O}}_{\rm{3}}}\)) central \({\rm{O}}\) hybridization (b) carbon dioxide (\({\rm{C}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{C}}\) hybridization (c) nitrogen dioxide (\({\rm{N}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{N}}\) hybridization (d) phosphate ion (\({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\)) central \({\rm{P}}\) hybridization.

A molecule is the smallest unit of a substance that holds the compound's chemical characteristics. Molecules are made up of atoms arranged in groups.

Ozone (\({{\rm{O}}_{\rm{3}}}\)): In a trigonal planar structure, the oxygen atom is surrounded by three zones of electron density. In a trigonal planar electron pair geometry, the hybridization is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\), and the electrons are delocalized.

Carbon dioxide (\({\rm{C}}{{\rm{O}}_{\rm{2}}}\)): The carbon atom is surrounded by two electron density zones that are arranged in a linear pattern. In a linear electron pair geometry, the hybridization is \({\rm{sp}}\), and the electrons are not delocalized.

Carbon dioxide

Nitrogen dioxide (\({\rm{N}}{{\rm{O}}_{\rm{2}}}\)): In a trigonal planar structure, the core nitrogen atom is surrounded by three zones of electron density. In a trigonal planar electron pair geometry, the hybridization is \({\rm{s}}{{\rm{p}}^{\rm{2}}}\), and the electrons are delocalized.

Nitrogen dioxide molecule

Phosphate ion (\({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\)): In a tetrahedral structure, the core phosphorus atom is surrounded by four zones of electron density. In a tetrahedral electron pair geometry, the hybridization is \({\rm{s}}{{\rm{p}}^{\rm{3}}}\) and the electrons are delocalized

Phosphate ion