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Chapter 8: Q29E (page 449)

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.

Short Answer

Expert verified

(a)\({\rm{s}}{{\rm{p}}^{\rm{2}}}\)with electrons delocalized.

(b)\({\rm{sp}}\)with electrons not delocalized.

(c)\({\rm{s}}{{\rm{p}}^{\rm{2}}}\)with electrons delocalized.

(d) \({\rm{s}}{{\rm{p}}^{\rm{3}}}\) with electrons delocalized.

Step by step solution

01

Define molecule

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.

02

Subpart (a)

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.

03

Subpart (b)

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

04

Subpart (c)

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

05

Subpart (d)

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

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Most popular questions from this chapter

Another acid in acid rain is nitric acid, HNO3, which is produced by the reaction of nitrogen dioxide, NO2, with atmospheric water vapor. What is the hybridization of the nitrogen atom in NO2? (Note: the lone electron on nitrogen occupies a hybridized orbital just as a lone pair would.)

Sulfuric acid is manufactured by a series of reactions represented by the following equations:

\(\begin{array}{l}{{\rm{S}}_{\rm{8}}}{\rm{(s) + 8}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{8S}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\\{\rm{2S}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2S}}{{\rm{O}}_{\rm{3}}}{\rm{(g)}}\\{\rm{S}}{{\rm{O}}_{\rm{3}}}{\rm{(g) + }}{{\rm{H}}_{\rm{2}}}{\rm{O(l)}} \to {{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{(l)}}\end{array}\)

Draw a Lewis structure, predict the molecular geometry by VSEPR, and determine the hybridization of sulfur for the following:

(a) circular \({{\rm{S}}_{\rm{8}}}\)molecule

(b) \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)molecule

(c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}\)molecule

(d) \({{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\)molecule (the hydrogen atoms are bonded to oxygen atoms)

Use valence bond theory to explain the bonding in\({{\rm{O}}_{\rm{2}}}\). Sketch the overlap of the atomic orbitals involved in the bonds in \({{\rm{O}}_{\rm{2}}}\).

The bond energy of a C鈥揅 single bond averages \({\rm{347 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\); that of a

C 鈮� C triple bond averages \({\rm{839 kJ mo}}{{\rm{l}}^{{\rm{ - 1}}}}\). Explain why the triple bond is not three times as strong as a single bond.

Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds: (a) \({\rm{ClNO}}\) (\({\rm{N}}\) is the central atom) (b) \({\rm{C}}{{\rm{S}}_{\rm{2}}}\) (c) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (\({\rm{C}}\) is the central atom) (d) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\) (\({\rm{S}}\) is the central atom) (e) \({\rm{S}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{S}}\) is the central atom) (f) \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{{\rm{F}}_{\rm{2}}}\) (\({\rm{Xe}}\) is the central atom) (g) \({\rm{ClO}}{{\rm{F}}_{\rm{2}}}^{\rm{ + }}\) (\({\rm{Cl}}\) is the central atom).
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