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Chapter 11: Problem 89

Briefly describe each of the following ideas: (a) hybridization of atomic orbitals; (b) \(\sigma\) -bond framework; (c) Kekulé structures of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}\) (d) band theory of metallic bonding.

Short Answer

Expert verified
Hybridization of atomic orbitals involves atomic orbitals of similar energy on a single atom mixing to produce equal number of hybrid orbitals. Sigma bond is a strong covalent bond formed by head-to-head overlapping of orbitals on two different atoms. The Kekulé structures of benzene are two alternating ring structures composed of six carbon atoms each bonded to two others and one hydrogen atom. Band theory of metallic bonding describes how electrons behave in solids, forming closely spaced energy levels that allow electrons to move freely and conduct electricity.

Step by step solution

01

Explanation of Hybridization of Atomic Orbitals

Hybridization of atomic orbitals is a process by which several atomic orbitals of similar energy on a single atom mix to produce an equal number of hybridized orbitals. These hybrid orbitals are particularly useful in the description of the chemical bonding in molecules. For example, in methane, \(\mathrm{CH}_{4}\), the carbon atom forms four bonds suggesting that it utilizes four orbitals. These orbitals are the result of hybridization of its 2s, 2px, 2py, and 2pz orbitals.
02

Defining Sigma-Bond Framework

A sigma bond (σ-bond) is the strongest type of covalent chemical bond. They are formed by head-to-head overlapping of orbitals on two different atoms. A single bond is usually a sigma bond. Molecules with multiple bonds, like double and triple bonds, have sigma bonds as well. For example, in carbon dioxide, \(\mathrm{CO}_{2}\), each oxygen atom is sigma-bonded to the carbon atom.
03

Illustrating Kekulé structures of Benzene

The Kekulé structures of benzene, \(\mathrm{C}_{6} \mathrm{H}_{6}\), are two equivalent and alternating forms of the ring structure for benzene. This model proposes that benzene is composed of a ring of six carbon atoms where each carbon atom is bonded to two others and one hydrogen atom. Two forms are created by alternating double and single bonds between carbon atoms. These structures are often drawn with a circle inside a hexagon to signify the delocalized electrons.
04

Understanding Band Theory of Metallic Bonding

The band theory describes how electrons behave in solids. Metals have many closely spaced empty energy levels that electrons can move into. These closely spaced energy levels form a 'band'. Since there are many empty energy levels, electrons can move freely, which allows metals to conduct electricity. This forms the basis for the band theory of metallic bonding.

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Most popular questions from this chapter

Construct a concept map that connects the ideas of molecular orbital theory.

Consider the molecules \(\mathrm{CO}^{+}\) and \(\mathrm{CN}^{-}\) and use molecular orbital theory to answer the following: (a) Write the molecular orbital configuration of each ion (ignore the 1 s electrons). (b) Predict the bond order of each ion. (c) Which of these ions is paramagnetic? Which is diamagnetic? (d) Which of these ions do you think has the greater bond length? Explain.

Construct a molecular orbital diagram for \(\mathrm{HF}\), and label the molecular orbitals as bonding, antibonding, or nonbonding.

Describe the bond order of diatomic carbon, \(\mathrm{C}_{2},\) with Lewis theory and molecular orbital theory, and explain why the results are different.

In which of the following, \(\mathrm{CO}_{3}^{2-}, \mathrm{SO}_{2}, \mathrm{CCl}_{4}, \mathrm{CO}\) \(\mathrm{NO}_{2}^{-},\) would you expect to find \(s p^{2}\) hybridization of the central atom? Explain.
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