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Chapter 11: Problem 90

Explain the important distinctions between the terms in each of the following pairs: (a) \(\sigma\) and \(\pi\) bonds; (b) localized and delocalized electrons; (c) bonding and antibonding molecular orbitals; (d) metal and semiconductor.

Short Answer

Expert verified
σ bonds are based on a direct overlap of atomic orbitals, making them stronger than π bonds that are based on a perpendicular overlap. Localized electrons are confined to a specific atom or bond, while delocalized electrons are spread over several adjacent atoms. Bonding molecular orbitals are formed when atomic orbitals combine to decrease energy, resulting in stability, while antibonding orbitals result from enough energy difference, leading to instability. Metals have high electrical conductivity and allow free electron movement, while a semiconductor's lower conductivity can be manipulated through doping.

Step by step solution

01

Analyze the Difference between σ and π bonds

In a σ bond, the bonding electrons are located in the area directly between the two atomic nuclei. This is the strongest type of covalent bond because the electron pair is held firmly between the two nuclei. On the other hand, a π bond is based on the overlap of p orbitals perpendicular to the line that directly connects the two nuclei. Sharing two electron pairs, π bonds are weaker than σ bonds because of the less significant overlap of atomic orbitals.
02

Distinguish Localized and Delocalized Electrons

Electrons in an atom can either be localized or delocalized. Localized electrons are those electrons that are confined to one orbital, either in a bond or lone pair. These electrons belong to definite atoms and stay near those atoms. In contrast, delocalized electrons are not attached to a single atom or a covalent bond. Instead, they are spread over several adjacent atoms which often gives compounds distinctive properties.
03

Differentiate Bonding and Antibonding Molecular Orbitals

A bonding molecular orbital refers to the formation of an orbital when two atomic orbitals of similar energies combine. This results in a decrease in energy, leading to a stable configuration. Antibonding molecular orbitals, however, are created when the two atomic orbitals have enough difference in energy levels. The result is an unstable configuration because the energy of the antibonding molecular orbital is higher than the energy of the original atomic orbitals.
04

Compare Metal and Semiconductor

A metal is a substance that has high electrical conductivity, lustre, and ductility, and which freely allows the movement of electrons, leading to the characteristic property of conductivity. A semiconductor, however, has lower conductivity than a metal. It cannot freely allow the movement of electrons, but its electrical conductivity can be manipulated by the addition of impurities, known as doping. This property makes semiconductors essential components in modern electronic devices.

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Most popular questions from this chapter

For the following pairs of molecular orbitals, indicate the one you expect to have the lower energy, and state the reason for your choice. (a) \(\sigma_{1 s}\) or \(\sigma_{1 s}^{*} ;\) (b) \(\sigma_{2 s}\) or \(\sigma_{2 p}\) (c) \(\sigma_{1 s}^{*}\) or \(\sigma_{2 s} ;\) (d) \(\sigma_{2 p}\) or \(\sigma_{2 p}^{*}\)

Explain why the electrical conductivity of a semiconductor is significantly increased if trace amounts of either donor or acceptor atoms are present, but is unchanged if both are present in equal number.

Is it correct to say that when a diatomic molecule loses an electron, the bond energy always decreases (that is, that the bond is always weakened)? Explain.

Lewis theory is satisfactory to explain bonding in the ionic compound \(\mathrm{K}_{2} \mathrm{O},\) but it does not readily explain formation of the ionic compounds potassium superoxide, \(\mathrm{KO}_{2}\), and potassium peroxide, \(\mathrm{K}_{2} \mathrm{O}_{2}\) (a) Show that molecular orbital theory can provide this explanation. (b) Write Lewis structures consistent with the molecular orbital explanation.

Explain how it is possible to avoid the concept of resonance by using molecular orbital theory.
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