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Chapter 11: Problem 42

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

Short Answer

Expert verified
The concept of resonance is bypassed in Molecular Orbital (MO) theory because it provides a better depiction of electron behavior. Resonance suggests that electrons move between multiple locations, whereas in MO theory, electrons are in a superimposed state, occupying molecular orbitals spread over the molecule. Therefore, a molecule doesn't need multiple resonance structures for its representation as required in resonance theory.

Step by step solution

01

Understanding the Concept of Resonance

Resonance is a concept in chemistry where a molecule cannot be aptly described by a single Lewis structure. Instead, multiple Lewis structures, called resonance structures, are used to depict the molecule. Although resonance structures individually do not represent actual structures of the molecule, the true structure is considered to be an amalgamation of these structures. This is often simplified by representing the molecule with a resonance hybrid, where the bonding in the molecule is spread out, or delocalized, over the entire molecule.
02

Understanding the Concept of MO Theory

Molecular Orbital theory is an advanced method of examining bonding in molecules. It combines the atomic orbitals of the atoms in a molecule to produce new mathematical objects called molecular orbitals, which describe the behavior and energetics of electrons in molecules. In MO theory, electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the atomic nuclei in the whole molecule. This is a more sophisticated view than the localized bond approach.
03

Correlating MO Theory with Resonance

In resonance theory, the location of electrons and the shape of the molecule changes from one resonance structure to another, giving the impression that the molecule oscillates between forms. But MO theory, due to its quantum mechanical basis, presents a tough picture: electrons are in a superimposed state, occupying molecular orbitals that are spread (delocalized) over the entire molecule, and they do not 'jump around' or oscillate between states. Therefore, the concept of resonance is not needed when molecules are described using MO theory.

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Most popular questions from this chapter

Use the valence molecular orbital configuration to determine which of the following species is expected to have the greatest electron affinity: (a) \(\mathrm{C}_{2}^{+} ;\) (b) \(\mathrm{Be}_{2}\) (c) \(\mathrm{F}_{2} ;\) (d) \(\mathrm{B}_{2}^{+}\)

Construct a concept map that embodies the ideas of valence bond theory.

Why does the hybridization \(s p^{3} d\) not account for bonding in the molecule BrF \(_{5} ?\) What hybridization scheme does work? Explain.

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.

Consider the molecules \(\mathrm{NO}^{+}\) and \(\mathrm{N}_{2}^{+}\) 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.
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