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Chapter 5: Problem 73

Are resonance structures examples of electron delocalization? Explain your answer.

Short Answer

Expert verified
Explain your answer. Answer: Yes, resonance structures are examples of electron delocalization. This is because resonance structures represent the idea that the true structure of certain molecules cannot be described by a single Lewis structure. Instead, the actual electronic distribution is an average of the contributing resonance forms, which shows that electrons are shared among multiple locations in the molecule, rather than being fixed to specific bonds or lone pairs. This spreading of electrons over multiple bonding arrangements represents electron delocalization.

Step by step solution

01

Understand Resonance Structures and Electron Delocalization

To solve the problem, it is important to know what resonance structures and electron delocalization are: Resonance Structures: They are different Lewis structures that represent the same molecule and illustrate the fact that several arrangements of bonds and lone pairs can legitimately describe the molecule's electron distribution. Electron Delocalization: It refers to the spreading of electron density over a larger region of space, instead of being confined to a specific area, usually in molecules with conjugated systems or alternating single and double bonds.
02

Relate Resonance Structures to Electron Delocalization

Resonance structures capture the idea that the true structure of certain molecules cannot be represented by a single Lewis structure. Instead, the actual electronic distribution is an average of the contributing resonance forms. This implies that the electrons are not fixed to a particular set of bonds or lone pairs but rather shared among multiple locations in the molecule.
03

Conclude and Explain the Answer

Based on the relationship between resonance structures and electron distribution, resonance structures are indeed examples of electron delocalization. The reason is that they illustrate the spreading of electrons over multiple bonding arrangements in the molecule. So, instead of being confined to a specific location, the electrons are delocalized and spread out over a larger area in the molecule.

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