The compound benzene has only one type of carbon-carbon...

Name: Problem 12, Chapter 1: Organic Chemistry
Uploaded: 2022-01-14T18:53:25-08:00
Duration: 1 min 59 s
Channel: Adriano Chikande
Description: The compound benzene has only one type of carbon-carbon bond, and this bond has a length intermediate between that of a single bond and a double bond. Draw a resonance structure of benzene that, taken with the following structure, accounts for the carbon-carbon bond length.

The compound benzene has only one type of carbon-carbon bond, and this bond has a length intermediate between that of a single bond and a double bond. Draw a resonance structure of benzene that, taken with the following structure, accounts for the carbon-carbon bond length.

Key Concepts

Aromaticity

Aromaticity is a property of cyclic, planar molecules with a conjugated ? electron system that meets specific criteria (such as Hückel’s rule). This results in exceptional stability and unique properties, including uniform bond lengths, due to the complete delocalization of electrons across the ring.

Resonance

Resonance is a concept in which more than one valid Lewis structure can be drawn for a molecule, with the actual structure being a hybrid of these forms. In aromatic systems, resonance explains the uniform distribution of electron density and bond characteristics, such as intermediate bond lengths, by showing how double bonds can shift positions.

Delocalization of Electrons

Delocalization refers to the spreading out of electrons over several adjacent atoms rather than being confined between just two. This phenomenon increases stability by allowing electrons to be shared throughout the entire molecule, particularly in cyclic conjugated systems like aromatic compounds.

Carbon-Carbon Bond Order

Carbon-carbon bond order describes the extent of bonding between carbon atoms, where a single bond has an order of 1 and a double bond has an order of 2. In molecules like benzene, the bond order is intermediate because the electrons associated with double bonds are delocalized, leading to bond lengths that are between those typical of single and double bonds.

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