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Chapter 15: Problem 5

How do the calculated bond orders for benzene compare to the bond orders predicted by the Lewis structure?

Short Answer

Expert verified
The bond order for benzene, calculated using both the Lewis structure and Molecular Orbital Theory, is 1.5. This means that the Lewis structure prediction and the theoretical calculation agree.

Step by step solution

01

Understanding bond order

The bond order is a measure of the number of shared electron pairs between two atoms in a molecule. It is used to estimate the strength of the bond. A higher bond order implies a stronger, shorter bond.
02

Predicting bond order using Lewis structure

The Lewis structure for benzene shows a hexagon of carbon atoms, with alternating double and single bonds and a hydrogen atom attached to each carbon. This means the six carbon-carbon bonds in benzene are neither double bonds nor single bonds, but a blend of both. Therefore, the average bond order predicted by the Lewis structure is \( \frac{1+2}{2} = 1.5 \). This means there are 1.5 bonds per carbon-carbon connection in benzene.
03

Calculated bond order using Molecular Orbital Theory

According to the Molecular Orbital Theory (which uses quantum mechanics), the electrons in a benzene molecule are delocalized over the entire molecule, creating a ring of electron density above and below the plane of the carbon atoms. This means that all carbon-carbon bonds in benzene are equivalent and share the same bond order. Thus, the calculated bond order would still be 1.5.
04

Comparison

Comparing the bond orders predicted by the Lewis structure and calculated using the Molecular Orbital Theory, it can be confirmed that both methods yield the same bond order of 1.5 for benzene. Therefore, the bond orders of benzene calculated using these two methods are in agreement.

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Most popular questions from this chapter

Predict the \(\mathrm{C}-\mathrm{C}\) bond length for a molecule with a \(\mathrm{C}-\mathrm{C}\) bond order of \(1.5\).

How do the calculated bond orders for ethane, ethene, and ethyne compare to bond orders predicted by the Lewis structures?
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