Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 11: Problem 41

Explain why the concept of delocalized molecular orbitals is essential to an understanding of bonding in the benzene molecule, $\mathrm{C}_{6} \mathrm{H}_{6}$

Short Answer

Expert verified
The concept of delocalized molecular orbitals, which allows electrons to move freely across multiple atoms, is essential to understanding bonding in the benzene molecule. In benzene, six p electrons form delocalized molecular orbitals across all six carbon atoms, creating a ring of pi electron density that stabilizes the molecule and contributes to its unique chemical behavior.

Step by step solution

01

Describe Benzene Structure

Benzene, \( C_{6} H_{6} \), is an organic compound composed of six carbon atoms arranged in a hexagonal planar ring. Each carbon atom is bonded to its two neighbors and one hydrogen atom through sigma bonds. This leaves one electron in a p orbital perpendicular to the plane of the ring on each carbon atom.
02

Explain Concept of Delocalized Molecular Orbitals

In many molecules, electrons are not confined between two adjacent atoms, but rather can be spread over three or more atoms, creating delocalized molecular orbitals. These orbitals extend over several adjacent atoms, allowing electrons, particularly π electrons, to move freely across multiple atoms.
03

Link Concept of Delocalized Molecular Orbitals to Benzene

The six p electrons in the benzene molecule, which were not used in the sigma bonding, form delocalized molecular orbitals across all six carbon atoms. This delocalization creates a ring of pi electron density above and below the plane of the carbon atoms. It stabilizes the benzene molecule and contributes to its unique chemical behavior.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The energy gap, \(\Delta E\), for silicon is \(110 \mathrm{kJ} / \mathrm{mol}\). What is the minimum wavelength of light that can promote an electron from the valence band to the conduction band in silicon? In what region of the electromagnetic spectrum is this light?

The ion \(\mathrm{F}_{2} \mathrm{Cl}^{-}\) is linear, but the ion \(\mathrm{F}_{2} \mathrm{Cl}^{+}\) is bent. Describe hybridization schemes for the central \(\mathrm{Cl}\) atom consistent with this difference in structure.

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

Write plausible molecular orbital diagrams for the following heteronuclear diatomic species: (a) \(\mathrm{NO} ;\) (b) \(\mathrm{NO}^{+}\) (c) \(\mathrm{CO} ;\) (d) \(\mathrm{CN} ;\) (e) \(\mathrm{CN}^{-} ;\) (f) \(\mathrm{CN}^{+} ;\) (g) BN.

Which of the following substances, when added in trace amounts to silicon, would produce a \(p\) -type semiconductor: (a) sulfur, (b) arsenic, (c) lead, (d) boron, (e) gallium arsenide, (f) gallium? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Organic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free