Delocalization of Electrons Section 14.3. Introduction Delocalization allows the pi electrons to...

Delocalization of Electrons

Section 14.3

Introduction

Delocalization allows the pi electrons to spread over more than two nuclei

This spreading out of the electrons gives the species a lower potential energy making it more stable

Best example is with benzene The molecule is a planar hexagonal shape Each carbon atom is sp2 hybridized

More about Benzene

One of the sp2 orbitals forms a sigma bond with H Two other orbitals forms sigma bonds with the C on

each side The remaining electron is in a p-orbital

perpendicular to the plane of the sigma bonds These p-orbitals on each C atom interact to produce

a delocalized pi bond The ring has high electron density above and below

the ring

Benzene Ring

Ethene (C2H4) Benzene (C6H6)

More

Resonance hybrids show delocalization of electrons which leads to: Greater stability and an intermediate bond length

and strength Less reactivity Ability to conduct electricity (because electrons are

more free to move, i.e. delocalized)