Benzene

Many compounds can have the chemical formula C₆H₆.

One of these structures is benzene, which contains a six-sided carbon ring with 120° bond angles.

Experimental evidence shows that, in benzene, all of the carbon-carbon bonds are equal in length and strength.

Structure of Benzene

The explanation for the true structure of benzene is resonance.

Electrons in the double bonds of benzene are delocalized and can spread equally throughout the entire ring.

This results in carbon-carbon bonds that are equal in length and strength

Properties of Benzene

Resonance makes benzene very stable.

Usually, substances with such a high carbon to hydrogen ratio are more reactive.

Molecular Orbitals

When two orbitals overlap head-on, a (sigma) σ-bond is formed. Each orbital donates one electron to the sigma bond. The two orbitals forming the σ-bond fuse into a molecular orbital. Both electrons would go into the molecular orbital.

When two orbitals overlap side-to-side, a (pi) π-bond is formed. Each orbital donates an electron to the bond. In benzene, there are many π- bonds. The six electrons in those π-bonds are distributed into 3 molecular orbitals with two electrons in each orbital.

Resonance

when more than one Lewis structure can be drawn for a molecule

Resonance hybrids are the best descriptions of actual compound. They show delocalized electrons.

ex: CO3^-2