Why is benzene non-polar?

Benzene is a non-polar molecule due to its symmetrical and planar structure. It consists of six carbon atoms forming a hexagonal ring with alternating single and double carbon-carbon bonds. Each carbon atom is also bonded to a hydrogen atom.

The carbon-carbon double bonds in benzene result in the presence of pi (π) electrons, which are spread over the entire ring rather than localized between two specific carbon atoms. This delocalization of π electrons creates a cloud of electron density above and below the plane of the molecule.

Since the π electrons are evenly distributed around the benzene ring, there are no significant differences in electronegativity or partial charges between carbon atoms. Additionally, the carbon-hydrogen bonds are nonpolar as well because the electronegativity difference between carbon and hydrogen is relatively small.

As a result of this symmetrical distribution of electrons and the lack of any significant dipole moments within the molecule, benzene is considered a non-polar molecule. It does not have a permanent dipole moment and does not exhibit strong intermolecular forces like hydrogen bonding or dipole-dipole interactions. Instead, it experiences relatively weaker dispersion forces (London dispersion forces) as the dominant intermolecular force.