Final answer:
Aromatic carbon compounds like benzene are stabilized by electron resonance, where pi electrons are delocalized over the entire molecule, contributing to their unique stability and reactivity.
Step-by-step explanation:
The characteristic of benzene being planar and very stable with double-bond character extending around the entire ring is caused by electron resonance. Benzene, an aromatic carbon compound, displays a form of bonding where the pi electrons are delocalized over the entire structure of the molecule. This delocalization is marked by a hexagon with a circle inside, representing an electron-rich region surrounding the six carbon atoms of the ring. The electrons in the benzene ring contribute to the stability of the molecule, making it less reactive than other hydrocarbons with a similar size.
Aromatic hydrocarbons like benzene are important in a wide range of natural substances and biomolecules, and they exhibit unique physical and chemical properties that differ greatly from those of alkanes. The sp² hybridization of the carbon atoms in benzene leads to a flat planar structure, favoring delocalization and contributing to the molecule's notable stability. Aromaticity, governed by the Huckel rule, provides significant resonance stabilization, known as aromatic stabilization, making these compounds more stable than otherwise expected.