Why are aromatic compounds considered stable?

Aromatic compounds are considered stable primarily due to the presence of delocalized π electrons that form resonance structures. In aromatic systems, particularly those following Huckel's rule (which states that a compound must have 4n + 2 π electrons, where n is a non-negative integer), the electrons are shared over the entire ring structure rather than being associated with a single bond.

This delocalization results in a lower overall energy for the molecule, enhancing its stability significantly compared to non-aromatic compounds. The resonance structures that can be drawn indicate that the actual structure is a hybrid of these forms, leading to bonds that are of equal length and strength, unlike typical alternating single and double bonds.

The stability provided by these delocalized electrons is a key characteristic of aromatic compounds, making option C the correct choice. Factors like the presence of single bonds, localized electrons, or saturation with hydrogen do not account for the unique stability associated with aromatic compounds in the same way.