Final answer:
The incorrect statement is that benzene 'contains double bonds.' Instead, benzene's structure features delocalized electrons that contribute to its stability and make it an aromatic compound with unique chemical reactivity.
Step-by-step explanation:
The statement that is not correct about benzene is that it 'contains double bonds'. While benzene is often depicted as having alternating single and double bonds, its electrons are actually delocalized over the aromatic ring structure.
Benzene is an aromatic compound, but the uniqueness of its structure means the typical double bond reactivity is not observed. Instead, the pi bonding electrons are free to move around the ring, creating a ring of electron density that contributes to its stability and particular chemical properties.
The stability of the benzene ring differentiates it from alkenes, which have distinct, localized double bonds that react differently. The molecular formula of benzene is C6H6, and despite the appearance of alternating single and double bonds in its typical representations, it does not partake in the type of reactions you would expect from such a structure.