The resonance structure of benzene is represented by two alternating structures, where the double bonds between the carbon atoms are located in different positions. These two structures are often depicted with a circle inside a hexagon, which represents the delocalization of the electrons.Benzene C6H6 is an aromatic hydrocarbon with a planar hexagonal ring of six carbon atoms, each bonded to a hydrogen atom. In the resonance structure, each carbon atom forms three bonds: one single bond with a hydrogen atom and two other bonds with adjacent carbon atoms. These two bonds with carbon atoms alternate between single and double bonds in the two resonance structures.The delocalization of electrons in benzene refers to the spreading of the six pi electrons across all six carbon atoms in the ring. Instead of being confined to individual double bonds, the electrons are shared equally among all the carbon atoms. This delocalization creates a stable electron cloud above and below the plane of the carbon atoms, which contributes to the stability of the compound.The stability of benzene can be explained by the concept of resonance energy. The actual structure of benzene is a hybrid of the two resonance structures, which results in a lower overall energy than either of the individual structures. This energy difference between the actual structure and the hypothetical isolated structures is called the resonance energy, and it contributes to the stability of benzene.In summary, the resonance structure of benzene consists of two alternating structures with different positions of double bonds. The delocalization of electrons across all six carbon atoms in the ring contributes to the stability of the compound, as it lowers the overall energy of the molecule.