According to this theory, the carbon atoms of the benzene molecule are hybridized trigonal (sp2 orbital ) which agrees with bond angles 120 ° and the hexagon formula.
Two of the sp2 orbital of each carbon overlap with two of its neighbors to form the hexagonal ring. The third orbital sp2 are links to the respective hydrogen atom. All these links both carbon-carbon, as carbon-hydrogen are signa-type and illustrated in the figure below.
carbocycle part of the molecule of benzene, consists entirely of links signa.
But recoprdemos that the fourth electron trigonal hybridization of the carbon atom remains in the 2pz orbital , which has not perpendincular hibiridado and the plane of the hybrid orbitals. The following figure shows the system formed by the six orbital P.
A quarter of a valence electron of each carbon atom in benzene remains in the 2pz orbital
Thus, each carbon atom would be the ability to form a pi bond with its neighbor. But since there are two neighboring atoms, linking two alternatives, which are represented schematically in Figure 1 and can be considered as belonging to the two resonance structures of benzene.
Each carbon atom in benzene is possible to form pi bonds with one or other of its neighbors, which gives rise to two alternative structures.
Both forms can set with equal justification, that is, neither has primacy over the other. Since it is possible that this molecule simultaneously the two structures, what happens is that electornes P (six in total) together form a pi system that takes the form of a ring with two regions, and the other by Ensim below the plane of the links signa, as illustrated in Fig.
The p electron of benzene is forming a pi-type electronically tag, which is shaped like a ring with two localisé regions on both sides of the plane of the links signa.
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