How do you find pure hybrid orbitals in benzene?

In benzene, which has a planar structure and a symmetrical arrangement of carbon atoms, the carbon atoms undergo hybridization to form sp² hybrid orbitals. Each carbon atom combines one s orbital and two p orbitals to create three equivalent sp² hybrid orbitals, which are oriented 120 degrees apart in a plane. This hybridization allows for the formation of sigma bonds with adjacent carbon atoms and one hydrogen atom, while the remaining unhybridized p orbital on each carbon atom overlaps to form a delocalized pi bond system, contributing to benzene's stability and aromatic properties.