Benzene is a hybrid of resonating structures given as: 

All six carbon atoms in benzene are $S{p}^2$ hybridized. The two $S{p}^2$ hybrid orbitals of each carbon atom overlap with the $S{p}^2$ hybrid orbitals of adjacent carbon atoms to form six sigma bonds in the hexagonal plane. The remaining $S{p}^2$ hybrid orbital on each carbon atom overlaps with the s-orbital of hydrogen to form six sigma C–H bonds. The remaining unhybridized p-orbital of carbon atoms has the possibility of forming three π bonds by the lateral overlap of

$C_1 - C_2 , C_3 - C_4 , C_5 - C_6 , or C_2 , C_4 - C_5 , C_6 - C_1$

                             

The six π’s are delocalized and can move freely about the six-carbon nuclei. Even after the presence of three double bonds, these delocalized π-electrons stabilize benzene.