Why is benzene extraordinarily stable though it contains three double bonds?

(N/A) Benzene is a hybrid of resonating structures. All six carbon atoms in benzene are $sp^2$ hybridized.
The two $sp^2$ hybrid orbitals of each carbon atom overlap with the $sp^2$ hybrid orbitals of adjacent carbon atoms to form six sigma bonds in the hexagonal plane.
The remaining $sp^2$ 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 $\pi$ bonds by the lateral overlap of $C_1-C_2, C_3-C_4, C_5-C_6$ or $C_2-C_3, C_4-C_5, C_6-C_1$.
The six $\pi$ electrons are delocalized and can move freely about the six carbon nuclei.
Even with the presence of three double bonds,these delocalized $\pi$-electrons provide extra stability to benzene due to resonance energy.