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

(N/A) Benzene is a hybrid of resonating structures as shown in the figure.
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 $C-C$ 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 $C-H$ sigma bonds.
The remaining unhybridized $p$-orbital of each carbon atom overlaps laterally to form a continuous $\pi$-electron cloud above and below the plane of the ring.
The six $\pi$-electrons are delocalized over the entire ring,which provides extra stability to the benzene molecule. This delocalization is the reason why benzene is extraordinarily stable despite having three double bonds.