Pi-molecular orbital diagram of Benzene.

The pi-molecular orbital diagram of benzene can be explained in the following steps:

1. Benzene is a cyclic compound with 6 carbon atoms. Each carbon atom is sp2 hybridized, with one of its p-orbitals unhybridized. These p-orbitals overlap sideways to form pi-bonds.

2. The six overlapping p-orbitals form a pi-molecular orbital system. This system is delocalized, meaning the electrons are not confined to one bond or atom, but spread over the entire molecule.

3. The pi-molecular orbital system of benzene is represented by a diagram showing the energy levels of the molecular orbitals. The diagram has two levels: bonding and antibonding.

4. The bonding level is lower in energy and is more stable. It is formed by the constructive interference of the wave functions of the atomic orbitals. In benzene, this level is doubly degenerate, meaning it has two orbitals of the same energy. These are filled with 4 electrons.

5. The antibonding level is higher in energy and less stable. It is formed by the destructive interference of the wave functions of the atomic orbitals. In benzene, this level is triply degenerate, meaning it has three orbitals of the same energy. These are filled with 2 electrons.

6. The resulting pi-molecular orbital diagram of benzene shows a stable molecule with a fully filled bonding level and a partially filled antibonding level. This explains the aromaticity and stability of benzene.