Question

@ Explain the delocalization energy СА (resonance)
of benzene in terms of nodal planes, energies
of columbic forces and resonance terms​

Answer 1

Answer:

The advantage of MO theory becomes more apparent when we think about π bonds, especially in those situations where two or more π bonds are able to interact with one another. Let’s first consider the π bond in ethene from an MO theory standpoint (in this example we will be disregarding the various sigma bonds, and thinking only about the π bond). According to MO theory, the two atomic 2pz orbitals combine to form two π molecular orbitals, one a low-energy π bonding orbital and one a high-energy π-star (π*) antibonding molecular orbital. These are sometimes denoted in molecular diagrams with the Greek letter psi (Ψ) instead of π (Figure 11.6.1 ).

Answer 2

Answer:

delocalized bonding

The advantage of MO theory becomes more apparent when we think about π bonds, especially in those situations where two or more π bonds are able to interact with one another. Let’s first consider the π bond in ethene from an MO theory standpoint (in this example we will be disregarding the various sigma bonds, and thinking only about the π bond). According to MO theory, the two atomic 2pz orbitals combine to form two π molecular orbitals, one a low-energy π bonding orbital and one a high-energy π-star (π*) antibonding molecular orbital. These are sometimes denoted in molecular diagrams.