Why is molecular orbital theory useful?

Molecular orbital theory revolutionized the study of chemical bonding by approximating the states of bonded electrons—the molecular orbitals—as linear combinations of atomic orbitals (LCAO). Molecular orbital theory and valence bond theory are the foundational theories of quantum chemistry.

Which best describes the difference between valence bond theory and molecular orbital MO theory?

Valence bond theory assumes that electrons in a molecule are simply the electrons in the original atomic orbitals, with some used while bonding. By working out a full molecular orbital diagram to see how the electrons are distributed then, you are using molecular orbital theory.

Which of the following is the most important condition for valence bond theory?

An important aspect of the valence bond theory is the condition of maximum overlap, which leads to the formation of the strongest possible bonds. This theory is used to explain the covalent bond formation in many molecules.

Why are bonding molecular orbitals more stable than antibonding molecular orbitals?

Bonding molecular orbital has lower energy and hence greater stability than the corresponding antibonding molecular orbital.

What is valence bond theory What are the limitations of valence bond theory?

Limitations of Valence Bond Theory No insight offered on the energies of the electrons. The theory assumes that electrons are localized in specific areas. It does not give a quantitative interpretation of the thermodynamic or kinetic stabilities of coordination compounds. No distinction between weak and strong ligands.

What is valence bond theory and its limitations?

Limitations of Valence Bond Theory It has its own set of limitations. They are: It fails to explain the tetravalency of carbon. This theory does not discuss the electrons’ energies. The assumptions are about the electrons being localized to specific locations.