(a) Why does the bond order of O₂⁻ decrease compared to O₂? What does this imply about the stability and bond length of O₂⁻? (b) Can a molecule with an odd number of electrons ever be diamagnetic? Explain why or why not. (c) If molecular orbitals are created by combining five atomic orbitals from atom A and five atomic orbitals from atom B combine, how many molecular orbitals will result?

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Molecular Orbital Theory for Homonuclear Diatomic Molecules, Bond Order and Magnetic Properties from MO Theory | PadhAiPro

Question

TextMolecular Orbital Theory for Homonuclear Diatomic MoleculesBond Order and Magnetic Properties from MO Theory

Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.

Use molecular orbital theory to explain why the Be2 molecule does not exist.

Compare the relative stability of the following species and indicate their magnetic properties; O2, O2⁺, O2⁻ (superoxide), O2²⁻ (peroxide)

Write the significance of a plus and a minus sign shown in representing the orbitals.

What is meant by the term bond order? Calculate the bond order of : N2, O2, O2⁺ and O2⁻.

Which of the following statements is true regarding the molecular orbital theory for homonuclear diatomic molecules?