According to MO theory, which molecule or ion has the highest bond energy? O₂, O₂^- , O₂^2-

Verified step by step guidance

1. Identify the molecular orbitals (MOs) for each species: O_2, O_2^-, and O_2^{2-}.
2. Determine the electron configuration for each species using the MO diagram for diatomic oxygen molecules.
3. Calculate the bond order for each species using the formula: Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2.
4. Compare the bond orders: the higher the bond order, the higher the bond energy.
5. Conclude which species has the highest bond energy based on the bond order comparison.

Key Concepts

Molecular Orbital Theory (MO Theory)

Molecular Orbital Theory describes the behavior of electrons in molecules, where atomic orbitals combine to form molecular orbitals that can be occupied by electrons. This theory helps predict the bond order, stability, and magnetic properties of molecules by considering the distribution of electrons across these orbitals.

Bond Energy

Bond energy is the amount of energy required to break a bond between two atoms in a molecule. It is a measure of the bond's strength; higher bond energy indicates a stronger bond. In the context of MO theory, bond energy can be related to the bond order, which is the difference between the number of bonding and antibonding electrons.

Bond Order

Bond order is a concept in MO theory that quantifies the number of chemical bonds between a pair of atoms. It is calculated as half the difference between the number of bonding and antibonding electrons. A higher bond order typically correlates with greater bond strength and stability, influencing the bond energy of the molecule or ion.