The bond order of O2 is 2, which signifies a double bond between the two oxygen atoms. This value is derived using the molecular orbital theory, considering the distribution of electrons in bonding and nonbonding orbitals.
Understanding Bond Order
Bond order is a crucial concept in chemistry, particularly in molecular orbital theory. It quantifies the number of chemical bonds between a pair of atoms in a molecule. A higher bond order generally indicates a stronger, shorter, and more stable bond.
The general formula to calculate bond order is:
Bond Order = 1/2 (Number of Bonding Electrons - Number of Nonbonding Electrons)
Calculating Bond Order for O2
To determine the bond order for the O2 molecule, we follow these steps based on its molecular orbital configuration:
- Identify Bonding Electrons: In the molecular orbital configuration of O2, there are 10 bonding electrons occupying the bonding molecular orbitals. These electrons contribute to the formation and stability of the chemical bond between the oxygen atoms.
- Identify Nonbonding Electrons: Correspondingly, there are 6 nonbonding (antibonding) electrons occupying the antibonding molecular orbitals. These electrons work against the bond formation.
- Apply the Bond Order Formula:
- Substitute the electron counts into the formula:
Bond Order = 1/2 (10 - 6) - Perform the subtraction:
Bond Order = 1/2 (4) - Complete the calculation:
Bond Order = 2
- Substitute the electron counts into the formula:
This calculation precisely demonstrates that the bond order for the O2 molecule is 2, indicating a stable double bond. This double bond is characteristic of diatomic oxygen, explaining its properties and typical molecular structure.
