Bond Order Calculator

Bond order is a measure of the number of chemical bonds between two atoms. It indicates bond stability and strength - higher bond order means stronger, shorter bonds with higher bond energy.

For diatomic molecules, use the formula: Bond Order = (Bonding electrons - Antibonding electrons) / 2. Count electrons in bonding and antibonding molecular orbitals from the MO diagram.

Bonding electrons occupy molecular orbitals that stabilize the bond, while antibonding electrons occupy orbitals that destabilize it. Antibonding orbitals are higher in energy and weaken the overall bond.

Calculate the average bond order by dividing total bond-order units by the number of equivalent bonds. For example, CO₃²⁻ has 4 bond-order units distributed among 3 equivalent C-O bonds, giving 4/3 = 1.33.

Fractional bond orders occur in molecules with resonance structures or unpaired electrons. For example, NO has a bond order of 2.5, indicating it's between a double and triple bond in strength.

Yes, a bond order of zero means no net bonding (like He₂), indicating the molecule is unstable. Negative bond orders are theoretically possible but represent highly unstable, non-existent bonds.

H₂ has bond order 1, O₂ has bond order 2, N₂ has bond order 3, and NO has bond order 2.5. These correspond to single, double, triple, and intermediate bonds respectively.

Higher bond order means shorter bond length and higher bond energy. Triple bonds (order 3) are shorter and stronger than double bonds (order 2), which are shorter and stronger than single bonds (order 1).