<Dd> B.O. = number of bonding electrons − number of antibonding electrons 2 (\ displaystyle (\ text (B.O.)) = (\ frac ((\ text (number of bonding electrons)) - (\ text (number of antibonding electrons))) (2)) \) </Dd> <P> Generally, the higher the bond order, the stronger the bond . Bond orders of one - half may be stable, as shown by the stability of H (bond length 106 pm, bond energy 269 kJ / mol) and He (bond length 108 pm, bond energy 251 kJ / mol). </P> <P> The bond order concept is used in molecular dynamics and bond order potentials . The magnitude of the bond order is associated with the bond length . According to Linus Pauling in 1947, the bond order is experimentally described as </P> <Dl> <Dd> s i j = exp ⁡ (d 1 − d i j b) (\ displaystyle s_ (ij) = \ exp (\ left ((\ frac (d_ (1) - d_ (ij)) (b)) \ right))) </Dd> </Dl>

What is the bond order of the carbon- carbon bond in the ethylene molecule