why is the bond order of CO+ 3.5??? explain in detail
Answers
he highest occupied molecular orbital (or HOMO) is the σ *2s MO. Bond order is defined as the number of electrons in bonding MOs minus the number of electrons in antibonding MOs .
The order of energy of the orbitals is “not” the same as it would be for a homonuclear diatomic molecule such as O2 where both atoms are the same.
For heteroatomic dinuclear molecule, energy of BMO closely matches with those of more electronegative atom & energy of ABMO closely matches with those of less electronegative atom.
In the case of CO, the 2s atomic orbital on Oxygen is much lower in energy than the 2s atomic orbital in carbon.
The discrepancy in energies allows the π2px & π2py bonding molecular orbitals to sink lower in energy than the “ σ*2s MO” in the MO diagram of CO.
For CO+: electron is removed from σ*2s MO hence,
Bond Order of CO+ = (8-1)/2 = 3.5
Answer:
Bond order is a number that tells us how strong the bond between two atoms forming a molecule is. The BO in CO+ is 3.5 because the order of the orbitals is not the same as it would be for a homonuclear diatomic molecule such as O2where both atoms are the same.
Bond order = [(Number of electrons in bonding molecules) - (Number of electrons in antibonding molecules)]/2
Total number of electrons = 6 + 8 = 14.
The bond order of CO is 3.
The BO in CO+ is 3.5 because the order of the orbitals is not the same as it would be for a homonuclear diatomic molecule such as O2where both atoms are the same.
The bond order of CO+ = (8-1)/2 = 3.5