Bond order of O₂⁺
Bond order 2.5, paramagnetic. 15 electrons: Nb = 10, Na = 5.
Molecular orbitals
15 electrons2.5bond order
paramagnetic
paramagnetic
(Nb − Na) / 2 = (10 − 5) / 2
The atom columns show neutral atoms; the ion has 1 fewer electron in the molecule.
σ1s² σ*1s² σ2s² σ*2s² σ2pz² (π2px² = π2py²) (π*2px¹ = π*2py⁰)
Bond order step by step
- O₂⁺ has 15 electrons: 8 from each O, minus one for the positive charge.
- For O₂, F₂ and their ions, σ2pz lies below the π2p pair and fills first.
- Configuration: σ1s² σ*1s² σ2s² σ*2s² σ2pz² (π2px² = π2py²) (π*2px¹ = π*2py⁰)
- Bonding electrons Nb = 10, antibonding electrons Na = 5.
- Bond order = (Nb − Na) / 2 = (10 − 5) / 2 = 2.5.
- One electron is unpaired (in one of the π*2p orbitals), so O₂⁺ is paramagnetic.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Bond order of O2+: quick answers
What is the bond order of O2+?
2.5. Bond order = (Nb − Na) / 2 = (10 − 5) / 2 = 2.5. Bonding electrons Nb = 10, antibonding electrons Na = 5.
Is O2+ paramagnetic or diamagnetic?
Paramagnetic. One electron is unpaired (in one of the π*2p orbitals), so O₂⁺ is paramagnetic.
What is the molecular orbital configuration of O2+?
σ1s² σ*1s² σ2s² σ*2s² σ2pz² (π2px² = π2py²) (π*2px¹ = π*2py⁰), with 15 electrons in all.