Bond order of N₂
Bond order 3, diamagnetic. 14 electrons: Nb = 10, Na = 4.
Molecular orbitals
14 electrons3bond order
diamagnetic
diamagnetic
(Nb − Na) / 2 = (10 − 4) / 2
σ1s² σ*1s² σ2s² σ*2s² (π2px² = π2py²) σ2pz²
Why this shape
- Each N has 5 valence electrons. It uses three in one triple bond to N, so two are left as one lone pair.
- Steric number = one sigma bond + one lone pair = 2, so each N is sp hybridised. A double or triple bond counts once: only its sigma bond uses a hybrid orbital.
- Two electron pairs point in opposite directions, along a line (linear electron geometry). With only two atoms, the molecule itself is a straight line.
- Two atoms always lie on a straight line, so there is no bond angle.
- Both atoms are the same, so the bond is non-polar.
Lewis structure
10 valence electronsFormal charges: none
Bond order step by step
- N₂ has 14 electrons: 7 from each N.
- Up to N₂ (and its ions), the π2p pair lies below σ2pz and fills first.
- Configuration: σ1s² σ*1s² σ2s² σ*2s² (π2px² = π2py²) σ2pz²
- Bonding electrons Nb = 10, antibonding electrons Na = 4.
- Bond order = (Nb − Na) / 2 = (10 − 4) / 2 = 3.
- Every electron is paired, so N₂ is diamagnetic.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Bond order of N2: quick answers
What is the bond order of N2?
3. Bond order = (Nb − Na) / 2 = (10 − 4) / 2 = 3. Bonding electrons Nb = 10, antibonding electrons Na = 4.
Is N2 paramagnetic or diamagnetic?
Diamagnetic. Every electron is paired, so N₂ is diamagnetic.
What is the molecular orbital configuration of N2?
σ1s² σ*1s² σ2s² σ*2s² (π2px² = π2py²) σ2pz², with 14 electrons in all.