Bond order of F₂
Bond order 1, diamagnetic. 18 electrons: Nb = 10, Na = 8.
Molecular orbitals
18 electrons1bond order
diamagnetic
diamagnetic
(Nb − Na) / 2 = (10 − 8) / 2
σ1s² σ*1s² σ2s² σ*2s² σ2pz² (π2px² = π2py²) (π*2px² = π*2py²)
Why this shape
- Each F has 7 valence electrons. It uses one in one single bond to F, so six are left as three lone pairs.
- Steric number = one sigma bond + three lone pairs = 4, so each F is sp³ hybridised.
- Four electron pairs point to the corners of a tetrahedron (tetrahedral 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
14 valence electronsFormal charges: none
Bond order step by step
- F₂ has 18 electrons: 9 from each F.
- 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*2px² = π*2py²)
- Bonding electrons Nb = 10, antibonding electrons Na = 8.
- Bond order = (Nb − Na) / 2 = (10 − 8) / 2 = 1.
- Every electron is paired, so F₂ is diamagnetic.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Bond order of F2: quick answers
What is the bond order of F2?
1. Bond order = (Nb − Na) / 2 = (10 − 8) / 2 = 1. Bonding electrons Nb = 10, antibonding electrons Na = 8.
Is F2 paramagnetic or diamagnetic?
Diamagnetic. Every electron is paired, so F₂ is diamagnetic.
What is the molecular orbital configuration of F2?
σ1s² σ*1s² σ2s² σ*2s² σ2pz² (π2px² = π2py²) (π*2px² = π*2py²), with 18 electrons in all.