Lewis structure of F₂
14 valence electrons. One F-F single bond, with three lone pairs on F.
Lewis structure
14 valence electronsFormal charges: none
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.
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)
How to draw it
- Count the valence electrons: 2 × F 7 = 14 valence electrons, 7 pairs.
- Join the atoms with single bonds: the F atoms to each other and the H atoms around them.
- Give each outer atom lone pairs until it has an octet (H needs only two electrons), then put any electrons left over on the central atom.
- Result: one F-F single bond, with three lone pairs on F.
- Formal charge = valence electrons − lone pair electrons − number of bonds. Here: none.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Lewis structure of F2: quick answers
How many valence electrons are in F2?
2 × F 7 = 14 valence electrons, 7 pairs.
What are the formal charges in the Lewis structure of F2?
Every atom has a formal charge of zero.
How many lone pairs are in the Lewis structure of F2?
6 in all, 3 of them on the central F.