Lewis structure of NF₃
26 valence electrons. Three N-F single bonds, with one lone pair on N.
Lewis structure
26 valence electronsFormal charges: none
Why this shape
- N has 5 valence electrons. It uses three in three single bonds to F, so two are left as one lone pair.
- Steric number = three sigma bonds + one lone pair = 4, so N is sp³ hybridised.
- Four electron pairs point to the corners of a tetrahedron (tetrahedral electron geometry). With one lone pair in place of atoms, the atoms make a trigonal pyramidal shape.
- F pulls the bond pairs away from N, so they repel each other less than in NH3 and the angle closes to about 102 degrees.
- It is polar, but much less than NH3: the N-F bond dipoles point away from the lone pair and partly cancel its moment. NCERT compares the two.
How to draw it
- Count the valence electrons: N 5 + 3 × F 7 = 26 valence electrons, 13 pairs.
- Put N in the middle and join it to the three outer atoms with single bonds.
- 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: three N-F single bonds, with one lone pair on N.
- Formal charge = valence electrons − lone pair electrons − number of bonds. Here: none.
Class 11, Chapter 4 Chemical Bonding and Molecular Structure.
Lewis structure of NF3: quick answers
How many valence electrons are in NF3?
N 5 + 3 × F 7 = 26 valence electrons, 13 pairs.
What are the formal charges in the Lewis structure of NF3?
Every atom has a formal charge of zero.
How many lone pairs are in the Lewis structure of NF3?
10 in all, 1 of them on the central N.