N2 Lewis Structure
The Lewis dot structure of nitrogen gas (N2): a triple bond between the two nitrogen atoms, with one lone pair left on each.
How to draw the Lewis structure of N2
- Count valence electrons: each nitrogen has 5, so the total is 5 + 5 = 10 electrons.
- Connect the two nitrogens with a single bond (2 electrons), then check if both atoms have a full octet — they don't yet (each only has 6 electrons: 2 shared + 4 as lone pairs).
- Turn the single bond into a triple bond by moving 2 lone pairs from each nitrogen into 2 more shared bonding pairs, using 6 electrons total for the bond.
- That leaves 1 lone pair (2 electrons) on each nitrogen, giving both atoms a full octet: 6 bonding electrons + 2 lone pair electrons = 8.
Worked example: counting the octet
Each nitrogen in N≡N has 3 shared bonding pairs (6 electrons, but only counts as 3 towards that atom's own 4 electron pairs since bonding pairs are shared) plus 1 lone pair. Counting all electrons around one nitrogen: 6 from the triple bond + 2 from its own lone pair = 8 electrons, a full octet.
Build N2 and other molecules atom by atom, and watch multiple bonds form in 3D, in the Molecule Builder below.
Frequently asked questions
Why does N2 have a triple bond?
Each nitrogen atom needs 3 more electrons to complete its octet (it has 5 valence electrons). Sharing 3 electron pairs between the two atoms — a triple bond — gives both nitrogens a full octet.
How many lone pairs does N2 have?
Two: one lone pair on each nitrogen atom, left over after the triple bond uses 6 of the 10 total valence electrons.
Is N2 polar or nonpolar?
Nonpolar. Both atoms are nitrogen with identical electronegativity, so there is no difference in electron pull and no dipole.
Why is N2 so unreactive?
Its triple bond is very strong (one of the strongest bonds known), so breaking it apart to react takes a lot of energy — this is why nitrogen gas makes up 78% of the atmosphere without reacting away.
