Nitrogen is tricky! This simple diatomic molecule introduces students to the concept of triple bonds. This easy to follow drawing shows how this occurs.

1. For diatomic nitrogen, the Lewis-dot structure correctly predicts that there will be a triple bond between nitrogen atoms:
Step 1) The middle (green) pair of electrons pair up to form a pair of electrons. But, neither N atom has an octet.
Step 2) The top (blue) electrons slide down into place to form the left pair of electrons. They are still not happy! (Don’t have an octet).
Step 3) Lastly, the bottom (purple) electrons slide up to form the right pair of electrons. Finally, both N2 atoms an octet.
They each have their own lone pair (two “outside” electrons), and share the middle 6 electrons to form a triple bond. (Memory Aid – 6 electrons = married, strongest bonds.) This
triple bond is very strong. The strength of the triple bond makes the N2 molecule very stable against chemical change, and, in fact, N2 is considered to be a chemically inert gas.