The strongest intermolecular force (IMF) in nitrogen is the London dispersion force.
Nitrogen is a diatomic molecule (N<sub>2</sub>) and is nonpolar due to its symmetrical structure. It experiences only weak London dispersion forces, which arise from temporary fluctuations in electron distribution. These forces are present in all molecules but are particularly significant in nonpolar molecules like nitrogen.
While hydrogen bonding and dipole-dipole interactions are stronger forces, they are not present in nitrogen because it lacks a permanent dipole moment and hydrogen atoms directly bonded to highly electronegative atoms.
The London dispersion forces in nitrogen are relatively weak, which is why it has a low boiling point (-196°C).
