Each nitrogen molecule is two nitrogen atoms bound together by a very strong triple covalent bond. Its strongly bonded symmetrical structure makes nitrogen very stable and unreactive, requiring a lot of energy to break the bond within the molecule, significantly more than is available at room temperature.
The attractive forces between nitrogen molecules themselves are dispersion forces (or London forces). The kinetic energy of nitrogen molecules at room temperature is sufficient to overcome these weak forces of attraction between molecules, enabling them freely move apart and exist in a gaseous state.
The key distinction is the strong attractive forces between atoms within the molecule and the weak attractive forces between the molecules themselves.