How do the intermolecular forces in nitrogen gas compare to those in metals?

The intermolecular forces in nitrogen gas are characterized as weak due to the nature of the molecules. Nitrogen gas exists as diatomic molecules (N2), which are held together by relatively weak van der Waals (London dispersion) forces. These forces arise from temporary dipoles that occur when electron clouds around the nitrogen molecules fluctuate.

In contrast, metals exhibit strong metallic bonding, where positively charged metal ions are surrounded by a 'sea' of delocalized electrons. This type of bonding results in significant attraction between the positively charged metal ions and the negatively charged electrons, leading to strong intermolecular forces.

Therefore, the weak intermolecular forces in nitrogen gas make it a gas at room temperature, while the strong forces present in metals give them solid, malleable, and conductive properties.