What describes the molecular forces in nitrogen gas, N₂?

In nitrogen gas (N₂), the primary interactions are weak intermolecular forces known as van der Waals forces. These forces occur between the molecules due to temporary dipoles that form when the electrons within each nitrogen molecule are unevenly distributed. Nitrogen itself consists of diatomic molecules held together by a strong covalent bond, which is not what is being referred to when discussing the molecular forces in the context of the entirety of the gas.

The reason weak intermolecular forces are the most appropriate description for nitrogen gas is that, in its gaseous state, the molecules are widely separated and move freely. These weak forces are responsible for the low boiling and melting points of nitrogen. Unlike solids or liquids, where stronger attractions or bonds significantly influence structure and properties, the weak intermolecular forces in gases like nitrogen allow for a much less organized arrangement.

In contrast, the other options suggest stronger forms of attraction, such as covalent or ionic bonds, which are more characteristic of the bonds within molecules or between different elements in compound forms rather than in gaseous states. Liquid bonding forces would indicate a state where molecules are close enough that higher energy interactions occur, which again does not apply to nitrogen gas at standard conditions. Thus, weak intermolecular forces aptly describe the