What characteristic leads nitrogen gas, N₂, to be a gas at room temperature?

Nitrogen gas (N₂) exists as a diatomic molecule, meaning that it consists of two nitrogen atoms bonded together through a strong triple bond. While this strong covalent bond contributes to the stability of the nitrogen molecule, it is the weak intermolecular forces present in gaseous nitrogen that primarily account for its state at room temperature.

In gases, molecules are in constant motion and are relatively far apart, which leads to minimal interaction between them. Nitrogen's weak intermolecular forces, specifically London dispersion forces, result in low attraction between N₂ molecules. This means that even though nitrogen has a strong molecular bond, the forces that act between separate nitrogen molecules are weak, allowing them to move freely and occupy a gaseous state at room temperature.

Other options do not primarily explain nitrogen's gaseous state. Strong covalent bonds actually contribute to the stability of the nitrogen molecule rather than influencing its state as a gas. A high melting point and low molecular weight may be relevant factors, but they do not specifically pinpoint the reason for nitrogen being a gas at room temperature. Therefore, the key characteristic that allows nitrogen to exist as a gas at room temperature is indeed the presence of weak intermolecular forces between its molecules.