What is typically true of molecular compounds at low temperatures?

Molecular compounds, which are composed of molecules held together by intermolecular forces, generally exhibit a variety of behaviors when temperatures drop. At low temperatures, if there are sufficient attractive forces between the molecules—such as hydrogen bonds, dipole-dipole interactions, or London dispersion forces—these compounds can condense from a gaseous state to a liquid state and subsequently freeze into a solid. This transition occurs when the temperature decreases enough for the energy of the molecules to be overcome by the attractive forces, leading to a more ordered solid structure.

In contrast, many molecular compounds may remain gaseous at low temperatures if their intermolecular forces are weak, but this does not apply universally. The statement regarding very high melting points is typically more associated with ionic compounds rather than molecular ones, which often have lower melting points due to weaker forces. The idea that molecular compounds do not solidify contradicts the concept that they can form solids when conditions allow for the attractive forces to take effect. Thus, the understanding of the behavior of molecular compounds at low temperatures is encapsulated correctly by the notion that they will condense and freeze if attractive forces exist.