Final answer:
In H₂ and N₂, liquid state condensation is primarily driven by weak van der Waals forces, specifically London dispersion forces, as the temperature lowers and kinetic energy decreases, allowing molecules to come closer together.
Step-by-step explanation:
The condensation of ₂ and N₂ into their liquid states from the gaseous state can be explained through intermolecular forces. These are forces that exist between molecules, affecting their physical properties and states of matter. For H₂ and N₂, the intermolecular force responsible for condensation is primarily van der Waals forces, which include London dispersion forces. These forces are weaker than chemical bonds, such as covalent bonds, but become significant at low temperatures when the kinetic energy of the molecules decreases, allowing the attractions to bring molecules closer together to form a liquid.
Van der Waals forces are a form of weak attractions that arise due to temporary fluctuations in electron distribution around atoms or molecules, leading to transient dipoles that attract each other. These forces increase with the size of the molecules and the number of electrons. Since H₂ and N₂ are nonpolar and do not have permanent dipoles, the London dispersion forces are the main intermolecular forces leading to their condensation when cooled sufficiently.