A compound consisting of atoms of large atomic mass is more likely to require: less kinetic energy to melt more kinetic energy to freeze a higher temperature to liquefy a lower temperature to liquefy

compound consisting of atoms with large atomic mass is more likely to require a higher temperature to liquefy. This is because compounds with larger atomic masses generally have stronger intermolecular forces, such as van der Waals forces or dipole-dipole interactions, which require more energy (in the form of heat) to overcome in order to transition from a solid to a liquid state. Therefore, they typically have higher melting points and require higher temperatures to liquefy.