When comparing the energy needed for phase changes, which is true about liquid to gas conversion?

The conversion from liquid to gas, known as vaporization or boiling, indeed requires more energy compared to the phase change from solid to liquid (melting). This is because, during the transition from liquid to gas, the molecules must overcome intermolecular forces that hold them closely together in the liquid state. These forces are relatively strong, and breaking them apart to allow the molecules to escape as gas requires a significant amount of energy, referred to as the heat of vaporization.

In contrast, during the solid to liquid phase change, the energy required to break some of the intermolecular forces is less than what is needed to completely separate molecules in the liquid phase from each other to form gas. Therefore, the liquid to gas phase change demands a higher energy input because it must account for the complete transition to a less ordered, more energetic state.