Final answer:
As temperature increases due to added thermal energy, the motion of particles within a substance becomes more vigorous, resulting in a disordered arrangement and increased entropy. The rise in kinetic energy leads to higher temperatures and potential phase changes, and this process is a reflection of the kinetic-molecular theory.
Step-by-step explanation:
As the temperature of a substance increases, there is a corresponding increase in the thermal energy of its particles, which is manifested through their motion. For solids, particles experience more extensive vibrations, whereas, in liquids and gases, particles undergo more rapid translations (movement from one place to another). A direct result of this increased particle motion is a broader distribution of kinetic energy among the atoms or molecules, leading to an increase in entropy - a measure of disorder or randomness in a system. Hence, as thermal energy and temperature rise, particles move more vigorously, and their arrangement becomes more disordered.
When viewed macroscopically, the addition of heat to a substance increases its temperature, signifying that the particles are vibrating quickly and have a higher average kinetic energy. When enough energy is supplied, the substance may undergo a phase change, such as melting or vaporizing, representing a substantial and discontinuous increase in entropy as the particles arrange themselves even more freely.