Final answer:
Particle movement and vibration, dictated by kinetic energy and intermolecular forces, are key determinants of a substance's state, whether solid, liquid, or gas. Temperature changes alter the kinetic energy of particles, causing transitions between these states of matter. In gases, these properties are even more sensitive to temperature and pressure variations.
Step-by-step explanation:
Particle vibration and movement are fundamental in determining the state of matter, whether it be solid, liquid, or gas. The kinetic molecular theory (KMT) provides the framework for understanding how the energy of particles impacts their movement and interactions, influencing the state of the matter.
In solids, the particles vibrate in place due to intermolecular forces that are strong enough to keep them in a fixed position. These forces give solids a definite shape and volume. As we increase the temperature, particles gain kinetic energy, and their vibrations become more vigorous, which can lead to melting, turning the solid into a liquid.
Liquids exhibit particles that have enough kinetic energy to partially overcome intermolecular forces. This allows the particles to move freely around each other while maintaining a definite volume, though lacking a fixed shape. Further heating introduces more energy, enabling the particles to completely overcome intermolecular attractions and become a gas.
Gaseous states are characterized by particles with sufficient kinetic energy to move independently and spread out, filling the available space. In this state, the particles are much further apart compared to solids and liquids. Factors like temperature and pressure are sensitive in gasses and can significantly alter the state by modifying kinetic energy and intermolecular interactions.