Final answer:
Kinetic Molecular Theory explains the different properties of solids, liquids, and gases by considering the arrangement, motion, and forces between particles. Solids have particles in fixed positions, liquids allow particles to move past each other, and gases have particles that move freely and independently.
Step-by-step explanation:
Kinetic Molecular Theory (KMT) describes the behavior of matter in terms of particles in motion, providing crucial insights into the differences between solids, liquids, and gases. In a solid, particles are tightly packed in a regular pattern, vibrating around fixed positions, and maintaining a definite shape and volume. In a liquid, particles are close but without a regular arrangement, allowing them to move past each other; liquids maintain a definite volume while adapting their shape to their container. In the gaseous state, particles are at large separations in a random arrangement, moving independently at high speeds; gases have neither definite shape nor volume and expand to fill their containers.
These states are influenced by intermolecular forces and thermal energy. In solids, intermolecular forces dominate, restricting movement and maintaining structure. In liquids, though the forces still significantly influence movement, thermal energy allows particles some freedom to move. Gases have particles that are far apart compared to their size where intermolecular forces are negligible, except during collisions. This freedom of movement explains why gases can quickly occupy any available volume.
Matter can transition between these states through physical changes like melting or boiling, which involve changes in energy and intermolecular forces without altering the chemical composition.