Final answer:
The arrangement of particles in solids, liquids, and gases varies with solids having tightly packed, orderly arranged particles; liquids having closely packed, disordered particles; and gases having widely separated particles moving independently. These differences are due to the interplay of intermolecular forces and particle energy, and they influence the unique properties of each state, including density, shape, and volume.
Step-by-step explanation:
The Arrangement of Particles in Different States of Matter
The arrangement of particles in solids, liquids, and gases differs due to the varying amount of intermolecular attraction and the energy within the particles. In a solid, particles are tightly packed together, often in a regular, orderly arrangement and vibrate about fixed positions. Liquids have particles that are close together with no regular arrangement, allowing them to move past each other while remaining in contact. In gases, particles have enough energy to overcome intermolecular forces and are separated by large distances, moving about randomly and independently.
The variation in particle arrangement directly impacts the properties of each state of matter. Solids exhibit a definite shape and volume due to their incompressible and densely packed structure. Liquids adapt to the shape of their container but maintain a constant volume, providing them with fluidity. In contrast, gases have neither a definite shape nor volume, expanding to fill their container and becoming far less dense than solids or liquids.
Temperature is a key variable influencing the phase of a substance. When temperature increases, particle energy can overcome the intermolecular attractions, leading to phase changes such as melting, evaporation, or sublimation. In essence, as we progress from solid to liquid to gas, the particles gain energy and freedom, moving from a highly ordered state to a state of complete disorder and movement.