Final answer:
In solids, particles vibrate in place due to strong intermolecular forces. In liquids, particles have more energy, partially overcoming these forces to move past each other. In gases, particles have sufficient energy to move freely and independently.
Step-by-step explanation:
Particles in solids, liquids, and gases exhibit distinct behaviors due to differences in energy and intermolecular forces. In a solid, particles are tightly packed in a regular pattern, vibrating around fixed positions without moving relative to each other. This is because the intermolecular attractions in solids are quite strong. As the solid is heated and particles gain energy, they vibrate more vigorously and may transition into a liquid state.
In a liquid, particles have enough energy to partially overcome intermolecular attractions, allowing them to move past each other while staying in contact, resulting in a definitive volume but no fixed shape. Liquids can flow since their particles can slide over one another.
When it comes to gases, particles have sufficient energy to completely overcome intermolecular forces, and they move about randomly in space. Gas particles are far apart and move independently of each other, except when they collide. Gases have neither a definite shape nor a definite volume and will expand to fill any container.
The state of matter is largely dependent on temperature, as it determines the energy of the particles. Higher temperatures typically mean more energy for the particles, leading to weaker intermolecular forces and the possibility of a state change from solid to liquid or from liquid to gas.