How do particles behave differently in solids, liquids, and gases?

Particles in solids vibrate in fixed positions, in liquids they move freely within a confined space, and in gases they move randomly.

In solids, particles are tightly packed together in a regular pattern and have the least amount of energy compared to particles in liquids and gases. They vibrate around a fixed position but do not have enough energy to move from their positions. This is why solids have a definite shape and volume. The strong forces of attraction between the particles keep them close together and only allow them to vibrate on the spot.

In liquids, particles have more energy than in solids and are able to move more freely. They are still close together but not in a regular pattern. They can slide past each other, which is why liquids can flow and take the shape of their container. However, the forces of attraction between the particles in a liquid are still strong enough to keep the particles close together, which is why liquids have a definite volume but not a definite shape.

In gases, particles have the most energy and are far apart from each other in a random pattern. They move in all directions and at high speeds. This is why gases can flow and completely fill their container. The forces of attraction between gas particles are very weak, or in some cases, non-existent. This is why gases do not have a definite shape or volume. The behaviour of particles in gases can be explained by the kinetic theory of gases, which states that the temperature of a gas is proportional to the average kinetic energy of its particles.

In summary, the behaviour of particles in solids, liquids, and gases is determined by their energy and the forces of attraction between them. The more energy the particles have, the more freely they can move, and the weaker the forces of attraction between them, the further apart they can be.