How do physical properties differ among solid, liquid, and gas?

Solid, liquid, and gas differ in terms of shape, volume, compressibility, and particle arrangement and movement.

In a solid, particles are tightly packed in a fixed, regular arrangement. This gives solids a definite shape and volume. They are not easily compressible because there is little free space between particles. The particles vibrate about a fixed position but do not move from place to place.

In contrast, liquids have particles that are close together but can move around each other. This allows liquids to flow and take the shape of their container, although they still maintain a definite volume. Liquids are slightly compressible due to the small amount of free space between particles.

Gases have particles that are far apart and move randomly at high speeds. This gives gases the ability to flow and completely fill their container, taking both the shape and volume of the container. Gases are easily compressible because there is a large amount of free space between particles.

The differences in physical properties among solids, liquids, and gases are due to the differences in their particle arrangement and movement. In solids, the strong intermolecular forces keep the particles close together and restrict their movement. In liquids, the intermolecular forces are weaker, allowing the particles to slide past each other. In gases, the intermolecular forces are very weak or negligible, giving the particles freedom to move independently.

Temperature also plays a role in these differences. As temperature increases, particles gain energy and move more, which can lead to a change in state from solid to liquid (melting), or from liquid to gas (evaporation). Conversely, decreasing temperature can cause a gas to condense into a liquid or a liquid to freeze into a solid. These changes of state demonstrate the dynamic nature of matter and the interplay of energy, particle movement, and intermolecular forces.