1. Indefinite Shape and Volume:
* Gases: Gases have no fixed shape or volume. They take on the shape and volume of their container.
* Liquids: Liquids have a definite volume, but they take the shape of their container up to the volume they occupy.
2. Compressibility:
* Gases: Gases are highly compressible. Their volume can be significantly reduced by applying pressure.
* Liquids: Liquids are relatively incompressible. Their volume changes very little even under high pressure.
3. Diffusion:
* Gases: Gases diffuse very rapidly. Gas molecules move freely and randomly, quickly spreading throughout the container.
* Liquids: Diffusion occurs in liquids, but it is much slower than in gases. Liquid molecules are closer together and have weaker intermolecular forces.
4. Density:
* Gases: Gases have very low densities compared to liquids and solids. This is due to the large spacing between gas molecules.
* Liquids: Liquids have higher densities than gases, but lower densities than solids.
5. Intermolecular Forces:
* Gases: Gas molecules have weak intermolecular forces. This allows them to move freely and independently.
* Liquids: Liquids have stronger intermolecular forces than gases, but weaker than solids. This attraction keeps the molecules closer together but allows them to flow.
6. Thermal Expansion:
* Gases: Gases expand significantly when heated. This is because the increased thermal energy causes the molecules to move faster and spread further apart.
* Liquids: Liquids expand to a lesser extent than gases when heated.
7. Viscosity:
* Gases: Gases have very low viscosity. This means they flow easily with little resistance.
* Liquids: Liquids have higher viscosity than gases. This is due to the stronger intermolecular forces that create more resistance to flow.
In summary, gases are characterized by their lack of fixed shape and volume, high compressibility, rapid diffusion, low density, weak intermolecular forces, large thermal expansion, and low viscosity.
