1. Increased Kinetic Energy: The particles in a liquid gain more kinetic energy (energy of motion). This can happen due to an increase in temperature or a decrease in pressure.
2. Overcoming Intermolecular Forces: The particles in a liquid are held together by relatively weak intermolecular forces (like hydrogen bonding, dipole-dipole interactions, and London dispersion forces). As the particles gain more energy, they vibrate faster and move further apart, overcoming these forces.
3. Increased Separation: The particles become more widely spaced. In a liquid, particles are close together and can move around each other. In a gas, the particles are much farther apart and move freely and randomly.
4. Change in Density: The density of the substance dramatically decreases. This is because the particles in a gas are much more spread out than in a liquid.
5. Diffusion: Gas particles move rapidly and randomly in all directions. They collide with each other and with the walls of their container, resulting in the phenomenon of diffusion.
In summary: The transition from liquid to gas involves particles gaining energy, overcoming intermolecular forces, moving farther apart, decreasing in density, and exhibiting rapid, random motion. This is why gases are compressible, occupy the entire volume of their container, and diffuse readily.
