Chemistry-Kinetic particle theory

States of matter
1. Matter is a substance that has mass and occupies space.
2. The three states of matter are solid, liquid and gas.
3. Changes in temperature and pressure can change the state of matter.

Kinetic particle theory
1. The kinetic particle theory states that all matter is made up of particles that are in constant, random motion.
2. The differences in the states of matter can be explained in terms of kinetic particle theory.

Properties	Solid	Liquid	Gas
Arrangement of particles	Orderly	Disorderly	Disorderly
Forces between particles	Very strong	strong	Very far apart
Kinetic energy of particles	Very low	Low	high
Particle motion	Vibrate and rotate about a fixed position	Slide over each other	More about at great speeds
Particles	Closely packed	Not really packed	Very far apart

Changes of state and the kinetic particle theory
1. Particles and solids, liquids and gases have different amounts of kinetic energy. Gases have the highest, followed by liquid then solid.
2. Changes of state occur when particles lose or gain energy.

Diffusion
1. Gases with a lower molecular mass diffuse faster than gases with higher molecular mass.
2. Diffusion is the movement of particles from a region of a higher concentration to a region of lower concentration until they are equal on both sides.
3. The relative rates of diffusion: liquid --> slow diffusion, gases --> fast diffusion

Factors affecting diffusion
1. The greater the difference of concentration between the two region, the greater the rate of diffusion.
2. The greater the resistance to diffusion, the lower the rate of diffusion. Resistance refers to anything that affects the rate of diffusion.
3. Temperature increases the rate of molecular movement, increasing the rate of diffusion.
4. Pressure increases the speed of molecules, increasing the rate of diffusion.

Kinetic particle theory
Shows how the particles interact with one another, there are a few assumptions.
1. Molecules are point masses. (no volume)
2. Gas molecules exert no forces on each other unless they collide.
3. Collision of molecules with each other on the walls of the container do not decrease the energy of the system.
4. The molecules of gas are in constant and random motion.
5. The temperature of a gas depends on its average kinetic energy, the energy of an ideal gas is entirely kinetic.