# States of Matter

Mind Map by Hiba, updated more than 1 year ago
 Created by Hiba over 6 years ago
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### Description

Cambridge IGCSE Physics (Solids, Liquids and Gases) Mind Map on States of Matter, created by Hiba on 10/04/2013.

## Resource summary

States of Matter
1 Solids
1.1 Definite, rigid shape
1.2 Dense
1.3 Particles closely packed in a regular arrangement
1.3.1 Strong forces between particles
1.4 Vibrate in fixed positions
2 Liquids
2.1 No definite shape
2.1.1 Denser than gases
2.2 Still attraction between particles
2.3 No fixed arrangement
3 Gases
3.1 Particles spread out with large spaces between them
3.1.1 Expand to fill all available space
3.2 Forces holding them together are small
3.2.1 Bump into the walls of the container
3.3 Can be compressed
4 Brownian Motion
4.1 Particles of fluids are continuously bumping into each other and into tiny particles. Sometimes there will be more collisions on one side of the pollen grain than on another, and this will make the pollen grain change its direction or speed of movement.
5 Boyle's Law
5.1 Air is squashy! Wow!
5.2 Robert Bowle noticed that air can be squashed and then springs back to its original volume when you release it.
5.2.1 Pressure is the force acting per unit area. This is measured in N/m2 = one N/m2 is called a Pascal
5.2.1.1 He noticed that when he DOUBLED the pressure, the volume of the gas HALVED
5.2.1.2 Pressure is proportional to 1/v
5.2.1.3 p1V1 = p2V2
5.2.1.4 If you take a fixed mass of gas that has a pressure 1 and a volume 1, and change either the pressure or the volume, the formula applies.
5.2.1.4.1 If the same number of particles are squeezed into a smaller volume, they will hit the container walls more often. More collisions per second means a greater average force on the wall and therefore = a GREATER pressure.
6 Absolute Zero
6.1 He conducted his experiment at a constant temperature because he knew that temperature also had an effect on the pressure.
6.1.1 Pressure of the gas increases as the temperature increases.
6.1.1.1 Absolue zero is approximately -273º C and that's when the pressure of the gas cannot possibly go down further.
6.2 temperature in K = temperature in ºC + 273
6.2.1 Pressure of the gas is proportional to its Kelvin temperature.

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