1. Kinetic Theory of Matter
Chapter 16 Section 1 Part A
Kinetic Theory of Matter

2. Kinetic Theory Explains how particles behave Three basic ideas:
All matter made of small particles
All particles are in constant motion
Particles collide
Collisions transfer energy

3. Kinetic Energy Remember, kinetic energy is the energy of motion
KE = ½ m v2
Since all particles are moving, all particles have kinetic energy
Temperature is the measure of the AVERAGE kinetic energy of particles in matter

4. Potential Energy Particles also have potential energy
Potential energy is stored energy
May be due to gravity, chemical nature

5. Thermal energy Thermal energy is the total energy in matter
Thermal energy is the sum of kinetic and potential energy of the particles
Thermal energy determines the state of matter

6. States of Matter Five recognized states of matter
The state depends on the balance between kinetic and potential energy of the particles
The states:
Solid
Liquid
Gas
Plasma
Bose-Einstein Condensate

7. Solid Particles close together
Usually packed in a particular pattern (crystal)
Particles vibrate in place, do not move apart
As a result:
Definite volume
Definite shape

8. Liquid Particles not as close as solid
Do not have regular pattern
Particles move and slide past each other
As a result:
No definite shape
Definite volume

9. Gas Particles free to move away from each other
Particles constantly collide and bounce away
As a result:
No definite shape
No definite volume

10. Plasma Extremely high energy rips electrons away from atoms
Interaction of ionic particles
Example: any star, lightning

11. Bose-Einstein Condensate
Proposed by Satyendra Nath Bose and Albert Einstein in the 1920s
First created and observed in 1995
First accomplished by Eric Cornell and Carl Wieman in Boulder, Colorado
BEC Homepage
Gaseous superfluid cooled to near absolute zero
All atoms can flow past one another behaving almost like a synchronized wave 

12. Phase Transitions
Changing kinetic energy causes a change in the state of matter
Change from liquid  gas: vaporization
Change from gas  liquid: condensation
Change from liquid  solid: freezing (crystallization)
Change from solid  liquid: melting
Each of these changes requires a specific amount of kinetic energy change

13. Phase Transitions
Change from gas  liquid (or vice versa) requires change in energy
Heat of vaporization: specific amount of energy required to change the particle distance and motion from gas to liquid
Change from solid  liquid (or vice versa) requires change in energy
Heat of fusion: specific amount of energy required to change the particle distance and motion from solid to liquid

15. Phase Transitions Melting point (freezing point): Boiling point:
Temperature at which the substance changes from liquid to solid (or vice versa)
Boiling point:
Temperature at which the substance changes from liquid to gas (or vice versa)

16. Phase Transitions Not all substances change state in an orderly way
Amorphous solids: solids with no orderly particle structure
Liquid crystals: keep orderly particle structure even as a liquid