1. States of matter

2. Common states of matter on Earth
Solid
Definite shape and volume
Liquid
Definite volume but not shape
Gas
No definite shape or volume

3. Other states of matter Plasma Bose-Einstein Condensate
exists at extremely high temperatures
Makes up 99% of the matter in the universe, but is nearly nonexistent on Earth
Bose-Einstein Condensate

4. Kinetic Theory
Kinetic Theory: all particles of matter are in constant motion
Kinetic energy: the energy that comes from an object’s motion.
KE = ½ mv2

5. Intermolecular forces
There are attractive forces between all the particles of matter
In gases, particles move so quickly these forces can be ignored
In liquids, the particles have enough kinetic energy to change the shape, but the forces keep a constant volume
In solids, the particles simply vibrate in place, held tight by the forces

6. Phase changes

7. Melting and Freezing Melting is sometimes called fusion
The quantity of heat required to fully melt a certain mass of a substance is called the heat of fusion
The heat of fusion of water is 334 Joules per gram

8. Vaporization Vaporization: either boiling or evaporating
Boiling occurs when vapor pressure equals atmospheric pressure
Vapor pressure: pressure that comes from the gases above the liquid
The quantity of energy required to completely boil a certain mass of liquid is called heat of vaporization
Heat of vaporization of water is 2261 Joules per gram

9. Phase Changes Phase change: reversible, physical change
Temperature does not change during a phase change

10. Heating curve for water

11. Exothermic and endothermic phase changes
Endothermic changes absorb heat
In order for molecules to speed up and break formation, they must grab heat from their surroundings
Exothermic changes release heat
In order for molecules to slow down, they must dump heat into their surroundings

12. Exothermic or Endothermic phase change?
Freezing…………..
Melting…………….
Vaporization………
Condensation…….
Sublimation………
Deposition………..

13. Gas Laws

14. Pressure Pressure is the result of a force distributed over an area
In a gas, pressure comes from collisions between particles and the wall of the container

15. Units of Pressure Newtons per square meter (N/m²)
One N/m² is called a pascal (Pa)
We often use kilopascals (kPa, 1kPa = 1000 Pa)
Standard atmosphere (atm)
1 atm = 101,325 Pa or kPa

16. Factors that affect gas pressure
Number of particles
Increasing the number of particles of gas will increase its pressure if volume and temperature are constant
Temperature
Increasing the temperature of a gas will increase its pressure if the number of particles and volume are constant
Volume
Decreasing the volume of a gas will increase its pressure if the number of particles and temperature are constant

17. Charles’ Law Jacques Charles, 1780
Published by Joseph Louis Gay-Lussac in 1802

18. Charles Law
Note: Temperature must be in kelvin
K = ºC + 273

19. Absolute Zero
William Thomson
“Lord Kelvin”

20. Boyle’s Law
Robert Boyle, 1662

21. Boyle’s Law

22. The Combined Gas Law
Note: Temperature must be in kelvin K = ºC + 273