1. CHAPTER 10
STATES OF MATTER

2. liquid solid gas Kinetic vs. Potential energy
Which state of matter has the greatest KE?

3. KINETIC THEORY
Particles are small hard spheres, with insignificant volume, mostly empty space, no attractive or repulsive forces
Particles in constant and rapid motion (speed in excess of 1700 km/hr at room temp)
All collisions are perfectly elastic

4. GAS PRESSURE
Definition-FORCE exerted by gas molecules PER UNIT SURFACE AREA
VACUUM-no particles, no pressure
ATMOSPHERIC PRESSURE
Decreases as altitude increases
Collisions decrease as pressure decreases

6. MEASURING PRESSURE Barometer is common device used to measure pressure
SI unit of pressure is kPa-KILOPASCAL
Other units equal to kPa
1 atmosphere (atm)
760 mm Hg
30 inches Hg
760 torr
Distinguish between using aneroid vs. mercury barometer.

7. KINETIC ENERGY AND KELVIN TEMPERATURE
TEMPERATURE IS A MEASURE OF THE AVERAGE KINETIC ENERGY
Increase KE, increase temp
Decrease KE, decrease temp
Absolute zero—0 K, or oC

8. Particles must have sufficient KE to overcome the intermolecular forces

9. EVAPORATION
Definition-conversion at the surface of a liquid to a gas or vapor at a temperature below the boiling point
To evaporate molecules must have a certain minimum kinetic energy to overcome attractive forces
Cooling process

10. Liquid Gas At equilibrium rate of evaporation =rate of condensation

11. VAPOR PRESSURE High vapor pressure vs. low vapor pressure
Easily goes up into vapor
Difficult to go up into vapor

12. BOILING POINT
The temperature at which the vapor pressure of the liquid is just equal to the external pressure
Boiling point decreases as pressure decreases

13. SOLIDS
melting
Solid Liquid
freezing

14. IONIC VS. MOLECULAR Which one has a higher melting point? NaCl vs. H2O
801 oC 0 0C
What is the freezing point of water?

15. Buckminsterfullerene
Aka: Buckeyball

16. Phase Diagram of Water

17. The phase diagram for carbon dioxide.
Sublimation: solid to gas