1. Physical Behavior of Matter Phases of Matter

2. 2 Forms of Energy Kinetic Energy Potential Energy Energy of motion
Temperature is the measurement of the average K.E.
Higher Temp = Higher K.E.
Heat is a form of energy
Stored Energy

3. Phases of Matter (H2O) Solid (0 ‘C) Liquid (50 ‘C) Gas (100 ‘C)
More distance
More KE
Still an intermolecular
force of attraction b/w
molecules
Hydrogen bonds
Fixed regular geometric
pattern w/ “Vibratory” motion
little distance b/w
molecules
Little KE *** see the temp?
Less Randomness
(Entropy S)
Greatest distance
Most KE
No IMF of
attraction present
Random motion

4. Phases of Matter (H2O) Solid Liquid Gas Solid (0 ‘C) Gas (100 ‘C)
Liquid (50 ‘C)
Solid
Liquid
Gas
Definite Shape
Yes
No, it takes the shape of the container, not entire
No, it takes the shape of the entire container
Definite Volume No

5. If you have Gas, that’s a no no !

6. Calibration of a Thermometer
2 Fixed Points
Boiling (Condensation) Point C and 373 K
(AS MEASURED BY THE WATER / VAPOR EQUILIBRIUM)
Melting (freezing) Point 0 C and 273K
(AS MEASURED BY THE ICE / WATER EQUILIBRIUM)

7. Calibration of a Thermometer
2 Fixed Points
Boiling (Condensation) Point C and 373 K
Melting (freezing) Point 0 C and 273K
Boiling Pt / Condensation Pt
100 C / 373 K
100 ‘ change
Melting Pt / Freezing Pt.
0 C / 273 K
0 ‘K
Absolute Zero
No Particle Motion

8. Two Kinds of Reactions Endothermic Absorb Energy Heat + AB  A +B
Heat is a reactant
Break Bonds
+ H
Exothermic
Release Energy
A + B  AB + Heat
Heat is a product = Stability
Bond formation H

9. Heating Curve D E C B A
A= Heating the Solid KE / 0 PE B = Phase Change 0 KE / PE
C = Heating the Liquid KE/ 0 PE Melting pt. (1st see a liquid) (Hf fusion)
E = Heating the Gas KE / 0 PE
D = Phase Change Freezing (1st see the solid) (Solidification)
Boiling pt (1st see the gas) (Vaporization)
Condensation (1st see the liquid)

10. S L G Hf Heat of Fusion HV Heat of Vaporization Solidification
Condensation
Sublimation
Deposition
Remember, there is no increase in KE because all energy is being
used for the Phase change!

12. Heat Calculations (Q) Q=mc T Q=mHf Q=mHv (Ref Table)

13. C = Specific heat capacity
This is the amount of heat needed to raise the temperature of
1g of water by 1 ‘C

14. Heat Calculations

16. Vapor Pressure
Is the amount of pressure that a vapor
Exerts on the walls of a sealed container.
STP = Standard Temperature Pressure
0 ‘C 1atm
273 ‘K kpa
When Vapor Pressure = atmospheric pressure
BOILING OCCURS

17. Standard
Pressure
101.3 kpa
Weakest IMF
Strongest IMF

18. Gases: Ideal vs Real Real gas All characteristics are the same except
Kinetic Molecular Theory
Gases travel in straight line, random motion
When they collide, transfer energy between particles
Collisions are elastic
Actual Volume of a gas is negligible (small) as compared to the volume they occupy
There is no attraction between gas particles
These describe the characteristics of an IDEAL GAS
Real gas
All characteristics are the same except
No Elastic Collisions
There is a slight IMF of attraction between gas particles

19. So, How can we make: 1. a real gas act like an ideal gas 2
So, How can we make: 1. a real gas act like an ideal gas 2. an ideal gas act like a real gas What conditions of temperature and pressure favor these gases? What is your IDEAL vacation? Watch this!

20. CO2 CO2 CO2 CO2