2. Physical Behavior of Matter Phases of Matter

3. 2 Forms of Energy Kinetic Energy Energy of motion Temperature is the measurement of the average K.E. Higher Temp = Higher K.E. Heat is a form of energy Potential Energy Stored Energy

4. Phases of Matter (H 2 O) Solid (0 ‘C) Liquid (50 ‘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) Gas (100 ‘C) Greatest distance Most KE No IMF of attraction present Random motion

5. Phases of Matter (H 2 O) Solid (0 ‘C) Liquid (50 ‘C) Gas (100 ‘C) SolidLiquidGas Definite ShapeYesNo, it takes the shape of the container, not entire No, it takes the shape of the entire container Definite Volume Yes No

6. If you have Gas, that’s a no no !

7. Calibration of a Thermometer 2 Fixed Points Boiling (Condensation) Point 100 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)

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

9. 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

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

11. SGL H f Heat of Fusion Condensation Solidification H V Heat of Vaporization Deposition Sublimation Remember, there is no increase in KE because all energy is being used for the Phase change!

13. Heat Calculations (Q)Q=mc T Q=mH f Q=mH v (Ref Table) Q=mH f Q=mH v

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

15. 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 ‘C1atm 273 ‘K101.3 kpa When Vapor Pressure = atmospheric pressure BOILING OCCURS

17. Weakest IMF Strongest IMF Standard Pressure 101.3 kpa

18. Gases: Ideal vs Real 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. 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. CO 2