1. States of Matter

2. 3 States of Matter Solids  _____________________________________ Liquids  ______________________________________ Gases  ______________________________________ Most Dense Least Dense

3. The 4 th State of Matter What happens if you raise the temperature to super- high levels…between 1000°C and 1,000,000,000°C?PLASMA!!   A plasma is an ionized gas.   A plasma is a very good conductor of electricity and is affected by magnetic fields.   Plasma, like gases have an indefinite shape and an indefinite volume.

4. Nature of Gases Minimal attractive forces between particles Particles have lots of energy and move freely Kinetic Molecular Theory: = a model or theory used to describe the behavior of gases 1.) The particles in a gas are considered to be _________________________ __________________________________________________________ 2.) The motion of the particles in a gas is ____________________________ __________________________________________________________ 3.) All collisions between particles in a gas are perfectly elastic  _________________________________________________________ _________________________________________________________

5. Gas Pressure Gas pressure = _______________________________________ _______________________________________ **atmospheric pressure = ______________________ _______________________________ _______________________________  measured with a barometer  Units: kilopascal (kPa) mmHg atm torr 1 atm = 101.3 kPa = 760 mmHg = 760 torr

6. Nature of Liquids Particles are free to flow from one locations to another BUT... The particles are attracted to each other via intermolecular forces.

7. Nature of Solids Particles are orderly and packed tightly together. Particles vibrate in fixed positions only Most solid substances are crystalline.  _______________________________________________________

8. Phase Changes Liquid Gas Solid

9. Temperature Temperature = a measure of the average _________________ of particles = _____________________ **At a given temperature, the particles of all substances, regardless of physical state, have the same average kinetic energy.** Kelvin Scale =_______________________________________________  boiling point of water = ____ K  freezing pt of water = ____ K  absolute zero = ____ K Reference Tables: - Table A (STP) - Table T (degrees Celcius to Kelvin

10. Phase Changes: Heating Curve ***A substance will change phase from solid to liquid to gas when heat energy is added.**

11. Phase Changes: Cooling Curve ***A substance will change phase from gas to liquid to solid when heat energy is lost.**

12. Heating/Cooling Curve Combined

13. Vaporization Vaporization = ___________________________________________  Evaporation : __________________________________________ : __________________________________________ __________________________________________ : ___________________________________________

14.   Vapor Pressure = _____________________________________________ **(Remember: gas particles collide with the walls of the sealed container)** In a system at constant vapor pressure, a dynamic equilibrium exists between the vapor and the liquid. The system is in equilibrium because the rate of evaporation of liquid equals the rate of condensation of vapor.

15.   Vapor Pressure & Temperature: How will temperature affect vapor pressure?______________________________________________ Why? _______________________________________________ **The higher the vapor pressure of a substance, the more volatile it is.  volatility = ______________________________

16.   Boiling Point = ______________________________________________________________ ______________________________________________________________ ______________________________________________________________ **Normal boiling point = boiling point of a substance at the standard pressure of 101.3 kPa

17. Two factors affect the boiling point of a substance: 1.) Pressure  ________________________________________________________ **Why does it take longer to cook food in water at high altitudes?** 2.) Intermolecular forces  _________________________________________________________

18. Reference Tables: Table H