1. States of Matter
Investigate relationships among the pressure, temperature, and volume of gases and liquids.
Distinguish among solids, liquids, gases, and plasmas
Describe and illustrate the physical differences among solids, liquids, and gases in terms of their mass, volume, density, shape, and particle arrangement.

2. States of Matter
Solids Liquids Gases

3. Solids Have definite shape and volume Atoms packed close together
Won’t change if you change the container
Atoms packed close together
Ordered arrangement of atoms
Almost all elements on the table are solids at room temperature

4. Liquids Definite volume but variable shape Atoms not as close together
Takes the shape of its container
Atoms not as close together
More random arrangement of atoms
Only mercury and bromine are liquids at room temperature

5. Gases No definite shape or volume Atoms far apart
Takes the shape and volume of its container
Atoms far apart
Completely random arrangement of atoms
H, He, N, O, F, Ne, Cl, Ar, Kr, Xe, Rn, are gases

6. Plasma 99% of all matter in the universe is in this state
Ions swirling around each other at extremely high temperatures
Found in stars

7. Kinetic Theory Molecules are always moving
Molecules are always running into each other or their containers
As you increase temperature, speed of molecules increases
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8. Kinetic Theory and the States
Gases
Random, constant motion
Motion of one doesn’t affect motion of another, unless they hit
Attraction between atoms can be ignored
Liquids
Slower speed than gases
Motion of one atom affects another
Attraction between atoms cannot be ignored
Solids
Even slower speeds
Atoms just vibrate in place
Can’t move around or switch places

9. Gas Laws

10. Pressure Force distributed over area Larger area, less pressure
SI Unit Pascal (Pa)
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11. Factors That Affect Pressure
Collisions of molecules against a container cause pressure
Temperature
Kinetic Theory
Increase temperature, speed increases
Raising temperature raises pressure
Volume
Lowering volume raises pressure
Number of particles
Adding more molecules raises pressure

12. Charles’s Law As temperature increases, volume increases
Pressure remains constant
Volume is in L
Temperature is in K
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13. V1P1=V2P2 Boyle’s Law As volume decreases, pressure increases
Temperature remains constant
Volume in L
Pressure in Pa
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V1P1=V2P2

14. Combined Gas Law Used when multiple variables change
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15. Types Phase Changes
Phase changes-reversible physical change from one state to another
Melting-solid to liquid
Freezing-liquid to solid
Vaporization-liquid to gas
Condensation-gas to liquid
Sublimation-solid to gas
Deposition-gas to solid

16. Temperature and Phase Change
Temperature does not change during phase change
Only after all material has changed state can temperature increase or decrease

17. Energy and Phase Change
Energy is absorbed or released during phase change
Endothermic
Absorbs energy
Melting
Boiling
Subliming
Exothermic
Releases energy
Freezing
Condensing
Depositing

18. Melting and Freezing Melting Heat of fusion Freezing
Molecules become less ordered
Average kinetic energy increases
Temperature rises
Heat of fusion
Amount of energy needed to melt
Freezing
Molecules become more ordered
Average kinetic energy decreases
Temperature decreases

19. Vaporization and Condensation
Heat of vaporization
Amount of energy needed to boil
Evaporation
Takes place at the surface
Temperatures lower than the boiling point
Boiling
Requires energy
Kinetic energy increases
Condensation
Releases energy
Molecules more ordered

20. Sublimation and Deposition
Requires energy
Molecules become less ordered
Deposition
Releases energy
Molecules become more ordered