2. Chapter 3

3. 1. SOLIDS Have a definite shape and volume. HLHLeast amount of movement of particles. HPHParticles often arranged in a regular pattern, and tightly packed.

4. 2. LIQUIDS H No definite shape, but do have a definite volume. H A liquid will assume the shape of its container. H Particles are close together but move about freely.

5. 3. GASES HNHNo definite shape nor volume HCHCan fill any container HPHParticles are spread out and move very fast. (1000 mph)

6. PLASMA H Most common phase of matter in the universe. H Not found on earth. H Where can this be found?

7. Kinetic Theory H All particles of matter are in constant motion. Solids, liquids, and gases. H There are also forces of attraction between particles

8. Pressure H A force exerted over a certain area H Measured in newtons/m 2 or pascals (Pa)

9. 3 Factors that affect pressure: 1) Temperature 2) Volume 3) Number of particles

10. Charles’ Law HTHThe volume of a fixed amount of gas varies directly with the temperature in degrees kelvin of a gas. HEHExample: –H–Hot air balloons

11. Boyle’s Law H Named after Irish chemist Robert Boyle. H The volume of a fixed amount of gas varies inversely with the pressure of a gas. H Example: –Balloon in vacuum

12. Combined Gas Law H When you look at the effect of both temperature and pressure on a closed system of gas at the same time. H Formula: P 1 V 1 /T 1 = P 2 V 2 /T 2

13. Phase Changes HAHALL ARE PHYSICAL CHANGES HTHThe six types are: –M–Melting, freezing, vaporization, condensation, sublimation, and deposition

14. What happens to temperature and heat energy during a phase change? H There is always a change in heat energy.  Endothermic = heat energy is absorbed  Exothermic = heat energy is released  Temperature always remains constant.

15. Melting and freezing H Melting H Changing from a solid to a liquid. H The substance absorbs energy H Freezing H Changing from a liquid to a solid. H The substance releases energy

17. vaporization H Change of a substance from a liquid to a gas. H Must absorb energy. H 2 types: 1.Boiling 2.Evaporation

18. EVAPORATION HVHVaporization occurring at the surface of the liquid only.

19. BOILING HVHVaporization throughout the liquid.

20. Can you boil water when it is cold? H Boiling point depends on air pressure. H EARTHMOON

21. Condensation HCHChange of a gas to a liquid. HRHReleases heat energy

22. Sublimation HCHChanging directly to a gas from the solid phase skipping the liquid state. HeHex. –d–dry ice, iodine, ice and snow

23. Deposition H Changing directly from a gas to a solid. H Frost forming on windows from the humidity in the air.

24. ASSIGNMENT H Pages 95-96 –1-10, 17, 18, 21, 24, 27, 28, 29, 31, 32 –Page 97 1-6