1. Ch. 1 - Matter I. States of Matter  Kinetic Energy  States of Matter

2. A. Kinetic Energy  Particles of matter are always in motion.  The kinetic energy (speed) of these particles increases as temperature increases.

3. B. Four States of Matter  Solids  very low KE - particles vibrate but can’t move around  fixed shape  fixed volume

4. B. Four States of Matter  Liquids  low KE - particles can move around but are still close together  Take the shape of the container  fixed volume

5. B. Four States of Matter  Gases  high KE - particles can separate and move throughout container  variable shape  variable volume

6. B. Four States of Matter  Plasma  very high KE - particles collide with enough energy to break into charged particles (+/-)  gas-like, variable shape & volume  stars

7. Ch. 1 - Matter II. Matter Flowchart  Pure Substances  Mixtures

8. A. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions

9. A. Matter Flowchart  Examples:  graphite  pepper  sugar (sucrose)  paint  soda element hetero. mixture compound hetero. mixture solution

10. B. Pure Substances  Element  composed of identical atoms  EX: copper wire, aluminum foil

11. B. Pure Substances  Compound  composed of 2 or more elements in a fixed ratio  properties differ from those of individual elements  EX: table salt (NaCl)

12. C. Mixtures  Combination of 2 or more pure substances. HeterogeneousHomogeneous

13. C. Mixtures  Solution  homogeneous  very small particles  particles don’t settle  EX: rubbing alcohol

14. C. Mixtures  Colloid  heterogeneous  medium-sized particles  particles don’t settle  EX: milk

15. C. Mixtures  Suspension  heterogeneous  large particles  particles settle  EX:fresh-squeezed lemonade

16. C. Mixtures  Examples:  mayonnaise  muddy water  fog  saltwater  Italian salad dressing colloid suspension colloid solution suspension

17. Ch. 1 - Matter III. Properties & Changes in Matter  Extensive vs. Intensive  Physical vs. Chemical

18. A. Extensive vs. Intensive  Extensive Property  depends on the amount of matter present  Intensive Property  depends on the identity of substance, not the amount

19. A. Extensive vs. Intensive  Examples:  boiling point  volume  mass  density  conductivity intensive extensive intensive

20. B. Physical vs. Chemical  Physical Property  can be observed without changing the identity of the substance  Chemical Property  describes the ability of a substance to undergo changes in identity

21. B. Physical vs. Chemical  Examples:  melting point  flammable  density  magnetic  tarnishes in air physical chemical physical chemical

22. B. Physical vs. Chemical  Physical Change  changes the form of a substance without changing its identity  properties remain the same  Chemical Change  changes the identity of a substance  products have different properties

23. B. Physical vs. Chemical  Signs of a Chemical Change  change in color or odor  formation of a gas  formation of a precipitate (solid)  change in light or heat

24. B. Physical vs. Chemical  Examples:  rusting iron  dissolving in water  burning a log  melting ice  grinding spices chemical physical chemical physical