1. Qualitative Vs. Quantitative Observations

2. Qualitative Vs. Quantitative

3. Physical Property A characteristic of matter that you can observe without changing the identity of the matter. COLOR ODOR DENSITY STATE MELTING POINT VOLUME MASS LENGTH HEIGHT

4. An extensive property of a material depends upon how much matter is being considered. An intensive property of a material does not depend upon how much matter is being considered. mass length volume density temperature color Extensive and Intensive Properties 1.6

5. Solids  Particles packed close together and are fixed in position.  though they may vibrate  Incompressible.  Retain their shape and volume when placed in a new container, don’t “flow”  Low energy 5

6. Crystalline Solids  Particles arranged in an orderly geometric pattern=crystalline solids.  salt  diamonds  sugar 6

7. Amorphous Solids  particles randomly distributed without pattern=amorphous solids.  plastic  glass  Charcoal  Some Metals 7

8. Liquids  Closely packed, some ability to move around.  Also largely incompressible.  take the shape of their container and “flow”; won’t escape or expand to fill the total container.  Medium Energy 8

9. Gases  Constantly movement, bumping into each other and the container.  lots of empty space between the particles.  on average  High Energy 9

10. Gases  Particles can be squeezed closer together; therefore, gases are compressible.  expand to fill and take the shape of their container, and will flow. 10

11. States of Matter

12. What is Plasma?

13. Energy and States of Matter

15. Endothermic and Exothermic Rxns

16. Endo- vs Exothermic

18. Chemical Property A chemical property is a characteristic that becomes evident during a chemical reaction.  It’s any quality that can be established only by changing a substance's chemical identity. Does it combust? Does it react with water? oxygen? Does it tarnish? Does it rust? Does it ferment?

19. Chemical Changes in Matter The rusting of iron is a chemical change. The iron atoms in the nail combine with oxygen atoms from O 2 in the air to make a new substance, rust, with a different composition. 19

20. processes that cause changes in the matter that change its composition rusting processes that release lots of energy burning Common Chemical Changes C 3 H 8 (g) + 5 O 2 (g) → 3 CO 2 (g) + 4 H 2 O(l)

21. Signs of chemical change  Gas forms – bubbles or odor  Precipitate (solid) forms – becomes cloudy or see sediment settle to the bottom  Release/absorption of energy – change in temperature or gives off light  Color change

22. Matter is Conserved… Nothing is lost or gained in a chemical reaction!

23. Physical Changes in Matter The boiling of water is a physical change. The water molecules are separated from each other, but their structure and composition do not change. 23

24. Summary - Physical change  Form of substance changes (size, state of matter) but not the composition  Ex- change in state of matter  Ex- dissolving sugar  Ex- Crushing solid into powder

25. Summary Chemical Change  Identity and composition of substance changes (new product forms)  In a chemical reaction: Reactants  products  Atoms of reactants break apart and rearrange to join with different atoms to make the new product  but all of the atoms originally there are still there at the end

26. Chemical Changes

28.  118 elements have been identified  82 elements occur naturally on Earth  gold, aluminum, lead, oxygen, carbon  36 elements have been created by scientists  technetium, americium, seaborgium 1.4 An element (atom) is a pure substance that cannot be separated into simpler substances by chemical means. Elements

30. Diatomic Elements A pure substance containing two atoms of the same element combined: Seven elements: H, N, O, F, Cl, Br, I Tend to be stable Can be chemically broken apart

31. Diatomic Elements

32. Compounds A pure substance containing two or more different elements: Distinct physical & chemical properties Can be chemically broken down to other substances Unique structure & ratio of elements

34. Mixtures Any combination of two or more different substances: Not considered “pure” Each part retains its distinct physical & chemical properties Can be physically broken down to other substances

35. Homogeneous Mixture A mixture that is the same throughout. Different substances are evenly spread out Similar properties throughout Also referred to as a “solution”

36. Heterogenous Mixture A mixture with areas of different concentrations of each substance. Substances are clumped or layered together Different areas may have different properties

39. Separation Techniques Density: Separation based on different densities. One sinks, one floats Decantation

40. Separation Techniques Distillation: Separation based on different boiling points

41. Separation Techniques Filtration: Separation of solid and liquid (or gas) Not good for dissolved materials

42. Separation Techniques Evaporation: Dry mixture until one substance completely evaporates

43. Separation Techniques Sifting : Separate small and large particles

44. Separation Techniques Magnetism: Separate magnetic and non magnetic materials

45. K = 0 C + 273.15 0 F = x 0 C + 32 9 5 1.7 273 K = 0 0 C 373 K = 100 0 C 32 0 F = 0 0 C 212 0 F = 100 0 C

46. Convert 172.9 0 F to degrees Celsius. 0 F = x 0 C + 32 9 5 0 F – 32 = x 0 C 9 5 x ( 0 F – 32) = 0 C 9 5 0 C = x ( 0 F – 32) 9 5 0 C = x (172.9 – 32) = 78.3 9 5 1.7