1. Matter and Change Ms. Miller 8 th SSI

2. A) Classification of Matter Review of prior knowledge: Talk with your shoulder partner, how is matter classified?

3. Some Criteria for the Classification of Matter Properties State (solid, liquid, gas) Composition

4. Properties Intensive -DOES NOT depend on amount of matter. Extensive -DOES depend on amount of matter present.

5. Intensive and Extensive Properties Sulfur

6. Properties Physical: observed without without changing the composition of the substance. Chemical: the ability of a substance to undergo a specific chemical change

7. Examples of Physical Properties Color, odor, hardness, density, melting point, boiling point, state, solubility.

8. SubstanceStateColor Melting Point (C°) Boiling Point (C°) Density (g/cm 3 ) OxygenO2O2 GasColorless-218-1830.0014 MercuryHgLiquidSilvery- white -3935713.5 BromineBr 2 LiquidRed-brown-7593.12 WaterH2OH2OLiquidColorless01001.00 Sodium Chloride NaClSolidWhite80114132.17 Example: Physical Properties

9. States of Matter Solid fixed shape and volume, incompressible Liquid fixed volume, takes the shape of its container Gas takes the volume and shape of its container

11. Solid Liquid Gas http://www.chem.purdue.edu/gchelp/atoms/states.html

12. Bromine Gas (Vapor) Liquid

13. Change of Phase Meltingsolid  liquid Condensationgas  liquid Freezingliquid  solid Evaporationliquid  gas Sublimationsolid  gas Boiling: Evaporation occurring beneath the liquid’s surface.

14. Is changing phase a physical or chemical change? Review of prior knowledge: Talk with your shoulder partner and be prepared to share out

15. Classification of Matter (by composition)

16. (Pure) Substance Matter that has a uniform and definite composition. Elements Compounds

17. Mixture: a physical blend of two or more substances that are not chemically combined. Homogeneous Heterogeneous

18. Mixtures Homogeneous Heterogeneous

19. Homogeneous mixture (solution) Uniform composition throughout. One phase.

20. Copper II Sulfate and its solution in water.

21. Example: Stainless Steel A homogeneous mixture of: -Iron (Fe) -Chromium (Cr) -Nickel (Ni)

22. Example: Gaseous Mixture Elements argon and nitrogen and a compound (water vapor).

23. Heterogeneous Mixtures Non-uniform composition throughout the mixture Two or more phases. Example: Oil and vinegar

24. Note: Mixtures can be physically separated. Mixtures exhibit physical properties similar to the components of the mixture.

25. Separation Methods Use differences in the physical properties of the components of the mixture.

26. Example: Separate iron filings from sulfur using a magnet.

27. Filtration: separates a solid from a liquid in a heterogeneous mixture

28. Distillation: - separate dissolved solids from a liquid -uses boiling and condensation.

29. Distillation of Crude Oil (Refining) Crude Oil is a mixture of Hydrocarbons

30. Distillation of Crude Oil

31. c) Elements and Compounds

32. Elements The simplest substances. Can not be separated into simpler substances. Building blocks of all matter. More than 100 known elements. Represented by chemical symbols.

33. Chemical Symbols of Elements System started by Jons Berzelius (Sweden, 1779-1848) One or two first letters of name of the element. Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

34. Examples: Americium, Am Einsteinium, Es Bromine, Br Helium, He Lead(Plumbum), Pb Niobium, Nb Iron (Ferrum), Fe Mendelevium, Md

35. Compound A substance that contains two or more elements chemically combined. Compounds have different properties from the individual substances. (Ex: H 2 O)

36. Example: H 2 O

37. Substance or mixture? If composition is fixed and may not change  substance

39. d) Chemical Properties and Chemical Changes

40. H 2 O composition is fixed- compound Gaseous PhaseLiquid Phase

41. Chemical Properties The ability of a substance to transform into a new substance (to undergo a chemical change). Example: Magnesium reacts with oxygen to form magnesium oxide.

42. Magnesium Mg

43. Burning of Magnesium 2Mg+ O 2  2MgO

44. Physical Changes Physical change: a change in the physical properties of a substance. Composition does not change. May be reversible or irreversible. Examples: Reversible: Irreversible:

45. Chemical Change A change that produces matter with a different composition than the original matter. Atoms rearrange themselves into new combinations.

46. Burning of Methane CH 4 +2O 2  CO 2 + 2H 2 O

48. Recognizing a Chemical Change energy exchange production of a gas color change formation of a precipitate

49. Formation of a Precipitate Cu(OH) 2 Precipitate

50. The Law of Conservation of Mass (Antoine Lavoisier) In any chemical or physical change, mass is neither created or destroyed Mass is CONSTANT