1. Physical Property Describes form or behavior of matter

2. Physical Properties ColorColor LusterLuster MalleabilityMalleability ConductivityConductivity HardnessHardness CleavageCleavage Phase at room temp.Phase at room temp. Vapor pressureVapor pressure Melting point Boiling point Heat of fusion Heat of vaporization Density Specific Heat Physical constants!

3. Chemical Property Describes how matter interacts with other matter: reactivity

4. Chemical Change Identity Change

5. Examples of Chemical Change Synthesis, Decomposition, Single Replacement, Double Replacement, Combustion, Polymerization, Esterification, etc.

6. Monatomic One-atom Molecule

7. 2 or more uppercase letters in formula Compound

8. Physical Change Identity stays the same

9. H 2 O(l)  H 2 O(g) Phase changes are physical changes. Identity stays the same.

10. 2H 2 O(l)  2H 2 + O 2 (g) Identity changes. Chemical change.

11. Diatomic 2-Atom Molecule

12. Gases Take the shape & volume of their container

13. Physical Constant Physical property expressed with a # & unit. Independent of sample size.

14. Liquids Definite volume but no definite shape

15. Solids Definite volume & definite shape

16. Compound 2 or more elements chemically combined

17. Element Cannot be broken down into anything simpler by ordinary chemical or physical methods

18. Mixture Physical combination of 2 or more pure substances.

19. Pure Substances Elements & Compounds

20. Mixtures Heterogeneous or Homogeneous

21. Distillation Physical method of separating mixture of 2 or more liquids based on differences in boiling points.

22. Solution Homogeneous Mixture. Liquid & gas phase solutions transmit light. Look translucent. Do not separate on standing.

23. Suspension Heterogeneous Mixture. Scatter light. Look cloudy. Need to be shaken or stirred. Separate on standing.

24. NaCl(aq) Homogeneous Mixture. NaCl dissolved in water.

25. NaCl(s) Pure substance. NaCl in the solid phase.

26. Variable Composition Mixture

27. NaCl(l) Pure substance. NaCl in the liquid phase.

28. NaCl(g) Pure substance. NaCl in the gas phase.

29. Homogeneous Uniform, constant, the same throughout.

30. Always Homogeneous Pure substance: Element or Compound

31. Filtration Physical separation technique used to separate heterogeneous mixtures. Based on differences in particle size.

32. Sorting Physical separation technique used to separate heterogeneous mixtures. Based on differences in appearance.

33. Definite & Unique Properties Pure substance. Element or Compound.

34. Broken into components by chemical decomposition reaction Compound

35. Definite Composition Pure substance. Element or Compound.

36. Separated by physical technique Mixture

37. Triatomic 3-atom Molecule

38. May be homogeneous or heterogeneous Mixture

39. Density, melting point, boiling point Examples of physical constants

40. Law of conservation of matter Mass Before = Mass After

41. Given: X + 2Y  Q + 3Z Mass Before = Mass After When 44 grams of X react completely with 128 grams of Y, 32 grams of Q are produced. How much Z will be made? The equation is a distractor. 44 + 128 – 32 = grams Z = 140 g.

42. No new properties. Properties are a mix of properties of components. Mixture

43. C 6 H 12 O 6 (s)  C 6 H 12 O 6 (aq) Equation represents dissolving. Dissolving is a physical change.

44. Physical Properties Used to identify substances.

45. Atoms can vibrate back & forth about a fixed position. Solid state

46. Matter Substances ElementsCompounds Mixtures Heterogeneous Mixtures Homogeneous Mixtures Mixtures  Separated by physical methods. Compounds  Separated by chemical methods. Phys. M. Chem. (solutions)(suspensions)

47. Ways to separate heterogeneous mixtures Sorting Filtration Crystallization Evaporation Distillation Chromatography Differences in density Differences in magnetic properties Differences in solubility

48. Change of phase terms Evaporation = Freezing = Melting = Condensation = Boiling = Deposition = Fusion = Vaporization = Sublimation = Liquid to gas Liquid to solid Solid to liquid Gas to liquid Gas to solid Solid to gas

49. Molecules are relatively far apart from each other & can move from place to place. Gas Phase

50. One substance dissolved in another substance Solution

51. Phase at room temperatrue Physical property

52. Molecules are pretty close, but have enough room to slide or tumble past each other. Liquid Phase

53. Chromatography Physical separation technique based on differences in intermolecular forces.

54. Vapor Gas phase of a substance that is usually a liquid at room temperature.

55. Names for some chemical changes Corrosion, Decomposition, Neutralization, Burning, Fermentation

56. # of atoms of each element before = # of atoms of each element after Law of Conservation of Matter

57. Percent Part X 100% Whole

58. 1 upper case letter in formula Element

59. Cutting, Crumpling, Tearing, Pulling into wire, Hammering into sheet Examples of physical changes

60. Phase Changes Physical changes

61. Dissolving Physical Change

62. Evidence of Chemical Change Production of heat & lightProduction of heat & light Formation of a gas (bubbles)Formation of a gas (bubbles) Formation of a precipitateFormation of a precipitate Change in identifying propertiesChange in identifying properties

63. Opposite of dissolving. Solid comes out of solution. Precipitation

64. Particles arranged in a regular geometric pattern. Solid

65. Particle Diagrams                    Pure substance: units the same. molecules of a triatomic compound. Mixture: units differ. monatomic element, diatomic element, triatomic compound.   

66. Mixture Pure Substance