1. Matter chapter 3

2. Matter massspace anything that has mass & occupies space –mass: gramskilograms –mass: measured in grams or kilograms volumeliterscm 3 –space/volume: measured in liters or cm 3

3. Phases SOLIDS LIQUIDS GASES

4. solid: solid: definite volume definite shape

5. liquid 0 definite volume indefinite shape takes the shape of container

6. gas indefinite volume indefinite shape takes the shape & volume of container

7. States of Matter 1.How are the particles packed in each phase? 2.How do the particles move in each phase? 3.Why do liquids and gases flow? 4.Why are gases so easy to compress?

8. 4 th phase of matter plasmaplasma exists in stars, lightning bolts e lectrons are stripped from atoms

9. Physical Properties describe appearance & form of matter descriptive words: color, texture, luster, odor solid, liquid, gasmeasurements: a number and a unit

10. Intensive Properties –physical constants –independent –independent of sample size –amount doesn’t matter density, freezing/melting points, and boiling point solubility in water (g/ml)

11. Extensive Properties extensive properties:extensive properties: depend on sample size: amount) mattersquantity (amount) matters mmass & volume

12. Chemical Properties describe how matter: behaves in presence of other matter changes into another kind of matter examples: –flammability –resistance to corrosion –ability to neutralize acids or bases

13. Properties of Copper physical prop: reddish brown shiny malleable ductile good conductor density = 8.92 g/cm 3 mp = 1085  C bp = 2570  C chemical prop: reacts to form green copper carbonate forms deep blue solution when in contact with NH 3 forms new substances with HNO 3

14. Physical Change identityform or appearance of matter may change but identity remains same phase changes dissolving crushing, grinding cutting tearing

15. Dissolving dissolving is physical change: think of putting sugar in water still have sugar – sugar molecules just spread out between water molecules C 6 H 12 O 6 (s)  C 6 H 12 O 6 (aq)

16. Phase Changes phase changes are physical changes no new substance is created (chemical formula stays the same) ex: ice melting: H 2 O(s)  H 2 O(l) water boiling: H 2 O (l)  H 2 O(g)

17. Chemical Change chemical change - identity of matter is changed new substance with own unique properties is formed chemical formula changes

18. Burning oxidation reactioncommon name for oxidation reaction indicates matter reacting with oxygen chemical change: original substance changed into new kind(s) of matter ex: CH 4 (g) + 2O 2 (g)  CO 2 (g) + 2H 2 O(g)

19. Evidence of Chemical Change 1.bubbling [formation of a gas]

20. 2. color change

21. 3. heat absorbed/released

22. 4. light produced

23. 5. formation of a solid 2 liquids mix and solid is formed - this is a precipitate (ppt)

24. What kinds of matter are there?

25. Matter SubstancesMixtures Elements Compounds Heterogeneous Mixtures Homogeneous Mixtures mixtures  separated by physical methods compounds  separated by chemical methods

26. Element substance that: cannot be broken down (decomposed) into simpler substance only 1 kind of atom has definite properties formulas have 1 uppercase letter K Br

27. Element Song

28. Atom smallest particle of element that retains properties of element smallest particles of element that can undergo a chemical reaction represented by SINGLE symbol Cu Co Ag Au

29. Compounds 2 or more DIFFERENT elements chemically combined in a definite ratio homogeneous in composition formulas have 2 or more symbols CO 2 MgO H 2 O

30. Compounds different properties of compound are different from properties of elements formed from ex: sodium chloride (table salt) is created from sodium metal and chlorine gas 2Na(s) + Cl 2 (g)  2NaCl(s)

31. Compounds can be separated into elements by chemical decomposition reaction ex: 2H 2 O(l)  2H 2 (g) + O 2 (g)

32. Mixtures combo of 2 or more pure substances NOTphysically combined NOT chemically combined physically can be separated each substance retains its own identity and properties

33. Mixtures variable composition no unique properties (think of sugar and salt mixed together) may be homogeneous or heterogeneous

34. Types of Mixtures

35. homogeneous: uniform composition throughout single phase –ex: solutions (all 3 phases)

36. heterogeneous: see a boundary or regions that look different ex: ice water, granite, suspensions, colloids

38. Suspensions particles in suspensions are larger than those in solutions components of suspension can be evenly distributed by mechanical means (shaking the contents) but components will settle out

39. Colloids homogeneous combination of molecules mixed through another substance that will not settle out or join with the other substance made up of very small, insoluble particles that remain in suspension in a surrounding solid, liquid, or gas medium of different matter can be solid, liquid, or gas

40. Colloid subtypes

41. Aerosols: solid or liquid particles in gas smoke: solid in a gas fog: liquid in a gas

42. Foams: substance where air or gas bubbles are trapped inside a solid or liquid Styrofoam: air in solid whipped cream: air in liquid

43. Sols: –solid particles in a liquid ex: milk of magnesia (solid MgOH in water)

44. Emulsions: liquid particles in liquid milk: fat in water mayonnaise: oil in water

45. Gels: –liquids in solid ex: jello: protein in water quicksand: sand in water

46. Hints to distinguish homogeneous from heterogeneous mixtures:

47. Homogeneous Mixtures solutions in gas & liquid phases transmit light particles not big enough to scatter light look translucent

48. Heterogeneous Mixtures suspensions look cloudy particles big enough to scatter light settle on standing

49. Separating Mixtures mixtures are PHYSICALLY combined separation based on physical properties

50. Sorting: based on size & appearance of particles

51. Filtration: solid in liquid liquid goes through filter paper but solid stays behind

52. Distillation: liquids mixed together but have with different boiling points

53. crystallization: solubility of solid in liquid

54. Magnets: separate magnetic metals from non-magnetic substances

55. chromatography: variable solubility of mixed liquids (“travel” ability)

56. Conservation of Mass mass begin with = mass end up with # of atoms before = # of atoms after 10 H’s as reactants = 10 H’s as products

57. Particle Diagrams             atoms of a monatomic element (single same atoms) molecules of a diatomic element (double same atoms)

58. Particle Diagrams                    molecules of a triatomic compound mixture: - monatomic element - diatomic element - triatomic compound   