Matter chapter 3

1. Matterchapter 3

2. Matter Anything that has mass and occupies space • Mass is measured in grams or kilograms • Space or volume is measured in liters or cm3

3. Phases • SOLIDS • LIQUIDS • GASES

4. Solid: • definite volume • definite shape

5. Liquid • definite volume • indefinite shape • takes the shape of container

6. Gas • indefinite volume • indefinite shape • takes the shape and volume of container

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

8. 4th Phase of matter • Plasma • exists in stars • electrons are stripped from atoms

9. Physical Properties • Describe the appearance and form of matter Words: • color, texture, luster, odor, solid, • liquid, gas Measurements: • a number and a unit

10. Intensive properties • Physical Constants • independent of sample size • Density, freezing point, and melting point • Solubility in water (g/ml)

11. Extensive Properties • Mass  volume • depends on amount of matter in sample • Extensive propertiesdepend on quantity of matter

12. Chemical Properties • Describe how matter behaves in presence of other matter • Describe how matter changes intoanother kind of matter • Flammability • Resistance to corrosion • Ability to neutralize acids or bases

13. Chemical Prop. Reacts to form green copper carbonate Forms a deep blue solution when in contact with NH3 Forms new substances with HNO3 Properties of Copper Physical Prop. • Reddish brown • Shiny • Malleable • Ductile • Good Conductor • Density = 8.92 g/cm3 • MP = 1085C • BP = 2570C

14. Physical Change • The form or appearance of sample may change but identityremains same • Cutting, crushing, grinding,tearing • Phase changes • Dissolving

15. Dissolving • Dissolving is physical change • Think of sugar in water • still have sugar – you just spread it out with water molecules in between • C6H12O6(s)  C6H12O6(aq)

17. Phase Changes • Phase changes are physical changes • No new substance is created (chemical formula stays the same) • Ex: • ice melting: H2O(s)  H2O(l) • water boiling: H2O (l)  H2O(g)

18. Chemical Change • chemical change - identity of matter is changed • new substance with unique properties is formed • The chemical formula changes • Ex: 2H2O(l)  2H2(g) + O2(g)

19. Burning • Common name for oxidation reaction • Burning means reacting with oxygen • Burning is chemical change, because original substance is changed into new kinds of matter Ex: CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)

20. What kinds of matter are there?

21. Matter Substances Mixtures Elements Compounds Heterogeneous Mixtures Homogeneous Mixtures Mixtures  Separated by physical methods Compounds  Separated by chemical methods

22. Element • Substance that: • cannot be broken down or decomposed into simpler substance • only 1 kind of atom • has definite properties • Formulas have 1 uppercase letter

23. Element Song

24. Atom • smallest particle of element that retains propertiesofelement • smallest particles of element that can undergo a chemical reaction

25. Compounds • 2 or more elements chemically combined in a definite ratio • Properties are different from those of elements formed from • Homogeneous • Broken into elements by chemical decomposition reaction • Formulas have 2 or more uppercase letters

26. 2Na + Cl2 2NaCl

27. Mixtures • Combo of 2 or more pure substances • Physically combinednotchemically combined • Each substance retains its own identity and properties

28. Mixtures • Variable composition • No unique properties (Think of sugar and salt mixed together) • Separated byphysical methods • May be homogeneous or heterogeneous

29. Types of Mixtures • Heterogeneous: See aboundaryor regions that look different • Ex: Colloids Suspensions ice water granite

30. Colloids • particles larger than size of molecule but smaller than particles seen with naked eye • colloidal dispersion • consists of colloids in a dispersing medium • Ex: whipped cream, mayonnaise, milk, butter, gelatin, jelly, colored glass

31. Aerosols: • solid or liquid particles in gasEx: • Smoke: solid in a gas • Fog: liquid in a gas

32. Sols: • solid particles in a liquidEx: • Milk of Magnesia (solid magnesium hydroxide in water)

33. Emulsions: • liquid particles in liquidEx: • Mayonnaise: oil in water

34. Gels: • liquids in solidEx: • Gelatin: protein in water • Quicksand: sand in water

35. 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

36. Homogeneous: constant composition throughout, single phase • Ex: Solutions (all 3 phases) such as air, windex, kool-aid

37. Hints for Mixtures • Solutions in gas & liquid phases transmit light • particles not big enough to scatter light • look translucent • Suspensions look cloudy • particles big enough to scatter light • settle on standing

39. source source CuSO4(aq)

40.            Particle Diagrams Atoms of a monatomic element   Molecules of a diatomic element   

41.                    Particle Diagrams Molecules of a triatomic compound    Mixture: monatomic element, diatomic element, triatomic compound

42. Separating Mixtures • Physically combined • Separation based on physical properties • Sorting: size & appearance • Filtration: size solid in liquid • Distillation: different bp’s liquids mixed • Crystallization: solubility solid in liquid • Magnet: magnetization • Chromatography: solubility liquids mixed • “Travel” ability

43. source

45. source Distillation

46. source source Paper Chromatograhy

47. Crystallization source

48. Conservation of Mass Mass before = Mass after # of atoms before = # of atoms after