1. Atomic Structure: Chpt. 4 Atom Robert Milliken Democritus J.J Thomson John Dalton James Chadwick Dalton’s Atomic Theory Ernest Rutherford Protons Electron Neutrons Cathode Ray Eugen Goldstein

3. Objectives: 1. I can classify matter into substances and mixtures. 2. I can identify and distinguish between physical and chemical properties. 3. I can identify and distinguish between the two types of forces that affect the nature of molecules. 4. I can understand and distinguish between physical and chemical changes. 5. I can identify techniques used to separate mixtures.

4. Daily Objective I can define matter. I can identify and distinguish between the classes of matter.

5. What is Matter?

6. wallpaperbase.com

7. csc-ut.org

8. What’s The Matter?

9. fccps.org maniacworld.com

10. What is Matter? Students used background knowledge and peers to answer this question.

11. What do all matter have in common? Atoms!

12. What is Matter? One or more atoms that take up space and has mass. Emphasized that all matter’s properties and changes are due to the chemical make-up and interactions on the atomic level.

14. Classes of Matter SubstanceMixture ElementHomogenous Mixture CompoundHeterogenous Mixture

15. Classification of Matter

16. Classifying Matter: Substances vs. Mixtures Substances Definite chemical make-up Elements or compounds Ex. Silicon chip or H 2 O Mixtures Varied chemical make- up 2 or more substances physically combined Homo or Hetero Mixtures Pizza and salt water

17. Classifying Matter: Substances vs. Mixtures Element Pure and simplest substance One type of atom Periodic table Symbol, (He= Helium) Homogenous Mixture 2 or more substances physically combined. Substances are very soluble in one another-mix well – one phase Substances in mix properties are preserved Separated by physical processes. Also called a solution Ex. salt water, kool-aid Compound 2 or more substances chemically combined Definite composition Break-down only thru chemical processes Substances making up cmpd gain new properties. Chemical Formula, H 2 O Ex. iron rust Heterogenous Mixture 2 or more substances physically combined. Substances are not soluble in one another-do not mix well-multiple phases Substances in mixture properties are preserved. Separated by physical processes Ex. Oil and water, pizza, soil

18. Periodic Table

19. Compounds: Compounds = Chemical Combination of elements in fixed amount. Ex. Sodium Chloride (salt) NaCl Sodium (Na) + Chlorine (Cl) = Salt (NaCl)

20. Heterogenous Mixures Observe multiple phases or parts because substances do not mix well.

21. Homogenous Mixtures Substances mix well so observe one phase or part.

22. Homongenous Mixtures Also called solutions. Solutions: -Solute: what is dissolved -Solvent: what dissolves Solubility= the ability of the solute to dissolve in the solvent..

23. Classify each type of Matter Iron Ore, Fe Iron Rust, FeO

24. Bell Ringer: Matter 1.What is matter? 2.What is the difference between: a.substances and mixtures b.compounds and mixtures 3.Classify each of the following examples: a.sugar b.sugar water c.gold ring d.Iron rust (FeO) e.Italian dressing

25. Classifying Matter one kind of atom physical combination of substances multiple phases one phase chemical combination of substances same chemical make-up from sample to sample properties are preserved when substances combine varied chemical make-up from sample to sample properties change when substances combine oxygen (O 2 ) muddy water limestone (CaCO 3 ) tap water

26. Substances Element Compound Substance

27. Mixtures Homogenous MixHeterogenous Mix Mixtures

28. Classifying Matter Lab Students with peers observed various samples of matter and classified them as an element, compound, homo mixture, or hetero mixture.

29. Classifying Matter 1. Classify each as either an element, compound, homo mixture, or hetero mixture a. soil b. orange juice with no pulp c. copper wire d. car gasoline (C 8 H 18 ) 2. What is the difference between a compound and a mixture?

30. Classification of Matter

31. Classifying Matter Lab Students re-assess their classification of matter lab examples.

32. Chemical Changes A chemical process Substance(s) chemical make-up is changed producing new substances. New properties are observed. Ex. Iron Rust (FeO)

33. Intramolecular Forces H 2 O compound Forces within a compound that holds the atoms together. Also called chemical bonds.

34. Types of Chemical Changes Combustion Decaying Digesting Baking Neutralization (acidic and basic chemicals) Growing Spoiled

35. Physical Changes Physical process Substance(s) chemical make-up is preserved so no new substance is produced. Properties are preserved Ex. Making Lemonade

36. Intermolecular Forces Forces between compounds in a sample of matter. (group forces)

37. Types of Physical Changes Phase changes Breaks Dissolves Crushes Cuts Absorbs

38. Physical vs. Chemical Changes Re-assess Chemical and Physical Change Lab Homework: Physical vs. Chemical Change Worksheet

39. What kind of forces are affected ?.

40. Mixture Separation Lab Students work in groups to determine what physical processes they can use to separate out each substance in a given mixture. They will design and carry out their experiment to successfully separate out each substance in the mixture. Reiterate the concept that substances in a mixture maintain their physical properties because their chemical make-up is preserved.

41. Mixture Separation Lab What physical properties did you use to separate the substances in the mixture?

42. Scientific Skills Exam

43. Homongenous Mixtures Also called solutions. Solutions: -Solute: what is dissolved -Solvent: what dissolves.

45. What comes to mind?.

46. Mixture Separation Lab What physical properties did you use to separate the substances in the mixture?

47. Physical Separation of Mixtures: Extraction 1. Extraction- separating substances in a heterogenous mixture from one another based on their unique physical properties.. Physically separate oil from water because they are not soluble in one another. How could we separate iron fillings and sand?

48. Solubility of Mixtures Chemistryland.com Sciencephoto.com Solubility: How well substances physically combine.

49. Solubility of Mixtures Chemistryland.com

50. Physical Separation of Mixtures: Filtration Commonly used to separate a solid from a liquid in a heterogenous mixture due to differences in size or solubility.

51. Physical Separation of Mixtures Distillation Separation of liquids in a mixture by their differences in boiling points. Ex. Ethanol (78 0 C) and Water (100 0 C)

52. Chromotography Separates homogenous mixtures based on solubility. Chromotography has two phases: -Stationary Phase: solid Mobile Phase: liquid or gas Substances in mixture will separate based on their degree of solubility toward the mobile phase.

53. Physical Separation Techniques Separation Technique Heterogenous Mixture Homogenous Mixture What physical properties are used? Filtration Extraction Distillation Chromotography

54. Matter and Energy I can…. Establish a relationship between changes in matter, the forces involved, and the flow of energy.

55. Phases of Matter

56. Phase Change Processes A. Melting B. Freezing C. Evaporation D. Condensation E. Sublimation F. Deposition G. Ionization H. Deionization

57. Phase Changes

58. Particles in Matter The particles that make-up matter are in constant motion. The particles speed of motion depends upon?

59. Heat Energy Heat Energy = Energy that is transferred between matter of different temperatures. (joules/calories) How does heat energy move between objects? Heat Energy Flow: System: matter you are studying/measuring Surrounding : environment around the system Endothermic Process: heat ______by system Exothermic Process: heat ________by system (released or absorbed)

60. Heat Energy Heat energy alters the: -speed of particles -strength of the intermolecular forces Heat Energy

61. Temperature Scales Visionlearning.com Temperature only measures the heat energy that alters the speed of particles.

62. Molecular Kinetic Theory Heat Energy OCOC Establishes a relationship between physical changes, intermolecular forces, and energy flow.

63. Conservation of Matter and Energy Matter: Matter undergoes changes, but the atoms are conserved as a whole or as parts. Energy: Energy is also conserved during changes that matter undergoes. If energy increases for a system, then its surroundings must decrease in energy by the same amount.

64. Pre-AP The following slides pertain only to pre-AP chemistry classes.

65. Heat Capacity Heat Capacity: The amount of heat needed to raise the temperature of a substance 1.0 o C. What does heat capacity depend upon?

66. Specific Heats of Common Substances Substances Specific Heat J/g* 0 C Specific Heat Cal/g* 0 c water4.181.00 Grain alcohol2.40.58 ice2.10.50 steam1.7.40 aluminum0.900.21 silver0.240.057 mercury0.140.033

67. Specific Heat Capacity Specific Heat Capcity: The amount of heat it takes to raise 1g of the substance 1 0 C.

68. Heat Calculation The temperature of a 95.4 g piece of copper increases from 25.0 o C to 48.0 o C when the copper absorbs 849 Joules of heat. What is the specific heat of copper?

69. Heat Calculations How much heat is required to raise the temperature of 250.0g of mercury to 52 o C?

70. Bell Ringer 1.What is the difference between heat energy (q) and specific heat energy (C)? 2.When 150.0 J of energy is absorbed by a 42.1 g sample of silver the temperature increases by 15.0 o C. What is the specific heat of silver? 3. If an 8.8 gram sample of aluminum increases in temperature from 25 o C to 55 o C how much heat was absorbed by the aluminum sample?

71. Specific Heats of Common Substances Substances Specific Heat J/g* 0 C Specific Heat Cal/g* 0 c water4.181.00 Grain alcohol2.40.58 ice2.10.50 steam1.7.40 aluminum0.900.21 iron0.460.11 silver0.240.057 mercury0.140.033