1. Warm-up: 1. What is an element? 2. What is a compound?

2. 1. Hydrogen 2. Helium 3. Lithium 4. Boron 5. Carbon 6. Nitrogen 7. Oxygen 8.Neon 9. Sodium 10. Aluminum 11. Silicon 12. Sulfur 13. Chlorine 14. Potassium 15. Calcium 16. Titanium 17. Iron 18. Nickel 19. Copper 20. Tin 21. Iodine 22. Tungsten 23. Gold 24. Mercury 25. Lead 26. Radon

3. Notes: Properties of Matter

4. Matter is anything that has mass and takes up space.

5. Elements and Compounds are PURE SUBSTANCES

6. A mixture is when two or more substances are mixed together but not combined chemically

7. A mixture retains properties of all original ingredients.

8. MIXTURE OR PURE SUBSTANCE?

9. NaHCO3 - Sodium Bicarbonate

10. MIXTURE OR PURE SUBSTANCE? Soil

11. MIXTURE OR PURE SUBSTANCE? Milk

12. MIXTURE OR PURE SUBSTANCE? Sugar: C 12 H 22 O 11

13. MIXTURE OR PURE SUBSTANCE? Air

14. MIXTURE OR PURE SUBSTANCE? Oxygen

15. Homogeneous Mixtures are the same throughout.

16. Warm-Up: 1. Is H 2 O a _____________. a. Element b. Compound c. Mixture d. All of the Above 2. Why is tap water considered a mixture?

17. Steel is a homogeneous mixture.

18. Heterogeneous Mixtures are not the same throughout.

19. 4 States of Matter: -Solid -Liquid -Gas -Plasma

20. In a gas, molecules are very far apart

21. In a liquid, molecules are closer together but still move around

22. In a solid, molecules vibrate in place and do not move around

23. Plasmas are gases that are so energized that some of their electrons have been stripped away

24. Gasses and liquids take the shape of their containers, solids do not.

25. Energy must be added to change a solid to a liquid;

26. More energy must be added to change a liquid to a gas

30. Warm-Up: 1. In which state of matter are the molecules moving the fastest? 2. In which state of matter are the molecules not moving around, just vibrating in place? 3. Matter in which two states takes the shape of its container? 4. To make matter change from a solid to a liquid, what must happen to the molecules?

31. WARM-UP: 1. Matter in which two states takes the shape of its container? 2. To make matter change from a solid to a liquid, what must happen to the molecules?

32. WARM-UP: 1. Which state of matter is the most dense? 2. When a substance changes from a solid to a liquid what is this called? 3. When a substance changes from a liquid to a gas what is this called? 4. When a substance changes from a gas to a liquid, what is this called?

33. WARM-UP: 1. What is volume? Give two examples of two things that have different volumes. 2. What makes each element different from one another? 3. What is atomic number?

34. 1. What are the types of pure substances? 2. What are the types of mixtures? 3. What is density? Describe two things that have different densities. 4. What combination of substances retains the properties of its components?

35. 5. Give an example of a homogeneous mixture. 6. Give an example of a heterogeneous mixture. 7. List the phases of matter in ascending order of density. 8. What must be done to change a gas to a liquid?

36. 9. What is the phase change called when a solid changes directly to a gas? 10. Is density a physical or chemical property of matter? 11. Nitrogen boils at -196 o C. Is this a physical or chemical property? 12. List these items in order of ascending density: -a bowling ball –a beach ball – a penny – a hot air balloon in the air

37. Physical Properties of matter describe the matter’s physical characteristics

38. Boiling/Melting Points H 2 O = 100 0 C (212 0 F) CO 2 = -57 0 C (-70 0 F)

39. Density is a physical property

40. Density = Mass Volume Practice: A material has a mass of 100g and a volume of 10 cm 3. Calculate the density.

41. Others include: -Thermal Conductivity

42. -Malleability (ability to be pounded into thin sheets)

43. -Ductility (ability to be drawn into a thin wire)

44. Chemical Properties describe how a substance reacts chemically with another substance

45. In a chemical reaction, you always get a new substance.

46. Law of Conservation of Matter/Mass: Matter can never be created or destroyed

47. Warm-Up: 1. Find the density of an object with a mass of 40g and a volume of 5 cubic cm. 2. Find the mass of a sample of a substance with a density of 5 g/ml and a volume of 2 ml 3. List three physical properties of H 2 O

48. Solutions: S o l u t i o n s - A homogeneous mixture composed of only one phase

49. Solutions: – S o l v e n t - the most abundant substance in a solution. The solvent dissolves the solute. – S o l u t e - the least abundant substance in a solution. The solute dissolves into the solvent. – In a sugar water solution, water is the solvent & sugar is the solute. – In steel (a solution which becomes a solid) iron is the solvent and carbon is the solute – Air is a solution

50. Solutions Homogeneous mixture Homogeneous mixture Mixed molecule by molecule Mixed molecule by molecule Can occur between any state of matter. Can occur between any state of matter. – Solid in liquid- Kool-aid – Liquid in liquid- antifreeze – Gas in gas- air – Solid in solid - brass – Liquid in gas- water vapor

51. Concentration of Solution Shows level of solute in the solvent Can be Expressed in several ways – Relative Concentrations Dilute – small amounts of solute compared to solvent Concentrated – large amounts of solute compared to solvent – Levels of Concentration Unsaturated solution – is able to dissolve more solute Saturated solution – has dissolved the maximum amount of solute Supersaturated solution – has dissolved excess solute (at a higher temperature). Solid crystals generally form when this solution is cooled.

52. Percent Composition (by mass) We can consider percent by mass (or weight percent, as it is sometimes called) in two ways: The parts of solute per 100 parts of solution. The fraction of a solute in a solution multiplied by 100. We need two pieces of information to calculate the percent by mass of a solute in a solution: The mass of the solute in the solution. The mass of the solution. Use the following equation to calculate percent by mass: (Write the equation)

53. Rate of Dissolving

54. Factors Affecting How Fast a Solute Dissolves

55. 1. Temperature If we heat particles they will move faster The solvent will carry the solute particles away faster Hotter = Dissolve Faster

56. 2. Agitating Stirring or shaking a solution moves the solute particles around so that they are closer to the solvent. The solvent particles can then attract them easily and carry them away! Stir or Shake = Dissolve Faster

57. 3. Crushing (More Surface Area) When a solute is broken into small pieces, the individual particles can get closer to solvent particles so they can be easily dissolved So smaller pieces= dissolves faster

58. Dissolving happens on the surface of particles When solute is broken up, there is more surface area where dissolving can occur broken up

59. 4. Pressure Pressure forces solute particles into the spaces between the solvent particles More pressure = Dissolve Faster gas

60. Warm-Up 1.Find the density of a bowling ball with a mass of 6,000 g and a volume of 300 ml. 2. Find the mass of an object with a density of 20 g/ml and a volume of 100 ml.

61. Types of Chemical Reactions Synthesis reactions occur when two elements combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product Basically: A + B  AB Example: 2H 2 + O 2  2H 2 O Example: C + O 2  CO 2

62. Practice Predict the products. Write and balance the following synthesis reaction equations. Sodium metal reacts with chlorine gas Na + Cl 2  Solid Magnesium reacts with fluorine gas Mg + F 2  Aluminum metal reacts with fluorine gas Al + F 2 

63. Decomposition reactions occur when a compound breaks up into the elements or in simpler compounds 1 Reactant  Product + Product In general: AB  A + B Example: 2 H 2 O  2H 2 + O 2 Example: 2 HgO  2Hg + O 2

64. Practice Predict the products. Then, write and balance the following decomposition reaction equations: Solid Lead (IV) oxide decomposes PbO 2(  Aluminum nitride decomposes AlN 

65. Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2 + O 2  BaCO 3  Co + S  NH 3 + H 2 CO 3  NI 3 

66. Single Replacement Reactions occur when one element replaces another in a compound. element + compound  element + compound A + BC  AC + B (if A is a metal) OR A + BC  BA + C (if A is a nonmetal)

67. Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Compound + compound  compound + compound AB + CD  AD + CB

68. Combustion reactions occur when a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the “ fire triangle ” : 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)

69. Combustion Reactions In general: C x H y + O 2  CO 2 + H 2 O Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by-products like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 )

70. Combustion Reactions Edgar Allen Poe’s drooping eyes and mouth are potential signs of CO poisoning.

71. Combustion Example C 5 H 12 + O 2  CO 2 + H 2 O Write the products and balance the following combustion reaction: C 10 H 22 + O 2  5 6 8

72. Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2 + O 2  BaCO 3  Co + S  NH 3 + H 2 CO 3  NI 3 

73. Warm-Up: State the type of reaction and predict the products: 1.BaCl 2 + H 2 SO 4  2.C 6 H 12 + O 2  3.Zn + CuSO 4  4.Cs + Br 2  5.FeCO 3 

74. Warm-Up: In one paragraph, explain why a glass of ice water forms droplets of water on the outside of the glass. Use the following terms: -temperature -molecules -decrease

75. Warm-Up: 1. What does CO 2 (dry ice) do at room temperature? 2. Name a physical property of charcoal. 3. Name a chemical property of charcoal.

76. Warm-Up: 1. What is the change of state called when matter goes from a solid directly to a gas? 2. What are some ways to make a substance dissolve faster? 3. If a solvent cannot dissolve any more of the solute, what is this called?

77. Warm-Up: As you sit by the fireplace, your little brother says “we need to add more wood to the fire because these logs have almost disappeared – the fire has destroyed them.” How would you respond to your brother? Explain.

78. 1. Find the area of a section of carpet that is 10 m wide and 12 m long. 2. Find the area of a roof that is 15 m wide and 20 m long. 3. Find the area of a county that is shaped like a square with boundaries that are 30 km by 30 km.

79. Warm-Up: 1. What is the difference between a physical change and a chemical change? 2. What are some clues that a chemical change/reaction has taken place?

80. Warm-Up: 1. List three physical properties of matter. 2. Describe a chemical change.

81. 2 11 12 14 16 33 34 36 43 44

82. Warm-Up: 1. What is volume? 2. What is density?

83. Warm-Up: 1. What is volume? 2. What is density? 3. What is the difference between a physical change and a chemical change? 4. What are some clues that a chemical change/reaction has taken place?

84. Warm-up Understanding Density In class today, we are going to make a density column. Predict what order these liquids will settle into if they are poured into the same cylinder: Water Alcohol Dawn dish soap Vegetable oil Syrup Milk (whole)

85. SubstanceMass (g)Volume (mL)Density g/mL water alcohol Syrup Vegetable oil Milk (whole) Fill out this chart on page 39 of your notebook. You have 4 minutes.

86. Pure Substances Elements Compounds Homogeneous MATTER Heterogeneous Mixtures Solute Solution SolventExamples:

87. Pure Substances Made of one type of matter Elements Made of one type of atom Compounds Made of 2 or More atoms bonded together Homogeneous Smooth; consistent MATTER Made of Atoms Has Mass & takes up Space Heterogeneous Chunky; inconsistent Mixtures Made of more than one type of matter Solute The stuff that is dissolved In the liquid Ex: Kool-Aid mix Atom + Atom = Element Atom + Atom = Molecule Solution Homogeneous; All one phase Ex: Kool-Aid Solvent The liquid that forms the solution Ex: Water Examples: Trail Mix Salad

88. Characteristics Physical Properties Chemical Properties Changes of State Signs of Change Chemical Reactions Examples States Properties of Matter

89. Characteristics Color Shape Size Texture Mass Volume Density Physical Properties Describe a Substance Changes of State Melting Freezing Boiling Condensation Ionization Relaxation States Solid Liquid Gas Plasma Properties of Matter Chemical Properties Describe how it can form a new substance Signs of Change Odor Change in Temp Change in Color Bubbles form Solids form Chemical Reactions Atoms in two substances combine to form new substances Examples Burning Rusting Rotting Tarnishing Examples 2Na+Cl 2  2NaCl 2H 2 +O 2  2H 2 O

90. Solid _____Energy Atoms ______stuck together Liquid ____________Energy Atoms __________stuck together Gas ______Energy Atoms _____stuck together Plasma ________Energy Atoms ____stuck together _____________ _________ __________ ____________ __________ ____________ _________Point _______Point ______Point _________Point States of Matter Temperature

91. Solid Low Energy Atoms tightly stuck together Liquid Medium Energy Atoms loosely stuck together Gas High Energy Atoms not stuck together Plasma Highest Energy Atoms not stuck together Freezing Melting Relaxation Condensation Ionization Evaporation _Melting Point Boiling Point Dew Point Freezing Point States of Matter Temperature

92. Match the Columns 1.Molecule____ 2.Element ____ 3.Compound ____ 4.Volume ____ 5.Mixture ____ 6.Atom ____ 7.Mass ____ 8.Matter ____ A.Amount of matter in an object B.The smallest building block of matter C.2 or more atoms combined together D.The amount of space an object occupies E.Is made of atoms F.A substance with only 1 type of atom G.A substance with 2 or more atoms bound together H.A combination of different substances which retain their individual properties

93. Match the Columns_Answers 1.Molecule__C__ 2.Element __F__ 3.Compound _G__ 4.Volume _D___ 5.Mixture __H__ 6.Atom __B__ 7.Mass __A__ 8.Matter __E__ A.Amount of matter in an object B.The smallest building block of matter C.2 or more atoms combined together D.The amount of space an object occupies E.Is made of atoms F.A substance with only 1 type of atom G.A substance with 2 or more atoms bound together H.A combination of different substances which retain their individual properties