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. What does CO 2 (dry ice) do at room temperature? 2. Name a physical property of charcoal. 3. Name a chemical property of charcoal.

61. 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?

62. 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?

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