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
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
Lead
Radon

3. Notes: Properties of Matter

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

5. Matter is divided into TWO main categories for purposes of classification.
All matter is either a PURE SUBSTANCE or a MIXTURE

6. Elements and Compounds are PURE SUBSTANCES

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

8. A mixture retains properties of all original ingredients.

9. MIXTURE OR PURE SUBSTANCE?

10. MIXTURE OR PURE SUBSTANCE?
NaHCO3 - Sodium Bicarbonate

11. MIXTURE OR PURE SUBSTANCE?
Soil

12. MIXTURE OR PURE SUBSTANCE?
Milk

13. MIXTURE OR PURE SUBSTANCE?
Sugar: C12H22O11

14. MIXTURE OR PURE SUBSTANCE?
Air

15. MIXTURE OR PURE SUBSTANCE?
Oxygen

16. Homogeneous Mixtures are the same throughout.

17. Warm-Up: 1. Is H2O a _____________. a. Element b. Compound c. Mixture d. All of the Above 2. Why is tap water considered a mixture?

18. Steel is a homogeneous mixture.

19. Heterogeneous Mixtures are not the same throughout.

20. Targets 9/10/14
Identify the following as pure substances or mixtures.
Oxygen
Milk
Vegetable oil
Coffee
Aluminum
Nitrogen
Water
Carbon dioxide

21. Density is a physical property

22. Density = Mass Volume Practice: A material has a mass of 100g and a volume of 10 cm3. Calculate the density.

23. Warm-Up. Density = Mass. Volume 1
Warm-Up Density = Mass Volume 1. A material has a mass of 500g and a volume of 10 cm3. Calculate the density. 2. A sample of water has a volume of 50mL and a mass of 50g. What is the density? 3. Which type of substance cant be separated into a simpler substance?

24. Matter Density Element Compound Pure substance Mixture Homogeneous
Illustrated Dictionary
On each square, complete the following:
Write the word and provide a paraphrased definition.(left)
Use the word in a complete sentence (left)
Provide an illustration of the word on the right.
Matter
Density
Element
Compound
Pure substance
Mixture
Homogeneous
Heterogeneous

25. 4 States of Matter: -Solid -Liquid -Gas -Plasma

26. In a gas, molecules are very far apart

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

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

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

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

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

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

36. 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?

37. 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?

38. WARM-UP: 1. Which state of matter is the most dense. 2
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?

39. WARM-UP: 1. What is volume
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?

40. 1. What are the types of pure substances. 2
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?

41. 5. Give an example of a homogeneous mixture. 6
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?

42. 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 -196oC. 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

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

44. Boiling/Melting Points
H2O = 1000C (2120F)
CO2 = -570C (-700F)

45. Density is a physical property

46. Density = Mass Volume Practice: A material has a mass of 100g and a volume of 10 cm3. Calculate the density.

47. Others include: -Thermal Conductivity

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

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

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

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

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

53. 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 H2O

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

55. 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

56. Solutions Homogeneous mixture Mixed molecule by molecule
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

57. 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.

58. 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)

59. Rate of Dissolving

60. Factors Affecting How Fast a Solute Dissolves

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

62. 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

63. 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

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

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

66. Warm-Up: 1. What does CO2 (dry ice) do at room temperature. 2
Warm-Up: 1. What does CO2 (dry ice) do at room temperature? 2. Name a physical property of charcoal. 3. Name a chemical property of charcoal.

67. 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?

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