1. How are elements, compounds, and mixtures related?
Objective: Describe the difference between pure substances (elements and compounds) and mixtures

2. What is Matter?
Matter is anything that has mass and takes up space (volume) There are different types of Matter: Pure Substances (elements and compounds) and Mixtures The composition (structure) of a substance determines its Matter type.

3. Characteristics of Pure Substances
What does this mean?
Fixed composition
Distinct properties
Cannot be separated into simpler substances by physical methods
Can only be changed in identity and properties by chemical methods
Properties do not vary one sample to another sample

4. Types of Pure Substances:
Elements And Compounds

5. Sample of the Element Lead Sample of the Element Chlorine
Elements
Made up of one type of atom
Cannot be broken down by physical and chemical methods
Examples: Oxygen, Nitrogen, Carbon
Sample of the Element Lead
Sample of the Element Chlorine

6. Compounds
Form when two or more different elements join (bond) together chemically
Composition is identical in each sample
Can be separated only by chemical methods
Properties of a compound are totally different than the properties of the elements that form them
Examples: Water, Carbon dioxide, Sugar
Animated images and notes from

7. Compounds

8. Elements and Compounds Study Jams Video

9. Mixtures Form when elements and/or compounds are combined physically
Composition varies from sample to sample
Can be separated by physical methods
Examples of Mixtures: Tea, Perfume, Air, Salad, Beach sand, oil and vinegar salad dressing, etc.

10. Mixture of Different Elements Mixture of Different Compounds
Mixtures
Mixture of Different Elements
Mixture of Different Compounds

11. Match the Picture to the Description
Compound of 2 Elements
Mixture of Molecules
Element Molecule
Compound of 3 Elements
Element/ Atoms
Mixture of Atoms

12. Summarizing: C. A. B. D. Mixture Compound
The diagram below shows how two elements can be mixed together…Which is a Compound? A Mixture? A. B. C. D.
Compound
Mixture

13. Mixtures are often referred to as homogeneous or heterogeneous.

14. Mixtures Homogeneous mixtures (Solutions) have a uniform distribution.
For example: Tea, Perfume, Air

15. Mixtures Heterogeneous mixtures do not have a uniform distribution.
Parts are often visible
For example: Salad, Beach Sand, Oil and Vinegar dressing

16. Mixtures Study Jams Video

17. Determine if the box
Contains element only,
Compound, or mixture.

18. DO NOW What are the two types of mixtures?
Homogeneous and heterogeneous
Give example of each.

19. Heterogeneous Mixture: unevenly blended Chicken soup- has chunks
Yogurt with fruit- has chunks
Bowl of cereal
Homogeneous Mixture: evenly blended
Salt and pepper shaken together
Sugar in Kool-Aid ©
per8

20. Heterogeneous or Homogeneous mixture:
This is a mixture of sand and water:
This is a mixture of salt and water:

21. Mixtures Combinations of substances that
can be separated by physical means.
Just about everything that you can think of is probably a mixture.
Even the purest of materials still contain other compounds as impurities
Evenly Blended
HOMOgeneous
SOLUTIONS are homogeneous mixtures.
HETEROgeneous
UnEvenly Blended

23. Solution A homogeneous mixture. One substance is dissolved in another.
Salt in salt water
Iced Tea mix in water
Blue in the toilet bowl
Food coloring in water
Air !
Metal Alloys (Brass, Bronze, Steel)
Watered down vinegar
Soda !

24. Air is a solution of many different gases.
Oxygen
Hydrogen
Nitrogen
Carbon Dioxide

25. TYPES OF SOLUTIONS
1. Gas – Example: air is a solution of different gasses.
2. Solid in a Liquid – Example: Salt water which is in the liquid state.
3. Gas in a liquid – Example: Carbonated beverage.
4. Solid – brass and bronze

26. Making a Solution How many parts are there to a solution?
Two! The liquid and the material you are adding. Ex: water and iced tea
What do you do to make a solution?
Add the solid material to the liquid and stir.

27. Water is an excellent solvent.
Solute vs Solvent
Solvent: The dissolver. The liquid that dissolves other substances.
Solute: The substance being dissolved.
Water is an excellent solvent.

28. Using Nail Polish Remover
Solvent =
Nail Polish Remover
Solute =
Nail Polish

29. How much will dissolve?
The concentration of a solution tells you how much solute is present compared to the amount of solvent.
Which is more concentrated?
100 mg sugar in 1000 ml of water
500 mg sugar in 1000 ml of water

30. Solubility The ability of a given solute to dissolve in a solvent.
The resulting solution is called a saturated solution

31. Degree of saturation Unsaturated Solution
Less than the maximum amount of solute for that temperature is dissolved in the solvent.
No solid remains in flask.
IPC-Solutions-Borders

32. Degree of saturation Saturated solution
Solvent holds as much solute as is possible at that temperature.
Undissolved solid remains in flask.
IPC-Solutions-Borders

33. Precipitate
The leftover solute that cannot be dissolved and falls to the bottom of the container is called the precipitate.

34. Saturated Solution
IPC-Solutions-Borders

35. Do now:
What are the three ways to make a solution
more soluble?

36. Factors That Affect Solubility
What can be done to make the sugar dissolve faster?
1. Increase Temperature
Hotter = Faster
Stirring
Increase Surface Area
More surface area = Faster

37. Surface Area
Which will dissolve faster? A B

38. precipitate

39. Graphing Solubility: Temp vs grams solute in 100 grams H2O
Generally, the solubility of solid solutes in liquid solvents increases with increasing temperature.
IPC-Solutions-Borders
Chemistry-Borders

40. Affect of temperature on solubility of gases
The opposite is true of gases. Higher temperature drives gases out of solution.
Carbonated soft drinks are more “bubbly” if stored in the refrigerator.
Warm lakes have less O2 dissolved in them than cool lakes.
IPC-Solutions-Borders

41. Separating Mixtures Each part of a mixture retains its properties
and therefore can be separated.

42. Separating Mixtures ...how could you separate this mixture?
Mixing sulphur and iron...
...how could you separate this mixture?

43. Separating Mixtures

44. How can you separate the pulp from the Oj?
Filtration: Separating a solid from a liquid

45. Can you separate salt water?
Evaporation!
Water
Evaporating dish
Mixture (salt and water)
Salt
Bunsen burner

46. Separating Mixtures: Distillation
What is happening here?
Water Vapour
Mixture (salt and water)
Bunsen burner
Water

47. Filtration, Evaporation and Distillation
of-materials/2295.html

48. Separation of a Mixture Activity

49. Original Mixture Mixture The Mass of the Mixture is the Difference

50. Extraction
Mass

51. Filtration
Mass

52. Evaporation
Mass
The Mass of the Salt is the Difference

53. Mass of the Mixture Before
% Error
(Mass of the Mixture After Separation – Mass of the Mixture Before Separation) x 100
Mass of the Mixture Before
= %
( ) g x 100
( ) g

54. Analysis/Conclusion In addition to our usual conclusion… Include:
Description of the techniques used.
Physical properties we utilized.
Why was there a difference before and after separation? …