2. Aim: How do Physical and Chemical Changes differ? Do Now: writing activity HW: handout

3. DO NOW: Writing Activity The students will describe the three states of matter and include the following : At least one example of each state A description of each state

4. MATTER Matter is everywhere. Matter is anything that takes up space and has mass. Matter is constantly experiencing both chemical and physical changes.

5. Physical Change occur when matter changes its property but NOT its chemical nature. changes could include a change in: texture, shape, size, color, odor, volume, mass, weight, and density.

6. Physical Change

7. Chemical Change are changes matter undergoes when it becomes new or different matter. To identify a chemical change look for signs such as color change, bubbling and fizzing, light production, smoke, and presence of heat.

8. Chemical Change A chemical change occurs when fireworks are used. Fireworks are made of metals such as magnesium and copper. These change chemically as they light up the sky.

9. Is it a chemical or physical change? Sugar dissolving in tea Chemical Change Physical Change

10. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

11. Correct!

12. Is it a chemical or physical change? Logs burning Chemical Change Physical Change

13. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

14. Correct!

15. Is it a chemical or physical change? Breaking water up by separating it into hydrogen and oxygen Chemical Change Physical Change

16. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

17. Correct!

18. Is it a chemical or physical change? Cutting paper Chemical Change Physical Change

19. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

20. Correct!

21. Is it a chemical or physical change? Crushing an aspirin Chemical Change Physical Change

22. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

23. Correct!

24. Is it a chemical or physical change? Metal rusting Chemical Change Physical Change

25. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

26. Correct!

27. Is it a chemical or physical change? Lighter fluid burining Chemical Change Physical Change

28. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

29. Correct!

30. Is it a chemical or physical change? An egg rotting Chemical Change Physical Change

31. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

32. Correct!

33. Is it a chemical or physical change? An egg breaking Chemical Change Physical Change

34. OOPS! Did it change size, color, shape (Physical Change)? or Did it become different matter (Chemical Change)?

35. Correct!

36. Writing Activity Write a paragraph about the difference between a chemical and physical change. Give examples of each.

37. Aim: How do we read a solubility curve? HW: HANDOUT

39. A solution is actually a type of mixture. Think of the example of sand in water. This is also called a "heterogeneous mixture." Think of the example of salt water. This is also called a "homogenous mixture."

40. Definitions A solution is a homogeneous mixture of 2 or more substances that are uniform throughout. One constituent is usually regarded as the SOLVENT and the others as SOLUTES.

41. Parts of a Solution SOLUTE – the part of a solution that is being dissolved (usually the lesser amount) SOLVENT – the part of a solution that dissolves the solute (usually the greater amount) SoluteSolventExample solid Metal alloys solidliquidSalt water gassolidMoth balls liquid Alcohol in water gasliquidsoda gas air Solute + Solvent = Solution

42. Definitions Solutions can be classified as saturated or unsaturated and super saturated A saturated solution contains the maximum quantity of solute that dissolves at that temperature. An unsaturated solution contains less than the maximum amount of solute that can dissolve at a particular temperature

43. Solubility curve Saturated Unsaturated Supersaturated

44. Solubility curve Any point on a line represents a saturated solution. In a saturated solution, the solvent contains the maximum amount of solute. Example At 90 o C, 40 g of NaCl(s) in 100g H 2 O(l) represent a saturated solution.

45. Solubility curve Any point below a line represents an unsaturated solution. In an unsaturated solution, the solvent contains less than the maximum amount of solute. Example At 90 o C, 30 g of NaCl(s) in 100g H 2 O(l) represent an unsaturated solution. 10 g of NaCl(s) have to be added to make the solution saturated.

46. Solubility curve Any point above a line represents a supersaturated solution. In a supersaturated solution, the solvent contains more than the maximum amount of solute. A supersaturated solution is very unstable and the amount in excess can precipitate or crystallize. Example At 90 o C, 50 g of NaCl(s) in 100g H 2 O(l) represent a supersaturated solution. Eventually, 10 g of NaCl(s) will precipitate.

47. Solubility curve Any solution can be made saturated, unsaturated, or supersaturated by changing the temperature.