1. Objectives/Warm-Up  SWBAT describe and choose appropriate separation techniques.  Draw a diagram of: a solid and gas in a closed flask, a solid and gas in a closed flask, a liquid and solid in a closed flask, a liquid and solid in a closed flask, a solid, liquid and gas together in a closed flask. a solid, liquid and gas together in a closed flask.

2. Drill – 10/1 Draw a diagram of: 1. a solid and gas in a closed flask, 2. a liquid and solid in a closed flask, 3. a solid, liquid and gas together in a closed flask.

3. Drill – 9/28  Identify the type of matter – element, compound, homogenous mixture, heterogeneous mixture a. steel b. calcium chloride c. a person

4. FYI  There will be a Unit 2 Quiz next Tuesday on: Types of matter – element, compound, homogenous mixture, heterogeneous mixture Types of matter – element, compound, homogenous mixture, heterogeneous mixture Phases/States of matter – solid, liquid, & gas Phases/States of matter – solid, liquid, & gas Physical & Chemical changes Physical & Chemical changes Separations Separations Law of Conservations of Mass & Energy Law of Conservations of Mass & Energy

5. Phase Changes Deposition

6. Physical & Chemical Properties!  Physical properties: Do not change the chemical nature of matter  Chemical properties: Do change the chemical nature of matter

7. Physical & Chemical Changes  In a physical change, nothing new is created, the matter has just changed to another phase, separated or combined.  In a chemical change, the substances are altered chemically and display different physical and chemical properties after the change.

8.  Take out the green strips of paper and organize into Physical properties vs. Chemical properties!

9.  Get a textbook and Read pgs. 6-14 and Do #1-12 on pg. 25 on your own paper. You don’t need complete sentences, but you must write enough information to know the question and answer (i.e. don’t just use letters)

10. FYI  We will have a quiz next Tuesday on: Types of matter – element, compound, homogenous mixture, heterogeneous mixture Types of matter – element, compound, homogenous mixture, heterogeneous mixture Phases/States of matter – solid, liquid, & gas Phases/States of matter – solid, liquid, & gas Physical & Chemical changes Physical & Chemical changes Separations Separations Law of Conservations of Mass & Energy Law of Conservations of Mass & Energy

11. Physical Separations  Predict how to separate each of the following heterogeneous mixtures: Salt and pepper Salt and pepper Sand and iron filings Sand and iron filings Mud (dirt from the water) Mud (dirt from the water) Fruit salad (the different types of fruit) Fruit salad (the different types of fruit)

12. Drill – 9/29  Indicate if the following are physical or chemical changes: 1. Wood burning 2. Plants growing 3. Cutting paper 4. Ice melting

13.  “Separate This” WS

14. Techniques for Physical Separations  Filtration Filtration  Evaporation Evaporation  Centrifugation Centrifugation  Chromatography Chromatography  Decantation Decantation  Crystallization Crystallization  Distillation Distillation  Filtration Filtration  Evaporation Evaporation  Centrifugation Centrifugation  Chromatography Chromatography  Decantation Decantation  Crystallization Crystallization  Distillation Distillation

15. Filtration  A mixture is poured into a funnel fitted with a piece of filter paper.  Used for beer production and tap water (to remove solid impurities)

16. Evaporation  A homogenous mixture is heated so that the water evaporates and just leaves the solid behind

17. Centrifugation  Really fast spinning forces the solid or denser substance to the bottom of a sample

18. Chromatography  A mixture is allowed to move along a fixed material. The components of the mixture move at different speeds (based on their attraction to the solvent and the material) and so they separate from each other.

19. Decantation  Let the solid settle and then pour off the liquid, using something to block the solid

20. Crystallization  The process of forming crystals. Used to separate solids from solution.

21. Distillation When a solution is heated, the liquid with a lower boiling point evaporates. The hot vapor that formed can be condensed back to liquid again on a cold surface. EVAPORATION + CONDENSATION

22. Chemical Separations  Electrolysis  Chemical Reactions  Decomposition

23. Electrolysis Using electric current to force a chemical reaction with a separation occurring at the electrodes

24. Drill – 9/30  How would you separate a mixture of salt, sand, iron filings, ethanol and water into each of the components?

25. Law of Conservation of Matter and Energy  Matter and energy cannot be created nor destroyed, only changed in form.

26. Energy  Energy is the capacity to do work or to produce heat  Forms of Energy Potential – stored energy Potential – stored energy Kinetic – energy of motion Kinetic – energy of motion

27. Measuring Energy A calorie is the amount of heat needed to raise the temperature of 1 gram of water by 1 Celsius degree 1 cal = 1 gram x 1 C 0 The SI unit of energy is the joule (J) 1 cal = 4.184 J

29.  Chromatography Lab next class! We will use columns as our medium.

30. Drill – 10/5  Explain what chromatography is and how it works.

31. Chromatography  A mixture is allowed to move along a fixed material. The components of the mixture move at different speeds (based on their attraction to the solvent and the material) and so they separate from each other.

32. Each section is a fraction of the original sample

33.  2 phases:  Stationary phase = What you run your sample through. We will use a column. The column is non-polar  Mobile phase = The solvent that is run through the column. We will use water and isopropyl alcohol.