1. I. Classification of Matter MATTER (anything that has mass & takes up space)

2. MATTER PURE SUBSTANCE (matter with a definite composition) Ex- water, helium, carbon dioxide, sodium

3. MATTER MIXTURE (2 or more pure substances combined in ANY ratio) Ex- lemonade, concrete, shaving cream

4. Pure Substances COMPOUND (2 or more elements chemically bonded together) Ex- sodium chloride, water, glucose, CLUE- chemical formulas have 2 capital letters; it is NOT on the periodic table

5. Pure Substances ELEMENT (cannot be broken down any further) Ex- carbon, oxygen, lithium, hydrogen CLUE- It is any substance written on the periodic table

6. Mixtures SOLUTION (a homogeneous mixture that cannot be filtered & will NEVER settle upon standing)homogeneous Ex- saline solution, grape juice CLUE- It is clear (might be clear & colored)

7. Mixtures COLLOIDAL SUSPENSION (a homogeneous mixture that cannot be filtered & will EVENTUALLY settle upon standing) Ex- mayo, milk, fog, cool whip CLUE- it creates the Tyndall EffectTyndall Effect

8. Mixtures COURSE SUSPENSION (a heterogeneous mixture that can be filtered & will QUICKLY settle upon standing) Ex- Italian Dressing, OJ CLUE- it has distinguishable “pieces” in it.

9. SOLUTION ALLOY (a special type of solution where 2 or more METALS mix together----a “metallic solution”) Ex- brass (zinc & copper); pewter (tin & lead); steel (iron & carbon) CLUE- It is NOT on the periodic table

10. VOCABULARY HELP: Homogeneous: ___________________________ ________________________________________ when a material appears the SAME throughout

11. Heterogeneous: __________________________ ________________________________________ When a material appears to be DIFFERENT throughout

12. Tyndall Effect: ___________________________ _______________________________________ Real Life Examples: the effect of light scattering on particles in a colloid that makes it appear to be cloudy under the light. (even though it might look clear otherwise) -Fog -The reason we see the sky as blue

13. Mixture Demonstrations: Watch the following demos to describe different mixtures. One of each type of mixture (solution, colloid, & course suspension) will be demonstrated. Pick at least one of each type of mixture and write/draw it to describe what happened. LABEL the demo as an example of either a solution, colloid or course suspension & GIVE YOUR PROOF. Type of Mixture DemonstrationProof COLLOID SOLUTION COARSE SUSPENSION

14. II. Physical Properties of matter that we will use to help us separate a solution? A. ___________________________ Magnetism Demonstration – Magnetism:

15. B. ___________________________ C. ____________________________ 1. Lab techniques that uses phase change separation. a. ____________________________ ____________________________ ___________________________ Density Phase Changes Distillation – uses different boiling points of the pure substances involved to separate and CAPTURE all of the substances of the mixture

16. Distillation Demo:

17. b. ______________________ D. ___________________________ 1. Lab techniques that use particle size separation. a. ____________________________ ____________________________ Crystallization – separation technique that uses the boiling point to capture ONLY the substance with the HIGHEST boiling point Particle Size Filtering – using a screen or paper to help retain the larger items, while the smaller pass through

22. E.__________________________________Can dissolve in water (Soluble in water)

23. III. Characteristics of Solutions A. Parts of a Solution Solvent – the substance doing the dissolving Solute – the substance being dissolved

24. B. Terms related to solutions: 1. Soluble -___________________________ _________________________________ ex – 2. Insoluble - _________________________ __________________________________ ex - Able to dissolve in each other Salt is soluble in water NOT able to dissolve in each other Water is insoluble in water

25. 3. concentration - _________________________ _____________________________________ 4. Diluted solution - _______________________ ______________________________________ 5. Concentrated solution - __________________ ______________________________________ the amount of solute in a solution when you add more solvent to a solution in order to decrease the overall concentration when you remove solvent from a solution in order INCREASE the overall concentration

26. C. Rate of solution: 1. Definition: ________________________ ________________________________ the speed at which a solvent is able to dissolve a solute

27. 2. Ways to increase the speed at which the solvent dissolves the solute. a. _____________________________ Demo: b. _____________________________ Demo: c. _____________________________ Demo: Increase temperature Increase surface area Stir or Shake

28. D. How do You Describe The Amount of Solute in a Solution? 1. Definition of each: a. Unsaturated- _____________________ ________________________________ Does not have all of the solute that it could at a given temperature

29. i. if you add one more piece of _____________ to an unsaturated solution, it will _______________ into the beaker of solution. solute dissolve

30. b. Saturated - ____________________________ _____________________________________ i. if you add one more piece of _____________ to a saturated solution, it will __________________ in the beaker. Has all of the solute that it can at a given temperature solute Stay as a crystal

31. c. supersaturated - _______________________ ____________________________________ i. if you add one more piece of _____________ to a super-saturated solution, it will __________________ in the beaker. Has more solute than it SHOULD at a given temperature solute crystalize

32. Demonstration – Super Saturated Solution:

33. E. Solubility and Solubility Curves 1. Solubility - __________________________ ___________________________________ 2. Solubility Curve – __________________________ ________________________________________ The total amount of solute necessary to make a saturated solution at a GIVEN TEMPERATURE a graph that illustrates the solubility of given solutes in certain solvents

34. 1.What is the title of this graph? 2.What is the x-axis label? 3.What is the x-axis unit of measurement? 4.What is the y-axis label? 5.What is the y-axis unit of measurement? 6.What is the general trend expressed by this graph?

35. UNSATURATED- anything under the line SUPERSATURATED- anything above the line SATURATED - anything on the line

36. 1.What is the temperature of a saturated solution of 36 g / 100 g of water? 2.What is the solubility of BaCl2 at 60 C? 3.If a solution has 40 g of BaCl2 dissolved in 100 g of water and it is at 70 C, how would you characterize it?

37. 4. How would you create a supersaturated solution?

38. c. Common trend between temperature and heat i. as temperature __________________, solubility _________________. increases

39. 1.Which salt is the most soluble at 70 C? 2.Which salt’s solubility is least affected by temperature? 3.Which salt’s solubility is most affected by temperature?