1. Unit 1 thus far… What we have discussed… What we have yet to discuss…
States of matter
Phase changes
Physical/chemical properties and changes
Density and specific heat calculations
What we have yet to discuss…
Classification of matter
How to separate matter physically
Test next Tuesday, September 19th

2. How is matter classified? How can mixtures be separated?
Essential Questions
How is matter classified?
How can mixtures be separated?

3. Classification of Matter
Pure Substance – materials that always have the same (definite) composition
B. Mixture – 2 or more different materials physically combined

4. Pure Substances
1. Element – simplest forms of matter made up of one type of atom
Ex: carbon, sodium, helium
2. Compound – substance that is made from the atoms of two or more elements that are chemically bonded
Ex: NaCl – sodium chloride
sugar (sucrose) – C12H22O11

5. Mixtures
1. Homogeneous – uniform in composition & properties throughout Ex) salt water, air, alloys

6. Homogeneous Mixture Example
Solution – homogeneous mixture consisting of a solute & a solvent
i . solute – dissolved material
ii. solvent – material doing the dissolving

7. Mixtures Cont.
Heterogeneous – not uniform in composition & properties throughout
Ex: sand, chocolate chip cookie dough
a. Suspension – particles are dispersed throughout a liquid, but eventually settle out (muddy water)

8. Review
How would you classify matter that you cannot separate physically, but you can chemically?

9. Review
How would you classify matter that you can separate physically, and is not uniform throughout?

10. Review How is a colloid different from a solution?
How is a colloid different from a suspension?

11. Review
Describe the Tyndall Effect.

12. b. Colloid – tiny particles are dispersed throughout another substance, but will not settle out (jello)
Aerosols –solid or liquid particles in a gas Ex. Spray paint, fog, smoke
Foams – a gas in a liquid Ex. whipped cream, marshmallow
Emulsion – a liquid in a liquid Ex. mayonnaise. cheese
Sols – solids in liquids or solids in solids Ex. jellies, Jello!

13. Emulsion

14. 1. Separation of a Mixture
*Mixtures can occur in any state or combination of states and can be separated physically

15. Lab # 3 Writeup
Intro: a procedure of what you did in paragraph form. Include the name of the technique you used
Data: Any data you recorded in list format
Data Analysis: Calculation in lab. Be sure to label
Conclusion: answer the questions in the lab as thorough as you can.

16. Filtration Separates an insoluble solid from a liquid
Solid is collected on filter paper
Filtrate (remaining liquid) is
collected in a beaker
LAB HINTS:
Always measure the mass of your
filter paper before filtering

17. Evaporation Used when 2 substances have different boiling points
Only 1 of the substances remains
LAB HINTS:
Measure the mass of
the empty evaporating dish
Don’t heat on high the entire time

18. Distillation
Separation of two liquids with different boiling points

19. Extraction
Separation based on differences in solubility in at least two different solvents (liquids)
LAB HINTS:
You can also use a pipet if you don’t have a separatory funnel

20. Centrifuge Used to collect precipitate formed from two solutions
1st centrifuge the mixture
Uses centripetal force to push solid to bottom
2nd decant (pour off) the remaining liquid

21. Magnetism & Floatation
Magnetism-separates one magnetic substance from a non-magnetic substance
LAB HINT: Wrap magnet in plastic wrap
Floatation-uses the concept of different densities to separate a mixture

22. How would you separate the following mixtures?
When two liquids combine, a precipitate (solid) is formed. How would you separate the precipitate from the remaining solution?

23. How would you separate the following liquids?
You have two liquids with very different boiling points. What technique would you use to separate them if you want to end up with both liquids?
If you only need to keep one of the liquids?

24. Separation of a mixture
How would you separate a mixture containing corn oil, salt, and water?

25. Lab
You have a mixture of salt, sand, iron, and styrofoam. Describe a procedure you could do to end up with all four components. (This will be multiple steps)

26. Lab Get a weigh boat, put your names on it, find mass
Get sample from Mr. Keith, find mass of mixture
Use the following techniques to separate mixtures:
Note: Be sure to measure and label EVERYTHING!!!!!!

27. Essential Question
How do matter and energy relate to chemistry?

28. Conservation of mass
Think: looking at the name, what is your own definition of the conservation of mass?
Think about the conservation of energy

29. Conservation of Mass
In a closed system, the mass of the reactants is equal to the mass of the products.
CaC2 + H2O  Ca(OH)2 + C2H2
Example: Calcium carbide and water react to form calcium hydroxide and acetylene. If 8.0 g of calcium carbide react with 10.0g of water to form 16.0 g of calcium hydroxide, what mass of acetylene was produced?

30. Endothermic vs. Exothermic
What is the difference?

31. Endothermic vs. Exothermic
Ammonium nitrate + barium hydroxide
Draw an energy diagram for this reaction.