2. Wednesday, October 14 Objective:
Students will be able to apply the law of conservation of mass to reactions, contrast mixtures and substances.
Quick Chem: Label each as either a chemical change or a physical change.
Paper burning
Water freezing
Sugar carmelizing
Ice melting
Crushing rocks into smaller pieces

3. 4 Minutes Remaining…

4. Wednesday, October 14 Objective:
Students will be able to apply the law of conservation of mass to reactions, contrast mixtures and substances.
Quick Chem: Label each as either a chemical change or a physical change.
Paper burning
Water freezing
Sugar carmelizing
Ice melting
Crushing rocks into smaller pieces

5. 3 Minutes Remaining…

6. Wednesday, October 14 Objective:
Students will be able to apply the law of conservation of mass to reactions, contrast mixtures and substances.
Quick Chem: Label each as either a chemical change or a physical change.
Paper burning
Water freezing
Sugar carmelizing
Ice melting
Crushing rocks into smaller pieces

7. 2 MINUTES REMAINING…

8. Tuesday, October 13 last chance to view BR - 1 min
Objective:
Students will be able to apply the law of conservation of mass to reactions, contrast mixtures and substances.
Quick Chem: Label each as either a chemical change or a physical change.
Paper burning
Water freezing
Sugar carmelizing
Ice melting
Crushing rocks into smaller pieces

9. 30 Seconds Remaining…

10. 10 Seconds Remaining…

11. TURN IN YOUR BELLRINGER!

12. October 14, 2009 Today’s Goal: AGENDA: 1 – Quick Chem and Discussion
To apply law of conservation of mass, contrast mixture and substance.
HOMEWORK:
1. Make vocab flashcards for the vocabulary from sections 3.2 and 3.3.
AGENDA:
1 – Quick Chem and Discussion
2 – Quiz
3 – Brain POP
4 – Cornell Notes
5 – Exit Slip

13. Quiz: Define physical change.
Describe a phase change and give one example using the water cycle.
Define chemical change.
In your words, state the law of conservation of mass.

14. States of Matter Review
Definite shape
Indefinite shape
Definite volume
Indefinite volume
liquid
gas
solid

15. Review: Chemical vs. Physical Changes
Cornell Notes
Ms. Barkume
10/14
Review: Chemical vs. Physical Changes
What are the main differences between physical and chemical changes?
Example of Physical changes:
Examples of chemical changes:
Melting ice, crumpling paper, freezing water, cutting metal etc.
Any chemical reaction, Metal rusting, fruit ripening, cooking meat, burning gasoline in a car etc.
Summary: Finish as homework.
Physical Change
Chemical Change
Changes a characteristic that can be measured or observed without changing the sample’s composition. Reversible.
Ability to combine with one or more substances to form a new substance.
Ex. Color change, change in temperature, gas is evolved.

16. Cornell Notes Review: Phase Changes Solid Liquid Gas Freezing
Ms. Barkume
10/14
Review: Phase Changes
What are phase changes?
Physical changes that occur between the 3 states of matter.
Summary: Finish as homework.
Solid
Freezing
Sublimation
Melting
Condensation
Liquid
Gas
Evaporation

17. Cornell Notes Law of Conservation of Mass
Ms. Barkume
10/14
Law of Conservation of Mass
What is the law of conservation of mass?
Example:
Mass can neither be created nor destroyed, only changed.
Massreactants (beginning) = Massproducts(end)
Mass is conserved; products have same mass of reactants.
In a car’s catalytic converter CO reacts with 16 grams of O2 to form 44 grams of CO2. How much CO was reacted?
Massreactants= Massproducts
MCO + 16 grams O2 = 44 grams CO2
MCO = 44 grams – 16 grams
MCO = 28 grams
Summary (finish for homework or in class if time permits)

18. Cornell Notes Law of Conservation of Mass
Ms. Barkume
10/14
Law of Conservation of Mass
What is the law of conservation of mass?
Examples:
(put these in your notebook. #3 is your exit slip, put on another sheet of paper and turn it into the homework bin before you leave).
Massreactants (beginning) = Massproducts(end)
10.0 grams of hydrogen gas was reacted with 79.4 grams of oxygen to from water. How many grams of water was formed?
15.6 grams of sodium metal (Na) was reacted with an excess of chlorine gas (Cl) to from 39.7 grams of NaCl (table salt). How much Chlorine gas (Cl) was reacted?
A 10.0 gram sample of magnesium (Mg) reacts with oxygen (O2) to form 16.6 grams of magnesium oxide (MgO). How many grams of oxygen reacted?
Challenge: of HCl gas reacted with an unknown amount of NH3 to produce grams of NH4Cl. How many grams of NH3 reacted?
Summary (finish for homework or in class if time permits)

19. Cornell Notes Mixtures and Solutions
Ms. Barkume
10/14
Mixtures and Solutions
What are mixtures?
What are types of mixtures?
What are solutions?
Types of solutions:
Mixtures are combination of two or more pure substances where each retains its chemical properties.
Heterogeneous: does not blend smoothly throughout, individual substances remain distinct. (ex. Salad dressing, OJ with pulp)
Homogeneous: Constant composition throughout; a small sample will include all parts of the mixture. (ex. Salt water, air, metal alloys)
Homogeneous mixtures are also referred to as solutions. There is a constant composition throughout. Can be any phase of matter.
Gas-Gas, Gas-Liquid, Liquid-Liquid, Liquid-Solid, Solid-Solid
Summary (finish for homework or in class if time permits)

20. Exit Slip
Make a VENN DIAGRAM comparing and contrasting mixtures and solutions.
Mixtures
Solutions

21. Percent Error Percent Error: (Accepted Value – Measured Value) x 100
Example: Accepted value = 1.2
Measured value = 1.3
(1.2 – 1.3) x 100 = 8.3 %
1.2
Actual Density of H2O = 1.00 g/mL

22. Steps of Inquiry Ask a QUESTION Make a PROCEDURE Interpret RESULTS
Make a Conclusion
Guides
Influences (data)
Using data to:

23. Quiz (10 pts)
What is the volume of water in the graduated cylinder? Measure to 2 figures (numbers)

24. Density volume (mL) Density is a physical property of matter.
Defined as the amount of mass per unit of volume.
Density = mass (grams)
volume (mL)

25. Reading Graduated Cylinders
Graduated cylinders are used to measure volume of liquids.
How much liquid is the graduated cylinder?

26. Reading Graduated Cylinders
Graduated cylinders are used to measure volume of liquids (in mL).
How much liquid is the graduated cylinder?
The curved line is the meniscus. Read the volume from the bottom of the curve.
The volume of the liquid is 35 mL.

27. Reading Graduated Cylinders
Graduated cylinders are used to measure volume of liquids (in mL).
To read, find the lines labeled with numbers
Count the steps between
Divide
10/10 =1
Every tick mark is 1mL

28. Reading Graduated Cylinders
Read at the meniscus
10/10 =1
Every tick mark is 1mL
Volume = 35 mL
1/5 = 0.2
Every tick mark is 0.2 mL
Volume is 6.2 mL

29. Types of Data Data does not equal scientific evidence
Previous knowledge + DATA = Scientific Evidence
Qualitative Data: information that describes color, odor, shape, or some other physical properties
Quantitative Data: Numerical information that tells you how much, how little, how big, how tall or how fast.
Data Tables organize data for display and understanding.

30. September 14, 2009 Today’s Goal: AGENDA: HOMEWORK:
To understand the importance of lab safety and lab safety rules
HOMEWORK:
Complete lab safety worksheet
AGENDA:
1 – Quick Chem and Discussion
2 – Get in lab groups
3 – Safety Activity
4 – Data and Data Tables
5 – Wrap Up

31. Data Table Data Tables display data
Previous knowledge + DATA = Scientific Evidence
Qualitative Data: information that describes color, odor, shape, or some other physical properties
Quantitative Data: Numerical information that tells you how much, how little, how big, how tall or how fast.

32. Understanding Lab Safety
You should NEVER try to taste any of the substances.
You should ALWAYS wear your lab goggles. Some of the lab materials are skin, eye irritants.
Always dispose of the laboratory materials appropriately.
Wear appropriate clothing and shoes.
REMEMBER the class rule: FOLLOW DIRECTIONS!