wednesday, october 14 objective: students will be able to apply the law of conservation of mass to...
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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
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
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
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
October 14, 2009
AGENDA:1 – Quick Chem and
Discussion2 – Quiz3 – Brain POP4 – Cornell Notes5 – Exit Slip
Today’s Goal: 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.
Quiz:
1. Define physical change.2. Describe a phase change
and give one example using the water cycle.
3. Define chemical change.4. In your words, state the
law of conservation of mass.
States of Matter Review
Definite shape Indefinite shape Indefinite shape
Definite volume Definite volume Indefinite volume
solid liquid gas
Cornell Notes Ms. Barkume10/14
Review: Chemical vs. Physical ChangesWhat 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.
Cornell Notes Ms. Barkume10/14
Review: Phase Changes
What are phase changes?
Physical changes that occur between the 3 states of matter.
Summary: Finish as homework.
Solid
Liquid Gas
Free
zing
Mel
tin
gEvaporation
Condensation
Sublimatio
n
Cornell Notes Ms. Barkume10/14
Law of Conservation of MassWhat 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 gramsMCO = 28 grams
Summary (finish for homework or in class if time permits)
Cornell Notes Ms. Barkume10/14
Law of Conservation of MassWhat 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)
1. 10.0 grams of hydrogen gas was reacted with 79.4 grams of oxygen to from water. How many grams of water was formed?
2. 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?
3. 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?
4. Challenge: 106.5 of HCl gas reacted with an unknown amount of NH3 to produce 157.5 grams of NH4Cl. How many grams of NH3 reacted?
Summary (finish for homework or in class if time permits)
Cornell Notes Ms. Barkume10/14
Mixtures and SolutionsWhat 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)
Percent Error
Percent Error: (Accepted Value – Measured Value) x
100 Accepted Value
Example: Accepted value = 1.2 Measured value = 1.3 (1.2 – 1.3) x 100 = 8.3 % 1.2Actual Density of H2O = 1.00 g/mL
Steps of Inquiry
Ask a QUESTION
Make a PROCEDURE
Interpret RESULTS
Make a Conclusion
Guides
Influences (data)
Using data to:
Density
Density is a physical property of matter.
Defined as the amount of mass per unit of volume.
Density = mass (grams)volume (mL)
Reading Graduated Cylinders
Graduated cylinders are used to measure volume of liquids.
How much liquid is the graduated cylinder?
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.
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
Reading Graduated Cylinders
Read at the meniscus10/10 =1
Every tick mark is 1mL
Volume = 35 mL
1/5 = 0.2
Every tick mark is 0.2 mLVolume
is 6.2 mL
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.
September 14, 2009
AGENDA:1 – Quick Chem and
Discussion2 – Get in lab groups3 – Safety Activity4 – Data and Data
Tables5 – Wrap Up
Today’s Goal: To understand the
importance of lab safety and lab safety rules
HOMEWORK:1. Complete lab
safety worksheet
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.
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!