Wednesday, Sept. 5th: “A” Day
Thursday, Sept. 6th: “B” Day
Agenda
 Homework Questions/Collect (Pg. 9: 1-10)
 Sec. 1.1 Quiz: “What is Chemistry?”
 Lab discussion
 Sec 1.2: “Describing Matter”
 Matter, volume, mass, weight
 Units of measurement (base/derived)
 Conversions between units
 Properties of matter: physical & chemical
 Homework: 1. Sec. 1.2 review, pg. 19: #1-11
2. Concept Review: “Describing Matter”
Homework
Pg. 9: #1-10
Questions?
Collect
Section 1.1 Quiz
“What is Chemistry?”
You may use your guided notes and your book
to complete the quiz……
“Lab Techniques”
Lab Discussion
I just wanted to take a few minutes to go over
the lab analysis/conclusion questions so that
you know what I expect in future labs…
Sec 1.2: “Describing Matter”
Matter: anything that has mass and takes up
space.
Sort Into: Matter, not matter, not sure.
Peanut butter, water, fish, energy, garbage, time,
motion, the human brain, carbon dioxide, air,
yourself, an idea, a tree.
The Space an Object Occupies is its
Volume
Volume: A measure of the size of a body or
region in 3-dimensional space
How to find volume:
Solids: (length) X (width) X (height)
OR
Liquid displacement
Liquids: graduated cylinder
The Quantity of Matter is the Mass
Mass: A measure of the amount of matter in
an object; a fundamental property of an object
that is not affected by the forces that act on
the object, such as the gravitational force
How to measure mass:
Balances, either mechanical or electronic
Mass is not Weight
Weight: A measure of the gravitational force
exerted on an object; its value can change
with the location of the object in the universe
Weight and mass are not the same thing!
Weight vs. Mass
If you were on the moon, would your mass change?
What about your weight?
Qualitative vs. Quantitative
Terms such as heavy, light, rough, and smooth
describe matter qualitatively.
They describe the “quality” of matter but
DO NOT use numbers.
Scientists describe matter in quantitative
terms, using numbers.
They describe the “quantity” of matter.
Examples: 200˚C, 15 mL, 10 sec
Quantities and Units
Quantity: something that has magnitude,
size, or amount
Unit: a quantity adopted as a standard of
measurement
Example: a graduated cylinder
Quantity = the volume of a liquid
Unit = milliliter (mL)
Units of Measurement
The 7 BASE UNITS of measurement in the SI
system are:
“SI” stands for Systeme Internationale d’Unites
Units of Measurement
Sometimes, the base units can be too big or
too small for certain measurements, so
prefixes are added to the base units.
Converting One Unit to Another
Other equivalent values that you need to
know…..
1 L = 1,000 mL = 1,000 cm3
1 mL = 1 cm3
Often, volumes are measured in cm3 and not mL
cm3 is read “cubic centimeter” or “cc”
(think of doctor shows…I need 500 cc’s, stat!)
Converting One Unit to Another
 Conversion factor: A ratio that is derived from the
equality of 2 different units and that can be used to
convert from one unit to the other.
**Conversion factors are fractions that are always
equal to 1**
 Example: 1 dozen eggs = 12 eggs
The 2 conversion factors are:
12 eggs OR 1 dozen
1 dozen
12 eggs
 It’s just like you’re multiplying by 1. Multiplying by 1
doesn’t change the value, right?
Sample Problem A, Pg. 14
Converting Units
Convert 0.851 L to milliliters, mL.
1. Always “start with what you know”: 0.851 L
2. Multiply by a conversion factor to get the unit you
want. In this case, 1 L = 1,000 mL
3. The unit that you WANT always goes ON TOP of
the conversion factor!
0.851 L X 1,000 mL = 851 mL
1L
More Conversion Practice
Convert 0.765 g to kilograms.
1. Always “start with what you know”: 0.765 g
2. Multiply by a conversion factor to get the unit you
want. In this case, 1 Kg = 1,000 g
3. The unit that you WANT always goes ON TOP of
the conversion factor!
0.765 g X 1 Kg = .000765 Kg
1,000 g
More Conversion Practice
Convert 17.3 m to centimeters.
Convert 5.13 m to millimeters.
Derived Units
Derived units: units found by multiplying or
dividing the 7 base units.
Examples:
Speed is m/s (meters divided by seconds)
Area is m2 (length X width)
Volume is cm3 (length X width X height)
Properties of Matter
Matter has many properties.
These properties can be classified as either
physical or chemical…
Properties of Matter
Physical property: A characteristic of a
substance that does not involve a chemical
change, such as density, color, or hardness.
Examples
color, state, melting point, boiling point,
density, hardness, etc.
Density
Density: the ratio of the mass of a substance
to the volume of the substance; often
expressed as grams per cubic centimeter
(g/cm3) for solids and liquids and as grams per
liter (g/L) for gases.
Density = mass
volume
The density of a substance is the same no
matter what the size of the sample is.
Density is a PHYSICAL property.
Density can be used to identify
substances
As I was walking through the parking lot this
morning, I found this necklace. I wonder if it’s
pure silver? How could I test it to find out?
Chemical Properties
Chemical property: a property of matter that
describes a substance’s ability to participate in
chemical reactions.
Examples:
Reactivity with oxygen
Sensitivity to light
Homework
Sec. 1.2 review, pg. 19: #1-11
Concept Review: “Describing Matter”
(Concept Review packet is due day of Chapter test)
Looking Ahead
Next Time:
Section 1.2 Quiz: “Describing Matter”
Lab Write-up
Wednesday:
High School Open House
6:30 – 8:00 pm