Wednesday, Sept. 5th: “A” DayThursday, Sept. 6th: “B” Day

AgendaHomework Questions/Collect (Pg. 9: 1-10)Sec. 1.1 Quiz: “What is Chemistry?”Lab discussionSec 1.2: “Describing Matter”

Matter, volume, mass, weightUnits of measurement (base/derived) Conversions between unitsProperties of matter: physical & chemical

Homework: 1. Sec. 1.2 review, pg. 19: #1-11 2. Concept Review: “Describing Matter”

HomeworkPg. 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 MassMass: 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 WeightWeight: 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. QuantitativeTerms 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 UnitsQuantity: something that has magnitude, size, or amountUnit: a quantity adopted as a standard of measurement

Example: a graduated cylinderQuantity = the volume of a liquidUnit = milliliter (mL)

Units of MeasurementThe 7 BASE UNITS of measurement in the SI

system are:

“SI” stands for Systeme Internationale d’Unites

Units of MeasurementSometimes, 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 mLcm3 is read “cubic centimeter” or “cc”

(think of doctor shows…I need 500 cc’s, stat!)

Converting One Unit to AnotherConversion 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. 14Converting Units

Convert 0.851 L to milliliters, mL.

1.Always “start with what you know”: 0.851 L2.Multiply by a conversion factor to get the unit you

want. In this case, 1 L = 1,000 mL3.The unit that you WANT always goes ON TOP of the

conversion factor!0.851 L X 1,000 mL = 851 mL

1 L

More Conversion Practice

Convert 0.765 g to kilograms.1.Always “start with what you know”: 0.765 g2.Multiply by a conversion factor to get the unit you

want. In this case, 1 Kg = 1,000 g3.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 PracticeConvert 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 MatterMatter 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.

Examplescolor, state, melting point, boiling point,

density, hardness, etc.

DensityDensity: 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 PropertiesChemical property: a property of matter that

describes a substance’s ability to participate in chemical reactions.

Examples:Reactivity with oxygenSensitivity to light

Homework

Sec. 1.2 review, pg. 19: #1-11Concept 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