# Wednesday, Sept. 5 th : “A” Day Thursday, Sept. 6 th : “B” Day Agenda  Homework Questions/Collect (Pg. 9: 1-10)  Sec. 1.1 Quiz: “What is Chemistry?”

• Published on
05-Jan-2016

• View
213

• Download
0

Embed Size (px)

Transcript

• Wednesday, Sept. 5th: A DayThursday, Sept. 6th: B DayAgendaHomework Questions/Collect (Pg. 9: 1-10)Sec. 1.1 Quiz: What is Chemistry?Lab discussionSec 1.2: Describing MatterMatter, volume, mass, weightUnits of measurement (base/derived) Conversions between unitsProperties of matter: physical & chemicalHomework: 1. Sec. 1.2 review, pg. 19: #1-11 2. Concept Review: Describing Matter

• HomeworkPg. 9: #1-10Questions?

Collect

• Section 1.1 QuizWhat is Chemistry?

You may use your guided notes and your book to complete the quiz

• Lab TechniquesLab DiscussionI 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 MatterMatter: 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 VolumeVolume: 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. MassIf 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: 200C, 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 dUnites

• 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 AnotherOther equivalent values that you need to know..

1 L = 1,000 mL = 1,000 cm31 mL = 1 cm3

Often, volumes are measured in cm3 and not mLcm3 is read cubic centimeter or cc(think of doctor showsI need 500 ccs, 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

Its just like youre multiplying by 1. Multiplying by 1 doesnt change the value, right?

• Sample Problem A, Pg. 14Converting UnitsConvert 0.851 L to milliliters, mL.

Always start with what you know: 0.851 LMultiply by a conversion factor to get the unit you want. In this case, 1 L = 1,000 mLThe unit that you WANT always goes ON TOP of the conversion factor!0.851 L X 1,000 mL = 851 mL1 L

• More Conversion PracticeConvert 0.765 g to kilograms.Always start with what you know: 0.765 gMultiply by a conversion factor to get the unit you want. In this case, 1 Kg = 1,000 gThe 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 UnitsDerived 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 MatterPhysical 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 substancesAs I was walking through the parking lot this morning, I found this necklace. I wonder if its pure silver? How could I test it to find out?

• Chemical PropertiesChemical property: a property of matter that describes a substances ability to participate in chemical reactions.

Examples:Reactivity with oxygenSensitivity to light

• HomeworkSec. 1.2 review, pg. 19: #1-11Concept Review: Describing Matter(Concept Review packet is due day of Chapter test)

• Looking AheadNext Time: Section 1.2 Quiz: Describing MatterLab Write-up

Wednesday:High School Open House6:30 8:00 pm