INTRODUCTION TO CHEMISTRYLAB SAFETYMATTER

Chapters 1-2

WELCOME TO CHEMISTRY!! Please find your table with the same letter as what is on

your lined index card (you may sit in any seat at that table)

On the same side (lined) of the index card, please write your… Name – (First) (Last) (name like to be called)

**This is how I will be taking attendance today!!*** Where you would like to sit (like where you are, front,

back, around people, etc) What you are most and least looking forward to in this

class

Please pick up the three sheets of paper by Lab Station 1 Syllabus Green “Student Information Sheet”-start filling out for

me please “FLINN Safety Contract”

SYLLABUS AND RULES OF THE CLASS

Looking over the unit you will find we have quite a bit to cover….

What you will need to be successful: Pens and pencils (mechanical pencils) 3 Ring Binder and notebook paper Dividers (Bell work, worksheets, hw, study

guides) CALCULATOR!! Scientific works best!

PROCEDURES IN THE CLASSROOM

RISK Turn in papers - Absent/Make up work Extra Help

After school on Tuesdays/Thursdays, or by requestSGA Advisor/softball coach so please let me know

ahead of time! Tests– Students can retake tests within ONE WEEK of return date

as long as they have all of their homework in for that unit and they attend teacher remediation outside of Husky Help; students with a class average of 70% or below will be allowed to remediate in Husky Help.

 Retakes take a different form than the initial test. If the student is absent on the retest day, their absence must be

excused and they must take the test the day they return.

FLINN SAFETY CONTRACT

Take a few minutes to read over the Safety Contract.

We will watch a movie and I want you to highlight what rule(s) you saw in the movie

http://www.youtube.com/watch?v=B5wyM_CRsqw

Be ready for a Safety Quiz on WEDNESDAY!

CREATING A DIVERSITY QUILT

With the index card you filled out this morning….please put your name you would like to be called on the front

Decorate this card to represent who YOU are. Ex: Ms. Nock’s card

CHEMISTRY MISCONCEPTIONS

Try to answer each question the best you can. For every false, explain why you think it is

false

**I encourage you to work in partners/groups on this**

In 15 minutes we will go over the answers….

Warm Up for Tuesday, August 25(Remember to write the question AND answer to prepare you for

the quiz!

1. Whose responsibility is it to keep the lab clean?

2. Describe at least three different safety rules we discussed in class yesterday.

TURN IN YOUR Green SHEET TO THE BIN IF YOU HAVE IT SIGNED!

MILK LAB

Lab Procedures: Please stay at your station If you need to gather supplies, only send one

person in your group to get the supplies Limit the amount of papers going to the station

(1 sheet is all you need per student) **Milk, food coloring, and soap will be used, if

you have an allergies please let me know**

BEFORE YOU BEGIN THIS LAB, WRITE YOUR HYPOTHESIS!

LAB SAFETY

GLASSWARE SAFETYHandle glassware carefully.Never use broken or chipped glassware.Never heat glassware that is not

thoroughly dry. Always clean glassware at the end of each lab.

FIRE SAFETY Always wear safety goggles. Never heat anything unless instructed to

do so. Never heat anything in a closed container. Never leave a lit burner or hot plate

unattended. Never reach across a flame. Tie back long hair and do not wear loose

clothing. Always maintain a neat work area

especially when using a flame. Flammable liquids (ex. alcohol) should

never be poured/ placed near an open flame.

Always use tongs or heat-resistant gloves to handle hot objects.

Know the location of the fire blanket/extinguisher.

If there is a fire, notify the teacher immediately and wait for instructions.

CHEMICAL SAFETYWear goggles, lab aprons,

closed-toed shoes when dealing with chemicals.

Check the labels on chemical bottles twice before removing any of the contents.

Never return unused chemicals to their original container.

Keep all lids closed when chemicals are not in use.

Dispose of all chemicals as instructed by your teacher.

CHEMICAL SAFETY (CONT’D) Immediately rinse with water any chemicals,

particularly acids, that get on your skin and clothes. Then notify your teacher.

Never touch, taste, or mix any chemical unless instructed to do so.

Never smell any chemical directly from its container. Use your hand to waft some of the odors from the top of the container toward your nose, but ONLY if you are instructed to do so.

ACID SAFETYDo not smell, waft, or touch acids. If acid gets on your skin or clothes,

immediately rinse with water.

To dilute an acid, add acid slowly to water, while stirring.

If acid is spilled, it can be neutralized with sodium bicarbonate solution and then soaked up with paper towels.

MSDS

Hazard Rating Chart

EYE & FACE SAFETY

Wear safety goggles any time you are using chemicals, heat, or glassware.

Do not remove your goggles at any time during the lab.

When you are heating a test tube or bottle, always point it away from you and others.

If a chemical should splash in your eye or on your skin, immediately flush with water from the eyewash station or safety shower for at least 20 minutes.

ELECTRICAL SAFETY

Never use long extension cords to plug in electrical devices. Do not plug too many appliances into one socket or you may

overload the socket and cause a fire. Never touch an electrical appliance or outlet with wet hands.

Make sure lab table surface is dry.

GENERAL SAFETYNo unnecessary movementAbsolutely no horseplayFollow all instructions and do not improvise. If

you are uncertain about what to do next, ask your teacher first.

Report any accidents/spills to instructor immediately – no matter how trivial. Clean up spills immediately.

Use appropriate disposal techniques for chemicals.- Flammable liquids or solid chemicals must be placed in a designated chemical waste container.

Clean your lab area thoroughly before leaving.Keeping a clean laboratory is the responsibility of

the students leaving the lab.

WHAT MATH DID YOU TAKE?

We will take a math skills assessment to see how well you did and what level you are going into this class.

If you feel that you are struggling, do not worry. We can talk individually to see where you want to be

#7 you are solving for M1 Please turn in assessment into bin (behind

TV) and pick up the Misconceptions Sheet. Start working on this individually and then we will discuss!

Chapter 1

INTRODUCTION TO CHEMISTRY

WHAT IS CHEMISTRY?

Chemistry: study of the composition of matter & the changes that matter undergoes.

Matter: anything that has volume and mass. Volume: the amount of space an object takes up Mass: the amount of matter in an object (i.e. # of particles)

What is NOT matter? Light, Heat, Radio waves,

Magnetic fields

SUBDISCIPLINES OF CHEMISTRY

Organic Chemistry Inorganic Chemistry Biochemistry Analytical Chemistry Physical Chemistry

ORGANIC CHEMISTRY

Study of chemicals containing carbon. All life is carbon-based!

INORGANIC CHEMISTRY

Study of chemicals that (in general) do not contain carbon.

Chemicals that are found mainly in non-living things.

BIOCHEMISTRY

Study of processes that take place in organisms.

ANALYTICAL CHEMISTRY

Focuses on the composition of matter. Ex. How much lead is found in tap water?

Gas Chromatography

PHYSICAL CHEMISTRY

The mechanism, the rate, and the energy transfer that occur when matter undergoes a change.

THE SCALE…. HOW SMALL IS SMALL?

Macroscopic: properties of matter that are large enough to be seen with the unaided eye.

Microscopic: objects or properties of matter that can only be seen using a light microscope.

Submicroscopic: matter that cannot be seen even with the most powerful light microscope. Example: Atoms (pencil dot = 1 x 1020 atoms) Scanning tunneling microscope (STM): produces images on

a computer screen of the locations of individual atoms.

SCANNING ELECTRON MICROSCOPE IMAGES

Ant Pollen

SCANNING TUNNELING MICROSCOPE

Silicon surface atoms enlarged 20 million times by a Scanning Tunneling Microscope.

NUMBERS IN CHEMISTRY

Measurement (Ch 3)

Warm-Up-or piece of paper if you do not have one yet

1. Name the equipment:a. b.

c.

2. List all safety rules of the classroom for your quiz today (without looking ;) )

**Turn in the student info. Sheet if you have it signed! ***

◦ We can use a word like a “dozen” to specify a certain quantity.

Mole (mol): SI unit for measuring the amount of a substance.

1 mol = 6.02 x 1023 representative particles

Avogadro’s Number: 6.02 x 1023

Representative Particle: smallest unit that has all the characteristics of that substance.

The Mole

Conversions

4 moles Ca = atoms Ca.

4 moles Ca 6.02 x 1023 atoms Ca 1 mole Ca

= 2.41 x 1024 atoms Ca

Conversions 5 x 1018 atoms Cu = moles

Cu.

5 x 1018 atoms Cu 1 mole Cu 6.02 x 1023 atoms Cu

= 8.3 x 10-6 moles Cu

Warm Up-Convert the following 

0.35 mole He = ______________ atoms

4.5 x 1023 molecules C6H12O6 = __________ moles

  2.5 moles O2 = ___________ molecules

1.5 x 1020 atoms Cu = ________ moles 

Conversions

9.2 moles F2 = molecules F2?

9.2 moles 6.02 x 1023 molecules F2

1 mole= 5.5 x 1024 molecules F2

ONCE YOU ARE FINISHED WITH THE QUIZ…

Place quiz in bin Try the worksheet you picked up front when

you are finished. Work quietly until everyone is finished.

WHEN YOU ARE FINISHED WITH THE QUIZ..

Place quiz in the bin Take out your packet and try to work on

scientific notation quietly until everyone is finished.

THE NUMBER COMFORT ZONE

We are used to Small Numbers Lunch for $2.25 or $5.50 Tickets for $25, $50, or $125 Car for $2,500, or $23,000

But $9,000,000,000,000 deficit is too big to get our mind around. (Nine Trillion Dollars)

Science uses very large or very small numbers

TWO WAYS SCIENTISTS GET NUMBERSINTO THE COMFORT ZONE

Use units to express amount Kilobuck

$ 1000 Milligram

60 milligram Tylenol tablet has 0.060 grams ingredient.

Use Scientific Notation 6.023 x 1023 atoms per mole

SCIENTIFIC NOTATION

Scientific Notation was developed in order to easily represent numbers that are either very large or very small.

Scientific Notation is based on powers of the base number 10.

Examples:The number 200,000,000,000 grams in

scientific notation is written as 2 x 1011 grams

The number 0. 000,006,645 kilometers in scientific notation is written as 6.645 x 10-6 kilometers

WRITING SCIENTIFIC NOTATION

6.645 x 10-6

Liters

 

Coefficient• Must be greater or

equal to 1 and less than 10

Base• Must ALWAYS be

10

Exponent (Power of 10)• Shows the number of

places the decimal needs to be moved to change the number to standard notation

• A negative exponent means the standard notation is less than one

CHANGING FROM STANDARD FORM TO SCIENTIFIC NOTATION

1. Place decimal point such that there is one non-zero digit to the left of the decimal point.

For example:42864900000 = 42864900000. Move the decimal:

4.2864900000

CHANGING FROM STANDARD FORM TO SCIENTIFIC NOTATION

2. Count number of decimal places the decimal has "moved" from the original number.  This will be the exponent of the 10.

4.2864900000. Originally the decimal was at the end.

The decimal moved 10 places to the LEFT.

CHANGING FROM STANDARD FORM TO SCIENTIFIC NOTATION

3. Determine if the exponent is negative or positive. If the original number was less than 1, the

exponent is negative. i.e. 0.00001114 = negative exponent

If the original number was greater than 1, the exponent is positive. i.e. 111,400,000 = positive exponent

WARM UP FOR THURSDAY, AUGUST 28 Write the following

numbers in Scientific Notation:96,400

0.361

0.0057300

6,587,234,000

8.00

= 9.64 x 104

= 3.61 x 10-

1

= 5.7300 x 10-3

= 6.587234 x 109

= 8.00 x 100

PRACTICE

Write the following numbers in Standard Notation:3.97 x 103

8.862 x 10-1

6.251 x 109

5.12 x 10-8

3.159 x 102

= 3,970

= 0.8862

= 6,251,000,000= 0.0000000512

= 315.9

CONVERSIONS!! REMEMBER THESE? 1 Megameter (Mm) = 1 x 106 meters 1 kilometer (km) = 1000 meters 1 hectometer (hm) = 100 meters 1 dekameter (dkm or dam) = 10 meters--------------------------------------------- 1 meter = 10 decimeters (dm) 1 meter = 100 centimeters (cm) 1 meter = 1000 millimeters (mm) 1 meter = 1 x 106 micrometers (μm) 1 meter = 1 x 109 nanometers (nm) 1 meter = 1 x 1012 picometers (pm)

EXAMPLES

Calculate the number of seconds in one day. Conversion Factors needed:

1 day = 24 hours 1 hour = 60 minutes 1 minute = 60 seconds

1 day xxx 24 hr1 day

60 min 1 hr

60 sec 1 min

The conversion factors are written as:

UNKNOWN KNOWN

PRACTICE

At a meeting, 28 people are each given 3 pens. If there are eight pens in one package, priced at $1.88 per package, what is the total cost of giving away the pens?

28 people

x $1.881 pkg

1 pkg8 pens

3 pens 1 person

xx

Answer: $19.74

SI UNIT PREFIXES

SI = Standard International Metric System (based on power of 10)

Mega- (M) = 1,000,000 (1 x 106) Kilo- (k) = 1,000 (1 x 103) Hecto- (h) = 100 (1 x 102) Deca- (dc) = 10 (1 x 101) BASE = 1 (1 x 100) Deci- (d) = .1 (1 x 10-1) Centi- (c) = .01 (1 x 10-2) Milli- (m) = .001 (1 x 10-3) Micro- (μ) = .000001 (1 x 10-6) Nano- (n) = .000000001 (1 x 10-9) Pico- (p) = .000000000001 (1 x 10-12)

1 Megameter (Mm) = 1 x 106 meters 1 kilometer (km) = 1000 meters 1 hectometer (hm) = 100 meters 1 dekameter (dkm or dam) = 10 meters--------------------------------------------- 1 meter = 10 decimeters (dm) 1 meter = 100 centimeters (cm) 1 meter = 1000 millimeters (mm) 1 meter = 1 x 106 micrometers (μm) 1 meter = 1 x 109 nanometers (nm) 1 meter = 1 x 1012 picometers (pm)

CONVERSION FACTORS – MEMORIZE-COPY INTO YOUR NOTES! WARM UP

CONVERTING BETWEEN UNITS

How many grams are in 3.4 kg?

1 kg = 1000 g

Therefore:

3.4 kg 3400 g

1000 g 1 kg

=x

PRACTICE

250 cm = ________ m

1.46 L = ________ mL

4.6 x 10-4 dg = ________ g

2.50

1460

4.6 x 10-3

SI BASE UNITS

Base Quantity Base Unit Symbol

Length Meter m

Mass Kilogram kg

Time Second s

Temperature Kelvin K

Amount of Substance Mole mol

Pressure Atmosphere atm

Electric Current Ampere A

Volume Liter L

Energy Joule J

WARM UP FOR FRIDAY, AUGUST 28-ALL GREEN SHEETS DUE TODAY! TURN INTO BIN PLEASE !

Express in scientific notation:1. ) 0.0032. ) 204000

Express in Standard:3)3 x 10-5

4) 6.589 x 103

Convert (show your work): 5) How many molecules are in 25 mol Cl2?

6) How many moles are in 3.45x1025 molecules?

Convert (K=273+ °C)7) 400K = ? °C

8) 25°C = ? K

BELL WORK QUIZ

1 mol = 6.02x1023

When you are finished, place quiz into the bin and go straight to the lab station you were left at yesterday and finish your lab!

ARE YOU ACCURATE OR PRECISE?

SCIENTIFIC MEASUREMENT

Measurement: a quantity that has both a

number and a unit.

Accuracy: The closeness of a

measurement to its accepted value.

Precision: A measure of how close a

series of measurements is to one another.

PERCENT ERROR

% Error = experimental value – accepted value x 100%

accepted value

Used to determine accuracy and precision.

Experimental Value/Calculated Value: value measured in lab

Accepted Value: correct value based on reliable references

FACTOR-LABEL METHOD

Most important mathematical process in Chemistry!

What does “Factor-Label” mean?

Factors are the numbersLabels are the units

i.e. 84.465 milliliter

All measurements must have a number and a unit!

FACTOR-LABEL METHOD

When using the factor-label method, problems consist of three parts: GKU

1. a known beginning – GIVEN

2. a desired end – UNKNOWN

3. a connecting path – KNOWN

CONVERSION FACTORS What are conversion factors?

EQUALITIES For example: 12 in = 1 ft

1 mi = 5280 ft

Conversion factors will be written as “tops & bottoms” For example:

12 in 1 ft

1 mi 5280 ft

Conversion factors can be “flipped” depending on which unit needs to be canceled.

PRACTICE

Elephants tend to travel in herds, which consist of 10-20 elephants. If a herd of elephants contain 17 elephants, how many elephant legs are there? (HINT: 1 elephant=4 legs) <-usually17

elephants 4 legs1 elephant

x

Answer: 68 elephant legs

WARM-UP ON INDEX CARD PLEASE WRITE THREE TOPICS AND

TURN TO THE BIN1.) What types of equipment would you use to measure

Volume of a liquid?

2.) What is a theory?

3.) Convert 789 km to cm

4.)Using the formula: K = 273 + °C, find the following:

a. 35 °C = K? b. 250K = °C?

5. )Convert the following to scientific/standard notation.

a.) 0.005 b.) 1200500

c.) 1.5 x104 d.) 3.75x10-2

6.)What volume of silver metal will weigh exactly 2500 g? The density of silver is 10.5 g/cm3.

WHEN YOU ARE FINISHED WITH THE QUIZ

Start working on your Study Guide Review (packet you picked up front)until everyone is finished

MAKE SURE YOU TURN IN YOUR 3 TOPICS FOR THE HONORS PROJECT INTO THE BIN!

TEMPERATURE CONVERSIONS

Two temperature systems used: oC (Celcius scale) K (Kelvin scale)

Reference Tables: K = oC + 273 The Kelvin Scale can NEVER go below zero. Absolute zero (0 Kelvin) is when all particles stop

moving.

EXAMPLES

0 K = _______ oC

1538 oC = _______ K

5778 K = _________ oC

0 - 273 = -273

-273

1538 + 273 = 1811

1811

5778 - 273 = 5505

5505

WARM UP-PRACTICE FOR YOUR QUIZ TODAY!**

Convert1.) 9.6 m to km2.) 68.7 µl to ml3.) 20.5 oC to K4.) 400K to oC

WARM UP FOR TUESDAY, SEPTEMBER 2ND

1. Silver has a density of 10.5 g/cm3. What is the mass of 5 cm3 of silver?

2. What word is the definition below:b. Closeness to true valuec. Narrowness of range of measuremnetsd. Amount of space an object takes upe. The quantity of matter an object containsf. Lowest point on the Kelvin scaleg. SI unit for Temperature

3.) Convert: (Remember K= 273+ oC )a) 20.5 oC to Kb) 400K to oC

4) What is 660 nm expressed in cm?((1 x10 9 nm = 1 meter) (1 meter = 100 cm) )

DENSITY

DENSITY

Density: a ratio of the mass of a substance to the volume

“the number of particles per square inch”

d = m V

Units Mass (m): grams (g)

Remember: Mass is the amount of matter in an object! Volume (V): cm3 (for solids) or mL (for liquids/gases)

Remember: Volume is the amount of space an object takes up.

Density (d): g/cm3, g/mL, or g/L

RELATIVE DENSITY OF STATES OF MATTER

GENERAL TREND:In order from most dense to least dense:solid, liquid, gas

Exception: Water is most dense at 4oC (liquid).

DENSITY

What is the density of an object that has a mass of 47 g. and a volume of 3.7 mL?

d = ? m = ? V = ?

What is the density of an object that has a mass of 47 g. and a volume of 3.7 mL?

d = ? m = 47 g V = 3.7 mL d = m/V

What is the density of an object that has a mass of 47 g. and a volume of 3.7 mL?

d = ? m = 47 g V = 3.7 mL d = m/V = 47/3.7 = 12.7 g/mL

DENSITY

What is the mass of a sample of aluminum that has a density of 2.5 and a volume of 34 mL?

d = ? m = ? V = ?

DENSITY

What is the mass of a sample of aluminum that has a density of 2.5 and a volume of 34 mL?

d = 2.5 g/mL m = ? V = 34 mL d = m/V

DENSITY

What is the mass of a sample of aluminum that has a density of 2.5 and a volume of 34 mL?

d = 2.5 g/mL m = ? V = 34 mL d = m/V m = dV

What is the mass of a sample of aluminum that has a density of 2.5 and a volume of 34 mL?

d = 2.5 g/mL m = ? V = 34 mL d = m/V m = dV 2.5 X 34 = 85 g