Welcome Grab an info sheet from the front, and complete it. Return it to the front when completed This won’t be you.

Welcome

Grab an info sheet from the front, and complete it.

Return it to the front when completed

This won’t be you

Schedule

7:15 Student Release 7:25 Warning 7:30 – 9:00 First Block 9:05 – 10:35 Second Block 10:35 – 11:30 Flex Block 11:30 – 1:00 Third Block 1:05 – 2:35 Fourth Block 2:40 Busses Loaded

Materials:

Binder—3” 3 ring binder Notebook paper Pens & Pencils Notecards Highlighter Box of tissues, hand sanitizer, etc.

What is Chemistry?

The study of matter and its changes.

Matter is anything that has mass and volume (takes up space).

Who are Some Scientists???

Einstein

NewtonMendeleev

“Doc” Back to the future

Why Study Chemistry?

Learn fundamental physical models Develop problem solving skills Appreciate life’s little mysteries Prepare for college Get an advanced diploma*************** Be an informed citizen Satisfy your curiosity about the natural

world.

Classroom Rules

I am king of this classroom Respect themselves and other people Follow safety precautions in lab*

– *VIOLATION OF ANY PART OF THIS RULE CAN AFFECT YOUR GRADE AND WILL RESULT IN PERMANENT REMOVAL FROM LAB ACTIVITIES

Come to class on time Come to class prepared Participate in class Follow the KGHS Code of Conduct

Grading Policy

70 % Tests

15 % Lab Work & Activities

15 % Graded Homework & Classwork, Card Quizzes, Warm-Ups etc.

Late work & Make-up work

Assignment Sheet: Students receive a list of assignments at the beginning of each unit. This will list the daily activities, classwork, & homework.

Late Work: Late work will not be accepted unless complete: 75% if 1 day late, 50% if 2 days late, 25 % if 3 days late.

After 3 days I will NOT accept late work

Late work & Make-up work Con’t

Excused Absence: Students will use their assignment sheet, which lists classwork and homework, to identify any worksheets they need to retrieve from the folders/crates located in the front of the room.

Students are responsible for getting any notes they missed from another student.

Students will schedule a make-up time for tests and labs

– Make-up tests will generally be short answer & essay tests (not multiple chioce).

– I will not beg you to come take a test, it’s a 0 until you make it up

Daily Quizzes:

Quizzes that will be given at the beginning of class several times a week.

They cover the notes, assignments, and homework from the day or two before.

.

How to Succeed in Chemistry

Don’t miss class. Take good notes – many topics are covered differently in the text. Keep up with assignments (classwork, homework, reading, lab

reports). Expect to work hard and do chemistry every night. For many of

you, chemistry is the hardest class you take in high school. Complete all test reviews and study for tests. Keep your notebook in order so that you have what you need.

melting melting pointpoint

freezingfreezingpointpoint

GAS

condensingcondensingpointpoint

boilingboilingpointpointSOLID LIQUID

Lab Safety

Sign your lab safety contract.

Have a parent or guardian sign your safety contract.

Return the contract and student/parent info sheet to me.

Sad Panda

• Bad day?• 1 card per student• 1 card per semester

• What it is:• Homework pass • Get out of (moderate)

trouble card• Participation pass

• What it is not:• Get out of jail free card• Do what I want pass

• *I reserve the right to ignore any and all passes for any and all reasons at my discretion

Uncertainty Notes

Uncertainty in Measurement

Every measurement has some uncertainty due to errors in equipment and human error.

When making a measurement: Always read the instrument to the smallest scale marking and then estimate one digit. * Always read between the lines

If an uncertainty is not given (i.e. ± 0.1 mL), – Assume that the uncertainty is ± ½

the smallest increment. (Divide the smallest increment by 2)

Still Lost?

Bob reads his weight as closest to the 142-pound mark. – He knows his weight must be larger than 141.5

pounds (or else it would be closer to the 141-pound mark), but smaller than 142.5 pounds (or else it would be closer to the 143-pound mark). So Bob's weight must be:

weight = 142 +/- 0.5 pounds

Definitions Accuracy and Precision …sound the

same thing…

…is there a difference?

?

Precision = How close several measurements are to each other.– Measure of reproducibility of measurements

Accuracy = How close a measurement is to the actual or true value. – Measure of correctness of measurements

% Error = │accepted - experimental│ X 100

accepted_____ precision

_____ accuracy

_____ precision

_____ accuracy

____ precision

____ accuracy

Accuracy : In your experiments, you need to consider the accuracy of your measuring instrument.

•An expensive thermometer is likely to be more accurate than a cheap one. •It is also likely to be more sensitive. •It will give a result nearer to the true value.

For example

A

B

A beaker is weighed on A, 3 times:The readings are: 73 g, 77 g, 71 gIt is then weighed on B, 3 times:The readings are: 75 g, 73 g, 74 g

Balance B has better precision.Its readings are grouped closer together.

A precise instrument gives a consistent reading when it is used repeatedly for the same measurements.

Accuracy compared with Precision

0

truevalue

0

0

Precise (grouped) but not accurate.

Accurate (the mean) but not precise.

Accurate and Precise.

Sig Figs Intro Video

https://www.khanacademy.org/math/pre-algebra/decimals-pre-alg/sig-figs-pre-alg/v/significant-figures

Significant Figures

A significant figure is one which is known to be reasonably reliable.

Significant figures (or sig figs) are numbers that are actually measured.

How many numbers you have can tell you how exact a measurement is. For instance, knowing that a number is 4 inches is different from knowing that it is 3.999998 inches.

Sig Fig Rules

Count all non-zero numbers. EX: 1234 has four sig figs.

Count zeros that are in-between non-zero numbers.– Ex: 708 has three sig figs, 1.048 has four sig figs

If a number is less than one, count all the numbers after the first non-zero number, including that non-zero number. Do not count the zeros to the left of the first non-zero number.

– Ex: 0.00098 has two sig figs, 0.00009870 has four sig figs.

More Sig Fig Notes

If a number is greater than one and no decimal point is written, count only the non-zero numbers and zeros in-between non-zero numbers.

– Ex: 48000 has two sig figs, 408000 has three sig figs. If a number is greater than one and a decimal point is

written, count all numbers. – Ex: 9487.443 has seven sig figs, 1000.000 also has

seven

* EXACT Numbers, have an infinite number of significant figures. They are not measurements.

EX: 100 years in a century, # of people in a room, there are 500 sheets of paper in a ream.

NumberDigits to

countExample

Number of Significant

Digits

Nonzero digits

All *8341* 4

Leading Zeros

None 0.000*79* 2

Captive zeros

All *1200.00043* 9

Trailing Zeros

Only if decimal

point

*400.0* and *4*00

4 and 1

Scientific Notation

All *3.7* X 10-2 2

Rounding Sig Figs

When Multiplying and dividing. You are concerned with the number of sig figs

Multiply or divide the numbers– Count the total number of significant figures in

each number– Round your answer to the least number of sig. figs.

Example:

6.70 moles * 1.1 moles =7.37 = 7.4 moles (2 sig figs)

4000 moles/ 2.9 moles =1400

=1000 moles ( 1 sig fig)

Rules for Addition and Subtraction

Example 8

Y = 232.234 + 0.27 Find Y.Answer: Y = 232.50

NOTE: 232.234 has 3 decimal places and 0.27 has 2 decimal places. The least amount of decimal places is 2. Thus, the answer must be rounded to the 2nd decimal place (thousandth).

When adding or subtracting numbers, the end result should have the same amount of decimal places as the number with the least amount of decimal places. 

5.0 cm

+ 4.352 cm

9.352 cm

= cm

5.000 cm- 4.352 cm

0.648 cm

5.029 cm

- 4.3 cm

0.73 cm

= cm

404,000 cm

+ 10.0 cm

404,010.0cm

cm

Rounding Sig. Figs.

When adding or subtracting . Line up the decimal point Add or subtract the numbers Look at the given numbers and mark the sig. fig

farthest to the right. Round to the place of the sig fig farthest to the left. DO NOT LEAVE OFF IMPORTANT ZERO’s

Rules for Multiplication and Division

Example 9

Y = 28 x 47.3 Find YAnswer: Y = 1300

NOTE: 28 has 2 significant digits and 47.3 has 3 significant digits. The least amount of significant digits is 2. Thus, the answer must me rounded to 2 significant digits (which is done by keeping 2 significant digits and replacing the rest of the digits with insignificant zeroes).

When multiplying or dividing numbers, the end result should have the same amount of significant digits as the number with the least amount of significant digits. 

Sig Fig Examples

100.0 g X 1.000 cal/gC X 28.80 C =2880

44 + 13.4 + 87.40 = 144.8 = 145

21.6 mL + 43.57 mL - 1 mL =64.17 = 64.2

6.79 cm X 13.5 cm = 91.665 = 91.7

25.1 g ÷ 5.9 cm3 =4.254237288 = 4.3

43.2 dm X 3.00 cm3=129.6 = 130

3.14159 X 5.0 cm =15.70795 = 16

2.00 X 102 g X 1 cal/gC X 28.6 C = 5720 = 6000

Examples

1.034 X 1.549 = 1.601666 =

40.06 X 739.51 = 29624.7706 =

0.0000624 X 82.000 = 0.0051168 =

22 g + 14.3 g + 97.03 g = 133.33 g=

71.6 mL + 45.32 mL – 8 mL = 108.92 mL=

3.14159 X 4.0 = 12.56636 =

27.2 g ÷ 2.00 cm3 = 13.6 =

WHY SIG FIGS

You do not want to tell someone that a measurement was measured more specifically than it actually was. For example:

There are around 1000 students in this school. 3 new students just enrolled. How many student are there now?

Scientific Notation Notes

• Complete the Daily Quiz from the front

• When Finished get out your notes AND your homework packet

• Reminder: Tomorrow you need your book

Your test results

Block 2 Avg: 33.13%

Block 1 Avg: 29.76

Scientific Notation *For very large or very small numbers

Proper Scientific Notation is always in this form: _.___ X 10exponent

Put the decimal after the 1st nonzero #. Count the number of spaces between where you put the decimal

& where it was before. Moving to the Right: your exponent is + (Big #) Moving to the left, your exp. is - (Small #) Examples:

875,900,000 =

0.0008907 =

23.93 X 105 =

- 804 X 108 =

-0.0000289 = -6.022 X 10-6 = -3.93 X 108 =

Taking #’s out of Scientific Notation

Move the decimal– If the exp. is - , move decimal to left.– If the exp is +, move decimal to right.– EX: 6.022 X 10-6 = 0.000 006 022– EX: 3.93 X 108 = 393,000,000

Multiplying & Dividing in Sci. Not.

Multiplying: Multiply the #’s & add the exp.– EX: 4 X 105 * 2 X 108 = 8 X 1013

– EX: 1.2 X 104 X 4 X 10-9 = 4.8 X 10-5

Dividing: Divide the #’s & subtract the exp.– EX: 4 X 105 ÷ 2 X 108 = 2 X 10-3

– EX: 4 X 104 ÷ 2 X 10-9 = 2 X 1013

Adding & Subtracting in Sci. Not.

The exponents must be the same. Add or subtract the #’s. Keep the exponent

the same. EX: 1.2 X 105 + 2.7 X 105 = 3.9 X 105

1.2 X 105 + 2.7 X 103 (need to change 1) 1.2 X 105 + 0.027 X 105 = 1.227 X 105

2.3 X 10-9 - 2.3 X 10-7 (need to change 1) 0.023 X 10-7 - 2.3 X 10-7 = -2.277 X 10-7

9-3-14

DO NOT turn over the paper at your desk. Get out a pencil Sit Quietly

This probably wont work as a pick up line

Metric System

Standards of the past

People used to use parts of their body to determine the length of something.

The standard would be a part of the king’s anatomy.

The standard yard was the distance from the king’s nose to his outstretched arm

People would use their feet to measure distance

This is how the term foot came about.

Today the standard “foot” in the English system is

12 inches = 1 foot

Units of Measurement & The Metric System

The metric system is a universal system of measurement based on the number 10.

Mass & Weight are not the same thing Mass = measure of the quantity/amount of

matter Weight = measure of the force of gravity on

an objects mass. (changes when gravity changes)

Measurement

No human endeavor can be called science if it can not be demonstrated mathematically.

Leonardo da Vinci (1452 -1519)

The SI System

Le Systeme Internationale (SI) is a set of notations that are standard in science. Pg 73

Quantity SI Base Unit Symbol

Length meter m

Mass kilogram kg

Temperature kelvin commonly use Celcius

K

Time second s

Amount of Substance Mole mol

Volume(separate table in text)

dm3 commonly use Liter 1 cm3 = 1 mL

dm3

Metric Prefixes - used to adjust the size of base units

Prefix Symbol Meaning Conversion

giga G Billion (1 000 000 000 X) 109 b = 1 Gb

mega M Million (1 000 000 X) 106 b = 1 Mb

kilo k Thousand (1 000 X) * 1000 b = 1 kb

hecto H Hundred (100 X) 100 b = 1 Hb

deca D Ten (10 X) 10 b = 1 Db

Base Unit

deci d Tenth (1/10) 1 b = 10 db

centi c Hundredth (1/100) * 1 b = 100 cb

milli m Thousandth (1/1000) * 1 b = 1000 mb

micro Millionth (1/1 000 000) * 1 b = 106 b

nano n Billionth (1/1 000 000 000) * 1 b = 109 nb

pico p Trillionth (1/1 000 000 000 000) 1 b = 1012 pb

B = base unit = liters (L), meter (m), gram (g), Joule (J), calorie (cal), atmosphere (atm), pascal (Pa) etc.

Left

Simple Conversions

Move the decimal 1 space for each zero. If one wants to move from a smaller unit to

a larger unit move the decimal point to the left.

If one wants to move from a higher unit to a smaller unit move the decimal point to the right.

If your unit gets larger, your number gets smaller.

If your unit gets smaller, your number gets larger.

Examples:

23.5 m = ___________________________ cm 134.56 mm = ________________________m 98.43 L = ___________________________mL 34 g = ______________________________kg 32.5 L = ____________________________nL 456.3 g = ___________________________Mg 123.43 cg = _________________________Hg 3908.3 kL = _________________________mL 3859.839 mm = _______________________Mm

Dimensional Analysis/Factor Labeling/ Solving Problems Method

1. Read & determine what the ? is asking for.

2. Write a ? with the unit you are looking.

3. Write =

4. Write down information the problem gives you. The number with the unit. -If the problem gives you more than one pieces

of information write down the information that is not paired up with anything else.

5. Write a large ( )

6. On the bottom of the fraction sign, write the units of the given information. NO NUMBERS yet!!

7. Cross out units that match (cancel out) on the top and the bottom.

8. On the top of the fraction sign, write the units of the desired information. NO NUMBERS yet!!

-If you don’t have a relationship between what you are looking for and what you are given put the units of something you DO KNOW about on the top of the fraction sign. Continue until the units left match the unit/s you are looking for.

9. Put in the numbers that match the units you wrote.

10. Multiply and divide. Multiply by all of the #’s on top of the parenthesis and divide by the #’s on the bottom of the parenthesis.

11. Write out the answer WITH units, and sig figs.

Basic Format

? Desired Unit= Starting unit X XLinking Unit

Starting UnitDesired UnitLinking Unit

Desired Unit=

Examples

How many centimeters are in 3 inches? 2.54 cm = 1 in

How many millimeters are in 4 inches?

Convert 1.2 years to seconds.

Convert 89 kg to g.

More Solving Problems

How many g are in 101.3 Hg?

Convert 98 kg/mL to g/cm3.

If the density of hexane is 0.0068 g/ml, how

many liters are in 98 g of hexane?

Temperature

Degree of hotness or coldness of an object.– Heat always moves from hotter to colder.

Celsius - based on the freezing point of water (0ºC) & boiling point of water is 100ºC.

Kelvin – (absolute scale). Zero point is 0 K or -273ºC. ºC & K have the same size increments, but K starts lower.

ºC + 273 = K ; K – 273 = ºC (know these)

Fahrenheit (you do not need to memorize these formulas)

ºF = 1.8(ºC) + 32 ; ºC = (ºF -32)/1.8

The Three Major Temperature Scales

20F C

50.0 C F

20.0 F K

9-5-2014 Warm-up

Up front: NO NOTES

Basic Lab Safety Rules

MSDS (now the SDS)

Material Safety Data Sheet A Material Safety Data Sheet (MSDS) is designed to

provide both workers and emergency personnel with the proper procedures for handling or working with a particular substance.

– include physical data (melting point, boiling point, flash point etc.)

– toxicity, health effects, – first aid, reactivity, – storage, disposal,– protective equipment, and spill/leak procedures.

MSDS's vary in length depending on their format, content, and font size. We have seen them from 1 to 10 pages, with most being 2 to 4 pages.

The Scientific Method Question/Problem/Observation Hypothesis – an EDUCATED Guess proposed

reason for what is observed Experiment – To test hypothesis. Create a

controlled experiment with one experimental variable, constants, and controls. – Quantitative Data = a measurement which

gives definite, usually numeric results. – Qualitative Data = a measurement which

gives descriptive, nonnumeric results. Analyze Data – Create Graphs, Perform

calculations Etc. Conclusion – Compare experimental results

with hypothesis. Create a new hypothesis.

Observations Hypothesis Experiments Theory

Scientific Law

Law VS Theory

Theory = Thoroughly tested explanation of why experiments give certain results. Can not be proved, but it can be disproved. They give you a model that explains natural phenomena

Scientific Law = Concise statement that summarizes the results of a broad spectrum of observations and experiments. Laws describe phenomena, but do not attempt to explain it.

Example MSDS

Hazardous Materials Classification

Laboratory Notebooks

Small spiral or composition book. For each experiment – before you come to

class Write the

– Title – Purpose – Make data tables to collect data required for exp.

Writing a Laboratory Report

Grading Rubric – I give this to you Title page

Title

Name

Date Performed: 00/00/00

Date Due: 00/00/00

Purpose: Complete sentences. Brief statement about what you will accomplish – hope to learn.

Purpose: The purpose of this experiment is to become familiar with the measurement scale of a balance, graduated cylinder, and a thermometer. I will also familiarize myself with the scale of each piece of lab equipment and learn to read each scale as accurately as possible.

Data & Observations: – In the form of a table– Include all units– Label all columns & rows– Neatly rewrite what was written in lab notebook

Calculation & Questions: – Must be in a table

– You must show all calculation either in the table or on a separate piece of paper.

– Graphs or charts will also be attached to this section

Questions Answers

1.

Conclusion

MUST be in paragraph (¶) form. Compare the purpose of the experiment to

what you actually did (what did you accomplish? Was the purpose achieved?)

Use your data & calculations to support (explain) your findings.

Answer all questions specific to lab. Make a statement about what you learned

(new equipment, process, etc)

How to Label Assignments

At the top of the first page Name: ___________________ Date: ____________ Title of Assignment: __________________ Label each new section with the page

number from your text. Each new piece of paper needs your

name and page number at the top SHOW ALL WORK (no work = no credit)

EXAMPLE:

  Covey McConnell 2

  Chapter Assessment pg. 96

  63. a. second c. Kelvin

  b. meter d. kilogram

  65. a. 35.6 cm

  b. 0.98 m

  c. 11.5 in

  87. D of ethanol=m/V

 = 127 g/158 cm3 = 0.804g/cm3

1

  Covey McConnell

  9/10/05

  Measurement bookwork

  pg.19

  1. metric

  2. 3*4 = 12

  3. solid

  8. ruler

  pg.23

 12. 19.6 cm (1 m/2.54 cm) =

7.72 m

Notebooks /Portfolio (3-Ring)

It is your responsibility to have the materials you will need in class.

Table of Contents All notes, tables, diagrams, HW, CW, Worksheets, Labs,

Test Review Worksheets, Bookwork. Your notebook must be neat and orderly. Your notebook will be graded towards the end of each 6

week period and there will be occasional notebook check card quizzes.

All work needs to be completed and correct. All non-worksheet assignments need to be labeled

properly (name, date, title, book sections and pages). SEE EXAMPLE at front of room.