Chemistry Class Schedule and Rules

1. Top left of the room (my desk) Bench Space Back of the room by the table

2. Top left of the room (my desk) Bench Space Back of the room by the table

3. Chemistry with Dr. S • Grab all the materials on the back table • Return the “welcome to chemistry” to the front when completed This won’t be you

4. Chemistry Dr. S

5. 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

6. Materials: • Binder—3” 3 ring binder • Notebook paper • Pens & Pencils • Notecards • Highlighter • Box of tissues, hand sanitizer, etc. For real I need these

7. Classroom Rules • I am king of this classroom • Respect yourself 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 – HW is due at the beginning of class • Participate in class • Follow the KGHS Code of Conduct

8. What is Chemistry? • The study of matter and its changes. • Matter is anything that has mass and volume (takes up space).

9. Who are Some Scientists??? Mendeleev Newton “Doc” Back to the future Einstein

10. 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.

11. BYOD • When I say so, it is allowed, if I have not EXPLICIDLY told you- you may not use it, it may not be out…. • If I say you are allowed to use it you may select music, and put the phone down 1st Time = warning 2nd Time = your device and everyone else’s device will be taken from you 3rd & subsequent Time = device taken (kept) & referral

12. Grading Policy • 70 % Tests • 15 % Lab Work & Activities • 15 % Graded Homework & Classwork, Card Quizzes, Warm-Ups etc.

13. 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

14. 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 complete • 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

15. 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. .

16. 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. freezing point condensing point GAS SOLID melting point boiling point LIQUID

17. 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.

18. 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

19. Uncertainty Notes

20. 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)

21. 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

24. Definitions Accuracy and Precision …sound the same thing… …is there a difference??

25. _____ precision _____ accuracy ____ precision ____ accuracy _____ precision _____ accuracy • Precision = How close several measurements are to each other. • Measure of reproducibilityof measurements • Accuracy = How close a measurement is to the actual or true value. • Measure of correctness of measurements % Error = │accepted - experimental│ X 100 accepted

26. 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.

27. A precise instrument gives a consistent reading when it is used repeatedly for the same measurements. A B For example A beaker is weighed on A, 3 times: The readings are: 73 g, 77 g, 71 g It 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.

28. 0 true value 0 0 Accuracycompared withPrecision Precise (grouped) but not accurate. Accurate (the mean) but not precise. Accurate and Precise.

30. Sig Figs Intro Video • https://www.khanacademy.org/math/pre-algebra/decimals-pre-alg/sig-figs-pre-alg/v/significant-figures

31. 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.

32. 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.

33. More Sig Fig Notes • If a number is greater than one and no decimal point is written, count only the non-zero numbers and zerosin-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.

35. 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:

36. Rules for Addition and Subtraction 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.

37. 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

38. Rules for Multiplication and Division 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.

39. Sig Fig Examples • 100.0 g X 1.000 cal/gC 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/gC X 28.6 C = 5720 = 6000

40. 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 =

42. 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?

43. Scientific Notation Notes • Complete the Daily Quiz from the front – turn in to me • TURN IN HOMEWORK

44. 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:

45. 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

46. 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

47. 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

48. 8-26-15 • Get out a piece of paper and answer the following: This probably wont work as a pick up line

50. BLK 1: 32.1 % Blk 2: 33.8%