1. Block 3 & 4 Dalton’s Atomic Theory & Rounding

2. Warm-Up Pick up handouts & put away cell phones! Finish collecting the lab data. WEAR YOUR LAB GOGGLES! If you’re done start working on your conclusion.

3. Warm-up Pick up handouts & put away cell phones! On a sheet of paper under the warm-up section of your binder answer the following in complete sentences! Title: Theory of the Atom The first idea of the atom was brought about in 400 BC. Write an entry to the Roman Philosophers Committee on your theory of the atom.

4. Instrumentation & Measurement The more divisions of measurement the more EXACT we can be. The more decimals (or significant figures) the more exact a measurement is When is it important to have exact measurements?

5. How can we increase precision? Increasing the numbers of significant digits! Significant digit- all numbers in a measurement plus an extra for estimation. 6.63 mL 6.60 mL

6. Take Away Accuracy- how close a measured value is to an accepted value Precision- how close a series of measurements are to one another Practice: The known mass of Cobalt is 58.93 g/mol 58.9, 58.92, 59.0 50, 51, 45 62, 62.1, 62.0 Not accurate or precise Precise but not Accurate Both accurate & precise

7. Learning Check On a quarter sheet of paper write your name & period Title: Learning Check- METRIC Answer the following on your own 1.What instrument do we use to measure volume? 2.Write BOTH conversion factors for how many mm in a cm 3.______ Hg in 43.2 cg

8. ATOMIC THEORY FOLDABLE With the paper horizontal, fold two flaps of equal size inward Vertically fold paper into thirds. Open back up. Cut along the horizontal folds on the FRONT FLAPS ONLY

9. Roots of Atomic Theory Democritus 1 st proposed idea matter was no infinitely divisible Matter made of particles called atomos Atoms cannot be created, destroyed, or further divided Different atoms have different sizes and shapes Aristotle Empty space cannot exist Matter is made of earth, fire, and water

10. Atomic Theory Postulates It took 2,000 years to disprove Aristotle’s idea of nature. Postulate- a thing suggested or assumed as true, existent, or fact as a basis for reasoning, discussion, or belief Revise your warm-up idea or expand it based on the previous philosopher’s concepts.

11. John Dalton Sept 6 th 1766 – July 27 th 1844 First job age 10 Became a teacher at 12 Proficient in Latin by 14 Meteorology, Color Blindness, & Hiking Atomic Theory from studying gasses in 1803

12. All matter consists of a large number of tiny particles Matter Anything that has mass and takes up space Atom smallest particle of an element that retains the properties of the element

13. Atoms of an element are unique, indestructible, and indivisible Element- pure substance that cannot be broken down into simpler substances Each element has its own characteristics Atoms cannot destroyed or divided Smallest unit of matter

14. Atoms of a given element are identical in size, mass, and chemical properties Mass measure that reflects the amount of matter Chemical property ability or inability of a substance to combine with or change into one or more new substances

15. Chemical rxn involve separating, combining, or rearranging of atoms Atoms are neither created, destroyed, divided into parts, or converted into atoms of another element Chemical reaction (rxn) Process by which the atoms of one or more substances are rearranged to form different substances Indicated by change in temperature, color, odor, and physical state

16. Block 4 Phones away! I’m going to make sure there are 4 in every box! Turn in your metric one step worksheet & work to the black trays WARM-UP: On page 11 of your packet, complete the chart on Dalton’s Postulates as best you can. Try not to use your foldable!

17. Homework Content Learning Sapling Due Thurs 11:00 pm Content Quiz Next Block! Pg 11- Review Dalton’s Postulates #1-5 Dalton’s Postulates Rounding Numbers Metric One-Step Conversions

18. Language of Chemistry (LoC) List 1 x 2 The “2” is a subscript (s) solid. written after a chemical formula x 2 The “2” is a superscript ( l ) liquid. written after a chemical formula 2x The “2” is a coefficient (g) gas. written after a chemical formula → “yield”; shows a chemical reaction took place ( aq ) aqueous. written after the formula for a chemical dissolved in water. Chemical formula A 2 B, element symbols and subscripts Chemical equation 2A + B → A 2 B, chemical formulas, a yield sign, and coefficients (usually)

19. Element Quiz Remediation On the back of your quiz write the elements you got wrong 3 times each Name, Symbol, Name, Symbol, Name, Symbol IN A STRAIGHT LINE We always go by the spelling on the periodic table

20. TRADE & GRADE HMWK DO NOT grade your own paper. Write you name NEATLY on the right side of the page IF I find a mistake or you “grade nicely” not only will I regrade that person’s paper, but I’ll take the same points off your paper!

21. ROUNDING NUMBERS!

22. Packet Pg 4

23. Classifying Matter Using your notes & the textbook, define the three types of matter discussed in Dalton’s atomic theory on PG 11 of your packet Element Compound Mixture

24. Element Vs. Compound Elements are PURE SUBSTANCES found on the periodic table Compounds are two or more elements chemically bonded together

25. Diatomic Molecules Two of the same element bonded together is called a diatomic Element They are unstable being alone and must bond to themselves Br I N Cl H O F

26. Mixtures Two or more different substances that are not chemically combined and can be separated through physical means Heterogeneous mixtures- does not have uniform composition; can see different substances Homogeneous mixtures- uniform composition and a single phase; also called a solution

27. Let’s Practice Pg 13

28. LAB ACTIVITY You will find samples at each lab station You must do each of the following for every sample: Label by Table Number Write a short qualitative description Determine if it is a element, compound, or mixture Total of 12 Samples! There can be more than 1 think in each container

29. In your groups Look at the labels I’ve handed you and the descriptions you made with a partner What table(s) would you place your description at? Have one person at your table go place your labels next to the sample you believe it is

30. Homework Content Learning Sapling Due Thurs 11:00 pm Content Quiz Next Block! Pg 11- Review Dalton’s Postulates #1-5 Dalton’s Postulates Rounding Numbers Metric One-Step Conversions

31. Metric REVIEW

32. SHOWDOWN The Captain of your team is the person with the next birthday. You will write your answer on the board and keep it to yourself. Once everyone has had a chance to answer your captain will say “showdown” Everyone should compare answers. Talk about any differences and come to a conclusion. If you get the question correct you get a point. Captians keep tabs on the points!

33. Write the conversion fraction for how many centigrams in a gram.

34. What is the conversion factor for how many millimeters are in a meter

35. Conversion Factor for kiloliters in a liter

36. How many cg is 56.7 g SHOW YOUR WORK

37. If the next town is 96 km away how far do I have to drive in meters? Show all work

38. A fat cat masses 23,004 mg. how fat is the cat in g?

39. How many sigfigs did the mass of the fat cat have? 23,004 mg

40. What is the estimated digit for a volume reading of 56.89 mL?

41. Draw the instrument used to take this reading. BE SURE to mark the proper measurement lines!

42. If a flame burned for 450 milliseconds, how fast did it burn in Dekaseconds? Make sure you go to the base unit! (TWO STEP CONVERSION!!)