1. Alchemy 2015

2. Good Morning! Please find the seat that matches the element you were given. On the back of the card you were given please write: Name Home Phone Number Book Number Fold the index card in half (lengthways). Make a name placard on the other side of your index card

3. Good Morning! In your spiral notebook create a title page (this is page 1): Alchemy: Atoms, Elements, & Compounds Now draw a picture of an atom & list at least 5 things you know about atoms.

4. Agenda - 6/18/12 The Tools of the Trade / Safety Scientific Method (Lycopodium Demo) Qualitative vs. Quantitative Observations (Dollar Demo) A Penny For Your Thoughts Whatsa Matter? Significant Figures Significant Figures Reading Significant Figures (Measuring) Activity All That Glitters

5. Tools of the Trade Matter is defined as anything that has mass and takes up space. Make a list of at least 4 tools or pieces of equipment you think a chemist might use in order to measure the mass and volume of some matter…. How do chemists study matter? What tools do they use when studying matter?

6. Scientific Method What is the scientific method? A systematic process for studying nature that involves observations, hypotheses, and experiments. Make observations State the problem collect data Formulate hypotheses Perform experiments

7. Observations Lycopodium Demo Draw the set-up (page 5) List all observations Methane Bubbles Draw the set-up (page 5) List all observations Divide observations into 3 categories (you choose) ~ page 4

8. The Scientific Method Observation Hypothesis Experiment LawTheory Prediction Experiment Theory modified as needed

9. A Penny for Your Thoughts Long ago, early scientists tried to turn ordinary things into gold. This pursuit was called alchemy and the people who engaged in alchemy were called alchemists. Do you think alchemists were successful in turning things to gold? Explain your thinking.

10. A Penny for Your Thoughts In your notebook answer the following question: Can we turn a penny into gold? Complete Teacher-directed Lab Activity Make a procedure/observation T-Chart and complete Answer question 2 & 3 in your Lab notebook.

11. Whatsa Matter? What do you think matter is? Name two things that are matter and two things that are not matter. Complete Whatsa Matter Activity on page 8 of your classwork notebook.

12. Matter Matter is anything that has mass and volume. Matter is anything that takes up space Matter is anything of substance in the known universe.

13. What is energy? Energy is the ability to do work Nuclear, mechanical, chemical, electrical, thermal Kinetic energy is the energy of motion Potential energy is the energy of position

14. Energy The ability of a system to do work or supply heat. Not considered to be matter because it does not take up space nor does it have mass.

15. Law of Conservation of Energy (1st Law of Thermodynamics) In any physical or chemical process, energy is neither created nor destroyed. The energy of the universe is constant. Energy is converted from one form to another. Study of Energy

16. Energy change is a State Function A property of a system that does not depend on the pathway.

17. energy (has ability to do work) Energy is Conserved!!! matter (has mass / takes up space) Everything in the Universe  physically separable  chemically separable / chemical reaction Draw the following in your Notebook:

18. Mass Communication Using a Balance Measuring volume Complete Mass Communication

19. Mass What types of units are used to measure mass? Weight? In science, mass commonly is measured in units of grams (g) or kilograms (kg) 1 kg = 1000 g How do you think mass and weight are different?

20. Volume What types of units are used to measure volume? In a laboratory, graduated cylinders are used to measure the volume of liquid. 1000 mL = 1 L There are several methods for measuring the volume of solids. 1 mL = 1 cm 3

21. Significant Figures Rules and Practice 123.45 0.0045 10200

22. Significant Figures?????

23. Significant Figures (Place sig fig reading on page 12 of CW Notebook) The significant figures in a measurement include all the digits that can be known precisely plus a last digit that must be estimated.

24. Significant Figure Activity You will need two different objects to measure. Your notebook, etc.

25. Significant Figures The Three Rules Addition and Subtraction Multiplication and Division

26. 1. Every nonzero digit in a recorded measurement is significant. Examples: 243, 87.9, and 714 all have 3 significant figures. Practice: How many sig figs are in the following numbers? 1.832 2.22.9 3.458,569,258

27. 2. Zeros A. Leading Zero’s….. are zeros that precede all of the nonzero digits. They never count as significant digits. Examples: 0.0071, 0.42, and 0.00000099 all have 2 significant figures. Practice: How many sig figs are in the following numbers? 1.0.00832 2.0.23 Beginningze ro’s

28. 2. Zeros B. Captive Zero’s….. are zero’s that fall between nonzero digits. Examples: 7003, 40.79, and 1.503 all have 4 significant figures. Practice: How many sig figs are in the following numbers? 1.8320 2.20.001 Middle Zero’s

29. 2. Zeros C. Trailing Zeros…... Are zeros at the right end of the number. They are significant only if the number is written with a decimal point. Examples: 43.00, 1.010, and 9.000 all have 4 significant figures. Practice: How many sig figs are in the following numbers? 1.2.00 2.8320 Ending Zeros

30. 3. Exact Numbers Often calculations involve numbers thata were not obtained using measuring devices but were measured by counting. 10 experiments, 3 apples, 8 molecules These numbers can be assumed to have an unlimited number of significant figures. Exact numbers can also arise from definitions. 1 inch = 2.54 cm

31. Assignment A How many significant figures do these measurements contain? 1) 123 2) 40506 3)0.123 4)4.5600 5)980000 6)980000. 7)0.07080 8) 456 9) 40006 10)0.023 11)4.8760

32. Addition and Subtraction In addition and subtraction, the answer can have no more digits to the right of the decimal point than are contained in the measurement with the least number of digits to the right of the decimal point.

33. Assignment E #1 7 9. 2

34. Assignment E #2: 7. 3 3

35. Assignment E #3: 1 1. 5 3

36. Assignment E #4: 1 7. 3

37. Assignment E #5: 2 9.

38. Multiplication and Division The answer must contain no more significant figures than the measurement with the least number of significant figures. The position of the decimal point is irrelevant.

39. Multiplication/Division 16) 123 x 40506 17)0.123 x 4.5600 18)980000 / 1.07080 19)980000. / 1.07080 20) 456 x 40006 x 0.023 21)4.8760 x 102000 22)102000. / 9.0600900 23)5.730 / 3.0 24)8765 x 0.00073 25)40.0007 x 3000 26)3000. x 0.010

40. Calculators w/ Scientific Notation When entering scientific notation in your calculator: Enter the 1 st Press the 2 nd Followed by the, Enter the appropriate exponent “E” means “x 10”

41. Homework Complete Significant Figures WS (moodle – odds only) Complete Measurement & Density HW Reading Resources Modern Chem: pp 29–38, 46-53 Read Sig Fig Reading from Moodle.