2. Chemistry is the study of matter and the transformations it can undergo…

3. Matter is anything that has MASS and takes up SPACE.

4. Basic Safety Rules Use common sense. No unauthorized experiments. No horseplay. Handle chemicals/glassware with respect.

5. Safety Features of the Lab safety shower fire blanket fire extinguisher eye wash fume hood circuit breaker switch

6. Government Regulation The government regulates chemicals to protect the… OSHA worker FDA USDA FAA CPSC consumer EPA environment

7. Chemical Exposure a one-time exposure causes damage acute exposurechronic exposure damage occurs after repeated exposure

8. Toxicity Which is more toxic? Chemical A: LD 50 = 3.2 mg/kg Chemical B: LD 50 = 48 mg/kg Chemical A is more toxic because less of it proves fatal to half of a given population.

9. The Functions of Science pure scienceapplied science the search for knowledge; facts using knowledge in a practical way

10. Fundamental Properties of Models A model does not equal reality. Models are oversimplifications, and are therefore often wrong. Models become more complicated as they age. We must understand the underlying assumptions in a model so that we don’t misuse it.

11. Using the scientific method requires that one be a good observer. observationinference involves a judgment or assumption uses the five senses

12. Data Observations are also called data. There are two types of data. qualitative dataquantitative data descriptions; measurements; no numbersmust have numbers and UNITS

13. Scientific Law vs. Scientific Theory Law of Gravity A theory tries to explain why or how something happens. A law states what happens. Theory of Gravity Atomic Theory Collision Theory of Reactions

14. Experiments Law – A verbal or mathematical description of a phenomenon that allows for general predictions – Describes what happens and not why – Unlikely to change greatly over time unless a major experimental error is discovered Theory – Attempts to explain why nature behaves as it does – Is incomplete and imperfect, evolving with time to explain new facts as they are discovered Copyright 2007 Pearson Benjamin Cummings. All rights reserved.

15. Areas of Chemistry organic physical inorganic biochemistry everything except carbon e.g., compounds containing metals the study of carbon- containing compounds measuring physical properties of substances e.g., the melting point of gold the chemistry of living things

16. Graphs Line Graph –Used to show trends or continuous change Bar Graph –Used to display information collected by counting Pie Graph –Used to show how some fixed quantity is broken down into parts

17. The International System of Units Lengthmeter m Masskilogram kg Timesecond s Amount of substancemole mol Thermodynamic temperatureKelvin K Electric currentamperes amps Luminous intensitycandela cd QuantityNameSymbol Dorin, Demmin, Gabel, Chemistry The Study of Matter, 3 rd Edition, 1990, page 16

18. Derived Units Commonly Used in Chemistry Areasquare meter m 2 Volumecubic meter m 3 Forcenewton N Pressurepascal Pa Energyjoule J Powerwatt W Voltagevolt V Frequencyhertz Hz Electric chargecoulomb C Quantity Name Symbol

19. Area and Volume: Derived Units Area = length x width = 5.0 m x 3.0 m = 15 ( m x m) = 15 m 2 Volume = length x width x height = 5.0 m x 3.0 m x 4.0 m = 60 ( m x m x m) = 60 m 3

20. Prefixes in the SI System Power of 10 for Prefix SymbolMeaning Scientific Notation _______________________________________________________________________ mega-M 1,000,00010 6 kilo-k 1,00010 3 deci-d 0.110 -1 centi-c 0.0110 -2 milli-m 0.00110 -3 micro-  0.00000110 -6 nano-n 0.00000000110 -9 The Commonly Used Prefixes in the SI System Zumdahl, Zumdahl, DeCoste, World of Chemistry  2002, page 118

21. Accuracy vs. Precision Random errors: reduce precision Good accuracy Good precision Poor accuracy Good precision Poor accuracy Poor precision Systematic errors: reduce accuracy (person)(instrument)

22. Precision Accuracy  reproducibility  check by repeating measurements  poor precision results from poor technique  correctness  check by using a different method  poor accuracy results from procedural or equipment flaws.

23. SI Prefixes kilo-1000 deci- 1 / 10 centi- 1 / 100 milli- 1 / 1000 Also know… 1 mL = 1 cm 3 and 1 L = 1 dm 3

24. Practice Measuring 4.5 cm 4.54 cm 3.0 cm Timberlake, Chemistry 7 th Edition, page 7 cm 0 12345 0 12345 0 12345

25. Implied Range of Uncertainty 5 64 3 Implied range of uncertainty in a measurement reported as 5 cm. 5 64 3 Implied range of uncertainty in a measurement reported as 5.0 cm. Dorin, Demmin, Gabel, Chemistry The Study of Matter 3rd Edition, page 32 5 64 3 Implied range of uncertainty in a measurement reported as 5.00 cm.

26. 750 740 760 Here is a final example, with the vernier at yet another position. The pointer points to a value that is obviously greater than 751.5 and also less than 752.0. Looking for divisions on the vernier that match a division on the scale, the 8 line matches fairly closely. So the reading is about 751.8. In fact, the 8 line on the vernier appears to be a little bit above the corresponding line on the scale. The 8 line on the vernier is clearly somewhat below the corresponding line of the scale. So with sharp eyes one might report this reading as 751.82 ± 0.02. This "reading error" of ± 0.02 is probably the correct error of precision to specify for all measurements done with this apparatus. 5 0 10 http://www.upscale.utoronto.ca/PVB/Harrison/Vernier/Vernier.html

27. How to Read a Thermometer (Celcius) 10 5 0 4.0 o C 10 5 0 8.3 o C 100 50 0 64 o C 5 0 3.5 o C

28. 0oC0oC 10 o C 20 o C 30 o C 40 o C 50 o C 60 o C 0oC0oC 1oC1oC 2oC2oC 3oC3oC 4oC4oC 5oC5oC 6oC6oC 0oC0oC 5oC5oC 10 o C 15 o C 20 o C 25 o C 0oC0oC 20 o C 40 o C 60 o C 80 o C 100 o C 0oC0oC 20 o C 40 o C 60 o C 80 o C 100 o C Record the Temperature (Celcius) A B C D E 30.0 o C 3.00 o C19.0 o C 48 o C 60. o C

29. Rules for Counting Significant Figures 1. Nonzero integers always count as significant figures. 2. Zeros: There are three classes of zeroes. a.Leading zeroes precede all the nonzero digits and DO NOT count as significant figures. Example: 0.0025 has ____ significant figures. b.Captive zeroes are zeroes between nonzero numbers. These always count as significant figures. Example: 1.008 has ____ significant figures. c.Trailing zeroes are zeroes at the right end of the number. Trailing zeroes are only significant if the number contains a decimal point. Example: 1.00 x 10 2 has ____ significant figures. Trailing zeroes are not significant if the number does not contain a decimal point. Example: 100 has ____ significant figure. 3.Exact numbers, which can arise from counting or definitions such as 1 in = 2.54 cm, never limit the number of significant figures in a calculation. 2 4 3 1 Ohn-Sabatello, Morlan, Knoespel, Fast Track to a 5 Preparing for the AP Chemistry Examination 2006, page 53

30. Significant figures: Rules for zeros Leading zeros are not significant. Captive zeros are significant. Trailing zeros are significant. Leading zero Captive zero Trailing zero 0.421 4012 114.20 – three significant figures – four significant figures – five significant figures

31. Significant Figures Number of QuantityCertainUncertainSignificant DigitsDigitsFigures 14.379 g1 4 3 7 9 (thousandths) 5 6.02 mL6 0 2 (hundredths) 3 120.580 m1 2 0 5 8 0 (thousandths) 6 7.5 g7 5 (tenths) 2 0.037 g3 7 (thousandths) 2 0.0370 g3 7 0 (ten-thousandths) 3 *The position of the decimal point has nothing to do with the number of significant figures. Ralph A. Burns, Fundamentals of Chemistry 1999, page 52

32. ___ BAH TR x = Basic Algebra Solve for x. ___ x BA = TR H ___ BAH = xTR One way to solve this is to cross-multiply. BAH = xTR Then, divide both sides by TR. The answer is… 1 TR () ___1 TR () ___

33. Solve for T 2, where… P 1 = 1.08 atm P 2 = 0.86 atm V 1 = 3.22 L V 2 = 1.43 L T 1 = 373 K P 1 V 1 T 2 = P 2 V 2 T 1 ____ T1T1 P1V1P1V1 = P2V2P2V2 T2T2 1 P1V1P1V1 () 1 P1V1P1V1 () T 2 = P1V1P1V1 ______ P2V2T1P2V2T1 130 T 2 = (1.08 atm)(3.22 L) _____________________ (0.85 atm)(1.43 L)(373 K) = K

34. Scientific Method A step by step process where a scientist investigates a question by observing and performing experiments. Step 1 - State the problem or pose a question Step 2 - Gather information (has someone already investigated this?) Step 3 - Form a hypothesis -- a possible explanation or answer

35. Step 4 - Test the hypothesis with an experiment Experiments have 2 variables Independent variable - what you change Responding variable (dependent) - what you measure If you want to test the affect of fertilizer, you would add fertilizer to a plant (independent variable) and measure how the plant grows (responding variable) A control is something you do nothing to, used to compare your results you will also have a plant that receives no fertilizer

36. Step 5 - Analyze data Organize data into charts or graphs that can be read by others Step 6 - Draw Conclusions Determine if hypothesis is supported or rejected If hypothesis is not supported - modify hypothesis If hypothesis is supported - repeat experiment

37. Scientific Method in Action 1. What is the best material for insulation? Question. 2. Investigate materials (wool, down, leather) 3. Form a hypothesis 4. Design and conduct experiment. 5. Analyze data 6. Draw conclusions

38. Does your grade depend on how much time you spend on your work?

39. –The dependent variable depends on other factors (how much you studied, effort, etc.)

40. Does your grade depend on how much time you spend on your work? –The dependent variable depends on other factors (how much you studied, effort, etc.) –Independent variable is the one you have control over (how much you studied).

41. Does your grade depend on how much time you spend on your work? –The dependent variable depends on other factors (how much you studied, effort, etc.) –Independent variable is the one you have control over (how much you studied). You have control over your grades.

42. Variable: Changing quantity of something. –-

43. Variable: Changing quantity of something. –-

44. Variable: Changing quantity of something. –-

45. Independent: (Change) The variable you have control over, what you can choose and manipulate.

48. Dependent: (Observe) What you measure in the experiment and what is affected during the experiment.

49. Control: (Same) Quantities that a scientist wants to remain constant so it a fair test.

52. Everything is exactly the same except for the independent variable

53. Pick A Question and Design an Experiment 1. Will human urine repel sharks? 2. Does the color red make lizards more aggressive? 3. Will fish grow larger if placed in a larger tank? 4. Does exercise reduce your risk of heart attack? 5. Does aspirin keep cut flowers fresh longer?