1. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 CHEMISTRY 101  Textbook: Zumdahl, 6 th Edition

2. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 2 Students Responsibilities 1.Read and Study every detail in textbook. 2.Use the CD-ROM and internet educational tools provided by Zumdahl and others. 3.Search for other sources of information: other textbooks and references, internet, etc. 4.Solve and submit homeworks on time. 5.Homeworks are NOT enough to get a good grade, students should solve all the problems they can and also old exams.

3. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 3 Instructor’s Role To summarize important points of each chapter. Give directions on how and where to find information. Solve typical problems and give quizzes during recitation. Answer your questions during office hours. In summary, I am a facilitator and NOT a teacher that will feed information in your brains. You are responsible now for your life.

4. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 4 Steps in the Scientific Method 1.Observations  quantitative  qualitative 2.Formulating hypotheses  possible explanation for the observation 3.Performing experiments  gathering new information to decide whether the hypothesis is valid whether the hypothesis is valid

5. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 5 Outcomes Over the Long-Term Theory (Model)  A set of tested hypotheses that give an overall explanation of some natural phenomenon. overall explanation of some natural phenomenon. Natural Law  The same observation applies to many different systems different systems  Example - Law of Conservation of Mass

6. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 6 Law and Theory A law summarizes what happens; A theory (model) is an attempt to explain why it happens.

7. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 7 Figure 1.4: The fundamental steps of the scientific method.

8. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 8 Figure 1.5: The various parts of the scientific method.

9. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 9 Nature of Measurement Measurement - quantitative observation consisting of 2 parts Part 1 - number Part 2 - scale (unit) Part 2 - scale (unit)Examples: 20 grams 6.63    Joule seconds

10. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 10 International System (le Système International) Based on metric system and units derived from metric system.

11. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 11 The Fundamental SI Units

12. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 12

13. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 13 Figure 1.6: Measurement of volume

14. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 14 Figure 1.7: Common types of laboratory equipment used to measure liquid volume.

15. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 15 Figure 1.8: An electronic analytical balance.

16. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 16 Uncertainty in Measurement A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty.

17. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 17 Figure 1.9: Measurement of volume using a buret. The volume is read at the bottom of the liquid curve (called the meniscus). 20.16ml 20.17ml 20.15ml 20.18ml ±0.01ml

18. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 18 Precision and Accuracy Accuracy refers to the agreement of a particular value with the true value. Precision refers to the degree of agreement among several elements of the same quantity.

19. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 19 Figure 1.10: The results of several dart throws show the difference between precise and accurate.

20. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 20 Types of Error Random Error (Indeterminate Error) - measurement has an equal probability of being high or low. Systematic Error (Determinate Error) - Occurs in the same direction each time (high or low), often resulting from poor technique.

21. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 21 Rules for Counting Significant Figures - Overview 1.Nonzero integers 2.Zeros  leading zeros  captive zeros  trailing zeros 3.Exact numbers

22. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 22 Rules for Counting Significant Figures - Details Nonzero integers always count as significant figures. 3456 has 4 sig figs.

23. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 23 Rules for Counting Significant Figures - DetailsZeros  Leading zeros do not count as significant figures. 0.0486 has 3 sig figs.

24. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 24 Rules for Counting Significant Figures - DetailsZeros  Captive zeros always count as  Captive zeros always count as significant figures. 16.07 has 4 sig figs.

25. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 25 Rules for Counting Significant Figures - DetailsZeros  Trailing zeros are significant only  Trailing zeros are significant only if the number contains a decimal point. 9.300 has 4 sig figs.

26. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 26 Rules for Counting Significant Figures - Details Exact numbers have an infinite number of significant figures. 1 inch = 2.54 cm, exactly

27. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 27 Rules for Significant Figures in Mathematical Operations Multiplication and Division: # sig figs in the result equals the number in the least precise measurement used in the calculation. 6.38  2.0 = 12.76  13 (2 sig figs)

28. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 28 Rules for Significant Figures in Mathematical Operations Addition and Subtraction: # sig figs in the result equals the number of decimal places in the least precise measurement. 6.8 + 11.934 = 22.4896  22.5 (3 sig figs)

29. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 29 Rules for Counting Significant Figures.

30. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 30 Dimensional Analysis Proper use of “unit factors” leads to proper units in your answer.

31. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 31

32. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 32 Temperature Celsius scale =   C Kelvin scale = K Fahrenheit scale =   F

33. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 33 Temperature

34. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 34 Figure 1.11: The three major temperature scales.

35. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 35 Figure 1.12: Normal body temperature on the Fahrenheit, Celsius, and Kelvin scales.

36. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 36 Density Density is the mass of substance per unit volume of the substance:

37. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 37 Matter: Anything occupying space and having mass.

38. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 38 Classification of Matter Three States of Matter: Solid: rigid - fixed volume and shape Liquid: definite volume but assumes the shape of its container Gas: no fixed volume or shape - assumes the shape of its container

39. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 39

40. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 40 Types of Mixtures Mixtures have variable composition. A homogeneous mixture is a solution (for example, vinegar) A heterogeneous mixture is, to the naked eye, clearly not uniform (for example, a bottle of ranch dressing)

41. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 41

42. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 42 Pure Substances Can be isolated by separation methods:  Chromatography  Filtration  Distillation

43. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 43 Figure 1.15a: Paper chromatography of ink. (a) A line of the mixture to be separated is placed at one end of a sheet of porous paper.

44. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 44 Figure 1.15b: Paper chromatograph y of ink. (b) The paper acts as a wick to draw up the liquid.

45. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 45 Figure 1.15c: Paper chromatography of ink. (c) The component with the weakest attraction for the paper travels faster than the components that cling to the paper.

46. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 46 Figure 1.14: Simple laboratory distillation apparatus.

47. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 47 Element: A substance that cannot be decomposed into simpler substances by chemical means. Compound: A substance with a constant composition that can be broken down into elements by chemical processes.

48. Copyright©2000 by Houghton Mifflin Company. All rights reserved. 48 Figure 1.16: The organization of matter.