2. Chemistry 103 Instructor: Dr. David W. Hatchett Lecture 1

3. OUTLINE Introduction to Course What is Chemistry? –Matter defined –Physical vs. Chemical Historical Perspectives The Scientific Method The Periodic Table

4. Outline Mathematics of Chemistry (Measurements) –Units –Significant Figures (Sig Figs) –Calculations & Sig Figs –Scientific Notation –Dimensional Analysis

5. Course Introduction Dr. David W. Hatchett Office CHE 213 Office Hours: 1:30 – 3:00 pm daily, or by appointment. E-mail: david.hatchett@unlv.edudavid.hatchett@unlv.edu Phone: 895-3509

6. Introduction to Course Purpose of Course

7. Introduction to Course Academic Success Center http://academicsuccess.unlv.edu/

8. Introduction to Course Course Resources Website

9. Web Lectures and homework Website (downloadable materials.) http://sciences.unlv.edu/Chemistry/Hatchett/ Weblectures Syllabus Homework

10. Introduction to Course Homework Quizzes Three Exams (last one comprehensive)

11. Introduction to Course Purpose of Course Academic Success Grading

12. Grading Scale GRADING: This course is graded on a letter grade basis only (no S/F grade). Your final grade will be based on three exams (300 points) and quizzes (50 points). The following grading scale will be used: A 100 – 90% B 89-80% C 79-70% D 69-60% F 56-0% –TOTAL: 350 points; percentage = [(your points)/350] x 100

13. Chemistry Success Complete Homework Seek Help during office hours Form study groups Don’t become overly confident with early material. Don’t cram before an exam.

14. The “good and evil” of chemistry

15. PhysicsChemistryBiology Scientific Overlap Physical Analytical Inorganic Organic Biochemistry

16. What is Chemistry? Chemistry is the study of Matter.

17. What is Matter? Matter is anything that has mass and takes up space.

18. Matter is anything that has mass and takes up space.

19. Matter has both physical and chemical properties

20. Physical Properties Physical properties are: Characteristics observed or measured without changing the identify of a substance. Shape, physical state, odor, boiling and freezing points, density, and color of that substance.

21. States of Matter All substances known as matter exist in one of three forms or states: Solids Have definite volumes and shapes Liquids Have definite volumes, but take the shapes of containers Gases Have no definite volumes or shapes Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

22. Physical Properties of Copper Copper has physical properties: Reddish-orange Very shiny Excellent conductor of heat and electricity Solid at 25  C Melting point 1083  C Boiling point 2567  C Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

23. Chemical Properties Chemical properties describe the ability of a substance To interact with other substances To change into a new substance Example: Iron has the ability to form rust when exposed to oxygen. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

24. Chemistry 103 This course serves as introduction into the world of chemistry, and includes both chemical and physical processes.

25. Historical Perspective Ancient Greeks and the 4 basic elements:

26. Historical Perspective Ancient Greeks and the 4 basic elements: Air,

27. Historical Perspective Ancient Greeks and the 4 basic elements: Fire,

28. Historical Perspective Ancient Greeks and the 4 basic elements: Water

29. Historical Perspective Ancient Greeks and the 4 basic elements: & Earth.

30. Historical Perspective Ancient Greeks and the 4 basic elements: Air, Fire, Water & Earth.

31. Historical Perspectives Alchemists Attempted to turn base metals into gold Attempted to find the “Exilir of Life”

32. Scientific Method The scientific method is the process used by scientists to explain observations in nature. Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

33. Scientific Method The scientific method involves: Making Observations Writing a Hypothesis Doing Experiments Proposing a Theory Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

34. Summary of the Scientific Method Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

35. Periodic Table Primary resource for a chemist as well as other scientists. Lists all the known elements in a “periodic way” Element - a substance that can not be broken down into simpler substances by chemical means.

36. Periodic Table Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings

37. Symbols for the Elements H O Ag Au Hg He Na

38. Symbols for the Elements HHydrogen OOxygen AgSilver AuGold HgMercury HeHelium NaSodium

39. Chemical Progression Atoms ---> Compounds ---> Chemical Reactions

40. Measured vs Exact numbers

41. Scientists make many kinds of measurements –The determination of the dimensions, capacity, quantity or extent of something –Length, Mass, Volume, Density All measurements are made relative to a standard All measurements have uncertainty Units and Measurements

42. Systems of Measurement English System –Common measurements –Pints, quarts, gallons, miles, etc. Metric System –Units in the metric system consist of a base unit plus a prefix.

43. Metric Base Units

44. Exact (Defined) and Inexact (Measured) Numbers Exact numbers –Have no uncertainty associated with them –They are known exactly because they are defined or counted –Example: 12 inches = 1 foot Measured numbers –Have some uncertainty associated with them –Example: all measurements

45. Accuracy vs. Precision Accuracy How closely a measurement comes to the true, accepted value Precision How closely measurements of the same quantities come to each other

46. Significant Figures Are the digits in any measurement known with certainty, plus one digit that is uncertain. Measured numbers convey *Magnitude *Units *Precision