1 / 32

Chemistry 212 - Course Outline

Chemistry 212 - Course Outline. Grade Distrn. The REQUIRED textbook for this course is:. Author/Title: Brown/LeMay/Bursten/Murphy/Woodward, “Chemistry, The Central Science”. 2012. Course/Section: Principles of Chemistry I, 212 Sec’s 1,2,3 Professor: Dr. C.B. William Ng

fairly
Télécharger la présentation

Chemistry 212 - Course Outline

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemistry 212 - Course Outline Grade Distrn

  2. The REQUIREDtextbook for this course is: Author/Title: Brown/LeMay/Bursten/Murphy/Woodward, “Chemistry, The Central Science”. 2012. Course/Section: Principles of Chemistry I, 212 Sec’s 1,2,3 Professor: Dr. C.B. William Ng Why you NEED this text: RYou will be TESTED from this textbook RReading assignments, Practice problems ROnline Assignments (5% course total) Ng-Website

  3. Study of Chemistry Composition Structure Properties Interactions Physical Sciences Life Sciences Macroscopic Microscopic cold hot HC

  4. Lab To Do’s List • Complete Individual Pre-lab (Mass/Volume expt, page 16) • Read Safety Rules, Print/Sign/Date page 3. • Safety Goggles (Z87.1), available for sale next week, $10 or $5. • Proper lab clothing: No shorts, No sandals. • Formation of lab groups of three. • Read “Mass and Volume Measurements” experiment.

  5. Introduction: Basic Principles of Chemistry [Ch. 1]

  6. Law Theory Theory Modified Theory Tested by Further Experiments The Scientific Method Observations

  7. Winona State University Biochemistry Analytical Environmental Organic Chemistry Physical Chemistry Inorganic Chemistry Polymer Chemistry Chemical Education & Information Svingen Mann Reuter Lee Franz Engen Whaley Nalli Hein Chan Ng Zemke Nydegger Zemke Gilman Kopitzke Zemke Major Fields in Chemistry Lab. Specialist: Barb Keller Dept. Manager: Peggy Killian

  8. Basic SI Units

  9. Commonly Used Metric Prefixes

  10. Scientific Notation ± real ± integer

  11. Uncertainty in Measurement Uncertainty in Measurement • All scientific measures are subject to error. • These errors are reflected in the number of figures reported for the measurement. • These errors are also reflected in the observation that two successive measures of the same quantity are different. Precision and Accuracy • Measurements that are close to the “correct” value are accurate. • Measurements that are close to each other are precise.

  12. Uncertainty in Measurement Precision and Accuracy

  13. Rules of Significant Figures • Counting zeros • Rounding • Product/Quotient can have no more sig. Figs. Than numbers with the least sig. Figs. • Sum/Difference can have no more decimals than numbers with least decimals. • Keep at least one extra digit for intermediate calculations • Exact Numbers

  14. Dimensional Analysis Box #’s andClass/Random-ID#’s Dimensional Analysis • Method of calculation utilizing a knowledge of units • Conversion factors => simple ratios relating two units • Desired unit = given unit  (conversion factor) Test Etiquette

  15. Example-1 Convert 6,352x104 km to ? m (con. sci. notn.) 6.352x1010 m

  16. Example-2 Change 952 cg to ? ng (csn) 9.52x109ng

  17. Example-3 Convert 723 cm-2 to ? m-2 (csn) 7.23x106 m-2

  18. Example-4 Example #5: Speed Conversions

  19. Example-5 Example #5: Speed Conversions

  20. Units of Measurement Density • Used to characterize substances. • Defined as mass divided by volume: • Units: g/cm3 or g/mL . • Originally based on mass (the density was defined as the mass of 1.00 g of pure water). Test Etiquette

  21. Density Example • The sun is estimated to have a mass of 2x1036 kg . Assuming it to be a sphere of average radius 6.96x105 km , calculate the average density of the sun in units of g cm-3 . Mathcad Solution

  22. Density Calculations Mathcad Solution

  23. Bet. Cel. and Fehr. Temperature Conversions Between Celsius and Kelvin

  24. Introduction: Basic Principles of Chemistry [Ch. 1] Test Etiquette

More Related