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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

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Chemistry 212 - Course Outline

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  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

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