2. Chemistry 212 - Course Outline Grade Distrn

3. The REQUIRED textbook for this course is: Author/Title: Brown/LeMay/Bursten/Murphy/Woodward/ Stoltzfus, “Chemistry, The Central Science”. 13e, 2014. Course/Section: Principles of Chemistry I, 212 Sec’s 1,2,3 Professor: Dr. C.B. William Ng Why you NEED this text:  You will be TESTED from this textbook  Reading assignments, Practice problems  Online Assignments via MasteringChemistry (5% course total) Ng-Website

4. Study of Chemistry CompositionStructure PropertiesInteractions Life Sciences Physical Sciences Macroscopic Microscopic cold hot HC

5. Nitrogen Degree Celsius (  C ) Degree Fahrenheit (  F ) Degree Kelvin ( K ) Melting point-210-34663 Boiling point-200-32873

6. 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.

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

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

9. Major Fields in Chemistry Winona State University Biochemistry Physical Chemistry Ng Zemke Nydegger, M Organic Chemistry Inorganic Chemistry Polymer Chemistry Chemical Education & Information Analytical Environmental Nalli Hein Chan Sichula Franz Engen Whaley Mann Lee Mauser West Zemke Gilman Nydegger, I KopitzkeZemke Dept. Manager: Peggy Killian Lab. Specialist: Barb Keller

10. Basic SI Units

11. Commonly Used Metric Prefixes

12. Scientific Notation ± integer± real

16. 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. Uncertainty in Measurement

17. Precision and Accuracy Uncertainty in Measurement

18. 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

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

23. Example-1 Convert 6,352x10 4 km to ? m (con. sci. notn.) 6.352x10 10 m

24. Example-2 Change 952 cg to ? ng (csn) 9.52x10 9 ng

25. Example-3 Convert 723 cm -2 to ? m -2 (csn) 7.23x10 6 m -2

26. Example-4 Example #5: Speed Conversions

27. Example-5 Example #5: Speed Conversions

28. Density Used to characterize substances. Defined as mass divided by volume: Units: g/cm 3 or g/mL. Originally based on mass (the density was defined as the mass of 1.00 g of pure water). Units of Measurement Test Etiquette

29. Density Example The sun is estimated to have a mass of 2x10 36 kg. Assuming it to be a sphere of average radius 6.96x10 5 km, calculate the average density of the sun in units of g cm -3. Mathcad Solution

31. Density Calculations Mathcad Solution

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

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