Introduction. Chem 110: Chemical Principles 1 Sections 40-52

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1 Introduction Chem 110: Chemical Principles 1 Sections Instructor: Dr. Squire J. Booker 302 Chemistry Building squire@psu.edu (sjb14@psu.edu) Lectures: Monday (M), Wednesday (W), Friday (F) 1:25 2:05 Recitations: Wednesday or Thursday (Depends on Section Assigned) Must Attend Assigned Recitation

2 Requirements and Prerequisites Some High School Chemistry Algebra (including logarithms) A General Familiarity with Chapters 1 4 and Chapter 10 in Textbook If you have NEVER studied chemistry, this course is probably not for you. Come and talk to me! Must take Pre-Quiz to insure proper placement

3 Teaching Assistants Section 40 Section 41 Section 42 Section 43 Section 44 Section 45 Section 46 Section 47 Section 48 Section 49 Section 50 Section 51 Section 52 Tamara Badger Mark Merritt Seth Michalski Tamara Badger Ian Sines Mark Merritt Tamara Badger Seth Michalski Mark Merritt Ian Sines Mark Merritt Seth Michalski Mark Merritt You are required to bring your text, student packet, calculator, and COMPLETED homework to recitation.

4 Chem110 Student Packet 1. General Information about Course 2. Syllabus 3. General Information Sheet 4. Basic Skill Check Instructions 5. Supplemental Homework Problems 6. Supplemental Problems Answer Key 7. Equations Sheet 8. Periodic Table 9. Fall 2007 Practice Exams 10. Fall 2007 Practice Exams Answer Keys 11. Spring 2008 Practice Exams 12. Spring 2008 Practice Exams Answer Keys

5 Course Web Page 1. General Information (almost everything you need to know about the class. 2. Abbreviated Lecture Notes (Not necessarily complete) 3. Announcements 4. Exam schedule Monday Evenings (6:30 7:45) Locations to be announced Exam 1 September 22 Exam 2 October 13 Exam 3 November 10 Comprehensive Final during Final Exam Week

6 Recitations Recitations are mandatory Bring textbook, student packet, calculator and COMPLETED homework before recitation. This week: Read Chapter 1 Do Chapter 1 Problems: 17, 24a-d, 27, 50, 78 and Suppl. 1-5 Starting with second recitation: Quizzes given each week Homework collected One randomly selected problem per lecture will be collected in recitation and graded by your TA Details given in recitation.

7 Quizzes Quiz points available 140 Maximum Quiz points possible 100 Homework points available 140 Maximum homework points possible 100 No make up for quizzes or homework! Basic Skills Course Points 10 Instructions in Packet Try them out: questions on Wednesday

8 Basic Skills Basic Skills are basic concepts and the principles that underlie many of the calculations and problems assigned in Chem 110. Math (algebra) Metric system and metric conversions Electron Configurations Periodic Trends Nomenclature of Ions, Molecular Compounds and Ionic Compounds Lewis Structures Concentration and Dilution Aqueous Chemicals and Net Ionic Equations These computer based tests can be accessed through Angel ( Login using your access account and password. Data base with thousands of questions No two tests are alike Tests can be taken many times: Practice Detailed instructions are in course packet and are posted on the Course Web page

9 Grading Exam I Exam II Exam III Final Quizzes Homework Basic Skills Total 34 points 34 points 34 points 56 points 16 points 16 points 10 points 200 points Typical Distribution of Grades Grade Percent Points A,A B+, B, B C+, C D F Make-up exams ONLY for excused absences

10 Advice for Success Spend at least 10 hours per week outside of class Read text before lecture Bring lecture notes to class Try problems in text Work supplemental problems o Work together o Work alone All homework should be done before recitation. Get help in Chemistry Resource Center (211 Whitmore) if necessary See How to Do Well in Chem 110 Select handouts posted on Chem 110 Website

11 General Information Chemistry Undergraduate Office (210 Whitmore) o registration o drop/add o incorrect exam grades Chemistry Resource Center (CRC) (211 Whitmore) o Free tutoring o Hours: Monday-Friday (9:05 am 4:25 pm) Information on Web ( o Syllabus o Announcements o Exam locations o CRC hours (211 Whitmore) o Lecture Notes

12 Chemistry The Central Science Life Sciences Agriculture & Environment CHEMISTRY Materials Engineering Physics Math

13 Chemistry the Molecular Science Macroscale: Nanoscale: What we can see (observe) What transpires on the molecular level How does the behavior of atoms and molecules connect to the behavior of matter that we observe? Why Study Chemistry? Learn the language of chemistry Structure affects function (properties) Connecting microscopic properties to macroscopic properties How do we know what we know (Modern analytical techniques and instrumentation Energy store in molecules? Develop analytical problem solving skills

14 Chemistry The study of matter and the changes it undergoes

15 Matter Atoms are the building blocks of matter Each element is made of the same kind of atom A compound is made of two or more different kinds of elements

16 States of Matter

17 SI Units Système International d Unités a different base unit for each quantity Metric System

18 Derived SI Units Volume (length) 3 Density = mass/volume

19 Uncertainty in Measurement The difference between Precision and Accuracy

20 Uncertainty in Measurement Significant Figures Measured quantities are reported in such a way that only the last digit is uncertain

21 Significant Figures (Dealing with Zeros) All nonzero digits are significant Zeros between nonzero digits are always significant Example: (four sig figs) Zeros at the beginning of a number are never significant. They are merely place holders Example: (two sig figs) Zeros at the end of a number are significant only if the number contains a decimal point Examples:5000 (1 sig fig) (4 sig figs) x 10 3 (4 sig figs)

22 Significant Figures in Calculations Addition and Subtraction The result contains the same number of decimal places as the measurement with the fewest number of decimal places Add these numbers (2.9321; ; ; 10425) Multiplication and Division The results contains the same number of significant figures as the measurement with the fewest significant figures Multiply these numbers (21.5, 100, 38, 101) Multiply these numbers (21.5, 1.00, 38, 101)

23 Dimensional Analysis 1. Keep track of units and carry them throughout your calculations. 2. Use proper conversion factors to convert given units into desired units Example: The average speed of a nitrogen molecule in air at 25 C is 515 m/s. Convert this speed into miles per hour. (1 mile = km)

24 Problem Solving Making Connections What are you given? What else do you known? Organize the information. What connections can you make? Example: An unknown liquid has a density of 2.14 g/cm 3. How many mm 3 would a 6.42 mg sample of this liquid occupy if dispensed into a 10 mm 3 UV-vis spectrophotometer cuvette? mm mm mm mm 3 5. none of the above

25 Before Recitation this Week Read Chapter 1 Work Problems at End of Chapter o 17, 24a-d, 27, 50, 78 o And o Supplemental 1-5 in student packet Take Pre-Quiz Before Wednesday Read Chapter and

AP Chemistry

AP Chemistry 2016-2017 Welcome to AP Chemistry! I am so excited to have you in this course next year! To get geared up for the class, there are some things that you need to do this summer. None of it is