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While every effort has been made to make sure this electronic syllabus is error-free, it is not official.
The definitive source of course information remains the original (paper) syllabus distributed in class.
LYCOMING COLLEGE     CHEMISTRY 110     FALL 1998
Course Description - Chemistry 110 constitutes a quantitative introduction to the concepts and models of chemistry. Topics include the experimental foundations of the atomic theory of matter, stoichiometry, thermochemistry, periodic trends in atomic properties, the electronic structure of atoms, chemical bonding and the geometry of molecules. These concepts are used to develop models for the behavior of gases, liquids, solids, solutions and simple chemical reactions. Prerequisite: credit for or exemption from Math 100.
 
Faculty  Responsibilities  Office  Office Hours  email
Dr. David A. Franz  lectures, recitation HBC 232, ext. 4181  MWF, 9-10; MF,1:30-3:00  franz@lycoming.edu
Dr. Charles H. Mahler labs U,X,Y HBC 202, ext. 4351 MWF, 10-11; MW, 1-2 mahler@lycoming.edu
 Dr. Henry Berkheimer  lab T  HBC 213   berkheim@lycoming.edu
Miss Lou Ann Miller  lab Z     louann_miller@merck.com
Ms. Amy Hall  study group facilitator      halamy@lycoming.edu

Course Format
•Lectures - MWF, 11:30 a.m., HBC G09, attendance required (3 pt. penalty per absence > three).
•Recitation - one hour on Thursday, attendance checked, possibly required.
•Laboratory - one three-hour period, attendance required in the scheduled period.
•Assigned homework - covered each Thursday in Recitation. Past experience has shown that a student's performance on homework correlates very positively with his or her performance in the course.
•Study Group – an optional session, time and place to be announced, facilitated by Amy Hall, a Junior chemistry major.

Grading Scheme
The final grade is based on the percentage of a total score of 800 points, distributed as follows:

10 best quizzes, 15 points each  = 150
3 hour exams, 100 points each  = 300
1 lab average, 200 points  = 200
1 final exam, 120 points  = 120
1 homework/class average  =  30
800
 
•Bonus points may be earned by attending the weekly Chemistry Colloquium (3 pts each, max of 21 pts), and/or by completing extra-credit problems and papers to be announced later.

•There will be no make-up exams. If the final exam % grade is higher than any one hour exam grade, the lowest hour exam grade will be dropped and the final exam % grade substituted for it.

•Assignment of letter grades is based roughly on the following: A (90%-100%); B (80%-89%); C(70%-79%); D (60%-69%); F (below 60%). Plus and minus grades are included in these ranges. Consideration is also given to student performance as evidenced in the classroom, laboratory, and on homeworks.  

Texts and Other Items
•Chemistry, Molecules, Matter and Change – Atkins and Jones (Freeman, 1997).
•Lab safety glasses - available from the Chemistry Club. Also, long pants required in lab, and no bare feet or sandals.
•Lab notebook with quadrille pages (Freeman) - available at the Campus Store.
•Scientific calculator (with log functions and scientific notation) - no passing of this item during quizzes and tests.
•Student Study Guide (optional) to accompany the text.
•CD-Rom 3.0 (optional) to accompany the text.
•Website (optional) – http://www.whfreeman.com/chemistry3e

Academic Honesty - Unless otherwise stated, all work submitted for a grade must be your own. Students found cheating on examinations, quizzes, or laboratory reports will be dealt with according to the procedures in the Faculty Handbook, which allow for either a reduction in course grade or expulsion from the course with a grade of F. You are encouraged to work on homework problems with other students. However, for any homework which is collected for grading, you must submit your own work; outright copying of homework will be penalized.

Special Invitation - Please feel free to bring to any of the faculty your interests, difficulties, questions, or perplexities. Or just come by for a chat. If our posted office hours don't suit, you are welcome to make an appointment.

 
Tentative Lecture Outline for General Chemistry, Fall 1998
Day
 Date  Reading  Topic  Lab 
M
 8-31    Introduction; Atoms, Elements & Periodic Table  Orientation; Check - In 
W 
 9- 2  1.1 – 1.7  e-,p+,n; Rutherford Model; Isotopes 
F
 9- 4  1.8 – 1.9  QUIZ 1 (1.1 – 1.7); Compounds & Mixtures; Ionic Compounds   
M
 9- 7  1.13 - 1.16  Nomenclature  Separations (#2)  
W
 9- 9  2.1 – 2.7  Units, Density, Conversions, Significant Figures   
F
 9-11  2.8 – 2.10  QUIZ 2 (1.8 - 2.7); Mole, Molar Mass, Measuring Compounds   
M 
 9-14  2.10 – 2.13  Molar Mass, % Composition, Empirical and Molecular Formulas  Density (#1) 
W
 9-16  2.14 – 2.15  Molarity, Dilution   
F 
 9-18  2.14 – 2.15  QUIZ 3 (2.8 – 2.15); Molarity, Dilution   
M
 9-21  3.2 – 3.3  Chemical Reactions and Equations; Electrolytes  % Water (#4) 
W
 9-23  3.3 – 3.5  Electrolytes; Ionic Reactions and Net Ionic Equations    
F
 9-25  3.6 – 3.11  QUIZ 4 (2.14 – 3.5); Precipitation, Acid-Base Reactions   
M
 9-28  3.12 – 3.16  Oxidation-Reduction (Redox); Balancing Redox Equations  Nine Bottle (#9) 
W
 9-30  17.1 – 17.2  Half Reactions and Balancing Redox Equations   
F
 10- 2    EXAM 1, Chapters 1 – 3 & 17   
M
 10- 5  4.1 – 4.5  Stoichiometry, Yield, and Limiting Reactant  Alum (#3) 
W
 10- 7  4.5 – 4.6  Stoichiometry, Combustion Analysis   
F
 10- 9  5.1 – 5.9  QUIZ 5 (Chapter 4); Gases and Gas Laws   
M
 10-12  5.9 – 5.15  Gas Laws, Stoichiometry, Partial Pressures  Atomic Weight (#6) 
W
 10-14  5.16 – 5.17  Molecular Motion, Kinetic Theory, Real Gases   
F
 10-16    LONG WEEKEND, NO CLASS    
M
 10-19  6.1 – 6.7  QUIZ 6 (Chapter 5); Energy, Heat, Enthalpy and Calorimetry  Distillation (#7A) 
W
 10-21  6.8 – 6.10  Calorimetry, Reaction Enthalpies, Hess’ Law   
F
 10-23  6.10 – 6.12  Enthalpies of Combustion, Standard Heats of Formation   
M
 10-26  7.1 – 7.4  QUIZ 7 (Chapter 6); Light and Atomic Spectra  Calorimetry (#8) 
W
 10-28  7.5 – 7.8  Quantum Mechanical Model of the Atom   
F
 10-30    EXAM 2, Chapters 4 - 6   
M
 11- 2  7.9 – 7.11  Orbitals, Energy Levels, Electron Configurations  FP, Density, IR (#7B) 
W
 11- 4  7.12 – 7.20  Ions, Periodic Properties and Trends   
F
 11- 6  7.21 – 7.23  QUIZ 8 (7.1 - 7.20); Descriptive Chemistry   
M
 11- 9  8.1 – 8.3  Lewis Symbols & Ionic Compounds  ReCrystl, MP (#7C) 
W
 11-11  8.4 – 8.9  Lewis Structures, Octet Rule, Resonance, Formal Charges   
F
 11-13  8.9 – 8.14  QUIZ 9 (7.21- 8.9); Octet Exceptions, Electronegativity   
M
 11-16  9.1 – 9.5  Molecular Shape by VSEPR  Mol. Wt. (#7D) 
W
 11-18  9.6 – 9.7  VSEPR; Polar Bonds and Polar Molecules   
F
 11-20  9.8 – 9.11  QUIZ 10 (8.9 – 9.7); Bond Strengths and Lengths   
M
 11-23 9.12 – 9.16  Valence Bond Theory and Hybrid Orbitals  No lab 
W
     THANKSGIVING BREAK   
F
        
M
 11-30 11 Carbon-Based Materials and Structures GC, IR, UV (#7E) 
W
 12- 2    EXAM 3, Chapters 7 - 9   
F
 12- 4  10.6 – 10.12  Intermolecular Forces; The Liquid State   
M
 12- 7  10.13 – 10.17  Course Evaluations; Phase Changes, Phase Diagrams   Check - Out 
W
 12- 9    Review   
F
 12-11   QUIZ 11 (Chapter 10); Illustrated Review   
M-F
 12-    Final Exam, date and time to be announced   
   
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    •  Last updated September 14, 1998.
    The URL for this page is http://lyco2.lycoming.edu/dept/chem/fall1998/110syl.htm