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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 1999

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        
 Miss Lou Ann Miller       lab Z
 Ms. Sara Hirst               study group facilitator

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 Sara Hirst.

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
    •General Chemistry, An Integrated Approach, 2nd Ed. – Hill and Petrucci (Prentice Hall, 1999).
    •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.
    •Chem CDX, a CD-ROM included with the text.
    •Website (optional) – http://www.prenhall.com/~chem  or via the CD-ROM

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 1999
 
Day Date Reading Topic Lab
8-30 1.1 – 1.2 Introduction; Matter & Properties Orientation; Check - In
9-1  1.3 – 1.6  Units; Sig. Figs.; Conversions; Density
9-3  2.1 – 2.2  QUIZ 1 (1.1 – 1.6); Atomic Theory
9-6  2.3 – 2.5  e-,p+,n; Isotopes; Atomic Masses; Periodic Table  Density (#1)
9-8  2.6 – 2.9  Molecular & Ionic Compounds; Formulas & Names; Acids, Bases, Salts 
9-10  2.10 – 2.11  QUIZ 2 (2.1 - 2.9); Organic Compounds
9-13  2.10 – 2.13  Organic Compounds  Separations (#2)
9-15  3.1 – 3.3  Molecular Masses; The Mole & Avogadro’s Number; g/mol conversions 
9-17  3.4 – 3.6  QUIZ 3 (2.10 – 3.3); Mass % & Formulas 
9-20  3.7 – 3.10  Chemical Equations; Stoichiometry; Limiting Reactants; % Yields  Alum (#3)
9-22  3.11  Solutions, Molarity, and Dilution; Solution Stoichiometry 
9-24  QUIZ 4 (3.4 – 3.11); Open Review 
9-27  EXAM 1, Chapters 1 – 3  % Water (#4)
9-29  4.1  Electrolytes, Arrhenius’ Theory; Acids & Bases 
10-1  4.2 – 4.3  Ionic Equations; Precipitation Reactions 
10-4  4.4  Oxidation-Reduction (Redox); Balancing Redox Equations  Nine Bottle (#9)
10-6  4.5 – 4.6  Half Reactions and Balancing Redox Equations 
10-8  5.1 – 5.2  QUIZ 5 (Chapter 4); Gases and Gas Laws 
10-11 5.3 – 5.8  Gas Laws, Stoichiometry, Partial Pressures  Atomic Weight (#6)
10-13  5.9 – 5.12  Molecular Motion, Kinetic Theory, Real Gases 
10-15  LONG WEEKEND, NO CLASS
10-18  6.1 – 6.4  QUIZ 6 (Chapter 5); Energy, Heat, Enthalpy and Calorimetry  Distillation (#7A)
10-20 6.5 – 6.6  Calorimetry, Reaction Enthalpies, Hess’ Law
10-22  6.7 – 6.8 Enthalpies of Combustion, Standard Heats of Formation
10-25 7.1 – 7.5  QUIZ 7 (Chapter 6); Light and Atomic Spectra Calorimetry (#8)
10-27  7.6 – 7.8 Quantum Mechanical Model of the Atom
10-29  EXAM 2, Chapters 4 - 6 
11-1 7.9 – 8.5 Orbitals, Energy Levels, Electron Configurations FP, Density, IR (#7B)
11-3 8.6 – 8.9  Ions, Periodic Properties and Trends 
11-5  9.1 – 9.5  QUIZ 8 (Chapters 7 & 8);  Lewis Symbols & Ionic Compounds
11-8  9.6 – 9.8 Lewis Structures, Octet Rule, Resonance, Formal Charges ReCrystl, MP (#7C)
11-10 9.9 – 9.10  Octet Exceptions; Bond Lengths and Bond Energies
11-12 9.11 QUIZ 9 (9.1 – 9.10); Alkenes, Alkynes, Polymers 
11-15  10.1 Molecular Shape by VSEPR  Mol. Wt. (#7D)
11-17  10.2  VSEPR; Polar Bonds and Polar Molecules 
11-19 10.3 QUIZ 10 (Chapters 9 & 10); Atomic Orbital Overlap
11-22 10.4 – 10.5 Valence Bond Theory and Hybrid Orbitals No lab
11-24 THANKSGIVING BREAK 
F 11-26 THANKSGIVING BREAK 
M 11-29  10.8 – 10.9  Benzene and Aromatic Compounds  GC, IR, UV (#7E)
12-1  11.1 – 11.3  Intermolecular Forces; Phase Changes 
12-3 EXAM 3, Chapters 7 - 10 
12-6 11.4 – 11.7 Course Evaluations; Phase Diagrams; The Liquid State Check - Out
12-8  11.8 – 11.10 The Solid State
12-10 QUIZ 11 (Chapter 11); Illustrated Review
M-F  12-  FINAL EXAM, date and time to be announced 
 
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  •  Last updated September 1, 1999.
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