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.

Links to Web Sites associated with the textbook:
Prentice-Hall The Publisher
Tripod Tools for Life


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.

Faculty                Responsibilities      Office              Office Hours
Dr. David A. Franz     lectures, recitation  HBC 232, ext. 4181  11-12 & 1-2, MWF
Dr. Charles H. Mahler  labs                  HBC 202, ext. 4351  M, 2-3; WF, 10-11 
Miss Lou Ann Miller    lab
Mr. Bradley K. Deacon  lab
Texts and Required Items
  • Chemistry - McMurray and Fay (Prentice-Hall, Inc., 1995)
  • Partial Solutions Manual to accompany the above.
  • Lab safety glasses - available at the Campus Store.
  • 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.

    Prerequisites Credit for or exernption from Math 100.

    Course Format

  • Lectures - MWF, 9:00 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 perforrnance on homework correlates very positively with his or her performance in the course.

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

             10 weekly quizzes, 15 points each    = 150
             3 hour exams, 100 poinb each         = 300
             1 lab average, 200 points            = 200
             1 final exam, 120 points             = 120
             1 homework/class average             =  30
  • Bonus points may be earned by attending the weekly Chemistry Colloquium (3 pts each, max of 30 pts), and/or by completing extra credit problems and papers to be announced later.
  • There will be no makeup 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.

    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 1996
    (For Lab Schedule see Lab Syllabus below)

    Day  Date   Reading   Topic
    M    8-26   1.1-1.4    Introduction; Matter & Properties; Elements & Periodic Table 
    W    8-28   1.5-1.13   Significant Figures; Conversions; Density         
    Th   8-29              Review of ungraded homework #1
    F    8-30   2.1        QUIZ 1 (Chapter 1); Atomic Theory
    M    9-2    2.1-2.7    e-,p+,n; Rutherford; Nuclides; Atomic Weights     
    W    9-4    2.8-2.9    Molecules, Ions; Acids and Bases
    F    9-6    2.10       QUIZ 2 (2.1 - 2.9); Nomenclature
    M    9-9    3.1-3.3    Chemical Equations; Avogadro's Number; Molar Mass
    W    9-11   3.4-3.6    Stoichiometry; Yield; Limiting Reactant
    F    9-13   3.7-3.8    QUIZ 3 (3.1 - 3.6); Molarity; Dilution
    M    9-16   3.9-3.10   Solution Stoichiometry
    W    9-18   3.11-3.13  % Composition; Empirical and Molecular Formulas
    F    9-20   4.1        QUIZ 4 (3.7- 3.13); Review; Reaction Types
    M    9-23              EXAM 1, Chapters 1 - 3
    W    9-25   4.1-4.3    Reaction Types; Electrolytes; Ionic Reactions
    F    9-27   4.4-4.6    Precipitation, Acid-Base, and Redox Reactions
    M    9-30   4.6-4.10   Oxidation-Reduction (Redox); Balancing Redox Equations
    W    10-2   5.1-5.5    Periodic Table; Light; Atomic Spectra
    F    10-4   5.6-5.8    QUIZ 5 (Chapter 4); Quantum Mechanical Model; Quantum #'s
    M    10-7   5.9-5.12   Orbitals; Energy Levels; Electron Configurations
    W    10-9   5.13-5.16  Ions; Periodic Properties
    F    10-11  6.1-6.4    QUIZ 6 (Chap. 5); Ionization Energy; Electron Affinity; Ionic Bond
    M    10-14  6.5-6.6    Alkali Metals; Alkaline Earths
    W    10-16  6.7-6.10   Aluminum; Halogens; Noble Gases
    F    10-18             LONG WEEKEND, NO CLASS
    M    10-21  7.1-7.4    Covalent Bond; Bond Strengths; Lewis Structures
    W    10-23  7.4-7.7    Lewis Structures; Resonance; Electronegativity
    F    10-25             EXAM 2, Chapters 4 - 6
    M    10-28  7.8-7.9    Formal Charges; Molecular Shapes by VSEPR
    W    10-30  7.9        Molecular Shapes by VSEPR
    F    11- 1  7.10-7.12  QUIZ 7 (7.1 - 7.9); Valence Bond Theory; Hybrid Orbitals
    M    11- 4  8.1-8.4    Heat & Energy; First Law; Work
    W    11- 6  8.5-8.6    Enthalpy; Calorimetry
    F    11- 8  8.7        QUIZ 8 (7.10-7.12; 8.1 - 8.6); Calorimetry
    M    11-11  8.8-8.11   Hess' Law; Heats of Formation (DHf)
    W    11-13  8.12-8.13  Entropy; Free Energy
    F    11-15  9.1        QUIZ 9 (8.7 - 8.13); Gases and Gas Laws
    M    11-18  9.2-9.4    Gas Laws; Ideal Gas Law; Stoichiometry
    W    11-20  9.5-9.6    Partial Pressure; Kinetic Molecular Theory
    F    11-22  9.7-9.9    QUIZ 10 (9.1 - 9.6); Graham's Law; Real Gases; The Atmosphere
    M    11-25             EXAM 3, Chapter 7 - 9
                           Thanksgiving Break
    M    12- 2  10.1-10.2  Course Evals; Polar Bonds, Molecules; Intermolecular Forces 
    W    12- 4  10.3-10.5  Liquids; Changes of State 
    F    12- 6  10.6,10.10 QUIZ 11 (10.1 - 10.5); Solids; PhaseDiagrams
    M-F  12-9              FINAL EXAM, date and time to be announced


    Fall 1996 Lycoming College Lab Coordinator: Dr. Mahler (Heim 202, 321-4351)

    Unsafe behavior in Lab will not be tolerated. Repeated unsafe behavior will result in a zero for that lab. In lab: 1) Goggles must be worn at all times; 2) No eating, drinking, or smoking; 3) No horseplay; 4) No unauthorized, "independent" experiments; 5) No sandals (enclosed shoes only); 6) No shorts (long pants only); 7) Additional safety rules given in Lab. You are expected to read the safety information in the Lab Folder and to come to lab each week well prepared. Report all accidents and injuries immediately. Know the location of all exits and emergency equipment (fire extinguishers, fire blanket, eye wash, showers, etc.) When in doubt, ask.

    Wearing contact lenses in lab is highly discouraged. If you do wear them in lab, please let the lab instructor and the lab assistant know (you will not be penalized - it is good to know in case of an accident). Wear older clothes - they could be stained or ruined. Above all, use common sense and your chemical intuition - THINK. As a student chemist, you will be working in many situations which demand your utmost care and attention to protect the safety and health of yourself, your fellow students, and the environment. Preparation and careful, patient work are needed to obtain the results required in each experiment.

    Your Lab Notebook should be neat, well organized, up-to-date and complete, with a Table of Contents. Leave room to record your data, the uncertainties in measurements, and any observations about the experiment. Make a copy of each notebook page with carbon.

    Lab reports consist of the report form, sample calculations, and any graphs or other material needed. Graphs should be on proper paper, fill the page, show data points in ink, have linear (or proper) scales with units and labels on axes. Data from unknowns and values determined from the graph should be clearly marked. Additional instructions will be given in the prelab lectures.

    In order to make-up a lab, only absences notified ahead of time will be excused. Each lab section is very full, so all requests to make up a lab or attend a section other than your normal lab must go through Dr. Mahler. Students who simply show up at a different lab section will not be admitted to that lab. Prelabs are due at the start of lab, and will not be accepted late. Lab reports are generally due one week after completing the lab. Due dates will be announced in lab.

    Tentative Laboratory Schedule for Chemistry 110, Fall 1996

    Week of        Lab
    8/26-8/30      Orientation, Check in, Safety, and the Lab Notebook
    9/2-9/6        Density of Liquids and Solids (#1)
    9/9-9/13       The Separation of a Mixture (#2)
    9/16-9/20      Synthesis of Potassium Aluminum Sulfate (#3)
    9/23-9/27      Percent Water in a Hydrate (#4)
    9/30-10/4      The Nine Bottle Problem (#9)
    10/7-10/11     Separation, Purification & ID of a Mixture: Distillation and Boiling Point (#7A)
    10/14-10/18    Freezing Point and Density of Solvent (#7B)
    10/21-10/25    Recrystallization and Melting Point of Solute (#7C)
    10/28-11/1     Molecular Mass of Solvent by Vapor Density (#7D)
    11/4-11/8      Spectroscopic Identification Solute & Solvent(#7E)
    11/11-11/15    Calorimetry (#8)
    11/18-11/22    Atomic Weight of a Metal (#6) 
    11/25-11/29    THANKSGIVING BREAK - NO LABS
    12/2-12/6      Checkout of Lab

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