SYLLABUS

I. Chemistry 111-112, General Chemistry 3 cr. hrs per semester.

II. Fall 2001-Spring 2002

Instructor: Dr. Stanley Leslie Latesky Room: Farr-Chinnock 308

Office Phone: 869-6222

Home Phone: 869-0453

e-mail: slatesky@lmunet.edu

Web: www.lmunet.edu/faculty/latesky/

Office Hours: MWF 9:00-10:00 a.m.

T R: 1:30 - 2:30 p.m.

III. Course Prerequisite or co-requisite: Math 111, high school chemistry recommended

IV. Course Description/Goals: An in-depth study of the principles of chemistry: atomic structure, chemical bonding, types of compounds, energy relationships involving chemical reactions, periodic relationships, chemical properties, chemical reactions, mass relationships in chemistry, and material science. Goals: 1) To teach students how to intuitively solve problems. 2) To give students an introduction to chemistry, the central science. 3) To help students gain the confidence and discipline required for studying and learning a variety of subjects. 4) To give students an in-depth survey of three areas of chemistry; analytical, inorganic and physical chemistry. 5) To prepare students for further study in chemistry.

V. Relationship of this course to content area knowledge and skills: The subject of chemistry is required for the study of subjects. Subject areas that would be served by this course would be chemistry, biology, physics, math, engineering, medicine and secondary education. This course develops the study habits and skills required for students in these disciplines. It is a course designed for students that have a high school background in the sciences and is intended for those students who wish to pursue a career in the sciences, engineering, or health sciences.

VI. Textbook: Atkins and Jones, “Chemical Principles: The Quest for Insight”, 2^nd edition, Freeman, 2002.

VII. Course Objectives: 1) To improve basic problem solving skills. 2) To relate to students the necessity of understanding basic chemistry. 3) To gain an understanding of the scientific method and to apply it to other disciplines. 4) To understand the basic principles of analytical chemistry (mole concept, calculations involving stoichiometry, acid-base chemistry, balancing chemical reactions), inorganic chemistry (acid-base chemistry, reaction chemistry, periodic properties and trends, solid state structure), and physical chemistry (thermochemistry, enthalpy, entropy, calorimetry, bonding, molecular structure, gas laws, solution chemistry, equilibrium, electrochemistry, and kinetics).

VIII. Outline of Course Content/Units of Instruction:

1) Atoms, Molecules and Ions: Atomic theory, structure of the atom, isotopes, atomic masses, periodic table, chemical substances, nomenclature, writing and balancing chemical reactions.

2) Chemical reactions: Types of reactions, oxidation reduction reactions, acid-base reactions.

3) Calculations involving chemical formulas and equations: mole concept, determination of chemical formula, stoichiometry, calculations involving materials in solution, analysis of materials.

4) The Gaseous State: gas laws, experimental conditions, mixtures of gases, kinetic molecular theory.

5) Chemical equilibrium: the equilibrium condition, the equilibrium constant, applications of equilibrium calculations.

6) Acids and bases: pH, acid and base theories, weak acids and bases, calculations involving weak acids and bases.

7) Applications of aqueous equilibria: common ion effect, buffers, titrations, pH curves, solubility equilibria, complex ion equilibria.

8) Energy, enthalpy, and thermochemistry; energy, enthalpy, thermodynamics of gases, calorimetry, Hess's law, Standard enthalpies of formation.

9) Spontaneity, entropy, and free energy: spontaneous processes, ideal gas applications, entropy, temperature effects, free energy.

10) Electrochemistry: galvanic and electrolytic cells, standard reduction potentials, electrolysis.

11) Quantum mechanics and atomic theory: light, atomic spectra, the Bohr model of the atom, orbitals and quantum numbers, periodic trends.

12) Bonding: types of bonds, electronegativity, polarity, partial ionic character, covalent bonding, Lewis structures, resonance, molecular structure.

13) Covalent bonding: orbitals, molecular orbitals, homonuclear and heteronuclear diatomic molecules.

14) Chemical Kinetics: rates of reactions, rate laws, integrated rate laws, orders of a reaction.

15) Liquids and solids: intermolecular forces, structure of solids, vapor pressure, phase diagrams.

16) Properties of solutions: colligative properties, solution composition, solubility of gases, vapor pressure of solutions, electrolyte solutions.

17) Nuclear Chemistry: nuclear reactions, processes, medical applications

The material covered in this course will consist of chapter by chapter coverage of the textbook.

Any material that will not be covered will be announced by the instructor. The student is responsible for reading each chapter and section therein, even if not discussed in lecture.

IX. Required Readings: Textbook and supplementary material distributed by the instructor.

X. Suggested ReadindBiblioaraphy: None

XI. Method of Instruction and Learning: Classroom lecture, problem solving, and homework will be the principle method of instruction. Homework will be collected on a regular basis. Students will be expected to read the assignments before coming to class.

XII. Course Requirements/Methods of Assessment/Evaluation/Documentation: All students are expected to attend classes regularly, to complete assignments on time, to study, and to work. If you choose not to attend class you are responsible for obtaining any notes and class material from the instructor, at which time you will be asked for a reason for your absence. If you miss an examination, and the absence is considered unexcused, you will not be allowed to make up the examination. Examples of unexcused absences include, but are not limited to: sleeping in, not ready for examination, did not feel like taking exam, had a hospital clinical the day before and did not have a chance to prepare for the exam, had an organic exam the day before and did not have a chance to prepare for the exam, had a headache, etc. Excused absences might include death in the family, hospitalization, illness (You will need a Doctor’s excuse), etc. This class is scheduled for a 75-minute period. If you come to an exam late, you will only have the remainder of the period to finish the examination. There will be a comprehensive final examination given at the completion of both semesters. The final exam for the second semester will be a two semester comprehensive examination.

The numerical method of assessment is described below:

4 Examinations 4 Problem Assignments Comprehensive Final	400 points 400 points 200 points
Total	1000 points
900 to 1000 pt's 800 to 899 pt's 700 to 799 pt's 600 to 699 pt's < 600 pt's	A B C D F

+ grades will be assigned to any student in the upper 20% bracket of any grade group

- grades will be assigned to any student in the bottom 30% bracket of any grade group

XIII. Clinical/Laboratory/Field Experience: See accompanying syllabus for Chemistry 111-112 Laboratory.

XIV. Date of Last Revision: August 10 2001