Course Description: The first semester in the two semester General Chemistry Program for Science Majors. This course can not serve as a prerequisite for CHM 231 or CHM 232.

Prerequisites:

• High School Chemistry or CHM 109
  
  MTH 110 (College Algebra)
  

Faculty Information:

• Name: Prof. Stephen Matchett
  
  Office: 352 PAD
  

Office Hours:

• M 9-11 am; Thurs 10-11 am and 4-5 pm
  
  Phone: 895-3879
  
  e-mail matchets@gvsu.edu
  

Text: Required: Chemistry: Structure and Dynamics; Bodner, G.M. John Wiley and Sons, Inc. New York, 1995. and the Modular Chapters supplement.

Objectives:

• 1) Provide a clear understanding of the fundamental principles of chemistry from a molecular/theoretical perspective.
  
  2) Explain basic chemical reactivity using current theories and models for chemical bonding.
  
  3) Provide the student with the relevance of chemistry to their daily lives.
  
  4) Stress the interconnections between the various topics so that students can see how the major themes of Stoichiometry, Chemical Bonding, Chemical Energy, and Periodicity run throughout the material.
  

Instruction Methods:

• Lecture (4 fifty minute lectures/week)
  
  Discussion (1 fifty minute discussion session/week)
  
  Lab (1 two hour lab/week)
  
  

Calculators: You will need a battery or solar powered calculator for the exams. A scientific calculator capable of scientific notation, "log" and "inverse log" calculations is required for several of the exams. Each student must have their own calculator since they may not be shared during an exam. Students may not use a programable or graphing calculator on any exam. This requirement provides a level playing field for all and was the suggestion of many previous students.

Discussion Period: You are expected to attend one of the discussion sections handled by your instructor (Sections B1, B2, B3, B4). During these weekly sessions, topics which are central to that weeks lectures will be analyzed and discussed. This discussion will include a forum for you to ask questions you may have from the problem assignment, the laboratory work or the lectures. Since it is a discussion, you will be expected to participate.

A short quiz will be given in the discussion section every week (including the weeks in which there is an exam). There are no make-up quizzes. These quizzes will cover the problem assignments for that week. You will receive 3 points if your answer is completely correct (no partial credit), 1.5 point for attempting the problem or 0 points if you were absent. The quiz grade will account for 75% of your discussion section grade.

In the first discussion section you will be divided into groups. Each week in discussion section, there will be a problem or worksheet to be completed in class with your group. This will be turned in for credit at the end of that discussion period. This exercise will account for the remaining 25% of your discussion section grade.

The formation and maintenance of study groups is strongly encouraged.

Problem Assignments: The ability to master the material is best achieved by working a series of mathematical and conceptual problems. Each week you will receive a problem set. These will not be collected, but they will serve as the basis for your weekly quizzes. If you miss them in class, the weekly problem sets are posted on the web page as they are assigned.

Laboratory Requirements: Laboratory experience is a requirement for credit in this course. There will be 14 lab experiments, one each week, with a report required for each one.

1. There are two types of labs that will be taugtht: an inquiry style lab (written lab reports) and a standard verification style lab (fill in the data sheets).
2. The reports for the inquiry style labs (1, 3, 4, 5 & 6) are due 2 days after the lab was held and will be turned in at a location decided upon by the lab instructors. Labs that are turned in late will be penalized 10% points for each day late. Any lab turned in after the start of the next lab period will not be accepted.
3. No one may leave the inquiry style labs early, unless you turn in your lab as completed and ready for grading. If you leave early without turning in a report, you will not be allowed to submit a report for that lab.
4. Reports for the remaining labs are due before you leave the lab.
5. Each week you must complete the prelab questions prior to attending lab. This advance preparation will make each of the labs flow more smoothly.

In order to pass the entire course, you must pass the lab with better than a 60% average.

You must attend the lab session in order to receive any credit. There are no make-up labs. If you miss a lab you must fill out a laboratory absence form (found in the lab manual). The first absence will be taken on the students word. Any additional absence will be counted as a zero unless written verification of the reason is obtained and deemed acceptable by the instructor.

Each student who enrolls in a lab course pays a laboratory fee. This fee covers the cost of chemicals, non-reusable equipment, and a nominal amount of breakage for each student. Individual students will be billed for any excessive breakage.

Exams: Lecture hour exams are used to evaluate the students progress and will determine a large portion of the students grade. Exams will be graded and returned to the student as a study tool as quickly as possible. The final exam, however, will not be returned to the student. Books, papers and notes of any kind are prohibited during exams. If a student is caught cheating, the student will fail the course and potentially face further action.

Exams will consist of two parts: The first part will be multiple choice (approximately 20-25 questions) involving both theory and calculations. The second part of the exam will be open format where students will be allowed to show their work for partial credit on a series of problems and/or essay style questions.

There will be no make-up exams (no exceptions). If a student is unable to attend an exam, the points from that exam will be used to increase the weight of the comprehensive final.

Course Grade is determined by the weighted average of the following components. If the student takes all 4 tests then:

• Exams (4) 60%
  
  Lab Average 12%
  
  Final Exam 15%
  
  Discussion Section Average 13%
  

If the student misses one exam then:

• Exams (3) 45%
  
  Lab Average 12%
  
  Final Exam 30%
  
  Discussion Section Average 13%
  

If the student misses more than one exam, each additional absence will be assigned a percentage score of zero. (Hint: don't miss the tests!)

Grading Scale: Grading will be based on the following scale:

A = 90+; A- = 87-89; B+ = 84-86; B = 80-83; B- = 77-79; C+ = 74-76; C = 70-73; C- = 67-69; D+ = 64-66; D = 60-63; F = < 60

Incompletes: The grade "I" is sometimes granted when a student is temporarily unable to complete course requirements because of unusual circumstances. It may be assigned when illness, necessary absence, or other reasons generally beyond the control of the student, prevents completion of the course requirements by the end of the semester. This grade may not be given as a substitute for a failing grade or withdraw.

The "I" grade will not be assigned for incomplete course work which was due before the twelfth week of the semester. A request for an "I" grade must be made in writing before the final exam. To make this request you must schedule an interview with the instructor.

Lectures    Topic

1-3         1. Basic Atomic Concepts

4-8         2. Nuclear Chemistry

             a) Discovery and Historical Context

             b) Types of Decay

             c) Nuclear Stability and Binding Energy

             d) Fission

               1) Basic nuclear power

               2) The Atomic Bomb

             e) Fusion

               1) Contrast to fission

               2) Origin of the Elements

               3) The Hydrogen Bomb

9-16        3. Quantum Chemistry and the Concept of Atomic Orbitals

             a) Light, energy and the electromagnetic spectrum

             b) Deducing Electronic Structure

               1) Flame tests

               2) Emission Spectra

             c) The Bohr Model and its failure

             d) Experimental Data in search of a new model

             e) The Wave Model and quantum mechanics

             f) Quantum numbers

             g) Atomic Orbitals

             h) Electronic configurations

              i) Relation of quantum numbers to the periodic table

             j) Aufbau filling and exceptions

             k) Orbital Diagrams and Hunds Rule

             l) Magnetic properties

               1) Paramagnetic vs Diamagnetic

               2) Ferromagnetic (True Magnetism)

17-20      5. Periodic Properties

            a) Effective Core charge

            b) Atomic Radii

            c) Ionization Potential

            d) Electron Affinity & Electronegativity

            e) Average Valence Electron Energy

             f) Overview of Main Group Elements

            g) General contrast of 2nd Period vs 3rd and Higher Periods

21-24     6. Basic Redox Chemistry

            a) Formation of ions (Cations and anions)

            b) Simple Electron Transfer between atoms

            c) Oxidation and Reduction

              1) Simple mass balancing of reactions

              2) Oxidizing agents and reducing agents

              3) Activity Series of Metals

24-28    7. Ionic Bonding

           a) Formulas for Ionic Compounds

           b) Making compounds from ions

           c) Formula weight and moles

           d) Empirical and molecular formulas

           e) Nomenclature of ionic compounds

           f) The energetics of ionic bonding/properties of ionic solids

29-32    8. The Descriptive Chemistry of Group 1 (I) and 2 (II)

          a) General Properties

          b) Binary Compounds

            1) Balancing Equations

            2) Reaction Stoichiometry

            3) Limiting Reagents

          c) Anomalies of Lithium

          d) Summary of Similarities and Differences Between Groups 1 and 2

33-39    9. Covalent Bonding

          a) Bond Energy and the nature of the covalent bond

          b) Nomenclature

          c) Theories Representing the Covalent Bond

            1) Lewis dot structures

            2) VSEPR (Electron Domain) theory and Shapes

            3) Valance bond theory

          d) Polarity of Covalent Molecules

40-41   10. The Chemistry of Group 14 (IV): The Transition from Ionic to Covalent Bonding

          a) Carbon

           1) Basic Hydrocarbons

           2) Combustion

          b) Silicon

           1) Elemental Si and Silicon Oxides

           2) The concept of Specific heat

           3) Semiconductors

          c) Lead and Drinking Water

42-47    11. Intermolecular Forces and Phase changes

          a) Identification of the types of forces

          b) Delta H of Phase changes

          c) Phase diagrams

          d) Properties of Solids

          e) Properties of the Liquid State

48-52    12. Solutions

          a) Factors affecting solubility

          b) Solution Concentration

          c) Vapor Pressure Lowering/Colligative Properties

          d) Reactions in Solution and Solution Stoichiometry

          e) Delta H for a reaction

            1) Heats of Solution

            2) Heats of Reaction

            3) Heat Summation

Week Lab

1 * Safety Lab.

2 Density

3 * Introduction to Atomic Spectra: Construction of a Spectrocope and Calibration

4 * Measuring Atomic Spectra: Testing the Bohr Model

5 * Light Beer not Lite Beer: Measuring the Ion Content of Beer Using Atomic Spectroscopy

6 * Electrons in Solids: Determination of Electronic Structure Using Magnetic Properties.

7 Experimental Determination of Avogadros Number

8 Determination of a Chemical Formula: The Atomic Mass of Sn.

9 Determination of a Molecular Formula using Gypsum

10 Shapes of Molecules (a Modeling Lab).

11 Water Hardness

12 Redox Titration

13 Solution Concentrations

14 Thermochemistry.

* = Inquiry Style Lab Experiment


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