College of Environmental and Physical Sciences, Department of Chemistry
GENERAL CHEMISTRY I
CH 115 Sec 001, Fall 2005
Drop-In Office Hours Monday & Tuesday and Wednesday
Course Description: CH 115 General Chemistry I (5 semester credits)
General Chemistry is the introductory university level course for students pursuing further study in science. A solid foundation in chemical principles is needed for continuing your studies in chemistry, biology, engineering, geology, physics, health sciences and environmental studies. This course will work to emphasize the integration of concepts and applications with factual information and to stress approaches to both conceptual and numerical problem solving. Throughout the course, chemistry will be used to understand everyday phenomena, to evaluate the risks and benefits environmental issues, and be related to other disciplines.
Catalog Description: Fundamental principles of chemistry with emphasis on atomic structure, molecular structure, and stoichiometry. Co- or Prerequisite: MA111 or equivalent
Lecture: Chemistry: Matter and Its Changes. 4th Edition. Brady & Senese Wiley 2004
Lab: General Chemistry Lab 7e for LSSU CH115 Beran.
Other Required Materials:
State Council of State Science Supervisors:
Ø H-ITT Classroom Response Clicker – details to be announced
Plus – packaged with textbook/lab packet, available online from Wiley
Ø Chemical Splash Goggles, must be indirectly vented with plugs INSTALLED
Ø A NON-PROGRAMMABLE SCIENTIFIC CALCULATOR is required for exams
Ø Scantron sheets for major exams and final and first lab
Optional: Laboratory apron and gloves, Student Study Guide, Student Solution Manual, ACS study guide for General Chemistry (available directly from LSSU Chemistry Club)
Additional resources are available online through dedicated websites for this course. The LSSU WebCT site (http://WebCT.lssu.edu), http://education.lssu.edu/myton , and the Wiley course site http://www.wiley.com/college/brady including the eGrade homework.
1: Atoms and Elements
Learning Objectives: Be able to use the scientific method, build models of nature, classify materials by properties, use subatomic particles to describe atoms compounds, and explain the organization of periodic table
2: Compounds and Chemical Reactions
Learning Objectives: Be able to compare elements and compounds, write and balance chemical equations, identify energy change in chemical changes, name molecular and ionic compounds, and compare the properties of molecular and ionic compounds
Ø Ch 3: Measurement
Learning Objectives: Be able to select and use measurement tools, relate measurements in various units, convert between units using dimensional analysis, understand uncertainty in measurement, use significant figures in measurements, calculations and reporting of values, understand and perform calculations using density and other related units.
4: The Mole: Connecting the Macroscopic
and Molecular Worlds.
Learning Objectives: Be able to use large-scale measurements to count tiny objects, relate the mole to mass and number of atoms/molecules, write and use molecular and ionic formulas, use chemical equations to relate between species, identify limiting reactant and theoretical yield.
5. Reactions Between Ions in Aqueous
Learning Objectives: Be able to use terminology applied to solutions, write ionic equations, predict products of precipitation, acid/base, and gas-forming reactions, name acids and bases, describe a solution by concentration units including molarity, perform calculations using solution concentrations, and stoichiometry of balanced reactions including gravimetric and titration reactions
6: Oxidation-Reduction Reactions
Learning Objectives: Be able to identify oxidation/reduction processes, oxidation number, balance using ion-electron method, predict displacement reactions based on redox potential, perform calculations using stiochiometry of redox reactions
7: Energy and Chemical Change: Breaking and Making Bonds
Learning Objectives: Be able to relate energy work and heat, calculate heat from temperature changes, determine enthalpy changes using stoichiometric relationships, use Hess’ law and tabulated standard heats of reaction to predict energy changes
8: The Quantum Mechanical Atom
Learning Objectives: Be able to describe radiation as wave or particle, explain atomic line spectra, relate electron energy transitions to electronic orbital theory, describe the periodic properties of elements and explain chemical and physical properties on the basis of electronic configurations
9: Chemical Bonding: General Concepts
Learning Objectives: Be able to relate electron transfer to ionic bonding, track valence electrons, explain bond structure bond length, polarity and electronegativity, draw Lewis structures using formal charges to evaluate, and predict resonance structures
10: Chemical Bonding and Molecular Structure
Learning Objectives: predict molecular shape, determine bond angles for chemical compounds on the basis of VSEPR Theory and identify the atomic hybridization in compounds, and use molecular and hybrid orbital theory to explain bonding
11: Properties of Gases
Learning Objectives: Use Kinetic Molecular Theory to describe the properties of gases, use the gas laws to predict the behavior of gases, solve stoichiometry problems involving gases, explain effusion and diffusion, evaluate the behavior of non-ideal gases
12: intermolecular Attractions and Properties of Liquids and Solids
Learning Objectives: Relate the properties of liquids and solids using the KMT, strength of intermolecular forces, relationship of vapor pressure, boiling points to intermolecular forces, entropy changes and concept of dynamic equilibrium, make predictions using phase diagrams
13: Structures, Properties and Applications of Solids
Learning Objectives: Be able to relate the physical properties of crystalline solids to their crystal structure, intermolecular forces as a function of crystal type, explain polymer formation,
Class/Laboratory Schedule: Class meets fifty minutes four times a week, Lab meets two hours and fifty minutes each week through a 14 week semester. A 2-hour course comprehensive final examination is required during finals week
This course serves as prerequisite to the following courses: CH116 General Chemistry II, a grade of C or higher must be earned in CH115 as prerequisite to CH116.
Course Coordinator: David Myton dmyton@LSSU.edu
CH115 001 General Chemistry I MTWR 11-11:50 CRW204
CH115 00A Lab
CH115 00B Lab B Stevens T CRW333
CH115 00C Lab C Dunham T 6:00-8:50 pm CRW333
CH115 00D Lab D Iretski W 2:00-4:50 pm CRW333
CH115 00E Lab
Grading: Course grades will be derived from Assessments 75%, Homework 8% and Laboratories 10%, other (in-class quizzes, participation, and attendance) 7%. The laboratory work is a mandatory component for the course, a passing grade in the lab must be achieved to receive a passing grade in the course. In the occasional circumstance where a student is repeating this course, the laboratory is still required and must be completed irregardless of their past laboratory experience. Assessments includes online quizzes, term paper, scheduled tests and the final exam. Grading is progressively weighted with later tests (whose content is cumulative for the entire course to date) weighted more than earlier tests. Scantron forms and #2 pencil are required for each test/exam date and the first laboratory. Attendance at all class sessions is strongly advised, graded activities will be included without further notice. If you find that the class sessions are not meeting your needs please let me know how you feel we could change the structure to assist you.
Exam Dates: Regular exams are scheduled for September
19, October 10, October 31 and November 22.
Please note the Final Exam date is:
Exams: Each student is advised to bring a personal calculation aid with them to every class, laboratory and test/examination (abacus, slide rule or calculator) - these cannot be shared during tests and should be capable of manipulating scientific notation, logarithms and exponents. Only NON-PROGRAMMABLE SCIENTIFIC CALCULATORS may be used during tests, quizzes and examinations. My philosophy regarding the memorization of formula and physical constants is that each student can and will learn those that they find useful and valuable on an ongoing basis. Therefore I, for this semester only, (don’t count on anyone else doing this) will allow the use during any quiz or mid-semester test, in addition to your personal calculator, pencil, and blank scratch paper, the use of one and only one 3”x5” conventional index card. No card may be used on the course final – you must work toward full independence by the end of the course. This one card may contain any physical constants, formulas, sample calculations, prayers and/or meditative verse that you believe you may find useful. All information on the card must be handwritten. I will provide unusual or unique physical constants for specific chemicals, bond energies, activities of metals, and standard molar enthalpies, etc. Each student may possess one and only one card as described above, violations of this rule are considered academic dishonesty - severe penalties will be enforced. It is vital that you report promptly for exams, as no time extensions are possible.
Online Homework/Quizes: Success in General Chemistry is undeniably linked to the amount of time invested in learning the material and problem solving. Online quizzes and homework will be assigned through the publisher’s website. Additional information on the assignments will be given in class. Quizes must be completed prior to the exam for each chapter, and must be completed within the allocated time. Follow the WebCT links to the additional resources for non-graded practice questions for each chapter to test your knowledge and to reinforce and review for exams.
Each student will write a term paper (between three and five printed pages, 1” margins, 12pt font or less, double spaced) on any subject covered in the first semester of this course (or the first 13 chapters of the textbook) that is of interest to him or to her. “Topics might include the types of glass used in thermal heating, graphite used in fishing rods and sporting equipment, diamonds, films used in the motion picture industry, Teflon, nuclear reactors, penicillin, ether, etc.”
“The paper should contain an introduction, a narrative section, and a conclusion. The introduction should be fairly brief and explain why you’re writing the paper or why the topic you’ve chosen is important or interesting. The narrative section should contain some historical background, the information you’ve learned from your reading and from your searching of the Internet and the basis for any arguments you’re going to put forth in your paper. For example, if your paper is on fats in the American diet and you think there is too much fat in the average diet, you need to define what fats do, why fats are a necessary part of the diet, what evidence there is that too much fat is eaten and what might happen from eating too many fatty foods. Just saying that the average American is over-weight because she or he eats too many fatty foods will not suffice. . . . The conclusion should also be brief and contain your “take home message” or the main points you’re trying to make in your narrative. For example, continuing the fat-theme, you might conclude that the percentage of total calories that originates from fats in the diet is more important than the total amount of fat in the diet.”
At least three references must be used, and one of these references must be a book or a scientific journal that is actually in the library (the citation would include the page number). “Some references to consider are: Scientific American, Nature, Science, Chemical and Engineering News, Journal of Chemical Education, and Chemical Heritage. The latter journal is especially good for historical subjects.” Do not bother citing People, National Inquirer, Time for Kids or the “Ask Dr. Science” archives.
Your paper will be
graded based on both content and format, spelling and grammar “count”. The paper will be counted in the final grade at
a weight equivalent to one of the course tests.
The introduction and bibliography are due Monday, October 3. The complete paper is due Monday, November
28. Turn in a paper copy AND an
electronic copy by email (email@example.com subject line: “CH115 paper”) You
may include the words written by others directly only when presented in
quotation marks and properly cited. You
may include the facts and ideas of others in any format only when you properly
cite the source. You may include your
own original work without restriction.
For example, this assignment is based on an article written by Dr. David
The Fine Print:
Laboratory: Chemistry is an experimental science. You are encouraged to think independently about the data you collect and you will not be graded solely on whether you acquire the right number or deduce the correct explanation, but rather whether your explanations and hypotheses follow logically from the data and that your reasoning is clearly stated. In the laboratory component of this course students may OCCASIONALLY work together in teams of no more than two, as directed by the instructor. Each student team member is responsible for assuming an equal share of the lab responsibilities and work load. Students are to prepare the pre-laboratory assignments before coming to lab, and to complete and turn in their own laboratory reports as assigned. Students are advised to read the laboratory procedures and carefully plan their work to maximize efficiency and guarantee success. If you must be absent from a laboratory session you should contact your laboratory instructor and attend one of the other sessions that has available space within the next week. Missed labs cannot be made up after the end of the week following the scheduled lab.
Week# - Monday’s Date - Experiment/Activity
9. Oct 24 Exp 21: Calorimetry
10. Oct 31 Exp 11: Periodic Table and Periodic Law
11. Nov 7 Dry lab 3: Atomic Structure
12. Nov 14 Exp. 5: Chemistry of Copper
13. Nov 21 Thanksgiving Week – no lab. Writing Assignment due Monday.
14. Nov 28 Exp. 19: Calcium Carbonate Analysis
15. Nov 5 Exp 18: molar Mass of a Volatile Liquid
16. Nov 12 Finals Week – No Laboratories
Lab Grading: Text: Beran - Laboratory Exercises Wiley Publishing.
The laboratory grade is included in the
course grade. ***It is MANDATORY that
you attend and pass the laboratory. Failing
to complete two or more laboratories, or earning a failing grade in the
laboratory may result in a failing grade for the class.
Periodic Table source: http://dph1701.tripod.com/chemistry/smallelements.htm