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CHE 112 |
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CHE 112 - GENERAL CHEMISTRY II |
INSTRUCTOR: J. PADULA |
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HOME | SYLLABUS | CONTACTS | LECTURE NOTES | ASSIGNMENTS |
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SYLLABUS - SPRING 2012
Jan Padula
Phone: 562-4335
Office: 217T
e-mail: Padula's Contact Information
Catalog Description: This is the second semester course in a two-semester sequence which presents the basic laws and concepts of general quantitative chemistry. This course will focus on the principles of reactivity of solids, liquids and gases with respect to chemical kinetics, chemical equilibrium, acid-base chemistry, precipitation reactions, entropy, free energy, red-ox chemistry, and an introduction to nuclear chemistry. There are three hours of lecture and one two-hour laboratory per week. Pre-requisite: CHE 111 or equivalent.
General Education Learning Outcomes: Students will demonstrate the ability to:
1. understand the methods scientists use to explore natural phenomena, including:
§ observation
§ hypothesis development
§ measurement and data collection
§ experimentation
§ evaluation of evidence
§ employment of mathematical analysis
2. apply scientific data, concepts and models in one of the natural sciences
Course Objectives: As the result of instructional activities, students will be able
to:
1. use appropriate chemical terminology and nomenclature to effectively communicate their understanding of concepts in chemistry
2. describe the phases of matter and their molecular and elemental properties
a. define the Basic Gas Laws
b. perform calculations using Boyle’s, Charles, Gay-Lussac’s and the Ideal Gas Laws
c. define partial pressure and Dalton’s Law
d. define the Kinetic-Molecular Theory of Gases
e. define the Real Gas Law behaviordescribe the difference between diffusion & effusion
f. define the properties of liquids in terms of vapor pressure, boiling, surface tension, capillary action & viscosity
g. distinguish between the intermolecular forces involving polar molecules
h. distinguish between the intermolecular forces involving non-polar molecules
i. distinguish between different types of solids
j. draw a phase diagram and label it completely
3. define the units of concentration
a. calculate molarity, molality, mole fraction, weight percent, and ppm
b. convert concentrations from one unit to another
4. explain solubility of solutions
a. describe the process of liquids dissolving in liquids
b. describe the process of solids dissolving in liquids
c. define factors that affect solubility of gases dissolved in liquids in terms of Henry’s Law
d. calculate the enthalpy of solutions from thermodynamic data
5. describe colligative properties of solutions
a. calculate Raoult’s Law for changes in vapor pressure
b. determine the boiling point elevation, freezing point depression and use colligative properties to calculate variables present in these relationships (molar mass and molality)
6. distinguish between the different types of colloids
a. identify and explain how a surfactant works
b. define osmotic pressure
7. determine rates of chemical reactions
a. determine order of reactions calculate and graph first-order reaction kinetic data
b. calculate and graph second-order reaction kinetic data
c. calculate and graph zero-order reaction kinetic data
d. calculate and graph half-life for first, second & zero-order reactionswrite a rate equation
e. determine the rate constant (k)
f. calculate R (rate) using a rate law expression and k
g. describe reaction conditions that determine reaction rates
8. explain Collision Theory
a. distinguish between the effect concentration and temperature has on reaction rates
b. calculate activation energy using the Arrhenius Equation
c. define the function of a catalyst and the effect it has on reaction rates
9. describe reaction mechanisms
a. describe molecularity and rate equations for elementary steps
b. define molecularity and reaction order
c. determine reaction mechanisms from kinetic data
10. define chemical equilibrium
a. write an equilibrium constant expression for a balanced equilibrium reaction
b. define the meaning of the equilibrium constant K
c. determine the reaction quotient Q for a reaction
d. use equilibrium constants in calculations
11. explain Le Chateliers Principle
a. explain the effects of the addition or removal of reactants or products
b. explain the effects of volume changes on gas-phase equilibria
c. explain the effects of temperature changes on equilibria
12. define acids and bases in terms of Arrhenius, Bronsted-Lowry and Lewis
a. describe basic properties of acids & bases
b. determine conjugate acid base pairs
c. explain cationic & molecular Lewis acids and Lewis bases
13. describe the self ionization of water and Kw
a. describe and calculate Ka & Kb in acid base equilibria
b. predict the direction of an acid base equation
14. define the pH scale and calculate pH using logarithms and Kw
a. determine the relationship of acid-base reactions with respect to strength of each reactant
b. perform an acid base titration
15. define pKa and calculate using the Henderson-Hasselbach equation
16. determine the molecular structure, bonding and behavior of acids and bases
a. determine the acid strength of metal halides
b. compare strengths of oxoacids
c. describe carboxylic acids and draw its functional group
17. define the common ion effect
a. calculate concentration and pH of buffered solution
b. construct a pH titration curve
18. define solubility of slightly soluble salts and determine Ksp
a. explain the effect of basic anions on salt solubility
19. define entropy & free energy
a. calculate standard enthalpy values
b. summarize spontaneous reactions
c. calculate Gibbs free energy
d. define standard free energies of formation
20. define oxidation-reduction reactions
a. balance red-ox equations
21. describe simple and commercial voltaic cells
a. draw a voltaic cell from electrochemical cell notation
b. define dry cells and alkaline batteries
c. describe a fuel cell
22. determine standard electrochemical potentials
a. use a table of standard reduction potentials
b. describe relative strengths of oxidizing and reducing agents
c. define the Nernst equation
23. define natural radioactivity
a. determine rates of nuclear decay
b. write balance nuclear equations
c. describe the difference between nuclear fission and nuclear fusion
24. describe the kinetics of nuclear decay
a. calculate half-life of a nuclear reaction
b. describe carbon dating
c. define nuclear medicine and explain its uses
25. define the processes, pros and cons of nuclear energy
Laboratory Objectives: The laboratory experience will reinforce the understanding that experimental work is the foundation of chemical knowledge and which requires fundamental laboratory skills. Students will:
1. anticipate, recognize, and respond properly to potential hazards in laboratory procedures
a. complete laboratory safety training as designed by the CCC science department
b. review the contents of MSDS & location of MSDS sheets storage area
2. keep accurate and complete experimental records
a. write all lab records in a bound lab notebook using Proper Lab Documentation (PLD) as required for Good Lab Practices (GLP)
b. enter all data as it is generated in the lab
3. perform accurate quantitative measurements
a. use properly calibrated instruments (i.e. spectrophotometers) and volumetric glassware
4. interpret experimental results and draw reasonable conclusions
a. record in the lab notebook all information/data using tables, graphs, formulas and calculations
b. write a conclusion of results in the lab notebook at the end of each lab to summarize what was discovered in the laboratory
5. communicate effectively through oral and written reports
a. write 5 formal lab reports – Freezing Point Depression, Iodine Clock, Le Chatelier’s Principle, Acid/Base Titration of an Unknown Acid, and pH Titration Curve
b. write 2 Standard Operating Procedures (SOP’s) – Calibration of a pH Meter and Calculations of Buffered Solutions
c. perform 2 oral laboratory presentations/demonstrations – Solids, Liquids & Gases and Electrochemistry
d. report required information such as tables, graphs, formulas, calculations background and summary in electronic format
e. use Excel, Word and PowerPoint to present laboratory data and reports to the instructor and classmates as required
6. analyze data statistically, assess the reliability of experimental results, and discuss the sources of systematic and random error in experiments
a. use statistical interpretation as needed in the summary of lab information and required lab reports
b. include correlation of data on all graphs via electronically generate linear trend lines
7. plan & execute experiments through the use of appropriate chemical literature & electronic resources
a. research background information required for labs and lab reports from reputable sources such as American Chemical Society (ACS) or .edu, .org, and .gov websites
Course Design: This course will be presented by a series of lectures, demonstrations, interactive computer exercises, journal articles, and laboratory experiments. A term paper, lab reports, and chapter exams will constitute the final grade. The grading scheme is as follows:
5 Module exams @ 100 points = 500 points
Homework & Quizzes
varied = 100 "
Term paper outline @ 50 points = 50 "
Term paper @ 100 points = 100 "
15 Graded Labs varied = 250 "
Final grade total 1000
points / 100 = grade
Text and materials: Kotz, John C., Treichel, Paul M., & Townsend, John R., Chemistry & Chemical Reactivity, 7th ed., Thomson Brooks/Cole, 2009. textbook (e-books are okay) , a scientific or graphing calculator, a bound composition notebook with graph paper pages for lab, safety glasses, and a straight edge are all required for this course. Study groups are required!
Attendance:
It is extremely important to attend all classes, labs and sessions. In order to be successful in this course, you
are expected to spend at least (on average) an additional 15 hours per week
reading the textbook, doing the assignments, writing up your labs and preparing
for/completing your exams. The College policy states that students must attend
class regularly. Students who miss more than 15% of classes may be withdrawn
from the course or given a grade of "F". Attendance will be marked during the first
few minutes of class. Entering the classroom late is disruptive to me and to
other students. Please make every effort to be on time.
Attending class is defined in this course as arriving on time,
remaining in the classroom until the end of class, and being attentive and not
engaging in disruptive or distracting behaviors.
Attention and Distractions
On the days you attend class, you should
plan to be fully present and focused on class for the entire period. Cell
phones must be OFF, not on vibrate or silence. Talking to others, sleeping,
and any other behaviors that do not contribute to your learning or could
distract other students are included under this policy
Disruptive or distracting behavior will result in the student
being marked absent for the day.
Students will be informed at the end of class or via email when this
policy is enforced to avoid any further disruption to the class.
Note: Refer to your student handbook for policies that pertain to attendance, academic integrity, and behavior. Please understand your work must be your own. YOUR LAB REPORTS MUST BE WRITTEN BY YOU; NOT AS A JOINT REPORT WITH YOUR LAB PARTNER. I have a zero tolerance for anyone caught cheating or plagiarizing work. In order to understand what constitutes plagiarism, check out the following websites:
http://www.indiana.edu/~wts/pamphlets/plagiarism.shtml
http://owl.english.purdue.edu/handouts/research/r_plagiar.html
I hope you enjoy this class! Do not hesitate to seek help from me, tutors in the Academic Assistance Center or fellow classmates to clarify course materials. Study groups work very well in this course. If you need help finding a study partner, just tell me.
If you have or suspect that you may have, any type of disability or learning problem that may require extra assistance or special accommodations, please speak to me privately as soon as possible so I can help you obtain any assistance you may need to successfully complete this course. You should also contact Laurie Bethka, Room 420M in the Academic Assistance Center, for further assistance.
If you have any allergies to chemicals or latex, suspect that you may be pregnant or have an illness or condition that may be complicated by working in the lab, please let me know. I can remove you from handling chemicals in certain labs depending on the situation.
Course Outline by General Topics:
Chapter 1-10, Brief Review of General Chemistry I
Chapter 11, Gases & Their Properties
Chapter 12, Intermolecular Force & Liquids
Chapter 13, Chemistry of Solids
Chapter 14, Solution Chemistry
EXAM 1
Chapter 15, Chemical Kinetics
EXAM 2
Chapter 16, Chemical Equilibrium
EXAM 3
Chapter 17, Acids & Bases
Chapter 18, Aqueous Ionic Equilibrium
EXAM 4
Chapter 19, Free Energy and Thermodynamics
Chapter 20, Electrochemistry
Chapter 23, Radioactivity and Nuclear Chemistry
EXAM 5
**I hope you enjoy
this class! Do not hesitate to seek help
from me, tutors in the
LABORATORY EXERCISES
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DATE |
NUMBER |
TITLE of LAB EXERCISE |
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1/27 |
LAB 1 |
Introduction, Lab Safety, MSDS & Orientation (PLD) |
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1/31 |
LAB 2 |
Solids, Liquids & Gases |
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2/7 |
LAB 3 |
Freezing Point Depression |
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2/14 |
LAB 4 |
Solutions & Preparation of Solutions for Iodine Clock |
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2/21 |
LAB 5 |
Iodine Clock Reaction |
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2/28 |
LAB 6 |
Iodine Clock Calculations |
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3/6 |
LAB 7 |
Reaction Mechanisms |
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3/20 |
LAB 8 |
Le Chatelier’s Principle – Haber-Bach Process |
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3/27 |
LAB 9 |
Standardization of NaOH |
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4/3 |
LAB 10 |
Acid /Base Titration of an Unknown Acid |
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4/10 |
LAB 11 |
Calibration of a pH Meter |
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4/17 |
LAB 12 |
pH Titration Curve |
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4/24 |
LAB 13 |
Preparation & Calculations of Buffered Solutions |
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5/1 |
LAB 14 |
Energy Presentations |
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5/8 |
LAB 15 |
Chernobyl & the Nuclear Regulatory Commission |
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TBA |
Presentation of Term Papers |
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Please note that you are required to record all of you lab experiences in pen
(blue or black permanent ink) and glue all attachments in with acid free
glue into a bound lab notebook.
Chemistry Research Paper – SPRING 2012
A six to ten page term paper on any current research in CHEMISTRY that interests you is to be organized and written over this semester. This is NOT a history paper on a general topic. The research may be ongoing or recently completed. You will report the information as you are part of the research team. The schedule for this TERM paper is as follows:
¨ Bibliographic Instruction in the Douglas Library - Friday, Feb. 3
¨ Topic approved by me no later than – Tuesday, Feb. 7
¨ Extensive outline (50 points) due no later than noon – Friday, Feb.24
¨ Final paper (100 points) due no later than – Friday, April 27
The paper must have at least 5 references, 2 may be from the Internet - but beware that your Internet sources are reputable. The other three sources must be from a current book and/or scientific journal. All sources must be properly referenced by either APA or ACS depending on your choice, and must be consistent throughout the paper. (See grading matrix below.)
Journals that are strongly suggested are as follows:
Science
Science News
Discover
Chemical & Engineering News
Nature
To start the paper, ask yourself a question concerning a specific research topic in chemistry. Develop your paper by answering your question. It’s easier to focus in on a narrow topic rather than staying too broad. Some topics of interest are but not limited to the following:
Chemical/Industrial
Processes
Physical Chemistry
Forensic Chemistry
Atmospheric Chemistry
Nutrition, Health, or Medicine
Genetics
Environmental Issues
Chemical Technology
The paper must be structured in the following way and appear so in the outline.
1. Introduction – This should contain a discussion of the question or problem that is to be presented in the paper. ex. What current research is being done on "state-of-the-art control technology" used to sequester CO2 in coal-fired electrical power generation and how is it expected to work?
2. General Background – This section should include a discussion of the chemicals pertinent to your topic. Chemical structure, molecular weight, physical and chemical properties, general reactivity, and reaction mechanisms are all part of this section.
3. Current Research & Theoretical Perspectives– You should discuss the current research being done on this topic as well as theories that are used to explain the research topic as presented by the researcher. (This is the bulk of your paper.)
4. Opinion – What is your perspective on the "science" of this topic? You should discuss your agreement or disagreement with the information, research, and approach with respect to the current research and theoretical perspectives. A discussion on ethics relative to this topic could also take place in this portion of the paper if applicable.
5. Conclusion – Wrap the paper up into a final discussion or summary that serves as an overview of the question or statement made in your introduction.
6. Bibliography - must be complete and follow the style writing you chose to use in the paper.
CHEMISTRY 112 - TERM PAPER
Acceptable topic - Graded as follows:
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Component |
Possible Points |
Your Score |
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Validity of Sources |
10 |
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References Cited |
10 |
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Format |
20 |
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Content |
50 |
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Spelling & Grammar |
10 |
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TOTAL |
100 |
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Presentation:
COMMENTS:
If you need to contact me, go to Padula's Contact Information.
Last Updated: 01/27/2012