HOUSTON COMMUNITY COLLEGE SOUTHWEST (Stafford & West Loop Campuses )
COURSE OUTLINE FOR CHEM 1412 – General Chemistry II
Spring, 2011
Class Number 76836/76744
Time and location
5:30 – 8:30 Mon/Wed (Rooms 121/109, lab) Stafford Campus
5:30 – 9:30 Tue/Thu (Rooms151/164, lab) West Loop Campus
Instructor
Albert D. Kweyete
Office Hours: Before Class
Office Phone: 713-718-6771
E-mail: Albert.kweyete@hccs.edu
Web sites:
http://learning.swc.hccs.edu/members/albert.kweyete
http://learning.swc.hccs.edu
Textbook
Chemistry, 10th Edition, by Raymond Chang. McGraw-Hill: 2007.
TBA (Hardcover Edition)
“Split” soft cover versions are available at HCC bookstores.
Laboratory Manual
HCCS SW Chemistry Lab Manual, Custom Laboratory Program
for Chemistry 1411 &1412 Cache House 2008
Optional Study Guide and Solutions Manual
Student Study Guide for Chemistry, 9th Edition, by Kim Woodrum. McGraw-Hill: 2007.
Student Solutions Manual for Chemistry, 9th Edition, by Brandon J. Cruickshank and Raymond Chang.
McGraw-Hill: 2007.
Optional Study Guide
Student Solutions Manual to accompany Chemistry, Ninth Edition, prepared by Brandon Cruickshank. McGraw
Hill.
Course Catalog Description
Continuation of CHEM 1411. Topics include solutions, chemical kinetics, equilibrium and equilibrium
phenomena in aqueous solution, acids and bases, pH, thermodynamics, electrochemistry, nuclear chemistry, and
introduction to organic chemistry, and biochemistry. The laboratory includes appropriate experiments.
Prerequisites: CHEM 1411 Credit: 4 (3 lecture, 3 lab)
Course Prerequisites
These are stated in the course description in the HCC catalog (quoted just above) and they are stressed again here
for emphasis. Lack of satisfactory completion of the course prerequisites are one of the main reasons that cause
students to do poorly in chemistry. Basic math and problem solving skills at the level of college algebra are
essential. If you are not sure if your prior coursework meets these prerequisites, come and talk to me or to the
department chair for advice. With the prerequisites satisfactorily completed (preferably with a grade of B or
better), you can be confident that you are well-prepared for this course.
Course Intent
This course is intended for students majoring in one of the physical sciences or life sciences, or for students who
are pursuing pre-professional programs in medicine, dentistry, pharmacy, veterinary medicine, or other health
programs. The course is also beneficial to students who are preparing themselves for higher level science courses
in their respective curricula.
Course Content
See the course schedule below for the topics (listed by chapter title) that will be covered in this class. College
level general chemistry is very similar to a good high school course, but will usually cover the topics in greater
detail and will place a greater emphasis on problem solving.
Attendance Policy
The HCCS attendance policy is stated in the College Catalog or Handbook: “Students are expected to attend
classes regularly. Students are responsible for materials covered during their absences, and it is the student's
responsibility to consult with instructors for make-up assignments. Class attendance is checked daily by
instructors. Although it is the responsibility of the student to drop a course for non-attendance, the instructor has
full authority to drop a student for excessive absences. A student may be dropped from a course for excessive
absences after the student has accumulated absences in excess of 12.5% of the hours of instruction (including
lecture and laboratory time).”
Note that 12.5% is approximately 2 classes or labs for a 4-semester hour course, such as this one, which
meets 4 times per week in a 5-week semester. If circumstances significantly prevent you from attending classes,
please inform me. I realize that sometimes outside circumstances can interfere with school, and I will try to be as
accommodating as possible, but please be aware of the attendance policy.
Student Learning Outcomes
The student will be able to:
1. Distinguish between the different ways of measuring concentrations of solutions, and relate concentration to
the colligative properties of solutions.
2. Determine and analyze the rates of chemical reactions.
3. Write equilibrium constant expressions for chemical reactions and calculate the value of the equilibrium
constant and the concentration of reactants and products at equilibrium.
4. Demonstrate proficiency in acid-base and solubility product calculations.
5. Express the three laws of thermodynamics and interrelate the enthalpy, free energy and equilibrium constant
for the reaction.
6. Based on the principles of oxidation and reduction, balance oxidation-reduction reactions, calculate cell
potentials of voltaic cells based on oxidation-reduction reactions, and make quantitative calculations based on
electrolysis.
7. Identify modes of radioactive decay, balance nuclear reactions, calculate energy changes associated with
nuclear reactions, and relate quantities of radioactive elements with time based on the kinetics of nuclear
processes.
8. Classify, name, and draw the structure of basic organic compounds; student can write chemical reactions of
alkanes, alkenes, and alkynes.
Learning Objectives:
Students will:
1.1. Relate the concentration of solutions to their colligative properties.
1.2. Determine if two compounds will mix to form a solution or not based on their structures.
1.3. Given the mass of a solute and the volume of a solution or the mass of the solvent, calculate the relevant
concentration (molarity, molality, percent concentration, mole fraction, or ppm). Convert a given
concentration from one concentration unit to another.
1.4. Determine the molecular weight of an unknown solute, given the value of a colligative property.
2.1. Determine the average rate and instantaneous rate of a reaction from concentration-time data.
2.2. Determine the order of a reaction with respect to each reactant and write the rate law for the reaction.
Determine the value of the rate constant, k.
2.3. Write the integrated rate law of first and second order reactions and use the rate law to relate concentration
of
the reactant with reaction time, rate constant, and half-life.
2.4. Given different initial reactant concentrations and the respective initial rate of the reaction, determine the
value of the exponents in the rate law and the value of the rate constant.
2.5. Relate the effect of temperature and activation energy to reaction rate using the Arrhenius equation.
2.6. Relate the rate law to the mechanism of the reaction and to the molecularity of the elementary reactions
comprising the mechanism.
3.1. Write the equilibrium constant expression for homogeneous and heterogeneous reactions.
3.2. Given one or more concentrations at equilibrium, calculate the value of the equilibrium constant for the
reaction and/or the equilibrium concentrations of the other substances in the reaction.
3.3. Given one or more initial concentrations, calculate the concentrations of the reactants and products at
equilibrium and/or the value of the equilibrium constant, using the "ICE" table method.
3.4. From the value of the reaction quotient, Q, determine whether a reaction is at equilibrium, and if not, which
direction the reaction will initially proceed in order to reach equilibrium.
3.5. Apply LeChâtelier’s Principle to determine the effects of changes in concentrations, temperature on
compositions of equilibrium mixtures.
4.1. Know the three different definitions and principles of acids and bases (Arrhenius, Bronsted-Lowry, and
Lewis).
4.2. Calculate [H+], [OH–], pH, and pOH.
4.3. Use dissociation constants for weak monoprotic acids and bases to determine the pH of their aqueous
solutions.
4.4. Differentiate between acidic, basic and neutral salts and determine the pH of aqueous solutions of salts.
4.5. Understand the common ion effect and its relevance to buffers; determine the pH of buffered solutions
using the Henderson-Hasselbalch equation.
4.6. Calculate the pH at various stages of titration curves for (i) strong acids & strong bases, (ii) weak acids &
strong bases, (iii) strong acids & weak bases.
4.7. Write solubility product expressions and interconvert between the solubility constant, Ksp and
concentrations
of dissolved ions in saturated solutions of slightly soluble salts.
4.8. Given Ksp, determine whether precipitation will occur when two aqueous solutions of salts are mixed that
react to form a sparingly soluble salt.
5.1. Express the concept of entropy and predict the sign of the entropy change for a given reaction.
5.2. Calculate the entropy change of a reaction using Hess's law or standard entropies.
5.3. From the Gibbs equation, relate and calculate the values of the entropy, enthalpy, free energy, and
temperature of a reaction.
5.4. Relate and calculate the value of the equilibrium constant to the entropy, enthalpy, free energy and
temperature of the reaction.
6.1. Determine the oxidation state of elements in compounds.
6.2. Based on changes in oxidation states, determine which substance in a reaction is oxidized and which is
reduced.
6.3. Balance oxidation-reduction reactions in acidic and basic solution using the method of half-reactions.
6.4. Sketch voltaic and electrolytic cells, identifying the anode, cathode, anode compartment, cathode
compartment, salt bridge, and direction of electron flow.
6.5. Calculate standard cell potentials from standard reduction potentials.
6.6. Rank reducing agents and oxidizing agents based on standard reduction potentials.
6.7. Determine non-standard cell potentials from standard cell potentials using the Nernst equation.
6.8. Interconvert between time, current, and masses of reactants and products in electrolysis processes.
7.1. Identify common modes of radioactive decay.
7.2. Write balanced nuclear reactions.
7.3. Differentiate between the different modes of decay and predict the likely mode of decay.
7.4. Interconvert between rates of nuclear decay, half-lives of radioactive nuclei, and amounts of radioactive
nuclei.
7.5. Determine energy changes of nuclear reactions and stability of nuclei using Einstein’s equation.
7.6. Distinguish between subcritical, critical, and supercritical masses; contrast nuclear fission with nuclear
fusion processes.
7.7. Identify the major components and principle of operation of nuclear reactors.
8.1. Given the structure, name alkanes using the IUPAC rules of nomenclature, and vice-versa.
8.2. Classify organic compounds based on the functional group present in their structures.
8.3. Given the structure, name alkenes and alkynes using the IUPAC rules of nomenclature, and vice-versa.
8.4. Optional if time permits. Write combustion and halogenation reactions of alkanes; write addition reactions
of alkenes and alkynes
Last Day for Administrative and Student Withdrawals
See table inserted. After the withdrawal date no W can be given, you must receive a regular grade (A-F) in
the course. I urge any student who is contemplating withdrawing from the class to see me first! You may be
doing better than you think. Either way, I want to be accessible and supportive. I believe in each and everyone in
this class to be responsible and would not want to be put in a position to drop a student from the class.
If you need assistance, do not hesitate to contact me (my phone number and e-mail address are listed above). I'm
here to help.
IMPORTANT NOTICE:
Students who repeat a course three or more times may soon face significant tuition/fee increases at HCC and
other Texas public colleges and universities. If you are considering course withdrawal because you are not
earning passing grades, confer with your instructor/counselor as early as possible about your study habits,
reading and writing homework, test-taking skills, attendance, course participation, and opportunities for
tutoring or other assistance that might be available.
Disability Support Services (DSS)
HCCS is committed to compliance with the American with Disabilities Act and the Rehabilitation Act of 1973
(section 504)
"Any student with a documented disability (e.g. physical, learning, psychiatric, vision, hearing, etc.) who
needs to arrange reasonable accommodations must contact the Disability Services Office at the respective
college at the beginning of each semester. Faculty are authorized to provide only the accommodations
requested by the Disability Support Services Office."
If you have any special needs or disabilities which may affect your ability to succeed in college classes or
participate in college programs/activities, please contact the office of disability support services at the college.
Upon consultation and documentation, you will be provided with reasonable accommodations and/or
modifications. Please contact the DSS office as soon as you begin the term. For questions, contact Donna Price
at 713 718 5165 or the Disability Counselor at HCC-Southwest: Dr. Becky A. Hauri at 713 718 7909; also see
page 5 of the Schedule of Classes ’Fall 08’ for additional DSS numbers.
Also visit the ADA web site at: http://www.hccs.edu/students/disability/index.htm. Faculty Handbook/
Faculty Orientation is also available at http://www.hccs.edu/students/disability/faculty.htm
Academic Honesty
Students are responsible for conducting themselves with honor and integrity in fulfilling course requirements.
Disciplinary proceedings may be initiated by the college system against a student accused of scholastic
dishonesty. Penalties can include a grade of "0" or "F" on the particular assignment, failure in the course,
academic probation, or even dismissal from the college. Scholastic dishonesty includes, but is not limited to,
cheating on a test, plagiarism, and collusion.
Laboratory Policy
On the first day of lab a safety video will be shown (about 35 min long) and a safety "quiz" will be given and
reviewed. Each student will then sign a statement affirming his or her commitment to following safe procedures
in the laboratory, and turn the form in to the instructor. You should be especially aware of the need for adequate
eye protection and proper dress in the laboratory. Glasses or goggles must be worn at all times during the
laboratory period. Any student not wearing glasses or goggles after the experiment has begun may be given a zero
for that experiment! Experiments will be performed in groups of up to two students each. Before you leave the
lab, be sure to show me your report so I can review and initial it. Each student should arrive at the lab on time,
with his or her lab manual. Laboratory reports are due on or before the next lab experiment. Each report must be
done individually, but of course you can work with your lab partners. If you are not sure about a calculation or a
particular section, always feel free to ask me about it! Each report will be graded in 3 parts: the pre-lab, exercise
report and the post-lab. Submit the pre-lab before the lab exercise begins and both the exercise report and post-lab
the following week the lab was completed. Come to lab prepared. Read through the experiment beforehand, and
review the pre-lab questions and answer them in the lab manual. You will be much better organized when doing
the experiments, and your laboratory experience will be much more rewarding!
Exams, Quizzes, and Make-up Policy
Examinations will consist of three non-cumulative regular exams (45%) plus a comprehensive final (20%).
Make-up exams will not normally be given, so make every effort to take the exams on their scheduled dates. In
the event that you must miss one and only one regular exam, the final exam grade may be substituted for the
missed exam. Remember that the final exam will be comprehensive and is usually more difficult than the regular
exam (meaning that it will cover all of the material from the whole semester, not just the last part). If you do not
miss any of the regular exams, I will replace your lowest exam score with your final exam score if the final exam
grade is higher.
During the semester I will periodically give a short chapter quiz at the beginning of class. I will drop the lowest
quiz grade. The remainder will count as a regular exam grade (15%) which cannot be dropped. These quizzes are
highly beneficial for learning the material and are intended to help you in this regard.
Please note:
1) All students are required to take the final (no student can be exempted),
2) After the withdrawal date, a grade of W cannot be given.
Grading
The overall score is based on the following:
Three Regular Exams
Quiz Grade
45%
15%
Laboratory
20%
Final Exam
20%
Overall Score = 0.45(Average of three regular exams) + 0.15(Quiz Grade) + 0.20(Laboratory grade) +
0.20(Final Exam)
The course grade is then obtained from the overall score:
Final Average
Letter Grade
90 - 100
A
80 - 89
B
70 – 79
C
60 – 69
D
SPRING - TRADITIONAL 16-WEEK SEMESTER
November 1 Monday Online Registration Begins
November 18 Thursday Application Deadline for International Students Outside the U.S.
December 1 Wednesday Veterans Last Day to Apply for Advance Pay
December 20 – 31
Offices Closed - Christmas Break
January 4 Monday On-Campus Registration Begins
January 14 Thursday Last Day for 100% Refund
January 17 Monday Offices Closed - Martin Luther King, Jr. Observance
January 18 Tuesday Classes Begin - Drop/Add/Swap Fee ($15.00) Begins
January 18- February 3 70% Refund
January 19 Wednesday Registration Ends
January 19 Wednesday Last Day for Drop/Add/Swap
January 31 Monday Official Date of Record
February 4-9
25% Refund
February 15 Tuesday Priority Deadline for Spring Completion of Degrees or Certificates
February 21 Monday Office Closed – President Day Holiday
March 14- 20 Mon-Sun Offices Closed - Spring Break
April 14 Thursday Veteran’s Advanced-Pay Application Deadline for Summer Session
April 15 Friday Deadline for Spring Federal Student Loans
April 21 Thursday Last Day for Administrative/Student Withdrawals - 4:30 pm
April 22-24 Fri-Sun Office Closed – Easter Holiday
May 8 Sunday Instruction Ends
May 9 –16 Mon - Sun Final Examinations
TBA
Graduation Exercises
May 15 Sunday Semester Ends
May 16 Monday Grades Due by - 12:00 Noon
May 20 Friday Grades Available to Students
< 60
F
Other Information
Free chemistry tutoring is available. A tutoring schedule will be posted in the classroom and lab and will also be
placed on my web site and departmental web site. There are many interesting chemistry resources on the Internet.
These are interesting and informative, but spending long hours searching for sites or waiting for graphics intensive
sites to load, is not beneficial! Your best immediate source of information is your textbook - make thorough use of
it.
General Suggestions
Chemistry is a vast field, ranging from the study of simple inorganic salts to enormously complex molecules such
as enzymes and nucleic acids in living organisms. In this course, the major topics we will be covering are
Chemical Formulas, Reactions, and Stoichiometry Calculations, Chemical Thermodynamics, Electron
Configuration and Chemical Bonding, Gas Laws, and Solutions. As you might suspect, it can be easy to fall
behind and, as a result, to not be ready for the exams. Following are some general tips that may be helpful:
Learning chemistry takes time. A reasonable guide is to allow yourself two hours of study for each hour
of lecture. Heavy work and/or class loads are not compatible with learning chemistry!
Attend class regularly (!) and take generous notes during class. Ask questions.
When beginning a new chapter, I recommend that you read through it quickly the first time, just to give
yourself a good feel for what it is about. I you are really on the job you will have done this before the
class lecture on the chapter! You will understand what's going on in class much better if you do this.
Next, start tackling the end of chapter problems! Often, working problems facilitates understanding
much better than just reading and rereading the chapter itself. Chemistry is a "hands on" course working problems is essential. However, do not spend an inordinate amount of time on a single problem
- skip it for the time being and go on to another. Try working some of the sample exercises. They are
worked out in the chapter and are very helpful.
Get a good, scientific calculator that has scientific notation ("EE" or "EXP" key), log, ln, x2, , etc.
Business calculators usually do not have all of these features. I still use a good old' TI-36 Solar myself.
Review basic math operations such as properties of logarithms, if you are rusty.
Study groups can be very helpful. Keep the group small though, no more than three or four people.
Finally, keep a positive attitude! Chemistry can be hard, but with the right attitude and approach, you
will succeed in mastering it!
I hope you find chemistry to be an interesting and rewarding subject which will not only be useful in your
academic major, but will give you a better insight into the many scientific challenges we are facing today. I look
forward to working with you this semester!
Wed/Thu (Lab)
Week 1
Lab Rules & Safety
Chapter 12
Physical Properties of
Solutions
Tentative Schedule: SPRING 2011
Mon/Tue (Lecture)
Wed/Thu (Lab)
Week 2
Week 2
Chapter 12
Lab 11(Reactions in
Physical Properties of
Aqueous Solutions
Solutions
Mon/Tue (Lecture)
Week 3
Chapter 13 Chemical
Kinetics
Week 3
Lab 12 (Colligative
Properties: Freezing
Point Depression and
Molar Mass
Week 4
Chapter 14 : Chemical
Equilibrium
Week 5
Lab 14. Acid-Base
Properties of Salt
Solutions: Hydrolysis
Week 6
Chapter 15: Acids and
Bases
Week 7
Lab 16. Determination
of the dissociation
Constant of a weak Acid
Week 8
Chapter 18: Entropy, Free
Energy and Equilibrium
Week 8
Lab.17 Identification of
an Unknown Cation;
Development of An
Analysis Scheme
Week 9
Exam 2: Chapters
(15, 16, 18)
Week 9
Lab. 19 Molecular
Geometry: Experience
with Models (Take
Home Lab.)
Week 10
Week 10
Chapter 19:
Electrochemistry
Lab 20. Preparation of
Aspirin
Week 11
Chapter 23: Nuclear
Chemistry
Week 12
Chapter 24 Organic
Chemistry
Week 13
Make up lab / Misc
Week 12
Chapter 24 Organic
Chemistry
Week 4
Lab 13 Rate of a
chemical Reaction
Week 6
Lab 15. Determination
of purity of Potassium
Hydrogen
Phthalate(KHP)
* This date is subject to change or modification
Important Dates
Exam 1 (Chapters 12, 13, 14)
Exam 2 (Chapters 15, 16, 18)
Exam 3 (Chapters 19, 23, 24)
Comprehensive Final Exam (All Chapters)
Week 5
Exam 1: Chapters
(12,13,14)
Week 7
Chapter 16: Acid-Base
Equalibria and Solubility
Equilibria
Week 13
Exam 3 Chapters
(19,23,24)