Syllabus for Chem111.001
Fall 2010
Instructors: Liina Ladon
Office for Ladon: SM538
Lecture: MoWeFr 10:00am – 11:50am in SM506 Lab Lecture: W 11:00am -11:50am
Lab: W 12:00am – 1:50 pm in SM507
in SM508
Phone: 410-704-3054
E-mail: lladon@towson.edu
Office hours: By appointment
Web page: www.towson.edu/~ladon
Required Materials:
Lecture Textbook: General Chemistry, Raymond Chang, 5th ed., McGraw-Hill, Boston,
2008, ISBN 978-0-07-304851-2. If you took CHEM110 last semester, it is the same book.
Lab Textbook: Laboratory Experiments In General Chemistry: CHEM110 and CHEM111,
Version 8.0, 2005, Towson University. This is an “in-house” manual. Make sure you get the
correct version. If you took CHEM110 last semester, it is the same manual.
Laboratory Goggles: Must be ANSI approved and cover the eyes completely. The chemistry
club sells goggles for $10.00. They are cheaper and more comfortable than the goggles sold
at the university bookstore. Hopefully, most of you have them from CHEM110.
Laboratory Notebook: Must have carbon copy pages that can be turned in as a duplicate of
what has been recorded in the notebook. These are also sold by the chemistry club ($11.00),
and at a price that is cheaper than the bookstore. You may use the same notebook from
CHEM110, if you have pages leftover.
Calculator: A nonprogrammable scientific calculator is required for the course. The
calculator should be able to display scientific notation, be able to take roots of numbers, raise
numbers to any power, take logarithms and antilogarithms in base 10 and base e. I will not
allow TI8x or TI9x type calculators for this course due to increasing incidence of students
storing illegal information in the memory these calculators. I suggest a calculator, such as
the TI36X, which is solar (no batteries needed) and simpler to operate than the
programmable calculators. Note: Palm pilots and cell phones may not be used for exams!
Attendance:
Prompt attendance is strongly recommended. If you are late or miss a lecture, it is your
responsibility to acquire information given out during lecture. Make-up exams will not be
given. In the event an exam is missed the final exam will be weighted an additional 10% to
cover points missed. Quizzes will be given once a week. I will drop the lowest 3 quizzes. If
you miss taking a quiz, then it becomes one of the quizzes dropped. Please turn off cell phones
and MP3 players while in class out of consideration for your classmates. You can’t take notes or
pay attention in class if you are texting. Also, class time is not a social hour. Please refrain from
casual conversation during class time.
Students should not attend classes or other university events from the onset of flu-like symptoms
until at least 24 hours after the fever subsides without the use of fever reducing medications.
Such absences will be considered excused absences; however, students are responsible for the
material covered during the period of their absence.
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Blackboard website:
I will be using Blackboard, an online information hub for coursework. I hope to post useful
information, announcements, and have a chance for you use the discussion board for help from
your classmates or myself on course material. Any suggestions from those of you who have
used Blackboard in the past are welcome! Most of you should already have been enrolled into
Blackboard by PeopleSoft when you registered for the class. To access Blackboard, launch your
browser and open http://learnonline.towson.edu. Click the Courses tab and locate this course
using either the course ID or my name.
Lab Reports:
Lab reports will be due at the beginning of the performance of the next experiment. Any reports
handed in after the due date will be considered late, and a grade penalty will be assessed. The
grade penalty is a reduction of one letter grade for each day the report is late. Lab reports will be
graded based on completeness (all parts of the report are included), accuracy of the calculations
(where appropriate), accuracy of answers to post lab questions, and accuracy of results (where
appropriate). Unless specified otherwise, all post lab questions are to be answered (for each part
of the experiment performed.) If the report is incomplete or has calculation errors, points will be
deducted accordingly, so it is to your benefit to check your report carefully for completeness and
check your calculations for accuracy before submitting the report. Any report not turned in will
receive a grade of 0. A complete report that is turned in will receive a minimum grade of 70%.
Please feel free to seek help in the tutoring center, should you need help with your reports.
Reports should be prepared using a word processor. Calculations may be hand written. Graphs
should be prepared using CurveExpert or Excel. Other graphing programs may be used, but
please show a sample graph to your lab instructor for their approval.
Grading:
3 lecture tests
1 final exam
30 %
30%
laboratory experiments
challenge problem
quizzes
25 %
5 %
10 %
Your course grade will be based on the percentage of points earned. As you can see, a good
course grade is achieved by performance in all aspects of the course. Our department policy is
that you must pass both lab and lecture to pass the course. Failing either lecture or lab will result
in an F for the course. The final exam is cumulative for good reason. The material you will have
learned in both CHEM110 and CHEM111 is essential background material for your future
chemistry courses. Course grades will be assigned as follows:
93 –100
90 – 92.9...
87 – 89.9…
83 – 86.9…
80 – 82.9…
A
AB+
B
B-
77 – 79.9…
70 – 76.9…
67 – 69.9…
60 – 66.9…
<60
C+
C
D+
D
F
<60
F
Your grade will be calculated as follows:
Grade = 0.30(lecture exam ave) + 0.25(lab ave.) + 0.30(final exam) + 0.10(quiz ave) +
0.05(challenge problem)
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I do not give opportunity for “extra credit”. The reason for this is to promote good work habits
for the future. When you are at the work place, your employer will not give you a chance for
“extra credit”. Instead, they will dismiss you and hire someone who can do the work correctly
and on time. I do have a “forgiveness” policy. If you do poorly on only one lecture exam but do
well on the other exams and the final exam, I tend to discount the one poor grade as not
representative of your ability. Everyone has a “bad day”.
In 30 years of teaching, I have never had to curve grades. 
Cheating
I “take no prisoners” when it comes to people cheating on exams. If you want to guarantee
yourself an F in the course, then cheat on the exam. All incidences of cheating will be reported
to the University Academic Standards Committee, and you will risk dismissal from the
university and have a notation of academic dishonesty be placed on you permanent school
record. It would thus seem that doing poorly on an exam, if unprepared, would be preferable.
Tutoring
Tutoring is available, free of charge at the Chemistry Tutoring Center located in SM538. No
appointment is needed to access the service. Check the schedule located on the door for specific
times—there may be a few “gaps” in the times. Since I am in charge of the tutoring for math
and sciences—please feel free to seek me out in the tutoring center, or one of the student tutors.
I encourage you to avail yourselves to this service—we have helped many students do well in
chemistry courses. Another resource is the tutoring center’s home page:
http://www.towson.edu/~ladon. There are well over 200 pages of study aids there for your use.
General Advice
1) Don’t procrastinate—a lab report isn’t going to magically appear on your monitor in the 45
minutes before it is due, nor is 3 weeks’ worth of lecture material going to download into
your brain in 3 hours before the exam.
2) Work as many problems from the textbook as you can. If you can only correctly answer 50%
of the problems, then you have a good idea of your potential test score—GET HELP!
3) Let the information build—the subject gets easier, not harder, if you do this. There are only
24 hours to a day. If you have to relearn what you forget, at some point there won’t be
enough time to do all the work needed to review the old material and learn the new material.
Do whatever it takes you to put information into long-term memory. (Association, repetition,
reinforcement—using flashcards you can make, working problems, thinking about the
concept, talking or explaining the concept to someone else, rewriting notes, mnemonic
devices.) Review your class notes every week from beginning to end to do a “refresh”.
4) When taking an exam, all you can ask of yourself is the best you can do—so don’t stress.
5) Form a study group and explain concepts to each other. The best way to truly learn
something is to have to teach to others. You will find that your retention improves
dramatically if you do this!
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Chemistry 111 Lecture and Laboratory Schedule
Date
Topics covered
8/25 Chapter 6.6
8/27
Chapter 12.1 – 12.2
8/30
Chapter 12.3 – 12.5 We are skipping 12.4
9/1
Chapter 12.6 - 12.7
9/1
Laboratory Introduction, Safety and Check-In
Experiment 15A, Synthesis and Analysis of a Compound of Iron (SACI), Part A
9/3
Chapter 13.1 – 13.2
9/6
Labor Day! No class!
9/8
Chapter 13.3
9/8
Experiment 16: Intermolecular Forces
9/10
Chapter 13.4 – 13.5
9/13
Chapter 13.6
9/15
Chapter 14.1 – 14.2
9/15
Experiment 15B: SACI, Iron Analysis, Part B
9/17
Chapter 14.3, Chapter 21.3
9/20
Chapter 14.4
9/22
Chapter 14.5 – 14.6 ** End of Exam 1 material
9/22
Experiment 17: Freezing Point Depression
9/24
Chapter 15.1 – 15.2
9/27
EXAM 1 covers Chapters 6.6, 12 –14, 21.3
9/29
Chapter 15.3
9/29
Experiment 17: Freezing Point Depression, continued
10/1
Chapter 15.4
10/4
Chapter 16.1 – 16.3
10/6
Chapter 16.4
10/6
Experiment 20AB: Chemical Kinetics: Reaction of Thiosulfate Ion with Hydrogen Ion
10/8
Chapter 16.5 – 16.6
4
10/11 Chapter 16.7 – 16.8
10/13 Chapter 16.9
10/13 Experiment 21: Chemical Equilibrium & LeChatelier’s Principle
10/15 Chapter 16.10 –16.11
10/18 Chapter 17.1 – 17.2
10/20 Chapter 17.3 – 17.4
10/20 15CD: SACI Water & Oxalate Analyses, Parts C, D
10/22 Chapter 17.5
10/25 Chapter 17.6 – 17.7
10/27 Chapter 17.8 **End of Exam 2 material **
10/27 Experiment 22ABD: Acids, Bases, Salts and Buffers, Parts A, B, D
10/29 Chapter 18.1 – 18.2
11/1
Chapter 18.3
11/3
EXAM 2 covers Chapters 15 – 17
11/3
Experiment 22CEF: Acids, Bases, Salts and Buffers, Parts C,E, F
11/5
Chapter 18.4
11/8
Chapter 18.5
11/10 Chapter 18.6
11/10 Experiment 23: Introduction to Qualitative Analysis
11/12 Chapter 19.1
11/15 Chapter 19.2
11/17 Chapter 19.3
11/17 Experiment 25: Environmental Forensics
11/19 Chapter 19.4 ** End of exam 3 material **
11/22 Chapter 19.5
12/1
Experiment 25: Environmental Forensics continued
11/24 THANKSGIVING DAY
11/25
BREAK
11/26
RELAX!
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11/29 Chapter 19.6
12/1
Chapter 19.7
12/1
Experiment 25: Environmental Forensics continued
12/3
In class review for Final Exam/Catch up day
12/6
EXAM 3 covers Chapters 18 – 19
12/8
In class review for Final Exam/Catch up day
12/8
Experiment 25: Environmental Forensics continued; Checkout of lab.
12/10 CUMULATIVE FINAL EXAM AT 8:00am – 10:00am in SM506
Be on time!!!! Good luck!!!
Date
Expt
9/1
15A
Chemistry 111.001 Laboratory Schedule
Fall 2010
Experiment Title
Lab Report Due
Introduction, Check-In
Synthesis & Analysis of a Compound of Iron
(SACI), Part A
none
none
9/8
16
Intermolecular Forces
9/15
15B
SACI, Iron Analysis, Part B
Expt 16
9/22
17
Freezing Point of a Solution
Expt 15B
9/29
17
Freezing Point of a Solution, continued
10/6
20
Chemical Kinetics: Reaction of Thiosulfate Ion
with Hydrogen Ion
Expt 17
10/13 21
Chemical Equilibrium & LeChatelier’s Principle
Expt 20
10/20 15CD
SACI, Water and Oxalate Analyses, Parts C, D
Expt 21
10/27 22ABD
Acids, Bases, Salts & Buffers, Parts A, B, D
none
11/3
Acids, Bases, Salts & Buffers, Parts C, E, F
Expt15 C – G
11/10 23
Introduction to Qualitative Analysis
Expt 22A - F
11/17 25
Environmental Forensics, Preliminary Investigation
12/1
25
Environmental Forensics, Follow-up Investigation
12/8
25
Check-Out & Experiment 25 Team Oral Reports
22CEF
Expt 23
none
Expt 25
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Chemistry 111 Suggested Problems and Study Guide
Chapter 6.6 Study Guide
1. Review the terms standard enthalpy, standard enthalpy of formation, Hess’ Law
2. Be able to calculate the heat of reaction using standard enthalpies of formation and
Hess’ Law
Chapter 6.6 Suggested Problems
6.26, 6.54, 6.62
Chapter 12
Study Guide
1. Know the meaning behind the key words listed on page 418 and be able to apply them
to either conceptual or numeric problems.
2. Know the Clausius-Clapeyron Equation and be able to solve for any of the variables in
this equation.
3. Be able to determine the type of interparticle force present for a given compound.
4. Know the relative strengths of interparticle forces.
5. Be able to describe a phase diagram.
Chapter 12 Suggested Problems
Practice exercise 12.5
End of chapter problems 12.10, 12.12, 12.36, 12.42, 12.80, 12.86, 12.90
Chapter 13 Study Guide
1. Know the key terms listed on page 447.
2. Know and be able to apply the key equations listed on page 447.
3. Be able convert from one concentration unit to another. The concentration units you
are responsible are the ones discussed in class: mass percent, volume percent,
molarity, molality, mole fraction, ppt, ppm, ppb.
4. Be able to use Henry’s Law in a problem.
5. Know the colligative properties, vapor pressure lowering, boiling point elevation,
freezing point depression, and osmotic pressure, and be able to work qualitative and
quantitative problems dealing with these properties.
Chapter 13 Suggested Problems
13.20, 13.22, 13.36, 13.50, 13.56, 13.58, 13.64, 13.88, 13.98
Chapter 14 and Chapter 21.3 Study Guide
1. Know the key terms listed on page 487.
2. Know and be able to apply the key equations listed on page 486. (exceptions: 14.6,
14.10, 14.12)
3. Be to qualitatively explain chemical reactions based on what is described in kinetic
molecular theory.
4. Be able to determine the reaction order and the rate law from experimental data.
5. Be able to determine the half-life or amount remaining for a radioactive decay.
6. Be able to apply rate laws to predict a reaction mechanism as shown in class.
7. Be able to use the Arrhenius equation to solve for any of its variables.
Chapter 14 and Chapter 21.3 Suggested Problems
14.18, 14.20, 14.24, 14.34, 14.36, 14.66, 14.72, 14.78, 21.26, 21.68
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Chapter 15
Study Guide
1. Know the key terms listed on page 520.
2. Know and be able to apply the key equations listed on page 519.
3. Be able to write an equilibrium constant expressions for a homogeneous or a
heterogeneous equilibrium.
4. Be able to convert between Kp and Kc.
5. Be able to apply LeChatelier’s Principle.
6. Be able to calculate the concentrations of components involved in an equilibrium or
the equilibrium constant.
7. Be able to use the reaction quotient to predict an equilibrium shift.
Chapter 15
Suggested Problems
Practice exercises: 15.1,15.3, 15.5, 15.8
End of chapter problems: 15.14, 15.20, 15.24, 15.32, 15.48, 15.60, 15.72, 15.78,15.88
Chapter 16
Study Guide
1. Know the key terms listed on page 567.
2. Know and be able to apply the key equations listed on page 567.
3. Be able to identify an acid, base, conjugate acid and conjugate base using the Brønsted
definition.
4. Know the strong acids: HCl, HBr, HI, HNO3, HClO4, H2SO4 (1st dissociation only),
and that they dissociate completely.
5. Be able to convert between pH, pOH, [H3O+], [OH¯], Ka, and Kb for both strong and
weak acids and bases.
6. Be able to write the dissociation of a weak acid or weak base in aqueous solution.
7. Be able to find the percent ionization of an acid.
8. Be able to write the hydrolysis equilibrium reaction of salts.
9. Be able to qualitatively predict the acid or base properties of salts and quantitatively
determine the pH of salts (hydrolysis).
10. It is probably a good idea to review naming ionic compounds and relearn the
polyatomic ions (formula and charge) if you have forgotten them.
Chapter 16
Suggested Problems
Practice exercises: 16.8, 16.9, 16.11, 16.13, 16.14
End of chapter problems: 16.4, 16.5, 16.6, 16.16, 16.34, 16.44, 16.56, 16.58, 16.74,
16.84, 16.86, 16.102, 16.106, 16.116
Chapter 17
Study Guide
1. Know the key terms listed on page 603.
2. Know and be able to apply the key equations listed on page 603.
3. Be able to describe the components of an acidic buffer or an alkaline buffer.
4. Be able to calculate the pH of a buffer solution.
5. Be able to write the equilibrium expression of a buffer solution.
6. Be able to describe the type of equilibrium taking place at points along a titration
curve (0 mL base added, before the equivalence pt, at the equivalence pt and beyond the
equivalence pt.)
7. Know how acid-base indicators work.
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8. Review and relearn the solubility rules.
9. Be able to write the equilibrium reaction describing the dissociation of a salt.
10. Be able to determine the solubility of a salt.
11. Using a reaction quotient, be able to predict whether a mixture of two solutions will
produce a precipitate.
12. Be able to qualitatively and quantitatively describe how the introduction of a
common ion affects solubility and why some salts are soluble in acid solution.
13. Be able to calculate the concentration of all species present in a complex ion
equilibrium.
Chapter 17
Suggested Problems
Practice exercises: 17.1, 17.2, 17.4, 17.6, 17.8, 17.9, 17.10
End of chapter problems: 17.6, 17.8, 17.12, 17.14, 17.20, 17.34, 17.36, 17.42, 17.46,
17.54, 17.64, 17.74, 17.80
Chapter 18
Study Guide
1. Know the key terms listed on page 635.
2. Know and be able to apply the key equations listed on page 634.
3. Know qualitatively what each thermodynamic function (enthalpy, entropy and free
energy) tells you about a process.
4. Be able to calculate the enthalpy change, entropy change and free energy change using
the appropriate thermodynamic data. Note: there are a number of ways to find the free
energy change!
5. Be able to use the free energy change to predict spontaneity, calculate Q, and Keq.
6. Know the three Laws of Thermodynamics.
7. Be able to describe the spontaneity as affected by enthalpy and entropy.
8. Review what is a state function (see Chapter 6)
Chapter 18
Suggested Problems
Practice exercises: 18.2, 18.4, 18.7, 18.8
End of chapter problems: 18.12, 18.14, 18.18, 18.20, 18.26, 18.50, 18.56, 18.74, 18.90
Chapter 19
Study Guide
1. Know the key terms listed on page 675.
2. Know and be able to apply the key equations listed on page 674.
3. Be able to balance redox reactions in acidic solution or basic solution.
4. Know standard cell notation for a galvanic cell.
5. Be able to calculate the cell potential of a standard cell.
6. Be able to use the Nernst Equation.
7. Be able to apply the relationship between cell potential and free energy.
8. Know how cell potential, free energy and the equilibrium constant are related.
9. Know some applications of electrochemistry.
Chapter 19
Suggested Problems
Practice exercises: 19.2, 19.3, 19.4, 19.5, 19.6
End of chapter problems: 19.1, 19.2, 19.12, 19.16, 19.18, 19.22, 19.26, 19.30, 19.46
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