Syllabus for Chem110.002
Summer 2008
Lecture Instructor: Liina Ladon
Office: Chemistry Tutoring Center, SM538
Office Hours: By appointment
Phone: 410-704-3054
E-mail: lladon@towson.edu
Lecture/Lab: MTWRF 8:00am – 11:50pm
Lecture meets in SM506 on MTR and SM524 on WF
Lab meets in SM507
Web page: www.towson.edu/~ladon
Blackboard site log-in:
http://learnonline.towson.edu/
Required Materials:
Lecture Textbook: General Chemistry, Raymond Chang, 5th Ed., McGraw Hill, Boston,
2005, Text ISBN 978-0-07-304851-2
Lab Textbook: Laboratory Experiments In General Chemistry: CHEM110 and CHEM111,
Version 8.0, 2005, Towson University. This is an “in-house” manual.
Laboratory Goggles: Must be ANSI approved and cover the eyes completely. The chemistry
club sells two varieties ($10.00). They are cheaper and more comfortable than the goggles
sold at the university bookstore. Additionally, there are a limited number of used pairs for
$5.00, but they sell out quickly. The used pairs have been sanitized.
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.
Calculator: Calculator: A scientific calculator is recommended 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
programmable calculators for this course due to increasing incidence of students storing illegal
information in the memory of TI83 type calculators. I suggest a calculator, such as the TI36X,
which is solar (no batteries needed) and simpler to operate than the TI83. 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, you must bring valid documentation (obit, garage receipt, doctor’s
note, etc.) Pending approval by the instructor, the final exam will be weighted an additional 13.3 %
to cover points missed. Over-sleeping, for instance, is not a valid excuse. Invalid absences from an
exam will result in a grade of 0 for that exam. Only one make-up exam per student per semester! If
you are more than 20 minutes late for a lab, you will not be able to perform the experiment and will
receive a grade of 0 for that lab.
Please turn off cell phones and beepers while in class out of consideration for your classmates. It can
be very distracting – especially during an exam! In addition, class time is not a social hour. Please
refrain from casual conversation during class time. You will be asked to leave the classroom if you
disrupt the class.
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Blackboard website:
I will be trying out the use of Blackboard, an online information hub for coursework. Please be
patient! I confess I am a Blackboard “amateur”. I hope to post useful information, the challenge
problems, old exams and have a chance for you use the discussion board for help from your
classmates and me on course material. Any suggestions from those of you who have used
Blackboard in the past are welcome! To access Blackboard, you need to create an account for this
course. To do so, launch your browser and open http://learnonline.towson.edu. Click Create
Account, follow the instructions on the screen and fill in the form accordingly. The username must
be lower case. If you have trouble, please see me and I’ll see what I can do to help you. Once you
have logged into the LearnOnline, click the Courses tab and locate this course using either the
course ID or my name. Next, click Enroll and then Submit.
ARIS website:
The textbook has a useful website: http://www.aris.mhhe.com which is a great resource of
supplemental material. You do not need to sign in or register for the site and it is free of charge. In
particular are many animations (for you “visual learners”) and self-assessment quizzes. Choose
“chemistry” as the subject, Chang, 5th ed. as the textbook. When the textbook section appears,
choose the Resource tab at the upper left corner of the tool bar and go nuts! You do not login with a
username or password. Pick a chapter and see what you find!
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.
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. If you do not attend lab and do not turn in a report, a grade of 0% is
given. If you attend a lab, but do not turn in a report, a grade of 50% is given. 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.
Graphs should be prepared using Excel. Other graphing programs may be used, but please show a
sample graph to your lab instructor for his/her approval. If you are submitting a report via e-mail,
please make sure it is in Microsoft Word format. If I cannot open the attachment, or the attachment
is unreadable, I cannot count it as a report. You will be working with a lab partner. Please make
sure that your lab report is not identical to your partner’s. This carries the penalty of plagiarism.
Grading:
3 lecture exams
11 laboratory experiments
1 final exam (cumulative)
40 %
25 %
35 %
Your course grade will be based on the percentage of points earned. As you can see, a good course
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grade is achieved by performance in all aspects of the course. Don’t count on any one section of the
course to either pass or fail you. The final exam is cumulative for good reason. The material you
will have learned in Chem110 is essential background material for Chem111 and beyond.
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…
73 – 76.9…
70 – 72.9…
67 – 69.9…
60 – 66.9…
C+
C
CD+
D
<60
F
Your course grade is calculated as a weighted average:
Final course grade = 0.4(lecture exam average) + 0.25(lab average) + 0.35(final exam grade)
Also, you must pass both lab and lecture in order to pass the course. This is a departmental
policy.
In over 20 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 placed on you permanent school record. It would thus seem that
flunking an exam, if unprepared, would be preferable. Additionally, a lab report must not be
identical to that of another classmate.
Tutoring
Since I am in charge of the tutoring for the sciences—please feel free to seek me out in the tutoring
center. Tutoring is available, free of charge at the Chemistry Tutoring Center located in SM538.
No appointment is needed to access the service. I have other duties to attend to at times, such as
meetings, so I may not always be there when scheduled. When this happens, I will try to post a sign
in advance, and/or let you know during lecture. In the summer, it’s best to call ahead and make sure I
am available to help. I encourage you to avail yourselves to this service—many students do well in
chemistry courses with help from the tutoring center. Also available as a resource is the tutoring
center’s home page: http://www.towson.edu/~ladon. There are well over 150 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
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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.)
4)
When taking an exam, all you can ask of yourself is the best you can do—so don’t stress.
Chemistry 110 Lecture/Lab Schedule
Summer 2008
Date Topics covered
Date
Topic (hours)
Section(s) in Chang
5/27
Introduction; Studying Chemistry (1)
Classification of Matter (0.5)
Measurement and Units (0.5)
Numbers and Problem-solving (1.5)
1.1-1.2
1.3-1.4
1.5
1.6-1.7
5/28
Atomic Structure (1)
LAB: Record Keeping in the Laboratory
The Laboratory Report
Laboratory Safety
Check-in
Computer Graphing Programs
What are Extensive and Intensive Properties? (Experiment #1)
2.1-2.3
LM 3
LM 9, A-33
LM A-5, A-9
LM A-3, A-37
LM A-19; Handout
LM 15
5/29
Radioactivity; Nuclear Reactions (1.5)
LAB: What is the Relationship…? (Experiment #2) (2.5)
21.1, 21.3-21.5
(sections)
LM 17
5/30
Structure of Matter (1)
Nomenclature (2)
2.4-2.6
2.7
6/2
LAB: How Can the Density of a Substance…?(Experiment #3)
(4)
Atomic, Molar, and Molecular Masses (1)
LAB: How can Matter be Classified?(Experiment #4) (3)
LM 21
6/4
Chemical Formulas (1.5)
Chemical Equations (0.5)
Stoichiometry (1)
3.5-3.6
3.7
3.8
6/5
Stoichiometry (2)
LAB: Synthesis and Limiting Reactant (#8) (2)
3.8-3.9
LM 55
6/6
Reactions in Aqueous Solution (3)
4.1-4.3; Handout
6/9
Hour Examination I (1)
LAB: Determination of the Identity… (#6) (2.5)
Ch. 1-3, 21
LM 41
6/10
Redox Reactions (1)
4.4
6/3
3.1-3.3
LM 29
4
LAB: Chemical Reactions (#7) (2.5)
LM 45
6/11
Solution Concentrations and Stoichiometry (2)
Gas Laws (1.5)
4.5-4.6
5.1-5.3
6/12
LAB: Acid-Base Titration (#9) (3.5)
LM 59
6/13
Ideal Gas Law; Dalton’s Law (1)
Kinetic-Molecular Theory (1)
Energy (1)
5.4-5
5.6-5.7
6.1-6.3
6/16
Calorimetry (1)
LAB: Application of Gas Laws…. (#14) (3)
6.5
LM 97
6/17
Energy and Chemical Reactions (1)
LAB: Calorimetry: Heat of Reaction (#10) (3)
6.4
LM 67
6/18
Hour Examination II (1)
Nature of Light (1)
Bohr Theory of the Hydrogen Atom (1)
Ch. 4-6
7.1-7.2; 7.4
7.3
6/19
LAB: Emission Line Spectrum… (#11) (2)
Quantum Theory of the Atom (1)
Electronic Configurations and the Periodic Table (1)
LM 79
7.5-7.7
7.8, 7.9, 8.1, 8.2
6/20
Periodic Properties (1)
Covalent Bonding; Lewis Structures (2)
8.3-8.6
9.1-9.4; 9.6-9.7
6/23
Bond Energy (0.5)
Geometry and Polarity (1)
LAB: Bonding and Molecular Structure (#13) (1.5)
9.8
10.1-10.2
LM 91
6/24
LAB: Bonding and Molecular Structure (#13) (2)
LAB: Check-out
LM 91
LM A-3
6/25
Hour Examination III (1)
Valence-Bond Theory; Hybrid Orbitals (1.5)
Ch. 7-9
10-3-10.5
6/26
General Review (?)
All Above
6/27
Final Examination (9-11 AM)
All Above (esp. Ch. 10)
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Chem110 Suggested Problems and Study Guide
Chapter 1
Study Guide
1. Make sure you memorize the metric prefixes and how to do unit conversions within
the metric system and between the English and the metric system.
2. Learn how to handle significant figures in calculations.
3. Learn how to use you calculator to do scientific notation.
4. Know the meaning of the terms listed under Key Words on page 22.
Chapter 1
Suggested Problems
1.2 – 1.6, 1.10, 1.18, 1.22, 1.24, 1.30, 1.32, 1.38, 1.44, 1.66
Chapter 2
Study Guide
1. Be able to describe the work of any scientist described in this chapter.
2. Learn the names and symbols of the representative elements and the first two rows of
the transition metals.
3. Know how to recognize whether a compound is ionic or covalent.
4. Know how to name ionic compounds.
5. Know how to name covalent compounds.
6. Know how to name acids.
7. Know the meaning of the terms listed under Key Words on page 53
Chapter 2
Suggested Problems
2.4, 2.10, 2.16, 2.34, 2.46, 2.48, 2.50, 2.53, 2.59
Chapter 3
1.
2.
3.
4.
5.
6.
7.
8.
Chapter 3
Study Guide
Know the relationship between mass, moles, particles and Avogadro’s Number.
Be able to find the molar mass of a substance.
Be able to find the percent composition of a compound.
Be able to calculate the empirical formula and molecular formula of a compound from
its percent composition.
Be able to balance a chemical reaction.
Be able to determine the amount of reactant, product (theoretical yield) and percent
yield for a chemical reaction.
Be able to find the limiting reagent.
Know the meaning of the terms listed under Key Words on page 86.
Suggested Problems
3.14, 3.16, 3.18, 3.20, 3.24, 3.26, 3.40, 3.44, 3.50, 3.54, 3.60, 3.66, 3.72, 3.86, 3.92
Chapter 4
Study Guide
1. Review the polyatomic ions from Chapter 2.
2. Be able to write the molecular, total ionic and net ionic equation for a precipitation
reaction and an acid/base reaction.
3. The solubility rules will be given on the exam, but you have to be able to apply them
correctly.
4. Be able to determine the oxidation state of element(s) in a compound.
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5. Be able to identify the compound oxidized, compound reduced, oxidizing agent and
reducing agent in a redox reaction.
6. Be able to calculate the molarity of a solution.
7. Be able to do a solution stoichiometry problem.
8. Know the Key Equations on page 123.
9. Know the meaning of the terms listed under Key Words on page 124.
Chapter 4
Suggested Problems
4.10, 4.22, 4.34, 4.40, 4.42, 4.54, 4,56, 4.58, 4.64, 4.74, 4.80, 4.92
Chapter 5
Study Guide
1. Know how to convert between pressure units. The conversion factors will be given
on the exam.
2. Review how to convert a given temperature from Fahrenheit or
Celsius to Kelvin.
3. Know what is STP.
4. Know the various gas laws discussed in the chapter.
5. Know the Key Equations on page 162 except the van der Waals equation.
6. Know the meaning of the terms listed under Key Words on page 163.
Chapter 5
Suggested Problems
5.13, 5.14, 5.20, 5.24, 5.32, 5.40, 5.44, 5.48, 5.60, 5.84, 5.108
Chapter 6
Study Guide
1. Understand the terms system and surroundings.
2. Know the sign conventions for work and heat.
3. Be able to calculate the internal energy change or enthalpy change for a process.
4. Be able to describe a reaction as endothermic or exothermic based on the enthalpy
change.
5. Be able to find any of the variables in a calorimetry problem (heat, mass, specific heat
capacity, initial temperature or final temperature).
6. Know the Key Equations on page 197.
7. Know the meaning of the terms listed under Key Words on page 198.
Chapter 6
Suggested Problems
6.1, 6.7, 6.18, 6.20, 6.26, 6.34, 6.36, 6.38, 6.54, 6.58, 6.90
Chapter 7
1.
2.
3.
4.
5.
6.
7.
Study Guide
Know the relationship between wavelength, frequency and energy.
Know the Bohr Model for an atom and the Bohr’s Equation.
Know the quantum numbers and what they signify.
Be able to give the electron configuration of an atom.
Know the Key Equations on page 237.
Know the meaning of the terms listed under Key Words on page 238.
Know the regions of the electromagnetic spectrum.
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Chapter 7
Suggested Problems
7.1 – 7.4, 7.8, 7.16, 7.32, 7.42, 7.54, 7.82, 7.84, 7.86, 7.98
Chapter 8
Study Guide
1. Be able to write the electron configuration of an ion.
2. Know the periodic trends for atomic size, ionic size, effective nuclear charge,
ionization energy, electron affinity.
3. Know the meaning of the terms listed under Key Words on page 272.
Chapter 8
Suggested Problems
8.5, 8.6, 8.11, 8.18, 8.28, 8.32, 8.38, 8.44, 8.51, 8.58, 8.80
Chapter 9
Study Guide
1.
2.
3.
4.
Review the difference between an ionic compound and a covalent compound.
Know the following terms: octet, electronegativity, resonance.
Be able to do Lewis structures.
Be able to find the enthalpy change for a reaction using bond energies and review the
terms endothermic and exothermic.
5. Know the meaning of the terms listed under Key Words on page 306.
Chapter 9
Suggested Problems
9.1 – 9.11, 9.34, 9.38, 9.49, 9.70, 9.74, 9.98 note: omit formal charges.
Chapter 10
Study Guide
1. Be able to draw the Lewis structure, give the structure type (AB2, etc.), hybridization,
bond angles, and molecular geometry of a compound.
2. Be able to use valence bond theory (box diagrams) to show how hybridization
takes place.
3. Be able to identify sigma and pi bonds in molecules.
4. Know the meaning of the terms listed under Key Words on page 349.
5. We are skipping section 10.6 on Molecular Orbital Theory.
Chapter 10
Suggested Problems
10.7, 10.10, 10.12, 10.34, 10.36, 10.4010.66
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