Syllabus for Chem110.002
Summer 2009
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 9:00am – 12:50pm
Lecture meets in SM524
Lab meets in SM507
Webpage: 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, 2008,
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. Make sure you get the
correct version!
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.
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 10% 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. 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, beepers and MP3 players 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.
Blackboard website:
I will be using Blackboard, an online information hub for coursework. I hope to post useful
information, the challenge problems 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. Chose
“chemistry” as the subject, Chang, 5th ed. as the textbook. When the textbook section appears,
choose the “Resourses” tab at the upper left corner of the tool bar and go nuts! Pick a chapter and
see what you find! Do not sign in – that is a pay portion of the site.
Grading:
3 lecture exams
10 quizzes
15 laboratory experiments
30 %
10 %
25 %
1 challenge problems
1 final exam (cumulative)
5%
30 %
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. 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…
70 – 76.9…
67 – 69.9…
60 – 66.9…
<60
C+
C
D+
D
F
<60
F
Your course grade is calculated as a weighted average:
Final course grade = 0.3(lecture exam average) + 0.1(quiz average) + 0.25(lab average) +
0.05(challenge problem average) + 0.3(final exam grade)
Also, you must pass both lab and lecture in order to pass the course. 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. Check the schedule located on the door for
specific times—there may be a few “gaps” in the times specified above. I may 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. 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://pages.towson.edu/ladon. There are well over 150 pages of study aids there for your use. The
Academic Achievement Center, CK505, offers numerous workshops throughout the semester to
build your study skills. I urge you to take advantage of these free workshops to improve your
study skills and thus success in your coursework.
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.) Look
over your class notes from day one to the current day at least once a week to refresh your
knowledge. This will make studying for a cumulative final exam easy!
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
Date
Summer 2009
Topics covered
Date
Topic
Section(s) in Chang
5/26
Introduction; Studying Chemistry
Classification of Matter
Measurement and Units
Numbers and Problem-solving
1.1-1.2
1.3-1.4
1.5
1.6-1.7
5/27
Atomic Structure
LAB: Record Keeping in the Laboratory
The Laboratory Report
Laboratory Safety
Check-in
2.1-2.3
LM 3
LM 9, A-33
LM A-5, A-9
LM A-3, A-37
Computer Graphing Programs
LM A-19; Handout
(Expt #1) What are Extensive and Intensive Properties?
LM 15
Radioactivity; Nuclear Reactions
Structure of Matter
Nomenclature
21.1, 21.3-21.5
(sections)
2.4-2.6
2.7
5/29
LAB: (Expt #2)What is the Relationship…?
LM 17
6/1
LAB: (Expt #3) How Can the Density of a Substance…?
LM 21
6/2
Nomenclature (continued, if needed)
Atomic, Molar, and Molecular Masses
2.7
3.1-3.3
6/3
LAB: (Expt #4) How can Matter be Classified?
LM 29
6/4
Chemical Formulas
Chemical Equations
Stoichiometry
3.5-3.6
3.7
3.8
6/5
Stoichiometry
LAB: (Expt #8) Synthesis and Limiting Reactant
3.8-3.9
LM 55
6/8
Reactions in Aqueous Solution
4.1-4.3; Handout
6/9
Hour Examination 1
LAB: (Expt #6)Determination of the Identity…
LAB: (Expt #7)Chemical Reactions
Ch. 1-3, 21
LM 41
LM 45
6/10
Redox Reactions, Solution Concentrations
and Stoichiometry, Gas Laws
4.4-4.6
5.1-5.3
5/28
6/11
LAB: (Expt #9)Acid-Base Titration
LM 59
6/12
Ideal Gas Law; Dalton’s Law
Kinetic-Molecular Theory
Energy
5.4-5
5.6-5.7
6.1-6.3
6/15
Calorimetry
LAB: (Expt #14)Application of Gas Laws
6.5
LM 97
6/16
Energy and Chemical Reactions
LAB: (Expt #10) Calorimetry: Heat of Reaction
6.4
LM 67
6/17
Hour Examination 2
Nature of Light
Bohr Theory of the Hydrogen Atom
LAB: (Expt #11) Emission Line Spectrum
Ch. 4-6
7.1-7.2; 7.4
7.3
LM 79
6/18
NO CLASS TODAY!
6/19
Quantum Theory of the Atom
Electronic Configurations and the Periodic Table
Periodic Properties
Covalent Bonding; Lewis Structures
7.5-7.7
7.8, 7.9, 8.1, 8.2
8.3-8.6
9.1-9.4; 9.6-9.7
6/22
Bond Energy
Geometry and Polarity
LAB: (Expt #13)Bonding and Molecular Structure
9.8
10.1-10.2
LM 91
6/23
Valence-Bond Theory; Hybrid Orbitals
10-3-10.5
6/24
Hour Examination III
Ch. 7-9
6/25
General Review … Bring your questions!!
All Above
6/26
Final Examination (9-11 AM)
All Above (esp. Ch. 10)
IT’S BEEN A PLEASURE! GOOD LUCK WITH YOUR FUTURE STUDIES!!!
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
Study Guide
1. Know the relationship between mass, moles, particles and Avogadro’s Number.
2. Be able to find the molar mass of a substance.
3. Be able to find the percent composition of a compound.
4. Be able to calculate the empirical formula and molecular formula of a compound from
its percent composition.
5. Be able to balance a chemical reaction.
6. Be able to determine the amount of reactant, product (theoretical yield) and percent
yield for a chemical reaction.
7. Be able to find the limiting reagent.
8. Know the meaning of the terms listed under Key Words on page 86.
Chapter 3
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.
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.
2.
3.
4.
Understand the terms system and surroundings.
Know the sign conventions for work and heat.
Be able to calculate the internal energy change or enthalpy change for a process.
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
Study Guide
1. Know the relationship between wavelength, frequency and energy.
2. Know the Bohr Model for an atom and the Bohr’s Equation.
3. Know the quantum numbers and what they signify.
4. Be able to give the electron configuration of an atom.
5. Know the Key Equations on page 237.
6. Know the meaning of the terms listed under Key Words on page 238.
7. Know the regions of the electromagnetic spectrum.
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. Review the difference between an ionic compound and a covalent compound.
2. Know the following terms: octet, electronegativity, resonance.
3. Be able to do Lewis structures.
4. 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, 10.40, 10.66