Syllabus for Chem110/111.727
Spring/Summer2012
Lecture Instructor: Liina Ladon
Office: Chemistry Tutoring Center, SM538
Lecture MW in SM356
Office Hours: By appointment
Lab: M or R as per schedule in SM505/507
Phone: 410-704-3054
E-mail: lladon@towson.edu
Web page: www.towson.edu/~ladon
Lecture or Lab: Monday/Wednesday unless otherwise noted from 6:00pm – 10:00pm
Required Materials:
Lecture Textbook: Chemistry, Thomas R. Gilbert, etal., 3rd ed. W. W. Norton & Company,
New York, 2012, ISBN 978-0-393-93431-1
Lab Textbook: Laboratory Experiments In General Chemistry: CHEM110 and CHEM111,
Version 9.0, 2010, Towson University. This is an “in-house” manual. Make sure you get the
correct version! Older editions are not acceptable, there are too many changes.
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: 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 this variety of calculators. I suggest a calculator, such as the TI36X or TI30X,
which are solar (no batteries needed) and simpler to operate. 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 7.5 % to cover points
missed. If you are more than 20 minutes late for a lab lecture, you will not be able to perform the
experiment and will receive a grade of 0 for that lab. If you miss any lab session, you may make up
the lab only if you have a verifiable excuse for your absence. Please take into consideration that it
takes the same amount of time for the lab manager to prepare a lab for one person as it does for an
entire section.
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.
SmartWork Online Homework website:
You will be able to access SmartWork upon enrolling on the site. Nine assignments will be
posted. It is your responsibility to complete the assignments on time. These assignments are
graded and count 10% of your course grade. Please enroll in SmartWork as soon as possible.
The enrollment key for my class is CHEM31713. A link for instructions on how to enroll in
SmartWork is under the Course Documents tab in Blackboard.
Grading:
lecture exams
homeworks (drop 3 lowest)
laboratory experiments/course
40 %
10 %
25 %
challenge problems
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…
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 = 0.3(lecture exam average) + 0.1(homework 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 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 placed on you permanent school record. It would thus seem that a
poor performance on 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. The general hours of operation will be: Monday thru
Thursday from 8:00am - 6:00pm. 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 24 hours before the exam. Cramming before an exam only leads to “surface learning”
the material. You will retain the information for only a short period of time. You need to hang
onto as much of this information as possible to do well on the final exam and for use in future
courses. Keep in mind you are now learning a profession and not just passing a course.
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 Ner Israel 2012
Date Topics covered
4/19
Introduction, Chapter 1
4/23
Lab Check-in, Experiments 1 & 2
4/25
Chapter 2
4/30
Experiment 3
5/2
EXAM 1 covering Chapters 1 & 2; start Chapter 3
5/7
Finish Chapter 3 and Experiment 8
5/9
Chapter 4
5/14
start Chapter 5; Experiment 9
5/16
EXAM 2 covering Chapters 3 & 4; finish Chapter 5
5/21
Experiment 10
5/23
Chapter 6
5/30
Chapter 7
6/4
EXAM 3 covering Chapters 5 & 6; Experiment 11 & 12
6/6
Chapter 8
6/11
Chapter 9
6/13
EXAM 4 covering Chapters 7 & 8; Finish Chapter 9
6/18
Experiment 15A(in preparation for CHEM111)
6/20
FINAL EXAM for CHEM110 (cumulative)
6/25
Chapter 10
6/27
Chapter 11
7/2
Experiment 15B
7/3
EXAM 1 covering Chapters 10 & 11
7/5
Experiment 15CD
7/9
Chapter 14 (we are skipping Chapters 12 & 13)
7/11
Chapter 15
7/12
Chapter 16; Experiment 20
7/16
EXAM 2 covering Chapters 14 & 15; Chapter 16
7/18
Chapter 17
7/19
Experiment 21
7/23
Chapter 17
7/25
Chapter 17
7/26
Experiment 22ABD
7/30
EXAM 3 covering Chapters 16 & 17
8/1
Chapter 18 we are doing only the first 3 sections; Chapter 19
8/2
Chapter 19; Experiment 22CEF
8/7
FINAL EXAM for CHEM111 (Cumulative) Check out of lab.
CHEM111 begins
Chem110 Study Guide
Chapter 1
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 terms and equations listed in the summaries on pages 35 – 36.
Chapter 2
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 the names and formulas of the ions listed in Tables 2.3 and 2.4 and be able to
apply them in naming compounds.
5. Know how to systematically name ionic compounds and covalent compounds.
6. Know how to name acids.
7. Know the terms listed in the summaries on pages 70 – 71.
Chapter 3
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 terms listed in the summaries on pages 122 – 123.
Chapter 4
1. Review the polyatomic ions from Chapter 2.
2. Be able to write the molecular, total ionic and net ionic equation for precipitation
reactions and acid/base reactions.
3. Know the solubility rules given on Table 4.5 and be able to apply them.
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 balance redox reactions in acidic or alkaline solution using the half reaction
method.
7. Be able to calculate the molarity of a solution.
8. Be able to do a solution stoichiometry problem.
9. Know the Key Equations on page 123.
10. Know the terms and equations listed in the summaries on pages 178 – 179 except
those associated with section 4.8 that was skipped.
Chapter 5
1. Know the terms system, surroundings and the sign conventions for work and heat.
2. Be able to calculate the internal energy change or enthalpy change for a process.
3. Be able to apply Hess’s Law.
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 terms and equations listed in the summaries on pages 236 – 237.
Chapter 6
1. Know how to convert between pressure units.
2. Review how to convert temperatures between Fahrenheit, Celsius and Kelvin.
3. Know what is STP (Standard temperature and pressure).
4. Know the various gas laws discussed in the chapter.
5. Know the terms and equations listed in the summaries on pages 296 – 297.
Chapter 7
1. Know the relationship between wavelength, frequency and energy.
2. Know the regions of the electromagnetic spectrum.
3. Know the Bohr Model for an atom and the Bohr’s Equation.
4. Know the quantum numbers and what they signify.
5. Be able to give the electron configuration of an atom or ion.
6. Know the periodic trends for atomic size, ionic size, effective nuclear charge,
ionization energy, electron affinity.
7. Know the terms and equations listed in the summaries on pages 358 – 359.
Chapter 8
1. Review the difference between an ionic compound and a covalent compound.
2. Know the following terms: octet, electronegativity, resonance, formal charge.
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 terms and equations listed in the summaries on pages 401 – 402 except
those associated with section 8.4 that we skipped.
Chapter 9
1. Be able to draw the Lewis structure, give the structure type (AB2, etc., as discussed in
class), 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 molecular orbital theory.
5. Know the terms and equations listed in the summaries on pages 454 – 455.
Chem111 Study Guide
Chapter 10
1. Be able to identify the different types of interparticle forces present in a compound and
between different compounds.
2. Know how polarity and solubility are related.
3. Know Henry’s Law.
4. Be able to interpret a phase diagram.
5. Be able to explain surface tension, capillary action and viscosity.
6. Know the key terms and equations listed on page 492.
Chapter 11
1. Be able to construct a simple Born-Haber Cycle diagram.
2. Understand the relationship between vapor pressure and boiling point.
3. Know Raoult’s Law.
4. Be able to use the Clausius-Clapeyron Equation.
5. Know the colligative properties: freezing point depression, boiling point elevation,
osmostic pressure.
6. Know how to calculate the molar mass of a compound using colligative properties.
7. Know the key terms and equations listed on pages 537 – 538.
Chapter 14
1. Understand the concept of entropy and how it affects a reaction’s spontaneity.
2. Understand the concept of free energy and how it is used to predict a reaction’s
spontaneity.
3. Be able to calculate entropy, enthalpy and Gibb’s free energy using the equations
discussed in the chapter and by applying Hess’s Law.
4. Know the key terms and equations listed on pages 692 – 693.
Chapter 15
1. Understand the concept of a reaction rate and the factors that affect a reaction rate.
2. Be able to determine a rate law given experimental data.
3. Be able to confirm a mechanism using experimental data.
4. Understand the concepts of reaction order and half life.
4. Be able to calculate reaction rates, half life and time elapsed for first order and second
order reactions.
5. Be able to use the Arrhenius equation.
6. Understand how a catalyst works.
7. Know the key terms listed on pages 747 – 748.
Chapter 16
1. Understand the concept of a dynamic equilibrium.
2. Be able to write equilibrium constant expressions, Kc or Kp.
3. The relationship between Kp and Kc.
4. Be able to manipulate an equilibrium constant.
5. Understand the concept of a reaction quotient.
6. Understand and be able to apply LeChatelier’s Principle.
7. Be able to calculate an equilibrium constant.
8. Be able to calculate the equilibrium amounts present in a system given an initial
amount of reactants or products and an equilibrium constant.
9. Know the relationship between the Gibbs Free Energy and an equilibrium.
10. Be able to calculate K from ΔG° and vice versa.
11. Know the key terms and equations listed on pages 806 – 807.
Chapter 17
1. Know the different definitions for acids and bases: Arrhenius, Brønsted-Lowry and
Lewis definitions.
2. Understand amphoterism and how it applies to water.
3. Understand the pH scale.
4. Be able to calculate for the [H3O+], [HO¯], pH and pOH of any acid or base.
5. Know the strong acids and bases: HCl, HBr, HI, HNO3, HClO4 and H2SO4 (first
dissociation only).
6. Understand the concept of a strong acid/base and weak acid/base.
7. Be able to write the equilibrium for any acid or base in water.
8. Know how a polyprotic acid dissociates.
9. Be able to calculate the equilibrium amounts of any acid or base.
10. Be able to determine the Ka or Kb or a weak acid or weak base, respectively.
11. Be able to explain the pH of any salt.
12. Understand buffers and be able to calculate the pH of a buffer.
13. Understand solubility equilibria and be able to calculate the equilibrium amounts
present for an insoluble salt as the pure salt in solution or with a common ion
introduced into solution using the Ksp of the salt.
14.Understand how acid-base indicators work.
15. Understand acid-base titrations and be able to calculate the pH at any point along the
titration curve.
16. Know the key terms and equations listed on pages 868 – 869.
Chapter 18 (Sections 18.1 – 18. 3 only)
1. Understand the concept of complex-ion equilibria.
2. Be able to calculate the equilibrium amounts in a complex-ion equilibrium.
Chapter 19
1. Understand cell potentials and cell diagrams.
2. Be able to calculate cell potentials.
3. Be able to use the Nernst Equation.
4. Be able to relate Gibbs Free Energy, the equilibrium constant and cell potential.
5. Understand electrolytic cells and calculate: the amount of metal deposited, current
required, time required during an electrolytic process.
6. Know the key terms and equations listed on pages 947 – 948.