General Chemistry II
Chemistry 111 Section D
Spring 2005
University of New England
Instructor: Dr. Clinton S. Nash
Office/lab: Decary 353; Phone: ext 2152; e-mail: cnash@une.edu
Class Website: http://faculty.une.edu/cas/cnash/CH111
Office Hours: I have a very liberal policy on office hours. Always assume that it is okay to see
me unless I tell you otherwise. If you come to my office and I am unable to speak with you, I’ll
just let you know and I’ll do my best to work with you and come up with a mutually agreeable
time to get together.
Text: Chemistry: The Molecular Nature of Matter and Change, 3rd Ed., by Silberberg, McGrawHill, 2003 (ISBN 0072396814). Required course text.
Study Guide and Solutions Manual: To accompany Silberberg. Optional.
Lab Manual: The Lab Manual will be provided; the production costs are included in your
laboratory fee.
Course Objectives: Chemistry 111 is a study of several important topics related to the behavior
of chemical and physical systems. The material in this course serves as a foundation for all
subsequent courses in chemistry and disciplines that rely on chemistry (e.g., biology, medical
technology, environmental science, oceanography, and biochemistry). This course should be of
interest even to those not intending to pursue study in the sciences, because an understanding of
the principles discussed will make you better able to make informed decisions in our increasingly
complex world. This course will assume that you have a solid understanding of the principles and
concepts introduced in CHE-110, the successful completion of which is a prerequisite for this
course. You probably will find the material more interesting, more cohesive, and more
challenging than the material in CHE-110, and notice that it flows in a very logical progression
as we explore the factors that describe and control chemical reactions.
By the end of this course, you should have gained an understanding of the principles and
applications of material in four main subject areas: 1) Thermodynamics - the study of energy
relationships in systems, which tells us whether or not chemical reactions are likely to occur
spontaneously when substances are mixed, 2) Chemical Kinetics - the study of how fast or slow
chemical reactions proceed, 3) Chemical Equilibrium, including solubility and acid/base
equilibria, which will provide a foundation for understanding the complex dynamic behavior of
natural systems, and 4) Electrochemistry - the study of electron-transfer processes and
electrochemical cells. We also will explore some of the properties of solutions.
In order to succeed in this course, you must keep up with the material daily by
completing reading assignments and problem sets in a timely fashion. If you get behind early in
the semester, things will get worse quickly, as the material builds on what has come before it. We
generally will not have time to review in class, so if you feel deficient or rusty in any area of
CHE-110, you ought to review the appropriate sections of Silberberg and/or your CHE-110
notes, and seek help outside of class. See your instructor if you have questions or would like to
review CHE 110 material. Don't hesitate to ask questions!
Class Attendance Policy: I do not take attendance in class, it’s your own business. However, it
is usually very obvious to me who is skipping class and I am usually not as accommodating to
outside assistance for those students unless there is a reason that absences have been excessive
(illness, etc.) Note especially that "make-up" exams and quizzes are not given, so do not miss an
exam or quiz unless you can provide documented evidence of illness or other serious problem.
See the instructor in advance if you anticipate a schedule problem. Quizzes may not be made up
under any circumstances. If documented evidence of illness, etc., is presented, the missed quiz
score may be dropped from your total point collection calculation.
Lab Attendance Policy: Because lab is an integral part of the course, you are encouraged not to
miss any lab sessions. Each experiment missed will lower your final course grade because of the
points you will have missed. Two or more missed labs will result in automatic failure in the
course if they are not made up. If you miss your regularly scheduled lab period, you should see
your lab instructor immediately, so you can make arrangements to complete the experiment in
another lab section, before the chemicals and equipment are removed from the lab. Make every
effort to complete a missed experiment within 1 week of when it was scheduled; otherwise
reagents and equipment may not be available.
Things to get: (In addition to the text and lab manual)
1. Approved Safety Goggles (required). They must be worn at all times when anyone is
working in the lab.
2. Nonprogrammable Calculator (optional). Only nonprogrammable calculators will be
allowed during exams. Basic calculators will be provided to those needing them for exam use.
Due dates for assignments and lab reports: Due dates for all assignments will be announced
when the assignments are given. Most lab reports will be due before leaving the lab on the day of
the experiment, unless you are informed otherwise by your lab instructor. There will be a 10%
per week late fee on all work (except homework problem sets, which will not be accepted after
their due dates). Absolutely no work will be accepted after 5:00 pm on the last day of
classes.
Laboratory: See the separate schedule for the sequence of lab experiments. This sequence will
follow the lecture as closely as possible, but, unfortunately, it is not possible to keep lab and
lecture completely coordinated. You are expected to read carefully each experiment and any
associated handouts and text references BEFORE coming to lab, so you are prepared to work
when the lab opens. This is especially important in cases where an experiment is to be done
before the relevant material is covered in class. Some experiments are purposely scheduled ahead
of the lecture material; they are intended as “discovery-based” learning experiences. If you have
questions about an experiment, see your course or lab instructor well before the lab starts (not 10
minutes before lab; this indicates lack of preparation on your part).
Exams & Quizzes: Exams are designed to allow you to demonstrate your understanding of, and
ability to synthesize and use, the material covered. You will be expected to apply your
knowledge to problems that may not be exactly like ones you have seen in class or on homework
sets. In other words, memorization of example problem solutions is insufficient for success in
this course; you must be able to think critically and apply your knowledge in order to solve
problems. Weekly quizzes (Fridays) are designed to encourage you to keep up with the material
and provide frequent feedback on your level of mastery of the material, but they are not meant to
simulate exam questions. In general and in an attempt to incentivize your doing the homework,
your quizzes will be based on the weekly assigned homework problems. Programmable
calculators are not permitted when taking exams; you will be provided with a calculator for
your use during exams if you do not have a nonprogrammable model. The Final Exam will be an
American Chemical Society Standardized exam, comprehensive over the full year of General
Chemistry.
Abbreviated Chem 110 Outline: This brief outline is included as a guide for you if you need to
review. You should understand the concepts in all of the areas listed below. As noted above, if
you feel deficient, see the instructor for review help.
General Topic Area
Chapter
in
Silberberg
I. Introductory Material: Matter & Measurement
1
II. Components of Matter: Atoms, Compounds, Formulas, and Nomenclature
2
III. Composition Stoichiometry, Chemical Reactions, & Reaction Stoichiometry
3
IV. Major Types of Chemical Reactions; Chemistry in Aqueous Solutions
4
V. Atomic Structure
7
VI. Electron Configurations and Chemical Periodicity
8
VII. Chemical Bonding; molecular structure/geometry (excluding molecular orbital theory)
9, 10, 11
VIII. Properties of Gases and the Kinetic-Molecular Theory
5
IX. Intermolecular Forces and Properties of Liquids
12
(through 12.5)
Evaluation: TENTATIVE grade distribution (some values are approximate):
Exams (3 @ 100 pts each)
Quizzes (Fridays; 11 @ 20 pts each)
Lab: reports, quizzes, etc
Final Exam (full year comprehensive)
Total (approx)
300
200
200
150
850
Final grades will be determined by the total number of points accumulated divided by the total
possible number of points. Course grade assignment is based on the standard scale: 90-100% =
A-/A, 80-89% = B-/B/B+, and so on. You may estimate your course standing at any point in the
semester by computing your own percentage and comparing with those norms.
A Word (or two) About Math Proficiency: In addition to having an understanding of the
principles discussed in CHE-110, you should be adept (not to be confused with inept) at
performing basic mathematical operations. You will be expected to carry out basic algebraic
operations including those involving natural and common logarithms. If you are uneasy about
math, do something about it NOW, before it's too late. Inability to do math will make it much
more difficult for you to master the chemistry content in the course. This course involves
considerably more mathematical problem-solving than did CHE-110.
Homework Problems: Homework assignments (readings and problems) will be distributed on a
regular basis (reading assignments also are included in the outline which follows). It is your
responsibility to keep up with the work as it is covered in class and as suggested on the course
outline. The best way to learn the material and prepare for tests is to work as many problems as
possible and seek to understand the principles behind the problems, not merely the mechanics of
the problem-solving process. If you do not truly understand the material, you will be unable to
solve problems that are not exactly like the ones in the assignments. You will be expected to
think in this course, not simply memorize material. Work on the assignments regularly and as
the material is presented in class; do not wait until two days before a test or quiz to work out 4
weeks' worth of problems.
Exam and Quiz Schedule: Quizzes will be given at the end of class (~10 minutes) each Friday
except weeks in which an exam is given. Exams will be given outside of class time to remove the
50-minute time constraint and allow you to demonstrate more thoroughly your accumulated
knowledge and skills. Although designed to be completed in one hour, exams will be allowed at
least two hours to work. Exams will start at 6:00 p.m. on the dates indicated below (schedule is
tentative). If you have a schedule conflict with an exam (e.g., work commitment or other
scheduled class), see the instructor in advance to arrange an alternative time. If you are enrolled
with the OSSD, you must make exam arrangements with the instructor in advance.
Exam I:
Exam II:
Exam III:
Thursday, February 24. Alfond 113 or 205
Thursday, March. 31. Alfond 113 or 205
Thursday, April. 28. Alfond 113 or 205
The Final Exam will be held during the Final Exam Week and will be scheduled by the
Registrar’s Office. Please do not make post-semester travel plans until you receive your Final
Exam schedule. No alternative Final Exam times will be available.
Lab Grading Procedure: Will be discussed by your lab instructor.
Lab Safety Lecture: If you have not attended a lab safety lecture during this academic year (i.e.,
since September), you must attend one before attending lab. Consult Dan Callahan, ext. 2490.
Chemistry 111 Course Outline
Spring, 2005
NOTE: Sections of the course text containing the relevant information are included in
parentheses
0. Catch Up Material, Intermolecular Forces
1. Types of IMF’s
2. Phase Changes
3. Properties of Liquids/Water
I. Physical Properties of Condensed Phases II: Solutions
1. The Solution Process; The Role of IMFs in solubility (13.1)
2. Energy Changes in Solution Processes (13.2)
3. Factors Affecting Solubility (13.3)
4. Concentrations; Saturated Solutions, & Molar Solubility (13.4)
5. Colligative Properties (13.5)
II. Thermodynamics: Can we predict reaction spontaneity?
A. Thermochemistry
1. Forms of energy; 1st Law of Thermodynamics; etc. (6.1)
a. internal energy; kinetic & potential energy
b. work and heat
c. state functions
2. Enthalpy (6.2)
a. exothermic vs. endothermic processes
3. Calorimetry (6.3)
a. constant volume calorimetry
b. constant pressure calorimetry
4. Thermochemical Equations (6.4)
5. Hess's Law (6.5)
6. Standard Enthalpies of Formation; calculating Horctn (6.6)
B. Thermodynamics of Chemical Systems
1. Spontaneous Processes; the Second Law of Thermodynamics (20.1)
2. Entropy (20.2)
3. Third Law of Thermodynamics
4. Gibbs Free Energy and reaction spontaneity (20.3)
III. Chemical Kinetics: How fast will spontaneous reactions proceed?
A. Rates of reactions and factors that affect rate (16.1 – 16.2)
B. Rate Laws; reaction order (16.3)
C. Time vs. Concentration: The Integrated Rate Equations (16.4)
E. Activation energy and temperature dependence of rate (16.5)
F. Kinetics Theories: Collision Theory and Transition State Theory (16.6)
F. Reaction mechanisms (16.7)
G. Catalysts (16.8)
IV. General Aspects of Chemical Equilibrium: Change and Constancy in Dynamic Systems
A. Dynamic equilibrium; reaction reversibility (17.1)
B. Reaction Quotients and the Equilibrium Constant (17.2; 17.4)
C. Heterogeneous Equilibria; KC and KP (17.3)
D. Calculations & applications involving equilibrium constants; LeChatlier's Principle
(17.5 - 17.6)
E. Equilibrium and Thermodynamics (20.4)
1. relation between Go and the equilibrium constants
V. Solubility Equilibria; Ksp (19.3)
1. unsaturated, saturated and supersaturated solutions
2. determining solubility from Ksp values
3. common ion effect
4. predicting formation of a precipitate
5. the effect of pH on solubility
VI. Acid/Base Equilibria
A. Acids and bases: introduction and review (4.1; 4.4; 18.1)
B. Ionization of water (18.2)
1. pH scale
C. Strong and weak acids and bases (18.3 – 18.6)
1. definitions
2. pKa and pKb
3. conjugate acid/base pairs
4. finding solution pH from total acid or base concentration
5. factors affecting acid/base behavior
D. Buffers (19.1)
E. Diprotic and polyprotic acids and bases
F. Hydrolysis & Salts (18.7)
G. Acid - Base titrations (19.2)
VII. Oxidation/Reduction Reactions and Electrochemistry: Electron Transfer in Chemical
Systems
A. Oxidation - Reduction reactions (4.5)
1. Intro.; Definitions (review; 4.5; 21.1)
2. oxidation numbers (review; 4.5)
3. balancing redox reactions by ion-electron (half-reaction) method (20.1)
4. Descriptive examples of selected redox reactions
B. Electrochemical Cells I: Galvanic Cells (21.2 - 21.3)
1. Cell potentials; standard cell potentials
2. Standard reduction potentials (20.4)
3. Effect of concentration on Ecell ; the Nernst Equation (21.4)
C. Spontaneity of redox reactions; Cell potentials and Thermodynamics (21.4)
F. Examples of Important Galvanic Cells: Batteries and Corrosion (21.5 – 21.6; read on
your own)
H. Electrochemical Cells II: Electrolytic cells (21.7)
Note: You are expected to come to lab prepared to do the experiment. This means that you
should carefully read the experimental background and procedure BEFORE getting to lab,
including any text references.
Note 2: Background information on any experiment can be found in Brown/LeMay/Bursten. If
the lab’s material has not yet been covered in class, it is your responsibility to prepare by reading
the appropriate text sections.
Note 3: Pre-Lab quizzes may be expected at the start of each lab period. Material for such
quizzes will be drawn from the Lab Manual and text references.
Note 4: Anyone leaving the lab untidy will have points be deducted from the lab report score.
Group areas (e.g., balance area or reagent shelf) left messy will result in the deduction of points
from the report scores of all students in the offending lab section.
Laboratory Experiment Schedule
General Chemistry II
Spring 2005
(CHE 111 Lab - all sections)
Author
First Lab Date
Experiment Title
Date
Lab
Jan 24 25 26 27
Jan 31 Feb 1 2 3
Feb 7 8 9 10
Feb 14 15 16 17
Feb 21 22 23 24
Feb 28 Mar 1 2 3
Mar 7 8 9 10
Mar 21 22 23 24
Mar 28 29 30 31
Apr 4 5 6 7
Apr 11 12 13 14
April 18 19 20 21
April 25 26 27 28
Synthesis & Analysis of Aspirin wk. I
Synthesis & Analysis of Aspirin wk II
Colligative Properties of Solutions wk I
Colligative Properties of Solutions wk II
Thermochemistry
Chemical Kinetics
Chemical Equilibrium wk I
Chemical Equilibrium wk II
Solubility Equilibria
Acid/Base Equilibria, Hydrolysis
Oxidation-Reduction Reactions
Electrochemical Cells wk I
Electrochemical Cells wk II