CHEMISTRY 1211:
GENERAL CHEMISTRY I
A
Course in the General Education Program
Program
Description: The General Education Program at KSU offers a
common academic experience for all its students. In a series of interrelated courses in the
liberal arts and sciences, it provides the opportunity for them to acquire the
intellectual skills and knowledge characteristic of educated persons. Thus, it lays the foundation for success in
their academic, professional, and personal lives. Whereas the major program contributes to a
college education depth in a designated specialization, the General Education
Program provides breadth by introducing and connecting a variety of
disciplines.
Program Goals: The General
Education Program at KSU has five goals.
During the course of the program, students should achieve the
following:
·
develop
productive habits of mind
·
develop
effective communication skills
·
expand knowledge
and understanding
·
expand creative
capabilities
·
exhibit understanding of the impact of ethical and aesthetic
values.
Course Description: Chemistry
1211 is the first course in a two-semester sequence covering the fundamental
principles and applications of chemistry for science majors. Course content includes electronic structure
of atoms and molecules, bonding fundamentals, fundamentals of chemical
reactions, and energy.
University
Policies
Special
Needs Students:
If you are a student with special needs as
approved by the disAbled Student Support Services
office, you must indicate this to the instructor with the letter from the disAbled Student Support Services office within the
first two weeks of classes. After
private consultation with the instructor special testing will be provided.
Late Registration: A $30.00 transaction fee will be
charged for permission for late registration after the regular drop/add has
ended. If you wish to be added to a course that is full, there may be an
opening after the last drop date. In
such a case, you have 2 days to “late register” in order to get into the course.
A $30.00 transaction fee will be charged.
Integrity: Every KSU student is responsible for
upholding the provisions of the Student Code of Conduct, as published in the
Undergraduate Catalog. Section II of the
Student Code of Conduct addresses the University’s policy on academic honesty,
including provisions regarding plagiarism and cheating, unauthorized
access to University materials, misrepresentation / falsification of University
records or academic work, malicious removal, retention, or destruction of
library materials, malicious / intentional misuse of computer facilities and /
or services, and misuse of student identification cards. Incidents of alleged academic misconduct will
be handled through the established procedures of the University Judiciary
Program, which includes either an “informal” resolution by a faculty member,
resulting in a grade adjustment, or a formal hearing procedure, which
may subject a student to the Code of Conduct’s minimum one semester suspension requirement.
Behavior: It is the purpose of the institution to provide
a campus environment, which encourages academic accomplishment, personal
growth, and a spirit of understanding and cooperation. An important part of
maintaining such an environment is the commitment to protect the health and
safety of every member of the campus community. Belligerent, abusive, profane,
threatening and/or inappropriate behavior on the part of students is a
violation of the Kennesaw State University Student Conduct Regulations.
Students who are found guilty of such misconduct may be subject to immediate
dismissal from the institution. In addition, these violations of state law may
also be subject to criminal action beyond the University disciplinary process.
Departmental
Policies
Departmental
On-Line Lecture Notes (See Dr. Leon Combs with questions): This course is taught in an on-line
mode, as well (Chem 1211, Section 05). Students are required to develop independent
study skills for this course. Access to
the On-Line Lecture notes is available from the link below. The web site is available for your assistance
in learning the material. Note that the
assignments on the pages are for the students in the on-line course. Chem 1211: http://GenChem1.kennesaw.edu/
A Note From the Department Chair (Dr. Leon Combs): Some general "fatherly" advice: "W" grades on your transcript are a
negative factor in evaluating your academic performance. Some professional schools go through a
transcript, substitute “F” for every “W”, and recalculate the GPA. For all students, and especially for anyone
serious about a professional school of any kind, we would recommend that your
transcript should show no more than four "W" grades. Even if you have only four "W's"
when you graduate, you should have an excellent reason for each one of them
(sickness, death in the family, etc.).Please take your academic experience very seriously,
and have a frank discussion with an advisor about your strengths and weaknesses
so that you do not waste time in an area where you are not likely to be
successful. Your instructors will do what they can to help all students
succeed, but each student has to do their part in the learning process. It is very important to understand
that a lot of "W" grades on your transcript is
very negative. You should decide during the "drop/add" period if you
should stay in this course rather than waiting until later in the semester when
you will get a "W" if you withdraw then.
Computing Facilities: There is a Science Computer Lab on the Second Floor
of the
Chemistry 1211
Policy
Fall 2005
UPDATED
Course: General Chemistry I, Chem
1211, Section 02 and Section 06, Fall 2005
Instructor: Dr.
Daniel J. Williams
Room 431
Science
Phone:
770-423-6174
Email: dwilliam@kennesaw.edu
http://science.kennesaw.edu/~dwilliam
Prerequisite: High
school chemistry or CHEM 1151
Corequisites: Chem 1211L, MATH 1112 or MATH
1113 or placement in Math 1190 on their
completion.
Textbook: Silberberg, M.S. Chemistry,
4th Ed., McGraw-Hill,
Class: Section
02: Mondays and Wednesdays
Section 06: Tuesdays and Thursdays
Tutoring: Provided
free of charge in SC 452 at scheduled times.
Times are posted on the door and on my homepage. Supplemental Instruction may also be provided
and will be announced.
Last
Day
to
Withdraw:
Last
Day
of
lectures:
|
Holidays: September
3 - 5: |
Labor Day Break, NO
CLASSES, Saturday – Monday |
|
Holidays: Nov. 23 - 27: |
Fall Break, NO CLASSES,
Wednesday – Sunday |
Email Policy: One of the course requirements is an
email address. This is not an option. You have a free student account through the
university or use whatever service provider you desire. When
e-mailing the instructor, please use Chem 1211 in the
subject heading of the e-mail. Other
subject topics can then be added. For
example: for a student with a question
on Chapter 4, question 22 and other questions, the subject may be “Chem 1211, Chapter 4, Question 22 and other
questions”. Any e-mail that does not
look official is considered “spam” or is considered to contain a virus and is
deleted without opening or reading.
Electronic Device
Policy: In order to minimize the level of
distraction, all beepers and cellular phones must be on quiet mode during class
meeting times. Students who wish to use a computer/PDA for note-taking need
prior approval of the instructor since key clicks and other noises can distract
other students. Recording of lectures by any method requires prior approval of
the instructor. You must leave
the room to make a phone call. Please do
so as quietly as possible.
Homework: Problem
solving is strongly recommended as part of your study habits. It will not be collected or graded,
however. The colored problems in your
text have answers given in the back.
There are also online problems through www.chemskillbuilder.com which is
part of your text package. Registration
is online, and you will have access to self-graded problem sets. Your instructor will be working some of the
book problems as illustrations during class.
Calculator:
You must bring the approved
calculator to every class and every test and exam. Only approved calculators may be used
on tests and exams. The
following are the approved Calculators for Chem
1211. Other calculators need prior
approval by the instructor. Cell phones,
Blackberries, PDA’s, etc may NOT be used as calculators for exams. They must be stowed and in the off position
during the exam (airplane mode).
Examples of approved calculators are shown below. Make sure
your calculator batteries are fresh. YOUR
INSTRUCTOR IS NOT A SOURCE OF EXTRA CALCULATORS. DO NOT ASK.
TI 30Xa Casio FX 300W Plus Casio FX 250 HC Casio FX 260 Solar
Other Study
Material: Thinkwell Chemistry I CD-Rom. 2001 Edition. Available in the bookstore. The study guide to accompany your text and
the problem solutions manual may also be helpful, but they are optional.
WebCT: We will be using WebCT for bulletin board messages
and other communication. Access to the
Internet can be found all over the campus. The site URL is http://courses.kennesaw.edu. Leave messages for the class on the
discussion forum. Ask questions and answer questions. This counts as part of
your class participation.
Course
Content: Please see below tentative schedule showing
chapters to be covered in the text.
Syllabus
Changes: Syllabus
changes, when they occur, will be announced in class and posted on the Chem 1211 WebCT site
Office Policy: My office is
in room 431, and office hours will be announced in class as well as on my
homepage. My general policy is you are
welcome whenever my door is open.
(You'll always find my door open if I'm in my office.)
Attendance
Policy: Class attendance is
strongly recommended but not mandatory.
The only exception to this is on exam days and the final exam (see below
under Make-up Policy). Informal
monitoring of attendance will be considered when determining class
participation, however. Attendance on a
regular basis is considered in assigning participation points. If you are not attending on a regular basis,
please don't expect special tutorial sessions in my office or in the SI
sections. Regular attendance doesn't
guarantee success, but you will increase your odds if you take advantage of the
class instructional period. You will be
responsible for all announcements and material presented in class.
Class
Participation: As mentioned above, one way to
participate in class is, of course, to be there. Additionally, asking relevant questions
regarding problems and concepts, or answering questions when asked are also
considered in class participation. A big
area of participation is the bulletin board which will net the largest number
of participation points. E-mailing questions to the instructor is also
considered as participation provided that you are attending class regularly.
Testing and
Grading: There will be five unit
exams. Your lowest exam score will be
dropped in averaging your unit exams. Topics
covered by each unit exam are found in the textbook chapters listed for each
unit. There will also be one two-hour American Chemical Society standardized final
exam. If you score in the top 10% of the
nationwide standard in the ACS exam, you will receive an automatic A in the
course no matter what your scores were up to this point.
Final Exam: Since
the final exam is a standard ACS exam, if you do better on the final than what
your unit exam average was after dropping the lowest grade, your final will
replace your unit exam average. For
example, if your average for the unit exams came out to be 78%, but on the
final you scored 85%, the final exam grade will substitute for your unit exam
average so they both will be 85%. The
top 10% rule cited above still holds as well.
Make-up Policy: There are no
make-up exams. You must attend every
exam session as well as the final exam.
If you miss a unit exam, that will constitute your dropped score. If you miss a final exam,
that will constitute failure in the course unless extenuating
circumstances can be documented.
Course Breakdown
and Grading
Scale:
70% Unit Exams
(17.5% each)
25%
Final Exam
5% Class Participation (including WebCT)
Grade Score
A 90
and above
B 80-89
C 70-79
D 60-69
F 59 and below
Chemistry
1211
Tentative Schedule
Fall
2005
UNIT I Chapters/Sections
EXAM:
Section 02: Monday, September 12th
Section 06: Tuesday,
September 13th
UNIT
II
EXAM:
Section 02: Monday,
October 3rd
Section 06: Tuesday,
October 4th
UNIT
III
EXAM: Section
02: Monday, October 24th
Section 06: Tuesday,
October 25th
UNIT IV
EXAM:
Section 02: Monday, November 14th
Section 06: Tuesday,
November 15th
UNIT V Ch.
6 – All Sections
EXAM:
Section 02: Monday, December 5th
Section 06: Thursday,
December 1st
FINAL EXAM Section 02: Monday, December 12th
Section
06: Tuesday, December 13th
UNIVERSITY
SYSTEM OF
Principles
of Chemistry (CHEM 1211)
Common
Learning Outcomes
Common
Student Learning Outcomes for the Core Curriculum
Quantitative
Reasoning and Mathematics:
Quantitative reasoning and mathematics
will be characterized by logic, critical evaluation, analysis, synthesis,
generalization, modeling, and verbal, numeric, graphic, and symbolic problem
solving.
Scientific
Reasoning:
Scientific reasoning will be
characterized by understanding and applying scientific method, laboratory
techniques, mathematical principles, and experimental design to natural
phenomena.
Content-based
Learning Outcomes for Principles of Chemistry
As the result of instruction, we expect
students successfully completing the Principles of Chemistry I and Principles
of Chemistry II courses to understand and remember the following concepts and
principles:
Properties
of Matter
1.
Chemistry is the study of the composition and
properties of matter, and how those properties are affected by changes in
composition and external conditions.
2.
All matter has mass and takes up space, and is
composed of particles interacting through forces. The properties of matter depend, in part, on
the relative strength of interacting forces.
This model of matter is useful for explaining the general properties of
the three phases of matter (solid, liquid, gas) and the transitions between
phases.
Atomic
Theory
- All matter is composed of just over
100 different types of particles, called atoms. Matter may be composed of a single type
of atom (an element), or different types of atoms may bond to each other
in fixed proportions to form compounds (molecules or crystals). A chemical reaction occurs
when atoms rearrange their bonding structures, which may include adding or
removing atoms to the basic chemical unit, resulting in new compounds.
- Atoms combine chemically as whole
units; therefore, a pure compound may be identified by its chemical
formula. Different types of atoms
have different relative masses; therefore, the number of particles in a
fixed sample of a pure substance may be calculated by dividing by the
relative mass of the atoms in the substance. The mole is a unit of measurement
that has been defined to expedite the conversion between the mass of a
substance and the number of particles in a substance. One mole is the quantity of a substance
such that the relative mass of all the atoms in the chemical formula is
equal to that mass of the substance in grams.
- It has proven useful in the study of
chemistry to recognize different types or classes of reactions; some
examples are replacement, combination, combustion, and acid-base
reactions.
Thermochemistry: Temperature, Heat and Energy
- Energy is stored in chemical
bonds. Therefore, energy may be
absorbed or released as chemical bonds are broken and formed in a chemical
reaction. Exothermic reactions
release heat as a result of a reaction, resulting in warmer surroundings;
endothermic absorb heat in a reaction, resulting in colder
surroundings. Enthalpy is a measure
of the amount of heat absorbed or released in a chemical reaction.
- Heat and work are two methods for
transferring energy from one
substance to another. Heat
involves random motions of the particles of a substance; work results from
non-random motions.
- Temperature is a property of matter;
it is proportional to the average kinetic energy of the particles of a
substance. The addition or removal
of heat usually (but not always) results in an increase or decrease in temperature,
respectively. However, heat added
to or removed from a substance may result in other changes in the energy
of the substance besides an increase or decrease in random kinetic energy.
The Gaseous
State
9. Four
fundamental properties of all gases are pressure, volume, temperature, and
quantity. These properties are related
to each other mathematically in a relatively simple way. Observing two properties at a time while holding
the other two constant results in the empirical gas laws; an equation relating
all four properties simultaneously is called the ideal gas law. The ideal gas law is a very useful but
approximate result; variations have been added to the ideal gas law to make it
more closely reflects the behavior of real gasses.
10. Kinetic-molecular
theory assumes that an ideal gas consists of point-like particles that only
interact when they collide, and conserve kinetic energy before and after a
collision. The pressure of gaseous
systems is described as collisions of the point-like particles with the walls
of the container. The ideal gas law may
be derived from the assumptions of the theory and the application of classical
mechanics to a large aggregate of point-like particles.
11. Measurements made on gaseous systems have lead to the identification of
an absolute temperature scale. The
lowest possible temperature in this scale is zero, designated as absolute
zero. An ideal gas (in theory) would
possess no energy at absolute zero, and therefore exhibits no pressure and have
no volume.
Atomic Structure
12. Experimental
evidence supports the concept of a nuclear atom: a positively charged core which occupies less
than 1% of the volume of the atom surrounded point-like negatively charged
electrons. The positively charged core,
or nucleus, is very massive compared to the electrons surrounding it. The motion of the electrons is
unspecified: they do not travel around
the nucleus in regular or predictable
paths, but out best mathematical model suggest they are most likely to be found
in specific regions of space known as orbitals.
13. A useful model
of the nucleus suggests it is composed of positively charged protons and
neutral neutrons, held together
by a ‘strong force’. The number of
protons determines the type of atom; the sum of protons and neutrons determines
the relative mass of the atom.
14. Chemical bonding involves a balance of attractive and repulsive forces
between the electrons and nuclei. Most
descriptions of bonding characterize chemical bonds in terms of the electrons
only. Electrons can be described by
quantum numbers, which identify the mostly likely locations of the electrons
in space and also their relative energies.
Quantum numbers are very helpful in explaining the number and types of
bonds that an atom may form with other atoms.
Periodicity and Chemical Bonding
15. The structure
of the periodic chart is the result of electron quantum numbers. The outermost electrons (valence electrons)
in a column have certain quantum numbers that are the same, and therefore those
elements generally bond and behave
chemically in similar ways. An
orbital may hold either 0, 1, or 2 electrons, but
never more than two electrons. Elements in a row, or period, of the Chart are
generally adding electrons to a set pf orbitals with
the same ‘principal’ quantum numbers.
The start of a new period represents a significant increase in the
energy of an electron compared to the previous period.
16. Experimental evidence has shown that the last column of the periodic
table contains a set of mainly unreactive atoms: the noble gases. They share the common property of having
completely filled orbitals in their valence
shell. This configuration results in an
energetically stable atom. One guiding
principle of chemical bonding is that attaining the same ‘electron configuration’
as the noble gasses is desirable, and is often a consequence for atoms in a
compound after a chemical reaction.
17. Chemical bonds
that result in the transfer of electrons from one atom to another are called
ionic bonds; chemical bonds that result from the sharing of electrons are
called covalent bonds. The transfer of
electrons results in the formation of charged chemical species, called
ions. Most chemical bonds are neither
purely ionic nor purely covalent in nature. Covalent bonds are often imagined
to be the end result of the overlap of atomic orbitals,
leading to a new set of ‘molecular’ orbitals.
18. A method of
accounting for valence electrons and their known properties has been developed
which is able to help predict bonding patterns in many small molecules and ions
(Lewis structures).
Geometry, Molecular Structure, and
Properties
19. Application of the basics of electrostatic repulsion leads to a
systematic method for determining the equilibrium geometry of a molecule. Geometry, bond strength, the distribution of charge
(dipoles), and the resulting intermolecular forces determine the properties of
pure substances in the liquid and solid states.
Process-based
Learning Outcomes for Principles of Chemistry
As the result of instruction, we expect
students successfully completing the Principles of Chemistry I and Principles
of Chemistry II courses to be able to successfully complete the following
tasks:
1. Write correct
formulas for compounds from their names, and vice versa. Identify the meaning of a chemical formula.
2. Balance simple
chemical reactions. Explain or interpret
the meaning of the
coefficients of a balanced
chemical reaction and any subscripts.
3. Report
numerical answers to word problems using the correct number of significant
figures, and evaluate the error in a measurement or calculation.
4. Solve word
problems based on realistic chemistry situations, using appropriate
mathematical equations associated with the subject at hand and correctly
substituting data found in the word problem in the equation(s) in order to
solve for an unknown quantity.
5. Use dimensional
analysis to perform mathematical operations, such as converting between the
mass and moles of substances using data obtained from the periodic chart,
chemical formulas, and balanced equations.
6. Communicate
ideas and concepts using appropriate grammatical forms in both oral and written
formats.