OCCC Chem 1115 Syllabus
COURSE:
CHEM 1115, GENERAL CHEMISTRY I
Oklahoma City Community College, Fall 2011
INSTRUCTOR:
______________________________
PHONE:
682-1611 EXT. ________________
EMAIL:
______________________________
OFFICE LOCATION:
______________________________
OFFICE HOURS:
______________________________
LEARNING MATERIALS
Textbook:
If you plan only to take Chem 1115, please obtain:
Chemistry: The Central Science, Custom 12th Edition (Chem
1115 only) (bundled with the MasteringChemistry™ Student
Access Kit). Brown, LeMay, Bursten, Murphy, and Woodward.
2012. Pearson.
-- OR –
If you plan to take both Chem 1115 and Chem 1215, please
obtain:
Chemistry: The Central Science, Custom 12th Edition (Chem
1115 and 1215) (bundled with the MasteringChemistry™ Student
Access Kit). Brown, LeMay, Bursten, Murphy, and Woodward.
2012. Pearson.
-- OR –
Chemistry: The Central Science 12th Edition eBook with
MasteringChemistry™ Student Access Kit. Brown, LeMay,
Bursten, Murphy, and Woodward. 2012. Pearson.
The access kit is good for two years. If you purchased an
access kit for Chem 1115 or 1215 in the last 20 months, it will
work for this course.
Lab Manual:
Chemistry 1115/0110 General Chemistry I Laboratory Manual.
Oklahoma City Community College. 2011.
Goggles:
Approved chemical splash goggles.
Optional Materials:
Mega Molecules Molecular Geometry kit.
Non-programmable scientific calculator (such as TI-30XA or
Casio FX-260)
OCCC Chem 1115 Syllabus
Fall 2011
COURSE DESCRIPTION
Prerequisite: (R), (W), MATH 1513 or MATH 1533 or both MATH 0403 and high school
chemistry or CHEM 1123. A grade of "C" or better is required in all prerequisite courses.
5 CREDITS. This course is designed for science and engineering majors. The course
covers nomenclature, atomic and molecular structure, stoichiometry, acid/base and other
aqueous reactions, states of matter, phase changes, gas laws, and an introduction to
thermochemistry. Laboratory is an integral part of the course. GenEd Requirement
COURSE COMPETENCIES
As stated in the course description, when you complete this course, you should be able to
apply the principles and theories of chemistry to interpret fundamental chemical
phenomena and predict the results of chemical reactions. You should be able to
demonstrate through tests, homework assignments, and laboratory exercises a basic
knowledge of the periodicity of the elements, inorganic nomenclature, stoichiometry,
metathesis reactions, redox reactions, properties of gases, atomic structure, and molecular
geometry. A list of specific learning objectives relating to these general competencies is
attached.
ATTENDANCE
Oklahoma City Community College requires regular class attendance and punctuality of
students.
EMAIL
Your OCCC email account (it has the form [email protected]) is your official
school email account. You will be held responsible for any course information that comes
to you via OCCC email, so be sure to check it regularly throughout the semester.
WITHDRAWING FROM CLASS:
It is your responsibility to withdraw from the course if you cannot complete the course.
Your professor cannot withdraw you for non-attendance. You can withdraw until the end
of the twelfth week during the Fall and Spring semesters or until the end of the sixth week
in the Summer semester.
ACCOMMODATIONS FOR STUDENTS WITH SPECIAL NEEDS:
Oklahoma City Community College Complies with Section 504 of the Rehabilitation Act
and the Americans with Disabilities Act. Students with disabilities who seek
accommodations must make their request by contacting the Office of Student Support
Services located on the first floor of the main building near SEM entry 3 or by calling 6827520. All accommodations must be approved by the Assistant Director, Student Disability
Services.
p. 2
OCCC Chem 1115 Syllabus
Fall 2011
ASSESSMENT OF STUDENT LEARNING
Oklahoma City Community College is committed to providing quality educational
experiences to all students and to striving for continuous improvement in its programs and
services. Student assessment is vital to the educational process and can be of significant
value to you and to the students who follow you.
To ensure that adequate assessment information is available to allow OCCC to
continuously improve programs and services, you may be asked to participate in personal
interviews; take program and/or general education assessments, which could be tests; give
oral presentations, write assignments, take surveys, or engage in other activities. You may
be asked to complete the assessments, tests, and other activities during designated times,
which may include class periods. These opportunities are your chance to help OCCC
improve the courses, programs, and services which could affect you and will certainly
impact students in the future.
DECLARATION OF A MAJOR
Students enrolled in this course who plan to complete a certificate or a degree should
officially declare a major and request a faculty advisor in the area of their major.
The procedure for declaring a major is as follows:
1. Request a Declaration of Major form from the Office of Admissions and Records.
2. Meet with a counselor in Counseling and Assessment or a faculty member in your
major to clarify certificate or degree selection. Return completed form to Counseling
and Assessment or to the faculty member who gave you the form.
3. Receive notification of an advisor assignment by mail after processing is completed.
Some degree programs have a special application procedure and require that a student
be assigned to a counselor before being admitted to the program. For Diversified
Studies majors, degree plans must be submitted for approval to the Office of
Academic Division Support Services. Contact a counselor for additional information.
GOGGLE POLICY
You are required to purchase your own pair of chemical splash goggles and to wear those
goggles at all times in the laboratory. You may purchase your goggles in the OCCC
bookstore. If you choose to purchase goggles elsewhere, they must be approved by your
professor. Woodworking goggles are NOT acceptable. If your goggles have vent covers
that can be opened, they must be closed at all times during use.
The OCCC Chemistry faculty has a zero tolerance policy on goggle violations. Failing to
wear or removing your goggles during lab may result in dismissal from the laboratory
and a grade of zero for that lab. Repeated violations of the goggle or safety rules and
policies may result in a grade of “F” for the course.
p. 3
OCCC Chem 1115 Syllabus
Fall 2011
PERSONAL ATTIRE POLICY
You must wear appropriate personal attire in the chemistry laboratory: a shirt with
sleeves that covers the shoulders and entire torso and either pants or a skirt that
covers the entire leg. Tank tops, tube tops, spaghetti straps, midriff shirts, shorts, and
short dresses are not acceptable. In general, wearing a T-shirt, jeans and tennis shoes will
be appropriate to meet the lab safety rules.
Shoes that cover the entire foot, including the toes, the top of the foot, and the heel
must be worn at all times in the chemistry laboratory. Sandals, flip-flops, slippers,
Crocs®, and other open or perforated shoes are not permitted in the chemistry lab area.
You will not be allowed to complete the lab if you are not dressed appropriately.
GRADING
The grade assigned for this course will be determined by your performance on unit tests, a
comprehensive final, online quizzes, and lab assignments. Detailed information about each
grading area is outlined below.
1) Exams (6 x 100 pts = 600 pts). There will be six unit exams worth 100 points each
plus a comprehensive final exam worth 100 points for a total of 700 points. You are
expected to take all exams in class. If you miss the in-class exam, you must take the makeup exam in the Test Center within 7 calendar days.* If you do not take the exam in the
specified time, you will receive a zero for that exam. Ten percentage points will be
deducted from the make-up exam score regardless of the reason for missing the inclass exam.
If you take a unit exam in class and receive less than 60%, you may re-take that exam.*
You will receive the higher score from the two exams up to a maximum of 70%. All retests must be completed within 14 days of the day the exam was given in class. You may
not re-test on the comprehensive final exam or on a make-up exam.
*You are limited to a total of two retests and/or make-up exams during the semester.
In other words, you can re-test on two units you failed, you can make up one exam and retake one exam you failed, or you can make up two exams.
2) Comprehensive Final (100 points). A comprehensive final exam covering material
from all of General Chemistry I will be given in class on the last day of the semester.
Objectives for the final are given later in the syllabus. You are expected to take the
comprehensive final exam in class. You may not re-test on the comprehensive final. A
make-up exam will be given only under extraordinary circumstances (as defined and
approved by your instructor).
In order to receive an “A,” “B,” or “C” in the course, a student must earn the
minimum final exam score described in the table in the “Grading Scale” section.
Failure to achieve the minimum final exam score will result in a one letter grade
reduction in the student’s overall course grade. See the “Grading Scale” section for
details.
p. 4
OCCC Chem 1115 Syllabus
Fall 2011
3) Quizzes (6 x 15 pts = 90 pts). There will be six online quizzes given throughout the
semester. Quiz questions will often be taken directly from or based upon homework
problems. Each quiz is worth fifteen points giving a total of 90 points possible on the
quizzes. No late quizzes will be accepted. A score of zero will be recorded for any
missed quiz. Due dates for quizzes will be specified by your instructor (check your lecture
schedule). Typically, you will have about ten days to access and complete an online quiz.
You MAY ask your instructor for help with online quiz questions or any homework
problems.
Computer access for MasteringChemistry online quizzes: Since each quiz is open for
several days, technical problems discovered on the due date of a quiz are not
considered a viable excuse for not completing the quiz on time. We strongly
recommend that you access each quiz on the first day it becomes available so that your
instructor can help you resolve any technical difficulties you may encounter. Although you
do have to purchase access to MasteringChemistry, you do not have to access it with your
own computer. The computers in the Physical Science Center (or any student accessible
computer on campus) may be used to access and complete your MasteringChemistry
assignment.
4) Lab Exercises (145 pts). There are 12 lab exercises, ten worth 10 points each, one
worth 20 points, and one worth 25 points. Lab reports (data sheets) will be submitted to
your lab instructor who will grade the reports. The lab instructor will forward your lab
grades to your lecture instructor at the end of the semester for use in determining your final
grade.
IN ORDER TO PASS THIS COURSE, YOU MUST COMPLETE AND RECEIVE A
SATISFACTORY GRADE (≥ 2 pts) ON AT LEAST 10 OF THE 12 LAB REPORTS.
You must do at least 10 of the 12 laboratory experiments -- you are expected to complete
all 12 -- and submit completed data sheets for those labs. There will be only one week in
the semester that may be used to make up a missed lab, and we strongly advise you to
complete all 12 labs and reports. Although only 10 labs are required to pass the course,
please understand that the lab grade consists of 145 points: if you choose not to make up
a lab, that lab grade will be a zero.
Labs are due at the start of the following pre-lab period. Late labs – this includes
makeup labs - will be assessed a five point penalty. Labs that are turned in after start of
the pre-lab period will be considered late, regardless of the reason.
To receive full credit, all questions on the data sheet must be answered, appropriate
calculations must be shown on the data sheet or on attached sheets of paper (as specified in
the lab instructions), results must be within the expected range, and all calculations should
be done according to the rules for significant figures.
You can lose points on labs according to the following criteria:
Late lab - 5 point penalty
Incomplete lab report (i.e. some questions or calculations omitted) - 1 to 4 point penalty,
depending upon how many calculations or questions are omitted
Poor results - 0.5 to 2 point penalty, depending upon how bad the results are
Calculation errors - 0.5 to 3 point penalty, depending upon how many errors are made
Incorrect answers to questions - 0.5 to 1 point each
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OCCC Chem 1115 Syllabus
Fall 2011
Incorrect use of significant figures - 0.5 to 1 point penalty, depending upon how many
errors are made
(Notice that it would be relatively easy to fall below the 2 point minimum required for
passing this class if you submit an incomplete data sheet with a few calculation errors and
poor results or incorrect responses to questions. Submitting a late lab means that you
should take extra care in making sure the lab is complete and your calculations are
correct so that you do not fall below the 2 point minimum.)
Grading Scale:
Total points possible = 600 + 100 + 90 + 145 = 935 points
Your course grade will be determined primarily using the overall percentage of points
earned during the course. However, in order to receive an “A” or “B” in the course, you
must also score at least 70.0% on the comprehensive final exam. In order to receive a
“C” in the course, you must also score at least 60.0% on the comprehensive final
exam. See the grading scale table below.
Failure to satisfy the minimum final exam score requirements will result in a one
letter grade reduction in your overall course grade. For example, a student who earns
95.3% of the 935 points possible but scores a 69.5% on the comprehensive final exam will
receive a “B” in the course. Similarly, a student who earns 79.2% of the 935 points
possible but scores a 59.5% on the comprehensive final exam will receive a “D” in the
course.
Grade
%
A
B
C
D
F
90.0 – 100
80.0 – 89.9
70.0 – 79.9
60.0 – 69.9
59.9 or less
Minimum Final Exam
Score
70.0%
70.0%
60.0%
none
none
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OCCC Chem 1115 Syllabus
Fall 2011
TRANSFERRING LAB GRADES
You must be enrolled in a section of CHEM 0110. If you need to complete any labs at all,
you will be expected to attend the first lab session to complete safety activities. However,
if you have completed some or all of the Chem 0110 lab work at OCCC within the past
calendar year, you may transfer the grades for those completed labs to your current Chem
1115 lecture instructor and you will only have to attend those labs which you did not
complete previously. To transfer your lab grades, please email Dr. Steven Shore at
[email protected] the following information: 1) your name and student ID number, 2) the
name of your former Chem 0110 lab instructor, 3) the name of your former Chem 1115
lecture instructor, 4) the name of your current Chem 1115 instructor, and 5) either the name
of your current lab instructor or your current lab section number. The request for lab grade
transfer should be made by the end of the second week of class.
INCOMPLETES
An "I" grade may be given to students under extenuating circumstances. Please understand
that the issuing of an "I" grade is the instructor's prerogative and not a "right" of the
student.
ACADEMIC DISHONESTY
Academic dishonesty (such as copying from someone else or using unauthorized notes on
exams) will result in a zero being given for the work in question and a record of the
incident will be forwarded to the Office of the Vice President for Academic Affairs.
Further disciplinary action may result.
THINGS TO REMEMBER
You are not allowed to use programmable calculators on tests or quizzes in class or in
the Test Center. A simple scientific calculator is all you need.
For make-up exams or retests
1) Know the Test Center operating hours!
2) The Test Center will not give out tests later than one hour before closing time.
3) You must have an OCCC photo ID to receive a test.
4) The Test Center closes promptly at the posted times. You will be required to turn
in your test by closing time.
5) Make-up exams are subject to a 10 percentage point penalty and must be
completed within 7 calendar days of the in-class exam.
6) Re-tests on failed exams must be completed within 14 calendar days of the inclass exam.
7) You are limited to a total of two retests and/or make-up exams during the
semester.
p. 7
OCCC Chem 1115 Syllabus
Fall 2011
SAFETY AND SECURITY EMERGENCY PROCEDURES
The health and safety of all our students, faculty, and staff are OCCC's prime concern. The
procedures outlined below are designed to deal with emergencies of various types.
Students should always follow the lead of their instructors.
Fire
First notification will come from the fire alarm horns, sirens, and strobes. The class should
gather their belongings, exit the building using the nearest exit, and move to a parking lot.
Do not use the elevators. No alarm should be treated as a false alarm. Horns, sirens, and
strobes are only used for fire alarms.
Fire (Special Considerations)
If someone in your area is not physically capable of descending the stairwell, please ensure
that they remain in the "area of safe refuge" located just inside each upper-level enclosed
fire stairwell. There are emergency phones located near each of these areas.
Medical
For all medical related issues push the "emergency" button located on each classroom
phone. The phone will display your room number, allowing for fast response to your
location. All security officers are trained as first responders and will assist in guiding
EMSA to your location. Treat all bodily fluids as if they were contaminated.
Bomb
If you receive a bomb threat, document as much information as possible and push the
"emergency" button on the phone. If the decision to evacuate is given, the phone will
sound an alarm and display a text message. The class should gather their belongings, exit
the building using the nearest exit, and move to an open grassy area. Please turn off all
wireless devices. (Cell phones, radios, laptops, and other portable devices.)
Weather
Tornado warnings that include OCCC will be sent directly to the classroom phone. The
phone will sound an alarm and display a text message. The class should gather their
belongings, move away from exterior glass and exits, and move to safer areas. These areas
are lower-level interior classrooms, restrooms, and stairwells. You should familiarize
yourself with the safer areas near your classroom(s). If the city/county sirens are sounding
and OCCC is not in the warning area a message will be sent to the classroom phone
advising this information.
Disturbance/Threats
If someone is causing a disturbance in a classroom call security immediately. Push the
"emergency" button located on each classroom phone. Distance yourself from that person,
do not place yourself in the person's exit path and remove all potential weapons from the
area. Shelter in place: If there is an armed person or shooter on campus: Close and lock
your hallway doors. Turn off the lights, shut the blinds or move away from exposed areas.
Use desks, tables and other objects to provide protection. Updated information will be sent
to the classroom phone.
p. 8
OCCC Chem 1115 Syllabus
Fall 2011
UNIT OBJECTIVES FOR CHEM 1115
UNIT 1
INTRODUCTION: MATTER AND MEASUREMENT
Reading: Chapter 1, Chapter 2 (2.5 only, p. 49-52), Chapter 7 (7.1 only, p. 250-251)
Homework:
Chapter 1: 1.1, 1.4, 1.7, 1.11, 1.13, 1.14, 1.19, 1.24, 1.25, 1.27, 1.28, 1.29, 1.33, 1.35, 1.37,
1.39, 1.40, 1.47, 1.48, 1.49, 1.51, 1.65, 1.68, 1.74
Chapter 2: 2.3, 2.37, 2.38, 2.94 a-f
1.
Define and/or recognize an acceptable definition or example of the terms listed in the
"Summary and Key Terms" section at the end of the chapter.
2.
Given the name of a chemical element, you will be able to supply its symbol; given the
symbol of a chemical element, you will be able to write its name. You will be
responsible for the following elements:
ELEMENT
SYMBOL
ELEMENT
SYMBOL
Aluminum
Antimony
Arsenic
Barium
Bismuth
Boron
Bromine
Cadmium
Calcium
Carbon
Cesium
Chlorine
Chromium
Cobalt
Copper
Fluorine
Gold
Helium
Hydrogen
Iodine
Iron
Al
Sb
As
Ba
Bi
B
Br
Cd
Ca
C
Cs
Cl
Cr
Co
Cu
F
Au
He
H
I
Fe
Lead
Lithium
Magnesium
Manganese
Mercury
Neon
Nickel
Nitrogen
Oxygen
Phosphorus
Platinum
Potassium
Radon
Silicon
Silver
Sodium
Sulfur
Tin
Uranium
Zinc
Pb
Li
Mg
Mn
Hg
Ne
Ni
N
O
P
Pt
K
Rn
Si
Ag
Na
S
Sn
U
Zn
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OCCC Chem 1115 Syllabus
Fall 2011
3.
For any of the following quantities: length; mass; time; temperature; or amount of
substance, you will be able to list the base (fundamental) unit and its symbol in the
International System of Units (the "SI" system).
4.
Given the value of a temperature in either °F, °C, or K and given the conversion
equations, you will be able to convert the given value to either of the other two
temperature scales.
5.
Given two of the three variables - mass, volume, and density, be able to calculate the
third variable.
6.
Given a number expressed as a decimal or in exponential notation, you will be able to
indicate how many significant figures are present in that number. Given an indicated
calculation involving addition, subtraction, multiplication and/or division, you will be
able to perform the calculation correctly and express the answer to the proper number of
significant figures.
7.
Given a measured value, including its units, you will be able to convert the given value to
a new specified unit using dimensional analysis. You will be able to state or use the
metric-metric conversions for mega, kilo, centi, milli, and micro.
8.
Using information given in a problem, you will be able to write an appropriate
conversion factor and use the conversion factor (with or without other conversion factors)
to solve a problem using dimensional analysis.
9.
Given the periodic table, you will be able to do the following:
a. classify a given element as being a metal, nonmetal, or metalloid;
b. classify a given element as being an alkali metal, alkaline earth metal, halogen, or
noble gas;
c. classify a given element as being a main group (representative) element, transition
metal, lanthanide, or actinide;
d. name two elements which are liquids at "room conditions" of temperature and
pressure;
e. list the elements that occur naturally as diatomic molecules.
10.
Given a list of physical properties, you will be able to indicate which are characteristic
properties of metallic elements and which are characteristic properties of nonmetallic
elements.
11.
Given a list of chemical properties, you will be able to indicate which are properties of
metals and which are properties of nonmetals.
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OCCC Chem 1115 Syllabus
Fall 2011
UNIT 2
ATOMS, IONS, AND MOLECULES
ELECTRONIC STRUCTURE AND PERIODIC PROPERTIES OF ATOMS AND IONS
Reading: Chapter 2, Chapter 6, and Chapter 7 (7.1 - 7.6)
Homework:
Chapter 2: 2.17, 2.25, 2.27, 2.43, 2.45, 2.49, 2.51, 2.55, 2.57, 2.63, 2.65, 2.67, 2.99, 2.103,
2.104
Chapter 6: 6.9, 6.10, 6.23, 6.35, 6.51, 6.53, 6.55, 6.56, 6.65, 6.69 (omit e – write complete and
condensed electron configurations and draw orbital diagrams), 6.71
Chapter 7: 7.25, 7.37, 7.45, 7.47
1.
Define and/or recognize an acceptable definition or example of the terms listed in the
"Summary and Key Terms" sections at the end of Chapter 2, Chapter 6, and Chapter 7
(Sections 7.1-7.6 only).
2.
You will be able to state or recognize a statement of the Law of Conservation of Mass
and the Law of Constant Composition.
3.
Given some combination of the number of protons, the number of neutrons, the number
of electrons, the isotopic mass, and the complete isotopic symbol for some isotope, you
will be able to supply the missing component(s) of the above list for that isotope.
(Unit 2 objectives continued on next page.)
p. 11
OCCC Chem 1115 Syllabus
4.
Fall 2011
Given the name of a common ion, you will be able to write its symbol including the
correct charge. Given the symbol of a common ion, you will be able to write its name.
You will be responsible for the following common ions:
ION
SYMBOL
ION
SYMBOL
Hydrogen
Lithium
Sodium
Potassium
Rubidium
Cesium
Silver
Magnesium
Calcium
Strontium
Barium
Zinc
Iron (II)
Iron (III)
Aluminum
H+
Li+
Na+
K+
Rb+
Cs+
Ag+
Mg2+
Ca2+
Sr2+
Ba2+
Zn2+
Fe2+
Fe3+
Al3+
Fluoride
Chloride
Bromide
Iodide
Oxide
Sulfide
Nitride
Phosphide
F
Cl
Br
I
O2
S2
N3
P3
OH
CN
NO3
C2H3O2
SO42
HSO4
Ammonium
NH4+
Hydroxide
Cyanide
Nitrate
Acetate
Sulfate
Hydrogen sulfate
(bisulfate)
Carbonate
Hydrogen carbonate
(bicarbonate)
Phosphate
CO32
HCO3
PO43
5.
Using the names and symbols of the common ions identified in the previous objective
and a list of the names and symbols of less common ions, you will be able to name and
write the formula for compounds composed of these species.
6.
Given the formula of an ionic compound formed from the cations and anions, you will be
able to write the name of the compound. Given the name of a compound formed from
these ions, you will be able to write the chemical formula.
7.
Given the name of one of the following household products, you will be able to write the
name or formula of the ionic compound present in it: baking soda, table salt, and bleach.
8.
Given the appropriate equations and constants, and given the value of one of the three
characteristics of a photon (its wavelength, frequency, or energy), you will be able to
calculate the values of the remaining two characteristics. Given the energy of a covalent
bond, you will be able to calculate the wavelength, frequency, or energy of a photon
needed to break that bond.
9.
You will be able to recognize statements about the quantum mechanical model of the
atom. You will be able to recognize definitions of the four quantum numbers used in the
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OCCC Chem 1115 Syllabus
Fall 2011
quantum mechanical model of the atom. You will also be able to recognize allowed sets
of quantum numbers.
10.
Given the atomic number of any representative element or first-row transition element,
you will be able to represent the electron configuration in complete form, in standard
shorthand or "core" notation, or as an orbital diagram.
11.
You will be able to represent the electron configuration for a specified ion in complete
form, in shorthand or “core” notation, or as an orbital diagram.
12.
You will be able to state or recognize statements describing the Pauli Exclusion Principle,
Hund's Rule, and the aufbau principle.
13.
You will be able to state the general trends within the periodic table affecting the
magnitude of each of the following properties: first ionization energy, electron affinity,
atomic size, and metallic character. For a given pair of elements, you will be able to
indicate which has the larger or smaller value of any of these properties.
14.
For an atom of a given element and an ion of that same element be able to state which has
the larger or smaller size. For atoms and ions within the same group or in an
isoelectronic series, you will be able to predict the relative size of the ions.
15.
You will be able to answer questions or solve problems relating to the previous unit. You
will be able to answer questions and solve problems incorporating material from the past
unit with the current unit objectives.
p. 13
OCCC Chem 1115 Syllabus
Fall 2011
UNIT 3
INTRODUCTION TO COVALENT BONDING AND MOLECULAR GEOMETRY
Reading: Chapter 2 (p. 64-66), Chapter 8, Chapter 9 (9.1-9.3 only)
Homework:
Chapter 2: 2.59, 2.69, 2.70, 2.71, 2.72
Chapter 8: 8.1, 8.10, 8.13, 8.14, 8.17, 8.19, 8.39, 8.42, 8.47, 8.48, 8.51, 8.53, 8.55, 8.57, 8.63,
8.65, 8.90, 8.92
Chapter 9: 9.3, 9.4, 9.22, 9.23, 9.26, 9.28, 9.30, 9.31, 9.32, 9.36, 9.39, 9.44
1.
Define and/or recognize an acceptable definition or example of the terms listed for the
appropriate sections in the "Summary and Key Terms" section at the end of each chapter.
2.
Given a formula of a compound formed between two nonmetals, you will be able to write
the name of the compound; given the name of a compound formed between two
nonmetals, you will be able to write the formula.
3.
Given the name of an acid, you will be able to write its chemical formula; given the
chemical formula of an acid, you will be able to write its name.
4.
Given the name of one of the following household products, you will be able to write the
name or formula of the chemical present in it: water, ammonia, natural gas, vinegar,
hydrogen peroxide, drinking alcohol, rubbing alcohol, and nail polish remover.
5.
For a given atom or monatomic ion, you will be able to write its correct electron-dot
(Lewis) symbol.
6.
Given a series of binary compounds or a series of specific covalent bonds and the
relevant electronegativities, you will be able to predict which would be most polar or to
rank them in order of their polarity.
7.
For a given molecule or ion, you will be able to draw the Lewis structure representation
(including all resonance structures).
8.
Given a set of correct Lewis structures for a molecule or polyatomic ion, you will be able
to assign formal charges to all of the atoms and evaluate which of the structures best
describe the bonding in that molecule or polyatomic ion.
9.
Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the
electron-domain geometry (electron-pair geometry/VSEPR classification) for the
molecule or polyatomic ion.
10.
Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the
molecular structure (or geometry) of that molecule or ion based on the VSEPR model.
11.
For a given molecular structure of a molecule or polyatomic ion, you will be able to
represent the bond dipoles and tell if the species is polar or non-polar.
12.
You will be able to answer questions or solve problems relating to previous units. You
will be able to answer questions and solve problems incorporating material from past
units with the current unit objectives.
p. 14
OCCC Chem 1115 Syllabus
Fall 2011
UNIT 4
STOICHIOMETRY
Reading: Chapter 3
Homework:
3.1, 3.11, 3.13, 3.19, 3.21, 3.23 (a,d), 3.25a, 3.31, 3.33, 3.35, 3.37, 3.39, 3.43,
3.45, 3.49, 3.51, 3.53, 3.61, 3.63, 3.65, 3.67 (a,b), 3.73, 3.75, 3.77, 3.81, 3.101
1.
Define and/or recognize an acceptable definition or example of the terms listed in the
"Summary and Key Terms" section at the end of the chapter.
2.
Given a chemical equation with all of the formulas correct, you will be able to properly
balance that equation.
3.
Given the formula of a compound, you will be able to calculate its formula mass or molar
mass.
4.
Given a periodic table and the formula of a substance or given the necessary mass data,
you will be able to calculate the percent composition of that substance.
5.
Given the periodic table and the formula of a substance, you will be able to interconvert
between the mass, the number of moles, the number of molecules or atoms of that
substance, or the number of moles or atoms of an element within a compound.
6.
Given the percent composition or molecular formula of a compound determine its
empirical formula; given mass data obtained by quantitative analysis calculate empirical
formulas; given the formula mass and empirical formula of a compound determine its
molecular formula.
7.
You will be able to work the following types of stoichiometry problems: mass-mass;
mass-moles; moles-moles; moles-formula units; mass-formula units.
8.
Given a balanced equation and mass data for a specified reaction, you will be able to
determine the limiting reactant in that reaction, calculate the maximum (theoretical)
yield, and calculate the percent yield of that reaction given the mass of product actually
obtained.
9.
You will be able to answer questions or solve problems relating to previous units. You
will be able to answer questions and solve problems incorporating material from past
units with the current unit objectives.
p. 15
OCCC Chem 1115 Syllabus
Fall 2011
UNIT 5
REACTION TYPES AND SOLUTION STOICHIOMETRY
Reading: Chapter 4
Homework: 4.1, 4.2, 4.5, 4.7, 4.11, 4.13, 4.16, 4.19, 4.21, 4.22, 4.23, 4.26,4.30, 4.31, 4.35,
4.37, 4.39, 4.41, 4.43, 4.45, 4.49, 4.50, 4.51, 4.61, 4.63, 4.65, 4.67, 4.69, 4.71, 4.73, 4.75, 4.77
4.79, 4.81, 4.83, 4.85, 4.92, 4.95, 4.107
1.
Define and/or recognize an acceptable definition or example of the terms listed in the
"Summary and Key Terms" section at the end of the chapter.
2.
You will be able to explain and/or illustrate the basis of the strong interaction between
two water molecules or between a water molecule and an ion.
3.
Given the reactants side of an equation representing a metathesis reaction, you will be
able to predict the correct formulas of the products and their physical states.
4.
Given a balanced molecular equation for a metathesis reaction and the physical states of
all the components, you will be able to write complete ionic and net ionic equations for
that reaction.
5.
You will be able to list the seven strong acids and eight strong bases by name and
formula.
6.
You will be able to write a balanced neutralization reaction for a specified acid and base.
7.
Given a set of oxidation number rules, you will be able to determine oxidation numbers
of elements and identify whether an element was oxidized or reduced in a reaction and
whether it was an oxidant (oxidizing agent) or reductant (reducing agent) in the reaction.
8.
Given a balanced molecular equation for the oxidation of a metal by an acid or a salt of
another metal, you will be able to write the total ionic and net ionic equations for the
reaction.
9.
Given the molarity of a specified solution, you will be able to determine the volume of
solution required to obtain a certain mass or number of moles of solute or a specified ion.
10.
Given the molarity of a solution to be prepared or the molarity of a specified ion, you will
be able to determine the mass of a solid solute needed to prepare a specified volume of
the appropriate solution. You will be able to describe how to prepare a specified volume
of a solution with a specified molarity of solute or ion.
11.
You will be able to calculate the molarity of a solution given the volume of the solution
and the mass or the number of moles of the solute in the solution.
p. 16
OCCC Chem 1115 Syllabus
Fall 2011
12.
Given the appropriate information, you will be able to calculate the concentration of a
solution prepared by diluting a specified volume of a stock solution.
13.
Given the appropriate information, you will be able to calculate the volume of a stock
solution that is needed to prepare a specified volume of a more dilute solution. You will
be able to determine the volume of water needed to make the solution.
14.
Given the appropriate information, you will be able to describe the steps required to
prepare a specified solution by diluting a stock solution.
15.
Given the concentration of a standard solution and a balanced equation representing a
neutralization reaction, you will be able to determine the concentration of an acid or base
of unknown concentration.
16.
You will be able to answer questions or solve problems relating to previous units. You
will be able to answer questions and solve problems incorporating material from past
units with the current unit objectives.
p. 17
OCCC Chem 1115 Syllabus
Fall 2011
UNIT 6
GASES, PHASE CHANGES, AND INTRODUCTION TO THERMOCHEMISTRY
Reading: Chapter 10
Homework: 10.2, 10.21, 10.28, 10.30, 10.35, 10.36, 10.39, 10.41, 10.42, 10.45, 10.49, 10.51,
10.53, 10.57, 10.59, 10.65, 10.69, 10.71, 10.75, 10.93, 10.121 (a), 10.129
Reading: Chapter 5 (p. 159 – 176)
Homework: 5.4, 5.27, 5.39a, 5.43a-c, 5.46 a-b, 5.47a-b, 5.51a-d, 5.53a
Reading: Chapter 11 (p. 438 – 442)
Homework: 11.39, 11.43, 11.45, 11.46, 11.59
1.
Define and/or recognize an acceptable definition or example of the terms listed in the
"Summary and Key Terms" section at the end of Chapter 10 as well as the definition of a
real gas.
2.
You will be able to write the correct symbols for the following units of pressure and to
use dimensional analysis to convert between any two of them: atmosphere, millimeter of
mercury, inches of mercury, pounds per square inch, torr, pascal, kilopascal, bar, and
millibar.
3.
You will be able to identify the SI unit of pressure and define it in terms of fundamental
SI units.
4.
Be able to state or recognize statements given in either words or as mathematical
expressions for each of the following relationships:





Pressure-Volume Law (Boyle's Law)
Temperature-Volume Law (Charles's Law)
Avogadro's Hypothesis and Avogadro’s Law
Dalton's Law of Partial Pressures
Graham's Law of Gas Effusion
5.
Given values of the universal gas constant and three of the four variables (P, V, T, n) in
the Ideal Gas Law equation, you will be able to calculate the value of the unknown
parameter.
6.
You will be able to state the values for "standard temperature and pressure" (or STP) and
for "standard molar volume."
7.
You will be able to determine the new pressure, new temperature, or new volume of a
sample of gas in which there are changes in the other variables.
8.
Given the necessary ideal gas data, you will be able to calculate the molar mass or
density of a gas.
p. 18
OCCC Chem 1115 Syllabus
Fall 2011
9.
You will be able to use the Ideal Gas Law equation to carry out stoichiometric
calculations for reactions involving gases when you are given reactions and necessary
data.
10.
You will be able to calculate the mole fraction of a component present in a mixture of
gases and calculate the partial pressure of that component when given the total pressure.
You will be able to find the partial pressure of a gas collected over water.
11.
You will be able to state or recognize statements describing the postulates of the kinetic
molecular theory of gases.
12.
You will be able to state or recognize conditions under which real gases depart from ideal
behavior and state or recognize the reasons for non-ideal behavior.
13.
You will be able to define or recognize an acceptable definition or example of each of the
following: freezing, boiling, fusion, melting, sublimation, deposition, vaporization,
condensation, boiling point, normal boiling point, melting point, normal melting point,
triple point, critical temperature, critical pressure, critical point, heat, work, internal
energy, kinetic energy, potential energy, specific heat, endothermic, exothermic, heat of
fusion, and heat of vaporization.
14.
Given the amount of heat gained or lost by a system and the amount of work done on or
by the system, you will be able to calculate the change in internal energy of the system.
15.
You will be able to identify a specified physical change of state as being either
endothermic or exothermic.
16.
Given appropriate relationships, you will be able to use dimensional analysis to convert
between any two appropriate units for heat.
17.
Given any three of the following: heat, mass, temperature change, or specific heat, you
will be able to calculate the fourth quantity.
18.
Given the heat of fusion or heat of vaporization of a substance and the mass or number of
moles of that substance, you will be able to calculate the amount of heat gained or lost.
19.
Given a thermochemical equation, you will be able to calculate the enthalpy change for a
reaction involving a given number of moles or grams of a reactant or product. Given a
thermochemical equation, you will be able to determine the enthalpy change for the
reverse reaction.
20.
You will be able to explain the various segments of a heating/cooling curve. You will be
able to explain the impact that intermolecular forces have during the phase changes that
occur. Given the heat of fusion, heat of vaporization, and specific heat of a substance,
you will be able to calculate the heat necessary to completely convert a given mass of the
substance from one temperature and physical state to another.
p. 19
OCCC Chem 1115 Syllabus
Fall 2011
21.
You will be able to use a phase diagram to determine the state (phase) of a substance
given its temperature and pressure. You will be able to state which phases are in
equilibrium on the boundary lines on a phase diagram. You will be able to locate the
triple point of a substance on a phase diagram and identify the equilibrium it defines.
Given a phase diagram, you will be able to describe the phase changes in a substance as
its temperature is changed at constant pressure or as its pressure is changed at constant
temperature.
22.
You will be able to answer questions or solve problems relating to previous units. You
will be able to answer questions and solve problems incorporating material from past
units with the current unit objectives.
p. 20
OCCC Chem 1115 Syllabus
Fall 2011
CHEM 1115
Objectives for Comprehensive Final Exam
1. Given the name of a chemical element, you will be able to write its symbol. Given the
symbol of an element, you will be able to write its name. You will be responsible for the
elements given in objective 2 of unit 1.
2. Given two of the three variables—density, mass, and volume—you will be able to calculate
the third.
3. You will be able to convert from one set of units to another set of units using dimensional
analysis. You will be able to state or use the metric-metric conversions for mega, kilo, centi,
milli, and micro.
4. You will be able to classify an element as:
a. Metal, nonmetal, or metalloid
b. Alkali metal, alkaline earth metal, halogen, or noble gas
c. Main group, transition metal, lanthanide or actinide
5. You will be able to list the elements that occur naturally as diatomic molecules.
6. Given the name of a common ion, you will be able to write its symbol including the correct
charge. Given the symbol of a common ion, you will be able to write its name. You are
responsible for the common ions given in Objective 4 of Unit 2.
7. Given the formulas of ionic compounds formed from the cations and anions described in the
previous objective, you will be able to write the name of the compound. Given the name of a
compound formed from these ions, you will be able to write its chemical formula.
8. Given the formula of a binary molecular compound, you will be able to write the name of the
compound. Given the name of such a compound, you will be able to write its formula.
9. You will be able to write the electron configuration either in complete form or using core
notation for any main group atom or ion.
10. You will be able to recognize definitions or descriptions of the four quantum numbers used
in the quantum mechanical model of the atom. You will also be able to recognize allowed
sets of quantum numbers.
11. You will be able to predict the relative size of the following: any two atoms in the periodic
table, two atoms/ions in an isoelectronic series, an ion and its parent atom, or two ions in the
same group.
12. Given the formula for a molecular compound or a polyatomic ion, you will be able to draw a
valid Lewis structure for that substance.
13. Given the formula for a molecular compound or a polyatomic ion, you will be able to give
the name of the electron domain geometry and the molecular geometry for that substance.
14. Given the names and/or formulas of the reactants and products involved in a chemical
reaction, you will be able to write a balanced chemical equation.
p. 21
OCCC Chem 1115 Syllabus
Fall 2011
15. You will be able to work the following types of stoichiometry problems: mass-mass, massmoles, moles-moles, mass-volume, and volume-volume.
16. Given the names and/or formulas of two reactants and the solubility guidelines, you will be
able to write a balanced molecular equation, complete ionic equation, and net ionic equation
for a precipitation or acid/base (neutralization) reaction.
17. Given the appropriate information, you will be able to calculate the concentration of a
solution prepared by diluting a specified volume of a stock solution.
18. Given the appropriate information, you will be able to calculate the volume of a stock
solution that is needed to prepare a specified volume of a more dilute solution.
19. Given the appropriate information, you will be able to describe the steps required to prepare a
specified solution by diluting a stock solution.
20. Given mass of solute and total volume, you will be able to calculate the molarity of a
solution.
21. You will be able to recognize statements of the following gas laws either in words or as
mathematical expressions: Boyle’s Law, Charles Law, and Avogadro’s Law.
22. You will be able to apply the previous gas laws to determine whether volume of a gas will
increase, decrease, or stay the same when a specified change is made in the temperature,
pressure, or number of moles of the sample of gas.
23. Given values of the universal gas constant and three of the four variables (P, V, T, n) in the
Ideal Gas Law equation, you will be able to calculate the value of the unknown parameter.
24. You will be able to determine the new pressure, new temperature, or new volume of sample
of gas in which there are changes in the other variables.
25. Given any three of the following: heat, mass, temperature change, or specific heat, you will be
able to calculate the fourth quantity.
26. Given the heat of fusion or heat of vaporization of a substance and the mass or number of moles
of that substance, you will be able to calculate the amount of heat gained or lost.
27. You will be able to identify a specified physical change of state as being either endothermic or
exothermic.
28. Given a thermochemical equation, you will be able to calculate the enthalpy change for a
reaction involving a given number of moles or grams of a reactant or product. Given a
thermochemical equation, you will be able to determine the enthalpy change for the reverse
reaction.
29. You will be able to use a phase diagram to determine the state (phase) of a substance given its
temperature and pressure. You will be able to state which phases are in equilibrium on the
boundary lines on a phase diagram. You will be able to locate the triple point of a substance on
a phase diagram and identify the equilibrium it defines. Given a phase diagram, you will be
able to describe the phase changes in a substance as its temperature is changed at constant
pressure, or as its pressure is changed at constant temperature.
p. 22
OCCC Chem 1115 Syllabus
Fall 2011
p. 23
OCCC Chem 1115 Syllabus
Fall 2011
Final Grade Calculations:
Total points possible = 600 + 100 + 90 + 145 = 935 points
Grading Scale (provided that the minimum score on the final exam is attained):
842 points or higher for an “A”
748 – 841 points for a “B”
655 – 747 points for a “C”
561 – 654 points for a “D”
560 points or lower for an “F”
Tests are 75% of your grade. Quizzes and labs together represent 25% of your grade.
You should keep track of your grades throughout the semester, recording grades as papers are
handed back to you.
Grade record:
Exam 1
Exam 2
Exam 3
Exam 4
Exam 5
Exam 6
Final*
Total
_____
_____
_____
_____
_____
_____
_____
______
Lab 1
Lab 2
Lab 3
Lab 4
Lab 5
Lab 6
Lab 7
Lab 8
Lab 9
Lab 10
Lab 11
Lab 12
_____
_____
_____
_____
_____
_____
_____
_____
_____
_____
_____
_____
Total _____
Quiz 1
Quiz 2
Quiz 3
Quiz 4
Quiz 5
Quiz 6
____
____
____
____
____
____
Total _____
Total of all points: __________
*Must meet minimum required score for an A, B, or C. See “Grading Scale” in “Grading”
section.
Note: You can get a pretty good idea of your standing in the class by looking at the average of
your exams. If your average is one or two points away from the next grade level, the points for
the labs and quizzes could bring your final grade up to the next level. For instance, if you have
an 88 average on your exams, you can still get an “A” provided that you have most of the points
for the labs and quizzes. On the flip side, if you have done poorly on quizzes or a number of labs
were late, your grade could potentially drop a letter grade.
p. 24