Florida State College at Jacksonville Syllabus:
CHM 2046C: General Chemistry II 4 cr.
Section: 309985
Summer
Term 2009
SITE: D-211/D204
DAY/TIME: Lecture: Tuesday
and Thursday* 7:00-10:00 p.m. D-210
Lab: Thursday 8:00*-10:00 p.m. D-204
Pretesting: Tuesday
and Thursday 6:00-7:00 p.m.; 10:00-10:30 p.m.
FCCJ
Course Description:
This course, a continuation
of General Chemistry and Qualitative Analysis I, stresses chemical equilibrium,
chemical kinetics, electrochemistry, oxidation-reduction and selected families
of metals and non-metals. Laboratory work includes studies of ionic equilibrium
in aqueous solutions and semi-micro qualitative analysis. Six contact hours:
three lecture hours, three laboratory hours. A.A., A.S., A.A.S.
Prerequisites: grade of C or better in CHM 2045C.
(3 class hours, 3 lab hours, 4 credit hours)
Required
Textbook:
Text Web Site: http://www.pearsonhighered.com/educator/academic/product/0,3110,0131993232,00.html
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Chemistry, 5/E (text
used by Dr. Lorenzo and Dr. Gant for 2045C) Publisher: Prentice Hall |
Grading Outline for Students using McMurray 5th edition:
McMurray 5th
edition: http://www.fccj.us/chm2046/46grdSum09McMurray.htm
Exam#1
11. Solutions and Their Properties
12. Chemical Kinetics
Exam#2
13. Chemical Equilibrium
14. Aqueous Equilibria:
Acids and Bases.
Exam#3
15. Applications of Aqueous Equilibria
16. Thermodynamics: Entropy, Free
Energy, and Equilibrium
Exam#4
17. Electrochemistry
22. Nuclear Chemistry
Exam#5
7. Covalent Bonds and Molecular Structure and Hybrid Orbitals
23. Organic Chemistry
24.
Biochemistry
Companion Web
Site: http://wps.prenhall.com/esm_mcmurry_chemistry_5/
Old Lecture
Text, Laboratory Text, Supplies, and Materials (Textbook Option):
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6th Edition © 2006* *(some may have 7th Edition sold in
Bookstore) 1322 Pages Case
Bound 8 1/2 x 10 ISBN: 053499766X Book
is an Old Edition only the 7th Edition is in Bookstore (Grading
outline will be developed week by week for the 7th edition.) CHM 2046C covers Chapter 11, 13-20, 23
in Eight Modules |
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Table of Contents |
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CHM 2046C
General Chemistry and Qualitative Analysis II 11.
Carbon--More Than Just Another Element. Interchapter: THE CHEMISTRY OF LIFE: BIOCHEMISTRY 13.
Intermolecular Forces, Liquids, and Solids. Interchapter:
THE CHEMISTRY OF MODERN MATERIALS Interchapter:
THE CHEMISTRY OF THE ENVIRONMENT
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Laboratory Research Notebook in
the bookstore, ISBN #r 9781930882508
for ~$12.50
(McMurray
Lab Manual Not required-Optional)
Required: Scientific Calculator (minimal non-alphanumeric)
Optional Texts/Online Activity:
Student
Study Guide and Student’s Solutions Manual not at North bookstore
Scientific
Calculator that has Log and inverse Antilogs
Goggles
or Visorgogs or use safety glasses available in lab
Bring you own antibacteria wipes (we are out till Fall)
Instructor: John
T. Taylor About Me Resume
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Office:
D-270 Office
Phone: 904-766-6763 Internet: (904) 410-1924
Cell Phone:
904-614-0531 or leave messages at instructor’s home at
designated times or extreme emergencies on weekends. ( Link
to site: http://www.fccj.us/OfficeSum09.htm
for
current office hours The instructor is available for additional office
hours by appointment. Appointments
must be made at least two days in advance, except for extreme emergencies. Office hours are subject to change |
email: johtaylo@fccj.edu
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E-Mail assignments to both
addresses below Subjects of emails must describe briefly
the assignments being submitted and begin with the # 46: i.e. 46:
First Email or 46: your subject |
Email Requirement:
Each student should send
the instructor an email during the first week from both your FCCJ email account
and/or an outside email account for your primary contact, and the other as a
backup contact. Be certain you put in subject box:
46: first email
Tell me
about yourself. Why are you taking this course? When did you
complete CHM 2045C, where, with which instructor, and your grade. What
is your highest math course completed? Where do you live? What are your
telephone numbers? What is your external email address which can serve as a
backup to FCCJ assigned email.
Always begin the subject
of each email with 46:
Subject-less
emails will be deleted or subjects without the number code may be deleted.
Attachments will only be opened if the number code is in the subject line. This
prevents viruses and spam.
ATTENDANCE:
Students are expected to attend class and will be
responsible for all material presented. The student must sign the attendance
roster to earn credit for attendance.
Each on campus class attended will be worth one point. The student will
fill out a data card similar to your instructor one the last page of this
syllabus worth one point of the two points for the first day’s attendance. One
student will serve as attendance monitor and record the day’s attendance for
end of term point assignment. Student will sign lab role twice, once in the
beginning of lab and then when they leave noting time out.
Online First Week Activities: The descriptions may be found at:
http://www.hccfl.edu/faculty/john_taylor/cgs1555/spring04/syllabus/activity.htm
Free
Time Chart: Find me 10 hours per week of the 168 weekly total: List them
Description: http://www.hccfl.edu/faculty/john_taylor/cgs1555/spring04/syllabus/freetime.htm
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Free
Time First Lab Exercise: Chemistry takes a lot of time to study. Each student should identify at least 10
hours or more per week of free time that she/he will commit towards his/her
study of chemistry. The following are
suggested strategies for scheduling your study times. Make an hour by hour seven day matrix 8
columns (hour and each day of the week) by 24 lines (representing each hour).
See Master Student Web Site above. A
blank matrix has been attached to this syllabus for you to complete. |
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Starting
with wake-up and end with sleeping:
1.
Schedule fixed blocks of time first. These include work, class time, eating,
and sleeping.
2.
Include time for travel and errands
3.
Schedule time for fun.
4.
Set realistic goals.
5.
Allow flexibility in your schedule.
6.
Study at least two hours for every hour in class plus an extra two for computer
assignments in the open lab and an extra two with a cooperative group member
for homework comparison and checking.
7.
Avoid scheduling marathon study sessions.
8.
Set clear starting and stopping times.
9.
Plan for the Unplanned!
Study
Groups/Phone Network/Lab Partner:
On the first day of class each student
will complete a Data Card, Interview a peer, and introduce (if time permits)
that peer to the class. From these exercises and the learning styles inventory,
study groups, a phone network, and lab partners need to be established. Study
areas, as well as the classroom, should be used for study groups plus lunch and
learn sessions. Some portions of the office times may meet in the library
computer learning lab. Each week volunteers will be appreciated to assist in the
group operation of the class. The first personal assistant volunteer will
prepare a matrix with each student’s free study time so that study groups may
begin to be formed the second week of school. The phone network will be
established so that in case of emergencies by the instructor each student will
be responsible to call two other students in the network to alert the student
of the emergency so that information may be distributed prior to the next
scheduled class. Emergencies will usually also include a group email on the
morning/afternoon of the class meeting.
E-Instruction (option) or Clickers:
During a scheduled class (75-90 minutes), after going through the
lecture on the assigned chapters via many modalities of teaching including
Internet web sites, the instructor will utilize either the last 10 minutes or
the first 10 minutes of class to go through the Power Point for the assigned
chapter as a review.
However, multiple choice questions will be inserted into the online
power points which will require all students to answer via the instructor’s e-Instruction system (keypads). Each
correct response will be worth one point, while an incorrect response will
count zero points. e-Instruction system will be worth no more than 50
points (out of 100 possible) for the term (5% total if used Fall Term 2008).
For each exam when e-Instruction is not used, the multiple choice section of
the modules will be increased at five to ten questions per chapter.
Students are expected to get 50% correct on each day’s e-Instruction questions. During the term, the instructor may pretest a section of the multiple choice for the course using the e-Instruction system where the responses will count 1 point each of the 10 to 15 points assigned to multiple choice for that Module.
Daily
Pretest Quizzes (optional):
Pretest quizzes may be
administered before (12:30-1:00), sometimes during, and/or after (6:00-7:00)
every class which is not a scheduled exam day. These pretest quizzes may not be made up outside of class
time, unless directed by the instructor to complete the pretest in the test
center during an assigned period of time.
Scored
pretest quizzes are NOT recorded in the instructor’s grade book or on
Blackboard, but must be attached to the Modular Exam Grading
Outline the day of the exam to receive the pretest grade. This pretest packet
is submitted as a separate packet. Students must write the scores on both the
cover sheet of the pretest packet and on the front page of each exam.
The student
will skip the section of the modular exam that is pre-tested. The Pretest scores sometimes may be recorded
on the attendance sheet, but only for your instructor’s sense of current levels
of class achievement. If you loose the graded pretests, you will have to do the
section over on the exam.
The instructor
only records Module Exam totals and the Final Exam in his grade book and on
Blackboard. Multiple choice and vocabulary sections of modules are usually only
tested on exam day and are usually never pre-tested or post-tested.
Do Not Staple the Modular Exams together as they are
graded separately, listed on Blackboard separately, and returned separately
after the exam day. Please staple carefully as directed. Mixing the modular
papers on Exam day may result in a lower grade.
1. Pretests
are exams. They are not open book. They are not open notes. They are not
collaboration with your neighbor.
2. The
pretests may NOT be used during the exam!
3. You
must do the pretests in class. You may NOT take the pretests home.
Samples of each
section (pretest) of each exam may be found on the grading outline on the web
site. On the sample tests are suggestions for paper and pencil homework in the
textbook. The grading outline may be found at:
Kotz 6th
Edition: http://www.fccj.us/chm2046/46grdF08.htm
McMurray 5th edition: http://www.fccj.us/chm2046/46grdF08McM.htm
Pre-testing
is a privilege not a right!
Our classroom D-210
may not have a scheduled class in the room before our class
on
Tuesday and Thursday. Pretesting will begin at 6:00
to 7:00 p.m. each class day and must be completed before class begins at 7:00. Students
who are late to class (after 7:00), will not be allowed to pretest until after
class. Students should plan to stay late if they can not arrive early. Many
times the pretest will not be administered till the last 10 minutes of class so
that student may complete the item after class has concluded. Pretest will be
graded for all students who stay after 10:00 p.m. Pretesting
may also be done 10:00-10:30 p.m.
MAKE-UP POLICY:
Make-up exams are usually not
given. In the event of an unavoidable absence on exam day (jury duty,
hospitalization, incarceration, and death in the immediate family), you will be
allowed make-up tests only upon the instructor’s approval..
You must contact the instructor, no later than, the week of the exam in order to
discuss what arrangements might be made. This may be done with a quick email. A message must be left on the instructor's e-mail
(johtaylo@fccj.edu ) or his office phone 766-6763 if the instructor
cannot be reached. If a makeup is allowed, it must be completed prior to return
of the exam papers completed by the students attending the scheduled exam. Missed
exams will otherwise count as 0 points. Papers are returned usually after one
or two weekends after the exam.
Students who take the test on the assigned day are guaranteed to receive their graded exam on or before the next exam day, otherwise the student will be assigned a 100% grade for the un-graded paper. Students not taking the exam on the assigned exam day may not receive their grade until days or weeks after the class papers are returned.
A-16 Tentative Exam
Schedule North Campus:
TBA
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Major Learning Outcomes
(Goals): This course is designed as the second
semester of a two semester sequence of College Chemistry. CHM 2046C has been modified and streamlined
to accomplish the following major learning outcomes in 45-60 total hours of
class and instruction. Students entering the class should have had CHM2045C
with a passing grade. |
. Learning Objectives for General Chemistry II
Students who have completed General Chemistry I (CHM 2045C) are expected to demonstrate knowledge of the following content-based learning objectives. The learning objectives are arranged by major content area.
Module 8-Part II Solutions and Their Behavior
(Chapter 11)
Students must know or be able to do the following:
·
Know and be able
to carry out calculations using molarity, molality, mole fraction, weight percent, parts per million,
and parts per billion.
·
Define
solubility, saturated solution, unsaturated solution, supersaturated solution,
miscible, and immiscible.
·
Determine the
solubility of a salt based on the change in enthalpy of solution.
·
Know and apply
the affects of pressure and temperature on the solubility of a gas in a liquid.
·
Know and apply
the affect of temperature on the solubility of a solid in a liquid.
·
Define and give
examples of colligative properties.
·
Define and
perform calculations using Raoult’s Law.
·
Calculate
freezing point depression and boiling point elevation when a solute is added to
a solvent when the solute is an electrolyte and a nonelectrolyte.
·
Calculate molar
masses of compounds based on colligative properties.
·
Define ion
pairing and describe its affect on colligative
properties.
·
Define osmosis,
reverse osmosis, and osmotic pressure.
·
Calculate osmotic
pressure.
·
Define and give
examples of the various types of solutions including isotonic, hypotonic, and
hypertonic.
·
Define crenation and homolysis.
·
Define and give
examples of colloidal dispersions.
·
Define and give
examples of an emulsion, emulsifying agent, and surfactant.
·
Describe how soap
is made and how it works.
·
Define
hydrophobic and hydrophilic.
·
Describe what is
meant by the term “hard water”.
Module 9 Principles of Reactivity: Chemical Kinetics (Chapter 12)
Students must know or be able to do the following:
·
Define kinetics.
·
Calculate the
average and instantaneous rate of a chemical reaction.
·
Know the factors
that affect the rate of a chemical reaction and how they affect the rate
including concentration, temperature, state of subdivision, and addition of a
catalyst.
·
Write rate
equations for chemical reactions based on experimental data.
·
Determine the
order of a chemical reaction.
·
Determine the
rate constant based on experimental data.
·
Know and apply
first order rate equations including calculation of half-lives.
·
Know and apply
zero order and second order rate equations.
·
Define and apply
the collision theory.
·
Use the Arrhenius
equation to find activation energy.
·
Define reaction
mechanism, intermediate, and free radical.
·
Write rate
equations for mechanistic steps.
· Define rate-determining step.
Module 10: Principles of Reactivity: Chemical Equilibria
(Chapter 13)
Students must know or be able to do the following:
·
Define
equilibrium.
·
Write equilibrium
constant expressions for chemical reactions applying rules.
·
Calculate
equilibrium constants using equilibrium constants of other related reactions
and from equilibrium concentrations.
·
Interpret
equilibrium constants in terms of whether the reaction is reactant or product
favored.
·
Assess reaction
quotient to determine how a reaction will proceed.
·
Calculate
equilibrium concentrations based on initial concentrations and the equilibrium
constant.
·
Define and apply LeChatelier’s Principle.
·
Know how
reactions at equilibrium are affected by stresses such as temperature,
concentration, and pressure.
Module 11 Principles of Reactivity: The Chemistry of Acids and Bases (Chapter 14)
Students must know or be able to do the following:
·
Describe the
properties of acids and bases.
·
Define acids and
bases in terms of the Arrhenius or Classical definition, the Bronsted-Lowry definition, and the Lewis definition.
·
Predict the
products of a neutralization reaction.
·
Provide the
self-ionization reaction for water.
·
Memorize a list
of acids and bases including their name, formula, number of protons they can
donate or accept, and strength.
·
Define monoprotic, diprotic, and triprotic acids and bases.
·
Write ionization
reactions for acids and bases.
·
Define and give
examples of species which are amphiprotic and amphoteric.
·
Define and apply
the terms conjugate acid and conjugate base.
·
Determine the
equilibrium position of an acid-base reaction.
·
Determine acid
and base strength based on Ka and Kb.
·
Describe the
leveling effect.
·
Write equilibrium
expressions for the ionization of weak acids and bases.
·
Define, apply,
and perform calculations using the pH and pOH
equations.
·
Correlate
acidity, basicity, pH, pOH,
hydronium ion concentration, and hydroxide
concentration.
·
Perform
calculations using the equilibrium expression for the ionization of water.
·
Know two ways to
determine pH.
·
Calculate pH from
Ka or Kb using initial concentrations and the equilibrium
expression.
·
Calculate %
ionization of a weak acid or base.
·
Be familiar with
the common acid and basic ions that form acidic and basic salts.
·
Determine
equilibrium concentrations for all ionization products of diprotic
and triprotic acids.
·
Describe how acid
strength is affected by the inductive effect and bond strength.
· Describe molecules as Lewis acids or bases.
Module 11: Principles of Reactivity: Other Aspects to Aqueous Equilibria
(Chapter 15)
Students must know or be able to do the following:
·
Define and apply
the concept of buffer solutions.
·
Define pKa and use it in calculations.
·
Know and apply the Henderson-Hasselbach Equation to buffer systems.
·
Calculate the pH
of a buffer solution before and after a strong acid or base is added.
·
Perform
calculations to determine how you would prepare a buffer solution at a given
pH.
·
Perform
calculations that apply the common ion effect to acid and base ionization
reactions.
·
Predict the
acidity/basicity of a solution at the equivalence
point of a titration based on the strength of the acid and base reacted.
·
Calculate the pH
at all of the various points during a titration - prior to the equivalence
point, at the equivalence point, and after the equivalence point for all of the
following combinations - strong acid/strong base, strong acid/weak base, and
strong base/weak acid.
·
Generate
titration curves for all of the following combinations of reactants: strong acid/strong base, strong acid/weak
base, and strong base/weak acid.
·
Predict the shape
of a titration curve for the titration of a diprotic
or triprotic acid.
· Define acid-base indicator and determine which is the best choice for predicting the equivalence point of a particular acid/base combination.
Module 12: Principles of Reactivity: Precipitation Reactions (Chapter 15)
Students must know or be able to do the following:
·
Define Ksp.
·
Write the Ksp expression for a slightly soluble salt.
·
Determine Ksp from experimental measurements.
·
Determine salt
solubility from Ksp.
·
Predict whether
precipitation will occur based on calculation of
reaction quotient.
·
Calculate
solubility before and after a common ion is added to the solution.
·
Predict the Knet of a reaction via simultaneous equilibria.
·
Provide equations
and discussion to explain how the solubility of a salt is increased by addition
of a weak acid and decreased by the addition of strong acid.
·
Be familiar with
the solubility of complex ions.
Module 13: Principles of Reactivity: Entropy and Free Energy (Chapter 16)
Students must know or be able to do the following:
·
Define
thermodynamics.
·
Know the three
laws of thermodynamics.
·
Know the two
fundamental laws of nature.
·
Define all of the
following – change in enthalpy, entropy, and free energy – and give the meaning
of a positive and negative value for each.
·
Provide examples
where entropy is increasing and decreasing.
·
Calculate the
entropy of a system using the equation: DS = q/T.
·
Calculate the
entropy of the Universe using the equation: DSuniverse = DSsystem + DSsurroundings
·
Calculate the
entropy, enthalpy, and free energy changes of a system by finding the
difference in the summation of the product formation (S, H, or G) minus the
summation of the reactant formation (S, H, or G).
·
Utilize the
equation DG = DH – TDS
·
Determine if a
reaction is enthalpy of entropy-driven.
·
Describe how a
reactant-favored reaction can be made product-favored by coupling it to a very
product-favored reaction.
·
Determine the
minimum temperature needed to make a reaction spontaneous.
·
Use the equation,
DG = R T ln K, to find DG or K
.
Module 14: Principles of Reactivity: Electron Transfer Reactions (Chapter 17)
Students must know or be able to do the following:
·
Define redox reaction, oxidation, reduction, oxidizing agent, and
reducing agent.
·
Provide some
examples of redox reactions.
·
Balance redox reactions in neutral, acidic, and basic solution.
·
Draw and describe
how an electrochemical cell works.
·
Calculate DG using cell potential: DGo
= - n F Eo
·
Calculate cell
potential using standard reduction potentials.
·
Describe how the
standard reduction potentials are generated.
·
Describe the
standard hydrogen electrode and provide its purpose.
·
Describe how a
positive/negative reduction potential indicates a better
oxidizing/reducing agents.
·
Use the Nernst
equation to calculate cell potential under non-standard conditions.
·
Calculate the
equilibrium constant for a reaction using cell potential via
Ln K = nEo /
0.0257
·
Define and give
examples of primary batteries, secondary batteries, and fuel cells
·
Define corrosion
and be familiar with what causes it.
·
Provide at least
two ways to prevent corrosion.
·
Define
electrolysis and Faraday’s Law
· Apply Faraday’s Law in an electrolysis calculation.
Module 15: Nuclear Chemistry (Chapter 22)
Students must know or be able to do the following:
·
Define
radioactivity and give a brief description of its discovery.
·
Know the three
forms of radiation including symbol, charge, mass, speed, and penetrating
power.
·
Predict products
in an alpha emission, beta emission, positron emission, and electron
capture.
·
Briefly describe
“Band of Stability”.
·
Define binding
energy and use Einstein’s equation to predict its value.
·
Define half-life
and apply first order kinetics to radioactive decays.
·
Define Carbon-14
dating and Artificial Transmutation.
·
Predict products
in artificial transmutation reactions.
·
Define nuclear
fission and nuclear fusion.
·
Describe the
parts of a nuclear power reactor.
·
Define breeder
reactor.
·
Describe nuclear
bombs.
·
Describe several
units of radiation.
·
Describe the
major sources of radiation exposure.
·
Provide some
examples of the applications of radioactivity including food irradiation,
radioactive tracers, and medical imaging.
Module 4 Part II: Objectives
(Chapter 7): (Review from CHM 2045C)
Terms:
valence electrons, chemical bond formation, bonding in ionic compounds,
covalent bonding, bond properties, charge distribution, in covalent compounds,
molecular shapes, molecular polarity, orbitals and
bonding theories, valence bond theory, and molecular orbital theory.
1.
Predict molecular geometry of a molecule.
2. Predict and explain the polarity of a
molecule.
3. Explain the geometry of a molecule
using one of the bonding theories.
4. Predict the hybrid orbital type for an atom in a covalent molecular
Module 16 formerly Module 4_III Organic
Chemistry (Chapter 23)
Students must know or be able to do the following:
·
Define organic
chemistry.
·
Know the four
types of hydrocarbons including their general formula, hybridization, bond
angle, name ending, and some examples of each.
·
Define structural
isomers and stereoisomers and provide examples of
each.
·
Describe the
difference between saturated and unsaturated hydrocarbons and give examples.
·
Define functional
group.
·
Provide general
structure, functional group, name ending and some examples of several families
of organic compounds including alcohols, aldehydes, ketones.,
carboxylic acids, esters, amines, and amides.
Module
17 Biochemistry (Chapter 24)
Students must know or be able to do the following:
·
Define polymer,
plastic, thermoplastic, and thermoset.
·
Describe the two
reaction types used to synthesize polymers and give some specific examples of
each.
·
Know the
synthesis of polyethylene and its derivatives, polyamides, and polyesters.
·
Know the “Big
Six” plastics including recycling number, abbreviation, name, structure of the
monomer, thermoplastic or thermoset, and addition or
condensation.
· Compare the structural differences, physical properties, and uses of LDPE and HDPE
Laboratory
Students must know or be able to do the following:
·
Carry out an
experiment involving intermolecular forces.
·
Carry out an
experiment involving solubility.
·
Carry out an
experiment involving colligative properties.
·
Carry out a kinetics
experiment
·
Carry out an
equilibrium experiment.
·
Carry out an
experiment using a pH meter.
·
Carry out an
experiment involving acid-base titration curves.
·
Carry out an
experiment involving a buffer solution.
·
Carry out a
qualitative analysis experiment.
·
Carry out a redox experiment.
·
Carry out an
organic synthesis.
·
Carry out a lab
involving polymers.
Quiz monitors,
attendance monitor, personal assistants, test preparers, camera
persons/editors, study guide word processor assistant, Chemistry WebMasters, as well as study groups are forms of
cooperative learning environments where the student needs to learn how to
function in teams. Each
student MUST take charge of his/her commitment to learning in order to achieve
success in not only this course but also in college.
Grading Scale:
|
Overall Percentages |
Grade |
|
100 – 90 % |
A* |
|
89 – 80 % |
B* |
|
79 – 65 % |
C* |
|
64 – 50 % |
D* |
|
< 50 % |
F |
*Lab is an essential part of this
class. If you acquire less than 60% in
lab, you will automatically receive a letter grade of ‘F’ in this course. If
you make less than 70% in lab you may not earn a final grade above ‘D’
Grade Review:
See Grading Sheet (distributed separately) for a point by point summary
of the course. It also serves as a Course outline, indicating sections of the
text being covered on each exam.
Grading
Outline: http://www.fccj.us/chm2046/46grdSum09.htm
Grade Calculator: http://www.fccj.us/chm2046/46grdcal.html
% Weighting of the Components of the
Course:
Exams 60-65%
Attendance 5%
e-Instruction
0- 5%
Final Exam 10%
Lab Assignments 20%
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Total 100%
ON-Line Grade Calculator:
http://www.fccj.us/chm2046/46grdcal.html
Instructor’s Right to Change or Modify Grading Procedures:
This instructor reserves the right to make changes in
this syllabus whenever he feels it is appropriate to do so. The instructor
reserves the right to modify or change the grading progress as the course
proceeds. Any additional course assignments will substitute for deleted
items. Some may also be modified if not
deleted. The instructor will not add
major examinations as a modification and maintain the above general category
point distributions. Tests will constitute ~60-65% of the grade excluding the
final’s 10%, 20% for the
laboratory component, 0-5%
of the grade for Interactive Classroom Presentation System, and 5% for attendance.
Students
absent on exam days will do a makeup exam outside of class time when they
return on the next Tuesday or Thursday following the absence or by special
arrangements in the
Student who takes the test on the assigned test day are guaranteed to receive their graded exam on or before the next exam day after completion of the new exam, otherwise the student will be assigned a 100% grade for the un-graded paper.
Lab Reports/Write-ups, and/or Lab Notebook are due prior to the next scheduled lab. Lab reports submitted after that date may be subject to a one to two point (10-20%) penalty depending on whether the instructor has graded that weeks lab. Lab Data submitted without calculation will receive a minimum of 5 points (50%). Labs not submitted receive a grade of zero. Students absent from lab receive a zero. Students attending and submitting all lab reports receive up to 10 extra points as a student is allowed only one absence from lab.
Other
Pertinent Information (Supplemental Notes):
Students with Disabilities: Qualified students with documented disabilities are eligible for
physical and academic accommodations under the American Disabilities Act and
Section 504 of the Rehabilitation Act of 1973.
Students requesting accommodations should contact Student Development
Services at 264-7220 (voice) or 264-3371 (TTY) and this professor during the first week of class.
Withdrawal Policy:
Students will be allowed to withdraw from this class any time during the
semester through Monday, July XX for an A-16 schedule and will receive a grade of “W”.
Students failing to attend class for the first two consecutive weeks are
subject to withdrawal by the instructor according to FCCJ policy. These ‘no shows’ must be reported to
Admissions and Records by the end of two weeks Tuesday May 19
Academic Misconduct:
Academic misconduct or dishonesty such as cheating and plagiarism is not permitted. Suspected cases may be reported to the Dean of Liberal Arts and may result in failure of an assignment, failure for the course or exclusion from the class. Also, the instructor reserves the right to reassign work to students if the instructor senses the work submitted is not the work of the student. (No questions asked-The instructor may tell the student to resubmit the work to earn the daily pretest grade or examination grade or may be assigned a zero if second request is made).
Classroom Etiquette:
Students are expected to conduct themselves as
adults in the classroom showing respect to their classmates. Only persons
registered for this class are permitted in the laboratory. As a courtesy to the instructor and your
fellow classmates, cellular
telephones and pagers should be cut off before entering the classroom or
laboratory. Likewise, the instructor sometimes forgets to shut his down
at the beginning of class, so hopefully someone sitting close to the front may
remind the instructor with a hand gesture for him to check his phone,
Children in the Classroom
Policy: It is the goal of FCCJ to provide a safe and
effective learning environment for all students. Any action, which interferes with this goal,
will not be permitted. Children must not
be left unattended at any time on campus.
If an emergency arises which requires a student to bring an underage
child (defined as any child under the
age of sixteen who is not a FCCJ student enrolled in a credit class) to campus,
the child must be under the direct supervision of an adult at all times. Parents and guardians of children considered
disruptive or unsupervised will be asked to remove the children from the campus
immediately.
Bringing children to the classroom is not
permissible under most circumstances.
However, if an emergency arises which necessitates bringing a child to class, the student must receive the prior consent of the
faculty member involved. Children who
are ill may not be brought to class regardless of the circumstances. Due to the nature of the equipment, the
subject matter involved, and the level of supervision necessary, underage
children will not be allowed in college laboratories or in the
Children enrolled in non-credit classes must be under the direct supervision of an adult at all times. Likewise, children attending campus events must be supervised at all times. Any child under the age of 16 must be under the direct supervision of his/her parent, legal guardian, or other responsible adult when in the college library unless the child is part of a call AND the supervising teacher or paraprofessional is present
Instructor
Requested Information:
During the
first week of class, the student will fill out a 4x6 file card. The instructor
has provided a sample below with his personal data and his block scheduled
time. The completion of this card is
worth (2 points)
toward the student's final grade
Data Card (4x6 file
card): Front Side (Personal Data)
--------------------------------------------------------------------------------------
Name: John Taylor CHM 2046C
Office: D-270
Address:
Telephone: 904-766-6763
(office)
Cell: 904 614-0531 Home:
904-992-2052
E-MAIL : johtaylo@fccj.edu or jtaylor@hccfl.edu
Employment: FCCJ since 8/21/06
Full time chemistry faculty
Major:
Instructional Technologies Minor:
Chemical Education
Long Term
Goal: Educational Software Developer
Prerequisite: MAC
1105 equivalent Algebra completed: yes
Chemistry
Background: CHM 2045C: yes A
Physics
Background: High School Physics completed: no
Software/Computer
Literacy: WP, Word, Excel, HTML, Javascript
Home Computer: yes Internet ISP: yes or have access
Why are you
taking this course? Required for chemistry major
--------------------------------------------------------------------------------------
Data Card (4x6 file card): Back
Side (Scheduled Time Blocks)
Class/Work Schedule Summary:
Number Section Room Time Days
TBA
Class/Office Matrix Schedule (Where is Your
Instructor?):
My Schedule Matrix: I have 10
hours of office hours, Office/Pretest
means I am in the course’s classroom, while Office means my office D-270.
You must find 10 hours in you weekly matrix for studying chemistry. Please make
your own!
|
Time |
Monday |
Tuesday |
Wednesday |
Thursday |
Friday |
|
7:30 |
|
At Home |
|
At Home |
|
|
8:00 |
At Home |
On the Road |
|
On the Road |
Community |
|
8:45 |
|
On the Road |
|
On the Road |
Service |
|
9:00 |
|
CHM 2045C |
|
CHM 2045C |
Projects |
|
9:30 |
|
|
|
|
Off Campus or |
|
10:00 |
|
|
|
|
Corporate |
|
10:30 |
|
|
|
|
Computer |
|
11:00 |
|
|
|
|
Training |
|
11:30 |
|
|
|
|
Off Campus or |
|
12:00 |
|
|
|
|
Special |
|
12:30 |
|
|
|
|
Help |
|
1:00 |
|
Pretest 2045 |
|
Pretest 2045 |
Pre-testing |
|
1:15 |
|
|
|
|
Sessions |
|
1:30 |
|
|
|
|
as |
|
2:00 |
|
|
|
|
announced |
|
2:30 |
|
|
|
|
via |
|
3:00 |
|
|
|
|
email |
|
3:30 |
|
|
|
|
On Campus |
|
4:00 |
|
|
|
|
|
|
4:15 |
|
|
|
|
|
|
4:30 |
|
|
|
|
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|
5:30 |
|
|
|
|
|
|
6:00 |
|
Pretest 2046 |
|
Pretest 2046 |
|
|
6:30 |
|
|
|
|
|
|
7:00 |
|
CHM 2046C |
|
CHM 2046C |
|
|
7:15 |
|
|
|
|
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|
7:30 |
|
|
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|
8:00 |
|
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8:30 |
|
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9:00 |
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9:30 |
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10:00 |
|
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10:15 |
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10:30 |
|
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|
|
Student’s Class/Work Matrix Schedule:
Where can you find 10 hours per week minimum to study?
Name:
___________________________ CHM 2046C Fall Term 2008
|
Time |
Monday |
Tuesday |
Wednesday |
Thursday |
Friday |
Saturday |
Sunday |
|
7:30 |
|
|
|
|
|
|
|
|
8:00 |
|
|
|
|
|
|
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|
8:45 |
|
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9:00 |
|
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9:30 |
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10:00 |
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10:30 |
|
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11:00 |
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11:30 |
|
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12:00 |
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12:30 |
|
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1:00 |
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1:30 |
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2:00 |
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2:10 |
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2:30 |
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3:00 |
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3:30 |
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4:00 |
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4:30 |
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5:00 |
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5:30 |
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6:00 |
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6:30 |
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7:15 |
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7:30 |
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8:00 |
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8:30 |
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9:00 |
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9:30 |
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10:00 |
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10:15 |
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10:30 |
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|
Submit this form the second class period