Coastal
CHEM 1212: Principles of Chemistry II 4 cr.
Sections:
34532
Spring Term 2005
SITE: AB204
DAY/TIME: 34532: Tuesday and Thursday mornings
CGCC
Course Description:
Second
course in a two-semester sequence covering the fundamental principles and
applications of chemistry for science majors.
Laboratory exercises supplement the lecture materials.
Prerequisites: CHEM 1211.
(3 class hours, 3 lab hours, 4 credit hours)
Required
Textbooks:
Lecture
Text, Laboratory Text, Supplies, and Materials:
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1184 pages Case Bound 8
1/2 x 10 ISBN: 003033604X (Contains
most assigned homework problems. Contains complete solutions for in-chapter
exercises and designated, darkened end-of-chapter questions.) CHEM 1211 will
cover Chapters 1-10 and 12 in Eight Modules (or Units) |
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Table of Contents |
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CHEM
1212 Principle of Chemistry II ------------------------------------------------------------------------------------------------------------------------------------------------------- 11.
Carbon--More Than Just Another Element. 13.
Intermolecular Forces, Liquids, and Solids. |
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Preparing for Your ACS
Examinations In General Chemistry The Official Guide; Eubanks, Lucy T, & Eubanks, Dwaine
I, American Chemical Society Division of Chemical Education; 1998 |
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GCSG |
General Chemistry - Official Study
Guide ($12.00) |
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Topics Covered ·
Atomic Structure (CHEM 1211) ·
Molecular Structure and Bonding (CHEM 1211) ·
Stoichiometry (CHEM
1211) ·
States of Matter / Solutions (CHEM 1211) ·
Energetics (CHEM 1211) ·
Dynamics (CHEM 1212) ·
Equilibrium (CHEM 1212) ·
Electrochemistry / Redox (CHEM 1212)
(CHEM 1211) ·
Descriptive Chemistry / Periodicity (CHEM 1212)
(CHEM 1211) ·
Laboratory Chemistry (CHEM 1211) (CHEM 1212) Features ·
Description of important ideas included in each topic ·
Questions that emphasize the concepts most frequently studied ·
Analysis of how to think through each study question ·
Worked-out solution for each study question ·
Insight into how wrong responses are constructed ·
Practice questions for you to try on your own ·
Answers for all questions |
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WebAssign Access Code.
Bookstore $7 (only purchase after instructor requests)
Laboratory Text: Weekly Printouts from
Student CD and also
Posted on Web Site
(May be printed in Library)
Scientific calculator (non-alphanumeric)
(TI-30XaSE will be used on all exams)
Periodic Table
Goggles or
Visorgogs
Recommended
Additional Textbooks:
Solutions Manual: Student Solutions
Manual to Accompany Chemistry & Chemical Reactivity;
5th edition 2003; Banks;
Thompson Learning: Brooks Cole.
(Contains complete
solutions for designated, darkened end-of-chapter questions.)
Study Guide: Student Study Guide to Accompany
Chemistry & Chemical Reactivity;
5th edition 2003; Banks;
Thompson Learning: Brooks Cole.
Student Lecture Outline: Student
Lecture Outline to Accompany Chemistry & Chemical
Reactivity; 5th edition 2003; Banks;
Thompson Learning: Brooks Cole
Special Dates:
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Drop & Add
Adjustments |
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Class
dates |
1/5-4/25,
2005 |
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Administrative
Adjustment |
TBA |
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Last Day to
Withdraw |
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Final Exam |
Thursday April 26 |
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No classes scheduled |
Monday 1/17
(Martin Luther King), Wed-Fri
3/9-3/12 (Spring Break)); |
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Last
Day to Remove ‘I’ |
TBA |
Instructor: John
T. Taylor
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Office:
none (classroom and library) Office
Phone: none Cell Phone:
813-361-4379 or leave messages at instructor’s home at
designated times or extreme emergencies on weekends. ( Office Hours (tentative):
12:
AB 204 for
brown bag (Dinner & Learn sessions)
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Link
to site: http://www.hccfl.edu/faculty/john_taylor/office/office.html for
current 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.
E-MAIL:
Each student is required to
have an E-mail address. Free Emails may be obtained from Hotmail
[www.hotmail.com, Yahoo [www.mail.yahoo.com], or email assigned by CGCC.
Students must view their email prior to each class.
First Email to the Instructor:
Each student must submit a
first email to the instructor to all three of the above addresses before the
second class. The subject line must appear as below. The body of the email must
introduce the student to the instructor, why the student is taking the course,
what is the student’s major, what is the student’s chemistry background: high
school/college, what is the student’s math background. When does the student
plan to graduate, where will the student transfer when graduating from CGCC. Where does the student work? How many hours per week?
How many credits is the student attempting? This assignment is worth 2 points
if completed for the first lab report, but minus 10 points if not completed by
Tuesday 1/11 9:30 am.
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E-Mail assignments to all
three addresses above Subjects of emails must describe briefly
the assignments being submitted and begin with 12n: i.e. 12n:
First Email |
Attendance:
Lecture and laboratory attendance is essential for success in this course. Students
are expected to be on time and to remain for the entire class period. Tardiness to pre-lab will result in a
reduction in the lab assignment grade for that day. The instructor will ask
each student to give his or her word that they will attend every class. Student
must sign the attendance sheet to receive credit for attendance for that
day. Reading, homework assignments, and
group assignments should be completed before coming to each class. Either
on-line quizzes or short in-class quizzes will pretest sections of each exam
covering the daily assignments.
Students missing more than two lecture classes and/or one lab class
during the term must see the instructor outside of class time to investigate
alternatives for the student. Chemistry
is very sequential: what you learn today will be used tomorrow. Absent students forfeit the right to make-up
the pretest quizzes. After the second
absence additional points will deducted for each absence in excess of two lectures/one
lab. Students absent from class are expected to
contact a member of his/her cooperative group prior to the next class to
determine what was missed and what is assigned for homework as the course
calendar is dynamic and is edited every week, sometimes after a class.
Student may contact class
members about assignments at::
http://www.hccbrandon.net/chem1212/12email.html
Required Assessments Week One: (.)**
CHEM
1212 PreTest (ACS One Year Exam)**
Obtain
CGCC or other email and send first email to the instructor at all three email
addresses
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 group and lunch and
learn sessions. Some portions of the office times may meet in the library
computer 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.
ACS Final Exam
(Complete Year):
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During the first week all students must take the CHEM 1212 ACS General Chistry Exam during the first scheduled lab (Thursday 1/6). It is a pre-assessment of chemistry skills and will be post course tested the week of finals. The test includes 70 multiple choice questions divided into ten sections listed below. Students should be able to score at least half correct for 7 of the sections as they were CHEM 1211 topics from last semester |
ACS
General Chemistry Exam (Complete year)
____(7) Atomic Sructure
____(7) Molecular Structure
____(7) Stoichiometry
____(7) Energies (Thermo I)
____(7) Dynamics (Kinetics)
____(7) States of Matter/Solutions
____(7) Equilibrium
____(7) Electrochemistry/Redox
____(7) DescriptiveChemistry/Periodicity
____(7) Experimental
____(70) Total
CHEM
1212 Practice/Take Home/or Pre-Final Exam:
During the last week of school, (April 24-28 students will complete the on-line practice final exam during the last scheduled lab section after completing the Post ACS Toledo Placement test (No other lab activities are scheduled during final exam week). The course calendar has one of the previous finals designated as the practice final (usually the latest term available) or a new mock ACS exam will be developed for Spring Term 2005. The exam will be closed book and taken with your lab partner in the library computer center. It will be interactive allowing you to change answers after initial scoring. Each cooperative group will submit one practice final section for each module completed during the course. Both students will receive the same grade for the practice final (correct/possible x 20). The practice final will count as the first 20% completion towards the final exam grade.
ACS General
Chemistry Exam-Second-Term (Final Exam)
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The final exam is not optional. It will be the 75 (best 50 will be scored) questions of the standard American Chemical Society General Chemistry-Second Term Exam. The Final counts as two to three modular test scores or 10% of the total grade. The multiple choice sections of the module exams are mini-tests of the final as well as online multiple choice homework. If you score more than 50 correct answers, the instructor will award bonus 1 point per correct answer (not adjusted to 2.0 factor for the first 50 correct questions). |
ACS
General Chemistry-Second Term Breakdown
____(10) Solutions
____(10) Kinetics
____(10) Equilibrium
____(10) Thermodynamics
____(10) Electrochemistry
____(05) Nuclear
____(05) Polymers
____(05) Descriptive
____(05) Organic
____(05) Solids
____(75) Total
Final
Exam Challenge:
If a
student scores a higher % on the final exam (all 75 questions-adjusted ACS norm
score) then the grade earned through the total points assigned, then the Final
Exam score will constitute the final grade average for the lecture. The
instructor will not drop the
lowest exam score during the course, but may allow retest the last two weeks to
raise a poor score earned earlier in the course.
Chemistry and the World
Wide Web:
CHEM 1212 Home Page: http://www.hcc.cc.fl.us/faculty/john_taylor/chem1212.htm
Grading Outline/Sample Quizzes: http://www.hccbrandon.net/chem1212/12grdS05.html
Online Grade Calculator: http://www.hccbrandon.net/chem1212/12grdcal.html
Email/Phone Contacts: http://www.hccbrandon.net/chem1212/12email.html
Practice Multiple Choice Quiz Menu:
http://www.hccbrandon.net/chem1212/12testmenu.html
Kotz Text Power
Points: http://www.hccbrandon.net/chem1212/12powerppt.html
Online Lab Manual: http://www.hccbrandon.net/chem1212/12labmenu.html
Daily Quizzes (optional):
Each class, either
before, during the break, or after class the instructor will have some pretest
of the exam topics available prior to the exam day. Scored pretest quizzes are
NOT recorded in the instructor’s grade book, but must be attached to the
Modular Exam the day of the exam to receive the pretest grade. The scores may
be recorded on the attendance sheet. The
instructor only records Module Exam totals, the Final in his grade book. The pretests may NOT be used during the exam!
Samples of each section (pretest) of each exam may be found on the
grading outline:
http://www.hccbrandon.net/chem1212/12grdS05.html
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Major Learning Outcomes
(Goals): This course is designed as the second
semester of a two semester sequence of College Chemistry. CHEM 1212 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 high CHEM1211
with a passing grade. The same test will be administered at the end of the
course. The Topics will incorporate the American
Chemical Society General Chemistry-Second Term Exam Topics: |
. Learning Objectives for Principles of Chemistry II
Students who have completed Principles of Chemistry II (CHEM 1212) are expected to demonstrate knowledge of the following content-based learning objectives. The learning objectives are arranged by major content area.
M-7 Part II Liquids and Solids
Students must know or be able to do the following:
· Describe the difference between intermolecular and intramolecular forces.
· Describe and apply the various intermolecular forces including ion/dipole, dipole/dipole, hydrogen bonding, dipole/induced dipole, and induced dipole/induced dipole.
· Know the properties of liquids in relation to their intermolecular forces.
· Define and apply the terms critical temperature, critical pressure, surface tension, capillary action, cohesive force, adhesive force, and viscosity.
· Be familiar with the characteristics of the two types of solids – amorphous and crystalline.
· Be familiar with the characteristics of the four types of crystalline solids – ionic, metallic, molecular, and network.
· Define and apply the terms space lattice and unit cell.
· Be familiar with the characteristics of the three types of cubic unit cell – simple, body-centered, and face-centered.
· Calculate the radius of an atom or ion based on type of cubic unit cell.
· Be familiar with the characteristics of a simple and face-centered cubic unit cell of an ionic compound in terms of lattice points occupied by anions and holes occupied by cations.
· Define vaporization or boiling point and melting point.
· Be familiar with the change in enthalpy of fusion, crystallization, vaporization, and condensation.
· Use a phase diagram.
· Define triple point.
Module 8-Part II Solutions and Their Behavior
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
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
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
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: Reactions Between Acids and Bases
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
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
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
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
lnK = 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
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_III Organic Chemistry
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.
I. Polymer Chemistry
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.
II. 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.
Goals
and Objectives (CGCC Chemistry Department)
Goals and Objectives
Unit 1 Objectives:
Unit 2 Objectives:
Unit 3 Objectives: Ch. 17 – acid – base
definitions, self-ionization of water, strengths of acids and bases, ionization
constant for water, acids and bases, pH, pH equations, acidic and basic salts,
and polyprotic acids and bases. Ch. 18.1 – 18.3 – analyze pH at all points
during a titration between strong and weak acids and bases.
Unit 4 Objectives:
Unit 5 Objectives:
Unit 6 Objectives: (Additional topics to be covered
in lab.)
Course
Calendar for Class Meetings:
CRN: 34532 (Lecture:
(Lab: 7:15-8:50 pm Thur)
Wallace’s CHEM
1212 Tentative Course Schedule /Calendar:
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Wednesday, 1/5 |
Syllabus, Pre-Test Chapter 13 - Bonding and Molecular Structure: Intermolecular Forces, Liquids, and Solids |
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Friday, 1/7 |
Chapter 13 Lab – Safety / Check-In |
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Monday, 1/10 |
Chapter 13 |
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Wednesday, 1/12 |
Chapter 14 – Solutions and Their Behavior |
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Friday, 1/14 |
Lab –Evaporation and Intermolecular Forces |
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Monday, 1/17 |
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Wednesday, 1/19 |
Chapter 14 |
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Friday, 1/21 |
Lab - Effect of Temperature on the Solubility of a Salt |
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Monday, 1/24 |
Chapter 15 – Principles of Chemical Reactivity: Chemical Kinetics |
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Wednesday, 1/26 |
Exam I (Chapters 13
&14) |
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Friday, 1/28 |
Lab - Using Freezing Point Depression to Find Molar Mass |
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Monday, 1/31 |
Chapter 15 |
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Wednesday, 2/2 |
Chapter 16 – Principles of Chemical Reactivity: Chemical Equilibrium |
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Friday, 2/4 |
Lab – Iodine Clock and Solid Solutions |
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Monday, 2/7 |
Chapter 16 |
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Wednesday, 2/9 |
Chapter 17 – Principles of Chemical Reactivity: The Chemistry of Acids and Bases |
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Friday, 2/11 |
Lab – Crystal Violet Kinetics |
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Monday, 2/14 |
Exam II (Chapters 15 &
16) |
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Wednesday, 2/16 |
Chapter 17 |
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Friday, 2/18 |
Lab – Household Acids and Bases
and Equilibrium
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Monday, 2/21 |
Chapter
17 and Chapter 18 – Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria (18.1-18.3)
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Wednesday, 2/23 |
Chapter 18 (18.1 – 18.3) |
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Friday, 2/25 |
Lab Midterm
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Monday, 2/28 |
Chapter 18 (18.1-18.3) |
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Tuesday, 3/1 |
LAST DAY TO DROP WITHOUT ACADEMIC PENALTY
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Wednesday, 3/2 |
Chapter 18 (18.4 – 18.7)
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Friday, 3/4 |
Lab - Titration Curves of Weak
and Strong Acids |
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Monday, 3/7 |
Exam III (Chapters 17 & 18.1-18.3)
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Wednesday, 3/9 |
Spring Break |
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Friday, 3/11 |
Spring Break |
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Monday, 3/14 |
Chapter 18 (18.4-18.7)
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Wednesday, 3/16 |
Chapter 19 - Principles of Chemical
Reactivity: Entropy and Free Energy
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Friday, 3/18 |
Lab - The Buffer in Lemonade
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Monday, 3/21 |
Chapter 19 |
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Wednesday, 3/23 |
Chapter 20 – Principles of Chemical Reactivity: Electron Transfer Reactions |
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Friday, 3/25 |
Lab – Qualitative Analysis:
Mystery Powders |
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Monday, 3/28 |
Exam IV (Chapters 18.4-18.7 & 19) |
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Wednesday, 3/30 |
Lab – Introduction to Organic |
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Friday, 4/1 |
Lab –Synthesis of Aspirin, Part I |
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Monday, 4/4 |
Chapter 20 |
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Wednesday, 4/6 |
Chapter 23 – Nuclear Chemistry |
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Friday, 4/8 |
Lab – Synthesis of Aspirin, Part II and Lab - Establishing a Table of
Reduction Potentials: Micro-Voltaic
Cells |
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Monday, 4/11 |
Chapter 23 |
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Wednesday, 4/13 |
Lab – Introduction to Polymers |
|
Friday, 4/15 |
Lab- Classification and Identification of Common Plastics |
|
|
|
|
Monday, 4/18 |
Exam V (Chapters 20 & 23) |
|
Wednesday, 4/20 |
Review
for Final
|
|
Friday, 4/22 |
Lab Final
|
|
|
|
|
Monday, 4/25 |
ACS Post Test
|
|
Tuesday, 4/26 – Thursday, 4/28 |
Final Exam
|
CHEM 1212 Lab Schedule and tentative
Lecture Class Schedule
|
Thursday, 1/6 |
ACS General
Chemistry Pretest |
|
Thursday 1/6 |
Review Syllabus |
|
Thursday, 1/6 |
Lab – Safety,
MSDS, and Check In |
|
Thursday, 1/6 |
Module 9-Chapter 13 |
|
|
|
|
Tuesday, 1/11 |
Module 9-Chapter 13 |
|
Thursday, 1/13 |
Module 8 Part
II Chapter 14 Solutions and Their
Behavior |
|
Thursday, 1/13 |
Lab
–Evaporation and Intermolecular Forces |
|
|
|
|
Monday, 1/17 |
Martin Luther
King Holiday |
|
Tuesday, 1/18 |
Finish Module
8 Part II Chapter 14 |
|
Thursday, 1/20 |
Exam-Module 9
and 8 Part II (Chap 13 & 14) |
|
Thursday, 1/20 |
Lab - Effect
of Temperature on the Solubility of a Salt |
|
|
|
|
Tuesday, 1/25 |
Module 10 Chapter 15 –Chemical Kinetics |
|
Thursday, 1/27 |
Continue
Module 10 |
|
Thursday, 1/27 |
Lab - Using
Freezing Point Depression to Find Molar Mass |
|
|
|
|
Tuesday, 2/1 |
Finish Module 10 |
|
Thursday, 2/3 |
Module 11: Chapter 16:
Chemical Equilibrium |
|
Thursday, 2/3 |
Lab – Iodine
Clock and Solid Solutions |
|
|
|
|
Tuesday, 2/8 |
Module 11: Chapter 16:
Chemical Equilibrium |
|
Thursday, 2/10 |
Module 11: Chapter 16:
Chemical Equilibrium |
|
Thursday, 2/10 |
Lab – Crystal
Violet Kinetics |
|
|
|
|
Tuesday, 2/15 |
Module 12: Acid-Base Equilibria Chapter 17 –The Chemistry of Acids and Bases |
|
Thursday, 2/17 |
Exam Module 10
& 11 |
|
Thursday, 2/17 |
Lab – Household Acids and Bases and
Equilibrium |
|
|
|
|
Tuesday, 2/22 |
Continue Module 12 |
|
Thursday, 2/24 |
Finish Module 12 |
|
Thursday, 2/24 |
Lab Midterm |
|
|
|
|
Tuesday, 3/1 |
LAST DAY TO DROP WITHOUT ACADEMIC PENALITY |
|
Tuesday, 3/1 |
Module 13: Hetergeneous Equilibria Chapter 18 – Other Aspects of Aqueous Equilibria (18.1-18.3) |
|
Thursday, 3/3 |
Continue Module 13 |
|
Thursday, 3/3 |
Lab - Titration Curves
of Weak and Strong Acids
|
|
|
|
|
Tuesday, 3/8 |
Exam-Module 12
& 13 |
|
|
No lab Spring Break week |
|
Thursday, 3/10 |
CGCC is on
Spring Break |
|
|
|
|
Tuesday, 3/15 |
|
|
Tuesday, 3/17 |
Lab - The
Buffer in Lemonade |
|
Thursday, 3/17 |
|
|
Wed-Fri 3/16-3/18 |
Wallace also out
of town Thur 3/17 |
|
Tuesday, 3/22 |
|
|
Thursday, 3/24 |
|
|
Thursday, 3/24 |
Lab –
Qualitative Analysis: Mystery Powders |
|
|
|
|
Tuesday, 3/29 |
|
|
Thursday, 3/31 |
Lab –
Introduction to Organic |
|
Thursday,
3/31 |
Lab
–Synthesis of Aspirin, Part I |
|
|
|
|
Tuesday, 4/5 |
|
|
Thursday, 4/7 |
|
|
Thursday, 4/7 |
Lab –
Synthesis of Aspirin, Part II and Lab - Establishing a Table of Reduction
Potentials: Micro-Voltaic Cells |
|
|
|
|
Tuesday, 4/12 |
|
|
Thursday,
4/14 |
Lab –
Introduction to Polymers
|
|
Thursday,
4/14 |
Lab-
Classification and Identification of Common Plastics |
|
|
|
|
Tuesday, 4/19 |
|
|
Thursday, 4/21 |
|
|
Thursday 4/21 |
Lab Final |
|
|
|
|
Tuesday 4/26 |
Post Test – ACS General Chemistry Exam |
|
Thursday, 4/26 |
Final Exam – ACS
General Chemistry-Complete Year |
|
|
|
A more detailed course calendar will be developed which includes the scheduled quizzes for each lecture class and the weekly homework both on WebAssign and online. The tentative URL is:
Course Calendar: http://www.hccbrandon.net/chem1212/12calendarS05.html
Power Points from the textbook may be downloaded by the student for their study. Go to:
Power Points
prepared the instructor may be viewed at:
http://www.hccfl.edu/faculty/john_taylor/chem1212/powerpoints/12pptF04.html
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.
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.hccbrandon.net/chem1212/12grdS05.html
Grade Calculator: http://www.hccbrandon.net/chem1212/12grdcal.html
Point Grade Summary:
_______(010) Explorations
Lab week 1 [Email (2); Dis
Wheel: (2) LrnSty:(4)
Time:(2) Card (2)
_______(000) ACS Placement
Pre Test Lab week 1
_______(030) Attendance
[Lecture 30+ lectures x 1 point each]
_______(050) Homework via
Web Assign [up to 25 bonus points]
_______(020) On-Line
Homework/Presentation System Responses
_______(500) Modular Exams
_______(050) ACS
_______(120) Final Exam
[20 Practice + 50 of 70 x 2 pts ACS Exam]
_______(140) Lab
Assignments [14x10]
_______(030) Lab Midterm
_______(050) Lab Final
_______(1000) Grand Total
Tentative (point)
% Weighting of the Components of the
Course:
Exams 50%
Homework
7%
Attendance 3%
Post-Test 5%
Final Exam 12%
Lab Assignments 15%
Lab Midterm and Lab Final 8%
Total 100%
Grade Calculation:
The
following example illustrates how the final grade is determined using weighted
averages. Note: This sample contains less
grades than you will actually have. For
example, there should be 8 exam grades instead of 3 as each of the actual exams
will.
|
Component Grades (points received / points possible, # in parentheses is percentage) |
Average (percentages
added together and divided by total
number of grades) |
Average x Weight |
Total (% points received for this component/ possible % points) |
|
Explore: 10/10 |
100% |
100 x 0.01 |
1/1 |
|
Attendance 28/30 |
93.3% |
93.3 x 0.03 |
2.8/3 |
|
Exam Grades: 42/50 (84%), 45/50 (90%),
36/50 (72%) |
(84 + 90+ 72) / 3= 82.0% |
82.0 x 0.50 = |
41.0/50 |
|
Homework-WebAssign: 23/25 (92%), 20/27 (74%), 21/24 (88%) |
(92 + 74 + 88) / 3 = 84.7% |
84.7 x 0.05 = |
4.2/5 |
|
Homework-Online 18/20 |
90.0% |
90.0 x 0.02 |
1.8/2 |
|
Lab Assignments: 9/10 (90%), 10/10 (100%),
10/10 (100%), 9/10 (90%) |
(90 + 100 + 100 + 90) / 4 = 95% |
95 x 0.14 = |
13.3/14 |
|
Lab Midterm and Final: 42/50 (84%), 36/50 (72%) |
(84+ 72) / 2 = 78% |
86 x 0.10 = |
8.6/10 |
|
ACS Post Test: 46/55 (84%) |
84% |
84 x 0.05 = |
4.2/5 |
|
ACS Final Exam: 38/50(70)=(76%)x1.6=60.9(80) 60.9+20=80.9(100) |
80.9% |
80.9 x .0.10 = |
8.1/10 |
|
|
|
Totaling last column à |
85.0/100 (85%) Grade = B |
Grade Availability:
Grades
may be calculated using a computer program specifically designed for that
purpose. The student may access an online version at anytime at:
http://www.hccbrandon.net/chem1212/12grdcal.html
The
instructor may have access to another similar program through Dr. Andrea
Wallace, who teaches the other section of CHEM 1211 and is the chair of the Department A hard
copy computer print out of your grades may be provided to you just prior to
midterm through Dr. Wallace’s program. Students should keep track of all their
grades on the hard copy of the grading outline attached to this syllabus, Then
they can input their grades into the on line calculator. The calculator will
ignore all sections and tests not yet completed. This allows to student to do
the “What if” I make this on the next test or the final and estimate what the
final outcome will be.
ON-Line Grade Calculator:
http://www.hccbrandon.net/chem1212/12grdcal.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 ~50% of the grade excluding the
final’s 12%, 23-25% for the laboratory
component [15% weekly work and 3% for the midterm and 5% for the final], 7% of
the grade for Homework, Interactive Classroom Presentation System and/or
Computer online Homework, 5% for the Post ACS Placement Test, and 3% 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. This exam must be completed before the next scheduled exam or the day the instructor returns the exam missed. The instructor guarantees the student two days to make up the exam, but thereafter it depends on the day the test are returned.
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 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 reports not returned prior to the Lab Midterm or those due after midterm not returned prior to the Final receive an automatic 10 points (100%). 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):
Department of Natural Sciences
and Mathematics Class Attendance Policy
The Department of Natural Sciences and Mathematics (DNSM) recognizes the importance of class attendance for success in college courses. The emphasis on class attendance may vary with the instructor, the course and the method of instruction being used.
The DNSM attendance policy
is as follows:
- Class attendance is a student responsibility.
- Class attendance is strongly encouraged,
the DNSM will support any instructor who chooses to include a statement
concerning absences and/or tardiness in his/her syllabus.
- DNSM instructors can give an “F” to a student who, for any reason, is counted
absent from 25% or more of the regularly scheduled class hours of a
course.
- DNSM instructors can use absences and tardiness as factors when calculating the
final grade.
- The attendance policy for each course must be distributed in writing by
the instructor at the beginning of each semester. The announcement will include a statement concerning academic penalties that
may result from excessive absences or tardiness.
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 Tuesay,
Academic Misconduct:
Academic misconduct or dishonesty such as cheating and plagiarism is not permitted. Suspected cases will be reported to the Vice President of Student Development Services and may result in failure of an assignment 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 quiz grade or examination grade or may sign 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 Coastal Georgia Community
College (CGCC) 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 CGCC 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.
Studying: In order to do well in this
course, it is essential to study and work problems. The following is a list of study suggestions
1)
Read the text chapters before the material is covered in class.
2)
Take good notes and review them daily.
3)
Work all assigned homework problems.
Do not get behind!!!!!!
4)
Work the practice exams that will be made available without looking at
the answer key.
5)
Work problems in ACS study guide.
6)
Use the interactive CD-Rom for studying.
Master Student Exercises:
The instructor
understands that the average attention span for a student listening to a
lecture is less than 20 minutes. Each
class is 150 minutes (two 75 minute sections and a 10-15 minute break). Generally, the instructor will attempt to
cover the lecture topic is short sound bites
|
Also the instructor
may incorporate exercises from the Becoming a Master Student
program. The $42 text may be ordered
online. It is one of the best
investments a college student may make.
The Discovery Wheel and Learning Styles Inventory are both assessments
from the Master Student text. It
is not required by this course, but suggested for students who need to
improve their study skills
From day-to-day the instructor and/or student groups may use
exercises from the program to break-up the lecture and expose the student
general learning principles. Most
instructors use story telling, group exercises, problem solving examples, etc
to break-up a long lecture so as to allow the brain to shift-gears. |
|
The instructor’s
experience is that we math and science folks just go on-and-on-and-on, which
research shows is successful with 35 to 40% of the students. Those 35-40% need
to understand the problem with the other 65% who are struggling. Many times, athletes are mislabeled ‘dumb
jocks’ when they are excellent kinesthetic
learners and go absolutely crazy after 5 minutes of a traditional transmission
science lecture. All students need to
know their best learning style (auditory, visual, kinesthetic, mixed
modality) and find strategies to succeed in experiences not presented in
their preferred learning style. Go back
to high school, which homework did you attempt first, why? Did you put-off those dreaded subjects to
last, why?
During the first week all students will
complete a learning styles inventory supplied by the instructor or completed
online to be counted as part of the first week of lab.
Learning
Styles Web Site: http://www.hcc.cc.fl.us/faculty/john_taylor/learnstyle/menu.html
Beta
Test LSI Online: http://www.hccbrandon.net/learnstyle/lsi.html
(submit cycle and Grid) 2pts
MBTI:
http://www.hccbrandon.net/learnstyle/bryanpsy.html
(submit Analysis) 2pts
Master Student Discovery and Intention
Journal Entry System
One way to become a
better student is to use the Discovery
and Intention Journal Entry System to increase your effectiveness with the
least possible struggle. It’s a way to
focus your energy, and it is closely related to the idea of taking a First Step
such as the First Step in Alcoholics Anonymous.
Alcoholics must tell the truth about their drinking before they can
begin to change. Students must admit to
their strengths and weaknesses before they can take action. Students may first use a paper and pencil
journal (notebook), but by the third or fourth week journal activities should
be electronic word processing documents which may be E-mailed to the
instructor.
Through Discovery Statements, the student can learn “where you are.” They are
a record of what you learn about yourself as a student-both strengths and
weaknesses. Discovery Statements can also be declarations of what you want,
descriptions of your attitudes, statements of your feelings, transcripts of
your thoughts, and chronicles of your behavior.
Intention
Statements can be used to alter your course. They are statements of your commitment to do
a specific task, to take a specific action.
An intention arises out of your choice to direct your energy toward a
particular goal.
The following are the seven guidelines for Discovery and
Intention Statements:
Discovery Statements: Intention Statements:
1. Discover what you want. 1.
Make you intentions positive.(never use try)(use do)
2. Record the specifics. 2.
Make intentions small and keep able.
3. Notice your inter voices and pictures. 3.
Use observation criteria for success.
4. Notice physical sensations. 4.
Set time lines.
5. Use discomfort as a signal. 5.
Be careful of intentions that depend on others.
6. Suspend self-judgement.(be
kind) 6.
Anticipate self-sabotage.
7. Tell the truth. 7. Identify your rewards.