COURSE:                                          CHEM 1215, GENERAL CHEMISTRY II

                                                            Oklahoma City Community College, Spring 2012

 

INSTRUCTOR:                                  ______________________________

 

PHONE:                                             682-1611 EXT. ________________

 

EMAIL:                                              ______________________________

 

OFFICE LOCATION:                       ______________________________

 

OFFICE HOURS:                              ______________________________

 

 

LEARNING MATERIALS           

 

         Textbook:                       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 1215/0220 General Chemistry II Laboratory Manual.  Oklahoma City Community College, 2011.

         Goggles:                         Approved chemical splash goggles

 

         Periodic Table:               8 1/2" x 11" copy in the bookstore

 

         Optional Materials:        Solutions to Red Exercises for Chemistry:  The Central Science, 12th Edition,  Brown and Wilson, 2012,  Prentice-Hall.

                                                Mega Molecules Molecular Geometry kit.  

 

COURSE DESCRIPTION 

 

Prerequisite:  CHEM 1115 with a grade of "C" or better; MATH 1513 or MATH 1533 with a grade of "C" or better

 

5 CREDITS.   This course is a continuation of CHEM 1115 with emphasis on thermochemistry, intermolecular forces, properties of solutions, acid/base properties, kinetics, equilibrium, thermodynamics, electrochemistry, and organic chemistry.  Laboratory is an integral part of the course.  GenEd Requirement

COURSE COMPETENCIES

 

         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 inorganic nomenclature, stoichiometry, properties of solutions, kinetics, thermodynamics, electrochemistry, acid/base theory, bonding theories, and some basic organic chemistry.  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 your.name@email.occc.edu) 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 Spring and Fall 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 682-7520. All accommodations must be approved by the Assistant Director, Student Disability Services.

 

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.

 

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 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 of these grading areas is outlined below. 

 

         1)  Unit Exams. (6 Unit Exams @ 115 points = 690 points) Six unit exams will be given during the semester.  You are expected to take all exams in class except as indicated by your professor.  If you miss the in-class exam, you must take the make-up 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 in-class 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 re-tests must be completed within 14 days of the day the exam was given in class.  You may not re-test 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 re-take one exam you failed, or you can make up two exams. 

 

         2)  Quizzes.  (8 quizzes x 15 points = 120 points)  Eight online quizzes will be given throughout the semester.  No make-up quizzes will be given.  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.  Typically, you will have about ten days to access and complete an online quiz.  You MAY ask your instructor for help with online quiz problems 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.          

         3)  Lab Exercises. (13 lab exercises x 10 points = 130 points)  You are expected to complete 13 lab exercises which are worth 10 points each.  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 11 OF THE 13 LAB REPORTS.

 

You must do at least 11 of the 13 laboratory experiments -- you are expected to complete all 13 -- and submit completed data sheets for those labs.   There will only be one week during the semester that may be used to make up a missed lab.  We strongly advise you to complete all 13 labs and reports.  Although only 11 labs are required to pass the course, please understand that the lab exercises are worth 130 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 (this includes makeup labs) - 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

           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.)

 

         4)  Formal Lab Reports.  (2 x 15 points = 30 points)

 

         You are expected to independently write and submit two formal lab reports during the semester.  Your instructor will identify the specific labs for which a formal report is required and will provide you with the format for the formal lab report. 

 

5)  Comprehensive Final – (1 final exam x 100 points = 100 points)

 

A comprehensive final exam covering material from both General Chemistry I and General Chemistry II will be given in class on the last day of the semester.  Objectives for both the General Chemistry I and General Chemistry II portions of this exam 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.

 

Grading Scale:

 

Total points possible = 690 + 120 + 130 + 30 + 100 = 1070 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 55.0% 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 1070 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 1070 points possible but scores a 54.5% on the comprehensive final exam will receive a “D” in the course.

 

Grade

%

Minimum Final Exam Score

A

90.0 – 100

70.0%

B

80.0 – 89.9

70.0%

C

70.0 – 79.9

55.0%

D

60.0 – 69.9

none

F

59.9 or less

none

 

         Exams and quizzes represent 85% of your final grade.  Lab assignments represent 15% of your final grade. You should keep track of your scores throughout the semester, recording your scores as papers are returned to you.  Use the grade record form on the final page of the syllabus to record your scores.

 

 

TRANSFERRING LAB GRADES

 

IMPORTANT:  Beginning with the Summer 2012 semester, lab grades earned during a previous attempt at CHEM 1215 will no longer transfer to subsequent semesters.  This means that if you withdraw from CHEM 1215 this spring, you must take both lecture and ALL labs again.

 

You must be enrolled in a section of CHEM 0220.  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 0220 lab work at OCCC within the past calendar year, you may transfer the grades for those completed labs to your current Chem 1215 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 sshore@occc.edu the following information:  1) your name and student ID number, 2) the name of your former Chem 0220 lab instructor, 3) the name of your former Chem 1215 lecture instructor, and 4) the name of your current Chem 1215 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 ABOUT MAKE-UP EXAMS AND RETESTS

 

         You are not allowed to use programmable or graphing calculators on tests or quizzes in class or in the Test Center.  A simple scientific calculator is all you need.

            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 in-class exam.

            7)  You are limited to a total of two retests and/or make-up exams during the semester.

            8)  You may not retest on the comprehensive final exam.

 

 

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.

UNIT OBJECTIVES

 

Unit 1:  Thermochemistry

Reading:          Chapter 5

Textbook

Homework:     Chapter 5 – 5.3, 5.4, 5.8, 5.27, 5.29, 5.35, 5.39, 5.41, 5.43, 5.45, 5.49, 5.52, 5.55,  5.57, 5.59, 5.61, 5.65, 5.67, 5.69, 5.73, 5.75, 5.77, 5.99, 5.100, 5.102

 

OBJECTIVES

 

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 calculate DE for a system given information about the heat absorbed or produced by a system and the work done on the system or done by the system.  You will be able to calculate the amount of work done on or by a system given pressure and volume information.  You will be able to relate DE and DH and state their definitions.

3.      You will be able to express enthalpy changes and internal energy changes using a variety of units.

4.      Given the necessary calorimetric data you will be able to calculate the heat of combustion at constant volume of a substance in a bomb calorimeter or the heat of reaction or the heat of solution of a specified process in a constant-pressure calorimeter.  Given appropriate data, you will be able to calculate heat capacities, specific heat capacities, molar heat capacities, and temperature changes occurring in a calorimeter or elsewhere.

5.      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 reaction component.  Given a thermochemical equation and a specific enthalpy change, you will be able to calculate the number of grams or moles of a reaction component necessary to give the specified enthalpy change.

6.      Given appropriate thermochemical information, you will be able to apply Hess's law to determine the enthalpy change for a specified reaction.

7.      Given a table of standard enthalpies of formation, you will be able: (a) to write a chemical equation representing the heat of formation of a substance, and (b) to calculate the ∆ for a reaction representing the formation of any specified number of moles of a given substance from its elements in their standard states.

8.      Given the standard enthalpy change for a specified reaction and the standard heats of formation for all but one of the reaction components, you will be able to calculate the unknown DHf°.

9.      You will be able to answer questions or solve problems relating to material from General Chemistry I.  You will be able to answer questions and solve problems incorporating material from General Chemistry I with the current unit objectives.

Unit 2:  Inorganic Nomenclature, Intermolecular Forces, and Properties of Solutions

 

Reading:          Chapter 2 (sections 2.7 and 2.8 only), Chapter 11 (sections 11.1, 11.2, 11.4,
11.5,  and 11.6 only), and Chapter 13 (sections 13.2 to 13.5 only)

Textbook

Homework:     Chapter 2 –2.56, 2.60, 2.61, 2.66, 2.68, 2.70, 2.71, 2.73

                        Chapter 3 – 3.58

Chapter 11 – 11.2, 11.4, 11.5, 11.6, 11.9, 11.17, 11.18, 11.40, 11.45, 11.47, 11.49, 11.54, 11.78, 11.85, 11.91

Chapter 13 – 13.1, 13.15, 13.16, 13.23, 13.28, 13.29, 13.33, 13.35, 13.37, 13.39, 13.41, 13.45, 13.47, 13.49, 13.51, 13.52, 13.53, 13.62, 13.69, 13.71, 13.73, 13.75, 13.77

 

OBJECTIVES

 

NOTE:  Objectives 1-4 are review from Chem 1115 and will not be covered in lecture.  Objectives 1-4 will constitute 20% of the Unit 2 Exam.

 

1.      Given any of the following terms, you will be able to define that term and/or recognize an acceptable definition:  cation, anion, binary compound, polyatomic ion, oxyanion, ionic compound, molecular (covalent) compound.

2.      Given the formula of a compound that has a metal or NH4+ as its positive part, you will be able to write an acceptable name for that compound; given the name of such a compound, you will be able to write the formula for it.

3.      Given the formula of a compound formed from two nonmetals, you will be able to write the name for that compound; given the name of such a compound, you will be able to write the formula for it.

4.      Given the formula of an acid, you will be able to write the name of that acid; given the name of that acid, you will be able to write the formula for it.

5.      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, vapor pressure, boiling point, normal boiling point, melting point, normal melting point, triple point, critical temperature, critical pressure, critical point, volatile, nonvolatile, colligative property, osmosis, supercooling, heat of fusion, heat of vaporization, heat of solution, dynamic equilibrium, unsaturated solution, saturated solution, supersaturated solution, hypotonic solution, isotonic solution, hypertonic solution, molarity, molality, mass percent, parts per million, and parts per billion.

6.      Given a molecule, you will be able to predict the types of intermolecular forces present.  Given a list of molecules, you will be able to rank them in order of relative boiling points, freezing points, vapor pressures, or water solubilities based upon the intermolecular forces present.  You will be able to relate vapor pressure and boiling point.

7.      You will be able to explain the various segments of a heating/cooling curve.  Given the heat of fusion, heat of vaporization, and the appropriate specific heats of a substance, you will be able to calculate the heat needed/evolved to completely convert a given mass of the substance in its solid or liquid state to its gaseous state and vice versa.

8.      You will be able to use a phase diagram to determine the state (phase) of a substance given its temperature and pressure.  You will recognize that the boundary lines on the phase diagram represent equilibria between two phases and be able to state which phases are in equilibrium.  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.

9.      You will be able to define critical temperature and critical pressure and be able to find the critical point on a phase diagram.

10.    You will be able to discuss and/or recognize factors affecting the solubility of substances.  You will be able to apply Henry's Law to determine the solubility of a gas.

11.    Given experimental data, you will be able to determine the effect of temperature on solubility.

12.    You will be able to express the concentration of a solution in molarity, mass percent, molality, mole fraction, and parts per million (ppm) and be able to convert from one unit of concentration to another.  You will recognize that molality, mole fraction, mass percent, and ppm are concentration units that are independent of temperature while molarity is dependent on temperature.

13.    You will be able to determine the concentrations of solutions (in any of the units of objective 12) made by dilution of a stock solution.

14.    You will be able to use Raoult’s Law to determine the vapor pressure of a solution.

15.    You will be able to calculate freezing point depression, boiling point elevation, the molar mass of a solute, or the molality of a solution.

16.    You will be able to explain how electrolytes affect colligative properties as compared to nonelectrolytes and be able to predict which one of a group of compounds should have the greatest effect on the colligative properties of a solution

17.    You will be able to describe how hypertonic, isotonic, and hypotonic solutions affect the morphology of a red blood cell.

18.    You will be able to answer questions or solve problems relating to previous units and/or General Chemistry I.  You will be able to answer questions and solve problems incorporating material from past units and/or General Chemistry I with the current unit objectives.

 

Unit 3:  Chemical Kinetics

Reading:          Chapter 14

Textbook

Homework:     Chapter 14: 14.1,14.3, 14.5, 14.9, 14.17, 14.19, 14.21, 14.23, 14.25, 14.27, 14.29, 14.31, 14.33, 14.34, 14.35, 14.37, 14.39, 14.40, 14.41, 14.43, 14.49, 14.55, 14.57, 14.61, 14.63a, 14.65, 14.73, 14.75, 14.91a, 14.95a

Chapter 21- 21.33, 21.34, 21.35, 21.36

 

OBJECTIVES

 

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 know that the rates of chemical reactions depend upon concentrations of reactants, reaction orders, and rate constants.

3.      You will be able to distinguish zero, first, and second order reactions using rate data.  Given appropriate data you will be able to write a rate law expression for a chemical reaction and determine values for the rate constant (including proper units).  Given a reaction order for a reactant, you will be able to predict how rates will be affected by changes in concentration of that reactant.

4.      You will be able to relate the rate of change in the concentration of a reactant or product to the rate of change in the concentration of another reactant or product.  Given concentrations and a time interval, you will be able to calculate an average reaction rate.

5.      Given the half-life or rate constant of a first order process and an initial amount of a reactant or radioactive isotope, you will be able to predict the amount of a reactant or isotope present at any later time.  Given the initial amount of material present, you will be able to calculate the amount of time needed to reach a specified final amount of reactant or isotope.  Given an initial amount and a final amount present after a certain time, you will able to calculate the half-life of a reactant or isotope or calculate the rate constant for the decomposition.

6.      Given concentrations at different times and a reaction order, you will be able to calculate the rate constant for the reaction.

7.      You will be able to discuss and/or recognize the role collisions and relative orientations play in reactions.  You will be able to write rate law expressions for elementary reactions.

8.      You will be able to label reactants, transition states, and products on an energy profile.  Given an energy profile for a reaction, you will be able to identify the overall delta H for the reaction and the energy of activation.

9.      You will be able to determine the effect of activation energies or changes in activation energies on relative reaction rates.

10.    You will know that the rate constant depends on temperature and activation energy and will be able to compute the rate constant at a given temperature using the Arrhenius equations.  You will be able to determine the  activation energy when given a graph of ln k versus 1/T or when given rate constants as a function of temperature.

11.    You will be able to answer questions or solve problems relating to previous units and/or General Chemistry I.  You will be able to answer questions and solve problems incorporating material from past units and/or General Chemistry I with the current unit objectives.

Unit 4:  Chemical Equilibrium, Acid-Base Chemistry, and Acid-Base Equilibria

 

Reading:          Chapter 15, Chapter 16, and Chapter 17 (sections 17.1-17.6)

 

Textbook

Homework:     Chapter 15:  15.15, 15.17, 15.23, 15.33, 15.35, 15.37, 15.39, 15.45, 15.47, 15.49b, 15.51, 15.53, 15.57, 15.59, 15.61, 15.83, 15.87, 15.93

                        Chapter 4:  4.39, 4.81 (a &b), 4.83, 4.103, 4.106

                        Chapter 16:  16.15, 16.17, 16.25, 16.29 (a & b), 16.31, 16.37, 16.43, 16.45, 16.47, 16.51, 16.57, 16.59, 16.71, 16.73, 16.75, 16.89, 16.97

                        Chapter 17:  17.15, 17.21, 17.23 a, 17.29, 17.37c, 17.41, 17.43c, 17.45 d, 17.51, 17.57, 17.67, 17.72, 17.88a

                        Note:  Some homework questions require the use of the tables of Ka’s, Kb’s, and Ksp’s found in Appendix D of the text.

 

OBJECTIVES

 

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 chapters plus the terms molar solubility and solubility product constant.

2.      Given the equation representing a homogeneous or heterogeneous equilibrium you will be able to write the equilibrium expression.

3.      Given appropriate data, you will be able to calculate the value of an equilibrium constant for a reaction.

4.      Given appropriate data, you will be able to calculate a reaction quotient and be able to state the direction in which the system will shift in order to obtain equilibrium.

5.      You will be able to determine equilibrium concentrations of reaction components given initial concentrations and an equilibrium constant.

6.      You will know that equilibrium constants are temperature dependent and that a temperature change is the only factor that can change the value of the equilibrium constant for a given equilibrium.

7.      Given a reaction at equilibrium and whether it is exothermic or endothermic, you will be able to apply LeChâtelier's principle to predict the direction in which the reaction will shift due to disturbances such as (a) a temperature change, (b) a change in the amount of one of the reaction components, (c) a change in the volume of the system, (d) a change in the pressure of a system due to the addition of an inert gas, or (e) the addition of a catalyst.

8.      Given the concentrations (or information that can be used to calculate the concentrations) of a cation and an anion in a solution and the appropriate solubility product constant, predict whether precipitation will occur.

9.      Given the concentrations of two or more cations in a solution and the appropriate solubility product constants, calculate the concentration of an anion required to begin the precipitation of each cation.  Given the concentrations of two or more cations in solution and the appropriate solubility product constants, predict which cation will precipitate first.

 

10.    Given a chemical equation, you will be able to identify the Brønsted-Lowry acid and Brønsted-Lowry base and their respective conjugates.

11.    Given a chemical equation, you will be able to identify the Lewis acid and the Lewis base.

12.    You will be able to relate the strengths of acids to Ka or the relative strengths of two oxyacids or two binary acids to molecular structure.

13.    You will know the names and formulas of the seven common strong acids and the eight strong inorganic bases.  Given the molarity of a solution of any of these acids or bases, you will be able to calculate H+ ion concentration, OH- concentration, pH, and pOH.

14.    Given any one of the following, you will be able to calculate the others:  [H+], [OH-], pH, pOH.

15.    Given the concentration of a weak acid and its Ka, you will be able to calculate the [H+] and pH of the solution.

16.    Given the concentration of a weak base and its Kb, you will be able to calculate the pOH, [H+], and the pH of the solution.

17.    You will be able to calculate the pH of a buffered solution using the Henderson-Hasselbalch equation.  Given the pH of a buffered solution of a particular substance, you will be able to calculate the conjugate base to acid ratio needed to obtain the desired pH.  You will be able to relate buffering capacity to pH and to concentrations and/or volumes of buffers.

18.    For an acid-base neutralization reaction (such as occurs in a titration or in the action of a buffer), you will be able to write and balance the equation for the neutralization reaction and calculate the initial and final concentrations of reactants and products. 

19.    You will be able to interpret a titration curve to identify the following information:  the equivalence point, the volume of base required to reach an equivalence point, the region of maximum buffering capacity, the pKa’s, and the region where the pH depends upon the initial acid concentration.  Given the concentration of the base and the volume of acid solution used or the mass of acid used, you will be able to determine the concentration of the acid or its molar mass.

20.    You will be able to calculate the pH at the equivalence point of a titration.

21.    Given the names or formulas of an ionic compound, you will be able to write the chemical equation for the dissolution of that compound in water. 

22.    Given the value of the equilibrium constant for the dissolution of an ionic compound, you will be able to calculate the solubility of the compound or the equilibrium concentrations of the constituent ions.  Given equilibrium concentrations of ions, you will be able to calculate the equilibrium constant for the dissolution process.

23.    You will be able to answer questions or solve problems relating to previous units and/or General Chemistry I.  You will be able to answer questions and solve problems incorporating material from past units and/or General Chemistry I with the current unit objectives.

 

Unit 5:  Thermodynamics, Spontaneity, Free Energy, Redox Reactions, Electrochemistry, and the Nernst Equation

 

Reading:          Chapter 19, Chapter 4 (section 4.4 only), and Chapter 20 (omit section 20.9)

 

Textbook

Homework:     Chapter 19 – 19.7, 19.11, 19.17a & b, 19.25, 19.37, 19.41, 19.43, 19.53, 19.57, 19.59a & b, 19.61c & d, 19.65, 19.71a & b, 19.75, 19.77, 19.79, 19.81, 19.83, 19.85, 19.93, 19.98 (note typo…you are to find DG not DG° ), 19.108a, 19.112a-c

                        Chapter 4 - 4.49, 4.50, 4.51, 4.52

                        Chapter 20 - 20.11, 20.15, 20.19, 20.23, 20.24, 20.27, 20.31, 20.35, 20.37, 20.43, 20.47, 20.51, 20.53, 20.65, 20.67

 

OBJECTIVES

 

1.      Define and/or recognize an acceptable definition or example of each of the following:   oxidation-reduction (redox) reaction, oxidation, reduction, oxidizing agent (oxidant), reducing agent (reductant), oxidation state, activity series, half-reaction, voltaic (galvanic) cell, cathode, anode, standard hydrogen electrode (SHE), faraday, spontaneous process, reversible process, irreversible process, entropy, Gibbs energy or free energy, standard free energy of formation, First Law of Thermodynamics, Second Law of Thermodynamics, Third Law of Thermodynamics.

2.      Given a reaction, you will be able to predict whether the entropy change for that reaction will be positive or negative without actually calculating its value.

3.      Given a table of standard entropies, you will be able to calculate a standard entropy change for a reaction.

4.      Given the signs, or information that can be used to determine the signs, of DH and DS for a given reaction you will be able to predict whether that reaction will be (a) spontaneous at all temperatures, (b) spontaneous only at relatively high temperatures, (c) spontaneous only at relatively low temperatures or (d) nonspontaneous at all temperatures.

5.      You will be able to determine the standard free energy change for a specified reaction given (a) the standard enthalpy and standard entropy changes for that reaction or (b) the standard free energies of formation of each of the reactants and products in that reaction.

6.      You will know that the Gibbs free energy change for a reaction represents the maximum work that can be obtained from that reaction.  Given grams or moles of a substance, you will be able to calculate the maximum work that can be obtained from that amount of substance reacting in a combustion reaction that you write and balance yourself.

7.      Given the necessary information you will be able to (a) determine the free energy change for a specified reaction under standard or nonstandard conditions, (b) predict whether that reaction is spontaneous or nonspontaneous, and (c) explain your reasoning for that conclusion.

8.      Given the equilibrium constant for a specified reaction (or the necessary information to determine that value), you will be able to calculate the value of DG° for that reaction.

 

9.      Given the value of DG° for a specified equilibrium (or the necessary information to determine DG°), you will be able to calculate the value of the equilibrium constant for the reaction.

10.    Given the formula of a compound, you will be able to determine the oxidation numbers of specified elements in the compound.

11.    Given a balanced oxidation-reduction (redox) reaction, you will be able to identify the oxidizing and reducing agents in the reaction.

12.    Given an unbalanced equation for a redox reaction in acidic or basic solution, you will be able to balance the equation by the half-reaction method.

13.    Given two half-cell reactions of a galvanic cell and a table of standard reduction potentials, you will be able to write a balanced reaction, determine the standard cell potential of the galvanic cell, and identify the anode and cathode of the galvanic cell.

14.    You will be able to relate ease of oxidation and reactivity to standard reduction potentials.

15.    You will be able to determine the spontaneity of a redox reaction under standard and nonstandard conditions using either ΔG or the emf (E) of the reaction.

16.    You will be able to calculate DG°, or K, or E° given any one of the three, or given information that would be sufficient to calculate any one of the three.

16.    Given the Nernst equation, you will be able to determine the emf of a cell based on the concentrations of reactant and products or the ratio of products to reactants based on emf.

17.    You will be able to answer questions or solve problems relating to previous units and/or General Chemistry I.  You will be able to answer questions and solve problems incorporating material from past units and/or General Chemistry I with the current unit objectives.

 

 

Unit 6:  Theories of Covalent Bonding and Organic Chemistry

 

Reading:          Chapter 8 (sections 8.1 to 8.7 only), Chapter 9, and Chapter 24

 

Textbook

Homework:     Chapter 8 – 8.19, 8.47, 8.48 a, c, & d, 8.63, 8.90

                        Chapter 9 – 9.25, 9.27, 9.31, 9.43, 9.45, 9.55, 9.61 a-c, 9.63. 9.65, 9.73 a, b, & d, 9.79, 9.81, 9.82

                        Chapter 24 – 24.1, 24.4, 24.9, 24.10, 24.15, 24.28, 24.29 (omit d), 24.43, 24.44, 24.55 a & b, 24.86, 24.95

 

OBJECTIVES

 

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 each of the chapters.

2.      You will be able to describe and/or recognize a description of the basic approaches taken by the valence-bond theory and by the molecular orbital theory in explaining covalent bonding and will be able to describe the major differences between the two theories.

3.      For a given molecule or polyatomic ion, you will be able to draw a valid Lewis structure and use the electron-pair geometries from VSEPR theory to deduce the hybrid orbitals used by a specified atom in that molecule or ion to form its bonds.

4.      You will be able to fill out an energy-level diagram for a diatomic molecule or ion and determine its bond order and whether it is paramagnetic or diamagnetic.           

5.      You will be able to draw structural isomers for a given alkane.

6.      Given the structural formula of an alkane, cycloalkane, alkene, alkyne, or alcohol with ten or fewer carbons in the main chain or ring, you will be able to give a systematic name for the compound, including any geometric isomer designations.  Given the systematic name of such a compound you will be able to write a correct structural formula for that compound. 

7.      You will be able to state the essential and distinguishing characteristic of an aromatic compound.

8.      Given the structural formula for an organic or biological molecule containing one or more functional groups, you will be able to identify the functional group(s) and name the class of each functional group present.

9.      Given the name or structure of an alcohol, you will be able to state whether it is primary, secondary, or tertiary.

10.    You will be able to answer questions or solve problems relating to previous units and/or General Chemistry I.  You will be able to answer questions and solve problems incorporating material from past units and/or General Chemistry I with the current unit objectives.

 

Objectives for Comprehensive Final Exam

 

 

1.      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.

2.      Given the density and volume of a liquid, you will be able to calculate the mass or number of moles of that substance.

3.      You will be able to classify an element as:

                        Metal, nonmetal, or metalloid

                        Alkali metal, alkaline earth metal, halogen, noble gas, or other

                                    Main group, transition metal, lanthanide or actinide

4.      You will be able to list or recognize the names and formulas of elements that occur naturally as diatomic molecules.

5.      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. 

6.      Given the formula of an ionic compound, you will be able to write the name of the compound.  Given the name of an ionic compound, you will be able to write its chemical formula.

7.      Given the name of one of the common strong acids, you will be able to write its formula.  Given the formula for one of the common strong acids, you will be able to write its name.

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.      Given the names and/or formulas of the reactants and products (including simple organic compounds) involved in a chemical reaction, you will be able to write a balanced chemical equation.

10.    You will be able to work the following types of stoichiometry problems:  mass-mass, mass-moles, and moles-moles.

11.    Given mass of solute and total volume, you will be able to calculate the molarity of a solution.

12.    Given the molarity of reactants and/or products, you will be able to work the following types of stoichiometry problems:  volume A – mass B, volume A – mol A, volume A – mol B, volume A – volume B.

13.    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.

14.    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.

15.    Given the appropriate information, you will be able to describe the steps required to prepare a specified solution by diluting a stock solution.

16.    Given the formula for a molecular compound or a polyatomic ion, you will be able to draw a valid Lewis structure for that substance.

17.    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.

18.    Given a thermochemical equation, you will be able to calculate the enthalpy change for a reaction involving a given mass of a reactant or product for either the forward or reverse reactions.

19.    Given information about the heat gained or lost by a system and the work done on or by the system, you will be able to calculate the change in internal energy for the system.

20.    Given the necessary calorimetric data, you will be able to calculate the specific heat of a substance, heat of combustion, or heat of solution of a substance.

21.    You will be able to explain the various segments of a heating/cooling curve.  Given the heat of fusion, heat of vaporization, and specific heats of a substance, you will be able to calculate the heat necessary to completely convert a given mass of the substance in its solid or liquid state to its gaseous state and vice versa.

22.    Given a molecule, you will be able to predict the types of intermolecular forces present.  Given a list of molecules, you will be able to rank them in order of relative boiling points, freezing points, vapor pressures, or water solubilities based upon the intermolecular forces present.  You will be able to relate vapor pressure and boiling point.

23.    You will be able to express the concentration of a solution in molarity, mass percent, molality, mole fraction, and parts per million (ppm) and be able to convert from one unit of concentration to another. 

24.    Given a phase diagram, you will be able to determine the melting/freezing point, the boiling/condensation point, and the sublimation/deposition point of a substance at a given pressure.  You will also be able to identify the triple point and the equilibrium it represents, critical point, critical temperature and critical pressure.

25.    Given appropriate experimental data, you will be able to write a rate law expression for a chemical reaction, determine the value of the rate constant, and calculate the rate of the reaction using a new set of reactant concentrations.

26.    Given a balanced chemical equation and the rate of change in the concentration of a reactant or product, you will be able to calculate the rate of change of a different reactant or product.

27.    Given concentrations of a reactant or product and a time interval, you will be able to calculate the average reaction rate.

28.    Given an energy profile for a reaction, you will be able to label the reactants, products, and transition states as well as determine the overall ∆H for the reaction and the energy of activation.

29.    Given an equation representing a homogeneous or heterogeneous equilibrium, you will be able to write the equilibrium constant expression.

30.    Given appropriate data, you will be able to calculate the value of an equilibrium constant.

31.    Given a reaction at equilibrium and whether it is exothermic or endothermic, you will be able to apply LeChâtelier's principle to predict the direction in which the reaction will shift due to disturbances such as (a) a temperature change, (b) a change in the amount of one of the reaction components, (c) a change in the volume of the system, (d) a change in the pressure of a system due to the addition of an inert gas, or (e) the addition of a catalyst.

32.    Given the molarity of a strong acid or strong base solution, you will be able to calculate, [H+], [OH-], pH, and pOH for the solution at 25°C.

33.    Given the concentration of a weak acid solution and its Ka, you will be able to calculate the [H+] and pH of the solution.

34.    Given a chemical equation, you will be able to identify the Brønsted-Lowry acid and Brønsted-Lowry base and their respective conjugates.

35.    You will be able to relate the strengths of acids to Ka  or pKa.

36.    You will be able to interpret a titration curve in order to find the volume of base required to reach an equivalence point.  Given the concentration of the base and the volume of acid solution used or the mass of acid used, you will be able to determine the concentration of the acid or its molar mass.  You will be able to find the pKa from a titration curve.

37.    Given an unbalanced equation for a redox reaction in acidic or basic solution, you will be able to balance the equation by the half-reaction method.

38.    Given a balanced redox reaction, you will be able to identify the element being oxidized, the element being reduced, the oxidizing agent, and the reducing agent.

39.    Given the standard reduction potentials of two half-reactions, you will be able to calculate the emf of a galvanic cell.  You will be able to write a balanced chemical equation for the overall reaction.

40.    Given a reaction or process, you will be able to predict whether the entropy change for the reaction/process will be positive or negative without calculating its actual value.

41.    Given the signs, or information that can be used to determine the signs, of DH and DS for a given reaction you will be able to predict whether that reaction will be (a) spontaneous at all temperatures, (b) spontaneous only at relatively high temperatures, (c) spontaneous only at relatively low temperatures or (d) nonspontaneous at all temperatures.

42.    You will be able to determine the standard free energy change for a specified reaction given the standard enthalpy and standard entropy changes for that reaction.

43.    Given DG° for an equilibrium process, you will be able to calculate the equilibrium constant and determine the equilibrium concentration of the reactants and/or products.

44.    Given a balanced equation and free energies of formation, you will be able to calculate DG° for the reaction.

45.    Given the structure of an organic compound, you will be able to identify and name the functional groups present.

46.    Given the name of an alkane, alkene, alkyne, or alcohol containing no more than 10 carbons in the longest chain, you will be able to draw its structure.  Given the structure of an alkane, alkene, alkyne, or alcohol containing no more than 10 carbons in the longest chain, you will be able to give its IUPAC name.

47.    You will be able to identify the hybrid orbitals used by carbon atoms involved in single, double, and triple bonds.

 

 

 

 

Total points possible = 690 + 120 + 130 + 30 + 100 = 1070 points

 

Grading Scale:            

                        90.0% or higher and at least a 70.0% on the final for an “A”

                        80.0 - 89.9% and at least a 70.0% on the final for a “B”

                        70.0 – 79.9% and at least a 55.0% on the final for a “C”

                        60.0 – 69.9% for a “D”

                        Under 60.0% for an “F”

Grade record:

 

Exam 1  _____

Lab 1      _____

Quiz  1  _____

Exam 2  _____

Handout _____

Quiz  2  _____

Exam 3  _____

Lab 2      _____

Quiz  3  _____

Exam 4  _____

Lab 3      _____

Quiz  4  _____

Exam 5  _____

Lab 4      _____

Quiz  5  _____

Exam 6  _____

Lab 5      _____

Quiz  6  _____

*Final      _____

Lab 6      _____

Quiz  7  _____

 

Lab 7      _____

Quiz  8  _____

 

Lab 8      _____

 

 

Lab 9      _____

 

 

Lab 10    _____

 

 

Lab 11    _____

Lab 12    _____

 

 

 

 

 

Formal 1 _____

 

 

Formal 2 _____

 

 

 

 

 

 

 

Total    ______

Total _____

Total _____

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Total of all points:   __________

 

 

*Must meet minimum required score for an A, B, or C.  See “Grading Scale” above.

 

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 possibly bring your final grade up to that next level.  For instance, if you have an 88% average on your exams, you might get an “A” provided that you have most of the points for the labs and quizzes.  On the other hand, if you have an “A” exam average but have turned in several late labs and you have missed quizzes, an “A” could potentially drop to a “B,” a “B” could drop to a “C”, etc.