COURSE:                                          CHEM 1115, GENERAL CHEMISTRY I

                                                            Oklahoma City Community College, Spring 2012

 

INSTRUCTOR:                                  ______________________________

 

PHONE:                                             682-1611 EXT. ________________

 

EMAIL:                                              ______________________________

 

OFFICE LOCATION:                       ______________________________

 

OFFICE HOURS:                              ______________________________

 

 

LEARNING MATERIALS           

 

         Textbook:                       If you plan only to take Chem 1115, please obtain:

Chemistry:  The Central Science, Custom 12th Edition (Chem 1115 only)  (bundled with the MasteringChemistry™ Student Access Kit).  Brown, LeMay,  Bursten, Murphy, and Woodward.  2012.  Pearson.

                                                                                    -- OR –

If you plan to take both Chem 1115 and Chem 1215, please obtain:

Chemistry:  The Central Science, Custom 12th Edition (Chem 1115 and 1215)  (bundled with the MasteringChemistry™ Student Access Kit).  Brown, LeMay,  Bursten, Murphy, and Woodward.  2012.  Pearson.

                                                                                    -- OR –

                                                Chemistry:  The Central Science 12th Edition eBook with MasteringChemistry™ Student Access Kit. Brown, LeMay,  Bursten, Murphy, and Woodward.  2012.  Pearson.

                                                The access kit is good for two years.  If you purchased an access kit for Chem 1115 or 1215 in the last 20 months, it will work for this course.

 

         Lab Manual:                   Chemistry 1115/0110 General Chemistry I Laboratory Manual.  Oklahoma City Community College.  2011.

         Goggles:                         Approved chemical splash goggles.

 

         Optional Materials:        Mega Molecules Molecular Geometry kit.

                                                Non-programmable scientific calculator  (such as TI-30XA or Casio FX-260) 

 

 

COURSE DESCRIPTION 

 

         Prerequisite:  (R), (W), MATH 1513 or MATH 1533 or both MATH 0403 and high school chemistry or CHEM 1123.  A grade of "C" or better is required in all prerequisite courses.

 

5 CREDITS.    This course is designed for science and engineering majors.  The course covers nomenclature, atomic and molecular structure, stoichiometry, acid/base and other aqueous reactions, states of matter, phase changes, gas laws, and an introduction to thermochemistry.  Laboratory is an integral part of the course.  GenEd Requirement

 

COURSE COMPETENCIES        

 

         As stated in the course description, when you complete this course, you should be able to apply the principles and theories of chemistry to interpret fundamental chemical phenomena and predict the results of chemical reactions.  You should be able to demonstrate through tests, homework assignments, and laboratory exercises a basic knowledge of the periodicity of the elements, inorganic nomenclature, stoichiometry, metathesis reactions, redox reactions, properties of gases, atomic structure, and molecular geometry.  A list of specific learning objectives relating to these general competencies is attached.

 

ATTENDANCE

 

         Oklahoma City Community College requires regular class attendance and punctuality of students.

 

EMAIL

 

         Your OCCC email account (it has the form 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 Fall and Spring semesters or until the end of the sixth week in the Summer semester.

 

ACCOMMODATIONS FOR STUDENTS WITH SPECIAL NEEDS:

 

Oklahoma City Community College Complies with Section 504 of the Rehabilitation Act and the Americans with Disabilities Act. Students with disabilities who seek accommodations must make their request by contacting the Office of Student Support Services located on the first floor of the main building near SEM entry 3 or by calling 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 allowstriving for continuous improvement in its programs and services.  Student learningassessment is vital to the educational process and can be of significant value to you and to the students who follow youthe student as well as contribute to their education success.

 

To ensure that adequate adequate assessment information is available to allow OCCC to continuously improve programs and services, studentsyou 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 adesignated times, which may include class periods in a semester.  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 or perforated shoes are not permitted in the chemistry lab area.

You will not be allowed to complete the lab if you are not dressed appropriately.

 

GRADING

 

         The grade assigned for this course will be determined by your performance on unit tests, a comprehensive final, online quizzes, and lab assignments.  Detailed information about each grading area is outlined below. 

         1)  Exams (6 x 100 pts = 600 pts).  There will be six unit exams worth 100 points each plus a comprehensive final exam worth 100 points for a total of 700 points.  You are expected to take all exams in class.  If you miss the in-class exam, you must take the 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 the comprehensive final exam or on a make-up exam.

         *You are limited to a total of two retests and/or make-up exams during the semester.  In other words, you can re-test on two units you failed, you can make up one exam and re-take one exam you failed, or you can make up two exams.

         2)  Comprehensive Final (100 points).  A comprehensive final exam covering material from all of  General Chemistry I will be given in class on the last day of the semester.  Objectives for the final are given later in the syllabus.  You are expected to take the comprehensive final exam in class.  You may not re-test on the comprehensive final.  A make-up exam will be given only under extraordinary circumstances (as defined and approved by your instructor).

         In order to receive an “A,” “B,” or “C” in the course, a student must earn the minimum final exam score described in the table in the “Grading Scale” section.  Failure to achieve the minimum final exam score will result in a one letter grade reduction in the student’s overall course grade.  See the “Grading Scale” section for details.

 

 

            3)  Quizzes (6 x 15 pts = 90 pts).  There will be six online quizzes given throughout the semester.  Quiz questions will often be taken directly from or based upon homework problems.  Each quiz is worth fifteen points giving a total of 90 points possible on the quizzes.         No late quizzes will be accepted.  A score of zero will be recorded for any missed quiz.  Due dates for quizzes will be specified by your instructor (check your lecture schedule).  Typically, you will have about ten days to access and complete an online quiz.  You MAY ask your instructor for help with online quiz questions or any homework problems.

Computer access for MasteringChemistry online quizzes:  Since each quiz is open for several days, technical problems discovered on the due date of a quiz are not considered a viable excuse for not completing the quiz on time.  We strongly recommend that you access each quiz on the first day it becomes available so that your instructor can help you resolve any technical difficulties you may encounter.  Although you do have to purchase access to MasteringChemistry, you do not have to access it with your own computer.  The computers in the Physical Science Center (or any student accessible computer on campus) may be used to access and complete your MasteringChemistry assignment.

         4)  Lab Exercises (145 pts).  There are 12 lab exercises, ten worth 10 points each, one worth 20 points, and one worth 25 points.  Lab reports (data sheets) will be submitted to your lab instructor who will grade the reports.  The lab instructor will forward your lab grades to your lecture instructor at the end of the semester for use in determining your final grade.

         IN ORDER TO PASS THIS COURSE, YOU MUST COMPLETE AND RECEIVE A SATISFACTORY GRADE (≥ 2 pts) ON AT LEAST 10 OF THE 12 LAB REPORTS.

         You must do at least 10 of the 12 laboratory experiments -- you are expected to complete all 12 -- and submit completed data sheets for those labs.   There will be only one week in the semester that may be used to make up a missed lab, and we strongly advise you to complete all 12 labs and reports.  Although only 10 labs are required to pass the course, please understand that the lab grade consists of 145 points:  if you choose not to make up a lab, that lab grade will be a zero.

         Labs are due at the start of the following pre-lab period.  Late labs – this includes makeup labs - will be assessed a five point penalty.  Labs that are turned in after start of the pre-lab period will be considered late, regardless of the reason.   

         To receive full credit, all questions on the data sheet must be answered, appropriate calculations must be shown on the data sheet or on attached sheets of paper (as specified in the lab instructions), results must be within the expected range, and all calculations should be done according to the rules for significant figures.

         You can lose points on labs according to the following criteria:

            Late lab - 5 point penalty

            Incomplete lab report (i.e. some questions or calculations omitted) - 1 to 4 point penalty, depending upon how many calculations or questions are omitted

            Poor results - 0.5 to 2 point penalty, depending upon how bad the results are

            Calculation errors - 0.5 to 3 point penalty, depending upon how many errors are made

            Incorrect answers to questions - 0.5 to 1 point each

                 Incorrect use of significant figures - 0.5 to 1 point penalty, depending upon how many errors are made

 

         (Notice that it would be relatively easy to fall below the 2 point minimum required for passing this class if you submit an incomplete data sheet with a few calculation errors and poor results or incorrect responses to questions.  Submitting a late lab means that you should take extra care in making sure the lab is complete and your calculations are correct so that you do not fall below the 2 point minimum.)

 

Grading Scale:

 

         Total points possible = 600 + 100 + 90 +  145 = 935 points

         Your course grade will be determined primarily using the overall percentage of points earned during the course.  However, in order to receive an “A” or “B” in the course, you must also score at least 70.0% on the comprehensive final exam.  In order to receive a “C” in the course, you must also score at least 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 935 points possible but scores a 69.5% on the comprehensive final exam will receive a “B” in the course.  Similarly, a student who earns 79.2% of the 935 points possible but scores a 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

 

 

 

TRANSFERRING LAB GRADES

 

You must be enrolled in a section of CHEM 0110.  If you need to complete any labs at all, you will be expected to attend the first lab session to complete safety activities.  However, if you have completed some or all of the Chem 0110 lab work at OCCC within the past calendar year, you may transfer the grades for those completed labs to your current Chem 1115 lecture instructor and you will only have to attend those labs which you did not complete previously.  To transfer your lab grades, please email Dr. Steven Shore at sshore@occc.edu the following information:  1) your name and student ID number, 2) the name of your former Chem 0110 lab instructor, 3) the name of your former Chem 1115 lecture instructor, 4) the name of your current Chem 1115 instructor, and 5) either the name of your current lab instructor or your current lab section number.  The request for lab grade transfer should be made by the end of the second week of class.

 

INCOMPLETES

 

         An "I" grade may be given to students under extenuating circumstances.  Please understand that the issuing of an "I" grade is the instructor's prerogative and not a "right" of the student.

 

ACADEMIC DISHONESTY

 

            Academic dishonesty (such as copying from someone else or using unauthorized notes on exams) will result in a zero being given for the work in question and a record of the incident will be forwarded to the Office of the Vice President for Academic Affairs.  Further disciplinary action may result. 

 

THINGS TO REMEMBER

 

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

 

         For make-up exams or retests

                 1)    Know the Test Center operating hours!

                 2)    The Test Center will not give out tests later than one hour before closing time.

                 3)    You must have an OCCC photo ID to receive a test.

                 4)    The Test Center closes promptly at the posted times.  You will be required to turn in your test by closing time.

        5)    Make-up exams are subject to a 10 percentage point penalty and must be completed within 7 calendar days of the in-class exam.

                 6)    Re-tests on failed exams must be completed within 14 calendar days of the in-class exam.

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


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 FOR CHEM 1115

 

UNIT 1

 

INTRODUCTION:  MATTER AND MEASUREMENT

 

Reading:  Chapter 1, Chapter 2 (2.5 only, p. 49-52), Chapter 7 (7.1 only, p.  250-251)

 

Homework:    

Chapter 1:   1.1, 1.4, 1.7, 1.11,  1.13, 1.14, 1.19, 1.24, 1.25, 1.27, 1.28, 1.29, 1.33, 1.35, 1.37, 1.39, 1.40, 1.47, 1.48, 1.49, 1.51, 1.65, 1.68, 1.74

Chapter 2:   2.3, 2.37, 2.38, 2.94 a-f

 

1.         Define and/or recognize an acceptable definition or example of the terms listed in the "Summary and Key Terms" section at the end of the chapter.

2.         Given the name of a chemical element, you will be able to supply its symbol; given the symbol of a chemical element, you will be able to write its name.  You will be responsible for the following elements:

 

 

ELEMENT                

SYMBOL      

ELEMENT       

SYMBOL

                       

 

 

 

Aluminum                  

Al

Lead

Pb

Antimony

Sb

Lithium

Li

Arsenic

As

Magnesium     

Mg

Barium

Ba

Manganese     

Mn

Bismuth

Bi

Mercury          

Hg

Boron

B

Neon

Ne

Bromine

Br

Nickel

Ni

Cadmium

Cd

Nitrogen         

N

Calcium

Ca

Oxygen

O

Carbon

C

Phosphorus     

P

Cesium

Cs

Platinum         

Pt

Chlorine

Cl

Potassium       

K

Chromium

Cr

Radon

Rn

Cobalt

Co

Silicon

Si

Copper           

Cu

Silver

Ag

Fluorine

F

Sodium           

Na

Gold                           

Au

Sulfur                         

S

Helium

He

Tin

Sn

Hydrogen

H

Uranium         

U

Iodine

I

Zinc

Zn

Iron

Fe

 

 

 

 

 

 

 

 

3.         For any of the following quantities:  length; mass; time; temperature; or amount of substance, you will be able to list the base (fundamental) unit and its symbol in the International System of Units (the "SI" system).

4.         Given the value of a temperature in either °F, °C, or K and given the conversion equations, you will be able to convert the given value to either of the other two temperature scales.

5.         Given two of the three variables - mass, volume, and density, be able to calculate the third variable. 

6.         Given a number expressed as a decimal or in exponential notation, you will be able to indicate how many significant figures are present in that number.  Given an indicated calculation involving addition, subtraction, multiplication and/or division, you will be able to perform the calculation correctly and express the answer to the proper number of significant figures.

7.         Given a measured value, including its units, you will be able to convert the given value to a new specified unit using dimensional analysis.  You will be able to state or use the metric-metric conversions for mega, kilo, centi, milli, and micro.

8.         Using information given in a problem, you will be able to write an appropriate conversion factor and use the conversion factor (with or without other conversion factors) to solve a problem using dimensional analysis.

9.         Given the periodic table, you will be able to do the following:

            a.     classify a given element as being a metal, nonmetal, or metalloid;

            b.     classify a given element as being an alkali metal, alkaline earth metal, halogen, or noble gas;

            c.     classify a given element as being a main group (representative) element, transition metal, lanthanide, or actinide;

            d.    name two elements which are liquids at "room conditions" of temperature and pressure;

            e.     list the elements that occur naturally as diatomic molecules.

 

10.       Given a list of physical properties, you will be able to indicate which are characteristic properties of metallic elements and which are characteristic properties of nonmetallic elements.

11.       Given a list of chemical properties, you will be able to indicate which are properties of metals and which are properties of nonmetals.

 

 

UNIT 2

 

ATOMS, IONS, AND MOLECULES

ELECTRONIC STRUCTURE AND PERIODIC PROPERTIES OF ATOMS AND IONS

 

 

Reading:  Chapter 2, Chapter 6, and Chapter 7 (7.1 - 7.6)

 

Homework:    

Chapter 2:   2.17, 2.25, 2.27, 2.43, 2.45, 2.49, 2.51, 2.55, 2.57, 2.63, 2.65, 2.67, 2.99, 2.103, 2.104

 

Chapter 6:   6.9, 6.10, 6.23, 6.35, 6.51, 6.53, 6.55, 6.56, 6.65, 6.69 (omit e – write complete and condensed electron configurations and draw orbital diagrams), 6.71

 

Chapter 7:   7.25, 7.37, 7.45, 7.47

 

1.         Define and/or recognize an acceptable definition or example of the terms listed in the "Summary and Key Terms" sections at the end of Chapter 2, Chapter 6, and Chapter 7 (Sections 7.1-7.6 only).

 

2.         You will be able to state or recognize a statement of the Law of Conservation of Mass and the Law of Constant Composition.

 

3.         Given some combination of the number of protons, the number of neutrons, the number of electrons, the isotopic mass, and the complete isotopic symbol for some isotope, you will be able to supply the missing component(s) of the above list for that isotope.

 

(Unit 2 objectives continued on next page.)

 

4.         Given the name of a common ion, you will be able to write its symbol including the correct charge.  Given the symbol of a common ion, you will be able to write its name.  You will be responsible for the following common ions:

 

ION

SYMBOL

 

ION

SYMBOL

 

 

 

 

 

Hydrogen

H+

 

Fluoride

F-

Lithium

Li+

 

Chloride

Cl-

Sodium

Na+

 

Bromide

Br-

Potassium

K+

 

Iodide

I-

Rubidium

Rb+

 

Oxide

O2-

Cesium

Cs+

 

Sulfide

S2-

Silver

Ag+

 

Nitride

N3-

Magnesium

Mg2+

 

Phosphide

P3-

Calcium

Ca2+

 

 

 

Strontium

Sr2+

 

Hydroxide

OH-

Barium

Ba2+

 

Cyanide

CN-

Zinc

Zn2+

 

Nitrate

NO3-

Iron (II)

Fe2+

 

Acetate

C2H3O2-

Iron (III)

Fe3+

 

Sulfate

SO42-

Aluminum

Al3+

 

Hydrogen sulfate

HSO4-

 

 

 

    (bisulfate)

 

Ammonium

NH4+

 

Carbonate

CO32-

 

 

 

Hydrogen carbonate

HCO3-

 

 

 

    (bicarbonate)

 

 

 

 

Phosphate

PO43-

 

5.    Using the names and symbols of the common ions identified in the previous objective and a list of the names and symbols of less common ions, you will be able to name and write the formula for compounds composed of these species. 

 

6.         Given the formula of an ionic compound formed from the cations and anions, you will be able to write the name of the compound.  Given the name of a compound formed from these ions, you will be able to write the chemical formula.

 

7.         Given the name of one of the following household products, you will be able to write the name or formula of the ionic compound present in it:  baking soda, table salt, and bleach.

 

8.         Given the appropriate equations and constants, and given the value of one of the three characteristics of a photon (its wavelength, frequency, or energy), you will be able to calculate the values of the remaining two characteristics.  Given the energy of a covalent bond, you will be able to calculate the wavelength, frequency, or energy of a photon needed to break that bond.

 

9.         You will be able to recognize statements about the quantum mechanical model of the atom.  You will be able to recognize definitions of the four quantum numbers used in the quantum mechanical model of the atom.  You will also be able to recognize allowed sets of quantum numbers.

 

10.       Given the atomic number of any representative element or first-row transition element, you will be able to represent the electron configuration in complete form, in standard shorthand or "core" notation, or as an orbital diagram.

 

11.       You will be able to represent the electron configuration for a specified ion in complete form, in shorthand or “core” notation, or as an orbital diagram.

 

12.       You will be able to state or recognize statements describing the Pauli Exclusion Principle, Hund's Rule, and the aufbau principle.

 

13.       You will be able to state the general trends within the periodic table affecting the magnitude of each of the following properties:  first ionization energy, electron affinity, atomic size, and metallic character.  For a given pair of elements, you will be able to indicate which has the larger or smaller value of any of these properties.

           

14.       For an atom of a given element and an ion of that same element be able to state which has the larger or smaller size.  For atoms and ions within the same group or in an isoelectronic series, you will be able to predict the relative size of the ions.

 

15.       You will be able to answer questions or solve problems relating to the previous unit.  You will be able to answer questions and solve problems incorporating material from the past unit with the current unit objectives.

 

 

 

            UNIT 3

 

     INTRODUCTION TO COVALENT BONDING AND MOLECULAR GEOMETRY

 

Reading:  Chapter 2 (p. 64-66), Chapter 8, Chapter 9 (9.1-9.3 only)

 

Homework:                         

Chapter 2:   2.59, 2.69, 2.70, 2.71, 2.72

Chapter 8:   8.1, 8.10, 8.13, 8.14, 8.17, 8.19, 8.39, 8.42, 8.47, 8.48, 8.51, 8.53, 8.55, 8.57, 8.63,
                     8.65, 8.90, 8.92

Chapter 9:   9.3, 9.4, 9.22, 9.23, 9.26, 9.28, 9.30, 9.31, 9.32, 9.36, 9.39, 9.44

 

1.         Define and/or recognize an acceptable definition or example of the terms listed for the appropriate sections in the "Summary and Key Terms" section at the end of each chapter.

2.         Given a formula of a compound formed between two nonmetals, you will be able to write the name of the compound; given the name of a compound formed between two nonmetals, you will be able to write the formula.

3.         Given the name of an acid, you will be able to write its chemical formula; given the chemical formula of an acid, you will be able to write its name.

4.         Given the name of one of the following household products, you will be able to write the name or formula of the chemical present in it:  water, ammonia, natural gas, vinegar, hydrogen peroxide, drinking alcohol, rubbing alcohol, and nail polish remover.

5.         For a given atom or monatomic ion, you will be able to write its correct electron-dot (Lewis) symbol.

6.         Given a series of binary compounds or a series of specific covalent bonds and the relevant electronegativities, you will be able to predict which would be most polar or to rank them in order of their polarity.

7.         For a given molecule or ion, you will be able to draw the Lewis structure representation (including all resonance structures). 

8.         Given a set of correct Lewis structures for a molecule or polyatomic ion, you will be able to assign formal charges to all of the atoms and evaluate which of the structures best describe the bonding in that molecule or polyatomic ion.

9.         Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the electron-domain geometry (electron-pair geometry/VSEPR classification) for the molecule or polyatomic ion. 

10.       Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the molecular structure (or geometry) of that molecule or ion based on the VSEPR model.

11.       For a given molecular structure of a molecule or polyatomic ion, you will be able to represent the bond dipoles and tell if the species is polar or non-polar.

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

 

UNIT 4

 

                                                             STOICHIOMETRY

 

Reading:  Chapter 3

 

Homework:     3.1, 3.11, 3.13, 3.19, 3.21, 3.23 (a,d), 3.25a, 3.31, 3.33, 3.35, 3.37, 3.39, 3.43, 3.45, 3.49, 3.51, 3.53, 3.61, 3.63, 3.65, 3.67 (a,b), 3.73, 3.75, 3.77, 3.81, 3.101

 

1.         Define and/or recognize an acceptable definition or example of the terms listed in the "Summary and Key Terms" section at the end of the chapter.

 

2.         Given a chemical equation with all of the formulas correct, you will be able to properly balance that equation.

 

3.         Given the formula of a compound, you will be able to calculate its formula mass or molar mass.

 

4.         Given a periodic table and the formula of a substance or given the necessary mass data, you will be able to calculate the percent composition of that substance.

 

5.         Given the periodic table and the formula of a substance, you will be able to interconvert between the mass, the number of moles, the number of molecules or atoms of that substance, or the number of moles or atoms of an element within a compound.

 

6.         Given the percent composition or molecular formula of a compound determine its empirical formula; given mass data obtained by quantitative analysis calculate empirical formulas; given the formula mass and empirical formula of a compound determine its molecular formula.

 

7.         You will be able to work the following types of stoichiometry problems:  mass-mass; mass-moles; moles-moles; moles-formula units; mass-formula units.

 

8.         Given a balanced equation and mass data for a specified reaction, you will be able to determine the limiting reactant in that reaction, calculate the maximum (theoretical) yield, and calculate the percent yield of that reaction given the mass of product actually obtained.

 

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

 

 

UNIT 5

 

                          REACTION TYPES AND SOLUTION STOICHIOMETRY

 

Reading:  Chapter 4

 

Homework:     4.1, 4.2, 4.5, 4.7, 4.11, 4.13, 4.16, 4.19, 4.21, 4.22, 4.23, 4.26,4.30, 4.31, 4.35, 4.37, 4.39, 4.41, 4.43, 4.45, 4.49, 4.50, 4.51, 4.61, 4.63, 4.65, 4.67, 4.69, 4.71, 4.73, 4.75, 4.77 4.79, 4.81, 4.83, 4.85, 4.92, 4.95, 4.107

 

 

1.         Define and/or recognize an acceptable definition or example of the terms listed in the "Summary and Key Terms" section at the end of the chapter.

 

2.         You will be able to explain and/or illustrate the basis of the strong interaction between two water molecules or between a water molecule and an ion.

 

3.         Given the reactants side of an equation representing a metathesis reaction, you will be able to predict the correct formulas of the products and their physical states.

 

4.         Given a balanced molecular equation for a metathesis reaction and the physical states of all the components, you will be able to write complete ionic and net ionic equations for that reaction.

 

5.         You will be able to list the seven strong acids and eight strong bases by name and formula.

 

6.         You will be able to write a balanced neutralization reaction for a specified acid and base.

 

7.         Given a set of oxidation number rules, you will be able to determine oxidation numbers of elements and identify whether an element was oxidized or reduced in a reaction and whether it was an oxidant (oxidizing agent) or reductant (reducing agent) in the reaction.

 

8.         Given a balanced molecular equation for the oxidation of a metal by an acid or a salt of another metal, you will be able to write the total ionic and net ionic equations for the reaction.

 

9.         Given the molarity of a specified solution, you will be able to determine the volume of solution required to obtain a certain mass or number of moles of solute or a specified ion.

 

10.       Given the molarity of a solution to be prepared or the molarity of a specified ion, you will be able to determine the mass of a solid solute needed to prepare a specified volume of the appropriate solution.  You will be able to describe how to prepare a specified volume of a solution with a specified molarity of solute or ion.

 

11.       You will be able to calculate the molarity of a solution given the volume of the solution and the mass or the number of moles of the solute in the solution.

 

12.       Given the appropriate information, you will be able to calculate the concentration of a solution prepared by diluting a specified volume of a stock solution.

 

13.       Given the appropriate information, you will be able to calculate the volume of a stock solution that is needed to prepare a specified volume of a more dilute solution.  You will be able to determine the volume of water needed to make the solution.

 

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

 

15.       Given the concentration of a standard solution and a balanced equation representing a neutralization reaction, you will be able to determine the concentration of an acid or base of unknown concentration.

 

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

 

 

                                                                             


 

UNIT 6

 

     GASES, PHASE CHANGES, AND INTRODUCTION TO THERMOCHEMISTRY

 

Reading:  Chapter 10

Homework:     10.2, 10.21, 10.28, 10.30, 10.35, 10.36, 10.39, 10.41, 10.42, 10.45, 10.49, 10.51, 10.53, 10.57, 10.59, 10.65, 10.69, 10.71, 10.75, 10.93, 10.121 (a), 10.129

 

Reading:  Chapter 5 (p. 159 – 176)

Homework:     5.4, 5.27, 5.39a, 5.43a-c, 5.46 a-b, 5.47a-b, 5.51a-d, 5.53a

 

Reading:  Chapter 11 (11.4, 11.6)

Homework:     11.39, 11.43, 11.45, 11.46, 11.59

 

1.                  Define and/or recognize an acceptable definition or example of the terms listed in the "Summary and Key Terms" section at the end of Chapter 10 as well as the definition of a real gas. 

 

2.                  You will be able to write the correct symbols for the following units of pressure and to use dimensional analysis to convert between any two of them:  atmosphere, millimeter of mercury, inches of mercury, pounds per square inch, torr, pascal, kilopascal, bar, and millibar.

 

3.                  You will be able to identify the SI unit of pressure and define it in terms of fundamental SI units.

 

4.                  Be able to state or recognize statements given in either words or as mathematical expressions for each of the following relationships:

 

·         Pressure-Volume Law (Boyle's Law)

·         Temperature-Volume Law (Charles's Law)

·         Avogadro's Hypothesis and Avogadro’s Law

·         Dalton's Law of Partial Pressures

·         Graham's Law of Gas Effusion

 

5.                  Given values of the universal gas constant and three of the four variables (P, V, T, n) in the Ideal Gas Law equation, you will be able to calculate the value of the unknown parameter.

 

6.                  You will be able to state the values for "standard temperature and pressure" (or STP) and for "standard molar volume."

 

7.                  You will be able to determine the new pressure, new temperature, or new volume of a sample of gas in which there are changes in the other variables.

 

8.                  Given the necessary ideal gas data, you will be able to calculate the molar mass or density of a gas.

 

9.                  You will be able to use the Ideal Gas Law equation to carry out stoichiometric calculations for reactions involving gases when you are given reactions and necessary data.

 

10.              You will be able to calculate the mole fraction of a component present in a mixture of gases and calculate the partial pressure of that component when given the total pressure.  You will be able to find the partial pressure of a gas collected over water.

 

11.              You will be able to state or recognize statements describing the postulates of the kinetic molecular theory of gases.

 

12.              You will be able to state or recognize conditions under which real gases depart from ideal behavior and state or recognize the reasons for non-ideal behavior.

 

13.              You will be able to define or recognize an acceptable definition or example of each of the following:  freezing, boiling, fusion, melting, sublimation, deposition, vaporization, condensation, boiling point, normal boiling point, melting point, normal melting point, triple point, critical temperature, critical pressure, critical point, heat, work, internal energy, kinetic energy, potential energy, specific heat, endothermic, exothermic, heat of fusion, and heat of vaporization.

 

14.              Given the amount of heat gained or lost by a system and the amount of work done on or by the system, you will be able to calculate the change in internal energy of the system.

 

15.              You will be able to identify a specified physical change of state as being either endothermic or exothermic.

 

16.              Given appropriate relationships, you will be able to use dimensional analysis to convert between any two appropriate units for heat.

 

17.              Given any three of the following: heat, mass, temperature change, or specific heat, you will be able to calculate the fourth quantity. 

 

18.              Given the heat of fusion or heat of vaporization of a substance and the mass or number of moles of that substance, you will be able to calculate the amount of heat gained or lost.

 

19.              Given a thermochemical equation, you will be able to calculate the enthalpy change for a reaction involving a given number of moles or grams of a reactant or product. Given a thermochemical equation, you will be able to determine the enthalpy change for the reverse reaction.

 

20.              You will be able to explain the various segments of a heating/cooling curve.  You will be able to explain the impact that intermolecular forces have during the phase changes that occur.  Given the heat of fusion, heat of vaporization, and specific heat of a substance, you will be able to calculate the heat necessary to completely convert a given mass of the substance from one temperature and physical state to another.

 

21.              You will be able to use a phase diagram to determine the state (phase) of a substance given its temperature and pressure.  You will be able to state which phases are in equilibrium on the boundary lines on a phase diagram.  You will be able to locate the triple point of a substance on a phase diagram and identify the equilibrium it defines.  Given a phase diagram, you will be able to describe the phase changes in a substance as its temperature is changed at constant pressure or as its pressure is changed at constant temperature.

 

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

 

 

 

CHEM 1115

Objectives for Comprehensive Final Exam

 

 

1.      Given the name of a chemical element, you will be able to write its symbol.  Given the symbol of an element, you will be able to write its name.  You will be responsible for the elements given in objective 2 of unit 1.

2.      Given two of the three variables—density, mass, and volume—you will be able to calculate the third.

3.      You will be able to convert from one set of units to another set of units using dimensional analysis.  You will be able to state or use the metric-metric conversions for mega, kilo, centi, milli, and micro.

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

a.       Metal, nonmetal, or metalloid

b.      Alkali metal, alkaline earth metal, halogen, or noble gas

c.       Main group, transition metal, lanthanide or actinide

5.      You will be able to list the elements that occur naturally as diatomic molecules.

6.      Given the name of a common ion, you will be able to write its symbol including the correct charge.  Given the symbol of a common ion, you will be able to write its name.  You are responsible for the common ions given in Objective 4 of Unit 2.

7.      Given the formulas of ionic compounds formed from the cations and anions described in the previous objective, you will be able to write the name of the compound.  Given the name of a compound formed from these ions, you will be able to write its chemical formula.

8.      Given the formula of a binary molecular compound, you will be able to write the name of the compound.  Given the name of such a compound, you will be able to write its formula.

9.      You will be able to write the electron configuration either in complete form or using core notation for any main group atom or ion.

10.  You will be able to recognize definitions or descriptions of the four quantum numbers used in the quantum mechanical model of the atom.  You will also be able to recognize allowed sets of quantum numbers. 

11.  You will be able to predict the relative size of the following:  any two atoms in the periodic table, two atoms/ions in an isoelectronic series, an ion and its parent atom, or two ions in the same group.

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

13.  Given the formula for a molecular compound or a polyatomic ion, you will be able to give the name of the electron domain geometry and the molecular geometry for that substance.

14.  Given the names and/or formulas of the reactants and products involved in a chemical reaction, you will be able to write a balanced chemical equation.

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

16.  Given the names and/or formulas of two reactants and the solubility guidelines, you will be able to write a balanced molecular equation, complete ionic equation, and net ionic equation for a precipitation or acid/base (neutralization) reaction.

17.  Given the appropriate information, you will be able to calculate the concentration of a solution prepared by diluting a specified volume of a stock solution.

18.  Given the appropriate information, you will be able to calculate the volume of a stock solution that is needed to prepare a specified volume of a more dilute solution.

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

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

21.  You will be able to recognize statements of the following gas laws either in words or as mathematical expressions:  Boyle’s Law, Charles Law, and Avogadro’s Law.

22.  You will be able to apply the previous gas laws to determine whether volume of a gas will increase, decrease, or stay the same when a specified change is made in the temperature, pressure, or number of moles of the sample of gas.

23.  Given values of the universal gas constant and three of the four variables (P, V, T, n) in the Ideal Gas Law equation, you will be able to calculate the value of the unknown parameter.

24.  You will be able to determine the new pressure, new temperature, or new volume of sample of gas in which there are changes in the other variables.

25.  Given any three of the following: heat, mass, temperature change, or specific heat, you will be able to calculate the fourth quantity.

26.  Given the heat of fusion or heat of vaporization of a substance and the mass or number of moles of that substance, you will be able to calculate the amount of heat gained or lost.

27.  You will be able to identify a specified physical change of state as being either endothermic or exothermic.

28.  Given a thermochemical equation, you will be able to calculate the enthalpy change for a reaction involving a given number of moles or grams of a reactant or product.  Given a thermochemical equation, you will be able to determine the enthalpy change for the reverse reaction.

29.  You will be able to use a phase diagram to determine the state (phase) of a substance given its temperature and pressure.  You will be able to state which phases are in equilibrium on the boundary lines on a phase diagram.  You will be able to locate the triple point of a substance on a phase diagram and identify the equilibrium it defines.  Given a phase diagram, you will be able to describe the phase changes in a substance as its temperature is changed at constant pressure, or as its pressure is changed at constant temperature.

 

 

Final Grade Calculations:

            Total points possible = 600 + 100 + 90 + 145 = 935 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”

 

Tests are 75% of your grade.  Quizzes and labs together represent 25% of your grade.

 

You should keep track of your grades throughout the semester, recording grades as papers are handed back to you.

 

Grade record:

 

Exam 1  _____

Lab 1    _____

Quiz 1  ____

Exam 2  _____

Lab 2    _____

Quiz 2  ____

Exam 3  _____

Lab 3    _____

Quiz 3  ____

Exam 4  _____

Lab 4    _____

Quiz 4  ____

Exam 5  _____

Lab 5    _____

Quiz 5  ____

Exam 6  _____

Lab 6    _____

Quiz 6  ____

Final*    _____

Lab 7    _____

 

 

Lab 8    _____

 

 

Lab 9    _____

 

 

Lab 10  _____

 

 

Lab 11  _____

 

 

Lab 12  _____

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

Total    ______

Total _____

Total _____    

 

 

 

 

Total of all points:   __________

 

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

 

Note:  You can get a pretty good idea of your standing in the class by looking at the average of your exams.  If your average is one or two points away from the next grade level, the points for the labs and quizzes could bring your final grade up to the next level.  For instance, if you have an 88 average on your exams, you can still get an “A” provided that you have most of the points for the labs and quizzes.  On the flip side, if you have done poorly on quizzes or a number of labs were late, your grade could potentially drop a letter grade.