COURSE: CHEM 1115, GENERAL CHEMISTRY I -2015 ... 1115 Syllabus...OCCC CHEM 1115 Syllabus COURSE:...

OCCC CHEM 1115 Syllabus

COURSE: CHEM 1115, GENERAL CHEMISTRY I

Oklahoma City Community College, 2014-2015 Academic Year

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 Modified 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 Modified

MasteringChemistry™ Student Access Kit). Brown, LeMay,

Bursten, Murphy, and Woodward. 2012. Pearson.

-- OR –

Chemistry: The Central Science 12th Edition eBook with

Modified MasteringChemistry™ Student Access Kit. Brown,

LeMay, Bursten, Murphy, and Woodward. 2012. Pearson.

The access kit is good for two years and can be used in CHEM

1215. If you purchased an access kit for Chem 1115

previously, you will need to contact your instructor to

exchange it for a new Modified MasteringChemistry™ code.

Lab Manual: Chemistry 1115/0110 General Chemistry I Laboratory Manual.

Oklahoma City Community College. 2014.

Goggles: Approved chemical splash goggles.

Calculator: Casio FX-260, TI 30XA, or TI 30X IIS non-programmable

scientific calculator (other models must be approved by your

instructor)

Optional Materials: Mega Molecules Molecular Geometry kit.

OCCC CHEM 1115 Syllabus 2014-2015 Academic Year

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COURSE DESCRIPTION

Prerequisite: (R), (W), MATH 1513 or MATH 1533 or both MATH 0403 and high school

chemistry or CHEM 1123. A grade of "C" or better is required in all prerequisite courses.

5 CREDITS. This course is designed for science and engineering majors. The course

covers nomenclature, atomic and molecular structure, stoichiometry, acid/base and other

aqueous reactions, states of matter, phase changes, gas laws, and an introduction to

thermochemistry. Laboratory is an integral part of the course. GenEd Requirement

COURSE COMPETENCIES

As stated in the course description, when you complete this course, you should be able to

apply the principles and theories of chemistry to interpret fundamental chemical

phenomena and predict the results of chemical reactions. You should be able to

demonstrate through tests, homework assignments, and laboratory exercises a basic

knowledge of the periodicity of the elements, inorganic nomenclature, stoichiometry,

metathesis reactions, redox reactions, properties of gases, atomic structure, and molecular

geometry. A list of specific learning objectives relating to these general competencies is

attached.

ATTENDANCE

Oklahoma City Community College requires regular class attendance and punctuality of

students.

EMAIL

Your OCCC email account (it has the form [email protected]) is

your official school email account. You will be held responsible for any course

information that comes to you via OCCC email, so be sure to check it regularly throughout

the semester.

WITHDRAWING FROM CLASS:

It is your responsibility to withdraw from the course if you cannot complete the course.

Your professor cannot withdraw you for non-attendance. You can withdraw until the end

of the twelfth week during the Fall and Spring semesters or until the end of the sixth week

in the Summer semester.

ACCOMMODATIONS FOR STUDENTS WITH SPECIAL NEEDS:

Oklahoma City Community College complies with Section 504 of the Rehabilitation Act &

the Americans with Disabilities Act. Students with disabilities who seek academic

adjustments/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

mailto:[email protected]


p. 3

calling 405-682-7520. All academic adjustments/accommodations must be approved by

Student Support Services.

If you have been approved by Student Support Services to receive academic

adjustments/accommodations you must talk with me either after class or during my office

hours. This will allow me to be better informed on how to assist you with access during the

semester. To respect your privacy I will not approach you, but the academic

adjustments/accommodations must be discussed to ensure ideal implementation for you.

All information will remain confidential.

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


p. 4

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 crew-neck 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.

Unit Exams – 6 x 100 pts = 600 pts

Six unit exams worth 100 points each will be given during the semester. You are expected

to take all exams in class. If you have an accommodation from Student Support Services

that allows you to take exams in the Test Center, you are expected to take exams at the

same time as all other students unless alternative arrangements are approved by your

instructor before the test date.

Late Exam Policy: 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.

Retest Policy: 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. All work, including make-up

exams and retests, must be completed by the end of the semester.


p. 5

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, you 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

your overall course grade. See the “Grading Scale” section for details.

Quizzes – 6 x 15 pts = 90 pts

Six online quizzes worth 15 points each will be given throughout the semester. Each quiz

will be accessed online using Modified MasteringChemistry. You will typically have about

ten days to access and complete each quiz. All answers must be submitted electronically.

You are encouraged to ask your instructor for help with online quiz questions if needed.

Due dates for the quizzes are specified in your lecture schedule. No late quizzes will be

accepted. A score of zero will be recorded for any missed quiz.

Computer access for MasteringChemistry online quizzes: Since each quiz is open for

several days, technical problems, including those discovered on the due date of a quiz,

are not considered a valid 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 Modified MasteringChemistry, you do not have to access it

with your own computer. Any computer with Internet access, including the ones in the

Physical Science Center (or any student accessible computer on campus), may be used to

access and complete your MasteringChemistry assignment.

Lab Exercises 12 x 8 pts = 96 pts

You are expected to complete 12 lab exercises worth 8 points each during the semester.

Your 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 will have the opportunity to make up one lab exercise during the make-up week at the

end of the semester. Although only 10 labs are required to pass the course, we strongly

advise you to complete all 12 labs and reports. Please understand that the lab portion of

your grade consists of 96 points. If you choose not to make up a lab, that lab grade will

be a zero.


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Labs are due at the start of the following pre-lab period. Late labs – this includes

makeup labs - will be assessed a four 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 - 4 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 + 96 = 886 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 886 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 886 points

possible but scores a 54.5% on the comprehensive final exam will receive a “D” in the

course.

Grade % of Available

Points (886 pts)

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


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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. An approved scientific calculator such as the Casio FX-260, TI

30XA, or TI 30X IIS is all you need/will be allowed.

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 (late) 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.


p. 8

SAFETY AND SECURITY EMERGENCY PROCEDURES

The health and safety of all our students, faculty, and staff are OCCC's prime concern. The

procedures outlined below are designed to deal with emergencies of various types.

Students should always follow the lead of their instructors.

Fire

First notification will come from the fire alarm horns, sirens, and strobes. The class should

gather their belongings, exit the building using the nearest exit, and move to a parking lot.

Do not use the elevators. No alarm should be treated as a false alarm. Horns, sirens, and

strobes are only used for fire alarms.

Fire (Special Considerations)

If someone in your area is not physically capable of descending the stairwell, please ensure

that they remain in the "area of safe refuge" located just inside each upper-level enclosed

fire stairwell. There are emergency phones located near each of these areas.

Medical

For all medical related issues push the "emergency" button located on each classroom

phone. The phone will display your room number, allowing for fast response to your

location. All security officers are trained as first responders and will assist in guiding

EMSA to your location. Treat all bodily fluids as if they were contaminated.

Bomb If you receive a bomb threat, document as much information as possible and push the

"emergency" button on the phone. If the decision to evacuate is given, the phone will

sound an alarm and display a text message. The class should gather their belongings, exit

the building using the nearest exit, and move to an open grassy area. Please turn off all

wireless devices. (Cell phones, radios, laptops, and other portable devices.)

Weather

Tornado warnings that include OCCC will be sent directly to the classroom phone. The

phone will sound an alarm and display a text message. The class should gather their

belongings, move away from exterior glass and exits, and move to safer areas. These areas

are lower-level interior classrooms, restrooms, and stairwells. You should familiarize

yourself with the safer areas near your classroom(s). If the city/county sirens are sounding

and OCCC is not in the warning area a message will be sent to the classroom phone

advising this information.

Disturbance/Threats

If someone is causing a disturbance in a classroom call security immediately. Push the

"emergency" button located on each classroom phone. Distance yourself from that person,

do not place yourself in the person's exit path and remove all potential weapons from the

area. Shelter in place: If there is an armed person or shooter on campus: Close and lock

your hallway doors. Turn off the lights, shut the blinds or move away from exposed areas.

Use desks, tables and other objects to provide protection. Updated information will be sent

to the classroom phone.


p. 9

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 Molybdenum Mo

Bromine Br Neon Ne

Cadmium Cd Nickel Ni

Calcium Ca Nitrogen N

Carbon C Oxygen O

Cesium Cs Phosphorus P

Chlorine Cl Platinum Pt

Chromium Cr Potassium K

Cobalt Co Radon Rn

Copper Cu Silicon Si

Fluorine F Silver Ag

Gold Au Sodium Na

Helium He Sulfur S

Hydrogen H Tin Sn

Iodine I Uranium U

Iron Fe Zinc Zn


p. 10

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 (scientific) 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 number in decimal notation, you will be able to write it in proper exponential

(scientific) notation. Given a number in exponential (scientific) notation, you will be

able to write it in decimal notation.

8. 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, micro, and nano. You will be able

to state or use the relationship between milliliters and cubic centimeters.

9. 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.

10. 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 by name and formula the elements that occur naturally as diatomic molecules.

11. 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.

12. Given a list of chemical properties, you will be able to indicate which are properties of

metals and which are properties of nonmetals.


p. 11

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


"Summary and Key Terms" sections at the end of Chapter 2, Chapter 6, and Chapter 7

(Sections 7.1-7.6 only).

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

and the Law of Constant Composition.

3. Given some combination of the number of protons, the number of neutrons, the number

of electrons, the isotopic mass, and the complete isotopic symbol for some isotope, you

will be able to supply the missing component(s) of the above list for that isotope.

(Unit 2 objectives continued on next page.)


p. 12

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 CO3

2

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


p. 13

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.


p. 14

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

the name of the compound; given the name of a compound formed between two

nonmetals, you will be able to write the formula.

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

chemical formula of an acid, you will be able to write its name.

4. Given the name of one of the following household products, you will be able to write the

name or formula of the chemical present in it: water, ammonia, natural gas, vinegar,

hydrogen peroxide, drinking alcohol, rubbing alcohol, and nail polish remover.

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

(Lewis) symbol.

6. Given a series of binary compounds or a series of specific covalent bonds and the

relevant electronegativities, you will be able to predict which would be most polar or to

rank them in order of their polarity.

7. For a given molecule or ion, you will be able to draw the Lewis structure representation

(including all resonance structures).

8. Given a set of correct Lewis structures for a molecule or polyatomic ion, you will be able

to assign formal charges to all of the atoms and evaluate which of the structures best

describe the bonding in that molecule or polyatomic ion.

9. Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the

electron-domain geometry (electron-pair geometry/VSEPR classification) for the

molecule or polyatomic ion.

10. Given a formula of a molecule or polyatomic ion, you will be able to name and sketch the

molecular structure (or geometry) of that molecule or ion based on the VSEPR model.

11. For a given molecular structure of a molecule or polyatomic ion, you will be able to

represent the bond dipoles and tell if the species is polar or non-polar.

12. You will be able to answer questions or solve problems relating to previous units. You

will be able to answer questions and solve problems incorporating material from past

units with the current unit objectives.


p. 15

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



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

balance that equation.

3. Given the name of a metal or the formula of an organic compound containing carbon,

hydrogen, and/or oxygen, you will be able to identify the co-reactant required and the

product(s) formed by the complete combustion of the substance. You will be able to

write a balanced equation for the complete combustion of the substance.

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

mass.

5. 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.

6. 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.

7. 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.

8. You will be able to work the following types of stoichiometry problems: mass-mass;

mass-moles; moles-moles; moles-formula units; mass-formula units.

9. 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.





p. 16

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



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 the equation for a neutralization reaction, you will be able to identify the acid and

the base.

8. 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.

9. 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.

10. 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.

11. 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.


p. 17

12. 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.

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. You will

be able to determine the volume of water needed to make the 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 names or formulas of the reactants involved in a precipitation reaction or a

neutralization reaction, you will be able to work the following types of stoichiometry

problems: mass-volume, volume-volume, mass-concentration, and volume-

concentration.

17. 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.




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


"Summary and Key Terms" section at the end of Chapter 10 as well as the definition of a

real gas.


p. 18

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,


p. 19

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. Given a thermochemical equation, you will be able to identify the reaction as either

endothermic or exothermic.

21. 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.

22. 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.

23. Given a phase diagram labeled with points representing various temperature/pressure

combinations, you will be able to identify points that correspond to the triple point, critical

point, boiling point, melting point, and/or sublimation point. You will be able identify the

equilibrium involved for each of these points (with the exception of the critical point).

24. Given a phase diagram, you will be able to describe the phase changes in a substance as its

temperature is changed at constant pressure, or as its pressure is changed at constant

temperature.


p. 20





p. 21

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, micro, and nano. You will be able to state or use the relationship between milliliters

and cubic centimeters.

4. Given a number expressed as a decimal or in exponential (scientific) 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.

5. Given a number in decimal notation, you will be able to write it in proper exponential

(scientific) notation. Given a number in exponential (scientific) notation, you will be able to

write it in decimal notation.

6. 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

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

8. 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.

9. 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.

10. 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.

11. 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.

12. Given some combination of the number of protons, the number of neutrons, the number of

electrons, the isotopic mass (mass number), and the complete isotopic (nuclear) symbol for

an isotope, you will be able to supply the missing component(s) of the above list for that

isotope.


p. 22

13. You will be able to write the electron configuration either in complete form or using core

notation for any main group atom or ion.

14. 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.

15. 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.

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.

You will be able to draw a 3-dimensional structure for the electron domain geometry and the

molecular geometry for the substance.

18. 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.

19. Given the name or chemical formula of a substance, you will be able to calculate the percent

composition of that substance.

20. Given the name or formula of a substance, you will be able to interconvert between the mass,

the number of moles, the number of atoms or molecules of that substance or the number of

moles or atoms of an element within a compound.

21. Given a balanced chemical equation, you will be able to work the following types of

stoichiometry problems: mass-mass, mass-moles, moles-moles, mass-volume, and volume-

volume.

22. Given the names or formulas for the reactants in a precipitation or neutralization reaction,

you will be able to work the following types of stoichiometry problems: mass-mass, mass-

moles, moles-moles, mass-volume, and volume-volume.

23. 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.

24. Given the balanced molecular equation for a precipitation, neutralization, or oxidation-

reduction reaction, you will be able to write the balanced total (complete) ionic or net ionic

equation for the reaction.

25. Given the equation for a neutralization reaction, you will be able to identify the acid and the

base.

26. Given a set of oxidation number rules, you will be able to determine oxidation numbers of a

specified element in a substance. You will be able to identify the element oxidized and the

element reduced in a redox reaction.

27. 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.


p. 23

28. 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.

29. Given the appropriate information, you will be able to describe the steps required to prepare a

specified solution by diluting a stock solution.

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

solution.

31. 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.

32. 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.

33. 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.

34. 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.

35. 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.

36. 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.

37. Given any three of the following: heat, mass, temperature change, or specific heat, you will be

able to calculate the fourth quantity.

38. 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.

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

exothermic.

40. 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.

41. Given a thermochemical equation, you will be able to identify the reaction as either endothermic

or exothermic.

42. 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.

43. Given a phase diagram labeled with points representing various temperature/pressure

combinations, you will be able to identify points that correspond to the triple point, critical

point, boiling point, melting point, and/or sublimation point. You will be able identify the

equilibrium involved for each of these points (with the exception of the critical point).

44. Given a phase diagram, you will be able to describe the phase changes in a substance as its

temperature is changed at constant pressure, or as its pressure is changed at constant

temperature.


p. 24

Final Grade Calculations: Total points possible = 600 + 100 + 90 + 96 = 886 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 79% of your grade. Quizzes and labs together represent 21% 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.

COURSE: CHEM 1115, GENERAL CHEMISTRY I -2015 ... 1115 Syllabus...OCCC CHEM 1115 Syllabus COURSE:...

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