General Chemistry I Syllabus - Oakton Community College



Oakton Community College

General Chemistry I Syllabus

31220 – CHM 121 – 007

Fall 2008

Instructor: Elizabeth Kershisnik

Office: B214 (RHC)

Email: ekershis@oakton.edu

Voicemail: 847-376-7802

Lecture Meeting Times: 12:30 pm - 1:45 pm TR A212 (RHC)

Lab Meeting Times: 2:00 pm - 4:45 pm T A242 (RHC)

Office Hours: 11:00 am - 12:30 pm T

5:00 pm – 5:30 pm T

11:00 am - 12:30 pm R

2:00 pm – 5:30 pm R

6:45 pm – 7:30 pm R

I. Course Course Course

Prefix Number Section Course Name Credit Lecture Lab

CHM 121 007 General College Chemistry I 4 3 3

II. Prerequisites:

MAT 120 with minimum grade of C, and one year of high school chemistry or CHM 101 or CHM 105 with minimum grade of C, or consent of instructor. MAT 140, or MAT 149, is recommended.

III. Course (Catalog) Description

Course is first of two semester sequence (CHM 121 and CHM122). Content includes the periodic table of elements, atomic structure, basic concepts of quantum theory, stoichiometry of compounds and reactions, thermochemistry, molecular structure, bonding, intermolecular interactions, the gaseous state, and solutions. Weekly hands-on lab activities. Intended for students enrolled in science and/or pre-professional curricula.

IV. Learning Objectives

A. General Education Objectives. After successful completion of this course, students will have

practiced and enhanced their ability to do the following.

1. Define problems.

2. Construct hypothesis.

3. Gather, analyze, and interpret data and/or information.

4. Place basic chemical concepts and models within a historical framework.

5. Differentiate between observation and interpretation (fact and opinion).

6. Compare and evaluate alternative solutions.

7. Communicate findings effectively in writing and speech.

8. Work effectively with people from diverse backgrounds, individually and in teams.

B. Chemistry Specific Objectives. After successful completion of this course, students will have

developed their ability to do the following at an acceptable level.

1. Describe the differences between a mixture and a substance, and between a compound and an element in terms

of macroscopic and nanoscopic properties.

2. Describe qualitatively how distance and charge affect the electrostatic force between charged particles

3. Describe the current basic model of an atom (and its history), including the nature and location of its components

and the energy-level/orbital model of electronic structure; describe the nuclear composition and electron

distribution in any atom or monatomic ion.

4. Use the periodic table and model of electronic structure to identify/explain properties of elements (and trends of

such) and predict the nature of compounds formed from two elements.

5. Describe the bonding in molecular and ionic compounds; draw Lewis structures of simple molecules and ions,

including resonance structures and formal charges; predict the geometry around centers in molecules and ions

using Valence Shell Electron Repulsion Theory, and describe the atomic and hybrid orbitals used in σ and π

bonding using Valence Bond Theory.; predict (if given electronegativity values) whether bonds are nonpolar or

polar (or ionic), and whether molecules are polar or nonpolar.

6. State the meaning of a chemical formula of any compound; calculate atomic and molar mass of a compound, as

well as the mass percent of elements in a compound, from its formula.

7. Calculate the mass percent of elements in a compound and the empirical formula (and molecular formula) of a

compound, if given experimental mass data (and molecular weight).

8. Write the formula of an ionic compound, acid, or binary molecular compound, if given its name; name an ionic

compound, acid, or binary molecular compound if given its formula.

9. Understand the meaning of the symbols in a chemical equation, and distinguish between a chemical equation and

chemical reaction; balance/write molecular and net ionic equations, applying solubility rules as needed.

10. Safely demonstrate basic laboratory skills including gas collection, filtration, observation/testing of properties of

various unknowns, and use of a Bunsen burner, high-precision balances, and other basic equipment.

11. Perform routine laboratory measurements including mass, volume, and temperature, and record them with proper

indication of precision/uncertainty and units; distinguish between measured and calculated quantities, and

between variables and constants, and report calculated quantities with proper indication of precision/uncertainty.

12. Use and understand chemical terminology, especially with respect to nanoscopic amounts (and types) of

chemical entities (e.g., formula units, molecules, atoms, ions) and macroscopic amounts of chemical entities

(e.g., moles). Understand the meaning of and distinction between “atomic/molecular mass” (in amus) and

“molar mass” (in grams).

13. Construct and/or use conversion factors (dimensional analysis) as needed in calculations to properly relate or

determine quantities; be able to use scientific notation in calculations as needed.

14. Use a balanced equation representing a certain reaction to predict how much of a certain reactant is required to

combine with another, or how much product can form (theoretical yield) from a specific combination of reactants

(with a limiting reactant); distinguish actual and theoretical yields, and determine percent yield

15. Determine the amount of heat produced (absorbed) when a given amount of reactant reacts, if given the

appropriate enthalpy values and balanced equation; calculate the temperature change associated with a certain

heat flow if given the appropriate specific heats or heat capacities (and vice versa); understand the concept of

state function and be able to do Hess's Law type calculations/problems.

16. Know (and understand the meaning of the variables in) the simple gas laws, and use them to

calculate/predict/estimate the value (or factor of change in value) of any (appropriate) variable if given a

sufficient amount of information pertaining to the other (appropriate) variables.

17. Understand and be able to apply the kinetic molecular theory to explain the relationship between any two of the

following gas properties: P, V, n, T if the others are held constant; understand how to interpret velocity and

kinetic energy distribution curves; understand the concept of gas mixtures and partial pressures; state how

density, velocity, and concentration of a gas vary with P, V, n, and T changes (and gas identity).

18. Describe the behavior of molecules in a gas, liquid, or solid in terms of kinetic molecular theory, including the

role of temperature and intermolecular forces of attraction; understand the different kinds of intermolecular

forces of attraction, and use them to predict relative values of substances' melting and boiling points, vapor

pressures, and enthalpies of melting and vaporization; understand how properties of ionic and covalent network

solids are related to the interactions/forces between their basic units (ions or atoms).

19. Distinguish the nature of solutions of molecular vs. ionic compounds; find the molarity, molality, weight percent,

parts per million (billion, etc.), or mole fraction of a solute in a described solution; be able to prepare a

designated volume of a solution with a specified concentration; use polarity ideas to predict solubility of

molecular substances in liquids; describe "colligative properties" and predict which solution has the greater

boiling point, freezing point, etc.

20. Draw meaningful depictions of small molecules, formula units of an ionic compound, or ions in solution if given

their chemical formula; use these to help describe/illustrate how chemical reaction involves rearrangement of

atoms or ions.

Academic Integrity

Students and employees at Oakton Community College are required to demonstrate academic integrity and follow Oakton’s Code of Academic Conduct. This code prohibits:

• cheating,

• plagiarism (turning in work not written by you, or lacking proper citation),

• falsification and fabrication (lying or distorting the truth),

• helping others to cheat,

• unauthorized changes on official documents,

• pretending to be someone else or having someone else pretend to be you,

• making or accepting bribes, special favors, or threats, and

• any other behavior that violates academic integrity.

There are serious consequences to violations of the academic integrity policy. Oakton’s policies and procedures provide students a fair hearing if a complaint is made against you. If you are found to have violated the policy, the minimum penalty is failure on the assignment and, a disciplinary record will be established and kept on file in the office of the Vice President for Student Affairs for a period of 3 years.

Details of the Code of Academic Conduct can be found in the Student Handbook.

VI. Instructional Materials

Textbook (required) Chemistry, 7th edition, Zumdahl and Zumdahl

(optional) Student Solutions Manual

Eduspace®

Calculator (required) Bring to class.

TI-30X, TI-36X or equivalent

Laboratory Manual (required) Chemistry 121 Lab Manual, Oakton Community College,

Slowinski,

Wolsey, and Masterson

Safety Goggles (required) Must be worn in lab at all times. NO EXCEPTIONS.

Must meet following criteria:

• Fit snuggly against the forehead & face, protecting against splashes

• Be impact resistant; ANSI rating of Z87 or higher

• Include only indirect venting

Can be purchased in the bookstore

VII. Evaluations

Grading:

Based on the following:

• Participation

• Homework

• Quizzes

• Laboratory Reports

| |Point Breakdown |Points |Percentage |

|Participation |3/class, 10/final evaluation day* |100 |10.5% |

|Homework |11 x 10 |110 |11.6% |

|Quizzes |8 x 50 |400 |42.1% |

|Final Exam |1 x 160 |160 |16.8% |

|Lab Reports |Best 12 of 14 x 15 |180 |18.9% |

| | | | |

|Totals | |950 |100% |

* Each class is worth a minimum of 1 point up to a maximum of 3 points. 1 point is awarded for the

student attending class for the entire scheduled time. Up to 3 points is awarded if the student

participates in class i.e. asks questions, answers instructor’s questions, adds constructive comments

during class etc. 10 points will be awarded to each student that takes the final exam during the

scheduled evaluation day.

|Grade |Total Points |Percentage |

|A |855 – 950 |90 - 100% |

|B |760 – 854 |80 - 89% |

|C |665 – 759 |70 - 79% |

|D |570 – 664 |60 – 69% |

|F |0 - 569 |0 – 59% |

I/W: These grades will not be assigned except in special cases. You are responsible for withdrawing from the class. The instructor will not accept assignments after the semester is completed.

Late Work:

Assignments not turned in at the designated time will be penalized 20% for each class session it is late. An assignment will not be accepted more than two class sessions after its due date.

Quizzes:

Quizzes will be administered at the start of class. No make-up quizzes will be offered. If you know

ahead of time that you will miss a quiz and have a valid excuse, I will schedule the quiz to be taken at

the Assessment Center before the regularly scheduled quiz.

Make-up Labs:

It is in your best interest to attend labs. No labs can be made up but only 12 of the 14 labs will be used toward the final grade. If all 14 labs are attended and write-ups for all 14 submitted, the lowest two lab reports will be dropped.

Lab Reports:

The report should be two typed pages maximum.

Lab manual pages with raw data and questions should be stapled to the lab report and filled out in INK. Any errors should be lined out (one single line) and initialed.

The reports will be graded on neatness, accuracy of experimental data, and completeness.

Each student will be responsible for his/her own lab report even if the experiment was done in pairs.

Each advanced study lab assignment is due at the beginning of the lab period and is worth 2 points.

Lab Report Format:

Your Name

(1 Point) Experiment Number and Name

Date

Purpose: (2 Point)

A short explanation of the principles being investigated (one to two sentences).

Procedure: (3 Points)

Describe in your own words how YOU performed the experiment (mistakes and all).

This can be in a paragraph or in bullet format. Do not write out the procedure from the

lab manual.

Data, Calculations, Questions, Practice calculations, etc.: (4 points)

The filled in lab manual pages (in ink), graphs, etc.. Staple to the lab report in order.

Conclusion: (3 Points)

Summary of concepts covered in lab, what was learned, known errors and how they could be corrected, modifications to procedures to improve lab outcome, data trends/comparisons, etc.

VII. Other Course Information

Attendance:

Prompt and regular attendance is expected. You will be responsible for filling out and turning in at the

end of lecture class a participation slip. Slips not turned in at the end of class will not be counted and

participation points will be deducted. Consistent tardiness (late 3 or more times) or leaving early will

result in loss of participation points for that class.

Electronic Devices:

Cell phones, PDAs, IPods, etc. must be turned off and stored away during class and lab.

Instructional Method:

It is in the student’s best interest to read the assigned chapter(s) prior to coming to class.

Lectures are meant to be interactive and I can better aid in your instruction if you are prepared and have

questions.

Study recommendations:

• Read the assigned chapters from the textbook prior to class

• Read the assigned experiment prior to lab.

• Take extra notes in class

• Participate in class discussions and ask questions if you are unclear on a concept

• Seek out the instructor if in need of additional instruction

• Complete the scheduled quizzes and exams

• Complete the assigned lab activities

• Complete the assigned homework sets

If a student suspects she is pregnant, she should consult her physician before participating in a chemistry lab.

If you have a documented learning, psychological, or physical disability, you may be entitled to reasonable academic accommodations or services. To request accommodations of services, contact the ASSIST office in Instructional Support Services. All students are expected to fulfill essential course requirements. The College will not waive any essential skills or requirements of a course or degree program.

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