Subject: Syllabus for Chemistry 3A
From: <Saved by Windows Internet Explorer 7>
Date: Thu, 13 Aug 2009 11:21:14 -0700

CHEM 3A: Introductory General Chemistry

Fall 2009 Section 57421

Lecture MWF (9:00-9:50) in PHY 82

Lab T (11:00-1:50) in PHY 82

Instructor:      Veronica Cornel

Contact info:   e-mail [email-masked] using “Chem3A” in subject line, or 638-3641 ext 3449

Webpage:       http://blackboard2.fresnocitycollege.edu/

Office Hours:    PHY 78 (MWF) 10-11

Course Objectives: Chemistry 3A is an elementary survey course in chemistry including lab work. It is designed to give the student a chemistry background for a wide variety of careers including forestry, nutrition, nursing, physical therapy, teaching and other biological and health related fields.

Course Advisories: CHEM 10 or high school chemistry, MATH 103, and eligibility for ENGL 125. Many students try and do CHEM3A without any prior chemistry. It is possible, but it takes a lot of hard work. They need to start seeing a tutor right from the beginning. Students will need to be familiar with basic algebra before taking this course as there is a lot of math involved.

Text and Materials:

1.      Nivaldo J. Tro: “Introductory Chemistry” 3rd Ed.

2.      “Chemistry Labs”, Cengage publishers customized lab book (Weiner and Peters, Introduction to Chemical Principles, A Laboratory Approach, 6th Ed. can still be used but 4 new labs in bold will have to be photocopied)

You will need safety glasses ($5 at hardware store), materials to take notes and a calculator with “exp” (or “EE”) and “log” keys ($12 at Walmart).

Lecture Notes: The ability to listen carefully and to take good lecture notes in an essential college skill. Students should print out the fill-in notes and homework assignments off my Blackboard website prior to coming to class. Studies have shown that 90% of the lecture material is retained if you review the lecture within 24 hours after class. If you wait a week you will only retain 35%.

Laboratory Work: Lab work will follow as closely as possible the material discussed in the lectures. The student is required to complete all the assigned experiments. 50% of the final lab grade will include the average of the graded lab report sheets, the efforts to reach the goal of the experiments, the accuracy of measurements and calculations, and the lab technique shown during the experiments.  The other 50% of your lab grade is determined by the average of the lab quizzes. Please refer to the lab schedule. If you know you need to miss a lab, attend another lab on Monday or Wednesday afternoon or Wed evening the same week, or make an arrangement with your lab instructor to make up the lab the following Friday. Points will be deducted for the instructor having to do a make-up lab for you.  No make up labs will be allowed after the week they were assigned as the chemicals and equipment will no longer be available.

Homework: Homework will be assigned every lecture. It is essential to your success in this class that you do all the assigned homework and read the relevant sections in your Textbook. All homework will be collected at the beginning of the following lecture and selected problems graded. This is to ensure that you work consistently and can apply what you learn to problems. There will be no make-up homework assignments, but I will drop the lowest two homework assignments. Do not just copy somebody else’s homework or you will not be able to do the problems for yourself in the exams. You only learn by doing the homework problems for yourself. You can ask another student or tutor to help you with some problems, but you need to work them out for yourself. Even if you get all the problems wrong, you will still get 70% for the assignment for attempting all the problems yourself, and you will learn where you are going wrong when I go over the homework.

Drop Date: The last day to drop this class is Friday October 16, 2009. After this date a grade will be assigned.

Change to Pass/No Pass: The last day to make this change is Tuesday, September 18, 2009

Martin Luther King Jr. Day: Monday, January 19. No classes held

Lincoln Day: Friday February 13. No classes held

Washington Day: Monday February 16. No classes held

Spring Break: April 6-10

Final Exam Date: Wednesday, May 20. 10:00-11:50 am in PHY 82. Not cumulative except for nomenclature and mole calculations.

Attendance: Attendance in lecture and lab is mandatory. As an incentive to attend lectures, an additional two homework assignments will be dropped at the end of the semester if a student attends 90% of the lectures. The student will be dropped automatically if she/he misses 6 consecutive classes without contacting the instructor. Always inform the instructor ahead of time if you know you have to miss an exam. If you miss a lecture you need to read and summarize the chapter in the textbook before meeting with the instructor to discuss any problems. The homework will be on the internet notes so that you can do the homework even if you missed the lecture. If you know that you will miss a class you can submit your homework at switchboard or your answers via e-mail, but I must receive the homework before I go over the answers in class.

Grading and Exams:  There will be 6 exams covering the material of previous lectures and nomenclature. The first 5 exams will count 10% each and the final exam will count 15%. The final exam will include some questions from the whole semester. There will be 3 lab quizzes covering the material from the previous labs. Participation will be graded on completion of homework and participation during class and lab.

The final grade is calculated as follows:

Laboratory (25%):

Lab Quizzes 12.5%

Assignments 12.5%

Lecture Material (75%):

Exams 65%

Homework Assignments 10%

The grading scale to be used is A 90-100%, B 80-89%, C 70-79%, D 60-69%, F 0-59%

Student Learning Outcomes:

Upon completion of this course, students will be able to:

A.     demonstrate an appreciation for the impact of chemistry on modern society and the relationship between chemistry and other disciplines including agriculture, the medical field, and industry;

B.     classify types of matter, recognize physical properties and chemical properties, and a general understanding of the Law of Conservation of Mass and the Law of Conservation of Energy;

C.     perform unit conversions using the correct significant figures; between the English and metric systems, temperatures in different units, density, energy, and with SI units;

D.     use the periodic table to predict physical and chemical  properties of elements and calculate molar masses of compounds and molecules;

E.      recognize the electromagnetic spectrum and have a basic understanding of the quantum mechanical model of the atom;

F.      demonstrate the ability to name inorganic compounds given their formulas, and write formulas given names;

G.     distinguish and identify metals, non-metals, metalloids, and the elements of alkali metals, alkaline earth metals, halogens, noble gases, transition metals, and elements of the lanthanide and actinide;

H.     distinguish and identify between different types of intramolecular and intermolecular forces of attraction present in various substances based on chemical formulas and structures;

I.        write Lewis Electron-Dot Formulas and identify the shape using VSEPR method;

J.       write and balance chemical equations, and use these equations along with stoichiometry and the mole concept to convert quantities (e.g. grams or moles) of a given substance into quantities of an unknown substance;

K.    calculate, empirical formulas, and percentage composition given the appropriate data;

L.      distinguish and balance chemical equations of different types of reactions;

M.   perform calculations involving a limiting reagent and determining the percent yield;

N.    predict the physical behavior of gases to pressure, temperature, and volume changes;

O.    solve simple mathematical problems involving formula calculations related to gas laws;

P.      use gas laws and stoichiometry to calculate quantities (e.g. moles, volume, grams) of gas produced or consumed during a reaction;

Q.    calculate various parameters of solutions including molarity, dilution techniques, percentage concentration, and density.

R.     construct heating and cooling curves;

S.      describe state and energy changes accompanying heating and cooling curves;

T.      apply the principles of equilibrium in reversible reactions, saturated solutions, solutions of weak electrolytes and solutions of gases in solving related problems;

U.     use solution properties and stoichiometry to calculate quantities (e.g. moles, volume, grams) produced or consumed during a reaction;

V.     describe colligative properties of solutions (e.g. boiling point elevation, freezing point depression, and osmotic pressure);

W.   define and identify acids and bases and be able to perform math calculations involving the pH;

X.      determine the nature and applications for electron exchange reactions;

Y.     understand the structure of the atomic nucleus;

Z.      understand the fundamental types of nuclear radiation and the effects they have on biological systems

AA.                       and demonstrate laboratory skills which include operating an analytical balance; calibrating and/or use fundamental lab equipment such as a thermometer, barometer, buret, pipette; recognizing use and limitations of laboratory glassware; recording and reporting observations; using error analysis techniques to evaluate certainty of data; use safety precautions and general laboratory procedures.

Please be aware of the following rules:

Tardiness, leaving early, and sleeping during lecture or lab sessions are considered disruptive behavior and will result in a partial or full absence being recorded. Students will need to sign the sign-in sheet within the first 10 minutes of class.
Fraudulent behavior during exams is graded with a (0) zero.
Copying of homework, experimental data, and lab reports is considered fraudulent behavior for both the copier and the originator. DO NOT HAND IN IDENTICAL WORK. Points may be deducted from both the originator and copier.
Hand in your lab report before leaving the lab. Turning in lab reports later (including if you do a make-up a lab) will result in deduction of points.
No homework may be handed in after I have gone over it in class.  No alternative homework will be given. I will drop the lowest two homework assignments though.
No extra credit will be given. You need to work consistently from the beginning.
Dangerous behavior in the lab will result in the student being asked to leave the lab.
Please turn your cell phones onto “silent buzzer” mode during lectures so as not to disturb the class. No cell phones or i-pods will be allowed during exams.
In the lab:

·        Safety glasses need to be worn whenever somebody near you is conducting an experiment.

·        No experiments may be conducted without the instructor or teaching assistant present

·        No horseplay or unauthorized experiments. Do not taste any chemical or smell any chemical directly.

·        No visitors inside the lab. You need to go outside to meet with them.

·        No food or drinks allowed.

·        Backpacks should not be left on the floor where others can trip over them.

·        Shoes must be worn in the lab at all times.

·        Long hair should be tied back so it will not fall into chemicals or flames.

·        If any accident occurs in the lab, inform your instructor and follow safety procedures. (To be discussed during first lab period)

·        Clean up any spills promptly (Clean-up procedures will be discussed during first lab period)

·        Do not point the open end of a test tube towards anybody

·        Turn off flames when working with organic solvents. Dispose of them in waste bottles in the fume hood, not down the sink.

·        At the beginning of each lab your instructor will inform you of any special safety precautions and how to dispose of used chemicals. You need to be on time for the lab so that you hear these instructions.

·        Do not dispose of matches, paper or solid chemicals in the sink. Use the large evaporating dishes for spent matches.

·        Put broken glassware in the “broken glassware bucket”, not with the trash.

·        Before leaving the lab, wipe the desktop and wash your hands with soap and water.

If you have a verified need for an academic accommodation or materials in alternate media (i.e., Braille, large print, electronic text, etc.) per the Americans with Disabilities Act (ADA) or Section 504 of the Rehabilitation Act, please contact me as soon as possible.

Lecture and Lab Schedule:

Chemistry 3A   Fall 2009

Week

Lab Date

Labs  (Tuesdays)

Lectures  (M/W/F)

1

Aug 18

1.Safety in the laboratory

Safety Quiz.

Check in lockers.

Intro, Periodic Table

2.2 Scientific Notation

2.3 Significant Figures

2

Aug 25

6. Densities of Liquids and Solids

2.6 Dimensional Analysis & Measurements

3. Matter, Physical and Chemical Changes

4. Atoms, Elements and Ions

3

Sep 1

2. Properties and Changes of Matter

4.6 Periodic Table

Exam 1 (Wed)

5. Chemical Nomenclature: Molecules

4

Sep 8

4. Separation of Cations by Paper Chromatography

No lecture Monday (Labor Day)

5. Chemical Nomenclature: Compounds

5.7 and 5.9 Nomenclature:

Polyatomic ions and Hydrates

5

Sep 15

Nomenclature Handout

5.11 and 6.1-6.1 The Mole

6.7 Percent Composition

6.8 Empirical Formulas

Exam 2 (Fri)

6

Sep 22

7. Simplest Formula of a Compound

7. Chemical Reactions

7.4 Balancing and

7.9-7.10  Types of Reactions

7

Sep 29

8. Hydrates

Lab Quiz 1

8. Stoichiometry

8.6 Limiting Reactants and

8.7 Percent Yield

7.7 Net Ionic Equations, electrolytes

8

Oct 6

9. Percentage of Oxygen in Potassium Chlorate

6. Thermochemistry and Calorimetry

Exam 3 (Wed)

9

Oct 13

17: Calorimetry

9 Electronic configuration

9.7 Periodic table and

9.9 and 10.2 Periodic Trends

10. Bonding

Fri Oct 16 Last Day to drop a class to get a “W”

10

Oct 20

Mole Ratio for a Chemical Reaction - Handout

10.5 Lewis diagrams

10.7 Geometry

10.8 Electronegativity, Polar Covalent Bonds and Polar Molecules

11

Oct 27

18. Molecular Models

11. Gases

Exam 4 (Wed)

12

Nov 3

10. Types of Chemical Reactions

11. Gases

13

Nov 10

11. Production of Hydrogen Gas.

Lab Quiz 2

12. Liquids, Solids and Intermolecular Forces

No lecture Wednesday

(Veteran’s Day)

13. Solutions, Dilutions

14

Nov 17

12. The Molecular Weight of a Volatile Compound

14. Acids and Bases

Exam 5 (Wed)

15

Nov 24

13. Chemistry of Household Products

14. pH

14.6 Titrations

No classes Thurs and Friday

(Thanksgiving)

16

Dec 1

14. Titration of acids and bases I and II

15. Chemical Equilibrium

17. Radioactivity and Nuclear Chemistry

17

Dec 8

16. Action of Antacid Tablets

Lab Quiz 3

Review

18 Mon

Dec 14

Final Exam 9:00-10:50 am in PHY 82

| | | |