Subject: Syllabus for Chemistry 3A
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Date: Thu, 13 Aug 2009 11:20:53 -0700

SYLLABUS FOR CHEMISTRY 1A – FALL 2009

Sections 57650 and 57651

Instructor:       Veronica Cornel

Contact info:   e-mail  [email-masked] (using “Chem1A” as the subject or I will delete it) or leave message at the front desk or on my voicemail (559) 638-3641 ext. 3449

Website: http://blackboard.reedleycollege.edu

Office Hours:  10-11am MWF in PHY78

Course Objectives: Chemistry 1A is an general course in chemistry designed not only for chemistry majors, but also for biology, physics, chemical engineering, pre-medical and pre-pharmacy majors.  As a prerequisite students need to have passed CHEM10, or High School chemistry, with at least a C grade as well as basic algebra (Math 103).

Textbook:          Nivaldo J. Tro: Chemistry: A Molecular Approach (same as Fresno City College) A softcover, customized version of this book is available at our bookstore with just the first half of the book that will be used in CHEM1A. A softcover version of the second half of the book will be available for CHEM1B next semester.

Lab Manual:      Dekker: Quantitative and Qualitative Laboratory Experiments BOOK A  (not BOOK B)

Other Supplies:  A calculator is required (needs exponents and logs, but not a programmable calculator)

Approved safety glasses, lab coat and closed shoes

Lecture Notes: Download from my Blackboard website prior to class and fill in the notes during class. Homework is assigned at the end of the notes and is due the next lecture period. Studies have shown that 90% of the lecture material is retained if you review the lecture within 24 hours.

Homework: Homework will be assigned every lecture, collected at the beginning of the following lecture and a few problems graded. It is essential to your success in this class that you do all the assigned homework and read the relevant sections in your textbook. 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 do your homework with somebody else. 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. If two students hand in identical homework, I will deduct points from both students! 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. If you can’t attend the lecture, give your homework to me or to switchboard prior to the class period they are due. .

Attendance: Attendance in lectures and lab is mandatory. The student will be dropped automatically if she/he misses two weeks of lectures without contacting the instructor. If you miss a lecture you need to obtain the notes to fill in from another student and read the section in the textbook before meeting with the instructor/tutor to discuss any problems. 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. If a student is disruptive (including using cell-phones, interrupting the instructor continuously) they may be asked to leave the lecture/lab and recorded as "absent".

Drop Date: The last day to drop this class is Friday October16 , 2009. After this date a grade will be assigned.

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

Labor Day: Monday, September 7 (No classes held)

Veteran’s Day: Wednesday, November 11 (No classes held)

Thanksgiving: Thursday and Friday, November 26-27 (No classes held)

Final Exam Date: Monday, December 14, 11:00-12:50. Cumulative to a certain extent. Selected questions will be given from the entire semester (will be told which types of questions) as well as the last few weeks of work.

Grading : There will be 5 lecture exams, the first 4 counting 12% of your grade and the final counting towards 17% of your grade. Half of the final exam will be on the last few weeks of material, and the rest will be questions similar to those on the earlier 4 exams. Homework will count 10% and your lab work will count 25% (12.5% lab reports and 12.5% lab quizzes)

General Grading break-off : A 90-100%, B 80-89%, C 70-79%, D 60-69%, F 0-59%

Tutoring: Free tutoring is available at the Tutorial Center at the Library

Please be aware of the following rules:

Tardiness, leaving early, or sleeping during lectures will result in a partial or full absence being recorded. Students 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 HOMEWORK.
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.
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.

LABS

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.
Dangerous behavior in the lab will result in the student being asked to leave the lab.
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.
Closed shoes and lab coats 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 or sand bucket for spent matches.
Put broken glassware in the “broken glassware box”, not in 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 (especially in labs) 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.

Course Outline:  Each Topic takes 1-2 weeks References are to “Chemistry: A Molecular Approach” by Nivaldo Tro.

A.  Matter and energy (Chapter 1)

1.   The Laws of conservation of matter and energy (Chapter 1.2)

2.   States of Matter (Chapter 1.3)

3.   Chemical and physical properties of matter (Chapter 1.4)

4.   Chemical and physical changes of matter (Chapter 1.4)

B.   Measurements in chemistry

1.   Length, mass, volume (Chapter 1.6)

2.   Density and specific gravity (Chapter 1.6)

3.   Significant Figures (Chapter 1.7)

4.   Dimensional Analysis  (Chapter 1.8)

C.   Atoms, molecules, ions, compounds, elements and mixtures (Chapter 2)

Atomic mass units and isotopes (Chapter 2.6)

D. Nomenclature

1. Naming inorganic compounds with monatomic and polyatomic ions (Chapter 3.5)

2. Naming moleculular compounds (Chapter 3.6)

E.   Stiochiometry, chemical formulas, and equations

1.   Formulas of compounds, etc., and what they mean (Chapter 3.5-3.6)

2.   The mole, Avogadro’s Number, and molar mass (Chapter 3.7)

3.   Formula weight, molecular weights, and moles (Chapter 3.7)

4.   Writing and balancing chemical equations (Chapter 3.10)

5.   Percent composition and formulas of compound (Chapter 3.8)

a.    Empirical formula (Chapter 3.9)

b.   Molecular formula (Chapter 3.9)

1)  Chemical equations and calculations (Stoichiometry) (Chapter 4.2)

2)  Percent purity, yield, and limiting reagent in equations (Chapter 4.3)

F.   Concentration of solutions (Chapter 4.4)

1.   Percent by mass and volume

2.   Molarity (M) molar concentration

3.   Dilution of solutions

G.  A systematic study of chemical reactions

1.   Aqueous solutions, electrolytes, nonelectrolytes and extent of ionization (Chapter 4.5)

2.   Solubility rules (chapter 4.5)

4.   Net Ionic equations (Chapter 4.7)

5.   Classification of chemical reactions

a.    combination and decomposition

b.   single replacement reactions

c.    metathesis or double replacement reactions (precipitation, acid-base neutralization) (Chapter 4.6 and 4.8)

d.   combustion reactions

H.  Acids, Bases, and Salts (Chapter 4.7-4.8)

1.   Arrhenius acids and bases

2.   Bronsted-Lowry acids and bases

3.   Properties of acids and bases

4.   Preparation of acids and bases

5.   Concentrations and acid-base reactions in aqueous solutions.

6.    Titrations

I.    Oxidation Reduction Reaction (Chapter 4.9)

1.   Assigning oxidation numbers

2.   Recognizing redox equations by changing in oxidation state

3.   Balancing simple redox equations (Chapter 18.2)

J.    Physical behavior of gases (Chapter 5)

1.   The relationship of pressure and volume; Boyle’s Laws (Chapter 5.3)

2.   The relationship of volume and temperature.  Charles’ Gay Lussac Law (Chapter 5.3)

3.   Temperature (Kelvin absolute scale) (Chapter 5.3)

4.   STP : standard temperature and pressure (Chapter 5.3)

5.   Combined gas laws and molar volume (Chapter 5.3)

6.    The Ideal Gas Law (Chapter 5.4)

7.   Molecular weight calculation and Dalton’s Law of partial pressures (Chapter 5.5 and 5.6)

8.   Graham’s Law of effusion (Chapter 5.9)

K.  Thermochemistry (Chapter 6)

1.   Heats of reactions and calorimetry (Chapter 6.5-6.6)

2.   Work (Chapter 6.3)

3.   The first Law of Thermodynamics (Chapter 6.2)

4.   Hess’s Law (Chapter 6.8)

5.   Standard enthalpies of formation (Chapter 6.7-6.8)

L.   Atomic Structure (Chapters 2, 7 and 8)

1.   Fundamental particles of atom (Chapter 2.6)

2.   History of atomic structure and fundamental particles  (Chapter 2.4-2.5)

3.   Atomic number and mass number (Chapter 2.6)

4.   Nuclear stability and binding energy (Chapter 2.6)

5.   Atomic spectra and the Bohr atoms (Chapter 7.3)

6.   Quantum numbers, orbitals, main shells and subshells (7.5-7.6, 8.3)

7.    Electronic configuration (Chapter 8.3)

M.  Chemical periodicity and ionic bonding

1.   The periodic table (Chapter 8.2)

2.   Periodic properties and trends (Chapter 8.6)

3.   Ionization energy, electron affinity, electronegativity, and size of atoms (Chapter 8.7-8.8)

4.   Metals, non-metals and metalloids (Chapter 2.7)

5.    Valence Electrons (Chapter 8.4)

N.  Chemical Bonding (Chapter 9)

1.   Kinds of chemical bonds

2.   Ionic bonding, ionic changes, oxidation numbers

3.   The covalent bond

a.    polar and nonpolar bonds (Chapter 10.5) and intermolecular forces (Chapter 11.2)

b.   Lewis dot formulas (Chapter 9.7)

c.    Octet rule and its limitations (Chapter 9.8? and 9.9)

d.   Basic motions of bonding theory and resonance (Chapter 9.8)

e.    Formal charges of Lewis dot formulas (Chapter 9.8)

O.  Covalent bonding and molecular structure (Chapter 10)

1.   VSEPR Theory and Valence Bond theory (Chapter 10.2-10.3)

2.   Geometry of molecules from VSEPR or Valence Bond theory (Chapter 10.4)

3.   Geometry of polyatomic ions (Chapter 10.5)

4.   The shape of molecular orbitals (Chapter 10.7)

5.   Energy level diagram of orbitals

6.   Homonuclear and heteronuclear diatomic molecules (Chapter 10.8)

P.   Liquids and Solids (Chapter 11)

1.   Liquid state, adhesive and cohesive forces (Chapter 11.3)

a.    Viscosity

b.   Surface tension

c.    Vapor pressure

d.   Boiliing points and freezing points

e.    Heat transfer

2.   The Solid State (Chapter 11.12)

a.    Melting point

b.   Heating point

c.    Sublimation and vapor pressure

d.   Crystal structure and amorphous

e.    Bonding in solids

f.    Metallic bonding (Chapter 9.11)

Q.  Solutions (Chapter 12)

1.   Solutions terminology

2.   Concentration units (mole fraction, molality, molarity)

3.   Dilution of solutions

Student Learning Outcomes: In the process of completing this course, students will:

A.        learn the names and symbols of the representative elements;

B.        identify the first ten transition elements and selected others as they are introduced;

C.        name inorganic compounds and the rules for these names;

D.        predict ionic and covalent bonding between species;

E.         convert from the English to the metric system in weights, volume, and linear measurements;

F.         calculate molecular weights, formula weights, gas volumes, temperature, pressure concentration of solutions, molarity, empirical and molecular formulas, and percentage composition;

G.        solve oxidation reduction equations, assign oxidation numbers, and use both molecular and net ion forms of the equation;

H.        define the structural periodicity of elements;

I.          interpret the gradual change from metal to non-metal as one goes across the periodic table from left to right;

J.          discuss the trends in all directions on the periodic chart and the terms for grouping elements, i.e., metalloids, transition elements, inner transition, etc.;

K.        apply the Arrhenius definition of acid and base;

L.         solve limiting reagent problems involving molecular and ionic compounds as pure substances and as solutions;

M.        describe covalently bonded structures using Lewis theory, valence bond theory (including hybrid orbitals), and molecular orbital theory of diatomic molecules;

N.        define the theoretical and mathematical description of ideal gases, including the concepts of temperature and kinetic energy distribution;

O.        describe colligative properties of solutions of ionic and non-ionic substances and solve their numerical problems;

P.         solve thermochemical problems, including using Hess’s Law and calorimetry;

Q.        demonstrate skills in laboratory in the use of the analytical balance, thermometer calibration and usage, barometer reading, working with glass, filtration, titration, simple synthesis, spectroscopy, the care of one’s equipment, and the recognition that if an experiment is not correct, there must have been a mistake and how to find this mistake.

Chemistry 1A   Fall 2009

Week

Date

Labs   (T/Th)

Lectures  (M/W/F)

1

Aug 18

Unit 1: Introduction to Laboratory Safety, and Inventory Check-in

1. Matter

Dimensional Analysis

Scientific Notation and Significant Figures

Aug 20

Unit 2: Mixtures and Pure Substances

2

Aug 25

Unit 3: Measurement

2. Atoms

3.5  Ionic Compounds

3.6 Molecules

Aug 27

Unit 4: Gravimetric Analysis

3

Sep 1

Nomenclature Worksheet

2.9 Mole

Exam 1 (Wed)

Go over exam

Sep 3

Unit 7: The Mole

4   Mon

Sep 7

Labor Day

No lecture Monday

3.10, 4.6  Writing and Balancing Reactions

3.8-9 Empirical

Sep 8

Unit 6: Halides

Sep 10

Lab Quiz 1 (Labs 1,2,3,4,7,  Safety and Nomenclature)

5

Sep 15

Empirical Formulas: Oxide of Tin and Worksheet

4.2 Stoichiometry

4.3 Limiting

4.4 Solutions

Sep 17

Unit 8: The Formula of a Hydrate

6

Sep 22

Unit 5: Double Displacement Reactions

4.5 Electrolytes and

4.8 Acid-Base reactions

Exam 2 (Friday)

Sep 24

Unit 9: Stoichiometry

7

Sep 29

Unit 10: Alum Crystallization.  Recycling Aluminum Cans

Go over exam

4.7 Titrations and Reaction Types

4.9 Redox Reactions

Oct 1

Unit 11: Properties of Solutions

8

Oct 6

Unit 15: Redox Reactions- The Burning of Magnesium

18.2 Balancing Redox Reactions and Redox titrations

5. Gas 1-2

Oct 8

Lab Quiz 2 (Labs 5-6, 8-11 and empirical formulas)

9    Tue

Thur

Fri

Oct 13

Unit 16: Formation of a Simple Salt and Complex Ions

5. Gas 3-4

Exam 3 (Friday)

Oct 15

Unit 21: Charles's Law

Oct 16

Last Day to drop class to get a “W”

10

Oct 20

Unit 22: Molecular Mass of a Volatile Liquid

Go over exam

6. Thermo 1 and 2

Oct 22

Unit 23: Atomic Mass of an Unknown Divalent Metal Unit

11

Oct 27

27: Heat Flow, Calorimetry

6. Thermo 3

7. Light 1 and 2

Oct 29

Thermochemistry Worksheet

12

Nov 3

Unit 13: Acids and Bases

8.4 Electron Configuration

7. Quantum Numbers

Exam 4 (Friday)

Nov 5

Unit 14: Buffers and Antacids

13  Tue

Wed

Thur

Nov 10

Lab Quiz 3 (Labs 15-16, 21-23, 27)

Go over exam and

8. Periodicity

No lecture Wednesday

9. Lewis Diagrams

Nov 11

Veteran’s Day

Nov 12

Unit 17: Percent Iron (II) in an Unknown

14

Nov 17

Unit 19: Vitamin C in Fruit Juices

9.8 Formal Charges

10. Geometry 1 and 2

Nov 19

Unit 28: Molecular Geometry Part 1

15

Th-F

Nov 24

Unit 28: Molecular Geometry Part 2

10.7 Hybridization

Nov 26-27

Thanksgiving

16

Dec 1

Unit 29: Polarity Parts 2 and 3

9.8 Resonance

10.5 Dipoles and

11.2 Intermolecular Forces

Dec 3

Unit 30: Freezing Point Depression

17

Dec 8

Unit 31: Polymers Part 3: Slime

11.2/3  Liquids

11.6/7/8/11/12  Solids

Dec 10

Lab Quiz 4 (Labs 13-14, 17, 19,

28-30)

18 Mon

Dec 14 : Final Exam 11:00am-12:50pm in PHY 76