SYLLABUS FOR CHEMISTRY 1A – FALL 2008 (Sections 57650 and 57651)

LFS-A MWF 11-11:50am and Labs TTh 8:00-10:50am or 11:00-1:50pm

 

Instructor:      Veronica Cornel     

Contact info:  e-mail vmcornel@scccd.org  (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:  10-11 am MW, and 9-11am Fridays in LFS B

 

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 101).

 

Textbook:          Nivaldo J. Tro: Chemistry: A Molecular Approach (same as Fresno City College)

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

Other Supplies: A calculator is required (needs exponents and logs – a graphing calculator is not needed)

                           Approved safety goggles, 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.

 

Drop Date: Students are responsible for dropping the course before October 17. After this date a letter grade will be given. 

 

Attendance: Attendance in lectures and lab is mandatory and the College requires the instructor to take attendance every lecture and lab. The student will be dropped automatically if she/he misses 2 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. Arriving late or leaving early or sleeping during class will result in the student being recorded as “absent”. If a student is disruptive (including using cell-phones) they may be asked to leave the lecture/lab and be marked as "absent".  As an incentive, students who attend 90% of the lectures will be allowed to drop 4 homework assignments.

 

Class Cancellation Policy: If the instructor is absent, and official yellow “class cancellation” notice and instructions will be posted on the door of the classroom. We will try and put a timely announcement on Blackboard and the Reedley College website.

 

Homework will be collected every lecture and selected problems will be graded. Homework needs to be done individually and you need to show all your work, not just the answers. Another student or tutor may help you but must not give you the answers. If two students hand in identical homework both students will loose points. Even if you get all the problems wrong, you will still get 70% for the homework assignment for completing it yourself. If you are absent it’s your responsibility to hand the homework in at the switchboard or to me before the beginning of the next lecture. No late or make-up homework assignments will be allowed. Instead, two homework assignments will be dropped, and if you attend 90% of the lectures you may drop a total of 4 homework assignments.

 

Grading : There will be 4 lecture exams, equally weighted and counting towards 65% of your grade. The final exam will be mainly on the last four weeks of material, but will include questions similar to those on the earlier 3 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:

  • 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 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 miss a lab you need to make up the lab at the next lab period or you will be given zero for that lab. You may attend the other lab section if you cannot make your usual lab section.

 

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

 

Course Objectives: 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.

 

 

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.

 

                                CHEM1A Fall 2008 T/Th

Week

Date

Lab

1  

Aug 19

Unit 1: Introduction to Laboratory Safety. Safety Quiz

    

Aug 21

Unit 2: Mixtures and Pure Substances

2  

Aug 26

Unit 3: Measurement

    

Aug 28

Unit 4: Nomenclature and Gravimetric Analysis

3   M

Sep 1

Labor Day (No lecture)

     T

Sep 2

Unit 5: Double Displacement Reactions

     Th

Sep 4

Nomenclature Worksheet. Review for Lab Quiz 1

4   

Sep 9

Lab Quiz 1: Lab Safety and Units 1, 2, 3, 4, 5

 

Sep 11

Lecture Exam 1

5

Sep 16

Unit 7: The Mole

 

Sep 18

Unit 8: The Formula of a Hydrate

6

Sep 23

Unit 9: Stoichiometry

 

Sep 25

Unit 10: Alum Crystallization.  Recycling Aluminum Cans

7

Sep 30

Unit 11: Properties of Solutions

 

Oct 2

Unit 16: Formation of a Simple Salt and Complex Ions

8

Oct 7

Review for Lab Quiz 2

 

Oct 9

Lab Quiz 2: Units 7, 8, 9, 10, 11, 16

9    T

Oct 14

Lecture Exam 2

     Th

Oct 16

Unit 15: Redox Reactions- The Burning of Magnesium

      F

Oct 17

Drop Date

10

Oct 21

Unit 21: Charles's Law

 

Oct 23

Unit 22: Molecular Mass of a Volatile Liquid 

11

Oct 28

Unit 23: Atomic Mass of an Unknown Divalent Metal

 

Oct 30

Unit 27: Heat Flow, Calorimetry

12

Nov 4

Unit 13: Acids and Bases

 

Nov 6

Unit 14: Buffers and Antacids

13  T

Nov 11

Veteran’s Day (No Class)

Th

Nov 13

Lab Quiz 3: Units 13, 14, 15, 21, 22, 23, 27,

14  T

Nov 18

Lecture Exam 3

 

Nov 20

Unit 17: Percent Iron (II) in an Unknown

15

Nov 25

Unit 19: Vitamin C in Fruit Juices

  Th-F

Nov 27-28

Thanksgiving Holidays

16

Dec 2

Unit 28: Molecular Geometry Part 1

 

Dec 4

Unit 28: Molecular Geometry Part 2

17

Dec 9

Unit 30: Freezing Point Depression. Review for Lab Quiz 4

 

Dec 11

Lab Quiz 4.

18

Monday

Dec 15

Lecture Exam 4: 11-12:50 in LFS A