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CHE 111

CHE 111 - GENERAL CHEMISTRY I

INSTRUCTOR: J. PADULA

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SYLLABUS - Spring 2012

Janice Padula                                                                             

Phone: 562-4335

Office 217T 

e-mail: Padula's Contact Information

 

Course Description:    This is the first semester course in a two-semester sequence which presents the basic laws and concepts of general quantitative chemistry.  This course will include measurement, stoichiometry, thermochemistry, the periodic table, an introduction to acids and bases, reduction and oxidation, ionic and covalent bonding, molecular structure, VSEPR and MO Theory. There are three hours of lecture and one two-hour laboratory per week.  Prerequisite: ENG 094 and MAT 101 or equivalent. Co-requisite: ENG 101

 

General Education Learning Outcomes:  This course meets the SUNY General Education knowledge area for science.  Students will demonstrate the ability to:

1.          understand the methods scientists use to explore natural phenomena, including:

§         observation

§         hypothesis development

§         measurement and data collection

§         experimentation

§         evaluation of evidence

§         employment of mathematical analysis

2.          apply scientific data, concepts and models in one of the natural sciences

 

Course Objectives: As the result of instructional activities, students will be able to:

  1. use appropriate chemical terminology and nomenclature to effectively communicate their understanding of  concepts in chemistry
  2. describe the phases of matter and their molecular and elemental properties
    1. distinguish between solids, liquids, gases and plasmas
  3. define the difference between homogeneous & heterogeneous mixtures
    1. identify and apply methods of separation of mixtures using physical properties
    2. apply methods of separation using chemical instrumentation such as HPLC & GC
  1. explain atomic theory, atomic structure, atomic mass, atomic number, isotopes and ions of a given particular element
    1. calculate atomic mass from mass spectroscopy data to determine the atomic mass of an element on the periodic table
    2. define the concept of a mole, molar mass and Avagadro’s number
    3. calculate conversion between grams to moles and moles to grams
  1. describe stoichiometry with respect to reactions and solve related problems
    1. write balanced equation
    2. determine stoichiometric relationships between reactants and products
    3. calculate limiting reactants, excess reactants, theoretical yield, & percent yield
  1. explain chemical reactions and distinguish between the different types
    1. identify and balance combination, decomposition, displacement, and metathesis reactions
    2. write and balance ionic and net ionic equations, precipitation reactions with respect to solubility, neutralization reactions, red-ox reactions, and combustion reactions
  1. define acids and bases in terms of Arrhenius
    1. calculate molarity
    2. describe titrametric methods
  1. explain kinetic and potential energy, concept of heat, heat capacity, and enthalpy
    1. distinguish between endothermic and exothermic processes
    2. calculate specific heats of reactions
    3. define and use Hess’s Law to calculate the enthalpy of a reaction
    4. calculate standard enthalpies of formation
  1. describe the concepts in quantum mechanics to explain electron motion
    1. describe a photon and how it is emitted
    2. define line spectra and give examples
    3. describe the electromagnetic spectrum and how each type of radiation relates to the others with respect to wavelength, frequency and energy
    4. define Heisenberg’s uncertainty principle
    5. list the 4 quantum numbers, giving both symbol and name, and explain what each one means and give an example
    6. draw all the orientations of s, p, and d orbitals
  1.  define electron configuration and periodicity for all elements
    1. write electron configuration and orbital diagrams for all elements from H to Ba and their ions
    2. list Aufbar’s filling order
    3. define periodic trends with respect to ionization energy, electron affinity and atomic radii
  1. explain bonding and molecular structures using VSEPR and MO theory
    1. write complete bond descriptions including hybrid orbital’s of sp, sp2 and sp3
    2. draw Lewis structures for molecules, identify the bond directions, geometry and hybridization
    3. describe linear, trigonal planar, tetrahedral, trigonal bipyramidal and octahedral molecular geometry, sub-classifications of each and the associated vertex angle for the 5 geometric model
    4. draw a Molecular Orbital Diagram (MO) for all diatoms from H2 to Ne2, determine the bond order, and if the molecule is paramagnetic or diamagnetic

Laboratory Objectives: The laboratory experience will reinforce the understanding that experimental work is the foundation of chemical knowledge and which requires fundamental laboratory skills. Students will:

1.      anticipate, recognize, and respond properly to potential hazards in laboratory procedures

a.       complete laboratory safety training as designed by the CCC science department

b.      review the contents of MSDS & location of MSDS sheets storage area

2.      keep accurate and complete experimental records

a.       write all lab records in a bound lab notebook using Proper Lab Documentation (PLD) as required for Good Lab Practices (GLP)

b.      enter all data as it is generated in the lab

3.      perform accurate quantitative measurements

a.       use properly calibrated instruments (i.e. spectrophotometers) and volumetric glassware

4.      interpret experimental results and draw reasonable conclusions

a.       record in the lab notebook all information/data using tables, graphs, formulas and calculations

b.      write a conclusion of results in the lab notebook at the end of each lab to summarize what was discovered in the laboratory

5.      communicate effectively through oral and written reports

a.       write 3 formal lab reports – Empirical Formula, Hess’s Law and UV/Vis Spectroscopy

b.      report required information such as tables, graphs, formulas, calculations background and summary in electronic format

c.       use Excel, Word and PowerPoint to present laboratory data and reports to the instructor and classmates as required

6.      analyze data statistically, assess the reliability of experimental results, and discuss the sources of systematic and random error in experiments

a.       use statistical interpretation as needed in the summary of lab information and required lab reports

b.      include correlation of data on all graphs via electronically generate linear trend lines

7.      plan & execute experiments through the use of appropriate chemical literature & electronic resources

a.       research background information required for labs and lab reports from reputable sources such as American Chemical Society (ACS) or .edu, .org, and .gov websites

 

Course Design:          This course will be presented by a series of lectures, demonstrations, interactive computer exercises, journal articles, and laboratory experiments.  Angel will be an important part of this course to access course notes, lab information, discussions, and grades. The grading scheme is as follows:                     

  6 Module exams          @   100 points   =   600 points

  Final Exam              @    50    "     =    50   "

  Homework & Quizzes      @    varied      =    50   "

  5 Journal Discussions   @     10    "     =    50   "

  15 Graded Labs          @    varied      =   250   "

  Final grade total            1000 points / 10 = grade

 

Text and materials:    Kotz, John C., Treichel, Paul M., & Townsend, John R., Chemistry & Chemical Reactivity, 7th ed., Thomson Brooks/Cole, 2009. textbook (e-books are okay) , a scientific or graphing calculator, a bound composition notebook with graph paper pages for lab, safety glasses, and a straight edge are all required for this course. Study groups are required!

 

Attendance:     It is extremely important to attend all classes, labs and sessions.  In order to be successful in this course, you are expected to spend at least (on average) an additional 15 hours per week reading the textbook, doing the assignments, writing up your labs and preparing for/completing your exams. The College policy states that students must attend class regularly. Students who miss more than 15% of classes may be withdrawn from the course or given a grade of "F".  Attendance will be marked during the first few minutes of class. Entering the classroom late is disruptive to me and to other students. Please make every effort to be on time. 

 

Attending class is defined in this course as arriving on time, remaining in the classroom until the end of class, and being attentive and not engaging in disruptive or distracting behaviors.

 

Attention and Distractions

On the days you attend class, you should plan to be fully present and focused on class for the entire period.  Cell phones must be OFF, not on vibrate or silence. Talking to others, sleeping, and any other behaviors that do not contribute to your learning or could distract other students are included under this policy

 

Disruptive or distracting behavior will result in the student being marked absent for the day.  Students will be informed at the end of class or via email when this policy is enforced to avoid any further disruption to the class.

 

 

Note:    Refer to your student handbook for policies that pertain to attendance, academic integrity, and behavior. Please understand your work must be your own. YOUR LAB REPORTS MUST BE WRITTEN BY YOU; NOT AS A JOINT REPORT WITH YOUR LAB PARTNER.  I have a zero tolerance for anyone caught cheating or plagiarizing work. In order to understand what constitutes plagiarism, check out the following websites: 

 

http://www.plagiarism.org/resources/documentation/plagiarism/learning/preventing_plagiarism_instructor.doc

http://www.indiana.edu/~wts/pamphlets/plagiarism.shtml

http://owl.english.purdue.edu/handouts/research/r_plagiar.html 

 

           I hope you enjoy this class!  Do not hesitate to seek help from me, tutors in the Academic Assistance Center or fellow classmates to clarify course materials.  Study groups work very well in this course.  If you need help finding a study partner, just tell me.

If you have or suspect that you may have, any type of disability or learning problem that may require extra assistance or special accommodations, please speak to me privately as soon as possible so I can help you obtain any assistance you may need to successfully complete this course.  You should also contact Laurie Bethka, Room 420M in the Academic Assistance Center, for further assistance.

If you have any allergies to chemicals or latex, suspect that you may be pregnant or have an illness or condition that may be complicated by working in the lab, please let me know.  I can remove you from handling chemicals in certain labs depending on the situation.

 

                        

              CHE 111 - Course Outline  

Introduction - An overview of the course

Chapter 1 – Basic Concepts of Chemistry

Chapter 2 - Atoms & Molecules and Ions

EXAM 1 & First Journal Discussion

Chapter 3 – Chemical Reactions

EXAM 2 & Second Journal Discussion

Chapter 4 – Stoichiometry: Chemical Reactions                           

EXAM 3 & Third Journal Discussion

Chapter 5 - Thermodynamics

                        EXAM 4 & Fourth Journal Discussion

Chapter 6 – Quantum Theory and the Electronic Structure of Atoms

Chapter 7 - Periodic Relationships among the Elements

                        EXAM 5 & Fifth Journal Discussion

Chapter 8 – Chemical Bonding I: Basic Concepts

Chapter 9 - Chemical Bonding II: Molecular Geometry & Hybridization of Atomic Orbitals

                        EXAM 6

Final Exam Week Schedule: Final Assessment Exam on Wednesday from 12:40-3:10, last class meeting Friday 10:00-12:30

 LABORATORY EXERCISES – SPRING 2012

DATE 

 NUMBER 

TITLE

1/30

LAB 1

Introduction, Lab Safety, MSDS & Orientation

1/30

LAB 2

Mixtures and Separations

2/6

LAB 3

Density and  Measurement

2/13

LAB 4

Ions, Polyatomic Ions, CD & Flashcards

2/20

LAB 5

Decomposition of Potassium Chlorate

2/27

LAB 6

Balancing Equations, Solubility & Net Ionic Equations

3/5

LAB 7

Acid /Base Titration

3/19

LAB 8

Hess’s Law

3/26

LAB 9

Hess’s Law Calculations

4/2

LAB 10

Energy: Solar/Photovoltaics

4/9

LAB 11

Absorption Spectroscopy of CoCl2

4/16

LAB 12

Electron Configuration

4/23

LAB 13

Lewis Structures

4/30

LAB 14

VSEPR

5/7

LAB 15

Molecular Geometry

5/16

12:40-3:10

Final Assessment

If you need to contact me, go to Padula's Contact Information.

Last Updated: 04/04/2012