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Chemistry Department
Fall, 2008
Course Prefix and Number: CHEM 1211, Principles of Chemistry I
Contact/Credit: 3 lecture/3 credit hours
Catalog Course Description: This course is an introduction to a quantitative study of the physical and chemical behavior of matter in its several phases and a consideration of modern theories of bonding forces at the molecular level. Atomic and molecular structure, chemical nomenclature, stoichiometry, thermochemistry, the gaseous state, and properties of solutions are discussed.
Prerequisites: MATH 1111 OR MATH 1113
Co-requisites: CHEM 1211L
Class Location: BSC 1011 (Auditorium) Class Times/Days: Lecture: T TH, 11:00 12:50 am
Instructor: Dr. de la Garza Telephone Number: (229) 333-5340
email: ldelagarza@valdosta.edu
Office Location: BSC 3080 Office Hrs./Days: T: 1 pm 3 pm; F: 8 am-9:30 am Any other time by appointment
Required Textbooks(s): CHEMISTRY and CHEMICAL REACTIVITY, Kotz, Treichel, Weaver, 6th Ed or higher
Additional required Materials: OWL access code (https://owl1.thomsonlearning.com/); calculator.
Student Outcomes: Upon successful completion of this course, the student will be able to:
Determine the moles and masses of substances consumed or produced in a chemical reaction by using a balanced chemical equation;
Predict the structure of a molecule and its hybridization based on VSEPR theory;
Determine the number of protons, neutrons, and electrons in an atom or ion using the periodic table;
Identify physical properties and chemical properties of elements;
Calculate the enthalpy change of a reaction by using the thermodynamics table;
Name compounds using IUPAc rules and write formulas;
Course Requirements:
1-Partial tests: 3 exams will be administered, covering chapters 1-4; 5-6; and 7-9. Please keep up with the material so you dont get overwhelmed. Also, the material covered in previous chapters is used later on: study from the beginning and dont skip material.
2- Final exam: 1 comprehensive final exam will be given; this is a standard test contains questions from chapters 1 through 14. Students who do not take the final exam will fail the course, students who make 35% or less will have a drop in the letter grade (if your final average is 80 = B, but you made 35 or less on the final your final grade will be a C, etc).
2- Homework: 14 required OWL assignments (each with 6 to 14 end-of-chapter questions) are assigned throughout the semester. You will need to read the book and study before you attempt them. Make sure that you know how to solve these types of problems and the concepts they involve (as the concepts will be included in exams). Please complete them by their due date. Complete instructions on pages 3-4 of this syllabus.
3- Quizzes: 6 to 8 quizzes will be given throughout the semester with concepts and topics to be addressed in tests.
4- Bibliographic Research Team Project: One team report will be submitted, with ALL students contributing to the work and evaluating peers reports and team leaders submitting the document and student evaluations. Complete instructions on pages 5-6 of this syllabus.
Evaluation of Performance:
54% = Three partial exams (18% ea)
16% = Final exam
19% = Bibliographic Research Team Project
7% = Homework (0.5% ea)
4% = Quizzes (0.5% ea)
Grading Scale:
Grade Numerical Points
A 90 and higher
PRIVATE B 80-89 tc \l 2 "B Above Average 86-93 3.0"
C 70-79
D 60-69
F 59 and lower
Disability Access Statement: Students requesting classroom accommodations or modifications because of a documented disability should contact the Access Office for Students with Disabilities located in Room 1115 Nevins Hall. The phone numbers are 245-2498 (voice) and 219-1348 (TTY). Any needs must be discussed with the professor at the beginning of the term.
Attendance:
Lecture attendance is required. Students are to be seated when lecture begins. In accordance with ɫ policy, 20% or more absences can result in a course grade of F. It is responsibility of the student to drop a course they choose not to attend. NO food allowed during the lecture. CELL phones and pagers must be OFF during lecture. No hats allowed during examinations.
Course Outline and Tentative Schedule:
Week of Lecture Assignments due
Aug 18 Ch. 1 Matter
Aug 25 Ch. 2 Elements Ch 1, 2 due Mon Sep 1.
Sep 1 Ch. 3 Compounds
Sep 8 Ch. 4 Chemical Reactions 1st Set of Team Reports due Tue Sep 9
Sep 15 Ch. 5 Reactions in Aq. Solutions Ch 3, 4 due Mon Sep 15.
EXAM I will be given on Tuesday Sep 16 (Ch 1-4).
Sep 22 Ch. 5 Reactions in Aq. Solutions Ch 5 due Mon Sep 29.
Sep 29 Ch. 6 Energy and Reactions 2nd Set of Team Reports due Thur Oct 2
Oct 06 Ch. 6 Energy and Reactions Ch 6 due Wed Oct 8.
EXAM II will be given on Thursday Oct 9 (Ch 5, 6).
Oct 13 Fall Break Oct 13-14
Oct 20 Ch. 7 Atomic Structure Ch 7 due Mon Oct 27.
Oct 27 Ch. 8 Electronic Configuration Ch 8 due Mon Nov 3.
Nov 3 Ch. 9 Bonding: Fundamentals 3rd Set of Team Reports due Thur Nov 6
Nov 10 Ch. 10,11 Bonding* Ch 9 due Mon Nov 10.
EXAM III will be given on Tuesday Nov 11 (Ch 7-9).*Chapters 10 & 11 will not be included in the third partial exam but are important for the final exam.
Nov 17 Ch. 12 Gases Ch 10, 11 due Mon Nov 17.
Nov 24 Thanksgiving break Nov 26-28 Ch 12 due Mon Dec 1.
Dec 1 Ch. 13 Intermolecular Forces & Ch 14. Solutions
Dec 8 Ch 13, 14 due Mon Dec 8.
FINAL EXAM will be given on Friday Dec 12.
Exam dates
Exam I: Tuesday September 16, 2008.
Exam II: Thursday October 9, 2008.
Exam III: Tuesday November 11, 2008.
Final Exam: Friday December 12, 2008 at 10:15 AM-12:15 PM
Final exam revisions during Dec 12 (2-4 pm).
Make up exams or quizzes will NOT be given. * Any emergency needs to be informed to the Office of Students Affairs (phone: 333-5359).
Please keep up with the material, if you need HELP please see me in office hours or by appointment (and please honor your appointments). Laboratory time is an important part of your practice. Attend to the laboratory experiments for a different way to learn the material.
Other important dates:
Mid Term: Thursday October 9, 2008. (Last day to drop a course)
Last Class Day: Thursday December 4, 2008.
Holidays:
Fall Break: October 13-14, 2008.
Thanksgiving: November 26-28, 2008.
Instructions for Take-home assignments:
Fourteen (14) OWL assignments (each with 6 to 14 end-of-chapter questions) are assigned throughout the semester. Only the Questions for End of Chapter - Multiple Choice and Short Answer are required, the other OWL exercises are for extra-points.
Submit your answer on the OWL web-site for the corresponding end-of-chapter exercise before the due date. Due times might change, check your OWL website continuously. START WORKING ON PROBLEMS AS THE MATERIAL IS COVERED, DO NOT WAIT UNTIL LAST DAY TO SUBMIT ANSWERS!
Below are the SAME required questions for each chapter with their textbook number, so in case you do not have online access at home, you can work on the problems and then submit your answers before the due date using a school computer.
Chapter 1: Matter and Measurement (10 exercises)
Solve end-of-chapter questions # 1, 14, 25, 28, 35, 38, 60, 87, 98, and 102.
Chapter 2: Atoms and Elements (10 exercises)
Solve end-of-chapter questions # 1, 11, 13, 18, 26, 30, 32, 36, 40, and 64.
Chapter 3: Molecules, Ions, and Compounds (12 exercises)
Solve end-of-chapter questions # 6, 14, 18, 22, 28, 32, 36, 42, 51, 58, 80, and 86.
Chapter 4: Chemical Equations (10 exercises)
Solve end-of-chapter questions # 1, 6, 14, 18, 28, 34, 48, 54, 64, and 65.
Specific objetives: Upon successful completion of this section, the student will be able to:
Use the Kinetic Molecular Theory to describe the physical states of matter;
Perform density calculations;
Recognize between intensive and extensive properties;
Recognize between accuracy and precision;
Use the periodic table to find elements;
Give the names and symbols of elements and names and formulas of compounds;
Perform calculations with isotopes and atomic weight;
Recognize ionic vs. molecular compounds;
Recognize polyatomic ions;
Perform % mass composition calculations;
Use the Law of Conservation of Matter to balance chemical equations, specially combustion reactions;
Use the mole concept to perform stoichiometric and limiting reactant calculations.
Chapters 1-4 are included in Exam I.
Chapter 5: Reactions in Solutions (14 exercises)
Solve end-of-chapter questions # 4, 12, 16, 22, 28, 36, 40, 44, 52, 58, 62, 80, 84, and 100.
Chapter 6: Energy (10 exercises)
Solve end-of-chapter questions # 7, 11, 14, 24, 28, 33, 46, 50, 66 and 89.
Student Outcomes : Upon successful completion of this section, the student will be able to:
Perform molarity calculations;
Explain how soluble ionic compounds are dissolved in water;
Recognize soluble vs. insoluble compounds;
Write net ionic equations;
Classify reactions by their type (precipitation, acid-base, gas evolution, redox);
Find the oxidation number of atoms in given compounds;
Explain the difference between temperature and heat;
Perform heat and spec i f i c h e a t c a l c u l a t i o n s ;
D r a w h e a t v s . T d i a g r a m s ;
U s e t h e F i r s t L a w o f T h e r m o d y n a m i c s t o c l a s s i f y c h e m i c a l r e a c t i o n s i n e x o t h e r m i c v s . e n d o t h e r m i c r e a c t i o n s ;
K n o w w h a t i s a S t a t e F u n c t i o n ;
P e r f o r m e n t h a l p y ( DH ) c a l c u l a t i o n s u s i n g t h e H e s s s L a w a n d u s i n g standard enthalpy of formation values.
Chapters 5 and 6 are included in Exam II.
Chapter 7: Atomic Structure (10 exercises)
Solve end-of-chapter questions # 2, 10, 23, 32, 34, 48, 60, 66, 70, and 78.
Chapter 8: Electron Configuration (12 exercises)
Solve end-of-chapter questions # 1, 4, 20, 32, 34, 41, 44, 55, 57, 58, 70, and 72.
Chapter 9: Bonding (12 exercises)
Solve end-of-chapter questions # 2, 15, 19, 32, 42, 43, 45, 53, 60, 66, 80, and 96.
Chapter 10: Molecular Orbitals (8 exercises)
Solve end-of-chapter questions # 9, 23, 26, 28, 46, 52, 54, and 55.
Chapter 11: Carbon Compounds (6 exercises)
Solve end-of-chapter questions # 13, 14, 16, 64, 86, and 89.
Student Outcomes : Upon successful completion of this section, the student will be able to:
Perform frequency/wavelength calculations;
Know the electromagnetic spectrum;
Identify quantum numbers and give their meaning;
Know the types of orbitals and how they are represented by quantum numbers;
Find valance electrons of atoms;
Write electronic configurations of atoms and ions or find the atom or ion form the electronic configuration;
Explain the periodic trends: AR, IE, EA and the relations between them;
Draw Lewis dot structures and give the electronic and molecular geometry of simple molecules or ions using VSEPR theory;
Identify different types of bonds;
Use the periodic table to predict properties applying periodic trends;
Classify substances as polar or nonpolar;
Perform enthalpy calculations using bond strength data;
Give the hybridization of the center atom in simple molecules or ions based on MO;
Identify the types of organic groups;
Know the properties of carbohydrates and polymers.
Chapters 7-9 are included in Exam III.
Chapter 12: Gases (14 exercises)
Solve end-of-chapter questions # 4, 5, 11, 16, 20, 27, 31, 33, 46, 66, 84, 90, 97, and 100.
Chapter 13: Intermolecular Forces (12 exercises)
Solve end-of-chapter questions # 2, 6, 7, 23, 32, 33, 38, 39, 44, 50, 68, and 75.
Chapter 14: Solutions (8 exercises)
Solve end-of-chapter questions # 5, 8, 46, 50, 52, 66, 97, and 102.
Student Outcomes: Upon successful completion of this section, the student will be able to:
Explain the KMT of gases;
Perform calculations using gas laws equations;
Describe properties of gases;
Identify the types of intermolecular forces present in various chemicals;
Describe properties of liquids (especially water);
Classify substances as solids, liquids, or gas;
Classify solids by their type;
Draw simple unit cells;
Perform molality calculations;
Perform calculations for the colligative properties and their applications.
Chapters 1-14 are included in the Final Exam.
Instructions for Bibliographic Research Team Project:
Form groups of 4 to 5 students with the team leaders if you do not find a group, youll be assigned to one. Each group will be assigned one of the topics listed and the group will decide how to do a bibliographic investigation on it. This means each team should get organized by giving different activities to each member (find information, type information, check overall report, etc.). Each report should have references: at least two books (one may be your textbook), as many as needed scientific journals, and no more than two electronic (websites) references. A library technician will visit our class to give you some hints on how to start a bibliographic research. You are encouraged to contact him/her to find the information you need.
The group will type a report of 4 to 5 pages maximum and the team leader will turn it in class in print (for the 1st set, the due day is Tuesday Sep 9) and send it to the instructor (HYPERLINK "mailto:ldelagarza@valdosta.edu"ldelagarza@valdosta.edu) electronically before 11 AM of the due date. The team leader may submit a draft of the report to the instructor for suggestions (please bring a printed copy during office hours for review). Use the Times New Roman font size 12 and 1.5 line spacing with 0.75 for all margins and submit as a .doc or .docx document. The report should include:
A presentation page with title and names of the members of the group (listed alphabetically). (first page)
Introduction
Report
Conclusions (Introduction, report, and conclusion should take 4 to 5 pages)
References (last page)
If images are used in the report, they should have a description (like the figures in your textbook) and they should be mentioned in the main report. A figure should take no more than 1/4 of the page (this space will not count in the 4-5 pages). In the conclusions section please make comments about the information you found. When information is taken directly from a reference, please use text end notes to cite that reference with a subscript number.
The reports will be posted online on the instructors website and each group (all groups in the class) will evaluate the reports and the team leader of each group will give the grades for the reports to the instructor (for the 1st set, the due day is Thursday Sep 17). The grades can go from 0 to 100 and should include an evaluation of why they deserved that grade (what was good, what was bad of the report). If no evaluations of peers reports are submitted by a team, points will be deducted from their own report. If a team starts loosing members, groups with fewer members can get together and form a new team with instructors approval.
First Set: 7 topics, for the first seven groups:
Submit: Tuesday September 9 Evaluate: Thursday September 17
History of the development of the Periodic Table, PT importance to chemists
The International System of Units, how SI units where determined and are defined today
Marie Curie, her history and discoveries, what they imply for us today
Rosalind Franklin, consequences of her work
Mass Spectrometry, a powerful analytical technique, the newest applications and developments
Avogadros number, who found it, what is it used for
Water, why is this small molecule so special
Second Set: 7 topics, for the next seven groups:
Submit: Thursday October 2 Evaluate: Tuesday October 10
A titration experiment, some real life applications
The pH scale, some examples of the extremes
Antioxidants, how do they work?
Corrosion, reactions involved in corrosion, an everyday fight
Energy transformations, from photosynthesis to solar panels
Hydrogen, the fuel of the future
Energy, where should we get it from
Third Set: 7 topics, for the next seven groups:
Submit: Thursday November 6 Evaluate: November 14
Properties of light: reflection, refraction, diffraction, absorption, etc and applications to everyday life
The Bohrs model of atom, which postulates are no longer valid
Louis de Broglie, consequences of his work
The Orbital Types
Gilbert Newton Lewis, consequences of his work
Linus Pauling, consequences of his work
The DNA, how life is defined by 4 letters
PAGE
PAGE 3
End note example.
For format of references, see your book page 292 under suggested readings:
Book:
R. A. Hinrichs and M. Kleinbachl: Energy- Its use and the Environment, 3rd ed. Orlando, Harcourt, 2002.
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WWW:
US Department of Energy: Energy Efficiency and Renewable Energy,
www. eere.nergy.gov/hydrogenandfuelcells. Accessed May 2004.
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