VALDOSTA STATE UNIVERSITY
Chemistry Department
Summer 2009
Course Prefix and Number: CHEM 1211, Principles of Chemistry I
Contact/Credit: 3 lecture/3 credit hours
This course is a 3 hr credit course; you need to dedicate 4 hrs per each credit hour, 3 x 4 = 12.
Because in summer there is less time than in a regular semester, this is an intensive course where you
are expected to dedicate about twice the time (24 hrs): ~5 hours we spend in class, you have 19 hr to
study at home, about 4 hr x 5 times / week.
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.
Co-requisites: MATH 1111 (OR MATH 1113) & CHEM 1211L
Class Location: BSC 3017
Class Times/Days: M-Th, 12:45 – 2:10 pm
Instructor:
Telephone Number: (229) 333-5340
email: ldelagarza@valdosta.edu
website: www.valdosta.edu/~ldelagarza
Dr. de la Garza
Office Location: BSC 3080
Office Hrs./Days:
M, W: 2:15-2:45 pm
Any other time by appointment
Required Textbook: CHEMISTRY and CHEMICAL REACTIVITY, Kotz, Treichel, Weaver 7th Ed.
Additional required Materials: OWL access code (https://owl1.thomsonlearning.com/), instructions
for signing in are in Dr. de la Garza website, register ASAP; calculator.
Student Outcomes*: Upon successful completion of this course, the student will be able to:
1- Determine the moles and masses of substances consumed or produced in a chemical reaction by
using a balanced chemical equation.
2- Predict the structure of a molecule and its hybridization based on its chemical formula.
3- Determine the number of protons, neutrons and electrons in an atom or ion using the periodic table.
4- Identify changes in physical and chemical properties of the element by using the periodic table.
5- Predict the products of fundamental metathesis and oxidation-reduction reactions.
6- Calculate the enthalpy change of a reaction by using the thermodynamics table.
7- Name inorganic compounds or (exert original text) of a name using IUPAC rules.
* Refer to specific student outcomes for each chapter in pages 3-4 of this syllabus.
Course Requirements:
1-Partial tests: 3 exams will be administered. Please keep up with the material so you don’t get
overwhelmed. Also, the material covered in previous chapters is used later on: study from the
beginning and don’t skip material.
2- Final exam: the final exam will be given in two comprehensive exams; one of them is a standard
test that will contain general and very basic questions of the covered material. Students who do not
take the final exams will fail the course (F), students who make 35% or less on either exam 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).
3- Homework: 14 required OWL assignments (online - homework tutors) 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.
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4- Quizzes: ~6 quizzes will be given throughout the semester with concepts and topics to be addressed
in tests.
5- Participation: collaboration on discussion, answering questions, asking questions, solving problems,
etc. is part of everyday class activities.
6- Written report: essay on chemistry, chemistry personalities, and current issues. All reports will be
published online and graded by the peers and instructor. Complete instructions on separate handout.
Academic Honesty: Academic honesty will be enforced. Any plagiarism, fraud, or cheating will result
on a 0 (zero) in the project, homework, test, essay, etc. and it will be reported to the Student Conduct
Office in the Dean of Students Office and will be kept on student’s records. Information about policies
and procedures at: http://www.valdosta.edu/academic/AcademicHonestyPoliciesandProcedures.shtml
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 VSU
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.
Evaluation of Performance:
42% = Three partial exams (14% each exam)
20% = Final exam (two parts will be averaged)
12% = Written report
14% = OWL Homework (1% each chapter)
6% = Participation
6% = Quizzes
100 + up to 10 extra points (for 80% OWL extra point problems)
Grading Scale:
Grade
A
B
C
D
F
Numerical Points
90 and higher
80-89
70-79
60-69
59 and lower
Course Outline and Tentative Schedule (subject to change):
Week of
June 8
June 15
June 22
June 29
July 6
July 13
July 20
July 27
Lecture
Assignments due (OWL Chapters)___
Basic Concepts & Tools / Interchapter p. 338
Ch 1, Tools due Mon Jun 15
Atoms, Molec & Ions / Chem Reactions
Ch 2 due Wed Jun 17, 3 due Mon Jun22
Chem Reactions / Stoichiometry
Ch 4 due Tue Jun 30
Stoichiometry / Energy
Ch 5 due Mon Jul 6
Structure of Atoms / Periodic Trends
Ch 6 due Fr Jul 10, 7 due Tue Jul 14
Bonding & Structure / Hybrid & Molecular Orb
Ch 8, 9 due Mon Jul 20
Ch 10** due Th Jul 23
Gases / Intermolecular Forces & Liquids
Ch 11, 12 due Mon Jul 27
Solids / Solutions
Ch 13, 14 due Wed Jul 29
** Chapter 10 is recommended reading / OWL hmk required.
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. Very important labs for class will
be posted on my website. Student Success Center has tutors available: http://www.valdosta.edu/ssc/
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Exam dates
EXAM I will be given on Tuesday June 23, 2009 (chapters 1, Tools, 2 and part of 3)
EXAM II will be given on Wednesday July 8, 2009 (chapters 3, 4, 5)
EXAM III will be given on Tuesday July 21, 2009 (chapters 6, 7, 8, 9)
FINAL EXAM Part 1 will be given on Wednesday July 29, 2009 (comprehensive)
Part 2 will be given on Thursday July 30, 2009 at 2 to 4 pm (comprehensive).
Make up exams or quizzes will NOT be given. * Any emergency needs to be informed to the Office of
Students Affairs (phone: 333-5359).
Important dates:
Wed Jun 10 - First day of classes
Thursday Jul 2 – Midterm (last day to drop the course)
Monday Jul 6 - No classes
Wed Jul 29 - Last day of classes, final exam (chapters 1 to 14)
Thursday Jul 30 - Final exam (standardized examination – cumulative)
Instructions for Take-home assignments on OWL:
Fourteen (14) OWL assignments are assigned throughout the semester. Only the “End of Chapter
Questions – Homework Tutors” are required, the other OWL exercises are for extra-points or optional.
Submit your answer on the OWL web-site for the corresponding homework tutors 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 or SIMILAR 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 (not guaranteed and in extreme situations you
may submit your written work for credit).
Chapter 1: Basic Concepts (7 exercises)
Study questions Ed 7: on page 20: 2, 4, 6, 8, 10, 19, 37
Let’s Review: Tools (10 exercises)
Study questions Ed 7: on page 43: 3, 10, 14, 16, 18, 20, 32, 34, 40, 60
Chapter 2: Atoms and Elements (26 exercises)
Study questions Ed 7 on page 100: # 2, 4, 5, 8, 10, 15, 21, 23, 29, 33, 35, 36, 41, 43, 49, 51, 53, 55,
57, 59, 61, 67, 71, 76, 105, 141
Chapter 3: Chemical Reactions (24 exercises)
Study questions Ed 7 on page 152: # 2, 4, 9, 11, 13, 15, 19, 21, 26, 28, 33, 34, 37, 39, 41, 44, 45,
46, 48, 52, 63, 68, 73, 76
Specific objectives: Upon successful completion of this section, the student will be able to:
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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;
Recognize ionic vs. molecular compounds;
Recognize polyatomic ions;
Give the names and symbols of elements and
names and formulas of compounds;
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Perform calculations with isotopes and atomic
weight;
Perform % mass composition 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.
Chapter 4: Stoichiometry (18 exercises)
Study questions Ed 7 on page 195: # 2, 5, 8, 12, 16, 19, 29, 37, 39, 41, 46, 47, 54, 55,
62, 67, 71, 106
Chapter 5: Energy (14 exercises)
Study questions Ed 7 on page 242: # 8, 10, 12, 18, 20, 21, 24, 28, 30, 34, 44, 46, 54, 79
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Specific objectives: Upon successful completion of this section, the
1- Perform molarity calculations;
62- Use the mole concept to perform
stoichiometric and limiting reactant
calculations.
783- Explain the difference between temperature
and heat;
4- Perform heat and specific heat calculations;
5- Draw heat vs. T diagrams;
student will be able to:
Use the First Law of Thermodynamics to
classify chemical reactions in exothermic vs.
endothermic reactions;
Know what is a State Function;
Perform enthalpy (H) calculations using the
Hess’s Law and using standard enthalpy of
formation values.
Chapter 6: Atomic Structure (15 exercises)
Study questions Ed 7 on page 297: # 1, 3, 9, 18, 28, 32, 34, 36, 40, 44, 51, 60, 62, 67,
78.
Chapter 7: Electron Configuration (16 exercises)
Study questions Ed 7 on page 332: # 2, 6, 11, 18, 20, 24, 26, 28, 30, 32, 40, 41, 44, 56,
59, 64.
Chapter 8: Bonding (16 exercises)
Study questions Ed 7 on page 395: # 6, 10, 12, 14, 18, 27, 28, 29, 34, 38, 42, 47, 50, 53,
56, 86.
Chapter 9: Molecular Orbitals (10 exercises)
Study questions Ed 7 on page 434: # 3, 4, 11, 12, 14, 22, 23, 34, 44, 54.
Chapter 10: Carbon Compounds (2 exercises)
Study questions Ed 7 on page 488: # 51, 95.
Specific objectives: Upon successful completion of this section, the student will be able to:
1- Perform frequency/wavelength calculations;
10- Identify different types of bonds;
2- Know the electromagnetic spectrum;
11- Use the periodic table to predict properties
3- Identify quantum numbers and give their
applying periodic trends;
meaning;
12- Classify substances as polar or nonpolar;
4- Know the types of orbitals and how they are
13- Perform enthalpy calculations using bond
represented by quantum numbers;
strength data;
5- Find valance electrons of atoms;
14- Give the hybridization of the center atom in
6- Write electronic configurations of atoms and
simple molecules or ions based on MO;
ions or find the atom or ion form the
15- Use the Law of Conservation of Matter to
electronic configuration;
balance chemical equations, specially
7- Explain the periodic trends: AR, IE, EA and the
combustion reactions;
relations between them;
16- Identify the types of organic groups;
8- Use the periodic table to predict properties
17- Know the properties of carbohydrates and
applying periodic trends.
polymers.
9- Draw Lewis dot structures and give the
electronic and molecular geometry of simple
molecules or ions using VSEPR theory;
Chapter 11: Gases (12 exercises)
Study questions Ed 7 on page 546: # 1, 6, 12, 18, 22, 24, 32, 34, 39, 41, 45, 65.
Chapter 12: Intermolecular Forces & Liquids (12 exercises)
Study questions Ed 7 on page 581: # 2, 4, 6, 8, 14, 17, 18, 20, 25, 28, 39, 41.
Chapter 13: Solids (6 exercises)
Study questions Ed 7 on page 581: # 11, 13, 14, 20, 22, 26.
Chapter 14: Solutions (10 exercises)
Study questions Ed 7 on page 648: # 6, 13, 28, 32, 41, 53, 58, 60, 93, 96.
Specific objectives: Upon successful completion of this section, the student will be able to:
1- Explain the KMT of gases;
6- Classify substances as solids, liquids, or
gas;
2- Perform calculations using gas laws
7- Classify solids by their type;
equations;
3- Describe properties of gases;
8- Draw simple unit cells;
4- Identify the types of intermolecular forces
9- Perform molality calculations;
present in various chemicals;
10- Perform calculations for the colligative
5- Describe properties of liquids (especially
properties and their applications.
water);
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