Chemistry
Central College
CHEM 1411- General Chemistry Ir
CRN 67700 - Spring 2011
Central College -Central Campus - Room LHSB408/409| 8:00- 4:00 pm | FriOnly
3 Hour Lecture and 3 Hour Labcourse / 96 hours per semester/ 12 Weeks
Instructor: Ms. Dawn Wittry
Instructor Contact Information: dawn.wittry@hccs.edu / 713-822-3766
Office location and hours
Contact by email/phone
Course Description
CHEM 1411
- Freshman chemistry course for science and engineering majors: General Chemistry I
- Content: Chapters 1-11 (Textbook) + appropriate experiments (Laboratory)
- Mandatory course in order to take Organic Chemistry
- Core Curriculum course
Prerequisites
- One year of high school chemistry
- Must be placed into college-level reading (or take GUST 0342 as a co-requisite) and
be placed into MATH 0312 (or higher) and be placed into college-level writing (or take
ENGL 0310/0349 as a co-requisite)
Course Goal
1. To provide the student a basic and practical understanding of chemistry (formulas,
reactions, and calculations) and recognize its relevance in our daily lives.
2. To prepare our students to meet with success in higher level chemistry and other
science courses when they transfer to four-year universities.
3. To prepare our students for professional programs requiring a mastery of General
Chemistry and Organic Chemistry, such as Nursing, Medicine, Dentistry, and
Pharmacy.
Student Learning Outcomes
The student will be able to:
1. Give names and formulas of elements, ions, and ionic and molecular compounds.
2. Categorize, complete, and balance chemical reactions.
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3. Perform chemistry calculations involving reaction stoichiometry and energy changes.
4. Relate the properties of electromagnetic radiation (frequency, wavelength, and
energy) to each other and to the energy changes atoms undergo which accompany
electronic transitions.
5. Identify the parts of the periodic table and the trends in periodic properties of atoms.
6. Relate the properties of gases with the gas laws and extend the application of these
relationships to reaction stoichiometry, gas mixtures, and effusion/diffusion of gases.
7. Depict chemical bonding with dot structures and valence bond theory and determine
the molecular shapes (geometry) of molecules based on VSEPR and valence bond
theory.
Learning objectives
Students will:
1. Give names and formulas of elements, ions, and ionic and molecular compounds.
a. Given the name, identify the formula and charge of positive and negative ions, and
vice-versa.
b. Given the name, write the formula of ionic compounds, binary molecular compounds,
and acids. Given the formulas of these types of compounds, name them.
2. Categorize, complete, and balance chemical reactions.
a. Identify given reactions as combination, decomposition, single displacement, and
double displacement.
b. Starting with the reactants, complete the reaction by writing the reaction products.
c. Given the reactants and products, balance the equation for the reaction.
3. Perform chemistry calculations involving reaction stoichiometry and energy changes.
a. Convert amounts in units of mass or volume to moles, and vice-versa.
b. Given the amount of one substance in a reaction, calculate the amount of the other
substances that react and form.
c. Identify the limiting reactant and excess reactant in a reaction where more than one
reactant amount is given.
d. Determine the amount of the excess reactant that remains as unreacted excess.
e. Calculate energy changes associated with chemical reactions using Hess's law,
standard enthalpies of formation, or calorimetry.
4. Relate the properties of electromagnetic radiation (frequency, wavelength, and
energy) to each other and to the energy changes atoms undergo which accompany
electronic transitions.
a. Relate frequency, wavelength, and the speed of electromagnetic radiation.
b. From the frequency or wavelength of electromagnetic radiation, calculate its energy.
c. Relate the energy change in the hydrogen atom to its electronic transitions using the
Bohr model.
d. Identify and relate the four quantum numbers that can be associated with electrons.
e. Write the electronic configurations of atoms and ions, including the box diagram
method.
5. Identify the parts of the periodic table and the trends in periodic properties of atoms.
a. Identify the common regions of the periodic table. Identify by name selected groups
of elements in the periodic table.
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b. Using the periodic table, identify the trend (increasing or decreasing in value) of
selected properties of atoms such as atomic radius, ionization energy, and electron
affinity.
c. Identify reaction similarities of elements within the same group in the periodic table.
6. Relate the properties of gases with the gas laws and extend the application of these
relationships to reaction stoichiometry, gas mixtures, and effusion/diffusion of gases.
a. Relate and calculate the pressure, volume, temperature, or amount of gas using
Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, the combined gas law,
and the ideal gas law.
b. Perform stoichiometry calculations which involve gaseous substances.
c. Use Dalton's law and Graham's law to perform calculations involving gaseous
mixtures and effusion and diffusion of gases.
d. Explain the assumptions of the kinetic-molecular theory of gases.
7. Depict chemical bonding with dot structures and valence bond theory and determine
the molecular shapes (geometry) of molecules based on VSEPR and valence bond
theory.
a. Draw the Lewis dot structure of molecules containing two or more atoms.
b. Based on the dot structure of the molecule, determine its electron domain geometry
and molecular geometry based on VSEPR theory.
c. Given the dot structure, identify the hybridization of and geometry about each atom.
d. Explain the nature of sigma and pi bonding using hybrid atomic orbitals.
8. Perform, understand, and report the results of laboratory experiments, including the
use of sophisticated instruments, in a safe environment..
SCANS or Core Curriculum Statement and Other Standards
Credit: 4 (3 lecture, 3 lab)
Science and engineering majors study atomic structure, chemical reactions,
thermodynamics, electronic configuration, chemical bonding, molecular structure,
gases, states of matter, and properties of solutions. The laboratory includes appropriate
experiments. Core Curriculum Course. Note: only one of CHEM1305, CHEM1405, or
CHEM1411 can be used toward associate degree in natural science.
12 WEEKS CALENDAR
Date
Lecture
Lab
Feb 18
Syllabus, Ch. 1 & 2
Rules & Safety
Feb 25
Ch. 3, Review for Test 1
Exp. 1
Mar 4
Test 1 (Ch. 1-3)
Exp. 2
Mar 11
Go over Test 1
Ch. 4 & 5
Homework
Ch. 1, Ch. 2, Prelab 1
Ch. 3, Lab 1, Test, Prelab 2
Lab 2
Ch. 4, Ch. 5, Prelab 3
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Mar 18
SCHOOL CLOSED - SPRING BREAK
Mar 25
Ch. 6, Review for Test 2
Exp. 3
Apr 1
Test 2 (Ch. 4-6)
Exp. 5
Apr 8
Go over Test 2
Ch. 7 & 8
Apr 15
Ch. 9 & 10
Apr 22
SCHOOL CLOSED - EASTER HOLIDAY
Apr 29
Test 3 (Ch. 7-10)
May 6
Lab 5
Ch. 7, Ch. 8
Review for Test 3
Go over Test 3
FINAL EXAM
Friday, May 13
Ch. 6, Lab 3, Test, Prelab 5
Ch. 11, Exp. 6 & 8
Final Exam Review
Final Exam (Chapters 1-11)
8:00
Ch. 9&10, Test, Prelab 6&8
Ch. 11, Labs 6 & 8
Study Final
LHSB408
*This is a proposed schedule. Adjustments made will be discussed in class in the
event of change.
Instructional Methods
Lectures, covering Chapters 1-11 from the Textbook, homework problem sets, assigned
laboratory experiments, three exams plus one final exam.
Student Assignments
Chapters 1-11 from the Textbook
Problem Sets for each Chapter
Midterm Exam
Three regular exams to be given during the course: Chapters 1-3, Chapters 4-6, and
Chapters 7-11. For full credit, all work must be shown.
THERE ARE NO MAKE-UP EXAMS.
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Final Exam
Comprehensive, Departmental Final Exam to cover Chapters 1-11.
Approximately 67% Multiple Choice, 33% Calcualations (show work).
Laboratory
Assigned Experiments from the Lab Manual
Upon entering the lab, students are to submit the Pre-Lab Questions for the scheduled
experiment.
Experiments will be performed in groups of 3-4.
Any student arriving 20 minutes after the start of lab will not be allowed to perform the
lab.
Students must practice safe laboratory habits or they will not be allowed to remain in the
lab.
The completed laboratory report will be due the following class meeting.
NO LATE LABORATORY REPORTS WILL BE ACCEPTED.
There are NO MAKE-UP LABORATORIES. One lab grade will be dropped.
Assessments
Three regular tests, with the lowest grade dropped.
Chapters 1-11 problem sets, attendance, and participation.
Laboratory reports.
Final Exam.
Instructional Materials
Textbook: Raymond Chang, Chemistry, 10th Edition.
Lab Manual: Yiyan Bai, et. al. Chemistry 1411/1412 Laboratory Manual with
Instrumental Analysis. 2nd Edition (2010).
Safety Goggles (safety glasses are NOT acceptable).
Calculator with exp and log functions (cell phones will NOT be allowed as calculators on
tests)
HCC Policy Statement - ADA
Any student with a documented disability (e.g., physical, learning, psychiatric, vision,
hearing, etc.) who needs to arrange reasonable accommodations must contact the
Disability Services Office at the respective college at the beginning of each semester.
Faculty is authorized to provide only the accommodations requested by the Disability
Support Services Office.
To visit the ADA website, visit www.hccs.edu, click Future Students, scroll down the
page, and click on the words Disability Services.
For questions, contact a disability counselor at 713-718-6164, or the District ADA
Coordinator at 713-718-5165.
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HCC Policy Statement: Academic Honesty
See the Student Handbook at www.hccs.edu/hccs/current-students.
Cheating on a test includes:
copying from another student or using unauthorized materials on the test.
Plagiarism is any submission by a student not authored by that student (copied from a
source or another student).
Collusion : group work will be utilized in both lecture and lab; however, submissions
should be the thoughts and work of the student whose name is on the submission.
HCC Policy Statements
HCC Course Withdrawal Policy
Thursday April 21 is the last day for administrative/student withdrawals. Beginning Fall
2007, the State of Texas imposed penalties on students who drop courses excessively.
Students are limited to no more than SIX total course withdrawals throught their
educational career at a Texas public college or university.
If you have any issues, contact your professor regarding your academic performance.
You may also want to contact your academic advisor or counselor to learn about helpful
HCC resources (e.g., online tutoring, child care, financial aid, job placement, etc.).
All students are expected to attend classes regularly. HCC may drop students for
excessive absences without notice. However, it is the responsibility of the student to
drop a course by the deadline in order to receive a W rather than an F (if the student
has a failing average).
Repeat Course Fee
Students who repeat a course for a third or more times may soon face significant
tuition/fee increases at HCC and other Texas public colleges and universities.
Classroom Behavior
Students are expected to participate in group activities including all experiments.
Students should not exhibit any behavior that would detract from the ability of other
students to comprehend the lecture/lab materials. Only students who follow the safety
guidelines will be allowed to perform experiments.
Use of Camera and/or Recording Devices
No recording devices are allowed unless authorized by our Disability Support Office.
Instructor Requirements
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As your Instructor, it is my responsibility to:
summarize the content for General Chemistry I, utilizing methods which will assist
student comprehension. I will also enable excellence in the laboratory, encouraging
understanding of the methods and content of experiments we perform. I will devise
appropriate instruments to assess student comprehension and assign grades
accordingly.
To be successful in this class, it is the student’s responsibility to:
Attend class, pay attention to lectures, participate in group work and in experiments,
complete and turn in homework and lab reports, prepare for and pass exams. Student
work MUST be turned in by the due date and time.
Hints for success:
- Plan to study at least 2 hours for each hour of lecture time (8 hours per week)
- Seek a tutor if needed
- Come to class - be ON TIME and ready to work
- Bring your calculator to lecture and lab and know how to use it
- Read the chapter summary prior to lecture and work through sample exercises
- Complete problem sets for each chapter and turn it in
- Complete all work and turn it in ON TIME - NO LATE WORK WILL BE GRADED
- Prepare for labs by completing the Pre-Lab, for safety and efficiency
NOTE: Students will be given credit only for independent work. In the case of copying,
neither student will receive credit.
Program/Discipline Requirements
The final exam is mandatory, comprehensive, and departmental.
Grading
All exams and lab reports will be graded on a 100 point scale, as a percentage correct.
Homework will be graded as 100 (check), 80 (check minus), 50, or 0.
Grading Scale
A 90-100
B 80-89
C 70-79
D 60-69
F <60
Grading Percentages
2 Regular Exams (3 given, 1 is dropped)
Labs (1 is dropped)
Homework and participation
Final Exam
45%
20%
10%
25%
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