Chemistry 102 – General Chemistry
Spring 2012
Professor Farah Firtha 
ffirtha@msjc.edu
951-639-5743
Description: This class is a continuation of Chemistry 101. Special emphasis is given to
chemical kinetics and equilibrium, thermodynamics, acid- base equilibria, electrochemistry,
common reactions of metals and non-metals with an introduction to qualitative analysis.
Office Hours: Office-LRC 806. Hours- M 12:30-1:30pm. Tue 9:30am-12:30pm. W 12:30-1:30pm.
Also by appointment and after class. You are encouraged to meet with me if you have any questions
regarding the lecture, homework, tests, labs, or your performance in the course. When you contact the
instructor please use Chem 102 in the subject. Emails without this subject may be overlooked.
Prerequisite: Chemistry 101
Requirements: You must have an active email account for this class. If you do not the college can
issue you one and you may use the computers in the library to access your account. You may also need
to gain access to Blackboard for course material at my.msjc.edu Blackboard allows you to easily
communicate with your instructor and fellow students. I will post power-point lectures and handouts on
blackboard usually under course documents; you can find your current points on blackboard under
tools; important announcements can be found on the home page of blackboard. If you took math or
chemistry awhile ago I suggest watching videos on Khan Academy.org to refresh your memory.
Resources:
Khanacademy.org a free university…sort of. You tube video lectures on many topics… including
chemistry.
Mastering chemistry if you bought the book new then you have access to this website. It has more
quizzes and other helpful resources.
Smarthinking an online tutoring (usually 24/7), yes they have chemistry. You can access this in
blackboard under tools.
Texts: Chemistry: A Molecular Approach , Nivaldo J. Tro. 2nd ed.
Chemistry 102 Lab Manual, Mary Bodo
Chemistry Study Guide, Nivaldo J. Tro. Recommended
Supplies: A non-graphing scientific calculator, closed-toed shoes and safety googles.
Lecture: T TH 12:30-1:50pm Room 304. Attendance is required to succeed in the course. Each lecture
has a discussion component or demonstration and may be more in-depth than the material presented in
the text. If you must miss a lecture, please inform me beforehand, if possible, and copy the notes from a
member of your study group. You are responsible for any information you missed. In general, late
work is not accepted and missed assignments cannot be made-up.
Laboratory: T TH 2-5pm Room 306. Laboratory is an integral part of the course; it is important to
arrive on time as important safety information and demonstration of procedures may take place at the
beginning of the lab period. If you are late, you may not be able to perform the experiment and will
receive a zero for that laboratory. The experiments are designed to enhance and extend your
understanding of concepts discussed in lecture and students should read the assigned experiment before
the lab meeting. Students must attend lab and cannot receive credit by ‘borrowing’ experimental data
from others. Usually, lab reports are due at the end of each lab period and the pre-labs or assignments
are due at the beginning of the lab period. Work due during a lecture or lab time is late at the beginning
of the assigned period. In general, late work is not accepted and missed labs cannot be made-up. Please
meet with me to discuss any situation that may arise that will preclude your attendance. I am in the lab
to help you, but I will not do the lab for you.
You must do the laboratory, the lab report, and the pre-labs to receive credit for each lab grade.
CAUTION: Lab partners may share data, but they are not allowed to turn in the same lab report.
Any student who misses more than TWO labs may be automatically dropped from the course or given
a failing grade. The lab portion of your grade is calculated after dropping the one lowest lab grades of
the semester. Most labs are worth 15 points. Two-day labs are worth 25 points and QUAL IV is worth
35 points. Points will be deducted if lab groups become greater than 3 students.
Lab safety: You are required to wear safety glasses, closed toes shoes and attire that protects your legs. I
reserve the right to dismiss you from lab if you do not wear the proper attire and you will receive a zero
for that lab. COME PREPARED.
Study: The main point of this course is to guide your development of critical thinking processes as they
pertain to the study of Chemistry. For you to succeed in this course you must practice the concepts
covered and prepare for each class. Before each lecture, read the material to be covered. Do not spend
too much time on any one point; simply obtain an overview of the relevant topics to be covered. After
lecture, reread the material more critically referring to your notes for difficult concepts. Try the
assigned exercises and review at the end of each chapter. You may want to wait a day or more after
reading the chapter to attempt the exercises in the back of the chapter. Waiting will test your retainment
of the material. Discuss the concepts and exercises with your weekly study group. If you have trouble
with a particular concept or assignment, ask for help in class or come to my office. You are encouraged
to utilize the facilities available on campus including the Learning Resource Center.
Do not try to just memorize material. THINK about the material!! Does the material make sense?
Is the material related to what you already know? Many concepts or problems may seem difficult,
but are rather simple when related to what you already know.
Tests: There will be FOUR, 100 point tests during the semester and a comprehensive, 200 point final
exam. Missed tests cannot be made-up and every test day will be announced the first week of class. All
test questions are based on lecture, assigned reading, homework and laboratory work. Missed tests
cannot be made-up unless arrangements are made with the instructor PRIOR to the exam date.
Arrangements may be made in person or by phone. However, phone messages are not acceptable. It is
the responsibility of the student to get in touch with the instructor. Every test day will be announced the
first week of class. These tests are closed book. During the test no cell phones or PDAs can be in use.
There will be no trips outside the classroom during the test so plan accordingly.
 Do not wait until the day before the exam to study the material. There will be POP quizzes
throughout the semester, so always study the material.
Quizzes: There may be a quiz or a test almost every week. Quizzes will be based on assigned
homework and lecture material. If you have completed and understood the homework and practice
problems in class, the quizzes should be straightforward.
Participation Points:
Book Homework: Homework may be periodically collected. You will be given a one day
notice of collection
Projects/ Assignments: There will be various assignments through-out the semester.
Student Behavior: A student who has not attended class for a total of 4 class meetings may be dropped
from the class. Any disruptive behavior, including cell-phones and beepers, will not be tolerated in class
and may result in dismissal from the class. During Exams, everything must be removed from your
surrounding area. You will be required to put your backpacks and notebooks in the front of class during
the exam. A student cheating on any assignment, including plagiarism, will receive a zero on that
assignment and may be referred to a disciplinary hearing and/or receive an F in the class. Also, it is the
student’s responsibility to withdraw from class.
HOW TO TURN IN ASSIGNMENTS: please SEPARATE each assignment into piles. You may receive
a zero on an assignment if I did not see it because it was stapled to another assignment. Assignments are
due at the beginning of the classes. Pre-lab assignments are due at the beginning of the class. Lab
reports are due at the end of the lab period.
Grading: A ten-point scale will be used for grading as shown below:
A: 90-100%, B: 80-89%, C: 70-79%, D: 60-69%, F: Below 60%.
POINT SUMMARY
TEST 1 100 points
TEST 2 100 points
TEST 3 100 points
TEST 4 100 points
Scores above = 400 points
16 graded labs = 320pts total
Participation/ Hwrk/ Pop quiz points=80pts
Final Exam = 200 points
 It is the responsibility of the student throughout the semester to maintain knowledge of their
current grade.
In order to receive a grade of C or better, your overall lecture average (tests, quizzes
and final exam) must be higher than 65%. Even if your overall average (including labs
and extra credit) in the class is 70% or better, if your lecture average is less than 65%
you will receive a D letter grade.
This syllabus is subject to change without notice per the discretion of the instructor.
A Few Support Services (there are many more available on campus)
Mt. San Jacinto College abides by the Americans with Disabilities Act and Section 504 of the
Rehabilitation Act of 1973 that prohibits federal and state agencies or programs from discriminating
against qualified individuals with disabilities. Students in this course who have a documented disability,
that limits a major life activity which may have some impact on your work in this class and for which
you may require accommodations should meet with a counselor in Disabled Students Services and
Program(DSP&S) as soon as possible.
Learning Center has tutors available.
STEM Program MSJC has been awarded funds to strengthen the Science, Technology, Engineering
and Math programs on campus.
Learning Communities Create a community with your fellow students and take classes together.
Disabled Student Programs and Services can help students with physical, learning or mental
disabilities.
EOPS provides support services for financially disadvantaged students and first-generation college
students.
Child Care is made available through the Child Development Center.
The Writing Center helps students with writing assignments in any subject.
The Counseling Department can assist you in developing your academic goals or personal counseling.
Puente Program
Student Life Join a club. Studies show that students who are active on campus and participate in a club
have higher grades 
Outline of Lecture Topics CHEM 102 1-12-12 ffirtha@msjc.edu
This is a tentative schedule. I will try to stay as close to this schedule as possible, but we may be
slightly ahead or behind. Homework will be assigned in class on the first day we begin each chapter. If
you have a documented disability please see me or a DSPS Counselor so that appropriate
accommodations can be made.
LECTURE SCHEDULE
Days
Day
Topic
T Jan24
Review. Reading tips.vocab
TH Jan 26
More Vocab, Intro to Chp 11
T Jan 31
Chp 11: Intermolecular forces
TH Feb 2
Chp 11:Phase diagrams and crystal structures
T Feb 7
Chp 12 : Solutions
TH Feb 9
Chp 12: Solubility and colligative properties
T Feb 14
Chp 12 , review
TH Feb 16 REVIEW and intro to Chp 13
T Feb 21
Chp 13: Reactions rates and orders
TH Feb 23
Chp 13: Reactions Mechanisms
T Feb 28
Chp 13: Catalysis
TH Mar 1
Chp 14: Equilibrium
T Mar 6
Chp 14: Le Chatelier's principle
TH Mar 8
Chp 14: Factors effecting Le Chatelier's
T Mar 13
Chp 14, REVIEW
TH Mar 15 REVIEW, Chp 15 intro
T Mar 20
Chp 15: Acid and Base properties
TH Mar 22
Chp 15: pH scales
T Mar 27
Chp 15: Disassociation
TH Mar 29
Chp 15: Factors effecting pH
Apr 3 to 5
NO LAB
SPRING BREAK
T Apr 10
Chp 16: Solution Equilibrium
TH Apr 12
Chp 16: Buffers
T Apr 17
Chp 16: Solubility Equilibrium
TH Apr 19
Chp 16 : Solubility Product
T Apr 24
Chp 16, REVIEW
TH Apr 26 REVIEW, Chp 17 intro
T May 1
Chp 17: Chaos and Entropy
TH May 3
Chp 17: Free Energy and equilibrium
T May 8
Chp 18: Electrochemical Cells
TH May 10
Chp 18: Batteries
T May 15
REVIEW, Finish chp 18?
TH May 17
Review
T May 22
Review
Final Exam TUESDAY MAY 29 at 12pm
TENTATIVE LAB SCHEDULE Chem 102 ffirtha@msjc.edu
1-10-2012
PRE-LAB DUE THE SAME DAY OF LAB. REPORTS ARE DUE THE END of LAB.
DATE
T Jan24
TH Jan 26
T Jan 31
TH Feb 2
T Feb 7
TH Feb 9
T Feb 14
TH Feb 16
T Feb 21
TH Feb 23
T Feb 28
TH Mar 1
T Mar 6
TH Mar 8
T Mar 13
TH Mar 15
T Mar 20
TH Mar 22
T Mar 27
TH Mar 29
Apr 3 to 5
T Apr 10
TH Apr 12
T Apr 17
TH Apr 19
T Apr 24
TH Apr 26
T May 1
TH May 3
T May 8
TH May 10
T May1 5
TH May1 7
T May 22
LAB (points)
Safety Discussion/ check into lockers
Acid Base Titrations (15pt)
Analysis of Consumer Bleaching Agents(15pt)
Preparation of Alum using Aluminum Cans(25pt)
Preparation of Alum Cont’
Gravimetric Analysis(15pt)
Molar Mass of a Solid(15pt)
Exam 1 (Chp 11 and 12)
Lecture, Preface to qualitative Analysis
Common Anions (15pt)
Factors Affecting Reactions Rates (15pt)
Chemical Kinetics (25pt)
Chemical Kinetics
Equilibrium Exercise (15pt)
Equilibrium and Le Chatelier’s Principle(15pt)
Exam 2 (Chp 13 and 14)
Solubility Product of Silver Acetate (25pt)
Solubility Product of Silver Acetate Cont’
Acid/Base Buffers (25pt)
Acid/Base Buffers Cont’
NO LAB
SPRING BREAK
Qual I (25pt)
Qual I Cont’
Qual II (25pt)
Qual II Con’t
Qual III (15pt)
Exam 3 (Chp 15 and 16)
Work on Lab Practicum Procedures
Qual IV- Unknown Examination (35pt)
Lecture/Review
Electrochemistry- Galvanic cells (15pt)
Exam 4 (Chp17 and 18)
Review for Final and locker check-out
Review Exam 4
Final Exam TUESDAY MAY 29 at 12pm
Prelab
Chapter Homework Assignments 2nd ed.
These will help prepare you for the tests. Some of this may be collected.
Book work C102 Ed 2
Learning Objectives
1. Describe:
- the various types of intermolecular forces.
- the difference between an amorphous and crystalline solid.
- how intermolecular forces effect physical properties
- three types of unit cell lattice structures.
2. Describe:
- the relationship between vapor pressure, enthalpy of vaporization and boiling point.
- how boiling points, freezing points and osmotic pressures of electrolytic and nonelectrolytic solutions change with solution composition.
Calculate:
- molarity, mass percent, normality and molality for various solutions.
- changes in colligative properties and determine solute molecular weights when given
appropriate colligative property data.
Evaluate:
- how structural factors of substances and their temperature and pressure would
affect its solubility in a given solvent.
- phase diagrams, cooling curves and heating curves.
3. Determine:
- the rate law of a chemical reaction if supplied changing concentration versus time
data.
- graphically, the reaction order when given experimental data of
concentration versus time.
- the half-life of a reaction if given concentration versus time data.
- the overall reaction and rate expression when provided the reaction mechanism.
- the activation energy of a reaction graphically or by calculation when given rate
constant versus temperature data and distinguish between homogenous and
heterogenous catalysis.
4. Calculate:
- equilibrium concentrations for a reaction system using the concept
of mass action.
Predict:
- using LeChatelier's principle, a shift in direction of a chemical
reaction with changes of pressure, temperature and concentration.
5. Determine:
- the pH of weak and strong acid, base and salt solutions.
- percent dissociation using the concepts of equilibrium.
- how molecular structure effects acid and base properties.
6. Determine :
- the pH and change in pH of various buffer solutions.
- the solubility and equilibrium constant of a salt when given appropriate data
- the proper indicator to be used in a titration.
- how changing pH and the common ion effect will effect the solubility of a salt.
Construct:
- titration curves for a weak acid and strong base titrations, strong acid and weak base
titrations.
7. Determine:
- using the Second Law of Thermodynamics, the direction of entropy changes for
chemical and physical systems
- whether a physical or chemical system will be spontaneous or non-spontaneous using
Free Energy tables
8. Calculate:
- the cell emf using the Nernst equation given the concentrations or pressures and
temperature of the cell components.
- the time or mass for product deposition in an electrolytic process.
Construct:
- a diagram of an electrochemical cell, given the cell line notation and determine if the
cell reaction is spontaneous or non-spontaneous
Outline
11. Intermolecular Forces of Liquids and Solids
- intermolecular forces
- the liquid state
- crystal structure
- x-ray diffraction of crystals
- phase changes and phase diagrams
12. Physical Properties of Solutions
- a molecular view of the solutions process
- solution compositions and concentration units
- energies of solution formation
- factors affecting solubility
- colligative properties of electrolytic and non-electrolytic solutions
13. Chemical Kinetics
- reaction rates
- rate laws
- first order and second order reactions
- activation energy and temperature dependence of rate constants
- collision theory and the Arrhenius equation
- reaction mechanisms
- catalysis
14. Chemical Equilibrium
- chemical equilibrium and the equilibrium constant
- Le Chatelier's principle
- factors that effect chemical equilibrium
- solving equilibrium problems
15. Acids and Bases: General Properties
- the nature of acids and bases
- strength of acids and bases
- autoionization and the pH scale
- acid - base properties of salts
- the effect of structure on acid-base properties
- acid-base properties of oxides
- the Lewis acid-base model
16. Applications of Aqueous Equilibria
- solutions of acids or bases containing a common ion
- buffered solutions and buffer capacity
- titration curves
- acid-base indicators
- complex ion equilibria
- solubility equlibria and the solubility product constant
- precipitation and qualitative analysis
17. Spontaneity, Entropy and Free Energy
- spontaneous processes and entropy
- the second law of thermodynamics and spontaneous processes
- free energy
- entropy changes and free energy in chemical reactions
- free energy and equilibrium
18. Electrochemistry
- electrochemical cells and standard reduction potentials
- cell potential, electrical work and free energy
- dependence of cell potential on concentration
- batteries
- electrolysis
Student Learning Outcomes
Chem 102
1. When given initial concentrations or partial pressures of reactants and products, students will be
able to apply the principles of chemical equilibrium to find their final concentrations.
2. Given data of concentration versus time, students will be able to graphically determine if the
reaction is zero, first or second order.
3. Given the crystal structure and edge length of a certain element, the student will be able to
calculate the density of the element.