GENERAL CHEMISTRY II (CHM175) SYLLABUS, SUMMER 2015
INSTRUCTOR: Jon Obrecht
OFFICE #: N/A
OFFICE PHONE: N/A
E-MAIL: jobrecht@eicc.edu
ONLINE (eCompanion): http://www.iowacconline.com
OFFICE HOURS: Available by appointment after class
CLASS CANCELATION: For class cancellation information calls 563-441-4001 or visit
www.eicc.edu/students. In case of inclement weather visit our website or call our weather line at 563-4414144
ACADEMIC ACCOMMODATION: Anyone who feels he or she may need an academic
accommodation based on the impact of a documented disability should contact Jan Weis at the Disability
Resources Office by calling 564-441-4027 to arrange an appointment as soon as possible. At the
appointment, course format, individual needs, and potential accommodations will be discussed. This
service is FREE and confidential.
TEXTS: Chemistry; Structure and properties, 1st Ed, by Nivaldo J. Tro. Student’s selected solutions
manual for Chemistry: Structure and Properties. Laboratory Manual (Notes written by R. Ford & J.
Tayh).
LECTURE CONTENT: Chapters: 12-21 (More details are in the handout)
OBJECTIVES: This course is designed for science students to complete part II of general chemistry.
EXAMS: Exams will be on the following dates:
Exam 1 (12-15): June 11
Exam 3 (19-20): July 16
Exam 2 (16-18): July 2
Final Exam (cumulative): July 24
The first three exams will be 100 points each. The final exam will be worth 150 points and will be
comprehensive over the material that has been covered by exams 1, 2, and 3 (chapters 12-21). All exams
are in the multiple choice/true-false formats. There will also be some problem solving on each exam.
The student is not allowed to keep exams. They are returned to the student at the next scheduled
class meeting for discussion, and then they are returned back to the instructor at the end of the
period. Any exam not returned will be recorded as a zero grade.
MAKE-UP EXAMS: Make up of missed exams with a valid excuse (illness or unavoidably absence) are
allowed. Make up for missed exams without a valid excuse are also allowed, but you are going to lose
10% of the grade of the first missed exam, 15% of the second, and 20% of the third. Make-ups for the
first 3 exams must be taken within one week of the scheduled missed exam date with a different format.
It is the responsibility of the student to contact the instructor to arrange for any make ups and to contact
the “Testing Center” in person one day before the scheduled make up.
QUIZZES: Quizzes will be given occasionally, as needed, one before each exam, worth about 20 points
each. Quizzes will make up about 100 points of your final grades.
ELECTRONIC DEVICES: carrying all electronic equipments (cell phones, I-Pad, I-Pod,..) is prohibited
during taking exams and quizzes (except calculators).
LAB: (No make-up) there will be 10 points for each lab session. Lab grades include; the report sheet, and
two lab exams (midterm and a final, each worth about 25 points). Lab's reports must be done
individually and submitted individually, copying from others will be considered as cheating. Lab
reports are due on the first lab meeting after the experiment, and late reports will lose one point/day.
ATTENDANCE: Attendance will be kept for all lectures and labs. If you turned in lab report for
experiment in which you did not attend, you will be given a zero for that experiment and you will lose
another 10 points. There will be a BONUS of 12 points for perfect attendance in the lectures.
LECTURE PROBLEM ASSIGNMENT: I will give you lists of problems to do as a study guide for the
exams. They do not have to be turned in, however, I expect you to do them because they are part of the
NOTES and CLASS (Refer to the solution manual for the answers).
GRADES: Your grades will be based on: examinations, quizzes, and laboratory reports. Your efforts are
needed in order for you to pass this course, but there is NO GRADE FOR EFFORT. It is your
responsibility to check your progress and ask for help when needed. The grading scheme will be as
follows:
Quizzes (5 x 20)
100 points
Exams 1-3 at 100 each
300 points
Final exam
150 points
14 Labs (10 points each)
140 points
Total points
690 points
(A, A-) 100-90% (B+, B, B-) 89-80%
(C+, C, C-) 79-70% (D+, D, D-) 69-60% (F) 59-0%
Are you ready for this class?
If any or all of the following situations apply to you, then you are not ready to take this class;
1) You think that you can pass the class without attending class.
2) Your work (job) does not allow you enough time to study or cause you to miss classes.
3) You think that you are going to pass the class just by showing up and not studying at home.
4) When you need help, you don’t ask for it.
5) You don’t have the intention/determination to pass the class.
6) You did not take CHM I within the last five years.
Study Guide for Chemistry
Before reaching the frustration stage in this class and start blaming others, please do the following;
1) Read from the textbook/notes before you come to class.
2) Read what has been covered in class right after (on the same day).
3) Study the material in details focusing on the concepts that have been covered in class. Make sure
that you understand the examples given in class and textbook.
4) Memorize the new terminology (New vocabulary) by using flash cards or other methods.
5) Do the homework (assigned problems at the end of each chapter) at least twice on different days.
6) If you do bad on the first quiz that means you have to change your studying habit or;
7) This is the right time to ask for help or to complain!! If you complain after this point of time NO
ONE WILL LISTEN TO YOU. If you ask for help later it will be TOO LATE.
8) Ask for help from tutors (available free), your instructor (available free), or other students.
9) If you follow the above steps and still your performance did not improve then you can blame your
teacher and/or the College.
DO NOT wait till the end of the semester to ask for help, because at that time you will blame only
yourself. (IT IS TOO LATE!!)
The equation for “A” grade:
Attending class + Studying on time + Practice the homework + Ask for help  “A” grade
Lab Schedule
06-05-15:
06-12-15:
06-19-15:
06-26-15:
07-03-15:
07-10-15:
07-17-15:
Exp 30: Intermolecular forces (Slime Gel) & Exp 29: Hydrogen bonding
Exp 17: Solutions & Exp 18: Colligative Properties
Exp 19: Rates of chemical reactions & Exp 20: Chemical equilibrium
Exp 21: pH of aqueous solutions & Exp 23: Ka for acetic acid
Exp 25: Ksp for calcium hydroxide & Exp 26: Distillation
Exp 24: Vitamin C & Exp 22: Analysis of Bleach
Exp 27: Electrochemistry & Exp 28: Nuclear Chemistry
Study Guide and Homework of General Chemistry II (175)
Chapter 12

Comparison between; solids, liquids, and gases.

Intermolecular forces, Intermolecular forces in action; surface tension, viscosity, capillary action.

Vaporization and vapor pressure. Temperature effect on vapor pressure and boiling point.

Sublimation and fusion.

Heating curves.
Homework: 13, 15, 16, 17, 19, 24, 29, 33, 35, 37, 39, 41, 43, 45, 47, 49, 53.
Chapter 13

Phase diagrams for different substances.

Crystalline solids, the unit cell.

Types of crystalline solids; molecular, ionic, and atomic.

The structure of ionic solids and Network covalent atomic solids.
Homework: 19, 23, 37, 39, 41, 49, 59.
Chapter 14:

Types of solutions and solubility. Effect of intermolecular forces on solubility.

The energetics of solution formation of solid in liquids, liquids in liquids and gas in liquid.
Saturated, unsaturated, and supersaturated solutions.

Effect of temperature and pressure on solubility.

Expressing Solution concentration: molarity, molality mole fraction, and mass percent.

Colligative properties of nonelectrolytes and electrolytes.
Homework: 25, 27, 29, 31, 37, 39, 47, 49, 51, 53, 55, 57, 59, 63, 67, 73, 75, 77, 79, 81, 83, 85, 87, 89,
93.
Chapter 15

Rates of chemical reactions.

Instantaneous rate, reaction rates and stoichiometry.

Measuring reaction rates.

Rate laws and rate constants and the reaction's order.

Initial rates and the rate laws.

The effect of concentration on reaction rates: Zero, first and second-order reactions.

Integrated rate laws (concentration versus time).

Effect of temperature on reaction rate. Activation energy and collision model.

Reaction mechanisms; unimolecular and bimolecular reactions.

Intermediates and the rate-determining step.

Catalysis. Types of catalysts.
Homework: 27, 29, 33, 35, 39, 41, 43, 47, 53, 55, 57, 59.
Chapter 16

The dynamic equilibrium.

The equilibrium constant (Kc), and reaction Quotient (Q). Expression of Kc for homogenous and
heterogeneous equilibrium.

Calculations of Kc and the of Kc and Qc in calculating the concentrations and prediction the
direction of a reaction.

Factors that affect equilibria: concentration, volume/pressure, temperature, and catalyst.
Homework: 21, 23, 25, 27, 29, 31, 33, 35, 37, 39, 41, 43, 47, 49, 53, 55, 59, 63, 65, 67.
Chapter 17

Definitions of Acids and bases.

Acid strength and molecular structure.

Ionization constants for weak acids (Ka).

Ion product of water. Kw = Ka x Kb = 1.0x10-14

pH and pOH, pH + pOH = 14 = pKw.

Calculating [H+] and pH of a strong acid and weak acid.

Percent ionization of a weak acid.

Finding the [OH-] and pH of strong and weak bases (kb).

Acid-base properties of ions and salts. Classifications of salts.

pH of a Polyprotic acids.

Lewis Acids and Bases.
Homework: 31, 33, 35, 36, 39, 41, 45, 49, 51, 53, 57, 59, 65, 67, 71, 73, 77, 83, 89, 91, 95, 103, 104.
Chapter 18

Common ion effect on the ionization of weak acids and bases.

Buffer solutions, pH of buffers, and buffering capacity.

Titration and pH curves.

Titration of a strong acid with a strong base.

Titration of a weak acid with a strong base.

Solubility equilibria and solubility product constant (Ksp).

Uses of Ksp in calculating the molar and the gram solubility.

The common ion effect and pH on solubility..

Predicting Precipitation and selective precipitation.
Homework: 25, 27, 31, 37, 39, 45, 47, 51, 55, 63, 65, 69, 83, 85, 87, 91, 93, 97, 99, 103, 105.
Chapter 19

Spontaneity and reversible or irreversible process..

Entropy (S) and the second law.

Predicting entropy for a chemical reaction.

Standard Molar entropy. ∆S(reaction) = {∆nSf(products) - ∆nSf(reactants)}

Heat transfer and entropy change s of the surroundings.

Free energy (G), ∆G = ∆H - T∆S,

∆G(reaction) = {∆nGf(products) - ∆nGf(reactants)}

Using ∆G to predict the spontaneity of the reactions.

The relationship between ∆G and Kc, ∆ G = -RTLnKc.
Homework: 29, 33, 35, 37, 41, 43, 45, 49, 53, 59, 61, 65, 67, 69, 75.
Chapter 20

Oxidation numbers, redox reactions and oxidizing/reducing agents.

Balancing redox equations.

Galvanic [voltaic] cells and electrodes

Cell potentials (E), standard electrical potential and standard cell voltages.

Spontaneity of redox reactions.

Free energy equilibrium constant and cell potential.

Effect of concentration on Ecell and Nernst equation.

Commercial voltaic cells; batteries, electrolysis, and electroplating.
Homework: 33, 35, 37, 39, 43, 45, 49, 53, 57, 59, 61, 63, 67, 69, 71, 73, 77.
Chapter 21 (time permitting)

Nuclear structure; protons, and neutrons.

Nuclide symbols and nuclear equations.

Types of radioactivity: Nuclear decay and the particles that appear in nuclear decay.

Patterns of nuclear stability and detecting radioactivity.

Rates of radioactive decay and carbon dating.

Nuclear reactions; nuclear fission, nuclear fusion, and Nuclear reactors.

Energy changes in nuclear reactions.

Nuclear transmutations.

Biological effects of radiation.

Applications of radioactivity.
Homework: 31, 33, 35, 37, 45, 47, 49, 51, 59, 67, 69, 71.