CHEMISTRY 131 WINTER 2008



CHEM-134 GENERAL CHEMISTRY II Winter 2015

Instructor: Sarah Simmons Phone: 269-294-4205

Email: ssimmons@glenoaks.edu Office: G-217

Office Hours: Open Door Policy, M, W: 10:30-11:00am, 12:30-1:00pm, 5:00-6:00pm, F: 7:00-8:00am

Classroom: Lecture: M,W 1-2:25pm Rm G-207 Lab: F 1-3:45pm Rm G-221

Website: sarahsimmonschemistry.

Course Description: This is a continuation of NSC 133 General Chemistry. Topics covered include theories of covalent bonding, phase changes and intermolecular forces, properties of mixtures, organic compounds, kinetics, equilibrium, acid/base equilibria, equilibrium in aqueous systems, and thermodynamics.

PREREQUISITES: NSC 133 and 2.0 or higher in Math 100 or 104 or 151 or equivalent or by placement into 104.

Required Materials:

▪ Chemistry: The Molecular Nature of Matter and Change. 6th ed. Silberberg.

▪ Scientific calculator (log and exponential functions),

▪ Chemical Principles in the Laboratory. 10th ed. Slowinski, Masterton, and Wolsey.

Methodology and Activities: This is a lecture/laboratory combination course. Lecture sessions discuss the main and/or troublesome topics and include sample problems. Lecture sessions are formal to semi-formal with open and general discussion on a pertinent topic preferred. The laboratory sessions are used to introduce new concepts or to reinforce concepts discussed in the lecture sessions.

Quizzes: There will be several pop quizzes given in lecture throughout the semester. They will be fairly short, lasting only 5-10 minutes at the beginning of class, and may deal with topics already discussed or from the reading assignments.

Exams: There will be 5 in-class exams. Each exam will count for 100 points and will include a combination of multiple choice, problem solving and short answer questions. There will also be a cumulative final exam at the end of the semester.

Absences: Due to the complex nature of this course it is important that students attend each lecture. If absence is unavoidable the student is responsible for obtaining the missed lecture notes from another student. Make-up homework and exams are not available without a documented emergency. If extra help is needed for missed information, you must have a copy of the notes before asking the instructor for additional help.

Make-up Policy:

No labs will be dropped in calculating the final grade. One make-up lab will be available (see schedule).

Two quizzes will be dropped when calculating the final grade. No make-up quizzes will be available.

One exam will be dropped when calculating the final grade. The final exam will count as 2 exams.

Grading: The final grade will be calculated as follows

▪ Lecture: Quizzes 10%, Exams: 65%

▪ Laboratory: 25%

Grades will be assigned according to the following scale

Percentage Grade Percentage Grade

100 – 90% 4.0 74 – 70% 2.0

89 – 85% 3.5 69 – 65% 1.5

84 – 80% 3.0 64 – 60% 1.0

79 – 75% 2.5 59 – 0% 0.0

Classroom Etiquette: Proper classroom behavior is expected at all times. Talking in class and disruptive behavior will not be permitted and may result in dismissal from the class. Please turn off cell phones and any other noisemaker. No children will be allowed in the classroom. Remember, we are all here to learn and respect for the instructor and other students is a part of that process.

Incomplete and Withdrawal Policy: An “I” or incomplete for a course will not be given unless at least 75% of the course work has been completed. Withdrawal from class is your privilege and responsibility. It is necessary for you to follow correct procedures. A grade of W is automatically given through February 27th. After this date if you stop attending class and do not follow the official procedures for dropping or withdrawing from the class you shall receive a semester grade of 0.0 or whatever your total point accumulation permits. The last day a faculty may issue a W is April 26th.

Assistance: If you are a student with a documented disability and you believe you are entitled to receive accommodations for this class, please contact me privately so we may discuss your specific needs. You will also need to contact the Student Support Specialist to schedule an appointment for an intake if you have not already done so, You may contact the Student Support Specialist by calling 269-467-9945 and ask for Student Services.

Academic Dishonesty: Academic dishonesty includes, but is not limited to taking, using, or copying another’s work and submitting it as your own, using notes on exam’s, intentionally falsifying information or taking another’s ideas with intention of passing in class as one’s own. Academic Dishonesty will not be tolerated and will result in a zero.

Sensitivity: Glen Oaks Community College is committed to providing equal access to education for all persons regardless of race, color, sex, age, religion, national origin, sexual orientation, disability, veteran status, or other status as protected by law.  The College is committed to an environment that demonstrates civility, caring and respect. Harassment of any kind is a barrier to effective work and academic achievement.  Glen Oaks Community College values diversity of expression, collaboration, partnering and finding ways to communicate effectively across differences in the college community.  If you feel that you have been the focus of discrimination or harassment, you may report the incident or by phone at 1-877-743-4127. You may also contact a counselor by calling (269) 467-9945 and asking for Student Services

Emergency Evacuation Procedures: A map of the wing where this classroom is located is posted near the wing entrances marking evacuation routes and the designated tornado shelter area. This is an area where emergency service personnel will go first to look for individuals who need assistance in exiting the building. Please make sure to review the maps to ensure you will know how to evacuate in case of an emergency. Students who may need assistance should identify themselves to the teaching faculty.

Learning Outcomes

By the completion of this course, successful students will:

A. Safety

• Explain a Material Safety Data Sheet (MSDS) including different parts and the value or need for each part. (2)

• Identify different types of fire extinguishers and what types of fires they are to be used upon. (5)

• Explain the correct usage of a fire blanket, eyewash and shower. (2, 5)

• State and explain what universal precautions are and why and how they are used. (2)

• Describe proper disposal methods for chemicals. (2)

• Describe the effects of improper disposal methods on the environment. (2)

• Recognize and correctly name laboratory equipment, glassware, and supplies that are used. (2, 5)

• Define safety terms. (2)

B. Theories of Covalent Bonding

• Explain the process of hybridization in valence bond theory and determine the hybridization of orbitals in a molecule. (2, 5)

• Draw the orbital overlap in molecules involving single, double, and triple bonds (5)

• Determine the number of sigma and pi bonds in a molecule and determine a bonds relative stability (5)

• Explain the mixing of orbitals in molecular orbital theory (5)

• Draw an energy level diagram and determine the electron configuraton and bond order for a molecule (5)

• Explain the advantages and disadvantage of valence bond theory and molecular orbital theory (2, 5)

C. Intermolecular Forces: Liquids, Solids, and Phase Changes

• Describe the interactions of molecules in the three physical states and determine their amount of kinetic and potential energy. (2, 5)

• Determine the amount of energy exchange during phase changes using heat of vaporization and heat of fusion (5)

• Define and locate the triple point, critical point, liquid, gas, and solid state on a heating-cooling curve (2, 5)

• Define intermolecular interactions, including dipole-ion forces, dipole-dipole forces, hydrogen bonding, and London dispersion forces, and determine the forces that a substance possesses. (2, 5)

• Determine the structure of solids, and draw the unit cell of primitive cubic, body-centered cubic, and face-centered cubic structures. (5)

D. The Properties of Mixtures: Solutions and Colloids

• Determine the concentration of a solution in Molarity, molality, and mass percent (5)

E. Organic Compounds and the Atomic Properties of Carbon

• Draw the structure of hydrocarbons and proper names (5)

• Name hydrocarbons with single, double, and triple bonds (5)

• Name and draw structures of cyclic hydrocarbons (5)

• Define chirality and determine if a molecule is chiral (2, 5)

• Name and draw structures of some aromatic compounds (5)

• Name and draw structures of molecules including functional groups, including, halogens, alcohols, esters, carboxylic acids, aldehydes, ketones, ethers, amines, and amides (5)

• Determine the product of some basic organic reactions including substitution, elimination, addition, and reduction reactions (5)

F. Kinetics: Rates and Mechanisms of Chemical Reactions

• Determine the reaction rate in terms of reactant and product concentration (5)

• Determine the rate law and reaction order for each reactant (5)

• Determine the rate constant of the reaction (5)

• Describe Reaction rate in terms of Kinetic Molecular Theory (2, 5)

• Determine how concentration, temperature, and catalysts affect reaction rate (5)

• Draw an energy diagram of a reaction and determine the energy of activation. (5)

• Draw the transition state of a reaction by using the reaction mechanism (5)

G. Equilibrium: The Extent of Chemical Reactions

• Determine the reaction quotient and equilibrium constant (5)

• Calculate Kc and Kp and convert between them (5)

• Determine the reaction direction using Q and K (5)

• Determine the amount of products and reactants formed through the equilibrium constant (5)

• Determine the direction of reaction when equilibrium is disturbed (Le Chatelier’s Principle) (5)

H. Acid-Base Equilibria

• Define acids and bases using Arrhenius and Bronsted-Lowry definitions (2, 5)

• Determine the Ka and Kb (5)

• Determine the relative strength of acids based on structure (5)

• Determine the pH of strong and weak acids and bases (5)

• Determine the pH of a salt solution (5)

I. Ionic Equilibria in Aqueous Systems

• Define buffer and its purpose (2, 5)

• Determine the pH of a buffer solution using the Henderson-Hasselbalch equation (5)

• Determine the buffer capacity and range (5)

• Explain how to prepare a buffer (2, 5)

• Determine the titration curve of strong and weak acids and bases (5)

• Determine the Ksp of slightly soluble ionic compounds (5)

J. Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

• Define a spontaneous reaction and how enthalpy and entropy determines spontaneity (2, 5)

• Define entropy and determine if a system is becoming more or less disorganized (2, 5)

• Determine the Gibb’s Free Energy of a system from enthalpy and entropy (5)

• Determine the free energy of reactions at equilibrium (5)

K. Instrumentation

• Define instrumentation. (2)

• Describe the operation of a gas chromatograph. (2)

• Describe the operation of a liquid chromatograph. (2)

• Illustrate applications for gas and liquid chromatography. (2, 5)

• Describe spectrophotometry. (2)

• Operate analytical balances. (5)

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