!!! HOUSTON COMMUNITY COLLEGE CHEM 1412 GENERAL CHEMISTRY II, Spring 2016

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1 HOUSTON COMMUNITY COLLEGE CHEM 1412 GENERAL CHEMISTRY II, Spring 2016 Welcome: Welcome to General Chemistry II. I hope that you will enjoy this semester of chemistry 1412 and will carry that enjoyment of chemistry beyond the end of this class. This syllabus contains the course policies, useful information to help you get acquainted with the course procedures, and expectations for this chemistry course. Please peruse these pages, as they represent an agreement between us, me, your instructor, and you, the student. Instructor Yuliya Sumskaya Office Hours: by appointment yuliya.sumskaya@hccs.edu Learning Web : Time and location (CRN 91662) West Loop Campus Lecture 2:00 pm 5:00 pm; T, Room C220 Lab 2:00 pm 5:00 pm; Th, Room C164 Textbook (Required) CHEM 1412: (Second half of text book only) Zumdahl/Zumdahl, Chemistry 9th ed. Volume II, Cengage 2014 ISBN: The full hardcover edition for CHEM 1411 & 1412 is also available. ISBN-13: OPTIONAL - Student Study Guide for both CHEM 1411/1412: Student study guide to accompany Zumdahl, Chemistry 9th ed. ISBN: Laboratory Manual Laboratory Manual for CHEM 1412, General Chemistry II, Blue Door Publishing: ISBN-13: Access to OWLv2 (Required) OWL, an acronym for Online Web-based Learning, is a tutoring and homework system. Students that purchase a new textbook may have an access code bundled with their textbook. You may be able to purchase access to OWL V2 at your bookstore. Check with the bookstore to find out what they offer for your course. An access code may be purchased on-line from Cengage at

2 Computer Requirements You will need to have access to a computer with internet access and a contemporary web browser and needed plug-ins. You are responsible for maintaining your own hardware and software. If you are incapable of maintaining your own system, please use the computers available on campus. Scientific Calculator You will need an inexpensive scientific calculator. Be aware that programmable and internet accessible calculators are not allowed for the exams. Course Catalog Description: CHEM 1412 General Chemistry II Prerequisites: One year of high school chemistry and MATH 1314 and Chem Credit: 4 (3 lecture, 3 lab); Continuation of CHEM Topics include solutions, chemical kinetics, equilibrium and equilibrium phenomena in aqueous solution, acids and bases, ph, thermodynamics, electrochemistry, nuclear chemistry, organic chemistry, and biochemistry. Core curriculum course. Course Description: ACGM or WECM General principles, problems, fundamental laws, and theories. Course content provides a foundation for work in advanced chemistry and related sciences. THIS COURSE WILL REQUIRE A CONSIDERABLE TIME INVESTMENT BY YOU PLEASE BE PREPARED Plan on dedicating around hours per week studying for this course (and probably a little bit more initially while you are becoming familiar with the course materials) This works out to around 5-6 hours every five to six days out of a 7 day week. You will need to structure your life where you can dedicate this time to the class. Use TIME MANAGEMENT TOOLS such as a scheduler / planner to ORGANIZE YOUR TIME THIS IS THE MOST IMPORTANT SECRET TO YOUR SUCCESS IN THIS COURSE. You will get out of the class what you put into in it is all up to you Academic Discipline Program Learning Outcomes 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.

3 4. To enhance class lectures with a meaningful, hands-on laboratory experience involving making measurements, observing reactions, evaluating the results, and drawing conclusions with the involvement of lab group or other class members. Course Student Learning Outcomes (SLO) 1. Distinguish between the different ways of measuring concentrations of solutions, and relate concentration to the colligative properties of solutions. 2. Determine and analyze the rates of chemical reactions. 3. Write equilibrium constant expressions for chemical reactions and calculate the value of the equilibrium constant and the concentration of reactants and products at equilibrium. 4. Demonstrate proficiency in acid-base and solubility product calculations. 5. Express the three laws of thermodynamics and interrelate the enthalpy, free energy and equilibrium constant for the reaction. 6. Based on the principles of oxidation and reduction, balance oxidation/reduction reactions, calculate cell potentials of voltaic cells based on oxidation-reduction reactions, and make quantitative calculations based on electrolysis. 7. Identify modes of radioactive decay, balance nuclear reactions, calculate energy changes associated with nuclear reactions, and relate quantities of radioactive elements with time based on the kinetics of nuclear processes. 8. Classify, name, and draw the structure of basic organic compounds; student can write chemical reactions of alkanes, alkenes, and alkynes. Learning Objectives (Numbering system linked to SLO) 1.1 Determine if two compounds will mix to form a solution or not based on their structures. 1.2 Given the mass of a solute and the volume of a solution or the mass of the solvent, calculate the relevant concentration molarity, molality, percent concentration, mole fraction, or ppm). Convert a given concentration from one concentration unit to another. 1.3 Relate the concentration of solutions to their colligative properties. 1.4 Determine the molecular weight of an unknown solute, given the value of a colligative property. 2.1 Determine the average rate and instantaneous rate of a reaction from concentration time data. 2.2 Determine the order of a reaction with respect to each reactant and write the rate law for the reaction. Determine the value of the rate constant, k. 2.3 Write the integrated rate law of first and second order reactions and use the rate law to relate concentration of the reactant with reaction time, rate constant, and half-life. 2.4 Given different initial reactant concentrations and the respective initial rate of the reaction, determine the value of the exponents in the rate law and the value of the rate constant. 2.5 Relate the effect of temperature and activation energy to reaction rate using the Arrhenius equation. 2.6 Relate the rate law to the mechanism of the reaction and to the molecularity of the elementary reactions comprising the mechanism. 3.1 Write the equilibrium constant expression for homogeneous and heterogeneous reactions. 3.2 Given one or more concentrations at equilibrium, calculate the value of the equilibrium constant for the reaction and/or the equilibrium concentrations of the other substances in the reaction. 3.3 Given one or more initial concentrations, calculate the concentrations of the reactants and products at equilibrium and/or the value of the equilibrium constant, using the "ICE" table method. 3.4 From the value of the reaction quotient, Q, determine whether a reaction is at equilibrium, and if not, which direction the reaction will initially proceed in order to reach equilibrium. 3.5 Apply LeChâtelier s Principle to determine the effects of changes in concentrations, temperature on compositions of equilibrium mixtures. 4.1 State the three different definitions and principles of acids and bases (Arrhenius, Bronsted-Lowry, and Lewis). 4.2 Calculate [H+], [OH ], ph, and poh. 4.3 Use dissociation constants for weak monoprotic acids and bases to determine the ph of their aqueous solutions. 4.4 Differentiate between acidic, basic and neutral salts and determine the ph of aqueous solutions of salts. 4.5 State the common ion effect and its relevance to buffers; determine the ph of buffered solutions using the Henderson-Hasselbalch equation. 4.6 Calculate the ph at various stages of titration curves for (i) strong acids & strong bases, (ii) weak acids & strong bases, (iii) strong acids & weak bases. 4.7 Write solubility product expressions and interconvert between the solubility constant, Ksp and concentrations of dissolved ions in saturated solutions of slightly soluble salts. 4.8 Given Ksp, determine whether precipitation will occur when two aqueous solutions of salts are mixed that react to form a sparingly soluble salt. 5.1 Express the concept of entropy and predict the sign of the entropy change for a given reaction. 5.2 Calculate the entropy change of a reaction using Hess's law or standard entropies. 5.3 From the Gibbs equation, relate and calculate the values of the entropy, enthalpy, free energy, and temperature of a reaction. 5.4 Relate and calculate the value of the equilibrium constant to the entropy, enthalpy, free energy and temperature of the reaction. 6.1 Determine the oxidation state of elements in compounds.

4 6.2 Based on changes in oxidation states, determine which substance in a reaction is oxidized and which is reduced. 6.3 Balance oxidation-reduction reactions in acidic and basic solution using the method of half-reactions. 6.4 Sketch voltaic and electrolytic cells, identifying the anode, cathode, anode compartment, cathode compartment, salt bridge, and direction of electron flow. 6.5 Calculate standard cell potentials from standard reduction potentials. 6.6 Rank reducing agents and oxidizing agents based on standard reduction potentials. 6.7 Determine non-standard cell potentials from standard cell potentials using the Nernst equation. 6.8 Interconvert between time, current, and masses of reactants and products in electrolysis processes. 7.1 Identify common modes of radioactive decay. 7.2 Write balanced nuclear reactions. 7.3 Differentiate between the different modes of decay and predict the likely mode of decay. 7.4 Interconvert between rates of nuclear decay, half-lives of radioactive nuclei, and amounts of radioactive nuclei. 7.5 Determine energy changes of nuclear reactions and stability of nuclei using Einstein s equation. 7.6 Distinguish between subcritical, critical, and supercritical masses; contrast nuclear fission with nuclear fusion processes. 7.7 Identify the major components and principle of operation of nuclear reactors. 8.1 Given the structure, name alkanes using the IUPAC rules of nomenclature, and vice versa. 8.2 Classify organic compounds based on the functional group present in their structures. 8.3 Given the structure, name alkenes and alkynes using the IUPAC rules of nomenclature, and viceversa. 8.4 Optional if time permits. Write combustion and halogenation reactions of alkanes; write addition reactions of alkenes and alkynes. SCANS and/or Core Curriculum Competencies Reading, Writing, Speaking/Listening, Critical Thinking, Computer/Information Literacy Schedule: Week Date Class Events Assignments Due 1 T 01/19 Th 01/21 2 T 01/26 Th 01/28 3 T 02/02 Th 02/04 4 T 02/09 Th 02/11 Introduction, Syllabus review, Learning Web Introduction, Lab Safety Video Lab # 1 Solubility & Metathesis Reactions in Aqueous Solutions Chapter 11: Properties of solutions Lab # 2 Molecular Weight Determination by Freezing Point Depression Chapter 12: Chemical Kinetics Chapter 13: Chemical Equilibrium EXAM # 1 (Chapters 11-13) Lab # 9 Qualitative Analysis of Cations

5 Week Date Class Events Assignments Due 5 T 02/16 Th 02/18 6 T 02/23 Th 02/25 Chapter 14: Acids and Bases Exp. # 4 Kinetics of a Chemical Reaction: The Iodine Clock Reaction (lab report due Th 02/25) Chapter 14: Acids and Bases Chapter 14: Acids and Bases REPORT #4 7 T 03/01 Th 03/03 8 T 03/08 Th 03/10 Chapter 15: Acid-Base Equilibria Exp. # 6 Acid-Base Titration: Determination of the Purity of Potassium Hydrogen Phthalate (pre-lab due Th 03/03, lab report due Th 03/10) Chapter 16: Solubility and Complex Ion Equilibria Exp. # 5 Hydrolysis Reactions of Anions and Cations of Salts (pre-lab due Th 03/10, lab report due T 03/22) QUIZ CHAPTER#14 HW CHAPTER#14 REPORT #6 QUIZ CHAPTER#15 HW CHAPTER#15 9 T 03/15 Spring Break - NO CLASSES Th 03/17 10 T 03/22 Spring Break - NO CLASSES Chapter 16: Solubility and Complex Ion Equilibria REPORT #5 Th 03/24 Review for the Mid-Term Exam (Chapters 11-16) QUIZ CHAPTER#16 HW CHAPTER#16 11 T 03/29 Th 03/31 MIDTERM EXAM (Chapters 11-16) Chapter 17: Spontaneity, Entropy and Free Energy 12 Tuesday, April 5th is the last day to drop the class and receive a W. If you stop coming to class, but do not do the necessary paperwork by 04/05/16, you will get a regular grade (A - F), not a W in your transcript. T 04/05 Th 04/07 13 T 04/12 Th 04/14 Chapter 17: Spontaneity, Entropy and Free Energy MIDTERM EXAM RETAKE (Chapters 11-16) Chapter 18: Electrochemistry Chapter 18: Electrochemistry QUIZ CHAPTER#17 HW CHAPTER#17

6 Week Date Class Events Assignments Due 14 T 04/19 Th 04/21 15 T 04/26 Th 04/28 16 T 05/03 CLASSES CANCELLED Chapter 19: The Nucleus: A Chemist s View Chapter 19: The Nucleus: A Chemist s View Chapter 22: Organic and Biological Molecules Exp. # 15 Structural Formulas and Isomerism (prelab due Th 05/03, lab report due T 05/05) QUIZ CHAPTER#18 HW CHAPTER#18 QUIZ CHAPTER#19 HW CHAPTER#19 17 Th 05/12 FINAL EXAM (Cumulative) 2:00-5:00 pm, room C164 Methods of Instruction - The method of instruction will include, but is not necessarily limited to: directed and independent readings, homework, class discussions, and laboratory exercises. The following grade distribution scale will determine your course grade: GRADING: COURSE GRADE: Attendance 5 % 90.0% and above A Homework 10% 80.0% % B Class quizzes 15 % 70.0% % C Laboratory 25 % 60.0% % D Midterm Exam 20 % 59.9% or below F Final Exam 25% - Total 100% Th 05/05 FINAL REVIEW, Practice Exam (Chapters 17, 18, 19, 22) The student is encouraged to keep track of their daily grade Classroom Environment HW CHAPTER#22 REPORT #15 Students will respect the classroom environment. Students will not intentionally obstruct, disrupt or interfere with the teaching and learning that occurs in the classroom. Students will not engage in any activity that demeans any student, instructor, or administrator. Such activities include, but are not limited to, oral and written communication that is ethnically derogatory, sexist, or racist in nature; unwanted sexual advances or intimidation; profane communication in any manner. Please turn off cell phones and computers during class. Failure to comply may result in removal from class. Sleeping (including resting head on desk or labtop) is not allowed. You are free to stand at any point during

7 the class. Failure to comply may result in removal from class. Disability Support Services (DSS) "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." For questions, contact Donna Price at or the Disability Counselor at each college. Also visit the ADA web site at: If you have any special needs or disabilities which may affect your ability to succeed in college classes or participate in any college programs or activities, please contact the DSS office for assistance. Academic Honesty Students are responsible for conducting themselves with honor and integrity in fulfilling course requirements. Disciplinary proceedings may be initiated by the college system against a student accused of scholastic dishonesty. Penalties can include a grade of "0" or "F" on the particular assignment, failure in the course, academic probation, or even dismissal from the college. Scholastic dishonesty includes, but is not limited to, cheating on a test, plagiarism, and collusion. In this class, the penalty for willful cheating on exams is a grade of F in the course. This is the standard policy of the Physical Sciences department at Southwest College. Laboratory Policy On the first day of lab a safety video will be shown (about 35 min long) and a safety "quiz" will be given and reviewed. Each student will then sign a statement affirming his or her commitment to following safe procedures in the laboratory, and turn the form in to the instructor. You should be especially aware of the need for adequate eye protection in the laboratory. Protective glasses or goggles must be worn at all times during the laboratory period. Any student not wearing protective glasses or goggles after the experiment has begun may be given a zero for that experiment Exams and Make-up Policy Examinations will consist of three non-cumulative regular exams plus a comprehensive final. Make-up exams will not be given, so make every effort to take the exams on their scheduled dates. Remember that the final exam will be comprehensive (meaning that it will cover all of the material from the whole semester). Please note that all students are required to take the final exam. Procedures I check my frequently and strive for a less than 48-hour response time to your messages, but please be patient. In order to manage the great many s I receive from students, I am asking that you include the following information in each 1. Identify the course number and course title. 2. Identify yourself stating your full name as you registered for this course. 3. Identify the assignment and date due or the subject of your message/question. Attendance Policy Students are expected to attend classes regularly. Students are responsible for materials covered during their absences, and it is the student's responsibility to consult with instructors for missed assignments. Class attendance is checked daily by instructors. Although it is the responsibility of the student to drop a course for nonattendance, the instructor has full authority to drop a student for excessive absences. A student may be dropped from a course for excessive absences after the student has accumulated absences in excess of 12.5% of the hours of instruction (including lecture and laboratory time). If circumstances significantly prevent you from attending classes, please inform me. I realize that sometimes outside circumstances can interfere with school, and I will try to be as accommodating as possible, but please be aware of the attendance policy. Assignment Policy Students are responsible for all information covered in the course. It is your responsibility to complete and submit all assignments and tests by their respective due dates. No late work will be accepted. No deadline extensions will be granted. No modifications will be made to the course schedule. Class Quiz/Attendance (5%)

8 At the beginning of every lecture there may be a pre-lecture quiz on the assigned reading. The quiz will also account for your attendance. This assignment will be complete and graded during the beginning of each lecture. Notes are allowed for the quiz. OWLv2 Homework (10% + *10% extra credit) OWLv2, an acronym for Online Web-based Learning, is a tutoring and homework system. As you study an assigned chapter you will perform the assigned homework on OWLv2. The homework consists of two sections: 1) Mastery (worth ¼ of your chapter homework grade) 2) EOC (worth ¾ of your chapter homework grade) You are given ample time to complete and submit your answers to OWLv2 by the deadline. If you miss the deadline for submitting your answers, you will receive a zero for those questions. As noted earlier in this syllabus, if you use a non-college computer to access OWL, you are responsible for its performance. No additional time will be provided. You can repeat the homework UP TO 10 times. The highest grade recorded by the deadline for completing a chapter homework will be your grade for that chapter. *A minimum of 50% of the homework is required to be completed for full credit. Additional completed homework will be counted as extra credit. OWLv2 Quizzes (15%) When you are confident that you have mastered the assigned OWLv2 assigned homework, you will then take the chapter quiz. You may only take the quiz once. You have 2 hours to complete 20 questions. This is ample time to complete and submit your answers. If you miss the deadline for submitting your quiz, you will receive a zero for the missed work. As noted earlier in this syllabus, if you use a non-college computer to access OWL, you are responsible for its performance. No additional time will be provided. Laboratory Exercises (20%) Each assignment should be clearly titled and the answers to each exercise complete. Before you leave the lab, be sure to show me your report so I can review and initial it. Each student should arrive at the lab on time, with his or her lab manual. Laboratory reports are due one week after the experiment. Each report must be done individually, but of course you can work with your lab partners on it. Each report will be graded on a 10-point basis. Come to lab prepared. Read through the experiment beforehand, and answer the pre-lab questions in the lab manual. Exams (30%) The student is expected to understand the assigned materials before the test is administered. The tests have a 2-hour time limit. Exams I, II, and III will consist of 25 multiple choice questions. Students may use calculators for the exams. CELLULAR PHONES, PROGRAMMABLE/INTERNET ACCESSABLE CALCULATORS, AND COMPUTERS ARE NOT ALLOWED. Students need to bring a scantron to the exams. Final Exam (20%) The student is expected to understand the assigned materials before the test is administered. The final exam has a 2-hour time limit. The comprehensive final exam will consist of multiple choice and short answer questions. Students may use calculators for the exams. CELLULAR PHONES, PROGRAMMABLE/INTERNET ACCESSABLE CALCULATORS, AND COMPUTERS ARE NOT ALLOWED. Students need to bring a scantron to the exams. Extra Credit Extra credit opportunities may be offered throughout the semester, at the sole discretion of the professor. EXTRA CREDIT IS NOT GUARANTEED. Disclaimer To accommodate emergent circumstances, the instructor reserves the right to make reasonable changes in the syllabus while the course is in progress. Any question of interpretation of course requirements or of understandings between a student and the instructor will be at the discretion of the instructor and/or the Chair of the Science Department. VCL S and In Class Exercises Acetate Buffer Lab Acid-Base Titration Lab Arrhenius Lab

9 Electrochemical Cell Part I: Voltaic Cell Lab Electrochemical Cell Part II: Concentration Cell Lab Le Chatlier s Principle Lab Unknown Acid-Base Titration Lab Weak Acid Titration Lab Drawing Organic Structures in class exercise Drawing Organic Structures II in class exercise Organic Functional group Chart in class exercise I Organic Nomenclature I - in class exercise Organic Nomenclature II - in class exercise Course Syllabus and HCC Central Learning Web: Chem 1412 GENERAL CHEMISTRY II Spring 15 Syllabus Lecture Slides Virtual Chemistry Labs Organic Chemistry in Class Worksheets Unit Analysis Document Lab Safety Video Chemistry Lab Equipment

Textbook (Required) CHEM 1411: (First half of text book only) Zumdahl/Zumdahl, Chemistry 9th ed.

Textbook (Required) CHEM 1411: (First half of text book only) Zumdahl/Zumdahl, Chemistry 9th ed. HOUSTON COMMUNITY COLLEGE CHEM 1411 0082 GENERAL CHEMISTRY I, SUMMER 2015 Welcome: Welcome to General Chemistry I. I hope that you will enjoy this semester of chemistry 1411 and will carry that enjoyment