GENERAL CHEMISTRY II Lecture & Recitation

Transcription

1 Howard University Department of Chemistry Fall 2010 GENERAL CHEMISTRY II Lecture & Recitation Chem 004, Section 04, CRN 82454; Section 05, CRN 82456; Section 06, CRN Credit Hours Course Time & Room: Lectures MWF 9:10 10:00 a.m., room 108 (Chem. Bldg.) Recitation: Section 04 M 10:10 11:00 a.m., room 305 (Chem. Bldg.) Section 05 T 1:10 2:00 p.m., room G06 (Chem. Bldg.) Section 06 W 10:10 11:00 a.m., room 305 (Chem. Bldg.) Instructor: Office: Office Phone: Office Hours: Dr. Galina G. Talanova, Associate Professor of Chemistry Room 113 (202) gtalanova@howard.edu MW 11:30 a.m.-12:30 p.m.; T 2:30-3:30 p.m. or by appointment (which may be made in person, by phone or ) Textbook & Other Materials: Brown, Lemay and others, Chemistry: The Central Science (11 th Edition), Pearson, Prentice Hall, 2009 Solutions Manual and Student s Study Guide Periodic Table of Elements (in any form) scientific NON-PROGRAMMING calculator (required) (optional) (required) (required) Note: Students are required to bring calculators to each lecture class and recitation session. Course Description The course deals with the fundamental principles of chemistry, of chemical and physical properties of the elements and their most common compounds, and methods of qualitative inorganic analysis. Prerequisite: General Chemistry I and College Algebra. This course is taught with active use of Blackboard on-line environment. It is student s responsibility to obtain access to the class website in Blackboard from the very beginning of the semester. To increase students chances for success in General Chemistry courses this year, Department of Chemistry will be using ALEKS (Assessment and Learning in Knowledge 1

2 Spaces) on-line tool as a required component: performance in ALEKS will contribute to the overall class grade (see below). ALEKS will be used to identify rapidly and accurately any areas of strength or weakness in the student s background needed for the course, and where gaps are found, to help the student firm up knowledge of pre-requisite topics and further on, to learn the material during the semester. Student learning outcomes: A detailed list of learning outcomes from this course, i. e., skills the students will gain upon successful completion of the course, is attached (see pp. 6-9). Course Policies American with Disability Act (ADA) Compliance: Howard University is committed to providing an educational environment that is accessible to all students. In accordance with this policy, students in need of accommodations due to a disability should contact the Office of the Dean for Special Student Services for verification and determination of reasonable accommodations as soon as possible after admission to the University, or at the beginning of each semester. The Dean of the Office of Special Student Services, Dr. Elaine Heath, can be reached at (202) Student Code of Conduct: Howard University expects that a student s conduct will be in accordance with accepted standards of behavior. In keeping with this expectation, a student may be disciplined for academic offences, particularly cheating and/or plagiarism. For further details view the Student Reference Manual for Fall 2010 (page 40) at Attendance: Attendance of the lectures and recitation sessions is mandatory. You are responsible for all of the material presented in class (including the information which is not provided in the textbook), announcements, assignments, and any schedule changes that may occur. Homework: Home reading is an important part of your course work! Students are required to read the appropriate chapter in the textbook after each lecture and strongly encouraged to read the material in advance. You will be required to complete on-line homework assignments ( objectives ) in ALEKS. 15% of your overall class grade will be calculated from the ALEKS Gradebook. Quizzes: There will be 10 short quizzes which may be given either online (in the Blackboard) or during the recitation sessions. A tentative quiz schedule is provided. (Be aware: changes in the schedule may occur during the semester!). You are expected to take all of the quizzes. At the end of the semester, for each of you, 2 the lowest-score quizzes will be dropped and therefore, only 8 of 10 quizzes will contribute to your overall grade. There will be no make-up quizzes. Exams: Four hourly exams will be given during the semester (for a tentative schedule, see the attached Course Syllabus). The exams will take place during the lecture class in room 2

3 108. Note: No exams are dropped in this course. Cumulative Final exam will be given on December 10 (Friday) at 8:00-10:00 a.m. in room 108. In an exam, you are expected to show your work on the problems in order to get credit. Please be aware that for problems requiring calculations, the answers given without the work shown will not be accepted and shall result in zero (0) points. Please note: Do not be late for the exams, you will NOT be given extra time! Important! You must notify the instructor in advance (by phone or ) if illness or other unavoidable circumstances prevent you from taking an exam at the scheduled time. Make-up exams may be given under exceptional circumstances only and will require appropriately documented justification. Standardized (ACS) Departmental Exam: In addition to 3 hourly exams and final exam, in accord with the Department policies, all students enrolled in General Chemistry classes must take a standardized (American Chemical Society) Departmental exam which will be administered on December 7, 2010 at 6:00 p.m. (room TBA). The Departmental exam is given to evaluate knowledge gained by the Howard University students in General Chemistry as compared to their peers nationwide. The score from the Departmental exam will be used as extra credit for this course and may contribute (depending on the performance) up to 5% added to your overall class grade earned for the regular course work (see Grading Policies below). Please note: a minimum score of 60% must be received on the standardized exam in order to obtain an extra credit. The following performance-based distribution of the extra credit points will be applied: exam score of 60-69% entitles the student to extra 2% added to the class grade; 70-79% extra 3%; 80-89% extra 4%; and % extra 5%. However, please be aware that in order to enforce taking the standardized exam, a penalty of -1% will be imposed to a student s overall class grade for missing this assignment. A student may be excused from taking the standardized exam under exceptional circumstances only (such as severe health condition or death in the immediate family), which requires an appropriately documented justification. Grading Policies: Assignments Hourly exams (4) Final exam Quizzes (8 of 10) Homework (ALEKS) Departmental exam % Weight 60% 20% 5% 15% Extra-credit (up to 5%) Cut-Offs A % B 80-89% C 70-79% D 60-69% Civility in the Classroom: Students are expected to assist in maintaining a classroom environment that is conducive to learning. Please show respect to the instructor and the classmates. Any kind of troublesome behavior in the classroom that disturbs the instructor and/or the students during the class period will not be tolerated. Inappropriate behavior in the classroom shall result, minimally, in a request to leave the class. 3

4 And please turn off your cell-phones before coming to class. In accord with Student Code of Conduct, sending or receiving text messages during the class is NOT allowed. Academic Dishonesty: Will not be tolerated. If discovered, it will be dealt with in accordance with the Howard University policies (see Student Reference Manual for Fall 2010, page 40). Note: Using cell-phones or any other electronic communication devices during exams and quizzes is NOT allowed. Students are prohibited from having such devices on their work stations during exams and quizzes. Any deviation from this rule shall result in a failing grade for the exam/quiz. Help Resources: If you have any difficulties in understanding the material or completing assignments, please come by to see me during my office hours or by appointment. If you are unable to keep the scheduled appointment, your responsibility is to notify me in advance. Also, you are encourages to bring questions to the recitation sessions and, if necessary, send them to me by . However, no consulting by phone will be provided. And please remember: Do not wait too long before seeking for help if you feel that such is needed! Important dates: August Change of program period. Change or drop a course without a W on the transcript. September 6 Labor Day observed September 24 Opening Convocation. Classes suspended from 10 a.m. till 1 p.m. October 11 Columbus Day observed October 15 Deadline for instructors to submit mid-term grades, UW and NR grades November 11 Veteran s Day observed November 12 Last day to withdraw from the course November Thanksgiving Recess December 2 Formal classes end December 3-5 Reading period December 8-15 Final exams December 15 Fall semester ends 4

5 Course Outlines Tentative Dates Topic Chapter Homework (ALEKS) Quizzes August September 1-10 Introduction; Intermolecular Forces; Liquids and Solids Properties of Solutions 11 #1 #1 13 #2 #2 September Chemical Kinetics 14 #3 #3 September September 27- October 6 September 17: 1 st exam during the lecture class, room 108 Chemical Kinetics (contd.) 14 #4 #4 Chemical 15 #5 #5 Equilibrium October 8: 2 nd exam during the lecture class, room 108 October Acid-Base Equilibria 16 #6 #6 October Additional Aspects of Aqueous Equilibria 17 #7 #7 October 29: 3 rd exam during the lecture class, room 108 November 1-8 Thermodynamics 19 #8 #8 November Electrochemistry 20 #9 #9 November 22- December 1 November 19: 3 rd exam during the lecture class, room 108 December 7 (Tuesday): Nuclear Chemistry 21 #10 #10 Departmental Exam (comprehensive), 6:00-8:00 p.m. December 10 (Friday): Final Exam (comprehensive), 8:00-10:00 a.m., room 108 The instructor reserves the right to make any changes to the course policy and schedule as the semester proceeds, with exception for the Departmental Exam and Final Exam date and time. 5

6 Student Learning Outcomes Upon successful completion of the course, students will (skills gained, by chapter): Chapter 11 Understand and be able to describe the intermolecular attractive interactions that exist between molecules and ions. Be able to compare the relative strengths of intermolecular attractions in substances based on their molecular structure or physical properties. Understand the concepts of polarizability, viscosity and surface tension in liquids. Know the names of various phase changes for a pure substance. Interpret heating curves and be able to calculate quantities related to temperature and enthalpies of phase changes. Define critical pressure, critical temperature, vapor pressure, normal boiling point, normal melting point, critical point, triple point. Be able to interpret and sketch phase diagrams. Classify solids based on their bonding/intermolecular forces and understand how differences in bonding relates to physical properties. Chapter 13 Understand and be able to explain: how enthalpy and enthropy changes affect solution formation; relationship between intermolecular forces and solubility. Describe the effect of temperature on the solubility of solids and gases. Describe the relationship between the partial pressure of a gas and its solubility. Be able to calculate the concentration of a solution in terms of molarity, molality, molar fraction, weight % composition, and parts per million and be able to interconvert between the units of concentration. Describe colligative properties of a solution and explain the differenec between the effects of nonelectrolytes and electrolytes on the colligative properties. Be able to calculate the vapor pressure of a solvent over a solution. Be able to calculate the boiling point elevation and freezing point depression of a solution. Be able to calculate the osmotic pressure of a solution. Chapter 14 Understand and be able to explain the factors that affect the rate of chemical reactions. Be able to determine the rate of a reaction given the time and concentration information. Be able to relate the rate of formation of products and rate of disappearance of reactants based on the stoichiometry of the reaction. Understand the form and meaning of a rate law, reaction order and rate constant. Be able to determine the rate law and rate constant for a reaction from a series of experiments given the measured concentrations of reactants as they change with time. Be able to use the integrated for of a rate law to calculate the concentration of a reactant at a given time. Explain how the activation energy affects a reaction rate and be able to use the Arrhenius equation. Understand the terms mechanism and molecularity of a reaction. 6

7 Be able to predict a rate law for a reaction having a multistep mechanism given the individual steps in the mechanism. Explain how catalysis works. Chapter 15 Understand the meaning of chemical equilibrium and its relationship to reaction rates. Be able to write the equilibrium-constant expression for any reaction. Relate and calculate K c and K p. Relate the magnitude of an equilibrium constant to the relative amounts of reactants and products present in an equilibrium mixture. Manipulate the equilibrium constant to reflect changes in the chemical equation. Write the equilibrium-constant expression for a heterogenious reaction. Calculate an equilibrium constant from the concentration measurements. Predict the direction of a reaction given the equilibrium constant and concentrations of the reactants and products. Calculate the equilibrium concentrations give the equilibrium constant and one of the following: -- all but one equilibrium concentration; -- initial concentrations. Understand how changing the concentrations, volume, temperature or pressure of a system at equilibrium affects the equilibrium position (Le Châtelier s Principle) and be able to apply this principle to predict any changes in the equilibrium position of a reaction. Chapter 16 Be able to define and identify Arrhenius acids and bases. Define and identify Brønsted-Lawry acids and bases, and identify conjugate acid-base pairs. Relate the strength of an acid to the strength of its conjugate base; K a and K b. Describe the strength of an acid/base in terms of position of equilibrium of proton transfer. Describe the autoionization of water and relationship between [H 3 O + ] and [OH - ]. Calculate the ph of a strong acid or base given its concentration. Calculate K a or K b of a weak acid or base given its concentration and the solution ph. Calculate the ph of a weak acid/base or its percent ionization given its concentration and K a or K b. Predict whether an aqueous solution of a salt will be acidic, basic, or neutral. Predict the relative strength of a series of acids from their molecular structure. Define and identify Lewis acids and bases. Chapter 17 Explain the common-ion effect. Explain how a buffer works. Calculate the ph of a buffer solution. Henderson-Hasselbalch equation. Calculate the ph of a buffer upon addition of small amounts of a strong acid or base. Calculate the ph at any point of acid-base titration of -- a strong acid and strong base; 7

8 -- a weak acid with a strong base or a weak base with a strong acid. Understand the differences between the titration curves for a strong acid-strong base titration and titration curves for a weak acid/base. Calculate the K sp from molar solubility and molar solubility from K sp. Calculate molar solubility in the presence of the common ion. Predict the effect of ph on solubility. Predicting whether a precipitate will form upon mixing solutions by comparing Q and K sp. Calculate the ion concentrations required to begin precipitation. Understand the process of complex formation and K f. Explain the effect of complex ion formation of solubility. Chapter 19 Understand the meaning of spontaneous process, reversible process, irreversible process, isothermal process. Be able to state the 2 nd law of thermodynamics. Describe the kinds of molecular motion for a molecule. Explain the relation of the entropy to the number of accessible microstates. Predict the sign of S for physical and chemical processes. State the 3 rd law of thermodynamics. Calculate standard entropy changes for a reaction from standard molar entropies. Calculate entropy changes in the surroundings for isothermal processes. Calculate the Gibbs free energy from the enthalpy and entropy changes at a given temperature. Predict whether a reaction will be spontaneous from the Gibbs free energy change. Calculate free energy change from standard free energies of formation. Predict the effect of temperature on the reaction spontaneity given H and S. Calculate G under non-standard conditions. Relate G and equilibrium constant. Chapter 20 Be able to identify reduction and oxidation processes, reducing and oxidizing agents in a chemical reaction. Complete and balance redox reaction equations by half-reaction method. Sketch a voltaic cell and identify the cathode, anode, and the direction of electrons flow. Calculate standard cell potentials (emf), E cell, from standard reduction potentials. Use standard reduction potentials to predict spontaneity of a redox-reaction. Relate E cell to G and equilibrium constants. Calculate the potential under nonstandard conditions (the Nernst equation). Calculate the equilibrium constant from the potential. Describe the reactions in the electrolytic cells. Predict the products of electrolysis. Relate the amounts of products of electrolysis to electric charge (Faraday s law). Chapter 21 Understand and be able to explain the difference between regular chemical reactions and nuclear reactions. 8

9 Write and balance nuclear reactions. Be able to predict nuclear stability in terms of neutron-to-proton ratio. Understand the kinetics of radioactive decay; be able to calculate ages of objects or amounts of radioactive material using half-life of isotopes. Know units of nuclear activity. Be able to calculate mass and energy changes for nuclear reactions. Understand the meaning of terms of radiation dosage. Understand the biological effects of different kinds of radiation. Good luck and have a great semester! 9