CHEMISTRY IIBSP

CHEM 502

Equilibrium and Thermochemistry

Syllabus for Summer 2009

Instructors:Robert Huie, Elizabeth Mtembu, Jason Evans

TA:Dong Zheng
E-mail:
Telephone: 617-287-6149
Office hours:before or after class
Office: RM Science 1-084

Dates: July 20-31
Class time: M-F8:30-3:00 in Science 1-025

Objective:This course is a part of the core group of courses supporting the Boston Science Partnership initiative. This course focuses on energetics of chemical reactions and it is designed to support the professional development of high school and middle school teachers in the Greater Boston area. The course combines advancedchemistry content while modeling sound pedagogy. Using current and future curriculum materials, as well as State and National standards for the teaching of chemistry at the high school level, this course offers an in-depth exploration of fundamental principles of equilibrium, solubility, acid-base reaction, electrochemistry, and thermodynamics. A major component of this course will involve working in groups to produce new laboratory exercises that can be used in middle school or high school curricula.

Textbook:Chemistry, The Molecular Nature of Matter and Change, 4th Ed. by Silberberg

Supplementary Works:

Quantitative Chemical Analysis, 6th Ed. Harris

Fundamentals of Analytical Chemistry, 7th Ed. Skoog, West, Holler

Principles of Instrumental Analysis, 6th Ed. Skoog, Holler, Crouch

Chemical Principles The Quest for Insight 4th Ed. Atkins and Jones

Science Curriculum Topics Study Bridging the Gap Between Standards and Practice,

Keeley

How People Learn, Brain, Mind, Experience, and School, National Research Council

Living by Chemistry; Alchemy, Smells, Weather, Fire, Toxins, Angela Stacy

Grading:

Pretest

Taken on first day, 0 pts

Lab Work

30 pts; Six Laboratory Exercises, 5pts each

Homework 15

15 pts; Three Homework Assignments

Development of Original Laboratory Exercises

30 pts; Five assignments, 6 pts each

Presentation:

10 pts

Final Exam

Absolute score, 10pts

Improvement over pre-test, 5pts

Grading Scale:

You must accumulate 80 points to earn a B and 90 points to earn an A.

Attendance: You are expected to attend the ten days of class in their entirety. This is a 2-week course. As a result, no opportunity to make-up any course work will be provided. If you miss substantial segments (over 1 hr) on more than one day without prior approval, you will be given a failing grade for the course.

Academic dishonesty:It is expected that all work will be a collaborative effort, except for the pre-test and post-test, which are only worth 15 % of the total grade. Cheating on the exams will not be tolerated.

Homework:

You will be given problem sets out of the book that will be collected and graded the next day of class.

Lecture Schedule:

An example of a typical day

Morning:

Go over homework problems/working on laboratory projects

Introduction of daily topic

Classroom demo

Short lecture

Problem solving session

Classroom demo

Introduction to daily laboratory exercise

Lunch:

Afternoon:

Laboratory exercise

Data analysis

Completing laboratory report

Working on laboratory projects and homework

day / Notes and Suggested Problems / Chapter
1 / Pre-test
1 / Material: Course overview, Avogadro’s number; Classification of reactions, Stoichiometry, Energetics of Reactions, Calorimetry / 3, 6, 4
1 / Lab Work, Experiment 1: Investigating Reaction Stoichiometry
1 / Assign Problem set 1,
Ch 3; 14, 18, 28, 37, 39, 53, 65, 77, 81, 96
Ch 4; 31, 45, 49, 74, 91, 93
Ch 6; 26, 35, 50, 63, 77
2 / Calorimetry, thermodynamics, G, H, S, intermolecular interactions, hydrogen bonding
2 / Lab Work, Experiment 2: Thermodynamics of Mixing
3 / Go over problem set 1, Assign Problem set 2,
Ch 17; 12, 16, 20, 27, 31, 35, 49, 51, 63, 71, 65
Ch 18; 11, 13, 15, 25, 27, 51, 65, 69, 77, 94, 108, 121, 143
Ch 19; 15, 27, 56, 58
3 / acid-base chemistry, pH, weak acid/base equilibrium, buffers / 18
4 / Lab 3: Spectrometric Determination of the Acid Dissociation Constant of an Acid-base Indicator / 18
4 / Project Development
5 / Equilibrium, Le Chatelier’s Principle / 17
5 / Lab 4: Alkalinity and Buffer Capacity
5 / Go over problem set 2; Assign Problem set 3,
Ch 19; 70, 80, 86, 96, 98, 104
Ch 21; 10, 14, 27, 29, 42, 46, 58, 66, 70
6 / Titrations, polyprotic systems, solubility Ksp, common ion effect / 19
6 / Project Development
7 / Lab work; Experiment 5: Solubility of CaSO4
7 / Activity, ion-selective electrodes, experimental design
8 / Redox reactions, half-reactions, Nernst Equation Electrocemical cells, reference electrodes indictor electrodes, ion-sensitive electrodes, Redox titrations
9 / Go over Problem set 3 / 21
9 / Lab work; Experiment 5: Determining Relative Standard Reduction Potentials of Various Metals
9 / Work in small groups on various problem sets, project design, or advanced materials in preparation for the exam
9 / Review for exam
10 / Exam
10 / 15 minute presentations
10 / Course Evaluation
10

Laboratory Projects:

After each laboratory experiment you will be arranged in small, homogeneous (according to the grade that you teach) groups of three or four. You will be asked to brain storm ideas for developing a novel laboratory exercise appropriate to use in your classrooms that is loosely related to the topic investigated in the laboratory experiment performed earlier. You will then be group heterogeneously to exchange ideas. Finally you will get together with your previous homogeneous group to work on a detailed proposal. You will decide on a proposed exercise, define the target grade level and the learning goals, outline the procedure, and develop a grading rubric. You will get to work on this project the next day, as well, and you will hand your work in the following day.

Presentations: You will present have 15 minutes to present a lesson that you feel works really well for you in class. It can be on any science topic. Choose a topic that is challenging, but yet one that you have developed a unique approach to that works well in your classroom. The goal is to share your approach towards teaching a generally difficult topic with you classmates and instructors.

Homework Assignments

Assign 1
Section / Questions / Goals
3.1-3.3 / 14,15 / g-mol-rp
18,19 / % composition
28,29 / Combination
3.4-3.6 / 37,38 / empirical formula
39,40 / molecular formula
53,54 / balancing reactions
3.8-3.12 / 65,66 / Stoichiometry
77,78 / limiting reactant
81,82 / % yield
3.13-3.17 / 96,97 / solution chemistry
4.3 / 31,32 / precipitiation rx
4.4-4.5 / 45,46 / Acid base rx
49,50 / acid base titration
4.6-4.9 / 74,75 / balancing redox
"4.10" / 91,92 / redox agents
93,94 / stoichiometry redox
6.2 / 26,27 / endo-exothermic
6.3-6.5 / 35,36 / heat capacity
6.6 / 50,51 / enthalpy rx
6.7 / 63,64 / Hess's Law
6.8-6.9 / 77,78 / enthalpy formation
Assign 2
17.1-17.3 / 12,13 / Qc
16,17 / Kc
20,21 / hetero equil
17.4 / 27,28 / ∂n gas
31,32 / Kc vs Kp
17.5 / 35,36 / Q vs. K
17.6 / 49,50 / Equilibrium
"17.10" / 51,52 / "
17.11 / 63,64 / LeChatelier
71,72 / ∂H vs K
65,66 / V vs K
18.1 / 11,12 / Ka expression
13,14 / acid strength
15,16 / acid base strength
18.2-18.3 / 27,28 / pH
25,26 / Kw vs pH
18.4-18.5 / 51,52 / net ionic
55,56 / net direction
18.6-18.8 / 65,66 / Ka equation
69,70 / % dissociation
77,78 / Kz vs % dissociation
18.9-18.10 / 94,95 / Ka vs Kb
108,109 / acid strength
18.11-18.12 / 121,122 / salt A-B
18.13 / 143,144 / Arrhenius B-L, Lewis
19.1-19.2 / 15,16 / Henderson Hasselbach
27,28 / Buffer
19.3 / 56,57 / Titration
58,59 / equivalence point
Assign 3
19.4-19.9 / 70,71 / Ksp vs solubility
80,81 / solubility vs Ksp
86,87 / precipitation vs Ksp
19.10-19.11 / 96,97 / Kf equations
98,99 / complex formation
19.12 / 104,105 / Ionic quant analysis
21.1 / 10,11 / Redox
14,15 / balancing redox
21.2 / 27,28 / voltaic cells
29,30 / voltaic cell observation
21.3-21.4 / 42,43 / balance, E, ∂G
46,47 / strength of oxidizers
21.5-21.7 / 58,59 / K vs E
66,67 / K vs E vs ∂G
70,71 / nernst equation