CHEM 1212
Principles of Chemistry II
Spring 2016
Instructor
Dr. Sharmistha Basu-Dutt
Office: TLC- 2136
E-mail: sbdutt@westga.edu
Phone: (678)839-6018
Office Hours:
M, W: 10 am – noon
T, R: 2 pm – 3 pm
Purpose
This is the second course in a two-semester sequence covering the fundamental principles and
applications of chemistry for science majors. The course satisfies Core Requirement in Area D.
The “flipped” classroom model will be used in lecture to promote active student learning as
well as logical thinking and analytical reasoning in problem solving.
Textbook
Chemistry: Structure and Properties by Nivaldo J. Tro, 1st edition, Pearson is required. Students
Solutions Manual accompanying textbook is optional.
Learning Outcomes
Each student will:
 acquire a basic understanding of chemical bonding, equilibrium, kinetics, thermodynamics.
 apply scientific reasoning and methods of inquiry to explain natural phenomena.
 use appropriate scientific tools and instruments to acquire data, process information, and
communicate results
Academic Honesty Policy
We take academic honesty very seriously. Plagiarism of any sort will not be tolerated. Plagiarism
is the use of someone else’s ideas or words as your own. This definition includes copying
another student’s exam or assignment, as well as using material from a book or Internet site
without acknowledging the source. If you plagiarize any part of an assignment for this course,
you will receive a zero for the entire assignment, and disciplinary action will be taken. UWG
Academic
Integrity
and
Honor
Code
Pledge
is
available
at
http://www.westga.edu/handbook/59.php.
Course Policies and Guidelines
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The official communication method between the instructor and students will be through
campus e-mail (myUWG email account).
Some of the course materials including the syllabus, class-notes, sample exams are available
through Course Den. You will be responsible to print notes.
The class meets on Mondays and Wednesdays from 12:30 pm – 1:50 pm in TLC 2105 AND
the lab meets on Fridays from noon – 1:50 pm in TLC 3108. Please come to class on time,
and do not leave early. Remember to fill your water bottle or use the restroom before class.
You are expected to behave professionally in this course, which means considering the
effect that your behavior will have on other people involved in the course. Use of cell
phones and/or personal laptops will not be allowed during lecture and lab.
No make up quizzes or exams will be given. In case of an illness or a dire emergency, the
instructor must be contacted prior to the examination in-person, via phone or email.
Accommodations for missed exams, quizzes and assignments will be handled depending on
the severity of the situation between the student and the instructor.
In-Class/Take-Home Assignments
These assignments include announced/unannounced quizzes where you may need to use a
scientific calculator and textbook. Remember to bring your calculators and textbooks to class
every day since you cannot share these resources. You must be present in class to get credit for
in-class assignments or submit take-home assignments on the due date.
Examinations
There will be four examinations and a comprehensive final examination during the semester.
Each examination will be closed book and notes. You will need to bring a calculator to the tests.
If necessary, I will provide the scantron sheets, periodic charts and conversion tables. The
standardized examination (multiple choice) from the American Chemical Society will serve as
the final examination. If there is a conflict with the final exam time, you must provide me with
written authorization from the Dean of Science and Mathematics to move your final exam time.
Semester Grades
All exam and quiz grades will be based on your ability to DEMONSTRATE full understanding
of the material. Full credit will only be given if you SHOW ALL YOUR WORK, not just for
obtaining the correct answer. Your grade will be calculated based on the following components:
In-class exams (4 @ 100 points each)
Final (Comprehensive)
In-class assignments
TOTAL
400 points
100 points
100 points
600 points
The grading scale will be as follows: 90% : A; 80 – 89% : B; 70 – 79% : C; 60 – 69% : D; <
60% : F
Tentative Schedule for the Course
WEEK
Monday
Wednesday
1
January 11 – Chapter 12
January 13 – Chapter 12
2
January 18 – No class
January 20 – Chapter 12
3
January 25 – Chapter 13
January 27 – Chapter 14
4
February 1 – EXAM 1
February 3 – Chapter 14
5
February 8 – Chapter 14
February 10 – Chapter 15
6
February 15 – Chapter 15
February 17 – Chapter 15
7
February 22 – Chapter 15
February 24 – EXAM 2
8
February 29 – Chapter 16
March 2 – Chapter 16
9
March 7 – Chapter 17
March 9– Chapter 17
10
March 21 – Chapter 18
March 23 – Chapter 18
11
March 28 – Chapter 18
March 30 – EXAM 3
12
April 4 – Chapter 19
April 6 – Chapter 19
13
April 11 – Chapter 19
April 13 – Chapter 20
14
April 18 – Chapter 20
April 20 – EXAM 4
15
April 25 – No class
April 27 – FINALS
(11 am – 1:30 pm)
Homework – won’t be graded but will help to prepare for tests
Chapter 12: 35, 37, 39, 41, 43, 45, 47, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 79
Chapter 13: 19, 21, 23
Chapter 14: 25, 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 51, 55, 59, 61, 63, 67, 69, 73, 77, 81,
83, 85, 89
Chapter 15: 27, 29, 37, 39, 41, 43, 45, 49, 51, 53, 55, 57, 59, 61, 63, 65, 67, 69, 71, 77
Chapter 16: 21, 23, 25, 27, 29, 31, 33, 35, 37, 39, 41, 43, 45, 47, 49, 53, 55, 57, 61, 71
Chapter 17: 33, 39, 41, 47, 49, 51, 55, 59, 61, 65, 69, 71, 73, 77, 85, 87, 93, 99, 103, 109
Chapter 18: 27, 29, 31, 35, 39, 41, 43, 45, 47, 49, 53, 59, 61, 67, 69, 71, 73, 79, 83, 87
Chapter 19: 25, 27, 29, 35, 37, 41, 43, 45, 49, 51, 53, 55, 59, 61, 63, 65, 67, 69, 71, 75
Chapter 20: will be assigned later
Topics to read in the book
12
Liquids, Solids, and Intermolecular Forces
12.1
12.2
12.3
12.4
Structure Determines Properties
Solids, Liquids, and Gases: A Molecular Comparison
Intermolecular Forces: The Forces That Hold Condensed States Together
Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
12.5
12.6
Sublimation and Fusion
12.7
Heating Curve for Water
12.8
13
13.3
Vaporization and Vapor Pressure
Water: An Extraordinary Substance
Phase Diagrams and Crystalline Solids
13.1
Sliding Glaciers
13.2
Phase Diagrams
Crystalline Solids: Determining Their Structure by X-Ray Crystallography
13.4
Crystalline Solids: Unit Cells and Basic Structures
13.5
Crystalline Solids: The Fundamental Types
13.6
13.7
The Structures of Ionic Solids
Network Covalent Atomic Solids: Carbon and Silicates
14
14.1
14.2
Energetics of Solution Formation
Solution Equilibrium and Factors Affecting Solubility
14.5
14.6
Antifreeze in Frogs
Types of Solutions and Solubility
14.3
14.4
Solutions
Expressing Solution Concentration
Colligative Properties: Vapor Pressure Lowering, Freezing Point Depression, Boiling Point Elevation,
and Osmotic Pressure
14.7
Colligative Properties of Strong Electrolyte Solutions
15
Chemical Kinetics
15.1
15.2
15.3
15.4
15.5
Catching Lizards
Rates of Reaction and the Particulate Nature of Matter
Defining and Measuring the Rate of a Chemical Reaction
The Rate Law: The Effect of Concentration on Reaction Rate
The Integrated Rate Law: The Dependence of Concentration on Time
15.6
The Effect of Temperature on Reaction Rate
15.7
Reaction Mechanisms
15.8
16
16.1
16.2
16.5
16.6
The Concept of Dynamic Equilibrium
The Equilibrium Constant (K)
Expressing the Equilibrium Constant in Terms of Pressure
Heterogeneous Equilibria: Reactions Involving Solids and Liquids
Calculating the Equilibrium Constant from Measured Equilibrium Concentrations
16.7
The Reaction Quotient: Predicting the Direction of Change
16.8
16.9
Chemical Equilibrium
Fetal Hemoglobin and Equilibrium
16.3
16.4
Catalysis
Finding Equilibrium Concentrations
Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
17
Acids and Bases
17.1
17.2
The Nature of Acids and Bases
17.3
Definitions of Acids and Bases
17.4
17.5
Acid Strength and Molecular Structure
Acid Strength and the Acid Ionization Constant (Ka)
17.6
17.7
Batman’s Basic Blunder
Autoionization of Water and pH
Finding the [H3O+] and pH of Strong and Weak Acid Solutions
17.8
Finding the [OH-] and pH of Strong and Weak Base Solutions
17.9
The Acid–Base Properties of Ions and Salts
17.10 Polyprotic Acids
17.11 Lewis Acids and Bases
18
Aqueous Ionic Equilibrium
18.1
18.2
18.3
The Danger of Antifreeze
Buffers: Solutions That Resist pH Change
Buffer Effectiveness: Buffer Range and Buffer Capacity
18.4
18.5
Titrations and pH Curves
Solubility Equilibria and the Solubility Product Constant
18.6
18.7
19
19.5
19.8
Energy Spreads Out
19.2
Spontaneous and Nonspontaneous Processes
19.3
Entropy and the Second Law of Thermodynamics
Predicting Entropy and Entropy Changes for Chemical Reactions
Heat Transfer and Entropy Changes of the Surroundings
19.6
19.7
Complex Ion Equilibria
Free Energy and Thermodynamics
19.1
19.4
Precipitation
Gibbs Free Energy
Free Energy Changes in Chemical Reactions: Calculating
Free Energy Changes for Nonstandard States: The Relationship between and
19.9
Free Energy and Equilibrium: Relating to the Equilibrium Constant (K)