CHM 121: Chemistry II – Syllabus and Course Structure Overview

Course Overview

Introduction to Chemistry II

This course is the second in a two-course sequence introducing the fundamental concepts and principles of chemistry. It covers the physical and chemical properties of matter, chemical bonding, thermodynamics, kinetics, equilibrium, acids and bases, electrochemistry, and selected topics in descriptive chemistry. The course emphasizes both theoretical understanding and laboratory skills.

• Course Code: CHM 121

• Semester: Fall 2023

• Instructor: Prof. Eileen York

• Lecture Times: MWF, 8:00–8:50 AM

• Laboratory: Mondays, 11:00 AM–12:50 PM or Wednesdays, 2:00–3:50 PM

Course Learning Objectives

• To master a basic language of chemistry

• To develop conceptual understanding of physical and chemical factors influencing chemical reactivity

• To apply mathematical and graphical methods to chemical problems

• To develop an understanding of the nature of chemical equilibrium and rates of reaction

• To understand the energetics of chemical reactions

• To explore the chemistry of acids, bases, and buffers

• To develop laboratory skills for quantitative/qualitative data collection and analysis

Major Topics and Weekly Schedule

Topics Covered

The following topics are covered, corresponding to the chapters in the course textbook:

Week	Textbook Chapters	Topics	Laboratory
1	Ch. 9, 14	Gases; Chemical Equilibrium	Lab Check-in
2	Ch. 10	Thermochemistry	Lab 1: Molar Volume of a Gas
3	Ch. 11	Intermolecular Forces and Phase Changes	Lab 2: Physical Properties
4	Ch. 12	Solutions and Colligative Properties	Lab 3: Colligative Properties
5	Ch. 13	Kinetics of Chemical Reactions	Lab 4: Kinetics of a Reaction
6	Ch. 14	Chemical Equilibrium	Lab 5: Equilibrium Constant
7	Ch. 15	Acids and Bases	Lab 6: Acid-Base Titration
8	Ch. 16	Buffers, Titrations, and Solubility Equilibria	Lab 7: Buffer Solutions
9	Ch. 17	Electrochemistry	Lab 8: Specific Heat of a Metal
10	Ch. 18	Chemistry of Solids	Practical Titration Curve
11	Ch. 19	Introduction to Organic Chemistry	Thanksgiving Break
12	Review	Final Exam Preparation	Homework Week

Additional info: The schedule above is inferred from the syllabus table and may be subject to minor changes during the semester.

Assessment and Grading

Means of Evaluation

• Exams: 52.5%

• Quizzes: 7.5%

• Assignments (Homework, etc.): 12.5%

• Lab: 17.5%

• Participation: 10%

Final grades are assigned as follows:

Letter Grade	Percentage Range
A	93–100%
A-	90–92%
B+	87–89%
B	83–86%
B-	80–82%
C+	77–79%
C	73–76%
C-	70–72%
D+	67–69%
D	63–66%
F	0–62%

Laboratory Component

Lab Techniques and Procedures

The laboratory portion of the course is designed to reinforce lecture concepts and develop hands-on skills in experimental chemistry. Students are expected to:

• Follow safety protocols and proper lab techniques

• Collect and analyze quantitative and qualitative data

• Prepare lab reports summarizing methods, results, and conclusions

Example: In the "Molar Volume of a Gas" lab, students measure the volume of hydrogen gas produced in a reaction and use the ideal gas law to calculate molar volume.

Course Policies and Resources

• Attendance: Required for both lectures and labs

• Assignments: Due as scheduled; late work may not be accepted

• Academic Integrity: Plagiarism and cheating are strictly prohibited

• Accessibility: Accommodations available through the Office of Accessibility Services

• Resources: Supplemental instruction, tutoring, and online resources are available

Key General Chemistry II Topics (as covered in this course)

• Gases: Properties, laws (Boyle's, Charles's, Avogadro's), and the ideal gas law $PV = nRT$

• Thermochemistry: Energy changes in chemical reactions, enthalpy, calorimetry

• Intermolecular Forces: Types (dipole-dipole, hydrogen bonding, London dispersion), effects on boiling/melting points

• Solutions and Colligative Properties: Concentration units, effects on boiling/freezing points

• Kinetics: Reaction rates, rate laws, activation energy, catalysts

• Chemical Equilibrium: Dynamic equilibrium, equilibrium constant $K_{eq}$, Le Châtelier's Principle

• Acids and Bases: Definitions (Arrhenius, Brønsted-Lowry, Lewis), pH calculation $pH = -\log[H^+]$

• Buffers and Titrations: Buffer capacity, titration curves, Henderson-Hasselbalch equation $pH = pK_a + \log\left(\frac{[A^-]}{[HA]}\right)$

• Electrochemistry: Redox reactions, galvanic cells, standard reduction potentials

• Chemistry of Solids: Types of solids, crystal structures, properties

• Introduction to Organic Chemistry: Basic structure and nomenclature of organic molecules

Additional info: The above list is based on the syllabus schedule and standard General Chemistry II curriculum.

Example Equations and Concepts

• Ideal Gas Law: $PV = nRT$

• First Law of Thermodynamics: $\Delta E = q + w$

• Rate Law (for a reaction): $\text{Rate} = k[A]^m[B]^n$

• Equilibrium Constant: $K_{eq} = \frac{[C]^c[D]^d}{[A]^a[B]^b}$

• pH Calculation: $pH = -\log[H^+]$

• Henderson-Hasselbalch Equation: $pH = pK_a + \log\left(\frac{[A^-]}{[HA]}\right)$

• Gibbs Free Energy: $\Delta G = \Delta H - T\Delta S$

• Nernst Equation (Electrochemistry): $E = E^\circ - \frac{0.0592}{n} \log Q$

Study and Success Tips

• Attend all lectures and labs; participation is essential

• Review textbook chapters before and after class

• Complete all assignments and lab reports on time

• Utilize office hours, supplemental instruction, and tutoring resources

• Practice with online tutorials and past exam questions