Course Overview

General Chemistry II: Scope and Structure

General Chemistry II (ICCH 102) at Mahidol University International College is a foundational course designed for science students, building upon concepts introduced in General Chemistry I. The course covers advanced topics in chemistry, including solutions, equilibria, acids and bases, solubility, electrochemistry, chemical kinetics, main-group and transition elements, coordination compounds, nuclear chemistry, and selected topics in chemistry. The course aims to equip students with both qualitative and quantitative skills for understanding and applying chemical principles.

• Credits: 4 (lecture/lab/self-study)

• Prerequisite: ICCH 101 General Chemistry I

• Teaching Methods: Lecture, discussion, student presentation, exercises, and quizzes

• Assessment: Attendance, quizzes, homework, midterm, presentation, portfolio, and final exam

Course Topics and Weekly Outline

Major Topics Covered

The course is structured around the following key topics, each corresponding to a chapter in the recommended textbooks:

• Solutions (Properties, concentration, colligative effects)

• Chemical Equilibrium (Dynamic equilibrium, equilibrium constant, Le Chatelier's principle)

• Acids and Bases (Definitions, properties, pH calculations, titrations)

• Solubility and Complex-Ion Equilibria (Solubility product, common ion effect, complex ions)

• Electrochemistry (Redox reactions, electrochemical cells, Nernst equation)

• Chemical Kinetics (Reaction rates, rate laws, activation energy)

• Main-Group Elements (Properties and reactions)

• Transition Elements and Coordination Compounds (Coordination chemistry, ligand types, crystal field theory)

• Nuclear Chemistry (Radioactivity, nuclear reactions, applications)

Course Schedule

Weekly Breakdown

The following table summarizes the weekly schedule and topics:

Assessment and Grading

Evaluation Methods

• Attendance and Quizzes: 15%

• Online Individual Homework: 15%

• Midterm Examination: 30%

• Presentation: 5%

• Learning Portfolio: 5%

• Final Exam: 30%

All assessments are individual, but collaborative academic discussion is encouraged during class exercises. The MUIC grading scale applies: <60% for F and >=90% for A.

References and Resources

Recommended Textbooks

• Petrucci's General Chemistry: Principles and Modern Applications (12th ed., 2023)

• Chemistry by Zumdahl (11th ed., 2024)

• Atkins' Physical Chemistry (12th ed., 2022)

Additional resources include books published by ACS and NSTDA, as well as online materials provided via CANVAS and Google Drive.

Course Policies and Additional Information

Attendance and Academic Honesty

• 80% attendance required to take the final exam

• Three late attendances (15 minutes or more) equal one absence

• MUIC policies regarding uniform and academic honesty apply at all times

Learning Management System

• CANVAS is the primary platform for course announcements, materials, and submissions

• Google Drive is used for accessing shared files

Appeal Procedure

• Scores are available on CANVAS on the same day as quizzes and exams

• Students must dispute scores within 72 hours of release

Important Links

• CANVAS Login

• Crowdsourced Notes

• Tutoring Information

Course QR Code

The following QR code provides quick access to the course's CANVAS page or related resources:

Summary of Key Chemistry Topics

Solutions

Solutions are homogeneous mixtures of two or more substances. Key properties include concentration (molarity, molality), solubility, and colligative properties (boiling point elevation, freezing point depression).

• Molarity (M):

• Molality (m):

• Colligative Properties: Depend on the number of solute particles, not their identity.

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.

• Equilibrium Constant (K): (for a given reaction)

• Le Chatelier's Principle: A system at equilibrium will adjust to counteract changes in concentration, temperature, or pressure.

Acids and Bases

Acids and bases are defined by their ability to donate or accept protons (Brønsted-Lowry) or produce/accept hydroxide ions (Arrhenius). The pH scale measures acidity.

• pH:

• Acid-Base Titration: Used to determine concentration of an acid or base.

Solubility and Complex-Ion Equilibria

Solubility product (Ksp) describes the equilibrium between a solid and its ions in solution. Complex ions form when metal ions bind to ligands.

• Solubility Product:

• Common Ion Effect: Addition of a common ion decreases solubility.

Electrochemistry

Electrochemistry studies redox reactions and the generation of electrical energy from chemical reactions. Key concepts include electrochemical cells and the Nernst equation.

• Cell Potential:

• Nernst Equation:

Chemical Kinetics

Chemical kinetics examines the rates of chemical reactions and the factors affecting them, such as concentration, temperature, and catalysts.

• Rate Law:

• Activation Energy: Minimum energy required for a reaction to occur.

Main-Group and Transition Elements

Main-group elements include s- and p-block elements, while transition elements are d-block metals. Their properties and reactions are central to inorganic chemistry.

• Coordination Compounds: Complexes formed by transition metals and ligands.

• Crystal Field Theory: Explains color and magnetism in transition metal complexes.

Nuclear Chemistry

Nuclear chemistry involves the study of radioactive decay, nuclear reactions, and their applications in energy and medicine.

• Radioactive Decay:

• Half-Life: Time required for half of a radioactive sample to decay.

Additional info: The QR code included is directly relevant as it provides access to course resources and is referenced in the syllabus for student use.