Course Overview

Introduction to Honors General Chemistry 2

This course is the second part of a two-semester general chemistry sequence, designed for students in the Honors College. It covers advanced topics in chemistry, including solutions, thermodynamics, equilibrium, acids and bases, electrochemistry, and nuclear chemistry. The course emphasizes quantitative reasoning, laboratory skills, and the application of chemical principles to real-world problems.

• Prerequisites: CHM 2045, CHM 2045L

• Course Objectives: Develop understanding of chemical concepts, problem-solving skills, and laboratory techniques.

Course Topics and Chapter Mapping

Major Topics Covered

The following topics are covered in the course, mapped to textbook chapters and aligned with the General Chemistry curriculum:

• Solutions and Colligative Properties (Ch. 14)

• Thermochemistry and Thermodynamics (Ch. 15, 16)

• Chemical Equilibrium (Ch. 17, 18, 19, 20)

• Acids, Bases, and Buffers (Ch. 19)

• Electrochemistry (Ch. 21)

• Nuclear Chemistry (Ch. 22)

• Polymeric and Organic Chemistry (Ch. 23)

Detailed Topic Breakdown

Solutions and Colligative Properties

Solutions are homogeneous mixtures of two or more substances. Colligative properties depend on the number of solute particles in a solution, not their identity.

• Solution Formation: The process by which solutes dissolve in solvents to form a solution.

• Vapor Pressure of Solutions: The reduction in vapor pressure due to the presence of solute particles.

• Osmotic Pressure: The pressure required to stop osmosis, given by .

• Boiling Point Elevation and Freezing Point Depression: Changes in boiling and freezing points due to solute addition.

• Example: Salt added to water increases boiling point and decreases freezing point.

Thermochemistry and Thermodynamics

Thermochemistry studies the energy changes during chemical reactions, while thermodynamics deals with the laws governing energy and entropy.

• Heat of Reaction: The enthalpy change () during a chemical reaction.

• First Law of Thermodynamics: Energy cannot be created or destroyed, only transformed.

• Second Law of Thermodynamics: Entropy () of the universe increases in spontaneous processes.

• Gibbs Free Energy: determines spontaneity.

• Example: Combustion reactions release heat and increase entropy.

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 (): at equilibrium.

• Le Châtelier's Principle: The system shifts to counteract changes in concentration, pressure, or temperature.

• Example: Increasing reactant concentration shifts equilibrium toward products.

Acids, Bases, and Buffers

Acids donate protons (), bases accept protons, and buffers resist changes in pH.

• Acid-Base Equilibria: and express the strength of acids and bases.

• Buffer Solutions: Mixtures of weak acids and their conjugate bases that maintain pH.

• Example: Acetic acid and sodium acetate form a buffer.

Electrochemistry

Electrochemistry studies chemical reactions that involve electron transfer, including galvanic cells and electrolysis.

• Galvanic Cells: Devices that convert chemical energy into electrical energy.

• Cell Potential ():

• Nernst Equation:

• Example: Zinc-copper cell generates electricity from redox reactions.

Nuclear Chemistry

Nuclear chemistry focuses on reactions involving changes in atomic nuclei, such as radioactive decay and nuclear fission.

• Radioactive Decay: Spontaneous emission of particles or energy from unstable nuclei.

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

• Nuclear Fission and Fusion: Splitting or combining nuclei to release energy.

• Example: Uranium-235 undergoes fission in nuclear reactors.

Polymeric and Organic Chemistry

Polymeric chemistry studies large molecules made of repeating units, while organic chemistry focuses on carbon-containing compounds.

• Polymers: Long chains of repeating monomer units.

• Organic Compounds: Molecules containing carbon, hydrogen, and other elements.

• Example: Polyethylene is a common polymer used in plastics.

Course Grading Scale

Grading Table

The following table summarizes the grading scale used in the course:

Additional Academic Information

• Instructional Methods: Lectures, online assignments, and exams.

• Required Textbook: "Chemistry: The Molecular Nature of Matter and Change" by Silberberg et al.

• Technology Requirements: Computer with internet access, webcam, microphone, and recommended browsers.

• Policies: Attendance, makeup work, academic integrity, and disability accommodations are strictly enforced.

Additional info: The syllabus provides a comprehensive outline of topics, grading, and policies for a General Chemistry 2 course, suitable for exam preparation and academic planning.