General Chemistry II Syllabus and Study Guide

General Chemistry II: Course Overview

Course Structure and Content

This course covers advanced topics in general chemistry, focusing on the study of the states of matter, thermochemistry, solutions, kinetics, equilibrium, and related chemical principles. It is designed for students who have completed introductory chemistry and are seeking a deeper understanding of chemical processes and their applications.

• Course Number: CH 221Z

• Credits: 4

• Prerequisites: CH 221 or CH 221Z with C- or better, or CH 231 with C- or better, or equivalent.

• Topics Covered: Thermochemistry, Gases, Liquids and Solids, Solutions, Chemical Kinetics, Chemical Equilibrium.

Course Topics and Weekly Breakdown

Thermochemistry

Thermochemistry explores the energy changes that occur during chemical reactions and physical changes. It is essential for understanding how energy is transferred and conserved in chemical systems.

• Key Concepts: Heat, work, internal energy, enthalpy, calorimetry.

• Important Equations:

  • $q = m c \Delta T$ (heat transfer)

  • $\Delta H = \Delta E + P \Delta V$ (enthalpy change)

• Example: Calculating the heat absorbed by water when its temperature increases.

Gases

The study of gases involves understanding their properties, behavior, and the laws that govern them. The kinetic molecular theory provides a molecular-level explanation for gas laws.

• Key Concepts: Pressure, volume, temperature, ideal gas law, kinetic molecular theory.

• Important Equations:

  • $PV = nRT$ (Ideal Gas Law)

  • $P_1V_1/T_1 = P_2V_2/T_2$ (Combined Gas Law)

• Example: Determining the volume of a gas at different temperatures and pressures.

Liquids and Solids

This topic covers the physical properties of liquids and solids, including intermolecular forces, phase changes, and the structure of solids.

• Key Concepts: Intermolecular forces, boiling and melting points, phase diagrams, crystalline and amorphous solids.

• Example: Comparing boiling points of substances based on intermolecular forces.

Solutions

Solutions are homogeneous mixtures of two or more substances. This section examines solution formation, concentration units, and factors affecting solubility.

• Key Concepts: Solubility, concentration (molarity, molality), colligative properties.

• Important Equations:

  • $M = \frac{\text{moles of solute}}{\text{liters of solution}}$ (Molarity)

  • $\Delta T_f = K_f m$ (Freezing point depression)

• Example: Calculating the molarity of a solution prepared by dissolving a known mass of solute.

Chemical Kinetics

Chemical kinetics studies the rates of chemical reactions and the factors that influence them, such as concentration, temperature, and catalysts.

• Key Concepts: Reaction rate, rate laws, activation energy, catalysts.

• Important Equations:

  • $\text{Rate} = k[A]^m[B]^n$ (General rate law)

  • $k = A e^{-E_a/RT}$ (Arrhenius equation)

• Example: Determining the rate constant from experimental data.

Chemical Equilibrium

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

• Key Concepts: Dynamic equilibrium, equilibrium constant ($K$), Le Châtelier's principle.

• Important Equations:

  • $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$ (Equilibrium constant expression)

• Example: Predicting the effect of changing concentration or temperature on equilibrium position.

Course Specific Measurable Student Learning Outcomes

• Apply stoichiometry to a variety of chemical systems.

• Apply kinetic molecular theory and gas laws to predict the behavior of gases.

• Identify types of intermolecular forces and apply them to physical properties of solids, liquids, and solutions.

• Describe the effects of concentration and factors affecting solution properties.

• Analyze chemical changes and factors on chemical reaction rates and examine the mechanisms of chemical reactions.

• Describe the relationship between thermochemistry, energy transfer, and the energy changes in chemical reactions.

• Explain and apply concepts of equilibrium in gas, solution, and collective systems, including acid-base and solubility equilibria.

Grading Scale

Grade	Percent 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
D-	60-62
F	0-59

Assessment and Assignments

• Pre-Class Quizzes: Short quizzes to prepare for each class session.

• Weekly Quizzes: Comprehensive quizzes covering weekly material.

• Homework: Online assignments and adaptive follow-ups for practice.

• Midterm Exams: In-person exams testing understanding of major topics.

• Final Exam: Comprehensive assessment of all course material.

• Participation: Collaborative group activities and engagement in class.

Course Policies and Support

• Academic Integrity: Commitment to honesty and ethical conduct in all coursework.

• AI Policy: Use of AI applications is not permitted for assignments.

• Support Services: Resources available for academic and personal support.

• Student Learning Experience Survey: Feedback opportunity for course improvement.