General Chemistry II: Course Syllabus and Study Guide

Course Overview

This course syllabus outlines the weekly topics, key questions, laboratory activities, and homework assignments for a second-semester general chemistry course. The curriculum covers advanced concepts in chemical solutions, kinetics, equilibrium, acids and bases, thermodynamics, and electrochemistry.

Weekly Topics and Study Guide

Week 1: Molecular Interactions and Structure-Property Relationships

• Main Questions: How do molecules interact? How does structure influence properties?

• Key Concepts:

  • Intermolecular Forces (IMFs): Types include London dispersion, dipole-dipole, hydrogen bonding.

  • Structure-Property Relationships: Molecular geometry and bonding affect boiling/melting points, solubility, and reactivity.

• Preparation: Math review, review Chapters 3-4, read Chapters 12 and 14.

• Lab: No lab this week.

• Homework: Chapter 14.

Week 2: Mixtures and Solution Concentrations

• Main Questions: How are mixtures defined? How can I convert between units of concentration? How does mixture concentration determine properties?

• Key Concepts:

  • Mixtures: Homogeneous (solutions) vs. heterogeneous mixtures.

  • Concentration Units: Molarity (M), molality (m), percent composition, mole fraction.

  • Colligative Properties: Properties that depend on solute concentration, not identity (e.g., boiling point elevation, freezing point depression).

• Preparation: Review Chapter 5, read Chapter 14.

• Lab: Intermolecular Forces (IMFs).

• Homework: Chapter 14.

Week 3: Chemical Kinetics – Reaction Rates

• Main Questions: How is reaction speed defined and measured? What is the difference between rate law, rate constant, and rate?

• Key Concepts:

  • Reaction Rate: Change in concentration of reactant or product per unit time.

  • Rate Law: Mathematical relationship between rate and concentration: $\text{rate} = k [A]^m [B]^n$

  • Rate Constant (k): Proportionality constant specific to a reaction at a given temperature.

• Preparation: Read Chapter 15, pp. 631-649.

• Lab: Concentration effects on rate.

• Homework: Chapter 15.

Week 4: Chemical Kinetics – Graphical Analysis and Structure Effects

• Main Questions: How do I analyze graphs in chemical kinetics? How does reaction speed relate to chemical structure?

• Key Concepts:

  • Graphical Analysis: Determining reaction order from concentration vs. time plots.

  • Integrated Rate Laws: For first-order: $\ln [A]_t = -kt + \ln [A]_0$

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

• Preparation: Read Chapter 15, pp. 650-666.

• Lab: Colligative properties.

• Homework: Chapter 15.

• Exam 1: February 13.

Week 5: Chemical Equilibrium – Introduction

• Main Questions: How can reactions go backwards? What is equilibrium? How is the equilibrium constant defined and used?

• Key Concepts:

  • Dynamic Equilibrium: Forward and reverse reactions occur at equal rates.

  • Equilibrium Constant (K): $K = \frac{[C]^c [D]^d}{[A]^a [B]^b}$ for reaction $aA + bB \rightleftharpoons cC + dD$

• Preparation: Read Chapter 15, pp. 650-666 and Chapter 16.

• Lab: Kinetics.

• Homework: Chapter 16.

Week 6: Chemical Equilibrium – Calculations and ICE Charts

• Main Questions: Are states of matter relevant to equilibrium? How is a non-equilibrium condition defined? How do I solve an ICE chart?

• Key Concepts:

  • Phases in Equilibrium: Only gases and aqueous species appear in K expressions.

  • Reaction Quotient (Q): Used to determine direction of shift to reach equilibrium.

  • ICE Chart: Table for Initial, Change, and Equilibrium concentrations.

• Preparation: Read Chapter 16 and Chapter 17, pp. 731-757.

• Lab: Kinetics.

• Homework: Chapter 17.

Week 7: Acids and Bases – Definitions and Calculations

• Main Questions: How are acids and bases defined using equilibrium? How do I calculate pH? What’s the difference between weak and strong acids?

• Key Concepts:

  • Acid-Base Definitions: Arrhenius, Brønsted-Lowry, Lewis.

  • pH Calculation: $\text{pH} = -\log [H^+]$

  • Strong vs. Weak Acids: Strong acids dissociate completely; weak acids only partially.

• Preparation: Read Chapter 17, pp. 731-757.

• Lab: Equilibrium.

• Homework: Chapter 17.

• Exam 2: March 6.

Week 8: Acids and Bases – Basic Solutions and Predicting Acidity/Basicity

• Main Questions: How do I calculate pH for a basic solution? How do I predict the acidity/basicity of a chemical?

• Key Concepts:

  • pOH and pH Relationship: $\text{pOH} = -\log [OH^-]$, $\text{pH} + \text{pOH} = 14$

  • Acid/Base Strength: Determined by structure, electronegativity, resonance, and inductive effects.

• Preparation: Read Chapter 17, pp. 758-775 and Chapter 18, pp. 787-816.

• Lab: Acid-Base.

• Homework: Chapter 18.

Week 9: Acids and Bases – Buffers and Titrations

• Main Questions: What makes strong acids strong? How does a buffer work? How do I calculate pH during a titration?

• Key Concepts:

  • Buffer Solutions: Resist changes in pH; made from weak acid/base and its conjugate.

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

  • Titration Curves: Show pH changes as titrant is added.

• Preparation: Read Chapter 18.

• Lab: Acid-Base.

• Homework: Chapter 18.

Week 10: Solubility and the Common Ion Effect

• Main Questions: How does equilibrium apply to solubility? What is the common ion effect?

• Key Concepts:

  • Solubility Product Constant (Ksp): $K_{sp} = [A^+]^m [B^-]^n$ for $A_mB_n$

  • Common Ion Effect: Solubility decreases when a common ion is added.

• Preparation: Read Chapter 18, pp. 817-833; review Chapter 7.

• Lab: Acid-Base.

• Homework: Chapter 18.

Week 11: Precipitation, Entropy, and Energy Relationships

• Main Questions: How can I predict precipitations using equilibrium data? What is entropy and how does it relate to energy? What is the relationship between equilibrium and energy?

• Key Concepts:

  • Precipitation: Occurs when $Q > K_{sp}$.

  • Entropy (S): Measure of disorder; increases with number of microstates.

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

• Preparation: Review Chapter 7, read Chapter 18, pp. 817-833, and Chapter 19.

• Lab: Solubility.

• Homework: Chapter 19.

Week 12: Thermodynamics – Standard States and Spontaneity

• Main Questions: What are standard state conditions? How is spontaneity defined?

• Key Concepts:

  • Standard State: 1 atm pressure, 1 M concentration, 25°C (298 K).

  • Spontaneity: A process is spontaneous if $\Delta G < 0$.

• Preparation: Read Chapter 19.

• Lab: Thermodynamics.

• Homework: Chapter 19.

• Exam 3: April 17.

Week 13: Electrochemistry – Redox Reactions and Electrochemical Cells

• Main Questions: What are reduction and oxidation reactions? What are the parts of an electrochemical cell? How do I balance redox reactions?

• Key Concepts:

  • Redox Reactions: Involve transfer of electrons; oxidation is loss, reduction is gain.

  • Electrochemical Cell Components: Anode (oxidation), cathode (reduction), salt bridge.

  • Balancing Redox: Use half-reaction method.

• Preparation: Read Chapter 20.

• Lab: Electrochemistry.

• Homework: Chapter 20.

Week 14: Electrochemistry – Cell Potentials and Review

• Main Questions: How do I determine the spontaneity of an electrochemical reaction?

• Key Concepts:

  • Cell Potential (Ecell): $E_{cell} = E_{cathode} - E_{anode}$

  • Spontaneity: If $E_{cell} > 0$, the reaction is spontaneous.

• Preparation: Review for final exam.

• Lab: No lab.

• Homework: Chapter 20.

• Final Exam: May 2.

Summary Table: Weekly Topics and Chapters

Week	Main Topic	Chapters	Lab
1	Molecular Interactions	3, 4, 12, 14	None
2	Mixtures & Concentrations	5, 14	IMFs
3	Kinetics: Rates	15	Concentration
4	Kinetics: Graphs	15	Colligative Properties
5	Equilibrium Intro	15, 16	Kinetics
6	Equilibrium Calculations	16, 17	Kinetics
7	Acids & Bases I	17	Equilibrium
8	Acids & Bases II	17, 18	Acid-Base
9	Buffers & Titrations	18	Acid-Base
10	Solubility	7, 18	Acid-Base
11	Precipitation & Entropy	7, 18, 19	Solubility
12	Thermodynamics	19	Thermodynamics
13	Electrochemistry I	20	Electrochemistry
14	Electrochemistry II & Review	20	None

Additional Info

• This syllabus covers core topics from General Chemistry II, including solutions, kinetics, equilibrium, acids and bases, thermodynamics, and electrochemistry.

• Students are expected to read assigned textbook chapters before class and complete corresponding homework and laboratory exercises.

• Exams are scheduled after major topic blocks to assess understanding and application of concepts.