Course Overview

Introduction

CHM 2046, Chemistry Fundamentals II, is a college-level course designed to build upon foundational chemistry concepts. The course covers advanced topics such as intermolecular forces, solutions, chemical kinetics, equilibrium, thermodynamics, electrochemistry, and nuclear chemistry. It is essential for students pursuing further studies in chemistry or related scientific fields.

Student Learning Outcomes

Key Objectives

• Understanding Core Concepts: Students will explain how chemical concepts are fundamental to advanced coursework and careers in science.

• Application of Chemistry: Use chemistry knowledge to formulate and execute plans for solving quantitative and qualitative problems.

• Collaborative Learning: Work in teams to develop conceptual understanding and solve problems related to course topics.

• Self-Assessment: Reflect on learning approaches and their impact on performance.

• Predicting Material Behavior: Make predictions about materials based on molecular structure.

• Mathematical Relationships: Use mathematical relationships to predict chemical behavior.

• Data Analysis: Analyze tabulated and graphed data to determine chemical properties.

• Real-World Applications: Explain real-world experiences using chemical concepts.

Main Topics and Subtopics

1. Liquids, Solids, and Intermolecular Forces

This topic explores the properties of liquids and solids, focusing on the forces that hold molecules together.

• Intermolecular Forces: Types include London dispersion forces, dipole-dipole interactions, hydrogen bonding, and ion-dipole forces.

• Properties of Solids: Classification into crystalline and amorphous solids; unit cells and lattice structures.

• Phase Changes: Melting, freezing, vaporization, condensation, sublimation, and deposition.

• Example: Water's high boiling point is due to strong hydrogen bonding between molecules.

2. Solutions and Their Properties

Solutions are homogeneous mixtures of two or more substances. This section covers how solutions form and their properties.

• Solubility: The ability of a solute to dissolve in a solvent, influenced by temperature and pressure.

• Concentration Units: Molarity (), molality, percent composition.

• Colligative Properties: Properties that depend on the number of solute particles, such as boiling point elevation and freezing point depression.

• Example: Adding salt to water lowers its freezing point, a principle used in de-icing roads.

3. Chemical Kinetics

Chemical kinetics studies the rates of chemical reactions and the factors affecting them.

• Reaction Rate: The change in concentration of a reactant or product per unit time.

• Rate Law: An equation that relates the reaction rate to the concentrations of reactants.

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

• Catalysts: Substances that increase reaction rate without being consumed.

• Example: Enzymes act as biological catalysts in metabolic reactions.

4. 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 (): Expresses the ratio of product to reactant concentrations at equilibrium.

• Le Châtelier's Principle: If a system at equilibrium is disturbed, it will shift to counteract the disturbance.

• Example: Increasing the concentration of reactants shifts the equilibrium toward products.

5. Acids and Bases

This section covers the properties, definitions, and calculations related to acids and bases.

• Definitions: Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases.

• pH and pOH: Measures of acidity and basicity.

• Acid-Base Equilibria: Calculating the and for weak acids and bases.

• Example: Vinegar contains acetic acid, a weak acid with a known value.

6. Aqueous Ionic Equilibrium

This topic includes buffer solutions, solubility equilibria, and titration curves.

• Buffers: Solutions that resist changes in pH when small amounts of acid or base are added.

• Solubility Product Constant (): The equilibrium constant for the dissolution of a sparingly soluble salt.

• Titration: A technique to determine the concentration of an unknown solution.

• Example: Blood maintains a stable pH due to the bicarbonate buffer system.

7. Free Energy and Thermodynamics

Thermodynamics deals with energy changes in chemical reactions, focusing on spontaneity and equilibrium.

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

• Gibbs Free Energy (): Determines spontaneity of a reaction.

• Entropy (): A measure of disorder or randomness in a system.

• Example: Ice melting at room temperature is a spontaneous process due to increased entropy.

8. Electrochemistry

Electrochemistry studies the relationship between electricity and chemical reactions.

• Redox Reactions: Involve the transfer of electrons between species.

• Electrochemical Cells: Devices that convert chemical energy into electrical energy (galvanic cells) or vice versa (electrolytic cells).

• Standard Electrode Potentials (): Used to calculate cell voltage.

• Example: Batteries operate based on redox reactions in electrochemical cells.

9. Radioactivity and Nuclear Chemistry

This section covers the properties and reactions of atomic nuclei, including radioactive decay and nuclear energy.

• Types of Radiation: Alpha, beta, and gamma radiation.

• Radioactive Decay: The process by which unstable nuclei lose energy.

• Nuclear Fission and Fusion: Processes that release large amounts of energy from atomic nuclei.

• Example: Nuclear power plants use fission to generate electricity.

Grading and Assessment

Assignment Types and Weight Distribution

Grades are based on a combination of homework, quizzes, tests, and a cumulative final exam. The following table summarizes the weight distribution:

Grading Scale

Course Schedule (Topics by Week)

• Weeks 1-5: Liquids, Solids, Intermolecular Forces, Solutions

• Weeks 6-7: Chemical Kinetics

• Weeks 8-9: Chemical Equilibrium

• Weeks 10-11: Acids and Bases

• Weeks 12-13: Aqueous Ionic Equilibrium

• Weeks 14-15: Free Energy, Thermodynamics, Electrochemistry

• Weeks 16: Radioactivity and Nuclear Chemistry

Required and Recommended Materials

• Textbook: "A Molecular Approach: Mastering Chemistry with Pearson eText" by Nivaldo J. Tro (6th Edition)

• Online Homework: Mastering Chemistry platform access is required.

• Calculator: Scientific calculator (no graphing calculators or programming functions allowed).

• Scantrons: 4 Pink Scantrons for in-person tests.

Academic Integrity and Policies

• On-time Assignments: Only on-time assignments are accepted unless excused for valid reasons (e.g., military duty, university-sponsored activities, court/legal obligations, religious observances).

• Emergency Exam Policy: Students with valid emergencies may be excused from exams with documentation.

• Academic Integrity: All work must be original; violations may result in disciplinary action.

Instructor Communication

• Expect a response within 24-48 hours for email or Webcourses messages.

• Use professional, respectful language in all correspondence.

Additional info:

• Some details about specific weekly assignments and deadlines are available in the full course schedule and may be referenced for planning study time.

• Students are encouraged to use the textbook and online resources for additional practice and mastery of concepts.