I. General Information

1. Course Title:
Chemical Principles II

2. Course Prefix & Number:
CHEM 1425

3. Course Credits and Contact Hours:

Credits: 5

Lecture Hours: 4

Lab Hours: 3

Internship Hours: 0

4. Course Description:

This course is a continuation of CHEM 1424 and includes topics in solution chemistry, reaction rate, equilibrium, acid-base theories, solubility and complex in equilibrium, thermodynamics and equilibrium, electrochemistry, nuclear chemistry and an introduction to organic chemistry. Four hours of lecture and three hours of lab weekly.

5. Placement Tests Required:

6. Prerequisite Courses:

7. Other Prerequisites

9. Co-requisite Courses:

II. Transfer and Articulation

1. Course Equivalency - similar course from other regional institutions:

2. Transfer - regional institutions with which this course has a written articulation agreement:

3. Prior Learning - the following prior learning methods are acceptable for this course:
CLEP

III. Course Purpose

1. Program-Applicable Courses – This course is required for the following program(s):

2. MN Transfer Curriculum (General Education) Courses - This course fulfills the following goal area(s) of the MN Transfer Curriculum:
Goal 3 – Natural Sciences

IV. Learning Outcomes

1. College-Wide Outcomes

2. Course Specific Outcomes - Students will be able to achieve the following measurable goals upon completion of the course:

V. Topical Outline

Listed below are major areas of content typically covered in this course.

1. Lecture Sessions

1. Carbon
   
   • Hydrocarbons
   • Alcohols, Ethers, and Amines
   • Compounds with a Carbonyl Group
2. Gases and Their Properties
   
   • Gas Laws
   • The Ideal Gas Law
   • Gas Laws and Chemical Reactions
   • Gas Mixtures and Partial Pressures
   • The Kinetic-Molecular Theory of Gases
   • Diffusion and Effusion
   • Nonideal Behavior: Real Gases
3. Intermolecular Forces and Liquids
   
   • States of Matter and Intermolecular Forces
   • Hydrogen Bonding
   • Dipole/Induced Dipole Forces
   • London Dispersion Forces
   • Properties of Liquids
4. The Chemistry of Solids
   
   • Crystal Lattices and Unit Cells
   • Structures and Formulas of Ionic Solids
   • Bonding in Ionic Compounds: Lattice Energy
   • Molecular Solids
   • Network Solids
   • Amorphous Solids
   • Phase Changes Involving Solids
   • Phase Diagrams
5. Solutions and Their Behavior
   
   • Units of Concentration
   • The Solution Process
   • Factors Affecting Solubility: Pressure and Temperature
   • Colligative Properties
6. Chemical Kinetics: The Rates of Chemical Reactions
   
   • Rates of Chemical Reactions
   • Reaction Conditions and Rate
   • Effect of Concentration on Reaction Rate
   • Rate Equations
   • The Order of a Reaction
   • The Rate Constant
   • Determining a Rate Equation
   • First-Order Reactions
   • Second-Order Reactions
   • A Microscopic View of Reaction Rates
   • Activation Energy
   • The Arrhenius Equations
7. Principles of Reactivity: Chemical Equilibria
   
   • The Equilibrium Constant and Reaction Quotient
   • Determining an Equilibrium Constant
   • Using Equilibrium Constants in Calculations
   • Disturbing a Chemical Equilibrium
8. The Chemistry of Acids and Bases
   
   • The Bronsted-Lowry Concept of Acids and Bases Extended
   • Conjugate Acid-Base Pairs
   • Water and the pH Scales
   • The pH Scale
   • Calculating pH
   • Equilibrium Constants for Acids and Bases
   • Predicting the Direction of Acid-Base Reactions
   • Types of Acid-Base Reactions
   • Calculations with Equilibrium Constants
   • Determining K from Initial Concentrations and Measured pH
   • Polyprotic Acids and Bases
   • The Lewis Concept of Acids and Bases
9. Principles of Reactivity: Other Aspects of Aqueous Equilibria
   
   • The Common Ion Effect
   • Controlling pH: Buffer Solutions
   • Acid-Base Titrations
   • Solubility of Salts
   • The Solubility Product Constant, Ksp
   • Relating Solubility and Ksp
   • Precipitation Reactions
   • Ksp and the Reaction Quotient, and Precipitation
10. Principles of Reactivity: Entropy and Free Energy
    
    • Spontaneity and Energy Transfer as Heat
    • Dispersal of Energy: Entropy
    • Entropy Measurement and Values
    • Entropy Changes and Spontaneity
    • Gibbs Free Energy
    • Calculating and Using Free Energy

2. Laboratory/Studio Sessions

1. Find the Relationship
2. Boyle's Law
3. Evaporation
4. Vapor Pressure
5. Crystals
6. Beer’s Law
7. Effect of Temperature on Solubility
8. Decomposition of H2O2
9. Chemical Equilibrium
10. Acid Dissociation Constant
11. Standardizing a Solution
12. Buffers