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:

9. Co-requisite Courses:

There are no corequisites for this course.

II. Transfer and Articulation

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

St. Cloud State University, CHEM 211 General Chemistry 2, 4 credits
Bemidji State University, CHEM 1212 Principles of Chemistry II, 4 credits

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):

Criminalistics, AS Degree

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

College-Wide Outcomes/Competencies	Students will be able to:
Demonstrate written communication skills	complete written reports using data collected from the laboratory.
Apply abstract ideas to concrete situations	predict physical properties of matter using atomic and molecular theories.
Work as a team member to achieve shared goals	work together as team members to successfully complete laboratory experiments.

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

• Apply the gas laws to solve problems involving pressure, volume, moles, temperature, formula weight, density and chemical reactions.  MnTC Goal 3
• Identify the intermolecular forces within a pure substance or mixture and predict the vapor pressure, melting point, boiling point and surface tension of liquids.  MnTC Goal 3
• Calculate atomic mass, unit cell dimensions or density for various crystal lattice problems.  MnTC Goal 3
• Interpret phase diagrams to determine the stable phase of a material at a given pressure and temperature.  MnTC Goal 3
• Define terms and solve problems involving molarity, mass percentage, molality and mole fraction.  MnTC Goal 3
• Calculate the boiling point elevation or freezing point depression caused by a solute in a solvent.  MnTC Goal 3
• Describe factors that affect reaction rate.  MnTC Goal 3
• Derive a rate equation from experimental information.  MnTC Goal 3
• Calculate the activation energy from rate constants at different temperatures.  MnTC Goal 3
• Write an equilibrium expression for a given chemical equation.  MnTC Goal 3
• Calculate equilibrium concentrations from an equilibrium constant and initial concentrations.  MnTC Goal 3
• Apply Le Chatelier's principle to determine the shift in direction of a chemical reaction as it refers to adding or removing reactants or products, changing pressure of a gaseous reaction by changing the volume, and changing the temperature of a reaction.  MnTC Goal 3
• Determine the pH and concentrations of all species of a weak acid and common ion solution from initial concentration of the weak acid and common ion and appropriate K_a or K_b values.  MnTC Goal 3
• Calculate an equilibrium constant for a chemical reaction from changes in Gibbs free energy at standard conditions.  MnTC Goal 3
• Name and write structural formulas of alkanes, cycloalkanes and alkenes.  MnTC Goal 3

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