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 gas chemistry, solution chemistry, reaction rate, equilibrium, acid-base theories, solubility and complex in equilibrium, thermodynamics and equilibrium, electrochemistry and nuclear chemistry. MnTC Goal 3

5. Placement Tests Required:

Accuplacer (specify test):

Algebra College Level or Pre-Calculus College Level or Calculus College Level

Score:

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:

III. Course Purpose

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:

• Explain the major points of the kinetic molecular theory of gases and 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, viscosity and surface tension of liquids (MnTC Goal 3);
• Describe the molecular interactions that differentiate solids, liquids, and gases (MnTC Goal 3);
• Interpret phase diagrams and calculate the energies of phase change (MnTC Goal 3);
• Describe the energetics of solution formation (MnTC Goal 3);
• Define terms and solve problems involving molarity, mass percentage, molality and mole fraction (MnTC Goal 3);
• Calculate the vapor pressure lowering, freezing point depression, boiling point elevation or osmotic pressure caused by a solute in a solvent (MnTC Goal 3);
• Determine the order of a reaction from the rate law (MnTC Goal 3);
• Apply the integrated rate law and half-life equations for zero-order, first-order, and second-order reactions (MnTC Goal 3);
• Describe how temperature, activation energy, and molecular orientation influence reaction rates, including the Arrhenius equation and how a catalyst influences the rate of a reaction (MnTC Goal 3);
• Determine the rate law from a reaction mechanism (MnTC Goal 3);
• Write equilibrium constant expressions for chemical equations and find equilibrium concentrations from initial concentrations and the equilibrium constant (MnTC Goal 3);
• Determine the effect of concentration change, volume change, temperature change, and addition of a catalyst on equilibrium using Le Chatelier's Principle (MnTC Goal 3);
• Define and identify acids and bases using the Arrhenius, Brønsted-Lowry, and Lewis definitions; relate strengths of acids and bases to their conjugate pairs (MnTC Goal 3);
• Analyze equilibria of acids and bases using acid and base dissociation constants (MnTC Goal 3);
• Calculate pH of acids, bases, and buffers solutions and construct acid/base titration curves (MnTC Goal 3);
• Calculate K_sp using solubility data and use K_sp to determine solubility of pure compounds and in the presence of a common ion (MnTC Goal 3);
• Describe the factors that affect solubility, including the common ion effect, pH, and complex ion formation (MnTC Goal 3);
• Determine oxidation numbers and balance aqueous redox reactions in acidic and basic solutions (MnTC Goal 3);
• Calculate standard potentials for electrochemical cells and relate to standard free energy, potentials under nonstandard conditions, and the equilibrium constant (MnTC Goal 3);
• Calculate ?H, ?S, and ?G for phase transitions and chemical reactions, using appropriate standard values from thermodynamic tables. This includes finding the temperature range (and the value of T*), over which a reaction is spontaneous (MnTC Goal 3);
• Apply the relationships between thermodynamic quantities such as enthalpy, entropy, and Gibbs energy, and the direction of change in natural processes (MnTC Goal 3);
• Predict, on the basis of qualitative reasoning, the sign of ?S for reactions and phase transitions (MnTC Goal 3);
• Relate thermodynamic data (?H, ?S, and ?G) to the value of the equilibrium constant for a reaction (and vice versa) (MnTC Goal 3);
• Write balanced nuclear equations and identify types of nuclear reactions including radioactive decay, fission and fusion (MnTC Goal 3);
• Analyze first-order decay of radionuclides and use mass defect to calculate energy changes in nuclear reactions (MnTC Goal 3);
• Analyze first-order decay of radionuclides (MnTC Goal 3);
• Use mass defect to calculate energy changes in nuclear reactions (MnTC Goal 3);
• Conduct laboratory work in compliance with guidelines for personal lab safety and responsible management of chemical waste; this includes appropriate use of personal protective equipment and interpretation of Globally Harmonized System for Hazard Communication (GHS) labels (MnTC Goal 3);
• Measure quantities such as mass, volume, temperature, and absorbance with proper technique, and record the results of measurements with the appropriate number of significant figures and units (MnTC Goal 3);
• Record observations of chemical processes (such as precipitate formation, gas evolution, etc.) and write chemical reactions consistent with their observations (MnTC Goal 3);
• Use proper techniques for laboratory procedures, such as titration, filtration, solution preparation, spectrophotometric measurements, etc. (MnTC Goal 3);
• Properly use glassware and equipment including beakers, Erlenmeyer flasks, volumetric pipets, burets, volumetric flasks, watch glasses, graduated cylinders, filtration apparatus, single-beam spectrophotometer, pH meter, balances (MnTC Goal 3);
• Effectively communicate lab procedures, observations, and results in the form of laboratory notebook, written reports, and verbal presentation (MnTC Goal 3);
• Interpret and analyze qualitative observations and quantitative results, incorporating graphs and tables as appropriate (MnTC Goal 3).

V. Topical Outline

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

1. Lecture Sessions

1. 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
2. Intermolecular Forces and Liquids
   
   • States of Matter and Intermolecular Forces
   • Hydrogen Bonding
   • Dipole/Induced Dipole Forces
   • London Dispersion Forces
   • Properties of Liquids
3. 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
4. Solutions and Their Behavior
   
   • Units of Concentration
   • The Solution Process
   • Factors Affecting Solubility: Pressure and Temperature
   • Colligative Properties
5. 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
6. Principles of Reactivity: Chemical Equilibria
   
   • The Equilibrium Constant and Reaction Quotient
   • Determining an Equilibrium Constant
   • Using Equilibrium Constants in Calculations
   • Disturbing a Chemical Equilibrium
7. 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
8. 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
9. 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
10. Principles of Reactivity: Electron Transfer Reactions
    • Oxidation-Reduction Reactions
    • Simple Voltaic Cells
    • Standard Electrochemical Potentials
    • Electrochemical Cells under Nonstandard Conditions
    • Electrochemistry and Thermodynamics
11. Nuclear Chemistry
    • Natural Radioactivity
    • Nuclear Reactions and Radioactivity Decay
    • Stability of Atomic Nuclei
    • Rates of Nuclear Decay
    • Artificial Nuclear Reactions
    • Nuclear Fission
    • Nuclear Fusion

 

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