I. General Information

1. Course Title:
Chemical Principles I

2. Course Prefix & Number:
CHEM 1424

3. Course Credits and Contact Hours:

Credits: 5

Lecture Hours: 4

Lab Hours: 3

Internship Hours: 0

4. Course Description:

This course includes a more rigorous collegiate treatment of topics in physical measurement, dimensional analysis, state of matter, nomenclature, chemical reactions, stoichiometry, gas laws, thermochemistry, atomic structure, and molecular bonding theory. 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:

Name of Institution	Course Number and Title	Credits
St. Cloud State University	CHEM 210 General Chemistry 1	4
Bemidji State University	CHEM 1211 PRINCIPLES OF CHEMISTRY I	4

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):

Name of Program(s)	Program Type
Engineering A.S. Degree	AS
Criminalistics A.S. Degree	AS

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 a team member to successfully complete laboratory experiments.

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

Expected Outcome	MnTC Goal Area
solve chemistry related problems using experimental or simulated data	3
use the scientific method to formulate and test hypothesis and scientific laws	3
relate chemical principles to the real world	3

V. Topical Outline

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

1. Lecture Sessions

1. Basic Concepts of Chemistry
   
   • Hypotheses, Laws, and Theories
   • States of Matter and Kinetic Molecular Theory
   • Matter at the Macroscopic and Particulate Levels
   • Pure Substances
   • Mixtures: Homogeneous and Heterogeneous
   • Elements and Atoms
   • Compounds and Molecules
   • Physical Properties
   • Extensive and Intensive Properties
   • Physical and Chemical Changes
2. The Tools of Quantitative Chemistry
   
   • Units of Measurement
   • Temperature Scales
   • Experimental Error
   • Standard Deviation
   • Exponential of Scientific Notation
   • Significant Figures
   • Problem Solving by Dimensional Analysis
3. Basic Concepts of Chemistry
   
   • Hypotheses, Laws, and Theories
   • States of Matter and Kinetic Molecular Theory
   • Matter at the Macroscopic and Particulate Levels
   • Pure Substances
   • Mixtures: Homogeneous and Heterogeneous
   • Elements and Atoms
   • Compounds and Molecules
   • Physical Properties
   • Extensive and Intensive Properties
   • Physical and Chemical Changes
4. The Tools of Quantitative Chemistry
   
   • Units of Measurement
   • Temperature Scales
   • Experimental Error
   • Standard Deviation
   • Exponential of Scientific Notation
   • Significant Figures
   • Problem Solving by Dimensional Analysis
5. Atoms, Molecules, and Ions
   
   • Atomic Structure
   • Atomic Number
   • Atomic Weight and the Atomic Mass Unit
   • Mass Number
   • Isotope Abundance
   • Determining Atomic Mass and Isotope Abundance
   • Atomic Weight
   • The Periodic Table
   • Molecules, Compounds, and Formulas
   • Ionic Compounds
   • Formulas of Ionic Compounds
   • Names of Ionic Compounds
   • Atoms and Molar Mass
   • Percent Composition
   • Empirical and Molecular Formulas from Percent Composition
   • Determining a Formula from Mass Data
   • Hydrated Compound
6. Chemical Reactions
   
   • Balancing Chemical Equations
   • Chemical Reactions in Aqueous Solution
   • Ions and Molecules in Aqueous Solution
   • Predicting the Outcome of a Precipitation Reaction
   • Net Ionic Equations
   • Acids and Bases: The Arrhenius Definition
   • Acids and Bases: The Bronsted-Lowry Definition
   • Gas-Forming Reactions
   • Oxidation-Reduction Reactions
   • Classifying Reactions in Aqueous Solution
7. Stoichiometry: Quantitative Information about Chemical Reactions
   
   • Mass Relationships in Chemical Reactions: Stoichiometry
   • A Stoichiometry Calculation with a Limiting Reactant
   • Percent Yield
   • Chemical Equations and Chemical Analysis
   • Solution Concentration: Molarity
   • Preparing Solutions of Known Concentration
   • pH, a Concentration Scale for Acids and Bases
   • Solution Stoichiometry
   • Standardizing and Acid or Base
8. Principles of Chemical Reactivity: Energy and Chemical Reactions
   
   • Temperature and Heat
   • Systems and Surroundings
   • Energy Units
   • Specific Heat Capacity
   • Energy Changes of State
   • The First Law of Thermodynamics
   • Enthalpy
   • Enthalpy
   • State Functions
   • Enthalpy Changes for Chemical Reactions
   • Calorimetry
   • Hess’s Law
   • Standard Enthalpies of Formation
   • Enthalpy Change for a Reaction
9. The Structure of Atoms
   
   • Electromagnetic Radiation
   • Planck’s Equation
   • Einstein and the Photoelectric Effect
   • Energy and Chemistry: Using Planck’s Equation
   • The Bohr Model of the Hydrogen Atom
   • Particle-Wave Duality
   • Quantum Numbers and Orbitals
   • Shells and Subshells
   • The Shapes of Atomic Orbitals
   • Electron Spin
10. The Structure of Atoms and Periodic Trends
    
    • The Pauli Exclusion Principle
    • Atomic Subshell Energies and Electron Assignments
    • Effective Nuclear Charge, Z*
    • Electron Configurations of Atoms
    • Electron Configurations of Ions
    • Atomic Properties and Periodic Trends
    • Periodic Trends and Chemical Properties
11. Bonding and Molecular Structure
    
    • Covalent Bonding and Lewis Structures
    • Atom Formal Charges in Covalent Molecules and Ions
    • Resonance
    • Exceptions to the Octet Rule
    • Molecular Shapes
    • Bond Polarity and Electronegativity
    • Bond and Molecular Polarity
    • Bond Properties: Order, Length, Energy
12. Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals
    
    • Orbitals and Theories of Chemical Bonding
    • Valence Bond Theory

2. Laboratory/Studio Sessions

1. Safety and Laboratory Techniques
2. Measurement of Density
3. Hydrate Analysis
4. Determination of a Formula
5. Chemical Nomenclature
6. Copper Cycle
7. Vitamin C Analysis
8. Standarization of HCl and NaOH
9. Gravimetric Analysis
10. Antacid Analysis
11. Enthalpy of Neutralization
12. Energy in Foods