I. General Information

1. Course Title:
Life Science Chemistry

2. Course Prefix & Number:
CHEM 1407

3. Course Credits and Contact Hours:

Credits: 4

Lecture Hours: 3

Lab Hours: 2

4. Course Description:

This course will provide the student with an introduction to general, organic and biological chemistry.  Topics include: scientific measurement, atomic and molecular structure, periodicity, chemical bonding, nomenclature, chemical reactions, nuclear chemistry, solutions, acids, bases, organic functional groups, carbohydrates, lipids, amino acids, proteins and enzymes. The laboratory will reinforce lecture concepts.

5. Placement Tests Required:

Accuplacer (specify test):	Reading College Level CLC or Reading College Level, and Fundamentals of Math Pre-College Level or Math Pre-College Level or Math Introductory College Level or Algebra College Level or Pre-Calculus College Level or Calculus College Level	Score:
Other (specify test):	Next Gen Quant	Score:	265

6. Prerequisite Courses:

There are no prerequisites for this course.

9. Co-requisite Courses:

There are no corequisites for this course.

II. Transfer and Articulation

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

Bemidji State Univesity, CHEM 1110 Chemistry for Allied Health, 3 credits
St. Cloud State University, CHEM 131 Introductory Chemistry for Health Sciences, 4 credits

III. Course Purpose

1. Program-Applicable Courses – This course fulfills a requirement for the following program(s):

Practical Nursing, Diploma
Nursing, Associate of Science 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 oral communication skills	Complete lab reports with detailed information relating to each experiment.
Analyze and follow a sequence of operations	Follow a given lab protocol to successfully complete a lab experiment in the time allowed.
Apply abstract ideas to concrete situations	Apply theories concerning particles which are not visible to construct atomic structure and calculate gram amounts to use in an experiment.

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

• Use conversion factors to convert from one unit or dimension of measurement to another.  MnTC Goal 3
• Draw a Bohr model for any representative element and predict it’s chemical reactivity. MnTC Goal 3
• Compare and contrast ionic and covalent bonds.  MnTC Goal 3
• Construct and name chemical formulas for various combinations of representative metals and nonmetals.  MnTC Goal 3
• Describe the models and list the properties for the three states of matter.  MnTC Goal 3
• Classify changes in matter as either physical or chemical.  MnTC Goal 3
• Balance a chemical equation.  MnTC Goal 3
• Use a periodic table, when given a chemical formula, to convert from grams to moles and vice versa.  MnTC Goal 3
• State the factors that affect rates of chemical reactions and draw potential energy diagrams, indicating activation energies, for exothermic and endothermic reactions.  MnTC Goal 3
• Apply the Bronsted-Lowry theory to identify conjugate acid base pairs.  MnTC Goal 3
• Write the IUPAC name for an alkane or alkene from a given structural formula . MnTC Goal 3
• Identify the chemical structural features of carbohydrates, lipids and proteins.  MnTC Goal 3

 

V. Topical Outline

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

1. Lecture Sessions

1. Basic Concepts
• States of Matter,
• Properties of Matter
• Changes in Matter
• Pure Substances and Mixtures
• Elements and Compounds,
• Names and Symbols
• Chemical Formulas    
2. Measurements in Chemistry:
• Measurement Systems
• Metric System Units
• Scientific Notation
• Conversion Factors
• Dimensional Analysis
• Density
• Temperature Scales
3. Atomic Structure and the Periodic Table
• Internal Structure of an Atom
• Atomic Number and Mass Number
• Isotopes and Atomic Masses
• Periodic Law and Periodic Table
• Metals and Nonmetals, Electron Arrangements
• Classification of the Elements
4. Chemical Bonding
• The Ionic Bond Model: Chemical Bonds
• Valence Electrons and Lewis Structures
• Octet Rule
• Ionic Bond Mode
• Lewis Structures for Ionic Compounds
• Chemical Formulas of Ionic Compounds
• The Structure of Ionic Compounds
• Recognizing and Naming Ionic Compounds
• Polyatomic Ions
• Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions
5. Chemical Bonding
• The Covalent Bond Model: Lewis Structures for Molecular Compounds and Polyatomic Ions
• Naming Binary Molecular Compounds
6. Chemical Calculations:
• Formula Masses
• Chemical Formulas and the Mole Concept
• The Mole and Chemical Calculations
• Writing and Balancing Chemical Equations
7. Solutions:
• Characteristics of Solutions
• Solubility
• Solution Formation
• Solutions Concentrations
• Colloidal Dispersions
8. Chemical Reactions
• Redox Reactions
• Terminology Associated with Redox Processes
• Collision Theory
• Exothermic and Endothermic Reactions
• Factors that Influence Chemical Reaction Rates
• Chemical Equilibrium
• Altering Equilibrium Conditions: Le Chateliers Principle
9. Acids, Bases, and Salts
• Bronsted-Lowry Acid-Base Theory
• Mono-, Di- and Tripotic Acids
• Acid-Base Neutralization Chemical Reactions
• Self-Ionization of Water
• pH Concept
• Buffers
• Electrolytes
10. Nuclear Chemistry
• Stable and Unstable Nuclides
• The Nature of Radioactive Emissions
• Equations and Radioactive Decay
• Chemical Effects of Radiation
• Biochemical Effects of Radiation
11. Saturated Hydrocarbons
• Bonding Characteristics of Carbon
• Alkanes
• Structural Formulas
• Alkane Isomerism,
• IUPAC Nomenclature for Alkanes
• Line-Angle Structural Formulas for Alkanes
• Branched-Chain Alkyl Group
• Cycloalkanes
• IUPAC Nomenclature for Cycloalkanes
12. Unsaturated Hydrocarbons
• IUPAC Nomenclature of Alkenes
• Line-Angle Structural Formulas for Alkenes
• Constitutional Isomerism in Alkenes
• Cis-Trans Isomerism in Alkenes
• Aromatic Hydrocarbons
• Names of Aromatic Hydrocarbons
13. Structural Characteristics
• Alcohols
• Phenols
• Ether
• Aldehydes
• Ketones
• Carboxylic Acids
• Esters
• Amines
• Amides
14. Carbohydrates
• Classification of Carbohydrates
• Chirality
• Using Fischer Projection Formulas
• Classification of Monosaccharides
• Biochemically Important Monosaccarides
• Cyclic Forms of Monosaccharides
• Disaccharides
• Polysaccharides
• Storage Polysaccharides
• Structural Polysaccharides
15. Lipids
• Structure and Classification of Lipids
• Types of Fatty Acids
• Energy-Storage Lipids
• Chemical Reactions of Triacylglyerols
• Membrane Lipids
• Phospholipids
• Cholesterol
• Emulsification Lipids
• Steroids
16. Proteins
• Characteristics of Proteins
• Amino Acids
• Chirality and Amino Acids
• Acid-Base Properties of Amino Acids
• Peptides
• Structural Characteristics of Proteins
• Primary, Secondary, Tertiary and Quaternary Structure of Proteins
• Protein Classifications
• Protein Hydrolysis
• Protein Denaturation
• Glycoproteins
• Lipoproteins
• Enzymes

2. Laboratory/Studio Sessions

1. Safety Rules
• Goggles
• Shoes
• Hair
• Safety shower
• Chemical Spill
• Eye wash station
• First aid kit
• Broken glass
• Report Accidents
• Fume hoods
• Chemical labels
• Chemical properties
• Chemical waste
• Bunsen burners
• Heating test tubes
• Diluting acids
• Food in lab
• Work area
• Medical disability
• Cleanup
2. Laboratory Techniques
• Transferring solids
• Reading scales
• Using the balance
• Measuring volumes
• Graduated cylinder
• Mohr pipet
• Buret
• Volumetric pipet
• Volumetric flask
• Using the gas burner
• Gravity filtration
• Vacuum filtration
3. Density
• Measure density of unknown solid
• Measure density of unknown liquid
• Use % KI and density correlation table
• % KI determination by evaporation
4. Flame Test
• Identification of metallic ions by flame emission
5.  Nomenclature
• Ionic formulas to names
• Ionic names to formulas
• Molecular formulas to name
• Molecular names to formulas
• Physical and chemical property internet search by formula and name
6. Electrolytes and Non-Electrolytes
• Measure conductivity of solutions of ionic compounds
• Measure conductivity of solutions molecular compounds
• Classification of strong, weak and non-electrolytes
7. A Cycle of Copper Reactions
• Conversion of copper to copper (II) nitrate
• Conversion of copper (II) nitrate to copper (II) hydroxide
• Conversion of copper (II) hydroxide to copper (II) oxide
• Conversion of copper (II) oxide to copper (II) sulfate
• Conversion of copper (II) sulfate to copper
8. Exothermic and Endothermic Reactions
• Measure and graph time vs temperature for the reaction of citric acid with sodium bicarbonate
• Measure and graph time vs temperature for the reaction of hydrochloric acid with magnesium
9. Household Acids and Bases
• Using a pH meter, litmus paper and red cabbage juice indicator measure pH values for various household acids and bases
10. Buffers
• Preparation and testing of two buffer solutions using a pH meter and buret.
11.  Molecular Models
• Build and name various organic functional groups using a molecular modeling kit.
12. Computerized Molecular Modeling
• Using a computer program build models of carbohydrates, fats, and proteins and other biochemicals.
13. Energy Content of Food
• Using a simple calorimeter measure the energy content of various foods.
14. Diet Analysis
• Using a computer program analyze a daily record of student food consumption for total calories, grams fat, grams carbohydrates, grams protein, grams trans fat, grams saturated fat, grams polyunsaturated fat, monosaturated fat, milligrams cholesterol, grams fiber, sodium, sugars and percentage calcium
15. Preparation of Aspirin and other Organic Compounds
16. Preparation of Soap