Elements of Chemistry

I.     Course Prefix/Number: CHM 105

       Course Name: Elements of Chemistry

       Credits: 4 (3 lecture; 3 lab)

II.    Prerequisite

MAT 070, or MAT 051 (after Summer 2007) or MAT 052, each with a grade of P; or MAT 114 with minimum grade of C; or placement into a higher MAT course; or consent of instructor.

III.   Course (Catalog) Description

Course is one-semester survey of concepts of general, organic and biochemistry. Content includes classification, properties and states of matter; atomic structure and bonding; reactions of some inorganic compounds; a survey of functional groups, structure and properties of organic and biochemical compounds. Intended for students preparing for nursing and certain other health career programs. Credit cannot be received in both CHM 101 and CHM 105.

IV.   Learning Objectives

General Education.

  1. Identify, define, analyze, interpret, and evaluate: ideas, concepts, information, problems, solutions, and consequences. This includes the ability to compute and comprehend quantitative information and to engage in the scientific process.


  1. Explain observations and laws using models, and apply the scientific approach to knowledge.
  2. Classify matter according to its state, composition, and properties.
  3. Differentiate between physical and chemical changes and between physical and chemical properties.
  4. Evaluate the reliability of measured and calculated quantities and report those values using standard SI units, rules of significant figures and rules of scientific notation.
  5. Utilize units (dimensional analysis) as a guide to problem solving.
  6. Predict properties of atoms, elements and compounds using the Periodic Table of Elements and modern atomic theory.
  7. Represent compounds using their names, chemical formulas, and models.
  8. Apply the concepts of mole and stoichiometry.
  9. Represent solutes and reactions in aqueous solutions, and write molecular, complete ionic and net ionic equations.
  10. Quantify solubility and solution concentration.
  11. Correlate the tenets of kinetic molecular theory with ideal gas behavior.
  12. Summarize the nature of energy, and quantify energy changes.
  13. Describe the quantum mechanical model of the atom.
  14. Apply Lewis theory and the VSEPR model.
  15. Correlate the physical properties of substances with intermolecular forces.
  16. Quantify properties of aqueous solutions of acids and bases.
  17. Describe the basic structure of organic molecules and simple organic functional groups.
  18. Relate the chemical structure of carbohydrates, lipids, proteins, and nucleic acids to their function.


  2. Safely demonstrate basic laboratory skills including filtration, titration, observation and testing of properties of various unknowns, as well as use of a Bunsen burner, high-precision balances, and other basic equipment and glassware.
  3. Perform routine laboratory measurements including mass, volume, and temperature, and record them with proper precision and units; distinguish between measured quantities (raw data) and calculated quantities.

V.    Academic Integrity and Student Conduct


• cheating,
• falsification and fabrication (lying or distorting the truth),
• helping others to cheat,
• unauthorized changes on official documents,
• any other behavior that violates academic integrity.



VI.   Sequence of Topics

  1. The Scientific Method and Introduction to Chemistry
    1. Scientific method
    2. Types of outcomes of scientific method
    3. Knowledge changes with time in science
  2. Measurements, Calculations, and Problem Solving in Chemistry
    1. Physical Quantities and Measurement Systems (SI)
    2. SI prefixes
    3. Significant Figures – Writing and in Calculations
    4. Scientific Notation
    5. Problem Solving and Unit Conversion
    6. Ball Park Answers
    7. Density
  3. Classification and Properties of Matter
    1. Matter
    2. Mixture vs. Pure Substance
    3. Compound vs. Element
    4. Homogeneous vs. Heterogeneous Mixture
    5. Element Symbols
    6. Physical and Chemical Separation
    7. States of Matter
    8. Physical and Chemical Properties and Changes
    9. Types of Energy and Energy changes (Endothermic and Exothermic)
    10. Temperature, Heat, Specific Heat Definitions and Problems
    11. Laws of Conservation of Mass and Energy
  4. Atoms and Elements
    1. History of the Concept of Atoms
    2. Dalton’s Atomic Theory
    3. More Current Models of the Atom (Electrons, Protons, Neutrons)
    4. Isotopes
    5. Average Atomic Mass
    6. History of the Periodic Table
    7. Periodic Law
    8. Ions, Octet Rule
    9. Some Group Characteristics
  5. Compounds—Formulas, Naming, and Nanoscopic Units of
    1. Law of definite composition
    2. Law of multiple proportions
    3. Chemical formulas (diatomic elements, compounds)
    4. Nomenclature of binary and ternary ionic compounds
    5. Nomenclature of binary and ternary acids
    6. Nomenclature of binary covalent compounds
    7. Definitions: formula unit, molecule, ions
    8. Formula mass
  6. Amounts of Chemical Species—the Mole
    1. Mole definition
    2. Avogadro’s number
    3. Molar mass of Monatomic Elements
  7. Composition of Compounds—Quantitative Aspects
    1. Mole to Mole Ratios in Formulas
    2. Mass to Mass Ratios
    3. Calculations of the Following: Molar mass, Formula Weight, Mass Percent Composition from Formulas and Experimental Data
    4. Empirical Formulas
    5. Molecular Formulas
  8. Chemical Reactions and Equations
    1. Types Of Equations, Reactants, Products, Balancing Equations
    2. General Types of Chemical Reactions: Combination, Decomposition, Single Replacement, Double Replacement, Combustion
    3. Specific Types of Chemical Reactions: Acid Base, Precipitation, and Redox Reactions
    4. Net Ionic Equations
    5. Activity Series
  9. Stoichiometric Calculations
    1. Mole Ratios from a Balanced Equation
    2. Mass Ratios
    3. Percent Yield
  10. Electrons in Atoms and the Periodic Table
    1. Electromagnetic Spectrum
    2. Ground and Excited States for Electrons
    3. Quantum Mechanical Model of the Atom
    4. Electron Probability, Shells, Subshells, Orbitals
    5. Electron Configuration
    6. Orbital Diagrams
    7. Periodicity and the Periodic Law
    8. Valence Electrons and Periodicity /Periodic Properties
    9. Periodic Trends: Atomic Radii, Ionization Energy
  11. Chemical Bonding
    1. Electron Dot Structure
    2. Octet Rule reminder
    3. Lewis Theory
    4. Ionic Bonds, Formula Units and Solids
    5. Covalent Bonds
    6. Lewis Dot Structures
    7. Molecular Shapes: VSEPR
    8. Electronegativity
    9. Bond Polarity
    10. Molecular Polarity
    11. General Properties of Ionic And Covalent Compounds
  12. Properties of Gases
    1. Phases of Matter
    2. Kinetic Molecular Theory
    3. Measurement of Gases
    4. Qualitative Gas Laws Idea Using The Definition Of Gas Pressure
  13. Intermolecular Forces—Liquids and Solids
    1. Molecular Polarity Review
    2. Intermolecular Forces: Dipole-Dipole, Dispersion, Hydrogen Bonding
    3. Viscosity
    4. Surface Tension
    5. Phase Changes
    6. Enthalpies of Phase Changes
    7. Vapor Pressure, Boiling Point
    8. Solids: Ionic, Molecular, Covalent Network, Metallic
  14. Solutions
    1. Mixture Type (review)
    2. Homogenous (Solution, Colloid), Heterogeneous (Suspension)
    3. Types of Solutions
    4. Solution Process, Interactions and Enthalpy
    5. Solvent and Solute Polarity and Solution Formation
    6. Factors Affecting Solubility and Rate of Solution Formation
    7. Concentration Units Including w/v %, w/w %, v/v %, ppm, ppb, M
    8. Stoichiometry With Molarity
    9. Dilutions
  15. Acids and Bases
    1. Arrhenius Theory, Hydronium Ion
    2. Bronsted-Lowry Theory; Conjugates
    3. Acid-Base Strength
    4. pH
    5. Titration
  16. Introduction to Organic Chemistry
    1. History of organic chemistry
    2. Condensed structural and line formulas
    3. Nomenclature: hydrocarbons, alkanes, alkenes, aromatics
    4. General reactions alkanes, alkenes
    5. Functional group description and structure including alkyl halide, phenyl, alcohol, ether, aldehyde, ketone, carboxylic acid, ester, amine, amide
    6. Isomers
    7. Polymers
  17. Introduction to Biochemistry
    1. Carbohydrates: structure, function, monosaccharides, disaccharides, polysaccharides
    2. Lipids: structure, function, fatty acids, triglycerides, saponification, hydrogenation, phospholipid, glycolipid
    3. Proteins: structure, function, amino acid, peptide bonds, primary, secondary, tertiary structure, hydrogen bonding, enzymes
    4. Nucleic acids: structure, function, DNA, RNA, nucleotide, transcription, translation, DNA replication

Laboratory Activities

The laboratory activities will include a safety overview including the location and demonstration of the use of safety equipment. The weekly laboratory activities will include 12-16 of the activities listed below.

  1. Laboratory Techniques and Measurements
  2. Mass
  3. Volume
  4. Density
  5. Physical and Chemical Properties
  6. Preparation and properties of oxygen
  7. Nomenclature (dry lab)
  8. Chemical Reactions (Single and Double Displacement)
  9. Determination of the percent yield of a reaction
  10. Stoichiometry of a Precipitation Reaction
  11. Building small molecular models of covalent compounds and polyatomic ions
  12. Properties of acids, bases, and salts
  13. Acid-Base Titration (Standardization of a Base Solution)
  14. Calorimetry and Specific Heat
  15. Caloric Content of Food
  16. Building molecular models and determination of organic functional groups
  17. Fat Extraction from Food
  18. Vitamin Solubility
  19. Chemical Basis of Life
  20. Preparation of Soap
  21. Solubility and Properties of Solutions
  22. Determination of the mass percent of oxygen in a compound (potassium chlorate)

VII.  Methods of Instruction

  • Lectures, which may be supplemented with classroom discussion, use of molecular models, use of multimedia, and/or use of computer based materials at the discretion of the instructor.
  • Hands-On Laboratory Activities
  • Individual and/or Group Problem Solving


VIII. Course Practices Required

  • Participation in class and/or small group discussions
  • Problem solving to include basic algebraic manipulations
  • Hands-on laboratory activities
  • Course may be taught as face-to-face, hybrid or online course.


IX.   Instructional Materials


Lecture text:  Introductory Chemistry, 5th edition, 2015 by Nivaldo Tro (ISBN 13:  978-03219-1029-5), or comparable text.

Laboratory manual: Elements of Chemistry: Laboratory Explorations, 2010, Department of Chemistry, Oakton Community College, or comparable manual.

Individual instructors may supplement the course with additional materials.

Beginning with the Spring 2007 semester, students will be required to purchase their own Chemical Safety/Splash Goggles.  These goggles must meet the following criteria:

  • Fit snuggly against the forehead and face, protecting against splashes
  • Be impact resistant; ANSI rating of Z87 or higher
  • Include only indirect venting

Two varieties of such goggles compliant with the above criteria are available for purchase in the bookstore (cost range ~ $6-$12).  Students may also elect to find an alternative source for purchase, so long as the goggles meet the above criteria and are approved by the instructor.


X.    Methods of Evaluating Student Progress

Depending upon the instructor, any combination of the following assessments may be used to evaluate student progress and determine the course grade.

  • Quizzes, tests, and/or examinations which may include essay, short answer, multiple choice, true/false, and/or problem solving questions
  • Laboratory assignments, reports, results and/or practicals
  • Individual and/or group written reports
  • Individual and/or group oral reports
  • Individual and/or group problem solutions

XI.   Other Course Information

  1. Regular attendance at all sessions is expected.
  2. Reading the text and laboratory manual ahead of the class or laboratory session is expected.
  3. Regular attendance at all sessions is expected.  Missed laboratory sessions will not be able to be made-up
  4. Class policies on make-up of exams and acceptance of late work will be determined by the individual instructor.
  5. Students will be required to review and sign off on this review, their understanding and adherence to basic laboratory safety regulations.
  6. Support services include the availability of open computer laboratories, the college library, and the availability of free tutoring through the Learning Center and/or office hours with the instructor.



Resources and support for
  • pregnancy-related and parenting accommodations; and
  • victims of sexual misconduct
can be found at www.oakton.edu/title9/.



