Course Descriptions & Syllabi

Course Descriptions & Syllabi

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Note: some or all of the courses in the subjects marked as "Transfer" can be used towards a transfer degree: Associate of Science and Arts or Associate of Engineering Science at DACC. Transferability for specific institutions and majors varies. Consult a counselor for this information.

Areas of Study | | CHEM100 syllabus

COURSE TITLE:Introduction to Chemistry (for Non-Science Majors)
IAI CODE(S): P1 902L
DELIVERY MODE:Hybrid, In-Person

A one-semester introductory course in basic concepts and language of chemistry for the non-science major. Fundamentals of inorganic and organic chemistry with applications to everyday life. Face-to-Face class meets for 3 hours of lecture and 2 hours of lab per week. Hybrid course is taught with an online lecture and meets 3 hours per week--2 hours for lab and an hour for questions and testing. Lectures for the Hybrid sections use the same slides as the Face-to-Face course with a lecture recorded over it.

Place into MATH107.

NOTES: A lab is required for this course. Some sections will require a separate lab, while other sections will include the lab.

Students completing this course will exhibit knowledge and competency in describing properties and reactivity of matter through words, calculations and experimental procedures. The student must be able to:
  • Measure physical properties using appropriate measurement tools and units
    • Determine the length, mass, volume, temperature or density of an object given proper tools or data, either in the lab or in story problems
    • Express terms of length, mass, volume, temperature or density in standard metric units
    • Convert between the metric and English system using dimensional analysis
    • Express data or calculated physical data in the correct number of significant figures using rounding and scientific notation based on the limits of the data or the instrument
  • Describe and categorize types of matter using proper vocabulary and nomenclature by
    • Listing the characteristics of solids, liquids and gases
    • Distinguishing between and listing examples of physical properties, chemical properties, physical changes and chemical changes
    • Identifying an element as a metal, nonmetal or metalloid given a Periodic Table
    • Identifying a compound as either ionic or molecular given the compound's name or chemical formula
    • Naming a compound appropriately using either the prefix or stock system of naming given the chemical formula
  • Apply basic concepts and principles of atomic structure and bonding through
    • Descriptions of the various models of the atom
    • Identification of the orbitals in each energy level and the electrons that occupy those orbitals
    • Drawing correct Lewis dot diagrams to aid in the drawing of Lewis structures of chemical compounds
    • Predicting properties and chemical reactivity of elements or compounds based on trends of the Periodic Table
    • Predicting molecular shapes using VSEPR Theory
  • Evaluate chemical reactivity of chemical species by:
    • Writing balanced, chemical equations
    • Distinguishing between different types of chemical reactions based on the reagents and conditions given
    • Calculating molecular weights, percent composition, mole ratios, limiting reagents and yields of chemical reactions through stoichiometry and the use of chemical formulas and balanced chemical reactions
  • Apply knowledge of chemical properties and reactivity in a laboratory setting by:
    • Creating appropriate experimental setups with glassware and equipment
    • Completing experiments in a time-efficient manner
    • Describing experiment success through calculations of percent error and percent yield
    • Summarizing the results and analyzing experimental methods through writing

  • Standards for Measurements (10%)
    • Measurement of length, mass, volume, temperature and density
    • Conversion of measurements between the metric and English system using dimensional analysis
    • Rounding numbers, significant figures and scientific notation
  • Classification and Properties of Matter, Early Atomic Theory, Nomenclature (15%)
    • States of matter, compounds and elements, substances and mixtures
    • Metals, nonmetals, metalloid, their names and symbols
    • Physical and chemical changes
    • The basic structure of the atom and the scientists who made major contributions to the development of the model
    • How protons, neutrons and electrons are arranged in the atom and ions
    • Calculating average atomic mass using the various isotopic weights and relative abundances
    • Nomenclature of inorganic compounds
    • Names of polyatomic ions and the compounds they form
  • Quantitative Composition of Compounds (10%)
    • The mole, molar mass, and percent composition of compounds
    • The empirical formula of compounds
  • Chemical Equations (15%)
    • Writing and balancing double displacement reactions
    • Writing and balancing single displacement reactions
    • Predicting whether the reaction forms products or not
  • Modern Atomic Theory and the Periodic table. The Chemical Bond (15%)
    • The electromagnetic spectrum and the spectrum of hydrogen
    • The Bohr atom, energy levels and sublevels
    • Electronic structure: s, p, d, f as it relates to the periodic table
    • Lewis dot diagrams
    • Ionic and covalent bonding
    • Polarity of molecules
  • Solutions, acids, bases, salts (15%)
    • Solubility as it relates to polar and nonpolar materials
    • Calculations using molarity
    • Definition of acids, bases and the products of neutralization
    • Electrolytes and the percent of dissociation
    • Titration
    • Calculating pH
  • The Gaseous state of matter (10%)
    • The kinetic molecular theory
    • Boyle's Law
    • Charles' Law
  • Introduction to Organic Chemistry (10%)
    • The carbon atom and hydrocarbons
    • Structural formulas and isomers
    • Aliphatic and aromatic compounds
    • Alcohols, ethers, aldehydes, ketones, carboxylic acids esters, and their reactions
    • Nomenclature
All labs are conducted in a wet-lab and are hands-on.
  • Lab 1 - Safety & Procedures
    • Students will review safety information, as well as laboratory policies and procedures
  • Lab - Laboratory Techniques (Optional-not all semesters allow 16 weeks of experiments)
    • The techniques of cutting, bending and fire-polishing glass are practiced
    • Other techniques include filtering, forming precipitates and Bunsen burner operation
  • Lab 2 - Measurements
    • Precision and accuracy are introduced. Measurements of length, volume, mass and temperature are performed
    • Calculations are performed to determine density of known and unknown substances
  • Lab 4 - Freezing Points - Graphing of Data
    • Examine freezing point depression with varying chemicals
  • Lab 5 - Calorimetry
    • Determine the specific heats of common metals through an energy transfer process
  • Lab 6 - Water in Hydrates
    • The concept of percent composition is introduced
    • A hydrated sample is heated and water is driven off
    • The weight of water lost is measured and calculations are performed to determine the percentage of water in the sample
  • Lab 7 - Composition of Potassium Chlorate
    • The theoretical percentage of oxygen in potassium chlorate is calculated and compared to the experimental value
    • Verification of the identity of the product formed is demonstrated using double displacement reactions
  • Lab 8 - Single Displacement Reactions
    • Reactions of metals with their aqueous solutions are performed for the students to create the Activity Series
  • Lab 9 - Double Displacement Reactions
    • Twelve double displacement reactions are performed and correlated with the factors which predict formation of products during chemical reactions
  • Lab 10 - Quantitative Preparation of Potassium Chloride
    • Prepare standard reagent quality potassium chloride from simple starting materials
  • Lab 11 - Electromagnetic Energy and Spectroscopy
    • Examine energy as it relates to waves
  • Lab 12 - Lewis Structures and Molecular Models
    • Examine geometric properties of molecules using model kits
  • Lab 13 - Gases
    • Examine the relationship between pressure and volume for gases
  • Lab 14 - Properties of Solutions
    • The quantitative portion of the lab is the calculation of the mass percent of potassium chloride in a saturated solution
    • The qualitative portion of this lab introduces students to the concept of solvent polarity and the solubility rule: "like dissolves like"
  • Lab 15 - Titration I
    • Learn about the principles of acid/base reactions using the standard procedure of titration
  • Lab 16 - Chemical Equilibrium - Reversible Reactions
    • Examine reactions in equilibrium and learn about the importance of concentration


Foundations of College Chemistry, by Morris Hein and Susan Arena 14th Edition.

Foundations of Chemistry in the Laboratory, by Morris Hein and Susan Arena, 14th Edition—Custom.

  • Supplies: Scientific calculator, splash goggles, appropriate lab clothing.
    • Safety Goggles:
      • Students must purchase their own laboratory safety goggles.
      • Goggles are available in the DACC Bookstore.
      • If you already have your own, they must offer complete protection of the side of your eyes. (Look for the markings "Z87" stamped on the goggles.) Lab safety glasses are not acceptable for students.
    • Calculator:
      • Any simple scientific or graphing calculator is sufficient.
      • A calculator may only be necessary for a very small portion of this class.
    • Enclosed Shoes & Pants:
      • For lab days.
      • If you are not dressed appropriately you will not be allowed to participate.

Grading is based on a weighted percentage of five different categories with overall grade divisions at 90, 80, 70 and 60 percent. The five categories are:
  • four or more midterm tests (best three) accounting for forty percent of the course grade
  • lab reports accounting for twenty percent of the course grade
  • ten quizzes (best eight) accounting for ten percent of the course grade
  • homework assignments accounting for ten percent of the course grade and a final exam accounting for twenty percent of the course grade

Attendance is required and a student may be withdrawn from the class roster due to unexcused absences.

Laboratory work must be performed during the regularly scheduled laboratory period.

"Make-up" laboratory work at an alternate time will not be an option.

No credit will be given for laboratory reports submitted if the student was absent from that laboratory session

If a student has a valid excuse for missing a lecture or laboratory class, credit for the missed period may be arranged with instructor.

It will not be "automatic".

All students must pass the laboratory portion of the class in order to pass the course.

The final exam will include all the material that is covered in the semester. Every student is required to take the final exam at the scheduled time. Each student must take and pass the cumulative final exam in order to pass the course.

A curve may be applied at the instructor's discretion.


Membership in the DACC community brings both rights and responsibility. As a student at DACC, you are expected to exhibit conduct compatible with the educational mission of the College. Academic dishonesty, including but not limited to, cheating and plagiarism, is not tolerated. A DACC student is also required to abide by the acceptable use policies of copyright and peer-to-peer file sharing. It is the student’s responsibility to become familiar with and adhere to the Student Code of Conduct as contained in the DACC Student Handbook. The Student Handbook is available in the Information Office in Vermilion Hall and online at:

Any student who feels s/he may need an accommodation based on the impact of a disability should contact the Testing & Academic Services Center at 217-443-8708 (TTY 217-443-8701) or stop by Cannon Hall Room 103. Please speak with your instructor privately to discuss your specific accommodation needs in this course.

Spring 2019

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