2022-2023 Catalog 
    Sep 27, 2022  
2022-2023 Catalog
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CHEM 220 - College Chemistry I

5 Credit: (4 lecture, 2 lab, 0 clinical) 6 Contact Hours: [Reading Level 3  and Writing Level 3  and Math Level 4 ]

Fundamental principles, laws and theories of general chemistry, including nomenclature, chemical reactions and solution stoichiometry, gas laws, thermochemistry, atomic structure, periodicity and chemical bonding are covered. Concurrent laboratory/workshop sessions include exercises illustrating the principles discussed in lecture. Students who anticipate enrolling in additional chemistry courses are encouraged to take this course as it is basic to all advanced chemistry courses and many professional degrees.
OFFERED: fall semesters

Course Goals/ Objectives/ Competencies:
Goal 1:  Identify units of measurement used in science.


  1. Use significant figures when measuring and performing calculations.
  2. Apply the metric system prefixes.
  3. Properly measure length, area, and volume in correct units.
  4. Perform various conversions (dimensional analysis) using given conversion factors.
  5. Differentiate between qualitative and quantitative measurements.
  6. Differentiate between intensive and extensive physical properties.
  7. Problem solving by unit cancellation method.

Goal 2:  Classify matter based on physical and chemical attributes.


  1. Compare and contrast homogeneous versus heterogeneous materials.
  2. Describe the differences between mixtures, solutions, and pure substances.
  3. Describe various methods of physical separation, including distillation, filtration, extraction, and chromatography.
  4. Understand and apply the concept of specific heat to various problems.
  5. Contrast physical and chemical changes in matter.

Goal 3:  Describe the fundamental particles of an atom in terms of charge, mass and other properties.


  1. Differentiate between atomic mass and mass number.
  2. Describe the differences between isotopes of various atoms.
  3. Know the relative mass and charge of alpha, beta, and gamma radiation and summarize the concept of half-life of a radioactive isotope.
  4. Explain how Rutherford was able to deduce the nuclear model of the atom.
  5. Recite the name and symbol for approximately 50 common elements.
  6. Determine the common charge associated with the main group ions.
  7. Differentiate between mono and polyatomic ions.
  8. Summarize the reasons for the placement of elements in the periodic table.

Goal 4:  Explain the system of nomenclature for ionic and binary covalent compounds.


  1. Name and write formulas for binary and polyatomic ionic compounds containing main group cations.
  2. Name and write formulas for binary and polyatomic ionic compounds containing transition and multiple charged cations using both the roman numeral system and the “traditional” system.
  3. Name and write formulas for various acids.

Goal 5:  Summarize the basic reactions for aqueous ionic substances and properly use the solubility rules.


  1. Write a complete balanced chemical equation from a word equation.
  2. Recognize and predict the products for double replacement, single replacement, and combustion of hydrocarbon reactions.
  3. Use the solubility rules to determine the physical states of the products of single and double replacement reactions.
  4. Recognize synthesis and decomposition reactions.
  5. Recognize oxidation-reduction reactions and determine the: substance oxidized, substance reduced, oxidizing agent, reducing agent.

Goal 6:  Apply the mole concept to a variety of problems.


  1. Determine the molar mass of various substances.
  2. Perform various mole calculations (mass ↔mol, mass ↔ number of particles, mol ↔ number of particles).
  3. Perform percent composition problems.
  4. Determine empirical formulas from laboratory data.
  5. Determine molecular formulas from laboratory data.
  6. Perform combustion analysis type problems.
  7. Calculate and prepare solutions of various concentrations (Molarity).

Goal 7:  Perform stoichiometric problems dealing with various systems (gases, solids, aqueous solutions, liquids).


  1. Perform mole to mole, mole to mass, mass to mol, mass to mass stoichiometry problems.
  2. Perform limiting reactant problems and recognize both the limiting reactant and the excess reagent and determine the amount in excess.
  3. Determine the percent yield for various stoichiometry problems.
  4. Perform various titration problems.

Goal 8:  Apply the concepts of thermodynamics to chemical systems.


  1. Determine heats of reactions using standard heats of formation data.
  2. Determine heats of reaction by using Hess’ Law.
  3. Apply the concept of entropy to physical and chemical processes.

Goal 9:  Use the various gas laws and relate them to the Kinetic Molecular Theory of gases.


  1. List and explain the postulates of the Kinetic Molecular Theory.
  2. Apply Boyle’s Law.
  3. Apply Charles’ Law.
  4. Apply the Combined Gas Law.
  5. Apply the Ideal gas equation.
  6. Apply Dalton’s Law of Partial Pressures.
  7. Apply Graham’s Law of diffusion/effusion.
  8. Solve gas density problems.
  9. Describe possible deviations from ideal gas behavior.

Goal 10:  Describe modern atomic theory and use it to predict periodic trends.


  1. Use the Bohr model of the atom to explain atomic absorption and atomic emission spectroscopy.
  2. Compare and contrast between flame tests and Bright-line spectroscopy.
  3. Recite the electromagnetic spectrum from low to high energy, low to high frequency, and long to short wavelength. Know the colors of the visible spectrum.
  4. Utilize a variety of mathematical equations dealing with energy and quantum theory.
  5. Understand the importance of the DeBroglie wavelength in terms of quantum theory and the generation of Schrodinger’s equations.
  6. Write both entire and noble gas core electron configurations for atoms and ions.
  7. Predict various periodic trends (ionization energy, electronegativity, atom size, ion size) based on electron configuration and periodic table placement.
  8. Use quantum numbers to describe various electrons in an atom.

Goal 11:  Apply the VSEPR Theory to determine molecular geometry.


  1. Write Lewis electron-dot diagrams and Lewis structures for various molecules.
  2. Recognize molecules with expanded octets.
  3. Be able to draw molecules with the following three-dimensional shapes, and know the relative bond angles: linear, trigonal planar, tetrahedral, trigonal pyramid, angular, trigonal bipyramid, octahedral.
  4. Explain the concept of a “polar bond” and a “polar molecule”. Be able to predict molecular polarity.
  5. Know and describe the various van der Waal’s forces of attraction (dipole-dipole, H-bonding, dipole-induced-dipole, London forces).
  6. Draw resonance structures and explain resonance in terms of chemical bonding.

Goal 12:  Predict hybridization and bond order.


1.  Determine the hybridization (sp3, sp2, sp, dsp3, s2sp3) of various atoms in molecules.

2. Draw molecular orbital diagrams for various homonuclear diatomic molecules and determine bond order.

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