Course Number: Chm 1025C

Course Number: Chm 1025C

CHM 1025C

Introductory Chemistry

CHM 1025C Introductory Chemistry (5) (A.A.) Three hours lecture, three hours lab per week. Prerequisite: MAT 1033 with a grade of “C” or better. This course meets area V requirements for the A.A./A.S. general education requirements. This course is designed primarily to prepare students for entrance into the general chemistry course, CHM 2045C.

STUDENT LEARNING OUTCOMES

At the successful completion of this course, the student should be able to:

  1. Apply the scientific method to experimentation and justify its importance to scientific discoveries.
  2. Differentiate between physical and chemical changes, physical and chemical properties, and intensive and extensive properties.
  3. Implement dimensional analysis method to solve problems such as conversions within the metric system, between the metric and the English system and between mass and volume given density.
  4. Use exponential numbers, scientific notation, significant figures and units in calculations.
  5. Classify matter as heterogeneous or homogeneous, pure substance or mixture, element or compound.
  6. Describe and apply the behavior of solids, liquids and gases using the Kinetic Molecular Theory and intermolecular forces of attraction.
  7. Employ the current system of nomenclature for common elements, monatomic ions (using Stock system for metal ions), common polyatomic ions, ionic compounds, acids and binary molecular compounds.
  8. Compare and contrast the evolution of atomic theory, including evolution of Dalton’s Theory into the modern atomic theory from ancient Greece to modern times.
  9. Explain the atom’s nuclear composition, isotopes, atomic number and mass number.
  10. Calculate atomic mass from isotopic masses and abundance data.
  11. Relate the number of particles to mass and moles using the mole concept.
  12. Use the periodic table to deduce periodic and group trends including electron configuration, valence electrons, ionization energy, atomic size and electronegativity.
  13. Differentiate between ionic and covalent bonding, describing chemical bonding by using Lewis structures.
  14. Apply VSEPR theory to molecular geometry such as linear, planar triangular, bent, triangular pyramid and tetrahedral for simple compounds.
  15. Classify reactions as combination, decomposition, single replacement and double replacement. Write balanced equations from descriptions of these reactions.
  16. Employ solubility information to complete balanced equations for double replacement reactions featuring precipitation, neutralization and formation of unstable products.
  17. Indicate the behavior of an ideal gas, using the gas laws and the kinetic molecular theory.
  18. Determine the volume, temperature, pressure, density, number of moles and molar mass using the gas laws.
  19. Correlate experimental data to empirical and molecular formulas.
  20. Calculate theoretical yield, percent yield and limiting reactant based on the coefficients of a balanced equation (stoichiometry).
  21. Determine percent by mass and molarity of aqueous solutions.
  22. Differentiate between oxidation and reduction processes, writing simple balanced half-reactions and adding them to get net-ionic equations for full redox reactions.
  23. Perform laboratory experiments utilizing core safety guidelines and reporting laboratory data correctly and effectively to illustrate and supplement lecture content.
  24. Demonstrate the relationship between energy and matter and calculate thermodynamic values.
  25. Demonstrate an ability to convey current chemical information in spoken or written form.

Date of Original Submission:Unknown, prior to 1984 (CHM 1010)

Date of Last Revision: 11/8/93, 10/28/04, 10/18/13

Date of Last Review:11/8/93, 10/28/04, 10/18/13