CHM 2045 - General Chemistry I

College of Natural Sciences

Credit(s): 3
Contact Hours: 47
Effective Term Fall 2025 (655)

Requisites

((Prerequisite CHM 1025 with a minimum grade of C and
Prerequisite CHM 1025L with a minimum grade of C) or
Prerequisite Passing score on Chemistry Placement Exam) and
(Prerequisite MAC 1105 with a minimum grade of C or
Pre- or Co-requisite Any higher level math course with a MAC prefix (excluding liberal arts and statistic courses)) and
Pre- or Co-requisite CHM 2045L with a minimum grade of C

Course Description

This course is designed for students pursuing careers in the sciences or who need a more rigorous presentation of chemical concepts than is offered in an introductory course. Students will engage in problem solving and critical thinking while applying chemical concepts. Topics will include the principles of chemistry including atomic theory, electronic and molecular structure, measurement, stoichiometry, bonding, periodicity, thermochemistry, nomenclature, solutions, and the properties of gases. State Core Course Description (State Rule 6A-14.0303). This course satisfies the Natural Sciences General Education Core.

Learning Outcomes and Objectives

  1. *Students will apply the law of conservation of matter and energy.
  2. *Students will implement rules of significant numbers to all measurements.
  3. *Students will explain the fundamental properties of matter including but not limited to atomic and electronic structure, and periodicity.
    1. The student will classify matter into various groups based upon similarity of chemical and physical properties by:
      1. distinguishing homogeneous and heterogeneous matter; solutions, substances, compounds, and elements.
      2. describing the separation of mixtures by distillation and fractional crystallization into pure substances, and the properties of those substances upon which separation depends.
      3. using the Periodic Table to identify metals, nonmetals, and metalloids; and between "A" group and transition elements.
    2. The student will apply the principles of ideal and real gas systems by:
      1. describing and applying Boyle's law, Charles' law and Avogadro's law.
      2. predicting the effect of a change in conditions upon a variable such as volume.
      3. calculating the density of a gas at a given temperature and pressure.
      4. using the ideal gas law to calculate the molecular mass of a gas, knowing the mass of a given volume or the density at a known pressure and temperature.
      5. relating volumes of gases involved in chemical reactions from information obtained from chemical equations.
      6. using Dalton's law of partial pressures of gases in mixtures.
      7. listing the assumptions of Kinetic-Molecular theory and describing gas behavior in terms of the theory.
      8. describing and applying Graham's law to relate molecular masses, rates of effusion, times of effusion, and molecular velocities of gases.
      9. describing how real gases deviate from the assumptions of the ideal gas law, and indicating the conditions where these deviations are most significant for most gases.
    3. The student will explain the characteristics of the solid and liquid states of matter and phase diagrams by:
      1. determining vapor pressure of liquids at given temperatures and pressures.
      2. predicting and describing the various intermolecular forces present in a molecular substance.
      3. classifying a given substance as ionic, nonpolar molecular, polar molecular, macromolecular, or metallic.
      4. listing the general physical properties associated with each of the five categories of substances listed above.
      5. determining the enthalpy change associated with a given phase change.
      6. interpreting phase diagrams and applying them to predict phase changes associated with changes in temperature and pressure.
    4. The student will apply the principles of thermochemistry by:
      1. using thermochemical equations to relate heat flow in a reaction to moles, and grams of products or reactants.
      2. calculating enthalpy changes for reactions from molar heats of formation.
      3. relating and comparing the enthalpy changes of reactions whose equations differ in direction or in the values of the coefficients of the equations.
      4. using Hess' Law to determine the enthalpy change associated with an equation from enthalpy changes of other equations which can be combined in such a manner to give the first equation.
      5. using bond energies to estimate enthalpy changes for reactions involving substances in the gas phase.
      6. using calorimetric data to determine the heat flow, Q, for a reaction.
      7. using the First Law of Thermodynamics to calculate internal energy change, work, and heat flow, and relate internal energy change and enthalpy change and the experimental conditions under which the two can be measured.
  4. *Students will apply IUPAC rules of nomenclature.
  5. *Students will predict molecular geometry and properties from bonding theories.
    1. The student will explain the nature of covalent and ionic bonding by:
      1. given a Periodic Table, predicting and comparing bond polarity.
      2. drawing Lewis structures for molecules and polyatomic ions.
      3. given or having written the Lewis structure of a molecule or ion, predicting its geometry.
      4. predicting molecular polarity from Lewis structures.
      5. predicting orbital hybridization from Lewis structures and geometry.
      6. predicting the kind and number of sigma and pi bonds in a molecular species.
      7. writing resonance structures for molecules or polyatomic ions.
      8. writing molecular orbital diagrams for simple diatomic species.
  6. *Students will predict and explain the products of chemical reactions (e.g., acid-base, oxidation-reduction, precipitation, dissociation).
    1. Students will perform calculations involving chemical equations and stoichiometry.
*Major Learning Outcome is set by and in compliance with DOE State Rule 6A-14.0303.

Criteria Performance Standard

Upon successful completion of the course the student will, with a minimum of 70% accuracy, demonstrate mastery of each of the above stated objectives through classroom measures developed by individual course instructors.

History of Changes

Revised 8/84 DBT 2/86 Effective Session I, 1986-87 SCN change 11/5/86 Effective Session I, 1987-88 DBT 5/15/90 Effective Session I, 1990-91 Reviewed C&I 2/5/91 3 YR C&I Review 8/94 C&I 3/18/98; DBT 4/20/98 Effective Session I, 98-99 C&I 4/14/98; DBT 5/29/98 Effective Session 19981 C&I 12/1/98; DBT 12/14/98 Effective Session 19991 C&I 11/9/99; DBT 12/15/99 Effective Session 19992 2007 3-year review: C&I 11/13/07, BOT 12/17/07, Eff 20072(0390). C&I Approval: 10/12/2010, BOT Approval: 11/16/2010, Effective Term: Spring 2011 (435). C&I Approval: 11/21/2014, BOT Approval: 02/17/2015, Effective Term: Fall 2015 (505).
C&I Approval: , BOT Approval: , Effective Term: Fall 2025 (655)

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