APPROVED COURSE OUTLINE
GENERAL
CHEMISTRY
CHM 1045 AND
QUALITATIVE ANALYSIS I 3__
Prefix Number Course
Title Cr.Hrs.
A. Course Description:
Prerequisite:
ENC 0020 and REA 0002 or ENS 1481C, (1) CHM 1025, CHM 1025L, and MAT 1033
(or appropriate score on math placement test) or
(2) CHM 1026 and MAT
1033 (or appropriate score on math placement test) or (3) One year of high school chemistry and permission of the program director.either CHM
1026 or CHM 1025 with grade of A (or grade of B with instructor recommendation)
or two years of high school chemistry each with a laboratory and one semester
of college algebra - MAC 1105. Corequisite: CHM 1045L. The sequence CHM 1045-CHM 1046 with CHM 1045L and
CHM 1046L is designed to meet first-year college chemistry requirements for science
majors and
engineering students. This course includes the study of
periodicity, basic quantum theory, bonding, thermochemistry, stoichiometry, gas
laws, properties of the liquid and solid states, and solutions. 47Forty-seven
contact hours.
B. Major Learning Outcomes:
1. The student will understand
be able to apply the
basic mathematical principles involved in chemical calculations, and will have
thorough understanding of the metric system of measurement.
2. The student will understand
the classification ofbe
able to classify matter into various groups based
upon similarity of chemical and physical properties.
3. The student will comprehend
andbe able to interpret
chemical symbols, formulae, names, chemical equations, and calculations that
apply, stressing stoichiometry.
4. The student will understand
be able to apply the
principles of thermochemistry.
5. The student will comprehend and apply the
principles of gas behavior in ideal as well as real gas systems.
6. The student will understand
be able to explain the
electronic arrangement of the atom in terms of quantum theory, and will use the
periodic table to link electronic configuration to the properties of the
elements.
7. The student will understand
be able to explain the
nature of covalent and ionic bonding.
8. The student will understand
be able to explain the
characteristics of the solid and liquid states of matter and phase diagrams.
9. The student will understand
be able to define and apply concentration
terms used in solution chemistry and the colligative properties of solutions.
C. Course
Objectives Stated in Performance Terms:
1. The student will understand
be able to apply the
basic mathematical principles involved in chemical calculations, and will have
thorough understanding of the metric system of measurement by:.
The student will be able to:
a. Express expressing any number in exponential
notation, and useusing
exponential notation in calculations.
b. Apply applying the rules of significant
figures to calculations based upon experimental measurements.
c. Useusing
dimensional analysis to convert within the metric system and between metric and
nonmetric units.
d. Uuseing an algebraic equation to solve for
an unknown quantity, given or having calculated all the other quantities in the
equation.
2. The student will understand
the classification of be
able to classify matter into various groups based
upon similarity of chemical and physical properties by:.
The student will be able to:
a. Ddistinguishing: homogeneous and heterogeneous
matter; solutions, substances, compounds, and elements.
b. Ddescribinge the separation of mixtures by
distillation and fractional crystallization into pure substances, and the properties
of those substances upon which separation depends.
c. Useusing
the Periodic Table to identify metals, nonmetals, and metalloids; and between
"A" group and transition elements.
3. The student will comprehend
andbe able to interpret
chemical symbols, formulae, names, chemical equations, and calculations that
apply, stressing stoichiometry by:.
The student will be able to:
a. Use using mass
composition data for two or more compounds of two elements to illustrate the
Law of Multiple Proportions.
b. Relate relating the
number of protons, neutrons, and electrons in an atom to its nuclear symbol and
charge.
c. Relate relating the
numbers of electrons and protons to the charge on anion.
d. Relate relating the
charges on an ion and cation to the formula for anionic compound.
e. Relate relating the
atomic mass of an element to the abundances and the masses of its isotopes.
f. determining
the formula mass, Given given an ionic or molecular formula, . determine the formula mass.
g. Relate relating the
numbers of particles (atoms, molecules, or ions) and the mass in grams of a
sample of matter.
h. Given giving the
formula of a substance, relate relating the number of moles and the
mass in grams of the sample.
i. Write writing and
interpreting the formulas for some common
substances.
j. calculating
the percentages by mass of the elements, givenGiven the
formula of a compound.,
calculate the
percentages by mass of the elements.
k. Determine determining
the simplest formula of a compound, given the mass percentages of
the elements or the analytical data from which these can be calculated.
l. Determine determining
the molecular formula of a compound, given the simplest formula
and at least an approximate molecular mass.
m. Use using the
Periodic Table to obtain the charges of ions formed by the main-group elements.
n. Write writing the
formula for an ionic compound given either the formulas of the ions or the name
of the compound.
o. giving the
name of a compound when given its formula. Given the
formula for a compound, give its name.
p. Describe describing some
experimental methods of determining percent composition.
q. Write writing and
balance balancing chemical
equations and interpreting
the various symbols used in chemical equations to represent the conditions of
the reaction system.
r. Relate relating the
number of moles of any two substances taking part in a reaction.
s. Relate relating the
masses of any two substances taking part in a reaction.
t. Given given or having calculated two of the
three quantities, concentration, number of moles of solute, volume of solution,
determine determining
the other quantity.
u. Given given the balanced equation for a
reaction involving species in solution, relate relating the volumes or concentrations
of two reactant species.
v. Describe describing reactions
in water solution as involving precipitation, acid-base, and
oxidation-reduction.
w. Given given the number of moles or masses of
all reactants, determine determining
which is the limiting reactant and calculate the theoretical yield
of any product.
x. Calculate calculating
the percent yield, given the actual and theoretical yields.
4. The student will understand
be able to apply the
principles of thermochemistry by:.
The student will be able to:
a. Use using thermochemicalthermochemical
equations to heat flow in a reaction to moles, and grams of products or
reactants.
b. Calculate calculating
enthalpy changes for reactions from molar heats of formation.
c. Relate relating and
compare comparing the
enthalpy changes of reactions whose equations differ in direction or in the
values of the coefficients of the equations.
d. Apply applying Hess's 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.
e. Use using bond
energies to estimate enthalpy changes for reactions involving substances in the
gas phase.
f. Use using calorimetric
data to determine the heat flow, Q, for a reaction.
g. Apply applying 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.
5. The student will comprehend and apply the
principles of gas behavior in ideal as well as real gas systems by:.
The student will be able to:
a. Describe describing and
applying Boyle's law, Charles and
Gay-Lussac's law, and Avogadro's law.
b. Apply applying the ideal gas law to predict
the effect of a change in conditions upon a variable such as volume.
c. Apply applying the ideal gas law to
calculate the density of a gas at a given temperature and pressure.
d. Use 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.
e. Relate relating volumes
of gases involved in chemical reactions from information obtained from chemical
equations.
f. Apply applying Dalton's law of partial
pressures of gases in mixtures.
g. List listing the assumptions of
Kinetic-Molecular theory and describe describing gas behavior in terms of
the theory.
h. Describe describing and
applying Graham's law to relate molecular
masses, rates of effusion, times of effusion, and molecular velocities of
gases.
i. Describe describing how
real gases deviate from the assumptions of the ideal gas law, and indicate indicating
the conditions where these deviations are most significant for
most gases.
6. The student will understand
be able to explain the
electronic arrangement of the atom in terms of quantum theory, and will use the
periodic table to link electronic configuration to the properties of the
elements by:.
The student will be able to:
a. State stating and
describe describing
the postulates of quantum theory and compare quantum and classical
theories.
b. Relate relating the
wavelength and frequency of a spectral line to the energy of photon and to the
change in energy of an atom.
c. Determine determining
the number of electrons that may be accommodated by any given
principal energy level or sublevel.
d. Given given the atomic number of an element,
write writing the
electron configuration of its isolated gaseous atom in the ground state.
e. Given given the electron configuration, state stating and
applying Hund's rule and drawing orbital diagram of the atom.
f. Describe describing the
four quantum numbers, and the rules for assigning them;. aApplying
the rules and assigning them to each of the various
electrons in an atom.
g. State stating and
applying Pauli's Exclusion principle.
h. Relate relating electronic
configurations to the periodic table and to periodic in general.
i. Using using the periodic table, predicting
the relative values of ionization energy, electronegativity, and atomic radius.
7. The student will understand
be able to explain the
nature of covalent and ionic bonding by:.
The student will be able to:
a. Given given a Periodic Table, predicting and compare comparing bond polarity.
b. Draw drawing Lewis structures for molecules
and polyatomic ions.
c. Given given or having written the Lewis
structure of a molecule or ion, predicting
its geometry.
d. Predict predicting molecular polarity from
Lewis structures.
e. Predict predicting orbital hybridization from
Lewis structures and geometry.
f. Predict predicting the kind and number of
sigma and pi bonds in a molecular species.
g. Write writing resonance
structures for molecules or polyatomic ions.
h. Write writing molecular
orbital diagrams for simple diatomic species.
8. The student will understand
be able to explain the
characteristics of the solid and liquid states of matter and phase diagrams by:.
The student will be able to:
a. Determine determining
vapor pressure of liquids at given temperatures and pressures.
b. Predict predicting and describe describing the various intermolecular
forces present in a molecular substance.
c. Classify classifying a given substance as
ionic, nonpolar molecular, polar molecular, macromolecular, or metallic.
d. List listing the general physical
properties associated with each of the five categories of substances listed
above.
e. Write writing equations
for the thermal decomposition of carbonates, hydroxides, and hydrates.
f. Determine determining
the enthalpy change associated with a given phase change.
g. Interpret interpreting phase diagrams and applying them to predict phase changes
associated with changes in temperature and pressure.
9. The student will understand
be able to define and apply concentration
terms used in solution chemistry and the colligative properties of solutions by:.
The student will be able to:
a. Applying applying Raoult's Law, calculate the
vapor pressure of a solution.
b. Applying applying Henry's Law, given data for
one set of conditions, determine the concentration of a gas in solution at a
second set of conditions.
c. Perform performing calculations related to
molarity, molality, normality, molefraction, and mass percent.
d. Perform performing calculations related to
colligative properties: freezing point
depression and boiling point elevation.
D. 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.
Revised 8/84 C&I
11/9/99; DBT 12/15/99
DBT 2/86 Effective
Session 19992
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 I, 99-2000