APPROVED COURSE OUTLINE
GENERAL CHEMISTRY
CHM 1046 AND
QUALITATIVE ANALYSIS II ___3__
Prefix Number Course
Title Cr.Hrs.
A. Course Description:
Prerequisite:
CHM 1045, and CHM
1045L, and MAC 1105, and
MAC 1106. Corequisite: CHM 1046L. This course is a
continuation of General Chemistry and Qualitative
Analysis II and extends the study of chemical
principles in thermodynamics, kinetics, acid-base reactions,
oxidation-reduction, electrochemistry, nuclear chemistry, and gaseous and
solution equilibra. Forty-seven 47 contact
hours.
B. Major Learning Outcomes:
1. The student will be able to comprehend be
able to describe the nature of gas phase equilibrium
systems.
2. The student will be able to understand andbe
able to apply the
principles of chemical kinetics.
3. The student will be able to understand be
able to explain the nature of aqueous solution
systems and apply the principles of solubility to problems involving these
systems.
4. The student will be able to understand andbe
able to apply
acid-base chemical principles.
5. The student will be able to comprehend be
able to explain the nature of aqueous ionic
equilibrium systems.
6. The student will be able to understand be
able to explain and analyze the
formation and properties of coordination compounds and complex ions.
7. The student will be able to understand be
able to describe and analyze the properties of
electrochemical systems involving oxidation-reduction reactions.
8.
The
student will be able to understand
andbe able to apply
the principles of chemical thermodynamics.
9.
The
student will be able to explain principles of radioactive
decay.
C. Course
Objectives Stated in Performance Terms:
1. The student will be able to be able to describecomprehend the nature of gas phase
equilibrium systems by:.
The student will be able to:
a. writing the corresponding expression for KC Given when given a balanced equation for a reaction
involving gases,. write the corresponding expression for Kc
b. Interpret interpreting
the magnitude of Kc
KC in relation to the extent of forward
and reverse reactions.
c. For using a given equation, calculatecalculate
the numerical value of KcKC , and know the equilibrium
concentrations of all species.
d. For calculating
the numerical value of KC, knowing the original concentrations of all
species and the equilibrium concentration of one species for a given equation, .calculate the numerical value of Kc knowing
the original concentrations of all species and the equilibrium concentration of
one species.
e. predicting the direction in which a chemical system
will move to reach equilibrium when Given given the value of KcKC. predict the direction in which a chemical system
will move to reach equilibrium.
f. predicting the equilibrium concentration of one
species, knowing the concentrations of all other species at equilibrium when Given given the
value of KCKc, .predict the equilibrium concentration of one
species, knowing the concentrations of all other species at equilibrium.
g. predicting the equilibrium concentrations of all
species, given their initial concentrations Given when given the
value of KCKc. predict
the equilibrium concentrations of all species, given their initial
concentrations.
h. predicting the effect of a change in number of
moles, volume, or temperature upon the position of an equilibrium by Using using Le
Chatelier's Principle., predict the effect of a change in number of
moles, volume, or temperature upon the position of an equilibrium.
2. The student will be able to be able to understand and apply the principles of
chemical kinetics by:
The student will be able to:
a. Determinedetermining the order of a reaction,
given the rate as a function of concentration of reactants.
b. Determinedetermining the order of a reaction,
given the concentration of reactant asaas a function of time.
c. writing a rate expression for the reaction, and
calculating the rate constant given the rate at a known concentration Given when given the order of a reaction,. write a rate expression for the reaction, and calculate the rate
constant given the rate at a known concentration.
d. Useusing rate equations to determine
original concentrations and the rate constants.
e. Useusing the rate equations to determine
the time required for the concentration of reactant to drop to a particular
value, given the rate constant and the original concentration. (Also be able to determinedetermining the initial concentration
given the concentration at some particular time).
f. calculating the other quantity Given when given either the half-life
or rate constant for a first order reaction. calculate the other quantity.
g. Describe describing and assessing energy diagrams showing energy of
activation and enthalpy change and describe describing the effect of catalysis.
h. List listing and
describe describing
the three factors which effect rates of reaction according to
collision theory.
i. Useusing the Arrhenius
equation to obtain the rate constant at T2 T2 given its value and T1 T1 and the energy of
activation.
j. Useusing the Arrhenius
equation to obtain the activation energy given rate constants at two different
temperatures.
3. The student will be able to be able to explainunderstand the nature of aqueous solution
systems and apply the principles of solubility to problems involving these
systems by:.
The student will be able to:
a. predicting whether it will be an electrolyte or a nonelectrolyte in aqueous solution when Given given the
formula for a substance,. predict
whether it will be an electrolyte or a nonelectrolyte in aqueous solution.
b. Predict predicting
the relative solubilities of different
solutes in water.
c. Predict predicting
the effect on solubility of a change in temperature or pressure.
d. Writewriting balanced net ionic equations
for the formation of a solution, and for the formation of precipitates.
e. Utilizing using an equation for a precipitation
reaction, relaterelating
the amounts of reactants and products.
4. The student will be able to be able to understand and apply acid-base
chemical principles by:.
The student will be able to:
a. Given giving the following: [H++],
[calculatecalculating
any of the others.
b. Writewriting equations for the dissociation
of strong acids or strong bases.
c. Writewriting equations for the dissociation equilibria of weak acids and weak bases in aqueous
solutions.
d. Predict predicting
whether a given substance will give an acidic, basic, or neutral
aqueous solution, and writewriting
an equation for the solution system.
e. Writewriting equations for the reactions of
acids and bases, and describe describing
the solutions that result as acidic, basic, or neutral.
f. Useusing titration data for an acid-base
reaction to determine: the concentration of an acid or a base in aqueous
solutions, and molecular mass of an acid or a base.
g. Select selecting an
acid-base indicator appropriate for a given acid-base titration.
h. Classify classifying
any given species in a reaction as an acid or base, according to
the Arrhenius, Bronsted and
Lowry, or Lewis models and. Indicate indicating the conjugate acid-base
pairs.
5. The student will be able to be able to explaincomprehend the nature of aqueous ionic
equilibrium systems by:.
The student will be able to:
a. Writewriting an equilibrium constant
expression for KspKSP, for the solution of as
lightly soluble ionic substance; Ka KA for the dissociation of
a weak acid in water solution; and KbKB,
for the reaction of a weak base with water.
b. Utilize using equilibrium constant expressions
to determine equilibrium concentrations and equilibrium constants associated
with ionic equilibria.
c. Predict predicting
the formation of precipitates or solubility using solubility
product, Ksp KSP data.
d. Utilize using KAKa, KBKb, and Kw KW as well as appropriate
equilibrium constant expressions to predict equilibrium concentrations in
acid-base systems.
e. Utilize using acid and base dissociation
constants to determine pH and concentrations in buffer solutions.
f. Calculatecalculating
the equilibrium constant for a reaction, given the equilibrium constant for the
reverse reaction, and/or equilibrium constants for two or more other, related
reactions. State Stating the law of multiple equilibria.
6. The student will be able to be able to explain and analyzeunderstand
the formation and properties of coordination compounds and complex ions by:.
The student will be able to:
a. determining the charge on the central metal atom
when Given given the
formula of a complex ion or coordination compound, .determine the charge on the central metal atom.
b. Illustrate illustrating the geometry of complex
ions given their formula by determining the coordination number, relating it to
the geometry, and sketching the complex.
c. Recognize recognizing geometrical isomers, and
drawing structural formula that
distinguish between them.
d. Writewriting the electron configuration and
orbital diagram for a given transition metal or its ions.
e. drawing an orbital diagram for the electrons around
the central metal atom and showing the hybrid orbitals
used when Given given the composition of a complex and
its geometry,. draw an orbital diagram for the electrons around
the central metal atom and show the hybrid orbitals used.
7. The student will be able to be able to describe and analyzeunderstand the properties of
electrochemical systems involving oxidation-reduction reactions by:.
The student will be able to:
a. Determine determining
the oxidation number of each atom in a molecule or an ion when given the
molecular or ionic formula.
b. Balance balancing redox
reactions using the half-equation method.
c. Label labeling the
oxidizing and the reducing agents and the species being oxidized and reduced in
a balanced oxidation-reduction reaction.
d. Utilize using standard voltages to: decide
whether or not a given redox reaction will occur at
standard concentration and pressure at 298K.
e. For using a
given redox reaction, writewrite the expression for the Nernst equation and useUuse the equation to calculate: the
voltage E of a cell, given E0E0,
and the concentrations of all other species.
f. For using a reaction, writewrite
the expression for the Nernst equation and then use it to calculate the cell voltage,
given the standard voltage and concentrations of all species.
g. calculating the concentration of one of the
reactant species when Given given the balanced equation for a redox reaction and titration date for the reaction,. calculate the concentration of one of the reactant species.
8. The student will be
able to understand
and be able to pply the principles of
chemical thermodynamics by:.
The
student will be able to:
a. calculating the standard entropy change for a
reaction when Given given the standard molar entropies of
reactants and products,. calculate the standard entropy change for a reaction.
b. Given giving the enthalpy change and the standard
entropy change for a reaction, calculatecalculate the standard free energy
change at 298K and at any other temperature.
c. calculating the temperature at which equilibrium
will exist at 1 atmosphere when Given given the enthalpy change and the
standard entropy change for a reaction,. calculate the
temperature at which equilibrium will exist at 1 atm.
d. Qquantitatively
relaterelating
the standard free energy change and the E0 for a given reaction at 298K.
e. Qquantitatively
relaterelating
the standard free energy change and the K for a reaction in an aqueous system.
f. f. Apply applying the
laws of thermochemistry to calculations involving
standard entropy change, standard free energy change, and enthalpy change.
9.
The
student will be able to explain principles of radioactive
decay by:
a.
identifying and describing the
types of nuclear changes in an atom.
b.
quantitatively relating nuclear
changes with atomic mass changes.
c.
predicting nuclear stability from
atomic number and atomic mass.
d.
calculating the amount of a decaying
substance remaining after a specified length
of time.
e.
calculating the mass and energy changes
for nuclear reactions.
f.
describing nuclear fusion and
nuclear fission.
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 3
YR C&I Review 9899
DBT 2/86 C&I
Effective
Session 19861 Effective
19992.
DBT
7/16/87 3
Year Review 2003.
Effective Session 19871
DBT
Effective Session 19901
3 YR C&I REVIEW 1993-94
3 Year Review 9899
3
Year Review 9899