CURRICULUM PROPOSAL
TRANSMITTAL
(To be completed for all
proposals)
PART
I. IDENTIFICATION OF PROPOSAL: ____ New
__X_ Change ____ Delete
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ONLY FOR a course change,
please use an X to identify all applicable categories:
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PART II. IDENTIFICATION OF ORIGINATOR:
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PART III. APPROVAL OF PROGRAM DIRECTOR AND SUBMISSION
TO CORRESPONDING PROGRAM DIRECTORS ON OTHER CAMPUSES, if applicable
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*If disapproved, please
contact originating department and Curriculum Coordinator.
The proposal
originator’s Program Director e-mails the proposal to each of the following
Provosts & then places a check mark by each of their names below:
Proposals have been sent
to the following Provosts electronically by proposal originator’s program
director:
__X__ Nick
Billiris (TC) __X__Esther
Oliver (AC)
__X__ John Cromer
(HC) __X__ James Olliver (SE)
__X__ Steve
Johnson (CL) __X__
Charlie Roberts (SP/G)
Provosts
will email approval or disapproval to the Curriculum Office, but may address
concerns or questions regarding the proposal with the proposal originator or
his/her Program Director.
*If multiple proposals from one academic program
are submitted as a package, the receiving program director and provost may
indicate approval by one transmittal to the Curriculum Office.
ST. PETERSBURG COLLEGE
APPROVED COURSE OUTLINE
CHM 1025 INTRODUCTORY
CHEMISTRY__ _3__
Prefix Number Course
Title Cr.Hrs.
A. Course Description:
Prerequisite: (ENC 0020 and REA 0002
and MAT 0024) or (EAP 1695 and MAT 0024) or (appropriate score on math SPC placement test.)
Corequisite: CHM 1025L. This introductory
course is a presentation of modern chemistry concepts, periodicity
and atomic structure, states of matter, chemical formulas and nomenclature,
chemical reactions, chemical calculations, and solutions. This course iswill prepare
students for General Chemistry and
Qualitative Analysis I but is not
designed for credit toward a major in chemistry and may not be
taken for credit subsequent to receiving a grade of "C" or better in
CHM 1045, CHM 1045L and or CHM 1046, CHM 1046L. or by independent study methods.47
contact hours.
B. Major Learning Outcomes:
1. The student will be able to understand and apply principles
involved in measurement and problem solving.
2. The student will be able to understand be
able to explain the nature and variety of forms of
matter and energy found in the universe.
3. The student will be able to understand be
able to explain the structure of atoms and will apply the periodic law to predict
chemical and physical properties of the elements.
4. The student will be able to comprehend be
able to explain the nature of compounds, their
formation, composition and nomenclature.
5. The student will be able to comprehend be
able to analyze chemical equations and utilize use them
in stoichiometric calculations.
6. The student will be able to understand and apply the principles of
gas behavior in ideal systems.
7.
The
student will be able to understand
be able to describe the
properties of aqueous solution systems and the theories describing the behavior
of acids and bases in aqueous systems.
7.
C. Course
Objectives Stated in Performance Terms:
1. The student will be able to understand and apply principles
involved in measurement and problem solving by:.
The student will be able to:
a. Definedefining: mass, weight, significant figures, heat,
temperature, density, specific gravity.
b. Explainexplaining
the difference between mass and weight.
c. Listlisting
the basic metric units of mass, length, and volume.
d. Listlisting
the equivalents of the metric prefixes in exponential notation.
e. Givegiving
the number of significant figures in any number.
f. Express expressing the results of arithmetic
operations to the proper number of significant figures.
g. Express expressing any number in exponential
notation.
h. Set setting up factors to convert from one
unit to another with dimensional analysis.
i. Convertconverting
measurements within the metric system.
j. Listlisting
the conversion factors between non-metric and metric units for mass, length,
and volume.
k. Convertconverting
between the English and metric systems.
l. Make making temperature
conversions between Fahrenheit, Celsius, and Kelvin.
m. Explainexplaining
the differences between heat and temperature.
n. Calculatecalculating
the density, volume, or mass of a substance from a given set of data.
o. Calculatecalculating
specific gravity from density and vice versa.
2. The student will be able to be able to explainunderstand the nature and variety of
forms of matter and energy found in the universe by:.
The student will be able to:
a. Definedefining:
matter, amorphous, homogeneous, heterogeneous, phase, substance, mixture,
kinetic energy, potential energy, reactant, and product.
b. Listlisting
and distinguishing the three physical states of
matter.
c. Classifyclassifying
properties as physical or chemical.
d. Classifyclassifying
changes as physical or chemical.
e. Statestating
the Llaws of
conservation of matter and energy.
f. Calculatecalculating percent composition of
compounds from masses of elements involved in a chemical reaction.
g. Definedefining:
element, atom, compound, molecule, ion, chemical formula, chemical equation,
mixture, metal, nonmetal, and metalloid.
h. Classifyclassifying
common materials as compounds, elements or mixtures.
i. Writewriting
the symbols for all the most common elements.
j. Namenaming
the most common elements when given their symbols.
k. Statestating
the law of definite composition.
l. Interpretinterpreting
chemical formulas in terms of number of atoms of each element present.
m. Writewriting
formulas for compounds when given the number of atoms of each element in the
compound.
n. Listlisting
the characteristics of metals and nonmetals.
o. Namenaming
binary compounds when given the formulas.
p. Listlisting
the elements that occur as diatomic molecules.
3. The student will be able to be able to explainunderstand the structure of atoms and
will apply the periodic law to predict chemical and physical properties of the
elements by:. The
student will be able to:
a. Definedefining: nucleus, orbital, atomic number, electron
shell, kernmel, noble
gas, isotopes, atomic mass unit, atomic weight, gram-atomic-weight, Avogadro's
number, and mole.
b. Listlisting
the major points of Dalton's Atomic Theory.
c. Listlisting
the electrical charge and relative mass for each of the three primary subatomic
particles.
d. Describedescribing
the atom as conceived by Rutherford following his alpha particle scattering
experiment.
e. Describedescribing
the atom as conceived by Niels Bohr.
f. Calculatecalculating
the maximum number of electrons that can exist in any given energy level.
g. Drawdrawing
an s orbital and a p orbital, and recognize recognizing d orbitals.
h. Givegiving
the sublevel electron structure (1s22s22p6,
etc.) (1s22s22p6, etc.) for any of the first 56 elements, or
identifying the element when given the
sublevel electron configuration.
i. Diagram diagramming the
atomic structure showing the composition of the nucleus and the number of
electrons in each principle energy level for any element.
j. Givegiving
the electron dot structure for any element falling in an A group in the
periodic table.
k. Namenaming
the three isotopes of hydrogen and givegiving the number of protons,
neutrons, and electrons in each.
l. Listlisting
the number of protons, neutrons, and electrons for any element when given the
atomic number and atomic weight.
m. Calculatecalculating
the number of atoms, moles, or grams from appropriate data.
n. Definedefining:
periods of elements, groups or families of elements, and transition elements.
o. Statestating
the periodic law.
p. Indicateindicating
the location on a periodic table of the metals, the nonmetals, the metalloids,
and the noble gasses.
q. Indicateindicating
on the periodic table areas in which s, p, d, and c sublevels of electrons are
being filled.
r. Describedescribing
the change in the atomic radius in moving across a period and in moving down a
family on the periodic table.
s. Describedescribing
the change in outer-energy level electron structures in moving across a period
and in moving down a group on the periodic table.
t. Predict predicting the formulas of simple
binary compounds for Group A elements using the periodic table.
u. Describedescribing
the electronic configuration of transition elements.
4. The student will be able to be able to explaincomprehend the nature of compounds, their
formation, composition and nomenclature by:.
a. definedefining
ionization energy, valence electrons, electro negativity, chemical bond,
electrovalent bond, ionic bond, covalent bond, non-polar covalent bond, polar
covalent bond, bond dissociation energy, coordinate covalent bond, polyatomic
ion, oxidation number, oxidation, reduction.
b. Describedescribing
the variation of the ionization energies of the elements with respect to
position in the periodic table and with respect to removal of successive
electrons.
c. Describedescribing
the formation of ions by electron transfer between two elements and the nature
of the ionic bond formed.
d. Predict predicting the formulas of the nonatomicmonatomic
ions formed from group A elements.
e. Show showing pictorially in the form of a
chemical equation with electron dot structures the formation of an ionic
compound from atoms.
f. Describedescribing
the relative sizes of atoms compared to their ions.
g. Drawdrawing
electron dot structures for common covalent compounds.
h. Explainexplaining why ionic bonding results in crystalline
compounds while covalent bonding results in molecules.
i. Describedescribing
the change in electronegativityelectro
negativity in moving across a period and in moving down a family
on the periodic table.
j. Predict predicting whether a covalent bond
will be polar.
k. Predict predicting whether molecules will be
dipoles.
l. Identify identifying which bonds are coordinate
covalent in the dot structures of a compound.
m. Classifyclassifying
the bonding in a compound as primarily ionic or primarily covalent.
n. Drawdrawing
the dot structures for simple polyatomic ions.
o. Givegiving
the names or formulas of the common ions.
p. Writewriting
formulas of compounds which are simple combinations of common ions.
q. Assign assigning oxidation numbers to each
element in a compound or ion.
r. Givegiving
the name or formula for inorganic binary compounds in which the metal has only
one common oxidation state.
s. Givegiving
the name or formula for inorganic binary compounds containing metals of
variable oxidation state, using either the stock system or classical
nomenclature.
t. Givegiving
the name or formula for inorganic binary compounds containing two nonmetals.
u. Givegiving
the name or formula for binary acids.
v. Givegiving
the name or formula for ternary inorganic acids.
w. Givegiving
the name or formula for ternary salts.
x. Givegiving
the name or formula for salts containing more than one positive ion.
y. Givegiving
the name or formula for inorganic bases.
z. Statestating
how each of the following is used in naming inorganic compounds: -ide, -ous, -ic, hypo-, per-, -ite, -ate, and
Roman numerals.
aa. Givegiving
the formula for familiar substances as identified by the instructor.
bb. Definedefining: formula weight, molecular weight,
gram-formula weight, gram-molecular-weight, empirical formula, and molecular
formula.
cc. Determine determining
the formula weight or molecular weight of a compound when given
the formula.
dd. Calculatecalculating
moles, gram-formula weights, gram-molecular weights, molecules, or grams from
appropriate data.
ee. Calculatecalculating
the percentage composition by weight of a compound when given the formula.
ff. Explainexplaining the relationship between an empirical
formula and a molecular formula.
gg. Calculatecalculating
the empirical formula of a compound from its percentage composition.
hh. Calculatecalculating
the molecular formula of a compound from its percentage composition and
molecular weight.
5. The student will be able to analyzecomprehend
chemical equations and utilizeuse them in stoichiometric
calculations by:.
The student will be able to:
a. Bdefinedefining: chemical equation, word equation, reactant,
product, balanced equation, combination reaction, decomposition reaction,
single replacement reaction, double replacement reaction, exothermic reaction,
endothermic reaction, and heat of reaction.
b. Identify identifying and use using common symbols in writing
chemical equations.
c. Balance balancing chemical
equations.
d. Interpretinterpreting
a balanced equation in terms of molecules, atoms, grams, or moles of each
substance used or produced.
e. Classifyclassifying
reactions as combination, decomposition, single replacement, or double replacement.
f. Complete completing and
balance balancing simple
combination, decomposition, single replacement, and double replacement
reactions.
g. Interpretinterpreting
a chemical equation in terms of exothermic or endothermic heat effect.relate
h. Definedefining: stoichiometry, mole ration, limiting reagent,
excess reagent, theoretical yield, and actual yield.
i. Givegiving
mole ratios involving any two specified substances when given chemical
equations.
j. Calculatecalculating
the number of moles of a substance involved in a chemical reaction from the
mass of another substance used or produced in the reaction.
k. Calculatecalculating
the mass of a substance involved in a chemical reaction from a given mass of
another substance used or produced in the reaction.
l. Calculatecalculating
the mass of a substance involved in a chemical reaction from a given mass of
another substance used or produced in the reaction.
m. Deduce deducing the
limiting and excess reagents when given masses of each and a balanced chemical
equation.
n. Apply applying theoretical yield or actual
yield data in stoichiometric calculations.
6. The student will be able to understand and apply the principles of gas behavior in ideal systems by:. The
student will be able to:
a. Bdefinedefining:
pressure, ideal gas, diffusion, atmospheric pressure, barometer, one
atmosphere, standard conditions, and molar volume.
b. Listlisting
the principle assumptions of kinetic molecular theory.
c. Describedescribing
how a gas exerts pressure.
d. Describedescribing
how a barometer works.
e. Express expressing one atmosphere in terms of
mm or Hg, inches of Hg, torr, and lbs/in2.
f. Statestating
and applying Boyle's law.
g. Statestating
and applying Charles law.
h. Apply applying the combined gas laws to find the volume of a gas when both
the temperature and pressure change.
i. Use using the
molar volume of a gas in conjunction with the combined gas laws to solve for
gram-molecular-mass, mass, or volume of a gas.
j. Calculatecalculating
the density of an ideal gas at Standard Temperature Pressure (STP).
k. Calculatecalculating
the specific gravity of a gas at STP.
l. Statestating
and applying Dalton's law of partial pressures in determining the
pressures of component gases in a mixture of gases.
7. The
student will be
able to describe understand
the properties of aqueous solution systems and the theories
describing the behavior of acids and bases in aqueous systems by:. The
student will be able to:List
a. Describedescribing the water molecule with respect to electron dot structure,
and polarity.
b. Complete completing and
balance balancing equations
for neutralization.
c. Identify identifying hydrates as such, writewriting
balanced equations for their decomposition reactions to water and the
anhydride.
d. Bdefinedefining: solution, solute, solvent, solubility,
miscible, immiscible, concentration of a solution, dilute solution,
concentrated solution, saturated solution, unsaturated solution, supersaturated
solution, mass-percent, molarity, normality.
e. Qualitatively
qualitatively predicting the effect of temperature change
on the solubility of solids and gases in liquids.
f. Calculatecalculating
the mass-percent concentration of a solution.
g. Calculatecalculating
the mass or volume of solute, or mass or volume of solution when given the
mass-percent or volume percent concentration.
h. Calculatecalculating
the molarity of a solution.
i. Calculatecalculating
the moles or the mass of solute, or volume of solution when given the molarity
and other appropriate data.
j. Calculatecalculating
the resulting molarity when a solution of known molarity is diluted with water
or mixed with another solution.
k. Relate relating mass,
moles, solution volume, or gas volume of substances in a chemical reaction when
given the chemical equation.
l. Bdefinedefining:
salt, hydronium ion, amphoteric, electrolyte, nonelectrolyte, dissociation,
ionization, strong electrolyte, weak electrolyte, pH, neutralization, titration,
spectator ions.
m. Givegiving
the Arrhenius definitions of acids and bases.
n. Classifyclassifying
common compounds as electrolytes or nonelectrolytes.
o. Classifyclassifying
common acids, based, and salts as strong or weak electrolytes.
p. Relate relating pH
and hydrogen ion concentration.
q. Solve solving for
the concentration of an unknown solution when given titration data.
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 7/25/83 |
3 YR C&I Review
1993-94 |
Online
effective session 2000 1. |
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Revised 8/84 |
DBT 5/17/94 |
Effective Sess
20011 |
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DBT 2/86 |
Effective Session 19941 |
C&I 11/11/03, BOT 12/16/03, eff20032. |
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Effective Session 19861 |
C&I 3/17/98; DBT 4/20/98 |
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SCN Change 11/5/86 |
Effective Session 19981 |
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Effective Session 19871 |
C&I 12/1/98; DBT 12/14/98 |
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DBT 5/15/90 |
Effective Session 19991 |
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Effective Session 19901 |
C&I 11/9/99; DBT 12/14/99 Effective Session 19992 |
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