Miami-Dade Community
College
CHM 1025 – Introductory Chemistry
Prerequisites and Corequistes:
MAT 1033 or acceptable score on the Algebra Placement test.
Course Competencies:
Competency 1: The
student will demonstrate a knowledge of the basic units, calculations,
conversions, and measurements that are at the very foundation of chemistry by:
a. Demonstrating how very large or very small
numbers are expressed in scientific or exponential notation.
b. Converting ordinary numbers into scientific or
exponential notation and vice-versa.
c. Adding, subtracting, multiplying, and dividing
numbers in scientific or exponential notation
d. Applying the concept of significant figures and
rounding off.
e. Categorizing units as either units of length,
mass, volume, or temperature.
f. Applying dimensional analysis to solve unit
conversion problems.
g. Showing an ability to use the metric system of
measurements by solving metric conversion and English-to-metric conversion
problems.
h.
Converting among the
three common temperature scales.
i.
Defining density
j. Performing density calculations.
Competency 2: The
student will demonstrate a knowledge of matter’s classification, properties,
and changes by:
a. Classifying matter as either a pure substance
or mixture.
b. Classifying pure substances as either elements
or compounds.
c. Classifying a mixture as either homogeneous or
heterogeneous.
d.
Distinguishing between
the physical and chemical properties of matter.
e.
Distinguishing between
the physical and chemical changes that matter undergoes.
f.
Characterizing the three
common states of matter.
g.
Applying the Law of
Conservation of Matter.
h.
Applying the Law of
Conservation of Energy.
Competency 3: The
student will demonstrate a knowledge of the basic building blocks of matter by:
a. Identifying the three major subatomic particles
(electrons, protons, and neutrons) of the atom and describing their general
arrangement within the atom.
b. Defining isotope and determining how the
properties and structure of various isotopes of a single element differ.
c. Relating an element’s isotopic abundance and
mass to its average atomic mass.
d. Identifying the number of protons, neutrons,
electrons, mass number, and atomic number that an atom has given its isotopic
symbol.
e. Learning the name and symbols of several common
elements.
f. Describing the formation of ions from their
parent atoms, and learning their names.
g. Showing how atoms or ions combine to form
compounds.
h. Identifying the basic repeating unit of
elements (atom, molecule, or formula unit), ions (ion or formula unit), and
compounds (molecule or formula unit).
Competency 4: The
student will demonstrate an ability to understand several of the intricacies of
the periodic table by:
a.
Distinguishing between periods and groups on the periodic table.
b. Showing
the relationship between position on the periodic table and atomic number.
c.
Using the structure of
the periodic table to classify elements (e.g., metal, non-metal, metalloid,
noble gas, representative element, transition element, inner transition
element, alkali metal, alkaline earth metal, and/or halogen).
d.
Showing the relationship
between elements having similar chemical properties and being in the same
group.
e.
Giving the reason for
elements having similar chemical properties based upon their atomic structures.
f. Using
the periodic table to identify common patterns such as atomic radii and
electronegativity within periods and groups of elements.
g. Describing
the relationship that exists between the number of valence electrons an element
has and its group number.
h. Describing
the relationship between an element’s group number and the ion that it commonly
forms.
i. Identifying
the s, p, d and f blocks in the periodic table.
Competency 5: The
student will demonstrate a knowledge of electronic structure by:
a. Demonstrating the relationship that exists
between wavelength, frequency, and energy of electromagnetic radiation.
b.
Giving the maximum
number of electrons that can be accommodated in the various energy levels, sublevels, and orbitals.
c.
Applying Pauli’s
Exclusion Principle and Hund’s Rule to construct electron orbital
diagrams.
d. Writing electronic configurations for
neutral atoms and ions.
e. Giving the number of valence electrons in an
atom.
f. Relating electronic configurations to the
position of elements in the periodic table.
Competency 6: The
student will demonstrate a knowledge of chemical bonding by:
a.
Predicting the type of
bond that two atoms will form.
b.
Describing how and why
ionic and covalent bonds form.
c.
Describing the
difference between polar and non-polar covalent bonds.
d.
Defining
electronegativity.
e. Predicting bond polarity by calculating the
electronegativity differences of the elements involved in bonding.
f. Pointing out the traits of ionic compounds and
covalent compounds.
g. Writing the Lewis electron dot structure of
elements, ions, ionic compounds, and covalent compounds.
h. Using the Valence Shell Electron-Pair Repulsion
Theory to determine molecular geometry and bond angles of chemical species
containing up to four pair of valence electrons.
Competency 7: The
student will demonstrate a knowledge of composition stoichiometry by:
a.
Pointing out what atoms
are present in a compound and in what ratio.
b.
Giving the definition of
a mole
c. Calculating the molar mass of a substance from
the sum of its atomic masses.
d. Converting between mass, moles, and number of
atoms or molecules in a sample of a substance.
e.
Showing how to find the
mass percent of an element in a given compound.
f.
Using the mass percent
to find the amount of an element in a given size sample of a compound.
g.
Defining empirical
formula
h. Determining the empirical formula of a compound
from elemental masses or mass percentages.
i. Determining the molecular formula of a compound
given its empirical formula and molar mass.
Competency 8: The
student will demonstrate a knowledge of chemical reactions in relation to
reaction stoichiometry by:
a.
Balancing chemical
equations.
b.
Pointing out the
significance of the coefficients in a balanced chemical equation.
c. Solving various stoichiometry problems.
d. Determining which reactant in a chemical
reaction is the limiting reagent.
e. Using the limiting reagent concept in
calculations.
f.. Comparing the amount of substance actually
formed in the reaction (actual yield) with the predicted amount (theoretical
yield) to determine the percent yield of a chemical reaction.
Competency 9: The
student will demonstrate a knowledge of the properties of solutions by:
a. Distinguishing between a solute and solvent in
a solution.
b. Distinguishing between the different types of
solutions: saturated, unsaturated, and supersaturated.
c. Defining the concentration of a solution in
terms mass percent and showing how to calculate it.
d. Defining the concentration of a solution in
terms molarity and showing how to calculate it.
e. Calculating the concentration of a solution
made by dilution of a stock solution.
Competency 10: The
student will demonstrate a knowledge of writing chemical formulas and chemical
nomenclature of inorganic compounds by:
a.
Determining the
oxidation number of atoms in a neutral compound.
b. Determining the oxidation number of atoms
in a polyatomic ion.
c. Naming common polyatomic ions given their
formulas.
d. Writing the formula of common polyatomic
ions given their names.
e.
Distinguishing between
binary compounds and ternary compounds.
f.
Using oxidation numbers
to write formulas of binary and ternary compounds.
g.
Distinguishing between
metals with one oxidation number and metals with variable oxidation numbers.
h.
Naming a binary metal,
non-metal compound given its formula.
i.
Writing the formula of a
binary metal, non-metal compound given its name.
j.
Naming a compound
containing a metal and a polyatomic ion given its formula.
k.
Writing the formula of a
compound containing a metal and a polyatomic ion given its name.
l.
Naming a compound
containing only non-metals given its formula.
m.
Writing the formula of a
compound containing only non-metals given its name.
n.
Naming a binary acid
given its formula
o.
Writing the formula of a
binary acid given its name
p.
Naming an oxo-acid given
its formula
q.
Writing the formula of
an oxo-acid given its name.
Competency 11: The
student will demonstrate a knowledge of some of the various aspects involved in
chemical reactions by:
a. Categorizing chemical reactions (e.g.
combination, decomposition, single replacement, and double replacement).
b. Showing how the solubility rules and
electromotive series are used to predict whether or not a chemical reaction
will occur.
c. Using the rules of solubility as a means of
determining the physical state of substances involved in aqueous chemical
reactions.
d. Writing chemical equations in molecular, ionic, and net ionic form.