The following is a list of skills and understandings that were provided by faculty members at Iowa State University when
asked for guidance as to what students should know when they leave a high school college prep chemistry class.
A--BASIC MATHEMATICS
Solve simple linear equations.
Solve simple quadratic equations
using the quadratic formula and/or factoring.
Solve problems involving the multiplication and division of exponential
numbers.
Given any number, write that number in proper scientific notation.
Add, subtract, multiply,
and divide numbers in scientific notation.
Use a calculator to determine the common and natural logarithms of
a number.
Given a common or natural logarithm, use a calculator to determine the antilogarithm.
B--SIGNIFICANT DIGITS AND UNCERTAINTY
Determine the correct number of significant digits in a given measurement.
Report the results of calculations
to the correct number of significant digits.
Express the precision of a measured quantity in terms of the range
of uncertainty, the relative uncertainty, and the percent uncertainty.
Given experimental values and their uncertainties,
be able to report correct results of calculations and state the uncertainty of the calculated results.
C--BASIC CONCEPTS AND MEASUREMENTS
List
the basic metric units and the common metric prefixes.
Convert metric measurements into equivalent metric and/or
English measurements, and vice versa given.
Calculate the density of a substance from given data.
Distinguish between heat and temperature.
Convert temperature measurements between the Fahrenheit and Celsius
scales.
D--CHEMICAL ELEMENTS, COMPOUNDS AND
MIXTURES
Give a classification of the types of matter.
Define the terms compound and
element.
Define the terms physical and chemical property.
Know the names and symbols of frequently
encountered elements.
Describe the atomic theory of matter.
Define the terms isotope, atomic mass,
formula mass, and mole.
Determine the number of grams per mole of an element given references or a periodic
table.
Convert the mass of an element to moles, or the number of moles of an element to mass.
Describe
the meaning and give the molar interpretation of the formula of a compound.
Determine the mass of a given number
of moles of a compound, or the number of moles in a given mass of a compound.
Determine the number of atoms
in a given mass of an element, or the mass of a given number of atoms of an element.
Given the formula of a
compound, determine the number of molecules and the number of atoms of each kind in a given mass of the compound.
Calculate the percentage by mass composition of a compound from its formula or from experimental data.
Determine
the empirical formula of a compound from experimental data.
List the elements that at room temperature are gases
or liquids, and name the elements that in the free state occur as diatomic molecules.
Balance simple chemical
equations given the formulas of the reactants and products.
E--ATOMIC STRUCTURE
Give a description of Rutherford's concept of a nuclear
atom.
Define the term atomic number.
Define the term isotope as it relates to nuclear composition.
Give a description of the Bohr model of the atom.
Describe an excited atom.
Give
a description of the quantum mechanical model of the atom including energy level structure.
Write the electronic
configuration of an element in orbital notation.
State the periodic law.
Locate, on a periodic
table, families (groups) of elements, periods, the transition elements, the alkali metals, the alkaline earth metals, the
halogens and the noble gases.
Give the number of outer energy level electrons in an atom of a representative
element given the group number.
Write the electron dot symbol for a representative element of any major group.
F--CHEMICAL BONDING
State the octet rule.
Describe an ionic bond.
Predict likely ion charges formed from various
groups.
Predict likely formulas for compounds formed among various groups.
Describe the covalent
bond.
Give a definition of a molecule, and of a covalent (molecular) compound.
Write the electron
dot structures of simple molecules and simple polyatomic ions.
Describe a multiple covalent bond.
Recognize common polyatomic ions.
G--PERIODIC PROPERTIES
OF THE ELEMENTS
Describe how ionization energy of the elements varies within the periodic table.
Describe why the ionization energy of the elements varies within a group.
Describe why the ionization
energy of the elements varies within a period.
Describe how and why the sizes of the atoms vary in the periodic
table.
Describe how the size of an atom compares to the size of the ion of that atom.
Define oxidation
number.
Deduce the oxidation number of an element in a compound or polyatomic ion.
List the expected
oxidation numbers for each group of the periodic table.
Give the formula for a compound predicted on the basis
of expected oxidation numbers.
H--NOMENCLATURE OF CHEMICAL
COMPOUNDS
Name simple compounds (including common acids and typical ternary compounds) given the
formulas, and write the formulas given the names.
I--GASES
AND GAS BEHAVIOR
Describe gases using the kinetic molecular theory.
Describe
how a gas exerts pressure.
Describe barometers and manometers and indicate how they are used.
Define
standard conditions.
Define the molar volume.
State Boyle's and Charles' laws.
Use the gas laws to calculate the new condition of a gas given a change in original conditions.
Calculate
the density of an ideal gas at specific conditions.
Calculate the molar mass of a material from experimental
vapor density data.
J--STOICHIOMETRY
Give the molar interpretation of an equation.
Calculate the number of moles or mass of materials reacting
in a chemical reaction.
Calculate the volume (at standard conditions) of gaseous materials involved in a chemical
reaction.
State Avogadro's hypothesis.
Calculate the percentage yield in a reaction from experimental
data.
K--SOLUTIONS
Define
solution, solute, and solvent.
Define molarity and calculate molarity given appropriate data.
Calculate
the number of moles of a solute in a given volume of a solution.
Calculate the mass of solute in a given volume
of a solution.
Calculate the volume of a solution needed to contain a given mass or number of moles of a solute.
Calculate the molarity of diluted solutions.
Describe a state of dynamic equilibrium.
Give definitions of solubility, saturated solution, unsaturated solution, and a supersaturated solution.
Give
definitions of a strong electrolyte, weak electrolyte, and a nonelectrolyte.
L--CHEMICAL REACTIONS
Describe the five main types of inorganic chemical reaction:
synthesis, decomposition, simple-replacement, ion exchange, and combustion.
Describe precipitation, acid-base,
and oxidation-reduction reactions.
Write a balanced equation for the reaction of a metal oxide or non-metal
oxide with water.
Given a table of the electromotive series of the elements, predict whether a reaction will
occur among potential reactants.
Write a balanced equation for the neutralization of acids and bases.
Give the formulas of ions formed when a typical ionic compound is dissolved in water.
Write balanced
net ionic equations for reactions involving ionic materials.
Predict the production of a precipitate in a reaction
based on solubility rules.
Give the definition of an acid and a base according to the Br0nsted-Lowry theory.
Describe a strong acid and a weak acid.
Define oxidation and reduction.
Define
the terms oxidizing agent and reducing agent.
Write balanced net ionic equations for redox reactions.
Describe the titration process.
Calculate the molarity of a solution using titration data.
