1. No category

Atomic structure
ls on a periodic table.
-metals, and noble gases are found on a periodic table. Specify how to
predict the charge expected for the most stable ion of an atom.
the line spectra of atomic species relate to the idea of quantized states of electrons in atoms.
A Jablonksi diagram may be helpful in this discussion (so might understanding the 'wave' versus 'particle'
picture of electromagnetic radiation).
explain atomic orbitals and electron shells. How are quantum numbers associated with the
number, energies, and shapes of atomic orbitals? What is nuclear spin?
ion and
momentum of an electron in an atom?
representation of electron configurations in atoms with many electrons.
the periodic table, e.g., atomic radii of neutral atoms (and ionic
atomic species), ionization energy, electron affinity.
Intermolecular interactions, bonding, and molecular structure
ral formula.
ionic compounds.
ral formula) of the major organic groups alkanes, alkenes, alkynes, alcohols, carboxylic acids, ketones, and aldehydes.
f
moles to molecules (and vice-versa).
with the dissolution of molecular compounds in water. Also, be able to establish the relationship between
strong and weak electrolytes and type of chemical compound, i.e., ionic versus molecular compounds.
the formal charge (what is the formal charge?) on each atom.
versus multiple bonds), polar covalent bonds, hydrogen bonds, dative bonds.
de examples of structural resonance.
and bond length.
-dipole, London
dispersion, and hydrogen bonding.
interactions and molecular volumes cause real gases to deviate from this law.
Chemistry 1
Chemical reactions
olution.
-base, and
oxidation-reduction reactions.
-Lowry, and Lewis
definitions).
-ionization of water and the relationship between [OH-] and [H+].
] or [H+] and (b) a strong acid or base solution
given concentration.
a or Kb in terms of the entities (i.e. chemical species) for a stoichiometric
equation for any weak monoprotic acid or base.
to calculate Ka when given Kb (or vice versa).
– strong base titrations and for titrations when either
the base or acid is weak.
reaction coordinate or pathway diagram for
an endothermic and exothermic reaction.
Equilibrium
tion.
ant and initial reactant
and product concentrations, e.g., solubility calculations.
ss the difference between the Gibbs energy and the standard Gibbs energy.
Gibbs energy.
Thermodynamics and energy
does one predict the sign of the change in entropy for physical and chemical processes?
G) and the standard Gibbs free energy (G°), and the
relationship of these entities to the temperature, entropy, and enthalpy.
ΔG) for a reaction.
e able to relate the change in the standard Gibbs energy (ΔG°) to the equilibrium constant.
Chemistry 2
Kinetics
e rate of a reaction given concentration and time data.
based on stoichiometric coefficients.
lationship between the rate law and the
reaction order and rate constant.
erstand how a catalyst works with respect to activation energy.
to draw (and label all important parameters on) a reaction coordinate or pathway diagram for an
endothermic and exothermic reaction.
Instrumental (spectroscopic) techniques
ned? How is this method typically used, e.g., quantitatively or
qualitatively?
components, e.g., sources,
detectors, analytical signal?
an image, a table.
Chemistry 3