General Chemistry II Student Competencies
Chemistry: The Central Science, Brown, Lemay, and Bursten, 2000.
Chapter 14 Student competencies
Upon completion of this chapter, students
should be able to:
-
Use kinetic-molecular theory to explain how reactions occur. Be
able to explain the underlying reason for why concentration and temperature
changes affect reaction rates.
-
Understand the main factors that control the rate of a reaction.
-
Understand exactly what “reaction rate” means and be able to calculate
the rate of a reaction when given data showing concentrations at various
times.
-
Be able to use reaction stoichiometry to write the rate of a reaction in
terms of how each product or reactant concentration changes with time
-
Given a set of data showing reaction rates for various combinations of
concentrations, calculate the rate law and the rate constant.
-
Be able the write the rate law expression. Understand
the units associated with rate, what reaction order is, and how the units
of the rate constant k vary with reaction order.
-
Understand and be able to use the Arrhenius expression:
-
Be able to show how the Arrhenius equation accounts for collision frequency
and orientation factors
-
Know how to determine the fraction of molecules with sufficient energy
to react at a given temperature for a given activation energy.
-
Demonstrate an understanding of how to graphically determine the activation
energy for a given reaction.
-
Given rate constants at multiple temperatures, know how to calculate the
activation energy for the reaction. From
the activation energy and rate constant at one temperature, be able to
predict the rate constant at any other temperature.
-
Understand first order reactions:
-
Be able to write the rate law for such a reaction
-
Know and be able to use the expression for how concentration changes with
time in a first order reaction
-
Know and be able to use the expression that relates the half-life with
the rate constant for a first order reaction.
-
Explain graphically what parameters to plot to show if a reaction is a
first order process.
-
Understand second order reactions:
-
Be able to write the rate law for such a reaction
-
Know and be able to use the expression for how concentration changes with
time in a second order reaction
-
Know and be able to use the expression that relates the half-life with
the rate constant for a second order reaction.
-
Explain graphically what parameters to plot to show if a reaction is a
second order process.
-
Understand how reaction rate varies with temperature and the two underlying
reasons for this. Use a kinetic molecular distribution diagram and
an energy reaction coordinate diagram to explain this.
-
Understand and be able to depict the change in enthalpy, the activated
complex, and the activation energies for a forward and reverse reaction
on an energy reaction coordinate diagram.
-
Explain what is meant by a reaction mechanism; be able to write the rate
laws for elementary steps and to clearly outline the significance of the
rate-determining step. Understand
the terminology associated with reaction mechanisms.
-
Given that a specific step in the reaction mechanism is identified as the
slowest step, predict the rate law associated with this mechanism.
-
Use an energy diagram to explain how a catalyst affects reaction rates.
-
Explain how heterogeneous and homogeneous catalysts work.
-
Understand the role of enzymes in living systems to include:
-
The lock-and-key model of enzyme action and an understanding of the active
site.
-
The specific types of interactions that occur between substrates and enzymes
-
The importance of enzyme inhibition and turnover number and how these are
related to toxic effects and activation energies respectively.
-
Identify the three major pollutants from automobiles and outline the reactions
that each undergo in catalytic converters.
Chapter15 Student competencies
Upon completion of this chapter, students
should be able to:
-
Relate forward and reverse reaction rates to equilibria and to equilibrium
constants.
-
Know what is meant by the Law of Mass Action. For both homogeneous and
heterogeneous reactions, be able to write the expression for the equilibrium
constants Kc and Kp. Relate the value of the equilibrium
constant to the position of equilibrium.
-
Given concentrations or pressures, determine the value of the equilibrium
constant. Be able to relate Kc and Kp.
-
Understand the factors that change the equilibrium constant.
-
Know what is meant by the reaction quotient Q. Given a set of concentrations
and the equilibrium constant, determine whether a particular reaction is
at equilibrium. If it is not, predict which way it would spontaneously
shift to reach equilibrium.
-
Given a set of initial concentrations and the equilibrium constant, calculate
the equilibrium concentrations.
-
Understand Le Chatelier's principle and be able to explicitly state it.
Understand how equilibria respond to pressure, temperature, and concentration
changes. Be able to explain why in terms of the relative effects
on the forward and reverse reaction rates.
-
Understand how a catalyst affects equilibria.
Chapter 16 Student competencies
Upon completion of this chapter, students
should be able to:
-
Be able to define and identify Arrhenius, Bronsted-Lowry, and Lewis acids
and bases.
-
Given the pH, pOH, [OH-], or [H3O+}; be
able to quickly calculate the other three to the correct number of significant
figures.
-
Understand what is meant by conjugate acid-base pairs and how the strength
of one is related to the weakness of the other.
-
Understand the Kw equilibrium and explain what the pH scale
represents.
-
Be able to identify the strong acids and bases and to calculate the pH,
or pOH for a given concentration.
-
Relate the Ka of an acid to the Kb of its conjugate
base.
-
From the Ka and an initial concentration, be able to determine
the pH of a weak acid solution. From the Kb and an initial concentration,
be able to determine the pOH of a weak base solution.
-
Be able to identify weak acids and weak bases and to write the reaction
of each with water.
-
Show the reactions that occur for polyprotic acids.
-
Be able to identify a species that can act as an acid or as a base; be
able to determine whether a solution of this species would be acidic basic,
or neutral.
-
Understand the acid-base properties of a salt solution. Given a salt,
be able to write the hydrolysis reactions of each of its ions (cation and
anion) with water. Use these to predict whether the reaction would
be acidic, basic, or neutral.
-
Understand the three main factors (bond polarity, bond strength, and stability
of conjugate base anion) that affect acid strength; use these to rank order
a series of structures in terms of their acidity or basicity.
-
Understand the relative acidity of oxyacids with differing number of oxygen
atoms.
-
Be familiar with the structure of carboxylic acids and understand why they
are acidic.
-
Understand and be able to diagram how metal ions not in Groups I or II
react with water. Relate acidity of metal ions to charge and size. Discuss
acidity of these metal ions in terms of Lewis acids and bases.
-
Be able to determine the percent ionization for a weak acid or base solution.
Chapter 17 Student competencies
-
Know what is meant by a buffer and understand
the pH range over which buffers are typically considered to be effective.
-
Know the Henderson-Hasselbalch equation; demonstrate an understanding of
how to use it to prepare buffers and to calculate the pH of a given solution
of an acid/conjugate base pair. Relate
the pH of a buffer system to the relative concentrations of the acid/conjugate
base pair.
-
For a given buffer system, write the reactions that would occur with the
addition of a strong base and with the addition of a strong acid.
-
Understand how to carry out an acid-base titration calculation.
-
For the titration of a weak base with a strong acid; outline what type
of solution remains at the equivalence point. Be
able to do the same for the titration of a weak acid with a strong base.
-
For a given ionic salt that has low solubility in water, demonstrate an
understanding of solubility equilibria and of Ksp.
-
For a given Ksp, calculate the solubility for the salt. For
a given solubility (given in M or in mg/dL), know how to determine Ksp.
-
Determine the solubility of a substance in a solution that already contains
one of the ions present in the salt.
-
For salts with basic anions, predict the effect of pH on solubility; demonstrate
an understanding of the underlying reasons for this using all appropriate
equilibria and Le Chatelier's principle.
-
Understand and diagram what a complex ion is; identify the Lewis acid and
base. Know the equilibria for complex ion formation. Discuss
how complexes affect the solubility of metal ions by showing appropriate
equilibria. Understand the role of complex ions in the human body..
-
For partially soluble salts with non Group I or II metal ions, predict
the effect of ligand concentrations (e.g. NH3) on solubility. Show
the underlying reasons for this using all appropriate equilibria and Le
Chatelier's principle.