Download Chemical Change and Electrical Work

Chemistry 11600
Fall 2012
Learning Objectives for
Oxidation-Reduction Reactions and
Electrochemistry: Chemical Change and Electrical Work
Oxidation-Reduction Reactions
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To describe the key chemical event in a oxidation-reduction reaction.
To assign oxidation numbers to atoms in elements, compounds and ions.
To describe “oxidation” and “reduction”.
To determine whether or not a chemical reaction is a oxidation-reduction reaction.
To identify species that are “oxidized” and/or “reduced” and to identify those species
that are “oxidizing agents” and/or “reducing agents” in an oxidation-reduction
reaction.
To balance oxidation-reduction reactions in neutral, acidic or basic solution by using
the “half-reaction method”.
Electrochemistry: Chemical Change and Electrical Work
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To describe electrochemical processes in terms of oxidation-reduction reactions.
To describe an overall oxidation-reduction reaction in terms of a (balanced)
oxidation half-reaction and a (balanced) reduction half-reaction.
To identify the two half-reactions that comprise an overall oxidation-reduction
reaction using a Table of Standard Reduction Potentials.
To describe why it is necessary that the half-reactions in a voltaic cell be physically
separated in order for the cell to do electrical work.
To describe why it is necessary that a salt bridge (or porous disk) be added to a
voltaic cell in order for the cell to produce an electrical current.
To list and describe the components that are needed for the operation of a voltaic
cell.
To identify the “anode” and “cathode” in a voltaic cell.
To identify the direction of electron flow in a voltaic cell.
To describe “cell potential” as a measure of the potential of a voltaic cell to do work
on the surroundings.
To draw a diagram for the “standard hydrogen electrode” and describe its purpose.
To describe why a platinum wire is used in the standard hydrogen electrode.
To describe how half-cell potentials are experimentally measured.
To draw a diagram that illustrates how a voltaic cell with a positive cell potential
would be constructed given either two half-cell reactions or an overall cell reaction
and a Table of Standard Reduction Potentials.
To predict whether or not a given reaction (oxidation-reduction, or otherwise) is
spontaneous under non-standard, and standard, conditions by using a Table of
Standard Reduction Potentials.
Chemistry 11600
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Fall 2012
To describe why multiplication of a half-reaction by a coefficient does not change
the value of the standard cell potential for the half-reaction.
To calculate the standard cell potential for an overall voltaic cell reaction using a
Table of Standard Reduction Potentials.
To use the Nernst equation to calculate cell potentials under non-standard conditions.
To describe the difference between a “cell potential” and a “standard cell potential”.
To describe “concentration cells” and how they are constructed.
To calculate the cell potential for a concentration cell.
To calculate values for equilibrium constants by using a Table of Standard Reduction
Potentials.
To draw an atomic-scale diagram that illustrates the electrochemical processes
involved in the corrosion of iron.
To describe why metals such as aluminum and copper corrode more slowly than iron.
To describe galvanizing, alloying and cathodic protection and how these methods are
used to prevent corrosion.
To describe the difference between an “oxidation potential” and a “reduction
potential”.
To describe what information the cell potential provides about the speed of the
oxidation-reduction reaction.
To describe the difference(s) between voltaic and electrolytic cells.
To describe Faraday’s Law of Electrolysis.
To perform calculations for electrolytic cells (e.g., time, amount of substance,
amount of charge, etc.).
To describe the construction and general operation of a lead storage battery used in
automobiles.
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