Page 895 - Chemistry--atom first

Chapter 16 | Electrochemistry 885
Key Terms
active electrode electrode that participates in the oxidation-reduction reaction of an electrochemical cell; the mass of an active electrode changes during the oxidation-reduction reaction
alkaline battery primary battery that uses an alkaline (often potassium hydroxide) electrolyte; designed to be an exact replacement for the dry cell, but with more energy storage and less electrolyte leakage than typical dry cell
anode electrode in an electrochemical cell at which oxidation occurs; information about the anode is recorded on the left side of the salt bridge in cell notation
battery galvanic cell or series of cells that produces a current; in theory, any galvanic cell
cathode electrode in an electrochemical cell at which reduction occurs; information about the cathode is recorded
on the right side of the salt bridge in cell notation
cathodic protection method of protecting metal by using a sacrificial anode and effectively making the metal that needs protecting the cathode, thus preventing its oxidation
cell notation shorthand way to represent the reactions in an electrochemical cell
cell potential difference in electrical potential that arises when dissimilar metals are connected; the driving force for
the flow of charge (current) in oxidation-reduction reactions
circuit path taken by a current as it flows because of an electrical potential difference
concentration cell galvanic cell in which the two half-cells are the same except for the concentration of the solutes; spontaneous when the overall reaction is the dilution of the solute
corrosion degradation of metal through an electrochemical process
current flow of electrical charge; the SI unit of charge is the coulomb (C) and current is measured in amperes

dry cell primary battery, also called a zinc-carbon battery; can be used in any orientation because it uses a paste as
the electrolyte; tends to leak electrolyte when stored
electrical potential energy per charge; in electrochemical systems, it depends on the way the charges are distributed
within the system; the SI unit of electrical potential is the volt
electrical work (wele) negative of total charge times the cell potential; equal to wmax for the system, and so equals
the free energy change (ΔG)
electrolysis process using electrical energy to cause a nonspontaneous process to occur
electrolytic cell electrochemical cell in which electrolysis is used; electrochemical cell with negative cell potentials
electroplating depositing a thin layer of one metal on top of a conducting surface
Faraday’s constant (F) charge on 1 mol of electrons; F = 96,485 C/mol e−
fuel cell devices that produce an electrical current as long as fuel and oxidizer are continuously added; more efficient than internal combustion engines
galvanic cell electrochemical cell that involves a spontaneous oxidation-reduction reaction; electrochemical cells with positive cell potentials; also called a voltaic cell