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Anode
The electrode that is the source of the negative charge, designated by a minus sign (-), this electrode is the site of oxidation.
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Cathode
The electrode that is the source of positive charge, designated by a plus sign (+), this electrode is the site of reduction.
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Cell Potential
The overall electrical potential of an electrochemical cell. It is the sum of the potential for the reduction potential of the cathode and the oxidation potential of the anode.
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Current
Charge flow.
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Electrochemistry
The study of the exchange between electrical and chemical energy.
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Electrode
A conducting material placed in physical contact with a half-reaction on which the electron transfers in the redox reaction take place.
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Electrolysis
A reaction that consumes electrical energy to split molecules apart.
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Electrolytic Cell
A cell that consumes electrical energy to promote a non-spontaneous redox reaction.
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Electroplating
The deposition of a solid material onto an electrode, almost always the cathode.
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Electrorefining
Process by which materials, usually metals, are purified by means of an electrolytic cell. The anode is the impure metal and the cathode is a very pure sample of the metal.
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emf
Electromotive force, i.e. a potential.
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Galvanic Cell
An electrochemical cell with a positive cell potential that allows that chemical energy to be converted into electrical energy available to do useful work.
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Half-Cell
A half-reaction and its electrode, it is half of a galvanic cell.
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Half-Reaction
Either an oxidation or a reduction reaction, it represents half of the redox reaction.
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Hess's Law
The sum of the state functions of a series of reactions is the same as the state function for the sum of the reactions.
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Line Notation
A shorthand way of describing an electrochemical cell without drawing a picture.
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Oxidation
The loss of an electron from a species (an increase in its oxidation number).
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Oxidation Number
A conceptual bookkeeping numbering system that allows us to track the number electrons transferred during a redox reaction.
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Oxidation Potential
The potential of a half-reaction written and an oxidation reaction, it is the opposite sign of the same reaction written as a reduction.
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Oxidizing Agent
A reactant in a redox reaction that accepts an electron from the oxidized species. The oxidizing agent is reduced.
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Potentiometer
A device that measures electrical potential.
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Reaction Quotient
Similar to the form of an equilibrium constant, the reaction quotient is the ratio of the product of the each product in a reaction raised to its stoichiometric power divided by the product of each reactant raised to its stoichiometric power from the bala nced equation.
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Redox
A reaction involving the transfer of one or more electrons from the reducing agent to the oxidizing agent.
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Reducing Agent
A reactant in a redox reaction that donates an electron to the reduced species. The reducing agent is oxidized.
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Reduction
The gain of an electron by a species (a decrease in oxidation number).
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Reduction Potential
Arbitrarily setting the potential of the standard hydrogen electrode, SHE, to zero, all other half reactions are measured by their power to reduce hydrogen. The voltage given by the construction of a galvanic cell between the SHE and the reduction of interest gives the standard reduction potential of that reduction.
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Standard State
An arbitrarily defined set of conditions--273K, 1atm for gasses, or 1M for solutions.
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Work
Force over a distance.
Terms
Formulae
| Adding Cell Potentials | Eocell = Eo1 + Eo2 |
| Nernst Equation | E = Eo - (RT/nF) ln Q |
