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9.9: Key Terms

Last updated

Aug 20, 2023
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- 9.8: Electrolysis
- 9.10: Key Equations

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Example and Directions
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Glossary Entries
Word(s)	Definition	Image	Caption	Link	Source
active electrode	electrode that participates as a reactant or product 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 similar to a dry cell that uses an alkaline (often potassium hydroxide) electrolyte; designed to be an improved 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
battery	single or series of galvanic cells designed for use as a source of electrical power
cathode	electrode in an electrochemical cell at which reduction occurs
cathodic protection	approach to preventing corrosion of a metal object by connecting it to a sacrificial anode composed of a more readily oxidized metal
cell notation (schematic)	symbolic representation of the components and reactions in an electrochemical cell
cell potential (E_cell)	difference in potential of the cathode and anode half-cells
concentration cell	galvanic cell comprising half-cells of identical composition but for the concentration of one redox reactant or product
corrosion	degradation of metal via a natural electrochemical process
dry cell	primary battery, also called a zinc-carbon battery, based on the spontaneous oxidation of zinc by manganese(IV)
electrode potential (E_X)	the potential of a cell in which the half-cell of interest acts as a cathode when connected to the standard hydrogen electrode
electrolysis	process using electrical energy to cause a nonspontaneous process to occur
electrolytic cell	electrochemical cell in which an external source of electrical power is used to drive an otherwise nonspontaneous process
Faraday’s constant (F)	charge on 1 mol of electrons; F = 96,485 C/mol e⁻
fuel cell	devices similar to galvanic cells that require a continuous feed of redox reactants; also called a flow battery
galvanic (voltaic) cell	electrochemical cell in which a spontaneous redox reaction takes place; also called a voltaic cell
galvanization	method of protecting iron or similar metals from corrosion by coating with a thin layer of more easily oxidized zinc.
half cell	component of a cell that contains the redox conjugate pair (“couple”) of a single reactant
inert electrode	electrode that conducts electrons to and from the reactants in a half-cell but that is not itself oxidized or reduced
lead acid battery	rechargeable battery commonly used in automobiles; it typically comprises six galvanic cells based on Pb half-reactions in acidic solution
lithium ion battery	widely used rechargeable battery commonly used in portable electronic devices, based on lithium ion transfer between the anode and cathode
Nernst equation	relating the potential of a redox system to its composition
nickel-cadmium battery	rechargeable battery based on Ni/Cd half-cells with applications similar to those of lithium ion batteries
primary cell	nonrechargeable battery, suitable for single use only
sacrificial anode	electrode constructed from an easily oxidized metal, often magnesium or zinc, used to prevent corrosion of metal objects via cathodic protection
salt bridge	tube filled with inert electrolyte solution
secondary cell	battery designed to allow recharging
standard cell potential	the cell potential when all reactants and products are in their standard states (1 bar or 1 atm or gases; 1 M for solutes), usually at 298.15 K
standard electrode potential ()	electrode potential measured under standard conditions (1 bar or 1 atm for gases; 1 M for solutes) usually at 298.15 K
standard hydrogen electrode (SHE)	half-cell based on hydrogen ion production, assigned a potential of exactly 0 V under standard state conditions, used as the universal reference for measuring electrode potential

active electrode | electrode that participates as a reactant or product 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 similar to a dry cell that uses an alkaline (often potassium hydroxide) electrolyte; designed to be an improved 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

battery | single or series of galvanic cells designed for use as a source of electrical power

cathode | electrode in an electrochemical cell at which reduction occurs

cathodic protection | approach to preventing corrosion of a metal object by connecting it to a sacrificial anode composed of a more readily oxidized metal

cell notation (schematic) | symbolic representation of the components and reactions in an electrochemical cell

cell potential (E_cell) | difference in potential of the cathode and anode half-cells

concentration cell | galvanic cell comprising half-cells of identical composition but for the concentration of one redox reactant or product

corrosion | degradation of metal via a natural electrochemical process

dry cell | primary battery, also called a zinc-carbon battery, based on the spontaneous oxidation of zinc by manganese(IV)

electrode potential (E_X) | the potential of a cell in which the half-cell of interest acts as a cathode when connected to the standard hydrogen electrode

electrolysis | process using electrical energy to cause a nonspontaneous process to occur

electrolytic cell | electrochemical cell in which an external source of electrical power is used to drive an otherwise nonspontaneous process

Faraday’s constant (F) | charge on 1 mol of electrons; F = 96,485 C/mol e⁻

fuel cell | devices similar to galvanic cells that require a continuous feed of redox reactants; also called a flow battery

galvanic (voltaic) cell | electrochemical cell in which a spontaneous redox reaction takes place; also called a voltaic cell

galvanization | method of protecting iron or similar metals from corrosion by coating with a thin layer of more easily oxidized zinc.

half cell | component of a cell that contains the redox conjugate pair (“couple”) of a single reactant

inert electrode | electrode that conducts electrons to and from the reactants in a half-cell but that is not itself oxidized or reduced

lead acid battery | rechargeable battery commonly used in automobiles; it typically comprises six galvanic cells based on Pb half-reactions in acidic solution

lithium ion battery | widely used rechargeable battery commonly used in portable electronic devices, based on lithium ion transfer between the anode and cathode

Nernst equation | relating the potential of a redox system to its composition

nickel-cadmium battery | rechargeable battery based on Ni/Cd half-cells with applications similar to those of lithium ion batteries

primary cell | nonrechargeable battery, suitable for single use only

sacrificial anode | electrode constructed from an easily oxidized metal, often magnesium or zinc, used to prevent corrosion of metal objects via cathodic protection

salt bridge | tube filled with inert electrolyte solution

secondary cell | battery designed to allow recharging

standard cell potential | the cell potential when all reactants and products are in their standard states (1 bar or 1 atm or gases; 1 M for solutes), usually at 298.15 K

standard electrode potential () | electrode potential measured under standard conditions (1 bar or 1 atm for gases; 1 M for solutes) usually at 298.15 K

standard hydrogen electrode (SHE) | half-cell based on hydrogen ion production, assigned a potential of exactly 0 V under standard state conditions, used as the universal reference for measuring electrode potential

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