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17.9: Key Terms

  • Page ID
    452867
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    Example and Directions
    Words (or words that have the same definition)The definition is case sensitive(Optional) Image to display with the definition [Not displayed in Glossary, only in pop-up on pages](Optional) Caption for Image(Optional) External or Internal Link(Optional) Source for Definition
    (Eg. "Genetic, Hereditary, DNA ...")(Eg. "Relating to genes or heredity")The infamous double helix https://bio.libretexts.org/CC-BY-SA; Delmar Larsen
    Glossary Entries
    Word(s)DefinitionImageCaptionLinkSource
    active electrodeelectrode 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 batteryprimary 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    
    anodeelectrode in an electrochemical cell at which oxidation occurs    
    batterysingle or series of galvanic cells designed for use as a source of electrical power    
    cathodeelectrode in an electrochemical cell at which reduction occurs    
    cathodic protectionapproach 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 (Ecell)difference in potential of the cathode and anode half-cells    
    concentration cellgalvanic cell comprising half-cells of identical composition but for the concentration of one redox reactant or product    
    corrosiondegradation of metal via a natural electrochemical process    
    dry cellprimary battery, also called a zinc-carbon battery, based on the spontaneous oxidation of zinc by manganese(IV)    
    electrode potential (EX)the potential of a cell in which the half-cell of interest acts as a cathode when connected to the standard hydrogen electrode    
    electrolysisprocess using electrical energy to cause a nonspontaneous process to occur    
    electrolytic cellelectrochemical 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 celldevices similar to galvanic cells that require a continuous feed of redox reactants; also called a flow battery    
    galvanic (voltaic) cellelectrochemical cell in which a spontaneous redox reaction takes place; also called a voltaic cell    
    galvanizationmethod of protecting iron or similar metals from corrosion by coating with a thin layer of more easily oxidized zinc.    
    half cellcomponent of a cell that contains the redox conjugate pair (“couple”) of a single reactant    
    inert electrodeelectrode that conducts electrons to and from the reactants in a half-cell but that is not itself oxidized or reduced    
    lead acid batteryrechargeable battery commonly used in automobiles; it typically comprises six galvanic cells based on Pb half-reactions in acidic solution    
    lithium ion batterywidely used rechargeable battery commonly used in portable electronic devices, based on lithium ion transfer between the anode and cathode    
    Nernst equationrelating the potential of a redox system to its composition    
    nickel-cadmium batteryrechargeable battery based on Ni/Cd half-cells with applications similar to those of lithium ion batteries    
    primary cellnonrechargeable battery, suitable for single use only    
    sacrificial anodeelectrode constructed from an easily oxidized metal, often magnesium or zinc, used to prevent corrosion of metal objects via cathodic protection    
    salt bridgetube filled with inert electrolyte solution    
    secondary cellbattery 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    

    17.9: Key Terms is shared under a CC BY 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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