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Standard Potentials definitions

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  • Voltage
    Amount of work done as electrons move between electrodes, measured in joules per coulomb.
  • Electrochemical Cell
    System where chemical energy is converted to electrical energy via electron transfer between electrodes.
  • Half Reaction
    Equation showing either reduction or oxidation, with electrons as reactants or products.
  • Reduction
    Process involving a decrease in oxidation number as electrons are gained by a species.
  • Oxidation Number
    Value indicating the hypothetical charge an atom would have if all bonds were ionic.
  • Standard Hydrogen Electrode
    Reference electrode assigned a potential of zero volts for comparing other half reactions.
  • Reference Electrode
    Electrode used as a baseline to measure and compare the potentials of other electrodes.
  • Cell Potential
    Difference in potential between cathode and anode, indicating the voltage produced by a cell.
  • Cathode
    Electrode where reduction occurs and electrons are accepted during a redox reaction.
  • Anode
    Electrode where oxidation occurs and electrons are released during a redox reaction.
  • Galvanic Cell
    Device that generates electrical energy from spontaneous redox reactions between electrodes.
  • Voltaic Cell
    Another term for a galvanic cell, producing electricity from spontaneous chemical reactions.
  • Nernst Equation
    Mathematical relationship used to calculate cell potential when ion concentrations differ from 1 molar.
  • Unity
    Condition where ion concentrations are exactly 1 molar, simplifying cell potential calculations.
  • Redox Reaction
    Chemical process involving simultaneous reduction and oxidation, with electron transfer between species.