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Electrochemical Cells definitions

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  • Galvanic Cell
    A spontaneous system generating electricity via oxidation at a negative electrode and reduction at a positive electrode, connected by a salt bridge.
  • Electrolytic Cell
    A non-spontaneous system requiring external power to drive electron flow, with forced oxidation and reduction at its electrodes.
  • Anode
    The electrode where oxidation occurs, electrons are lost, and mass decreases during cell operation.
  • Cathode
    The electrode where reduction occurs, electrons are gained, and mass increases as ions deposit.
  • Salt Bridge
    A tube containing neutral ions that completes the circuit by allowing ion flow between cell compartments.
  • Standard Cell Potential
    A measure of the cell's ability to drive electron flow, with higher values favoring reduction and strong oxidizing agents.
  • Oxidizing Agent
    A substance that gains electrons in a reaction, promoting reduction at the cathode.
  • Reducing Agent
    A substance that loses electrons in a reaction, promoting oxidation at the anode.
  • Line Notation
    A symbolic method using vertical lines to represent phase boundaries and salt bridges, summarizing cell components and reactions.
  • Half Reaction
    A representation of either oxidation or reduction, showing electron transfer at a single electrode.
  • Gibbs Free Energy
    A thermodynamic variable indicating reaction spontaneity; negative values correspond to spontaneous cell operation.
  • Equilibrium Constant
    A value relating product and reactant concentrations at equilibrium, used to predict cell spontaneity.
  • Reaction Quotient
    A ratio of current concentrations to equilibrium values, indicating the cell's progress toward equilibrium.
  • Standard Entropy
    A measure of disorder under standard conditions, influencing the spontaneity and direction of cell reactions.
  • Phase Boundary
    A separation between different physical states or oxidation states, represented by a single line in cell notation.