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Redox Reaction definitions

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Terms in this set (15)

  • Redox Reactions
    Involve the transfer of electrons from one reactant to another, encompassing both oxidation and reduction processes.
  • Oxidation
    The process where a species loses electrons, resulting in an increase in oxidation number.
  • Reduction
    The process where a species gains electrons, resulting in a decrease in oxidation number.
  • Oxidation Number
    A value assigned to an element in a compound representing its degree of oxidation or reduction.
  • Reducing Agent
    A substance that donates electrons in a redox reaction, undergoing oxidation itself.
  • Oxidizing Agent
    A substance that accepts electrons in a redox reaction, undergoing reduction itself.
  • Elemental Form
    A state where an element is uncombined with others, having an oxidation number of zero.
  • Peroxide
    A compound with the formula X2O2, where oxygen has an oxidation state of -1.
  • Superoxide
    A compound with the formula XO2, where oxygen has an oxidation state of -0.5.
  • Faraday's Constant
    The charge of one mole of electrons, approximately 9.647 x 10^4 coulombs per mole.
  • Coulombs
    The unit of electrical charge, represented by the symbol C.
  • Amperes
    The unit of electrical current, representing coulombs per second.
  • Voltage
    The potential difference measured in joules per coulomb, driving electron flow.
  • Ohm's Law
    A principle stating that current equals voltage divided by resistance.
  • Power
    The rate of doing work, measured in watts, equivalent to joules per second.