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Basic Concepts definitions

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  • Redox Reaction
    A process where electrons transfer between reactants, causing simultaneous oxidation and reduction.
  • Oxidation
    A process involving the loss of electrons, resulting in an increase in oxidation number.
  • Reduction
    A process involving the gain of electrons, resulting in a decrease in oxidation number.
  • Oxidation Number
    A value indicating the effective charge of an atom, reflecting electron loss or gain in reactions.
  • Reducing Agent
    A substance that donates electrons to another, causing itself to be oxidized.
  • Oxidizing Agent
    A substance that accepts electrons from another, causing itself to be reduced.
  • Electrochemical Cell
    A device that enables electron transfer between substances, generating voltage and electrical energy.
  • Faraday's Constant
    A value representing the charge carried by one mole of electrons, crucial for charge calculations.
  • Coulomb
    The SI unit of electrical charge, defined as the quantity transported by one ampere in one second.
  • Ampere
    The SI unit of electric current, representing one coulomb of charge passing per second.
  • Voltage
    A measure of electric potential difference, expressed as energy per unit charge in joules per coulomb.
  • Ohm's Law
    A relationship stating that current equals voltage divided by resistance in an electrical circuit.
  • Power
    The rate at which work is done or energy is transferred, measured in watts or joules per second.
  • Half-Reaction
    A component of a redox process showing either electron loss or gain, used for balancing equations.
  • Acidic Solution
    A reaction environment where H+ ions are present, affecting the method for balancing redox equations.
  • Basic Solution
    A reaction environment where OH- ions are present, requiring extra steps in balancing redox equations.