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Acid Strength definitions

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  • Binary Acid
    A molecule with a hydrogen ion bonded to a single electronegative nonmetal, such as halogens or chalcogens.
  • Oxyacid
    A compound containing hydrogen, a nonmetal, and oxygen, often with the nonmetal as part of a polyatomic ion.
  • Electronegativity
    A measure of an atom's ability to attract shared electrons, increasing toward the top right of the periodic table.
  • Atomic Radius
    The effective size of an atom, which increases down a group and influences acid strength in binary acids.
  • Strong Acid
    A substance that completely ionizes in water, producing nearly 100% ions and acting as a strong electrolyte.
  • Weak Acid
    A substance that only partially ionizes in water, establishing equilibrium and producing fewer ions.
  • Hydronium Ion
    The H3O+ species formed when a hydrogen ion associates with water, functionally equivalent to H+ in solution.
  • Strong Electrolyte
    A compound that dissociates completely in solution, resulting in high electrical conductivity.
  • Weak Electrolyte
    A compound that only partially dissociates in solution, resulting in low electrical conductivity.
  • Ka Value
    An equilibrium constant quantifying acid dissociation in water; values much greater than 1 indicate strong acids.
  • pKa Value
    The negative logarithm of the acid dissociation constant; negative values correspond to strong acids.
  • Amphoteric Species
    A molecule or ion capable of acting as either an acid or a base, often containing both hydrogen and a negative charge.
  • Polyatomic Ion
    A charged species composed of multiple atoms, often serving as the nonmetal component in oxyacids.
  • Exception
    A case where a compound does not follow the general rules for acid strength, such as oxalic acid or iodic acid.