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Bronsted Lowry Acid and Base definitions

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  • Bronsted-Lowry Theory
    A model describing acids as proton donors and bases as proton acceptors, applicable beyond just water-based solutions.
  • Arrhenius Definition
    A model where acids increase H+ concentration in water and bases produce OH-, limited to aqueous solutions.
  • Proton
    A hydrogen ion (H+) that can be donated by acids or accepted by bases in chemical reactions.
  • Acid
    A substance capable of donating a hydrogen ion (H+) to another species in a chemical reaction.
  • Base
    A substance capable of accepting a hydrogen ion (H+) from another species, often possessing lone pairs or negative charge.
  • Conjugate Acid-Base Pair
    Two species differing by only one hydrogen ion (H+), related through the gain or loss of a proton.
  • Hydronium Ion
    A water molecule with an extra hydrogen ion, represented as H3O+, formed when acids donate H+ in water.
  • Hydroxide Ion
    A negatively charged ion (OH-) formed when a base accepts a hydrogen ion or when water loses H+.
  • Lone Pair
    A pair of valence electrons not involved in bonding, often responsible for a base's ability to accept H+.
  • Aqueous Solution
    A mixture where water is the solvent, central to Arrhenius but not required for Bronsted-Lowry definitions.
  • Negative Charge
    An excess of electrons on a species, increasing its tendency to attract and accept a hydrogen ion.
  • Hydrogen Ion
    A single proton (H+) released by acids or accepted by bases, central to acid-base reactions.