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Identifying Acids and Bases definitions

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Terms in this set (15)

  • Hydronium Ion
    A positively charged ion (H3O+) formed when an acid dissolves in water.
  • Binary Acids
    Acids composed of hydrogen and one other electronegative element, lacking oxygen.
  • Haloacids
    Binary acids formed by hydrogen and halogens like F, Cl, Br, and I.
  • Oxyacids
    Acids containing hydrogen, oxygen, and a non-metal, formed by hydrating non-metal oxides.
  • Electronegativity
    A measure of an atom's ability to attract and hold electrons, influencing acid strength.
  • Atomic Radius
    The size of an atom, affecting the strength of binary acids in the same group.
  • Strong Electrolytes
    Substances that completely ionize in water, characteristic of strong acids and bases.
  • Weak Electrolytes
    Substances that partially ionize in water, characteristic of weak acids and bases.
  • Amphoteric Species
    Compounds that can act as either an acid or a base, often with a hydrogen and a negative charge.
  • Amines
    Organic compounds containing nitrogen and hydrogen, acting as weak bases.
  • Hydroxide Ion
    A negatively charged ion (OH-) commonly found in bases.
  • Hydride Ion
    A negatively charged ion (H-) formed when hydrogen gains an electron.
  • Oxide Ion
    A negatively charged ion (O2-) formed when oxygen gains electrons.
  • Amide Ion
    A negatively charged ion (NH2-) derived from ammonia, found in bases.
  • Methylamine
    An amine with the formula CH3NH2, acting as a weak base.