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Lewis Acid and Base definitions

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Terms in this set (15)

  • Lewis Acid
    A substance that accepts an electron pair, often having less than 8 valence electrons or a positive charge.
  • Lewis Base
    A substance that donates an electron pair, typically possessing lone pairs or a negative charge.
  • Electron Acceptor
    A chemical species that can accept electrons, often associated with Lewis acids.
  • Electron Donor
    A chemical species that can donate electrons, often associated with Lewis bases.
  • Electronegativity
    A measure of an atom's ability to attract and hold electrons, influencing Lewis acid behavior.
  • Lone Pair
    A pair of valence electrons not involved in bonding, crucial for Lewis base activity.
  • Octet Rule
    A principle stating atoms tend to have eight electrons in their valence shell, influencing Lewis acid behavior.
  • Valence Electrons
    Electrons in the outermost shell of an atom, important for determining Lewis acid or base properties.
  • Positive Charge
    A condition where an atom has more protons than electrons, making it a potential Lewis acid.
  • Negative Charge
    A condition where an atom has more electrons than protons, making it a potential Lewis base.
  • Transition Metals
    Elements that can act as Lewis acids due to having less than 8 valence electrons.
  • Boron Trifluoride
    A compound where boron acts as a Lewis acid due to having only 6 valence electrons.
  • Aluminum Bromide
    A compound where aluminum acts as a Lewis acid due to having only 6 valence electrons.
  • Zinc
    A transition metal that can act as a Lewis acid with 4 valence electrons.
  • Group 7A
    Elements like fluorine and chlorine, which can form Lewis acids when bonded to hydrogen.