🤲Lewis acid vs Lewis base🎁
The Lewis theory defines acids and bases by electron pairs, broadening the idea beyond protons and hydroxide ions.
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🤲Lewis acid
- ✓Accepts a pair of electrons
- ✓An electron-pair acceptor
- ✓Often has an empty orbital
- ✓Includes species with no protons
- ✓Examples: BF3, H+, metal cations
🎁Lewis base
- ✓Donates a pair of electrons
- ✓An electron-pair donor
- ✓Usually has a lone pair available
- ✓Includes species with no hydroxide
- ✓Examples: NH3, H2O, OH-
Verdict
Lewis acids accept electron pairs and Lewis bases donate them, a definition broad enough to cover reactions with no protons at all. They form a bond by sharing one pair.
Frequently asked
How does the Lewis definition differ?+
It focuses on electron pairs rather than proton transfer, so it covers far more reactions.
Is every Lewis base also a Brønsted base?+
Many are, but the Lewis definition is broader and includes species that accept no protons.
What bond forms in a Lewis reaction?+
A coordinate covalent bond, where the base supplies both shared electrons.
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