Arrhenius Theory
- Water solutions only
- Acids have more H+ than OH- in water
- Bases have more OH- than H+ in water
- NaC2H3O2 + H2O ---> Na+ + HC2H3O2 + OH-
Bronsted-Lowry Theory
- Works for any solvent that can accept a proton
- Acids are proton donors
- Bases are proton acceptors
- HClO4 + HC2H3O2 ---> H2C2H3O2+ + ClO4-
Lewis Acids and Bases
- A general definition used to describe formation of coordinate bonds
- Acids are electron pair acceptors
- Bases are electron pair donors
- BF3 (acid) + :NH3 (base) ---> F3B-NH3
- Used a lot when describing synthetic reactions in organic chemistry
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