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Understanding Lewis Acids and Bases: A Generalized Acid-Base Model

Learn how the Lewis acid-base model broadens our understanding of chemical reactions, with examples and comparisons to Arrhenius and Brønsted-Lowry definitions. Discover the roles of Lewis acids and bases in forming covalent bonds.

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Understanding Lewis Acids and Bases: A Generalized Acid-Base Model

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  1. The General Approach The Lewis Acid-Base Model

  2. History • Arrhenius Definition: Limited but useful • Definition is generalized by the introduction of the Brøwnsted-Lowry definition • Even broader model suggested by G.N. Lewis in 1920s

  3. Definitions • Lewis Acid: an atom, ion, or molecule that accepts an electron pair in order to form a covalent bond Lewis Base: an atom, ion, or molecule that donates an electron pair in order to form a covalent bond

  4. What does it mean? • A Lewis acid has an empty electron orbital to accept more electrons(like H+) • A Lewis base(like OH-) has electrons which can be given to a Lewis acid, forming a Lewis adduct

  5. So wait… • Yes. Arrhenius acids and Brøwnstead-Lowry Acids are also Lewis acids! Woah!

  6. Why should I care? • Because, it means that rxns like this can count as acid-base reactions Even though they don’t count as them under other definitions

  7. So, to summarize… • Let’s compare the definitions!

  8. Arrhenius acid-base definition • Acid H+: producer • Base: OH- produce • Only works in water

  9. Brøwnsted-Lowry Definition • Acid: H+ Dono • Base: H+ acceptor

  10. Lewis model • Acid, Electron-Pair acceptor • Base, Electron-Pair donator

  11. And now you know!

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