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The Chemistry of Acids and Bases

This chapter explores the chemistry of Lewis acids and bases, explaining their characteristics, formation, and reactions. Learn about coordinate covalent bonds, the amphoteric nature of metal hydroxides, and the basicity of oxoanions.

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The Chemistry of Acids and Bases

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  1. The Chemistry of Acids and Bases Chapter 17

  2. Lewis Acids & Bases Lewis acid = a substance that accepts an electron pair Lewis base = a substance that donates an electron pair

  3. Reaction of a Lewis Acid and Lewis Base New bond formed using electron pair from the Lewis base. • Coordinate covalent bond

  4. Lewis Acids & Bases Formation of hydronium ion is also an excellent example. • Electron pair of the new O-H bond originates on the Lewis base.

  5. Lewis Acid/Base Reaction

  6. Lewis Acids & Bases This explains AMPHOTERICnature of some metal hydroxides. Al(OH)3(s) + 3 H+D Al3+ + 3 H2O Here Al(OH)3 is a Brønsted base. Al(OH)3(s) + OH- --> Al(OH)4- Here Al(OH)3 is a Lewis acid.

  7. Basicity of Oxoanions NO3- These ions are BASES. They become more and more basic as the negative charge increases. As the charge goes up, they interact more strongly with polar water molecules. CO32- PO43-

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