20 - Chemistry 1000 Lecture 20: Lewis acids and bases Marc...

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Chemistry 1000 Lecture 20: Lewis acids and bases Marc R. Roussel
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Ammonia as a base We all know that ammonia is a Brønsted base: H H H H H N H H N + + .. + H Thinking of ammonia as a Brønsted base, we would say that it is accepting a proton. An alternative viewpoint is that ammonia is donating an electron pair to H + .
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Now consider B F F F F F N: H H H N H H H B F + This reaction and the reaction of NH 3 with H + are clearly of the same kind, even though one is a Brønsted acid-base reaction, and the other isn’t.
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Lewis acids and bases Lewis acid: electron pair acceptor Lewis base: electron pair donor
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CO 2 as a Lewis acid H :O: C :O: C :O: O O H H O H :O: C :O: O H H .. .. .. .. + .. .. .. Note that this Lewis acid-base reaction make CO 2 into the Brønsted acid H 2 CO 3 .
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In the gas phase, many of these exist as Lewis dimers: :Cl Al Cl: Al Cl: Al Cl Al Cl :Cl: :Cl: :Cl: :Cl: :Cl: :Cl: :Cl .. ..
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This note was uploaded on 03/03/2012 for the course CHEM 1000 taught by Professor Marc during the Fall '06 term at Lethbridge College.

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20 - Chemistry 1000 Lecture 20: Lewis acids and bases Marc...

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