Lewis acid | Wikipedia audio article
Channel: wikipedia tts
Date: 2018-12-08

This is an audio version of the Wikipedia Article:
Lewis acid


00:00:57 1 Depicting adducts
00:02:08 2 Examples
00:04:08 2.1 Simple Lewis acids
00:05:15 2.2 Complex Lewis acids
00:06:25 2.3 Hsup+/sup as Lewis acid
00:06:59 2.4 Applications of Lewis acids
00:07:32 3 Lewis bases
00:08:16 3.1 Applications of Lewis bases
00:09:22 4 Hard and soft classification
00:10:07 5 ECW model
00:11:39 6 There is no single order of Lewis base strengths
00:12:21 7 History
00:12:46 7.1 Reformulation of Lewis theory
00:12:57 7.2 Comparison with Brønsted–Lowry theory
00:13:16 8 See also
00:13:25 9 References
00:14:13 10 Further reading
00:15:21 undefined
00:16:31 undefined



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SUMMARY
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A Lewis acid is a chemical species that contains an empty orbital which is capable of accepting an electron pair from a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that has a filled orbital containing an electron pair which is not involved in bonding but may form a dative bond with a Lewis acid to form a Lewis adduct. For example, NH3 is a Lewis base, because it can donate its lone pair of electrons. Trimethylborane (Me3B) is a Lewis acid as it is capable of accepting a lone pair. In a Lewis adduct, the Lewis acid and base share an electron pair furnished by the Lewis base, forming a dative bond. In the context of a specific chemical reaction between NH3 and Me3B, the lone pair from NH3 will form a dative bond with the empty orbital of Me3B to form an adduct NH3•BMe3. The terminology refers to the contributions of Gilbert N. Lewis.