Difference between revisions of "Lewis base"
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Examples of Lewis bases are conventional amines, such as [[ammonia]] and all alkyl amines, organic compounds containing a nitrogen atom (where the nitrogen is in the +3 oxidation state) such as [[pyridine]] and its derivatives. | Examples of Lewis bases are conventional amines, such as [[ammonia]] and all alkyl amines, organic compounds containing a nitrogen atom (where the nitrogen is in the +3 oxidation state) such as [[pyridine]] and its derivatives. | ||
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| + | ==References== | ||
| + | <references/> | ||
| + | ===Relevant Sciencemadness threads=== | ||
| + | *[https://www.sciencemadness.org/whisper/viewthread.php?tid=30353 Lewis Acid/Base Interactions and Product Stabilization(Solvent Effects)] | ||
[[Category:Acid-base theory]] | [[Category:Acid-base theory]] | ||
[[Category:Lewis bases]] | [[Category:Lewis bases]] | ||
Revision as of 14:11, 27 October 2017
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Lewis bases are compounds which can donate a lone pair of electrons to form a new bond with a Lewis acid. All Brønsted-Lowry bases are Lewis bases, as they can accept protons as well as other electron deficient species.
Classification
Lewis bases are split in three categoris:
- amines of the formula NH3−xRx, where R = alkyl or aryl. Pyridine and its derivatives are also included here.
- phosphines of the formula PR3−xAx, where R = alkyl, A = aryl.
- compounds of O, S, Se and Te in oxidation state 2, including water, ethers, ketones.
Examples of Lewis bases are conventional amines, such as ammonia and all alkyl amines, organic compounds containing a nitrogen atom (where the nitrogen is in the +3 oxidation state) such as pyridine and its derivatives.
