Ate complex
An ate complex in chemistry is a salt formed by the reaction of a Lewis acid with a Lewis base whereby the central atom (from the Lewis acid) increases its valence and gains a negative formal charge.[1] (In this definition, the meaning of valence is equivalent to coordination number).
Often in chemical nomenclature the phrase ate is suffixed to the element in question. For example, the ate complex of a boron compound is called a borate. Thus trimethylborane and methyllithium react to form the ate compound Li+B(CH3)4−, lithium tetramethylborate(1-). This concept was introduced by Georg Wittig in 1958.[2][3] Ate complexes are common for metals, including the transition metals (groups 3-11), as well as the metallic or semi-metallic elements of group 2, 12, and 13. They are also well-established for third-period or heavier elements of groups 14–18 in their higher oxidation states.
Ate complexes are a counterpart to onium ions. Lewis acids form ate ions when the central atom reacts with a donor (2 e– X-type ligand), gaining one more bond and becoming a negative-charged anion. Lewis bases form onium ions when the central atom reacts with an acceptor (0 e– Z-type ligand), gaining one more bond and becoming a positive-charged cation.[4]
-ate suffix
The phrase -ate ion or ate ion can refer generically to many negatively charged anions. -ate compound or ate compound can refer to salts of the anions or esters of the functional groups.
Chemical terms ending in -ate (and -ite) generally refer to the negatively charged anions, neutral radicals, and covalently bonded functional groups that share the same chemical formulas (with different charges). For example, the nitrate anion, NO−
3; the nitrate functional group that forms nitrate esters, –NO
3 or –ONO
2; and the nitrate radical or nitrogen trioxide, NO•
3.
Most numerous are oxyanions (oxyacids that have lost one or more protons to deprotonation) and the radicals and functional groups that share their names. The large family starts with borate, carbonate, nitrate, fluorate, aluminate, silicate, phosphate, sulfate, chlorate, titanate, vanadate, chromate, manganate, ferrate, percobaltate, germanate, arsenate, selenate, bromate, molybdate, pertechnate, perruthenate, stannate, antimonate, tellurate, iodate, perxenate, tungstate, plumbate, bismuthate. Also the partially deprotonated hydrogensulfate, hydrogenphosphate, dihydrogenphosphate, etc. Also phosphonate, sulfonate, etc. Also carboxylate ions such as formate, acetate, propionate, butyrate, isobutyrate; oxalate, etc. Also methanolate / methoxide, ethanolate / ethoxide, etc. Also cyanate, isocyanate, thiocyanate, fulminate. Sulfur oxoanions, thioacetate, thiolates. Chlorosulfate, chloroacetate, etc.
A lyate ion is a generic solvent molecule that has become a negative ion by loss of one or more protons.
The -ate suffix also applies to negative fluoroanions, fluorides which have gained one or more protons and twice as many electrons. Tetrafluoroborate, BF−
4, is boron trifluoride, BF
3, which has gained one proton and two electrons.
References
- ^ Advanced organic Chemistry, Reactions, mechanisms and structure 3ed. Jerry March ISBN 0-471-85472-7
- ^ G. Wittig (1958). "Komplexbildung und Reaktivität in der metallorganischen Chemie". Angewandte Chemie. 70 (3): 65–71. doi:10.1002/ange.19580700302.
- ^ Wittig, Georg (1966). "The role of ate complexes as reaction-determining intermediates". Quarterly Reviews, Chemical Society. 20 (2): 191. doi:10.1039/QR9662000191.
- ^ Advanced Organic Chemistry: Reactions and mechanisms, Maya Shankar Singh, 2007, Dorling Kindersley, ISBN 978-81-317-1107-1
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