Hauser base

Hauser bases, also called magnesium amide bases, are magnesium compounds used in organic chemistry as bases for metalation reactions. These compounds were first described by Charles R. Hauser in 1947.[1] Compared with organolithium reagents, the magnesium compounds have more covalent, and therefore less reactive, metal-ligand bonds. Consequently, they display a higher degree of functional group tolerance and a much greater chemoselectivity.[2] Generally, Hauser bases are used at room temperature while reactions with organolithium reagents are performed at low temperatures, commonly at -78 °C.

Structure

Solid state structure

Like all Grignard dimers,[3] Hauser bases derived from 2,2,6,6-tetramethylpiperidine (TMP)[4] and HMDS[5] are bridged by halides in the solid state. In contrast to Grignard reagents, dimeric amido bridged Hauser bases exist, too. All have one in common: they are bridged by less bulky amido ligands such as Et2N−[6], Ph3P=N−[7] and iPr2N−.[8] The displacement to halide bridges may be a result of the bulky groups on the amide ligand.

TMP Hauser Base in the solid state
.
HMDS Hauser Base in the solid state
.
Diethylamido Hauser Base in the solid state
.

Solution structure

Although there is a great deal of information on the utility of these reagents, very little is known regarding the nature of Hauser bases in solution. One reason for that lack of information is that Hauser bases show a complex behaviour in solution. It was proposed that it could be similar to the Schlenk equilibrium of Grignard reagents in ether solution, where more than one magnesium containing species exists.[9] In 2016, Neufeld et al. showed by diffusion-ordered spectroscopy (DOSY)[10] that the solution structure of iPr2NMgCl is best represented by the common Schlenk equilibrium: [11]

iPr2NMgCl (A) ⇋ (iPr2N)2Mg (B) + MgCl2

This equilibrium is highly temperature dependent with heteroleptic (A) to be the main species at high temperatures and homoleptic (B) at low temperatures. Dimeric species with bridging chlorides and amides are also present in the THF solution, although alkyl magnesium chlorides do not dimerize in THF. At low temperatures, where an excess of MgCl2 is available MgCl2 co-coordinated species are present in solution, too.[11]

Uses

Hauser bases are generally used as metalation reagents, like organolithiums or metal amides. The breakthrough in synthetic protocols of Hauser bases culminates in the 1980s and 1990s. Eaton and co-workers showed that iPr2NMgBr selectively magnesiate carboxamides in ortho position. [12] Later, Kondo, Sakamo and co-workers reported the utility of iPr2NMgX (X= Cl, Br) as selective deprotonation reagents (exclusively at the 2-position) for heterocyclic thiophene [13] and phenylsulphonyl-substituted indoles. [14]

α-magnesiation of a carboxamide with TMP2Mg or iPr2NMgBr followed by the subsequent reaction with CO2 and CH2N2.
2-carbethoxythiophene was metalated at the ortho position by using an excess of iPr2NMgCl. Afterwards the magnesiated intermediate was treated with iodine to give iodothiophene in 77% yield.
Selective magnesiation of an indole in ortho position followed by the reaction with benzaldehyde give the substituted indol in 83% yield.

A huge disadvantage of Hauser bases is their poor solubility in THF. In consequence, the metalation rates are slow and a huge excess of base is required (mostly 10 equiv.). This circumstance complicates the functionalization of the metaled intermediate with an electrophile. A better solubility and reactivity was achieved by adding to the Hauser base stoichiometric amounts of LiCl. These so called Turbo-Hauser bases like e.g. TMPMgCl·LiCl and iPr2NMgCl·LiCl are commercially available[15] and show an enhanced kinetic basicity, excellent regioselectivity and high functional group tolerance for a large number of aromatic and heteroaromatic substrates. [16][17]

Preparation

The Hauser bases are prepared by mixing an amine and a Grignard reagent.

R2NH + R'MgX → R2NMgX + R'H

X = Cl, Br, I

Commonly used Hauser bases

iPr2NMgX

TMPMgX (TMP = 2,2,6,6,tetramethylpiperidino)

X= Cl, Br

References

  1. ↑ Hauser, C. R.; Walker, H, G. J. Am. Chem. Soc. 1947, 69, 295
  2. ↑ Li–Yuan Bao, R.; Zhao, R.; Shi, L. (2015). "Progress and developments in the turbo Grignard reagent i-PrMgCl·LiCl: a ten-year journey". Chem. Commun. 51: 6884–6900. doi:10.1039/C4CC10194D.
  3. ↑ e.g.; Seven, Ö.; Bolte, M.; Lerner, H.-W. (2013). "Di-μ-bromido-bis[(diethyl ether-κO)(2,4,6-trimethylphenyl)magnesium]: the mesityl Grignard reagent". Acta Crystallogr. E. 69: m424–m424. doi:10.1107/S1600536813017108.
  4. ↑ García–Álvarez, P.; Graham, D. V.; Hevia, E.; Kennedy, A. R.; Klett, J.; Mulvey, R. E.; O'Hara, C. T.; Weatherstone, S. (2008). "Unmasking Representative Structures of TMP-Active Hauser and Turbo-Hauser Bases". Angew. Chem. Int. Ed. 47: 8079–8081. doi:10.1002/anie.200802618.
  5. ↑ Yang, K.-C.; Chang, C.-C.; Huang, J.-Y.; Lin, C.-C.; Lee, G.-H.; Wang, Y.; Chiang, M. Y. (2002). "Synthesis, characterization and crystal structures of alkyl-, alkynyl-, alkoxo- and halo-magnesium amides". J. Organomet. Chem. 648: 176–187. doi:10.1016/S0022-328X(01)01468-1.
  6. ↑ García–Álvarez, P.; Graham, D. V.; Hevia, E.; Kennedy, A. R.; Klett, J.; Mulvey, R. E.; O'Hara, C. T.; Weatherstone, S. (2008). "Unmasking Representative Structures of TMP-Active Hauser and Turbo-Hauser Bases". Angew. Chem. Int. Ed. 47: 8079–8081. doi:10.1002/anie.200802618.
  7. ↑ Batsanov, A. S.; Bolton, P. D.; Copley, R. C. B.; Davidson, M. G.; Howard, J. A. K.; Lustig, C.; Price, R. D. (1998). "The metallation of imino(triphenyl)phosphorane by ethylmagnesium chloride: The synthesis, isolation and X-ray structure of [Ph3PNMgCl·OP(NMe2)3]2". J. Organomet. Chem. 550: 445–448. doi:10.1016/S0022-328X(97)00550-0.
  8. ↑ Armstrong D. R.; García–Álvarez, P.; Kennedy, A. R.; Mulvey, R. E.; Parkinson, J. A. (2010). "Diisopropylamide and TMP Turbo-Grignard Reagents: A Structural Rationale for their Contrasting Reactivities". Angew. Chem. Int. Ed. 49: 3185–3188. doi:10.1002/anie.201000539.
  9. ↑ Neufeld, R.: DOSY External Calibration Curve Molecular Weight Determination as a Valuable Methodology in Characterizing Reactive Intermediates in Solution. In: eDiss, Georg-August-Universität Göttingen. 2016.
  10. ↑ Neufeld, R.; Stalke, D. (2015). "Accurate Molecular Weight Determination of Small Molecules via DOSY-NMR by Using External Calibration Curves with Normalized Diffusion Coefficients". Chem. Sci. 6: 3354–3364. doi:10.1039/C5SC00670H.
  11. 1 2 Neufeld, R.; Teuteberg, T. L.; Herbst-Irmer, R.; Mata, R. A.; Stalke, D. (2016). "Solution Structures of Hauser Base iPr2NMgCl and Turbo-Hauser Base iPr2NMgCl·LiCl in THF and the Influence of LiCl on the Schlenk-Equilibrium". J. Am. Chem. Soc. 138: 4796–4806. doi:10.1021/jacs.6b00345.
  12. ↑ Eaton, P. E.; Lee, C. H.; Xiong, Y. (1989). "Magnesium amide bases and amido-Grignards. 1. Ortho magnesiation". J. Am. Chem. Soc. 138: 8016–8018. doi:10.1021/ja00202a054.
  13. ↑ Shilai, M.; Kondo, Y.; Sakamoto, T. (2001). "Selective metallation of thiophene and thiazole rings with magnesium amide base". J. Chem. Soc. Perkin Trans. 1: 442–444. doi:10.1039/B007376H.
  14. ↑ Kondo, Y.; Yoshida, A.; Sakamoto, T. (1996). "Magnesiation of indoles with magnesium amide bases". J. Chem. Soc. Perkin Trans. 1: 2331–2332. doi:10.1039/P19960002331.
  15. ↑ http://www.sigmaaldrich.com/chemistry/chemical-synthesis/technology-spotlights/chemetall.html
  16. ↑ Tilly, D.; Chevallier, F.; Mongin, F.; Gros, P. C. (1996). "Bimetallic Combinations for Dehalogenative Metalation Involving Organic Compounds". Chem. Rev. 114: 1207–1257. doi:10.1021/cr400367p.
  17. ↑ Klatt, T.; Markiewicz, J. T.; Sämann, C.; Knochel, P. (2014). "Strategies To Prepare and Use Functionalized Organometallic Reagents". J. Org. Chem. 79: 4253–4269. doi:10.1021/jo500297r.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.