Chin Hin
Leung
a,
Adelina M.
Voutchkova
a,
Robert H.
Crabtree
*a,
David
Balcells
b and
Odile
Eisenstein
*b
aDepartment of Chemistry, Yale University, 225 Prospect Street, New Haven, CT 06520-8017, USA. E-mail: robert.crabtree@yale.edu; Fax: +1 (203) 432 6344; Tel: +1 (203) 432 3925
bInstitut Charles Gerhardt, Université Montpellier 2, CNRS – cc-1501 Place Eugène Bataillon, 34095, Montpellier, France. E-mail: odile.eisenstein@univ-montp2.fr; Fax: +33 467144839; Tel: +33 467143306
First published on 6th June 2007
A mild synthetic route to amides involves imine oxidation to an oxaziridine followed by a transition-metal catalyzed rearrangement to the amide . This route shows potential for a greener pathway to amides . DFT studies showed a possible rearrangement pathway in the case of the Rh catalyst.
(1) |
Although acyl halides and esters can also react directly with amines to form amides , their preparation also generates undesirable waste (eqn (2)).
(2) |
Atom-economic and environmentally more benign synthetic methods are thus highly desirable. One approach involves formation of imine by condensation of aldehyde and amine , oxidation of the imine to the oxaziridine, and subsequent isomerization of the oxaziridine to the amide , catalyzed by transition metal complexes (Scheme 1). This approach was proposed by Duhamal and Plaquevent1 for peptide synthesis but using stoichiometric reagents. Using Mn, W, Ir and Rh catalysts, we now explore the potential of the oxaziridine route for a general synthesis of amides .
Scheme 1 |
Oxaziridines were first synthesized independently in the 1950s by Krimm,2 Emmons3 and Horner and Jurgens.4 Their unusual reactivity pattern is a consequence of the strained three-membered ring and of the weak N–O bond. Oxaziridines are well known as both aminating and oxygenating reagents.5
The principal synthetic routes to oxaziridines involve the oxidation of imines with peracids.6 Other methods to oxidize imines include oxone,7O2/CoCl2 (cat.),8H2O2/benzonitrile9 or H2O2/urea10 and H2O2/Na2WO4 (cat.).11 These alternatives to the harsh peracid methods usually generate stoichiometric amounts of undesirable waste. For example, in the O2/Co(II) system, an aldehyde has to be used as coreductant. The atom economic method of Rao and coworkers,11 using the catalyst Na2WO4 and the green oxidant H2O2,12 goes at room temperature in moderate yield.
Rearrangement of oxaziridines to amides usually requires harsh conditions. Treatment of certain oxaziridines with a strong base such as NaH in HMPA13 or LDA14 gives amides , but can also lead to decomposition.15 Both thermal and photochemical isomerization of oxaziridines are known, but nitrones are sometimes formed instead of amides .16
Oxaziridine rearrangements to amides with transition metal complexes are mostly stoichiometric.17 Apart from an early example by Emmons using FeSO4,3 catalytic oxaziridine rearrangements have been found with iron or manganese porphyrin catalysts with high (10–20%) catalyst loadings.18
While direct oxidation of imines to amides is sometimes possible, this usually requires stoichiometric oxidants such as KMnO419 or mCPBA/BF3.OEt2.20
(3) |
Entry | Catalystb | Loading (mol%) | Solvent | % Yield amide c |
---|---|---|---|---|
a Reaction time 12 h in refluxing solvent. b NHC = 1,3-dimethyl-imidiazole-2-ylidene; cod = 1,5-cyclooctadiene; TPPMnCl = tetraphenylporphyrin chloro manganese(III); L = 4′-phenyl-2,2′:6,2″-terpyridine. c Yields based on 1H NMR integrations using 1,3,5-trimethoxybenzene as internal standard. | ||||
1 | Pd(OAc)2 | 5 | MeCN | 14 |
2 | Pd(PPh3)2Cl2 | 5 | MeCN | 30 |
3 | [Rh(cod)Cl]2 | 2.5 | Toluene | 57 |
4 | [Rh(PPh3)2(cod)]BF4 | 5 | MeCN | 12 |
5 | [Rh(NHC)2(cod)]PF6 | 5 | MeCN | 56 |
6 | [Rh(py)2cod] PF6 | 5 | Toluene | 61 |
7 | Rh2(octanoate)4 | 2.5 | Toluene | 50 |
8 | [IrCp*Cl2]2 | 2.5 | Toluene | 36 |
9 | [Ir(cod)Cl]2 | 2.5 | Toluene | 58 |
10 | [Ir(py)2cod] PF6 | 5 | Toluene | 58 |
11 | TPPMnCl (2) | 5 | MeCN | 83 |
12 | [(L)2Mn2(µ-O)2(H2O)2] (ClO4)3 (3) | 2.5 | MeCN | 74 |
13 | Pd/C | 5 | Toluene | 0 |
14 | Rh/alumina | 5 | Toluene | 0 |
15 | MnO2 | 10 | Toluene | 0 |
Manganese complexes were tested based on the previously reported activity.19 Indeed, the two homogeneous manganese species showed the best activities for the rearrangement step (entries 11 and 12), and exclusion of air was not necessary. Manganese dioxide, on the other hand, was inactive.
The Mn catalyzed rearrangement showed some generality (Table 2) but yields of 2-t-butyl-3-phenyloxaziridine (entry 3) and 2-cyclohexyl-3-(p-nitrophenyl)oxaziridine (entry 7) were poor. TPPMnCl (2) did not catalyze the rearrangement of 2-t-butyl-3-phenyloxaziridine at all, but the sterically less hindered Mn dimer (3) achieved a low yield (36%, entry 3).
Fig. 1 DFT potential energy surface for the Rh-catalyzed rearrangement. Energies are given in kcal mol–1and [Rh] = Rh(cod). |
The coordination of the substrate to [Rh(cod)Cl] leads to the square-planar Rh(I) intermediate I1, with the oxaziridine coordinated to Rh via N. This process is exothermic with a ΔE of –27.9 kcal mol–1. Only potential energy (E) needs to be considered because the oxaziridine rearrangement is a unimolecular process.
TS1 is the transition state for oxidative addition of the oxaziridine. At TS1, O is coplanar with the plane defined by Rh, Cl and cod CC bond mid-points, and the N–O bond is perpendicular to that plane. TS1 is connected to the intermediate I2, on the reactant side of the reaction, and to I3, on the product side. In I2, the oxaziridine is bound to Rh via O and I2 is less stable than I1 by 14.7 kcal mol–1. I3 is a square pyramidal Rh(III) species with a four-membered metallacycle in which N occupies the apical site. The step I1 → TS1 → I3 has a ΔE of +7.9 kcal mol–1 and a ΔE‡ of +28.3 kcal mol–1, indicating that the oxidative addition is relatively slow and moderately endothermic.
It is remarkable that the N–O cleaving step starts from the O-bound complex I2 and not from the more stable N-bound complex I1. This is consistent with the fact that the N–O bond, with a bondlength of 1.486 Å in the free substrate, shortens to 1.477 Å in I1 and lengthens to 1.500 Å in I2. To cleave the N–O bond, Rh needs to transfer electron density into the σ*NO orbital, while avoiding the repulsive interaction from the heteroatom lone pairs. This situation is only obtained when Rh is coplanar with the three-membered ring, which is best achieved by coordination of Rh to the in-plane sp2 lone pair on oxygen.
The metallacycle I3 undergoes β-H elimination through the transition state TS2 leading to the formation of the hydride I4. The Rh–O bond is weakened on going from C–O to CO and the resulting hydride complex (I4) is octahedral, N and Cl being mutually trans. The exothermic and lower energy barrier β-H elimination, with ΔE = –28.4 kcal mol–1and ΔE‡ = +15.9 kcal mol–1, is more favourable than the endothermic and higher energy barrier oxidative addition. β-H elimination may be assisted by the N lone pair, via hyperconjugation of the lone pair into σ*CH and delocalization of the lone pair into the developing π system of the C–O bond.
At the transition state TS3 for the reductive elimination, the apical N bends over the Rh,O,H plane in order to approach the hydride while the Rh–N and Rh–H bonds elongate. TS3 connects to the square-planar intermediate I5 in which the amide is coordinated to Rh via O. At I5, the Rh–N bond is broken and the new N–H bond forms a hydrogen-bond with the Cl.
The I4 → TS3 → I5 step has a ΔE of –44.6 kcal mol–1 and a ΔE‡ of +21.3 kcal mol–1. These values indicate that the N–H reductive elimination is more exothermic than the β-H elimination but involves a moderately higher energy barrier. N–H reductive elimination has been relatively rarely observed.26–28 However, the energy released by the overall reaction (ΔE = –65.1 kcal mol–1) is a driving force for going over moderately high energy barriers.
The final amide decoordination from I5 releases the product and recycles the catalyst. The bond dissociation energy of the amide (+30.3 kcal mol–1) is slightly larger than that of the oxaziridine maybe because of the H-bond between N–H and Cl. However, the bond dissociation energies of the reactant and product are sufficiently similar to keep the catalyst active.
Footnote |
† Electronic supplementary information (ESI) available: Experimental details, computational references, optimized structures with E, H and G. See DOI: 10.1039/b706164a |
This journal is © The Royal Society of Chemistry 2007 |