Alicia Elvira
Cruz-Jiménez‡
a,
Paola Alejandra
Argumedo-Castrejón‡
a,
Jeferson B.
Mateus-Ruiz‡
a,
Victor A.
Lucas-Rosales‡
b,
Octavio Adrián
Valle-González
a,
J. Oscar C.
Jiménez-Halla
b and
J. Armando
Luján-Montelongo
*a
aDepartamento de Química, Centro de Investigación y de Estudios Avanzados (Cinvestav) Av. Instituto Politécnico Nacional 2508 San Pedro Zacatenco, 07360 Ciudad de México, Mexico. E-mail: jalujanm@cinvestav.mx
bDepartamento de Química, División de Ciencias Naturales y Exactas, Sede Noria Alta, Universidad de Guanajuato, Noria Alta s/n, C.P, 36050, Guanajuato, Gto., Mexico
First published on 9th May 2024
We present a novel deoxygenation method for heterocyclic N-oxides utilizing iodide as a catalyst. Iodide acts as a reducing catalyst that is regenerated by formic acid, which also serves as a Brønsted activator and solvent. The method demonstrates high efficiency and excellent selectivity in the reduction of a variety of heterocyclic N-oxides and tertiary amines. Our computational DFT investigation revealed that the reduction mechanism entails a direct interaction between iodide and the oxygen of the N-oxide within a Mg2+/formic acid framework, resulting in the formation of the N-heterocycle and the release of a hypoiodite unit. Additionally, a molecular mechanism for the regeneration of iodide from hypoiodite, facilitated by formic acid, is suggested. This method provides an environmentally friendly approach for the deoxygenation of N-oxides and related species.
Iodine-based deoxygenations of N-functionalities have emerged as alternatives,11,12 particularly since some methods employ green sacrificial reductants.12 In the case of iodide-based methodologies for NODs, iodide is often used as a sacrificial reductant, in stoichiometric or superstoichiometric quantities, and often paired with metals, including TMs.13
The search for cost-effective, efficient, and environmentally friendly methods for the selective reduction of heterocyclic N-oxides is crucial. Formic acid (FA) has emerged as a prominent reducing agent.14 Furthermore, its production from biomass or CO2 valorization adds a sustainable appeal.15 Recently, we introduced the I−/FA as a green reagent for reducing methylsulfinates and sulfoxides (Fig. 1c).16 This method utilizes iodide as the catalytic reductant, which is regenerated by formic acid. Additionally, formic acid serves both as the medium/solvent and in the elaboration of an activating Brønsted template. Under the optimal conditions, we observed exceptional reducing efficiency, coupled with remarkable orthogonality to various reducible functional groups.
Following our research program, which focuses on the development of TM-free16,17 and iodine/iodide-based synthetic methods,16,18 we present a practical method that enables the deoxygenation of pyridine N-oxides (and related species such as N-oxides derived from quinolines, isoquinolines and tertiary amines) using the I−/FA reagent. Our experimentation began exposing quinoline N-oxide (1a) to KI (10% mol) in formic medium, under MW irradiation, delivering 40% yield of quinoline (2a) (entry 1, Table 1). As expected, iodide was essential for the reduction as the absence of KI or its replacement by potassium salts such as K2SO4 and K2HPO4 delivered no reduced product (entries 2–4). Other iodide sources such as TBAI, NaI, KIO3, ZnI2, I2, and MgI2 were also evaluated, with the last two (entries 9 and 10) exhibiting superior performance compared to KI. Although KI, I2 and MgI2 delivered comparable results in terms of yield, MgI2 delivered better reproducibility and chemoselectivity, prompting us to proceed with it for subsequent experiments. We had prior evidence indicating that iodide demonstrated superior performance compared to other halides in similar reductions.16 This was reinforced for the N–O reduction through additional experiments employing magnesium chloride and bromide (entries 16 and 17), delivering low conversion. No contribution from Mg2+ was observed, further supporting the role of iodide as the reducing entity in MgI2 (cf. entries 10 and 11). From tuning of reaction conditions, we identified 10% mol of MgI2 and 3 h of reaction time as optimal (entry 14). An additional experiment conducted with conventional heating underscored the necessity of microwave activation (cf. entries 13 and 18).19,20
Entry | Halide source [I−] | (% mol) | Time (h) | Yield (%)a |
---|---|---|---|---|
a Determined by 1H-NMR. b Isolated yields. c Reaction performed using a conventional heating reactor at 140 °C (Anton-Paar Monowave® 50). | ||||
1 | KI | 10 | 1 | 40 |
2 | — | — | 1 | — |
3 | K2SO4 | 10 | 1 | — |
4 | K2HPO4 | 10 | 1 | — |
5 | TBAI | 10 | 1 | 39 |
6 | NaI | 10 | 1 | 37 |
7 | KIO3 | 10 | 1 | 37 |
8 | ZnI2 | 5 | 1 | 14 |
9 | I2 | 5 | 1 | 42 |
10 | MgI2 | 5 | 1 | 46 |
11 | MgSO4 | 5 | 1 | — |
12 | MgI2 | 5 | 3 | 57 |
13 | MgI2 | 10 | 1 | 47 |
14 | MgI 2 | 10 | 3 | 91/91 |
15 | MgI2 | 10 | 4 | 95/85b |
16 | MgCl2 | 10 | 3 | 2 |
17 | MgBr2 | 10 | 3 | 2 |
18c | MgI2 | 10 | 3 | 65/49b |
With the optimal conditions at hand, diverse N-oxides with varying substituents were submitted to the optimal deoxygenation conditions. Isoquinoline, benzo[h]quinoline, and phenazine N-oxides (1b–1d) were successfully deoxygenated with comparable yields to those obtained using TM-based technologies (Table 2).9
Interestingly, sterically hindered 2,6-methylated pyridine N-oxides (1e, 1f) underwent deoxygenation without any detrimental effects, yielding the corresponding pyridines with excellent yields. Furthermore, complete orthogonality was observed for carbonyl-containing N-oxides, such as 4-acetylpyridine N-oxide (1h) and 4-benzoylpyridine N-oxide (1i). These results significantly support a wider range of conditions under which the I−/FA reductive reagent is effective (90–140 °C), without affecting carbonyl groups.21 Additionally, a cyano-substituted substrate (1j) and 6-MeO-quinoline N-oxide (1m) underwent chemoselective N-deoxygenation, producing the corresponding heterocycles with excellent yields.
Under standard conditions, 3-nitroquinoline N-oxide (1k) underwent reduction of both the N-oxide and nitro groups, accompanied by formylation to yield product 2ka. In contrast, 2-aminopyridine N-oxide (1g) was deoxygenated with excellent yield and without formylation, a result attributed to the significant electronic differences between positions 2 and 3 on the pyridine ring.22 After adjusting the reaction conditions, 2k was successfully obtained with the nitro group remaining unaffected (see ESI†). As for 4-nitroquinoline N-oxide (1l), a Nef-type hydrolytic removal of the nitro group was impossible to avoid, delivering quinolin-4-(H)-one (2l) as the sole product.23 All attempts to adjust the conditions to obtain the nitro-containing deoxygenated product were unsuccessful (see ESI†). Finally, N-oxides of tertiary amines such as 1n and 1o were obtained with particularly good yields. Importantly, in all successful experimental trials, the reactor vial was pressurized during the reaction process and maintained a high pressure (>10 psi) after cooling to room temperature, which is consistent with the release of CO2 as byproduct.24 Upon completion of the reductions, the reaction mixtures typically developed a brownish hue, indicative of the presence of molecular iodine.
To get insight in the reaction mechanism for the N–O reduction, we performed DFT calculations (see ESI,† for further details) employing pyridine N-oxide as a model and considering the optimal conditions above discussed. First, we explored the interaction between MgI2 and solvent molecules (Fig. 2). In a recent previous work, we demonstrated that the coordination modes of the Mg metal center vary based on the σ-donor capability of the Lewis base.25 Consequently, FA acts as a ligand and magnesium can coordinate up to four units, through the carbonyl O atom, resulting in Mg–O–C angles of approximately 120°. Contrary to what one might expect, FA-ligands are monodentate and not bidentate. The formation of the lower coordination modes A-1 and A-2 is spontaneous, while the penta- and hexa-coordinated species, A-3 and A-4, corresponding to sp3d and sp3d2 hybridizations at the Mg center, exist in equilibrium with the tetrahedral A-2 mode. The NOD mechanistic pathway and the subsequent iodide regeneration begins with a double substitution of iodide for two FA-ligands within the Mg coordination sphere (A-4 → I-1 → I-2, Fig. 3). The formation of the [Mg2+(OCHOH)6]2I− complex (I-2) requires ΔGA-4 → I−2 = +4.2 kcal mol−1. Subsequently, the spontaneous addition of a pyridine N-oxide (C5H5NO) unit forms I-3 (ΔGI-2 → I-3 = −4.5 kcal mol−1). This addition is deemed favorable due to the hydrogen bonding between the oxygen in pyridine N-oxide and protons from formic acid units. Despite the pKa values of pyridine N-oxide (0.79)26 and formic acid (3.5)27 suggesting that proton transfer (PT) between these Brønsted species might not be favored, our findings show that this process is both barrierless and exergonic (ΔGI-3 → I-4 = −3.5 kcal mol−1). Thus, it seems that an effect of increased acidity of FA protons, through Mg-FA coordination, facilitates the PT process to access I-4 effortlessly. Next, a nucleophilic substitution (SN2-type) takes place, centered on the oxygen atom viaTS-1 (ΔG‡I-4 → TS-1 = +32.5 kcal mol−1, in agreement with T = 140 °C), marking the rate-determining step and resulting in the formation of the pyridine-hypoiodous acid pair in I-5. Remarkably, formic acid acts as a Brønsted-activator enabling the electrophilicity of the pyridine N-oxide, so the nucleophilic attack of iodide is feasible. From I-5, a hydrogen transfer process was determined viaTS-2A, with an energy barrier of ΔG‡I-5 → TS-2A = +20.1 kcal mol−1, leading to the production of hydroiodic acid and carbon dioxide (P-A) through a net exothermic process. Then, hydroiodic acid spontaneously transfers its proton to the pyridine supported by a H2O unit.
Fig. 2 Relative Gibbs free energy (kcal mol−1) profile for the progressive coordination of formic acid ligands to MgI2 at the (SMD:HCO2H)ωB97X-D/def2-TZVPP//ωB97X-D/def2-SVP level and 298.15 K. |
We identified an equilibrium between I-5 and a formyl hypoiodite species (I-6, ΔGI-5 → I-6 = −1.9 kcal mol−1). Finding a transition state connecting these minima proved to be difficult. Starting from I-6, I-5 can also lead to the formation of molecular iodine (I2, P-B) through iodide addition, with an energy barrier of ΔG‡I-6 → TS-2B = +9.6 kcal mol−1. These equilibria towards non-iodide productive species determines the molar percentage required for the iodide reactant, as amounts of MgI2 lower than standard significantly affect the conversion rate (cf. entries 12,14, Table 1). However, our thermochemical data suggest that iodine (P-B) can be converted into P-A by accessing I-5 and then proceeding through TS-2A, requiring an energy investment of ΔG‡P-B → TS-2A = +33.1 kcal mol−1.
Footnotes |
† Electronic supplementary information (ESI) available: Cartesian coordinates of the calculated reaction mechanism. See DOI: https://doi.org/10.1039/d4nj00913d |
‡ Contributed equally. |
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