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Article

New Oxidovanadium(IV) Complexes with 2,2′-bipyridine and 1,10-phenathroline Ligands: Synthesis, Structure and High Catalytic Activity in Oxidations of Alkanes and Alcohols with Peroxides

by
Iakov S. Fomenko
1,
Artem L. Gushchin
1,2,*,
Pavel A. Abramov
1,2,
Maksim N. Sokolov
1,2,
Lidia S. Shul'pina
3,
Nikolay S. Ikonnikov
3,
Maxim L. Kuznetsov
4,
Armando J. L. Pombeiro
4,
Yuriy N. Kozlov
5,6 and
Georgiy B. Shul’pin
5,6,7,*
1
Nikolaev Institute of Inorganic Chemistry, Siberian Branch of Russian Academy of Sciences, Prospekt Acad. Lavrentieva, dom 3, 630090 Novosibirsk, Russia
2
Novosibirsk State University, ul. Pirogova, dom 2, 630090 Novosibirsk, Russia
3
Nesmeyanov Institute of Organoelement Compounds, Russian Academy of Sciences, ul. Vavilova, dom 28, 119991 Moscow, Russia
4
Centro de Química Estrutural, Instituto Superior Técnico, Universidade de Lisboa, Avenida Rovisco Pais, 1049-001 Lisboa, Portugal
5
Semenov Institute of Chemical Physics, Department of Dynamics of Chemical and Biological Processes, Russian Academy of Sciences, ul. Kosygina, dom 4, 119991 Moscow, Russia
6
Chair of Chemistry and Physics, Plekhanov Russian University of Economics, Stremyannyi pereulok, dom 36, 117997 Moscow, Russia
7
RussiaPeople’s Friendship University of Russia, ul. Miklukho-Maklaya, dom 6, 117198 Moscow, Russia
*
Authors to whom correspondence should be addressed.
Catalysts 2019, 9(3), 217; https://doi.org/10.3390/catal9030217
Submission received: 24 January 2019 / Revised: 4 February 2019 / Accepted: 9 February 2019 / Published: 26 February 2019
(This article belongs to the Section Catalysis in Organic and Polymer Chemistry)
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Versions Notes

Abstract

:
Reactions of [VCl3(thf)3] or VBr3 with 2,2′-bipyridine (bpy) or 1,10-phenanthroline (phen) in a 1:1 molar ratio in air under solventothermal conditions has afforded polymeric oxidovanadium(IV) four complexes 1–4 of a general formula [VO(L)X2]n (L = bpy, phen and X = Cl, Br). Monomeric complex [VO(DMF)(phen)Br2] (4a) has been obtained by the treatment of compound 4 with DMF. The complexes were characterized by IR spectroscopy and elemental analysis. The crystal structures of 3 and 4a were determined by an X-ray diffraction (XRD) analysis. The {VOBr2(bpy)} fragments in 3 form infinite chains due to the V = O…V interactions. The vanadium atom has a distorted octahedral coordination environment. Complexes 1–4 have been tested as catalysts in the homogeneous oxidation of alkanes (to produce corresponding alkyl hydroperoxides which can be easily reduced to alcohols by PPh3) and alcohols (to corresponding ketones) with H2O2 or tert-butyl hydroperoxide in MeCN. Compound 1 exhibited the highest activity. The mechanism of alkane oxidation was established using experimental selectivity and kinetic data and theoretical DFT calculations. The mechanism is of the Fenton type involving the generation of HO• radicals.

1. Introduction

Many organic reactions catalyzed by metal complexes have been reported in the recent years. Organic and inorganic peroxides and especially hydrogen peroxide are widely employed for the oxidation of various organic compounds. Alkanes are also among these organic substrates, although saturated hydrocarbons exhibit very high inertness in reactions in solutions under mild conditions [1,2,3,4,5,6,7,8].
The reactions of alkanes (as well as alcohols containing C–H bonds) occur with the intermediate formation of free O- and C-centered radicals. The latter easily reacts with molecular oxygen if the reaction is carried out in air. Finally, less stable (alkyl hydroperoxides) or stable (ketones) derivatives are produced [9,10]. The typical role of a metal complex in such transformations is to generate active radicals that attack C–H bonds as well as to participate in various redox processes leading, finally, to the formation of stable products. Metal complexes with redox-active ligands have attracted considerable interest for use in the multi-electron activation of small molecules and in redox-based catalytic reactions [11,12,13,14,15,16,17].
Redox-active ligands have more energetically accessible levels for reduction or oxidation. As a result, either exclusively ligand-centered redox processes can occur, with the metal center remaining in the same oxidation state, or both the ligand and metal change their oxidation state in a synergistic fashion, creating ambiguity about the electronic state of both the metal and ligand.
Various vanadium derivatives are known to catalyze the oxidations of organic compounds with inorganic and organic peroxides (see reviews [18,19] and original papers [20,21,22]). Most oxidovanadium(IV) complexes have monomeric structures with an octahedral or square-pyramidal coordination geometry of vanadium [23,24,25,26,27,28,29,30,31,32]. Polynuclear linear chain structures ({V = O…V = O…}), where vanadium is coordinated by a terminal oxygen atom (V = O) of an adjacent molecule to complete the octahedral geometry, are much less common. Most of them belong to oxidovanadium(IV) complexes with tetradentate Schiff base ligands [33,34,35,36,37,38,39].
In 1993, Shul’pin and coworkers discovered a highly efficient system for the oxidation of hydrocarbons consisting of the combination of a vanadate anion and pyrazine-2-carboxylic acid [40,41]. Later, this system, which catalyzes the transformation of alkanes into corresponding alkyl hydroperoxides with hydrogen peroxide in an acetonitrile solution, was investigated in detail [42,43,44,45,46,47,48,49,50,51,52,53,54,55,56,57,58,59,60,61,62]. Very recently, we have reported the synthesis of monomeric square-pyramidal oxidovanadium(IV) complex ([VOCl2(dpp-bian)]) with the redox-active bis[N-(2,6-diisopropylphenyl)imino]acenaphthene ligand (dpp-bian). The complex demonstrated a high catalytic activity towards alkane oxygenation by H2O2 under mild conditions [63]. Expanding that work, herein, we carried out reactions of [VCl3(thf)3] or VBr3 with heterocyclic diimines such as 2,2′-bipyridine and 1,10-phenanthroline to yield polymeric oxidovanadium(IV) complexes [VO(L)X2]n (L = bpy, phen and X = Cl, Br) and studied their catalytic properties in alkane and alcohol oxidation reactions with peroxides.

2. Results and Discussion

2.1. Synthesis and Characterization of Compounds 1–4a

Solventothermal conditions were applied for the synthesis of oxidovanadium(IV) complexes 1–4a. Vanadium trichloride adduct with tetrahydrofuran ([VCl3(thf)3]) and vanadium tribromide (VBr3) were used as starting compounds which were oxidized during the reaction in air to give the V = O moiety (Scheme 1). This synthetic procedure was previously applied for the synthesis of other oxidovanadium(IV) complexes with chiral dehydrophenanthroline and diazofluorene ligands as well as with the redox-active bis(N-(2,6-diisopropylphenyl)imino)acenaphthene (dpp-bian) ligand [25,63]. The reactions of the corresponding vanadium precursor and 2,2′-bipyridine (bpy) or 1,10-phenanthroline (phen) in a 1:1 molar ratio resulted in microcrystalline products in yields ranging from moderate to high.
The IR spectra of the complexes 1–4a show a strong V = O stretching band around 880–890 cm−1 which is typical for linear chain V = O…V = O polymeric structures [34,35,36,37,38,39] This band is significantly blue-shifted in the IR spectra of monomeric oxidovanadium complexes [63,64,65,66]. A ferromagnetic intermolecular interaction between the molecules in the chains of polymeric oxidovanadium(IV) complexes with tetradentate Schiff base ligands have been found [39].

2.2. Crystal Structures of 3 and 4a

Of the five products, 1, 2, 3, 4 and 4a, only the green crystals of 3 and 4a obtained directly from the reaction mixture were of sufficient quality for X-ray diffraction (Table 1). Compound 3 forms a 1D-polymeric structure (Figure 1). The relevant bond distances are listed in Table 2. Vanadium is octahedrally coordinated by two nitrogen atoms of the chelating bpy ligand, as well as by two bromine atoms that lie in the plane of the bpy ligand and the oxygen atom from the vanadyl group, which is located perpendicular to the plane. The distorted octahedral environment is completed by the oxygen atom of the vanadyl group of the neighboring {VOBr2(bpy)} fragment. Thus, the {VOBr2(bpy)} fragments in 3 form infinite chains due to the V = O…V interactions (Figure 2). Based on the data of IR spectroscopy, we assume a similar structure for the remaining compounds (1, 2 and 4).
The V = O distance (1.617(5) Å) is longer and the V…O distance (2.123(5)–2.125(5) Å) is shorter than those of the polymeric [VO(5-NO2sal-meso-stien)] (1.599(3) and 2.437(3) Å, respectively) [39] and [VO{3-EtOsal-(R,R)-2,4-ptn}] (1.617(6) and 2.290(6) Å, respectively) [67] complexes with tetradentate Schiff base ligands.
Polymeric compounds 1–4 are insoluble in non-coordinating solvents and soluble in coordinating solvents such as DMF with the breaking up of the polymeric {V = O…V = O…} structure and the excision of monomeric links. Single crystals of [VO(DMF)(phen)Br2] (4a) were obtained by the treatment of 4 with DMF. An X-ray analysis of 4a shows a monomeric structure with an octahedral coordination environment around vanadium, completed with a coordinated DMF molecule (Figure 3). The main geometric parameters of 4a are summarized in Table 2.

2.3. Oxidation of Alkanes with Peroxides Catalyzed by Complexes 1–4

Systems based on metal complexes are known to catalyze hydrocarbon and alcohol oxygenations, i.e., replacing H atoms by oxygen. The chloride complexes 1 and 2 prepared in this work exhibited a high catalytic activity in the oxidation of alkanes with H2O2 in an acetonitrile solution. Thus, stirring at 20 °C a solution of 2 (5 × 10–4 M), cyclohexane (0.46 M), H2O2 (aqueous, 2 M) after 150 h gave 0.011 M of cyclohexanone and 0.041 M of cyclohexanol (analysis after the reduction of the solution with PPh3). An analogous reaction catalyzed by complex 1 (5 × 10–4 M) afforded cyclohexanone (0.015 M) and cyclohexanol (0.12 M). At a higher temperature (40 °C), the reactions proceeded faster: After 6 h, yields of cyclohexanone and cyclohexanol were 0.01 M and 0.112 M, respectively, in the case of catalyst 2. Complex 1 turned out to be more efficient, affording 0.02 M and 0.16 M of cyclohexanone and cyclohexanol, respectively, after the reduction of the solution with PPh3 (compare Figure 4 and Figure 5). This activity is comparable with that found by us previously for the other vanadium complexes in the alkane oxidations with peroxides [40,41,42,43,44,45,46,47,48,49,50,51,52,53,54,55,56,57,58,59,60,61,62,63].
The oxidation reactions catalyzed by compound 1 have been studied in more detail. Figure 4 clearly demonstrates that the reduction of the reaction solution with PPh3 gives rise to a higher concentration of cyclohexanol and a decrease of cyclohexanone concentration (compare Graphs A and B). These changes indicate (the so-called Shul’pin method [68,69,70,71,72,73,74,75,76,77,78,79,80,81,82]) that alkyl hydroperoxide is formed in the course of the oxidation. For the transfomations of cyclohexane, see a Scheme in Figure 4A.
The dependence of the initial oxidation rate W0 on the initial concentration of catalyst 1 is shown in Figure 6. The curve of dependence of the initial oxidation rate in the case of catalysis by complex 1 is approaching a plateau at a cyclohexane concentration of >0.46 M (Figure 7). The rate at [CyH]0 ≈ 0.2 M is approximately equal to half of the maximum rate.
The competitive oxidation of cyclohexane and acetonitrile (solvent) in the presence of complex 1 is demonstrated in Figure 7. The dependence of the oxidation rate in the case of catalyst 1 (Figure 8) is in a good agreement with the Arrhenius Equation (Ea = 20 ± 2 kcal/mol) and with the value calculated in accordance with the model shown below in Scheme 2 (ΔH’ = 19.6 kcal/mol). The proposed model is also in agreement with the experimental data: In both cases, the first order of the oxidation relative catalyst concentration was found (see Figure 6).
The bromide complexes 3 and 4 also catalyze the cyclohexane oxidation with H2O2; the corresponding kinetic curves of the product accumulation are presented in Figure 9. The dependence of the initial oxidation rate in the reaction catalyzed by complex 3 exhibits an approach to a plateau (see an analogous dependence in Figure 7).
The experiments shown in Figure 4 and Figure 5 indicate that the catalytic activity of complex 2 is practically equal to that of compound 1 (W0 1.1 × 10−5 and 1.0 × 10−5 M s−1, respectively). The activities of complexes 3 and 4 are a bit lower (W0 2.8 × 10−6 and 4.2 × 10−6 M s−1, respectively).
Compound 2 catalyzes the oxidation of cyclohexene (0.4 M) with H2O2 (0.32 mL) at 40 °C to afford, after 1 h, cyclohex-2-ene-1-ol (0.053 M) and cyclohex-2-one-1 (0.01 M). Cyclohexanol (0.5 M) was oxidized by tert-butyl hydroperoxide at 50 °C to produce cyclohexanone (0.23 M) after 4 h.
We determined the selectivity parameters for the oxidation of certain alkanes (n-heptane, methylcyclohexane and cis-1,2-dimethylcyclohexane catalyzed by complexes 1–4 (Table 3). The oxygenation of cis-1,2-dimethylcyclohexane with H2O2 catalysed by complex 3 gave corresponding isomeric tertiary alcohols in a trans/cis ratio of 0.8. These data as well as the character of dependence of the initial cyclohexane oxidation rate on the initial hydrocarbon concentration (approaching a plateau at [cyclohexane]0 > 0.3 M) indicate that the reaction occurs with the participation of hydroxyl radicals and that alkyl hydroperoxides are formed as the main primary products.
We can assume that the alkane oxidation is induced with an intermediate species generated in the catalytic decomposition of hydrogen peroxide. The dependence of the rate of cyclohexyl hydroperoxide (ROOH) formation on the initial concentration of cyclohexane (RH, see Figure 7 above) indicates a competition between cyclohexane and acetonitrile for the catalytically active species. The selectivity parameters measured in the oxidation of linear and branched alkanes (Table 3) are close to the parameters typical for the reactions of alkanes with hydroxyl radicals [83,84]. Taking this fact into account, we can consider the simplest scheme of the concurrent oxidation:
H2O2 + Cat →HO• Wi
HO• + RH→R• →→ROOH k1
HO• + CH3CN→→products k2
Here, Wi is the rate of generation of hydroxyl radicals, formed in the process of catalytic H2O2 decomposition; (1) and (2) are the transformations of RH into ROOH and CH3CN into products and where the rate limiting steps are the interactions of HO• with RH (k1) and with CH3CN (k2).
Assuming that the concentration of hydroxyl radicals is quasi-stationary during the reaction, we can obtain the term for the initial rate of ROOH formation:
(d[ROOH]/dt)0 = Wi/(1+k2[CH3CN]/k1[RH])
In order to analyze the experimental data shown in Figure 7, let us transform Equation (3) into Equation (4):
[RH]/(d[ROOH/dt)0 = ((k2/k1)[CH3CN] + [RH])(1/Wi)
The linear anamorphosis in coordinates
[RH]/(d[ROOH/dt)0 - [RH]
of the experimental dependence shown in Figure 7A is presented in Figure 7B. The analysis of this dependence leads to conclusions that: 1) the experimental data of Figure 7 satisfy the proposed model {Wi, 1, 2}; 2) the segment cut on the y-axis
(1/Wi)(k2/k1)[CH3CN] = 0.014.106 s
and 3) the tangent of the slope
(1/Wi) = 0.128.106 M-1 s
Thus, for the conditions shown in Figure 7, the experimental parameters are Wi = 8.10−6 M s−1 and k2[CH3CN]/k1 = 0.11 M. The latter ratio of rate constants is equal to the value obtained by some of us earlier for other hydroxyl radical generating systems [83,84].

2.4. Theoretical Mechanistic Study

With the aim to shed light on the mechanism of alkane oxidation with H2O2 catalyzed by the V(IV) complexes under study, DFT calculations have been performed for the monomeric form of 1 as a catalyst. In accordance with the experimental kinetic and selectivity data discussed above, the global reaction mechanism is radical one, involving the generation of the HO• species which then oxidize the alkane molecules R–H to give, upon the hydrogen abstraction, the corresponding alkyl radicals R• (Scheme 3). The latter react with molecular oxygen, producing the alkylperoxo radicals ROO• and then the corresponding alkyl hydroperoxide ROOH experimentally detected by GC. In accordance with the kinetic studies, the rate limiting step of the whole process is the generation of the HO• radicals.
The experimental data demonstrate that the polymeric pre-catalyst 1 is not stable in a DMF solution, transforming to the mononuclear species, presumably [V(=O)(bpy)(DMF)Cl2]. Similarly, the easy solvolysis of 1 in acetonitrile or aqueous solutions is expected to give [V(=O)(bpy)(N≡CMe)Cl2] (Ia) or [V(=O)(bpy)(H2O)Cl2] (Ib), respectively. Indeed, the calculations indicate that the transformations of 1 into Ia or Ib are exergonic by 5.2 or 2.0 kcal/mol, correspondingly. The structures of four possible geometric isomers of Ib were calculated (Figure 10), and the most stable isomer is that with two chloride ligands being in the trans-position.
In the presence of hydrogen peroxide, the acetonitrile or water ligands in I can be replaced for H2O2 to give [V(=O)(bpy)(H2O2)Cl2] (II) (Scheme 2). Such a substitution is endergonic by 8.1–9.7 kcal/mol. The coordination of H2O2 to the V(IV) center tremendously activates this molecule towards the O–O homolysis. Indeed, the energy of the homolytic O–O bond cleavage in II leading to III and HO• is −9.7 kcal/mol, indicating that this process is exergonic. Meanwhile, the activation barrier for the HO• generation from II via TS1 is 11.8 kcal/mol (see Supplementary Materials). The overall activation barrier of the HO• formation relative to the most stable complex Ia is 21.5 kcal/mol in terms of ΔG≠ and 19.6 kcal/mol in terms of ΔH≠. The latter value is in a good agreement with the experimentally obtained activation energy for this reaction catalyzed by complex 1 (20 ± 2 kcal/mol, see above Figure 8).
In principle, the formation of the alkyl radicals R• could occur in one step directly from II via TS2. This transition state should correspond to the simultaneous O–O and C–H bond cleavages and the O–H bond formation. However, all attempts to locate TS2 failed, leading to TS1 and C6H12 situating at the second coordination sphere.
Another plausible pathway of the HO• generation includes the preliminary proton transfer in II from the coordinated H2O2 to the oxo ligand to give complex [V(OH)(bpy)(OOH)Cl2] (IV). The following homolytic O–OH bond cleavage in the hydroperoxo ligand produces HO• and III. Two possible transition states for the proton transfer were found, i.e., the 4-membered cyclic TS3 and the 6-membered cyclic TS4, with H2O molecule playing the role of a proton shuttle. However, the calculated activation energy for such an H-transfer is too high for both these TSs (45.3 and 32.2 kcal/mol, respectively, relative to Ia). Thus, the calculations indicate that the simple Fenton mechanism is operating for the catalyst 1.

3. Experimental Section

3.1. Computational Details

The full geometry optimization of all structures and transition states (TSs) has been carried out at the DFT level of theory by using the M06 functional [85] with the help of the Gaussian 09 program package [86]. No symmetry operations were applied. The geometry optimization was carried out by using a relativistic Stuttgart pseudopotential which describes 10 core electron (MDF10) and the appropriate contracted basis set (8s7p6d1f)/[6s5p3d1f] [87] for the vanadium atom and the 6-311+G** basis set for other atoms. This level of theory was successfully applied recently for the analysis of mechanisms of the V-catalyzed oxidation of alkanes with peroxides [88].
The Hessian matrix was calculated analytically for the optimized structures to prove the location of correct minima (no imaginary frequencies) or saddle points (only one imaginary frequency) and to estimate the thermodynamic parameters, with the latter calculated at 25 °C. The nature of all transition states was investigated by analysis of the vectors associated with the imaginary frequency and by the calculations of the intrinsic reaction coordinates (IRC) by using the method developed by Gonzalez and Schlegel [89,90,91].
The total energies corrected for solvent effects Es were estimated at the single-point calculations on the basis of gas-phase geometries using the polarizable continuum model in the CPCM version [92,93] with CH3CN as solvent. The UAKS model was applied for the molecular cavity, and dispersion, cavitation and repulsion terms were taken into account. The entropic term in CH3CN solution (Ss) was calculated according to the procedure described by Wertz [94] and Cooper and Ziegler [95] using Equations (5)–(6):
ΔS1 = R ln(Vsm,liq/Vm,gas)
ΔS2 = R ln(V°m/Vsm,liq)
α = [S°,sliq – (S°,sgas + ΔS1)]/[S°,sgas + ΔS1]
Ss = Sg + ΔSsol = Sg + [ΔS1 + α(Sg + ΔS1) + ΔS2] =
Sg + [(–12.21 cal/mol•K) – 0.23(Sg – 12.21 cal/mol•K) + 5.87 cal/mol•K]
where Sg is the gas-phase entropy of solute, ΔSsol is the solvation entropy, So,sliq, So,sgas and Vsm,liq are the standard entropies and molar volume of the solvent in the liquid or gas phases (149.62 and 245.48 J/mol•K and 52.16 mL/mol, respectively, for CH3CN), Vm,gas is the molar volume of the ideal gas at 25 °C (24450 mL/mol), Vom is the molar volume of the solution that correspond to the standard conditions (1000 mL/mol). The enthalpies and Gibbs free energies in solution (Hs and Gs, respectively) were estimated using the expressions 9 and 10
Hs = Es – Eg + Hg
Gs = Hs – TSs
where Es and Eg are the total energies in solution and the gas phase and Hg is the gas-phase enthalpy. Gibbs free energies in solution are discussed in this work if not stated otherwise.

3.2. Materials

All manipulations were carried out in air. Vanadium tribromide (VBr3) was synthesized from elements as described in Reference [96]. The other reagent-grade chemicals were obtained from Aldrich and used without further purification. All solvents were distilled by standard methods before use.

3.3. Physical Measurements

An elemental analysis was performed on a Euro EA 3000 CHN elemental analyzer. The IR spectra (4000–400 cm−1) were recorded on a Scimitar FTS 2000 Fourier-spectrometer.

3.4. X-ray Crystallography

The crystallographic data and refinement details for 3 and 4a are given in Table 1. The diffraction data were collected on New Xcalibur (Agilent Technologies, Santa Clara, CA, United States) and Bruker Apex Duo diffractometers with MoKα radiation (λ = 0.71073). An absorption correction was done empirically using SCALE3 ABSPACK (CrysAlisPro, Agilent Technologies, Version 1.171.37.35 (release 13-08-2014 CrysAlis171 NET)) and SADABS (Bruker-AXS, 2004). The structures were solved by a dual algorithm [97] and refined by a full-matrix least-squares treatment against |F|2 in anisotropic approximation with SHELX 2017/1 [98] in the ShelXle program [99]. The hydrogen atoms were refined in geometrically calculated positions. The main geometrical parameters are summarized in Table 2. The crystallographic data have been deposed in the Cambridge Crystallographic Data Centre under the deposition codes CCDC 1879273 (3) and 1879274 (4a).

4. Conclusions

New polymeric oxidovanadium(IV) complexes, [VO(L)X2]n (L = bpy, phen and X = Cl, Br), have been synthesized and structurally characterized. The experimental kinetic and selectivity data and DFT calculations indicated that the simple Fenton mechanism is operating for the oxidation of alkanes catalyzed by the V(IV) complexes under study. This mechanism includes (i) the formation of the monomeric active catalytic forms [VO(L)X2(Solv)] (Solv = H2O, CH3CN), (ii) the substitution of the coordinated solvent for the H2O2 molecule, (iii) the generation of the HO• radical upon the HO–OH bond cleavage and (iv) the oxidation of the alkane molecules by HO• via hydrogen abstraction followed by the reaction with molecular oxygen to give alkyle hydroperoxides.

5. Syntheses of the Complexes

5.1. Synthesis of [VIVO(bpy)Cl2]n (1)

A mixture of [VCl3(thf)3] (100 mg, 268 µmol), 2,2′-bipyridine (42 mg, 268 µmol) and CH3CN (5 mL) was heated at 100 °C in a sealed Teflon container for 30 h. The slow cooling to room temperature gave needle-like crystals of 1 which were separated by filtration, washed with CH3CN and Et2O and dried in a vacuum. Yield: 71 mg (90%). Anal. Calc. for C10H8Cl2N2OV: C, 40.8%; N, 9.5%; and H, 2.7%. Found: C, 40.5%; N, 9.4%; and H, 2.8%. IR (KBr) ν/cm−1: 3113(w), 3077(w), 3053(w), 3038(w), 2001(vw), 1971(vw), 1942(vw), 1898(vw), 1867(vw), 1670(vw), 1643(vw), 1605(s), 1567(w), 1498(w), 1474(m), 1446(s), 1321(m), 1246(w), 1169(m), 1117(w), 1076(w), 1059(w), 1043(w), 973(w), 1031(m), 889(vs), 766(s), 729(s), 663(w), 653(w), 644(w), 451(w) and 414(w).

5.2. Synthesis of [VIVO(phen)Cl2]n (2)

The synthesis of 2 was carried out under the same conditions as described for 1 using [VCl3(thf)3] (100 mg, 268 µmol) and 1,10-phenanthroline (48 mg, 268 µmol). A green microcrystalline product was obtained. Yield: 57 mg (65%). Anal. Calc. for C12H8Cl2N2OV: C, 45.3%; N, 8.8%; and H, 2.5%. Found: C, 45.1%; N, 9.0%; and H, 2.7%. IR (KBr) ν/cm−1: 3080(w), 3053(br.w), 3010(w), 1629(w), 1607(w), 1584(m), 1521(s), 1495(w), 1428(vs), 1346(w), 1304(w), 1225(w), 1209(w), 1148(m), 1109(m), 891(bvs), 875(vs), 847(vs), 782(w), 739(m), 723(vs), 654(m), 559(w), 507(w) and 435(m).

5.3. Synthesis of [VIVO(bpy)Br2]n (3)

A mixture of VBr3 (150 mg, 516 µmol), 2,2′-bipyridine (81 mg, 516 µmol) and CH3CN (10 mL) was heated at 100 °C in a sealed Teflon container for 12 h. The slow cooling to room temperature gave a mixture of green crystals (major) and an orange powder (minor). The mixture was washed with CH3CN and Et2O and dried in a vacuum. The green crystals were mechanically separated from the orange powder. Yield: 124 mg (66%) Anal. Calc. for C10H8Br2N2OV: C, 31.4%; N, 7.3%; and H, 2.1%. Found: C, 31.1%; N, 7.1%; and H, 2.3%. IR (KBr) ν/cm−1: 3112(w), 3093(w), 3074(w), 3059(w), 3035(w), 2917(w), 2850(w), 1601(s), 1566(w), 1494(w), 1471(m), 1440(s), 1319(m), 1310(m), 1243(w), 1216(w), 1167(m), 1114(w), 1102(w), 1061(w), 1044(w), 1029(s), 1021(m), 875(vs), 769(s), 727(s), 661(m), 650(w), 643(w), 447(w) and 413(w).

5.4. Synthesis of [VIVO(phen)Br2]n (4)

The synthesis of 4 was carried out under the same conditions as described for 3 using VBr3 (150 mg, 516 µmol) and 1,10-phenanthroline (93 mg, 516 µmol). A green microcrystalline product was obtained. Yield: 124 mg (43%). Anal. Calc. for C12H8Br2N2OV: C, 35.4%; N, 6.9%; and H, 2.0%. Found: C, 34.9%; N, 7.0%; and H, 2.3%. IR (KBr) ν/cm−1: 3078(w), 3051(w), 3011(w), 1734(w), 1629(m), 1607(m), 1584(m), 1521(m), 1495(w), 1466(w), 1428(s), 1345(w), 1304(w), 1225(w), 1210(w), 1149(m), 1109(m), 978(w), 882(vs), 846(m), 779(w), 739(m), 721(s), 654(w), 509(w) and 434(m).

5.5. Oxidation of Alcohols and Hydrocarbons with Peroxides

The reactions of alcohols and hydrocarbons were usually carried out in air in thermostated Pyrex cylindrical vessels with vigorous stirring, using MeCN as the solvent. Typically, the catalyst (1–4) and the cocatalyst (acid) were introduced into the reaction mixture in the form of stock solutions in acetonitrile. The substrate (alcohol or hydrocarbon) was then added, and the reaction started when hydrogen peroxide or TBHP was introduced in one portion. (CAUTION: The combination of air or molecular oxygen and H2O2 with organic compounds at elevated temperatures may be explosive). The reactions with benzene and 1-phenyethanol were analyzed by the 1H NMR method (solutions in acetone-d6; “Bruker AMX-400” instrument, 400 MHz). For the determination of the concentrations of phenol and p-quinone, the signals in the aromatic region were integrated using added 1,4-dinitrobenzene as a standard. The areas of methyl group signals were measured to quantify the oxygenates formed in the oxidations of 1-phenylethanol.
In order to determine the concentrations of all the cyclohexane oxidation products, the samples of the reaction solutions after the addition of nitromethane as a standard compound were, in some cases, analyzed twice (before and after their treatment with PPh3) by GC (chromatograph-3700, fused silica capillary column FFAP/OV-101 20/80 w/w, 30 m × 0.2 mm × 0.3 µm; helium as a carrier gas) to measure the concentrations of cyclohexanol and cyclohexanone. This method (an excess of solid triphenylphosphine was added to the samples 10–15 min before the GC analysis) was proposed by one of us (Shul’pin, G.B.) earlier [4,5,46,47,68,69,70,71,72,73,74,75,76,77,78,79,80,81,82]. The attribution of peaks was made by a comparison with the chromatograms of authentic samples. Blank experiments with cyclohexane showed that, in the absence of the catalyst, no products were formed.

Supplementary Materials

The following are available online at https://www.mdpi.com/2073-4344/9/3/217/s1.

Author Contributions

A.L.G. and G.B.S. conceived and designed the experiments; I.S.F., P.A.A., N.S.I. and L.S.S. performed the experiments; M.L.K., Y.N.K., M.N.S., A.J.L.P. and G.B.S. analyzed the data; M.L.K. performed the DFT calculations and wrote the theoretical part; A.L.G. and G.B.S. wrote the paper.

Funding

This work has been supported by the Russian Foundation for Basic Research (Grants No. 19-03-142 and 18-03-00155) and the RUDN University Program “5-100” as well as by the Initiative Programs (State registration number АААА-А16-116020350251-6) in the frames of the State Task 0082-2014-0007, “Fundamental regularities of heterogeneous and homogeneous catalysis” and number AAAA-A17-1170406l0283-3 within the framework of the Programs of Fundamental Research of the Russian Academy of Sciences for 2013−2020 on the research issue of IChP RAS (Theme number in the Federal Agency for Scientific Organizations: 0082-2014-0004) and on the research issue of IPCP RAS (Theme number in the Federal Agency for Scientific Organizations: 0089-2014-0032). This work has been partially supported by the Fundação para a Ciência e a Tecnologia (FCT), Portugal (projects UID/QUI/00100/2013 and PTDC/QEQ-QIN/3967/2014).

Conflicts of Interest

The authors declare no conflict of interest.

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Sample Availability: A sample of the catalyst is not available from the authors.
Catalysts 09 00217 sch001 550
Scheme 1. The reactions carried out in the present study.
Scheme 1. The reactions carried out in the present study.
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Catalysts 09 00217 g001 550
Figure 1. The structure of complex 3.
Figure 1. The structure of complex 3.
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Figure 2. The crystal packing of complex 3.
Figure 2. The crystal packing of complex 3.
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Figure 3. The molecular structure of [VO(DMF)(phen)Br2] (4a).
Figure 3. The molecular structure of [VO(DMF)(phen)Br2] (4a).
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Catalysts 09 00217 g004 550
Figure 4. The accumulation of cyclohexanol and cyclohexanone in the oxidation of cyclohexane (0.46 M) with H2O2 (2.0 M) catalysed by complex 1 (5 × 10−4 M) at 40 °C: The concentrations of the products were measured by GC before (Graph A) and after (Graph B) the reduction of the reaction sample with solid PPh3.
Figure 4. The accumulation of cyclohexanol and cyclohexanone in the oxidation of cyclohexane (0.46 M) with H2O2 (2.0 M) catalysed by complex 1 (5 × 10−4 M) at 40 °C: The concentrations of the products were measured by GC before (Graph A) and after (Graph B) the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 g005 550
Figure 5. The accumulation of cyclohexanol and cyclohexanone in the oxidation of cyclohexane (0.46 M) with H2O2 (2.0 M) catalysed by complex 2 (5 × 10−4 M) at 40 °C: The concentrations of the products were measured by GC only after the reduction of the reaction sample with solid PPh3.
Figure 5. The accumulation of cyclohexanol and cyclohexanone in the oxidation of cyclohexane (0.46 M) with H2O2 (2.0 M) catalysed by complex 2 (5 × 10−4 M) at 40 °C: The concentrations of the products were measured by GC only after the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 g006 550
Figure 6. The dependence of the initial oxidation rate W0 on the initial concentration of catalyst 1 in the oxidation of cyclohexane (0.46 M) into cyclohexanol and cyclohexanone (a sum; after the reduction of the reaction mixture with PPh3) with H2O2 (2.0 M) catalysed by complex 1 at 40 °C: The concentrations of the products were measured by GC after the reduction of the reaction sample with solid PPh3.
Figure 6. The dependence of the initial oxidation rate W0 on the initial concentration of catalyst 1 in the oxidation of cyclohexane (0.46 M) into cyclohexanol and cyclohexanone (a sum; after the reduction of the reaction mixture with PPh3) with H2O2 (2.0 M) catalysed by complex 1 at 40 °C: The concentrations of the products were measured by GC after the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 g007 550
Figure 7. The dependence of the initial oxidation rate W0 on the initial concentration of cyclohexane (Graph A) in the oxidation of cyclohexane into cyclohexanol and cyclohexanone (via the formation of cyclohexyl hydroperoxide) with H2O2 (2.0 M) catalysed by complex 1. Graph B: the linearization of the curve depicted in Graph A. Conditions: catalyst 1 (5 × 10−4 M), 40 °C. The concentrations of products were measured by GC only after the reduction of the reaction sample with solid PPh3.
Figure 7. The dependence of the initial oxidation rate W0 on the initial concentration of cyclohexane (Graph A) in the oxidation of cyclohexane into cyclohexanol and cyclohexanone (via the formation of cyclohexyl hydroperoxide) with H2O2 (2.0 M) catalysed by complex 1. Graph B: the linearization of the curve depicted in Graph A. Conditions: catalyst 1 (5 × 10−4 M), 40 °C. The concentrations of products were measured by GC only after the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 sch002 550
Scheme 2. The mechanism of the HO• generation from the H2O2 catalyzed by I (Gibbs free energies are indicated in parentheses relative to Ia in kcal/mol).
Scheme 2. The mechanism of the HO• generation from the H2O2 catalyzed by I (Gibbs free energies are indicated in parentheses relative to Ia in kcal/mol).
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Catalysts 09 00217 g008 550
Figure 8. The Arrhenius dependence of the cyclohexane (0.46 M) oxidation with H2O2 (50%, 2.0 M) catalysed by compound 1 (5 × 10−4 M) in acetonitrile: The concentrations of the products were measured by GC after the reduction of the reaction sample with solid PPh3.
Figure 8. The Arrhenius dependence of the cyclohexane (0.46 M) oxidation with H2O2 (50%, 2.0 M) catalysed by compound 1 (5 × 10−4 M) in acetonitrile: The concentrations of the products were measured by GC after the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 g009 550
Figure 9. The kinetic curves for the oxidation of cyclohexane (0.46 M) into cyclohexanol and cyclohexanone with H2O2 (2.0 M) catalysed by complexes 3 (Graph A) or 4 (Graph B; the concentration of both catalysts was 5 × 10−4 M). Conditions: 40 °C. The concentrations of the products were measured by GC only after the reduction of the reaction sample with solid PPh3.
Figure 9. The kinetic curves for the oxidation of cyclohexane (0.46 M) into cyclohexanol and cyclohexanone with H2O2 (2.0 M) catalysed by complexes 3 (Graph A) or 4 (Graph B; the concentration of both catalysts was 5 × 10−4 M). Conditions: 40 °C. The concentrations of the products were measured by GC only after the reduction of the reaction sample with solid PPh3.
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Catalysts 09 00217 sch003 550
Scheme 3. The radical mechanism of the alkane oxidation with H2O2.
Scheme 3. The radical mechanism of the alkane oxidation with H2O2.
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Figure 10. The calculated equilibrium structures of various geometrical isomers of complexes [VIV(=O)(bpy)(H2O)Cl2] and [VV(=O)(bpy)(OH)Cl2]. (Gibbs free energies are indicated in parentheses in kcal/mol relative to the most stable isomers Ib and III.)
Figure 10. The calculated equilibrium structures of various geometrical isomers of complexes [VIV(=O)(bpy)(H2O)Cl2] and [VV(=O)(bpy)(OH)Cl2]. (Gibbs free energies are indicated in parentheses in kcal/mol relative to the most stable isomers Ib and III.)
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Table
Table 1. A summary of the crystal data for compounds 3 and 4a.
Table 1. A summary of the crystal data for compounds 3 and 4a.
34a
Crystal Data
Chemical formulaC10H8Br2N2OVC15H15Br2N3O2V
Mr382.94480.06
Crystal system, space groupMonoclinic, P21Monoclinic, P21/n
Temperature (K)130150
a, b, c (Å)7.4626 (3), 17.5643 (7), 9.3510 (4)7.1041 (6), 14.0723 (9), 17.2455 (12)
β (°)92.037 (4)90.614 (3)
V (Å3)1224.91 (9)1724.0 (2)
µ(mm−1)7.315.22
Crystal size (mm)0.25 × 0.06 × 0.060.10 × 0.06 × 0.05
Data collection
DiffractometerNew Xcalibur, AtlasS2Bruker Apex Duo
Absorption correctionMulti-scan CrysAlis PRO 1.171.38.41 (Rigaku Oxford Diffraction, 2015) Empirical absorption correction using spherical harmonics, implemented in SCALE3 ABSPACK scaling algorithm.Multi-scan SADABS (Bruker-AXS, 2004)
Tmin, Tmax0.739, 10000.545, 0.642
Table
Table 2. The selected geometric parameters (Å) for compounds 3 and 4a.
Table 2. The selected geometric parameters (Å) for compounds 3 and 4a.
Compound 3
V1—O11.617 (5)V2—Br32.4932 (16)
V1—O22.123 (5)V2—Br42.4919 (16)
V1—Br12.4944 (16)N1—V12.124 (7)
V1—Br22.5028 (16)N2—V12.129 (8)
V2—O1 i2.125 (5)N3—V22.124 (8)
V2—O21.617 (5)N4—V22.136 (8)
V1—O1—V2 ii176.2 (4)C10—N2—V1125.3 (7)
V2—O2—V1177.8 (4)C11—N3—V2125.2 (7)
C1—N1—V1125.2 (7)C15—N3—V2115.4 (6)
C5—N1—V1116.8 (6)C16—N4—V2115.5 (6)
C6—N2—V1116.7 (6)C20—N4—V2124.5 (7)
Compound 4a
O1—V21.600 (3)N2—V22.121 (3)
O2—V21.996 (3)Br1—V22.5450 (8)
N1—V22.296 (3)Br2—V22.5484 (7)
C14—O2—V2129.3 (3)C3—N2—V2117.8 (3)
C1—N1—V2129.6 (2)C4—N2—V2123.2 (3)
C2—N1—V2112.6 (3)
Note. Symmetry code(s): (i) x+1, y, z; (ii) x−1, y, z.
Table
Table 3. The selectivity parameters for the oxidation of certain alkanes with H2O2.
Table 3. The selectivity parameters for the oxidation of certain alkanes with H2O2.
n-Heptane MeCH1,2-cis-DMCH
EntryCatalystC(1):C(2):C(3):C(4)1°:2°:3°trans/cis
111.0:5.6:5.8:5.21.0:5.9:16.00.84
221.0:5.6:5.6:5.21.0:5.3:17.50.7
331.0:5.7:6.2:5.61.0:5.0:12.60.8
441.0:5.9:6.2:5.91.0:5.4:12.90.9

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MDPI and ACS Style

Fomenko, I.S.; Gushchin, A.L.; Abramov, P.A.; Sokolov, M.N.; Shul'pina, L.S.; Ikonnikov, N.S.; Kuznetsov, M.L.; Pombeiro, A.J.L.; Kozlov, Y.N.; Shul’pin, G.B. New Oxidovanadium(IV) Complexes with 2,2′-bipyridine and 1,10-phenathroline Ligands: Synthesis, Structure and High Catalytic Activity in Oxidations of Alkanes and Alcohols with Peroxides. Catalysts 2019, 9, 217. https://doi.org/10.3390/catal9030217

AMA Style

Fomenko IS, Gushchin AL, Abramov PA, Sokolov MN, Shul'pina LS, Ikonnikov NS, Kuznetsov ML, Pombeiro AJL, Kozlov YN, Shul’pin GB. New Oxidovanadium(IV) Complexes with 2,2′-bipyridine and 1,10-phenathroline Ligands: Synthesis, Structure and High Catalytic Activity in Oxidations of Alkanes and Alcohols with Peroxides. Catalysts. 2019; 9(3):217. https://doi.org/10.3390/catal9030217

Chicago/Turabian Style

Fomenko, Iakov S., Artem L. Gushchin, Pavel A. Abramov, Maksim N. Sokolov, Lidia S. Shul'pina, Nikolay S. Ikonnikov, Maxim L. Kuznetsov, Armando J. L. Pombeiro, Yuriy N. Kozlov, and Georgiy B. Shul’pin. 2019. "New Oxidovanadium(IV) Complexes with 2,2′-bipyridine and 1,10-phenathroline Ligands: Synthesis, Structure and High Catalytic Activity in Oxidations of Alkanes and Alcohols with Peroxides" Catalysts 9, no. 3: 217. https://doi.org/10.3390/catal9030217

APA Style

Fomenko, I. S., Gushchin, A. L., Abramov, P. A., Sokolov, M. N., Shul'pina, L. S., Ikonnikov, N. S., Kuznetsov, M. L., Pombeiro, A. J. L., Kozlov, Y. N., & Shul’pin, G. B. (2019). New Oxidovanadium(IV) Complexes with 2,2′-bipyridine and 1,10-phenathroline Ligands: Synthesis, Structure and High Catalytic Activity in Oxidations of Alkanes and Alcohols with Peroxides. Catalysts, 9(3), 217. https://doi.org/10.3390/catal9030217

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