Dmitry V. Yandulov

Bio: Dmitry V. Yandulov is an academic researcher from Massachusetts Institute of Technology. The author has contributed to research in topics: Stoichiometry & Density functional theory. The author has an hindex of 6, co-authored 6 publications receiving 1774 citations.

Catalytic Reduction of Dinitrogen to Ammonia at a Single Molybdenum Center

Abstract: This Account explores the catalytic reduction of dinitrogen by molybdenum complexes that contain the [HIPTN3N]3- ligand ([HIPTN3N]3- = [(HIPTNCH2CH2)3N]3-, where HIPT = 3,5-(2,4,6-i-Pr3C6H2)2C6H3) at room temperature and pressure with protons and electrons. A total of 7−8 equiv of ammonia is formed out of ∼12 possible (depending upon the Mo derivative employed). No hydrazine is formed. Numerous X-ray studies of proposed intermediates in the catalytic cycle suggest that N2 is being reduced at a sterically protected, single Mo center operating in oxidation states between MoIII and MoVI. Subtle variations of the [HIPTN3N]3- ligand are not as successful as a consequence of an unknown shunt in the catalytic cycle that consumes reduction equivalents to yield (it is proposed) dihydrogen.

Reduction of dinitrogen to ammonia at a well-protected reaction site in a molybdenum triamidoamine complex.

Abstract: We have synthesized a triamidoamine ligand ([(RNCH2CH2)3N]3-) in which R is 3,5-(2,4,6-i-Pr3C6H2)2C6H3 (HexaIsoPropylTerphenyl or HIPT). The reaction between MoCl4(THF)2 and H3[HIPTN3N] in THF followed by 3.1 equiv of LiN(SiMe3)2 led to formation of orange [HIPTN3N]MoCl. Reduction of [HIPTN3N]MoCl with magnesium in THF under dinitrogen led to formation of salts that contain the {[HIPTN3N]Mo(N2)}- ion. The {[HIPTN3N]Mo(N2)}- ion can be oxidized by zinc chloride to give [HIPTN3N]Mo(N2) or protonated to give [HIPTN3N]Mo-N=N-H. Other relevant compounds that have been prepared include {[HIPTN3N]Mo-N=NH2}+, [HIPTN3N]MoN, {[HIPTN3N]Mo=NH}+, and {[HIPTN3N]Mo(NH3)}+. (The anion is usually {B(3,5-(CF3)2C6H3)4}- = {BAr'4}-.) Reduction of [HIPTN3N]Mo(N2) with CoCp2 in the presence of {2,6-lutidinium}BAr'4 in benzene leads to formation of ammonia and {[HIPTN3N]Mo(NH3)}+. Preliminary X-ray studies suggest that the HIPT substituent creates a deep, three-fold symmetric cavity that protects a variety of dinitrogen reduction products against bimolecular decomposition reactions, while at the same time the metal is left relatively open toward reactions near the equatorial amido ligands.

Studies relevant to catalytic reduction of dinitrogen to ammonia by molybdenum triamidoamine complexes

Abstract: In this paper we explore several issues surrounding the catalytic reduction of dinitrogen by molybdenum compounds that contain the [(HIPTNCH2CH2)3N]3- ligand (where HIPT = 3,5-(2,4,6-i-Pr3C6H2)2C6H3). Four additional plausible intermediates in the catalytic dinitrogen reduction have now been crystallographically characterized; they are MoNNH (Mo = [(HIPTNCH2CH2)3N]Mo), [MoNNH2][BAr‘4] (Ar‘ = 3,5-(CF3)2C6H3), [MoNH][BAr‘4], and Mo(NH3). We also have crystallographically characterized a 2,6-lutidine complex, Mo(2,6-Lut)+, which is formed upon treatment of MoH with [2,6-LutH][B(C6F5)4]. We focus on the synthesis of compounds that have not yet been isolated, which include MoNNH2, MoNH, and Mo(NH2). MoNNH2, formed by reduction of [MoNNH2]+, has not been observed. It decomposes to give mixtures that contain two or more of the following: MoNNH, Mo⋮N, Mo(NH3)+, Mo(NH3), and ammonia. MoNH, which can be prepared by reduction of [MoNH]+, is stable for long periods in the presence of a small amount of CrCp*2, but in...

Molybdenum triamidoamine complexes that contain hexa-tert-butylterphenyl, hexamethylterphenyl, or p-bromohexaisopropylterphenyl substituents. An examination of some catalyst variations for the catalytic reduction of dinitrogen.

Abstract: Three new tetramines, (ArNHCH2CH2)3N, have been synthesized in which Ar = 3,5-(2,4,6-t-Bu3C6H2)2C6H3 (H3[HTBTN3N]), 3,5-(2,4,6-Me3C6H2)2C6H3 (H3[HMTN3N]), or 4-Br-3,5-(2,4,6-i-Pr3C6H2)2C6H2 (H3[pBrHIPTN3N]). The diarylated tetramine, {3,5-(2,4,6-t-Bu3C6H2)2C6H3NHCH2CH2}2NCH2CH2NH2, has also been isolated, and the “hybrid” tetramine {3,5-(2,4,6-t-Bu3C6H2)2C6H3NHCH2CH2}2NCH2CH2NH(4-t-BuC6H4) has been prepared from it. Monochloride complexes, [(TerNCH2CH2)3N]MoCl, have been prepared, as well as a selection of intermediates that would be expected in a catalytic dinitrogen reduction such as [(TerNCH2CH2)3N]Mo⋮N and {[(TerNCH2CH2)3N]Mo(NH3)}{BAr‘4} (Ter = HTBT, HMT, or pBrHIPT and Ar‘ = 3,5-(CF3)2C6H3)). Intermediates that contain the new terphenyl-substituted ligands are then evaluated for their efficiency for the catalytic reduction of dinitrogen under conditions where analogous [HIPTN3N]Mo species give four turnovers to ammonia under “standard” conditions with an efficiency of ∼65%. Only [pBrHIPTN3N]Mo compo...

Synthesis and reactions of molybdenum triamidoamine complexes containing hexaisopropylterphenyl substituents.

Abstract: We have synthesized a triamidoamine ligand ([(RNCH2CH2)3N]3-) in which R is 3,5-(2,4,6-i-Pr3C6H2)2C6H3 (hexaisopropylterphenyl or HIPT). The reaction between MoCl4(THF)2 and H3[HIPTN3N] in THF followed by 3.1 equiv of LiN(SiMe3)2 led to formation of orange [HIPTN3N]MoCl. Reduction of MoCl (Mo = [HIPTN3N]Mo) with magnesium in THF under dinitrogen led to formation of salts that contain the {Mo(N2)}- ion. The {Mo(N2)}- ion can be oxidized by zinc chloride to give Mo(N2) or protonated to give MoNNH. The latter was found to decompose to yield MoH. Other relevant compounds that have been prepared include {MoN−NH2}+ (by protonation of MoNNH), Mo⋮N, {Mo=NH}+ (by protonation of Mo⋮N), and {Mo(NH3)}+ (by treating MoCl with ammonia). (The anion is usually {B(3,5-(CF3)2C6H3)4}- = {BAr‘4}-.) X-ray studies were carried out on {Mg(DME)3}0.5[Mo(N2)], MoNNMgBr(THF)3, Mo(N2), Mo⋮N, and {Mo(NH3)}{BAr‘4}. These studies suggest that the HIPT substituent on the triamidoamine ligand creates a cavity that stabilizes a variety of...

Mechanism of Nitrogen Fixation by Nitrogenase: The Next Stage

Abstract: Brian M. Hoffman,* Dmitriy Lukoyanov, Zhi-Yong Yang,† Dennis R. Dean,*,‡ and Lance C. Seefeldt*,† †Department of Chemistry and Biochemistry, Utah State University, 0300 Old Main Hill, Logan, Utah 84322, United States ‡Department of Biochemistry, Virginia Tech, 900 West Campus Drive, Blacksburg, Virginia 24061, United States Departments of Chemistry and Molecular Biosciences, Northwestern University, 2145 Sheridan Road, Evanston, Illinois 60208, United States

Thermochemistry of Proton-Coupled Electron Transfer Reagents and its Implications

Abstract: Many, if not most, redox reactions are coupled to proton transfers. This includes most common sources of chemical potential energy, from the bioenergetic processes that power cells to the fossil fuel combustion that powers cars. These proton-coupled electron transfer or PCET processes may involve multiple electrons and multiple protons, as in the 4 e–, 4 H+ reduction of dioxygen (O2) to water (eq 1), or can involve one electron and one proton such as the formation of tyrosyl radicals from tyrosine residues (TyrOH) in enzymatic catalytic cycles (eq 2). In addition, many multi-electron, multi-proton processes proceed in one-electron and one-proton steps. Organic reactions that proceed in one-electron steps involve radical intermediates, which play critical roles in a wide range of chemical, biological, and industrial processes. This broad and diverse class of PCET reactions are central to a great many chemical and biochemical processes, from biological catalysis and energy transduction, to bulk industrial chemical processes, to new approaches to solar energy conversion. PCET is therefore of broad and increasing interest, as illustrated by this issue and a number of other recent reviews.

Beyond fossil fuel-driven nitrogen transformations.

Abstract: BACKGROUND The invention of the Haber-Bosch (H-B) process in the early 1900s to produce ammonia industrially from nitrogen and hydrogen revolutionized the manufacture of fertilizer and led to fundamental changes in the way food is produced. Its impact is underscored by the fact that about 50% of the nitrogen atoms in humans today originate from this single industrial process. In the century after the H-B process was invented, the chemistry of carbon moved to center stage, resulting in remarkable discoveries and a vast array of products including plastics and pharmaceuticals. In contrast, little has changed in industrial nitrogen chemistry. This scenario reflects both the inherent efficiency of the H-B process and the particular challenge of breaking the strong dinitrogen bond. Nonetheless, the reliance of the H-B process on fossil fuels and its associated high CO 2 emissions have spurred recent interest in finding more sustainable and environmentally benign alternatives. Nitrogen in its more oxidized forms is also industrially, biologically, and environmentally important, and synergies in new combinations of oxidative and reductive transformations across the nitrogen cycle could lead to improved efficiencies. ADVANCES Major effort has been devoted to developing alternative and environmentally friendly processes that would allow NH 3 production at distributed sources under more benign conditions, rather than through the large-scale centralized H-B process. Hydrocarbons (particularly methane) and water are the only two sources of hydrogen atoms that can sustain long-term, large-scale NH 3 production. The use of water as the hydrogen source for NH 3 production requires substantially more energy than using methane, but it is also more environmentally benign, does not contribute to the accumulation of greenhouse gases, and does not compete for valuable and limited hydrocarbon resources. Microbes living in all major ecosystems are able to reduce N 2 to NH 3 by using the enzyme nitrogenase. A deeper understanding of this enzyme could lead to more efficient catalysts for nitrogen reduction under ambient conditions. Model molecular catalysts have been designed that mimic some of the functions of the active site of nitrogenase. Some modest success has also been achieved in designing electrocatalysts for dinitrogen reduction. Electrochemistry avoids the expense and environmental damage of steam reforming of methane (which accounts for most of the cost of the H-B process), and it may provide a means for distributed production of ammonia. On the oxidative side, nitric acid is the principal commodity chemical containing oxidized nitrogen. Nearly all nitric acid is manufactured by oxidation of NH 3 through the Ostwald process, but a more direct reaction of N 2 with O 2 might be practically feasible through further development of nonthermal plasma technology. Heterogeneous NH 3 oxidation with O 2 is at the heart of the Ostwald process and is practiced in a variety of environmental protection applications as well. Precious metals remain the workhorse catalysts, and opportunities therefore exist to develop lower-cost materials with equivalent or better activity and selectivity. Nitrogen oxides are also environmentally hazardous pollutants generated by industrial and transportation activities, and extensive research has gone into developing and applying reduction catalysts. Three-way catalytic converters are operating on hundreds of millions of vehicles worldwide. However, increasingly stringent emissions regulations, coupled with the low exhaust temperatures of high-efficiency engines, present challenges for future combustion emissions control. Bacterial denitrification is the natural analog of this chemistry and another source of study and inspiration for catalyst design. OUTLOOK Demands for greater energy efficiency, smaller-scale and more flexible processes, and environmental protection provide growing impetus for expanding the scope of nitrogen chemistry. Nitrogenase, as well as nitrifying and denitrifying enzymes, will eventually be understood in sufficient detail that robust molecular catalytic mimics will emerge. Electrochemical and photochemical methods also demand more study. Other intriguing areas of research that have provided tantalizing results include chemical looping and plasma-driven processes. The grand challenge in the field of nitrogen chemistry is the development of catalysts and processes that provide simple, low-energy routes to the manipulation of the redox states of nitrogen.

Catalytic Reduction of Dinitrogen to Ammonia at a Single Molybdenum Center

Abstract: This Account explores the catalytic reduction of dinitrogen by molybdenum complexes that contain the [HIPTN3N]3- ligand ([HIPTN3N]3- = [(HIPTNCH2CH2)3N]3-, where HIPT = 3,5-(2,4,6-i-Pr3C6H2)2C6H3) at room temperature and pressure with protons and electrons. A total of 7−8 equiv of ammonia is formed out of ∼12 possible (depending upon the Mo derivative employed). No hydrazine is formed. Numerous X-ray studies of proposed intermediates in the catalytic cycle suggest that N2 is being reduced at a sterically protected, single Mo center operating in oxidation states between MoIII and MoVI. Subtle variations of the [HIPTN3N]3- ligand are not as successful as a consequence of an unknown shunt in the catalytic cycle that consumes reduction equivalents to yield (it is proposed) dihydrogen.

Challenges in reduction of dinitrogen by proton and electron transfer

Abstract: Ammonia is an important nutrient for the growth of plants. In industry, ammonia is produced by the energy expensive Haber–Bosch process where dihydrogen and dinitrogen form ammonia at a very high pressure and temperature. In principle one could also reduce dinitrogen upon addition of protons and electrons similar to the mechanism of ammonia production by nitrogenases. Recently, major breakthroughs have taken place in our understanding of biological fixation of dinitrogen, of molecular model systems that can reduce dinitrogen, and in the electrochemical reduction of dinitrogen at heterogeneous surfaces. Yet for efficient reduction of dinitrogen with protons and electrons major hurdles still have to be overcome. In this tutorial review we give an overview of the different catalytic systems, highlight the recent breakthroughs, pinpoint common grounds and discuss the bottlenecks and challenges in catalytic reduction of dinitrogen.