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Transition metal dinitrogen complexes arecoordination compounds that containtransition metals as ion centers thedinitrogen molecules (N2) asligands.[2]
Transition metal complexes of N2 have been studied since 1965 when the first complex was reported by Allen and Senoff.[3] Thisdiamagnetic complex,[Ru(NH3)5(N2)]2+, was synthesized fromhydrazine hydrate andruthenium trichloride and consists of a [Ru(NH3)5]2+ centre attached to one end of N2.[4][5] The existence of N2 as a ligand in this compound was identified by IR spectrum with a strong band around 2170–2100 cm−1.[4] In 1966, the molecular structure of [Ru(NH3)5(N2)]Cl2 was determined by Bottomly and Nyburg byX-ray crystallography.[6]
The dinitrogen complextrans-[IrCl(N2)(PPh3)2] is made by treatingVaska's complex with aromaticacyl azides. It has a planar geometry.[7]
The first preparation of a metal-dinitrogen complex using dinitrogen was reported in 1967 by Yamamoto and coworkers. They obtained [Co(H)(N2)(PPh3)3] by reduction ofCo(acac)3 with AlEt2OEt under an atmosphere of N2. Containing both hydrido and N2 ligands, the complex was of potential relevance to nitrogen fixation.[8]
From the late 1960s, a variety of transition metal-dinitrogen complexes were made including those with iron,[9] molybdenum[10] and vanadium[11] as metal centers. Interest in such complexes arises because N2 comprises the majority of the atmosphere and because many useful compounds contain nitrogen. Biologicalnitrogen fixation probably occurs via the binding of N2 to those metal centers in the enzymenitrogenase, followed by a series of steps that involveelectron transfer andprotonation.[12]
In terms of its bonding to transition metals, N2 is related toCO andacetylene as all three species havetriple bonds. A variety of bonding modes have been characterized. Based on whether the N2 molecules are shared by two more metal centers, the complexes can be classified into mononuclear and bridging. Based on the geometric relationship between the N2 molecule and the metal center, the complexes can be classified into end-on or side-on modes. In the end-on bonding modes of transition metal-dinitrogen complexes, the N-N vector can be considered in line with the metal ion center, whereas in the side-on modes, the metal-ligand bond is known to be perpendicular to the N-N vector.[13]
As a ligand, N2 usually binds to metals as an "end-on" ligand, as illustrated by [Ru(NH3)5N2]2+. Such complexes are usually analogous to related CO derivatives. This relationship is illustrated by the pair of complexesIrCl(CO)(PPh3)2 and IrCl(N2)(PPh3)2.[14] In these mononuclear cases, N2 is both as a σ-donor and a π-acceptor. The M-N-N bond angles are close to 180°.[2] N2 is a weaker pi-acceptor than CO, reflecting the nature of the π* orbitals on CO vs N2. For this reason, few examples exist of complexes containingboth CO and N2 ligand.
Transition metal-dinitrogen complexes can contain more than one N2 as "end-on" ligands, such asmer-[Mo(N2)3(PPrn2Ph)3], which has octahedral geometry.[15] In another example, the dinitrogen ligand inMo(N2)2(Ph2PCH2CH2PPh2)2 can be reduced to produce ammonia.[16] Because many nitrogenases contain Mo, there has been particular interest in Mo-N2 complexes.
N2 also serves as a bridging ligand with "end-on" bonding to two metal centers, as illustrated by {[Ru(NH3)5]2(μ-N2)}4+. These complexes are also called multinuclear dinitrogen complexes. In contrast to their mononuclear counterpart, they can be prepared for both early and late transition metals.[2]
In 2006, a study of iron-dinitrogen complexes by Holland and coworkers showed that the N–N bond is significantly weakened upon complexation with iron atoms with a lowcoordination number. The complex involved bidentate chelating ligands attached to the iron atoms in the Fe–N–N–Fe core, in which N2 acts as a bridging ligand between two iron atoms. Increasing the coordination number of iron by modifying the chelating ligands and adding another ligand per iron atom showed an increase in the strength of the N–N bond in the resulting complex. It is thus suspected that Fe in a low-coordination environment is a key factor to the fixation of nitrogen by thenitrogenase enzyme, since its Fe–Mo cofactor also features Fe with low coordination numbers.[17]
The averagebond length of those bridging-end-on dinitrogen complexes is about 1.2 Å. In some cases, the bond length can be as long as 1.4 Å, which is similar to those of N-N single bonds.[18] Hasanayn and co-workers have shown that theLewis structures of end-on bridging complexes can be assigned based on π-molecular-orbital occupancy, in analogy with simple tetratomic organic molecules. For example the cores of N2-bridged complexes with 8, 10, or 12 π-electrons can generally be formulated, respectively, as M≡N-N≡M, M=N=N=M, and M-N≡N-M, in analogy with the 8-, 10-, and 12-π-electron organic molecules HC≡C-C≡CH, O=C=C=O, and F-C≡C-F.[19]
In comparison with their end-on counterpart, the mononuclear side-on dinitrogen complexes are usually higher in energy and the examples of them are rare. Dinitrogen act as a π-donor in these types of complexes. Fomitchev and Coppens has reported the first crystallographic evidence for side-on coordination of N2 to a single metal center in a photoinduced metastable state. When treated with UV light, the transition metal-dinitrogen complex, [Os(NH3)5(N2)]2+ in solid states can be converted into a metastable state of [Os(NH3)5(η2-N2)]2+, where the vibration of dinitrogen has shifted from 2025 to 1831 cm−1.
Some other examples are considered to exist in thetransition states of intramolecular linkage isomerizations. Armor and Taube has reported these isomerizations using15N-labelled dinitrogen as ligands.[20]
In a second mode of bridging, bimetallic complexes are known wherein the N-N vector is perpendicular to the M-M vector, which can be considered as side-on fashion. One example is [(η5-C5Me4H)2Zr]2(μ2,η2,η2-N2).[21] The dimetallic complex can react with H2 to achieve the artificialnitrogen fixation by reducing N2.[22] A related ditantalum tetrahydride complex could also reduce N2.[13]
Whenmetal nitrido complexes are produced from N2, the intermediacy of a dinitrogen complex is assumed.Some Mo(III) complexes also cleave N2:[23]
Some electron-rich metal dinitrogen complexes are susceptible to attack by electrophiles on nitrogen. When theelectrophile is a proton, the reaction is of interest in the context ofabiological nitrogen fixation. Some metal-dintrogen complexes even catalyze thehydrogenation of N2 toammonia in a cycle that involves N-protonation of a reduced M-N2 complex.[24][25]