Chemistry:Agostic interaction
In organometallic chemistry, agostic interaction refers to the interaction of a coordinatively-unsaturated transition metal with a C−H bond, when the two electrons involved in the C−H bond enter the empty d-orbital of the transition metal, resulting in a three-center two-electron bond.[1] Many catalytic transformations, e.g. oxidative addition and reductive elimination, are proposed to proceed via intermediates featuring agostic interactions. Agostic interactions are observed throughout organometallic chemistry in alkyl, alkylidene, and polyenyl ligands.
History
The term agostic, derived from the Ancient Greek word for "to hold close to oneself", was coined by Maurice Brookhart and Malcolm Green, on the suggestion of the classicist Jasper Griffin, to describe this and many other interactions between a transition metal and a C−H bond. Often such agostic interactions involve alkyl or aryl groups that are held close to the metal center through an additional σ-bond.[2][3]
Short interactions between hydrocarbon substituents and coordinatively unsaturated metal complexes have been noted since the 1960s. For example, in tris(triphenylphosphine) ruthenium dichloride, a short interaction is observed between the ruthenium(II) center and a hydrogen atom on the ortho position of one of the nine phenyl rings.[4] Complexes of borohydride are described as using the three-center two-electron bonding model.
The nature of the interaction was foreshadowed in main group chemistry in the structural chemistry of trimethylaluminium.
Characteristics of agostic bonds
Agostic interactions are best demonstrated by crystallography. Neutron diffraction data have shown that C−H and M┄H bond distances are 5-20% longer than expected for isolated metal hydride and hydrocarbons. The distance between the metal and the hydrogen is typically 1.8–2.3 Å, and the M┄H−C angle is in the range of 90°–140°. The presence of a 1H NMR signal that is shifted upfield from that of a normal aryl or alkane, often to the region normally assigned to hydride ligands. The coupling constant 1JCH is typically lowered to 70–100 Hz versus the 125 Hz expected for a normal sp3 carbon–hydrogen bond.
Strength of bond
On the basis of experimental and computational studies, the stabilization arising from an agostic interaction is estimated to be 10–15 kcal/mol. Recent calculations using compliance constants point to a weaker stabilisation (<10 kcal/mol).[6] Thus, agostic interactions are stronger than most hydrogen bonds. Agostic bonds sometimes play a role in catalysis by increasing 'rigidity' in transition states. For instance, in Ziegler–Natta catalysis the highly electrophilic metal center has agostic interactions with the growing polymer chain. This increased rigidity influences the stereoselectivity of the polymerization process.
Related bonding interactions
2(HSiPh3).png)
The term agostic is reserved to describe two-electron, three-center bonding interactions between carbon, hydrogen, and a metal. Two-electron three-center bonding is clearly implicated in the complexation of H2, e.g., in W(CO)3(PCy3)2H2, which is closely related to the agostic complex shown in the figure.[8] Silane binds to metal centers often via agostic-like, three-centered Si┄H−M interactions. Because these interactions do not include carbon, however, they are not classified as agostic.
Anagostic bonds
Certain M┄H−C interactions are not classified as agostic but are described by the term anagostic. Anagostic interactions are more electrostatic in character. In terms of structures of anagostic interactions, the M┄H distances and M┄H−C angles fall into the ranges 2.3–2.9 Å and 110°–170°, respectively.[2][9]
Function
Agostic interactions serve a key function in alkene polymerization and stereochemistry, as well as migratory insertion.
References
- ↑ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "agostic interaction". doi:10.1351/goldbook.AT06984
- ↑ 2.0 2.1 Brookhart, Maurice; Green, Malcolm L. H. (1983). "Carbon-hydrogen-transition metal bonds". J. Organomet. Chem. 250: 395–408. doi:10.1016/0022-328X(83)85065-7..
- ↑ Brookhart, Maurice; Green, Malcolm L. H.; Parkin, Gerard (2007). "Agostic interactions in transition metal compounds". Proc. Natl. Acad. Sci. 104 (17): 6908–14. doi:10.1073/pnas.0610747104. PMID 17442749. Bibcode: 2007PNAS..104.6908B.
- ↑ La Placa, Sam J.; Ibers, James A. (1965). "A Five-Coordinated d6 Complex: Structure of Dichlorotris(triphenylphosphine)ruthenium(II)". Inorg. Chem. 4 (6): 778–783. doi:10.1021/ic50028a002.
- ↑ Z. Dawoodi; M. L. H. Green; V. S. B. Mtetwa; K. Prout; A. J. Schultz; J. M. Williams; T. F. Koetzle (1986). "Evidence for Carbon–Hydrogen–Titanium Interactions: Synthesis and Crystal Structures of the Agostic alkyls [TiCl3(Me2PCH2CH2PMe2)R (R = Et or Me)"]. J. Chem. Soc., Dalton Trans. (8): 1629. doi:10.1039/dt9860001629. https://zenodo.org/record/1230034.
- ↑ Von Frantzius, Gerd; Streubel, Rainer; Brandhorst, Kai; Grunenberg, Jörg (2006). "How Strong is an Agostic Bond? Direct Assessment of Agostic Interactions Using the Generalized Compliance Matrix". Organometallics 25 (1): 118–121. doi:10.1021/om050489a.
- ↑ Nikonov, G. I. (2005). "Recent Advances in Nonclassical Interligand SiH Interactions". Adv. Organomet. Chem.. Advances in Organometallic Chemistry 53: 217–309. doi:10.1016/s0065-3055(05)53006-5. ISBN 9780120311538.
- ↑ Kubas, G. J. (2001). Metal Dihydrogen and σ-Bond Complexes. New York: Kluwer Academic. ISBN 978-0-306-46465-2.
- ↑ Braga, D.; Grepioni, F.; Tedesco, E.; Biradha, K.; Desiraju, G. R. (1997). "Hydrogen Bonding in Organometallic Crystals. 6. X−H┄M Hydrogen Bonds and M┄(H−X) Pseudo-Agostic Bonds". Organometallics 16 (9): 1846–1856. doi:10.1021/om9608364.
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