Abstract
The phenomenon and nature of agostic interactions are reviewed in light of combined molecular orbital and charge density studies. As an introduction a historical perspective is given, illustrating the successes and short falls of the various bonding concepts developed during the past 45 years since the discovery of the phenomenon in transition metal complexes. The finding that β-agostic species might represent stable intermediates along the β-elimination reaction coordinate classifies them as suitable benchmark systems to study the microscopic origin of C–H bond activation processes. We outline the salient electronic parameters that control and quantify the extent of agostic interactions on the basis of physically observable charge density properties. Despite the focus on charge density studies, we also complement these studies with arguments based on molecular orbital theory and an irrefutable body of crystallographic, kinetic, and spectroscopic evidence.
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- 1.
It is interesting to note that the agostic interaction in this agostic benchmark complex represents a rare example of a so-called γ-agostic [4] interaction. In agostic alkyl complexes of early transition d0 metal complexes, β-agostic interactions are generally stronger than their α- or γ-counterparts. Hence, the first literature example of an agostic transition metal complex already suggests that the nature and strength of an agostic interaction might depend on the electronic situation at the metal center (d-electron count) and that of the ligand (presence of hetero atoms).
- 2.
The term agostic has been introduced by MLH Green and is derived from the Greek word àγοστóζ, which might be translated as to clasp, to draw towards, to hold to oneself; see p. 3. of [8].
- 3.
According to Poater et al., the delocalization indices δ(Ω, Ω′) were calculated from the DFT wavefunctions using an approximate formula that makes use of an HF-like second order exchange density matrix. According to a recent study by Gatti et al. [46], this approximation affords δ(Ω, Ω′) values which are very close to the HF ones if the HF and DFT optimized geometries are similar, although it erroneously implies that the electron pair density matrix can be constructed, within DFT, using the same simple formalism valid for the HF method.
- 4.
Delocalization indices were computed using GTO-type bases of triple-zeta quality and the B3LYP hybrid functional as implemented in Gaussian03 [50].
- 5.
We note that the barrier of methyl group rotation in the d8 species 5a is close to the one computed for our theoretical d0 model system EtTiCl2 + (2.8 kJ mol−1) (Fig. 4) suggesting a comparable agostic stabilization in both types of compounds.
- 6.
On the basis of this concept, β-agostic interactions can be clearly discriminated from σ-complexes formed by metal centers and η2-coordinating X–H moieties (e.g., X = H, B, C, Si). In the latter case, only bonding and antibonding σ(X–H) orbitals are involved in the metal interaction, while β-agostic compounds are characterized by the additional delocalization of the M–Cα bonding pair via negative hyperconjugation.
- 7.
The hindrance of NHC delocalization by charge polarization is documented by a comparison of the situation in [CH2CH3]− 12 and [CH2CH3]−[Li+] 14. The large NHC in 12 vs. 14 is reflected not only by a smaller CCα(1) charge concentration of 16.3 eÅ−5 in 12 but also by a remarkable activation of the Cβ–Hβ bond trans to the Cα lone pair (ca. 0.04 Å) in 12 which is less pronounced in 14 (ca. 0.01 Å). As another consequence, CCα(1) in the agostic [EtCa]+ cation is only slightly smaller (17.8 eÅ−5) compared with the one in the neutral non-agostic lithium congener (18.0 eÅ−5) (Fig. 8).
- 8.
As another consequence of the destabilizing four electron p(Cα)–π(CβHβ) interactions, the ethyl anion is assumed to be less stable than the methyl anion; see [71].
- 9.
Bader et al. have demonstrated that the negative Laplacian of the charge density distribution, L(r) = −∇2 ρ(r), determines where the charge density distribution is locally concentrated (L(r) > 0) or locally depleted (L(r) < 0). Accordingly, the L(r) function can be used to resolve the shell structure for elements with Z ≤ 18. However, the shell structure of the transargonic elements is not fully represented by the Laplacian. In general, the fourth, fifth, or sixth shell for elements of periods 4−6, respectively, is not revealed in the Laplacian. As a convention, Bader et al. suggested that the outermost shell of charge concentration (CC) of an atom (second shell of CC of the carbon atoms and third shell of CC of the nickel atom) represents its (effective) valence shell charge concentration (VSCC).
- 10.
We note that the higher polarity of the Ti–Cl bond is signaled in the charge density picture by the vanishing of the corresponding BCCs in the total charge density distribution in the Ti–Cl bonding region and by a smaller magnitude of trans-CC(Cl) vs. trans-CC(C).
- 11.
As a consequence of the phosphine coordination trans to the Cβ atom, a weakly defined (3, −1) saddle point is formed in the L(r) pattern at the titanium atom along the Ti–Cβ vector. In the experimental charge density distributions, however, a subtle (3, +1) CD zone is preserved opposite to the Cβ atom.
- 12.
Hence, the presence of local Lewis-acidic sites in the coordination region of agostic CβHβ moieties might reflect the presence of d-acceptor orbitals which accommodate the CβHβ → M donation in the MO picture.
- 13.
We note that the relative magnitudes of CCα(1), CCα(2), and CCβ(2) are similar in the experimental and calculated models. However, the experimentally determined charge concentrations appear to be larger than their respective theoretical ones. This might be due to the fact that core contraction/expansion phenomena have not been taken into account during the multipolar refinements [106].
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This work was supported by the DFG (SPP1178) and NanoCat (an international Graduate Program within the Elitenetzwerk Bayern)
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Scherer, W., Herz, V., Hauf, C. (2012). On the Nature of β-Agostic Interactions: A Comparison Between the Molecular Orbital and Charge Density Picture. In: Stalke, D. (eds) Electron Density and Chemical Bonding I. Structure and Bonding, vol 146. Springer, Berlin, Heidelberg. https://doi.org/10.1007/978-3-642-30802-4_77
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