Decamethyldizincocene

Decamethyldizincocene
Properties
Molecular formula C20H30Zn2
Molar mass 401.27 g mol−1
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Decamethyldizincocene is an organozinc compound with the formula [Zn2(η5–C5Me5)2]. It is an unusual example of a compound with a Zn-Zn bond.[1] Decamethyldizincocene is a colorless crystalline solid that burns spontaneously in the presence of oxygen and reacts with water. It is stable at room temperature and especially soluble in diethyl ether, benzene, pentane, or tetrahydrofuran.[2]

Contents

Synthesis

The ability of metals to form heteronuclear or homonuclear metal-metal bonds varies throughout the periodic table. Among the group 12 elements, mercury readily forms [M-M]2+ units whereas the elements cadmium and zinc form fewer examples of such species.[1] Decamethyldizincocene was reported in 2004 by Carmona and coworkers as an unexpected product of the reaction between decamethylzincocene (Zn(C5Me5)2) and diethyl zinc (ZnEt2).[1] The analogous reaction of zincocene (Zn(C5H5)2) with diethyl zinc (ZnEt2) gives (η5-C5Me5)ZnEt.[3] Therefore, the stabilizing effect of the methyl groups on the cyclopentadienyl rings is of great importance in the formation of decamethydizincocene. The use of ZnEt2 as a reactant is of particular significance.

The organozinc precursor is important. Diphenylzinc (Zn(C6H5)2), despite its lower solubility, can be utilized in place of ZnEt2. On the other hand, ZnMe2 gives only the half-sandwich compound (η5-C5Me5)ZnMe.[2]

Both (η5-C5Me5)ZnEt and decamethyldizincocene are produced from the reaction between Zn(η5-C5Me5)2 and ZnEt2. The relative amounts depend on reaction conditions, which can be optimized to favor one or the other.[1] For instance, if this reaction is conducted in pentane at -40 °C, (η5-C5Me5)ZnEt is the sole product. Conversely, if the reaction is conducted in diethyl ether at -10 °C, (Zn2(η5 – C5Me5)2) is the major product.

Unpredictability of synthesis

The formation of decamethyldizincocene is, however, rather unpredictable. Several duplications of this reaction (under conditions that favor the formation of decamethyldizincocene) have inexplicably led to the formation of only the half-sandwich complex (η5-C5Me5)ZnEt. The formation of the products (η5-C5Me5)ZnEt and Zn2(η5 - C5Me5)2 occurs via separate, competitive reaction pathways and, therefore, the two products do not interconvert when left to react over extended periods of time.[2]

The formation of the half-sandwich complex is believed to occur via hydrocarbyl-bridged intermediates. The reaction mechanism is, however, uncertain. Previously it was hypothesized that the creation of decamethyldizincocene occurred through the decomposition of diethylzinc, whose decomposition products would have had the capability of reducing decamethylzincocene to decamethyldizincocene. However, it is now believed that the formation of decamethyldizincocene occurs via a radical reaction involving the combination of two (η5-C5Me5)Zn• radicals.

In a new more efficient and more general route to decamethyldizincocene, KH is used to reduce decamethylzincocene to decamethyldizincocene (Figure 3). Other reductants such as K, Na, or CaH2 may be used as well in the reduction of decamethylzincocene to decamethyldizincocene. [2]

This complex does not react with [Lewis base]]s such PMe3, PPh3, NEt3, or pyridine nor does it react with H2, CO2, or CO. This compound decomposes at 11 °C and sublimes at 70°C.[1]

Structure

Various methods have been employed in order to determine the structure of decamethyldizincocene, including x-ray diffraction, 1H NMR, and mass spectrometry. Through X-ray diffraction methods it has been found that the zinc atoms are sandwiched between two parallel C5Me5 rings whose planes are perpendicular to the metal-metal bond axis.[2] The separation between the two ring planes is approximately 6.40 Å. The C5Me5 rings are in an eclipsed conformation with the methyl substituents bent slightly outward (away from the central metal atoms) at angles of 3 to 6 degrees.[4]

In mononuclear metallocenes the bending of substituents attached to the rings serves to prevent steric hindrance; however, the radius of a methyl group is only 2.0 Å and therefore the bending in decamethyldizincocene does not serve this purpose since the distance between the two rings is much greater than this value. It is believed that in the case of decamethyldizincocene the bending of the methyl groups attached to the cyclopentadienyl ligands is preferential because it concentrates the electron density away from the central, positively charged metal atoms. The separation between each Zn atom and the center of the cyclopentadienyl ring attached to it is approximately 2.04 Å and the Zn-C(ring) distances range from 2.27 to 2.30 Å.[2] The Zn-Zn bond distance is 2.035 Å, which indicates considerably strong bonding between the two zinc atoms. This can be compared to the known [Hg-Hg]2+ bond length of 2.5 to 2.7 Å.[5] Two separate types of structures for dimetallocenes have been hypothesized including a coaxial structure (which is the structure of decamethyldizincocene) and a perpendicular structure in which the metal-metal bond axis is parallel to the plane of the cyclopentadienyl ligands (which is predicted to be the structure for dicuprocenes).[6] The compound addressed in this paper is essentially linear with Zn-Zn bond angles of approximately 177°:[2]

Absence of bridging ligands

1H NMR and mass spectrometry studies have been useful in proving that decamethyldizincocene does not include bridging ligands. This study is important considering that the complex previously hypothesized to be Co2(η5-C5Me5)2 was later found using 1H NMR and mass spectrometry data to be supported by three bridging hydrogens.[7] The 1H NMR of decamethyldizincocene shows only one signal at δ 2.02 due to the hydrogens attached to the methyl groups on the cyclopentadienyl ligands.[2]

Electronic structure and bonding characteristics

Decamethyldizincocene has an accumulation of electron density between the two zinc atoms, which indicates bonding.[8] This bond has a predicted dissociation energy of 62 kcal·mol−1 and is approximately as strong as those found among metal-halide bonds. NBO (Natural Bond Order) analysis has indicated that sigma bonding occurs between the 4s orbitals of the central metal atoms with a bonding orbital occupancy of 1.9445.9 Using fragment molecular orbital analysis (FMOA) it has been found that there is one principal molecular orbital that participates in the Zn-Zn bonding with approximately 88% bonding character concentrated between the Zn atoms.

References

  1. ^ a b c d e Resa, I.; Carmona, E.; Gutierrez-Puebla, E.; Monge, A. (2004). "Decamethyldizincocene, a Stable Compound of Zn(I) with a Zn-Zn Bond". Science 305 (5687): 1136–8. doi:10.1126/science.1101356. PMID 15326350. 
  2. ^ a b c d e f g h Grirrane, A; Resa, I; Rodriguez, A; Carmona, E; Alvarez, E; Gutierrez-Puebla, E; Monge, A; Galindo, A et al. (2007). "Zinc-zinc bonded zincocene structures. Synthesis and characterization of Zn2(eta5-C5Me5)2 and Zn2(eta5-C5Me4Et)2". J. Am. Chem. Soc. 129 (3): 693–703. doi:10.1021/ja0668217. PMID 17227033. 
  3. ^ Haaland, A.; Samdal, S.; Seip, R. (1978). "The molecular structure of monomeric methyl(cyclopentadienyl)zinc, (CH3)Zn(η-C5H5), determined by gas phase electron diffraction". J. Organomet. Chem. 153 (2): 187. doi:10.1016/S0022-328X(00)85041-X. 
  4. ^ Philpott, M; Kawazoe, Y. THEOCHEM 2006, 733, 43.
  5. ^ Xie, Y.; Schaefer, H.F.; King, R. B. (2005). "The Dichotomy of Dimetallocenes:  Coaxial versus Perpendicular Dimetal Units in Sandwich Compounds". J. Am. Chem. Soc. 127 (9): 2818. doi:10.1021/ja042754+. 
  6. ^ Lutz, F.; Bau, R.; Wu, P.; Koetzle, T. F.; Kruger, C.; Schneider, J. J. (1996). "Neutron Diffraction Structure Analysis of a Triply-Bridged Binuclear Cobalt Hydride Complex, [(η5-Cp*)Co]2H3". Inorg. Chem. 35 (9): 2698. doi:10.1021/ic951297i. 
  7. ^ Kang, H. (2005). "Theoretical Study of Complexes of Extended Cyclopentadienyl Ligands with Zinc and Cadmium". J. Phys. Chem. A 109 (19): 4342. doi:10.1021/jp044293k. 
  8. ^ Kress, J. (2005). "Density Functional Theory Investigation of Decamethyldizincocene". J. Phys. Chem. A 109 (34): 7757. doi:10.1021/jp051065x.