From Wikipedia, the free encyclopedia
Jump to: navigation, search
Space-filling  model of nickelocene
Nickelocen an einem Kühlfinger.jpg
IUPAC name
Other names
Bis(cyclopentadienyl) nickel(II)
ECHA InfoCard 100.013.672
RTECS number QR6500000
Molar mass 188.88 g/mol
Appearance Green crystals
Density 1.47 g/cm3
Melting point 171 to 173 °C (340 to 343 °F; 444 to 446 K)
D5h, D5d
0 D
Harmful Xn
R-phrases R20/21/22, R42/43
S-phrases S22, S24, S36/37, S45
NFPA 704
Flammability code 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g., propane Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g., phosphorus Special hazards (white): no codeNFPA 704 four-colored diamond
Lethal dose or concentration (LD, LC):
490 mg kg−1 (oral, rat)
600 mg kg−1 (oral, mouse)
Related compounds
Related compounds
CoCp2, FeCp2
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Nickelocene is the organonickel compound with the formula Ni(η5-C5H5)2. Also known as bis(cyclopentadienyl)nickel or NiCp2, this bright green paramagnetic solid is of enduring academic interest,[1] although it does not yet have any known practical applications.

Structure and bonding[edit]

Ni(C5H5)2 belongs to a group of organometallic compounds called metallocenes. Metallocenes usually adopt structures in which a metal ion is sandwiched between two parallel cyclopentadienyl (Cp) rings. In the solid-state, the molecule has D5h symmetry, wherein the two rings are eclipsed.[2]

The Ni center has a formal +2 charge, and the Cp rings are usually assigned as cyclopentadienyl anions (Cp), related to cyclopentadiene by deprotonation. The structure is similar to ferrocene. In terms of its electronic structure, three pairs of d electrons on nickel are allocated to the three d orbitals involved in Ni–Cp bonding: dxy, dx2y2, dz2. One of the two remaining d-electrons resides in each of the dyz and dxz orbitals, giving rise to the molecule's paramagnetism, as manifested in the unusually high field chemical shift observed in its 1H NMR spectrum. With 20 valence electrons, nickelocene has the highest electron count of the transition metal metallocenes. Cobaltocene, Co(C5H5)2, with only 19 valence is, however, a stronger reducing agent, illustrating the fact that electron energy, not electron count determines redox potential.


Nickelocene was first prepared by E. O. Fischer in 1953, shortly after the discovery of ferrocene, the first metallocene compound.[3] It has been prepared in a one-pot reaction, by deprotonating cyclopentadiene with ethylmagnesium bromide, and adding anhydrous nickel(II) acetylacetonate.[4] A modern synthesis entails treatment of anhydrous sources of NiCl2 with sodium cyclopentadienyl:[5]

[Ni(NH3)6]Cl2 + 2 NaC5H5 → Ni(C5H5)2 + 2 NaCl + 6 NH3


Like many organometallic compounds, Ni(C5H5)2 does not tolerate extended exposure to air before noticeable decomposition.[6] Samples are typically handled with air-free techniques.

Most chemical reactions of nickelocene are characterized by its tendency to yield 18-electron products with loss or modification of one Cp ring.

Ni(C5H5)2 + 4 PF3 → Ni(PF3)4 + organic products

The reaction with secondary phosphines follows a similar pattern:

2 Ni(C5H5)2 + 2 PPh2H → [Ni2(PPh2)2(C5H5)2] + 2 C5H6

Nickelocene can be oxidized to the corresponding cation, which contains Ni(III).

Gaseous Ni(C5H5)2 decomposes to a nickel mirror upon contact with a hot surface, releasing the hydrocarbon ligands as gaseous coproducts. This process has been considered as a means of preparing nickel films.


  1. ^ Elschenbroich, C. (2006). Organometallics. Weinheim: Wiley-VCH. ISBN 978-3-527-29390-2. 
  2. ^ P. Seiler; J. D. Dunitz (1980). "The structure of nickelocene at room temperature and at 101 K". Acta Cryst. B36: 2255–2260. doi:10.1107/S0567740880008539. 
  3. ^ Fischer, E. O.; Pfab, W. (1952). "Zur Kristallstruktur der Di-Cyclopentadienyl-Verbindungen des zweiwertigen Eisens, Kobalts und Nickels" [On the crystal structure of biscyclopentadienyl compounds of divalent iron, cobalt and nickel]. Z. Naturforsch. B. 7: 377–379. 
  4. ^ Wilkinson, G.; Pauson, P. L.; Cotton, F. A. (1954). "Bis-cyclopentadienyl Compounds of Nickel and Cobalt". J. Am. Chem. Soc. 76 (7): 1970–4. doi:10.1021/ja01636a080. 
  5. ^ Girolami, G. S.; Rauchfuss, T. B.; Angelici, R. J. (1999). Synthesis and Technique in Inorganic Chemistry. Mill Valley, CA: University Science Books. ISBN 0935702482. 
  6. ^ Jaworska-Augustyniak, Anna; Wojtczak, Jan (1979). "Charge-transfer complexes of cobaltocene and nickelocene with tetrachloromethane". Monatshefte für Chemie. 110 (5): 1113–1121. doi:10.1007/BF00910959. 

External links[edit]