Ferrocene

Ferrocene
Names
IUPAC name
ferrocene, bis(η5-cyclopentadienyl)iron
Other names
dicyclopentadienyl iron
Identifiers
102-54-5 YesY
ChEBI CHEBI:30672 N
ChemSpider 7329 YesY
Jmol interactive 3D Image
PubChem 11985121
UNII U96PKG90JQ YesY
Properties
C10H10Fe
Molar mass 186.04 g/mol
Appearance light orange powder
Odor camphor-like
Density 1.107 g/cm3 (0 °C), 1.490 g/cm3 (20 °C)[1]
Melting point 172.5 °C (342.5 °F; 445.6 K)[2]
Boiling point 249 °C (480 °F; 522 K)
Insoluble in water, soluble in most organic solvents
Hazards
Main hazards Very hazardous in case of ingestion. Hazardous in case of skin contact (irritant), of eye contact (irritant), of inhalation[3]

[4]

US health exposure limits (NIOSH):
TWA 15 mg/m3 (total) TWA 5 mg/m3 (resp)[5]
TWA 10 mg/m3 (total) TWA 5 mg/m3 (resp)[5]
N.D.[5]
Related compounds
Related compounds
 cobaltocene, nickelocene, chromocene, ruthenocene, osmocene, plumbocene
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

Ferrocene is an organometallic compound with the formula Fe(C5H5)2. It is the prototypical metallocene, a type of organometallic chemical compound consisting of two cyclopentadienyl rings bound on opposite sides of a central metal atom. Such organometallic compounds are also known as sandwich compounds.[6][7] The rapid growth of organometallic chemistry is often attributed to the excitement arising from the discovery of ferrocene and its many analogues.

History

Pauson and Kealy's original (incorrect) notion of ferrocene's molecular structure[8]

Ferrocene was first prepared unintentionally. In 1951, Pauson and Kealy at Duquesne University reported the reaction of cyclopentadienyl magnesium bromide and ferric chloride with the goal of oxidatively coupling the diene to prepare fulvalene. Instead, they obtained a light orange powder of "remarkable stability.".[8] A second group at British Oxygen also unknowingly discovered ferrocene. Miller, Tebboth and Tremaine were trying to synthesise amines from hydrocarbons such as cyclopentadiene and ammonia in a modification of the Haber process. They published this result in 1952 although the actual work was done three years earlier.[9][10][11] The stability of the new organoiron compound was accorded to the aromatic character of the negatively charged cyclopentadienyls, but they were not the ones to recognize the η5 (pentahapto) sandwich structure.

Robert Burns Woodward and Geoffrey Wilkinson deduced the structure based on its reactivity.[12] Independently Ernst Otto Fischer also came to the conclusion of the sandwich structure and started to synthesize other metallocenes such as nickelocene and cobaltocene.[13]

The structure of ferrocene was confirmed by NMR spectroscopy and X-ray crystallography.[10][14][15][16] Its distinctive "sandwich" structure led to an explosion of interest in compounds of d-block metals with hydrocarbons, and invigorated the development of the flourishing study of organometallic chemistry. In 1973 Fischer of the Technische Universität München and Wilkinson of Imperial College London shared a Nobel Prize for their work on metallocenes and other aspects of organometallic chemistry.[17]

Structure and bonding

The carbon-carbon bond distances are 1.40 Å within the five-membered rings, and the Fe-C bond distances are 2.04 Å. Although X-ray crystallography (in the monoclinic space group) points to the Cp rings being in a staggered conformation, it has been shown through gas phase electron diffraction[18] and computational studies[19] that in the gas phase the Cp rings are eclipsed. The staggered conformation is believed to be most stable in the condensed phase due to crystal packing. The point group of the staggered conformation is D5d and the point group of the eclipsed conformation is D5h.

The Cp rings rotate with a low barrier about the Cp(centroid)-Fe-Cp(centroid) axis, as observed by measurements on substituted derivatives of ferrocene using 1H and 13C nuclear magnetic resonance spectroscopy. For example, methylferrocene (CH3C5H4FeC5H5) exhibits a singlet for the C5H5 ring.[20]

In terms of bonding, the iron center in ferrocene is usually assigned to the +2 oxidation state, consistent with measurements using Mössbauer spectroscopy. Each cyclopentadienyl (Cp) ring is then allocated a single negative charge, bringing the number of π-electrons on each ring to six, and thus making them aromatic. These twelve electrons (six from each ring) are then shared with the metal via covalent bonding. When combined with the six d-electrons on Fe2+, the complex attains an 18-electron configuration.

Synthesis and handling properties

The first reported[21] synthesis of ferrocene used the Grignard reagent cyclopentadienyl magnesium bromide, which can be prepared by reacting cyclopentadiene with magnesium and bromoethane in anhydrous benzene. Iron(III) chloride is then suspended in anhydrous diethyl ether and added to the Grignard reagent. An idealized equation for this synthesis is:

6 C5H5MgBr + 2 FeCl3 → 2 Fe(C5H5)2 + 6 MgBrCl + 2 "(C5H5)2"

Numerous other syntheses have been reported, including the direct reaction of gas-phase cyclopentadiene with metallic iron[22] at 350 °C or with iron pentacarbonyl.[23]

Fe + 2 C5H6(g) → Fe(C5H5)2 + H2(g)
Fe(CO)5 + 2 C5H6(g) → Fe(C5H5)2 + 5 CO(g) + H2(g)

More efficient preparative methods are generally a modification of the original transmetalation sequence using either commercially available sodium cyclopentadienide[24] or freshly cracked cyclopentadiene deprotonated with potassium hydroxide[25] and reacted with anhydrous iron(II) chloride in ethereal solvents:

2 NaC5H5 + FeCl2 → Fe(C5H5)2 + 2 NaCl
FeCl2.4H2O + 2 C5H6 + 2 KOH → Fe(C5H5)2 + 2 KCl + 6 H2O

Even some amine bases can be used for the deprotonation, though the reaction proceeds more slowly than when using stronger bases:[24]

2 C5H6 + 2 (CH3CH2)2NH + FeCl2 → Fe(C5H5)2 + 2 (CH3CH2)2NH2Cl

Direct transmetalation can also be used to prepare ferrocene from other metallocenes, such as manganocene:[26]

FeCl2 + Mn(C5H5)2 → MnCl2 + Fe(C5H5)2
Crystals of ferrocene after purification by vacuum sublimation

As expected for a symmetric and uncharged species, ferrocene is soluble in normal organic solvents, such as benzene, but is insoluble in water. Ferrocene is an air-stable orange solid that readily sublimes, especially upon heating in a vacuum. It is stable to temperatures as high as 400 °C.[27] The following table gives typical values of vapor pressure of ferrocene at different temperatures:[28]

Pressure (Pa) 1 10 100
Temperature (K) 298 323 353

Reactions

With electrophiles

Ferrocene undergoes many reactions characteristic of aromatic compounds, enabling the preparation of substituted derivatives. A common undergraduate experiment is the Friedel-Crafts reaction of ferrocene with acetic anhydride (or acetyl chloride) in the presence of phosphoric acid as a catalyst.

Important reactions of ferrocene with electrophiles and other reagents.

Lithiation

Ferrocene reacts readily with butyl lithium to give 1,1'-dilithioferrocene, which in turn is a versatile nucleophile. But reaction of Ferrocene with t-BuLi produces monolithioferrocene only.[29] These approaches are especially useful methods to introduce main group functionality, e.g. using S8, chlorophosphines, chlorosilanes. The strained compounds undergo ring-opening polymerization.[30]

Some transformations of dilithioferrocene.

Phosphorus derivatives

Many phosphine derivatives of ferrocenes are known and some are used in commercialized processes.[31] Simplest and best known is 1,1'-bis(diphenylphosphino)ferrocene (dppf) prepared from dilithioferrocene. For example, in the presence of aluminium chloride Me2NPCl2 and ferrocene react to give ferrocenyl dichlorophosphine,[32] whereas treatment with phenyldichlorophosphine under similar conditions forms P,P-diferrocenyl-P-phenyl phosphine.[33] In common with anisole the reaction of ferrocene with P4S10 forms a diferrocenyl-dithiadiphosphetane disulfide.[34]

Redox chemistry -- the ferrocenium (a.k.a. ferricinium) ion

Main article: Ferrocenium

Unlike the majority of organic compounds, ferrocene undergoes a one-electron oxidation at a low potential, around 0.5 V vs. a saturated calomel electrode (SCE). This reversible oxidation has itself been used as standard in electrochemistry as Fc+/Fc = 0.64 V vs. the standard hydrogen electrode. Some electron-rich organic compounds (e.g., aniline) also are oxidized at low potentials, but only irreversibly. Oxidation of ferrocene gives the stable blue-colored cation [Fe(C5H5)2]+ originally called ferricinium, but now more commonly ferrocenium (these terms denote the same ion, contrary to what one would expect from the fact that ferric and ferrous denote different ions of a single iron atom). On a preparative scale, the oxidation is conveniently effected with FeCl3, to give the ion, which is often isolated as its PF6− salt. Alternatively, silver nitrate may be used as the oxidizer.

Ferrocenium salts are sometimes used as oxidizing agents, in part because the product ferrocene is fairly inert and readily separated from ionic products.[35] Substituents on the cyclopentadienyl ligands alters the redox potential in the expected way: electron withdrawing groups such as a carboxylic acid shift the potential in the anodic direction (i.e. made more positive), whereas electron releasing groups such as methyl groups shift the potential in the cathodic direction (more negative). Thus, decamethylferrocene is much more easily oxidised than ferrocene. Ferrocene is often used as an internal standard for calibrating redox potentials in non-aqueous electrochemistry.

Stereochemistry

A planar chiral ferrocene derivative

A variety of substitution patterns are possible with ferrocene including substition at one or both of the rings. The most common substitution patterns are 1-substituted (one substituent on one ring) and 1,1'-disubstituted (one substituent on each ring). Usually the rings rotate freely, which simplifies the isomerism. Disubstituted ferrocenes can exist as either 1,2-, 1.3- or 1,1'- isomers, none of which are interconvertible. Ferrocenes that are asymmetrically disubstituted on one ring are chiral – for example [CpFe(EtC5H3Me)] is chiral but [CpFe(C5H3Me2)] is achiral. This planar chirality arises despite no single atom being a stereogenic centre. The substituted ferrocene shown at right (a 4-(dimethylamino)pyridine derivative) has been shown to be effective when used for the kinetic resolution of racemic secondary alcohols.[36]

Applications of ferrocene and its derivatives

Ferrocene and its numerous derivatives have no large-scale applications, but have many niche uses that exploit the unusual structure (ligand scaffolds, pharmaceutical candidates), robustness (anti-knock formulations, precursors to materials), and redox (reagents and redox standards).

Fuel additives

Ferrocene and its derivatives are antiknock agents used in the fuel for petrol engines; they are safer than tetraethyllead, previously used.[37] It is possible to buy at Halfords in the UK, a petrol additive solution which contains ferrocene which can be added to unleaded petrol to enable it to be used in vintage cars which were designed to run on leaded petrol.[38] The iron-containing deposits formed from ferrocene can form a conductive coating on the spark plug surfaces.

Pharmaceutical

Some ferrocenium salts exhibit anticancer or antimalarial activity,[39] and an experimental drug has been reported which is a ferrocenyl version of tamoxifen.[40] The idea is that the tamoxifen will bind to the estrogen binding sites, resulting in a cytotoxicity effect.[40][41][42]

Materials chemistry

Ferrocene, being readily decomposed to iron nanoparticles, can be used as a catalyst for the production of carbon nanotubes.[43] The vinyl ferrocene from ferrocene can be made by a Wittig reaction of the aldehyde, a phosphonium salt and sodium hydroxide.[44] The vinyl ferrocene can be converted into a polymer which can be thought of as a ferrocenyl version of polystyrene (the phenyl groups are replaced with ferrocenyl groups).

As a ligand scaffold

Chiral ferrocenyl phosphines are employed as ligands for transition-metal catalyzed reactions. Some of them have found industrial applications in the synthesis of pharmaceuticals and agrochemicals. For example, the diphosphine 1,1'-bis(diphenylphosphino)ferrocene (dppf) is a valuable ligand for palladium-coupling reactions.

Derivatives and variations

Ferrocene analogues can be prepared with variants of cyclopentadienyl. For example, bisindenyliron and bisfluorenyliron.[31]

Carbon atoms can be replaced by heteroatoms as illustrated by Fe(η5-C5Me5)(η5-P5) and Fe(η5-C5H5)(η5-C4H4N) ("azaferrocene"). Azaferrocene arises from decarbonylation of Fe(η5-C5H5)(CO)2(η1-pyrrole) in cyclohexane.[45] This compound on boiling under reflux in benzene is converted to ferrocene.[46]

Because of the ease of substitution, many structurally unusual ferrocene derivatives have been prepared. For example, the penta(ferrocenyl)cyclopentadienyl ligand,[47] features a cyclopentadienyl anion derivatised with five ferrocene substituents.

Structure of hexaferrocenylbenzene

In hexaferrocenylbenzene, C6[(η5-C5H4)Fe(η5-C5H5)]6, all six positions on a benzene molecule have ferrocenyl substituents (R).[48] X-ray diffraction analysis of this compound confirms that the cyclopentadienyl ligands are not co-planar with the benzene core but have alternating dihedral angles of +30° and −80°. Due to steric crowding the ferrocenyls are slightly bent with angles of 177° and have elongated C-Fe bonds. The quaternary cyclopentadienyl carbon atoms are also pyramidalized.[49]

The synthesis of hexaferrocenylbenzene has been reported using Negishi coupling of hexaiodidobenzene and diferrocenylzinc, using tris(dibenzylideneacetone)dipalladium(0) as catalyst, in tetrahydrofuran:[48]

The yield is only 4%, which is further evidence consistent with substantial steric crowding around the arene core.

See also

References

  1. ↑ "Ferrocene(102-54-5)". Retrieved 3 February 2010.
  2. ↑ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. p. 3.258. ISBN 0-8493-0486-5.
  3. ↑ "Ferrocene MSDS - ScienceLab". www.sciencelab.com/msds.php?msdsId=992404.
  4. ↑ "Material Safety Data Sheet. Ferrocene. MSDS# 03388. Section" (PDF). https://www.nwmissouri.edu/naturalsciences/sds/f/Ferrocene.pdf. External link in |website= (help)
  5. 1 2 3 "NIOSH Pocket Guide to Chemical Hazards #0205". National Institute for Occupational Safety and Health (NIOSH).
  6. ↑ Federman Neto, Alberto; Pelegrino, Alessandra Caramori; Darin, Vitor Andre (2004). "Ferrocene: 50 Years of Transition Metal Organometallic Chemistry – From Organic and Inorganic to Supramolecular Chemistry". ChemInform 35 (43). doi:10.1002/chin.200443242.
  7. ↑ Pauson, P. L. (2001). "Ferrocene-how it all began". J. Organomet. Chem. 637–639: 637–639. doi:10.1016/S0022-328X(01)01126-3.
  8. 1 2 Kealy, T. J.; Pauson, P. L. (1951). "A New Type of Organo-Iron Compound". Nature 168 (4285): 1039. Bibcode:1951Natur.168.1039K. doi:10.1038/1681039b0.
  9. ↑ Miller, S. A., Tebboth, J. A., Tremaine, J. F. (1952). "114. Dicyclopentadienyliron". J. Chem. Soc.: 632–635. doi:10.1039/JR9520000632.
  10. 1 2 Pierre Laszlo, Roald Hoffmann, (2000). "Ferrocene: Ironclad History or Rashomon Tale?". Angewandte Chemie International Edition 39 (1): 123–124. doi:10.1002/(SICI)1521-3773(20000103)39:1<123::AID-ANIE123>3.0.CO;2-Z. PMID 10649350.
  11. ↑ Werner, H (2012). "At Least 60 Years of Ferrocene: The Discovery and Rediscovery of the Sandwich Complexes". Angew. Chem. Int. Ed 51: 6052–6058. doi:10.1002/anie.201201598.
  12. ↑ G. Wilkinson, M. Rosenblum, M. C. Whiting, R. B. Woodward (1952). "The Structure of Iron Bis-Cyclopentadienyl". Journal of the American Chemical Society 74 (8): 2125–2126. doi:10.1021/ja01128a527.
  13. ↑ E. O. Fischer, W. Pfab (1952). "Zur Kristallstruktur der Di-Cyclopentadienyl-Verbindungen des zweiwertigen Eisens, Kobalts und Nickels". Zeitschrift für Naturforschung B 7: 377–379.
  14. ↑ Dunitz, J. D., Orgel, L. E. (1953). "Bis-Cyclopentadienyl – A Molecular Sandwich". Nature 171 (4342): 121–122. Bibcode:1953Natur.171..121D. doi:10.1038/171121a0.
  15. ↑ J. Dunitz, L. Orgel, A. Rich (1956). "The crystal structure of ferrocene". Acta Crystallographica 9 (4): 373–375. doi:10.1107/S0365110X56001091.
  16. ↑ P. F. Eiland and R. Pepinsky (1952). "X-ray examination of iron biscyclopentadienyl". Journal of the American Chemical Society 74 (19): 4971. doi:10.1021/ja01139a527.
  17. ↑ "Press Release: The Nobel Prize in Chemistry 1973". The Royal Swedish Academy of Sciences. 1973.
  18. ↑ Haaland, A.; Nilsson, J. E. (1968). "The Determination of Barriers to Internal Rotation by Means of Electron Diffraction. Ferrocene and Ruthenocene". Acta Chemica Scandinavica 22: 2653–2670. doi:10.3891/acta.chem.scand.22-2653.
  19. ↑ Coriani, Sonia; Haaland, Arne; Helgaker, Trygve; Jørgensen, Poul (2006). "The Equilibrium Structure of Ferrocene". ChemPhysChem 7: 245–249. doi:10.1002/cphc.200500339.
  20. ↑ E. W. Abel, N. J. Long, K. G. Orrell, A. G. Osborne, V. Sik (1991). "Dynamic NMR studies of ring rotation in substituted ferrocenes and ruthenocenes". Journal of Organometallic Chemistry 403: 195–208. doi:10.1016/0022-328X(91)83100-I.
  21. ↑ Kealy, T. J.; Pauson, P. L. (1951). "A New Type of Organo-Iron Compound". Nature 168 (4285): 1039. Bibcode:1951Natur.168.1039K. doi:10.1038/1681039b0.
  22. ↑ Wilkinson, G.; Pauson, P. L.; Cotton, F. A. (1954). J. Am. Chem. Soc. 76 (7): 1970. doi:10.1021/ja01636a080. Missing or empty |title= (help)
  23. ↑ Wilkinson, G.; Cotton, F. A. (1959). "Cyclopentadienyl and Arene Metal Compounds". Progress in Inorganic Chemistry. Progress in Inorganic Chemistry 1: 1–124. doi:10.1002/978-0-470-16602-4.ch1. ISBN 978-0-470-16602-4.
  24. 1 2 Geoffrey Wilkinson (1963). "Ferrocene". Org. Synth.; Coll. Vol. 4, p. 473
  25. ↑ Jolly, W. L., The Synthesis and Characterization of Inorganic Compounds, Prentice-Hall: New Jersey, 1970.
  26. ↑ Wilkinson, G.; Cotton, F. A.; Birmingham, J. M. (1956). "On manganese cyclopentadienide and some chemical reactions of neutral bis-cyclopentadienyl metal compounds". J. Inorg. Nucl. Chem. 2 (2): 95. doi:10.1016/0022-1902(56)80004-3.
  27. ↑ Solomons, Graham, and Craig Fryhle. Organic Chemistry. 9th ed. USA: John Wiley & Sons, Inc., 2006.
  28. ↑ Monte, Manuel J. S.; Santos, Luís M. N. B. F.; Fulem, Michal; Fonseca, José M. S.; Sousa, Carlos A. D. (2006). "New Static Apparatus and Vapor Pressure of Reference Materials: Naphthalene, Benzoic Acid, Benzophenone, and Ferrocene". Journal of Chemical & Engineering Data 51 (2): 757. doi:10.1021/je050502y.
  29. ↑ Rebiere, F; Samuel, O; Kagan, H.B (1990). "A convenient method for the preparation of monolithioferrocene". Tetrahedron Letters 31 (22): 3121–3124. doi:10.1016/S0040-4039(00)94710-5.
  30. ↑ David E. Herbert, Ulrich F. J. Mayer, Ian Manners (2007). "Strained Metallocenophanes and Related Organometallic Rings Containing pi-Hydrocarbon Ligands and Transition-Metal Centers". Angew. Chem. Int. Ed. 46 (27): 5060–5081. doi:10.1002/anie.200604409.
  31. 1 2 Petr Stepnicka "Ferrocenes: Ligands, Materials and Biomolecules" J. Wiley, Hoboken, 2008. ISBN 0-470-03585-4
  32. ↑ G.R. Knox, P.L. Pauson and D. Willison (1992). "Ferrocene derivatives. 27. Ferrocenyldimethylphosphine". Organometallics 11 (8): 2930–2933. doi:10.1021/om00044a038.
  33. ↑ G.P. Sollott, H.E. Mertwoy, S. Portnoy and J.L. Snead (1963). "Unsymmetrical Tertiary Phosphines of Ferrocene by Friedel-Crafts Reactions. I. Ferrocenylphenylphosphines". J. Org. Chem. 28 (4): 1090–1092. doi:10.1021/jo01039a055.
  34. ↑ Mark R. St. J. Foreman, Alexandra M. Z. Slawin and J. Derek Woollins (1996). "2,4-Diferrocenyl-1,3-dithiadiphosphetane 2,4-disulfide; structure and reactions with catechols and [PtCl2(PR3)2](R = Et or Bun)". J. Chem. Soc., Dalton Trans. (18): 3653–3657. doi:10.1039/DT9960003653.
  35. ↑ N. G. Connelly, W. E. Geiger (1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
  36. ↑ Ruble, J. C.; Latham, H. A.; Fu, G. C. (1997). "Effective Kinetic Resolution of Secondary Alcohols with a Planar-Chiral Analogue of 4-(dimethylamino)pyridine. Use of the Fe(C5Ph5) Group in Asymmetric Catalysis". J. Am. Chem. Soc. 119 (6): 1492–1493. doi:10.1021/ja963835b.
  37. ↑ Application of fuel additives
  38. ↑ U.S. Patent 4,104,036 "Iron-containing motor fuel compositions and method for using same" Tai S. Chao et al. Issue date: Aug 1, 1978
  39. ↑ Biot, C.; Nosten, F.; Fraisse, L.; Ter-Minassian, D.; Khalife, J.; Dive, D. (2011). "The antimalarial ferroquine: from bench to clinic". Parasite 18 (3): 207–214. doi:10.1051/parasite/2011183207. ISSN 1252-607X. PMC 3671469. PMID 21894260.
  40. 1 2 S. Top, A. Vessières, G. Leclercq, J. Quivy, J. Tang, J. Vaissermann, M. Huché and G. Jaouen (2003). "Synthesis, Biochemical Properties and Molecular Modelling Studies of Organometallic Specific Estrogen Receptor Modulators (SERMs), the Ferrocifens and Hydroxyferrocifens: Evidence for an Antiproliferative Effect of Hydroxyferrocifens on both Hormone-Dependent and Hormone-Independent Breast Cancer Cell Lines". Chemistry, a European Journal 9 (21): 5223–36. doi:10.1002/chem.200305024. PMID 14613131.
  41. ↑ Ron Dagani (16 September 2002). "The Bio Side of Organometallics". Chemical and Engineering News 80 (37): 23–29. doi:10.1021/cen-v080n037.p023.
  42. ↑ S. Top, B. Dauer, J. Vaissermann and G. Jaouen (1997). "Facile route to ferrocifen, 1-[4-(2-dimethylaminoethoxy)]-1-(phenyl-2-ferrocenyl-but-1-ene), first organometallic analogue of tamoxifen, by the McMurry reaction". Journal of Organometallic Chemistry 541: 355–361. doi:10.1016/S0022-328X(97)00086-7.
  43. ↑ Devin Conroya, Anna Moisalab, Silvana Cardosoa, Alan Windleb and John Davidson (2010). "Carbon nanotube reactor: Ferrocene decomposition, iron particle growth, nanotube aggregation and scale-up". Chemical Engineering Science 65 (10): 2965–2977. doi:10.1016/j.ces.2010.01.019.
  44. ↑ Liu, Wan-yi; Xu, Qi-hai; Ma, Yong-xiang; Liang, Yong-min; Dong, Ning-li; Guan, De-peng (2001). "Solvent-free synthesis of ferrocenylethene derivatives". J. Organomet. Chem. 625: 128–132. doi:10.1016/S0022-328X(00)00927-X.
  45. ↑ Zakrzewski, J; Giannotti, Charles (1990). "An improved photochemical synthesis of azaferrocene". Journal of Organometallic Chemistry 388: 175. doi:10.1016/0022-328X(90)85359-7.
  46. ↑ Efraty, Avi.; Jubran, Nusrallah; Goldman, Alexander (1982). "Chemistry of some .eta.5-pyrrolyl- and .eta.1-N-pyrrolyliron complexes". Inorganic Chemistry 21 (3): 868. doi:10.1021/ic00133a006.
  47. ↑ Y. Yu, A.D. Bond, P. W. Leonard, K. P. C. Vollhardt, G. D. Whitener (2006). "Syntheses, Structures, and Reactivity of Radial Oligocyclopentadienyl Metal Complexes: Penta(ferrocenyl)cyclopentadienyl and Congeners". Angewandte Chemie International Edition 45 (11): 1794–1799. doi:10.1002/anie.200504047. PMID 16470902.
  48. 1 2 Yong Yu, Andrew D. Bond, Philip W. Leonard, Ulrich J. Lorenz, Tatiana V. Timofeeva, K. Peter C. Vollhardt, Glenn D. Whitener and Andrey A. Yakovenko (2006). "Hexaferrocenylbenzene". Chem. Commun. (24): 2572–2574. doi:10.1039/b604844g. PMID 16779481.
  49. ↑ Also, the benzene core has a chair conformation with dihedral angles of 14° and displays bond length alternation between 142.7 pm and 141.1 pm, both indications of steric crowding of the substituents.

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