[{"@context":"http:\/\/schema.org\/","@type":"BlogPosting","@id":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/pentacarbonalferro-wikipedia-wikipedia\/#BlogPosting","mainEntityOfPage":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/pentacarbonalferro-wikipedia-wikipedia\/","headline":"Pentacarbonalferro – Wikipedia Wikipedia","name":"Pentacarbonalferro – Wikipedia Wikipedia","description":"before-content-x4 The pentacarbonilferro , commonly known as pentacarbonile , is the Formula FE (C\u2261O) mixture 5 (Carbon monoxide as a","datePublished":"2020-09-01","dateModified":"2020-09-01","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/44a4cee54c4c053e967fe3e7d054edd4?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/44a4cee54c4c053e967fe3e7d054edd4?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/2\/2e\/Gnome-applications-science.svg\/25px-Gnome-applications-science.svg.png","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/2\/2e\/Gnome-applications-science.svg\/25px-Gnome-applications-science.svg.png","height":"25","width":"25"},"url":"https:\/\/wiki.edu.vn\/all2en\/wiki32\/pentacarbonalferro-wikipedia-wikipedia\/","wordCount":4002,"articleBody":"     (adsbygoogle = window.adsbygoogle || []).push({});before-content-x4The pentacarbonilferro , commonly known as pentacarbonile , is the Formula FE (C\u2261O) mixture 5 (Carbon monoxide as a binder is called “Carbonile”). In standard conditions it is a light yellow liquid with a pungent smell. FE (CO) 5 It is the precursor of numerous iron complexes, many of which are useful in organic synthesis. [2] Fe (CO) 5 It is commercially available cheap.FE (CO) 5 It is a homolytic metallocarbonile, i.e. the terminal co [3] It is the only binder that complex the metal. Other examples are CR (CO) 6 e n (Co) 4 . The iron also forms the polynuclear carbonils Fe 2 (CO) 9 e Fe 3 (CO) twelfth . All these charcoal compounds are very toxic.        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4As is the case for other metallocarbonili m (co) n , to the iron atom in Fe (Co) 5 It is attributed, conventionally, state of zero oxidation. In most of the low -state oxidation complexes, the central metal tends to take an external electronic configuration of 18 electrons (3 d ten 4 s 2 4 p 6 ). Fe (CO) 5 This rule follows 18 electrons as the iron atom has 8 Valenza electrons and each co -tied CO contributes with two electrons, those of the solitary couple on C. The structure of the FE Molecule (CO) 5 It is that of a trigonal bipiramide with the iron atom in the center, as seen in the figure on the right (symmetry D 3H in the gaseous phase [4] , but molecule slightly distorted in the crystal [5] ). Three binders are lying on one plane and they say equatorial binders, while the other two are arranged along the axis perpendicular to that plan and say axial. This geometric structure is similar to that adopted by PF 5 , AsF 5 And halogen and halogenocomplexes of non -pentacoordinated non -metals. [6] Contrary to the latter, however, in Fe (Co) 5 The axial carbons are, albeit slightly, closer to the iron than the equatorial ones and the same thing happens in the Isoelectronic Aion MN (CO) 5 – . [7] All FE – C – or linear groups are linear. Given the symmetry of the structure, the molecule is apolar and the substance is at room temperature as a volatile liquid, soluble in organic solvents that go, as polarity, from alcohol to hydrocarbons, while it is practically insoluble in water. Fe (CO) 5 It is a typical flower molecule; The binders with the axials and equatorials can exchange position through the intramolecular rearrangement mechanism called pseudorotation of Berry, and are indistinguishable in the scale of the times of MRI spectroscopy at room temperature, but are well distinguishable in the infrared spectrum. [8] The magnetic resonance spectrum of the nucleus 13 C di Fe (CO) 5 In solution it shows a single signal due to the rapid exchange of co between the non -equivalent coordination sites, but the one recorded in the solid state with MAS technique ( magic angle spinning ) shows a rather limited exchange speed; This is unlike what happens with Aion’s salts [HFE (CO) 4 ] – (see below), in which the exchange is instead very quick. [9] Fe (CO) 5 it is isoelectronic with carbonal anions [MN (CO) 5 ] – , [Cr (CO) 5 ] 2\u2212 e [in (what) 5 ] 3\u2212 . [ten] The mixture was obtained for the first time by Ludwig Mondo and Friedrich Quincke in 1891. [11] Fe (CO) 5 It can be synthesized for direct combination of metal and co, like Ni (CO) 4 . To produce Ni (CO) 4 It is sufficient to operate in normal conditions, but to obtain FE (CO) 5 It is necessary to operate at high temperature, using finely divided powder iron and carbon monoxide, co, under pressure.        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4Table of ContentsCO replacement reactions [ change | Modifica Wikitesto ] Oxidation and reduction reactions [ change | Modifica Wikitesto ] Acid-base reactions [ change | Modifica Wikitesto ] Replacements with dieni [ change | Modifica Wikitesto ] CO replacement reactions [ change | Modifica Wikitesto ] These reactions allow you to obtain thousands of FE (CO) derivatives 5 . By replacing the CO with bases of Lewis, L, the FE (CO) derivatives are obtained 5-x L x . Examples of common bases of Lewis are the isocianuri, phosphines and tertiary arsine and alcheni. Generally, binders with more limited \u03c0 accepted capacity than carbon monoxide replace only one or two binders, but with similar or even greater access skills of the CO, such as PF 3 , AsF 3 and Isocianuri (C\u2261n-R), all five coal can also be replaced. The replacement reactions are often induced with catalysts or irradiation. [twelfth] For example, the synthesis of the bis (trifenilfospine) complex, FE (CO) 3 (P(C 6 H 5 ) 3 ) 2 , can be led by photochemical, but also by addition of Naoh or Nabh 4 . [13] To replace CO binders with other L bigners, the nucleophilic and oxidant action of the trimetilamine can be used N -Osside according to the following reaction: M (CO) n +  Me 3 No + l \u2192 (C) n-1 L  +  Me 3 N + what 2 Here the oxygen atom of me 3 No, bringing on itself a negative formal charge, acts as a nucleophilic by attacking the electrophilic c of a co. The transfer of an or CO oxidizes it to CO2: this is no longer a donor and detaches itself from the iron; Now the metal center comes to find itself with only 16 electrons of value, therefore coordinatively unsaturated, and therefore it can be combined with the binder l present.        (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4Oxidation and reduction reactions [ change | Modifica Wikitesto ] Most metallocarbonili can be oxidized with halogens. For example, FE (CO) 5 reacts with halogen forming fe (co) 4 X 2 (X = i, br, cl), where iron is in the state of oxidation +2. These species for heating forgive Co and form the corresponding iron halogen (II), such as iron chloride (II). The reduction of FE (CO) 5 With Sodio it produces the Tetracarbonilferrato anion, FE (CO) 4 2\u2212 , also called Collman’s reagent , where iron is in the state of oxidation – 2. This dianion is isoelectronic with Ni (CO) 4 , but it is much more nucleophilic. [14] Acid-base reactions [ change | Modifica Wikitesto ] Fe (CO) 5 It cannot be directly proton, but is attacked by hydroxide ions. For treatment of FE (CO) 5 With watery alkaline hydroxides, anionic hydruro [HFE (CO) is obtained 4 ] – (and bicarbonate anion): [15] [16] Fe (CO) 5 +  2 OH – \u2192 HFER (C) 4 – +  HCO 3 – This can be oxidized to give the Trinuclear carbonal metal FE 3 (CO) twelfth . For acidification of [HFE (CO) solutions 4 ] – you get h 2 Fe (CO) 4 , unstable sopa at -20 \u00b0 C, with the two atoms h in cis among them in a distorted octahedral coordination (symmetry C 2V ): [17] HFA (C) 4 – +  H + \u2192  H 2 Fe (CO) 4 Which was the first known metal hydrur. [18] All these species, such as the progenitor Fe (Co) 5 , they are confident of the 18 electrons rule. Replacements with dieni [ change | Modifica Wikitesto ] The dieni react with fe (co) 5 per formation (Diene) Fe (CO) 3 , where two Co binders have been replaced by the two \u03c0 ties of the Diene. This reaction takes place with many dieni, in particular 1,3-Butadiene Econ Norbornadiene. A derivative of considerable historical importance is the iron cyclobutadic Tricarbonile, (c 4 H 4 ) Fe (CO) 3 , where c 4 H 4 It is the cyclobutadiene, a molecule in itself antiartomatic, very unstable if not coordinated with iron. [19] Much attention was paid to the complexes with cyclingsading, starting from 1.4-dieces obtainable with the reduction of Birch. The 1.4-dieni isomerize at 1.3-dieni following complexion. [20] Fe (CO) 5 reacts in diciclopentadiene [21] To form the dimer of the iron cyclopentadicii dicarbonile, [Fe (c 5 H 5 )(CO) 2 ] 2 . This compound can be considered a hybrid between Ferrone and FE (CO) 5 , even if as reactivity it does not resemble either of them. [22] In Europa Fe(CO) 5 It was used in the past as an anti -high agent in petrol, before the advent of tetraethyle lead. Two more modern alternatives are Ferrocene and Manganese Metilcicliclopentadienil Tricarbonile, (CH 3 C 5 H 4 ) Mn (CO) 3 . In research and in its applications it is the primary standard for nuclear iron magnetic resonance spectrars, which is based on the nucleus 57 Fe (spin 1\/2-). [23] Industrially, the most important use of FE (CO) 5 It is in the production of Carbonile iron , a form of finely divided iron, material used in high frequency magnetic nuclei for radio and televisions, and for the manufacture of some materials that absorb radar radiation. FE (CO) 5 It is widely used as a precursor for the synthesis of iron nanoparticles. It was found that Fe (Co) 5 It is a strong flame delay in fires powered by oxygen. [24] A few hundred PPM of FE (CO) 5 They reduce the flame speed of a methane-air stechiometric mixture by about 50%. However, it is not used as a flame delay due to its toxicity. Fe (CO) 5 it is toxic, even if less than ni (co) 4 , and is dangerous for its volatility, having a steam pressure of 21 mmhg at 20 \u00b0 C. It is also flammable, like the other metallocarbonili. ^  Sigma Aldrich; rev. del 28.12.2012  ^  S. Samson e G. R. Stephenson, Pentacarbonyliron , in L. Pacquette (the care of), Encyclopedia of Reagents for Organic Synthesis , New York, J. Wiley & Sons, 2004, DOI: 10,1002\/047084289 .  ^  In metallocarbonili, sometimes some Co binders can also act as a bridge between two metal centers, as happens for example for two of them in co 2 (CO) 8 In the solid state, in which these bind the two Co. centers in such cases it is said that the CO is “bridge”, while the others are united only to one of the two centers linearly and therefore “terminals” are said.  ^  ( IN ) A. Almenningen, A. Haaland E K. Wahl, A Gas Phase Electron Diffraction Investigation of Iron Pentacarbonyl. , in Acta Chemica Scandinavica , vol. 23, 1969, pp. 2245\u20132252, two: 10.3891\/acta.chem.scand.23-2245 . URL consulted on February 4, 2021 .  ^  Dario Braga, Fabrizia Gopioni and A. Guy Orpen, Nickel carbonyl [Ni(CO)4] and iron carbonyl [Fe(CO)5]: molecular structures in the solid state , in Organometallics , vol. 12, n. 4, 1 April 1993, pp. 1481\u20131483, Doi: 10.1021\/om00028a082 . URL consulted on February 4, 2021 .  ^  J. HUEEILE, E. ERITE TO R. PIN DINE, Inorganic cjimica, principles, structures, reactivity , 2a ed., picn, 1999, p. 233, ISBN 88-299-1470-3  ^  ( IN ) Angelo R. Rossi e Roald. Hoffmann, Transition metal pentacoordination , in Inorganic Chemistry , vol. 14, n. 2, 1975-02, pp. 365\u2013374, DOI: 10.1021\/ic50144a032 . URL consulted on February 3, 2021 .  ^  Adams, R. D.; Barnard, T. S.; Cortopassi, J. E.; Wu, W.; Li, Z. “Platinum-ruthenium carbonyl cluster complexes” Inorganic Syntheses 1998, volume 32, pp. 280-284. DOI:\u00a0 10.1002\/9780470132630.ch44  ^  ( IN ) Brian E. Hanson e Kenton H. Whitmire, Exchange of axial and equatorial carbonyl groups in pentacoordinate metal carbonyls in the solid state. The variable temperature magic angle spinning carbon-13 NMR spectroscopy of iron pentacarbonyl, [Ph3PNPPh3][HFe(CO)4], and [NEt4][HFe(CO)4] , in Journal of the American Chemical Society , vol. 112, n. 3, 1990-01, pp. 974\u2013977, DOI: 10.1021 \/ JA00159A011 . URL consulted on February 4, 2021 .  ^  J. HUEEILE, E. ERITE TO R. PIN DINE, Inorganic chemistry, principles, structures, reactivity , 2\u00aa ed., 1999, P. 640, ISBN 8829914703.  ^   L. Mond e F. Quincke, About a fleeting connection of iron with carbon oxide , in Ber. German. chem. Ges. , vol. 24, n. 1, 1891, pp. 2248-2250, DOI: 10.1002\/Cber.189102401375 . URL consulted on January 31, 2011 .  ^  M. J. Therien, W. C. Trogler, R. Silva E M. Y. Darensbourg, Bis(phosphine) derivatives of iron pentacarbonyl and tetracarbonyl(tri-tert-butylphosphine)iron(0) , in Inorg. Synth. , vol. 28, 1990, pp. 173\u2013179, two: 10.1002\/9780470132593.ch45 . URL consulted on January 31, 2011 .  ^  R. L. Keiter, E. A. Keiter, C. A. Boecker, D. R. Miller, K. hecker, G. B. Kauffman, J. D Tricarbonylbis(Phosphine)Iron(0) Complexes , in Inorg. Synth. , vol. 31, 1997, pp. 210-214, two: 10.1002\/9780470132623.ch31 . URL consulted on January 31, 2011 .  ^  R. G. Finke e T. N. Sorrell, Nucleophilic acylation with disodium tetracarbonylferrate: methyl 7-oxoheptanoate and methyl 7-oxooctonoate , in Org. Synth. , vol.\u00a059, 1979,  p.\u00a0102. URL consulted on January 31, 2011  (archived by URL Original on June 5, 2011) .  ^  ( OF ) W. Hieber E F. Leutert, To the knowledge of the coordinatively bound carbon oxide: formation of iron carbonyly substances , in Natural Sciences , vol. 19, n. 17, 1931-04, pp. 360\u2013361, DOI: 10.1007\/bf01522286 . URL consulted on December 5, 2021 .  ^  ( IN ) Peter Rittmeyer e Ulrich Wietelmann, Hydrides , Wiley-Vch Verlag Gmbh & Co. Kgaa, 15 GUGNO 2000, pp. A13_199, DOI: 10.1002\/14356007.A13_199 , ISBN\u00a0978-3-527-30673-2. URL consulted on December 5, 2021 .  ^  ( IN ) E. A. McNNeilley a F. R. Scots, Molecular structure of the gaseous metal carbonyl hydrides of manganese, iron, and cobalt , in Journal of the American Chemical Society , vol. 99, n. 19, 1977-09, pp. 6243\u20136249, DOI: 10.1021\/Ja00461A011 . URL consulted on December 5, 2021 .  ^  Arthur A. Blanchard, George W. Coleman e C. M. Mason, Iron Tetracarbonyl Dihydride , John Wiley & Sons, Inc., 5 January 2007, pp. 243\u2013244, doi: 10.1002\/9780470132333.ch77 , ISBN\u00a0978-0-470-13233-3. URL consulted on December 5, 2021 .  ^  R. Pettit e J. Henery, Cyclobutadieneiron tricarbonyl , in Org. Synth. , vol.\u00a050, 1970,  p.\u00a021. URL consulted on January 31, 2011 .  ^  A. J. Birch e K. B. Chamberlain, Tricarbonyl((2,3,4,5-\u03b7)-2,4-cyclohexadien-1-one)iron and tricarbonyl((1,2,3,4,5-\u03b7)-2-methoxy-2,4-cyclohexadien-1-yl)iron(1+) hexafluorophosphate(1-) from anisole , in Org. Synth. , vol.\u00a057, 1977,  p.\u00a0107. URL consulted on January 31, 2011  (archived by URL Original on June 5, 2011) .  ^  At room temperature, the Cyclopentadiene is in a balance of balance with its Dimero (Diels-Alder).  ^   G. Girolami, T. Rauchfuss e R. Angelic, Synthesis and technique in inorganic chemistry , 3 to ed., sarusalito: University Science Books, 1999, ISBN 978-0-935702-48-4   ^  Dieter Rehder, HETERONUCLEAR NMR APPLICATIONS (SC\u2013ZN) , in J. Lindon (the care of), Encyclopedia of Spectroscopy and Spectrometry , vol.\u00a01, Elsevier,  p.\u00a0731, ISBN\u00a00-12-226680-3.  ^  G. Lask e H. G. Wagner, Influence of additives on the velocity of laminar flames , in Eighth International Symposium on Combustion , 1962,  pp.\u00a0432\u2013438.   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