Nickel tetracarbonyl

In nickel tetracarbonyl, the oxidation state for nickel is assigned as zero, because the Ni−C bonding electrons come from the C atom and are still assigned to C in the hypothetical ionic bond which determines the oxidation states. The formula conforms to the 18-electron rule. The molecule is tetrahedral, with four carbonyl (carbon monoxide) ligands. Electron diffraction studies have been performed on this molecule, and the Ni−C and C−O distances have been calculated to be 1.838(2) and 1.141(2) angstroms respectively.{{ cite journal | last1 = Hedberg | first1 = L. | last2 = Iijima | first2 = T. | last3 = Hedberg | first3 = K. | title = Nickel tetracarbonyl, Ni(CO)₄. I. Molecular Structure by Gaseous Electron Diffraction. II. Refinement of Quadratic Force Field | journal = The Journal of Chemical Physics | year = 1979 | volume = 70 | issue = 7 | pages = 3224–3229 | doi = 10.1063/1.437911 | bibcode = 1979JChPh..70.3224H }}

Ni(CO)₄ was first synthesised in 1890 by Ludwig Mond by the direct reaction of nickel metal with carbon monoxide.{{ cite journal | last1= Mond|first1= L. |last2 = Langer|first2= C.| last3= Quincke|first3= F.| author-link1 = Ludwig Mond | title = Action of Carbon Monoxide on Nickel | journal = J. Chem. Soc. Trans. | year = 1890 | volume = 57 | pages = 749–753 | doi = 10.1039/CT8905700749 |url= https://zenodo.org/record/2160347 }} This pioneering work foreshadowed the existence of many other metal carbonyl compounds, including those of vanadium, chromium, manganese, iron, and cobalt. It was also applied industrially to the purification of nickel by the end of the 19th century.{{ cite journal | journal = Nature | title = The Extraction of Nickel from its Ores by the Mond Process | year = 1898 | volume = 59 | issue = 1516 | pages = 63–64 | doi = 10.1038/059063a0 | bibcode = 1898Natur..59...63. | doi-access = free }}

At {{convert|323|K|C F}}, carbon monoxide is passed over impure nickel. The optimal rate occurs at 130 °C.{{ Ullmann | author = Lascelles, K. | author2 = Morgan, L. G. | author3 = Nicholls, D. | author4 = Beyersmann, D. | title = Nickel Compounds | doi = 10.1002/14356007.a17_235.pub2 }}

Ni(CO)₄ is not readily available commercially. It is conveniently generated in the laboratory by carbonylation of commercially available bis(cyclooctadiene)nickel(0).{{cite encyclopedia|first=P. W. |last=Jolly |title=Nickel Tetracarbonyl |encyclopedia=Comprehensive Organometallic Chemistry |volume=I |editor1-first=Edward W. |editor1-last=Abel |editor2-link=F. Gordon A. Stone|editor2-first=F. Gordon A. |editor2-last=Stone |editor3-link=Geoffrey Wilkinson|editor3-first=Geoffrey|editor3-last=Wilkinson |date=1982 |publisher=Pergamon Press |location=Oxford |isbn= 0-08-025269-9}} It can also be prepared by reduction of ammoniacal solutions of nickel sulfate with sodium dithionite under an atmosphere of CO.{{cite book|author=F. Seel|chapter=Nickel Carbonyl|title=Handbook of Preparative Inorganic Chemistry|edition=2nd |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY|volume=2|pages=1747–1748}}

File:Nickel kugeln.jpg

On moderate heating, Ni(CO)₄ decomposes to carbon monoxide and nickel metal. Combined with the easy formation from CO and even very impure nickel, this decomposition is the basis for the Mond process for the purification of nickel or plating onto surfaces. Thermal decomposition commences near {{convert|180|C}} and increases at higher temperature.

Like other low-valent metal carbonyls, Ni(CO)₄ is susceptible to attack by nucleophiles. Attack can occur at nickel center, resulting in displacement of CO ligands, or at CO. Thus, donor ligands such as triphenylphosphine react to give {{chem2|Ni(CO)3(PPh3)}} and {{chem2|Ni(CO)2(PPh3)2}}. Bipyridine and related ligands behave similarly.{{ cite book | last1 = Elschenbroich |first1=C. | last2 = Salzer |first2=A. | title = Organometallics: A Concise Introduction | edition = 2nd | year = 1992 | publisher = Wiley-VCH | location = Weinheim | isbn = 3-527-28165-7 }} The monosubstitution of nickel tetracarbonyl with other ligands can be used to determine the Tolman electronic parameter, a measure of the electron donating or withdrawing ability of a given ligand.

:File:NiP2(CO)2.svg

Treatment with hydroxides gives clusters such as {{chem2|[Ni5(CO)12](2−)}} and {{chem2|[Ni6(CO)12](2−)}}. These compounds can also be obtained by reduction of nickel carbonyl.

Thus, treatment of Ni(CO)₄ with carbon nucleophiles (Nu⁻) results in acyl derivatives such as {{chem2|[Ni(CO)3C(O)Nu)]−}}.{{ cite encyclopedia | encyclopedia = Encyclopedia of Reagents for Organic Synthesis | year = 2003 | publisher = John Wiley & Sons | last= Pinhas|first= A. R. | doi = 10.1002/047084289X.rt025m | chapter= Tetracarbonylnickel | isbn = 0471936235 }}

Nickel carbonyl can be oxidized. Chlorine oxidizes nickel carbonyl into NiCl₂, releasing CO gas. Other halogens behave analogously. This reaction provides a convenient method for precipitating the nickel portion of the toxic compound.

Reactions of Ni(CO)₄ with alkyl and aryl halides often result in carbonylated organic products. Vinylic halides, such as PhCH=CHBr, are converted to the unsaturated esters upon treatment with Ni(CO)₄ followed by sodium methoxide. Such reactions also probably proceed via oxidative addition. Allylic halides give the π-allylnickel compounds, such as {{chem2|(allyl)2Ni2Cl2}}:{{ OrgSynth | author = Semmelhack, M. F. | author2 = Helquist, P. M. | title = Reaction of Aryl Halides with π-Allylnickel Halides: Methallylbenzene | year = 1972 | volume = 52 | pages = 115 | collvol = 6 | collvolpages = 722 | prep = cv6p0722 }}

{{chem2|2 Ni(CO)4 + 2 ClCH2CH\dCH2 -> Ni2 (μ\-Cl)2(\h{3}C3H5)2 + 8 CO}}

The hazards of Ni(CO)₄ are far greater than that implied by its CO content, reflecting the effects of the nickel if released in the body. Nickel carbonyl may be fatal if absorbed through the skin or more likely, inhaled due to its high volatility. Its LC₅₀ for a 30-minute exposure has been estimated at 3 ppm, and the concentration that is immediately fatal to humans would be 30 ppm. Some subjects exposed to puffs up to 5 ppm described the odour as musty or sooty, but because the compound is so exceedingly toxic, its smell provides no reliable warning against a potentially fatal exposure.{{ cite book | chapter-url = http://books.nap.edu/openbook.php?record_id=12018&page=159 | title = Acute Exposure Guideline Levels for Selected Airborne Chemicals | volume = 6 | year = 2008 | author = Board on Environmental Studies and Toxicology | publisher = National Academies Press | pages = 213–259 | chapter = Nickel Carbonyl: Acute Exposure Guideline Levels | doi = 10.17226/12018 | pmid = 25032325 | isbn = 978-0-309-11213-0 }}

The vapours of Ni(CO)₄ can autoignite. The vapor decomposes quickly in air, with a half-life of about 40 seconds.{{ cite journal | last1= Stedman|first1= D. H. | last2 = Hikade|first2= D. A. | last3 = Pearson |first3=R. Jr. | author4 = Yalvac, E. D. | title = Nickel Carbonyl: Decomposition in Air and Related Kinetic Studies | journal = Science | year = 1980 | volume = 208 | issue = 4447 | pages = 1029–1031 | doi = 10.1126/science.208.4447.1029 | pmid = 17779026 |bibcode= 1980Sci...208.1029S |s2cid= 31344783 }}

Nickel carbonyl poisoning is characterized by a two-stage illness. The first consists of headaches and chest pain lasting a few hours, usually followed by a short remission. The second phase is a chemical pneumonitis which starts after typically 16 hours with symptoms of cough, breathlessness and extreme fatigue. These reach greatest severity after four days, possibly resulting in death from cardiorespiratory or acute kidney injury. Convalescence is often extremely protracted, often complicated by exhaustion, depression and dyspnea on exertion. Permanent respiratory damage is unusual. The carcinogenicity of Ni(CO)₄ is a matter of debate, but is presumed to be significant.

It is classified as an extremely hazardous substance in the United States as defined in Section 302 of the U.S. Emergency Planning and Community Right-to-Know Act (42 U.S.C. 11002), and is subject to strict reporting requirements by facilities which produce, store, or use it in significant quantities.{{Cite web| publisher = Government Printing Office | title = 40 C.F.R.: Appendix A to Part 355—The List of Extremely Hazardous Substances and Their Threshold Planning Quantities | url = http://edocket.access.gpo.gov/cfr_2008/julqtr/pdf/40cfr355AppA.pdf | edition = July 1, 2008 | access-date = October 29, 2011 | archive-url = https://web.archive.org/web/20120225051612/http://edocket.access.gpo.gov/cfr_2008/julqtr/pdf/40cfr355AppA.pdf | archive-date = February 25, 2012 | url-status = dead }}

"Requiem for the Living" (1978), an episode of Quincy, M.E., features a poisoned, dying crime lord who asks Dr. Quincy to autopsy his still-living body. Quincy identifies the poison—nickel carbonyl.

In the 1979 novella Amanda Morgan by Gordon R. Dickson, the remaining inhabitants of a mostly evacuated village resist an occupying military force by directing the exhaust from a poorly-tuned internal combustion engine onto a continually renewed "waste heap" of powdered nickel outside a machine shop (under the guise of civilian business) in order to eliminate the occupiers, at the cost of their own lives.

In chapter 199 of the manga Dr. Stone, a machine is made that purifies nickel via the Mond Process. It is mentioned that the process creates a "fatal toxin" (nickel carbonyl).

In the 2019 novel Delta-v from New York Times bestselling author Daniel Suarez a team of eight private miners reach a near-earth asteroid to extract volatiles (water, CO₂, etc.) and metals (iron, nickel and cobalt); these are stored as solid carbonyl for transfer back to near Earth orbit, and used for in-situ fabrication of a spacecraft, via decomposition in vacuum.

{{Reflist}}

• {{ cite journal | last= Shi|first= Z. | title = Nickel Carbonyl: Toxicity and Human Health | journal = Science of the Total Environment | year = 1991 | volume = 148 | issue = 2–3 | pages = 293–298 | pmid = 8029705 | doi = 10.1016/0048-9697(94)90406-5 }}
• {{ cite journal | last= Sunderman|first= F. W. | title = A Pilgrimage into the Archives of Nickel Toxicology | journal = Annals of Clinical and Laboratory Science | year = 1989 | volume = 19 | issue = 1 | pages = 1–16 | pmid = 2644888 }}
• {{ cite journal | last=Armit|first= H. W. | title = The Toxicology of Nickel Carbonyl. Part I | journal = Journal of Hygiene | year = 1907 | volume = 7 | issue = 4 | pages = 525–551 | pmid = 20474327 | pmc = 2236193 | doi = 10.1017/S0022172400033507 }}
• {{ cite journal | last= Armit|first= H. W. | title = The Toxicology of Nickel Carbonyl. Part II | journal = Journal of Hygiene | year = 1908 | volume = 8 | issue = 5 | pages = 565–610 | pmid = 20474374 | pmc = 2167169 | doi = 10.1017/S0022172400015989 }}
• {{ cite journal | last1= Barceloux|first1= D. G. | last2 = Barceloux | first2 = Donald | title = Nickel | journal = Clinical Toxicology | year = 1999 | volume = 37 | issue = 2 | pages = 239–258 | pmid = 10382559 | doi = 10.1081/CLT-100102423 }}

• [http://www.inchem.org/documents/icsc/icsc/eics0064.htm International Chemical Safety Card 0064]
• [https://web.archive.org/web/20060820041610/http://www.npi.gov.au/database/substance-info/profiles/63.html National Pollutant Inventory – Nickel carbonyl fact sheet]
• [https://www.cdc.gov/niosh/npg/npgd0444.html NIOSH Pocket Guide to Chemical Hazards]
• [https://web.archive.org/web/20081224153750/http://monographs.iarc.fr/ENG/Monographs/vol49/volume49.pdf IARC Monograph "Nickel and Nickel compounds"]

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Category:Organonickel compounds

Category:Nickel compounds

Category:Carbonyl complexes

Category:IARC Group 1 carcinogens

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