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{{Chembox {{Chembox
| Verifiedfields = changed
⚫ | verifiedrevid = 385929346
| Watchedfields = changed
⚫ | verifiedrevid = 424305424
| ImageFile = Nitrosonium-tetrafluoroborate-2D.png | ImageFile = Nitrosonium-tetrafluoroborate-2D.png
| ImageSize =
| ImageAlt =
| IUPACName = nitrosonium tetrafluoroborate | IUPACName = nitrosonium tetrafluoroborate
| PIN =
| OtherNames = nitrosyl tetrafluoroborate | OtherNames = nitrosyl tetrafluoroborate
| Section1 = {{Chembox Identifiers |Section1={{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 14635-75-7
| PubChem = 151929 | CASNo = 14635-75-7
| UNII_Ref = {{fdacite|correct|FDA}}
| SMILES = }}
| UNII = B99S282SUJ
⚫ | Section2 = {{Chembox Properties
| PubChem = 151929
⚫ | N = 1 | O = 1 | B = 1 | F = 4
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
⚫ | Appearance = colourless crystalline solid
| ChemSpiderID = 9312255
⚫ | Density = 2.185 g&nbsp;cm<sup>−3</sup>
| SMILES = (F)(F)(F)F.N#
| MeltingPt = 250&nbsp;°C (sublimes)
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| BoilingPt =
| StdInChI = 1S/BF4.NO/c2-1(3,4)5;1-2/q-1;+1
⚫ | Solubility = decomposes }}
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| Section3 = {{Chembox Hazards
| StdInChIKey = KGCNVGDHOSFKFT-UHFFFAOYSA-N }}
| MainHazards =
⚫ |Section2={{Chembox Properties
| FlashPt =
⚫ | N=1 | O=1 | B=1 | F=4
| Autoignition = }}
⚫ | Appearance = colourless crystalline solid
⚫ | Density = 2.185 g&nbsp;cm<sup>−3</sup>
| MeltingPtC = 250
| MeltingPt_notes = (sublimes)
⚫ | Solubility = decomposes}}
}} }}


'''Nitrosonium tetrafluoroborate''', also called '''nitrosyl tetrafluoroborate''', is a ] with the ] NOBF<sub>4</sub>. This colourless solid finds use in ] as a ].<ref>{{ cite web | url = http://www.alfa.com/en/GP100W.pgm?DSSTK=A15806 | title = A15806 Nitrosonium tetrafluoroborate, 98% | work = ] website | accessdate = 2010-09-04 }}</ref> '''Nitrosonium tetrafluoroborate''', also called '''nitrosyl tetrafluoroborate''', is a ] with the ] NOBF<sub>4</sub>. This colourless solid is used in ] as a ], ] and a mild oxidant.<ref>{{Citation |last=Olah |first=George A. |title=Nitrosonium Tetrafluoroborate |date=2004-10-15 |work=Encyclopedia of Reagents for Organic Synthesis |editor-last=John Wiley & Sons, Ltd |url=https://onlinelibrary.wiley.com/doi/10.1002/047084289X.rn058.pub2 |access-date=2024-11-27 |place=Chichester, UK |publisher=John Wiley & Sons, Ltd |language=en |doi=10.1002/047084289x.rn058.pub2 |isbn=978-0-471-93623-7 |last2=Surya Prakash |first2=G. K. |last3=Wang |first3=Qi |last4=Li |first4=Xing-ya |last5=Surya Prakash |first5=G. K. |last6=Hu |first6=Jinbo}}</ref>


NOBF<sub>4</sub> is the ] of ], and is composed of a ] ], <sup>+</sup>, and a ] ], <sup>−</sup>. NOBF<sub>4</sub> is the ] of ], and is composed of a ] ], <sup>+</sup>, and a ] ], <sup>−</sup>.<ref>{{Cite journal |last=Lozinšek |first=Matic |date=2021-11-28 |title=Nitrosonium tetrafluoridoborate, NOBF4 |url=https://scripts.iucr.org/cgi-bin/paper?S2414314621012153 |journal=IUCrData |volume=6 |issue=11 |doi=10.1107/S2414314621012153 |issn=2414-3146 |pmc=9462292 |pmid=36337464}}</ref>


==Reactions== ==Reactions==
The dominant property of NOBF<sub>4</sub> is the oxidizing power and electrophilic character of the nitrosonium cation. It forms colored ]es with hexamethylbenzene and with ]. The latter, a deep yellow species, provides a means to dissolve NOBF<sub>4</sub> in dichloromethane.<ref>{{cite journal |doi=10.1021/ic00346a008|title=Redox equilibria of the nitrosonium cation and of its nonbonded complexes|year=1990|last1=Lee|first1=K. Y.|last2=Kuchynka|first2=D. J.|last3=Kochi|first3=Jay K.|journal=Inorganic Chemistry|volume=29|issue=21|pages=4196–4204}}</ref>
⚫ Nitrosonium tetrafluoroborate may be used to prepare metal salts of the type <sub>2</sub> (M = Cr, Mn, Fe, Co, Ni, Cu). The nitrosonium cation acts as the oxidizer, itself being reduced to nitric oxide gas:<ref>{{cite journal | doi = 10.1002/0471224502.ch2 | journal = ] | volume = 33 | pages = 75–83 | title = 11. Homoleptic Transition Metal Acetonitrile Cations with Tetrafluoroborate or Trifluoromethanesulfonate Anions | author = Robert A. Heintz, Jennifer A. Smith, Paul S. Szalay, Amy Weisgerber, And Kim R. Dunbar}}</ref> With ] the ] is formed.<ref>{{cite journal | title = Solvent and electrolyte effects on the kinetics of ferrocenium-ferrocene self-exchange. A reevaluation | author = Roger M. Nielson, George E. McManis, Lance K. Safford, Michael J. Weaver | journal = ] | doi = 10.1021/j100342a086 | year = 1989 | volume = 93 | issue = 5 | pages = 2152}}</ref>


⚫ Nitrosonium tetrafluoroborate may be used to prepare metal salts of the type <sub>2</sub> (M = Cr, Mn, Fe, Co, Ni, Cu). The nitrosonium cation acts as the oxidizer, itself being reduced to nitric oxide gas:<ref>{{cite journal | doi = 10.1002/0471224502.ch2 | journal = ] | volume = 33 | pages = 75–83 | title = 11. Homoleptic Transition Metal Acetonitrile Cations with Tetrafluoroborate or Trifluoromethanesulfonate Anions | first1=Robert A. | last1=Heintz | first2=Jennifer A. | last2=Smith | first3=Paul S. | last3=Szalay | first4=Amy | last4=Weisgerber | first5=Kim R. | last5=Dunbar | date=August 2004 | isbn=978-0-471-46075-6}}</ref>


: M + NOBF<sub>4</sub> + ''x''CH<sub>3</sub>CN &rarr; (BF<sub>4</sub>)<sub>2</sub> + NO : {{chem2|M + 2NOBF4 + ''x''CH3CN → (BF4)2 + 2NO}}

With ] the ] is formed.<ref>{{cite journal | title = Solvent and electrolyte effects on the kinetics of ferrocenium-ferrocene self-exchange. A reevaluation |author1=Roger M. Nielson |author2=George E. McManis |author3=Lance K. Safford |author4=Michael J. Weaver | journal = ] | doi = 10.1021/j100342a086 | year = 1989 | volume = 93 | issue = 5 | pages = 2152}}</ref>

In its ] of this salt, ν<sub>NO</sub> is a strong peak at 2387 cm<sup>−1</sup>.<ref>{{cite journal |doi=10.1039/JR9630003557 |title=670. The Infrared Spectrum of the Nitrosonium Ion |date=1963 |last1=Sharp |first1=D. W. A. |last2=Thorley |first2=J. |journal=Journal of the Chemical Society (Resumed) |page=3557 }}</ref>


==References== ==References==
{{reflist}} {{reflist}}
{{Tetrafluoroborates}}

⚫ {{inorganic-compound-stub}}


] ]
] ]


⚫ {{inorganic-compound-stub}}

Latest revision as of 21:17, 27 November 2024

Nitrosonium tetrafluoroborate
Names
IUPAC name nitrosonium tetrafluoroborate
Other names nitrosyl tetrafluoroborate
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.035.148 Edit this at Wikidata
PubChem CID
UNII
CompTox Dashboard (EPA)
InChI
  • InChI=1S/BF4.NO/c2-1(3,4)5;1-2/q-1;+1Key: KGCNVGDHOSFKFT-UHFFFAOYSA-N
SMILES
  • (F)(F)(F)F.N#
Properties
Chemical formula BF4NO
Molar mass 116.81 g·mol
Appearance colourless crystalline solid
Density 2.185 g cm
Melting point 250 °C (482 °F; 523 K) (sublimes)
Solubility in water decomposes
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). ☒N verify (what is  ?) Infobox references
Chemical compound

Nitrosonium tetrafluoroborate, also called nitrosyl tetrafluoroborate, is a chemical compound with the chemical formula NOBF4. This colourless solid is used in organic synthesis as a nitrosating agent, diazotizing agent and a mild oxidant.

NOBF4 is the nitrosonium salt of fluoroboric acid, and is composed of a nitrosonium cation, , and a tetrafluoroborate anion, .

Reactions

The dominant property of NOBF4 is the oxidizing power and electrophilic character of the nitrosonium cation. It forms colored charge transfer complexes with hexamethylbenzene and with 18-crown-6. The latter, a deep yellow species, provides a means to dissolve NOBF4 in dichloromethane.

Nitrosonium tetrafluoroborate may be used to prepare metal salts of the type 2 (M = Cr, Mn, Fe, Co, Ni, Cu). The nitrosonium cation acts as the oxidizer, itself being reduced to nitric oxide gas:

M + 2NOBF4 + xCH3CN → [M(CH3CN)x](BF4)2 + 2NO

With ferrocene the ferrocenium tetrafluoroborate is formed.

In its infrared spectrum of this salt, νNO is a strong peak at 2387 cm.

References

  1. Olah, George A.; Surya Prakash, G. K.; Wang, Qi; Li, Xing-ya; Surya Prakash, G. K.; Hu, Jinbo (2004-10-15), John Wiley & Sons, Ltd (ed.), "Nitrosonium Tetrafluoroborate", Encyclopedia of Reagents for Organic Synthesis, Chichester, UK: John Wiley & Sons, Ltd, doi:10.1002/047084289x.rn058.pub2, ISBN 978-0-471-93623-7, retrieved 2024-11-27
  2. Lozinšek, Matic (2021-11-28). "Nitrosonium tetrafluoridoborate, NOBF4". IUCrData. 6 (11). doi:10.1107/S2414314621012153. ISSN 2414-3146. PMC 9462292. PMID 36337464.
  3. Lee, K. Y.; Kuchynka, D. J.; Kochi, Jay K. (1990). "Redox equilibria of the nitrosonium cation and of its nonbonded complexes". Inorganic Chemistry. 29 (21): 4196–4204. doi:10.1021/ic00346a008.
  4. Heintz, Robert A.; Smith, Jennifer A.; Szalay, Paul S.; Weisgerber, Amy; Dunbar, Kim R. (August 2004). "11. Homoleptic Transition Metal Acetonitrile Cations with Tetrafluoroborate or Trifluoromethanesulfonate Anions". Inorg. Synth. 33: 75–83. doi:10.1002/0471224502.ch2. ISBN 978-0-471-46075-6.
  5. Roger M. Nielson; George E. McManis; Lance K. Safford; Michael J. Weaver (1989). "Solvent and electrolyte effects on the kinetics of ferrocenium-ferrocene self-exchange. A reevaluation". J. Phys. Chem. 93 (5): 2152. doi:10.1021/j100342a086.
  6. Sharp, D. W. A.; Thorley, J. (1963). "670. The Infrared Spectrum of the Nitrosonium Ion". Journal of the Chemical Society (Resumed): 3557. doi:10.1039/JR9630003557.
Salts and covalent derivatives of the tetrafluoroborate ion
HBF4 He
LiBF4 Be B C7H7BF4
BF4
BF4
(TEDA)BF4 		NOBF4
NO2BF4
NH4BF4 		O F Ne
NaBF4 Mg(BF4)2 Al Si P S Cl Ar
KBF4 Ca(BF4)2 Sc Ti V (BF4)3
(BF4)2 		Mn(BF4)2 Fe(BF4)2
FeO(BF4)2
BF4 		Co(BF4)2 Ni(BF4)2
(BF4)2 		Cu(BF4)2 Zn(BF4)2 Ga Ge As Se Br Kr
RbBF4 Sr(BF4)2 Y Zr Nb (BF4)4
(BF4)4 		(BF4)4 (BF4)2 (BF4)3
(BF4)4 		(BF4)2 AgBF4 Cd(BF4)2 In(BF4)3 Sn(BF4)2 Sb Te (IPy2)BF4 Xe
CsBF4 Ba(BF4)2 * Lu Hf Ta W Re Os Ir Pt(BF4)2 Au Hg(BF4)2 TlBF4 Pb(BF4)2 Bi Po At Rn
Fr Ra ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb
** Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No


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