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{{Chembox
| Watchedfields = changed
| verifiedrevid = 448917315
| ImageFileL1 = fluorine-perchlorate-2D.png
| ImageSizeL1 = 130px
| ImageNameL1 = Full structural formula of fluorine perchlorate
| ImageFileR1 = Fluorine-perchlorate-3D-balls.png
| ImageSizeR1 = 110px
| ImageNameR1 = Ball-and-stick model of fluorine perchlorate
| IUPACName = Perchloryl hypofluorite
| OtherNames = Fluorine perchlorate
| Section1 = {{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 10049-03-3
| PubChem =
| SMILES = FOCl(O)(O)O }}
| Section2 = {{Chembox Properties
| Formula = {{chem|FClO|4}}
| MolarMass =
| Appearance =
| Density =
| MeltingPt = -167.3 °C
| BoilingPt = -16 °C
| Solubility = }}
| Section3 = {{Chembox Thermochemistry
| DeltaHf = 9 kcal/mol<ref>Breazeale, J. D.; MacLaren, R. O.. ''Thermochemistry of oxygen-fluorine bonding'', United Technology Center, Sunnyvale, CA, 1963. Accession Number: AD0402889. Retrieved online from [http://oai.dtic.mil/oai/oai?verb=getRecord&metadataPrefix=html&identifier=AD0402889] on 2009-05-21.</ref>}}
| Section4 = {{Chembox Hazards
| MainHazards = Highly explosive gas
| FlashPt =
| Autoignition = }}
}}
 
'''Fluorine perchlorate''' is the rarely encountered [[chemical compound]] of [[fluorine]], [[chlorine]], and [[oxygen]] with the [[chemical formula]] {{chem|FClO|4}} or {{chem|FOClO|3}}. It is an extremely unstable gas that explodes spontaneously<ref>Pradyot Patnaik. ''A comprehensive guide to the hazardous properties of chemical substances'', 3rd ed., Wiley-Interscience, 2007. ISBN 0-471-71458-5</ref> and has a penetrating odor.<ref>Robert Alan Lewis. ''Lewis' dictionary of toxicology'', CRC Press, 1998, p.&nbsp;508. ISBN 1-56670-223-2</ref>
 
== Synthesis ==
 
One synthesis uses fluorine and [[perchloric acid]],<ref>{{cite doi|10.1021/ja01195a063}}</ref> though the action of [[chlorine pentafluoride|ClF<sub>5</sub>]] on water is another method{{Citation needed|date=July 2013}}.
 
:<math>\rm \ F_2 + HClO_4 \rightarrow FClO_4 + HF</math>
 
Another method of synthesis involves the thermal decomposition of [[tetrafluoroammonium]] perchlorate, {{chem|NF|4|ClO|4}}, which yields very pure {{chem|FClO|4}} that may be manipulated and frozen without explosions.<ref>{{cite doi|10.1021/ic50199a056}}</ref>
 
:<math>\rm \ NF_4ClO_4 \xrightarrow{\Delta} NF_3 + FClO_4</math>
 
== Structure ==
 
Fluorine perchlorate is not analogous to perchloric acid because the fluorine atom does not exist as a positive ion. It contains an oxygen atom in a rare [[oxidation state]] of 0, due to the [[electronegativity]] of oxygen, which is higher than that of chlorine but lower than that of fluorine.
 
== Safety ==
 
FClO<sub>4</sub> has a very dangerous and unpredictable series of reactions associated with it, as a covalent perchlorate (chlorine in the +7 oxidation state) and a compound featuring a very sensitive O-F single bond. Small amounts of reducing agent, such as [[organic compounds]], can trigger explosive detonation. Products of these decomposition reactions could include oxygen halides, [[interhalogen]] compounds, and other hazardous substances.
 
Accidental synthesis is possible if precursors are carelessly mixed. Like similar covalent fluorides and perchlorates, it needs to be handled with extreme caution.
 
== Reaction ==
FClO<sub>4</sub> is a strong [[oxidant]] and it reacts with [[iodide]] ion:
 
:FOClO<sub>3</sub> + 2I<sup>-</sup> → ClO<sub>4</sub><sup>-</sup> + F<sup>-</sup> + I<sub>2</sub>
 
FClO<sub>4</sub> can also react with [[tetrafluoroethylene]]:<ref>{{Greenwood&Earnshaw}}</ref>
 
:CF<sub>2</sub>=CF<sub>2</sub> + FOClO<sub>3</sub> → CF<sub>3</sub>CF<sub>2</sub>OClO<sub>3</sub>
 
It may be a [[radical (chemistry)|radical]] [[addition reaction]].
<ref>{{cite journal|doi=10.1021/ic50199a056|title=Reactions of fluorine perchlorate with fluorocarbons and the polarity of the oxygen-fluorine bond in covalent hypofluorites|year=1979|last1=Schack|first1=Carl J.|last2=Christe|first2=Karl O.|journal=Inorganic Chemistry|volume=18|issue=9|pages=2619}}</ref>
 
== References ==
 
{{reflist}}
 
== External links ==
 
* Chemist [[Derek Lowe (chemist)|Derek Lowe]]'s [http://pipeline.corante.com/archives/2006/05/30/things_i_wont_work_with_frisky_perchlorates.php experiences with perchlorates]
 
[[Category:Explosive chemicals]]
[[Category:Perchlorates]]
[[Category:Oxidizing agents]]
 
{{inorganic-compound-stub}}

Revision as of 05:51, 28 August 2013

Template:Chembox

Fluorine perchlorate is the rarely encountered chemical compound of fluorine, chlorine, and oxygen with the chemical formula Template:Chem or Template:Chem. It is an extremely unstable gas that explodes spontaneously[1] and has a penetrating odor.[2]

Synthesis

One synthesis uses fluorine and perchloric acid,[3] though the action of ClF5 on water is another methodPotter or Ceramic Artist Truman Bedell from Rexton, has interests which include ceramics, best property developers in singapore developers in singapore and scrabble. Was especially enthused after visiting Alejandro de Humboldt National Park..

Another method of synthesis involves the thermal decomposition of tetrafluoroammonium perchlorate, Template:Chem, which yields very pure Template:Chem that may be manipulated and frozen without explosions.[4]

Structure

Fluorine perchlorate is not analogous to perchloric acid because the fluorine atom does not exist as a positive ion. It contains an oxygen atom in a rare oxidation state of 0, due to the electronegativity of oxygen, which is higher than that of chlorine but lower than that of fluorine.

Safety

FClO4 has a very dangerous and unpredictable series of reactions associated with it, as a covalent perchlorate (chlorine in the +7 oxidation state) and a compound featuring a very sensitive O-F single bond. Small amounts of reducing agent, such as organic compounds, can trigger explosive detonation. Products of these decomposition reactions could include oxygen halides, interhalogen compounds, and other hazardous substances.

Accidental synthesis is possible if precursors are carelessly mixed. Like similar covalent fluorides and perchlorates, it needs to be handled with extreme caution.

Reaction

FClO4 is a strong oxidant and it reacts with iodide ion:

FOClO3 + 2I- → ClO4- + F- + I2

FClO4 can also react with tetrafluoroethylene:[5]

CF2=CF2 + FOClO3 → CF3CF2OClO3

It may be a radical addition reaction. [6]

References

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External links

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  1. ↑ Pradyot Patnaik. A comprehensive guide to the hazardous properties of chemical substances, 3rd ed., Wiley-Interscience, 2007. ISBN 0-471-71458-5
  2. ↑ Robert Alan Lewis. Lewis' dictionary of toxicology, CRC Press, 1998, p. 508. ISBN 1-56670-223-2
  3. ↑ Template:Cite doi
  4. ↑ Template:Cite doi
  5. ↑ Template:Greenwood&Earnshaw
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