Perchloryl fluoride
Structural formula | |||||||||||||||||||
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General | |||||||||||||||||||
Surname | Perchloryl fluoride | ||||||||||||||||||
other names |
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Molecular formula | ClFO 3 | ||||||||||||||||||
Brief description |
colorless gas with a sweet smell |
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External identifiers / databases | |||||||||||||||||||
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properties | |||||||||||||||||||
Molar mass | 102.45 g · mol -1 | ||||||||||||||||||
Physical state |
gaseous |
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density |
1.39 g cm −3 |
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Melting point |
−146 ° C |
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boiling point |
−46.8 ° C |
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Vapor pressure |
1.04 M Pa (20 ° C) |
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solubility |
bad in water (0.6 g l −1 ) |
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safety instructions | |||||||||||||||||||
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MAK |
Switzerland: 3 ml m −3 or 13 mg m −3 |
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Toxicological data | |||||||||||||||||||
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Perchloryl fluoride (FClO 3 ) is a colorless, poisonous gas with an unpleasant odor, which is easily condensable ( boiling point approx. −47 ° C). Chemically it is the acid fluoride of perchloric acid . The chlorine is in its highest oxidation state + VII.
Manufacturing
Perchloryl fluoride can be obtained by fluorinating potassium chlorate with fluorine in antimony pentafluoride at −20 ° C or by reacting potassium perchlorate with fluorosulfonic acid . It can also be produced by reacting solid alkali metal fluorides (esp. CsF) with dichloroheptoxide (Cl 2 O 7 ).
It is also possible to display it by reacting potassium perchlorate with fluorosulfonic acid :
or by reacting potassium perchlorate with hydrogen fluoride and antimony (V) fluoride:
properties
Perchloryl fluoride is resistant up to over 400 ° C. It has a strong oxidising ( oxidizing ) and responds, v. a. when heated, violently with reducing agents . Many coating materials, plastics and rubber are also attacked. It reacts slowly with water , depending on the pH , to form perchloric and hydrofluoric acid .
The compound is suitable for the synthesis of (mostly explosive ) organic derivatives of perchloric acid. Perchloric acid esters can thus be produced by reaction with alcoholates ; with phenyllithium (C 6 H 5 Li), perchlorylbenzene C 6 H 5 ClO 3 is obtained . The reaction is explosive with pure sodium methylate . Perchlorylamides R (R ') N-ClO 3 can form with ammonia and amines , which have an acidic effect in the case of unsubstituted NH bonds.
safety instructions
In guinea pigs, inhalation of 220 mg m −3 perchloryl fluoride led to fibrosis of connective tissue in the lungs and chronic obstructive pulmonary disease as well as a reduction in the number of erythrocytes and the production of methaemoglobin in the blood.
Individual evidence
- ↑ a b c d e f g Entry on perchloryl fluoride in the GESTIS substance database of the IFA , accessed on July 30, 2013 (JavaScript required)
- ↑ Swiss Accident Insurance Fund (Suva): Limit values - current MAK and BAT values (search for 7616-94-6 or perchloryl fluoride ), accessed on November 2, 2015.
- ↑ a b c Entry on perchloryl fluoride in the ChemIDplus database of the United States National Library of Medicine (NLM)
- ↑ a b Spravochnik po Toksikologii i Gigienicheskim Normativam , Pg. 199, 1999.
- ↑ a b Penn Salt Chemicals Corp., Technical Div., New Products.
- ^ A b c A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , p. 491.
- ↑ Georg Brauer (Ed.), With the collaboration of Marianne Baudler a . a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 180.
- ↑ CA Wamser et al .: Perchloryl fluoride . In: Aaron Wold and John K. Ruff (Eds.): Inorganic Syntheses . tape 14 . McGraw-Hill Book Company, Inc., 1973, ISBN 07-071320-0 ( defective ) , p. 29-33 (English).
- ↑ a b L. Roth, U. Weller-Schäferbarthold: Hazardous chemical reactions - Potentially dangerous chemical reactions to over 1750 substances , entry for perchloryl fluoride, CD-ROM edition 4/2019, ecomed Sicherheit Landsberg / Lech, ISBN 978-3-609 -48040-4 .
- ↑ Cotton-Wilkinson, Inorganic Chemistry, 3rd Edition, Verlag Chemie 1974 ISBN 3-527-25503-6 .