Iodine fluoride

Structural formula
${\displaystyle \mathrm {I{-}F\ } }$
General
Surname	Iodine fluoride
other names	Iodine (I) fluoride Iodine monofluoride Fluoriodine
Molecular formula	IF
Brief description	white powder (at −78 ° C)
External identifiers / databases
CAS number 13873-84-2 PubChem 139637 Wikidata Q419914
properties
Molar mass	145.9 g mol −1
Physical state	solid (below −14 ° C)
Melting point	Decomposes above −14 ° C
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Iodine fluoride is an interhalogen compound that is unstable at room temperature and consists of the elements iodine and fluorine .

Physical Properties

Bond length in IF.

The bond length in the iodine fluoride molecule is about 191 pm.

Chemical properties

Iodine fluoride is a white powder and is only stable at temperatures below −78 ° C. Above −14 ° C the compound disproportionates into elemental iodine (I ₂ ) and iodine pentafluoride (IF ₅ ), a colorless liquid:

${\displaystyle \mathrm {5\;IF\longrightarrow 2\;I_{2}+IF_{5}} }$

Analogous to all other interhalogen compounds, iodine fluoride reacts with water to form hydrogen halide , in this case hydrogen fluoride (HF), and hypohalous acid , in this case hypoiodous acid (HOI):

${\displaystyle \mathrm {IF+H_{2}O\longrightarrow HF+HOI} }$

Iodine fluoride is to be classified as toxic in analogy to more stable interhalogen compounds.

Of all the interhalogens, it has the greatest tendency to decay, even at very low temperatures. Therefore an exact determination of the physical properties is not possible.

presentation

Iodine fluoride can be represented at low temperatures from the elements:

${\displaystyle \mathrm {I_{2}+F_{2}\longrightarrow 2\;IF} }$

However, the direct reaction of the elements leads to continuing leading fluorination of Iodfluorids easy to iodine trifluoride .

It can also be obtained by reducing iodine trifluoride with elemental iodine in a trichlorofluoromethane suspension in the presence of a catalytic amount of an organic N-base ( pyridine , acetonitrile ) at -40 ° C.

${\displaystyle \mathrm {IF_{3}+I_{2}\longrightarrow 3\ IF} }$

It cannot practically be made pure, and the detection of the compound is very difficult. Therefore most of the properties are unknown. It may have a polymeric structure.

Individual evidence

1. ^ ^{A b} A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 .
2. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
3. ↑ Sevim Hoyer, Structural Chemistry of Iodine Compounds in the Oxidation Levels +1/7 to +5, Dissertation at the Free University of Berlin .
4. ↑ 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. 171.

literature

• D. Naumann: Fluorine and fluorine compounds , Steinkopff-Verlag, Darmstadt, 1980
• WKR Musgrave: The Halogen Fluorides; their Preparation and Uses in Organic Chemistry , Adv. Fluorine Chem. 1 (1960)
• EH Wiebenga, EE Havinga, KH Boswijk: Structures of Interhalogen Compounds and Polyhalides , Adv. Inorg. Radiochem. 3 (1961)