Iodine trifluoride

Structural formula
General
Surname	Iodine trifluoride
other names	Iodine (III) fluoride
Molecular formula	IF 3
Brief description	yellow solid (−78 ° C)
External identifiers / databases
CAS number 22520-96-3 PubChem 13932268 ChemSpider 10329096 Wikidata Q419600
properties
Molar mass	183.9 g mol −1
Melting point	Decomposition> −28 ° 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 trifluoride is a chemical compound of iodine and fluorine . The interhalogen compound is very unstable as others of this class and is easily decomposed.

history

Iodine trifluoride was first prepared in 1960 by M. Schmeisser from the elements iodine and fluorine.

Extraction and presentation

Iodine trifluoride can be prepared in several ways. In addition to the synthesis from the elements, it is possible to obtain the compound by reacting iodine with xenon (II) fluoride in trichlorofluoromethane .

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

properties

The structure of the IF ₃ molecule can be explained using the VSEPR model . In addition to the three fluorine ligands, the iodine atom also has two free electron pairs . With these, the molecule forms a trigonal bipyramid ; if you only look at the atoms, it appears T-shaped. The axial fluorine-iodine bonds have a length of 198 pm, the equatorial one of 187 pm. The angles between the fluorine atoms are 80.1 °.

Iodine trifluoride is only stable at temperatures below −28 ° C. If it is heated above this temperature, it decomposes into iodine and iodine pentafluoride . Like other interhalogen compounds, iodine trifluoride is a fluorinating agent , but weaker than bromine or chlorine trifluoride .

use

Iodine fluoride can be produced by reacting iodine trifluoride with iodine in trichlorofluoromethane at low temperatures.

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

Individual evidence

1. ↑ iodine trifluoride at Webelements.com .
2. ^ ^{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 , pp. 459-460.
3. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
4. ↑ ^{a b} M. Schmeisser, E. Scharf: About iodine trifluoride JF ₃ and iodine monofluoride JF . In: Angewandte Chemie , 1960, 72, 9, p. 324, doi : 10.1002 / anie.19600720912 .
5. ↑ Thomas M. Klapötke , Inis C. Tornieporth-Oetting: Non-metal chemistry . Wiley-VCH, Weinheim 1994, ISBN 3-527-29257-8 .