Iodine heptafluoride

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Iodine heptafluoride
Structure of iodine heptafluoride(IF7)
Iodine heptafluoride
Iodine heptafluoride
Names
Other names
Iodine(VII) fluoride
Heptafluoroiodine
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.037.241 Edit this at Wikidata
UNII
  • InChI=1S/F7I/c1-8(2,3,4,5,6)7 checkY
    Key: XRURPHMPXJDCOO-UHFFFAOYSA-N checkY
  • InChI=1/F7I/c1-8(2,3,4,5,6)7
    Key: XRURPHMPXJDCOO-UHFFFAOYAO
  • FI(F)(F)(F)(F)(F)F
Properties
Chemical formula
 IF7
Molar mass 259.90 g/mol
Appearance colorless gas
Density 2.6 g/cm3 (6 °C)
2.7 g/cm3 (25 °C)
Melting point 4.5 °C (40.1 °F; 277.6 K) (triple point)
Boiling point 4.8 °C (40.6 °F; 277.9 K) (sublimes at 1 atm)
soluble [1]
Related compounds
Related compounds
 iodine pentafluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Iodine heptafluoride, also known as iodine(VII) fluoride or iodine fluoride, is an interhalogen compound with the chemical formula IF7.[2][3] It has an unusual pentagonal bipyramidal structure, as predicted by VSEPR theory.[4] The molecule can undergo a pseudorotational rearrangement called the Bartell mechanism, which is like the Berry mechanism but for a heptacoordinated system.[5] It forms colourless crystals, which melt at 4.5 °C: the liquid range is extremely narrow, with the boiling point at 4.77 °C. The dense vapor has a mouldy, acrid odour. The molecule has D5h symmetry.

Preparation[]

IF7 is prepared by passing F2 through liquid IF5 at 90 °C, then heating the vapours to 270 °C. Alternatively, this compound can be prepared from fluorine and dried palladium or potassium iodide to minimize the formation of IOF5, an impurity arising by hydrolysis.[6][7] Iodine heptafluoride is also produced as a by-product when dioxygenyl hexafluoroplatinate is used to prepare other platinum(V) compounds such as , using potassium fluoride in iodine pentafluoride solution:[8]

2 O2PtF6 + 2 KF + IF5 → 2 KPtF6 + 2 O2 + IF7

Safety considerations[]

IF7 is highly irritating to both the skin and the mucous membranes. It also is a strong oxidizer and can cause fire on contact with organic material.

References[]

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ Macintyre, J. E. (Ed.). (1992). Dictionary of Inorganic Compounds (Vol. 3). London: Chapman & Hall.
  3. ^ O'Neil, Maryadele J. (Ed.). (2001). The Merck Index (13th ed.). Whitehouse Station, NJ: Merck.
  4. ^ K. O. Christe; E. C. Curtis; D. A. Dixon (1993). "On the problem of heptacoordination: vibrational spectra, structure, and fluxionality of iodine heptafluoride". Journal of the American Chemical Society. 115 (4): 1520–1526. doi:10.1021/ja00057a044.
  5. ^ W. J. Adams; H. Bradford Thompson; L. S. Bartell (1970). "Structure, Pseudorotation, and Vibrational Mode Coupling in IF7: An Electron Diffraction Study" (PDF). Journal of Chemical Physics. 53 (10): 4040–4046. Bibcode:1970JChPh..53.4040A. doi:10.1063/1.1673876. hdl:2027.42/71219.
  6. ^ Schumb, W. C.; Lynch, M. A. (1950). "Iodine Heptafluoride". Industrial & Engineering Chemistry. 42 (7): 1383–1386. doi:10.1021/ie50487a035.
  7. ^ Ruff, O.; Keim, R. (1930). ""Das Jod-7-fluorid" (The iodine-7-fluoride)". Zeitschrift für Anorganische und Allgemeine Chemie (in German). 193 (1/2): 176–186. doi:10.1002/zaac.19301930117.
  8. ^ Beveridge, A. D.; Clark, H. C. (1967). "Pentahalides of the Transition Metals". In Gutmann, Viktor (ed.). Halogen Chemistry. 3. Academic Press. pp. 179–226. ISBN 9780323148474.

External links[]

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