Iodine heptafluoride

Iodine heptafluoride
Names
	Other names Iodine(VII) fluoride; Heptafluoroiodine
Identifiers
CAS Number	16921-96-3 ;
3D model (JSmol)	Interactive image;
ChemSpider	21477354 ;
PubChem CID	85645;
UNII	M080M03ILM ;
	InChI InChI=1S/F7I/c1-8(2,3,4,5,6)7 Key: XRURPHMPXJDCOO-UHFFFAOYSA-N ; InChI=1/F7I/c1-8(2,3,4,5,6)7 Key: XRURPHMPXJDCOO-UHFFFAOYAO;
	SMILES 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)
Solubility in water	soluble
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, is an interhalogen compound with the chemical formula I F₇.^[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 D_5h 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 potassium hexafluoroplatinate(V), using potassium fluoride in iodine pentafluoride solution:^[8]

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

Reactions

Iodine heptafluoride decomposes at 200 °C to fluorine gas and iodine pentafluoride.^[9]

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

↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN:0-07-049439-8
↑ Macintyre, J. E. (Ed.). (1992). Dictionary of Inorganic Compounds (Vol. 3). London: Chapman & Hall.
↑ O'Neil, Maryadele J. (Ed.). (2001). The Merck Index (13th ed.). Whitehouse Station, NJ: Merck.
↑ 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.
↑ W. J. Adams; H. Bradford Thompson; L. S. Bartell (1970). "Structure, Pseudorotation, and Vibrational Mode Coupling in IF₇: An Electron Diffraction Study". Journal of Chemical Physics 53 (10): 4040–4046. doi:10.1063/1.1673876. Bibcode: 1970JChPh..53.4040A. https://deepblue.lib.umich.edu/bitstream/2027.42/71219/2/JCPSA6-53-10-4040-1.pdf.
↑ Schumb, W. C.; Lynch, M. A. (1950). "Iodine Heptafluoride". Industrial & Engineering Chemistry 42 (7): 1383–1386. doi:10.1021/ie50487a035.
↑ Ruff, O.; Keim, R. (1930). ""Das Jod-7-fluorid" (The iodine-7-fluoride)" (in German). Zeitschrift für Anorganische und Allgemeine Chemie 193 (1/2): 176–186. doi:10.1002/zaac.19301930117.
↑ Beveridge, A. D.; Clark, H. C. (1967). "Pentahalides of the Transition Metals". in Gutmann, Viktor. Halogen Chemistry. 3. Academic Press. pp. 179–226. ISBN 9780323148474. https://books.google.com/books?id=q0j8Imd8yQsC&pg=PA212.
↑ Кнунянц, И. Л. (1990) (in ru). Химическая энциклопедия : в пяти томах. Советская Энциклопедия. p. 496. ISBN 5-85270-008-8. OCLC 19556260.

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[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". Journal of Chemical Physics 53 (10): 4040–4046. doi:10.1063/1.1673876. Bibcode: 1970JChPh..53.4040A. https://deepblue.lib.umich.edu/bitstream/2027.42/71219/2/JCPSA6-53-10-4040-1.pdf.

[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)" (in German). Zeitschrift für Anorganische und Allgemeine Chemie 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. Halogen Chemistry. 3. Academic Press. pp. 179–226. ISBN 9780323148474. https://books.google.com/books?id=q0j8Imd8yQsC&pg=PA212.

[9] Кнунянц, И. Л. (1990) (in ru). Химическая энциклопедия : в пяти томах. Советская Энциклопедия. p. 496. ISBN 5-85270-008-8. OCLC 19556260.

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v t e Iodine compounds
Iodine(-I)	HI AtI ICN I⁻
Iodine(I)	HIO ICl IF IBr
Iodine(III)	HIO₂ ICl₃ IF₃
Iodine(V)	HIO₃ IF₅ I₂O₅
Iodine(VII)	HIO₄ H₅IO₆ IF₇