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| ⚫ | | verifiedrevid = 446242167 | ||
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| ⚫ | | Name = Iodine heptafluoride | ||
| <!-- | ImageSize = 120px --> | |||
| | |
| ImageFile = Iodine-heptafluoride-2D-dimensions.png | ||
| | ImageFileL1 = Iodine-heptafluoride-3D-balls.png | |||
| | ImageName = Structure of iodine heptafluoride(IF7) | |||
| <!-- | ImageSizeL1 = 120px --> | |||
| | |
| ImageFileL1 = Iodine-heptafluoride-3D-balls.png | ||
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| ImageNameL1 = Iodine heptafluoride | ||
| ⚫ | | ImageFileR1 = Iodine-heptafluoride-3D-vdW.png | ||
| <!-- | ImageSizeR1 = 120px --> | |||
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| ImageNameR1 = Iodine heptafluoride | ||
| | |
| OtherNames = Iodine(VII) fluoride<br />Heptafluoroiodine | ||
| | |
|Section1={{Chembox Identifiers | ||
| | |
| InChI = 1/F7I/c1-8(2,3,4,5,6)7 | ||
| | InChIKey = XRURPHMPXJDCOO-UHFFFAOYAO | | InChIKey = XRURPHMPXJDCOO-UHFFFAOYAO | ||
| | SMILES = FI(F)(F)(F)(F)(F)F | | SMILES = FI(F)(F)(F)(F)(F)F | ||
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| | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | ||
| | StdInChIKey = XRURPHMPXJDCOO-UHFFFAOYSA-N | | StdInChIKey = XRURPHMPXJDCOO-UHFFFAOYSA-N | ||
| | CASNo_Ref = {{cascite|correct|??}} | |||
| | CASNo = 16921-96-3 | | CASNo = 16921-96-3 | ||
| | |
| UNII_Ref = {{fdacite|correct|FDA}} | ||
| | UNII = M080M03ILM | |||
| ⚫ | | ChemSpiderID=21477354 |
||
| | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | |||
| ⚫ | | ChemSpiderID =21477354 | ||
| | PubChem = 85645 | |||
| }} | }} | ||
| | |
|Section2={{Chembox Properties | ||
| | |
| Formula = IF<sub>7</sub> | ||
| | |
| Appearance = colorless gas | ||
| | |
| MolarMass = 259.90 g/mol | ||
| | |
| Density = 2.6 g/cm<sup>3</sup> (6 °C) <br> 2.7 g/cm<sup>3</sup> (25 °C) | ||
| | |
| Solubility = soluble <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref> | ||
| | |
| MeltingPtC = 4.5 | ||
| | MeltingPt_notes = (triple point) | |||
| ⚫ | | |
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| | BoilingPtC = 4.8 | |||
| ⚫ | | |
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| ⚫ | | BoilingPt_notes = (sublimes at 1 atm) | ||
| ⚫ | | |
||
| }} | |||
| ⚫ | |Section3={{Chembox Related | ||
| ⚫ | | OtherCompounds = ] | ||
| }} | |||
| }} | }} | ||
| '''Iodine heptafluoride''' |
'''Iodine heptafluoride''' is an ] with the chemical formula ]]<sub>7</sub>.<ref>Macintyre, J. E. (Ed.). (1992). ''Dictionary of Inorganic Compounds'' (Vol. 3). London: Chapman & Hall.</ref><ref>O'Neil, Maryadele J. (Ed.). (2001). ''The Merck Index'' (13th ed.). Whitehouse Station, NJ: Merck.</ref> It has an unusual ] structure, with ], as predicted by ].<ref>{{cite journal | ||
| | title = On the problem of heptacoordination: vibrational spectra, structure, and fluxionality of iodine heptafluoride | | title = On the problem of heptacoordination: vibrational spectra, structure, and fluxionality of iodine heptafluoride | ||
| | |
|author1=K. O. Christe |author2=E. C. Curtis |author3=D. A. Dixon | journal = ] | ||
| ⚫ | | journal = ] | ||
| | year = 1993 | | year = 1993 | ||
| | volume = 115 | | volume = 115 | ||
| Line 45: | Line 52: | ||
| | pages = 1520–1526 | | pages = 1520–1526 | ||
| | doi = 10.1021/ja00057a044 | | doi = 10.1021/ja00057a044 | ||
| }}</ref> The molecule can undergo a ]al rearrangement called the ], which is like the ] but for a |
}}</ref> The molecule can undergo a ]al rearrangement called the ], which is like the ] but for a heptacoordinated system.<ref>{{cite journal | ||
| | title = Structure, Pseudorotation, and Vibrational Mode Coupling in IF<sub>7</sub>: An Electron Diffraction Study | | title = Structure, Pseudorotation, and Vibrational Mode Coupling in IF<sub>7</sub>: An Electron Diffraction Study | ||
| | |
|author1=W. J. Adams |author2=H. Bradford Thompson |author3=L. S. Bartell | journal = ] | ||
| | journal = ] | |||
| | year = 1970 | | year = 1970 | ||
| | volume = 53 | | volume = 53 | ||
| Line 54: | Line 60: | ||
| | pages = 4040–4046 | | pages = 4040–4046 | ||
| | doi = 10.1063/1.1673876 | | doi = 10.1063/1.1673876 | ||
| |bibcode=1970JChPh..53.4040A | url = https://deepblue.lib.umich.edu/bitstream/2027.42/71219/2/JCPSA6-53-10-4040-1.pdf | |||
| | hdl = 2027.42/71219 | |||
| | hdl-access = free | |||
| }}</ref> | }}</ref> | ||
| 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. | |||
| Below 4.5 °C, IF<sub>7</sub> forms a snow-white powder of colorless crystals, melting at 5-6 °C. However, this melting is difficult to observe, as the liquid form is thermodynamically unstable at ]: instead, the compound begins to ] at 4.77 °C. The dense vapor has a mouldy, acrid odour.<ref>Lide, David R. (2011). '']'', 89th ed. p. <!-- NOT a range; do NOT replace with en dash -->].</ref><ref>{{harvnb|Ruff|Keim|1930|pp=180–182}}: "Das reine Jod-7-fluorid ist bei Zimmer­temperatur ein farbloses Gas, das an der Luft infolge seiner Umsetzung mit dem Wasser­dampf Nebel bildet und muffig sauer riecht. Beim Abkühlen wird es je nach den Versuchs­bedingungen als leicht bewegliche, farblose Flüssigkeit als schneeweißes lockeres Pulver oder in Form farbloser Kristalle erhalten....Die Schmelz­temperatur wurde durch Eintauchen von Proben, die in Quarzröhrchen eingeschmolzen waren, in Bäder passender Temperatur ermittelt und zu 5 bis 6° C gefunden. Messung der Dampfdrucke...gelangt man zu der Gleichung <math display=block>\log p=8,6604-\frac{1602,6}{T}</math>....Für den Druck von 760 mm errechnet sich eine Temperatur von 4,5° C. measurement of the vapor pressure...one arrives at the equation <math display=block>\log p=8.6604-\frac{1602.6}{T}</math>....At a pressure of 760 mm it computes a temperature of 4.5 °C.]"</ref> | |||
| ==Preparation== | ==Preparation== | ||
| IF<sub>7</sub> is prepared by passing ] through liquid ] at 90 °C, then heating the vapours to 270 °C. |
IF<sub>7</sub> is prepared by passing ] through liquid ] at 90 °C, then heating the vapours to 270 °C. Alternatively, this compound can be prepared from fluorine and dried ] or ] to minimize the formation of IOF<sub>5</sub>, an impurity arising by hydrolysis.<ref>{{cite journal| title = Iodine Heptafluoride | ||
| ⚫ | | first1 = W. C. | last1 = Schumb | first2 = M. A. | last2 = Lynch | journal = ] | ||
| | title = Iodine Heptafluoride | |||
| | author = W. C. Schumb, M. A. Lynch, Jr. | |||
| | journal = ] | |||
| | year = 1950 | | year = 1950 | ||
| | volume = 42 | | volume = 42 | ||
| Line 67: | Line 75: | ||
| | pages = 1383–1386 | | pages = 1383–1386 | ||
| | doi = 10.1021/ie50487a035 | | doi = 10.1021/ie50487a035 | ||
| }}</ref>{{sfn|Ruff|Keim|1930}} Iodine heptafluoride is also produced as a by-product when ] is used to prepare other platinum(V) compounds such as ], using ] in iodine pentafluoride solution:<ref>{{cite book | title = Halogen Chemistry | chapter = Pentahalides of the Transition Metals | pages = 179–226 | volume = 3 | first1 = A. D. | last1 = Beveridge | first2 = H. C. | last2 = Clark | editor-first = Viktor | editor-last = Gutmann | publisher = ] | year = 1967 | isbn = 9780323148474 | chapter-url = https://books.google.com/books?id=q0j8Imd8yQsC&pg=PA212}}</ref> | |||
| }}</ref><ref>{{cite journal | |||
| | title = "Das Jod-7-fluorid" (The iodine-7-fluoride) | |||
| :2 O<sub>2</sub>PtF<sub>6</sub> + 2 KF + IF<sub>5</sub> → 2 KPtF<sub>6</sub> + 2 O<sub>2</sub> + IF<sub>7</sub> | |||
| | author = Ruff O., Keim R. | |||
| | journal = Zeitschrift für Anorganische und Allgemeine Chemie | |||
| ==Reactions== | |||
| | year = 1930 | |||
| Iodine heptafluoride decomposes at 200 °C to fluorine gas and ].<ref>{{cite book | last=Кнунянц | first=И. Л. | title=Химическая энциклопедия : в пяти томах | publisher=Советская Энциклопедия |date=1990 | isbn=5-85270-008-8 | oclc=19556260 | language=ru |page=496}}</ref> | |||
| | volume = 193 | |||
| | issue = 1/2 | |||
| | pages = 176–186 | |||
| | doi = 10.1002/zaac.19301930117 | |||
| }}</ref> | |||
| ==Safety considerations== | ==Safety considerations== | ||
| IF<sub>7</sub> is highly irritating to both the skin and the mucous |
IF<sub>7</sub> is highly irritating to both the skin and the ]s. It also is a strong oxidizer and can cause fire on contact with organic material. | ||
| ==References== | ==References== | ||
| <references/> | |||
| {{reflist}} | |||
| ===Common sources=== | |||
| * {{Cite journal |last=Ruff |first=Otto |last2=Keim |first2=Rudolf |date=1930-10-21 |title=Das Jod-7-fluorid |trans-title=Iodine Heptafluoride |journal=Zeitschrift für anorganische und allgemeine Chemie |language=de |volume=193 |issue=1/2 |pages=176–186 |doi=10.1002/zaac.19301930117 |issn=0863-1786}} | |||
| ==External links== | ==External links== | ||
| * | * | ||
| * | * | ||
| * | * | ||
| {{Iodine compounds}} | {{Iodine compounds}} | ||
| {{fluorine compounds}} | |||
| ] | ] | ||
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| ] | ] | ||
| ] | ] | ||
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| {{inorganic-compound-stub}} | |||
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Latest revision as of 22:32, 5 April 2024
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| Names | |||
|---|---|---|---|
| Other names
Iodine(VII) fluoride Heptafluoroiodine | |||
| Identifiers | |||
| CAS Number | |||
| 3D model (JSmol) | |||
| ChemSpider | |||
| ECHA InfoCard | 100.037.241 
| ||
| PubChem CID | |||
| UNII | |||
| CompTox Dashboard (EPA) | |||
InChI
| |||
SMILES
| |||
| Properties | |||
| Chemical formula | IF7 | ||
| Molar mass | 259.90 g/mol | ||
| Appearance | colorless gas | ||
| Density | 2.6 g/cm (6 °C) 2.7 g/cm (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 , 100 kPa).
 N verify (what is ?)
Infobox references
| |||
Iodine heptafluoride is an interhalogen compound with the chemical formula IF7. It has an unusual pentagonal bipyramidal structure, with D5h symmetry, as predicted by VSEPR theory. The molecule can undergo a pseudorotational rearrangement called the Bartell mechanism, which is like the Berry mechanism but for a heptacoordinated system.
Below 4.5 °C, IF7 forms a snow-white powder of colorless crystals, melting at 5-6 °C. However, this melting is difficult to observe, as the liquid form is thermodynamically unstable at 760 mmHg: instead, the compound begins to sublime at 4.77 °C. The dense vapor has a mouldy, acrid odour.
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. 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:
- 2 O2PtF6 + 2 KF + IF5 → 2 KPtF6 + 2 O2 + IF7
Reactions
Iodine heptafluoride decomposes at 200 °C to fluorine gas and iodine pentafluoride.
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" (PDF). Journal of Chemical Physics. 53 (10): 4040–4046. Bibcode:1970JChPh..53.4040A. doi:10.1063/1.1673876. hdl:2027.42/71219.
- Lide, David R. (2011). The CRC Handbook of Chemistry and Physics, 89th ed. p. 4-67.
- Ruff & Keim 1930, pp. 180–182: "Das reine Jod-7-fluorid ist bei Zimmertemperatur ein farbloses Gas, das an der Luft infolge seiner Umsetzung mit dem Wasserdampf Nebel bildet und muffig sauer riecht. Beim Abkühlen wird es je nach den Versuchsbedingungen als leicht bewegliche, farblose Flüssigkeit als schneeweißes lockeres Pulver oder in Form farbloser Kristalle erhalten....Die Schmelztemperatur wurde durch Eintauchen von Proben, die in Quarzröhrchen eingeschmolzen waren, in Bäder passender Temperatur ermittelt und zu 5 bis 6° C gefunden. Messung der Dampfdrucke...gelangt man zu der Gleichung ....Für den Druck von 760 mm errechnet sich eine Temperatur von 4,5° C. measurement of the vapor pressure...one arrives at the equation ....At a pressure of 760 mm it computes a temperature of 4.5 °C.]"
- Schumb, W. C.; Lynch, M. A. (1950). "Iodine Heptafluoride". Industrial & Engineering Chemistry. 42 (7): 1383–1386. doi:10.1021/ie50487a035.
- Ruff & Keim 1930.
- Beveridge, A. D.; Clark, H. C. (1967). "Pentahalides of the Transition Metals". In Gutmann, Viktor (ed.). Halogen Chemistry. Vol. 3. Academic Press. pp. 179–226. ISBN 9780323148474.
- Кнунянц, И. Л. (1990). Химическая энциклопедия : в пяти томах (in Russian). Советская Энциклопедия. p. 496. ISBN 5-85270-008-8. OCLC 19556260.
....Für den Druck von 760 mm errechnet sich eine Temperatur von 4,5° C. measurement of the vapor pressure...one arrives at the equation 
....At a pressure of 760 mm it computes a temperature of 4.5 °C.]"
Common sources
- Ruff, Otto; Keim, Rudolf (1930-10-21). "Das Jod-7-fluorid" [Iodine Heptafluoride]. Zeitschrift für anorganische und allgemeine Chemie (in German). 193 (1/2): 176–186. doi:10.1002/zaac.19301930117. ISSN 0863-1786.
External links
- WebBook page for IF7
- National Pollutant Inventory - Fluoride and compounds fact sheet
- web elements listing
| Iodine compounds | |
|---|---|
| Iodine(−I) | |
| Iodine(I) | |
| Iodine(II) | |
| Iodine(III) | |
| Iodine(IV) | |
| Iodine(V) | |
| Iodine(VII) | |