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Iodine heptafluoride

From Wikipedia, the free encyclopedia
Iodine heptafluoride
Structure of iodine heptafluoride(IF7)
Structure of iodine heptafluoride(IF7)
Iodine heptafluoride
Iodine heptafluoride
Iodine heptafluoride
Iodine heptafluoride
Names
Other names
Iodine(VII) fluoride
Heptafluoroiodine
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard100.037.241Edit 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
IF7
Molar mass259.90 g/mol
Appearancecolorless gas
Density2.6 g/cm3 (6 °C)
2.7 g/cm3 (25 °C)
Melting point4.5 °C (40.1 °F; 277.6 K) (triple point)
Boiling point4.8 °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 theirstandard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Chemical compound

Iodine heptafluoride is aninterhalogen compound with the chemical formulaIF7.[2][3] It has an unusualpentagonal bipyramidal structure, withD5h symmetry, as predicted byVSEPR theory.[4] The molecule can undergo apseudorotational rearrangement called theBartell mechanism, which is like theBerry mechanism but for a heptacoordinated system.[5]

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 at760 mmHg: instead, the compound begins tosublime at 4.77 °C. The dense vapor has a mouldy, acrid odour.[6][7]

Preparation

[edit]

IF7 is prepared by passingF2 through liquidIF5 at 90 °C, then heating the vapours to 270 °C. Alternatively, this compound can be prepared from fluorine and driedpalladium orpotassium iodide to minimize the formation of IOF5, an impurity arising by hydrolysis.[8][9] Iodine heptafluoride is also produced as a by-product whendioxygenyl hexafluoroplatinate is used to prepare other platinum(V) compounds such aspotassium hexafluoroplatinate(V), usingpotassium fluoride in iodine pentafluoride solution:[10]

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

Reactions

[edit]

Iodine heptafluoride decomposes at 200 °C to fluorine gas andiodine pentafluoride.[11]

Safety considerations

[edit]

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

References

[edit]
  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. ^Lide, David R. (2011).The CRC Handbook of Chemistry and Physics, 89th ed. p. 4-67.
  7. ^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. [Durch] Messung der Dampfdrucke...gelangt man zu der Gleichunglogp=8,66041602,6T{\displaystyle \log p=8,6604-{\frac {1602,6}{T}}}....Für den Druck von 760 mm errechnet sich eine Temperatur von 4,5° C. [Pure iodine heptafluoride is at room temperature a colorless gas, which forms a fog in air on account of its reaction with the humidity and smells musty and acrid. When cooled, it takes the form, depending on experimental conditions, of a free-flowing colorless liquid, a loose snow-white powder, or colorless crystals....The melting point was measured by immersion of a probe in a bath of the right temperature, which was melting in a little quartz tube; and found to be 5‑6 °C. [From] measurement of the vapor pressure...one arrives at the equationlogp=8.66041602.6T{\displaystyle \log p=8.6604-{\frac {1602.6}{T}}}....For a pressure of 760 mm it computes a temperature of 4.5 °C.]"
  8. ^Schumb, W. C.; Lynch, M. A. (1950). "Iodine Heptafluoride".Industrial & Engineering Chemistry.42 (7):1383–1386.doi:10.1021/ie50487a035.
  9. ^Ruff & Keim 1930.
  10. ^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.
  11. ^Кнунянц, И. Л. (1990).Химическая энциклопедия : в пяти томах (in Russian). Советская Энциклопедия. p. 496.ISBN 5-85270-008-8.OCLC 19556260.

Common sources

[edit]
  • 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

[edit]
Iodine(−I)
Iodine(I)
Iodine(II)
Iodine(III)
Iodine(IV)
Iodine(V)
Iodine(VII)
Salts and covalent derivatives of thefluoride ion
HF?HeF2
LiFBeF2BF
BF3
B2F4
+BO3
CF4
CxFy
+CO3
NF3
FN3
N2F2
NF
N2F4
NF2
?NF5
+N
+NO3
OF2
O2F2
OF
O3F2
O4F2
?OF4
F2Ne
NaFMgF2AlF
AlF3
SiF4P2F4
PF3
PF5
+PO4
S2F2
SF2
S2F4
SF3
SF4
S2F10
SF6
+SO4
ClF
ClF3
ClF5
?ArF2
?ArF4
KFCaF
CaF2
ScF3TiF2
TiF3
TiF4
VF2
VF3
VF4
VF5
CrF2
CrF3
CrF4
CrF5
?CrF6
MnF2
MnF3
MnF4
?MnF5
FeF2
FeF3
FeF4
CoF2
CoF3
CoF4
NiF2
NiF3
NiF4
CuF
CuF2
?CuF3
ZnF2GaF2
GaF3
GeF2
GeF4
AsF3
AsF5
Se2F2
SeF4
SeF6
+SeO3
BrF
BrF3
BrF5
KrF2
?KrF4
?KrF6
RbFSrF
SrF2
YF3ZrF2
ZrF3
ZrF4
NbF4
NbF5
MoF4
MoF5
MoF6
TcF4
TcF
5

TcF6
RuF3
RuF
4

RuF5
RuF6
RhF3
RhF4
RhF5
RhF6
PdF2
Pd[PdF6]
PdF4
?PdF6
Ag2F
AgF
AgF2
AgF3
CdF2InF
InF3
SnF2
SnF4
SbF3
SbF5
TeF4
?Te2F10
TeF6
+TeO3
IF
IF3
IF5
IF7
+IO3
XeF2
XeF4
XeF6
?XeF8
CsFBaF2 LuF3HfF4TaF5WF4
WF5
WF6
ReF4
ReF5
ReF6
ReF7
OsF4
OsF5
OsF6
?OsF
7

?OsF
8
IrF2
IrF3
IrF4
IrF5
IrF6
PtF2
Pt[PtF6]
PtF4
PtF5
PtF6
AuF
AuF3
Au2F10
?AuF6
AuF5•F2
Hg2F2
HgF2
?HgF4
TlF
TlF3
PbF2
PbF4
BiF3
BiF5
PoF2
PoF4
PoF6
AtF
?AtF3
?AtF5
RnF2
?RnF
4

?RnF
6
FrFRaF2 LrF3RfDbSgBhHsMtDsRgCnNhFlMcLvTsOg
LaF3CeF3
CeF4
PrF3
PrF4
NdF2
NdF3
NdF4
PmF3SmF
SmF2
SmF3
EuF2
EuF3
GdF3TbF3
TbF4
DyF2
DyF3
DyF4
HoF3ErF3TmF2
TmF3
YbF2
YbF3
AcF3ThF2
ThF3
ThF4
PaF4
PaF5
UF3
UF4
UF5
UF6
NpF3
NpF4
NpF5
NpF6
PuF3
PuF4
PuF5
PuF6
AmF2
AmF3
AmF4
?AmF6
CmF3
CmF4
 ?CmF6
BkF3
BkF
4
CfF3
CfF4
EsF3
EsF4
?EsF6
FmMdF3No
PF6,AsF6,SbF6 compounds
AlF2−5,AlF3−6 compounds
chlorides, bromides, iodides
and pseudohalogenides
SiF2−6,GeF2−6 compounds
Oxyfluorides
Organofluorides
with transition metal,
lanthanide, actinide, ammonium
nitric acids
bifluorides
thionyl, phosphoryl,
and iodosyl
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