Iodine oxides are chemical compounds of oxygen and iodine. Iodine has only two stable oxides which are isolatable in bulk, iodine tetroxide and iodine pentoxide, but a number of other oxides are formed in trace quantities or have been hypothesized to exist.
The chemistry of these compounds is complicated with only a few having been well characterized. Many have been detected in the atmosphere and are believed to be particularly important in the marine boundary layer.[1]
Iodine oxides[2]
Molecular formula
I2O
IO[3]
IO2
I2O4
I2O5
I4O9
Name
diiodine oxide
iodine monoxide
iodine dioxide
iodine tetroxide
(diiodine tetroxide)
Iodine pentoxide
(diiodine pentoxide)
tetraiodine nonoxide
Structure
I2O
IO
IO2
(IO2)2
O(IO2)2
I(OIO2)3
Molecular model
CAS registry
39319-71-6
14696-98-1
13494-92-3
1024652-24-1
12029-98-0
66523-94-2
Appearance
Unknown
purple gas
yellow solid
yellow solid
white crystalline solid
dark yellow solid
Oxidation state
+1
+2
+4
+3 and +5
+5
+3 and +5
Melting point
not isolable
not isolable
not isolable
decomp. 100 °C
decomp. 300–350 °C
decomp. 75 °C
Specific gravity
4.2
4.8
Solubility in water
decomp. to HIO3 + I2
187 g/100 mL
decomp. to HIO3 + I2
Diiodine monoxide has largely been the subject of theoretical study,[4] but there is some evidence that it may be prepared in a similar manner to dichlorine monoxide, via a reaction between HgO and I2.[5] The compound appears to be highly unstable but can react with alkenes to give halogenated products.[6]
Radical iodine oxide (IO), iodine dioxide (IO2) and iodine tetroxide ((IO2)2) all possess significant and interconnected atmospheric chemistry. They are formed, in very small quantities, at the marine boundary layer by the photooxidation of diiodomethane, which is produced by macroalga such as seaweed or through the oxidation of molecular iodine, produced by the reaction of gaseous ozone and iodide present at the seasurface.[7][8] Despite the small quantities produced (typically below ppt) they are thought to be powerful ozone depletion agents.[9][10]
Diiodine pentoxide (I2O5) is the anhydride of iodic acid and the only stable anhydride of an iodine oxoacid.
Tetraiodine nonoxide (I4O9) has been prepared by the gas-phase reaction of I2 with O3 but has not been extensively studied.[11]
^Kaltsoyannis, Nikolas; Plane, John M. C. (2008). "Quantum chemical calculations on a selection of iodine-containing species (IO, OIO, INO3, (IO)2, I2O3, I2O4 and I2O5) of importance in the atmosphere". Physical Chemistry Chemical Physics. 10 (13): 1723–33. Bibcode:2008PCCP...10.1723K. doi:10.1039/B715687C. PMID 18350176.
^Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
^Nikitin, I V (31 August 2008). "Halogen monoxides". Russian Chemical Reviews. 77 (8): 739–749. Bibcode:2008RuCRv..77..739N. doi:10.1070/RC2008v077n08ABEH003788. S2CID 250898175.
^Novak, Igor (1998). "Theoretical study of I2O". Heteroatom Chemistry. 9 (4): 383–385. doi:10.1002/(SICI)1098-1071(1998)9:4<383::AID-HC6>3.0.CO;2-9.
^Forbes, Craig P.; Goosen, André; Laue, Hugh A. H. (1974). "Hypoiodite reaction: kinetic study of the reaction of 1,1-diphenyl-ethylene with mercury(II) oxide iodine". Journal of the Chemical Society, Perkin Transactions 1: 2350–2353. doi:10.1039/P19740002350.
^Cambie, Richard C.; Hayward, Rodney C.; Lindsay, Barry G.; Phan, Alice I. T.; Rutledge, Peter S.; Woodgate, Paul D. (1976). "Reactions of iodine oxide with alkenes". Journal of the Chemical Society, Perkin Transactions 1 (18): 1961. doi:10.1039/P19760001961.
^Hoffmann, Thorsten; O'Dowd, Colin D.; Seinfeld, John H. (15 May 2001). "Iodine oxide homogeneous nucleation: An explanation for coastal new particle production" (PDF). Geophysical Research Letters. 28 (10): 1949–1952. Bibcode:2001GeoRL..28.1949H. doi:10.1029/2000GL012399.
^Carpenter, Lucy J.; MacDonald, Samantha M.; Shaw, Marvin D.; Kumar, Ravi; Saunders, Russell W.; Parthipan, Rajendran; Wilson, Julie; Plane, John M.C. (13 January 2013). "Atmospheric iodine levels influenced by seasurface emissions of inorganic iodine" (PDF). Nature Geoscience. 6 (2): 108–111. Bibcode:2013NatGe...6..108C. doi:10.1038/ngeo1687.
^Saiz-Lopez, A.; Fernandez, R. P.; Ordóñez, C.; Kinnison, D. E.; Gómez Martín, J. C.; Lamarque, J.-F.; Tilmes, S. (10 December 2014). "Iodine chemistry in the troposphere and its effect on ozone". Atmospheric Chemistry and Physics. 14 (23): 13119–13143. Bibcode:2014ACP....1413119S. doi:10.5194/acp-14-13119-2014. hdl:11336/100317.
^Cox, R. A.; Bloss, W. J.; Jones, R. L.; Rowley, D. M. (1 July 1999). "OIO and the atmospheric cycle of iodine" (PDF). Geophysical Research Letters. 26 (13): 1857–1860. Bibcode:1999GeoRL..26.1857C. doi:10.1029/1999GL900439. S2CID 128402214.
^Sunder, S.; Wren, J. C.; Vikis, A. C. (December 1985). "Raman spectra of I4O9 formed by the reaction of iodine with ozone". Journal of Raman Spectroscopy. 16 (6): 424–426. Bibcode:1985JRSp...16..424S. doi:10.1002/jrs.1250160611.
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