Iodite
Names
IUPAC name
iodite
Systematic IUPAC name
dioxidoiodate(1−)
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/HIO2/c2-1-3/h(H,2,3)/p-1
  • [O-][I+][O-]
Properties
IO−
2
Molar mass 58.90 g/mol
Conjugate acid Iodous acid
Related compounds
Other anions
 Chlorite
Bromite
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

The iodite ion, or iodine dioxide anion, is the halite with the chemical formula IO−
2. Within the ion the Iodine exists in the oxidation state of +3.

Iodite anion

Iodites (including iodous acid) are highly unstable and have been observed[1] but never isolated.[citation needed] They will rapidly disproportionate to molecular Iodine and Iodates.[2] However, they have been detected as intermediates in the conversion between iodide and iodate.[3][4]

Iodous acid

Iodous acid
Ball-and-stick model of iodous acid
Ball-and-stick model of iodous acid
Space-filling model of iodous acid
Space-filling model of iodous acid
Names
IUPAC name
iodous acid
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/HIO2/c2-1-3/h(H,2,3)
  • O[I+][O-]
Properties
HIO2
Molar mass 159.91 g/mol
Conjugate base Iodite
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Iodous acid is acid form of the iodite ion, with the formula HIO2.

Other oxyanions

Iodine can assume oxidation states of −1, +1, +3, +5, or +7. A number of neutral iodine oxides are also known.

Iodine oxidation state −1 +1 +3 +5 +7
Name Iodide Hypoiodite Iodite Iodate periodate
Formula I− IO− IO−
2 		IO−
3 		IO−
4 or IO5−
6

References

  1. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. ^ Gupta, Yugul Kishore; Sharma, Devendra Nath (August 1971). "Kinetics and mechanism of the reduction of iodate to iodite by bromide in the presence of phenol". The Journal of Physical Chemistry. 75 (16): 2516–2522. doi:10.1021/j100685a018.
  4. ^ Gilles, Mary K.; Polak, Mark L.; Lineberger, W. C. (1992). "Photoelectron spectroscopy of the halogen oxide anions FO−, ClO−, BrO−, IO−, OClO−, and OIO−". The Journal of Chemical Physics. 96 (11): 8012. Bibcode:1992JChPh..96.8012G. doi:10.1063/1.462352.
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