Iodite

Iodous acid
Ball-and-stick model of iodous acid	Space-filling model of iodous acid
Names
	IUPAC name iodous acid
Identifiers
CAS Number	12134-99-5;
3D model (JSmol)	Interactive image;
ChemSpider	145806;
PubChem CID	166623;
CompTox Dashboard (EPA)	DTXSID901031417 ;
	InChI InChI=1S/HIO2/c2-1-3/h(H,2,3);
	SMILES O[I+][O-];
Properties
Chemical formula	HIO2
Molar mass	159.911
Conjugate base	Iodite
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Iodite
Names
	IUPAC name iodite
	Systematic IUPAC name dioxidoiodate(1−)
Identifiers
CAS Number	20499-55-2;
3D model (JSmol)	Interactive image;
ChemSpider	4574132;
PubChem CID	5460637;
CompTox Dashboard (EPA)	DTXSID901031417 ;
	InChI InChI=1S/HIO2/c2-1-3/h(H,2,3)/p-1;
	SMILES [O-][I+][O-];
Properties
Chemical formula	IO−; 2
Molar mass	58.90327 gm mol−1
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). Infobox references

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.^[2] They will rapidly disproportionate to molecular Iodine and Iodates.^[3] However, they have been detected as intermediates in the conversion between iodide and iodate.^[4]^[5]

Iodous acid

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

^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Ropp, R.C. (2013). Encyclopedia of the alkaline earth compounds. Oxford: Elsevier Science. p. 96. ISBN 0444595538.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ 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.
^ 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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[1] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[2] Ropp, R.C. (2013). Encyclopedia of the alkaline earth compounds. Oxford: Elsevier Science. p. 96. ISBN 0444595538.

[3] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.

[4] 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.

[5] 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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