Iodite
| Names | |
|---|---|
| IUPAC name
iodite | |
| Systematic IUPAC name
dioxidoiodate(1−) | |
| Identifiers | |
| 20499-55-2 | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 4574132 |
| PubChem | 5460637 |
| |
| |
| Properties | |
| IO− 2 | |
| Molar mass | 158.90327 |
| 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 | |
Iodite is an anion composed of iodine and oxygen, with the chemical formula IO−
2. Within this ion the iodine exists in oxidation state III.
Iodites (including iodous acid) are highly unstable and have never been isolated.[1] However they have been detected as intermediates in the conversion between iodide and iodate.[2][3]
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
- ↑ Ropp, R.C. (2013). Encyclopedia of the alkaline earth compounds. Oxford: Elsevier Science. p. 96. ISBN 0444595538.
- ↑ 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. doi:10.1063/1.462352.
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