Iodide

An iodide ion is the ion I−.[2] Compounds with iodine in formal oxidation state −1 are called iodides. In everyday life, iodide is most commonly encountered as a component of iodized salt, which many governments mandate. Worldwide, iodine deficiency affects two billion people and is the leading preventable cause of intellectual disability.[3]

"i-" redirects here. For the Internet-related prefix i-, see Wiktionary's entry i-.
Iodide
Names
Systematic IUPAC name
Iodide[1]
Identifiers
3D model (JSmol)
3587184
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.125.457
14912
KEGG
UNII
Properties
I−
Molar mass 126.90447 g·mol−1
Conjugate acid Hydrogen iodide
Thermochemistry
169.26 J K−1 mol−1
Related compounds
Other anions
 Fluoride

Chloride
Bromide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Structure and characteristics of inorganic iodides

Iodide is one of the largest monatomic anions. It is assigned a radius of around 206 picometers. For comparison, the lighter halides are considerably smaller: bromide (196 pm), chloride (181 pm), and fluoride (133 pm). In part because of its size, iodide forms relatively weak bonds with most elements.

Most iodide salts are soluble in water, but often less so than the related chlorides and bromides. Iodide, being large, is less hydrophilic compared to the smaller anions. One consequence of this is that sodium iodide is highly soluble in acetone, whereas sodium chloride is not. The low solubility of silver iodide and lead iodide reflects the covalent character of these metal iodides. A test for the presence of iodide ions is the formation of yellow precipitates of these compounds upon treatment of a solution of silver nitrate or lead(II) nitrate.[2]

Aqueous solutions of iodide salts dissolve iodine better than pure water. This effect is due to the formation of the triiodide ion, which is brown:

I− + I2 ⇌ I−
3

Redox, including antioxidant properties

Iodide salts are mild reducing agents and many react with oxygen to give iodine. A reducing agent is a chemical term for an antioxidant. Its antioxidant properties can be expressed quantitatively as a redox potential :

I− ⇌ ​1⁄2 I2 + e−      E° = 0.54 volts (versus SHE)

Because iodide is easily oxidized, some enzymes readily convert it into electrophilic iodinating agents, as required for the biosynthesis of myriad iodide-containing natural products. Iodide can function as an antioxidant reducing species that can destroy ozone[4] and reactive oxygen species such as hydrogen peroxide:[5]

2 I− + peroxidase + H2O2 + tyrosine, histidine, lipid, etc. → iodo-compounds + H2O + 2 e− (antioxidants).

Representative iodides
Compound Formula Appearance Use or occurrence
Potassium iodide KI white crystals iodine component of iodized salt
Hydrogen iodide HI colourless gas strong mineral acid
Silver iodide AgI yellow powder that darkens in light photoactive component of silver-based photographic film
Thyroxine
(3,5,3′,5′-tetraiodothyronine)		 C15H11I4NO4 pale yellow solid hormone essential for human health

Natural occurrence

Iodargyrite—natural, crystalline silver iodide—is the most common iodide mineral currently known. Iodide anions may sometimes also be found combined with mercury, copper and lead, but minerals with such compositions are even more scarce.[6]

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. "Iodide - PubChem Public Chemical Database". The PubChem Project. USA: National Center for Biotechnology Information.
  2. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. McNeil, Donald G. Jr (2006-12-16). "In Raising the World's I.Q., the Secret's in the Salt". New York Times. Retrieved 2008-12-04.
  4. Pillar, Elizabeth A.; Guzman, Marcelo I.; Rodriguez, Jose M. (2013-10-01). "Conversion of Iodide to Hypoiodous Acid and Iodine in Aqueous Microdroplets Exposed to Ozone". Environmental Science & Technology. 47 (19): 10971–10979. doi:10.1021/es401700h. ISSN 0013-936X.
  5. Küpper FC; Carpenter LJ; McFiggans GB; et al. (2008). "Iodide accumulation provides kelp with an inorganic antioxidant impacting atmospheric chemistry" (Free full text). Proceedings of the National Academy of Sciences of the United States of America. 105 (19): 6954–8. Bibcode:2008PNAS..105.6954K. doi:10.1073/pnas.0709959105. PMC 2383960. PMID 18458346.
  6. http://www.mindat.org
Salts and covalent derivatives of the iodide ion
HI He
LiI BeI2 BI3 CI4 NI3 I2O4,
I2O5,
I4O9		 IF,
IF3,
IF5,
IF7		 Ne
NaI MgI2 AlI3 SiI4 PI3,
P2I4		 S ICl,
ICl3		 Ar
KI CaI2 ScI3 TiI2
TiI3
TiI4		 VI3 CrI3 MnI2 FeI2 CoI2 NiI2 CuI ZnI2 Ga2I6 GeI2,
GeI4		 AsI3 Se IBr Kr
RbI SrI2 YI3 ZrI4 NbI5 Mo Tc Ru Rh Pd AgI CdI2 InI3 SnI4,
SnI2		 SbI3 TeI4 I Xe
CsI BaI2   HfI4 TaI5 W Re Os Ir Pt AuI Hg2I2,
HgI2		 TlI PbI2 BiI3 Po AtI Rn
Fr RaI2   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La Ce Pr Nd Pm SmI2 Eu Gd TbI3 Dy Ho Er Tm Yb Lu
Ac ThI4 Pa UI3,
UI4		 Np Pu Am Cm Bk Cf EsI3 Fm Md No Lr
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