Periodate

Periodate

The metaperiodate ion
The orthoperiodate ion
Names
Systematic IUPAC name tetraoxoiodate(1−) hexaoxoiodate(5−)
Identifiers
CAS Number	15056-35-6 (metaperiodate)
ChemSpider	146311 (metaperiodate) 5256770 (orthoperiodate)
Jmol 3D model	Interactive image
PubChem	167232 (metaperiodate) 6857432 (orthoperiodate)
InChI InChI=1S/ClO/c1-2/q-1 Y Key: WQYVRQLZKVEZGA-UHFFFAOYSA-N Y InChI=1S/HIO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 Key: KHIWWQKSHDUIBK-UHFFFAOYSA-M
SMILES [O-]I(=O)(=O)=O
Related compounds
Other anions	Perchlorate Perbromate Permanganate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Periodate /pəˈraɪ.ədeɪt/ is an anion composed of iodine and oxygen. It is one of a number of oxyanions of iodine and is the highest in the series, with iodine existing in oxidation state +7. Unlike other perhalogenates, such as perchlorate, it can exist in two forms: metaperiodate IO⁻
₄ and orthoperiodate IO⁵⁻
₆. In this regard it is comparable to the tellurate ion from the adjacent period. It can combine with a number of counter ions to form periodates, which may also be regarded as the salts of periodic acid.

Periodates were discovered by Heinrich Gustav Magnus and C. F. Ammermüller; who first synthesised periodic acid in 1833.

Synthesis

Classically, periodate was most commonly produced in the form of sodium hydrogen periodate (Na₃H₂IO₆). This is commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide. Or, similarly, from iodides by oxidation with bromine and sodium hydroxide:

NaIO₃ + Cl₂ + 4 NaOH → Na₃H₂IO₆ + 2 NaCl + H₂O

NaI + 4 Br₂ + 10 NaOH → Na₃H₂IO₆ + 8 NaBr + 4 H₂O

Modern industrial scale production involves the electrochemical oxidation of iodates, on a PbO₂ anode, with the following standard electrode potential:

H₅IO₆ + H⁺ + 2 e⁻ → IO⁻
₃ + 3 H₂O      E° = 1.6 V

Metaperiodates are typically prepared by the dehydration of sodium hydrogen periodate with nitric acid, or by dehydrating orthoperiodic acid by heating it to 100 °C under vacuum.

Na₃H₂IO₆ + 2 HNO₃ → NaIO₄ + 2 NaNO₃ + 2 H₂O

H₅IO₆ → HIO₄ + 2 H₂O

They can also be generated directly from iodates by treatment with other strong oxidizing agents such as hypochlorites:

NaIO₃ + NaOCl → NaIO₄ + NaCl

Forms and interconversion

Periodate can exist in a variety of forms in aqueous media, with pH being a controlling factor. Periodate has a number of acid dissociation constants.

H₅IO₆ ⇌ H
₄IO⁻
₆ + H⁺,      pK_a = 3.29

H
₄IO⁻
₆ ⇌ H
₃IO²⁻
₆ + H⁺,      pK_a = 8.31

H
₃IO²⁻
₆ ⇌ H
₂IO³⁻
₆ + H⁺,      pK_a = 11.60

The ortho- and metaperiodate forms also exist in equilibrium.

H
₄IO⁻
₆ ⇌ IO⁻
₄ + 2 H₂O,      K = 29

For this reason orthoperiodate is sometimes referred to as the dihydrate of metaperiodate, written IO⁻
₄·2H₂O; however, this description is not strictly accurate as X-ray crystallography of H₅IO₆ shows 5 equivalent I–OH groups.

At extremes of pH additional species can form. Under basic conditions a dehydration reaction can take place to form the diperiodate (sometimes referred to as mesoperiodate).

2 H
₃IO²⁻
₆ ⇌ H
₂I
₂O⁴⁻
₁₀ + 2 H₂O,      K = 820

Under strongly acid conditions periodic acid can be protonated to give the orthoperiodonium cation.

H
₆IO⁺
₆ ⇌ H₅IO₆ + H⁺,      pK_a = −0.8

Structure and bonding

In both the ortho- and metaperiodate the iodine is hypervalent, as it forms more bonds than would classically be allowed. This has been explained in terms of dative bonds, confirming the absence of double bonding in these molecules.

Exact structures vary depending on counter ions, however on average orthoperiodates adopt a slightly deformed octahedral geometry with X-ray diffraction showing I–O bond lengths of 1.89 Å. Metaperiodates adopt a distorted tetrahedral geometry with an average I–O distance of 1.78 Å.

Reactions

Cleavage reactions

Periodates can cleave carbon–carbon bonds on a variety of 1,2-difunctionalised alkanes. The most common example of this is diol cleavage, which was also the first to be discovered. In addition to diols, periodates can cleave 1,2-hydroxy ketones, 1,2-diketones, α-keto acids, α-hydroxy acids, amino acids, 1,2-amino alcohols, 1,2-diamines, and epoxides to give aldehydes, ketones and carboxylic acids.

Alkenes can also be oxidised and cleaved in the Lemieux–Johnson oxidation. This uses a catalytic loading of osmium tetroxide which is regenerated in situ by the periodate. The overall process is equivalent to that of ozonolysis.

Reactions proceed via a cyclic intermediate called a periodate ester. The formation of this may be affected by pH and temperature but is most strongly effected by the geometry of the substrate, with cis-diols reacting significantly faster than trans-diols. The reactions are exothermic and are typically performed at 0 °C. As periodate salts are only readily soluble in water reactions are generally performed in aqueous media. Where solubility is an issue periodic acid may be used, as this is soluble in alcohols; phase transfer catalysts are also effective in biphasic reaction mixtures. In extreme cases the periodate may be exchanged for lead tetraacetate which reacts in a similar manner and is soluble in organic solvents.

Periodate cleavage is often utilized in molecular biochemistry for the purposes of modifying saccharide rings, as many five- and six-membered sugars have vicinal diols. Historically it was also used to determine the structure of monosaccharides.

Periodate cleavage may be performed on an industrial scale to form dialdehyde starch which has uses in paper production.

Oxidation reactions

Periodates are powerful oxidising agents. They can oxidise catechol to 1,2-benzoquinone and hydroquinone to 1,4-benzoquinone. Sulfides can be effectively oxidised to sulfoxides. Periodates are sufficiently powerful to generate other strong inorganic oxidisers such as permanganate, osmium tetroxide and ruthenium tetroxide.

Niche uses

Periodates are highly selective etchants for certain ruthenium-based oxides.

Several staining agents use in microscopy are based around periodate (e.g. periodic acid–Schiff stain and Jones' stain)

Periodates have also been used as oxidising agents for use in pyrotechnics. In 2013 the US Army announced that it would replace the environmentally harmful chemicals barium nitrate and potassium perchlorate with sodium metaperiodate for use in their tracer ammunition.

Other oxyanions

Periodate is part of a series of oxyanions in which 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

See also

• Sodium periodate
• Potassium periodate
• Periodic acid