Sodium periodate

Sodium periodate
Names
IUPAC name
Sodium periodate
Other names
Sodium metaperiodate
Identifiers
7790-28-5 YesY
ChEBI CHEBI:75226 N
ChemSpider 58683 YesY
EC Number 232-197-6
Jmol interactive 3D Image
PubChem 23667635
RTECS number SD4550000
Properties
NaIO4
Molar mass 213.8918 g/mol
Appearance white crystals
Density 3.865 g/cm3 (anhydrous)
3/210 g/cm3
Melting point 300 °C (572 °F; 573 K) (anhydrous)
175 °C (347 °F; 448 K) (trihydrate) (decomposes)
soluble
Solubility soluble in acids
Structure
tetragonal (anhydrous)
trigonal (trihydrate)
Hazards
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
2
0
Related compounds
Other anions
 sodium perchlorate, sodium perbromate
Other cations
 potassium periodate, periodic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Sodium periodate is an inorganic salt, composed of a sodium cation and the periodate anion. It may also be regarded as the sodium salt of periodic acid. Like all periodates it can exist in two different forms: sodium metaperiodate, which has the formula NaIO4, and sodium orthoperiodate, normally this means sodium hydrogen periodate (Na2H3IO6) but the fully reacted sodium orthoperiodate salt, Na5IO6, can also be prepared. Both salts are useful oxidising agents.[1]

Preparation

Classically, periodate was most commonly produced in the form of sodium hydrogen periodate (Na3H2IO6).[2] This is commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide.[3] 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− → IO3− + 3 H2O   1.6 E° [4]

Sodium metaperiodate can be prepared by the dehydration of sodium hydrogen periodate with nitric acid.[2]

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

Structure

Sodium metaperiodate (NaIO4) forms tetragonal crystals (space group I41/a) consisting of slightly distorted IO4 ions with average I-O bond distances of 1.775 Å; the Na+ ions are surrounded by 8 oxygen atoms at distances of 2.54 and 2.60 Å[5]

Sodium hydrogen periodate (Na2H3IO6) forms orthorhombic crystals (space group Pnnm). Iodine and sodium atoms are both surrounded by an octahedral arraigement of 6 oxygen atoms; however the NaO6 octahedron is strongly distorted. IO6 and NaO6 groups are linked via common vertices and edges.[6]

Powder diffraction indicates that Na5IO6 crystallises in the monoclinic system (space group C2/m).[7]

Uses

Further information: Periodate reactions

Sodium periodate can be used in solution to open saccharide rings between vicinal diols leaving two aldehyde groups. This process is often used in labeling saccharides with fluorescent molecules or other tags such as biotin. Because the process requires vicinal diols, periodate oxidation is often used to selectively label the 3'-termini of RNA (ribose has vicinal diols) instead of DNA as deoxyribose does not have vicinal diols.

NaIO4 is used in organic chemistry to cleave diols to produce two aldehydes.[8]

In 2013 US Army announced that it would replace environmentally harmful chemicals barium nitrate and potassium perchlorate with sodium metaperiodate for use in their tracer ammunition.[9]

See also

References

  1. ↑ Andrew G. Wee, Jason Slobodian, Manuel A. Fernández-Rodríguez and Enrique Aguilar "Sodium Periodate" e-EROS Encyclopedia of Reagents for Organic Synthesis 2006. doi:10.1002/047084289X.rs095.pub2
  2. 1 2 Riley, edited by Georg Brauer ; translated by Scripta Technica, Inc. Translation editor Reed F. (1963). Handbook of preparative inorganic chemistry. Volume 1 (2nd ed.). New York, N.Y.: Academic Press. pp. 323–324. ISBN 012126601X.
  3. ↑ Hill, Arthur E. (October 1928). "TERNARY SYSTEMS. VII. THE PERIODATES OF THE ALKALI METALS". Journal of the American Chemical Society 50 (10): 2678–2692. doi:10.1021/ja01397a013.
  4. ↑ Parsons, Roger (1959). Handbook of electrochemical constants. Butterworths Scientific Publications Ltd. p. 71.
  5. ↑ Kálmán, A.; Cruickshank, D. W. J. (15 November 1970). "Refinement of the structure of NaIO4". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry 26 (11): 1782–1785. doi:10.1107/S0567740870004880.
  6. ↑ Jansen, Martin; Rehr, Anette (1988). "Na2H3IO6, eine Variante der Markasitstruktur". Zeitschrift für anorganische und allgemeine Chemie allgemeine Chemie (in German) 567 (1): 95–100. doi:10.1002/zaac.19885670111.
  7. ↑ Betz, T.; Hoppe, R. (May 1984). "Über Perrhenate. 2. Zur Kenntnis von Li5ReO6 und Na5ReO6 – mit einer Bemerkung über Na5IO6". Zeitschrift für anorganische und allgemeine Chemie (in German) 512 (5): 19–33. doi:10.1002/zaac.19845120504.
  8. ↑ McMurry, John. Organic chemistry (8th ed., [international ed.] ed.). Singapore: Brooks/Cole Cengage Learning. pp. 285–286. ISBN 9780840054531.
  9. ↑ "Picatinny to remove tons of toxins from lethal rounds". U.S. Army. Retrieved 31 October 2013.
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