Sodium periodate
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IUPAC name
Sodium periodate
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Other names
Sodium metaperiodate
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Identifiers | |
3D model (
JSmol ) |
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ChEBI | |
ChemSpider | |
ECHA InfoCard
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100.029.270 |
EC Number |
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PubChem CID
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RTECS number
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UNII | |
CompTox Dashboard (EPA)
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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) |
91 g/L[1] | |
Solubility | soluble in acids |
Structure | |
tetragonal (anhydrous) trigonal (trihydrate) | |
Hazards | |
NFPA 704 (fire diamond) | |
Related compounds | |
Other anions
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sodium perchlorate, sodium perbromate |
Other cations
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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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Sodium periodate is an
Preparation
Classically, periodate was most commonly produced in the form of sodium hydrogen periodate (Na3H2IO6).[3] This is commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide.[4] Or, similarly, from iodides by oxidation with bromine and sodium hydroxide:
Modern industrial scale production involves the
Sodium metaperiodate can be prepared by the dehydration of sodium hydrogen periodate with nitric acid.[3]
Structure
Sodium metaperiodate (NaIO4) forms
4 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.[6]
Sodium hydrogen periodate (Na2H3IO6) forms
Uses
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′-ends 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.[9]
In 2013 the
See also
- lead tetraacetate - also effective for diol cleavage via the Criegee oxidation
References
- ^ Record of Natriumperiodat in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2018-01-08.
- ^ ISBN 012126601X.)
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has generic name (help)CS1 maint: multiple names: authors list (link - .
- ^ Parsons, Roger (1959). Handbook of electrochemical constants. Butterworths Scientific Publications Ltd. p. 71.
- .
- .
- .
- ISBN 9780840054531.
- ^ "Picatinny to remove tons of toxins from lethal rounds". U.S. Army. Retrieved 31 October 2013.
- See Fatiadi, Synthesis (1974) 229–272 for a review of periodate chemistry.