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sodium periodate

{{Chembox

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 464402875

| ImageFile = Sodium metaperiodate.svg

| ImageSize = 150px

| IUPACName = Sodium periodate

| OtherNames = Sodium metaperiodate

|Section1={{Chembox Identifiers

| index_label=meta

| index1_label=para

| index2_label=ortho

| index3_label=trihydrogen

| Abbreviations =

| InChI = 1/HIO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1

| InChIKey = JQWHASGSAFIOCM-REWHXWOFAO

| CASNo = 7790-28-5

| CASNo1 = 13940-38-0

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo3 = 15599-97-0

| EC_number3 = 239-681-6

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 98W4A29X43

| EINECS = 232-197-6

| EC_number1 = 237-720-1

| PubChem = 23667635

| PubChem1 = 9796123

| PubChem2 = 21982945

| PubChem3 = 22765006

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID = 58683

| ChemSpiderID1 = 7971889

| ChemSpiderID3 = 129318857

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey = JQWHASGSAFIOCM-UHFFFAOYSA-M

| SMILES = [O-]I(=O)(=O)=O.[Na+]

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChI = 1S/HIO4.Na/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1

| RTECS = SD4550000

| MeSHName =

| ChEBI_Ref = {{ebicite|changed|EBI}}

| ChEBI = 75226

| KEGG_Ref = {{keggcite|correct|kegg}}

| KEGG =

| QID1 = Q4161310

| QID3 = Q17388101

| InChI1=1S/H5IO6.3Na/c2-1(3,4,5,6)7;;;/h(H5,2,3,4,5,6,7);;;/q;3*+1/p-3

| InChIKey1 = DSYMXPNUZLZKOA-UHFFFAOYSA-K

| SMILES1 = OI(=O)(O)([O-])([O-])[O-].[Na+].[Na+].[Na+]

| InChI2=1S/H5IO6.5Na/c2-1(3,4,5,6)7;;;;;/h(H5,2,3,4,5,6,7);;;;;/q;5*+1/p-5

| InChIKey2 = RAJUJHHGBPSUAC-UHFFFAOYSA-I

| SMILES2 = [O-]I(=O)([O-])([O-])([O-])[O-].[Na+].[Na+].[Na+].[Na+].[Na+]

| InChI3=1S/H5IO6.2Na/c2-1(3,4,5,6)7;;/h(H5,2,3,4,5,6,7);;/q;2*+1/p-2

| InChIKey3 = PEPDKRLBEGSBRW-UHFFFAOYSA-L

| SMILES3 = OI(=O)(O)(O)([O-])[O-].[Na+].[Na+]

}}

|Section2={{Chembox Properties

| Formula = NaIO4

| MolarMass = 213.8918 g/mol

| Appearance = white crystals

| Density = 3.865 g/cm3 (anhydrous)
3.210 g/cm3

| MeltingPt = {{convert|300|C|F K}} (anhydrous)
{{convert|175|C|F K}} (trihydrate)

| MeltingPt_notes = (decomposes)

| BoilingPt =

| BoilingPt_notes =

| Solubility = 91 g/L{{GESTIS|Name=Natriumperiodat|ZVG=490496|CAS=7790-28-5|Date=2018-01-08}}

| SolubleOther = soluble in acids

| Solvent =

| pKa =

| pKb =

}}

|Section3={{Chembox Structure

| CrystalStruct = tetragonal (anhydrous)
trigonal (trihydrate)

}}

|Section7={{Chembox Hazards

| ExternalSDS =

| MainHazards =

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 3

| NFPA-S = ox

| HPhrases =

| PPhrases =

| GHS_ref =

| FlashPt =

| AutoignitionPt =

| ExploLimits =

| PEL =

}}

|Section8={{Chembox Related

| OtherAnions = sodium perchlorate, sodium perbromate

| OtherCations = potassium periodate, periodic acid}}

}}

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 many periodates, it can exist in two different forms: sodium metaperiodate (formula‍ NaIO4) and sodium orthoperiodate (normally Na2H3IO6, but sometimes the fully reacted salt Na5IO6). Both salts are useful oxidising agents.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}}

Preparation

Classically, periodate was produced in the form of sodium hydrogen periodate ({{chem2|Na3H2IO6}}). This commercially available, but can also be produced by the oxidation of iodates with chlorine and sodium hydroxide.{{cite book|author=M. Schmeisser|chapter=Periodic acid|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY,NY|volume=2pages=323}}{{cite journal|last=Hill|first=Arthur E.|title=Ternary Systems. VII. The Periodates of the Alkali Metals|journal=Journal of the American Chemical Society|date=October 1928|volume=50|issue=10|pages=2678–2692|doi=10.1021/ja01397a013|bibcode=1928JAChS..50.2678H }} Or, similarly, from iodides by oxidation with bromine and sodium hydroxide:

:{{chem2| NaIO3 + Cl2 + 4 NaOH -> Na3H2IO6 + 2NaCl + H2O}}

:{{chem2|NaI + 4 Br2 + 10 NaOH -> Na3H2IO6 + 8 NaBr + 4 H2O}}

Modern industrial scale production involves the electrochemical oxidation of iodates, on a lead dioxide ({{chem2|PbO2}}) anode, with the following standard electrode potential:

:{{chem2|H5IO6 + H+ + 2e- -> IO3- + 3 H2O}}{{spaces|5}}{{nowrap|1=E° = 1.6 V}}{{cite book|last=Parsons|first=Roger|title=Handbook of electrochemical constants|url=https://archive.org/details/ost-chemistry-parsons-handbookofelectrochemicalconstants|year=1959|publisher=Butterworths Scientific Publications Ltd|page=[https://archive.org/details/ost-chemistry-parsons-handbookofelectrochemicalconstants/page/n41 71]}}

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

:{{chem2|Na3H2IO6 + 2 HNO3 -> NaIO4 + 2 NaNO3 + 2 H2O}}

Structure

Sodium metaperiodate (NaIO4) forms tetragonal crystals (space group I41/a) consisting of slightly distorted {{chem|IO|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.{{cite journal|last=Kálmán|first=A.|author2=Cruickshank, D. W. J. |title=Refinement of the structure of NaIO4|journal=Acta Crystallographica Section B|date=15 November 1970|volume=26|issue=11|pages=1782–1785|doi=10.1107/S0567740870004880|bibcode=1970AcCrB..26.1782K }}

Sodium hydrogen periodate (Na2H3IO6) forms orthorhombic crystals (space group Pnnm). Iodine and sodium atoms are both surrounded by an octahedral arrangement of 6 oxygen atoms; however the NaO6 octahedron is strongly distorted. IO6 and NaO6 groups are linked via common vertices and edges.{{cite journal|last=Jansen|first=Martin|author2=Rehr, Anette |title=Na2H3IO6, eine Variante der Markasitstruktur|journal=Zeitschrift für anorganische und allgemeine Chemie|date=1988|volume=567|issue=1|pages=95–100|doi=10.1002/zaac.19885670111|language=de}}

Powder diffraction indicates that Na5IO6 crystallises in the monoclinic system (space group C2/m).{{cite journal|last=Betz|first=T.|author2=Hoppe, R. |title=Über Perrhenate. 2. Zur Kenntnis von Li5ReO6 und Na5ReO6 – mit einer Bemerkung über Na5IO6|journal=Zeitschrift für anorganische und allgemeine Chemie|date=May 1984|volume=512|issue=5|pages=19–33|doi=10.1002/zaac.19845120504|language=de}}

Uses

{{further|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′-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.{{cite book|last=McMurry|first=John|title=Organic chemistry|date=2012 |publisher=Brooks/Cole Cengage Learning|location=Singapore|isbn=9780840054531|pages=285–286|edition=8th ed., [international ed.]}}

File:Periodate cleavage.svg

In 2013 the US Army announced that it would replace environmentally harmful chemicals barium nitrate and potassium perchlorate with sodium metaperiodate for use in their tracer ammunition.{{cite web|title=Picatinny to remove tons of toxins from lethal rounds|date=19 September 2013 |url=https://www.army.mil/article/109769/Picatinny_to_remove_tons_of_toxins_from_lethal_rounds/|publisher=U.S. Army|access-date=31 October 2013}}

See also

References

{{reflist}}

  • See Fatiadi, Synthesis (1974) 229–272 for a review of periodate chemistry.

{{Sodium compounds}}

{{Periodates}}

{{DEFAULTSORT:Sodium Periodate}}

Category:Periodates

Category:Sodium compounds

Category:Oxidizing agents