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NaIO 3 sodium iodate + Cl 2 + 4 NaOH ⟶ Na 3 H 2 IO 6 + 2 NaCl + H 2 O {\displaystyle {\ce {{\overset {sodium\ iodate}{NaIO3}}+Cl2{}+4NaOH->Na3H2IO6{}+2NaCl{}+H2O}}} NaI + 4 Br 2 + 10 NaOH ⟶ Na 3 H 2 IO 6 + 8 NaBr + 4 H 2 O {\displaystyle {\ce {NaI + 4 Br2 + 10 NaOH -> Na3H2IO6 + 8 NaBr + 4 H2O}}} Feikema, Y. D. (10 June 1966). "The crystal structures of two oxy-acids of iodine. I. A study of orthoperiodic acid, H 5IO 6, by neutron diffraction". Acta Crystallographica. 20 (6): 765–769. doi: 10.1107/S0365110X66001828. Metaperiodates are typically prepared by the dehydration of sodium hydrogen periodate with nitric acid, [2] or by dehydrating orthoperiodic acid by heating it to 100 °C under vacuum. Sodium hydrogen periodate (Na 2H 3IO 6) forms orthorhombic crystals (space group Pnnm). Iodine and sodium atoms are both surrounded by an octahedral arrangement of 6 oxygen atoms; however the NaO 6 octahedron is strongly distorted. IO 6 and NaO 6 groups are linked via common vertices and edges. [7] lone pairs. One oxygen atom will take three lone pairs following the octal rule (oxygen atoms cannot keep more than

Periodic acid is also used as an oxidising agent of moderate strength, as exemplified in the Babler oxidation of secondary allyl alcohols which are oxidised to enones by stoichiometric amounts of orthoperiodic acid with catalyst PCC. [12] Other oxyacids [ edit ] There are four oxygen atoms and iodine atom in periodate ion. Iodine atom is located at the center and there is a -1 charge on one oxygen atom. Now, there are fourteen electrons around iodine atom. This is acceptable because iodine can keep more than eightPeriodic acid was discovered by Heinrich Gustav Magnus and C. F. Ammermüller in 1833. [3] Synthesis [ edit ] Each oxygen atom has a -1 charge and iodine has a +3 charge. Having so many charges on atoms on a structure is Classically, periodate was most commonly produced in the form of sodium hydrogen periodate ( Na 3H 2IO 6). [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: Sodium metaperiodate (NaIO 4) forms tetragonal crystals ( space group I4 1/ a) consisting of slightly distorted IO − Periodates were discovered by Heinrich Gustav Magnus and C. F. Ammermüller; who first synthesised periodic acid in 1833. [1] Synthesis [ edit ]

H 5 IO 6 + H + + 2 e − ⟶ IO 3 − + 3 H 2 O {\displaystyle {\ce {H5IO6 + H+ + 2e- -> IO3- + 3 H2O}}} E° = 1.6 V [5] a b Riley, edited by Georg Brauer; translated by Scripta Technica, Inc. Translation editor Reed F. (1963). Handbook of preparative inorganic chemistry. Volume 1 (2nded.). New York, N.Y.: Academic Press. pp.323–324. ISBN 012126601X. {{ cite book}}: |first= has generic name ( help) CS1 maint: multiple names: authors list ( link)H 5IO 6 ⇌ H 4IO − 6 + H +, p K a=3.29 H 4IO − 6 ⇌ H 3IO 2− 6 + H +, p K a=8.31 H 3IO 2− 6 ⇌ H 2IO 3− 6 + H +, p K a=11.60 Orthoperiodic acid can be dehydrated to give metaperiodic acid by heating to 100°C under reduced pressure.

Greenwood, N. N.; Earnshaw, A (1997). Chemistry of the elements (2nded.). Butterworth-Heinemann. p.872. doi: 10.1016/C2009-0-30414-6. ISBN 978-0-7506-3365-9. Modern industrial scale production involves the oxidation of a solution of sodium iodate under alkaline conditions, either electrochemically on a PbO 2 anode, or by treatment with chlorine: [4] IO − 3 + 6 HO − - 2 e − → IO 5− 6 + 3 H 2O ( counter ions omitted for clarity) E°=-1.6V [5] IO − 3 + 6 HO − + Cl 2 → IO 5− 6 + 2 Cl − + 3 H 2O Orthoperiodic acid has a number of acid dissociation constants. [7] [8] The p K a of metaperiodic acid has not been determined.Aylett, founded by A.F. Holleman; continued by Egon Wiberg; translated by Mary Eagleson, William Brewer; revised by Bernhard J. (2001). Inorganic chemistry (1st English ed., [edited] by Nils Wiberg.ed.). San Diego, Calif.: Berlin: Academic Press, W. de Gruyter. p.453. ISBN 0123526515. {{ cite book}}: CS1 maint: multiple names: authors list ( link)