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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. Riley (1963). Brauer, Georg (ed.). Handbook of preparative inorganic chemistry. Volume 1. Translated by Scripta Technica, Inc. Translation editor Reed F. (2nded.). New York, N.Y.: Academic Press. pp.323–324. ISBN 012126601X. 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] 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 ] Na 3 H 2 IO 6 + 2 HNO 3 ⟶ NaIO 4 + 2 NaNO 3 + 2 H 2 O {\displaystyle {\ce {Na3H2IO6 + 2 HNO3 -> NaIO4 + 2 NaNO3 + 2 H2O}}} H 5 IO 6 ⟶ HIO 4 + 2 H 2 O {\displaystyle {\ce {H5IO6 -> HIO4 + 2 H2O}}}

There are one iodine atom and four oxygen atoms in the periodate ion. Also there is a -1 overall charge on Next step is, marking those twelve valence electrons pairs on outside atoms (in this case, oxygen atoms) as Burgot, Jean-Louis (2012-03-30). Ionic equilibria in analytical chemistry. New York: Springer. p.358. ISBN 978-1441983824. To be the center atom, ability of having greater valance is important. Iodine can show valence upto 7. But,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: Periodate / p ə ˈ r aɪ . ə d eɪ t/ 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 − 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. 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. [10] See also [ edit ] 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]

ions with average I–O bond distances of 1.775Å; the Na + ions are surrounded by 8 oxygen atoms at distances of 2.54 and 2.60Å. [6] They can also be generated directly from iodates by treatment with other strong oxidizing agents such as hypochlorites: Sodium metaperiodate can be prepared by the dehydration of sodium hydrogen periodate with nitric acid. [3] Na 3 H 2 IO 6 + 2 HNO 3 ⟶ NaIO 4 + 2 NaNO 3 + 2 H 2 O {\displaystyle {\ce {Na3H2IO6 + 2 HNO3 -> NaIO4 + 2 NaNO3 + 2 H2O}}} Structure [ edit ] Fábry, J.; Podlahová, J.; Loub, J.; Langer, V. (1982). "Structure of the 1:1 adduct of orthoperiodic acid and urea". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 38 (3): 1048–1050. doi: 10.1107/S0567740882004932.Orthoperiodic acid has a number of acid dissociation constants. [7] [8] The p K a of metaperiodic acid has not been determined. 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. Jansen, Martin; Rehr, Anette (1988). "Na 2H 3IO 6, eine Variante der Markasitstruktur". Zeitschrift für anorganische und allgemeine Chemie (in German). 567 (1): 95–100. doi: 10.1002/zaac.19885670111. 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 Like all periodates periodic acid can be used to cleave various 1,2-difunctional compounds. Most notably periodic acid will cleave vicinal diols into two aldehyde or ketone fragments ( Malaprade reaction).

Further heating to around 150°C gives iodine pentoxide ( I 2O 5) rather than the expected anhydride diiodine heptoxide ( I 2O 7). Metaperiodic acid can also be prepared from various orthoperiodates by treatment with dilute nitric acid. [6] Betz, T.; Hoppe, R. (May 1984). "Über Perrhenate. 2. Zur Kenntnis von Li 5ReO 6 und Na 5ReO 6 – mit einer Bemerkung über Na 5IO 6". Zeitschrift für anorganische und allgemeine Chemie (in German). 512 (5): 19–33. doi: 10.1002/zaac.19845120504. 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}}} Classically, periodate was most commonly produced in the form of sodium hydrogen periodate ( Na 3H 2IO 6). [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: If charges exist on atoms, they should be marked on now. Marking charges of atoms is important because it is

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 [4] 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. Periodic acid ( / ˌ p ɜːr aɪ ˈ ɒ d ɪ k/ per-eye- OD-ik) is the highest oxoacid of iodine, in which the iodine exists in oxidation state +7. It can exist in two forms: orthoperiodic acid, with the chemical formula H 5IO 6, and metaperiodic acid, which has the formula HIO 4.