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Iodate is one of several oxyanions of iodine, and has an oxidation number of +5. It participates in several redox reactions, such as the iodine clock reaction. Iodate shows no tendency to disproportionate to periodate and iodide, in contrast to the situation for chlorate. Iodate is reduced by sulfite: [1] 6HSO − 3 + 2IO − 3 → 2I − ...
Periodate (/ p ə ˈ r aɪ. ə d eɪ t / pə-RY-ə-dayt) 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.
An oxyanion, or oxoanion, is an ion with the generic formula A x O z− y (where A represents a chemical element and O represents an oxygen atom). Oxyanions are formed by a large majority of the chemical elements. [1] The formulae of simple oxyanions are determined by the octet rule. The corresponding oxyacid of an oxyanion is the compound H z ...
In this protocol, iodide ion is generated by the following slow reaction between the iodate and bisulfite: IO − 3 + 3 HSO − 3 → I − + 3 HSO − 4. This first step is the rate determining step. Next, the iodate in excess will oxidize the iodide generated above to form iodine: IO − 3 + 5 I − + 6 H + → 3 I 2 + 3 H 2 O
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Hypervalent iodine oxyanions are known for oxidation states +1, +3, +5, and +7; organic analogues of these moieties are known for each oxidation state except +7. In terms of chemical behavior, λ 3 ‑ and λ 5 ‑iodanes are generally oxidizing and/or electrophilic species. They have been widely applied towards those ends in organic synthesis. [1]
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A fluorooxoiodate or fluoroiodate is a chemical compound or ion derived from iodate, by substituting some of the oxygen by fluorine. They have iodine in the +5 oxidation state. The iodine atoms have a stereochemically active lone-pair of electrons.