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Potassium iodate, KIO 3, like potassium iodide, has been issued as a prophylaxis against radioiodine absorption in some countries. [4] [5] It is also one of the iodine compounds used to make iodized salt. [6] Potassium hydrogen iodate (or potassium biiodate), KH(IO 3) 2, is a double salt of potassium iodate and iodic acid, as well as an acid ...
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.
A fundamental property of this system is that hydrogen peroxide has a redox potential which enables the simultaneous oxidation of iodine to iodate: 5 H 2 O 2 + I 2 → 2 IO − 3 + 2 H + + 4 H 2 O. and the reduction of iodate back to iodine: 5 H 2 O 2 + 2 IO − 3 + 2 H + → I 2 + 5 O 2 + 6 H 2 O
Iodous acid and iodite are even less stable and exist only as a fleeting intermediate in the oxidation of iodide to iodate, if at all. [13] Iodates are by far the most important of these compounds, which can be made by oxidising alkali metal iodides with oxygen at 600 °C and high pressure, or by oxidising iodine with chlorates .
Shape of water molecule showing that the real bond angle 104.5° deviates from the ideal sp 3 angle of 109.5°.. In chemistry, Bent's rule describes and explains the relationship between the orbital hybridization and the electronegativities of substituents.
The I-F bond is about 0.2 Å longer than the I-O bond. The fluorine atoms repel each other in [IO 2 F 2 ] − and are almost opposite each other. The ∠OIF angle is close to 90° and the oxygen atoms ∠OFO are at about 102°, [ 2 ] so they resemble an octahedral arrangement, with two adjacent positions deleted.
An alternative protocol uses a solution of iodate ion (for instance potassium iodate) to which an acidified solution (again with sulfuric acid) of sodium bisulfite is added. [3] 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
When iodic acid acts as oxidizer, then the product of the reaction is either iodine, or iodide ion. Under some special conditions (very low pH and high concentration of chloride ions, such as in concentrated hydrochloric acid), iodic acid is reduced to iodine trichloride , a golden yellow compound in solution and no further reduction occurs.