"Iodide accumulation provides kelp with an inorganic antioxidant impacting atmospheric chemistry" (Free full text). ^ Küpper FC Carpenter LJ McFiggans GB et al."Conversion of Iodide to Hypoiodous Acid and Iodine in Aqueous Microdroplets Exposed to Ozone". "In Raising the World's I.Q., the Secret's in the Salt". USA: National Center for Biotechnology Information. ^ "Iodide - PubChem Public Chemical Database".A number of neutral iodine oxides are also known. Iodine can assume oxidation states of −1, +1, +3, +5, or +7. Iodide anions may sometimes also be found combined with mercury, copper and lead, but minerals with such compositions are even more scarce.
Iodargyrite-natural, crystalline silver iodide-is the most common iodide mineral currently known. Photoactive component of silver-based photographic film → iodo-compounds + H 2O + 2 e − (antioxidants). Iodide can function as an antioxidant reducing species that can destroy ozone and reactive oxygen species such as hydrogen peroxide: 2 I − + peroxidase + H 2O 2 + tyrosine, histidine, lipid, etc. Its antioxidant properties can be expressed quantitatively as a redox potential :ĢI − ⇌ I 2 + E° = 0.54 volts (versus SHE)īecause iodide is easily oxidized, some enzymes readily convert it into electrophilic iodinating agents, as required for the biosynthesis of myriad iodide-containing natural products. A reducing agent is a chemical term for an antioxidant. Iodide salts are mild reducing agents and many react with oxygen to give iodine. This effect is due to the formation of the triiodide ion, which is brown:ģ Redox, including antioxidant properties Īqueous solutions of iodide salts dissolve iodine better than pure water. A test for the presence of iodide ions is the formation of yellow precipitates of these compounds upon treatment of a solution of silver nitrate or lead(II) nitrate. The low solubility of silver iodide and lead iodide reflects the covalent character of these metal iodides. One consequence of this is that sodium iodide is highly soluble in acetone, whereas sodium chloride is not. Iodide, being large, is less hydrophilic compared to the smaller anions. Most iodide salts are soluble in water, but often less so than the related chlorides and bromides. In part because of its size, iodide forms relatively weak bonds with most elements. For comparison, the lighter halides are considerably smaller: bromide (196 pm), chloride (181 pm), and fluoride (133 pm). It is assigned a radius of around 206 picometers. Iodide is one of the largest monatomic anions. Structure and characteristics of inorganic iodides 1.1 Redox, including antioxidant properties.1 Structure and characteristics of inorganic iodides.
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