30ml 15% White Iodine Solution Max Strength Decolourised Clear Solution

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At room temperature, it is a colourless gas, like all of the hydrogen halides except hydrogen fluoride, since hydrogen cannot form strong hydrogen bonds to the large and only mildly electronegative iodine atom. It melts at −51.0°C and boils at −35.1°C. It is an endothermic compound that can exothermically dissociate at room temperature, although the process is very slow unless a catalyst is present: the reaction between hydrogen and iodine at room temperature to give hydrogen iodide does not proceed to completion. The H–I bond dissociation energy is likewise the smallest of the hydrogen halides, at 295kJ/mol. [47] R = Me, Et, Bu n) may still be isolated. Anhydrous hydrogen iodide is a poor solvent, able to dissolve only small molecular compounds such as nitrosyl chloride and phenol, or salts with very low lattice energies such as tetraalkylammonium halides. [47] Other binary iodine compounds [ edit ]

white iodine - IODINE RESOURCE white iodine - IODINE RESOURCE

and the various periodate anions. It is the least abundant of the stable halogens, being the sixty-first most abundant element. As the heaviest essential mineral nutrient, iodine is required for the synthesis of thyroid hormones. [5] Iodine deficiency affects about two billion people and is the leading preventable cause of intellectual disabilities. [6] Place two spatulas of the food sample into a test tube or 1 cm 3 if the sample is liquid. Add about 1 cm 3 depth of water to the tube and stir to mix.monosaccharides – such as glucose close glucose A simple sugar used by cells for respiration. and fructose close fructose A monosaccharide which joins with glucose to make sucrose. Lower iodides may be produced either through thermal decomposition or disproportionation, or by reducing the higher iodide with hydrogen or a metal, for example: [55] TaI 5 + Ta → 630 ∘ C ⟶ 575 ∘ C thermal gradient Ta 6 I 14 {\displaystyle {\ce {TaI5{}+Ta->[{\text{thermal gradient}}][{\ce {630 due to the very weak hydrogen bonding between hydrogen and iodine, though its salts with very large and weakly polarising cations such as Cs + and NR +

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The Vegan Society has more information about iodine and vegan diets What happens if I take too much iodine? The melting and boiling points of iodine are the highest among the halogens, conforming to the increasing trend down the group, since iodine has the largest electron cloud among them that is the most easily polarised, resulting in its molecules having the strongest van der Waals interactions among the halogens. Similarly, iodine is the least volatile of the halogens, though the solid still can be observed to give off purple vapor. [21] Due to this property iodine is commonly used to demonstrate sublimation directly from solid to gas, which gives rise to a misconception that it does not melt in atmospheric pressure. [27] Because it has the largest atomic radius among the halogens, iodine has the lowest first ionisation energy, lowest electron affinity, lowest electronegativity and lowest reactivity of the halogens. [21] Structure of solid iodine The iodine molecule, I 2, dissolves in CCl 4 and aliphatic hydrocarbons to give bright violet solutions. In these solvents the absorption band maximum occurs in the 520 – 540nm region and is assigned to a π * to σ * transition. When I 2 reacts with Lewis bases in these solvents a blue shift in I 2 peak is seen and the new peak (230 – 330nm) arises that is due to the formation of adducts, which are referred to as charge-transfer complexes. [45] Hydrogen iodide [ edit ]

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The halogens darken in colour as the group is descended: fluorine is a very pale yellow, chlorine is greenish-yellow, bromine is reddish-brown, and iodine is violet. In 1873 the French medical researcher Casimir Joseph Davaine (1812–1882) discovered the antiseptic action of iodine. [18] Antonio Grossich (1849–1926), an Istrian-born surgeon, was among the first to use sterilisation of the operative field. In 1908, he introduced tincture of iodine as a way to rapidly sterilise the human skin in the surgical field. [19] Aqueous hydrogen iodide is known as hydroiodic acid, which is a strong acid. Hydrogen iodide is exceptionally soluble in water: one litre of water will dissolve 425 litres of hydrogen iodide, and the saturated solution has only four water molecules per molecule of hydrogen iodide. [48] Commercial so-called "concentrated" hydroiodic acid usually contains 48–57% HI by mass; the solution forms an azeotrope with boiling point 126.7°C at 56.7g HI per 100g solution. Hence hydroiodic acid cannot be concentrated past this point by evaporation of water. [47] Unlike gaseous hydrogen iodide, hydroiodic acid has major industrial use in the manufacture of acetic acid by the Cativa process. [49] [50] Iodine can also be found in plant foods, such as cereals and grains, but the levels vary depending on the amount of iodine in the soil where the plants are grown. How much iodine do I need? Given the large size of the iodide anion and iodine's weak oxidising power, high oxidation states are difficult to achieve in binary iodides, the maximum known being in the pentaiodides of niobium, tantalum, and protactinium. Iodides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydroiodic acid, and then dehydrated by mildly high temperatures combined with either low pressure or anhydrous hydrogen iodide gas. These methods work best when the iodide product is stable to hydrolysis. Other syntheses include high-temperature oxidative iodination of the element with iodine or hydrogen iodide, high-temperature iodination of a metal oxide or other halide by iodine, a volatile metal halide, carbon tetraiodide, or an organic iodide. For example, molybdenum(IV) oxide reacts with aluminium(III) iodide at 230°C to give molybdenum(II) iodide. An example involving halogen exchange is given below, involving the reaction of tantalum(V) chloride with excess aluminium(III) iodide at 400°C to give tantalum(V) iodide: [55] 3 TaCl 5 + 5 AlI 3 ( excess ) ⟶ 3 TaI 5 + 5 AlCl 3 {\displaystyle {\ce {3TaCl5 + {\underset {(excess)}{5AlI3}}-> 3TaI5 + 5AlCl3}}}

Iodine - Wikipedia

Taking high doses of iodine for long periods of time could change the way your thyroid gland works. If you are following a strict vegan diet and do not eat any fish, eggs, cows' milk or other dairy products, then you may want to consider foods fortified with iodine or consider taking an iodine supplement.The longest-lived of the radioactive isotopes of iodine is iodine-129, which has a half-life of 15.7millionyears, decaying via beta decay to stable xenon-129. [29] Some iodine-129 was formed along with iodine-127 before the formation of the Solar System, but it has by now completely decayed away, making it an extinct radionuclide that is nevertheless still useful in dating the history of the early Solar System or very old groundwaters, due to its mobility in the environment. Its former presence may be determined from an excess of its daughter xenon-129. [30] [31] [32] [33] [34] Traces of iodine-129 still exist today, as it is also a cosmogenic nuclide, formed from cosmic ray spallation of atmospheric xenon: these traces make up 10 −14 to 10 −10 of all terrestrial iodine. It also occurs from open-air nuclear testing, and is not hazardous because of its very long half-life, the longest of all fission products. At the peak of thermonuclear testing in the 1960s and 1970s, iodine-129 still made up only about 10 −7 of all terrestrial iodine. [35] Excited states of iodine-127 and iodine-129 are often used in Mössbauer spectroscopy. [21] The dominant producers of iodine today are Chile and Japan. Due to its high atomic number and ease of attachment to organic compounds, it has also found favour as a non-toxic radiocontrast material. Because of the specificity of its uptake by the human body, radioactive isotopes of iodine can also be used to treat thyroid cancer. Iodine is also used as a catalyst in the industrial production of acetic acid and some polymers.