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

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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. Taking high doses of iodine for long periods of time could change the way your thyroid gland works. Taking 0.5mg or less a day of iodine supplements is unlikely to cause any harm. What does the Department of Health and Social Care advise?

Vitamins and minerals - Iodine - NHS

Of the thirty-seven known isotopes of iodine, only one occurs in nature, iodine-127. The others are radioactive and have half-lives too short to be primordial. As such, iodine is both monoisotopic and mononuclidic and its atomic weight is known to great precision, as it is a constant of nature. [21] 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. 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]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. 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. 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 +

White Iodine Solution - Max Strength Decolourised 50ml 15% White Iodine Solution - Max Strength Decolourised

Unlike hydrogen fluoride, anhydrous liquid hydrogen iodide is difficult to work with as a solvent, because its boiling point is low, it has a small liquid range, its permittivity is low and it does not dissociate appreciably into H 2I + and HI − With the exception of the noble gases, nearly all elements on the periodic table up to einsteinium ( EsI 3 is known) are known to form binary compounds with iodine. Until 1990, nitrogen triiodide [51] was only known as an ammonia adduct. Ammonia-free NI 3 was found to be isolable at –196 °C but spontaneously decomposes at 0 °C. [52] For thermodynamic reasons related to electronegativity of the elements, neutral sulfur and selenium iodides that are stable at room temperature are also nonexistent, although S 2I 2 and SI 2 are stable up to 183 and 9 K, respectively. As of 2022, no neutral binary selenium iodide has been unambiguously identified (at any temperature). [53] Sulfur- and selenium-iodine polyatomic cations (e.g., [S 2I 4 2+][AsF 6 –] 2 and [Se 2I 4 2+][Sb 2F 11 –] 2) have been prepared and characterized crystallographically. [54] Iodine helps make thyroid hormones, which help keep cells and the metabolic rate (the speed at which chemical reactions take place in the body) healthy. Good sources of iodine The other iodine radioisotopes have much shorter half-lives, no longer than days. [29] Some of them have medical applications involving the thyroid gland, where the iodine that enters the body is stored and concentrated. Iodine-123 has a half-life of thirteen hours and decays by electron capture to tellurium-123, emitting gamma radiation; it is used in nuclear medicine imaging, including single photon emission computed tomography (SPECT) and X-ray computed tomography (X-Ray CT) scans. [36] Iodine-125 has a half-life of fifty-nine days, decaying by electron capture to tellurium-125 and emitting low-energy gamma radiation; the second-longest-lived iodine radioisotope, it has uses in biological assays, nuclear medicine imaging and in radiation therapy as brachytherapy to treat a number of conditions, including prostate cancer, uveal melanomas, and brain tumours. [37] Finally, iodine-131, with a half-life of eight days, beta decays to an excited state of stable xenon-131 that then converts to the ground state by emitting gamma radiation. It is a common fission product and thus is present in high levels in radioactive fallout. It may then be absorbed through contaminated food, and will also accumulate in the thyroid. As it decays, it may cause damage to the thyroid. The primary risk from exposure to high levels of iodine-131 is the chance occurrence of radiogenic thyroid cancer in later life. Other risks include the possibility of non-cancerous growths and thyroiditis. [38]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 ] Iodine is a chemical element with the symbol I and atomic number 53. The heaviest of the stable halogens, it exists at standard conditions as a semi-lustrous, non-metallic solid that melts to form a deep violet liquid at 114°C (237°F), and boils to a violet gas at 184°C (363°F). The element was discovered by the French chemist Bernard Courtois in 1811 and was named two years later by Joseph Louis Gay-Lussac, after the Ancient Greek Ιώδης 'violet-coloured'.