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

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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] 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 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]

15% White Iodine - Essential Minerals

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] The Vegan Society has more information about iodine and vegan diets What happens if I take too much iodine? In early periodic tables, iodine was often given the symbol J, for Jod, its name in German. [20] Properties [ edit ] Iodine vapour in a flask.

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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. Iodine is quite reactive, but it is much less reactive than the other halogens. For example, while chlorine gas will halogenate carbon monoxide, nitric oxide, and sulfur dioxide (to phosgene, nitrosyl chloride, and sulfuryl chloride respectively), iodine will not do so. Furthermore, iodination of metals tends to result in lower oxidation states than chlorination or bromination; for example, rhenium metal reacts with chlorine to form rhenium hexachloride, but with bromine it forms only rhenium pentabromide and iodine can achieve only rhenium tetraiodide. [21] By the same token, however, since iodine has the lowest ionisation energy among the halogens and is the most easily oxidised of them, it has a more significant cationic chemistry and its higher oxidation states are rather more stable than those of bromine and chlorine, for example in iodine heptafluoride. [23] Charge-transfer complexes [ edit ] 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? 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 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.

Iodine - Wikipedia

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 ] 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 {630Unlike 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 − 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 + 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]