what is iodized aluminum?
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Anodising, or anodizing, is a process used to protect aluminum from abrasion and corrosion and to allow it to be dyed in a wide range of colors. The process derives its name from the fact that the part to be treated forms the anode portion of an electrical circuit in this electrolytic process.\n\nAnodized aluminum can be found on paintball guns, carabiners, and other extreme sports equipment due to its aesthetic properties but also the protection it offers to aluminum.\n\nThe aluminum oxide coating is grown from and into the surface of the aluminum. Because of this (unlike coatings), it is not prone to peeling or cracking. It also possesses excellent thermal and electrical insulation qualities.
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It is not a combination of iron and tin, or anything else besides protons, electrons, and neutrons.\n\nThere's a naturally occurring ore called bauxite, which was discovered near Les Baux in the south of France, which is refined to produce aluminum.\n\nAt this link   \n\nhttp://volcano.und.edu/vwdocs/minerals/bauxite.html\n\nthere's a pie chart showing where it is mined today.  A lot of it comes from Australia, but that's not the only source.
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For the exterior, it is aluminum. However, multiple metals are used for the interior/engine etc., like titanium.
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lake test is the test for the identification of aluminium ions in a salt sample\nthe solution apparently containing Al ions is taken and to it is added ammonium hydroxide and ammonium chloride(excess)\nthe precipitate obtained is filtered, dried ,washed and dissolved in dilute nitric acid, followed by addition of two drops  of blue litmus solution. now excess ammonium hydroxide is added when a blue floating mass is obtained which is called as a lake.\nthis is called the lake test
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Silver iodide is released into the clouds which baically grabs hold of supercooled water droplets (water that is colder than ice but still liquid) and if the conditions are right, the supercooled water droplets will freeze, attract more water droplets and eventually form snowflakes....\n\nPlease understand that this is a very basic description but gives the idea...
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Aluminum as an ion has a 3+ charge, and oxygen as an ion has a 2- charge. So, to balance out these charges and get a neutral compound, the formula for aluminum oxide is Al2O3.\n\nAnd, no, aluminum oxide isn't just transparent aluminum. Definitely not. The crystal form of aluminum oxide is what's better known as rubies and sapphires.
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< < i·o·dine (ī'ə-dīn', -dĭn, -dēn') \nn.\n(Symbol I)2 A lustrous, grayish-black, corrosive, poisonous halogen element having radioactive isotopes, especially I 131, used as a medical tracer and in thyroid disease diagnosis and therapy. Iodine compounds are used as germicides, antiseptics, and dyes. Atomic number 53; atomic weight 126.9045; melting point 113.5°C; boiling point 184.35°C; specific gravity (solid, at 20°C) 4.93; valence 1, 3, 5, 7. \nA liquid containing iodine dissolved in ethyl alcohol, used as an antiseptic for wounds.\n[French iode, iodine (from Greek ioeidēs, violet-colored : ion, violet + -oeidēs, -oid) + –INE2.]\n\n\niodine (ī'ədīn, –dĭn) [Gr.,=violet], nonmetallic chemical element; symbol I; at. no. 53; at. wt. 126.9045; m.p. 113.5°C; b.p. 184.35°C; sp. gr. 4.93 at 20°C; valence −1, +1, +3, +5, or +7. Iodine is a dark-gray to purple-black, lustrous, solid element with a rhombic crystalline structure. It is the least active of the halogens, which are found in group VIIa of the periodic table. It is normally diatomic, i.e., it has 2 iodine atoms in each molecule, in the solid, liquid, and vapor states. When heated it passes directly from the solid to the vapor state (sublimation), the vapor having an intense violet color and a characteristic irritating odor. Iodine is only slightly soluble in water but dissolves readily in a solution of sodium or potassium iodide. Tincture of iodine is a solution of iodine and potassium iodide in alcohol. Iodine also dissolves in carbon disulfide, carbon tetrachloride, and chloroform, giving a deep violet solution. Iodine forms many compounds. With hydrogen it forms hydrogen iodide, which in water solution becomes hydriodic acid. It forms compounds with certain nonmetals (e.g., carbon, nitrogen, phosphorus, and oxygen) and with most metals. Iodine is displaced from its compounds by the other halogens. The element is obtained from salt deposits, as from the saltpeter beds in Chile, where it occurs in small quantities as an iodate, and from the salt brines associated with some oil wells in California and Louisiana. It is also found as an iodide in the ash of certain seaweeds. Iodine may be prepared by displacement from its compounds with chlorine. Treating an iodide with manganese dioxide and sulfuric acid sublimes the iodine. Iodine is important in medical treatment; tincture of iodine and iodoform are widely used. Iodine is employed in the preparation of certain drugs and in the manufacture of some dyes. Silver iodide, a yellow salt, is used in photography; it is water insoluble and turns black when exposed to light. Starch turns deep blue (almost black) in the presence of a small amount of iodine; this reaction serves as a test for either starch or iodine. Iodine in small amounts is essential to human nutrition; in the thyroid gland it becomes a part of the iodine-containing hormones. Goiter, a swelling of the thyroid, is often a symptom of inadequate iodine in the diet. Iodine has only one stable isotope, iodine–127; it is the only isotope of iodine occurring in nature, although 24 iodine isotopes are known. Iodine–131 is a radioactive isotope with a half-life of 8 days. It is used medically to diagnose abnormalities of the thyroid gland. It is also a component of fallout produced by nuclear explosions. Iodine was discovered in 1811 by Bernard Courtois.
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China Clay is a naturally hydrated Aluminium Silicate.  The chemical formula is Al2Si2O5(OH)4..
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why do you need it?  how much do you want to spend to figure out what it is, or what alloy it is. \n\nyou can just do the density measurement\nmeasure the radius of the wire and length. \ndo the pi r squared length deal and then weigh it, and run it through the density equation. \n\nyou need a ruler and a calipers or micrometer that reads in inches. \n\nso lets say you have .125 inch wire.  divide that by 2 to get the radius. =  .0625"\nthen square it.  .0039" and multiply by 3.14. \n\nand multiply it by the length in inches  \n\nthen weigh it.  in lbs. \n\ndensity of al is between .096 lb/cu in. and .100 lb/cu in\n\nyou might want to buy wire that is certified as the type of aluminum you need.  the stuff is cheap.  you can get at the electical supply store or maybe a hardware store. \n\nwiring used for electical applications is 8000 series alloy for modern applications \n\nolder wire is 1350 alloy.
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B.\n\nthe process is called passivation. and may be increased to a greater extent on purpose by electrolysing aluminum in acid to increase the oxide layer. this is called anodizing.
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Arsenic is the metal, but at temperatures much lower than its melting point (not boiling point).  It sublimes at 614 degrees C and melts under pressure at 817 degrees C.\n\nAlthough Iodine has a metallic luster, it is not a metal.  It sublimes (evaporates) near its \nMelting Point of 114 degrees C.\n\nSee the reference below:
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If the bottle says 3.1 % v/v this the bottle is not labeled correctly.  Iodine is a solid and the label should have said 3.1 % w/v.  This means that there is 3.1 grams of iodine in every 100 mL of solution.\nThe 1 % titratable iodine means that the free (not bound to other substances) iodine is at least one percent of the solution.  Iodine concentration is often determined by titration with sodium or potassium thiosulate.\nYour bottle of Iodine is probably an aqueous (in water) solution.  Tinctures are made by dissolving iodine in denatured ethyl (grain) alcohol or 70 % isopropyl (rubbing) alcohol.
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Alright, I looked up the history of the spelling of Aluminum.  We Americans don't, in truth, spell it incorrectly.  There are simply two variant spellings.  See below:\n\n"Etymology/nomenclature history\nThe earliest citation given in the Oxford English Dictionary for any word used as a name for this element is alumium, which Humphry Davy employed in 1808 for the metal he was trying to isolate electrolytically from the mineral alumina. The citation is from his journal Philosophical Transactions: "Had I been so fortunate as..to have procured the metallic substances I was in search of, I should have proposed for them the names of silicium, alumium, zirconium, and glucium." [11]\n\nBy 1812, Davy had settled on aluminum, which, as other sources note, matches its Latin root. He wrote in the journal Chemical Philosophy: "As yet Aluminum has not been obtained in a perfectly free state."[12] But the same year, an anonymous contributor to the Quarterly Review, a British political-literary journal, objected to aluminum and proposed the name aluminium, "for so we shall take the liberty of writing the word, in preference to aluminum, which has a less classical sound." [13]\n\nThe -ium suffix had the advantage of conforming to the precedent set in other newly discovered elements of the period: potassium, sodium, magnesium, calcium, and strontium (all of which Davy had isolated himself). Nevertheless, -um spellings for elements were not unknown at the time, as for example platinum, known to Europeans since the 16th century, molybdenum, discovered in 1778, and tantalum, discovered in 1802.\n\nAmericans adopted -ium for most of the 19th century, with aluminium appearing in Webster's Dictionary of 1828. In 1892, however, Charles Martin Hall used the -um spelling in an advertising handbill for his new electrolytic method of producing the metal, despite his constant use of the -ium spelling in all the patents he filed between 1886 and 1903. Hall's domination of production of the metal ensured that the spelling aluminum became the standard in North America; the Webster Unabridged Dictionary of 1913, though, continued to use the -ium version.\n\nIn 1926, the American Chemical Society officially decided to use aluminum in its publications; American dictionaries typically label the spelling aluminium as a British variant"
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It is treated with Bromine which displaces the Iodine
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Iodine is used to identify the presence of starch in a cell.  The most likely source would be a plant cell vacuole that contained large amounts of starch.  In Microbiology iodine is used as a morduant to fix the first stain of Grams stain (crystal violet).
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You could work out that in I2O7, the iodine is in a +7 oxidation state, so it can't go any higher.\nSimilarly, in Cl- it is -1, and it can't go any lower.
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Nitrogen triiodide, also called ammonium triiodide or nitrogen iodide, is a highly explosive compound of nitrogen and iodine, NI3. It is a contact explosive, and small quantities explode with a gunpowder-like snap when touched by even a feather, releasing a volatile cloud of iodine vapor. The decomposition of nitrogen triiodide occurs via the following reaction:\n\n    2NI3 (s) → N2 (g) + 3I2 (g)\n\nPure nitrogen triiodide is a dark red compound, first prepared in 1990 by reaction of boron nitride with iodine monofluoride in trichlorofluoromethane at -30°C.\n\nThe compound usually referred to as nitrogen triiodide is an ammonia adduct, NI3·NH3, synthesized by reacting iodine with ammonia. It was first prepared by Bernard Courtois in 1812, and its formula was finally determined unequivocally in 1905 by Silberrad.[1] Its solid state structure consists of zig-zag chains of corner-sharing NI4 tetrahedra, with ammonia molecules between the chains.\n\nSmall amounts of nitrogen triiodide are sometimes synthesized as a demonstration to high school chemistry students. However, because the compound is so unstable, it has not been used in blasting caps or primers for explosives. While still wet, nitrogen triiodide is safer to handle than the dry compound, but is still prone to spontaneous explosion. NI3·NH3 explosions leave orange-to-purple iodine stains that are difficult to wash. However, they can be easily removed by sodium thiosulfate solution. (wikipedia.com)