what happens to iodine and magnesium when mixed and heated?
821448
maybe forming an MgI2
179839
It depends on the salt. A salt of calcium, magnesium, or iron will form an insoluble compound that will precipitate with a soap molecule that is known as soap scum.\n\nHere is a typical reaction:\nCa2+(aq)  + 2C17H35COO-(aq)  ==> (C17H35COO-)2Ca2+(s)\n\nSodium chloride will not form a precipitate with soap as long as the soap is a carboxylate.\nhttp://dl.clackamas.cc.or.us/ch106-04/structur1.htm
810145
depends what the magnesium is for. If this is for a chemical reaction, it's because copper is less reactive than magnesium (it's lower on the activity series list).
442899
Manganese and manganese dioxide. Also potassium iodide does a good job.
659725
Magnesium will react with any gas except noble gases when heated, because of its low electronegativity. In vacuum or noble gas atmosphere it can be heated up to melting point of 625°C, just at or below red glow.\n\nWhile red or white hot iron will oxidize on the surface, the heat released by that process is not sufficient to start a chain reaction like in burning magnesium. The higher melting point of iron depends mostly on the crystal lattice of iron.
277253
MgCl + H2O = MgO + H2Cl
701112
If Br water ismixed with KI the Br will replace the I in KI and make Kbr and free I2(diatomic) It is not terribly soluble in water. It could buble out as a violet gas if the temp were high enough. \n\nIf KF is mixed with Cl water no reaction because Cl will not replace F. They will replace each oter from bottom up. Nothing replaces F.
727675
Magnesium reacts with water to produce hydrogen.  It's salts are water soluble.
977174
Removal and recovery of magnesium, strontium and barium \n\nMagnesium is removed from brine by contacting the brine with calcium hydroxide at temperatures above about 80.degree. C. but below the boiling point of the brine. The contacting results in the formation of magnesium hydroxide precipitate which is substantially insoluble in the mother liquor at those temperatures and strontium hydroxide which is dissolved in the mother liquor. When the contacting is carried out at a temperature above about 90.degree. C., magnesium hydroxide precipitate is fast settling and filterable; accordingly, it is removed from the mother liquor by a conventional process, such as filtering. The mother liquor is then cooled to cause the precipitation of at least a substantial part of strontium hydroxide present in the mother liquor. The precipitate of strontium hydroxide is recovered by a conventional process such as filtering. If precipitation upon cooling is insufficient, carbon dioxide gas is introduced into the mother liquor to effect the precipitation of strontium hydroxide. Barium can be removed and recovered in the form of barium sulfate by reacting the remaining mother liquor with sodium sulfate. In order to produce a faster-settling precipitate of magnesium hydroxide, the brine is contacted with a sufficient amount of a solution or slurry of calcium hydroxide in water to bring the concentration of magnesium in the resulting liquid to the range from about 0.023 mols of magnesium per liter to about 0.04 mols of magnesium per liter.
656581
Yes.  Mg  is more reactive than the Al, so the Mg will reduce the Al, and form an oxide or hydroxide.  Much depends on the conditions.  This would be helped along by a little water, acid would help even more, and a catalyst may also help.
445950
As the metal flexes, the molecules which make up the compound are temporarily displaced and generate kinetic energy which is dissipated as heat.   The process can be demonstrated in reverse i.e. when metal is heated, the molecules are displaced and the metal becomes pliable
5530
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:
869943
You could dissolve the crystal compound in water and measure the temperature change and specify whether there is an endothermic or exothermic change.  \n\nYou will need a thermometer.  Be careful as some crystal compounds are violently exothermic when dissolved in water.\n\nAndy
326922
Another easy reaction:\n\nMg(s) + HNO3 ===========> Mg(NO3)2 + H2 (g)\n\nMagnesium reacts rapidly with nitric acid to make magnesium nitrate and hydrogen gas
813421
Na2CO3(aq) + MgCl2(aq) --> 2NaCl(aq) + MgCO3(aq)
298301
Hmm. This is exactly what I've been doing for the past few weeks. I'm assuming these are aqueous solutions of the three, right?\n\nWell, both magnesium and strontium form precipitates with hydroxides, so you could add some sodium hydroxide and centrifuge it down. To the liquid remaining, add some kind of sulfate, like potassium sulfate, because barium precipitates with sulfates, forming BaSO4.\n\nTo the solid containing strontium and magnesium, add ammonia to make the solution basic, then add sodium carbonate. The magnesium should complex with the carbonate and fall out, forming Mg4(CO3)3(OH)2. Then, whatever's left is strontium.
279959
iodine turns starch black or a dark brown so you know if iodine is present in teh starch