Magnesium+chloride

Magnesium Chloride is a chemical compound with the formula MgCl2. Magnesium Cholirde has many uses. We see the use of magnesium chloride in such things as culinary use in places such as japan where it is used in prepatation of tofu and soy milk. It is also used in horticulture as a subsititue for magnesium sulfate for plants with magnesium defifiency. It is also used every winter as a liquid de-icer and anti-icer. MgCl2 works as a de-icer because it breaks the bonds between ice to deter its formation, and it combines natural elemetns on the road to keep the ice metled for the maximum amount of time which gives the best traction for vehivles.

Magnesium chloride often serves a treatment for magnesium deficiency in the human body because it is more bioavailable than other magnesium compounds.

Structure, preparation, and general properties
MgCl2 crystallizes in the [|cadmium chloride] motif, which features octahedral Mg. A variety of hydrates are known with the formula MgCl2(H2O)x, and each loses water with increasing temperature: x = 12 (-16.4 °C), 8 (-3.4 °C), 6 (116.7 °C), 4 (181 °C), 2 (ca. 300 °C). [|[1]] In the hexahydrate, the Mg2+ remains [|octahedral], but is coordinated to six water [|ligands]. [|[2]] The thermal dehydration of the hydrates MgCl2(H2O)x (x = 6, 12) does not occur straightforwardly. [|[3]] As suggested by the existence of some hydrates, anhydrous MgCl2 is a [|Lewis acid], although a very weak one. In the [|Dow process], magnesium chloride is regenerated from magnesium hydroxide using [|hydrochloric acid] : [|Mg(OH)2] ( [|s] ) + 2 HCl → MgCl2(aq) + 2 [|H2O] ( [|l] ) It can also be prepared from [|magnesium carbonate] by a similar reaction. In most of its derivatives, MgCl2 forms octahedral complexes. Derivatives with tetrahedral Mg2+ are less common. Examples include salts of ( [|tetraethylammonium] )2MgCl4 and [|adducts] such as MgCl( [|TMEDA] ). [|[4]]

Applications
Magnesium chloride serves as precursor to other magnesium compounds, for example by precipitation: MgCl2( [|aq] ) + [|Ca(OH)2] (aq) → [|Mg(OH)2] ( [|s] ) + [|CaCl2] (aq) It can be [|electrolysed] to give [|magnesium] metal: [|[5]] MgCl2( [|l] ) → Mg( [|l] ) + Cl2( [|g] ) This process is practiced on a substantial scale. Magnesium chloride is used for a variety of other applications besides the production of [|magnesium] : the manufacture of [|textiles], [|paper] , [|fireproofing agents] , [|cements] and [|refrigeration] brine, [|[5]] and dust and erosion control. Mixed with hydrated magnesium oxide, magnesium chloride forms a hard material called [|Sorel cement]. Magnesium ion Mg2+ (usually added as the chloride) is an important component in the [|polymerase chain reaction], a procedure used to amplify DNA fragments. It is generally used in experimental biology whenever RNA and DNA and their enzymes are to function [|in vitro], since Mg2+ is a necessary associate ion for [|nucleotides] in biology, such as ATP. Magnesium chloride is also used in several medical and topical (skin related) applications. It has been used in pills as supplemental sources of magnesium, where it serves as a soluble compound which is not as laxative as [|magnesium sulfate], and more bioavailable than [|magnesium hydroxide] and [|magnesium oxide] , since it does not require stomach acid to produce soluble Mg2+ ion. It can also be used as an effective anaesthetic for cephalopods, some species of crustaceans, [|[6]] and several species of bivalve, including oysters. [|[]

Ion formation of magnesium chloride