Magnesium

<h2 id="characteristics">Characteristics</h2>
<h3>Physical properties</h3>
Elemental magnesium is a gray-white lightweight metal, two-thirds the density of aluminium. Magnesium has the lowest melting (923 K (650 °C)) and the lowest boiling point (1,363 K (1,090 °C)) of all the alkaline earth metals.<a class="footnote-ref" id="fnref:5" href="#fn:5">5</a>
Pure polycrystalline magnesium is brittle and easily fractures along <a href="/facts/Shear_band/u0TNv0fl">shear bands</a>. It becomes much more <a href="/facts/Ductility/SBJsahEk">malleable</a> when alloyed with small amounts of other metals, such as 1% aluminium.<a class="footnote-ref" id="fnref:6" href="#fn:6">6</a> The malleability of polycrystalline magnesium can also be significantly improved by reducing its grain size to about 1 <a href="/facts/Micrometre/7eDFxD2L">μm</a> or less.<a class="footnote-ref" id="fnref:7" href="#fn:7">7</a>
When finely powdered, magnesium reacts with water to produce hydrogen gas:

Mg(s) + 2 H2O(g) → Mg(OH)2(aq) + H2(g) + 1203.6 kJ/mol
However, this reaction is much less dramatic than the reactions of the alkali metals with water, because the magnesium hydroxide builds up on the surface of the magnesium metal and inhibits further reaction.<a class="footnote-ref" id="fnref:8" href="#fn:8">8</a>

<h3>Chemical properties</h3>
<h4>Oxidation</h4>
The principal property of magnesium metal is its reducing power. One hint is that it <a href="/facts/Tarnish/GCskvFrN">tarnishes</a> slightly when exposed to air, although, unlike the heavier <a href="/facts/Alkaline_earth_metals/Ts4U5zIe">alkaline earth metals</a>, an oxygen-free environment is unnecessary for storage because magnesium is protected by a thin layer of oxide that is fairly impermeable and difficult to remove.<a class="footnote-ref" id="fnref:9" href="#fn:9">9</a>
Direct reaction of magnesium with air or oxygen at ambient pressure forms only the "normal" oxide MgO. However, this oxide may be combined with hydrogen peroxide to form <a href="/facts/Magnesium_peroxide/QC6Vqqgc">magnesium peroxide</a>, MgO2, and at low temperature the peroxide may be further reacted with ozone to form magnesium superoxide Mg(O2)2.<a class="footnote-ref" id="fnref:10" href="#fn:10">10</a>
Magnesium reacts with nitrogen in the solid state if it is powdered and heated to just below the melting point, forming <a href="/facts/Magnesium_nitride/TJDtoc1p">Magnesium nitride</a> Mg3N2.<a class="footnote-ref" id="fnref:11" href="#fn:11">11</a>
Magnesium reacts with water at room temperature, though it reacts much more slowly than calcium, a similar group 2 metal.<a class="footnote-ref" id="fnref:12" href="#fn:12">12</a> When submerged in water, <a href="/facts/Hydrogen/BoYHjl0J">hydrogen</a> bubbles form slowly on the surface of the metal; this reaction happens much more rapidly with powdered magnesium.<a class="footnote-ref" id="fnref:13" href="#fn:13">13</a> The reaction also occurs faster with higher temperatures (see § Safety precautions). Magnesium's reversible reaction with water can be harnessed to store energy and run a <a href="/facts/Magnesium_injection_cycle/JDtQ8tjT">magnesium-based engine</a>. Magnesium also reacts exothermically with most acids such as <a href="/facts/Hydrochloric_acid/HqItJlUT">hydrochloric acid</a> (HCl), producing <a href="/facts/Magnesium_chloride/uk1f69LG">magnesium chloride</a> and hydrogen gas, similar to the HCl reaction with aluminium, zinc, and many other metals.<a class="footnote-ref" id="fnref:14" href="#fn:14">14</a> Although it is difficult to ignite in mass or bulk, magnesium metal will ignite.
Magnesium may also be used as an igniter for <a href="/facts/Thermite/vIbVld9Y">thermite</a>, a mixture of aluminium and iron oxide powder that ignites only at a very high temperature.

<h4>Organic chemistry</h4>
Further information: <a href="/facts/Grignard_reagent/0vkLtPo1">Grignard reagent</a>
Organomagnesium compounds are widespread in <a href="/facts/Organic_chemistry/djxhxaNg">organic chemistry</a>. They are commonly found as <a href="/facts/Grignard_reagents/0vkLtPo1">Grignard reagents</a>, formed by reaction of magnesium with <a href="/facts/Haloalkane/Enb7LQqt">haloalkanes</a>. Examples of <a href="/facts/Grignard_reagents/0vkLtPo1">Grignard reagents</a> are <a href="/facts/Phenylmagnesium_bromide/lx5S0Jl6">phenylmagnesium bromide</a> and <a href="/facts/Ethylmagnesium_bromide/X1GUmLcQ">ethylmagnesium bromide</a>. The <a href="/facts/Grignard_reagents/0vkLtPo1">Grignard reagents</a> function as a common <a href="/facts/Nucleophile/xYccoaJQ">nucleophile</a>, attacking the <a href="/facts/Electrophilic/1AHFg1zm">electrophilic</a> group such as the carbon atom that is present within the polar bond of a <a href="/facts/Carbonyl/KJ71bo3X">carbonyl</a> group.
A prominent organomagnesium reagent beyond Grignard reagents is <a href="/facts/Magnesium_anthracene/xtRGH3jl">magnesium anthracene</a>, which is used as a source of highly active magnesium. The related <a href="/facts/Butadiene/j9W2LxGv">butadiene</a>-magnesium adduct serves as a source for the butadiene dianion.
Complexes of dimagnesium(I) have been observed.<a class="footnote-ref" id="fnref:15" href="#fn:15">15</a>

<h4>Detection in solution</h4>
The presence of magnesium ions can be detected by the addition of <a href="/facts/Ammonium_chloride/SfXdntlv">ammonium chloride</a>, <a href="/facts/Ammonium_hydroxide/pRg1m03X">ammonium hydroxide</a> and <a href="/facts/Monosodium_phosphate/v1o4fvpj">monosodium phosphate</a> to an aqueous or dilute HCl solution of the salt. The formation of a white precipitate indicates the presence of magnesium ions.
<a href="/facts/Azo_violet/TIrS5JqA">Azo violet</a> dye can also be used, turning deep blue in the presence of an alkaline solution of magnesium salt. The color is due to the <a href="/facts/Adsorption/ARH9peYM">adsorption</a> of azo violet by <a href="/facts/Magnesium_hydroxide/0hKR5Ica">Mg(OH)2</a>.

<h2 id="forms">Forms</h2>
<h3>Alloys</h3>
Main article: <a href="/facts/Magnesium_alloy/mmKDGhDL">Magnesium alloy</a>

As of 2013, consumption of magnesium alloys was less than one million tonnes per year, compared with 50 million tonnes of <a href="/facts/Aluminium_alloy/1EzR3Y4t">aluminium alloys</a>. Their use has been historically limited by the tendency of Mg alloys to corrode,<a class="footnote-ref" id="fnref:16" href="#fn:16">16</a> <a href="/facts/Creep_(deformation)/6GtcMsBt">creep</a> at high temperatures, and combust.<a class="footnote-ref" id="fnref:17" href="#fn:17">17</a>

<h4>Corrosion</h4>
In magnesium alloys, the presence of <a href="/facts/Iron/DkICCKIC">iron</a>, <a href="/facts/Nickel/KwMCHYRP">nickel</a>, <a href="/facts/Copper/I8PEE8oX">copper</a>, or <a href="/facts/Cobalt/gqhScEw4">cobalt</a> strongly activates <a href="/facts/Corrosion/lIC7H4we">corrosion</a>. In more than trace amounts, these metals precipitate as <a href="/facts/Intermetallic_compound/nnzksayl">intermetallic compounds</a>, and the precipitate locales function as active <a href="/facts/Cathode/tqdlGayU">cathodic</a> sites that reduce water, causing the loss of magnesium.<a class="footnote-ref" id="fnref:18" href="#fn:18">18</a> Controlling the quantity of these metals improves corrosion resistance. Sufficient <a href="/facts/Manganese/j9ELd1TL">manganese</a> overcomes the corrosive effects of iron. This requires precise control over composition, increasing costs.<a class="footnote-ref" id="fnref:19" href="#fn:19">19</a> Adding a cathodic poison captures atomic hydrogen within the structure of a metal. This prevents the formation of free hydrogen gas, an essential factor of corrosive chemical processes. The addition of about one in three hundred parts <a href="/facts/Arsenic/k1c4f44D">arsenic</a> reduces the corrosion rate of magnesium in a salt solution by a factor of nearly ten.<a class="footnote-ref" id="fnref:20" href="#fn:20">20</a><a class="footnote-ref" id="fnref:21" href="#fn:21">21</a>

<h4>High-temperature creep and flammability</h4>
Magnesium's tendency to <a href="/facts/Creep_(deformation)/6GtcMsBt">creep</a> (gradually deform) at high temperatures is greatly reduced by alloying with <a href="/facts/Zinc/80b1qgk3">zinc</a> and <a href="/facts/Rare-earth_elements/PQSUQumk">rare-earth elements</a>.<a class="footnote-ref" id="fnref:22" href="#fn:22">22</a> Flammability is significantly reduced by a small amount of <a href="/facts/Calcium/hf252CC0">calcium</a> in the alloy.<a class="footnote-ref" id="fnref:23" href="#fn:23">23</a> By using rare-earth elements, it may be possible to manufacture magnesium alloys that are able to not catch fire at higher temperatures compared to magnesium's <a href="/facts/Liquidus/RtXE2d8B">liquidus</a> and in some cases potentially pushing it close to magnesium's boiling point.<a class="footnote-ref" id="fnref:24" href="#fn:24">24</a>

<h3>Compounds</h3>
Main article: <a href="/facts/Magnesium_compounds/XyIhd2FG">Magnesium compounds</a>
Magnesium forms a variety of compounds important to industry and biology, including <a href="/facts/Magnesium_carbonate/ymvhw5R8">magnesium carbonate</a>, <a href="/facts/Magnesium_chloride/uk1f69LG">magnesium chloride</a>, <a href="/facts/Magnesium_citrate/a96acJgM">magnesium citrate</a>, <a href="/facts/Magnesium_hydroxide/0hKR5Ica">magnesium hydroxide</a> (milk of magnesia), <a href="/facts/Magnesium_oxide/0GfLn47t">magnesium oxide</a>, <a href="/facts/Magnesium_sulfate/o3GwKEoQ">magnesium sulfate</a>, and magnesium sulfate heptahydrate (<a href="/facts/Epsom_salts/o3GwKEoQ">Epsom salts</a>).<a class="footnote-ref" id="fnref:25" href="#fn:25">25</a><a class="footnote-ref" id="fnref:26" href="#fn:26">26</a>
As recently as 2020, <a href="/facts/Magnesium_hydride/CxLCwhHE">magnesium hydride</a> was under investigation as a way to store hydrogen.<a class="footnote-ref" id="fnref:27" href="#fn:27">27</a><a class="footnote-ref" id="fnref:28" href="#fn:28">28</a>

<h3>Isotopes</h3>
Main article: <a href="/facts/Isotopes_of_magnesium/pv5hSrhW">Isotopes of magnesium</a>
Magnesium has three stable <a href="/facts/Isotope/KD9B1y6o">isotopes</a>: 24Mg, 25Mg and 26Mg. All are present in significant amounts in nature (see table of isotopes above). About 79% of Mg is 24Mg. The isotope 28Mg is radioactive and in the 1950s to 1970s was produced by several nuclear power plants for use in scientific experiments. This isotope has a relatively short half-life (21 hours) and its use was limited by shipping times.
The nuclide 26Mg has found application in <a href="/facts/Isotope/KD9B1y6o">isotopic</a> <a href="/facts/Geology/WGvVRIYF">geology</a>, similar to that of aluminium. 26Mg is a <a href="/facts/Radiogenic/KXP6MKk6">radiogenic</a> daughter product of <a href="/facts/Aluminium-26/INwQYapg">26Al</a>, which has a <a href="/facts/Half-life/kGVH8BAB">half-life</a> of 717,000 years. Excessive quantities of stable 26Mg have been observed in the <a href="/facts/Ca-Al-rich_inclusions/vTAYA3wV">Ca-Al-rich inclusions</a> of some <a href="/facts/Carbonaceous_chondrite/TnCY8ssz">carbonaceous chondrite</a> <a href="/facts/Meteorite/NsmHlBlX">meteorites</a>. This anomalous abundance is attributed to the decay of its parent 26Al in the inclusions, and researchers conclude that such meteorites were formed in the <a href="/facts/Solar_nebula/cgElXHpM">solar nebula</a> before the 26Al had decayed. These are among the oldest objects in the <a href="/facts/Solar_System/QIcLSazQ">Solar System</a> and contain preserved information about its early history.
It is conventional to plot 26Mg/24Mg against an Al/Mg ratio. In an <a href="/facts/Isochron_dating/SL0As6rJ">isochron dating</a> plot, the Al/Mg ratio plotted is 27Al/24Mg. The slope of the isochron has no age significance, but indicates the initial 26Al/27Al ratio in the sample at the time when the systems were separated from a common reservoir.

<h2 id="production">Production</h2>
See also: <a href="/facts/Magnesium_production_by_country/nrYtoU4f">Magnesium production by country</a>

<h3>Occurrence</h3>
See also: Category:Magnesium minerals
See also: <a href="/facts/Boninite/p61vogzy">Boninite</a>
Magnesium is the eighth-most-abundant element in the Earth's crust by mass and tied in seventh place with <a href="/facts/Iron/DkICCKIC">iron</a> in <a href="/facts/Molarity/P2WL5b9q">molarity</a>.<a class="footnote-ref" id="fnref:29" href="#fn:29">29</a> It is found in large deposits of <a href="/facts/Magnesite/X0tdEuYy">magnesite</a>, <a href="/facts/Dolomite_(mineral)/tQfyK6AF">dolomite</a>, and other <a href="/facts/Mineral/LkUFbNmv">minerals</a>, and in mineral waters, where magnesium ion is soluble.<a class="footnote-ref" id="fnref:30" href="#fn:30">30</a>
Although magnesium is found in more than 60 <a href="/facts/Mineral/LkUFbNmv">minerals</a>, only <a href="/facts/Dolomite_(mineral)/tQfyK6AF">dolomite</a>, <a href="/facts/Magnesite/X0tdEuYy">magnesite</a>, <a href="/facts/Brucite/g7PAmGnq">brucite</a>, <a href="/facts/Carnallite/N7RQQwRd">carnallite</a>, <a href="/facts/Talc/9sUSo6rA">talc</a>, and <a href="/facts/Olivine/tLLL4rae">olivine</a> are of commercial importance.<a class="footnote-ref" id="fnref:31" href="#fn:31">31</a>
The Mg2+ <a href="/facts/Cation/wrbwhF3z">cation</a> is the second-most-abundant cation in seawater (about 1⁄8 the mass of sodium ions in a given sample), which makes seawater and sea salt attractive commercial sources for Mg.

<h3>Production quantities</h3>
World production was approximately 1,100 kt in 2017, with the bulk being produced in China (930 kt) and Russia (60 kt).<a class="footnote-ref" id="fnref:32" href="#fn:32">32</a> The United States was in the 20th century the major world supplier of this metal, supplying 45% of world production even as recently as 1995. Since the Chinese mastery of the Pidgeon process the US market share is at 7%, with a single US producer left as of 2013: US Magnesium, a <a href="/facts/Renco_Group/WC8u8H2y">Renco Group</a> company located on the shores of the <a href="/facts/Great_Salt_Lake/TexYwwas">Great Salt Lake</a>.<a class="footnote-ref" id="fnref:33" href="#fn:33">33</a>
In September 2021, China took steps to reduce production of magnesium as a result of a government initiative to reduce energy availability for manufacturing industries, leading to a significant price increase.<a class="footnote-ref" id="fnref:34" href="#fn:34">34</a>

<h3>Pidgeon and Bolzano processes</h3>

The <a href="/facts/Pidgeon_process/XplhU5TG">Pidgeon process</a> and the <a href="/facts/Bolzano_process/WUT3Vm13">Bolzano process</a> are similar. In both, magnesium oxide is the precursor to magnesium metal. The magnesium oxide is produced as a solid solution with calcium oxide by calcining the mineral <a href="/facts/Dolomite_(mineral)/tQfyK6AF">dolomite</a>, which is a solid solution of calcium and magnesium carbonates:

CaCO3·MgCO3 → MgO·CaO + 2 CO2
Reduction occurs at high temperatures with silicon. A ferrosilicon alloy is used rather than pure silicon as it is more economical. The iron component has no bearing on the reaction, having the simplified equation:

MgO·CaO +Si → 2 Mg + Ca2SiO4
The calcium oxide combines with silicon as the oxygen scavenger, yielding the very stable calcium silicate. The Mg/Ca ratio of the precursors can be adjusted by the addition of MgO or CaO.<a class="footnote-ref" id="fnref:35" href="#fn:35">35</a>
The Pidgeon and the Bolzano process differ in the details of the heating and the configuration of the reactor. Both generate gaseous Mg that is condensed and collected. The Pidgeon process dominates the worldwide production.<a class="footnote-ref" id="fnref:36" href="#fn:36">36</a><a class="footnote-ref" id="fnref:37" href="#fn:37">37</a> The Pidgeon method is less technologically complex and because of distillation/vapour deposition conditions, a high purity product is easily achievable.<a class="footnote-ref" id="fnref:38" href="#fn:38">38</a> China is almost completely reliant on the <a href="/facts/Silicothermic_reaction/WmxIMU20">silicothermic</a> <a href="/facts/Pidgeon_process/XplhU5TG">Pidgeon process</a>.

<h3>Dow process</h3>

"Dow process (magnesium)" redirects here. For other Dow processes, see <a href="/facts/Dow_process_(disambiguation)/njlB5ukU">Dow process (disambiguation)</a>.
Besides the Pidgeon process, the second most used process for magnesium production is <a href="/facts/Electrolysis/pU75nCDI">electrolysis</a>. This is a two step process. The first step is to prepare feedstock containing magnesium chloride and the second step is to dissociate the compound in <a href="/facts/Electrolytic_cell/Cn3U4dSp">electrolytic cells</a> as magnesium metal and <a href="/facts/Chlorine/y27UwYBM">chlorine gas</a>.<a class="footnote-ref" id="fnref:39" href="#fn:39">39</a>
To extract the magnesium, <a href="/facts/Calcium_hydroxide/Kz2KzRd8">calcium hydroxide</a> is added to the <a href="/facts/Seawater/fRBJjbws">seawater</a> to <a href="/facts/Precipitate/s3BgsLLY">precipitate</a> <a href="/facts/Magnesium_hydroxide/0hKR5Ica">magnesium hydroxide</a>.<a class="footnote-ref" id="fnref:40" href="#fn:40">40</a>

MgCl2 + Ca(OH)2 → Mg(OH)2 + CaCl2
Magnesium hydroxide (<a href="/facts/Brucite/g7PAmGnq">brucite</a>) is poorly soluble in water and can be collected by filtration. It reacts with <a href="/facts/Hydrochloric_acid/HqItJlUT">hydrochloric acid</a> to <a href="/facts/Magnesium_chloride/uk1f69LG">magnesium chloride</a>.<a class="footnote-ref" id="fnref:41" href="#fn:41">41</a>

Mg(OH)2 + 2 HCl → MgCl2 + 2 H2O
From magnesium chloride, <a href="/facts/Electrolysis/pU75nCDI">electrolysis</a> produces magnesium.<a class="footnote-ref" id="fnref:42" href="#fn:42">42</a>
The basic reaction is as follows:

MgCl2 → Mg(g) + Cl2(g)
The temperatures at which this reaction is operated is between 680 and 750 °C.<a class="footnote-ref" id="fnref:43" href="#fn:43">43</a>
The magnesium chloride can be obtained using the <a href="/facts/Dow_process_(magnesium)/XyIhd2FG">Dow process</a>, a process that mixes sea water and dolomite in a flocculator or by dehydration of magnesium chloride brines. The electrolytic cells are partially submerged in a molten salt electrolyte to which the produced magnesium chloride is added in concentrations between 6–18%.<a class="footnote-ref" id="fnref:44" href="#fn:44">44</a> This process does have its share of disadvantages including production of harmful <a href="/facts/Chlorine_gas/y27UwYBM">chlorine gas</a> and the overall reaction being very energy intensive, creating environmental risks.<a class="footnote-ref" id="fnref:45" href="#fn:45">45</a> The Pidgeon process is more advantageous regarding its simplicity, shorter construction period, low power consumption and overall good magnesium quality compared to the electrolysis method.<a class="footnote-ref" id="fnref:46" href="#fn:46">46</a>
In the United States, magnesium was once obtained principally with the Dow process in <a href="/facts/Corpus_Christi_TX/t67U3xU4">Corpus Christi TX</a>, by <a href="/facts/Electrolysis/pU75nCDI">electrolysis</a> of fused magnesium chloride from <a href="/facts/Brine/xsN2GcLF">brine</a> and <a href="/facts/Sea_water/fRBJjbws">sea water</a>. A saline solution containing Mg2+ ions is first treated with <a href="/facts/Calcium_oxide/Wh9C8l7j">lime</a> (calcium oxide) and the precipitated <a href="/facts/Magnesium_hydroxide/0hKR5Ica">magnesium hydroxide</a> is collected:

Mg2+(aq) + CaO(s) + H2O(l) → Ca2+(aq) + Mg(OH)2(s)
The hydroxide is then converted to <a href="/facts/Magnesium_chloride/uk1f69LG">magnesium chloride</a> by treatment with <a href="/facts/Hydrochloric_acid/HqItJlUT">hydrochloric acid</a> and heating of the product to eliminate water:

Mg(OH)2 + 2 HCl → MgCl2 + 2 H2O
The salt is then electrolyzed in the molten state. At the <a href="/facts/Cathode/tqdlGayU">cathode</a>, the Mg2+ ion is reduced by two <a href="/facts/Electron/L0KBo5cW">electrons</a> to magnesium metal:

Mg2+ + 2e− → Mg
At the <a href="/facts/Anode/TjYt95zG">anode</a>, each pair of Cl− ions is oxidized to <a href="/facts/Chlorine/y27UwYBM">chlorine</a> gas, releasing two electrons to complete the circuit:

2Cl− → Cl2(g) + 2e−
<h3>Carbothermic process</h3>
The <a href="/facts/Carbothermic_reaction/gj0GA25m">carbothermic</a> route to magnesium has been recognized as a low energy, yet high productivity path to magnesium extraction. The chemistry is as follows:

C + MgO → CO + Mg
A disadvantage of this method is that slow cooling the vapour can cause the reaction to quickly revert. To prevent this from happening, the magnesium can be dissolved directly in a suitable metal solvent before reversion starts happening. Rapid <a href="/facts/Quenching/UUCW0GQD">quenching</a> of the vapour can also be performed to prevent reversion.<a class="footnote-ref" id="fnref:47" href="#fn:47">47</a>

<h3>YSZ process</h3>

A newer process, solid oxide membrane technology, involves the electrolytic reduction of MgO. At the cathode, Mg2+ ion is reduced by two <a href="/facts/Electron/L0KBo5cW">electrons</a> to magnesium metal. The electrolyte is <a href="/facts/Yttria-stabilized_zirconia/gQduqJhV">yttria-stabilized zirconia</a> (YSZ). The anode is a liquid metal. At the YSZ/liquid metal anode O2− is oxidized. A layer of graphite borders the liquid metal anode, and at this interface carbon and oxygen react to form carbon monoxide. When silver is used as the liquid metal anode, there is no reductant carbon or hydrogen needed, and only oxygen gas is evolved at the anode.<a class="footnote-ref" id="fnref:48" href="#fn:48">48</a> It was reported in 2011 that this method provides a 40% reduction in cost per pound over the electrolytic reduction method.<a class="footnote-ref" id="fnref:49" href="#fn:49">49</a>

<h3>Rieke process</h3>
Rieke et al. developed a "general approach for preparing highly reactive metal powders by reducing metal salts in ethereal or hydrocarbon solvents using alkali metals as reducing agents" now known as the <a href="/facts/Rieke_process/02JWpSDx">Rieke process</a>.<a class="footnote-ref" id="fnref:50" href="#fn:50">50</a> Rieke finalized the identification of <a href="/facts/Rieke_metals/02JWpSDx">Rieke metals</a> in 1989,<a class="footnote-ref" id="fnref:51" href="#fn:51">51</a> one of which was Rieke-magnesium, first produced in 1974.<a class="footnote-ref" id="fnref:52" href="#fn:52">52</a>

<h2 id="history">History</h2>
The name magnesium originates from the <a href="/facts/Ancient_Greek/LIK7NlUh">Greek</a> word for locations related to the tribe of the <a href="/facts/Magnetes/zNvEfAyR">Magnetes</a>, either a district in <a href="/facts/Thessaly/G76Tml8X">Thessaly</a> called <a href="/facts/Ancient_Magnesia/GEWsPTJu">Magnesia</a><a class="footnote-ref" id="fnref:53" href="#fn:53">53</a> or <a href="/facts/Magnesia_ad_Sipylum/7Lb75fKz">Magnesia ad Sipylum</a>, now in Turkey.<a class="footnote-ref" id="fnref:54" href="#fn:54">54</a> It is related to <a href="/facts/Magnetite/SVxoGUs2">magnetite</a> and <a href="/facts/Manganese/j9ELd1TL">manganese</a>, which also originated from this area, and required differentiation as separate substances. See <a href="/facts/Manganese/j9ELd1TL">manganese</a> for this history.
In 1618, a farmer at Epsom in England attempted to give his cows water from a local well. The cows refused to drink because of the water's bitter taste, but the farmer noticed that the water seemed to heal scratches and rashes. The substance obtained by evaporating the water became known as <a href="/facts/Magnesium_sulfate/o3GwKEoQ">Epsom salts</a> and its fame spread.<a class="footnote-ref" id="fnref:55" href="#fn:55">55</a> It was eventually recognized as hydrated magnesium sulfate, MgSO4·7 H2O.<a class="footnote-ref" id="fnref:56" href="#fn:56">56</a>
The metal itself was first isolated by <a href="/facts/Humphry_Davy/aDNRfNou">Sir Humphry Davy</a> in England in 1808. He used electrolysis on a mixture of <a href="/facts/Magnesia_alba/0GfLn47t">magnesia</a> and <a href="/facts/Mercury(II)_oxide/uE9xSlQe">mercuric oxide</a>.<a class="footnote-ref" id="fnref:57" href="#fn:57">57</a> <a href="/facts/Antoine_Bussy/bhXcWMhg">Antoine Bussy</a> prepared it in coherent form in 1831. Davy's first suggestion for a name was 'magnium',<a class="footnote-ref" id="fnref:58" href="#fn:58">58</a> but the name magnesium is now used in most European languages.<a class="footnote-ref" id="fnref:59" href="#fn:59">59</a>
Further discoveries about magnesium were made by the father of <a href="/facts/Physical_chemistry/WqwnJjRM">physical chemistry</a> in <a href="/facts/Imperial_Russia/hg1g5SpV">Imperial Russia</a>, <a href="/facts/Nikolai_Beketov/eV6dz8Rq">Nikolai Beketov</a> (1827–1911), who established that magnesium and zinc displaced other metals from their salts under high temperatures.

<h2 id="uses">Uses</h2>
<h3>Magnesium metal</h3>

Magnesium is the third-most-commonly-used structural metal, following <a href="/facts/Iron/DkICCKIC">iron</a> and aluminium.<a class="footnote-ref" id="fnref:60" href="#fn:60">60</a> The main applications of magnesium are, in order: aluminium alloys, <a href="/facts/Die-casting/9bdIWfoe">die-casting</a> (alloyed with <a href="/facts/Zinc/80b1qgk3">zinc</a>),<a class="footnote-ref" id="fnref:61" href="#fn:61">61</a> removing <a href="/facts/Sulfur/IK0amTfM">sulfur</a> in the production of iron and steel, and the production of <a href="/facts/Titanium/53ArnDoy">titanium</a> in the <a href="/facts/Kroll_process/xzTkfDCQ">Kroll process</a>.<a class="footnote-ref" id="fnref:62" href="#fn:62">62</a>
Magnesium is used in lightweight materials and alloys. For example, when infused with silicon carbide <a href="/facts/Nanoparticle/k8kNxX4E">nanoparticles</a>, it has extremely high specific strength.<a class="footnote-ref" id="fnref:63" href="#fn:63">63</a>
Historically, magnesium was one of the main aerospace construction metals and was used for German military aircraft as early as World War I and extensively for German aircraft in World War II. The Germans coined the name "<a href="/facts/Elektron_(alloy)/8AW3LITw">Elektron</a>" for magnesium alloy, a term which is still used today. In the commercial aerospace industry, magnesium was generally restricted to engine-related components, due to fire and corrosion hazards. Magnesium alloy use in aerospace is increasing in the 21st century, driven by the importance of fuel economy.<a class="footnote-ref" id="fnref:64" href="#fn:64">64</a> Magnesium alloys can act as replacements for aluminium and steel alloys in structural applications.<a class="footnote-ref" id="fnref:65" href="#fn:65">65</a><a class="footnote-ref" id="fnref:66" href="#fn:66">66</a>

<h4>Aircraft</h4>
<ul><li><a href="/facts/Wright_Aeronautical/f3mynmUm">Wright Aeronautical</a> used a magnesium <a href="/facts/Crankcase/5Gb3fTHQ">crankcase</a> in the WWII-era <a href="/facts/Wright_R-3350_Duplex_Cyclone/1AnowCoR">Wright R-3350 Duplex Cyclone</a> aviation engine. This presented a serious problem for the earliest models of the <a href="/facts/Boeing_B-29_Superfortress/79pXKprr">Boeing B-29 Superfortress</a> heavy bomber when an in-flight engine fire ignited the engine crankcase. The resulting combustion was as hot as 5,600 °F (3,100 °C) and could sever the wing spar from the <a href="/facts/Fuselage/vVXlHEE4">fuselage</a>.<a class="footnote-ref" id="fnref:67" href="#fn:67">67</a><a class="footnote-ref" id="fnref:68" href="#fn:68">68</a><a class="footnote-ref" id="fnref:69" href="#fn:69">69</a></li></ul>
<h4>Automotive</h4>

<ul><li><a href="/facts/Mercedes-Benz/pGrJrQHC">Mercedes-Benz</a> used the alloy <a href="/facts/Elektron_(alloy)/8AW3LITw">Elektron</a> in the bodywork of an early model <a href="/facts/Mercedes-Benz_300_SLR/KU8mN0QE">Mercedes-Benz 300 SLR</a>; these cars competed in the <a href="/facts/1955_World_Sportscar_Championship/FUfg1Jog">1955 World Sportscar Championship</a> including a win at the <a href="/facts/1955_Mille_Miglia/1BrU0nEA">Mille Miglia</a>, and at <a href="/facts/24_Hours_of_Le_Mans/lotVMp31">Le Mans</a> where one was involved in the <a href="/facts/1955_Le_Mans_disaster/8KIMJFgC">1955 Le Mans disaster</a> when spectators were showered with burning fragments of elektron.<a class="footnote-ref" id="fnref:70" href="#fn:70">70</a></li>
<li><a href="/facts/Porsche/9S83Lb11">Porsche</a> used magnesium alloy frames in the <a href="/facts/Porsche_917/QIYujtzJ">917/053</a> that won Le Mans in 1971, and continues to use magnesium alloys for its engine blocks due to the weight advantage.<a class="footnote-ref" id="fnref:71" href="#fn:71">71</a></li>
<li><a href="/facts/Volkswagen_Group/xg9cPekV">Volkswagen Group</a> has used magnesium in its engine components for many years.<a class="footnote-ref" id="fnref:72" href="#fn:72">72</a></li>
<li><a href="/facts/Mitsubishi_Motors/XXWlxHRw">Mitsubishi Motors</a> uses magnesium for its <a href="/facts/Paddle_shifters/QP5nmyNz">paddle shifters</a>.<a class="footnote-ref" id="fnref:73" href="#fn:73">73</a></li>
<li><a href="/facts/BMW/cJd8y02r">BMW</a> used magnesium alloy blocks in their <a href="/facts/BMW_N52/QQL2rgDz">N52</a> engine, including an aluminium alloy insert for the cylinder walls and cooling jackets surrounded by a high-temperature magnesium alloy <a href="/facts/AJ_alloys/vgpofXTp">AJ62A</a>. The engine was used worldwide between 2005 and 2011 in various 1, 3, 5, 6, and 7 series models; as well as the Z4, X1, X3, and X5.<a class="footnote-ref" id="fnref:74" href="#fn:74">74</a></li>
<li><a href="/facts/Chevrolet/lp04IP4m">Chevrolet</a> used the magnesium alloy AE44 in the 2006 Corvette <a href="/facts/Corvette_C6/Jv1Yjztg">Z06</a>.<a class="footnote-ref" id="fnref:75" href="#fn:75">75</a></li></ul>
Both AJ62A and AE44 are recent developments in high-temperature low-<a href="/facts/Creep_(deformation)/6GtcMsBt">creep</a> magnesium alloys. The general strategy for such alloys is to form <a href="/facts/Intermetallic/nnzksayl">intermetallic</a> precipitates at the <a href="/facts/Crystallite/nXSgR0wp">grain boundaries</a>, for example by adding <a href="/facts/Mischmetal/kCm2tjJ8">mischmetal</a> or <a href="/facts/Calcium/hf252CC0">calcium</a>.<a class="footnote-ref" id="fnref:76" href="#fn:76">76</a>

<h4>Electronics</h4>
Because of low density and good mechanical and electrical properties, magnesium is used for manufacturing of mobile phones, laptop and <a href="/facts/Tablet_computers/6pGX2I7b">tablet computers</a>, cameras, and other electronic components.<a class="footnote-ref" id="fnref:77" href="#fn:77">77</a> It was used as a premium feature because of its light weight in some 2020 laptops.<a class="footnote-ref" id="fnref:78" href="#fn:78">78</a>

<h4>Source of light</h4>
Magnesium is flammable, burning at a temperature of approximately 3,100 °C (3,370 K; 5,610 °F),<a class="footnote-ref" id="fnref:79" href="#fn:79">79</a> and the <a href="/facts/Autoignition_temperature/bRATNu6d">autoignition temperature</a> of magnesium ribbon is approximately 473 °C (746 K; 883 °F).<a class="footnote-ref" id="fnref:80" href="#fn:80">80</a> Magnesium's high combustion temperature makes it a useful tool for starting emergency fires. When burning in air, magnesium produces a brilliant white light that includes strong ultraviolet wavelengths.
Magnesium powder (<a href="/facts/Flash_powder/TW3lHt9s">flash powder</a>) was used for subject illumination in the early days of <a href="/facts/Photography/ezLPT43M">photography</a>.<a class="footnote-ref" id="fnref:81" href="#fn:81">81</a><a class="footnote-ref" id="fnref:82" href="#fn:82">82</a> Magnesium filament used in electrically ignited single-use photography <a href="/facts/Flash_(photography)/bfegk3Xy">flashbulbs</a> replaced this usage eventually. Magnesium powder is used in <a href="/facts/Fireworks/sPEQcu3h">fireworks</a> and marine <a href="/facts/Flare/LuXg6UXI">flares</a> where a brilliant light is required, and in trick self-relighting birthday candles. It was also used for various theatrical effects,<a class="footnote-ref" id="fnref:83" href="#fn:83">83</a> such as lightning,<a class="footnote-ref" id="fnref:84" href="#fn:84">84</a> pistol flashes,<a class="footnote-ref" id="fnref:85" href="#fn:85">85</a> and supernatural appearances.<a class="footnote-ref" id="fnref:86" href="#fn:86">86</a>

Magnesium is often used to ignite thermite or other materials that require a high ignition temperature. Magnesium continues to be used as an <a href="/facts/Incendiary_device/Evu6eJWY">incendiary</a> element in warfare.<a class="footnote-ref" id="fnref:87" href="#fn:87">87</a>
Flame temperatures of magnesium and magnesium alloys can reach 3,100 °C (5,610 °F),<a class="footnote-ref" id="fnref:88" href="#fn:88">88</a> although flame height above the burning metal is usually less than 300 mm (12 in).<a class="footnote-ref" id="fnref:89" href="#fn:89">89</a> Once ignited, such fires are difficult to extinguish because they resist several substances commonly used to put out fires; combustion continues in <a href="/facts/Nitrogen/Nf1QpGDz">nitrogen</a> (forming <a href="/facts/Magnesium_nitride/TJDtoc1p">magnesium nitride</a>),<a class="footnote-ref" id="fnref:90" href="#fn:90">90</a> in <a href="/facts/Carbon_dioxide/xGzpppEp">carbon dioxide</a> (forming <a href="/facts/Magnesium_oxide/0GfLn47t">magnesium oxide</a> and <a href="/facts/Carbon/ukrgQexo">carbon</a>),<a class="footnote-ref" id="fnref:91" href="#fn:91">91</a> and in water (forming magnesium oxide and hydrogen, which also combusts due to heat in the presence of additional oxygen). This property[which?] was used in incendiary weapons during the <a href="/facts/Firebombing/NeN74JUX">firebombing</a> of cities in <a href="/facts/World_War_II/2efV5L1U">World War II</a>, where the only practical <a href="/facts/Civil_defense/xa73Rr3S">civil defense</a> was to smother a burning flare under dry sand[why?] to exclude atmosphere from the combustion.

<h4>Chemical reagent</h4>
In the form of turnings or ribbons, to prepare <a href="/facts/Grignard_reagent/0vkLtPo1">Grignard reagents</a>, which are useful in <a href="/facts/Organic_synthesis/WLFePEzH">organic synthesis</a>.<a class="footnote-ref" id="fnref:92" href="#fn:92">92</a>

<h4>Other</h4>
<ul><li>In the production of <a href="/facts/Ductile_iron/nLmcVYWP">nodular graphite in cast iron</a>.<a class="footnote-ref" id="fnref:93" href="#fn:93">93</a></li>
<li>As an additive agent in conventional propellants.<a class="footnote-ref" id="fnref:94" href="#fn:94">94</a></li>
<li>As a reducing agent to separate <a href="/facts/Uranium/n2sGWBzU">uranium</a> and other metals from their <a href="/facts/Salt_(chemistry)/lsSKwGpn">salts</a>.<a class="footnote-ref" id="fnref:95" href="#fn:95">95</a></li>
<li>As a <a href="/facts/Sacrificial_anode/lGBuszfA">sacrificial (galvanic) anode</a> to protect boats, underground tanks, pipelines, buried structures, and water heaters.<a class="footnote-ref" id="fnref:96" href="#fn:96">96</a></li>
<li>Alloyed with zinc to produce the zinc sheet used in <a href="/facts/Photoengraving/snXCBjWM">photoengraving</a> plates in the printing industry, <a href="/facts/Dry_cell/bqEpm4ue">dry-cell battery</a> walls, and <a href="/facts/Flashing_(weatherproofing)/2qNUauWP">roofing</a>.<a class="footnote-ref" id="fnref:97" href="#fn:97">97</a></li>
<li>Alloyed with aluminium with aluminium-magnesium alloys being used mainly for <a href="/facts/Beverage_can/c6FofnmS">beverage cans</a>,<a class="footnote-ref" id="fnref:98" href="#fn:98">98</a> sports equipment such as golf clubs,<a class="footnote-ref" id="fnref:99" href="#fn:99">99</a> fishing reels,<a class="footnote-ref" id="fnref:100" href="#fn:100">100</a> and <a href="/facts/Archery/VjHPRszQ">bows and arrows</a>.<a class="footnote-ref" id="fnref:101" href="#fn:101">101</a></li>
<li>Many car and aircraft manufacturers have made engine and body parts from magnesium.<a class="footnote-ref" id="fnref:102" href="#fn:102">102</a></li>
<li><a href="/facts/Magnesium_battery/xrk6ljoU">Magnesium batteries</a> have been commercialized as <a href="/facts/Primary_battery/udJP2wJ1">primary batteries</a>, and are an active topic of research for <a href="/facts/Rechargeable_battery/A6zUkPkW">rechargeable batteries</a>, such as <a href="/facts/Magnesium_sulfur_battery/TFY2BPzQ">magnesium sulfur batteries</a>.<a class="footnote-ref" id="fnref:103" href="#fn:103">103</a><a class="footnote-ref" id="fnref:104" href="#fn:104">104</a></li></ul>
<h3>Compounds</h3>
Magnesium compounds, primarily <a href="/facts/Magnesium_oxide/0GfLn47t">magnesium oxide</a> (MgO), are used as a <a href="/facts/Refractory/LoKrzGkR">refractory</a> material in <a href="/facts/Metallurgical_furnace/11qWf4A3">furnace</a> linings for producing <a href="/facts/Iron/DkICCKIC">iron</a>, <a href="/facts/Steel/aN6qWo4H">steel</a>, <a href="/facts/Nonferrous_metal/lY7X8rAY">nonferrous metals</a>, <a href="/facts/Glass/hezRsAGf">glass</a>, and <a href="/facts/Cement/VfDMkk12">cement</a>. Magnesium oxide and other magnesium compounds are also used in the agricultural, chemical, and construction industries. Magnesium oxide from <a href="/facts/Calcination/hghqlHwo">calcination</a> is used as an electrical insulator in <a href="/facts/Mineral-insulated_copper-clad_cable/1EVHQosM">fire-resistant cables</a>.<a class="footnote-ref" id="fnref:105" href="#fn:105">105</a>
Magnesium reacts with <a href="/facts/Haloalkane/Enb7LQqt">haloalkanes</a> to give <a href="/facts/Grignard_reagent/0vkLtPo1">Grignard reagents</a>, which are used for a wide variety of <a href="/facts/Organic_reaction/SESmeGWm">organic reactions</a> forming <a href="/facts/Carbon%25E2%2580%2593carbon_bond/nLE4z5BK">carbon–carbon bonds</a>.<a class="footnote-ref" id="fnref:106" href="#fn:106">106</a>
Magnesium salts are included in various <a href="/facts/Food/RgNq6NAK">foods</a>,<a class="footnote-ref" id="fnref:107" href="#fn:107">107</a> <a href="/facts/Fertilizer/ysh3r6NJ">fertilizers</a><a class="footnote-ref" id="fnref:108" href="#fn:108">108</a> (magnesium is a component of <a href="/facts/Chlorophyll/1Sb0NyyM">chlorophyll</a><a class="footnote-ref" id="fnref:109" href="#fn:109">109</a>), and <a href="/facts/Culture_medium/97IMkpFP">microbe culture media</a>.<a class="footnote-ref" id="fnref:110" href="#fn:110">110</a>
<a href="/facts/Magnesium_sulfite/DpcU1rRT">Magnesium sulfite</a> is used in the manufacture of <a href="/facts/Paper/FUETwwKV">paper</a> (<a href="/facts/Sulfite_process/edJVxor2">sulfite process</a>).<a class="footnote-ref" id="fnref:111" href="#fn:111">111</a>
<a href="/facts/Magnesium_phosphate/fxXVb1xB">Magnesium phosphate</a> is used to fireproof wood used in construction.<a class="footnote-ref" id="fnref:112" href="#fn:112">112</a>
Magnesium hexafluorosilicate is used for moth-proofing <a href="/facts/Textile/PJrVeM5S">textiles</a>.<a class="footnote-ref" id="fnref:113" href="#fn:113">113</a>

<h2 id="biological-roles">Biological roles</h2>
Main articles: <a href="/facts/Magnesium_in_biology/ENuowoyY">Magnesium in biology</a> and <a href="/facts/Magnesium_(medical_use)/NIspfBdt">Magnesium (medical use)</a>
<h3>Mechanism of action</h3>
The important interaction between <a href="/facts/Phosphate/FDGVCxUG">phosphate</a> and magnesium ions makes magnesium essential to the basic <a href="/facts/Nucleic_acid/2tTgcI0v">nucleic acid</a> chemistry of all cells of all known living organisms. More than 300 <a href="/facts/Enzyme/DSI1Fh7y">enzymes</a> require magnesium ions for their catalytic action, including all enzymes using or synthesizing <a href="/facts/Adenosine_triphosphate/nB9bwgcU">ATP</a> and those that use other <a href="/facts/Nucleotides/pQKEwlJI">nucleotides</a> to synthesize <a href="/facts/DNA/nB89Iauz">DNA</a> and <a href="/facts/RNA/HxPeNfNj">RNA</a>. The ATP molecule is normally found in a <a href="/facts/Chelation/4G79sXBB">chelate</a> with a magnesium ion.<a class="footnote-ref" id="fnref:114" href="#fn:114">114</a>

<h3>Nutrition</h3>
Magnesium intake—especially from diet—may modestly lower <a href="/facts/Blood_pressure/VtqqSM2J">blood pressure</a> and reduce risks of <a href="/facts/Stroke/DwpjdzY0">stroke</a> and <a href="/facts/Cardiac_arrest/HIAm9AWX">sudden cardiac death</a>, but evidence is mixed, effects are small, and more robust <a href="/facts/Clinical_trial/q8LMr832">clinical trials</a> are needed to clarify its role in <a href="/facts/Cardiovascular_disease/HD420nMv">cardiovascular disease</a> prevention.<a class="footnote-ref" id="fnref:115" href="#fn:115">115</a>

<h4>Diet</h4>
 
Spices, nuts, cereals, cocoa and vegetables are good sources of magnesium.<a class="footnote-ref" id="fnref:116" href="#fn:116">116</a> Green leafy vegetables such as spinach are also rich in magnesium.<a class="footnote-ref" id="fnref:117" href="#fn:117">117</a>

<h4>Dietary recommendations</h4>
In the <a href="/facts/United_Kingdom/kuPAILt2">UK</a>, the recommended daily values by the <a href="/facts/Dietary_Reference_Intake/FWaI93Dm">Dietary Reference Intake</a> for magnesium are 300 mg for men and 270 mg for women.<a class="footnote-ref" id="fnref:118" href="#fn:118">118</a>
In the U.S. the <a href="/facts/Recommended_Dietary_Allowances/TemwCsC3">Recommended Dietary Allowances</a> (RDAs) are 400 mg for men ages 19–30 and 420 mg for older; for women 310 mg for ages 19–30 and 320 mg for older.<a class="footnote-ref" id="fnref:119" href="#fn:119">119</a>

<h4>Supplementation</h4>
Numerous <a href="/facts/Magnesium_(pharmaceutical_preparation)/NIspfBdt">pharmaceutical preparations of magnesium</a> and <a href="/facts/Dietary_supplement/SHXNNxaS">dietary supplements</a> are available. Most people get enough magnesium through a <a href="/facts/Healthy_diet/sjJBXc4l">healthy diet</a>, though supplements may help in specific conditions like magnesium deficiency, pregnancy complications, or certain chronic health issues.<a class="footnote-ref" id="fnref:120" href="#fn:120">120</a>
A 2014 <a href="/facts/Literature_review/SIE3DITr">literature review</a> found limited evidence supporting oral magnesium supplementation for <a href="/facts/Migraine/5XaE1W25">migraine</a> prevention, suggesting that increasing dietary magnesium intake may be a more effective option for patients open to lifestyle changes.<a class="footnote-ref" id="fnref:121" href="#fn:121">121</a>

<h3>Metabolism</h3>
An adult body contains 22–26 grams of magnesium,<a class="footnote-ref" id="fnref:122" href="#fn:122">122</a><a class="footnote-ref" id="fnref:123" href="#fn:123">123</a> with 60% in the <a href="/facts/Skeleton/FXc9Y2lF">skeleton</a>, 39% intracellular (20% in skeletal muscle), and 1% extracellular.<a class="footnote-ref" id="fnref:124" href="#fn:124">124</a> Serum levels are typically 0.7–1.0 mmol/L or 1.8–2.4 <a href="/facts/Equivalent_(chemistry)/ksgd425g">mEq</a>/L. Serum magnesium levels may be normal even when intracellular magnesium is deficient. The mechanisms for maintaining the magnesium level in the serum are varying <a href="/facts/Gastrointestinal_tract/nK2zwqBS">gastrointestinal</a> absorption and <a href="/facts/Renal/HBspPrv9">renal</a> excretion. Intracellular magnesium is correlated with intracellular <a href="/facts/Potassium/5lcumVgo">potassium</a>. Increased magnesium lowers <a href="/facts/Calcium/hf252CC0">calcium</a><a class="footnote-ref" id="fnref:125" href="#fn:125">125</a> and can either prevent hypercalcemia or cause hypocalcemia depending on the initial level.<a class="footnote-ref" id="fnref:126" href="#fn:126">126</a> Both low and high protein intake conditions inhibit magnesium absorption, as does the amount of <a href="/facts/Phosphate/FDGVCxUG">phosphate</a>, <a href="/facts/Phytate/qkmaLQ85">phytate</a>, and <a href="/facts/Fat/87HcP11s">fat</a> in the gut. Unabsorbed dietary magnesium is excreted in feces; absorbed magnesium is excreted in urine and sweat.<a class="footnote-ref" id="fnref:127" href="#fn:127">127</a>

<h3>Detection in serum and plasma</h3>
Magnesium status may be assessed by measuring serum and erythrocyte magnesium concentrations coupled with <a href="/facts/Urinary_system/CJxvtE0S">urinary</a> and <a href="/facts/Feces/r9HDKB8G">fecal</a> magnesium content, but intravenous magnesium loading tests are more accurate and practical.<a class="footnote-ref" id="fnref:128" href="#fn:128">128</a> A retention of 20% or more of the injected amount indicates deficiency.<a class="footnote-ref" id="fnref:129" href="#fn:129">129</a> As of 2004, no <a href="/facts/Biomarker/nk2LgXtq">biomarker</a> has been established for magnesium.<a class="footnote-ref" id="fnref:130" href="#fn:130">130</a>
Magnesium concentrations in plasma or serum may be monitored for efficacy and safety in those receiving the drug <a href="/facts/Therapy/2ytkGbgT">therapeutically</a>, to confirm the diagnosis in potential poisoning victims. The newborn children of mothers who received <a href="/facts/Parenteral_nutrition/a27wA3AH">parenteral</a> magnesium sulfate during labor may exhibit toxicity with normal serum magnesium levels.<a class="footnote-ref" id="fnref:131" href="#fn:131">131</a>

<h3>Deficiency</h3>
Low plasma magnesium (<a href="/facts/Hypomagnesemia/GBVGeFw9">hypomagnesemia</a>) is common: it is found in 2.5–15% of the general population.<a class="footnote-ref" id="fnref:132" href="#fn:132">132</a> From 2005 to 2006, 48 percent of the United States population consumed less magnesium than recommended in the <a href="/facts/Dietary_Reference_Intake/FWaI93Dm">Dietary Reference Intake</a>.<a class="footnote-ref" id="fnref:133" href="#fn:133">133</a> Other causes are increased renal or gastrointestinal loss, an increased intracellular shift, and proton-pump inhibitor antacid therapy. Most are asymptomatic, but symptoms referable to <a href="/facts/Neuromuscular_medicine/rdJRWxq4">neuromuscular</a>, <a href="/facts/Circulatory_system/EGs6Y7sI">cardiovascular</a>, and metabolic dysfunction may occur.<a class="footnote-ref" id="fnref:134" href="#fn:134">134</a> <a href="/facts/Alcoholism/KGPzpChp">Alcoholism</a> is often associated with magnesium deficiency. Chronically low serum magnesium levels are associated with <a href="/facts/Metabolic_syndrome/jI70tRBv">metabolic syndrome</a>, <a href="/facts/Diabetes_mellitus_type_2/zCMXksmt">diabetes mellitus type 2</a>, <a href="/facts/Fasciculation/zUfJuPMQ">fasciculation</a>, and hypertension.<a class="footnote-ref" id="fnref:135" href="#fn:135">135</a>

<h3>Therapy</h3>
<ul><li>Intravenous magnesium is recommended by the ACC/AHA/ESC 2006 Guidelines for Management of Patients With Ventricular Arrhythmias and the Prevention of Sudden Cardiac Death for patients with ventricular <a href="/facts/Heart_arrhythmia/ooEpr46Q">arrhythmia</a> associated with <a href="/facts/Torsades_de_pointes/dsdr4HPF">torsades de pointes</a> who present with <a href="/facts/Long_QT_syndrome/kX1NAAUh">long QT syndrome</a>; and for the treatment of patients with digoxin induced arrhythmias.<a class="footnote-ref" id="fnref:136" href="#fn:136">136</a></li>
<li>Intravenous magnesium sulfate is used for the management of <a href="/facts/Pre-eclampsia/FG1BrbC8">pre-eclampsia</a> and <a href="/facts/Eclampsia/K5roBd1g">eclampsia</a>.<a class="footnote-ref" id="fnref:137" href="#fn:137">137</a><a class="footnote-ref" id="fnref:138" href="#fn:138">138</a></li>
<li>Hypomagnesemia, including that caused by alcoholism, is reversible by oral or parenteral magnesium administration depending on the degree of deficiency.<a class="footnote-ref" id="fnref:139" href="#fn:139">139</a></li>
<li>There is limited evidence that magnesium supplementation may play a role in the prevention and treatment of <a href="/facts/Migraine/5XaE1W25">migraine</a>.<a class="footnote-ref" id="fnref:140" href="#fn:140">140</a></li></ul>
<h4>Other medical applications</h4>
Sorted by type of magnesium salt, other therapeutic applications include:

<ul><li><a href="/facts/Magnesium_sulfate/o3GwKEoQ">Magnesium sulfate</a>, as the <a href="/facts/Hydrate/dev82l69">heptahydrate</a>, also known as <a href="/facts/Epsom_salts/o3GwKEoQ">epsom salts</a> from its source mineral, is used as bath salts, a laxative, and a highly soluble fertilizer.<a class="footnote-ref" id="fnref:141" href="#fn:141">141</a></li>
<li><a href="/facts/Magnesium_hydroxide/0hKR5Ica">Magnesium hydroxide</a>, suspended in water, is used in <a href="/facts/Milk_of_magnesia/0hKR5Ica">milk of magnesia</a> antacids and laxatives.</li>
<li><a href="/facts/Magnesium_chloride/uk1f69LG">Magnesium chloride</a>, <a href="/facts/Magnesium_oxide/0GfLn47t">oxide</a>, <a href="/facts/Magnesium_gluconate/V4kJRdI7">gluconate</a>, <a href="/facts/Magnesium_malate/e8exTDbE">malate</a>, <a href="/facts/Magnesium_orotate/SkMGNTjb">orotate</a>, <a href="/facts/Magnesium_glycinate/CYhNpsSG">glycinate</a>, <a href="/facts/Magnesium_ascorbate/nrdlLAVJ">ascorbate</a> and <a href="/facts/Magnesium_citrate/a96acJgM">citrate</a> are all used as oral magnesium supplements.</li>
<li>Magnesium borate, <a href="/facts/Magnesium_salicylate/BhacRFb8">salicylate</a>, and <a href="/facts/Magnesium_sulfate/o3GwKEoQ">sulfate</a> are used as <a href="/facts/Antiseptic/ua05WK9M">antiseptics</a>.</li>
<li><a href="/facts/Magnesium_stearate/55JQEh13">Magnesium stearate</a> is a slightly flammable white powder with lubricating properties. In <a href="/facts/Pharmacology/4Rx8s7Ie">pharmaceutical</a> technology, it is used in pharmacological manufacture to prevent <a href="/facts/Tablet_(pharmacy)/PcYmnjd0">tablets</a> from sticking to the equipment while compressing the ingredients into tablet form.</li>
<li><a href="/facts/Magnesium_carbonate/ymvhw5R8">Magnesium carbonate</a> powder is used by athletes such as gymnasts, weightlifters, and climbers to eliminate palm sweat, prevent sticking, and improve the grip on gymnastic apparatus, lifting bars, and climbing rocks.</li></ul>
<h3>Overdose</h3>
Overdose from dietary sources alone is unlikely because excess magnesium in the blood is promptly filtered by the <a href="/facts/Kidney/HBspPrv9">kidneys</a>. Overdose is more likely in the presence of impaired renal function.<a class="footnote-ref" id="fnref:142" href="#fn:142">142</a> Overdose is likely in cases of excessive intake of supplements. <a href="/facts/Megavitamin_therapy/0GDpHtrh">Megavitamin therapy</a> has caused death in a child,<a class="footnote-ref" id="fnref:143" href="#fn:143">143</a> and severe <a href="/facts/Hypermagnesemia/D1vCcEYC">hypermagnesemia</a> in a woman and a young girl who had healthy kidneys.<a class="footnote-ref" id="fnref:144" href="#fn:144">144</a><a class="footnote-ref" id="fnref:145" href="#fn:145">145</a> The most common symptoms of overdose are nausea, vomiting, and diarrhea; other symptoms include <a href="/facts/Hypotension/BhrdVVRS">hypotension</a>, confusion, slowed heart and <a href="/facts/Respiratory_system/IG8v5JEr">respiratory</a> rates, deficiencies of other minerals, <a href="/facts/Coma/N9oQ7g7R">coma</a>, <a href="/facts/Cardiac_arrhythmia%2fbradycardia/70msP5HD">cardiac arrhythmia</a>, and death from <a href="/facts/Cardiac_arrest/HIAm9AWX">cardiac arrest</a>.<a class="footnote-ref" id="fnref:146" href="#fn:146">146</a>

<h3>Function in plants</h3>
Plants require magnesium to synthesize <a href="/facts/Chlorophyll/1Sb0NyyM">chlorophyll</a>, essential for <a href="/facts/Photosynthesis/TMV7w693">photosynthesis</a>.<a class="footnote-ref" id="fnref:147" href="#fn:147">147</a> Magnesium in the center of the <a href="/facts/Porphyrin_ring/lKNtdXp1">porphyrin ring</a> in chlorophyll functions in a manner similar to the iron in the center of the porphyrin ring in <a href="/facts/Heme/fRhyJAAb">heme</a>. <a href="/facts/Magnesium_deficiency_(plants)/GBVGeFw9">Magnesium deficiency</a> in plants causes late-season yellowing between leaf veins,<a class="footnote-ref" id="fnref:148" href="#fn:148">148</a> especially in older leaves, and can be corrected by either applying epsom salts (which is rapidly leached), or crushed dolomitic limestone, to the soil.

<h2 id="safety-precautions">Safety precautions</h2>

Magnesium metal and its alloys can be explosive hazards; they are highly flammable in their pure form when molten or in powder or ribbon form. Burning or molten magnesium reacts violently with water. When working with powdered magnesium, <a href="/facts/Safety_glasses/ER3sFKmJ">safety glasses</a> with <a href="/facts/Eye_protection/18AyUXLY">eye protection</a> and UV filters (such as welders use) are employed because burning magnesium produces <a href="/facts/Ultraviolet/kncBUqn5">ultraviolet</a> light that can permanently damage the <a href="/facts/Retina/v0ISNX2S">retina</a> of a human eye.<a class="footnote-ref" id="fnref:149" href="#fn:149">149</a>
Magnesium is capable of reducing <a href="/facts/Water_(molecule)/FFsl65l1">water</a> and releasing highly flammable <a href="/facts/Hydrogen/BoYHjl0J">hydrogen</a> gas:<a class="footnote-ref" id="fnref:150" href="#fn:150">150</a>

Mg(s) + 2 H2O(l) → <a href="/facts/Magnesium_hydroxide/0hKR5Ica">Mg(OH)2</a>(s) + H2(g)
Therefore, water cannot extinguish magnesium fires. The hydrogen gas produced intensifies the fire. Dry sand is an effective smothering agent, but only on relatively level and flat surfaces.
Magnesium reacts with <a href="/facts/Carbon_dioxide/xGzpppEp">carbon dioxide</a> exothermically to form <a href="/facts/Magnesium_oxide/0GfLn47t">magnesium oxide</a> and <a href="/facts/Carbon/ukrgQexo">carbon</a>:<a class="footnote-ref" id="fnref:151" href="#fn:151">151</a>

2 Mg(s) + CO2(g) → 2 MgO(s) + C(s)
Hence, carbon dioxide fuels rather than extinguishes magnesium fires.
Burning magnesium can be quenched by using a <a href="/facts/Fire_extinguisher/Lh96vD2x">Class D</a> dry chemical fire extinguisher, or by covering the fire with <a href="/facts/Sand/MdTIt0M8">sand</a> or magnesium foundry flux to remove its air source.<a class="footnote-ref" id="fnref:152" href="#fn:152">152</a>

<h2 id="see-also">See also</h2>
<ul><li><a href="/facts/List_of_countries_by_magnesium_production/nrYtoU4f">List of countries by magnesium production</a></li>
<li><a href="/facts/Magnesium_oil/KCQ0yKuh">Magnesium oil</a></li></ul>
<h2 id="notes">Notes</h2>

<h2 id="cited-sources">Cited sources</h2>
<ul><li>Rumble, John R., ed. (2018). <a href="/facts/CRC_Handbook_of_Chemistry_and_Physics/qjxzC2Cu">CRC Handbook of Chemistry and Physics</a> (99th ed.). Boca Raton, Florida: <a href="/facts/CRC_Press/duTuH4hz">CRC Press</a>. <a href="/facts/ISBN_(identifier)/15AdSPa9">ISBN</a> 978-1-1385-6163-2.</li></ul>
<h2 id="external-links">External links</h2>
<ul><li><a href="http://www.periodicvideos.com/videos/012.htm">Magnesium</a> at <a href="/facts/The_Periodic_Table_of_Videos/vC5kbN0M">The Periodic Table of Videos</a> (University of Nottingham)</li>
<li><a href="http://www.rsc.org/chemistryworld/podcast/element.asp">Chemistry in its element podcast</a> (MP3) from the <a href="/facts/Royal_Society_of_Chemistry/1fg4xnqR">Royal Society of Chemistry</a>'s <a href="/facts/Chemistry_World/kYJKs768">Chemistry World</a>: <a href="http://www.rsc.org/images/CIIE_Magnesium_48kbps_tcm18-128524.mp3">Magnesium</a></li>
<li><a href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC4455823">"Magnesium – a versatile and often overlooked element: New perspectives with a focus on chronic kidney disease"</a>. Clinical Kidney Journal. 5 (Suppl 1): NP. February 2012. <a href="/facts/Doi_(identifier)/muM9Etpq">doi</a>:<a href="https://doi.org/10.1093%2Fndtplus%2Fsfs035">10.1093/ndtplus/sfs035</a>. <a href="/facts/PMC_(identifier)/dX1zMt71">PMC</a> <a href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC4455823">4455823</a>. <a href="/facts/PMID_(identifier)/JlHAvMHt">PMID</a> <a href="https://pubmed.ncbi.nlm.nih.gov/26069823">26069823</a>.</li></ul>

<h2 id="references">References</h2>

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</ol>

Magnesium open-in-new

Magnesium