{"id":186,"date":"2012-05-22T12:26:43","date_gmt":"2012-05-22T12:26:43","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=186"},"modified":"2017-12-07T02:08:08","modified_gmt":"2017-12-07T07:08:08","slug":"magnesium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/magnesium.html","title":{"rendered":"Magnesium Element Facts"},"content":{"rendered":"<div class=\"insidepagelinks\">\n<a href=\"#data\">Data Zone<\/a> |  <a href=\"#discovery\">Discovery<\/a> |  <a href=\"#facts\">Facts<\/a> | <a href=\"#appear\">Appearance &amp; Characteristics<\/a> | <a href=\"#uses\">Uses<\/a> | <a href=\"#abund\">Abundance &amp; Isotopes<\/a>  | <a href=\"#refer\">References<\/a>\n<\/div>\n<div class=\"alkalieT\">\n<div class=\"atnorT\">12<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Mg<\/div>\n<div class=\"atweiT\">24.30<\/div>\n<\/div>\n<p>The chemical element magnesium is classed as an alkali earth metal. It was discovered in 1808 by Humphrey Davy.<\/p>\n<div style=\"clear:both;\"><\/div>\n<div class=\"adsense300\">\n<div class=\"adsense300spacer\">\n<div style=\"line-height:10px;\"><img decoding=\"async\" src=\"\/\/www.chemicool.com\/ad.png\" alt=\"\" \/><\/div>\n<p><script async src=\"\/\/pagead2.googlesyndication.com\/pagead\/js\/adsbygoogle.js\"><\/script><ins class=\"adsbygoogle\" style=\"display: block;\" data-ad-client=\"ca-pub-9461632227417539\" data-ad-slot=\"8753977201\" data-ad-format=\"auto\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/p>\n<p><a id=\"data\"><\/a><\/p>\n<h2>Data Zone<\/h2>\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Classification:<\/td>\n<td> Magnesium is an alkali earth metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  silvery-white   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   24.305 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">State:<\/td>\n<td>   solid   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Melting point:<\/td>\n<td> 650 <sup>o<\/sup>C, 923 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1090 <sup>o<\/sup>C, 1363 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>12<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>12<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>12<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>    1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  1.738 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a320a85ca2eb\"  tabindex=\"0\" title=\"Show more, including: Heats, Energies, Oxidation,&lt;br \/&gt; Reactions, Compounds, Radii, Conductivities\"    >Show more, including: Heats, Energies, Oxidation,<br \/> Reactions, Compounds, Radii, Conductivities<\/span><div id=\"target-id6a320a85ca2eb\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   13.97 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hcp: hexagonal close packed <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    2.5 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  1.02 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 8.48 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  146 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    127.4 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 737.7 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1450.6 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    7732.6 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   78 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  0    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Min. common oxidation no.<\/td>\n<td>  0  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Maximum oxidation number <\/td>\n<td> 2 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 1.31    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   10.6 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> vigorous, w\/ht &#8658;  MgO, Mg<sub>3<\/sub>N<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  vigorous &#8658; NO<sub>x<\/sub>,  Mg(NO<sub>3<\/sub>)<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td> mild  &#8658; H<sub>2<\/sub>, MgCl<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>   none  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> MgO <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   MgH<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  MgCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   150 pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (1+ ion) <\/td>\n<td> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>  86  pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Ionic radius (1- ion) <\/td>\n<td>   &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Ionic radius (2- ion) <\/td>\n<td> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Ionic radius (3- ion) <\/td>\n<td>   &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Thermal conductivity <\/td>\n<td> 156 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td> 22.4 x 10<sup>6<\/sup> S m<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Freezing\/Melting point:<\/td>\n<td> 650 <sup>o<\/sup>C, 923 K    <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<div class=\"leftimagepadding\">\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-magnesium-metal.jpg\" width=\"300\" height=\"154\" alt=\"Magnesium metal\" class=\"size-full\" \/><p class=\"wp-caption-text\">Magnesium metal. Image by Maral10.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-milk-magnesia.jpg\" width=\"300\" height=\"132\" alt=\"Magnesia\" class=\"size-full\" \/><p class=\"wp-caption-text\">Joseph Black was investigating magnesia alba (magnesium carbonate) as a cure for indigestion when he made his chemical discoveries. Milk of magnesia, made with magnesium hydroxide, is now used to relieve indigestion. The hydroxide has an advantage over Black&#8217;s carbonate: its reaction with stomach acid (HCl) doesn&#8217;t release carbon dioxide, so it doesn&#8217;t cause belching. It does, however, form magnesium chloride, which is a laxative.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-magnesium-fireworks.jpg\" width=\"300\" height=\"144\" alt=\"Magnesium Firworks\" class=\"size-full\" \/><p class=\"wp-caption-text\">Magnesium gives intense, white light in fireworks.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Magnesium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Magnesium and calcium were once thought to be the same substance. In 1755 Scottish chemist Joseph Black showed by experiment that the two were different. Black wrote: <\/p>\n<p>\t\t&#8220;We have already shewn by experiment, that magnesia alba [magnesium carbonate] is a compound of a peculiar earth and fixed air.&#8221; <sup>(1)<\/sup> <\/p>\n<p>\t\tMagnesium was first isolated by Sir Humphrey Davy in 1808, in London, England. Davy had built a large battery and used it to pass electricity through salts. In doing so, he discovered or isolated for the first time several alkali and alkali earth metals. <\/p>\n<p>\t\tIn magnesium&#8217;s case, Davy&#8217;s method was similar to the one he used for <a href=\"https:\/\/www.chemicool.com\/elements\/barium.html\">barium<\/a>, <a href=\"calcium.htm\">calcium<\/a> and <a href=\"strontium.html\">strontium<\/a>.<\/p>\n<p>\t\tDavy made a paste of moist magnesium oxide and red mercury oxide. <sup>(2)<\/sup><\/p>\n<p>\t\tHe made a depression in the paste and placed about 3.5 grams of <a href=\"https:\/\/www.chemicool.com\/elements\/mercury.html\">mercury metal<\/a> there to act as the negative electrode. He used <a href=\"platinum.html\">platinum<\/a> as the positive electrode. Davy did the experiment under naphtha (a liquid hydrocarbon under which he had found he could safely store <a href=\"https:\/\/www.chemicool.com\/elements\/potassium.html\">potassium<\/a> and <a href=\"sodium.html\">sodium<\/a>).<\/p>\n<p> \t\tWhen electricity was passed through the paste, a magnesium-mercury amalgam formed at the mercury electrode. (In later experiments Davy used moist magnesium sulfate instead of the oxide and obtained the amalgam much faster.) <sup>(2)<\/sup>    <\/p>\n<p>\t\tThe mercury was then removed from the amalgam by heating to leave magnesium metal. <sup>(2)<\/sup><\/p>\n<p>\t\tIn a lecture to the Royal Society in June 1808, Davy described how the magnesium he obtained was not pure because of difficulties in removing the mercury entirely from the magnesium. He was, however, able to observe that in air the metal turned into a white powder, gaining weight as it reacted with oxygen and returned to its oxide form. \t\t<sup>(2)<\/sup> <\/p>\n<p>\t\tDavy thought the logical name for the new metal was &#8216;magnesium&#8217; but instead called it &#8216;magnium.&#8217;<br \/>\n\t\tHe thought the name &#8216;magnium&#8217; was, &#8220;objectionable, but magnesium has been already applied to metallic manganese&#8230;&#8221;<\/p>\n<p>\t\tBy 1812, Davy had changed his mind, following the &#8220;candid criticisms of some philosophical friends,&#8221; and the new metal became known as magnesium, while metallic manganese became known as&#8230; manganese. <sup>(3)<\/sup> <\/p>\n<p>\t\tMagnesium&#8217;s name is derived from magnesia, which Davy used in his experiment. Magnesia is the district of Thessaly in Greece where magnesia alba [magnesium carbonate] was found.  <\/p>\n<p>\t\tIn France, in 1830, Antoine Bussy published his work showing how pure magnesium metal could be obtained. Bussy had read Friedrich W&#246;hler&#8217;s 1828 publication of how he had produced pure <a href=\"aluminum.html\">aluminum<\/a> by reacting aluminum chloride with potassium. By analogy, Bussy thought he could do something similar to produce pure magnesium from magnesium chloride; he was correct. <\/p>\n<p>\t\tUnder red heat he reacted magnesium chloride with potassium vapor and obtained pure magnesium. He wrote, &#8220;The metal is silvery white, very brilliant, very malleable, flattens into flakes under a hammer&#8230; dilute acids attack the metal, releasing hydrogen.&#8221; <sup>(4)<\/sup><\/p>\n<p>Visit Chemicool&#8217;s <a href=\"https:\/\/www.chemicool.com\/elements\/magnesium-facts.html\">Cool Magnesium Facts Page<\/a><\/p>\n<div style=\"clear:both;line-height:20px;\">&nbsp;<\/div>\n<div class=\"adsense300\">\n<div class=\"adsense300spacer\">\n<div style=\"line-height: 10px;\"><img decoding=\"async\" src=\"\/\/www.chemicool.com\/ad.png\" alt=\"\" \/><\/div>\n<p><script async src=\"\/\/pagead2.googlesyndication.com\/pagead\/js\/adsbygoogle.js\"><\/script><ins class=\"adsbygoogle\" style=\"display: inline-block; width: 336px; height: 280px;\" data-ad-client=\"ca-pub-9461632227417539\" data-ad-slot=\"2986645201\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/p>\n<div class=\"leftimagepadding\">\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/wqErrNvns4o?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Should I use carbon dioxide to extinguish a magnesium fire?<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/95O-bQo04Ok?rel=0\" allowfullscreen><\/iframe> <\/p>\n<div class=\"youtubecaption\">Is it a good idea to extinguish burning magnesium with water?<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p><a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p><strong>Harmful effects:<\/strong> <\/p>\n<p>\t \tMagnesium powder is an explosive hazard.<\/p>\n<p>\t\tThe bright white light plus ultraviolet from burning magnesium can cause permanent eye damage.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Magnesium is a silvery-white, low density, reasonably strong metal that tarnishes in air to form a thin oxide coating. Magnesium and its alloys have very good corrosion resistance and good high temperature mechanical properties. <\/p>\n<p>\t\tThe metal reacts with water to produce <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen gas<\/a>.<\/p>\n<p>\t\tWhen it burns in air, magnesium produces a brilliant white light.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Magnesium<\/h2>\n<p>\t\tThe brilliant light it produces when ignited is made use of in photography, flares, and pyrotechnics. <\/p>\n<p>\t\tWith a density of only two-thirds that of <a href=\"https:\/\/www.chemicool.com\/elements\/aluminum.html\">aluminum<\/a>, and just over one-fifth that of <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a>, magnesium alloys are used in aircraft, car engine casings, and missile construction.    <\/p>\n<p>\t\tThe metal is widely used in the manufacturing of mobile phones, laptop computers, cameras, and other electronic components.<\/p>\n<p>\t\tOrganic magnesium compounds (<a href=\"https:\/\/www.chemicool.com\/definition\/grignard_reagents.html\">Grignard reagents<\/a>) are important in the synthesis of organic molecules. <\/p>\n<p>\t\tMagnesium compounds such as the hydroxide (milk of magnesia, Mg(OH<sub>2<\/sub>)), sulfate (Epsom salts), chloride and citrate are used for medicinal purposes.<\/p>\n<p>\t\tMagnesium is the second most important intracellular cation and is involved in a variety of metabolic processes including glucose metabolism, ion channel translocation, stimulus-contraction coupling, stimulus secretion coupling, peptide hormone receptor signal transduction. <sup>(5)<\/sup><\/p>\n<p><a id=\"abund\"><\/a><\/p>\n<h2>Abundance and Isotopes<\/h2>\n<p><span class=\"elemgl\">Abundance earth&#8217;s crust:<\/span>  2.3 % by weight, 2.0 % by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 700 parts per million by weight, 30 parts per million by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $3.7 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $0.29 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Magnesium is the eighth most abundant element in the Earth&#8217;s crust and the sixth most abundant metal. Magnesium is obtained commercially by the &#8216;Pidgeon&#8217; process. This high temperature method uses silicon as a reducing agent to extract magnesium from minerals such as dolomite (MgCa(CO <sub>3<\/sub>)<sub>2<\/sub>) or magnesite (MgCO <sub>3<\/sub>) or saltwater. <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span>  Magnesium has 15 isotopes whose half-lives are known with mass ranges from 20 to 34. Naturally occurring magnesium is a mixture of its three stable isotopes and they are found in the percentages shown: <sup>24<\/sup>Mg (79.0%), <sup>25<\/sup>Mg (10.0%) and <sup>26<\/sup>Mg (11.0%). <\/p>\n<div style=\"max-width: 750px;\">\n<div style=\"line-height: 10px;\"><img decoding=\"async\" src=\"\/\/www.chemicool.com\/ad.png\" alt=\"\" \/><\/div>\n<p><script async src=\"\/\/pagead2.googlesyndication.com\/pagead\/js\/adsbygoogle.js\"><\/script><ins class=\"adsbygoogle\" style=\"display: block;\" data-ad-client=\"ca-pub-9461632227417539\" data-ad-slot=\"8753977201\" data-ad-format=\"auto\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/p>\n<\/div>\n<p><a id=\"refer\"><\/a><\/p>\n<h4>References<\/h4>\n<ol>\n<li><a href=\"http:\/\/web.lemoyne.edu\/~giunta\/Black.html\">Joseph Black, Experiments upon Magnesia Alba, Quick-Lime, and some other Alkaline Substances (1756)<\/a><\/li>\n<li>John Davy (Editor), The Collected Works of Sir Humphry Davy, Vol V, 1840, p110-115 Smith, Elder and Co. Cornhill.<\/li>\n<li>Sir Humphry Davy,\t<a href=\"http:\/\/books.google.com\/books?id=YjMwAAAAYAAJ&#038;pg=PA60&#038;dq=Elements+of+chemical+philosophy:+part+1,+Volume+1,+Part+1+By+Sir+Humphry+Davy&#038;cd=1#v=onepage&#038;q&#038;f=false\">Elements of Chemical Philosophy<\/a>., 1812, Part 1, Vol. 1,  p198.<\/li>\n<li>Gay-Lussac et al, Annals of Chemistry and Physics, 1831, Vol. XLVI, p434-437.<\/li>\n<li>Nancy E. Bernhardt, Artur M. Kasko, Nutrition for the Middle Aged and Elderly., (2008) p333. Nova Science Publishers <\/li>\n<\/ol>\n<h4>Cite this Page<\/h4>\n<p>For online linking, please copy and paste one of the following:<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\"&gt;Magnesium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\"&gt;Magnesium Element Facts&lt;\/a&gt;\r\n<\/pre>\n<p>To cite this page in an academic document, please use the following MLA compliant citation:<\/p>\n<pre class='code'>\r\n\"Magnesium.\" Chemicool Periodic Table. Chemicool.com. 07 Oct. 2012. Web. <script type=\"text\/javascript\">\r\n<!--\r\nvar currentTime = new Date()\r\nvar month = currentTime.getMonth() + 1\r\nvar day = currentTime.getDate()\r\nvar year = currentTime.getFullYear()\r\ndocument.write(month + \"\/\" + day + \"\/\" + year)\r\n\/\/-->\r\n<\/script> \r\n&lt;https:\/\/www.chemicool.com\/elements\/magnesium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 12 Mg 24.30 The chemical element magnesium is classed as an alkali earth metal. It was discovered in 1808 by Humphrey Davy. Data Zone Classification: Magnesium is an alkali earth metal Color: silvery-white Atomic weight: 24.305 State: [&hellip;]<\/p>\n","protected":false},"author":3,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"class_list":{"0":"post-186","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/186","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/users\/3"}],"replies":[{"embeddable":true,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/comments?post=186"}],"version-history":[{"count":27,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/186\/revisions"}],"predecessor-version":[{"id":4261,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/186\/revisions\/4261"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=186"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}