{"id":688,"date":"2012-06-01T17:36:27","date_gmt":"2012-06-01T17:36:27","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=688"},"modified":"2017-12-07T02:08:38","modified_gmt":"2017-12-07T07:08:38","slug":"samarium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/samarium.html","title":{"rendered":"Samarium Element Facts \/ Chemistry"},"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=\"rareT\">\n<div class=\"atnorT\">62<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Sm<\/div>\n<div class=\"atweiT\"> 150.4<\/div>\n<\/div>\n<p>The chemical element samarium is classed as a lanthanide and rare earth metal. It was discovered in 1853 by Jean Charles Galissard de Marignac.<\/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> Samarium is a lanthanide and rare 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>   150.4 <\/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> 1170 <sup>o<\/sup>C, 1443 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1790 <sup>o<\/sup>C, 2063 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>62<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>62<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>90<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,24,8,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 4f<sup>6<\/sup> 6s<sup>2<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  7.54 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69e7b72dc8d89\"  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-id69e7b72dc8d89\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   20.0 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   close packed (ABCBCACAB)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>    0.20 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>   8.62  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  207 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   191.63   kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 543.3  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>    1068   kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>     2260    kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>  &#8211;  <\/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> 3 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td> 3  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td>   1.17     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>    28.8   &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> mild,  &#8658;  Sm<sub>2<\/sub>O<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  mild, &#8658; Sm(NO<sub>3<\/sub>)<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td>  mild, &#8658;  H<sub>2<\/sub>, SmCl<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td> &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td>   SmO, Sm<sub>2<\/sub>O<sub>3<\/sub> (samaria) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>  SmH<sub>2<\/sub>, SmH<sub>3<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td> SmCl<sub>2<\/sub>, SmCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   185 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>    136 pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td>  109.8 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> &#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>  13.3  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   1.1 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> 1170 <sup>o<\/sup>C, 1443 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:\/\/www.chemicool.com\/elements\/images\/300-samarium-montage2.jpg\" width=\"300\" height=\"141\" alt=\"Samarium uses montage\" class=\"size-full\" \/><p class=\"wp-caption-text\">Samarium-cobalt magnets are used in quartz watches and in camera shutters. <sup>(3)<\/sup><\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Samarium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    In 1853, in Geneva, Switzerland, chemist Jean Charles Galissard de Marignac discovered samarium when he found lines in mineral spectra he was studying that matched no known element.<\/p>\n<p>Paul-&#201;mile Lecoq de Boisbaudran isolated a samarium salt in 1879, in Paris.<\/p>\n<p>First, Boisbaudran extracted &#8216;didymium&#8217; from the mineral samarskite and made a solution of &#8216;didymium&#8217; nitrate. He then added ammonium hydroxide and found two precipitates were formed; one containing &#8216;didymium&#8217; and the other a new element &#8211; samarium. <sup>(1),(2)<\/sup><\/p>\n<p>We should bear in mind that &#8216;didymium&#8217; had been incorrectly identified as a new element by Carl Mosander in 1841.<\/p>\n<p>&#8216;Didymium&#8217; was even given the symbol Di in Mendeleev&#8217;s first edition of the periodic table in 1869.<\/p>\n<p>It wasn&#8217;t until 1885 that Carl Auer von Welsbach established that &#8216;didymium&#8217; was actually composed of two distinct, new elements: <a href=\"neodymium.html\">neodymium<\/a> and <a href=\"praseodymium.html\">praseodymium<\/a>.<\/p>\n<p>The new element samarium was named after the mineral samarskite in which it had been found. (The mineral samarskite had been named in 1847 by mineralogist Heinrich Rose after a Russian mine official, Vasili Samarsky-Bykhovets, who had given him a sample of it.)<\/p>\n<p>In addition to samarium, Lecoq discovered <a href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\">gallium<\/a> in 1875 and he went on to isolate <a href=\"https:\/\/www.chemicool.com\/elements\/gadolinium.html\">gadolinium<\/a> in 1885 and <a href=\"https:\/\/www.chemicool.com\/elements\/dysprosium.html\">dysprosium<\/a> in 1886.<\/p>\n<p>In 1901 Eug&#232;ne-Antole Demar&#231;ay found that Lecoq&#8217;s samarium was impure and he successfully isolated europium magnesium nitrate from a sample of samarium magnesium nitrate.  <sup>(1)<\/sup><\/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=\"225\" src=\"https:\/\/www.youtube.com\/embed\/IFmAhhiam9g?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A brief introduction to the lanthanides.<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-samarium-montage.jpg\" width=\"300\" height=\"305\" alt=\"Samarium uses\" class=\"size-full\" \/><p class=\"wp-caption-text\">Samarium is used in headphones, iPods and guitar pickups.<\/p><\/div>\n<\/div>\n<\/div>\n<\/div>\n<p><a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p>\t  <strong>Harmful effects:<\/strong> <\/p>\n<p>\t \tSamarium is considered to be moderately toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Samarium is a bright, fairly hard, silvery white metal. It is one of the lanthanide rare earth metals.<\/p>\n<p>It is stable in air at normal temperatures, but ignites in air when the temperature is 150 <sup>o<\/sup>C or higher. In moist air it tarnishes to the oxide.<\/p>\n<p>In its compounds Samarium usually exists as a trivalent ion, Sm<sup>3+<\/sup>. Most of its salts are pale yellow in color. <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Samarium<\/h2>\n<p>\t\tSamarium&#8217;s main use is in samarium-cobalt alloy magnets for headphones, small motors and pickups for some electric guitars. These magnets have a high resistance to demagnetization. They keep their ferromagnetism at temperatures up to 700 <sup>o<\/sup>C. <sup>(3)<\/sup> As a result of their ability to operate at high temperatures, SmCo magnets are used in precision-guided weapons.<\/p>\n<p>\t\tSamarium oxide (samaria) is used as a catalyst for the dehydration and dehydrogenation of ethanol. Samarium oxide is also used in infrared absorbing glass.<\/p>\n<p>    Radioactive <sup>153<\/sup>Sm is used in the treatment of cancers.<\/p>\n<p>\t\tSamarium is also used as an absorber in nuclear reactors. <\/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> 6 parts per million by weight, 0.8 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  1 part per billion by weight,  10 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $360 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span> $  per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Samarium is not found free in nature but is found in a number of minerals mainly monazite and bastnaesite. Commercially, it is recovered from monazite sand and bastnaesite using ion exchange and solvent extraction techniques. Samarium metal can be produced by electrolysis of the molten chloride with sodium chloride.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Samarium has 30 isotopes whose half-lives are known, with mass numbers 131 to 160.  Naturally occurring samarium is a mixture of seven isotopes and they are found in the percentages shown: <sup>144<\/sup>Sm (3.1%), <sup>147<\/sup>Sm (15.0%), <sup>148<\/sup>Sm (11.2%), <sup>149<\/sup>Sm (13.8%), <sup>150<\/sup>Sm (7.4%), <sup>152<\/sup>Sm (26.7%) and <sup>154<\/sup>Sm (22.8%). The most abundant isotope is <sup>152<\/sup>Sm at 26.7%.<\/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>\tFerenc Szabadv&#225;ry, Handbook of the Chemistry and Physics of the Rare Earths Vol. 11., Elsevier Science Publishers., 1998, p52 and p62.\t\t <\/li>\n<li>\t John Emsley, Nature&#8217;s building blocks: an A-Z guide to the elements., Oxford University Press, 2003, p372.<\/li>\n<li>\t\t Per Enghag, Encyclopedia of the elements: technical data, history, processing, applications., John Wiley and Sons, 2004, page 485.<\/li>\n<li> Photo: <a href=\"https:\/\/www.llnl.gov\/news\/aroundthelab\/2010\/Nov\/ATL-111910_workshop.html\">LLNL<\/a><\/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\/samarium.html\"&gt;Samarium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/samarium.html\"&gt;Samarium 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\"Samarium.\" Chemicool Periodic Table. Chemicool.com. 18 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\/samarium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 62 Sm 150.4 The chemical element samarium is classed as a lanthanide and rare earth metal. It was discovered in 1853 by Jean Charles Galissard de Marignac. Data Zone Classification: Samarium is a lanthanide and rare earth [&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-688","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/688","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=688"}],"version-history":[{"count":19,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/688\/revisions"}],"predecessor-version":[{"id":4297,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/688\/revisions\/4297"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=688"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}