{"id":723,"date":"2012-06-02T11:10:41","date_gmt":"2012-06-02T11:10:41","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=723"},"modified":"2017-12-07T02:08:58","modified_gmt":"2017-12-07T07:08:58","slug":"thulium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/thulium.html","title":{"rendered":"Thulium 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\">69<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Tm<\/div>\n<div class=\"atweiT\"> 168.9<\/div>\n<\/div>\n<p>The chemical element thulium is classed as a lanthanide and rare earth metal. It was discovered in 1879 by Per Teodor Cleve.<\/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> Thulium is a lanthanide and rare earth metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td> silvery-gray  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   168.9342 <\/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> 1550 <sup>o<\/sup>C, 1823 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1950 <sup>o<\/sup>C, 2223 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>69<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>69<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>100<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,31,8,2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 4f<sup>13<\/sup> 6s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  9.33 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69e121eee4d3b\"  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-id69e121eee4d3b\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>  18.1 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hexagonal close packed  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.16 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>   16.840  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 232 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    191.0   kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 596.7  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1163   kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  2285    kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   99 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> 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>  1.25   <\/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;  Tm<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; Tm(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>, TmCl<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>   Tm<sub>2<\/sub>O<sub>3<\/sub> (thulia) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   TmH<sub>2<\/sub>, TmH<sub>3<\/sub>     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   TmCl<sub>2<\/sub>, TmCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  175 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>   117  pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 102  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> 16.9  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td> 1.3 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> 1550 <sup>o<\/sup>C, 1823 K   <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<div class=\"leftimagepadding\">\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Thulium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    \tPer Teodor Cleve discovered two new materials, one green and one brown, while working with erbia (erbium oxide) in 1879, in Uppsala, Sweden. These turned out to be oxides of two new elements: thulium and <a href=\"https:\/\/www.chemicool.com\/elements\/holmium.html\">holmium<\/a>. <sup>(1), (2)<\/sup><\/p>\n<p>The green substance he named thulia, which he later found to be thulium oxide and the brown substance he named holmia, which he later found to be holmium oxide.<\/p>\n<p>Cleve&#8217;s discovery was similar to those of Swedish chemist Carl Gustaf Mosander in 1843. Mosander discovered <a href=\"https:\/\/www.chemicool.com\/elements\/erbium.html\">erbium<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/terbium.html\">terbium<\/a> in yttria, which is mainly comprised of yttrium oxide.<\/p>\n<p>Charles James in New Hampshire, prepared the first pure thulium in 1911 by repeated bromate fractional crystallizations, which became known as the &#8216;James Method.&#8217;   <sup>(3),(4) <\/sup><\/p>\n<p> The element name comes from &#8216;Thule&#8217;, an ancient name for Scandinavia.<\/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<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-europium-euro-note.jpg\" width=\"300\" height=\"158\" alt=\"Thulium anti-counterfeiter\" class=\"size-full\" \/><p class=\"wp-caption-text\">Euro banknotes use rare earth chemistry to defeat counterfeiters. Shining UV light on a euro results in blue fluorescence from thulium Tm<sup>3+<\/sup>, red from europium Eu<sup>3+<\/sup>, and green from terbium Tb<sup>3+<\/sup>.<\/p><\/div>\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\">Thulium is a rare earth metal in the lanthanide series.<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-thulium-blood-irradiator.jpg\" width=\"300\" height=\"234\" alt=\"Thulium blood irradiator\" class=\"size-full\" \/><p class=\"wp-caption-text\">An innovative portable blood irradiator which uses thulium and vitreous <a href=\"https:\/\/www.chemicool.com\/elements\/carbon.html\">carbon<\/a> to destroy circulating lymphocyctes. Photo: <a href=\"http:\/\/picturethis.pnl.gov\/picturet.nsf\/All\/44YM2V?opendocument\">PNNL<\/a><\/p><\/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 \tThulium is considered to be non-toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\tThulium is a bright, soft, malleable, silvery-gray metal.<\/p>\n<p>\t\tIt is a rare earth metal and is one of the least abundant.<\/p>\n<p>\t\tThe metal tarnishes slowly in dry air to form the oxide and reacts with water to form the hydroxide and hydrogen gas.<\/p>\n<p>\t\tTm<sup>3+<\/sup> ions emit a strong blue luminescence when excited. <\/p>\n<p>\t\tWhen present in compounds, thulium exists usually in the trivalent state, Tm<sup>3+<\/sup>. It forms compounds &#8211; mostly green in color &#8211; with oxygen and the halogens.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Thulium<\/h2>\n<p>\t\tRadioactive isotope <sup>170<\/sup>Tm is produced by bombarding thulium in a nuclear reactor. It has a half-life of 128 days and is used as a portable source of x-rays.<\/p>\n<p>\t\tThulium is used to dope yttrium aluminum garnets (YAG) used in lasers.<\/p>\n<p>\t\tThulium is also used in alloys with other rare earth metals.<\/p>\n<p>\t\tThulium is used in euro banknotes for its blue fluorescence under UV light to defeat counterfeiters. <\/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> 0.5 parts per million by weight, 50 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  200 parts per trillion by weight,  1 part per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span> $700 per 10g<\/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> Thulium is not found free in nature but is found in a number of minerals: mainly monazite, gadolinite, xenotime and euxenite. Commercially, it is isolated by ion exchange and solvent extraction. The metal can be isolated by reduction of the anhydrous fluoride with calcium metal, or by the reduction of the oxide with lanthanum metal.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Thulium has 32 isotopes whose half-lives are known, with mass numbers 146 to 177. Naturally occurring thulium consists of its one stable isotope, <sup>169<\/sup>Tm.<\/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>Mary Elvira Weeks, The Discovery of the Elements XVI., Journal of Chemical Education., October 1932, p1761,1762. <\/li>\n<li>\t\tRobert E. Krebs, The history and use of our earth&#8217;s chemical elements: a reference guide., JGreenwood Publishing Group, 2006, p300.<\/li>\n<li>\t\tJames Roy Newman, The International encyclopedia of science., Volume 4, Nelson, 1965, p1186.  <\/li>\n<li>\tUniversity of New Hampshire Alumni Association, <a href=\"http:\/\/unhmagazine.unh.edu\/f10\/charles_james_3.html\">The Life and Work of Charles James.<\/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\/thulium.html\"&gt;Thulium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/thulium.html\"&gt;Thulium 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\"Thulium.\" Chemicool Periodic Table. Chemicool.com. 24 Jul. 2015. 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\/thulium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 69 Tm 168.9 The chemical element thulium is classed as a lanthanide and rare earth metal. It was discovered in 1879 by Per Teodor Cleve. Data Zone Classification: Thulium is a lanthanide and rare earth metal Color: [&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-723","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/723","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=723"}],"version-history":[{"count":22,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/723\/revisions"}],"predecessor-version":[{"id":4313,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/723\/revisions\/4313"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=723"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}