{"id":705,"date":"2012-06-01T19:42:50","date_gmt":"2012-06-01T19:42:50","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=705"},"modified":"2017-12-07T02:07:40","modified_gmt":"2017-12-07T07:07:40","slug":"dysprosium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/dysprosium.html","title":{"rendered":"Dysprosium 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\">66<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Dy<\/div>\n<div class=\"atweiT\">  162.50<\/div>\n<\/div>\n<p>The chemical element dysprosium  is classed as a lanthanide and rare earth metal. It was discovered in 1886 by Paul &#201;mile Lecoq de Boisbaudran.<\/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> Dysprosium 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>   162.50 <\/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> 1410 <sup>o<\/sup>C, 1683 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>   2560 <sup>o<\/sup>C , 2833  K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>66<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>66<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>98<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,28,8,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>    [Xe] 4f<sup>10<\/sup> 6s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  8.536 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69e34201f2fcb\"  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-id69e34201f2fcb\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   19.0 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\">Hardness: <\/td>\n<td>  &#8211;   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>    0.17 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>   11.060  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  291 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   230.0 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 571.9  kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1126    kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  2200     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>    1.22     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   24.5    &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, &#8658;  Dy<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; Dy(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>, DyCl<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>   Dy<sub>2<\/sub>O<sub>3<\/sub> (dysprosia) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>  DyH<sub>2<\/sub>, DyH<sub>3<\/sub>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  DyCl<sub>2<\/sub>, DyCl<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>    121 pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 105.2 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>  10.7  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> 1410 <sup>o<\/sup>C, 1683 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 Dysprosium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>   Dysprosium was discovered in 1886 by French chemist Paul &#201;mile Lecoq de Boisbaudran when he separated dysprosium oxide from holmium oxide.<\/p>\n<p>\t\tBoisbaudran also discovered <a href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\">gallium<\/a> in 1875 and isolated <a href=\"https:\/\/www.chemicool.com\/elements\/samarium.html\">samarium<\/a> for the first time in 1879 using fractional separation.<\/p>\n<p>\t\tBoisbaudran developed an intricate and time-consuming procedure for the separation of dysprosium. This involved 32 precipitations of the hydroxide using ammonia followed by 26 precipitations of the insoluble oxalate salt. <sup>(1)<\/sup><\/p>\n<p>\t\tFittingly he named the element dysprosium, from the Greek &#8216;dysprositos&#8217; meaning &#8216;hard to obtain.&#8217;<\/p>\n<p>\t\tContinuing to live up to its name, pure metallic dysprosium was not isolated for about another eighty years: ion-exchange <a href=\"https:\/\/www.chemicool.com\/definition\/chromatography.html\">chromatography<\/a> finally succeeded in the 1950s.<\/p>\n<p>     The image below shows a selection of rare earth metals and salts. The left-most metal disc is cast dysprosium, resting on a sheet of sublimated dysprosium. The other metal disc is scandium and the metal cylinder is gadolinium. Image Ref.<sup>(2)<\/sup><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-dysprosium.jpg\" width=\"300\" height=\"176\" alt=\"Dysprosium Rare earth metals and salts.\" class=\"aligncenter size-full\" \/><\/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<p><iframe loading=\"lazy\" width=\"300\" height=\"169\" src=\"https:\/\/www.youtube.com\/embed\/7YaNKnre0b0?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Dysprosium in the auto industry.<\/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 \tDysprosium  is considered to be moderately toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Dysprosium is a bright, soft, silvery-white, rare earth metal.<\/p>\n<p>\t\tIt tarnishes slowly in air at room temperature and dissolves in both dilute and concentrated acids.<\/p>\n<p>\t\tWhen present in compounds, dysprosium exists usually in the trivalent state, Dy<sup>3+<\/sup>. <\/p>\n<p>\t\tDysprosium and <a href=\"https:\/\/www.chemicool.com\/elements\/holmium.html\">holmium<\/a> have the highest magnetic strengths of any elements.<\/p>\n<p>\t\tDysprosium also has a high thermal neutron absorption cross-section. which makes it an excellent neutron absorber.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Dysprosium<\/h2>\n<p>\t\tDysprosium is good at absorbing neutrons and so it is used in dysprosium-oxide-nickel cement in control rods in nuclear reactors. <\/p>\n<p>\t\tTerfenol-D (a <a href=\"https:\/\/www.chemicool.com\/elements\/terbium.html\">terbium<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a> and dysprosium alloy) expands or contracts in the presence of a magnetic field (magnetostriction) and is used in ships&#8217; sonar systems and in sensors and transducers. Terfenol-D is also used in a speaker called the &#8216;SoundBug&#8217;, which turns any flat surface into a speaker.<\/p>\n<p>\t\tDysprosium is used in data storage applications such as compact discs and hard discs.<\/p>\n<p>\t\tIt is also used in medium source rare-earth lamps (MSRs) in the film industry. Dysprosium iodide is used these lamps to produce an intense white light.<\/p>\n<p>\t\tWith <a href=\"https:\/\/www.chemicool.com\/elements\/vanadium.html\">vanadium<\/a>, dysprosium is used in laser materials.<\/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, 790 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 2 parts per billion by weight,  10 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span> $450 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span> $30  per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span>  \t\tDysprosium 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. Dysprosium metal can be produced by reduction of its trifluoride with <a href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\">calcium<\/a> metal.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Dysprosium has 29 isotopes whose half-lives are known, with mass numbers 141 to 169. Naturally occurring dysprosium is a mixture of seven isotopes and they are found in the percentages shown: <sup>156<\/sup>Dy (0.06%), <sup>158<\/sup>Dy (0.1%), <sup>160<\/sup>Dy (2.3%), <sup>161<\/sup>Dy (18.9%), <sup>162<\/sup>Dy (25.5%), <sup>163<\/sup>Dy (24.9%) and <sup>164<\/sup>Dy (28.2%). The most abundant isotope is <sup>164<\/sup>Dy at 28.2%.<\/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>Ferenc Szabadv&#225;ry, Handbook of the Chemistry and Physics of the Rare Earths Vol. 11., Elsevier Science Publishers., 1998, p56.<\/li>\n<li>Photo: <a href=\"https:\/\/www.ameslab.gov\/news\/inquiry\/2010-2-root\">Ames Laboratory<\/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\/dysprosium.html\"&gt;Dysprosium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/dysprosium.html\"&gt;Dysprosium 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\"Dysprosium.\" Chemicool Periodic Table. Chemicool.com. 05 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\/dysprosium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 66 Dy 162.50 The chemical element dysprosium is classed as a lanthanide and rare earth metal. It was discovered in 1886 by Paul &#201;mile Lecoq de Boisbaudran. Data Zone Classification: Dysprosium 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-705","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/705","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=705"}],"version-history":[{"count":21,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/705\/revisions"}],"predecessor-version":[{"id":4225,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/705\/revisions\/4225"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=705"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}