{"id":379,"date":"2012-05-24T21:10:51","date_gmt":"2012-05-24T21:10:51","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=379"},"modified":"2017-12-07T02:08:38","modified_gmt":"2017-12-07T07:08:38","slug":"ruthenium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/ruthenium.html","title":{"rendered":"Ruthenium 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=\"tmetalsT\">\n<div class=\"atnorT\">44<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Ru<\/div>\n<div class=\"atweiT\"> 101.1<\/div>\n<\/div>\n<p>The chemical element ruthenium is classed as a transition metal. It was discovered in 1844 by Karl K. Klaus.<\/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>  Ruthenium is a transition 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>   101.07 <\/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> 2330 <sup>o<\/sup>C, 2603 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  4150 <sup>o<\/sup>C, 4423  K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>44<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>44<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>58<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,15,1   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Kr] 4d<sup>7<\/sup> 5s<sup>1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  12.2 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2620c9af14a\"  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-id6a2620c9af14a\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   8.3 cm<sup>3<\/sup>\/mol <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hcp: hexagonal close pkd  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>   6.5  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.238   J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  24.0 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>652  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   595.0 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  711.1 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1617.1  kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2746.9 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    101  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  -2    <\/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> 8 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  4  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 2.2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   9.6 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  w\/ht, &#8658;   RuO<sub>4<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  w\/ht, &#8658;   RuO<sub>4<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td> none  <\/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> RuO<sub>2<\/sub>, RuO<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>  &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  RuCl<sub>2<\/sub>, RuCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   134 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> 82  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> 117  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  14.9 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> 2330 <sup>o<\/sup>C, 2603 K    <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<div class=\"leftimagepadding\">\n<div style=\"width:300px;\">\n<strong>The Platinum Group Metals<\/strong><br \/>\nThese metals have similar properties and are often present in the same mineral ores.\n<\/div>\n<table class=\"navbar\">\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/ruthenium.html\" title=\"ruthenium \"><sup>44<\/sup><br \/>Ru<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/rhodium.html\" title=\"rhodium \"><sup>45<\/sup><br \/>Rh<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/palladium.html\" title=\"palladium \"><sup>46<\/sup><br \/>Pd<\/a> <\/td>\n<\/tr>\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/osmium.html\" title=\"osmium \"><sup>76<\/sup><br \/>Os<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/iridium.html\" title=\"iridium \"><sup>77<\/sup><br \/>Ir<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\" title=\"platinum \"><sup>78<\/sup><br \/>Pt<\/a> <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Ruthenium <\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>Ruthenium was the last of the six platinum group metals (platinum, palladium, rhodium, osmium, iridium and ruthenium) to be discovered.<\/p>\n<p>The initial discovery of ruthenium was thought to have occurred in 1828, when Swedish chemist Jons Jacob Berzelius and Russian chemist Gottfried W. Osann examined the residues left from crude platinum ores after dissolving them in aqua regia (a concentrated solution of hydrochloric and nitric acids).<\/p>\n<p>Osann believed that there were three new metals in these residues, which he called pluranium, polinium and ruthenium. Berzelius was, however, skeptical. <\/p>\n<p>Later, in 1844, in Kazan, Russia, Karl K. Klaus repeated Osann&#8217;s work to clarify the results. He proved that there was only one new metal present in the residues. He kept Osann&#8217;s name of ruthenium for this new metal.<\/p>\n<p>Klaus used a lengthy process to obtain the salt, ammonium chlororuthenate, (NH<sub>4<\/sub>)<sub>2<\/sub>RuCl<sub>6<\/sub>, from which he could isolate the metal ruthenium and identify its properties. <sup>(1)<\/sup>  <\/p>\n<p>The element&#8217;s name comes from the Latin word &#8216;Ruthenia&#8217; meaning Russia, as the platinum ores were originally from the Ural Mountains in Russia.<\/p>\n<p>Below is a photo, by Tomihahndorf, of a 1 gram bead of high-purity ruthenium.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-ruthenium.jpg\" width=\"300\" height=\"160\" alt=\"1 gram bead of high-purity ruthenium\" 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=\"169\" src=\"https:\/\/www.youtube.com\/embed\/H7Ng4sOVkns?rel=0&#038;start=4\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Ruthenium is immune to concentrated acids, but can be dissolved by household bleach. Do not try this at home!\n<\/div>\n<div style=\"width: 305px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-ruthenium-graphene.jpg\" width=\"295\" height=\"275\" alt=\"Ruthenium\" class=\"size-full\" \/><p class=\"wp-caption-text\">The surface of ruthenium metal provides a suitable environment to grow high quality, large area <a href=\"carbon.html\">graphene<\/a> layers. Image: <a href=\"http:\/\/www.bnl.gov\/today\/story.asp?ITEM_NO=1756\">BNL<\/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 \tRuthenium is a suspected carcinogen and its compounds strongly stain the skin. Ruthenium tetroxide (RuO<sub>4<\/sub>) is highly toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Ruthenium is a very rare, hard, lustrous, brittle, silvery-white metal that does not tarnish at room temperature. <\/p>\n<p>Typical of transition metals, ruthenium can exist in many oxidation states, its most common being the oxidation states II, III and IV.<\/p>\n<p>\t\tThe metal is unaffected by air, water and acids. <\/p>\n<p>\t\tIt reacts with molten alkali and halogens and can oxidize explosively.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Ruthenium<\/h2>\n<p>\t\tSmall amounts of ruthenium are used to harden <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/palladium.html\">palladium<\/a> and it can also be alloyed with these metals to make electrical contacts for severe wear resistance.<\/p>\n<p>\t\tThe addition of 0.1% ruthenium improves the corrosion resistance of <a href=\"https:\/\/www.chemicool.com\/elements\/titanium.html\">titanium<\/a> a hundred times over.<\/p>\n<p>\t\tRuthenium has catalytic properties; for example, hydrogen sulfide can be split by light in the presence of an aqueous suspension of cadmium sulfide particles loaded with ruthenium dioxide.<\/p>\n<p>Interestingly, ruthenium is used in some Parker pen nibs, such as the Parker 51 whose nib is marked &#8216;RU&#8217;, and consists of 96.2% ruthenium and 3.8% iridium<sup>(2)<\/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>  1 part per billion by weight,  0.2 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 5 parts per billion by weight,  0.06 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>   $1400 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>   $650 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Ruthenium is found free in nature often with the other platinum group metals. Commercially, it is obtained from pentlandite (a sulfide of <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/nickel.html\">nickel<\/a>) which contains small quantities of ruthenium. <\/p>\n<p>\t\tRuthenium can also be extracted from spent nuclear fuel, however if obtained this way it will contain radioactive isotopes. It has to be stored safely for at least ten years until the radioactive isotopes have decayed. <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span>   Ruthenium has 26 isotopes whose half-lives are known, with mass numbers from 90 to 115. Naturally occurring ruthenium is a mixture of seven isotopes and they are found in the percentages shown: <sup>96<\/sup>Ru (5.5%), <sup>98<\/sup>Ru (1.9%), <sup>99<\/sup>Ru (12.8%), <sup>100<\/sup>Ru (12.6%), <sup>101<\/sup>Ru (17.1%), <sup>102<\/sup>Ru (31.6%), and<sup>104<\/sup>Ru (18.6%). Naturally, the most common isotope is <sup>102<\/sup>Ru with an abundance of 31.6%.<\/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. VIII. The Platinum Metals., J. Chem. Educ., June 1932, p1028-1032.<\/li>\n<li><a href=\"http:\/\/www.nibs.com\/article4.html\">The Nibster &#8211; Where&#8217;s The Iridium?<\/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\/ruthenium.html\"&gt;Ruthenium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/ruthenium.html\"&gt;Ruthenium 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\"Ruthenium.\" 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\/ruthenium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 44 Ru 101.1 The chemical element ruthenium is classed as a transition metal. It was discovered in 1844 by Karl K. Klaus. Data Zone Classification: Ruthenium is a transition metal Color: silvery-white Atomic weight: 101.07 State: solid [&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-379","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/379","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=379"}],"version-history":[{"count":24,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/379\/revisions"}],"predecessor-version":[{"id":4295,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/379\/revisions\/4295"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=379"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}