{"id":293,"date":"2012-05-23T12:46:56","date_gmt":"2012-05-23T12:46:56","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=293"},"modified":"2017-12-07T02:07:40","modified_gmt":"2017-12-07T07:07:40","slug":"cobalt","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/cobalt.html","title":{"rendered":"Cobalt 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\">27<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Co<\/div>\n<div class=\"atweiT\">58.93<\/div>\n<\/div>\n<p>The chemical element cobalt is classed as a transition metal. It was discovered in 1735 by George Brandt.<\/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<tbody>\n<tr>\n<td class=\"elemglb\">Classification:<\/td>\n<td>Cobalt is a transition metal<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>bluish-white<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>58.9332<\/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>1495 <sup>o<\/sup>C, 1768 K<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>2930 <sup>o<\/sup>C, 3203 K<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>27<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>27<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>32<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>2,8,15,2<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>[Ar] 3d<sup>7<\/sup> 4s<sup>2<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>8.90 g\/cm<sup>3<\/sup><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a442f2606713\"  tabindex=\"0\" title=\"Show more: Heats, Energies, Oxidation, Reactions,&lt;br \/&gt; Compounds, Radii, Conductivities\"    >Show more: Heats, Energies, Oxidation, Reactions,<br \/> Compounds, Radii, Conductivities<\/span><div id=\"target-id6a442f2606713\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tbody>\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>6.7 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>5.0 mohs<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>0.42 J g<sup>-1<\/sup> K<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>16.190 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>426 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>373.3 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>758.4 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>1646 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>3232.2 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>63.8 kJ mol<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>-1<\/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>5<\/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>1.88<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Polarizability volume<\/td>\n<td>7.5 \u00c5<sup>3<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Reaction with air<\/td>\n<td>mild, w\/ht ? Co<sub>3<\/sub>O<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Reaction with 15 M HNO<sub>3<\/sub><\/td>\n<td>vigorous, ? Co(NO<sub>3<\/sub>)<sub>2<\/sub>, NO<sub>x<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Reaction with 6 M HCl<\/td>\n<td>mild, ? H<sub>2<\/sub>, CoCl<sub>2<\/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>CoO, Co<sub>3<\/sub>O<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hydride(s)<\/td>\n<td>None<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Chloride(s)<\/td>\n<td>CoCl<sub>2<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius<\/td>\n<td>135 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>83.8 pm<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion)<\/td>\n<td>71.8 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>100 W m<sup>-1<\/sup> K<sup>-1<\/sup><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrical conductivity<\/td>\n<td>17.9 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>1495 <sup>o<\/sup>C, 1768 K<\/td>\n<\/tr>\n<\/tbody>\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 Cobalt<\/h2>\n<p>Since ancient times cobalt compounds have been used to produce blue glass and ceramics.<\/p>\n<p>The element was first isolated by Swedish chemist George Brandt in 1735. He showed it was the presence of the element cobalt that caused the blue color in glass, not <a href=\"https:\/\/www.chemicool.com\/elements\/bismuth.html\">bismuth<\/a> as previously thought.<\/p>\n<p>In about 1741 he wrote, &#8220;As there are six kinds of metals, so I have also shown with reliable experiments&#8230; that there are also six kinds of half-metals: a new half-metal, namely cobalt regulus in addition to mercury, bismuth, zinc, and the reguluses of antimony and arsenic.&#8221;<\/p>\n<p>The word cobalt is derived from the German &#8216;kobold&#8217;, meaning goblin or elf. The image of cobalt below is by Ben Mills.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-cobalt.jpg\" width=\"300\" height=\"155\" alt=\"Cobalt\" 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\" src=\"https:\/\/www.youtube.com\/embed\/GS9kIj9n-BU\" width=\"300\" height=\"233\"><\/iframe><\/p>\n<div class=\"youtubecaption\">Adding HCl shifts the equilibrium and color of a cobalt chloride solution. HCl added to the pink colored Co<sup>2+<\/sup> solution results in the formation of a blue colored solution of CoCl<sub>4<\/sub><sup>2-<\/sup> ions. The reaction is reversible and the colors can switch back and forth when the Cl<sup>&#8211;<\/sup> concentration changes.\n<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/cobalt-electron-shells.gif\" width=\"300\" height=\"300\" alt=\"Cobalt's electron shells\" class=\"size-full\" \/><p class=\"wp-caption-text\">Cobalt&#8217;s electron shells<\/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>Cobalt and its compounds are considered to be slightly toxic by skin contact and moderately toxic by ingestion.<\/p>\n<p><strong>Characteristics:<\/strong><\/p>\n<p>Cobalt is a bluish-white, lustrous, hard, brittle metal. It is ferromagnetic.<\/p>\n<p>The metal is active chemically, forming many compounds. Cobalt stays magnetic to the highest temperature of all the magnetic elements (it has a Curie point of 1121<sup>o<\/sup>C).<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Cobalt<\/h2>\n<p>Cobalt is used in alloys for aircraft engine parts and in alloys with corrosion\/wear resistant uses.<\/p>\n<p>Cobalt is widely used in batteries and in electroplating.<\/p>\n<p>Cobalt salts are used to impart blue and green colors in glass and ceramics.<\/p>\n<p>Radioactive <sup>60<\/sup>Co is used in the treatment of cancer.<\/p>\n<p>Cobalt is essential to many living creatures and is a component of vitamin B<sub>12<\/sub>.<\/p>\n<p>Cobalt is also used in samarium-cobalt permanent magnets. These are used in guitar pickups and high speed motors.<\/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> 25 parts per million by weight, 8 parts per million by moles<\/p>\n<p><span class=\"elemgl\">Abundance solar system:<\/span> 4 parts per million by weight, 0.7 parts per million by moles<\/p>\n<p><span class=\"elemgl\">Cost, pure:<\/span> $21 per 100g<\/p>\n<p><span class=\"elemgl\">Cost, bulk:<\/span> $4.40 per 100g<\/p>\n<p><span class=\"elemgl\">Source:<\/span> Cobalt is not found as a free element in nature. It is found in mineral ores. The main ores of cobalt are cobaltite (CoAsS), erythrite (hydrated arsenate of cobalt), glaucodot (Co,Fe)AsS, and skutterudite (Co,Ni)As<sub>3<\/sub>. Cobalt is generally produced as a by-product of <a href=\"https:\/\/www.chemicool.com\/elements\/nickel.html\"> nickel<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a> mining.<\/p>\n<p><span class=\"elemgl\">Isotopes:<\/span> Cobalt has 22 isotopes whose half-lives are known, with mass numbers 50 to 72. Naturally occurring cobalt consists of its one stable isotope, <sup>59<\/sup>Co.<\/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:\/\/books.google.com\/books?id=WX1GAQAAIAAJ&#038;pg=PA693&#038;dq=Abbe+Hauy+beryl&#038;cd=1#v=onepage&#038;q=beryl&#038;f=false\">Edward Smedley, Hugh James Rose, Henry John Rose, Encyclopaedia Metropolitana; or Universal Dictionary of Knowledge<\/a>., 1845, Volume 4, p693 William Clowes and Sons.<\/li>\n<\/ol>\n<h4>Cite this Page<\/h4>\n<h4 class=\"heading\">Cite this Page<\/h4>\n<p>For online linking, please copy and paste one of the following:<\/p>\n<pre class=\"code\">&lt;a href=\"https:\/\/www.chemicool.com\/elements\/cobalt.html\"&gt;Cobalt&lt;\/a&gt;<\/pre>\n<p>or<\/p>\n<pre class=\"code\">&lt;a href=\"https:\/\/www.chemicool.com\/elements\/cobalt.html\"&gt;Cobalt Element Facts&lt;\/a&gt;<\/pre>\n<p>To cite this page in an academic document, please use the following MLA compliant citation:<\/p>\n<pre class=\"code\">\"Cobalt.\" Chemicool Periodic Table. Chemicool.com. 16 Oct. 2012. Web.<script type=\"text\/javascript\">\/\/ <![CDATA[\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\/cobalt.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 27 Co 58.93 The chemical element cobalt is classed as a transition metal. It was discovered in 1735 by George Brandt. Data Zone Classification: Cobalt is a transition metal Color: bluish-white Atomic weight: 58.9332 State: solid Melting [&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-293","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/293","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=293"}],"version-history":[{"count":31,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/293\/revisions"}],"predecessor-version":[{"id":4219,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/293\/revisions\/4219"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=293"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}