{"id":465,"date":"2012-05-26T06:46:54","date_gmt":"2012-05-26T06:46:54","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=465"},"modified":"2017-12-07T02:08:58","modified_gmt":"2017-12-07T07:08:58","slug":"tungsten","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/tungsten.html","title":{"rendered":"Tungsten 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\">74<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">W<\/div>\n<div class=\"atweiT\">183.8<\/div>\n<\/div>\n<p>The chemical element tungsten is classed as a transition metal. It was discovered in 1779 by Peter Woulfe.<\/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>  Tungsten 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>   183.84 <\/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> 3422 <sup>o<\/sup>C, 3695 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  5550 <sup>o<\/sup>C, 5823 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>74<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>74<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>110<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,32,12,2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 4f<sup>14<\/sup> 5d<sup>4<\/sup> 6s<sup>2<\/sup>      <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  19.3 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a59469603fe5\"  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-id6a59469603fe5\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   9.53 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   bcc: body-centered cubic  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>   7.5 mohs   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.13  J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 35.40  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  860 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  824.0   kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  770 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td> 1700 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   &#8211;   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>     78.6 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> 6 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  6  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 2.36   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   11.1   &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  w\/ht, &#8658;  WO<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  none  <\/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>   &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> WO<sub>2<\/sub>, WO<sub>3<\/sub> (tungstic oxide) <\/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>  WCl<sub>2<\/sub>, WCl<sub>4<\/sub>, WCl<sub>6<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  139 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\"> 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>  173 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   18.2 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> 3422 <sup>o<\/sup>C, 3695 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 Tungsten<\/h2>\n<p>In 1779 Irish chemist Peter Woulfe deduced the existence of a new element &#8211; tungsten &#8211; from his analysis of the mineral wolframite (an iron manganese tungstate mineral).<\/p>\n<p>Tungsten was isolated as tungstic oxide (WO<sub>3<\/sub>) in 1781, in Sweden, by Carl W. Scheele from the mineral scheelite (calcium tungstate). However he did not have a suitable furnace to reduce the oxide to the metal.<\/p>\n<p>Tungsten was finally isolated by brothers Fausto and Juan Jose de Elhuyar in 1783, in Spain, by reduction of acidified wolframite with charcoal. <\/p>\n<p>The element name comes from the Swedish words &#8216;tung sten&#8217; meaning heavy stone.<\/p>\n<p>The chemical symbol, W, comes from the original name of the element, Wolfram.<\/p>\n<p>Tungsten is one of the five major refractory metals (metals with very high resistance to heat and wear). <\/p>\n<p><strong>The Five Refractory Metals &#8211; note their close relationship in the periodic table<\/strong><br \/>\nThe other refractory metals are <a href=\"https:\/\/www.chemicool.com\/elements\/niobium.html\">niobium<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/molybdenum.html\">molybdenum<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/tantalum.html\">tantalum<\/a>, and <a href=\"https:\/\/www.chemicool.com\/elements\/rhenium.html\">rhenium<\/a>. <\/p>\n<table class=\"navbar\">\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/niobium.html\" title=\"niobium \"><sup>41<\/sup><br \/>Nb<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/molybdenum.html\" title=\"molybdenum \"><sup>42<\/sup><br \/>Mo<\/a> <\/td>\n<td><\/td>\n<\/tr>\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/tantalum.html\" title=\"tantalum \"><sup>73<\/sup><br \/>Ta<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/tungsten.html\" title=\"tungsten \"><sup>74<\/sup><br \/>W<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/rhenium.html\" title=\"rhenium \"><sup>75<\/sup><br \/>Re<\/a> <\/td>\n<\/tr>\n<\/table>\n<div style=\"height:15px;\"><\/div>\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-tungsten.jpg\" width=\"300\" height=\"160\" alt=\"Tungsten metal\" class=\"size-full\" \/><p class=\"wp-caption-text\">Tungsten metal. Photo by Tomihahndorf.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-tungsten-telescope.jpg\" width=\"300\" height=\"196\" alt=\"Tungsten layers - large area telescope\" class=\"size-full\" \/><p class=\"wp-caption-text\">The Large Area Telescope (LAT) explores cosmic rays by tracking the electrons and positrons they produce after striking layers of tungsten. Credit: NASA\/Goddard Space Flight Center Conceptual Image Lab.<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"169\" src=\"https:\/\/www.youtube.com\/embed\/_cs3_fjjCbI?rel=0&#038;start=26\"  allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">The halogen lamp, more properly known as the tungsten halogen lamp.<\/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 \tTungsten is considered to be of low toxicity.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Tungsten is a very hard, dense, silvery-white, lustrous metal that tarnishes in air, forming a protective oxide coating. In powder form tungsten is gray.<\/p>\n<p>\t\tThe metal has the highest melting point of all metals, and at temperatures over 1650 <sup>o<\/sup>C also has the highest tensile strength. Pure tungsten is ductile, and tungsten wires, even of a very small diameter, have a very high tensile strength.<\/p>\n<p>\t\tTungsten is highly resistant to corrosion. It forms tungstic acid (H<sub>2<\/sub>WO<sub>4<\/sub>), or wolframic acid from the hydrated oxide (WO<sub>3<\/sub>) and its salts are called tungstates, or wolframates.<\/p>\n<p>When present in compounds, tungsten exists mostly in the oxidation state VI.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Tungsten<\/h2>\n<p>\t\tTungsten and its alloys are widely used for filaments in older style (not energy saving) electric bulbs and electronic tubes.<\/p>\n<p>Tungsten is also used as the filament in halogen tungsten lamps.  These lamps use halogens like bromine and iodine to prevent the tungsten filament from degrading and are therefore more energy efficient than standard incandescent light bulbs.<\/p>\n<p>High speed steel (which can cut material at higher speeds than carbon steel), contains up to 18% tungsten.<\/p>\n<p>Tungsten is used in heavy metal alloys because of its hardness and in high-temperature applications such as welding.<\/p>\n<p>Tungsten carbide (WC or W<sub>2<\/sub>C) is extremely hard and is used to make drills. It is also used for jewelry because of its hardness and wear resistance.<\/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>  1.25 parts per million by weight,  0.1 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 4 parts per billion by weight, 30 part per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $11 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>   $2.95 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Tungsten is not found free in nature. The principal ores of tungsten are wolframite (an <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a> <a href=\"https:\/\/www.chemicool.com\/elements\/manganese.html\">manganese<\/a> tungstate) and scheelite (<a href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\">calcium<\/a> tungstate, CaWO<sub>3<\/sub>). Commercially, the metal is obtained by reducing tungsten oxide with <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> or <a href=\"https:\/\/www.chemicool.com\/elements\/carbon.html\">carbon<\/a>.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Tungsten has 33 isotopes whose half-lives are known with mass numbers from 158 to 190. Naturally occurring tungsten is a mixture of five isotopes and they are found in the percentages shown: <sup>180<\/sup>W (0.1%), <sup>182<\/sup>W (26.5%), <sup>183<\/sup>W (14.3%), <sup>184<\/sup>W (30.6%) and <sup>186<\/sup>W (28.4%).<\/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<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\/tungsten.html\"&gt;Tungsten&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/tungsten.html\"&gt;Tungsten 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\"Tungsten.\" 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\/tungsten.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 74 W 183.8 The chemical element tungsten is classed as a transition metal. It was discovered in 1779 by Peter Woulfe. Data Zone Classification: Tungsten is a transition metal Color: silvery-white Atomic weight: 183.84 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-465","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/465","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=465"}],"version-history":[{"count":25,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/465\/revisions"}],"predecessor-version":[{"id":4316,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/465\/revisions\/4316"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=465"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}