{"id":524,"date":"2012-05-29T05:56:01","date_gmt":"2012-05-29T05:56:01","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=524"},"modified":"2017-12-07T02:07:25","modified_gmt":"2017-12-07T07:07:25","slug":"bismuth","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/bismuth.html","title":{"rendered":"Bismuth 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=\"ometalsT\">\n<div class=\"atnorT\">83<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Bi<\/div>\n<div class=\"atweiT\"> 209.0<\/div>\n<\/div>\n<p>The chemical element bismuth is classed as an other metal. It was discovered in 1753 by Claude Geoffroy the Younger.<\/p>\n<div style=\"clear:both;\"><\/div>\n<div class=\"adsense300\">\n<div class=\"adsense300spacer\">\n<div style=\"line-height:10px;\">\n<img decoding=\"async\" alt=\"\" src=\"\/\/www.chemicool.com\/ad.png\"\/>\n<\/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=\"3265846807\"><\/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>  Bismuth is an &#8216;other metal&#8217;   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  silver-white <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   208.9804 <\/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> 271.4 <sup>o<\/sup>C, 544.5 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1564 <sup>o<\/sup>C, 1837 K      <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>83<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>83<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>126<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,32,18,5    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 4f<sup>14<\/sup> 5d<sup>10<\/sup> 6s<sup>2<\/sup> 6p<sup>3<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  9.807 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a559c93b36fd\"  tabindex=\"0\" title=\"Show more, including: Heats, Energies, Oxidation, Reactions,&lt;br \/&gt; Compounds, Radii, Conductivities\"    >Show more, including: Heats, Energies, Oxidation, Reactions,<br \/> Compounds, Radii, Conductivities<\/span><div id=\"target-id6a559c93b36fd\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   21.3 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>  rhombohedral <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    2.25 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.123 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  11.3 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 207 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  151 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 703 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1610 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2466 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    91 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  -3    <\/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> 2.02   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>  7.4 &Aring;<sup>3<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>   mild, w\/ht &#8658; Bi<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; Bi(NO<sub>3<\/sub>)<sub>3<\/sub>, NO<sub>x<\/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> Bi<sub>2<\/sub>O<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>    BiH<sub>3<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  BiCl<sub>3<\/sub>, BiCl<sub>4<\/sub><\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   160 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>  117  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>  7.92 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   0.867 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> 271.4 <sup>o<\/sup>C, 544.5 K     <\/td>\n<\/tr>\n<\/table>\n<\/div><\/div>\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-bismuth-crystal.jpg\" width=\"300\" height=\"171\" alt=\"Bismuth Crystal\" class=\"size-full\" \/><p class=\"wp-caption-text\">A crystal of bismuth. The colors come from light interference in a thin oxide layer on the surface of the crystal. Image Ref. <sup>(1)<\/sup><\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/hnbfGaqNvjU?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A cube of bismuth sits between two bismuth plates. A large <a href=\"neodymium.html\">neodymium<\/a> magnet is held above the plates and cube. Bismuth is diamagnetic; this means it produces a magnetic field in opposition to any applied magnetic field. Here bismuth opposes the neodymium magnet&#8217;s magnetic field, with the result that the cube floats in the air. <a href=\"carbon.html\">Carbon<\/a> in its graphite form is also diamagnetic.<\/div>\n<\/div>\n<\/div>\n<p>\t\t\t<a id=\"discovery\"><\/a>\t<\/p>\n<h2>Discovery of Bismuth<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Bismuth has been known since the fifteenth century. <\/p>\n<p>In 1753, French chemist Claude Geoffroy the Younger established that it was an element in its own right rather than a form of <a href=\"lead.html\">lead<\/a>.<\/p>\n<p>Bismuth is considered to be stable, although it is actually radioactive with an extremely slow rate of decay. <\/p>\n<p>If precisely 100 grams of bismuth-209 had been present at the beginning of the universe 14 billion years ago, about 99.9999999 grams of it would still be around today.<\/p>\n<p>The name bismuth is probably a latinized version of the old German word for bismuth &#8216;weissmuth&#8217; meaning &#8216;white substance&#8217;, possibly named after its white oxide.<\/p>\n<p>     <a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p>\t  <strong>Harmful effects:<\/strong> <\/p>\n<p>Bismuth is not known to be toxic. <\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\tBismuth is a crystalline, brittle, metal. Lying on the right side of the periodic table, bismuth is the most naturally diamagnetic metal; this means it resists being magnetized and is repelled by a magnetic field. One effect of this can be seen in the video (left). <\/p>\n<p>\t\tBismuth also has unusually high electrical resistance for a metal. Its thermal conductivity is lower than any metal, except <a href=\"https:\/\/www.chemicool.com\/elements\/mercury.html\">mercury<\/a>.<\/p>\n<p>\t\tBismuth has the unusual property that (like water) it expands as it freezes. Four other elements expand when they freeze: <a href=\"https:\/\/www.chemicool.com\/elements\/silicon.html\">silicon<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\">gallium<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/antimony.html\">antimony<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/germanium.html\">germanium<\/a>.<\/p>\n<p>\t\t<a id=\"uses\"><\/a><\/p>\n<h2>Uses of Bismuth<\/h2>\n<p>\t\tBismuth is used in medicine (bismuth subnitrate and subcarbonate), cosmetics (bismuth oxychloride), low-melting alloys, fire detection\/extinguishing systems, replacement for lead in shot and bullets (bismuth-<a href=\"https:\/\/www.chemicool.com\/elements\/tin.html\">tin<\/a> alloy).  <\/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>  9 parts per billion by weight, 0.7 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 10 parts per billion by weight,  0.07 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $39 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $2.83 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Commercially, bismuth is produced as a byproduct of refining copper, <a href=\"https:\/\/www.chemicool.com\/elements\/lead.html\">lead<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/tin.html\">tin<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/silver.html\">silver<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/gold.html\">gold<\/a>, and <a href=\"https:\/\/www.chemicool.com\/elements\/zinc.html\">zinc<\/a> ores.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Bismuth has 33 isotopes with mass numbers ranging from 185 to 217. Of these only <sup>209<\/sup>Bi is considered to be effectively stable, although it is actually radioactive with an extremely slow rate of alpha particle decay: its half-life is 1.9 x 10<sup>19<\/sup> years. If precisely 100 grams of <sup>209<\/sup>Bi had been present at the beginning of the universe 14 billion years ago, 99.9999999 grams of it would still be around today.<\/p>\n<div style=\"clear:both;line-height:2px;\">&nbsp;<\/div>\n<div style=\"max-width:750px;\">\n<div style=\"line-height:10px;\">\n<img decoding=\"async\" alt=\"\" src=\"\/\/www.chemicool.com\/ad.png\"\/>\n<\/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>\n<\/div>\n<p>\t\t<a id=\"refer\"><\/a><\/p>\n<h4>References<\/h4>\n<ol>\n<li>Photo by <a rel=\"nofollow\" href=\"http:\/\/commons.wikimedia.org\/wiki\/User:Micha_L._Rieser\">Micha L. Rieser<\/a><\/li>\n<\/ol>\n<p><a id=\"Cite\"><\/a><\/p>\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\/bismuth.html\"&gt;Bismuth&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/bismuth.html\"&gt;Bismuth 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\"Bismuth.\" Chemicool Periodic Table. Chemicool.com. 15 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\/bismuth.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 83 Bi 209.0 The chemical element bismuth is classed as an other metal. It was discovered in 1753 by Claude Geoffroy the Younger. Data Zone Classification: Bismuth is an &#8216;other metal&#8217; Color: silver-white Atomic weight: 208.9804 State: [&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-524","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/524","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=524"}],"version-history":[{"count":20,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/524\/revisions"}],"predecessor-version":[{"id":4206,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/524\/revisions\/4206"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=524"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}