{"id":541,"date":"2012-05-30T08:26:44","date_gmt":"2012-05-30T08:26:44","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=541"},"modified":"2018-12-14T11:23:58","modified_gmt":"2018-12-14T16:23:58","slug":"astatine","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/astatine.html","title":{"rendered":"Astatine 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=\"halogensT\">\n<div class=\"atnorT\">85<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">At<\/div>\n<div class=\"atweiT\"> (210)<\/div>\n<\/div>\n<p>The chemical element astatine is classed as a halogen and a nonmetal. It was discovered in 1940 by Dale R. Coson, Kenneth Ross Mackenzie and Emilio Segr&#232;.<\/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>  Astatine is a halogen and a nonmetal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td> Presumed very dark <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   (210), no stable isotopes<\/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> 302 <sup>o<\/sup>C, 575.2 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  337 <sup>o<\/sup>C,  610 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>85<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>85<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>125<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,32,18,7     <\/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>5<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  7 g\/cm<sup>3<\/sup> approx.   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69e0e00ebb3de\"  tabindex=\"0\" title=\"Show more, including: Heats, Energies, Oxidation, Reactions, Compounds, Radii, Conductivities\"    >Show more, including: Heats, Energies, Oxidation, Reactions, Compounds, Radii, Conductivities<\/span><div id=\"target-id69e0e00ebb3de\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>  30 cm<sup>3<\/sup>\/mol approx.  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   unknown <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 6 kJ mol<sup>-1<\/sup> of I<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  92 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  40 kJ mol<sup>-1<\/sup> of I<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  890 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  &#8211;    <\/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>   270 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>  -1   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Maximum oxidation number <\/td>\n<td> 7 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  1  <\/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>    6 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td> &#8211; <\/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> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   HAt  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/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\"> 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> 1.7 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Freezing\/Melting point:<\/td>\n<td> 302 <sup>o<\/sup>C, 575.2 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:\/\/www.chemicool.com\/elements\/images\/300-nickel-5g.jpg\" width=\"300\" height=\"300\" alt=\"5g Coin\"  class=\"size-full\" \/><p class=\"wp-caption-text\">The amount of naturally occurring astatine in the world is about 25g. That&#8217;s the weight of five U.S. nickels.<\/p><\/div>\n<p><strong>Astatine&#8217;s Periodic Table<br \/> Neighborhood<\/strong><\/p>\n<table class=\"navbar\">\n<tr>\n<td class=\"info\"><\/td>\n<td class=\"info\">Group 16<\/td>\n<td class=\"info\">Group 17<\/td>\n<td class=\"info\">Group 18<\/td>\n<\/tr>\n<tr>\n<td class=\"info\">4<\/td>\n<td><a class=\"onm\" href=\"https:\/\/www.chemicool.com\/elements\/selenium.html\" title=\"selenium\"><sup>34<\/sup><br \/>Se<\/a> <\/td>\n<td><a class=\"halogens-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/bromine.html\" title=\"bromine\"><sup>35<\/sup><br \/>Br<\/a> <\/td>\n<td><a class=\"ngases\" href=\"https:\/\/www.chemicool.com\/elements\/krypton.html\" title=\"krypton\"><sup>36<\/sup><br \/>Kr<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">5<\/td>\n<td><a class=\"metalloid\"  href=\"https:\/\/www.chemicool.com\/elements\/tellurium.html\" title=\"tellurium\"><sup>52<\/sup><br \/>Te<\/a> <\/td>\n<td><a class=\"halogens\" href=\"https:\/\/www.chemicool.com\/elements\/iodine.html\" title=\"iodine\"><sup>53<\/sup><br \/>I<\/a> <\/td>\n<td><a class=\"ngases\" href=\"https:\/\/www.chemicool.com\/elements\/xenon.html\" title=\"xenon\"><sup>54<\/sup><br \/>Xe<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">6<\/td>\n<td><a class=\"metalloid\" href=\"https:\/\/www.chemicool.com\/elements\/polonium.html\" title=\"polonium\"><sup>84<\/sup><br \/>Po<\/a> <\/td>\n<td><a class=\"halogens\" href=\"https:\/\/www.chemicool.com\/elements\/astatine.html\" title=\"astatine\"><sup>85<\/sup><br \/>At<\/a> <\/td>\n<td><a class=\"ngases\" href=\"https:\/\/www.chemicool.com\/elements\/radon.html\" title=\"radon\"><sup>86<\/sup><br \/>Rn<\/a> <\/td>\n<\/tr>\n<\/table>\n<div style=\"font-size:0.8em; text-align:center;width:290px\">\nLike the other halogens, astatine  is a nonmetal, although it shows more metallic character in its chemistry than the others. Astatine and the elements on either side of it, <a href=\"https:\/\/www.chemicool.com\/elements\/polonium.html\">polonium<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/radon.html\">radon<\/a>, have no stable isotopes. Too little astatine has ever been present in one place for anyone to actually see it &#8211; in fact, since astatine&#8217;s boiling point is just 337 &deg;C, any visible quantity of it would be instantly vaporized by the energy released by its rapid radioactive decay.\n<\/div>\n<\/div>\n<\/div>\n<p>\t\t\t<a id=\"discovery\"><\/a>\t<\/p>\n<h2>Discovery of Astatine<\/h2>\n<div class=\"author\">Author: Dr. Doug Stewart<\/div>\n<p>The first periodic table, produced by Russian chemist Dmitri Mendeleev in 1869, had a space directly underneath iodine. The element to fill this space became known as eka-iodine. This alerted scientists to the possibility that if they looked, they could find the element that would fit into this space. <\/p>\n<p>Many tried to find the new element in nature, but without success.<\/p>\n<p>71 years after Mendeleev published his first periodic table, the element had still not been found, but was instead synthesized in the laboratory using one of the earliest particle accelerators.<\/p>\n<p>Astatine was first produced in 1940 by Dale R. Coson, Kenneth Ross Mackenzie and Emilio Segr&#232; at the University of California, Berkeley. <\/p>\n<p>Segr&#232;, working with Carlo Perrier, had previously synthesized technetium in 1937.<sup>(2), (3)<\/sup><\/p>\n<p>Astatine was made by bombarding bismuth-209 with alpha particles in a cyclotron (particle accelerator) to produce, after emission of two neutrons, astatine-211. The scientists found that the isotope they created was radioactive, so they named the element using the Greek &#8216;astatos&#8217; meaning unstable. <\/p>\n<p>It is now known that there are no stable astatine isotopes &#8211; the longest lived isotope, astatine-210, has a half-life of 8.3 hours.<sup> (3)<\/sup><\/p>\n<p>Three years later, astatine was found in nature by Berta Karlik and Traude Bernert as an intermediate in radioactive decay chains. Traces of the element appear naturally in uranium and thorium minerals as a decay product. <\/p>\n<p>At any given time, about 25 grams of naturally occurring astatine exists on our planet.<sup> (3), (4)<\/sup><\/p>\n<p>     <a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p><strong>Harmful effects:<\/strong> <\/p>\n<p>\t \tHighly radioactive<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>    Astatine is highly radioactive and is only available in tiny quantities. Its properties are inferred from its position in the periodic table and by studying its chemistry in extremely dilute solutions.<\/p>\n<p>\t\tLike the other halogens, astatine would be expected to form salts with metals such as <a href=\"https:\/\/www.chemicool.com\/elements\/sodium.html\">sodium<\/a>. Astatine can also react with <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> to form hydrogen astatide, which when dissolved in water, forms hydroastatic acid.  <\/p>\n<p>\t\tAstatine is the least chemically reactive of the halogens and exhibits the most metallic properties of the halogen group.<\/p>\n<p>\t\t<a id=\"uses\"><\/a><\/p>\n<h2>Uses of Astatine<\/h2>\n<p>\tAstatine-211 is sometimes used as a radioactive tracer and in cancer treatment.<\/p>\n<p>\t\tLike <a href=\"https:\/\/www.chemicool.com\/elements\/iodine.html\">iodine<\/a>, it is known to accumulate in the thyroid gland. <\/p>\n<p><a id=\"abund\"><\/a><\/p>\n<h2>Abundance and Isotopes<\/h2>\n<p><span class=\"elemgl\">Abundance arth&#8217;s crust:<\/span>  About 25 grams exists in Earth&#8217;s crust at any given time. <\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> negligible<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $ per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>   $ per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Astatine is produced synthetically by bombarding bismuth with alpha particles.  It can be obtained naturally from thorium or uranium decay.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> More than 30 isotopes of astatine have been identified.  All are very short-lived; astatine-210 has the longest half-life of 8 hours 10 minutes.<\/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>Image: <a rel=\"nofollow\" href=\"http:\/\/commons.wikimedia.org\/wiki\/User:Inductiveload\">Inductiveload<\/a><\/li>\n<li>Gurdeep Raj, Advanced Inorganic Chemistry Vol-I, 1998, Krishna Prakashan Media, p344<\/li>\n<li>Egon Wiberg, A.F. Holleman, Nils Wiberg, Inorganic Chemistry, 2001, Academic Press, p423<\/li>\n<li>B.K. Sharma, Nuclear and Radiation Chemistry, 1997, Krishna Prakashan Media, p147<\/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\/astatine.html\"&gt;Astatine&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/astatine.html\"&gt;Astatine 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\"Astatine.\" 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\/astatine.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 85 At (210) The chemical element astatine is classed as a halogen and a nonmetal. It was discovered in 1940 by Dale R. Coson, Kenneth Ross Mackenzie and Emilio Segr&#232;. Data Zone Classification: Astatine is a halogen [&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-541","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/541","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=541"}],"version-history":[{"count":26,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/541\/revisions"}],"predecessor-version":[{"id":4661,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/541\/revisions\/4661"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=541"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}