{"id":82,"date":"2012-05-21T11:28:44","date_gmt":"2012-05-21T11:28:44","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=82"},"modified":"2017-12-07T02:07:25","modified_gmt":"2017-12-07T07:07:25","slug":"beryllium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/beryllium.html","title":{"rendered":"Beryllium 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=\"alkalieT\">\n<div class=\"atnorT\">4<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Be<\/div>\n<div class=\"atweiT\">9.012<\/div>\n<\/div>\n<p>The chemical element beryllium is classed as an an alkali earth metal. Pure beryllium was discovered in 1828 by Friederich W&#246;hler and Antoine Bussy.<\/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>  Beryllium is an alkali earth metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  steel gray  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   9.01218 <\/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>  1278 <sup>o<\/sup>C, 1551.2 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2469 <sup>o<\/sup>C, 2742 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>4<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>4<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>5<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>  2,2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   1s<sup>2<\/sup> 2s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  1.848 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69eb46ffa7a7f\"  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-id69eb46ffa7a7f\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   4.9 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hcp: hexagonal close packed <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    5.5 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  1.82 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 7.895 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 324 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    297 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 899.5 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1757.1 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   14848.7 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   0 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  0    <\/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> 2 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 1.57  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   5.6 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> vigourous, w\/ht &#8658; BeO, Be<sub>3<\/sub>N<sub>2<\/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>  mild &#8658; H<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>    mild &#8658; H<sub>2<\/sub>, [Be(OH)<sub>4<\/sub>]<sup>2<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> BeO<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   BeH<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  BeCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  112 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>   45  pm  <\/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>  200 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  25 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>  1278 <sup>o<\/sup>C, 1551.2 K    <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/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-beryllium-foils.jpg\" width=\"300\" height=\"159\" alt=\"Beryllium\" class=\"size-full\" \/><p class=\"wp-caption-text\">Beryllium Foils. Image: Deglr6328 (Ref. 6.)<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-beryllium-beryl-emerald.jpg\" width=\"300\" height=\"150\" alt=\"Beryl and Emerald\" class=\"size-full\" \/><p class=\"wp-caption-text\">Three varieties of beryl (left) and an emerald (right). Beryl and emerald&#8217;s formula is Be<sub>3<\/sub>Al<sub>2<\/sub>(SiO<sub>3<\/sub>)<sub>6<\/sub>. The different colors are caused by traces of different elements. For example, emeralds are colored by traces of chromium <sup>3+<\/sup> (blue-green) or vanadium <sup>3+<\/sup> (yellow-green) ions. <sup>(5)<\/sup> Images from Reno Chris and Jan Arkesteijn.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-berylium-oxide-xtal.jpg\" width=\"300\" height=\"262\" alt=\"Beryllium Oxide Crystal Structure\" class=\"size-full\" \/><p class=\"wp-caption-text\">The hexagonal crystal structure of BeO (beryllium oxide). Study of crystals of beryl and emerald provided a clue to the existence of the new element beryllium. Image from <a rel=\"nofollow\" href=\"http:\/\/en.wikipedia.org\/wiki\/User:Solid_State\">Solid State<\/a><\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Beryllium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    In 1798, in France, Ren&#233; Ha&#252;y saw similarities in the crystal structures and properties of beryl and emerald. Beryl can appear in a number of different colors. Emerald is green. (See images on left.)<\/p>\n<p>Ha&#252;y wondered if, despite their different colors, beryl and emerald could be made of the same elements. He approached Nicolas Louis Vauquelin, a French chemist who specialized in analysis, and asked him to have a look. <sup>(1)<\/sup><\/p>\n<p>Vauquelin discovered a new, sweet-tasting substance in both emerald and beryl. We now call this substance beryllia, BeO. Despite its sweet taste, we now know that beryllium and its compounds are highly toxic.<\/p>\n<p>Although frowned upon today, old style chemists often tasted chemicals as part of their analyses.<\/p>\n<p>For some, the taste test put their careers into terminal decline. One such chemist was Karl Scheele from Sweden, who discovered <a href=\"chlorine.html\">chlorine<\/a> and <a href=\"oxygen.html\">oxygen<\/a>. Scheele is believed to have died from poisoning caused by a variety of his experiments.<\/p>\n<p>Vauquelin proposed that beryllia contained a previously undiscovered element, an earth metal. He initially called this new element &#8216;earth of beryl.&#8217; <sup>(2)<\/sup><\/p>\n<p>The sweet taste of the salts then led to the new element being renamed &#8216;glyceynum,&#8217; then &#8216;glucina&#8217; or &#8216;glucine.&#8217; The Greek &#8216;glykis&#8217; means &#8216;sweet&#8217; and is the source of our word &#8216;glucose.&#8217; <sup>(1), (3)<\/sup><\/p>\n<p>Pure beryllium was first isolated from its salts in 1828 by Friederich W&#246;hler in Germany and, independently, Antoine Bussy in France.  <\/p>\n<p>Both chemists reacted <a href=\"https:\/\/www.chemicool.com\/elements\/potassium.html\">potassium<\/a> with beryllium chloride in a <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a> crucible yielding potassium chloride and beryllium.<\/p>\n<p>W&#246;hler was unhappy with the name the new element had been given, preferring beryllium from the Greek word &#8216;beryllos,&#8217; meaning the mineral beryl.<\/p>\n<p>W&#246;hler&#8217;s countryman, Martin Klaproth, had already pointed out in 1801 that yttria also forms sweet salts. A name derived from &#8216;beryllos&#8217; would be less likely to cause confusion than one derived from &#8216;glykis.&#8217; Klaproth also noted that a genus of plants was already called glucine.  <sup>(4)<\/sup><\/p>\n<p>Bussy, however, preferred to call the new element &#8216;glucinium.&#8217;<\/p>\n<p>Finally, in 1949, IUPAC chose beryllium as the element&#8217;s name and this decision became official in 1957. <sup>(2)<\/sup><\/p>\n<p>Beryllium played a large part in proving the existence of neutrons. In 1932, James Chadwick, an English physicist, bombarded a sample of beryllium with alpha-rays (<a href=\"helium.html\">helium<\/a> nuclei). He observed that the bombarded sample emitted a subatomic particle, which had mass but no charge.<\/p>\n<p>This neutral particle was the neutron.<\/p>\n<div style=\"clear: both; line-height: 20px;\"><\/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=\"233\" src=\"https:\/\/www.youtube.com\/embed\/Ii5GfEahbbE?rel=0&#038;start=93\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Uses of Beryllium<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-beryllium-xtal.jpg\" width=\"300\" height=\"238\" alt=\"Beryllium\" class=\"size-full\" \/><p class=\"wp-caption-text\">A large beryllium crystal of 99%+ purity. (Photo: <a rel=\"nofollow\" href=\"http:\/\/de.wikipedia.org\/wiki\/Benutzer:Alchemist-hp\">Alchemist-hp<\/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 \tBeryllium and its salts are both toxic and carcinogenic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Beryllium is light, silver-gray, relatively soft metal that is strong but brittle.<\/p>\n<p>\t\tBeryllium has the highest melting point of the light metals, melting at 1278 <sup>o<\/sup>C &#8211;  considerably higher than, for example, <a href=\"https:\/\/www.chemicool.com\/elements\/lithium.html\">Lithium<\/a> (180 <sup>o<\/sup>C) <a href=\"https:\/\/www.chemicool.com\/elements\/sodium.html\">Sodium<\/a> (98 <sup>o<\/sup>C)\t\t<a href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\">Magnesium<\/a> (650 <sup>o<\/sup>C) <a href=\"https:\/\/www.chemicool.com\/elements\/aluminum.html\">Aluminum<\/a> (660 <sup>o<\/sup>C) or <a href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\">Calcium<\/a> (839 <sup>o<\/sup>C). <\/p>\n<p> Under normal conditions, a thin layer of the hard oxide BeO forms on beryllium&#8217;s surface, protecting the metal from further attack by water or air. <\/p>\n<p>\t\tAs a result of this BeO layer, beryllium does not oxidize in air even at 600<sup>o<\/sup>C and it resists corrosion by concentrated nitric acid.<\/p>\n<p>\t\tBeryllium also has high thermal conductivity and is nonmagnetic<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Beryllium<\/h2>\n<p>\t\tUnlike most metals, beryllium is virtually transparent to x-rays and hence it is used in radiation windows for x-ray tubes.<\/p>\n<p>\t\tBeryllium alloys are used in the aerospace industry as light-weight materials for high performance aircraft, satellites and spacecraft.<\/p>\n<p>\t\tBeryllium is used as an alloy with copper to make spark-proof tools.<\/p>\n<p>\t\tBeryllium is also used in nuclear reactors as a reflector and absorber of neutrons, a shield and a moderator. <\/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>  2.8 parts per million by weight,  4.6 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  parts per billion by weight,    parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span> $748 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $93 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> The mineral beryl, Be<sub>3<\/sub>Al<sub>2<\/sub>(SiO<sub>3<\/sub>)<sub>6<\/sub> is the most important source of beryllium.<br \/>\n\t\tCommercially it is produced by the reduction of the fluoride with magnesium metal.  <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Beryllium has nine isotopes with known half-lives. <sup>9<\/sup>Be is the only stable isotope.<br \/>\n\t\t Cosmogenic <sup>10<\/sup>Be (half-life 1.51 million years) is produced in the atmosphere by the impact of cosmic rays on oxygen and nitrogen.<\/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<li>     Kenneth A. Walsh, <a href=\"http:\/\/books.google.com\/books?id=3-GbhmSfyeYC&#038;pg=PA7&#038;dq=wohler+beryllium&#038;cd=5#v=onepage&#038;q&#038;f=false\">Beryllium Chemistry and Processing<\/a>., 2009,  p7, ASM International.<\/li>\n<li>\t\t\t Mary Elvira Weeks, The Discovery of the Elements. XII., J. Chem. Educ., 1932, 9 (8), p1386 <\/li>\n<li>\t\t\t    Martin Heinrich Klaproth, <a href=\"http:\/\/books.google.com\/books?id=Ld4JAAAAIAAJ&#038;pg=RA1-PA59&#038;dq=klaproth+beryl+glucine+yttria&#038;hl=en&#038;ei=eVfSTdrND5Co8APKlJDxCg&#038;sa=X&#038;oi=book_result&#038;ct=result&#038;resnum=1&#038;ved=0CDsQ6AEwAA#v=onepage&#038;q&#038;f=false\">Analytical Essays Towards Promoting the Chemical Knowledge of Mineral Substances<\/a>., 1801, LXXVI, p59, T. Cadell, Jun. and W. Davies. <\/li>\n<li>\t\t\t      George Robert Rapp, <a href=\"http:\/\/books.google.com\/books?id=7VMVguiMmY0C&#038;pg=PA141&#038;lpg=PA141&#038;dq=Archaeomineralogy+By+George+Robert+Rapp&#038;source=bl&#038;ots=6aQQbTdoca&#038;sig=8JUgBBlMnMAUEiydFRNEr_2MhF8&#038;hl=en&#038;ei=UmDSTfmQNc22hAfJ_8yDCg&#038;sa=X&#038;oi=book_result&#038;ct=result&#038;resnum=3&#038;ved=0CCkQ6AEwAg#v=onepage&#038;q&#038;f=false\">Archaeomineralogy<\/a>., 2002,  p101, Springer. <\/li>\n<li>Image courtesy <a href=\"http:\/\/en.wikipedia.org\/wiki\/User:Deglr6328\">Deglr6328<\/a>; <a href=\"https:\/\/www.chemicool.com\/GNUFreeDocumentationLicense.html\">GNU<\/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\/beryllium.html\"&gt;Beryllium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/beryllium.html\"&gt;Beryllium 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\"Beryllium.\" 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\/beryllium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 4 Be 9.012 The chemical element beryllium is classed as an an alkali earth metal. Pure beryllium was discovered in 1828 by Friederich W&#246;hler and Antoine Bussy. Data Zone Classification: Beryllium is an alkali earth metal Color: [&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-82","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/82","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=82"}],"version-history":[{"count":55,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/82\/revisions"}],"predecessor-version":[{"id":4205,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/82\/revisions\/4205"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=82"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}