{"id":438,"date":"2012-05-25T15:33:54","date_gmt":"2012-05-25T15:33:54","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=438"},"modified":"2017-12-07T02:07:25","modified_gmt":"2017-12-07T07:07:25","slug":"barium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/barium.html","title":{"rendered":"Barium 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\">56<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Ba<\/div>\n<div class=\"atweiT\">  137.3<\/div>\n<\/div>\n<p>The chemical element barium is classed as an an alkali earth metal. It was discovered in 1774 by Carl W. Scheele.<\/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>  Barium is an alkali earth 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>    137.33  <\/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> 725 <sup>o<\/sup>C,  998.2 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1897 <sup>o<\/sup>C, 2170 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>56<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>56<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>82<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>    2,8,18,18,8,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 6s<sup>2<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  3.59 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69eaa05309aba\"  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-id69eaa05309aba\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   39.24 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>    1.25 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.204 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 7.12 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  182 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    140.3 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  502.9 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   965.2 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   3600 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    14 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>  0.89  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>  39.7 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> vigorous, w\/ht &#8658;  BaO, Ba<sub>2<\/sub>N<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; Ba(NO<sub>3<\/sub>)<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td>  vigorous, &#8658; H<sub>2<\/sub>, BaCl<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>   passivated  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> BaO, BaO<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>  BaH<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   BaCl<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  215 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>  149  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>  18.4 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   2.8 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> 725 <sup>o<\/sup>C,  998.2 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-barium.jpg\" width=\"300\" height=\"165\" alt=\"Barium\" class=\"size-full\" \/><p class=\"wp-caption-text\">Barium. Photo by Matthias Zepper.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-barite.jpg\" width=\"300\" height=\"225\" alt=\"Barite\" class=\"size-full\" \/><p class=\"wp-caption-text\">Barium was first discovered in barite, also known as barium sulfate. This mineral attracted attention in the 17<sup>th<\/sup> century, when it was found to radiate red light after heating. Image from Missouri Dept. of Natural Resources.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-phosphorescent-toy.jpg\" width=\"300\" height=\"220\" alt=\"Phosphorescent Toy\" class=\"size-full\" \/><p class=\"wp-caption-text\">When Vincentius Casciorolus saw rocks that glowed in the dark, he thought he might be looking at the philosopher&#8217;s stone. Nowadays, nearly everyone has seen phosphorescent materials in action. Image by Luu Ly.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Barium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>In the early 1600s, Vincentius Casciorolus, a shoemaker with an interest in alchemy, was excited.  He had learned there was a heavy, silvery-white mineral with remarkable properties in the mountains near Bologna, Italy. Perhaps, he thought, it might even be the philosopher&#8217;s stone.<\/p>\n<p>When the mineral was heated and combusted, its product emitted a phosphorescent red glow &#8211; very neat. But what really excited Casciorolus &#8211; and others &#8211; was that if the combusted material was exposed to sunshine, it would glow in the dark for up to an hour afterwards.<\/p>\n<p>We now know that the silvery white mineral was impure barium sulfate, BaSO<sub>4<\/sub>. After heating, it became impure barium sulfide, BaS. <sup>(1), (2), (3), (4)<\/sup><\/p>\n<p>Sadly for Casciorolus, although this material&#8217;s properties were interesting, it proved useless as a means of making gold from other metals and failed to make him immortal. Rather than &#8216;philosopher&#8217;s stone&#8217; it became known as &#8216;Bologna stone&#8217; &#8211; a curiosity. <\/p>\n<p>Sadly, also, no-one took the opportunity to discover the new element present in Bologna stone. Of course, at the time, nobody suspected there were any new elements to be discovered!<\/p>\n<p>About 170 years passed before barium was first recognized as a new element by Swedish scientist Carl W. Scheele. Investigating magnesium oxide in 1774, Scheele found a new earth metal: &#8220;an earth differing from all earths hithero known.&#8221; He called this new metal &#8216;terra ponderosa.&#8217; (Latin: heavy earth.) <\/p>\n<p>A comparison was made with Bologna stone, and the two were found to contain the same substance. (Until this point, people had thought Bologna stone was a compound of <a href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\">calcium<\/a>. <sup> (2)<\/sup>)<\/p>\n<p>Barium metal was isolated for the first time in 1808 by English chemist Sir Humphrey Davy in London. Davy followed the advice of Swedish chemist Jacob Berzelius, who had told him that barium sulfate could be decomposed by electrolysis. This was correct, and Davy isolated strontium in a similar way. The experimental details are on our <a href=\"https:\/\/www.chemicool.com\/elements\/strontium.html\">strontium<\/a> page.<\/p>\n<p>The element was called barium because it was found in barite (barium sulfate) a mineral given its name because of its high density. The Greek &#8216;barys&#8217; means heavy. \t<\/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><strong>Barium&#8217;s Periodic Table Neighborhood<\/strong><\/p>\n<table class=\"navbar\">\n<tr>\n<td class=\"info\"><\/td>\n<td class=\"info\">Group 1<\/td>\n<td class=\"info\">Group 2<\/td>\n<td class=\"info\">Group 3<\/td>\n<\/tr>\n<tr>\n<td class=\"info\">5<\/td>\n<td><a class=\"alkali\" href=\"https:\/\/www.chemicool.com\/elements\/rubidium.html\" title=\"rubidium \"><sup>37<\/sup><br \/>Rb<\/a> <\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/strontium.html\" title=\"strontium \"><sup>38<\/sup><br \/>Sr<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/yttrium.html\" title=\"yttrium \"><sup>39<\/sup><br \/>Y<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">6<\/td>\n<td><a class=\"alkali-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/cesium.html\" title=\"cesium \"><sup>55<\/sup><br \/>Cs<\/a> <\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/barium.html\" title=\"barium \"><sup>56<\/sup><br \/>Ba<\/a> <\/td>\n<td><a class=\"actlan\"  href=\"https:\/\/www.chemicool.com\/elements\/lanthanum.html\" title=\"lanthanum\"><sup>57<\/sup><br \/>La<\/a><\/td>\n<\/tr>\n<tr>\n<td class=\"info\">7<\/td>\n<td><a class=\"alkali-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/francium.html\" title=\"francium \"><sup>87<\/sup><br \/>Fr<\/a> <\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/radium.html\" title=\"radium \"><sup>88<\/sup><br \/>Ra<\/a> <\/td>\n<td><a class=\"actlan\"  href=\"https:\/\/www.chemicool.com\/elements\/actinium.html\" title=\"actinium\"><sup>89<\/sup><br \/>Ac<\/a><\/td>\n<\/tr>\n<\/table>\n<div style=\"font-size:0.8em; text-align:center;width:290px\">\nBarium sits close to the bottom of the periodic table&#8217;s Group 2. It is Group 2&#8217;s final stable element. Radium, which follows, is radioactive. Group 2 elements are sufficiently reactive that the free metals are never found naturally; they are, however, much less reactive that Group 1 metals. In general, reactivity increases as one looks down Group 2; so barium is more reactive than strontium and calcium, for example.\n<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/5QhBvXsJ53E?rel=0\" allowfullscreen><\/iframe><\/p>\n<div style=\"width: 290px; font-size: 12px; font-weight: bold; text-align: center; padding-bottom: 10px; position: relative; top: -16px;\">Barium is used in medicine to detect abnormalities in the digestive system.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/MyAzjSdc3Fc?rel=0\" allowfullscreen><\/iframe><\/p>\n<div style=\"width: 290px; font-size: 12px; font-weight: bold; text-align: center; padding-bottom: 10px; position: relative; top: -16px;\">The reaction between ammonium thiocyanate and barium hydroxide octahydrate is endothermic. As a result, the temperature will drop quickly. This causes the beaker to freeze to the wooden board.<\/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 Barium compounds that are water or acid soluble are highly poisonous. Barium powder can ignite spontaneously in air.<\/p>\n<p>\tBarium sulfate, used in x-ray imaging, is highly insoluble in water, and is therefore nontoxic and completely removed from the digestive tract.<\/p>\n<p>\t\t<strong>Characteristics:<\/strong><\/p>\n<p>\t\t Barium is a metallic element chemically resembling calcium but more reactive. It is a soft, silvery metal and when cut it quickly turns a black color due to the formation of barium oxide, (BaO).<\/p>\n<p>It is also highly reactive with water or alcohol.<\/p>\n<p>When present in compounds barium exists usually in the Ba<sup>2+<\/sup>, divalent state.<\/p>\n<p>Barium dissolves in most aqueous acids. The exception is sulfuric acid, due to the formation of an insoluble protective layer of barium sulfate. <\/p>\n<p>\t\tBarium is most commonly found as the mineral barite (BaSO<sub>4<\/sub>) and witherite (BaCO<sub>3<\/sub>) <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Barium<\/h2>\n<p>Barium is used as a &#8220;flashed getter&#8221; in vacuum tubes to remove the last traces of gases.<\/p>\n<p>\t\tBarium is an important element in yttrium barium copper oxide (YBCO) superconductors.<\/p>\n<p>\t\tAn alloy of barium with nickel is used in sparkplug wire. <\/p>\n<p>\t\tBarium sulfate (barite) is used to increase the contrast in x-ray imaging of the digestive system.<\/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>  425 parts per million by weight,  41 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>  $55 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> Commercially obtained from the electrolysis of molten Barium Chloride, BaCl<sub>2<\/sub><\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span>  Barium has 37 isotopes.  Naturally occurring barium is a mixture of seven stable isotopes and they are found in the percentages shown:<br \/>\n\t\t <sup>138<\/sup>Ba (71.7%), <sup>137<\/sup>Ba (11.2%), <sup>136<\/sup>Ba (7.9%), <sup>135<\/sup>Ba (6.6%), <sup>134<\/sup>Ba (2.4%), <sup>130<\/sup>Ba (0.1%) and <sup>132<\/sup>Ba (0.1%). <\/p>\n<p>\t\t Of the radioactive isotopes, <sup>133<\/sup>Ba is the longest lived with a half-life of 10.51 years.<\/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>Mary Elvira Weeks, The Discovery of the Elements. X. The Alkaline Earth Metals and Magnesium and Cadmiun, Journal of Chemical Education., June 1932, p1050.<\/li>\n<li>J.W. Mellor, A Comprehensive Treatise on Inorganic and Theoretical Chemistry, Volume III, 1928, Longmans, Green and Co. Ltd, p619-621<\/li>\n<li>Thomas Lamb Phipson, Phosphorescence: or, The emission of light by minerals, plants, and animals., L. Reeve &amp; co., 1862, p12.<\/li>\n<li>James L. Marshall and Virginia R. Marshall, Rediscovery of The Elements Phosphoro di Bologna., University of North Texas., p1.<\/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\/barium.html\"&gt;Barium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/barium.html\"&gt;Barium 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\"Barium.\" 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\/barium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 56 Ba 137.3 The chemical element barium is classed as an an alkali earth metal. It was discovered in 1774 by Carl W. Scheele. Data Zone Classification: Barium is an alkali earth metal Color: silvery white Atomic [&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-438","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/438","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=438"}],"version-history":[{"count":24,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/438\/revisions"}],"predecessor-version":[{"id":4439,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/438\/revisions\/4439"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=438"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}