{"id":467,"date":"2012-05-26T07:13:24","date_gmt":"2012-05-26T07:13:24","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=467"},"modified":"2017-12-07T02:08:38","modified_gmt":"2017-12-07T07:08:38","slug":"rhenium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/rhenium.html","title":{"rendered":"Rhenium 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\">75<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Re<\/div>\n<div class=\"atweiT\"> 186.2<\/div>\n<\/div>\n<p>The chemical element rhenium is classed as a transition metal. It was discovered in 1925 by Walter Noddack, Ida Tacke, and Otto Berg.<\/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>  Rhenium 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>   186.207 <\/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> 3186 <sup>o<\/sup>C, 3459  K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>   5596 <sup>o<\/sup>C, 5869  K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>75<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>75<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>112<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>    2,8,18,32,13,2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>    [Xe] 4f<sup>14<\/sup> 5d<sup>5<\/sup> 6s<sup>2<\/sup>     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  21.0 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2bb2d072076\"  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-id6a2bb2d072076\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   8.85 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hcp: hexagonal close pkd  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    7.0 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> 33.20  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  776 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   715.0   kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  760 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1260 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   2510kJ 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>  -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> 7 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  4  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td>  1.9  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   9.7   &Aring;<sup>3<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> mild, w\/ht &#8658; Re<sub>2<\/sub>O<sub>7<\/sub> (rhenium heptoxide)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  mild, &#8658; HReO<sub>4<\/sub> (perrhenic acid) <\/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> ReO<sub>2<\/sub>, ReO<sub>3<\/sub>, Re<sub>2<\/sub>O<sub>3<\/sub>, Re<sub>2<\/sub>O<sub>5<\/sub>, Re<sub>2<\/sub>O<sub>7<\/sub> <\/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>   Re<sub>3<\/sub>Cl<sub>9<\/sub>, ReCl<sub>4<\/sub>, ReCl<sub>5<\/sub>, ReCl<sub>6<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  137 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> 48.0 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   5.8 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> 3186 <sup>o<\/sup>C, 3459  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-rhenium.jpg\" width=\"300\" height=\"150\" alt=\"Rhenium Metal.\" class=\"size-full\" \/><p class=\"wp-caption-text\">Rhenium Metal.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-columbite.jpg\" width=\"300\" height=\"180\" alt=\"Columbite\" class=\"size-full\" \/><p class=\"wp-caption-text\">Rhenium was first found by Walter Noddack, Ida Tacke, and Otto Berg in columbite (shown above) and platinum ores. Image from New York State Museum.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of  Rhenium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>Russian chemist Dmitri Mendeleev created the periodic table in 1869. From gaps he saw in the table, Mendeleev predicted the existence of undiscovered elements. <\/p>\n<p>He said two of the elements he had predicted would have similar properties to manganese. He called these eka-manganese, now technetium, and dvi-manganese, now rhenium.<sup> (1)<\/sup> (Sanskrit: &#8216;eka&#8217; means first and &#8216;dvi&#8217; means second.)<\/p>\n<p>Despite Mendeleev&#8217;s prediction, these elements remained undiscovered.<\/p>\n<p>Rhenium&#8217;s existence was again predicted in 1913 by English physicist Henry Moseley. <\/p>\n<p>Moseley had found that it made more sense to arrange elements in the periodic table by atomic number, not atomic weight as they had been previously. This led to gaps where undiscovered elements belonged; one of these was element 75. <\/p>\n<p>Scientists now knew an element with atomic number 75 was definitely available for discovery. Another 12 years passed before the discovery was finally made.<\/p>\n<p>In 1925, in Berlin, Germany, Walter Noddack, Ida Tacke, and Otto Berg found the new element in platinum ores and columbite. The group also announced their discovery of element 43 &#8211; now known as technetium &#8211; at the same time. They claimed to have found both elements through X-ray analysis. <\/p>\n<p>Their discoveries were disputed by many, but repeated experiments proved element 75 had indeed been discovered.<sup> (2) (3)<\/sup><\/p>\n<p>56 years had passed since Mendeleev had published his periodic table; the periodic table was now complete, at least for stable elements. Rhenium was the final element discovered which had at least one stable isotope. <\/p>\n<p>All future discoveries would be of elements with no stable isotopes; elements that would undergo radioactive decay.<\/p>\n<p>The element name comes from Latin word &#8216;Rhenus&#8217; meaning Rhine. <\/p>\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-rhenium-f15.jpg\" width=\"300\" height=\"158\" alt=\"F-15 engine constructed with second-generation superalloys containing rhenium\" class=\"size-full\" \/><p class=\"wp-caption-text\">F-15 engine constructed with second-generation superalloys containing rhenium<\/p><\/div>\n<div style=\"width:290px;\">\n<strong>The Five Refractory Metals<\/strong><br \/>\nRhenium is one of the five refractory metals &#8211; note their close neighborhood relationship in the periodic table.\n<\/div>\n<table class=\"navbar\">\n<tr>\n<td class=\"info\"><\/td>\n<td class=\"info\">Group 5<\/td>\n<td class=\"info\">Group 6<\/td>\n<td class=\"info\">Group 7<\/td>\n<\/tr>\n<tr>\n<td class=\"info\">5<\/td>\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 class=\"info\">6<\/td>\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>\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 \tThe toxicity of rhenium and its compounds is not well documented. Elemental rhenium has been described as &#8216;relatively inert&#8217; in the body.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Rhenium is a rare, silvery-white, lustrous, dense metal.<\/p>\n<p>\t\t It resists corrosion and oxidation but slowly tarnishes in moist air.<\/p>\n<p>\t\t Of the elements, only <a href=\"https:\/\/www.chemicool.com\/elements\/carbon.html\">carbon<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/tungsten.html\">tungsten<\/a> have higher melting points and only <a href=\"https:\/\/www.chemicool.com\/elements\/iridium.html\">iridium<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/osmium.html\">osmium<\/a>, and <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a> are more dense. <\/p>\n<p>\t\t Rhenium is one of the five major refractory metals (metals with very high resistance to heat and wear). <\/p>\n<p>\t\t The other refractory metals are <a href=\"https:\/\/www.chemicool.com\/elements\/tungsten.html\">tungsten<\/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\/niobium.html\">niobium<\/a>.<\/p>\n<p>\t\t Rhenium compounds include oxides, halides and sulfides.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Rhenium<\/h2>\n<p>\t\tRhenium is used with <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a> as catalysts in the production of <a href=\"https:\/\/www.chemicool.com\/elements\/lead.html\">lead<\/a>-free, high-octane gasoline. <\/p>\n<p>\t\tThe metal is used  in alloys for jet engines and in <a href=\"https:\/\/www.chemicool.com\/elements\/tungsten.html\">tungsten<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/molybdenum.html\">molybdenum<\/a> based alloys. <\/p>\n<p>\t\tIt is widely used as filaments for mass spectrographs. <\/p>\n<p>\t\tRhenium is also used as an electrical contact material.  <\/p>\n<p>\t\tRhenium catalysts are exceptionally resistant to poisoning from <a href=\"https:\/\/www.chemicool.com\/elements\/nitrogen.html\">nitrogen<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/sulfur.html\">sulfur<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/phosphorus.html\">phosphorous<\/a> and are useful in the hydrogenation of fine chemicals.<\/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>   7 parts per billion by weight,  0.8 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 100 parts per trillion by weight, 0.5 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $1600 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> Rhenium is not found free in nature but is found in small quantities in <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/molybdenum.html\">molybdenum<\/a> ores and many minerals. Commercially, rhenium is recovered as a by-product of <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a> refining.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Rhenium has 33 isotopes whose half-lives are known, with mass numbers from 160 to 192. Naturally occurring rhenium is a mixture of two isotopes, <sup>185<\/sup>Re and <sup>187<\/sup>Re, with natural abundances of 37.4% and 62.6% respectively.   <\/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> Carsten Reinhart, Chemical Sciences in the 20th Century: Bridging Boundaries, 2008, John Wiley &#038; Sons, p132<\/li>\n<li>Harry Julius Emel&eacute;us, Advances in Inorganic Chemistry and Radiochemistry, 1968, Academic Press, p3<\/li>\n<li>Loren C. Hurd, The Discovery of Rhenium, Journal of Chemical Education, October 1933, p605<\/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\/rhenium.html\"&gt;Rhenium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/rhenium.html\"&gt;Rhenium 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\"Rhenium.\" 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\/rhenium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 75 Re 186.2 The chemical element rhenium is classed as a transition metal. It was discovered in 1925 by Walter Noddack, Ida Tacke, and Otto Berg. Data Zone Classification: Rhenium is a transition 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-467","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/467","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=467"}],"version-history":[{"count":26,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/467\/revisions"}],"predecessor-version":[{"id":4291,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/467\/revisions\/4291"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=467"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}