{"id":386,"date":"2012-05-25T06:56:53","date_gmt":"2012-05-25T06:56:53","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=386"},"modified":"2017-12-07T02:08:24","modified_gmt":"2017-12-07T07:08:24","slug":"palladium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/palladium.html","title":{"rendered":"Palladium 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\">46<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Pd<\/div>\n<div class=\"atweiT\"> 106.4 <\/div>\n<\/div>\n<p>The chemical element palladium is classed as  a transition metal. It was discovered in 1803 by William H. Wollaston.<\/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>  Palladium 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>   106.4 <\/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> 1555 <sup>o<\/sup>C, 1828 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2960 <sup>o<\/sup>C, 3233 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>46<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>46<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>60<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,18  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Kr] 4d<sup>10<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  12.02 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a67b0e7ef42f\"  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-id6a67b0e7ef42f\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   8.9 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   ccp (cubic close-packed) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    4.8  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.24   J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  17.60  kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  378 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   357.0 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 804.7 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td> 1894 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   3177.2 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    53.7  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> 4 <\/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> 2.2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>  4.8 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild  w\/ht, &#8658;  PdO   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>   mild &#8658; Pd(NO<sub>3<\/sub>)<sub>2<\/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>  PdO, PdO<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   PdH<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   PdCl<sub>2<\/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> 73 pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>  78pm   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 90  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> 71.8   W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  10 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> 1555 <sup>o<\/sup>C, 1828 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-palladium.jpg\" width=\"300\" height=\"195\" alt=\"Nanoscale image of palladium metal surfac\" class=\"size-full\" \/><p class=\"wp-caption-text\">Nanoscale image of palladium metal surface. Image Ref.<sup>(1)<\/sup><\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Palladium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>Palladium was discovered in 1803, in London, by English chemist William H. Wollaston (who also discovered rhodium in the same year).<\/p>\n<p>He examined the residues left from platinum after dissolving it in aqua regia, a concentrated solution of hydrochloric and nitric acids. He then isolated palladium in a series of chemical reactions, finally heating palladium cyanide to extract palladium metal.<\/p>\n<p>Wollaston shared his discovery in an unconventional manner. He left a quantity of the metal for sale with a mineral dealer in Gerrard Street, London, and anonymously posted handbills throughout the city, describing the new metal&#8217;s properties. <\/p>\n<p>Suspicions over this uncommon method of announcement arose and Richard Chenevix, a celebrated chemist at the time, declared palladium to be a platinum-mercury alloy.  <sup>(2)<\/sup><\/p>\n<p>In response, Wollaston anonymously offered a reward of twenty guineas to anyone who could artificially produce palladium. Nobody ever claimed this money.<\/p>\n<p>In 1805, Wollaston spoke before the Royal Society of London about palladium&#8217;s properties and how it could be isolated from platinum. He finished his talk by revealing himself to be the discoverer of palladium. <\/p>\n<p>He explained that he had remained anonymous so that he would have the time to understand and explain all of the metal&#8217;s properties before putting his name to an account. <sup>(3)<\/sup><\/p>\n<p>The element is named after the then-recently discovered asteroid, Pallas. The asteroid&#8217;s name refers to the ancient Greek goddess of wisdom. <sup>(4)<\/sup><\/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:\/\/www.chemicool.com\/elements\/images\/300-metal-asteroid-impact.jpg\" width=\"300\" height=\"225\" alt=\"Asteroid brings metals\" class=\"size-full\" \/><p class=\"wp-caption-text\">It is possible that a number of Earth&#8217;s metals arrived by asteroid and comet impact after the planet had already formed, explaining why the dense metals palladium, gold and platinum are available relatively close to our planet&#8217;s surface. <a href=\"http:\/\/www.nasa.gov\/topics\/solarsystem\/features\/planet_growth_spurt.html\">Image by NASA.<\/a><\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-palladium-catalyst.jpg\" width=\"300\" height=\"376\" alt=\"Palladium Catalyzed Reaction\" class=\"size-full\" \/><p class=\"wp-caption-text\">Palladium is commonly used as a catalyst. Here it is used to catalyze the reduction of carbon dioxide to carbon monoxide. <a href=\"http:\/\/picturethis.pnl.gov\/picturet.nsf\/by+id\/DRAE-72C2Q3\">Image by PNL<\/a>.<\/p><\/div>\n<\/div>\n<\/div>\n<\/div>\n<p><a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<h3 class=\"heading\">Appearance and Characteristics<\/h3>\n<p>\t  <strong>Harmful effects:<\/strong> <\/p>\n<p>\t Palladium is considered to be of low toxicity. <\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Palladium is a rare, lustrous, silvery-white metal. <\/p>\n<p>It is one of the of the six platinum group metals consisting of platinum, palladium, rhodium, osmium, iridium and ruthenium.<\/p>\n<p><strong>The Platinum Group Metals<\/strong><br \/>\nThese metals have similar properties and are often present in the same mineral ores.<\/p>\n<table class=\"navbar\">\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/ruthenium.html\" title=\"ruthenium \"><sup>44<\/sup><br \/>Ru<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/rhodium.html\" title=\"rhodium \"><sup>45<\/sup><br \/>Rh<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/palladium.html\" title=\"palladium \"><sup>46<\/sup><br \/>Pd<\/a> <\/td>\n<\/tr>\n<tr>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/osmium.html\" title=\"osmium \"><sup>76<\/sup><br \/>Os<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/iridium.html\" title=\"iridium \"><sup>77<\/sup><br \/>Ir<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\" title=\"platinum \"><sup>78<\/sup><br \/>Pt<\/a> <\/td>\n<\/tr>\n<\/table>\n<div style=\"height:15px;\"><\/div>\n<p>\t\t Palladium is malleable and ductile and like <a href=\"https:\/\/www.chemicool.com\/elements\/gold.html\">gold<\/a>, it can be beaten into thin leaf.<\/p>\n<p>\t\t It does not tarnish in air but does tarnish lightly in moist air containing <a href=\"https:\/\/www.chemicool.com\/elements\/sulfur.html\">sulfur<\/a>.<\/p>\n<p>\t\t The metal is strongly resistant to corrosion in air and to the action of acids (except nitric acid) at ordinary temperatures.<\/p>\n<p>\t\t When present in compounds, palladium exists mostly in the oxidation state II.<\/p>\n<p>\t\t Palladium is remarkable in its capacity to absorb up to 900 times its own volume of <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a>. As it absorbs the hydrogen, it expands visibly, like a sponge swelling up when absorbing water.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of  Palladium<\/h2>\n<p>\t\tThe largest use of palladium is in catalytic converters for automobiles.<\/p>\n<p>\t\tFinely divided palladium is used as a catalyst for hydrogenation\/dehydrogenation reactions and for petroleum cracking.<\/p>\n<p>\t\tThe metal is used in jewelry, for example in white gold (an alloy of gold decolorized by the addition of palladium).<\/p>\n<p>\t\tPalladium is used in dentistry, watch making, and in making surgical instruments and electrical contacts.<\/p>\n<p>\t\tIt is also used to purify hydrogen because the gas easily diffuses through heated palladium. <\/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>   15 parts per billion by weight,  2 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  3 parts per billion by weight, 40 part per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $5833 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $1571 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span>Palladium occurs in nature as a free metal and also alloyed with <a href=\"https:\/\/www.chemicool.com\/elements\/gold.html\">gold<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/platinum.html\">platinum<\/a>, and other platinum group metals. Commercially, it is produced from <a href=\"https:\/\/www.chemicool.com\/elements\/nickel.html\">nickel<\/a>&#8211;<a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a> ore deposits where it is found in small quantities.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Palladium has 33 isotopes whose half-lives are known, with mass numbers from 94 to 120. Naturally occurring palladium is a mixture of its six stable isotopes and they are found in the percentages shown: <sup>102<\/sup>Pd (1.0%), <sup>104<\/sup>Pd (11.1%), <sup>105<\/sup>Pd (22.3%), <sup>106<\/sup>Pd (27.3%), <sup>108<\/sup>Pd (26.5%), and <sup>110<\/sup>Pd (11.7%).<\/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>Photo by <a href=\"http:\/\/www.pnl.gov\/science\/highlights\/highlight.asp?id=518\">PNNL<\/a><\/li>\n<li>Thomas Wood, The Action of Carbon on Palladium: Inaug. Diss. of the Georgia Augusta University, G\u00f6ttingen, 1859, T. Chapman Browne, p4-6<\/li>\n<li>R. Hastings, The Chemist, Volume 7, 1846, George Peirce., p388-389<\/li>\n<li>Mary Elvira Weeks, The Discovery of the Elements VIII. The Platinum Metals, Journal of Chemical Education., June 1932, p1022.<\/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\/palladium.html\"&gt;Palladium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/palladium.html\"&gt;Palladium 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\"Palladium.\" Chemicool Periodic Table. Chemicool.com. 17 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\/palladium.html&gt;.<\/pre>\n<p><script async src=\"\/\/pagead2.googlesyndication.com\/pagead\/js\/adsbygoogle.js\"><\/script><ins class=\"adsbygoogle\" style=\"display:inline-block;width:200px;height:90px\" data-ad-client=\"ca-pub-9461632227417539\" data-ad-slot=\"1328172000\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 46 Pd 106.4 The chemical element palladium is classed as a transition metal. It was discovered in 1803 by William H. Wollaston. Data Zone Classification: Palladium is a transition metal Color: silvery-white Atomic weight: 106.4 State: solid [&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-386","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/386","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=386"}],"version-history":[{"count":26,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/386\/revisions"}],"predecessor-version":[{"id":4280,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/386\/revisions\/4280"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=386"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}