{"id":718,"date":"2012-06-02T10:30:51","date_gmt":"2012-06-02T10:30:51","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=718"},"modified":"2017-12-07T02:07:40","modified_gmt":"2017-12-07T07:07:40","slug":"erbium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/erbium.html","title":{"rendered":"Erbium Element Facts \/ Chemistry"},"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=\"rareT\">\n<div class=\"atnorT\">68<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Er<\/div>\n<div class=\"atweiT\"> 167.3<\/div>\n<\/div>\n<p>The chemical element erbium is classed as a lanthanide and rare earth metal. It was discovered in 1843 by Carl Gustaf Mosander. <\/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>  Erbium is a lanthanide and rare 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>  167.26 <\/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> 1530 <sup>o<\/sup>C, 1803 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>   2860 <sup>o<\/sup>C, 3133  K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>68<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>68<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>98<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,30,8,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Xe] 4f<sup>12<\/sup> 6s<sup>2<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>   9.05 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2409963be55\"  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-id6a2409963be55\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   18.4  cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>  hexagonal close packed  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>      <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.17 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  19.90  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  317 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  292.88   kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  588.7  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1151   kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2194    kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>  &#8211; <\/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> 3 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  3  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td>   1.24    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   22.7    &Aring;<sup>3<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild,  &#8658;  Er<sub>2<\/sub>O<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; Er(NO<sub>3<\/sub>)<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td>  mild, &#8658;  H<sub>2<\/sub>, ErCl<sub>3<\/sub>  <\/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>  Er<sub>2<\/sub>O<sub>3<\/sub> (erbia) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   ErH<sub>2<\/sub>, ErH<sub>3<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   ErCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  175 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>  103 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> 14.5   W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   1.2 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> 1530 <sup>o<\/sup>C, 1803 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-erbium.jpg\" width=\"300\" height=\"162\" alt=\"Erbium metal\" class=\"size-full\" \/><p class=\"wp-caption-text\">Erbium metal. Photo by Tomihahndorf.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-dysprosium.jpg\" width=\"300\" height=\"176\" alt=\"Rare-earth refining\" class=\"size-full\" \/><p class=\"wp-caption-text\">Getting high purity research-quality rare-earth metals takes time. First rare earth oxides, like the yellow (cerium), black (praseodymium) and blue (neodymium) oxides in the dishes are exposed to the highly reactive gas hydrogen fluoride. This turns the powder into a fluoride, such as the bright green praseodymium fluoride crystals (far right). A reduction reaction and further processing turns the rare-earth fluorides into their pure metal forms, (from top center) scandium disc, dysprosium disc resting on a sheet of sublimated dysprosium and gadolinium cylinder. Photo: <a href=\"https:\/\/www.ameslab.gov\/news\/inquiry\/2010-2-root\">Ames Laboratory <\/a>.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Erbium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Erbium was discovered in 1843 by the Swedish chemist Carl Gustaf Mosander. <\/p>\n<p>Four years earlier Mosander had discovered <a href=\"https:\/\/www.chemicool.com\/elements\/lanthanum.html\">lanthanum<\/a>. His former supervisor, Jacob Berzelius, had discovered the new element <a href=\"https:\/\/www.chemicool.com\/elements\/cerium.html\">cerium<\/a> in cerite. Mosander continued to study cerite and was rewarded with the discovery of lanthanum. <sup>(1)<\/sup><\/p>\n<p>In 1843, Mosander began studying the mineral gadolinite. Gadolinite contained yttria (yttrium oxide) in which Johan Gadolin had discovered the element yttrium in 1794. Mosander wondered if he might repeat his earlier triumph and find another new element hiding with a known element.<\/p>\n<p>Using ammonium hydroxide he precipitated fractions of different basicity from yttria. In these fractions he found two differently colored, previously unknown substances. These he called erbia and terbia; they contained the new rare earth metals erbium and <a href=\"terbium.html\">terbium<\/a>. Mosander had now discovered three new elements, all rare earths, and all in minerals other scientists had discarded after making their own discoveries. <sup>(2), (3), (4)<\/sup><\/p>\n<p>Mosander named <a href=\"https:\/\/www.chemicool.com\/elements\/erbium.html\">erbium<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/terbium.html\">terbium<\/a> after the Ytterby Mine in Sweden, the source of gadolinite mineral they were discovered in. (The elements <a href=\"https:\/\/www.chemicool.com\/elements\/yttrium.html\">yttrium<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/ytterbium.html\">ytterbium<\/a> were also named after the same mine.)<\/p>\n<p>The identities (and even the existence) of a number of rare earth elements was settled finally by George Urbain in Paris, who carried out tens of thousands of fractional crystallizations of rare earth salts.<\/p>\n<p>Crystallizations could take years to produce small samples of pure salts.<\/p>\n<p>Urbain finally put to rest uncertainty about the identities of pure earths whose salts had never before been completely free of other rare earth salts.<\/p>\n<p>Urbain found there were fifteen rare earth metals &#8211; we now recognize seventeen &#8211; one of which was erbium. In the process, he discovered the rare earth <a href=\"https:\/\/www.chemicool.com\/elements\/lutetium.html \">lutetium<\/a>, adding his own name to the list of scientists who have discovered elements. <sup>(5), (6), (7), (8), (9)<\/sup><\/p>\n<p>Metallic erbium was not isolated until 1935 by W. Klemm and H. Bommer who reduced its anhydrous chloride with potassium vapor. <sup>(10)<\/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-erbium-slow.jpg\" width=\"300\" height=\"225\" alt=\"Erbium atoms\" class=\"size-full\" \/><p class=\"wp-caption-text\">A purple laser beam slows erbium atoms emerging from an oven at 1300<sup>o<\/sup>C, in preparation for trapping and cooling. The unusual properties of erbium atoms and the new capability to trap them could lead to development of novel technologies. Photo: <a href=\"http:\/\/www.nist.gov\/public_affairs\/techbeat\/tb2006_0428.htm\">NIST<\/a><\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/IFmAhhiam9g?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A brief introduction to the lanthanides.<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p><a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p>\t  <strong>Harmful effects:<\/strong> <\/p>\n<p>\t \tErbium is considered to be moderately toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Erbium is a bright, soft, malleable, silvery-white metal.<\/p>\n<p>\t\tIt is one of the rare earth metals.<\/p>\n<p>\t\tThe metal slowly tarnishes in air, reacts slowly with water and dissolves in acids.<\/p>\n<p>\t\tWhen present in compounds, erbium exists mostly in the trivalent state, Er<sup>3+<\/sup>. Erbium salts are a rose pink color.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Erbium<\/h2>\n<p>\t\tErbium isotopes are good neutron absorbers and are used in nuclear reactor control rods.<\/p>\n<p>\t\tThe oxide erbia is used as a pink coloring agent in glazes and glasses.<\/p>\n<p>\t\tErbium is used in alloys especially with vanadium to decrease the hardness of metals.<\/p>\n<p>\t\tIt is also used in amplifiers and lasers.<\/p>\n<p>\t\tErbium is used in photographic filters to absorb infrared light.<\/p>\n<p>\t\tErbium is also used in yttrium aluminum garnet (YAG) medical lasers for procedures involving skin resurfacing such as acne scars, mole removal tattoo removal and warts.<\/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> 3 parts per million by weight, 0.4 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  1 part per billion by weight,  10 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $540 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $65  per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> <\/p>\n<p>\t\tErbium  is not found free in nature but is found in a number of minerals: mainly monazite, bastnasite, xenotime and euxenite. Commercially it is refined from xenotime and euxenite using a complex ion-exchange process. Erbium is then isolated from the oxide or its salts by heating at 1450 <sup>o<\/sup>C with calcium in an argon atmosphere.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Erbium has 31 isotopes whose half-lives are known, with mass numbers 145 to 175. Naturally occurring erbium is a mixture of six isotopes and they are found in the percentages shown: <sup>162<\/sup>Er (0.1%), <sup>164<\/sup>Er (1.6%), <sup>166<\/sup>Er (33.6%), <sup>167<\/sup>Er (22.9%), <sup>168<\/sup>Er (26.8%) and <sup>170<\/sup>Er (14.9%). The most abundant isotope is <sup>166<\/sup>Er at 33.6%.<\/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=U8M-AAAAYAAJ&#038;pg=PA390\">Latanium, a New Metal<\/a>.,  The London and Edinburgh Philosophical Magazine and Journal of Science, 1839, 14, p3901.<\/li>\n<li>Mary Elvira Weeks, The discovery of the elements. XVI. The rare earth elements., J. Chem. Educ., 1932, p1751.<\/li>\n<li>Per Enghag, <a href=\"http:\/\/books.google.com\/books?id=aff7sEea39EC\">Encyclopedia of the elements: technical data, history, processing, applications<\/a>., John Wiley and Sons, 2004, p447.<\/li>\n<li>Paul Caro, Rare earths., Editorial Complutense., 1998, p35. <\/li>\n<li>Georges Champetier and Charlotte H. Boatner, Georges Urbain., 1940, J. Chem. Educ., p103.<\/li>\n<li>G. Eberhard, A Spectroscopic Investigation of Dr. Urbain&#8217;s Preparations of Terbium., Astrophysical Journal., 1906 vol. 24, p309.<\/li>\n<li>Ralph P. Oesper, \tGeorges Urbain., 1938, J. Chem. Educ., p201.<\/li>\n<li>G. Urbain, On a yttria earth neighboring gadolinium. Comptes Rendus, 1904, 139, p736.<\/li>\n<li>G. Urbain, On the isolation of terbium., Comptes Rendus, 1905, 141, p521.<\/li>\n<li>Charles T. Lynch, CRC handbook of materials science., CRC Press, 1974, p.17.<\/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\/erbium.html\"&gt;Erbium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/erbium.html\"&gt;Erbium 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\"Erbium.\" Chemicool Periodic Table. Chemicool.com. 05 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\/erbium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 68 Er 167.3 The chemical element erbium is classed as a lanthanide and rare earth metal. It was discovered in 1843 by Carl Gustaf Mosander. Data Zone Classification: Erbium is a lanthanide and rare 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-718","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/718","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=718"}],"version-history":[{"count":25,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/718\/revisions"}],"predecessor-version":[{"id":4403,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/718\/revisions\/4403"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=718"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}