{"id":401,"date":"2012-05-25T10:09:33","date_gmt":"2012-05-25T10:09:33","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=401"},"modified":"2017-12-07T02:08:08","modified_gmt":"2017-12-07T07:08:08","slug":"indium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/indium.html","title":{"rendered":"Indium 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=\"ometalsT\">\n<div class=\"atnorT\">49<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">In<\/div>\n<div class=\"atweiT\">114.8<\/div>\n<\/div>\n<p>The chemical element indium is classed as an <em>other metal<\/em>. It was discovered in 1863 by Ferdinand Reich.<\/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>  Indium is an &#8216;other metal&#8217;  <\/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>   114.82 <\/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> 156.6 <sup>o<\/sup>C, 429.8 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td> 2070 <sup>o<\/sup>C, 2343 K      <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>49<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>49<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>66<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,18,3    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>  [Kr] 4d<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sup>1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td> 7.31 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id69e3265e3b838\"  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-id69e3265e3b838\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   15.7 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   tetragonal, distorted fcc structure <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>   1.2 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.23 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 3.263 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 244 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   231.50 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  558.3  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1820.6 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   2704.5 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    39  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> 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> 1.78  <\/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;  In<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; In(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>,  InCl<sub>3<\/sub>  <\/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>  InO, In<sub>2<\/sub>O<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   InH  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  InCl, InCl<sub>2<\/sub>, InCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  155 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>  94  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> 81.8  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  3.4 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> 156.6 <sup>o<\/sup>C, 429.8 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-indium-bar.jpg\" width=\"300\" height=\"160\" alt=\"A bar of indium metal and a penny.\" class=\"size-full\" \/><p class=\"wp-caption-text\">A bar of indium metal and a penny.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Indium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>In 1863, Ferdinand Reich discovered indium in Germany. He had intended to investigate whether zinc sulfide ore (sphalerite) also contained <a href=\"https:\/\/www.chemicool.com\/elements\/thallium.html\">thallium<\/a>. Instead, as a result of his careful observations, he became the discoverer of a new element. <sup>(1)<\/sup> <\/p>\n<p>After roasting the ore to remove most of the <a href=\"https:\/\/www.chemicool.com\/elements\/sulfur.html\">sulfur<\/a>, he decomposed the remaining material with hydrochloric acid. <\/p>\n<p>He saw a straw colored solid appear.  Reich began to suspect that this straw colored precipitate might be the sulfide of a new element. <sup>(2)<\/sup> <\/p>\n<p>He investigated this further by getting an emission spectrum for the sample. Unfortunately for Reich, his color-blindness prevented him from accurately interpreting this for himself. <\/p>\n<p>He asked his countryman, German chemist Hieronymus T. Richter, to look at the flame colors produced. Richter observed a brilliant indigo line, which did not match the spectral line of any known element. <sup>(3)<\/sup>  <\/p>\n<p>This line enabled Reich and Richter to show that a new element was present in their sample.<\/p>\n<p>The men later isolated the metal by a lengthy series of precipitations and made a thorough study of its properties. The yield of indium was 0.1% from the original zinc sulfide ore. <sup>(1)<\/sup>  <\/p>\n<p>The element was named after its characteristic spectral line &#8211; the &#8216;indi&#8217; coming from the color indigo.<\/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-indium.jpg\" width=\"300\" height=\"139\" alt=\"Indium\" class=\"size-full\" \/><p class=\"wp-caption-text\">Indium in a test tube. Photo by Schtone.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-indium-led.jpg\" width=\"300\" height=\"243\" alt=\"pop\" class=\"size-full\" \/><p class=\"wp-caption-text\">When indium is added to gallium nitride in LEDs, violet, blue and green colors can be produced. Image by <a href=\"http:\/\/www.lbl.gov\/Science-Articles\/Archive\/MSD-perfect-solar-cell-2.html\">LBL<\/a><\/p><\/div>\n<p><strong>Indium&#8217;s Periodic Table Neighborhood<\/strong><\/p>\n<table class=\"navbar\">\n<tr>\n<td class=\"info\"><\/td>\n<td class=\"info\">Group 12<\/td>\n<td class=\"info\">Group 13<\/td>\n<td class=\"info\">Group 14<\/td>\n<\/tr>\n<tr>\n<td class=\"info\">Row 4<\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/zinc.html\" title=\"zinc \"><sup>30<\/sup><br \/>Zn<\/a> <\/td>\n<td><a class=\"ometals-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\" title=\"gallium \"><sup>31<\/sup><br \/>Ga<\/a> <\/td>\n<td><a class=\"metalloid\"  href=\"https:\/\/www.chemicool.com\/elements\/germanium.html\" title=\"germanium \"><sup>32<\/sup><br \/>Ge<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">Row 5<\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/cadmium.html\" title=\"cadmium \"><sup>48<\/sup><br \/>Cd<\/a> <\/td>\n<td><a class=\"ometals\" href=\"https:\/\/www.chemicool.com\/elements\/indium.html\" title=\"indium \"><sup>49<\/sup><br \/>In<\/a> <\/td>\n<td><a class=\"ometals\" href=\"https:\/\/www.chemicool.com\/elements\/tin.html\" title=\"tin \"><sup>50<\/sup><br \/>Sn<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">Row 6<\/td>\n<td><a class=\"tmetals-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/mercury.html\" title=\"mercury \"><sup>80<\/sup><br \/>Hg<\/a> <\/td>\n<td><a class=\"ometals\" href=\"https:\/\/www.chemicool.com\/elements\/thallium.html\" title=\"thallium \"><sup>81<\/sup><br \/>Tl<\/a> <\/td>\n<td><a class=\"ometals\" href=\"https:\/\/www.chemicool.com\/elements\/lead.html\" title=\"lead \"><sup>82<\/sup><br \/>Pb<\/a> <\/td>\n<\/tr>\n<\/table>\n<div style=\"font: 500 13px\/17px Arial,Helvetica,sans-serif;text-align:center;padding-bottom:10px;width: 290px;\">Indium sits in Group 13, Row 5 of the periodic table. Its neighborhood contains a number of low-melting point metals.<\/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 \tIndium is considered to be of low toxicity.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Indium is a very soft, silvery-white lustrous metal. <\/p>\n<p>\t\tIndium liquid clings to or wets glass and similar surfaces. <\/p>\n<p>\t\tLike <a href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\">gallium<\/a>, indium remains in a liquid state over a wide range of temperatures.<\/p>\n<p>When present in compounds, indium exists mostly in the oxidation state III.  <\/p>\n<p>\t\tWhen heated above its melting point, it burns with a violet flame to the yellow sesquioxide (In<sub>2<\/sub>O<sub>3<\/sub>).<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Indium<\/h2>\n<p>\t\tIndium is used in the production of low-melting alloys, typically with <a href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\">gallium<\/a>.<\/p>\n<p>\t\tThe melting point depends on the ratio of indium to gallium.<\/p>\n<p>\t\tAn alloy with 24% indium and 76% gallium, for example, melts at just 16 <sup>o<\/sup>C. <sup>(4)<\/sup><\/p>\n<p>\t\tThis type of alloy can be used as a non-toxic alternative to <a href=\"https:\/\/www.chemicool.com\/elements\/mercury.html\">mercury<\/a> in some applications.<\/p>\n<p>\t\tCompounds of indium are used in the semiconductor industry for  <a href=\"https:\/\/www.chemicool.com\/elements\/germanium.html\">germanium<\/a> transistors, thermistors, rectifiers and photocells.<\/p>\n<p>\t\tIndium can be coated on metals and evaporated onto glass, to form mirrors equal to that made with <a href=\"https:\/\/www.chemicool.com\/elements\/silver.html\">silver<\/a> but more corrosion resistant.<\/p>\n<p>\t\tIndium-tin oxide thin films are used for liquid crystal displays (LCDs).\t<\/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> 250 parts per billion by weight, 47 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  4 parts per billion by weight, 40 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $968 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $54 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Indium has no minerals or ores with a high concentration of the element. Commercially, indium is extracted as a by-product of <a href=\"https:\/\/www.chemicool.com\/elements\/zinc.html\">zinc<\/a> refining. It is also extracted from <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/lead.html\">lead<\/a>, and <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a> ores.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Indium has 35 isotopes whose half-lives are known, with mass numbers from 100 to 134. Of these, one is stable: <sup>113<\/sup>In.  Naturally occurring indium is a mixture of two isotopes: <sup>115<\/sup>In, with a half-life of 4.41 x 10<sup>14<\/sup> years and an abundance of 95.7% and <sup>113<\/sup>In with an abundance of 4.3%.  <\/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>J.W. Mellor, A Comprehensive Treatise on Inorganic and Theoretical Chemistry., 1929, vol v, Longmans, Green and Co., p 387,388.<\/li>\n<li>Mary Elvira Weeks, Discovery of the Elements, 2003, Kessinger Publishing, p198.<\/li>\n<li>U. Schwarz-Schampera, P.M. Herzig, Indium: Geology, Mineralogy, and Economics, 2002, Springer, p5<\/li>\n<li>&#8220;<a href=\"http:\/\/scitoys.com\/scitoys\/scitoys\/thermo\/liquid_metal\/liquid_metal.html\">A metal alloy that is liquid at room temperature<\/a>.&#8221; Scitoys. 10\/21\/2009.<\/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\/indium.html\"&gt;Indium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/indium.html\"&gt;Indium 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\"Indium.\" Chemicool Periodic Table. Chemicool.com. 09 Nov. 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\/indium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 49 In 114.8 The chemical element indium is classed as an other metal. It was discovered in 1863 by Ferdinand Reich. Data Zone Classification: Indium is an &#8216;other metal&#8217; Color: silvery-white Atomic weight: 114.82 State: solid Melting [&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-401","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/401","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=401"}],"version-history":[{"count":35,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/401\/revisions"}],"predecessor-version":[{"id":4249,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/401\/revisions\/4249"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=401"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}