{"id":351,"date":"2012-05-24T10:29:04","date_gmt":"2012-05-24T10:29:04","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=351"},"modified":"2018-12-03T06:00:48","modified_gmt":"2018-12-03T11:00:48","slug":"strontium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/strontium.html","title":{"rendered":"Strontium 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\">38<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Sr<\/div>\n<div class=\"atweiT\"> 87.62<\/div>\n<\/div>\n<p>The chemical element strontium is classed as an alkali earth metal. It was discovered in 1790 by Adair Crawford.<\/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>  Strontium is an alkali earth metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td> silvery    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   87.62 <\/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> 777 <sup>o<\/sup>C, 1050 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  1380  <sup>o<\/sup>C, 1653 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>38<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>38<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>50<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,8,2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>  [Kr] 5s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  2.6 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2b380328883\"  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-id6a2b380328883\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   33.7 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>    1.5 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.30 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 8.30  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  164 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   144.0   kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  549.5  kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1064.2    kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  4138   kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>  5  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>    0.95   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   27.6  &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> vigorous, &#8658;  SrO, Sr<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>  vigorous, &#8658; H<sub>2<\/sub>, Sr(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>, SrCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>   vigorous, &#8658;  none  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> SrO, SrO<sub>2<\/sub> (strontium peroxide)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>    SrH<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  SrCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  200  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>    132  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> 35.4  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  5 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> 777 <sup>o<\/sup>C, 1050 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:\/\/www.chemicool.com\/elements\/images\/300-strontium.jpg\" width=\"300\" height=\"160\" alt=\"Strontium\" class=\"size-full\" \/><p class=\"wp-caption-text\">Strontium. Photo by Matthias Zepper.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Strontium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>Strontium was recognized as a new element in 1790 when Adair Crawford analyzed a mineral sample from a lead mine near Strontian, Scotland. Until then scientists had thought strontium and <a href=\"barium.html\">barium<\/a> were the same element, and only barium&#8217;s existence had been recognized.<\/p>\n<p>The mineral took its name from the Scottish town and was called strontianite (strontium carbonate). <\/p>\n<p>Strontium metal was first isolated in 1808 by Sir Humphry Davy working in London using electrolysis.  <\/p>\n<p>Davy had built a very large 600-plate battery, which he used to pass electricity through salts, breaking them down in order to isolate new elements.<\/p>\n<p>He mixed magnesium oxide to a paste with (probably) strontium sulfate. He made a depression in the paste and placed <a href=\"mercury.html\">mercury<\/a> metal there to act as an electrode. <a href=\"platinum.html\">Platinum<\/a> was used as a counter electrode.<\/p>\n<p>When electricity was passed through the paste, a strontium-mercury amalgam formed at the mercury electrode.<\/p>\n<p>Davy removed the mercury from the amalgam by heating it to leave strontium metal. <sup>(1),(2)<\/sup>.<\/p>\n<p>The element was named strontium by Davy after the mineral it was produced from.<\/p>\n<p>Davy discovered or isolated for the first time several alkali and alkali earth metals including <a href=\"potassium.html\">potassium<\/a>, <a href=\"sodium.html\">sodium<\/a>, <a href=\"barium.html\">barium<\/a>, <a href=\"calcium.html\">calcium<\/a> and <a href=\"magnesium.html\">magnesium<\/a>.<\/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-strontium-fireworks.jpg\" width=\"300\" height=\"167\" alt=\"Strontium fireworks\" class=\"size-full\" \/><p class=\"wp-caption-text\">Strontium nitrate produces a red color in pyrotechnic displays. Strontium is the source of the red color.<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/kDuE3CVWjUk\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Strontium metal burns in air with a distinctive red flame, forming a mixture of strontium oxide and nitride.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/4d9IU-Dyemo\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">The world&#8217;s most accurate atomic clock, based on strontium atoms, would neither gain nor lose a second in more than 200 million years.<\/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 \tStrontium&#8217;s non-radioactive isotopes are considered non-toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Strontium is a soft, silvery metal. When cut it quickly turns a yellowish color due to the formation of strontium oxide (strontia, SrO). Finely powdered strontium metal is sufficiently reactive to ignite spontaneously in air.<\/p>\n<p>\t\tIt reacts with water quickly (but not violently like the Group 1 metals) to produce strontium hydroxide and <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> gas.<\/p>\n<p>\t\tStrontium and its compounds burn with a crimson flame and are used in fireworks.<\/p>\n<p><strong>Strontium&#8217;s Periodic Table Neighborhood<\/strong><br \/>\nStrontium is a Group 2 Alkaline earth metal. It usually exists as a divalent ion, Sr<sup>2+<\/sup>, in its compounds. Strontium&#8217;s chemistry is very similar to that of calcium, which sits above it in Group 2.<\/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\">4<\/td>\n<td><a class=\"alkali\" href=\"https:\/\/www.chemicool.com\/elements\/potassium.html\" title=\"potassium \"><sup>19<\/sup><br \/>K<\/a> <\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\" title=\"calcium \"><sup>20<\/sup><br \/>Ca<\/a> <\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/scandium.html\" title=\"scandium \"><sup>21<\/sup><br \/>Sc<\/a> <\/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<\/table>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Strontium<\/h2>\n<p>\t\tStrontium is used for producing glass (cathode ray tubes) for color televisions. It is also used in producing ferrite ceramic magnets and in refining zinc.<\/p>\n<p>\t\tThe world&#8217;s most accurate atomic clock, accurate to one second in 200 million years, has been developed using strontium atoms.<\/p>\n<p>\t\tStrontium salts are used in flares and fireworks for a crimson color.<\/p>\n<p>\t\tStrontium chloride is used in toothpaste for sensitive teeth.<\/p>\n<p>\t\tStrontium oxide is used to improve the quality of pottery glazes.<\/p>\n<p>\t\tThe isotope <sup>90<\/sup>Sr is one of the best long-lived, high-energy beta emitters known. It is used in cancer therapy.<\/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>  370 parts per million by weight, 87 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 50 parts per billion by weight, 0.7 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $100 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> Strontium is never found free in nature. The principal strontium ores are celestine (strontium sulfate, SrSO<sub>4<\/sub>) and strontianite (strontium carbonate, SrCO<sub>3<\/sub>). The main commercial process for strontium metal production is reduction of strontium oxide with <a href=\"https:\/\/www.chemicool.com\/elements\/aluminum.html\">aluminum<\/a>.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Strontium has 28 isotopes whose half-lives are known, with mass numbers 75 to 102. Naturally occurring strontium is a mixture of its four stable isotopes and they are found in the percentages shown: <sup>84<\/sup>Sr (0.6%), <sup>86<\/sup>Sr (9.9%), <sup>87<\/sup>Sr (7.0%) and <sup>88<\/sup>Sr (82.6%). <\/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>Mary Elvira Weeks, Discovery of the Elements., Journal of Chemical Education (June 1932) p1046. <\/li>\n<li><a href=\"http:\/\/www.chemheritage.org\/discover\/magazine\/articles\/26-4-science-and-celebrity.aspx?page=1\">T. K. Kenyon, Science and Celebrity: Humphry Davy&#8217;s Rising Star., Chemical Heritage Magazine, (2008\/9 edition)<\/a>. <\/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\/strontium.html\"&gt;Strontium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/strontium.html\"&gt;Strontium 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\"Strontium.\" Chemicool Periodic Table. Chemicool.com. 24 Jul. 2015. 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\/strontium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 38 Sr 87.62 The chemical element strontium is classed as an alkali earth metal. It was discovered in 1790 by Adair Crawford. Data Zone Classification: Strontium is an alkali earth metal Color: silvery Atomic weight: 87.62 State: [&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-351","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/351","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=351"}],"version-history":[{"count":27,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/351\/revisions"}],"predecessor-version":[{"id":3694,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/351\/revisions\/3694"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=351"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}