{"id":250,"date":"2012-05-23T09:24:30","date_gmt":"2012-05-23T09:24:30","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=250"},"modified":"2017-12-07T02:08:58","modified_gmt":"2017-12-07T07:08:58","slug":"titanium","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/titanium.html","title":{"rendered":"Titanium 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\">22<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Ti<\/div>\n<div class=\"atweiT\"> 47.87<\/div>\n<\/div>\n<p>The chemical element titanium is classed as a transition metal. It was discovered in 1791 by Reverend William Gregor.<\/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>  Titanium 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>   47.87 <\/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> 1668 <sup>o<\/sup>C, 1941 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  3287 <sup>o<\/sup>C, 3560 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>22<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>22<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>26<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>    2,8,10,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Ar] 3d<sup>2<\/sup> 4s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  4.50 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a369f8b6fedf\"  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-id6a369f8b6fedf\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>  10.64 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>   6.0  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.52   J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 14.15 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>   471   kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   425 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 658 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1310.3  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2652.5 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>  7.6  kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  -1    <\/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> 1.54    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>  14.6 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht  &#8658;  TiO<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>   passivated  <\/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> TiO, Ti<sub>2<\/sub>O<sub>3<\/sub>, TiO<sub>2<\/sub> (titania) + more <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>    TiH<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  TiCl<sub>2<\/sub>, TiCl<sub>3<\/sub>, TiCl<sub>4<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   140 pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (1+ ion) <\/td>\n<td> 128  pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>   100  pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 81  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> 21.9  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  2.6 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> 1668 <sup>o<\/sup>C, 1941 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-titanium.jpg\" width=\"300\" height=\"160\" alt=\"Titanium\" class=\"size-full\" \/><p class=\"wp-caption-text\">The Guggenheim Museum, Bilbao, covered with titanium panels.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-titanium-ilmenite.jpg\" width=\"300\" height=\"214\" alt=\"ilmenite\" class=\"size-full\" \/><p class=\"wp-caption-text\">Ilmenite, the mineral in which William Gregor discovered titanium.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Titanium<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>     Titanium&#8217;s discovery was announced in 1791 by the amateur geologist Reverend William Gregor from Cornwall, England.  <sup>(1), (2)<\/sup><\/p>\n<p>Gregor found a black, magnetic sand that looked like gunpowder in a stream in the parish of Mannacan in Cornwall, England. (We now call this sand ilmenite; it is a mixture consisting mainly of the oxides of iron and titanium.)<\/p>\n<p>Gregor analyzed the sand, finding it was largely magnetite (Fe<sub>3<\/sub>O<sub>4<\/sub>) and the rather impure oxide of a new metal, which he described as &#8216;reddish brown calx.&#8217;<\/p>\n<p>This calx turned yellow when dissolved in sulfuric acid and purple when reduced with <a href=\"iron.html\">iron<\/a>, <a href=\"tin.html\">tin<\/a> or <a href=\"zinc.html\">zinc<\/a>. Gregor concluded that he was dealing with a new metal, which he named manaccanite in honor of the parish of Mannacan.<\/p>\n<p>Having discovered a new metal, Gregor returned to his pastoral duties.<\/p>\n<p>Little more happens in our story until 1795, when the well-known German chemist Martin Klaproth experienced the thrill of discovering a new metallic element. Klaproth called the new metal titanium, after the Titans, the sons of the Earth goddess in Greek mythology.<\/p>\n<p>Klaproth discovered titanium in the mineral rutile, from Boinik, Hungary. Just like Gregor&#8217;s calx, the rutile was a red color. In 1797 Klaproth read Gregor&#8217;s account from 1791 and realized that the red oxide in which he had found titanium and the red oxide in which Gregor had found manaccanite were in fact the same; titanium and maccanite were the same element and Gregor was the element&#8217;s true discoverer.<\/p>\n<p>Gregor may have beaten Klaproth to the new metal, but scientists preferred Klaproth&#8217;s &#8216;titanium&#8217; to Gregor&#8217;s &#8216;manaccanite.&#8217;<\/p>\n<p>Obtaining a sample of pure titanium proved to be much harder than discovering it. <\/p>\n<p>Many scientists tried, but it took 119 years from its discovery until 99.9% pure titanium was isolated in 1910 by metallurgist Matthew Hunter in Schenectady, New York, who heated titanium (IV) chloride with sodium to red-heat in a pressure cylinder. <sup>(2)<\/sup><\/p>\n<p>In 1936, the Kroll Process (heating titanium (IV) chloride with <a href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\">magnesium<\/a>) made the commercial production of titanium possible. By 1948 worldwide production had reached just 3 tons a year.<\/p>\n<p>By 1956, however, scientists and engineers had realized titanium&#8217;s properties were highly desirable and worldwide production had exploded to 25,000 tons a year. <sup>(3)<\/sup><\/p>\n<p>The 2011 forecast for worldwide production of titanium metal using the Kroll process was 223,000 metric tons.   <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<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/e_uO7PU8l8Y\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A blacksmith makes a knife from titanium and shows the metal&#8217;s properties.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/8W5bNGlhrsA\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Finely divided titanium burns easily.<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-titanium-nanotube.png\" width=\"300\" height=\"300\" alt=\"titanium atoms on carbon nanotube\" class=\"size-full\" \/><p class=\"wp-caption-text\">Computer generated image of titanium atoms (blue) bonded to a carbon nanotube in a hydrogen (red) fuel-cell. Molecules like this could improve the efficiency of fuel-cells for automotive use. Image: <a href=\"http:\/\/www.nist.gov\/pml\/div688\/news_nanotubes.cfm\">T. Yildirim\/NIST<\/a><\/p><\/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 \tTitanium metal is considered to be non-toxic. As metal shavings, or powder, it is a considerable fire hazard. Titanium chlorides are corrosive.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Pure titanium is a light, silvery-white, hard, lustrous metal. It has excellent strength and corrosion resistance and also has a high strength to weight ratio.<\/p>\n<p>\t\tTitanium&#8217;s corrosion rate is so low that after 4000 years in seawater, corrosion would only have penetrated the metal to the thickness of a thin sheet of paper. <sup>(3)<\/sup><\/p>\n<p>\t\tAt high temperatures the metal burns in air and, unusually, titanium also burns in pure nitrogen.<\/p>\n<p>\t\tTitanium is ductile and is malleable when heated. <\/p>\n<p>\t\tIt is insoluble in water, but soluble in concentrated acids. <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Titanium<\/h2>\n<p>\t\tTitanium metal is used as an alloying agent with metals including aluminum, <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/molybdenum.html\"> molybdenum<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/manganese.html\"> manganese<\/a>. Alloys of titanium are mainly used in aerospace, aircraft and engines where strong, lightweight, temperature-resistant materials are needed.<\/p>\n<p>\t\tAs a result of its resistance to seawater, (see above) titanium is used for hulls of ships, propeller shafts and other structures exposed to the sea.<\/p>\n<p>\t\tTitanium is also used in joint replacement implants, such as the ball-and-socket hip joint.<\/p>\n<p>\t\tAbout 95% of titanium production is in the forum of titanium dioxide (titania). This intensely white pigment, with a high refractive index and strong UV light absorption, is used in white paint, food coloring, toothpaste, plastics and sunscreen.<\/p>\n<p>    Titanium is used in several everyday products such as drill bits, bicycles, golf clubs, watches and laptop computers. <\/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>  0.56% by weight, 0.25% by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 4 parts per million by weight,  100 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>   $661 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> Titanium is the ninth most abundant metal in the Earth&#8217;s crust. Titanium is not found freely in nature but is found in minerals such as rutile (titanium oxide), ilmenite (iron titanium oxide) and sphene (titanite or calcium titanium silicate).<\/p>\n<p>      Commercially, the metal is isolated using the Kroll process which initially prepares titanium oxide from the mineral ilmenite. The oxide TiO<sub>2<\/sub> is then converted to the chloride ( TiCl<sub>4<\/sub>) through carbochlorination. This is condensed and purified by fractional distillation and then reduced with molten magnesium in an argon atmosphere.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Titanium has 18 isotopes whose half-lives are known, with mass numbers 39 to 57. Naturally occurring titanium is a mixture of its five stable isotopes and they are found in the percentages shown: <sup>46<\/sup>Ti (8.2%), <sup>47<\/sup>Ti (7.4%), <sup>48<\/sup>Ti (73.7%), <sup>49<\/sup>Ti (5.4%) and <sup>50<\/sup>Ti (5.2%). The most naturally abundant of these isotopes is <sup>48<\/sup>Ti at 73.7%.  <\/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>William Gregor, <a href=\" http:\/\/books.google.com\/books?id=pqc5AAAAcAAJ&#038;printsec=frontcover&#038;source=gbs_ge_summary_r&#038;cad=0#v=onepage&#038;q&#038;f=false\">Beobachtungen und Versuche &#252;ber den Menakanite, einen in Cornwall gefundenen magnetischen Sand<\/a>., in Lorenz Crell&#8217;s Chemische Annalen, 1791, p40. <\/li>\n<li>Mary Elvira Weeks, The discovery of the elements. XI. Some elements isolated with the aid of potassium and sodium: Zirconium, titanium, cerium, and thorium., J. Chem. Educ., 1932, p1231. <\/li>\n<li>Tom Margerison, <a href=\"http:\/\/books.google.com\/books?id=4FWAg4pGJhcC\">The Future of Titanium<\/a>., New Scientist Jun 12, 1958, p156.<\/li>\n<li><a href=\"http:\/\/www.abare.gov.au\/interactive\/08_ResearchReports\/Titanium\/htm\/chapter_4.htm\">Research and development in titanium<\/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\/titanium.html\"&gt;Titanium&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/titanium.html\"&gt;Titanium 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\"Titanium.\" 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\/titanium.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 22 Ti 47.87 The chemical element titanium is classed as a transition metal. It was discovered in 1791 by Reverend William Gregor. Data Zone Classification: Titanium is a transition metal Color: silvery-white Atomic weight: 47.87 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-250","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/250","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=250"}],"version-history":[{"count":19,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/250\/revisions"}],"predecessor-version":[{"id":4315,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/250\/revisions\/4315"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=250"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}