{"id":165,"date":"2012-05-22T10:08:38","date_gmt":"2012-05-22T10:08:38","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=165"},"modified":"2017-12-07T02:07:55","modified_gmt":"2017-12-07T07:07:55","slug":"fluorine","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/fluorine.html","title":{"rendered":"Fluorine 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=\"halogensT\">\n<div class=\"atnorT\">9<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">F<\/div>\n<div class=\"atweiT\">19.00<\/div>\n<\/div>\n<p>The chemical element fluorine is classed as a halogen and a nonmetal . It was discovered in 1813 by Humphrey Davy.<\/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>  Fluorine is a halogen and a nonmetal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  pale yellow <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   18.998403 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">State:<\/td>\n<td>   gas   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Melting point:<\/td>\n<td> -219.6 <sup>o<\/sup>C, 53.6 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  -188.1 <sup>o<\/sup>C, 85.1 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>9<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>9<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>10<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,7   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>5<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  0.001696 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a3bc95d342df\"  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-id6a3bc95d342df\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   17.1 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   cubic crystals in solid phase  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>  &#8211;   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.82  J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 0.510 kJ mol<sup>-1<\/sup> of F<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 79 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   6.62 kJ mol<sup>-1<\/sup> of F<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 1681 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   3374.1 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   6050.3 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   328  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>  -1   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Maximum oxidation number <\/td>\n<td> 0 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  0  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 3.98   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>  0.634 &Aring;<sup>3<\/sup><br \/>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> none  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 3 M HNO<sub>3<\/sub> <\/td>\n<td>  &#8658; NO<sub>3<\/sub>F   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td>  vigorous,  &#8658;  HF, OF<sub>2<\/sub>, ClF<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>   m vigorous,  &#8658;  O<sub>2<\/sub>, NaF  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> OF<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   HF (fluoric acid)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td> ClF, ClF<sub>3<\/sub>,   ClF<sub>5<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  50 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\"> Ionic radius (1- ion) <\/td>\n<td>   119  pm  <\/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> 0.0277 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Freezing\/Melting point:<\/td>\n<td> -219.6 <sup>o<\/sup>C, 53.6 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-fluoride-toothpaste.gif\" width=\"300\" height=\"158\" alt=\"fluoride\/fluorine\" class=\"size-full\" \/><p class=\"wp-caption-text\">The fluoride ion, from the element fluorine, inhibits tooth decay.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-fluorite-before.jpg\" width=\"300\" height=\"188\" alt=\"Fluorite in light\" class=\"size-full\" \/><p class=\"wp-caption-text\">Fluorite (originally called fluorspar) crystals in daylight.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-fluorite-after.jpg\" width=\"300\" height=\"189\" alt=\"Fluorite in darkness\" class=\"size-full\" \/><p class=\"wp-caption-text\">The same fluorite crystals fluorescing in darkness after exposure to light. The phenomenon of fluorescence was given its name because it was first observed in fluorite. Actually, the glow does not come from fluorine but from small amounts of <a href=\"europium.html\">europium<\/a> in the fluorite. Photo Credits: Rob Lavinsky, <a href=\"http:\/\/www.irocks.com\/\">iRocks.com<\/a><\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Fluorine<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>In 1530, German mineralogist Georgius Agricola described the use of the mineral fluorspar in metal refining. Fluorspar (which we now know is mainly calcium fluoride) was very useful because it combined with the unwanted parts of metal ores, allowing the pure metal to flow and be collected. <\/p>\n<p>\t\tThe element fluorine had not yet been discovered and the &#8216;fluor&#8217; in fluorspar came from the Latin word &#8216;fluere,&#8217; meaning &#8216;to flow,&#8217; because this is what it allowed metals to do. The element name fluorine ultimately came from the &#8216;fluor&#8217; in fluorspar.<\/p>\n<p>\t\tSeveral chemists carried out experiments on fluorspar in the early 1800s including Gay Lussac, Louis Jacques Thenard, Humphry Davy, Carl Wilhelm Scheele and Joseph Priestley.<sup>(1)<\/sup><\/p>\n<p>\t\tOften they produced what they called fluoric acid &#8211; now named hydrofluoric acid &#8211; a highly reactive and potentially deadly acid. Even small splashes of this acid on skin can be fatal.<sup>(2)<\/sup><\/p>\n<p>\t\tSeveral early attempts to isolate fluorine led to blindings and fatalities. English chemist Humphrey Davy wrote: &#8220;[fluoric acid] is a very active substance, and must be examined with great caution.<sup>(1)<\/sup> <\/p>\n<p>\t\tIn 1809, French scientist Andre-Marie Ampere proposed that fluoric acid was a compound of hydrogen with a new element. He exchanged letters with Humphry Davy, and in 1813 Davy announced the discovery of the new element fluorine, giving it the name suggested to him by Ampere.<\/p>\n<p>\t\tDavy wrote: &#8220;&#8230; it appears reasonable to conclude that there exists in the fluoric compounds a peculiar substance, possessed of strong attractions for metallic bodies and hydrogen&#8230; it may be denominated fluorine, a name suggested to me by M. Ampere.&#8221; <sup>(1)<\/sup>  <\/p>\n<p>\t\tFluorine was finally isolated in 1886, by French chemist Henri Moissan &#8211; whose own work was interrupted four times by serious poisoning caused by the element he was pursuing.<sup>(3)<\/sup> <\/p>\n<p>\t\tMoissan isolated fluorine by electrolysis of dry potassium hydrogen fluoride and anhydrous hydrofluoric acid.<\/p>\n<p>\t\tTo limit corrosion he carried out his work in a platinum container and cooled the electrolytic solution in it to -23 <sup>o<\/sup>F (-31 <sup>o<\/sup>C.) The stoppers were made out of fluorite (a more modern name for our old friend fluorspar, which we began this section with). Fluorine was produced at the positive electrode.<sup>(3)<\/sup><\/p>\n<p>\t\tHenri Moissan received the 1906 Nobel Prize in Chemistry for his achievement.<\/p>\n<p><a id=\"facts\"><\/a><\/p>\n<h2>Interesting Facts about Fluorine<\/h2>\n<ul>\n<li>Henri Moissan, who first isolated fluorine, also produced the world&#8217;s first artificial diamonds by applying huge pressures to charcoal.<\/li>\n<li>Fluorine is the most chemically reactive element. It reacts, often very vigorously, with all of the other elements except oxygen, helium, neon and krypton.<\/li>\n<li>Fluorine is the most electronegative element. This means that in molecules fluorine attracts electrons more powerfully than any other element can.<\/li>\n<li>Hydrofluoric acid, HF, dissolves glass. Its fluoride ions have a high affinity for calcium and can cause death by interfering with the body&#8217;s blood calcium metabolism when absorbed through the skin.<\/li>\n<\/ul>\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\/RkomnTbPLNc?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Fluorine gas, when it contacts other chemicals, results in flames.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"182\" src=\"https:\/\/www.youtube.com\/embed\/wqLnSkLalOE?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Fluorine gas is so reactive that when it flows onto a brick, the brick ignites!<\/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  Fluorine is highly toxic and corrosive. \t<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\tFluorine is the most reactive and the most electronegative of all the elements.<\/p>\n<p>\t\tFluorine is a pale yellow, diatomic, highly corrosive, flammable gas, with a pungent odor. It is the lightest halogen. <\/p>\n<p>\t\tIt reacts violently with water to produce oxygen and the extremely corrosive hydrofluoric acid.  <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Fluorine<\/h2>\n<p>\t\tFluorine and its compounds &#8211; mostly uranium hexafluoride &#8211; are used in processing nuclear fuel. <\/p>\n<p>\t\tFluorochemicals, including many high-temperature plastics such as Teflon, are also made using fluorine.<\/p>\n<p>\t\tCompounds of fluorine, including sodium fluoride, are used in toothpaste and in drinking water to prevent dental cavities.<\/p>\n<p>\t\tHydrofluoric acid can dissolve glass and is used to etch the glass in light bulbs and in other products.<\/p>\n<p>\t\tChlorofluorocarbons (CFCs) were used in as refrigerants in air conditioning units and freezers but they have now been banned because they contribute to ozone depletion.<\/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>  585 parts per million by weight, 104 part per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 500 parts per billion by weight,  30 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $190 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> In nature, fluorine occurs mainly in the minerals fluorspar (CaF<sub>2<\/sub>) and cryolite (Na<sub>3<\/sub>AlF<sub>6<\/sub>). Commercially, production of fluorine involves the electrolysis of a mixture of molten potassium fluoride and hydrofluoric acid. Fluorine gas forms at the anode, and <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> gas at the cathode.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Fluorine has 11 isotopes whose half-lives are known, with mass numbers 15 to 25. Naturally occurring fluorine consists of its one stable isotope, <sup>19<\/sup>F.<\/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>H. Davy, <a href=\" http:\/\/books.google.com\/books?id=qpRJAAAAYAAJ&#038;dq=Sir%20H.%20Davy%20Fluor%20Spar&#038;pg=PA263#v=onepage&#038;q&#038;f=false\">Some Experiments and Observations on the Substances Produced in Different Chemical Processes on Fluor Spar.<\/a>,  Philosophical Transactions of the Royal Society of London,  Vol 103, (1813) p263-279.<\/li>\n<li> <a href=\"http:\/\/www.bt.cdc.gov\/agent\/hydrofluoricacid\/basics\/facts.asp\">Facts About Hydrogen Fluoride.<\/a>  Centers for Disease Control and Prevention (CDC), National Institute for Occupational Safety and Health (NIOSH).<\/li>\n<li>Elvira Weeks, The Discovery of the Elements., J. Chem. Ed., Vol 9 No 11, (1933) p1915 &#8211; 1939.<\/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\/fluorine.html\"&gt;Fluorine&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/fluorine.html\"&gt;Fluorine 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\"Fluorine.\" Chemicool Periodic Table. Chemicool.com. 16 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\/fluorine.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 9 F 19.00 The chemical element fluorine is classed as a halogen and a nonmetal . It was discovered in 1813 by Humphrey Davy. Data Zone Classification: Fluorine is a halogen and a nonmetal Color: pale yellow [&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-165","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/165","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=165"}],"version-history":[{"count":26,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/165\/revisions"}],"predecessor-version":[{"id":4237,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/165\/revisions\/4237"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=165"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}