{"id":97,"date":"2012-05-21T14:04:52","date_gmt":"2012-05-21T14:04:52","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=97"},"modified":"2017-12-07T02:07:25","modified_gmt":"2017-12-07T07:07:25","slug":"boron","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/boron.html","title":{"rendered":"Boron 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=\"metalloidT\">\n<div class=\"atnorT\">5<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">B<\/div>\n<div class=\"atweiT\">10.81<\/div>\n<\/div>\n<p>The chemical element boron is classed as a metalloid. It was discovered in 1808 by Joseph L. Gay-Lussac and L. J. Th&eacute;nard and independently by Sir Humphry 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>  Boron is a metalloid  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>   black  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   10.81 <\/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> 2075 <sup>o<\/sup>C, 2348 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  3727 <sup>o<\/sup>C , 4000 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>5<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>5<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>6<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,3   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  2.34 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a4481490de21\"  tabindex=\"0\" title=\"Show more, including: Heats, Energies, Oxidation, Reactions,&lt;br \/&gt; Compounds, Radii, Conductivities\"    >Show more, including: Heats, Energies, Oxidation, Reactions,<br \/> Compounds, Radii, Conductivities<\/span><div id=\"target-id6a4481490de21\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   4.6 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   rhombohedral; B<sub>12<\/sub> is icosahedral. <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>     9.3 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   1.02 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>50.2 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 563 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   480 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 800.6 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   2427.1 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>   3659.7 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    26.7 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> 2.04  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   3 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht &#8658; B<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>  none  <\/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> B<sub>2<\/sub>O<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   B<sub>2<\/sub>H<sub>6<\/sub> and many B<sub>x<\/sub>H<sub>y<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  BCl<sub>3<\/sub> and many B<sub>x<\/sub>Cl<sub>y<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  85 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> 41  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> 27.4 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  5.0 x10<sup>-6<\/sup> S m<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Freezing\/Melting point:<\/td>\n<td> 2075 <sup>o<\/sup>C, 2348 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\" class=\"size-full\" src=\"https:\/\/chemicool.com\/elements\/images\/300-boron.jpg\" alt=\"Boron\" width=\"300\" height=\"148\" \/><p class=\"wp-caption-text\">Amorphous Boron in sample-tube. (Photo by Tomihahndorf)<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" class=\"size-full\" src=\"https:\/\/chemicool.com\/elements\/images\/300-boron-lussac.jpg\" alt=\"Boron was discovered by Joseph Louis Gay-Lussac.\" width=\"300\" height=\"330\" \/><p class=\"wp-caption-text\">Joseph Louis Gay-Lussac and Jean-Baptiste Biot collecting air samples at different altitudes. In addition to discovering boron, Gay-Lussac discovered that the composition of the atmosphere does not change with increasing altitude.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Boron<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Boron compounds such as borax (sodium tetraborate, Na<sub>2<\/sub>B<sub>4<\/sub>O<sub>7<\/sub>&middot;10H<sub>2<\/sub>O) were known and used by ancient cultures for thousands of years. Borax&#8217;s name comes from the Arabic <i>buraq<\/i>, meaning &#8220;white.&#8221; <\/p>\n<p>\t\tBoron was first partially isolated in 1808 by French chemists Joseph L. Gay-Lussac and L. J. Th&eacute;nard and independently by Sir Humphry Davy in London. Gay-Lussac &amp; Th&eacute;nard reacted boric acid with <a href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\">magnesium<\/a> or <a href=\"https:\/\/www.chemicool.com\/elements\/sodium.html\">sodium<\/a> to yield boron, a gray solid. <sup>(1)<\/sup> They believed it shared characteristics with <a href=\"https:\/\/www.chemicool.com\/elements\/sulfur.html\">sulfur<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/phosphorus.html\">phosphorus<\/a> and named it <i>bore<\/i>. <sup>(2)<\/sup><\/p>\n<p>Davy first tried to produce boron by electrolysis of boric acid, but was not satisfied with the results. He enjoyed greater success reacting boric acid with <a href=\"https:\/\/www.chemicool.com\/elements\/potassium.html\">potassium<\/a> in a <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> atmosphere. The result was a powdery substance.<\/p>\n<p>Davy commented the substance was, &#8220;of the darkest shades of olive. It is opake, very friable, and its powder does not scratch glass.&#8221; After carrying out a number of chemical reactions to verify the uniqueness of the substance, Davy wrote, &#8220;there is strong reason to consider the boracic basis as metallic in nature, and I venture to propose for it the name of <i>boracium<\/i>.&#8221; <sup>(2)<\/sup><\/p>\n<p>\t\tNeither party had, in fact, produced pure boron. Their samples were only about 60% pure. <\/p>\n<p>\t\tIn 1909, American chemist Ezekiel Weintraub produced 99% pure boron, by reducing boron halides with <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a>.<\/p>\n<p>\t\tAlmost a century later, in 2004, Jiuhua Chen and Vladimir L. Solozhenko produced a new form of boron, but were uncertain of its structure.<\/p>\n<p>\t\tIn 2009, a team led by Artem Oganov was able to demonstrate the new form of boron contains two structures, B<sub>12<\/sub> icosohedra and B<sub>2<\/sub> pairs. <sup>(3)<\/sup> Gamma-boron, as it has been called, is almost as hard as diamond and more heat-resistant than diamond.<\/p>\n<p>\t\tTalking about boron&#8217;s part metal, part non-metal properties,  Oganov said, &#8220;Boron is a truly schizophrenic element. It&#8217;s an element of complete frustration. It doesn&#8217;t know what it wants to do. The outcome is something horribly complicated.&#8221; <sup>(4)<\/sup><\/p>\n<p><a id=\"facts\"><\/a><\/p>\n<h2>Interesting Facts about Boron<\/h2>\n<ul>\n<li>Boron is a tough element &#8211; very hard, and very resistant to heat. In its crystalline form it is the second hardest of all the elements on the mohs scale &#8211; only carbon (diamond) is harder. Only 11 elements have higher melting points than boron: these are C, W, Re, Os, Ta, Mo, Nb, Ir, Ru, Hf, and Tc. (As a challenge, how many of these elements can you name without looking them up?)<\/li>\n<li>Boron is an essential nutrient for all green plants.<\/li>\n<li>Boron in its crystalline form is very unreactive. Amorphous boron is reactive.<\/li>\n<li>Unusually, the universe&#8217;s atoms of boron were not made by nuclear fusion within stars and were not made in the big bang. They were made by nuclear fusion in cosmic-ray collisions. Most of the universe&#8217;s boron was made in this way before the formation of our solar system. <\/li>\n<li>Boron is an indispensable element in NIB magnets (Neodymium &#8211; Iron &#8211; Boron). NIB magnets are very powerful magnets invented in the early 1980s. They are used in computers, cell phones, medical equipment, toys, motors, wind turbines and audio systems.<\/li>\n<li>Boron is used to control nuclear reactions. It is an excellent neutron absorber. Alloyed with steel or reacted with carbon, titanium or zirconium, it is used in control rods for nuclear reactors.<\/li>\n<li>Pure boron can exist as a mixture of positive and negative boron ions.<\/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\/WQFua-X3SDQ?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Boron compounds burn with a green flame. The distinctive color leads to use in fireworks.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/_ud84u5Uck0?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Boron is an ionic element &#8211; pure boron can exist as a mixture of positive and negative boron ions.<\/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 \tElemental boron is not known to be toxic. <\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>Boron is a metalloid, intermediate between metals and non-metals. It exists in many polymorphs (different crystal lattice structures), some more metallic than others. Metallic boron is extremely hard and has a very high melting point.<\/p>\n<p>Boron does not generally make ionic bonds, it forms stable covalent bonds.<\/p>\n<p>Although opaque to visible light, boron can transmit portions of infrared light.<\/p>\n<p>Boron is a poor room temperature conductor of electricity but its conductivity improves markedly at higher temperatures.\t <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Boron<\/h2>\n<p>\t\tBoron is used to dope <a href=\"https:\/\/www.chemicool.com\/elements\/silicon.html\">silicon<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/germanium.html\">germanium<\/a> semiconductors, modifying their electrical properties. <\/p>\n<p>      Boron oxide (B<sub>2<\/sub>O<sub>3<\/sub>) is used in glassmaking and ceramics.<\/p>\n<p>\t\t  Borax (Na<sub>2<\/sub>B<sub>4<\/sub>O<sub>7<\/sub>.10H<sub>2<\/sub>O) is used in making fiberglass, as a cleansing fluid, a water softener, insecticide, herbicide and disinfectant.<\/p>\n<p>\t\t  Boric acid (H<sub>3<\/sub>BO<sub>3<\/sub>) is used as a mild antiseptic and as a flame retardant.<\/p>\n<p>\t\t\tBoron Nitride&#8217;s\thardness is second only to diamond, but it has better thermal and chemical stability, hence boron nitride ceramics are used in high-temperature equipment. <\/p>\n<p>\t\t\tBoron nitride nanotubes can have a similar structure to <a href=\"https:\/\/www.chemicool.com\/elements\/carbon.html\">carbon<\/a> nanotubes. BN nanotubes are more thermally and chemically stable than carbon nanotubes and, unlike carbon nanotubes, boron nitride nanotubes are electrical insulators. <\/p>\n<p>\t\t\tBoron carbide (B<sub>4<\/sub>C) is used in tank armor and bullet proof vests.<\/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>  10 parts per million by weight, 1 part per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 2 parts per billion by weight, 0.2 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $1114 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $500 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Boron compounds are usually is found in sediments and sedimentary rock formations. The chief sources of boron are Na<sub>2<\/sub>B<sub>4<\/sub>O<sub>6<\/sub>(OH)<sub>2<\/sub>.3H<sub>2<\/sub>O &#8211; known as rasorite or kernite; borax ore (known as tincal); and with <a href=\"https:\/\/www.chemicool.com\/elements\/calcium.html\">calcium<\/a> in colemanite (CaB<sub>3<\/sub>O<sub>4<\/sub>(OH)<sub>4<\/sub>.H<sub>2<\/sub>O). Boron also occurs as orthoboric acid in some volcanic spring waters.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> 11 whose half-lives are known, with mass numbers 7 to 17. Naturally occurring boron is a mixture of its two stable isotopes and they are found in the percentages shown: <sup>10<\/sup>B (19.9%) and <sup>11<\/sup>B (80.1%). <sup>10<\/sup>B  is used in nuclear reactors as a neutron-capturing substance.<\/p>\n<div style=\"clear:both;line-height:2px;\">&nbsp;<\/div>\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>Alaa S. Abd-El-Aziz, Macromolecules Containing Metal and Metal-Like Elements Volume 8  Boron-Containing Polymers., (2007) p2.  Wiley-Interscience<\/li>\n<li><a href=\"http:\/\/books.google.com\/books\/download\/New_England_journal_of_medicine_and_surg.pdf?id=E0OVC_AWShYC&#038;output=pdf&#038;sig=ACfU3U0_By9mK31N4cX-12rQpu-RVW_5fQ\">Walter Channing, John Ware, New-England Journal of Medicine and Surgery, and Collateral Branches of Science., (1812) p220. T. B. Wait and Co.<\/a> (pdf download 19.8 MB)<\/li>\n<li>Artem R. Oganov et al, <a href=\"http:\/\/www.nature.com\/nature\/journal\/v457\/n7231\/full\/nature07736.html#a3\">Ionic high-pressure form of elemental boron<\/a>., Nature 457, 863-867 (12 February 2009)<\/li>\n<li>Kenneth Chang, <a href=\"http:\/\/www.nytimes.com\/2009\/02\/03\/science\/03boron.html?_r=1\">Theory and Experiment Meet, and a New Form of Boron Is Found<\/a>., (February 2, 2009) New York Times Online<\/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\/boron.html\"&gt;Boron&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/boron.html\"&gt;Boron 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\"Boron.\" Chemicool Periodic Table. Chemicool.com. 15 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\/boron.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 5 B 10.81 The chemical element boron is classed as a metalloid. It was discovered in 1808 by Joseph L. Gay-Lussac and L. J. Th&eacute;nard and independently by Sir Humphry Davy. Data Zone Classification: Boron is a [&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-97","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/97","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=97"}],"version-history":[{"count":26,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/97\/revisions"}],"predecessor-version":[{"id":4612,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/97\/revisions\/4612"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=97"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}