{"id":173,"date":"2012-05-22T10:30:31","date_gmt":"2012-05-22T10:30:31","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=173"},"modified":"2017-12-07T02:08:24","modified_gmt":"2017-12-07T07:08:24","slug":"neon","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/neon.html","title":{"rendered":"Neon 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=\"ngasesT\">\n<div class=\"atnorT\">10<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Ne<\/div>\n<div class=\"atweiT\">20.18<\/div>\n<\/div>\n<p>The chemical element neon is classed as a noble gas and a nonmetal. It was discovered in 1898 by William Ramsay and Morris Travers.<\/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>  Neon is a noble gas and a nonmetal  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  colorless <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   20.180 <\/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> -248.57 <sup>o<\/sup>C, 24.53 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  -246.0 <sup>o<\/sup>C, 27.1 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>10<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>10<\/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>    2,8   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup>     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  0.0009 g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a4fb7ec34613\"  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-id6a4fb7ec34613\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   16.7 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   fcc: face-centered cubic <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.904 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 0.3317 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 0 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    1.7326  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 2080.6 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  3952.2 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  6121.9 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   &#8211;  <\/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> 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> &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   0.396 &Aring;<sup>3<\/sup>  <\/td>\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 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> none  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   none   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  none  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  38 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>   &#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> 0.05  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> -248.57 <sup>o<\/sup>C, 24.53 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:\/\/www.chemicool.com\/elements\/images\/300-neon-ionized.jpg\" width=\"300\" height=\"285\" alt=\"Neon Glow\" class=\"size-full\" \/><p class=\"wp-caption-text\">The glow which so excited Ramsay and Travers is from neon. The neon gas in this image is also excited &#8211; ionized and emitting light.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-neonsign.jpg\" width=\"300\" height=\"153\" alt=\"Neon\" class=\"size-full\" \/><p class=\"wp-caption-text\">Neon gas spells &#8216;open&#8217; with the help of a few thousand volts needed to ionize it.<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Neon<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Neon was discovered in 1898 by William Ramsay and Morris Travers at University College London.<\/p>\n<p>\t\tThis was not the first time Ramsay had discovered a new element. <\/p>\n<p>\t\tIn 1894, he and Lord Rayleigh had discovered argon. Then, in 1895, Ramsay obtained the world&#8217;s first sample of helium. (Cleve and Langlet independently also obtained helium.)<\/p>\n<p>\t\tRamsay was aware an element must sit between helium and argon in the periodic table. But how could he find it?<\/p>\n<p>\t\tHaving found <a href=\"helium.html\">helium<\/a> in a radioactive mineral, Ramsay thought it was possible he could find the new element in another such mineral. He and Travers spent some time working with a number of minerals, trying unsuccessfully to drive out some of the as yet undiscovered gas. <sup>(1)<\/sup> <\/p>\n<p>\t\tAware of the history of chemistry, Ramsay knew that sometimes one new element can hide another. For example, Berzelius discovered <a href=\"cerium.html\">cerium<\/a> in the mineral that came to be known as cerite.\tSome years later Mosander, one of Berzelius&#8217;s former students, who had continued to study cerite, discovered the new element <a href=\"https:\/\/www.chemicool.com\/elements\/lanthanum.html\">lanthanum<\/a>. Lanthanum had been present in the cerite all along, but Berzelius had not found it. Ramsay wondered about the possibility of finding small amounts of the elusive new element hiding in one of his earlier discoveries, <a href=\"argon.html\">argon<\/a>.<\/p>\n<p>\t\tRamsay and Travers froze a sample of argon using liquid air. They then slowly evaporated the argon under reduced pressure and collected the first gas that came off.<\/p>\n<p>\t\tTo obtain the gas&#8217;s spectrum, Ramsay applied a high voltage to the gas in a vacuum tube and we may reasonably guess that his mouth fell open at what he saw. \t<\/p>\n<p>\t\tTravers later commented, &#8220;the blaze of crimson light from the tube told its own story and was a sight to dwell upon and never forget&#8230;  For the moment the actual spectrum of the gas did not matter in the least, for nothing in the world gave a glow such as we had seen.&#8221; <sup>(2)<\/sup> <\/p>\n<p>\t\tThis was the first time anyone had seen the glow of a neon light. Ramsay named the newly discovered element &#8216;neon&#8217; which is Greek for &#8216;new.&#8217;\t<\/p>\n<p><a id=\"facts\"><\/a><\/p>\n<h2>Interesting Facts about Neon<\/h2>\n<ul>\n<li>0.0018 percent of Earth&#8217;s atmosphere is neon. <\/li>\n<li>Although it is relatively rare on our planet, neon is the fifth most abundant element in the universe. <\/li>\n<li>If you could gather all the neon from the rooms in a typical new home in the United States, you would get 10 liters (2 gallons) of neon gas. <sup>(3),(4)<\/sup> <\/li>\n<li>Neon forms in stars with a mass of eight or more Earth suns. Near the end of their lives, these stars enter the carbon burning phase, also making <a href=\"oxygen.html\">oxygen<\/a>, <a href=\"sodium.html\">sodium<\/a> and <a href=\"magnesium.html\">magnesium<\/a>. (For oxygen production, stars need a mass of &#8216;just&#8217; five of our suns.) <sup>(5),(6)<\/sup> <\/li>\n<li>Neon has no stable compounds. <\/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\/qXQDEBqnAwQ?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Neon glowing in high voltage from Tesla coil.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/hwgmpoHRFME?rel=0\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Glowing neon an exhibition of the Museum of Neon Art.<\/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 \tNeon is not known to be toxic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Neon is a light, very inert gas.<\/p>\n<p>\t\t Colorless under normal conditions, it glows a reddish-orange in a vacuum discharge tube.<\/p>\n<p>\t\t Neon forms no known stable compounds.<\/p>\n<p>\t\t It has the smallest liquid range of any element (2.6 <sup>o<\/sup>C).<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Neon<\/h2>\n<p>\t\tWhen a few thousand volts are applied to neon, it emits an orange\/red light. It is therefore often used in brightly lit advertising signs. Georges Claude was the first person to make glass tubes of neon in 1910. He later bent the glass tubes to makes letters that glowed and produced the first neon advertising signs.<\/p>\n<p>\t\tNeon is also used in high-voltage warning indicators, in Geiger counters and in television tubes.<\/p>\n<p>\t\tLiquid neon is used as a cryogenic refrigerant. <\/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>  5 parts per billion by weight, 5 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 1,000 ppm by weight, 70 ppm by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $33 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> Neon is obtained commercially by fractional distillation of liquid air. <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Neon has 14 isotopes whose half-lives are known, with mass numbers 16 to 29. Naturally occurring neon is a mixture of its three stable isotopes and they are found in the percentages shown: <sup>20<\/sup>Ne (90.5%), <sup>21<\/sup>Ne (0.7%) and <sup>22<\/sup>Ne (9.2%).<\/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, J. Chem. Educ., 1932, 9 (10), p 1751. <\/li>\n<li>\t Morris William Travers, The Discovery of the Rare Gases, 1928, Edward Arnold and Co.<\/li>\n<li> <a href=\"\/\/news.bbc.co.uk\/1\/hi\/8201900.stm\">Room to swing a cat? Hardly<\/a> BBC Report. <\/li>\n<li>  <a href=\"\/\/www.ux1.eiu.edu\/~cfjps\/1400\/atmos_origin.html\">Origin of the Earth&#8217;s Atmosphere<\/a>.<\/li>\n<li>\t\t<a href=\"\/\/outreach.atnf.csiro.au\/education\/senior\/astrophysics\/stellarevolution_postmain.html\">Post-Main Sequence Stars<\/a>.<\/li>\n<li>\t\t   William J. Kaufman III, Universe, 1987, W. H. Freeman and Company, New York, p434. <\/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\/neon.html\"&gt;Neon&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/neon.html\"&gt;Neon 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\"Neon.\" Chemicool Periodic Table. Chemicool.com. 17 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\/neon.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 10 Ne 20.18 The chemical element neon is classed as a noble gas and a nonmetal. It was discovered in 1898 by William Ramsay and Morris Travers. Data Zone Classification: Neon is a noble gas and 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-173","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/173","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=173"}],"version-history":[{"count":22,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/173\/revisions"}],"predecessor-version":[{"id":4603,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/173\/revisions\/4603"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=173"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}