{"id":191,"date":"2012-05-22T13:06:16","date_gmt":"2012-05-22T13:06:16","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=191"},"modified":"2017-12-07T02:07:25","modified_gmt":"2017-12-07T07:07:25","slug":"aluminum","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/aluminum.html","title":{"rendered":"Aluminum 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=\"ometalsT\">\n<div class=\"atnorT\">13<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Al<\/div>\n<div class=\"atweiT\">26.98<\/div>\n<\/div>\n<p>The chemical element aluminum is classed as an other metal. It was discovered in the 1750s by Andreas Marggraf.<\/p>\n<div style=\"clear:both;\"><\/div>\n<div class=\"adsense300\">\n<div class=\"adsense300spacer\">\n<div style=\"line-height:10px;\"><img decoding=\"async\" alt=\"\" src=\"\/\/www.chemicool.com\/ad.png\"\/><\/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=\"3265846807\"><\/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<tbody>\n<tr>\n<td class=\"elemglb\">Classification:<\/td>\n<td> Aluminum is an &#8216;other metal&#8217;   <\/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>   26.98154 g\/mol <\/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> 660.32 <sup>o<\/sup>C, 933.57 K  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td> 2466.85 <sup>o<\/sup>C, 2740.00 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>13<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>13<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>14<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,3  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>   2.702 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a3ff342c4f45\"  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-id6a3ff342c4f45\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>  9.98 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\">Hardness: <\/td>\n<td>  2.8 mohs    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.90 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 10.790 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 326 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   293.40 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  577.6 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1816.6 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2744.7 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    42.6 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> 1.61  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   8.3 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht &#8658; Al<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>   passivated   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M HCl <\/td>\n<td>  mild, &#8658;  H<sub>2<\/sub>, AlCl<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>   mild, &#8658;  H<sub>2<\/sub>, [Al(OH)<sub>4<\/sub>]<sup>&#8211;<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td>  Al<sub>2<\/sub>O<sub>3<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>    AlH<sub>3<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  AlCl<sub>3<\/sub> &amp; Al<sub>2<\/sub>Cl<sub>6<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  125 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> 53.5 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> 237 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  37.6676 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> 660.32 <sup>o<\/sup>C, 933.57 K  <\/td>\n<\/tr>\n<\/table>\n<\/div><\/div>\n<div style=\"padding:0 0 0 16px;\">\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-louis-de-morveau-balloon.jpg\" width=\"300\" height=\"446\" alt=\"Louis de Morveau and balloon.\" class=\"size-full\" \/><p class=\"wp-caption-text\">Louis de Morveau believed a new metal could be discovered in the oxide alumina. He was right, but he was unable to isolate it. De Morveau devised the first systematic method of naming chemicals, and, as we can see, he was a pioneering balloonist.<br \/><\/p><\/div>\n<p><strong>Aluminum&#8217;s Periodic Table<br \/> Neighborhood<\/strong><\/p>\n<table class=\"navbar\">\n<tr>\n<td class=\"info\"><\/td>\n<td class=\"info\">Group<br \/>2 or 12<\/td>\n<td class=\"info\">Group<br \/> 13<\/td>\n<td class=\"info\">Group<br \/> 14<\/td>\n<\/tr>\n<tr>\n<td class=\"info\">2<\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/beryllium.html\" title=\"beryllium \"><sup>4<\/sup><br \/>Be<\/a> <\/td>\n<td><a class=\"metalloid\" href=\"https:\/\/www.chemicool.com\/elements\/boron.html\" title=\"boron \"><sup>5<\/sup><br \/>B<\/a> <\/td>\n<td><a class=\"onm\" href=\"https:\/\/www.chemicool.com\/elements\/carbon.html\" title=\"carbon \"><sup>6<\/sup><br \/>C<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">3<\/td>\n<td><a class=\"alkalie\" href=\"https:\/\/www.chemicool.com\/elements\/magnesium.html\" title=\"magnesium \"><sup>12<\/sup><br \/>Mg<\/a> <\/td>\n<td><a class=\"ometals\" href=\"https:\/\/www.chemicool.com\/elements\/aluminum.html\" title=\"aluminum \"><sup>13<\/sup><br \/>Al<\/a> <\/td>\n<td><a class=\"metalloid\" href=\"https:\/\/www.chemicool.com\/elements\/silicon.html\" title=\"silicon \"><sup>14<\/sup><br \/>Si<\/a> <\/td>\n<\/tr>\n<tr>\n<td class=\"info\">4<\/td>\n<td><a class=\"tmetals\" href=\"https:\/\/www.chemicool.com\/elements\/zinc.html\" title=\"zinc \"><sup>30<\/sup><br \/>Zn<\/a> <\/td>\n<td><a class=\"ometals-liquid\" href=\"https:\/\/www.chemicool.com\/elements\/gallium.html\" title=\"gallium \"><sup>31<\/sup><br \/>Ga<\/a> <\/td>\n<td><a class=\"metalloid\" href=\"https:\/\/www.chemicool.com\/elements\/germanium.html\" title=\"germanium \"><sup>32<\/sup><br \/>Ge<\/a> <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Aluminum<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    People have used alum since ancient times for dyeing, tanning and to stop bleeding.  Alum is potassium aluminum sulfate.<\/p>\n<p>\t\tIn the 1750s German chemist Andreas Marggraf found he could use an alkali solution to precipitate a new substance from alum. Marggraf had previously been the first person to isolate <a href=\"\/elements\/zinc.html\">zinc<\/a> in 1746.<\/p>\n<p>\t\tThe substance Marggraf obtained from alum was named alumina by French chemist Louis de Morveau in 1760. We now know that alumina is aluminum oxide &#8211; chemical formula Al<sub>2<\/sub>O<sub>3<\/sub>.<\/p>\n<p>\t\tDe Morveau believed alumina contained a new metallic element, but, like Marggraf, he was unable to extract this metal from its oxide. <sup>(1), (2)<\/sup><\/p>\n<p>\t\tIn 1807 or 1808, English chemist Humphry Davy decomposed alumina in an electric arc to obtain a metal. The metal was not pure aluminum, but an alloy of aluminum and <a href=\"\/elements\/iron.html\">iron<\/a>.<\/p>\n<p>\t\tDavy called the new metal alumium, then renamed it aluminum. <sup>(3)<\/sup><\/p>\n<p>\t\tAluminum was first isolated in 1825 by Hans Christian &#216;rsted (Oersted) in Copenhagen, Denmark who reported, &#8220;a lump of metal which in color and luster somewhat resembles <a href=\"\/elements\/tin.html\">tin<\/a>.&#8221;<\/p>\n<p>\t\t&#216;rsted produced aluminum by reducing aluminum chloride using a potassium-mercury amalgam. The <a href=\"\/elements\/mercury.html\">mercury<\/a> was removed by heating to leave aluminum. <\/p>\n<p>\t\tGerman chemist Friedrich W&#246;hler (Woehler) repeated &#216;rsted&#8217;s experiment but found it yielded only <a href=\"\/elements\/potassium.html\">potassium<\/a> metal. W&#246;hler developed the  method further two years later, reacting volatalized aluminum trichloride with potassium to produce small amounts of aluminum. <sup>(1)<\/sup><\/p>\n<p>\t\tIn 1856 Berzelius stated that it was W&#246;hler  who had succeeded in 1827. W&#246;hler  is therefore usually given credit for the discovery. <\/p>\n<p>\t\tMore recently, Fogh repeated the original experiments and has shown that &#216;rsted&#8217;s method can give satisfactory results. <\/p>\n<p>\t\tThis has strengthened the priority of &#216;rsted&#8217;s original work and his position as discoverer of aluminum. <sup>(4)<\/sup><\/p>\n<p>\t  For almost three decades, aluminum remained a novelty, expensive to produce and more valuable than gold, until in 1854 Henri Saint-Claire Deville in Paris, France found a way of replacing potassium with much cheaper sodium in the reaction to isolate aluminum. Aluminum then became more popular but, because it was still quite expensive, was used in ornamental rather than practical situations.<\/p>\n<p>\t  Finally, in 1886 American chemist Charles Martin Hall and French chemist Paul H&eacute;roult independently invented the Hall-H&eacute;roult process, which inexpensively isolates aluminum metal from its oxide electrolytically. <\/p>\n<p>\t\tAluminum is still manufactured using the Hall-H&eacute;roult process today.<\/p>\n<div style=\"clear: both;\"><\/div>\n<p><a id=\"facts\"><\/a><\/p>\n<h2>Interesting Facts about Aluminum<\/h2>\n<ul>\n<li>Aluminum manufacturing takes a lot of energy &#8211; 17.4 megawatt hours of electrical energy to produce one metric ton of aluminum; that&#8217;s three times more energy than is needed to make a metric ton of steel. <sup>(5)<\/sup><\/li>\n<li>Aluminum is a great metal to recycle. Recycling uses only 5% of the energy needed to produce aluminum from its ore, bauxite. <sup>(6)<\/sup> <\/li>\n<li>Aluminum does not stick to magnets under normal conditions.<\/li>\n<li>There is more aluminum in the Earth&#8217;s crust than any other metal. At about 8 percent, aluminum is the third most abundant element in our planet&#8217;s crust, behind oxygen and silicon.<\/li>\n<li>Despite its high abundance, in the 1850s aluminum was more valuable than gold. In 1852 aluminum was priced at $1200 per kg and gold was $664 per kg.<\/li>\n<li>Aluminum prices illustrate the perils of financial speculation: in 1854 Saint-Claire Deville found a way of replacing potassium with much cheaper sodium in the reaction to isolate aluminum. By 1859, aluminum was priced at $37 per kg; its price had dropped 97% in just five years.<\/li>\n<li>Where the previous item highlights the perils of speculation, this item highlights one of the triumphs of chemistry: the Hall-Heroult electrolytic process was discovered in 1886. By 1895, aluminum&#8217;s price had dropped to just $1.20 per kg.  <\/li>\n<li>Ruby gemstones are mainly aluminum oxide in which a small number of the aluminum ions have been replaced by chromium ions. <\/li>\n<li>Aluminum is made in the nuclear fires of heavy stars when a proton adds to <a href=\"\/elements\/magnesium.html\">magnesium<\/a>. (Magnesium is itself made in stars by nuclear fusion of two <a href=\"\/elements\/carbon.html\">carbons<\/a>.) <sup>(7)<\/sup> <\/li>\n<\/ul>\n<div style=\"clear: both;line-height:20px;\">&nbsp;<\/div>\n<div style=\"float:left; width:310px; margin: 0 0  0 20px;\">\n<p><img loading=\"lazy\" decoding=\"async\" alt=\"Inside Earth\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-inside-the-earth.png\" width=\"300\" height=\"184\"><\/p>\n<div style=\"width:290px;text-align:center;font-weight:400;font-size:0.7em;position:relative;top:-20px;\">Aluminum is the most abundant metal in our planet&#8217;s crust: only oxygen and silicon are more abundant. Image by USGS.\n<\/div>\n<\/div>\n<div style=\"float:left; width:310px; margin: 0 0 0 20px;\">\n<p><img loading=\"lazy\" decoding=\"async\" alt=\"Aluminum collector\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-aluminum-collector.jpg\" width=\"300\" height=\"184\"><\/p>\n<div style=\"width:290px;text-align:center;font-weight:400;font-size:0.7em;position:relative;top:-20px;\">The aluminum collector from the Genesis spacecraft. The aluminum accumulated fast moving noble gas species from the solar wind; these species impacted and stuck within the metal. The spacecraft returned to Earth and the noble gases were analyzed to learn about the origins of the Solar System. Image by <a href=\"http:\/\/genesismission.jpl.nasa.gov\/gm2\/news\/features\/wrapup.htm\">NASA\/JSC<\/a>.<\/div>\n<\/div>\n<div style=\"clear:both; line-height:20px;\">&nbsp;<\/div>\n<div class=\"adsense300\">\n<div class=\"adsense300spacer\">\n<div style=\"line-height:10px;\">\n<img decoding=\"async\" alt=\"\" src=\"\/\/www.chemicool.com\/ad.png\"\/>\n<\/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 style=\"padding:0 0 0 16px;\">\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/U8oFAJWwhnA?rel=0\" allowfullscreen><\/iframe><\/p>\n<div style=\"width:290px;font-size:12px;font-weight: 700;text-align: center;padding-bottom: 10px;position:relative;top:-16px;\">\nPouring molten aluminum.\n<\/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 \tNo proven issues; ingestion may cause alzheimer&#8217;s disease<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Aluminum is a silvery-white metal. It does not stick to magnets (it is paramagnetic and so its magnetism under normal conditions is very, very weak). It is an excellent electrical conductor. It is of low density and high ductility. It is too reactive to be commonly found as the metal although, very rarely, the native metal can be found. <sup>(8)<\/sup><\/p>\n<p>\t\tAluminum&#8217;s appearance is dulled and its reactivity is passivated by a film of aluminum oxide that naturally forms on the surface of the metal under normal conditions. The oxide film results in a material that resists corrosion. The film can be thickened using electrolysis or oxidizing agents and aluminum in this form will resist attack by dilute acids, dilute alkalis and concentrated nitric acid.<\/p>\n<p>\t\tAluminum lies sufficiently far on the right side of the  periodic table that it shows some hints of nonmetal behavior, reacting with hot alkalis to form aluminate ions [Al(OH)<sub>4<\/sub>]<sup>&#8211;<\/sup> as well as the more typical metal reaction with acids to release <a href=\"https:\/\/www.chemicool.com\/elements\/hydrogen.html\">hydrogen<\/a> gas and form the positively charged metal ion, Al<sup>3+<\/sup>. i.e. aluminum is <a href=\"https:\/\/www.chemicool.com\/definition\/amphoteric.html\">amphoteric<\/a>.<\/p>\n<p>\t\tPure aluminum is quite soft and lacking in strength. Aluminum used in commercial applications has small amounts of <a href=\"\/elements\/silicon.html\">silicon<\/a> and <a href=\"\/elements\/iron.html\">iron<\/a> (less than 1%) added, resulting in greatly improved strength and hardness.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Aluminum<\/h2>\n<p>As a result of its low density, low cost, and corrosion resistance, aluminum is widely used around the world. <\/p>\n<p>\t\tIt is used in an extensive range of products from drinks cans to window frames and boats to aircraft. A Boeing 747-400 contains 147,000 pounds (66,150 kg) of high-strength aluminum.<\/p>\n<p>\t\tUnlike some metals, aluminum has no aroma &#8211; hence its widespread use in food packaging and cooking pots.<\/p>\n<p>\t\tAlthough not quite as good as silver or copper, aluminum is an excellent electrical conductor. It is also considerably cheaper and lighter than these metals, so it is used widely in overhead power lines.<\/p>\n<p>\t\tOf all the metals, only <a href=\"\/elements\/iron.html\">iron<\/a> is used more widely than aluminum.<\/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>  8.23 % by weight,  6.32 % by moles<\/p>\n<p>\t\t\t <span class=\"elemgl\">Abundance solar system:<\/span>  56 ppm by weight, 2.7 ppm by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $15.72 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $0.20 per 100g<\/p>\n<p>\t\t\t<span class=\"elemgl\">Source:<\/span> Aluminum is the most abundant metal in the earth&#8217;s crust and the third most element in the earth&#8217;s crust, after <a href=\"https:\/\/www.chemicool.com\/elements\/oxygen.html\">oxygen<\/a> and <a href=\"https:\/\/www.chemicool.com\/elements\/silicon.html\">silicon<\/a>. Aluminum is too reactive to be found pure. Bauxite (mainly aluminum oxide) is the most important ore. <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> 15 whose half-lives are known, mass numbers 22 to 35. Of these, only two occur naturally: <sup>27<\/sup>Al, which is stable, and <sup>26<\/sup>Al, which is radioactive with half-life is 7.17 x 10<sup>5<\/sup> years. <sup>26<\/sup>Al is formed by cosmic-ray bombardment of <a href=\"https:\/\/www.chemicool.com\/elements\/argon.html\">argon<\/a> in Earth&#8217;s atmosphere.<\/p>\n<div style=\"max-width:750px;\">\n<div style=\"line-height:10px;\">\n<img decoding=\"async\" alt=\"\" src=\"\/\/www.chemicool.com\/ad.png\"\/>\n<\/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>\n<\/div>\n<p><a id=\"refer\"><\/a><\/p>\n<h4>References<\/h4>\n<ol>\n<li>Ian McNeil, Encyclopaedia of the History of Technology., (1996) p102. Routledge<\/li>\n<li>David R. Lide, CRC Handbook of Chemistry and Physics., (2007) 4-3. CRC<\/li>\n<li>Halvor Kvande, Two hundred years of aluminum &#8230; or is it aluminium?, Journal of the Minerals, Metals and Materials Society, (2008) Volume 60, Number 8: p23-24.<\/li>\n<li><a href=\"http:\/\/www.nature.com\/nature\/journal\/v135\/n3417\/abs\/135638b0.html\">http:\/\/www.nature.com\/nature\/journal\/v135\/n3417\/abs\/135638b0.html<\/a>\n\t\t\t<\/li>\n<li><a href=\"http:\/\/www.deripaska.com\/newsroom\/chinas-aluminium-foil\">China&#8217;s aluminum foil, Wall Street Journal<\/a>\n\t\t<\/li>\n<li>Paolo Ventura, Roberta Carini, Francesca D&#8217;Antona, <a href=\"http:\/\/arxiv.org\/pdf\/1105.0603v1\">A deep insight into the Mg-Al nucleosynthesis in massive AGBs and SAGB stars<\/a>., Mon. Not. R. Astron. Soc., 2002.<\/li>\n<li>Burrows et al., Chemistry<sup>3<\/sup>, (2009) Oxford University Press, p1201.<\/li>\n<li>Dekov et al., American Mineralogist., (2009) 94: p1283-1286.<\/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\/aluminum.html\"&gt;Aluminum&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/aluminum.html\"&gt;Aluminum 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\"Aluminum.\" Chemicool Periodic Table. Chemicool.com. 26 Jul. 2014. 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\/aluminum.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 13 Al 26.98 The chemical element aluminum is classed as an other metal. It was discovered in the 1750s by Andreas Marggraf. Data Zone Classification: Aluminum is an &#8216;other metal&#8217; Color: silvery Atomic weight: 26.98154 g\/mol 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-191","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/191","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=191"}],"version-history":[{"count":32,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/191\/revisions"}],"predecessor-version":[{"id":4365,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/191\/revisions\/4365"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=191"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}