{"id":309,"date":"2012-05-23T14:17:00","date_gmt":"2012-05-23T14:17:00","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=309"},"modified":"2017-12-07T02:07:40","modified_gmt":"2017-12-07T07:07:40","slug":"copper","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/copper.html","title":{"rendered":"Copper 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\">29<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Cu<\/div>\n<div class=\"atweiT\"> 63.55<\/div>\n<\/div>\n<p>The chemical element copper is classed as a transition metal. It has been known since ancient times. Its discoverer and discovery date are unknown.<\/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>  Copper is a transition metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  orange-red  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   63.546 <\/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> 1084.62 <sup>o<\/sup>C, 1357.77 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2560 <sup>o<\/sup>C, 2833 K      <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>29<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>29<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>34<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>    2,8,18,1   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>  [Ar] 3d<sup>10<\/sup> 4s<sup>1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  8.96  g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2f4fe2c9a3a\"  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-id6a2f4fe2c9a3a\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   7.1 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>    3.0  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.38   J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 13.050 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 338  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  300.30 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  745.4 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1957.9 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  3553.5 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   118.5   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> 4 <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Max. common oxidation no. <\/td>\n<td>  2  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 1.95  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   6.7 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht &#8658;  CuO, Cu<sub>2<\/sub>O  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td> mild,  &#8658; Cu(NO<sub>3<\/sub>)<sub>2<\/sub>, NO<sub>x<\/sub>  <\/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>  &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td>  CuO, Cu<sub>2<\/sub>O (cuprite) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   CuH  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td> CuCl, CuCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td> 135 pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (1+ ion) <\/td>\n<td> 91  pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>  87  pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 68  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>  401  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   60.7 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> 1084.62 <sup>o<\/sup>C, 1357.77 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-copper-native.jpg\" width=\"300\" height=\"162\" alt=\"Native Copper\" class=\"size-full\" \/><p class=\"wp-caption-text\">A nugget of natural, native copper with imbedded copper minerals<\/p><\/div>\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Copper<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>    Of all the metals, copper is the one most likely to be found in its native state, often released by the chemical reaction of its ores. <\/p>\n<p>\t\tAlthough only small amounts of native copper can be found, there was enough of it for our ancestors to discover the metal and begin using it.<\/p>\n<p>\t\tCopper has been used by humans for as many as ten thousand years. Beads made from native copper dating from the eighth millennium BC have been found in Turkey. <sup>(1)<\/sup><\/p>\n<p>    Crucibles and slags found in Europe suggest that smelting of copper (producing the metal from its ores) took place in the fifth millennium BC. <\/p>\n<p>\t\tCopper mining and smelting were commonplace by 4500 BC in the Balkans &#8211; Bulgaria, Greece, Serbia and Turkey. <sup>(2), (3) <\/sup><\/p>\n<p>\t\tThe Copper Age sits between the Neolithic (Stone) and Bronze Ages. It took place at different times in different cultures, when people began using copper tools alongside stone tools.<\/p>\n<p>\t\tThe Copper Age was followed by the Bronze Age, when people learned that by adding <a href=\"tin.html\">tin<\/a> to copper, a harder metal that is also more easily cast was formed. Again this happened at different times in different locations in the world.<\/p>\n<p>\t\t  The word copper is derived from the Latin word &#8216;cuprum&#8217; meaning &#8216;metal of Cyprus&#8217; because the Mediterranean island of Cyprus was an ancient source of mined copper. <\/p>\n<p>\t\t\tThe element symbol Cu also comes from &#8216;cuprum.&#8217; <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<div style=\"width: 370px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/copper-sulfate.jpg\" width=\"360\" height=\"250\" alt=\"copper sulfate crystals\" class=\"size-full\" \/><p class=\"wp-caption-text\">Growing copper sulfate crystals is cool &#8211; chemicool in fact.<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/RKuEBKUU1sA\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Copper compounds burn with a distinctive green flame. This is copper (I) chloride.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/MRw91oBy2xs\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Copper metal is extracted from an acidic solution of copper nitrate.<\/div>\n<div style=\"width: 370px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/copper-verdigris.jpg\" width=\"360\" height=\"200\" alt=\"verdigris\" class=\"size-full\" \/><p class=\"wp-caption-text\">Verdigris (corroded copper) on rooftop decorations.<\/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 \tCopper is essential in all plants and animals. Excess copper is, however, toxic.<\/p>\n<p>\t\tCooking acidic food in copper pots can cause toxicity. Copper cookware should be lined to prevent ingestion of toxic verdigris (compounds formed when copper corrodes). \t <\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t  Copper is a reddish orange, soft metal that takes on a bright metallic luster.<\/p>\n<p>\t\tIt is malleable, ductile, and an excellent conductor of heat and electricity &#8211; only silver has a higher electrical conductivity than copper.<\/p>\n<p>\t\tCopper surfaces exposed to air gradually tarnish to a dull, brownish color.<\/p>\n<p>\t\tIf water and air are present, copper will slowly corrode to form the carbonate verdigris often seen on roofs and statues.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Copper<\/h2>\n<p>\t\tAs a result of its excellent electrical conductivity, copper&#8217;s most common use is in electrical equipment such as wiring and motors.<\/p>\n<p>\t\tBecause it corrodes slowly, copper is used in roofing, guttering, and as rainspouts on buildings.<\/p>\n<p>\t\tIt is also used in plumbing and in cookware and cooking utensils. <\/p>\n<p>\t\tCommercially important alloys such as brass and bronze are made with copper and other metals.<\/p>\n<p>\t\tGun metals and American coins are copper alloys.<\/p>\n<p>\t\tCopper sulfate is used as a fungicide and as an algicide in rivers, lakes and ponds.<\/p>\n<p>\t\tCopper oxide in Fehling&#8217;s solution is widely used in tests for the presence of monosaccharides (simple sugars).   <\/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>  60 parts per million by weight, 19 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 700 parts per billion by weight,  10 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>   $9.76 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $0.66 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Copper is occasionally found native (i.e. as the uncombined metal), and is also found in many minerals such as the oxide; cuprite (Cu<sub>2<\/sub>O), the carbonates; malachite (Cu<sub>2<\/sub>CO<sub>3<\/sub>(OH)<sub>2<\/sub>)and azurite (Cu<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>2<\/sub>(OH)<sub>2<\/sub>) and the sulfides; chalcopyrite (CuFeS<sub>2<\/sub>) and bornite (Cu<sub>5<\/sub>FeS<sub>4<\/sub>).<\/p>\n<p>\t\t Most copper ore is mined or extracted as copper sulfides. Copper is then obtained by smelting and leaching. Finally, the resulting crude copper is purified by electrolysis involving plating onto pure copper cathodes. <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span>  Copper has 24 isotopes whose half-lives are known, with mass numbers 57 to 80. Naturally occurring copper is a mixture of its two stable isotopes, <sup>63<\/sup>Cu and <sup>65<\/sup>Cu, with natural abundances of 69.2% and 30.8% respectively.  <\/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>Andrew Jones, <a href=\"http:\/\/books.google.com\/books?id=bQMxOC66jvsC&#038;printsec=frontcover&#038;dq=Prehistoric+Europe:+theory+and+practice+By+Andrew+Jones&#038;cd=1#v=onepage&#038;q&#038;f=false\">Prehistoric Europe: Theory and Practice<\/a>., 2008, p195. Blackwell Publishing. <\/li>\n<li>Douglass Whitfield Bailey, Balkan Prehistory: Exclusion, Incorporation and Identity, 2000, p210.  Routledge.<\/li>\n<li>Sarunas Milisauskas, European Prehistory., 2003, p207.  Kluwer Academic\/Plenum.<\/li>\n<li>Saul S. Hauben, The derivations of the names of the elements, J. Chem. Educ., 1933, 10 (4), p227. <\/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\/copper.html\"&gt;Copper&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\"&gt;Copper 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\"Copper.\" 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\/copper.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 29 Cu 63.55 The chemical element copper is classed as a transition metal. It has been known since ancient times. Its discoverer and discovery date are unknown. Data Zone Classification: Copper is a transition metal Color: orange-red [&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-309","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/309","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=309"}],"version-history":[{"count":25,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/309\/revisions"}],"predecessor-version":[{"id":4594,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/309\/revisions\/4594"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=309"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}