{"id":390,"date":"2012-05-25T08:46:51","date_gmt":"2012-05-25T08:46:51","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=390"},"modified":"2017-12-07T02:08:38","modified_gmt":"2017-12-07T07:08:38","slug":"silver","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/silver.html","title":{"rendered":"Silver 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\">47<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Ag<\/div>\n<div class=\"atweiT\"> 107.9<\/div>\n<\/div>\n<p>The chemical element silver is classed as 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>  Silver is a transition metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>   silver   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   107.868 <\/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> 961.95 <sup>o<\/sup>C, 1235.1 K   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2155 <sup>o<\/sup>C, 2428 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>47<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>47<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>60<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,18,1   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>  [Kr] 4d<sup>10<\/sup> 5s<sup>1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  10.5 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a480a0171c26\"  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-id6a480a0171c26\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   10.3 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>    2.5  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.235   J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 11.30 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  284   kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>   250.580 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td> 731 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   2073.5  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    3360.6 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>   125.6  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>  1  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td> 1.93   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   7.9 &Aring;<sup>3<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> mild,  &#8658;  Ag<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;  AgNO<sub>3<\/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> Ag<sub>2<\/sub>O, AgO (silver peroxide:Ag<sub>2<\/sub>O.Ag<sub>2<\/sub>O<sub>3<\/sub>) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   &#8211;  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>  AgCl  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  160 pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (1+ ion) <\/td>\n<td> 128  pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>   108  pm <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td> 89  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> 429  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  62.9 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> 961.95 <sup>o<\/sup>C, 1235.1 K   <\/td>\n<\/tr>\n<\/table>\n<\/div><\/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\/silver-field.jpg\" width=\"300\" height=\"158\" alt=\"Silver\" class=\"size-full\" \/><p class=\"wp-caption-text\">Silver nuggets found in the field &#8211; native silver.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-galena.jpg\" width=\"300\" height=\"287\" alt=\"Galena\" class=\"size-full\" \/><p class=\"wp-caption-text\">Galena (lead sulfide). Galena would have been noticed by anyone looking for metals in ancient times. Galena generally contains silver, sometimes in significant quantities. Image: 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 Silver<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p>Silver has been in use since prehistoric times. We do not know who discovered it, although the discovery would almost certainly have been of native silver. <\/p>\n<p>Nuggets of native silver metal can be found in minerals and sometimes in rivers; but they are rare. Despite native silver&#8217;s rarity, very large pieces of it have been found, such as those found in the early 1900s in Northern Ontario, Canada described as &#8220;pieces of native silver as big as stove lids and cannon balls.&#8221; <sup>(1)<\/sup><\/p>\n<p>\t\tSilver has a special place in the history of the elements because it is one of the first five metals discovered and used by humans. The others were <a href=\"gold.html\">gold<\/a>, <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a>, <a href=\"lead.html\">lead<\/a> and <a href=\"iron.html\">iron<\/a>. <\/p>\n<p>    Silver objects dating from before 4000 BC have been found in Greece and from slightly later in Anatolia (in modern Turkey). Silver artifacts have been found in the Sumerian city of Kish dating from about 3000 BC. <sup>(2), (3), (4)<\/sup><\/p>\n<p>     Silver and lead often appear together in nature, for example in the mineral galena which is mainly lead sulfide. Galena actually looks metallic (see image) and would have caught the eyes of people looking for metals.<\/p>\n<p>\t\tThe silver objects found in Greece, Turkey and Kish were made of silver that was refined from lead-containing ores such as galena. (Humans have been successful chemists for a surprisingly long time.) <\/p>\n<p>    First the ore was smelted under reducing conditions to obtain a mixture of silver and lead. The metals then went through cupellation: the metals were heated to about 1000  <sup>o<\/sup>C in a strong stream of air. Under these conditions lead reacts with oxygen forming lead oxide, leaving liquid silver metal floating on top. <sup>(3), (4)<\/sup><\/p>\n<p>\t\tOur name for the element is derived from the Anglo-Saxon for silver, &#8216;seolfor,&#8217; which itself comes from ancient Germanic &#8216;silabar.&#8217;<\/p>\n<p>\t\tSilver&#8217;s chemical symbol, Ag, is an abbreviation of the Latin word for silver, &#8216;argentum.&#8217; The Latin word originates from argunas, a Sanskrit word meaning shining. <sup>(5)<\/sup><\/p>\n<p>\t\tThe historical association between silver and money is still found in some languages. The French word for silver is argent, and the same word is used for money. The Romans used the word &#8216;argentarius&#8217; to mean banker (silver trader). <sup>(6)<\/sup>\t<\/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<p><iframe loading=\"lazy\" width=\"300\" height=\"168\" src=\"https:\/\/www.youtube.com\/embed\/aPnx1GHskAY\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Silver tarnishes quickly in sulfur dioxide released from a boiled egg, then the tarnish is instantly removed using electrochemistry.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"168\" src=\"https:\/\/www.youtube.com\/embed\/8e0-AbwBDYM\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A demonstration of basic photography using silver chloride.<\/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 Silver is considered to be non-toxic. However, most silver salts are poisonous and some may be carcinogenic.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Silver is a soft, ductile, malleable, lustrous metal. It has the highest electrical and thermal conductivity of all metals.<\/p>\n<p>\t\tSilver is stable in oxygen and water, but tarnishes when exposed to sulfur compounds in air or water to form a black sulfide layer. <\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of  Silver<\/h2>\n<p>\t\tSterling silver (an alloy of 92.5% silver and 7.5% copper) or Britannia silver (an alloy of 95.8% silver and 4.2% copper) are used for jewelry and silverware.<\/p>\n<p>\t\tSilver is used as a food additive\/coloring and is given the E number E174.<\/p>\n<p>\t\tAbout 30% of silver produced is used in the photographic industry, mostly as silver nitrate.<\/p>\n<p>\t\tSilver is used in solders, electrical contacts, and silver-cadmium and silver-zinc batteries. Silver paints are used in the manufacture of electronic printed circuits.<\/p>\n<p>\t\tIt is used in superior mirror production, as silver is the best known reflector of visible light, although it does tarnish over time.<\/p>\n<p>\t\tSilver iodide is used in artificial rain making to seed clouds.<\/p>\n<p>\t\tSilver compounds were used successfully to prevent infection in World War 1.  <\/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>  75 parts per billion by weight, 20 parts per billion by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 1 part per billion by weight,  10 parts per trillion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $120 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $57.5 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Silver is found in elemental form and also in various ores such as argentite (silver sulfide, Ag<sub>2<\/sub>S) and horn silver (silver chloride, AgCl). Commercially, the main sources of silver are <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a>, copper-nickel, gold, lead, and lead-zinc ores. Silver is extracted from the anode waste sludges of electrolytic copper-refining.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Silver has 35 isotopes whose half-lives are known, with mass numbers 94 to 128. Naturally occurring silver is a mixture of its two stable isotopes, <sup>107<\/sup>Ag and <sup>109<\/sup>Ag with natural abundances of 51.8% and 48.2% 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> Charles Dumaresq, <a href=\"http:\/\/www.cobaltmininglegacy.ca\/mininghistory.php\">The Rise and Fall of a Mining Camp<\/a>., Cobalt Mining Legacy.\t\t<\/li>\n<li> Barbara S. Ottaway and Ben Roberts, <a href=\"http:\/\/books.google.com\/books?id=bQMxOC66jvsC&#038;printsec=frontcover&#038;source=gbs_ge_summary_r&#038;cad=0#v=onepage&#038;q&#038;f=false\">The Emergence of Metalworking<\/a>., Prehistoric Europe: Theory and Practice edited by Andrew Jones, 2008,  p208, Wiley-Blackwell.<\/li>\n<li> Hadi Ozbal, <a href=\"http:\/\/www.transanatolie.com\/english\/turkey\/Turkey%20PDF\/SOMP-05-Research-Ancient%20Metallurg-Ozbal.pdf\">Ancient Anatolian Metallurgy<\/a>., 2001. (pdf download)<\/li>\n<li> <a href=\"http:\/\/history-world.org\/mesopotamia_9000.htm\">Mesopotamia<\/a>, The International History Project, 2003.<\/li>\n<li>Vivi Ringnes, Origin of the Names of Chemical Elements., J. Chem. Educ., 1989, 66 (9), p731.<\/li>\n<li>Thomas Patrick Mohide, <a href=\"http:\/\/books.google.com\/books?id=XZ6Vs_vpJCIC&#038;printsec=frontcover&#038;source=gbs_ge_summary_r&#038;cad=0#v=onepage&#038;q&#038;f=false\">The International Silver Trade<\/a>., 1992, p2, Woodhead Publishing.<\/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\/silver.html\"&gt;Silver&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/silver.html\"&gt;Silver 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\"Silver.\" Chemicool Periodic Table. Chemicool.com. 09 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\/silver.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 47 Ag 107.9 The chemical element silver is classed as transition metal. It has been known since ancient times. Its discoverer and discovery date are unknown. Data Zone Classification: Silver is a transition metal Color: silver Atomic [&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-390","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/390","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=390"}],"version-history":[{"count":22,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/390\/revisions"}],"predecessor-version":[{"id":4615,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/390\/revisions\/4615"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=390"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}