{"id":404,"date":"2012-05-25T10:34:00","date_gmt":"2012-05-25T10:34:00","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=404"},"modified":"2017-12-07T02:08:58","modified_gmt":"2017-12-07T07:08:58","slug":"tin","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/tin.html","title":{"rendered":"Tin 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\">50<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Sn<\/div>\n<div class=\"atweiT\">118.7 <\/div>\n<\/div>\n<p>The chemical element tin is classed as an other metal (white tin) or a nonmetal (gray tin). 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>  Tin can behave as an &#8216;other metal&#8217; (white tin)   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> <\/td>\n<td>  or a nonmetal (gray tin). <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td> silvery-white  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   118.69 <\/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> 231.928 <sup>o<\/sup>C, 505.078  K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2620 <sup>o<\/sup>C, 2893  K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>50<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>50<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>70<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,18,18,4    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>    [Kr] 4d<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  7.30 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a2444ce2fb2f\"  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-id6a2444ce2fb2f\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   16.3 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   distorted diamond   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    1.5 mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>  0.227 J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  7.029 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 302 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>    295.80 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  708.6  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>   1411.8 kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    2943 kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron affinity<\/td>\n<td>    107  kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Minimum oxidation number<\/td>\n<td>  -4    <\/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>  4  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electronegativity (Pauling Scale) <\/td>\n<td>  1.96   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   7.7  &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht &#8658; SnO<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>  mild, &#8658;  SnO<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>   mild, &#8658;   H<sub>2<\/sub>, [Sn(OH<sub>6<\/sub>)]<sup>2-<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td>  SnO , SnO<sub>2<\/sub> (stannic oxide)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   SnH<sub>4<\/sub>, Sn<sub>2<\/sub>H<sub>6<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   SnCl<sub>2<\/sub> &amp; SnCl<sub>4<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>  140.5 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\"> 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>  66.8 W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   8.7 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> 231.928 <sup>o<\/sup>C, 505.078  K    <\/td>\n<\/tr>\n<\/table>\n<\/div>\n<\/div>\n<div class=\"leftimagepadding\">\n<\/div>\n<\/div>\n<p><a id=\"discovery\"><\/a><\/p>\n<h2>Discovery of Tin<\/h2>\n<div class=\"author\">Dr. Doug Stewart<\/div>\n<p> Tin has been known since ancient times. We do not know who discovered it.<\/p>\n<p>The Bronze Age began in about 3000 BC and tin was used in bronze, which contains roughly ninety percent <a href=\"copper.html\">copper<\/a> and ten percent tin. <\/p>\n<p>The addition of tin to bronze alloys improves their properties compared with pure copper: for example, bronze is harder and more easily cast than copper. <\/p>\n<p>The ancient Greeks obtained their tin by sea-trade and referred to the source as  &#8216;The Cassiterides&#8217;, meaning Tin Islands.<\/p>\n<p>These islands were most likely to have been in Cornwall, Great Britain and\/or north-west Iberia, Spain where there are large tin deposits.<\/p>\n<p>In less ancient times, British scientist Robert Boyle published a description of his experiments on the oxidation of tin in 1673.<\/p>\n<p>Tin&#8217;s chemical symbol, Sn, comes from its Latin name, &#8216;stannum.&#8217;<\/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: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-tin-ore.jpg\" width=\"300\" height=\"160\" alt=\"Crystals of cassiterite \" class=\"size-full\" \/><p class=\"wp-caption-text\">Crystals of cassiterite &#8211; SnO<sub>2<\/sub> &#8211; tin ore (Photo by Chris Ralph)<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/sXB83Heh3_c\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Time lapse movie of tin&#8217;s allotropes. Metallic white tin becomes non-metallic gray tin. This is known as &#8216;tin pest&#8217; and is a problem at low temperatures. 1 second of movie equals one hour in real time.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"225\" src=\"https:\/\/www.youtube.com\/embed\/D26gaY6jAto\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">A piece of zinc metal in tin chloride solution. Zinc is more reactive than tin, so zinc chloride forms, replacing the tin chloride. Crystals of pure metallic tin begin to form on the zinc.<\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-tin-solder.jpg\" width=\"300\" height=\"193\" alt=\"tin solder\" class=\"size-full\" \/><p class=\"wp-caption-text\">Solder can be used to secure electronic components. Solder is usually about 60% tin and 40% lead. Here solder is being removed from a circuit board. Image by Hugo.<\/p><\/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 \tTin is considered to be non-toxic but most tin salts are toxic. The inorganic salts are caustic but of low toxicity. Organometallic compounds of tin are highly toxic.   <\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Tin is a silvery-white, soft, malleable metal that can be highly polished. <\/p>\n<p>\t\tTin has a highly crystalline structure and when a tin bar is bent, a &#8216;tin cry&#8217; is heard, due to the breaking of these crystals.<\/p>\n<p>                In compounds tin is usually in the divalent state (Sn<sup>2+<\/sup>) or tetravalent state (Sn<sup>4+<\/sup>).<\/p>\n<p>\t\tIt resists oxygen and water but dissolves in acids and bases. Exposed surfaces form an oxide film. When heated in air, tin forms tin(IV) oxide (stannic oxide) which is feebly acidic.<\/p>\n<p>\t\tTin has two allotropic forms at normal pressure, gray tin and white tin. Pure white tin slowly tends to become the gray powder (gray tin), a change commonly called &#8216;tin pest&#8217; at temperatures below 13.2 <sup>o<\/sup>C. Gray tin has no metallic properties at all. Commercial quality tins are resistant to tin pest as a result of the inhibiting effects of minor impurities.<\/p>\n<p><a id=\"uses\"><\/a><\/p>\n<h2>Uses of Tin<\/h2>\n<p>\t\t Tin is used as a coating on the surface of other metals to prevent corrosion. &#8216;Tin&#8217; cans, for example, are made of tin-coated steel.<\/p>\n<p>                 Tin can be rolled into thin foil sheets (tinfoil).  Present day \u2018tinfoil\u2019 to cover or wrap food is usually made from aluminum.<\/p>\n<p>\t\tAlloys of tin are commercially important in, for example, soft solder, pewter, bronze and phosphor bronze.<\/p>\n<p>\t\tTin chloride (stannous chloride, SnCl<sub>2<\/sub>) is used as a mordant in dyeing textiles and for increasing the weight of silk.<\/p>\n<p>\t\tStannous fluoride (SnF<sub>2<\/sub>) is used in some toothpastes.\t<\/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>  2.3 parts per million by weight,  0.4 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span>  9 parts per billion by weight, 0.1 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $24 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $1.80 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Tin very rarely occurs free in nature. The chief ore is cassiterite (SnO<sub>2<\/sub>). The metal is prepared from cassiterite by reducing the ore with coal.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Tin has 35 isotopes whose half-lives are known, mass numbers 100 to 134. Tin has ten stable isotopes, the most of any element.<\/p>\n<p>Naturally occurring tin is a mixture of its ten stable isotopes and they are found in the percentages shown: <sup>112<\/sup>Sn (1.0%), <sup>114<\/sup>Sn (0.7%), <sup>115<\/sup>Sn (0.3%), <sup>116<\/sup>Sn (14.5%), <sup>117<\/sup>Sn (7.7%), <sup>118<\/sup>Sn (24.2%), <sup>119<\/sup>Sn (8.6%), <sup>120<\/sup>Sn (32.6%), <sup>122<\/sup>Sn (4.6%) and <sup>124<\/sup>Sn (5.8%). The most abundant is <sup>120<\/sup>Sn at 32.6%.<\/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<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\/tin.html\"&gt;Tin&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/tin.html\"&gt;Tin 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\"Tin.\" Chemicool Periodic Table. Chemicool.com. 24 Jul. 2015. 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\/tin.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 50 Sn 118.7 The chemical element tin is classed as an other metal (white tin) or a nonmetal (gray tin). It has been known since ancient times. Its discoverer and discovery date are unknown. Data Zone Classification: [&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-404","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/404","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=404"}],"version-history":[{"count":23,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/404\/revisions"}],"predecessor-version":[{"id":4314,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/404\/revisions\/4314"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=404"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}