{"id":321,"date":"2012-05-23T14:46:06","date_gmt":"2012-05-23T14:46:06","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=321"},"modified":"2017-12-07T02:08:58","modified_gmt":"2017-12-07T07:08:58","slug":"zinc","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/zinc.html","title":{"rendered":"Zinc 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\">30<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Zn<\/div>\n<div class=\"atweiT\"> 65.41  <\/div>\n<\/div>\n<p>The chemical element zinc 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;\">\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=\"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<tr>\n<td class=\"elemglb\">Classification:<\/td>\n<td>  Zinc is a transition metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  bluish silver    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>  65.41 <\/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> 419.53 <sup>o<\/sup>C, 692.68 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  910 <sup>o<\/sup>C, 1183 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>30<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>30<\/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>    2,8,18,2    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>  [Ar] 3d<sup>10<\/sup> 4s<sup>2<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  7.14  g\/cm<sup>3<\/sup>  <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a3124d609699\"  tabindex=\"0\" title=\"Show more: Heats, Energies, Oxidation,&lt;br \/&gt; Reactions, Compounds, Radii, Conductivities\"    >Show more: Heats, Energies, Oxidation,<br \/> Reactions, Compounds, Radii, Conductivities<\/span><div id=\"target-id6a3124d609699\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   9.2 cm<sup>3<\/sup>\/mol   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   hcp: hexagonal close packed   <\/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>   0.39    J g<sup>-1<\/sup> K<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td> 7.322 kJ mol<sup>-1<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td> 131  kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  115.30  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  906.4 kJ mol<sup>-1<\/sup>>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1733.2 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>    3832.6 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> 2 <\/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> 1.65  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>   6.4 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td> vigorous,  &#8658;  ZnO    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 15 M HNO<sub>3<\/sub> <\/td>\n<td>   vigorous,  &#8658; Zn(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>  mild,  &#8658;  H<sub>2<\/sub>, ZnCl<sub>2<\/sub>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with 6 M NaOH <\/td>\n<td>  mild,  &#8658; [Zn(OH<sub>4<\/sub>)]<sup>2-<\/sup>, H<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Oxide(s) <\/td>\n<td> ZnO, ZnO<sub>2<\/sub> (zinc peroxide)  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>    ZnH<sub>2<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td> ZnCl<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> &#8211; <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (2+ ion) <\/td>\n<td>  88  pm  <\/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>  116  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>  16.9 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> 419.53 <sup>o<\/sup>C, 692.68 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-zinc-batteries.jpg\" width=\"300\" height=\"178\" alt=\"zinc batteries\" class=\"size-full\" \/><p class=\"wp-caption-text\">Batteries &#8211; the outside of these batteries is made of zinc &#8211; zinc acts as both battery electrode and container.<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"182\" src=\"https:\/\/www.youtube.com\/embed\/AowDcxRnwmE\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Zinc reacts very vigorously with sulfur. Here&#8217;s a test firing of a sulfur\/zinc rocket.<\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/xT9V7Y1iKYc\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Reaction of zinc with iodine.<\/div>\n<\/div>\n<\/div>\n<p>\t\t\t<a id=\"discovery\"><\/a>\t<\/p>\n<h2>Discovery of Zinc<\/h2>\n<p>   Zinc ores have been used to make brass (a mixture of <a href=\"https:\/\/www.chemicool.com\/elements\/copper.html\">copper<\/a> and zinc) and other alloys since ancient times.<\/p>\n<p>\t\t A zinc alloy comprising 87.5% zinc was discovered in an ancient site in Transylvania.<\/p>\n<p>\t\t Zinc smelting began in the 12th century in India by reducing calamine (zinc carbonate, ZnCO<sub>3<\/sub>) with wool and other organic materials.<\/p>\n<p>\t\t The element name is reported to come from the old German word &#8216;zinke&#8217; meaning pointed; a reference to the sharp pointed crystals formed after smelting.<\/p>\n<p>\t\t Credit for isolating the metal is usually given to Andreas Marggraf in 1746, in Berlin. He heated a mixture of calamine ore and carbon in a closed vessel without copper to produce the metal.<\/p>\n<p>     <a id=\"appear\"><\/a><\/p>\n<h3>Appearance and Characteristics<\/h3>\n<p>\t   <strong>Harmful effects:<\/strong> <\/p>\n<p>\t \tZinc is not considered to be particularly toxic.<\/p>\n<p>\t\tZinc is essential for good health, but excess zinc is toxic and can cause nausea.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\tZinc is a bluish-silver, lustrous metal that tarnishes in moist air, producing a layer of carbonate. It is somewhat brittle at room temperature but malleable above 100 <sup>o<\/sup>C.<\/p>\n<p>\t\tZinc reacts with both acids and alkalis.<\/p>\n<p>\t\tIt is a fair conductor of electricity, and burns in air with a bright bluish-green flame producing white clouds of the oxide.  <\/p>\n<p>\t\t<a id=\"uses\"><\/a><\/p>\n<h2>Uses of Zinc<\/h2>\n<p>\t\tZinc is used to galvanize <a href=\"https:\/\/www.chemicool.com\/elements\/iron.html\">iron<\/a> to inhibit corrosion.<\/p>\n<p>\t  Zinc forms many alloys with other metals such as brass, German silver, nickel silver, typewriter metal and solders. Zinc alloys are used in die-castings for the car industry.<\/p>\n<p>\t\tThe metal acts as both the container and as an electrode in zinc-carbon batteries. The drawback of this dual use is that the electrode is consumed when the battery is in use, getting thinner until eventually the battery starts leaking.<\/p>\n<p>\t\tZinc is an <a href=\"https:\/\/www.chemicool.com\/elements\/foods-high-in-zinc.html\">essential trace element<\/a> for animals and plants.<\/p>\n<p>\t\tZinc oxide, a white powder, is a versatile compound that has many uses.<\/p>\n<p>It is used in sun block, make-up and in ointments such as calamine lotion. <\/p>\n<p>It is also used in the rubber industry, concrete manufacturing and in paints.<\/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>  70 parts per million by weight, 22 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 2 part per million by weight,  30 parts per billion by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $5.30 per 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $0.18 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Zinc is found in nature combined with other elements as ores. The main ores of zinc are sphalerite (sulfide), smithsonite (carbonate), hemimorphite (silicate), and franklinite (zinc, manganese, iron oxide).<\/p>\n<p>\t\t Commercially, zinc is obtained from zinc sulfide minerals. The minerals are concentrated and then usually roasted to oxidize the zinc sulfide to zinc oxide. Zinc is then extracted by either large-scale electroplating (electrowinning) or by pyrometallurgy, where processing reduces zinc oxide with carbon or carbon monoxide at 950 <sup>o<\/sup>C into the metal.\t  <\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Zinc has 25 isotopes whose half-lives are known, with mass numbers 57 to 83. Naturally occurring zinc is a mixture of five isotopes and they are found in the percentages shown: <sup>64<\/sup>Zn (48.6%), <sup>66<\/sup>Zn (27.9%), <sup>67<\/sup>Zn (4.1%), <sup>68<\/sup>Zn (18.8%) and <sup>70<\/sup>Zn (0.6%).  Over 48.6% of naturally occurring zinc is in the form of <sup>64<\/sup>Zn.\t  <\/p>\n<div style=\"clear:both;line-height:2px;\">&nbsp;<\/div>\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>\t\t<a id=\"refer\"><\/a><\/p>\n<h4>References<\/h4>\n<p><a id=\"Cite\"><\/a><\/p>\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\/zinc.html\"&gt;Zinc&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/zinc.html\"&gt;Zinc 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\"Zinc.\" Chemicool Periodic Table. Chemicool.com. 18 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\/zinc.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 30 Zn 65.41 The chemical element zinc is classed as a transition metal. It has been known since ancient times. Its discoverer and discovery date are unknown. Data Zone Classification: Zinc is a transition metal Color: bluish [&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-321","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/321","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=321"}],"version-history":[{"count":19,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/321\/revisions"}],"predecessor-version":[{"id":3174,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/321\/revisions\/3174"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=321"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}