{"id":273,"date":"2012-05-23T10:40:17","date_gmt":"2012-05-23T10:40:17","guid":{"rendered":"http:\/\/www.chemicool.com\/elements\/?page_id=273"},"modified":"2017-12-07T02:08:08","modified_gmt":"2017-12-07T07:08:08","slug":"manganese","status":"publish","type":"page","link":"https:\/\/www.chemicool.com\/elements\/manganese.html","title":{"rendered":"Manganese 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\">25<\/div>\n<div class=\"clearT\"><\/div>\n<div class=\"elnamT\">Mn<\/div>\n<div class=\"atweiT\"> 54.93 <\/div>\n<\/div>\n<p>The chemical element manganese is classed as a transition metal. It was first recognized as a distinct chemical element in 1740.<\/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><br \/>\n<a id=\"data\"><\/a>\t<\/p>\n<h2>Data Zone<\/h2>\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Classification:<\/td>\n<td>  transition metal   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Color:<\/td>\n<td>  gray-white  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic weight:<\/td>\n<td>   54.9380 <\/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> 1250 <sup>o<\/sup>C, 1523 K    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Boiling point:<\/td>\n<td>  2060 <sup>o<\/sup>C, 2333 K     <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electrons:<\/td>\n<td>25<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Protons:<\/td>\n<td>25<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Neutrons in most abundant isotope:<\/td>\n<td>30<\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron shells:<\/td>\n<td>   2,8,13,2   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Electron configuration:<\/td>\n<td>   [Ar] 3d<sup>5<\/sup> 4s<sup>2<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Density @ 20<sup>o<\/sup>C:<\/td>\n<td>  7.43 g\/cm<sup>3<\/sup>   <\/td>\n<\/tr>\n<\/table>\n<span class=\"collapseomatic \" id=\"id6a5726bebc874\"  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-id6a5726bebc874\" class=\"collapseomatic_content \">\n<table class=\"datatop\">\n<tr>\n<td class=\"elemglb\">Atomic volume:<\/td>\n<td>   7.4 cm<sup>3<\/sup>\/mol  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Structure:<\/td>\n<td>   complex (cubic) <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Hardness: <\/td>\n<td>    6.0  mohs  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Specific heat capacity<\/td>\n<td>   0.48   J g<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of fusion<\/td>\n<td>  12.91 kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of atomization<\/td>\n<td>  283    kJ mol<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Heat of vaporization<\/td>\n<td>  219.74  kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">1<sup>st<\/sup> ionization energy<\/td>\n<td>  717.4  kJ mol<sup>-1<\/sup>    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">2<sup>nd<\/sup> ionization energy<\/td>\n<td>  1509  kJ mol<sup>-1<\/sup>   <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">3<sup>rd<\/sup> ionization energy<\/td>\n<td>  3248.3  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>  -3    <\/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> 7 <\/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> 1.55    <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Polarizability volume <\/td>\n<td>    9.4 &Aring;<sup>3<\/sup>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Reaction with air<\/td>\n<td>  mild, w\/ht  &#8658;  \tMn<sub>3<\/sub>O<sub>4<\/sub>, Mn<sub>3<\/sub>N<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; Mn(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>, MnCl<sub>2<\/sub>\t <\/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> MnO, Mn<sub>3<\/sub>O<sub>4<\/sub>,  Mn<sub>2<\/sub>O<sub>3<\/sub>, Mn<sub>2<\/sub>O<sub>7<\/sub>  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Hydride(s) <\/td>\n<td>   None  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Chloride(s) <\/td>\n<td>   MnCl<sub>2<\/sub> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Atomic radius <\/td>\n<td>   140 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>   89  pm  <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\">Ionic radius (3+ ion) <\/td>\n<td>  75.3  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>  7.81  W m<sup>-1<\/sup> K<sup>-1<\/sup> <\/td>\n<\/tr>\n<tr>\n<td class=\"elemglb\"> Electrical conductivity <\/td>\n<td>   0.5 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> 1250 <sup>o<\/sup>C, 1523 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:\/\/www.chemicool.com\/elements\/images\/300-manganese-ores.jpg\" width=\"300\" height=\"108\" alt=\"Manganese Ores\" class=\"size-full\" \/><p class=\"wp-caption-text\">Manganese Ores: Rhodochrosite (manganese carbonate) on left: pink Mn<sup>2+<\/sup>. Pyrolusite (manganese dioxide) on right: black Mn<sup>4+<\/sup>.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-manganese-green-plant.jpg\" width=\"300\" height=\"213\" alt=\"Green leaves\" class=\"size-full\" \/><p class=\"wp-caption-text\">Without manganese, this picture would not exist. In fact, there would be no advanced life forms on our planet.  Manganese is essential for photosynthesis.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-manganese-black-smokers.jpg\" width=\"300\" height=\"169\" alt=\"Black Smokers on Ocean Floor\" class=\"size-full\" \/><p class=\"wp-caption-text\">Manganese dioxide makes the black color in black smokers &#8211; hot geothermal vents on the ocean floor. Image courtesy: NASA.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/chemicool.com\/elements\/images\/300-manganese-lascaux.jpg\" width=\"300\" height=\"167\" alt=\"Cave paintings manganese dioxide\" class=\"size-full\" \/><p class=\"wp-caption-text\">Cave paintings, 16,000 years old, in Lascaux, France. The black color was made by our ancestors using manganese dioxide.<\/p><\/div>\n<\/div>\n<\/div>\n<p>\t\t\t<a id=\"discovery\"><\/a>\t<\/p>\n<h2>Discovery of Manganese<\/h2>\n<div class=\"author\">Author: Dr. Doug Stewart<\/div>\n<p>Manganese compounds have been used since ancient times.<\/p>\n<p>\t\tIn the first century AD, Pliny the Elder, the Roman author, described how black powder (manganese dioxide) was used to manufacture colorless glass. <sup>(1)<\/sup> It is still used for the same purpose today.<\/p>\n<p>\t\tThe first recognition of manganese&#8217;s existence as a distinct element was in 1740, when the German chemist Johann Heinrich Pott stated that pyrolusite (manganese dioxide) contained a new earth metal.  Until then pyrolusite was believed to have been a compound of <a href=\"\/elements\/iron.html\">iron<\/a>.  <\/p>\n<p>\t\tPott prepared potassium manganate by fusing caustic potash (potassium hydroxide) with pyrolusite in air.<\/p>\n<p>\t\tThe color changes he observed in the product were green\/blue\/red\/green, establishing that pyrolusite did not contain iron. <sup>(2),(2.1),(3)<\/sup> <\/p>\n<p>\t\tDetails of the first isolation of metallic manganese were published in 1770 by Ignatius Gottfried Kaim in a dissertation under the supervision of the chemist Jakab Jozsef Winterl. <\/p>\n<p>    Working in Vienna, Kaim mixed powdered pyrolusite with twice its weight of black flux and heated the mixture strongly.  The composition of Kaim&#8217;s flux is uncertain, although it was probably based on charcoal. (A flux is a reducing agent.) If so, the reaction would have been:<\/p>\n<p>\t  MnO<sub>2<\/sub> + C &nbsp; &#8594; &nbsp;  Mn + CO<sub>2<\/sub><\/p>\n<p>   Kaim described the product of the reaction as a blue-whitish shiny brittle metal with many differently shaped facets.  When broken and viewed side-on, he observed blue flecks. <\/p>\n<p>\t Kaim claimed that no iron was present in his product, but he was aware his manganese was not pure. <\/p>\n<p>\t He invited other chemists to find a flux that could produce the pure metal. <sup> (4), (5)<\/sup><\/p>\n<p>\tIn Sweden, Carl Wilhelm Scheele &#8211; the discoverer of <a href=\"\/elements\/chlorine.html\">chlorine<\/a> and one of <a href=\"\/elements\/oxygen.html\">oxygen<\/a>&#8216;s independent discoverers &#8211; was aware that pyrolusite contained a new element. His attempts to isolate it failed and he asked his friend Johan Gottlieb Gahn to try.<\/p>\n<p>  Gahn used a similar method to the one Kaim had used a few years earlier, with charcoal as the reducing agent. Gahn used a blowpipe to increase the temperature of the reaction.<\/p>\n<p>\tThe metal he produced was white, hard and brittle; when broken it had a granular structure. Gahn&#8217;s manganese was also impure, but the new metallic element now gained widespread recognition.  <sup> (2)<\/sup><\/p>\n<p>\t\tManganese&#8217;s name comes from the use of its compounds in glass-making. These compounds were called &#8216;magnes&#8217; in Latin, meaning &#8216;magnet.&#8217;  <sup> (6)<\/sup><\/p>\n<p>\tManganese is not actually magnetic!<\/p>\n<h2 class=\"headingt\">Interesting Facts about Manganese<\/h2>\n<ul>\n<li>\n\tManganese is an essential element in photosynthesis. Without it, there would be no free oxygen on earth.\n\t<\/li>\n<li>\n\tHuman bodies contain a tiny amount of manganese: about 10 &#8211; 20 mg. If you chopped a 10c coin into 100 equal pieces, each piece would weigh more than the weight of manganese in an average human. Despite this, we cannot survive without it; manganese performs vital metabolic functions.\n\t <\/li>\n<li>\n\tManganese in humans needs to be topped up frequently because our bodies cannot store it.\n\t<\/li>\n<li>\n\tNeanderthals may have used black manganese dioxide as a cosmetic 50 000 years ago. <sup>(7),(8)<\/sup>\n\t<\/li>\n<\/ul>\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 class=\"leftimagepadding\">\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-color-wheel.png\" width=\"300\" height=\"302\" alt=\"Color Wheel\" class=\"size-full\" \/><p class=\"wp-caption-text\">Colors on opposite sides of the color wheel cancel.<\/p><\/div>\n<div style=\"width: 310px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/www.chemicool.com\/elements\/images\/300-manganese-cans.jpg\" width=\"300\" height=\"209\" alt=\"Aluminum cans with manganese\" class=\"size-full\" \/><p class=\"wp-caption-text\">Ever wondered how drink cans can be so thin? Manganese stiffens aluminum, so less of it is needed to make soft drink cans.<\/p><\/div>\n<p><iframe loading=\"lazy\" width=\"300\" height=\"233\" src=\"https:\/\/www.youtube.com\/embed\/jRQserZYXbI\" allowfullscreen><\/iframe><\/p>\n<div class=\"youtubecaption\">Transition metals are well-known for their multiple colored ions. Watch the changes in color as manganese changes its oxidation state from +7 to +6 to +4.<\/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 \tExcess manganese, particularly inhalation of the powder\/dust, is toxic. Exposure to manganese or  manganese oxide(s) dust  can result in a medical condition called manganism; symptoms resemble those of Parkinson&#8217;s disease. Workers at particular risk of exposure include miners and welders.<\/p>\n<p>\t  <strong>Characteristics:<\/strong><\/p>\n<p>\t\t Manganese is a gray-white, hard, brittle, metal that can take a high polish. It is not magnetic. The metal tarnishes on exposure to air and, when heated, oxidizes to manganese(II, III) oxide (Mn<sub>3<\/sub>O<sub>4<\/sub>).<\/p>\n<p>\t\tLike other transition metals, manganese has more than one common oxidation state. The most stable is +2, which is a pale pink color in aqueous solutions. Also important is +4, brown\/black, which is found in manganese dioxide; and +7 found in the purple permanganate anion MnO<sub>4<\/sub><sup>&#8211;<\/sup>. Manganese&#8217;s +6 oxidation state is green.<\/p>\n<p>\t\t<a id=\"uses\"><\/a><\/p>\n<h2>Uses of Manganese<\/h2>\n<p>\t\tFor over 2000 years manganese dioxide has been used to make colorless glass. Glass is made from sand (silica) and most sand contains iron (II) oxide, which naturally gives glass a green color. It is sometimes incorrectly stated that the manganese dioxide oxidizes the iron (II) oxide to iron (III) oxide; with a corresponding color change from intense green to pale yellow &#8211; and the pale yellow is too faint to be seen.<\/p>\n<p>\t\tIn fact, the real reason the glass decolorizes is complementary colors. Colors that are directly opposite one another on the color wheel (image: left) cancel one another out, to leave a pale gray.<\/p>\n<p>\t\tIn glass the manganese dioxide forms a violet silicate which cancels the green color of Iron (II). <sup>(9)<\/sup><\/p>\n<p>\t\tManganese dioxide is also used as a black-brown pigment in paint and as a filler in dry cell batteries.<\/p>\n<p>\t\tThe great majority of manganese ore ends up in steel production where the manganese desulfurizes and deoxidizes the steel.  <\/p>\n<p>\t\tIt is also is used extensively to produce a variety of important alloys. For example, the <a href=\"\/elements\/aluminum.html\">aluminum<\/a> used to make most soft drinks cans contains about 1% manganese to improve the cans&#8217; stiffness and corrosion resistance.<\/p>\n<p>\t\tOrgano-manganese compounds can be added to gasoline to increase its octane rating and reduce engine knock. <\/p>\n<p>\t\tManganese is the twelfth most abundant element in the earth&#8217;s crust and it is an essential trace element for all life on earth.<\/p>\n<p>\t\tIn the human body several manganese-containing enzymes are need to metabolize carbohydrates, cholesterol, and amino acids. Typically our bodies have about 10 &#8211; 20 mg manganese. This needs to be topped up frequently because our bodies cannot store it. About a quarter of the manganese in our bodies is in bone, while the rest is evenly distributed through our tissues. <sup>(10)<\/sup> <\/p>\n<p>\t\t\t<a id=\"abund\"><\/a><\/p>\n<h2>Abundance and Isotopes<\/h2>\n<p><span class=\"elemgl\">Abundance earth&#8217;s crust:<\/span>  0.1% by weight, 360 parts per million by moles<\/p>\n<p>\t\t<span class=\"elemgl\">Abundance solar system:<\/span> 10 parts per million by weight,  0.2 parts per million by moles<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, pure:<\/span>  $6.5 100g<\/p>\n<p>\t\t\t\t<span class=\"elemgl\">Cost, bulk:<\/span>  $0.28 per 100g<\/p>\n<p>\t\t<span class=\"elemgl\">Source:<\/span> Manganese occurs mainly as the mineral pyrolusite (MnO<sub>2<\/sub>) and as rhodochrosite (MnCO<sub>3<\/sub>). Manganese can be found in manganese nodules on the ocean floor, but these are currently commercially unviable. Commercially, manganese is produced by reduction of its ores using aluminum.  High purity manganese is made by electrolysis of manganese sulfate in solution.<\/p>\n<p>\t\t<span class=\"elemgl\">Isotopes:<\/span> Manganese has 21 isotopes whose half-lives are known, with mass numbers 46 to 66. Naturally occurring manganese consists of its one stable isotope, <sup>55<\/sup>Mn. <\/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>\t\t<a id=\"refer\"><\/a><\/p>\n<h4>References<\/h4>\n<ol>\n<li>S. Venetskii, Metal from black stone., Metallurgist, 1 July 1966, Vol 10, Issue 7, p423-425.<\/li>\n<li>Mary Elvira Weeks, The discovery of the elements. III. Some eighteenth-century metals., J. Chem. Educ., 1932, 9 (1), p22.  2b. Mary Elvira Weeks, The discovery of the elements., 1960, Sixth Edition, p169-173, Journal of Chemical Education.<\/li>\n<li>Leopold Gmelin, <a href=\"http:\/\/books.google.com\/books?pg=PA882&#038;id=96M5AAAAcAAJ#v=onepage&#038;q&#038;f=false\">Handbuch der Theoretischen Chemie<\/a>., 1827, Vol. 1, Part 2, p882.<\/li>\n<li>\t    Peter Joseph Macquers,  <a href=\"http:\/\/gdz.sub.uni-goettingen.de\/dms\/load\/img\/?PPN=PPN346192188\">Chymisches W&#246;rterbuch oder Allgemeine Begriffe der Chymie nach Alphabetischer Ordnung<\/a>, 1788, p572-573.<\/li>\n<li>            J.C. Wiegleb, <a href=\"http:\/\/books.google.com\/books?id=lL05AAAAcAAJ&#038;lpg=PA439&#038;ots=ybQxXZrsi4&#038;dq\">Geschichte des Wachsthums und der Erfindungen in der Chemie in der neuern Zeit<\/a>, Zweyter Band von 1750 bis 1790., 1791, p104.<\/li>\n<li>             Saul S. Hauben, The derivations of the names of the elements, J. Chem. Educ., 1933, 10 (4), p227.  <\/li>\n<li>\t\t\t\t\t\t  Winfried Henke, Thorolf Hardt, <a href=\"http:\/\/books.google.com\/books?id=vhoRdbTrjc8C&#038;pg=PA1733#v=onepage&#038;q&#038;f=false\">Handbook of Paleoanthropology<\/a>, 2007, Volume 1, p1733, Springer.<\/li>\n<li>\t\t\t\t\t\t   BBC Report,  <a href=\"http:\/\/news.bbc.co.uk\/1\/hi\/sci\/tech\/8448660.stm\">Neanderthal &#8216;make-up&#8217; containers discovered<\/a> 9 January 2010.<\/li>\n<li>\t\t\t\t\t\t     David Dingledy, Decolorization of glass., J. Chem. Educ., 1965, 42 (3), p160.<\/li>\n<li>\t\t\t\t\t\t\t\t    J. S. Garrow, W.P.T. James, A Ralph, <a href=\"http:\/\/books.google.com\/books?id=a-pSOMMaoaUC&#038;pg=PA202\">Human nutrition and dietetics<\/a>., 2000, p202, Churchill Livingstone. <\/li>\n<\/ol>\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\/manganese.html\"&gt;Manganese&lt;\/a&gt;\r\n<\/pre>\n<p>or<\/p>\n<pre class='code'>\r\n&lt;a href=\"https:\/\/www.chemicool.com\/elements\/manganese.html\"&gt;Manganese 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\"Manganese.\" Chemicool Periodic Table. Chemicool.com. 07 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\/manganese.html&gt;.<\/pre>\n","protected":false},"excerpt":{"rendered":"<p>Data Zone | Discovery | Facts | Appearance &amp; Characteristics | Uses | Abundance &amp; Isotopes | References 25 Mn 54.93 The chemical element manganese is classed as a transition metal. It was first recognized as a distinct chemical element in 1740. Data Zone Classification: transition metal Color: gray-white Atomic weight: 54.9380 State: solid Melting [&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-273","1":"page","2":"type-page","3":"status-publish","5":"entry"},"_links":{"self":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/273","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=273"}],"version-history":[{"count":50,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/273\/revisions"}],"predecessor-version":[{"id":3419,"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/pages\/273\/revisions\/3419"}],"wp:attachment":[{"href":"https:\/\/www.chemicool.com\/elements\/wp-json\/wp\/v2\/media?parent=273"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}