{"id":1127,"date":"2019-12-03T13:34:33","date_gmt":"2019-12-03T13:34:33","guid":{"rendered":"http:\/\/chemdictionary.org\/?p=1127"},"modified":"2019-12-03T13:34:39","modified_gmt":"2019-12-03T13:34:39","slug":"aluminium","status":"publish","type":"post","link":"https:\/\/chemdictionary.org\/aluminium\/","title":{"rendered":"Aluminium"},"content":{"rendered":"\n<h2>Introduction<\/h2>\n\n\n\n<p>Aluminium is a light weight metal with silvery white appearance <strong>[1]. <\/strong>It is denoted by symbol \u201cAl\u201d. In Purest form, the aluminium metal\nis bluish- white in colour.<\/p>\n\n\n\n<h2>Position in Periodic table <\/h2>\n\n\n\n<p>It belongs to group 13 of the periodic table. This group has 3 electrons in their outermost shell. Elements of this group including aluminum are metallic in nature. Among all elements, Boron and aluminum have greater commercial value than others in the same group [2]. <\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter\"><img loading=\"lazy\" width=\"460\" height=\"321\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-10.png\" alt=\"\" class=\"wp-image-1128\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-10.png 460w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-10-300x209.png 300w\" sizes=\"(max-width: 460px) 100vw, 460px\" \/><\/figure><\/div>\n\n\n\n<h2>Periodic table information <\/h2>\n\n\n\n<ul><li><strong>Atomic number<\/strong><\/li><\/ul>\n\n\n\n<p>Atomic number of aluminium is 13.<\/p>\n\n\n\n<ul><li><strong>Atomic weight <\/strong><\/li><\/ul>\n\n\n\n<p>Atomic weight of aluminium is 26.98\namu.<\/p>\n\n\n\n<ul><li><strong>Electronic configuration <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium\nhas 13 electrons and 14 neutrons. The proton number is also 13. The electron configuration for Aluminum is 1s<sup>2<\/sup>2s<sup>2<\/sup>2p<sup>6<\/sup>3s<sup>2<\/sup>3p<sup>1<\/sup>.\n&nbsp;Aluminium has 3 electrons in valence\nshell [3] [6]. <\/p>\n\n\n\n<ul><li><strong>Oxidation states <\/strong><\/li><\/ul>\n\n\n\n<p>Three oxidation states of aluminium\nare +3, +1 and+2. In compound Al<sub>2<\/sub> O<sub>3, <\/sub>Aluminium has\noxidationstate of +3 [4].<\/p>\n\n\n\n<ul><li><strong>Occurrence<\/strong> <\/li><\/ul>\n\n\n\n<p>Aluminium rarely\noccurs free in nature. Mostly, it binds with oxygen to form Alumina. This bound\nform of aluminium is present in nature. However it is among most abundant\nmetals on earth. It is usually present in Bauxite and Cryolite form. These are\nbasically Aluminium Silicates [5]. More forms of aluminium present in nature\nare Micas, Feldspar, Vermiculite, Gibbsite, garnet and emerald. <\/p>\n\n\n\n<ul><li><strong>Earth crust:<\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium is third most occurred metal\npresent in earth crust. It covers almost 7% to 8 % of earth\u2019s crust [<strong>7] [8].<\/strong><\/p>\n\n\n\n<ul><li><strong>Discovery: <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium was\nalready being used by ancient Greeks and Romans and was given name alumina. It\nwas further discovered and called as \u201calum\u201d <strong>[9].<\/strong> Davy identified its\nexistence but it was not successfully isolated by him. <\/p>\n\n\n\n<ul><li><strong>Nomenclature: <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminum is given this name from a word of Latin origin \u201cAlumen or alum\u201d.\nGuyton de Morveau gave it name \u201calumina\u201d in 1761. After that, it was given name\n\u201cAlumium\u201d by Humphrey Davy in 1807. After some time, he renamed\nit as \u201cAluminum\u201d <strong>[10]. <\/strong>After some time conforming with named of a lot of other elements, it was\nrenamed as Aluminium. This name was further adopted by IUPAC and is still used\nall over the world except in North America. So both spellings \u201cAluminum\u201d and \u201cAluminium\u201d\nare considered correct in periodic table.<\/p>\n\n\n\n<ul><li><strong>Extraction of aluminium:<\/strong><\/li><\/ul>\n\n\n\n<p>It was first isolated by Hans Oersted in 1825. He heated and mixed anhydrous\nAlumnium Chloride with potassium amalgam to get minute quantity of aluminium. <\/p>\n\n\n\n<p>It was then isolated in 1827 by Fredrick Wohler. &nbsp;He heated and mixed Aluminium chloride with\npotassium in a platinum container to obtain Aluminium. <\/p>\n\n\n\n<p>Bauxite is the substance having greater amount of naturally occurring Alumnium\nand impurities present in bauxite can be removed from aluminium. &nbsp;90 % of bauxite is used for aluminium production.\nBauxite is hydrated oxide of aluminium. Impurities present in bauxite are\nsilica, ferric oxide and clay. Bauxite is used for extraction of aluminium <strong>[11]. <\/strong>It is a complicated process. When this process is performed at industrial\nscale, it gives maximum yield of aluminium.<\/p>\n\n\n\n<p>Karl Josef Bayer (Austria) in 1888 patented the method to produce aluminum and the process known as Bayer process. Another process was invented in 1886 by Charles Martin Hall and Paul Louis Toussaint H\u00e9roult and the process known as \u201cHall-Herolt Process\u201d.Bauxite is first dissolved in molten sodium hydroxide at 1200 \u00baC and is then precipitated with carbon dioxide after that, it is dissolved in cryolite at 950 \u00baC and electrolyzed by Bayer process [12].<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter\"><img loading=\"lazy\" width=\"328\" height=\"241\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-11.png\" alt=\"\" class=\"wp-image-1129\" srcset=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-11.png 328w, https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-11-300x220.png 300w\" sizes=\"(max-width: 328px) 100vw, 328px\" \/><\/figure><\/div>\n\n\n\n<h2>Chemical properties [13].<\/h2>\n\n\n\n<ul><li><strong>Reaction with air:<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium don\u2019t necessarily react with oxygen in air due to the presence\nof a protective oxide coating on metal surface. Still, if some surface remains\nunprotected, then it will react with oxygen giving aluminium oxide as product. <\/p>\n\n\n\n<p><strong>4Al (s) + 3O<sub>2 <\/sub>(l) \u2192 2Al<sub>2<\/sub>O<sub>3<\/sub>(s)<\/strong><\/p>\n\n\n\n<ul><li><strong>Reaction with acids<\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium is rapidly dissolved in concentrated\nhydrochloric acid.<\/p>\n\n\n\n<p><strong>2Al(s)\n+ 3H<sub>2<\/sub>SO<sub>4<\/sub>(aq) \u2192 2Al<sup>3+<\/sup>(aq) + 2SO<sub>4<\/sub><sup>2-<\/sup>(aq)\n+ 3H<sub>2<\/sub>(g)<\/strong><\/p>\n\n\n\n<ul><li><strong>Reaction with Halogens:<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium\nmetal reacts with halogens to form halides. This is usually vigorous reaction.<\/p>\n\n\n\n<p><strong>2Al(s) + 3Cl<sub>2<\/sub>(l) \u2192 2AlCl<sub>3<\/sub>(s)<\/strong><\/p>\n\n\n\n<ul><li><strong>Reaction with bases:<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium\nreacts with bases by following reactions.<\/p>\n\n\n\n<p><strong>2Al(s) + 2NaOH(aq) + 6H<sub>2<\/sub>O\n\u2192 2Na<sup>+<\/sup>(aq) + 2[Al(OH)<sub>4<\/sub>]<sup>&#8211;<\/sup>&nbsp;+ 3H<sub>2<\/sub>(g)<\/strong><\/p>\n\n\n\n<h2>Physical properties [14]<\/h2>\n\n\n\n<ul><li><strong>Density<\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium\nhas a density of 2.7 g\/cm<sup>3<\/sup><\/p>\n\n\n\n<ul><li><strong>Melting point <\/strong><\/li><\/ul>\n\n\n\n<p>It has melting\npoint of 660 degree Celsius.<\/p>\n\n\n\n<ul><li><strong>Boiling point <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium has\nboiling point of 2470 degree Celsius.<\/p>\n\n\n\n<ul><li><strong>Isotopes<\/strong>:<\/li><\/ul>\n\n\n\n<p>Alumnium has around 22 isotopes. Among these isotopes <sup>27 <\/sup>Al is\nstable. <\/p>\n\n\n\n<ul><li><strong>Crystal\nstructure<\/strong><\/li><\/ul>\n\n\n\n<p>Solid Aluminium has crystal structure of face centre cube.<\/p>\n\n\n\n<ul><li><strong>Specific\ngravity <\/strong><\/li><\/ul>\n\n\n\n<p>Specific gravity of aluminium is 2.7.<\/p>\n\n\n\n<ul><li><strong>Light weight<\/strong><\/li><\/ul>\n\n\n\n<p>Atomic weight of aluminium is 26.9. <\/p>\n\n\n\n<ul><li><strong>Corrosion resistance:<\/strong><\/li><\/ul>\n\n\n\n<p>Self protecting and coating process helps aluminium to attain maximum\ncorrosion resistance. <\/p>\n\n\n\n<ul><li><strong>Electrical conductivity <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium is excellent\nconductor of electricity. This is the reason it in found in various wirings. Especially\nit is used for long distance transmission of electricity. The electrical\nconductivity of aluminium is about twice of the copper <strong>[15].<\/strong><\/p>\n\n\n\n<ul><li><strong>Thermal\nconductivity<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium has relatively higher thermal conductibbity. There is about 50%\n-60% of increased conductivity in aluminium a compared to that of copper.<\/p>\n\n\n\n<ul><li><strong>Reflectivity :<\/strong><\/li><\/ul>\n\n\n\n<p>The reflective\nnature of aluminium with other alloys make it upcoming good source for mirror\npolishing.<\/p>\n\n\n\n<ul><li><strong>Ductility: <\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium in\nits purest form is very ductile. This is reason it cannot be used in purest\nform for construction purpose. Addition of silicon or iron makes it perfect for\nuse as building material.<\/p>\n\n\n\n<ul><li><strong>Impermeable:<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium inform of sheets is totally impermeable to heat and light, which\nmakes its good option for food storage and transportation.<\/p>\n\n\n\n<ul><li><strong>Recycling:<\/strong><\/li><\/ul>\n\n\n\n<p>Materials made up of aluminium can be easily\nrecycles to yield aluminium back. This recycling loop makes it good source\nmaterial to be used in everyday life [16]. <\/p>\n\n\n\n<h2>Alloys of aluminium:<\/h2>\n\n\n\n<p>When any element or group of elements are added to Alumnium in order to improve the physical properties, then they are known as alloys of Alumnium. &nbsp;Aluminium is usually used in alloy form as pure aluminium is not strong. For this purpose, some alloys are produced to improve the strength of aluminium products but keeping in mind that light weight nature of metal remains same. Some alloys are shown in table below:<\/p>\n\n\n\n<div class=\"wp-block-image\"><figure class=\"aligncenter\"><img loading=\"lazy\" width=\"274\" height=\"250\" src=\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/11\/image-12.png\" alt=\"\" class=\"wp-image-1130\"\/><\/figure><\/div>\n\n\n\n<h2>Uses of aluminium <\/h2>\n\n\n\n<p>Physical properties of aluminium\nmake it possible to be used in variety of purposes. Some of these uses make it\nreally important in our everyday life <strong>[17].<\/strong><\/p>\n\n\n\n<ul><li><strong>Utensils<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium is a good conductor of heat and\nlight in weight. These two qualities make it a good choice for kitchen utensils\n[18].<\/p>\n\n\n\n<ul><li><strong>House materials<\/strong><\/li><\/ul>\n\n\n\n<p>House building materials such as windows are made up of Alumnium.<\/p>\n\n\n\n<ul><li><strong>Automotive industry <\/strong><\/li><\/ul>\n\n\n\n<p>From last many years, aluminium has been used in automotive\nindustries. Major applications in this field includes: Auto body, chassis and\nother structural components. Light weight vehicles made up of aluminium parts,\nwith maximum corrosion resistance can help reducing fuel consumption. It is\neasier to clean this metal and that\u2019s reason it is used in automotive industry.\nNo surface protection is required if aluminium is used.<\/p>\n\n\n\n<ul><li><strong>Marine applications <\/strong><\/li><\/ul>\n\n\n\n<p>With the\nadvancement in aluminium industry and with invention of new aluminium alloys,\nit has now been used in marine applications. This is due to the fact, aluminium\nhas higher corrosion resistance. So, for marine travel, this quality is of much\nimportance, along with being light in weight [19].<\/p>\n\n\n\n<ul><li><strong>Food packaging<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium\nis being used in food packaging such as cans and in aluminium foil for kitchen\nuse. <\/p>\n\n\n\n<ul><li><strong>Sporting goods<\/strong><\/li><\/ul>\n\n\n\n<p>Some sport\nequipments are nowadays made up of aluminium. Example is: Golf carts and bicycles.<\/p>\n\n\n\n<ul><li><strong>Furniture<\/strong><\/li><\/ul>\n\n\n\n<p>Some\nfurniture such as beds is also made up of aluminium. <\/p>\n\n\n\n<ul><li><strong>In Drugs<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium\nin form of aluminium hydroxide is used as antacid drugs.<\/p>\n\n\n\n<ul><li><strong>Printing plates<\/strong><\/li><\/ul>\n\n\n\n<p>Alumnium\nin form of thin sheets is used for printing plates.<\/p>\n\n\n\n<ul><li><strong>Paper Making<\/strong><\/li><\/ul>\n\n\n\n<p>Aluminium Sulphate has been used in\npaper industry. Paper manufacturers use it as binder of dyes and glues.<\/p>\n\n\n\n<ul><li><strong>Nano technology<\/strong><\/li><\/ul>\n\n\n\n<p>Anodic aluminium oxide (AAO) is compound of aluminium with\nreally great properties. It has a unique structure which makes it available to\nbe used in nanotechnology. <\/p>\n\n\n\n<ul><li><strong>Aviation industry:<\/strong><\/li><\/ul>\n\n\n\n<p>Wright brother, while discovering the\nfirst aeroplane, also used aluminium as major component of aircraft engine.\nThis is due to its light weight property. Nowadays due to its favourable\nphysical properties, it has been extensively used in aviation industry.\nAluminium, when interacts with oxygen, makes a protective coating which prevent\nmetal from corrosion.<\/p>\n\n\n\n<p>Alumnium is\nwidely used metal. It has a great number of applications depending upon its\nphysical and chemical properties.<\/p>\n\n\n\n<h4>REFERENCES<\/h4>\n\n\n\n<ol><li>https:\/\/www.britannica.com\/science\/aluminum<strong>https:\/\/rsc.org\/periodic-table\/element\/13\/aluminiumhttps:\/\/www.saburchill.com\/chemistry\/visual\/atoms\/013.htmlhttps:\/\/chem.libretexts.org\/Bookshelves\/Inorganic_Chemistry\/Supplemental_Moduleshttp:\/\/science.marshall.edu\/castella\/chm448\/elements1.pdf(Inorganic_Chemistry)\/Descriptive_Chemistry\/Elements_Organized_by_Block\/2_pBlock_Elements\/Group_13%3A_The_Boron_Family\/Z%3D013_Chemistry_of_Aluminum_(Z%3D13)www.aalco.co.ukRoesky,\nHerbert &amp; Kumar, Shravan. (2005). Chemistry of Aluminum (I). Chemical\ncommunications (Cambridge, England). 32. 4027-38. 10.1039\/b505307b.<a href=\"https:\/\/en.wikipedia.org\/wiki\/Louis-Bernard_Guyton_de_Morveau\">Guyton de Morveau, L. B.<\/a>&nbsp;(1782), &#8220;M\u00e9moire sur les d\u00e9nominations chimiques, la\nnecessit\u00e9 d&#8217;en perfectionner le syst\u00e8me et les r\u00e8gles pour y\nparvenir&#8221;,&nbsp;Observations sur la Physique,&nbsp;19: 370\u2013382<em>.<\/em><em><\/em>Sir Humphry Davy. Elements of\nchemical Philosophy. Part 1. Volume 1 (1812) https:\/\/chem.libretexts.org\/Bookshelves\/Inorganic_Chemistry\/Supplemental_Modules_(Inorganic_Chemistry)\/Descriptive_Chemistry\/Elements_Organized_by_Block\/2_p\nBlock_Elements\/Group_13%3A_The_Boron_Family\/Z%3D013_Chemistry_of_Aluminum_(Z%3D13)\/Aluminium_Metallurgy<a href=\"https:\/\/www.sciencedirect.com\/science\/article\/pii\/B9781845696542500031\">Production of primary aluminium<\/a> H.&nbsp;Kvande, in&nbsp;<a href=\"https:\/\/www.sciencedirect.com\/book\/9781845696542\">Fundamentals of Aluminium Metallurgy<\/a>, 2011https:\/\/www.webelements.com\/aluminium\/chemistry.htmlhttps:\/\/www.asminternational.org\/documents\/10192\/1849770\/06787G_Sample.pdf\nhttps:\/\/www.thoughtco.com\/aluminum-or-aluminium-3980635Corrosion of Aluminum and Aluminum Alloys (#06787G)\nEditor(s): J.R. Davishttps:\/\/www.aluminum.org\/industries\/production\/recyclingm. j. freir\u00eda g\u00e1ndara: aluminium: the metal of choice.\nmateriali in tehnologije \/ materials and technology 47 (2013) 3, 261\u2013265 https:\/\/aluminiuminsider.com\/aluminium-alloys-in-shipbuilding-a-fast-growing-trend\/https:\/\/opportunitymuse.com\/5-benefits-using-aluminum-cookware.https:\/\/www.azom.com\/article.aspx?ArticleID=4193<\/strong><\/li><\/ol>\n","protected":false},"excerpt":{"rendered":"<p>Introduction Aluminium is a light weight metal with silvery white appearance [1]. It is denoted by symbol \u201cAl\u201d. In Purest form, the aluminium metal is bluish- white in colour. Position in Periodic table It belongs to group 13 of the periodic table. This group has 3 electrons in their outermost shell. Elements of this group &#8230; <a title=\"Aluminium\" class=\"read-more\" href=\"https:\/\/chemdictionary.org\/aluminium\/\" aria-label=\"More on Aluminium\">Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[1],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":0,"star_result":0,"total_max_option_value":5,"adjusted_score_result":0,"score_result":0,"percentage_result":0,"adjusted_percentage_result":0,"count":0,"post_id":1127}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1127"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=1127"}],"version-history":[{"count":5,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1127\/revisions"}],"predecessor-version":[{"id":1316,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/1127\/revisions\/1316"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=1127"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=1127"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=1127"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}