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Title: Chemistry/Elements/Phosphorus - It's Elemental: Phosphorus Basic physical and historical information.
LANL__Phosphorus Properties, handling, production, and uses.

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Phosphorus Data tables and historic information.

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WebElements__Phosphorus Extensive information on history, uses, occurrence, compounds, and properties of the element.

Wikipedia__Phosphorus Properties of the element, including its history, applications, and characteristics.

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It's Elemental - The Element PhosphorusPrivacy and Security NoticeJefferson LabJefferson Lab HomeSearchContact JLabScience Education----------------------Science Education HomeTeacher ResourcesStudent ZoneGames and PuzzlesPrograms and EventsSearch EducationIt's ElementalPrevious ElementPrevious ElementTable of ElementsNext ElementNext Element 15PPhosphorus30.973762PhosphorusAtomic Number:15Atomic Weight:30.973762Melting Point:317.30 K (44.15°C or 111.47°F)Boiling Point:553.65 K (280.5°C or 536.9°F)Density:1.82 grams per cubic centimeterPhase at Room Temperature:SolidElement Classification:Non-metalPeriod Number:3Group Number:15Group Name:PnictogenWhat's in a name?From the Greek word for light bearing, phosphoros.Say what?Phosphorus is pronounced as FOS-fer-es.History and Uses:In what is perhaps the most disgusting method of discovering an element, phosphorus was first isolated in 1669 by Hennig Brand, a German physician and alchemist, by boiling, filtering and otherwise processing as many as 60 buckets of urine. Thankfully, phosphorus is now primarily obtained from phosphate rock (Ca3(PO4)2).Phosphorus has three main allotropes: white, red and black. White phosphorus is poisonous and can spontaneously ignite when it comes in contact with air. For this reason, white phosphorus must be stored under water and is usually used to produce phosphorus compounds. Red phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight. Red phosphorus is not poisonous and is not as dangerous as white phosphorus, although frictional heating is enough to change it back to white phosphorus. Red phosphorus is used in safety matches, fireworks, smoke bombs and pesticides. Black phosphorus is also formed by heating white phosphorus, but a mercury catalyst and a seed crystal of black phosphorus are required. Black phosphorus is the least reactive form of phosphorus and has no significant commercial uses.Phosphoric acid (H3PO4) is used in soft drinks and to create many phosphate compounds, such as triple superphosphate fertilizer (Ca(H2PO4)2·H2O). Trisodium phosphate (Na3PO4) is used as a cleaning agent and as a water softener. Calcium phosphate (Ca3(PO4)2) is used to make china and in the production of baking powder. Some phosphorus compounds glow in the dark or emit light in response to absorbing radiation and are used in fluorescent light bulbs and television sets.Estimated Crustal Abundance:1.05×103 milligrams per kilogramEstimated Oceanic Abundance:6×10-2 milligrams per literNumber of Stable Isotopes:1(View all isotope data)Ionization Energy:10.487 eVOxidation States:+5, +3, -3Electron Shell Configuration:1s22s22p63s23p3This page is maintained by Steve Gagnon.Citation and linking information
 

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