Element 15 | Article about Element 15 by The Free Dictionary Element 15 | Article about Element 15 by The Free Dictionary Related to Element 15: Element 115 , Element 14 , Element 16 , Element 25 phosphorus (fŏs`fərəs) [Gr.,=light-bearing], nonmetallic chemical element; symbol P; at. no. 15; at. wt. 30.97376; m.p. 44.1&degC;; b.p. about 280&degC;; sp. gr. 1.82 at 20&degC;; valence −3, +3, or +5. Solid phosphorus has a tetratomic molecule (P4) with molecular weight 123.8952 atomic mass units (amu). Phosphorus was discovered c.1674 by Hennig Brand of Hamburg, an alchemist, who prepared it from urine. Phosphoric acid was discovered in 1770 by K. W. Scheele and J. G.

Gahn in bone ash (see ash ash, in chemistry, solid residue of combustion. The chemical composition of an ash depends on that of the substance burned. Wood ash contains metal carbonates (e.g., potassium carbonate) and oxides formed from metals originally compounded in the wood. ..... Click the link for more information. ); Scheele later isolated phosphorus from bone ash (1774) and produced phosphoric acid by the action of nitric acid on phosphorus (1777). Forms Phosphorus exhibits allotropy allotropy [Gr.,=other form]. A chemical element is said to exhibit allotropy when it occurs in two or more forms in the same physical state; the forms are called allotropes. ..... Click the link for more information. (i.e., it has multiple forms in the same physical state); the physical constants given above are for the common white phosphorus. White phosphorus is an extremely poisonous, yellow to white, waxy, solid substance, nearly insoluble in water but very soluble in carbon disulfide. When exposed to air it ignites spontaneously, burning to form white fumes of phosphorus pentoxide, P2O5.

Because of its toxicity and pyrophoric nature, phosphorus is stored underwater. Contact with the skin may cause burns. White phosphorus is phosphorescent (i.e., glows without emitting heat). When white phosphorus is heated to about 250&degC; in the absence of air, it changes into the more stable red phosphorus. This form appears as dull, reddish-brown cubic crystals or amorphous powder. Its specific gravity is 2.34. The red form is less dangerous than the white form, but should be handled with caution. It is insoluble in carbon disulfide and most other solvents. It does not ignite unless heated to about 200&degC;, does not phosphoresce, and is not poisonous. Another form of phosphorus is black phosphorus, a crystalline electrically conductive material similar to graphite in appearance. It was first prepared by P. W. Bridgman by heating white phosphorus to 200&degC; under a pressure of 12,000 atmospheres. Its specific gravity is 2.70.

Natural Occurrence and Commercial Preparation Because of its chemical activity phosphorus does not occur uncombined in nature but is widely distributed in many minerals. A major source is apatite apatite , mineral, a phosphate of calcium containing chlorine or fluorine, or both, that is transparent to opaque in shades of green, brown, yellow, white, red, and purple. Apatite is a minor constituent in igneous and metamorphic rocks. ..... Click the link for more information. , an impure calcium phosphate mineral found in phosphate rocks. In the United States major deposits are found in Florida, Tennessee, Montana, and Idaho. White phosphorus is prepared commercially from phosphate rock in an electric furnace or blast furnace. The principal use of phosphorus is in compounds; for this reason, most of the phosphorus produced in furnaces is burned to make phosphorus pentoxide, a white powdery substance. While the pentoxide is used as a drying agent and chemical reagent, it is chiefly converted to phosphoric acid phosphoric acid, any one of three chemical compounds made up of phosphorus, oxygen, and hydrogen (see acids and bases). The most common, orthophosphoric acid, H3PO4, is usually simply called phosphoric acid.

..... Click the link for more information. , H3PO4, also called orthophosphoric acid, by reaction with water. Another important source of phosphoric acid is from phosphate rocks by treatment with sulfuric acid; this is the so-called wet-acid process. Biological Importance and Applications Phosphorus is present in plants and animals. There is over 1 lb (454 grams) of phosphorus in the human body. It is a component of adenosine triphosphate adenosine triphosphate (ATP) , organic compound composed of adenine, the sugar ribose, and three phosphate groups. ATP serves as the major energy source within the cell to drive a number of biological processes such as photosynthesis, muscle contraction, and the synthesis of ..... Click the link for more information. (ATP), a fundamental energy source in living things. It is found in complex organic compounds in the blood, muscles, and nerves, and in calcium phosphate, the principal material in bones and teeth. Phosphorus compounds are essential in the diet. Organic phosphates, ferric phosphate, and tricalcium phosphate are added to foods. Dicalcium phosphate is added to animal feeds.

White phosphorus is used as a deoxidizing agent in the preparation of steel and phosphor bronze. It is also used in rat poisons and to make smoke screens (by burning) for warfare. Red phosphorus is used in making matches. The major use of phosphorus compounds is in fertilizers, especially in a mixture called superphosphate, obtained from phosphate minerals by sulfuric acid treatment; and in nitrophosphates. Phosphorus compounds are also used commercially in detergents, water softeners, pharmaceuticals, dentifrices, and in many other less important uses. Toxic nerve gases such as sarin contain phosphorus. Phosphoric acid is primarily used in the production of phosphate phosphate, salt or ester of phosphoric acid, H3PO4. Because phosphoric acid is tribasic (having three replaceable hydrogen atoms), it forms monophosphate, diphosphate, and triphosphate salts in which one, two, or three of the hydrogens of the acid are ..... Click the link for more information. compounds. It is also used in pickling metals, in sugar refining, and in soft drinks.

Phosphorus forms a number of compounds with the halogens, e.g., the trichloride, PCl3, and the pentachloride, PCl5, both used as reagents. It also forms an oxychloride, POCl3. It reacts with sulfur to form a pentasulfide, P2S5, and a thiochloride, PSCl3, used in insecticides and oil additives. Phosphine, PH3, is a poisonous gas. Besides the pentoxide, phosphorus forms several other oxides; there are several acids other than the orthophosphoric acid noted above. Phosphorus also combines with various other nonmetals and with some metals. Phosphorus P, a chemical element of group V of Mendeleev’s periodic system; a nonmetal. Atomic number, 15; atomic weight, 30.97376.

Phosphorus occurs naturally only as the stable isotope 31P; six artificial radioisotopes have been obtained, namely 28P (half-life, 6.27 sec), 29P (4.45 sec), 30P (2.55 min), 32P (14.22 days), 33P (25 days), and 34P (12.5 sec). The isotope 32P is the most valuable; the energy associated with beta radiation is significant, and the isotope is used in both chemical and biological research as a tracer. History. According to some sources, a method of preparing phosphorus was known as early as the 12th century by Arab alchemists. However, the generally accepted date for the discovery of the element is 1669, when H. Brand (Germany), upon roasting sand and a residue obtained from the evaporation of urine and then distilling the preparation in the absence of air, obtained a substance that glowed in the dark. Phosphorus was originally named cold fire; its present name comes from the Greek word phosphoros (light-bearing).

The method of obtaining phosphorus soon became known to the German chemists J. Krafft and J. Kunckel and was published in 1682. In 1743, A. S. Marggraf developed a method for preparing phosphorus. Here, a mixture of lead chloride and urine was subjected to evaporation until dry and then heated until all the volatile products had been given off. The residue was mixed with charcoal in powder form and was subjected to distillation in a clay retort, and the phosphorus vapors were condensed in a container with water. The simplest method of preparing phosphorus, involving the roasting of bone ash with coal, was proposed in 1771 by C. Scheele. Phosphorus was established as an element by A. Lavoisier. The second half of the 19th century saw commercial production of phosphorus from phosphate rocks in retorts heated by coal-fired furnaces, which in the early 20th century gave way to electric furnaces. Distribution.

The average phosphorus content in the earth’s crust (clarke) is 9.3 × 10–2 percent by weight; it is 1.6 × 10–1 percent in intermediate rocks, 1.4 × 10–1 in basic rocks, 7 × 10–2 in granites and other acidic igneous rocks, and still lower—1.7 × 10–2—in ultrabasic rocks (mantle). In sedimentary rocks, the phosphorus content varies from 1.7 × 10–2 percent (sandstones) to 4 × 10–2 percent (carbonate rocks). Phosphorus figures in magmatic processes and migrates widely in the biosphere. The magmatic processes and migration are both associated with large accumulations of phosphorus, which form commercial deposits of apatites and phosphate rocks. Phosphorus is an exceptionally important biogenic element; it is accumulated by many organisms. Many processes of phosphorus concentration in the earth’s crust are associated with biogenic migration.

Since phosphorus is taken in by living matter and is readily precipitated from water in the form of insoluble minerals, the concentration of the element in seawater is only 7 × 10–6 percent. Approximately 180 minerals of phosphorus are known, mainly phosphates of various types. Calcium phosphates are the most widely distributed. Physical properties. Elemental phosphorus occurs in several allotropes, the main ones being the white, the red, and the black. White phosphorus is a waxlike transparent substance with a characteristic odor; it is formed on condensation of phosphorus vapor. In the presence of trace amounts of red phosphorus, arsenic, iron, and other elements white phosphorus becomes yellow. For this reason, commercial white phosphorus is referred to as yellow phosphorus. White phosphorus exists in an α form and β form.

The α modification occurs as crystals of the cubic system (a = 18.5 angstroms [Å]); it has a density of 1.828 g/cm3, a melting point of 44.1 °C, a boiling point of 280.5°C, and a heat of fusion of 2.5 kilojoules (kJ) per mole of P4 (0.6 kilocalorie [kcal] per mole of P4). The heat of vaporization is 58.6 kJ per mole of P 4 (14.0 kcal per mole of P4), and the vapor pressure at 25°C is 5.7 newtons (N) per sq m (0.043 mm of mercury). The coefficient of linear expansion in the temperature range 0°–44°C is 12.4 × 10–4, and the thermal conductivity at 25°C is 0.56 watt (W) per m·°K [1.1346 × 10–3cal/(cm · sec · °C)].

The electrical properties of α-white phosphorus are similar to those of dielectrics. The forbidden band comprises approximately 2.1 electron volts (eV), and the resistivity is 1.54 × 1011 ohm·cm. The α form is diamagnetic, with a magnetic susceptibility of –0.86 × 10–6. The Brinell hardness is 6 meganewtons (MN) per sq m (0.6 kilogram-force [kgf] per sq mm). The a form of white phosphorus is readily soluble in carbon disulfide but only sparingly soluble in liquid ammonia, benzene, and carbon tetra-chloride. At a temperature of –76.9°C and a pressure of 0.1 MN/m2 (1 kgf/cm2), the α form is converted into the β form (density, 1.88 g/cm3). If the pressure is increased to 1,200 MN/m2 (12,000 kgf/cm2), the transition will occur at 64.5°C.

The β form occurs as crystals exhibiting double refraction; the structure of the crystals, however, has not been conclusively established. White phosphorus is poisonous. Since it ignites spontaneously in the air at a temperature of approximately 40°C, the element must be stored in water (the solubility in water at 25°C being 3.3 × 10–4 percent). If white phosphorus is heated in the absence of air at 250°–300°C for several hours, red phosphorus is obtained. The transition is exothermic and is accelerated by ultraviolet rays as well as by impurities (iodine, sodium, selenium). Standard commercial red phosphorus is nearly completely amorphous, its color ranging from dark brown to violet. With prolonged heating, it can be irreversibly converted to one of the crystal forms (triclinic, cubic), whose properties differ.

The density varies from 2.0 to 2.4 g/cm3, the melting point from 585° to 610°C (at a pressure of tens of atmospheres), the sublimation point from 416° to 423°C, and the resistivity from 109 to 1014 ohm-cm. Red phosphorus does not ignite spontaneously in the air at temperatures up to 240°–250°C but does burn with friction or impact. It is insoluble in water, as well as in benzene and carbon disulfide, and soluble in phosphorus tribromide. At its sublimation point, red phosphorus is converted into vapor, which on cooling yields mainly white phosphorus. Black phosphorus is formed by heating white phosphorus to 200°–220°C at a pressure of (1.2–1.7) × 103 MN/m2 [(12–17) × 103 kgf/cm2].

This conversion can be carried out without pressure provided that mercury and a small quantity of black phosphorus crystals (seeds) are present and that a temperature of 370°C is maintained for eight days. Black phosphorus occurs as crystals of orthorhombic structure (a= 3.31 Å, b= 4.38 Å, c= 10.50 Å); the lattice is constructed of corrugated layers with a pyramidal arrangement of atoms that is typical of phosphorus. The density is 2.69g/cm3, and the melting point approximately 1000°C at a pressure of 1.8 × 103 MN/m2 (18 × 103 kgf/cm2). Black phosphorus is outwardly similar to graphite. A semiconductor, it has a forbidden band of 0.33 eV at 25°C, a resistivity of 1.5 ohm-cm, and a temperature coefficient of resistivity of 0.0077. It is diamagnetic, with a specific magnetic susceptibility of –0.27 × 10–6.

When heated to 560°–580°C under its own vapor pressure, black phosphorus is converted into red phosphorus. Black phosphorus is only slightly reactive; it does not catch fire easily when ignited and therefore can be subjected to mechanical working and exposure to the air. Phosphorus has an atomic radius of 1.34 Å and ionic radii of 0.35 Å (P5+), 0.44 Å (P3+), and 1.86 Å (P3–). Phosphorus atoms unite to form diatomic (P2), tetratomic (P4), and polymer molecules. Under normal conditions, polymer molecules containing long chains of interconnected P4 tetrahedra are the most stable. In the liquid form, in the solid form (white phosphorus), and in the vapor form (at temperatures below 800°C), phosphorus is made up of P4 molecules. Above 800°C, the P4 molecules dissociate into P2 molecules, which in turn are broken down into single atoms at temperatures above 2000°C. Only white phosphorus is composed of P4 molecules; all the other modifications are polymers.

Chemical properties. The electron configuration of the outer orbitals of the phosphorus atom is 3s23p3; oxidation states of +5, + 3, and –3 are most characteristic of phosphorus in its compounds. Like nitrogen, phosphorus forms mainly covalent bonds in its compounds. Compounds with ionic bonds, such as the phosphides Na3P and Ca3P2, are very few. Unlike nitrogen, phosphorus has free 3d orbitals with relatively low energies, which makes an increase in the coordination number possible and leads to the formation of donor-acceptor bonds. Phosphorus is chemically active; white phosphorus exhibits the most activity, whereas red and black phosphorus are considerably more passive in chemical reactions. The oxidation of white phosphorus occurs through a chain reaction. The oxidation of phosphorus is usually accompanied by chemiluminescence. The burning of phosphorus in an excess of oxygen yields the pentoxide P4O10 (or P2O5); an insufficiency of oxygen results in the formation of mainly the trioxide P4O6 (or P2O3).

The existence of P4O7, P4O8, P2O6, PO, and other phosphorus oxides in the vapors has been spectroscopically established. Phosphorus pentoxide is produced commercially by burning elemental phosphorus in an excess of dry air. Subsequent hydration of P4O10 yields orthophosphoric acid (H3PO4) and polyphosphoric acids (Hn+2PnO3n+1). In addition, phosphorus forms phosphorous acid (H3PO3), hypophosphoric acid (H4P2O6), and hypophosphorous acid (H3PO2), as well as two peracids, namely perphosphoric acid (H4P2O8) and monoperphosphoric acid (H3PO5). The salts of phosphoric acids—phosphates—have found wide application, whereas phosphites and hypophosphites are less widely used.

Phosphorus combines directly with all halogens, liberating a large amount of heat and forming trihalides (PX3, X being a halogen), pentahalides with the general formula PX5, and oxyhalides, for example, POX3. The fusion of phosphorus and sulfur at temperatures below 100°C yields solid solutions based on the two elements; temperatures above 100°C bring about the exothermic reaction for the formation of the crystalline sulfides P4S3, P4S5, P4S7, and P4S10. Of these, only P4S5 decomposes into P4S3 and P4S7 when heated above 200°C; the others melt without decomposition. The known oxysulfides of phosphorus are P2O3S2, P2O2S3, P4O4S3, P6O10S5, and P4O4S3. Compared with nitrogen, phosphorus is less capable of forming compounds with hydrogen. Hydrogen phosphide, or phosphine (PH3), and diphosphine (P2H4) can be obtained only by indirect means.

The known compounds with nitrogen include the nitrides PN, P2N3, and P3N5—solid, chemically stable substances obtained by passing phosphorus vapor and nitrogen through an electric arc. Polymeric phosphonitrilic halides [(PNX2)], for example, polyphosphonitrilic chloride, are obtained by the reaction of halides of the general formula PX5 with ammonia under various conditions. Amidoimidophosphates as a rule are polymeric compounds that contain P—NH—P bonds in addition to P—O—P bonds. At temperatures above 2000°C, phosphorus reacts with carbon to form the carbide PC3, a substance that is not soluble in ordinary solvents and that reacts with neither acids nor alkalies. When heated with metals, phosphorus forms phosphides. Phosphorus forms numerous organophosphorus compounds. Derivation.

Elemental phosphorus is produced through the electrothermal reduction of naturally occurring phosphates (apatites or phosphate rocks) by coke at 1400°–1600°C in the presence of silica (quartz sand): 2Ca3(PO4)2 + 10C + nSiO2 = P4 + 10CO + 6CaO·nSiO2 Previously ground and dressed phosphorus-containing ore is mixed in given proportions with silica and coke and then charged into an electric furnace. Silica is necessary for reducing the temperature of the reaction and increasing the reaction rate. The latter effect is due to the bonding of the calcium oxide given off during the reduction process to form calcium silicate, which is continuously removed in the form of molten slag. Silicates and oxides of aluminum, magnesium, iron, and other impurities also enter the slag. Another component of the slag is ferrophosphorus (Fe2P, FeP, Fe3P), which is formed from the reaction of part of the reduced ifon with phosphorus.

Ferrophosphorus, as well as the small amounts of the phosphides of manganese and other metals that are dissolved in it, is removed from the furnace as it accumulates for use in the manufacture of special steels. Phosphorus vapor is discharged from the electric furnace along with gaseous by-products and volatile impurities (CO, SiF4, PH3, steam, products of the pyrolysis of organic impurities in the charge) at a temperature of 250°–350°C. After being purified of dust, the phosphorus-containing gases are fed into condensation units, where at a temperature not below 50°C liquid commercial white phosphorus is collected under water. Methods of phosphorus production involving gaseous reducing agents and plasma reactors are being developed. These methods are designed to increase the yield through an increase of temperature to 2500°–3000°C, that is, to a point above the dissociation temperatures of naturally occurring phosphates and reducing gases, such as methane, that are used as transport gases in low-temperature plasma. Use.

Most of the phosphorus that is produced commercially is processed into phosphoric acid and into the phosphorus fertilizers and commercial salts (phosphates) based on the acid. White phosphorus is used in incendiary bombs and devices and smoke bombs; red phosphorus is used in the production of matches. Phosphorus is used as a deoxidizing agent in the production of nonferrous metal alloys. The addition of phosphorus (up to 1 percent) increases the high-temperature strength of such alloys as fechral and Chromal. The element is also added to certain bronzes since it increases flowability and resistance to wear. The phosphides of metals, as well as of certain nonmetals (B, Si, As), are used in the production and doping of semiconductor materials. Phosphorus is used in preparing the chlorides and sulfides that serve as source material for the manufacture of phosphorus-containing plasticizers (tricresyl phosphate, tributyl phosphate), medications, and organophosphorus pesticides. The element is also used in preparing the chlorides and sulfides that are additives in lubricants and fuels. Safety measures. White phosphorus and its compounds are highly toxic.

Work with phosphorus requires that all equipment and apparatus be hermetically sealed. White phosphorus must be stored under water or in hermetically sealed metal containers. Safety regulations should be strictly observed when working with phosphorus. L. V. K UBASOVA Biological functions. Phosphorus is one of the most important biogenic elements; it is required for the vital activities of all organisms. The element is present in living cells in the form of orthophosphoric and pyrophosphoric acids and their derivatives, and it is also a component of nucleotides, nucleic acids, phosphoproteins, phospholipids, phosphorus esters of hydrocarbons, and many coenzymes and other organic compounds. Owing to the characteristic features of their chemical structure, phosphorus atoms, like sulfur atoms, are able to form energy-rich bonds in such high-energy compounds as adenosinetriphosphoric acid and creatine phosphate. During evolution, it was the phosphorus compounds that became the primary, universal guardians of genetic information and the energy carriers in all living systems.

The importance of phosphorus compounds in organisms is also evident in the enzyme-catalyzed addition of the phosphoryl residue to various organic compounds (phosphorylation); this addition is a prerequisite for the compounds’ participation in metabolism. Conversely, detachment of the phosphoryl residue (dephosphorylation) precludes metabolic activity. The enzymes of phosphorus metabolism comprise the kinases, phosphorylases, and phosphatases. The liver figures prominently in the conversion of phosphorus compounds in humans and animals. The metabolism of phosphorus compounds is regulated by hormones and vitamin D. The phosphorus content (mg per 100 g dry matter) in the tissues of plants is 230–350; it is 400–1,800 in marine animals, 1,700–4,400 in terrestrial animals, and approximately 3,000 in bacteria. In humans, there are large amounts of phosphorus in bone tissue (slightly more than 5,000 mg per 100 g dry matter), brain tissue (approximately 4,000), and muscles (220–270).

The daily human requirement of phosphorus is 1–1.2 g (children requiring more than adults). The food products richest in phosphorus are cheese, meat, eggs, and legumes (peas, beans). The phosphorus balance in organisms depends on the overall state of metabolism. Disruption of phosphorus metabolism leads to serious biochemical changes, first and foremost in energy metabolism. Phosphorus deficiency in humans and animals induces osteoporosis and other bone diseases; in plants, it causes phosphoric hunger. Phosphorus is obtained by organisms from its inorganic compounds that are present in the soil and dissolved in water. The element is extracted from the soil in the form of soluble phosphates by plants. Animals usually take in a sufficient amount of phosphorus in their food. When an organism dies, phosphorus reenters the soil and bottomset beds, thereby taking part in the earth’s cycle of matter. The important role of phosphorus in the regulation of metabolic processes derives from the extreme sensitivity of many enzyme systems in living cells to the action of organophosphorus compounds. This condition is used in medicine in developing therapeutic preparations and in agriculture in creating phosphorus fertilizers and effective insecticides.

Many phosphorus compounds are extremely toxic, and certain organophosphorus compounds are considered war gases (sarin, soman, tabun). The radioisotope 32P is widely used in biology and medicine as a tracer in studying all types of metabolism and energy exchange in organisms. N. N. C HERNOV Poisoning. Poisoning can occur when working with white phosphorus; it is also possible during the thermoelectric sublimation of phosphorus and its compounds and during the production and use of the compounds. Organophosphorus compounds are highly toxic, having the effect of anticholinesterase. The element enters the body through the respiratory organs, gastrointestinal tract, and skin. The symptoms of acute poisoning include a burning sensation in the mouth and stomach, headache, weakness, nausea, and vomiting. After two or three days, jaundice manifests itself, and pain is felt in the epigastric region and right hypochondriac region.

Chronic poisoning is attended by inflammation of the mucosa in the upper respiratory tract, symptoms of toxic hepatitis, disruption of calcium metabolism (development of osteoporosis; fragility and, sometimes, necrosis of the bone tissue, usually the mandible), and disorders of the cardiovascular and nervous systems. First aid in cases of acute poisoning, occurring most often through the mouth, includes pumping of the stomach and administration of cathartics and enemas. Solutions of glucose, calcium chloride, and other substances are administered intravenously. For skin burns, the affected area is treated with solutions of blue vitriol or soda. Eyes should be rinsed with a 2-percent solution of sodium bicarbonate. Safety measures are important in working with phosphorus, as are personal and oral hygiene and regular (every six months) medical examinations. Pharmaceuticals containing phosphorus (adenosinetriphosphoric acid, Phytin, calcium glycerophosphate, phosphrene) affect mainly the processes of endogenous metabolism; they are used against diseases of the muscles and nervous system, tuberculosis, anorexia, and anemia.

Radioisotopes of phosphorus are used as tracers in studying metabolism and diagnosing diseases; they are also used in radiotherapy against tumors. A. A. K It's Elemental - The Element Phosphorus It's Elemental Melting 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 centimeter Phase at Room Temperature: Solid Element Classification: Non-metal Period Number: 3 Group Number: 15 Group Name: Pnictogen What'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 kilogram Estimated Oceanic Abundance: 6×10-2 milligrams per liter Number of Stable Isotopes: 1 ( View all isotope data ) Ionization Energy: 10.487 eV Etymologies of element names | PlanetStar Wiki | Fandom powered by Wikia Etymologies of element names Share Ad blocker interference detected! Wikia is a free-to-use site that makes money from advertising. We have a modified experience for viewers using ad blockers Wikia is not accessible if you’ve made further modifications. Remove the custom ad blocker rule(s) and the page will load as expected. This is the list of 173 elements discussing their etymologies, including official, proposed, predicted, and made-up names.

A subatomic particle neutron , since this element only contains neutron(s) in its nucleus . 1 Hydrogen H From the Latin hydor genes, derived from the Ancient Greek ὕδωρ γείνομαι (hydor geinomai), meaning "to beget water," because water is the most common and important hydrogen compound . 2 From the Greek ἥλιος ( Helios ), meaning " Sun " and also " the god of Sun " in mythology . 3 Lithium Li From the Greek λιθος (lithos), meaning "stone," because this element was discovered from a mineral while other common alkali metals (sodium and potassium) were discovered from plant tissue. 4 Beryllos, denoting " beryl ," which contains beryllium. 5 لاعقشا (buraq), derived from the Persian "بورون" (burah), referring to " borax ." 6 Carbon C From the French charbone, which in turn came from the Latin carbo, meaning "charcoal." (In German and Dutch , kohlenstoff and koolstof, respectively, both literally meaning " coal -stuff").

7 N From the Latin nitrum genes, derived from the Greek νιτρον γείνομαι (nitron geinomai), meaning "native-soda ( niter ) forming." It is sometimes known as Azotum, which means "Ashdod", the English name of that element, and its symbol is sometimes known as "Az". 8 Oxygen O From the Greek οξύς γείνομαι (oxys geinomai), meaning "acid to bring forth," as he believed it to be an essential component of acids. 9 Fluorspar , one of its compounds. Fluor is the Latin for "flowing." 10 From the Greek νέος (neos), meaning "new." 11 Sodium Na From the English soda , used in names for sodium compounds such as caustic soda , soda ash , and baking soda . The symbol Na is from the Modern Latin name Natrium, derived from the Greek νιτρον (nítron), meaning "natural soda," a kind of salt.

12 From the Ancient Greek Μαγνήσια ( Magnesia ) (district in Thessaly ), where this element was discovered. 13 From the Latin alum , meaning "bitter salt." 14 From the Latin silex or silicis, meaning " flint ," a kind of stone. 15 Phosphorus P From the Greek φωσ φόρος (phós phoros), meaning "light bearer," because "white phosphorus" emits a faint glow upon exposure to oxygen. Phosphorus was an ancient name for the " planet Venus " as Phosphorus ( Morning Star ). 16 Sulfur S Almost certainly from the Arabic صفرا (sufra), "yellow," the bright color of the naturally occurring form. The word passed into Sanskrit गन्धक (sulvere or sulvari), the Latin "sulpur," the English "sulphur" or "sulfur," and also was commonly referred as "brimstone" in English translations of the Bible .

17 Chlorine Cl From the Greek χλώρος (chlorós), meaning "yellowish green" or "greenish yellow," because of the color of the gas. 18 Means "inactive" in Greek (literally "lazy"). 19 Potassium K From the English potash , meaning "pot-ash" ( potassium compound prepared from an alkali extracted in a pot from the ash of burnt wood or tree leaves). The symbol K is from this elment's Latin name, Kalium, derived from the Arabic القلي (al qalīy), meaning "calcined ashes." 20 Calcium Ca From the Latin calx, meaning "lime." Calcium was known as early as the first century when the Romans prepared lime as calcium oxide . 21 From the Latin Scandia, meaning " Scandinavia ." 22 Titanium Ti From the Greek τιτάν (titan), meaning " Earth ." Also from Titans , the first sons of Gaia in Greek mythology. 23 From Vanadis , a goddess in Scandinavian mythology , because of its beautifully multicolored chemical compounds. 24 From the Greek chroma, meaning " color ," because there are many colorful chromium compounds .

25 From the Latin magnes, meaning "magnet," for Magnetite or its magnetic property. 26 Iron Fe "Iron" (īsern) may derive from the Etruscan aisar, meaning "the god (s)," because the earliest iron to be worked (by the Sumerians and Egyptians , around 4000 BC) was obtained from meteorites , and meteorites fall from the sky. Starting with two letters in this symbol: Fe, the Latin name of this element is Ferrum, meaning "Iron", which is the English name of that element. 27 Cobalt Co From the German kobalt, meaning "evil spirit," the metal being so called by miners, because this element was poisonous and troublesome ( polluted and degraded the other mined elements like nickel). Other sources cite the origin as stemming from silver miners' belief that cobalt had been placed by " Kobolds " who had stolen the silver. Some also think the name may be derive from the Greek kobalos, meaning "mine," and which may have common roots with kobold, goblin, and cobalt.

28 Nickel Ni From the Swedish kupfernickel, meaning "copper-colored ore"; this referred to the ore niccolite from which this element was obtained. 29 Copper Cu Possibly derived from the Greek χαλκός (chalkos), meaning "copper (the metal)." May also be derived from the Latin (during the Roman empire) aes cyprium, ("aes" being the generic Latin term for copper alloys such as bronze , etc). Cyprium means " Cyprus ," where so much of this element was mined; the name was simplified to cuprum and then eventually anglicized as "copper." 30 Borrowed from a Proto-Indo-European language , and has cognates in several Germanic and Celtic languages . The symbol Sn is from the Latin name Stannum. 51 Antimony Sb Possibly from the Greek αντι μόνος (anti monos), approximately meaning "opposed to solitude," as believed never to exist in pure form, or anti-monachos, (the French antimoine, still has adherents) for "monk-killer," because many early alchemists were monks and antimony is poisonous.

May also be derived from the Pharaonic ( Ancient Egypt ), Antos Ammon (expression), which could be translated as "bloom of the god Ammon." The symbol Sb is from Latin name, Stibium. The word derived from the Greek στιμμί (stimmi), probably a loan word from Arabic or Egyptian. Littré suggests the first form derives from stimmida, an accusative of stimmi. The Arabic word for the substance, as "mark" or "the cosmetic," can appear as ithmid, athmoud, othmod or uthmod. 52 Te From the Latin Tellus, meaning " Earth ." Also from Terra Mater , the Roman goddess personifying the Mother Earth . 53 Thule , an ancient Roman name for a mythical country in the far north, perhaps Scandinavia. 70 Ytterbium Yb Ytterbia , the oxide compound of ytterbium .

((Neo-)Ytterbium was named after (Neon, from the Greek νέος (neos), meaning "new", and) Ytterby, the Swedish village near Vaxholm ) where the mineral gadolinite was found.) An alternative, but rejected name is Aldebaranium (Ad), after the red giant star, Aldebaran , located about 68 light years away in the zodiac constellation of Taurus. 71 Lu From the Latin Lutetia, the city of " Paris ." An alternative name is Cassiopium (Cp), after the constellation in the northern sky, Cassiopeia , named after a vain queen ho boasted about her unrivalled beauty. 72 From the Latin Hafnia, meaning " Copenhagen ," the capital of Denmark . 73 Tantalum Ta From the Greek ταντάλυς ( Tantalus ), who was punished after death by being condemned to stand knee-deep in water, if he bent to drink water, it drained below the level he could reach (in Greek mythology ).

This was considered similar to tantalum's general non-reactivity because of its inertness (it sits among reagents and is unaffected by them). 74 Tungsten W From the Swedish and Danish languages tung sten, meaning "heavy stone." The symbol W is from scientific name Wolfram. The element and its ore Wolframite , was named in honor of " Peter Woulfe ," who discovered its existence. The names Wolfram or Volfram are still used in Swedish and several languages. 75 Honoring Ernest Rutherford , who pioneered the Bohr model of the atom and discovered the atomic nucleus . An alternative, but rejected name is Kurchatovium (Ku), honoring Igor Vasilevich Kurchatov , who shared fundamental understanding of the uranium chain reaction and the nuclear reactor. 105 Db Dubna , a town in Russia where this element was synthesized (in the Joint Institute for Nuclear Research). Two alternative, but rejected names are Hahnium (Ha) and Joliotium (Jl), honoring Otto Hahn , who shared the discovery of nuclear fission with Fritz Strassmann and Lise Meitner. He also discovered numerous radioactive elements, and Frédéric Joliot-Curie .

106 Seaborgium Sg Honoring Glenn T. Seaborg , who synthesized the chemistry of the transuranium elements , shared discoveries and isolated 10 elements, developed and proposed the actinide series .

107 The Parts of the Periodic Table Elements named after countries, states, or other geographical features: Californium: state (and University) of California Francium: France Gallium: Latin word for France, Gallia Germanium: Latin word for Germany, Germania Hassium: German state of Hesse, where the GSI is located Magnesium: named after Magnesia, a district in Thessaly in central Greece Polonium: named for Marie Curie's native country of Poland Rhenium: named after the Latin word for the Rhine River, Rhenus Ruthenium: named after the Latin word for Russia, Ruthenia Scandium: named after the Latin word for Scandinavia, Scandia Thulium: named after the ancient word for Scandinavia, Thule Elements named after cities: Berkelium: Berkeley, California, home of the University of California, where a number of synthetic elements have been produced Darmstadtium: Darmstadt, Germany, home of the Laboratory for Heavy Ion Research (GSI, Gesellschaft fï¿½r Schwerionenforschung) where a number of synthetic elements have been produced Dubnium: Dubna, Russia, home of the Joint Institute for

 Nuclear Research (JINR, Объединённый институт ядерных исследований, ОИЯИ), where a number of synthetic elements have been produced Erbium, Terbium, Ytterbium, Yttrium: all named after the Swedish village of Ytterby (near Vaxholm), where these elements were first isolated (as well as Holmium, Scandium, and Tantalum) Hafnium: Copenhagen (Hafnia), Denmark Fermium: Enrico Fermi, the inventor of the first nuclear reactor Lawrencium: Ernest O.

Lawrence, inventor of the cyclotron Meitnerium: Lise Meitner, one of the first scientists to recognize that uranium could undergo nuclear fission Mendelevium: Dimitri Mendelev, the deviser of the Periodic Table of the Elements Nobelium: Alfred Nobel, the inventor of dynamite and founder of the Nobel Prize Roentgenium: Wilhelm Rï¿½ntgen, the discoverer of X-rays Rutherfordium: Ernest Rutherford, discoverer of the atomic nucleus, and a pioneer in the study of nuclear physics Seaborgium: Glenn T.

Seaborg, who discovered/synthesized a number of transuranium elements Most of the rest of the names of the elements are derived from various chemical or physical properties: Actinium: Greek: aktinos, "ray" (because it glows with a blue light in the dark) Antimony: Greek: anti + monos, "not alone" (because it was never found uncombined with another element) Argon: Greek: argos, "idle" (because of its unreactivity) Astatine: Greek: astatos, "unstable" (because it is) Barium: Greek: barys, "heavy" (in reference to the high density of some barium minerals) Bromine: Greek: bromos, "stench" (elemental bromine has a terrible smell) Cobalt: German: kobold, "goblin" (because of the toxic fumes of arsenic that were produced when silver miners heated the arsenic-containing ore smaltite, mistaking it for silver ore) Dysprosium: Greek: dysprositos, "hard to get at" (because the first isolation of the element required a tedious separation sequence) Fluorine: Latin: fluere,

 "to flow" Hydrogen" Greek: hydro + genes, "water forming" Krypton: Greek: kryptos, "hidden" (since it had been "hidden" in a sample of argon) Lanthanum: Greek: lanthanein, "to be hidden" (because the element was discovered "hidden" as an impurity in ores of cerium) Manganese: Latin: magnes, "magnet" (because it can be made to be ferromagnetic with the right treatment) Neodymium: Greek: neos + didymos, "new twin" Neon" Greek: neos, "new" Nickel: German: kupfernickel, "Old Nick's copper" (i.e., copper of the devil, or false copper, because it was frequently mistaken for copper) Nitrogen: Latin: nitron + genes, "nitre [potassium nitrate] forming" Osmium: Greek: osme, "odor" (because of its nasty smell, which is actually caused by osmium tetroxide) Oxygen: Latin: oxy + genes, "acid forming" Phosphorus: Greek: phos + phoros, "light bringing" (because it glows

 in the dark, and spontaneously burst into flame in air) Radium: Latin: radius, "ray" (because of its ability to glow in the dark with a faint blue light) Technetium: Greek: technetos, "artificial" Tungsten: Swedish: tung sten, "heavy stone" (because of the elements high density) Xenon: Greek: xenos, "stranger" (because at the time, it did not form compounds with other elements References John Emsley, The Elements, 3rd edition.

Oxford: Clarendon Press, 1998. John Emsley, Nature's Building Blocks: An A-Z Guide to the Elements. Oxford: Oxford University Press, 2001. Table of Elements in Greek and Latin (Rome) Language. Sidebar Periodic Table of Elements The Greek language and Greek myth have contributed greatly to the sciences, including chemistry. This is most apparent in the Periodic Table of Elements. A table of the elements with mythological influences, or at least have the Greek language to thank for their names, is below. For kicks, I have included the Latin (Roman) terms also. (Please note: this is not the complete table of elements, only those with Greek or Latin influences.) Actinium From the Greek wordaktinos (ray) Aluminum From the Latin wordalumen, or"bitter". Antimony From the Greek words anti (opposed) and monos (solitude) Argon From the Greek wordargon (inactive) Arsenic From the Greek wordarsenikos and the Latin wordarsenicum, meaning "yellow orpiment".

Astatine From the Greek wordastatos (unstable) Barium From the Greek wordbarys (heavy) Bromine From the Greek wordbrômos (stench) Cadmium Symbol: Cd Atomic Number: 48 From the Greek wordkadmeia (ancient name for calamine) and from the Latin word cadmia.Cadmus, in Greek myth, was the founder of Thebes. Calcium From the latin wordcalcis (lime) Carbon Ceres (asteroid), and the Roman version of Demeter, the goddess of agriculture. Cesium From the Latin wordcaesius (sky blue) Chlorine From the Greek wordkhlôros (green) Chromium From the Greek wordchrôma (color) Copper From the Latin wordcyprium, after the island of Cyprus and birthplace of Aphrodite. Dysprosium From the Greek worddysprositos (hard to get at). Fluorine From the Latin wordfluo (flow) Gold From the Latin wordaurum (gold). In Roman mythology, Aurora was the goddess of dawn--golden indeed.

Helium From the Greek wordhêlios (sun); Helios in Greek mythology was the god of the Sun. Hydrogen Symbol: H Atomic Number: 1 From the Greek words hudôr (water) and gennan(generate). Heracles fought the Hydra of Lerna (a sea town) for his second labor. Iodine From the Greek wordiôdes (violet). Iridium Symbol: Ir Atomic Number: 77 From the Latin wordiridis (rainbow). The Greeks had a messenger goddess, Iris, whose colorful cape flowed behind her. Iron From the Latin wordferrum (iron) Krypton Symbol: Kr Atomic Number: 36 From the Greek wordkryptos (hidden). In modern language, words such as "encrypt" can be discerned from the Greek. Lanthanum From the Greek wordlanthaneis (to lie hidden). Lead Symbol: Pb Atomic Number: 82 Name Origin: From the Greek word protos (first). Some Greeks believd that the first god ever was Protogonus, or "first born".

Symbol Origin: From the Latin wordplumbum (lead) Lithium From the Greek wordlithos (stone) Manganese From the Latin wordmangnes (magnet) Molybdenum From the Greek word molubdos (lead) Neodymium Symbol: Nd Atomic Number: 60 From the Greek words neos (new) anddidymos (twin). Twins appear regularly in Greek myth, from the Dioscuri (Castor & Polydeuces) to the divine twins (Artemis & Apollo). Neon Form the Greek word neos (new) Neptunium After the planet Neptune, the Roman sea god, identified as Poseidon in Greek myth. Niobium Symbol: Nb Atomic Number: 41 After Niobe, daughter of mythical king (Tantalus). She had bragged about her set of seven girls and seven boys, scoffing at Leto for only having two children. Apollo and Artemis promptly killed her offspring. Niobe, in despair, was turned to stone by the gods.

Osmium From the Greek word osmë (odor) Oxygen From the Greek words oxus (acid) andgennan (generate) Palladium From the Greek goddess (Pallas) and after an asteroid Phosphorous Symbol: P Atomic Number: 15 From the Greek words phôs (light) andphoros (bearer), Phosphoros was a god of light in Greek myth. Plutonium After the planet Pluto and the Latin god of the Underworld (Hades in Greek). Potassium Symbol Origin: From the Latin word kalium Praseodymium From the Greek words prasios (green) anddidymos (twin) Promethium From the Titan Prometheus who stole fire of the sky and gave it to man. Protactinium From the Greek word protos (first) [see name origin for lead]. Radium From the Latin word radius (ray) Rhodium From the Greek word rhodon (rose) Rubidium From the Latin word rubidus (red) Ruthenium From the Latin word Ruthenia (Russia) Selenium From the Greek word Selênê, known as the goddess of the moon.

Sodium Symbol Origin: From the Latin wordnatrium (sodium) Silicon From the Latin word silex (flint) Sulfur From the Latin word sulfur (brimstone) Tantalum Symbol: Ta Atomic Number: 73 After king Tantalus, a son of Zeus who earned the disfavor of the gods for attempting to serve his son Pelops as a meal. He was condemned to the Underworld with eternal thirst and hunger though a river and fruit tree were just beyond his grasp. Technetium From the Greek word technêtos (artificial) Tellurium From the Greek word tellus (Earth) Thallium From the Greek word thallos (young shoot) Tin Symbol Origin: From the Latin wordstannum (tin) Titanium From the Greek word titanos (Titans). The Titans were the "original" gods before the Olympians. Uranium Symbol: U Atomic Number: 92 After the planet Uranus, the original sky god who was the son and spouse of Gaia, or Mother Earth. Xenon What does Phosphorus mean?

Definitions for Phosphorusˈfɒs fər əs; -fəˌraɪ This page provides all possible meanings and translations of the word Phosphorus Princeton's WordNet(0.00 / 0 votes)Rate this definition: phosphorus, P, atomic number 15(noun) a multivalent nonmetallic element of the nitrogen family that occurs commonly in inorganic phosphate rocks and as organic phosphates in all living cells; is highly reactive and occurs in several allotropic forms morning star, daystar, Phosphorus, Lucifer(noun) a planet (usually Venus) seen just before sunrise in the eastern sky Wiktionary(0.00 / 0 votes)Rate this definition: phosphorus(Noun) a chemical element (symbol P) with an atomic number of 15, that exists in several allotropic forms. phosphorus(Noun) A name sometimes used for Hesperus, the personification in Greek mythology of the planet Venus. Phosphorus(ProperNoun) An ancient Greek name for the morning star (the planet Venus when it is visible in the eastern sky before sunrise).

Origin: From Latinised Greek Phosphorus, from Φωσφόρος, from φῶς + φέρω. Webster Dictionary(4.00 / 1 vote)Rate this definition: Phosphorus(noun) the morning star; Phosphor Phosphorus(noun) a poisonous nonmetallic element of the nitrogen group, obtained as a white, or yellowish, translucent waxy substance, having a characteristic disagreeable smell. It is very active chemically, must be preserved under water, and unites with oxygen even at ordinary temperatures, giving a faint glow, -- whence its name. It always occurs compined, usually in phosphates, as in the mineral apatite, in bones, etc. It is used in the composition on the tips of friction matches, and for many other purposes. The molecule contains four atoms. Symbol P. Atomic weight 31.0 Phosphorus(noun) hence, any substance which shines in the dark like phosphorus, as certain phosphorescent bodies Origin: [L., the morning star, Gr.

fwsfo`ros, lit., light bringer; fw^s light + fe`rein to bring.] Freebase(0.00 / 0 votes)Rate this definition: Phosphorus Phosphorus is a nonmetallic chemical element with symbol P and atomic number 15. A multivalent pnictogen, phosphorus as a mineral is almost always present in its maximally oxidised state, as inorganic phosphate rocks. Elemental phosphorus exists in two major forms—white phosphorus and red phosphorus—but due to its high reactivity, phosphorus is never found as a free element on Earth. The first form of elemental phosphorus to be produced emits a faint glow upon exposure to oxygen – hence its name given from Greek mythology, Φωσφόρος meaning "light-bearer", referring to the "Morning Star", the planet Venus. The term "phosphorescence", meaning glow after illumination, originally derives from this property of phosphorus, although this word has since been used for a different physical process that produces a glow. The glow of phosphorus itself originates from oxidation of the white phosphorus— a process now termed chemiluminescence.

The vast majority of phosphorus compounds are consumed as fertilisers. Other applications include the role of organophosphorus compounds in detergents, pesticides and nerve agents, and matches. Phosphorus is essential for life. As phosphate, it is a component of DNA, RNA, ATP, and also the phospholipids that form all cell membranes. Demonstrating the link between phosphorus and life, elemental phosphorus was historically first isolated from human urine, and bone ash was an important early phosphate source. Phosphate minerals are fossils. Low phosphate levels are an important limit to growth in some aquatic systems. The chief commercial use of phosphorus compounds for production of fertilisers is due to the need to replace the phosphorus that plants remove from the soil. Chambers 20th Century Dictionary(0.00 / 0 votes)Rate this definition: Phosphorus fos′fō-rus, n. the morning-star: a yellowish substance, like wax, inflammable and giving out light in the dark.—n. Phos′phate, a salt formed by the combination of phosphoric acid with a base.—adj. Phosphat′ic, of the nature of, or containing, a phosphate.—ns.

Phos′phide, a compound formed of phosphorus and some other element, as copper or iron; Phos′phite, a salt of phosphorous acid; Phos′phor, the morning-star: (obs.) phosphorus.—v.t. Phos′phorate, to combine or impregnate with phosphorus.—n. Phos′phor-bronze, an alloy of copper, tin, and phosphorus.—v.i. Phosphoresce′, to shine in the dark like phosphorus.—n. Phosphoresc′ence.—adjs. Phosphoresc′ent, shining in the dark like phosphorus; Phosphor′ic, Phos′phorous, pertaining to or obtained from phosphorus.—ns. Phos′phorite, a massive radiated variety of apatite; Phos′phuret, a compound of phosphorus with a metal.—adj. Phos′phuretted, combined with phosphorus.—n. Phos′sy-jaw, phosphorous poisoning.—Phosphatic diathesis (med.), the condition in which there is a tendency in the urine to deposit white gravel.

[L.,—Gr.,—phōsphoros, light-bearer—phōs, light, phoros, bearing, from pherein, to bear.] U.S. National Library of Medicine(0.00 / 0 votes)Rate this definition: Phosphorus A non-metal element that has the atomic symbol P, atomic number 15, and atomic weight 31. It is an essential element that takes part in a broad variety of biochemical reactions. Editors Contribution(0.00 / 0 votes)Rate this definition: phosphorus Is a chemical element. Phosphorus is a chemical element found in many minerals, is an important component in steel making and are a component of DNA, RNA, ATP in the human body. Numerology The numerical value of Phosphorus in Chaldean Numerology is: 9 Pythagorean Numerology

Question: Which chemical element (atomic number 15) derives its name from the Greek for "light bearing"?
Answer: Phosphorus