The relative atomic mass of phosphorus. White phosphorus: properties, history of discovery and application

(Phosphorus) ?? chemical element 15 (Va) of the group of the Periodic system, atomic number 15, atomic mass 30.974. Known 23 isotope of phosphorus 24 P ?? 46 P, among them one stable 31 P and only it is found in nature. The half-life of the isotope is 30 P 2.55 minutes; it is the first radioactive isotope obtained artificially in 1934 by Frederic and Irene Joliot-Curie.

It is possible that phosphorus in elemental form was obtained as early as the 12th century. the Arab alchemist Alkhid Bekhil during the distillation of urine with clay and lime, this is evidenced by the ancient alchemical manuscript stored in the Paris library. However, the discovery of phosphorus is usually attributed to the ruined Hamburg merchant Hennig Brand. The entrepreneur was engaged in alchemy to get a philosopher's stone and an elixir of youth, with the help of which he could easily improve his financial situation. After evaporation of 50–60 buckets of urine (he took it in the soldiers’ barracks) for two weeks and the subsequent strong calcination of the dry residue with coal and sand in the retort, Brand in 1669 was able to condense the released vapors under water and get a small amount of yellow substance. It glowed in the dark and was therefore called Brand “cold fire” (kaltes Feuer). Brand's contemporaries called this substance phosphorus because of its ability to glow in the dark (dr. Greek jwsjoroV). In general, since ancient times, “phosphors” called all substances that can emit light in the dark. So, is Bologna phosphorus widely known ?? barium sulfide.

In 1682, Brand published the results of his research, and now he is rightly considered the discoverer of element number 15. Phosphorus was the first element, the discovery of which is documented, and its discoverer is known.

The interest in the new substance was tremendous, and did Brand take this ?? he demonstrated phosphorus only for money or exchanged small amounts of it for gold. Despite numerous efforts, realize his cherished dream ?? The Hamburg merchant couldn’t get gold from lead with the help of “cold fire”, and so he soon sold the recipe for a new substance to a certain Kraft from Dresden for two hundred thalers. The new owner managed to put together a much larger state on phosphorus ?? with "cold fire" he traveled all over Europe and demonstrated it to scientists, dignitaries and even royals, for example, Robert Boyle, Gottfried Leibniz, Karl II. Although the method for the preparation of phosphorus was kept a closely guarded secret, in 1682 Robert Boyle managed to get it, but he only announced his methodology at a closed meeting of the Royal Society of London. Boyle's method was made public after his death, in 1692.

For a long time, phosphorus was not considered a simple substance, and it was only in the 1770s that the French chemist Antoine Laurent Lavoisier in his works on the study of air composition, could firmly establish that phosphorus is an elementary substance.

Figurovsky N.A. Discovery of elements and the origin of their names. M., Science, 1970
Phosphorus in the environment. Ed. E. Griffith. M., "World", 1977
Phosphorus technology. Ed. V.A. Ershova. L., "Chemistry", 1979
Corbridge D. Phosphorus: the basics of chemistry, biochemistry, technology. M., "World", 1982
Popular library of chemical elements. M., Science, 1983

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Phosphorus (from Greek phosphoros - luminiferous; Lat. Phosphorus) - an element of the periodic system of chemical elements of the periodic table, one of the most common elements of the earth's crust, its content is 0.08-0.09% of its mass. The concentration in sea water is 0.07 mg / l. In a free state does not occur due to high chemical activity. It forms about 190 minerals, the most important of which are apatite Ca 5 (PO 4) 3 (F, Cl, OH) phosphate Ca 3 (PO 4) 2 and others. Phosphorus is found in all parts of green plants, even more in fruits and seeds (see phospholipids). Contained in animal tissues, part of proteins and other essential organic compounds (ATP, DNA), is an element of life.

Story

Phosphorus was discovered by the Hamburg alchemist Hennig Brand in 1669. Like other alchemists, Brand tried to find the philosopher's stone, and received a luminous substance. Brand focused on experiments with human urine, since he believed that, having a golden color, it might contain gold or something needed for production. Initially, his method was that at first the urine settled for several days until the unpleasant odor disappeared, and then boiled to a sticky state. By heating this paste to high temperatures and leading to the appearance of bubbles, he hoped that, having condensed, they would contain gold. After several hours of intense boiling, grains of white wax-like substance were obtained, which burned very brightly and also flickered in the dark. Brand called this substance phosphorus mirabilis (lat. "Miraculous carrier of light"). The discovery of phosphorus by Brand was the first discovery of a new element since antiquity.
  Somewhat later, phosphorus was obtained by another German chemist, Johann Kunkel.
  Regardless of Brand and Kunkel, phosphorus was obtained by R. Boyle, who described it in the article “A Method for the Preparation of Phosphorus from Human Urine,” dated October 14, 1680 and published in 1693.
  An improved method for producing phosphorus was published in 1743 by Andreas Marggraf.
  There is evidence that phosphorus was still able to get Arab alchemists in the XII century.
  The fact that phosphorus is a simple substance was proved by Lavoisier.

origin of name

In 1669, Henning Brand, when he heated a mixture of white sand and boiled urine, received a substance glowing in the dark, first called “cold fire”. The secondary name "phosphorus" comes from the Greek words "φῶς" - light and "φέρω" - I carry. In ancient Greek mythology, the name Phosphorus (or Eosphorus, other Greek Φωσφόρος) was borne by the guard of the Morning Star.

Getting

Phosphorus is obtained from apatites or phosphorites as a result of interaction with coke and silica at a temperature of 1600 ° C:
   2Ca 3 (PO 4) 2 + 10C + 6SiO 2 → P4 + 10CO + 6CaSiO 3.

The resulting white phosphorus vapor condenses in a receiver underwater. Instead of phosphorites, other compounds, for example, metaphosphoric acid, can also be reduced:
   4HPO 3 + 12C → 4P + 2H 2 + 12CO.

Physical properties

Elementary phosphorus under ordinary conditions is a few stable allotropic modifications; the issue of phosphorus allotropy is complex and not fully resolved. Four modifications of a simple substance are usually distinguished - white, red, black and metallic phosphorus. Sometimes they are also called the main allotropic modifications, implying that all the rest are a variation of the four. Under ordinary conditions, there are only three allotropic modifications of phosphorus, and under ultrahigh pressure there is also a metal form. All modifications vary in color, density and other physical characteristics; there is a tendency towards a sharp decrease in chemical activity during the transition from white to metallic phosphorus and an increase in metallic properties.

Chemical properties

The chemical activity of phosphorus is significantly higher than that of nitrogen. The chemical properties of phosphorus are largely determined by its allotropic modification. White phosphorus is very active, in the process of transition to red and black phosphorus, the chemical activity decreases sharply. White phosphorus in the air glows in the dark, the glow is due to the oxidation of phosphorus vapors to lower oxides.
  In liquid and dissolved states, as well as in vapors up to 800 ° С, phosphorus consists of P 4 molecules. When heated above 800 ° C, the molecules dissociate: P 4 = 2P 2. At temperatures above 2000 ° C, the molecules decompose into atoms.

PHOSPHORUS (lat. Phosphorus), P, a chemical element of group V of the periodic table of the Mendeleev, atomic number 15, atomic mass 30.97376.

Properties:

Phosphorus forms several allotropic modifications, which differ markedly in properties. White phosphorus is a soft crystalline substance. Consists of P 4 molecules. It melts at a temperature of 44.1 ° C. Very soluble in carbon disulfide CS 2. Extremely toxic and light on fire.
   When white phosphorus is heated, red phosphorus is formed. It is a mixture of several modifications that have different lengths of molecules. The color of red phosphorus, depending on the method and preparation conditions, can vary from light red to purple and dark brown. Its melting point is 585-600 °.
   Black phosphorus is the most stable modification. In appearance, it looks like graphite. Unlike white phosphorus, red and black phosphorus do not dissolve in carbon disulfide, they are not toxic and not flammable.
   Phosphorus is chemically more active than nitrogen. The chemical activity of phosphorus depends on the allotropic modification in which it is located. So, white phosphorus is most active, and black phosphorus is the least active.
In the equations of chemical reactions, white phosphorus is usually written as P 4, which corresponds to the composition of its molecules. Red and black modifications of phosphorus are usually written by the formula P. The same symbol is used if the modification is unknown or can be any.
1. Interaction with simple substances - non-metals.  Phosphorus can react with many non-metals: oxygen, sulfur, halogens, phosphorus does not react with hydrogen. Depending on whether phosphorus is in excess or deficiency, phosphorus compounds (III) and (V) are formed, for example:
   2P + 3Br 2 = 2PBr 3 or 2P + 5Br 2 = 2PBr 5
   2. Interaction with metals. When phosphorus is heated with metals, phosphides are formed:
   3Mg + 2P = Mg 3 P 2
   The phosphides of some metals can decompose with water to form gaseous phosphine PH 3:
   Mg 3 P 2 + 6H 2 O = 3Mg (OH) 2 + 2PH 3
   Phosphine PH? chemical properties similar to ammonia NH ?.
   3. Interaction with alkalis. When heating white phosphorus in an alkali solution, it disproportionates:
0 -3 +1
   P 4 + 3NaOH + 3H 2 O = PH 3 + 3NaH 2 PO 2

Receiving. Phosphorus in industry is obtained from calcium phosphate Ca 3 (PO 4) 2, which is isolated from phosphorites and fluorapatites. The production method is based on the reaction of reduction of Ca 3 (PO 4) 2 to phosphorus.
   Coke (carbon) is used as a reducing agent for phosphorus compounds. To bind calcium compounds, silica sand SiO 2 is added to the reaction system. The process is carried out in electric furnaces (production is referred to as electrothermal). The reaction proceeds according to the equation:
   2Ca 3 (PO 4) 2 + 6SiO 2 + 10C = 6CaSiO 3 + P 4 + 10CO
   The reaction product is white phosphorus. Due to the presence of impurities, technical phosphorus is yellow, so in industry it is called yellow phosphorus.

Phosphate fertilizer. Phosphorus, as well as nitrogen, is an important element for ensuring the growth and vital activity of plants. Plants extract phosphorus from the soil, so its reserves must be replenished by periodically adding phosphorus fertilizers. Phosphoric fertilizers are produced from calcium phosphate, which is part of natural phosphorites and fluorapatites.
   The simplest phosphate fertilizer - phosphate rock is ground Ca 3 (PO 4) 2 phosphate. This fertilizer is hardly soluble, it can be absorbed by plants only on acidic soils.
The action of sulfuric acid on calcium phosphate produces simple superphosphate, the main component of which is calcium dihydrogen phosphate Ca (H 2 PO 4) 2. It is a soluble substance, and it is well absorbed by plants. The method for producing simple superphosphate is based on the reaction
   Ca 3 (PO 4) 2 + 2H 2 SO 4 = Ca (H 2 PO 4) 2 + 2 CaSO 4
   In addition to the main component, superphosphate contains up to 50% calcium sulfate, which is ballast. To increase the phosphorus content in the fertilizer, phosphorite is treated with phosphoric acid:
   Ca 3 (PO 4) 2 + 4H 3 PO 4 = 3Ca (H 2 O 4) 2
   The resulting fertilizer is called double superphosphate. Another phosphorus fertilizer with a high phosphorus content is CaHPO 4 · 2H 2 O precipitate.
   Highly concentrated phosphoric fertilizers are prepared on the basis of superphosphoric acid - a mixture of polyphosphoric acids H 4 P 2 O 7, H 5 P 3 O 10, and others. These acids are formed by heating phosphoric acid H 3 PO 4 in vacuum.
   The interaction of polyphosphoric acids with ammonia produces ammonium polyphosphates, which are used as complex nitrogen-phosphorus fertilizers.
   Together with nitrogen, phosphorus is part of some other complex fertilizers, for example ammophos and diammophos.

Name: from the Greek "phosphoros" (luminiferous).

Obtaining: extracted from apatite and phosphorite.

Being in the nature:  present in living cells in the form of ortho- and pyrophosphoric acids and their derivatives.

Application: the main consumer is agriculture (phosphate fertilizers); used in match production, metallurgy (deoxidizing agent and component of certain alloys), in organic synthesis, etc.

Phosphorus

PHOSPHORUS   -but; m  [from the Greek phōsphoros - luminiferous] A chemical element (P) that plays an important role in the life of animals and plants (found in some minerals, in animal bones, in animal and plant tissues). Red f. Black f. Fish has a lot of phosphorus. F. is needed to strengthen bones. White f.  (flammable and glowing in the dark substance). The sea shines, shines with phosphorus  (glows at night with a greenish light due to the abundance of microorganisms).

◁    Phosphoric (see).

(lat. Phosphorus), a chemical element of group V of the periodic system. Named from Greek. phōsphóros - luminiferous. It forms several modifications - white phosphorus (density 1.828 g / cm 3, t  pl 44.14 ° C), red phosphorus (density 2.31 g / cm 3, t pl 593 ° C), etc. White phosphorus is easily self-igniting, glows in the dark (hence the name), poisonous; red is less chemically active, poisonous. Extracted from apatite and phosphorite. The main consumer is agriculture (phosphate fertilizers); used in match production, metallurgy (deoxidizing agent and component of certain alloys), in organic synthesis, etc. It is present in living cells in the form of ortho- and pyrophosphoric acids and their derivatives.

PHOSPHORUS (lat. - Phosphopus), P (read "pe"), a chemical element with atomic number 15, atomic mass 30.973762. Located in the VA group in the 3rd period of the periodic system. It has one stable nuclide 31 P. The configuration of the outer electronic layer 3 s 2 r 3   . It exhibits oxidation states from –3 to +5 in compounds. Valencies from III to V. The most stable oxidation state in compounds is +5.
The radius of the neutral atom is P 0.134 nm, the radius of ions: P 3 - 0.186 nm, P 3+ 0.044 nm (coordination number 6) and P 5+ - 0.017 nm (coordination number 4) and 0.038 nm (coordination number 6). The sequential ionization energies of the neutral P atom are 10.486, 19.76, 30.16, 51.4, and 65 eV. The electron affinity is 0.6 eV. Poling electronegativity (cm.  Pauling Linus)  2.10. Non-metal.
Discovery story
  In 1669, the first free phosphorus state was received by the Hamburg alchemist H. Brand (there is evidence that a substance similar in properties was obtained back in the 12th century by the Arab alchemist Behil). Finding the Sorcerer's Stone (cm.  ELIXIR)  he calcined in a closed vessel the dry residue from the evaporation of urine with river sand and charcoal. After calcination, the vessel with the reagents began to glow in the dark with white light (this was phosphorus, which was recovered from its compounds contained in urine).
In 1680, phosphorus glowing in the dark (from the Greek "phosphorus" - luminiferous) was received by the Englishman R. Boyle. (cm.  BOULE Robert)  In subsequent years, it was found that phosphorus is found not only in urine, but also in brain tissue, in the bones of the skeleton. The simplest method for producing phosphorus by calcining bone ash with coal was proposed in 1771 by C. Scheele (cm.  SHEELE Carl Wilhelm). The elementary nature of phosphorus was established at the end of the 18th century by A. L. Lavoisier. (cm.  LOVOISE Antoine Laurent)
Being in nature
  The content in the earth's crust is 0.105% by mass, which significantly exceeds the content, for example, of nitrogen (cm.  NITROGEN). In sea water, 0.07 mg / l. In its free form, phosphorus does not occur in nature, but it is part of 200 different minerals. The most famous phosphorite (cm.  PHOSPHORITES)  calcium Ca 3 (PO 4) 3, apatites (cm.  Apatity)  (fluorapatite 3Ca 3 (PO 4) 3 · CaF 2, or, Ca 5 (PO 4) 3 F), monazite (cm.  MONACYT), turquoise (cm.  TURQUOISE). Phosphorus is part of all living organisms.
Getting
  Phosphorus production is carried out by electrothermal reduction of it from phosphorites and apatites at 1400-1600 ° C with coke in the presence of silica:
2Са 3 (РО 4) 2 + 6SiO 2 + 10C = P 4 + 6CaSiO 3 + 10CO
4Са 5 (РО 4) 3 F + 21SiO 2 + 30C = 3P 4 + 20CaSiO 3 + 30CO + SiF 4
The released P 4 vapors are then treated with superheated water vapor to obtain thermal phosphoric acid H 3 PO 4:
P 4 + 14H 2 O = 4H 3 PO 4 + 8H 2
Upon desublimation of P 4 vapor, white phosphorus is formed. It is processed into red phosphorus by heating without air at a temperature of 200-300 ° C in reactors equipped with a screw shredder for the reaction mixture.
Structural features of allotropic modifications and their physical properties
  Elementary phosphorus exists in several allotropic modifications, the main of which are white (phosphorus III), red (phosphorus II) and black (phosphorus I).
White phosphorus is a waxy, transparent substance with a characteristic odor. It consists of tetrahedral P 4 molecules that can rotate freely. White phosphorus has a molecular type cubic crystal lattice, the cell parameter but  = 1.851 nm. The density of 1.828 kg / DM 3. Melting point 44.14 ° C, boiling point 287 ° C. There are two forms of white phosphorus: the a-modification, with a cubic crystal lattice, at –76.9 ° C transforms into the b-modification, the crystal lattice of which is not installed and there is no free rotation of P 4 molecules. Dielectric. It is soluble in ethanol, benzene, carbon disulfide CS 2.
By heating white phosphorus without air at 250-300 ° C, red phosphorus is obtained. Admixtures of sodium, iodine and selenium and UV rays accelerate the transition of one modification to another.
Red phosphorus is amorphous, has a color from scarlet to dark brown and purple. There are several crystalline forms with various properties. Crystalline red phosphorus (Hittorf phosphorus) is obtained by cooling a solution of red phosphorus in molten lead saturated at a temperature of 600 ° C. It has a monoclinic lattice, unit cell parameters but  = 1.02 nm, at= 0.936 nm, with = 2.51 nm, angle b 118.8 °. The density of red phosphorus is 2.0-2.4 kg / dm 3. Dielectric. When heated, red phosphorus evaporates in the form of P 4 molecules, the condensation of which leads to the formation of white phosphorus.
When white phosphorus is heated to 200-220 ° C under a pressure of 1.2 GPa, crystalline black phosphorus is formed. The lattice is built of fibrous layers with a pyramidal arrangement of atoms. The most stable variety of black phosphorus has an orthorhombic lattice, parameters but  = 0.3314 nm, at= 0.4376 nm, s = 1.0478 nm. The density of black phosphorus is 2.702 kg / dm 3. It looks like graphite; semiconductor, diamagnetic. When heated to 560-580 ° C, it turns into red phosphorus. Black phosphorus is inactive, hardly ignites.
Chemical properties
  Phosphorus in the compounds is mainly covalent. Phosphorus has free 3d orbitals, which leads to the formation of donor-acceptor bonds. The most active is white phosphorus. It is oxidized in air. Oxidation occurs by the mechanism of chain reactions and is accompanied by chemoluminescence. When phosphorus is burned in excess of oxygen, P 2 O 5 is obtained, which forms P 4 O 10 dimers and P 8 O 20 tetramers. With a lack of oxygen, P 2 O 3 is obtained. It spontaneously ignites in air due to the heat released during oxidation. Red phosphorus in the air oxidizes slowly, does not ignite spontaneously. Black phosphorus does not oxidize in air.
Phosphorus (V) oxide is an acid oxide. It reacts with water with the release of a large amount of heat. In this case, first a polymer metaphosphoric acid (NRA 3) n is formed. When treated with hot water, it turns into tribasic orthophosphoric acid of medium strength N 3 PO 4:
P 4 O 10 + 2H 2 O = (NRA 3) 4; (NRA 3) 4 + 4H 2 O = 4H 3 PO 4
or P 2 O 5 + 3H 2 O = 2H 3 PO 4
Phosphorus interacts with halogens with the release of a large amount of heat. With F, Cl, Br forms trihalides and pentahalides, with I - only tri triide PI 3. All phosphorus halides are easily hydrolyzed to orthophosphoric H 3 PO 4, phosphorous H 3 PO 3 and hydrohalic acids:
PCl 5 + 4H 2 O = H 3 PO 4 + 5CH
PI 3 + 3H 2 O = H 3 PO 3 + 3HI
Phosphorus trihalides are a trihedral pyramid with halogen atoms at the base and a phosphorus atom at the top. The pentahalide molecule is two trihedral pyramids with a common face. The phosphorus oxyhalides of POF 3, POCl 3, and POBr 3 were obtained.
With sulfur, phosphorus forms sulfides P 4 S 3, P 4 S 5, P 4 S 7, P 4 S 10. Known phosphorus oxysulfides: P 2 O 3 S 2, P 2 O 2 S 3, P 4 O 4 S 3, P 6 O 10 S 5, P 4 O 4 S 3. Phosphorus reacts with Se and Te, forms compounds with Si and C (PC 3).
It does not directly react with hydrogen. When interacting with a dilute solution of potassium hydroxide KOH, gaseous phosphine PH 3 is formed:
4P + 3KOH + 3H 2 O = 3KN 2 PO 2 + PH 3
As an impurity, diphosphine P 2 H 4 is also formed. Both phosphines have a characteristic smell of rotten fish.
Phosphine PH 3 in chemical properties resembles ammonia NH 3, but is less stable.
Phosphorus during fusion reacts with metals. With alkaline earth forms M 3 P 2 ionic phosphides, decomposing upon contact with water:
Mg 3 P 2 + 6H 2 O = 3Mg (OH) 2 + 2PH 3,
Ca 3 P 2 + 6H 2 O = 3Ca (OH) 2 + 2PH 3
With transition metals, phosphorus forms metal-like phosphides Mn 3 P, FeP, Ni 2 P.
Phosphorus is part of inorganic acids. This is orthophosphoric acid H 3 PO 4 (its salts are orthophosphates, monohydrophosphates, Na 2 HPO 4 and dihydrophosphates, Ca (H 2 PO 4) 2); metaphosphoric acid (NRA 3)   n  (its salts are metaphosphates), hypophosphorous acid H 3 PO 2 (its salts are hypophosphites, NaH 2 PO 2), dibasic phosphorous acid H 3 PO 3 (its salts are phosphites, Na 2 HPO 3).
Phosphorus is a part of organic esters, alcohols and acids: phosphinic RRP (O) OH, phosphonous RH 2 PO 2 and phosphonic RP (O) (OH) 2, where R and R are organic radicals.
Application
  White phosphorus is used in the manufacture of phosphoric acid H 3 PO 4 (for the production of food phosphates and synthetic detergents). It is used in the manufacture of incendiary and smoke shells, bombs.
Red phosphorus is used in the manufacture of mineral fertilizers, match production. Phosphorus is used in the production of non-ferrous metal alloys as a deoxidizer and serves as an alloying additive. It is used in the production of soft magnetic alloys, in the preparation of semiconductor phosphides. Phosphorus compounds serve as starting materials for the production of medicines.
Body content
Phosphorus is present in living cells in the form of ortho-and pyrophosphoric acids, is part of nucleotides, nucleic acids, phosphoproteids, phospholipids, coenzymes, enzymes. Human bones consist of hydroxylapatite 3Ca 3 (PO 4) 3 · CaF 2. The composition of the tooth enamel includes fluorapatite. The main role in the conversion of phosphorus compounds in humans and animals is played by the liver. The exchange of phosphorus compounds is regulated by hormones and vitamin D. The daily human need for phosphorus is 1-2 g. With a lack of phosphorus, various bone diseases develop in the body.
Physiological effect
  Phosphorus compounds are toxic. The lethal dose of white phosphorus is 50-150 mg. Getting on the skin, white phosphorus gives severe burns. Chemical warfare agents sarin, soman, herd are phosphorus compounds. Acute phosphorus poisoning is manifested by burning in the mouth and stomach, headache, weakness, vomiting. After 2-3 days develop jaundice. Chronic forms are characterized by impaired calcium metabolism, damage to the cardiovascular and nervous systems. First aid for acute poisoning - gastric lavage, laxative, cleansing enemas, intravenous glucose solutions. For skin burns, treat the affected areas with copper sulfate or soda solutions. MPC phosphorus vapors in the air 0.03 mg / m 3. Dust red phosphorus, falling into the lungs, causes pneumonia.

encyclopedic Dictionary. 2009 .

See what is "phosphorus" in other dictionaries:

  - (Greek, from phos light, and phoros bearing). A simple body, yellowish in color, flammable and glowing in the dark. Dictionary of foreign words included in the Russian language. Chudinov, AN, 1910. PHOSPHORUS grech. phosphoros, from phos, genus. pad. ... ... Dictionary of foreign words of the Russian language

PHOSPHORUS  - Phosphorus, chem. element (symbol P) with am. at. 31.02, belonging to the V group and 3 series of the periodic system (serial number 15). F. is widespread in nature, but only in the form of oxygen compounds: the soil contains it in the form of salts ... ... Big Medical Encyclopedia

Phosphorus  - is a solid, soft and plastic in consistency, obtained by treating natural phosphates mixed with sand and carbon in an electric furnace. There are two main types of phosphorus: a) white phosphorus, ... ... Official terminology

- (symbol P), the chemical element of the fifth group of the periodic table, first discovered in 1669. Found in the form of phosphates in minerals, the main source of phosphorus APATIT. This element is used for the manufacture of phosphoric acid, ... ... Scientific and Technical Encyclopedic Dictionary

  - (Phosphorus), P, chemical element of the V group of the periodic system, atomic number 15, atomic mass 30.97376; non-metal white (lit on air, tpl 44,14 ° C), red (tpl 593 ° C) or black (tpl 1000 ° C) color. Phosphorus is used in ... ... Modern Encyclopedia

  - (Lat. Phosphorus) P, chemical element of the V group of the periodic table, atomic number 15, atomic mass 30.97376. The name of the Greek. phosphoros luminiferous. Forms several modifications of white phosphorus (density 1,828 g / cm & sup3, tm ... ... Big Encyclopedic Dictionary

Phosphorus  - (Phosphorus), P, chemical element of the V group of the periodic system, atomic number 15, atomic mass 30.97376; non-metal white (glows in air, tpl 44,14 ° C), red (tpl 593 ° C) or black (tpl 1000 ° C) color. Phosphorus is used in ... ... Illustrated Encyclopedic Dictionary

phosphorus  - a, m. phosphore m. & lt; gr. phos light + phoros carrier. Common chemical element that plays a big role in the life of animals and plants. White, red, black phosphorus. ALS 1. There are natural and art-produced phosphors ... Historical Dictionary of Russian Gallicisms

P (lat. Phosphorus * a. Phosphorus; N. Phosphor; f. Phosphore; and. Fosforo), chem. element of the V group of periodic Mendeleev's systems, at. 15, at. 30.97376 m. Natural ph. Is represented by one stable isotope 31P. 6 arts are known. ... ... Geological encyclopedia

PHOSPHORUS, phosphorus, pl. no husband (Greek phosphoros luminiferous) (chemical). A chemical element that is highly flammable and glowing in the dark, a substance found in some minerals, in the bones of animals, in animal and plant tissues. ... ... Explanatory Dictionary Ushakov

Ipi Lucifer Prosphorus, Lucifer), i.e. the light carrier. The name of the planet Venus as the morning star. As an evening star, she was called Hesper, or Vesper, and was considered the son of Astrea and Eos, the father of the Hesperides. (