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. There are 23 known phosphorus isotopes 24 P - 46 P, among them one stable 31 P, and only it occurs in nature. The half-life of the isotope 30 P is 2.55 minutes; it is the first radioactive isotope produced artificially in 1934 by Frederic and Irene Joliot-Curie.

It is possible that phosphorus in its elementary form was obtained as early as the 12th century. by the Arab alchemist Alhid Behil during the distillation of urine with clay and lime, this is evidenced by an ancient alchemical manuscript kept 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 in order to obtain the philosopher's stone and the elixir of youth, with the help of which one could easily improve his financial situation. After evaporation of 50-60 buckets of urine (he took it from the soldiers' barracks) for two weeks and the subsequent strong calcination of the dry residue with coal and sand in the retort, Brand succeeded in 1669 to condense the emitted vapors under water and obtain a small amount of a yellow substance. It glowed in the dark and was therefore called by Brand "cold fire" (kaltes Feuer). Brand's contemporaries called this substance phosphorus because of its ability to glow in the dark (ancient Greek jwsjoroV). In general, since ancient times, all substances capable of emitting light in the dark have been called "phosphorus". So, the widely known "Bologna phosphorus" - barium sulfide.

In 1682 Brand published the results of his research, and now he is rightly considered the discoverer of element No. 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 Brand took advantage of this - he demonstrated phosphorus only for money or exchanged small amounts of it for gold. Despite numerous efforts, the Hamburg merchant could not fulfill his cherished dream - to obtain gold from lead with the help of "cold fire", and therefore he soon sold the recipe for the new substance to a certain Kraft from Dresden for two hundred thalers. The new owner managed to amass a much larger fortune on phosphorus - with "cold fire" he traveled all over Europe and demonstrated it to scientists, high-ranking officials and even royalty, for example, Robert Boyle, Gottfried Leibniz, Charles II. Although the method of preparing phosphorus was kept in the strictest confidence, in 1682 Robert Boyle managed to get it, but he also announced his method only 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 only in the 1770s the French chemist Antoine Laurent Lavoisier, in his works devoted to the study of the composition of air, was able to 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 environment ... Ed. E. Griffith. M., "World", 1977
Phosphorus technology... Ed. V.A. Ershova. L., "Chemistry", 1979
Corbridge D. Phosphorus: Fundamentals of Chemistry, Biochemistry, Technology... M., "World", 1982
Popular library chemical elements ... M., Science, 1983

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Phosphorus (from the Greek phosphoros - luminiferous; Latin Phosphorus) - the element periodic system 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. Concentration in seawater 0.07 mg / l. It does not occur in a free state due to its high chemical activity. Forms about 190 minerals, the most important of which are apatite Ca 5 (PO 4) 3 (F, Cl, OH) phosphorite Ca 3 (PO 4) 2 and others. Phosphorus is found in all parts green plants, even more of it in fruits and seeds (see phospholipids). Contained in animal tissues, it is a part of proteins and other important 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, as he believed that, having a golden color, it could contain gold or something needed for extraction. Initially, his method consisted in the fact that at first the urine was settled for several days until the unpleasant odor disappeared, and then it was boiled until it was sticky. 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 a white, wax-like substance were obtained, which burned very brightly and, moreover, flickered in the dark. Brand named this substance phosphorus mirabilis (Latin for "miraculous bearer of light"). Brand's discovery of phosphorus was the first discovery of a new element since antiquity.
Somewhat later, phosphorus was obtained by another German chemist, Johann Kunkel.
Independently of Brand and Kunkel, phosphorus was obtained by R. Boyle, who described it in the article "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 the Arab alchemists were still able to obtain phosphorus in the XII century.
Lavoisier proved that phosphorus is a simple substance.

origin of name

In 1669, Henning Brand, heating a mixture of white sand and evaporated urine, received a substance glowing in the dark, which was first called "cold fire". The secondary name "phosphorus" comes from the Greek words "φῶς" - light and "φέρω" - I bear. V ancient greek mythology the name Phosphorus (or Eosphorus, ancient Greek Φωσφόρος) was borne by the guardian of the Morning Star.

Receiving

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 vapors condense in the receiver under water. Instead of phosphorites, other compounds can also be reduced, for example, metaphosphoric acid:
4HPO 3 + 12C → 4P + 2H 2 + 12CO.

Physical properties

Elemental phosphorus in normal conditions represents several stable allotropic modifications; the issue of phosphorus allotropy is complex and not fully resolved. There are usually four modifications of a simple substance - white, red, black and metallic phosphorus... Sometimes they are also called the main allotropic modifications, implying that all the others are a variety of these four. Under normal conditions, there are only three allotropic modifications of phosphorus, and under ultrahigh pressures, also metal mold... All modifications differ in color, density and others physical characteristics; there is a noticeable tendency to 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 much higher than that of nitrogen. Chemical properties phosphorus is largely determined by its allotropic modification. White phosphorus very active, in the process of transition to red and black phosphorus, chemical activity decreases sharply. White phosphorus in air glows in the dark, the glow is caused by the oxidation of phosphorus vapors to lower oxides.
In the liquid and dissolved state, as well as in vapors up to 800 ° C, 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 break down into atoms.

PHOSPHORUS (Latin Phosphorus), P, chemical element of group V of the periodic system of 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. Melts at a temperature of 44.1 ° C. Let's very well dissolve in carbon disulfide CS 2. Extremely poisonous and easily ignites.
When white phosphorus is heated, red phosphorus is formed. It is a mixture of several modifications that have different molecular lengths. The color of red phosphorus, depending on the method and conditions of production, can vary from light red to violet and dark brown. Its melting point is 585-600 °.
Black phosphorus is the most stable modification. By outward appearance it looks like graphite. Unlike white phosphorus, red and black phosphorus do not dissolve in carbon disulfide, they are not poisonous or flammable.
Phosphorus is chemically more reactive than nitrogen. The chemical activity of phosphorus depends on the allotropic modification in which it is located. Thus, the most active is white phosphorus, and the least active is black phosphorus.
In equations chemical reactions white phosphorus is usually written by the formula P 4, which corresponds to the composition of its molecules. The 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 simple substances- non-metals. Phosphorus can react with many non-metals: oxygen, sulfur, halogens, phosphorus does not react with hydrogen. Depending on whether there is an excess or deficiency of phosphorus, 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
Phosphides of some metals can be decomposed by water to form phosphine gas PH 3:
Mg 3 P 2 + 6H 2 O = 3Mg (OH) 2 + 2PH 3
Phosphine PH? chemically similar to ammonia NH ?.
3. Interaction with alkalis. When white phosphorus is heated in an alkali solution, it disproportionates:
0 -3 +1
P 4 + 3NaOH + 3H 2 O = PH 3 + 3NaH 2 PO 2

Receiving. Phosphorus is industrially obtained from calcium phosphate Ca 3 (PO 4) 2, which is isolated from phosphorites and fluorapatites. The preparation method is based on the reduction reaction of Ca 3 (PO 4) 2 to phosphorus.
Coke (carbon) is used as a reducing agent for phosphorus compounds. To bind calcium compounds, add to the reaction system quartz sand SiO 2. 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 has yellow, therefore, in the industry it is called yellow phosphorus.

Phosphate fertilizers... Phosphorus, like nitrogen, is important element to ensure the growth and life of plants. Plants extract phosphorus from the soil, so it must be replenished by periodically adding phosphorus fertilizers. Phosphate fertilizers are produced from calcium phosphate, which is part of natural phosphorites and fluorapatites.
The simplest phosphoric fertilizer - phosphate rock is ground phosphorite Ca 3 (PO 4) 2. This fertilizer is difficult to dissolve, it can be absorbed by plants only on acidic soils.
The action of sulfuric acid on calcium phosphate produces a simple superphosphate, the main component of which is calcium dihydrogen phosphate Ca (H 2 PO 4) 2. It is a soluble substance and is well absorbed by plants. Method of obtaining simple superphosphate based on reaction
Ca 3 (PO 4) 2 + 2H 2 SO 4 = Ca (H 2 PO 4) 2 + 2CaSO 4
In addition to the main component, superphosphate contains up to 50% calcium sulfate, which is a 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 phosphorus fertilizers are prepared on the basis of super phosphoric acid- mixtures of polyphosphoric acids H 4 P 2 O 7, H 5 P 3 O 10, etc. These acids are formed by heating phosphoric acid H 3 PO 4 in a vacuum.
When polyphosphoric acids interact with ammonia, ammonium polyphosphates are formed, which are used as complex nitrogen-phosphorus fertilizers.
Together with nitrogen, phosphorus is included in some other complex fertilizers, for example, ammophos and diammophos.

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

Obtaining: mined from apatite and phosphorite.

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

Application: main consumer - Agriculture(phosphate fertilizers); used in match production, metallurgy (deoxidizer and a component of some alloys), in organic synthesis, etc.

Phosphorus

PHOSPHORUS-a; m.[from the Greek. phōsphoros - luminiferous] Chemical element (P) that plays important role in the life of animals and plants (contained in some minerals, in the bones of animals, in animal and plant tissues). Red F. Black F. Fish contains 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).

(Latin Phosphorus), a chemical element of group V of the periodic system. Named from the Greek. phōsphóros - luminiferous. 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), is poisonous; red is less active chemically, poisonous. Extracted from apatite and phosphorite. The main consumer is agriculture (phosphate fertilizers); it is used in match production, metallurgy (a deoxidizer and a component of some alloys), in organic synthesis, etc. It is present in living cells in the form of ortho- and pyrophosphoric acids and their derivatives.

Phosphorus (Latin - Phosphopus), P (read "pe"), a chemical element with atomic number 15, atomic mass 30.973762. Located in group VA in the 3rd period of the periodic system. Has one stable nuclide 31 R. Configuration of the outer electron layer 3 s 2 R 3 ... In compounds, it exhibits oxidation states from –3 to +5. Valences from III to V. The most stable oxidation state in compounds is +5.
The radius of the neutral atom P is 0.134 nm, the ion radius is: 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. Pauling electronegativity (cm. POLING Linus) 2.10. Non-metal.
Discovery history
The first to receive phosphorus in a free state in 1669 was the Hamburg alchemist H. Brand (there is evidence that a substance similar in properties was obtained in the 12th century by the Arab alchemist Behil). In Search of the Philosopher'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 reagents began to glow in the dark with a white light (this was phosphorus, reduced from its compounds contained in urine).
In 1680 the Englishman R. Boyle received phosphorus glowing in the dark (from the Greek "phosphoros" - luminiferous). (cm. BOYLE Robert) In subsequent years, it was found that phosphorus is contained not only in urine, but also in the tissues of the brain, in the bones of the skeleton. The simplest method for obtaining phosphorus by calcining bone ash with coal was proposed in 1771 by K. Scheele (cm. SCHEELE Karl Wilhelm)... The elementary nature of phosphorus was established at the end of the 18th century by A.L. Lavoisier. (cm. LAVOISIER Antoine Laurent)
Being in nature
Content in the earth's crust is 0.105% by mass, which is significantly higher than the content of, for example, nitrogen (cm. NITROGEN)... In seawater 0.07 mg / l. Phosphorus is not found in free form in nature, but it is included in 200 different minerals. The most famous phosphorite (cm. PHOSPHORITES) calcium Ca 3 (PO 4) 3, apatite (cm. APATITES)(fluorapatite 3Ca 3 (PO 4) 3 CaF 2, or Ca 5 (PO 4) 3 F), monazite (cm. MONACITH), turquoise (cm. TURQUOISE)... Phosphorus is part of all living organisms.
Receiving
Phosphorus is produced by electrothermal reduction from phosphorites and apatites at 1400-1600 ° C with coke in the presence of silica:
2Ca 3 (PO 4) 2 + 6SiO 2 + 10C = P 4 + 6CaSiO 3 + 10CO
4Ca 5 (PO 4) 3 F + 21SiO 2 + 30C = 3P 4 + 20CaSiO 3 + 30CO + SiF 4
The evolved vapors P 4 are further treated with superheated steam to obtain thermal phosphoric acid H 3 PO 4:
P 4 + 14H 2 O = 4H 3 PO 4 + 8H 2
When P 4 vapor is desublimated, white phosphorus is formed. It is processed into red phosphorus by heating without air access at a temperature of 200-300 ° C in reactors equipped with a screw grinder of the reaction mass.
Structural features of allotropic modifications and their physical properties
Elementary phosphorus exists in several allotropic modifications, the main ones being: white (phosphorus III), red (phosphorus II) and black (phosphorus I).
White phosphorus is a waxy, transparent substance with a characteristic odor. Consists of tetrahedral P 4 molecules, which can rotate freely. White phosphorus has a molecular-type cubic crystal lattice, cell parameter a= 1.851 nm. Density 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 has not been established and there is no free rotation of Р 4 molecules. Dielectric. Dissolves in ethyl alcohol, benzene, carbon disulfide CS 2.
By heating white phosphorus without access to air at 250-300 ° C, red phosphorus is obtained. Impurities of sodium, iodine and selenium and UV rays accelerate the transition from one modification to another.
Red phosphorus is amorphous, ranging in color from scarlet to dark brown and purple. There are several crystalline forms with different properties. Crystalline red phosphorus (Hittorfa phosphorus) is obtained by cooling a solution of red phosphorus saturated at a temperature of 600 ° C in molten lead. It has a monoclinic lattice, unit cell parameters a= 1.02 nm, v= 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 a= 0.3314 nm, v= 0.4376 nm, c = 1.0478 nm. The density of black phosphorus is 2.702 kg / dm 3. Outwardly similar to graphite; semiconductor, diamagnetic. When heated to 560-580 ° C, it turns into red phosphorus. Black phosphorus is inactive and hardly ignites.
Chemical properties
Phosphorus in 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 oxidizes in air. Oxidation occurs by the mechanism chain reactions and is accompanied by chemiluminescence. When phosphorus burns in an 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 ignites spontaneously in air due to the heat released during oxidation. Red phosphorus oxidizes slowly in air, does not self-ignite. Black phosphorus does not oxidize in air.
Phosphorus (V) oxide - acid oxide... It reacts with water, producing a lot of heat. In this case, polymeric metaphosphoric acid (HPO 3) n is first formed. When processing hot water it turns into a tribasic orthophosphoric acid of medium strength H 3 PO 4:
P 4 O 10 + 2H 2 O = (HPO 3) 4; (NRO 3) 4 + 4H 2 O = 4H 3 PO 4
or P 2 O 5 + 3H 2 O = 2H 3 PO 4
Phosphorus reacts with halogens to generate a lot of heat. With F, Cl, Br forms trihalides and penthalides, with I - only PI 3 triodide. 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 + 5HCl
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 consists of two triangular pyramids with a common face. Phosphorus oxyhalides 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. Phosphorus oxysulfides are known: 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 potassium hydroxide solution KOH, gaseous phosphine PH 3 is formed:
4P + 3KON + 3H 2 O = 3KN 2 PO 2 + PH 3
In this case, diphosphine P 2 H 4 is also formed as an impurity. Both phosphines have a characteristic rotten fish odor.
Phosphine PH 3 chemically resembles ammonia NH 3, but is less stable.
Phosphorus reacts with metals when fused. With alkaline earth forms ionic phosphides М 3 Р 2, which decompose on contact with water:
Mg 3 P 2 + 6H 2 O = 3Mg (OH) 2 + 2PH 3,
Ca 3 R 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, monohydrogen phosphates, Na 2 HPO 4 and dihydrogen phosphates, Ca (H 2 PO 4) 2); metaphosphoric acid (HPO 3) n(its salts are metaphosphates), monobasic 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 mineral fertilizers, match production. Phosphorus is used in the production of non-ferrous metal alloys as a deoxidizing agent and as an alloying additive. It is used in the production of soft magnetic alloys, in the production of semiconductor phosphides. Phosphorus compounds are used as precursors for the production of medicines.
Content in the body
Phosphorus is present in living cells in the form of ortho- and pyrophosphoric acids, is a part of nucleotides, nucleic acids, phosphoproteins, phospholipids, coenzymes, and enzymes. Human bones are composed of hydroxylapatite 3Ca 3 (PO 4) 3 · CaF 2. Tooth enamel contains fluorapatite. The main role in the conversion of phosphorus compounds in the human and animal body 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 in the body, various bone diseases develop.
Physiological action
Phosphorus compounds are toxic. The lethal dose of white phosphorus is 50-150 mg. When it gets on the skin, white phosphorus causes severe burns. The chemical warfare agents sarin, soman, and herd are phosphorus compounds. Acute phosphorus poisoning is manifested by burning in the mouth and stomach, headache, weakness, vomiting. Jaundice develops after 2-3 days. 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. In case of skin burns, treat the affected areas with solutions copper sulfate or soda. The maximum concentration limit for phosphorus vapors in the air is 0.03 mg / m 3. Dust of red phosphorus, entering the lungs, causes pneumonia.

encyclopedic Dictionary . 2009 .

See what "phosphorus" is in other dictionaries:

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

PHOSPHORUS- Phosphorus, chem. element (symbol P) with at. v. 31.02, belonging to the V group and the 3rd row of the periodic system of Mendeleev (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 ... ... Great medical encyclopedia

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

- (symbol P), a chemical element of the fifth group of the periodic table, first discovered in 1669. Found as PHOSPHATES in minerals, the main source of phosphorus is APATITE. This element is used for the manufacture of PHOSPHORIC ACID, ... ... Scientific and technical encyclopedic dictionary

- (Phosphorus), P, chemical element of group V of the periodic system, atomic number 15, atomic mass 30.97376; non-metal white (glows in air, tm 44.14shC), red (tm 593shC) or black (tm 1000shC) color. Phosphorus is used in ... ... Modern encyclopedia

- (Latin Phosphorus) P, chemical element of group V of Mendeleev's periodic system, atomic number 15, atomic mass 30.97376. The name is from the Greek. phosphoros is luminiferous. Forms several modifications White phosphorus (density 1.828 g / cm & sup3, tmelt ... ... Big Encyclopedic Dictionary

Phosphorus- (Phosphorus), P, chemical element of group V of the periodic system, atomic number 15, atomic mass 30.97376; non-metal white (glows in air, tp 44.14 ° C), red (tp 593 ° C) or black (tm 1000 ° C). Phosphorus is used in ... ... Illustrated Encyclopedic Dictionary

phosphorus- a, m. phosphore m.gr. phos light + phoros carrier. A common chemical element that plays an important 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 (Latin Phosphorus * a. Phosphorus; N. Phosphor; F. phosphore; I. fosforo), chem. element of group V periodic. Mendeleev system, at.n. 15, at. m. 30.97376. Natural phosphorus is represented by one stable isotope, 31P. 6 arts are known. ... ... Geological encyclopedia

Phosphorus, phosphorus, pl. no, husband. (Greek phosphoros luminiferous) (chem.). A chemical element, a highly flammable and glowing in the dark substance found in some minerals in animal bones, in animal and plant tissues. ... ... Dictionary Ushakova

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