Phosphorus
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Phosphorus, symbol P, reactive nonmetallic element that is important to living organisms and has many industrial uses. The atomic number of phosphorus is 15, and its atomic weight is 30.974. Phosphorus is in group 15 (or Va) of the periodic table.
Phosphorus was discovered about 1669 by the German alchemist Hennig Brand in the course of experiments in which he attempted to prepare gold from silver.
PROPERTIES AND OCCURRENCE
Phosphorus exists in three main allotropic (distinctly different) forms: ordinary (or white) phosphorus, red phosphorus, and black phosphorus. Of these, only white and red phosphorus are of commercial importance. When freshly prepared, ordinary phosphorus is white, but it turns light yellow when exposed to sunlight. It is a crystalline, translucent, waxy solid, which glows faintly in moist air and is extremely poisonous. It ignites spontaneously in air at 34° C (93° F) and must be stored under water. It is insoluble in water, slightly soluble in organic solvents, and very soluble in carbon disulfide. White phosphorus melts at 44.1° C (111.4° F) and boils at 280° C (536° F).
White phosphorus is prepared commercially by heating calcium phosphate with sand (silicon dioxide) and coke in an electric furnace. When heated to between 230° and 300° C (446° and 572° F) in the absence of air, it is converted into the red form. Red phosphorus is a microcrystalline, nonpoisonous powder. It sublimates (passes from the solid state directly to the gaseous state) at 416° C (781° F) and has a specific gravity of 2.34. Black phosphorus is made by heating white phosphorus at 200° C (392° F) at very high pressure. It has a specific gravity of 2.69.
USES
Most compounds of phosphorus are trivalent or quinquevalent. Phosphorus combines readily with oxygen to form oxides, of which the most important are phosphorous oxide and phosphoric oxide. Phosphorus oxide, a white crystalline solid, is used as a reducing agent. It is deliquescent—that is, it is dissolved by the moisture in air. The vapor is toxic. Phosphoric oxide, a white, deliquescent, amorphous solid, sublimes at 250° C (482° F). It reacts with water to form phosphoric acid and is used as a drying agent.
All of the halogens combine directly with phosphorus to form halides, which are used in the preparation of halogen acids and organic compounds. The most important commercial compounds of phosphorus are phosphoric acid and the salts of phosphoric acid, called phosphates. The bulk of phosphorus-containing compounds are used as fertilizers. Phosphorus compounds are also used in clarifying sugar solutions, weighing silk, and fireproofing, and in such alloys as phosphor bronze and phosphor copper. White phosphorus is used in the making of rat poison, and red phosphorus is used in matches.
Phosphorus was discovered about 1669 by the German alchemist Hennig Brand in the course of experiments in which he attempted to prepare gold from silver.
PROPERTIES AND OCCURRENCE
Phosphorus exists in three main allotropic (distinctly different) forms: ordinary (or white) phosphorus, red phosphorus, and black phosphorus. Of these, only white and red phosphorus are of commercial importance. When freshly prepared, ordinary phosphorus is white, but it turns light yellow when exposed to sunlight. It is a crystalline, translucent, waxy solid, which glows faintly in moist air and is extremely poisonous. It ignites spontaneously in air at 34° C (93° F) and must be stored under water. It is insoluble in water, slightly soluble in organic solvents, and very soluble in carbon disulfide. White phosphorus melts at 44.1° C (111.4° F) and boils at 280° C (536° F).
White phosphorus is prepared commercially by heating calcium phosphate with sand (silicon dioxide) and coke in an electric furnace. When heated to between 230° and 300° C (446° and 572° F) in the absence of air, it is converted into the red form. Red phosphorus is a microcrystalline, nonpoisonous powder. It sublimates (passes from the solid state directly to the gaseous state) at 416° C (781° F) and has a specific gravity of 2.34. Black phosphorus is made by heating white phosphorus at 200° C (392° F) at very high pressure. It has a specific gravity of 2.69.
USES
Most compounds of phosphorus are trivalent or quinquevalent. Phosphorus combines readily with oxygen to form oxides, of which the most important are phosphorous oxide and phosphoric oxide. Phosphorus oxide, a white crystalline solid, is used as a reducing agent. It is deliquescent—that is, it is dissolved by the moisture in air. The vapor is toxic. Phosphoric oxide, a white, deliquescent, amorphous solid, sublimes at 250° C (482° F). It reacts with water to form phosphoric acid and is used as a drying agent.
All of the halogens combine directly with phosphorus to form halides, which are used in the preparation of halogen acids and organic compounds. The most important commercial compounds of phosphorus are phosphoric acid and the salts of phosphoric acid, called phosphates. The bulk of phosphorus-containing compounds are used as fertilizers. Phosphorus compounds are also used in clarifying sugar solutions, weighing silk, and fireproofing, and in such alloys as phosphor bronze and phosphor copper. White phosphorus is used in the making of rat poison, and red phosphorus is used in matches.
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