Matches, phosphorus

More than 90 percent of commercial phosphorus production is in the form of calcium salts of phosphoric acid, H3PO4, used as fertilizers. Other significant uses of phosphorus compounds are in the manufacture of matches (phosphorus sulfides), food products and beverages (purified phosphoric acid and its salts), detergents (sodium polyphosphates), plasticizers for polymers (esters of phosphoric acid), and pesticides (derivatives of phosphoric acid). Related to the phosphorus pesticides are nerve gases, poisonons com-potmds that rapidly attack the central nervous system, initially developed during World War II. see also Deoxyribonucleic Acid (DNA) Fertilizer Pesticides. 

Phosphorus compounds are very important as fertilizers (world use 1976/77 27-3 megatonnes as P2O5) but are widely used in matches, pesticides, special glasses and china ware, alloys (sleels. phosphor bronze), and metal treating (10%), detergents (40%), electrical components (e.g. GaP), foods and drinks (15%). Phosphates are an essential constituent of living organisms. U.S. production of phosphorus 1982 372 000 tonnes. 

FLALffiRETARDANTS - PHOSPHORUS FLALffi RETARDANTS] (Vol 10) a matches TCHES] (Vol 16)... 

Phosphorus and compounds SPA Phosphoric acid Boiler blowdown Corrosion protection Detergents Fertilizers Matches Metal finishing... 

About 80-90% of the elemental P produced is reoxidized to (pure) phosphoric acid (p. 521). The rest is used to make phosphorus oxides (p. 503). sulfides (p. 506), phosphorus chlorides and oxochloride (p. 4%). and organic P compounds. A small amount is convened to red phos rftorus (see below) for use in the striking surface of matches for pyrotechnics and as a flame retarding agent (in polyamides). Bulk price for P4 is S2.00/kg. 

The large strtke-anywhere (SAW) or kitchen match has a small, easily ignitable tip composed of phosphorus sesquisulfide affixed to a larger... 

Chlorates are useful oxidizing agents. Potassium chlorate is used as an oxidant in fireworks and in matches. The heads of safety matches consist of a paste of potassium chlorate, antimony sulfide, and sulfur, with powdered glass to create friction when the match is struck as mentioned in Section 15.1, the striking strip contains red phosphorus, which ignites the match head. 

The X-ray crystallographic analysis of the unsymmetrical BisP shows a strong distortion of the five-membered chelation ring as compared to that of symmetric BisP [32]. The large difference in the steric repulsions between the bulky substituent borne on one phosphorus atom and the neighboring atoms on the one hand and the other (different) bulky substituent borne on the other phosphorus atom and the same neighboring atoms on the other hand is believed to be responsible for better steric matching with some substrates. 

Nitrogen is a colorless diatomic gas. Phosphorus has several elemental forms, but the most common is a red solid that is used for match tips. Arsenic and antimony are gray solids, and bismuth is a silvery solid. Classify these elements of Group 15 as metals, nonmetals, or metalloids. 

MRH Barium chlorate 5.06/83, calcium chlorate 5.61/77, potassium chlorate 6.07/76, sodium bromate 4.98/80, sodium chlorate 7.32/75, zinc chlorate 6.11/76 Dry finely divided mixtures of red (or white) phosphorus with chlorates, bromates or iodates of barium, calcium, magnesium, potassium, sodium or zinc will readily explode on initiation by friction, impact or heat. Fires have been caused by accidental contact in the pocket between the red phosphorus in the friction strip on safety-match boxes and potassium chlorate tablets. Addition of a little water to a mixture of white or red phosphorus and potassium iodate causes a violent or explosive reaction. Addition of a little of a solution of phosphorus in carbon disulfide to potassium chlorate causes an explosion when the solvent evaporates. The extreme danger of mixtures of red phosphorus (or sulfur) with chlorates was recognised in the UK some 50 years ago when unlicenced preparation of such mixtures was prohibited by Orders in Council. 

The sections below review the coordination chemistry of the most important classes of extractants used commercially. Particular attention is paid to the importance of secondary bonding between extractant components. This facilitates the assembly of ligating packages which match the coordination requirements of particular metal cations or their complexes and enhances both the selectivity and strength of extraction. Flydrogen bonding between ligands—e.g., esters of phosphorus(V) acids (see Section 9.17.4.3)—is particularly prevalent in the hydrocarbon solvents commonly used in industrial processes. 

Several allotropic forms of phosphorus are known, the most common of which are the white, red, and black forms. Heating the white form at 400 °C for several hours produces red phosphorus, which is known to include several forms. A red form that is amorphous can be prepared by subjecting white phosphorus to ultraviolet radiation. In the thermal process, several substances (I2, S8, and Na) are known to catalyze the conversion of phosphorus to other forms. Black phosphorus consists of four identifiable forms that result when white phosphorus is subjected to heat and pressure. Phosphorus is used in large quantities in the production of phosphoric acid and other chemicals. White phosphorus has been used extensively in making incendiary devices, and red phosphorus is used in making matches. 

Tetraphosphorus trisulfide (P4S3) which is also called phosphorus sesquisulfide, can be obtained by heating a stoichiometric mixture of phosphorus and sulfur at 180 °C in an inert atmosphere. The compound (m.p. 174 °C) is soluble in toluene, carbon disulfide, and benzene, and it is used with potassium chlorate, sulfur, and lead dioxide in matches. 

Several of these phosphorus sulfides are produced commercially for industrial applications. P4S3 is one of the key chemical constituents of strike-anywhere matches and has been used industrially for this purpose ever since 1898. P4S10 is the most widely industrially used of the phosphorus sulfides with applications in the preparation of lubricant additives and pesticides and in organic chemistry to convert carbonyl or alcohol groups into their sulfur analogues (see Section 5.4). 

Schleyer et al. very recently also investigated the stabilization and NIGS of triphosphinine. For the symmetric triphosphinine and for 1,3-diphosphinine, the (HF/6-3H-G(d)) NICS(O) is —5.9 and —7.2, respectively. The HF/6-31H-G(d,p) NICS(l) values are —9.6 and —10.3, matching favorably with the —10.8 and —11.3 values for phosphinine and benzene, respectively. This behavior indicates the rather large influence of the PC o contributions, which die out above the ring plane. Schleyer et al. also observed that with reference to the homodesmotic eq 10, for benzene (X = CH) the variation is 2—4 kcal/mol if a CH unit is replaced by phosphorus. ... 

Red phosphorus is less reactive than the white variety. It is not poisonous, but large amounts can explode. It is used in fireworks and matches. 

Red phosphors are formed either by heating white phosphorus or by exposing white phosphorus to sunlight. It is quite different from the explosive white phosphorus. For instance, when scratched on a surface, the heads of safety matches made of red phosphorus convert back to white phosphorus and ignite due to the heat of the shght friction of the match on a rough surface. Red phosphorus is also used in fireworks, smoke bombs, and pesticides and to make phosphoric acid, electroluminescent paints, and fertilizers. 

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