| Phosphorous
CAS: 7723-14-0 Description: Soft white waxy solid, brownish-red powder or black solid Classification: Non-metal Date of Discovery: 1669 Discoverer: Hennig Brand Name Origin: Greek phôs, "light", and phoros "bearer"; ancient name for planet Venus |
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Atomic Number: 15
Number of Neutrons: 16 Atomic Mass: 30.973762(4) amu Melting Point: 44.15 °C Boiling Point: 280.5 °C Density (293 K): 1.82 g/cm3 (white) 2.20 g/cm3 (red) 2.25-2.69 g/cm3 (black) Atomic volume: 17.0 cm3/mol Electrical resistivity: 1.0e-17 10-6/cm 
Thermal conductivity: 0.00235 W/cmK Enthalpy of atomization: 314.64 kJ/mol Enthalpy of vaporization: 12.129 kJ/mol Enthalpy of fusion: 0.657 kJ/mol Specific heat capacity: 0.77 J/gK |
Energy levels: 2-8-5
Electron configuration: [Ne]3s23p3 Crystal Structure: Monoclinic Atomic radius: 1.23 Å Covalent radius: 1.06 Å Oxidation States: -3, +3, +4, +5 Electronegativity, Pauling: 2.19 Electron affinity: 0.7465 eV First ionization energy: 10.486 eV 2nd ionization energy: 19.725 eV 3rd ionization energy: 30.18 eV Polarizability: 3.63 10-24cm3 |
| Isotope | Natural Abundance | Atomic Mass | Half-life | Decay Mode | Spin |
| 26P | 26.0118 |  20 ms |
 +, p |
3+ | |
| 27P | 26.99919 | 0.3 s | - |
1/2+ | |
| 28P | 27.992312 | 270 ms | + |
3+ | |
| 29P | 28.981801 | 4.14 s | + |
1/2+ | |
| 30P | 29.978314 | 2.50 m | + |
1+ | |
| 31P | 100. | 30.9737615 | Stable | 1/2+ | |
| 32P | 31.9739071 | 14.28 d | - |
1+ | |
| 33P | 32.971725 | 25.3 d | - |
1/2+ | |
| 34P | 33.973636 | 12.4 s | - |
1+ | |
| 35P | 34.973314 | 47 s | - |
1/2+ | |
| 36P | 35.97826 | 5.7 s | - |
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| 37P | 36.97961 | 2.3 s | - |
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| 38P | 37.9845 | 0.6 s | - |
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| 39P | 38.9864 | 0.16 s |
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| 40P | 39.9911 | ||||
| 41P | 40.9948 | 0.12 s | |||
| 42P | 42.001 | 0.11 s | - |
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Phosphorus exists in four or more allotropic forms: white (or yellow), red, and black (or violet). White phosphorus has two modifications: alpha and beta with a transition
temperature at -3.8 °C. Never found free in nature, it is widely distributed in combination with minerals. Seventeen isotopes of phosphorus are recognized. Phosphate rock, which contains the mineral apatite, an impure tri-calcium phosphate, is an important source of the element. Large deposits are found in the U.S.S.R., in Morocco, and in Florida, Tennessee, Utah, Idaho, and elsewhere. Phosphorus in an essential ingredient of all cell protoplasm, nervous tissue, and bones. Ordinary phosphorus is a waxy white solid; when pure it is colorless and transparent. It is insoluble in water, but soluble in carbon disulfide. It takes fire spontaneously in air, burning to the
pentoxide. It is very poisonous, 50 mg constituting an approximate fatal dose. Exposure to white phosphorus should not exceed 0.1 mg/cu. m (8-hour time-weighted average - 40-hour work week). White phosphorus should be kept under water, as it is dangerously reactive in air, and it should be handled with forceps, as contact with the skin
may cause severe burns. When exposed to sunlight or when heated in its own vapor to 250 °C, it is converted to the red variety, which does not phosphoresce in air as does the white variety. This form does not ignite spontaneously and it is not as dangerous as white phosphorus. It should, however, be handled with care as it does convert to the white form at some temperatures and it emits highly toxic fumes of the oxides of phosphorus when heated. The red modification is fairly stable, sublimes with a vapor pressure of 1 atm at 4l7 °C, and is used in the manufacture of safety matches,
pyrotechnics, pesticides, incendiary shells, smoke bombs, tracer bullets, etc. White phosphorus may be made by several methods. By one process, tricalcium phosphate, the essential ingredient of phosphate rock, is heated in the presence of carbon and silica in an electric furnace or fuel-fired furnace. Elementary phosphorus is liberated as vapor and may be collected under water. If desired, the phosphorus vapor and carbon monoxide produced by the reaction can be oxidized at once in the presence of moisture to produce phosphoric acid, an important compound in making super-phosphate fertilizers. In recent years, concentrated phosphoric acids, which may contain as much as 70 to 75% P2O5 content, have become of great importance to agriculture and farm production. Worldwide demand for fertilizers has caused record phosphate production. Phosphates are used in the production of special glasses, such as those used for sodium lamps. Bone-ash, calcium phosphate, is also used to produce fine chinaware and to produce mono-calcium phosphate used in baking powder.
Phosphorus is also important in the production of steels, phosphor bronze, and many other products. Trisodium phosphate is important as a cleaning agent, as a water softener, and for preventing boiler scale and corrosion of pipes and boiler tubes. Organic compounds of phosphorus are important.
LINKS: Giant Soybeans Suck Up Phosphorus from the Soil Interception and Inactivation of Phosphorus in Lakes and Ponds Phosphorus Chemistry Phosphorus Nutrition Info. Phosphorus Metabolism Disorders Phosphorus Pollution Phosphorus Research Web United Phosphorus Limited Return
Sources for the information on this website include: Lide, David R., ed. CRC Handbook of Chemistry and Physics, 78th Ed., 1997-1998. |
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