Phosphorus (P)
nonmetalSolid
Peso atomico standard
30,973762 uConfigurazione elettronica
[Ne] 3s2 3p3Punto di fusione
44,15 °CPunto di ebollizione
280,5 °CDensità
1820 kg/m³Stati di ossidazione
−3, −2, −1, 0, +1, +2, +3, +4, +5Elettronegatività (Pauling)
2,19Energia di ionizzazione (1ª)
10,486686 eVAnno della scoperta
1669Raggio atomico
100 pmDettagli
Phosphorus is a reactive nonmetal in group 15 and is essential to life as a component of nucleic acids, phospholipids, and energy-transfer molecules. It does not occur naturally as the free element because it is readily oxidized, but it is abundant in phosphate minerals. Elemental phosphorus is notable for its several allotropes, especially highly reactive white phosphorus and more stable red and black forms.
Phosphorus exists in four or more allotropic forms: white (or yellow), red, and black (or violet). Ordinary phosphorus is a waxy white solid; when pure it is colorless and transparent. White phosphorus has two modifications: alpha and beta with a transition temperature at -3.8°C.
It is insoluble in water, but soluble in carbon disulfide. It takes fire spontaneously in air, burning to the pentoxide.
The name derives from the Greek phosphoros for "bringing light" because it has the property of glowing in the dark. This was also the ancient name for the planet Venus, when it appears before sunrise. Phosphorus was discovered by the German merchant Hennig Brand in 1669.
In what is perhaps the most disgusting method of discovering an element, phosphorus was first isolated in 1669 by Hennig Brand, a German physician and alchemist, by boiling, filtering and otherwise processing as many as 60 buckets of urine. Thankfully, phosphorus is now primarily obtained from phosphate rock (Ca3(PO4)2).
From the Greek phosphoros, light bearing; ancient name for the planet Venus when appearing before sunrise. Brand discovered phosphorus in 1669 by preparing it from urine.
White phosphorus consists of soft, waxy, pale material made of P₄ molecules and may glow faintly in air. Red phosphorus is a dark red to violet amorphous or polymeric solid. Black phosphorus is a layered, dark, graphite-like crystalline solid and is the most thermodynamically stable allotrope at ordinary conditions.
Most phosphorus is used indirectly through phosphate compounds, especially fertilizers, animal feed supplements, detergents where permitted, food additives, and industrial phosphates. Elemental white phosphorus has military use in smoke, illumination, and incendiary munitions, subject to legal restrictions. Red phosphorus is used on safety-match striking surfaces, in some flame-retardant systems, and as a reagent in chemical synthesis. Black phosphorus is studied for electronic and optoelectronic materials, but it is not a bulk commodity.
Phosphorus has three main allotropes: white, red and black. White phosphorus is poisonous and can spontaneously ignite when it comes in contact with air. For this reason, white phosphorus must be stored under water and is usually used to produce phosphorus compounds. Red phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight. Red phosphorus is not poisonous and is not as dangerous as white phosphorus, although frictional heating is enough to change it back to white phosphorus. Red phosphorus is used in safety matches, fireworks, smoke bombs and pesticides. Black phosphorus is also formed by heating white phosphorus, but a mercury catalyst and a seed crystal of black phosphorus are required. Black phosphorus is the least reactive form of phosphorus and has no significant commercial uses.
Phosphoric acid (H3PO4) is used in soft drinks and to create many phosphate compounds, such as triple superphosphate fertilizer (Ca(H2PO4)2·H2O). Trisodium phosphate (Na3PO4) is used as a cleaning agent and as a water softener. Calcium phosphate (Ca3(PO4)2) is used to make china and in the production of baking powder. Some phosphorus compounds glow in the dark or emit light in response to absorbing radiation and are used in fluorescent light bulbs and television sets.
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. World-wide 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 used to create 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.
Phosphorus is also an essential ingredient of all cell protoplasm, nervous tissue, and bones.
Isotopes in Biology
32P (half-life of 14.3 days) is a radioactive isotope of phosphorus that is used to help understand the biological and chemical processes in plants. It is chemically identical to other isotopes of phosphorous and can be substituted in biological and chemical reactions. For example, a phosphate solution containing 32P (which has the identical behavior of non-radioactive 31P) can be inserted into the roots of a plant and its movement can then be tracked throughout the plant with the use of a Geiger counter. This movement detection study helps scientists to better understand how plants use phosphorous to reproduce and grow [131] B. Singh, J. Singh, A. Kaur. Int. J. Biotechnol. Bioeng. Res.4, 167 (2013)., [132] S. N. Levine, M. P. Stainton, D. W. Schindler. Can. J. Fish. Aquat.Sci.43, 366 (1986)..
At the molecular level, 32P can substitute for 31P in nucleotides of DNA or RNA (ribonucleic acid, a single stranded molecule that regulates genes). Radioactive probes can be created to help identify the presence, absence, and quantity of genes in a system [133] E. K. J. Pauwels, F. J. Cleton. Radiother. Oncol.1, 333 (1984)., [134] C. B. Wilson, A. A. Epenetos. Baillieres Clin. Gastroenterol.1, 115 (1987)..
Isotopes in Earth/Planetary Science
32P has been used as a tracer to help determine phosphorus nutrient cycling in eutrophied lakes (lakes rich in organic and mineral nutrients commonly leading to the excessive growth of phytoplankton, a self-feeding water organism) (Fig. IUPAC.15.1). In one experiment, phosphoric acid labeled with 32P was added to a lake that had been experimentally eutrophied. 32P was measured in microphytoplankton (plankton visible only with a microscope), phytoplankton, and zooplankton (tiny animals that live suspended in fresh or salt water), and the amount of incorporated 32P was determined [132] S. N. Levine, M. P. Stainton, D. W. Schindler. Can. J. Fish. Aquat.Sci.43, 366 (1986)..
33P has been used to better understand phosphorus dynamics in the environment at the sediment-surface level. Phosphorus is a necessary nutrient for many biota (the plant and animal life of a particular habitat, region, or geological period). Understanding bioavailability and sorption (bonding) of this nutrient to particles in soil is important for understanding ecosystem health. Organic and inorganic phosphorus substrates isotopically labeled with 33P can be tracked within a sediment system to determine their transport properties and availability to biota [135] L. Tuominen, H. Hartikainen, T. Kairesalo, P. Tallberg. Water Res.32, 2001 (1998)..
Isotopes in Industry
32P was added to tires in the 1950s by Goodrich Laboratories to help determine the location and depth of tire wear in performance tests [136] Popular Science Monthly: Mechanic and Handicraft, 91 (1951)..
Isotopes in Medicine
Beta emissions from the radioactive isotope 32P can be used in drug therapy of cancerous bone masses. By injecting a patient with a 32P pharmaceutical, tumors and other cells can be targeted for cell death, which also helps to alleviate pain [137] E. B. Silberstein, A. H. Elgazzar, A. Kapilivsky. Semin. Nucl. Med.22, 17 (1992)., [138] S. C. Srivastava. Braz. Arch. Biol. Technol.45, 45 (2002).. For example, Polycythemia vera is the condition of having excess red blood cells in the bone marrow: 32P can be used to treat this condition by reducing the number of red blood cells. However, there is no cure for this condition [139] Mayo Clinic staff. Polycythemia Vera: Treatments and Drugs, Mayo Clinic (2017), April 4; http://www.mayoclinic.org/diseases-conditions/polycythemia-vera/diagnosis-treatment/treatment/txc-20307498.. Using a 32P labeled bio-silicone product, 32P has been used as the radioactive target in brachytherapy of solid tumors in the lung [140] A. S. W. Goh, A. Y. F. Chung, R. H. G. Lo, T. N. Lau, S. W. K. Yu, M. Chng, S. Satchithanantham, S. L. E. Loong, D. C. E. Ng, B. C. Lim, S. Connor, P. K. H. Chow. Int. J. Radiat. Oncol. Biol. Phys.67, 786 (2007).. Depending on the type of 32P-labeled compound (antibody or pharmaceutical drug), when it is ingested or injected into the body, specific body parts (blood, tumors, joints, or bones) can be targeted for visualization and imaged using a gamma camera. This is useful for imaging cancer sites and for treatment monitoring of oncologic patients [133] E. K. J. Pauwels, F. J. Cleton. Radiother. Oncol.1, 333 (1984)., [134] C. B. Wilson, A. A. Epenetos. Baillieres Clin. Gastroenterol.1, 115 (1987)., [138] S. C. Srivastava. Braz. Arch. Biol. Technol.45, 45 (2002)..
Phosphorus commonly forms compounds in the −3, +3, and +5 oxidation states. Phosphate chemistry, based on the PO₄³⁻ ion, dominates its geology and biology; calcium phosphate phases include apatite minerals and bone mineral. Phosphoric acid (H₃PO₄) is a major industrial acid and a precursor to many salts. Phosphorus trichloride (PCl₃) and phosphorus pentachloride (PCl₅) are important chlorinating and phosphorus-transfer reagents. Phosphine (PH₃) contains phosphorus in a reduced state and is toxic and flammable.
See more information at the Phosphorus compound page.
White phosphorus is pyrophoric, causes severe chemical burns, and is acutely toxic; it is commonly stored under water or inert atmosphere. Red phosphorus is much less reactive but can ignite if finely divided or contaminated with oxidants. Phosphine (PH₃) is a highly poisonous gas. Phosphate nutrients are biologically necessary, but concentrated acids, salts, dusts, and industrial reagents require normal chemical controls.
Phosphorus is very poisonous, 50 mg constituting an approximate fatal dose. Exposure to white phosphorus should not exceed 0.1 mg/m3 (8-hour time-weighted average per 40-hour work week). White phosphorus should be kept under water (as it is dangerously reactive in air) and should be handled with forceps, as contact with the skin may cause severe burns.
Phosphorus cycles mainly as phosphate in rocks, soils, waters, and organisms. Weathering releases phosphate, while biological uptake and sedimentation return it to soils and aquatic sediments. It is often a limiting nutrient in freshwater and some terrestrial systems. Excess runoff from fertilizers, manure, and wastewater can promote eutrophication and harmful algal growth. There is no significant atmospheric reservoir comparable to nitrogen.
Phosphorus supply is based chiefly on mining phosphate rock, especially apatite-rich sedimentary deposits and some igneous deposits. Most mined material is converted to phosphoric acid (H₃PO₄) or processed directly for fertilizer production. Elemental phosphorus is made industrially by reducing phosphate rock with carbon in electric furnaces in the presence of silica, but this route is energy intensive and serves smaller chemical markets. Supply concerns focus on ore grade, impurities such as cadmium or uranium in some deposits, transport costs, and the concentration of high-quality reserves. Recycling from manure, sewage sludge, and food-system wastes is increasingly important but not yet a full substitute for mined phosphate.
Never found free in nature, it is widely distributed in combination with minerals. Phosphate rock, which contains the mineral apatite, an impure tri-calcium phosphate, is an important source of the element. Large deposits are found in Russia, in Morocco, and in Florida, Tennessee, Utah, Idaho, and elsewhere.
Phosphorus is far less abundant cosmically than carbon, nitrogen, oxygen, or sulfur. It is produced in massive stars and supernova-related nucleosynthesis and is incorporated into interstellar dust, meteorites, and planetary crusts. In the Solar System it occurs mainly in phosphate minerals and, in reduced meteoritic settings, in phosphides such as schreibersite.
- White phosphorus was historically called a light-bearing substance because it slowly oxidizes and glows in moist air.
- Safety matches separate the oxidizer in the match head from red phosphorus on the striking surface.
- Black phosphorus can be exfoliated into phosphorene, a two-dimensional semiconductor studied in research.
- Phosphate rock may contain variable trace metals, so ore source affects fertilizer impurity profiles.
- Phosphorus has only one stable isotope, ³¹P.
Immagini
Proprietà
Fisiche
- Raggio atomico (empirico)
- 100 pm Confronta Raggio atomico (empirico) di tutti gli elementi →
- Raggio covalente
- 107 pm Confronta Raggio covalente di tutti gli elementi →
- Raggio di van der Waals
- 180 pm Confronta Raggio di van der Waals di tutti gli elementi →
- Raggio metallico
- 110 pm Confronta Raggio metallico di tutti gli elementi →
- Densità
- 1820 kg/m³ Confronta Densità di tutti gli elementi →
- Volume molare
- 0,017 L/mol
- Fase in condizioni STP
- Solido Confronta Fase in condizioni STP di tutti gli elementi →
- Punto di fusione
- 44,15 °C Confronta Punto di fusione di tutti gli elementi →
- Punto di ebollizione
- 280,5 °C Confronta Punto di ebollizione di tutti gli elementi →
- Capacità termica specifica
- 0,769 J/(g·K) Confronta Capacità termica specifica di tutti gli elementi →
- Capacità termica molare
- 23,824 J/(mol·K) Confronta Capacità termica molare di tutti gli elementi →
- Struttura cristallina
- Cubica Confronta Struttura cristallina di tutti gli elementi →
Chimiche
- Elettronegatività (Pauling)
- 2,19 Confronta Elettronegatività (Pauling) di tutti gli elementi →
- Elettronegatività (Allen)
- 2,253
- Affinità elettronica
- 0,7466 eV
- Energia di ionizzazione (1ª)
- 10,486686 eV Confronta Energia di ionizzazione (1ª) di tutti gli elementi →
- Energia di ionizzazione (2ª)
- 19,769558 eV Confronta Energia di ionizzazione (2ª) di tutti gli elementi →
- Energia di ionizzazione (3ª)
- 30,202744 eV Confronta Energia di ionizzazione (3ª) di tutti gli elementi →
- Energia di ionizzazione (4ª)
- 51,444047 eV Confronta Energia di ionizzazione (4ª) di tutti gli elementi →
- Energia di ionizzazione (5ª)
- 65,025334 eV Confronta Energia di ionizzazione (5ª) di tutti gli elementi →
- Stati di ossidazione
- −3, −2, −1, 0, +1, +2, +3, +4, +5 Confronta Stati di ossidazione di tutti gli elementi →
- Elettroni di valenza
- 5 Confronta Elettroni di valenza di tutti gli elementi →
- Allotropi
- ["red", "white"]
- Configurazione elettronica
- [Ne] 3s2 3p3
Termodinamiche
- Punto critico (temperatura)
- 721 °C
- Calore di fusione
- 0,00684044 eV Confronta Calore di fusione di tutti gli elementi →
- Calore di vaporizzazione
- 0,12851739 eV Confronta Calore di vaporizzazione di tutti gli elementi →
- Calore di sublimazione
- 3,271597 eV
- Calore di atomizzazione
- 3,271597 eV
- Entalpia di atomizzazione
- 3,280303 eV
Nucleari
- Protoni
- 15 Confronta Protoni di tutti gli elementi →
- Neutroni
- 16 Confronta Neutroni di tutti gli elementi →
- Isotopi noti
- 24 Confronta Isotopi noti di tutti gli elementi →
- Isotopi stabili
- 1 Confronta Isotopi stabili di tutti gli elementi →
- Isotopo più stabile
- P-31
- Anno della scoperta
- 1669
Abbondanza
- Abbondanza (crosta terrestre)
- 1050 mg/kg Confronta Abbondanza (crosta terrestre) di tutti gli elementi →
- Abbondanza (oceano)
- 0,06 mg/L Confronta Abbondanza (oceano) di tutti gli elementi →
Struttura cristallina
- Costante reticolare a
- 717 pm
Struttura elettronica
- Elettroni per guscio
- 2, 8, 5 Confronta Elettroni per guscio di tutti gli elementi →
Identificativi
- Numero CAS
- 7723-14-0 Confronta Numero CAS di tutti gli elementi →
- Simbolo di termine
- 4S°3/2
- InChI
- InChI=1S/P
- Chiave InChI
- OAICVXFJPJFONN-UHFFFAOYSA-N
Configurazione elettronica Misurato
P: 3s² 3p³[Ne] 3s² 3p³1s² 2s² 2p⁶ 3s² 3p³Modello atomico
Gli isotopi modificano il numero di neutroni, la massa e la stabilità — non la configurazione elettronica di un atomo neutro.
Modello atomico schematico, non in scala.
Impronta atomica
Spettro di emissione / assorbimento
Distribuzione isotopica
| Numero di massa | Massa atomica (u) | Abbondanza naturale | Emivita |
|---|---|---|---|
| 31 Stabile | 30,97376199842 ± 0,0000000007 | 100,0000% | Stabile |
Fase / Stato
Motivo: 19,2 °C sotto il punto di fusione (44,15 °C)
Schema non in scala
Punti di transizione di fase
Energie di transizione
Energia necessaria per fondere 1 mol al punto di fusione
Energia necessaria per vaporizzare 1 mol al punto di ebollizione
Energia necessaria per sublimare 1 mol al punto di sublimazione
Densità
In condizioni standard
In condizioni standard
Avanzate
Spettri atomici
Sono visualizzati 10 di 15. Ordinamento per carica ionica crescente.
Righe disponibili ?
| Ione | Carica | Righe totali | Probabilità di transizione | Designazioni dei livelli |
|---|---|---|---|---|
| P I | 0 | 258 | 132 | 133 |
| P II | +1 | 100 | 73 | 73 |
| P III | +2 | 70 | 23 | 23 |
| P IV | +3 | 129 | 78 | 78 |
| P V | +4 | 48 | 30 | 30 |
| P VI | +5 | 5 | 5 | 5 |
| P VII | +6 | 3 | 3 | 3 |
| P VIII | +7 | 20 | 20 | 20 |
| P IX | +8 | 47 | 47 | 47 |
| P X | +9 | 26 | 26 | 26 |
Livelli disponibili ?
| Ione | Carica | Livelli |
|---|---|---|
| P I | 0 | 289 |
| P II | +1 | 162 |
| P III | +2 | 129 |
| P IV | +3 | 211 |
| P V | +4 | 68 |
| P VI | +5 | 60 |
| P VII | +6 | 62 |
| P VIII | +7 | 65 |
| P IX | +8 | 48 |
| P X | +9 | 58 |
Raggi ionici
| Carica | Coordinazione | Spin | Raggio |
|---|---|---|---|
| +3 | 6 | N/D | 44 pm |
| +5 | 4 | N/D | 17 pm |
| +5 | 5 | N/D | 28.999999999999996 pm |
| +5 | 6 | N/D | 38 pm |
Composti
Isotopi (1)
| Numero di massa | Massa atomica (u) | Abbondanza naturale | Emivita | Modalità di decadimento | |
|---|---|---|---|---|---|
| 31 Stabile | 30,97376199842 ± 0,0000000007 | 100,0000% | Stabile | stable |
Righe spettrali
Sono visualizzati 50 di 122. Per impostazione predefinita sono mostrate soltanto le righe spettrali con intensità misurata.
| Lunghezza d'onda (nm) | Intensità | Stadio di ionizzazione | Tipo | Transizione | Accuratezza | Fonte | |
|---|---|---|---|---|---|---|---|
| 460.2069 nm | 600 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | Misurata | NIST | |
| 422.2198 nm | 500 | P III | emission | 3s2.4s 2S → 3s2.4p 2P* | Misurata | NIST | |
| 458.8032 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | Misurata | NIST | |
| 458.9846 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | Misurata | NIST | |
| 494.3497 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | Misurata | NIST | |
| 602.418 nm | 500 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | Misurata | NIST | |
| 604.308 nm | 500 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | Misurata | NIST | |
| 405.9312 nm | 400 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | Misurata | NIST | |
| 442.0712 nm | 400 | P II | emission | 3s2.3p.4s 1P* → 3s2.3p.4p 1S | Misurata | NIST | |
| 529.6077 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3S | Misurata | NIST | |
| 542.588 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 545.0709 nm | 400 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 603.404 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | Misurata | NIST | |
| 424.672 nm | 350 | P III | emission | 3s2.4s 2S → 3s2.4p 2P* | Misurata | NIST | |
| 608.784 nm | 350 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | Misurata | NIST | |
| 616.56 nm | 350 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | Misurata | NIST | |
| 395.7641 nm | 300 | P III | emission | 3s.3p.(3P*).4s 4P* → 3s.3p.(3P*).4p 4P | Misurata | NIST | |
| 408.0089 nm | 300 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | Misurata | NIST | |
| 424.9655 nm | 300 | P IV | emission | 3s.4s 1S → 3s.4p 1P* | Misurata | NIST | |
| 462.6708 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | Misurata | NIST | |
| 465.8309 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | Misurata | NIST | |
| 495.4367 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | Misurata | NIST | |
| 496.9701 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | Misurata | NIST | |
| 525.3479 nm | 300 | P II | emission | 3s2.3p.4s 1P* → 3s2.3p.4p 1D | Misurata | NIST | |
| 534.4729 nm | 300 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 538.6895 nm | 300 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 531.6055 nm | 250 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 537.8192 nm | 250 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 558.8301 nm | 250 | P II | emission | 3s2.3p.4p 3S → 3s2.3p.5s 3P* | Misurata | NIST | |
| 605.55 nm | 250 | P II | emission | 3s2.3p.4p 1D → 3s2.3p.5s 1P* | Misurata | NIST | |
| 390.4811 nm | 200 | P III | emission | 3s.3p.(3P*).4s 4P* → 3s.3p.(3P*).4p 4P | Misurata | NIST | |
| 405.7449 nm | 200 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | Misurata | NIST | |
| 438.5393 nm | 200 | P II | emission | 3s2.3p.4p 1P → 3s2.3p.5s 1P* | Misurata | NIST | |
| 447.527 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.4d 3D* | Misurata | NIST | |
| 449.923 nm | 200 | P II | emission | 3s2.3p.4p 1D → 3s2.3p.4d 1F* | Misurata | NIST | |
| 486.4426 nm | 200 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | Misurata | NIST | |
| 540.9722 nm | 200 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 548.3519 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 549.9697 nm | 200 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | Misurata | NIST | |
| 550.7174 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 554.1139 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 558.3235 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | Misurata | NIST | |
| 534.5854 nm | 180 | P I | emission | 3s2.3p2.(3P).4s 2P → 3s2.3p2.(3P).5p 2P* | Misurata | NIST | |
| 547.7672 nm | 180 | P I | emission | 3s2.3p2.(3P).4s 2P → 3s2.3p2.(3P).5p 2D* | Misurata | NIST | |
| 716.547 nm | 180 | P I | emission | 3s2.3p2.(3P).4p 4D* → 3s2.3p2.(3P).5d 4F | Misurata | NIST | |
| 717.666 nm | 180 | P I | emission | 3s2.3p2.(3P).4p 4D* → 3s2.3p2.(3P).5d 4F | Misurata | NIST | |
| 492.7197 nm | 150 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | Misurata | NIST | |
| 519.1393 nm | 150 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3S | Misurata | NIST | |
| 510.9625 nm | 140 | P I | emission | 3s2.3p2.(3P).4s 4P → 3s2.3p2.(3P).5p 4P* | Misurata | NIST | |
| 515.4842 nm | 140 | P I | emission | 3s2.3p2.(3P).4s 4P → 3s2.3p2.(3P).5p 4D* | Misurata | NIST |
Proprietà estese
Raggi covalenti (dati estesi)
- Raggio covalente (Pyykkö)
- 111 pm
- Raggio covalente (Pyykkö, legame doppio)
- 102 pm
- Raggio covalente (Pyykkö, legame triplo)
- 94 pm
Raggi di van der Waals
- Bondi
- 180 pm
- Batsanov
- 195 pm
- Alvarez
- 190 pm
- UFF
- 414,7 pm
- MM3
- 222 pm
- Dreiding
- 415 pm
Raggi atomici e metallici
- Raggio atomico (Rahm)
- 223 pm
- Raggio metallico (C12)
- 128 pm
Scale di numerazione
- Mendeleev
- 94
- Pettifor
- 90
- Glawe
- 89
Scale di elettronegatività
- Ghosh
- 0
- Miedema
- 6
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
Polarizzabilità e dispersione
- Polarizzabilità dipolare
- 25 a.u.
- Polarizzabilità dipolare (inc.)
- 1 a.u.
- C₆
- 185 Ha·Bohr6
- C₆ (Gould–Bučko)
- 187 Ha·Bohr6
Affinità chimica
- Affinità protonica
- 626,8 kJ/mol
- Basicità in fase gassosa
- 604,8 kJ/mol
Parametri di Miedema
- Volume molare di Miedema
- 8,6 cm3/mol
- Densità elettronica di Miedema
- 4
Rischio di approvvigionamento ed economia
- Concentrazione della produzione
- 39
- Rischio relativo di approvvigionamento
- 5
- Distribuzione delle riserve
- 45
- Stabilità politica (principale produttore)
- 24
- Stabilità politica (principale detentore di riserve)
- 29
Transizioni di fase e allotropi
| Punto di fusione | 317,3 K |
| Punto di ebollizione | 553,65 K |
| Punto critico (temperatura) | 994,15 K |
| Punto di fusione | 852,35 K |
| Punto di ebollizione | 704,15 K |
| Punto critico (temperatura) | 994,15 K |
Categorie degli stati di ossidazione
Dati di riferimento avanzati
Costanti di schermaggio (5)
| n | Orbitale | σ |
|---|---|---|
| 1 | s | 0,4422 |
| 2 | p | 4,0388 |
| 2 | s | 5,175 |
| 3 | p | 10,1136 |
| 3 | s | 9,3582 |
Dettaglio dei raggi cristallini (4)
| Carica | CN | Spin | rcrystal (pm) | Origine |
|---|---|---|---|---|
| 3 | VI | 58 | Ahrens (1952) ionic radius, | |
| 5 | IV | 31 | ||
| 5 | V | 43 | ||
| 5 | VI | 52 | calculated, |
Modalità di decadimento degli isotopi (50)
| Isotopo | Modalità | Intensità |
|---|---|---|
| 24 | p | — |
| 24 | B+ | — |
| 24 | B+p | — |
| 25 | p | — |
| 26 | B+ | 100% |
| 26 | B+p | 35,1% |
| 26 | 2p | 2% |
| 27 | B+ | 100% |
| 27 | B+p | 0,1% |
| 28 | B+ | 100% |
Fattori di diffusione dei raggi X (504)
| Energia (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 8,47738 |
| 10,1617 | — | 8,27092 |
| 10,3261 | — | 8,06949 |
| 10,4931 | — | 7,87297 |
| 10,6628 | — | 7,68123 |
| 10,8353 | — | 7,49416 |
| 11,0106 | — | 7,31165 |
| 11,1886 | — | 7,13359 |
| 11,3696 | — | 6,95985 |
| 11,5535 | — | 6,79035 |
Dati aggiuntivi
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.05×103 milligrams per kilogram
Riferimenti (1)
- [5] Phosphorus https://education.jlab.org/itselemental/ele015.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
6×10-2 milligrams per liter
Riferimenti (1)
- [5] Phosphorus https://education.jlab.org/itselemental/ele015.html
Sources
Sources of this element.
Never found free in nature, it is widely distributed in combination with minerals. Phosphate rock, which contains the mineral apatite, an impure tri-calcium phosphate, is an important source of the element. Large deposits are found in Russia, in Morocco, and in Florida, Tennessee, Utah, Idaho, and elsewhere.
Riferimenti (1)
- [6] Phosphorus https://periodic.lanl.gov/15.shtml
Production
Production of this element (from raw materials or other compounds containing the element).
White phosphorus may be made by several methods. By one process, tri-calcium 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 phosphoric acid, an important compound in making super-phosphate fertilizers.
Riferimenti (1)
- [6] Phosphorus https://periodic.lanl.gov/15.shtml
Riferimenti
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Phosphorus.
The element property data was retrieved from publications.