Phosphorus (P)
nonmetalSolid
표준 원자량
30.973762 u전자 배치
[Ne] 3s2 3p3녹는점
44.15 °C끓는점
280.5 °C밀도
1820 kg/m³산화 상태
−3, −2, −1, 0, +1, +2, +3, +4, +5전기 음성도(Pauling)
2.19제1 이온화 에너지
10.486686 eV발견 연도
1669원자 반지름
100 pm상세 정보
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.
이미지
특성
물리적 특성
- 원자 반지름(경험값)
- 100 pm 모든 원소의 원자 반지름(경험값) 비교 →
- 공유 결합 반지름
- 107 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 180 pm 모든 원소의 반데르발스 반지름 비교 →
- 금속 반지름
- 110 pm 모든 원소의 금속 반지름 비교 →
- 밀도
- 1820 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.017 L/mol
- STP에서의 상
- 고체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- 44.15 °C 모든 원소의 녹는점 비교 →
- 끓는점
- 280.5 °C 모든 원소의 끓는점 비교 →
- 비열
- 0.769 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 23.824 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 입방 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 2.19 모든 원소의 전기 음성도(Pauling) 비교 →
- 전기 음성도(Allen)
- 2.253
- 전자 친화도
- 0.7466 eV
- 제1 이온화 에너지
- 10.486686 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 19.769558 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 30.202744 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 51.444047 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 65.025334 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- −3, −2, −1, 0, +1, +2, +3, +4, +5 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 5 모든 원소의 원자가 전자 비교 →
- 동소체
- ["red", "white"]
- 전자 배치
- [Ne] 3s2 3p3
열역학적 특성
- 임계점(온도)
- 721 °C
- 융해열
- 0.00684044 eV 모든 원소의 융해열 비교 →
- 기화열
- 0.12851739 eV 모든 원소의 기화열 비교 →
- 승화열
- 3.271597 eV
- 원자화열
- 3.271597 eV
- 원자화 엔탈피
- 3.280303 eV
핵 특성
- 양성자 수
- 15 모든 원소의 양성자 수 비교 →
- 중성자 수
- 16 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 24 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 1 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- P-31
- 발견 연도
- 1669
존재비
- 존재비(지각)
- 1050 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 0.06 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 717 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 5 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7723-14-0 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 4S°3/2
- InChI
- InChI=1S/P
- InChI 키
- OAICVXFJPJFONN-UHFFFAOYSA-N
전자 배치 측정값
P: 3s² 3p³[Ne] 3s² 3p³1s² 2s² 2p⁶ 3s² 3p³원자 모형
동위원소에 따라 중성자 수, 질량, 안정성은 달라지지만, 중성 원자의 전자 배치는 달라지지 않습니다.
개략적인 원자 모형이며 실제 비율과 다릅니다.
원자 지문
방출 / 흡수 스펙트럼
동위원소 분포
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 |
|---|---|---|---|
| 31 안정 | 30.97376199842 ± 0.0000000007 | 100.0000% | 안정 |
상 / 상태
이유: 녹는점(44.15 °C)보다 19.2 °C 낮음
개략도이며 실제 비율과 다름
상전이점
전이 에너지
녹는점에서 1 mol을 녹이는 데 필요한 에너지
끓는점에서 1 mol을 기화시키는 데 필요한 에너지
승화점에서 1 mol을 승화시키는 데 필요한 에너지
밀도
표준 조건에서
표준 조건에서
심화
원자 스펙트럼
전체 15개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 스펙트럼선 데이터 ?
| 이온 | 전하 | 총 스펙트럼선 수 | 전이 확률 | 준위 표기 |
|---|---|---|---|---|
| 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 |
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| 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 |
이온 반지름
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +3 | 6 | 해당 없음 | 44 pm |
| +5 | 4 | 해당 없음 | 17 pm |
| +5 | 5 | 해당 없음 | 28.999999999999996 pm |
| +5 | 6 | 해당 없음 | 38 pm |
화합물
동위원소 (1)
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 31 안정 | 30.97376199842 ± 0.0000000007 | 100.0000% | 안정 | stable |
스펙트럼선
전체 122개 중 50개를 표시합니다. 기본적으로 세기가 측정된 스펙트럼선만 표시됩니다.
| 파장(nm) | 세기 | 이온화 단계 | 유형 | 전이 | 정확도 | 출처 | |
|---|---|---|---|---|---|---|---|
| 460.2069 nm | 600 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | 측정값 | NIST | |
| 422.2198 nm | 500 | P III | emission | 3s2.4s 2S → 3s2.4p 2P* | 측정값 | NIST | |
| 458.8032 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | 측정값 | NIST | |
| 458.9846 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | 측정값 | NIST | |
| 494.3497 nm | 500 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 602.418 nm | 500 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | 측정값 | NIST | |
| 604.308 nm | 500 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | 측정값 | NIST | |
| 405.9312 nm | 400 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | 측정값 | NIST | |
| 442.0712 nm | 400 | P II | emission | 3s2.3p.4s 1P* → 3s2.3p.4p 1S | 측정값 | NIST | |
| 529.6077 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3S | 측정값 | NIST | |
| 542.588 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 545.0709 nm | 400 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 603.404 nm | 400 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | 측정값 | NIST | |
| 424.672 nm | 350 | P III | emission | 3s2.4s 2S → 3s2.4p 2P* | 측정값 | NIST | |
| 608.784 nm | 350 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | 측정값 | NIST | |
| 616.56 nm | 350 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3D | 측정값 | NIST | |
| 395.7641 nm | 300 | P III | emission | 3s.3p.(3P*).4s 4P* → 3s.3p.(3P*).4p 4P | 측정값 | NIST | |
| 408.0089 nm | 300 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | 측정값 | NIST | |
| 424.9655 nm | 300 | P IV | emission | 3s.4s 1S → 3s.4p 1P* | 측정값 | NIST | |
| 462.6708 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | 측정값 | NIST | |
| 465.8309 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.4d 3F* | 측정값 | NIST | |
| 495.4367 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 496.9701 nm | 300 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 525.3479 nm | 300 | P II | emission | 3s2.3p.4s 1P* → 3s2.3p.4p 1D | 측정값 | NIST | |
| 534.4729 nm | 300 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 538.6895 nm | 300 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 531.6055 nm | 250 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 537.8192 nm | 250 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 558.8301 nm | 250 | P II | emission | 3s2.3p.4p 3S → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 605.55 nm | 250 | P II | emission | 3s2.3p.4p 1D → 3s2.3p.5s 1P* | 측정값 | NIST | |
| 390.4811 nm | 200 | P III | emission | 3s.3p.(3P*).4s 4P* → 3s.3p.(3P*).4p 4P | 측정값 | NIST | |
| 405.7449 nm | 200 | P III | emission | 3s2.3d 2D → 3s2.4p 2P* | 측정값 | NIST | |
| 438.5393 nm | 200 | P II | emission | 3s2.3p.4p 1P → 3s2.3p.5s 1P* | 측정값 | NIST | |
| 447.527 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.4d 3D* | 측정값 | NIST | |
| 449.923 nm | 200 | P II | emission | 3s2.3p.4p 1D → 3s2.3p.4d 1F* | 측정값 | NIST | |
| 486.4426 nm | 200 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 540.9722 nm | 200 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 548.3519 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 549.9697 nm | 200 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3P | 측정값 | NIST | |
| 550.7174 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 554.1139 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 558.3235 nm | 200 | P II | emission | 3s2.3p.4p 3P → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 534.5854 nm | 180 | P I | emission | 3s2.3p2.(3P).4s 2P → 3s2.3p2.(3P).5p 2P* | 측정값 | NIST | |
| 547.7672 nm | 180 | P I | emission | 3s2.3p2.(3P).4s 2P → 3s2.3p2.(3P).5p 2D* | 측정값 | NIST | |
| 716.547 nm | 180 | P I | emission | 3s2.3p2.(3P).4p 4D* → 3s2.3p2.(3P).5d 4F | 측정값 | NIST | |
| 717.666 nm | 180 | P I | emission | 3s2.3p2.(3P).4p 4D* → 3s2.3p2.(3P).5d 4F | 측정값 | NIST | |
| 492.7197 nm | 150 | P II | emission | 3s2.3p.4p 3D → 3s2.3p.5s 3P* | 측정값 | NIST | |
| 519.1393 nm | 150 | P II | emission | 3s2.3p.4s 3P* → 3s2.3p.4p 3S | 측정값 | NIST | |
| 510.9625 nm | 140 | P I | emission | 3s2.3p2.(3P).4s 4P → 3s2.3p2.(3P).5p 4P* | 측정값 | NIST | |
| 515.4842 nm | 140 | P I | emission | 3s2.3p2.(3P).4s 4P → 3s2.3p2.(3P).5p 4D* | 측정값 | NIST |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 111 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 102 pm
- 공유 결합 반지름(Pyykkö, 삼중 결합)
- 94 pm
반데르발스 반지름
- Bondi
- 180 pm
- Batsanov
- 195 pm
- Alvarez
- 190 pm
- UFF
- 414.7 pm
- MM3
- 222 pm
- Dreiding
- 415 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 223 pm
- 금속 반지름(C12)
- 128 pm
번호 척도
- Mendeleev
- 94
- Pettifor
- 90
- Glawe
- 89
전기 음성도 척도
- Ghosh
- 0
- Miedema
- 6
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
분극률 및 분산
- 쌍극자 분극률
- 25 a.u.
- 쌍극자 분극률(불확도)
- 1 a.u.
- C₆
- 185 Ha·Bohr6
- C₆ (Gould–Bučko)
- 187 Ha·Bohr6
화학 친화력
- 양성자 친화도
- 626.8 kJ/mol
- 기체상 염기성
- 604.8 kJ/mol
미데마 매개변수
- 미데마 몰 부피
- 8.6 cm3/mol
- 미데마 전자 밀도
- 4
공급 위험 및 경제성
- 생산 집중도
- 39
- 상대적 공급 위험
- 5
- 매장량 분포
- 45
- 정치적 안정성(최대 생산국)
- 24
- 정치적 안정성(최대 매장국)
- 29
상전이 및 동소체
| 녹는점 | 317.3 K |
| 끓는점 | 553.65 K |
| 임계점(온도) | 994.15 K |
| 녹는점 | 852.35 K |
| 끓는점 | 704.15 K |
| 임계점(온도) | 994.15 K |
산화 상태 분류
심화 참고 데이터
차폐 상수 (5)
| n | 오비탈 | σ |
|---|---|---|
| 1 | s | 0.4422 |
| 2 | p | 4.0388 |
| 2 | s | 5.175 |
| 3 | p | 10.1136 |
| 3 | s | 9.3582 |
결정 반지름 상세 정보 (4)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 3 | VI | 58 | Ahrens (1952) ionic radius, | |
| 5 | IV | 31 | ||
| 5 | V | 43 | ||
| 5 | VI | 52 | calculated, |
동위원소 붕괴 방식 (50)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 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% |
X선 산란 인자 (504)
| 에너지 (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 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.05×103 milligrams per kilogram
참고 문헌 (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
참고 문헌 (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.
참고 문헌 (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.
참고 문헌 (1)
- [6] Phosphorus https://periodic.lanl.gov/15.shtml
참고 문헌
(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.