Arsenic (As)
metalloidSolid
标准原子量
74.921595 u电子排布
[Ar] 4s2 3d10 4p3熔点
816.85 °C沸点
613.85 °C密度
5776 kg/m³氧化态
−3, −2, −1, 0, +1, +2, +3, +4, +5电负性（鲍林）
2.18第一电离能
9.78855 eV发现年份
1250原子半径
115 pm详细信息
Arsenic is a metalloid in group 15, chemically related to phosphorus and antimony. It occurs mainly in sulfide minerals and in arsenide or sulfosalt ores, rather than as the native element. Its chemistry is dominated by the +3 and +5 oxidation states, with important differences in mobility and toxicity among species. Arsenic is technologically useful in small quantities, especially in compound semiconductors, but it is better known for the toxicity of many of its inorganic compounds.
The element is a steel gray, very brittle, crystalline, semimetallic solid; it tarnishes in air, and when it is heated it rapidly oxidizes to arsenous oxide, which smells of garlic. Arsenic and its compounds are poisonous.
The name derives from the Latin arsenicium and the Greek arsenikos for "masculine" or "male" because the ancients thought that metals were different sexes. Arsenic was known in prehistoric times for its poisonous sulfides. The German scientist and philosopher, Albert von Bollstadt (Albert the Great or Albertus Magnus) is thought to have obtained the metal around 1250.
Although arsenic compounds were mined by the early Chinese, Greek and Egyptian civilizations, it is believed that arsenic itself was first identified by Albertus Magnus, a German alchemist, in 1250. Arsenic occurs free in nature, but is most often found in the minerals arsenopyrite (FeAsS), realgar (AsS) and orpiment (As2S3). Today, most commercial arsenic is obtained by heating arsenopyrite.
From the Latin word arsenicum, Greek arsenikon. Elemental arsenic occurs in two solid modifications: yellow, and gray or metallic, with specific gravities of 1.97, and 5.73, respectively. It is believed that Albertus Magnus obtained the element in 1250 A.D. In 1649 Schroeder published two methods of preparing the element. Mispickel arsenopyrite, (FeSAs), is the most common mineral from which, on heating, the arsenic sublimes leaving ferrous sulfide.
Pure arsenic is most commonly encountered as gray arsenic, a brittle, metallic-looking solid with a steel-gray surface. It sublimes readily on heating rather than melting at ordinary pressure. Yellow and black allotropes are known but are less stable under ordinary conditions.
Elemental arsenic has limited direct use. Small additions have been used to harden lead alloys, especially for shot, grids, and some bearing materials. The most important modern use is in high-purity compound semiconductors, notably gallium arsenide (GaAs), which is used in radio-frequency electronics, optoelectronics, infrared devices, and some high-efficiency solar cells. Arsenic compounds were formerly used widely in pesticides, herbicides, wood preservatives, pigments, and medicines, but many such uses have been restricted or abandoned because of toxicity and persistence.
Arsenic and its compounds are poisonous. They have been used to make rat poison and some insecticides. Small amounts of arsenic are added to germanium to make transistors. Gallium arsenide (GaAs) can produce laser light directly from electricity.
If you were paying careful attention to the physical data listed above, you may have noticed that arsenic's boiling point is lower than its melting point. This occurs because these two temperatures are measured at different atmospheric pressures. When heated at standard atmospheric pressure, arsenic changes directly from a solid to a gas, or sublimates, at a temperature of 887 K. In order to form liquid arsenic, the atmospheric pressure must be increased. At 28 times standard atmospheric pressure, arsenic melts at a temperature of 1090 K. If it were also measured at a pressure of 28 atmospheres, arsenic's boiling point would be higher than its melting point, as you would expect.
Arsenic is used in bronzing, pyrotechny, and for hardening and improving the sphericity of shot. The most important compounds are white arsenic, the sulfide, Paris green, calcium arsenate, and lead arsenate; the last three have been used as agricultural insecticides and poisons. Marsh's test makes use of the formation and ready decomposition of arsine. Arsenic is finding increasing uses as a doping agent in solid-state devices such as transistors. Gallium arsenide is used as a laser material to convert electricity directly into coherent light.
Isotopes in Biology
73As and 76As (with half-lives of 80.3 days and 1.1 days, respectively) are important radioactive tracers used in environmental and biomedical studies to quantify arsenic uptake [270] J. De Kimpe, R. Cornelis, L. Mees, R. Vanholder. Fundam. Appl. Toxicol.34, 240 (1996).. 74As (with a half-life of 17.8 days) has been used to investigate the biotransformation (modification of a chemical compound by an organism) of arsenate by mammals. In one study rabbits were injected with 74As-labeled arsenate. After a given amount of time, blood and blood products were sampled and tested for the presence and quantity of labeled arsenate metabolites [270] J. De Kimpe, R. Cornelis, L. Mees, R. Vanholder. Fundam. Appl. Toxicol.34, 240 (1996).. Inhalation of dust or smoke containing 74As is thought to be a causal agent of lung cancer. In one study [271] R. H. Holland, M. S. McCall, H. C. Lanz. Cancer Res.19, 1154 (1959)., the “absorption rate from the bronchial tree (a respiratory tract, which conducts air into the lungs) was rapid for the first several days and then tapered off slowly. In three patients an average of 45 percent of the inhaled arsenic was eliminated in the urine in 10 days and about 0.5 percent in the stools. The remainder must be assumed to have been deposited in the body, exhaled, and/or eliminated in body secretions and excreta over a long period of time.” See Fig. IUPAC.33.1.
Isotopes in Medicine
72As (with a half-life of 26 h) and 74As are useful in molecular imaging because they are radioactive isotopes that emit positrons that can be designed to bind to monoclonal antibodies (moAb), which accumulate in tumors and then 72As- or 74As-labeled ligands will bind to the moAbs. Once the 72As- or 74As-labeled ligand binds to the moAb, positron emission tomography (PET) is used to visualize the exact location of the tumor [272] M. Jennewein, A. Hermanne, R. P. Mason, P. E. Thorpe, F. Rösch. Nucl. Instrum. Methods Phys. Res. A569, 512 (2006).. A specific example of using radiolabeled antibodies for better imaging of tumors is the combination of 74As with bavituximab, which is an antibody that binds strongly to unique lipids on the surface of tumors. When a thiol group is introduced to bavituximab, arsenic is able to bind covalently, creating a simple and elegant radio-label for targeting cancerous tumors [269] M. Jennewein, M. A. Lewis, D. Zhao, E. Tsyganov, N. Slavine, J. He, L. Watkins, V. D. Kodibagkar, S. O’Kelly, P. Kulkarni, P. P. Antich, A. Hermanne, F. Rösch, R. P. Mason, P. E. Thorpe. Clin. Cancer Res.14, 1377 (2008)..
Arsenic forms covalent and ionic compounds in several oxidation states, chiefly −3, +3, and +5. Arsenic trioxide (As₂O₃) is a major industrial intermediate and dissolves to give arsenite species. Arsenic pentoxide (As₂O₅) and arsenic acid (H₃AsO₄) contain arsenic in the +5 state and are related to arsenate salts. Arsine (AsH₃) is a highly toxic, volatile hydride. Important minerals include arsenopyrite (FeAsS), realgar (As₄S₄), and orpiment (As₂S₃). Organoarsenic compounds also exist, including methylated species found in biological and environmental systems.
See more information at the Arsenic compound page.
Arsenic metal is hazardous mainly through dust, fumes, and conversion to soluble or volatile compounds. Many inorganic arsenic(III) compounds are acutely toxic, and chronic exposure to inorganic arsenic in drinking water or industrial settings is associated with serious disease, including cancers. Arsine (AsH₃) is especially dangerous because it is a potent hemolytic gas. Toxicity depends strongly on chemical form, dose, route of exposure, and solubility; organic arsenic species in seafood are often much less toxic than inorganic arsenic.
Arsenic enters the environment through natural weathering of minerals, volcanic emissions, geothermal waters, and human activities such as mining, smelting, coal combustion, and historical pesticide use. In groundwater, its mobility is controlled by pH, redox conditions, adsorption to iron and manganese oxides, and microbial transformations. Arsenate species generally predominate under oxidizing conditions, while arsenite species are more important under reducing conditions and are often more mobile and toxic.
Arsenic is not usually mined as a primary commodity. It is recovered mainly as arsenic trioxide (As₂O₃) from flue dusts and residues generated during the smelting and refining of copper, lead, gold, and other nonferrous ores. Demand is much smaller than in the past because agricultural chemicals and chromated copper arsenate wood preservatives have been reduced or phased out in many regions. High-purity arsenic for gallium arsenide (GaAs) is a specialized market requiring stringent purification. Supply depends heavily on by-product recovery, environmental controls at smelters, and the ability to handle or stabilize arsenic-bearing wastes.
Found in mispickel (arsenopyrite)
Arsenic is a relatively uncommon element in the cosmos. Its stable isotope, ⁷⁵As, is produced by neutron-capture processes in evolved stars and supernova-related environments. In planetary materials, arsenic behaves as a moderately chalcophile and siderophile trace element, so it is commonly associated with sulfides and metallic phases rather than silicate minerals alone. Meteorites contain small amounts of arsenic in mineral and metal fractions.
- Natural arsenic consists essentially of one stable isotope, ⁷⁵As.
- Gray arsenic sublimes at ordinary pressure, which complicates simple melting-point measurements.
- Garlic-like odor during heating often comes from volatile arsenic compounds, not a safe warning sign.
- Arsenopyrite (FeAsS) is one of the most important arsenic-bearing ore minerals.
- Gallium arsenide (GaAs) has higher electron mobility than silicon, but it is costlier and more brittle.
- Some microorganisms can transform arsenic between arsenite, arsenate, and methylated forms.
图片
性质
物理性质
- 原子半径（经验值）
- 115 pm 比较所有元素的原子半径（经验值） →
- 共价半径
- 119 pm 比较所有元素的共价半径 →
- 范德华半径
- 185 pm 比较所有元素的范德华半径 →
- 金属半径
- 121 pm 比较所有元素的金属半径 →
- 密度
- 5776 kg/m³ 比较所有元素的密度 →
- 摩尔体积
- 0.0131 L/mol
- 标准温度和压力下的物相
- 固态 比较所有元素的标准温度和压力下的物相 →
- 熔点
- 816.85 °C 比较所有元素的熔点 →
- 沸点
- 613.85 °C 比较所有元素的沸点 →
- 比热容
- 0.329 J/(g·K) 比较所有元素的比热容 →
- 摩尔热容
- 24.64 J/(mol·K) 比较所有元素的摩尔热容 →
- 晶体结构
- 菱方 比较所有元素的晶体结构 →
化学性质
- 电负性（鲍林）
- 2.18 比较所有元素的电负性（鲍林） →
- 电负性（Allen）
- 2.211
- 电子亲和能
- 0.81 eV
- 第一电离能
- 9.78855 eV 比较所有元素的第一电离能 →
- 第二电离能
- 18.589264 eV 比较所有元素的第二电离能 →
- 第三电离能
- 28.349098 eV 比较所有元素的第三电离能 →
- 第四电离能
- 50.150173 eV 比较所有元素的第四电离能 →
- 第五电离能
- 62.770216 eV 比较所有元素的第五电离能 →
- 氧化态
- −3, −2, −1, 0, +1, +2, +3, +4, +5 比较所有元素的氧化态 →
- 价电子
- 5 比较所有元素的价电子 →
- 同素异形体
- ["gray"]
- 电子排布
- [Ar] 4s2 3d10 4p3
热力学性质
- 三相点（温度）
- 817 °C
- 三相点（压力）
- 3.7e+6 Pa
- 临界点（温度）
- 1400 °C
- 临界点（压力）
- 2.23e+7 Pa
- 汽化热
- 0.36275069 eV 比较所有元素的汽化热 →
- 升华热
- 3.138312 eV
- 原子化热
- 3.138312 eV
- 原子化焓
- 3.135202 eV
核性质
- 质子
- 33 比较所有元素的质子 →
- 中子
- 42 比较所有元素的中子 →
- 已知同位素
- 33 比较所有元素的已知同位素 →
- 稳定同位素
- 1 比较所有元素的稳定同位素 →
- 最稳定同位素
- As-75
- 发现年份
- 1250
丰度
- 丰度（地壳）
- 1.8 mg/kg 比较所有元素的丰度（地壳） →
- 丰度（海洋）
- 3.7 mg/L 比较所有元素的丰度（海洋） →
晶体结构
- 晶格常数a
- 413 pm
电子结构
- 各电子层电子数
- 2, 8, 18, 5 比较所有元素的各电子层电子数 →
标识符
- CAS登记号
- 7440-38-2 比较所有元素的CAS登记号 →
- 谱项符号
- 4S°3/2
- InChI
- InChI=1S/As
- InChI Key
- RQNWIZPPADIBDY-UHFFFAOYSA-N
电子排布 实测值
As: 3d¹⁰ 4s² 4p³[Ar] 3d¹⁰ 4s² 4p³1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p³原子模型
不同同位素的中子数、质量和稳定性不同，但中性原子的电子排布不变。
原子模型示意图，未按比例绘制。
原子指纹
发射 / 吸收光谱
同位素分布
| 质量数 | 原子质量（u） | 天然丰度 | 半衰期 |
|---|---|---|---|
| 75 稳定 | 74.92159457 ± 0.00000095 | 100.0000% | 稳定 |
物相 / 状态
原因: 低于升华点（613.85 °C）588.9 °C
示意图，未按比例绘制
相变点
相变能
在沸点汽化1 mol物质所需的能量
在升华点升华1 mol物质所需的能量
密度
标准条件下
标准条件下
高级
原子光谱
已显示10项，共33项。 按离子电荷升序排列。
收录能级 ?
| 离子 | 电荷 | 能级 |
|---|---|---|
| As I | 0 | 116 |
| As II | +1 | 167 |
| As III | +2 | 22 |
| As IV | +3 | 34 |
| As V | +4 | 9 |
| As VI | +5 | 44 |
| As VII | +6 | 50 |
| As VIII | +7 | 2 |
| As IX | +8 | 2 |
| As X | +9 | 2 |
离子半径
| 电荷 | 配位 | 自旋 | 半径 |
|---|---|---|---|
| +3 | 6 | 暂无 | 57.99999999999999 pm |
| +5 | 4 | 暂无 | 33.5 pm |
| +5 | 6 | 暂无 | 46 pm |
化合物
同位素 (1)
| 质量数 | 原子质量（u） | 天然丰度 | 半衰期 | 衰变方式 | |
|---|---|---|---|---|---|
| 75 稳定 | 74.92159457 ± 0.00000095 | 100.0000% | 稳定 | stable |
扩展性质
共价半径（扩展）
- 共价半径（Pyykkö）
- 121 pm
- 共价半径（Pyykkö，双键）
- 114 pm
- 共价半径（Pyykkö，三键）
- 106 pm
- 共价半径（Bragg）
- 126 pm
范德华半径
- Bondi
- 185 pm
- Batsanov
- 205 pm
- Alvarez
- 188 pm
- UFF
- 423 pm
- MM3
- 236 pm
- Dreiding
- 415 pm
原子半径与金属半径
- 原子半径（Rahm）
- 231 pm
- 金属半径（C12）
- 148 pm
编号标度
- Mendeleev
- 95
- Pettifor
- 89
- Glawe
- 90
电负性标度
- Ghosh
- 0
- Miedema
- 5
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
极化率与色散
- 偶极极化率
- 30 a.u.
- 偶极极化率（不确定度）
- 1 a.u.
- C₆
- 246 Ha·Bohr6
- C₆ (Gould–Bučko)
- 260 Ha·Bohr6
Miedema参数
- Miedema摩尔体积
- 11.85 cm3/mol
- Miedema电子密度
- 3
供应风险与经济性
- 生产集中度
- 64
- 相对供应风险
- 8
- 政治稳定性（最大生产国）
- 24
相变与同素异形体
| 熔点 | 1090.15 K |
| 沸点 | 889.15 K |
| 临界点（温度） | 1673.15 K |
| 临界点（压力） | 22.3 MPa |
| 三相点（温度） | 1090.15 K |
| 三相点（压力） | 3700 kPa |
氧化态分类
高级参考数据
屏蔽常数 (8)
| n | 轨道 | σ |
|---|---|---|
| 1 | s | 0.7217 |
| 2 | p | 3.9264 |
| 2 | s | 8.873 |
| 3 | d | 15.6216 |
| 3 | p | 15.1503 |
| 3 | s | 14.4045 |
| 4 | p | 25.5508 |
| 4 | s | 24.056 |
晶体半径详情 (3)
| 电荷 | CN | 自旋 | rcrystal (pm) | 来源 |
|---|---|---|---|---|
| 3 | VI | 72 | Ahrens (1952) ionic radius, | |
| 5 | IV | 47.5 | from r^3 vs V plots, | |
| 5 | VI | 60 | calculated, |
同位素衰变方式 (50)
| 同位素 | 模式 | 强度 |
|---|---|---|
| 60 | p | — |
| 61 | p | — |
| 62 | p | — |
| 63 | p | — |
| 64 | B+ | 100% |
| 64 | B+p | — |
| 65 | B+ | 100% |
| 65 | B+p | — |
| 66 | B+ | 100% |
| 67 | B+ | 100% |
X射线散射因子 (506)
| 能量 (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 4.62596 |
| 10.1617 | — | 4.67742 |
| 10.3261 | — | 4.72945 |
| 10.4931 | — | 4.78206 |
| 10.6628 | — | 4.83525 |
| 10.8353 | — | 4.88904 |
| 11.0106 | — | 4.94342 |
| 11.1886 | — | 4.99841 |
| 11.3696 | — | 5.05401 |
| 11.5535 | — | 5.11023 |
补充数据
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
1.8 milligrams per kilogram
参考文献 (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
3.7-3 milligrams per liter
参考文献 (1)
参考文献
(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 Arsenic.
The element property data was retrieved from publications.