Radium (Ra)
alkaline-earth-metalSolid
标准原子量
[226]电子排布
[Rn] 7s2熔点
699.85 °C沸点
1139.85 °C密度
5000 kg/m³氧化态
+2电负性（鲍林）
0.9第一电离能
5.278424 eV发现年份
1898原子半径
215 pm详细信息
Radium is a heavy alkaline earth metal and the element below barium in group 2. All of its isotopes are radioactive; ²²⁶Ra, with a half-life of about 1600 years, is the best known and occurs in uranium ores as part of the ²³⁸U decay series. Its chemistry is dominated by the Ra²⁺ ion, which resembles Ba²⁺ but is less commonly handled because intense radioactivity limits direct study.
Radium is obtained commercially as bromide and chloride; it is doubtful if any appreciable stock of the isolated element now exists. The pure metal is brilliant white when freshly prepared, but blackens on exposure to air, probably due to formation of the nitride. It exhibits luminescence, as do its slats; it decomposes in water and is somewhat more volatile than barium. It is a member of the alkaline-earth group of metals. Radium imparts a carmine red color to a flame. Radium emits alpha, beta, and gamma rays and when mixed with beryllium produce neutrons. One gram of 226Ra undergoes 3.7 x 1010 disintegrations per second. The curie is defined as that amount of radioactivity which has the same disintegration rate as 1 g of 226Ra. Twenty five isotopes are now known; radium 226, the common isotope, has a half-life of 1600 years.
Radium was discovered by Marie Sklodowska Curie, a Polish chemist, and Pierre Curie, a French chemist, in 1898. Marie Curie obtained radium from pitchblende, a material that contains uranium, after noticing that unrefined pitchblende was more radioactive than the uranium that was separated from it. She reasoned that pitchblende must contain at least one other radioactive element. Curie needed to refine several tons of pitchblende in order to obtain tiny amounts of radium and polonium, another radioactive element discovered by Curie. One ton of uranium ore contains only about 0.14 grams of radium. Today, radium can be obtained as a byproduct of refining uranium and is usually sold as radium chloride (RaCl2) or radium bromide (RaBr2) and not as a pure material. Radium's most stable isotope, radium-226, has a half-life of about 1600 years. It decays into radon-222 through alpha decay or into lead-212 by ejecting a carbon-14 nucleus.
Radium was discovered in 1898 by Madame Curie in the pitchblende or uraninite of North Bohemia, where it occurs. There is about 1 g of radium in 7 tons of pitchblende. The element was isolated in 1911 by Mme. Curie and Debierne by the electrolysis of a solution of pure radium chloride employing a mercury cathode; on distillation in an atmosphere of hydrogen, this amalgam yielded the pure metal.
Freshly prepared radium metal has been reported as silvery white, but it rapidly darkens in air, probably through formation of nitride and oxide surface films. Macroscopic samples are extremely rare, and many physical details are less well established than for stable alkaline earth metals.
Radium once had major uses in self-luminous paints, radiation sources, and early cancer radiotherapy, chiefly because ²²⁶Ra and its decay products emit penetrating radiation. These applications have largely been abandoned or replaced by safer, more controllable radionuclides and non-radioactive phosphor systems. Today radium is used only in limited scientific, calibration, and historical-material contexts; some isotopes, especially ²²³Ra in specific radiopharmaceutical preparations, have specialized medical use as radioactive nuclides rather than as elemental metal.
The Curie, a unit used to describe the activity of a radioactive substance, is based on radium-226. It is equal to the number of atoms in a one gram sample of radium-226 that will decay in one second, or 37,000,000,000 decays per second.
Radium had been used to make self-luminous paints for watches, aircraft instrument dials and other instrumentation, but has largely been replaced by cobalt-60, a less dangerous radioactive source. A mixture of radium and beryllium will emit neutrons and is used as a neutron source. Radium is used to produce radon, a radioactive gas used to treat some types of cancer. A single gram of radium-226 will produce 0.000l milliliters of radon a day.
Radium is about one million times more active than uranium. The lab notebooks used by the Curies are too highly contaminated to be safely handled today.
One gram of radium produces about 0.0001 ml (stp) of emanation, or radon gas, per day. This is purged from the radium and sealed in minute tubes, which are used in the treatment of cancer and other diseases. Radium was used in the producing of self-luminous paints, neutron sources, and in medicine for the treatment of disease. Other radioisotopes, such as 60Co, are now being used in place of radium. Some of these sources are much more powerful, and others are safer to use. Radium loses about 1% of its activity in 25 years, being transformed into elements of lower atomic weight. Lead is a final product of disintegration. Stored radium and radium-containing products or minerals should be ventilated to prevent build-up of radon.
Isotopes in Earth/Planetary Science
The radioactive isotopes 223Ra (with a half-life of 275 h), 224Ra (with a half-life of 88 h), 226Ra (with a half-life of 1600 years), and 228Ra (with a half-life of 5.75 years) are used as tracers to determine water flow rates. They are ideal environmental tracers because they behave conservatively once released into a water mass (meaning only mixing and decay processes affect their distribution) [578] United States Geological Survey. Resources on Isotopes-Periodic Table-Radium, U.S. Geological Survey (2014), Feb. 25; http://wwwrcamnl.wr.usgs.gov/isoig/period/ra_iig.html.. The activity ratios A(224Ra)/A(223Ra), A(223Ra)/A(226Ra), A(224Ra)/A(228Ra), and A(228Ra)/A(226Ra) have been used in lake studies to monitor and detect water inflow and mixing, to determine sources of inflowing water, and to monitor introduced water masses as they move within a body of water (i.e. a lake) [578] United States Geological Survey. Resources on Isotopes-Periodic Table-Radium, U.S. Geological Survey (2014), Feb. 25; http://wwwrcamnl.wr.usgs.gov/isoig/period/ra_iig.html., [579] T. F. Kraemer. Limnol. Oceanogr.50, 158 (2005).. For example, submarine groundwater discharge is an important pathway that transports dissolved substances from aquifers below a seabed to the coastal ocean. Submarine groundwater discharge can be difficult to quantify because it is both spatially and temporally variable. As a result, its relative importance in coastal ocean chemical budgets is commonly poorly known. Peterson et al. [572] R. N. Peterson, W. C. Burnett, M. Taniguchi, J. Chen, I. R. Santos, T. Ishitobi. J. Geophys. Res.113, C09021 (2008). used an hourly time series of measurements of multiple radium isotopes 223Ra, 224Ra, and 226Ra to quantify submarine groundwater discharge. They also used 222Rn (with a half-life of 3.8 days) measurements to independently quantify submarine groundwater discharge.
Isotopes in Geochronology
226Ra and 228Ra can be used for dating materials up to a few thousand years in age because the half-lives of 226Ra and 228Ra are 1600 years and 5.75 years, respectively, even though the long-lived 226Ra is found in nature as a result of its continuous production by the decay of 238U. For example, long-lived 226Ra has been used to date a limestone cave in central Switzerland, corals in the Indian Ocean, and Pleistocene gravel terraces [580] J. Eikenberg. “Radium isotope systematics in nature: applications in geochronology and hydrogeochemistry”, in Habilitation Thesis, Earth Science Department.. The activity ratio A(224Ra)/A(223Ra) is a potential age calculator for old lake water because the low 223Ra and 224Ra activities in old lake water are relatively unaffected by mixing [579] T. F. Kraemer. Limnol. Oceanogr.50, 158 (2005)..
Isotopes in Medicine
226Ra is used in brachytherapy (Fig. IUPAC.88.1), which is a method of localized treatment of various types of cancer. A sealed implant (such as a rod, seed, or needle) containing the radioactive isotope 226Ra is inserted into or near a patient’s tumor to apply a high dose of radiation to the tumor. The sealed implant is inserted by a physician or by an automated device (called a remote afterloader), and it is removed from the patient once the tumor is destroyed [75] J. Peterson, M. McDonell, L. Haroun, F. Monette, R. D. Hildebrand, A. Taboas. Radiological and Chemical Fact Sheets to Support Health Risk Analyses for Contaminated Areas, Prepared by Argonne National Laboratory Environmental Science Division in collaboration with U.S. Department of Energy, Richland Operations Office and Chicago Operations Office (2014), Feb. 22; http://www.remm.nlm.gov/ANL_ContaminantFactSheets_All_070418.pdf., [581] United States Nuclear Regulatory Commission (U.S. NRC). Frequently Asked Questions (FAQs) Regarding Radium-226 Overview, United States Nuclear Regulatory Commission (U.S. NRC) (2017), April 8; https://scp.nrc.gov/narmtoolbox/radium%20faq102008.pdf..
Radium chemistry is almost entirely divalent. Representative salts include radium chloride (RaCl₂), radium bromide (RaBr₂), radium sulfate (RaSO₄), and radium carbonate (RaCO₃). The sulfate is very sparingly soluble, resembling barium sulfate (BaSO₄), and this behavior is important in separations and environmental immobilization. Radium forms ionic compounds rather than strongly covalent species, and detailed structural data are limited by radioactivity and scarcity.
See more information at the Radium compound page.
Radium is highly radiotoxic. Ingested or inhaled Ra²⁺ can follow calcium pathways and deposit in bone, where alpha-emitting decay products deliver damaging local doses. ²²⁶Ra also produces radioactive radon (²²²Rn), creating an inhalation hazard in enclosed spaces. External gamma radiation, contamination spread, and long-lived residues make radium sources difficult to handle safely.
Inhalation, injection, or body exposure to radium can cause cancer and other body disorders. The maximum permissible border in the total body for 226Ra is 7400 becquerel.
Natural radium is produced continuously by decay of uranium and thorium isotopes in rocks and soils. It can enter groundwater, especially where reducing chemistry, salinity, or mineral dissolution mobilizes alkaline earth ions. Radium may co-precipitate with barite and other sulfate or carbonate minerals, limiting transport in some settings. Its environmental significance comes from radioactivity rather than chemical abundance.
Radium has no ordinary commodity market. It was historically isolated from uranium ores, notably pitchblende residues, by laborious chemical separations, but routine industrial demand disappeared as its hazards became clear and alternatives became available. Present supplies are small, controlled, and usually associated with legacy sources, regulatory management, or isotope-specific production and purification. Disposal, security, and contamination control are often more economically important than acquisition of new radium metal or salts.
Originally, radium was obtained from the rich pitchblende ore found in Joachimsthal, Bohemia. The carnotite sands of Colorado furnish some radium, but richer ores are found in the Republic of Zaire and the Great Lake region of Canada. Radium is present in all uranium minerals, and could be extracted, if desired, from the extensive wastes of uranium processing. Large uranium deposits are located in Ontario, New Mexico, Utah, Australia, and elsewhere.
Radium is not a primordial stable element. Its isotopes are generated in decay chains of heavier nuclides, mainly uranium and thorium, whose ultimate origins are rapid neutron-capture nucleosynthesis before incorporation into the Solar System. Because radium isotopes are short-lived on geological and cosmic timescales, any detectable natural radium indicates continuing production from longer-lived parents.
- Radium was named from the Latin word for ray because of its intense radioactivity.
- Pure radium compounds can self-warm from radioactive decay energy.
- Radium luminous paints used zinc sulfide phosphors, not glowing radium metal.
- The isotope ²²⁸Ra belongs to the ²³²Th decay series.
- Radium and barium are chemically similar enough to make separation difficult.
图片
性质
物理性质
- 原子半径（经验值）
- 215 pm 比较所有元素的原子半径（经验值） →
- 共价半径
- 221 pm 比较所有元素的共价半径 →
- 范德华半径
- 283 pm 比较所有元素的范德华半径 →
- 密度
- 5000 kg/m³ 比较所有元素的密度 →
- 摩尔体积
- 0.045 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
- 699.85 °C 比较所有元素的熔点 →
- 沸点
- 1139.85 °C 比较所有元素的沸点 →
化学性质
- 电负性（鲍林）
- 0.9 比较所有元素的电负性（鲍林） →
- 电负性（Allen）
- 0.89
- 电子亲和能
- 0.096 eV
- 第一电离能
- 5.278424 eV 比较所有元素的第一电离能 →
- 第二电离能
- 10.147215 eV 比较所有元素的第二电离能 →
- 第三电离能
- 31.000107 eV 比较所有元素的第三电离能 →
- 第四电离能
- 41.000141 eV 比较所有元素的第四电离能 →
- 第五电离能
- 52.900182 eV 比较所有元素的第五电离能 →
- 氧化态
- +2 比较所有元素的氧化态 →
- 价电子
- 2 比较所有元素的价电子 →
- 电子排布
- [Rn] 7s2
热力学性质
- 熔化热
- 0.08291444 eV 比较所有元素的熔化热 →
- 汽化热
- 1.171167 eV 比较所有元素的汽化热 →
- 升华热
- 1.647925 eV
- 原子化热
- 1.647925 eV
- 原子化焓
- 1.647925 eV
核性质
- 质子
- 88 比较所有元素的质子 →
- 中子
- 138 比较所有元素的中子 →
- 已知同位素
- 35 比较所有元素的已知同位素 →
- 稳定同位素
- 0 比较所有元素的稳定同位素 →
- 质量数（最稳定同位素）
- 226
- 最稳定同位素
- Ra-226
- 发现年份
- 1898
丰度
- 丰度（地壳）
- 9e-7 mg/kg 比较所有元素的丰度（地壳） →
- 丰度（海洋）
- 8.9 × 10−11 mg/L 比较所有元素的丰度（海洋） →
晶体结构
暂无
电子结构
- 各电子层电子数
- 2, 8, 18, 32, 18, 8, 2 比较所有元素的各电子层电子数 →
标识符
- CAS登记号
- 7440-14-4 比较所有元素的CAS登记号 →
- 谱项符号
- 1S0
- InChI
- InChI=1S/Ra
- InChI Key
- HCWPIIXVSYCSAN-UHFFFAOYSA-N
电子排布 实测值
Ra: 7s²[Rn] 7s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p⁶ 7s²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
无稳定同位素。
| 质量数 | 原子质量（u） | 天然丰度 | 半衰期 |
|---|---|---|---|
| 206 放射性 | 206.003828 ± 0.000019 | 暂无 | 240 ms |
| 205 放射性 | 205.006268 ± 0.000076 | 暂无 | 220 ms |
| 216 放射性 | 216.0035334 ± 0.0000094 | 暂无 | 172 ns |
| 231 放射性 | 231.041027 ± 0.000012 | 暂无 | 104 秒 |
| 230 放射性 | 230.037055 ± 0.000011 | 暂无 | 93 分钟 |
物相 / 状态
原因: 低于熔点（699.85 °C）674.9 °C
示意图，未按比例绘制
相变点
相变能
在熔点熔化1 mol物质所需的能量
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
原子光谱
已显示10项，共88项。 按离子电荷升序排列。
收录能级 ?
| 离子 | 电荷 | 能级 |
|---|---|---|
| Ra I | 0 | 82 |
| Ra II | +1 | 37 |
| Ra III | +2 | 2 |
| Ra IV | +3 | 2 |
| Ra V | +4 | 2 |
| Ra VI | +5 | 2 |
| Ra VII | +6 | 2 |
| Ra VIII | +7 | 2 |
| Ra IX | +8 | 2 |
| Ra X | +9 | 2 |
暂无晶体结构数据
离子半径
| 电荷 | 配位 | 自旋 | 半径 |
|---|---|---|---|
| +2 | 8 | 暂无 | 148 pm |
| +2 | 12 | 暂无 | 170 pm |
化合物
同位素 (5)
| 质量数 | 原子质量（u） | 天然丰度 | 半衰期 | 衰变方式 | |
|---|---|---|---|---|---|
| 206 放射性 | 206.003828 ± 0.000019 | 暂无 | 240 ms | α ≈100%β+ ? | |
| 205 放射性 | 205.006268 ± 0.000076 | 暂无 | 220 ms | α ≈100%β+ ? | |
| 216 放射性 | 216.0035334 ± 0.0000094 | 暂无 | 172 ns | α =100%ε<1e-8% | |
| 231 放射性 | 231.041027 ± 0.000012 | 暂无 | 104 秒 | β- =100% | |
| 230 放射性 | 230.037055 ± 0.000011 | 暂无 | 93 分钟 | β- =100% |
谱线
已显示50项，共90项。 默认仅显示具有实测强度的谱线。
| 波长（nm） | 强度 | 电离级 | 类型 | 跃迁 | 准确度 | 来源 | |
|---|---|---|---|---|---|---|---|
| 381.44219 nm | 200 | Ra II | emission | 7s 2S → 7p 2P* | 实测值 | NIST | |
| 468.22394 nm | 100 | Ra II | emission | 7s 2S → 7p 2P* | 实测值 | NIST | |
| 482.59281 nm | 100 | Ra I | emission | 7s2 1S → 7s.7p 1P* | 实测值 | NIST | |
| 566.0812 nm | 50 | Ra I | emission | 7s.6d 3D → 6d.7p 3F* | 实测值 | NIST | |
| 714.12167 nm | 50 | Ra I | emission | 7s2 1S → 7s.7p 3P* | 实测值 | NIST | |
| 453.3111 nm | 30 | Ra II | emission | 7p 2P* → 8s 2S | 实测值 | NIST | |
| 620.0304 nm | 30 | Ra I | emission | 7s.6d 3D → 6d.7p 3F* | 实测值 | NIST | |
| 443.6259 nm | 20 | Ra II | emission | 7p 2P* → 7d 2D | 实测值 | NIST | |
| 540.0231 nm | 20 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 540.6796 nm | 20 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 555.5852 nm | 20 | Ra I | emission | 7s.7p 3P* → 7s.7d 3D | 实测值 | NIST | |
| 581.3628 nm | 20 | Ra II | emission | 7p 2P* → 8s 2S | 实测值 | NIST | |
| 644.62 nm | 20 | Ra I | emission | 7s.7p 3P* → 7s.7d 3D | 实测值 | NIST | |
| 648.7319 nm | 20 | Ra I | emission | 7s.6d 3D → 6d.7p 3F* | 实测值 | NIST | |
| 698.0232 nm | 20 | Ra I | emission | 7s.6d 3D → 6d.7p 3F* | 实测值 | NIST | |
| 711.8486 nm | 20 | Ra I | emission | 7s.6d 3D → 6d.7p 3F* | 实测值 | NIST | |
| 722.5166 nm | 20 | Ra I | emission | 7s.6d 1D → 6d.7p 1D* | 实测值 | NIST | |
| 485.6071 nm | 10 | Ra I | emission | 7s.6d 3D → 7s.5f 3F* | 实测值 | NIST | |
| 485.942 nm | 10 | Ra II | emission | 5f 2F* → 6g 2G | 实测值 | NIST | |
| 492.752 nm | 10 | Ra II | emission | 5f 2F* → 6g 2G | 实测值 | NIST | |
| 520.5948 nm | 10 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 528.3277 nm | 10 | Ra I | emission | 7s.7p 3P* → 7s.7d 3D | 实测值 | NIST | |
| 532.029 nm | 10 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 539.9784 nm | 10 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 550.1985 nm | 10 | Ra I | emission | 7s.7p 3P* → 7p2? 3P | 实测值 | NIST | |
| 555.3574 nm | 10 | Ra I | emission | 7s.7p 3P* → 7s.7d 3D | 实测值 | NIST | |
| 561.6661 nm | 10 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 633.6899 nm | 10 | Ra I | emission | 7s.6d 1D → 7s.8p 1P* | 实测值 | NIST | |
| 659.3341 nm | 10 | Ra II | emission | 5f 2F* → 5g 2G | 实测值 | NIST | |
| 671.932 nm | 10 | Ra II | emission | 5f 2F* → 5g 2G | 实测值 | NIST | |
| 731.0269 nm | 10 | Ra I | emission | 7s.7p 3P* → 7s.8s 3S | 实测值 | NIST | |
| 419.4091 nm | 8 | Ra II | emission | 5f 2F* → 7g 2G | 实测值 | NIST | |
| 424.472 nm | 8 | Ra II | emission | 5f 2F* → 7g 2G | 实测值 | NIST | |
| 464.1284 nm | 8 | Ra I | emission | 7s.6d 3D → 7s.5f 3F* | 实测值 | NIST | |
| 469.9272 nm | 8 | Ra I | emission | 7s.6d 3D → 7s.5f 3F* | 实测值 | NIST | |
| 548.215 nm | 8 | Ra I | emission | 7s.6d 3D → 6d.7p 3D* | 实测值 | NIST | |
| 508.1036 nm | 6 | Ra I | emission | 7s.6d 3D → 6d.7p 3P* | 实测值 | NIST | |
| 566.165 nm | 6 | Ra II | emission | 8p 2P* → 9d 2D | 实测值 | NIST | |
| 389.455 nm | 5 | Ra II | emission | 5f 2F* → 8g 2G | 实测值 | NIST | |
| 497.179 nm | 5 | Ra I | emission | 7s.6d 3D → 6d.7p 3P* | 实测值 | NIST | |
| 504.154 nm | 5 | Ra I | emission | 7s.6d 3D → 6d.7p 3P* | 实测值 | NIST | |
| 560.143 nm | 5 | Ra I | emission | 7s.6d 3D → 7s.8p 3P* | 实测值 | NIST | |
| 577.824 nm | 5 | Ra I | emission | 7s.6d 1D → 6d.7p 3P* | 实测值 | NIST | |
| 579.5745 nm | 5 | Ra I | emission | 7s.7p 3P* → 7p2? 3P | 实测值 | NIST | |
| 581.1588 nm | 5 | Ra I | emission | 7s.6d 3D → 6d.7p 1D* | 实测值 | NIST | |
| 616.7051 nm | 5 | Ra I | emission | 7s.6d 3D → 6d.7p 1D* | 实测值 | NIST | |
| 707.79042 nm | 5 | Ra II | emission | 6d 2D → 7p 2P* | 实测值 | NIST | |
| 417.798 nm | 4 | Ra I | emission | 7s.6d 3D → 7s.6f 3F* | 实测值 | NIST | |
| 430.5 nm | 4 | Ra I | emission | 7s.6d 3D → 7s.6f 3F* | 实测值 | NIST | |
| 490.3263 nm | 4 | Ra I | emission | 7s.6d 3D → 6d.7p 3P* | 实测值 | NIST |
扩展性质
共价半径（扩展）
- 共价半径（Pyykkö）
- 201 pm
- 共价半径（Pyykkö，双键）
- 173 pm
- 共价半径（Pyykkö，三键）
- 159 pm
范德华半径
- Truhlar
- 283 pm
- UFF
- 367.7 pm
- MM3
- 327 pm
原子半径与金属半径
- 原子半径（Rahm）
- 292 pm
编号标度
- Mendeleev
- 10
- Pettifor
- 13
- Glawe
- 13
电负性标度
- Ghosh
- 0
极化率与色散
- 偶极极化率
- 246 a.u.
- 偶极极化率（不确定度）
- 4 a.u.
相变与同素异形体
| 熔点 | 969.15 K |
氧化态分类
高级参考数据
晶体半径详情 (2)
| 电荷 | CN | 自旋 | rcrystal (pm) | 来源 |
|---|---|---|---|---|
| 2 | VIII | 162 | from r^3 vs V plots, | |
| 2 | XII | 184 | from r^3 vs V plots, |
同位素衰变方式 (55)
| 同位素 | 模式 | 强度 |
|---|---|---|
| 201 | A | 100% |
| 202 | A | 100% |
| 203 | A | 100% |
| 203 | B+ | — |
| 204 | A | 100% |
| 204 | B+ | — |
| 205 | A | 100% |
| 205 | B+ | — |
| 206 | A | 100% |
| 206 | B+ | — |
X射线散射因子 (516)
| 能量 (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0.04162 |
| 10.1617 | — | 0.04479 |
| 10.3261 | — | 0.0482 |
| 10.4931 | — | 0.05188 |
| 10.6628 | — | 0.05584 |
| 10.8353 | — | 0.0601 |
| 11.0106 | — | 0.06468 |
| 11.1886 | — | 0.06961 |
| 11.3696 | — | 0.07492 |
| 11.5535 | — | 0.08102 |
补充数据
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
9×10-7 milligrams per kilogram
参考文献 (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
8.9×10-11 milligrams per liter
参考文献 (1)
Sources
Sources of this element.
Originally, radium was obtained from the rich pitchblende ore found in Joachimsthal, Bohemia. The carnotite sands of Colorado furnish some radium, but richer ores are found in the Republic of Zaire and the Great Lake region of Canada. Radium is present in all uranium minerals, and could be extracted, if desired, from the extensive wastes of uranium processing. Large uranium deposits are located in Ontario, New Mexico, Utah, Australia, and elsewhere.
参考文献 (1)
- [6] Radium https://periodic.lanl.gov/88.shtml
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 Radium.
The element property data was retrieved from publications.