Potassium (K)
alkali-metalSolid
標準原子量
39.0983 u電子配置
[Ar] 4s1融点
63.38 °C沸点
758.85 °C密度
890 kg/m³酸化数
−1, +1電気陰性度（Pauling）
0.82第1イオン化エネルギー
4.340664 eV発見年
1807原子半径
220 pm詳細
Potassium is an alkali metal and a major rock-forming and biological element. It occurs naturally only in compounds, chiefly as K⁺ in salts, feldspars, micas, and clay minerals. The metal is highly electropositive, reacts vigorously with water, and is stored away from air and moisture. In living cells, potassium is the principal intracellular cation and is central to osmotic balance and electrical signaling.
It is one of the most reactive and electropositive of metals. Except for lithium, it is the lightest known metal. It is soft, easily cut with a knife, and is silvery in appearance immediately after a fresh surface is exposed. It rapidly oxidizes in air and must be preserved in a mineral oil such as kerosene.
As with other metals of the alkali group, it decomposes in water with the evolution of hydrogen. It catches fire spontaneously on water. Potassium and its salts impart a violet color to flames.
The name derives from the English "potash" or "pot ashes" because it is found in caustic potash (KOH). The symbol K derives from the Latin kalium via the Arabic qali for alkali. It was first isolated by the British chemist Humphry Davy in 1807 from electrolysis of potash (KOH).
Although potassium is the eighth most abundant element on earth and comprises about 2.1% of the earth's crust, it is a very reactive element and is never found free in nature. Metallic potassium was first isolated by Sir Humphry Davy in 1807 through the electrolysis of molten caustic potash (KOH). A few months after discovering potassium, Davy used the same method to isolate sodium. Potassium can be obtained from the minerals sylvite (KCl), carnallite (KCl·MgCl2·6H2O), langbeinite (K2Mg2(SO4)3) and polyhalite (K2Ca2Mg(SO4)4·2H2O). These minerals are often found in ancient lake and sea beds. Caustic potash, another important source of potassium, is primarily mined in Germany, New Mexico, California and Utah. Pure potassium is a soft, waxy metal that can be easily cut with a knife. It reacts with oxygen to form potassium superoxide (KO2) and with water to form potassium hydroxide (KOH), hydrogen gas and heat. Enough heat is produced to ignite the hydrogen gas. To prevent it from reacting with the oxygen and water in the air, samples of metallic potassium are usually stored submerged in mineral oil.
From the English word, potash - pot ashes; Latin kalium, Arab qali, alkali. Discovered in 1807 by Davy, who obtained it from caustic potash (KOH); this was the first metal isolated by electrolysis.
Pure potassium is a very soft, silvery metal when freshly cut. It tarnishes rapidly in air as oxide, hydroxide, and carbonate layers form. It has a low melting point for a metal and can be cut with a knife; samples are commonly kept under dry mineral oil or inert gas.
Elemental potassium has limited direct use because sodium is cheaper and less reactive for many purposes. It is used in some laboratory reductions and in potassium-sodium alloys for heat-transfer applications where a liquid metal is useful. Most practical demand is for potassium compounds, especially fertilizers that supply plant-available K⁺. Potassium salts are also used in glass, soaps, pyrotechnics, food processing, and chemical manufacturing.
Potassium forms an alloy with sodium (NaK) that is used as a heat transfer medium in some types of nuclear reactors.
Potassium forms many important compounds. Potassium chloride (KCl) is the most common potassium compound. It is used in fertilizers, as a salt substitute and to produce other chemicals. Potassium hydroxide (KOH) is used to make soaps, detergents and drain cleaners. Potassium carbonate (KHCO3), also known as pearl ash, is used to make some types of glass and soaps and is obtained commercially as a byproduct of the production of ammonia. Potassium superoxide (KO2) can create oxygen from water vapor (H2O) and carbon dioxide (CO2) through the following reaction: 2KO2 + H2O + 2CO2 => 2KHCO3 + O2. It is used in respiratory equipment and is produced by burning potassium metal in dry air. Potassium nitrate (KNO3), also known as saltpeter or nitre, is used in fertilizers, match heads and pyrotechnics.
The greatest demand for potash has been in its use for fertilizers. Potassium is an essential constituent for plant growth and is found in most soils.
An alloy of sodium and potassium (NaK) is used as a heat-transfer medium. Many potassium salts are of utmost importance, including the hydroxide, nitrate, carbonate, chloride, chlorate, bromide, iodide, cyanide, sulfate, chromate, and dichromate.
Isotopes in Biology
The mole fraction of 40K, n(40K)/n(K), is used to study the effects of potassium in soil on the growth of plants. Plants need potassium to promote growth and reproduction, and potassium also helps plants resist drought and diseases. The mole fraction of 40K is being studied at different depths in several soil types to determine how soil properties affect the fractionation of 40K [178] R. Fujiyoshi, Y. Satake, T. Sumiyoshi. J. Radioanal. Nucl. Chem.281, 553 (2009)..
Isotopes in Geochronology
The amount ratio n(40K)/n(40Ar) is used in potassium-argon dating by geologists, archaeologists, and paleoanthropologists to determine the age of rocks. This dating method is based on the radioactive decay of 40K, having a half-life of 1.248×109 years, to 40Ar. When lava crystalizes, 40Ar can no longer escape and begins increasing in concentration in a rock (Fig. IUPAC.19.1) [179] United States Geological Survey. Geology and Geophysics, U.S. Geological Survey (2014), Feb. 25; http://geomaps.wr.usgs.gov/common/geochronology.html., [180] New Mexico Bureau of Geology & Mineral Resources. K/Ar and 40Ar/39Ar Methods, New Mexico Bureau of Geology & Mineral Resources (2014), Feb. 25; http://geoinfo.nmt.edu/labs/argon/methods/home.html..
Isotopes in Medicine
38K, which has a half-life of 7.6 min and is produced by a nuclear reaction involving 38Ar and 40Ar as targets, is a widely used blood-flow tracer. Because 38Ar is more expensive, 40Ar, which also offers many additional advantages as a target, is more commonly used to produce 38K for medical purposes [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., [176] K. Nagatsu, A. Kubodera, K. Suzuki. Appl. Radiat. Isot.49, 1505 (1998)., [181] P. G. Melon, C. Brihaye, C. Degueldre, M. Guillaume, R. Czichosz, P. Rigo, H. E. Kulbertus, D. Comar. J. Nucl. Med.35, 1116 (1994)..
Potassium chemistry is dominated by the +1 oxidation state and the K⁺ ion. Common compounds include potassium chloride (KCl), the main fertilizer potash salt; potassium hydroxide (KOH), a strong base used in alkaline chemistry; potassium carbonate (K₂CO₃); potassium nitrate (KNO₃), an oxidizing salt; and potassium permanganate (KMnO₄), in which potassium is only the counterion to permanganate. Potassium forms ionic halides, oxides, superoxide potassium superoxide (KO₂), and many double salts and aluminosilicates.
See more information at the Potassium compound page.
Metallic potassium is a severe fire and chemical hazard. It reacts with water to form potassium hydroxide (KOH) and hydrogen (H₂), often with enough heat to ignite the gas. Concentrated potassium hydroxide is strongly corrosive. Soluble potassium salts vary widely in hazard; ordinary dietary amounts are essential, but excessive intake or medical exposure can disturb heart rhythm. Natural potassium contains radioactive ⁴⁰K at low abundance.
Potassium is abundant in the crust and is released slowly by weathering of silicate minerals, then cycled through soils, waters, plants, and organisms as K⁺. It is not degraded, but it is redistributed by erosion, leaching, uptake, and ion exchange on clays. Potassium is an essential plant nutrient, and deficiency limits crop growth in many soils. The isotope ⁴⁰K is a natural source of background radiation.
The potassium economy is centered on potash minerals and brines rather than the free metal. Commercial products are mined or solution-mined from evaporite deposits and processed mainly into potassium chloride (KCl), with potassium sulfate (K₂SO₄) important for chloride-sensitive crops. Demand is strongly linked to agriculture, so fertilizer logistics and ore quality dominate supply. Elemental potassium is made by chemical reduction or electrochemical routes on a much smaller scale and is not a bulk commodity comparable with sodium.
The metal is the seventh most abundant and makes up about 2.4% by weight of the earth's crust. Most potassium minerals are insoluble and the metal is obtained from them only with great difficulty.
Certain minerals, however, such as sylvite, carnallite, langbeinite, and polyhalite are found in ancient lake and sea beds and form rather extensive deposits from which potassium and its salts can readily be obtained. Potash is mined in Germany, New Mexico, California, Utah, and elsewhere. Large deposits of potash, found at a depth of some 3000 ft in Saskatchewan, promise to be important in coming years.
Potassium is also found in the ocean, but is present only in relatively small amounts, compared to sodium.
Potassium is produced in stellar nucleosynthesis and supernova-related processes but is far less abundant cosmically than lighter elements such as sodium, magnesium, and silicon. In rocky planets it behaves as a moderately incompatible lithophile element, concentrating in crustal rocks and evolved magmas. Radioactive ⁴⁰K contributed heat to early planetary interiors and remains important in geochronology.
- The chemical symbol K comes from kalium, a Neo-Latin name derived from alkali sources.
- Potassium metal is less dense than water, although contact with water is violently reactive.
- Potassium chloride can be purple or reddish as a mineral because of impurities or radiation-induced color centers.
- Potassium-argon dating depends on the decay of ⁴⁰K to ⁴⁰Ar trapped in minerals.
- Potassium superoxide (KO₂) has been used in breathing equipment because it reacts with CO₂ and moisture to release O₂.
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性質
物理的性質
- 原子半径（経験値）
- 220 pm 全元素の原子半径（経験値）を比較 →
- 共有結合半径
- 203 pm 全元素の共有結合半径を比較 →
- ファンデルワールス半径
- 275 pm 全元素のファンデルワールス半径を比較 →
- 金属半径
- 203 pm 全元素の金属半径を比較 →
- 密度
- 890 kg/m³ 全元素の密度を比較 →
- モル体積
- 0.0453 L/mol
- 標準温度・圧力（STP）での相
- 固体 全元素の標準温度・圧力（STP）での相を比較 →
- 融点
- 63.38 °C 全元素の融点を比較 →
- 沸点
- 758.85 °C 全元素の沸点を比較 →
- 熱伝導率
- 79 W/(m·K) 全元素の熱伝導率を比較 →
- 比熱容量
- 0.757 J/(g·K) 全元素の比熱容量を比較 →
- モル熱容量
- 29.6 J/(mol·K) 全元素のモル熱容量を比較 →
- 結晶構造
- 体心立方構造 全元素の結晶構造を比較 →
化学的性質
- 電気陰性度（Pauling）
- 0.82 全元素の電気陰性度（Pauling）を比較 →
- 電気陰性度（Allen）
- 0.734
- 電子親和力
- 0.5014 eV
- 第1イオン化エネルギー
- 4.340664 eV 全元素の第1イオン化エネルギーを比較 →
- 第2イオン化エネルギー
- 31.625109 eV 全元素の第2イオン化エネルギーを比較 →
- 第3イオン化エネルギー
- 45.803258 eV 全元素の第3イオン化エネルギーを比較 →
- 第4イオン化エネルギー
- 60.91721 eV 全元素の第4イオン化エネルギーを比較 →
- 第5イオン化エネルギー
- 82.660285 eV 全元素の第5イオン化エネルギーを比較 →
- 酸化数
- −1, +1 全元素の酸化数を比較 →
- 価電子
- 1 全元素の価電子を比較 →
- 電子配置
- [Ar] 4s1
熱力学的性質
- 臨界点（温度）
- 1950 °C
- 臨界点（圧力）
- 1.6e+7 Pa
- 融解熱
- 0.02414883 eV 全元素の融解熱を比較 →
- 蒸発熱
- 0.79701508 eV 全元素の蒸発熱を比較 →
- 昇華熱
- 0.92449604 eV
- 原子化熱
- 0.92449604 eV
- 原子化エンタルピー
- 0.92242317 eV
原子核
- 陽子数
- 19 全元素の陽子数を比較 →
- 中性子数
- 20 全元素の中性子数を比較 →
- 既知の同位体
- 29 全元素の既知の同位体を比較 →
- 安定同位体
- 2 全元素の安定同位体を比較 →
- 最も安定な同位体
- K-39
- 発見年
- 1807
存在度
- 存在度（地殻）
- 2.09e+4 mg/kg 全元素の存在度（地殻）を比較 →
- 存在度（海洋）
- 399 mg/L 全元素の存在度（海洋）を比較 →
結晶構造
- 格子定数a
- 523 pm
電子構造
- 各電子殻の電子数
- 2, 8, 8, 1 全元素の各電子殻の電子数を比較 →
識別子
- CAS登録番号
- 7440-09-7 全元素のCAS登録番号を比較 →
- 項記号
- 2S1/2
- InChI
- InChI=1S/K
- InChI Key
- ZLMJMSJWJFRBEC-UHFFFAOYSA-N
電子配置 測定値
K: 4s¹[Ar] 4s¹1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹原子モデル
同位体によって中性子数、質量、安定性は変わりますが、中性原子の電子配置は変わりません。
模式的な原子モデルです。実際の縮尺とは異なります。
原子の指紋
発光／吸収スペクトル
同位体分布
| 質量数 | 原子質量（u） | 天然存在比 | 半減期 |
|---|---|---|---|
| 39 安定 | 38.9637064864 ± 0.0000000049 | 93.2581% | 安定 |
| 41 安定 | 40.9618252579 ± 0.0000000041 | 6.7302% | 安定 |
相／状態
理由: 融点（63.38 °C）より38.4 °C低い
模式図、実際の縮尺とは異なります
相転移点
相転移エネルギー
融点で1 molを融解させるのに必要なエネルギー
沸点で1 molを蒸発させるのに必要なエネルギー
昇華点で1 molを昇華させるのに必要なエネルギー
密度
標準条件下
標準条件下
詳細
原子スペクトル
全22件中10件を表示しています。 イオンの電荷の昇順で並べています。
準位データの収録状況 ?
| イオン | 電荷 | 準位 |
|---|---|---|
| 41K I 同位体 | 0 | 8 |
| 40K I 同位体 | 0 | 3 |
| 39K I 同位体 | 0 | 123 |
| K I | 0 | 299 |
| K II | +1 | 97 |
| K III | +2 | 40 |
| K IV | +3 | 38 |
| K V | +4 | 40 |
| K VI | +5 | 28 |
| K VII | +6 | 81 |
イオン半径
| 電荷 | 配位 | スピン | 半径 |
|---|---|---|---|
| +1 | 4 | データなし | 137 pm |
| +1 | 6 | データなし | 138 pm |
| +1 | 7 | データなし | 146 pm |
| +1 | 8 | データなし | 151 pm |
| +1 | 9 | データなし | 155 pm |
| +1 | 10 | データなし | 159 pm |
| +1 | 12 | データなし | 164 pm |
化合物
同位体 (2)
Seventeen isotopes of potassium are known. Ordinary potassium is composed of three isotopes, one of which is 40°K (0.0118%), a radioactive isotope with a half-life of 1.28 x 109 years.
| 質量数 | 原子質量（u） | 天然存在比 | 半減期 | 崩壊形式 | |
|---|---|---|---|---|---|
| 39 安定 | 38.9637064864 ± 0.0000000049 | 93.2581% ± 0.0044% | 安定 | stable | |
| 41 安定 | 40.9618252579 ± 0.0000000041 | 6.7302% ± 0.0044% | 安定 | stable |
スペクトル線
全141件中50件を表示しています。 初期設定では、強度の測定値があるスペクトル線のみを表示します。
| 波長（nm） | 強度 | 電離段階 | 種類 | 遷移 | 精度 | 出典 | |
|---|---|---|---|---|---|---|---|
| 693.8764 nm | 20 | K I | emission | 3p6.4p 2P* → 3p6.6s 2S | 測定値 | NIST | |
| 691.10815 nm | 19 | K I | emission | 3p6.4p 2P* → 3p6.6s 2S | 測定値 | NIST | |
| 404.41422 nm | 18 | K I | emission | 3p6.4s 2S → 3p6.5p 2P* | 測定値 | NIST | |
| 404.72132 nm | 17 | K I | emission | 3p6.4s 2S → 3p6.5p 2P* | 測定値 | NIST | |
| 580.17662 nm | 17 | K I | emission | 3p6.4p 2P* → 3p6.7s 2S | 測定値 | NIST | |
| 583.18899 nm | 17 | K I | emission | 3p6.4p 2P* → 3p6.5d 2D | 測定値 | NIST | |
| 578.23999 nm | 16 | K I | emission | 3p6.4p 2P* → 3p6.7s 2S | 測定値 | NIST | |
| 581.21521 nm | 15 | K I | emission | 3p6.4p 2P* → 3p6.5d 2D | 測定値 | NIST | |
| 535.95761 nm | 14 | K I | emission | 3p6.4p 2P* → 3p6.6d 2D | 測定値 | NIST | |
| 533.96873 nm | 13 | K I | emission | 3p6.4p 2P* → 3p6.8s 2S | 測定値 | NIST | |
| 511.225448 nm | 12 | K I | emission | 3p6.4p 2P* → 3p6.7d 2D | 測定値 | NIST | |
| 532.32786 nm | 12 | K I | emission | 3p6.4p 2P* → 3p6.8s 2S | 測定値 | NIST | |
| 534.29693 nm | 12 | K I | emission | 3p6.4p 2P* → 3p6.6d 2D | 測定値 | NIST | |
| 693.62861 nm | 12 | K I | emission | 3p6.4p 2P* → 3p6.4d 2D | 測定値 | NIST | |
| 696.46903 nm | 12 | K I | emission | 3p6.4p 2P* → 3p6.4d 2D | 測定値 | NIST | |
| 464.23725 nm | 11 | K I | emission | 3p6.4s 2S → 3p6.3d 2D | 測定値 | NIST | |
| 509.717137 nm | 11 | K I | emission | 3p6.4p 2P* → 3p6.7d 2D | 測定値 | NIST | |
| 509.920005 nm | 11 | K I | emission | 3p6.4p 2P* → 3p6.9s 2S | 測定値 | NIST | |
| 464.1875 nm | 10 | K I | emission | 3p6.4s 2S → 3p6.3d 2D | 測定値 | NIST | |
| 496.503213 nm | 10 | K I | emission | 3p6.4p 2P* → 3p6.8d 2D | 測定値 | NIST | |
| 508.423399 nm | 10 | K I | emission | 3p6.4p 2P* → 3p6.9s 2S | 測定値 | NIST | |
| 482.924 nm | 9 | K II | emission | 3p5.4s 3P* → 3p5.4p 3S | 測定値 | NIST | |
| 486.975897 nm | 9 | K I | emission | 3p6.4p 2P* → 3p6.9d 2D | 測定値 | NIST | |
| 495.081801 nm | 9 | K I | emission | 3p6.4p 2P* → 3p6.8d 2D | 測定値 | NIST | |
| 495.614802 nm | 9 | K I | emission | 3p6.4p 2P* → 3p6.10s 2S | 測定値 | NIST | |
| 389.7896 nm | 8 | K II | emission | 3p5.4s 3P* → 3p5.4p 1D | 測定値 | NIST | |
| 418.6232 nm | 8 | K II | emission | 3p5.4s 3P* → 3p5.4p 3D | 測定値 | NIST | |
| 460.849 nm | 8 | K II | emission | 3p5.4s 1P* → 3p5.4p 1D | 測定値 | NIST | |
| 480.43395 nm | 8 | K I | emission | 3p6.4p 2P* → 3p6.10d 2D | 測定値 | NIST | |
| 485.609209 nm | 8 | K I | emission | 3p6.4p 2P* → 3p6.9d 2D | 測定値 | NIST | |
| 486.348075 nm | 8 | K I | emission | 3p6.4p 2P* → 3p6.11s 2S | 測定値 | NIST | |
| 500.564 nm | 8 | K II | emission | 3p5.4s 3P* → 3p5.4p 3S | 測定値 | NIST | |
| 612.028 nm | 8 | K II | emission | 3p5.3d 3F* → 3p5.4p 3D | 測定値 | NIST | |
| 381.7547 nm | 7 | K II | emission | 3p5.4p 3D → 3p5.(2P*<3/2>).5s 2[3/2]* | 測定値 | NIST | |
| 400.122 nm | 7 | K II | emission | 3p5.4s 3P* → 3p5.4p 3P | 測定値 | NIST | |
| 413.4705 nm | 7 | K II | emission | 3p5.4s 3P* → 3p5.4p 3D | 測定値 | NIST | |
| 422.296 nm | 7 | K II | emission | 3p5.4s 1P* → 3p5.4p 3P | 測定値 | NIST | |
| 422.566 nm | 7 | K II | emission | 3p5.3d 3P* → 3p5.4p 1D | 測定値 | NIST | |
| 426.334 nm | 7 | K II | emission | 3p5.4s 3P* → 3p5.4p 3D | 測定値 | NIST | |
| 430.498 nm | 7 | K II | emission | 3p5.3d 3P* → 3p5.4p 1D | 測定値 | NIST | |
| 430.911 nm | 7 | K II | emission | 3p5.4s 1P* → 3p5.4p 3P | 測定値 | NIST | |
| 438.816 nm | 7 | K II | emission | 3p5.4s 1P* → 3p5.4p 1P | 測定値 | NIST | |
| 475.737719 nm | 7 | K I | emission | 3p6.4p 2P* → 3p6.11d 2D | 測定値 | NIST | |
| 479.104132 nm | 7 | K I | emission | 3p6.4p 2P* → 3p6.10d 2D | 測定値 | NIST | |
| 484.98645 nm | 7 | K I | emission | 3p6.4p 2P* → 3p6.11s 2S | 測定値 | NIST | |
| 505.625 nm | 7 | K II | emission | 3p5.3d 3P* → 3p5.4p 3S | 測定値 | NIST | |
| 630.728 nm | 7 | K II | emission | 3p5.3d 3F* → 3p5.4p 3D | 測定値 | NIST | |
| 696.41712 nm | 7 | K I | emission | 3p6.4p 2P* → 3p6.4d 2D | 測定値 | NIST | |
| 380.0162 nm | 6 | K II | emission | 3p5.4p 3D → 3p5.(2P*<3/2>).5s 2[3/2]* | 測定値 | NIST | |
| 381.657 nm | 6 | K II | emission | 3p5.4p 3P → 3p5.4d 3P* | 測定値 | NIST |
詳細な性質
共有結合半径（詳細）
- 共有結合半径（Pyykkö）
- 196 pm
- 共有結合半径（Pyykkö、二重結合）
- 193 pm
- 共有結合半径（Bragg）
- 207 pm
ファンデルワールス半径
- Bondi
- 275 pm
- Batsanov
- 280 pm
- Alvarez
- 273 pm
- UFF
- 381.2 pm
- MM3
- 309 pm
原子半径と金属半径
- 原子半径（Rahm）
- 234 pm
- 金属半径（C12）
- 235 pm
番号付けの尺度
- Mendeleev
- 3
- Pettifor
- 10
- Glawe
- 10
電気陰性度の尺度
- Ghosh
- 0
- Miedema
- 2
- Gunnarsson–Lundqvist
- 2
- Robles–Bartolotti
- 1
分極率と分散
- 双極子分極率
- 289.7 a.u.
- 双極子分極率（不確かさ）
- 0.3 a.u.
- C₆
- 3923 Ha·Bohr6
- C₆ (Gould–Bučko)
- 3910 Ha·Bohr6
ミーデマパラメータ
- ミーデマモル体積
- 45.63 cm3/mol
- ミーデマ電子密度
- 0
供給リスクと経済性
- 生産集中度
- 21
- 相対供給リスク
- 5
- 埋蔵量の分布
- 61
- 政治的安定性（最大生産国）
- 81
- 政治的安定性（最大埋蔵国）
- 81
相転移と同素体
| 融点 | 336.65 K |
| 沸点 | 1032.15 K |
| 臨界点（温度） | 2223.15 K |
| 臨界点（圧力） | 16 MPa |
酸化数の分類
専門参考データ
遮蔽定数 (6)
| n | 軌道 | σ |
|---|---|---|
| 1 | s | 0.5105 |
| 2 | p | 3.9728 |
| 2 | s | 5.9938 |
| 3 | p | 11.2744 |
| 3 | s | 10.3201 |
| 4 | s | 15.5048 |
結晶半径の詳細 (7)
| 電荷 | CN | スピン | rcrystal (pm) | 由来 |
|---|---|---|---|---|
| 1 | IV | 151 | ||
| 1 | VI | 152 | ||
| 1 | VII | 160 | ||
| 1 | VIII | 165 | ||
| 1 | IX | 169 | ||
| 1 | X | 173 | ||
| 1 | XII | 178 |
同位体の崩壊形式 (53)
| 同位体 | モード | 強度 |
|---|---|---|
| 31 | 3p | 100% |
| 32 | p | — |
| 33 | p | — |
| 34 | p | — |
| 35 | B+ | 100% |
| 35 | B+p | 0.4% |
| 36 | B+ | 100% |
| 36 | B+p | 0% |
| 36 | B+A | 0% |
| 37 | B+ | 100% |
X線散乱因子 (503)
| エネルギー (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0.03426 |
| 10.1617 | — | 0.03529 |
| 10.3261 | — | 0.03635 |
| 10.4931 | — | 0.03744 |
| 10.6628 | — | 0.03856 |
| 10.8353 | — | 0.03972 |
| 11.0106 | — | 0.04091 |
| 11.1886 | — | 0.04214 |
| 11.3696 | — | 0.0434 |
| 11.5535 | — | 0.04471 |
追加データ
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.09×104 milligrams per kilogram
参考文献 (1)
- [5] Potassium https://education.jlab.org/itselemental/ele019.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
3.99×102 milligrams per liter
参考文献 (1)
- [5] Potassium https://education.jlab.org/itselemental/ele019.html
Sources
Sources of this element.
The metal is the seventh most abundant and makes up about 2.4% by weight of the earth's crust. Most potassium minerals are insoluble and the metal is obtained from them only with great difficulty.
Certain minerals, however, such as sylvite, carnallite, langbeinite, and polyhalite are found in ancient lake and sea beds and form rather extensive deposits from which potassium and its salts can readily be obtained. Potash is mined in Germany, New Mexico, California, Utah, and elsewhere. Large deposits of potash, found at a depth of some 3000 ft in Saskatchewan, promise to be important in coming years.
Potassium is also found in the ocean, but is present only in relatively small amounts, compared to sodium.
参考文献 (1)
- [6] Potassium https://periodic.lanl.gov/19.shtml
Production
Production of this element (from raw materials or other compounds containing the element).
Potassium is never found free in nature, but is obtained by electrolysis of the hydroxide, much in the same manner as prepared by Davy's first process. Thermal methods also are commonly used to produce potassium (such as by reduction of potassium compounds with CaC2, C, Si, or Na).
参考文献 (1)
- [6] Potassium https://periodic.lanl.gov/19.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 Potassium.
The element property data was retrieved from publications.