Thallium (Tl)
post-transition-metalSolid
표준 원자량
204.38 u [204.382, 204.385]전자 배치
[Xe] 6s2 4f14 5d10 6p1녹는점
303.85 °C끓는점
1472.85 °C밀도
1.18e+4 kg/m³산화 상태
−5, −2, −1, +1, +2, +3전기 음성도(Pauling)
1.62제1 이온화 에너지
6.108287 eV발견 연도
1861원자 반지름
190 pm상세 정보
Thallium is a soft post-transition metal in group 13. It is chemically notable for the stability of the +1 oxidation state, which reflects the inert-pair effect and makes many thallium(I) salts resemble alkali-metal salts in size and solubility behavior. The element is rare in ores and is usually recovered as a by-product of processing sulfide minerals. Its severe toxicity has greatly reduced former consumer and agricultural uses.
When freshly exposed to air, thallium exhibits a metallic luster, but soon develops a bluish-gray tinge, resembling lead in appearance. A heavy oxide builds up on thallium if left in air, and in the presence of water the hydride is formed. The metal is very soft and malleable. It can be cut with a knife. Twenty five isotopic forms of thallium, with atomic masses ranging from 184 to 210 are recognized. Natural thallium is a mixture of two isotopes. A mercury-thallium alloy, which forms a eutectic at 8.5% thallium, is reported to freeze at -60C, some 20 degrees below the freezing point of mercury.
The name derives from the Greek thallos for "green shoot" or "twig" because of the bright green line in its spectrum. Thallium was discovered by the English physicist and chemist William Crookes in 1861. Metallic thallium was first isolated by the French chemist Claude-Auguste Lamy in 1862.
Thallium was discovered spectroscopically by Sir William Crookes, an English chemist, in 1861. Crooks had obtained the sludge left over from the production of sulfuric acid (H2SO4) from a friend. After removing all of the selenium from the sludge, he inspected it with a device known as a spectroscope to look for signs of tellurium. Rather than seeing the yellow spectral lines produced by tellurium, he observed a bright green line that no one had ever seen before. He named the new element that was producing the green line thallium, after the greek word for 'green twig', thallos. He isolated samples of thallium the next year. Thallium is found in the minerals crooksite (CuThSe), lorandite (TlAsS2) and hutchinsonite ((Pb, Tl)2As5S9), but is usually obtained as a byproduct of the production of sulfuric acid or as a byproduct of refining zinc or lead.
From Greek thallos, meanin a green shoot or twig. Thallium was discovered spectroscopically in 1861 by Crookes. The element was named after the beautiful green spectral line, which identified the element. The metal was isolated both by Crookes and by Lamy in 1862 at about the same time.
Pure thallium is a very soft, heavy metal with a fresh silvery luster. It tarnishes readily in air, developing a dull gray oxide coating. It is malleable enough to be cut with a knife and has a relatively low melting point for a metal.
Current uses are limited by toxicity and regulation. Thallium is used in some specialty infrared optical materials, low-melting glasses, and semiconductor or detector research. Thallium-201 is an important medical radioisotope for diagnostic imaging of cardiac perfusion. Historical uses included rodenticides, insecticides, and depilatory agents, but these were abandoned or tightly restricted in many countries because of poisoning risks.
There are no uses for metallic thallium since pure thallium quickly combines with oxygen and water vapor from the atmosphere, forming a black, powdery substance. Thallium, used in conjunction with sulfur or selenium and arsenic, forms low melting glass. Thallium sulfate (Tl2SO4), an odorless, tasteless thallium compound, was once used as a rat and ant poison, although it has been banned from household use in the United States since 1974. Thallium sulfide (Tl2S), thallium iodide (TlI) and thallium bromide (TlBr) are all compounds used in devices to detect infrared radiation.
Thallium sulfate has been widely employed as a rodenticide and ant killer. It is odorless and tasteless, giving no warning of its presence. Its use, however, has been prohibited in the U.S. since 1975 as a household insecticide and rodenticide. The electrical conductivity of thallium sulfide changes with exposure to infrared light, and this compound is used in photocells. Thallium bromide-iodide crystals have been used as infrared optical materials. Thallium has been used, with sulfur or selenium and arsenic, to produce low melting glasses with become fluid between 125 and 150C. These glasses have properties at room temperatures similar to ordinary glasses and are said to be durable and insoluble in water. Thallium oxide has been used to produce glasses with a high index of refraction, and is used in the manufacture of photo cells. Thallium has been used in treating ringworm and other skin infections; however, its use has been limited because of the narrow margin between toxicity and therapeutic benefits.
Isotopes in Earth/Planetary Science
Because molecules, atoms, and ions of the stable isotopes of thallium possess slightly different physical and chemical properties, they commonly will be fractionated during physical, chemical, and biological processes, giving rise to variations in isotopic abundances and in atomic weights. There are substantial variations in the isotopic abundances of thallium in natural terrestrial materials (Fig. IUPAC.81.1). These variations are useful in investigating the origin of substances and studying environmental, hydrological, and geological processes [538] M. Rehkamper, M. Frank, J. R. Hein, D. Porcelli, A. Halliday, J. Ingri, V. Liebetrau. Earth. Planet. Sci. Lett.197, 65 (2002).. The isotope-amount ratio n(205Tl)/n(203Tl) has been used to study how trace metals are transported and distributed in hydrothermal fluids [538] M. Rehkamper, M. Frank, J. R. Hein, D. Porcelli, A. Halliday, J. Ingri, V. Liebetrau. Earth. Planet. Sci. Lett.197, 65 (2002).. The n(205Tl)/n(203Tl) ratio has also been used to study the cycling, distribution, and behavior of thallium in the marine environment [538] M. Rehkamper, M. Frank, J. R. Hein, D. Porcelli, A. Halliday, J. Ingri, V. Liebetrau. Earth. Planet. Sci. Lett.197, 65 (2002)..
Isotopes in Medicine
201Tl scintigraphy is used to detect coronary artery disease [539] G. A. Beller, B. L. Zaret. Circulation101, 1465 (2000).. Imaging of 201Tl (with a half-life of 3 days), can be used for exercise perfusion tests of the myocardium (muscular tissue of the heart), which determine damage to the heart caused by a heart attack or by heart disease (Fig. IUPAC.81.2) [539] G. A. Beller, B. L. Zaret. Circulation101, 1465 (2000)..
Isotopes Used as a Source of Radioactive Isotope(s)
203Tl is used in the production of 201Tl via the 203Tl (p, 3 n) 201Pb reaction, which is followed by a subsequent electron capture decay reaction of 201Pb to finally yield 201Tl. 205Tl is used as an alternative target in the production of 201Tl.
Thallium chemistry is dominated by thallium(I), Tl⁺, and thallium(III), Tl³⁺, with Tl⁺ usually more stable in aqueous and many solid-state compounds. Representative thallium(I) compounds include thallium(I) sulfate, Tl₂SO₄, thallium(I) nitrate, TlNO₃, and thallium(I) chloride, TlCl. Thallium(III) oxide, Tl₂O₃, and thallium(III) chloride, TlCl₃, are stronger oxidizing or less stable species. Mixed thallium compounds occur in chalcogenide and halide materials used for optical and electronic studies.
See more information at the Thallium compound page.
Thallium and soluble thallium compounds are highly toxic by ingestion, inhalation, or skin exposure. Tl⁺ can interfere with potassium-dependent biological processes, and poisoning may have delayed neurological, gastrointestinal, and hair-loss symptoms. Dusts, fumes, and soluble salts are the main occupational hazards. Radioisotopes such as thallium-201 add external and internal radiation hazards that are isotope- and activity-dependent.
The element and its compounds are toxic and should be handled carefully. Contact of the metal with skin is dangerous, and when melting the metal adequate ventilation should be provided. Exposure to thallium (soluble compounds) - skin, as Tl, should not exceed 0.1 mg/m3 (8-hour time-weighted average - 40-hour work week). Thallium is suspected of carcinogenic potential for man.
Thallium occurs naturally at low concentrations, commonly associated with potassium minerals, sulfide ores, and some coals. Mining, smelting, cement production, and coal combustion can mobilize it locally. In the environment, Tl⁺ is relatively mobile in some waters and can be taken up by plants because of its chemical similarity to K⁺. It has no known beneficial biological role and can be a concern near contaminated industrial sites.
Thallium is not mined as a primary product. It is recovered mainly from flue dusts, residues, and by-product streams generated during refining of zinc, lead, copper, and other sulfide ores. Demand is small and specialized, with toxicity limiting broader applications and encouraging substitution. Supply can therefore depend more on base-metal processing practices, regulatory controls, and purification capacity than on dedicated thallium mining. Recycling is limited to particular industrial or research materials.
Thallium occurs in crooksite, lorandite, and hutchinsonite. It is also present in pyrites and is recovered from the roasting of this ore in connection with the production of sulfuric acid. It is also obtained from the smelting of lead and zinc ores. Extraction is somewhat complex and depends on the source of the thallium. Manganese nodules, found on the ocean floor, contain thallium.
Thallium is a heavy, rare element in cosmic terms. Its stable isotopes, ²⁰³Tl and ²⁰⁵Tl, are produced by neutron-capture processes in earlier generations of stars, with contributions from both slow and rapid neutron-capture pathways. It is not a major rock-forming element, but on planets it can concentrate in sulfide phases and volatile-rich geochemical reservoirs.
- Thallium was discovered by its bright green spectral line, which inspired its name from the Greek word for a green shoot
- Fresh thallium can be cut easily, but the exposed surface dulls quickly in air
- Tl⁺ is close enough in behavior to K⁺ to enter some biological potassium pathways
- Thallium(I) sulfate, Tl₂SO₄, was once used as a rodenticide before its toxicity led to severe restrictions
- Natural thallium consists chiefly of two stable isotopes, ²⁰³Tl and ²⁰⁵Tl
이미지
특성
물리적 특성
- 원자 반지름(경험값)
- 190 pm 모든 원소의 원자 반지름(경험값) 비교 →
- 공유 결합 반지름
- 145 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 196 pm 모든 원소의 반데르발스 반지름 비교 →
- 금속 반지름
- 144 pm 모든 원소의 금속 반지름 비교 →
- 밀도
- 1.18 × 104 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.0172 L/mol
- STP에서의 상
- 고체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- 303.85 °C 모든 원소의 녹는점 비교 →
- 끓는점
- 1472.85 °C 모든 원소의 끓는점 비교 →
- 열전도율
- 46.1 W/(m·K) 모든 원소의 열전도율 비교 →
- 비열
- 0.129 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 26.32 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 육방 조밀 충전 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 1.62 모든 원소의 전기 음성도(Pauling) 비교 →
- 전기 음성도(Allen)
- 1.789
- 전자 친화도
- 0.377 eV
- 제1 이온화 에너지
- 6.108287 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 20.42837 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 29.852103 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 51.140176 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 62.600215 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- −5, −2, −1, +1, +2, +3 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 3 모든 원소의 원자가 전자 비교 →
- 전자 배치
- [Xe] 6s2 4f14 5d10 6p1
열역학적 특성
- 융해열
- 0.04290822 eV 모든 원소의 융해열 비교 →
- 기화열
- 1.71011 eV 모든 원소의 기화열 비교 →
- 승화열
- 1.888376 eV
- 원자화열
- 1.888376 eV
- 원자화 엔탈피
- 1.888376 eV
핵 특성
- 양성자 수
- 81 모든 원소의 양성자 수 비교 →
- 중성자 수
- 124 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 43 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 2 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- Tl-205
- 발견 연도
- 1861
존재비
- 존재비(지각)
- 0.85 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 1.9 × 10−5 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 346 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 18, 32, 18, 3 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7440-28-0 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 2P°1/2
- InChI
- InChI=1S/Tl
- InChI 키
- BKVIYDNLLOSFOA-UHFFFAOYSA-N
전자 배치 측정값
Tl: 4f¹⁴ 5d¹⁰ 6s² 6p¹[Xe] 4f¹⁴ 5d¹⁰ 6s² 6p¹1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f¹⁴ 5d¹⁰ 6s² 6p¹원자 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 |
|---|---|---|---|
| 203 안정 | 202.9723446 ± 0.0000014 | 29.5200% | 안정 |
| 205 안정 | 204.9744278 ± 0.0000014 | 70.4800% | 안정 |
상 / 상태
이유: 녹는점(303.85 °C)보다 278.9 °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
원자 스펙트럼
전체 81개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 스펙트럼선 데이터 ?
| 이온 | 전하 | 총 스펙트럼선 수 | 전이 확률 | 준위 표기 |
|---|---|---|---|---|
| Tl I | 0 | 65 | 25 | 11 |
| Tl II | +1 | 82 | 3 | 7 |
| Tl III | +2 | 22 | 0 | 0 |
| Tl IV | +3 | 35 | 0 | 0 |
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| Tl I | 0 | 70 |
| Tl II | +1 | 82 |
| Tl III | +2 | 109 |
| Tl IV | +3 | 44 |
| Tl V | +4 | 2 |
| Tl VI | +5 | 2 |
| Tl VII | +6 | 2 |
| Tl VIII | +7 | 2 |
| Tl IX | +8 | 2 |
| Tl X | +9 | 2 |
이온 반지름
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +1 | 6 | 해당 없음 | 150 pm |
| +1 | 8 | 해당 없음 | 159 pm |
| +1 | 12 | 해당 없음 | 170 pm |
| +3 | 4 | 해당 없음 | 75 pm |
| +3 | 6 | 해당 없음 | 88.5 pm |
| +3 | 8 | 해당 없음 | 98 pm |
화합물
동위원소 (2)
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 203 안정 | 202.9723446 ± 0.0000014 | 29.5200% ± 0.0100% | 안정 | stable | |
| 205 안정 | 204.9744278 ± 0.0000014 | 70.4800% ± 0.0100% | 안정 | stable |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 144 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 142 pm
- 공유 결합 반지름(Pyykkö, 삼중 결합)
- 150 pm
- 공유 결합 반지름(Bragg)
- 190 pm
반데르발스 반지름
- Bondi
- 196 pm
- Batsanov
- 220 pm
- Alvarez
- 247 pm
- UFF
- 434.7 pm
- MM3
- 259 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 242 pm
- 금속 반지름(C12)
- 160 pm
번호 척도
- Mendeleev
- 85
- Pettifor
- 78
- Glawe
- 81
전기 음성도 척도
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 2
분극률 및 분산
- 쌍극자 분극률
- 50 a.u.
- 쌍극자 분극률(불확도)
- 2 a.u.
- C₆ (Gould–Bučko)
- 509 Ha·Bohr6
미데마 매개변수
- 미데마 몰 부피
- 17.23 cm3/mol
- 미데마 전자 밀도
- 1
상전이 및 동소체
| 녹는점 | 577.15 K |
| 끓는점 | 1746.15 K |
산화 상태 분류
심화 참고 데이터
차폐 상수 (15)
| n | 오비탈 | σ |
|---|---|---|
| 1 | s | 1.5591 |
| 2 | p | 4.5138 |
| 2 | s | 21.3158 |
| 3 | d | 13.4658 |
| 3 | p | 22.6335 |
| 3 | s | 23.5809 |
| 4 | d | 37.6112 |
| 4 | f | 38.1324 |
| 4 | p | 35.7832 |
| 4 | s | 34.9212 |
결정 반지름 상세 정보 (6)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 1 | VI | 164 | from r^3 vs V plots, | |
| 1 | VIII | 173 | from r^3 vs V plots, | |
| 1 | XII | 184 | from r^3 vs V plots, estimated, | |
| 3 | IV | 89 | ||
| 3 | VI | 102.5 | from r^3 vs V plots, | |
| 3 | VIII | 112 | calculated, |
동위원소 붕괴 방식 (69)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 176 | p | 100% |
| 176 | A | — |
| 176 | B+ | — |
| 177 | A | 73% |
| 177 | p | — |
| 178 | A | 62% |
| 178 | B+ | 38% |
| 178 | B+SF | 0.1% |
| 179 | A | 60% |
| 179 | B+ | — |
X선 산란 인자 (516)
| 에너지 (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 1.80392 |
| 10.1617 | — | 1.75555 |
| 10.3261 | — | 1.69589 |
| 10.4931 | — | 1.59546 |
| 10.6628 | — | 1.46625 |
| 10.8353 | — | 1.39341 |
| 11.0106 | — | 1.31349 |
| 11.1886 | — | 1.20783 |
| 11.3696 | — | 1.13261 |
| 11.5535 | — | 1.07387 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
8.5×10-1 milligrams per kilogram
참고 문헌 (1)
- [5] Thallium https://education.jlab.org/itselemental/ele081.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
1.9×10-5 milligrams per liter
참고 문헌 (1)
- [5] Thallium https://education.jlab.org/itselemental/ele081.html
Sources
Sources of this element.
Thallium occurs in crooksite, lorandite, and hutchinsonite. It is also present in pyrites and is recovered from the roasting of this ore in connection with the production of sulfuric acid. It is also obtained from the smelting of lead and zinc ores. Extraction is somewhat complex and depends on the source of the thallium. Manganese nodules, found on the ocean floor, contain thallium.
참고 문헌 (1)
- [6] Thallium https://periodic.lanl.gov/81.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 Thallium.
The element property data was retrieved from publications.