Xenon (Xe)
noble-gasGas
표준 원자량
131.293 u전자 배치
[Kr] 5s2 4d10 5p6녹는점
-111.79 °C끓는점
-108.1 °C밀도
5.887 kg/m³산화 상태
0, +2, +4, +6, +8전기 음성도(Pauling)
2.6제1 이온화 에너지
12.129844 eV발견 연도
1898원자 반지름
해당 없음상세 정보
Xenon is a heavy noble gas with a closed-shell electron configuration and very low chemical reactivity under ordinary conditions. It occurs in the atmosphere only as a trace constituent and is obtained from air-separation processes. Its high atomic mass, ease of ionization, and strong ultraviolet emission make it technologically useful, while its ability to form stable compounds with highly electronegative elements distinguishes it from the lighter noble gases.
Xenon is used in super bright lamps used for deep sea observation.
The name derives from the Greek xenos for "the stranger". It was discovered by the Scottish chemist William Ramsay and the English chemist Morris William Travers in 1898 in a liquefied air sample.
Xenon was discovered by Sir William Ramsay, a Scottish chemist, and Morris M. Travers, an English chemist, on July 12, 1898, shortly after their discovery of the elements krypton and neon. Like krypton and neon, xenon was discovered through the study of liquefied air. The earth's atmosphere is about 0.0000087% xenon.
From the Greek word xenon, stranger. Discovered in 1898 by Ramsay and Travers in residue left after evaporating liquid air. Xenon is a member of the so-called noble or "inert" gases. It is present in the atmosphere to the extent of about one part in twenty million. Xenon is present in the Martian atmosphere to the extent of 0.08 ppm. the element is found in the gases evolved from certain mineral springs, and is commercially obtained by extraction from liquid air.
Pure xenon is a colorless, odorless, monatomic gas at ordinary temperature and pressure. When cooled it forms a colorless liquid and a crystalline solid. In an electrical discharge it emits a blue to lavender glow, which is an excitation effect rather than the color of the gas itself.
Xenon is used in high-intensity discharge lamps, photographic flash lamps, stroboscopes, and some specialized projection and automotive lighting systems, although many lighting uses have declined with solid-state alternatives. Xenon is an efficient propellant for ion thrusters in spacecraft because it is dense, inert, and readily ionized. It is also used in radiation detectors, excimer and exciplex laser mixtures, plasma displays of historical importance, and as an inhaled anesthetic where cost and equipment allow.
Xenon produces a brilliant white flash of light when it is excited electrically and is widely used in strobe lights. The light emitted from xenon lamps is also used to kill bacteria and to power ruby lasers.
Due to its high atomic weight, xenon ions were used as a fuel in an experimental ion engine aboard the space probe Deep Space 1.
Once thought to be completely inert, xenon will form compounds, usually with fluorine, oxygen and platinum. XePtF6, XeF2, XeF4, XeF6 and XeO4 are some of the xenon compounds that have been formed.
The gas is used in making electron tubes, stoboscopic lamps, bactericidal lamps, and lamps used to excite ruby lasers that generate coherent light. Xenon is used in the nuclear energy field in bubble chambers, probes, and other applications where a high molecular weight is of value. The perxenates are used in analytical chemistry as oxidizing agents. 133Xe and 135Xe are produced by neutron irradiation in air cooled nuclear reactors. 133Xe has useful applications as a radioisotope. The element is available in sealed glass containers of gas at standard pressure. Xenon is not toxic, but its compounds are highly toxic because of their strong oxidizing characteristics.
Isotopes in Forensic Science and Anthropology
Radiogenic xenon isotopes are produced by nuclear reactions in atomic bombs and nuclear reactors. For example, 131Xe, 133Xe, and 135Xe are some of the fission products of 235U and 239Pu, and finding these isotopes would be evidence of a nuclear bomb reaction. Measurements of xenon isotopes (e.g. in the atmosphere or the subsurface) have been used to identify contamination from these sources, for example, to detect faults in nuclear reactors or to monitor compliance with nuclear test bans (Fig. IUPAC.54.1) [396] P. R. J. Saey, C. Schlosser, P. Achim, M. Auer, A. Axelsson, A. Becker, X. Blanchard, G. Brachet, L. Cella, L.-E. De Geer, M. B. Kalinowski, G. Le Petit, J. Peterson, V. Popov, Y. Popov, A. Ringbom, H. Sartorius, T. Taffary, M. Zähringer. Pure Appl. Geophy.167, 499 (2010)..
Isotopes in Geochronology
The stable isotopes of xenon hold many clues about the formation of the elements, solar-system history, and Earth processes [29] M. Ozima, F. A. Podosek. Noble Gas Geochemistry: 2nd Edition, p. 286, Cambridge University Press, Cambridge, UK (2002)., [101] Noble Gases in Geochemistry and Cosmochemistry: Reviews in Mineralogy and Geochemistry, D. Porcelli, C. J. Ballentine, and R. Wieler (Eds.), p. 844, Mineralogical Society of America and the Geochemical Society, Washington, DC (2002).. For example, 129Xe has been used as a detector of “extinct” radionuclides. Some 129Xe is radiogenic as a result of being produced by the radioactive decay of 129I (half-life of 1.7×107 years). Because the half-life of 129I is much smaller than the age of the Earth, primordial 129I (i.e. that which was present at the beginning of Earth’s history) is essentially gone after it decayed to 129Xe over geologic time. This means that radiogenic 129Xe could be a marker of the former existence of the “extinct” isotope 129I. Because primordial 129I was produced largely in supernovae, detection of radiogenic 129Xe in meteorites and terrestrial samples also implies that the time elapsed between 129I supernova nucleosynthesis and planetary condensation was short compared to the subsequent history of the Solar System. The many isotopes and reaction mechanisms of xenon have contributed numerous insights into Earth processes through the study of “xenology” (xenon isotopic variations used as geodynamic tracers to study the dynamics of the Earth) [397] J. H. Reynolds. J. Geophys. Res.68, 2939 (1963)..
Isotopes in Medicine
Xenon isotopes are used in numerous ways to investigate the movement of inhaled gases in lungs and other parts of the body. If radioactive isotopes of xenon [ 127Xe (with a half-life of 0.1 year), 133Xe, and hyperpolarized (having non-equilibrium alignment of nuclear spins, suitable for magnetic resonance) 129Xe] are inhaled, they can be tracked throughout the body by externally monitoring their decay products using magnetic resonance microscopy [high resolution magnetic resonance imaging (MRI) at microscopic (nanometer) levels] (Fig. IUPAC.54.2). This imaging technique is used to assess how well oxygen is taken up and transported by the blood [398] B. Driehuys, L. W. Hedlund. Toxicol. Pathol.35, 49 (2007)..
Isotopes Used as a Source of Radioactive Isotope(s)
124Xe is used in the production of radioisotopes 123I and 125I (with half-lives of 0.55 day and 59 days, respectively) via the reactions 124Xe (n, n p) 123I and 124Xe (n, γ) 125I, respectively, which are used in diagnostic procedures and cancer treatment, respectively [398] B. Driehuys, L. W. Hedlund. Toxicol. Pathol.35, 49 (2007)..
Xenon chemistry is dominated by positive oxidation states stabilized by fluorine and oxygen. Xenon difluoride (XeF₂), xenon tetrafluoride (XeF₄), and xenon hexafluoride (XeF₆) are well-established fluorides and strong fluorinating or oxidizing reagents. Oxygen-containing species include xenon trioxide (XeO₃), xenon tetroxide (XeO₄), and perxenate salts containing the XeO₆⁴⁻ ion. Xenon also forms coordination compounds and adducts with very strong Lewis acids, but no ordinary aqueous cation chemistry is known.
See more information at the Xenon compound page.
Xenon is chemically inert and not toxic by ordinary chemical mechanisms, but it can displace oxygen and cause asphyxiation in confined or poorly ventilated spaces. Compressed xenon cylinders present pressure hazards. Liquid xenon is cryogenic and can cause cold burns or material embrittlement. Radioactive xenon isotopes, such as ¹³³Xe, require isotope-specific radiation controls; stable xenon does not share those radiological hazards.
Atmospheric xenon is chemically persistent and present at very low concentration. It is released and recaptured mainly through physical processes rather than chemical cycling. Natural radioactive xenon isotopes are short-lived products of nuclear fission and can serve as tracers of underground nuclear activity or reactor releases. Stable xenon has no known biological role and little direct ecological reactivity.
Commercial xenon is recovered as a minor by-product of large-scale cryogenic air separation, usually from the same rare-gas streams that can also yield krypton. Its supply is constrained by the amount of air processed for oxygen and nitrogen rather than by xenon demand alone. Purification is energy- and capital-intensive because atmospheric concentration is very low. Demand is led by space propulsion, specialized lighting, electronics, detectors, and medical uses. Recycling is practical in some closed systems, especially where high purity gas is valuable.
Obtain from the small quantities in liquid air.
Xenon is produced mainly by neutron-capture processes in evolved stars and by fission of heavy nuclei. It is less abundant cosmically than lighter noble gases but is important in isotope studies. Xenon isotope ratios in meteorites, planetary atmospheres, and lunar samples record nucleosynthetic components, radiogenic additions, and atmospheric loss processes. Its isotopic anomalies are a notable tool in planetary science.
- Xenon was the first noble gas shown to form a stable neutral compound under ordinary laboratory isolation conditions.
- Natural xenon contains nine stable isotopes, an unusually large number for one element.
- Liquid xenon is widely used as a scintillation and ionization medium in rare-event physics detectors.
- The name xenon comes from a Greek word meaning stranger or foreigner.
- Xenon excimer systems can generate intense ultraviolet light without a conventional hot filament.
- Atmospheric xenon is anomalously depleted relative to krypton when compared with some simple planetary models.
이미지
특성
물리적 특성
- 공유 결합 반지름
- 140 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 216 pm 모든 원소의 반데르발스 반지름 비교 →
- 밀도
- 5.887 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.0429 L/mol
- STP에서의 상
- 기체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- -111.79 °C 모든 원소의 녹는점 비교 →
- 끓는점
- -108.1 °C 모든 원소의 끓는점 비교 →
- 열전도율
- 0.006 W/(m·K) 모든 원소의 열전도율 비교 →
- 비열
- 0.158 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 20.786 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 면심 입방 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 2.6 모든 원소의 전기 음성도(Pauling) 비교 →
- 전기 음성도(Allen)
- 2.582
- 전자 친화도
- -0.8 eV (음수 값 — 추가 전자를 결합하지 않을 것으로 예측됨)
- 제1 이온화 에너지
- 12.129844 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 20.975072 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 31.050107 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 42.200145 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 54.100186 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- 0, +2, +4, +6, +8 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 8 모든 원소의 원자가 전자 비교 →
- 전자 배치
- [Kr] 5s2 4d10 5p6
열역학적 특성
- 삼중점(온도)
- -111.75 °C
- 삼중점(압력)
- 8.16e+4 Pa
- 임계점(온도)
- 16.583 °C
- 임계점(압력)
- 5.842e+6 Pa
- 융해열
- 0.02352697 eV 모든 원소의 융해열 비교 →
- 기화열
- 0.13100482 eV 모든 원소의 기화열 비교 →
- 원자화열
- 0 eV
핵 특성
- 양성자 수
- 54 모든 원소의 양성자 수 비교 →
- 중성자 수
- 78 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 43 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 6 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- Xe-132
- 발견 연도
- 1898
존재비
- 존재비(지각)
- 3e-5 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 5 × 10−5 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 620 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 18, 18, 8 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7440-63-3 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 1S0
- InChI
- InChI=1S/Xe
- InChI 키
- FHNFHKCVQCLJFQ-UHFFFAOYSA-N
전자 배치 측정값
Xe: 4d¹⁰ 5s² 5p⁶[Kr] 4d¹⁰ 5s² 5p⁶1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶원자 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 |
|---|---|---|---|
| 126 안정 | 125.9042983 ± 0.0000038 | 0.0890% | 안정 |
| 128 안정 | 127.903531 ± 0.0000011 | 1.9102% | 안정 |
| 129 안정 | 128.9047808611 ± 0.000000006 | 26.4006% | 안정 |
| 130 안정 | 129.903509349 ± 0.00000001 | 4.0710% | 안정 |
| 131 안정 | 130.90508406 ± 0.00000024 | 21.2324% | 안정 |
| 132 안정 | 131.9041550856 ± 0.0000000056 | 26.9086% | 안정 |
상 / 상태
이유: 끓는점(-108.1 °C)보다 133.1 °C 높음
개략도이며 실제 비율과 다름
상전이점
전이 에너지
녹는점에서 1 mol을 녹이는 데 필요한 에너지
끓는점에서 1 mol을 기화시키는 데 필요한 에너지
밀도
표준 조건에서
현재 온도 T에서 이상 기체 법칙으로 추정
심화
원자 스펙트럼
전체 54개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 스펙트럼선 데이터 ?
| 이온 | 전하 | 총 스펙트럼선 수 | 전이 확률 | 준위 표기 |
|---|---|---|---|---|
| Xe I | 0 | 1143 | 187 | 1143 |
| Xe II | +1 | 1115 | 22 | 1115 |
| Xe III | +2 | 1512 | 0 | 1512 |
| Xe IV | +3 | 769 | 0 | 769 |
| Xe V | +4 | 273 | 0 | 273 |
| Xe VI | +5 | 126 | 0 | 126 |
| Xe VII | +6 | 131 | 0 | 131 |
| Xe VIII | +7 | 135 | 0 | 135 |
| Xe IX | +8 | 144 | 0 | 144 |
| Xe X | +9 | 83 | 0 | 83 |
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| Xe I | 0 | 445 |
| Xe II | +1 | 164 |
| Xe III | +2 | 158 |
| Xe IV | +3 | 95 |
| Xe V | +4 | 55 |
| Xe VI | +5 | 73 |
| Xe VII | +6 | 73 |
| Xe VIII | +7 | 83 |
| Xe IX | +8 | 61 |
| Xe X | +9 | 63 |
이온 반지름
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +8 | 4 | 해당 없음 | 40 pm |
| +8 | 6 | 해당 없음 | 48 pm |
화합물
동위원소 (6)
Natural xenon is composed of nine stable isotopes. In addition to these, 20 unstable isotopes have been characterized. Before 1962, it had generally been assumed that xenon and other noble gases were unable to form compounds. Evidence has been mounting in the past few years that xenon, as well as other members of zero valance elements, do form compounds. Among the "compounds" of xenon now reported are sodium perxenate, xenon deuterate, xenon hydrate, difluoride, tetrafluoride, and hexafluoride. Xenon trioxide, which is highly explosive, has been prepared. More than 80 xenon compounds have been made with xenon chemically bonded to fluorine and oxygen. Some xenon compounds are colored. Metallic xenon has been produced, using several hundred kilobars of pressure. Xenon in a vacuum tube produces a beautiful blue glow when excited by an electrical discharge.
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 126 안정 | 125.9042983 ± 0.0000038 | 0.0890% ± 0.0002% | 안정 | stable | |
| 128 안정 | 127.903531 ± 0.0000011 | 1.9102% ± 0.0008% | 안정 | stable | |
| 129 안정 | 128.9047808611 ± 0.000000006 | 26.4006% ± 0.0082% | 안정 | stable | |
| 130 안정 | 129.903509349 ± 0.00000001 | 4.0710% ± 0.0013% | 안정 | stable | |
| 131 안정 | 130.90508406 ± 0.00000024 | 21.2324% ± 0.0030% | 안정 | stable | |
| 132 안정 | 131.9041550856 ± 0.0000000056 | 26.9086% ± 0.0033% | 안정 | stable |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 131 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 135 pm
- 공유 결합 반지름(Pyykkö, 삼중 결합)
- 122 pm
반데르발스 반지름
- Bondi
- 216 pm
- Alvarez
- 228 pm
- UFF
- 440.4 pm
- MM3
- 228 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 232 pm
번호 척도
- Mendeleev
- 116
- Pettifor
- 5
- Glawe
- 5
전기 음성도 척도
- Ghosh
- 0
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
분극률 및 분산
- 쌍극자 분극률
- 27.32 a.u.
- 쌍극자 분극률(불확도)
- 0.2 a.u.
- C₆ (Gould–Bučko)
- 302 Ha·Bohr6
화학 친화력
- 양성자 친화도
- 499.6 kJ/mol
- 기체상 염기성
- 478.1 kJ/mol
비활성 기체 특성
| O₂ | forms oxides indirectly (XeO3, XeO4) |
| HALOGENS | XeF2, XeF4, XeF6 |
| OXIDES_TYPE | acidic |
상전이 및 동소체
| 녹는점 | 161.4 K |
| 끓는점 | 165.05 K |
| 임계점(온도) | 289.73 K |
| 임계점(압력) | 5.84 MPa |
| 삼중점(온도) | 161.4 K |
| 삼중점(압력) | 81.77 kPa |
산화 상태 분류
심화 참고 데이터
차폐 상수 (11)
| n | 오비탈 | σ |
|---|---|---|
| 1 | s | 1.0785 |
| 2 | p | 4.1654 |
| 2 | s | 14.197 |
| 3 | d | 14.0532 |
| 3 | p | 18.3324 |
| 3 | s | 18.4236 |
| 4 | d | 32.1068 |
| 4 | p | 29.0428 |
| 4 | s | 27.8272 |
| 5 | p | 41.5755 |
결정 반지름 상세 정보 (2)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 8 | IV | 54 | ||
| 8 | VI | 62 |
동위원소 붕괴 방식 (68)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 108 | A | 100% |
| 109 | A | 100% |
| 109 | B+ | — |
| 109 | B+p | — |
| 110 | A | 64% |
| 110 | B+ | 36% |
| 110 | B+p | — |
| 111 | B+ | 89.6% |
| 111 | A | 10.4% |
| 111 | B+p | — |
X선 산란 인자 (509)
| 에너지 (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0 |
| 10.1617 | — | 0 |
| 10.3261 | — | 0 |
| 10.4931 | — | 0 |
| 10.6628 | — | 0 |
| 10.8353 | — | 0 |
| 11.0106 | — | 0 |
| 11.1886 | — | 0 |
| 11.3696 | — | 0 |
| 11.5535 | — | 0 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
3×10-5 milligrams per kilogram
참고 문헌 (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
5×10-5 milligrams per liter
참고 문헌 (1)
Isotopes in Forensic Science and Anthropology
Information on the use of this element's isotopes in forensic science and anthropology.
Radiogenic xenon isotopes are produced by nuclear reactions in atomic bombs and nuclear reactors. For example, 131Xe, 133Xe, and 135Xe are some of the fission products of 235U and 239Pu, and finding these isotopes would be evidence of a nuclear bomb reaction. Measurements of xenon isotopes (e.g. in the atmosphere or the subsurface) have been used to identify contamination from these sources, for example, to detect faults in nuclear reactors or to monitor compliance with nuclear test bans (Fig. IUPAC.54.1) [396] P. R. J. Saey, C. Schlosser, P. Achim, M. Auer, A. Axelsson, A. Becker, X. Blanchard, G. Brachet, L. Cella, L.-E. De Geer, M. B. Kalinowski, G. Le Petit, J. Peterson, V. Popov, Y. Popov, A. Ringbom, H. Sartorius, T. Taffary, M. Zähringer. Pure Appl. Geophy.167, 499 (2010)..
참고 문헌 (2)
- [396] P. R. J. Saey, C. Schlosser, P. Achim, M. Auer, A. Axelsson, A. Becker, X. Blanchard, G. Brachet, L. Cella, L.-E. De Geer, M. B. Kalinowski, G. Le Petit, J. Peterson, V. Popov, Y. Popov, A. Ringbom, H. Sartorius, T. Taffary, M. Zähringer. Pure Appl. Geophy.167, 499 (2010).
- [4] IUPAC Periodic Table of the Elements and Isotopes (IPTEI) https://doi.org/10.1515/pac-2015-0703
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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 Xenon.
The element property data was retrieved from publications.