Jump to content

Krypton

Edit links
This is a good article. Click here for more information.
Page semi-protected
From Wikipedia, the free encyclopedia
(Redirected from Krypton (element))
This article is about the chemical element. For other uses, see Krypton (disambiguation).

Krypton, 36Kr
A krypton-filled discharge tube glowing white
Krypton
Pronunciation/ˈkrɪptɒn/ ​(KRIP-ton)
Appearancecolorless gas, exhibiting a whitish glow in an electric field
Standard atomic weight Ar°(Kr)
Krypton in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
Ar
↑
Kr
↓
Xe
bromine ← krypton → rubidium
Atomic number (Z)36
Groupgroup 18 (noble gases)
Periodperiod 4
Block  p-block
Electron configuration[Ar] 3d10 4s2 4p6
Electrons per shell2, 8, 18, 8
Physical properties
Phase at STPgas
Melting point115.78 K ​(−157.37 °C, ​−251.27 °F)
Boiling point119.93 K ​(−153.415 °C, ​−244.147 °F)
Density (at STP)3.749 g/L
when liquid (at b.p.)2.413 g/cm3[3]
Triple point115.775 K, ​73.53 kPa[4][5]
Critical point209.48 K, 5.525 MPa[5]
Heat of fusion1.64 kJ/mol
Heat of vaporization9.08 kJ/mol
Molar heat capacity20.95[6] J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 59 65 74 84 99 120
Atomic properties
Oxidation statescommon: +2
+1,?
ElectronegativityPauling scale: 3.00
Ionization energies
  • 1st: 1350.8 kJ/mol
  • 2nd: 2350.4 kJ/mol
  • 3rd: 3565 kJ/mol
Covalent radius116±4 pm
Van der Waals radius202 pm
Color lines in a spectral range
Spectral lines of krypton
Other properties
Natural occurrenceprimordial
Crystal structure ​face-centered cubic (fcc) (cF4)
Lattice constant
Face-centered cubic crystal structure for krypton
a = 583.57 pm (at triple point: 115.78 K)[7]
Thermal conductivity9.43×10−3  W/(m⋅K)
Magnetic orderingdiamagnetic[8]
Molar magnetic susceptibility−28.8×10−6 cm3/mol (298 K)[9]
Speed of sound(gas, 20 °C) 221 m·s−1
(liquid) 1120 m/s
CAS Number7439-90-9
History
Discovery and first isolationWilliam Ramsay and Morris Travers (1898)
Isotopes of krypton
Main isotopes[10] Decay
abun­dance half-life (t1/2) mode pro­duct
78Kr 0.360% 9.2×1021 y[11] εε 78Se
79Kr synth 35 h ε 79Br
β+ 79Br
γ –
80Kr 2.29% stable
81Kr trace 2.3×105 y ε 81Br
81mKr synth 13.10 s IT 81Kr
ε 81Br
82Kr 11.6% stable
83Kr 11.5% stable
84Kr 57.0% stable
85Kr trace 11 y β− 85Rb
86Kr 17.3% stable
 Category: Krypton
| references

Krypton (from Ancient Greek: κρυπτός, romanized: kryptos 'the hidden one') is a chemical element; it has symbol Kr and atomic number 36. It is a colorless, odorless noble gas that occurs in trace amounts in the atmosphere and is often used with other rare gases in fluorescent lamps. Krypton is chemically inert.

Krypton, like the other noble gases, is used in lighting and photography. Krypton light has many spectral lines, and krypton plasma is useful in bright, high-powered gas lasers (krypton ion and excimer lasers), each of which resonates and amplifies a single spectral line. Krypton fluoride also makes a useful laser medium. From 1960 to 1983, the official definition of the metre was based on the wavelength of one spectral line of krypton-86, because of the high power and relative ease of operation of krypton discharge tubes.

History

Sir William Ramsay, the discoverer of krypton

Krypton was discovered in Britain in 1898 by William Ramsay, a Scottish chemist, and Morris Travers, an English chemist, in residue left from evaporating nearly all components of liquid air. Neon was discovered by a similar procedure by the same workers just a few weeks later.[12] William Ramsay was awarded the 1904 Nobel Prize in Chemistry for discovery of a series of noble gases, including krypton.[13]

In 1960, the International Bureau of Weights and Measures defined the meter as 1,650,763.73 wavelengths of light emitted in the vacuum corresponding to the transition between the 2p10 and 5d5 levels in the isotope krypton-86.[14][15] This agreement replaced the 1889 international prototype meter, which was a metal bar located in Sèvres. This also made obsolete the 1927 definition of the ångström based on the red cadmium spectral line,[16] replacing it with 1 Å = 10−10 m. The krypton-86 definition lasted until the October 1983 conference, which redefined the meter as the distance that light travels in vacuum during 1/299,792,458 s.[17][18][19]

Characteristics

Krypton is characterized by several sharp emission lines (spectral signatures) the strongest being green and yellow.[20] Krypton is one of the products of uranium fission.[21] Solid krypton is white and has a face-centered cubic crystal structure, which is a common property of all noble gases (except helium, which has a hexagonal close-packed crystal structure).[22]

Isotopes

Main article: Isotopes of krypton

Naturally occurring krypton in Earth's atmosphere is composed of five stable isotopes, plus one isotope (78Kr) with such a long half-life (9.2×1021 years) that it can be considered stable. (This isotope has the third-longest known half-life among all isotopes for which decay has been observed; it undergoes double electron capture to 78Se).[11][23] In addition, about thirty unstable isotopes and isomers are known.[24] Traces of 81Kr, a cosmogenic nuclide produced by the cosmic ray irradiation of 80Kr, also occur in nature: this isotope is radioactive with a half-life of 230,000 years. Krypton is highly volatile and does not stay in solution in near-surface water, but 81Kr has been used for dating old (50,000–800,000 years) groundwater.[25]

85Kr is an inert radioactive noble gas with a half-life of 10.76 years. It is produced by the fission of uranium and plutonium, such as in nuclear bomb testing and nuclear reactors. 85Kr is released during the reprocessing of fuel rods from nuclear reactors. Concentrations at the North Pole are 30% higher than at the South Pole due to convective mixing.[26]

Chemistry

Like the other noble gases, krypton is chemically highly unreactive. The rather restricted chemistry of krypton in the +2 oxidation state parallels that of the neighboring element bromine in the +1 oxidation state; due to the scandide contraction it is difficult to oxidize the 4p elements to their group oxidation states. Until the 1960s no noble gas compounds had been synthesized.[27]

Following the first successful synthesis of xenon compounds in 1962, synthesis of krypton difluoride (KrF
2) was reported in 1963. In the same year, KrF
4 was reported by Grosse, et al.,[28] but was subsequently shown to be a mistaken identification.[29] Under extreme conditions, krypton reacts with fluorine to form KrF2 according to the following equation:

Krypton gas in a krypton fluoride laser absorbs energy from a source, causing the krypton to react with fluorine gas, producing the exciplex krypton fluoride, a temporary complex in an excited energy state:[30]

The complex can undergo spontaneous or stimulated emission, reducing its energy state to a metastable, but highly repulsive ground state. The ground state complex quickly dissociates into unbound atoms:

The result is an exciplex laser which radiates energy at 248 nm, near the ultraviolet portion of the spectrum, corresponding with the energy difference between the ground state and the excited state of the complex.[31]

Kr(H2)4 and H2 solids formed in a diamond anvil cell[32]
Structure of Kr(H2)4. Krypton octahedra (green) are surrounded by randomly oriented hydrogen molecules.[32]

Compounds with krypton bonded to atoms other than fluorine have also been discovered. There are also unverified reports of a barium salt of a krypton oxoacid.[33] ArKr+ and KrH+ polyatomic ions have been investigated and there is evidence for KrXe or KrXe+.[34]

The reaction of KrF
2 with B(OTeF
5)
3 produces an unstable compound, Kr(OTeF
5)
2, that contains a krypton-oxygen bond. A krypton-nitrogen bond is found in the cation [HC≡N–Kr–F]+
, produced by the reaction of KrF
2 with [HC≡NH]+
[AsF−
6] below −50 °C.[35][36] HKrCN and HKrC≡CH (krypton hydride-cyanide and hydrokryptoacetylene) were reported to be stable up to 40 K.[27]

Krypton hydride (Kr(H2)4) crystals can be grown at pressures above 5 GPa. They have a face-centered cubic structure where krypton octahedra are surrounded by randomly oriented hydrogen molecules.[32]

Natural occurrence

Earth has retained all of the noble gases that were present at its formation except helium. Krypton's concentration in the atmosphere is about 1 ppm. It can be extracted from liquid air by fractional distillation.[37] The amount of krypton in space is uncertain, because measurement is derived from meteoric activity and solar winds. The first measurements suggest an abundance of krypton in space.[38]

Applications

Krypton gas discharge tube

Krypton's multiple emission lines make ionized krypton gas discharges appear whitish, which in turn makes krypton-based bulbs useful in photography as a white light source. Krypton is used in some photographic flashes for high speed photography. Krypton gas is also combined with mercury to make luminous signs that glow with a bright greenish-blue light.[39]

Krypton is mixed with argon in energy efficient fluorescent lamps, reducing the power consumption, but also reducing the light output and raising the cost.[40] Krypton costs about 100 times as much as argon. Krypton (along with xenon) is also used to fill incandescent lamps to reduce filament evaporation and allow higher operating temperatures.[41]

Krypton's white discharge is sometimes used as an artistic effect in gas discharge "neon" tubes. Krypton produces much higher light power than neon in the red spectral line region, and for this reason, red lasers for high-power laser light-shows are often krypton lasers with mirrors that select the red spectral line for laser amplification and emission, rather than the more familiar helium-neon variety, which could not achieve the same multi-watt outputs.[42]

The krypton fluoride laser is important in nuclear fusion energy research in confinement experiments. The laser has high beam uniformity, short wavelength, and the spot size can be varied to track an imploding pellet.[43]

In experimental particle physics, liquid krypton is used to construct quasi-homogeneous electromagnetic calorimeters. A notable example is the calorimeter of the NA48 experiment at CERN containing about 27 tonnes of liquid krypton. This usage is rare, since liquid argon is less expensive. The advantage of krypton is a smaller Molière radius of 4.7 cm, which provides excellent spatial resolution with little overlapping. The other parameters relevant for calorimetry are: radiation length of X0=4.7 cm, and density of 2.4 g/cm3.

Krypton-83 has application in magnetic resonance imaging (MRI) for imaging airways. In particular, it enables the radiologist to distinguish between hydrophobic and hydrophilic surfaces containing an airway.[44]

Although xenon has potential for use in computed tomography (CT) to assess regional ventilation, its anesthetic properties limit its fraction in the breathing gas to 35%. A breathing mixture of 30% xenon and 30% krypton is comparable in effectiveness for CT to a 40% xenon fraction, while avoiding the unwanted effects of a high partial pressure of xenon gas.[45] The metastable isotope krypton-81m is used in nuclear medicine for lung ventilation/perfusion scans, where it is inhaled and imaged with a gamma camera.[46] Krypton-85 in the atmosphere has been used to detect clandestine nuclear fuel reprocessing facilities in North Korea[47] and Pakistan.[48] Those facilities were detected in the early 2000s and were believed to be producing weapons-grade plutonium. Krypton-85 is a medium lived fission product and thus escapes from spent fuel when the cladding is removed.[49]

Krypton is used occasionally as an insulating gas between window panes.[50] SpaceX Starlink uses krypton as a propellant for their electric propulsion system.[51]

Precautions

Krypton compared to other anaesthetic gases (minimum alveolar concentration is an inverse indicator of potency)

Krypton is considered to be a non-toxic asphyxiant.[52] Being lipophilic, krypton has a significant anaesthetic effect (although the mechanism of this phenomenon is still not fully clear,[53] there is good evidence that the two properties are mechanistically related), with narcotic potency seven times greater than air, and breathing an atmosphere of 50% krypton and 50% natural air (as might happen in the locality of a leak) causes narcosis in humans similar to breathing air at four times atmospheric pressure. This is comparable to scuba diving at a depth of 30 m (100 ft) and could affect anyone breathing it.

References

  1. ^ "Standard Atomic Weights: Krypton". CIAAW. 2001.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
  3. ^ Krypton. encyclopedia.airliquide.com
  4. ^ "Section 4, Properties of the Elements and Inorganic Compounds; Melting, boiling, triple, and critical temperatures of the elements". CRC Handbook of Chemistry and Physics (85th ed.). Boca Raton, Florida: CRC Press. 2005.
  5. ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, Florida: CRC Press. p. 4.121. ISBN 1-4398-5511-0.
  6. ^ Shuen-Chen Hwang, Robert D. Lein, Daniel A. Morgan (2005). "Noble Gases". Kirk Othmer Encyclopedia of Chemical Technology. Wiley. pp. 343–383. doi:10.1002/0471238961.0701190508230114.a01.
  7. ^ Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  8. ^ Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
  9. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  10. ^ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  11. ^ a b Patrignani, C.; et al. (Particle Data Group) (2016). "Review of Particle Physics". Chinese Physics C. 40 (10): 100001. Bibcode:2016ChPhC..40j0001P. doi:10.1088/1674-1137/40/10/100001. See p. 768
  12. ^ William Ramsay; Morris W. Travers (1898). "On a New Constituent of Atmospheric Air". Proceedings of the Royal Society of London. 63 (1): 405–408. doi:10.1098/rspl.1898.0051.
  13. ^ Davies, Alwyn G. (March 2012). "Sir William Ramsay and the Noble Gases". Science Progress. 95 (1): 23–49. doi:10.3184/003685012X13307058213813. ISSN 0036-8504. PMC 10365523. PMID 22574384. S2CID 12592582.
  14. ^ "The BIPM and the evolution of the definition of the metre". Bureau International des Poids et Mesures. 2014-07-26. Retrieved 2016-06-23.
  15. ^ Penzes, William B. (2009-01-08). "Time Line for the Definition of the Meter". National Institute of Standards and Technology. Archived from the original on 2016-08-12. Retrieved 2016-06-23.
  16. ^ Burdun, G. D. (1958). "On the new determination of the meter". Measurement Techniques. 1 (3): 259–264. Bibcode:1958MeasT...1..259B. doi:10.1007/BF00974680. S2CID 121450003.
  17. ^ Kimothi, Shri Krishna (2002). The uncertainty of measurements: physical and chemical metrology: impact and analysis. American Society for Quality. p. 122. ISBN 978-0-87389-535-4.
  18. ^ Gibbs, Philip (1997). "How is the speed of light measured?". Department of Mathematics, University of California. Archived from the original on 2015-08-21. Retrieved 2007-03-19.
  19. ^ Unit of length (meter), NIST
  20. ^ "Spectra of Gas Discharges". Archived from the original on 2011-04-02. Retrieved 2009-10-04.
  21. ^ "Krypton" (PDF). Argonne National Laboratory, EVS. 2005. Archived from the original (PDF) on 2009-09-29. Retrieved 2007-03-17.
  22. ^ Borden, Brett; Radin, Charles (1981-08-15). "The crystal structure of the noble gases". The Journal of Chemical Physics. 75 (4): 2012–2013. Bibcode:1981JChPh..75.2012B. doi:10.1063/1.442240. ISSN 0021-9606.
  23. ^ Gavrilyuk, Yu. M.; Gangapshev, A. M.; Kazalov, V. V.; Kuzminov, V. V.; Panasenko, S. I.; Ratkevich, S. S. (4 March 2013). "Indications of 2ν2K capture in 78Kr". Phys. Rev. C. 87 (3): 035501. Bibcode:2013PhRvC..87c5501G. doi:10.1103/PhysRevC.87.035501.
  24. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton, Florida: CRC Press. ISBN 0-8493-0486-5.
  25. ^ Thonnard, Norbert; MeKay, Larry D.; Labotka, Theodore C. (2001-02-05). "Development of Laser-Based Resonance Ionization Techniques for 81-Kr and 85-Kr Measurements in the Geosciences" (PDF). University of Tennessee, Institute for Rare Isotope Measurements. pp. 4–7. Retrieved 2007-03-20.
  26. ^ "Resources on Isotopes". U.S. Geological Survey. Archived from the original on 2001-09-24. Retrieved 2007-03-20.
  27. ^ a b Bartlett, Neil (2003). "The Noble Gases". Chemical & Engineering News. Retrieved 2006-07-02.
  28. ^ Grosse, A. V.; Kirshenbaum, A. D.; Streng, A. G.; Streng, L. V. (1963). "Krypton Tetrafluoride: Preparation and Some Properties". Science. 139 (3559): 1047–1048. Bibcode:1963Sci...139.1047G. doi:10.1126/science.139.3559.1047. PMID 17812982.
  29. ^ Prusakov, V. N.; Sokolov, V. B. (1971). "Krypton difluoride". Soviet Atomic Energy. 31 (3): 990–999. doi:10.1007/BF01375764. S2CID 189775335.
  30. ^ Johnson, Thomas H.; Hunter, Allen M. (1980-05-01). "Physics of the krypton fluoride laser". Journal of Applied Physics. 51 (5): 2406–2420. Bibcode:1980JAP....51.2406J. doi:10.1063/1.328010. ISSN 0021-8979.
  31. ^ Preston, S. G.; Sanpera, A.; Zepf, M.; Blyth, W. J.; Smith, C. G.; Wark, J. S.; Key, M. H.; Burnett, K.; Nakai, M.; Neely, D.; Offenberger, A. A. (1996-01-01). "High-order harmonics of 248.6-nm KrF laser from helium and neon ions". Physical Review A. 53 (1): R31–R34. Bibcode:1996PhRvA..53...31P. doi:10.1103/PhysRevA.53.R31. PMID 9912935.
  32. ^ a b c Kleppe, Annette K.; Amboage, Mónica; Jephcoat, Andrew P. (2014). "New high-pressure van der Waals compound Kr(H2)4 discovered in the krypton-hydrogen binary system". Scientific Reports. 4: 4989. Bibcode:2014NatSR...4.4989K. doi:10.1038/srep04989.
  33. ^ Streng, A.; Grosse, A. (1964). "Acid of Krypton and Its Barium Salt". Science. 143 (3603): 242–243. Bibcode:1964Sci...143..242S. doi:10.1126/science.143.3603.242. PMID 17753149. S2CID 11607538.
  34. ^ "Periodic Table of the Elements" (PDF). Los Alamos National Laboratory's Chemistry Division. pp. 100–101. Archived from the original (PDF) on November 25, 2006. Retrieved 2007-04-05.
  35. ^ Holloway, John H.; Hope, Eric G. (1998). Sykes, A. G. (ed.). Advances in Inorganic Chemistry. Academic Press. p. 57. ISBN 978-0-12-023646-6.
  36. ^ Lewars, Errol G. (2008). Modeling Marvels: Computational Anticipation of Novel Molecules. Springer. p. 68. ISBN 978-1-4020-6972-7.
  37. ^ "How Products are Made: Krypton". Retrieved 2006-07-02.
  38. ^ Cardelli, Jason A.; Meyer, David M. (1996). "The Abundance of Interstellar Krypton". The Astrophysical Journal Letters. 477 (1): L57–L60. Bibcode:1997ApJ...477L..57C. doi:10.1086/310513.
  39. ^ "Mercury in Lighting" (PDF). Cape Cod Cooperative Extension. Archived from the original (PDF) on 2007-09-29. Retrieved 2007-03-20.
  40. ^ Lighting: Full-Size Fluorescent Lamps. McGraw-Hill Companies, Inc. (2002)
  41. ^ Properties, Applications and Uses of the "Rare Gases" Neon, Krypton and Xenon. Uigi.com. Retrieved on 2015-11-30.
  42. ^ "Laser Devices, Laser Shows and Effect" (PDF). Archived from the original (PDF) on 2007-02-21. Retrieved 2007-04-05.
  43. ^ Sethian, J.; M. Friedman; M. Myers. "Krypton Fluoride Laser Development for Inertial Fusion Energy" (PDF). Plasma Physics Division, Naval Research Laboratory. pp. 1–8. Archived from the original (PDF) on 2011-09-29. Retrieved 2007-03-20.
  44. ^ Pavlovskaya, GE; Cleveland, ZI; Stupic, KF; Basaraba, RJ; et al. (2005). "Hyperpolarized krypton-83 as a contrast agent for magnetic resonance imaging". Proceedings of the National Academy of Sciences of the United States of America. 102 (51): 18275–9. Bibcode:2005PNAS..10218275P. doi:10.1073/pnas.0509419102. PMC 1317982. PMID 16344474.
  45. ^ Chon, D; Beck, KC; Simon, BA; Shikata, H; et al. (2007). "Effect of low-xenon and krypton supplementation on signal/noise of regional CT-based ventilation measurements". Journal of Applied Physiology. 102 (4): 1535–44. doi:10.1152/japplphysiol.01235.2005. PMID 17122371.
  46. ^ Bajc, M.; Neilly, J. B.; Miniati, M.; Schuemichen, C.; Meignan, M.; Jonson, B. (27 June 2009). "EANM guidelines for ventilation/perfusion scintigraphy". European Journal of Nuclear Medicine and Molecular Imaging. 36 (8): 1356–1370. doi:10.1007/s00259-009-1170-5. hdl:2158/774307. PMID 19562336.
  47. ^ Sanger, David E.; Shanker, Thom (2003-07-20). "N. Korea may be hiding new nuclear site". Oakland Tribune. Archived from the original on 2016-04-09. Retrieved 2015-05-01.
  48. ^ Bradley, Ed; Martin, David (2000-03-16). "U.S. Intelligence Find Evidence of Pakistan Producing Nuclear Weapons, CBS". CBS Evening News with Dan Rather. Archived from the original on 2016-10-18. Retrieved 2015-05-01.
  49. ^ Różański, K. (1979-01-01). "Krypton-85 in the atmosphere 1950–1977: a data review". Environment International. 2 (3): 139–143. Bibcode:1979EnInt...2..139R. doi:10.1016/0160-4120(79)90071-0. ISSN 0160-4120.
  50. ^ Ayre, James (2018-04-28). "Insulated Windows 101 — Double Glazing, Triple Glazing, Thermal Performance, & Potential Problems". cleantechnica.com. Retrieved 17 May 2018.
  51. ^ SpaceX (23 May 2019). "Starlink Mission". YouTube. Event occurs at 7:10. Archived from the original on 2021-11-03.
  52. ^ Properties of Krypton Archived 2009-02-19 at the Wayback Machine. Pt.chemicalstore.com. Retrieved on 2015-11-30.
  53. ^ Kennedy, R. R.; Stokes, J. W.; Downing, P. (February 1992). "Anaesthesia and the 'Inert' Gases with Special Reference to Xenon". Anaesthesia and Intensive Care. 20 (1): 66–70. doi:10.1177/0310057X9202000113. ISSN 0310-057X. PMID 1319119. S2CID 29886337.

Further reading

Retrieved from "https://en.wikipedia.org/w/index.php?title=Krypton&oldid=1254764703"