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Krypton

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This article is about the chemical element. For other uses, see Krypton (disambiguation).
Krypton,  36Kr
Krypton discharge tube.jpg
A krypton-filled discharge tube glowing white
Krypton Spectrum.jpg
Spectral lines of krypton
General properties
Name, symbol krypton, Kr
Pronunciation /ˈkrɪptɒn/
KRIP-ton
Appearance colorless gas, exhibiting a whitish glow in a high electric field
Krypton in the periodic table
Hydrogen (diatomic nonmetal)
Helium (noble gas)
Lithium (alkali metal)
Beryllium (alkaline earth metal)
Boron (metalloid)
Carbon (polyatomic nonmetal)
Nitrogen (diatomic nonmetal)
Oxygen (diatomic nonmetal)
Fluorine (diatomic nonmetal)
Neon (noble gas)
Sodium (alkali metal)
Magnesium (alkaline earth metal)
Aluminium (post-transition metal)
Silicon (metalloid)
Phosphorus (polyatomic nonmetal)
Sulfur (polyatomic nonmetal)
Chlorine (diatomic nonmetal)
Argon (noble gas)
Potassium (alkali metal)
Calcium (alkaline earth metal)
Scandium (transition metal)
Titanium (transition metal)
Vanadium (transition metal)
Chromium (transition metal)
Manganese (transition metal)
Iron (transition metal)
Cobalt (transition metal)
Nickel (transition metal)
Copper (transition metal)
Zinc (transition metal)
Gallium (post-transition metal)
Germanium (metalloid)
Arsenic (metalloid)
Selenium (polyatomic nonmetal)
Bromine (diatomic nonmetal)
Krypton (noble gas)
Rubidium (alkali metal)
Strontium (alkaline earth metal)
Yttrium (transition metal)
Zirconium (transition metal)
Niobium (transition metal)
Molybdenum (transition metal)
Technetium (transition metal)
Ruthenium (transition metal)
Rhodium (transition metal)
Palladium (transition metal)
Silver (transition metal)
Cadmium (transition metal)
Indium (post-transition metal)
Tin (post-transition metal)
Antimony (metalloid)
Tellurium (metalloid)
Iodine (diatomic nonmetal)
Xenon (noble gas)
Caesium (alkali metal)
Barium (alkaline earth metal)
Lanthanum (lanthanide)
Cerium (lanthanide)
Praseodymium (lanthanide)
Neodymium (lanthanide)
Promethium (lanthanide)
Samarium (lanthanide)
Europium (lanthanide)
Gadolinium (lanthanide)
Terbium (lanthanide)
Dysprosium (lanthanide)
Holmium (lanthanide)
Erbium (lanthanide)
Thulium (lanthanide)
Ytterbium (lanthanide)
Lutetium (lanthanide)
Hafnium (transition metal)
Tantalum (transition metal)
Tungsten (transition metal)
Rhenium (transition metal)
Osmium (transition metal)
Iridium (transition metal)
Platinum (transition metal)
Gold (transition metal)
Mercury (transition metal)
Thallium (post-transition metal)
Lead (post-transition metal)
Bismuth (post-transition metal)
Polonium (post-transition metal)
Astatine (metalloid)
Radon (noble gas)
Francium (alkali metal)
Radium (alkaline earth metal)
Actinium (actinide)
Thorium (actinide)
Protactinium (actinide)
Uranium (actinide)
Neptunium (actinide)
Plutonium (actinide)
Americium (actinide)
Curium (actinide)
Berkelium (actinide)
Californium (actinide)
Einsteinium (actinide)
Fermium (actinide)
Mendelevium (actinide)
Nobelium (actinide)
Lawrencium (actinide)
Rutherfordium (transition metal)
Dubnium (transition metal)
Seaborgium (transition metal)
Bohrium (transition metal)
Hassium (transition metal)
Meitnerium (unknown chemical properties)
Darmstadtium (unknown chemical properties)
Roentgenium (unknown chemical properties)
Copernicium (transition metal)
Ununtrium (unknown chemical properties)
Flerovium (post-transition metal)
Ununpentium (unknown chemical properties)
Livermorium (unknown chemical properties)
Ununseptium (unknown chemical properties)
Ununoctium (unknown chemical properties)
Ar

Kr

Xe
brominekryptonrubidium
Atomic number (Z) 36
Group, block group 18 (noble gases), p-block
Period period 4
Element category   noble gas
Standard atomic weight (±) (Ar) 83.798(2)[1]
Electron configuration [Ar] 3d10 4s2 4p6
per shell
2, 8, 18, 8
Physical properties
Phase gas
Melting point 115.78 K ​(−157.37 °C, ​−251.27 °F)
Boiling point 119.93 K ​(−153.415 °C, ​−244.147 °F)
Density at stp (0 °C and 101.325 kPa) 3.749 g/L
when liquid, at b.p. 2.413 g/cm3[2]
Triple point 115.775 K, ​73.53 kPa[3][4]
Critical point 209.48 K, 5.525 MPa[4]
Heat of fusion 1.64 kJ/mol
Heat of vaporization 9.08 kJ/mol
Molar heat capacity 20.95[5] 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 states 2, 1, 0 ​(rarely more than 0; unknown oxide)
Electronegativity Pauling scale: 3.00
Ionization energies 1st: 1350.8 kJ/mol
2nd: 2350.4 kJ/mol
3rd: 3565 kJ/mol
Covalent radius 116±4 pm
Van der Waals radius 202 pm
Miscellanea
Crystal structure face-centered cubic (fcc)
Face-centered cubic crystal structure for krypton
Speed of sound (gas, 23 °C) 220 m·s−1
(liquid) 1120 m/s
Thermal conductivity 9.43×10−3  W/(m·K)
Magnetic ordering diamagnetic[6]
CAS Number 7439-90-9
History
Discovery and first isolation William Ramsay and Morris Travers (1898)
Most stable isotopes of krypton
iso NA half-life DM DE (MeV) DP
78Kr 0.36% >1.1×1020 y (β+β+) 2.846 78Se
79Kr syn 35.04 h ε 79Br
β+ 0.604 79Br
γ 0.26, 0.39, 0.60
80Kr 2.29% 80Kr is stable with 44 neutrons
81Kr trace 2.29×105 y ε 81Br
γ 0.281
82Kr 11.59% 82Kr is stable with 46 neutrons
83Kr 11.50% 83Kr is stable with 47 neutrons
84Kr 56.99% 84Kr is stable with 48 neutrons
85Kr syn 10.756 y β 0.687 85Rb
86Kr 17.28% (ββ) 1.2556 86Sr
Decay modes in parentheses are predicted, but have not yet been observed
| references

Krypton (from Greek: κρυπτός kryptos "the hidden one") is a chemical element with symbol Kr and atomic number 36. It is a member of group 18 (noble gases) elements. A colorless, odorless, tasteless noble gas, krypton occurs in trace amounts in the atmosphere and is often used with other rare gases in fluorescent lamps. With rare exceptions, 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. From 1960 to 1983, the official length of a meter was defined by the 605 nm wavelength of the orange 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 Sir 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.[7] William Ramsay was awarded the 1904 Nobel Prize in Chemistry for discovery of a series of noble gases, including krypton.

In 1960, the International Conference on Weights and Measures defined the meter as 1,650,763.73 wavelengths of light emitted by the krypton-86 isotope.[8][9] This agreement replaced the 1889 international prototype meter located in Paris, which was a metal bar made of a platinum-iridium alloy (one of a series of standard meter bars, originally constructed to be one ten-millionth of a quadrant of the Earth's polar circumference). This also obsoleted the 1927 definition of the ångström based on the red cadmium spectral line,[10] 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 a vacuum during 1/299,792,458 s.[11][12][13]

Characteristics

Krypton is characterized by several sharp emission lines (spectral signatures) the strongest being green and yellow.[14] Krypton is one of the products of uranium fission.[15] Solid krypton is white and has a face-centered cubic crystal structure, which is a common property of all noble gases (except helium, with a hexagonal close-packed crystal structure).

Isotopes

Main article: Isotopes of krypton

Naturally occurring krypton in Earth's atmosphere is composed of six stable isotopes. In addition, about thirty unstable isotopes and isomers are known.[16] 81Kr, the product of atmospheric reactions, is produced with the other naturally occurring isotopes of krypton. Being radioactive, it has 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.[17]

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.[18]

Chemistry

Kr(H2)4 and H2 solids formed in a diamond anvil cell.[19]
Structure of Kr(H2)4. Krypton octahedra (green) are surrounded by randomly oriented hydrogen molecules.[19]

Like the other noble gases, krypton is highly chemically unreactive. In fact, before the 1960s, no noble gas compounds had been synthesized.[20]

However, 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.,[21] but was subsequently shown to be a mistaken identification.[22] Under extreme conditions, krypton reacts with fluorine to form KrF2 according to the following equation:

Kr + F2 → KrF2

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.[23] ArKr+ and KrH+ polyatomic ions have been investigated and there is evidence for KrXe or KrXe+.[24]

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.[25][26] HKrCN and HKrC≡CH (krypton hydride-cyanide and hydrokryptoacetylene) were reported to be stable up to 40 K.[20]

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.[19]

Recently, Zaleski-Ejgierd et al. predicted that a whole new class of krypton compounds – krypton oxides – should stabilize thermodynamically at elevated pressures. In particular, krypton monoxide (KrO) should form spontaneously from a mixture of the pure elements at approximately 285 GPa (2.85 million atmospheres). In it krypton atoms are expected to form strong covalent bonds with the oxygen atoms.[27]

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.[28] 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.[29]

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 brilliant white light source. Krypton is used in some photographic flashes for high speed photography. Krypton gas is also combined with other gases to make luminous signs that glow with a bright greenish-yellow light.[30]

Krypton is mixed with argon in energy efficient fluorescent lamps, reducing the power consumption, but also reducing the light output and raising the cost.[31] 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.[32] A brighter light results with more blue color than conventional incandescent lamps.

Krypton's white discharge is often used to good effect in colored gas discharge tubes, which are simply painted or stained to create the desired color (for example, "neon" type multi-colored advertising signs are often entirely krypton-based). Krypton is 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.[33]

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.[34]

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.

The sealed spark gap assemblies in ignition exciters in some older jet engines contain a small amount of krypton-85 to produce consistent ionization levels and uniform operation.

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.[35]

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.[36]

Krypton-85 in the atmosphere has been used to detect clandestine nuclear fuel reprocessing facilities in North Korea[37] and Pakistan.[38] Those facilities were detected in the early 2000s and were believed to be producing weapons-grade plutonium.

Precautions

Krypton is considered to be a non-toxic asphyxiant.[39] Krypton has a 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) (see nitrogen narcosis) and could affect anyone breathing it. At the same time, that mixture would contain only 10% oxygen (rather than the normal 20%) and hypoxia would be a greater concern.

See also

References

  1. ^ Standard Atomic Weights 2013. Commission on Isotopic Abundances and Atomic Weights
  2. ^ Krypton. encyclopedia.airliquide.com
  3. ^ "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. 
  4. ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.121. ISBN 1439855110. 
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  12. ^ Gibbs, Philip (1997). "How is the speed of light measured?". Department of Mathematics, University of California. Retrieved 2007-03-19. 
  13. ^ Unit of length (meter), NIST
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  16. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5. 
  17. ^ Thonnard, Norbert; Larry D. MeKay; Theodore C. Labotka (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. 
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  35. ^ 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 U.S.A. 102 (51): 18275–9. Bibcode:2005PNAS..10218275P. doi:10.1073/pnas.0509419102. PMC 1317982free to read. PMID 16344474. 
  36. ^ 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. 
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Further reading

External links