Krypton

Krypton
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For other uses, see Krypton (disambiguation).
36 bromine ← krypton → rubidium
Ar
↑
Kr
↓
Xe
Periodic Table - Extended Periodic Table


General
Name, Symbol, Number krypton, Kr, 36
Chemical series noble gases
Group, Period, Block 18, 4, p
Appearance colorless

Standard atomic weight 83.798(2)  g·mol−1
Electron configuration [Ar] 3d10 4s2 4p6
Electrons per shell 2, 8, 18, 8
Physical properties
Phase gas
Density (0 °C, 101.325 kPa)
3.749 g/L
Melting point 115.79 K
(-157.36 °C, -251.25 °F)
Boiling point 119.93 K
(-153.22 °C, -244.12 °F)
Triple point 115.775 K, 73.2 kPa[1]
Critical point 209.41 K, 5.50 MPa
Heat of fusion 1.64  kJ·mol−1
Heat of vaporization 9.08  kJ·mol−1
Heat capacity (25 °C) 20.786  J·mol−1·K−1
Vapor pressure P(Pa) 1 10 100 1 k 10 k 100 k
at T(K) 59 65 74 84 99 120

Atomic properties
Crystal structure cubic face centered
Oxidation states 2
Electronegativity 3.00 (scale Pauling)
Ionization energies
(more) 1st:  1350.8  kJ·mol−1
2nd:  2350.4  kJ·mol−1
3rd:  3565  kJ·mol−1
Atomic radius (calc.) 88  pm
Covalent radius 110  pm
Van der Waals radius 202 pm
Miscellaneous
Magnetic ordering nonmagnetic
Thermal conductivity (300 K) 9.43 m W·m−1·K−1
Speed of sound (gas, 23 °C) 220 m/s
Speed of sound (liquid) 1120 m/s
CAS registry number 7439-90-9
Selected isotopes
Main article: Isotopes of krypton iso NA half-life DM DE (MeV) DP
78Kr 0.35% 2.3×1020 y ε ε - 78Se
79Kr syn 35.04 h ε - 79Br
β+ 0.604 79Br
γ 0.26, 0.39, 0.60 -
80Kr 2.25% Kr is stable with 44 neutrons
81Kr syn 2.29×105 y ε - 81Br
γ 0.281 -
82Kr 11.6% Kr is stable with 46 neutrons
83Kr 11.5% Kr is stable with 47 neutrons
84Kr 57% Kr is stable with 48 neutrons
85Kr syn 10.756 y β- 0.687 85Rb
86Kr 17.3% Kr is stable with 50 neutrons

References
Krypton (IPA: /ˈkrɪptən/ or /ˈkrɪptan/) is a chemical element with the symbol Kr and atomic number 36. A colorless, odorless, tasteless noble gas, krypton occurs in trace amounts in the atmosphere, is isolated by fractionally distilling liquified air, and is often used with other rare gases in fluorescent lamps. Krypton is inert for most practical purposes but it is known to form compounds with fluorine. Krypton can also form clathrates with water when atoms of it are trapped in a lattice of the water molecules.

From 1960 to 1983, the length of the meter was defined in terms of the orange-red spectral line of krypton-86, an isotope of krypton. It as well as all other noble gases can be used in lighting and photography. Krypton has an important role in production and usage of the krypton fluoride laser.

Contents [hide]
1 Physical properties
2 History
2.1 Metric role
3 Occurrence
4 Compounds
5 Isotopes
6 Uses
7 References
7.1 Other references
8 External links



[edit] Physical properties

A krypton filled discharge tube in the shape of the element's atomic symbol.Krypton is characterized by a brilliant green and orange spectral signature. It is one of the products of uranium fission.[2] Solidified krypton is white and crystalline with a face-centered cubic crystal structure which is a common property of all noble gases.


[edit] History
Krypton (Greek κρυπτόν, krypton meaning "hidden thing" or "hidden one") was discovered in Great Britain in 1898 by Sir William Ramsay and Morris Travers in residue left from evaporating nearly all components of liquid air.[2][3]


[edit] Metric role
In 1960 an international agreement defined the metre in terms of light emitted from a krypton isotope. This agreement replaced the longstanding standard metre located in Paris which was a metal bar made of a platinum-iridium alloy (the bar was originally estimated to be one ten millionth of a quadrant of the earth's polar circumference).[4] But only 23 years later, the krypton-based standard was replaced itself by the speed of light—the most reliable constant in the universe. In October 1983 the Bureau International des Poids et Mesures (International Bureau of Weights and Measures) defined the metre as the distance that light travels in a vacuum during 1/299,792,458 s.[5]


[edit] Occurrence
The concentration of krypton in earth's atmosphere is about 1 ppm. It can be extracted from liquid air by fractional distillation.[6] The amount of krypton in space is uncertain as is the amount is derived from the meteoritic activity and that from solar winds. The first measurements suggest an overabundance of krypton in space.[7]


[edit] Compounds
Like the other noble gases, krypton is chemically inert. However, following the first successful synthesis of xenon compounds in 1962, synthesis of krypton difluoride was reported in 1963.[8] Other fluorides and a salt of a krypton oxoacid have also been found. ArKr+ and KrH+ molecule-ions have been investigated and there is evidence for KrXe or KrXe+.[9]

At the University of Helsinki in Finland, HKrCN and HKrCCH (krypton hydride-cyanide and hydrokryptoacetylene) were synthesized and determined to be stable up to 40K(M. Räsänen et al.).[8]


[edit] Isotopes
Main article: isotopes of krypton
There are 31 known isotopes of krypton.[10] Naturally occurring krypton is made of five stable and one slightly radioactive isotope. Its spectral signature can be produced with some very sharp lines. 81Kr, the product of atmospheric reactions is produced with the other naturally occurring isotopes of krypton. Being radioactive it has a half-life of 250,000 years. Krypton is highly volatile when it is near surface waters and 81Kr has been used for dating old (50,000 - 800,000 year) groundwater.[11]

85Kr is an inert radioactive noble gas with a half-life of 10.76 years. It is produced by fission of uranium and plutonium. It is produced by 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 as most nuclear reactors are in the northern hemisphere.[12]


[edit] Uses
Krypton's multiple emission lines make ionized krypton gas discharges appear white, which in turn makes krypton-based bulbs useful in photography as a brilliant white light source. Krypton is thus used in some types of photographic flashes used in high speed photography. Fluorescent light bulbs are filled with a mixture of krypton and argon gases. Krypton gas is also combined with other gases to make luminous signs that glow with a bright greenish-yellow light.[13]

Krypton's white discharge is often used to good effect in colored gas discharge tubes, which are then simply painted or stained in other ways to allow the desired color (for example, "neon" type advertising signs where the letters appear in differing colors, are often entirely krypton-based). Krypton is also capable of much higher light power density than neon in the red spectral line region, and for this reason, red lasers for high power laser light shows are krypton lasers with mirrors which select out the red spectral line for laser amplification and emission, rather than the more familiar helium-neon variety, which could never practically achieve the multi-watt red laser light outputs needed for this application.[14]

Krypton has an important role in production and usage of the krypton fluoride laser. The laser has been important in the nuclear fusion energy research community in confinement experiments. The laser has high beam uniformity, short wavelength, and the ability to modify the spot size to track an imploding pellet.[15]


[edit] References
^ (2005) "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 edition, Boca Raton, Florida: CRC Press.
^ a b Krypton (English) 1. Argonne National Laboratory, EVS (08 2005). Retrieved on 2007-03-17.
^ William Ramsay, Morris W. Travers (1898). "On a New Constituent of Atmospheric Air". Proceedings of the Royal Society of London 63: 405-408.
^ Measurement Theroy. Capgo Pty Ltd. Retrieved on 2007-03-19.
^ Gibbs, Philip (1997). How is the speed of light measured? (English). Department of Mathematics, University of California. Retrieved on 2007-03-19.
^ How Products are Made: Krypton. Retrieved on 2006-07-02.
^ Cardelli, Jason A.; Meyer, David M. (18). The Abundance of Interstellar Krypton (English) 1-4. The American Astronomical Society. Retrieved on 2007-04-05.
^ a b Bartlett, Neil (2003). The Noble Gases (English). Chemical & Engineering News. Retrieved on 2006-07-02.
^ Periodic Table of the Elements (English) 100-101. Los Alamos National Laboratory's Chemistry Division. Retrieved on 2007-04-05.
^ Isotopes of Krypton. Nuclear Science Division. Retrieved on 2007-03-20.
^ Thonnard, Norbert; Larry D. MeKay, Theodore C. Labotka (31). Development of Laser-Based Resonance Ionization Techniques for 81-Kr and 85-Kr Measurements in the Geosciences (English) 4-7. University of Tennessee, Institute for Rare Isotope Measurements. Retrieved on 2007-03-20.
^ Resources on Isotopes. U.S. Geological Survey. Retrieved on 2007-03-20.
^ Mercury in Lighting. Cape Cod Cooperative Extension. Retrieved on 2007-03-20.
^ Laser Devices, Laser Shows and Effect (PDF). Retrieved on 2007-04-05.
^ Sethian, J.; M. Friedman, M.Myers. Krypton Fluoride Laser Development for Inertial Fusion Energy (English) 1-8. Plasma Physics Division, Naval Research Laboratory. Retrieved on 2007-03-20.

[edit] Other references
Los Alamos National Laboratory - Krypton
"Chemical Elements: From Carbon to Krypton" By: David Newton & Lawrence W. Baker
"Krypton 85: a Review of the Literature and an Analysis of Radiation Hazards" By: William P. Kirk

[edit] External links
Wikimedia Commons has media related to:
KryptonLook up krypton in
Wiktionary, the free dictionary.WebElements.com – Krypton
Krypton Fluoride Lasers
Computational Chemistry Wiki
Retrieved from "http://en.wikipedia.org/wiki/Krypton"
Categories: Chemical elements | Noble gases | Krypton