Xenon

Xenon - Xe

CAS: 7440-63-3
Description: Colorless, odorless, tasteless gas
Classification: Noble Gas
Date of Discovery: 1898
Discoverer: Sir William Ramsay
Name Origin: Greek xenon, "stranger"

Atomic Number: 54
Number of Neutrons: 77
Atomic Mass: 131.29(2) amu
Melting Point: -111.75 °C
Boiling Point: -108.0 °C
Density (293 K): 5.887 ± 0.009 g/cm³
liquid - 3.52 g/cm³ (-109 °C)
Atomic volume: 37.3 cm³/mol
Electrical resistivity:
Thermal conductivity: 5.69 x 10^-5W/cmK
Enthalpy of atomization:
Enthalpy of vaporization: 12.636 kJ/mol
Enthalpy of fusion: 2.297 kJ/mol
Specific heat capacity: 0.158 J/gK

Energy levels: 2-8-18-18-8
Electron configuration: [Kr]4d¹⁰5s²5p⁶
Crystal Structure: Cubic face centered
Atomic radius: 1.24 Å
Covalent radius: 1.31 Å
Oxidation States: usually 0
Electronegativity, Pauling:
Electron affinity: not stable
First ionization energy: 12.130 eV
2nd ionization energy: 21.21 eV
3rd ionization energy: 32.10 eV
Polarizability: 4.044 10^-24cm³

Isotope	Natural Abundance	Atomic Mass	Half-life	Decay Mode	Spin
¹¹⁰Xe	109.9445	0.2 s	⁺
^111mXe	0.9 s	EC, ⁺
¹¹¹Xe	110.9416	EC, ⁺;
¹¹²Xe	111.9357	3 s	EC, ⁺;
¹¹³Xe	112.9334	2.8 s	EC; ⁺
¹¹⁴Xe	113.9281	10.0 s	⁺, EC	0+
¹¹⁵Xe	114.9270	18 s	⁺, EC	(5/2+)
¹¹⁶Xe	115.9214	56 s	⁺, EC	0+
¹¹⁷Xe	116.9206	1.02 m	⁺, EC	(5/2+)
¹¹⁸Xe	117.917	4 m	⁺, EC	0+
¹¹⁹Xe	118.9156	5.8 m	⁺, EC	7/2+
¹²⁰Xe	119.91216	40 m	⁺, EC; ⁺	0+
¹²¹Xe	120.91138	39 m	⁺; EC	5/2+
¹²²Xe	121.9086	20.1 h	EC	0+
¹²³Xe	122.90848	2.00 h	⁺; EC	1/2+
¹²⁴Xe	0.10(1)	123.905895	Stable
^125mXe	57 s	IT	(9/2-)
¹²⁵Xe	124.906398	17.1 h	EC	1/2+
¹²⁶Xe	0.09(1)	125.90427	Stable	0+
^127mXe	1.15 m	IT	(9/2-)
¹²⁷Xe	126.905179	36.4 d	EC	1/2+
¹²⁸Xe	1.91(3)	127.903531	Stable	0+
^129mXe	8.89 d	IT	11/2-
¹²⁹Xe	26.4(6)	128.904780	Stable	1/2+
¹³⁰Xe	4.1(1)	129.903509	Stable	0+
^131mXe	11.9 d	IT	11/2-
¹³¹Xe	21.2(4)	130.905083	Stable	3/2+
¹³²Xe	26.9(5)	131.904155	Stable	0+
^133mXe	2.19 d	IT	11/2-
¹³³Xe	132.905906	5.243 d	^-	3/2+
¹³⁴Xe	10.4(2)	133.905395	Stable	0+
^135mXe	15.3 m	IT	11/2-
¹³⁵Xe	134.90721	9.10 h	^-	3/2+
¹³⁶Xe	8.9(1)	135.90722	Stable	0+
¹³⁷Xe	136.91156	3.82 m	^-	7/2-
¹³⁸Xe	137.91399	14.1 m	^-	0+
¹³⁹Xe	138.91879	39.7 s	^-
¹⁴⁰Xe	139.9216	13.6 s	^-	0+
¹⁴¹Xe	140.9267	1.72 s	^-	5/2+
¹⁴²Xe	141.9297	1.22 s	^-	0+
^143mXe	0.96 s	^-
^143mXe	142.9352	0.30 s	^-
¹⁴⁴Xe	143.9385	1.2 s	^-
¹⁴⁵Xe	0.9 s	^-, n
Discovered by Ramsay and Travers in 1898 in the residue left after evaporating liquid air components. 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. Natural xenon is composed of nine stable isotopes. In addition to these, thirty-five unstable isotopes and isomers 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 the zero valence elements, do form compounds. Among the "compounds" of xenon now reported are xenon hydrate, sodium perxenate, xenon deuterate, difluoride, tetrafluoride, hexafluoride, and XePtF₆ and XeRhF₆. 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. The gas is used in making electron tubes, stroboscopic lamps, bactericidal lamps, and lamps used to excite ruby lasers for generating coherent light. Xenon is used in the atomic energy field in bubble chambers, probes, and other applications where its 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. Xenon is not toxic, but its compounds are highly toxic because of their strong oxidizing characteristics. Xenon produces inhalation anesthesia similar to Nitrus Oxide, however there is not enough xenon in the earth's atmosphere to be used for this purpose. LINKS: Gas Phase MRI using Xenon Xenon as a Heavy Atom? Xenon - An Introduction to Neutron Poisons Xenon head-lights Xenon Ion Propulsion Return Sources for the information on this website include: Lide, David R., ed. CRC Handbook of Chemistry and Physics, 78th Ed., 1997-1998.

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