Xenon is a rare, odorless, colourless, tasteless, chamically unreactive gas. It was regarded as completely inert until, in 1962, Neil Barlett reported synthesis of xenon haxafluoroplatinate. In a gas filled tube xenon emits blue light when excited by electrical discharge.

Applications

Xenon has relatively little commercial use. It is used in photographic flash lamps, stroboscopic lamps, high-intensitive arc-lamps for motion picture projection and high-pressure arc lamps to product ultraviolet light (solar simulators). Other uses are as general anaesthetic, xenon 'blue' headlights and fog lights are used on some vehicles and are said to be less tiring on the eyes. They illuminate road signs and markings better than conventional lights.

Xenon in the environment

Xenon si a trace gas in the Earth's atmosphere, occurring in 1 part in 20 million. The only commercial source of xenon is from industrial liquid-air plants. World production is less than 1 tonne per year, although reserved of xenon gas in the atmosphere amount to 2 billion tonnes.

Health effects of xenon

Inhalation: This gas is inert and is classified as a simple asphyxiant. Inhalation in excessive concentrations can result in dizziness, nausea, vomiting, loss of consciousness, and death. Death may result from errors in judgment, confusion, or loss of consciousness which prevent self-rescue. At low oxygen concentrations, unconsciousness and death may occur in seconds without warning. 

The effect of simple asphyxiant gases is proportional to the extent to which they diminish the amount (partial pressure) of oxygen in the air that is breathed. The oxygen may be diminished to 75% of it's normal percentage in air before appreciable symptoms develop. This in turn requires the presence of a simple asphyxiant in a concentration of 33% in the mixture of air and gas. When the simple asphyxiant reaches a concentration of 50%, marked symptoms can be produced. A concentration of 75% is fatal in a matter of minutes. Symptoms: The first symptoms produced by a simple asphyxiant are rapid respirations and air hunger. Mental alertness is diminished and muscular coordination is impaired. Later judgment becomes faulty and all sensations are depressed. Emotional instability often results and fatigue occurs rapidly. As the asphyxia progresses, there may be nausea and vomiting, prostration and loss of consciousness, and finally convulsions, deep coma and death.  

This agent is not considered a carcinogen. 

Effects of xenon on the environment

Xenon is a rare atmospheric gas and as such is non-toxic and chemically inert. The extreme cold temperature (-244^oC) will freeze organisms on contact, but no long term ecological effects are anticipated.

Disposal considerations: When disposal becomes necessary, vent gas slowly to a well-ventilated out door location remote from personnel work areas and building air intakes. Do not dispose of any residual gas in compressed gas cylinders. Return cylinders to the supplier with residual pressure, the cylinder valve tightly closed. Please be advised that state and local requirements for waste disposal may be more restrictive or otherwise different from federal regulations. Consult state and local regulations regarding the proper disposal of this material.

http://www.lenntech.com/Periodic-chart-elements/Xe-en.htm

Detaljnije na wikipediji.

xenon is a "noble" or "inert" gas present in the atmosphere to a small extent. Xenon is present in the Martian atmosphere to the extent of about 0.08 ppm. Before 1962, it was generally assumed that xenon and other noble gases were unable to form compounds. Among the compounds of xenon now reported are xenon hydrate, sodium perxenate, xenon deuterate, difluoride, tetrafluoride, hexafluoride, and XePtF₆ and XeRhF₆. The highly explosive xenon trioxide, XeO₃, is known.

Metallic xenon is produced by applying several hundred kilobars of pressure. Xenon in a vacuum tube produces a blue glow when excited by an electrical discharge and finds use in strobe lamps. It is an odourless, colourless, inert gas.

http://www.webelements.com/xenon/

History

(Gr. 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.

Isotopes

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.

Uses

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.

Title Picture: xenon is used in super bright lamps used for deep sea observation

http://periodic.lanl.gov/elements/54.html
 

http://environmentalchemistry.com/yogi/periodic/Xe.html