Structural Biochemistry/Noble Gases

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Background Information[edit]

The Noble Gases are:

  • Helium (He)
  • Neon (Ne)
  • Argon (Ar)
  • Krypton (Kr)
  • Xenon (Xe)
  • Radon (Rn)

Noblefe.gif The inert gases are the 18th group in the periodic table. They are also sometimes called the "noble gasses" due to their lack of reactivity with other chemicals. The elements in this group are typically inert because they possess a full valence shell. All of the noble gases are monatomic, as opposed to other gases (i.e. H2, O2, N2, F2, Cl2) which exist as diatomic at room temperature and atmospheric pressure. The inert gas helium has been employed in respiratory obstruction, in investigative and diagnostic testing, and in hyperbaric applications[2].

The noble gases have weak interatomic force, and consequently have very low melting and boiling points. They are all monatomic gases under standard conditions, including the elements with larger atomic masses than many normally solid elements. Helium has several unique qualities when compared with other elements: its boiling and melting points are lower than those of any other known substance; it is the only element known to exhibit superfluidity; it is the only element that cannot be solidified by cooling under standard conditions—a pressure of 25 standard atmospheres (2,500 kPa; 370 psi) must be applied at a temperature of 0.95 K (−272.200 °C; −457.960 °F) to convert it to a solid. The noble gases up to xenon have multiple stable isotopes. Radon has no stable isotopes; its longest-lived isotope, 222Rn, has a half-life of 3.8 days and decays to form helium and polonium, which ultimately decays to lead.

The noble gases are colorless, odorless, tasteless, and nonflammable under standard conditions. They were once labeled group 0 in the periodic table because it was believed they had a valence of zero, meaning their atoms cannot combine with those of other elements to form compounds. However, it was later discovered some do indeed form compounds, causing this label to fall into disuse. Very little is known about the properties of the most recent member of group 18, ununoctium (Uuo).

The noble gases show extremely low chemical reactivity; consequently, only a few hundred noble gas compounds have been formed. Neutral compounds in which helium and neon are involved in chemical bonds have not been formed (although there are some theoretical evidence for a few helium compounds), while xenon, krypton, and argon have shown only minor reactivity. The reactivity follows the order Ne < He < Ar < Kr < Xe < Rn.

Neon, argon, krypton, and xenon are obtained from air using the methods of liquefaction of gases, to convert elements to a liquid state, and fractional distillation, to separate mixtures into component parts. Helium is typically produced by separating it from natural gas, and radon is isolated from the radioactive decay of radium compounds.[11] The prices of the noble gases are influenced by their natural abundance, with argon being the cheapest and xenon the most expensive. As an example, the table to the right lists the 2004 prices in the United States for laboratory quantities of each gas.

Helium[edit]

Helium is colorless and odorless. Of all the elements in the periodic table, it has the lowest boiling and melting points. It only exists in gas form at extreme environmental conditions. Pierre Janssen and Norman Lockyer first observed this element in 1868 when they found there existed a yellow line of light in a solar eclipse. Helium is the second lightest element and second most abundant element in the universe. This is due to the high binding energy of helium to lithium, beryllium, and boron. Helium has two electrons in the orbital around the nucleus with two protons.

Applications of Helium[edit]

Helium was initially used in dirigible-balloons, however, nowadays it is used in the production of inert gaseous during magnesium, aluminum and titanium welding. Helium is also used in the cooling of nuclear reactors as a transfer media because of its inert/unreactive properties. Helium mixed with oxygen is used for asthma treatment because of its capability of diffusing through lungs so easily. Helium can also be used in respiratory mixtures for high depth divers because of its deprived solubility in blood as apposed to nitrogen. In the liquid state, helium can also be used to achieve extremely low temperatures in electronic devices or for studies in regions of extremely low temperature.

Krypton[edit]

Krypton, found oftentimes in fluorescent lamps, is also colorlesss and odorless and is isolated for research or industrial purposes by distilling air. Krypton can be used to construct high power lasers or krypton fluoride lasers. It has very unique spectral signatures because of its strong spectrum lines. The amount of krypton available in the history of the universe was derived from meteors and solar wind. It acts as a great light source for high end photography.

Applications of Krypton[edit]

Due to the rarity of krypton its applications are dramatically diminished. However krypton is used commercially int he illumination industry where together with argon can be ised in fluorescent lamps. Krypton is also used in flashed for high-speed pictures because it allows for an emission of intense light in a reduced time. This is because when krypton is excited, it emits an intense flash of photons that last only 1/50000 of a second. In smaller amounts, krypton can be used to increase the life of tungsten filaments and in addition be in the medical industry as an absorber of x-ray emissions.

Argon[edit]

Argon is more soluble in water than nitrogen gas. During room temperature, argon will not form any stable formations. Argon was isolated in 1894 by William Ramsay when he removed oxygen, carbon dioxide, water, and nitrogen from clean air. Earth's atmosphere is composed of 1.29% of argon. Argon exists in the most common isotopes as Argon 40, Argon 36, Argon 38, and Argon 40.

Applications of Argon[edit]

The primary use of argon of specific isotopes can be using to date metamorphic and igneous minerals. In addition, different isotopes of argon can be used to date the movement on fault systems. The dating of such minerals and systems may provide the age information on a rock but generally assumptions must be made. In addition to dating, argon can be used in electric light and fluorescent tubes, photo tubes, glow tubes and in lasers. Being an inert gas, it can be used fr welding and cutting, blanketing reactive elements, and act as a protective atmosphere for growing crystals of silicon and germanium due to its nonreactive properties.

Xenon[edit]

Xenon served as an important tool to gain insight of the solar system. Xenon exists in nine stable isotopes but there are actually over 40 stable isotopes that undergo half life and decay. Xenon exists in trace amounts in the earth's atmosphere and in mineral springs. The light properties of xenon have a broad spectrum of visible light and emits bluish light in a gas tube. Nuclear reactors oftentimes expel xenon as well.

Applications of Xenon[edit]

Similar to krypton, due to its high cost and limited abundance, it has very little applications. It is used in photography flashed and, in proportional amounts, used in filling gas mixtures for radiation detection. It is capable of doing so because of its high cross section of ionization of x-rays and gamma rays. AS a stretch, xenon has been used in the past as analytical oxidizing agents and fluorizing agents for specific purposes.

Neon[edit]

Of all the elements, Neon has the smallest range of liquid state. Neon emits red light in neon lamps and in discharge tubes. It exists in trace amounts in the earth's atmosphere and in air.It is the second lightest noble gas, and its density is only 2/3 that of air. Neon emits the strongest discharge of light at normal conditions. Glow-discharge lamps are typically very small but give off a good amount of light. Although all noble gases are unreactive, neon is considered the least reactive. The rarity of neon gas makes attaining small quantities for research very expensive.

Radon[edit]

Radon is a very dense gas at room temperature and is a health hazard. It has high radioactivity therefore it's hard to study it. Radon is formed from the decay of a chain or uranium. High concentrations of radon can cause lung cancer therefore it is considered a very toxic air contaminant and facilities must be evacuated if radon is released. Miners are most exposed to radon. Lung cancer and bad ventilation occurred among many miners in Schneeberg, Germany during the early years of the Cold War.

Applications of Radon[edit]

Radon has been used as a radiation source in cancer therapy with advantages over the currently used radium. It is also used as a radioactive tracer to spot gas leeks and in fluid measurements.

References[edit]

1. Oxtoby, David. (2008). Principles of Modern Chemistry, 6th Ed., ISBN0-534-49366-1.

2. Goodman, Louis S, and Alfred Goodman Gilman. The Pharmacological Basis of Therapeutics. 7th ed. New York, N.Y.: Macmillan, 1985.