Barium

Main article: Isotopes of barium
iso	NA	half-life	DM	DE (MeV)	DP
¹³⁰Ba	0.106%	¹³⁰Ba is stable with 74 neutrons
¹³²Ba	0.101%	¹³²Ba is stable with 76 neutrons
¹³³Ba	syn	10.51 y	ε	0.517	¹³³Cs
¹³⁴Ba	2.417%	¹³⁴Ba is stable with 78 neutrons
¹³⁵Ba	6.592%	¹³⁵Ba is stable with 79 neutrons
¹³⁶Ba	7.854%	¹³⁶Ba is stable with 80 neutrons
¹³⁷Ba	11.23%	¹³⁷Ba is stable with 81 neutrons
¹³⁸Ba	71.7%	¹³⁸Ba is stable with 82 neutrons

References

Barium (pronounced /ˈbɛəriəm/) is a chemical element. It has the symbol Ba, and atomic number 56. Barium is a soft silvery metallic alkaline earth metal. It is never found in nature in its pure form due to its reactivity with air. Its oxide is historically known as baryta but it reacts with water and carbon dioxide and is not found as a mineral. The most common naturally occurring minerals are the very insoluble barium sulfate, BaSO₄ (barite), and barium carbonate, BaCO₃ (witherite). Benitoite is a rare gem containing barium.

1 Notable characteristics
2 Applications
3 History
4 Occurrence
5 Compounds
6 Isotopes
7 Precautions
8 References
9 External links

[edit] Notable characteristics

Barium is a metallic element that is chemically similar to calcium but more reactive. This metal oxidizes very easily when exposed to air and is highly reactive with water or alcohol, producing hydrogen gas. Burning in air or oxygen produces not just barium oxide (BaO) but also the peroxide. Simple compounds of this heavy element are notable for their high specific gravity. This is true of the most common barium-bearing mineral, its sulfate barite BaSO₄, also called 'heavy spar' due to the high density (4.5 g/cm³).

[edit] Applications

Barium has some medical and many industrial uses:

Barium compounds, and especially barite (BaSO₄), are extremely important to the petroleum industry. Barite is used in drilling mud, a weighting agent in drilling new oil wells.
Barium sulfate is used as a radiocontrast agent for X-ray imaging of the digestive system ("barium meals" and "barium enemas").
Barium carbonate is a useful rat poison and can also be used in making bricks. Unlike the sulfate, the carbonate dissolves in stomach acid, allowing it to be poisonous.
An alloy with nickel is used in spark plug wire.
Barium oxide is used in a coating for the electrodes of fluorescent lamps, which facilitates the release of electrons.
The metal is a "getter" in vacuum tubes, to remove the last traces of oxygen.
Barium carbonate is used in glassmaking. Being a heavy element, barium increases the refractive index and luster of the glass.
Barite is used extensively in rubber production.
Barium nitrate and chlorate give green colors in fireworks.
Impure barium sulfide phosphoresces after exposure to the light.
Lithopone, a pigment that contains barium sulfate and zinc sulfide, is a permanent white that has good covering power, and does not darken in when exposed to sulfides.
Barium peroxide can be used as a catalyst to start an aluminothermic reaction when welding rail tracks together. It can also be used in green tracer ammunition.
Barium titanate was proposed in 2007[2] to be used in next generation battery technology for electric cars.
Barium Fluoride is used in infrared applications.
Barium is a key element in YBCO superconductors.

[edit] History

Barium (Greek barys, meaning "heavy") was first identified in 1774 by Carl Scheele and extracted in 1808 by Sir Humphry Davy in England. The oxide was at first called barote, by Guyton de Morveau, which was changed by Antoine Lavoisier to baryta, from which "barium" was derived to describe the metal.

[edit] Occurrence

Because barium quickly becomes oxidized in air, it is difficult to obtain this metal in its pure form. It is primarily found in and extracted from the mineral barite which is crystallized barium sulfate. Because barite is so insoluble, it cannot be used directly for the preparation of other barium compounds. Instead, the ore is heated with carbon to reduce it to barium sulfide^[1]

BaSO₄ + 2C → BaS + 2CO₂

The barium sulfide is then hydrolyzed or reacted with acids to form other barium compounds such as the chloride, nitrate, and carbonate.

Barium is commercially produced through the electrolysis of molten barium chloride (BaCl₂) Isolation (* follow):

(cathode) Ba²⁺* + 2e^- → Ba

(anode) Cl^-* → ½Cl₂ (g) + e^-

[edit] Compounds

The most important compounds are barium peroxide, barium chloride, sulfate, carbonate, nitrate, and chlorate.

[edit] Isotopes

Main article: isotopes of barium

Naturally occurring barium is a mix of seven stable isotopes. There are twenty-two isotopes known, but most of these are highly radioactive and have half-lives in the several millisecond to several minute range. The only notable exceptions are ¹³³Ba which has a half-life of 10.51 years, and ^137mBa (2.55 minutes).

[edit] Precautions

All water or acid soluble barium compounds are extremely poisonous. At low doses, barium acts as a muscle stimulant, while higher doses affect the nervous system, causing cardiac irregularities, tremors, weakness, anxiety, dyspnea and paralysis. This may be due to its ability to block potassium ion channels which are critical to the proper function of the nervous system.

Barium sulfate can be taken orally because it is highly insoluble in water, and is eliminated completely from the digestive tract. Unlike other heavy metals, barium does not bioaccumulate.^[2] However, inhaled dust containing barium compounds can accumulate in the lungs, causing a benign condition called baritosis.

Oxidation occurs very easily and, to remain pure, barium should be kept under a petroleum-based fluid (such as kerosene) or other suitable oxygen-free liquids that exclude air.

Barium acetate could lead to death in high doses. Marie Robards poisoned her father with the substance in Texas in 1993. She was tried and convicted in 1996.