# barium

properties
[ Xe ] 6 s 2
56 Ba
General
Name , symbol , atomic number Barium, Ba, 56
Element category Alkaline earth metals
Group , period , block 2 , 6 , p
Appearance white-gray metallic
CAS number 7440-39-3
EC number 231-149-1
ECHA InfoCard 100.028.317
Mass fraction of the earth's envelope 0.026%
Atomic
Atomic mass 137,327 (7) et al
Atomic radius (calculated) 215 (253) pm
Van der Waals radius 268 pm
Electron configuration [ Xe ] 6 s 2
1. Ionization energy 5.211 664 6 (12) eV 502.85 kJ / mol
2. Ionization energy 10.003 826 (12) eV 965.22 kJ / mol
3. Ionization energy 35.8438 (25) eV3 458.4 kJ / mol
4. Ionization energy 47.0 (3) eV4 530 kJ / mol
5. Ionization energy 58.0 (1.9) eV5 600 kJ / mol
Physically
Physical state firmly
Crystal structure body-centered cubic
density 3.62 g / cm 3 (20 ° C ) at 293 K.
Mohs hardness 1.25
magnetism paramagnetic ( Χ m = 6.8 10 −6 )
Melting point 1000 K (727 ° C)
boiling point 1910 K (1637 ° C)
Molar volume 38.16 10 −6 m 3 mol −1
Heat of evaporation 149 kJ / mol
Heat of fusion 8.0 kJ mol −1
Speed ​​of sound 1620 m s −1
Work function 2.7 eV
Electric conductivity 2.94 · 10 6 A · V −1 · m −1
Thermal conductivity 18 W m −1 K −1
Chemically
Oxidation states +2
Normal potential −2.92 V
(Ba 2+ + 2 e - → Ba)
Electronegativity 0.89 ( Pauling scale )
Isotopes
isotope NH t 1/2 ZA ZE (M eV ) ZP
128 Ba {syn.} 2.43 d ε 0.521 128 Cs
129 Ba {syn.} 2.23 h ε 2,433 129 Cs
130 Ba 0.106% Stable
131 Ba {syn.} 11.50 d ε 1,370 131 Cs
132 Ba 0.101% Stable
133 Ba {syn.} 10.51 a ε 0.517 133 Cs
134 Ba 2.417% Stable
135 Ba 6.592% Stable
136 Ba 7.854% Stable
137 Ba 11.23% Stable
138 Ba 71.7% Stable
139 Ba {syn.} 83.06 min β - 2,317 139 La
140 Ba {syn.} 12,752 d β - 1.047 140 La
For other isotopes see list of isotopes
NMR properties
Spin
quantum
number I
γ in
rad · T −1 · s −1
E r  ( 1 H) f L at
B = 4.7 T
in MHz
135 Ba 3/2 + 1.21013 · 10 7 0.00079 19.9
137 Ba 3/2 1.08178 · 10 7 0.00033 22.2
safety instructions
GHS labeling of hazardous substances

danger

H and P phrases H: 228-261
EUH: 014
P: 210-231 + 232-280-370 + 378-402 + 404-501
As far as possible and customary, SI units are used.
Unless otherwise noted, the data given apply to standard conditions .

Barium (from Greek βαρύς barýs , German   heavy '' , because of the high density of the barium mineral barite ) is a chemical element with the element symbol Ba and the atomic number 56. In the periodic table it is in the sixth period and the 2nd main group or the 2nd .  IUPAC group and is therefore one of the alkaline earth metals . Barium oxide was first presented by Carl Wilhelm Scheele in 1774 . Barium is metallic, shiny and silvery-white in color. Because of its high reactivity, it does not occur elementally in nature; u. a. it is highly flammable. Water-soluble barium compounds are poisonous.

## history

Carl Wilhelm Scheele

Minerals containing barium were examined for the first time in 1602 by the Italian shoemaker and alchemist Vincenzo Casciarolo (1571–1624), who noticed shiny stones that glowed in the dark after heating. They became known to a wider audience as the “Bolognese Stone” through the publications of Ulisse Aldrovandi . It was barite, which phosphoresces when heated with organic substances .

In 1774 the Swedish chemist Carl Wilhelm Scheele first identified barium oxide (BaO), which was initially called new alkaline earth , while studying gypsum . Two years later, Johan Gottlieb Gahn found the same connection in similar research. Also in the 18th century, the English mineralogist William Withering noticed a heavy mineral in lead mines in Cumberland , which could not be a lead ore and which he named " terra ponderosa ". It is known today as Witherite ( barium carbonate BaCO 3 ).

Metallic barium, but not in its pure form, was first produced in 1808 by Sir Humphry Davy in England by electrolysis of a mixture of barium oxide and mercury oxide. This was followed by the name barium after the barium mineral barite.

The first pure preparation of barium was achieved in 1855 by Robert Bunsen and Augustus Matthiessen by melt electrolysis of a mixture of barium chloride and ammonium chloride . In 1910 Marie Curie isolated the heavier radium using its chemical similarity to barium. The metal also played an important role in 1938 in the nuclear chemistry experiments of Otto Hahn and Fritz Straßmann , who bombarded uranium with slow neutrons and, to their astonishment, found the much lighter element barium in the reaction products. They correctly interpreted this finding as a split in the uranium nucleus.

## Occurrence

Alstonite barite

Because of its high reactivity, barium does not occur elementally in nature, but only in compounds. With a share of around 0.039%, barium is the 14th most common element in the earth's crust .

Barium is mainly found in the minerals barite (barite = crystallized barium sulfate) and withitherite (barium carbonate), with barite being the most common. The annual world production of barite rose from about 4.8 million tons to 6.7 million tons in the years 1973 to 2003, the worldwide reserves are estimated at about two billion tons. The German occurrences of barium compounds are in the Sauerland, Harz and Rhineland-Palatinate. The main producing countries of barium are the People's Republic of China , Mexico , India , Turkey , USA , Germany , Czech Republic , Morocco , Ireland , Italy and France .

## Extraction and presentation

Elemental barium, sublimed under high vacuum

Only a small part of barite is processed into barium metal. The sulfate is first reduced to sulfide. The barium sulfide is then converted into barium carbonate and further into barium oxide, which is finally reduced to the pure metal with silicon or aluminum at 1200 ° C in a vacuum. The reactions proceed according to the following equations:

• ${\ displaystyle \ mathrm {BaSO_ {4} \, (s) +2 \, C \, (s) \ rightarrow BaS \, (s) +2 \, CO_ {2} \, (g)}}$
• Barium sulfate reacts with carbon to form barium sulfide and carbon dioxide .
• ${\ displaystyle \ mathrm {BaS (s) + H_ {2} O \, (l) + CO_ {2} \, (g) \ rightarrow BaCO_ {3} \, (s) + H_ {2} S \, (g)}}$
• Barium sulfide is mixed with water and carbon dioxide and reacts to form barium carbonate and hydrogen sulfide .
• ${\ displaystyle \ mathrm {BaCO_ {3} \, (s) \ rightarrow BaO \, (s) + CO_ {2} \, (g)}}$
• Barium carbonate is insoluble in water; it breaks down to barium oxide and carbon dioxide when heated.
• ${\ displaystyle \ mathrm {3 \, BaO \, (s) +2 \, Al \, (s) \ rightarrow Al_ {2} O_ {3} \, (s) +3 \, Ba \, (s) }}$
• Barium oxide reacts with aluminum to form aluminum oxide and barium metal.

The extraction of metal from barium carbonate is easier according to this scheme, but it is less common in nature. Highly pure barium is obtained from molten barium chloride by electrolysis with subsequent high vacuum sublimation.

## properties

### Physical Properties

Barium is a solid, paramagnetic alkaline earth metal that crystallizes in a body-centered cubic lattice . Its silver-white color quickly turns matt gray in the air because an oxide layer forms.

Barium has a green to pale green flame color with the characteristic spectral lines of 524.2 and 513.7 nm. Barium has a density of 3.62 g / cm 3 (at 20 ° C) and is therefore one of the light metals . With a Mohs hardness of 1.25 it is comparatively soft and also the softest of the alkaline earth metals. The melting point is 727 ° C, the boiling point is 1637 ° C. The electrochemical standard electrode potential is -2.912  V .

### Chemical properties

In terms of its chemical properties, it is similar to calcium and the other alkaline earth metals. It reacts more violently than most other alkaline earth metals with water and with oxygen and dissolves easily in almost all acids - with the exception of concentrated sulfuric acid , as the formation of a sulphate layer ( passivation ) stops the reaction. Barium can therefore be described as one of the most base metals. Because of this high reactivity, it is stored under protective liquids.

It reacts directly with halogens , oxygen, nitrogen and sulfur . It always forms compounds in which it is present as a divalent cation. When heated in air, the metal burns with the typical green flame color to form barium oxide.

As a very base metal, barium reacts with water to form hydrogen and hydroxide. Barium hydroxide is also already formed when the metal comes into contact with moist air.

${\ displaystyle \ mathrm {Ba + 2 \ H_ {2} O \ longrightarrow Ba (OH) _ {2} + H_ {2} \ uparrow}}$

In contrast to other alkaline earth metals, barium only forms a thin, poorly passivating oxide layer and can therefore self-ignite in moist air.

## Isotopes

There are seven stable barium isotopes in nature , with 138 Ba being the most common isotope with 71.8% . Furthermore, 33 radioactive isotopes of barium with half-lives between 10.5 years at 133 Ba and 150 nanoseconds at 153 Ba are known; most disintegrate within a few seconds. The barium isotopes have between 58 ( 114 Ba) and 97 ( 153 Ba) neutrons .

Stable barium isotopes arise from different series of decays, for example 137 I in 137 Ba. The radioactive isotopes break down into lanthanum , xenon , cesium and iodine isotopes .

The following are two examples of nuclear fission that produce radioactive isotopes of barium:

• ${\ displaystyle \ mathrm {^ {1} _ {0} n \ + \ _ {\ 92} ^ {235} U \ \ longrightarrow \ _ {\ 56} ^ {145} Ba \ + \ _ {36} ^ {88} Kr \ + \ 3 \ _ {0} ^ {1} n}}$
Uranium captures a slow neutron and breaks down into barium, krypton and three fast neutrons (first evidence of nuclear fission ).
• ${\ displaystyle \ mathrm {^ {252} _ {\ 98} Cf \ \ longrightarrow \ _ {\ 56} ^ {142} Ba \ + \ _ {\ 42} ^ {106} Mon \ + \ 4 \ _ { 0} ^ {1} n}}$
Californium spontaneously decays into barium, molybdenum and four neutrons.

In addition, the metastable isomer barium-137m can be produced from the decay of cesium -137 with a cesium-barium generator . Barium-137m decays with a half-life of 153.1 (1) seconds with the emission of gamma radiation to form stable barium-137.

## use

Elemental barium is only used on a small scale, and production is only a few tons per year. The most important application is as getter material in vacuum tubes , for example of televisions or as solar collectors , because it quickly binds unwanted residual gases such as oxygen, nitrogen, carbon dioxide and water vapor ; unreactive gases are also trapped and thus removed from the vacuum tube. The vapor pressure of the metal is low at the temperatures used. Nickel alloyed with barium is also used in spark plugs . It also increases the hardness of lead alloys , which are used as bearing metals .

In connection with iron as barium ferrite (BaFe) it is used as a material for high-capacity magnetic tapes.

## Biological importance

Plants take up barium cations from the soil and enrich them. The highest concentration in a useful plant is found in the Brazil nut with a proportion of 1% corresponding to 10,000 ppm (millionths of a proportion) .

Ornamental algae (Desmidiaceae), a family of unicellular green algae (Chlorophyta) about one millimeter in size , that occur in cold, nutrient-poor freshwater, especially in raised bogs , are really dependent on barium . In their cells there are fluid-filled cavities in which there are tiny crystals of barium sulfate. For this purpose, barium is evidently selectively withdrawn from the water even at vanishingly low concentrations of only 1  ppb , whereby even concentrations of the chemically similar alkaline earth metal calcium that are orders of magnitude above do not compete. The algae also tolerate barium concentrations of up to 35 ppm (parts per million), which are lethal for other organisms. Barium is essential for the algae because they stop growing when withdrawn. The biological function of the crystals is still unclear; a role in the perception of gravity is suspected.

Barium also occurs in the human body, the average tissue content is 100 ppb, in blood and bones it is somewhat lower at up to 70 ppb each. About one milligram of barium is ingested with food every day.

## Safety instructions and toxicology

All water or acid soluble barium compounds are poisonous. The maximum workplace concentration (MAK value) is 0.5 mg / m 3 . A dose of 1 to 15 grams is fatal to an adult , depending on the solubility of the barium compound. The water-insoluble contrast agent barium sulfate used in radiology , which is used to depict the gastrointestinal tract or the act of swallowing in X-ray cinematography , must therefore be free of soluble barium compounds, i.e. it must be supplied as a pure substance. It should also be noted that the Latin terms “Barium sulfuricum” (barium sulfate) and “Barium sulfuratum” (barium sulfide) used in pharmacies' language can be confused. Barium poisoning mostly occurs at work or in the vicinity of barium-processing industries. It can be inhaled or enter the body through the drinking water.

Barium ions are deposited in the muscles, lungs and bones, into which it is absorbed, similar to calcium, but more quickly. Its half-life in bone is estimated to be 50 days. As a competitor of calcium on cell membranes , it increases - at low doses - membrane permeability and strengthens muscle contraction. This can lead to an increase in blood pressure with a lowering of the heart rate and to muscle cramps . Higher doses cause muscle weakness and even paralysis , also due to impairment of the central nervous system . Cardiac arrhythmias ( extrasystole and ventricular fibrillation ), tremor , general weakness, dizziness , anxiety and breathing problems can occur. In acute and subacute poisoning, gastrointestinal disorders such as abdominal pain, vomiting and diarrhea can occur. In high concentrations, barium blocks the passive potassium channels in the cell membrane of the muscle cells , so that potassium can no longer leave the muscle cells. Since the sodium-potassium-ATPase pumps potassium into the cells undiminished, the potassium level in the blood drops . The resulting hypokalemia causes the failure of the muscle reflexes ( areflexia ) with subsequent muscle and respiratory paralysis .

First aid can be given by administering sodium sulphate or potassium sulphate solution, which binds the barium ions as barium sulphate , which is poorly soluble and therefore non-toxic. In the hospital, barium can be removed by dialysis .

## proof

### Wet chemical methods

One detection reaction is the reaction with dilute sulfuric acid , whereupon white barium sulfate precipitates:

${\ displaystyle \ mathrm {SO_ {4} ^ {2 -} + \ BaCl_ {2} \ longrightarrow BaSO_ {4} \! \ downarrow + \ 2 \, Cl ^ {-}}}$

If barium is in company with other elements that also form sparingly soluble sulfates, this process cannot be used. If only alkaline earth elements are present, separation and verification are carried out according to the chromate-sulfate process (see under ammonium carbonate group ). As part of this process, potassium chromate solution is added to the barium solution, and a yellow precipitate of barium chromate is formed . If other elements with sparingly soluble sulfates are also present, a suitable cation separation process must be carried out.

### Instrumental methods

A method suitable for detecting barium is atomic spectroscopy . The detection of barium and barium salts takes place via the characteristic spectrum . With a flame atomic absorption spectrometer or an atomic emission spectrometer with inductively coupled high-frequency plasma, even small traces of barium can be detected. With the classic detection, the sample is held in a Bunsen burner flame and the green color of the flame is observed. However, this method is ambiguous when there are elements with similar flame colors.

Fireworks: Green color of the barium

Barium compounds are almost exclusively in the + II oxidation state . These are mostly colorless, salty solids. The green color of the flame is characteristic of barium compounds.

### Oxygen compounds

There are two different barium-oxygen compounds , barium oxide and barium peroxide . Barium oxide adsorbs water and carbon dioxide and is used accordingly. Barium peroxide, which can be made from barium oxide, is a powerful oxidizing agent and is used in pyrotechnics. It is also a possible starting material for the production of hydrogen peroxide . If barium oxide is dissolved in water, the strong base barium hydroxide is formed, which can be used to detect carbonate ions.

### Halogen compounds

With halogens, barium forms compounds of the type BaX 2 , which crystallize in the lead (II) chloride structure. Barium fluoride , which crystallizes differently in the fluorite structure , has a wide transparent spectral range and is used in the optical industry. The poisonous and readily soluble barium chloride is the basic material for other barium compounds and serves as a precipitant for sulfate , for example for detection or for water softening.

### Compounds with oxo acids

Barium sulfate is the technically most important barium compound. Compared to other barium compounds, it has the advantage of being non-toxic due to its very low solubility. It is mainly used in oil production to increase the density of drilling mud . It also serves as a filler for plastics , as an X-ray contrast medium and is used as a paint .

Barium carbonate is an effective rat poison , it is also used as a raw material for glass manufacture and in the production of hard magnetic ferrites .

Barium nitrate , barium iodate and barium chlorate are used in pyrotechnics because of their fire-promoting properties and the green color of the flame .

Further barium compounds can be found in the category: barium compounds

## literature

Commons : Barium  - collection of images, videos and audio files
Wiktionary: Barium  - explanations of meanings, word origins, synonyms, translations
• Entry to barium. In: Römpp Online . Georg Thieme Verlag, accessed on January 3, 2015.
• Barium in the federal environmental sample database

## Individual evidence

1. a b Harry H. Binder: Lexicon of the chemical elements. S. Hirzel Verlag, Stuttgart 1999, ISBN 3-7776-0736-3 .
2. The values ​​for the properties (infobox) are taken from www.webelements.com (barium) , unless otherwise stated .
3. Manjeera Mantina, Adam C. Chamberlin, Rosendo Valero, Christopher J. Cramer, Donald G. Truhlar: Consistent van der Waals Radii for the Whole Main Group. In: J. Phys. Chem. A . 113, 2009, pp. 5806-5812, doi: 10.1021 / jp8111556 .
4. Entry on barium in Kramida, A., Ralchenko, Yu., Reader, J. and NIST ASD Team (2019): NIST Atomic Spectra Database (ver. 5.7.1) . Ed .: NIST , Gaithersburg, MD. doi : 10.18434 / T4W30F ( https://physics.nist.gov/asd ). Retrieved June 11, 2020.
5. Entry on barium at WebElements, https://www.webelements.com , accessed on June 11, 2020.
6. ^ Norman N. Greenwood, Alan Earnshaw: Chemistry of the elements. 1st edition. VCH, Weinheim 1988, ISBN 3-527-26169-9 , p. 136.
7. Robert C. Weast (Ed.): CRC Handbook of Chemistry and Physics . CRC (Chemical Rubber Publishing Company), Boca Raton 1990, ISBN 0-8493-0470-9 , pp. E-129 to E-145. Values ​​there are based on g / mol and given in cgs units. The value specified here is the SI value calculated from it, without a unit of measure.
8. a b Yiming Zhang, Julian RG Evans, Shoufeng Yang: Corrected Values ​​for Boiling Points and Enthalpies of Vaporization of Elements in Handbooks. In: Journal of Chemical & Engineering Data . 56, 2011, pp. 328-337, doi: 10.1021 / je1011086 .
9. Ludwig Bergmann, Clemens Schaefer, Rainer Kassing: Textbook of Experimental Physics . Volume 6: Solids. 2nd Edition. Walter de Gruyter, Berlin 2005, ISBN 3-11-017485-5 , p. 361.
10. a b Entry on barium in the GESTIS substance database of the IFA , accessed on April 29, 2017(JavaScript required) .
11. a b c Robert Kresse u. a .: Barium and Barium Compounds. In: Ullmann's Encyclopedia of Industrial Chemistry. 6th edition. 2007, doi: 10.1002 / 14356007.a03_325 .
12. ^ Norman N. Greenwood, Alan Earnshaw: Chemistry of the elements. 1st edition. VCH, Weinheim 1988, ISBN 3-527-26169-9 , p. 133.
13. ^ Entry on barium. In: Römpp Online . Georg Thieme Verlag, accessed on January 3, 2015.
14. Entry on Barium-137m at the National Nuclear Data Center , accessed on June 6, 2016.
15. ^ AF Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 102nd edition. Walter de Gruyter, Berlin 2007, ISBN 978-3-11-017770-1 , p. 1239.
16. World's 1st exabyte storage system. January 31, 2011, accessed October 29, 2015 .
17. ^ Concise International Chemical Assessment Document (CICAD) for Barium and Barium Compounds , accessed November 18, 2014.
18. Yu-Jen Su et al. a .: An Industrial Worker Hospitalized With Paralysis After an Aerosolized Chemical Exposure . In: American Journal of Kidney Diseases . tape 56 , no. 3 , 2010, p. A38-A41 , doi : 10.1053 / j.ajkd.2010.02.004 ( ajkd.org ).
19. ^ E. Schweda: Jander / Blasius: Inorganic Chemistry I - Introduction & Qualitative Analysis. 17th edition. Hirzel, 2012, ISBN 978-3-7776-2134-0 , p. 312.
20. ^ William Morton: Poisoning by barium carbonate. In: The Lancet . 2, 1945, pp. 738-739 ( doi: 10.1016 / S0140-6736 (45) 91071-3 ).