Barium - wikipedia Barium Barium, Ba General properties Pronunciation / ˈbɛriəm / ​ ( BAIR - ee - əm ) Appearance silvery gray ; with a pale yellow tint Standard atomic weight ( A ) 7002137327000000000 ♠ 137.327 ( 7 ) Barium in the periodic table Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury ( element ) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson Sr ↑ Ba ↓ Ra caesium ← barium → lanthanum Atomic number ( Z ) 56 Group, period group 2 ( alkaline earth metals ), period 6 Block s - block Element category alkaline earth metals Electron configuration ( Xe ) 6s Electrons per shell 2, 8, 18, 18, 8, 2 Physical properties Phase ( at STP ) solid Melting point 1000 K ​ ( 727 ° C, ​ 1341 ° F ) Boiling point 2118 K ​ ( 1845 ° C, ​ 3353 ° F ) Density ( near r.t. ) 3.51 g / cm when liquid ( at m.p. ) 3.338 g / cm Heat of fusion 7.12 kJ / mol Heat of vaporization 142 kJ / mol Molar heat capacity 28.07 J / ( mol K ) Vapor pressure P ( Pa ) 10 100 1 k 10 k 100 k at T ( K ) 911 1038 1185 1388 1686 2170 Atomic properties Oxidation states + 2, + 1 ​ ( a strongly basic oxide ) Electronegativity Pauling scale : 0.89 Ionization energies 1st : 502.9 kJ / mol 2nd : 965.2 kJ / mol 3rd : 3600 kJ / mol Atomic radius empirical : 222 pm Covalent radius 215 ± 11 pm Van der Waals radius 268 pm Spectral lines Miscellanea Crystal structure ​ body - centered cubic ( bcc ) Speed of sound thin rod 1620 m / s ( at 20 ° C ) Thermal expansion 20.6 μm / ( m K ) ( at 25 ° C ) Thermal conductivity 18.4 W / ( m K ) Electrical resistivity 332 nΩ m ( at 20 ° C ) Magnetic ordering paramagnetic Magnetic susceptibility + 20.6 10 cm / mol Young 's modulus 13 GPa Shear modulus 4.9 GPa Bulk modulus 9.6 GPa Mohs hardness 1.25 CAS Number 7440 - 39 - 3 History Discovery Carl Wilhelm Scheele ( 1772 ) First isolation Humphry Davy ( 1808 ) Main isotopes of barium Isotope Abundance Half - life ( t ) Decay mode Product Ba 0.11 % ( 0.5 -- 2.7 ) × 10 y εε Xe Ba 0.10 % stable Ba syn 10.51 y ε Cs Ba 2.42 % stable Ba 6.59 % stable Ba 7.85 % stable Ba 11.23 % stable Ba 71.70 % stable view talk references in Wikidata Barium is a chemical element with symbol Ba and atomic number 56. It is the fifth element in group 2 and is a soft, silvery alkaline earth metal. Because of its high chemical reactivity, barium is never found in nature as a free element. Its hydroxide, known in pre-modern history as baryta, does not occur as a mineral, but can be prepared by heating barium carbonate. The most common naturally occurring minerals of barium are barite ( barium sulfate, BaSO ) and witherite ( barium carbonate, BaCO ), both insoluble in water. The barium name originates from the alchemical derivative `` baryta '', from Greek βαρύς ( barys ), meaning `` heavy. '' Baric is the adjectival form of barium. Barium was identified as a new element in 1774, but not reduced to a metal until 1808 with the advent of electrolysis. Barium has few industrial applications. Historically, it was used as a getter for vacuum tubes. It is a component of YBCO ( high - temperature superconductors ) and electroceramics, and is added to steel and cast iron to reduce the size of carbon grains within the microstructure. Barium compounds are added to fireworks to impart a green color. Barium sulfate is used as an insoluble additive to oil well drilling fluid, as well as in a purer form, as X-ray radiocontrast agents for imaging the human gastrointestinal tract. The soluble barium ion and soluble compounds are poisonous, and have been used as rodenticides. Contents 1 Characteristics 1.1 Physical properties 1.2 Chemical reactivity 1.3 Compounds 1.4 Isotopes 2 History 3 Occurrence and production 3.1 Gemstone 4 Applications 4.1 Metal and alloys 4.2 Barium sulfate and barite 4.3 Other barium compounds 5 Toxicity 6 See also 7 References 8 External links Characteristics Physical properties Oxidized barium Barium is a soft, silvery - white metal, with a slight golden shade when ultrapure. The silvery - white color of barium metal rapidly vanishes upon oxidation in air yielding a dark gray oxide layer. Barium has a medium specific weight and good electrical conductivity. Ultrapure barium is very difficult to prepare, and therefore many properties of barium have not been accurately measured yet. At room temperature and pressure, barium has a body - centered cubic structure, with a barium -- barium distance of 503 picometers, expanding with heating at a rate of approximately 1.8 × 10 / ° C. It is a very soft metal with a Mohs hardness of 1.25. Its melting temperature of 1,000 K ( 730 ° C ; 1,340 ° F ) is intermediate between those of the lighter strontium ( 1,050 K or 780 ° C or 1,430 ° F ) and heavier radium ( 973 K or 700 ° C or 1,292 ° F ) ; however, its boiling point of 2,170 K ( 1,900 ° C ; 3,450 ° F ) exceeds that of strontium ( 1,655 K or 1,382 ° C or 2,519 ° F ). The density ( 3.62 g cm ) is again intermediate between those of strontium ( 2.36 g cm ) and radium ( ~ 5 g cm ). Chemical reactivity Barium is chemically similar to magnesium, calcium, and strontium, but even more reactive. It always exhibits the oxidation state of + 2, except in a few rare and unstable molecular species that are only characterised in the gas phase such as BaF. Reactions with chalcogens are highly exothermic ( release energy ) ; the reaction with oxygen or air occurs at room temperature, and therefore barium is stored under oil or in an inert atmosphere. Reactions with other nonmetals, such as carbon, nitrogen, phosphorus, silicon, and hydrogen, are generally exothermic and proceed upon heating. Reactions with water and alcohols are very exothermic and release hydrogen gas : Ba + 2 ROH → Ba ( OR ) + H ↑ ( R is an alkyl or a hydrogen atom ) Barium reacts with ammonia to form complexes such as Ba ( NH ). The metal is readily attacked by most acids. Sulfuric acid is a notable exception because passivation stops the reaction by forming the insoluble barium sulfate on the surface. Barium combines with several metals, including aluminium, zinc, lead, and tin, forming intermetallic phases and alloys. Compounds Selected alkaline earth and zinc salts densities, g cm O2 − S2 − F − Cl − SO 2 − CO 2 − O2 − H − Ca 2 + 3.34 2.59 3.18 2.15 2.96 2.83 2.9 1.7 Sr 2 + 5.1 3.7 4.24 3.05 3.96 3.5 4.78 3.26 Ba 2 + 5.72 4.3 4.89 3.89 4.49 4.29 4.96 4.16 Zn 2 + 5.6 4.09 4.95 2.09 3.54 4.4 1.57 -- Barium salts are typically white when solid and colorless when dissolved, and barium ions provide no specific coloring. They are denser than the strontium or calcium analogs, except for the halides ( see table ; zinc is given for comparison ). Barium hydroxide ( `` baryta '' ) was known to alchemists, who produced it by heating barium carbonate. Unlike calcium hydroxide, it absorbs very little CO in aqueous solutions and is therefore insensitive to atmospheric fluctuations. This property is used in calibrating pH equipment. Volatile barium compounds burn with a green to pale green flame, which is an efficient test to detect a barium compound. The color results from spectral lines at 455.4, 493.4, 553.6, and 611.1 nm. Organobarium compounds are a growing field of knowledge : recently discovered are dialkylbariums and alkylhalobariums. Isotopes Main article : Isotopes of barium Barium found in the Earth 's crust is a mixture of seven primordial nuclides, barium - 130, 132, and 134 through 138. Barium - 130 undergoes very slow radioactive decay to xenon - 130 by double beta plus decay, and barium - 132 theoretically decays similarly to xenon - 132, with half - lives a thousand times greater than the age of the Universe. The abundance is ~ 0.1 % that of natural barium. The radioactivity of these isotopes is so weak that they pose no danger to life. Of the stable isotopes, barium - 138 composes 71.7 % of all barium, and the lighter the isotope, the less abundant. In total, barium has about 50 known isotopes, ranging in mass between 114 and 153. The most stable metastable isotope is barium - 133 with a half - life of approximately 10.51 years. Five other isotopes have half - lives longer than a day. Barium also has 10 meta states, out of which barium - 133m1 is the most stable with a half - life of about 39 hours. History Sir Humphry Davy, who first isolated barium metal Alchemists in the early Middle Ages knew about some barium minerals. Smooth pebble - like stones of mineral barite were found in volcanic rock near Bologna, Italy, and so were called `` Bologna stones. '' Alchemists were attracted to them because after exposure to light they would glow for years. The phosphorescent properties of barite heated with organics were described by V. Casciorolus in 1602. Carl Scheele determined that barite contained a new element in 1774, but could not isolate barium, only barium oxide. Johan Gottlieb Gahn also isolated barium oxide two years later in similar studies. Oxidized barium was at first called `` barote '' by Guyton de Morveau, a name that was changed by Antoine Lavoisier to baryta. Also in the 18th century, English mineralogist William Withering noted a heavy mineral in the lead mines of Cumberland, now known to be witherite. Barium was first isolated by electrolysis of molten barium salts in 1808 by Sir Humphry Davy in England. Davy, by analogy with calcium, named `` barium '' after baryta, with the `` - ium '' ending signifying a metallic element. Robert Bunsen and Augustus Matthiessen obtained pure barium by electrolysis of a molten mixture of barium chloride and ammonium chloride. The production of pure oxygen in the Brin process was a large - scale application of barium peroxide in the 1880s, before it was replaced by electrolysis and fractional distillation of liquefied air in the early 1900s. In this process barium oxide reacts at 500 -- 600 ° C ( 932 -- 1,112 ° F ) with air to form barium peroxide, which decomposes above 700 ° C ( 1,292 ° F ) by releasing oxygen : 2 BaO + O ⇌ 2 BaO Barium sulfate was first applied as a radiocontrast agent in X-ray imaging of the digestive system in 1908. Occurrence and production The abundance of barium is 0.0425 % in the Earth 's crust and 13 μg / L in sea water. The primary commercial source of barium is barite ( also called barytes or heavy spar ), a barium sulfate mineral. with deposits in many parts of the world. Another commercial source, far less important than barite, is witherite, a barium carbonate mineral. The main deposits are located in England, Romania, and the former USSR. Barite, left to right : appearance, graph showing trends in production over time, and the map showing shares of the most important producer countries in 2010. The barite reserves are estimated between 0.7 and 2 billion tonnes. The maximum production, 8.3 million tonnes, was produced in 1981, but only 7 -- 8 % was used for barium metal or compounds. Barite production has risen since the second half of the 1990s from 5.6 million tonnes in 1996 to 7.6 in 2005 and 7.8 in 2011. China accounts for more than 50 % of this output, followed by India ( 14 % in 2011 ), Morocco ( 8.3 % ), US ( 8.2 % ), Turkey ( 2.5 % ), Iran and Kazakhstan ( 2.6 % each ). The mined ore is washed, crushed, classified, and separated from quartz. If the quartz penetrates too deeply into the ore, or the iron, zinc, or lead content is abnormally high, then froth flotation is used. The product is a 98 % pure barite ( by mass ) ; the purity should be no less than 95 %, with a minimal content of iron and silicon dioxide. It is then reduced by carbon to barium sulfide : BaSO + 2 C → BaS + 2 CO ↑ The water - soluble barium sulfide is the starting point for other compounds : reacting BaS with oxygen produces the sulfate, with nitric acid the nitrate, with carbon dioxide the carbonate, and so on. The nitrate can be thermally decomposed to yield the oxide. Barium metal is produced by reduction with aluminium at 1,100 ° C ( 2,010 ° F ). The intermetallic compound BaAl is produced first : 3 BaO + 14 Al → 3 BaAl + Al O BaAl is an intermediate reacted with barium oxide to produce the metal. Note that not all barium is reduced. 8 BaO + BaAl → Ba ↑ + 7 BaAl O The remaining barium oxide reacts with the formed aluminium oxide : BaO + Al O → BaAl O and the overall reaction is 4 BaO + 2 Al → 3 Ba ↑ + BaAl O Barium vapor is condensed and packed into molds in an atmosphere of argon. This method is used commercially, yielding ultrapure barium. Commonly sold barium is about 99 % pure, with main impurities being strontium and calcium ( up to 0.8 % and 0.25 % ) and other contaminants contributing less than 0.1 %. A similar reaction with silicon at 1,200 ° C ( 2,190 ° F ) yields barium and barium metasilicate. Electrolysis is not used because barium readily dissolves in molten halides and the product is rather impure. Benitoite crystals on natrolite. The mineral is named for the San Benito River in San Benito County where it was first found. Gemstone The barium mineral, benitoite ( barium titanium silicate ), occurs as a very rare blue fluorescent gemstone, and is the official state gem of California. Applications Metal and alloys Barium, as a metal or when alloyed with aluminium, is used to remove unwanted gases ( gettering ) from vacuum tubes, such as TV picture tubes. Barium is suitable for this purpose because of its low vapor pressure and reactivity towards oxygen, nitrogen, carbon dioxide, and water ; it can even partly remove noble gases by dissolving them in the crystal lattice. This application is gradually disappearing due to the rising popularity of the tubeless LCD and plasma sets. Other uses of elemental barium are minor and include an additive to silumin ( aluminium -- silicon alloys ) that refines their structure, as well as bearing alloys ; lead -- tin soldering alloys -- to increase the creep resistance ; alloy with nickel for spark plugs ; additive to steel and cast iron as an inoculant ; alloys with calcium, manganese, silicon, and aluminium as high - grade steel deoxidizers. Barium sulfate and barite Amoebiasis as seen in radiograph of barium - filled colon Barium sulfate ( the mineral barite, BaSO ) is important to the petroleum industry as a drilling fluid in oil and gas wells. The precipitate of the compound ( called `` blanc fixe '', from the French for `` permanent white '' ) is used in paints and varnishes ; as a filler in ringing ink, plastics, and rubbers ; as a paper coating pigment ; and in nanoparticles, to improve physical properties of some polymers, such as epoxies. Barium sulfate has a low toxicity and relatively high density of ca. 4.5 g cm ( and thus opacity to X-rays ). For this reason it is used as a radiocontrast agent in X-ray imaging of the digestive system ( `` barium meals '' and `` barium enemas '' ). Lithopone, a pigment that contains barium sulfate and zinc sulfide, is a permanent white with good covering power that does not darken when exposed to sulfides. Other barium compounds Green barium fireworks Other compounds of barium find only niche applications, limited by the toxicity of Ba ions ( barium carbonate is a rat poison ), which is not a problem for the insoluble BaSO. Barium oxide coating on the electrodes of fluorescent lamps facilitates the release of electrons. By its great atomic density, barium carbonate increases the refractive index and luster of glass and reduces leaks of X-rays from cathode ray tubes ( CRT ) TV sets. Barium, typically as barium nitrate imparts a yellow or `` apple '' green color to fireworks ; for brilliant green barium monochloride is used. Barium peroxide is a catalyst in the aluminothermic reaction ( thermite ) for welding rail tracks. It is also a green flare in tracer ammunition and a bleaching agent. Barium titanate is a promising electroceramic. Barium fluoride is used for optics in infrared applications because of its wide transparency range of 0.15 -- 12 micrometers. YBCO was the first high - temperature superconductor cooled by liquid nitrogen, with a transition temperature of 93 K ( − 180.2 ° C ; − 292.3 ° F ) that exceeded the boiling point of nitrogen ( 77 K or − 196.2 ° C or − 321.1 ° F ). Ferrite, a type of sintered ceramic composed of Iron Oxide ( Fe O ) and barium oxide ( BaO ), is both electrically nonconductive and ferrimagnetic, and can be temporarily or permanently magnetized. Toxicity Because of the high reactivity of the metal, toxicological data are available only for compounds. Water - soluble barium compounds are poisonous. In low doses, barium ions act as a muscle stimulant, and higher doses affect the nervous system, causing cardiac irregularities, tremors, weakness, anxiety, shortness of breath, and paralysis. This toxicity may be caused by Ba blocking potassium ion channels, which are critical to the proper function of the nervous system. Other organs damaged by water - soluble barium compounds ( i.e., barium ions ) are the eyes, immune system, heart, respiratory system, and skin causing, for example, blindness and sensitization. Barium is not carcinogenic and it does not bioaccumulate. Inhaled dust containing insoluble barium compounds can accumulate in the lungs, causing a benign condition called baritosis. The insoluble sulfate is nontoxic and is not classified as a dangerous goods in transport regulations. To avoid a potentially vigorous chemical reaction, barium metal is kept in an argon atmosphere or under mineral oils. Contact with air is dangerous and may cause ignition. Moisture, friction, heat, sparks, flames, shocks, static electricity, and exposure to oxidizers and acids should be avoided. Anything that may contact with barium should be electrically grounded. Anyone who works with the metal should wear pre-cleaned non-sparking shoes, flame - resistant rubber clothes, rubber gloves, apron, goggles, and a gas mask. Smoking in the working area is forbidden. Thorough washing is required after handling barium. See also Han purple and Han blue -- synthetic barium copper silicate pigments developed and used in ancient and imperial China Books View or order collections of articles Barium Period 6 elements Alkaline earth metals Chemical elements ( sorted alphabetically ) Chemical elements ( sorted by number ) Portals Access related topics Chemistry portal Medicine portal Find out more on Wikipedia 's Sister projects Media from Commons Definitions from Wiktionary Source texts from Wikisource Learning resources from Wikiversity References Jump up ^ Greenwood, Norman N. ; Earnshaw, Alan ( 1997 ). Chemistry of the Elements ( 2nd ed. ). Butterworth - Heinemann. p. 112. ISBN 0 - 08 - 037941 - 9. Jump up ^ Meija, J. ; et al. ( 2016 ). `` Atomic weights of the elements 2013 ( IUPAC Technical Report ) ''. Pure Appl. Chem. 88 ( 3 ) : 265 -- 91. doi : 10.1515 / pac - 2015 - 0305. Jump up ^ Lide, D.R., ed. ( 2005 ). `` Magnetic susceptibility of the elements and inorganic compounds ''. 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External links Barium at The Periodic Table of Videos ( University of Nottingham ) Elementymology & Elements Multidict 3 - D Holographic Display Using Strontium Barium Niobate Barium compounds Ba ( BO ) BaBr Ba ( CH CO ) Ba ( C H O ) Ba ( ClO ) Ba ( ClO ) BaCO BaC O Ba ( ClO ) Ba ( ClO ) Ba ( CN ) BaCl BaCrO BaF BaFeO BaFe O BaI Ba ( IO ) Ba ( Mn O ) Ba ( N ) Ba ( NO ) BaO BaO Ba ( OH ) BaS BaSO BaSO BaTiO Ba TiO Periodic table ( Large cells ) 5 6 7 8 9 10 11 12 13 14 15 16 17 18 He Li Be O Ne Na Mg Al Si Cl Ar Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe 6 Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og Alkali metal Alkaline earth metal Lanthanide Actinide Transition metal Post - ​ transition metal Metalloid Polyatomic nonmetal Diatomic nonmetal Noble gas Unknown chemical properties LCCN : sh85011853 GND : 4140300 - 9 NDL : 00560541 Retrieved from `` https://en.wikipedia.org/w/index.php?title=Barium&oldid=814468890 '' Categories : Barium Chemical elements Alkaline earth metals Toxicology Reducing agents Hidden categories : Good articles Wikipedia articles with LCCN identifiers Wikipedia articles with GND identifiers Talk Contents About Wikipedia Afrikaans አማርኛ Aragonés Armãneashti Asturianu Azərbaycanca বাংলা Bân - lâm - gú Беларуская Беларуская ( тарашкевіца ) ‎ भोजपुरी Български བོད ་ ཡིག Bosanski Brezhoneg Català Чӑвашла Cebuano Čeština Corsu Cymraeg Dansk Deutsch Eesti Ελληνικά Español Esperanto Euskara فارسی Fiji Hindi Føroyskt Français Furlan Gaeilge Gaelg Gàidhlig Galego 贛 語 ગુજરાતી 客家 語 / Hak - kâ - ngî Хальмг 한국어 Հայերեն हिन्दी Hrvatski Ido Bahasa Indonesia Interlingua Íslenska Italiano עברית Basa Jawa ಕನ್ನಡ ქართული Қазақша Kiswahili Коми Kreyòl ayisyen Kurdî Кыргызча Кырык мары Latina Latviešu Lëtzebuergesch Lietuvių Ligure Limburgs La. lojban. 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Question: where can barium be found in the world
Answer: never found in nature