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| Atomic symbol: Ba |
| Atomic number: 56 |
| Atomic weight: 137.33 |
| Atomic volume: 39.24 cm3/mol |
| Density: 3.51 g/cm3 |
| Period Number: 6 |
| Group number: 2 |
| Group name: Alkali Earth |
| Element classification: Metal |
| Phase at room temperature: Solid |
| Melting Point: 998.2 K |
| Boiling point: 2123 K |
| Heat of fusion: 7.750 kJ/mol |
| Heat of vaporization: 142.0 kJ/mol |
| Ionization Energy: 5.212 eV |
| 1st ionization energy: 502.9 kJ/mole |
| 2nd ionization energy: 965.2 kJ/mole |
| 3rd ionization energy: kJ/mole |
| Electronegativity: 0.89 |
| Electron affinity: kJ/mole |
| Specific heat: 0.204 J/gK |
| Heat atomization: 180 kJ/mole atoms |
| Shells: 2,8,18,18,8,2 |
| Electron Shell Configuration: [Xe] 6s2 |
| Minimum oxidation number: 0 |
| Maximum oxidation number: 2 |
| Minimum common oxidation number: 0 |
| Maximum common oxidation no: 2 |
Appearance & Characteristics |
| Structure:: bcc: body-centered cubic |
| Color: silvery-white |
| Hardness: mohs |
| Toxicity: ? |
| Characteristics: soft |
| Uses: X-ray imaging agnt(BaSO4) |
| Reaction with air: vigorous,wt/ht=>BaO,Ba2N3 |
| Reaction with 6M HCl: vigorous, =>H2, BaCl2 |
| Reaction with 15M HNO3: mild, =>Ba(NO3)2 |
| Reaction with 6M NaOH: passivated |
| Number of isotopes: 7 |
| Oxide(s): BaO |
| Hydride(s): BaH2 |
| Chloride(s): BaCl2 |
| Atomic Radius: 222 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): 149 pm |
| Ionic radius (3+ ion): pm |
| Thermal conductivity: 18.4 J/m-sec-deg |
| Electrical conductivity: 1/mohm-cm |
| Polarizability: 39.7 A^3 |
| Source: Barite (sulfate) |
| Relative abundance solar system: 0.652 log |
| Abundance earth's crust: 2.6 log |
| Estimated crustal abundance: 4.25×102 milligrams per kilogram |
| Estimated oceanic abundance: 1.3×10-2 milligrams per liter |
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| (Gr. barys: heavy) Baryta was distinguished from lime by Scheele in 1774; the element was discovered by Sir Humphrey Davy in 1808. |
| It is found only in combination with other elements, chiefly with sulfate and carbonate and is prepared by electrolysis of the chloride. |
| Barium is a metallic element, soft, and when pure is silvery white; it belongs to the alkaline earth group, chemically resembling calcium . The metal oxidizes very easily and should be kept under petroleum or other suitable oxygen-free liquids to exclude air. It is decomposed by water or alcohol. |
| The metal is used as a "getter" in vacuum tubes. The most important compounds are the peroxide, chloride, sulfate, carbonate, nitrate, and chlorate. Lithopone, a pigment containing barium sulfate and zinc sulfide, has good covering power, and does not darken in the presence of sulfides. The sulfate, as permanent white is also used in paint, in X-ray diagnostic work, and in glassmaking. Barite is extensively used as a weighing agent in oil well drilling fluids, and is used in making rubber. The carbonate has been used as a rat poison, while the nitrate and chlorate give colors in pyrotechnics. The impure sulfide phosphoresces after exposure to the light. All barium compounds that are water or acid soluble are poisonous. Naturally occurring barium is a mixture of seven stable isotopes. Twenty two other radioactive isotopes are known to exist. |
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