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| Atomic symbol: Pu |
| Atomic number: 94 |
| Atomic weight: (244) |
| Atomic volume: 12.32 cm3/mol |
| Density: 19.8 g/cm3 |
| Period Number: 7 |
| Group number: none |
| Group name: Rare Earth, Actinides |
| Element classification: Metal |
| Phase at room temperature: Solid |
| Melting Point: 914.2 K |
| Boiling point: 3503 K |
| Heat of fusion: 2.840 kJ/mol |
| Heat of vaporization: 344.0 kJ/mol |
| Ionization Energy: 6.06 eV |
| 1st ionization energy: 585 kJ/mole |
| 2nd ionization energy: kJ/mole |
| 3rd ionization energy: kJ/mole |
| Electronegativity: 1.3 |
| Electron affinity: kJ/mole |
| Specific heat: 0.13 J/gK |
| Heat atomization: 352 kJ/mole atoms |
| Shells: 2,8,18,32,24,8,2 |
| Electron Shell Configuration: [Rn] 5f6 7s2 |
| Minimum oxidation number: 0 |
| Maximum oxidation number: 7 |
| Minimum common oxidation number: 0 |
| Maximum common oxidation no: 4 |
Appearance & Characteristics |
| Structure:: fcc: face-centered cubic |
| Color: silvery |
| Hardness: mohs |
| Toxicity: ? |
| Characteristics: Radioactive |
| Uses: weapon fuel, pacemakers |
| Reaction with air: ? |
| Reaction with 6M HCl: ? |
| Reaction with 15M HNO3: passivated |
| Reaction with 6M NaOH: ? |
| Number of isotopes: 0 |
| Oxide(s): PuO Pu2O3 PuO2 |
| Hydride(s): PuH2 PuH3 |
| Chloride(s): PuCl2 PuCl3 |
| Atomic Radius: 159 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): pm |
| Ionic radius (3+ ion): 114 pm |
| Thermal conductivity: 6.3 J/m-sec-deg |
| Electrical conductivity: 7.072 1/mohm-cm |
| Polarizability: 24.5 A^3 |
| Source: Synthetic |
| Relative abundance solar system: log |
| Abundance earth's crust: log |
| Estimated crustal abundance: Not Applicable |
| Estimated oceanic abundance: Not Applicable |
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| (Planet Pluto) Plutonium was the second transuranium element of the actinide series to be discovered. The isotope 238Pu was produced in 1940 by Seaborg, McMillan, Kennedy, and Wahl by deuteron bombardment of uranium in the 60-inch cyclotron at Berkeley, California. Plutonium also exists in trace quantities in naturally occurring uranium ores. It is formed in much the same manner as neptunium: by irradiation of natural uranium with the neutrons which are present. |
| The metal has a silvery appearance and takes on a yellow tarnish when slightly oxidized. It is chemically reactive. A relatively large piece of plutonium is warm to the touch because of the energy given off in alpha decay. Larger pieces will produce enough heat to boil water. The metal readily dissolves in concentrated hydrochloric acid, hydroiodic acid, or perchloric acid. The metal exhibits six allotropic modifications having various crystalline structures. The densities of these vary from 16.00 to 19.86 g/cm3. |
| Plutonium has assumed the position of dominant importance among the trasuranium elements because of its successful use as an explosive ingredient in nuclear weapons and the place which it holds as a key material in the development of industrial use of nuclear power. One kilogram is equivalent to about 22 million kilowatt hours of heat energy. The complete detonation of a kilogram of plutonium produces an explosion equal to about 20,000 tons of chemical explosive. Its importance depends on the nuclear property of being readily fissionable with neutrons and its availability in quantity. The world's nuclear-power reactors are now producing about 20,000 kg of plutonium/yr. By 1982 it was estimated that about 300,000 kg had accumulated. The various nuclear applications of plutonium are well known: 238Pu has been used in the Apollo lunar missions to power seismic and other equipment on the lunar surface. As with neptunium and uranium, plutonium metal can be prepared by reduction of the trifluoride with alkaline-earth metals. |
By far of greatest importance is the isotope 239Pu, with a half-life of 24,100 years, produced in extensive quantities in nuclear reactors from natural uranium: 238U(n, gamma) --> 239U--(beta) --> 239Np--(beta) --> 239Pu. Fifteen isotopes of plutonium are known.
Plutonium also exhibits four ionic valence states in aqueous solutions: Pu+3 (blue lavender), Pu+4 (yellow brown), PuO+ (pink?), and PuO+2(pink-orange). The ion PuO+ is unstable in aqueous solutions, and it disproportionates into Pu+4 and PuO+2. The Pu+4 thus formed, however, oxidizes the PuO+ into PuO+2, itself being reduced to Pu+3, resulting finally in Pu+3 and PuO+2. Plutonium forms binary compounds with oxygen: PuO, PuO2, and intermediate oxides of variable composition; with the halides: PuF3, PuF4, PuCl3, PuBr3, PuI3; with carbon, nitrogen, and silicon: PuC, PuN, PuSi2. Oxyhalides are also well known: PuOCl, PuOBr, PuOI.
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