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| Atomic symbol: Ge |
| Atomic number: 32 |
| Atomic weight: 72.59 |
| Atomic volume: 13.6 cm3/mol |
| Density: 5.323 g/cm3 |
| Period Number: 4 |
| Group number: 14 |
| Group name: Metal, Carbon group |
| Element classification: Semi-metal |
| Phase at room temperature: Solid |
| Melting Point: 1210.6 K |
| Boiling point: 3123 K |
| Heat of fusion: 36.940 kJ/mol |
| Heat of vaporization: 330.90 kJ/mol |
| Ionization Energy: 7.900 eV |
| 1st ionization energy: 762.1 kJ/mole |
| 2nd ionization energy: 1537.4 kJ/mole |
| 3rd ionization energy: 3301.7 kJ/mole |
| Electronegativity: 2.01 |
| Electron affinity: 120 kJ/mole |
| Specific heat: 0.32 J/gK |
| Heat atomization: 377 kJ/mole atoms |
| Shells: 2,8,18,4 |
| Electron Shell Configuration: [Ar] 3d10 4s2 4p2 |
| Minimum oxidation number: -4 |
| Maximum oxidation number: 4 |
| Minimum common oxidation number: -4 |
| Maximum common oxidation no: 4 |
Appearance & Characteristics |
| Structure:: diamond |
| Color: gray-black |
| Hardness: mohs |
| Toxicity: ? |
| Characteristics: semimetal, brittle |
| Uses: transistor, wide-ang lens |
| Reaction with air: mild, w/ht =>GeO2 |
| Reaction with 6M HCl: none |
| Reaction with 15M HNO3: mild, =>Ge(IV), NOx |
| Reaction with 6M NaOH: none |
| Number of isotopes: 5 |
| Oxide(s): GeO GeO2 |
| Hydride(s): GeH4 Ge2H6 + more |
| Chloride(s): GeCl2 GeCl4 |
| Atomic Radius: 122.3 pm |
| Ionic radius (1- ion): pm |
| Ionic radius (1+ ion): pm |
| Ionic radius (2- ion): pm |
| Ionic radius (2+ ion): 87 pm |
| Ionic radius (3+ ion): pm |
| Thermal conductivity: 60.2 J/m-sec-deg |
| Electrical conductivity: 0 1/mohm-cm |
| Polarizability: 6.1 A^3 |
| Source: Zn smelting by-product |
| Relative abundance solar system: 2.076 log |
| Abundance earth's crust: 0.7 log |
| Estimated crustal abundance: 1.5 milligrams per kilogram |
| Estimated oceanic abundance: 5×10-5 milligrams per liter |
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| (Latin Germania: Germany) Mendeleev predicted the existence of Germanium in 1871 as ekasilicon, and the element was discovered by Winkler in 1886. |
The metal is found in
- argyrodite, a sulfide of germanium and silver ;
- germanite, which contains 8 percent of the element;
- zinc ores;
- coal; and
- other minerals
The element is commercially obtained from the dusts of smelters processing zinc ores, as well as recovered from combustion by-products of certain coals. A large reserve of the elements for future uses in insured in coal sources.
Germanium can be separated from other metals by fractional distillation of its volatile tetrachloride. The techniques permit the production of germanium of ultra-high purity.
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| The element is a gray-white metalloid. In pure state, the element is crystalline and brittle, retaining its luster in air at room temperature. It is a very important semiconductor. Zone-refining techniques have led to production of crystalline germanium for semiconductor use with an impurity of only one part in 1010. |
When germanium is doped with arsenic , gallium , or other elements, it is used as a transistor element in thousands of electronic applications. The most common use of germanium is as a semiconductor. Germanium is also finding many other applications including use as an alloying agent, as a phosphor in fluorescent lamps, and as a catalyst.
Germanium and germanium oxide are transparent to the infrared and are used in infrared spectroscopes and other optical equipment, including extremely sensitive infrared detectors.
The high index of refraction and dispersion properties of its oxide's have made germanium useful as a component of wide-angle camera lenses and microscope objectives.
The field of organo-germanium chemistry is becoming increasingly important. Certain germanium compounds have a low mammalian toxicity, but a marked activity against certain bacteria, which makes them useful as chemotherapeutic agents.
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