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Titanium - Ti General Information Discovery Titanium was discovered by the Rev. W. Gregor in 1791 in Creed, Cornwall, and named by M.H. Klaproth in 1795 in Berlin. However, the pure metal was not made until 1910 by Hunter, who heated titanium (IV) chloride with sodium in a steel bomb. Appearance Titanium is a hard, lustrous, silvery metal. Source Titanium is the ninth most abundant element on earth. It is almost always present in igneous rocks and the sediments derived from them. It occurs in the minerals rutile, ilmenite, and sphene, and is present in titanates and many iron ores. Titanium is produced commercially by reducing titanium tetrachloride with magnesium. The major use of this element is as titanium oxide. This is produced commercially by either the Sulphate Process or the Chloride Process, both of which prepare titanium oxide from the mineral ilmenite. Uses Titanium is as strong as steel but much lighter. It is therefore important as an alloying agent with many metals including aluminium, molybdenum and iron. These alloys are principally used in aircraft and missiles as they are materials which are light yet can withstand extremes of temperature. Titanium also has potential use in desalination plants which convert sea water to fresh water. The metal has excellent resistance to sea water and so is used to protect the hulls of ships, and other parts exposed to sea water. However, the largest use of titanium is in the form of titanium oxide, which is extensively used in both house paint and artists. paint. This paint is also a good reflector of infrared radiation and so is used in solar observatories where heat causes poor visibility. Biological Role Titanium has no known biological role, and is non-toxic. It can have a stimulatory effect, and is a suspected carcinogen. General Information Titanium burns in air and is the only element that burns in nitrogen. It is ductile only in an oxygen-free atmosphere. It is resistant to dilute hydrochloric and sulphuric acids, most organic acids, chlorine gas and chloride solutions. It is also resistant to alkalis. It combines with oxygen at red heat and chlorine at 550K. |
| Physical Information | |||
| Atomic Number | 22 | ||
| Relative Atomic Mass (12C=12.000) | 47.88 | ||
| Melting Point/K | 1933 | ||
| Boiling Point/K | 3560 | ||
| Density/kg m-3 | 4540 (293K) | ||
| Ground State Electron Configuration | [Ar]3d24s2 | ||
| Electron Affinity(M-M-)/kJ mol-1 | -2 |
| Key Isotopes | ||||||
| nuclide | 44Ti | 46Ti | 47Ti | 48Ti | 49Ti | |
| atomic mass | 43.952 | 45.952 | 46.948 | 47.948 | 48.948 | |
| natural abundance | 0% | 8.2% | 7.4% | 73.8% | 5.4% | |
| half-life | 48 yrs | stable | stable | stable | stable | |
| nuclide | 50Ti | |||||
| atomic mass | 49.945 | |||||
| natural abundance | 5.2% | |||||
| half-life | stable | |||||
| Other Information | ||
| Enthalpy of Fusion/kJ mol-1 | 20.9 | |
| Enthalpy of Vaporisation/kJ mol-1 | 425.5 | |
| Oxidation States | ||
| main | TiIV | |
| others | Ti-I, TiO, TiII, TiIII | |
| Covalent Bonds /kJ mol-1 | ||
| not applicable | ||
| Ionisation Energies/kJ mol-1 | ||
| M - M+ | 658 | |
| M+ - M2+ | 1310 | |
| M2+ - M3+ | 2652 | |
| M3+ - M4+ | 4175 | |
| M4+ - M5+ | 9573 | |
| M5+ - M6+ | 11516 | |
| M6+ - M7+ | 13590 | |
| M7+ - M8+ | 16260 | |
| M8+ - M9+ | 18640 | |
| M9+ - M10+ | 20830 | |
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