Titanium (Ti)
transition-metalSolid
Masse atomique relative standard
47,867 uConfiguration électronique
[Ar] 4s2 3d2Point de fusion
1667,85 °CPoint d’ébullition
3286,85 °CMasse volumique
4500 kg/m³États d’oxydation
−2, −1, 0, +1, +2, +3, +4Électronégativité (Pauling)
1,54Énergie d’ionisation (1re)
6,82812 eVAnnée de découverte
1791Rayon atomique
140 pmDétails
Titanium is a light, strong transition metal with a high melting point and exceptional resistance to corrosion in many natural and industrial environments. Its chemistry is dominated by the +4 oxidation state, although +3 and lower states occur in specialized compounds. The metal is abundant in Earth’s crust but is rarely found in concentrated metallic form because it bonds strongly to oxygen and nitrogen. Its combination of low density, strength, and passivation makes it important in aerospace, chemical equipment, pigments, and medical materials.
Titanium, when pure, is a lustrous, white metal. It has a low density, good strength, is easily fabricated, and has excellent corrosion resistance. It is ductile only when it is free of oxygen. The metal, which burns in air, is the only element that burns in nitrogen.
Titanium is resistant to dilute sulfuric and hydrochloric acid, most organic acids, most chlorine gas, and chloride solutions.
Natural titanium is reported to become very radioactive after bombardment with deuterons. The emitted radiations are mostly positrons and hard gamma rays. The metal is dimorphic. The hexagonal alpha form changes to the cubic beta form very slowly at about 880°C. The metal combines with oxygen at red heat, and with chlorine at 550°C.
Titanium metal is considered to be physiologically inert. When pure, titanium dioxide is relatively clear and has an extremely high index of refraction with an optical dispersion higher than diamond.
The name derives from the Latin titans, who were the mythological "first sons of the earth". It was originally discovered by the English clergyman William Gregor in the mineral ilmenite (FeTiO3) in 1791. He called this mineral menachanite and the element menachin, for the Menachan parish where it was found. It was rediscovered in 1795 by the German chemist Martin Heinrich Klaproth, who called it titanium because it had no characteristic properties to use as a name. Titanium metal was first isolated by the Swedish chemists Sven Otto Pettersson and Lars Fredrik Nilson.
Titanium was discovered in 1791 by the Reverend William Gregor, an English pastor. Pure titanium was first produced by Matthew A. Hunter, an American metallurgist, in 1910. Titanium is the ninth most abundant element in the earth's crust and is primarily found in the minerals rutile (TiO2), ilmenite (FeTiO3) and sphene (CaTiSiO5). Titanium makes up about 0.57% of the earth's crust.
From the Latin titans, the first sons of the Earth, Greek mythology.
Discovered by Gregor in 1791; named by Klaproth in 1795. Impure titanium was prepared by Nilson and Pettersson in 1887; however, the pure metal (99.9%) was not made until 1910 when Hunter heated TiCl4 with sodium in a steel bomb.
Pure titanium is a silvery gray metal. It is ductile when sufficiently pure, but interstitial oxygen, nitrogen, carbon, or hydrogen can harden and embrittle it. At ordinary temperatures it is protected by a thin, adherent oxide film that reforms rapidly after scratching in air or water.
Most titanium mined is not converted to metal but to titanium dioxide, TiO₂, a white pigment used in paints, plastics, paper, inks, ceramics, and sunscreens. Metallic titanium and its alloys are used where high strength-to-weight ratio and corrosion resistance justify the cost, including aircraft structures, jet-engine parts, marine hardware, heat exchangers, and chemical-process equipment. Biocompatible titanium alloys are used for dental and orthopedic implants. Titanium is also used in some sporting goods, architecture, and as a getter or alloying addition in metallurgy.
Titanium is a strong, light metal. It is as strong as steel and twice as strong as aluminum, but is 45% lighter than steel and only 60% heavier than aluminum. Titanium is not easily corroded by sea water and is used in propeller shafts, rigging and other parts of boats that are exposed to sea water. Titanium and titanium alloys are used in airplanes, missiles and rockets where strength, low weight and resistance to high temperatures are important. Since titanium does not react within the human body, it is used to create artificial hips, pins for setting bones and for other biological implants. Unfortunately, the high cost of titanium has limited its widespread use.
Titanium oxide (TiO2) is used as a pigment to create white paint and accounts for the largest use of the element. Pure titanium oxide is relatively clear and is used to create titania, an artificial gemstone. Titanium tetrachloride (TiCl4), another titanium compound, has been used to make smoke screens.
A final bit of titanium trivia titanium is one of the few elements that will burn in an atmosphere of pure nitrogen.
Titanium is important as an alloying agent with aluminum, molybdenum, manganese, iron, and other metals. Alloys of titanium are principally used for aircraft and missiles where lightweight strength and ability to withstand extremes of temperature are important.
Titanium is as strong as steel, but 45% lighter. It is 60% heavier than aluminum, but twice as strong.
Titanium has potential use in desalination plants for converting sea water into fresh water. The metal has excellent resistance to sea water and is used for propeller shafts, rigging, and other parts of ships exposed to salt water. A titanium anode coated with platinum has been used to provide cathodic protection from corrosion by salt water.
It is produced artificially for use as a gemstone, but it is relatively soft. Star sapphires and rubies exhibit their asterism as a result of the presence of TiO2.
Titanium dioxide is extensively used for both house paint and artist's paint, because it is permanent and has good covering power. Titanium oxide pigment accounts for the largest use of the element. Titanium paint is an excellent reflector of infrared, and is extensively used in solar observatories where heat causes poor viewing conditions.
Titanium tetrachloride is used to iridize glass. This compound fumes strongly in air and has been used to produce smoke screens.
Isotopes in Earth/Planetary Science
The isotope-amount ratio n(50Ti)/n(46Ti) is used to study the early history of the Solar System. The value of the ratio can help determine whether the Solar System was created from a well-homogenized source [197] I. Leya, M. Schönbächler, U. Krähenbühl, A. N. Halliday. Astrophys. J.702, 1118 (2009)., [198] R. Courtland. Titanium Reveals Explosive Origins of the Solar System, New Scientist (2014), Feb. 25; http://www.newscientist.com/article/dn16969-titanium-reveals-explosive-origins-of-the-solar-system.html.. For example, variations in titanium isotopic compositions of various groups of meteorites can be observed (Fig. IUPAC.22.1) [199] J. Zhang, N. Dauphas, A. M. Davis, A. Pourmand. J. Anal. At. Spectrom.26, 2197 (2011)..
Isotopes in Industry
The isotope-amount ratio n(48Ti)/n(49Ti) has been used in Isotope Ratio Method (IRM) analysis (initial titanium ratio/final titanium ratio) to estimate the energy production of nuclear reactors. This ratio can also be used to confirm that a reactor is being used for non-proliferation purposes (purposes other than to assist in the formation of nuclear weapon grade materials) [201] D. C. Gerlach, C. J. Gesh, D. E. Hurley, M. R. Mitchell, G. H. Meriwether, B. D. Reid. Final Report on Isotope Ratio Techniques for Light Water Reactors, PNNL-18573. U.S. Department of Energy (2009)..
Titanium forms stable oxides, halides, nitrides, carbides, and organometallic compounds. Titanium dioxide, TiO₂, occurs mainly as rutile, anatase, and brookite and is chemically durable and optically important. Titanium tetrachloride, TiCl₄, is a volatile liquid used in metal production and pigment processing; it fumes in moist air by hydrolysis. Titanium nitride, TiN, is a hard, gold-colored ceramic coating. Titanium carbide, TiC, is a very hard refractory material. In aqueous chemistry, Ti⁴⁺ hydrolyzes strongly, while Ti³⁺ compounds are reducing and less stable in air.
See more information at the Titanium compound page.
Massive titanium metal is generally of low toxicity and is widely used in implants, but fine powder, turnings, and dust can burn vigorously and may pose explosion hazards when dispersed. Hot titanium reacts readily with oxygen, nitrogen, and hydrogen. Titanium tetrachloride, TiCl₄, is highly corrosive and releases hydrogen chloride, HCl, on contact with moisture. Titanium dioxide, TiO₂, is chemically inert in many uses, but inhalation of respirable dust is controlled in occupational settings.
Titanium is a common lithophile element in rocks and soils, mostly locked in resistant oxide and silicate minerals. It has low biological availability because Ti⁴⁺ is strongly hydrolyzed and insoluble under many environmental conditions. Weathering can concentrate titanium minerals such as rutile and ilmenite in heavy-mineral sands. Titanium dioxide particles are persistent, and their environmental behavior depends on particle size, surface coating, and light exposure rather than simple dissolution.
Titanium supply is tied mainly to mineral feedstocks used for pigment production, especially ilmenite and rutile, rather than to metallic titanium demand. Metal production is energy- and process-intensive because titanium cannot be reduced easily from its oxide; the Kroll process converts titanium tetrachloride, TiCl₄, with magnesium to produce sponge metal. Alloy fabrication and machining are costly compared with steel or aluminum. Recycling of clean titanium scrap is important in aerospace and medical supply chains, while contaminated scrap is harder to reuse in high-grade alloys.
Titanium is present in meteorites and the sun. Rocks obtained during the Apollo 17 lunar mission showed presence of 12.1% TiO2; rocks obtained during earlier Apollo missions show lower percentages.
Titanium oxide bands are prominent in the spectra of M-type stars. The element is the ninth most abundant in the crust of the earth. Titanium is almost always present in igneous rocks and in the sediments derived from them.
It occurs in the minerals rutile, ilmenite, and sphene, and is present in titanates and in many iron ores. Titanium is present in ash of coal, in plants, and in human body.
The metal was a laboratory curiosity until Kroll, in 1946, showed that titanium could be produced commercially by reducing titanium tetrachloride with magnesium. This method is still largely used for producing the metal. The metal can be purified by decomposing the iodide.
Titanium is produced in massive stars and supernova environments by nuclear burning and related explosive nucleosynthesis. It is a minor but widely detected element in the Sun, meteorites, and many stellar spectra. In rocky planets it behaves as a refractory lithophile element and is incorporated into oxide and silicate minerals rather than metallic cores. Calcium-aluminum-rich inclusions in meteorites can contain titanium-bearing refractory phases.
- Titanium was named after the Titans of Greek mythology, not after the element’s strength.
- The metal’s useful corrosion resistance comes from a nanometer-scale TiO₂ film.
- Titanium can burn in nitrogen at high temperature, forming titanium nitride.
- Commercially pure titanium grades differ largely by controlled oxygen content.
- Titanium tetrachloride produces dense white fumes in humid air.
- Rutile TiO₂ has one of the highest refractive indices of common colorless solids.
Images
Propriétés
Propriétés physiques
- Rayon atomique (empirique)
- 140 pm Comparer : Rayon atomique (empirique) de tous les éléments →
- Rayon covalent
- 160 pm Comparer : Rayon covalent de tous les éléments →
- Rayon de van der Waals
- 187 pm Comparer : Rayon de van der Waals de tous les éléments →
- Rayon métallique
- 132 pm Comparer : Rayon métallique de tous les éléments →
- Masse volumique
- 4500 kg/m³ Comparer : Masse volumique de tous les éléments →
- Volume molaire
- 0,0106 L/mol
- Phase aux CNTP
- Solide Comparer : Phase aux CNTP de tous les éléments →
- Point de fusion
- 1667,85 °C Comparer : Point de fusion de tous les éléments →
- Point d’ébullition
- 3286,85 °C Comparer : Point d’ébullition de tous les éléments →
- Conductivité thermique
- 21,9 W/(m·K) Comparer : Conductivité thermique de tous les éléments →
- Capacité thermique massique
- 0,523 J/(g·K) Comparer : Capacité thermique massique de tous les éléments →
- Capacité thermique molaire
- 25,06 J/(mol·K) Comparer : Capacité thermique molaire de tous les éléments →
- Structure cristalline
- Hexagonal compact Comparer : Structure cristalline de tous les éléments →
Propriétés chimiques
- Électronégativité (Pauling)
- 1,54 Comparer : Électronégativité (Pauling) de tous les éléments →
- Électronégativité (Allen)
- 1,38
- Affinité électronique
- 0,0755 eV
- Énergie d’ionisation (1re)
- 6,82812 eV Comparer : Énergie d’ionisation (1re) de tous les éléments →
- Énergie d’ionisation (2e)
- 13,575547 eV Comparer : Énergie d’ionisation (2e) de tous les éléments →
- Énergie d’ionisation (3e)
- 27,491805 eV Comparer : Énergie d’ionisation (3e) de tous les éléments →
- Énergie d’ionisation (4e)
- 43,267319 eV Comparer : Énergie d’ionisation (4e) de tous les éléments →
- Énergie d’ionisation (5e)
- 99,299342 eV Comparer : Énergie d’ionisation (5e) de tous les éléments →
- États d’oxydation
- −2, −1, 0, +1, +2, +3, +4 Comparer : États d’oxydation de tous les éléments →
- Électrons de valence
- 4 Comparer : Électrons de valence de tous les éléments →
- Configuration électronique
- [Ar] 4s2 3d2
Propriétés thermodynamiques
- Enthalpie de fusion
- 0,14665492 eV Comparer : Enthalpie de fusion de tous les éléments →
- Enthalpie de vaporisation
- 4,40483 eV Comparer : Enthalpie de vaporisation de tous les éléments →
- Enthalpie de sublimation
- 4,851531 eV
- Enthalpie d’atomisation
- 4,851531 eV
- Enthalpie d’atomisation
- 4,902316 eV
Propriétés nucléaires
- Protons
- 22 Comparer : Protons de tous les éléments →
- Neutrons
- 26 Comparer : Neutrons de tous les éléments →
- Isotopes connus
- 29 Comparer : Isotopes connus de tous les éléments →
- Isotopes stables
- 5 Comparer : Isotopes stables de tous les éléments →
- Isotope le plus stable
- Ti-48
- Année de découverte
- 1791
Abondance
- Abondance (croûte terrestre)
- 5650 mg/kg Comparer : Abondance (croûte terrestre) de tous les éléments →
- Abondance (océan)
- 0,001 mg/L Comparer : Abondance (océan) de tous les éléments →
Structure cristalline
- Paramètre de maille a
- 295 pm
Structure électronique
- Électrons par couche
- 2, 8, 10, 2 Comparer : Électrons par couche de tous les éléments →
Identifiants
- Numéro CAS
- 7440-32-6 Comparer : Numéro CAS de tous les éléments →
- Symbole de terme
- 3F2
- InChI
- InChI=1S/Ti
- Clé InChI
- RTAQQCXQSZGOHL-UHFFFAOYSA-N
Configuration électronique Mesuré
Ti: 3d² 4s²[Ar] 3d² 4s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d² 4s²Modèle atomique
Les isotopes diffèrent par leur nombre de neutrons, leur masse et leur stabilité — pas par la configuration électronique de l’atome neutre.
Modèle atomique schématique, non à l’échelle.
Empreinte atomique
Spectre d’émission / d’absorption
Distribution isotopique
| Nombre de masse | Masse atomique (u) | Abondance naturelle | Demi-vie |
|---|---|---|---|
| 46 Stable | 45,95262772 ± 0,00000035 | 8,2500% | Stable |
| 47 Stable | 46,95175879 ± 0,00000038 | 7,4400% | Stable |
| 48 Stable | 47,94794198 ± 0,00000038 | 73,7200% | Stable |
| 49 Stable | 48,94786568 ± 0,00000039 | 5,4100% | Stable |
| 50 Stable | 49,94478689 ± 0,00000039 | 5,1800% | Stable |
Phase / État
Explication: 1642,8 °C en dessous du point de fusion (1667,85 °C)
Schématique, non à l’échelle
Points de transition de phase
Énergies de transition
Énergie nécessaire pour faire fondre 1 mol au point de fusion
Énergie nécessaire pour vaporiser 1 mol au point d’ébullition
Énergie nécessaire pour sublimer 1 mol au point de sublimation
Masse volumique
Dans les conditions standard
Dans les conditions standard
Spectres atomiques
Affichage de 10 sur 22. Tri par charge ionique croissante.
Raies répertoriées ?
| Ion | Charge | Nombre total de raies | Probabilités de transition | Désignations des niveaux |
|---|---|---|---|---|
| Ti I | 0 | 4029 | 496 | 4029 |
| Ti II | +1 | 1872 | 470 | 1872 |
| Ti III | +2 | 819 | 297 | 819 |
| Ti IV | +3 | 86 | 39 | 86 |
| Ti V | +4 | 252 | 4 | 252 |
| Ti VI | +5 | 71 | 14 | 71 |
| Ti VII | +6 | 92 | 13 | 92 |
| Ti VIII | +7 | 85 | 37 | 85 |
| Ti IX | +8 | 85 | 50 | 85 |
| Ti X | +9 | 162 | 78 | 162 |
Niveaux répertoriés ?
| Ion | Charge | Niveaux |
|---|---|---|
| Ti I | 0 | 559 |
| Ti II | +1 | 253 |
| Ti III | +2 | 200 |
| Ti IV | +3 | 40 |
| Ti V | +4 | 66 |
| Ti VI | +5 | 59 |
| Ti VII | +6 | 62 |
| Ti VIII | +7 | 44 |
| Ti IX | +8 | 32 |
| Ti X | +9 | 83 |
Rayons ioniques
| Charge | Coordinence | Spin | Rayon |
|---|---|---|---|
| +2 | 6 | N/D | 86 pm |
| +3 | 6 | N/D | 67 pm |
| +4 | 4 | N/D | 42 pm |
| +4 | 5 | N/D | 51 pm |
| +4 | 6 | N/D | 60.5 pm |
| +4 | 8 | N/D | 74 pm |
Composés
Isotopes (5)
Natural titanium consists of five isotopes with atomic masses from 46 to 50. All are stable. Eight other unstable isotopes are known.
| Nombre de masse | Masse atomique (u) | Abondance naturelle | Demi-vie | Mode de désintégration | |
|---|---|---|---|---|---|
| 46 Stable | 45,95262772 ± 0,00000035 | 8,2500% ± 0,0300% | Stable | stable | |
| 47 Stable | 46,95175879 ± 0,00000038 | 7,4400% ± 0,0200% | Stable | stable | |
| 48 Stable | 47,94794198 ± 0,00000038 | 73,7200% ± 0,0300% | Stable | stable | |
| 49 Stable | 48,94786568 ± 0,00000039 | 5,4100% ± 0,0200% | Stable | stable | |
| 50 Stable | 49,94478689 ± 0,00000039 | 5,1800% ± 0,0200% | Stable | stable |
Raies spectrales
Affichage de 50 sur 1717. Seules les raies spectrales dont l’intensité a été mesurée sont affichées par défaut.
| Longueur d’onde (nm) | Intensité | Degré d’ionisation | Type | Transition | Précision | Source | |
|---|---|---|---|---|---|---|---|
| 521.03843 nm | 21000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Mesurée | NIST | |
| 506.46526 nm | 17000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Mesurée | NIST | |
| 519.29686 nm | 17000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Mesurée | NIST | |
| 517.37431 nm | 15000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Mesurée | NIST | |
| 498.17305 nm | 14000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 503.99574 nm | 14000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Mesurée | NIST | |
| 468.19089 nm | 13000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Mesurée | NIST | |
| 499.1066 nm | 13000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 499.9503 nm | 12000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 501.41861 nm | 11000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Mesurée | NIST | |
| 399.86363 nm | 10000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Mesurée | NIST | |
| 466.75845 nm | 10000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Mesurée | NIST | |
| 500.72093 nm | 10000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 453.32394 nm | 9200 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 398.17616 nm | 8800 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Mesurée | NIST | |
| 398.97582 nm | 8800 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Mesurée | NIST | |
| 501.42762 nm | 8700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 395.82055 nm | 8600 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Mesurée | NIST | |
| 465.64693 nm | 8400 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Mesurée | NIST | |
| 395.63338 nm | 8000 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Mesurée | NIST | |
| 453.47761 nm | 7900 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 394.86705 nm | 7000 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Mesurée | NIST | |
| 484.08737 nm | 6600 | Ti I | emission | 3d2.4s2 a 1D → 3d2.(1D).4s.4p.(1P*) y 1D* | Mesurée | NIST | |
| 430.59074 nm | 6400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Mesurée | NIST | |
| 453.55686 nm | 6100 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 394.77683 nm | 5700 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(1D).4s.4p.(3P*) 3P* | Mesurée | NIST | |
| 502.00263 nm | 5100 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 430.10787 nm | 4900 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Mesurée | NIST | |
| 503.5903 nm | 4900 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Mesurée | NIST | |
| 502.28679 nm | 4800 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 453.59176 nm | 4700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 430.05538 nm | 4400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Mesurée | NIST | |
| 453.60403 nm | 4000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 503.64639 nm | 4000 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Mesurée | NIST | |
| 501.61609 nm | 3800 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 451.8022 nm | 3700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 488.50794 nm | 3700 | Ti I | emission | 3d3.(2G).4s a 3G → 3d3.(2G).4p y 3H* | Mesurée | NIST | |
| 392.45264 nm | 3600 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Mesurée | NIST | |
| 402.45711 nm | 3600 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Mesurée | NIST | |
| 390.47826 nm | 3500 | Ti I | emission | 3d2.4s2 a 1D → 3d2.(1D).4s.4p.(1P*) y 1F* | Mesurée | NIST | |
| 452.2797 nm | 3500 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 502.48444 nm | 3500 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Mesurée | NIST | |
| 398.24811 nm | 3400 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3P).4s.4p.(3P*) z 5S* | Mesurée | NIST | |
| 454.87635 nm | 3400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 455.24533 nm | 3400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Mesurée | NIST | |
| 400.89274 nm | 3300 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Mesurée | NIST | |
| 503.83979 nm | 3300 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Mesurée | NIST | |
| 392.98737 nm | 3200 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Mesurée | NIST | |
| 429.86657 nm | 3200 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Mesurée | NIST | |
| 489.99088 nm | 3200 | Ti I | emission | 3d3.(2G).4s a 3G → 3d3.(2G).4p y 3H* | Mesurée | NIST |
Propriétés étendues
Rayons covalents (données étendues)
- Rayon covalent (Pyykkö)
- 136 pm
- Rayon covalent (Pyykkö, liaison double)
- 117 pm
- Rayon covalent (Pyykkö, liaison triple)
- 108 pm
- Rayon covalent (Bragg)
- 140 pm
Rayons de van der Waals
- Batsanov
- 215 pm
- Alvarez
- 246 pm
- UFF
- 317,5 pm
- MM3
- 239 pm
Rayons atomiques et métalliques
- Rayon atomique (Rahm)
- 257 pm
- Rayon métallique (C12)
- 147 pm
Échelles de numérotation
- Mendeleev
- 43
- Pettifor
- 51
- Glawe
- 51
Échelles d’électronégativité
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
Polarisabilité et dispersion
- Polarisabilité dipolaire
- 100 a.u.
- Polarisabilité dipolaire (incertitude)
- 10 a.u.
- C₆
- 1044 Ha·Bohr6
- C₆ (Gould–Bučko)
- 1200 Ha·Bohr6
Affinité chimique
- Affinité protonique
- 876 kJ/mol
- Basicité en phase gazeuse
- 853,7 kJ/mol
Paramètres de Miedema
- Volume molaire de Miedema
- 10,58 cm3/mol
- Densité électronique de Miedema
- 4
Risque d’approvisionnement et économie
- Concentration de la production
- 21
- Risque relatif d’approvisionnement
- 5
- Répartition des réserves
- 29
- Stabilité politique (principal producteur)
- 81
- Stabilité politique (principal détenteur de réserves)
- 24
Transitions de phase et allotropes
| Point de fusion | 1943,15 K |
| Point d’ébullition | 3560,15 K |
Catégories d’états d’oxydation
Données de référence avancées
Constantes d’écran (7)
| n | Orbitale | σ |
|---|---|---|
| 1 | s | 0,5591 |
| 2 | p | 3,9352 |
| 2 | s | 6,6234 |
| 3 | d | 13,8586 |
| 3 | p | 11,8963 |
| 3 | s | 10,9669 |
| 4 | s | 17,1832 |
Détail des rayons cristallins (6)
| Charge | CN | Spin | rcrystal (pm) | Origine |
|---|---|---|---|---|
| 2 | VI | 100 | estimated, | |
| 3 | VI | 81 | from r^3 vs V plots, | |
| 4 | IV | 56 | calculated, | |
| 4 | V | 65 | calculated, | |
| 4 | VI | 74,5 | from r^3 vs V plots, | |
| 4 | VIII | 88 | calculated, |
Modes de désintégration des isotopes (47)
| Isotope | Mode | Intensité |
|---|---|---|
| 37 | p | — |
| 38 | 2p | — |
| 39 | B+ | 100% |
| 39 | B+p | 93,7% |
| 39 | 2p | — |
| 40 | B+ | 100% |
| 40 | B+p | 95,8% |
| 41 | B+ | 100% |
| 41 | B+p | 91,1% |
| 42 | B+ | 100% |
Facteurs de diffusion des rayons X (530)
| Énergie (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 1,51668 |
| 10,1428 | — | 1,54246 |
| 10,3068 | — | 1,57217 |
| 10,4735 | — | 1,60245 |
| 10,6429 | — | 1,63331 |
| 10,8151 | — | 1,66477 |
| 10,99 | — | 1,70636 |
| 11,1677 | — | 1,75257 |
| 11,3484 | — | 1,80003 |
| 11,5319 | — | 1,84878 |
Données complémentaires
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
5.65×103 milligrams per kilogram
Références (1)
- [5] Titanium https://education.jlab.org/itselemental/ele022.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
1×10-3 milligrams per liter
Références (1)
- [5] Titanium https://education.jlab.org/itselemental/ele022.html
Sources
Sources of this element.
Titanium is present in meteorites and the sun. Rocks obtained during the Apollo 17 lunar mission showed presence of 12.1% TiO2; rocks obtained during earlier Apollo missions show lower percentages.
Titanium oxide bands are prominent in the spectra of M-type stars. The element is the ninth most abundant in the crust of the earth. Titanium is almost always present in igneous rocks and in the sediments derived from them.
It occurs in the minerals rutile, ilmenite, and sphene, and is present in titanates and in many iron ores. Titanium is present in ash of coal, in plants, and in human body.
The metal was a laboratory curiosity until Kroll, in 1946, showed that titanium could be produced commercially by reducing titanium tetrachloride with magnesium. This method is still largely used for producing the metal. The metal can be purified by decomposing the iodide.
Références (1)
- [6] Titanium https://periodic.lanl.gov/22.shtml
Références
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Titanium.
The element property data was retrieved from publications.