Titanium (Ti)
transition-metalSolid
Peso atomico standard
47,867 uConfigurazione elettronica
[Ar] 4s2 3d2Punto di fusione
1667,85 °CPunto di ebollizione
3286,85 °CDensità
4500 kg/m³Stati di ossidazione
−2, −1, 0, +1, +2, +3, +4Elettronegatività (Pauling)
1,54Energia di ionizzazione (1ª)
6,82812 eVAnno della scoperta
1791Raggio atomico
140 pmDettagli
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.
Immagini
Proprietà
Fisiche
- Raggio atomico (empirico)
- 140 pm Confronta Raggio atomico (empirico) di tutti gli elementi →
- Raggio covalente
- 160 pm Confronta Raggio covalente di tutti gli elementi →
- Raggio di van der Waals
- 187 pm Confronta Raggio di van der Waals di tutti gli elementi →
- Raggio metallico
- 132 pm Confronta Raggio metallico di tutti gli elementi →
- Densità
- 4500 kg/m³ Confronta Densità di tutti gli elementi →
- Volume molare
- 0,0106 L/mol
- Fase in condizioni STP
- Solido Confronta Fase in condizioni STP di tutti gli elementi →
- Punto di fusione
- 1667,85 °C Confronta Punto di fusione di tutti gli elementi →
- Punto di ebollizione
- 3286,85 °C Confronta Punto di ebollizione di tutti gli elementi →
- Conducibilità termica
- 21,9 W/(m·K) Confronta Conducibilità termica di tutti gli elementi →
- Capacità termica specifica
- 0,523 J/(g·K) Confronta Capacità termica specifica di tutti gli elementi →
- Capacità termica molare
- 25,06 J/(mol·K) Confronta Capacità termica molare di tutti gli elementi →
- Struttura cristallina
- Esagonale compatta Confronta Struttura cristallina di tutti gli elementi →
Chimiche
- Elettronegatività (Pauling)
- 1,54 Confronta Elettronegatività (Pauling) di tutti gli elementi →
- Elettronegatività (Allen)
- 1,38
- Affinità elettronica
- 0,0755 eV
- Energia di ionizzazione (1ª)
- 6,82812 eV Confronta Energia di ionizzazione (1ª) di tutti gli elementi →
- Energia di ionizzazione (2ª)
- 13,575547 eV Confronta Energia di ionizzazione (2ª) di tutti gli elementi →
- Energia di ionizzazione (3ª)
- 27,491805 eV Confronta Energia di ionizzazione (3ª) di tutti gli elementi →
- Energia di ionizzazione (4ª)
- 43,267319 eV Confronta Energia di ionizzazione (4ª) di tutti gli elementi →
- Energia di ionizzazione (5ª)
- 99,299342 eV Confronta Energia di ionizzazione (5ª) di tutti gli elementi →
- Stati di ossidazione
- −2, −1, 0, +1, +2, +3, +4 Confronta Stati di ossidazione di tutti gli elementi →
- Elettroni di valenza
- 4 Confronta Elettroni di valenza di tutti gli elementi →
- Configurazione elettronica
- [Ar] 4s2 3d2
Termodinamiche
- Calore di fusione
- 0,14665492 eV Confronta Calore di fusione di tutti gli elementi →
- Calore di vaporizzazione
- 4,40483 eV Confronta Calore di vaporizzazione di tutti gli elementi →
- Calore di sublimazione
- 4,851531 eV
- Calore di atomizzazione
- 4,851531 eV
- Entalpia di atomizzazione
- 4,902316 eV
Nucleari
- Protoni
- 22 Confronta Protoni di tutti gli elementi →
- Neutroni
- 26 Confronta Neutroni di tutti gli elementi →
- Isotopi noti
- 29 Confronta Isotopi noti di tutti gli elementi →
- Isotopi stabili
- 5 Confronta Isotopi stabili di tutti gli elementi →
- Isotopo più stabile
- Ti-48
- Anno della scoperta
- 1791
Abbondanza
- Abbondanza (crosta terrestre)
- 5650 mg/kg Confronta Abbondanza (crosta terrestre) di tutti gli elementi →
- Abbondanza (oceano)
- 0,001 mg/L Confronta Abbondanza (oceano) di tutti gli elementi →
Struttura cristallina
- Costante reticolare a
- 295 pm
Struttura elettronica
- Elettroni per guscio
- 2, 8, 10, 2 Confronta Elettroni per guscio di tutti gli elementi →
Identificativi
- Numero CAS
- 7440-32-6 Confronta Numero CAS di tutti gli elementi →
- Simbolo di termine
- 3F2
- InChI
- InChI=1S/Ti
- Chiave InChI
- RTAQQCXQSZGOHL-UHFFFAOYSA-N
Configurazione elettronica Misurato
Ti: 3d² 4s²[Ar] 3d² 4s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d² 4s²Modello atomico
Gli isotopi modificano il numero di neutroni, la massa e la stabilità — non la configurazione elettronica di un atomo neutro.
Modello atomico schematico, non in scala.
Impronta atomica
Spettro di emissione / assorbimento
Distribuzione isotopica
| Numero di massa | Massa atomica (u) | Abbondanza naturale | Emivita |
|---|---|---|---|
| 46 Stabile | 45,95262772 ± 0,00000035 | 8,2500% | Stabile |
| 47 Stabile | 46,95175879 ± 0,00000038 | 7,4400% | Stabile |
| 48 Stabile | 47,94794198 ± 0,00000038 | 73,7200% | Stabile |
| 49 Stabile | 48,94786568 ± 0,00000039 | 5,4100% | Stabile |
| 50 Stabile | 49,94478689 ± 0,00000039 | 5,1800% | Stabile |
Fase / Stato
Motivo: 1642,8 °C sotto il punto di fusione (1667,85 °C)
Schema non in scala
Punti di transizione di fase
Energie di transizione
Energia necessaria per fondere 1 mol al punto di fusione
Energia necessaria per vaporizzare 1 mol al punto di ebollizione
Energia necessaria per sublimare 1 mol al punto di sublimazione
Densità
In condizioni standard
In condizioni standard
Spettri atomici
Sono visualizzati 10 di 22. Ordinamento per carica ionica crescente.
Righe disponibili ?
| Ione | Carica | Righe totali | Probabilità di transizione | Designazioni dei livelli |
|---|---|---|---|---|
| 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 |
Livelli disponibili ?
| Ione | Carica | Livelli |
|---|---|---|
| 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 |
Raggi ionici
| Carica | Coordinazione | Spin | Raggio |
|---|---|---|---|
| +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 |
Composti
Isotopi (5)
Natural titanium consists of five isotopes with atomic masses from 46 to 50. All are stable. Eight other unstable isotopes are known.
| Numero di massa | Massa atomica (u) | Abbondanza naturale | Emivita | Modalità di decadimento | |
|---|---|---|---|---|---|
| 46 Stabile | 45,95262772 ± 0,00000035 | 8,2500% ± 0,0300% | Stabile | stable | |
| 47 Stabile | 46,95175879 ± 0,00000038 | 7,4400% ± 0,0200% | Stabile | stable | |
| 48 Stabile | 47,94794198 ± 0,00000038 | 73,7200% ± 0,0300% | Stabile | stable | |
| 49 Stabile | 48,94786568 ± 0,00000039 | 5,4100% ± 0,0200% | Stabile | stable | |
| 50 Stabile | 49,94478689 ± 0,00000039 | 5,1800% ± 0,0200% | Stabile | stable |
Righe spettrali
Sono visualizzati 50 di 1717. Per impostazione predefinita sono mostrate soltanto le righe spettrali con intensità misurata.
| Lunghezza d'onda (nm) | Intensità | Stadio di ionizzazione | Tipo | Transizione | Accuratezza | Fonte | |
|---|---|---|---|---|---|---|---|
| 521.03843 nm | 21000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Misurata | NIST | |
| 506.46526 nm | 17000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Misurata | NIST | |
| 519.29686 nm | 17000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Misurata | NIST | |
| 517.37431 nm | 15000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3F* | Misurata | NIST | |
| 498.17305 nm | 14000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 503.99574 nm | 14000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Misurata | NIST | |
| 468.19089 nm | 13000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Misurata | NIST | |
| 499.1066 nm | 13000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 499.9503 nm | 12000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 501.41861 nm | 11000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3D* | Misurata | NIST | |
| 399.86363 nm | 10000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Misurata | NIST | |
| 466.75845 nm | 10000 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Misurata | NIST | |
| 500.72093 nm | 10000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 453.32394 nm | 9200 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 398.17616 nm | 8800 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Misurata | NIST | |
| 398.97582 nm | 8800 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Misurata | NIST | |
| 501.42762 nm | 8700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 395.82055 nm | 8600 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Misurata | NIST | |
| 465.64693 nm | 8400 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(3P*) z 3G* | Misurata | NIST | |
| 395.63338 nm | 8000 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Misurata | NIST | |
| 453.47761 nm | 7900 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 394.86705 nm | 7000 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Misurata | NIST | |
| 484.08737 nm | 6600 | Ti I | emission | 3d2.4s2 a 1D → 3d2.(1D).4s.4p.(1P*) y 1D* | Misurata | NIST | |
| 430.59074 nm | 6400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Misurata | NIST | |
| 453.55686 nm | 6100 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 394.77683 nm | 5700 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(1D).4s.4p.(3P*) 3P* | Misurata | NIST | |
| 502.00263 nm | 5100 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 430.10787 nm | 4900 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Misurata | NIST | |
| 503.5903 nm | 4900 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Misurata | NIST | |
| 502.28679 nm | 4800 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 453.59176 nm | 4700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 430.05538 nm | 4400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Misurata | NIST | |
| 453.60403 nm | 4000 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 503.64639 nm | 4000 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Misurata | NIST | |
| 501.61609 nm | 3800 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 451.8022 nm | 3700 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 488.50794 nm | 3700 | Ti I | emission | 3d3.(2G).4s a 3G → 3d3.(2G).4p y 3H* | Misurata | NIST | |
| 392.45264 nm | 3600 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Misurata | NIST | |
| 402.45711 nm | 3600 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Misurata | NIST | |
| 390.47826 nm | 3500 | Ti I | emission | 3d2.4s2 a 1D → 3d2.(1D).4s.4p.(1P*) y 1F* | Misurata | NIST | |
| 452.2797 nm | 3500 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 502.48444 nm | 3500 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5G* | Misurata | NIST | |
| 398.24811 nm | 3400 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3P).4s.4p.(3P*) z 5S* | Misurata | NIST | |
| 454.87635 nm | 3400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 455.24533 nm | 3400 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p y 5F* | Misurata | NIST | |
| 400.89274 nm | 3300 | Ti I | emission | 3d2.4s2 a 3F → 3d2.(3F).4s.4p.(1P*) y 3F* | Misurata | NIST | |
| 503.83979 nm | 3300 | Ti I | emission | 3d3.(4F).4s b 3F → 3d3.(4F).4p w 3G* | Misurata | NIST | |
| 392.98737 nm | 3200 | Ti I | emission | 3d2.4s2 a 3F → 3d3.(4F).4p y 3D* | Misurata | NIST | |
| 429.86657 nm | 3200 | Ti I | emission | 3d3.(4F).4s a 5F → 3d3.(4F).4p x 5D* | Misurata | NIST | |
| 489.99088 nm | 3200 | Ti I | emission | 3d3.(2G).4s a 3G → 3d3.(2G).4p y 3H* | Misurata | NIST |
Proprietà estese
Raggi covalenti (dati estesi)
- Raggio covalente (Pyykkö)
- 136 pm
- Raggio covalente (Pyykkö, legame doppio)
- 117 pm
- Raggio covalente (Pyykkö, legame triplo)
- 108 pm
- Raggio covalente (Bragg)
- 140 pm
Raggi di van der Waals
- Batsanov
- 215 pm
- Alvarez
- 246 pm
- UFF
- 317,5 pm
- MM3
- 239 pm
Raggi atomici e metallici
- Raggio atomico (Rahm)
- 257 pm
- Raggio metallico (C12)
- 147 pm
Scale di numerazione
- Mendeleev
- 43
- Pettifor
- 51
- Glawe
- 51
Scale di elettronegatività
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 5
- Robles–Bartolotti
- 4
Polarizzabilità e dispersione
- Polarizzabilità dipolare
- 100 a.u.
- Polarizzabilità dipolare (inc.)
- 10 a.u.
- C₆
- 1044 Ha·Bohr6
- C₆ (Gould–Bučko)
- 1200 Ha·Bohr6
Affinità chimica
- Affinità protonica
- 876 kJ/mol
- Basicità in fase gassosa
- 853,7 kJ/mol
Parametri di Miedema
- Volume molare di Miedema
- 10,58 cm3/mol
- Densità elettronica di Miedema
- 4
Rischio di approvvigionamento ed economia
- Concentrazione della produzione
- 21
- Rischio relativo di approvvigionamento
- 5
- Distribuzione delle riserve
- 29
- Stabilità politica (principale produttore)
- 81
- Stabilità politica (principale detentore di riserve)
- 24
Transizioni di fase e allotropi
| Punto di fusione | 1943,15 K |
| Punto di ebollizione | 3560,15 K |
Categorie degli stati di ossidazione
Dati di riferimento avanzati
Costanti di schermaggio (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 |
Dettaglio dei raggi cristallini (6)
| Carica | 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, |
Modalità di decadimento degli isotopi (47)
| Isotopo | Modalità | Intensità |
|---|---|---|
| 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% |
Fattori di diffusione dei raggi X (530)
| Energia (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 |
Dati aggiuntivi
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
5.65×103 milligrams per kilogram
Riferimenti (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
Riferimenti (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.
Riferimenti (1)
- [6] Titanium https://periodic.lanl.gov/22.shtml
Riferimenti
(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.