Titanium (Ti)
White metallic transition element. Occurs in numerous minerals. Used in strong, light corrosion-resistant alloys. Forms a passive oxide coating when exposed to air. First discovered by Gregor in 1789.
| Atomic Number | 22 |
|---|---|
| Atomic Weight | 47.867 |
| Mass Number | 48 |
| Group | 4 |
|---|---|
| Period | 4 |
| Block | d |
| Protons | 22 p+ |
|---|---|
| Neutrons | 26 n0 |
| Electrons | 22 e- |
Properties
| Atomic Radius | 140 pm
|
|---|---|
| Atomic Volume | 10.6 cm³/mol
|
| Covalent Radius | 136 pm
|
| Metallic Radius | 132 pm
|
| Ionic Radius | 86 pm
|
| Crystal Radius | 100 pm
|
| Van der Waals radius |
211 pm
|
| Density | 4.506 g/cm³
|
| Boiling Point | 3,560 K
|
| Melting Point | 1,933 K
|
| Electrons per shell | 2, 8, 10, 2 |
| Electronegativity |
1.54
|
| Electrophilicity | 0.8836023565739 eV/particle
|
| Proton Affinity | 876 kJ/mol
|
| Electron Affinity | 0.079 eV/particle
|
| Ionization Potential | 6.82812 eV/particle
|
| Heat of Vaporization | 422.6 kJ/mol
|
| Heat of Fusion | 18.8 kJ/mol
|
| Heat of Formation | 473 kJ/mol
|
| Molar Heat Capacity | 25.06 J/(mol K)
|
| Specific Heat Capacity | 0.523 J/(g⋅K)
|
| Thermal Conductivity | 21.9 W/(m K)
|
| Gas Basicity | 853.7 kJ/mol
|
| Dipole Polarizability | 100 a₀
|
| C6 Dispersion Coefficient | 1,044 a₀
|
| Oxidation States | -1, 2, 3, 4 |
| Color | Silver
|
| Crystal Structure | Simple Hexagonal (HEX) |
| Lattice Constant | 2.95 Å
|
| Bulk Modulus | |
| Electrical Resistivity | |
| Electron Configuration | [Ar] 3d2 4s2 |
| Magnetic Ordering | |
| Magnetic Susceptibility | |
| Phase | Solid |
| Poisson Ratio | |
| Shear Modulus | |
| Young's Modulus | |
| Allotropes | |
| Alternate Names | |
| Adiabatic Index | |
| Appearance | |
| Electric Conductivity | |
| Critical Pressure | |
| Critical Temperature | |
| Curie Point | |
| Electrical | |
| Hardness | |
| Magnetic Susceptibility | |
| Magnetic | |
| Neel Point | |
| Neutron Cross Section | |
| Neutron Mass Absorption | |
| Gas Phase | |
| Quantum Numbers | |
| Refractive Index | |
| Space Group | |
| Speed of Sound | |
| Superconducting Point | |
| Thermal Expansion | |
| Valence Electrons | |
| Classification | |
| Category | Transition metals, Transition metals |
| CAS Group | IVA |
| IUPAC Group | IVB |
| Glawe Number | 51 |
| Mendeleev Number | 43 |
| Pettifor Number | 51 |
| Geochemical Class | first series transition metal |
| Goldschmidt Class | litophile |
| Radioactivity | |
| Radioactive | No |
| Decay Mode | |
| Half-Life | |
| Lifetime | |
| Abundance | |
| Abundance in Earth's crust | 5,650 mg/kg
|
| Abundance in Oceans | 0.001 mg/L
|
| Abundance in Human Body | |
| Abundance in Meteor | |
| Abundance in Sun | |
| Abundance in Universe | 0.0003% |
Isotopes of Titanium
Stable Isotopes
46Ti 47Ti 48Ti 49Ti 50Ti
Unstable Isotopes
38Ti 39Ti 40Ti 41Ti 42Ti 43Ti 44Ti 45Ti 51Ti 52Ti 53Ti 54Ti 55Ti 56Ti 57Ti 58Ti 59Ti 60Ti 61Ti 62Ti 63Ti
History
William Gregor found the oxide of titanium in ilmenite in 1791. Martin Heinrich Klaproth independently discovered the element in rutile in 1795 and named it. The pure metallic form was only obtained in 1910 by Matthew A. Hunter. In 1936, the Kroll Process made the commercial production of titanium possible. From the Latin titans, the first sons of the Earth, Greek mythology
| Discoverers | William Gregor |
|---|---|
| Discovery Location | England |
| Discovery Year | 1791 |
| Name Origin | Greek: titanos (Titans). |
Titanium metal is considered to be non-toxic
Titanium is one of the few elements that burns in pure nitrogen gas
Uses
Titanium is used in steel as an alloying element to reduce grain size and as a deoxidizer, and in stainless steel to reduce carbon content. Titanium has potential use in desalination plants for converting sea water into fresh water. Titanium is used in several everyday products such as drill bits, bicycles, golf clubs, watches and laptop computers. Since it is strong and resists acids it is used in many alloys. Titanium dioxide (TiO2), a white pigment that covers surfaces very well, is used in paint, rubber, paper and many others.
Sources
Usually occurs in the minerals ilmenite (FeTiO3) or rutile (TiO2). Also in Titaniferous magnetite, titanite (CaTiSiO5), and iron ores. Pure metal produced by heating TiO2 with C and Cl2 to produce TiCl4 then heated with Mg gas in Ar atmosphere.