▸▸
  • 🇬🇧 Titanium
  • 🇺🇦 Титан
  • 🇨🇳 鈦
  • 🇳🇱 Titaan
  • 🇫🇷 Titane
  • 🇩🇪 Titan
  • 🇮🇱 טיטניום
  • 🇮🇹 Titanio
  • 🇯🇵 チタン
  • 🇵🇹 Titânio
  • 🇪🇸 Titanio
  • 🇸🇪 Titan
  • 🇷🇺 Титан

The bond energy in the gaseous diatomic species TiTi is 141.4 ±21 kJ mol-1.

Titanium: bond enthalpies in gaseous diatomic species

The following values refer to neutral heterodiatomic molecules in the gas phase. These numbers may well differ considerably from, say, single bond energies in a solid. All values are given in kJ mol-1.

Diatomic TiX bond enthalpies. All values are quoted in kJ mol-1. Each formula in the table (TiO, TiF, and so on) is a link - select these to see visual periodicity representations for bond enthalpies involving titanium to elements of your choice.
TiH             TiHe
204.6 ±8.8              
TiLi TiBe TiB TiC TiN TiO TiF TiNe
    276 ±63 423 ±29 476.1 ±33.1 672.4 ±9.2 569 ±33  
TiNa TiMg TiAl TiSi TiP TiS TiCl TiAr
          418 ±3 494  
TiK TiCa TiGa TiGe TiAs TiSe TiBr TiKr
          381 ±42 439  
TiRb TiSr TiIn TiSn TiSb TiTe TiI TiXe
          289 ±17 310 ±42  
TiCs TiBa TiTl TiPb TiBi TiPo TiAt TiRn
               
TiFr TiRa            
               
Image showing periodicity of element-element diatomic bond energies for the chemical elements as size-coded columns on a periodic table grid.
Image showing periodicity of element-element diatomic bond energies for the chemical elements as size-coded columns on a periodic table grid.

Notes

I am grateful to Professor J.A. Kerr (University of Birmingham, UK) for the provision of the bond strengths of diatomic molecules data.

The values given here are at 298 K. All values are quoted in kJ mol-1. Generally, these data were obtained by spectroscopic or mass spectrometric means. You should consult reference 1 for further details. A note of caution: the strength of, say, the C-H bond in the gaseous diatomic species CH (not an isolable species) is not necessarily, the same as the strength of a C-H bond in, say, methane.

The strongest bond for a diatomic species is that of carbon monoxide, CO (1076.5 ± 0.4 kJ mol-1). The strongest bond for a homonuclear diatomic species is that of dinitrogen, N2 (945.33 ± 0.59 kJ mol-1).

References

  1. J.A. Kerr in CRC Handbook of Chemistry and Physics 1999-2000 : A Ready-Reference Book of Chemical and Physical Data (CRC Handbook of Chemistry and Physics, D.R. Lide, (ed.), CRC Press, Boca Raton, Florida, USA, 81st edition, 2000.

Titanium: lattice energies

All values of lattice energies are quoted in kJ mol-1.

Table. All values of lattice energies are quoted in kJ mol-1.
Compound Thermochemical cycle / kJ mol-1 Calculated / kJ mol-1
TiF2 (no value) 2724
TiF3 (no value) 5644
TiF4 9908 10012
TiCl2 2501 2431
TiCl3 5134 5134
TiCl4 (no value) 9431
TiBr2 2419 2360
TiBr3 5007 5012
TiBr4 9039 9288
TiI2 2329 2259
TiI3 (no value) 4845
TiI4 8893 9108
TiH 1407 996
TiH2 (no value) 2866
TiH3 2845 (no value)
TiO 3811 3832
Ti2O3 14149 14702
TiO2 (no value) 12150
  1. H.D.B. Jenkins - personal communication. I am grateful to Prof Don Jenkins (University of Warwick, UK) who provided the lattice energy data, which are adapted from his contribution contained within reference 2.
  2. H.D.B. Jenkins in CRC Handbook of Chemistry and Physics 1999-2000 : A Ready-Reference Book of Chemical and Physical Data (CRC Handbook of Chemistry and Physics, D.R. Lide, (ed.), CRC Press, Boca Raton, Florida, USA, 79th edition, 1998.

Standard Reduction Potentials

Standard reduction potentials of Ti
Standard reduction potentials of titanium

References

The standard reduction potentials given here for aqueous solutions are adapted from the IUPAC publication reference 1 with additional data and an occasional correction incorporated from many other sources, in particular, references 2-7.

  1. A.J. Bard, R. Parsons, and J. Jordan, Standard Potentials in Aqueous Solutions, IUPAC (Marcel Dekker), New York, USA, 1985.
  2. N.N. Greenwood and A. Earnshaw, Chemistry of the Elements, 2nd edition, Butterworth-Heinemann, Oxford, UK, 1997.
  3. F.A. Cotton and G. Wilkinson, Advanced Inorganic Chemistry, 5th edition, John Wiley & Sons, New York, USA, 1988.
  4. B. Douglas, D.H. McDaniel, and J.J. Alexander, Concepts and models of Inorganic Chemistry, 2nd edition, John Wiley & Sons, New York, USA, 1983.
  5. D.F. Shriver, P.W. Atkins, and C.H. Langford, Inorganic Chemstry, 3rd edition, Oxford University Press, Oxford, UK, 1999.
  6. J.E. Huheey, E.A. Keiter, and R.L. Keiter in Inorganic Chemistry : Principles of Structure and Reactivity, 4th edition, HarperCollins, New York, USA, 1993.
  7. G.T. Seaborg and W.D. Loveland in The elements beyond uranium, John Wiley & Sons, New York, USA, 1990.