Solid-State Metathesis Materials Synthesis

By: Dr. Richard G. Blair1, Prof. Richard B. Kaner2, Chemfiles Volume 5 Article 13

1Materials and Device Technologies Division,
Jet Propulsion Laboratory Pasadena, CA

2Department of Chemistry & Biochemistry
and California NanoSystems Institute,
University of California, Los Angeles, CA

In the last two decades, a new method termed solid-state metathesis (SSM) has been developed to synthesize compounds that are often difficult to produce conventionally. Alkali or alkaline-earth metal main group compounds are combined with halides to form oxides,17 sulfides,3,8 selenides,3,8 tellurides,3 nitrides,915 phosphides,1618 arsenides,17 antimonides,17 carbides,19,20 silicides,21 borides,15,22,23 and aluminides.24 Additionally, nanostructured materials such as nanotubes,25 nanocrystals,26,27 and high-surface-area materials28can be produced. These reactions provide a novel tool for preparing difficult-to-synthesize materials. Although the precursor is usually a halide, an oxide can be used as well. For example, we have shown that MgSiN2 can be synthesized by reacting SiO2 with Mg3N2.13Oxides have also been successfully used as precursors for hydroxyapatite29 and silicides.21

The driving force behind solid-state metathesis reactions is the formation of stable byproducts. For example, combining GaI3 with Li3N to produce GaN, as given in Scheme 1, has a ΔHrxn of –515 kJ.


Scheme 1. Solid-state metathesis of gallium nitride


This is more than four times as energetic as the elemental reaction Ga + 0.5N2       > GaN (ΔH = –110 kJ).

SSM reactions can be initiated by flame, furnace, heated filament, ball mill, or microwave. The phase produced is often determined by the rate of the reaction.24 Similarly, the reaction rate can be tuned to control the crystallite size of the products formed.9 Diluents or fast reaction times can be used to produce nanoscale powders or materials with high surface areas.9

In a typical SSM reaction, an alkali or alkaline-earth metal compound with the desired anion is reacted with a metal halide or oxide. Reaction temperatures are controlled through the choice of halide, alkali or alkaline-earth metal,30 dilution, and vessel design. It is important to note that the driving force for these reactions is the heat released by the formation of alkali or alkaline-earth halides.

Alkali halides usually have lower heats of formation than alkalineearth halides, so reactions utilizing alkaline-earth metals will generally result in higher reaction temperatures. The upper limit of the reaction temperature is usually governed by the boiling point of the salt produced. Alkaline-earth salts have higher melting and boiling points, thereby increasing the upper limit of the reaction temperature.

The heavier the halogen used, generally the lower the reaction temperature. This can be useful for the synthesis of compounds that are unstable at high temperatures. For example, it is easier to obtain GaN from GaI3 than GaCl3 in a reaction with Li3N,10 due to the differences in heats of formation of LiI (ΔH = –270.4 kJ/mol) vs LiCl (ΔH = –408.5). Conversely, the synthesis of some materials is favored by high temperatures. The use of AlCl3 is a better choice than AlI3 when preparing AlN from the reaction with Ca3N2.9

Another effective method for lowering a reaction temperature is by using a diluent.31 This can be realized by adding inert salts, such as the byproduct salt itself, to the reaction mixture. This process can be improved for nitrides by adding low-melting or -vaporizing nitrogen containing compounds (like NH4Cl or LiNH2).10 Not only do these compounds act as a heat sink, but they can supply nitrogen to the reaction as well.

A final method for reducing a reaction temperature is by controlling the heat loss. In this way, these reactions can be effectively scaled up without producing destructive amounts of heat. This can be achieved by specifically designing the reaction vessel10 or by controlling the amount of heat produced by slow addition of precursors into the reactor. If a hotter reaction is desired, choose the starting materials carefully or begin these reactions at an elevated temperature.

In summary, solid-state metathesis (SSM) reactions have developed over the past two decades into an effective method for synthesizing materials that are difficult to make by conventional methods.31

back to top

Halides



Name Formula MW CAS MP BP Density at 25 °C Cat. No.
Aluminum chloride, 99.99% AlCl3 133.34 [7446-70-0] 190 °C   2.48 g/mL 449598-5G
449598-25G
Copper(II) fluoride, hydrate, 99.999% CuF2 · xH2O 101.54   785 °C 1676 °C 2.93 g/mL 401536-5G
401536-25G
Gallium(III) chloride, beads, –10 mesh, 99.999+% GaCI3 176.08 [13450-90-3] 78 °C 201 °C 2.47 g/mL 427128-5G
427128-25G
427128-100G
Gallium(III) iodide, 99.999% GaI3 450.43 [13450-91-4] 345 °C (subl.)   4.15 g/mL 429341-1G
429341-5G
Hafnium(IV) chloride, 98% HfCl4 320.3 [13499-05-3] 432 °C     258202-10G
258202-50G
Molybdenum(V) chloride, 95% MoCl5 273.21 [10241-05-1] 194 °C 268 °C 2.928 g/mL 208353-25G
208353-100G
Niobium(V) chloride, 99.999% NbCl5 270.17 [10026-12-7] 204.7 °C 254 °C 2.75 g/mL 510696-5G
510696-25G
Ammonium chloride, 99.998% NH4Cl 53.49 [12125-02-9] 340 °C (subl.)     254134-5G
254134-25G
254134-100G
Tantalum(V) chloride, 99.999% TaCl5 358.21 [7721-01-9] 210 °C 233 °C 3.68 g/mL 510688-5G
510688-25G
Tungsten(VI) chloride, 99.9+% WCl6 396.57 [13283-01-7] 275 °C 347 °C 3.52 g/mL 241911-10G
241911-100G
Zirconium(IV) chloride, 99.9+% ZrCl4 233.03 [10026-11-6]   331 °C 2.8 g/mL 357405-10G
357405-100G

back to top

Materials

     

References

  1. Gillan, E. G.; Kaner, R. B. J. Mater. Chem. 2001, 11, 1951.
  2. Wiley, J. B. et al. Mater. Res. Bull. 1993, 28, 893.
  3. Parkin, I. P.; Rowley, A. T. Polyhedron 1993, 12, 2961.
  4. Hector, A.; Parkin, I. P. Polyhedron 1993, 12, 1855.
  5. Hector, A.; Parkin, I. P. J. Mater. Sci. Lett. 1994, 13, 219.
  6. Mandal, T. K.; Gopalakrishnan, J. J. Mater. Chem. 2004, 14, 1273.
  7. Parhi, P. et al. Mater. Lett. 2004, 58, 3610.
  8. Bonneau, P. R. et al. Inorg. Chem. 1992, 31, 2127.
  9. Janes, R. A. et al. Inorg. Chem. 2003, 42, 2714.
  10. Cumberland, R. W. et al. J. Phys. Chem. B 2001, 105, 11922.
  11. O’Loughlin, J. L. et al. Inorg. Chem. 2001, 40, 2240.
  12. Wallace, C. H. et al. Appl. Phys. Lett. 1998, 72, 596.
  13. Blair, R. G. et al. Chem. Mater. 2005, 17, 2155.
  14. Shemkunas, M. P. et al. J. Am. Cer. Soc. 2002, 85, 101.
  15. Gibson, K. et al. Z. Anorg. Allg. Chem. 2003, 629, 1863.
  16. Jarvis, R. F., Jr. et al. Inorg. Chem. 2000, 39, 3243.
  17. Treece, R. E. et al. Inorg. Chem. 1994, 33, 5701.
  18. Rowley, A. T.; Parkin, I. P. J. Mater. Chem. 1993, 3, 689.
  19. Nartowski, A. M. et al. J. Mater. Chem. 1999, 9, 1275.
  20. Nartowski, A. M. et al. J. Mater. Chem. 2001, 11, 3116.
  21. Nartowski, A. M.; Parkin, I. P. Polyhedron 2002, 21, 187.
  22. Rao, L. et al. J. Mater. Res. 1995, 10, 353.
  23. Lupinetti, A. J. et al. Inorg. Chem. 2002, 41, 2316.
  24. Blair, R. G. et al. Chem. Mater. 2003, 15, 3286.
  25. O’Loughlin, J. L. et al. J. Phys. Chem. B 2001, 105, 1921.
  26. Ye, X. R. et al. Adv. Mater. 1999, 11, 941.
  27. McMillan, P. F. et al. J. Solid State Chem. 2005, 178, 937.
  28. Janes, R. A. et al. Chem. Mater. 2003, 15, 4431.
  29. Feng, J. et al. Wuji Huaxue Xuebao 2005, 21, 801.
  30. Parkin, I. P.; Nartowski, A. M. Polyhedron 1998, 17, 2617.
  31. Gillan, E. G.; Kaner, R. B. Chem. Mater. 1996, 8, 333.

back to top

Related Links