Hexaperchloratoaluminate
The hexaperchloratoaluminate ion is a polyatomic anion with the chemical formula [Al(ClO4)6]3−. It is composed of six perchlorate (ClO−4) anions bound to a central aluminium ion (Al3+), resulting in a net charge of –3. This ion is a highly oxidizing and reactive complex, similar to other hexacoordinate aluminium complexes such as hexanitratoaluminate.
The aluminium perchlorate salts formed with hexaperchloratoaluminate are of particular interest due to their potential uses as energetic materials. The series of hexaperchloratoaluminate salts includes lithium hexaperchloratoaluminate, ammonium hexaperchloratoaluminate, tetramethylammonium hexaperchloratoaluminate, and trinitronium hexaperchloratoaluminate. Each of these compounds possess unique properties and may have potential applications in areas such as rocket propellants, pyrotechnics, and other explosive-based technologies.[1]
Preparation
Hexaperchloratoaluminates can be synthesized by combining aluminum trichloride and various perchlorates in liquid sulfur dioxide at a temperature of –10°C:[1]
- 3 [NO2]ClO4 + 3 LiClO4 + AlCl3 → 3 NO2Cl + Li3[Al(ClO4)6],
- 3 [NO2]ClO4 + 3 [NH4]ClO4 + AlCl3 → 3 NO2Cl + [NH4]3[Al(ClO4)6],
- 6 [NO2]ClO4 + AlCl3 → 3 NO2Cl + [NO2]3[Al(ClO4)6].
To form hexaperchloratoaluminates, one can heat aluminium nitrate in the presence of nitrosonium or nitronium perchlorate at a temperature of 125 °C: [1]
- 10–14 [NO]ClO4 + Al(NO3)3 → [NO2]3[Al(ClO4)6] + (gaseous products),
- 6–10 [NO2]ClO4 + Al(NO3)3 → [NO2]3[Al(ClO4)6] + (gaseous products),
- 3 [NO2]ClO4 + 3 KClO4 + AlCl3 → 3 NO2Cl + K3[Al(ClO4)6].
Obtaining hydrazinium hexaperchloratoaluminate in a highly pure form is problematic. According to the available studies, this compound can only be produced via a low-yielding synthesis route including the reaction of aluminium chloride, hydrazinium perchlorate, and nitronium perchlorate:[1]
- 3 [NO2]ClO4 + 3 [N2H5]ClO4 + AlCl3 → 3 NO2Cl + [N2H5]3[Al(ClO4)6].
Guanidinium hexaperchloratoaluminate can be synthesized via the following reaction:[1]
- 3 [NO2]ClO4 + 3 [C(NH2)3]ClO4 + AlCl3 → 3 NO2Cl + [C(NH2)3]3[Al(ClO4)6].
References
- ^ a b c d e Guibert, C. R.; A. D. McElroy (10 Feb 1964). "Annual Report Studies of Complex Perchlorates". Callery Chemical Company. pp. 5–7. Archived from the original on March 3, 2016. Retrieved 3 October 2014.
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Salts and covalent derivatives of the perchlorate ion
| HClO4 | He | ||||||||||||||||||||
| LiClO4 | Be(ClO4)2 | B(ClO4)−4 B(ClO4)3 | ROClO3 | N(ClO4)3 NH4ClO4 NOClO4 NO2ClO4 | H3OClO4 | FClO4 | Ne | ||||||||||||||
| NaClO4 | Mg(ClO4)2 | Al(ClO4)3 Al(ClO4)−4 Al(ClO4)2−5 Al(ClO4)3−6 | Si | P | S | ClO−4 ClOClO3 Cl2O7 | Ar | ||||||||||||||
| KClO4 | Ca(ClO4)2 | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3 VO2(ClO4) | Cr(ClO4)3 | Mn(ClO4)2 | Fe(ClO4)2 Fe(ClO4)3 | Co(ClO4)2 Co(ClO4)3 | Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge | As | Se | BrOClO3 | Kr | ||||
| RbClO4 | Sr(ClO4)2 | Y(ClO4)3 | Zr(ClO4)4 | Nb(ClO4)5 | MoO2(ClO4)2 | Tc | Ru | Rh(ClO4)3 | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In(ClO4)3 | Sn(ClO4)4 | Sb(ClO4)3 | TeO(ClO4)2 | I(OClO3)3 | Xe(OClO3)2 | ||||
| CsClO4 | Ba(ClO4)2 | * | Lu(ClO4)3 | Hf(ClO4)4 | Ta(ClO4)5 TaO(ClO4)3 TaO2ClO4 | WO(ClO4)4 | ReO3ClO4 | Os | Ir | Pt | Au(ClO4)−4 | Hg2(ClO4)2 Hg(ClO4)2 | Tl(ClO4) Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po | At | Rn | |||
| FrClO4 | Ra | ** | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| * | La(ClO4)3 | Ce(ClO4)x | Pr(ClO4)3 | Nd(ClO4)3 | Pm | Sm(ClO4)3 | Eu(ClO4)3 | Gd(ClO4)3 | Tb(ClO4)3 | Dy(ClO4)3 | Ho(ClO4)3 | Er(ClO4)3 | Tm(ClO4)3 | Yb(ClO4)3 | |||||||
| ** | Ac | Th(ClO4)4 | Pa | UO2(ClO4)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | |||||||
