Chemistry:Titanium perchlorate
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3D model (JSmol)
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| Properties | |
| Ti(ClO4)4 | |
| Molar mass | 445.65 g·mol−1 |
| Appearance | white crystals, deliquescent |
| Density | 2.49 g/cm3 (anhydrous) |
| Melting point | 85 °C (185 °F; 358 K) (anhydrous) slight decomposition |
| Boiling point | decomposition |
| high | |
| Related compounds | |
Other anions
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Titanium nitrate |
Other cations
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Zirconium perchlorate Hafnium perchlorate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Titanium perchlorate, or more precisely titanium(IV) perchlorate, is a molecular compound of titanium and perchlorate groups with formula Ti(ClO4)4. Anhydrous titanium perchlorate decomposes explosively at 130 °C and melts at 85 °C with a slight decomposition. It sublimes in a vacuum as low as 70 °C. Being a molecular with four perchlorate ligands, it is an unusual example of a transition metal perchlorate complex.
Properties
packing of Ti(ClO
4)
4 molecules in the crystal.
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In Ti(ClO4)4, the four perchlorate groups binds as bidentate ligands. Thus the Ti center is bound to eight oxygen atoms.[2] So the molecule could also be called tetrakis(perchlorato-O,O')titanium(IV).[3]
In the solid form it forms monoclinic crystals, with unit cell parameters a=12.451 b=7.814 c=12.826 Å α=108.13. Unit cell volume is 1186 Å3 at -100 °C. There are four molecules per unit cell.[1]
It reacts with petrolatum, nitromethane, acetonitrile, dimethylformamide, and over 25° with carbon tetrachloride.[2]
Titanyl perchlorate form solvates with water, dimethyl sulfoxide, dioxane, pyridine-N-oxide, and quinoline-N-oxide.[2]
Thermolysis of titanium perchlorate gives TiO2, ClO2 and dioxygen O2 The titanyl species TiO(ClO4)2 is an intermediate in this decomposition.[2]
- Ti(ClO4)4 → TiO2 + 4ClO2 + 3O2 ΔH = +6 kcal/mol (25 kJ/mol).[2]
Formation
Titanium perchlorate can be formed by reacting titanium tetrachloride with perchloric acid enriched in dichlorine heptoxide.[2] Another way uses titanium tetrachloride with dichlorine hexoxide. This forms a complex with Cl2O6 which when warmed to 55° in a vacuum, sublimes and can crystallise the pure anhydrous product from the vapour.[1]
Related
In the salt dicaesium hexaperchloratotitanate, Cs2Ti(ClO4)6 the perchlorate groups are monodentate, connected by one oxygen to titanium.[4]
Titanium perchlorate can also form complexes with other ligands bound to the titanium atom including binol,[5] and gluconic acid.[6]
A polymeric oxychlorperchlorato compound of titanium, Ti6O4Clx(ClO4)16−x, is made from excess TiCl4 and dichlorine hexoxide. This has a varying composition, and ranges from light to dark yellow.[7]
References
- ↑ 1.0 1.1 1.2 Fourati, Mohieddine; Chaabouni, Moncef; Belin, Claude Henri; Charbonnel, Monique; Pascal, Jean Louis; Potier, Jacqueline (April 1986). "A strongly chelating bidentate perchlorate. New synthesis route and crystal structure determination of titanium(4+) perchlorate". Inorganic Chemistry 25 (9): 1386–1390. doi:10.1021/ic00229a019.
- ↑ 2.0 2.1 2.2 2.3 2.4 2.5 Babaeva, V. P.; Rosolovskii, V. (1974). "Volatile titanium perchlorate". Bulletin of the Academy of Sciences of the USSR Division of Chemical Science 23 (11): 2330–2334. doi:10.1007/BF00922105. ISSN 0568-5230.
- ↑ Macintyre, Jane E. (1992) (in en). Dictionary of Inorganic Compounds. CRC Press. p. 2963. ISBN 9780412301209. https://books.google.com/books?id=9eJvoNCSCRMC&pg=PA2963.
- ↑ Babaeva, V. P.; Rosolovskii, V. Ya. (November 1975). "Production of cesium hexaperchloratotitanate by the reaction of titanium perchlorate with cesium perchlorate". Bulletin of the Academy of Sciences of the USSR Division of Chemical Science 24 (11): 2278–2281. doi:10.1007/BF00921631.
- ↑ Mikami, Koichi; Sawa, Eiji; Terada, Masahiro (January 1991). "Asymmetric catalysis by chiral titanium perchlorate for carbonyl-ene cyclization". Tetrahedron: Asymmetry 2 (12): 1403–1412. doi:10.1016/S0957-4166(00)80036-1.
- ↑ Guthrie, R. D. (1970) (in en). Carbohydrate Chemistry. 3. London: Royal Society of Chemistry. p. 144. ISBN 9780851860220. https://books.google.com/books?id=d1SUAE2qD80C&pg=PA144.
- ↑ Fourati, M.; Chaabouni, M.; Pascal, J.L.; Potter, J. (March 1986). "Synthesis and vibrational analysis of new anhydrous oxochloroperchlorato complexes of titanium IV". Journal of Molecular Structure 143 (1–2): 147–150. doi:10.1016/0022-2860(86)85225-5. Bibcode: 1986JMoSt.143..147F.
Compounds containing perchlorate group
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| HClO4 | He | ||||||||||||||||||
| LiClO4 | Be(ClO4)2 | B(ClO4)−4 B(ClO4)3 |
ROClO3 | N(ClO4)3 NH4ClO4 NOClO4 |
O | FClO4 | Ne | ||||||||||||
| NaClO4 | Mg(ClO4)2 | Al(ClO4)3 | 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)3 | Co(ClO4)2, Co(ClO4)3 |
Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge | As | Se | Br | Kr | ||
| RbClO4 | Sr(ClO4)2 | Y(ClO4)3 | Zr(ClO4)4 | Nb(ClO5)4 | Mo | Tc | Ru | Rh(ClO4)3 | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In(ClO4)3 | Sn(ClO4)4 | Sb | TeO(ClO4)2 | I | Xe | ||
| CsClO4 | Ba(ClO4)2 | Hf(ClO4)4 | Ta(ClO5)5 | W | Re | Os | Ir | Pt | Au | Hg2(ClO4)2, Hg(ClO4)2 |
Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po | At | Rn | |||
| FrClO4 | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(ClO4)x | Pr | Nd | 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 | Lu(ClO4)3 | |||||
| Ac | Th(ClO4)4 | Pa | UO2(ClO4)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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