Titanium(IV) nitrate
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| Names | |
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| Other names
titanium tetranitrate, tetranitratotitanium
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.222.601 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Ti(NO3)4 | |
| Molar mass | 295.8866 g/mol |
| Appearance | white volatile solid |
| Density | 2.192[3] |
| Melting point | 58[4] °C (136 °F; 331 K) |
| Boiling point | decompose |
| Reacts[5] | |
| Structure[6] | |
| monoclinic | |
| P21/C | |
a = 7.80, b = 13.57, c = 10.34 Å α = 90°, β = 125·0°, γ = 90°
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Lattice volume (V)
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896.52 Å3 |
Formula units (Z)
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4 |
| 8 | |
| flattened tetrahedral | |
| Related compounds | |
Related compounds
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hafnium nitrate, zirconium nitrate, titanium phosphate, titanium perchlorate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Titanium nitrate is the inorganic compound with formula Ti(NO3)4. It is a colorless, diamagnetic solid that sublimes readily. It is an unusual example of a volatile binary transition metal nitrate. Ill defined species called titanium nitrate are produced upon dissolution of titanium or its oxides in nitric acid.
Preparation
[edit]Similarly to its original method,[7][8] Ti(NO3)4 is prepared by the nitration of titanium tetrachloride using dinitrogen pentoxide[9] or chlorine nitrate:[10]
- TiCl4 + 4 N2O5 → Ti(NO3)4 + 4 ClNO2
Hydrated titanium nitrate, the nitrate salt of the aquo complex [Ti(H2O)6]3+, is produced upon dissolution of titanium compounds in nitric acid.[11]
Structure
[edit]The complex has D2d symmetry, with four bidentate nitrate ligands. The N-O distances are 1·29 Å and 1·185 Å (noncoordinated).[6]
Physical properties
[edit]In the infrared spectrum, it absorbs strongly at 1635 cm−1, assigned to a N-O vibrational mode.[12]
It is soluble in nonpolar solvents silicon tetrachloride and carbon tetrachloride.[13][8]
Reactions
[edit]Titanium nitrate is hygroscopic, converting to ill-defined hydrates.[14] The anhydrous material is highly reactive, even toward hydrocarbons.[14] Titanium nitrate also reacts with n-dodecane,[15] p-dichlorobenzene, anisole, biphenyl,[15][16]
It decomposes thermally to titanium dioxide.[17]
References
[edit]- ^ Garner, C. D.; Wallwork, S. C. (1966). "The crystal structures of anhydrous nitrates and their complexes. Part III. Titanium(IV) nitrate". J. Chem. Soc. A: 1496–1500. doi:10.1039/J19660001496.
- ^ "ICSD 26639 : ICSD Structure : N4 O12 Ti". Cambridge Structural Database: Access Structures. Cambridge Crystallographic Data Centre. Retrieved 2021-05-08.
- ^ "Titanium(iv) nitrate (Ti(NO3)4)". Retrieved 27 September 2014.
- ^ Chemistry of the Elements (Second Edition). N. N. Greenwood and A. Earnshaw. P966. 21.3.4 Compounds with oxoanions
- ^ Nathaniel Howell Furman; R. J. Mundy; G. H. Morrison (1955). The Distribution of Uranyl Nitrate from Aqueous Solutions to Diethyl Ether. the University of Michigan: U.S. Atomic Energy Commission. Technical Information Service. p. 51.
- ^ a b Garner, C. David; Ian H. Hillier; Martyn F. Guest (1975). "Ab initio self-consistent field molecular-orbital calculation of the ground state of tetranitratotitanium(IV); comments on the reactivity of anhydrous metal nitrates". Journal of the Chemical Society, Dalton Transactions (19): 1934. doi:10.1039/DT9750001934. ISSN 0300-9246.
- ^ Reihlen, Hans; Andreas Hake (1927). "Über die Konstitution des N2O4 und N2O3 und die Additionsverbindungen von Nitro- und Nitrosokörpern an Zinn- und Titantetrachlorid". Justus Liebig's Annalen der Chemie (in German). 452 (1): 47–67. doi:10.1002/jlac.19274520104. ISSN 0075-4617.
- ^ a b Schmeisser, Martin (1955). "Die Chemie der anorganischen Acylnitrate (ein Problem des Nitrylchlorids) und Acylperchlorate (ein Problem des Dichlorhexoxyds)". Angewandte Chemie (in German). 67 (17–18): 493–501. Bibcode:1955AngCh..67..493S. doi:10.1002/ange.19550671708. ISSN 0044-8249.
- ^ P. Ehrlich "Titanium Tetranitrate" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1237.
- ^ Schmeisser, M.; Brandle, K. Acyl nitrates and perchlorates. IV. ClNO3 as starting material for acyl nitrates. Angewandte Chemie, 1957. 69: 781. ISSN: 0044-8249.
- ^ Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 1331. ISBN 9780123526519. Retrieved 28 September 2014.
- ^ Addison, C. C.; Logan, N.; Wallwork, S. C.; Garner, C. D. (1971). "Structural Aspects of Co-ordinated Nitrate Groups". Quarterly Reviews, Chemical Society. 25 (2): 289. doi:10.1039/qr9712500289.
- ^ Amos, D.W.; G.W. Flewett (1974). "Raman spectra of titanium (IV) and tin (IV) nitrates". Spectrochimica Acta Part A: Molecular Spectroscopy. 30 (2): 453–461. Bibcode:1974AcSpA..30..453A. doi:10.1016/0584-8539(74)80085-1. ISSN 0584-8539.
- ^ a b Amos, D.W.; D.A. Baines, G.W. Flewett (1973). "Nitration by titanium (IV) nitrate". Tetrahedron Letters. 14 (34): 3191–3194. doi:10.1016/S0040-4039(00)79808-X. ISSN 0040-4039.
- ^ a b Coombes, Robert G.; Leslie W. Russell (1974). "Nitration of aromatic compounds by tetranitratotitanium(IV) in carbon tetrachloride solution". Journal of the Chemical Society, Perkin Transactions 2 (7): 830. doi:10.1039/P29740000830. ISSN 0300-9580.
- ^ Schofield, Kenneth (1980). Aromatic Nitration. CUP Archive. pp. 97–98. ISBN 9780521233620. Retrieved 27 September 2014.
- ^ Allendorf, Mark Donald (1999-01-01). "Titanium Oxide CVD from Titanium (IV) Nitrate ...". Proceedings of the Symposium on Fundamental Gas-Phase and Surface Chemistry of Vapor-Phase Materials Synthesis. The Electrochemical Society. pp. 395–397. ISBN 9781566772174. Retrieved 27 September 2014.
Other reading
[edit]- Partington, J. R.; A. L. Whynes (1949). "660. Reactions of nitrosyl chloride. Part II". Journal of the Chemical Society (Resumed): 3135. doi:10.1039/JR9490003135. ISSN 0368-1769.
- Dauerman, L.; G.E. Salser (1973). "Mass spectra of covalent inorganic nitrates: copper(II) nitrate and titanium(IV) nitrate". Journal of Inorganic and Nuclear Chemistry. 35 (1): 304–306. doi:10.1016/0022-1902(73)80643-8. ISSN 0022-1902.