Titanium(IV) nitrate
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Other names
titanium tetranitrate, tetranitratotitanium
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Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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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
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
Structure
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
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
Titanium nitrate is hygroscopic, converting to ill-defined hydrates.
It decomposes thermally to titanium dioxide.[17]
References
- .
- ^ "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.
- ^ ISSN 0300-9246.
- ISSN 0075-4617.
- ^ 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.
- ISBN 9780123526519. Retrieved 28 September 2014.
- .
- ISSN 0584-8539.
- ^ ISSN 0040-4039.
- ^ ISSN 0300-9580.
- ISBN 9780521233620. Retrieved 27 September 2014.
- ISBN 9781566772174. Retrieved 27 September 2014.
Other reading
- Partington, J. R.; A. L. Whynes (1949). "660. Reactions of nitrosyl chloride. Part II". Journal of the Chemical Society (Resumed): 3135. 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. ISSN 0022-1902.