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.
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]
^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.
^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.
^
abGarner, 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.
ISSN0300-9246.
^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.
ISSN0075-4617.
^
abSchmeisser, 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.
ISSN0044-8249.
^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.
^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.
^
abCoombes, 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.
ISSN0300-9580.
^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.
ISBN9781566772174. 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.
doi:
10.1039/JR9490003135.
ISSN0368-1769.
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.
ISSN0022-1902.