Titanium nitrate
Not to be confused with Titanium nitride.
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| Names | |
|---|---|
| Other names
titanium tetranitrate, tetranitratotitanium | |
| Identifiers | |
12372-56-4  | |
| 3D model (Jmol) | Interactive image |
| ChemSpider | 8123716 |
| ECHA InfoCard | 100.222.601 |
| PubChem | 139314 |
| |
| |
| Properties | |
| Ti(NO3)4 | |
| Molar mass | 295.8866 g/mol |
| Appearance | white volatile solid |
| Density | 2.192 |
| Melting point | 58.5 °C (137.3 °F; 331.6 K) |
| Boiling point | decompose |
| carbon tetrachloride (0.1 mol/L at 10 °C).[1] | |
| Related compounds | |
| Related compounds |
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). | |
| Infobox references | |
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,[2][3] Ti(NO3)4 is prepared by the nitration of titanium tetrachloride using dinitrogen pentoxide:[4]
- TiCl4 + 4 N2O5 → Ti(NO3)4 + 4 ClNO2
A hydrated titanium nitrate is produced upon dissolution of titanium compounds in nitric acid.[5]
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.[7]
It is soluble in nonpolar solvents silicon tetrachloride and carbon tetrachloride.[8] or .[3]
Reactions
Titanium nitrate is hygroscopic, converting to ill-defined hydrates.[9] The anhydrous material is highly reactive, even toward hydrocarbons.[9] Titanium nitrate also reacts with n-dodecane,[1] p-dichlorobenzene, anisole, biphenyl,[1][10]
It decomposes thermally to titanium dioxide.[11]
References
- 1 2 3 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.
- ↑ 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.
- 1 2 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. 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.
- ↑ Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. p. 1331. ISBN 9780123526519. Retrieved 28 September 2014.
- ↑ 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.
- ↑ C. C. Addison, N. Logan, S. C. Wallwork and C. D. Garner, "Structural Aspects of Coordinated Nitrate Groups" Quart. Rev., Chem. Soc., 1971, volume 25, 289-322. 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.
- 1 2 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.
- ↑ 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
- 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.
| Salts and covalent derivatives of the Nitrate ion | |||||||||||||||||||
|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
| HNO3 | He | ||||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO3)4− | C | N | O | FNO3 | Ne | ||||||||||||
| NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si | P | S | ClONO2 | Ar | ||||||||||||
| KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)3 | Co(NO3)2, Co(NO3)3 |
Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | Br | Kr | ||
| RbNO3 | Sr(NO3)2 | Y | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb | Te | I | Xe(NO3)2 | ||
| CsNO3 | Ba(NO3)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(NO3)2, Hg(NO3)2 |
Tl(NO3)3 | Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |||
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(NO3)3, Ce(NO3)4 |
Pr | Nd | Pm | Sm | Eu | Gd(NO3)3 | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
| Ac | Th | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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