Nickel(II) titanate
Names
IUPAC name
Nickel(IV) titanate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.031.647 Edit this at Wikidata
EC Number
  • 234-825-4
RTECS number
  • QS0635000
  • InChI=1S/Ni.3O.Ti/q+2;3*-2;+4
    Key: KJLFZWJDCDJCFB-UHFFFAOYSA-N
  • [O-2].[O-2].[O-2].[Ti+4].[Ni+2]
Properties
NiTiO3
Molar mass 154.61 g/mol
Appearance yellow powder
Density 4.44 g/cm3
0.0396 g/100 mL
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nickel(II) titanate, also known as nickel titanium oxide, is an inorganic compound with the chemical formula NiTiO3.[1] It is a coordination compound between nickel(II), titanium(IV) and oxide ions. It has the appearance of a yellow powder. Nickel(II) titanate has been used as a catalyst for toluene oxidation.[2]

Molecular and crystal structure

Nickel(II) titanate crystallizes at 600 °C[2] and is stable at room temperature and normal pressure in an ilmenite structure with rhombohedral R3 symmetry.[3] Nickel(II) titanate's rhombohedral structure has layers of Ni and Ti alternate along the rhombohedral axis with O layers between them. The XRD data supports nickel(II) titanate's ilmenite structure with its rhombohedral symmetry.[2] Other descriptions of nickel(II) titanite's Illemite structure consists of a pseudo close packed hexagonal array of O2− ions with two thirds occupied by an ordered hexagonal like cation.[4] The Average crystallites size for nickel(II) titanate was estimated at 42 nm with lattice constants of a = 5.032 Å, b = 5.032 Å, c = 4.753 Å.[4] The structure was established by using X-ray power intensities.[3]

Synthesis

There are several methods of synthesis for nickel(II) titanate. The first method involves nickel(II) titanate's melting temperature of over 500 °C at which its precursor decomposes to give nickel(II) titanate as a residue.[2] The second method involved using enthalpy and entropy on the reaction to synthesize nickel(II) titanate through its phase transition.[5]

Nickel(II) titanate was synthesized using the polymeric precursor method. This involved spontaneous combustion of Ti(OCH(CH3)2)4 with Ni(NO3)2·6H2O and C3H7NO2 in a molar ratio of 1:1:20 in isopropyl alcohol solution.[2] The product of nickel(II) titanate was calcinated from the precursor at 600 °C for 3 hours.[2]

Nickel(II) titanate was also formed by heating NiO and TiO2 at 1350 °C for three hours. Then it was then cooled until room temperature.[5]

NiO + TiO2 + (heat) → NiTiO3

Applications

Due to nickel(II) titanate's brilliant yellow color and high UV-vis-NIR reflectance, it has the potential to serve as a pigment for building coating. Ilmenite-type NiTiO3 are well known as functional inorganic materials with wide application in electronic materials, including electrodes of solid fuel cells, gas sensors, chemical catalysts and so on due to their high static dielectric constants, weak magnetism and semiconductivity.[6] NiTiO3 as a semiconductor has excellent catalytic activity due to its absorption bands.[6] Analysis of the band structures and density of states have implied that nickel(II) titanate has immense potential in the areas of high-density data storage, gas sensor data and integration in circuit devices.[6] NiTiO3 has even been utilized as a catalyst in toluene oxidation.[2] Other applications of nickel(II) titanate have yet to be found.

Interesting facts about compound in History

MTiO3 (M= Ni, Fe, Mn) compounds have received attention as possible candidates for multiferroic materials capable of magnetization through application of electric field.[7]

Nickel(II) titanate furthermore has many different names such as nickel titanium oxide; nickelous; titanium nickel oxide; nickel titanium trioxide.[8]

Through an experiment to see if NiTiO3 could serve as a catalyst for toluene oxidation in comparison to NiFe2O4, NiTiO3 achieved greater results than its experimental counterpart in oxidating toluene.[2]

A single-source heterobimetallic complex Ni2Ti2(OEt)2(μ-OEt)6(2,4-pentanedionate)4 was synthesized and underwent thermal decomposition at 500 °C to give NiTiO3 residue.[4]

By doping the NiTiO3 with Ga2O3, the anomalous increase of the electrical conductivity is shifted to lower temperatures.[5]

It is used as a yellow pigment.

References

  1. ^ University of Akron Chemical Database
  2. ^ a b c d e f g h Traistaru, G.A. (July 2011). "Synthesis and Characterization of NiTiO3 and NiFe2O4 as catalysts for Toluene Oxidation" (PDF). Digest Journal of Nanomaterials and Biostructures.
  3. ^ a b Shirane, Gen; Pickart, S. J.; Ishikawa, Yoshikazu (1959-10-15). "Neutron Diffraction Study of Antiferromagnetic MnTiO3 and NiTiO3". Journal of the Physical Society of Japan. 14 (10): 1352–1360. Bibcode:1959JPSJ...14.1352S. doi:10.1143/JPSJ.14.1352. ISSN 0031-9015.
  4. ^ a b c Tahir, Asif Ali; Mazhar, Muhammad; Hamid, Mazhar; Wijayantha, K.G. Upul; Molloy, Kieran C. (2009-05-06). "Photooxidation of water by NiTiO3 deposited from single source precursor [Ni2Ti2(OEt)2(μ-OEt)6(acac)4] by AACVD". Dalton Transactions (19): 3674–3680. doi:10.1039/B818765G. ISSN 1477-9234. PMID 19417932.
  5. ^ a b c Lerch, M.; Laqua, W. (1992-04-01). "Beiträge zu den Eigenschaften von Titanaten mit Ilmenitstruktur. II. Zur Thermodynamik und elektrischen Leitfähigkeit von NiTiO3 und anderen oxidischen Phasen mit Ilmenitstruktur". Zeitschrift für Anorganische und Allgemeine Chemie. 610 (4): 57–63. doi:10.1002/zaac.19926100110. ISSN 1521-3749.
  6. ^ a b c Zhang, Xiaochao; Lu, Bingqian; Li, Rui; Fan, Caimei; Liang, Zhenhai; Han, Peide (2015-11-01). "Structural, electronic and optical properties of Ilmenite ATiO3 (A=Fe, Co, Ni)". Materials Science in Semiconductor Processing. 39: 6–16. doi:10.1016/j.mssp.2015.04.041.
  7. ^ Varga, Tamas; Droubay, Timothy C.; Bowden, Mark E.; Nachimuthu, Ponnusamy; Shutthanandan, Vaithiyalingam; Bolin, Trudy B.; Shelton, William A.; Chambers, Scott A. (2012-06-30). "Epitaxial growth of NiTiO3 with a distorted ilmenite structure". Thin Solid Films. 520 (17): 5534–5541. Bibcode:2012TSF...520.5534V. doi:10.1016/j.tsf.2012.04.060.
  8. ^ Pubchem. "Nickel titanium oxide | NiO3Ti - PubChem". pubchem.ncbi.nlm.nih.gov. Retrieved 2016-04-29.
source: http://en.wikipedia.org/wiki/Nickel(II)_titanate