Nickel(II) titanate

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Nickel(II) titanate
Names
IUPAC name
Nickel(IV) titanate
Identifiers
12035-39-1
EC Number 234-825-4
Jmol 3D model Interactive image
PubChem 166728
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
Vapor pressure {{{value}}}
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Nickel(II) titanate is an inorganic compound with the chemical formula NiTiO3 [1] Nickel (II) Titanate, also known as Nickel Titanium Oxide, is a coordination compound between Nickel, Titanium and Oxygen ions. It has the appearance of a yellow powder. 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] Nickel (II) Titanate has been used as a catalyst for toluene oxidation.[2] The second method involved using enthalpy and entropy on the reaction to synthesize Nickel (II) TItanate through its phase transition.[3]

Molecular and Crystal Structure

Nickel (II) Titanate crystallizes at 600 °C[2] and is stable at room temperature and normal pressure in a Ilmenite structure with Rhombohedral R3 symmetry.[4] 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’ 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.[5] 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.[5] The structure was established by using X-ray power intensities.[4]

Synthesis

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 degrees C for 3 hours.[2]

Ti(OCH(CH3)2)4 + Ni(NO3)2(6H2O) + 20 C3H7NO2 + C3H8O → NiTiO3

Nickel (II) Titanate was also formed by heating NiO and TiO2 at 1350 degrees C for three hours. Then it was then cooled until room temperature.[3]

NiO + TiO2 + (heat) → NiTO3

Applications

Due to Nickel (II) Titanate’s brilliant yellow color and high UV-vis-NIR reflectance have had 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; Nickel(II) titanate; Nickelous; oxygen(-2) anion; titanium(+4) cation; Nickel-titanate; 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.[5]

By doping the NiTiO3 with Ga2O3, the anomalous increase of the electrical conductivity is shifted to lower temperatures.[3]

It is used as a yellow pigment.

References

  1. ↑ University of Akron Chemical Database
  2. ↑ 2.0 2.1 2.2 2.3 2.4 2.5 2.6 2.7 Lua error in package.lua at line 80: module 'strict' not found.
  3. ↑ 3.0 3.1 3.2 Lua error in package.lua at line 80: module 'strict' not found.
  4. ↑ 4.0 4.1 Lua error in package.lua at line 80: module 'strict' not found.
  5. ↑ 5.0 5.1 5.2 Lua error in package.lua at line 80: module 'strict' not found.
  6. ↑ 6.0 6.1 6.2 Lua error in package.lua at line 80: module 'strict' not found.
  7. ↑ Lua error in package.lua at line 80: module 'strict' not found.
  8. ↑ Lua error in package.lua at line 80: module 'strict' not found.


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