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Titanium(II) oxide
Titanium(II) oxide
Titanium(II) oxide
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Titanium(II) oxide
Titanium(II) oxide
Titanium(II) oxide
Names
IUPAC name
Titanium(II) oxide
Other names
Titanium monoxide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.032.020 Edit this at Wikidata
EC Number
  • 235-236-5
  • InChI=1S/O.Ti/q-2;+2
    Key: VKRWBTVMYISSEF-UHFFFAOYSA-N
  • InChI=1S/O.Ti
    Key: OGIDPMRJRNCKJF-UHFFFAOYSA-N
  • [O-2].[Ti+2]
Properties
TiO
Molar mass 63.866 g/mol
Appearance bronze crystals
Density 4.95 g/cm3
Melting point 1,750 °C (3,180 °F; 2,020 K)
Structure
cubic
Hazards
Flash point Non-flammable
Related compounds
Titanium(III) oxide
Titanium(III,IV) oxide
Titanium(IV) oxide
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(II) oxide (TiO) is an inorganic chemical compound of titanium and oxygen. It can be prepared from titanium dioxide and titanium metal at 1500 °C.[1] It is non-stoichiometric in a range TiO0.7 to TiO1.3 and this is caused by vacancies of either Ti or O in the defect rock salt structure.[1] In pure TiO 15% of both Ti and O sites are vacant,[1] as the vacancies allow metal-metal bonding between adjacent Ti centres. Careful annealing can cause ordering of the vacancies producing a monoclinic form which has 5 TiO units in the primitive cell that exhibits lower resistivity.[2] A high temperature form with titanium atoms with trigonal prismatic coordination is also known.[3] Acid solutions of TiO are stable for a short time then decompose to give hydrogen:[1]

2 Ti2+(aq) + 2 H+(aq) → 2 Ti3+(aq) + H2(g)

Gas-phase TiO shows strong bands in the optical spectra of cool (M-type) stars.[4][5] In 2017, TiO was claimed to be detected in an exoplanet atmosphere for the first time; a result which is still debated in the literature.[6][7] Additionally, evidence has been obtained for the presence of the diatomic molecule TiO in the interstellar medium.[8]

References

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Titanium(II) oxide

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Titanium(II) oxide, chemical formula TiO, is an consisting of in the +2 bonded to oxygen, forming a non-stoichiometric metal with a defect rock salt (NaCl-type) crystal structure. This material exhibits metallic conductivity due to its partially filled titanium d-orbitals and is characterized by significant vacancies (approximately 15%) on both titanium and oxygen lattice sites, leading to a composition range from TiO0.7 to TiO1.3. It appears as or yellow cubic crystals and is highly stable thermally, with a around 1750 °C and a of 4.95 g/cm³. The physical and chemical properties of titanium(II) oxide make it distinct among titanium oxides; it is insoluble in , dilute acids, and organic solvents but soluble in concentrated , , and alkaline solutions. With a molecular weight of 63.87 g/mol and a cubic lattice parameter of approximately 4.18 (space group ), it displays slight ( χm = +88 × 10−6 emu) and can undergo semiconductor-to-metal transitions depending on composition.

Properties

Physical properties

Titanium(II) oxide (TiO) manifests as bronze-colored crystals, a characteristic appearance attributed to its metallic luster and composition. The compound exhibits a of 4.95 g/cm³ for the stoichiometric form, with slight variations possible due to non-stoichiometric compositions. Its is 63.866 g/mol, calculated from the atomic weights of titanium and oxygen. The material has a high of 1,750 °C, reflecting its thermal stability in solid form. It exhibits metallic conductivity due to partially filled d-orbitals. (II) oxide is non-flammable, consistent with the inert nature of lower oxides under standard conditions.

Chemical properties

(II) oxide, with the TiO, features in the +2 , where the metal balances the -2 charge of the anion. This compound represents one of the lower s accessible to , distinguishing it from more common higher-valent oxides like TiO₂. As a typical metal , titanium(II) acts as a basic anhydride, exhibiting reactivity toward acids by forming corresponding titanium salts and . This basic character arises from the ability of the oxide ion to accept protons, underscoring its role in acid-base chemistry within inorganic systems. It also dissolves in concentrated acids such as sulfuric and , reflecting its chemical affinity for proton donors. Titanium(II) oxide is inherently non-stoichiometric, stable across a composition range from approximately TiO_{0.8} to TiO_{1.3}, which accommodates deviations from ideal 1:1 Ti:O ratios without altering its fundamental rock-salt cubic framework. This variability influences its overall chemical behavior while maintaining the core +2 for in the stoichiometric limit.

Synthesis

Laboratory methods

Titanium(II) oxide is prepared in laboratory settings primarily through the direct solid-state reduction of with metallic . A stoichiometric of TiO₂ and Ti is heated to around 1500 °C in a high , yielding TiO via the reaction \ceTiO2+Ti−>2TiO\ce{TiO2 + Ti -> 2 TiO} This method produces the monoxide phase, with temperatures typically between 1400 and 1600 °C to ensure complete reaction while minimizing oxidation. The environment is critical to prevent atmospheric oxygen from reacting with the highly reactive titanium species and product. Alternative laboratory approaches for titanium suboxides, such as Magnéli phases (TiₙO₂ₙ₋₁), involve reducing TiO₂ with or carbon at high temperatures under inert or reducing atmospheres. These methods allow for controlled partial reduction but often require temperatures exceeding 1000 °C and extended reaction times. For TiO specifically, reduction of TiO₂ at 2000 °C and 130 atm can be used. Non-stoichiometric variants of TiO can be obtained by adjusting the Ti to TiO₂ ratio in the primary synthesis, leading to oxygen-deficient or excess structures depending on the conditions. Mechanochemical synthesis, involving milling of Ti and TiO₂ powders under argon followed by annealing in vacuum at 900–1000 °C, produces nanocrystalline TiO.

Industrial methods

Industrial production of titanium(II) oxide (TiO) is limited, as it is primarily synthesized in laboratories or for specialized applications. Methods for related titanium suboxides, such as Magnéli phases, include carbothermic reduction of titanium dioxide (TiO₂) feedstock with carbon, typically carbon black, at elevated temperatures ranging from 850°C to 1100°C under an inert atmosphere such as argon or vacuum. This process proceeds through a sequential reduction pathway, yielding intermediate Magnéli phases (TiₙO₂ₙ₋₁, where n=4–9), such as Ti₄O₇, with reaction efficiencies up to 98.5% when the carbon-to-TiO₂ ratio is precisely controlled to prevent over-reduction to titanium carbide. The method's scalability stems from its use of abundant TiO₂ precursors derived from ilmenite ores, making it viable for bulk production of suboxide powders employed in conductive materials and electrodes. Alternative large-scale approaches for suboxide powders utilize metal hydrides such as (TiH₂) or (CaH₂) to reduce TiO₂ at lower temperatures of 350–550°C, enabling the formation of nanostructured phases like Ti₄O₇ and Ti₂O₃ with reduced and improved purity for applications in . Plasma processes, particularly thermal plasma treatment of hydrogen titanate (H₂TiO₃), offer rapid synthesis of Magnéli phase nanoparticles (20–100 nm) under high-energy conditions, enhancing conductivity and facilitating continuous production lines for advanced ceramics.

Structure

Crystal structure

Titanium(II) oxide, in its stoichiometric form, adopts a cubic rock salt (NaCl-type) , characterized by a face-centered cubic lattice where titanium and oxygen atoms alternate along the edges. The is Fm\overline{3}m (No. 225), with each titanium atom octahedrally coordinated to six oxygen atoms and vice versa, forming a three-dimensional network of edge-sharing octahedra. The lattice parameter is approximately 4.18 , as determined from studies on near-stoichiometric samples. The ε-phase of TiO exhibits a hexagonal with P\overline{6}2m, where titanium atoms adopt trigonal prismatic coordination to oxygen atoms, differing from the octahedral arrangement in the rock salt phase. Unlike the defective rock salt phase, the ε-phase is vacancy-free. This variant features lattice parameters of a ≈ 4.99 Å and c ≈ 2.88 Å and represents a thermodynamically more stable configuration for stoichiometric TiO according to first-principles calculations, though it is synthesized under specific conditions such as using a bismuth flux. While the ideal structures provide the geometric foundation, actual TiO materials often deviate due to non-stoichiometry introduced by lattice defects.

Non-stoichiometry and defects

Titanium(II) oxide exhibits significant non-stoichiometry, with compositions ranging from TiO0.7_{0.7} to TiO1.3_{1.3}, arising from substantial vacancies on both titanium and oxygen lattice sites. In the stoichiometric TiO composition, these vacancies constitute about 15% of each sublattice, enabling a wide homogeneity region while preserving the overall rock salt framework. This defect concentration distinguishes TiO from ideal binary oxides, as the vacancies are intrinsic structural features rather than extrinsic impurities. The defect structure adopts a rock salt lattice with vacancies that can be either randomly distributed or ordered, influencing the material's and stability. At elevated temperatures above approximately 990°C, vacancies are randomly positioned, yielding a disordered cubic phase. Upon cooling below 950°C, vacancies order periodically, transforming the structure into a monoclinic form, such as Ti5_5O5_5 with C2/m, which reflects the adaptation to minimize strain from uneven vacancy distribution. This ordering is driven by thermodynamic favorability at lower temperatures, leading to reflections observable in . These structural defects profoundly affect electronic properties, imparting metallic conductivity to TiO across its composition range. The vacancies introduce defect states near the , facilitating delocalization and a residual resistivity component typical of metals, with temperature-dependent variations linked to vacancy-induced scattering. Off-stoichiometric compositions further modulate this behavior through imbalances in and oxygen vacancies, enhancing overall conductivity without transitioning to insulating states.

Reactivity

Reactions with acids

Titanium(II) oxide is insoluble in dilute acids but soluble in concentrated sulfuric acid and hydrofluoric acid. Although titanium oxides generally display amphoteric tendencies, the reactions of TiO with acids are influenced by its reducing nature stemming from the Ti^{2+} oxidation state.

Oxidation and stability

Titanium(II) oxide exhibits significant oxidative reactivity in air, particularly at elevated temperatures, where it readily converts to higher titanium oxides such as Ti₂O₃ and ultimately TiO₂. This process follows a stepwise oxidation mechanism, with low-valence titanium oxides like TiO being more susceptible to further oxidation than metallic titanium due to their lower thermodynamic stability. At temperatures below 900 °C, the primary oxidation products include TiO₂ along with minor amounts of intermediate phases like Ti₂O₃, driven by the availability of oxygen and the diffusion kinetics at the surface. The Gibbs free energy for these oxidation reactions remains negative across typical experimental temperatures, confirming the thermodynamic favorability of TiO oxidation in oxygen-rich environments. In aqueous environments, titanium(II) oxide demonstrates instability through oxidation processes that lead to the formation of higher oxides, primarily TiO₂. The compound is insoluble in . This reactivity is exacerbated in humid conditions, where adsorbed facilitates oxygen incorporation, promoting the transformation to more stable oxide phases over time. Titanium(II) oxide maintains thermal stability up to its of approximately 1,750 °C. This high reflects the strong Ti-O bonding in its rock-salt structure, allowing it to withstand extreme temperatures without significant phase changes or volatilization. Substoichiometric forms of titanium(II) oxide, such as those with compositions ranging from TiO_{0.7} to TiO_{1.25}, are inherently metastable due to their non-equilibrium defect structures, including oxygen vacancies and disordered lattices. These variants, often embedded in amorphous matrices or as thin films, exhibit kinetic barriers that prevent rapid transition to stoichiometric TiO or higher oxides, enabling temporary stability under specific synthesis conditions like high-temperature or . The metastability arises from the wide homogeneity range of the Ti-O system, where structural vacancies stabilize lower oxidation states, but exposure to oxidants or annealing induces rearrangement to more thermodynamically favorable phases.

Applications

Materials and electronic uses

Titanium(II) oxide finds applications in ceramics, glass manufacturing, and optic components due to its thermal stability and properties. It is also used in solid oxide fuel cells as a material, in oxygen generation systems, and in lightweight structural components for applications. Titanium(II) oxide (TiO) is utilized as an evaporation source for depositing high-quality (TiO₂) thin films via reactive evaporation processes. In this method, granular TiO is evaporated using an electron-beam evaporator under high vacuum (base pressure ~5×10⁻⁸ ) with the introduction of high-purity oxygen, forming stoichiometric TiO₂ films on substrates like SiO₂–Si(111) at substrate temperatures around 150 °C. The resulting films display grain sizes of 28–35 nm, high optical transparency, and an O/Ti ratio close to 2, making them suitable for optical applications such as Mo/Si multilayer mirrors in , as well as for optoelectronic devices and solar cells where low-temperature deposition is advantageous. Non-stoichiometric forms of TiO, expressed as TiO_{1+δ} (where δ > 0), enable the production of conductive thin films exhibiting low electrical resistivity due to their unique microstructure. These films typically have an average composition of TiO_{1.6} to TiO_{1.77}, consisting of cubic titanium monoxide (γ-TiO) grains embedded in an amorphous matrix; upon annealing at ~450 °C, they achieve conductivities up to 1000 S cm⁻¹ (corresponding to a resistivity of ~0.001 Ω cm), approaching metal-like behavior. This enhanced conductivity stems from internal forming metallic Ti nanocrystals, with defect-induced mechanisms such as oxygen vacancies promoting electron hopping and delocalization for potential use in transparent electrodes and sensors. Titanium suboxides, including TiO as a key component, find applications in energy devices and protective coatings owing to their metallic conductivity and . In lithium-sulfur batteries, suboxides like Ti₄O₇ act as efficient hosts, providing strong adsorption and high reversible capacity (e.g., via mesoporous structures with surface areas ~197 m² g⁻¹), thereby improving cycling performance and mitigating shuttle effects. For solar cells, TiO layers serve as optical spacers in devices, enhancing sunlight absorption and charge separation to boost power conversion efficiency. In anticorrosion coatings, suboxide integrations such as Ti₄O₇ offer superior durability, maintaining structural integrity in aggressive media like 1.0 M H₂SO₄ with projected half-lives exceeding 50 years. The incorporation of Magnéli phase titanium suboxides, which encompass structures related to TiO, significantly advances photocatalysis and electrocatalysis by leveraging their shear-plane defects for improved charge transport. In photocatalysis, phases like Ti₄O₇ integrate with anatase TiO₂ to mediate electron-hole separation, enabling cocatalyst-free hydrogen evolution rates up to 5432 μmol h⁻¹ g⁻¹ under UV-visible light and extending activity into the near-infrared spectrum via oxygen vacancies. For electrocatalysis, these phases support oxygen evolution reaction (OER) and hydrogen evolution reaction (HER) in water splitting, with Ti₄O₇-based electrodes delivering specific activities of ~1.50 mA cm⁻² and exceptional stability in acidic or basic conditions due to their high conductivity (~1000 S cm⁻¹) and oxygen evolution overpotential >2.5 V vs. SHE, positioning them as durable alternatives for wastewater remediation and fuel cell components.
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