WS₂’s chemical properties reflect its stability and inertness, typical of transition metal dichalcogenides. It consists of tungsten in the +4 oxidation state bonded covalently to two sulfur atoms (-2 each), forming a layered hexagonal lattice with weak interlayer van der Waals forces. Chemically, WS₂ is largely inert at room temperature, resisting reaction with water, alcohols, dilute acids (e.g., HCl), and most organic solvents, making it suitable for harsh environments.
In air, WS₂ is stable up to 510°C, beyond which it oxidizes: WS₂ + 7/2 O₂ → WO₃ + 2 SO₂. This reaction is slow below 400°C, allowing practical use in moderate heat. In inert conditions, it withstands 1250°C before decomposing to W and S₂. WS₂ resists bases like NaOH at room temperature but reacts with molten alkalis (e.g., NaOH at 500°C), forming tungstates (e.g., Na₂WO₄) and sulfides. Strong oxidizing agents like aqua regia (HNO₃ + HCl) attack it slowly, producing WO₃ and H₂S, though it’s less reactive than MoS₂.
Its inertness stems from saturated W-S bonds and a lack of reactive sites, unlike metals prone to corrosion. WS₂’s hydrophobicity repels water, aiding stability in humid conditions, though prolonged exposure to strong acids or oxidants degrades it over time. In catalysis, WS₂’s sulfur edges can be active (e.g., hydrodesulfurization), but bulk material is unreactive. These properties suit it for lubricants, coatings, and electronics where chemical durability is key.
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