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Hazard Predictions

• Generates heat: Exothermic reaction at ambient temperatures (releases heat)
• Intense or explosive reaction: Reaction may be particularly intense, violent, or explosive

The combination of very strong oxidizing agents and normally non-redox-active salts may result in exothermic oxidation-reduction reactions. Caution should be used before proceeding. Further research of comparable examples in the literature or very small scale, carefully controlled experiments may be needed to fully assess compatibility.

Chlorine trifluoride is a potent oxidizer and reacts violently with many metal oxides and some salts, including calcium oxide, magnesium oxide, manganese dioxide, aluminum oxide, arsenic trioxide, bismuth trioxide, chromic oxide, lanthanum oxide, lead dioxide, molybdenum trioxide, stannic oxide, tantalum pentoxide, tungsten trioxide, vanadium pentoxide, mercury iodide, and potassium iodide (Urben, P.G. 1995. Bretherick's Handbook of Reactive Chemical Hazards, 5th Edition. Oxford: Butterworth-Heinemann. Vol. 1, pp. 1237).

Oxygen difluoride reacts exothermically with aluminum oxide (alumina). This reaction can be explosive under certain conditions (e.g. confinement) (Streng, A. G., Chem. Eng. News, 1965, 43(12), 5).

Titanium dioxide is not easily oxidized under normal conditions (Swiler, D. R. 2005. Pigments, Inorganic. Kirk-Othmer Encyclopedia of Chemical Technology. (Online)).

Several metal oxides, including those of cobalt, iron, lead, manganese, mercury, and nickel, are active catalysts for the potentially explosive decomposition of hydrogen peroxide (Urben, P.G. 1995. Bretherick's Handbook of Reactive Chemical Hazards, 5th Edition. Oxford: Butterworth-Heinemann. Vol. 1, pp. 1531).