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Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and hydrofluoric acid containing small quantities of water. [7] [8] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide, with sodium fluoride as a side-product:
Oxygen difluoride. A common preparative method involves fluorination of sodium hydroxide: 2 F 2 + 2 NaOH → OF 2 + 2 NaF + H 2 O. OF 2 is a colorless gas at room temperature and a yellow liquid below 128 K. Oxygen difluoride has an irritating odor and is poisonous. [3] It reacts quantitatively with aqueous haloacids to give free halogens:
Dioxygen difluoride is a compound of fluorine and oxygen with the molecular formula O 2 F 2. It can exist as an orange-red colored solid which melts into a red liquid at −163 °C (110 K). It can exist as an orange-red colored solid which melts into a red liquid at −163 °C (110 K).
Compounds containing oxygen in other oxidation states are very uncommon: − 1 ⁄ 2 (superoxides), − 1 ⁄ 3 , 0 (elemental, hypofluorous acid), + 1 ⁄ 2 , +1 (dioxygen difluoride), and +2 (oxygen difluoride). Oxygen is reactive and will form oxides with all other elements except the noble gases helium, neon, argon and krypton. [1]
It is also the only hypohalous acid that can be isolated as a solid. HOF is an intermediate in the oxidation of water by fluorine, which produces hydrogen fluoride, oxygen difluoride, hydrogen peroxide, ozone and oxygen. HOF is explosive at room temperature, forming HF and O 2: [1] 2 HOF → 2 HF + O 2. This reaction is catalyzed by water. [2]
Unlike other hydrohalic acids, such as hydrochloric acid, hydrogen fluoride is only a weak acid in water solution, with acid dissociation constant (pK a) equal to 3.19. [36] HF's weakness as an aqueous acid is paradoxical considering how polar the HF bond is, much more so than the bond in HCl, HBr, or HI. The explanation for the behavior is ...
Calcium difluoride is a notable compound. In the form of the mineral fluorite it is the major source of commercial fluorine. It also has an eponymic crystal structure, which is an end member of the spectrum starting from bixbyite and progressing through pyrochlore .
Dioxygen monofluoride is a binary inorganic compound radical of fluorine and oxygen with the chemical formula O 2 F. [ 1 ] [ 2 ] [ 3 ] The compound is stable only at low temperature. This is one of many known oxygen fluorides .