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Oxygen difluoride is a chemical compound with the formula OF 2. As predicted by VSEPR theory, the molecule adopts a bent molecular geometry. [citation needed] It is a strong oxidizer and has attracted attention in rocketry for this reason. [5] With a boiling point of −144.75 °C, OF 2 is the most volatile (isolable) triatomic compound. [6]
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 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 .
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]
The oxygen (0) atom is the root of hypofluorous acid's strength as an oxidizer, in contrast to the halogen (+1) atom in other hypohalic acids. This alters the acid's chemistry. Where reduction of a general hypohalous acid reduces the halogen atom and yields the corresponding elemental halogen gas,
It reacts vigorously with water to form ozone and oxygen difluoride, and with iodine or sulfur at room temperature. BiF 5 fluorinates paraffin oil (hydrocarbons) to fluorocarbons above 50 °C and oxidises UF 4 to UF 6 at 150 °C. At 180 °C, bismuth pentafluoride fluorinates Br 2 to BrF 3 and Cl 2 to ClF. [1]
Here are a few unexpected ways you can use salt and save a few bucks at the same time. But what most people don't realize is that salt can be used for a lot more than cooking.
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).