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Dioxygen difluoride can be obtained by subjecting a 1:1 mixture of gaseous fluorine and oxygen at low pressure (7–17 mmHg (0.9–2.3 kPa) is optimal) to an electric discharge of 25–30 mA at 2.1–2.4 kV. [3] A similar method was used for the first synthesis by Otto Ruff in 1933. [4] Another synthesis involves mixing O.
Oxygen difluoride is a chemical compound with the formula OF2. As predicted by VSEPR theory, the molecule adopts a bent molecular geometry. 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:
The dioxygenases (EC 1.13.11) catalyze the oxidation of a substrate without the reduction of one oxygen atom from dioxygen into a water molecule. However, this definition is ambiguous because it does not take into account how many substrates are involved in the reaction. The majority of dioxygenases fully incorporate dioxygen into a single ...
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Dioxygen monofluoride is a binary inorganic compound radical of fluorine and oxygen with the chemical formula O2F. [ 1][ 2][ 3] The compound is stable only at low temperature. This is one of many known oxygen fluorides.
The dioxygenyl ion, O+. 2, is a rarely-encountered oxycation in which both oxygen atoms have a formal oxidation state of + 1 2 . It is formally derived from oxygen by the removal of an electron: O 2 → O+. 2 + e −. The energy change for this process is called the ionization energy of the oxygen molecule.
Alex G. Streng was an experimental chemist, notable for his work with fluorine compounds. [1] [2] His work on the synthesis and properties of dioxygen difluoride, published in 1963 in the Journal of the American Chemical Society, is notorious for Streng's willingness to push the limits of experimental endeavour with this highly reactive and dangerous material.
Oxygen compounds. Water (H 2 O) is the most familiar oxygen compound. The oxidation state of oxygen is −2 in almost all known compounds of oxygen. The oxidation state −1 is found in a few compounds such as peroxides. Compounds containing oxygen in other oxidation states are very uncommon: − 1⁄2 (superoxides), − 1⁄3 (ozonides), 0 ...