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Dioxygen difluoride

Oxygen. Oxygen does not react directly with fluorine under ordinary conditions, although ia addition to oxygen difluoride, three other oxygen fluorides are known (29). Dioxygen difluoride [7783-44-0] 2 2 difluoride [16829-28-0] 3 2 tetraoxygen difluoride [12020-93-8] 4 2 ... [Pg.124]

Dioxygen difluoride, O2F2, is best prepared by passing a silent electric discharge through a low-pressure mixture of F2 and O2 the products obtained depend markedly on conditions, and the... [Pg.639]

Chromyl chloride Organic solvents Dioxygen difluoride Various materials Fluorine nitrate Organic materials... [Pg.342]

See Dioxygen difluoride Various materials Disilyl oxide... [Pg.1405]

This material is now considered to be an equimolar mixture of dioxygen difluoride and tetraoxygen difluoride, rather than the title species. [Pg.1527]

Mixtures with dioxygen difluoride explode at —148° C, and with dioxygen triflu-oride (probably mixed dioxygen di- and tetra-fluorides) at — 183°C. [Pg.1871]

Dioxygen difluoride, 02F2, is a yellow-orange solid with a melting point of —163 °C. The structure of the molecule is... [Pg.557]

Bromine bromate, 0276 Bromine dioxide, 0258 Bromine perchlorate, 0235 Bromine trioxide, 0259 Bromyl fluoride, 0239 Chlorine dioxide, 4042 Chlorine perchlorate, 4101 Chlorine trifluoride oxide, 3982 Chlorine trioxide, 4044 Chloryl hypofluorite, 3973 Chloryl perchlorate, 4104 Dichlorine oxide, 4095 Dichlorine trioxide, 4100 Dicyanogen AW -dioxidc. 0998 Dioxygen difluoride, 4320 Fluorine perchlorate, 3976 Hexaoxygen difluoride, 4327 Iodine dioxide trifluoride, 4334 Iodine(V) oxide, 4627 Iodine(VII) oxide, 4628 Oxygen difluoride, 4317 Perbromyl fluoride, 0240 Perchloryl fluoride, 3974... [Pg.185]

Dioxygen difluoride, 4320 Hexaoxygen difluoride, 4327 Oxygen difluoride, 4317 Trioxygen difluoride , 4323 See other HALOGEN oxides... [Pg.299]

Nitrous oxide reacts with dioxygen difluoride at ordinary temperatures forming various fluorinated products, such as FNO, FNO2, and FONO2 ... [Pg.665]

Xenon tetrafluoride also can be prepared by oxidizing xenon with dioxygen difluoride, O2F2, or by photolysis of xenon-fluorine mixture. [Pg.973]

The results of this calculation are gralifyingly congruent, and we feel reasonably confident in a value of about 167 kJ mol-1 (40 kcal mol-1) for the N—N bond. Similar results can be obtained for hydrogen peroxide and dioxygen difluoride to obtain an estimate of about 142 kJ mol"1 (34 kcal mot" ) for the O—O bond. [Pg.506]

See other pages where Dioxygen difluoride is mentioned: [Pg.331]    [Pg.221]    [Pg.221]    [Pg.292]    [Pg.639]    [Pg.292]    [Pg.191]    [Pg.244]    [Pg.244]    [Pg.753]    [Pg.1405]    [Pg.1526]    [Pg.1532]    [Pg.1532]    [Pg.1536]    [Pg.1894]    [Pg.1894]    [Pg.140]    [Pg.308]    [Pg.318]    [Pg.121]    [Pg.289]    [Pg.299]    [Pg.520]    [Pg.331]    [Pg.658]    [Pg.156]    [Pg.210]    [Pg.271]    [Pg.271]    [Pg.828]    [Pg.1451]   
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Dioxygen difluoride reactions

The peculiar structure of dioxygen difluoride, FOOF anomeric delocalization

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