Bromine trifluoride structure

The simple method of drawing electron-dot structures that works well for most compounds of second-row elements sometimes breaks down for compounds that contain elements below the second row of the periodic table. As we saw in Section 6.12, elements in the third row and lower have unfilled d orbitals and are therefore able to expand their valence shell beyond the normal octet of electrons, forming more than the "normal" number of bonds predicted by their group number. In bromine trifluoride, for instance, the bromine atom forms three electron-pair bonds rather than one and has ten electrons in its valence shell rather than eight ... 

T he interest in conductivity measurements on fluorinated inorganic com pounds at cryogenic temperatures lies in the ability of these compounds to form ions for possible synthesis of potential solid oxidizers. In this study we are concerned with the conductivity measurements of solid chlorine and bromine trifluorides to determine their electrical conductivities and its bearing on structural problems. Specific conductivities of <10" at 0° C. (I) and 10 ohm-1cm. 1 (3) have been reported for chlorine trifluoride and 8.0 X l ohm-1cm. 1 at 25° C. (1) for bromine trifluoride. In this work a conductivity cell has been developed for measuring fluorine-containing oxidizers at cryogenic temperatures. The variations of conductivity with temperature of chlorine trifluoride have been measured from +11.3° C. (b.p.) to —130° C. (well below m.p., —83° C.) and of bromine trifluoride from -j-80° C. to —196° C. (m.p., 8.8° C.). Possible mechanisms are discussed. 

F (I) ion donor as selenium tetrafluoride and it is probable that in the platinum tetrafluoride-bromine trifluoride adduct the association is by bifluorine bridging, as represented in (I) or by monofluorine bridging to yield a polymeric structure. 

Bromine triflouiide, BrF The central atom bromine has seven electrons in its valence shell. Three electrons form bonds widi three fluorine atoms while four of them do not participate in bonding. In bromine trifluoride molecule there are a total of five electron pairs in the outer shell. The structure is a trigonal bipyramid. There are three bond pairs and two lone pairs. 

However, when ethyl acetoacetate was treated with diethylaminosulfur trifluoride, an entirely unexpected difluoro compound, C6H8F202, was obtained. The compound was an ester, and decolorized a solution of bromine in carbon tetrachloride. What is the structure of the product ... 

The molecular structures of some representive neutral interhalogens, (a) chlorine trifluoride, CIF3 (distorted T-shaped) b) bromine pentafluoride, BrFs (square pyramidal) (c) iodine heptafluoride, IF7 (pentagonal bipyramidal) and (d) diiodine hexachloride, I2CI6 (planar dimer). 

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