Chlorine trifluoride structure

This last reaction is typical of many in which F3CIO can act as a Lewis base by fluoride ion donation to acceptors such as MF5 (M = P, As, Sb, Bi, V, Nb, Ta, Pt, U), M0F4O, Sip4, BF3, etc. These products are all white, stable, crystalline solids (except the canary yellow PtFe ) and contain the [F2CIO] cation (see Fig. 17.26h) which is isostructural with the isoelectronic F2SO. Chlorine trifluoride oxide can also act as a Lewis acid (fluoride ion acceptor) and is therefore to be considered as amphoteric (p. 225). For example KF, RbF and CsF yield M [F4C10] as white solids whose stabilities increase with increasing size of M+. Vibration spectroscopy establishes the C4 structure of the anion (Fig. 17.29g). 

The Lewis structure of chlorine trifluoride is treated in Example. Determine the molecular geometry and draw a three-dimensional picture of the molecule. 

Chlorine trifluoride dioxide, 18 361-367 bonding in, 18 366, 367 internal force constants of, 18 366 molecular structure of, 18 364-367 properties of, 18 362-364 stretching force constants of, 18 366 synthesis of, 18 362-364 thermodynamic data for, 18 387 vibrational spectra of, 18 364, 365... 

Chlorine trifluoride oxide, 18 331-340 chemical properties of, 18 337-340 internal force constants, 18 335 molecular structure of, 18 334-336 physical properties of, 18 336, 337 reactions of, 18 338, 339 stretching force constants, 18 336 synthesis of, 18 331-334 thermodynamic data for, 18 386, 387 vibrational spectra of, 18 334 Chlorine trioxide hydroxide, structure of, 5 219... 

Chlorexolone as diuretic, 1, 174 Chlorides synthesis, 1, 448 Chlorin, 4, 370 metal chelates, 4, 391 Chlorin, dihydroxy-, 4, 393 Chlorin e6, 4, 404 trimethyl ester, 4, 398 synthesis, 4, 416 Chlorination pyridazines, 3, 20, 21 Chlorine trifluoride bonding, 1, 564 Chlorin-phlorin, 4, 398 Chlorins, 4, 378 absorption spectra, 4, 389 formation, 4, 394 molecular structure, 4, 385 oxidation, 4, 395 Chlorisondamine chloride as hypertensive agent, 1, 176 Chlormethiazoles metabolism, 1, 235 Chlormethiuron against ectoparasites veterinary use, 1, 217 Chlormezanone as antidepressant, 1, 169 Chlorocruoroheme, 4, 380 Chlorofucin conformation, 7, 703 Chloronium iodide, biphenylene-reactions, 1, 566... 

If the proposed structures can be demonstrated to be true products of these irradiation experiments, they will constitute the first members of a new class of compounds where other substituents replace fluorine atoms in the parent molecule chlorine trifluoride. 

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. 

Boron trifluoride forms addition compounds that incorporate an sp hybridized boron into a tetravalent structure. Salts of BF4 are readily formed with BF3 and a suitable fluoride donor. Halogen fluorides such as chlorine trifluoride react with BF3 to generate interhalogen cations such as [C1F2]+[BF4]. Some further examples are shown in equations (43) and (44). In an organic application, the Schiemann reaction provides an entry into fluorinated aromatics by thermal decomposition of a diazonimn tetrafluoroborate (equation 45). 

Liquid-phase halogenation of hexachlorobenzene with chlorine trifluoride appears to proceed by a series of additions and vinylic and allylic substitutions until all of the hexachlorobenzene is converted into chlorofluorocyclohexenes, C6F (Clio ) (n = mainly 4, 5 and 6), and conversion to cyclohexane derivatives occurs only upon the passage of quite a large excess of chlorine trifluoride [177] (Figure 2.29). The cyclohexene derivatives produced mainly retain the structure —CC1=CC1—. 

Rocket Fuel In the 1950s, the reaction of hydrazine with chlorine trifluoride (GIF3) was used as a rocket fuel. Draw the Fewis structure for GIF 3 and identify the hybrid orbitals. 

Reactivity and Incompatibility Violent reactions of lead with sodium azide, zirconium, sodium acetylide, and chlorine trifluoride have been reported. Reactivity of lead compounds varies depending on structure. 

Example 5. Chlorine trifluoride CIF3. It is not easy to tell what kind of structure we will have. Well, it is easy with VSEPR. The central atom will be chlorine. It has 7 valence electrons. Each fluorine contributes one electron. Thus, altogether the chlorine has 7 + 3 = 10 electrons, i.e. five electron pairs. This means a trigonal bipyramide in VSEPR. However, this does not tell us where the lone pairs and where the fiuorine atoms are. Indeed, there are two physically distinct positions in such a bipyramide the axial and the equatorial, Fig. 8.30. 

Practice Exercise Draw the Lewis structure for chlorine trifluoride (CIF3). (AH fluorine atoms are bonded to the central chlorine atom.)... 

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). 

Earlier in this ehapter, the structure of PTFE was likened to a carbon rod completely blanketed with fluorine atoms which render the C-F bond impervious to solvent attack. This postulate has been proven by testing the effect of almost all common solvents on this polymer. There are no known solvents for PTFE below its melting point. PTFE is attacked only by molten alkali metals, chlorine trifluoride, and gaseous fluorine. Attack by alkali metals results in defluorination and surface oxidation of PTFE parts which is a convenient route to render them adherable. 

Table 5.9 lists the structures of polychloroprenes that form by free-radical polymerization at different temperatures. Chloroprene polymerizes by cationic polymerization with the aid of Lewis acids in chlorinated solvents. When aluminum chloride is used in a mixture of ethyl chloride-methylene chloride solvent mixture at -80 °C, the polymer has 50% 1,4 units. If it is polymerized with boron trifluoride, the product consists of 50-70% 1,4-adducts. A veiy high trans-1,4-poly(2-chloro-1,3-butadiene) forms by X-ray radiation polymerization of large crystals of... 

The cationic polymerization of cyclopentadiene is catalyzed by tin-tetrachloride/ trichloroacetic acid/boron trifluoride [402-407]. The polymers that are partially insoluble in hydrocarbons feature 40 to 60% 1,2-structures next to trans-, 4 portions [Structures (60) and (61)]. With Ti(OC4H9)Cl3, soluble high-molecular-weight polycyclopentadiene is formed. Due to H-atoms in allyl and tertiary positions of the chain, the polymer is extremely sensitive to oxidation. This can be overcome by chlorination of the double bonds [408,409]. 

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