Chlorine fluoride molecule

Elimination reactions of fluorine compounds are not limited to the removal of simple molecules Frequently, large molecules or combination of smaller ones are formed as by-products, especially in pyrolytic reactions For example perhalo genated acid chlorides lose not only carbon monoxide but also chlorine fluoride [106, 107] (equations 74 and 75)... 

Fig. 1. Geometries of the chlorine oxyfluoride molecules and their ions compared to those of the corresponding chlorine fluorides. Since the C1+ cation would possess only an electron sextet, it is stabilized by a GIF molecule to form the C12F+...

As can be seen from Fig. 1, the structures of all the chlorine oxyfluoride molecules and ions can be derived from those of the corresponding binary chlorine fluorides (53) by replacing a free chlorine valence electron pair by a doubly bonded oxygen atom without significant rearrangement of the rest of the molecule. 

In many respects the chlorine oxyfluorides resemble the chlorine fluorides. For example, they exhibit little or no self-ionization, but are amphoteric. With strong Lewis acids or bases they can form stable adducts. The tendency to form adducts was found (64) not to be so much a function of the relative acidity of the parent chlorine oxyfluoride but rather to depend on the structure of the amphoteric molecule and of that of the anion or the cation formed. The preferred structures are the energetically favored tetrahedron and octahedron. Consequently, a trigonal bipyramidal molecule, such as CIF3O (64), exhibits a pronounced tendency to form either a stable pseudotetrahedral cation or a pseudo-octahedral anion ... 

Assuming covalent bonds, write electronic structures for the molecules GIF (chlorine fluoride), BrFg (bromine trifluofide), SbCl5 (antimony penta chloHde), HgSg (hydrogen disulfide). In which of these molecules are there atoms with electron configurations that are not noble-gas configurations ... 

Although poly(vinyl fluoride) resembles PVC in its low water absorption, resistance to hydrolysis, insolubility in common solvents at room temperature and a tendency to split off hydrogen halides at elevated temperatures, it has a much greater tendency to crystallise. This is because the fluorine atom (c.f. the chlorine atom) is sufficiently small to allow molecules to pack in the same way as polythene. 

The structures of the chlorine oxide fluorides are summarized in Fig. 17.26, together with those of related cationic and anionic species formed from the neutral molecules by gain or loss or F . The first conclusive evidence for free FCIO in the gas phase came in 1972 during a study of the hydrolysis of CIF3 with substoichiometric amounts of H2O in a flow reactor ... 

Chemists refer to the bond in a molecule like sodium chloride as ionic , meaning that its electron pair resides entirely on chlorine. At the other extreme is the covalent bond in the hydrogen molecule, where the electron pair is shared equally between the two hydrogens. Intermediate cases, such as the bond in hydrogen fluoride which is clearly polarized toward fluorine, are generally referred to as polar covalent bonds (rather than partially ionic bonds). Are these situations really all different or do they instead represent different degrees of the same thing ... 

Most plastics react chemically with chlorine because of their hydrocarbon structural makeup. This reactivity is avoided with some plastics in which fluorine atoms nave been substituted into the hydrocarbon molecule. The Chlorine Institute recommends that hoses constructed with such an inner lining "have a structural layer braid of polyvinyli-dene fluoride (PVDF) monofilament material or a structural braid of Hastelloy C-276. An underlying lesson here is material compatibility. Material compatibility tables exist that engineers can consult, including in other sections within this volume. 

It has been suggested that the carbon atom in the carbonium ion which is usually represented as containing only six electrons in its outer shell may actually contain six of its own electrons and two electrons which are donated by chlorine atom from aluminum chloride or, presumably, a fluorine from boron fluoride (N. V. Sidgwick, private communication to Hunter and Yohe, 17). Combination with a second molecule of olefin would then involve the breaking of the carbon-chlorine coordinate bond and the formation of a carbon-carbon bond. 

In the same way as intramolecular displacement leads to particularly stable atomic groupings within a molecule, the disproportionation reactions between several molecules are attributable to the tendency for the more stable compound with the higher fluorine content to form. Reactions of this kind are sometimes used to obtain highly fluorinated compounds from products with lower fluorine contents, for example, the catalytic fluorination of chloroalkanes with hydrogen fluoride or with fluorination agents such as antimony(V) fluoride or antimony(III) fluoride. The chlorine compound formed as the second product of the disproportionation process is reused as the starting material for the preparation of the compound to be dispropor-tionated. 

Copper 11 halides are formed with chlorine, bromine and iodine, the chloride and bromide by reduction of the coppertll) halides with copper powder, and the iodide by reduction of coppertll) sulfate. CuSOj solulion with potassium iodide. The fluoride appears never to have been made, despite reports to the contrary. All are insoluble in H20. CoppertUl fluoride, CuF may be made from CuO and hydrofluoric acid at 400°C. coppertll) chloride. CuCl by dissolving the oxide or carbonate in HCI, and coppertll) bromide. CuBr from copper and bromine water coppertll) iodide. Cub, is unstable at room temperature with respect to decomposition intu Cul and iodine. The chloride and bromide are water-soluble, and ionic. The fluoride is only slightly water-soluble. Anhydrous copper(U) chloride. Cud , is monoclinic and its structure contains infinite-chain molecules formed by CuCLi groups that share opposite edges. CuBr. has a similar structure. 

Halogen atoms in certain inorganic compounds may be replaced by fluorine by the use of antimony (III) fluoride without a catalyst. In other cases, varying amounts of different kinds of catalysts are required. For example, sometimes the addition of chlorine in the amount of 1 % of the antimony (III) fluoride will suffice. Molecules which are more difficult to fluorinate may require chlorine, bromine, or antimony(V) chloride in quantities amounting to as much as 5% of the weight of antimony (III) fluoride used. 

The reaction involves the replacement of the halogen atoms in nonpolar halide molecules by fluorine atoms. The fluorinating agent is usually resublimed antimony (III) fluoride. If necessary, a catalyst, such as antimony(V) chloride, chlorine, or bromine, may be used. 

If a molecule has a multiple bond and a nucleophilically mobile chlorine atom, then the fluoride ion attacks the double bond, generating a carbanion stabilized by two trifluoromethyl groups, and intramolecular nucleophilic cyclization forming a five-membered heterocycle 48 is possible. 

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