Chlorine trifluoride CIF

Teflon is attacked by only two clami of ehamicals al Molten alkali metals such as sodium ft potassium b) Fluorochamleals such as chlorine trifluoride (CIF ) and oxygen difkioridg (OF ). and fluorine gas at alavatad tamperaturaft praiiura... 

Fluorine was first produced commercially ca 50 years after its discovery. In the intervening period, fluorine chemistry was restricted to the development of various types of electrolytic cells on a laboratory scale. In World War 11, the demand for uranium hexafluoride [7783-81-5] UF, in the United States and United Kingdom, and chlorine trifluoride [7790-91 -2J, CIF, in Germany, led to the development of commercial fluorine-generating cells. The main use of fluorine in the 1990s is in the production of UF for the nuclear power industry (see Nuclearreactors). However, its use in the preparation of some specialty products and in the surface treatment of polymers is growing. 

The use of CIF and BrF as ionizing solvents has been studied (102,103). At 100°C and elevated pressures, significant yields of KCIF [19195-69-8] CsClF [15321-04-7], RbClF [15321-10-5], I-CBrF [32312-224], RbBrF [32312-224], and CsBrF [26222-924]obtained. Chlorine trifluoride showed no reaction with lithium fluoride or sodium fluoride. 

The behaviour of chlorine irifluoride differs sharply from that of bromine trifluoride for, when it is added to potassium fluoride, the latter may be recovered quantitatively by evaporation in vacuum at room temperature. The same is true of other metallic fluorides and it appears that the (C1F4) anion is inherently unstable. There is some indication that chlorine trifluoride may form acids with the fluorides of some of the non-metallic elements, though this point has not cis yet been fully investigated. No direct evidence is yet available as to whether other halogen fluorides can give rise to acids and bases, though this is perhaps less probable for compounds such as CIF, BrFj and IF7. 

Chlorine monofluoride, CIF Chlorine trifluoride, CIF3 Bromine monofluoride, BrF Bromine trifluoride, BrF3 Bromine pentafluoride, BrF5 Bromine monochloride, BrCI Iodine trifluoride, IF3 Iodine pentafluoride, IF5 Iodine heptafluoride, IF7 Iodine monobromide, IBr Iodine monochloride, ICI Iodine pentabromide, IBr5 Iodine tribromide, IBr3 Iodine trichloride, ICI3 Iodine pentachloride, ICI5... 

Chlorine monofluoride is a colorless gas that condenses to a very pale yellow liquid. It is prepared by the interaction of chlorine trifluoride and chlorine or by heating chlorine and fluorine together in a 1 1 ratio. It can be used to saturate multiply bonded systems or oxidize coordinatively unsaturated central atoms. Scheme 8 illustrates some types of CIF reactivity. 

The interhalogen compounds are highly reactive substances, especially those containing fluorine. Chlorine trifluoride (CIFj) of b.p. 11°C is in many respects more reactive than fluorine and flames instantaneously not only with many organic substances but even with aluminum oxide and magnesium oxide. Similar in behavior is bromine trifluoride (BrF ) of m.p. 8.8 C and b.p. IBSX. Other interhalogen compounds, all very reactive, are CIF, BrF, BrF, IFj, and IF,. More recently discovered was the compound chlorine pentafluoride (ClF ) of m.p, approximately — 103"C and a b.p. of — 18.1 C. 

Microwave discharge in a 1 1 mixture of nitrogen trifluoride and chlorine yielded CIF, Ng, and HF as principal products smaller amounts of HCl, NgFg, and HCIO were also formed [3]. 

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