Fluorine oxoacids

Oxidation State Fluorine Oxoacids Chlorine Oxoacids Bromine Oxoacids Iodine Oxoacids General Name... 

Hypofluorous acid is the most recent of the halogen oxoacids to be prepared. Traces were obtained in 1968 by photolysis of a mixture of F2 and H2O in a matrix of solid N2 at 14-20 K but weighable amounts of the compound were first obtained by M. H. Studier and E. H. Appelman in 1971 by the fluorination of ice ... 

Oxidation A half-reaction in which there is an increase in oxidation number, 88 chromium, 548 electrolysis and, 498 fluorine, 557 halogens, 557-558 oxoacids, 568-570 oxoanions, 568-570 species strength, 506-507q transition metals, 546t zinc, 86-87... 

Except for fluorine the elements have an extensive oxoacid chemistry. Figure shows Frost diagrams with the oxidation states found in acid and alkaline solution. The sharp trend in oxidising power of the elements (X2/X- potential) can be seen. As expected from Pauling s rules the hypohalous acids X(OH)... 

The oxoacids and their salts are very stable, in contrast to the lack of stability of the halogen oxides themselves. A large number of these acids exist at the representative oxidation states of the halogens, namely, +1, +3, +5, and +7. Even perbromic acid, HBr04, has been synthesized by fluorination ofbromates. 

Fluorine does not form an oxoacid the element is more electronegative than oxygen. In the chlorine, bromine and iodine compounds the halogen atom is positive in relation to the oxygen atoms, as indicated by the <5 s ... 

The only oxoacid of fluorine that has been prepared is unstable hypofluorous acid, HOF. Aqueous hypohalous acids (except HOF) can be prepared by reaction of free halogens (CI2, Br2, I2) with cold water. The smaller the halogen, the farther to the right the equilibrium lies. 

Most halogen oxides are of low stability, but several oxoacids are known except for fluorine. Redox stability depends on pH, Cl2 and Br2 disproportionating in alkaline... 

Fluorine has an oxidation number of 1 in all its compounds. Other halogens (Cl, Br, and I) have negative oxidation numbers when they occur as hahde ions in their compounds. When combined with oxygen—for example in oxoacids and oxoan-ions (see Section 2.7)—they have positive oxidation numbers. 

Chlorous acid, HCIO2, is the only known halous acid. All the halogens except fluorine form halic and perhalic acids. The Lewis structures of the chlorine oxoacids are... 

The reactivity, toxicity, and oxidizing ability of the halogens decrease from fluorine to iodine. The halogens all form binary acids (HX) and a series of oxoacids. 

Fluorine is unique among the halogens in forming no species in which it has a formal oxidation state other than — 1. The only known oxoacid is hypofluorous acid, HOF, which is unstable and does not ionize in water but reacts according to equation 16.54 no salts are known. It is obtained by passing F2 over ice at 230 K (equation 16.55) and condensing the gas produced. At 298 K, HOF decomposes rapidly (equation 16.56). 

Bismuth commonly forms cations of + 3 charge. It forms the basic oxide Bi20j and salts of oxoacids such as Bi2(S04)3 and Bi(N03)3- Reaction of the metal with hahdes such as fluorine and chlorine results in a salt with the formula of BiXj. Because of the size of the metal atom, the linkages are more ionic than those found for other group members. 

Halogen oxides are typically not very stable, and some oxygen compounds form as oxoacids instead (with the exception of fluorine there are no oxoac-... 

Suppose for the moment that fluorine formed the acid that would be called, by analogy with the other halogen oxoacids, fluoric acid, HFO3. Draw Lewis stmc-tures for this fictional compound and analyze why it does not exist. 

Fluorine, the most electronegative element, adopts the -1 oxidation state in its compounds. The other halogens, when bonded to a more electronegative element such as oxygen, can have any one of several positive oxidation states +1, +3, +5, or +7. This variability of oxidation states, which was illustrated through electrode potential diagrams for chlorine (Fig. 22-4), is emphasized again by the oxoacids listed in Table 22.7. The structures of some of these... 

The hypothetical oxoacid of fluorine, HF02(H0F0), would have a positive formal charge on the central F atom. 

This is not something that we would expect of fluorine, the most electronegative of all the elements. Flypothetical oxoacids with more O atoms would have the F atom with even higher positive formal charges. Fluorine does form HOF, an oxoacid with no formal charges H—O — Ft, but HOF exists only in the solid and liquid states. In water, HOF decomposes to HF, H2O2, and O2. 

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