Sulfur anion name

These anions, S 06, with n up to 22 or higher, can be separated chromatographically only lower members are well characterized. They are normally named according to the total number of sulfur atoms, namely, trithionate, S3C, and so on. They are occasionally called sulfane-disulfonates, for example, disulfanedisulfonate for S4062-. The free acids are unstable as are also the HS 06 ions. 

If the anion name ends in -ate, the suffix -ic is added to the root name. For example, H2SO4 contains the sulfate anion (S04 ) and is called sulfuric acid H3PO4 contains the phosphate anion (P04 ) and is called phosphoric acid and HC2H3O2 contains the acetate ion (C2H302 ) and is called acetic acid. 

An ionic compound composed of a cation and the anion from an acid is often referred to as a salt. Table salt, NaCl, contains the anion from hydrochloric acid. Calcium sulfate, CaSO, is a salt containing an anion from sulfuric acid. Some salts contain anions in which one or more hydrogen atoms from the acid are retained. Such anions are named by adding the word hydrogen or the prefix bi- to the anion name. The best known such anion comes from carbonic acid. 

Other prominent sites for electrophilic addition are non-bonding electron pairs as they are present in many heteroatom-containing organic molecules. One example has already been mentioned, namely the RS conjugation with the sulfur anion function in thiolate. As formulated in the back reaction of equilibrium (14) this yields the three-electron bonded disulfide radical anion, (RS SR)in which the unpaired thiyl electron couples with the free p-electron pair at the thiolate sulfur. In this context, a significant consequence emerges with respect to the overall redox properties of such a system. As has been stated already, the... 

Sulfonium Compounds. Sulfonium compounds of the type R R R S X are named by citing in alphabetical order the radical names followed by -sulfonium and the name of the anion. For heterocyclic compounds, -ium is added to the name of the ring system. Replacement of > CH by sulfonium sulfur is denoted by the prefix thionia-, and the name of the anion is added at the end. 

The sulfur-rich oxides S 0 and S 02 belong to the group of so-called lower oxides of sulfur named after the low oxidation state of the sulfur atom(s) compared to the best known oxide SO2 in which the sulfur is in the oxidation state +4. Sulfur monoxide SO is also a member of this class but is not subject of this review. The blue-green material of composition S2O3 described in the older literature has long been shown to be a mixture of salts with the cations S4 and Ss and polysulfate anions rather than a sulfur oxide [1,2]. Reliable reviews on the complex chemistry of the lower sulfur oxides have been published before [1, 3-6]. The present review deals with those sulfur oxides which contain at least one sulfur-sulfur bond and not more than two oxygen atoms. These species are important intermediates in a number of redox reactions of elemental sulfur and other sulfur compounds. 

Reports on the organozinc chemistry with heavier group 16 donor ligands for the reviewed period were limited to sulfur donors. As with the organozinc chemistry of anionic oxygen donors, three themes dominate this area of research, namely the use of organozinc compounds ... 

Generally, oxo-selenates can be classified according to the oxidation state of the selenium atom as oxu-selenates(IV), and o.Yo-selenates(VI). The same applies for the respective tellurates. Besides this systematically correct naming, chemists usually use the terms selenites and tellurites instead of o. o-selenates(IV) and oxo-tellurates(IV), and selenates and tellurates instead of OAO-selenates(VI) and oxo-tellurates(VI). Therefore, both nomenclatures will be used in parallel throughout this chapter. Compared to the respective sulfur species, the oxo-selenate(IV) and oxo-tellurates(IV) ions are very stable so that numerous compounds with these anions have been prepared. 

Radical anions are also present in solutions of sulfur in oleum and in various polychalcogenide fluxes. However, only one radical ion Sg has been successfully characterized in the solid state, namely in [Ph4P]S6, which can be prepared according to Equation (3) by treating Ph4P]N3 with H2S in the presence of trimethylsilyl azide.35... 

The (8O3) radical is essentially the sulfur trioxide anion-radical. It is named the sulfite anion-radical because it is obtained from sodimn sulfite on reaction with titanimn trichloride in water. This reaction usually proceeds in the presence of ethylene diamine tetraacetic acid as a complexing agent and hydrogen peroxide as an oxidant (Bradic and Wilkins 1984). Under these conditions, the... 

The (864) radical is essentially the sulfur tetroxide anion-radical. It is named the snlfate radical because it is formed from the persulfate ion as a result of UV irradiation or heating (at 80-100°C) of persulfate salts M282O8 in aqueous solutions. Under these conditions, 820 -> 2804 dissociation takes place (Minisci et al. 1983, Dias and Vieira 1996). 

The removal of potassium cations makes the results of the liquid-phase and electrode reactions similar. In the presence of crown ether, the eight-membered complex depicted in Scheme 2.16 is destroyed. The unprotected anion-radicals of azoxybenzene are further reduced by cyclooctatet-raene dianion, losing oxygen and transforming into azodianion. The same particle is formed in the electrode reaction shown in Scheme 2.13. In the chemical reduction, stabilization of azodianion is reached by protonation. Namely, addition of sulfuric acid to the reaction results in the formation of hydrazobenzene, which instantly rearranges into benzidine (4,4 -diamino-l,l"-diphenyl). The latter was isolated from the reaction, which proceeded in the presence of crown ether. 

You can attach the prefixes in Table 6-2 to any of the elements in a molecular compound, as exemplified by SO3 (sulfur trioxide) and N2O (dinitrogen monoxide). The second element in each compound receives the -ide suffix, as in ionic compounds (which we discuss earlier in this chapter). In the case of molecular compounds, where cations or anions aren t involved, the more electronegative element (in other words, the element that s closer to the upper right-hand corner of the periodic table) tends to be named second. 

The use of -ous. -ic. per-, hypo-, ortho-, and meta- should be restricted to those compounds and to their derivatives their anions are named by changing -ous into -ite and -ic into -ate. In addition, and exceptionally, sulfur and phosphorus compounds lose the... 

Analogous oxoanions of elements in the same group of the periodic table are named similarly. Based on the names of the oxoanions of phosphorus and sulfur, name the following anions ... 

The use of alpha and beta bonds simplifies describing several familiar "inorganic" anions. Figure 7 illustrates the traditional Lewis structure of the sulfate ion, with an explanatory note that a more realistically picture (which will involve metric, as well as graph theoretical, distances [12]) is a tetrahedral resonance hybrid [13]. In other words, there are four identical oxygen atoms, each bonded by 1 and 1/2 bonds to the central sulfur atom, rather than two single and two double bonds. The name for this aggregation ... 

The sulfur-containing anion, S204, formed by the reduction of HSOj with zinc, has been called at various times hypomlfite, hydrosulfite, and dithionite. The latter name is that currently assigned to the ion, together with the structural formula O—S—S—02, An alternate structure,... 

A semiprecious deep-blue gem lapis lazuli has been known from ancient times and is available in synthetic forms under the name ultramarine. These are aluminosilicates of the sodalite type that contain sulfur in the form of the radical anions S3 and S2. The former, always present, causes a deep-blue color, and when S2 is also present a green hue is produced. 

Note that this anion can be viewed as a sulfate ion in which one of the oxygen atoms has been replaced by sulfur, which is reflected in the name thio-sulfate. The thiosulfate ion can be formed by heating sulfur with a sulfite salt in aqueous solution ... 

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