Iron oxychloride

Small amounts of iron oxychloride are always apt to be present in ferrous chloride, even when the latter is most carefully made. 

In a recent publication (190), these techniques were applied to elucidate the crystal structure of low-dimensional compounds such as iron oxychloride, FeOCl, and its alkoxy substituents, FeOCl (OR), where R is Me or Et. It was shown that the local symmetry around the iron atom becomes higher for methoxy substituents compared to that for FeOCl. In fact, it is similar to that for y-FeOOH. Similarity of the one-dimensional electron density map along the c axis, obtained separately from X-ray crystallographic studies and from EXAFS fitting, reflects the reliability of the EXAFS fit and indicates its applicability to other two-dimensional systems with poor crystallinity. 

Iron oxychloride FeOCl presents a layered structure encountered in the various MOX derivatives of 3d elements that have been prepared, i.e., TiOCl, VOCl, CrOCl, FeOCl, TiOBr, VOBr, CrOBr. Table 1 shows the parameters of the orthorhombic unit cell. 

In this study a series is presented at which the HCl concentration has been fixed at 1000 vppm and the amount of OT rgen has been varied (Fig. 30.10). The most accelerated corrosion has been observed at 16 vol.% O2. Similar to the test carried out in Ar-8 vol.% O2-2OOO vppm HCl, a mass loss appears after about 60 or 70 h due to the evaporation of iron chloride. Therefore the formation of volatile iron chloride is favoured in Ar-02-HCl atmospheres if either the HCl and/or O2 concentration is increased. A possible reason for this may be the formation of iron chloride, subsequently evaporating. This effect has to be studied in further detail. Iron oxychloride can be excluded because it can be formed only at temperatures higher than 320°C. The stabiUly of FeOCl in the temperature range of 325-350°C is restricted at pCCy > 0.0186 bar and 4.68 x 10 bar < p(02) < 10 bar, depending on pCCy at 330°C. 

Iron Oxychloride as a Precursor to Lamellar Iron Phosphonates by Soft Chemistry... 

Iron oxychloride was prepared from Fe203 and FeQ3 by the usual sealed-tubes technique. All iron phosphonates were obtained according to the following chemical process n mmoles of phosphonic acid react with one mmole of FeOQ in 5 mL of solvent in sealed Pyrex tubes. Some reactions have been also realized in round-bottom flasks under nitrogen. 

Recovery of Bismuth from Tin Concentrates. Bismuth is leached from roasted tin concentrates and other bismuth-beating materials by means of hydrochloric acid. The acid leach Hquor is clarified by settling or filtration, and the bismuth is precipitated as bismuth oxychloride [7787-59-9] BiOCl, when the Hquors are diluted usiag large volumes of water. The impure bismuth oxychloride is usually redissolved ia hydrochloric acid and reprecipitated by diluting several times. It is then dried, mixed with soda ash and carbon, and reduced to metal. The wet bismuth oxychloride may also be reduced to metal by means of iron or 2iac ia the presence of hydrochloric acid. The metallic bismuth produced by the oxychloride method requites additional refining. 

New Developments Based on Non-Micaceous Systems. The class of single crystal lustrous pigments is not limited to the non-absorbing types like bismuth oxychloride and basic lead carbonate. Recent developments are absorbing pigments such as platelet-like graphite, laminar phthalocyanines and flaky iron oxides. These flakes... 

There has been some controversy in the literature over the proper interpretation of reactions in solvents such as phosphorus oxychloride. Drago and coworkers18 have suggested the "coordination model" as an alternative to the solvent system approach. They have stressed the errors incurred when the solvent system concept has been pushed further than warranted by the facts. In addition, they have pointed out that iron(lll) chloride dissolves in triethyl phosphate with the formation of letrachloro-... 

Meek and Drago8 showed that the reaction between tetramethylammonium chloride and iron(III) chloride can take place just as readily in triethyl phosphate, OP(OEt), as in phosphorus oxychloride, OPCl,. They suggested that the similarities in physical properties of the two solvents, principally the dielectric constant, were more impor tant in this reaction than the difference in chemical properties, namely, the presence or absence of autoionization to form chloride ions.9... 

---