Iodine magnetic susceptibility

This unusual compound, in which the valence of iodine is +6, between iodate (+5) and periodate (+7), results from the thermal decomposition of Li2H3I06.50 Detailed X-ray, infrared, and magnetic susceptibility measurements were used to establish the chemical individuality of the salt which is stable to about 450°C. 

This salt, in which iodine is in a +6 oxidation state, results from heating Na2H3IOe at 120 to 180°C.101 Using X-ray diffraction, magnetic susceptibility, and infrared absorption, the chemical individuality of the salt was established i.e., it is not a mixture of NaIOs and Na3I05. The compound is stable up to 370°C, but its decomposition products were not identified. 

Gillespie and Milne (2) have shown, by conductometric, spectro-photometric, and magnetic susceptibility measurements in fluorosulfuric acid, that the blue iodine species observed in strong acids is la. When iodine was oxidized by peroxodisulfuryl difluoride in fluorosulfuric acid, the concentration of the blue iodine species reached a maximum at the 2 1 Ij/SgOeFa mole ratio [Eq. (4)] and not at the 1 1 mole ratio as would... 

In the case of Eu and Yb the reactions proceed at temperatures ranging from -40 to -20 C. Samarium is less active and after an activation by treatment with iodine interacts with RI at 30 C to give blue-green solutions of RSml. The solutions of Eu and Yb derivatives are brown. The products were not isolated from the reaction mixture as individual compounds, however the formation of them is reliably confirmed by the data of acidimetry and iodometry, reactions with iodine, as well as by reactions characteristic for Grignard reagents with Michler s ketone, water, benzophenone, Me3SiCl. The measurement of magnetic susceptibility has shown that in the Eu and Yb complexes from 85 to 100% of the metal is in bivalent state. In the Sm complexes up to 50% of the metal is present as Sm(III). 

For iodine, the situation is even more complicated. Although complexes with iodine were known for a long time [5], the electrical conductivity was only studied after the bromine complex was reported, independently by Kommandeur and Hall [6] and by Uchida and Akamatu [7]. Both found crystals with the (Per) l2 ratio of 2 3 but the Japanese group, based on X-ray diffraction patterns and magnetic susceptibility measurements, claimed also the existence of a different complex with stoichiometry Per(l2)3. Room temperature values of conductivity agree quite well in the two publications, (1-1.25) x 10 S/cm for the 2 3 complex but disagreement appears about the energy gap, 0.038 eV from Kommandeur and Hall but 0.06 eV... 

Weigh out accurately about 0.2 g of your preparation, add excess of 10% KI solution and shake well until maximum colour of iodine is formed. Titrate using standardised 0.05 M thiosulphate solution as in Sec.7.3.3. Characterise the freshly prepared product by ir spectroscopy and by measuring its magnetic susceptibility (Sec.2.1.3). 

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