SnI4 Research Articles

Spectrophotometric determination of iridium with stannous iodide reagent

Iridium ions react with tin(II) iodide reagent to form a stable complex with an absorption maximum at 446 mμ. Beer's law is not obeyed but the reaction is reproducible and the absorbancy is proportional to iridium concentration with an accuracy of ±0.9% over the range 0.8–11.7 p.p.m. Prior separation of iridium from rhodium and other transition metals is necessary. The procedure compares favorably with the tin(II) bromide method. The tin(II) halide reactions with platinum group metals are shown to diverge from true homologous series.

Spectrophotometric determination of rhodium with stannous iodide reagent

The tin(II) iodide reagent reacts with rhodium to form a stable colored complex with an absorption maximum at 460 mμ. The system obeys Beer's law and exhibits a molar absorptivity of 3.9·10 4 at 460 mμ. Rhodium concentrations between 0.4 and 3 p.p.m. can be determined with an average deviation of only 0.3%. The method compares favorably with the tin(II) chloride and bromide methods for rhodium and is considerably more sensitive. Ir, Pd, Pt, Sb, Ti, Cu, Co, Ni and Fe interfere with the method. Consequently, just as is the case with the chloride and bromide reagent, Rh must be separated from most samples prior to an analysis.

Spectrophotometric determination of iridium with stannous iodide reagent

Iridium ions react with tin(II) iodide reagent to form a stable complex with an absorption maximum at 446 mμ. Beer's law is not obeyed but the reaction is reproducible and the absorbancy is proportional to iridium concentration with an accuracy of ±0.9% over the range 0.8–11.7 p.p.m. Prior separation of iridium from rhodium and other transition metals is necessary. The procedure compares favorably with the tin(II) bromide method. The tin(II) halide reactions with platinum group metals are shown to diverge from true homologous series.

Spectrophotometric determination of rhodium with stannous iodide reagent

The tin(II) iodide reagent reacts with rhodium to form a stable colored complex with an absorption maximum at 460 mμ. The system obeys Beer's law and exhibits a molar absorptivity of 3.9·10 4 at 460 mμ. Rhodium concentrations between 0.4 and 3 p.p.m. can be determined with an average deviation of only 0.3%. The method compares favorably with the tin(II) chloride and bromide methods for rhodium and is considerably more sensitive, Ir, Pd, Pt, Sb, Ti, Cu, Co, Ni and Fe interfere with the method. Consequently, just as is the case with the chloride and bromide reagent, Rh must be separated from most samples prior to an analysis.

Separation of tin by benzene extraction of stannic iodide

Benzene extraction of tin(IV) iodide from a sodium iodide-perchloric acid-sodium perchlorate solution (e.g. 0.5 M NaI, 1.5M HClO 4, 3 M NaClO 4) provides a simple means of separating microgram (or larger) amounts of tin from most elements. Germanium and arsenic are extracted to a small extent, but even as much as 1 mg. Ge does not cause significant error when tin is determined spectrophotometrically with phenylfluorone. As little as 2 μg. Sn can be determined in the presence of 100 mg. Fe(III) after iodide extraction.

The partial molal volume and entropy of solution of stannic iodide

The partial molal volume and entropy of solution of stannic iodide

Correlation of solubility relations of stannic iodide, iodine, sulphur and phosphorus

Correlation of solubility relations of stannic iodide, iodine, sulphur and phosphorus

The Molecular Polarizations and Apparent Dipole Moments of Titanium Tetrachloride, Tin Tetrachloride and Tin Tetraiodide in Non-polar Solvents

The Molecular Polarizations and Apparent Dipole Moments of Titanium Tetrachloride, Tin Tetrachloride and Tin Tetraiodide in Non-polar Solvents

The crystal structure of tin tetraiodide

The crystal structure of tin tetraiodide was determined by Dickinson (1923). The unit cell is cubic with a o --12.26 /~ (Dickinson's a 0 = 12.23 _~); there are eight molecules per unit cell. The space group is ~ P a 3 . The structure, as described by Dickinson, can be visualized in terms of small deviations from an 'ideal' structure consisting of tin atoms occupying one-eighth of the tetrahedral interstices in a cubic close packing of iodine atoms. In the 'ideal' structure the tin atoms and one of the iodine atoms of each SnI~ tetrahedron would be located on one of the threefold cube axes; the other three iodine atoms of the tetrahedron would lie in a plane perpendicular to this axis. Assuming that the regular tetrahedral coordination of the SnI~ group is maintained, three shifts from the 'ideal' may be considered: Ca) The tetrahedron may be translated along the threefold axis; (b) the tetrahedron may be contracted or expanded; (c) the iodine atoms in general positions may be rotated about the threefold axis. Dickinson permitted all three types of deviations from the 'ideal' structure in addition to possible distortion of the tetrahedron. In terms of the unit-cell edge the magnitudes of these shifts were 0.004 for type (a), 0-001 for contraction of type (b), and 3 ° for type (c). His determination was based on analysis of Laue diagrams and spectral photographs, and the parameters (Table 1) were obtained by a systematic trial-and-error procedure.

Rapid Exchange between Iodine and Stannic Iodide in Carbon Tetrachloride at 0°1

Rapid Exchange between Iodine and Stannic Iodide in Carbon Tetrachloride at 0°¹

Phase Studies on the Binary Systems of Tin Tetrabromide, Tin Tetraiodide and Trichlorosilane with Some Aliphatic Ethers

Phase Studies on the Binary Systems of Tin Tetrabromide, Tin Tetraiodide and Trichlorosilane with Some Aliphatic Ethers

An Irregularity in the Solvent Powers of Paraffins

The solubility relations of n-heptane with f-heptane, iodine, sulfur, stannic iodide, and phosphorus are all accounted for within the usual limits of accuracy for regular solution theory by a solubility parameter 8.1 instead of the value 7.45 derived from its energy of vaporization per cc. Solutions of 2,2,4-trimethyl pentane with f-heptane and with iodine are similarly accounted for by the empirical value 7.45 instead of 6.85. Such an adjustment for paraffins is a practical alternative to the treatment used by Simons and Dunlap for the system n-pentane, ``pentforane,'' which they recently reported upon, and is, at the same time, consistent with their assumption that the exceptional behavior of paraffins is to be attributed to an irregularity in their mutual repulsions.

Reaction between nitric acid and tin in presence of catalysts—Part II

1. Iodides of sodium and potassium retard the reaction between nitric acid and tin. This retardation may be due to the specific action of the alkali ions as suggested in the earlier paper. 2. Unimolar solutions of NaI, KI and LiI inhibit the reaction for about three months and thereafter cause the formation of a thin layer of stannous iodide on the surface of tin and the formation of the oxidation products of HI in the reaction mixture are responsible for this behaviour.

Solubility. XV. The Solubility of Liquid and Solid Stannic Iodide in Silicon Tetrachloride

Solubility. XV. The Solubility of Liquid and Solid Stannic Iodide in Silicon Tetrachloride

The Heat of Fusion and Vapor Pressure of Stannic Iodide

The Heat of Fusion and Vapor Pressure of Stannic Iodide

The Heat of Fusion of Stannic Iodide

The Heat of Fusion of Stannic Iodide

II. Remarks on organo-metallic bodies; 4th memoir

In a former Memoir the author described the production of a new series of organic compounds containing the metal tin in com­bination with the radicals methyl, ethyl, and amyl. His attention was at that time especially directed to the compound formed by the union of tin with ethyl, and to which the name stanethyl was given. The iodide of stanethyl was prepared by exposing iodide of ethyl to light or heat in the presence of tinfoil; and, by acting with zinc upon the aqueous solution of this iodide of stanethyl or of the chloride of the same body, stanethyl itself (C 4 H 5 Sn) was obtained. In accordance with a theory of the constitution of all organo-metallic bodies which the author then suggested, the above com­pounds were respectively represented as the analogues of the protiodide and biniodide of tin, thus— It is evident that the application of this theory to the above bodies would receive considerable additional support if the second equivalent of iodine in the stannic iodide could be replaced by ethyl, or some other analogous organic group. In the Memoir already alluded to, it was mentioned, that in studying the behaviour of stanethyl under the influence of heat, evidence was obtained of the existence of this very compound, —stannic ethide, or binethide of tin , as it was then named. This body obviously bears the same re­lation to stannic iodide as stanethyl bears to stannous iodide.