Über Metallokomplexe Die Kristallstruktur des Argentosulfoniumnitrats, [Ag<sub>3</sub>S][NO<sub>3</sub>]

Bergerhoff, G.

doi:10.1002/zaac.19592990511

Cited by 21 publications

(4 citation statements)

References 14 publications

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“…7), possesses a cubic structure containing approximately trigonal prismatic SAg6 groups linked through common corners to form a three-dimensional framework. The ionically bonded N03groups are located in the cavities (66). Other framework complexes include the dimercuro(II)ammonium salts, [Hg2N]X (28), and dimercuro(II)phosphonium trichloromercurate(II), [Hg2P]HgCl3 (38).…”

Section: Framework Complexesmentioning

confidence: 99%

“…A solution of 2.16 g (0.006 mol) of HgBra in 80 ml of boiling H20 is added with mechanical stirring to a solution of 0.2 g (0.002 mol) of NH4Br in 100 ml of 0.1 M aq Figure 7. Triargerltosulfonium nilrate, [Ag3S]N03 (66). Ag ions are located at the corners ot the polyhedra and S ions are located at the centers of the polyhedra.…”

Section: Nitronium Complexesmentioning

confidence: 99%

“…Triargentosulfonium Nitrate, [Ag3S]N03 (66). A solution of 10.0 g (0.0588 mol) of AgN03 in 10 ml of 2IV HNO3 is mechanically shaken vigorously with 1.70 ml (0.0282 mol) of CS2 (CAUTION: Flammable and toxic) in a stoppered brown or actinic red flask for 24 h. (An ordinary flask protected from light with metal foil wrapping is satisfactory.)…”

Section: Sulfonium Complexesmentioning

confidence: 99%

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Metallo complexes: An experiment for the undergraduate laboratory

Kauffman¹,

Karbassi²,

Bergerhoff³

1984

J. Chem. Educ.

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While among the great majority of coordination compounds the elementary atoms acting as centers of the complex structure are more electropositive than the elementary atoms which accept the bonding of the adding molecular components, there exists a small group of compounds, for which the opposite is the case and to which attention has recently been drawn (1).With these words, which introduce his treatment of "complex compounds with negative central atoms," Alfred Werner , the founder of coordination chemistry (2), recognized as early as 1909 the existence of a peculiar class of compounds in which the coordination center is a nonmetal surrounded by one or more metal atoms that function as ligands (3). Although these so-called metallo complexes are of great theoretical interest, even their existence is still unknown to most professional chemists, not to mention students of chemistry. Consequently, the syntheses and characterizations of representatives of these scholastically neglected substances are described herein (4). The introduction of such intriguing and exotic compounds into the laboratory curriculum has served not only to increase student motivation but also to add a thought-provoking dimension to the more traditional topics in coordination chemistry.Werner concluded his first discussion of "complex compounds with negative central atoms" with the prophetic words:From the above it is evident that various beginnings for the development of the chemistry of this remarkably peculiar class of compounds exist. In any case, however, the field is much more extensive than is apparent today. It will therefore first be necessary to investigate in which areas the existence of such compounds can be established (la, p. 249).Accordingly, a general background discussion of such compounds will be given prior to the specific preparations to be described in this experiment. DefinitionsBefore Werner was even born, Johann Wilhelm Hittorf , in his classic series of experiments on the migration of ions (1853-1859), established the fundamental distinction between complex salts and double salts by showing that when solutions of salts such as K[Ag(CN)2], K^PtCLt], K^FelCNjcl, and K3[Fe(CN)6] are electrolyzed, the transition metal migrates to the anode (5). Opposed to these complex salts, the bracketed portion of which remains intact as a unit in solution, are the double salts, such as the alums, M(I)2S04-M(II1)2(S04)3-24H20, which dissociate in solution

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Section: Framework Complexesmentioning

confidence: 99%

Section: Nitronium Complexesmentioning

confidence: 99%

Section: Sulfonium Complexesmentioning

confidence: 99%

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Metallo complexes: An experiment for the undergraduate laboratory

Kauffman¹,

Karbassi²,

Bergerhoff³

1984

J. Chem. Educ.

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“…The latter was only obtained if the mixture was heated before filtration. The new compound could also be obtained by precipitating silver nitrate solution with a suitable mixture of sodium sulphate and sulphide, suggesting that it might be (Ag3S)2SO4, the sulphate analogue of the known compound Ag3SNO 3 (Poleck & Thiimmel, 1883;Bergerhoff, 1959). However, the stoichiometry proved to be different.…”

Section: Origin Of Specimensmentioning

confidence: 99%

New crystal data for silver sulphide sulphate, Ag₈S₃SO₄

Hirsch¹

1979

J Appl Cryst

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In Hart & Rodrigues [J. Appl. Cryst. (1978), 11, 248-253] equation (6) AbstractThe title compound was recognized from the new and unexpected powder pattern of aged precipitates obtained by mixing solutions of excess silver nitrate and sodium thiosulphate under specified conditions. The possible crystalline impurities were identified and conditions were established to yield a pure product. The brown microcrystalline material is tetragonal with a=b=7.201; c=10.220 A. It is a solid electrolyte, has an irreversible transition point at 246°C and melts at 405°C. Method of preparation and powder data are given.

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