Alternate arrangements of two different metals at chemically-equivalent binding sites on a circle

Journal of the American Chemical Society

Volumn 131, Issue 13, 2009, Pages 4592-4593

  Hiraoka, Shuichi ^a,b   Goda, Mitsuyoshi ^a,b   Shionoya, Mitsuhiko ^a,b  

^a UNIVERSITY OF TOKYO   (Japan)

^b JAPAN SCIENCE AND TECHNOLOGY AGENCY   (Japan)

Author keywords

[No Author keywords available]

Indexed keywords

DIVALENT METAL ION; ELECTROSTATIC INTERACTIONS;

BINDING ENERGY; BINDING SITES; DYES; MERCURY (METAL); METAL IONS; TRACE ANALYSIS;

METALS;

COPPER; MERCURY; SILVER;

ARTICLE; BINDING SITE; CHEMICAL STRUCTURE; COMPLEX FORMATION; ELECTROSPRAY MASS SPECTROMETRY; PROTON NUCLEAR MAGNETIC RESONANCE;

EID: 67949104898     PISSN: 00027863     EISSN: None     Source Type: Journal    
DOI: 10.1021/ja9006113     Document Type: Article

References (15)

1. (a) Burdinski, D.; Birkelbach, F.; Weyhermueller, T.; Floerke, U.; Haupt, H.-J.; Lengen, M.; Trautwein, A. X.; Bill, E.; Wieghardt, K.; Chaudhuri, P. Inorg. Chem. 1998, 37, 1009.
2. (b) Armstrong, D. R.; Clegg, W.; Drummond, A. M.; Liddle, S. T.; Mulvey, R. E. J. Am. Chem. Soc. 2000, 122, 11117.
3. (c) Bashall, A.; Cole, J. M.; Garcia, F.; Primo, A.; Rothenberger, A.; McPartlin, M.; Wright, D. S. Inorg. Chim. Acta 2003, 354, 41.
4. (d) Dikarev, E. V.; Andreini, K. W.; Petrukhina, M. Inorg. Chem. 2004, 43, 3219.
5. (e) Schmittel, M.; Kalsani, V.; Bats, J. W. Inorg. Chem. 2005, 44, 4115.
6. (f) Hull, K. L.; Carmichael, I.; Noll, B. C.; Henderson, K. W. Chem.-Eur. J. 2008, 14, 3939.
7. (a) Uppadine, L. H.; Gisselbech, J.-P.; Kyritsakas, N.; Nättinen, K.; Rissanen, K.; Lehn, J.-M. Chem.-Eur. J. 2005, 11, 2549.
8. (b) Bassani, D. M.; Lehn, J.-M.; Serroni, S.; Puntoriero, F.; Campagna, S. Chem.-Eur. J. 2003, 9, 5936.
9. (c) Akine, S.; Taniguchi, T.; Saiki, T.; Nabeshima, T. J. Am. Chem. Soc. 2005, 127, 540.
10. (d) Hiroaka, S.; Tanaka, T.; Shionoya, M. J. Am. Chem. Soc. 2006, 128, 13038.
11. Metal complexation of 3 bearing six nonsubstituted oxazoline rings was not successful in solution under the same conditions because of the extremely low solubility of both the metal-free ligand and the resulting metal complexes.
12. The [Cu622]6+ complex was stable under air for several months, while Cu(I) complexes generally are easily oxidized. Therefore, there was no need for special care in the preparation of this complex.
13. The 1H NMR spectrum of [Hg622]12+ differed from those for [Ag622]6+ and [Cu622]6+. For example, with [Hg622]12+, four resonances for the aromatic protons were found in the range of 7.2-7.5 ppm, and the two Ha and Hd protons in the oxazoline rings were inequivalent. This is probably due to structural differences, such as the helicity and/or conformational rigidity of the [Hg622]12+ complex.
14. Diastereotopic proton signals for the oxazoline rings of Ag3Hg322 · (OTf)9 complex were observed at 223 K, indicating that the complex has a helicity.
15. The identity of the counteranion also affects the stability of the complexes. For example, when N(CF3SO2)2 - (NTf2 -) was used as the counteranion, the stability of the Ag3Hg322 · (NTf2)9 complex, in which the two kinds of metal ions are alternately arranged, was lower than that of the triflate counterpart (Figure S10). Molecular modeling of the [Ag3Hg322]9+ complex (Figure S11) suggests that the counteranions weakly interact with the linear two-coordinate Ag+ and Hg2+ ions by the electrostatic force.