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By C.B. Anfinsen, John T. Edsall, Frederic M. Richards and David S. Eisenberg (Eds.)

This article, a part of a chain on protein chemistry, covers structural facets of steel liganding to useful teams in proteins, calcium-binding websites in proteins, copper protein buildings, non-heme iron protein chemistry and extra.

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The influence of the Jahn-Teller effect on bond lengths (A) of copper sulfate trihydrate (top) and pentahydrate (bottom). 45 A. , 1979) was searched for this information. Not only did these investigators find that the sulfur atom appeared to have a different radius in different directions but they found that nucleophiles and electrophiles approach it from different directions (Fig. 9). VII. STRENGTHS OF BONDSFROM METALIONSTO LICANDS In analyzing inorganic structures, Brown (1978) extended the “balland-stick” valence models of organic structures to inorganic structures, 22 JENNY P.

23). 92 A) in a heme lacking oxygen. 21. (a) Atomic designations and (b) stereo view of rubredoxin. Fe(I1) [4S]. 8 8, above the plane of the heme. 75 h;) can then fit in the heme plane (Hoard, 1966). , 1983). A distal uncoordinated histidine serves to control the oxygen-binding site, inhibiting the binding of carbon monoxide; this occurs because carbon monoxide binds iron in a linear fashion, while oxygen binds in a bent manner (Scheidt and Lee, 1987). GLUSKER \ cys41 Cysl8 cys35 FIG. 22. (a) Atomic designations and (b) stereo view of ferredoxin.

Brown has studied rules for cation coordination in inorganic structures, including minerals (Brown, 1987). , 1983) formed the basis from which the “bond valence model” was derived. Such analyses require that the sum of the partial negative charges contributed by each ligand around a cation must be the total cation charge. Thus, if a sodium ion, Na+, has six oxygen ligands, each of these ligands contributes a charge of -&. However, ligands with shorter Na+... 0 distances contribute a negative charge greater in value than Q, while those with longer Na+...

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