The extended environment of mononuclear metal centers in protein structures

The objectives of this and the following paper are to identify commonalities and disparities of the extended environment of mononuclear metal sites centering on Cu, Fe, Mn, and Zn. The extended environment of a metal site within a protein embodies at least three layers: the metal core, the ligand group, and the second shell, which is defined here to consist of all residues distant less than 3.5 Å from some ligand of the metal core. The ligands and second-shell residues can be characterized in terms of polarity, hydrophobicity, secondary structures, solvent accessibility, hydrogen-bonding interactions, and membership in statistically significant residue clusters of different kinds. Findings include the following: (i) Both histidine ligands of type I copper ions exclusively attach the Nδ1 nitrogen of the histidine imidazole ring to the metal, whereas histidine ligands for all mononuclear iron ions and nearly all type II copper ions are ligated via the Nɛ2 nitrogen. By contrast, multinuclear copper centers are coordinated predominantly by histidine Nɛ2, whereas diiron histidine contacts are predominantly Nδ1. Explanations in terms of steric differences between Nδ1 and Nɛ2 are considered. (ii) Except for blue copper (type I), the second-shell composition favors polar residues. (iii) For blue copper, the second shell generally contains multiple methionine residues, which are elements of a statistically significant histidine–cysteine–methionine cluster. Almost half of the second shell of blue copper consists of solvent-accessible residues, putatively facilitating electron transfer. (iv) Mononuclear copper atoms are never found with acidic carboxylate ligands, whereas single Mn2+ ion ligands are predominantly acidic and the second shell tends to be mostly buried. (v) The extended environment of mononuclear Fe sites often is associated with histidine–tyrosine or histidine–acidic clusters.

Glutathione-mediated destabilization in vitro of [2Fe-2S] centers in the SoxR regulatory protein.

SoxR is a transcription factor that governs a global defense against the oxidative stress caused by nitric oxide or excess superoxide in Escherichia coli. SoxR is a homodimer containing a pair of [2Fe-2S] clusters essential for its transcriptional activity, and changes in the stability of these metal centers could contribute to the activation or inactivation of SoxR in vivo. Herein we show that reduced glutathione (GSH) in aerobic solution disrupts the SoxR [2Fe-2S] clusters, releasing Fe from the protein and eliminating SoxR transcriptional activity. This disassembly process evidently involves oxygen-derived free radicals. The loss of [2Fe-2S] clusters does not occur in anaerobic solution and is blocked in aerobic solution by the addition of superoxide dismutase and catalase. Although H2O2 or xanthine oxidase and hypoxanthine (to generate superoxide) were insufficient on their own to cause [2Fe-2S] cluster loss, they did accelerate the rate of disassembly after GSH addition. Oxidized GSH alone was ineffective in disrupting the clusters, but the rate of [2Fe-2S] cluster disassembly was maximal when reduced and oxidized GSH were present at a ratio of approximately 1:3, which suggests the critical involvement of a GSH-based free radical in the disassembly process. Such a reaction might occur in vivo: we found that the induction by paraquat of SoxR-dependent soxS transcription was much higher in a GSH-deficient E. coli strain than in its GSH-containing parent. The results imply that GSH may play a significant role during the deactivation process of SoxR in vivo. Ironically, superoxide production seems both to activate SoxR and, in the GSH-dependent disassembly process, to switch off this transcription factor.

Classification of mononuclear zinc metal sites in protein structures

Our study of the extended metal environment, particularly of the second shell, focuses in this paper on zinc sites. Key findings include: (i) The second shell of mononuclear zinc centers is generally more polar than hydrophobic and prominently features charged residues engaged in an abundance of hydrogen bonding with histidine ligands. Histidine–acidic or histidine–tyrosine clusters commonly overlap the environment of zinc ions. (ii) Histidine tautomeric metal bonding patterns in ligating zinc ions are mixed. For example, carboxypeptidase A, thermolysin, and sonic hedgehog possess the same ligand group (two histidines, one unibidentate acidic ligand, and a bound water), but their histidine tautomeric geometries markedly differ such that the carboxypeptidase A makes only Nδ1 contacts, thermolysin makes only Nɛ2 contacts, and sonic hedgehog uses one of each. Thus the presence of a similar ligand cohort does not necessarily imply the same topology or function at the active site. (iii) Two close histidine ligands HXmH, m ≤ 5, rarely both coordinate a single metal ion in the Nδ1 tautomeric conformation, presumably to avoid steric conflicts. Mononuclear zinc sites can be classified into six types depending on the ligand composition and geometry. Implications of the results are discussed in terms of divergent and convergent evolution.

Determination of the binding sites of the proton transfer inhibitors Cd2+ and Zn2+ in bacterial reaction centers

The reaction center (RC) from Rhodobacter sphaeroides couples light-driven electron transfer to protonation of a bound quinone acceptor molecule, QB, within the RC. The binding of Cd2+ or Zn2+ has been previously shown to inhibit the rate of reduction and protonation of QB. We report here on the metal binding site, determined by x-ray diffraction at 2.5-Å resolution, obtained from RC crystals that were soaked in the presence of the metal. The structures were refined to R factors of 23% and 24% for the Cd2+ and Zn2+ complexes, respectively. Both metals bind to the same location, coordinating to Asp-H124, His-H126, and His-H128. The rate of electron transfer from QA− to QB was measured in the Cd2+-soaked crystal and found to be the same as in solution in the presence of Cd2+. In addition to the changes in the kinetics, a structural effect of Cd2+ on Glu-H173 was observed. This residue was well resolved in the x-ray structure—i.e., ordered—with Cd2+ bound to the RC, in contrast to its disordered state in the absence of Cd2+, which suggests that the mobility of Glu-H173 plays an important role in the rate of reduction of QB. The position of the Cd2+ and Zn2+ localizes the proton entry into the RC near Asp-H124, His-H126, and His-H128. Based on the location of the metal, likely pathways of proton transfer from the aqueous surface to QB⨪ are proposed.

Identification of the proton pathway in bacterial reaction centers: Inhibition of proton transfer by binding of Zn2+ or Cd2+

The reaction center (RC) from Rhodobacter sphaeroides converts light into chemical energy through the light induced two-electron, two-proton reduction of a bound quinone molecule QB (the secondary quinone acceptor). A unique pathway for proton transfer to the QB site had so far not been determined. To study the molecular basis for proton transfer, we investigated the effects of exogenous metal ion binding on the kinetics of the proton-assisted electron transfer kAB(2) (QA−•QB−• + H+ → QA(QBH)−, where QA is the primary quinone acceptor). Zn2+ and Cd2+ bound stoichiometrically to the RC (KD ≤ 0.5 μM) and reduced the observed value of kAB(2) 10-fold and 20-fold (pH 8.0), respectively. The bound metal changed the mechanism of the kAB(2) reaction. In native RCs, kAB(2) was previously shown to be rate-limited by electron transfer based on the dependence of kAB(2) on the driving force for electron transfer. Upon addition of Zn2+ or Cd2+, kAB(2) became approximately independent of the electron driving force, implying that the rate of proton transfer was reduced (≥ 102-fold) and has become the rate-limiting step. The lack of an effect of the metal binding on the charge recombination reaction D+•QAQB−• → DQAQB suggests that the binding site is located far (>10 Å) from QB. This hypothesis is confirmed by preliminary x-ray structure analysis. The large change in the rate of proton transfer caused by the stoichiometric binding of the metal ion shows that there is one dominant site of proton entry into the RC from which proton transfer to QB−• occurs.

Identification of the proton pathway in bacterial reaction centers: Both protons associated with reduction of QB to QBH2 share a common entry point

The reaction center from Rhodobacter sphaeroides uses light energy for the reduction and protonation of a quinone molecule, QB. This process involves the transfer of two protons from the aqueous solution to the protein-bound QB molecule. The second proton, H+(2), is supplied to QB by Glu-L212, an internal residue protonated in response to formation of QA− and QB−. In this work, the pathway for H+(2) to Glu-L212 was studied by measuring the effects of divalent metal ion binding on the protonation of Glu-L212, which was assayed by two types of processes. One was proton uptake from solution after the one-electron reduction of QA (DQA→D+QA−) and QB (DQB→D+QB−), studied by using pH-sensitive dyes. The other was the electron transfer kAB(1) (QA−QB→QAQB−). At pH 8.5, binding of Zn2+, Cd2+, or Ni2+ reduced the rates of proton uptake upon QA− and QB− formation as well as kAB(1) by ≈an order of magnitude, resulting in similar final values, indicating that there is a common rate-limiting step. Because D+QA− is formed 105-fold faster than the induced proton uptake, the observed rate decrease must be caused by an inhibition of the proton transfer. The Glu-L212→Gln mutant reaction centers displayed greatly reduced amplitudes of proton uptake and exhibited no changes in rates of proton uptake or electron transfer upon Zn2+ binding. Therefore, metal binding specifically decreased the rate of proton transfer to Glu-L212, because the observed rates were decreased only when proton uptake by Glu-L212 was required. The entry point for the second proton H+(2) was thus identified to be the same as for the first proton H+(1), close to the metal binding region Asp-H124, His-H126, and His-H128.