Sec. Microbiological Chemistry and Geomicrobiology
Volume 3 - 2012 | https://doi.org/10.3389/fmicb.2012.00057
Toward a mechanistic understanding of anaerobic nitrate-dependent iron oxidation: balancing electron uptake and detoxification
- 1 Department of Plant and Microbial Biology, University of California Berkeley, Berkeley, CA, USA
- 2 Department of Civil and Environmental Engineering, University of California Berkeley, Berkeley, CA, USA
The anaerobic oxidation of Fe(II) by subsurface microorganisms is an important part of biogeochemical cycling in the environment, but the biochemical mechanisms used to couple iron oxidation to nitrate respiration are not well understood. Based on our own work and the evidence available in the literature, we propose a mechanistic model for anaerobic nitrate-dependent iron oxidation. We suggest that anaerobic iron-oxidizing microorganisms likely exist along a continuum including: (1) bacteria that inadvertently oxidize Fe(II) by abiotic or biotic reactions with enzymes or chemical intermediates in their metabolic pathways (e.g., denitrification) and suffer from toxicity or energetic penalty, (2) Fe(II) tolerant bacteria that gain little or no growth benefit from iron oxidation but can manage the toxic reactions, and (3) bacteria that efficiently accept electrons from Fe(II) to gain a growth advantage while preventing or mitigating the toxic reactions. Predictions of the proposed model are highlighted and experimental approaches are discussed.
In recent years, significant progress has been made toward understanding the biochemical mechanisms used by bacteria to catalyze the aerobic and anaerobic oxidation of Fe(II) in the environment. Recent reviews focus on aerobic/microaerobic iron oxidation (Emerson et al., 2010) and iron oxidation by acidophiles and anoxygenic phototrophs (Bird et al., 2011), however a number of microorganisms have been described which can couple iron oxidation to nitrate reduction (Chaudhuri et al., 2001; Weber et al., 2001, 2006a,b; Finneran et al., 2002; Lack et al., 2002; Muehe et al., 2009) in the absence of oxygen and light. The growth benefit from anaerobic iron oxidation varies widely. In both photosynthetic and nitrate reducing bacteria, oxidation of Fe(II) may represent an important detoxification strategy (Muehe et al., 2009; Poulain and Newman, 2009), and in some cases may have also evolved into a metabolic strategy (Widdel et al., 1993; Croal et al., 2007; Jiao and Newman, 2007; Muehe et al., 2009; Weber et al., 2009; Chakraborty et al., 2011). In this paper, we suggest that the success of an iron-oxidizing microorganism depends on the extent to which electron donation from Fe(II) can be controlled and toxic reactions prevented or managed. We propose working models to analyze the results of experiments aimed at elucidating the mechanisms of iron oxidation by anaerobic nitrate reducing bacteria. We also highlight some of the predictions of the models that future experiments should address. Our intention is not to exhaustively review the literature, but rather to highlight some of the salient features of anaerobic nitrate-dependent iron oxidation and provide insight for new research directions.
Rusting Away in the Dark, without Oxygen: Evidence for Anaerobic Nitrate-Dependent Iron Oxidation by Environmental Bacteria
Bacterial species that couple the oxidation of Fe(II) to nitrate reduction have been isolated from a wide range of habitats and are phylogenetically diverse (Hafenbradl et al., 1996; Straub et al., 1996; Chaudhuri et al., 2001). Iron-oxidizing microbes have been demonstrated to oxidize both soluble and insoluble Fe(II) (Widdel et al., 1993; Chaudhuri et al., 2001; Weber et al., 2001, 2006c), and to produce a variety of insoluble Fe(III) mineral products (Machulla et al., 1998; Straub and Buchholz-Cleven, 1998; Chaudhuri et al., 2001; Weber et al., 2006c). Although the metabolism is based on thermodynamically favorable redox reactions (Koppenol, 1996; Bartberger et al., 2002; Shafirovich and Lymar, 2002; Dutton et al., 2005; Flores-Santana et al., 2011), little is known about the mechanisms used by anaerobic neutrophilic nitrate-dependent iron oxidizers (Weber et al., 2006a; Bird et al., 2011). However, a few studies do suggest an energetic benefit from this metabolism for the organisms involved (Muehe et al., 2009; Weber et al., 2009). Figure 1 presents several conceivable mechanisms for obtaining energetic benefit from iron oxidation catalyzed by anaerobic denitrifying bacteria. Some of these mechanisms may be inducible in specialized iron-oxidizing microorganisms, while others may be general to all nitrate reducing bacteria. One of these mechanisms (electron sparing) includes both enzymatically mediated components and abiotic interactions between Fe(II) and reactive intermediates resulting in a net energy gain. These mechanisms may be mutually exclusive, but based on reactive species formed during metabolism, it is more likely that hybrid abiotic/biotic mechanisms are functioning. To the best of our knowledge such hybrid abiotic/biotic mechanisms represent a novel metabolic process in microbiology. Below follows a brief description of these mechanisms and the evidence to support their existence.
Figure 1. Possible mechanisms for energetic benefit from iron oxidation coupled to nitrate reduction. (A) A true Fe(II):menaquinone oxidoreductase accepts electrons from iron and reduces the quinone pool, (B) Nar accepts electrons from Fe(II) and reduces nitrate cytoplasmically, consuming protons to generate a PMF, (C) the cytochrome bc1 complex accepts electrons from Fe(II) and reduces the quinone pool, (D) more protons are pumped per electron at Nar than other nitrogen oxide reductases. If abiotic reactions dominate for the reduction of an energetic benefit is conferred through an electron sparing mechanism. Nar, nitrate reductase; Nir, nitrite reductase; Nor, nitric oxide reductase; Nos, nitrous oxide reductase; QH2, reduced quinone; Q, oxidized quinone; bc1, cytochrome bc1; cyt c, cytochrome c.
A Dedicated Fe(II) Oxidoreductase
A dedicated Fe(II): menaquinone oxidoreductase protein, or protein complex, could oxidize iron at the cell surface or in the periplasm and reduce the quinone pool, providing reducing equivalents for downstream nitrogen oxide reductases (Figure 1A) allowing for proton motive force (PMF) generation. This mechanism predicts inducibility of iron oxidation and the expression of a specific protein or proteins in response to Fe(II).
Direct Electron Donation to Nitrate Reductase
In this model a standard membrane bound Nar could serve as the combined Fe(II) oxidase and nitrate reductase. If Nar can accept electrons from Fe(II) to catalyze cytoplasmic reduction to and H2O, two protons are consumed in the cytoplasm without the need for electrons from NADH resulting in an enhanced PMF (Figure 1B). Although, this mechanism may be inducible, it is unlikely as Nar will be expressed during nitrate reducing conditions regardless. As such, it could be an inadvertent mechanism of dissimilatory nitrate reduction using Nar. Transport into the cytoplasm by antiporters without consumption of periplasmic protons is necessary for this mechanism to generate a PMF. It is important to note that nitrate reductases with periplasmic sites for such as Nap, consume periplasmic protons to reduce nitrate and no energetic benefit would result from Fe(II) electron donation to catalyze reduction by Nap.
Cytochrome bc1 Complex Mediated Fe(II) Oxidation
A third possibility is that the cytochrome bc1 complex can accept electrons from Fe(II) and reduce the quinone pool This is similar to the proposed mechanism that Acidithiobacillus and anoxygenic phototrophs use to generate NADH from Fe(II) oxidation (Figure 1C; Bird et al., 2011). In these metabolisms, the cytochrome bc1 complex is proposed to be involved in reverse electron transfer to reduce the quinone pool (Bird et al., 2011). The exact mechanism and the net proton translocation associated with reverse electron transfer by bc1 is not well understood, but is thought to be at the expense of the PMF (Ferguson and Ingledew, 2008). For neutrophilic iron oxidation, the redox potential of Fe(III)/Fe(II) is low enough to reduce menaquinone (E°′ = −0.074 V; Wagner et al., 1974; Schoepp-Cothenet et al., 2009). However, for this mechanism to generate a PMF, the quinone pool must obtain protons from the cytoplasm upon reduction by the bc1 complex, and release those protons into the periplasm upon oxidation. Coupled to a quinol dehydrogenase, this would provide net proton translocation (Note: some NorBC are quinol dehydrogenases; Kraft et al., 2011). We envision that alternating fluxes of acetate and nitrate in the environment could be harnessed by a bc1 ferroxidase in this way. When high acetate concentrations are present, electrons flow through cytochrome c to sustain denitrification, and iron oxidation by bc1 is minimal. As acetate becomes scarce, the quinone pool is largely oxidized, and electrons from iron could be used to reduce the quinone pool at bc1.
A fourth mechanism for obtaining an energetic benefit from Fe(II) oxidation involves differential electron flow to the terminal reductases. If more protons are translocated per electron at the nitrate reductase (Nar) than at downstream reductases coupled to bc1, then a shift in electron flow to Nar would be beneficial (Figure 1D). If this is the case, under heterotrophic growth conditions with excess electron acceptor (e.g., ), abiotic redox reactions between Fe(II) and and other nitrogen oxides would allow greater net proton translocation per electron from Complex I. We refer to this phenomenon as electron sparing. More nitrate would be consumed in such a mechanism, but an energetic benefit to the organism would be gained per mole of electron donor (i.e., organic co-substrate, H2). This mechanism only applies to iron oxidizers when a co-substrate is available as an electron donor, and could be more pronounced when abiotically produced nitrogen oxide gases are continuously removed, as in flow through experimental setups. However, when electron acceptor is limiting, such reactions are likely to lead to a growth disadvantage due to a loss of electron accepting capacity. This hypothesis can be tested by looking for differences in growth on Fe(II) under donor or acceptor limiting conditions in batch culture. It is also important to emphasize that the location of the Fe(II) reaction with is potentially very important in determining the consequences for the bacterial cell. If the reaction happens in the periplasm, insoluble Fe(III) crusts may be harmful, but if the reaction happens outside of the cell, the could react with insoluble Fe(II) in minerals without negative consequences for the cell.
Thinking Outside of the Cell: Evidence for Abiotic Reduction of Nitrogen Oxides Catalyzed by Soluble Fe(II) and Insoluble Fe(II) Minerals
Regardless of whether abiotic reactions of nitrogen oxides and Fe(II) can lead to an energetic benefit through electron sparing, uncoupling the denitrification pathway is likely to create a significant flux of toxic reactive nitrogen species. The characterization of these products and the mechanisms whereby microorganisms cope with the toxicity will lead to an understanding of the benefit or cost of microbial iron oxidation.
The abiotic reaction of nitrate () with soluble Fe(II) is slow (Moraghan and Buresh, 1977). However, the reaction between () and soluble Fe(II) is rapid (Moraghan and Buresh, 1977). The products of the abiotic reactions vary with pH and include NO, N2O, and (Chalamet, 1973; Moraghan and Buresh, 1977). Copper (Cu2+) or silver (Ag+) can catalyze abiotic reduction coupled to Fe(II) oxidation at room temperature and neutral pH (Moraghan and Buresh, 1977; Ottley et al., 1997). Green rusts (GR), mixed Fe(II)/Fe(III) hydroxides, can also catalyze the reduction of nitrogen oxides (Figure 2A). As with soluble Fe(II), GR reactions with and produce NO, N2O, and NH4 depending on the pH (Figure 2A; Summers and Chang, 1993; Hansen et al., 1994, 1996). It has further been observed that the intercalating anion in the GR mineral affects the rate of reduction. GR intercalated with chloride (Cl−) has a 30- to 40-fold faster rate of reduction compared with GR intercalated with sulfate (Hansen et al., 2001). A number of microorganisms produce GR as intermediates or products of nitrate-dependent iron oxidation (Chaudhuri et al., 2001; Lack et al., 2002). Therefore, it is possible that abiotic reactions catalyzed by GR can contribute to nitrate removal in iron-oxidizing microcosms and cultures during the growth phase, after growth has stopped, or in non-growth cultures in which GR has formed.
Figure 2. Possible reactions resulting in toxicity and energetic loss during iron oxidation coupled to nitrate reduction and potential microbial responses. (A) Green rusts are capable of catalyzing nitrate reduction coupled to iron oxidation. If they are produced, they will consume and compete with bacteria for electron acceptor. (B) will rapidly react with Fe(II) to form NO. NO can be further reduced, but can also bind to metalloproteins and disrupt electron transport chains. Upregulation of Nor or other NO reductase proteins could protect cells from NO. (C) Soluble Fe(II) or Fe(III) could be exported from cells by heavy metal efflux pumps before it reacts with cellular components (in the case of Fe(II)) or precipitates to form mineral crusts (in the case of Fe(III)). (D) Extracellular polysaccharides or pili may scaffold the precipitation of Fe(III) outside of cells, or a local low pH or chelators may prevent the precipitation of Fe(III) in the periplasm.
A Wrench in the Gears: Evidence for Uncoupling of Bacterial Denitrification by Fe(II)
In Escherichia coli, it has been known for some time that the presence of millimolar Fe(II) and leads to an uncoupling of electron transport and dissimilatory nitrate reduction resulting in the production of high micromolar to millimolar levels of nitric oxide (NO) and nitrous oxide (N2O; Brons et al., 1991; Figure 2B). Further evidence for uncoupling of nitrate reduction electron transport by Fe(II) was observed with Shewanella putrefaciens 200 and Paracoccus denitrificans (Cooper et al., 2003; Coby and Picardal, 2005). The location and form of Fe(II), the pH, and the nitrogen oxide starting material are all likely to contribute to the products of abiotic uncoupling reactions during microbial nitrate and nitrite reduction (Chalamet, 1973; Moraghan and Buresh, 1977; Hansen et al., 2001).
As the reaction between Fe(II) and is slow, the first likely point of uncoupling is Fe(II) oxidation by to produce NO and Fe(III) as initial products (Figure 2B). In previous studies, NO was found to be produced at a higher rate and accumulate in cultures of heterotrophically grown nitrate reducers in the presence of Fe(II) (Brons et al., 1991). NO is a gas, and will partition into the headspace of sealed culture tubes, potentially representing a significant loss of electron accepting equivalents in open systems. However, NO is also toxic, and can react with metalloproteins in the cell and components of the electron transport chain, and in the presence of redox active metals can nitrosate thiols (Beckman and Koppenol, 1996). Fortunately, the respiratory NO reductase (Nor) of denitrifying bacteria can reduce NO to less toxic products, and other enzymes involved in the reduction of nitrogen oxides can play a protective role in addition to their respiratory function (Gardner et al., 2002; Gomes et al., 2002; Mills et al., 2008). Nor is independently regulated from other components of the denitrification pathway and can be upregulated to reduce excess NO (Rodionov et al., 2005).
Little should accumulate in denitrifying cultures as a result of fast abiotic reactions between and Fe(II). Contrary to this prediction, some previous studies have measured nitrite accumulation and attributed this finding to the inhibition of nitrite reductase by Fe(III) precipitation (Straub et al., 1996; Weber et al., 2006b). However, it should be noted that NO (and other nitrogen oxides) will rapidly react with O2 to form nitrite (Feelisch, 1991; Beckman and Koppenol, 1996). If samples are not kept anaerobic during sample preparation for nitrite analysis, the nitrite analyzed may also represent other reactive nitrogen species (Straub et al., 1996; Weber et al., 2006b). Some researchers have suggested that may function as a shuttle to oxidize iron (Miot et al., 2009a; Chakraborty et al., 2011). We find this hypothesis plausible, and have also proposed that abiotic reactions between Fe(II) and could lead to an energetic benefit through an electron sparing mechanism (Figure 1D).
Excess NO produced by bacteria can also further react to form other compounds. NO will bind to free Fe(II) outside of the cell to form stable iron–nitrosyl complexes (Brons et al., 1991; Figure 2B), but will not bind tightly to Fe(III). Thus, as Fe(II) oxidation continues, bound NO will be released. Further reduction of NO can produce the high energy intermediate nitroxyl (NO−, HNO) which can react with thiols to form hydroxylamine (Flores-Santana et al., 2011), or with another nitroxyl to form N2O (Beckman and Koppenol, 1996; Flores-Santana et al., 2011; Figure 2B). Some evidence for nitroxyl as an intermediate in denitrification exists (Turk and Hollocher, 1992), and though the redox potential of the NO/NO− couple is −0.8 V vs. SHE at pH 7 (Bartberger et al., 2002), the evidence for its presence and a role in other biological systems is increasing. It is possible that a nitroxyl-like species is an intermediate in biological and chemical denitrification pathways (Flores-Santana et al., 2011).
In a Metal Cage: Fe(II) Diffusion into Cells and Cell Encrustation by the Formation of Periplasmic and Outer Membrane Iron Oxide Minerals
Iron-oxidizing bacteria produce insoluble Fe(III) minerals as a product. In some cases, these insoluble minerals have been found associated with the periplasm of cells or on the cell surface. Precipitation outside of cell was observed for Rhodobacter capsulatus SW2 (Kappler and Newman, 2004), and a local drop in pH around the cells was proposed to be involved in preventing precipitation in the periplasm (Kappler and Newman, 2004). In contrast, precipitates in the periplasm were observed in the nitrate-dependent iron oxidizer Acidovorax sp. Strain BoFeN1 (Kappler et al., 2005, 2010; Miot et al., 2009b). More specifically, these precipitates appear to be initially localized to the periplasmic face of the inner membrane (Miot et al., 2011).
The insolubility of Fe(III) creates a serious problem for iron oxidizers. If ferric minerals begin to crystallize in the periplasm or on the surface of cells, damage to membranes, proteins, and other cellular components will likely ensue, and under extreme cases, the permeability of the cells to soluble nutrients may be impaired. If Fe(II) enters the cytoplasm, it can replace other metals in proteins, and participate in damaging redox reactions (Crichton, 2009). Cellular Fe(II) homeostasis is carefully controlled in microbes by the activity of metalloregulatory proteins such as the ferric uptake regulator, Fur (Crichton, 2009). Efflux pumps are widely used by bacteria for the export of toxic metal ions, and at the expense of ATP, provide a means of exporting metals from the cell (Nies, 2003). Most studies investigating transcriptional responses of microorganisms to iron have focused on iron uptake under iron limiting conditions, but environmental conditions certainly exist where a cell is faced with iron overload. It seems likely that under high iron conditions, efflux pumps would be upregulated (Figure 2C). Consumption of ATP by these pumps may attenuate any energy gains as a result of Fe(II) oxidation by the organism. Although significant research effort has focused on these efflux pumps, most studies have looked at their expression in the presence of metals other than Fe(II) (Nies, 2003).
It has been suggested that Fe(II) bound to cell surface minerals can further catalyze denitrification reactions (Coby and Picardal, 2005), and that these mineral deposits may prevent the diffusion of soluble electron acceptors into the cell. It appears that some bacteria are able to avoid periplasmic encrustation, but the mechanism for exporting the Fe(III) before it precipitates is not known. It has been suggested that a local low pH in the periplasm and outside of cells could prevent Fe(III) precipitation, and extracellular polysaccharide fibers or pili may provide a scaffold for mineralization outside of the cell (Figure 2D; Miot et al., 2009b).
A Balancing Act: Harnessing Electrons from Fe(II) and Avoiding Toxicity
Electrons from the oxidation of Fe(II) are thermodynamically poised to reduce (Koppenol, 1996; Bartberger et al., 2002; Shafirovich and Lymar, 2002; Dutton et al., 2005; Flores-Santana et al., 2011), but the kinetics of the abiotic reactions are slow (Moraghan and Buresh, 1977). Therefore, high rates of nitrate-dependent Fe(II) oxidation observed in many studies indicate that Fe(II) is enzymatically coupled to the reduction of nitrate to at least nitrite. This is further supported by the results of washed cell suspension experiments where nitrate-dependent oxidation occurs rapidly with Fe(II) as the sole electron donor (Chaudhuri et al., 2001; Lack et al., 2002; Weber et al., 2006b). If the reactions were entirely abiotic, the rate of Fe(II) oxidation should not differ from the heat-killed controls.
A number of bacteria are capable of growth in the presence of Fe(II) (Weber et al., 2006a), and in some cases, growth benefit from neutrophilic iron oxidation has been reported (Muehe et al., 2009; Weber et al., 2009; Chakraborty et al., 2011). It is clear from these studies that the culture conditions can greatly affect the growth benefit associated with iron oxidation (Weber et al., 2009; Chakraborty et al., 2011). What is not clear, however, are the exact mechanisms whereby diverse species of bacteria harness Fe(II) electrons in the presence of competing abiotic reactions with nitrogen oxides.
Our central hypothesis is that the mechanisms used by neutrophilic anaerobic nitrate-dependent iron-oxidizing bacteria likely exist along a continuum from purely abiotic reactions between microbially produced nitrogen oxides to mixed biotic/abiotic mechanisms involving direct electron donation from iron to cellular components. This fascinating and geochemically important process may also be unique in that the microbial metabolisms themselves might take advantage of abiotic reactions, for example by using as a shuttle (Miot et al., 2009a; Chakraborty et al., 2011), or through the electron sparing hypothesis in Figure 1D. With the growing number of pure isolates of robust iron oxidizing microorganisms, we are optimistic that the mechanistic proposals in this paper can be tested in the laboratory.
Conflict of Interest Statement
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
Research on microbial Fe(II) oxidation in the John D. Coates laboratory is supported by funding from the Energy Biosciences Institute, CA, USA.
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Keywords: nitrate dependent ferrous iron oxidation, NDFO, Fe(II) oxidoreductase, electron sparing, Acidovorax
Citation: Carlson HK, Clark IC, Melnyk RA, and Coates JD (2012) Toward a mechanistic understanding of anaerobic nitrate-dependent iron oxidation: balancing electron uptake and detoxification. Front. Microbio. 3:57. doi: 10.3389/fmicb.2012.00057
Received: 03 November 2011;
Paper pending published: 07 December 2011;
Accepted: 02 February 2012; Published online: 20 February 2012.
Edited by:Eric Roden, University of Wisconsin–Madison, USA
Reviewed by:Amy Michele Grunden, North Carolina State University, USA
Flynn Picardal, Indiana University, USA
Copyright: © 2012 Carlson, Clark, Melnyk and Coates. This is an open-access article distributed under the terms of the Creative Commons Attribution Non Commercial License, which permits non-commercial use, distribution, and reproduction in other forums, provided the original authors and source are credited.
*Correspondence: John D. Coates, Department of Plant and Microbial Biology, University of California Berkeley, Berkeley, CA 94720, USA. e-mail: firstname.lastname@example.org