Electron Donor Utilization and Secondary Mineral Formation during the Bioreduction of Lepidocrocite by Shewanella putrefaciens CN32

Probably not a substantial claim. The paper’s conclusions may not depend on it. It may state two separate claims as one.

Formate and lactate are established electron donors for DIR by S. putrefaciens CN32 and Shewanella spp. in general.

“Formate and lactate are established electron donors for DIR by S. putrefaciens CN32 [25,33,44,48] as well as Shewanella spp. in general [16,34,46,52,53,[71][72][73][74][75]77].”

• Also stated in: § 4.1. Electron Donor Utilization and Dissimilatory Iron(III) Reduction · boosted

  “Formate and lactate are established electron donors for DIR by S. putrefaciens CN32 [25,33,44,48] as well as Shewanella spp. in general [16,34,46,52,53,[71][72][73][74][75]77].”

• cites [25] Zachara, 1998, Bacterial reduction of crystalline Fe3+ oxides in single phase suspension and subsurface materials, Am. Mineral. sourcePartly supported

  The Experimental Procedures identify S. putrefaciens CN32 and state that sodium lactate was added as the electron donor; Biogenic mineralization likewise describes lactate-driven Fe reduction. The passages found do not establish formate as an electron donor or extend this result to Shewanella species generally (searched: formate electron donor CN32; formate lactate Shewanella). (LLM, conf=0.87)

  Experimental — accuracy not yet measured
• cites [33] Fredrickson, 1998, Biogenic iron mineralization accompanying the dissimilatory reduction of hydrous ferric oxide by a groundwater bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [44] Gorski, 2010, Effects of oxyanions, natural organic matter, and cell density on the bioreduction of lepidocrocite (g-FeOOH) and secondary mineral formation, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [48] Kukkadapu, 2004, Biotransformation of two-line silica-ferrihydrite by a dissimilatory Fe(III)-reducing bacterium: Formation of carbonate green rust in the presence of phosphate, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [16,34,46,52,53,[71][72][73][74][75]77]Not matched

  Couldn’t be matched to a paper in Crossref, so it can’t be checked.

It may state two separate claims as one.

In the absence of an exogenous electron donor, lepidocrocite reduction by S. putrefaciens CN32 was limited; within 72 days only 3.6 mM Fe(II) was produced.

“In the absence of an exogenous electron donor, lepidocrocite reduction by S. putrefaciens CN32 was limited; within 72 days only 3.6 mM Fe(II) was produced.”

It may state two separate claims as one.

The presence of specific anions had a significant effect on both the rate and extent of Fe(II) production, which were highest in the presence of carbonate.

“The presence of specific anions had a significant effect on both the rate and extent of Fe(II) production, which were highest in the presence of carbonate (Table 1).”

It may state two separate claims as one.

After the lag periods, Fe(II) production proceeded at similar rates in each lactate system leading to production of 56 and 59 mM total Fe(II) in chloride- and sulfate-amended systems, respectively.

“After the corresponding lag periods, Fe(II) production proceeded at similar rates (Table 1) in each system leading to production of 56 and 59 mM total Fe(II) in the chloride-and sulfate-amended systems, respectively.”

It may state two separate claims as one.

Bioreduction of lepidocrocite by S. putrefaciens CN32 was immediate and sustained when serine was provided as electron donor; nearly 90% of Fe(II) production occurred within first 10 days in both chloride- and sulfate-amended systems.

“The bioreduction of lepidocrocite by S. putrefaciens CN32 was immediate and sustained when serine was provided as the electron donor; nearly 90% of Fe(II) production occurred within the first 10 days in both the chloride-and sulfate-amended systems (Figure 14).”

It may state two separate claims as one.

In pyruvate systems, Fe(II) production was accompanied by complete depletion of pyruvate and accumulation of acetate.

“Fe(II) production was accompanied by complete depletion of pyruvate and accumulation of acetate.”

It may state two separate claims as one.

Compared to formate, lactate, and NAG, initial Fe(II) production was higher with pyruvate (7 mM within 6.5 h) and overall bioreduction of lepidocrocite was substantially faster, with >90% of total Fe(II) production occurring within first 10 days in both chloride- and sulfate-amended systems.

“Compared to formate, lactate, and NAG, the initial Fe(II) production was higher with pyruvate (7 mM within 6.5 h) and the overall bioreduction of lepidocrocite was substantially faster, with >90% of the total Fe(II) production occurring within the first 10 days; both the chloride-and sulfate-amended systems followed essentially the same trajectory (Figure 12).”

It may state two separate claims as one.

In our experimental systems we typically observed formation of either green rust or siderite, except in NAG-amended systems, where green rust and a minor amount of siderite (<30% of Fe(II)) were observed.

“In our experimental systems we typically observed formation of either green rust or siderite, except in the NAG-amended systems, where green rust and a minor amount of siderite (<30% of Fe(II)) were observed.”

It may state two separate claims as one.

In both NAG systems, Fe(II) production was accompanied by consumption of NAG and accumulation of acetate; after an initial pH increase to ~8.1, pH gradually decreased to ~7.6 by day 106.

“In both systems, Fe(II) production was accompanied by consumption of NAG and accumulation of acetate and after an initial increase in pH to ~8.1, the pH gradually decreased to ~7.6 by day 106 (Figure 9).”

It may state two separate claims as one.

In lactate systems, ~2.5 moles of Fe(II) was produced per mole of lactate consumed, substantially less than 4 moles expected from oxidation of lactate to acetate and carbon dioxide.

“In the case of lactate, ~2.5 moles of Fe(II) was produced per mole of lactate consumed, which is substantially less than 4 moles of Fe(II) per mole of lactate based on the oxidation of lactate to acetate and carbon dioxide (lactate → acetate + CO 2 = 4e -).”

It may state two separate claims as one.

Approximately 2 moles of Fe(II) were produced for each mole of formate consumed by S. putrefaciens CN32, consistent with stoichiometry of formate oxidation to carbon dioxide (2e-).

“Approximately 2 moles of Fe(II) produced for each mole of formate consumed (Table 1) by S. putrefaciens CN32, consistent with the stoichiometry of formate oxidation to carbon dioxide (formate  CO2 = 2e -) (Table 1).”

It may state two separate claims as one.

In serine systems, Fe(II) production was concurrent with acetate production, and pyruvate was observed as a transient species.

“We were unable to measure serine concentrations, but Fe(II) production was concurrent with acetate production, and pyruvate was observed as a transient species.”

It may state two separate claims as one.

Carbonate green rust formed in the chloride- and carbonate-amended H2 systems and sulfate green rust formed in the sulfate-amended H2 system.

“Carbonate green rust formed in the chloride-and carbonateamended systems and sulfate green rust formed in the sulfate-amended system (Figure 3).”

It may state two separate claims as one.

In the sulfate-amended NAG system, sulfate green rust formation was first observed at 7 days, followed by carbonate green rust at day 38 and siderite at day 69.

“Sulfate green rust formation was first observed at 7 days after inoculation, followed by the appearance of carbonate green rust at day 38 and siderite at day 69 (Figure 10).”

It may state two separate claims as one.

In the chloride-amended NAG system, ~3 mM Fe(II) was produced within first 24 h and there was minimal change over next 24 days.

“Within the first 24 h after inoculation, ~3 mM Fe(II) was produced in the chloride-amended system and there was minimal change over the next 24 days (Figure 9).”

It may state two separate claims as one.

In the sulfate-amended formate systems, sulfate green rust was observed by day 9, by day 15 both sulfate and carbonate green rust were present, and by day 62 only carbonate green rust was detected.

“In the sulfate-amended systems, indications of sulfate green rust were observed by day 9, by day 15 both sulfate and carbonate green rust were present, and by day 62 only carbonate green rust was detected (Figure 6).”

It may state two separate claims as one.

In sulfate-amended lactate systems, sulfate green rust was observed by day 7, and by day 17 both sulfate and carbonate green rust were present; both were present at day 62.

“In the sulfate-amended systems, indications of sulfate green rust were observed by day 7, and by day 17 both sulfate and carbonate green rust were present (Figure 8); unlike the sulfate-amended formate system, both sulfate and carbonate green rust were present at the end of the experiment (day 62).”

The quote only partly states this claim.

Pyruvate was observed as a transient intermediate during Fe(III) reduction in serine-amended systems.

“pyruvate was observed as a transient intermediate during Fe(III) reduction.”

It may state two separate claims as one.

In the formate systems, pXRD and Mössbauer spectroscopy indicated complete removal of lepidocrocite accompanied by formation of green rust.

“Analysis of the solids by pXRD (Figure 6) and Mössbauer spectroscopy (Table 2) indicates complete removal of lepidocrocite accompanied by the formation of green rust.”

It may state two separate claims as one.

In lactate systems, initial pH increase from 7.5 to 8.2 and a pulse of Fe(II) production (~4 mM) within first 24 h was followed by a lag in Fe(II) production lasting ~27 days and ~17 days in chloride- and sulfate-amended systems, respectively.

“As observed with formate, there was an initial increase in pH from 7.5 to 8.2 and a pulse of Fe(II) production (~4 mM) within the first 24 h, that was followed by a lag in Fe(II) production lasting ~27 days and ~17 days in the chloride-and sulfate-amended systems, respectively (Figure 7).”

It may state two separate claims as one.

With increasing a[HCO3-], the stability field of siderite increases and the stability fields of carbonate green rust and ferrous hydroxide shift to higher pH.

“With increasing a[HCO 3 -] the stability field of siderite increases and the stability fields of carbonate green rust and ferrous hydroxide shift to higher pH.”

It may state two separate claims as one.

Fe(II) concentrations approached steady state within 3 days and were largely unaffected by replenishment of headspace H2 or re-inoculation with freshly cultured S. putrefaciens CN32.

“Fe(II) concentrations approached steady state within 3 days and were largely unaffected by replenishment of headspace H2 or re-inoculation with freshly cultured S. putrefaciens CN32.”

It may state two separate claims as one.

In the case of lactate, ~2.5 moles of Fe(II) was produced per mole of lactate consumed, which is substantially less than 4 moles of Fe(II) per mole of lactate based on oxidation of lactate to acetate and carbon dioxide.

“In the case of lactate, ~2.5 moles of Fe(II) was produced per mole of lactate consumed, which is substantially less than 4 moles of Fe(II) per mole of lactate based on the oxidation of lactate to acetate and carbon dioxide (lactate  acetate + CO2 = 4e -).”

It may state two separate claims as one.

In the chloride-amended formate system, initial production of 2.3 mM Fe(II) within first 24 h was followed by a lag period lasting ~13 days, after which there was vigorous and sustained Fe(II) production concurrent with formate consumption.

“The initial production of 2.3 mM Fe(II) within the first 24 h was followed by a lag period lasting ~13 days in the chloride-amended system, after which there was vigorous and sustained Fe(II) production concurrent with formate consumption (Figure 5).”

It may state two separate claims as one.

Vivianite was not observed in any experimental systems (P:Fe = 0.005), and vivianite formation requires substantial phosphate (not observed at P:Fe lower than 0.08).

“Vivianite formation requires the presence of substantial phosphate (e.g., vivianite was not observed at P:Fe rations lower than 0.08 [33,43,48,63]), and vivianite was not observed in any of our experimental systems (P:Fe = 0.005 [63]).”

• cites [33] Fredrickson, 1998, Biogenic iron mineralization accompanying the dissimilatory reduction of hydrous ferric oxide by a groundwater bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [43] Bae, S., and Lee, W. (2013). Biotransformation of lepidocrocite in the presence of quinones and flavins. Geochim. Cosmochim. Acta, 10. sourceNot checked — no full text of the source
• cites [48] Kukkadapu, 2004, Biotransformation of two-line silica-ferrihydrite by a dissimilatory Fe(III)-reducing bacterium: Formation of carbonate green rust in the presence of phosphate, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [63] Boyanov, 2013, Effects of bound phosphate on the bioreduction of lepidocrocite (g-FeOOH) and maghemite (g-Fe2O3) and formation of secondary minerals, Environ. Sci. Technol. sourceNot checked — no full text of the source

It may state two separate claims as one.

In pyruvate systems, pH increased from 7.5 to 8.0 within 6 h, decreased to 7.1 over next 66 h, rebounded to pH 8 by day 6, and gradually increased to final pH 8.5 by day 106.

“Within 6 h of inoculation, the pH increased from 7.5 to 8.0, followed by a decrease to 7.1 over the next 66 h, a rebound to pH 8 by day 6, and a gradual increase to a final pH of 8.5 by day 106 (Figure 12).”

It may state two separate claims as one.

At day 62 in lactate systems, both pXRD and Mössbauer spectroscopy showed complete loss of lepidocrocite and formation of green rust.

“At the end of the experiment (day 62) both pXRD and Mössbauer spectroscopy showed complete loss of lepidocrocite and formation of green rust (Table 2 and Figure 8).”

It may state two separate claims as one.

In this study, reduction of Fe(III) by S. putrefaciens CN32 with H2 was rapid within first 2 days, then quickly plateaued to approximately 5, 10, and 15 mM Fe(II) in chloride, sulfate, and carbonate systems, respectively.

“In this study, reduction of Fe(III) by S. putrefaciens CN32 was rapid within the first 2 days, then quickly plateaued to approximately 5, 10, and 15 mM Fe(II) in the chloride, sulfate, and carbonate systems, respectively.”

It may state two separate claims as one.

Approximately 2 moles of Fe(II) were produced for each mole of formate consumed by S. putrefaciens CN32, consistent with the stoichiometry of formate oxidation to carbon dioxide.

“Approximately 2 moles of Fe(II) produced for each mole of formate consumed (Table 1) by S. putrefaciens CN32, consistent with the stoichiometry of formate oxidation to carbon dioxide (formate → CO 2 = 2e -) (Table 1).”

It may state two separate claims as one.

In the sulfate-amended NAG system, initial production of ~4 mM Fe(II) within first 24 h was followed by a lag of 3 days, after which Fe(II) increased to 14 mM at day 25 and remained essentially unchanged until day 31.

“As with the chloride system, there was an initial production of Fe(II) within the first 24 h (~4 mM), but this was followed by a much shorter lag period (3 days), after which the Fe(II) concentration increased to 14 mM at day 25 and remained essentially unchanged until Fe(II) production resumed at day 31.”

It may state two separate claims as one.

Reduction of Fe(III) by S. putrefaciens CN32 with H2 as electron donor was rapid within the first 2 days, then plateaued to approximately 5, 10, and 15 mM Fe(II) in chloride, sulfate, and carbonate systems, respectively.

“In this study, reduction of Fe(III) by S. putrefaciens CN32 was rapid within the first 2 days, then quickly plateaued to approximately 5, 10, and 15 mM Fe(II) in the chloride, sulfate, and carbonate systems, respectively.”

It may state two separate claims as one.

In the formate systems, pH increased from 7.5 to 8.3 within 18 h after inoculation and ultimately reached pH 9.1 by day 62.

“the pH increased from 7.5 to 8.3 within 18 h after inoculation followed by a slower pH increase, ultimately reaching pH 9.1 by day 62 (Figure 5).”

It may state two separate claims as one.

In pyruvate systems, solids remaining at end consisted of residual lepidocrocite and siderite; there were no indications of green rust formation at any point.

“The solids remaining at the end of the experiment consisted of residual lepidocrocite and siderite (Table 2 and Figure 13); there were no indications of green rust formation at any point during the experiment (data not shown).”

It may state two separate claims as one.

Production of Fe(II) was concurrent with NAG consumption and acetate production, consistent with NAG serving as an electron donor for Fe(III) reduction.

“The production of Fe(II) was concurrent with NAG consumption and acetate production, which is consistent with NAG serving as an electron donor for Fe(III) reduction.”

It may state two separate claims as one.

In the sulfate-amended NAG system, at 106 days Fe(II) concentration reached 71 mM, at which point lepidocrocite was no longer detected by Mössbauer or pXRD.

“At 106 days after inoculation, the Fe(II) concentration reached 71 mM, at which point lepidocrocite was no longer detected by Mössbauer or pXRD (Table 2 and Figure 10).”

It may state two separate claims as one.

In the chloride-amended NAG system, carbonate green rust formation was not evident until 38 days after inoculation and siderite was not observed until day 69.

“Carbonate green rust formation was not evident until 38 days after inoculation and siderite was not observed until day 69 (Figure 10).”

It may state two separate claims as one.

Fe(II) production rates in serine-amended systems were only slightly slower than rates in pyruvate-amended systems, consistent with conversion of serine to pyruvate and its subsequent utilization.

“Moreover, the Fe(II) production rates in the serine-amended systems were only slightly slower than the rates in the pyruvate-amended systems (which had the fastest rates among the donors tested (Table 1)), consistent with conversion of serine to pyruvate and its subsequent utilization.”

It may state two separate claims as one.

In the chloride-amended NAG system, substantial Fe(II) production occurred between day 25 and day 76 leading to ~61 mM Fe(II) at termination day 106; at which pXRD and Mössbauer indicated residual lepidocrocite and secondary minerals siderite and carbonate green rust.

“Substantial Fe(II) production was observed between day 25 and day 76 leading to an accumulation of ~61 mM Fe(II) at the termination of the experiment at day 106; at which time pXRD and Mössbauer spectroscopy indicated the presence of residual lepidocrocite and secondary minerals siderite and carbonate green rust (Table 2 and Figure 10).”

Probably not a substantial claim. The paper’s conclusions may not depend on it.

The taxonomic diversity of DIRB is reflected in the broad range of electron donors that support dissimilatory iron reduction.

“The taxonomic diversity of DIRB is reflected in the broad range of electron donors that support DIR [54]”

• cites [54] Dworkin, M. (2013). Dissimilatory Fe(III)- and Mn(IV)-reducing prokaryotes. The Prokaryotes—Prokaryotic Physiology and Biochemistry, Springer.Not matched

  Couldn’t be matched to a paper in Crossref, so it can’t be checked.

Probably not a substantial claim.

Many of these parameters are interdependent, often making it difficult to determine their relative contributions to formation of specific Fe(II)-bearing secondary minerals.

“Many of these parameters are interdependent (e.g., the rate of Fe(III) reduction may be controlled by the metabolic constraints placed on a given DIRB by the type and amount of electron donor available or by the system pH), often making it difficult to determine their relative contributions to the formation of specific Fe(II)-bearing secondary minerals.”

Probably not a substantial claim.

Salas et al. reported formation of siderite, green rust, and a combination of green rust and magnetite during DIR of ferrihydrite by Shewanella putrefaciens W3-18-1 with pyruvate, uridine, and lactate, respectively, as electron donors.

“Salas et al. [53] reported formation of siderite, green rust, and a combination of green rust and magnetite during DIR of ferrihydrite by Shewanella putrefaciens W3-18-1 with pyruvate, uridine, and lactate, respectively, as electron donors.”

• cites [53] Salas, 2009, The influence of carbon source on the products of dissimilatory iron reduction, Geomicrobiol. J. sourceNot checked — no full text of the source

Probably not a substantial claim. The paper’s conclusions may not depend on it. The quote only partly states this claim.

pXRD samples prepared under anoxic conditions showed no evidence of oxidation when scanned between 5 and 80° 2θ.

“although the pXRD analysis was conducted under ambient atmosphere, samples prepared in this manner showed no evidence of oxidation when scanned between 5 • and 80 • 2θ at a speed of 1.25 • 2θ min -1”

Probably not a substantial claim. The paper’s conclusions may not depend on it. It may state two separate claims as one.

The concentration of HCO3- was not measured directly during the experiments; a range of possible a[HCO3-] was calculated and used to create separate Eh-pH diagrams.

“As the concentration of HCO 3 -was not measured directly during the experiments, a range of possible a[HCO 3 -] was calculated and used to create separate Eh-pH diagrams to examine the effect of the range of a[HCO 3 -] on the stability of secondary iron minerals.”

Probably not a substantial claim.

Many factors contribute to formation of specific Fe(II)-bearing secondary minerals as products of dissimilatory iron reduction, including Fe(III) oxide mineralogy, particle aggregation, rate and extent of Fe(II) production, electron shuttles, DIRB species and population size, oxyanions, dissolved NOM, and electron donor concentration and type.

“Many factors have been identified as contributing to the formation of specific Fe(II)-bearing secondary minerals as products of DIR, including Fe(III) oxide mineralogy, [20,35]; Fe(III) oxide particle aggregation, [41]; the rate and extent of Fe(II) production, [33,35,42,43]; the presence of electron shuttles, [33]; the species and population size of the DIRB, [44][45][46]; the presence of oxyanio”

• cites [20] Cutting, 2009, Mineralogical and morphological constraints on the reduction of Fe(III) minerals by Geobacter sulfurreducens, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [35] Glasauer, 2003, Controls on Fe reduction and mineral formation by a subsurface bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [41] Zegeye, 2010, Bacterial and iron oxide aggregates mediate secondary iron mineral formation: Green rust versus magnetite, Geobiology sourceNot checked — no full text of the source
• cites [33] Fredrickson, 1998, Biogenic iron mineralization accompanying the dissimilatory reduction of hydrous ferric oxide by a groundwater bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [42] Zachara, 2002, Biomineralization of poorly crystalline Fe(III) oxides by dissimilatory metal reducing bacteria (DMRB), Geomicrobiol. J. sourceNot checked — no full text of the source
• cites [43] Bae, S., and Lee, W. (2013). Biotransformation of lepidocrocite in the presence of quinones and flavins. Geochim. Cosmochim. Acta, 10. sourceNot checked — no full text of the source

Probably not a substantial claim.

Dissimilatory iron-reducing bacteria can use soluble Fe(III) complexes, Fe(III) oxides, and Fe(III)-bearing clay minerals as terminal electron acceptors for anaerobic respiration.

“As a group, dissimilatory iron-reducing bacteria (DIRB) are able to use soluble Fe(III) complexes (e.g., ferric citrate), Fe(III) oxides, and Fe(III)-bearing clay minerals as terminal electron acceptors for anaerobic respiration [20][21][22][23][24][25][26][27][28].”

• cites [20] Cutting, 2009, Mineralogical and morphological constraints on the reduction of Fe(III) minerals by Geobacter sulfurreducens, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [21] Shelobolina, 2003, Use of ferric and ferrous iron containing minerals for respiration by Desulfitobacterium frappieri, Geomicrobiol. J. sourceNot checked — no full text of the source
• cites [22] Kostka, 1999, Respiration and dissolution of iron(III)-containing clay minerals by bacteria, Environ. Sci. Technol. sourceNot checked — no full text of the source

Probably not a substantial claim.

Products of dissimilatory iron reduction include Fe(II)-bearing secondary minerals such as magnetite, siderite, vivianite, green rust, chukanovite, and Fe(II)-bearing clays.

“The bioreduction of Fe(III) oxides by dissimilatory iron reducing bacteria (DIRB) may result in the production of a suite of Fe(II)-bearing secondary minerals, including magnetite, siderite, vivianite, green rusts, and chukanovite”

• Also stated in: § 1. Introduction · plain

  “The products of DIR comprise a broad range of Fe(II) species including soluble and adsorbed Fe(II) and mineral phases containing structural Fe(II) (e.g., magnetite, siderite (FeCO 3 ), vivianite [Fe 3 (PO 4 ) 2 •8H 2 O], green rust, chukanovite [Fe 2 (OH) 2 CO 3 ], and Fe(II)-bearing clays) [32][33][34][35][36][37][38][39][40].”

• cites [32] Lovley, 1987, Anaerobic production of magnetite by a dissimilatory iron-reducing microorganism, Nature sourceNot checked — no full text of the source
• cites [33] Fredrickson, 1998, Biogenic iron mineralization accompanying the dissimilatory reduction of hydrous ferric oxide by a groundwater bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [34] Abdelmoula, 2002, Iron(II,III) hydroxycarbonate green rust formation and stabilization from lepidocrocite bioreduction, Environ. Sci. Technol. sourceNot checked — no full text of the source

Probably not a substantial claim. It may state two separate claims as one.

Bioreduction of akaganeite by Shewanella sp. HN-41 resulted in formation of magnetite, siderite, and a combination of magnetite and siderite when lactate, pyruvate, and formate, respectively, were provided as electron donors.

“The bioreduction of akaganeite (β-FeOOH) by Shewanella sp.HN-41 resulted in the formation of magnetite, siderite, and a combination of magnetite and siderite when lactate, pyruvate, and formate, respectively, were provided as electron donors [52].”

• cites [52] Lee, 2007, Organic acid-dependent iron mineral formation by a newly isolated iron-reducing bacterium, Shewanella sp. HN-41, Geomicrobiol. J. sourceNot checked — no full text of the source

Probably not a substantial claim. The paper’s conclusions may not depend on it.

Mössbauer samples showed no indication of inadvertent oxidation.

“No indication of inadvertent oxidation was observed.”

Probably not a substantial claim. The paper’s conclusions may not depend on it.

All experimental systems were prepared in triplicate.

“All experimental systems were prepared in triplicate.”

Probably not a substantial claim. The paper’s conclusions may not depend on it.

Among Fe(II)-bearing secondary minerals resulting from DIR of Fe(III) oxides, green rusts are a particularly effective reductant for a wide range of contaminants of concern, including chlorinated solvents, nitroaromatics, azo dyes, toxic metals, metallolids, and radionuclides.

“Among the Fe(II)-bearing secondary minerals resulting from DIR of Fe(III) oxides, green rusts are a particularly effective reductant for a wide range of contaminants of concern, including chlorinated solvents, nitroaromatics, azo dyes, toxic metals, metallolids, and radionuclides [127,128,132-153].”

• cites [127,128,132-153]Not matched

  Couldn’t be matched to a paper in Crossref, so it can’t be checked.

Probably not a substantial claim. The paper’s conclusions may not depend on it.

Formate is utilized as an electron donor for dissimilatory iron reduction by S. putrefaciens CN32.

“Formate essentially served as a positive control given that we have previously shown that formate is utilized as an electron donor for DIR by S. putrefaciens CN32 [16,28,44,55,63].”

• cites [16] Scherer, 2007, Green rust formation from the bioreduction of g-FeOOH (lepidocrocite): Comparison of several Shewanella species, Geomicrobiol. J. sourceNot checked — no full text of the source
• cites [28] Gorski, 2015, Effects of phosphate on secondary mineral formation during the bioreduction of akaganeite (b-FeOOH): Green rust versus framboidal magnetite, Curr. Inorg. Chem. sourceNot checked — no full text of the source
• cites [44] Gorski, 2010, Effects of oxyanions, natural organic matter, and cell density on the bioreduction of lepidocrocite (g-FeOOH) and secondary mineral formation, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [55] 2008, Effects of electron transfer mediators on the biodegradation of lepidocrocite (g-FeOOH) by Shewanella putrefaciens CN32, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [63] Boyanov, 2013, Effects of bound phosphate on the bioreduction of lepidocrocite (g-FeOOH) and maghemite (g-Fe2O3) and formation of secondary minerals, Environ. Sci. Technol. sourceNot checked — no full text of the source

It may state two separate claims as one.

Pyruvate utilization by S. putrefaciens CN32 in the experimental systems likely involved fermentation of pyruvate and use of pyruvate and pyruvate fermentation products as electron donors for DIR.

“Our results suggest that a similar dynamic occurred with S. putrefaciens CN32 in our experimental systems containing pyruvate; if pyruvate was only utilized as an electron donor for DIR, only 30 mM would be needed to account for the ~60 mM of Fe(II) produced, yet all of the pyruvate (75 mM) was consumed.”

It may state two separate claims as one.

Magnetite was not observed as a secondary mineral in any experimental systems, likely due to trace levels of phosphate present in the lepidocrocite used, as low phosphate suppresses magnetite formation during DIR of Fe(III) oxides.

“However, magnetite was not observed as a secondary mineral in any of our experimental systems, likely due to trace levels of phosphate present in the lepidocrocite used in our experiments [63], as low levels of phosphate are known to suppress magnetite formation during DIR of Fe(III) oxides [28,33,44,47,63].”

• cites [63] Boyanov, 2013, Effects of bound phosphate on the bioreduction of lepidocrocite (g-FeOOH) and maghemite (g-Fe2O3) and formation of secondary minerals, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [28] Gorski, 2015, Effects of phosphate on secondary mineral formation during the bioreduction of akaganeite (b-FeOOH): Green rust versus framboidal magnetite, Curr. Inorg. Chem. sourceNot checked — no full text of the source
• cites [33] Fredrickson, 1998, Biogenic iron mineralization accompanying the dissimilatory reduction of hydrous ferric oxide by a groundwater bacterium, Geochim. Cosmochim. Acta sourceNot checked — no full text of the source
• cites [44] Gorski, 2010, Effects of oxyanions, natural organic matter, and cell density on the bioreduction of lepidocrocite (g-FeOOH) and secondary mineral formation, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [47] Borch, 2007, Phosphate imposed limitations on biological reduction and alteration of ferrihydrite, Environ. Sci. Technol. sourceNot checked — no full text of the source

It may state two separate claims as one.

Only carbonate green rust remained in the formate/sulfate system, while both carbonate and sulfate green rusts remained in the lactate/sulfate and NAG/sulfate systems, likely due to lower carbonate production in those systems.

“Only carbonate green rust remained in the formate/sulfate system, however both carbonate and sulfate green rusts remained in the lactate/sulfate, and NAG/sulfate systems, likely due to lower carbonate production in those systems.”

Probably not a substantial claim. It may state two separate claims as one.

Fe(II) is a reductant for a wide range of contaminants, but its redox reactivity depends strongly on its speciation.

“Fe(II) is a reductant for a wide range of contaminants, however, the redox reactivity of Fe(II) depends strongly on its speciation [127-131].”

• cites [127] Elsner, 2004, Reactivity of Fe(II)-bearing minerals toward reductive transformation of organic contaminants, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [128] Lee, 2003, Reductive capacity of natural reductants, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [129] Scheinost, 2008, Selenite reduction by mackinawite, magnetite and siderite: XAS characterization of nanosized redox products, Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [130] Scheinost, 2008, X-ray absorption and photoelectron spectroscopy investigation of selenite reduction by FeII-bearing minerals, J. Contam. Hydrol. sourceNot checked — no full text of the source
• cites [131] Kelly, 2010, XAFS investigation of the interactions of UVI with secondary mineralization products from the bioreduction of FeIII oxides, Environ. Sci. Technol. sourceNot checked — no full text of the source

It may state two separate claims as one.

Carbonate green rust formed in chloride-amended systems, consistent with the affinity of pyroaurite-type layered double hydroxides for carbonate in the interlayer relative to chloride.

“Carbonate green rust formed in chloride-amended systems, consistent with the affinity of pyroaurite-type layered double hydroxides for carbonate in the interlayer relative to chloride [120].”

• cites [120] Refait, 1997, The anionic species competition in iron aqueous corrosion: Role of various green rust compounds, Corros. Sci. sourceNot checked — no full text of the source

It may state two separate claims as one.

NAG was not consumed independent of Fe(III) reduction, suggesting S. putrefaciens CN32 does not ferment NAG.

“NAG was not consumed independent of Fe(III) reduction suggesting that S. putrefaciens CN32 does not ferment NAG.”

Probably not a substantial claim. The paper’s conclusions may not depend on it. It may state two separate claims as one.

Largely through the activity of DIRB, Fe(II) is typically one of the most abundant reductants present in aquatic and terrestrial environments under suboxic and anoxic conditions, often providing substantial redox buffering capacity.

“Largely through the activity of DIRB, Fe(II) is typically one of the most abundant reductants present in aquatic and terrestrial environments under suboxic and anoxic conditions [124-126], often providing substantial redox buffering capacity to these systems.”

• cites [124] Hochella, 1990, Oxidative and reductive dissolution of minerals, Mineral-Water Interface GeochemistryNot checked yet
• cites [125] Heron, 1995, Impact of sediment-bound iron on redox buffering in a landfill leachate polluted aquifer (Vejen, Denmark), Environ. Sci. Technol. sourceNot checked — no full text of the source
• cites [126] Hofstetter, 1998, Characterization of predominant reductants in an anaerobic leachate-contaminated aquifer by nitroaromatic probe compounds, Environ. Sci. Technol. sourceNot checked — no full text of the source

Probably not a substantial claim. The paper’s conclusions may not depend on it.

Limited reduction of Fe(III) was also observed during DIR of γ-FeOOH by S. putrefaciens CIP 8040T with H2 as electron donor.

“Limited reduction of Fe(III) was also observed during DIR of γ-FeOOH by S. putrefaciens CIP 8040 T with H2 as the electron donor [76].”

• cites [76] Zegeye, 2005, Formation of hydroxysulfate green rust 2 as a single iron(II-III) mineral in microbial culture, Geomicrobiol. J. sourceNot checked — no full text of the source

It may state two separate claims as one.

As carbonate accumulates from oxidation of organic electron donors, carbonate green rust forms as carbonate is preferred over sulfate in the interlayer.

“However, as carbonate accumulates from the oxidation of the organic electron donors, carbonate green rust forms as carbonate is preferred over sulfate in the interlayer.”