Skip to main content

Abiotic ammonium formation in the presence of Ni-Fe metals and alloys and its implications for the Hadean nitrogen cycle


Experiments with dinitrogen-, nitrite-, nitrate-containing solutions were conducted without headspace in Ti reactors (200°C), borosilicate septum bottles (70°C) and HDPE tubes (22°C) in the presence of Fe and Ni metal, awaruite (Ni80Fe20) and tetrataenite (Ni50Fe50). In general, metals used in this investigation were more reactive than alloys toward all investigated nitrogen species. Nitrite and nitrate were converted to ammonium more rapidly than dinitrogen, and the reduction process had a strong temperature dependence. We concluded from our experimental observations that Hadean submarine hydrothermal systems could have supplied significant quantities of ammonium for reactions that are generally associated with prebiotic synthesis, especially in localized environments. Several natural meteorites (octahedrites) were found to contain up to 22 ppm Ntot. While the oxidation state of N in the octahedrites was not determined, XPS analysis of metals and alloys used in the study shows that N is likely present as nitride (N3-). This observation may have implications toward the Hadean environment, since, terrestrial (e.g., oceanic) ammonium production may have been supplemented by reduced nitrogen delivered by metal-rich meteorites. This notion is based on the fact that nitrogen dissolves into metallic melts.


Ammonia (NH3) or ammonium (NH4+), henceforth NH3/NH4+, are necessary precursors for reactions associated with prebiotic syntheses, such as the Strecker synthesis. It has been experimentally shown that NH3/NH4+ environments are more efficient in organic synthesis than those dominated by dinitrogen (henceforth N2) in both aqueous and gaseous environments [e.g., [1]] [2, 3]. This notion is not unexpected, considering that, the strong triple bond (948 kJ.mol-1) of the N2 would presumably result in large reaction activation barriers (i.e., low conversion rates), even if the overall reaction is thermodynamically favored.

Several possible pathways to abiotic NH3/NH4+ on early the Earth have been proposed: reduction of NO2-/NO3- by Fe++/FeS in the ocean [e.g., [4]] [5, 6]; atmospheric production from N2 and HCN [e.g., [7]] [8]; release from rocks and minerals [e.g., [9]]; photoreduction on mineral surfaces [e.g., [10]] [11, 12]; and hydrothermal aqueous reduction from N2 in the presence of minerals under conditions typical of submarine hydrothermal systems [e.g., [13]] [14, 15]. Each of the mechanisms relies on a different set of assumptions and none of the proposed mechanisms has, in our opinion, gained universal acceptance in the scientific community as the predominant source of abiotic NH3/NH4+.

In this scientific contribution we focus on the catalytic properties of Ni and Fe metals and their alloys which can form in submarine hydrothermal systems (SHS), especially those driven by exothermic hydration reactions (e.g., serpentinization) in an off-axis tectonic setting. Upon dissolution of Ni-containing rock-forming minerals (e.g., olivine, pyroxene, amphibole), released Ni and Fe can react to form metals and alloys under extreme reducing conditions imposed on the system by the serpentinization processes [1618]. The conditions are commonly reducing enough to stabilize Ni-Fe alloys (e.g., awaruite – Ni3Fe), metallic nickel (Ni0) and even iron (Fe0). These minerals occur regularly, albeit in small quantities in both ancient and modern serpentinites [1926]. A compilation of representative chemical analyses of metals and alloys found in serpentinites is presented in Fig. 1. The observations from natural systems have been corroborated by laboratory experiments [27, 28].

Figure 1
figure 1

A ternary diagram of naturally occurring Ni-Fe-M (M = Cr, Sb, Pb, Cu, Co, As, Ag, PGE) alloys and their comparison to synthetic alloys used in this study. Analyses of natural samples were adapted from: [19] [22] [109-115]. Each data point represents an electron microprobe analysis expressed in weight percent.

An active global tectonic cycle is not required for the formation and operation of serpentinization-driven SHS and hence we assume that these environments were commonly present on the Hadean Earth. Moreover, the lack of oxygen and the possible presence of significant amounts of hydrogen gas in the Hadean atmosphere (and consequently in the ocean water) may have further enhanced the stability of base metals and their alloys [29, 30].

The most abundant reactant for abiotic NH3/NH4+ formation in the Hadean was N2 dissolved in the seawater from the N2-rich atmosphere. NO2- and NO3- are also thought to have been available, although likely in low concentrations. These oxidized N species could have formed in high energy events such as lightning, corona discharge and/or impacts and subsequently rain out into the ocean [3134].

In this contribution we report the results of an experimental study undertaken to evaluate the hypothesis that abiotic NH4+ formation from dissolved N2, NO2- and NO3- in the presence of Ni3Fe, NiFe, Ni0 and Fe0 was an operative synthetic route at anaerobic conditions potentially present in the Hadean Ocean. Furthermore, we attempt to quantify global NH4+ yields in the Hadean Ocean produced by investigated mechanisms.

Methods and materials

Reduction experiments

Three sets of experiments were conducted at three different temperatures: 200°C (runs 1–36), 70°C (runs 37–59) and 22°C (runs 60–83). The choice of reactors was based on experimental temperature: 15 mL passivated HIP® Titanium 64 tube reactors (200°C); 20 mL I-Chem® borosilicate vials with PTFE/Si septum caps (70°C) and 15 mL BD HDPE Falcon® tubes (22°C). Reactors were kept at constant temperature in a heated water bath (20, 70°C) or an Isotemp® oven (200°C). All experiments lasted 24 hours and were conducted in the absence of headspace (e.g., no gas phase). No additional pressure other than that of expanding liquid was imposed on the vessels (~400 psi/27 bars with Ni0 to ~800 psi/55 bars with Fe0 at 200°C).

All reacting solutions were prepared from freshly drawn UV/UF deionized water (henceforth DI) either by purging with a UHP gas of interest (e.g., Ar, N2, H2/N2) and/or by dissolving appropriate amounts of reagents. NH4+ content of all unreacted reagent solutions (e.g., blanks) was below the detection limit of ion chromatography (<0.1 μ, reported by the manufacturer). DI purged with N2 gas under ambient conditions results in equilibrium N2(aq) concentration of 0.59 The effect of O2 was, however, also determined (runs 39, 41, 45, 47, 50, 52, 56, 58, 62, 64, 68, 70, 74, 76, 80, 82) in experiments with DI equilibrated with present-day atmosphere (e.g., no N2 purging).

To ensure clean and fresh mineral surfaces (e.g., free of oxidation products and/or atmospheric sorbed gases), all metal/alloys were ultrasonically cleaned for 1 hour in 0.06 M HCl immediately preceding the experiments. Subsequently they were washed three times with the designated reacting solution and loaded into reactors in the form of slurry. This "wet loading" procedure eliminated sorption of gases from the atmosphere onto freshly cleaned metal surfaces which was especially important in blank experiments.

Background NH4+ production (e.g., release from reactants, reaction vessels, etc.) was assessed in blank experiments with Ar-saturated solutions and no added N source (runs 1, 9, 17, 25, 37, 43, 49, 54, 60, 66, 72, 78). NO3- and NO2- solutions were prepared by dissolution of ACS reagent grade KNO3 and KNO2, respectively. The pH was not buffered and was allowed to change as a result of solution-metal/alloy interactions and was recorded before and after the experiment. After pH measurements, all samples were acidified with 0.2 M HCl to ensure the conversion of NH3 to NH4+ and to prevent the formation of Fe precipitates. The samples were stored at 1°C and analyzed within 24 – 48 hours. The summary of all experimental conditions is presented in Tab. 1.

Table 1 Physical and chemical characteristics of alloys/metals used in study. Formula and the "a" parameter determined from EPMA analyses and from LeBail refinement of XRD data, respectively. The chemical composition of Ni-Fe alloys was confirmed by EPMA as: Ni49.78(± 0.49)Fe50.22(± 0.49) and Ni79.14(± 0.43)Fe20.86(± 0.43).

Analysis of solids, their surfaces, and reaction products

Metals and alloys representing an fcc solid solution of Ni in Fe were purchased from Alfa Aesar® and Goodfellow. All starting and selected reacted solids were characterized by X-Ray Diffractometry, X-Ray Photoelectron Spectroscopy, Scanning Electron Microscopy, B.E.T. surface analysis, and Electron Microprobe. The results of metal/alloy characterization are summarized in Tab. 2 and Fig. 2, 3.

Table 2 Conditions and results of reduction experiments conducted in this study. All concentrations are in μ Values and their errors bigger than 10 are rounded to the nearest whole number, those smaller than 10 are rounded to the nearest tenth.
Figure 2
figure 2

XRD patterns of metals/alloys used in this study. Note the similarity in patterns of Ni, Ni50Fe50 and Ni81Fe19 stemming from the same space group (Fm-3m). Fe0 possesses Im-3m space group.

Figure 3
figure 3

SEM photographs of unreacted alloys/metals used in this study. A) Ni metal, b) Ni81Fe19, c) Ni50Fe50 and d) Fe metal.

X-Ray Diffraction (XRD) data were collected using a Scintag PAD X diffractometer under the following conditions: CuKα1, 40 kV, 25 mA, 5° – 90° 2Θ, step 0.02° 2Θ and variable scan rates.

Scanning Electron Analysis (SEM) was performed on the LEO 1550 SFEG scanning electron microscope equipped with an EDAX energy dispersive X-ray spectrometer (EDS) using an accelerating voltage of 15 kV and a 30 μm aperture.

Oxidation state of Ni, Fe and the presence of N in alloys were determined by X-Ray Photoelectron Spectroscopy (XPS). The data were acquired with unmonochromatized Mg and Al radiation at 1253.6 eV and 1486.7 eV using a Physical Electronics source controller in a vacuum chamber with a base pressure of 1 × 10-9 Torr. A VG Microtech hemispherical analyzer was used to obtain the energy distribution of the photoemitted electrons at pass energies of 50 and 75 eV. The binding energies were calibrated by fixing the Au 4p3/2 and 4f7/2 peaks (546.3 eV, 87.5 eV) from a gold standard, and the metallic Fe 2p3/2 and Ni 2p3/2 cores (707.0 eV, 852.3 eV). Selected particles were sputtered with Ar+ accelerated to 2 kV to expose their interior and check for the presence of nitrogen using a Physical Electronics ion gun controller.

B.E.T. surface analysis (BET) was performed using a Micromeritics ASAP 2010 analyzer with a 10-mm Hg transducer using UHP N2 gas. The surface area was calculated from measurements at 5 different N2(g) pressures (42.58196, 85.30770, 132.82384, 180.25029 and 227.66101 Torr).

Chemical composition of alloys/metals was determined by a Cameca Camebax Micro electron microprobe (EPMA) equipped with four wavelength dispersive spectrometers and a Kevex Analyst 8000 energy dispersive detector. During all analyses, the accelerating voltage and beam current used were 15 kV and 10 nA (nominal), respectively.

Molecular hydrogen was analyzed on a SRI 8610C single column gas chromatograph (GC) with a TCD detector, 6' Hayesep D column and N2 carrier gas. The sample (~0.2 mL) was withdrawn from the reaction vessel into a gastight® Hamilton™ syringe with a Mininert™ valve and immediately analyzed using a 4-point calibration curve. Gas mixtures (Matheson™) of known composition were used as calibration standards.

Total nitrogen content of metals/alloys was analyzed by IMR Test Labs (Lansing, NY) by inert gas fusion [35]. During the analysis, N is released from the metal at 1900°C into the stream of He gas and analyzed in a thermal conductivity cell.

Experimental solutions were analyzed for NH4+ using a Dionex DX-500 ion chromatograph (IC) with a 100 μL sample loop. NH4+ and NO3-/NO2- were analyzed using a 4 mm Dionex IonPac® CS-16 (40°C, 34 mN H2SO4 eluent) and IonPac® AS4A-SC (22°C, 5 Na2B4O7 eluent), respectively. Concentrations were calculated from a 4-point calibration curve with R2 values above 0.99.

No other compounds were analyzed. It is expected, however, that other reaction products and/or intermediates (e.g., NO) may have formed during a complex sequence of electron transfer reactions.

Geochemical equilibrium modeling was performed with the Geochemist's Workbench 5 [36] software package with the thermodynamic database complemented with data for Ni3Fe and NiFe [37].


Dinitrogen reduction

The results of NH4+ formation from N2 and the effect of added H2 and KCl at 200°C (normalized to 1 m2 surface area) are shown in Fig. 4 and summarized in Tab. 1 (runs 1–32). All results are compared with respect to blank experiments conducted with Ar and no N2 added. The blank experiments thus represent the background NH4+ production from the metal/alloy involved and reactor catalysis. Error bars were calculated by propagating errors from solution dilutions and B.E.T. and IC analyses. Due to relatively large error bars, only results differing from the blank (or each other) by more than the calculated error will be discussed.

Figure 4
figure 4

NH4+ formation from N2 in the presence of Ni, Fe metals and alloys at 200°C. The dashed lines correspond to the Ar blank. The concentrations of KCl in the experiments were 459 μ in A, B and 476 μ in C, D. Results are normalized to 1 m2 of surface area.

In the presence of N2, only Ni81Fe19 did not show appreciable activity toward NH4+ formation (Fig. 4d). Within our experimental certainty, Fe0 was the material associated with the most NH4+ production (31 μ, Fig. 4a), followed by Ni0 (16 μ, Fig. 4b) and Ni50Fe50 (7 μ, Fig. 4c). H2(aq) was observed to form in the presence of all studied metals and alloys. Representative concentrations of H2(aq) at 200°C (measured in one experiment with N2-saturated, O2-free DI per metal/alloy only) were 0.38 with Ni0, 0.28 with Ni81Fe19, 0.7 with Ni50Fe50 and 21 with Fe0. We point out that this H2 production is relatively large compared to the background H2 production of the Ti reaction vessels that was determined to be 12 μ in an experiment with DI saturated with Ar at 200°C. An interesting observation during our experiments was that the reactivity of Fe0 towards O2-free DI was so rapid that gas bubbles were forming on its surface after just a few hours of exposure at 22°C (by analogy with 200°C experiments we assume it is H2).

Our results showed that the addition of H2 (5%/95% H2/N2) into the reaction mixture only resulted in change in the Fe0 circumstance where 158 μ NH4+ was produced (Fig. 4a). Fe0 was also the material most affected by the addition of K+ (KCl). In this case, 189 μ of NH4+ was produced, 158 μ more than with N2 alone (Fig. 4a). In general, our experiments showed that Ni81Fe19 was the least, and Fe0, the most, affected by the addition of H2 or KCl into the reacting solution (Fig. 4d, a).

Aqueous Fe and Ni cations (NiCl2, FeCl2) only had a small effect on N2 reduction chemistry, converting about 1% of the total available N into NH4+ at 200°C (Tab. 1). A post-reaction visual inspection of the FeCl2 solution showed a fine-grained colloid of reddish color that, in the presence of atmospheric O2 changed color to light brown. The amount of recovered solids was insufficient for analysis by XRD.

At temperatures of 70 and 22°C no NH4+ formation from N2 was observed (Tab 1, runs 38, 44, 50, 55, 61, 67, 73, 79). Use of these lower temperatures also resulted in lower background NH4+ production in solutions containing the metals/alloys. The yield of NH4+ ranged from 7.4 (Fe0) to 1.2 μ (Ni50Fe50) at 70°C (Tab. 1, runs 37, 43, 49, 54) and 1.4 (Fe0) to 0 μ (Ni50Fe50, Ni81Fe19) at 22°C (Tab. 1, runs 60, 66, 72, 78).

Nitrite and nitrate reduction

The results of our NO2- and NO3- reduction experiments are shown in Fig. 5. At 200°C all tested metals/alloys were found to be very effective in converting NO2-/NO3- into NH4+. To assess if the presence of NO2- or NO3- in the solution had any effect on N2 reduction, each experiment was conducted in duplicate with Ar (Tab. 1, runs 7, 8, 15, 16, 23, 24, 31, 32) and N2 (Tab. 1, runs 5, 6, 13, 14, 21, 22, 29, 30) saturated solutions (e.g., Fe0 with NO2-/N2 and NO2-/Ar). These experiments taken in sum showed that there was no difference between the N2 and Ar runs (Fig. 5a).

Figure 5
figure 5

NH4+ formation from nitrite and nitrate, expressed in terms of % conversion. Panels A, B and C correspond to sets of experiments at 200, 70 and 22°C, respectively.

The results collected at 70°C reveal prominent differences between alloys and metals (Fig. 5b). While Ni and Fe achieved almost 100% conversions of NO2-/NO3- to NH4+ (Tab. 1, runs 40, 42, 46, 48), interestingly, no- or insignificant reduction (less than 20%) was observed in solutions reacted with alloys (Tab. 1, runs 51, 53, 57, 59). The presence of O2 in the solution appears to have an inhibitive effect on the reduction process, especially in the presence of Ni81Fe19 alloy (Tab. 1, runs 56, 58; Fig. 5b).

Low temperature experiments (22°C) further confirmed the temperature dependence of NO2-/NO3- reduction in the presence of alloys (Fig. 5c). Compared to 200°C and even at 70°C, NH4+ formation was negligible (less than 1% conversion) (runs 63, 65, 69, 71, 75, 77, 81, 83). The effect of O2 in the reacted solution was most pronounced with NO3- in the presence of Ni0 (run 70). In general, at 22°C Fe0 was the most efficient material in converting NO2-/NO3- to NH4+, regardless of the O2 content (Tab. 1, runs 62–65; Fig. 5c).

It is important to note that at 200°C both NO2- and NO3- decomposed in the absence of metal/alloys as well (Tab. 1, runs 34, 34). 42% of the initial 497 μ KNO2 solution was converted into NO3- (~15%), NH4+ (~9%) and other N compounds (~18%) that were not analyzed. Of the initial 444 μ KNO3 solution, 71% was converted into NO2- (~61%), NH4+ (~1%) and about 9% corresponds to other unanalyzed N compounds. It is not clear if this is a result of thermally induced decomposition, catalysis or reaction by/with the titanium reaction vessel, or a combination of all; nevertheless, NH4+ was not the dominant reaction product. At 70 and 22°C, both NO2- and NO3- solutions were found to be stable in experiments without metals or alloys during the 24-hour reaction period.

Metal/alloy alteration

Generally, the extent of alteration of Fe-containing metal/alloy increased with temperature, as demonstrated by the presence of secondary minerals (Fig. 6). Magnetite (Fe3O4) was the most abundant alteration product, predominantly forming euhedral to subhedral crystals up to several μm in size (Fig. 6a, b, d, e). Pseudomorphoses of magnetite after reacted spherical Fe0 particles were common (Fig. 6d). The second most common alteration phase were Fe-(oxy)hydroxides (e.g., lepidocrocite) usually of amorphous appearance or forming needle-like (Fig. 6c) and platy crystals several tens of nm thin and several μm long. Both magnetite and Fe-(oxy)hydroxides commonly occur simultaneously in all reacted samples (SEM) (Fig. 6a,b); however, only magnetite is identified by the XRD method (Fig. 7). This suggests that the Fe-(oxy)hydroxides either lack long range order (e.g., "X-ray amorphous") and/or their abundance is less than 5%, the approximate detection limit of XRD. In general, the lower the Fe content, the lower the extent of alteration (Fig. 6e). In contrast, reacted Ni0 exhibited no microscale (SEM) evidence of reaction (Fig. 6f, compare with Fig. 3a), as corroborated by the XPS spectra documenting the presence of residual zero-valent Ni species on the surface (Fig. 8). As a result of solution interactions with metals/alloys, the resulting pH in most experiments was higher than the starting value (see discussion) (Tab. 1).

Figure 6
figure 6

SEM microphotographs of reacted metals and alloys. A) Fe0 reacted in N2(aq) solution depicting coexisting magnetite and Fe-(oxy)hydroxides; B) Detail of magnetite single crystals formed on Fe0; C) clusters of needle-like Fe-(oxy)hydroxide crystals formed on Fe0; D) pseudomorphoses of magnetite after Fe0 in the H2/N2 solution; E) magnetite crystals formed on Ni50Fe50 in the KNO3 solution; F) Ni0 skeletal crystal revealing no change after reaction.

Figure 7
figure 7

Normalized XRD patterns of unreacted (lower) reacted (upper) Fe0 showing the presence of magnetite (Mt).

Figure 8
figure 8

Ni 2p3/2 peaks showing the speciation of Ni on the surface Ni metal powder at various stages of the experiment. Note the presence of residual zerovalent Ni on the surface after 24 hour reaction at 200°C.


Nitrogen in alloys and metals

All the metals and alloys investigated in this work were found to contain N, which resulted in a background production of NH4+. The presence of atomic N was based on two lines of evidence: 1) The presence of the N1s peak in the XPS spectra of starting metals and alloys even after "cleaning" the surface by sputtering with Ar+ ions (Fig. 9) and; 2) quantitative analysis of Ntot content of the starting materials by inert gas fusion with a thermal conductivity detection (Tab. 3).

Table 3 Total N content of metals and alloys used in this study as determined by inert gas fusion – thermal conductivity method (IMR Test Labs).
Figure 9
figure 9

N 1 s peaks centered around 400 eV documenting the presence of N in the tested alloys and metals after sputtering with Ar+ (Ni0 400.1 eV, Ni50Fe50 399.7 eV, Fe0 398.9 eV).

Commercially available Ni, Fe metals/alloys may contain N due to the manufacturing process which employs either inert (N2, Ar) or reducing (NH3, H2) atmospheres to prevent oxidation [38, 39] [Alfa Aesar, Goodfellow – pers.comm]. For example, during the synthesis, N2 chemisorbs on the surface of molten/hot metal and dissociates (Equation 1).

N2 (gas) → 2N (in metal) (1)

In the subsequent step N enters the structure via diffusion or convection to form primarily monoatomic interstitial and to lesser extent substitutional solid solutions. This process is governed by the Sievert's law (Equation 2), which predicts that diatomic gases such as N2 dissolve in metals (c N ) proportionally to the square root of the partial pressure (pN2) in the coexisting gas phase [40, 41].

K = c N 2 p N 2 MathType@MTEF@5@5@+=feaafiart1ev1aaatCvAUfKttLearuWrP9MDH5MBPbIqV92AaeXatLxBI9gBaebbnrfifHhDYfgasaacPC6xNi=xI8qiVKYPFjYdHaVhbbf9v8qqaqFr0xc9vqFj0dXdbba91qpepeI8k8fiI+fsY=rqGqVepae9pg0db9vqaiVgFr0xfr=xfr=xc9adbaqaaeGaciGaaiaabeqaaeqabiWaaaGcbaGaem4saSKaeyypa0tcfa4aaSaaaeaacqWGJbWydaqhaaqaaiabd6eaobqaaiabikdaYaaaaeaacqWGWbaCdaWgaaqaaiabd6eaonaaBaaabaGaeGOmaidabeaaaeqaaaaaaaa@3630@

Assuming homolytic N2 bond cleavage, each N atom would have three unpaired electrons available for bonding with the surrounding metal atoms. XPS spectra collected from unreacted metals/alloys in our experiments point to nitride (N3-, 398.6 eV) as the likely N species (Fig. 9) [42]. Consequently, upon release into the solution, N3- is expected to react with available protons to form NH3/NH4+ (Reaction 3, 4) and contribute to their high background productivity.

N3- + 3H+ → NH3 (3)

N3- + 4H+ → NH4+ (4)

However, undissociated N2 gas may get trapped in the molten metal (e.g., in inclusions) as well.

Dinitrogen reduction

Although batch-type experiments, such as the ones described above, provide little insight into the kinetics of a reaction and much less the reaction mechanism, the results do allow one to compare the amount of NH3/NH4+ formed under different conditions. In addition the results can be placed in the context of previously published research related to the reduction of N-species to NH3/NH4+. Due to the immense importance of NH3/NH4+ in industry and agriculture, several decades of research exist on its synthesis and production from N2 gas [e.g., [43]]. The industrial Haber-Bosch process utilizes Fe0 catalyst at high temperatures and pressures (~500°C, ~100 bars) to synthesize NH3 from H2 and N2 gas (Reaction 5).

N2(g) + 3H2(g) → 2NH3(g) (5)

In brief, the reaction proceeds as follows: sorption of H2 and N2 gases on the surface is followed by the formation of atomic Hads and Nads (dissociative sorption). Fe0 then facilitates electron transfer from Hads to Nads (e.g., N reduction), followed by the formation of NH3 gas on the surface and subsequent desorption. The dissociative chemisorption of N2 is generally taken to be the rate-limiting step [44]. For comparison, modern life overcomes the reaction's activation barrier using the enzyme nitrogenase composed of dinitrogenase (MoFe center) and dinitrogenase reductase (Fe center) proteins. In Reaction 6, Fd stands for ferredoxin, the electron-transfer protein [45, 46].

N2(g) + 8Fd0red + 10H+ → 2NH4+ + 8Fd+ox + H2(g) (6)

Analogous overall reactions of abiotic N2 reduction can be written for aqueous solutions (Reaction 7, 8), although it is important to note that since this reaction requires a transfer of multiple electrons, several reaction intermediates must be involved. Once in solution, NH3 and NH4+ exist in a pH dependent equilibrium (Equation 9; valid for 25°C).

N2(aq) + 2H+ + 3H2(aq) → 2NH4+ (7)

N2(aq) + 3H2(aq) → 2NH3(aq)(8)

p H = 9.25 + log { [ N H 3 ] [ N H 4 + ] } MathType@MTEF@5@5@+=feaafiart1ev1aaatCvAUfKttLearuWrP9MDH5MBPbIqV92AaeXatLxBI9gBaebbnrfifHhDYfgasaacPC6xNi=xI8qiVKYPFjYdHaVhbbf9v8qqaqFr0xc9vqFj0dXdbba91qpepeI8k8fiI+fsY=rqGqVepae9pg0db9vqaiVgFr0xfr=xfr=xc9adbaqaaeGaciGaaiaabeqaaeqabiWaaaGcbaGaemiCaaNaemisaGKaeyypa0JaeGyoaKJaeiOla4IaeGOmaiJaeGynauJaey4kaSIagiiBaWMaei4Ba8Maei4zaC2aaiWaaKqbagaadaWcaaqaaiabcUfaBjabd6eaojabdIeainaaBaaabaGaeG4mamdabeaacqGGDbqxaeaacqGGBbWwcqWGobGtcqWGibasdaqhaaqaaiabisda0aqaaiabgUcaRaaacqGGDbqxaaaakiaawUhacaGL9baaaaa@47DD@

We hypothesize that reactions between H2, N2 and the metal/alloy surface are taking place in our experiments; however, they are orders of magnitude slower than those described above in the gas phase. Undoubtedly, this is due to the fact that aqueous reactions occurring in our experiments are not only more complex but also take place at much lower T, P conditions and H2/N2 concentrations than those typical for Haber-Bosch synthesis. Such kinetic constraints could explain low NH4+ yields, even though the thermodynamic equilibrium models predict NH4+ to be the dominant N species (Tab. 4).

Table 4 Predicted equilibrium pH and nitrogen speciation in the N-H2O-Fe-Ni system (only species with molalities above 1·10-8 shown). Concentrations and fugacities of dominant N species are in bold. The last column shows the predicted final mineral assemblage.

We speculate that in the presence of Fe0 most of the NH4+ was rapidly formed in the first few hours of the experiment when unreacted surface was still available for reaction. In this scenario (e.g., run 2) most (and possibly all) H2 is formed in situ as a result of interactions between the pristine Fe0 surface and H2O (Reaction 10) (e.g., mH2 = 0 at t0); however, the simultaneous Fe oxidation passivates the surface, reduces the availability of suitable H2/N2 sorption sites and the overall yield of the N2-reduction reaction.

Fe + 2H2O → H2 + Fe2+ + 2OH- (10)

This notion is corroborated by experiments carried out with conditions in which H2 was present in the system from the start of the reaction (e.g., run 3), as a result of purging the solution with a H2/N2 mixture prior to loading (e.g., mH2 > 0 at t0). Abundant H2 in this run correlates with greater NH4+ production as the overall N2 conversion rate increases from 2.5 to 10% (Tab. 2). Assuming that in both cases Fe0 surface passivates at the same rate, then the H2 purged system produces more NH4+ per unit of time because it does not depend on the Fe0 alteration process (Reaction 10) to provide H2. This circumstance may be more typical of natural serpentinization-driven SHS where H2 can be provided by a number of processes, especially by Fe2+ oxidation during alteration of rock-forming silicates [17, 47].

Similar assumptions can be made about Ni50Fe50 and Ni81Fe19 assuming that Fe atoms exposed on the surface played a role in the reduction process. Due to good corrosion resistance, Ni0 reacted to a much lesser extent and consistent with this lower activity is our experimental observation that the Ni0 surface was not significantly altered (e.g., by precipitation of neoformed phases) throughout the experiment. Different modes of metal/alloy participation in studied reactions are discussed below.

The addition of KCl into the Fe0-H2O-N2 system in our experiments resulted in higher NH4+ yield (Fig. 4a). While it may be intriguing to draw parallels with the Haber-Bosh process, where K is added to improve sticking coefficients and to help stabilize sorbed species [44], the apparent promoting effect of KCl may be partially or entirely caused by the presence of chloride ion (Cl-) in the solution. Cl- can react with dissolved iron in the solution (Reaction 11) and remove products from the Fe0 dissolution reaction (Reaction 10).

Fe2+ + 2Cl- → FeCl2 (11)

Such a complexation reaction would result in an equilibrium shift towards the product side and further drive the dissolution process and release of structurally bound reduced N species into the solution (Reactions 3, 4). This is in agreement with the results of Reardon [48] who observed an increase in Fe0 corrosion rates in low ionic strength (~0.02 m) anaerobic NaCl, NaHCO3 and Na2SO4 solutions compared to DI water. The NH4+ content of the KCl reagent solution at concentrations used in our experiments was found to be below the detection limit of ion chromatography.

Nitrite and Nitrate Reduction

Due to their status as environmental contaminants, NO2-/NO3- reduction has been extensively studied, especially focused on the reduction of NO3- by Fe0. Most of the published results concur that the reduction reaction (Reaction 12) at anaerobic ambient conditions exhibits the following set of features: 1) reaction rates decrease with increasing pH; 2) pH in unbuffered solutions becomes more alkaline as the reaction progresses; 3) NH4+ and Fe3O4 are the dominant reaction products; 4) NO3- reduction slows down once Fe0 is coated with Fe3O4 unless Fe2+, Cu2+, Al3+ or Fe3+ are present; 5) SO42- inhibits the reaction; and 6) the molar N2:NH4+ ratio in reaction products increases with pH [4957].

4Fe0 + 10H+ + NO3- → NH4+ + 4Fe2+ + 3H2O (12)

3Ni3Fe + 4NO2- + 24H2O → 32OH- + 4NH4+ + 3Fe2+ + 9Ni2+ (13)

Analogous reactions can be written for other metals/alloys as well as NO2- (Reaction 13), although they have been by comparison less studied. The absence of resonance structures in the NO2- molecule makes it easier to reduce than NO3- [58], which is reflected in reduction reaction rates. For example, NO3- reduction to NH4+ in the presence of Fe2+ was found to be a factor of 8 slower than that of NO2- [5]. Because the reduction from NO3- to NH4+ requires transfer of at least 8 electrons, several intermediates must be formed in the process. Moreover, the formation of any N-N bonds must be avoided because it is effectively inert under all but the highest temperatures investigated here.

It is widely recognized, however, that NO2- is a reaction intermediate in NO3- reduction [e.g., [51]] [57, 59]. For example, Wärna et al [59] proposed a reaction sequence from NO3- and NO2- through nitric oxide (NO), imidogen (HN˙) and aminyl radical (H2N¨) to NH3/NH4+ on the surface of Fe0. Several studies with NO2-/NO3- as well as some organic compounds suggest that Fe2+, Fe0, and Fe2+ sorbed on neoformed Fe minerals (e.g., magnetite) are likely electron donors for the reduction reactions [e.g., [60]] [61, 62]. The intriguing consequence of such a reaction mechanism in natural systems is that precipitation of secondary (neoformed) Fe minerals further along the flow path followed by surface sorption of Fe2+ would provide additional reaction sites for the reduction of NO2-/NO3- [e.g., [63]].

The role of alloys/metals

Based on the XPS (oxidation state of Ni) and SEM (abundance of Fe- and the absence of Ni alteration phases) results it is possible to construct an order of apparent stability of studied alloys and metals

Ni0 > Ni81Fe19 > Ni50Fe50 > Fe0

where Ni0 is most- and Fe0 is least stable under the studied experimental conditions. This enables us to generalize that the higher the Fe content, the higher the reactivity towards potential oxidizing agents (e.g., H2O, NO2-, NO3-) and thus the higher extent of alteration. Metals and alloys typically undergo reductive dissolution (e.g., Reaction 10); however alloys frequently dissolve the less noble metal preferentially, leaving the surface enriched in the more noble metal [e.g., [64]]. For example, the reductive dissolution of Ni50Fe50 alloys is expected to result in preferential release of Fe and a concomitant increase in the Ni:Fe ratio of the residual alloy.

Our findings are in agreement with metallurgical studies in which it has been demonstrated that Ni0 is more corrosion resistant than Fe0, a notion that serves as a basis for their frequent alloying [38, 65]. Unlike Fe0, Ni0 reacts to a lesser degree in aqueous environments (reaction produces H2 and Ni2+), especially under reducing conditions. The presence of an oxidizing agent is usually required for significant corrosion; however, a protective oxide film may develop and impede further reactions [38, 66]. Ni0 with a combination of catalytic properties and corrosion resistance (e.g., slow dissolution kinetics) may serve as a basis for a unique mechanism of N2 reduction, where Ni acts both as a reactant and a catalyst. We hypothesize that Ni0 reacts with H2O to produce H2, a portion of which may stay adsorbed on the surface in its atomic form (Hads) (Reaction 14). If N2 is also dissociatively chemisorbed (Reaction 15), surface-mediated reduction reactions may proceed (Reaction 16).

Ni + 2H2O → 2Hads + Ni2+ + 2OH- (14)

N2(aq) → 2Nads (15)

2Nads + 2H+ + 6Hads → 2NH4+ (16)

This set of reactions may operate until all plausible sorption sites are exhausted and/or deactivated. By analogy, we argue that if the experimental conditions were approaching the stability field of Fe metal (e.g., at sufficiently high fH2) it could behave in a similar manner.

There exist; however, "true" catalytic systems for NO2-/NO3- reduction, such as bimetallic Cu-Pt and Cu-Pd, Ag-Pd, Ag-Pt, which couple a noble metal and an oxidizable promoter. The reactions take place on the surface of Cu0 which acts as an electron donor for the reduction of N species and as an acceptor of electrons from dissociative sorption of H2 on the surface of Pt [67, 68]. Even though natural alloys of platinum group elements (Pt, Pd, Ir, Os, Rh, Ru) are scarce on modern Earth and are almost exclusively limited to magmatic segregation deposits, placers, and meteorites [e.g., [69]] [70, 71], their significance for prebiotic synthesis should not be overlooked [72].

The predominantly alkaline pH in reacted samples (Tab. 2) is likely a result of several pH controlling reactions such as reductive dissolution of metals (e.g., Reaction 10), mineral formation (e.g., magnetite), and the buffering reactions involving charged species including, but not limited to NO3-, NO2-, NH3, or NH4+. The fate of Fe2+ in the experiments reported here is difficult to constrain. Assuming completely anoxic conditions, temperatures below 85°C and a negligible pCO2 in our experiments, Fe(OH)2 (white rust) could precipitate (Reaction 17) and due to its instability serve as a precursor to other Fe oxides and hydroxides, most notably Fe3O4 (Reaction 18).

Fe++ + 2OH- → Fe(OH)2 (17)

3Fe(OH)2 → Fe3O4 + 2H2O + H2 (18)

At higher temperatures and/or in the presence of trace levels of O2 or other oxidizing agents (e.g., NO3-), mineral intermediates such as green rust (mixed-valence hydroxide) may have been involved [e.g., [73]] [74, 75].

The conversion of the original metal/alloy into a new mineral phase (e.g., coatings) may not necessarily negatively affect the NH3/NH4+ production. For example, wüstite (FeO) and green rust – both possible reaction products/intermediates during anaerobic Fe0 oxidation, have been shown to reduce NO2-/NO3- [e.g., [50]] [7678]. Magnetite and even goethite can also act as reductants for NO2-/NO3-, provided cations such as Fe2+, Cu2+, Fe3+, Al3+ are present in the system [e.g., [53]] [56, 79]. Equilibrium thermodynamic calculations, however, predict very little reactivity of magnetite, goethite, or ferrihydrite alone towards N2 and anaerobic experiments in the presence of green rust at ambient T, p conditions corroborate these predictions [80].

Implications for the Hadean Earth

Different modes of metal/alloy participation have different implications for natural systems, especially in terms of the amount of metal/alloy required to achieve the same NH3/NH4+ production. A catalyst remains stable during the reaction and therefore a small amount can, in theory, catalyze the formation of large amounts of NH3/NH4+. Conversely, a reactant would have to be present in sufficient amounts and/or would have to be continually formed in order to achieve comparable NH3/NH4+ production. While both mechanisms are plausible on the Hadean Earth, it is hard to assess which of the two would be prevalent. Based of equilibrium geochemical modeling, Smirnov [28] concluded that at 200°C Ni metal is stable at fH2 orders of magnitude lower than Fe metal and even Ni50Fe50 (tetrataenite) and Ni81Fe19 (awaruite). Combined with results acquired from this study, it would appear that Ni metal is the most suitable candidate for a sustained long-term NH3/NH4+ formation. Moreover, if we consider that the Hadean atmosphere may have had up to 30% H2 [29], the primordial ocean would contain significantly higher concentrations of dissolved H2 than today. In SHS, H2 from advected seawater combined with H2 formed by serpentinization could create conditions sufficiently reducing for stabilization of Fe containing alloys (e.g., awaruite, tetrataenite) and possibly even Fe0. Furthermore, as shown by Schoonen et al [72], seawater trapped in closed SHS (i.e., not open to seawater circulation) evolves to become extremely reduced as the partial pressure of hydrogen builds up.

The possibility of hydrothermal reduction of N2 to NH4+ permits us to attempt to constrain the total NH4+ flux from Hadean off-axis SHS. The following set of assumptions and variables were taken into account:

1) The total heat production of the Hadean Earth was several times higher than today [81, 82]. Because the exact value is unknown, we calculated scenarios for 2- to 8-times the present day heat flow (PDHF = 4.3 × 1013 W) [83] (Fig. 10); however, only values between 4 and 8 times PDHF are reported.

Figure 10
figure 10

Hadean hydrothermal flow as a function of total Earth's heat flow (expressed as multiplicities of present day heat flow – PDHF). Each data line thus represents percentage of the total heat flow released through hydrothermal systems at a given value of Hadean heat flow. The shaded area represents assumed realistic scenarios for the Hadean.

2) Because it is unclear if a global tectonic cycle was operational during the Hadean, we are unable to comment on the dissipation of Earth's internal heat, especially on the percentage of heat released through SHS. Therefore, two endmember scenarios are considered: a) heat is dissipated predominantly via volcanism (possibly through several supervolcanoes) and only 5% is released through hydrothermal activity; and b) 80% of heat is dissipated predominantly through hydrothermal activity (Fig. 10). For comparison, presently about 20% of PDHF is released through hydrothermal activity [83].

3) Due to the increased heat flow and possibly due to the blanketing effect of the atmosphere [e.g., [84]], we assume the mean ocean water temperature to be 70°C. Although modern serpentinization-driven SHS commonly vent fluids below 100°C [8587], we assume that the higher overall heat flow in the Hadean would also increase the fluid temperature of hydrothermal vents [e.g., [88]]. The temperature of the discharging fluid is thus assumed to be 200°C for the purpose of this calculation. Although the temperature of ambient seawater and of discharging fluid directly influences the total hydrothermal fluid mass flux (equation 19), their variations (± 20°C) only produced small changes in the final NH4+ fluxes (usually within the same order of magnitude; data not shown). The heat capacity (c p ) of hydrothermal seawater at 200°C and P ~100–600 bar is 4.1 J.g-1K-1[89].

4) Ocean water is assumed to be in equilibrium with 1 bar of N2, resulting in a dissolved N2(aq) concentration of 0.481 at 70°C [90]. For simplicity, no other gases and/or aqueous ions were taken into consideration.

5) Even though experimental results reported in this study suggest a conversion of N2-to-NH4+ 0.2 to 2.5% we calculate a variety of scenarios ranging from 0.1% to 10%. Although the 10% conversion may appear overly optimistic, our experiments suggest that the presence of advected H2 and or K+ may significantly improve the NH4+ production (Tab. 2; Fig. 4a). Metals/alloys may act as either catalysts or reactants, however, if metals/alloys do react, it must be assumed that the rate of their destruction (e.g., passivation, poisoning) is equal to their rate of formation (e.g., via serpentinization). It is important to point out that for simplicity, we do not distinguish between respective metals/alloys and we are only concerned with their capability to facilitate the conversion of N2 to NH4+ (in %).

The mass flux of seawater through hydrothermal systems (F) can be estimated from heat flux (H) in Watts, heat capacity of seawater (cp at 200°C) in J.g-1K-1 and temperature anomaly ΔT in Kelvin [83]:

F = H c p Δ T . MathType@MTEF@5@5@+=feaafiart1ev1aaatCvAUfKttLearuWrP9MDH5MBPbIqV92AaeXatLxBI9gBaebbnrfifHhDYfgasaacPC6xNi=xI8qiVKYPFjYdHaVhbbf9v8qqaqFr0xc9vqFj0dXdbba91qpepeI8k8fiI+fsY=rqGqVepae9pg0db9vqaiVgFr0xfr=xfr=xc9adbaqaaeGaciGaaiaabeqaaeqabiWaaaGcbaGaemOrayKaeyypa0tcfa4aaSaaaeaacqWGibasaeaacqWGJbWydaWgaaqaaiabdchaWbqabaGaeuiLdqKaemivaqfaaOGaeiOla4caaa@3653@

Using hydrothermal heat fluxes from Fig. 10 we can calculate annual seawater mass fluxes from SHS. Subsequently, using various N2-to-NH4+ conversion percentages (0.1 to 10%), annual NH4+ production of Hadean SHS is calculated (Fig. 11). Assuming the most conservative scenario with 0.1% conversion of N2 to NH4+, the annual NH4+ production would be between 5.9 × 108 mol (4 × PDTH) and 1.2 × 109 mol (8 × PDTH) if 5% of Earth's heat is removed via SHS and between 9.4 × 109 mol (4 × PDTH) and 1.9 × 1010 mol (8 × PDTH) if 80% of heat is removed via SHS. Conversely, with a 10% N2 conversion efficiency, the annual NH4+ production would be between 5.9 × 1010 mol (4 × PDTH) and 1.2 × 1011 mol (8 × PDTH) if 5% of heat is removed via SHS and between 9.4 × 1011 mol (4 × PDTH) and 1.9 × 1012 mol (8 × PDTH) if 80% of heat is removed by SHS (Tab. 5). To place these modeled fluxes in context we can compare their magnitude to those of other proposed NH3/NH4+ formation mechanisms (Fig. 11). An annual NH4+ flux at 1% conversion efficiency, for example, would be comparable to that based on a homogeneous reaction (Reaction 20) of Summers and Chang [4] or to the flux calculated by Brandes et al [13], which was based on NH3 formation in the presence of various minerals between 300 and 800°C.

Table 5 Total N content of four octahedrites analyzed by inert gas fusion (IMR Test Labs).
Figure 11
figure 11

NH4+ formation from N2 in Hadean hydrothermal systems. Fluxes are calculated as a function of N2 conversion between 1 and 10%. NH4+ formation from NO2-/NO3- is not included in these calculations.

6Fe2+ + 7H+ + NO2- → 6Fe(III) + 2H2O + NH3

Although we cannot comment on the total NH4+ content of the Hadean Ocean, we can estimate the contribution of hydrothermal N2 reduction per unit of time. For timescales longer than 1 year, the following equation may be used (21):

N H 4 + a d d i t i o n t o t h e o c e a n = a n n u a l N H 4 + p r o d u c t i o n V H a d e a n O c e a n t . MathType@MTEF@5@5@+=feaafiart1ev1aaatCvAUfKttLearuWrP9MDH5MBPbIqV92AaeXatLxBI9gBaebbnrfifHhDYfgasaacPC6xNi=xI8qiVKYPFjYdHaVhbbf9v8qqaqFr0xc9vqFj0dXdbba91qpepeI8k8fiI+fsY=rqGqVepae9pg0db9vqaiVgFr0xfr=xfr=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@832E@

NH4+ production in mol.yr-1 can be taken from Fig. 11 or Tab. 6 (or supplied from reader's own sources), t denotes the time period in years and Vocean is the total volume of Hadean Ocean in liters. We have calculated a scenario for one million years using the present-day global ocean volume (1.37 × 1021 L) but alternative calculations can be quickly performed for different volumes (e.g., if the Hadean ocean had twice the volume of the present-day ocean, the NH4+ concentrations in Fig. 12 and Tab 7 would be 50% smaller). For example, the conversion of 0.5% of N2 entrained in the advecting seawater would raise the NH4+ content of the (completely homogenized) Hadean ocean by ~8 to 17 μ (4× to 8× PDHF) every 1 Ma (Tab. 7). These results (Fig. 12, Tab. 7) represent an upper contribution limit of this reaction, because no sinks (ion exchange, photooxidation, loss to the gas phase, formation of organic molecules, etc) were taken into account. In the absence of a comprehensive Hadean Nitrogen Cycle model, it is difficult to quantitatively assess the annual loss of NH3/NH4+ from the ocean; however, the numbers in Fig. 12, Tab. 7 can be simply amended by assumption of loss expressed in %.

Table 6 NH4+ formation from N2 in Hadean hydrothermal systems. Fluxes ( are calculated as a function of N2 conversion between 1 and 10%. Note that NH4+ formation from NO2-/NO3- is not included in these calculations.
Table 7 Estimated increase in NH4+ concentration of the Hadean Ocean (in μmol.L-1) from the hydrothermal N2 reduction reaction per 1 Ma as a function of N2-to-NH4+ conversion percentages, heat flow and percentage of heat released via hydrothermal systems.
Figure 12
figure 12

Estimated increase in NH4+ concentration of the Hadean Ocean (in μmol.L-1) from the hydrothermal N2 reduction reaction per 1 Ma as a function of N2-to-NH4+ conversion percentages, heat flow and percentage of heat released via hydrothermal systems (5, 20 and 80%).

It is imperative to note that due to a large number of unknown and/or poorly constrained variables, these calculations should only be regarded as a first order approximation. However, it is clear that N2 reduction, albeit very inefficient, could have been a significant source of NH4+, especially in localized environments.

Because NO2-/NO3- are inherently easier to reduce than N2, its presence in advected seawater could have significantly increased the annual NH4+ hydrothermal flux. It is unclear; however, how much NO2-/NO3- would be advected into the crust, especially in the presence of such significant sinks as the reduction by Fe(II) [5]. While this process is a viable pathway to abiotic NH3/NH4+, its operation is dependent on atmospherically-driven processes of NO2-/NO3- formation as well as chemical composition of the Hadean Ocean, especially pH and mFe2+. A change in one of the parameters (e.g., a shift in oceanic pH) may have negatively affected or completely halted this pathway. We assume that serpentinization-driven SHS would have been less affected by changes in ocean water chemistry because their physico-chemical conditions (e.g., pH, fH2) are determined by fluid-rock interactions (e.g., availability of fresh rock) and possibly magmatic input rather than ocean composition. Moreover, the high temperature and pressure conditions combined with accumulations of suitable minerals would make these environments well suited for a long term, sustained NH3/NH4+ production on the Hadean Earth.

Besides facilitating the production of NH3/NH4+, metals and alloys in SHS may have been involved in other reactions potentially important for prebiotic synthesis. In the context of environmental science, for example, Fe0 was found to reduce nitrobenzene [91] or to facilitate reductive dehalogenation of carbon tetrachloride and chloroform [9294]; Fe2+ sorbed on Fe(III) minerals decomposes nitrobenzene [60]. Our future research will also assess SHS as potential sinks of prebiotic molecules during the late Hadean/early Archaean.

The notion that N is commonly present in Fe0 in its reduced form presents a possibility of meteoritic delivery of reduced N species to Earth, especially during the periods of heavy bombardment. Fe0 and its alloys (e.g., tetrataenite, awaruite, kamacite) are among the dominant mineral phases in iron meteorites and to a lesser extent in stony-iron meteorites [e.g., [95]] [9699].

To assess the possible importance of meteoric delivery of reduced N to Earth, we submitted four octahedrites for inert gas fusion analyses (IMR Test Labs, Lansing, NY). The meteorites – Bogou (IAB), Sikhote Alin (IIAB), Canyon Diablo (IAB), N'Goureyma (Ungrouped) [100103] (Stony Brook University's meteorite collection) contained 22 to 32 ppm of NTOT (Tab. 5). Although these analyses provided no insight into the oxidation state or speciation of nitrogen in these meteorites, it is likely to be present predominantly in the form of nitride (N3-) as is the case in similar commercially available metals, alloys and known meteorite minerals (e.g., roaldite, carlsbergite). Hence in the following calculation we assume that all meteorite-associated nitrogen is present as nitride. Nitride would be readily released from meteorites after falling into the Hadean Ocean as a result of the rapid and complete dissolution due to inherent instability of Fe0 in aqueous solutions (even in O2-free solutions). Aqueous nitride is expected to react quickly with protons to form NH3/NH4+. Similar scenario for meteoritic delivery of phosphorus has already been proposed by Pasek and collaborators [104, 105].

To constrain the influx of meteoritic N to the Hadean Ocean we have adapted the meteorite flux values used by Pasek et al [104, 105]: 2 × 105 kg.year-1 (current flux of iron meteorites to Earth; 50% of total meteoritic flux by weight) and meteoritic flux 105-106 times the present-day value during the Late Heavy Bombardment Period. Using these values we have created models for varying total reduced N content of iron meteorites: 5, 10, 15, 20, and 30 ppm. For comparison, average and median values for NTOT from 91 published analyses [106, 107] and four analyses acquired in this study were 20.1 and 12.3 ppm respectively.

The results presented in Fig. 13 show that during the Late Heavy Bombardment Period, iron meteorites could have delivered ~103 to 105 mol.yr-1 of NTOT to Earth which is approximately six to nine orders of magnitude less than our estimates for hydrothermal production (Fig. 11). Although the N influx was likely negligible on the global scale it is possible that crater lakes associated with iron meteorite impacts [108] may have contained significant concentrations of NH3/NH4+. Environments containing NH3/NH4+ and organic phosphorous compounds (e.g., phosphonates, organophosphates) from corroding iron meteorites ((Fe,Ni3)P) [104, 105] thus could have created very favorable, spatially-restricted conditions for prebiotic synthesis, perhaps unparalleled on the prebiotic Earth.

Figure 13
figure 13

Estimated annual flux of nitrogen from iron meteorites. Different line styles correspond to different average N content of iron meteorites. Shaded areas represent iron meteorite flux during the period of Late Heavy Bombardment.


1) N2 reduction to NH4+ was found to be limited (up to 2.5% at 200°C) compared to NO2-/NO3- (100% at 200°C)

2) Metals are more effective at reducing NO2-/NO3- than alloys; NH4+ is the dominant reaction product.

3) The reduction process exhibits a strong temperature dependence.

4) Fe0 and Ni0 were found to be least- and most resistant to alteration, respectively.

5) Ni0, Fe0, Ni50Fe50, Ni81Fe19 were found to contain up to 124 ppm of nitrogen in their structures, some of which is released upon dissolution and reacts to form NH4+.

6) Serpentinization-driven SHS were likely important sources of abiotic NH3/NH4+ in the Hadean Ocean.


  1. Hennet RJC, Holm NG, Engel MH: Abiotic synthesis of amino acids under hydrothermal conditions and the origin of life - A perpetual phenomenon. Naturwissenschaften. 1992, 79 (8): 361-365. 10.1007/BF01140180.

    Google Scholar 

  2. Marshall WL: Hydrothermal synthesis of amino acids. Geochim Cosmochim Ac. 1994, 58 (9): 2099-2106. 10.1016/0016-7037(94)90288-7.

    Google Scholar 

  3. Miller SL: A production of amino acids under possible primitive Earth conditions. Science. 1953, 117 (3046): 528-529. 10.1126/science.117.3046.528.

    Google Scholar 

  4. Summers DP: Sources and sinks for ammonia and nitrite on the early earth and the reaction of nitrite with ammonia. Orig Life Evol Biosph. 1999, 29 (1): 33-46. 10.1023/A:1006517823004.

    Google Scholar 

  5. Summers DP, Chang S: Prebiotic ammonia from reduction of nitrite by iron(II) on the early Earth. Nature. 1993, 365 (6447): 630-632. 10.1038/365630a0.

    Google Scholar 

  6. Summers DP: Ammonia formation by the reduction of nitrite/nitrate by FeS: Ammonia formation under acidic conditions. Orig Life Evol Biosph. 2005, 35 (4): 299-312. 10.1007/s11084-005-2040-1.

    Google Scholar 

  7. Kasting JF: Stability of ammonia in the primitive terrestrial atmosphere. J Geophys Res-Oc Atm. 1982, 87 (NC4): 3091-3098. 10.1029/JC087iC04p03091.

    Google Scholar 

  8. Zahnle K: Photochemistry of methane and the formation of Hydrocyanic Acid (HCN) in Earth's early atmosphere. J Geophys Res. 1986, 91 (D2): 2819-2834. 10.1029/JD091iD02p02819.

    Google Scholar 

  9. Eugster HP, Munoz J: Ammonium micas - Possible sources of atmospheric ammonia and nitrogen. Science. 1966, 151 (3711): 683-686. 10.1126/science.151.3711.683.

    Google Scholar 

  10. Schrauzer GN, Guth TD: Photolysis of water and photoreduction of nitrogen on titanium dioxide. J Am Chem Soc. 1977, 99 (22): 7189-7193. 10.1021/ja00464a015.

    Google Scholar 

  11. Schrauzer GN, Strampach N, Hui LN, Palmer MR, Salehi J: Nitrogen photo-reduction on desert sands under sterile conditions. P Natl Acad Sci USA. 1983, 80 (12): 3873-3876. 10.1073/pnas.80.12.3873.

    Google Scholar 

  12. Ranjit KT, Viswanathan B: Photocatalytic reduction of nitrite and nitrate ions over doped TiO2 catalysts. J Photoch Photobio A. 1997, 107 (1-3): 215-220. 10.1016/S1010-6030(97)00025-7.

    Google Scholar 

  13. Brandes JA, Boctor NZ, Cody GD, Cooper BA, Hazen RM, Yoder HS: Abiotic nitrogen reduction on the early Earth. Nature. 1998, 395 (6700): 365-367. 10.1038/26450.

    Google Scholar 

  14. Schoonen MAA, Xu Y: Nitrogen reduction under hydrothermal vent conditions: Implications for the prebiotic synthesis of C-H-O-N compounds. Astrobiology. 2001, 1 (2): 133-141. 10.1089/153110701753198909.

    Google Scholar 

  15. Dörr M, Kassbohrer J, Grunert R, Kreisel G, Brand WA, Werner RA, Geilmann H, Apfel C, Robl C, Weigand W: A possible prebiotic formation of ammonia from dinitrogen on iron sulfide surfaces. Angew Chem Int Ed Engl. 2003, 42 (13): 1540-1543. 10.1002/anie.200250371.

    Google Scholar 

  16. Kelley DS, Fruh-Green GL: Abiogenic methane in deep-seated mid-ocean ridge environments: Insights from stable isotope analyses. J Geophys Res-Planet. 1999, 104 (B5): 10439-10460. 10.1029/1999JB900058.

    Google Scholar 

  17. Mevel C: Serpentinization of abyssal peridotites at mid-ocean ridges. CR Geosci. 2003, 335 (10-11): 825-852. 10.1016/j.crte.2003.08.006.

    Google Scholar 

  18. Moody JB: An experimental study on the serpentinization of iron-bearing olivines. Can Miner. 1976, 14: 462-478.

    Google Scholar 

  19. Filippidis A: Chemical variation of olivine in the serpentinite of the central section in the Xerolivado chrome mine of Vourinos, Greece. Neues Jb Miner Abh. 1996, 170 (2): 189-205.

    Google Scholar 

  20. Chamberlain JA, McLeod CR, Traill RJ, Lachance GR: Native metals in the Muscox intrusion. Can J Earth Sci. 1965, 2: 189-215.

    Google Scholar 

  21. Dick HJB: Terrestrial nickel-iron from Josephine peridotite, its geologic occurrence, associations, and origin. Earth Planet Sc Lett. 1974, 24: 291-298. 10.1016/0012-821X(74)90107-1.

    Google Scholar 

  22. Ahmed Z, Bevan JC: Awaruite, iridian awaruite, and a new Ru-Os-Ir-Ni-Fe alloy from the Sakhakot-Qila Complex, Malakand-Agency, Pakistan. Mineral Mag. 1981, 44 (334): 225-230. 10.1180/minmag.1981.044.334.17.

    Google Scholar 

  23. Eckstrand OR: The Dumont serpentinite: A model for control of nickeliferous opaque mineral assemblages by alteration reactions in ultramafic rocks. Econ Geol. 1975, 70: 183-201.

    Google Scholar 

  24. Ashley PM: Opaque mineral assemblage formed during serpentinization in the Coolac ultramafic belt, New South Wales. J Geol Soc Aust. 1975, 22: 91-102.

    Google Scholar 

  25. Alt JC, Shanks III WC: Stable isotope compositions of serpentinite seamounts in the Mariana forearc: Serpentinization processes, fluid sources and sulfur metasomatism. Earth Planet Sc Lett. 2006, 242 (3-4): 272-285. 10.1016/j.epsl.2005.11.063.

    Google Scholar 

  26. Beard JS, Hopkinson L: A fossil, serpentinization-related hydrothermal vent, Ocean Drilling Program Leg 173, Site 1068 (Iberia Abyssal Plain): Some aspects of mineral and fluid chemistry. J Geophys Res-Planet. 2000, 105 (B7): 16527-16539. 10.1029/2000JB900073.

    Google Scholar 

  27. Filippidis A: Formation of awaruite in the system Ni-Fe-Mg-Si-O-H-S and olivine hydration with NaOH solution, an experimental study. Econ Geol. 1985, 80 (7): 1974-1980.

    Google Scholar 

  28. Smirnov A: Formation and Fate of Ammonium in the Hadean Ocean. Department of Geosciences. 2006, Stony Brook, NY , Stony Brook University, PhD: 177-

    Google Scholar 

  29. Tian F, Toon OB, Pavlov AA, De Sterck H: A hydrogen-rich early Earth atmosphere. Science. 2005, 308 (5724): 1014-1017. 10.1126/science.1106983.

    Google Scholar 

  30. Kasting JF: Earth's early atmosphere. Science. 1993, 259 (5097): 920-926. 10.1126/science.11536547.

    Google Scholar 

  31. Navarro-Gonzalez R, McKay CP, Nna-Mvondo D: A possible nitrogen crisis for Archaean life due to reduced nitrogen fixation by lightning. Nature. 2001, 412 (6842): 61-64. 10.1038/35083537.

    Google Scholar 

  32. Nna-Mvondo D, Navarro G, Raulin F, Coll P: Nitrogen fixation by corona discharge on the early Precambrian Earth. Origins Life Evol B. 2005, 35 (5): 401-409. 10.1007/s11084-005-1972-9.

    Google Scholar 

  33. Kasting JF: Theoretical constraints on oxygen and carbon dioxide concentrations in the Precambrian atmosphere. Precambrian Res. 1987, 34 (3-4): 205-229. 10.1016/0301-9268(87)90001-5.

    Google Scholar 

  34. Mancinelli RL, McKay CP: The evolution of nitrogen cycling. Origins Life Evol B. 1988, 18 (4): 311-325. 10.1007/BF01808213.

    Google Scholar 

  35. ASTM-E-1019-00: Standard test methods for determination of carbon, sulfur, nitrogen and oxygen in steel and in iron, nickel and cobalt alloys. Annual Book of ASTM Standards. 2002, ASTM International, 03.05: 754-773.

    Google Scholar 

  36. Bethke CM: The Geochemist's Workbench, Release 5.0. 2004, University of Illinois

    Google Scholar 

  37. Howald RA: The thermodynamics of tetrataenite and awaruite: A review of the Fe-Ni phase diagram. Metall Mater Trans A. 2003, 34A (9): 1759-1769. 10.1007/s11661-003-0142-9.

    Google Scholar 

  38. Davis JR: Nickel, cobalt and their alloys. 2000, Materials Park, OH , ASM International, 442-

    Google Scholar 

  39. Kodentsov AA, van Dal MJH, Cserhati C, Daroczi L, van Loo FJJ: Permeation of nitrogen in solid nickel and deformation phenomena accompanying internal nitridation. Acta Mater. 1999, 47 (11): 3169-3180. 10.1016/S1359-6454(99)00194-9.

    Google Scholar 

  40. Cottrell AH: An introduction to metallurgy. 1968, London , Edward Arnold Publishers Ltd., 548-

    Google Scholar 

  41. Beddoes J, Parr JG: Introduction to stainless steel. 1998, Materials Park, OH , ASM International, 315-3rd

    Google Scholar 

  42. Ech-chamikh E, Essafti A, Ijdiyaou Y, Azizan M: XPS study of amorphous carbon nitride (a-C:N) thin films deposited by reactive RF sputtering. Solar Energy Materials and Solar Cells. 2006, 90 (10): 1420-1423. 10.1016/j.solmat.2005.10.007.

    Google Scholar 

  43. Jennings JR: Catalytic ammonia synthesis. 1991, New York , Plenum Press, 476-

    Google Scholar 

  44. Ertl G: Elementary steps in Ammonia synthesis: The surface science approach. Catalytic ammonia synthesis. Edited by: Jennings JR. 1991, New York , Plenum Publishing, 109-132.

    Google Scholar 

  45. Alberty RA: Thermodynamics of the nitrogenase reactions. J Biol Chem. 1994, 269 (10): 7099-7102.

    Google Scholar 

  46. Howard JB, Rees DC: Structural basis of biological nitrogen fixation. Chem Rev. 1996, 96 (7): 2965-2982. 10.1021/cr9500545.

    Google Scholar 

  47. Moody JB: Serpentinization - Review. Lithos. 1976, 9 (2): 125-138. 10.1016/0024-4937(76)90030-X.

    Google Scholar 

  48. Reardon EJ: Anaerobic corrosion of granular iron: Measurement and interpretation of hydrogen evolution rates. Environ Sci Technol. 1995, 29 (12): 2936 -22945. 10.1021/es00012a008.

    Google Scholar 

  49. Chen YM, Li CW, Chen SS: Fluidized zero valent iron bed reactor for nitrate removal. Chemosphere. 2005, 59 (6): 753-759. 10.1016/j.chemosphere.2004.11.020.

    Google Scholar 

  50. Cheng IF, Muftikian R, Fernando Q, Korte N: Reduction of nitrate to ammonia by zero-valent iron. Chemosphere. 1997, 35 (11): 2689-2695. 10.1016/S0045-6535(97)00275-0.

    Google Scholar 

  51. Choe SH, Ljestrand HM, Khim J: Nitrate reduction by zero-valent iron under different pH regimes. Appl Geochem. 2004, 19 (3): 335-342. 10.1016/j.apgeochem.2003.08.001.

    Google Scholar 

  52. Hu HY, Goto N, Fujie K: Effect of pH on the reduction of nitrite in water by metallic iron. Water Res. 2001, 35 (11): 2789-2793. 10.1016/S0043-1354(00)00570-4.

    Google Scholar 

  53. Huang CP, Wang HW, Chiu PC: Nitrate reduction by metallic iron. Water Res. 1998, 32 (8): 2257-2264. 10.1016/S0043-1354(97)00464-8.

    Google Scholar 

  54. Huang YH, Zhang TC: Effects of low pH on nitrate reduction by iron powder. Water Res. 2004, 38 (11): 2631-2642. 10.1016/j.watres.2004.03.015.

    Google Scholar 

  55. Huang YH, Zhang TC: Enhancement of nitrate reduction in Fe-0-packed columns by selected cations. J Environ Eng-ASCE. 2005, 131 (4): 603-611. 10.1061/(ASCE)0733-9372(2005)131:4(603).

    Google Scholar 

  56. Huang YH, Zhang TC, Shea PJ, Comfort SD: Effects of oxide coating and selected cations on nitrate reduction by iron metal. J Environ Qual. 2003, 32 (4): 1306-1315.

    Google Scholar 

  57. Alowitz MJ, Scherer MM: Kinetics of nitrate, nitrite, and Cr(VI) reduction by iron metal. Environ Sci Technol. 2002, 36 (3): 299-306. 10.1021/es011000h.

    Google Scholar 

  58. Cruz-Carrera BME, Arancibia CG: Influence of metallic cadmium on the electrochemical reduction of nitrate and nitrite ions. An Quim B-Inorg Anal. 1980, 76 (2): 267-272.

    Google Scholar 

  59. Wärna J, Turunen I, Salmi T, Maunula T: Kinetics of nitrate reduction in monolith reactor. Chem Eng Sci. 1994, 49 (24B): 5763-5773. 10.1016/0009-2509(94)00331-9.

    Google Scholar 

  60. Klausen J, Tröber SP, Haderlein SB, Schwarzenbach RP: Reduction of substituted nitrobenzenes by Fe(II) in aqueous mineral suspensions. Environ Sci Technol. 1995, 29: 2396-2404. 10.1021/es00009a036.

    Google Scholar 

  61. Weber EJ: Iron-mediated reductive transformations: Investigation of reaction mechanism. Environ Sci Technol. 1996, 30 (2): 716 -7719. 10.1021/es9505210.

    Google Scholar 

  62. Huang YH, Zhang TC: Effects of dissolved oxygen on formation of corrosion products and concomitant oxygen and nitrate reduction in zero-valent iron systems with or without aqueous Fe2+. Water Res. 2005, 39 (9): 1751-1760.

    Google Scholar 

  63. Sorensen J, Thorling L: Stimulation by Lepidocrocite (gamma-FeOOH) of Fe(II)-dependent nitrite reduction. Geochim Cosmochim Ac. 1991, 55 (5): 1289-1294. 10.1016/0016-7037(91)90307-Q.

    Google Scholar 

  64. Seo M, Sato N: Selective surface oxidation of Fe30-Ni alloy: Mt. Fuji, Lake Yamanaka, Japan.1982, The Japan Institute of Metals, 175-182.

    Google Scholar 

  65. Neely JE, Bertone TJ: Practical metallurgy and materials of industry. 2002, Upper Saddle River, NJ , Prentice Hall, 464-6th

    Google Scholar 

  66. Cooley WE: Nickel. McGraw-Hill encyclopedia of chemistry. Edited by: Parker SP. 1993, New York , McGraw-Hill, Inc.

    Google Scholar 

  67. Epron F, Gauthard F, Pineda C, Barbier J: Catalytic reduction of nitrate and nitrite on Pt-Cu/Al2O3 catalysts in aqueous solution: Role of the interaction between copper and platinum in the reaction. J Catal. 2001, 198 (2): 309-318. 10.1006/jcat.2000.3138.

    Google Scholar 

  68. Gauthard F, Epron F, Barbier J: Palladium and platinum-based catalysts in the catalytic reduction of nitrate in water: effect of copper, silver, or gold addition. J Catal. 2003, 220 (1): 182-191. 10.1016/S0021-9517(03)00252-5.

    Google Scholar 

  69. Hoashi M, Brooks RR, Reeves RD: Palladium, platinum and rhutenium in iron meteorites and their taxonomic significance. Chem Geol. 1993, 106: 207-218. 10.1016/0009-2541(93)90027-G.

    Google Scholar 

  70. Tolstykh N, Krivenko A, Sidorov E, Laajoki K, Podlipsky M: Ore mineralogy of PGM placers in Siberia and the Russian Far East. Ore Geol Rev. 2002, 20 (1-2): 1-25. 10.1016/S0169-1368(02)00036-7.

    Google Scholar 

  71. Cawthorn RG, Lee CA, Schouwstra RP, Mellowship P: Relationship between PGE and PGM in the Bushveld Complex. Can Miner. 2002, 40: 311-328. 10.2113/gscanmin.40.2.311.

    Google Scholar 

  72. Schoonen MAA, Smirnov A, Cohn C: A perspective on the role of minerals in prebiotic synthesis. Ambio. 2004, 33 (8): 539-551. 10.1639/0044-7447(2004)033[0539:APOTRO]2.0.CO;2.

    Google Scholar 

  73. Blesa MA, Matijevič E: Phase transformations of iron oxides, oxohydroxides, and hydrous oxides in aqueous media. Adv Colloid Interfac Sci. 1989, 29 (3-4): 173-221. 10.1016/0001-8686(89)80009-0.

    Google Scholar 

  74. Refait P, Memet JB, Bon C, Sabot R, Genin JMR: Formation of the Fe(II)-Fe(III) hydroxysulphate green rust during marine corrosion of steel. Corros Sci. 2003, 45 (4): 833-845. 10.1016/S0010-938X(02)00184-1.

    Google Scholar 

  75. Cornell RM, Schwertmann U: The Iron Oxides: Structure, Properties, Reactions, Occurrences and Uses. 2003, Weinheim , Wiley, 703-2nd

    Google Scholar 

  76. Hansen HCB, Koch CB, NanckeKrogh H, Borggaard OK, Sorensen J: Abiotic nitrate reduction to ammonium: Key role of green rust. Environ Sci Technol. 1996, 30 (6): 2053-2056. 10.1021/es950844w.

    Google Scholar 

  77. Hansen HCB, Koch CB: Reduction of nitrate to ammonium by sulphate green rust: activation energy and reaction mechanism. Clay Miner. 1998, 33 (1): 87-101. 10.1180/000985598545453.

    Google Scholar 

  78. Rakshit S, Matocha CJ, Haszler GR: Nitrate reduction in the presence of wustite. J Environ Qual. 2005, 34 (4): 1286-1292. 10.2134/jeq2004.0459.

    Google Scholar 

  79. Ottley CJ, Davison W, Edmunds WM: Chemical catalysis of nitrate reduction by iron (II). Geochim Cosmochim Ac. 1997, 61 (9): 1819-1828. 10.1016/S0016-7037(97)00058-6.

    Google Scholar 

  80. Wander MCF, Kubicki JD, Schoonen MAA: Reduction of N2 by Fe2+ - comparison of homogeneous and heterogeneous reactions: A theoretical study. Astrobiology. 2006, Washington, DC , 6 (1): 112-

  81. Abbott DH, Hoffman SE: Archaean plate tectonics revisited. 1. Heat flow, spreading rate, and the age of subducting oceanic lithosphere and their effects on the origin and evolution of continents. Tectonics. 1984, 3 (4): 429-448. 10.1029/TC003i004p00429.

    Google Scholar 

  82. Turcotte DL: On the thermal evolution of the Earth. Earth Planet Sc Lett. 1980, 48: 53-58. 10.1016/0012-821X(80)90169-7.

    Google Scholar 

  83. Elderfield H, Schultz A: Mid-ocean ridge hydrothermal fluxes and the chemical composition of the ocean. Annu Rev Earth Pl Sc. 1996, 24: 191-224. 10.1146/

    Google Scholar 

  84. Kasting JF: Bolide impacts and the oxidation state of carbon in the Earth's early atmosphere. Origins Life Evol B. 1990, 20 (3-4): 199-231. 10.1007/BF01808105.

    Google Scholar 

  85. Charlou JL, Fouquet Y, Bougault H, Donval JP, Etoubleau J, Jean-Baptiste P, Dapoigny A, Appriou P, Rona PA: Intense CH4 plumes generated by serpentinization of ultramafic rocks at the intersection of the 15 degrees 20 ' N fracture zone and the Mid-Atlantic Ridge. Geochim Cosmochim Ac. 1998, 62 (13): 2323-2333. 10.1016/S0016-7037(98)00138-0.

    Google Scholar 

  86. Kelley DS, Karson JA, Blackman DK, Fruh-Green GL, Butterfield DA, Lilley MD, Olson EJ, Schrenk MO, Roe KK, Lebon GT, Rivizzigno P: An off-axis hydrothermal vent field near the Mid-Atlantic Ridge at 30 degrees N. Nature. 2001, 412 (6843): 145-149. 10.1038/35084000.

    Google Scholar 

  87. Von Damm KL: Seafloor hydrothermal activity - Black smoker chemistry and chimneys. Annu Rev Earth Pl Sc. 1990, 18: 173-204. 10.1146/annurev.ea.18.050190.001133.

    Google Scholar 

  88. Macleod G, McKeown C, Hall AJ, Russell MJ: Hydrothermal and oceanic pH conditions of possible relevance to the origin of life. Orig Life Evol Biosph. 1994, 24 (1): 19-41. 10.1007/BF01582037.

    Google Scholar 

  89. Bischoff JL, Rosenbauer RJ: An empirical equation of state for hydrothermal seawater (3.2 percent NaCl). Am J Sci. 1985, 285: 725-763.

    Google Scholar 

  90. Gaventman LH: Solubility of selected gases in water. CRC Handbook of Chemistry and Physics. Edited by: Lide DR. 1994, Boca Raton , CRC Press, 6-3. 75th

    Google Scholar 

  91. Agrawal A, Tratnyek PG: Reduction of nitroaromatic compounds by zero-valent iron metal. Environ Sci Technol. 1996, 30: 153-150. 10.1021/es950211h.

    Google Scholar 

  92. Matheson LJ, Tratnyek PG: Reductive dehalogenation of chlorinated methanes by iron metal. Environ Sci Technol. 1994, 28: 2045-2053. 10.1021/es00061a012.

    Google Scholar 

  93. Warren KD, Arnold RG, Bishop TL, Lindholm LC, Batterton EA: Kinetics and mechanism of reductive dehalogenation of carbon tetrachloride using zero-valent metals. J Hazard Mater. 1995, 41: 217-227. 10.1016/0304-3894(94)00117-Y.

    Google Scholar 

  94. Gillham RW, O'Hannesin F: Enhanced degradation of halogenated aliphatics by zero-valent iron. Ground Water. 1994, 32 (6): 958-967. 10.1111/j.1745-6584.1994.tb00935.x.

    Google Scholar 

  95. D'Orazio M, Folco L, Perchiazzi N: The Bagnone iron meteorite (Tuscany, Italy): History, mineralogy, and chemical classification. Meteorit Planet Sci. 2004, 39 (8): A133-A138.

    Google Scholar 

  96. Rubin AE: Euhedral awaruite in the Allende meteorite: Implications for the origin of awaruite- and magnetite-bearing nodules in CV3 chondrites. Am Mineral. 1991, 76 (1356-1362):

  97. Nagata T, Carleton BJ: Tetrataenite in carbonaceous chondrites. P Jpn Acad B-Phys. 1990, 66 (10): 183-188. 10.2183/pjab.66.183.

    Google Scholar 

  98. Nagata T, Carleton BJ: Tetrataenite in chondritic meteorites. P Jpn Acad B-Phys. 1989, 65 (6): 121-124. 10.2183/pjab.65.121.

    Google Scholar 

  99. Gattacceca J, Rochette P, Bourot-Denise M: Magnetic properties of a freshly fallen LL ordinary chondrite: the Bensour meteorite. Phys Earth Planet In. 2003, 140 (4): 343-358. 10.1016/j.pepi.2003.10.001.

    Google Scholar 

  100. Foote AE: Meteoritic iron of Canyon Diablo. Am J Sci. 1891, 42: 413-417.

    Google Scholar 

  101. Unik JP, Henderson DJ, Huizenga JR: Radioactive species produced by cosmic rays in the Bogou iron meteorite. Geochim Cosmochim Ac. 1964, 28: 593-594. 10.1016/0016-7037(64)90079-1.

    Google Scholar 

  102. Yavnel AA: Issledovanie struktury Sikhote-Alinskogo meteorita. Dokl Akad Nauk. 1948, 60 (8): 1381-1384.

    Google Scholar 

  103. Cohen E: Meteoric iron from N'Goureyma, near Djenne, Province of Macina, Soudan. Am J Sci. 1903, 15 (88): 254-258.

    Google Scholar 

  104. Pasek M, Lauretta DS: Aqueous corrosion of phosphide minerals from iron meteorites: A highly reactive source of prebiotic phosphorus on the surface of the early Earth. Astrobiology. 2005, 5 (4): 515-535. 10.1089/ast.2005.5.515.

    Google Scholar 

  105. Pasek MA, Dworkin JP, Lauretta DS: A radical pathway for organic phosphorylation during schreibersite corrosion with implications for the origin of life. Geochim Cosmochim Ac. 2007, 71 (7): 1721-1736. 10.1016/j.gca.2006.12.018.

    Google Scholar 

  106. Franchi IA, Wright IP, Pillinger CT: Constraints on the formation conditions of iron meteorites based on concentrations and isotopic compositions of iron meteorites. Geochim Cosmochim Ac. 1993, 57: 3105-3121. 10.1016/0016-7037(93)90297-A.

    Google Scholar 

  107. Prombo CA, Calyton RN: Nitrogen isotopic compositions of iron meteorites. Geochim Cosmochim Ac. 1993, 57: 3749-3761. 10.1016/0016-7037(93)90153-N.

    Google Scholar 

  108. Bland PA, Artemieva NA: The rate of small impacts on Earth. Meteorit Planet Sci. 2006, 41: 607-631.

    Google Scholar 

  109. Peretti A, Dubessy J, Mullis J, Frost BR, Trommsdorff V: Highly reducing conditions during Alpine metamorphism of the Malenco peridotite (Sondrio, Northern Italy) indicated by mineral paragenesis and H2 in fluid inclusions. Contrib Mineral Petr. 1992, 112 (2-3): 329-340. 10.1007/BF00310464.

    Google Scholar 

  110. Tarkian M, Economou-Eliopoulos M, Sambanis G: Platinum-group minerals in chromitites from the Pindos ophiolite complex, Greece. Neues Jahrbuch Fur Mineralogie-Monatshefte. 1996, 4: 145-160.

    Google Scholar 

  111. Auge T, Cabri LJ, Legendre O, McMahon G, Cocherie A: PGE distribution in base-metal alloys and sulfides of the New Caledonia ophiolite. Can Miner. 1999, 37: 1147-1161.

    Google Scholar 

  112. Agafonov LV, Lesnov FP: Platinoids in websterites from the Narun Massif of mafic and ultramafic rocks (Western Mongolia). Geol Geofiz. 1997, 38 (12): 1949-1954.

    Google Scholar 

  113. Arai S, Prichard HM, Matsumoto I, Fisher PC: Platinum-group minerals in podiform chromitite from the Kamuikotan zone, Hokkaido, northern Japan. Resour Geol. 1999, 49 (1): 39-47.

    Google Scholar 

  114. Zhmodik SM, Agafonov LV: Shandite and other nickel minerals from chromitites of ophiolite association in the southeast of East Sayan. Geol Geofiz. 2000, 41 (5): 712-721.

    Google Scholar 

  115. Ahmed Z: Comparison of the geochemistry of ophiolitic pyroxenites with a strongly fractionated dyke of pyroxenite from the Sakhakot-Qila Ophiolite, Pakistan. Chem Geol. 1991, 91 (4): 335-355. 10.1016/0009-2541(91)90094-8.

    Google Scholar 

Download references


This research was funded by NASA Exobiology Program (grant NAG 513438) to Martin Schoonen. Francis McCubbin is thanked for help with electron probe microanalysis. Matthew Wander's (SBU) comments and insight into mechanisms of N reduction are much appreciated. We are also thankful to Matthew Pasek (U. Arizona) for comments on N flux from iron meteorites. We appreciate the help of two anonymous reviewers for their valuable comments on an earlier version of this article. Dr. Ken B. Anderson is thanked for editorial handling of the manuscript.

Author information

Authors and Affiliations


Corresponding author

Correspondence to Alexander Smirnov.

Additional information

Competing interests

The authors declare that they have no competing interests.

Authors’ original submitted files for images

Rights and permissions

Open Access This article is distributed under the terms of the Creative Commons Attribution 2.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Reprints and Permissions

About this article

Cite this article

Smirnov, A., Hausner, D., Laffers, R. et al. Abiotic ammonium formation in the presence of Ni-Fe metals and alloys and its implications for the Hadean nitrogen cycle. Geochem Trans 9, 5 (2008).

Download citation

  • Received:

  • Accepted:

  • Published:

  • DOI:


  • Magnetite
  • HDPE
  • Reductive Dissolution
  • Iron Meteorite
  • Green Rust