Microbial and hydrothermal aspects of ferric oxyhydroxides and ferrosic hydroxides: the example of Franklin Seamount, Western Woodlark Basin, Papua New Guinea
© The Royal Society of Chemistry and the Division of Geochemistry of the American Chemical Society 2001
Received: 15 June 2001
Accepted: 17 August 2001
Published: 05 September 2001
Deposits of Fe-Si-Mn oxyhydroxides are commonly found on the seafloor on seamounts and mid-ocean spreading centers. At Franklin Seamount located near the western extremity of Woodlark Basin, Papua New Guinea, Fe-Si-Mn oxyhydroxides are being precipitated as chimneys and mounds upon a substrate of mafic lava. Previous studies have shown that the vent fluids have a low temperature (20–30°C) and are characterized by a total dissolved iron concentration of 0.038 mM kg-1, neutral pH (6.26) and no measurable H2S. The chimneys have a yellowish appearance with mottled red–orange patches when observed in situ from a submersible, but collected samples become redder within a few hours of being removed from the sea. The amorphous iron oxyhydroxides, obtained from active and inactive vents, commonly possess filamentous textures similar in appearance to sheaths and stalks excreted by the iron-oxidizing bacteria Leptothrix and Gallionella; however, formless agglomerates are also common. Textural relationships between apparent bacterial and non-bacterial iron suggest that the filaments are coeval with and/or growing outwards from the agglomerates. The amorphous iron oxyhydroxides are suggested to precipitate hydrothermally as ferrosic hydroxide, a mixed-valence (Fe2+-Fe3+) green–yellow iron hydroxide compound. Consideration of the thermodynamics and kinetics of iron in the vent fluid, suggest that the precipitation is largely pH controlled and that large amounts of amorphous iron oxyhydroxides are capable of being precipitated by a combination of abiotic hydrothermal processes. Some biologically induced precipitation of primary ferric oxyhydroxides (two-XRD-line ferrihydrite) may have occurred directly from the fluid, but most of the filamentous iron micro-textures in the samples appear to have a diagenetic origin. They may have formed as a result of the interaction between the iron-oxidizing bacteria and the initially precipitated ferrosic hydroxide that provided a source of ferrous iron needed for their growth. The processes described at Franklin Seamount provide insight into the formation of other seafloor oxyhydroxide deposits and ancient oxide-facies iron formation.
Amorphous iron oxyhydroxides combined with variable amounts of manganese oxyhydroxides and silica are common in the oceans. [1–3] but have not been as extensively studied as sulfide deposits. They are typically found in areas of volcanic activity such as at mid-ocean and back-arc spreading centers and on intraplate seamounts. Some are spatially associated with sulfide deposits, usually around the margins and, from their high base metal content, are clearly oxidation products of the sulfides. Others, the subject of this paper, were precipitated as oxides directly from hydrothermal fluids. These can form large deposits up to hundreds of meters across. They are found both in proximity to sulfide deposits and completely isolated from them. A distinctive characteristic is that, regardless of their location, these primary oxide deposits have a much lower content of base (except iron) and precious metals than those that have formed by oxidation of sulfides .
The observation of the active creation of these chimneys together with their distinctive chemical composition characterized by a paucity of hydrothermally immobile elements such as Al, Ti and Zr (ref. ) suggests a primary abiotic hydrothermal control on the formation of these types of deposits. Conversely, close examination of similar materials by Juniper and Fouquet, Alt and Fortin found they possess complex filamentous micro-textures of apparent bacterial origin. The central role of filamentous bacteria in the precipitation of iron in acid mine drainage environments, subterranean environments and acidic surface hot springs is well known. Fortin and Ferris[15, 16] discussed the capability of bacteria to provide nucleation sites favorable for iron and manganese deposition. However, the importance of such sites, whether or not due to active metabolic processes, are apt to diminish under the near-neutral pH conditions of warm seafloor springs because kinetic barriers to the chemical precipitation of iron are greatly reduced at higher pH.  In general, both the microbial and abiotic chemical processes that occur at seafloor vent sites need to be considered in relation to the genesis of large amorphous iron oxyhydroxide deposits because the free energy of crystal nucleation (and thus precipitation) is constrained thermo-dynamically by the bulk free energy of the solution and the interfacial free energy of available surfaces. [16, 17] Their study is important because such marine deposits are similar in their chemistry and geological setting to many ancient iron formations found on land. [8, 18]
Iron, because of its multi-valent nature, is a sensitive indicator of its redox environment thus its behavior at the seafloor sediment/water interface can serve as a tool to understanding the physicochemical conditions for the precipitation of the oxyhydroxides at Franklin Seamount. This paper presents mineralogical, chemical and morphological information on the oxyhydroxides from Franklin Seamount that is interpreted in light of the thermodynamics and kinetics of low temperature hydrothermal iron systems, systematics of vent fluid chemistry and previous research on bacterial processes and habitats. These interpretations are used to explain the precipitation of iron locally around the vent site and to make comparisons with analogous environments associated with the precipitation of iron such as in other seafloor locations, soils and ancient iron formations.
Method of investigation
The samples for this study were collected by submersible and consist essentially of amorphous iron oxyhydroxides. Once on board the ship, the raw wet samples were placed into plastic containers or bags and the material was not dried until it was being prepared for laboratory study a few months later. Nothing was done to preserve possible organic remains in the samples so observed textures attributed to such are fossils.
The air-dried samples were first examined by light microscopy. This was followed by examination by scanning electron microscope (SEM) with an attached energy dispersive spectrometer (EDS). The SEM was operated at 15 to 25 kV with magnifications of 1000 to 12,000. Carbon coating of many of the samples considerably improved the quality of the images. A transmission electron microscope (TEM) equipped with an EDS was used to examine individual grains at higher magnifications of 10,000 to 200,000 at 200 kV. Grains were also characterized by selected area electron diffraction (SAED).
Chemistry of low temperature vent fluid sample from Franklin Seamount, Woodlark Basin. All data from Binns et al.5
Alkalinity/u equiv l-1
2.5 × 10-6-4.5 × 10-6
4 × 10-6
Description of samples
The samples are very friable with a roughly laminated to stromatolitic to porous, clotted texture (Fig. 2b). Amorphous iron oxyhydroxides are commonly coated by the black Mn oxyhydroxides, birnessite and todorokite. Dark green non-tronite is found in the interiors of some samples although distinctive bright green patches were also observed from the submersible on the surface of an actively forming chimney near the vent orifice.  These bright green patches are suggestive of ferrous trioctahedral smectite, a reduced precursor to non-tronite. 
In thin section, the amorphous iron oxyhydroxide exhibits a complex mottled structure of hair-like strands or scattered circular patches together with filaments of probable biological origin that appear to emanate from the strands and patches (Fig. 2c,d). The filaments have a sinuous, apparently branching, morphology (Fig. 2e), or have the appearance of bunched streamers (Fig. 2f). The textures in Fig. 2 suggest that the iron-rich material forms a coating.
It is difficult to determine if samples containing voluminous apparently non-bacterial agglomerates are just masked filamentous textures. This is probably not the case because the observed filaments in such samples do not appear to be especially thickened by additional iron oxyhydroxide deposition (Fig. 3a,b,c,d,e,f,g). Filaments in some samples appear to be degraded making their distinction from the formless micro-textures uncertain (Fig. 3h). However, Fig. 3d,e,f,g show non-degraded filaments adjacent to the formless blebs. These images are different from that exhibited in Fig. 3h. No evidence was found for formless micro-textures replacing degraded filaments.
In summary, the amorphous iron oxyhydroxide in the samples displays a variety of morphologies that can be divided into three groups: (1) morphologies which appear to form or mold the walls of filamentous and/or stalked structures (Fig. 3a,b,c,d, and 4c,d,e); (2) morphologies which form discrete irregularly shaped formless agglomerates (Fig. 3c,d,e,f); and (3) morphologies which appear to have accumulated on the walls of the filaments and stalks (Fig. 4f). The first two groups are more abundant but their proportions are highly variable from sample to sample. The second group predominates in freshly precipitated material sampled from the actively venting part of a chimney, whereas nearly all of the material appears to be filamentous in samples from other parts of active chimneys and from inactive chimneys.
Iron oxidizing bacteria
A sheath is defined as a hollow cylindrical structure made up predominantly of encrusted iron and possibly manganese oxyhydroxides that surrounds a chain of cells. It is closely fitting but not in intimate contact with the cells so the bacterium may move out leaving behind a preserved cast.  The width, length and rough surface of the described filaments suggest that Leptothrix is the most common genus at the Franklin Seamount vent sites.
The samples from Franklin Seamount contain very little organic carbon (0.18 to 0.94 wt.% Corg, ref. ), so it is probable that the organisms had died and decomposed, leaving behind their fossil form. Submersible observations of the chimneys and shipboard examination of the samples found no indication of macro-biological activity except for a few worm casts. [4, 5] The genus Gallionella is identified at the vent sites by its spirally twisted stalk structure (Figs. 3d and 4e) formed by the rotation of the individual filaments of its apical cells. 
In summary, the morphologies of ferric iron casts suggest that the iron oxidizing bacteria Leptothrix and Gallionella once thrived within the iron oxyhydroxide chimneys at Franklin Seamount. A near neutral pH, low f(O2) and ferrous iron-rich vent fluid combined with a seawater environment rich in organic carbon favored the growth of these genera. Recognition of the casts made by these genera, and specifically the textures of the manganese and iron, is good evidence that microbially mediated deposition of iron is occurring at Franklin Seamount.
We postulate that, at the low temperatures of the vent fluids, chemical reactions involving iron phases are controlled by reaction kinetics which slow the attainment of true equilibria in these systems. In order to account for this thermodynamically, Lindsay and Ponnamperuma et al.  used the standard free energies of formation for unstable hydroxides rather than their crystalline counterparts when modeling the behavior of iron in soils at a temperature and pH similar to those of the vent fluids at Franklin Seamount. This is because, according to the Oswald step rule, an unstable phase does not necessarily transform directly to a stable phase, but may pass through successive intermediate phases due to there being lower activation energy barriers via that route. These intermediate unstable phases are preserved in the form of amorphous iron oxyhydroxides in both soils and in the submarine environment at Franklin Seamount. Iron has a greater solubility relative to amorphous iron oxyhydroxides than to their crystalline counterparts but the higher reactivity of the former results in their preferential precipitation from hydrothermal solutions. 
For the purposes of thermodynamic modeling, Fe(OH)3 or ferric hydroxide is used to describe unstable amorphous ferric oxyhydroxides or two-XRD-line ferrihydrite. This material is well characterized in the literature and displays a variety of brown to red colors depending on its crystallinity.  The true composition of ferric hydroxide is uncertain and variable depending upon its crystallinity with proposed examples such as Fe5HO8·4H2O (ref. ), Fe5(O4H3)3 (ref. ), 5Fe2O3·9H2O (ref. ), Fe4(O,OH,H2O)12 (ref. ) and VIFe2.9IV (Si,Fe,Al)1.3-(O,OH,H2O)12 (ref. ).
Fe3(OH)8 is used to describe a mixed-valence iron compound named ferrosic hydroxide. [25, 26, 31] It is variable in color ranging from yellow to olive green to green-blue in color[25, 31, 32] and is a major constituent in reduced iron-rich carbonate-poor soils. [26, 33] Ferrosic hydroxide is believed to be the unstable precursor to magnetite.  Ferrosic hydroxide belongs to a variable and wide range of mixed valence compounds named green rusts for which general compositions have been proposed which vary from Fe2(OH)5 (ref. ) to (Fe11(1 - x)Fe111 x -(OH)2)x+ (x/nAn- m/nH2O)x-, (ref. ) where A can be the anions OH-, Cl-, CO3 2- or SO4 2-.
At Franklin Seamount, the dominance of amorphous iron oxyhydroxide was demonstrated by XRD and electron diffraction combined with bulk chemical and spot EDS analyses.  Knowledge of the composition of the vent fluid at Franklin Seamount (Table 1, ref. ) provides an opportunity to place constraints on the physico-chemical environment of the iron precipitation assuming the fluid and the minerals are in equilibrium.
Gibbs free energies of low temperature iron and silica oxyhydroxides in the system Fe–Si–O–H at 25°C and 1 bar
Sadiq and Lindsay, 1979 (ref. 39) kcal mole-1
Ponamperuma et al., 1967 (ref 25) kcal mole -1
Langmuir, 1969 (ref. 360) kcal mole-1
Winters and Buckley, 1986 (ref. 43) kcal mole-1
SUPCRT92, Johnson et al., 1991 (ref. 19) kcal mole -1
Fe(OH)3 (s) soil amorphous ferric iron
Fe(OH)3 (s) aged amorphous ferric iron
Fe(OH)3 (s) 4 day old amorphous ferric iron
Fe(OH)3 (s) freshly precipitated amorphous ferric iron
Fe3(OH)8 (s) freshly precipitated amorphous mixed-valence iron
-451.2 (nature uncertain)
-202.89 (SiO2- nH20)
-312.6 (SiO2 [aq)]
Reactions used to model the precipitation of low temperature iron and silica oxyhydroxides in the system Fe–Si–O–H shown in Fig. 7
Fe (OH)3 (fresh ferric hydroxide) (s) + 2H+ =
Fe2+ + 5/2 H2O + 1/4O2
Fe3(OH)8 (fresh ferrosic hydroxide) + 6H+ =
3Fe2+ + 7H2O + 1/2O2
3Fe(OH)3 (fresh ferric hydroxide) =
Fe3(OH)8 (fresh ferrosic hydroxide) + 1/2H2O + 1/4O2
Fe3(OH)8 (fresh ferrosic hydroxide) =
3Fe(OH)2 (fresh ferrous hydroxide) + H2O + 1/2O2
Fe(OH)2 (fresh ferrous hydroxide) + 2H+ = Fe2+ + 2H2O
SiO2 (amorphous) + 2H2O = Si(OH)4
FeSiO3 (ferrosilite) + 3H2O = Fe(OH)2 (fresh ferrous hydroxide) +
FeSiO3 (ferrosilite) + 10H2O + 1/2O2 =
Fe3(OH)8 (fresh ferrosic hydroxide) + 3Si(OH)4
FeSiO3 (ferrosilite) + H2O + 2H+ = Fe2+ + Si(OH)4
When choosing the appropriate thermodynamic parameters for the amorphous iron oxyhydroxides at Franklin Seamount, it should be noted that these phases are actively precipitating from hydrothermal fluids and thus are very fresh when initially deposited. Accordingly, the free energy values chosen to model the formation of ferrosic hydroxide (Table 2) were those obtained from the laboratory experiments of Arden, as these conditions are most similar to the vent conditions on the seafloor. The solubility product for this fresh ferrosic hydroxide was obtained by potentiometric titration. The phase was precipitated at room temperature from an initial ferrous iron solution under rising pH, between 6.4–6.8, with the addition of a ferric sulphate solution. Hansen et al.  repeated the experiment, obtained a similar titration curve and the material formed was identified as sulphate-interlayed green rust. Frederickson et al.  concluded that the optimal pH range for the development of green rust is between 6.5 to 7.5. These conditions are similar to those in the low temperature vent fluid at Franklin Seamount so this value is incorporated in the thermodynamic database for soil phases given in Table 2 by Sadiq and Lindsay.  Free energy values for ferric hydroxide Fe(OH)3 in the Lindsay database, such as those of Schindler et al.  and Sadiq and Lindsay were not considered because these were obtained on aged material whose conditions of formation are far removed from the vent conditions at Franklin Seamount.
Fig. 6 demonstrates that the fresher the Fe(OH)3 in equilibrium with fresh Fe3(OH)8, the higher the f(O2) of the boundary between the two compounds. Since the free energy of amorphous materials has a negative correlation with grain size and because freshly precipitated primitive crystallites agglomerate together and grow in size with aging, it would be expected that the material's free energy would decrease as it becomes older. The free energy of formation provided by Langmuir  for Fe(OH)3 in Table 2 was obtained from solubility experiments conducted on a freshly precipitated phase and it has the least negative free energy among the Fe(OH)3 compounds shown. For this reason, this value best matches the precipitation of amorphous ferric oxyhydroxides at Franklin Seamount. Dzombak and Morel reported that freshly precipitated hydrous ferric oxyhydroxides are made up of spherical particles 10–100 Å in size, similar to samples from the actively precipitating vents at Franklin Seamount described by Boyd and Scott. 
In summary, the free energy database of Sadiq and Lindsay, excepting the value for fresh Fe(OH)3 from Langmuir substituting for the value of the 4 day old material, is used here to model the mineral equilibria of amorphous iron oxyhydroxides at an actively venting chimney at Franklin Seamount as shown in Table 3.
Silicon makes up on average 12.2 wt.% of the bulk samples and 7.0 wt.% of ferrihydrite from Franklin Seamount (the content of the iron end-member sample, M2192-loc. 1 106848, Boyd and Scott 1999, ref. ) so the element must be incorporated into the thermodynamic model of the vent sites. Based on XRD patterns of all the collected samples, excepting two, discrete silica mineralization of hydrothermal origin appears to be minor. However, as a caution Cremer found for the oxyhydroxide deposits at Loihi Seamount that the XRD response to amorphous silica is commonly masked by the iron oxyhydroxide. In the two non-conforming samples from Franklin Seamount, amorphous silica mantles iron minerals having filamentous textures (Fig. 3b) in a manner similar to that described by Juniper and Fouquet for samples from Explorer Ridge and the East Pacific Rise. The dynamic depositional environment and low temperature of the vent fluids at Franklin Seamount promote the precipitation of unstable amorphous silica rather than quartz in a similar fashion to the behavior of iron.
In general, the relative scarcity of amorphous silica phases at Franklin Seamount can be explained by the silicon content of the vent fluid (Table 1), which is calculated to be under-saturated with respect to amorphous silica by a factor of 5 at a temperature of 25°C. The presence of nontronite in the samples at Franklin Seamount, however, suggests that the silicon in the fluid does exert some control on the mineralogy of the deposits. Thermodynamic data for the phase ferrosilite (FeSiO3) in the Winters and Buckley compilation (originally from Helgeson et al.  in Table 2 is used to represent nontronite. This is a reasonable substitute provided the iron in nontronite is initially ferrous. Harder synthesized a ferrous trioctahedral smectite precursor to nontronite under Eh-pH conditions similar to those for which ferrosilite was expected, but was not successful in precipitating lembergite at higher Eh or lower pH.
Oxygen and hydrogen
The f(O2) of the vent fluid is not known but is believed to be much lower than that of seawater (0.06 atm at 2000 m depth).  End-member hydrothermal vent fluids at >300°C are extremely acidic before mixing with seawater. [46, 47] As the fluid cools, whether by mixing with seawater or conduction, the pH steadily increases and element concentrations decrease with the precipitation of phases.  Hannington and Scott used mineral equilibria to model the decrease in log f(O2) from -32 to -43 as the fluid cooled from 350 to 180°C at 21°N East Pacific Rise and Axial Seamount. A strong redox buffering capacity between the H2S in the vent fluid and SO4 in seawater was invoked to explain the down-temperature decrease in f(O2) with the increased mixing of the fluid with the oxygenated bottom seawater. The authors suggested that below 180°C, as the H2S content of the fluid dropped with the precipitation of sulfides, the redox buffer broke down.
There are, however, other possible redox buffers which could become important. Reaction between Fe2+ in the fluid and the precipitated iron phases would cause the oxygen fugacity of the evolving vent fluid to continue to fall with increased mixing. The equations in Table 3 demonstrate that for a fluid precipitating an iron phase, such as shown by the univariant boundaries in Fig. 6, a rise in pH due to mixing with seawater is accompanied by a concurrent drop in f(O2). The fluid would be held or buffered to that univariant line providing the Fe2+ is maintained in or close to mineral equilibria with the precipitating phases. These mineral equilibria would be maintained as long as the active vent was constantly replenishing ferrous iron to the system.
There have been no direct measurements of oxygen or Eh of vent fluids on the seafloor. However, it is likely that vent fluids at Franklin Seamount are considerably more reduced than seawater despite possessing no H2S and being more than 90% diluted by seawater. Bowers et al.  thermodynamically modeled the cooling of end-member hydrothermal fluids by mixing with seawater and found that log f(O2) steadily falls to below -70 at 25°C. The f(O2) then climbs sharply back up in response to the ambient seawater flooding the system. The calculations indicate that all the sulfides are precipitated between 300 and 150°C and yet the f(O2) continues to drop at temperatures below 150°C. Bowers et al.  analysed the composition of high temperature vent fluids obtained from 11–13°N and 21°N and found that a 50% decrease in iron in solution accompanied by a pH rise can be accounted for by a 15°C drop in temperature and the buffering of the solution by greenschist-facies mineral assemblages. The authors found that vent fluid compositions at 21°N were uniform with respect to time, based upon expeditions in 1979, 1981 and 1985, and concluded that the compositions of vent fluids and especially the iron are controlled by equilibria with solid phases.
In conclusion, the low temperature redox conditions at Franklin Seamount are consistent with results of studies of higher temperature seafloor hydrothermal systems. These results support the contention that iron participates in the redox balance between the vent fluid and its precipitated products, and are consistent with iron phases commonly being the dominant mineralization in both high and low temperature modern hydrothermal deposits.
Carbon and sulfur
No analyses of carbon in the vent fluid are available from Franklin Seamount, however, the pH drifted from 6.1 to 6.26 when exposed to the atmosphere indicating probable exsolution of CO2 from the fluid.  Based on the estimate that P(CO2) of surface seawater in equilibrium with the atmosphere is 3.3 × 10-4 bar, then doubling the P(CO2) will lower the pH by 0.28 units.  A drift of 0.16 pH units therefore is consistent with an estimated P(CO2) of 5.2 × 10-4 bar for the vent fluid providing its overall composition is not considerably different from seawater, as is the case (Table 1). A P(CO2) of at least 10-2 bar is required before iron carbonates such as siderite will start to precipitate in the hydrothermal system at Franklin Seamount. This is supported by the SEM and TEM examination of the samples that showed an absence of any hydrothermal carbonate minerals.
No H2S was detected in the vent fluid so sulfur was not incorporated into the thermodynamic calculations. The low level of sulfur in the system is consistent with the absence of hydrothermal sulfur bearing minerals in the samples.
Kinetic constraints on the hydrothermal precipitation of iron have been invoked by many researchers in proposing microbial mediation as an alternative explanation for the formation of voluminous iron oxyhydroxides on the seafloor. [10, 21] The rate of oxidation of ferrous iron in low temperature hydrothermal solutions is very slow. For example, at pH = 5 and P(O2) = 0.06 bar (2000 m depth in seawater), the half-life for the oxidation of Fe2+ to Fe3+ is 30 years.  The ferrous iron oxidation rate constant (k) in seawater, determined by Millero et al., as a function of temperature (T/K) and ionic strength (I) is:
log k = 21.56 - 1545/T - 3. 291(I) 1/2 + 1.52(I) (1)
Eqn. (1) is incorporated into an equation used to calculate the oxidation rate of iron as a function of P(O2), pH and the concentration of Fe2+ in the fluid:
- d[Fe2+]/dt = k[Fe2+][O2][OH-]2 (2)
The activity coefficient of H2O in seawater at 25°C and less than 1 kbar pressure is 0.98, the difference from unity being a function of ionic strength, so for the purposes of these calculations fugacity and activity are assumed to equal partial pressure and concentration, respectively.
The oxidation rate is extremely sensitive to changes in pH. From eqn. (2), the half-life for the oxidation of ferrous iron is calculated to be 44 min for the pH, temperature and iron concentration of the measured vent fluid at Franklin Seamount (Table 1) if that fluid had an oxygen content equal to that of surrounding seawater with P(O2) of 0.06 bar. This assumes the iron in the fluid is all Fe2+. The half-life decreases to 2.3 min for the pH (7.6) of the bottom water in Woodlark Basin (Table 1). Even at these accelerated rates of oxidation, however, almost all of the iron would be dispersed in the water column by the time the oxidation reactions were completed. Voluminous ferric oxyhydroxides dispersed in plumes have been found above areas of active hydrothermal deposition supporting the notion that most of the vented iron is lost to the seawater column.
Submersible observations during the sampling of the vent fluid at Franklin Seamount suggest that the fluid was exiting at a rate approximately 0.11 s-1 (ref. ). This is calculated from an estimated rate of emission of 5 cm s-1 from an orifice approximately 5 cm in diameter located on an oxyhydroxide mound at the base of a meter high spire. Based on the calculated oxidation rate of iron for bottom seawater at a pH of 6.26 and assuming that only the iron oxidized in the first 20 s (the approximate length of time a fluid is within a 1 m high chimney) is precipitated, then only 0.4 wt.% of the iron in the vent fluid would be accumulating within and on the chimneys and mounds. The rest would still be dissolved in the fluid and thus be dispersed by the ocean currents. At these discharge and oxidization rates, about 26 g of iron would be deposited around that single orifice in one year.
This amount is compared to the calculated oxyhydroxide accumulation rates at Loihi Seamount based upon radio-chemical dating reported in Cremer.  The average iron accumulation rate at the hydrothermally active Peles Vent area is 9.9 g cm-2 kyr-1 and at the less vigorously venting 1000 Fingers Field is 0.6 g cm-2 kyr. A marker, recovered in the Peles Vent area after six months deployment, was found to have accumulated iron at a rate of 23 g cm-2 kvr-1. 
Assuming the precipitates from that single vent at Franklin Seamount cover an area of one square meter, based on submersible observations of the chimneys, the rate of precipitation is too low by about an order of magnitude when compared to the iron accumulation at Peles Vent, but five times higher than at 1000 Fingers.
Other actively venting orifices were seen in the same oxyhydroxide mound and slowly emitting water was observed from numerous smaller crevices indicating that the amount of emitted fluid associated with the building of the spire and mound was probably considerably greater than that used in the calculation. Nevertheless, the presence of the large oxyhydroxide deposits at Franklin Seamount suggests that iron is being precipitated in the vent fluid at a much faster rate than that indicated by the kinetic equations. This could occur through: (1) passive or active microbial mediation overcoming the kinetic barriers to ferrous iron oxidation as suggested by previous investigators (e.g., refs. [10, 16] and ); or (2) by initially precipitated iron acting as a catalyst for the accelerated auto-catalytic hydrothermal deposition of voluminous iron oxyhydroxides. The initial precipitates occurring as mixed-valence ferrosic compounds in the latter process facilitate the decrease in the amount of ferrous iron required to be oxidized to complete the reaction.
Yariv and Cross state that the oxidation of an element is catalyzed by the presence, in suspension of colloidal materials, of that same element, and that the surface of a precipitated element will behave as a seed for additional deposition. This auto-catalytic precipitation will occur at a lower supersatura-tion ratio than that for the element in isolation. As previously mentioned, scanning transmission electron microscope images of amorphous iron oxyhydroxide samples from Franklin Seamount show agglomerated crystallites of < 100 Å diameter at high magnification which suggests that the drawn vent fluid sample contained numerous fine colloidal particles of iron. These particles would be highly reactive to hydrothermal chemical processes.
In summary, kinetic inhibitions are not a major barrier to the initial abiotic chemical oxidation and precipitation of iron at Franklin Seamount. Although the calculated rate of iron oxidation is somewhat too low to explain the large size of the deposits, this rate could be accelerated by auto-catalytic reactions and/or the deposition of mixed valence compounds, as well as by microbial mediation. The predominance of formless textures with no associated bacterial forms in some samples gathered from actively venting chimneys suggests that most of the initial precipitation could be abiotic, however an explanation is required for the dominance of biotic textures in other samples. Nevertheless, calculations show that the kinetic barriers are minimal enough to allow for the formation of seed crystallites that would act as nuclei for the more efficient auto-catalytic reactions to follow and investigation into the kinetic and thermodynamic conditions at the vent sites at Franklin Seamount permit the possibility that microbial processes are not necessary for the oxidation of ferrous iron in the fluid. This legitimizes the examination of hydrothermal explanations for the precipitation of the iron.
Chemical conditions of formation
Genin et al.  constructed similar models using thermodynamic data for various types of green rusts, identified as GR1 and GR2, such as Cl-bearing GR1 (Fe4(OH)8Cl), CO3-bearing GR1 (Fe6(OH)12CO3) and SO4-bearing GR2 (Fe6(OH)12SO4) in equilibrium with lepidocrocite or goethite and Fe2+. They obtained comparable results to this paper when examined with respect to the iron content in the vent fluid at Franklin Seamount (3.9 × 10-5 m). The ferric and ferrosic oxyhydroxides, Fe2+ triple point varies from pH of 7.8 and log f(O2) of -59 for Fe4(OH)8Cl, to a pH of 8.2 and log f(O2) of -64 for Fe6(OH)12CO3, and to a pH of 8.5 and log f(O2) of -70 for Fe6(OH)12SO4. The lower f(O2) and higher pH values in comparison to the results obtained in this paper are mostly due to the choice by Genin et al. of well ordered ferric oxyhydroxide minerals for their model which are not found at Franklin Seamount.  This is consistent with the aforementioned observed trend in Fig. 6 of lower f(O2) and higher pH with greater ferric iron oxyhydroxide crystallinity. It is probable, however, that the true composition of ferrosic hydroxide at Franklin Seamount is closer to that of the Cl-bearing than the SO4- or CO3-bearing varieties of green rusts because the former is in much higher concentration in seawater than the latter.
Although Si(OH)4 in the fluid was calculated to be under-saturated with respect to amorphous silica at the sampled vent site, Fig. 7 shows that silica can precipitate as FeSiO3 at a pH higher than 7.7 and lower f(O2) than for Fe3(OH)8. This would occur with increased seawater dilution of the fluid providing the redox balance between Fe2+ and the solid phases is maintained. Such an explanation is consistent with the relative rarity of hydrothermal Fe–Si smectites as opposed to amorphous iron oxyhydroxides in active vents since most of the time the seawater would flood the system and break down the equilibria before the fluid became very reduced.
The initial abiotic deposition of ferric and ferrosic hydroxides would accelerate the precipitation of the same resulting in a greater accumulation of iron than the 26 g yr-1 previously calculated. Tunnicliffe and Fontaine found much of the iron oxyhydroxides at the southern Juan de Fuca vent field were deposited non-specifically as orbs and formless masses suggesting that the oxidation of metals is auto-catalytic.
An understanding of the precipitation of the iron in low temperature systems, however, must account for the evidence of microbial activity at Franklin Seamount and other seafloor oxyhydroxide deposits. It is suggested here that the initially deposited ferrosic hydroxide and ferrous trioctahedral smectite would immobilize the ferrous iron into colloidal particles and thus provide a favorable ferrous substrate for the subsequent growth of iron oxidizing bacteria such as Leptothrix. Most of the filamentous textures observed in the oxyhydroxides probably formed in this fashion. This interpretation is consistent with the dominance of formless iron agglomerates in samples from some of the most active vents and the observation of filaments emanating from the agglomerates (Fig. 3f,g).
The filamentous textures in most samples taken from inactive vents appear very uncontaminated, that is, lacking large amounts of additional deposition of iron on their walls (Figs. 3a,c,d,e,f,g, 4c,d,e). This suggests that the paragenesis of the filaments is relatively late. Additional iron encrustations on sheaths may fill spaces between filaments and eventually coalesce to form irregular iron oxyhydroxide spheres but this texture is uncommon at Franklin Seamount. Difficulties in the identification of filamentous textures arise due to their degradation (Fig. 3h), rather than due to additional iron deposition obscuring the shapes.
This explanation invokes a mostly diagenetic role for the bacteria in the formation of the preserved ferric oxyhydroxides. The ferrosic hydroxides deposited within the relatively aerobic environment of the seawater would also be undergoing abiotic oxidation and transformation to ferric phases. The presence of ferrosic hydroxide on the seafloor is consistent with the observation of the yellowish actively forming deposits at Franklin Seamount. The change to a patchy orange-red coloration in some in situ chimneys on the seafloor is indicative that this transformation, whether microbial or abiotic driven, is occurring rapidly after deposition. Indications of the presence of ferrosic hydroxides therefore would only be found in samples from the most hydrothermally active areas. Iron oxyhydroxide samples obtained from older seafloor deposits would be dominated by filaments. The few hours it took for the gathered samples to darken and turn red on the ship's deck are consistent with oxidation rates of ferrous iron at an atmospheric oxygen concentration and neutral pH. 
Comparisons can be made to investigations into mixed valence hydroxides in soil environments. Ponnamperuma et al.25 stated that reduced soils which are high in iron and low in both sulfur and organic matter have a grey to green color similar to that of ferrosic hydroxide. Trolard et al.  reported that a waterlogged soil containing green rust once exposed to air was observed to change color rapidly over a number of stages from bluish-grey to greenish-grey to olive to grey over one day. Lindsay and Sadiq and Genin concluded, based on their own experiments and others studies, that mixed-valence iron hydroxide acts as a control on many aqueous systems even though the compound is thermodynamically unstable and very reactive in ambient conditions.
Iron oxides in other settings
Other seafloor deposits
At sites dominated by the active deposition of amorphous iron oxyhydroxides, such as at Franklin Seamount, Loihi Seamount and Galapagos, the agreement between the measured and calculated pH is good, suggesting that the iron in the vent fluid is in equilibrium with the triple point separating the Fe2+ and the solid phases. In contrast, there is little coincidence between the measured and calculated pH at Kasuga Seamount, Guaymas Basin and one of the sites at 21°N suggesting that the iron is not in equilibrium here. For example, the deposits at Kasuga Seamount have considerable elemental sulfur and the fluids contain H2S (ref. ); at Guaymas Basin the deposits contain voluminous hydrothermal carbonate and the fluids are very alkaline.  The Fe–O–H buffer of the pH and f(O2) at the vent site appears to be operative only in the absence of H2S and CO2. Fig. 9 suggests that the processes described for Franklin Seamount and in soils are occurring at those other seafloor deposits that are dominated by iron oxyhydroxides.
Hematite forms from the slow dehydration or thermal transformation of ferrihydrite.  Carlson and Schwertmann found that this transformation is inhibited by the incorporation of silicon into the material. The amorphous iron oxyhydroxides from Franklin Seamount contain considerable amounts of silicon intimately associated with the iron, so it would be expected that the transformation to magnetite from ferrosic hydroxides would occur much more rapidly than the formation of hematite from ferrihydrite. This is supported by the near absence of preserved ferrosic hydroxide in nature in contrast with the widespread occurrence of ferrihydrite and magnetite.
Schwab and Lindsay determined that Fe(OH)3 (ferrihydrite) and magnetite together are more stable relative to Fe3(OH)8, so the former two phases should replace the latter. The result is that magnetite in iron formation is probably not in equilibrium with hematite, but rather with its precursor Fe(OH)3. The phase boundary between hematite and magnetite (dashed line in Fig. 10) is at such a low f(O2) that the latter's stability field is usurped by iron silicates. The boundary between goethite and magnetite is similarly at a very low f(O2). . Therefore, goethite or hematite can precipitate with or replace magnetite only at very low Si concentration in an extremely reduced environment, so it would be expected that the occurrence of magnetite would be rare in iron formation if this were its means of formation. However, as magnetite is a major constituent of banded iron formation these conditions for replacement must not have prevailed.
As shown in Fig. 8, hematite originates from ferrihydrite formed as a by-product to the crystallization of magnetite, and/or due to the microbial or hydrothermal oxidation of ferrosic hydroxides and/or precipitated directly from hydrothermal solutions under aerobic conditions. Klein and Bricker noted that the calculated Eh–pH equilibria for magnetite could be too wide due to a lack of thermodynamic data on its precursor. However, the results of this investigation suggest that the authors successfully modeled the early diagenetic mineral assemblages of iron formation with the ferric hydroxides forming in equilibrium with magnetite.
The evidence that ferrosic hydroxide and ferrous trioctahedral smectite are precipitating directly on the seafloor provides an insight into the mineral assemblages of Algoma-type Archean banded iron formation (BIF). Magnetite in BIF could be derived from ferric iron reducing bacteria; however, a suboxic to anoxic seafloor environment, combined with a paucity of microbial activity would also preserve magnetite and iron silicates such as greenalite. An increase in f(O2), and/or microbial activity, would result in the dominance of hematite consistent with that found in ironstones of Cenozoic and Mesozoic age and iron exhalites associated with massive sulfides such as "tetsusekiei" flanking and overlying Kuroko massive sulfide deposits in Japan.  The above explanation is consistent with both the gradual oxygenation of the atmosphere and the evolution of the earth's biosphere since the Archean. According to Klein the average chemical compositions of BIF from 3.8 to 1.8 Ga (billion years) are very similar with a large amount of the iron occurring as Fe2+ while 95% of the total iron in Phanerozoic BIF, deposited between 0.8 to 0.6 Ga, is Fe3+.
An understanding of the role of iron bacteria in modern vents has direct bearing on the interpretation of their fossils in ancient rocks. Duhig et al.  describe the preservation of abundant microbial fossils and iron agglomerates in unmetamorphosed Cambrian silica–iron exhalites lateral to a massive sulfide deposit. The authors suggest that iron oxidizing bacteria mediated the deposition of the iron by catalyzing the oxidation of the Fe2+ in the fluid to Fe3+. Iron mineralization bound within and on bacterial cell fossils have been detected in 2.0 Ga red chert from the Gunflint Formation.  Sub-greenschist facies ironstone pods and BIF in the Archean Barberton greenstone belt are dominated by ferric oxides, but also contain early magnetite and indications that hematite and goethite pseudomorphed euhedral magnetite.  Delicate features suggestive of relict hydrothermal discharge such as chimney structures, honeycomb-like cavities and fluid-flow channels were identified in the well preserved Barberton rocks, but petrographic studies found no indication of microfossils. Fossils of filament-forming microbes up to 3.5 billion years old have been reported, although little is known how common their occurrence was during the Archean.
Previous studies have proposed that the amorphous iron oxyhydroxides were precipitated, directly or indirectly, due to microbial activity and suggest this may have played an important role in the formation of BIF. However, our investigation cautions that microbial micro-textures in ancient BIF cannnot be assumed to be primary. Instead, they could have formed by early diagenetic reactions similar to those in the oxyhydroxide deposits at Franklin Seamount.
Amorphous iron oxyhydroxides gathered from dormant and actively venting chimneys on the seafloor at Franklin Seamount contain volumetrically significant filamentous microbial features, although apparently non-bacterial agglomerates are also common. Spatial relationships between the two micro-textures suggest that the iron-microbe filaments are either forming subsequent to or together with the agglomerates.
The f(O2) of low temperature vent fluids emanating from hydrothermally active chimneys at Franklin Seamount may be much lower than the surrounding seawater. This is based on the in situ observation that yellow mixed-valence ferrosic hydroxide [Fe3(OH)8], red–orange ferric hydroxide [Fe(OH)3] and light green ferrous trioctahedral smectite appear to be precipitating on the surface of active chimneys coincident with the observation in the samples of fossils of Leptothrix and Gallionella, which prefer low f(O2) habitats. These observations are consistent with investigations into the thermodynamics of low temperature iron systems which show that, with increased cooling by mixing with seawater, the f(O2) of the fluid will drop to extremely low levels. In addition, the measured pH of a vent fluid sample (6.26) obtained from a chimney is similar to the pH of the triple point for Fe2+, Fe3(OH)8 and Fe(OH)3 which is calculated to occur at a log f(O2) of -44. Consideration of the thermodynamics and kinetics of iron in the vent fluid suggests that large amounts of amorphous iron oxyhydroxides are capable of precipitating by a combination of abiotic hydrothermal processes. Microbial mediation, however, possibly played a diagenetic role in transforming ferrosic hydroxides to ferric hydroxides resulting in older chimneys being dominated by filamentous textures.
Comparisons with experiments conducted on iron-rich soils and analyses of fluids gathered from actively venting oxyhydroxide chimneys at other seafloor sites provide supporting evidence of the importance of iron species and phases in the redox equilibria of low temperature iron systems. Comparisons with thermodynamic calculations of mineral equilibria in ancient iron formation suggest that the processes which are forming seafloor oxyhydroxide deposits today can be applied to understanding the origin of ancient BIF. Abundant magnetite and a relative paucity of microfossils in Archean iron formation are consistent with the preservation of the primary anoxic depositional environment. In contrast, hematite and abundant microfossils in Phanerozoic BIF are primarily diagenetic in origin reflecting their aerobic and microbial-rich surroundings that resulted in the oxidation of the initially precipitated ferrosic hydroxides.
Future work is needed to confirm the presence of ferrosic hydroxides or natural green rusts in actively venting low temperature sulfur-free springs by collecting samples of the associated iron hydroxide material in anaerobic chambers.
Samples from Franklin Seamount were obtained by the submersible supported Soviet Union–Papua New Guinea–Australia–Canada (SUPACLARK) expedition. We thank our numerous colleagues who assisted with the expedition and subsequent laboratory research. Ray Binns is thanked for his detailed submersible observations. Grant Ferris and Greg Anderson provided guidance in many aspects of the micro biological and geochemical research, respectively. The research was supported by grants to Scott from the Natural Sciences and Engineering Research Council of Canada and Bank of Nova Scotia.
- Rona PA, Scott SD: Econ Geol. 1993, 88-Google Scholar
- Hekinian R, Hoffard M, Larque P, Cheminee JL, Stoffers P, Bideau D: Econ Geol. 1993, 88-Google Scholar
- Boyd T, Scott SD, Hekinian R: Resource Geol Special Iss. 1993, 17-Google Scholar
- Lisitsin A, Binns RA, A Yu, Bogdanov SD, Scott LP, Zonenshayn VV, Gordeyev , Ye G, Gurvich KG, Murav'yev , Serova VV: Int Geol Rev. 1991, 33-Google Scholar
- Binns RA, Scott SD, Bogdanov YA, Lisitsin AP, Gordeev VV, Gurvich EG, Finlayson EJ, Boyd T, Dotter LE, Wheller GE, Muravyev KG: Econ Geol. 1993, 88-Google Scholar
- Benes V, Scott SD, Binns RA: J Geophys Res. 1994, 99-Google Scholar
- Taylor B, Goodliffe A, Martinez F, Hey R: Nature. 1995, 374-Google Scholar
- Boyd T, Scott SD: Can Mineral. 1999, 37-Google Scholar
- Juniper SK, Fouquet Y: Can Mineral. 1988, 26-Google Scholar
- Alt JC: Mar Geol. 1988, 81-Google Scholar
- Fortin D, Ferris FG, Scott SD: Am Mineral. 1998, 83-Google Scholar
- Bigham JM, Schwertmann U, Carlson L: Biomineralization Processes of Iron and Manganese-Modern and Ancient Environments. Edited by: Skinner HCW, Fitzpatrick RW. 1992, CATENA, 219-Supplement 21Google Scholar
- Ferris FG, Konhauser KO, Lyven B, Pedersen K: Geomicrobiol J. 1999, 16-Google Scholar
- Ferris FG, Beveridge TJ, Fyfe WS: Nature. 1986, 320-Google Scholar
- Fortin D, Ferris FG: Geomicrobiology. 1998, 15-Google Scholar
- Ferris FG: Microbial Sediments. Edited by: Riding RE, Awramik SM. 2000, Springer-Verlag, Berlin Heidelberg, 121-View ArticleGoogle Scholar
- Stumm W, Morgan JJ: Aquatic Chemistry. 1996, John Wiley, New York, 3Google Scholar
- Scott SD, Binns RA: Hydrothermal Vents and Processes. Edited by: Parson LM, Walker CL, Dixon D. 1995, Geol Soc London Spec Publ, 187: 191-Google Scholar
- Johnson JW, Oeikers EH, Helgeson HC: SUPCRIT92, a software package for calculating the standard molal thermodynamic properties of minerals, gases, aqueous species and reactions from 1 to 5000 bars and 0 to 1000°C, Earth Sciences Department, Lawrence Livermore National Laboratory. 1991Google Scholar
- Decarreau A, Bonnin D: Clay Miner. 1991, 21-Google Scholar
- Lundgren DG, Dean W: Biogeochemical Cycling of Mineral-Forming Elements. Edited by: Trudinger PA, Swaine DJ. 1979, Elsevier. Amsterdam, 211-View ArticleGoogle Scholar
- Mulder EG, Deinema MH: The Prokaryotes: a Handbook on Habitats, Isolation and Identification of Bacteria. Edited by: Starr MP, Stolp HG, Truper HG, Balows A, Schlegel HG. 1981, Springer-Verlag, New York, 425-View ArticleGoogle Scholar
- Hanert HH: The Prokaryotes: a Handbook on Habitats, Isolation and Identification of Bacteria. Edited by: Starr MP, Stolp HG, Truper HG, Balows A, Schlegel HG. 1981, Springer-Verlag, New York, 509-View ArticleGoogle Scholar
- Lindsay WL: Chemical Equilibria in Soils. 1979, John Wiley & Sons, New YorkGoogle Scholar
- Ponnamperuma FN, Tianco EM, Loy T: Soil Sci. 1967, 103-Google Scholar
- Schwab AP, Lindsay WL: Soil Sci Soc Am J. 1983, 47-Google Scholar
- Schwertmann U, Cornell RM: Iron Oxyhydroxides in the Laboratory Preparation and Characterization. 1991, VCH Publishers, Inc., New YorkGoogle Scholar
- Towe KM, Bradley WF: J Colloid Interface Sci. 1967, 24-Google Scholar
- Chukhrov FW, Zvyagin BB, Ermilova LP, Gorshov AI: New data on Fe-silica oxyhydroxides in the weathering zone. Proc Int Clay Conf 1970. Edited by: Serratosa JM. 1973, Div. de Ciencias C.S.I.C., MadridGoogle Scholar
- Eggleton R, Fitzpatrick RW: Clays Clay Miner. 1988, 36-Google Scholar
- Arden TV: J Chem Soc. 1950, 53-Google Scholar
- Trolard F, Genin JMR, Abdelmoula M, Bourrie G, Humbert B, Herbillon A: Geochim Cosmochim Acta. 1997, 61-Google Scholar
- Thind HS, Chahal DS: Agricult Sci Soc Cambridge. 1983, 101-Google Scholar
- Genin JMR, Bourrie G, Trolard F, Abdelmoula M, Refait P, Jaffrezic A, Maitre V, Humbert B, Herbillon A: Environ Sci Technol. 1998, 132-Google Scholar
- Helgeson HC, Delany JM, Nesbitt HW, Bird DK: Am J Sci. 1978, 278-A-Google Scholar
- Langmuir D: US Geol Surv Prof Pap. 1969, 650-B-Google Scholar
- Hansen HCB, Borggaard OK, Sørensen J: Geochim Cosmochim Acta. 1994, 58-Google Scholar
- Fredrickson JK, Zachara JM, Kennedy DW, Dong H, Onstott TC, Hinman NW, Shu-Mei L: Geochim Cosmochim Acta. 1998, 62-Google Scholar
- Sadiq M, Lindsay WL: Colorado State Univ Tech Bull. 1979, 134-Google Scholar
- von Schindler PN, Michaelis W, Feitknecht G: Helvetica Chim Acta. 1963, 46-Google Scholar
- Dzombak DA, Morel FM: Surface Complexation Modeling Hydrous Ferric Oxyhydroxide. 1990, John Wiley & Sons, New YorkGoogle Scholar
- Cremer MD: Geochemistry of Hydrothermal Deposits from the Summit Region of Loihi Seamount. 1994, Hawaii, Unpublished MSc Thesis, University of Hawaii, Hawaii, USAGoogle Scholar
- Winters GV, Buckley DE: Geochim Cosmochim Acta. 1986, 50-Google Scholar
- Harder H: Chem Geol. 1976, 18-Google Scholar
- Kester DR: Chemical Oceanography. Edited by: Riley JP, Skirrow G. 1975, Academic Press, London, 498-Google Scholar
- von Damm KL: Annu Rev Earth Planet Sci. 1990, 18-Google Scholar
- Hannington MD, Herzig PM, Scott SD: Gold Metallogeny and Exploration. Edited by: Foster RP. 1991, Blackie, London, 249-View ArticleGoogle Scholar
- Bowers TS, Von Damm KL, Edmond JM: Geochim Cosmochim Acta. 1985, 49-Google Scholar
- Hannington MD, Scott SD: Can Mineral. 1988, 26-Google Scholar
- Bowers TS, Campbell AC, Measures CI, Spivack AJ, Khadam M, Edmond JM: J Geophys Res. 1988, B93-Google Scholar
- Stumm W, Morgan JJ: Aquatic Chemistry: an Introduction Emphasizing Chemical Equilibria in Natural Waters. 1981, John Wiley & Sons, New York, 2Google Scholar
- Millero FJ, Sotolongo S, Izaguirre M: Geochim Cosmochim Acta. 1987, 51-Google Scholar
- Coale KH, Chin CS, Massoth GJ, Johnson KS, Baker ET: Nature. 1991, 352-Google Scholar
- Binns RA: Report on SUPACLARK Dive 7 on Mir-2 Submersible: Franklin Seamount, Woodlark Basin PNG, CSIRO Division of Exploration Geoscience Restricted Report 140R, Australia. 1990Google Scholar
- Skinner HCW, Fitzpatrick RW: Biomineralization Processes of Iron and Manganese-Modern and Ancient Environments. Edited by: Skinner HCW, Fitzpatrick RW. 1992, CATENA, 1-Supplement 21Google Scholar
- Yariv S, Cross H: Geochem Colloid Syst. 1979, Springer-Verlag, New YorkView ArticleGoogle Scholar
- Tunnicliffe V, Fontaine AR: J Geophys Res. 1987, 92B-Google Scholar
- Davidson W, Seed G: Geochim Cosmochim Acta. 1983, 47-Google Scholar
- Lindsay WL, Sadiq M: Sci Total Environ. 1983, 28-Google Scholar
- Karl DM, McMurtry GM, Malahoff A, Garcia MO: Nature. 1988, 335-Google Scholar
- McMurtry GM, Sedgewick PN, Fryer P, Vonderhaar DL, Yeh HW: Earth Planet Sci Lett. 1993, 114-Google Scholar
- von Damm KL: Chemistry of submarine hydrothermal solutions at 21°N, East Pacific Rise and Guaymas Basin, Gulf of California. 1983, Unpublished PhD Thesis, Woods Hole, Mass., USA, Woods Hole Oceanographic Institution-Massachusetts Institute of TechnologyGoogle Scholar
- Peter JM, Scott SD: Can Mineral. 1988, 26-Google Scholar
- Klein C, Bricker OP: Econ Geol. 1977, 72-Google Scholar
- Gross GA: Canadian Mineral Deposit Types: A Geological Synopsis. Edited by: Eckstrand OR. 1984, Geological Survey of Canada Economic Geology Report 36, 16-Google Scholar
- Klein C, Fink RP: Econ Geol. 1976, 71-Google Scholar
- Carlson L, Schwertmann U: Geochim Cosmochim Acta. 1981, 45: 421-429. 10.1016/0016-7037(81)90250-7.View ArticleGoogle Scholar
- Lovley DR: Biomineralization Processes of Iron and Manganese – Modern and Ancient Environments. Edited by: Skinner HCW, Fitzpatrick RW. 1992, CATENA, 101-Supplement 21Google Scholar
- Kalogeropoulos SI, Scott SD: The Kuroko and Related Volcanogenic Massive Sulfide Deposits. Edited by: Ohmoto H, Skinner BJ. 1983, Economic Geology Monograph 5, 412-Google Scholar
- Klein C: Geological Association of Canada-Mineralogical Association of Canada Waterloo 94 Program With Abstracts. 1994, 19-Google Scholar
- Duhig NC, Stolz J, Davidson GJ, Large RR: Econ Geol. 1992, 87-Google Scholar
- Tazaki K, Ferris FG, Wiese RG, Fyfe WS: Proceedings of the 9th International Clay Conference: Science and Geology. Edited by: Farmer VC, Tardy Y. 1990, 35-Google Scholar
- Ronde CJD, Wit MJD, Spooner ETC: Geol Soc Am Bull. 1994, 106-Google Scholar
- Svitil KA: Discovery. 1994, 15-Google Scholar
- Garrels RM, Christ CL: Solutions, Minerals and Equilibria. 1965, Harper & Row, New YorkGoogle Scholar