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Mass transfer in the Earth’s interior: fluid-melt interaction in aluminosilicate–C–O–H–N systems at high pressure and temperature under oxidizing conditions

Progress in Earth and Planetary Science volume 5, Article number: 6 (2018) Cite this article

Abstract

Understanding what governs the speciation in the C–O–H–N system aids our knowledge of how volatiles affect mass transfer processes in the Earth’s interior. Experiments with aluminosilicate melt + C–O–H–N volatiles were, therefore, carried out with Raman and infrared spectroscopy to 800 °C and near 700 MPa in situ in hydrothermal diamond anvil cells. The measurements were conducted in situ with the samples at the desired temperatures and pressures in order to avoid possible structural and compositional changes resulting from quenching to ambient conditions prior to analysis. Experiments were conducted without any reducing agent and with volatiles added as H2O, CO2, and N2 because both carbon and nitrogen can occur in different oxidation states.

Volatiles dissolved in melt comprise H2O, CO32-, HCO3-, and molecular N2, whereas in the coexisting fluid, the species are H2O, CO2, CO32-, and N2. The HCO3-/CO32- equilibrium in melts shift toward CO32- groups with increasing temperature with ∆H = 114 ± 22 kJ/mol. In fluids, the CO2 abundance is essentially invariant with temperature and pressure. For fluid/melt partitioning, those of H2O and N2 are greater than 1 with temperature-dependence that yields ∆H values of − 6.5 ± 1.5 and − 19.6 ± 3.7 kJ/mol, respectively. Carbonate groups, CO32- are favored by melt over fluid.

Where redox conditions in the Earth’s interior exceed that near the QFM oxygen buffer (between NNO and MW buffers), N2 is the stable nitrogen species and as such acts as a diluent of both fluids and melts. For fluids, this lower silicate solubility, in turn, enhances alkalinity. This means that in such environments, the transport of components such as high field strength cations, will be enhanced. Effects of dissolved N2 on melt structure are considerably less than on fluid structure.

Introduction

Characterization of the processes that govern the budget and recycling of volatile components in the Earth’s interior is central to our understanding of the formation and evolution of the solid Earth, its oceans, and atmosphere (e.g., Kasting et al. 1993; Jambon 1994; Tolstikhin and Marty 1998; Deines 2002). However, our knowledge of the nitrogen abundance in the Earth’s mantle and in mantle-derived magma is not well established with model-dependent mantle abundance suggested between about 1 and 35 ppm (Marty, 1995; Javoy, 1997). The nitrogen abundance likely also is heterogeneously distributed with considerably greater nitrogen contents in subduction zone environments where abundances above 0.1% N2 have been reported (Fisher et al. 2002). This latter environment likely also is where most of the exchange of volatiles (including nitrogen) occurs between the solid Earth and the atmosphere (Schmidt and Poli, 2003; Bebout, 2007).

Transfer of nitrogen from the Earth’s interior to the surface and atmosphere is accomplished via partitioning of nitrogen between solid mantle, partial melts and perhaps multicomponent fluids with melt/mineral and fluid/mineral N2 partition coefficients exceeding 1. Mass transport is at the core of these processes.

Characterization of transport processes requires data and models that describe physico-chemical properties of silicate melts and C–O–H–N fluids at high temperature and pressure under controlled redox conditions. Redox conditions are important because even within the redox range of natural magmatic processes in the Earth’s interior (Carmichael and Ghiorso 1990; Wood et al. 1990), carbon and nitrogen, in particular, may occur in different oxidation states (Libourel et al. 2003; Kadik et al. 2004 2010; Mysen et al. 2008 Mysen et al. 2011; Li and Keppler 2014). The nitrogen solubility and solution mechanism(s) in silicate melts are sensitive to the redox state of nitrogen (Libourel et al., 2003; Mysen and Yamashita, 2010; Kadik et al. 2015) and needs to be controlled, therefore, during experiments in order to describe the behavior of nitrogen during melting and crystallization in the Earth’s interior.

Nitrogen is but one of several volatile components in the Earth’s interior with the system C–O–H–N comprising the main components (Jambon, 1994). Solubility and solution mechanisms of C–O–H–N components in silicate melts and of silicate components in C–O–H–N fluid are, therefore, necessary, and may be carried out experimentally (e.g., Franz 1998; Newton and Manning 2005 2006; Li and Keppler 2014; Kadik et al. 2015). However, most of that information is from analysis of glasses formed by temperature-quenching of volatile-containing melts to form a glass at ambient temperature at high pressure followed by decompression and, finally, examination of these glasses. Application of such data to characterize high-temperature/pressure melts and fluids relies on the assumption that there are no changes of these materials as they are brought from high temperature and high pressure to ambient conditions. The structure of a glass formed is this way is not that of the melt. Rather, it is the structure frozen in at the glass transition (e.g., Moynihan et al. 1976; Richet and Bottinga 1986; Dingwell and Webb 1990; Richet et al. 1992) because melt structure is temperature (and pressure) dependent (e.g., Stebbins 1988; Mysen et al. 2003; Agee 2008; Yamada et al. 2011; Wu et al. 2014). Moreover, in melts that contain volatiles, their speciation can be temperature- and pressure-dependent (Nowak and Behrens, 1995; Mysen and Yamashita 2010; Wu et al. 2014). In addition, during quenching to ambient temperature and pressure, some or all of the volatiles may exsolve from the cooling melt because the solubility of volatiles in melts varies with both temperature and pressure. Therefore, neither the volatile content nor the speciation of a glass is that which existed in its molten state at high temperature and pressure.

An additional problem associated with examination of quenched material as a proxy of high-temperature/pressure is that the structure of C–O–H–N fluids in equilibrium with silicate at high temperature and pressure cannot be quenched for quantitative structure study at ambient conditions. This is partly because silicate and other oxides dissolved in fluids at such high temperatures and pressures often precipitate during quenching (e.g., Zhang and Frantz 2000; Mysen and Armstrong 2002; Kessel et al. 2004), and partly because the C–O–H–N fluid structure may change as pressure and temperature are reduced from the experimental to ambient conditions (e.g., Mysen and Yamashita 2010; Wu et al. 2014). In summary, it is necessary, therefore, to study melts and fluids at the temperature and pressure of interest in order to attain quantitative understanding of their structure and their structure-property relations.

Recent experimental studies have addressed structural and compositional aspects of silicate–COH fluid + melt systems while samples were at high temperature and pressure (Ni and Keppler 2013; Mysen 2015a, b). Less is known about chemically more complex situation in which the C–O–H–N system of volatiles in equilibrium with aluminosilicate melts. The objective of the present study is to address this latter type of system in order to provide experimental data with which to further our understanding the structure of fluids and melts of aluminosilicate–C–O–H–N systems relevant in the temperature and pressure range of the Earth’s crust and upper mantle under oxidizing conditions.

The experiments were conducted under conditions where nitrogen exists in its oxidized state, N2. We note, though, that nitrogen may be reduced to amide and ammine forms at and above hydrogen fugacities between those defined by the NNO–H2O (nickel–nickel oxide) and MW–H2O (magnetite–wüstite) redox conditions (Mysen et al. 2008), which are redox conditions within the range encountered in the Earth’s interior (Wood et al. 1990; Frost and McCammon, 2008). This information is, therefore, relevant only to the most oxidized part of this range of redox conditions.

Methods/Experimental

Optical and vibrational spectroscopic data from the samples were recorded while these were at the desired high pressure and temperature while contained in externally heated, hydrothermal diamond anvil cells (HDAC) of the type originally described by Bassett et al. (1996). In this cell, the upper and lower diamonds are surrounded by Mo wrap-around wire heaters. Two thermocouples in contact with the upper and lower diamonds, respectively, are located within less than 1 mm from the sample. The samples, themselves, were contained in the cell within 125 μm thick Ir gaskets with a 500 μm diameter sample hole. Iridium was used as gasket material because it does not react with the sample (melt and fluid) at the temperature and pressure conditions of these experiments.

The temperature was measured with K-type thermocouples that were calibrated against the melting temperature of NaCl (800.5 °C). Temperature error was about ± 3 °C with the thermal gradient across the sample volume less than 2 °C. Pressure was generated by the fluid at high temperature in the cell. Pressure is, therefore, a dependent variable in these experiments. It was determined from the one-phonon Raman shift of 13C synthetic diamond, which was used to avoid interference with the Raman signals of 12C from the diamond cell itself (Bassett et al. 1996; Schiferl et al. 1997; Mysen and Yamashita 2010). Ten to 30 μm across diamond pieces were grown from 13CH4 by using CVD techniques (Liang et al. 2009). Pressure uncertainty at high temperature is ± 110 MPa and precision ± 40 MPa determined from the precision of the Raman spectrometer (± 0.1 cm−1 by using Ne lines as internal spectrometer calibrant) and the uncertainty in the calibration by Mysen and Yamashita (2010).

The samples in the diamond cell were examined through optical microscopy and via confocal micro-Raman and microFTIR methods while at the temperature and pressure of interest. In the Raman spectroscopic studies, the samples (melt and fluid) were excited with the 490 nm line of a solid state laser in a JASCO model NRS-3100 confocal micro-Raman spectrometer. The spectrometer is equipped with a single monochromator, a holographic notch filter, and holographic gratings with 600, 1200, and 2400 grooves/mm. The laser was focused to about 1 μm diameter at the sample with power at the sample typically near 30 mW. Spectra were recorded through a × 50 magnification/0.42 N.A. long-working distance Mitutoyo objective lens. An Andor Model DV401-F1 1024 × 128 pixel (25 μm pixel size) Peltier-cooled CCD was used for signal detection. By using the confocal optics, > 85% of the signal was recorded from within 30 μm of a sample surface (Mysen 2015a). For infrared spectroscopy, a JASCO model IMV4000 FTIR microscope system operating in transmission mode with 10X objective and condenser cassegrain lenses, an InSb detector, CaF2 beam splitter, and a halogen light source was employed.

Staring materials were aluminosilicate glass chips of composition (Na2Si4O9)90(Na(NaAl)4O9)10 (denoted NA10) together with solid Ag2C2O4 and AgN3 as sources of CO2 and N2, respectively. No reducing agent was added to the starting materials so that all components, including N2 and CO2, remain in their oxidized form. The (Na2Si4O9)90(Na(NaAl)4O9)1o glass was from the batch originally synthesized by Mysen (2007), but remelted and quenched to glass to be used for starting materials here in order to eliminate incipient crystals and adsorbed and water that may contributed to the sample during its storage. The Ag2C2O4 breaks down to metallic Ag and CO2 gas in between 150° and 200 °C and AgN3 to metallic Ag and N2 gas under similar temperature conditions (Boettcher et al. 1973; Roskosz Mysen and Cody, 2006). A few experiments were also conducted with Ag2C2O4 + H2O only in order to generate reference spectra of volatiles in the COH fluid system.

The sample volume defined by the central hole in the Ir gaskets is about 0.025 mm3, which poses a major challenge for quantitative addition of individual components to the starting material. To overcome some of the problems posed by these very small samples, a mixture of NA10 + Ag2C2O4 + AgN3 with 8.7 wt% CO2 and 8.0 wt% N2 was prepared prior to sample loading. Double-distilled and deionized H2O was added with the aid of a micro-syringe, but the proportion of H2O relative to solid materials could not be determined quantitatively because the sample masses are on the order of 0.0x μg. It was, nevertheless attempted to add total solid (NA10 + Ag2C2O4 + AgN3) and liquid H2O visually estimated to about 1:1 volume proportions.

For both Raman and infrared spectroscopic measurements, the sample was first heated to the highest planned temperature and was kept at this condition for ~ 60 min. This duration is more than sufficient to reach equilibrium for which only several minutes are needed (Horita 1988 2014). Spectroscopic measurements of the sample (fluid, melt, and/or supercritical fluid) together with the 13C diamond were carried out at this highest temperature and pressure condition. The temperature was then decreased at 1 °C/s to the next temperature and pressure condition with the sample remaining in the HADC, and the measurement protocol was repeated. There was some deformation of the Ir gaskets at the highest temperatures of these experiments, which led to sample volume changes. This is why pressure does not decrease monotonously with decreasing temperature (Table 1). Ambient conditions Raman measurements of the 13C diamond were carried before and after a series of high-temperature and high-pressure experiments.

Table 1 Experimental data
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The FTIR measurements were conducted with the same sample contained in the diamond cell as that used for Raman measurements. This sample was subjected to the same temperatures and pressures by using the same protocol as the Raman measurements and was carried out after the Raman measurements were completed. Pressure could not be measured with the diamond shift in the FTIR system. It was assumed, therefore, that for given temperature, the pressure recorded with the 13C diamond in the Raman measurement series was the same during the subsequent FTIR measurements. The validity of this assumption was assessed by monitoring the temperature of gas exsolution from the fluid phase during the Raman and FTIR experiments. Gas exsolution at the same temperature at constant sample volume implies the same pressure at each temperature. In the present experiments, this exsolution temperature was within 10°–15 °C in the Raman and FTIR measurement series. This uncertainty corresponds to a ± 0.02 g/cm3 density uncertainty for pure H2O, which for the H2O density of the experiments reported here corresponds to ± 20 MPa. Equation-of-state data for the fluid mixture are not available, but given that H2O is a dominant volatile component, ± 20 MPa uncertainty seems reasonable. This conclusion implied a temperature/pressure evolution in the FTIR experiments within error the same as in the Raman measurement series.

The Raman and infrared transmission spectra include contributions from the diamond anvils. This background signal was eliminated in the FTIR spectra by normalizing to those of an empty diamond cell at the same temperature after the sample was removed. For the Raman spectra, the procedure is more complex, and the diamond background was subtracted by using the procedure of Dalou et al. (2015). Briefly, this required recording Raman spectra of the diamond cell away from the sample hole in the Ir gasket but within the same focal plane as the sample measurement at the same temperature and pressure. This spectrum was then subtracted from the sample spectra (melts, fluids, and supercritical fluids), which results in a spectrum without signal contribution from the second-order Raman signal intensity from the diamond cell itself.

The subtraction method used for the Raman spectra could not be used over more than several hundred cm−1 frequency range in part because the sensitivity of the CCD detector varies with frequency. Subtraction over wider ranges could, therefore, result in artificial intensity variations. Moreover, in frequency regions with rapid intensity variations, the spectrometer positioning uncertainty (2–3 cm−1) could result in artificial sharp intensity variations. Care was, therefore, exercised to narrow the frequency ranges of Raman spectra to within those of particular interest when conducting the background correction. The infrared spectra suffered from complications resulting from major variations in intensity across the spectra so that in order to obtain reasonable signals from CO2 and from the overtone/combination bands of water species (see also below) portions of the spectra could not be recorded as the signals commonly saturated the detector. Sample thickness is governed by the gasket thickness and could not, therefore, be varied greatly. It is for this reason that only portions of the infrared spectra are shown.

Results

Experimental conditions are shown in Table 1. In the temperature range from 475 to 750 °C, the samples comprise 30–40 μm diameter melt spheres in a matrix of fluid (Fig. 1). At 800 °C, there is a single fluid phase only. The melt spheres and the fluid matrix could be probed quantitatively with the confocal micro-Raman system because with the ~ 1 μm diameter laser beam the sampling depth is within the range of the sphere diameter or less. In the FTIR spectrometer, however, the minimum aperture is > 30 μm, which means that with the 30–40 μm diameter melt spheres in these experiments, quantitative infrared absorption spectra of melts were not possible because a significant portion of the infrared beam will pass through neighboring fluid. Only infrared absorption spectra of fluid spectra are, therefore, reported.

Fig. 1
figure1

Microphotograph of samples in the diamond cell at 550 °C and 262 MPa. a As viewed through the optical microscope during micro-Raman measurements. The width of the field of view is 200 μm. b View of the sample through the optical microscope in the microFTIR system. The numbering on the crosshair indicates μm. The shaded area centered in the cross-hear indicates the position and dimension of the aperture (100 × 150 μm) for fluid examination in this particular experiment

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Infrared absorption spectra

Infrared absorption spectra of fluid in the frequency range of the combination and overtone bands of OH and H2O (4000–7500 cm−1) can be used to infer changes in total H2O content as well as proportion of molecular H2O and OH groups that form bonding with Si4+ and Al3+ in silicate (e.g., Scholze 1959; Malfait and Xue 2014). The presence of molecular H2O in fluids (and melts) characteristically results in absorption centered near 5200 cm−1, which has been assigned to a combination band of the H–O–H bending vibration near 1600 cm−1 and the OH fundamentals near 3600 cm−1 (Fig. 2) (Scholze 1959). The 7200 cm−1 band is the first overtone of the 3600 cm−1 OH stretch vibrations and has been used to obtain total water content of the sample (Scholze 1959; Dixon et al. 1995; Behrens and Nowak 2003). The 5200 and 7200 cm−1 bands broaden significantly with increasing temperature with the broadening of the 7200 cm−1 including development of an asymmetry toward higher frequency at the highest temperatures.

Fig. 2
figure2

FTIR spectra of fluid at temperatures indicated. Corresponding pressures can be found in Table 1. The dashed line is the spectrum from a single-phase fluid. Insert shows expanded view of frequency region centered at 4500 cm−1. Note that all spectra are offset for clarity. The 0-intensity line passes through the background at 600 cm−1. In the insert, the 0 line is approximately that near 4300 cm−1

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There is also minor intensity centered near 4500 cm−1 at the higher temperatures in the infrared spectra of fluids (see insert in Fig. 2). The 4500 cm−1 band is a combination band of the OH fundamentals at 3600 cm−1 and vibrations in OH groups attached to Si and Al to form (Si,Al)–OH bond with its main vibrational band between 900 and 950 cm−1 (Malfait and Xue 2014). Its integrated intensity increases approximately linearly with increasing temperature to a maximum relative intensity of few percent relative to the 5200 cm−1 intensity (Fig. 3). Conversion of this information to concentration requires molar absorption coefficients, which are not available for these fluids. However, if we assume that the 10% difference in these coefficients between the 4500 and 5200 cm−1 absorption from Na2O–SiO2 glasses (Yamashita et al. 2008), from the relationship;

Fig. 3
figure3

Relationship between the area of the band centered near 4500 cm−1 and that near 5200 cm−1 (expressed in percent) from FTIR absorption spectra of fluid. The data point from 800 °C (open circle) is from single-phase fluid. The straight line is a simple linear fit to the data point (not including that from single-phase fluid at 800 °C); area ratio = 0.0100 ± 0.0009–5.4 ± 0.5 T(°C)

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$$ {C}_{\mathrm{OH}}/{C}_{\mathrm{H}2\mathrm{O}}={A}_{4500}/{\upvarepsilon}_{4500}/\left({A}_{5200}/{\upvarepsilon}_{5200}\right), $$
(1)

where C is concentration, A is integrated area, and ε is molar absorption coefficient. The ε5200 is about 10% larger than ε4500, which means that the area ratio in Fig. 3 at most underestimates the proportion of OH by about 10%.

Infrared spectroscopy also was employed to probe for species that comprise carbon or nitrogen (CO2, CO, N2, N2O, etc.) or both (e.g., carboxyl groups or CN groups). Among these species, molecular N2 is infrared inactive, but can be identified, if present, with Raman spectroscopy (see below).

In the spectra of fluids, the only absorption observed is that near 2350 cm−1 (Fig. 4), which is assigned as the v3 antisymmetric stretching in the CO2 molecule (see Nowak et al. 2003, and references therein). Its integrated intensity is essentially independent of temperature and pressure (see insert A in Fig. 4). Notably, though, the width of this absorption broadens with increasing temperature. It also is asymmetric, wherein a second band could be fitted near 2320 cm−1 (see insert B, Fig. 4). This second absorption might exist because there may be variations in the geometry of the CO2 molecule when dissolved in silicate-saturated C–O–H–N fluid.

Fig. 4
figure4

Infrared absorption spectra of fluids in the spectral region of C–O stretching in CO2 molecules as a function of temperature and pressure (see Table 1 for pressures). The spectra are offset for clarity. The vertical line is the scale bar for the Absorption intensity of the spectra. Inserts A and B show the integrated intensities of the absorption and an example of 2-line curve-fitted infrared spectrum by using Gaussian line shape. The spectrum shown was recorded while the sample was at 750 °C. Dashed line is from 800 °C where a single fluid phase only exists

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Raman spectra

Raman spectra provide information on a range of potentially volatile species as well as silicate species in fluids and melts.

H2O component

The 3000–4000 cm−1 frequency region of the Raman spectra comprises that where signals from the fundamental OH vibrations will occur when water is present in a sample (Walrafen 1967; Holtz et al. 1996). This Raman intensity includes contributions from both molecular H2O and structurally bound OH groups.

Sharp, nearly symmetric bands with intensity maxima slightly below 3600 cm−1 were recorded in the spectra of all fluids and all melts (Fig. 5a, b). By normalizing the integrated intensities to that in the spectrum of single-phase fluid at 800 °C (diamond in Fig. 5c), we find that this intensity passes through at maximum near 625 °C before decreasing with further temperature increase. The intensities in the spectra of fluid always exceed those of coexisting melt.

Fig. 5
figure5

Raman spectra of coexisting fluid and melt in the high-frequency region of fundamental O–H vibrations. a Spectra of fluid at temperatures indicated (corresponding pressures can be found in Table 1). b Spectra of coexisting melt (corresponding pressures can be found in Table 1). The spectra are normalized to the same acquisition time with identical focal plane and with otherwise identical instrumental parameters. c Normalized areas of coexisting melt and fluid as indicated. d Full width at half height, FWHH, from the spectra in Figs. A and B

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The width of the 3600 cm−1 Raman bands decreases with increasing temperature (Fig. 5d), which is qualitatively similar to that reported for pure H2O as well as that of water in silicate-rich hydrous fluids and melts in silicate–H2O systems (Frantz et al. 1993; Walrafen et al. 1999; Foustoukos and Mysen 2015). This decrease is associated with diminishing asymmetry on the low-frequency-side of the spectrum, a feature that has been ascribed to less influence of hydrogen bonding among water species with increasing temperature (Walrafen et al. 1996, 1999; Foustoukos and Mysen 2012). At all temperatures and pressures, the width of this band in spectra of hydrous melts is greater than in the spectra of silicate-bearing aqueous fluids. This difference reflects either different hydrogen bonding environment in fluids and melts or a broader range of different forms of OH groups might exist in hydrous melts, or both, in hydrous melts as compared with the silicate-bearing C–O–H–N fluids. It is likely that both features contribute. It has been shown, for example, that the enthalpy of hydrogen bond formation of water in silicate melts is less than 50% of the value in aqueous fluids (Mysen 2014). Given the much more silica-rich nature of hydrous melts compared with silicate-saturated C–O–H–N fluids in the temperature and pressure range under a study, it is not surprising that a broader range of types of OH formation would be found in water-bearing silicate melts.

Nitrogen component

The most common N-bearing species in the C–O–H–N system could be N2, N2O, (N..H)-species, nitride and perhaps CN complexes. Their individual stability depends on bulk composition, temperature, pressure, and redox conditions. There is no evidence in the present spectra for (N..H) complexes (in the 3000–3400 cm−1 range; Yeo and Ford, 1994), nitride substitution in SiO4 tetrahedra (> 1200 cm−1; Sato et al. 1990), and CN-complexes (2000–2200 cm−1 frequency range; see, for example, Nakamoto 2009). The lack of Raman signals in the frequency ranges of these possible compounds is consistent with the fact that nitrogen was added as N2 (from AgN3 decomposition) and no reducing agent was added to the sample.

Absent a reducing agent, nitrogen in the C–O–H–N system may exist as N2O, azide (N3−) or as N2, which are all detectable with Raman spectroscopy. For example, in an experimental study of N-bearing silicate glasses in which Raman and 15N MAS NMR spectroscopies were the structural tools, Roskosz Mysen and Cody (2006) reported that the principal Raman signals from nitrosyl (N2O) and azide (N≡N) are near 2100 and 2200 cm1. No Raman signals were detected in this frequency region thus ruling out detectable amounts of such species in either fluid or melt. Whether or not NO3 groups are formed will be addressed below in the presentation of the low-frequency range comprising vibrations of the silicate network because N–O vibrations occur in the same frequency range (between 1100 and 1200 cm−1; Fung et al. 1994). There is no Raman signal in this frequency range in spectra of fluids. The signal intensity in spectra of melts can be satisfied without resorting to the presence of Raman bands assignable to N–O vibrations in NO3 groups. This leaves molecular N2 as the only likely nitrogen species in fluids and melts in the silicate–C–O–H–N system under study here.

The N=N stretch vibrations from molecular N2 dissolved in silicate melts at high pressure result in Raman bands slightly above 2300 cm−1 (Roskosz Mysen and Cody, 2006). The spectra of fluids and melts in the silicate–C–O–H–N system exhibit a single sharp line near 2320 cm−1 after the background from second-order Raman peaks in this region from the diamonds in the diamond cell, itself, was subtracted (Fig. 6a, b). The peaks are Gaussian in shape, which is similar to that reported by Roskosz Mysen and Cody (2006) in Raman spectra of N2-saturated silicate glasses quenched from melts at pressures ≥ 1 GPa. In contrast, gaseous N2 spectra have sharp Lorentzian peaks. This difference likely reflects some interaction between the N2 molecules and the hydrous silicate melt matrix in which they are dissolved.

Fig. 6
figure6

Raman spectra of coexisting fluid and melt in the high-frequency region of fundamental N=N vibrations. a Spectra of fluid at temperatures indicated (corresponding pressures can be found in Table 1). b Spectra of coexisting melt (corresponding pressures can be found in Table 1). The spectra are normalized to the same acquisition time with identical focal plane and with otherwise identical instrumental parameters. c Areas of coexisting melt and fluid normalized to the area of single phase fluid at 800 °C as a function of temperature and pressure

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The integrated Raman intensities of these bands, normalized to the same acquisition time and retaining the same focal plane for all measurements show distinctly different abundance behavior with temperature and pressure relative to the value in the spectra of single phase fluid (Fig. 6c). Whereas the normalized abundance in fluid passes through a maximum before decreasing rapidly with increasing temperature and pressure, the normalized abundance of N2 in the coexisting melt is insensitive to temperature (and pressure).

Carbon component

Carbon speciation in fluids and melts is redox sensitive. Under reducing conditions such as those near the magnetite–wüstite buffer and more reducing, the most common species in silicate–COH system is CH4 with the dominant Raman signals near 2900–3000 cm−1 (Kadik et al. 2004; Mysen et al. 2011; Armstrong et al. 2015). In the absence of hydrogen and under reducing conditions, oxycarbide complexes have been proposed (Libourel et al. 2003; Renlund et al. 1991; Soraru et al. 1995) with the two dominant Raman bands near 1350 and slightly above 1500 cm−1, respectively (Soraru et al. 1995). There is no evidence for any of these species in the Raman spectra of fluids and melts, which is, of course, understandable given the conditions of no reducing agent in samples were carbon was added to the starting materials as CO2.

Molecular CO2, CO32-, and HCO3- groups are the three main C-bearing species under oxidizing conditions. Molecular CO2 was detected in the infrared absorption spectra of fluid as discussed above (Fig. 4). However, the Fermi diad of molecular CO2, which at ambient conditions occurs at 1280 and 1380 cm−1, respectively (Rosso and Bodnar 1995; Lamadric et al. 2017), cannot be identified in Raman spectra of the samples contained in diamond cells at high temperatures because the one-phonon Raman shift from the natural diamonds used as anvils in the cell results in a Raman band with intensity that covers those frequency regions. As noted above, infrared spectra could not be obtained from the melt spheres because of their small size. It could not be established, therefore, whether molecular CO2 also exists in the hydrous silicate melts at high temperature and pressure.

The Raman spectra of fluids and melts may, contain information relevant to possibility of CO32- and HCO3- groups because of their dominant C–O stretch vibrations near 1070 and 1020 cm−1 at ambient temperatures and pressures. The C–O stretch vibration in HCO3- is particularly sensitive to temperature and is located near 950 cm–1-near 500 °C, for example (Frantz 1998). In simple COH fluids equilibrated at 700 °C and above (without nitrogen and without silicate components), there is evidence for CO32- groups from Raman intensity near 1070 cm−1 (Fig. 7), which is assigned to C–O stretch vibrations in CO32- groups (White 1974; Frantz 1998). A peak that occurs slightly below 1100 cm−1 in the spectra of silicate–C–O–H–N melt from 550 °C to the highest temperatures (Fig. 8). The same peak can be detected in spectra of fluids from 550 °C to the highest temperatures. It is assigned to C–O vibrations in CO32- groups. Within the scatter of the data, there are no other peaks in this frequency region in the spectra of fluid (Fig. 8a). In the spectra of melts, a second band appears near 1000 cm−1 (Fig. 8b), which is assigned to C–OH vibrations in HCO3- groups (Frantz 1998). We cannot detect HCO3- groups in spectra of fluids. Neither is there any signal above 1100 cm−1, which could be due to N–O vibrations in NO3 groups in the fluids (Fung et al. 1994).

Fig. 7
figure7

Raman spectra of COH fluids at 600°, 700°, and 800 °C and corresponding pressures (see Table 1). The peak near 1070 cm−1 is assigned to C–O stretch vibrations in CO3 groups (Frantz et al. 1993) and marked CO3

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Fig. 8
figure8

Example of Raman spectra of silicate–C–O–H–N fluid and melt at 625° and 750 °C, respectively, fitted to Gaussian lines in the 950–1150 cm−1 frequency range. a Spectra from fluid with a single line assigned to C–O vibrations in CO3 groups. b Spectra from melts where three lines are needed. These are assigned to C–O stretching in HCO3- and CO32- groups and to Si–O stretching in Q3 silicate species (see text for discussion on these assignments)

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Absolute concentration of CO32- and HCO3- groups cannot be obtained from the spectra without assuming that the Raman cross-sections for the two vibrations are similar. It is clear, nevertheless, that in both fluid and coexisting melt, the CO32- abundance increase with temperature and pressure until the univariant line that separates melt + fluid from a single fluid is crossed (near 800 °C) (Fig. 9). In this regard, the evolution of the CO32- abundance with temperature and pressure resembles those of N2 and H2O (Figs. 5c and 6c). There is, however, a difference in that for N2 and H2O, these components are favored by the fluid, whereas for the CO32- groups, these are favored by melt.

Fig. 9
figure9

Evolution of CO32 abundance in coexisting fluid and melt as a function of temperature and pressure with concentration, expressed as area of the ~ 1070 cm−1 band normalized to the value for single phase fluid at 800 °C (diamond symbol)

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Silicate components

Silicate components and their species exist in coexisting silicate melts and C–O–H–N fluid. There are, however, significant differences between the silicate-saturated C–O–H–N fluid and the C–O–H–N-saturated silicate melts as seen, for example, in their significantly different Raman spectra (Fig. 10). In spectra of fluid, the dominant peak is near 780 cm−1, and is assigned to Si–O vibrations in Q0 species (Zotov and Keppler 2002; Mibe et al. 2008). The spectra of fluid characteristically also comprise a broad band centered near 600 cm−1, with two weaker bands near 810 and 900 cm−1, respectively. The latter two Raman bands are assigned Si–O vibrations in Q1 and Q2 species, respectively, whereas that centered near 600 cm−1 is an Si–O–Si bending vibration, which requires, therefore, bridging oxygen such as, for example, in Q1 and Q2 species (Zotov and Keppler 2002). At frequencies higher than 1000 cm−1 in spectra of fluids, there is a weak band near 1070 cm−1, assigned to C–O stretching in CO3 groups, as discussed under C-bearing species above (see also Fig. 8).

Fig. 10
figure10

Examples of Raman spectra of single phase fluid (at 800 °C) and coexisting fluids and melts at temperatures indicated (corresponding pressures in Table 1). Also shown in the spectra are fitted Gaussian lines relevant to structural assignments of silicate and carbonate species. The intensity scale in each spectrum is identical

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The spectra of coexisting melts differ significantly from those of fluids. They do comprise the 780, 810, and 900 cm−1 bands also seen in spectra of fluids, but in addition, there is a band near 1100 cm−1 not seen in the fluid spectra. There is also much more intensity at frequencies below 700 cm−1 (Fig. 10). The 1100 cm−1 is assigned to Si–O vibrations in Q3 species, whereas the extensive intensity below 700 cm−1 is due to bending and rocking motions in polymerized silicate species (McMillan 1984; Neuville et al. 2006; Mibe et al. 2008). The intensity near 500 cm−1, coupled with the shoulder near 550 cm−1, in the spectra of melts suggests that Q4 species may exist in the C–O–H–N-saturated silicate melts. The 1070 and 1000 cm−1 bands, assigned to C–O stretching in CO32- and HCO3- species, were discussed above (Fig. 8).

The abundance of Q-species and degree of polymerization, NBO/T, of silicate in fluids and melts were derived from the Raman spectra. This was accomplished by assuming that the Raman cross sections of Si–O stretch vibrations in Q0, Q1, Q2, and Q3 species were the same. The NBO/T can then be calculated from the simple relationship;

$$ \mathrm{NBO}/\mathrm{T}=\sum \limits_{n=1}^{n=4}{\left(\mathrm{NBO}/\mathrm{T}\right)}_{Q^n}\bullet {X}_{Q^n}, $$
(2)

where (NBO/T)Qn is the degree of polymerization of a specific Q-species and XQn its mol fraction.

The C–O–H–N-saturated melts become increasingly depolymerized (NBO/T increases) with increasing temperature and pressure, whereas that of silicate in the C–O–H–N fluid follows the opposite trend (Fig. 11). These trends qualitatively are the same as those observed in the simpler silicate–H2O systems (Mysen 2009) and reflect how the H2O component in silicate–C–O–H–N melts in breaks up the silicate network. The effect becomes more pronounced with increasing temperature and pressure because such increases also most likely are associated with increasing water concentration in the melt. In the C–O–H–N fluids, on the other hand, the silicate solubility increases with increasing temperature and pressure. Increasing silicate concentration in water-bearing fluids results in increasing silicate polymerization (Mysen et al. 2013).

Fig. 11
figure11

Evolution of Q-species abundance and bulk NBO/T of melt and coexisting fluid as a function of temperature (and pressure, see Table 1). Note that diamond symbol represents single phase

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The NBO/T evolution with temperature and pressure reflects the abundance evolution of the Q-species (Fig. 11). For melts, the Q0 abundance increases with temperature and pressure, that of Q1 is insensitive, whereas the abundance of more polymerized species, Q2 and Q3, decreases with increasing temperature and pressure and, therefore, increasing water content. In other words, the C–O–H–N-saturated melts behave as simpler H2O-saturated melts, which become increasingly depolymerized with increasing water content (Zotov and Keppler 1998). This behavior contrasts with the silicate dissolved in C–O–H–N fluid, where the abundance of Q0 species decreases and that of Q1 increases with increasing temperature and pressure and, therefore, likely total water content (Fig. 11).

Discussion

The solubility mechanisms of volatile species in silicate–C–O–H–N melts qualitatively resemble those in the simpler systems such as silicate–H2O and silicate–COH. Addition of nitrogen to the system under oxidizing conditions results in formation of molecular N2, which does not interact chemically with the other volatile components.

Water in the form of molecular H2O dominates in C–O–H–N fluids with OH groups forming less than 3% of the total water concentration even at the highest temperatures and pressures (Fig. 3). This is less than the proportion of OH groups in pure silicate–H2O systems at similar temperatures and pressures, where this proportion often exceeds 10% (Mysen 2010). In fact, by using the relationship between proportion of OH in fluid, expressed as A4500/(A4500 + A5200) from the FTIR data, and fugacity of H2O for the same silicate composition and pure H2O (Mysen 2010) (see Fig. 12a), the much lower proportion of OH groups in the C–O–H–N–silicate fluid implies very considerably dilution of water because the fH2O of pure H2O at the pressures and temperatures of these experiments is in the 200–700 MPa range.

Fig. 12
figure12

Relationship between fugacity of H2O, fH2O, and species abundance. a Proportion of OH and molecular H2O as a function of fH2O in NA10–H2O fluid from Mysen (2010) (open symbols). Solid symbols plotted onto the line are the date from the current silicate–C–O–H–N fluid. In both cases, the silicate starting composition is NA10. See text for discussion of approximation of OH/(OH + H2O) ratio with the FTIR absorbance ratio, A4500/(A4500 + A5200). Silicate polymerization of melt, NBO/T, as a function of fH2O in NA10–H2O fluid from Mysen (2010) (open symbols). b Evolution of NBO/T of the silicate component in the fluid as a function of temperature. Solid symbols plotted onto the line are the data from the current silicate–C–O–H–N fluid. In both cases, the silicate starting composition is NA10

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Equivalent OH/H2O for melt were not obtained for reasons discussed above. However, the overall degree of silicate polymerization as a function of water fugacity, using the NA10–H2O data from Mysen (2010) for calibration, results in an equivalent fH2O quite similar to that of pure H2O (Fig. 12b). This observation may suggest that the presence of C and N components in the melt has a much smaller influence on activity composition relations in the (C–O–H–N)-saturated melt than in fluid. This difference reflects the much smaller solubility if silicate components in the fluid than in the melt.

Fluid/melt partition coefficients can be obtained from the ratio of integrated intensities of bands in spectra of coexisting melts and fluids assigned to specific vibrations provided that the instrumental parameters such as acquisition time, slit settings, and focal depth are same during acquisition of both spectra. This can be done because in a ratio of integrated intensities from bands assigned to the same vibration, the remaining variables affecting Raman intensity is temperature, which, of course, is the same for coexisting fluid and melt. Then, the partition coefficient of component, i, between fluid and melt, f/m, is;

$$ {K_i}^{\mathrm{f}/\boldsymbol{m}}={A_i}^{\mathrm{f}}/{A_i}^{\mathrm{m}}, $$
(3)

where A i f and A i m are the integrated areas from the Raman spectra of a band assigned to a specific type of vibration in component, i.

The partition coefficient for total H2O (which includes all OH-bearing species) can be derived with Eq. (3) from the 3600 cm−1 band intensity in spectra of fluids and melts (Fig. 5). This partition coefficient is always greater than unity, which is similar to the partition coefficient in silicate–H2O systems (Mysen 2013; Webster et al. 2014). From the linear fit to the ln KH2Of/m vs/ 1/T (T is temperature in kelvin), the enthalpy from this partioning is − 6.5 ± 1.5 kJ/mol (Fig. 13), which is quite similar to the results in the simpler silicate–H2O (Mysen 2013) where ∆H = − 7.6 ± 0.7 kJ/mol. That fact that this ∆H value differs from 0 reflects, most likely, the different extent and type of speciation of H2O in the coexisting melt and fluid. We should also note that the decreasing partition coefficient with increasing temperature actually reflects an increase in pressure as well, which results in increased silicate solubility in fluid and decreased silicate content of hydrous melt (its water content increases). In the isobaric (0.2 GPa) experiments by Webster et al. (2014), no temperature-dependence was observed. That notwithstanding, their fluid/melt partitions fall naturally on the extension of the present data and those of Mysen (2013).

Fig. 13
figure13

Partition coefficient between fluid and melt of total H2O, KH2Of/m, as a function of temperature. The least squares straight line fit is, KH2Of/m = −0.6 ± 0.2 + 782 ± 189/T, r2 = 0.85. Also shown are data from natural samples by Webster et al. (2014) and from experimental data in silicate–H2O from Mysen (2014). The least squares fit through the data of Mysen (2013) yields the expression, KH2Of/m = −0.3 ± 0.1 + 782 ± 920/T, r2 = 0.97

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For carbon species in melts and fluids in the silicate–C–O–H–N system, there are also similarities between the data and those in the simpler silicate–COH system (Mysen 2015a). However, there also are differences. For example, in the silicate-saturated C–O–H–N fluid, we have evidence only of molecular CO2 and CO32 groups, whereas in the silicate–COH system, Mysen (2015a) also observed evidence of HCO3- groups in the fluid. This difference implies that in the C–O–H–N fluids studied here, the simple carbonate equilibrium;

$$ 2{{\mathrm{H}\mathrm{CO}}_3}^{\hbox{-} }=2{{\mathrm{CO}}_3}^2+2{\mathrm{H}}^{+}, $$
(4)

is shifted further to the left than was the case in the COH fluids studied by Mysen (2015a). The implication is that the C–O–H–N fluids examined here are more alkaline that those examined by Mysen (2015a).

For C–O–H–N-saturated melts, on the other hand, there is spectroscopic evidence for both CO32 and HCO3- groups. No evidence could be found for molecular CO2 in the spectra of melt. A simple solution mechanism involving an equilibrium between CO32 and HCO3- is (Mysen 2015a):

$$ 2{{\mathrm{CO}}_3}^{2\hbox{-} }+{\mathrm{H}}_2\mathrm{O}+2{\mathrm{Q}}^n=2{{\mathrm{H}\mathrm{CO}}_3}^{\hbox{-} }+2{\mathrm{Q}}^{n-1}. $$
(5)

In Eq. (5), Qn, and Qn−1, are silicate species with, respectively, n and n−1 bridging oxygen. The CO32-/HCO3- abundance ratio in melts increases with increasing temperature with ∆H = 114 ± 22 kJ/mol (Fig. 14). The HCO3- abundance in melt diminishes rapidly with increasing temperature and can barely be observed at 750 °C and cannot be seen in spectra of single phase fluids at 800 °C. In comparison, in the N-free system silicate–COH, also examined in the hydrothermal diamond anvil cell with similar protocol, the CO3/HCO3- ratio was determined for the fluid to be considerably less sensitive to temperature with a ∆H = 17 ± 3 kJ/mol (Fig. 14).

Fig. 14
figure14

Abundance ratio, CO3/HCO3, as a function of temperature (and pressure, see Table 1) in silicate–C–O–H–N melts. The straight line is least squares fitted to the expression, ln(CO3/HCO3) = − 13,738 ± 2680/T + 17 ± 3, r2 = 0.95. Also shown are the experimental data from an aluminosilicate–COH system under similar conditions from Mysen (2015a). Note that the label on the y-axis in the original plot in Mysen (2015a) was inverted. This is corrected for the present figure. The regression line for that regression is ln(CO32/HCO3-) = − 1999 ± 367/T + 0.9 ± 0.4, r2 = 0.94

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The fluid/melt partition coefficients for CO32- groups are in the range of ~ 0.2 to ~ 0.7 as a function of increasing temperature and pressure with an enthalpy of 52 ± 14 kJ/mol (Fig. 15). These values fall in the range reported by Webster et al. (2014) and Mysen (2015b) even though the compositions in those experiments differed significantly from those of the present compositions.

Fig. 15
figure15

Partition coefficient of CO32 groups between coexisting fluid and melt as a function of temperature. Partition coefficients were determined as discussed under Eq. (1) in the text. The straight line fit by least squares regression yields; ln K = 6 ± 2–6203 ± 1620/T, r2 = 0.83. Also shown are data from Mysen (2015a) from a silicate–COH system, also under oxidizing conditions. The dashed lines represents a least squares linear fit through those data, with the expression ln(CO32-/HCO3-) = − 11,893 ± 7610/T + 13 ± 8, r2 = 0.74 as well as data from Webster et al. (2014) using natural silicate melts and COH fluids that also contains halogens and sulfur

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Even though nitrogen exists in coexisting fluid and melt only as molecular N2, there are differences in the interaction between the C–O–H–N fluid matrix in fluid and N2 and silicate matrix in melts and N2. This difference results in distinctly temperature-dependent N2 partition coefficients with an enthalpy change (− 20 ± 4 kJ/mol; see Fig. 16) that is considerably greater than the − 6.5 ± 1.5 kJ/mol observed for H2O partitioning between fluid and melt, for example (Fig. 13). The nitrogen partition coefficients also are more than 20% greater (and increasing with decreasing temperature) than for H2O. It would seem, therefore, that the activity-composition relations of N2 in melts, and perhaps fluids, differ from those of H2O. This difference likely is because H2O may dissolve both as molecular H2O and as OH groups forming bonding the silicate network, whereas there is no evidence that N2 behaves in such a manner.

Fig. 16
figure16

Partition coefficient between fluid and melt of N2, KN2f/m, as a function of temperature. The least squares straight line fit is, KH2Of/m = −1.9 ± 0.5 + 2356 ± 450/T, r2 = 0.90

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Conclusions

It follows from the observations here and in the literature (Mysen et al. 2008; Li and Keppler 2014) that where redox conditions in the Earth are more oxidizing than those defined by the NNO–H2O and FMQ–H2O buffer nitrogen released into fluid or melt will most likely exist as molecular N2. In other words, there is no evidence to indicate chemical interaction between N2 and other volatile and silicate species under such circumstances.

Redox conditions similar to these are those observed in subduction zones, for example (Wood et al. 1990; Cottrell and Kelley 2011). Under these conditions, nitrogen effectively serves as a diluent of the volatile species. Dilution is indicated, for example, by the low OH/H2O ratio of the C–O–H–N fluid (Fig. 12), which indicates lesser water activity than in silicate–H2O fluids. This much lower OH/H2O ratio probably this because silicate solubility in C–O–H–N fluids must be considerably less than in the absence of N2. This follows from simple relationships of the form;

$$ {\mathrm{Si}}^{4+}+{\mathrm{H}}_2\mathrm{O}=\mathrm{Si}{\left(\mathrm{OH}\right)}^{3+}+{\mathrm{H}}^{+}, $$
(6)

Where Si4+ is a proxy for silicate components and Si(OH)3+ a proxy for hydroxylated silicate. This means that as the activity of silicate decreases, the equation shifts to the left thus reducing the proportion of OH groups in the system,

It also appears, therefore, that a decrease of silicate activity in solution in the fluid resulting from the dilution of H2O by other fluid components enhances fluid alkalinity. This feature, in turn, may alter the solubility of pH-dependent minor and trace elements in the fluid (e.g., high field strength cations; see Ayers et al. 2012) and, therefore result in different element patterns resulting from C–O–H–N fluid release than from release of fluids without N2, where the silicate solubility is greater and the fluid likely is less alkaline. These features are, of course, also dependent on redox conditions because under reducing conditions nitrogen may form ammonia or ammine-type complexes (Mysen and Fogel, 2010; Li and Keppler 2014), which results in significant changes the behavior of nitrogen in both fluids and melt.

It appears that C–O–H–N-saturated melts are less sensitive to the presence of N2 than C–O–H–N fluids as both the degree of melt polymerization, NBO/T, and silicate species abundance, appear insensitive to the existence of molecular N2. However, as is the case for fluids, when magmatic activity occurs where conditions are sufficiently reducing to nitrogen to ammonia and ammine groups (somewhere near the hydrogen fugacity defined by the magnetitie–wüstite–H2O redox buffer; see Mysen et al. 2008), this may change because the solubility of reduced nitrogen in silicate melts is much greater than oxidized nitrogen. Furthermore, the solution mechanism of reduced nitrogen as NH-complexes resembles that of dissolved H2O (Mysen et al. 2014). Thus, nitrogen in magmatic liquids under such reducing conditions would tend to enhance melt properties that are sensitive to melt polymerization.

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Acknowledgements

Instrument, electronics and library support was provided by Geophysical Laboratory technical staff. Their support is gratefully acknowledged.

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This research was supported in by grant EAR1212854 from the National Science Foundation.

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    Bjorn Mysen

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Mysen, B. Mass transfer in the Earth’s interior: fluid-melt interaction in aluminosilicate–C–O–H–N systems at high pressure and temperature under oxidizing conditions. Prog Earth Planet Sci 5, 6 (2018). https://doi.org/10.1186/s40645-017-0161-6

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Keywords

  • Volatiles
  • Spectroscopy
  • Melt structure
  • Fluid structure
  • Temperature
  • Pressure