Springer Nature is making SARS-CoV-2 and COVID-19 research free. View research | View latest news | Sign up for updates

Incorporation of Rare Earths and Yttrium in Calcite: A Critical Re-evaluation

  • 75 Accesses

Abstract

The reported partition coefficients of REE with calcite are reviewed and critically discussed. In some of the reported experimental sets, REE concentrations are found to be supersaturated with respect to individual REE2(CO3)3 but never to REE(OH)3. Although the solutions are unsaturated with respect to individual REY carbonates, REY including Y are incorporated in calcite surfaces, where they are overgrown by calcite. Charge balances may be obtained by building {REY–Na-(CO3)2}n or by exchange of 2Ca2+ against REY3+ + blank space calcite lattice. These surface compounds may either be homogeneously distributed or clustered. Both the size and frequency of clusters increase with [REY]/[Ca] or [ΣREY3+]/[Ca2+] in solution. If these surface precipitates are removed into solutions saturated with respect to ΣREE2(CO3)3, they start growing in the aqueous phase. In this case, the apparent DREY and kREY values decrease with increasing REY concentrations in solution. In previous studies, only the individual distribution coefficients are reported not considering that the entirety of REY determines their behavior in partitioning. Given enough time, these surface clusters equilibrate with the aqueous phase before being overgrown by calcite. In the double logarithmic plots of {REY}/{Ca} versus [REY]/[Ca] or [REY3+]/[Ca2+], two relationships evolve characterizing the REY distribution in marine calcite and experimental calcites grown in Mg2+-free solutions. The double logarithmic plots of partition coefficients of REYi3+ in calcite grown from seawater show a slope exceeding unity, whereas those from fluids without Mg2+ depict slopes less than unity being both in contrast to the Henderson–Kracek rule.

Introduction

Rare earth elements (REE) and yttrium (Y) behave similarly and are henceforth referred to as REY (Bau and Dulski 1995). When Y is absent in cited experiments, the term REE is used. This suite of REY is ubiquitous in nature and is particularly incorporated in omnipresent calcite. The heterogeneous, onion-shell-like (Eq. 1) and homogeneous partitioning (Eq. 2) was first applied to describe the partition of Ra2+ with barium sulfate (Doener and Hoskins 1925) and chromate (Henderson and Kracek 1927), respectively.

$$k = \log \left( {\left\{ {{\text{REY}}_{{\text{in}}} } \right\}/\left\{ {{\text{REY}}_{{\text{fin}}} } \right\}} \right)/\log \left( {\left[ {{\text{Ca}}_{{\text{in}}} } \right]/\left[ {{\text{Ca}}_{{\text{fin}}} } \right]} \right)$$
(1)
$$D_{i} = \left\{ {X_{{{\text{REY}}_{i} }} } \right\}/\left\{ {X_{\text{Ca}} } \right\}/\left( {\left[ {{\text{REY}}_{i} } \right]/\left[ {\text{Ca}} \right]} \right)$$
(2)

X = mole fraction of individual REE related to the entirety of cations in calcite; indices: i = individual REE; in = initial; fin = final; { } and [ ] indicate total concentrations of elements in solid and aqueous phases, respectively. Ionic charges are only given where specific ionic species are addressed; no charges indicate total concentrations.

The experimental determinations of the homogeneous REY partition coefficients, DREY, show widely scattering results (Fig. 1) in calcite precipitation under both different experimental conditions and applied REE3+ concentrations in parent solutions (Table 1). There are mainly four different procedures by which REE partition coefficients with calcite are determined:

Fig. 1
figure1

Compilation of distribution coefficients Di and ki of REE3+ in partitioning with calcite. a experimental results; b derived from analyses of limestone (Parekh et al. 1977), Mg-calcite cements of reefs (Scherer and Seitz 1980), and averages of biogenic carbonates of various coral species (Sholkovitz and Shen 1995; Agaki et al. 2004; Wyndam et al. 2004), all related to REE3+ in modern seawater

Table 1 Compilation of methods applied in determinations of REE partition coefficients
  1. 1.

    REE in diagenetic marine carbonates and reefal microbialites are related to REE in seawater (Fig. 1a). Parekh et al. (1977) extrapolated the coprecipitated fraction of REE in plots of REE in limestone samples versus their REE in associated acid insoluble residue. The derived apparent DREE values decrease from 1388 (La) to 464 (Lu). Scherer and Seitz (1980) analyzed calcitic cements from coral reefs of the Bahamas with about 15 mol% MgCO3. After oxidation of the organic matter by H2O2 for 24 h, the acid insoluble residue was determined. With the help of these residues, the individual, total REE abundance in carbonates was corrected and related to individual [REEi] in modern seawater yielding DREE values between 120 and 530 for La and Sm, respectively. The trend of average DREE values of 296 ± 30 for Heron microbialites, Great Barrier Reef, Australia (Webb and Kamber 2000) and 212–256 (except Ce with 327) in carboniferous to quaternary limestones from Japan (Toyama and Terakado 2019) resemble those reported by Scherer and Seitz (1980). After ultrasonically removing of Fe–Mn coatings in a reducing bath, Palmer (1985) determined REE abundance in calcitic foraminiferal skeletons from the Atlantic. The removed coatings contained about 1000 times more REE than the remaining calcite skeletons with DREE values of 125 (La) and 73 (Yb).

  2. 2.

    Steady-state condition in suspension of 5 g of calcite seeds in 2 L of phosphate-cleaned seawater was achieved by bubbling a CO2/N2 mixture with pCO2 of 0.0031, additional stirring by glass propeller and constant addition of calcite-saturated solution containing the REE spike (Zhong and Mucci 1993, 1995). The determination of the quantity of overgrowth by chemical means was not easy because of recovering all calcite sticking to the walls of the reactor. Their reported logarithmic DREE values decrease from 3.6 to 1.9 for La and Yb, respectively (Fig. 1b). Tanaka and Kawabe (2006) precipitated calcite on seed crystals suspended in Ca2+–Na+ solution by bubbling N2 containing 1% of CO2 through the solution and operating a magnetic stirrer chip in order to yield a homogeneous overgrowth on calcite seeds. Their initial REY concentrations ranged from 10 ppb in general and 20 ppb for Pr, Sm, Tb and Tm. The calcite overgrowth was derived from charge and mass balances. The developed log(DREE) values cover a range between 2.5 and 3.6 with a broad maximum of the intermediate REE (Fig. 1b). The uncertainty of DREE values between the extreme runs is about a factor of 3.7. Voigt et al. (2017) reported log(DREE) values of runs with either La or Yb and with both elements together. Using the constant addition technique, the experiments were performed under 1 atm CO2, pH 6–6.4 and variable amounts of seeds. Log(DREE) decreases with both increasing log(REE) and log(Ω − 1) (Ω = calcite saturation index) in solution indicating an inhibiting effect of REE on the growth of calcite.

  3. 3.

    An evaporation technique (no stirring) under constant addition of mother solution and spike was applied by Toyama and Terakado (2014). In a pre-phase, calcite seeds were grown on movable silica glass plates. In these experiments, the initial volume of the calcite-saturated solution with 15.6 g NaCl/l and REE spike was maintained by refilling the reactor. The overgrowth on calcite seeds was determined by electronical weighing of the plates. The calcite growth was exclusively diffusion-controlled, i.e., [Ca] and [REE] decreased around the growing calcite crystals. Although the initial [REE] in runs A and B differed by a factor of 10, the final [REE] differed only by factors 2–3 (Fig. 2). Experiments A1 + A2 and B1 + B2 represent results after 122 and 37 h of calcite growth, respectively. Log(DREE) of light REE (LREE) and heavy REE and Y (HREY) decrease in runs A-1 and (A-2) from 25–10 and 65–25, and in runs (B-1) and (B-2) from 70–40 and 95–65, respectively.

    Fig. 2
    figure2

    Di versus equilibrated REEi concentrations showing different behaviors of REE in partitioning. Runs A and B show two time intervals in solutions differing in initial REE3+ concentrations by a factor of 10. Data are taken from Toyama and Terakado (2014)

  4. 4.

    CO2 exsolution from a bicarbonate solution was applied by Terakado and Masuda (1988). According to the experimental procedure, Eq. (1) is used to quantify the coefficient kREE (Fig. 1b). The initial solution contained about 350 mg/l Ca. No seeds were applied. In different runs, they used a prepared spike solution of REE3+ covering a range of f = 0.2 to 7, where f is the multiplication factor of their standard spike composition that was added to the Ca(HCO3)2 solution. Although the individual REE concentrations in the initial solution vary between 40 and 0.9 ppb for Nd and Lu, respectively, the derived apparent kREE values differ between each f run but are almost similar within each f run for all REE (Fig. 3a). Their kREE values increase from f = 0.2 to f = 1 and then decrease with the further increase in REE abundance.

    Fig. 3
    figure3

    Correlations of data from Terakado and Masuda’s experiments (1988). a Distribution coefficients ki versus initial concentration of REEi. The dashed lines indicate the trends of all REE at the noted REE concentration level (f-factor; for details ref. to text). These trends indicate little specific differences within the series of REE in partitioning with calcite. b Saturation index SI of REE carbonates versus initial REE concentration show that only the very light REE are supersaturated in systems with f = 7 to 1. c Saturation index SI of REE carbonates versus distribution coefficient ki show variable trends of SI with increasing ki values for f = 7 to f = 1. For f = 0.2, the ki values are lower than for f = 7. The dashed lines with arrows indicate the trend of increasing individual SI values from f = 0.2 to f = 7

In the above reviewed work, the values of DREE or kREE depend on the state of calcite saturation (Voigt et al. 2017), growth rate of calcite (Zhong and Mucci 1995; Toyama and Terakado 2014; Voigt et al. 2017), salinity (Webb and Kamber 2000), concentration of REY (Terakado and Masuda 1988; Toyama and Terakado 2014), chemical complexation (Tanaka et al. 2004; Voigt et al. 2017), temperature, CO2 partial pressure, pH and performance of experiments.

Irrespective of the performance of REE partitioning during calcite precipitation, there are at least three important aspects affecting REY partitioning in calcite:

  • High REY concentrations induce precipitation of separate phases such as REY carbonates and hydroxides due to which REY abundance in solutions and consequently DREE values decrease;

  • Ion exchange of REY3+ against Ca2+ form variously composed surface compounds with different kinds of charge balance;

  • Chemical complexation in solutions.

The aim of this contribution is to search for a common process which could explain the wide spread of experimental partition coefficients DREE. Are REY really homogeneously distributed in calcite or do they agglomerate to flatspread or linear surface clusters which are then overgrown by calcite? The size of such compounds may show a strong dependence of partition coefficients on the sum of REY in solution because all REE and Y behave similarly.

An outlook on REY partitioning between alcite and seawater is given because one aspect of some published studies was to gain a deeper insight into the development of REY in seawater in deep time (Shields and Webb 2004; Tanaka et al. 2004; Tanaka and Kawabe 2006; Voigt et al. 2017; Toyama and Terakado 2019). Because calcite is omnipresent in the earth’s crust and preferentially precipitated from seawater, the partitioning of REY between calcite and its solution has also become a very important tool in hydrochemistry, where limestone aquifers play an important role (Johannesson et al. 1997; Möller et al. 2003; Siebert et al. 2014).

Interaction of REY with Calcite

Exchange of Mg2+ and REE3+ Against Ca2+ in Calcite Surface

Zhong and Mucci (1995) reported that REE concentrations immediately decreased after addition of the REE spike to the calcite suspension followed by a slow process (Fig. 4a). After this initial fast decrease in La and Yb concentration in solution (what they called: adsorption step), the further decrease of Yb is much less than of La with time. This difference in behavior may be due to differences in dehydration enthalpies which are less for the bigger La3+ than for the smaller Yb3+ favoring adsorption of La3+ but retarding the adsorption of Yb3+. About 25 and 40% of added Yb and La, respectively, is “adsorbed” causing high surface concentrations of REE. Except at thermodynamic equilibrium, the zeta potential of calcite is always negative (Moulin and Roques 2003) which promotes the adsorption REY3+ onto calcite surfaces.

Fig. 4
figure4

Exchange of Ca2+ in calcite surface against foreign ions. a Drop of REE concentration when adding the spike to the calcite seed suspension (Zhong and Mucci 1995); b exchange kinetic of Mg2+ against Ca2+ in calcite surface; c exchange of Mg2+ against Ca2+ in calcite surface as a function of Mg2+/Ca2+ in solution (Möller 1973; Möller and Sastri 1973; Möller and De Lucia 2019)

A similar kinetic behavior is reported for Mg2+ exchange against Ca2+ doped by radioactive 45Ca2+ in rhombohedral faces of calcite (Möller 1973) (Fig. 4b). With increasing Mg2+ in solution, 45Ca2+-doped Ca2+ in the calcite surface decreases. With increasing Mg2+/Ca2+ in solution, the Mg2+/Ca2+ in the calcite surface approach distinct ratios of 1 and 3 is indicated by significant changes in slopes (Fig. 4c). These ratios resemble those of the compositions of the minerals dolomite and huntite. The ratio of 1 suggests that Mg2+ and Ca2+ are either randomly distributed or are arranged in alternating lines of Ca2+ and Mg2+. Rhombohedral faces of calcite present lines of Ca2+ and CO32−. Thermodynamical estimates suggest that the arrangement of Mg2+ and Ca2+ in separate lines on rhombohedral surfaces of calcite has a minimum in free energy (Möller and Rajagopalan 1976). Using single crystals, it was shown that only about one molecular layer of calcite takes part in this type of ion exchange (Möller and Sastri 1974; Pokrovski and Sholkovitz 2001). The Mg2+ distribution in the calcite surface layer must have an effect on REY partitioning between calcite and seawater.

No specific studies of REY3+ exchange against Ca2+ in calcite surfaces are reported. Here the experience with REE3+ in groundwater may help out. The REY3+/Ca2+ values in groundwater from limestone aquifers are only about 2‰ of that in the dissolving calcite (Table 5; Fig. 5). Furthermore, [REY3+]/[Ca2+] values of seamount limestones are 102–104 times higher than their corresponding ratios in seawater (Tanaka et al. 2003; Miura et al. 2004; Toyama and Terakado 2019) indicating that during recrystallization REY from seawater are incorporated due to exchange against Ca2+. This process explains the high DREE values in limestones (Parekh et al. 1977) and disqualifies limestones as reliable reference material to derive DREE values in seawater carbonate systems.

Fig. 5
figure5

Relationship between REE in groundwater and limestone aquifer rocks (Möller and Siebert 2016). Note that the given ratios are similar, although limestones are from different geological periods (Avedat Group: Eocene; Judea Group: Cenomanian). For details refer to “Appendix 1

Charge balance

Substitution is maximum if the size of the foreign ion is comparable with the substituted Ca2+ in calcite leading to least lattice distortion. Thus, Na+ fits perfectly into Ca2+ position (Table 2). REY are either slightly larger or smaller than Ca2+. Secondly, the charge balance has to be achieved in the substitution process. There are different possibilities: associated substitution of 2 Ca2+ by REY3+ + Na+ (Eq. 3) and/or 3 Ca2+ by 2 REY3+ + blank space in cation lattice (Eq. 4)

$$2\left\{ {{\text{Ca}}^{2 + } } \right\} = \left\{ {{\text{REY}}^{3 + } + {\text{Na}}^{ + } } \right\}$$
(3)
$$3\left\{ {{\text{Ca}}^{2 + } } \right\} = \left\{ {2{\text{REY}}^{3 + } + \,\square } \right\}$$
(4)

□ blank space in the lattice.

Table 2 Ionic radii of species discussed in the text at coordination number VI (Shannon 1976)

In all reviewed experiments of partitioning of ΣREY between calcite and solutions, the concentrations of incorporated Na+ exceed by far REY3+ concentrations (Fig. 6). The excess Na+ amounts are suggested to be due to occupation of Na+ in crystal defects (White 1975; Busenberg and Plummer 1985; Lakstanov and Stipp 2004). Excess of Na+ in the lattice may also be compensated by substitution of CO32− by HCO3−.

Fig. 6
figure6

Cross-plots of log({Na+}/{Ca2+}) and log({ΣREE3+}/{Ca2+}) in calcite. Note that {Na+] exceeds by far {ΣREE3+}

Formation of REY carbonates

Minerals of REE and Y are either dominated by light REE, LREE or heavy REE and Y, HREY. LREE carbonates crystallize with 8 H2O (lanthanide: (La, Ce)2(CO3)3 × 8H2O). A similar HREY compound is unknown. HREY form carbonates such as tengerite (Y2(CO3)3 × 3H2O) and lokkaite (Ca, Y4(CO3)7 × 9H2O) (Cesbron 1989; Kim et al. 2018). In their experiments, Voigt et al. (2017) reported saturation states Ω of calcite and La-hydroxylbastnasite (La(OH)CO3) of 1 to 11 and − 1.5 to + 0.6, respectively. In any case, phases such as REY2(CO3)3, REY(OH)3 or REY(OH)CO3 may play a role in partitioning of REY.

Based on the initial concentrations in experimental solutions or seawater (Table 6), the saturation indices of REY carbonates and hydroxides in each experiment and in seawater are estimated (Table 7). SI values of REE hydroxides are all negative. The precipitation of REE carbonates (Fig. 3b, c) is mostly excluded by the authors of all the above-cited studies based on logarithms of solubility products, logKsp, of REE carbonates of Smith and Martell (1976) being about two orders of magnitude higher than the corresponding values of Spahiu and Bruno (1995). The initial SI of REE carbonate under conditions of the reaction solution are checked by PHREEQC with “llnl” database (Parkhurst and Appelo 2013) after implementation of Spahiu and Bruno’s data (Table 8), and results are summarized in Table 3.

Table 3 Results of estimated saturation indices SI with respect to REE carbonates and hydroxides

Often the less abundant REE and the very abundant Y are not determined in biogenic calcite and its diagenetic products. Particularly Y cannot be neglected in ΣREY. {Y} in calcite is approached by using [Y]/[Er] in seawater multiplied by [Er] in calcite. Other absent REY are determined in a similar way. REY partitioning in marine calcite depends on the composition of local seawater which is not always given by the authors. In these cases, REE in seawater reported by Sholkovitz and Schneider (1991) is used and Y is taken from the compilation of Bruland and Lohan (2003).

Following Table 3 (Table 7), in Toyama and Terakado’s (2014) and Tanaka and Kawabe’s (2006) experiments, all individual SI values of REE carbonates are negative. Under the conditions of Zhong and Mucci’s (1995) experiment, SI are positive for La–Sm carbonates. In Terakado and Masuda’s experiments (1988) ,SI of light REE2(CO3)3 the saturation indices in runs with f = 7 and 4 are positive for La, Ce and Nd. For f = 1, only Ce is positive and for f = 0.2 SI of all carbonates are negative.

Discussion

Different from solution without Mg2+, calcite from seawater environments is subjected to ion exchange of Mg2+ against Ca2+ in their surfaces (Sect. 2.1). In seawater, the Mg2+/Ca2+ values are about 5 and the surface ratio of {Mg2+}/{Ca2+} is about 1 (Fig. 4c). Thus, calcite surfaces expose only half of their theoretical surface Ca2+ in seawater. The minimum of free energy in the surface is obtained when the distribution of Ca2+ and Mg2+ resembles that in dolomite, i.e., alternating lines of Ca2+ and Mg2+ (Möller and Rajagopalan 1976). If such a surface structure is present, REY exchange only takes place in Ca2+ lines facing the solution. Thus, partitioning of REY between calcite and natural and artificial seawater can hardly be the same as in Mg2+-free systems.

Partitioning of individual REE

Except Ce, which often displays anomalous behavior because of oxidation to Ce(IV), REE seemingly behave alike in partitioning with respect to calcite (Terakado and Masuda 1988), irrespective of their actual concentrations in the fluid phase (Fig. 3a). Although the concentrations of La and Nd differ from Eu by factors of about 30 in the initial solution of these experiments, their derived kREE values are comparable for all REE in each experiment defined by f. The f-dependent changes of REY partitioning give evidence of different processes. Starting with the highest concentration of REE (f = 7), kREE values increase with decreasing REE concentration (f = 4 and 1) achieving maximum at about f = 1. This increase suggests that decreasing density of adsorbed REE3+ avoids nucleation of REY carbonates being separated from the surface. Indeed, LREE are supersaturated with respect to REE carbonates (Fig. 3b, c). The lowest kREE values are obtained at f = 0.2. Contrasting these results are those of Toyama and Terakado (2014) in which the initial differences of REE concentrations by a factor of 10 are not reflected in DREE values (Fig. 2). Although the input of REE in each run was constant over time, the resultant DREE values decreased from LREE to HREE, i.e., significant fractionation of REE3+ occurred. The fractionation of REE is similar in both runs. La does not show the highest coefficients in runs A1 and B1. Because DREE values depend on the degree of calcite saturation (Terakado and Masuda 1988; Voigt et al. 2017), the enforced growth of calcite seems to override the process of equilibration of REE between solution and adsorption onto surfaces and place changes across the surfaces until the exchange with Ca2+ occurs.

The values of {REEi}/{Ca2+} are derived from reported DREE,i values multiplied by corresponding [REEi]/[Ca] values according to Eq. (2). In the double logarithmic plot of {REEi}/{Ca} versus [REE]/[Ca] two possibly linear, subparallel relationships evolve (Fig. 7). The solid line (Eq. 5a) characterizes Mg2+-free systems based on Toyama and Terakado’s (2014) and Voigt’s et al. (2017) results. The average of eight experiments of Tanaka and Kawabe (2006) does not fit Eq. (5a). The dashed line (Eq. 6a) is based on results of Mg2+-dominated solutions such as seawater (Zhong and Mucci 1995; Parekh et al. 1977; Scherer and Seitz 1980; Palmer 1985; Toyama and Terakado 2019).

Fig. 7
figure7

Correlations between log({La3+}/{Ca2+}) in calcite as functions of either [REYi]/[Ca] or [REYi3+]/[Ca2+] and between log({ΣREYi}/{Ca}) as functions of either [ΣREY]/[Ca] or [ΣREYi3+]/[Ca2+]. Note that the slopes in the double logarithmic plots of a, c, or b, d are nearly the same. Any homogeneous partitioning should be indicated by a slope of n = 1

Using the dissolved species REY3+ and Ca2+ instead of concentrations of REY and Ca correlations (7a) and (8a) evolve (Fig. 7b). The overall fit of all reported values including the average of Tanaka and Kawabe (2006) is better than in Fig. 7a. Contrasting the total concentration of individual REEi, the dissolved REEi3+ species yield trend lines that seem to merge at low REY concentrations with the trend line representing partitioning between calcite and seawater (Fig. 7b).

Partition of the Entirety of REY

Although it is known that REY substitute each other in minerals, it is still common practice to consider the individual REE3+ and not the entirety of all REY as one “species” in partitioning between calcite and solutions. For instance, the individual log(DLa) and log(DYb) are slightly higher than those derived from mixtures of both elements (Voigt et al. 2017).

Equations (9a) and (12a) in Fig. 7c and d describe the correlation of {ΣREY}/{Ca} and either [ΣREY]/[Ca] or [ΣREYi3+]/[Ca2+], respectively. Note that Eqs. (9a) and (10a) resemble Eqs. (5a) and (6a), and Eqs. (11a) and (12a) resemble Eqs. (7a) and (8a). There is, however, a significant difference in using either total concentrations or dissolved species. Using the dissolved species, the resulting regression lines seemingly merge at very low concentrations of REY. The different slopes in Fig. 7 give evidence of the influence of Mg2+ on the incorporation of REY. The pre-factors are significantly smaller in the absence of Mg2+ than in its presence.

Partition Coefficients as Functions of REY Concentrations in Solution

Dividing Eqs. (5a)–(12a) by the correspondent ratios of either REY and Ca or REY3+ and Ca2+ in solution, the REY partition coefficients are obtained as functions of their corresponding ratios [Eqs. (5b)–(12b) in Table 4]. The resultant DREY values as function of the ratios of REY and Ca yield subparallel trends for DREY values in seawater and in Mg2+-free solutions (Fig. 8a). A different result is obtained for DREY values, if the tervalent species in solution are considered. DREY in seawater increases with REY, whereas DREY in Mg2+-free solution decreases with increasing REY (Fig. 8b).

Table 4 Compilation of regression lines in Fig. 7 and the derived trend lines of REY partition coefficients between, calcite and ambient solutions
Fig. 8
figure8

Correlations of log(DREY) and log(DLa) and REY in aqueous phases. The corresponding functions of D are taken from Table 4. Note the correspondence of log D when related to either ΣREY3+ or La3+, whereas in Mg2+-free systems different trend lines evolve

Which is the best representation of the behavior of REY in partitioning? The plots of tervalent dissolved species of REYi3+ are more reliable because Tanaka and Kawabe’s data plot along the regression lines [Eqs. (7a) and (11a) (Fig. 7b and 11b)]. Equation (7a) is seemingly the best representation in terms of linear regression line, whereas Eq. (11a) could also be fitted by a curve.

REE partitioning in calcite and aragonite in seawater

The evaluation of DREY values in marine carbonates has to consider that, independently of actually measured REE species, all REY are present in calcite.

The marine calcite and cleaned limestones cluster at log{La}/{Ca} of about − 5.5 to − 7 when plotted either against REYi or ΣREYi. Limestones and cements of corals are of diagenetic origin, i.e., recrystallization under exchange of seawater. Microbialites show enhanced REYi taken up during their recrystallization (Scherer and Seitz 1980; Wyndam et al. 2004). The foraminifera of Palmer are very high in REY which may be caused by exchange with their highly enriched REY of their coatings.

For comparison, aragonites from corals plot below log{La}/{Ca} = − 7.5. The corals from Bermuda reefs (Sholkovitz and Shen 1995), the Great Barrier Reef of Australia (Wyndam et al. 2004; Webb and Kamber 2000) and various coral species from Okinawa, Japan (Agaki et al. 2004), show species-dependent DREY between 0.6 and 5. Their growth is mediated by biogenic processes with insignificant fractionation of REY. For instance, {REE}/{Ca} of modern corals resembles [RΕΕ]/[Ca] in seawater (Sholkovitz and Shen 1995; Agaki et al. 2004; Wyndam et al. 2004).

Surface Processes Influencing Partitioning of REY

The regression lines of the marine calcite and the results of Zhong and Mucci in artificial seawater reveal enhanced data of log{La3+}/{Ca2+} compared with experimental results in the absence of Mg2+ (Figs. 7, 8). The slopes of these regression lines exceed unity (Fig. 7) or zero (Fig. 8), which is unexpected for homogeneous partitioning after Eq. (2). Based on total concentrations, the resulting partition coefficients increase with either increasing [REYi3+]/[Ca2+] and [ΣREYi3+]/[Ca2+] in solution. Contrasting this result, the slope in Mg2+-free systems is less than unity, when using dissolved species (Fig. 8b). Thus, the question arises, why does {REYi}/{Ca} and DREY increase in the presence of Mg2+-bearing solution and why does the ratio decrease in the absence of Mg2+ in Fig. 8b, whereas in both systems DREY increases when related to increasing total concentrations (Fig. 8a)?

In Mg2+-free solutions, the first step is adsorption of REY onto the surface of calcite. Moving across the surface, the adsorbed REY may come across already exchanged REY3+ for Ca2+ in the surface layer. Due to distortion of the anion layer, its exchange for a neighboring Ca2+ is favored, hence a linear structure of cluster starts growing as shown for Mg2+ exchange in calcite surfaces (Möller and Rajagopalan 1976). With the growth of calcite, large amounts of Ca2+ have to be adsorbed and some of them may replace REY in lattice sites of calcite surface. Thus, the {REY}/{Ca} value in the surface layer that will be overgrown by calcite loses some REYi.

In the presence of Mg2+, REY3+ exchange against Ca2+ only occurs in remaining Ca2+ lines, which, together with associated CO32-, dominate about 50% of the calcite surface in seawater. The exchange of REY against Mg2+ is unlikely because of the great difference in ionic ratios (Table 2). Along with growth of calcite, almost all Mg2+ has to be substituted by Ca2+, a process during which also REY3+ may be incorporated particularly because of their enhanced charge. Compared to a homogeneous distribution of REY on calcite surface in Mg2+-free solution, REY are enriched during growth of calcite. Each line or flatspread surface cluster consists of n lines presenting 2 or 2n sites for ongoing ion exchange, respectively (Fig. 9). The tendency to form surface clusters depends on the change of reaction free energy in the surface of calcite. Loss of free energy is higher for HREY3+ than for LREE3+ because the former are smaller than Ca2+ ions (Table 2). Once clusters formed, the enthalpy for removing a REE from a cluster is enhanced compared to removal of an isolated REY3+. These clusters seemingly build at REY concentrations in solutions much below the solubility products of REY carbonates. Na+ and REY3+ are probably placed near to each other. These assemblages correspond to REY incorporation in either line or surface clusters of the average composition of {REY–Na-(CO3)2} as suggested by Tanaka and Kawabe (2006). Voigt et al. (2017) suggested {REY(OH)(CO3)2}. Any homogeneous distribution is only achieved when the concentration of REY3+ in the calcite surface is extremely low keeping them clearly separated during growth of calcite. Although the saturation index for ΣREY carbonates in seawater is − 7.5 (Table 7), small REY clusters may still form (Fig. 9). The formation of clusters is the source of high enrichment of REY in growing calcite.

Fig. 9
figure9

Schematic arrangement of Ca2+, Na+, REY3+ in either line or surface clusters in a rhombohedral cleavage surface of calcite

The scatter in Fig. 7 may be caused by different processes: (1) The natural material was not clean enough and thus inappropriate to be used for determination of DREY coefficients and/or (2) the biogenic-sourced calcite differs from inorganically precipitated low magnesian calcite by enhanced REY3+ abundances in this material and this enhancement can be species-dependent. REE + Y in seawater do not form REY2(CO3)3, but the less soluble phosphates may be precipitated (Spahiu and Bruno 1995) and may be enclosed in growing calcite. For instance, log(Ksp) of LaPO4 is − 40.01, i.e., much lower than for La carbonate. REY–phosphate clusters may also be present in biogenic carbonates. Microbialites show enhanced REY taken up during their recrystallization (Scherer and Seitz 1980; Wyndam et al. 2004). The foraminifera of Palmer are very high in REY which may be caused by exchange with their highly enriched REY of their coatings.

Homogeneous distribution of REY3+ in calcite surfaces is only possible under extremely low [ΣREY3+]/[Ca2+] in aqueous systems and would require much lower concentrations than ΣREY3+ in seawater.

Conclusions

A critical re-evaluation of REY partitioning coefficients with respect to calcite reveals that the reported, wide-spread experimental DREY values reflect that two processes have been overlooked.

In the absence of Mg2+, the whole calcite surface is accessible for REY3+ exchange against Ca2+. The result of this exchange is reduced under the influence of continuing overgrowth of the next calcite layer. This leads to sub-proportional correlation of REY between the aqueous phase and the bulk of calcite.

The Mg2+ ion exchange against Ca2+ in calcite surface layers interfere with the exchange of REY3+ against Ca2+. All rhombohedral faces of calcite show a composition of Mg2+/Ca2+ of about 1 in seawater. Thus, only half of the theoretical numbers of Ca2+ ions are accessible for REY exchange against Ca2+. REY are slightly concentrated in these remaining Ca2+ lines. The growth of calcite requests that most of the Mg2+ has to be removed and substituted by Ca2+ and REY3+. REY3+ may be enriched because of their enhanced charge. These processes together may explain any over-proportional relationship of REY/Ca between the bulk of calcite and solution. Because REY partitioning in limestone is thought to be a key in understanding REY development in seawater, the effect of the presence of Mg2+ has to be considered.

Two different trend lines evolve: one for Mg2+ free systems and the other for artificial and natural seawater. Because of subtle exchange processes, the sum of all REY evidence that REY/Ca in solution are not linearly correlated with {ΣREY}/{Ca} in the bulk of calcite as expected by the Henderson and Kracek rule. It seems that REY form clusters in the surface of growing calcite, even if the solubility product of REY carbonates is not reached.

References

  1. Agaki T, Hashimoto Y, Fu FF, Tsuno H, Tao H, Yl Nakano (2004) Variation of the distribution coefficients of rare earth elements in modern coral-lattices: species and site dependence. Geochim Cosmochim Acta 68:2265–2273

  2. Bau M, Dulski P (1995) Evolution of yttrium–holmium systematics of seawater through time. Min. Mg. 58A:61–62

  3. Bruland KW, Lohan MC (2003) Controls of trace metals in seawater. In: Holland HD, Turekian KK (eds) Treatise on geochemistry, vol 6. Elsevier, Amsterdam, pp 23–47

  4. Busenberg E, Plummer LN (1985) Kinetics and thermodynamic factors controlling the distribution of SO42− and Na+ in calcites and selected aragonites. Geochim Cosmochim Acta 49:713–725

  5. Cesbron F (1989) Mineralogy of rare-earth elements. In: Möller P, Cerny P, Saupe F (eds) Lanthanides, tantalum and niobium. Springer, Berlin, pp 3–26

  6. Doener HA, Hoskins WM (1925) Co-precipitation of radium and barium sulfates. J Amer Chem Soc 47:662–675

  7. Henderson LM, Kracek FC (1927) The fractional precipitation of barium and radium chromates. Am Chem Soc 49:738–749

  8. Johannesson KH, Stezenbach KJ, Hodge VF (1997) Rare earth elements as geochemical tracers of regional groundwater mixing. Geochim Cosmochim Acta 61:3605–3618

  9. Kim P, Anderko A, Navrotzki A, Riman RE (2018) Trends in structure and thermodynamic properties of normal rare earth carbonates and rare earth hydroxycarbonates. Minerals. https://doi.org/10.3390/min8030106

  10. Lakstanov LZ, Stipp SLS (2004) Experimental study of europium(III) coprecipitation with calcite. Geochim Cosmochim Acta 68:819–827

  11. Miura N, Asahara Y, Kawabe I (2004) Rare earth element and Sr isotopic study of the Middle Perminan limestone-dolostone sequence in Kuzuu area, central Japan: seawater tetrad effect and Sr isotopic signature of seamount-type carbonate rocks. J Earth Planet Sci Nagoya Univ 51:11–35

  12. Möller P (1973) Determination of the composition of surface layers of calcite in solutions containing Mg2+. J Inorg Nucl Chem 35:395–401

  13. Möller P, De Lucia M (2019) The impact of Mg2+ ions on equilibration of Mg–Ca carbonates in groundwater and brines. http://eartharxiv.org/az39t. https://doi.org/10.31233/osf.io/az39t

  14. Möller P, Rajagopalan G (1976) Changes of excess free energies in the crystal growth process of calcite and aragonite due to presence of Mg2+ ions in solution. Z Physik. Chem NF 99:187–198

  15. Möller P, Sastri CS (1973) Exchange studies on single crystals of calcite. Inorg Nucl Chem Lett 9:759–763

  16. Möller P, Sastri CS (1974) Estimation of the number of surface layers of calcite involved in Ca–45Ca isotopic exchange with solution. Zt Physik Chem NF 89:80–87

  17. Möller P, Sastri CS (2016) Cycling of calcite and hydrous metal oxides and chemical changes of major elements and REE chemistry in monomictic hardwater lake: impact on sedimentation. Chemie der Erde 76:133–148

  18. Möller P, Rosenthal E, Dulski P, Geyer S, Guttman J (2003) Rare earths and yttrium hydrostratigraphy along the lake Kinneret–Dead Sea–Arava transform fault, Israel and adjoining territories. Appl Geochem 18:1613–1623

  19. Moulin P, Roques H (2003) Zeta potential measurements of calcium carbonate. J Colloid Interface Sci 261:115–126

  20. Palmer MR (1985) Rare earth elements in foraminifera tests. Earth Planet Sci Lett 73:285–298

  21. Parekh PP, Möller P, Dulski P, Bausch WM (1977) Distribution of trace elements between carbonate and non-carbonate phases of limestone. Earth Planet Sci Lett 34:39–50

  22. Parkhurst DL, Appelo CAJ (2013) Description of input and examples for PHREEQC version 3 - A computer program for speciation, batch-reaction, one-dimensional transport, and inverse geochemical calculations. U.S. Geological Survey Techniques and Methods, book 6, chap. A43, p 497. https://pubs.usgs.gov/tm/06/a43/. Accessed 02 Nov 2020

  23. Pokrovski OS, Sholkovitz J (2001) Kinetics and mechanism of dolomite dissolution in neutral to alkaline solutions revisited. Am J Sci 301:597–626

  24. Scherer M, Seitz H (1980) Rare earth element distribution in holocene and pleistocene corals and their redistribution during diagenesis. Chem Geol 28:279–289

  25. Shannon RD (1976) Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides. Acta Crystallogr A 32:751–767

  26. Shields GA, Webb GE (2004) Has the REE composition of seawater changed over geological times? Chem Geol 204:103–107

  27. Sholkovitz ER, Schneider DL (1991) Cerium redox cycles and rare earth elements in the Saragasso Sea. Geochim Cosmochim Acta 55:2737–2743

  28. Sholkovitz ER, Shen GT (1995) The incorporation of rare earth elements in modern coral. Geochim Cosmochim Acta 59:2749–2756

  29. Siebert C, Möller P, Geyer S, Kraushaar S, Dulki P, Guttman J, Subah A, Rödiger T (2014) Thermal waters in the Lower Yarmouk Gorge and their relation to surrounding aquifers. Chemie der Erde/Geochem 74:425–441

  30. Smith RM, Martell AE (1976) Critical stability constants: inorganic complexes, vol 4. Plenum Press, New York

  31. Spahiu K, Bruno J (1995) A selected thermodynamic database for REE to be used in HLNM performance assessment exercises. MBT Technologia Ambiental, Cerdanyola, Spain Technical Report 95-35; available through Swedish Nuclear Fuel and Waste Management CO, Stockholmn

  32. Tanaka K, Kawabe I (2006) REE abundance in ancient seawater inferred from marine limestones and experimental REE partition coefficients between calcite and aqueous solution. Geochem J 40:425–435

  33. Tanaka K, Miura N, Asahara Y, Kawabe I (2003) Rare earth element and strontium isotopic study of seamount-type limestone in mesozoic accretionary complex of southern Chichibu Terrane, central Japan: implication for incorporation process of seawater REE into limestones. Geochem J 37:163–180

  34. Tanaka K, Ohta A, Kawabe I (2004) Experimental REE partitioning between calcite and aqueous solutions at 25 °C and 1 atm: constraints on the incorporation of seawater REE into seamount-type limestones. Geochem J 69:103–110

  35. Terakado Y, Masuda A (1988) The coprecipitation of rare-earth elements with calcite and aragonite. Chem Geol 69:103–110

  36. Toyama K, Terakado Y (2014) Experimental study of rare earth element partitioning between calcite and sodium chloride solution at room temperature and pressure. Geochem J 48:463–477

  37. Toyama K, Terakado Y (2019) Estimation of the practical partitiom coefficients of rare earth elements between limestone and seawater: discussion and application. Geochem J 53:139–150

  38. Voigt M, Mavromatis V, Oelkers EH (2017) The experimental determination of REE partition coefficients in water-calcite system. Chem Geol 462:30–43

  39. Webb GE, Kamber BS (2000) Rare earth elements in Holocene reefal microbialites: a new shallow seawater proxy. Geochim Cosmochim Acta 64:1557–1565

  40. White AF (1975) Sodium and potassium coprecipitation in calcium carbonates. Ph.D. dissertation, Northwestern University, Evaston, IL, USA

  41. Wyndam T, McCulloch M, Fallon S, Alibert C (2004) High-resolution coral records of rare earth elements on coastal seawater: biochemical cycling and a new environment proxy. Geochim Cosmochim Acta 68:2067–2080

  42. Zhong S, Mucci A (1993) Calcite precipitation in seawater using a constant addition technique: a new overall reaction kinetic expression. Geochim Cosmochim Acta 57:1409–1417

  43. Zhong S, Mucci A (1995) Partitioning of rare earth elements (REEs) between calcite and seawater solutions at 25 °C and 1 atm, and high dissolved REE concentrations. Geochim Cosmochim Acta 59:443–453

Download references

Acknowledgements

Open Access funding provided by Projekt DEAL. The authors greatly acknowledged the comments of two anonymous reviewers which encouraged us to improve the manuscript.

Author information

Correspondence to Peter Möller.

Additional information

Publisher's Note

Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Appendices

Appendix 1: SI of Individual and the Entirety of REE Carbonates

Behavior of REY3+ in dissolution of limestone in groundwater. Only a few ‰ of released REY3+ remain in solution (Table 5).

Table 5 Relationship between {REY3 +}/{Ca2 +} in limestones and [REY3 +]/[Ca2 +] in groundwater. Both localities are located in Israel. Avedat group = Eocene; Judea group = upper cretaceous. Data are taken from Möller and Siebert (2016)

Appendix 2

Compilation of the initial concentrations in experimental solutions is compiled in Table 6.

Table 6 Analyses of initial solution in coprecipitation experiments

The logarithms of individual activities, log(aREE3+), log(aCO32−) and log(aOH) are estimated using PHREEQC with “lln” database (Table 7). From these data, the individual log(IAPi) is estimated after Eq. (5) and the results are compiled in Table 7. Using the corresponding log(Ksp,i) (Table 6), the individual saturation indices are calculated after Eq. (6). Results are tabulated in the lower part of Table 7.

$$\log ({\text{IAP}}_{i} ) = \log ({}^{{\text{a}}} {\text{REE}}^{3 + } ) \times 2 + \log ({}^{{\text{a}}} {\text{CO}}^{32 - } ) \times 3$$
(5)
$${\text{SI}}_{{i{{\text{-carb}}}}} = \log ({\text{IAP}}_{i} ) - \log (K_{{{\text{sp}},i}} + \log ({}^{{\text{a}}} {\text{REE}}_{i}^{3 + } ) - \log (\varSigma^{{\text{a}}} {\text{REE}}^{3 + } ))$$
(6)

Index i refers to the REE3+ involved in the experiment.

Table 7 Compilation of data necessary for estimating individual SI of REY carbonates and the approach of the corresponding SIΣREY of the entirety of REY

To estimate the saturation indices of the entirety of REE carbonates, the respective log(IAPcarb) and log(Ksp, ΣREY) are estimated after Eqs. (7) and (8). This activity product can hardly be lower than Ksp of La but could be higher than Ksp of Lu.

Dealing with the entirety of REY is limited by the unawareness of the corresponding solubility product of the whole suite, logKsp,ΣREY, a value that cannot be determined and is therefore approximated by the sum of individual Ksp weighted by the corresponding activity fraction of REY3+ species in solution (Table 7). SI values of the entirety of REY carbonates are approximated in Table 7, in which log(IAPΣREY) of REY carbonates are estimated from log(ΣaREY3+) and log(aCO32−) obtained by PHREEQC and its “llnl” database (Parkhurst and Appelo 2013). Log(IAPΣREY) of the entirety of REE carbonates is given by (log(aΣREY3+)×2 + 3×log(aCO32−). The derived values of SIΣREY = log(IAPΣREY) − log(Ksp,ΣREY) of the ΣREY carbonate are given in detail in Table 7 and are summarized in Table 3. The entirety of REY carbonates is supersaturated in Terakado and Masuda’s and Zhong and Mucci’s experiments.

$$\log \left( {{\text{IAP}}\varSigma_{{\text{REY}}} } \right) = \log (\varSigma^{{\text{a}}} {\text{REE}}^{3 + } \times 2 + \log \left( {^{{\text{a}}} {\text{CO}}_{3}^{2 - } } \right) \times 3$$
(7)
$$K_{{\text{sp,REY}}} = \varSigma \left( {K_{{{\text{sp}},i}} \times \left[ {^{{\text{a}}} {\text{REE}}_{i}^{3 + } } \right]/\left[ {\varSigma^{{\text{a}}} {\text{REE}}_{i}^{3 + } } \right]} \right)$$
(8)

The saturation indices SI for ΣREE carbonate, SIΣREY, follow from Eq. (9). The positive SIΣREY of the ΣαREE3+ is highlighted in the lower part of Table 7.

$${\text{SI}}_{{\varSigma {\text{REY}}}} = \log ({\text{IAP}}_{{\varSigma {\text{REY}}}} ) - \log (K_{\text{sp}} ,)$$
(9)

Appendix 3

See Table 8.

Table 8 Log Ksp of individual REE carbonate and hydroxides (Spahiu and Bruno 1995)

Rights and permissions

Open Access This article is licensed under a Creative Commons Attribution 4.0 International License, which permits use, sharing, adaptation, distribution and reproduction in any medium or format, as long as you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons licence, and indicate if changes were made. The images or other third party material in this article are included in the article's Creative Commons licence, unless indicated otherwise in a credit line to the material. If material is not included in the article's Creative Commons licence and your intended use is not permitted by statutory regulation or exceeds the permitted use, you will need to obtain permission directly from the copyright holder. To view a copy of this licence, visit http://creativecommons.org/licenses/by/4.0/.

Reprints and Permissions

About this article

Verify currency and authenticity via CrossMark

Cite this article

Möller, P., De Lucia, M. Incorporation of Rare Earths and Yttrium in Calcite: A Critical Re-evaluation. Aquat Geochem (2020). https://doi.org/10.1007/s10498-020-09369-9

Download citation

Keywords

  • Partitioning of rare earths with calcite
  • Formation of REY–Na carbonate compounds
  • Homogeneous partitioning
  • Individual versus entirety of rare earths’ partitioning between calcite and ambient solution