Mn-bearing purplish-red tourmaline from the Anjanabonoina pegmatite, Madagascar

Abstract A gem-quality purplish-red tourmaline sample of alleged liddicoatitic composition from the Anjanabonoina pegmatite, Madagascar, has been fully characterised using a multi-analytical approach to define its crystal-chemical identity. Single-crystal X-ray diffraction, chemical and spectroscopic analysis resulted in the formula: X(Na0.41□0.35Ca0.24)Σ1.00Y(Al1.81Li1.00Fe3+0.04Mn3+0.02Mn2+0.12Ti0.004)Σ3.00ZAl6 [T(Si5.60B0.40)Σ6.00O18] (BO3)3 (OH)3 W[(OH)0.50F0.13O0.37]Σ1.00 which corresponds to the tourmaline species elbaite having the typical space group R3m and relatively small unit-cell dimensions, a = 15.7935(4) Å, c = 7.0860(2) Å and V = 7.0860(2) Å3. Optical absorption spectroscopy showed that the purplish-red colour is caused by minor amounts of Mn3+ (Mn2O3 = 0.20 wt.%). Thermal treatment in air up to 750°C strongly intensified the colour of the sample due to the oxidation of all Mn2+ to Mn3+ (Mn2O3 up to 1.21 wt.%). Based on infrared and Raman data, a crystal-chemical model regarding the electrostatic interaction between the X cation and W anion, and involving the Y cations as well, is proposed to explain the absence or rarity of the mineral species ‘liddicoatite’.

The general chemical formula of tourmaline can be written as: XY 3 Z 6 T 6 O 18 (BO 3 ) 3 V 3 W, where X = Na, K, Ca and □ (= vacancy); Y = Al, Cr, V, Fe, Mg, Mn, Zn, Cu, Li and Ti; Z = Al, Cr, V, Fe and Mg; T = Si, Al and B 3+ ; B = B 3+ ; V = (OH) and O; and W = (OH), F and O. Note that the non-italicised letters X, Y, Z and B represent groups of cations hosted at the [9] X, [6] Y, [6] Z, [4] T and [3] B crystallographic sites (letters italicised). The letters V and W represent groups of anions accommodated at the [3] O3 and [3] O1 crystallographic sites, respectively. The H atoms occupy the H3 and H1 sites, which are related to O3 and O1, respectively. The dominance of specific ions at one or more sites of the structure gives rise to a range of distinct mineral species.
Tourmaline-supergroup minerals are currently classified into three groups, vacant, alkali and calcic, based on the X-site occupancy . The X-site occupancy is usually related to both paragenesis and crystallisation conditions of the host rock, and these relations may be used to reconstruct the host-rock thermal and chemical history (e.g. Henry and Dutrow, 1996;van Hinsberg et al., 2011a,b;Dutrow and Henry, 2018;Bosi et al., 2018Bosi et al., , 2019cAhmadi et al., 2019). A further level of classification into subgroups is based on charge arrangements at the Y and Z sites. Tourmalines are also distinguished by the dominant anion at the W position of the general formula into hydroxy-, fluorand oxy-species.
Tourmaline is also one of the most important gem materials on the market today, particularly renowned for its spectrum of colours: from colourless, through red, pink, yellow, orange, green, blue and violet, to brown and black (Pezzotta and Laurs, 2011). The transition elements (Ti, V, Cr, Fe, Mn and Cu) are often invoked as colour-causing agents. Red tourmalines are commonly given the varietal name 'rubellite', which refers to tourmalines with colours ranging from rose, dark pink to purplish red, but do correspond to several regular mineral species: elbaite, fluor-elbaite, rossmanite, fluor-liddicoatite (Pezzotta and Laurs, 2011) and oxy-dravite .
Specifically, fluor-liddicoatite was redetermined and renamed in 2011 by the Subcommittee on Tourmaline Nomenclature of the International Mineralogical Association's Commission on New Minerals, Nomenclature and Classification (IMA-CNMNC) when the nomenclature of tourmaline-supergroup minerals was reconsidered  and the 'liddicoatite' from the Antandrokomby type locality (Dunn et al., 1977;Aurisicchio et al., 1999;Webber, 2002;Dirlam et al., 2002;Ertl et al., 2006; regained proper attention. Note that with the renaming of the type material as fluorliddicoatite, the hydroxy species 'liddicoatite' is no longer properly defined as a species. A new type material definition is necessary to re-establish the name. Two gem-quality samples of purplish-red prismatic crystals of alleged 'liddicoatite' on quartz matrix from the collection of M.E. Ciriotti (MEC) were analysed with a Jeol JSM IT300LV scanning electron microscope (SEM) and energy dispersive X-ray spectroscopy (EDS) (University of Turin, Earth Sciences Department) to verify if they were F-dominant species. Although B and Li were not measured, both samples were determined to be F-dominant and were classified as fluor-liddicoatite. A small portion of a further alleged 'liddicoatite' sample (presented as 'probed' liddicoatite by its seller) in quartz-rhodizite matrix from Antandrokomby localities (the same type of purplish-red crystals are shown in the specimen in Fig. 1) was obtained by MEC, courtesy of the new owner. The sample was analysed through SEM-EDS and surprisingly showed no trace of F; in addition, its composition did not fit 'liddicoatite' in terms of Na and Ca.
In the present study, such a tourmaline sample from the Anjanabonoina pegmatite, central Madagascar, has been fully characterised by X-ray single-crystal diffraction, electron microprobe analysis, laser induced breakdown spectroscopy, micro-Raman, infrared and optical absorption spectroscopy, with the aim of defining its crystal-chemical identity and species.
The Anjanabonoina aplite-pegmatite field is situated in the Neoproterozoic Itrembo Group, which consists of a lower unit of gneisses and an upper unit of quartzites, schists and marbles (Pezzotta and Franchi, 1997;Fernandez et al., 2001). The pegmatites were emplaced in a complex geological environment, perhaps at the contact between the lower and upper unit. The gem-bearing pegmatites postdate the main tectonic phase and, therefore, are thought to have intruded during a late phase of the magmatic cycle about 490 Ma (Paquette and Nédélec, 1998). The Li-Cs-Ta (with minor Nb-Y-F) aplite-pegmatite field extends for ∼2.5 km. The veins are 2 to 12 m thick and large parts are kaolinised feldspars and/or deeply weathered (De Vito, 2002a,b).
More details about the history of the 1500s to 2000s explorations and mining of the Malagasy tourmaline gem deposits can be found in Strunz (1979), Pezzotta (1999) and Dirlam et al. (2002).

Thermal treatment
In order to study potential dehydration and redox effects, two oriented and polished crystals were heat treated in air at 700°C (20 h) and 750°C (90 h). These thermal conditions have previously been shown to be sufficient to impose changes in Fe redox states and intracrystalline cation distribution (e.g. Filip et al., 2012;Bosi et al., 2016a,b). The 55 and 309 μm thick samples were placed in a gold container and inserted in a preheated horizontal tube furnace equipped with a quartz-glass tube. The experiments were ended by pushing the sample container out to the cold zone of the quartz tube, which caused the sample to cool to room temperature within one minute. A distinct increase in colour intensity appeared after heat treatment, as shown in Fig. 2. Minor cracks appeared in the thicker sample after treatment at the higher temperature.

Single-crystal structure refinement (SREF)
A representative crystal fragment of the purplish-red tourmaline from Madagascar was selected for X-ray diffraction measurements on a Bruker KAPPA APEX-II single-crystal diffractometer (Sapienza University of Rome, Earth Sciences Department), equipped with a charge-coupled device (CCD) area detector (6.2 cm × 6.2 cm active detection area, 512 × 512 pixels) and a graphite-crystal monochromator using MoKα radiation from a fine-focus sealed X-ray tube. The sample-to-detector distance was 4 cm. A total of 3577 exposures (step = 0.2°, time/step = 20 s) covering a full reciprocal sphere with a redundancy of ∼12 was collected. Final unit-cell parameters were refined using the Bruker AXS SAINT program on reflections with I > 10 σ(I ) in the range 5°< 2θ < 78°. The intensity data were processed and corrected for Lorentz, polarisation and background effects using the APEX2 software program of Bruker AXS. The data were corrected for absorption using a multi-scan method (SADABS, Bruker AXS). The absorption correction led to an improvement in R int (from 0.033 to 0.027). No violation of R3m symmetry was detected.
Structure refinement was done using the SHELXL-2013 program (Sheldrick, 2015). Starting coordinates were taken from . Variable parameters were scale factor, extinction coefficient, atom coordinates, site-scattering values (for X, Y and Z sites) and atomic-displacement factors. Attempts to refine the extinction coefficient yielded values within its standard uncertainty, thus it was not refined. Neutral scattering factors were used for the cations and oxygen atoms. As for the atomic model refinement and in accordance with the chemical analysis results (see below), the X site was modelled by setting the vacancy content to 0.32 atoms per formula unit (apfu) and allowing the remainder of the site to refine as Ca = (0.65 -Na). Similarly, the Y site was refined by setting the (Mn+Fe) occupancy to 0.19 apfu and allowing the remainder of the site to refine as Al = (2.81 -Li) apfu. The T site was modelled by Si versus B. The Z, B and anion sites were modelled with Al, B and O scattering factors, respectively, and with a fixed occupancy of 1 as refinement with unconstrained occupancies showed no significant deviations from this value. A final refinement was then performed by modelling the site occupancy of the O1 site with O and F fixed to the value obtained from the empirical formula (see below). Similar chemical constraints were applied to refine the H1 and H3 sites. There were no correlations greater than 0.7 between the parameters at the end of the refinement. Table 1 lists crystal data, data-collection information and refinement details; Table 2 gives the fractional atom coordinates  Notes: R int = merging residual value; R 1 = discrepancy index, calculated from F-data; wR 2 = weighted discrepancy index, calculated from F 2 data; GooF = goodness of fit; Diff. Peaks = maximum and minimum residual electron density. and equivalent isotropic displacement parameters; Table 3 shows selected bond lengths. A Supplementary Table with anisotropic displacement parameters and a crystallographic information file have been deposited with the Principal Editor of Mineralogical Magazine and are available as Supplementary material (see below).

Micro-laser induced breakdown spectroscopy (μ-LIBS)
Lithium analysis, carried out on a representative sample fragment, was performed using a double pulse Q-Switched (Nd-YAG, λ = 1064 nm) laser with a 1 μs delay between the two pulses with an energy of 110 mJ per pulse. The small spot size (7-10 μm) was obtained using a petrographic optical microscope (objective lens 10X NA 0.25 WD 14.75 mm). The LIBS spectra were acquired by an AvaSpec Fiber Optic Spectrometer (390-900 nm with 0.3 nm resolution) with a delay of 2 μs after the second pulse and an integration time of 1 ms. The main problem regarding Li quantification by LIBS concerns the self-absorption of the emission line used to extract quantitative data. In the present tourmaline, the quantitative data were obtained from linear regression using the main Li emission line intensity (I Li = 670.706 nm, corresponding to the resonance transition 1s 2 2s > 1s 2 2p) in the range from 0.009 to 2.04 wt.% of Li 2 O. In this regard, we verified that the selfabsorption effect of this specific line was negligible in the studied concentration range, hence, not affecting the measurements. This is consistent with previous studies on beryl (McMillan et al., 2006;Tempesta and Agrosì, 2016;Tempesta et al., 2020). Moreover, the     (Table 4). It can be noted that μ-LIBS represents a very proficient localised analytical method, in particular if LIBS is mounted to a microscope to achieve a micrometric scale resolution. The intense emissivity of Li in optical emission spectroscopy makes the LIBS technique advantageous for Li quantification. Moreover, the potential of LIBS for Li analysis of geological materials at the micrometric scale has been validated in previous studies (Fabre et al., 2002;Sweetapple and Tassios, 2015;McMillan et al., 2018).

Micro-Raman spectroscopy
Raman spectra of the Mn 3+ -bearing red tourmaline were obtained using a micro/macro Jobin Yvon Mod. LabRam HRVIS (University of Turin, Interdepartmental Centre "G. Scansetti"), equipped with a motorised x-y stage and an Olympus microscope. The back-scattered Raman signal was collected with a 50× objective and the Raman spectrum was obtained for a 90°(perpendicular to c) oriented crystal. The 632.8 nm line of an He-Ne laser was used as excitation; laser power (20 mW) was controlled by means of a series of density filters. The minimum lateral and depth resolution was set to a few μm. The system was calibrated using the 520.6 cm -1 Raman band of silicon before each experimental session. The spectra were collected with a multiple and repeated acquisition (5) with single counting times of 50 seconds to improve the signal-to-noise ratio. The incident excitation light was scrambled to eliminate orientation and polarisation effects. The spectrum was recorded from 100 to 4000 cm -1 using the LabSpec 5 software package (Horiba Jobin Yvon GmbH, 2004, 2005. Band-component analysis was undertaken using a Lorentzian function (Fityk software package; Wojdyr, 2010). The intensity of the vibrational modes was proven to be very dependent on the polarisability tensor. The Raman spectrum of the present sample in the spectral region of the framework and (OH)-stretching vibrations is shown in Fig. 4.

Fourier-transform infrared (FTIR) spectroscopy
Polarised Fourier-transform infrared spectra were measured on two doubly polished single-crystal sections oriented by means of optical microscopy, and with thicknesses of 55 and 309 μm.
The spectrometer system consisted of a Bruker Vertex 70 spectrometer equipped with a halogen-lamp source and a CaF 2 beam-splitter coupled to a Hyperion 2000 microscope with a ZnSe wire-grid polariser and an InSb detector. Spectra were measured before and after heat-treatment experiments over the wavenumber range 2000-15,000 cm −1 with a resolution of 2 or 8 cm −1 . The measuring areas were masked by a 50-100 μm rectangular aperture to avoid cracks and inclusions. The FTIR spectra of the untreated and treated samples (e.g. Fig. 5) show typical, strongly pleochroic absorption bands in the (OH)-stretching region (3300-3800 cm -1 ), including bands above ∼3600 cm -1 that demonstrate the presence of W (OH) (see below).

Optical absorption spectroscopy (OAS)
Polarised, room temperature optical absorption spectra in the range 30,000-12,500 cm -1 (333-800 nm) were recorded at a spectral resolution of 1 nm on the same 309 μm thick section studied by FTIR spectroscopy, using an AVASPEC-ULS2048 × 16 spectrometer attached via a 400 μm ultraviolet (UV) optical fibre cable to a Zeiss Axiotron UV-microscope. A 75 W Xenon arc lamp was used as a light source, and Zeiss Ultrafluar 10× lenses served as objective and condenser. The diameter of the circular aperture was 50 μm for the untreated sample and 30 μm for the treated sample. A UV-quality Glan-Thompson prism with a working range from 40,000 to 3704 cm −1 (250 to 2700 nm) was used as a polariser. The wavelength scale of the spectrometer was calibrated against Ho 2 O 3 -doped and Pr 2 O 3 /Nd 2 O 3 -doped standards (Hellma glass filters 666F1 and 666F7). Spectral data in the range 12,150-2000 cm -1 (800-5000 nm) was taken from the FTIR measurements.
The optical absorption spectra of the untreated sample (Fig. 6) at energies below the UV-absorption edge show a set of broad absorption bands at 21,950, 19,800, ∼18,000, 13,500 and ∼9500 cm -1 (corresponding to 456, 505, 556, 741 and 1053 nm). In addition, a very weak and sharp absorption band occurs at 24,330 cm -1 (418 nm), and a set of very sharp, overlapping bands are recorded in the NIR spectral range between 6700-7200 cm -1 (1492-1389 nm). The absorption bands recorded in spectra of the untreated sample at 24,330, 21,950 and ∼18,000 cm -1 are more intense for light polarised perpendicular to the crystallographic c-axis. Conversely, the absorption band 19800 cm -1 is only observed as a broad shoulder in the E||c-spectrum. The set of sharp bands between 6700-7200 cm -1 is also completely E||c-polarised.    The absorption spectra recorded on the heat-treated sample (Fig. 6) display comparable features to those observed in the spectra of the natural sample. However, all absorption bands at 21,950, 19,800, ∼18,000, 13,500 and ∼9500 cm -1 show pronounced intensity gains, and the set of sharp absorption bands between 6700-7200 cm -1 distinctly decreases in intensity.

Determination of atomic fractions
For the untreated sample, manganese oxidation state was determined by OAS (see below and Table 4). All Fe was considered to be Fe 3+ based on the OAS results and Mn and Fe redox potential arguments. Lithium was determined by μ-LIBS. Regarding the B 3+ , the SREF data indicate that it fully occupies the B site, but relatively small amounts of B 3+ also occur at the T site: T-m.a.n. = 13.24(7) and <T-O> = 1.613 Å are in fact significantly smaller than the expected value for a T site fully occupied by Si ( T Si-m.a.n. = 14 and < T Si-O> = 1.619 ± 0.001 Å; , reflecting the presence of cations lighter and smaller than Si, such as B 3+ (Ertl et al., 2018). As a result, the B 2 O 3 and (OH) content were calculated by charge balance with the assumption (T + Y + Z + B) = 18.00 apfu and 31 anions.
For the heat-treated sample, all Mn was considered as Mn 3+ (i.e. Mn 2 O 3 = 1.21 wt.%), in conformity with the heat treatment conditions and the redox reaction:

Determination of site population and mineral formula
The anion site populations in the samples studied follow the general preference suggested for tourmaline (e.g. : the O3 site (V position in the general formula) is occupied by (OH) -, while the O1 site (W position in the general formula) can be occupied by O 2-, (OH)and F -. The refined Z-site scattering and <Z-O> values (13 and 1.906 Å, respectively) are the typical values observed for a Z site fully occupied by Al  The bond-valence analysis is consistent with the proposed site populations (Table 5) As for the treated sample, the following ordered formula is proposed: (OH). For formula electroneutrality reasons, the valency-imposed double site-occupancy for the Y site is required with an atomic arrangement (Li 1.5 Al 1.5 ) Σ6+ . In accordance with the tourmaline nomenclature and the IMA-CNMNC rules Bosi et al., 2019a,b), the present sample can be classified as Mn-bearing elbaite, Na(Li 1.5 Al 1.5 )Al 6 Si 6 O 18 (BO 3 ) 3 (OH) 3 OH.

Micro-Raman spectroscopy in the framework vibration region
In accordance with the studies of Mihailova et al. (1996), Reddy et al. (2007), McKeown (2008 and Watenphul et al. (2016b), five main ranges of framework vibrations can be identified in the Raman spectrum of the untreated sample (Fig. 4) and attributed to the following vibrating groups. (1) The range ∼200-300 cm -1 is dominated by YO 6 vibrations; in particular, the band at ∼274 cm -1 corresponds to the Mn-O bond, previously observed in a pink-tourmaline by Reddy et al. (2007). (2) The range ∼300-400 cm -1 (the strongest Raman peak) is generated by ZO 6 vibrations, in particular the sharp peak at 377 cm -1 may be given by the Z Al-O bond. (3) The range ∼500-750 cm -1 is dominated by breathing modes of bridging oxygen atoms of TO 4 rings.
With regard to the region of the (OH)-stretching vibrations (3300-3800 cm -1 ), the Raman scattering peaks of the untreated sample show wavenumbers similar to those of the infrared absorption bands (cf. Fig. 4 with Fig. 5); thus, the (OH)-stretching modes are discussed below. Note: Weighted bond valence according to Bosi (2014). Bond valence parameters from Brown and Altermatt (1985). a Expected mean atomic valence (or formal charge) from the empirical formula.

FTIR spectra in the (OH)-stretching region and band assignment
Infrared spectra of the untreated and treated samples recorded in polarised mode parallel to the c-axis direction display a very intense absorption feature in the 3400-3600 cm -1 region, which is truncated due to excessive absorption (Fig. 5). This problem is commonly encountered in polarised transmission spectra of tourmaline single crystals, and it is normally not possible to thin samples sufficiently to get this main band 'on scale'. Bands of lower intensity occur on both the low-energy (ca. 3340 cm -1 ) and high-energy (3650, 3665 and 3703 cm -1 ) sides of the major absorption band. Spectra polarised perpendicular to the c-axis direction (E⊥c) show a set of bands with substantially lower intensities (Fig. 5). The spectral range that is obscured by excessive absorption in the E||c direction displays here the presence of three bands at wavenumbers 3464, 3540 and 3597 cm -1 , indicating (OH)-dipoles aligned close to, but with a small inclination to the c-axis (Gatta et al., 2014). After thermal treatment, a number of changes can be observed in the FTIR spectra: the sharp band at 3665 cm -1 progressively decreases in intensity and almost disappears in the E||c direction (Fig. 7), whereas a new band appears at 3395 cm -1 , visible in the E⊥c direction (Fig. 8). The (OH) bands in the overtone region ( Fig. 9) show a distinct decrease in absorption intensity, amounting to 17±3% as estimated from spectral fitting. However, a general decrease in absorption band intensity is not observed in the principal (OH)-region in spectra of the heat-treated samples polarised in the E⊥c direction. Instead, we observe a weak increase in intensity, probably related to a decrease in polarisation efficiency due to microcracks and other crystal imperfections formed during heat treatment, leading to minor contributions from the extremely intense absorbance in the E||c direction.
The main difference between the FTIR spectra of the untreated and treated sample occurs in gradual decrease in the intensity of the band at 3665 cm -1 and the appearance of the band at 3395 cm -1 with the increase in temperature up to 750°C. As a result, these bands, in particular that at 3665 cm -1 , may be correlated directly with the decreased Mn 2+ and increased Mn 3+ content, according to the redox reaction (1), reported in the section 'Determination of atomic fractions'. However, it appears that (OH) is also lost by mechanisms other than the redox reaction. Only a partial loss of 0.12 (OH) apfu can be coupled to the oxidation of Mn 2+ , whereas the total (OH) loss as estimated from the decrease of (OH) overtone intensities (17 ± 3%) corresponds to ca. 0.6 (OH) apfu. The reason for this additional dehydration is unknown, but may be related to initial breakdown processes of the crystal structure.
Of particular interest is also the association of the O1 (OH) stretching modes with the X-site constituents: the bands between ∼3600-3700 cm -1 are considered associated with X □, whereas those above 3700 cm -1 are considered associated with X Na + . This distinction is related to the repulsive electrostatic interaction between the X n+ cation and H + of the O1 (OH) group, which reinforces the strength of the O1 O-H bond, shifting the (OH)-stretching mode towards higher wavenumbers (e.g. Gonzalez-Carreño et al., 1988;Berryman et al., 2016;Watenphul et al., 2016a). Consequently, the presence of X Na + determines an electrostatic repulsion with H1 H + along the crystallographic c-axis, whereas the substitution X □ → X Na + removes such a repulsion (Fig. 10). From the energetic-stability viewpoint, the rossmanite type arrangements (YYY)-O1 (OH)-X (□) should hence be more likely to occur than the elbaite type arrangement (YYY)-O1 (OH)-X (Na). The X n+ -H + repulsion effect will be stronger with the substitution X Ca 2+ → X Na + . On the other hand, this cation-cation repulsion can be removed by the chemical substitution O1 F -→ O1 (OH)or the deprotonation process O1 (OH) -+ ¼ O 2 (g) → O1 O 2-+ ½ H 2 O(g), both of which would favour the occurrence of fluor-liddicoatite and darrellhenryite type arrangements (YYY)-O1 (O,F)-X (Na,Ca).

Optical spectra
With the exception of the broad absorption band at ∼9500 cm -1 , the characteristics (band energy, band width and polarisation) of all observed bands in the spectra of the present sample are in very good agreement with those recorded for Mn 3+ -bearing tourmaline specimens (Reinitz and Rossman, 1988;Ertl et al., 2005;Novák et al., 2013;Bosi et al., 2017a). In agreement with these previously published studies we assign bands at 21,950, 19,800, ∼18,000, 13,500 cm -1 to electronic transitions in octahedrally coordinated Mn 3+ and the very weak and sharp band at 24,330 cm -1 to an electronic transition in octahedrally coordinated Mn 2+ . The set of strongly E||c-polarised, sharp bands in the Fig. 10. Simplified structure of tourmaline showing the relative positions of H1, H3, O1, O3 and X with respect to Y, Z and the ring of tetrahedra TO 4 . Of particular interest is the strong interaction between X and H1 (distance ≈2.21 Å) and the very weak interaction between X and H3 (distance ≈3.65 Å).
NIR region between 6700-7200 cm -1 are due to overtones of the fundamental (OH)-stretching modes.
Based on the intensity of the Mn 3+ band at ∼18,000 cm -1 in the spectrum perpendicular to the c-axes (Fig. 6) in combination with the published molar absorption coefficient for that absorption band (Reinitz and Rossman, 1988), we calculate an Mn 2 O 3 content of ∼1 wt.%. However, the strong intensity increase by a factor of ∼4× for this band in spectra of our heat-treated sample, in combination with the analysed MnO tot content, strongly suggests that the absorption coefficient for the band is somewhat higher than that indicated by Reinitz and Rossman (1988). Assuming that all Mn 2+ was oxidised to Mn 3+ during the heat treatment of our sample we determine an absorption coefficient of ∼30 l mole -1 cm -1 , compared to the value of ∼7.5 suggested by Reintitz and Rossman (1988). Based on this revised absorption coefficient we calculate a Mn 2 O 3 content of ∼0.2 wt.% for the untreated sample.
In view of the limited set of transition metals (Mn, Fe and Ti) in the present tourmaline, the number of potential origins for the broad absorption band recorded at ∼9500 cm -1 is very limited as well. The broadness of this band and its relatively high intensity exclude that it is caused by electron transitions in Mn 2+ or Fe 3+ , which all give rise to much weaker and also sharper spinforbidden absorption bands. Furthermore, redox potential arguments exclude the presence of Fe 2+ in a Mn 3+ -bearing substance. Finally, Ti 4+ is not a chromophore and Ti 3+ is also excluded on the basis of redox potential considerations. Consequently, there remain only transitions in Mn 3+ as a cause for the ∼9500 cm -1 band. This assignment is in agreement with observations of a broad Mn 3+ -related absorption band at ∼1040 nm (corresponding to ∼9615 cm -1 ) in optical spectra of oxidised Mn 2+ -rich elbaite (Ertl et al., 2012). It is also in agreement with the observed increase in band intensity on heat treatment (oxidation) of the present sample. The relatively low energy of this band offers two main alternative assignment schemes. Firstly, low-energy bands caused by transitions in Mn 3+ are frequently observed in spectra of substances, in which the cation is at the centre of octahedra that are characterised by one or two metal-ligand bonds deviating strongly from the remaining ones, either by being considerably shorter or longer (Burns, 1993). Secondly, transitions in tetrahedrally coordinated [4] Mn 3+ may also give rise to spectral bands of relatively low energy, as shown by a broad absorption band at 10,800 cm -1 in spectra of [4] Mn 3+ -doped spinel . The observed intensity increase for the ∼9500 cm -1 band in response to heat treatment, i.e. oxidation, represents a strong argument against this second suggestion, as this would require Mn 2+ to be located initially at the tetrahedrally coordinated sites of tourmaline, which is highly unlikely (Bačík and Fridrichová, 2020). Furthermore, the SREF results provides no indications for [4] Mn 3+ and consequently we prefer the suggestion that the band is caused by a transition in Mn 3+ cations at octahedrally coordinated sites, where the local electronic field around the cation is strongly distorted from the O h symmetry.