Acta Mineralogica-Petrographica, Abstract Series 5, Szeged, 2006<strong>THE</strong> PROTON: A CATION LIKE <strong>THE</strong> O<strong>THE</strong>RS <strong>IN</strong> ROCK-FORM<strong>IN</strong>G <strong>M<strong>IN</strong>ERAL</strong>SROBERT, J.-L.ISTO, UMR 6113, CNRS-Université d’Orléans, 45071 Orléans Cedex 2, France and IMPMC, UMR 7590, CNRS-UniversitésParis VI, Paris VII, IPG, 140 rue de Lourmel, 75015 Paris, FranceE-mail: jlrobert@cnrs-orleans.frIn hydrous rock-forming minerals, the hydroxyl hydrogenand the hydroxyl oxygen are usually considered as a wholeand permanent entity, i.e. the hydroxyl group, which acts as amonovalent anion within the structure. The reality is morecomplicated and more interesting, since the hydroxyl protonleads its life independently. Depending on the local chargebalances, the hydroxyl group can be considered as a pointcharge or as dipole in which oxygen and hydrogen play adifferent role, since hydrogen is able to share a part of itscharge with surrounding oxygens, usually the underbondedoxygens of adjacent tetrahedra.The properties of the OH group (O–H distance and resultingO–H stretching and bending wavenumbers) closely reflectthe local variations of crystal-chemical properties in themineral structure: charge distributions, and distances. Anexamination of these properties allow a careful description ofthe crystal-chemical landscape around the proton, up to thefifth cationic neighbour in favourable cases, and a predictionof many geochemical properties of H-bearing rock-formingphases.The main factor controlling these properties is the nature(bulk charge, electronegativity) of the first cationicneighbours. The higher the bulk charge carried by the immediatelyadjacent cations, the weaker the O–H bond within thehydroxyl group. Contrary to a commonly accepted idea, theorientation of the OH dipole is not the main factor controllingthese properties. An example is given by the comparisonbetween talc Mg 3 Si 4 O 10 (OH) 2 , a trioctahedral 2:1 layer silicate,with the OH dipole bonded to Mg 3 and perpendicular to(001), and pyrophyllite, (Al 2 )Si 4 O 10 (OH) 2 ( stands for anoctahedral vacancy), with the OH group adjacent to Al 2 and strongly tilted towards (001). The resulting OH bondstrength is the same in talc and pyrophyllite, as shown by thesimilarity between their OH-stretching wavenumbers (3676 ±1 cm –1 ). As long as the local charge balance around the OHgroup remains constant, the bond strength within the OHgroup and the resulting OH-stretching wavenumber remainconstant, whatever the mineral family. It is interesting to notethat the trioctahedral OH group in the tetrasilicic magnesiummica K(Mg 2.5 0.5 )Si 4 O 10 (OH) 2 , in richterite, a clinoamphibole,(K,Na)(NaCa)Mg 5 Si 8 O 22 (OH) 2 , and the inner OH-groupin dravite, a tourmaline, NaMg 3 Al 6 (BO 3 ) 3 (Si 6 O 18 )(OH)(OH) 3 ,have the same OH-stretching wavenumber, 3735 cm –1 , withinexperimental uncertainties. In these there major silicate families,the OH group is bonded to Mg 3 and point towards analkaline cation, in the middle of a ring of six SiO 4 tetrahedra,which can be summarised as follows: Mg 3 -OH → (6SiO 4 )-A +(with A + = Na + or K + ).A decrease of the local charge carried by the first adjacentcations raises the O–H bond strength and consequently theOH-stretching wavenumber, up to 3755 cm –1 , the highestvalue known in any compound under room conditions, observedin tainiolite K(Mg 2 Li)Si 4 O 10 (OH) 2 . By contrast, as thebulk charge carried by the first cationic neighbours increases,for example Mg 2 Al or Al 2 Li, the OH-stretching wavenumberdrops to values around or below 3650 cm –1 , indicating that apart of the proton charge is shared with surrounding oxygens.This is observed in all mineral families.Heterovalent cationic substitutions in octahedral sites adjacentto the OH-group are generally coupled with replacementsin other polyhedra, e.g. the tetrahedral sites, the interlayerspace in layer silicates, the pseudo-cubic antiprism M4site in amphiboles, the second, third, …, neighbours, must beconsidered.Using selected synthetic minerals allows to determine therespective influence of all substitutions, up to the fifth cationicneighbouring sites in favourable cases, through a carefulanalysis of the perturbations induced on the OH group. In thisway, it is possible to assign all observed OH vibrations to apeculiar environment, and then to deduce local order-disorderrelations around the hydroxyl proton.The influence of the A + cation can be analysed using A + -bearing and A + -free minerals. For example, the influence ofK + on hydroxyl properties can be deduced from the comparisonbetween talc [Mg 3 –OH → (6SiO 4 )] and the trioctahedralOH of the tetrasilicic Mg mica [Mg 3 –OH → (6SiO 4 )–K]. Theshift induced by K + facing the OH group is +59 cm –1 . A similarvalue is observed in amphiboles, for example betweentremolite Ca 2 Mg 5 Si 8 O 22 (OH) 2 and richteriteA + (NaCa)Mg 5 Si 8 O 22 (OH) 2 , and in tourmalines, Mg-foitite(Mg 2 Al) Al 6 (BO 3 ) 3 (Si 6 O 18 )(OH)(OH) 3 , compared to draviteNaMg 3 Al 6 (BO 3 ) 3 (Si 6 O 18 )(OH)(OH) 3 . Increasing the charge ofthe cation facing the hydroxyl group raises the OH-stretchingwavenumber, as observed along the phlogopiteKMg 3 (Si 3 Al)O 10 (OH) 2 –kinoshitalite BaMg 3 (Si 2 Al 2 )O 10 (OH) 2join, where the K + /Ba 2+ substitution provokes a shift of +20cm –1 in the OH-stretching wavenumber. The tilting of the OHgroup towards (001) in dioctahedral phases withdraws thisinteraction, as shown by the comparison between muscoviteor paragonite A + (Al 2 )(Si 3 Al)O 10 (OH) 2 , with A + = K + andNa + , respectively, and phlogopite KMg 3 (Si 3 Al)O 10 (OH) 2 .Contrary to a commonly accepted belief, the effect of theorientation of the OH group on the exchange properties ofclay minerals is practically negligible, since the interlayerwater molecules act as a screen between the hydroxyl protonand the compensating cation, and there is almost no interactionbetween them even in the case of trioctahedral smectites,like saponites. As a matter of fact, in one-layer high-chargesaponites, the OH-stretching wavenumber is only 3682 cm –1 ,e.g. very close to that of talc, a 2:1 layer silicate withoutinterlayer compensating cation. Therefore, in smectites, onlythe charge location and the charge value have an influence onexchange properties, and the behaviours of the dioctahedralbeidellites and trioctahedral saponites, both with tetrahedralcharge, on one side, and of the dioctahedral montmorillonitesand the trioctahedral hectorites, both with octahedral charge,102www.sci.u-szeged.hu/asvanytan/acta.htm
Acta Mineralogica-Petrographica, Abstract Series 5, Szeged, 2006on the other side, are similar provided that the layer charge isthe same.The properties of the OH-group also allow to investigatethe tetrahedral cationic distributions (mainly Si, Al), since theOH … O interactions depend on the charge balance on surroundingoxygens, i.e. the oxygens of tetrahedra. A carefulquantitative investigation of OH-stretching band intensitiesfor different first neighbours (octahedral), and secondneighbours (tetrahedral) shows that the Si, Al distributionsare generally not ordered, but follow a homogeneous chargedistribution pattern, in agreement with high-resolution NMRdata. Considering the influence of second cationic neighbourseffects (i.e. tetrahedrally coordinated cations), on band positionsand band intensities, leads to conclude that in manycases the extinction coefficients are constant, which allowquantitative determinations of cationic distributions aroundthe hydroxyl proton.The method is sensitive enough to enlight long distanceeffects, even for subtle substitutions like Ca 2+ /Mg 2+ at M4sites in clinoamphiboles along the tremoliteCa 2 Mg 5 Si 8 O 22 (OH) 2 –cummingtonite Mg 7 Si 8 O 22 (OH) 2join, or Na + /Li + along the ferri-clinoferroholmquistiteLi 2 Fe 2+ 3Fe 3+ 2Si 8 O 22 (OH) 2 –riebeckiteNa 2 Fe 2+ 3Fe 3+ 2Si 8 O 22 (OH) 2 series. Owing to the distances,these long-range effects are not direct. They are inducedthrough the structure by the propagation of tiny distortionsrequired by local charge balance requirements.In addition to this role of privileged observer, the protonH + frequently plays a key role in many situations. Deprotonationin the case of in situ oxidation of a variable chargecation, i.e. Fe 2+ → Fe 3+ , in biotites, hornblendes, and so, noprotonation when high cation (Mn 3+ , Ti 4+ ) are incorporated tocrystal structures, in micas like norrishiteK(Mn 3+ 2Li)Si 4 O 10 O 2 and many high-Ti phlogopites, or amphiboleslike ungarettiite NaNa 2 (Mn 2+ 2Mn 3+ 3)Si 8 O 22 O 2 , obertiiteNaNa 2 (Mg 3 Fe 3+ Ti)Si 8 O 22 O 2 and dellaventuraiteNaNa 2 (MgMn 3+ 2LiTi) Si 8 O 22 O 2 . Additional protonations arealso known in hydrous minerals, for example in partiallydioctahedral micas with a tetrahedrally coordinated cation,Be 2+ , Mg 2+ , Ni 2+ or Co 2+ , or in clinoamphiboles (richterites),with Li + replacing Ca 2+ at the M4 site.The approach is also very useful for identifying unusualcoordinations for cations, for example [4] M 2+ in micas and inamphiboles like joesmithite, PbCa 2 Mg 5 (Si 6 Be 2 )O 22 (OH) 2 , or[4] B 3+ in high pressure olenite (a tourmaline)NaAl 3 Al 6 (BO 3 ) 3 (Si 3 B 3 O 18 )(OH)(OH) 3 .The interactions of the hydroxyl proton with theneighbouring oxygens, influenced by the charge distributionsand the distances, also control the possible OH – /F – exchangeproperties, whatever the fluorine activity in the environment.When the hydroxyl proton has no or little interactions with itsneighbours, it acts as a point charge in the structure and theOH – /F – is easy. It is the case in most trioctahedral layer silicates,in all amphiboles and at the inner OH – site of tourmalines.By contrast, if the hydroxyl proton is involved in H-bonds with surrounding oxygens, its replacement by fluorineis more energetically difficult, and becomes impossible ifOH … O bonds are strong. It is why dioctahedral layer silicatesdo not trap much fluorine, and why outer hydroxyl groupscannot be replaced by fluorine in tourmalines.www.sci.u-szeged.hu/asvanytan/acta.htm 103
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