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Eprints ID: 8619
To link to this article:
DOI:10.1016/j.electacta.2011.12.039
http://dx.doi.org/10.1016/j.electacta.2011.12.039
To cite this version:
Bieber, Anne-Laure and Massot, Laurent and Gibilaro, Mathieu and Cassayre,
Laurent and Taxil, Pierre and Chamelot, Pierre Silicon electrodeposition in
molten fluorides. (2011) Electrochimica Acta, vol. 62 . pp. 282-289. ISSN
0013-4686
Silicon
electrodeposition
in
molten
fluorides
A.L.
Bieber, L.
Massot
∗, M.
Gibilaro, L.
Cassayre, P.
Taxil, P.
Chamelot
UniversitédeToulouse;INPT,UPS,CNRS;LaboratoiredeGénieChimique;118RoutedeNarbonne,F-31062Toulouse,France
Keywords: Instantaneousnucleation Silicon Electrodeposition Moltenfluorides Chronoamperometry
a
b
s
t
r
a
c
t
SiliconnucleationprocesswasinvestigatedinmoltenNaF–KF(40–60mol%)onsilverelectrodesinthe 820–950◦Ctemperaturerangeinordertooptimizesiliconcoatingoperatingconditions.
Chronoam-perometricmeasurementsevidencedthatsiliconelectrodepositionprocessinvolvedaninstantaneous nucleationwithdiffusion-controllednucleigrowthwhatevertemperatureandSi(IV)ionsconcentration inthemixture.Theoverpotentialandtemperatureinfluenceonnucleationsitesnumberwasalsostudied. Silicondepositswereobtainedusingthesametemperaturerangeasnucleationstudy,fordifferent currentdensitiesonsubstrates:Ni,Ag,CgraphiteandCvitreous.Asensitiveinfluenceofthecathodicsubstrate
onthedepositadherenceandroughnesswasobservedanddiscussed.
1. Introduction
Photovoltaictechnologyisemergingasamajorsourceof electri-calenergy[1],andthemostcommonbasematerialforphotovoltaic cell issolargradesilicon (SoG-Si).Duetoa constantlygrowing demandforSoG-Si,thedevelopmentofnewprocessesallowing theproductionofcheapSoG-Siisamainissueforthesolarenergy industry.
Inthe1980s,siliconelectrodepositioninmoltensaltshasbeen consideredasanattractiveoptionforSoG-Siproduction[2].Indeed, siliconmetalismorereductivethanhydrogenmeaningthatsilicon electrodepositionhastobecarriedoutinnon-aqueouselectrolytes suchasalkalimetalhalides.However,noelectrolyticSiproduction processhas foundcommercialapplicationuptonow. Consider-ing more recent concernsabout carbon-freeenergy production andgrowingneedsforSoG-Si,suchkindofprocessisnevertheless beingreassessed,and,forthatpurpose,basicinvestigationsonthe saltsproperties,Si(IV)reductionmechanismandsilicondeposition strategiesareneeded.
In the frameof a production route basedon electrorefining (eitherfromMG–SiorfromSicuttingremains[3]),itwasdecidedto focusontheelectrodepositionprocessofdissolvedSi(IV)inmolten fluoride.Themainobjectivewastoevaluatethefeasibilityofsuch reactionandtoprovideanacademicstudyoftheSi(IV)reduction reaction,thankstospecificelectrochemicaltechniques[4,5].Atthis
∗ Correspondingauthor.Tel.:+33561558194;fax:+33561556139.
E-mailaddress:massot@chimie.ups-tlse.fr(L.Massot).
pointof thestudy,thepurityof theobtaineddepositswasnot consideredasanissue.
Itwasshown,inapreviouswork[6],thatthevolatilityofSi(IV) compoundsgreatlydependsonthenatureofthefluoridemixture. TheNaF–KFeutecticmixture,whichhighlystabilizesSi(IV) com-pounds,wasthusselectedastheelectrolyteforthepresentstudy. Thearticledescribesanextstageinthepreparationofsilicon layersforsolarenergywhichisthedemonstrationofthe electrol-ysistechniquevalidityinmoltensaltstechniquetorecoverpure silicononacathode.
Forthispurpose,thenucleationprocessandthesiliconnuclei growthonsilverareinvestigated usingcyclicvoltammetryand chronoamperometryandtheseresultsarecomparedwithsuitable models[4,7]inordertostatewhetherthenucleationis instanta-neousorprogressive.Meanwhile,theovervoltageandtemperature influenceonthe nucleation mode and nucleation sitesnumber wereexamined. Then,silicondepositionrunswerecarriedwith variouselectrode substrates(Ni, Ag, Cgraphite andCvitreous),
cur-rentdensities (−20 to−200mAcm−2 range) and temperatures
(820–900◦Crange).Theinfluenceofeachparameteronthe
coat-ingadherenceandroughnesswasobservedbyscanningelectron microscopy(SEM).
2. Experimental
2.1. Cell
Thecellwasavitreouscarboncrucibleplacedinacylindrical vesselmadeofrefractorysteelandclosedbyastainlesssteellid cooledbycirculatingwater.Thedescriptionofthiscellhasbeen
detailedinpreviouswork[8].Theexperimentswereperformed underaninertargonatmosphere(Linde).Thecellwasheatedusing aprogrammablefurnaceandthetemperaturewasmeasuredusing achromel–alumelthermocouple.
The electrolytic bath consisted of the NaF–KF (40–60mol%) eutectic mixture (Carlo Erba 99.995%). As mentioned earlier, the choice of this specificsolvent was based on its stabilizing properties regarding to the volatility of Si(IV) compounds [6]. Themixturewasinitiallydehydratedbyheatingundervacuum (7×10−2mbar)fromambienttemperatureuptoitsmeltingpoint
duringone week.Silicon ionswereintroducedintothebathin theformofsodiumhexafluorosilicateNa2SiF6(AlfaAesar99.99%)
powder.
2.2. Electrodes
Silver wires (1mm diameter), vitreous and graphite car-bon rods (3mm diameter–Mersen spectroscopic quality) and nickel plates (50mm×10mm×1mm) were used as working electrode. Thesurface areaoftheworkingelectrodewas deter-minedaftereachexperimentbymeasuringtheimmersiondepth in the bath. The auxiliary electrode was a silicon thick plate (4mm×8mm×11mm) with a large surface area (3cm2). The
potentials were measured with reference to a silicon plate immersedinthemoltenelectrolyte.
2.3. Techniques
The electrochemical techniques used for the silicon nucle-ationand depositioninvestigationwerecyclicvoltammetryand chronoamperometry.Alltheelectrochemicalmeasurementswere performedwithanAutolabPGStat30potentiostat/galvanostat con-trolledbyacomputerusingtheresearchsoftwareGPES.
ThesilicondepositswereobservedbySEMcoupledwithEDX probe, aftercleaningina HCl–AlCl3–H2Omixtureat50◦Cwith
ultrasonicwaves.
3. Resultsanddiscussion
3.1. Si(IV)ionsreductionmechanism
Thesiliconionsreductioninfluoridesmediawasfoundtobea singlestepprocessexchanging4electrons(asalreadypresentedin Ref.[6]):
Si(IV)+4e−= Si (1)
Cyclic voltammetry was carried out on a silver electrode in NaF–KF–Na2SiF6 system in the 820–950◦C temperature
range. Fig. 1 presents a typical cyclic voltammogram of the NaF–KF–Na2SiF6 (0.24molkg−1)systemat850◦Consilicon
elec-trode.Thiscyclicvoltammogramexhibitsonlyonereductionpeak at−0.15VvsSianditsassociatedreoxidationpeakat0.15VvsSi. ThelinearrelationshipbetweenSi(IV)reductionpeakintensityand thesquarerootofthescanratehasbeenverified(seetheinsetof
Fig.1),provingthattheelectrochemicalreductionprocessis con-trolledbytheSi(IV)ionsdiffusioninthebath(Berzins–Delahay[9]
validforareversiblesoluble/insolublesystem): Ip=−0.61nFSc0
nFDRT
1/2v
1/2 (2)where n is the number of exchanged electrons, F is the Fara-day’sconstant(Cmol−1),Sistheelectrodesurfacearea(m2),c0
isthesoluteconcentration(molm−3),Disthediffusioncoefficient
(m2s−1),Tisthetemperature(K)and
v
isthepotentialscanrate(Vs−1).
Furthermore,thediffusioncoefficientDcanbecalculatedusing Eq.(2)and theresultsobtained fromtheinsetofFig.1.Atthe temperatureof850◦C,itsvalueis2.9×10−9m2s−1.The
temper-aturedependenceofthediffusioncoefficient,in the820–950◦C
temperaturerange,isgiveninEq.(3): D=1.13×10−5exp
−77.2 × 10 3 RT (3) -600 -400 -200 0 200 400 600 800 1000 -0.5 0 0.5 1 1.5 2 j/ m A cm -2 EvsSi/V -900 -800 -700 -600 -500 -400 -300 -200 -100 0 0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 jp / m A cm -2 v1/2/V1/2s-1/2Fig. 1. Cyclic voltammogram of NaF–KF–Na2SiF6 (c0=0.24molkg−1) at 850◦C; working electrode: Ag; auxiliary electrode: Si; reference electrode: Si; Scan
Fig.2. Cyclicvoltammogramhighlightingthenucleation cross-overforsilicondepositioninNaF–KF–Na2SiF6 (c0=0.24molkg−1)at850◦C;workingelectrode:Ag
(S=0.31cm2);auxiliaryelectrode:Si;referenceelectrode:Si;Scanrate=50mVs−1.
whereDisthediffusioncoefficient(m2s−1)andTthetemperature
(K).
3.2. Siliconelectrocrystallisationprocess 3.2.1. Cyclicvoltammetry
Fig.2showsacyclicvoltammogramwherethecathodiclimit potentialishigherthantheSi(IV)ionsreductionpeakpotential observedonFig.1.Thisfigurehighlightsthemainfeaturesofan electrocrystallisationprocess:
•Theobservationofacross-overofdirectandreversescanning curves,whichistheconsequenceoftheirreversiblenucleation stepduringthereductionscan[9,10].
•Theasymmetricalshapeofthereoxidationpeak,typicalofthe redissolutionofasolidphasedepositedduringthecathodicrun (strippingpeak).
•Thelowcathodicbackgroundcurrentobservedbetween0.02V/Si and−0.03V/Sicanbeattributedtotheformationofdissolved siliconintothecathodicsubstrate(Ag).
3.2.2. Chronoamperometry
Accordingtopreviousworksinmoltensalts[11,12], chronoam-perometry is a suitable technique to investigate nucleation phenomena.Thetransientcurvesshape(I=f(t))atthebeginningof thecathodicpolarizationallowstodeterminethenucleiformation mode,growthandgeometry[7,13,14].Aseriesof chronoamper-ogramsarepresentedinFig.3,atdifferentovervoltagesonsilver electrode,inNaF–KF–Na2SiF6 (c0=0.24molkg−1),at850◦C.This
techniquewasnotfoundsuitablefornucleationstudiesoncarbon substrates,sincethiselementalloyswithsiliconatthefirststage oftheSielectrodepositionaccordingtothebinarydiagram[15].
Thecurvesaredividedintothreeparts(cf.insetofFig.3): •PartI:Duringthispart,correspondingtothedouble-layer
charg-ing,thefirstnucleiformontheelectrode.Thetimedependence onthenumberofnucleigeneratedisgivenbythePoisson’slaw
[7]:
N=N0(1−e−At) (4)
whereNisthenucleidensity (cm−2),N
0 thetotal numberof
nucleationsites(cm−2),Athenucleationconstantforasite(s−1)
andtthetime(s).
-IfthevalueofAishigh,thusN=N0andthenucleationis
instan-taneousmeaningthatallthenucleiappearatthebeginningof thepolarization.
-ForlowvaluesofA,N=AN0t,meaningthatthenucleationis
progressive.
•PartII:Thecurrentrises,duetoanactivesurfaceareaincrease, owingtothenucleigrowth.Correlatively,theelectrolyte diffu-sionpromotesthecurrentdecrease.Thecompetitionbetween thesetwoeffectsleadstoamaximumpeakintensityandits coor-dinates(tm;Im)areusedforthenucleationmodeling.Forshort
times,thecurrentinthissecondpartallowsthenucleationmode determinationandobeysthefollowingrelationaccordingto[7]:
j=˛tx (5)
where˛andxdependonthegrowthcontrol,thenucleigeometry andthenucleationmode.Inthecaseofhemispherical3D nucle-ationlimitedbydiffusion,xisequalto1/2or3/2forinstantaneous orprogressivenucleationrespectively.Eq.(5)hasbeenplottedin
Fig.4andtheproportionalitybetweenjandt1/2evidencesthat
aninstantaneoussiliconnucleationoccurs.
•Part III: Si(IV) ions diffusion control is predominant, and a slowcurrentdecreaseisobservedfollowing theCottrell’s law
[8,9],whichimpliesa linearrelationshipbetweencurrentand
t−1/2.Scharifker and Hills [7] established a model based on a
dimensionalintensityandtime:(I/Im)2=f(t/tm).Foran
instan-taneousnucleation,thecurveparametersaredescribedbythe Eqs.(6)–(9)as:
I Im 2 =1.9542 t/tmn
1−exph
−1.2564 t tmi
o
2 (6) with tm=1.2564 N0kD k = 8c0M 1/2 (7) and Im=0.6382nFDc0(kN0)1/2 (8)Fig.3.ChronoamperogramsonsilverelectrodeatvariousovervoltagesinNaF–KF–Na2SiF6(c0=0.24molkg−1)at850◦C;auxiliaryelectrode:Si;referenceelectrode:Si/Inset:
Chronoamperogramonsilverelectrodeat=−0.04VinNaF–KF–Na2SiF6(c0=0.24molkg−1)at850◦C.
I2
mtm=0.1629(nFc0)2D (9)
wherenisthenumberofexchangedelectrons,FtheFaraday’s constant(Cmol−1),c
0thesoluteconcentration(molm−3),Mthe
molarmass(kgmol−1),thedensity(kgm−3)andDthediffusion
coefficient(m2s−1).
Using thechronoamperogramsatdifferenttemperatures,the experimentalcurves(I/Im)2=f(t/tm)arecomparedtothetheoretical
onesinFig.5.
The experimental data are in agreement withEq. (6), prov-ing that the instantaneous nucleation mode is predominant at theconsideredtemperature,overvoltageandconcentrationrange. BasedonSEMobservations,similarconclusionswereobtainedby
Fig.4. Plottingsofj=f(t1/2)ofthechronoamperogramsecondpartatvariousovervoltagesinNaF–KF–Na
2SiF6(c0=0.24molkg−1)at850◦C;workingelectrode:Ag;auxiliary
Fig.5. ComparisonofthedimensionlessexperimentaldataatvarioustemperatureswiththetheoreticalmodelsinNaF–KF–Na2SiF6;workingelectrode:Ag;auxiliary
electrode:Si;referenceelectrode:Si.
Carletonetal.forthesiliconnucleationmodeonvitreouscarbon inLiF–KF–K2SiF6at750◦C[16].TheSEMmicrographofnuclei,
pre-sentedinFig.6(t=1.1sand=−0.04VvsSi),seemstoconfirmthe instantaneousnucleationmodeandthehemisphericalgeometryof germs.
ThenucleationsitesnumberN0werecalculatedusingEqs.(6)
and(8)atvariousovervoltagesandtemperatures;thevaluesare gatheredinTable1.
Anincreaseinthenucleationsitesnumberwiththeovervoltage isobservedwhiletheproductIm2tmremainsconstant,asforeseen
in Eq.(9).AspreviouslydemonstratedinSection3.1,thenuclei growthislimitedbySi(IV)ionsdiffusion,which iseither hemi-sphericalorlinear.Inlineardiffusion,theslope˛(definedinEq.
Fig.6.SEMmicrographofsiliconnucleionsilverelectrodeinNaF–KF–Na2SiF6
(c0=0.24molkg−1)at850◦C;=−0.04VvsSi;t=1.1s.
Table1
OvervoltageinfluenceonthenucleifavourablesitesnumberinNaF–KF–Na2SiF6
(c0=0.24molkg−1)at850◦C;workingelectrode:Ag;auxiliaryelectrode:Si;
refer-enceelectrode:Si.
(V) im(Acm−2) tm(s) 10−2im2tm 10−11N0 −0.030 −0.098 1.55 1.49 2.10 −0.040 −0.158 0.680 1.70 4.79 −0.050 −0.236 0.298 1.66 10.9 −0.055 −0.274 0.218 1.64 14.9 −0.060 −0.316 0.167 1.66 19.5 −0.070 −0.393 0.116 1.79 28.1 −0.080 −0.469 0.076 1.67 42.8
(5))followsEq.(10)whereastheEq.(11)describesahemispherical diffusion: ˛=−8nFM2c03N0D3/2−2−1/2 (10) a=−nFN0(2Dc0)3/2
M 1/2 (11) TheN0 values,reportedin Table1,arecompared inTable2withtheonecalculatedfromtheslopesofj=f(t−1/2)(Fig.4)ineach
differentdiffusionconditions,derivedfromEqs.(10)and(11). ForthevaluesmentionedinTable2,thiscomparisonseemsto statethatthenuclei’sgrowthisgovernedbyalineardiffusionand thusshouldleadtoadendriticgrowth.
Table3showsthetemperatureinfluenceforsiliconnucleation on a silver electrode at various overvoltages. It indicates that thenucleationsitesnumberN0increasessignificantlywithboth
Table2
Comparison of the nuclei favourable sites number in NaF–KF–Na2SiF6
(c0=0.24molkg−1)at850◦Cfordifferentdiffusionmodels;workingelectrode:Ag;
auxiliaryelectrode:Si;referenceelectrode:Si.
(V) 10−11N 0 Lineardiffusion Eq.(10) Hemisphericaldiffusion Eq.(11) 10−11N 0 10−8N0 −0.03 2.10 2.14 0.47 −0.04 4.79 4.44 0.98 −0.05 10.9 6.49 1.44
-0.08 -0.07 -0.06 -0.055 -0.05 -0.045 -0.04
η/V
25 26 27 28 29 30 700 600 500 400 300 200 100 0 Ln (N 0 ) η-²/V-2Fig.7. LinearrelationshipbetweenthelogarithmofthenucleationfavourablesitesnumberandsquareovervoltageinverseinNaF–KF–Na2SiF6(c0=0.24molkg−1)at850◦C;
workingelectrode:Ag;auxiliaryelectrode:Si;referenceelectrode:Si.
temperature and overvoltage. In Fig. 7, a linear relationshipis evidencedbetweenln(N0)andtheinverseofsquareovervoltage
andobeysEq.(12)[13,17]: ln(N0)=A− B
2 (12)
Knowing thenucleation mode,Fig.7 allowsoptimized elec-trodepositionconditionstobeproposed.Indeed,toobtainasmooth coatingstructure,thecreationofahighnumberofnucleiis essen-tial,whichisfavouredbybothhightemperaturesandovervoltages. Neverthelessforhighovervoltage,atoohighelectrolytediffusion limitationcanpromotedendriticgrowthphenomena.Takinginto accounttheseconflictingeffects,itwasdecidedtorealisesilicon coatingsatdifferentovervoltagesandtemperatures.
3.3. Siliconelectrodeposition
Variousrunsofsiliconelectrodepositionondifferentcathodic substrates were performed taking into account the conditions suggested in the previous section. The electrolyses were con-ductedunderintentiostaticconditionsasmentionedinreferences
[16,18,19].
Thecurrentefficiencywasdeterminedongraphiteandsilver electrodesusingthemassdifferencebetweenthecathodebefore andaftertheelectrolysisrun.Itwasfoundtobebetween88and96% forlowcurrentdensities(-20and-100mAcm−2)resultingindense
deposits;athighcurrentdensities,thedepositswereverydendritic andbrittle,whichcausedsiliconlossesduringthewashing treat-ment:thecurrentefficiencycouldnotbeevaluated.Thesecurrent
Table3
Temperatureinfluenceonthenucleifavourablesitesnumberatdifferent
over-voltagesinNaF–KF–Na2SiF6(c0=0.24molkg−1);workingelectrode:Ag;auxiliary
electrode:Si;referenceelectrode:Si.
(V) tm(s) 10−11N0
850◦C 900◦C 850◦C 900◦C
−0.03 1.55 0.568 1.46 5.15
−0.04 0.680 0.336 3.41 8.70
−0.05 0.298 0.203 12.4 14.41
efficienciesarehigherthanthoseobtainedbyElwellandRao[20]
inLiF-KF-K2SiF6at750◦C:50%asanaveragecurrentefficiencyand
80%for−25mAcm−2currentdensity.
3.3.1. Operatingconditionsdependence
Several silicon coatings were obtained in NaF–KF–Na2SiF6
(c0=0.47molkg−1)inthe820–900◦Ctemperaturerangeoncarbon
rod,forappliedcurrentdensitiesbetween−20and−200mAcm−2.
After frozen salt removal, the coating microstructures were observedbySEM.Themicrographs,presentedinFig.8,suggest firstthathighertemperaturesfavoursomewhatthesurface coat-ingregularitybutalsothathighcurrentdensitiesaredetrimental forthisproperty,whichisinagreementwithstudiesfromElwellin NaF–CaF2–SiO2[19],BoenandBouteilloninLiF–NaF–Na2SiF6[18]
andalsoforothermetalsdeposition,e.g.ontantaluminmolten flu-orides[13].Forapplicationswherehighplatingratesarerequired, theuseofpulsedcurrentcouldhelppreventingthediffusion limita-tionandthusleadtomoreregularcoatingsathighcurrentdensities
[21–23].
EDXanalysisofthedepositsdidnotrevealanyothercompound thanSithatmeansthatthedepositpurityisassumedtobeatleast 99.9%.AsforthepurityoftheobtainedSi,whichisakeyissuefor thesolarindustry,recentworkfromNohiraetal.[24,25]showed that,inthecaseofprocessesinvolvingmoltensaltssolventsathigh temperatures,acarefuldesignoftheelectrorefinerhastobemade inordertoavoidpollutionfromthecellelements.
3.3.2. Substrateinfluence
Duetothestrongeffectofthecurrentdensityontheregularity ofthecoatingsurfacestateandthemoderateinfluenceofthe tem-perature,electrodepositionrunswerecarriedoutat−20mAcm−2
at820◦Cfor5h.Fig.9showsSEMmicrographsofsilicondeposits
onthreeelectrodesubstrates(Ni,AgandCv).
On nickel (a),silver substrate (b) and vitreouscarbon (c), a columnardendriticcoating,a siliconmicrowirestructure and a sponge-likestructurewereobservedrespectively.Thesmoothand densedepositobservedongraphitecarbonat820◦C,−20mAcm−2
(Fig.8)isinagreementwithRaoetal.work[26]inLiF–KF–K2SiF6
at750◦C.AccordingtoCarletonetal.[16],thedifferencesbetween
Fig.8. SEMobservationsofsiliconcoatingsoncarbonatvariouscurrentdensitiesandtemperatures.
properties leadingtosignificant differencesofnucleation active sites.
Fig.10presentsSEMobservationsofsiliconcoatingscross sec-tiononvarioussubstrates(Ni,Ag,Cand Cv)at−20mAcm−2 at
820◦C.
•Nickel substrate (a): Ni–Si alloys layers are observed at the substrate-coatingboundary,whichseemstopromoteaveryhigh adherenceofthesilicondepositonthesubstrate.SEM-EDX anal-ysis shows two silicide layers under thecolumnar layer and XRD measurement ontheNi–Si surface depositindicates the presence of Ni3Si2, NiSi and Si formation. Previousworks on
intermetallic compoundsNi–Si preparation byhigh tempera-turesoliddiffusionevidencedfournickelsilicides:Ni5Si,Ni2Si,
Ni3Si2,NiSi[27,28].Boriventetal.[27]showedthatthegrowth
ofNi3Si2proceedsbyneedles:itcouldexplainthatinthepresent
work,thesiliconcoatinggrowthoverNi3Si2needlesiscolumnar,
contrarytoothersubstrates.OurconclusionisthatNisubstrate isnotadaptedtosiliconelectrodepositionduetohigh interdiffu-sionratebetweenthecompoundswhichpromotestheformation ofintermetalliccompoundsinsteadofpureSi.
•Silverelectrode(b):noalloyformationisobserved,inaccordance withtheAg–Siphasediagram[29].Thesiliconlayer,coveringthe Agsurface,becomesprogressivelymoreporousandfilamentous andtendstobreakduringthewashingtreatment.
•Graphitecarbon(c):adenseSiClayer(∼10mm)wasformedby interdiffusionbetweensilicondepositandcarbonelectrode.On thisthinlayer,adenseandadherentsiliconlayerof∼100mm thicknesswasobtained.Similarresultsongraphitewereobtained byRaoetal.whoattributedthedepositcompactnesstothe coa-lescenceofsiliconnodulesinathree-dimensionalgrowth[30]. •Vitreouscarbon(d):aroughandpoorlyadherentdepositwas
obtained.Thisbrittledepositwasmostprobablybrokenduring thehotpressingcarriedoutforthesampleembedding.
Fig.9.SEMobservationsofsilicondepositsurfacesat−20mAcm−2at820◦
Fig.10.CrosssectionSEMobservationsofsilicondepositsat−20mAcm−2at820◦Cfor5honvarioussubstrates:(a)nickel;(b)silver;(c)graphitecarbon;(d)vitreous
carbon.
4. Conclusions
The silicon nucleation mechanism was studied in a NaF–KF–Na2SiF6salt mixture on silver electrode, using mainly
chronoamperometry: the silicon nuclei are generated instanta-neouslywithalineardiffusion-controlledhemisphericalgrowth. Moreover, the nucleation sites number N0 increases with the
temperatureandtheovervoltage.Then,galvanostaticelectrolyses wereperformedbyvaryingtemperatureandcurrentdensityon a carbon rod. SEM observations showedthat high temperature andlowcurrentdensityleadtoasmootherdeposit,withapurity (measuredbyEDX)higherthan99.9%.Thecathodicsubstratetests (Ni, Ag,Cand Cv)allowed concludingthatgraphitecarbon isa
well-adaptedcathodicmaterialduetothedepositadherenceand structure;onvitreouscarbon,thedepositsaredendritic;onsilver substrate,thedepositsarepoorlyadherentwhileonnickel,many alloyswereformed,hinderingpuresilicondeposition.Whenthe currentdensityincreases,thecoatingbecomesrougher. Athigh current densities, the silicon ions diffusion limitation strongly influencesthesilicongrowth,leadingtoamoredendriticdeposit. References
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