Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Chemistry and applications of chelating agents in flotation and flocculation P. Somasundaran and D. R. Nagaraj Synopsis Chelating agents, because of their metal specificity or selectivit)", can function as good flotaids and selective flocculants. In addition to the metal selectivity, chelating agents offer certain advantages over conventional mineral processing reagents even from the synthesis point of,-je,,". With the major donor atoms-S, N, 0 and, to some extent, P-numer<KJs possibilities exist to tailormake reagents for specific applications. For polymers the backbone offers funher possibilities for the incorporation of the required propenies. In general, the choice of a chelating agent or a group is made on the basis of its function in well-known analytical metal separations. Such a choice is limited in that the number orwell-known analytical separations is also limited. In the present work, a new and effective do"or atom approach is discussed for the design of mineralspecific chelating groups. This generalized approach is focused on the chemical properties of the imponant donors both in the reagent and on the mineral. Data from many chemical S<KJrceshave been summarized and applied to systems of relevance to mineral processing. Understanding of the chemical behaviour of donors is of param<KJnt imponance in predicting the propenies of chelating groups. Numerous investigations have been made of the application of chelating agents in mineral processing. The various fundamental aspects of the interactions between a mineral and a chelating group are, however, not clearly understood, although there is evidence to suggest that some form of a metal complex is formed at the surface. The separation of mineraJsfrom one another by flotation and floccu1ation depends mainly on the sdeaive 8dsorption of surfactants and polymers on them. Although many reagents have ~ng hem used in practi~ for the flotllion of mioera1s.most arc not as selecti\'e E is required for the efficient separation, in particular, of mineral fmes and ultrafmes. Reagents with chelating functional groups have received increased attention for this purpose in recent years, being known to exhibit exceUent metal selectirity in analytical separllions. MInY chelating agents have been tried E coUeCton for various mineral systems and excellent seper8tions have been obtained in cenain czcs. The mechanism~ that involve their colleCting action arc, however, not adequate~' understood. In particular, the differences in their mode of action at the mineral surface venus that in the bulk are oot fully ~ and, as a resuh, the dcve~pment of collecton based on their use in analytical separations is not ach~'ed easily. It is to be noted in this regard tha chelating coUecton are seldom ~tal-specific or mineral-specific and the propenies of both the chelating agents and the mineral are imponant in determining their colleCting action. The dIXlor atoms on the chelating agents, as well as those associatedwith the mineral species, playa governing role in their intenctions on the surface. In this paper the application of chelating agents in mineral processing systems is re\'iewed on the blSis of the donor properties of the c1'w:latinggroups and the metal species, and recent approaches to understand chelation are discussed briefly. Emphasis is given to the criteria for selecrioo of chelating agentS IS colleaors for various minerals and the prediCtabilit)" of the behaviour of a chelating agent for a given mineral system. Chelating agents Ch~latingagentsarecompoundsthat fonn metalcomplexes characterizedb)' ring struaurcs ilIusuatedin Fig, I.I.~.j In type I th~ metalis coordinatedto th~ four nitrogcnsof two moleculesof ethylcn~diamine,giving rise to a d1argedcmubleringed compla ,,'ith cbIorid~nNtralizing th~ two charges,I Other typesof dldating oomplcxesindudc t}"peII. "ith 81 inm-molccular hydrogenbridge.and type III. involving polynuclearhalogen bridges. .NH2-CHz Cf2 .W I 'NH2-C"z H3C\ I'c~o .. H HC " I (D) ~-O H,C .CI- ...:, (ID) ,ci. B FiB- I B GeIxr8I sUUCtUresof clr1ating -cents I Chd~ng agentscm be cl~sirlCdon the b85isof donor atoms involvrd (0-0, N-O, N-N, 5-0, 5-5, 5-N)or ring size(4-,5or 6-memberrd)or chlrg~ on th~ complex(Inion, cation, neutral)or numberof bondsto the meuI for everydteJating molecule(bidentat~I: 1 /A; M ) 'A bidentatc1:2 ( A 'M/A) A/ 'A ; A terdentBte M~) 'A) Specificityof chelatingagentsdependson the int~on 209 Weal ckIDOratoUD Ind sunKe species on the panicle. A list of /lOr atoms Ind funaional groups a>ntlining the four major lIDS(N, O. P and $) are given in Table 1. Halogen atoms, a. and I, panicipate in chelate ring formation in bridged S.illa" HO-CH-COOH I HO-CH-COOH UmuuDble CH2-COOH I CH2-COOH Table 1 Donor atomsand functional groups containing major donor atoms) t: rI N OH H ---"'t 0 I , P , s : I_!_~ ~ IAs L__- r I a: Br: I I I I I Tt Ii-.L_-J Sb -NH, 0 s -rooM -OH (mol 01' phenol) =0 -08 -P(O:.(OHh -5H -S-R (ajQ)1XII5 polynuclearcomplexesthat an of minimal imponancein mineralprocessing.As and Sefonn only a few usefulcomplexes and.tberef~, an seldomused. Requirements for c:helatinl8JeDU Thcr~ Ire. essentially, tWObasic:requir~mcnts that c:h~lating agents must satisfy to form metal cbclates: the molecules should hav~ suitabl~ functional groups and the functional groups must be situated to permit the formation of a ring with a mctaI a the closing m~mber. These t"-o conditions are ncces~', but not sufficient for the formation of a d1elat~ ring. For aample, under ccnain conditions and under sufficiently to.. pH valum, a potential chelating molecule may attach itself to a mcta1atom through only on~ ligand atom: "/ " a H ooc. CH zNH z ,0 Pt NH~2COOH or HOOC.CH:S-M I t hE been generaUyobserved that certain Iddioonal requirements must be satisfied b}. chelating agents for mineral processing applications: the chelates should, preferably. be neutral, if the chelating agent is to function IS a collector, and the dlelates should, preferably, be charged and very hydrophilic if the chelating agent is to function as a depressant. On a pol}'Dleric depressant or a flocculant this require~t is not stringent so long IS the backbone hE other hydrophilic groups (seebelow). Rcquirmtcuu for dr.pressanu:ionic chr.lMes,r..g. lCo(DMG)~HzO~'. and bydrophilizinggroupson moJecuJr. 210 H~H OH rt:JfH Neutral complexes arr usuallyinsolublr in wltrr and. therefore,promotr hydrophobicit},.For insolubilit}, in wltrr, howr\"er,it is not sufrlcimt that thr chrlltr br a neutral complex. A classicrxamplr is that of chrlatesof dimethylglyoximes (DMG) (5« Fig. 2). The 1:2complrx of nickelwith DMG is insolublr in wltrr. Thr coppercomplrx is, on the othrr hand, rdai,'rly ~'.rr-soluble. This resultsfrom the subtlr differences in thc shapesof the tWoIOOlecutcS and consequmtdiffrrmces in the IOOdrof packingof thc tWomolecuJes in their resprctivr crystals(Fig. 2). The nickel compoundis planarand the molrculesarr stackrdin thr crystal,sothr Ni atomsarr co-linrar md havr a wrak bond brtWrcn them. In the coppercompound, howr\.er,thc chelaterings arenot co-planarbut makea small angleof 28° with onr anothrr andthere is no metal-metal bonding.I The tetragonalpyramidalcopprr chrll(r molrculesarr pairrd in thr crystalin sucha waythat ram copperatomhz an 0 atomirom itSIdjKent molrcuk a onr of its fivr immediate neighboun, In thr Ni complexthr -OH md thr -0- are strOnlly internallyhydrogenbondrd Ind, bmce, lessreadily sol"atrd. The coppercomplrx aCtUallyhasa highrr stability constantthanthe Ni complexbut, sincr no intrrnal hYdrogrn bondingis po5siblr,thr complexis easilysolvatrd. Specificity and selectivity Most of the chelatinggroups form complexeswith almostall of the transition and many non-transition metalsand, therefore, specificity is not asabsoluteasis required for their selective adsorptionon minerals.In practiceselectivity is achievedby making useof differencesin stability constantsand chelate formation under various solution conditions. As wasindicated earlier, contribution from the donorsasthey arelocatedin the minerallanice hasto be consideredin obtaining the selectivity. Also, the solubility of the mineral, in addition to that of the metal chelate,hasa pronouncedinfluenceon the selectivityand the collectionpower of the chelatingagent. Stability of complexes _\1ajorfactorsthat determinethe stabilit~.constantare,in order of decreasingimponance, pK. of the ligand molecule, substin:ents,natureof donor atoms,central metalatom,and ring size,number of rings. The fIrStfour factorsarevery imponant in that they determi~ the natureand strengthof bonds.pi(. of the che~ agenthasa direct influenceon the chelateformation sinceit representsthe tendenC)'of the donor atomsto donateelectronsto metalatoms(or acceptfrom ~a1s, in cenain cases)andthus Ionn a chelate.Substitution on the chelatingmoleculehastWo imponant effects:J it altersthep?<.and/orit introduces steric Iactorsfor the formationof a c~late. The influenceofthc natureof donor atom and the central metal atomshouldbe consideredtogetherbecauseof the interrclatio:nshipbetweentheir behaviour(seelater). Properties of acceptors Acceptorscanbe divided convenientlyinto two maingroups basedon the unidentateligands:(a) thosewhidl form most stablecomplexeswith N, 0 and F, Illd (b) thosewhidl form moststabk complexeswith P, 5, and a (fable 2). The stability constantsof metalcomplexesthat beJongto the two groupsfollow the generalordersN»P>As>5b; 0>5; F>CI>Br>I; Illd for similar liglllds N>O>F; differencesin the seriesP>5>CI arefound to be lesspronounced.4It is seenthat a vastmajority of elementsbelongto group (a), i.e. they preferentiallycomplexwith 0- and N-containing liglllds. A given metal, funhermore, may belongto group (a) or (b), dependingon its oxidationstate:for example,Cu(I) belongsto group (b), wherasCU(II)belongsto the overlap regionof (a) and (b). A major shoncomingof the abovegrouping is that it is based on unidmtatt liglllds; the situation is complicatedwhenchelates (or bidentates)areinvolved. Considerationmust be given in this caseto chelatingagentsin which the donor atomsarethe same (examplesareethylenediamine,oxalateor thiooxalate)Illd chelatingagentsin which the donor atomsaredifferent (examplesareo-aminothiophenoland o-arninophenol).For nickel, tbiooxalateion is Believedto form a more stablenickel chelatethlll the oxalateion. For zinc, stability constlllts of the 0aminophenoland o-aminothiophenolcomplexesshowthat the substitutionof 5 for 0 doesha\'~a markedinfluenceon stability. A moreusefulgroupingis that basedon the electronic configurationof the metals.Thus metalscanbe classifiedinto threegroups-those which contain (a) inen-gastype configuration, (b) panially filled d or f orbitals and (c) ions of metals~;th filled d orbitals (Ag., Zn2+,etc). Metalsof group (a} reactprt:f~rentia1Jy ~;th O-containing ligands,suchascarboxylateions and th~ anionsof quinalizarin, Illd the p-diketones. Table 2 Classificationof acceptorsbasedon unidentateligands I ';:V/ '," 8/1';( NO F Ir,' Mg Sc Ti D ~ D ", ' G~ , V CLASS A BORDER Form stable complexes with K,O,F REGION Class B: Form stable complexes with P.S.Cl 211 0 J. ~- a 1f~ O' O' ..,..C Transition-metalionsform morestablecomplexeswith ligandsthat containpolarizableponions, suchasaminogroups andheterocyclicnitrogenatoms. Metals in group(c) alsoprefer highly polarizableligands, especiallyif the latter havesuitablevacantorbitals into which someofthc d electronsfrom metalscanhc 'back-bonded'. Examplesof suchligandsare thosewhich contain S asthe donor which is highly polarizableand basvacant3dorbitals.Thus, thioanalideforms insoluble complexeswith Cu, Ag, Cd, Hg(ll), 11, Sn(ll), Pb, As, Sb, Bi, Pt and Pd. 0 ~""I/::"T N H - ~...J,,~ II C SH - I CH 2 Thioanalide A reagent, such as dithizone, which oontains N and S dono~ therefore reactSwith a large part of the transition metal and filled d orbital series.To achieve the degree of selectivity that is desirable in praCtical applications it is usually necesSar).to arrive at the appropriate oombinations of dono~. Donor-acceptor relationships A useful classification of acceptors as well as donors is that based on Pearson's concept of hard and soft acids and bas6 (rable 3).S.6.7 The acids (or electrophiles) are mostly (metal) cations. This group also includes such electrophiles as CO2' 0, a and N and metals iI\ the zero oxidation state. The bases(or nucleophiles) are non-metal anions, neutral atoms and molecules. It should be noted that the donors 0 and N are hard basesand donor S and P are soft bases. Table 3 Characteristicsof bard andsoft acidsand bases Hard (acid or baK) Soft (acid or base) Smallsize Orbitals involved far apan in ener~' Ionic bonding coulombic attraction Large size Orbitals closein ~rgy High chargeions High chargeions Non-polarizabk Hard likes hard Polarizable Baseshave10"-proton affmity Soft likes soft High elecrronegativity Lo'" elcctroncgativity Co,"alentbonding The bondingcharacteristicsof thesegroupsaregivenin Table 3..ln general,hard basespreferentiallyreactwith hard acids,and similarly for soft bases.The former interactionis characterized by ionic bondingsincethe orbitals in"olved arefar apartin energ}',therebypromoting coulombicattraction.On the other hand,the interactionbetweensoft basesand soft acidsis characterizedby covalentbondingsincethe orbitalsinvolvedare closein energy. It is questionablewhether this sort of classificationwill be valid for mineralspecies,althoughthere is someevidencein the literature that the metalcationsthat prefer to reactwith 0 donorsalsotend to preferentiallyadsorbO-containing 212 coUccton on their min~ral surfaces.7 Similarly, S donorsreact pr~ferentiallywith sulphid~min~ra1s.It hasbeenpoint~dout that a bond betweenm~tal ions and soft basesmakesth~ metal ions soft acidsand vice v~na.8This is ~speciallyimportant to bord~rlin~ cations.From this viewpoint sulphidizationof oxidized min~ralsshould leadto an incr~asein the capacityof th~ir reactiv~centresto reactwith sulphydryl coUccton.7Thus, th~ imponant contribution of donon on th~ min~ralsurfacesto int~ractionsbetweenmineralsand ch~latingag~ntsmust be noted.Oxjd~ min~rals(which have0 donon) of soft-acid metal ions would preferentiallyadsorb0- and N-containing collccton, wh~reasth~ir correspondingsulphideswould pref~rentiallyadsorbS-containingcollectors. Properties of donor atoms The donors o and N belong to the first row of elements in the periodic table and follow the octet rule'-4,fo9"o,'1with valencies 2 and 3. The donors P and S belong to the second row, and these also follow the octet rule with valencies 3 and 2; however, P and S can exhibit higher valence states also since they have easily accessible vacant 3d orbitals. It is the electrons at or near the surface of atoms and ions that are the most important in determining their chemical andph)osical properties. This is especially true of donors P and S and transition metal ions. The laner have incompletdy filled d orbitals, which have quite large fractions of their tOtal volumes near the outsides of the ions, so they are easily accessible for bond formation. Additionally, the J orbitals are much more easily polarized, promoting a much more favourable orbital overlapping. The important properties of the four donors 0, N, S and Pare summarized in Table 4. o and N have 2p electrons and no accessiblevacant d orbitals. S and P have 3p electrons in their outermost shells, but they have, in addition, easily acce:ssiblevacant 3d orbitals. The electronegativities decreasein the order 0 ,3.5) N 3.07} s P :2.44: (2.06) Consequently, 0 invariably forms ionic bonds with a majority of elements in the periodic table. Thus, chelating Igents with 0-0 donors often form chelates with a large number of metals and are, therefore, lessselective. The selectivit). in general should increase from 0 to P. The normal ,'alencies are 2, 3, 2 and 3 for 0, N, S and P. respectively. 0 has tWo unpaired electrons or two elearon pairs to donate, but it seldom donates ooth pairs; only one pair is active. It can form a maximum of four oonds. but seldom attains all four (three oonds are common). 0 forms multiple oonds, N has five valence electrons. but only four orbitals and, therefore, a maximum of four oonds can be formed, It has one lone pair of electrons to donate when three electron-pair bonds are formed Like its neighoours C and 0, N also readily forms multiple oonds. In this respect N differs from P. S. As, Sb and Bi, S has rn'o valence electrons and its normal valency is 2, But it has four orbitals and easily accessibled orbitals. Consequently, S can torm two to six bonds. Similarly, P forms three to six oonds, although its normal valency is 3 and it has five valence electrons. .0\11 four donors have one active lone pair of electrons. Although 0 and N show strong prr-pir bonding (becauseof the pouter orbitals and no d orbitals). S and P show ver)'little or no tendency for P70-p1T.On the other hand, only S and P show strong d1T-d1Tbonding. In addition. S and P sho,,' d1T-p1T bonding (or back-oonding) since they can accommodate ela.~rons from metals in their vacant d orbitals, This ability for back-oonding for P and S, indeed, is an important distinction that puts these donors in a special class. The polarizability of the lone-pair electrons on these donors follo""5 an almost rC"'erse Table 4 Major propenicsof donor atoms0, N, S and P 0 CONFIGURATION lS22S22pl& 2 3 OF ORBITALS II 4 2 4+D OF BOUDS 3 II 2-6 ELECTRONS NORMAL VALENCY (VALENCY EXPAaSION) p [Nij 3S23PQ3Do [HE]3SQp3300 2.11i 2.44 5 2 3.07 5 VALENCE II lS22S22P3 3.5 2 ELECTRONEGATIVITY Ii s tl 3 /I + 0 1 1 2 1 pw-p. STRONG STRONG POOR NONE Ow-p. NONE NONE STRONG $TRatG POLARIZABILITY NIL GOOO STRONG GOOD H-BONDS STRONG STRONG VERY WEAK NONE BONDS MORE IONIC LESS IONIC COVALENT COVALENT STERIC ACCESSIBILITY LOW LOW HIGH HIGH LONE PAIRS {BACK-BONDING) ord~r ofth~ ~lectron~gativities. Thus, for polarizability ~«.s-p 0 and N have the distinction of having the ability to fonn very strong H bonds, whereas S and P show little or no such tenden~'. Since P and S h8\'e d orbitals, and large size, these donors Ire much more sterically accessiblefor bond formation than90rN. S is unique in its abilit). for catenation (forming bonds with itself); its common OCCUiTence is in the fonn of an eightmembered ring. S is also knO\\"Dto fonn higher polymers. This unique featUre of S is Ver)' important in all its interactions. 0 and S can enter into chelation either through the ether or thiOetber fonn R-O-R, R-S-R, or the R-OH, R-SH. The -SH group is much more acidic than -OH and is highly polarizable, but not an effective acceptor. The R-S-R group forms ~'ramidal bonds and is an effective drr acceptor. The R-SH sho\\'Sa strong tendent1' for unidentate bonds, and the R-S-R sho"'S a strong tendenC}' to form chelate rings. The C=S is more ionizable and has a greater volume than C=O. S is a better donor than 0 with reglrd to sharing or donating the lone pair of electrons. Similarly, N is also a better donor than O. It can be readily seen from the foregoing discussion that each donor has some unique properties. The acceptors also fall into certain \\'ell-recognized patterns. A judicial combination of donors for any given acceptor, taking into account the properties of both acceptors and donors (on mineral as well as the chelating agent), should provide the required selectivity in minerals processing applications, The "\\olecullr Orbital treatment is a powerful tool in understanding the donor-acceptor interactions. In this approachI '.10.12.13 the individual atoms \\'ith their nuclei are all placed in position and all the electrons concerned in bond formation are allotted to the various molecular orbitals, This treatment, however, has scarcely been used in understanding the mechanism of adsorption on minerals, Substituent effects The electron-donating or \\'ithdrawing tendencies of organic groups \\'ill influence the electron densities on donor atoms and the pKa of the molecule. ',1'.14-1"The inductive effect results from electronegativity differences, Much stronger changes in electron density and delocalization of electrons arise from the resonance or mesomeric effects. With alkyl amines, for example, the aJI,.-y1 group exertS an inductive effect on the nitrogen, making its unshared electron pair more available for bonding and thereby increasing the basicity. H H R-N:+H'~ R- N H' H H In carboxylicacidsthe inductive effectof analkyl group decreases the acidity; for formic acidtbe dissociationconstantK. = 17.7x 10-5,whereasforacenc acidK. = 1.75x 10-5-almost onc-tenthof the valuefor formic acid #0 ~, 0 R -+- C' {-] [K. decreases) If, on the other hand. the R group exerts Ul oppositeinductive effect owing to certain substitUents on R such IS Cl or NOl' the acid strength of the carboxylic acid incrcascs. R -+ ~' C?' ~, 0 Q (K. increzes] The electroniceffectsaremuch strongerin aromatic compounds.A benzenering oouldexertooth electron-donating andelectron-withdrawingeffects.In benzoicacidthe aromatic ring exertsan electron-withdra~ingeffectand,hence,it hasa much higherK. than that of aceticacid.An alkyl group in the para positionon the ring exertsan electron-releasing effect. Groups suchas-OH or -OCH} areelectron-releasing o~.jng to resonance,in spiteof the electronegative oxygenand the electron-withdrawinginductiveeffectsthat the groupscanbe soownto ~sess. The effectof electron-activesubstitUentson an aromaticring is well exemplifiedby aromatichydroxy oximes.For anelectronreleasingR group,suchz -CH) or -OCH)J the acidstrength decreases, andtih. increaseS, the releze of electrons destabilizingthe phenolateion (the electrondensityon N may alsoincrease): R R ! (;;"1RI -y ~/.--o." ! H~ OHNOH / OH NOH SALO 10.70 II -o-C-'-NH. Thus, s RO' Table S pK. of SALO II1d ligand field stabilizations 18 CH,.SALO 11.06 s RI SubstitucntsR = 0, NO2ttc., ha\'eoppositeeffects.The incrc~e in electrondensityon donorscan(a) enhanceb~icity and(b)thereforeenhancea bond stability, but (c)it may also decreaserr acceptorability of ligand and (a')thereforedecre~e donor rr-bond stability, Effects(c)and (a')could be pronouncedfor donorssuchasS sincethe donor-rr bond(or dativebond) is formedbetweenthe ~tal andthe organicreagent(in additionto the coordinativeor I-bond) ~ a result of tranSferof electronsfrom d orbitalsof metal into vacantd orbitalsof the donor.The formationof a dative bond,whidl reinforcesthe 0 bond, is moreprobablefor mttals in their IIjweroxidationstatesincethesewould havemore electronsthan thosein the higheroxidationstate.Another importantrequirementis that the donor atomshouldhaveeasily accessible vacantd orbitals(S). 0 and N, whidl do not have thesed orbitals,do not form a dativebond.The nitrogenin oximes,however,forms a donor-rr bond and,therefore,oximes arean exception.This explainsthe order of the ligand field stabilizationeffectsobservedfor the chelatesbetweeen substitutedsaliC)'ialdoximes (SALO) and Cu. Ni and Co (Table 5). pK. :to.OS Simultaneouslythe groupsRO and R INH could exert an electron-donatingefTect sincethe C+-S- is more stablethan -C=S. This tautomerism,togetherwith the inductive effect, would delocalizcelectronsover the entire activegroup Substituents introduced into the molecule influence the electron distribution and, therefore, produce some interesting effects. Russian investigators7.\) have done some extensive StUdy on substitUted thionocarbamates-especially phenyl substitUents. The. V-benzoyl thiOnocarbamate has been stUdied the most: S Ii 0.8 2.6 2.4 3.8 3.5 s , c-o-c CH: The aromaticring accentuates the eleCtroniceffectscompared with an alkyl analogue s II CH) CHzO- C 214 NH 0 II c -CH; In addition,the 0 of the C=O exertssomeelectron-withdrawing effect,beingstronglyelectronegative. The delocalizationof electronsis morepronounced.There is a decreasein electron dcnsi~' on S andthe pi(.. s 0 'I;~~~ NH =Jt.'V ~ substitutionof a phenylgroup insteadof a benzOylgroup mayleadto a different electroniceffect,sincethe phenylgroup caneither beeJectron-donating or electron-withdrawing. For thiol collectors(dithiophosphates, xanthates,and dithiocarbamates'the electrondensitieson tbe activeS donors dependon the inductiveeffectsin the molecules. s RO," P S- RO RO/ """'S- 1(/ DTP Xanthate C;5 'So DTC II NH .CH,CH) / 0 andN exen an electron-withdrawinginductive effect. R c-<Q) 10.1 The ligand field stabilization(LFS) increasesfor eachmetal asthe pK. decreases, i.e. asthe electrondensityon the donor atomsdecreases. This increasein LFS is attributed to the effect of substituentson the 1T-acceptor capabilityof the ligands.18 The thionocaroonates(Z-200 t).pe)arenot only excellent sulphidecollecton but alsootTeran interestingcasefor study. The moleculecontainsthe three iml'Ortant donors0, N and S. o andN arehard basesand S is a soft base. CH, 0 II CH, CH2O- C -NH- CLSALO NOrSALO 10.2S 8.72 8.4 1.5 1.1 7.S NHR The dectron-density order may follow S>O>N and, considering the sizes and polarizability of the donors, the steric accessibility would follow the order S>N,O. S may also show a tendenC)' to bond with S on the sulphide surface. Thus, S is a ve~' active donor in the thionocarbamate molecule. 7 ,', CH} CH20dt'= 0.6 "C S II O-E-C~NHRJ In DTP the {\\'o RO groupsexen an electron-withdrawing inductive effectbecauseof the higherelectronegativityof the 0 atoms.This will delocalizethe electronandstabilizethe anion. Funhermore,P is moreelectropositivethan C in xanthate.The electrondensityon S in DTP would be decreased and, consequently,DTP is a strongeracid,weakercollectorand more selectivethan xanthate.Theseelectroniceffectsareless pronouncedin xanthatesincethereis one lessRO group andC is lesseleCtropositive than P. In DTC N is lesselectronegative than 0 and has. highertcndenq to donateelearons. As a resultthe DTC would be . strongeroollector,weakeracid andless selectivethan DTP (DTC<X <DTP). 6 SALICYLALDOXIME O-HYOROXY ACETOPHENONE OXIME O-HYDROXY BUTYROPHENONE OXIME 0 Z-HYDROXY-5-METHOXY-BENZALDOXIME () Z-HYDROXY-5-METHYL-ACETOPHENONE ~ 2-HYDROXY-)-NAPHTHAL:>OXIME O-HYDROXY CYCLOHEXANONE OXIME a-HYDROXY BENZOPHENONE OXIME 0 0 Table 6 StructUreand water solubility of various hydroxyoximesl9 . OXIME . pH- 4.8 1001 p~? ? p 80 at >- ~ r 1 a: !oj ~ 60 u !oj a: z 9; f / / f f p I "" ~ ~ ~40 0 - .J "- 20 ~ -. 1-11- 165 INITIAL 10-4 103 COLLECTOR CCNC::NTR~7,ON.M Fig. 3 Flotation of c~'socolla ~'ith sa1i~'laldoximcand various subsutut~doxi~I' A recentdetailedstudy \\ith severalwater-solublechelaIing agents(fable 6) of the classof aromatichydroxy oxi~s showed 5e\'eralinterestingeffeCtS of substitution.Flotation results obtainedwith thesechemicals,which canbe representedb). the generalformula RI aregiven in Fig. 3. IfR~=H andR.=-H, -CH)or -CHzCHJ CH}) the effea on the oolle-.""tor efficient)' wasobservedto increasein the order -H«-CH)<-CH~CH:CH,. The introductionofth~ fl.'"St-CH2 in SALO resultsin a much largerchangein polari~' of the moleculein comparison with funher additionoft\\.o -CH~ groups.This is reflectedalso in the water-solubilit).of the oximes-SALO, OHAPO and OH-BuPO. Funhermore,the electron-donatingtendenC)'of -CH: group mayalsofavour chelationr~ction. Substitutionof a phenyl group on R. CRz=H)will makethe tDOlecule much lesspolar than SALO, asreflectedin the ~'atersolubili~.. On this basisOHBePOcanbe predictedto havea highercollectorefficien~.than SALO. The actualfmding ,,,'as, ho~'ever,cont~. to the prediction,suggestedasbeingdue to tbe possiblesterichindranceto chelationofferedby the second benzene ring and the slower kinetics of adsorption of OHBePO, Adsorption tests, ho\\'ever, snowed the adsorption of OHBePO on dlrysocolla to be significantly higher than that of SALO at the same oxime concentration, thereby suggesting that Steric hindrance or slow chelation kinetics m~' not be responsible for the lo~'er collector efficienC}' of OHBePO than that of SALO, Bubble size reduCtion observed during flotation may be the major faCtor in this case, Substitution in R2 by -CHJ(R,=CH; or H, respeCtively) not only decreasedthe \\'ater-solubility of the parem oximes but also decreasedthe collector efficienC}', The decteasein "'atersolubili~' is to be expected from the decreasein ~larity of the molecule as a resuh of substitution, The decreasein collector efficien~' could be attributed to the decreasein acid strength of the molecule o,,-ing to the increase in electron densi~' on the phenolic oxygen caused by the nucleophilic substituents,20This can, howe\'er, increase the metal-ligand stability, as is generally observed, 3The effeCt of eleCtron-releasing groups on the ring is, therefore, generally favourable for chelation, Again, the reduCtion in bubble size appears to be the major faCtor in regard to the lo"-er colleCtor efficienC}', This appears to hold for the low collector efficiency obsen'ed in the caseof OHNAO, although the solution concentrations stUdied \\'ere severely limited by its low solubility, Surface chelation I t is now generallybeli~'ed that the adsorptionof xanthateon galenaproceedsby the formation of a chelatecompoundPbX on the surfaceof galena- asopposedto PbX2in the bulk.21 Thus, the fint layer on galenais belie,.edto be PbX (with a high 215 ~ tenacity)overwhich iayen of PbX1build up by 'sheerphysical attachment'.n Taggartand co-workers23 proposedthat surfacecompounds differ greatlyin their propertiesfrom nortnally expectedbulk compounds.This is becausethe lattice ionsor atomson the sunlCehaveonly a part of their coordinationsphereto contributeto the formation of a surfacecompound In addition, stericeffectsassumea particularly significant role for reactions on surfaceof mineral asopposedto thosein the bulk. It is thereforeconceivablethat the first-layer compoundon mineral maybe different from the compoundformed by a reactionin the bulk. If it provesthat the bulk compoundis energetically morefavourable(e\'enafter taking into accountthe fact that adsorptionof collector is, in general,energericallyfavourable), eitherthe collectormoleculesor the surfacecompound comprisingthe collectormoleculesand latticeion or atom will be scaled-offor detached.Of course,contribution to this detachmentcould alsocomefrom physicalfactors. It is not known whetherthere is a direct relationshipbetween surfaceandbulk compounds.In manystudiesa I: I surface chelatehasbeentacitly assumedwith little experimental evidenceto suppon the assumption.Often elaboratestructures for surfacechelateshavebeenproposed24.2S (tWoexamplesare shownin Fig. 4). The imponanceof distinguishingbetWeensurfaceand bulk chelatesandquantitativelydeterminingthem in the samesystem underflotation conditionswasclearlyshownby Nagarajand So~undaran,19.2~.27 Surfacechelatewasfavouredunder certain conditionsandtheseconditionscoincidedwith thosein which flotationof tenoritewasobtainedwith SALO (Fig. 5). The bulk chelateformedunder a ,,'ide rangeof conditionsand this chelate wasineffectivein causingflotation whendispersedin the bulk aqueousphase.This chelate,howe\'er,could aid flotation ,,'henit is still attachedto the first layeron the mineral, asfor thiol collectorson sulphides.Chanderand Fuerstenau28 discussed the rolesof surfacereactionand bulk reactionin the system chalcocite-DTP. Ananathapadmanabhan and Somasundaran,29 basedon detailedcalculationsof relevantmineral-collector equilibria, haveclearlyshownthat much of the flotation results in the literature canbe explainedon the basisof surface reactionsor precipitation (asopposedto bulk reactionor precipitation). The influenceof bulk chelationasopposedto surfacechelation hasnot beentakeninto considemionin the pastfor most systems,evenwhenthe bulk chelationis Vcr)'pronounced.For mineralsthat havefinite solubility (or speciation)in water, bulk chelation(or precipitation)is inevitableif the kineticsof metal chelation(or other complexformation)arereasonablyrapid Any collectorassociated ,,'ith this chelatecanbe considered essentiallywastedin flotation s)"Sterns. Selective flocculation The useof chelatingagentsfor selecti"eflocculation and dispersionhasbeenclearly illustrated by several :~"co.t4 HCi ~.ro,. !' ~ ".}=.I ,0"-/0\ ~'C IC) H + COZ + H2O "C"-ro,-H -1 . ~ ~ 3~ ~ P J,o o .~, J ..-c I 0 ~ l' r-""\ .; --1 '..j -'..1 H ~ d .tC'" ,~-Cu ~, A 4 "'-to .~~ +COz+HaO:? - ~ 0 +COz+~O' :j " --- ~ (';::.yA ~ ~ ('~OH fv.D~~ CuC03gq+ H I~~ I I +(01 + HaO Fig. 4 Schematic illustrations «a)(l,ft}2' and (b) (abot.,f') of surfa~ chtlations 216 invesngators.-- -- 1.nsome 01 these WOrkSCneJatlQggroups were incorporated into a polymeric-type molecule) which acted IS selective flocculants. For example, Sresty and Somasundarann.)7 observed hydroxy propyl cellulose xantha1e containing an active thiol group to produce good flocculation of chalcopyrite with little effect on quartz (Fig. 6). 0 ... " u ~ .. Reagcots 0-0 t~ Minerals Cupferron Salicylaldehyde Q-Nitroso~-naphthol Cassiterite,uraninite, hematite Cassiterite Q)baltite Acctylaccton~ .\1kylhydroxamicacid (IMSO) Malachite, chrysocolla Chrysocolla,hematiteand minerals aIrItainingTi, Y, La, Nb, Sn andW Cassiterite Pbospbonic acids .\'-<.JIy~ P-HydroX}'oximes «-Hydroxyoximes 8-Hydroxyquinoline Cu oxide minerals Cu oxide minerals Cerussite, pyrochiorc, chr}~ocoUa .\' , Iypc Dipbenyiguanidine Dimetbylglyoxime Benzotriazo Ie Cu minerals Ni mi~ra1s Cu minerals S-S r_vpe Xanthates Dithiophosphates Dithiocarbamate5 Dithizone Applications Sulphideand tarnished sulphides Sulphides S -0 ',vl'" X-benzoyl a-alkyl tbionoclrbamac TestS "lth synthetic mixtUres of these minerals showed both grade and recover}- of chalcopyrite in the sedimcnt portion to improve with increase in the concentration of the above polymer, but at Ver)- high dosagesentrapment of the quartz by the bulky cha1cop~-riteflocs caused a decreasein the grade- This problem can, however, be overcome easily by cleaning the product by redispersion follo,,-ed by settling- All sulphid~ minerals .\"-S type .\ \crcaptobenzothiazole Fig. 6 Flocculation of chalcopyrite-andquartz fmcs in terms of per cent solidsscttJedin 45 s asa function of hydrox}-propylcellulosc xanthate(re.ntizing time, 30sy' Sulphides of chelating agents Even though the relativeproportion of chelating-typereagents amongthe industrial non-thio collectorsis not significant, the actualnumber of chelatingagentsthat havebeentested successfullyascollectors,depressantsand flocculantsfor variousmineral systems,at leaston a laboratoryscale,is large (Tables 7,8 and 9). It is e,-identthat the actualuseof these t).pcsof reagentsin the processingof mineralsis likely to undergoa significant rise in the coming decades. 217 ~ TableS Examplesof chelatingagentsasdepressants Reagent Tanaric acid Gallic acid Alizarin red S Starchxanthates CtlIu~ xantbates Mineral Reagents Starchxanthates Cellulosexanthates Selective flocculation and depression of sulphides Poly (4- and S-acr)'lamidosalyclic Cation-exchange polymer for Fe", Cu", Crt- and VOl" acids) Resincontaininghydroxy oximesgroup " ., " ~l}:h~~xamic acids .. " ,. Concluding remarks I t is clearthat althoughchelatingagentscanbe usedeffectively for the flotation of ores,they do not possessabsolutespecificity towardsmineralspeciesand it is only the judiciouschoiceof the chelatingagentsand conditionsfor selectiveseparationthat will maketheir us~possiblefor the beneficiationof many problematicores.In this regarda full understandingof the basic mechanismsinvolved in their chemicalinteractionwith mineral speciesin the bulk and on the surfacebecomesessential,even though thosein the interfacial regionmight be understood accuratelyonly by useof newexperimentalapproachesthat will permit direct probing of this region. The role of surfacechelationversusbulk chelationhasto be takeninto accountin the developmentof any mechanismfor it to be of significant usein flotation. Also, more importantly, the role of surfacechemical alterationsdueto either changein oxidation stateof surface speciesor precipitation of variousdissolvedmineralspecieswill haveto be consideredfor applicationof the aboveinformation in aaual mineralprocessingsystems. Acknowledgement The authorswish to thank the mineralsand primar}' materials programof the National ScienceFoundationfor the supportof this work. References 1. ~'Y~r F. P. and M~llor D. P.~ds.Chelaringagmua7ld_,alchela'es (N~w York: Acadrmic Press,1964),530p. 2. CbaberekS. and Man~U A. E. °rtoni, sequeslfflng agellu(N~w York: WiI~v, 1959). 3. Man~UA. E. and Calvin M. C},n,,;Sll:"of the_tal chelateCompoull4s (EnglewoodCliffs, K.J.: PrenticeHall, 1952). 4. P~rrin D. D. Organi.-.;ompieringreagmls(New York: Wiley, 1964). 5. Pnr$oa R. A.J. Am. chnll. Soc.,85,1963, 3533;J. Alii. Chelll.Soc., 89,1967, 103;J. chmI.Educ.,45, 1968,581;643. 6. K~nk S.F. A. CI'-OT.iinalion cOlllpou7lds (N~. York:AppletonuntUry-Crofts, 1~9),)20p. 7. Glembotskii A. V. Theoreticalprinciplesof foreclStingand modifying collectorpro~nics. Tn.". Melalry, Mosk., 50, no. 91977, 61-4. (Russiant~Xt); TJ':~I.M~Iall.v,N. Y., 18,no. 91977,68-72. 8. Fkming 1.Fronlin or/Iilalsa7ldorganicchemicalreaclioru(London: Wiley, 1976),258p. 9. Cotton F. A. and Wilkinson G. Adtoanced morganicchemistI:'. (London: Int~rscience,1966). 10. Org~1L. E. All i",r£'duc,;on10transition_,al ChemiSll:" (London: Wiley, 1966). 218 11. Zolotov Y. A. Extract;"" ofchelatecompolnlds (Ann Arbor: Humphrey Sciencc,1910). 12. WangT. T.J. Central-SouthInsc.Min. MecalJ.,4,no. 121980, 7-14. (Chineset~xt) 13. BogdanovO. S. et al. Reagentschemisorptionon mineralsasa proccssof formation of surfacecompoundswith a coordinationbond. In Prcxeedings of thel2ch incernationalmineralprocessing congrtss,1977 (SioPlu1o, Brazil: D.N.P.M., M.M.E., 1982),vol. 2,280-303. 14. Morrison R. T. and Boyd R. N. Organicchemistry(Boston:ADyn and Bacon,1972). 15. March J. Adt-anc,dorganicchemiscry: rtactions,mechanisms and st""cur,(N~. York: McGraw-HiD, 1968). 16. Millar I. T. and Springall H. D. Sidgwick'sorganicchtmistryof mtrog,n,Jrdedll (Oxford: QarendenPress,1966). 17. Burger K. Organicreagmcs ill _ca! ana/_vIis (N~w York: P~rgamon, 1973). 18. Burger K. and EgyedI. J. Sometheoreticaland practicalproblems in the useof organicreagentsin chemiClllna1~"Sis, V.J. inorg.IIucl. Clatm.,27,1965,2361-70. 19. NagarajD. R. and Somasundaran P. Cbelatingagentsascollectors in flotation: oximes-coppermin~ra1ss~..ems. "fin. Engng,N. Y., 33, S~pt. 1981,1351-7. 20. Pltel R. P. andPatelR. D. Protonligand stability constantsof some ortbo-hydroX)'ph~nonesand their oximes.J. inorg.nucl.Chem.,32, 1910,2591-600. 21. Gran\.iUr A. Finkelst~in~. P. and Allison S. A. Rt~wof~oDS in the flotation syst~ga1ena-xanthate-oxygen.TNIU. 1IUtnMin. M,call. (Stct. C: Mintral Process. EXIT.M,call.), 81,1972,Cl-30. 22. RaoS. R. Xanthat,sand relatedcompounds (NtW York.:Marcel D~kku, 1971). 23. Taggart A. F. TaylorT. C. and Ince C. R. Experimentswith flotation r~agents.Trans.Am. 1nsc.Min. Engrs,87, 1930,285-368. 24. CecileJ. L. Utilisation d~ riactifs tn flotation. Doctoral thesis, Univ~rsiteOrl~ans,France, 1978. 25. NagarajD. R. Cbelatingagentsasflotlids: hydroximts-copper mineralsysten1s.Doctoraldissenation,Columbia lTniversity, 1979. 26. NagarajD. R. and SomasundlranP. Cbelatingagrotsasflotaids: LIX8-coppu mineralsS}-St~ms. R,cmcDn.tlopmencs in Separation Sc;".a,S, 1979,81-93. 27. NagarajD. R. and Somasundaran P. Commercialcbelating ~xtractantsascolltctors: flOtationof coppermin~ralsusing"LIX" reagents.Trans.Alfl. Insc.Min. Engrs,266, 1979,1892-7. 28. Chandu S. and Fu~rstenauD. W. On th~ floatability of sulfid~ mineralswith thiol coUtctors:th~ chllcocitt/dittb~oJdithiophosphate syst~m.In Proc,edings11thincernacional mintral processingcongreu, Caglian, 19i5 (Cagliari: IstitUto di Ane Minuaria, 1975),583-604. 29. Ananthapadmanabhan K. P. and SomlsundaranP. Chemical tquilibira in h~'droIYZ8ble surfactantsolutionsand their rolt in fk>tabon. Paper~t~d to I 12thAI,\iE annul! meeting,Atlanta, March 1983. 30. Kitcb~ner J. A. Principlts of actionof pol}-m~ricflocculants.Br. Po/.vmer J., 4, 1972,217-29. 31. Somasundaran P. StltctiVt flocculationoffints.ln Thephysical chemistry' of ,nineral-reagmcinttraccionsin sulfid,/location: proceedings of symporium,April 6-7 1978RichardsonP. E. Hy~ G. R. and Ojalvo M. S. comps.lllform. Circ. [,'.S. Bur. Mines8818,1980,150-67. 32. Srcsi)' G. c. RajaA. and Somasundaran P. Selcctiveflocculationof mintral slimesusingpolymers.R«mc Deo/."lopmmls in Separat;.,.. Sci,nu,4,1978,93-105. 33. Somasundaran P. Principlts of flocculation,dispersionand selcctiv~flocculation. In Fin, parricltsproussingSomasundaran P. ed. (Ne~' York: AIME, 1980),\'01.2,947-76. 34. Ania Y. A. and Fu~rstenauD. W. Principlesof separationof or~ minuals by selcctiveflocculation.In R«mc Dn',lopmmu in S'paratiorr Scima, 4, 1978,51-69. 35. Ania Y. A.I. and Kitch~r J. A, Dtvelopment ofcompkxing poly~rs for stkctive flocculationof coppermintrals. Ref~rence28, 1233-48. 36. BaudetG. tl Qt.Syntbes~~t caracterisationd~ flocculantssElectifsi basedc derivesxanmes~ la ceUuloseet de ram~oJost. Induscnt minir.-minhalurgie 1-78,1978,19-35. 37. Srtstv G. C. and Somasundaran P. S~ltcti\'e flocculationof synthetic-mineralmixturesusing modifitd pol~.mers.lnl.J. Mintral Proc,ss.,6, 1980,303-20. 38. ClaussC. R. A. Appltton E. A. and Vink J. J. Seltctiveflocculation of cassittritt in mixtUreswith quartz usingI modified polyacrylamide flocculant.lllc. J. Mintral Pr""ss., 3, 19;6,2;-34. 39. Ania Y. A. Synthtsisof PAMG cl1tlatingpol~.mtrsfor th~ selcctive flocculationof copperminerals.Inc.J. Mineral PrOCtss., 4,1977, 191-208. 40. Rin~UiG. and Marabini A. M. A ne~.~~nt s~-stem for th~ seltctive flocculationof rutile. In Thirctmchinctmacionalminnal proctssingcongress, Warsa11:, 1979LaskowskiJ. ~d. (Amsttrdam, ~tc.: Else~r, 1981),vol. 1,316-45. 41. Rinelli G. and Marabini A. M. Dispersingpropeniesof tanning agentsand ~sibilities of their usein flotation of fine minerals. Reference33, 1012-33. 42 DrZ)omaIaJ. and LaskowskiJ. CJ1elating compoundsasflotation reagents.Physico-ckmicalProbl~msof M;n"aIProc~ssing,13,1981, 39-64. 43. Barber)' G. and CecileJ. C. Complexingreag~ntsin flotation and sclecti\.~flocculation: a ~\itW of possibilitiesand problems.Paper presentedto CIM annualm~~ting,Winnipeg, 1983. 219