Khera, H. C.

Mittal, S. G.

Mohan, M.

Srivastava, A. K.

English

NOPR

Indian Journal of ChemistryVol. 15A, August 1977, pp. 696-699Transition Metal Chemistry of Oxime Containing Ligands:Part III-Complexes of~~Fe(II), Co(II) & Ni(II) withPyridine-z-aldoxime & 6-Methylpyridine-2-aldoximeM. MOHAN*. S. G. MITTAL. H. C. KHERA & A. K. SRIVASTAVADepartment of Chemistry. N.R.E.C. College. Khurja 203131Received 17 June 1976; revised 19 December 1976; accepted 4 April 1977Complexes of the type [M(L),X,] {M= Fe(II) or Co(II); L = pyridine-2-aldoxime (HPOX)or 6-methylpyridine-2-aldoxime (HMPX); and X = CI, Br, I or NCS} and [Ni(L),X,] (L = HPOXor HMPX; and X = N03 or NCS) have been prepared and characterized on the basis of IR andelectronic spectral, magnetic moment and X-ray powder diffraction data. X-ray and electronicspectral data indicate that all the complexes have trans-pseudo-octahedral micro symmetryaround the metal ion. The magnetic susceptibilities for Fe(II) and Ni(II) complexes areindependent of temperature (80-3000K), whereas Co(II) complexes show a slight temperaturedependence of magnetic moment. Mossbauer spectra also indicate pseudo-octahedral geometryfor Fe(II) complexes.A NUMBER of transition metal complexes ofpyridine-2-aldoxime (HPOX) and 6-methyl-pyridine-2-aldoxime (HMPX) have beenreported in literaturev?". In continuation of ourearlier work on Cu(II) and Ni(IJ) complexes ofHPOX and HMPXll,l2, we report here the resultsof our investigation on the isolation and charac-terization of Fe(II) , Co(U) and Ni(II) complexes ofHPOX and H~iPX.Materials and MethodsFe(II). Co(IJ) and Ni(Il) salts. ammoniumthiocyanate (all reagent grade), pyridine-2-aldoximeand 6-methylpyridine-2-aldoxime (K & K Labora-tories) were used without further purification.Preparation of the complexes: FeL2X2 (L = HPOXor HMPX, and X = Cl , Br or I) - A solution offerrous halide (0·004 mole) in 70 ml of deoxygenatedabsolute ethanol was prepared and kept under astream of N2 gas. A solution of the ligand (0·008mole) in 90 ml of absolute ethanol was preparedby heating while bubbling a rapid stream of N2through the solution. The solution of ferrous halidewas then added very slowly under a stream of N2 tothe solution of the ligand. A red colour formed im-mediately, and a precipitate formed within minutes.The mixture was allowed to stand for 30 min underN2, then heated to boiling and filtered hot viasuction through a sintered glass under N2. Theprecipitate was dried in vacuo.FeL2(NCS)2 (L = HPOX or HMPX) - Anethanolic solution of ferrous thiocyanate (0·002mole). prepared from ferrous chloride tetrahydrateand NH4SCN, was filtered into a solution of theligand (0·005 mole) in hot ethanol (20 ml) and2,2' -dimcthoxypropane (20 ml). The mixture wasgently boiled under N2 gas for 30 min. The solidproduct was collected by filtration in an atmosphereof N2 and washed with anhydrous ethanol and ether.*To whom aU correspondence should be addressed.696CoL2X2 (L = HPOX or HMP X, and X = Ct. Bror I) - Anhydrous coba.lt(U) halide (0·01 mole)was dissolved in a minimum quantity of ethanoland the ligand (0·02 mole) dissolved in ethanol wasadded. On cooling the solution in refrigerator, apink crystalline solid was obtained. The complexwas filtered and washed with a small amount ofethanol and ether.CoL2(NCS)2 (L = HPOX or HMPX) - Cobaltchloride hexahydrate (0·01 mole) was dissolved inwater (20 ml) and the ligand (0'02 mole) dissolvedin a minimum quantity of hot ethanol was added.On adding excess solid NH4SCN a pink precipitatewas obtained immediately. The solid was filteredand washed well with water to remove any excessof thiocyanate and then with a small quantity ofanhydrous ethanol and cliethylether.NiL2(NOa)2 (L = HPOX or H111PX) _. Ni(K03h-6H20 (0·006 mole) was dissolved in a mixture of25 ml of ethanol and 25 ml of 2.2'-dimethoxypropaneand solution refluxed for several hours. The ligand(0·014 mole) was dissolved in 25 ml of 1:1 ethanol-2,2'-dimethoxypropane, refluxed and added dropwisewith continuous stirring to the hot metal saltsolution. Crystallization occurred almost im-mediately. A dark green solid was collected byfiltration, washed with anhydrous ether and driedin vacuo over P20S'NiL2(NCS)2 (L = HPOX or HMPX) -- A suspen-sion of NiL2(NOa)2 (0·01 mole) in absolute ethanolwas treated with solid NH4SCN (0·02 mole). Thegreen solid turned dark blue on shaking the mixture.The product was filtered and washed with ethanoland dried in vacuo over P20S'Physical measurements - Infrared spectra wererecorded in mull on Perkin-Elmer infracord, model180 (4000-400 crrr") and Beckman IR-12 (400-200crrr") instruments. Diffuse reflectance spectra atroom temperature and liquid nitrogen temperaturewere recorded on a Cary spectrophotometer modelMOHAN et al.: COMPLEXES OF OXIMES14 equipped with a diffuse reflectance accessoryusing magriesium oxide as the reference. Magneticmeasurements were obtained at various temperatures(80-300CK) on a standard Gouy balance. Thetube was calibrated with Co[Hg(NCS)4J as thestandard,X-ray powder photographs were obtained usinga Philips (Hungary) X-ray generator, nickel filteredcopper radiation and a Debye-Scherrer camera.A conventional constant acceleration Mossbauerspectrometer was used to obtain the Mossbauerspectral data with an accuracy of ± 0·01 mm/sec.C, Hand N analyses were obtained from themicroanalytical laboratory of IIT, Kanpur. Metalswere analysed by standard techniques's after de-composition of the complexes with aqua regia.Halide analyses were carried out by potentiometrictitration with AgN03, after decomposition of thecomplexes by sodium fusion. The analytical dataare presented in Table 1.Results and DiscussionThe X-ray powder diffraction patterns for presentcompounds and [Fe(pY)4(NCShJ suggest that all thecompounds are isomorphous. Therefore, in analogywith the known structure-s of [Fe(pY)4(NCS)2]the present complexes may also have trans-octahedralgeometry.The IR spectra of oximes normally show \lOHaround 3250 cm", This band is replaced bymultiple bands between 3194 and 2791 cm! inHPOX and HMPX, the strongest of which lies at",2791 crn'". This implies much stronger hydrogenbonding in HPOX and HMPX than in other oximes.The \lC=N in HPOX and HMPX occurs around1520 cm-l and is in the range observed by Krauseet c~l.3for oximes, The ring stretching frequencies,ring breathing mode, \IN-O, out-of-plane C-H defor-mation, skeletal modes and out-of-plane deformationbands appear in the regions 1620-1425, ",1000,",950, ",800, ",740 and ,....400 crrr+ respectivelyin HPOX and HMPX ligands.All the present complexes show bands in theregions 3250-3015, 1635-1630 and 1074-1040 cm-lwhich can be assigned to \lOH, \lC=N and \IN-Ofrequencies respectively. These data show thatoxime proton is not removed on complex forma-tion.The complexes of the general formula [M(L)2X2J{M = Fe (II) , or Co(II); L = HPOX or HMPX; andX = Cl, Br I or NCS} and [Ni(L)2X2] (L = HPOXor HMPX, and X = N03 or NCS) exhibit the fourring stretching frequencies in the following ranges:band-I, 1618-1612; band-II, 1578-1574; band-HI,1490-1477; and band-TV. 1440-1426 em'<. Band-Ishows a significant increase in frequency from thefree ligand value of ",1570 crrr<, an indication ofthe coordination of pyridine to the metal atom-s.The ring breathing mode observed at ......,996 em'?in the free ligands disappears in the complexes andis replaced by a band at 1005-1020 cm=. This shiftis also indicative of pyridine coordinationw,Two strong bands are observed in the spectra offree ligands at 798 and 741 crrr? which may be as-signed to \I(C-H) and \I(C-C) respect ivclytt The741 cm'" band splits into two components lying at718 and 752 cm". This splitting is also an indica-tion of pyrdine to metal coordination-e. The bandobserved at 798 cm" in the free ligands is observedas a single band lying between 780 and 824 crrr" inthe comtIexes,In thespectra of [M(L)2(CI)2]{M= Fe(II) or Co(U);and L = HPOX or HMPX} complexes, two bandsare observed at 240 and 270 em"! which may beassigned to \lM-Cl and \lM-N modes, respectively.The band at 270 cm-l cannot be assigned to \lM-Cl,since it is rather too high in energy and a band ofsimilar energy appears in the spectra of all the re-maining complexes also [including Ni(II) complexes].However, the \lM-Br and \lM-! bands appear belowTABLE 1 - ANALYTICALDATAOF THE COMPLEXESCompounds* Found (calc.). %C H N Metal XtFe(C.H.C\,O)2(CI)2 38·94 (38·84) 3·27 (3·23) 15·08 (15·10) 15·14 (15·08) 19·17 (19·14rFe(C.H.K2O),(Br), 31·34 (31·31) 2·57 (2·60) 12·19 (12·17) 12·65 (12·15) 34·82 (34·78)Fe(C.H.N2O)2(I)2 26·14 (26·00) 2·12 (2·16) 10·15 (10·11) 11·24 (10·09) 45·96 (45·85)Fe(C.H.N,o)2(KCS)2 34·69 (34·63) 2·98 (2·88) 13-97 (13-47) 14·10 (13·45) 28·20 (27·90)Fe(C7H.N,O)2(Cl)2 42·22 (42·11) 4-18 (4-01) 14-19 (14·04) 14·18 (14·02) 17·92 (17·80)Fe(C7H.N.O),(Br)2 34·50 (34·43) 3·23 (3·28) 11·51 (11-48) 11·82 (11·46) 32-86 (32·79)Fe(C7H.N2O)2(1), 29·10 (28·87) 2·82 (2·74) 9·74 (9·62) 9·90 (9-60) 43·72 (43·64)Fe(C7HsN,o)2(C\CS)2 37·99 (37·84) 3·72 (3·68) 12·70 (12-62) 12-90 (12·59) 26·52 (26·13)Co(C.H.X2O).(Cl)2 40·00 (38·50) 3·28 (3·20) 15·10 (14·97) 15·99 (15·78) 19·20 (18·99)Co(C.H.N.O)2(Br)2 31-19 (31·11) 2·62 (2·59) 12·30 (12·10) 12·95 (12·75) 34·60 (34·55)Co(C.H.N2°),(I)2 26·10 (25·85) 2·17 (2·15) 10·20 (10·06) 10·71 (1059) 45·70 (45·59)Co(C.H.K20).(:SCS), 34·41 (34·48) 2·90 (2·86) 13-42 (13·37) 14·28 (14·08) :1'1·80 (27·69)Co(C7HsN.o).(CI)2 41-84 (41·79) 4·20 (3·98) 14·12 (13·93) 14·91 (14·68) 17·85 (17·66)CO(C7HSN,O)2(Br). 34-42 (34·22) 3·36 (3·25) 11-42 (11·40) 12·14 (12·01) 32·70 (32-58)Co(C7HsN2O).(I)2 28·86 (28·72) 2·81 (2·73) 9·68 (9·57) 11·02 (10·09) 43·50 (43·41)Co(C7HsN2O)2(NCS). 37·70 (37·58) 3·70 (3·58) 12·66 (12·53) 13·97 (13·20) 26·20 (25·95)Ni(C.H.N,O)2(N03), 33·86 (33·75) 2·90 (2·81) 13-90 (13·76) 19·90 (19-69)Ni(C7HsN2O).(NO,), 37·12 (36·94) 3·62 (3·51) 18·52 (18·47) 13·30 (12-90)Ni(C.H.N,O),(NCS), 34·62 (34-40) 2·92 (2·86) 13-50 (13·38) 14-44 (14·02) 27·86 (27·71}Ni(C7H,N,O),(NCS)2 37·79 (37·61) 3-69 (3·58) 12·76 (12·58) 13·39 (13·14) 26·12 (25·97)*C.H.N20 = pyridine-2-aldoxime, C7HsN.O = 6-methylpyridine-2-aldoxime.tX = ci, Br, I, NO. or NCS.697INDIAN J. CHEM., VOL. 15A, AUGUST 1977200 crrr- outside the range of the instrument usedin the present study.IR data indicate that both the nitrate groups in[Ni(L)2(NOa)2J are coordinated. Assignments of Vlat 1310, V2at 1038 and Vaat 825 em? agree wellwith the published values for coordinated nitrategroups19,20. The very strong bands at 740 and1510 em'? can be assigned to the Vaand V4modesrespectively. IR bands usually associated withionic nitrate groups (Dah symmetry) were absentin the spectra of all the complexes studied.The occurrence of a strong band (vC=N) around2045 cm-1 in [M(L)2(NCS)2J {M= Fe(IJ) , Co(U) orNi(II); and L = HPOX or HMPX} indicates thepresence of N-bonded thiocyanate group2l-25. Theoccurrence of a band around 882 cm-1 which mavbe assigned to vC-S further corroborates the presenceof an N-bonded thiocyanate group'",The magnetic moments for Fe (II) , Co(lI) andNi(II) complexes have been measured as a functionof temperature (80-3000K) (Table 2). The magneticTABLE 2 - MAGNETICSUSCEPTIBILITIESOF THECOMPLEXESCompound Temperature(OK)297'5-83,0298,0-83,0295,0-101· 5297·5-103·5292·5-104·5290'5-102'5294'5-103'5290·5-102·5298,0-103'5296,5-103,0292'5-103·0291'5-101'5297'5-101'5299·5-105·0300·0-104·5295·5-104·0298·5-104·5297·5-104·0299·5-104·5292·5-101·5fLefi(BM)5,29-5'275'56-5'565'59-5'575'40-5·385,32-5'325'54-5'545-60-5'585,38-5'374·60-4-544·58-4-484·65-4·564·62-4·544·59-4·504·56-4-504'67-4·584'60-4·523-28-3-253-30-3-273-29-3-243-30-3-25Fe(HPOX).CI2Fe(HPOXl.Br.Fe(HPOX).I2Fe(HPOX)a(NCS).Fe(HMPX).Cl.Fe (HMPX).Br.Fe(HMPXl.I2Fe(HMPXl.(NCS).Co(HPOX).CI.Co(HPOX).Br.Co(HPOX).I2Co(HPOX).(NCS).Co(HMPX)2CI•Co(HMPX).Br2Co (HMPX).I.Co(HMPX) (NCS)aNi(HPOX).(NO.).Ni(HPOXl.(NCS).Ni(HMPX).(NO.).Ni(HMPX).(NCSl.moments of Fe (II) and Ni(IJ) complexes areessentially independent of temperature between107° and 298°R. The magnitude and temperatureindependence of the moments are in accord withtetragonally distorted octahedral, high spin struc-tures26-28_ Co(II) complexes show a slight tern-perature dependence of magnetic moments, theCurie-Weiss law is obeyed and the values of 6 arerelatively smalls".The electronic absorption spectra of Fe(II)complexes of the type [Fe(L)2X2] (X = Cl, Br, Ior NCS) are similar to one another. For Fe (II)complexes in the 0" field, a single electronic spectralband corresponding to the transition 5T2g-+5Eg isexpected and is usually observed around 9 kK30_If the field is lowered to D4 symmetry, state 5T2g issplit into the states 5Eg and 5B2g while the state 5Egsplits into 5A1g and 5B1g states.The reflectance spectra of the present Fe(IJ)complexes exhibit broad partially resolved bandsat 9 and 12 kK at room temperature and 9·2 and12'3 kK at liquid nitrogen temperature. On the basisof-a D4h symmetry, we assign the 9 kK band to thetransition 5B2g-+5Alg and the 12 kK band to thetransition 5B2g-+5B1g_ The small increase in theenergies of the electronic transitions at liquidnitrogen temperature is most likely a result of in-crease in the ligand field strength with decreasingtemperature which arises from a slight contractionof the unit cell volume at low temperature. Thespectra of the Fe(Il) complexes show a very strongand broad band at 18 kK also, which may be assignedas a charge-transfer band arising from metal toligand (t2g-+7t*) charge-transfer.The room temperature Mossbauer chemical isomershift, a, relative to iron foil is found to lie in therange 0·96-1·05 rum/see for several octahedral highspin, Fe(II) complexes containing nitrogen donoratoms31-33. We have studied the Mossbauer spectraof the [Fe(L)2X2J complexes at several temperaturesand the spectral parameters are given in Table 3which confirm pseudo-octahedral nature of thesecomplexes when compared to the Mossbauer dataof compounds of known structures'",TABLE 3 - M5sSBAUER SPECTRALPARAMETERSCompound T 8* ilEQ r1t r.t(OK) (mmjsec) (mm/sec) (mni/sec) (mmrsec)Fe(HPOX).(CI). 78 H6 2-00 0-26 0-26RT 1-06 1-54 0-25 0-24Fe(HPOX).(Br). 78 1-14 2-00 0-25 0-26RT 1-05 1-54 0-25 0-24Fe(HPOX).(I). 78 H2 1-96 0-26 0-25RT 0-99 1-50 0-25 0-24Fe(HPOXl.{NCS). 78 H5 2-00 0-25 0-25RT 0-98 1-49 0-25 0-24Fe(HMPX)2(CI)a 78 H5 1-99 0-26 0-26RT 1-04 1-53 0-26 0-25Fe(HMPX).(Br). 78 H2 1-99 0-25 0-25RT 1-02 1-50 0-25 0-24Fe(HMPXla(I). 78 HO 1-96 0-26 0-26RT 1-00 1-49 0-26 0-25Fe(HMPX).(NCS). 78 H4 1-96 0-25 0-24RT 0-98 1-49 0-25 0-25*Relative to natural iron foil.tFull width at half-maximum for low-velocity line 1\ and high-velocity line r2-698MOHAN et al.: COMPLEXES OF OXIMESTABLE 4 - CRYSTALFIELD PARAMETERS(eM-I) OF Ni(II) COMPLEXESCompound B Dqxy Dqz Dx Dt Dol Do3Ni(HPOX),(N03), 824·6 1174 644 533·5 290·1 150 3584·5Ni(HPOX).( TCS). 808·2 1150 600 634·5 314·7 330 4111·8Ni(H IPX),(NO,) 821·2 1173 672 523·1 286·2 138 3523-4Ni(HMPX)2( res), 815·2 1149 592 636·6 318'7 316 4139·9The electronic spectra of [CO(L)2X2J (X = Cl,Br, I or 1\CS) are similar to one another. The re-flectance spectra of Co(II) complexes consist of abroad band centred at 9·6 kK with a weak shoulderat 8·5 kK and a set of four closely spaced and moreintense banels at 18'6, 19'4, 20·1 anel 21·1 kK.Spin-allowed transitions for Co(U) in ell fieldare 41 g(F)-'»-4T2g(F)(Vl)' 4T1g (F)-'»-4A 2g(F)(V2l and4T 19(F)-'»-4T Ig(P)(V3)' The V2transition is a two-elec-tron transition and is normally not observeds+, Thusthe low-energy band is assigned to the VI transitionand the bands at 19·4 and 20·1 kK are assigned asthe components of Vs band. The structured natureof Vs is not uncommon in the spectra of Co(II)complexes and is considered to arise either fromspin-forbidden transitions to doublet terms or fromlow-symmetry ligand field components'". The latterfactor is of particular significance in the presentcase in view of the highly distorted octahedral coor-dination geometry. The bands observed at 8·5,18'6 and 21·1 kK, which on cooling to liquid nitrogentemperature intensify without changing in position,can be assigned to the transitions 4Tlg(Fl~Eg(H),'T1g-,»-4T2g, 2T1g, and 4Tlg(F)-'»-2Tlg(H) respectively.The reflectance spectra of Ni(II) complexes,[Ni(L)zX2J (X = NOs or NCS), exhibit features asso-ciated with the spectrum of [Ni(pyh(NCS)2J complexwhich has been shown to possess the nickel atomin distorted octahedral environrnent ", Therefore,the bands observed at 9·0, 11'7, 14·9, 16'8, 25·8 and26'7 kK in the present complexes may be assignedto the transitions sB1g-,»-3E g, sB 19-,»-3B2g, 3B 19-,»-3A2g,3B1g-'»-3Eg, 3B1g-,»-sA2g and 313.1g-'»-3Eg. The ,ligandfield parameters, calculated using the methods des-cribed by Lever-", are presented in Table 4 whichconfirm the pseudo-octahedral (D4h) coordinationfor these complexes.Acknow ledgernentWe are thankful to Dr P. C. Gupta and Dr A. S.Bhatnagar for providing necessary facilities andencouragement. Financial support to S.G.M.and H.C.K. by the UGC, New Delhi, is gratefullyacknowledged.References1. KRAUSE, R. A. & BUSCH, D. H., J. Am. chem. Soc., 82(1960), 4830.2. KRAUSE, R. A., JICHA, D. C. & BUSCH, D. H., J. Am.chem. Soc., 83 (1961), 528.3. KRAUSE, R A., COLTHUP, N. B. & BUSCH, D. H.J. phys. Chem., 65 (1961), 2216. '4. KRAUSE, R. A., GUY, C. & HOOKER,M. L, Inorg. Chem5 (1966), 1825. .,5. HANANIA, G. J. H. & IRVINE, D. H., J. chem. Sac(1962). 2745. .,6. Lnr, C. H. & Lru, C. F., J. Am. chem. Soc. 83 (1961)4167. ' ,7. Lru, C. F. & Lru, C. H., J. Am. chem. Soc., 83 (1961)~~. '8. GREEN, R. W. & SVASTI,M. C. K, Aust. J. cu»: 16(1963), 356. '9. HOLMES, F., LEES, G., UNDERHILL, A. E. & POWELLD., J. chem, Soc., (A) (1971), 333. '10. HOLMES, F., LEES, G. & UNDERHILL, A. E., J. chemSoc., (A) (1971), 999. .11. MOHAN,M., KHERA, H. C., MITTAL,S. G. & SRIVASTAVAA. K, Curro su., 46 (1977), 211. '12. MOHAN,M., KHERA, H. c.. MITTAL,S. G. & SRIVASTAV!\A. K., Acta chim., (in press). . ,.13. 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Transition Metal Chemistry of Oxime Containing Ligands: Part III-Complexes of Fe(II), Co(II) & Ni(II) with Pyridine-2-aldoxime & 6-Methylpyridine-2-aldoxime

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Transition Metal Chemistry of Oxime Containing Ligands: Part III-Complexes of Fe(II), Co(II) & Ni(II) with Pyridine-2-aldoxime & 6-Methylpyridine-2-aldoxime

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