Conseguences of soil crude oil pollution on some wood properties of olive trees Chemistry | 103 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Synthesis and Characterization of Transition Metals Ions Complexes with 2-Thioxoimidazolidin-4-One Schiff Base as Ligand Sinan Midhat Al-Bayati Anaam Majeed Rasheed Enas Zuhair Mohammed Zeina Kudair Hassan Amjad Chali Amal Mohammed Hussein Dept. of Chemistry/ College of Science/Al-Mustansiriyah University Received in:21/December/2015,Accepted in:30/March/2016 Abstract Mn(II), Co(II), Ni(II), Cu(II), and Cr(III) metal complexes with the ligand (L) [3-(2- nitro benzylidene) amino-2-thioxoimidazolidin-4-one] have been prepared and characterized in their solid state using the elemental micro analysis (C.H.N.S), flame atomic absorption, UV-Vis spectroscopy, FT-IR, magnetic susceptibility measurements, and electrical molar conductivity. The ratio of metal to ligand [M:L] was got for all complexes in the ethanol by using the molar ratio method, which produced comparable results with those results obtained for the solid complexes. From the data of all techniques, octahedral geometry was proposed for Cr(III), Mn(II), and Co(II) complexes, while tetrahedral structure was proposed for Ni(II), Cu(II) complexes. Keywords: Synthesis, Characterization, Bidentate Schiff Base, Transition Metal Complexes. Chemistry | 104 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Introduction Many Schiff base compounds of thiosemicarbazones and their complexes have been widely used and applied in biological, analytical, and pharmaceutical activities [1-3]. Studies of many Imidazol derivatives and their important heterocyclic complexes have been examined for their important biological activities like antibacterial, antifungal, anti-inflammatory, and analgesic [4]. However, these compounds have been variously used in the spectrophotometric determination of the metal ions. Therefore, many of those reagents give intense colors when react with the ions of transition metal [5]; providing probes that some of them can coordinate to rare earth ions also, forming the metal complexes whose interesting structures [6]. In the present paper, the preparation of Schiff base derivative [3-(2-niro benzylidene) amino -2-thioxoimidazolidin-4-one] (L) was used as ligand that provides two sites “potential donor” to produce some transition metal ions. (L) ligand and its complexes have been completely characterized. Experimental All the used chemicals were analytical annular and were highly pure. The Physical Measurements and Analysis The melting points were measured using Gallen Kamp melting point instrument and were uncorrected. While, FT-IR spectrum was measured using Shimadzu-8300 spectrophotometer at the range (4000-400 cm -1 ). UV-Vis. Spectrum was recorded on UV-1650-PC-Shimadzu spectrophotometer at room temperature. Furthermore, all these measurements were measured on a concentration of 10 -3 M of the complex in absolute ethanol as a solvent. The elemental (C.H.N.S) analysis was performed on an EM-017 mth instrument. The atomic absorption of the prepared complexes was measured using “Shimadzu Atomic Absorption 680 Flame” spectrophotometer. Moreover, the conductivity measurements were recorded on W.T.W. conductivity meter. All these measurements were got in “DMF” as a solvent using the concentration of (10 -3 M) at 25 o C. The measurements of magnetic susceptibility were got at 25 o C in solid state using Faraday’s method at “Bruker BM6” instrument. Synthesis 1- Synthesis of 2-nitro benzylidene thiosemicarbazone (1) A mixture of compound 2-nitro benzaldehyde (1.51 g, 0.01 mole) with thiosemicarbazide (0.91 g, 0.01 mole) was refluxed for 4 hrs. in the absolute ethanol (20 ml), the solvent was segregated, the solid product was collected and crystalized [7]. 2- Synthesis of [3-(2-nitrobenzylidene) amino-2- thioxoimidaz-olidin-4- one] (2) Mixture of the compound (1) (2.24 g, 0.01 mole) and (1.22 g, 0.01 mol) of ethylchloroacetate in (30 ml) of absolute ethanol and then sodium acetate (0.03 mole) was added. Afterwards, the mixture refluxed for 20 hrs. and cooled down to room temperature. The resulting solid recrystallized, and the prepared ligand physical properties are described in (Table 1). The structure of the proposed ligand is shown in scheme (1). Chemistry | 105 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 3- Synthesis of Complexes (C1-C5): Ethanol solution of each one of the following quantities of the metal ion salts (1mmol) (0.266, 0.198, 0.238, 0.237, 0.170) g of [CrCl3.6H2O, MnCl2.4H2O, CoCl2.6H2O, NiCl2.6H2O, and CuCl2.2H2O] was respectively added to ethanol solution (1mmole, 0.264 g) of (L) with continuous stirring. The mixture then heated with reflux for 2 hrs. Over this time, a precipitate starts forming, which was filtered, washed with water, recrystallized from the ethanol, and then dried using the oven at 50 o C for one hour. The prepared complexes physical data are shown in (Table 1). Results and Discussion Characterization of ligand (L) along its complexes was achieved by: (A) The Elemental Micro Analysis (L) and its metal complexes physical and analytical data are shown in (Table 1), which came in satisfactory agreement with the calculated values. The suggested molecular (formulas) are also supported with the subsequent spectra and the molar ratio, besides the magnetic moment. (B) Studying the Formation of Complex in Solution (L) complexes with the metal ions were thoroughly studied in the solution using the ethanol as a solvent to determine the ratio of [M:L] in the complex by depending the molar ratio method [8, 9]. A number of solutions were prepared whose a constant concentration (10 -3 M) for metal ion and (L). The ratio of [M:L] was set depending on the relationship between the light absorption and the [M:L] mole ratio. The complexes results of formation in solution suggested [1:1] metal to ligand for [C1-C5] that were comparable to those got in the study of solid state, (Table 1). (C) 1 H-NMR Spectra The spectrum data of the free ligand (L) in DMSO-d6 solution was reported along with the possible assignments in experiment. The NMR spectrum of the proton showed peaks at (8.8) ppm (s, 1H, N=CH), (7.9-8.2) ppm (S, 4H, phenyl-NO2), (4.1-4.2) ppm (m, -CH2), and (12.3) ppm (1H, bs, NH) [11]. The number of protons calculated from integration curves and the recorded chemical shifts in (Figure 1) reveal the proposed structure of the formed ligand (L). (D) Infrared Spectroscopic Study FT-IR spectra provided good information about complex behavior of the ligand with varied metal ions. The distinctive frequencies of the ligand and its metal complexes have been assigned in comparison to the values found in literature [10]. The structure of the ligand was affirmed by υ(C=O, C=S) imidazole stretching vibrations presence at (1728, 1201) cm -1 besides the band that appeared at (1631) cm -1 due to the azomethine group υ(C=N) [11], (Table 2), (Figure 2). With all complexes (C1-C5), the ligand (L) behaves as bidentate that coordinate to metal ion throw carbonyl imidazole oxygen and the azomethine group nitrogen; so the bands of (υC=O, and υC=N) were consequently shifted to lower frequencies [12], but the band at (1201) cm -1 of υC=S mode remained without change in all complexes, (Table 2). Moreover, these observations were indicated by (υM-N, υM-O and υM-Cl) appearance at (543-536) cm -1 , (470-455) cm -1 and (316-324) cm -1 respectively [12], (Table 2). Also, there is a broad band observed nearly at (3464-3406)cm -1 and weak band range at (952- Chemistry | 106 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 940) cm -1 in the complexes spectra that assigned to a (υO-H) suggested water molecules presence in the complexes [11], (Figure 3). (E) Studying of Electronic Spectra, Magnetic Moment, Conductance: The ligand (L) UV spectrum mostly showed two intense absorption peaks at 48543cm -1 and 34482 cm -1 , which belong to π→ π*, and n→ π* respectively [11], (Table 3), (Figure 4). The ligand metal complexes electronic spectra were measured for their solution in the absolute ethanol at the range (200-1100) nm, whereas the molar conductance was measured in dimethyl formamide (DMF) as a solvent. [Cr(L)(H2O)2Cl2]Cl: The electronic spectrum of Chromium (III) complex showed three absorption peaks in the region (15408, 21691, and 28571) cm -1 , respectively, which attributed to ( 4 A2g→ 4 T2g(F), 4 A2g→ 4 T1g(F), and 4 A2g→ 4 T1g(P)) transitions. These peaks positions are in a good agreement with octahedral geometry that are reported [13]. Additionally, the magnetic moment µeff., which is measured at room temperature was (3.82 B.M) that reveals high-spin inner-orbital octahedral stereo chemistry for the ligand around Cr(III) metal ion [14], (Figure 6). Furthermore, the conductivity in (DMF) demonstrated that the complex is ionic [1:1], (Table 3). [Mn(L)(H2O)2Cl2]: The electronic spectrum of Mn(II) complex showed absorption bands at (16891, 27173) cm -1 due to the transitions 6 A1g→ 4 T1g(G) , 6 A1g→ 4 T2g(D), respectively, indicating octahedral geometry [15]. The measured magnetic moment µeff. of Mn(II) complex is (5.18 B.M) which corresponds to five unpaired electronic indicates high-spin octahedral environment [16], (Table 3). Measuring the conductivity in (DMF) demonstrated that this complex has non-conductive behavior, (Figure 7). [Co(L)(H2O)2Cl2]: The electronic spectrum of Co(II) complex showed three peaks at (14858, 16528, and 30303) cm -1 assignable to 4 T1g→ 4 A2g(F), 4 T1g→ 4 T1g(P), and C.T transitions, respectively, (Table 3), (Figure 5) for an octahedral geometry [17]. Moreover, the magnetic moment µeff. of this complex in the sold state (4.50 B.M) suggests a high-spin octahedral geometry [18]. Furthermore, measuring the conductivity in (DMF) demonstrated that this complex has a non-conductive behavior, (Figure 7). [Ni(L)(H2O)Cl]: The electronic spectra of Ni(II) complex appears at (32786) cm -1 and this attributed to the charge transfer transition (C.T). in addition, the other peak which appears at (27397 cm -1 ) can be attributed to to ( 3 T1→ 1 T2) electronic transition, what suggests a tetrahedral geometry [19] around Ni ion. The magnetic measurement µeff. of the solid complex (3.21 B.M) demonstrated two unpaired electrons for Ni(II) ion which again suggests a tetrahedral geometry for Ni(II) complex [20]. Measuring the conductivity in (DMF) shows that this complex is ionic [1:1], (Table 3), (Figure 8). [Cu(L)(H2O)Cl]Cl: The electronic spectra of Co(II) complex demonstrated a peak at (3205) cm -1 which refers to (C.T) transition, while the peak that appears at (12658) cm -1 is attributed to ( 2 T→ 2 E) electronic transition. However, these transitions indicate that the complex has a tetrahedral geometry [21, 22]. Moreover, the value of measuring the magnetic moment is (1.87 B.M), what corresponds to one unpaired electron. Furthermore, measuring the conductivity in (DMF) demonstrated that the complex has electrolyte behavior [1:1], (Table 3), (Figure 8). Chemistry | 107 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Suggested Structure for the Complexes [C1-C5] According to the obtained results from the elemental and spectral analyses, besides measuring the magnetic moment and conductivity, the above mentioned compounds suggested structures can be explained as follows: Figure(6), Figure(7) and Figure(8). References 1. Konstantinovic S. S.; Rodovanovic B. C. and Soviij S. P., (2008), “Antimicrobial Activity of Some Isatin-3-Thiosemicarbazone Complexes”, J. Serb. Chem. Soc., 73(1) :7-13. 2. Shayma, A. S., (2010), “Synthesis, Spectral and Magnetic Studies of Newly Mixed Ligand Complexes of 4-Formyl Acetanilide Thiosemicarbazone and 3,4- Dihydroxy-Cinnamic Acid with Some Metal Ions”, Accepted in Journal of Chemistry, (in Press), 7(5). 3. Carolin, S., Hashim, and Mahasin F. Alias, (2012), “Synthesis, Spectroscopic study of Pt(IV), Au(III), Rh(III), Co(II), and V(IV) Complexes with Sodium [5(p-Nitro Phenyl)-4-Phenyl-1,2,4-Triazole-3-Dithiocarbamato Hydrazide] and Cytotoxicity Assay on Rhabdomyosarcom a Cell Line of Heavy Metals”, J. Baghdad for Sci., 9(4) :668-679. 4. Patel, A., Bari S.; Talele, G.; Patel J., and Sarangapani M., (2006), "Synthesis and Antimicrobial Activity of Some New Isatin Derivatives", Iranian Journal of Pharmaceutical Research, 4 :249-254. 5. Al-Hasani, R. M.; Al-Abodi., A. K., and Kadem, S. A., (2009), "Synthesis, Structural Study, and Antibacterial Activity of Pd(II), Ru(III), Rh(III), Au(III) and Pt(IV) Complexes of 4-Nitro-3-{[4-(4-Hydroxy Phenyl)-2-Methyl-5-Oxo-4,5-Dihydro- 1H-Imidazol-1-yl]Imino}-1,3-Dihydro-2H-Indol-2-One", Journal of Al-Nahrain University, 12(2) :35-45. 6. Smit, B. J., and Pavlovic, R. Z., (2013), “Synthesis, Characterization and Cytotoxicity of Palladium(II) Complex of 3-[(2-Hydroxybenzylidene) Amino]-2- Thioxoimidazolidin-4-One”, J. Serb. Chem. Soc., JSCS-4410, 78(2) :217-227. 7. Abd El-Fattah, M. E.; Soliman, A. H., and Abd Allah, H. H., (2010), In Proceedings of the 14 th International Electronic Conference on Synthetic Organic Chemistry (ECSOC-14), CD-ROM, MDPI, Basel, Abstract No. B024. 8. Skooge, D. A., (1988), "Fundamentals of Analytical Chemistry", 5 th Ed., New York. 9. Douglas, A. S.; Donald M. N.; Holler F. J.; Crouch S. R., and Chen S. C., (2011), “Introduction to Analytical Chemistry”, Case Bound, 1 st Ed. 10. Nakamoto, K., (1997), "Infrared of Inorganic and Coordination Compounds", 6 th Ed., John-Wiely Inc., New York, London. Chemistry | 108 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 11. Silverstein, R. M.; Bassler G. C., and Morrill T. G., (1988), "Spectrometric Identification of Organic Compounds", 5 th Ed., John-Wiley and Sons Inc., New York. 12. Nakamoto, K., (2009), "Infrared and Raman Spectra of Inorganic and Coordination Compounds", John Wiley and Sons Inc., New Jersey. 13. Sutton, D., (1968), "Electronic Spectra of Transition Metal Complexes", 1 st Ed., Mc.Graw-Hill Publishing, London. 14. Burger, K., (1973), "Coordination Chemistry, Experimental Methods”, Bult/Worths and Co. Publishers Ltd., London. 15. Figgis, B. N., and Hitchman M. A., (2000), "Ligand Field Theory and its Application", Wiley-VCH, New York, Singapore, Toronto. 16. Solomon, E. I., and Lever A. B. P., (2006), “Inorganic Electronic Structure and Spectroscopy: Applications and Case Studies”, (II), John Wiley and Sons Inc., New York, Chster, Singapore, Toronto. 17. Nichollas, D., (1973), "The Chemistry of Iron, Cobalt and Nickel", Pergamun Press, Oxford. 18. Mohammed, G. G.; Omer M. M., and Hindy A. M., (2006), “Metal Complexes of Schiff Base: Preparation, Characterization, and Biological Activity”, Turk J. Chem., 30 :361-382. 19. Satyanayane D. N., (2001), “Electronic Absorption Spectroscopy and Related Techniques”, Universities Press, Hyderabad. 20. Mahmoud, N. Al-Jiboun and Omar H. Al-Obaidi, (2013), “Preparation, Characterization, and Theoretical Study of Metal Complexes Derived from N5 Acyclic Ligand”, American Journal of Applied Chemistry, 1(3) :37-42. 21. Cotton, F. A., and Wilkison G., (1988), "Advanced Inorganic Chemistry", 3 rd Ed., 725, Wiley Interscience. 22. Ajaykumar, K.; Sangamesh P., and Prema B., (2009), "Electrochemical Properties of Some Transition Metal Complex: Synthesis, Characterization of In-Vitro Antimicrobial Studies of Co(II), Ni(II), Cu(II), Mn(II), Complexes", Int. J. Electrochem. Sci., 4 :717-729. Chemistry | 109 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Table (1): Ligand (L) and its Metal Complexes Physical Data Compound No. Color M. p. o C M.Wt g/mol M:L in EtOH %Elemental Analysis Found (Calc.) Metal M% Found (Calc.) Suggest Formula C H N S (L) Light Brown 197 264 - 45.15 (45.45) 3.40 (3.03) 21.45 (21.21) 12.38 (12.12) - C10H8N4O3S C1 Green 247d* 458.5 1:1 26.51 (26.17) 2.33 (2.61) 12.00 (12.21) 6.68 (6.98) 11.97 (11.34) [Cr(L)(H2O)2Cl2]C l C2 Pale Brown 280d* 426 1:1 28.62 (28.16) 2.57 (2.81) 13.48 (13.14) 7.59 (7.51) 12.40 (12.91) [Mn(L)(H2O)2Cl2] C3 Dark Green 275d* 430 1:1 27.46 (27.90) 2.35 (2.79) 13.41 (13.02) 7.64 (7.44) 13.23 (13.72) [Co(L)(H2O)2Cl2] C4 Yellow 202d* 411.7 1:1 29.40 (29.14) 2.69 (2.42) 13.28 (13.60) 7.39 (7.77) 14.02 (14.25) [Ni(L)(H2O)Cl]Cl C5 Green 270d* 416.5 1:1 28.53 (28.81) 2.48 (2.40) 13.09 (13.44) 7.46 (7.68) 15.66 (15.24) [Cu(L)(H2O)Cl]Cl d*= decomposition. Chemistry | 110 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Table (2): Ligand (L) and its Metal Complexes Characteristic Stretching Vibration Frequencies (cm -1 ) Located in the FT-IR Compound No. υC=O υC=N υC=S M-O M-N M-Cl (L) 1728 1631 1201 - - - C1 1627 1562 1201 543 470 320 C2 1627 1566 1207 543 474 324 C3 1643 1566 1203 536 462 316 C4 1647 1570 1203 540 455 320 C5 1627 1566 1203 543 455 316 Table (3): Ligand (L) and its Metal Complexes (C1-C3) Electronic Spectra, Conductance in (DMF) and Magnetic Moment (B.M) Compound No. Bands Cm -1 Assignment Molar Cond. ohm -1 .cm 2 .mol -1 eff. B.M Suggested Structure (L) 48543 34482 * * - - - C1 15408 21691 28571 4 A2g → 4 T2g(F) 4 A2g → 4 T1g(F) 4 A2g → 4 T1g(P) 70.62 3.82 Octahedral C2 16891 27173 6 A1g → 4 T1g(G) 6 A1g → 4 T2g(D) 19.35 5.18 Octahedral C3 14858 16528 30303 4 T1g → 4 A2g(F) 4 T1g → 4 T1g(P) C.T 16.48 4.50 Octahedral C4 27397 32786 3 T1 → 1 T2 C.T 87.94 3.21 Tetrahedral C5 12658 32051 2 T → 2 E C.T 76.25 1.87 Tetrahedral Chemistry | 111 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Figure (1): The 1 H-NMR Spectrum of the Ligand (L) Chemistry | 112 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 F ig u r e (2 ): L ig a n d (L ) F T -IR S p e c tr a Chemistry | 113 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 F ig u r e (3 ): C r C o m p le x F T -IR S p e c tr a Chemistry | 114 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 Figure (4): Ligand (L) Electronic Spectrum Figure (5): Co Complex Electronic Spectrum Chemistry | 115 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 N NO2 Cr N N H S O Cl Cl OH2 H2O Cl Figure (6): Octahedral Stereo Chemical Structure Suggested for Cr(III) Complex [Cr(C10H8N4O3S)(H2O)2Cl2]Cl N NO2 M N N H S O Cl Cl OH2 H2O M=Mn(II, or Co(II) Figure (7): Octahedral Stereo Chemical Structure Suggested for M(II) Complex [M(C10H8N4O3S)(H2O)2Cl2] N NO2 M N N H S O Cl OH2 Cl M=Ni(II, or Cu(II) Figure (8): Tetrahedral Stereo Chemical Structure Suggested for M(II) Complex [M(C10H8N4O3S)(H2O) Cl ]Cl Chemistry | 116 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 + O H NO2 NH2 NH CNH2 S EtOH Absolute reflux 4 hrs. CH NH NO2 NH C NH2 S (1) ClCH 2 COOEt reflux 20 hrs. CH 3 COO - Na + CH N NO2 N C NH S O .. (2) (L) .. Scheme (1): General Steps of Preparation of Ligand (L) Chemistry | 117 2016( عاو 3انعذد ) 29يجهت إبن انهٍثى نهعهىو انظزفت و انخطبٍمٍت انًجهذ Ibn Al-Haitham Jour. for Pure & Appl. Sci. Vol. 29 (3) 2016 يوَات انعُاصر أالَحقانيه نهيكُذ جحضير وجشخيص يعقذات بعض انًعقذات أل أوٌ كقواعذ شف-4-ثايوأوكسوإيادازونذيٍ-2 سُاٌ يذحث انبياجي أَعاو يجيذ رشيذ إيُاس زهير يحًذ زيُة خضير حسٍ غانيأيجاد أيم يحًذ حسيٍ لسى انكًٍٍاء/ كهٍت انعهىو/ انجايعت انًسخنظزٌت 3122/ارار/41,قبم في:3122/كاَوٌ األول/32اسحهى في: انخالصــة حضز وشخض انهٍكانذ [3-(2-nitrobenzylidene)amino-2-thioxoimidazolidin-4-one] ( II( واننحاس )IIاننٍكم ),( IIنج )اانكىب,( IIانًنغنٍز ),( IIIويعمذاحه يع بعض أٌىناث عناطز انكزوو ) ( C.H.N.S)انذري انههبً وانخحهٍم انذلٍك نهعناطز االيخظاصانطزائك انفٍزٌائٍت انًناسبت يثم حمنٍت باسخعًال اسٍتانحسو لٍاساث انخىطٍهٍت انكهزبائٍتإضافتً إنى انًزئٍت -فىق انبنفسجٍتاألشعت األشعت ححج انحًزاء و طٍفو ووجذ أنها يسخمزة عنذ اننسب وعٍنج اننسبت انًىنٍت بٍن انهٍكانذ وانفهز باسخعًال طزٌمت اننسب انًىنٍت .انًغناطٍسٍت نج, أيا يعمذي اانشكم ثًانً انسطىح نًعمذاث انكزوو وانًنغنٍز وانكىب ألخزح. ين انخحانٍم انسابمت [1:1]انًىنٍت ً انسطىح.لخزح انشكم رباعااننٍكم واننحاس فمذ حخهٍك حشخٍض لىاعذ شف ثنائٍت أنسن يعمذاث انعناطز االنخمانٍت. انكهًات انًفحاحية: