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The Synthesis of Four New Bis(Amino-p-Chlorophenylglyoximes) and their Polymeric Complexes
Transcript of The Synthesis of Four New Bis(Amino-p-Chlorophenylglyoximes) and their Polymeric Complexes
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The Synthesis of FourNew Bis(Amino-p-Chlorophenylglyoximes) andtheir Polymeric ComplexesAli Ihsan Pekacar a , Bedrettin Mercimek b & EmineÖzcan ca Niğde University, Faculty of Arts and Sciences,Chemistry Department, 51200, Niğde, Turkeyb Selçuk University, Faculty of Arts and Sciences,Chemistry Department, 42079, Konya, Turkeyc Pamukkale University, Faculty of Arts and Sciences,Chemistry Department, Denizli, TurkeyVersion of record first published: 18 Aug 2006.
To cite this article: Ali Ihsan Pekacar , Bedrettin Mercimek & Emine Özcan (1997):The Synthesis of Four New Bis(Amino-p-Chlorophenylglyoximes) and their PolymericComplexes, Synthesis and Reactivity in Inorganic and Metal-Organic Chemistry, 27:3,455-463
To link to this article: http://dx.doi.org/10.1080/00945719708000201
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SYNTH. REACT. INORG. MET.-ORG. CHEM., 27(3), 455-463 (1997)
THE SYNTHESIS OF FOUR NEW
AND 1HEIR POLYMERIC COMPLEXES BIS(AMIN0-p-CHL OROPHENYL GL YOXMES)
Ali hsan Pekacar* Nigde TJniversity, Faculty of A r t s and Sciences,
Chemisty Department, 51200 Nigde, Turkey
Bedrettin Mercimek Selguk University, Faculty of A r t s and Sciences, Chemistly Department, 42079 Konya, Turkey
Pamukkale Univergity, Faculty of Arts and Sciences, Chemistry Department, Denizli, Turkey
Emine Ozcan
ABSTRACT
In thiv study, four new bis(amino-p-chlorophenylglyoximes),
1,2-phenylenebis(aminomino-pchlorophenylglyoxime) L1€i2, 1,5-naphthylenebis(amino-p
chlorophenylglyoxime) L2H2, 3,4-tolylenebi~(amino-p-chlorophenylglyoxime) L3H7,
and 2,6-pyridylbis(amino-pchlorophlenylglyoxime) L4H2, have been synthesized from
&-p-chlorophenylchloroglyoxime and the corresponding aromatic diamines. Their
polymeric complexes with Ni(lI), Co(n) and Cu(II) have been prepercd. The Ni(I1) and
Cu(II) complexes of these ligands have been found to be square-planar, while the Co(i1)
complexes are octahedral with water molecules as axial ligands. 111 NMR, AAS, IR,
magnetic susceptibility and elemental analytical data of the complexes and ligands are
discussed.
455
Copyright 0 1997 by Marcel Dekker, Inc
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456 PEKACAR, MERCIMEK, AND OZCAN
INTRODUCTION
Since the increasing we of coordination compounds in analytical, pigment,
medicinal and biochemistry, many investigators have studied these topics, especially the
important role of the complexes of 1,Zdioximes in coordination chemistry. The
transition metal complexes of v*dioximes have been of particular interest as far as
biological model compounds1-3 are concerned. Thus, the synthesis of substituted
aminoglyoximes from a&-chloroglyoxime or a&-chlorophenylchloroglyoxime and the
corresponding amines has been reported*-’. It has been found that in these compounds
the two oxime groups are not equivalent. Additional substituents on the aromatic group,
bound to the N-atom of aminoglyoxime, are expected to enhance the difference between
the two oxime groups. In this paper we report the synthesis of polymeric complexes of
four new bis(amino-pchlorophenylglyoximes) as examples of unsymmetrically
substituted 1,3-dioximes.
RESUL TS AND DISCCTSSION
In this study, four new bis(amino-gchloroglyoximes) were synthesized from the
reaction of a&-pchlorophenylchloroglyoxime and the corresponding aromatic diamines
in ethanol at -10oC. The general structures of these compounds are given in Fig. 1. The
structures of the new ligands were confirmed by elemental analyses, lH NMR and IK
spectral data shown in Tables I, I1 and 111, respectively.
~ H N M R Svec:ra ofLipMdF and Comvkes
In the 1H NMR spectra of the ligands, two peaks are present for the OH protons of
the oxime groups. When the chemical shifi values of the two OH protons are compared
in the four different ligmds, the ones at lower field resemble each other quite closely
(12.07-11.61 ppm), however,for those at the higher field (11.17-10.30 ppm) a
considerable difference is observed (Table 11). The chemical shift for OH protons
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bis(AM1NO-p-CHLOROPHENYLGLYOXIME) COMPLEXES 457
Fig. 1. General Formulae of Ligands
TabkI. The Colors, Yields, Melting Points and Elemental Analytical Regultg of the Ligands.
aDisappears on D,O exchange 6: singlet m: mukiplet
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458 PEKACAR, MERCIMEK, AND OZCAN
Tabklll. Characteristic JR Bands of the Ligands as KRr Pellets (cm-I)
have characteristic value for these types of oximes8-10. The two deuterium
exchangeable singlets correspond to two non-equivalent OH protons which also indicate
the a-configuration of the OH group relative to each other1>5p8-12. The deuterium
exchangeable NH protons, neighboring the oxime groups, and the aromatic C-H protons
were observed at 8.63-8.52 ppm and 8.15-6.76 ppm, r e ~ p e c t i v e l y ~ ~ ~ ~ ~ ~ ~ ~ - ~ ~ . The
chemical shift values of the methylene protons appeared at 2.39 ppm as singlets.
a
Due to the low solubilities of the complexes in organic solvents, 113 NMR spectra
could not be obtained. The metal-ligand ratios in all these polymeric complexes were
1:1, but the Co(II) complexes had two coordinated water molecules for each complex.
Consequently, an octahedral structure for the Co(1I) and a square-planar structure for the
Ni(1I) and Cu(I1) compounds are proposed4 , Fig. 2.
IR Spectra ofLipandS and Comvlolc
In the IR spectra of the ligands (Table 110, NH (3460-3420 an-'), OH (3320-
3280 cm-'), C=N (1640-1620 cm-l), C-C1 (700-690 cm-l) and NO (1010-940 cm-1)
&etches appear at frequencies expected for substituted bis(amino-pchlorophenyl-
glyoximes)8-11,14,15.
In the JR spectra in Table I1 and lV of the complexes, the shifts of the C-N
stretching frequency to a lower frequency and the vibration of the N-0 band to a higher
frequency indicated the formation of coordination bonds between metal and the nitrogen
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bis(AMIN0-p-CHLOROPHENYLGLYOXIME) COMPLEXES 459
n MCI2
n Q C-C /iv"" H
// \ I N-R-N
I \ /;"""-a HON
H C-C
H*/ Q CI
- n
M = Ni(II), Cu(II), Co(II).ZHfl
Fig. 2. Octahedral andsquare-planar Pobmeric Metal ComprpXes
of B i s ( M c i n o - p c h l o r o p h e ~ ~ ~ ~ ~ ) .
I*&& f K Tht Colors, Mclting Pointsa, Yicfck and Elemental Analytical Results of the Complexes.
Cotnpounb --__
f=u
558.00
562.86
594.28
608 06
612.92
644.34
__
____ 512.03
576.89
608.30
___
-~
558.99
563.85
595 26
.-
~ ..~
Brown
Red
47.88
Bmm
und)% ___ - N M
15.06 10.52 (15.W) i10.67) 14.93 11 29
14.14 9.91 (14.17) (9.71)
13.82 965 j 1 3 . 7 4 (963)
13.71 10.36 (13.52) (10.30) 13.04 9.14
(13.34) (9.21)
14.69 10.26 (1457) (10.37)
14.56 11 01 (1437)- (10.87)
13.81 969 (13.61) (9.55)
17.54 10.50 117.35) (10.61)
17.39 11.27 (17.01) (11.?8) 16.41 9.90
(16.32) (9.98)
(11.4cj
_-
____
~
a Melting points of dl compounds are above 360 OC.
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460 PEKACAR, MERCIMEK, AND OZCAN
atoms of the liganh. In the case of the Co(II) complexes, the coordinated H2O groups
are identified by a broad OH absorption at around 3540-3300 cm-l which keeps its
intensity even after heating at 1 10°C for 24 h.
Magnetic Susceptility ofNit1I). CutII) and Co{II) Coinvhes
The magnetic susceptibility values of the complexes (Table V) show that the ds
configuration of the Ni(II) complexec ic diamagnetic, while the d9 Cu(I1) complexen and
d7 Co(I1) complexes are paramagnetic. The measured values for the Cu(I1) and Co(I1)
complexes are 1.75 B.M. and 2.40 B.M., respectively, which corresponds to a single
electron. These values also show that the Ni(II) and Cu(I1) complexes are of' square-
planar structure and that the Co(II) complexes are of octahedral structure6,16-22 (Fig.2).
EXPEIUMENTAL
All reagents were purchased from Merck (Germany) or Fluka (Switzerland), and
used without further purification. ?'he elemental analyses (C, H, and N) have been
determined by using a Carlo-Ebra 1106 model analyser. The magnetic moments of the
complexes were measured according to the Gouy method on a Newport Instrument type
D-104 magnet power supply. *H NMR spectra were recorded on a Varian T 100-A
model spectrophotometer, IR spectra on a Pye-TJnicam SP 1025 model instrument using
KBr pellets, and the atomic absorption spectra (AAS) on a Varian AA-175 iustrument
and pH on an Orion model 420A p€I meter.
Svnthesk of Substbred P h e n v C ~ r o u h ~ ~ ~ OXit?WSl
In this study, l,2-phenylenebir(amino-pchiorophenylglyoxime) L*Hz, 13-
naphthylenebis(amin0-pchlorophenylglyoxime) L2H2, 3,4-tolylenebis(amino-pchloro-
phenylglyoxime) L3H2 and 2,6-pyridylbir(amino-pchlorophlenylglyoxime) L4H2 have
been synthesized from a&-pchlorophenylchloroglyoxime and the corresponding
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bis(AMIN0-p-CHLOROPHENYLGLYOXIME) COMPLEXES 46 1
C-N v v
1650
1650
1650
1650
1640
1650
1620
1640
1630
______ 1640
1630
1630
Table V: Magnetic Moments and Characteristic IR Bands of the Complexes as KBr Pellets (cm-1).
N O
980
950
980
980
950
940 ~-
980
960
950 .-
loo0
980
9R0
-
0 - P O V
1720
1130
1700
.~ 1730
1715
1130
1740
1710
1710
___
1740
1150
11 10
--
aromatic diamhes. &ti-pchlorophenylglyoxime was prepared according to the
literatmes-'2,'4.'5.
A solution of 0.01 mol of the appropriate aromatic diamine compound [1,2-
phenylenediamine (1.08 g), or 1,5-naphthyldiamine (1.58 g), or 3,4-diaminotoluene
(1.22 g), or 2,6-diaminopyridine (1.09 g)] in 40 mL absolute ethanol was added
dropwise over 30 minutes to a stirred solution of 4.66 g (0.02 mol) of m-p- chlorophenylchloroglyoxime in 60 mL absolute ethanol at -1OoC. The reaction mixture
was stirred for further 2-3 h, left overnight at OOC, and then diluted with 100-120 ml.
water. The precipitate obtained was filtered and then recrystallized from ethanol-water
(1 : 1). The crystalline product was filtered, washed with water, and dried in a vacuum
oven.
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462 PEKACAR, MERCIMEK, AND OZCAN
The ligands were found to be soluble in ethanol, DMF, DMSO and slightly soluble
in acetone and insoluble in water. The colors, yields, melting points, elemental analyses,
1H NMR and IR data of these ligands are given in Tables I, II and I", respectively.
Svnthesis ofthe C d l l ) . Ni(IIj and Co(IIj C o m l a e s
A solution of 1 mmol metal salt (NiC12. 6H2O ( 0.238 g 1; or CuCI2. 2H20
(0.172 g); or CoC12. 6H2O (0.238 g) ] in 20 mL of water-ethanol (2:l) was added to a
solution of 1 mmol of the ligand [ L1H2 ( 0.501 g ); or L2H2 ( 0.551 g ); or L3H2
( 0.515 g ); or L4H2 ( 0.502 g) 1, dissolved in 40 mL of ethanol. The pH of the mixture
was 3.0-3.5 and its color turned to red-brown or dark-brown. After addition of 1%
NaOH solution in ethanol-water fl:1) to increase the pH to 4.5-5.0, the mixture was
stirred on a water-bath at SO-6O0C for 20 minutes. The precipitated complexes were
filtered while hot, washed with water, ethanol and diethyl ether, and then dried in a
vacuum oven. The colors, yields, melting points, elemental analytical results, magnetic
moments of the complexes and JR data of the compounds are given in Tables IV and V,
respectively.
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