# Synthesis, Optical Characterization, and Thermal Decomposition of Complexes Based on Biuret Ligand

Authors: Mei-Ling Wang; Guo-Qing Zhong; Ling Chen
Journal: International Journal of Optics
 (2016)

---

## Abstract

Four complexes were synthesized in methanol solution using nickel acetate or nickel chloride, manganese acetate, manganese chloride, and biuret as raw materials. The complexes were characterized by elemental analyses, UV, FTIR, Raman spectra, X-ray powder diffraction, and thermogravimetric analysis. The compositions of the complexes were [Ni(bi)2(H2O)2](Ac)2·H2O (1), [Ni(bi)2Cl2] (2), [Mn(bi)2(Ac)2]·1.5H2O (3), and [Mn(bi)2Cl2] (4) (bi = NH2CONHCONH2), respectively. In the complexes, every metal ion was coordinated by oxygen atoms or chlorine ions and even both. The nickel and manganese ions were all hexacoordinated. The thermal decomposition processes of the complexes under air included the loss of water molecule, the pyrolysis of ligands, and the decomposition of inorganic salts, and the final residues were nickel oxide and manganese oxide, respectively.


---

## Body

## 1. Introduction

Biuret contains two acylamino groups and one imino group, the structure of which determines its value on the synthesis of some complexes as a neutral ligand. In medicine, biuret can be used as pharmaceutical intermediates to preparation hypnotics, sedatives, and some special drugs which have the functions of diuresis and lowering the blood pressure. In chemical industry, biuret plays an important role in the produce of the flame retardants of papers, the fiber bleaching agent, the paint of textiles, the foaming agent of foamed plastics, and the additive agent of the paint, adhesives, resins, plastics, dyes, and lubricating oils, and so on. In agriculture, biuret can be utilized as long-effective fertilizers rich in nitrogen. In animal husbandry, biuret is an excellent nonprotein nitrogen feed additive, and it has a better palatability and higher-usage comparing with urea which is usually used as feed additive. Several teams had synthesized and characterized the complexes of rare earth metals [1], actinide metals [2, 3], and alkaline earth metals [4] based on biuret ligand. However, the complexes of transition metals with biuret ligand have been rarely reported [5, 6], particularly in the comparison between different metal ions on the synthesis of the biuret complexes. With the rapid development of animal industry in China, the prospects of biuret complexes which are used as feed additives for ruminants are considerable. The complexes of trace elements with biuret which are added in the feed of ruminants can play a dual role in supplementing both trace elements and nonprotein nitrogen, which can promote the growth of animals and improve the economic efficiency. Here we report the synthesis of four biuret complexes, study their optical properties, and characterize them by elemental analyses, UV, FTIR, Raman spectra, X-ray powder diffraction, and thermogravimetric analysis.


## 2. Experimental

### 2.1. Materials and Physical Measurements

All chemicals purchased were of analytical reagent grade and used without further purification. Nickel acetate, nickel chloride, manganese acetate, manganese chloride, and biuret were purchased from Sinopharm Chemical Reagent Co. Ltd. of Shanghai.Elemental analyses for C, H, N, and O in the complexes were measured on a Vario EL CUBE elemental analyzer, and the content of nickel and manganese was determined by EDTA complexometric titration with murexide and chrome black T as indicators, respectively. UV spectra were performed on a UV-3150 spectrophotometer. IR spectra were obtained with KBr pellets on a Nicolet 5700 FT-IR spectrophotometer in the range of 4000−400 cm−1. Raman spectra were recorded on an InVia Laser Raman spectrometer. The powder X-ray diffraction data were collected on a D/max-II X-ray diffractometer with Cu K
α
1 radiation, the voltage of 35 kV, the current of 60 mA, and the scanning speed of 8° min−1, in the diffraction angle range of 10−80°. The thermogravimetric analysis data were obtained using a SDT Q600 thermogravimetry analyzer in the air atmosphere in the temperature range of 25−800°C with a heating rate of 10°C min−1.


### 2.2. Synthesis of [Ni(bi)2(H2O)2](Ac)2·H2O (1)

Ni(Ac)2·4H2O (2.49 g, 10 mmol) and biuret (2.06 g, 20 mmol) were weighed and dissolved in 80 mL methanol, and the solution was green. The mixed solution was stirred on a magnetic stirrer for about 6 h under reflux reaction. After the solution cooling, the resultant was separated from the reaction mixture by filtration and washed by some methanol and dried in the phosphorus pentoxide desiccator for 1 week. The product was green powder (3.59 g) and the yield was about 82.2%.


### 2.3. Synthesis of [Ni(bi)2Cl2] (2)

Complex2 was synthesized by the same procedure as that for the synthesis of complex1 except for using NiCl2·6H2O (2.38 g, 10 mmol) instead of Ni(Ac)2·4H2O as the start reactant. The product was green powder (2.18 g) and the yield was about 64.9%.


### 2.4. Synthesis of [Mn(bi)2(Ac)2]·1.5H2O (3)

The synthesis of complex3 was similar to that of1 except that Mn(Ac)2·4H2O (2.45 g, 10 mmol) was used to replace Ni(Ac)2·4H2O. There was a difference that the reaction mixture was cooling in the refrigerator. The solubility of complex3 at room temperature was larger than that of complexes1 and2, and the yield was higher at low temperature. The product was pale pink powder (2.37 g) and the yield was about 58.3%.


### 2.5. Synthesis of [Mn(bi)2Cl2] (4)

The synthetic method of4 was the same as3 other than that Mn(Ac)2·4H2O was replaced by MnCl2·4H2O (1.98 g, 10 mmol). The product was pale pink powder (2.00 g) and the yield was about 60.2%.


## 2.1. Materials and Physical Measurements

All chemicals purchased were of analytical reagent grade and used without further purification. Nickel acetate, nickel chloride, manganese acetate, manganese chloride, and biuret were purchased from Sinopharm Chemical Reagent Co. Ltd. of Shanghai.Elemental analyses for C, H, N, and O in the complexes were measured on a Vario EL CUBE elemental analyzer, and the content of nickel and manganese was determined by EDTA complexometric titration with murexide and chrome black T as indicators, respectively. UV spectra were performed on a UV-3150 spectrophotometer. IR spectra were obtained with KBr pellets on a Nicolet 5700 FT-IR spectrophotometer in the range of 4000−400 cm−1. Raman spectra were recorded on an InVia Laser Raman spectrometer. The powder X-ray diffraction data were collected on a D/max-II X-ray diffractometer with Cu K
α
1 radiation, the voltage of 35 kV, the current of 60 mA, and the scanning speed of 8° min−1, in the diffraction angle range of 10−80°. The thermogravimetric analysis data were obtained using a SDT Q600 thermogravimetry analyzer in the air atmosphere in the temperature range of 25−800°C with a heating rate of 10°C min−1.


## 2.2. Synthesis of [Ni(bi)2(H2O)2](Ac)2·H2O (1)

Ni(Ac)2·4H2O (2.49 g, 10 mmol) and biuret (2.06 g, 20 mmol) were weighed and dissolved in 80 mL methanol, and the solution was green. The mixed solution was stirred on a magnetic stirrer for about 6 h under reflux reaction. After the solution cooling, the resultant was separated from the reaction mixture by filtration and washed by some methanol and dried in the phosphorus pentoxide desiccator for 1 week. The product was green powder (3.59 g) and the yield was about 82.2%.


## 2.3. Synthesis of [Ni(bi)2Cl2] (2)

Complex2 was synthesized by the same procedure as that for the synthesis of complex1 except for using NiCl2·6H2O (2.38 g, 10 mmol) instead of Ni(Ac)2·4H2O as the start reactant. The product was green powder (2.18 g) and the yield was about 64.9%.


## 2.4. Synthesis of [Mn(bi)2(Ac)2]·1.5H2O (3)

The synthesis of complex3 was similar to that of1 except that Mn(Ac)2·4H2O (2.45 g, 10 mmol) was used to replace Ni(Ac)2·4H2O. There was a difference that the reaction mixture was cooling in the refrigerator. The solubility of complex3 at room temperature was larger than that of complexes1 and2, and the yield was higher at low temperature. The product was pale pink powder (2.37 g) and the yield was about 58.3%.


## 2.5. Synthesis of [Mn(bi)2Cl2] (4)

The synthetic method of4 was the same as3 other than that Mn(Ac)2·4H2O was replaced by MnCl2·4H2O (1.98 g, 10 mmol). The product was pale pink powder (2.00 g) and the yield was about 60.2%.


## 3. Result and Discussion

### 3.1. Composition and Property

The results of elemental analyses for the complexes are shown in Table1. The experimental results coincide with the theoretical calculation, and the composition of the complexes is [Ni(bi)2(H2O)2](Ac)2·H2O, [Ni(bi)2Cl2], [Mn(bi)2(Ac)2]·1.5H2O, and [Mn(bi)2Cl2] (bi = NH2CONHCONH2), respectively. In order to make sure whether chlorine atoms were coordinated or ionic, a qualitative test was conducted; namely, a few drops of AgNO3 solution were added into the aqueous solution containing complexes2 and4; there was no precipitation formation. This indicates that the chlorine atoms are coordinated to the metal ions rather than ionic. The solid complexes are stable in the air, easily dissolved in water, and not easy to absorb moisture. Every Ni(II) ion in complex1 is coordinated by six oxygen atoms from two biuret molecules and two coordinated water molecules, while Ni(II) and Mn(II) ions in complexes2 and4 are coordinated with two chloride ions and four oxygen atoms from two biuret molecules. In contrast, the Mn(II) ion in complex3 is coordinated by six oxygen atoms from two biuret molecules and two acetate anions. Several complexes in which the acetate anions are coordinated had been reported [7–9]. In the four complexes, six coordinated atoms form an octahedral geometry, and four oxygen atoms presenting quadrilateral from two biuret are in the same plane with the metal ions. The other two coordinated atoms are on both sides of the plane. The metal ions are in the centre of the octahedron. And the octahedron is symmetric; thus, the structures of the complexes are stable.Table 1
Elemental analysis results of the complexes (calculated values are in brackets).
Complex
Formula
M
r
w
(M)/%
w
(C)/%
w
(H)/%
w
(O)/%
w
(N)/%
1
NiC8H22O11N6
436.97
13.29 (13.43)
22.03 (21.97)
5.17 (5.09)
40.36 (40.28)
19.15 (19.23)
2
NiC4H10O4N6Cl2
335.75
17.62 (17.48)
14.48 (14.30)
2.96 (3.01)
18.99 (19.06)
24.92 (25.04)
3
MnC8H19O9
.
5N6
406.19
10.79 (13.53)
23.19 (23.63)
3.69 (4.72)
43.34 (37.42)
28.79 (20.70)
4
MnC4H10O4N6Cl2
332.00
16.42 (16.55)
14.39 (14.46)
2.98 (3.04)
19.35 (19.28)
24.41 (25.32)


### 3.2. UV Spectroscopy Analysis

The UV spectra of the complexes and biuret are shown in Figure1. It is not difficult to find that there is an absorption peak around 200 nm for biuret as well as the four complexes we have synthesized, which shows a close spectral similarity between the four complexes and biuret. In other words, the UV absorption of the complexes derived from biuret. The very strong absorption at short wavelengths is attributed to π-π
∗ transitions, originating from the carbonyl groups of biuret ligand. The locations of the UV absorption peaks for these complexes are found to be a bit different, indicating that some changes in the π-electron system of biuret have taken place. The outer electronic structure of Ni2+ is 3d8, and there is no empty 3d orbit. Compared with Ni2+, the outer electronic structure of Mn2+ is 3d5, and there are two empty 3d orbits. As a result, the electrons of Cl− in 3p orbits can be filled into the empty 3d orbits of Mn2+. Therefore, the UV spectrum of complex4 differs from those of other studied complexes and the free biuret ligand. In conclusion, the oxygen atoms of the carbonyl groups in biuret molecules are coordinated to the metal ions.Figure 1
UV spectra of the complexes and biuret.


### 3.3. IR Spectroscopy Analysis

The IR spectra of the four complexes and biuret are shown in Figures2–4, and the main infrared spectral data of biuret and its complexes are listed in Table 2. In the spectra of the four complexes, two bands (3115−3430 cm−1) are observed in the N−H stretching region. The former one is alternatively assigned to bridging hydroxide whereas the water of hydration band appears near 3400 cm−1 in complexes1 and3. The N−H deformation vibrations are observed at 1530 cm−1 with significant intensities. The carbonyl stretching frequencies in compounds containing the CO−NH−CO group are reported to give rise to two bands [10, 11], the asymmetric stretching vibration peak appears above 1700 cm−1, and the symmetric vibration peak appears near 1700 cm−1. When coordination occurs it determines the amount of electron delocalization in the N−CO−N system; thus, coordination through the oxygen atom will produce a decrease in the double bond character of the C=O bonds and conduct a shift of the carbonyl stretching mode to lower frequencies [12]. The stretching vibration peaks of the C=O bonds in the complexes are detected at 1686, 1693, 1693, and 1685 cm−1, respectively, which are a little lower than the frequency of biuret (1719 cm−1). It is believed that the unprotonated biuret M(II) (M = Ni, Mn) complexes should have the M−O coordinated bonds. On the other hand, the bending vibration peaks of the C=O bonds found in the region of 621−664 cm−1 are the evidence of the coordination between metal ions and oxygen atoms in the ligand as well. In the nickel complexes, the frequency of the stretching vibration peak of the C=O bonds in complex1 containing acetate anions is a little lower than that of complex2 containing chloride anions. However, in the manganese complexes, it is higher in complex3 containing acetate anions than that of complex4 containing chloride anions. Compared with complex1, the stretching vibration peak of the C=O bonds in complex3 moves to high wavenumber, which can illustrate that both the oxygen atoms in biuret molecules and acetate anions are coordinated to the manganese ions in complex3. The absorption peaks at 476 cm−1 in complexes1 and2 are originated to the stretching vibrations of the Ni−O bonds, and the absorption peaks at 459 cm−1 in complexes3 and4 are the characteristic peaks of the Mn−O bonds [13–17].Table 2
Infrared spectra of the ligand and the complexes (cm−1).
bi
[Ni(bi)2(H2O)2](Ac)2·H2O
[Ni(bi)2Cl2]
[Mn(bi)2(Ac)2]·1.5H2O
[Mn(bi)2Cl2]
Vibration type
3415
3433, 3379
3383
3406
3406
ν
a
s(NH2) + ν(H2O)/ν
a
s(NH2)
3254
3196, 3115
3268, 3198
3216
3264, 3196
ν
s(NH2)
1719
1686
1693
1693
1685
ν(C=O)
1585
1530
1582
1551
1571
δ(NH2)
1499, 1423
1445, 1411
1490
1512
1485
ν(C−N) +ν(C−NH2)
1323
1343
1336
1336
1329
δ(N−H)
1130
1126
1127
1140
1120
ν(C−N) + δ(N−H)
1081
1054
1100
1099
1092
ν(C−N)
946
923
943
925
939
ν(C−N) +ν(C−NH2)
770
781
760
780
757
δ(C−NH2)
710
646
646
634
621
δ(C=O)Figure 2
IR spectra of complexes1 and2.Figure 3
IR spectra of complexes3 and4.Figure 4
IR spectrum of biuret.


### 3.4. Raman Spectroscopy Analysis

Figures5 and 6 show the Raman spectra of the complexes obtained in the 400−4000 cm−1 range, and the frequencies data of the biuret and its complexes are listed in Table 3. Obviously, there are many correlations among peaks when comparing the Raman spectra with the IR spectra. For example, the wide absorption peaks in the four complexes from the stretching vibrations of the O−H and N−H bonds appear in the region of 3430−3200 cm−1 in the IR spectra as well as in the Raman spectra. But some differences can be discovered that the bending vibration peaks of the N−H bond near 1320 cm−1 in the Raman spectra are found to be quite weak and even cannot be found comparing with those in the IR spectra. The result may be explained that the N−H bond in biuret is a polar bond, and it is Raman negative. It is well known that when the interaction between the metal cations (M2+) and the coordinated water molecules is strong enough, a Raman band due to the symmetric stretching vibration of M−OH2 is observed in the low-frequency region from 300 to 550 cm−1 [18–22]. The absorption peak at 467 cm−1 for complex1 is assigned to the symmetric M−OH2 stretching vibration.Table 3
Raman spectra of the complexes (cm−1).
bi
[Ni(bi)2(H2O)2](Ac)2·H2O
[Ni(bi)2Cl2]
[Mn(bi)2(Ac)2]·1.5H2O
[Mn(bi)2Cl2]
Vibration type
3370
3433
3382
3398
3398
ν
a
s(NH2) + ν(H2O)/ν
a
s(NH2)
3230
3203
3276
3210
3282
ν
s(NH2)
1690
1691
1685
1698
1685
ν(C=O)
1440
1439
1467
1441
1460
ν(C−N) +ν(C−NH2)
1150
1134
1123
1129
1129
ν(C−N) + δ(N−H)
965
955
938
956
936
ν(C−N) +ν(C−NH2)
775
750
750
709
748
δ(C−NH2)
647
638
627
618
619
δ(C=O)
—
467
473
456
463
ν(M−O)Figure 5
Raman spectra of complexes1 and2.Figure 6
Raman spectra of complexes3 and4.


### 3.5. X-Ray Powder Diffraction Analysis

X-ray powder diffraction (XRD) is measured to confirm the phase purity of the samples. The XRD patterns of the complexes and the ligand are shown in Figures7–9. The background of the XRD patterns is small and the diffractive intensity is strong, indicating that the complex has a fine crystalline state. The strong peak locations of the complexes are shown in Table 4, which are obviously changed comparing with biuret and nickel acetate (JCPDS 26-1282) or nickel chloride (JCPDS 22-0765), manganese acetate (JCPDS 29-0879), and manganese chloride (JCPDS 22-0721). All these strong peaks of the reactants are disappeared in the X-ray powder diffraction patterns of the complexes. The diffraction angle (2
θ), diffractive intensity, and spacing (d) of the products are completely different from the reactive materials, which may illuminate that the resultants are new compounds instead of the reactant mixture [23].Table 4
The data for X-ray powder diffraction patterns of the complexes and biuret.
Compound
The 2θ(°) locations of the main strong peaks (relative intensities are in brackets)
bi
23.51 (100)
28.71 (94)
11.30 (86)
18.88 (69)
21.83 (65)
[Ni(bi)2(H2O)2
](Ac)2·H2O
31.50 (100)
15.45 (60)
45.18 (56)
12.06 (24)
19.51 (22)
[Ni(bi)2Cl2
]
28.68 (100)
13.18 (90)
28.23 (75)
15.19 (74)
24.27 (61)
[Mn(bi)2(Ac)2
]·1.5H2O
23.78 (100)
13.52 (35)
13.13 (32)
29.92 (30)
16.86 (20)
[Mn(bi)2Cl2
]
28.45 (100)
13.13 (60)
27.58 (49)
14.99 (39)
24.12 (36)
Ni(Ac)2·4H2O
12.93 (100)
18.62 (30)
28.34 (20)
22.13 (19)
21.09 (13)
NiCl2·6H2O
15.26 (100)
36.24 (79)
30.08 (30)
51.78 (18)
52.58 (17)
Mn(Ac)2·4H2O
9.068 (100)
11.59 (32)
12.18 (25)
26.20 (8)
27.55 (8)
MnCl2·4H2O
17.93 (100)
20.03 (75)
30.67 (75)
34.54 (45)
16.04 (40)Figure 7
X-ray powder diffraction patterns of complexes1 and2.Figure 8
X-ray powder diffraction patterns of complexes3 and4.Figure 9
X-ray powder diffraction pattern of biuret.


### 3.6. Thermogravimetric Analysis

The thermal behavior of the four complexes is studied from 25°C to 800°C under air. The TG-DTG curves are shown in Figures10–13. The TG analysis (Figure 10) reveals that complex1 is decomposed through four major processes, namely, the loss of lattice water molecules, the coordinated water molecules, and the combustion of biuret ligand and nickel acetate. The first weight loss is approximately 4.27% (calcd. 4.12%) in the range of 64−105°C, corresponding to the weight of one lattice water molecule. There is a weight loss of 8.03% near 137°C for complex1, which is ascribed to the loss of two coordinated water molecules, and the measured value is in agreement with the calculated one (8.25%). The third weight loss occurs between 153°C and 514°C and is characteristic of the combustion of biuret ligand (found 47.58%, calcd. 47.17%). The last weight loss is considered to be the decomposition of nickel acetate (found 23.25%, calcd. 23.36%). As a result, the final residue is nickel oxide. As shown in Figure 11, there are two large weight losses of 60.67% (calcd. 61.40%, loss of two biuret molecules) and 16.73% (calcd. 16.35%, decomposition of nickel chloride) for complex2, and the residual weight in the TG curve is 22.60%, which agrees with the theoretical value (22.25%), and the final residue is determined as nickel oxide. Complex4 is similar to complex2. There are two stages weight losses with the increasing of the temperature, namely, the combustion of biuret ligand (found 61.88%, calcd. 62.10%) and the oxidation of manganese chloride (found 16.24%, calcd. 16.53%), and the final residue is MnO (found 21.88%, calcd. 21.37%). Compared with three other complexes, complex3 undergoes three weight losses of 6.85%, 49.65%, and 25.5% near 104°C, 215°C, and 485°C, respectively, and the first two weight losses agree with the loss of 1.5H2O (calcd. 6.65%) and two biuret molecules (calcd. 49.65%). The last weight losses are considered to be the decomposition of manganese acetate (found 25.40%, calcd. 25.14%) and the final residue is MnO (found 18.10%, calcd. 17.46%). All in all, the thermal behavior of the complexes corresponds to their composition.Figure 10
TG-DTG curves of complex1.Figure 11
TG-DTG curves of complex2.Figure 12
TG-DTG curves of complex3.Figure 13
TG-DTG curves of complex4.


## 3.1. Composition and Property

The results of elemental analyses for the complexes are shown in Table1. The experimental results coincide with the theoretical calculation, and the composition of the complexes is [Ni(bi)2(H2O)2](Ac)2·H2O, [Ni(bi)2Cl2], [Mn(bi)2(Ac)2]·1.5H2O, and [Mn(bi)2Cl2] (bi = NH2CONHCONH2), respectively. In order to make sure whether chlorine atoms were coordinated or ionic, a qualitative test was conducted; namely, a few drops of AgNO3 solution were added into the aqueous solution containing complexes2 and4; there was no precipitation formation. This indicates that the chlorine atoms are coordinated to the metal ions rather than ionic. The solid complexes are stable in the air, easily dissolved in water, and not easy to absorb moisture. Every Ni(II) ion in complex1 is coordinated by six oxygen atoms from two biuret molecules and two coordinated water molecules, while Ni(II) and Mn(II) ions in complexes2 and4 are coordinated with two chloride ions and four oxygen atoms from two biuret molecules. In contrast, the Mn(II) ion in complex3 is coordinated by six oxygen atoms from two biuret molecules and two acetate anions. Several complexes in which the acetate anions are coordinated had been reported [7–9]. In the four complexes, six coordinated atoms form an octahedral geometry, and four oxygen atoms presenting quadrilateral from two biuret are in the same plane with the metal ions. The other two coordinated atoms are on both sides of the plane. The metal ions are in the centre of the octahedron. And the octahedron is symmetric; thus, the structures of the complexes are stable.Table 1
Elemental analysis results of the complexes (calculated values are in brackets).
Complex
Formula
M
r
w
(M)/%
w
(C)/%
w
(H)/%
w
(O)/%
w
(N)/%
1
NiC8H22O11N6
436.97
13.29 (13.43)
22.03 (21.97)
5.17 (5.09)
40.36 (40.28)
19.15 (19.23)
2
NiC4H10O4N6Cl2
335.75
17.62 (17.48)
14.48 (14.30)
2.96 (3.01)
18.99 (19.06)
24.92 (25.04)
3
MnC8H19O9
.
5N6
406.19
10.79 (13.53)
23.19 (23.63)
3.69 (4.72)
43.34 (37.42)
28.79 (20.70)
4
MnC4H10O4N6Cl2
332.00
16.42 (16.55)
14.39 (14.46)
2.98 (3.04)
19.35 (19.28)
24.41 (25.32)


## 3.2. UV Spectroscopy Analysis

The UV spectra of the complexes and biuret are shown in Figure1. It is not difficult to find that there is an absorption peak around 200 nm for biuret as well as the four complexes we have synthesized, which shows a close spectral similarity between the four complexes and biuret. In other words, the UV absorption of the complexes derived from biuret. The very strong absorption at short wavelengths is attributed to π-π
∗ transitions, originating from the carbonyl groups of biuret ligand. The locations of the UV absorption peaks for these complexes are found to be a bit different, indicating that some changes in the π-electron system of biuret have taken place. The outer electronic structure of Ni2+ is 3d8, and there is no empty 3d orbit. Compared with Ni2+, the outer electronic structure of Mn2+ is 3d5, and there are two empty 3d orbits. As a result, the electrons of Cl− in 3p orbits can be filled into the empty 3d orbits of Mn2+. Therefore, the UV spectrum of complex4 differs from those of other studied complexes and the free biuret ligand. In conclusion, the oxygen atoms of the carbonyl groups in biuret molecules are coordinated to the metal ions.Figure 1
UV spectra of the complexes and biuret.


## 3.3. IR Spectroscopy Analysis

The IR spectra of the four complexes and biuret are shown in Figures2–4, and the main infrared spectral data of biuret and its complexes are listed in Table 2. In the spectra of the four complexes, two bands (3115−3430 cm−1) are observed in the N−H stretching region. The former one is alternatively assigned to bridging hydroxide whereas the water of hydration band appears near 3400 cm−1 in complexes1 and3. The N−H deformation vibrations are observed at 1530 cm−1 with significant intensities. The carbonyl stretching frequencies in compounds containing the CO−NH−CO group are reported to give rise to two bands [10, 11], the asymmetric stretching vibration peak appears above 1700 cm−1, and the symmetric vibration peak appears near 1700 cm−1. When coordination occurs it determines the amount of electron delocalization in the N−CO−N system; thus, coordination through the oxygen atom will produce a decrease in the double bond character of the C=O bonds and conduct a shift of the carbonyl stretching mode to lower frequencies [12]. The stretching vibration peaks of the C=O bonds in the complexes are detected at 1686, 1693, 1693, and 1685 cm−1, respectively, which are a little lower than the frequency of biuret (1719 cm−1). It is believed that the unprotonated biuret M(II) (M = Ni, Mn) complexes should have the M−O coordinated bonds. On the other hand, the bending vibration peaks of the C=O bonds found in the region of 621−664 cm−1 are the evidence of the coordination between metal ions and oxygen atoms in the ligand as well. In the nickel complexes, the frequency of the stretching vibration peak of the C=O bonds in complex1 containing acetate anions is a little lower than that of complex2 containing chloride anions. However, in the manganese complexes, it is higher in complex3 containing acetate anions than that of complex4 containing chloride anions. Compared with complex1, the stretching vibration peak of the C=O bonds in complex3 moves to high wavenumber, which can illustrate that both the oxygen atoms in biuret molecules and acetate anions are coordinated to the manganese ions in complex3. The absorption peaks at 476 cm−1 in complexes1 and2 are originated to the stretching vibrations of the Ni−O bonds, and the absorption peaks at 459 cm−1 in complexes3 and4 are the characteristic peaks of the Mn−O bonds [13–17].Table 2
Infrared spectra of the ligand and the complexes (cm−1).
bi
[Ni(bi)2(H2O)2](Ac)2·H2O
[Ni(bi)2Cl2]
[Mn(bi)2(Ac)2]·1.5H2O
[Mn(bi)2Cl2]
Vibration type
3415
3433, 3379
3383
3406
3406
ν
a
s(NH2) + ν(H2O)/ν
a
s(NH2)
3254
3196, 3115
3268, 3198
3216
3264, 3196
ν
s(NH2)
1719
1686
1693
1693
1685
ν(C=O)
1585
1530
1582
1551
1571
δ(NH2)
1499, 1423
1445, 1411
1490
1512
1485
ν(C−N) +ν(C−NH2)
1323
1343
1336
1336
1329
δ(N−H)
1130
1126
1127
1140
1120
ν(C−N) + δ(N−H)
1081
1054
1100
1099
1092
ν(C−N)
946
923
943
925
939
ν(C−N) +ν(C−NH2)
770
781
760
780
757
δ(C−NH2)
710
646
646
634
621
δ(C=O)Figure 2
IR spectra of complexes1 and2.Figure 3
IR spectra of complexes3 and4.Figure 4
IR spectrum of biuret.


## 3.4. Raman Spectroscopy Analysis

Figures5 and 6 show the Raman spectra of the complexes obtained in the 400−4000 cm−1 range, and the frequencies data of the biuret and its complexes are listed in Table 3. Obviously, there are many correlations among peaks when comparing the Raman spectra with the IR spectra. For example, the wide absorption peaks in the four complexes from the stretching vibrations of the O−H and N−H bonds appear in the region of 3430−3200 cm−1 in the IR spectra as well as in the Raman spectra. But some differences can be discovered that the bending vibration peaks of the N−H bond near 1320 cm−1 in the Raman spectra are found to be quite weak and even cannot be found comparing with those in the IR spectra. The result may be explained that the N−H bond in biuret is a polar bond, and it is Raman negative. It is well known that when the interaction between the metal cations (M2+) and the coordinated water molecules is strong enough, a Raman band due to the symmetric stretching vibration of M−OH2 is observed in the low-frequency region from 300 to 550 cm−1 [18–22]. The absorption peak at 467 cm−1 for complex1 is assigned to the symmetric M−OH2 stretching vibration.Table 3
Raman spectra of the complexes (cm−1).
bi
[Ni(bi)2(H2O)2](Ac)2·H2O
[Ni(bi)2Cl2]
[Mn(bi)2(Ac)2]·1.5H2O
[Mn(bi)2Cl2]
Vibration type
3370
3433
3382
3398
3398
ν
a
s(NH2) + ν(H2O)/ν
a
s(NH2)
3230
3203
3276
3210
3282
ν
s(NH2)
1690
1691
1685
1698
1685
ν(C=O)
1440
1439
1467
1441
1460
ν(C−N) +ν(C−NH2)
1150
1134
1123
1129
1129
ν(C−N) + δ(N−H)
965
955
938
956
936
ν(C−N) +ν(C−NH2)
775
750
750
709
748
δ(C−NH2)
647
638
627
618
619
δ(C=O)
—
467
473
456
463
ν(M−O)Figure 5
Raman spectra of complexes1 and2.Figure 6
Raman spectra of complexes3 and4.


## 3.5. X-Ray Powder Diffraction Analysis

X-ray powder diffraction (XRD) is measured to confirm the phase purity of the samples. The XRD patterns of the complexes and the ligand are shown in Figures7–9. The background of the XRD patterns is small and the diffractive intensity is strong, indicating that the complex has a fine crystalline state. The strong peak locations of the complexes are shown in Table 4, which are obviously changed comparing with biuret and nickel acetate (JCPDS 26-1282) or nickel chloride (JCPDS 22-0765), manganese acetate (JCPDS 29-0879), and manganese chloride (JCPDS 22-0721). All these strong peaks of the reactants are disappeared in the X-ray powder diffraction patterns of the complexes. The diffraction angle (2
θ), diffractive intensity, and spacing (d) of the products are completely different from the reactive materials, which may illuminate that the resultants are new compounds instead of the reactant mixture [23].Table 4
The data for X-ray powder diffraction patterns of the complexes and biuret.
Compound
The 2θ(°) locations of the main strong peaks (relative intensities are in brackets)
bi
23.51 (100)
28.71 (94)
11.30 (86)
18.88 (69)
21.83 (65)
[Ni(bi)2(H2O)2
](Ac)2·H2O
31.50 (100)
15.45 (60)
45.18 (56)
12.06 (24)
19.51 (22)
[Ni(bi)2Cl2
]
28.68 (100)
13.18 (90)
28.23 (75)
15.19 (74)
24.27 (61)
[Mn(bi)2(Ac)2
]·1.5H2O
23.78 (100)
13.52 (35)
13.13 (32)
29.92 (30)
16.86 (20)
[Mn(bi)2Cl2
]
28.45 (100)
13.13 (60)
27.58 (49)
14.99 (39)
24.12 (36)
Ni(Ac)2·4H2O
12.93 (100)
18.62 (30)
28.34 (20)
22.13 (19)
21.09 (13)
NiCl2·6H2O
15.26 (100)
36.24 (79)
30.08 (30)
51.78 (18)
52.58 (17)
Mn(Ac)2·4H2O
9.068 (100)
11.59 (32)
12.18 (25)
26.20 (8)
27.55 (8)
MnCl2·4H2O
17.93 (100)
20.03 (75)
30.67 (75)
34.54 (45)
16.04 (40)Figure 7
X-ray powder diffraction patterns of complexes1 and2.Figure 8
X-ray powder diffraction patterns of complexes3 and4.Figure 9
X-ray powder diffraction pattern of biuret.


## 3.6. Thermogravimetric Analysis

The thermal behavior of the four complexes is studied from 25°C to 800°C under air. The TG-DTG curves are shown in Figures10–13. The TG analysis (Figure 10) reveals that complex1 is decomposed through four major processes, namely, the loss of lattice water molecules, the coordinated water molecules, and the combustion of biuret ligand and nickel acetate. The first weight loss is approximately 4.27% (calcd. 4.12%) in the range of 64−105°C, corresponding to the weight of one lattice water molecule. There is a weight loss of 8.03% near 137°C for complex1, which is ascribed to the loss of two coordinated water molecules, and the measured value is in agreement with the calculated one (8.25%). The third weight loss occurs between 153°C and 514°C and is characteristic of the combustion of biuret ligand (found 47.58%, calcd. 47.17%). The last weight loss is considered to be the decomposition of nickel acetate (found 23.25%, calcd. 23.36%). As a result, the final residue is nickel oxide. As shown in Figure 11, there are two large weight losses of 60.67% (calcd. 61.40%, loss of two biuret molecules) and 16.73% (calcd. 16.35%, decomposition of nickel chloride) for complex2, and the residual weight in the TG curve is 22.60%, which agrees with the theoretical value (22.25%), and the final residue is determined as nickel oxide. Complex4 is similar to complex2. There are two stages weight losses with the increasing of the temperature, namely, the combustion of biuret ligand (found 61.88%, calcd. 62.10%) and the oxidation of manganese chloride (found 16.24%, calcd. 16.53%), and the final residue is MnO (found 21.88%, calcd. 21.37%). Compared with three other complexes, complex3 undergoes three weight losses of 6.85%, 49.65%, and 25.5% near 104°C, 215°C, and 485°C, respectively, and the first two weight losses agree with the loss of 1.5H2O (calcd. 6.65%) and two biuret molecules (calcd. 49.65%). The last weight losses are considered to be the decomposition of manganese acetate (found 25.40%, calcd. 25.14%) and the final residue is MnO (found 18.10%, calcd. 17.46%). All in all, the thermal behavior of the complexes corresponds to their composition.Figure 10
TG-DTG curves of complex1.Figure 11
TG-DTG curves of complex2.Figure 12
TG-DTG curves of complex3.Figure 13
TG-DTG curves of complex4.


## 4. Conclusion

In summary, the complexes [Ni(bi)2(H2O)2](Ac)2·H2O (1), [Ni(bi)2Cl2] (2), [Mn(bi)2(Ac)2]·1.5H2O (3), and [Mn(bi)2Cl2] (4) were successfully synthesized with nickel acetate or nickel chloride, manganese acetate, manganese chloride, and biuret as raw materials. The four complexes of Ni(II) and Mn(II) were hexacoordinated. It was special that the acetate anions in complex3 were coordinated to the Mn(II) ion, which was not common in most complexes. The optical properties of the complexes were studied via UV, FTIR, Raman spectra, and X-ray powder diffraction. The FTIR spectra were complementary to the Raman spectra, and the structures of the complexes were further verified. The thermal analysis results showed that the decomposition of complexes1 and3 contained the loss of water molecules, the oxidation and decomposition of biuret, and the oxidation of inorganic salts. The thermal decomposition processes of complexes2 and4 are thought to be only the oxidation and decomposition of biuret and the oxidation of inorganic salts, in which there is no water molecule. The final residues were NiO for complexes1 and2 and MnO for complexes3 and4.



---

*Source: 5471818-2016-02-25.xml*