Oxidation and Oxidative Bromination Reactions Catalyzed Bya Reusable Polymer-Anchored Iron(III) Complex in Waterat Room Temperature
Sk. Manirul Islam • Kajari Ghosh •
Anupam Singha Roy • Noor Salam •
Tanmay Chatterjee
Received: 9 September 2013 / Accepted: 14 December 2013 / Published online: 21 December 2013
� Springer Science+Business Media New York 2013
Abstract A polymer-anchored iron(III) catalyst was
synthesized and characterized. Its catalytic activity was
evaluated for the oxidation of various alkenes, sulfides,
aromatic alcohols and ethylbenzene with 30 % H2O2 as the
oxidizing agent. The catalyst was also effective for the
oxidative bromination reaction with 80–100 % selectivity
of monobrominated products with H2O2/KBr at room
temperature. The above reactions require a minimum
amount of H2O2 and short reaction time. Most importantly,
all the above reactions occur in aqueous medium. The
catalyst can be facilely recovered and reused six-atimes
without significant decrease in its activity and selectivity.
Keywords Polymer anchored � Iron(III) complex �Oxidative bromination, H2O2
1 Introduction
Metal complexes are essential elements in the toolbox of
organic chemists. The demand for environmentally friendly
and recyclable metal complexes, which can be used in
catalytic amount, has also increased in recent years [1]. The
separation and recovery of the products and the catalyst are
to be kept in mind. All these requirements are greatly
achieved by the use of heterogeneous catalysts. Thus, the
preparation of such catalysts with high stability is a matter
of great interest [2].
Transition metals like Mn(III), Fe(III), Cu(II) and
Co(II), which are supported on materials such as alumina,
amorphous silicates, polymers, zeolites and MCM-41, are
commonly used in heterogeneous catalysis [3–8]. Recently,
functionalized polystyrene-anchored catalysts were used to
carry out various catalytic organic transformations [9–11].
Among them chloromethylated polystyrene is widely used
as a support. These polystyrene-anchored transition metal
complexes are inert and reusable catalysts for various
organic functional group conversions [12–14].
Schiff bases play a central role as chelating ligands in
main group and transition metals coordination chemistry
[15] as they are capable of binding with transition, non-
transition, lanthanide and actinide metal ions to give
complexes with useful properties. The chelating ability of
Schiff bases combined with the ease of preparation and
flexibility in varying the chemical environment about the
C=N group make them interesting ligands in coordination
chemistry.
Oxidation of olefins is especially important because
oxidation of alkenes gives oxygen-containing products
such as alcohols, aldehydes, ketones, acids and epoxides,
which are extremely important and useful in both chemical
and pharmaceutical industries [16, 17]. Alkane oxidation is
one of the basic reactions in industrial organic synthesis
because aldehydes and ketones are key intermediates for
the manufacture of wide variety of valuable products [16,
18, 19]. Conversion of alcohols to aldehydes and ketones
are among the most important and widely used oxidation
reactions in organic chemistry. Benzaldehyde is a very
useful chemical that has widespread applications in
Electronic supplementary material The online version of thisarticle (doi:10.1007/s10904-013-0017-5) contains supplementarymaterial, which is available to authorized users.
Sk. M. Islam (&) � K. Ghosh � A. S. Roy � N. Salam
Department of Chemistry, University of Kalyani, Kalyani,
Nadia 741235, W.B., India
e-mail: [email protected]
T. Chatterjee
Department of Organic Chemistry, Indian Association for the
Cultivation of Science, Jadavpur, Kolkata 700032, India
123
J Inorg Organomet Polym (2014) 24:457–467
DOI 10.1007/s10904-013-0017-5
perfumery, dyestuff and agricultural chemical industries
[20, 21]. Sulfoxides and sulfones are also useful synthetic
intermediates for the synthesis of several important organic
compounds. Sulfoxides and sulfones are generally prepared
via oxidation of the corresponding sulfides [22–24].
Bromoaromatics are important synthetic intermediates
for a variety of transformations including carbon–carbon
bond formation and carbon–heteroatom bond formation
[25]. The reported methods involve an electrophilic bro-
mination of aromatic rings using brominating agents other
than molecular bromine [26, 27]; others are based on
oxidative bromination [28–32]. Oxyhalogenation is safer
and greener as low-cost and easy-to-handle metal halides
are used as halogenating agents.
Herein, the preparation, characterization and investiga-
tion of catalytic activities for oxidation and oxidative
bromination reactions of a polymer-anchored iron(III)
complex were carried out using H2O2 as the oxygen source.
The catalytic activity of the anchored complex was tested.
2 Experimental
2.1 Materials and Instruments
Analytical-grade reagents and freshly distilled solvents
were used throughout the experiment. Chloromethylated
poly(styrene-divinyl benzene) was supplied by Sigma-
Aldrich chemicals Company, USA. Other reagents were
obtained from Merck Co. Liquid substrates were predis-
tilled and dried with appropriate molecular sieves. Distil-
lation and purification of the solvents and substrates were
done by standard procedures [33].
A Perkin-Elmer 2400 C elemental analyzer was used to
collect micro-analytical data (C, H and N). FTIR spectra of
the samples were recorded on a Perkin-Elmer FTIR 783
spectrophotometer using KBr pellets. A Mettler Toledo
TGA/SDTA 851 instrument was used for the
thermogravimetric (TGA) analysis. The morphology of the
functionalized polystyrene and complex was analyzed
using a scanning electron microscope (SEM) (ZEISS
EVO40, England) equipped with EDAX facility. The metal
content in the catalyst was determined using a Varian
AA240 atomic absorption spectrophotometer (AAS).
Electron paramagnetic resonance (EPR) spectra of the
fresh and used catalyst were recorded at room temperature
with a JES-FA200 ESR spectrometer (JEOL).
2.2 Synthesis of Catalyst
The outline for the preparation of polymer anchored iro-
n(III) complex is given in Scheme 1.
2.2.1 Preparation of Schiff Base Compound (A)
Triethylenetetramine was reacted with salicylaldehyde (1:2
molar ratio) in methanol solvent at 70 �C with stirring for
24-h to prepare the yellow Schiff base compound. The
mixture was cooled to room temperature and then filtered.
The residue was washed with ethanol until the filtrate
became colorless and dried under vacuum.
C20H26N4O2 (Yield, 70 %). Calcd. (%): C 67.80, H
7.35, N 15.82; found: C 67.85, H 7.43, N 15.89. Mass
spectrum (EI): m/z 354 (M? = L?); Infrared spectrum
(cm-1, KBr disk): m(phenolic OH) 3,415(w); m(C=N)
1,632(s); m(phenolic C–O) 1,370(s); m(CH2) 858(m);
m(aromatic CH) 754(m). 1H NMR (CDCl3, ppm):
d = 13.21 (s, 2 H), 8.29 (s, 2H) 7.26–7.45 (m, 8 H),
3.65–3.72 (m, 4 H), 2.79 (t, 4 H), 2.62 (t, 4 H), 2.21 (s, 2H).
2.2.2 Preparation of Polymer-Bound Ligand (B)
The polymer-anchored ligand (B) was prepared as fol-
lows: Chloromethylated polystyrene (1.2 g) was added to
a methanolic solution of Schiff base compound (1 g) and
N NH
NH
N
OH HONH2 NH
NH
NH2
CHO
OH
MeOH, 500C, reflux(A)
OO
N
N
N=CH
N=CH
HO
HO
N
N
N C
N C
FeFeCl3
EtOH
(B)
RefluxMerrifield resign
MeOH, Reflux, 24h
(A)
Cl
OH2
(C)
Scheme 1 Synthesis of
polymer anchored Fe(III)
complex
458 J Inorg Organomet Polym (2014) 24:457–467
123
heated to reflux with continuous stirring. After refluxing,
the mixture was cooled to room temperature and filtered.
The yellow beads were washed with ethanol until the
filtrate became colorless. It was then dried under
vacuum.
2.2.3 Preparation of Polymer-Bound Fe(III) Complex (C)
To the polymer-anchored Schiff base ligand (1 g) in eth-
anol (20 mL), 5 mL of 1 % (w/v) ethanolic solution of
FeCl3 was added drop-wise over a period of *30-min
under constant stirring. The reaction mixture was refluxed
for 24-h. The complex [PS-Fe(III)teta] thus formed was
filtered and washed thoroughly with ethanol and dried at
room temperature under vacuum.
2.3 General Procedure for Oxidation Reaction
Catalyzed by [PS-Fe(III)teta]
Substrates (5 mmol) were dissolved in water (5 mL) for
different sets of reactions together with the catalyst
(50 mg) and H2O2 (10 mmol, 30 % in aq.). After reaction,
the organic products were separated from the mixture by
extraction with dichloromethane (5 mL 9 2). The com-
bined organic portions were dried and concentrated.
Product analysis was performed with a Varian 3400 gas
chromatograph equipped with a 30 m CP-SIL8CB capil-
lary column and a flame ionization detector using cyclo-
hexanone as internal standard. All reaction products were
identified by using Trace DSQ II GC–MS.
2.4 General Procedure for Oxidative Bromination
Reaction of Organic Substrates Catalyzed by [PS-
Fe(III)teta]
In a typical reaction, aqueous H2O2 (30 %, 20 mmol) was
added to a mixture of substrates (10 mmol) and KBr
(20 mmol) dissolved in 10 mL of water. The catalyst
(50 mg) and conc. H2SO4, (36 N, 5 mmol) were added and
the reaction mixture was stirred at room temperature.
Additional H2SO4 (15 mmol) was added to the reaction
mixture in three equal portions at 30-min intervals under
continuous stirring. After a specified time of reaction, the
catalyst was filtered and the solid was washed with ether.
The combined filtrates were washed with saturated sodium
bicarbonate solution and then shaken with ether in a se-
paratory funnel. The organic extract was dried over anhy-
drous sodium sulfate. The products were analyzed
chromatography equipped. The identity of the products was
confirmed by using Trace DSQ II GC–MS.
3 Results and Discussion
3.1 Characterization of Polymer Anchored Fe(III)
Complex
The Schiff base ligand obtained from salicylaldehyde and
triethylenetetramine was characterized and established
earlier [34]. Due to the insolubilities of the polymer-sup-
ported metal complex in all common organic solvents, its
structural investigation was limited to their physicochem-
ical properties, chemical analysis, SEM, TGA, FTIR, EPR
and UV–Vis spectral data. Table 1 provides the elemental
analysis data. The metal content of the polymer-supported
catalyst was estimated by atomic absorption spectroscopy.
The attachment of metal to the support was confirmed
by comparison of the FT-IR spectra (Fig. 1) (4,000–400
and 600–50 cm-1 regions) of the polymers before and after
loading with metals. The IR spectrum of pure chlorome-
thylated polystyrene has an absorption band at 1,261 cm-1
due to the C–Cl bond, which was absent in the ligand and
in the catalyst. The IR spectrum shows a stretching
vibration for –CH2 at 2,918 cm-1 for the polymer-bound
ligand and its complex. The C=N bond stretching vibration
appears at 1,655 cm-1 for the polymer-bound Schiff base
ligand and is lowered to 1,632 cm-1 in the metal complex.
This indicates the coordination of azomethine nitrogen to
the metal [35, 36]. Another band at 3,325 cm-1 is assigned
to O–H stretching, which is shifted to lower region for the
metal complex as the –OH group coordinates with the
metal through oxygen. The band for Fe–O in the metal
complex is observed at *556 cm-1. Bands due to the Fe–
N stretching vibrations at *460 cm-1 establishes the for-
mation of the metal complex through Fe–N bond. Another
peak at 1,366 cm-1 due to the C–O bond decreased to
1,315 cm-1 in (PS-Fe(III)teta) and confirms metal oxygen
coordination [37]. The stretching vibrations do not change
significantly, which suggests the existence of all the
properties in the recycled catalyst (Fig. 1c).
The electronic spectra (Fig. S1, Supporting information)
of the polymer-supported ligand and metal complex were
recorded in diffuse reflectance spectrum mode as MgCO3/
BaSO4 disks. In the UV spectrum of the ligand, two
absorption bands are observed at 235-265 and 330 nm,
Table 1 Chemical composition polymer-anchored ligand and its
iron(III) complex
Compound Colour C
(%)
H
(%)
N
(%)
Cl
(%)
Metal
PS-teta Yellow 78.70 6.99 7.99 3.37 –
PS-[Fe(III)teta] Grey 68.60 6.23 7.12 4.37 3.66
(3.65)a
a Reused catalyst
J Inorg Organomet Polym (2014) 24:457–467 459
123
which are assigned to the n–p* and p–p* transitions,
respectively. The band at 415 nm is presumably caused by
an intraligand charge transfer. These absorptions were also
present in the spectrum of the iron complex, but shifted
showing further evidence for complexation.
Field emission-scanning electron micrographs of a single
bead of pure chloromethylated polystyrene, polymer-
anchored ligand (PS-teta) and its complex [PS-Fe(III)teta]
were recorded. Morphological changes occurred on the
polystyrene beads at various stages of the synthesis. The
SEM images of pure chloromethylated polystyrene (A),
polymer-anchored ligand (B) and the immobilized Fe(III)
complex (C) are shown in Fig. 2. The pure chloromethylated
polystyrene bead has a smooth surface while the polymer-
anchored ligand and complex show a slight roughening of the
outer layer of the bead. This roughening appears relatively
complex. Also, the presence of iron is supported by EDAX
(Fig. S2, Supporting information), which suggests the for-
mation of the metal complex with the polymer-anchored
ligand.
The thermal stability (TGA–DTA) of the complex was
investigated in air from 30 to 600 �C at a heating rate of
10 �C/min. TGA curves of polymer anchored ligand and
iron complex are shown in Fig. S3 (Supporting informa-
tion). The polymer-anchored ligand decomposed from 320
to 330 �C. After complexation iron, the thermal stability
of the immobilized complex increased by 40–70 �C. The
polymer-anchored Fe(III) complex decomposed from 360
to 400 �C; i.e., at considerably higher temperature than
the precursor.
The EPR spectra of the fresh and the used iron catalysts
were recorded for the solid sample at room temperature
Fig. 1 FT-IR spectra of polymer anchored ligand (a), polymer anchored iron(III) catalyst (b) and reused catalyst (c)
Fig. 2 FE SEM images of chloromethylated polystyrene (a), polymer anchored ligand (b) and polymer anchored Fe(III) complex (c)
460 J Inorg Organomet Polym (2014) 24:457–467
123
(Fig. 3). The g values of the fresh catalyst are g1 = 7.84,
g2 = 4.19 and g3 = 1.99 and those of the used catalyst are
g1 = 8.19, g2 = 4.20 and g3 = 2.00. These data indicate
that iron remains in the 3? oxidation state in both the fresh
and used catalyst [38–40].
3.2 Catalytic Activity
The catalytic activity of the polymer-anchored iron(III)
complex was investigated for the oxidation of alkenes,
alkanes, alcohols and sulfides. The activity of the metal
complex as a catalyst was also tested for oxidative bromin-
ation. The reactions were carried out at room temperature
using water as a green solvent.
3.2.1 Oxidation of Alkenes with H2O2 Catalyzed by [PS-
Fe(III)teta]
Oxidation of olefins was carried out in water with H2O2 as
the oxygen source to test the catalytic activity of the metal
complex. For optimization of reaction conditions, styrene
was chosen as the alkene. In this case, styrene was selec-
tively converted to benzaldehyde (Scheme 2).
The effect of various oxidants on the conversion of
styrene and the selectivity of benzaldehyde using [PS-
Fe(III)teta] as a catalyst is summarized in Table S1 (Sup-
porting information). The ability of various oxidants like
TBHP, H2O2, NaIO4, PhIO, KHSO5 and molecular oxygen
for styrene oxidation was investigated (Table S1, entries
2–7). Styrene oxidation did not occur in the absence of an
oxidant (Table S1, entry 1). The reaction shows almost no
conversion when molecular oxygen is used as oxidant
(Table S1, entry 2). Table S1 shows that among the six
oxidants used in styrene oxidation reaction, H2O2 performs
best (Table S1, entry 3). Oxidants such as TBHP, PhIO and
NaIO4 are less efficient as evident from the percentage
conversion (Table S1, entries 4-6). The use of KHSO5 is
not favored because a buffer is needed (Table S1, entry 7).
The activity of the catalyst was also evaluated using three
different styrene-to-H2O2 molar ratios (Table S1, entries 3
and 8–9). The conversion of styrene increased from 69 to
97 % on increasing the molar ratio from 1:1 to 1:2, The
CHO
O
)b()a(enerytS
[PS-Fe(III)teta]
H2O2, H2O, rt
Scheme 2 Oxidation products of styrene
Table 2 Olefins oxidation using H2O2 catalyzed by polymer-
anchored Fe(III) catalyst
Entry Substrate Conversion
(%)aProduct (selectivity
%)aTON
1 Cyclohexene 82 2-Cyclohexene-1-one
(63)
2-cyclohexene-1-ol
(28) Cyclohexene
epoxide (9)
125
2 trans-Stilbene 66 Benzaldehyde (77)
Benzil (16) trans-
Stilbene oxide (7)
101
3 a-Pinene 50 Verbenol (31)
verbenone (55) a-
pinene oxide (14)
76
4 4-
Methylstyrene
82 4-Methyl
benzaldehyde (82)
4-methylstyrene
epoxide (18)
125
5 4-
Chlorostyrene
88 4-Chloro
benzaldehyde (85)
4-chlorostyrene
epoxide (15)
135
6 4-Nitrostyrene 85 4-Nitro
benzaldehyde (82)
4-Nitro styrene oxide
(18)
130
7 a-Methyl
styrene
80 Acetophenone (100) 122
Reaction conditions: catalyst (0.05 g), substrate (5 mmol), water
(5 mL), H2O2 (10 mmol), time (6 h)a Determined by GC
Fig. 3 X-band EPR spectra of Fe in (a) fresh catalyst and (b) used
catalyst
J Inorg Organomet Polym (2014) 24:457–467 461
123
conversion was barely affected by a further increase in
ratio to 1:3. Thus, a 1:2 ratio is sufficient for good con-
version of styrene. A control experiment (Table S1, entry
10) in the presence of an oxidant under the same reaction
conditions was also investigated and showed that H2O2
alone has poor oxidizing ability.
The above optimized reaction conditions can be applied
to the oxidation reaction of other olefins catalyzed by the
polymer-anchored Fe(III) catalyst. The results are shown in
Table 2. This catalyst efficiently converts olefins to their
corresponding allylic products with H2O2 in aqueous
medium. In the oxidation of cyclohexene, allylic products,
2-cyclohexene-1-one and 2-cyclohexene-1-ol, were pro-
duced. Substituted styrene was selectively converted to
their corresponding aldehydes. Acetophenone was detected
in the oxidation of a-methyl styrene as a major product.
trans-Stilbene was also oxidized by this heterogeneous
catalyst in high yields. trans-Stilbene gave benzaldehyde as
a major product with benzil. This catalytic system also
showed good activity in the case of a-pinene. In the oxi-
dation of a-pinene, the major products were verbenone and
verbenol.
3.2.2 Oxidation of Ethylbenzene with H2O2 Catalyzed
by [PS-Fe(III)teta]
Oxidation of ethylbenzene catalysed by [PS-Fe(III)teta]
using H2O2 as oxidant was performed; and, the products
were benzaldehyde (a), phenylacetic acid (b), acetophe-
none (c) and 1-phenylethane-1,2-diol (d) (Scheme 3).
The effect of the amount of oxidant (moles H2O2/moles
ethylbenzene) was studied. It was observed that the con-
version was best using a substrate:oxidant mole ratio of
1:3. The influence of H2O2 concentration on the oxidation
of ethylbenzene was studied considering ethylbenzene:
aqueous 30 % H2O2 molar ratios of 1:2, 1:3 and 1:4, while
keeping ethylbenzene (10 mmol), catalyst (0.050 g), H2O
(10 mL) constant. Thus, the conversion improved from
18 % at a molar ratio of 1:2 to 52 % at 1:3 and finally to
53 % at a molar ratio of 1:4 in an 8-h reaction time
(Fig. 4). However, at the expense of the oxidant, a mini-
mum molar ratio of 1:3 is necessary to observe maximum
oxidation.
The effect of the amount of catalyst on the oxidation of
ethylbenzene is illustrated in Fig. 5. Here the reaction
proceeded slowly to give only 16 % conversion with
0.040 g of catalyst using the above reaction conditions.
Increasing the catalyst amount to 0.050 g improved this
O
OH
OO HO
OH
[PS-Fe(III) teta]H2O2, H2O, rt
Ethylbenzene (a) (b) (c) (d)
+ + +
Scheme 3 Oxidation products
of ethyl benzene
0 100 200 300 400 5000
5
10
15
20
25
30
35
40
45
50
55
60
% c
onve
rsio
n
time/min
1:2 1:3 1:4
Fig. 4 Effect of amount of H2O2 on the oxidation of ethylbenzene.
Reaction conditions: ethylbenzene (10 mmol), PS-[Fe(III)teta]
(0.050 g), H2O (10 mL) and at room temperature
0 100 200 300 400 5000
5
10
15
20
25
30
35
40
45
50
55
60
% c
onve
rsio
n
time/min
0.040 g 0.050 g 0.060 g
Fig. 5 Effect of amount of catalyst on the oxidation of ethylbenzene.
Reaction conditions: ethylbenzene (10 mmol), H2O2 (30 mmol), H2O
(10 mL) and at room temperature
462 J Inorg Organomet Polym (2014) 24:457–467
123
conversion to 52 %. Further addition of catalyst showed no
improvement in oxidation. It was noticed that the products
formed are independent of the oxidant and catalyst amount
and follow the order: benzaldehyde (71.6 %) [ phenyla-
cetic acid (20.5 %) [ acetophenone (4.7 %) [ 1-phenyle-
thane-1,2-diol (3.2 %). A very small amount of an
unidentified product was also noticed. No significant
improvement in the oxidation of ethylbenzene was
observed beyond an 8-h reaction time. A blank experiment
under the optimized experimental conditions in the pre-
sence of oxidant and in the absence of the catalyst was also
investigated. The results showed that, without the catalyst,
H2O2 has poor ability to oxidize the alkane.
3.2.3 Oxidation of Aromatic Alcohols with H2O2
Catalyzed by [PS-Fe(III)teta]
Catalytic oxidation of alcohols generally needs an organic
solvent and addition of base. Thus in line with the
requirements of ‘‘green chemistry’’, we chose water as a
reaction medium to conduct the oxidation of alcohols in the
absence of base (Scheme 4).
The catalytic activity of the polymer anchored iron(III)
catalyst was examined for the oxidation of benzyl alcohol by
changing the various reaction conditions. The effect of the
amount of H2O2 on the oxidation of benzyl alcohol to
benzaldehyde was studied (Table 3). The percent conversion
of benzyl alcohol to benzaldehyde is dependent on the
quantity of H2O2 used to a considerable amount. The benzyl
alcohol-to-H2O2 molar ratio of 1:1 resulted in 67 % con-
version when the amount of catalyst was 50 mg (reaction
time, 6-h). When the molar ratio was increased to 1:2, the
conversion increased to 97 % (same reaction conditions).
However, the conversion was found to be almost constant
when the molar ratio was further increased to 1:3. Therefore,
a 1:2 molar ratio of benzyl alcohol-to-H2O2 is optimum.
The results for the oxidation of benzyl alcohol in the
presence of different amounts of catalyst are presented in
Fig. S4. All the tests were conducted with 5 mmol of
substrate, 10 mmol of H2O2, 5 mL of water under base free
condition at room temperature. A conversion of 25 %
within 6-h was obtained when 0.02 g of polymer-anchored
catalyst was used. No by-products such as benzoic acid
were detected. When the amount of the catalyst was
increased to 0.04 g, the conversion increased to 80 %
conversion. In this experiment, a small amount of benzoic
acid was detected. A further increase if catalyst amount to
0.05 g led to an increase in the conversion to 97 %.
However, when the catalyst amount was increased to 0.06
and 0.07 g, the conversion remained almost constant; but,
the selectivity for benzaldehyde was reduced. These find-
ings indicate that the oxidation of benzyl alcohol is highly
dependent on the amount of the catalyst.
In order to study the catalytic activity of the catalyst for
the oxidation of aromatic alcohols, a series of benzylic
alcohols was used. Substituted benzyl alcohols are also
oxidized to their corresponding aldehydes. In all the above
cases, trace amounts of acids as products were observed.
3.2.4 Oxidation of Sulfides with H2O2 Catalyzed by [PS-
Fe(III)teta]
Sulfide oxidation with the [PS-Fe(III)teta] catalyst was also
studied. Thus, when methyl phenyl sulfide was treated with
CH2OH CHO COOH
[PS-Fe(III) teta]
H2O2, H2O, rt
Benzyl alcohol (a) (b)
+
Scheme 4 Oxidation products of benzyl alcohol
Table 3 Oxidation of aromatic alcohols with 30 % H2O2 catalyzed
by Fe(III) catalyst
Entry Aromatic alcohol Conversion
(%)aProduct
Selectivity (%)aTON
1b Benzyl alcohol 67 Benzaldehyde (90)
Benzoic acid (10)
103
2c Benzyl alcohol 97 Benzaldehyde (94)
Benzoic acid (6)
149
3d Benzyl alcohol 95 Benzaldehyde (71)
Benzoic acid (29)
146
4 4-Methoxybenzyl
alcohol
80 4-Methoxy
benzaldehyde
(84)
4-Methoxy benzoic
acid (16)
123
5 4-Methylbenzyl
alcohol
85 4-methyl
benzaldehyde
(91)
4-methyl benzoic
acid (9)
130
6 4-Nitrobenzyl
alcohol
79 4-Nitro
benzaldehyde
(89)
4-Nitro benzoic
acid (11)
121
7 1-Phenyl ethanol 78 Acetophenone
(100)
120
Reaction condition: aromatic alcohol (5 mmol), 30 % H2O2 (10 mmol),
water (5 mL), catalyst (50 mg), time (6 h), room temperaturea Determined by GCb Benzyl alcohol:H2O2 = 1:1c Benzyl alcohol:H2O2 = 1:2d benzyl alcohol:H2O2 = 1:3
J Inorg Organomet Polym (2014) 24:457–467 463
123
[PS-Fe(III)teta] and 30 % H2O2 in water at room temper-
ature, methyl phenyl sulfoxide was obtained (Scheme 5).
Methyl phenyl sulfide as a model substrate was subjected to
different reaction conditions (Table S2). The effect of tem-
perature for the oxidation of methyl phenyl sulfide is given in
Table S2. The amount of H2O2 has a significant effect on the
conversion and selectivity the oxidation reaction. Conversion
increased when amount of H2O2 was increased from 5 mmol
(Table S2, run 2) to 10 mmol (Table S2, run 1). However,
there was no significant change in conversion when the
amount of H2O2 was increased to 15 mmol (Table S2, run 3,
same reaction conditions). Moreover, the selectivity of oxi-
dation of sulfide to sulfoxide decreased with the increase in the
amount of H2O2. This is due to further oxidation of sulfoxide
to the corresponding sulfone.
The reaction was also monitored using different quantities
of catalyst. On using a lower catalyst amount The reaction
takes a longer time and is incomplete with a smaller amount
of catalyst is used (Table S2, 40 mg, run 4). However, with
50 mg of catalyst (Table S2, run 1), the reaction complete
within 4-h, yielding 95 % sulfoxide with a small amount of
sulfone (5 %). On increasing the amount of catalyst to 60 mg
(Table S2, run 5), the reaction gives more sulfone along with
sulfoxide. Based on the above observations it is concluded
that 50 mg of polymer-anchored catalyst, 10 mmol 30 %
H2O2 with water as a solvent are the best conditions for the
selective oxidation of sulfide to sulfoxide. It was also found
that without H2O2, [PS-Fe(III)teta] alone cannot oxidize
sulfide (Table S2, run 6).
To examine further the reactivity of the catalyst, oxi-
dation of other sulfides were investigated (Table 4). The
substrate was extended to diphenyl sulfide, ethyl phenyl
sulfide and dibutyl sulfide. The sulfoxides were selectively
obtained in all cases. A series of substrates, aryl alkyl, aryl
allyl and dialkyl sulfides, can be oxidized to their corre-
sponding sulfoxides. The reactivity and conversion were
dependent on the nature of the substituent. In the case of
allyl sulfides, oxidation of the carbon–carbon double bond
was observed to a smaller extent. Similarly, benzylic sul-
fides can be oxidized to their corresponding sulfoxides with
a little amount of oxidation at the benzylic C–H position.
3.2.5 Oxidative Bromination Catalyzed by [PS-Fe(III)teta]
In the present study, oxidative bromination was optimized
using salicylaldehyde as a substrate (Scheme 6).
Two different parameters; e.g., volume of sulfuric acid and
amount of H2O2, were varied. The results showed that, for a
fixed amount of salicylaldehyde (10 mmol), catalyst
(0.050 g), KBr (20 mmol) in 10 mL water, at least 20 mmol of
H2SO4 and 20 mmol of H2O2 were sufficient to give maximum
conversion. The conversion of salicylaldehyde significantly
improved from 60 to 98 % with an increase on H2SO4 from 10
to 20 mmol. The presence of excess acid may decompose the
catalyst under the above reaction conditions. H2SO4 was added
to the reaction mixture in definite time intervals to prevent
decomposition of catalyst. Under optimized reaction condi-
tions, the performance of the polymer-anchored catalyst is
summarized in Table 5. Approximately 98 % conversion of
salicylaldehyde was obtained with ca. 100 % selectivity in the
formation of 5-bromosalicylaldehyde.
The effect of added salt was studied using H2O2 as an
oxidant and MBr (M = Li, Na, K) as a bromine source
(Table 5). Among the three salts, KBr was the most efficient
bromine source and a monoselective product is obtained.
The use of sodium bromide did not produce regioselective
products. LiBr, though efficient, was less than KBr.
SCH3
SCH3
O
SCH3
O
O[PS-Fe(III) teta]
H2O2, H2O, rt
Methyl phenyl sulfide Methyl phenyl sulfoxide Methyl phenyl sulfone
Scheme 5 Oxidation products
of methyl phenyl sulfide
OH
CHO
OH
CHOBr
[PS-Fe(III) teta]
H2O2, KBr, H2SO4,H2O, rt
Scheme 6 Oxidative bromination of salicylaldehyde
Table 4 Oxidation of sulfides using 30 % H2O2 catalyzed by poly-
mer-anchored Fe(III) catalyst
Entry Substrates Conversion
(%)a/time
(h)
Selectivity
of sulfoxide/
sulfone (%)a
TON
(approx)
1 C4H9SC4H9 89/5 78/22 137
2 PhSPh 94/4 90/10 144
3 PhSC2H5 92/4 89/11 71
4 PhSC6H13 85/5 89/11 141
5 PhSCH2Ph 85/4 83/17 130
6 PhSCH2CH=CH2 70/5 86/14 107
7 p-ClC6H4SCH3 88/4 70/30 134
8 p-CH3C6H4SCH3 93/4 90/10 143
Conditions: Sulfide (5 mmol); 30 % aq H2O2 (10 mmol); water
(5 mL); 50 mg catalyst at room temperaturea Conversion and selectivity were determined by GC
464 J Inorg Organomet Polym (2014) 24:457–467
123
The influence of temperature was also studied; there was
no effect on the conversion of salicylaldehyde. With an
increase in temperature, the conversion of salicylaldehyde
was almost the same.
The role of hydrogen peroxide was confirmed by con-
ducting a control experiment in which the formation of the
bromo compound was not observed.
Oxidative bromination of other organic substrates was
studied under optimized reaction conditions (Table 5). All the
substrates were selectively converted to their mono-bromi-
nated products. Substrates like phenol, resorcinol, anisole and
N,N-dimethylaniline showed high conversion and excellent
para-selectivity. Inactive substrates, like benzene, showed a
low conversion and required long reaction times. On the other
hand, deactivated aromatic rings gave no conversion at these
reaction conditions. 4-Substituted aromatics are selectively
converted to 2-bromo derivatives and vice versa.
4 Test for Heterogeneity
The leaching of iron from polymer-anchored iron(III) com-
plex was confirmed by carrying out analysis of the used
catalyst (EDX, IR) and the product mixtures (AAS, UV–
Vis). Analysis of the used catalyst did not show appreciable
loss of iron content relative to the fresh catalyst. An IR
spectrum of the recycled catalyst is similar to that of fresh
sample indicating the heterogeneous nature of the complex.
Analysis of the product mixtures showed that, if any iron was
present, it was below the detection limit. The UV–Vis
spectrum was also used to determine the stability of the
catalyst. Thus, the UV–Vis spectrum of the reaction solution
in the first run did not show absorption peaks characteristic of
iron metal, which indicates that the leaching of metal did not
take place during the course of the reaction. The metal
content of the recycled catalyst was determined by AAS. It
was found that the iron content of the recycled catalyst
remained almost unaltered. These observations strongly
suggest that the catalyst present is heterogeneous in nature.
A heterogeneity test was carried out for the oxidation of
styrene. For a rigorous proof of heterogeneity, a test was
carried out by filtering the catalyst from the reaction
mixture at room temperature after 4-h. The filtrate was
allowed to react up to the completion of the reaction (6-h).
The reaction mixture at 4 h and the filtrate were analyzed
by gas chromatography. No change in the % conversion
selectivity was found, which indicates that the catalyst is
heterogeneous.
Table 5 Oxidative bromination of various organic substrates catalyzed by polymer-anchored Fe(III) catalyst
Entry Substrate Conversion (%)a (time/h) Product selectivitya,b TON
1b Salicylaldehyde 60 (3.0) 5-Bromo-2-hydroxy benzaldehyde (100) 184
2c Salicylaldehyde 98 (3.0) 5-Bromo-2-hydroxy benzaldehyde (100) 300
3d Salicylaldehyde 90 (3.0) 5-Bromo-2-hydroxy benzaldehyde (80) 275
4e Salicylaldehyde 82 (3.0) 5-Bromo-2-hydroxy benzaldehyde (66) 251
5 Phenol 97 (2.5) 4-Bromophenol (100) 298
6 Resorcinol 96 (2.5) 4-Bromo-1,3-dihydroxybenzene (100) 294
7 4-Methylphenol 95 (2.5) 2-Bromo-4-methylphenol (100) 291
8 4-Nitrophenol 83 (6.0) 2-Bromo-4-nitrophenol (100) 254
9 Anisole 94 (3.0) 4-Bromoanisole (100) 288
10 Aniline 96 (2.5) 4-Bromoaniline (85) 294
11 4-Methylaniline 93 (3.0) 2-Bromo-4-methylaniline (87) 285
12 4-Chloroaniline 87 (3.0) 2-Bromo-4-chloroaniline (100) 266
13 2-Methylaniline 89 (3.0) 4-Bromo-2-methylaniline (82) 272
14 2-Chloroaniline 93 (3.0) 4-Bromo-2-chloroaniline (93) 285
15 N,N-Dimethylaniline 94 (3.0) 4-Bromo-N,N-dimethylaniline (100) 288
16 Benzene 12 (6.0) Bromobenzene (100) 37
17 Nitrobenzene – – –
Conditions: substrate (10 mmol); KBr (20 mmol); H2SO4 (20 mmol); 30 % aq H2O2 (20 mmol), water (10 mL), 50 mg catalyst at room
temperaturea Conversion and selectivity were determined by GCb H2SO4 (10 mmol)c KBr as bromine sourced LiBr as bromine sourcee NaBr as bromine source
J Inorg Organomet Polym (2014) 24:457–467 465
123
5 Recycling of Catalyst
The catalyst remained insoluble under the reaction condi-
tions. Hence, it can be easily separated by simple filtration
and washing. The catalyst was washed with dichloro-
methane and dried at 100 �C. Oxidation of styrene, ethyl
benzene, methyl phenyl sulfide and benzyl alcohol was
carried out with the recycled catalyst under the optimized
reaction conditions. The catalyst was recycled to test its
activity and stability. The results are presented in Fig. 6.
The catalyst did not exhibit any appreciable change in
activity, which indicates that it is stable and can be
regenerated for repeated use. Similarly, recycling of the
catalyst was tested for the oxidative bromination of sali-
cylaldehyde. No appreciable change in conversion and
selectivity indicates was observed for the reused catalyst.
6 Conclusions
A chloromethylated polystyrene-anchored iron(III) com-
plex was prepared and characterized. The complex is an
active and reusable catalyst for the oxidation of alkenes,
alkanes, sulfides and alcohols. The catalyst also shows
excellent catalytic activity in oxidative bromination. The
catalyst is stable and recyclable under the reaction condi-
tions used. The heterogeneous catalyst shows no significant
loss of activity in recycling experiments. The active sites
do not leach from the support and the catalyst can be reused
without appreciable loss of activity indicating effective
anchoring. The reusability of this catalyst is high (i.e. six-
times) without significant decrease in activity.
Acknowledgments SMI acknowledges Department of Science and
Technology (DST) and Council of Scientific and Industrial Research
(CSIR), New Delhi, India for funding. ASR acknowledges CSIR,
New Delhi, for providing his senior research fellowship. We
acknowledge Indian Association for the Cultivation of Science,
Kolkata for instrumental support.
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