chapter v poly (n-vinyl-2-pyrrolidone)-cu(oac) 2: an...
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CHAPTER V
Poly (N-vinyl-2-pyrrolidone)-Cu(OAc)2: An Efficient and Reusable
Catalyst for Sulfimidation
Chapter V
187
CHAPTER V
Poly (N-vinyl-2-pyrrolidone)-Cu(OAc)2: An Efficient and Reusable Catalyst for
Sulfimidation
Introduction
The vast chemistry of sulfoxides and sulfonium ylides make them very useful
reagents in organic synthesis. These compounds are important synthetic intermediates for
the construction of various chemically and biologically significant molecules.1 Several
successful methods have been developed for the synthesis of these compounds.2 But
Sulfimides, the nitrogen analogues of sulfoxides although have been widely used as
important auxillaries for chiral ligands and structural units in pseudopeptides,3 are less
investigated due to scarcity of appropriate nitrogen sources, as opposed to oxidants that
are available in wide variety and forms.4
Thus there have been many excellent methods developed for oxidation in terms of
stereoselectivity, mildness of reaction conditions, atom-efficiency and ecological
benignity; however the number of nitrogen-atom-transfer reactions satisfying such terms
has been very limited.3
In view of this, development of efficient methods for selective imidation of
sulfides to sulfimides has been desired for many years. However, only a few of them
have been found to yield the desired products in high yields under mild conditions.
State of the Art
In 1983, Groves and Takahashi reported that irradiation of Mn(porphyrin)(azide)
complex gave a nitride-Mn species that underwent aziridination by treatment with
trifluoroacetic anhydride in the presence of olefins, via an N-trifluoroacetyl nitrenoid
Chapter V
188
species.5 Later, nitride-Mn(salen) complex was also reported to undergo aziridination
under similar conditions.
Mansuy et al.6 demonstrated for the first time that PhI=NTs could convert Fe and
Mn complexes into corresponding nitrenoid species for aziridination and allylic
amination reactions, depending on the olefin used (Scheme 1).
PhI=NTs + FeIII
(TPP)
Ph Ph
NTs
Ph Ph
+ PhI + FeIII(TPP)
H2O
TsNH2 + [PhI=O + FeIII (TPP)]
or [PhI + (TPP)Fev=O ]
Ph Ph
O
Ph Ph
+ PhI + FeIII(TPP) + TsNH2
37%
Scheme 1
Evans et al.7
reported enantioselective aziridination of olefins using
bis(oxazoline)-copper complexes (Scheme 2).
Scheme 2
Jacobsen and co-workers studied the mechanistic aspects of the aziridination
reaction using Cu(I) (diimine) catalyst.8
Chapter V
189
Later, Bolm and co-workers3i
reported Fe(acac)3 catalyzed imidation of sulfides
and sulfoxides (Scheme 3).
Scheme 3
Latour and co-workers9 have reported amidation of thioanisole using a non-heme
iron complex (Scheme 4).
NFe
OFe
N
N
N
N
SH
III II
O O O O
X X
NFe
OFe
N
N
N
N
NHTs
III II
O O O O
X X
CH3CN
ArI=NTs
Scheme 4
Sharpless and co-workers10
reported metal free reactions in presence of
chloramine-T with moderate yields and longer reaction times (Scheme 5).
Scheme 5
Chapter V
190
Later, Bolm and co-workers11
described sulfimidation using 4-
nitobenzenesulfonamide (NsNH2) and iodobenzene diacetate [PhI(OAc)2] (Scheme 6).
Scheme 6
Initially, sulfimides were prepared in its chiral form either by conversion from
enantiomerically pure sulfoxides12
or by kinetic resolution of racemic sulfimides in the
presence of an optically active base.13
Later, Catalytic asymmetric sulfimidation using
PhI=NTs as nitrene donor in the presence of chiral Cu(I) bis(oxazoline) complex has
been described by Uemura et al.14
with moderate enantioselectivity albeit longer reaction
time (Scheme 7).
Scheme 7
Katsuki et al. reported asymmetric sulfimidation with good enantioselectivity
using Mn(salen)15
and Ru(salen)16
complexes (Scheme 8).
Chapter V
191
MePhS
MePhS+
-NTs
PhPh
O OMn
NMO (50mol%)
PhI=NTs, PhCl, rt
PF6
R
R
3'3
55%84%ee
Scheme 8
Owing to several economic and environmental advantages of heterogeneous
catalysts, like easy separation of the products reusability of the catalysts, heterogeneous
catalytic reactions are one of the most important ones and widely used in the industry.
Various supports have been used over the years to immobilize metal catalysts, one of the
important group among them are the polymers.
Polymer supported catalysts have been of great interest due to several advantages
such as the ease of product separation, isolation and reuse of the catalyst.17
But the use of
insoluble polymers as supports have some drawbacks as the reactivity and selectivity of
the supported catalysts is lesser than the unsupported analogs.18
Chapter V
192
In recent years, there have been intense efforts to develop methods to recover and
reuse homogenous catalysts.18,19
Poly (vinylpyrrolidone) (PVP) (Figure 1) is a water
soluble, biocompatible, physiologically inert polyamide polymer exhibiting unusual
colloidal and complexing properties.20
N
O
CH2
H2C
n
Figure 1. Molecular structure of PVP
PVP stabilized nanoscale metal colloids have been reported for selective
hydrogenation reactions21
(Scheme 9)
CH=CH C=O
H
CH=CH CH2OH
CH2 CH2 C=O
H
CH2 CH2 CH2OHPVP-metal nano-colloids
(1)
(2)
(3)
(4)
Scheme 9
Hu et al.22
reported PVP-CuCl2 catalyst for the oxidative carbonylation of
methanol to dimethyl carbonate (Scheme 10).
NO
Cu
ClCl
MeOH140oC; 1-7h;
Dimethyl carbonate
Scheme 10
Wang and co-workers23
reported PVP supported nanosized palladium metal
colloids for Sonogashira and Suzuki coupling reactions (Schemes 11 and 12).
Chapter V
193
H + I
Pd colloids on PVP
K2CO3, EtOH
Scheme 11
BF3K + X
R'R
Pd/PVP, K2CO3
H2O
R, R'= substituent
Scheme 12
Recently, Kantam et al.24
have reported catalytic sulfimidation of various sulfides
by using microencapsulated Cu(acac)2 and Cu(acac)2 immobilized in ionic liquids using
PhI=NTs (Scheme 13).
R2R1 S+
R2R1 S TsN=IPh
-NTs
MC-Cu(acac)2
R2R1 S+
R2R1 S TsN=IPh
-NTs
Cu(acac)2/ [bmim][BF4]
up to 92%
up to 94%
Scheme 13
There is a need for the development of new and efficient catalyst for the imidation
of sulfides with high selectivity, high atom efficiency and reusability.
Present Work
In this chapter, an efficient sulfimidation reaction using poly(vinylpyrrolidone)
supported cupric acetate in the presence of PhI=NTs [(N-(p-
tolylsulfonyl)imino]phenyliodinane) as nitrene donor has been described.
Scheme 14
Chapter V
194
Results and Discussion
Synthesis and Characterization of PVP-Cu(OAc)2
The preparation of PVP-Cu(OAc)2 was based on the literature procedure.22
Cupric
acetate (0.150 g) was added to a solution of PVP (Mw 40,000, 1g) in methanol (50 mL)
and the mixture was refluxed under nitrogen atmosphere for 12h. The resulting solution
was concentrated under reduced pressure to give powdered PVP-Cu(OAc)2 (Cu 0.467
mmol/g). The copper content in the catalyst was found to be 2.93% by AAS analysis.
The resulting catalyst was characterized by powdered X-ray photoelectron spectroscopy
(XPS), TGA-MS, Electron spin resonance spectroscopy, UV-Vis Diffuse Reflectance
Spectroscopy (UV-DRS) and FTIR spectroscopic techniques.
FTIR spectroscopy
The FTIR analysis of PVP, fresh and used PVP-Cu(OAc)2 has been carried out
and the IR spectrum (Figure 1) of PVP showed a characteristic stretching band
corresponding to amide carbonyl group at 1657 cm-1
whereas in PVP-Cu(OAc)2, there is
a red shift of the amide carbonyl group to 1631 cm-1
with a shoulder at 1637 cm-1
indicating the interaction of the metal ion with amide carbonyl moiety of PVP.22
Both
PVP and PVP-Cu(OAc)2 showed characteristic bands at 2925 and 3418 cm-1
originating
from the amide group of PVP.
Chapter V
195
Figure 2. IR spectra of (a) PVP, (b) fresh catalyst and (c) used catalyst.
Chapter V
196
X-ray photoelectron spectroscopy (XPS)
The XPS survey scan of PVP-Cu(OAc)2 showed the presence of oxygen (535
eV), nitrogen (400 eV), carbon (285 eV) and copper (935 eV). High resolution narrow
scan for Cu 2p in PVP-Cu(OAc)2 catalyst showed binding energy peaks at 934.9 and
955.1 eV (Table 1) corresponding to Cu 2p3/2 and Cu 2p1/2 photoelectron transitions
respectively characteristic of Cu in +2 oxidation state. The observed binding energies
peaks of N 1s (398.9 eV) and O 1s (531.2 eV) in PVP-Cu(OAc)2 are close to N 1s (399.0
eV) and O 1s (531.8 eV) peaks in PVP. These results indicate the electronic modification
of Cu(II) on coordination with the amide moiety of PVP and thus, Cu(II) being
immobilized on the polymer. However, XPS spectrum of the used catalyst showed the
presence of both Cu(I) and Cu(II) states (Fig. 3b).
Table 1. XPS data for the binding energies (eV) of PVP, PVP- Cu(OAc)2 and used PVP-
Cu(OAc)2
XPS peak PVP PVP-Cu(OAc)2 Used PVP-Cu(OAc)2
N1s 399.0 398.9 398.6
O1s 531.8 531.2 531.2
Cu 2p3/2, 2p1/2 - 934.9, 955.1 (934.6, 955.6), (932.4, 952.0)a
[a] Binding energy of Cu in +1 oxidation state
Chapter V
197
Figure 3. XPS high resolution narrow scan of Cu 2p in (a) PVP-Cu(OAc)2 fresh catalyst
and (b) PVP-Cu(OAc)2 used catalyst
ESR and UV DRS spectroscopy
ESR and UV-Vis-DR spectroscopy have been used to understand the coordination
of Cu2+
ions in PVP. Both the fresh and used catalysts exhibit axial ESR spectra of Cu2+
ions at room temperature with resolved hyperfine structure (Fig. 5). The observed
hyperfine splitting parameters for the fresh and used catalyst are g = 2.38, 2.37; g⊥ =
2.08, 2.07, and A = 14, 13 mT respectively. The UV-Vis-DRS spectra (Fig. 6) showed
Chapter V
198
a characteristic absorption band at 700-750 nm corresponding to d-d transitions between
T2g and Eg terms typical for isolated Cu(II) ions in an octahedral environment with slight
tetragonal distortion. Another peak is observed around 300 cm-1
which can be ascribed to
the n-π* transition of the carbonyl group in PVP. The shoulder around 350 cm-1
is due to
the presence of the carbonyl group in the copper acetate. These results are in good
agreement with the ESR and UV-Vis DR spectra of Cu2+
ions in various zeolites.25
Figure 4. ESR spectra of Cu2+
ions in (a) fresh and (b) used PVP-Cu(OAc)2 catalyst at
the X-band recorded at room temperature.
Chapter V
199
Fig. 5. UV-Vis-DR spectrum of (a) fresh PVP-Cu(OAc)2 (b) Cu(OAc)2 (c) used PVP-
Cu(OAc)2 and (d) PVP.
Catalytic activity of PVP-Cu(OAc)2 in sulfimidation reaction
In the preliminary experiments, sulfimidation of thioanisole using PhI=NTs in the
presence of PVP-Cu(OAc)2 has been studied in various solvents under nitrogen
atmosphere (Table 2). The reaction was found to be more efficient in acetonitrile
compared to methanol, ethanol and 2-propanol and there was no reaction in DMF,
DMSO and water.
Chapter V
200
Table 2. Effect of solvents for the sulfimidation of thioanisole with PhI=NTs using PVP-
Cu(OAc)2a
Entry Solvent Yield (%)
1 Acetonitrile 98
2 Methanol 48
3 Ethanol 50
4 2-Propanol 50
5 DMF -
6 DMSO -
7 H2O -
[a] Reaction conditions: Thioanisole (0.5 mmole), PhI=NTs (0.5 mmol),
catalyst (0.025 g, 2.3 mol %), solvent (3 mL) under nitrogen atmosphere
for 0.6 h
Different nitrene donors were evaluated for the synthesis of sulfimides and the
results are shown in (Table 3). PhI=NTs was found to be more efficient nitrene donor
compared to chloramine-T and bromamine-T.
Table 3. Sulfimidation of thioanisole using different nitrene donors.
Nitrene donor Time (h) Yield (%)a
PhI=NTs
Chloramine-T
Bromamine-T
0.6
12
12
98
15
18
[a] Isolated Yields
Different sulfides were studied for the reaction under the optimized conditions using
PVP-Cu(OAc)2 as catalyst and the corresponding sulfimides were obtained in good to
excellent yields (Table 4). However, the reaction in the presence of Cu(OAc)2. H2O gave
Chapter V
201
the product in 50% yield (Table 4, entry 1). Aliphatic as well as aromatic sulfides were
equally effective for the reaction. Aromatic sulfides with electron-releasing substituents
were found to be more reactive than aromatic sulfides with electron-withdrawing
substituents (Table 4, entries 2 and 3). Whereas, sterically hindered sulfides, diphenyl
sulfide required longer reaction time (Table 4, entry 5).
Further, when the reaction was applied to allylic sulfides, there was no aziridination of
the double bond. Instead, [2,3] sigmatropic rearrangement with the formation of
sulfonamide through a sulfimide intermediate has been observed. Allylic sulfides were
less reactive and required longer reaction times when compared to aliphatic sulfides
(Table 4 entries 8 and 9). The catalyst was reused for several cycles and showed
consistent activity (Table 4, entry 1). The leaching of the metal after the fourth cycle was
determined by AAS analysis and was found to be 2 %.
Chapter V
202
Table 4. Sulfimidation of sulfides with PhI=NTs using PVP-Cu(OAc)2 a
Entry
1
2
3
4
Sulfide Time (min) Product Yield (%)
5
6
7
S
S
S
S
S
Br
S
S
8
9
S
NTs
S
NTs
S
NTs
Br
S
NTs
S
NTs
S3 3
S3 3
NTs
ClS
Cl S
NTs
SN
Ts
SN
Ts
40
35
40
120
210
30
40
50
180
98, 95b, 48c
98
82
96
75
98
90
78d
72d
-
-
-
-
-
+
+
+
+
+
+
+
-
-
[a]
Reaction condition: Sulfide (0.5 mmole), PhI=NTs (0.5 mmol), catalyst
(0.025 g, 2.3 mol %), acetonitrile (3 mL) under nitrogen atmosphere for 0.5 to
3.5 h.
[b] Yield after 4
th cycle.
[c]
In the presence of Cu(OAc)2.H2O (2.3 mol %). d[2,3] sigmatropic
rearrangement.
Chapter V
203
In order to extend the scope of this methodology, the asymmetric synthesis of
sulfimides using 4, 4’-disubstituted bis(oxazolines) 1a and 1b (BOX) as chiral ligands
was carried out under similar reaction conditions (Scheme 15). When bis(oxazoline)
ligand 1a was used, higher ees were obtained in comparison to the reaction with 1b as the
ligand. Sulfides with electron donating substituents gave higher ee’s when compared to
the sulfides with electron withdrawing substituents (Table 5).
BOX (3-5 mol%) upto 68% ee
SR R'
PVP-Cu(OAc)2;CH3CN
PhI=NTs, rt RS
R'
NTs-
+ *
O
N N
O
R R
1a R = t- butyl 1b R = Ph
BOX
Scheme 15
Chapter V
204
Table 5. Asymmetric sulfimidation of sulfides with PhI=NTs using PVP-Cu(OAc)2 .a
Entry Substrate Ligand Isolated yield% % eeb[a]
1
SCH3
SCH3
SCH3
Br
2
3
1a
1b
1a
1b
1a
1b
95
96
95
95
78
80
50
10
7
4
68
5
92 24c
5Cl
S
4
S 1a
1b
1a
1b
90
80
88
85
5
2
60
5
Time (min)
35
40
40
120
40
[a]
Reaction condition: Sulfide (0.5 mmol), PhI=NTs (0.5 mmol), catalyst (0.025g,
2.3 mol%), bis(oxazoline)/Cu = 2, acetonitrile (3 mL) were used.
[b] The ee values were determined by HPLC using Daicel Chiralcel OJ-H column
(hexane/2-propanol = 4 : 1, flow rate 1.0 mL/min).
[c] With bis(oxazoline)/Cu = 1.
Reusability study of the catalyst in asymmetric sulfimidation
The catalyst was recovered, reused and the results are summarized in Table 6. The
decrease in enantioselectivity in the recycle experiments can be explained by the TGA-
MS studies of the bis(oxazoline) ligand in the fresh and the used catalyst.
Chapter V
205
Table 6. Recovery and reuse of PVP-Cu(OAc)2-BOX catalyst for asymmetric
sulfimidation of thioanisole.a
Entry Cycle no Isolated yield (%) ee%b
1 1 95 50
2 2 95 15, 50c
3 3 95 15
[a] Reaction condition:Sulfide (0.5 mmol), PhI=NTs (0.5 mmol), catalyst (0.025g)
acetonitrile (3 mL) were used.
[b] 2
nd and 3
rd cycle ee% obtained without the use of additional amount of ligand
[c] 3 mol% of ligand added.
As can be seen in Fig. 6 and 7, the evolved gas fragments as a function of
temperature showed the fragments m/Z values 15, 57, 84 and 126 a.m.u in both the
catalysts resulting from the presence of tertiary butyl substituted bis(oxazoline) ligand in
the catalyst. Remarkable changes were observed in the onset of the decomposition
temperatures in both the fresh and used catalyst. In the fresh catalyst the onset of the
ligand decomposition is observed at 425 oC whereas in the recovered catalyst it is
observed at 250 o
C, at much lower temperature. This clearly suggests that in the fresh
catalyst, the ligand is chemisorbed where as in the recovered catalyst the ligand appears
to be physically adsorbed, so the decrease in the onset of decomposition. These ligand
molecules present on the surface of the support are responsible for the 15% ee’s in the
recycle experiments, however consistent yield of the product was obtained in all the
recycles. On the other hand, addition of fresh amounts of ligand after the first cycle gave
the product with 50 % ee. Therefore, it can be concluded that the immobilization of
Chapter V
206
bis(oxazoline) ligand-Cu complex by electrostatic interactions cannot be properly
performed due to its low binding constant leading to the presence of ligand free copper
on the support after the first cycle, which noticeably reduces the enantioselectivity.
Fig. 6. TGA-MS of the fresh catalyst with t-butyl bis(oxazoline) ligand.
Chapter V
207
Fig 7. TGA-MS of the used catalyst with t-butyl bis(oxazoline) ligand.
Plausible Mechanism
A plausible mechanism of the sulfimidation reaction can be proposed on the basis
of the literature reports.16a
First the metal nitreneoid species (2) is formed by the
interaction of PhI=NTs with the catalyst by the loss of the labile acetate ligand (L), then
the intermediate sulfide-metal nitrene species (3) is formed in the next step by the
interaction of the metal with the sulfide, this sulfide-metal-nitrene species subsequently
losses the iodobenzene molecule and forms the S-N bond (4). This intermediate having
sulfide moiety bonded directly to the nitrene species then forms the sulfimide product.
The redox process involving Cu(II) and Cu(I) takes place during the course of the
reaction which is detected by XPS analysis of the new catalyst and the used catalyst
(Scheme 16).
Chapter V
208
N
Ts
S
R'
R
Cu
L
L
Cu
L
N
IPhTs
- L
PhI=NTs
RS
R'
PhI
Cu
N
Ts
Cu
RS+
R'
-NTs
II
II
II
II
= PVP
L= Acetate+2L
- L
RS
R'
PhI
Cu
I
(1)
(2)
(3)
(4)(5)
Scheme 16
Conclusions
In summary, PVP-Cu(OAc)2 was synthesized, well characterized and employed as a
catalyst for the sulfimidation of sulfides in the presence of PhI=NTs ([N-(p-
tolylsulphonyl)imino]-phenyliodinane) as nitrene donor to afford the corresponding
sulfimides in good to excellent yields. In the presence of chiral bis(oxazoline) ligand,
asymmetric induction occurs to afford chiral sulfimides with moderate
enantioselectivities. The catalyst can be reused for several cycles with consistent activity.
Chapter V
209
Experimental Section
General
X-ray photoelectron spectra were recorded on a KRATOS AXIS 165 with a dual
anode (Mg and Al) apparatus using the Mg-Kα anode. The pressure in the spectrometer
was about 10-9
Torr. For energy calibration the carbon 1s photoelectron line is used. The
carbon 1s binding energy was taken to be 285.0 eV. The spectra were deconvoluted using
Sun Solaris based Vision 2 curve resolver. The location and the full width at half
maximum (FWHM) for a species was first determined using the spectrum of a pure
sample. The location and FWHM of products which were not obtained as pure species
were adjusted until the best fit was obtained. Symmetric Gaussian shapes were used in all
cases. Binding energies for identical samples were in general, reproducible to within ±
0.1 eV. Diffuse reflectance UV-Vis absorption spectra for samples as KBr pellets were
recorded on a GBC Cintra 10e in the range 200-800 nm with a scan speed of 400 nm/min.
ESR spectra were recorded on JEOL JES-FA 200 ESR spectrometer operating in the X-
band frequencies with a field modulation of 100 kHz. The microwave frequency was set
at 9.45 GHz and the magnetic field was scanned between 225 mT to 425 mT. Infrared
spectra were recorded on a Thermo Nicolet Nexus 670 FT-IR spectrometer as KBr
pellets. Thermogravimetric (TG), differential thermal analysis (DTA) and mass of the
evolved gas during the thermal decomposition of the catalyst were studied on
TGA/SDTA Mettler Toledo 851e system coupled to MS Balzers GSD 300T, using open
alumina crucibles, containing samples weighing about 8-10mg with a linear heating rate
of 10oC min
-1. NMR spectra were recorded on a Varian Gemini (200 MHz), Bruker
Avance (300 MHz), Varian Unity (400MHz) spectrometer using TMS as an internal
Chapter V
210
standard and CDCl3 as solvent. Mass spectra were obtained at an ionisation potential of
70 eV [scanned on VG 70-70H (micro mass)]. Only selected ions are presented here.
Melting points were recorded on Barnstead electrothermal 9200 instrument and are
uncorrected. CHNS analysis was performed on a Vario EL analyzer. High performance
Liquid Chromatography (HPLC) was performed using AGILENT-1100 series liquid
chromatograph equipped with a single pump and UV detector (fixed at 205 nm) using
CHIRACEL-OJ-H capillary column with isopropanol/hexane as eluting agent. All the
other solvents and chemicals were obtained from commercial sources and purified using
standard methods. PVP (K=30) was purchased from Fluka. Cu(OAc)2. H2O was
purchased from S.D Fine Chemicals, India. Iodobenzene diacetate, p-toluene sulfonamide
and sulfides were purchased from Aldrich or Fluka and used without further purification.
ACME silica gel (100–200 mesh) was used for column chromatography. Thin-layer
chromatography was performed on Merck-precoated silica gel 60-F254 plates. All the
other solvents and chemicals were obtained from commercial sources and purified using
standard methods.
Synthesis of PVP-Cu(OAc)2 catalyst
The preparation of PVP-Cu(OAc)2 was based on the literature procedure.22
Cupric acetate (0.150 g) was added to a solution of PVP (Mw 40,000, 1g) in methanol
(50 mL) and the mixture was refluxed under nitrogen atmosphere for 12h. The resulting
solution was concentrated under reduced pressure to give powdered PVP-Cu(OAc)2 (Cu
0.467 mmol/g). The copper content in the catalyst was found to be 2.93% by AAS
analysis.
Chapter V
211
Typical procedure for sulfimidation using PVP-Cu(OAc)2
To acetonitrile (3 mL) were added PVP-Cu(OAc)2 (0.025 g, 2.3 mol %), methyl phenyl
sulfide (0.062 g, 0.5 mmol) and PhI=NTs (0.186 g, 0.5 mmol) and the reaction mixture
was stirred at room temperature for the appropriate time as shown in Table 2. The
reaction was monitored by the disappearance of PhI=NTs from the reaction mixture and
by thin layer chromatography. After completion of reaction, the reaction mixture was
concentrated and washed with 1:4 hexane/ethyl acetate. The combined organic extracts
were concentrated and the crude solid was purified by recrystallization from iso-propanol
and water or by column chromatography on silica gel (hexane/ethyl acetate, 20/80 v/v as
eluent) to afford the pure product as white solid.
Representative examples
S-p-tolyl, S-methyl N-p-toluenesulfonyl sulfimide (Table 4, entry 2)
Figure 8. 1H NMR (CDCl3, 300 MHz): δ = 2.37 (s, 3H), 2.43 (s, 3H), 2.82 (s, 3H), 7.15
(d, 2H), 7.29 (d, J= 8.3 Hz, 2H), 7.59 (d, J= 8.3 Hz, 2H), 7.71 (d, J= 8.3 Hz, 2H).
Figure 9. 13
C NMR (CDCl3, 75 MHz): δ = 21.35, 21.40, 39.15, 43.38, 123.5, 125.82,
126.25, 129.12, 130.00, 129.08, 130.60, 132.72, 141.29, 141.29, 141.57, 143.32.
S-Phenyl, S-ethyl, N-p-toluenesulfonyl sulfimide (Table 4, entry 4)
Figure 10. 1H NMR (CDCl3, 300 MHz): δ = 1.21 (t, J= 6.7 Hz, 3H), 2.36 (s, 3H), 3.00
(q, J= 6.7, 12.8 Hz, 2H), 7.15 (d, J= 8.3 Hz, 2H), 7.50 (d, 2H, Ar-H), 7.70 (m, 5H).
Figure 11. 13
C NMR (CDCl3, 75 MHz): δ = 21.33, 47.82, 126.22 (2C), 126.25 (2C),
129.08 (2C), 129.77 (2C), 132.26 (2C), 141.30, 141.53.
Rest of the products were characterized similarly and the results obtained were
similar to that reported in the literature.14, 16, 26
Chapter V
212
References
1. (a) J. Drabowski, P. Kielbasinski, M. Mikolajezyk, Synthesis of Sulfoxides, Wiley,
New York, 1994; (b) M. Mikolajczyk, Tetrahedron 1986, 42, 549.
2. (a) T. L. Gilchrist, C. J. Moody, Chem. Rev. 1977, 77, 409; (b) E. G. Mata
Phosphorus, Sulfur Silicon Related Elem. 1996, 117, 231; (c) H. Kagan, T.
Luukas Transition Met. Org. Synth. 1998, 2, 361.
3. (a) C. Bolm, K. Muniz, J. P. Hildebrande, Comprehensive Asymmetric Catalysis
Ed. E. N. Jacobsen, A. Pfaltz, H. Yamamoto, Berlin: Springer 1999, 697; (b) H.
B. Kagan, Catalytic Asymmetric Synthesis, Ed. I. Ojima, New York: Wiley-VCH
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