Oxidation of disulfides to thiolsulfinates with hydrogen peroxide and a cyclic seleninate ester catalyst peroxide and a cyclic seleninate ester catalyst

Article abstract of DOI:10.3390/molecules200610748

Cyclic seleninate esters function as mimetics of the antioxidant selenoenzyme glutathione peroxidase. They catalyze the reduction of harmful peroxides with thiols, which are converted to disulfides in the process. The possibility that the seleninate esters could also catalyze the further oxidation of disulfides to thiolsulfinates and other overoxidation products under these conditions was investigated. This has ramifications in potential medicinal applications of seleninate esters because of the possibility of catalyzing the unwanted oxidation of disulfide-containing spectator peptides and proteins. A variety of aryl and alkyl disulfides underwent facile oxidation with hydrogen peroxide in the presence of catalytic benzo-1,2-oxaselenolane Se-oxide affording the corresponding thiolsulfinates as the principal products. Unsymmetrical disulfides typically afforded mixtures of regioisomers. Lipoic acid and N,N′-dibenzoylcystine dimethyl ester were oxidized readily under similar conditions. Although isolated yields of the product thiolsulfinates were generally modest, these experiments demonstrate that the method nevertheless has preparative value because of its mild conditions. The results also confirm the possibility that cyclic seleninate esters could catalyze the further undesired oxidation of disulfides in vivo.

Full text of DOI:10.3390/molecules200610748

Molecules 2015, 20, 10748-10762; doi:10.3390/molecules200610748
OPEN ACCESS
molecules
ISSN 1420-3049
www.mdpi.com/journal/molecules
Article
Oxidation of Disulfides to Thiolsulfinates with Hydrogen
Peroxide and a Cyclic Seleninate Ester Catalyst
Nicole M. R. McNeil, Ciara McDonnell, Miranda Hambrook and Thomas G. Back *
Department of Chemistry, University of Calgary, Calgary, AB T2N 1N4, Canada;
E-Mails: nmrmcnei@ucalgary.ca (N.M.R.M.); mcdonnci@tcd.ie (C.M.);
miranda.hambrook@hotmail.com (M.H.)
* Author to whom correspondence should be addressed; E-Mail: tgback@ucalgary.ca;
Tel.: +1-403-220-6256.
Academic Editor: Derek J. McPhee
Received: 24 May 2015 / Accepted: 4 June 2015 / Published: 11 June 2015
Abstract: Cyclic seleninate esters function as mimetics of the antioxidant selenoenzyme
glutathione peroxidase. They catalyze the reduction of harmful peroxides with thiols, which
are converted to disulfides in the process. The possibility that the seleninate esters could
also catalyze the further oxidation of disulfides to thiolsulfinates and other overoxidation
products under these conditions was investigated. This has ramifications in potential medicinal
applications of seleninate esters because of the possibility of catalyzing the unwanted
oxidation of disulfide-containing spectator peptides and proteins. A variety of aryl and alkyl
disulfides underwent facile oxidation with hydrogen peroxide in the presence of catalytic
benzo-1,2-oxaselenolane Se-oxide affording the corresponding thiolsulfinates as the principal
products. Unsymmetrical disulfides typically afforded mixtures of regioisomers. Lipoic acid
and N,N′-dibenzoylcystine dimethyl ester were oxidized readily under similar conditions.
Although isolated yields of the product thiolsulfinates were generally modest, these experiments
demonstrate that the method nevertheless has preparative value because of its mild conditions.
The results also confirm the possibility that cyclic seleninate esters could catalyze the further
undesired oxidation of disulfides in vivo.
Keywords: cyclic seleninate esters; thiolsulfinates; disulfides; organoselenium redox catalysts;
glutathione peroxide mimetics

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1. Introduction
The selenoenzyme family of glutathione peroxidases (GPx) catalyzes the reduction of harmful
hydrogen peroxide and lipid hydroperoxides by the stoichiometric reductant glutathione. This process
provides protection to living organisms against oxidative stress caused by peroxides and other reactive
oxygen species they generate, such as the superoxide radical anion and the hydroxyl radical [1–3].
Consequently, the design and synthesis of small-molecule selenium compounds that emulate the function
of GPx has proven of interest as a means to suppress oxidative stress that is implicated in a variety of
disease states [4–9]. Our group [10–14] and that of H.B. Singh [15–17] have independently investigated
the use of various types of cyclic seleninate esters for this purpose. Thus, seleninate ester 1 and its
congeners effectively catalyze the in vitro conversion of benzyl thiol to the corresponding disulfide with
hydrogen peroxide, as shown in Scheme 1. In the course of this work, we recently observed that in the
case of certain related seleninate esters, the concentration of the disulfide reached a maximum at ca.
50%–60% completion of the reaction and then began to decrease in the later stages of the process [18].
Such unexpected behaviour suggested that the catalyst might be promoting further oxidation of the
initially formed disulfide in this model system. This hypothesis was confirmed by the isolation of
thiolsulfinate 2a (R = benzyl in Scheme 1) and the detection of products of its further decomposition
from the late-stage reaction mixtures [18]. In order to gain further insight into this process, which has
both biological relevance for these and other GPx mimetics, as well as potential synthetic utility, we
embarked on a further study of the oxidation of dibenzyl disulfide with hydrogen peroxide in the
presence of 1, as well as its extension to a variety of other symmetrical and unsymmetrical disulfides. It
is also worth noting that 1 is an effective catalyst for the oxidation of sulfides to sulfoxides, alkenes to
epoxides and enamines to α-hydroxy ketones (Scheme 2) [19].
Scheme 1. Catalytic reduction of hydrogen peroxide with thiols in the presence of cyclic
seleninate ester 1 as catalyst.

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Scheme 2. Catalytic oxidation of sulfides, alkenes and enamines with hydrogen peroxide
and cyclic seleninate ester 1 as catalyst.
Furthermore, it is relevant to note that thiolsulfinates have interesting biological properties. They are
produced by various Allium or Brassica species when chopped or crushed and contribute to the odour and
flavour of these plants [20]. Furthermore, some thiolsulfinates have been reported to display antibacterial,
antifungal, antiviral and anticancer activity [20–27]. For example, allicin (2i) is the compound that is
chiefly responsible for the reported antimicrobial activity of garlic. This compound was discovered
by Cavallito et al. in 1944 [21] and its biogenesis was later shown to proceed by C-S bond cleavage of
(S)-allylcysteine (S)-oxide, catalyzed by the enzyme alliinase and resulting in the formation of allyl
sulfenic acid. Condensation of two molecules of the latter with loss of water then affords 2i [27].
Recently, thiolsulfinates have been shown to function as antioxidants and radical inhibitors [28,29].
There are several existing methods for the preparation of thiolsulfinates. The most common ones
involve the oxidation of the corresponding disulfides with peracids [21,22,28,30–33]. Other oxidants
that have been employed include singlet oxygen [31,34], dioxiranes [35] and hydrogen peroxide or tert-butyl
hydroperoxide in the presence of vanadium [36,37], rhenium [38] molybdenum [39] or tungstic acid [40]
catalysts, or in protic acid [41] media. Uncatalyzed hydrogen peroxide reacts very slowly with
disulfides [42]. Connective methods via the reactions of sulfinyl chlorides [43,44], sulfinic acids [45]
or sulfinamides [46] with thiols or tin thiolates [43] provide alternative routes to thiolsulfinates. Several
enantioselective variations have also been reported [33,35–37,46]. Thiolsulfinates vary greatly in
stability and their preparation is often capricious. Exposure to acidic or basic media, or even to silica-gel
chromatography, can result in their decomposition. Furthermore, they are prone to overoxidation to
thiolsulfonates and other products [30,47–51]. The yields of thiolsulfinates obtained by these methods
are therefore highly variable and substrate-dependent. Many of the products described in the older literature
are poorly characterized. These considerations, the inexpensive and environmentally benign nature of
hydrogen peroxide, as well as our prior success in catalyzing the processes shown in Schemes 1 and 2
with cyclic seleninate ester 1 prompted us to investigate the oxidation of disulfides further with hydrogen
peroxide in the presence of 1. Finally, additional insight was required into the possibility that cyclic
seleninate esters such as 1 could catalyze the unintended oxidation of disulfide bonds in spectator
peptides and proteins during applications as biological antioxidants and therapeutic GPx mimetics.

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2. Results and Discussion
The optimization of the preparation of thiolsulfinate 2a from dibenzyl disulfide is summarized in
Table 1. In the examples in the table, the disulfide and hydrogen peroxide, each at a concentration of
0.1 M, were allowed to react in the indicated solvent at room temperature, in the presence of catalyst 1.
The reaction in chloroform proved relatively slow, achieving less than 50% completion after more than
4 h (entry 1). The use of acetonitrile, a 70:30 mixture of ethyl acetate and methanol or dichloromethane
resulted in more rapid reaction rates with improved conversion to the product 2a and higher isolated
yields (entries 2–4, respectively). A decrease in the amount of catalyst from 10 mol % to 5 or 1 mol %
reduced the reaction rate drastically (entries 5 and 6). A 95:5 mixture of dichloromethane and methanol
with 10 mol % of 1 afforded optimum conditions, with isolation of 64% of the thiolsulfinate (entry 7).
In our previous work [19], we had observed that the presence of trifluoroacetic acid (TFA) accelerated
the oxidations shown in Scheme 2, while basic conditions suppressed them. The same is evident in the
present case, where the inclusion of 20 mol % of TFA accelerated the reaction in dichloromethane-methanol
considerably and afforded a comparable yield of the product (entry 8), while the presence of 20 mol %
of cesium carbonate inhibited the oxidation completely (entry 9). Since some thiolsulfinates proved more
sensitive to acidic conditions than 2a, we chose the conditions of entry 7 for further applications. A
control reaction in the absence of the cyclic seleninate 1 revealed that the uncatalyzed background
oxidation of the disulfide with hydrogen peroxide is too slow to contribute significantly to the reaction
(entry 10). Finally, with the substrate and conditions indicated in Table 1, only traces of the corresponding
thiolsulfonate 3a (PhCH2SSO2CH2Ph) were detected.
Table 1. Optimization of conditions for the synthesis of thiolsulfinate 2a a.
Catalyst 1, mol %
Entry
Solvent
Time (h) Ratio of 2a:SM b Yield c, %
(+ Additive)
1
2
CHCl3
MeCN
10
4.25
1.0
3.0
2.0
4.5
29
43:57
85:15
85:15
85:15
62:38
13:87
15
46
57
53
35
8
10
3
EtOAc–MeOH (70:30)
CH2Cl2
10
4
10
5
CH2Cl2
5
6
CH2Cl2
1
7
CH2Cl2–MeOH (95:5)
CH2Cl2–MeOH (95:5)
10
3.0
1.25
6.0
24
92:8
64
66
0
d
8
10 (+ 20 mol % TFA)
9
CH2Cl2–MeOH (95:5) 10 (+ 20 mol % Cs2CO3)
CH2Cl2–MeOH (95:5)
0:100
0:100
10
0
0
b
a: Conditions: equimolar amounts of PhCH2SSCH2Ph and H2O2 were used at room temperature; : Ratio
1
determined by H-NMR integration of the crude material prior to chromatography; SM = starting material;
d
c: Isolated yields of thiolsulfinate 2a are reported; : In addition to 2a, a complex mixture of byproducts
was formed.

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The conditions of Table 1, entry 7, which also most closely resemble those of our assay for GPx-like
activity [10–14], were then applied to a variety of symmetrical and unsymmetrical disulfides (Tables 2 and
3, respectively). The oxidations of symmetrical diaryl disulfides are provided in entries 2–5 of Table 2,
while entry 1 shows the oxidation of the benzyl derivative 2a for comparison. Oxidation of the
electron-rich diaryl disulfide in entry 4 was accompanied by significant thiolsulfonate formation, while
the electron-withdrawing p-fluoro substituent in entry 3 suppressed reactivity, resulting in a substantial
amount of the unreacted disulfide under the usual conditions. The phenyl and 4-fluorophenyl derivatives
2b and 2c proved difficult to isolate and purify, resulting in a significant loss of material, although TLC
indicated their relatively clean initial conversion from the corresponding disulfides. In general, the
formation of the thiolsulfinates was accompanied by small amounts of thiolsulfonates 3, along with
minor quantities of the starting disulfides. The mixtures were separated by flash chromatography on
silica gel, which was carried out rapidly because some of the thiolsulfinates were prone to decomposition
during the process. The chromatographic separation of 2d and 3d (entry 4) could not be achieved and the
yield is reported for the unseparated mixture. The conversions of the dialkyl disulfides in entries 6–9 to the
corresponding thiolsulfinates 2f–2i proceeded smoothly, even in the case of the hindered t-butyl product
2f. The ether- and ester-substituted products 2j and 2k, respectively, showed no sign of overoxidation to
3j and 3k, while the 2-hydroxyethyl disulfide in entry 12 failed to undergo any significant oxidation under
the usual conditions. Again, substantial losses of the aliphatic products occurred during separation and
purification, resulting in relatively modest isolated yields, especially in the case of allicin (2i).
Table 2. Oxidation of symmetrical disulfides to thiolsulfinates 2 a.
Entry
R
PhCH2
Time (h)
2:3:SM b
92:trace:8
nd d
48:trace:52 e
59:35:6
92:trace:8
84:2:14
93:trace:7
88:8:4
Thiolsulfinate Yield, % c
1
2
3
4
2a
2b
2c
2d
2e
2f
64
23
38
90 f
55
41
54
56
31
59
50
NR
Ph
3
4-F-Ph
3
4
4-MeO-Ph
4-Me-Ph
t-Bu
4
5
5
6
2.5
3
7
n-Pentyl
iso-Bu
2g
2h
2i
8
3
9
Allyl
3
nd
10
11
12
MeOCH2CH2
PhC(=O)OCH2CH2
HOCH2CH2
6
80:0:20
92:0:8
2j
6
2k
4
NR
2l
a: Conditions: equimolar amounts of disulfide and H2O2 along with 10 mol % of 1 in dichloromethane-methanol
(95:5) were used at room temperature; b: Ratio of crude product mixture determined by integration of 1H-NMR
c
signals, except where otherwise indicated; SM = starting material; : Isolated yields of thiolsulfinates are
reported; NR = no reaction was observed; d: Ratio could not be determined due to absence or overlap of suitable
NMR signals for integration; e: Ratio was determined by integration of 19F-NMR signals; f: Yield is reported
for the unseparated mixture of 2d and 3d.

Molecules 2015, 20
Table 3. Oxidation of unsymmetrical disulfides to thiolsulfinates 4 and 5 a.
10753
Entry
R
Time (h) 4:5:6:SM b Thiolsulfinates c
Yield, % d
1
2
3
4-MeO-Ph
t-Bu
3
4
33:33:33:0
67:12:0:21
68:8:8:16
4a + 5a
4b + 5b
4c e
43
63
47
n-C6H13
3.5
a: Conditions: equimolar amounts of disulfide and H2O2 along with 10 mol % of 1 in dichloromethane-methanol
(95:5) were used at room temperature; b: Ratio in crude product mixture determined by integration of 1H-NMR
c
d
signals; SM = starting material; : Unseparated mixtures of regioisomers 4 and 5 were obtained; : Isolated
yields of thiolsulfinates are reported; e: Product 4c was isolated as a pure regioisomer in 47% yield; products
5c and 6c could not be separated and their combined yield was 16%.
The unsymmetrical disulfides shown in Table 3 were obtained by a literature method [52]. Their
oxidations were intrinsically more complex because inseparable regioisomers, as well as overoxidation
products, were possible. The aryl-substituted product in entry 1 was produced as a mixture of equal
amounts of the two regioisomers 4a and 5a. On the other hand, the phenyl alkyl-substituted disulfides
in entries 2 and 3 afforded predominantly the regioisomers 4, where oxidation occurred proximally to
the alkyl substituent, even in the case of the hindered t-butyl derivative 4b. The greater reactivity of the
more electron-rich alkyl-substituted sulfur atom is expected, and has been observed previously with
other electrophilic oxidants [30]. The thiolsulfinates in entries 1 and 3 were again accompanied by small
amounts of regioisomeric mixtures of thiolsulfonates. The similar oxidation of racemic lipoic acid (7)
afforded roughly equal amounts of four inseparable products 8–11. Based on the NMR spectra of the
mixture, we conclude that it consists of the two regioisomers, each formed as mixtures of two
diastereomers as a result of the chiral nature of the thiolsulfinate moiety (Scheme 3).
Scheme 3. Oxidation of (±)-lipoic acid with hydrogen peroxide and catalyst 1.
Finally, we investigated the oxidation of (L)-N,N′-dibenzoylcystine dimethyl ester (12) under the
usual conditions, catalyzed by seleninate ester 1. The complete consumption of the starting material was
observed after 6 h, resulting in a complex mixture of products that could not be separated. However, the
NMR and mass spectra of the mixture were consistent with the formation of the stereoisomers of the
corresponding thiolsulfinate, in addition to unidentified material (Scheme 4). This suggests that cyclic

Molecules 2015, 20
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seleninate ester 1 and its congeners could be capable of oxidizing disulfide linkages in native proteins
and peptides in the presence of peroxides when employed as GPx mimetics in vivo.
Scheme 4. Oxidation of a cystine derivative with hydrogen peroxide and catalyst 1.
While no direct mechanistic studies were carried out on the present oxidations of disulfides to
thiolsulfinates, the process very likely proceeds via a similar pathway to that described previously for
the oxidations shown in Scheme 2 [19]. This involves the initial formation of a peroxyseleninic acid 14
or peroxyselenurane 13 from 1 and hydrogen peroxide, which is enhanced by prior protonation of 1 with
an acid catalyst. This is followed by oxygen transfer to the most electron-rich sulfur atom of the disulfide,
as shown in Scheme 5. Failure of the reaction under basic conditions is attributed to the formation of
anions 15 or 16, which are unable to react further with hydrogen peroxide to generate the active oxidant
intermediates 13 or 14.
Scheme 5. Mechanism for the oxidation of disulfides with hydrogen peroxide and catalyst 1.
3. Experimental Section
3.1. General Information
Symmetrical disulfides were obtained from commercial sources, while unsymmetrical disulfides were
prepared by thiolysis of N-(phenylthio)phthalimide via the method of Harpp et al. [52] except that

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toluene instead of carbon tetrachloride was employed as the solvent. The preparation of cyclic seleninate
ester 1 was carried out by the previously described procedure [11,13]. Hydrogen peroxide (ca. 30%) was
titrated prior to use [53]. 1H-NMR spectra were recorded at 400 MHz, while 13C- and 77Se-NMR spectra
77
were obtained at 101 and 76 MHz, respectively. Chemical shifts of Se-NMR spectra were obtained
with diphenyl diselenide in CDCl3 (463.0 ppm) [54] as the standard, relative to dimethyl selenide
(0.0 ppm), while C6F6 (−164.9 ppm) in CDCl3, relative to CFCl3 (0.0 ppm), was the standard for 19F-NMR
spectra [55]. High resolution mass spectra were obtained using a time of flight (TOF) analyzer with
electron impact (EI) ionization or a quadrupole TOF analyzer with electrospray ionization (ESI).
3.2. Typical Procedure: Preparation S-Benzyl Phenylmethanesulfinothioate (2a)
Dibenzyl disulfide (245 mg, 1.00 mmol) and cyclic seleninate ester 1 (20 mg, 0.10 mmol) were
dissolved in 10 mL of dichloromethane at room temperature with stirring. Hydrogen peroxide (127 μL,
26.4% w/v, 1.00 mmol) was added to the solution. The mixture was stirred at room temperature and
progress was monitored by TLC. After 3 h, the reaction was diluted with dichloromethane, washed with
brine and dried with Na2SO4. The product was purified by flash chromatography on silica gel (hexane-ethyl
acetate, 10:1) to afford 139 mg (53%) of 2a. The product had properties identical to those reported
previously [18]. When the reaction was repeated in dichloromethane-methanol (95:5), a slightly higher yield
of 64% was obtained. The other thiolsulfinates in Tables 2 and 3 were prepared similarly, with any changes
to the above conditions as noted in the Tables. Characterization data for the other products follows.
3.3. S-Phenyl Benzenesulfinothioate (2b)
Pale yellow powder (23%; mixture of 2b (major) [43] and 3b (minor); IR (film) 1333, 1152, 1100,
1
1052, 743 cm−1; H-NMR (400 MHz, CDCl3) δ 7.66 (dd, J = 6.6, 3.0 Hz, 2 H), 7.55–7.33 (m, 8 H);
13C-NMR (101 MHz, CDCl3) δ 135.3, 131.5, 130.3, 129.2, 128.9, 124.3, 114.4 (signals from
thiolsulfonate 3b: δ 144.0, 136.6, 129.4, 129.3; 128.7, 127.5; HRMS (ESI-TOF) m/z [M + Na]+ calcd
for C12H10NaOS2: 257.0065; found: 257.0065.
3.4. S-4-Fluorophenyl 4-Fluorobenzenesulfinothioate (2c)
White solid (38%) [49,50]; mp 73–75 °C, lit. [49] mp 75.5–76.5 °C; IR (film) 1395, 1233, 1109,
1081, 833 cm−1; 1H-NMR (400 MHz, CDCl3) δ 7.63–7.56 (m, 2 H), 7.46–7.40 (m, 2 H), 7.17 (t, J = 8.6 Hz,
2 H), 7.07 (t, J = 8.6 Hz, 2 H); 13C-NMR (101 MHz, CDCl3) δ 164.5 (d, J = 253.1 Hz, CF), 164.4 (d,
J = 252.2 Hz, CF), 139.3 (d, J = 3.1 Hz), 137.8 (d, J = 9.0 Hz), 126.6 (d, J = 9.2 Hz), 123.8 (d, J = 3.5 Hz),
116.5 (d, J = 21.9 Hz), 116.3 (d, J = 22.8 Hz); 19F-NMR (376 MHz, CDCl3) δ −107.1, −109.1; HRMS
(ESI-TOF) m/z [M + H]+ calcd for C12H9F2OS2: 271.0057; found 271.0053; m/z [M + Na]+ calcd for
C12H8F2NaOS2: 292.9877; found: 292.9874.
3.5. S-4-Methoxyphenyl 4-Methoxybenzenesulfinothioate (2d)
The product was isolated as an inseparable mixture of the thiolsulfinate 2d [39] and thiolsulfonate 3d
as a yellow oil (90% total; 63:37). IR (film) 1323, 1319, 1167, 1133, 1100, 829 cm−1; 1H-NMR (400 MHz,
CDCl3) signals from 2d: δ 7.58 (crude d, J = 8.9 Hz, 2 H), 7.44 (crude d, J = 8.8 Hz, 2 H), 7.01 (crude d,

Molecules 2015, 20
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J = 8.8 Hz, 2 H), 6.92 (crude d, J = 8.8 Hz, 2 H), 3.88 (m, 3 H), 3.86 (s, 3 H); signals from 3d: δ 7.54
(crude d, J = 8.9 Hz, 2 H), 7.30 (crude d, J = 8.9 Hz, 2 H), 6.94–6.85 (m, 4 H), 3.89 (s, 3 H), 3.85 (s, 3 H);
13C-NMR (101 MHz, CDCl3) δ (both 2d and 3d) 163.6, 162.3, 161.8, 138.5. 137.6, 135.3, 135.1, 130.0,
126.3, 120.1, 119.1, 115.0, 114.9, 114.6, 114.5, 113.9, 55.8, 55.7, 55.59, 55.57; HRMS of 2d (ESI-TOF)
m/z [M + H]+ calcd for C14H15O3S2: 295.0457; found: 295.0448; HRMS of 3d (ESI-TOF) m/z [M + H]+
calcd for C14H15O4S2: 311.0406; found: 311.0402.
3.6. S-p-Tolyl 4-Methylbenzenesulfinothioate (2e)
White powder (55%); mp 85–86 °C, lit [56]. mp 87.5 °C; IR (film) 1634, 1424, 1087, 988, 729 cm−1;
1H-NMR (400 MHz, CDCl3) δ 7.57 (d, J = 8.3 Hz, 2 H), 7.44 (d, J = 8.2 Hz, 2 H), 7.30 (d, J = 8.0 Hz,
2 H), 7.19 (d, J = 7.9 Hz, 2 H), 2.42 (s, 3 H), 2.39 (s, 3 H); 13C-NMR (101 MHz, CDCl3) δ 142.1, 141.1,
140.8, 135.4, 130.1, 129.6, 126.3, 124.4, 21.5, 21.4; HRMS (ESI-TOF) m/z [M + H]+ calcd for C14H15OS2:
263.0562; found: 263.0559.
3.7. S-tert-Butyl 2-Methylpropane-2-sulfinothioate (2f)
Golden yellow oil [34,57] (41%); IR (film) 1367, 1167, 1090, 514 cm−1; 1H-NMR (400 MHz, CDCl3)
δ 1.53 (s, 9 H), 1.35 (s, 9 H); 13C-NMR (101 MHz, CDCl3) δ 59.6, 48.8, 32.5, 24.4 ppm; HRMS (EI-TOF)
m/z [M]+ calcd for C8H18OS2: 194.0799; found: 194.0803.
3.8. S-n-Pentyl Pentane-1-sulfinothioate (2g)
Pale yellow oil [22] (54%); IR( film) 1085, 728 cm−1; 1H-NMR (400 MHz, CDCl3) δ 3.16–3.00 (m,
4 H), 1.83–1.75 (m, 4 H), 1.41–1.32 (m, 8 H), 0.91 (t, J = 7.2 Hz, 3 H), 0.88 (t, J = 7.1 Hz, 3 H); 13C-NMR
(101 MHz, CDCl3) δ 56.3, 32.9, 30.7, 30.5, 23.2, 22.3, 22.1, 13.9, 13.8; HRMS (EI-TOF) m/z [M]+ calcd
for C10H22OS2: 222.1112; found: 222.1118.
3.9. S-Isobutyl 2-Methylpropane-1-sulfinothioate (2h)
1
Pale yellow oil [58] (56%); IR (film) 1390, 1085, 1057, 485 cm−1; H-NMR (400 MHz, CDCl3)
δ 3.10 (dd, J = 12.9, 5.8 Hz, 1 H), 3.05 (dd, J = 13.4, 6.7 Hz, 1 H), 2.97 (dd, J = 13.4, 6.7 Hz, 1 H), 2.89
(dd, J = 12.9, 8.5 Hz, 1 H), 2.26–2.20 (m, 1 H), 2.01–1.98 (m, 1 H), 1.07 (d, J = 6.7 Hz, 6 H), 1.01 (d,
J = 6.6 Hz, 3 H), 1.00 (d, J = 6.6 Hz, 3 H); 13C-NMR (101 MHz, CDCl3) δ 65.1, 41.6, 29.7, 24.9, 22.5,
21.64, 21.61, 21.5; HRMS (EI-TOF) m/z [M]+ calcd for C8H18OS2: 194.0799; found: 194.0798.
3.10. S-Allyl Prop-2-ene-1-sulfinothioate allicin (2i)
1
Pale yellow oil [21,22] (31%); IR (film) 1264, 1094, 1067, 808, 739 cm−1; H-NMR (400 MHz,
CDCl3) δ 5.99–5.86 (m, 2 H), 5.46–5.16 (m, 4 H), 3.87–3.69 (m, 4 H); 13C-NMR (101 MHz, CDCl3) δ 133.1,
126.1, 124.2, 119.3, 60.1, 35.2; HRMS (EI-TOF) m/z [M]+ calcd for C6H10OS2: 162.0173; found: 162.0165.

Molecules 2015, 20
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3.11. S-2-Methoxyethyl 2-Methoxyethanesulfinothioate (2j)
Yellow oil [59] (59%); IR (film) 1376, 1119, 1081, 952 cm−1; 1H-NMR (400 MHz, CDCl3) δ 3.89–3.77
13
(m, 2 H), 3.76–3.66 (m, 2 H), 3.40 (s, 3 H), 3.39 (s, 3 H), 3.36–3.26 (m, 4 H); C-NMR (101 MHz,
CDCl3) δ 71.8, 65.4, 59.0, 58.8, 56.4, 32.7; HRMS (ESI-TOF) m/z [M + H]+ calcd for C6H15O3S2:
199.0457; found: 199.0454.
3.12. S-2-Benzoyloxyethyl 2-Benzoylethanesulfinothioate (2k)
White solid (50%); mp 57–58 °C; IR (film) 1729, 1262, 1109, 1067, 1024 cm−1; 1H-NMR (400 MHz,
CDCl3) δ 8.07–8.02 (m, 4 H), 7.61–7.54 (m, 2 H), 7.47–7.40 (m, 4 H), 4.84 (dt, J = 12.3, 5.3 Hz, 1 H),
4.75 (ddd, J = 12.3, 6.9, 5.3 Hz, 1 H), 4.70–4.58 (m, 2 H), 3.65–3.55 (m, 3 H), 3.51 (dt, J = 14.5, 6.5 Hz,
1 H); 13C-NMR (101 MHz, CDCl3) δ 166.1, 166.0, 133.4, 133.2, 129.74, 129.68, 129.5, 129.3, 128.5, 128.4,
63.8, 57.8, 55.2, 31.9; HRMS (ESI-TOF) m/z [M + H]+ calcd for C18H18O5S2: 379.0668; found: 379.0662.
3.13. S-Phenyl 4-Methoxybenzenesulfinothioate (4a) and S-4-Methoxyphenyl Benzenesulfino-thioate (5a)
The product was isolated as a white solid (43% of a ca. 50:50 mixture of the two regioisomers [60,61]);
1
IR (film) 1257, 1171, 1095, 1057, 823 cm−1; H-NMR (400 MHz, CDCl3) signals for both isomers:
δ 7.70–7.30 (m, 7 H), 7.00 (crude d, J = 8.8 Hz, 1H), 6.89 (crude d, J = 8.8 Hz, 1H), 3.87 and 3.84 (s,
3 H for each isomer); 13C-NMR (101 MHz, CDCl3) δ 162.3, 161.7, 137.5, 135.2, 131.3, 130.1, 128.8,
126.1, 124.3, 114.8, 114.4, 55.5, 55.4; HRMS (ESI-TOF) of both regioisomers m/z [M + H]+ calcd for
C13H13O2S2: 265.0351; found: 265.0348.
3.14. S-Phenyl 2-Methylpropane-2-sulfinothioate (4b) [24] and S-tert-Butyl Benzenesulfinothioate (5b)
The product [43] was isolated as a yellow oil (63% of a 85:15 mixture of regioisomers); IR (film)
1371, 1361, 1171, 1167, 1095, 1085, 1057, 1014, 757, 752 cm−1; NMR signals of the major regioisomer
1
4c: H-NMR (400 MHz, CDCl3) δ 7.64 (dd, J = 7.5, 2.1 Hz, 2 H), 7.42–7.37 (m, 3 H), 1.47 (s, 9 H);
13C-NMR (101 MHz, CDCl3) δ 135.0, 129.9, 129.6, 129.4, 60.3, 24.2; NMR signals of the minor
regioisomer 5c: 1H-NMR (400 MHz, CDCl3) δ 7.73 (dd, J = 8.2, 1.5 Hz, 2H), 7.53–7.45 (m, 3 H), 1.65
13
(s, 9 H); C-NMR (101 MHz, CDCl3) δ 32.2; HRMS (ESI-TOF) of both regioisomers: m/z [M + H]+
exact mass calcd for C10H15OS2: 215.0559; found: 215.0556.
3.15. S-Phenyl Hexane-1-sulfinothioate (4c)
Yellow oil (47%); IR (film) 1090, 747 cm−1; 1H-NMR (400 MHz, CDCl3) δ 7.63 (dd, J = 7.9, 1.8 Hz,
2H), 7.47–7.38 (m, 3H), 3.13 (t, J = 7.7 Hz, 2H), 1.86 (ddd, J = 14.7, 7.5, 2.9 Hz, 2H), 1.47 (ddd,
J = 8.9, 4.1, 1.9 Hz, 2H), 1.34 (dq, J = 7.3, 3.7 Hz, 4H), 1.05–0.86 (m, 3H); 13C-NMR (101 MHz, CDCl3)
δ 135.1, 130.1, 129.4, 129.3, 56.1, 31.3, 28.3, 23.4, 22.3, 13.9; HRMS (ESI-TOF) m/z [M + H]+ calcd for
C12H19OS2: 243.0872; found: 243.0871.

Molecules 2015, 20
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3.16. S-Hexyl Benzenesulfinothioate (5d) and S-Hexyl Benzenesulfonothioate (6d)
The product was isolated as a yellow oil (16% of an 1:1 mixture of the thiolsulfinate 5d and
thiolsulfonate 6d); IR (film) 1324, 1133, 1095, 1062, 752 cm−1; 1H-NMR (400 MHz, CDCl3) δ 7.74 (dd,
J = 7.9, 1.7 Hz, 2H), 7.71–7.67 (m, 2H), 7.57–7.43 (m, 6H), 3.29–3.14 (m, 2H), 3.08 (dt, J = 13.4,
7.4 Hz, 2H), 1.97–1.85 (m, 2H), 1.79 (pd, J = 7.4, 2.9 Hz, 2H), 1.40 (dq, J = 12.3, 7.3 Hz, 4H),
1.35–1.26 (m, 10H), 0.89 (td, J = 7.0, 2.6 Hz, 6H); 13C-NMR (101 MHz, CDCl3) δ 136.3, 131.4, 131.3,
129.7, 129.0, 128.0, 126.9, 124.3, 59.5, 33.29, 31.2, 31.1, 30.5, 28.3, 27.6, 23.4, 22.4, 22.2, 13.9, 13.9;
HRMS (ESI-TOF) of 5d: m/z [M + H]+ calcd for C12H19OS2: 243.0872; found: 243.087; HRMS
(ESI-TOF) of 6d: m/z [M + NH4]+ exact mass calcd for C12H22NO2S2: 276.1086; found: 276.10.
3.17. Oxidation of (±)-Lipoic Acid (7)
The oxidation was carried out by the usual procedure. The product was isolated as a clear, colourless
oil in quantitative yield, but in ca. 90% purity, as attempts to remove residual catalyst 1 failed. The 400 MHz
13
1H-NMR spectrum was extremely complex, but C-NMR data (see Supporting Information) matched
those reported by Müller et al. [62] for a similar mixture of all four stereo- and regioisomers. IR (film)
1367, 1195, 1086, 1024 cm−1; HRMS (ESI-TOF) m/z [M + NH4]+ calcd for C8H18NO3S2: 240.0723;
found: 240.0725.
3.18. Oxidation of (L)-N,N′-Dibenzoylcystine Dimethyl Ester (12)
The oxidation was carried out by the usual procedure. The product was a mixture of products, but
appears to consist primarily of the two corresponding thiolsulfinate isomers. The methine signal of the
starting material at 5.1 ppm was replaced by four new signals between 5.0 and 5.3 ppm, while four new
methyl singlets were apparent. The original disulfide methylene signal at 3.4 ppm was absent and a complex
multiplet overlapping with the methyl peaks at 3.7–4.0 ppm was observed instead (see Supplementary
Materials). HRMS (ESI-TOF) m/z [M + H]+ calcd for C22H25N2O7S2: 493.1098; found: 493.1083.
4. Conclusions
In conclusion, cyclic seleninate ester 1 is an effective catalyst for the oxidation of disulfides to
thiolsulfinates with hydrogen peroxide, even in the absence of acidic cocatalysts. In most cases,
overoxidation to thiolsulfonates was largely suppressed by the use of only one equivalent of the peroxide.
Regioselectivity was poor or nonexistent with unsymmetrical diaryl disulfides and oxidation at the
alkyl-substituted sulfur atom was favoured in aryl alkyl derivatives. Product losses were significant during
the isolation and purification of the products. The facile oxidation of cystine analogue 12 under these
conditions indicates that damage to spectator disulfide-containing proteins and peptides is possible
during the use of 1 or its congeners as GPx mimetics or in other biological applications.
Supplementary Materials
Supplementary materials can be accessed at: http://www.mdpi.com/1420-3049/20/06/10748/s1.

Molecules 2015, 20
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Acknowledgments
We thank the Natural Sciences and Engineering Research Council of Canada (NSERC) for financial
support. N.M.R.M. gratefully acknowledges postgraduate scholarships from NSERC and from Alberta
Innovates Technology Futures. C.M. held an undergraduate research internship from Trinity College
(Dublin) and M.H. held an NSERC Undergraduate Summer Research Award.
Author Contributions
The experiments were conceived and designed by N.M.R.M and T.G.B., the experimental work was
carried out by N.M.R.M., C.D. and M.H. The paper was written by N.M.R.M. and T.G.B.
Conflicts of Interest
The authors declare no conflict of interest.
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