Selenium catalyzed oxidation of aldehydes: Green synthesis of carboxylic acids and esters

Article abstract of DOI:10.3390/molecules200610496

The stoichiometric use of hydrogen peroxide in the presence of a selenium-containing catalyst in water is here reported as a new ecofriendly protocol for the synthesis of variously functionalized carboxylic acids and esters. The method affords the desired products in good to excellent yields under very mild conditions starting directly from commercially available aldehydes. Using benzaldehyde as a prototype the gram scale synthesis of benzoic acid is described, in which the aqueous medium and the catalyst could be recycled at last five times while achieving an 87% overall yield.

Full text of DOI:10.3390/molecules200610496

Molecules 2015, 20, 10496-10510; doi:10.3390/molecules200610496
OPEN ACCESS
molecules
ISSN 1420-3049
www.mdpi.com/journal/molecules
Article
Selenium Catalyzed Oxidation of Aldehydes: Green Synthesis of
Carboxylic Acids and Esters
Luca Sancineto 1,†, Caterina Tidei 1,†, Luana Bagnoli 1, Francesca Marini 1, Eder J. Lenardão 2
and Claudio Santi 1,*
1
Group of Catalysis and Organic Green Chemistry, Department of Pharmaceutical Sciences,
University of Perugia, Via del Liceo 1, Perugia 06100, Italy; E-Mails: sancineto.luca@gmail.com (L.S.);
caterinatidei@libero.it (C.T.); luana.bagnoli@unipg.it (L.B.); francesca.marini@unipg.it (F.M.)
2
Laboratório de Síntese Orgânica Limpa (LASOL), Centro de Ciências Químicas,
Farmacêuticas e de Alimentos (CCQFA), Universidade Federal de Pelotas (UFPel), P.O. Box 354,
Pelotas 96010-900, Brazil; E-Mail: lenardao@ufpel.edu.br
†
These authors contributed equally to this work.
* Author to whom correspondence should be addressed; E-Mail: claudio.santi@unipg.it;
Tel.: +39-75-585-5102; Fax: +39-75-585-5116.
Academic Editor: Thomas G. Back
Received: 30 April 2015 / Accepted: 3 June 2015 / Published: 8 June 2015
Abstract: The stoichiometric use of hydrogen peroxide in the presence of a selenium-containing
catalyst in water is here reported as a new ecofriendly protocol for the synthesis of variously
functionalized carboxylic acids and esters. The method affords the desired products in good
to excellent yields under very mild conditions starting directly from commercially available
aldehydes. Using benzaldehyde as a prototype the gram scale synthesis of benzoic acid is
described, in which the aqueous medium and the catalyst could be recycled at last five times
while achieving an 87% overall yield.
Keywords: aldehydes; oxidation; selenium; catalysis; carboxylic acids; esters; hydrogen
peroxide; green chemistry

Molecules 2015, 20
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1. Introduction
Oxidation reactions play an important role in modern organic chemistry and during the recent decades,
several methods have been developed in response to an increasing demand for selective mild and
eco-friendly procedures [1,2]. The carboxylic acid moiety is a common functional group in a number of
organic molecules, including drugs, fine chemicals and industrially interesting compounds. It is usually
synthesized through oxidation reactions starting from reduced precursors such as alcohols [3],
aldehydes [4] or ketones [5]. Among these procedures, the transformation of aldehydes into carboxylic
acids is a very useful chemical reaction and many successful methods have been developed for that
purpose. For a long time, toxic heavy metals and hazardous compounds such as potassium permanganate,
chromates and chlorite have been used in stoichiometric amounts and organic solvents were usually
required. More sustainable and atom efficient procedures have been adopted, especially concerning the
use of hydrogen peroxide as greener oxidant, which however must be employed in the presence of
organic [6], inorganic [7] or transition metal-based catalysts [8–12] in order to allow the oxygen-transfer
reactions to proceed, usually in organic solvents.
During the last ten years, we have investigated in depth the possibility of using water as a reaction
medium for organoselenium and organosulfur chemistry [13–25] focusing a part of our efforts on the use of
organoselenenic acids as catalysts for new bio-inspired and eco-friendly oxidation reactions [17,21,24]. As
in the glutathione peroxidase catalytic cycle, selenium reduces hydrogen peroxide promoting the oxidation
of functionalized organic substrates. This general protocol has been successfully applied to the oxidation
of thiols into the corresponding disulfides and olefins into the corresponding vicinal diols [17,21,24].
In all the cases the reaction was efficiently effected in water suspensions that generally resulted to be
a convenient reaction medium enhancing the efficiency of the catalysts, reducing the undesired
disproportionation of hydrogen peroxide and facilitating the possibility to reuse the catalyst and the medium
several times without any kind of purification and/or activation [24]. Recently, other authors also reported
different applications in which the selenium catalyst is involved in the oxygen transfer oxidation from
hydrogen peroxide to organic substrates demonstrating a current and growing interest in the field [26,27].
In this paper, we describe a new and versatile method to achieve the oxidation of aldehydes using
aqueous hydrogen peroxide in the presence of catalytic amounts of diphenyl diselenide as pre-catalyst
demonstrating the possibility of reusing the aqueous medium at least five times in a gram scale
preparative protocol. As an extension of the reaction, by changing the reaction medium from water to an
alcohol, the direct synthesis of esters from aldehydes can be achieved.
2. Results and Discussion
Preliminary investigations were carried out using, as probe reaction, the oxidation of benzaldehyde (1a)
into the corresponding carboxylic acid 2a using a stoichiometric amount of diluted aqueous hydrogen
peroxide under various reaction conditions (summarized in Table 1). As can be seen in Table 1,
benzaldehyde (1a) is converted into benzoic acid (2a) using one equivalent of 10% (or 20%) aqueous
hydrogen peroxide and 1% (or 2%) of diphenyl diselenide (3) without any organic co-solvent (entries 2–5).
Because all the reactions occurred in non-homogeneous phases, they were effected under vigorous
stirring (800 rpm). Diselenide reacts with hydrogen peroxide affording the oxidized seleninic (5) and

Molecules 2015, 20
10498
perseleninic acid (4) forms that reasonably, are the actual catalyst of the process. Its presence is pivotal
in the oxidation mechanism and only trace amounts of benzoic acid were recovered when the reaction
was effected without diphenyl diselenide (entry 1). The proposed catalytic cycle is depicted in Scheme 1.
Table 1. Oxidation of benzaldehyde (1a) into benzoic acid (2a).
Entry
Catalyst
Oxidant Solvent Time (h) Yield a
1
2
none
10% H2O2
H2O
H2O
H2O
H2O
H2O
H2O
H2O
THF
H2O
6
4
6
6
6
6
6
6
6
trace
56%
61%
85%
>99%
trace
trace
80%
30%
1% (PhSe)2 10% H2O2
1% (PhSe)2 10% H2O2
1% (PhSe)2 20% H2O2
2% (PhSe)2 10% H2O2
2% (PhSe)2 10% H2O2
3
4
5
6 b
7
4% SeO2
2.5% (PhSe)2 10% H2O2
4% HCl 10% H2O2
10% H2O2
8
9
a: All the reactions were carried out at room temperature; b: The reaction was carried out in the presence of a
stoichiometric amount of TEMPO.
Ph SeSe Ph
3
H2O2
H2O
O
O
Ph SeOOH
H2O
R
R
H
1
4
O
O
2
Ph SeOH
H2O2
OH
5
Scheme 1. Diphenyl diselenide-mediated oxidation of aldehydes.
The best conditions, summarized in Table 1, entry 5, afforded the quantitative formation of 2a in six
hours. The yields resulted to be sensitive to and affected by a number of parameters: (a) the reaction time
(entry 2), (b) the amount of the catalyst (entry 3) and (c) the concentration of the oxidant (entry 4). The
reaction did not afford the desired product in the presence of (2,2,6,6-tetramethylpiperidin-1-yl)oxyl
(TEMPO) as radical trapping (entry 6), indicating a reasonable involvement of radical intermediates in
the mechanism. Mlochowsky et al., reported the selenium(IV) oxide-mediated oxidation of aldehydes
using overstoichiometric amounts of H2O2 in refluxing THF [28]; however, we proved that under the
conditions optimized for the benzenseleninic acid, only trace amounts of benzoic acid were observed
(entry 7). Furthermore, this preliminary investigation also demonstrated that the aqueous medium is
superior respect to the organic one (entry 8 vs. entry 5). When THF was used as the solvent in the

Molecules 2015, 20
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presence of benzenseleninic acid (5) as catalyst, according to the conditions previously reported by
Choi et al. [29] lower yields were obtained, despite the use of a higher amount of catalyst. When diphenyl
diselenide was substituted by HCl (4%) a 30% yield of 2a was obtained, evidencing only a slightly
catalytic effect of the acidity in effecting the oxidation.
With the optimized conditions in hands, we investigated the scope of the reaction employing variously
substituted aromatic aldehydes bearing electron withdrawing and donating groups, as well as aliphatic
and conjugated ones. The results are summarized in Table 2.
Table 2. Oxidation of aldehydes to carboxylic acids.
O
O
(PhSe)2 2% (cat)
R
R
H2O2 10% (1 eq)
r.t., water, 6 h
OH
H
1a-l
2a-l
Entry
Substrate
Product
Yield (%) a
O
O
1
1a
1b
2a
2b
>99
OH
O
H
O
OH
OH
2
75
H
OH
O
O
3
4
5
1c
1d
1e
2c
2d
2e
85
80
OH
H
O
O
MeO
O2N
MeO
OH
O
H
O
30, 88 b
O2N
F3C
OH
H
F3C
O
O
H
6
7
8
1f
1g
1h
2f
2g
2h
99
78
80
OH
F
F
F
F
O
O
H
OH
COOH
CHO
CHO
O
COOH
9
1i
1j
2i 20 (E), 65 (Z) c
COOH
O
O
10
2j
>99
H
O
OH
O
11
12
1k
1l
2k
2l
>99 d
>99 d
H
OH
O
H
OH
c
b
1
a: Yields of isolated products; : The reaction was carried out for 24 h; : E/Z ratio = 24:76 by H-NMR of
the crude; d: The reaction was carried out for 3 h.

Molecules 2015, 20
10500
The proposed protocol showed a broad applicability, as both aromatic (compounds 1a–g) and
aliphatic aldehydes (compounds 1h, l) were efficiently converted into the corresponding carboxylic acids
2a–g and 2h, l, respectively, in yields ranging from good to excellent. With the only exception of
p-nitrobenzaldehyde 1e (Table 2, entry 5), that required 24 h of reaction time to afford appreciable
amount of 2e, for the aromatic aldehydes the presence of the functional groups with different electronic
properties did not influence, in general, the outcome of the reaction. Electron withdrawing
group-containing aldehydes 1f and 1g yielded the target acids in 99 and 79% yields, while electron
donating group-containing ones (compounds 1b–d) gave the oxidized products in yields ranging from
75% to 85%. 2,2-Diphenylacetaldehyde (1h) was converted into the target acid 2h in 80% yield indicating
that the steric hindrance has a minor influence on the reaction. Aliphatic non-conjugated aldehydes resulted
reasonably more reactive, affording the carboxylic acids 2k and 2l quantitatively after 3 h instead of six
(Table 2, entries 10 and 11). It is interesting to observe that the oxidation of trans-cinnamaldehyde (1i)
gave the target cinnamic acid 2i in good yield but unexpectedly as a Z/E isomer mixture, in which the less
stable Z-isomer was the major product. On the contrary, the α,β-unsaturated (E)-hex-2-enal (1j) when
subjected to similar conditions, afforded, in excellent yield, only the E-2j isomer. In order to better investigate
this finding, a series of experiments were carried out and the results are summarized in Table 3. The
photoisomerization of E-cinnamic acid is the most commonly used procedure, among the few reported [30],
for the preparation of its Z isomer. To rule out photoactivation or light contribution to the isomerization of
E-cinnamic acid, the oxidation of cinnamaldehyde (1i) was performed under strict dark conditions; however,
the same results were obtained (Table 3, cf. entries 1 and 2).
Table 3. Studies on the isomerization of cinnamic derivatives.
Entry
X
H
% of 3 H2O2
E-Y
Z-Y
1
2 a
3
4 b
5
2
2
0
2
0
2
2
1 eq OH (24%) OH (76%)
1 eq OH (27%) OH (73%)
H
H
1 eq
H (100%)
H
none H (100%)
1 eq OH (100%)
1 eq OH (100%)
OH
OH
H
6
7 c
1 eq
H (100%)
b
a: The reaction was carried out under strict dark conditions; : The reaction was carried out in absence of
hydrogen peroxide; c: The reaction was performed in the presence of a stoichiometric amount of TEMPO.
As expected, both hydrogen peroxide and the catalyst 3 are required to obtain the oxidation/
isomerization (Table 3, entries 3 and 4) and no isomerization was observed starting from trans-cinnamic
acid (Table 3, entries 5 and 6), neither with nor without the catalyst. This indicates that it is reasonable
to assume that the isomerization and the oxidation reactions share the same mechanism. Even if we do
not have at this time a clear explanation for the mechanism, the involvement of radical intermediate has
been proven by performing the oxidation of trans-cinnamaldehyde (1i) in the presence of the radical trap

Molecules 2015, 20
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TEMPO (Table 3, entry 7), whereby only starting material was recovered after six hours, as in the case
of the previously discussed example using benzaldehyde (1a, Table 1, entry 7).
Recently, Pathak et al., reported that depending on the substrate, aldehydes can be converted into the
corresponding esters by using an over-stoichiometric amount of concentrated hydrogen peroxide (50%)
in the presence of alcohols and heating at 70–75 °C for 5–8 h [31]. In order to evaluate the ability of
diphenyl diselenide (3) to catalyze this reaction, we subjected the aldehyde 1a to the reaction with 2%
of 3 at 50 °C in the presence of a stoichiometric amount of both hydrogen peroxide (30%) and methanol.
After only two hours the reaction was complete evidencing a positive effect of the catalyst on allowing
the conversion to proceed under considerably milder conditions and in shorter reaction times (90% yield
in 2 h at 50 °C vs. 75% yield in 5 h at 75 °C [29]; Table 4, entry 1).
Table 4. Esterification of aldehydes.
O
O
H
O
(PhSe)2 2% (cat)
R
R OH
7c,d
R O
8d
R
OR'
H2O2 30% (1 eq)
R'OH
H
6a, c-j
1a, c-f
Yield (%) a
7
Entry
R
R′
T °C Conv (%)
6
8
1
2
1a
1c
–CH3
–CH3
50
50
>99
>99
90 (6a)
-
-
75 (6c) 15 (7c)
10 (6d) 35 (7d)
-
-
50
0
44
97
MeO
O2N
3
4
1d
1e
–CH3
–CH3
-
15 (7d) 80 (8d)
50
>99
95 (6e)
-
-
F3C
5
1f
–CH3
50
>99
96 (6f)
-
-
6
7
8
9
1a
1a
–C2H5
–C3H7
50
50
50
50
92
85
81
95
87 (6g)
80 (6h)
77 (6i)
70 (6j)
-
-
-
-
-
-
-
-
1a –iC3H7
1a –(CH2)6-
a Yields of isolated products.
With the optimized conditions of the esterification in hands, we explored the scope of the reaction
evaluating a panel of aldehydes and different alcohols. The results are collected in Table 4. The oxidation
occurred in excellent yields for benzaldehyde (1a) and for aldehydes bearing electron withdrawing
groups (Table 4, entries 1, 4 and 5), affording the corresponding methyl esters 6a, 6e and 6f (in up to 95%
yields). In the cases of p-methylbenzaldehyde (1c, entry 2) and p-methoxybenzaldehyde (1d, entry 3),
besides the target methyl esters 6c and 6d, we observed the formation of the corresponding p-cresol (7c)

Molecules 2015, 20
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and p-methoxyphenol (7d), presumably as a result of a competitive Dakin-like reaction facilitated by the
electron-donating character of the substituent at the para-position respect to the carbonyl group of the
aldehyde. The nature of the competitive mechanism is confirmed by the isolation of the formyl derivative
8d (80% yield) when the oxidation of 1d was effected at 0 °C (Table 4, entry 3).
Beside methanol, linear, branched and cyclic aliphatic alcohols were reacted with 1a yielding the
corresponding esters 6g–j in good to excellent isolated yields, showing only a slight detrimental effect
of the steric hindrance in the secondary alcohols respect to the primary ones (Table 4, entries 8 and 9 vs.
entries 1, 6 and 7).
In order to confirm the actual involvement of the in situ-formed benzenselenenic acid a representative
number of reactions were repeated using 4 mol % of preformed 5, observing no appreciable difference
in yields and reaction times either for the synthesis of carboxylic acids or esters. In addition, the mixture
resulting from the treatment of diphenyl diselenide with hydrogen peroxide in a molar ratio of 1:5 in
77
water has been analyzed by Se-NMR using for the NMR lock and shimming procedures a sealed
capillary tube containing DMSO-d6. The spectra evidenced three peaks at 1024, 1174 and 1293 ppm,
respectively. The chemical shift of 1174 ppm can be unambiguously assigned to PhSeO2H by comparison
with the spectra obtained from the commercially available original sample; beside that, it can be
supposed the presence of a less oxidized specie, PhSeOH (1024 ppm) and an over-oxidized one, like
PhSeO3H (1293 ppm) that confirm the proposed mechanism depicted in Scheme 1.
Considering the growing interest in protocols and procedures designed to minimize waste production,
we investigated the recyclability of the aqueous medium containing the water-soluble catalyst 5,
evaluating the efficiency in terms of conversion and overall yield in the oxidation of 1a for a number of
five subsequent reactions affording a gram scale synthesis of 2a.
As reported in Figure 1, after 6 h benzoic acid precipitated in the water and it was separated from the
reaction mixture simply by filtration. The conversion is quantitative after the first three cycles (see Figure 2,
spectra 1–3) and only in the 4th and 5th cycles a minimal residue of unreacted benzaldehyde (1a) was
observed. (Figure 2, spectra 4 and 5).
Figure 1. Recyclability of the aqueous medium and the catalyst in the synthesis of benzoic
acid (2a).

Molecules 2015, 20
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1
Figure 2. H-NMR (200 MHz, CDCl3 sol.) of the crudes obtained in the first 5 cycles
of recycling.
The purity of the benzoic acid was also checked by ICP-MS spectrometry, that evidenced the presence
of traces of selenium (<0.07%) that were undetectable after one recrystallization. This evidence also
explains the reduced efficiency of the catalytic system after 3 cycles. The protocol probably suffers of
the combination of two factors: a small loss of catalyst and a progressive dilution due to the addition of
new oxidant (30% hydrogen peroxide) at each cycle.
Worth summarizing in terms of the greenness of the proposed protocol is the fact that a gram scale
synthesis and purification of benzoic acid starting from the corresponding aldehyde can be performed
avoiding the use of organic solvents, using a stoichiometric amount of hydrogen peroxide, recycling and
reusing at least five times the reaction medium containing the catalyst (overall yield of 87%).
3. Experimental Section
3.1. General Information
Reactions were conducted in a round bottom flask and were stirred with Teflon-coated magnetic
stirring bars at 800 rpm. Solvents and reagents were used as received unless otherwise noted. Analytical
thin-layer chromatography (TLC) was performed on silica gel 60 F254 precoated aluminum foil sheets
and visualized by UV irradiation or by KMnO4 staining. Silica gel Kieselgel 60 (70–230 mesh, Merck,
Darmstadt, Germany) was used for column chromatography. NMR experiments were conducted at 25 °C
with a Bruker DPX 200 spectrometer (Bruker, Milan, Italy) operating at 200 MHz for 1H, 50.31 MHz

Molecules 2015, 20
10504
for 13C, and 94.07 MHz for 19F experiments or with a Bruker DRX spectrometer operating at 400 MHz
for 1H, 100.62 MHz for 13C and 76 MHz for 77Se experiments. 1H and 13C chemical shifts (δ) are reported
in parts per million (ppm), relative to TMS (δ = 0.0 ppm) and the residual solvent peak of CDCl3
1
(δ = 7.26 and 77.00 ppm in H and 13C-NMR, respectively). Data are reported as chemical shift
(multiplicity, coupling constants where applicable, number of hydrogen atoms, and assignment where
possible). Abbreviations are: s (singlet), d (doublet), t (triplet), q (quartet), dd (doublet of doublet),
dt (doublet of triplet), tt (triplet of triplet), m (multiplet), br. s (broad signal). Coupling constants (J) are
quoted in Hertz (Hz) to the nearest 0.1 Hz. Inductively coupled plasma mass spectrometry (ICP MS)
analysis was performed with a Varian 700-ES series instrument inductively coupled plasma-optical
emission spectrometer (Varian, Les Ulis Cedex, France).
3.2. General Procedure for the Synthesis of Carboxylic Acids 2
Diphenyl diselenide (3, 0.006 g; 0.02 mmol) was treated with H2O2 (30%·w/w, 0.1 mL, 1 mmol) and
water (0.2 mL) and stirred at room temperature at 800 rpm until the discoloration of the reaction mixture;
then, the aldehyde 1 (1 mmol) was added. After 6 h, the aqueous mixture was extracted three times with
EtOAc (3 × 20 mL). The collected organic layers were dried over Na2SO4 and the solvent evaporated
under reduced pressure.
Benzoic acid (2a). White solid, 99% yield, m.p. 122 °C [32], 1H-NMR (CDCl3) δ: 7.49 (dd, 2H, J = 7.6
and 6.8 Hz), 7.63 (t, 1H, J = 6.8 Hz), 8.13 (d, 2H, J = 7.6 Hz), 11.88 (brs, 1H); 13C-NMR (100 MHz,
CDCl3) δ: 128.5, 129.3, 130.2, 133.8, 172.5.
1
2-Hydroxybenzoic acid (2b). White solid, 73% yield, m.p. 160 °C [33], H-NMR (DMSO-d6) δ:
6.96–6.90 (m, 2H), 7.53–7.49 (m, 1H), 7.80 (dd, J = 1.2, 5.7 Hz, 1H), 11.36 (brs, 1H), 13.87 (brs, 1H);
13C-NMR (DMSO-d6) δ: 113.5, 117.6, 119.7, 130.8, 136.1, 161.7, 172.4.
1
4-Methylbenzoic acid (2c). Yellow solid, 85% yield, m.p. 179 °C [34], H-NMR (CDCl3) δ: 2.43
13
(s, 3H), 7.26 (d, 2H, J = 8.3 Hz), 7.99 (d, 2H, J = 8.3 Hz); C-NMR (CDCl3) δ: 21.8, 126.5, 129.1,
130.2, 144.5, 172.3.
4-Methoxybenzoic acid (2d). Colorless solid, 80% yield, m.p. 183 °C [35], 1H-NMR (DMSO-d6) δ: 3.82
13
(s, 3H), 7.00 (d, 2H, J = 8.8 Hz), 7.89 (d, 2H, J = 8.8 Hz), 12.61 (brs, 1H); C-NMR (DMSO-d6) δ:
55.4, 113.8, 123.0, 131.3, 162.8, 167.0.
4-Nitrobenzoic acid (2e). Colorless solid, 88% yield, m.p. 243 °C [36], 1H-NMR (DMSO-d6) δ: 8.10 (d,
2H, J = 8.3 Hz), 8.26 (d, 2H, J = 8.3 Hz), 13.61 (brs, 1H); 13C-NMR (DMSO-d6) δ 123.9, 130.9, 136.6,
150.2, 166.0.
3-(Trifluoromethyl)benzoic acid (2f). Colorless solid, 99% yield, m.p. 105 °C [37], 1H-NMR (DMSO-d6) δ:
7.76 (t, 1H, J = 8.0 Hz), 8.00 (d, 1H, J = 8.0 Hz), 8.17 (s, 1H), 8.22 (d, 1H, J = 8.0 Hz), 13.52 (br s, 1H);
13C-NMR (DMSO-d6) δ: 123.8 (q, JC–F = 271 Hz), 125.5 (q, JC–F = 4 Hz), 129.4 (q, JC–F = 4 Hz), 129.5
(q, JC–F = 32 Hz), 130.2, 131.9, 133.3, 166.1. 19F-NMR (DMSO-d6) 61.5 (s).

Molecules 2015, 20
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3,5-Difluorobenzoic acid (2g). Colorless solid, 78% yield, m.p. 121 °C [38], 1H-NMR (CDCl3) δ: 7.20
(tt, 1H, J = 3.0 and 9 Hz), 7.50–7.60 (m, 2H); 13C-NMR (CDCl3) δ: 109.4 (t, JC–F = 25 Hz), 113.2 (m), 132.3
(t, JC–F = 9 Hz), 162.8 (dd, JC–F = 12 and 249 Hz), 170 (t, JC–F = 3 Hz); 19F-NMR (DMSO-d6) 108 (s).
2,2-Diphenylacetic acid (2h) 80% yield, white solid, m.p. 143 °C [39], 1H-NMR (DMSO-d6) δ: 5.00 (s,
13
1H), 7.20–7.30 (m, 2H), 7.30–7.35 (m, 8H), 12.70 (br s, 1H), C-NMR (DMSO-d6) δ: 56.3, 126.8,
128.4, 128.5, 139.5, 173.4.
Cinnamic acid (2i) obtained as Z/E mixture (76:24) in 85% yield. Major isomer (Z-2i) 1H-NMR (CDCl3)
δ: 6.50 (d, 1H, J = 12.7), 7.25–7.35 (m, 3H), 7.50–7.55 (m, 2H), 7.85 (d, 1H, J = 12.7); 13C-NMR (CDCl3)
δ: 118.7, 128.1, 129.4, 129.9, 134.4, 145.8, 171.3.
(E)-Hex-2-enoic acid (2j). Oil [40], 99% yield, 1H-NMR (CDCl3) δ: 0.95 (t, 3H, J = 7.4 Hz), 1.45–1.55
(m, 2H), 2.20–2.25 (m, 2H), 5.80 (d, 1H, J = 15.6 Hz), 7.05 (dt, 1H, J = 15.9 and 6.9 Hz,); 13C-NMR
(CDCl3) δ: 13.8, 21.3, 34.4, 120.8, 152.4, 171.9.
Octanoic acid (2k). Oil [41], 99% yield, 1H-NMR (CDCl3) δ: 0.90 (t, 3 H, J = 5.0 Hz), 1.30–1.35 (m,
13
8H), 1.60 (q, 2 H, J = 5.0 Hz), 2.35 (t, 2 H, J = 5.0 Hz), 11.10 (br s, 1H); C-NMR (CDCl3) δ: 14.1,
22.7, 24.8, 29.0, 29.1, 31.7, 34.2, 180.6.
Hexenoic acid (2l). Oil [42], 99% yield, 1H-NMR (CDCl3) δ: 0.91 (m, 3H), 1.30–1.35 (m, 4H), 1.65 (m,
2H), 2.35 (t, J = 7.5 Hz, 2H); 13C-NMR (CDCl3) δ: 24.4, 22.3, 13.8, 31.2, 34.0, 180.2
3.3. General Procedure for the Synthesis of Esters 6
Diphenyl diselenide (3, 0.006 g; 0.02 mmol) was treated with H2O2 (30%·w/w, 0.15 mL, 1.5 mmol)
and stirred at room temperature until the discoloration of the reaction mixture. Then, the aldehyde 1
(1 mmol) and the appropriate alcohol (2.5 mmol) were added. The reaction mixture was stirred at
50 °C for 2 h and extracted three times with EtOAc (3 × 20 mL). The collected organic layers were dried
over Na2SO4 and the solvent evaporated under reduced pressure.
Methyl benzoate (6a). Colorless oil [31], 90% yield, 1H-NMR (CDCl3) δ: 3.88 (s, 3H,), 7.59–7.35 (m, 3H),
8.12–8.04 (m, 2H); 13C-NMR (CDCl3) δ: 52.4, 128.1, 129.3, 130.3, 132.6, 166.4.
Methyl 4-methyl-1-benzoate (6c). White solid, 75% yield, m.p. 34 °C [31], 1H-NMR (CDCl3) δ: 2.41(s,
13
3H), 3.90(s, 3H), 7.24(d, J = 8.0 Hz, 2H), 7.93(d, J = 8.0 Hz, 2H); C-NMR (CDCl3) δ: 21.5, 51.8,
127.4, 129.0, 129.5 143.4, 167.0.
Methyl 4-methoxy-1-benzoate (6d). Colorless oil [43], 10% yield, 1H-NMR (CDCl3) δ: 3.84 (s, 3H), 3.88
(s, 3H), 6.90 (d, 2H, J = 8.8 Hz), 7.98 (d, J = 8.8 Hz, 2H); 13C-NMR (CDCl3) δ: 51.8, 55.3, 113.5, 122.5,
131.5, 163.3, 166.9.
1
Methyl 4-nitro-1-benzoate (6e). White solid, 95% yield, m.p 90 °C [31], H-NMR (CDCl3) δ: 3.91
(s, 3H), 8.18 (d, J = 6.0 Hz, 2 H), 8.21 (d, J = 6.0 Hz, 2 H). 13C-NMR (CDCl3) δ: 52.8, 122.5, 130.7, 145.0,
150.5, 165.1.

Molecules 2015, 20
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1
Methyl 3-(trifluoromethyl) benzoate (6f). Colorless oil [44], 96% yield, H-NMR (CDCl3) δ: 3.95 (s,
3H), 7.55 (dd, J 7.8 and 7.8 Hz, 1H), 7.80 (d, J = 7.8 Hz, 1H), 8.22 (d, J = 7.8 Hz, 1H), 8.30 (s, 1H);
13C-NMR (CDCl3) δ: 52.7, 126.7, 129.3, 129.6, 131.2, 133.2, 133.6, 166.0.
Ethyl benzoate (6g). Colorless oil [45], 87% yield, 1H-NMR (CDCl3) δ: 1.38 (t, J = 7.2 Hz, 3H), 4.39
13
(q, J = 7.2 Hz, 2H), 7.40–7.45 (m, 2H), 7.55 (t, J = 7.4 Hz, 1H), 8.04 (d, J = 7.2 Hz, 2H); C-NMR
(CDCl3) δ: 17.1, 60.3, 128.4, 130.3, 131.9, 133.6, 168.7.
1
Propyl benzoate (6h). Colorless oil [45], 80% yield, H-NMR (CDCl3) δ: 1.02 (t, J = 7.2 Hz, 3H),
1.75–1.80 (m, 2H), 4.25 (t, J = 6.8 Hz, 2H), 7.40–4.45 (m, 2H), 7.50–7.55 (m, 1H), 8.00–8.05 (m, 2H);
13C-NMR (CDCl3) δ: 10.5, 22.1, 66.5, 128.3, 129.5, 130.5, 132.8, 166.6.
Isopropyl benzoate (6i). Colorless oil [46], 77% yield, 1H-NMR (CDCl3) δ: 1.36 (s, 3H), 1.38 (s, 3H),
5.26 (m, 1H), 7.41–8.06 (m, 5H); 13C-NMR (CDCl3) δ: 22.2, 68.6, 128.5, 129.7, 131.1, 132.9, 166.3.
1
Cyclohexyl benzoate (6j). Colorless oil [47], 70% yield, H-NMR (CDCl3) δ: 1.35-2.00 (m, 10H),
5.00–5.05 (m, 1H), 7.40–7.55 (m, 3H), 8.10–8.15 (m, 2H); 13C-NMR (CDCl3) δ: 23.6, 25.4, 31.5, 72.9,
128.2, 129.4, 130.9, 132.6, 165.9.
1
4-Methyl phenol (7c). Yellowish solid,15% yield, m.p. 35 °C [48], H-NMR (CDCl3) δ: 2.27 (s, 3H).
5.56 (s, 1H), 6.74 (d, J = 8.4 Hz, 2H), 7.03 (d, J = 8.4 Hz, 2H); 13C-NMR (CDCl3) δ: 20.6, 115.3, 130.1,
130.3, 153.4.
4-Metoxy phenol (7d). Yellow solid, 35% yield, m.p. 55 °C [48], 1H-NMR (CDCl3) δ: 3.75 (s, 3H), 5.31
(s, 1H), 6.72–6.82 (m, 4H); 13C-NMR (CDCl3) δ: 56.0, 114.9, 116.1, 149.7, 153.5.
4-Methoxyphenyl formate (8d). It was obtained in 60% yield as a colorless solid after performing the
reaction at 0 °C using an ice bath. m.p.: 30 °C [49], 1H-NMR (CDCl3) δ: 3.81 (s, 3H), 6.91 (d, J = 8.8 Hz,
2H), 7.05 (d, J = 8.8 Hz, 2H), 8.30 (s, 1H); 13C-NMR (CDCl3) δ: 55.5, 114.8, 121.5, 143.6, 156.4, 159.7.
4. Conclusions
In conclusion, a new protocol was developed to prepare carboxylic acids directly from aldehydes
selectively and in excellent yields using diluted hydrogen peroxide, diphenyl diselenide as the catalyst
and water as the solvent. Even if the oxidation of aldehydes has been widely explored in the past,
nowadays a number of very recent publications demonstrates that there is still an interest on this topic,
mainly focused on the development of more sustainable and green protocols [50,51] as well as on the
elucidation of the actual mechanism [52]. By changing the solvent for an alcohol instead water, it was
possible to prepare esters in very good yields and high selectivity directly from aldehydes. The method is
suitable for aromatic and aliphatic aldehydes and was successfully used in a gram scale preparation of
benzoic acid from benzaldehyde in which the solvent/catalyst system was reused with good results for five
successive reactions and no organic solvent was used in any step of the procedure, as benzoic acid was
recovered from the reaction mixture just by simple filtration. It is reasonable to envision that this latter
protocol can be used in all the cases in which the carboxylic acid can be directly crystalized in the reaction

Molecules 2015, 20
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medium (e.g., starting from aromatic aldehydes) especially in the cases in which the oxidation proceeded in
almost quantitative yields.
Acknowledgments
Financial support from the Dipartimento di Scienze Farmaceutiche, Università degli Studi di Perugia
“Fondo per il sostegno della Ricerca di Base 2015” and Fondazione Cassa di Risparmio di Perugia
(2014.01000.021) are gratefully acknowledged. The authors also thank Regione Umbria: project “POR
Umbria 2007–2013” for the fellowship to Luca Sancineto, Valeria Saccomandi for the help in conducting
some experiments, and Morena Nocchetti for the ICP-MS analysis. Eder J. Lenardão is Bolsista CAPES—
Processo No. BEX 6391/14-1. This research was undertaken as part of the scientific activity of the
international multidisciplinary “SeS Redox and Catalysis” network.
Author Contributions
Claudio Santi, Eder J. Lenardao, Francesca Marini, Luana Bagnoli designed the research; Claudio Santi,
Francesca Marini supervised the work; Caterina Tidei, and Luca Sancineto performed research and
analyzed the data; Claudio Santi and Eder J. Lenardao wrote the paper. All authors read and approved
the final manuscript.
Conflicts of Interest
The authors declare no conflict of interest.
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Sample Availability: Samples of the compounds are available from the authors.
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