Electrocarboxylation of halobenzonitriles: An environmentally friendly synthesis of phthalate derivatives

Article abstract of DOI:10.1016/j.electacta.2019.134576

This manuscript presents an efficient approach for producing high valuable compounds using CO₂ as building block. The methodology employed is based on electrochemical techniques, which allow performing eco-friendly chemistry solutions and maintaining the aim of offering a potential long-term strategy for reducing the CO₂ emissions in the atmosphere, while obtaining useful compounds, such as aromatic acids and phthalate derivatives. This work describes the electrochemical reduction behavior of 4-halobenzonitrile compounds using Glassy Carbon and Silver as cathodes under inert and carbon dioxide atmosphere. Controlled potential electrolysis of 4-halobenzonitriles under CO₂ allows obtaining, in very good yields, the corresponding mono- and di-carboxylated organic compounds in CO₂-saturated solutions of dimethylformamide containing 0.1 M of tetrabutylammonium tetrafluoroborate. Electro-catalytic effects are seen when Ag is used a cathode, which give very high yields, especially as regards di-carboxylated products. The methodology offers a new “green” route for the synthesis of different phthalate derivatives, which can be potentially used for making plastic polymers in a more environmentally friendly way.

Full text of DOI:10.1016/j.electacta.2019.134576

Accepted Manuscript
Electrocarboxylation of halobenzonitriles: An environmentally friendly synthesis of
phthalate derivatives
Irene Reche, Silvia Mena, Iluminada Gallardo, Gonzalo Guirado
PII:
S0013-4686(19)31421-5
10.1016/j.electacta.2019.134576
134576
DOI:
Article Number:
Reference:
EA 134576
To appear in:
Electrochimica Acta
Received Date:
Accepted Date:
21 May 2019
22 July 2019
Please cite this article as: Irene Reche, Silvia Mena, Iluminada Gallardo, Gonzalo Guirado,
Electrocarboxylation of halobenzonitriles: An environmentally friendly synthesis of phthalate
derivatives, Electrochimica Acta (2019), doi: 10.1016/j.electacta.2019.134576
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ACCEPTED MANUSCRIPT
Electrocarboxylation of halobenzonitriles: An
environmentally friendly synthesis of phthalate derivatives.
Irene Reche, Silvia Mena, Iluminada Gallardo, Gonzalo Guirado*
Departament de Química, Universitat Autònoma de Barcelona, Campus UAB, 08193-
Bellaterra, Barcelona, Spain
*gonzalo.guirado@uab.cat; Tel.: +00 34 93 581 4882
Abstract
This manuscript presents an efficient approach for producing high valuable compounds
using CO2 as building block. The methodology employed is based on electrochemical
techniques, which allow performing eco-friendly chemistry solutions and maintaining the
aim of offering a potential long-term strategy for reducing the CO2 emissions in the
atmosphere, while obtaining useful compounds, such as aromatic acids and phthalate
derivatives. This work describes the electrochemical reduction behavior of 4-
halobenzonitrile compounds using Glassy Carbon and Silver as cathodes under inert and
carbon dioxide atmosphere. Controlled potential electrolysis of 4-halobenzonitriles under
CO2 allows obtaining, in very good yields, the corresponding mono- and di-carboxylated
organic compounds in CO2-saturated solutions of dimethylformamide containing 0.1 M
of tetrabutylammonium tetrafluoroborate. Electro-catalytic effects are seen when Ag is
used a cathode, which give very high yields, especially as regards di-carboxylated
products. The methodology offers a new “green” route for the synthesis of different
phthalate derivatives, which can be potentially used for making plastic polymers in a more
environmentally friendly way.
Keywords: Carboxylation • Electrochemistry • Electrolysis • 4-halobenzonitrile •
Cyclic voltammetry
TOC:
CO2 + e
Ag or C
RX
OOC
COO
ROOC
COOR
NC
X
phthalate derivatives
Highlights:
Disclosure of electrochemical reduction mechanism of halobenzonitrile compounds using
Glassy Carbon and Silver cathodes under inert and CO2 atmosphere.
Electrocarboxylation of halobenzonitriles for producing high valuable compounds using
CO2 as building block.
Tuning electrochemical reactivity of CO2 using Silver cathodes.
New “green” route for the synthesis of different phthalate derivatives.
1

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1.
Introduction
The increasing concentration of CO2 in the atmosphere is a fact that threatens the
economy and the sustainability of the planet. In spite of the precautions and actions that
have been taken for reducing the emissions arising from fuel consumption processes,
more efficient and sustainable ways to ameliorate the climate change problem still need
to be investigated, not only for improving the quality life, but also because non-renewable
sources are, indeed, limited and still in high demand world-wide[1–3]. Possible alternatives
for reducing CO2 emissions are using low carbon-rich forms as fuel, and capturing and
storing CO2, and for what seems to be the most practical approach is to use it as a carbon
building block for producing high valuable compounds[4,5]. In this sense, one of the
problems associated with the chemical utilization of CO2 is related to its inherent
thermodynamic stability and kinetic inertness, hence, direct or indirect activation of the
functionalization process is required. On the other hand, the use of CO2 as C1 feedstock
has some advantages as an abundant, non-toxic, non-flammable, and a quite easily
available resource[6].
Transformation of CO2 studies to either convert the CO2 into more reduced forms or use
it as a carboxylating agent in combination with different molecules, have been widely
described in the literature. There are also a few examples reported where the CO2 acts as
a C1 building block, including: methane[7–9], methanol[10,11], ethylene glycol[12,13]
polyurethanes, urea[14] cyclic carbonates (propylene carbonate)[15–18], carbamates[19–21]
,
,
and ibuprofen[22–25]. Nevertheless, these transformations are normally associated with
high pressures and/or temperatures, low efficiency processes, formation of byproducts,
multiple synthetic steps, etc. In the present work, we have developed an electrochemical
method in order to overcome those disadvantages, that is, a more environmentally
respectful strategy for the utilization of CO2 to produce high value-added products, and
at the same time, a potential way to confront the climatic change at a long-term
perspective. In fact, electrochemistry can be seen as a branch of Green Chemistry as it is
in accordance with a set of principles for reducing the use of hazardous substances in the
design of processes and manufacture of chemical products[26]. The benefits of using
electrochemical experiments include mild chemical and process conditions, easy control,
high process selectivity, novel chemistry available, safer operation, electrons as
inexpensive reagents in comparison with the typical redox agents. In addition, the
electrons are capable of acting as heterogeneous catalysts able to be easily isolated from
the products.
Classical electrochemistry of CO2 consists of the electro-reduction of the molecule in the
presence of an organic aprotic or protic solvent and supporting electrolyte. Apart from
the solvent, the nature of the working electrode (WE), the temperature, and the
concentration are other important factors. These can be more or less adjustable, not only
for tuning the reduction potential of CO2 but also to modulate the subsequent formation
of different products (such us oxalate, carbonate, carbon monoxide, etc.)[27,28]
.
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The electrochemical promoted approaches for achieving carboxylated organic valuable
products can mainly be tackled in strategies (Scheme 1). In the first approach, the
·-
electrochemical generation of the CO2 radical anion (CO2 ) requires a fairly negative
potential (Scheme 1, route 1)[29], making this option costly in terms of energy consumed.
In the second approach (Scheme 1, route 2), the electrochemical reduction takes places in
the organic molecule (for instance, an organic halide RX); which is a more easily
reducible compound than CO2. After being reduced (RX·-), cleaves into the anion halide
(X-) and the organic radical (R·) (step 1). The electro-generated radical can be further
reduced to form the corresponding organic anion (R-) (step 2). If this organic anion is
stable enough in the electrolytic media, it will nucleophilically attack the CO2 dissolved
in the solution, and therefore the CO2 molecule would be added, leading to a carboxylate
-
derivative (RCO2 ) (step 3).
1e
Step 1
Step 2
CO2
+
CO2
CO2
RCO2 + X
R + CO2
RX
Route 1
RCO2
RCO2
Step 3a
Step 3b
1e
RCO2
1e
[RX]
1e
Step 1
Step 2
Step 3
RX
R + X
Route 2
R
R
R
RCO2
CO2
+
Scheme 1. Electrochemical strategies used for the synthesis of carboxylated products
There are some examples in the literature following the second carboxylation strategy.
Gennaro et.al have reported electro-reduction processes that lead to carboxylation of
different organic[30–32], and non-organic compounds in various solvents and/or working
electrodes[33–36]. In one of these studies, they showed that exhaustively controlled
potential electrolysis (at -1.5 V vs SCE) of electrochemical reduction of benzyl halides in
acetonitrile, using silver as working electrode, under of CO2 atmosphere at 25ºC, yielded
up to c.a. 45% of phenylacetic acid[36] Zhang et al also investigated the electro-catalytic
carboxylation of bromobenzene derivative using a silver cathode in the presence of CO2
(at 0ºC) achieving a 78% yield, Scheme 2[37]
.
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R: H (78 %)
COOH
Ag + e
R
Br
CO2
DMF
R: COOCH3 (60 %)
H3COOC
COOH
Scheme 2. Electrolysis of aryl bromides in the presence of CO2 in DMF using Ag as
working electrode[37].
According to the above mentioned electrocarboxylation strategies and previous studies
published[36,37], the use of halobenzonitriles seems to be an ideal starting material for
obtaining carboxylated products. The presence of the CN group in the molecule would
help to reduce the energy required for the reduction process, since it would act as an
electrophore. Thus, the carbon-halogen bond cleavage reaction will occur at less negative
potential. Note, that the nature of the electrode would also modify the reduction potential
value, so the use of Ag as cathode due to its electrocatalytic properties would also help to
decrease the reduction potential value.
Thus, the aim of this study is to valorize CO2 using halobenzonitriles as a starting material
for obtaining carboxylated derivatives using a “green” electrochemical route. The
electrocatalytic properties of using Ag instead of C as cathode in the electrochemical
reduction mechanism of 4-halobenzonitriles will also be analyzed. It is important to note
that the synthesis of dicarboxylated compounds using this strategy would potentially open
a very versatile and sustainable approach for making plastic polymers in a foreseeable
future (Scheme 3).
CO2 + e
Ag or C
RX
OOC
COO
ROOC
COOR
NC
Br
phthalate derivatives
Scheme 3. Electrochemical strategy used in this work for synthesizing phthalate
derivatives
2.
2.1. Reagents
All the commercially available reagents were purchased with the maximum purity
Experimental section
and used without previous purification. Solvents: Chloroform, SDS, Carlo Erba, for
HPLC stabilized with ethanol, ≥ 99.9%. Deuterated chloroform (CDCl3), Euriso-top,
99.8%. Dichloromethane, Carlo Erba, for HPLC, stabilized with ethanol, ≥ 99.9%.
Diethyl ether, SDS, Carlo Erba, purity ≥ 99.0% (GC). N, N’-dimethylformamide (DMF),
SDS, for synthesis. Toluene, SDS, pure for synthesis. Supporting electrolytes:
tetrabutylammonium tetrafluoroborate (TBABF4), Sigma-Aldrich, 99%. Electro-active
substances: 4-Bromobenzonitrile, Sigma-Aldrich, 99%. 4-Cyanobenzoate methyl ester,
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Sigma-Aldrich, 99%. 4-Chlorobenzonitrile, Sigma-Aldrich, 99%. 4-Fluorobenzonitrile,
Sigma-Aldrich, 99%. 4-Iodobenzonitrile, Sigma-Aldrich, 99%. 9-Fluorenone puriss.,
Fluka, ≥ 99%. Benzonitrile, Sigma-Aldrich, 99%. Carbon Dioxide, Linde, purity ≥
99.9993%. Dimethyl terephthalate, Fluka, ≥ 99.0% (GC). Other reagents: 2-
Bromoethylbenzene, Sigma-Aldrich, 98%. Hydrochloric acid (HCl), Sigma-Aldrich,
reactive 37%. Bromoethane (BrEt), Sigma-Aldrich, 98%. Methyl iodide (CH3I), Sigma-
Aldrich, 2.0 M solution in tert-butylmethyl ether, and anhydrous sodium sulfate, Na2SO4,
Sigma-Aldrich, 99.0%.
2.2. Methodology
2.2.1. Cyclic voltammetry
Firstly, a solution of the electro-active substance is prepared with a known
concentration (between 10 and 16 mM) containing 0.10 M of a supporting electrolyte
(tetrabutylammonium tetrafluoroborate, TBABF4) in 10 ml of dimethylformamide
(DMF). Once the solution is introduced into the cell, it is deoxygenated (or CO2 removed)
through an influx of an inert gas, Ar or N2, a process that is repeated between
measurements when the cell is opened to clean the working electrode. The working
electrode is a vitreous carbon disk of 1mm diameter. It is polished using a 1 mm diamond
paste before each new measurement with a mixture of lubricant and ethanol. The
electrochemical used for the set-up of the three-electrode system is conical. The counter
electrode is a Pt disk of < 1 mm diameter. All the potentials are reported versus an aqueous
saturated calomel electrode (SCE) isolated from the working electrode compartment by
a salt bridge. The salt solution of the reference calomel electrode is separated from the
electrochemical solution by a salt-bridge ended with a frit, which is made of a ceramic
material, allowing ionic conduction between the two solutions and avoiding appreciable
contamination. Ideally, the electrolyte solution present in the bridge is the same as the
one used for the electrochemical solution, to minimize junction potentials. The cyclic
voltammetry studies are performed for each concentration of electro-active substance at
different scan rates between 0.1 and 1.0 V·s-1. Overall, the I-E curves obtained lead to the
determination of the electrochemical (Ep, ΔEp, Ip/(c·(v)1/2)), and thermodynamic
parameters (Eº) of the target molecule.
2.2.2. Controlled Potential Electrolysis
For preparing the solutions to be electrolyzed, a known amount of the 4-
halobenzonitrile is firstly dissolved in DMF/0.1M TBABF4. The solution is then
deoxygenated with an influx of an inert gas (N2 or Ar), and an initial voltammogram is
recorded before starting the electrolysis. The solution is then saturated with CO2
(determined because no increase in intensity is observed in the I-E response, despite
continuing bubbling CO2 into it), and the electrolysis is immediately started. The applied
potential for the reduction of the electro-active substance is about 100 mV more negative
than the corresponding reduction wave. A graphite rod was used as a working electrode
and a Pt as a counter electrode, isolated from the solution by a salt bridge with electrolyte
5

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solution, and an SCE was used as a reference electrode, which was also separated from
the solution by a salt bridge. The electrolysis is finished, either when the desired charge
is consumed according to the Faraday’s Law, or when the initial intensity has been
reduced by over 90% (exhaustive electrolysis). At this point, 4 equivalents of an
alkylating agent are added (R-Y: R: methyl, ethyl, or 2-ethylbenzene; Y: I or Br) to the
solution and kept under constant N2 bubbling for 15-20 minutes.
The electrolyzed samples are then extracted with ether/HCl 1M in the same
proportion. The products that are more soluble in acid water (HCl 1M) (x3) being
extracted from the organic phase, and later with H2O (x2). The aqueous acid phase is
finally extracted using ether. The resulting organic phase is dried with anhydrous sodium
sulphate, filtered, and evaporated in a rotating evaporator. To finish, the crude reaction is
analyzed using 1H-NMR and GC-MS and compared with pure samples.
Typical Procedure for Preparative Electrolysis − Generation of isolated carboxylated
products by preparative Electrolysis: a solution solution of the halobenzonitrile (50-100
mg), which contains 0.1 M TBABF4 is electrolyzed following the above-mentioned
procedure. Four equivalents of the alkylaying agent were added at the end of the
electrolysis. After that the electrochemical cell was bubbled with nitrogen for 10 minutes.
Later an extraction with ether/HCl 1M was performed, and the crude product [or mixture
of product(s)] was purified or separated by chromatography on silica gel eluting with
mixtures of hexane/dichloromethante (40:60). The yield obtained for isolated products in
pure form were a 5 % less than the firstly determined for the non-purified crude.
Benzonitrile: GC-MS (70 eV): m/z (%): 103.0 (100) [M+], 76.0 (36) [M+ - CN], 63.0 (4),
52.0 (6), 51.0 (12).
4-cyanobenzoate methyl ester: GC-MS (70 eV): m/z (%): 161.0 (22) [M+], 130.0 (100)
[M+- CH3O], 102.0 (44) [M+- C2H3O2], 75.0 (14%), 51.0 (8). 1H-NMR (250 MHz,
CDCl3)  (ppm): 3.96 (s, 3H), 7.75 (d, 8.33 Hz, 2H), 8.14 (d, 8.33 Hz, 2H).
Dimethyl terephthalate: GC-MS (70 eV): m/z (%): 194.0 (18) [M+], 163.0 (100) [M+ -
CH3O], 135.0 (22) [M+ - C2H3O2), 120.0 (8) [M+ - C3H6O2], 103.0 (13) [M+ -
C3H6O3], 92.0 (3), 76.0 (13) [M+ - C4H6O4]. 1H-NMR (250 MHz, CDCl3)  (ppm):
3.95 (s, 6H), (s, 8.10 Hz, 4H).
Diethyl terephthalate: GC-MS (70 eV): 175.0 (13) [M+], 147.0 (34) [M+ - C2H5], 130.0
(100) [M+ - C2H5O], 102.0 (42) [M+ - C3H5O2], 87.0 (5), 75.0 (13) [M+ - C4H5O2N].
Terephthalic acid monoethyl ester: GC-MS (70 eV): m/z (%) 194.0 (11) [M+], 166.0 (35)
(M+ - C2H5], 149.0 (100) [M+ - C2H5O], 121.0 (17) [M+ - C3H5O2], 104.0 (6) [M+ -
C3H6O3], 76.0 (9) [M+ - C4H6O4], 65.0 (20), 51.0 (5).
4-cyanobenzoate ethyl ester: GC-MS (70 eV): m/z (%): 222.1 (6) [M+], 194.1 (20) [M+ -
C2H5], 177.1 (100) [M+ - C2H5O], 166.0 (35), 149.0 (86) [M+ - C3H5O2], 132.0 (2) [M+ -
C4H10O2], 121.0 (19) [M+ - C5H10O2], 104.0 (24) [M+ - C5H10O3], 76.0 (23) [M+ -
C6H10O4], 65.1 (21), 51.0 (4).
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Diethyl terephthalate: GC-MS (70 eV): 175.0 (13) [M+], 147.0 (34) [M+ - C2H5], 130.0
(100) [M+ - C2H5O], 102.0 (42) [M+ - C3H5O2], 87.0 (5), 75.0 (13) [M+ - C4H5O2N].
Terephthalic acid monoethyl ester: GC-MS (70 eV): m/z (%) 194.0 (11) [M+], 166.0 (35)
(M+ - C2H5], 149.0 (100) [M+ - C2H5O], 121.0 (17) [M+ - C3H5O2], 104.0 (6) [M+ -
C3H6O3], 76.0 (9) [M+ - C4H6O4], 65.0 (20), 51.0 (5).
4-cyanobenzoate ethyl ester: GC-MS (70 eV): m/z (%): 222.1 (6) [M+], 194.1 (20) [M+ -
C2H5], 177.1 (100) [M+ - C2H5O], 166.0 (35), 149.0 (86) [M+ - C3H5O2], 132.0 (2) [M+ -
C4H10O2], 121.0 (19) [M+ - C5H10O2], 104.0 (24) [M+ - C5H10O3], 76.0 (23) [M+ -
C6H10O4], 65.1 (21), 51.0 (4).
Diphenethyl terephthalate: GC-MS (70 eV): m/z (%) 374.4 [M+], 253.1 (6) [M+ - C8H9O],
149.0 (12) [M+ - C16H18O], 121.1 (5) [M+ - C17H18O2], 104.1 (100) [M+ - C17H18O3], 91.1
(5) [M+ - C17H15O4], 77.1 (3) [M+ - C18H17O4], 65.1 (5), 51.1 (1).
4-cyanobenzoate phenethyl ester: GC-MS (70 eV): m/z (%) 251.3 [M+], 130.0 (28) [M+
- C8H9O], 104.1 (100) [M+ - C9H9ON], 91.1 (13) [M+ - C9H6O2N], 77.1 (M+ - C10H8O2N],
65.1 (5), 51.1 (5).
3-phenylpropionitrile: GC-MS (70 eV): m/z (%): 131.1 (25) [M+], 103.1 (3) [M+ - 91.1
(100) [M+ - C2H2N], 77.1 (5) [M+ - C3H4N], 65.1 (12), 51.1 (7).
Benzoate phenethyl ester: GC-MS (70 eV): 226.3 [M+], 104.1 (100) [M+ - C8H9O], 91.1
(8) [M+ - C8H7O2], 77.0 (33) [M+ - C9H9O2], 65.0 (4), 51.0 (10).
2.2.3. Instrumentation
The cyclic voltammetry at different scan rates and controlled potential electrolysis are
performed using a PAR 273A potentiostat controlled by a computer. Powersuite software
is used for data acquisition and data treatment.
1
H NMR spectra were recorded on a Bruker DPX360 (360 MHz) spectrometer and GC-MS
analysis were performed using an Agilent Technologies 6850 GC instrument with a 5975C
detector.
7

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3.
Results and Discussion
3.1. Electrochemistry of 4-halobenzonitriles under N2 atmosphere
A study has been conducted order to establish the optimal experimental conditions
for the optimal electrochemical capture of CO2, the electrochemical behavior of 4-
halobenzonitriles (F, Br, Cl and I derivatives). Cyclic voltammograms of a 10 ml solution
in DMF using 0.1M of tetrabutylammonium tetrafluoroborate (TBABF4) were recorded
at different scan rates (from 0.10 a 1.0 V s-1) using Ag (solid lines) or Glassy Carbon (GC,
dotted line) as working electrodes under N2 atmosphere for each halobenzonitrile
derivative (Figure 1).
Figure 1. Cyclic voltammograms of 5-15 mM 4-halobenzonitriles (X: F, Cl, Br and I)
solutions using Ag (solid line) and GC (dotted lines) in DMF/0.1M TBABF4 under
nitrogen atmosphere. Scan rate: 0.5 V·s-1.
As it can be deduced from Figure 1, two different electrochemical pathways can be
distinguished. The 4-fluorobenzonitrile shows only an electron transfer process, whereas
the other halobenzonitrile derivatives show two electron transfer processes up to -2.5 V.
Focusing on the first electron transfer process, all the compounds show an irreversible
two electron reduction wave (Table 1). The peak width values (Epc) greater than 56mV
reveal a slow electron transfer process. According to previously reported cyclic
voltammetry studies performed in our laboratory[38–40], the second electron transfer
process seen when X ≠ F corresponds to one electron transfer process, is attributed to the
electrochemical reduction of benzonitrile. Thus, the benzonitrile moiety is the initial
8

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electron acceptor, and the cyano group acts as an intramolecular catalyst of the halogen
atom removal when X ≠ F. The electrochemical parameters of the electrochemical
reduction of 4-halobenzonitriles are summarized in Table 1. It is worth noting the shape
of the cyclic voltammograms recorded at the same for each compound when either GC
or Ag is used as a working electrode. The presence of halogen substituents in the aromatic
compounds, electron withdrawing groups (because of higher electronegativity), makes
easier to reduce them. A closer look to the Epc values of halobenzonitriles reveals
However, there is another effect related to the fact that their lone pair can be incorporated
that their tendency to gain electrons and get reduced follow the order I > Br > Cl>F, which
indicated that the halogen lone pair can be incorporated in conjugation of the systems
affecting the reduction potential values. However, a closer look reveals that, for all the
halobenzonitriles studied, the use of Ag to enable the compound to be reduced at less
negative potential values demonstrates the electrocatalytic effects of this material.
Table 1. Electrochemical parameters associated to the first reduction wave of 5-15 mM of 4-
halobenzonitrile solutions (X: F, Cl, Br, and I) contained in 10 ml DMF/0.1M TBABF4 under N2
atmosphere, using Ag or GC as WEs, respectively, Pt as counter-electrode, and SCE as reference
electrode.
Ag
GC
Electrocatalytic
effect:
4-
Epc
(V)
∆Epc
(mV)
Epc
(V)
∆Epc
(mV)
Halobenzonitriles
Epc(Ag)-Epc(GC)
Number of electrons
(mV)
30
F
Cl
Br
I
2
2
2
2
-2.35
-1.95
-1.75
-1.46
80
90
-2.38
-2.04
-1.94
-1.84
80
100
110
110
90
210
50
190
380
In order to demonstrate the electrochemical reduction mechanism of halobenzonitriles in
our experimental conditions, controlled-potential electrolysis was performed after the
first reduction wave. In the case of 4-fluorobenzonitrile, exhaustively controlled potential
electrolysis experiments were performed at -2.45 V (Vs SCE), using 20 mM solutions in
DMF/0.1M TBABF4. The distribution of products obtained after the reduction of the
sample depended on the nature of the electrode. In the case of using a carbon graphite rod
as cathode, the products obtained were benzonitrile and 4,4’-dicyanobibenzene, which is
in good agreement with previously reported studies using Pt as a cathode (Scheme 4).
The formation of 4,4’-biphenyldicarbonitrile from 4-fluorobenzonitrile can be
rationalized by a dimerization reaction of 4-fluoro-benzonitrile anion radical (Scheme 4,
step 2), which decomposes by the elimination of two fluoride anions, leading to the
corresponding dimer (step 3).
9

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1e
(1)
CN
CN
F
F
CN
F
2
F
2
N C
C N
(2)
(3)
F
2
2F
F
N C
C N
NC
CN
F
Scheme 4. Proposed mechanism for the formation of 4,4’-biphenyldicarbonitrile from
4-F-benzonitrile.
Benzonitrile and dimer derivatives are also obtained when silver (Ag) foil was used as
working electrode, (Scheme 5). In this sense, the electrochemical reduction mechanism
appears to be the same in both cases, although the use of silver seems to favor a de-
cyanidation process of the products formed, probably due to an adsorption process of the
reduction intermediates at the electrode surface. The presence of 4-hydroxybenzonitrile
can be explained due to the reactivity of the reactant (4-F-benzonitrile) in the medium
after the electrolysis.
CN
F
3 F, N2
-2.45 V (vs SCE)
Silver as a Working Eletrode
NC
Carbon as a Working Eletrode
NC
CN
OH
NC
(67 %)
(23 %)
(44 %)
(41 %)
NC
NC
(traces %)
(15 %)
Scheme 5. Electrolysis of a 16 mM solution of 4-F-benzonitrile in DMF/0.1M TBABF4,
applying a potential of -2.45 V (vs SCE), consuming 3 F of charge, under a N2
atmosphere, using silver foil as WE, a Pt counter-electrode, and a SCE reference
electrode.
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Controlled potential electrolysis experiments of Cl, Br, and I halobenzonitriles (applying
a reduction potential value of ~0.1 V more negative than its first reduction potential wave
using either using C graphite or Ag) reveal the quantitative formation of benzonitrile after
the passage of 2 F under nitrogen atmosphere (Scheme 6). The formation of benzonitrile
is related to a bond cleavage reaction coupled to the initial electron transfer process. The
benzonitrile radical formed is reduced at this potential value, yielding the corresponding
anion, which is protonated in last step. Those results are in good agreement with previous
work published in the literature using a C electrode, as a working electrode[38,39,41]
.
-2.00 V (vs SCE)
CN
X
CN
2 F, N2, Ag
100 %
Scheme 6. Electrolysis of 10 mM of 4-halobenzonitrile solutions in DMF/0.1M TBABF4
under N2 atmosphere using Ag as a working electrode.
From these electrochemical results obtained under inert atmosphere, it is possible to
conclude that in the case of Cl, Br and I benzonitrile derivatives the electrocarboxylation
process should take place through a nucleophilic attack between the benzonitrile anion
and CO2. Whereas, in the case of 4-F-benzonitrile the electrocarboxylation process would
be triggered through a reaction between of 4-F-benzonitrile radical anion and CO2.
3.2. Electrochemistry of 4-halobenzonitriles under CO2 atmosphere
Cyclic voltammetry of the different 4-halobenzonitriles (X: F, Cl, Br and I) are performed
using Ag and GC under CO2 atmosphere (Figure 2). In the case of 4-Br, 4-Cl and 4-I,
when either GC or Ag were used as a working electrode two reduction peaks were
observed at the same reduction potential values, which were previously determined under
inert atmosphere for each electrode. Hence, the first one is related to the reduction of the
4-halobenzonitrile, whereas the second one is related to the reduction of benzonitrile.
Note that under CO2 atmosphere, the benzonitrile reduction peak turns irreversible and
increases dramatically its peak current value, which indicates that benzonitrile is acting
as an organic mediator (catalyst) for the reduction of CO2 (Scheme 7). In the case of 1-
Fluorobenzonitrile only an increase in the cathodic peak current value is detected since
the reactant and products (benzonitrile and 4,4’-biphenyldicarbonitrile) , which act as a
catalyst appear at the same potential values[28,42]. Note that at low CO2 concentration
(5 mM, Figure 2D), it is possible to distinguish a third reduction peak at c.a. -2.4 V vs.
SCE. According to previous studies performed in our research group, this new reduction
peak corresponds to a CO2 direct reduction at the surface of silver electrode[43].
11

ACCEPTED MANUSCRIPT
A
B
F
NC
Cl
NC
32 mM [CO2]
47 mM [CO2]
-3,0
-2,5
-2,0
-1,5
-1,0
-3,0 -2,8 -2,6 -2,4 -2,2 -2,0 -1,8 -1,6 -1,4
Potential (V vs SCE)
Potential (V vs SCE)
C
D
I
NC
Br
NC
Ag 5 mM [CO2]
Ag 40 mM [CO2]
GC 40 mM [CO2]
31,7 mM [CO2]
-3,5
-3,0
-2,5
-2,0
-1,5
-1,0
-0,5
-2,8
-2,4
-2,0
-1,6
-1,2
Potential (V vs SCE)
Potential (V vs SCE)
Figure 2. Cyclic voltammograms of 5-15 mM 4-halobenzonitriles (X: F, Cl, Br and I)
solutions using Ag (black lines) and GC (grey lines) in DMF/0.1M TBABF4 under at scan
rate: 0.5 V·s-1 under CO2 atmosphere.
+ 2e-
NC
X
NC
First reduction peak
X: Cl, Br,I
NC
NC
NC
Solvent
+ e-
NC
Second reduction peak
NC
+ CO2
+ CO2
Oxalate and
other derivatives
NC
Scheme 7. Mechanism proposal for the reduction of 4-Cl, 4-Br and 4-I using GC
electrode under saturated CO2 atmosphere.
Electrolysis of 4-halobenzonitriles (X: F, Cl, Br, and I) are performed using a Ag foil
or Cgraphite bar, applying potentials ~0.1 V more negative than the previously determined
the first reduction wave of each 4-halobenzonitrile (Table 2) in CO2-saturated solutions
with ~12 mM of the organic compound in DMF and an excess of supporting electrolyte
(0.1M of TBABF4 for Ag or TEABF4 for C). After the consumption of the desired charge,
12

ACCEPTED MANUSCRIPT
an alkylating agent, methyl iodide (CH3I), was added to facilitate the separation of the
products.
The results of these experiments are depicted in Table 2 (entries 1-7 and 10-14). A
general trend is observed in all the cases independently of the nature of the electrode, Ag
or C, and the total charge passed (from 1.7 to 4.5 F). When 4-Br-, 4-Cl-, and 4-I-
halobenzonitriles solutions are electrolyzed a mix of mono- (4-cyanobenzoate methyl
ester) and di-carboxylated (dimethyl terephthalate) products are obtained after the
chemical treatment of the sample (Scheme 8 and Table 2, entries 1-7, and 10-14). In
contrast, with X = 4-F-, only the di-carboxylated compound is formed (Table 2, entries
1-3). In addition, in all the cases when the total charge passed increases, less reactant
remains, and the percentage of di-carboxylation increases.
CO2, Ag/C
4 eq. CH3I
O
O
O
O
O
O
+
NC
X = Cl, Br, I
X = F
NC
X
O
O
O
CO2, Ag
O
4 eq. CH3I
Scheme 8. Electrolysis of 10-14 mM 4-halobenzonitrile (X: F, Cl, Br, I) CO2-saturated
solutions in DMF/0.1M TBABF4 or TEABF4, with an Ag foil or a Cgraphite rod as WEs
and adding 4 equivalents of CH3I at the end of each experiment.
Table 2. Products distribution obtained by electrolysis of 10 mM 4-halobenzonitriles (X: F, Cl, Br, and
13

ACCEPTED MANUSCRIPT
I) CO2-saturated solutions in DMF/0.1M TBABF4 or TEABF4, with a Ag foil or Cgraphite, respectively,
after adding 4 equivalents of the corresponding alkylating agent indicated on the right column. “Mono-”
and “di-” terms refer to mono-carboxylated or di-carboxylated product.
Yield (%) of carboxylated
Halobenzonitrile
(X)
Eapplied
Alkylating
agent
products
WE
C mol-1
Entry
(V vs SCE)
mono-
di-
11
20
40
40
49
29
87
90
1
2
F
F
2.0
3.5
4.5
2.1
3.5
2.3
4.5
4.5
-2.45
-2.45
-2.75
-2.05
-2.05
-1.80
-1.90
-1.80
CH3I
CH3I
0
0
3
F
CH3I
0
4
Cl
Cl
Br
Br
Br
CH3I
20
31
36
1
5
CH3I
6
CH3I
Aga
7b
8
CH3I
Br-CH2CH3
10
2-Br-
CH2CHPh
9
Br
4.5
-1.80
17
49
10
11
12
I
I
2.0
3.5
1.7
2.0
1.7
-1.80
-1.80
-2.15
-2.10
-2.10
CH3I
CH3I
CH3I
CH3I
CH3I
39
28
15
27
16
31
67
23
18
12
Cl
Br
I
Cgraphite 13
14
a100% of conversion ratios, the reactant was the only product apart from the electrocarboxylation products
recovered at the end of the experiment. b In this case a 12 % of benzonitrile was obtained at the end of the process,
it can be attributed to the application of a higher negative reduction potential value. Under these conditions, CO2
can be also reduced and react with the halobenzonitrile derivative (Scheme 1 – Steps 1-3a). Finally, a radical
.
cleavage in the Kolbe reaction of the monocarboxylated product (R-CO2 ) will occur leading to benzonitrile and
CO2[44].
A closer look at Table 2 revealed that, when C is used as a cathode, moderate yields of
carboxylated products were obtained (from 24 % to 45 %) using high reduction potential
values (c.a. -2.00 V vs. SCE, entries 12-14) when non-fluorinated benzonitrile is used.
When fluorobenzonitrile is used as a starting material, no carboxylated products were
obtained using C graphite as a working electrode The observed reactivity can be related
to the ability of the aromatic radical anions to undergo cleavage of the carbon halogen
bond, with the peculiarity that in our case there is a stable fluoride radical anion that
dimerises[45].
14

ACCEPTED MANUSCRIPT
Replacing C cathode, which acts as an inert electrode, by Ag cathode not only allows
reducing the reduction potential value applied but also increasing the yield of
carboxylation products (entries 4-11). Ag electrode is recognized as a powerful catalytic
electrode in organic solvent, being its catalytic property ascribe to the adsorption between
metal surface and halogenated substrate as well as its reduction intermediates and
products. Hence, due to these adsorption processes that favors the stability of reduction
intermediates after the same total charge passed, the same consumption of charge, the
yield of carboxylation is higher for Ag, but also in global terms, carboxylation is 2-3 times
for Ag.
The maximum yield of dimethyl terephthalate (87%, entry 7) is reached for controlled
potential electrolysis of a bromobenzonitrile solution at -1.80 V (vs SCE) after the
passage of 4.5 F under CO2 atmosphere using Ag as a cathode. The use of 4-I-benzonitrile
also allows obtaining carboxylation yields close to 100 % after the passage of 3.5 F. The
ratio of % of di-carboxylation/charge consumed is the same in both cases, thus this could
suggest that maybe the adsorption of the I-derived reactant (Figures 1) plays an important
role for the carboxylation process.
As it was previously mention, no carboxylated products were obtained using C graphite
as a working electrode for fluorobenzonitrile. However, the use of silver as a working
electrode enables a maximum yield of 40% of dimethyl terephthalate (entry 3) to be
obtained after the passage of 4.5 F at of -2.75 V (vs SCE). It is worth noting that, after
the passage of the same number of Farads, the total yield of electrocarboxylation products
is as follows; I>Br>Cl>F. This fact can be explained by considering the bond dissociation
energies (BDEs) of the Ar-X bonds.
On observing the above-mentioned results, it is plausible to propose a mechanism for
the insertion of CO2 in 4-halobenzonitriles (X: Cl, Br, and I) the following mechanism
(Scheme 9). In a first step, the reduction of the 4-halobenzonitrile forms the correspondent
radical anion, which rapidly cleaves to give the benzonitrile radical, and the
corresponding halide (step 2). In a third step, the radical reduces at the electrode surface
leading to the benzonitrile anion. In a further step, this anion can react with CO2 under
CO2-saturated atmosphere, leading to 4-cyanobenzoate anion (step 4). Finally, the
addition of iodomethane as alkylating agent (R-Y) yields the correspondent ester (step 5).
15

ACCEPTED MANUSCRIPT
1e
Step 1
NC
X
CN
X
Step 2
Step 3
Step 4
CN
CN
X
CN
X
+
1e
CN
CN
CO2
R-Y
CO2
CN
CN
Step 5
CO2
+ Y
CN
CO2R
Scheme 9. Electrochemical Strategy for inserting CO2 in 4-halobenzonitriles (X: Cl, Br,
and I).
Note that the ratio of carboxylated products (4-cyanobenzoate methyl ester vs. dimethyl
terephthalate) can be tune in function of the charge passed during the electrolysis. This
fact should be related to the reduction of the 4-cyanobenzoate formed upon the
electrolysis, this dianion can act as a nucleophile and react with the CO2 (Scheme 10).
Lately, the decyanation of dianion has taken place. This mechanism is supported by the
detection of cyanide anion at the end of the electrolysis. Hence, the formation of the
carboxylated di-substituted products is related to the reactivity of the nitrile group in
presence of CO2. Moreover, reductive decyanation processes for similar compounds has
been previously reported in the literature[46–48].
1e
1e
CN
CO2
CN
CO2
CO2
CO2
CO2
- CN
O2C
CO2
RO2C
CO2R
R-Y
Scheme 10. Electrochemical reduction mechanism of 4-halobenzonitriles (X: Cl, Br, and
I) under CO2 atmosphere after the passage of 3-4 F.
In the case of 4-fluorobenzonitrile then only carboxylated product obtained after the
electrocarboxylation process in Ag was the dimethyl terephthalate. In this case, the
electrocarboxylation is very selective and enables yields of 40 % to be obtained, as has
been previously pointed. The plausible electrocarboxylation mechanism is depicted in
Scheme 10. The fluorobenzonitrile anion radical reacts with CO2 instead of dimerization
leading to a benzonitrile carboxylated derivate (Scheme 11). This derivate is not stable at
16

ACCEPTED MANUSCRIPT
high negative reduction processes values and further reduction are taking place following
the same mechanism that the previously described for the rest of halobenzonitriles
(Scheme 9). The process ends with the capture of CO2, and further alkylation processes.
1e
CN
F
CN
F
F
1e
CN
F
CN
CO2
CN
CO2
N C
CO2
- F
Scheme 11. 4-fluorobenzonitriles under CO2 atmosphere electrochemical reduction
mechanism
Once halobenzonitrile in CO2 cathode electrochemical reduction mechanism as well as
the electrocarboxylation conditions were optimized at the silver, other alkylation agents
were used in other to check the potentiality of the methodology. 4-bromo-benzonitrile
was selected as a starting material, since almost a 100 % of electrocarboxylation products
were obtained using methyl iodide as a methylated agent (Table 2, Entry 9). Hence,
controlled potential electrolysis, at –1.80 V vs. SCE, of a 10 mM DMF/0.1M TBABF4
solution of 4-bromo-benzonitrile in a CO2-saturated were performed using Ag foil as a
working electrode. After, the passage of 4.5 F, four equivalents of two different alkylating
agents: 1) bromoethane and (2-bromoethyl) benzene were added at the end of the
electrolysis. In the first case, the analysis of the electrocarboxylation process yields 75%
of diethyl terephthalate, 15 % of terephthalic acid mono-ethyl ester, and 10% 4-
cyanobenzoate ethyl ester, Scheme 12 (Table 3, entry 8). Changing the alkylating agent
for (2-bromoethyl) benzene, the analysis of the electrocarboxylation process revealed a
49% diphenethyl terephthalate, 13% 4-cyanobenzoate phenethyl ester, 8% 3-
phenylpropionitrile, and 4% benzoate phenethyl ester, and 25 % of the alkylating agent
is recovered (Scheme 12, Table 2, entry 9). As mentioned before, the presence of the 3-
phenylproprionitrile molecule can be explained by the reaction between the removed
cyanide anion from the reactant and the alkylating agent. Note that there is a steric
hindrance effect on the efficiency of alkylation reaction.
17

ACCEPTED MANUSCRIPT
HO
O
O
O
O
O
O
O
-1.80 V (vs SCE)
CO2, 4.5 F, Ag
15 %
75 %
O
O
4 eq. Br-ethane
NC
10 %
(a)
CN
Br
O
O
O
O
(b)
49 %
13 %
O
O
-1.80 V (vs SCE)
CO2, 4.5 F, Ag
CN
Br
4 eq. 2-Br-ethylbenzene
25 %
O
O
CN
8 %
4 %
Scheme 12. Electrolysis of 10-14 mM 4-bromobenzonitrile CO2-saturated solutions in
DMF/0.1M TBABF4 with an Ag foil. At the end of the electrocarboxylation process the
alkylation agent was added: a) bromoethane b) for (2-bromoethyl)benzene.
4.
Conclusions
Electrolysis of 4-halobenzonitrile in CO2-saturated employing a carbon graphite rods or
silver foils as a cathode lead to the formation of mono-, and di-substituted products from
moderate to almost quantitative yields. The maximum efficiency of the carboxylation
process is achieved with the passage of c.a. 4F. It has also been demonstrated that the use
of “small” alkylating agents, such as iodomethane or bromoethane, enables higher yields
to be obtained in terms of carboxylation products, probably due to hindrance effects. The
use of Ag as working electrode enables controlled potential electrolysis to be performed
at less negative potential values. Hence, electrocatalytic effects are seen when Ag is used
as cathode, giving very high yields in terms of di-carboxylated products, where two units
of CO2 are incorporated to one unit of halobenzonitrile. This “new” methodology offers
a new “green” route for the synthesis of different phthalate derivatives, which can
potentially be used for making plastic polymers in a more environmentally friendly way.
18

ACCEPTED MANUSCRIPT
Acknowledgements
This work was supported by projects CTQ2015-65439-R from the MINECO/FEDER and
APOSTA UAB. S.M. thanks the Universitat Autònoma de Barcelona for pre-doctoral PIF
fellowships.
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