# Cobalt-Salen Catalyzed Electroreductive Alkylation of Activated Olefins

Authors: Sylvie Condon; Céline Cannes; Fethi Bedioui
Journal: Journal of Chemistry
 (2019)

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## Abstract

Cobalt-Salen mediated electroreductive and regioselective alkylation of electron deficient olefins is reported in one step in an undivided electrochemical cell, in the presence of an iron rod as sacrificial anode. Although the reactivity depends on the class of alkyl halides, the reported study offers a green and expeditious electrosynthetic route for Csp3-Csp3 bond formation in mild conditions. This study also confirms the possible formation of the heterobinuclear cobalt-Salen-iron complex previously reported as the effective catalyst.


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## Body

## 1. Introduction

In the context of sustainable organic chemistry, electrosynthesis has gained a renewable interest because of its relevant green aspects [1–3]. This versatile process involves electrons as clean surrogates of dangerous, toxic, hazardous reductive or oxidative reagents. Furthermore, the possibility to generate in situ the active catalytic species, or the disposal of high valuable products in one step reaction pathway is on contemporary concerns. Various papers of our laboratory report the activation of aryl halides under cobalt or nickel catalysis for Csp2-Csp2 bond formation (biaryl access) [4–6] or Csp2-Csp3 bond formation (conjugate addition reaction) [7, 8] by using the sacrificial anode process [9]. However, less attention has been devoted to the Csp3-Csp3 bond formation. Some years ago, we have described the coupling of halogenated and pseudohalogenated glycerol carbonate with electron deficient olefins under nickel catalysis in greener solvent [10].The most common method of alkylation of activated olefin is a multistep procedure requiring the preparation of the alkylcopper reagent and then its reaction with the activated olefin [11]. This can be circumvented advantageously by activation of the alkyl halide by a transition metal complex and its further reaction with the electrophile. Such reactions can be carried out in one step procedure, in mild conditions. In most cases, the transition metal complex is reduced in situ either chemically, by Zn [12–14] or Mn [15], or electrochemically [16].The conjugate addition reactions catalyzed by transition metal complexes involve mainly nickel [8, 17–19] or cobalt [7, 20–23] complexes or chromium compounds [24–26]. In the case of cobalt [20–23], the catalyst is generally coordinated to Schiff base ligands, such as the vitamine B12 and cobaloximes, and the addition product is obtained with good yield in one step procedure. However, the reaction was generally conducted in a divided cell, by controlled potential electrolysis, and vitamin B12 is an expensive catalyst [20–23]. Few models of vitamin B12, such as N,N′-ethylenebis(salicylideneiminato)-cobalt (noted CoSalen), more simple and cheaper, have been then used as catalyst for the heterocoupling of organic halides and alkylation of alkyl halides with activated olefins [23]. In most cases, the reactions were carried out in hexamethylphosphoramide or hexamethylphosphoramide/tetrahydrofuran, in a double compartment electrochemical cell, on a mercury pool cathode and with poor and unsatisfactory yields.Thus, in the course of our work on the electrochemical activation of organic halides using the sacrificial anode process [9], we have found that alkylation of activated olefins can be carried out with a simple and cheap cobalt complex formed in situ. This allowed us to show that the combined use of cobalt-Salen (as catalyst) with the undivided electrochemical cell process offers substantial advantages in the reductive coupling of 2-bromooctane and methyl vinyl ketone (MVK) [27]. We report here a systematic study of some examples of reductive coupling of alkyl halides and activated olefins using cobalt complexes to assess the influence of the experimental parameters (ligand, solvent, temperature, and electrolysis conditions) in order to optimize the yield and to get a better insight into the electroassisted catalytic mechanism.


## 2. Experimental

All solvents and reagents were purchased from commercial sources and used as received. Dimethylformamide (DMF) was stored under an argon atmosphere. Electrosyntheses were carried out either in a double compartment cell or in an undivided electrochemical cell.Electrosyntheses carried out in a double compartment electrochemical cell equipped with a fritted glass separation were performed with an anode and a cathode made of carbon fibers (total geometric area of 30 cm2, from Prolabo). Both cathodic and anodic compartments were filled with 25 mL of DMF solution containing tetrabutylammonium bromide, noted TBABr (0.236 mol·L−1) and tetrabutylammonium iodide, noted TBAI (0.054 mol·L−1) and kept under argon atmosphere. The catalyst precursor was introduced in the cathodic compartment (15 mmol·L−1), and the solution was stirred during 15 minutes.Electrosyntheses carried out in an undivided electrochemical cell were performed with a cathode made of a nickel foam grid (geometric area of 30 cm2) and a sacrificial anode made of a rod of aluminum, magnesium, copper, zinc, or iron. The electrochemical cell was filled with DMF solution (35 mL) containing TBABr (10 mmol·L−1) and TBAI (8 mmol·L−1) and kept under argon atmosphere. CoSalen complex (10 mmol·L−1) or a mixture CoCl2/ligand (10 mmol·L−1 and 20 mmol·L−1, respectively) was then added and heated at 60–80°C. After stirring for 15 minutes, 2-bromooctane (0.2 mol·L−1) and MVK (0.535 mol·L−1) were introduced.In both cases, the electrolysis was run at constant current density (0.3 A·dm−2) or constant potential (−1.2 V or −1.6 V). The cathode potential was measured and referenced to a saturated calomel electrode (SCE) which was placed in a separate compartment containing the solvent and the supporting electrolyte. The reaction was monitored by gas chromatography analysis (GC) using ethyl undecanoate as internal standard and was stopped after 2-bromooctane was totally consumed. The reaction mixture was then hydrolyzed with hydrochloric acid (1 N, 30 mL). The aqueous layer was extracted with diethyl ether (2 × 30 mL). The combined organic layers were washed with water, dried over MgSO4, and concentrated. Finally, the product was purified by preparative column chromatography (silica gel 70–230 mesh; eluent: pentane/ether 95/5). The reaction products were identified by 1H and 13C-NMR (Brucker 200 MHz) in CDCl3 and mass spectrometry (Finnigan ITD 800). GC analyses were carried out using a 25 m DB1-capillary column. Elemental analyses were made by the Service Central de Microanalyses (CNRS, Lyon). Physical and spectral data are given as follows.


### 2.1. Ethyl 4-Methyl Decanoate3

Colorless liquid, 0.65 g (43%).1H-NMR (200 MHz, CDCl3): δ ppm 4.04 (q, 2H, J = 7.1 Hz), 2.20 (m, 2H), 1.55 (m, 2H), 1.15–1.37 (m, 14H), 0.8 (m, 6H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.8, 59.8, 36.5, 32.1, 31.8, 31.6 (2C), 29.3, 26.6, 22.4, 19.0, 13.8. MS: 215, 157, 101 (100%), 88, 73, 55.


### 2.2. Ethyl 3-Cyclohexylpropanonate4

CAS Registry Number 10094-36-7, colorless liquid, 0.47 g (37%) [28]. 1H-NMR (200 MHz, CDCl3): δ ppm 4.06 (q, J: 6.8 Hz, 2H), 2.24 (t, J: 7.6 Hz, 2H), 1.64–1.70 (m, 5H), 1.48 (m, 2H), 1.06–1.24 (m, 7H), 0.88 (m, 2H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.1, 59.5, 37.0, 32.7 (2C), 32.0, 31.4, 26.2, 26.0 (2C), 13.8. MS: 185, 155, 121, 101, 81, 73, 67, 60, 55 (100%).


### 2.3. Ethyl 4,4-Dimethylpentanoate5

CAS Registry Number 10228-99-6, colorless liquid, 0.37 g (33%).1H-NMR (200 MHz, CDCl3): δ ppm 4.00 (q, J: 7.1 Hz, 2H), 2.15 (m, 2H), 1.45 (m, 2H), 1.15 (t, J: 7.1 Hz, 3H), 0.80 (s, 9H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 174.1, 60.0, 38.5, 30.00 (4C), 28.8, 14.0. MS: 159, 143, 113, 102, 97, 74, 69, 57 (100%).


### 2.4. Ethyl 4-Phenylbutanoate6

CAS Registry Number 10031-93-3, 0.20 g (14%), colorless liquid [29]. 1H-NMR (200 MHz, CDCl3): δ ppm 7.15 (m, 5H), 4.02 (q, J: 7.15 Hz, 2H), 2.55 (t, J: 7.35 Hz, 2H), 2.20 (m, 2H), 1.86 (m, 2H), 1.15 (t, J: 7.15 Hz, 3H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.3, 141.3, 126.38 (2C), 126.26 (2C), 125.85, 60.1, 35.0, 33.5, 26.5, 14.1. MS: 192, 146, 104, 91 (100%), 70, 65.


### 2.5. 5-Methylheptadecan-2-one7

Colorless liquid, 0.98 g (52%) [30]. 1H-NMR (200 MHz, CDCl3): δ ppm 2.35 (m, 2H), 2.04 (s, 3H), 1.50 (m, 2H), 1.10–1.38 (m, 23H), 0.8 (m, 6H). MS: 269, 97, 85, 71 (100%), 55. Elemental analysis for C18H36O, calculated: C, 80.5; H, 13.5, found: C, 80.8; H, 13.2.


### 2.6. 4-Methyldecanenitrile8

CAS Registry Number 97763-97-8, colorless liquid, 0.58 g (50%) [30]. 1H-NMR (200 MHz, CDCl3): δ ppm 2.26 (m, 2H), 1.68–1.40 (m, 3H), 1.01–1.38 (m, 10H), 0.81 (m, 6H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 196.2, 35.9, 32.0, 31.7, 31.5, 29.1, 26.4, 22.3, 18.4, 14.5, 13.7. MS: 168, 124, 110, 96, 82, 69, 55 (100%).


### 2.7. Dimethyl 2-(1-Methylheptyl)butan-1,4-dioate9

CAS Registry Number 1622297-77-1, 0.90 g (50%), colorless liquid.1H-NMR (200 MHz, CDCl3): δ ppm 3.60 (m, 6H), 2.70 (m, 2H), 2.25 (m, 1H), 1.04–1.36 (m, 11H), 0.8 (m, 6H). MS: 259, 227, 185, 146, 55. Elemental analysis for C14H26O4, calculated: C, 65.1; H, 10.1, found: C, 64.9; H, 10.2.


### 2.8. Ethyl 3,4-Dimethyldecanoate10

Colorless liquid, 128 mg (8%),1H-NMR (200 MHz, CDCl3): δ ppm 4.04 (q, J: 7.1 Hz, 2H), 2.1 (m, 2H), 1.1–1.36 (m, 15H), 0.76 (m, 9H). MS: 229, 115(100%), 101, 88, 69, 55.Physical and spectral data of ethyl undecanoate1 and dodecan-2-one 2 are similar to commercial samples.


## 2.1. Ethyl 4-Methyl Decanoate3

Colorless liquid, 0.65 g (43%).1H-NMR (200 MHz, CDCl3): δ ppm 4.04 (q, 2H, J = 7.1 Hz), 2.20 (m, 2H), 1.55 (m, 2H), 1.15–1.37 (m, 14H), 0.8 (m, 6H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.8, 59.8, 36.5, 32.1, 31.8, 31.6 (2C), 29.3, 26.6, 22.4, 19.0, 13.8. MS: 215, 157, 101 (100%), 88, 73, 55.


## 2.2. Ethyl 3-Cyclohexylpropanonate4

CAS Registry Number 10094-36-7, colorless liquid, 0.47 g (37%) [28]. 1H-NMR (200 MHz, CDCl3): δ ppm 4.06 (q, J: 6.8 Hz, 2H), 2.24 (t, J: 7.6 Hz, 2H), 1.64–1.70 (m, 5H), 1.48 (m, 2H), 1.06–1.24 (m, 7H), 0.88 (m, 2H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.1, 59.5, 37.0, 32.7 (2C), 32.0, 31.4, 26.2, 26.0 (2C), 13.8. MS: 185, 155, 121, 101, 81, 73, 67, 60, 55 (100%).


## 2.3. Ethyl 4,4-Dimethylpentanoate5

CAS Registry Number 10228-99-6, colorless liquid, 0.37 g (33%).1H-NMR (200 MHz, CDCl3): δ ppm 4.00 (q, J: 7.1 Hz, 2H), 2.15 (m, 2H), 1.45 (m, 2H), 1.15 (t, J: 7.1 Hz, 3H), 0.80 (s, 9H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 174.1, 60.0, 38.5, 30.00 (4C), 28.8, 14.0. MS: 159, 143, 113, 102, 97, 74, 69, 57 (100%).


## 2.4. Ethyl 4-Phenylbutanoate6

CAS Registry Number 10031-93-3, 0.20 g (14%), colorless liquid [29]. 1H-NMR (200 MHz, CDCl3): δ ppm 7.15 (m, 5H), 4.02 (q, J: 7.15 Hz, 2H), 2.55 (t, J: 7.35 Hz, 2H), 2.20 (m, 2H), 1.86 (m, 2H), 1.15 (t, J: 7.15 Hz, 3H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 173.3, 141.3, 126.38 (2C), 126.26 (2C), 125.85, 60.1, 35.0, 33.5, 26.5, 14.1. MS: 192, 146, 104, 91 (100%), 70, 65.


## 2.5. 5-Methylheptadecan-2-one7

Colorless liquid, 0.98 g (52%) [30]. 1H-NMR (200 MHz, CDCl3): δ ppm 2.35 (m, 2H), 2.04 (s, 3H), 1.50 (m, 2H), 1.10–1.38 (m, 23H), 0.8 (m, 6H). MS: 269, 97, 85, 71 (100%), 55. Elemental analysis for C18H36O, calculated: C, 80.5; H, 13.5, found: C, 80.8; H, 13.2.


## 2.6. 4-Methyldecanenitrile8

CAS Registry Number 97763-97-8, colorless liquid, 0.58 g (50%) [30]. 1H-NMR (200 MHz, CDCl3): δ ppm 2.26 (m, 2H), 1.68–1.40 (m, 3H), 1.01–1.38 (m, 10H), 0.81 (m, 6H). 13C-NMR (50.32 MHz, CDCl3): δ ppm 196.2, 35.9, 32.0, 31.7, 31.5, 29.1, 26.4, 22.3, 18.4, 14.5, 13.7. MS: 168, 124, 110, 96, 82, 69, 55 (100%).


## 2.7. Dimethyl 2-(1-Methylheptyl)butan-1,4-dioate9

CAS Registry Number 1622297-77-1, 0.90 g (50%), colorless liquid.1H-NMR (200 MHz, CDCl3): δ ppm 3.60 (m, 6H), 2.70 (m, 2H), 2.25 (m, 1H), 1.04–1.36 (m, 11H), 0.8 (m, 6H). MS: 259, 227, 185, 146, 55. Elemental analysis for C14H26O4, calculated: C, 65.1; H, 10.1, found: C, 64.9; H, 10.2.


## 2.8. Ethyl 3,4-Dimethyldecanoate10

Colorless liquid, 128 mg (8%),1H-NMR (200 MHz, CDCl3): δ ppm 4.04 (q, J: 7.1 Hz, 2H), 2.1 (m, 2H), 1.1–1.36 (m, 15H), 0.76 (m, 9H). MS: 229, 115(100%), 101, 88, 69, 55.Physical and spectral data of ethyl undecanoate1 and dodecan-2-one 2 are similar to commercial samples.


## 3. Results and Discussion

Addition of 2-bromooctane to methylvinylketone (MVK) was studied as the model reaction in DMF as solvent (equation (1)):(1)We have first analyzed the influence of the cobalt ligands on the conjugate addition reaction yield (Table1).Table 1
Results of the reductive coupling reaction of 2-bromooctane with methylvinylketone with various cobalt complex catalysts.
Run
Catalyst
Yielda (%)
1
—
2
2
CoCl2 (5%)
8
3
CoCl2 (5%) + H2Salen (5%)
51b
4
CoSalenc (5%)
43
5
CoCl2 (5%) + 2, 2′-bipyridine (5%)
24
6
CoCl2 (5%) + phenantroline (10%)
20
7
CoCl2 (5%) + ephedrine (10%)
56
Experimental conditions: anode = Fe; cathode = Ni grid (surface area = 30 cm2); current intensity I = 0.1 A; solvent = DMF + TBABr (10−2 mol·L−1) + TBAI (8.10−3 mol·L−1); T = 60°C; 2-bromooctane = 0.1875 mol·L−1; methylvinylketone = 0.47 mol·L−1; aGC yield, with ethyl undecanoate as internal standard; bat 20°C, yield = 27%; at 80°C, yield = 61%; cfrom Sigma-Aldrich.In the absence of cobalt salt (run 1) or ligand (run 2), poor yields of alkylated product are obtained. Among the examined ligands, H2Salen (run 3 and 4) and ephedrine (run 7) are the most appropriate ones to provide highest chemical yields for the conjugate addition reaction. Therefore, the supposed active catalyst is a simple and cheap cobalt complex which can be prepared in situ.Solvent influence was also examined (Table2). We found that the best solvent is dimethylformamide either pure (run 1) or in the presence of proton donor. For example, in the case of NH4Cl (5.10−2 mol·L−1) as supporting electrolyte added to DMF (run 2) or DMF/ethanol (EtOH) (1/1) mixture (run 4), the yields, calculated by GC analysis with internal standard, are, respectively, 55% and 59%. Despite the fact the coupling product was obtained with moderate yields in solvent mixtures such as DMF/EtOH (1/1) or DMF/Acetonitrile (AN) (1/1), pure EtOH and AN are not suitable solvents (see Table 2).Table 2
Results of the reductive coupling reaction of 2-bromooctane with methylvinylketone in various solvents under CoCl2+ H2Salen catalysis.
Run
Solvent
Yielda
1
DMF
51%
2
DMF + NH4Clb
55%
3
DMF/EtOH (8/2)
46%
4
DMF/EtOH (1/1)
59%
5
DMF/EtOH (3/7)
22%
6
EtOH
4%
7
DMF/MeOH (1/1)
15%
8
DMF/AN (1/1)
46%
9
AN
Traces
Experimental conditions: anode = Fe; cathode = Ni grid (surface area = 30 cm2); current intensity I = 0.1 A; supporting electrolytes: TBABr (10−2 mol·L−1) + TBAI (8.10−3 mol·L−1); catalyst: CoCl2 (9.4.10−2 mol·L−1) + H2Salen (9.4.10−2 mol·L−1); T = 60°C; 2-bromooctane = 0.1875 mol·L−1; methylvinylketone = 0.47 mol·L−1; aGC yield, with ethyl undecanoate as internal standard; bNH4Cl was used as supporting electrolyte (5.10–2 mol·L−1) and as proton source.Anyhow, for reaction carried out in pure DMF (Table1, run 3), we have found that the yield was very dependent on the temperature: 27% at 20°C, 61% at 80°C. Also, we have noticed that if the electrolysis potential was more negative than −1.2 V/SCE, both the chemical yield (26%) and the Faradaïc yield decrease. This could be due to the direct reduction of the MVK which occurs at ca −1.7 V/SCE. In this case, other reactions, such as MVK polymerization, take place.The stoichiometry of the reaction between MVK and 2-bromooctane was examined. The results reported in Table3 reveal the importance of using excess amount of MVK to improve the yield of the coupling product. However, a large excess of olefin does not improve significantly the yields (run 3 and 4).Table 3
Stoichiometric study of the reaction between MVK and 2-bromooctane.
Run
Equiv. MVK
Yielda (%)
1
1
36
2
2.5
51
3
5
57
4
25
46
Experimental conditions: anode = Fe; cathode = Ni grid (surface area = 30 cm2); current intensity I = 0.1 A; solvent = DMF + TBABr (10−2 mol·L−1) + TBAI (8.10−3 mol·L−1); catalyst: CoCl2 (9.4.10−2 mol·L−1) + H2Salen (9.4.10−2 mol·L−1); methylvinylketone 1 to 25 equiv.; 2-bromooctane = 0.1875 mol·L−1; T = 60°C; aGC yield, with ethyl undecanoate as internal standard.Finally, we have observed that the nature of the anode is crucial to form selectively the addition product. Indeed, results in Table4 show that an iron rod is the most efficient anode, indicating a possible role of the cations anodically generated by its oxidation during the electrolysis.Table 4
Results of the reductive coupling reaction of 2-bromooctane with methylvinylketone with various anodes in an undivided cell.
Run
Anode
Yield∗ (%)
1
Fe
51
2
Zn
33
3
Al
8
4
Mg
6
5
Cu
3
Experimental conditions: anode = metal rod; cathode = Ni grid (surface area = 30 cm2); current intensity I = 0.1 A; T = 60°C; solvent = DMF + TBABr (10−2 mol·L−1) + TBAI (8.10−3 mol·L−1); catalyst = CoCl2 (9.4.10−2 mol·L−1) + H2Salen (9.4.10−2 mol·L−1); 2-bromooctane = 0.1875 mol·L−1; methylvinylketone = 0.47 mol·L−1; ∗GC yield, with ethyl undecanoate as internal standard.Such a crucial role of anodically generated cations has also been reported in other processes related to electroassisted reductions of organohalides catalyzed by nickel complexes [31]. Their occurrence in this reaction was analyzed by cyclic voltammetry and showed the possible formation of a catalytically active Co-Salen-Fe binuclear complex [27]. Indeed, Table 5 recapitulates the comparative analysis of the significant results obtained for reactions carried out with CoSalen, in various conditions, by using either a double compartment or an undivided electrochemical cell. It clearly appears from these results that both CoSalen complex and FeII cations issued from the anode dissolution are needed to allow the product formation with satisfactory yields (Table 4, run 3).Table 5
Results of the conjugate addition of 2-bromooctane to methylvinylketone, catalyzed by CoISalen−, in DMF solution and with various electrolysis conditions.
Run
Catalyst
Electrolysis conditions
Yield∗ (%)
1
CoSalen
Double separated
<10
Compartment cell
E = −1.2 V/SCE or −1.6 V/SCE
2
CoSalen
Undivided cell
<10
Anode = Al, Mg, Cu
Current density = 0.3 mA·dm−2
3
CoSalen
Undivided cell
43
Anode = Fe
Current density = 0.3 mA·dm−2
4
CoSalen + FeII
Undivided cell
25
Anode = Al
Current density = 0.3 mA·dm−2
5
—
Undivided cell
<10
Anode = Fe
Current density = 0.3 mA·dm−2
∗Yield is calculated by GC analysis with ethyl undecanoate as an internal standard.Table6 reports the results obtained in the reaction of the three classes of alkyl halides with electron deficient olefins under the optimized experimental conditions issued from the above described results. These results show that the addition product yield is low for a primary alkyl bromide (run 1–3) and medium for a secondary (run 4 and 5) or a tertiary alkyl bromide (run 6). The best yields are obtained for the reaction of 2-octyl bromide as secondary alkyl halide either with acrylonitrile (run 9), MVK (run 8), and dimethyl maleate (run 10). The reaction yield is lower if the olefin is disubstitued (run 11–13). Note that same trend has previously been observed in the arylation of activated olefins [32]. In view of these results, it appears that the coupling reaction is regioselective, without formation of 1, 2- addition product. Alkane and alkene which are produced, respectively, by a direct electrochemical reduction and by dehydrohalogenation reaction are the only byproducts observed. Finally, this study shows that the reaction procedure is more efficient when performed with secondary or tertiary alkyl halides than with primary alkyl halides.Table 6
Electroreductive alkylation of activated olefins electrocatalyzed by cobalt-Salen in an undivided cell with an iron anode.
Run
Alkyl bromide
Olefin
N°
Product
Isolated yield (%)
1
1-Bromooctane
1
16
2
1-Bromooctane
1
19
3
1-Bromooctane
2
20
4
2-Bromooctane
3
43
5
Bromocyclohexane
4
37
6
2-Bromo-2-methylpropane
5
33
7
(Bromomethyl)benzene
6
14
8
2-Bromotetradecane
7
52
9
2-Bromooctane
8
50
10
2-Bromooctane
9
50
11
2-Bromooctane
10
8
12
2-Bromooctane
11
<5
13
2-Bromooctane
12
<5
Experimental conditions: anode = Fe; cathode = Ni grid (surface area = 30 cm2); current intensity I = 0.1 A; T = 60°C; solvent = DMF + TBABr (10−2 mol·L−1) + TBAI (8.10−3 mol·L−1); catalyst: CoCl2 (9.4.10−2 mol·L−1) + H2Salen (9.4.10−2 mol·L−1); alkyl bromide = 0.187 mol·L−1; olefin = 0.47 mol·L−1.This observation suggests that radical R• resulted from alkyl halide reduction may be involved in the reaction mechanism [27]. This radical is trapped by the electron deficient olefin added in excess (2.5 equiv.). The heteronuclear CoII-Salen-FeII complex prepared in situ from CoSalen and from the release of FeII cations arising from the oxidation of the anode (equation (2)) is likely the key active species [27].(2)CoII−Salen⇄FeIICoII−Salen−FeIIThis complex is stable enough to promote the electroreductive coupling to some extent. Indeed, the continuous release of iron cations during the process is responsible for the Salen ligand displacement to produce CoII and FeIISalen (equation (3)). These two species do not catalyze the coupling reaction. This unwanted reaction accounts for the relatively moderate yields, around 50% under the optimized conditions.(3)CoII−Salen−FeII⇄FeIIFeII−Salen+CoII


## 4. Conclusion

Ifβ-elimination of HX from alkyl halides is a classic reaction in organic chemistry to get olefins, the described electrosynthesis procedure allows activation of alkyl halides and to some extent the further reaction with electron deficient olefins. From a methodological point of view, the conjugate addition products are obtained from available substrates, and the catalyst is generated in situ from cheap cobalt salt and Salen in an undivided cell fitted with an iron rod. This method based on the use of electricity as green reagent is accompanied by inherent release of iron salt which is not considered as toxic. This investigation also shows the crucial role of the anodically generated metallic cations with a particular emphasis on iron. This study completes advantageously the described voltammetric analysis and confirms the hypothesis of the formation of a catalytically active binuclear Co-Salen-Fe complex during the electrosynthesis.



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