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Zirconia-based catalyst for the one-pot synthesis of coumarin through Pechmann reaction

  • 1, 2,
  • 1, 2Email author,
  • 1, 2 and
  • 1, 2
Nanoscale Research Letters201611:345

https://doi.org/10.1186/s11671-016-1525-3

Received: 7 March 2016

Accepted: 24 June 2016

Published: 26 July 2016

Abstract

Coumarins play an important role in drug development with diverse biological applications. Herein, we present the synthesis of coumarin through Pechmann reaction by using zirconia-based heterogeneous catalysts (ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose) in a solvent-free condition at room temperature. ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose were identified through spectroscopic techniques such as FESEM, X-ray, EDS, XPS, and FT-IR. ZrO2-TiO2 showed the best catalytic performance while ZrO2/cellulose was inactive. The kinetic parameters were observed in a solvent-free condition as well as in toluene and ethanol. The temperature effect was extensively studied which revealed that increasing the temperature will increase the rate of reaction. The rate of reaction in a solvent-free condition, ethanol, and toluene were 1.7 × 10−3, 1.7 × 10−2, and 5.6 × 10−3 g mol−1 min−1, respectively.

Keywords

  • Zirconia
  • Heterogeneous catalyst
  • Coumarin
  • Pechmann reaction
  • Kinetic study
  • Room temperature
  • Solvent-free condition

Background

Heterogeneous catalysts play an extremely important role in the chemical industry which shows its applicability in our daily life [1]. Recently, scientists greatly reverted their attention towards the application of heterogeneous catalyst in the synthesis of important pharmaceutical scaffolds. It was estimated that more than 90 % of the chemical manufacturing depends on the catalytic processes [1]. The design and development of a catalyst with unique morphological and structural characteristics are the main focus in the field of catalysis [2]. The catalytic performance of a catalyst largely depends on the structural features and chemical composition, which in turn affect the active site of the catalyst, approachability of the molecules to the pore size of the catalyst and reactant product mass transport of the molecules [37]. A number of transition and normal element metal oxides (s and p blocks element) was largely used in various fields. Among transition metal oxide, zirconia (ZrO2) played an important role as heterogeneous catalyst, due to its dual nature (both acidic and basic) and semiconductor behavior. These properties attributed the use of zirconia in a number of industrially important chemical reactions (Fig. 1) [8].
Figure 1
Fig. 1

Diagrammatic view of the reaction

Various zirconia-based catalysts were reported for the synthesis of coumarin through Pechmann reaction. Coumarin belongs to a class of flavonoids and a type of benzo-2-pyrone, which is a plant secondary metabolite isolated from natural plants and some microorganisms. For instance, the antibiotic novobiocin, coumermycin A1, and chlorobiocin were isolated from microorganisms [1, 2]. Coumarin acts as a safeguard against viral, bacterial, and fungal attacks, wounds, and stress by a process called phytoalexins [3, 4]. The potential biological applications of coumarin were reported as platelet aggregation inhibition, antibacterial, anticancer, and antioxidant [7, 8]. Coumarin and its derivatives are widely used in synthetic, pharmaceutical, and agrochemicals industries and also used as optical brightening agents, insecticidal, additive in perfumes, and cosmetics [5, 6]. Coumarine serves as an intermediate in the synthesis of several organic reactions, i.e., furocoumarins, chromenes, coumarones, and 2-acylresorcinols [9]. Calanolides, a polycyclic coumarin, exhibited potent anti-HIV (NNRTI) activity and was isolated from genus Calophyllum [10].

The bioavailability of coumarin is sessional and environment dependent, so its production is variable at large scale from the natural resources. However, the remarkable application of coumarin and its derivatives needs it at large scale in medicinal, pharmaceutical, synthetic, and several other industries. Coumarin has been prepared through various strategies such as Perkin [11], Pechmann [12], Reformatsky [11], Knoevenagel [13], Wittig reactions [14], and flash vacuum hydrolysis [15]. Among all these reactions, Pechmann reaction was found as the most effective for this synthesis. Formerly, concentrated H2SO4 was employed for the synthesis of coumarin in Pechmann reaction. Several inorganic reagent and Lewis acid such as P2O5, FeCl3, ZnCl4, POCl3, AlCl3, PPA, HCl, phosphoric acid, trifluoroacetic acid, and montmorillonite clays were used for the synthesis of this scaffold [9]. A number of other catalysts were also successfully reported in the literature for this condensation reaction, i.e., Nafion-H, W/ZrO2 solid acid, zeolite H-BEA, montmorillonite clay, ionic liquids, and Amberlyst-15 [10].

The Pechmann reaction is an acid-catalyzed reaction that proceeds through three main steps. The first step is transesterification, which involved an exchange between phenol and β-ketoester followed by intramolecular hydroxyl alkylation in the second step and elimination of a water molecule in the third step as depicted in Fig. 8 [10, 16]. Therefore, the yield of an acid catalyzes reactions depends on the acidic strength of the catalyst [17].

A large number of reactions are preceded in the presence of hazardous catalysts that deteriorate the climatic condition. Therefore, an environmentally benign alternative catalyst is needed for those reactions that are catalyzed by expensive ionic liquid, hazardous acid, and toxic catalyst [1820]. This need can be fulfilled by the use of a catalyst that not only furnishes the required targets but also is eco-friendly. At present, zirconia got much attention as a solid acid catalyst in terms of their acidic strength, recyclability, and environmental benignity.

Based on the acidic strength of zirconia, we carried out Pechmann reaction with different zirconia-based catalyst (ZrO2-TiO2, ZrO2-ZnO, ZrO2/cellulose) that acts as a solid acid catalyst. The reaction was carried out under the solvent-free condition as well as in ethanol and toluene solvent. The kinetics of the reaction was studied for the first time for this reaction. The structures of the mentioned catalyst were determined by field emission electron microscope (FESEM), energy dispersive X-rays spectrometry (EDS), X-ray diffraction (XRD), and Fourier transform infrared spectroscopy (FT-IR). This method has several advantages such as simplicity of the reaction, solvent-free condition, room temperature, inexpensive starting material, no side product, high yield, high reaction rate, and no toxic waste material.

Experimental

Materials

Reagents such as a salt of zinc and zirconium nitrates, NaOH, cellulose acetate, and TiO2 were purchased from Sigma-Aldrich. Departmental Millipore-Q water purification assembly was used for deionized water. Ethyl acetoacetate and phenols (resorcinol and catechol) were taken from Koch-Light Laboratories Ltd.

Synthesis of Nanomaterial

Synthesis of ZrO2-TiO2

The nanoparticle ZrO2-TiO2 was synthesized according to our previous reports [2124]. The commercially available TiO2 was treated with the aqueous solution of Zr(NO3)2. The solution was basified with 0.1 M NaOH solution till the pH reached 9. The reactants were stirred vigorously for 24 h and the supernatant was removed by centrifugation to isolate the precipitate of ZrO2-TiO2. The procedure of centrifugation is repeated for three times by washing with ethanol. Finally, the resultant precipitate was washed with 1:1 water/ethanol solvent mixture for several times and dried at 50 °C for 24 h in an oven.

Synthesis of ZrO2-ZnO

The ZrO2-ZnO flowers were synthesized by the same method as employed for ZrO2-TiO2. An equimolar mixture of salts of Zn and Zr nitrates were mixed together and increased the pH of the solution above 11 by dropwise addition of 0.1 M NaOH solution. The resultant basified solution was kept on stirring for 24 h at 50 °C. After stirring, the precipitate was washed with ethanol and centrifuged to remove the supernatant solution. The resultant precipitate was finally washed with H2O:C2H5OH (1:1) mixture and then dried in an oven at 50 °C for 24 h.

Synthesis of ZrO2/Cellulose

ZrO2 nanoparticle was grown on the surface of cellulose by adding 1:1 mixture of cellulose and Zr(NO3)2 [25]. The solution mixture was basified with 0.1 M NaOH solution in order to facilitate the formation of the nanoparticle. Finally, the precipitate was centrifuged and washed with 1:1 H2O:C2H5OH mixture and dried at 50 °C in the oven for 24 h.

Characterization of Nanomaterials

The nanomaterials (ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose) were extensively studied through spectroscopic techniques. FESEM, JEOL (JSM-7600F, Japan), was used to find the morphology and average size of the nanomaterials. EDS oxford-EDS system was employed to investigate the elemental composition of the nanomaterials. The structures of nanomaterials were further analyzed by ARL X’TRA X-ray Diffractometer. The functional group in nanomaterial was characterized by FT-IR (Thermo scientific), while kinetics of the reactions were studied by UV/Visible spectrophotometer (Thermo scientific), and the product was identified through melting point (Buchi).

Results and Discussion

Structure Characterization of Nanoparticles

The morphology of ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose was largely characterized by FESEM. ZrO2-TiO2 was grown in the form of particles (Fig. 2a2c) while the ZrO2-ZnO was grown in flower shape (Fig. 2d, 2e). ZrO2-ZnO was basically grown in the form of nanoparticles with an average size of 25–30 nm which aggregate to make a flower-shaped structure. In the case of ZrO2/cellulose, ZrO2 was grown in the form of particles on the surface of cellulose as shown in Fig. 2f.
Figure 2
Fig. 2

FESEM images of ZrO2-TiO2 (a-c), ZrO2-ZnO (d, e), and ZrO2/cellulose (f)

The elemental composition of ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose were performed by EDS spectroscopy as indicated in Fig. 3a3c. The EDS spectrum of ZrO2-TiO2 nanoparticle revealed peaks for O, Ti, and Zr elements, in which the weight of Ti, Zr, and O was 22, 23, and 54 %, respectively, as shown in Fig. 3a. Similarly, ZrO2-ZnO exhibited peaks for O, Zn, and Zr element, having Zn, Zr, and O element in 68, 3, and 28 % by weight as indicated in Fig. 3b. The ZrO2/cellulose displayed peaks for C, Zr, and O element which are 43, 25, and 30 % by weight respectively as shown in Fig. 3c.
Figure 3
Fig. 3

EDS spectrum and elemental composition of ZrO2-TiO2 (a), ZrO2-ZnO (b), and ZrO2/cellulose (c)

Figure 4 shows XRD spectrum of ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose. ZrO2/cellulose nanomaterial has ZrO2 in monoclinic crystalline phase [25]. TiO2/ZrO2 and ZrO2-ZnO nanomaterials contain both TiO2 and ZnO phases along with ZrO2 phase, respectively. By comparing the intensities of two phases in ZrO2-TiO2 and ZrO2-ZnO nanomaterials, it can be seen that TiO2 and ZnO are the major components in ZrO2-TiO2 and ZrO2-ZnO, respectively.
Figure 4
Fig. 4

XRD spectrum of ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose

The functional groups in the nanomaterials (ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose) were explored by FT-IR spectrophotometer as indicated in Fig. 5. The FT-IR spectrum of all the nanomaterials exhibited a peak at around 500 cm−1 indicating stretching vibration for M = O in ZrO2-ZnO, ZrO2-TiO2, and ZrO2/cellulose. The sharp signal for carbonate anions appeared in the FT-IR spectrum of ZrO2-TiO2 and ZrO2-ZnO at 1362 and 1343 cm−1, respectively. The absorption peak at 3450 cm−1 confirmed the presence of OH stretching vibration. The peak for OH stretching vibration is the most prominent in ZrO2-TiO2 and ZrO2/cellulose while it is very weak in ZrO2-ZnO. A prominent peak appeared at 1739 cm−1 suggesting the presence of carbonyl group and the peak at 1224 cm−1 indicating the C–O bond in ZrO2/cellulose. The FT-IR data suggested that ZrO2-ZnO and ZrO2-TiO2 are metal oxides while in the case of ZrO2/cellulose, the ZrO2 is supported by cellulose [10, 15, 25, 26].
Figure 5
Fig. 5

FT-IR analysis of ZrO2-TiO2, ZrO2-ZnO, and ZrO2/cellulose

By the bombardment of X-ray, the number of electrons ejected from the surface of the sample was determined by X-ray photoelectron spectroscopy (XPS) as shown in Fig. 6a6c. ZrO2-TiO2 exhibited peaks for oxygen, titanium, and zirconium (O 1s, Ti 2p, Zr 3P, Zr 3d, and Zr 4P) while ZrO2-ZnO showed peaks for zinc, zirconium, and oxygen (O 1s, Zn 2P, Zn 3P, Zr 3P, Zr 3d and Zr 4p). Similarly, ZrO2/cellulose exhibited peaks for O 1s, C 1s, Zr 3P, and Zr 4P. Ti 2P, Zn 2P, and Zn 3P appeared in the XPS spectra at binding energies of 500.0, 1076, and 91.9 eV, respectively, as depicted in Fig. 6a. Zr 4P, Zr 3d, and Zr 3P appeared in the XPS spectra having binding energies of 350, 329, 37.9, and 1072.3 eV. Similarly, O 1s and C 1s were displayed at 535 and 185.0 eV in the XPS spectra as shown in Fig. 6a. The expanded XPS detailed spectra for all the materials are shown Fig. 6b. One can obviously see in these figures that Zr 3p peaks are shifted towards lower binding energies in both ZrO2-TiO2 and ZrO2-ZnO as compared to Zr 3p peak position in ZrO2/cellulose. Similar shift behavior has been reported [27] and can be attributed to the formation of ZrO2-TiO2 and ZrO2-ZnO binary oxides.
Figure 6
Fig. 6

XPS data of ZrO2-TiO2 (a), ZnO-ZrO2 (b), and ZrO2/cellulose

General Description for the Synthesis of Coumarin

The reaction was carried out between resorcinol and ethyl acetoacetate (1:2) by using 50 mg of the catalyst ZrO2-TiO2 in three-neck round-bottom flask in solvent-free condition at room temperature. The resultant product was formed without side product with a m.p. of 184–187 °C. The diagrammatic view of the reaction is depicted in Fig. 1. The reaction was also carried out between resorcinol and ethyl acetoacetate without a catalyst at 80 °C, but no product is formed as shown in Table 1. ZrO2-TiO2 showed good results as compared to ZrO2-ZnO and ZrO2/cellulose. The ZrO2/cellulose was inactive for this reaction. The reaction was also carried out between catechol and ethyl acetoacetate (1:2) with 50 mg of the catalyst ZrO2-TiO2 in a solvent-free condition. After 4 h, the reaction between catechol and ethyl acetoacetate gives 55 % yield at 80 °C but failed at room temperature as shown in Table 1. The reaction gives good yield with electron donating group such as resorcinol while failed with electron withdrawing group O-nitrophenol as shown in Table 1. Due to the strongest catalytic performance of ZrO2-TiO2 with resorcinol and ethyl acetoacetate, we further select this catalyst for the detailed study of this reaction. The reaction between resorcinol and ethyl acetoacetate (1:2) with 50 mg of the catalyst ZrO2-TiO2 was studied in a polar solvent (ethanol) and non-polar solvent (toluene) by varying the temperature condition (Table 2). The use of solvent-free condition is a better way while using a heterogeneous catalyst. Prior to the use of a catalyst, the reaction was carried out between resorcinol and ethyl acetoacetate in the absence of a catalyst in a solvent-free condition, toluene, and ethanol, but no product is formed. This confirms that solvent or temperature have no role; only catalyst played a central role in this reaction.
Table 1

The reaction in solvent-free condition at room temperature

Entry

Reactant

Catalyst

Temperature (°C)

Time (min.)

%Yield

M.P.

1

Resarcinol + ethylacetoacetate

ZrO2-TiO2

R.T.

180

97

184–187

2

Resarcinol + ethylacetoacetate

ZrO2-ZnO

R.T.

240

63

184–187

3

Resarcinol + ethylacetoacetate

ZrO2/cellulose

R.T.

180

N.R.

4

Catechole + ethylacetoacetate

ZrO2-TiO2

80

240 min

55

 

5

O-nitrophenol + ethylacetoacetate

ZrO2-TiO2

80

240

N.R.

 

6

Resarcinol + ethylacetoacetate

Without catalyst

80

240

N.R.

N.R. no reaction, M.P. melting point

Table 2

Comparison of the present work with literature data

Entry

Catalyst

Time (min.)

Temperature (°C)

Solvent

Yield

References

1

Zeolite BEA

240

130

PhNO2

63

[29]

2

PFPAT

180

110

Toluene

90

[30]

3

MFRH

50

80

S.F.

65

[30]

4

Nanoreactors

60

130

S.F.

30

[30]

5

CMK-5-SO3H

20

130

S.F.

95

[7]

6

CMK-5

60

130

S.F.

10

[7]

8

ZrO2-TiO2

180

Room temperature

S.F.

97

This work

9

ZrO2-TiO2

110

60

Toluene

95

This work

10

ZrO2-TiO2

150

60

Ethanol

92

This work

PhNO 2 nitrophenol, S.F. solvent-free condition

Temperature Effect

The temperature effect was observed on the reaction ZrO2-TiO2 (50 mg) in the presence of toluene and ethanol. It was observed that increasing the temperature will decrease the time for reaction completion as indicated in Tables 3 and 4.
Table 3

Effect of temperature in toluene solvent

Entry

Reactant

Catalyst

Temperature (°C)

%Yield

Time (min.)

1

Resarcinol + ethylacetoacetate

ZrO2-TiO2

100

95

20

2

Resarcinol + ethylacetoacetate

ZrO2-TiO2

80

95

35

3

Resarcinol + ethylacetoacetate

ZrO2-TiO2

60

95

110

4

Resarcinol + ethylacetoacetate

ZrO2-TiO2

45

83

130

5

Resarcinol + ethylacetoacetate

ZrO2-ZnO

100

70

30

6

Resarcinol + ethylacetoacetate

ZrO2-ZnO

80

63

50

7

Resarcinol + ethylacetoacetate

ZrO2-ZnO

60

55

140

8

Resarcinol + ethylacetoacetate

ZrO2-ZnO

45

40

170

9

Resarcinol + ethylacetoacetate

Without catalyst

80

N.R.

240

N.R. no reaction

Table 4

Effect of temperature in an ethanol solvent

Entry

Reactant

Catalyst

Temperature (°C)

%Yield

Time (min.)

1

Resarcinol + ethylacetoacetate

ZrO2-TiO2

100

97

20

2

Resarcinol + ethylacetoacetate

ZrO2-TiO2

80

95

50

3

Resarcinol + ethylacetoacetate

ZrO2-TiO2

60

92

150

4

Resarcinol + ethylacetoacetate

ZrO2-TiO2

45

80

160

5

Resarcinol + ethylacetoacetate

ZrO2-ZnO

100

74

40

6

Resarcinol + ethylacetoacetate

ZrO2-ZnO

80

67

60

7

Resarcinol + ethylacetoacetate

ZrO2-ZnO

60

60

120

8

Resarcinol + ethylacetoacetate

ZrO2-ZnO

45

43

150

9

Resarcinol + ethylacetoacetate

Without catalyst

80

N.R.

240

N.R. no reaction

Ethyl acetoacetate and resorcinol (1:2) was used as starting materials for the synthesis of coumarin along with 50 mg of the catalyst.

UV/Visible Data

The increase in product concentration was monitored gradually by taking the UV/Visible spectra periodically. A bathochromic shift was observed for the product, due to an increased conjugation as compared to the reactant. However, the product showed a different bathochromic shift in ethanol and toluene solvent. The bathochromic shift (increase in wavelength) was observed in ethanol at 372 nm while the same product appeared at 317 nm in toluene. In the presence of non-polar solvent (toluene), polar molecule showed hypsochromic shift due to n-π transition because it stabilizes the ground state more as compared to the excited state; therefore, a high amount of energy is required to promote an electron from the highest occupied molecular orbital (HOMO) of non-bonding orbital to the lowest unoccupied molecular orbital (LUMO) of antibonding π orbital, and so the wavelength is decreased. However, polar solvent (ethanol) forms hydrogen bonding to the excited state of the product (coumarin), which stabilizes the transition state of the product more as compared to the ground state. Therefore, less amount of energy is required to promote an electron from HOMO of non-bonding orbital to the LUMO of the antibonding π orbital and thus increasing the wavelength as shown in Fig. 7a.
Figure 7
Fig. 7

a UV/Vis data of ZrO2-TiO2 in solvent-free condition at room temperature. b Kinetics of ZrO2-TiO2 in solvent-free condition. c Kinetics of ZrO2-TiO2 in toluene and ethanol solvent at 60 °C

Kinetics of the Reaction

The kinetics was studied in solvent-free condition, ethanol, and toluene in the presence of ZrO2-TiO2 catalyst. The rate of reaction in solvent-free condition at room temperature was 1.7 × 10−3 g mol−1 min−1, while at 60 °C the rate of reaction in ethanol is 1.7 × 10−2 g mol−1 min−1 and toluene 5.6 × 10−3 g mol−1 min−1 as shown in Fig. 7a7c.

Mechanism of the Reaction

Several mechanisms were put forward for the synthesis of coumarin. In the whole scenario, one C–O and one C–C bond are generated by the reaction of phenol with β-ketoester [28]. During C–C bond formation, the metal in the nanocatalyst chelates with β-ketoester, followed by Friedel-Craft cyclization in which the π-electron of the benzene ring of phenol attacks the carbonyl carbon of β-ketoester to form an unstable anti-aromatic species (4n electron system). This highly unstable anti-aromatic species restore its aromaticity (4n + 2π electron system) by losing hydrogen atom. Transesterification occurred in the next step followed by condensation to form C–O bond as depicted in Fig. 8.
Figure 8
Fig. 8

Tentative mechanism for the synthesis of coumarin

Conclusions

In the present study, zirconia-based catalysts (ZrO2-TiO2, ZrO2-ZnO, ZrO2/cellulose) were synthesized for the one-pot synthesis of coumarin. The ZrO2-TiO2 showed strongest catalytic performance for this reaction as compared to ZrO2-ZnO. At room temperature, the rate of reaction in solvent-free condition is 1.7 × 10−3 g mol−1 min−1. However, at 60 °C, the rate of reaction in ethanol is 1.7 × 10−2 and toluene 5.6 × 10−3 g mol−1 min−1. The rate of reaction was increased by increasing the temperature of the reaction. The bathochromic shifts was observed in the UV/Visible spectrum of the ethanol. The product appeared at λ max 372 nm in the presence of the ethanol as it stabilized the excited state of the polar molecule (coumarin). Similarly, the product appeared at λ max 317 nm in toluene solvent as it stabilizes the ground state of the polar molecule (coumarin).

Declarations

Acknowledgements

The authors are grateful to the Center of Excellence for Advanced Material Research (CEAMR), King Abdulaziz University, Saudi Arabia, for providing research facilities.

Authors’ contributions

Shahid design and carried out all experiments and write the manuscript. Sher helps in experiment and revised the manuscript Abdullah also revised the manuscript and provide experimental facilities while Ikram help in experiment. All the authors read and approved the final manuscript.

Competing Interests

The authors declare that they have no competing interests.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (http://creativecommons.org/licenses/by/4.0/), which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

(1)
Chemistry Department, Faculty of Science, King Abdulaziz University, Jeddah, Saudi Arabia
(2)
Center of Excellence for Advanced Materials Research (CEAMR), King Abdulaziz University, Jeddah, Saudi Arabia

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