# Mg(HSO4)2/SiO2 as a Highly Efficient Catalyst for the Green Preparation of 2-Aryl-1,3-Dioxalanes/Dioxanes and Linear Acetals

Authors: Fariba Jafari; Saeed Khodabakhshi
Journal: Organic Chemistry International
 (2012)

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## Abstract

Silica-supported magnesium hydrogen sulfate has been used as a recyclable catalyst for the synthesis of some linear and cyclic aromatic acetals under solvent-free conditions. This environmentally friendly method has advantages, such as high yield of products, simple work-up procedure, and avoidance of the organic solvents, which will contribute in serving as a green process greatly.


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## Body

## 1. Introduction

Recently, silica supported catalysts have attracted the special attention of chemists [1–3] due to their eco-friendly nature, simple handling, recyclability, and high reactivity [4–6]. Similarly, protection of carbonyl functionaries from nucleophilic attack is one of the major problems faced during multistep syntheses. These problems remain a crucial challenge to organic chemists. A suitable method for solving this problem is the acetalization of carbonyl functions since acetals and 1,3-dioxanes are stable under neutral and basic conditions [7, 8]. Besides the interest in acetals as protecting groups, many of them can serve for fragrances in cosmetics, pharmaceuticals, detergents, lacquer industries, and applications as food and beverage additives [9–11].Until now, several methods for the acetalization of the carbonyl function have been reported using ionic liquids [12–15], protonic acids such as HCl and H2SO4 and Lewis acids [16–19], and transitional metal complexes including Rh, Pd, and Pt [20, 21]. Some of these strategies suffer from the drawback of green chemistry, and have been associated with several shortcomings such as use of corrosive protic acids and unrecyclable catalyst, long-reaction times and low product yields, difficult work-up procedure, and the use of organic solvents. Therefore, presentation of a new, inexpensive and eco-friendly method for the protection of carbonyl functionality is an important topic, and one which is an active ongoing research area. There is a scope for the further improvement towards green reaction conditions and improved yields. We wish to report here a green and simple method for the protection of aromatic aldehydes 1 by diols 2 or aromatic alcohols 3 as 1,3-dioxanes, 1,3-dioxalanes 4, and linear acetals 5 using a catalytic quantity of silica supported magnesium hydrogen sulfate under solvent-free conditions in excellent yields (Scheme 1).Scheme 1
Acetalization of aromatic aldehydes using Mg(HSO4)2/SiO2.


## 2. Results and Discussion

A solvent-free reaction reduces pollution and cost due to simplification of experimental procedure, work-up technique, and saving of labour. To exploit simple and suitable conditions for the synthesis of4 and 5 using Mg(HSO4)2/SiO2 as an efficient solid acid catalyst, the treatment of benzaldehyde and ethanediol was chosen as a model reaction (Scheme 2). Firstly, we found that in the absence of catalyst, the reaction did not proceed even at a high temperature (25–90°C). After examining the various amounts of Mg(HSO4)2/SiO2, we found that the condensation reaction can be efficiently carried out by adding 0.2 g of the catalyst under grinding conditions at room temperature in a short time span of 10 min. The use of excessive amounts of the catalyst does not increase the yield or reaction rate (Table 1).Table 1
Optimization of the amounts of Mg (HSO4)2/SiO2 under solvent-free conditions for the reaction of benzaldehyde with ethandiol.
Entry
catalyst amount (g)
Time (min)
Yield (%)a
Temp. (°C)
1
0.03
120
60
rt
2
0.05
120
75
rt
3
0.1
25
80
rt
4
0.2
5
98
rt
5
0.5
15
95
rt
aIsolated yields.Scheme 2
The reaction of benzaldehyde and ethanediol under solvent-free conditions.After optimization, the scope of this reaction was examined using a variety of aromatic aldehydes and aromatic alcohols and diols. It was found that both electron rich and electron poor aldehydes reacted well in this process to afford the corresponding products4and5 in excellent yields. The obtained results are summarized in Table 2.Table 2
Synthesis of4and5 using Mg(HSO4)2/SiO2 under solvent-free conditions.
Entry
Product
Time (min)
Yield (%)a
[References]
4a
10
98
[14]
4b
10
95
[13]
4c
10
92
[26]
4d
18
90
[26]
4e
15
90
[13]
4f
12
87
[26]
4g
10
90
[13]
4h
12
90
[14]
4i
8
92
[27]
4j
16
95
[27]
4k
15
90
[14]
5a
5
95
[19]
5b
5
97
[27]
5c
10
95
[27]
5d
7
97
[27]
aIsolated yields.The main advantages of the presented protocol over existing methods can be seen by comparing our results with those of some previous reported procedures, as shown in Table3 (Scheme 3).Table 3
Comparison of our method with previous reported method in the synthesis of4a.
Entry
Conditions (catalyst/temperature (°C)/solvent)
Time (min)
Yield (%)a
[References]
1
Ionic liquid [SOClMIm]Cl/40/-
1200
80
[15]
2
In(OTf)3/80 (reflux)/Benzene
180
92
[18]
3
Multi-SO3H functionalized ionic liquids/25/-
180
96.5
[13]
4
SG-[(CH2)3SO3H-HIM]HSO4
90
95
[12]
5
Ionic liquid [TMPSA]HSO4/25/-
30
77
[14]
6
SiO2-SO3H/68 (reflux)/n-hexane
60
58
[28]
7
Mg(HSO4)2/SiO2
10
98
This workScheme 3
The reaction of benzaldehyde and ethanediol under various conditions.As can be concluded from Table3, the present method is more appropriate than the others due to its excellent product yield in shorter reaction time without using organic solvents. In many cases, in order to achieve fast synthesis in an organic process, a catalyst must be used. The need to implement green chemistry principles (e.g., safer solvents, less hazardous chemical synthesis, atom economy, and catalysis) is a driving force towards the development of safe and reusable catalysts and avoidance of the use of organic solvents [22–25]. In this protocol, Mg(HSO4)2/SiO2 acts as a safe, highly efficient, and recyclable catalyst under solvent-free conditions. It should be also mentioned that our efforts on the acetalization of aliphatic aldehydes and ketalization of aromatic ketones using silica supported magnesium hydrogen sulfate under similar conditions were unsuccessful. The problem with alkyl aldehydes is likely to be a result of their being enolizable. To conclude, we present a new and green method for the synthesis of 1,3-dioxanes, 1,3-dioxalanes, and linear acetals by employing silica supported magnesium hydrogen sulfate as a safe, inexpensive, and reusable solid acid catalyst under solvent-free conditions. Higher yields and shorter reaction times than the classical methods, and simple work-up procedure are the appealing attributes of this work.


## 3. Experimental Section

### 3.1. General.

Chemicals were purchased from Fluka, Merck, and Aldrich chemical companies. Yields refer to isolated pure products. The products were characterized by comparison of their spectral (IR and1H-NMR) and physical data with authentic samples which were produced by other reported procedures.


### 3.2. Preparation of Silica Supported Magnesium Hydrogen sulfate

A 50 mL suction flask was equipped with a constant-pressure dropping funnel. The gas outlet was connected to a vacuum system through an adsorbing solution (water) and an alkali trap. Anhydrous magnesium chloride (4.0 g, 40 mmol) was charged in the flask and concentrated sulfuric acid (98%, 7.35 g, 40 mmol) was added dropwise over a period of 30 min at room temperature. HCl evolved immediately. After completion of the addition, the mixture was shaken for 30 min, while the residual HCl was eliminated by suction. The Mg(HSO4)2 (6.46 g) was obtained as white gel. The obtained solid acid was mixed by silica gel 40 (6.43 g).


### 3.3. General Procedure for the Synthesis of4 and 5

A mixture of 1 mmol of aldehyde, 1.5 mmol of diol or 2 mmol of aromatic alcohol, and Mg(HSO4)2/SiO2 (0.2 g) was added to a mortar. The mixture was thoroughly ground with a pestle at room temperature. The progress of the reaction was monitored by TLC (EtOAc/hexane, 1 : 3). After completion of the reaction, the mixture was dissolved in CHCl3 (2 × 10 mL) and the catalyst was filtered. After evaporation of the solvent under reduced pressure and addition of ethanol and water, almost pure 4 and 5 were obtained in 90–98%. Further purification was achieved by recrystallization from the appropriate solvent. The catalyst was washed with diethyl ether, dried at 70°C for 45 min and reused in another reaction.


## 3.1. General.

Chemicals were purchased from Fluka, Merck, and Aldrich chemical companies. Yields refer to isolated pure products. The products were characterized by comparison of their spectral (IR and1H-NMR) and physical data with authentic samples which were produced by other reported procedures.


## 3.2. Preparation of Silica Supported Magnesium Hydrogen sulfate

A 50 mL suction flask was equipped with a constant-pressure dropping funnel. The gas outlet was connected to a vacuum system through an adsorbing solution (water) and an alkali trap. Anhydrous magnesium chloride (4.0 g, 40 mmol) was charged in the flask and concentrated sulfuric acid (98%, 7.35 g, 40 mmol) was added dropwise over a period of 30 min at room temperature. HCl evolved immediately. After completion of the addition, the mixture was shaken for 30 min, while the residual HCl was eliminated by suction. The Mg(HSO4)2 (6.46 g) was obtained as white gel. The obtained solid acid was mixed by silica gel 40 (6.43 g).


## 3.3. General Procedure for the Synthesis of4 and 5

A mixture of 1 mmol of aldehyde, 1.5 mmol of diol or 2 mmol of aromatic alcohol, and Mg(HSO4)2/SiO2 (0.2 g) was added to a mortar. The mixture was thoroughly ground with a pestle at room temperature. The progress of the reaction was monitored by TLC (EtOAc/hexane, 1 : 3). After completion of the reaction, the mixture was dissolved in CHCl3 (2 × 10 mL) and the catalyst was filtered. After evaporation of the solvent under reduced pressure and addition of ethanol and water, almost pure 4 and 5 were obtained in 90–98%. Further purification was achieved by recrystallization from the appropriate solvent. The catalyst was washed with diethyl ether, dried at 70°C for 45 min and reused in another reaction.



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*Source: 475301-2012-08-22.xml*