Expeditious oxidation of alcohols to carbonyl compounds using iron(III) nitrate

Article abstract of DOI:10.1016/j.tetlet.2007.10.068

An efficient and solvent-free protocol for the oxidation of alcohols to corresponding carbonyl compounds using iron(III) nitrate nonahydrate has been developed.

Full text of DOI:10.1016/j.tetlet.2007.10.068

Available online at www.sciencedirect.com
Tetrahedron Letters 48 (2007) 8839–8842
Expeditious oxidation of alcohols to carbonyl compounds
using iron(III) nitrateI
Vasudevan V. Namboodiri, Vivek Polshettiwar and Rajender S. Varma*
Clean Processes Branch, National Risk Management Research Laboratory, U.S. Environmental Protection Agency,
26 W. Martin Luther King Drive, MS 443, Cincinnati, OH 45268, USA
Received 20 September 2007; revised 10 October 2007; accepted 12 October 2007
Available online 18 October 2007
Abstract—An efficient and solvent-free protocol for the oxidation of alcohols to corresponding carbonyl compounds using iron(III)
nitrate nonahydrate has been developed.
ꢀ 2007 Elsevier Ltd. All rights reserved.
The oxidation of alcohols to the corresponding carbonyl
compounds is one of the most important transforma-
tions in organic synthesis. There are numerous methods
available in the literature1 and the development of new
selective oxidative protocols is still considered a chal-
lenge.2 This void was filled, in part, by using a set of
clay-supported metal nitrate salts such as iron(III)
nitrate supported on clay, clayfen,3,4 and on zeolites,
zeofen,5 which are known for various applications includ-
ing oxidation of alcohols. The main drawbacks of clay-
fen and other related solid supported metal nitrate salts
in oxidative transformations are the use of large excess
of solvents, reflux reaction conditions, longer reaction
times, high ratio of reagent to substrate, and the gener-
ation of solid waste (40–50 g/mol). Varma and Dahiya
were able to eliminate solvents from these oxidations by
employing microwave heating which also helped to
reduce the reaction time from hours to seconds.2b
oxidation of secondary aliphatic, alicyclic, and benzylic
alcohols (Scheme 1).
Numerous reports have been described for the enhanced
oxidative potential of metal nitrates on various mineral
oxide supports.3–5 We decided to investigate the proper
control reactions in the absence of any solvent or sup-
port. In order to render these oxidations economically
more viable and simpler, we focused our attention on
iron(III) nitrate nonahydrate which is abundant, cheap,
and relatively nontoxic.3 Benzyl alcohol was used as a
model compound to evaluate the oxidative potential of
OH
Benzhydrol
Iron (III) nitrate
80 ºC
Iron (III) nitrate
55 ºC
In our continued quest for the development of environ-
mentally friendly alternatives,6 we sought to develop an
improved methodology which minimizes the use of any
solvent or support and requires a low catalyst/substrate
ratio. Herein, we describe this facile approach for the
O
Oxidative cleavage
80
O
º
C
Keywords: Iron(III) nitrate; Oxidation; Solvent-free reaction; Alcohols;
Carbonyl compounds.
q Presented, in part, at the IUPAC CHEMRAWN XIV Conference on
Green Chemistry: Towards Environmentally Benign Processes and
Products, Boulder, Colorado, June 9–13, 2001.
Benzophenone (100%)
Ether (100%)
*
Scheme 1. Iron(III) nitrate catalyzed oxidation of alcohol under
Corresponding author. Tel.: +1 513 487 2701; fax: +1 513 569
solvent-free condition.
7677; e-mail: Varma.Rajender@epa.gov
0040-4039/$ - see front matter ꢀ 2007 Elsevier Ltd. All rights reserved.
doi:10.1016/j.tetlet.2007.10.068

8840
V. V. Namboodiri et al. / Tetrahedron Letters 48 (2007) 8839–8842
Table 1. Reactivity trend of nitrate salts in the oxidation of benzyl
alcohol
Table 3. Effect of temperature on the benzyl alcohol oxidation with
iron nitratea
Entry Nitrate
Time
Temperature GC conversion
Entry
Temperature
(ꢁC)
Time
(min)
GC conversion
(%)
Isolated
yield (%)
(1 mmol) (min) (ꢁC)
(isolated yield) (%)
1
2
3
4
Fe
Cu
Zn
NH4
15
25
60
80
90
90
90
100 (97)
88 (91)
<20
1
2
3
4
5
30
50
60
70
80
240
30
15
10
5
<60
>90
>90
>90
>90
52
95
96
96
96
240
<5
a 0.66 mmol of Fe(NO3)3 per mmol of alcohol was used.
various nitrate salts and for optimizing the reaction con-
ditions (Table 1).
rate became relatively faster above the melting point of
iron nitrate nonahydrate due to increased homogeneity
of the reactant (Table 3).
Iron nitrate nonahydrate showed better reactivity than
copper nitrate at lower temperature and was selected
for the detailed investigations. The melting point of iron
nitrate nonahydrate is only 48 ꢁC and it is miscible with
the benzyl alcohol at this temperature. This makes the
oxidation a homogeneous catalytic reaction and the for-
mation of benzaldehyde can be visibly seen as a separate
layer that forms during the course of the reaction.
Copper nitrate was also equally effective but its higher
melting point requires an elevated reaction temperature
and relatively longer reaction time when compared to
iron nitrate. The oxidative protocol involves the liberation
of brown fumes of nitrogen dioxide which ceases upon
completion of the oxidation.3b
Effect of oxygen atmosphere on the benzyl alcohol oxi-
dation showed that under oxygen pressure iron nitrate
can be used in less quantity than the stoichiometric
amount (Table 4).
Using these optimized reaction conditions,7 the effi-
ciency of this approach was studied for the oxidation
of various benzylic alcohols and the results are summa-
rized in Table 5. All benzylic alcohols gave excellent
conversion, but chloro-, fluoro-, and bromo-substituted
benzylic alcohols were less reactive than the correspond-
ing benzyl alcohol with the reactivity order, Cl < Br < F
(entries 1–5). Oxidation of 1,4-benzenedimethanol deliv-
ered exclusively the corresponding 1,4-phthalaldehyde
while 1,2-benzenedimethanol gave 65% of aldehyde
and 35% isobenzofuranone (entry 8).
Since the iron nitrate and copper nitrate impregnated on
solid support are effective as oxidants, we questioned the
theory based on the premise that the oxidation rate
enhancements are due to their impregnation on the solid
supports.3 The earlier control experiments may have the
following drawback: a large excess of non-polar solvent
pentane was used as the reaction medium in which iron
nitrate is completely insoluble thus reducing the proba-
bility of interaction with the substrate. Undoubtedly, the
impregnation of iron nitrate on solid support helped to
disperse the oxidant and presumably polar alcohols got
trapped on the support to facilitate the reaction.
On close analysis of the reaction, we found that trace
amount of dibenzyl ether was formed during the oxida-
tion of benzyl alcohol. The amount of the benzyl ether
was higher at lower temperature indicating that the reac-
tion mechanism may involve the formation of ether as
an intermediate. A control experiment of the oxidation
of benzyl ether with iron nitrate was conducted at
60 ꢁC for 15 min that resulted in benzaldehyde. Simi-
larly, the oxidation of benzhydrol at 50 ꢁC led to the
quantitative formation of a white solid; the 13C and
1H NMR spectra and CHN analysis confirmed that
the intermediate was the ether of benzhydrol. This
benzhydrol ether also underwent oxidative cleavage to
benzophenone above 65 ꢁC. The rate of oxidation was
increased with temperature and a complete conversion
was obtained at 80 ꢁC. Direct heating of benzhydrol at
80 ꢁC for 30 min also gave complete conversion to benzo-
The amount of iron nitrate required for the complete
conversion is shown in Table 2, which indicates that
ꢀ0.66 mmol of iron nitrate was adequate for the safe
conversion of benzyl alcohol to benzaldehyde and is in
agreement with the earlier proposed mechanism that re-
quires at least two nitrate groups for the completion of
oxidation.3c
The reaction rate was slow at room temperature and
increased with the rise in temperature and the oxidation
Table 4. Effect of oxygen atmosphere in the oxidation of benzyl
alcohol
Table 2. Optimization of amount of iron nitrate for the oxidation of
benzyl alcohol to benzaldehydea
Alcohol Fe(NO3)3 Temperature Pressure Time GC yield
Entry Benzyl alcohol Iron nitrate GC conversion Isolated
(mmol) (mmol)
(ꢁC)
(bar)
(h)
(%)
(mmol)
(mmol)
(%)
yield (%)
5
10
50
50
50
50
1.00
1.00
1.00
1.00
1.00
1.00
80
80
50
60
80
60
1
1
20
20
20
20
1
1
5
5
5
5
>95
55
23
36
56
10a
1
2
3
4
5b
1
1
1
1
1
1.5
1
0.66
0.33
1
100
100
100
76
96
96
96
72
0
0
a The reaction was carried out at 60 ꢁC for 30 min.
a 2 ml water was added to check the effect of water.
b 1 mL of water as reaction medium.

V. V. Namboodiri et al. / Tetrahedron Letters 48 (2007) 8839–8842
Table 5. Iron nitrate catalyzed oxidation of substituted benzyl alcohols
8841
Entry
Alcohol
Fe(NO3)3 (mmol)
Temperature (ꢁC)
Time (min)
GC yield (isolated) (%)
1
2
3
4
5
6
7
8
9
4-F–benzyl alcohol
4-F–benzyl alcohol
4-Cl–benzyl alcohol
4-Br–benzyl alcohol
4-Cl–benzyl alcohol
1,4-benzenedimethanol
Naphthalene 2-methanol
1,2-Benzenedimethanol
Benzylether
0.66
0.66
0.66
0.66
0.66
1.32
1.00
1.32
0.66
1.00
1.00
60
60
60
60
60
60
60
60
60
80
50
15
30
15
15
30
15
30
15
15
30
15
76 (70)
100 (94)
60 (57)
70 (65)
100 (95)
100 (96)
100 (96)
100 (65,35)a
100 (95)
100 (95)
100b (98)
10
11
Benzhydrol
Benzhydrol
a 35% of the product is isobenzofuranone.
b Complete conversion to ether of benzhydrol.
Table 6. Oxidation of alcohols using iron(III) nitrate
Entry
Alcohol (1 mmol)
Fe(NO3)3 (mmol)
Temperature (ꢁC)
Time (min)
GC yield (%)
1
2
3
4
5
6
7
8
Norboneol
tert-Butylcyclohexanol
Isoborneol
1-Phenylethanol
Benzoin
Pinacol
1.00
1.00
1.00
1.00
1.00
0.66
0.66
0.66
80
80
80
60
60
80
60
60
30
30
30
30
30
5
69
60
85
52a
95
53
54
60
Pent-2-ol
Hexan-1-ol
30
30
a 32% is the ether of 1-phenylethanol.
phenone. These observations reveal that the formation
of ether via dehydration is the first step in the oxidation
of alcohols prior to the conversion to the corresponding
aldehyde/ketone. This may be a reason that the clayfen-
based method gave only about 78% benzaldehyde from
benzyl alcohol in which the proximity of the alcohol
molecules to form ether is rather limited.
support and delivered excellent yields without over oxi-
dation, and with minimum generation of waste. This
oxidative protocol can also be used to nitrate phenol,
toluene, and styrene and for the selective oxidation of
styrene to benzaldehyde.10
Acknowledgments
The thermogravimetric analysis of iron nitrate showed
that it is stable up to 120 ꢁC and then starts decompos-
ing.8 Under our mild reaction conditions with moderate
temperature the iron nitrate was stable enough and did
not produce completely anhydrous condition that mini-
mizes the possibility of explosion. The oxidations of
other alcohols were studied at different reaction condi-
tions and the results are summarized in Table 6. Primary
aliphatic alcohols, however, gave a mixture of products
which is in agreement with the earlier observations.3
V.V.N. and V.P. are postgraduate research participants
at the National Risk Management Research Laboratory
administered by the Oak Ridge Institute for Science and
Education through an interagency agreement between
the US Department of Energy and the US Environmen-
tal Protection Agency.
References and notes
The literature reports also show that supported reagents
such as clayfen may induce alkylation reactions in com-
petition with the oxidation reactions.9 In contrast, the
present method using only iron nitrate selectively
oxidized benzyl alcohols to benzaldehydes.
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Tetrahedron Lett. 2003, 44, 549; (e) Hu, J.; Chen, L.; Zhu,
K.; Suchopar, A.; Richards, R. Catal. Today 2007, 122,
277.
Conclusion
Relatively inexpensive iron nitrate nonahydrate was
used in the oxidation of benzyl alcohols and various sec-
ondary alcohols to generate the carbonyl compounds.
The reaction occurred simply by warming the alcohol
with the iron nitrate in the absence of any solvents or
2. (a) Delaude, I.; Lazlo, P. J. Org. Chem. 1996, 61, 6360; (b)
Varma, R. S.; Dahiya, R. Tetrahedron Lett. 1997, 38,
´
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V. V. Namboodiri et al. / Tetrahedron Letters 48 (2007) 8839–8842
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3 mmol) was admixed with Fe(NO3)3Æ9H2O (0.771 g,
1.98 mmol) in a 10 mL test tube equipped with a magnetic
stirrer bar and warmed at 80 ꢁC for 15 min on a water
bath. The progress of the reaction was followed by using
GC–MS and TLC. Upon completion of the reaction,
mixture was cooled to room temperature and 0.5 mL
water was added. The product was extracted with ether
(3 · 3 mL) and the ether layer was dried over anhydrous
magnesium sulfate and solvent removed under reduced
pressure on a rotary evaporator (0.316 g, 99%). The pure
benzaldehyde was obtained by filtering through a short
silica gel pad (0.310 g, 97%).
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