Reduction of azides to amines with zinc metal
in near-critical water
Wang Lei, Li Pinhua, Yan Jincan, Chen
Jianhui
(Department of Chemistry, Huaibei Coal Teachers College, Huaibei, Anhui 235000, China)
Received Dec. 16, 2002; Supported by
the National Natural Science Foundation of China (No. 20172018), the Excellent Scientist
Foundation of Anhui Province (No. 2001040), the Natural Science Foundation of the
Education Department of Anhui Province (No. 2002kj254zd), the Scientific Research
Foundation for the Returned Overseas Chinese Scholars, State Education Ministry (No.
2002247) and State Key Laboratory of Organometallic Chemistry, Shanghai Institute of
Organic Chemistry, Chinese Academy of Sciences (No.2002-34).
Abstract Zinc metal in
near-critical water (250ºC) reduces azides to
amines in good yields.
Keywords azides, amines, zinc metal, reduction, near-critical water (NCW)
1 INTRODUCTION
Organic reactions carried out in water have received much more attention in last decade[1-3].
Unfortunately, the limitation of water as solvent in organic synthesis is its poor
dissolving ability for most organic compounds at ambient temperature. On the other hand,
the unique properties of water near its critical point (Tc = 374ºC, Pc = 221 bar) have promoted researchers to use
it instead of organic solvents in organic synthesis. As water is heated towards its
critical point, it changes from a polar liquid to an almost non-polar fluid. Its
dielectric constant e decrease from 78.5 at room temperature to 20 at 275ºC, favoring the solubility of organics and ions. Its dissociation
constant, Kw, increases several orders of magnitude from ambient to
near-critical conditions (Kw = 10¨C11 at 275 ºC), providing hydronium and hydroxide ions that can act as the modest acid or
base in chemical reactions[4-5]. Although much of supercritical water research
has been focused on the total oxidation of organic compounds and geochemical modeling[6-8],
there are increasing number of
papers which suggest that near-critical water (250-325ºC) used as excellent solvent for organic reactions
because organic reactions in near-critical water offer many advantages over those in
traditional organic solvents. For example, it is environmentally benign and also easy for
the product separation[9,10].
Amines, widely used as important intermediates in the synthesis of
chemicals such as dyes, antioxidants, photographic, pharmaceutical and agricultural
chemicals, can be obtained easily from the reduction of azides using catalytic
hydrogenation and a variety of other reducing agents with good regio-, stereo- and
enantioselectivity. For example, zinc borohydride, samarium-iodine, diboranes, lithium
aminoborohydride, iodotrimethylsilane and benzyltriethylaminonium
tetrathiomolybdate have been recommended for this transformation[11-13].
However, most of them are carried out in organic solvents, which pose waste handling
problems. Because of its low cost and easy availability, zinc has been employed in
Barbier-type reaction, C-S coupling, reductive coupling cyclization reaction[14-18].
Here we report the reduction of azides with metallic zinc powder in near-critical water
(NCW) at 250ºC, which could
generate amines in good yields.
Scheme 1
2 EXPERIMENTAL
Melting points were measured on a WRS-1A melting point apparatus without calibration. 1H
NMR spectra were recorded on a 300 MHz Bruker AZ 300 spectrometer. Chemical shift was
given as d value with
reference to tetramethylsilane (TMS) as internal standard. IR spectra were obtained by
using a Nicolet NEXUS 470 spectrophotometer. The reagents were commercially available
without purification prior to use.
The reduction of azides with metallic zinc in near-critical water was
carried out as the following procedure: Azide (1.00 mmol) and metallic zinc powder (196
mg, 3.00 mmol) were added to a stainless steel reactor charged with tap water (10 mL)
under nitrogen atmosphere. The reactor was heated and remained at 250ºC for 3 h. After cooling, ether (10 mL¡Á2) was added to extract the
products. The organic layer was dried with anhydrous sodium sulfate, then the solvents
were evaporated under reduced pressure. The product was purified by flash chromatography
to yield amine.
Aniline£ºOil. 1H
NMR (CDCl3): d
7.23 (t, 2H, J = 8.6 Hz), 6.78 (m, 3H), 3.58 (s, 2H); IR (film): nmax 3460, 3362, 1600, 1495
cm-1.
p-Methylaniline: Mp 43-45ºC. 1H NMR (CDCl3): d 6.98 (d, 2H,
J = 8.2 Hz), 6.62 (d, 2H, J = 8.3 Hz), 3.42 (s, 2H), 2.28 (s, 3H). IR (KBr): nmax 3426, 3325, 1609, 1508
cm-1.
p-Chloroaniline: Mp 67-69ºC. 1H NMR (CDCl3): d 7.04 (d, 2H,
J = 8.5 Hz), 6.72 (d, 2H, J = 8.4 Hz), 3.40 (s, 2H). IR (KBr): nmax 3470, 3412, 1600, 1504
cm-1.
p-Bromoaniline: Mp 62-64ºC. 1H NMR (CDCl3): d 7.23 (d, 2H,
J = 8.6 Hz), 6.57 (d, 2H, J = 8.5 Hz), 3.65 (s, 2H). IR (KBr): nmax 3456, 3365, 1614, 1488
cm-1.
m-Methylaniline: Oil. Bp 199-201ºC. 1H NMR (CDCl3): d 7.02 (m, 1H),
6.56 (t, 1H, J = 8.1 Hz), 6.42 (m, 2H), 3.57 (s, 2H), 2.32 (s, 3H). IR (film): nmax 3416, 3335, 1605, 1503
cm-1.
m-Chloroaniline: Oil. Bp 220-222ºC. 1H NMR (CDCl3): d 7.04 (m, 1H),
6.72 (t, 1H, J = 7.2 Hz), 6.64 (s, 1H), 6.48 (m, 1H), 3.42 (s, 2H). IR (film): nmax 3456, 3405, 1612, 1514
cm-1.
m-Acetylaniline: Mp 92-94ºC. 1H NMR (CDCl3): d 7.24 (t, 1H,
J = 7.7 Hz), 7.08 (m, 2H), 6.68 (m, 1H), 3.62 (s, 2H), 2.59 (s, 3H). IR (KBr): nmax 3446, 3354, 1659, 1612,
1489 cm-1.
1-Naphthalenamine: Mp 47-48ºC. 1H NMR (CDCl3): d 7.82 (m, 2H), 7.38 (m,
2H), 7.15 (m, 2H), 6.67 (d, 1H, J = 8.0 Hz), 3.55 (s, 2H). IR (KBr): n max
3458, 3365, 1607, 1502 cm-1.
1-Dodecylamine: Mp 28-29ºC. 1H NMR (CDCl3): d 2.65 (t, J =
2.06 Hz, 2H), 2.35 (s, 2H), 1.55-1.30 (m, 20H), 0.89 (t, J = 6.80 Hz, 3H). IR
(film): nmax
3458, 3365, 1380 cm-1.
1-Hexadecanamine: Mp 45-47ºC. 1H NMR (CDCl3): d 2.68 (t, J =
2.10 Hz, 2H), 2.40 (s, 2H), 1.57-1.29 (m, 28H), 0.90 (t, J = 6.90 Hz, 3H). IR
(KBr): nmax
3462, 3360, 1380 cm-1.
Safety Warning: This procedure involves a high temperature and
pressure and must only be carried out in an apparatus which can stand for the appropriate
pressure at the reaction temperature. Meanwhile, the reaction should be performed in a
safety place.
3 RESULTS AND DISCUSSION
Our initial studies were conducted with the aim to explore the reaction conditions for the
reduction of azides with metallic zinc powder in hot water. The results are summarized in
Table 1. p-Methylphenyl azide was chosen as the model compound for this
investigation.
As seen from Table 1, the reaction temperature has a strong effect on
the reduction yield of p-methylphenyl azide with metallic zinc in hot water. It is
evident that p-methylphenyl azide could not be reduced to p-toluidine with
zinc metal in water at less than 175ºC without
any additive. Meanwhile, a moderate yield of reduction product was generated at 225ºC. When the reaction temperature reached 250ºC, a good yield of p-toluidine was obtained. However, the
reduction yield of azide decreased significantly as the reaction was carried out in
critical water (entry 8, Table 1) because of the unstablility of aromatic amine under
reaction conditions[19]. Concerning the effect of zinc mass, the results were
shown that if the ratio of zinc to p-methylphenyl azide was less than 2:1, the
reduction yield was relatively poor (entries 9 and 10, Table 1). Satisfactory results were
achieved while Zn/azide ratio>3:1 (entries 4, 11 and 12, Table 1). Further studies
revealed that the reaction was not completed when reaction time was less than 2 h (entries
13 and 14, Table 1). However, no increase of yield was observed when reaction time was
increased from 3 h to 4 h or 5 h (entries 15 and 16, Table 1). The optimum reaction
conditions for the reduction of p-methylphenyl azide with zinc metal in water were
found to be Zn (3 eq.), p-methylphenyl azide (1 eq.), H2O (10 mL),
temperature (250ºC), and reaction time (3 h).
Table 1 The reaction conditions for the reduction of p-methylphenyl azide with
zinc metal in watera
Entry |
Zn:Azide |
Temp.
(ºC) |
Time
(h) |
Yield
(%)b |
1 |
3:1 |
175 |
3 |
0
c |
2 |
3:1 |
200 |
3 |
19 |
3 |
3:1 |
225 |
3 |
52 |
4 |
3:1 |
250 |
3 |
90 |
5 |
3:1 |
275 |
3 |
89 |
6 |
3:1 |
300 |
3 |
82 |
7 |
3:1 |
350 |
3 |
67 |
8 |
3:1 |
374 |
3 |
45 |
9 |
1:1 |
250 |
3 |
43 |
10 |
2:1 |
250 |
3 |
71 |
11 |
4:1 |
250 |
3 |
90 |
12 |
5:1 |
250 |
3 |
89 |
13 |
3:1 |
250 |
1 |
34 |
14 |
3:1 |
250 |
2 |
77 |
15 |
3:1 |
250 |
4 |
88 |
16 |
3:1 |
250 |
5 |
85 |
a Reaction conditions: p-Methylphenyl
azide (1.00 mmol), tap water (10 mL) in a high T/p batch reactor system. b
Isolated yield. c Starting material p-methylphenyl azide (97 %) was
recovered.
A variety of azides were
successfully reduced to amines with metallic zinc powder in near-critical water (250ºC). The results were summarized in Table 2. The data in Table 2
indicated that, alkyl azides and aryl azides with either a general electron-donating group
(such as CH3) or a electron withdrawing group (such as CH3CO, Cl) on
the aromatic ring could be reduced smoothly to the desired amines in good yields with zinc
metal in water at 250ºC. No elimination of chloro
group was observed. However, bromo or iodo group on the aromatic ring underwent reductive
elimination of the Br or I in a competitive process. The reactivity of halogen atoms on
the aromatic ring is I> Br> Cl, which is consistent with the expected reactivity of
halogen atom in an aromatic ring and Poliakoff's experimental results[20].
Carboxylic group on the aromatic ring also underwent decarboxylation process.
Table 2 Reduction of azides to amines
with zinc metal in near-critical watera
Entry |
Azides |
Amines |
Yield
(%)b |
1 |
C6H5N3 |
C6H5NH2 |
82 |
2 |
p-CH3C6H4N3 |
p-CH3C6H4NH2 |
88 |
3 |
m-CH3C6H4N3 |
m-CH3C6H4NH2 |
86 |
4 |
m-CH3COC6H4N3 |
m-CH3COC6H4NH2 |
89 |
5 |
p-ClC6H4N3 |
p-ClC6H4NH2 |
90 |
6 |
p-BrC6H4N3 |
p-BrC6H4NH2
C6H5NH2 |
28c
44c |
7 |
m-ClC6H4N3 |
m-ClC6H4NH2 |
80 |
8 |
n-C12H25N3 |
n-C12H25NH2 |
87
|
9 |
n-C16H33N3 |
n-C16H33NH2 |
92 |
10 |
p-IC6H4N3 |
C6H5NH2 |
70 |
11 |
p-HO2CC6H4N3 |
C6H5NH2 |
72 |
12 |
a
-C10H7N3 |
a
-C10H7NH2 |
91 |
a Reaction conditions: Azide (1.00
mmol), metallic zinc powder (3.00 mmol), tap water (10 mL) in a high T/p batch
reactor system at 250ºC for 3 h. b
Isolated yield. c Determined by GC and NMR analysis of the reaction
mixture.
4 CONCLUSION
In summary, a novel, reliable and practical synthetic method for the preparation of amines
has been developed, which involves the reduction of azides by zinc metal in near-critical
water. The advantages of the present method are simple, giving good yields and
environmentally benign.
REFERENCES
[1] Li C J. Chem. Rev., 1993, 93 (6): 2023-2035.
[2] Lubineau A, Auge J, Queneau Y. Synthesis, 1994, (8): 741-760.
[3] Li C J, Chan T H. Organic Reactions in Aqueous Media, Wiley, New York, 1997.
[4] Franck E U. J. Chem. Thermodyn., 1987, 19 (3): 225.
[5] Marshall W L, Franck E U. J. Phys. Chem. Ref. Data, 1981, 10 (2): 295-304.
[6] Siskin M, Katritzky A R. Science, 1991, 254 (29): 231-237.
[7] Siskin M, Katritzky A R. Chem. Rev., 2001, 101 (4): 825-835.
[8] Savage P E. Chem. Rev., 1999, 99 (2): 603-621.
[9] Boix C, Fuente J M, Poliakoff M. New J. Chem., 1999, 23 (6): 641-643.
[10] Katritzky A R, Nichols D A, Siskin M et al. Chem. Rev., 2001, 101 (4): 837-892 and
references cited therein.
[11] Scriven E F V, Turnbull K. Chem. Rev., 1988, 88 (2): 297-368 and references cited
therein.
[12] Ranu B C, Sarkar A, Chakraborty R. J. Org. Chem., 1994, 59 (15): 4114-4116.
[13] Kamal A, Rao N V, Laxman E. Tetrahedron Lett., 1997, 38 (39): 6945-6948.
[14] Sun P, Wang L, Zhang Y. Tetrahedron Lett., 1997, 38 (31): 5549-5550.
[15] Wang D K, Dai, L-X, Hou, X-L et al. Tetrahedron Lett., 1996, 37 (24): 4187-4188.
[16] Ranu B C, Majee A, Das, A. R. Tetrahedron Lett., 1995, 36 (27): 4885-4888.
[17] Wang L, Sun X, Zhang Y. J. Chem. Research (S), 1998, (6): 336-337.
[18] Wang L, Zhang Y. Synth. Commun., 1998, 28(17): 3269-3277.
[19] Wang X, Gron L U, Klein M T. J. Supercrit. Fluids, 1995, 8 (2): 236.
[20] Poliakoff M, Boix C. J. Chem. Soc., Perkin Trans. 1, 1999, (11): 1487-1490.
¡¡
|