A Clean Conversion of D-Glucosamine Hydrochloride to a Pyrazine
FULL PAPER
ethyl ether (5 ϫ 40 mL) followed by evaporation of the solvent.
The light-orange aqueous phase was evaporated to dryness in va-
cuo, with the bath temperature kept below 40 °C. The semi-solid
residue was extracted with 15 mL of methanol/ethanol (2:1 v/v)
and then with pure ethanol. The extract was evaporated to dryness
and the procedure was repeated in order to remove the last portion
of NaCl. The residue obtained was triturated in 5 mL of MeOH
with heating to the boiling point. Dry ethanol (15 mL) was then
added dropwise with stirring, after which the mixture was allowed
to cool to room temperature. The light grey product was filtered
rate esters starts at pH ഠ 6.5; this relatively low pH value
(in comparison to glucose, for example) can be explained
by the stabilization of the ester by the pyrazine nitrogen
atom. A similar stabilization of the borate esters of amino-
diols has been described for the system boric acid/3-di-
methylamino-1,2-propandiol.[17] The effect of the pyrazine
nitrogen atoms may be responsible for the formation of 2.
The type of borate esters (mode of borate coordination)
was established using known characteristic values of 11B
NMR chemical shifts for various types of borate es- off, washed with ethanol and dried at 80 °C. Recrystallization from
ters.[14,17] The results are summarized in the Table 1.
MeOH/EtOH afforded 0.88 g (58%) of analytically pure 2; m.p.
157Ϫ158 °C (ref.[12] 161Ϫ162 °C); [α]2D1 ϭ Ϫ78.9 (c ϭ 0.033 )
Table 1. Comparison of the 11B chemical shifts of compound 2
with literature values
1
(ref.[12] Ϫ78). Ϫ H NMR (399.9 MHz, D2O): δ ϭ 2.93 (m, 1 H),
3.17 (m, 1 H), 3.64 (m, 3 H), 3.77 (d, 1 H), 3.81 (m, 3 H), 3.98 (m,
1 H), 5.13 (d, 1 H), 8.50 (d, 1 H), 8.65 (d, 1 H) Ϫ 13C NMR
(100.6 MHz, D2O): δ ϭ 39.15 (CH2), 64.08, 64.56, 72.64, 72.91,
72.96, 75.02, 76.05, (7 C, CHOH), 143.82 and 145.72 (2 C arom.
CH), 154.84 and 155.64 (2 C, arom. C).
Type of borate coordination
in the ester
11B chemical shift
typical range
observed
1,2-Bidentate
Tridentate
1,2-Bidentate with
interaction to nitrogen
Ϫ12.6 to Ϫ14.9[a]
Ϫ18.1 to Ϫ19.4[a]
Ϫ10.5 to Ϫ12.0[b]
Ϫ13.4
Ϫ18.3
Ϫ8.7; Ϫ6.3
Acknowledgments
Thanks are due to Ms T. W. Smoor for experimental assistance.
[a] Ref.[7]
Ϫ
[b] Ref.[17] converted into the H3BO3 chemical-shift scale.
For interaction of boronate with an aliphatic amino group.
[1]
K. B. Hicks, E. V. Symanski, P. E. Pfeffer, Carbohydr. Res.
1983, 112, 37Ϫ50.
[2]
Thus, the 11B NMR spectrum reveals the presence of 1,2-
bidentate and tridentate coordinated borate anions and two
non-equivalent borate anions having an interaction with ni-
trogen. At the same time, the sum of the intensities of the
signals at δ ϭ Ϫ18.3 and Ϫ8.7 is approximately equal to
the intensity of the signals at δ ϭ Ϫ13.3 or δ ϭ Ϫ6.3, prob-
ably due to an equilibrium between these forms. The struc-
tures of the borate esters in solution are depicted schematic-
ally in Scheme 3.
R. J. Ferrier, Adv. Carbohydr. Chem. 1978, 35, 31Ϫ80.
[3]
C. J. Griffiths, H. Weigel, Carbohydr. Res. 1980, 81, 17Ϫ21.
[4]
B. Augustinsson, E. Scholander, Carbohydr. Res. 1984, 126,
162Ϫ164.
[5]
M. Makkee, A. P. G. Kieboom, H. van Bekkum, Carbohydr.
Res. 1985, 138, 237Ϫ245.
[6]
J. E. McMurry, M. D. Evion, J. Am. Chem. Soc. 1985, 107,
2712Ϫ2720.
[7]
R. van den Berg, J. A. Peters, H. van Bekkum, Carbohydr. Res.
1995, 267, 65Ϫ77.
[8]
F. Ledl, E. Schleicher, Angew. Chem. 1990, 29, 597Ϫ626; An-
gew. Chem. Int. Ed. Engl. 1990, 29, 565Ϫ594.
[9]
K. Sumoto, M. Irie, N. Mibu, S. Miyano, Y. Nakashima, K.
Watanabe, T. Yamaguchi, Chem. Pharm. Bull. 1991, 39,
Experimental Section
792Ϫ794.
[10]
S. J. Eitelman, M. S. Feather, Carbohydr. Res. 1979, 77
205Ϫ211.
G. Candiano, G. M. Ghiggeri, R. Gusmano, L. Zetta, E.
NMR Experiments: NMR experiments were performed on a Varian
Unity-Inova 300 spectrometer in D2O as solvent at 25 °C. For the
1H and 13C NMR measurements tert-butyl alcohol was used as an
internal standard with the methyl signal calibrated at δ ϭ 1.2 and
31.2, repsectively. The 11B chemical shifts are reported with respect
to 0.1 H3BO3 in D2O as external standard (substitution method).
[11]
Benfenati, G. Icardi, Carbohydr. Res. 1988, 184, 67Ϫ75.
[12]
R. Kuhn, G. Krüger, H. J. Haas, A. Seeliger, Ann. 1961, 644,
122Ϫ127.
[13]
M. van Duin, J. A. Peters, A. P. G. Kieboom, H. van Bekkum,
Tetrahedron 1985, 41, 3411Ϫ3421.
R. van den Berg, J. A. Peters, H. van Bekkum, Carbohydr. Res.
1994, 253 1Ϫ12.
J. van Haveren, M. H. B. van den Burg, J. A. Peters, J. G.
Batelaan, A. P. G. Kieboom, H. van Bekkum, J. Chem. Soc.,
Perkin Trans. 2 1991, 321Ϫ327.
[14]
Deoxyfructosazine (2): Phenylboronic acid (3.05 g, 25 mmol) was
added to a solution of NaOH (1.00 g, 25 mmol) in 60 mL of water.
The resulting suspension was stirred until a clear solution was
formed. -Glucosamine hydrochloride (2.16 g, 10 mmol) was then
added portionwise during 5 min. and the mixture obtained was
stirred at room temperature for 3 h. During this time the color of
the reaction mixture turned to light yellow. The pH was decreased
to 2Ϫ3 by dropwise addition of 10% HCl. Phenylboronic acid pre-
cipitated and was quantitatively recovered by extraction with di-
[15]
[16]
S. L. Patt, J. N. Shoolery, J. Magn. Reson. 1982, 46, 535Ϫ539.
T. Oi, T. Takeda, H. Kakihana, Bull. Chem. Soc. Jpn. 1992,
[17]
65, 1903Ϫ1909.
Received February 21, 2001
[O01085]
Eur. J. Org. Chem. 2001, 3899Ϫ3901
3901