1
98
A.V. Gurbanov et al. / Inorganica Chimica Acta 469 (2018) 197–201
temperature on a Bruker Avance II + 300 (UltraShieldTM Magnet)
spectrometer operating at 300.130 and 75.468 MHz for proton
and carbon-13, respectively. The chemical shifts are reported in
ppm using tetramethylsilane as the internal reference. Electro-
spray mass spectra (ESI-MS) were run with an ion-trap instrument
Table 1
Crystallographic data and structure refinement details for 1 and 2.
1
2
Empirical formula
fw
Temperature (K)
Cryst. Syst.
Space group
a (Å)
C
17
H
21
N
3
8
NiO S
C
38 48 6 2
H N NiO14S
486.14
296(2)
935.65
100(2)
Orthorhombic
Pbca
19.7783(9)
9.6876(5)
22.0023(10)
90
90
90
4215.7(3)
4
1.474
(
Varian 500-MS LC Ion Trap Mass Spectrometer) equipped with an
Monoclinic
P 21/n
14.471(4)
7.838(2)
18.439(6)
90
92.048(11)
90
2090.1(10)
4
1.545
1.077
1008
0.0284
0.0684
1.081
electrospray ion source. For electrospray ionization, the drying gas
and flow rate were optimized according to the particular sample
with 35 p.s.i. nebulizer pressure. Scanning was performed from
m/z 0 to 1100 in methanol solution. The compounds were observed
in the positive mode (capillary voltage = 80–105 V).
b (Å)
c (Å)
a
, °
b, °
, °
c
1
2
.2. Synthesis of [Ni(HL )(H
O)
2 2
3
(CH OH)] (1)
3
V (Å )
Z
L1 were dissolved in 20 mL of metha-
COO) 4H O were added. The
ꢀ3
0
.1 mmol (38 mg) of NaH
2
qcalc (g cm
)
ꢀ
1
l(Mo K ) (mm
a
)
0.633
1960
0.0774
0.1954
1.207
nol, then 0.1 mmol (25 mg) of Ni(CH
3
2
2
F (0 0 0)
mixture was stirred for 5 min and left for slow evaporation. Green-
ish crystals of the product started to form after ca. 2 d at room tem-
perature; they were filtered off and dried in air.
a
R1 (I ꢁ 2
r
)
b
wR2 (I ꢁ 2
r)
GOOF
1
: Yield, 52% (based on Ni). Calcd. for C17
H
21
N
3
NiO
8
S (Mr.
a
R1 =
wR2 = [
R
||F
R
o c o
| – |F ||/R|F |.
=
486.12): C 42.00, H 4.35, N 8.64; found C 41.92, H 4.17, N 8.57.
b
2
2
2
[w(F2
)2]]1/2.
[w(F
o
– F
c
) ]/
R
o
+
MS (ESI, positive ion mode), m/z: 455.06 [MrꢀCH
3
OH + H] . IR
(
m
KBr): 3380 (s, br)
m
(OH), 3118 m(NH), 1676 (s) m(C@O), 1598 (s)
–
1
(C@N) cm
.
Table 2
Selected bond distances (Å) and angles (°) for 1 and 2.
2
2
.3. Synthesis of [Ni(H
2
L )
2
(H
2
O)
4
] [(CH
3 2 2
) S@O) ] (2)
1
2
Ni1ꢀO1
1.9847 (15)
2.0550 (15)
2.0445 (17)
2.0848 (17)
2.0700 (16)
2.0302 (18)
89.79 (6)
94.15 (6)
90.76 (7)
175.54 (7)
92.78 (6)
89.46 (6)
92.97 (6)
177.04 (6)
87.98 (7)
84.54 (6)
85.49 (7)
92.09 (7)
177.13 (6)
90.77 (6)
89.19 (7)
Ni1–O1
Ni1–O1
Ni1–O5
Ni1–O5
Ni1–O6
Ni1–O6
2.036 (3)
2.036 (3)
2.080 (3)
2.080 (3)
2.061 (3)
2.061 (3)
180.0
91.05 (12)
88.95 (12)
88.95 (12)
91.05 (12)
180.0
93.57 (11)
86.43 (11)
89.28 (11)
90.72 (11)
86.43 (11)
93.57 (11)
90.72 (11)
89.28 (11)
180.0
0
.1 mmol (37 mg) of H
3
L2 were dissolved in 25 mL of methanol,
COO) 4H O were added and the
0
0
0
Ni1ꢀO4
then 0.1 mmol (25 mg) of Ni(CH
3
2
2
Ni1ꢀO5
Ni1–O6
system was stirred for 10 min. After ca. 3 d at room temperature,
greenish crystals precipitated, which were then filtered off and
dried in air.
Ni1–O8
Ni1–N3
O1–Ni1ꢀN3
O1–Ni1ꢀO5
N3–Ni1ꢀO5
O1–Ni1ꢀO4
N3–Ni1ꢀO4
O5–Ni1ꢀO4
O1–Ni1ꢀO8
N3–Ni1ꢀO8
O5–Ni1ꢀO8
O4–Ni1ꢀO8
O1–Ni1ꢀO6
N3–Ni1ꢀO6
O5–Ni1ꢀO6
O4–Ni1ꢀO6
O8–Ni1ꢀO6
O1–Ni1ꢀO1
O1–Ni1ꢀO6
O1–Ni1ꢀO6
O1–Ni1ꢀO6
O1–Ni1ꢀO6
O6–Ni1ꢀO6
O1–Ni1ꢀO5
O1–Ni1ꢀO5
O6–Ni1ꢀO5
O6–Ni1ꢀO5
O1–Ni1ꢀO5
O1–Ni1ꢀO5
O6–Ni1ꢀO5
O6–Ni1ꢀO5
O5–Ni1ꢀO5
2
: Yield, 48% (based on Ni). Calcd. for C38
H
48
N
6
NiO14
S
2
(Mr.
0
0
=
935.64): C 48.78, H 5.17, N 8.98; found C 48.67, H 5.06, N 8.79.
+
MS (ESI, positive ion mode), m/z: 780.36 [Mrꢀ2(CH
3 2
) S@O + H] .
IR (KBr): 3437 (s, br) (OH), 3212 (NH), 1669 (s) (C@O), 1611 m
m
m
m
–
1
(
C@N) cm .
0
2
.4. Crystal structure determination
0
0
X-ray diffraction patterns of 1 and 2 were collected using a Bru-
ker SMART APEX-II CCD area detector equipped with graphite-
monochromated Mo-K radiation (k = 0.71073 Å) at room temper-
a
ature. Absorption correction was applied by SADABS [12,13]. The
structure was solved by direct methods and refined on F2 by full-
matrix least-squares using Bruker’s SHELXTL-97 [14]. All non-
hydrogen atoms were refined anisotropically. The details of the
crystallographic data, selected bond distances and angles for 1
and 2 are summarized in Tables 1 and 2. Crystallographic data
for the structural analysis have been deposited to the Cambridge
Crystallographic Data Center (CCDC 1564002 for 1 and 1564001
for 2). Copy of this information can be obtained free of charge from
The Director, CCDC, 12 Union Road, Cambridge CB2 1EZ, UK (Fax:
to the aldehyde) and the ratio between syn and anti isomers were
established by H NMR as reported previously [11,15–17]. The ade-
quacy of this procedure was proved by blank H NMR analyses
with 1,2-dimethoxyethane as an internal reference.
1
1
3. Results and discussion
3.1. Synthesis and characterization of 1 and 2
The known NaH
2
L1 and H
3
L2 were prepared according to our
1
2.5. General procedure for the study of catalytic activity
3 2 2 2
earlier works [10,11]. Reaction of Ni(CH COO) 4H O with NaH L
2
or H
3
L in methanol in the absence or presence of dimethylsulfox-
1
To a 10 mL vial were added the catalyst (1.0–4.0 mol%) and
ide led to the mononuclear Ni(II) complexes [Ni(HL )(H
OH)] (1) or [Ni(H L ) (H O) ] [(CH ) S@O) ] (2), respectively
2 2 3
O) (CH -
2
2
2
mL solvent (H O, MeOH or MeCN) and the solution was stirred
2 2 2 4 3 2 2
for 2 min at room temperature. Then, the aldehyde (1 mmol) and
nitroethane (4 mmol) were added and the resulting transparent
homogeneous solution was stirred at room temperature for the
appropriate time. After evaporation of the solvent, the residue
(Scheme 1). These complexes were characterized by both X-ray
structural determination and spectroscopic methods. In the IR
spectra of 1 and 2, the
m(C@O) and m(C@N) signals appear at
–
1
1676 and 1598, 1669 and 1611 cm , respectively, values that are
was dissolved in CDCl
lyzed by H NMR. The yield of the b-nitroalkanol product (relative
3
and this blurry solution filtrated, then ana-
significantly shifted in relation to the corresponding signals of
NaH L or H L [10,11]. Mass spectrometry of a methanol solution
2 3
1
1
2