Content uploaded by Milkhail A. Kiskin
Author content
All content in this area was uploaded by Milkhail A. Kiskin on Aug 10, 2018
Content may be subject to copyright.
Russian Chemical Bulletin, International Edition, Vol. 65, No. 12, pp. 2812—2819, December, 2016
2812
Published in Russian in Izvestiya Akademii Nauk. Seriya Khimicheskaya, No. 12, pp. 2812—2819, December, 2016.
10665285/16/65122812 © 2016 Springer Science+Business Media, Inc.
Binuclear nickel(II) complexes with 3,5ditertbutylbenzoate
and 3,5ditertbutyl4hydroxybenzoate anions and 2,3lutidine:
the synthesis, structure, and magnetic properties*
S. A. Nikolaevskii,a M. A. Kiskin,a A. A. Starikova,b N. N. Efimov,a A. A. Sidorov,a
V. M. Novotortsev,a and I. L. Eremenkoa
aN. S. Kurnakov Institute of General and Inorganic Chemistry, Russian Academy of Sciences,
31 Leninsky prosp., 119991 Moscow, Russian Federation.
Fax: +7 (495) 952 1279. Email: sanikol@igic.ras.ru
bInstitute of Physical and Organic Chemistry at Southern Federal University,
194/2 prosp. Stachki, 344090 RostovonDon, Russian Federation.
Fax: +7 (863) 243 4700. Email: alstar@ipoc.sfedu.ru
Two novel binuclear nickel(II) complexes [Ni2(O2CR)4(2,3lut)2] (O2CR is anion of
3,5di(tertbutyl)benzoic acid (bzo, 1) and 4hydroxy3,5di(tertbutyl)benzoic acid (hbzo, 2);
2,3lut is 2,3lutidine) with four carboxylate bridges were synthesized. The structure of complex
1 was determined by Xray diffraction. Both dimers 1 and 2 were characterized by elemental
analysis, IR spectroscopy, and magnetic measurements. The presence of the αsubstituent in
the apical lutidine ligand leads to a distortion of the geometry of the metal carboxylate core in
complex 1 as a result of short steric contacts Me(Lut)…O(OOCR) (3.134(7) Å). This is appar
ently responsible for a considerable decrease in the exchange parameters of complexes 1 and 2
(J = –30.0 and –23.6 cm–1, respectively) as compared to known analogues. Density functional
calculations of the structure and magnetic properties of 1 and 2 were carried out by the UB3LYP/
631G(d,p) method.
Key words: nickel(II) complexes, carboxylate complexes, Xray diffraction, magnetic prop
erties, quantum chemical calculations.
An analysis of published data on binuclear carboxyl
ates of 3d transition metals shows that these systems
are still of increased interest for researchers working
in different areas of science in spite of intensive re
search carried out in the last decades. Although the
emphasis is placed on unique catalytic1—5 and other
important properties of these complexes, recently partic
ular attention has been paid to the use of the complex
es as building blocks for chemical engineering of com
plex polynuclear architectures including coordination
polymers of different dimension,6 as well as metalorganic
frameworks.7—16 The use of magnetically active coor
dination binuclear carboxylates [LM(μO2CR)4ML]
(M = MnII, FeII, CoII, NiII, and CuII) as either pristine
or modified building blocks for chemical assembly of
more complicated polynuclear structures including com
binations in novel heteronuclear molecular architectures
suggests the possibility to design unusual molecular mag
netic systems including singlemolecule magnets. Partic
ular attention should be paid to binuclear magnetic sys
tems that exhibit magnetostructural correlations, includ
ing the possibility of varying the type and energy para
meters of spinspin exchange depending on (i) the nature,
number, and structural features of the bridging carboxyl
ate groups, (ii) the electronic structure and geometry
of the apical ligands L, and (iii) the distance between
the magnetic metal centers, which undoubtedly is of
great importance when choosing a starting binuclear
material.17—19
In this work, we studied two novel molecular binuclear
nickel(II) complexes with the 3,5di(tertbutyl) (bzo) and
4hydroxy3,5di(tertbutyl)benzoate (hbzo) anions and
2,3lutidine (2,3lut) as apical ligands, which extend
the number of known compounds of the general formula
[Ni2(O2CR)4L2].7—12,20—39 We have determined the
molecular structure of the title compounds and studied
their paramagnetic properties in the temperature range of
2—300 K. The results obtained were used to approximate
the experimental temperature dependence of χT. Quan
tum chemical calculations of the complexes were also
carried out.
* Dedicated to Academician of the Russian Academy of Sciences
R. Z. Sagdeev on the occasion of his 75th birthday.
Synthesis and structure of binuclear Ni complexes Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016 2813
Results and Discussion
Among numerous known binuclear complexes with
four carboxylate bridges [LM(μO2CR)4ML] (M = MnII,
CoII, FeII, NiII, CuII) with various donor apical ligands,40—42
the number of structurally characterized nickel(II) deriva
tives is relatively small. This is probably due to facile
formation of a moiety with three bridges {Ni(μH2O)
(μO2CR)2Ni} in the presence of even trace amounts of
water in the reaction medium.24,26 The situation can be to
some extent changed by assembling NiII dimers with four
carboxylate bridges from carboxylate anions with bulky
substituents and bulky apical ligands, which makes the
incorporation of water molecules between nickel ions im
possible, especially if substituents at carboxylate anions as
well as apical ligands bear hydrophobic, e.g., alkyl, groups.
Therefore, in this work novel carboxylate dimers contain
ing nickel ions were synthesized using 3,5di(tertbutyl)
benzoate (bzo) and 4hydroxy3,5di(tertbutyl)benzoate
(hbzo) anions and 2,3dimethylpyridine (lutidine) contain
ing alkyl groups. It was found that, although the reaction
mixture contained nickel(II) chloride solvated by water
molecules and ethanol (96%), the reactions of nickel chloride
and potassium salts of the acids cited above afford com
plexes [Ni2(O2CR)4(2,3lut)2] (O2CR = bzo (1), hbzo (2)).
According to Xray data, compound 1 crystallizes in
the space group P1
– with no solvate molecules (Fig. 1).
The inversion center lies between the Ni(1) and Ni(1A)
atoms of the binuclear molecule. The Ni(1) atom coordi
nates four O atoms of four bridging carboxylate groups
and the N atom of the 2,3lutidine molecule, thus forming
a distorted squarepyramidal environment (nickel atom
deviates from the O4 plane by 0.251(2) Å). The bond
lengths in the coordination unit and the Ni...Ni distance
(Table 1) are typical of the dimers having four carboxylate
bridges,20—39 although, unlike most analogues, complex 1
has a distorted N—Ni—Ni—N fragment. Deviation from
linearity (Ni—Ni—N angle is 152.23(14)°) can be appar
ently caused by steric effects of the methyl group in posi
tion 2 of the 2,3lutidine molecule (Me(Lut)...O(OOCR)
distance is 3.134(7) Å).
The angles between the aromatic ring planes and carb
oxylate groups are 11.1(2)° and 4.0(4)° for C(2)—C(7)
and O(1)C(1)O(2), C(17)—C(22) and O(3)C(16)O(4),
respectively. The angle between the C(2)—C(7) and
C(17)—C(22) aromatic rings is 84.2(2)°, while the angle
between the O(1)C(1)O(2) and O(3)C(16)O(4) carboxyl
ate group planes is 89.4(7)°. The coordinated 2,3lutidine
molecule deviates from the C(2)—C(7) and C(17)—C(22)
aromatic ring planes by 60.0(2)° and 19.6(2)°, respectively.
Note that the C(37)...O(4) distance is 3.134(7) Å, being
much shorter than the sum of the corresponding van der
Waals radii (3.22 Å).43 Earlier, shortened contacts be
tween the αmethyl group of the coordinated 2,3lutidine
molecule and the nearest O donor atoms of the carboxylate
anion were observed for complex [Ni2(piv)4(2,4lut)2] (piv
is pivalate anion and 2,4lut is 2,4lutidine).21 This specif
ic interaction causes the C(35)N(1)Ni(1) angle to increase
by 13.5° compared to the C(31)N(1)Ni(1) angle. An anal
ysis of the molecular packing shows that molecules in the
complex are isolated from one another. Selected bond
lengths and bond angles in complex 1 are listed in Table 1.
Fig. 1. Molecular structure of complex 1 (hydrogen atoms are
not shown).
Note. Fig. 1 is available in full color on the web page of the
journal (http://www.link.springer.com).
C(19)
C(20)
C(21)
C(22)
C(18)
C(17)
C(32) C(31)
C(33)
C(34)
C(36) C(37)
C(35)
N(1)
O(3)
O(4)
O(1A)
O(2A)
Ni(1) O(2)
O(3A)
O(1)
O(4A)
Ni(1A) N(1)
C(37A)
C(36A)
C(34A)
C(33A)
C(32A)
C(31A)
C(35A)
Table 1. Selected bond angles (ω) and bond lengths (d) in
complex 1
Angle ω/deg Bond d/Å
O(1)—C(1)—O(2) 123.1(5) Ni(1)—O(1) 2.040(4)
O(3)—C(16)—O(4) 126.7(5) Ni(1)—O(2) 2.101(4)
O(1)—Ni(1)—O(2) 165.1(2) Ni(1)—O(3) 2.017(4)
O(1)—Ni(1)—O(3) 189.5(2) Ni(1)—O(4) 1.997(4)
O(1)—Ni(1)—O(4) 191.7(2) Ni(1)—N(1) 2.044(5)
O(2)—Ni(1)—O(3) 186.5(2) Ni(1)...Ni(1) 2.720(2)
O(2)—Ni(1)—O(4) 188.9(2) C(1)—O(1) 1.264(6)
O(3)—Ni(1)—O(4) 166.1(2) C(1)—O(2) 1.255(6)
O(1)—Ni(1)—N(1) 102.3(2) C(16)—O(3) 1.261(6)
O(2)—Ni(1)—N(1) 192.2(2) C(16)—O(4) 1.251(6)
O(3)—Ni(1)—N(1) 191.6(2) C(31)—N(1) 1.352(7)
O(4)—Ni(1)—N(1) 101.6(2) C(35)—N(1) 1.355(7)
N(1)—Ni(1)—Ni(1A) 152.23(14) C(31)—C(32) 1.362(8)
C(31)—N(1)—Ni(1) 113.7(4) C(32)—C(33) 1.374(9)
C(35)—N(1)—Ni(1) 127.2(4) C(34)—C(35) 1.399(8)
Nikolaevskii et al.2814 Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016
We failed to obtain single crystals of complex 2 as yet,
but elemental analysis data suggest that the composition
of 2 exactly corresponds to the binuclear structure
[Ni2(hbzo)4(2,3lut)2]. An analysis of the IR spectra of 2
revealed a band at 3603 cm–1 corresponding to OH group.
Also, the spectra exhibit characteristic bands in the region
1620 cm–1 (1) and 1618 cm–1 (2), as well as at 1392 cm–1
(1) and 1384 cm–1 (2), which correspond to symmetric
(νs) and antisymmetric (νas) vibrations of carboxylate
groups. The νs – νas difference is 228 cm–1 for 1 and
234 cm–1 for 2, which is typical of the bridging coordina
tion of carboxylate groups. The absence of peaks in the
region 1700 cm–1 for both compounds suggests deproto
nation of all carboxylic groups.44,45
Our studies of the temperature dependences of the mag
netic susceptibility of compounds 1 and 2 in the tempera
ture range of 2—300 K revealed antiferromagnetic inter
actions (Fig. 2). The magnetic moment (μeff) is 4.19 μB
(χexpT = 2.20 cm3 K mol–1) for 1 and 4.20 μB
(χexpT = 2.21 cm3 K mol–1) for 2 at 300 K, being some
what higher than the theoretical value obtained for two
noninteracting Ni2+ ions (S = 1): μcalc = 4 μB (χcalcT =
= 2.02 cm3 K mol–1).46 As the temperature decreases to 2 K,
the effective magnetic moment decreases to 0.25 μB
(χexpT = 0.01 cm3 K mol–1) for 1 and 0.42 μB (χexpT =
= 0.02 cm3 K mol–1) for 2. At 100 < T < 300 K, the χ–1(T)
dependence is linear for both compounds (see Fig. 2, c, d),
being satisfactorily described by the Curie—Weiss equa
tion χM = C/(T – θ) with the parameters listed in Table 2.
The Weiss constant is highly negative for both compounds.
The considerable decrease in the magnetic moment and
the negative sign of the Weiss constant are indicative of
strong antiferromagnetic interactions in the samples.
To determine the exchange parameter, experimental
data χT(T) for the entire temperature range studied were
approximated by the van Vleck equation for S1 = S2 = 1
Fig. 2. Temperature dependences of magnetic susceptibility (1) and χT (2) of compounds 1 (a) and 2 (b) and the corresponding 1/χ(T)
plots (c, d). Closed and open circles as well as open squares denote experimental data; solid lines denote results of calculations.
1.2
0.9
0.6
0.3
χ•10–2/cm3 mol–1
2
1
0
χT/cm3 K mol–1
0 100 200 T/К
a
1.5
1.2
0.9
0.6
0.3
χ•10–2/cm3 mol–1
2
1
0
χT/cm3 K mol–1
0 100 200 T/К
b
1.4
1.2
1.0
0.8
1/χ•102/mol cm–3
200 300 T/К
с
1.4
1.2
1.0
0.8
1/χ•102/mol cm–3
200 300 T/К
d
1
2
1
2
Table 2. Bestfit parameters for approximations* for complexes 1
and 2
Com gJ/cm–1 P (%) Cθ/K
plex /cm3 K mol–1
12.35±0.03 –30±1 1 3.39 –167
22.25±0.03 –24±1 5 2.98 –106
* The g, J, P are the van Vleck equation parameters for the entire
temperature range; C, θ are the Curie—Weiss law parameters
at 100 < T < 300 K).
Synthesis and structure of binuclear Ni complexes Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016 2815
Table 3. Geometric parameters and results of approximation of magnetochemical data for known binuclear nickel(II)
complexes of the general formula [Ni2(O2CR)4L2]
Complex* d(Ni…Ni)/ÅAngle Ni—Ni—N/deg gJReference
[Ni2(piv)4(Metquin)2] 2.754 — .— –160 20
[Ni2(piv)4(2,4lut)2]** 2.708 166.65 2.40a–194a21
2.72b–224b
[Ni2(piv)4(2,5lut)2] 2.708 166.65 2.38 –128 21
[Ni2(piv)4(EtPy)2] 2.723 166.00 2.85 –221 21, 22
[Ni2(Et2CHCOO)4(quin)2].— — 2.35 –216 21
[Ni2(Me2PhCCOO)4(PPh3)2] 2.752c172.42c2.00 –206 23
2.765c166.64c
[Ni2(Me2PhCCOO)4(quin)2] 2.734 165.70 2.03 –142 22, 23
[Ni2(piv)4(2pic)2] 2.717 169.46 2.28 –223 22, 23
[Ni2(piv)4(Py)2] 2.604 176.7 2.175 –130 18, 24
[Ni2(PhCO2)4(NITpPy)2] 2.6454 172.9 2.02 –29.45 33
[Ni2(atc)4(Py)2] 2.700d171.9d2.20 –537 36
2.651d175.2d
[Ni2(L)2(4,4´bpy)2] 2.700 180.0 2.20 –103.56 37
[Ni2(dpa)2(MeOH)2] 2.582 167.8e2.2 –103 38
[Ni2(RCOO)4(4,4´bpy)2] 2.694 165.17 2.26 –190.03 39
[Ni2(bzo)4(2.3lut)2] 2.720 152.23 2.35 –30 ***
[Ni2(hbzo)4(2.3lut)2].— — 2.25 –24 ***
* Metquin is 2methylquinoline; 2,4lut is 2,4lutidine; 2,5lut is 2,5lutidine; EtPy is 2ethylpyridine; quin is quinoline;
2pic is 2picoline; Py is pyridine; NITpPy is 2(4pyridyl)4,4,5,5tetramethylimiadzoline1oxyl3oxide; atc is
9anthracenecarboxylate anion; 4,4´bpy is 4,4´bipyridyl; H2L is 2,4dibenzoylisophthalic acid; H2dpa is 2(2
carboxyphenyl)benzoic acid; and RCOOH is 4,4´pyridine2,6diyldiisophthalic acid.
** Parameters of exchange interactions for this complex were calculated using two mathematical models for the low
temperature region (a) and hightemperature region (b); Ni...Ni interatomic distances and Ni—Ni—P angles in two
independent molecules of the complex (c); Ni...Ni interatomic distances and Ni—Ni—N angles in two independent
molecules of the complex (d); and the Ni—Ni—O(MeOH) angle (e).
*** This work.
taking into account noninteracting paramagnetic
Ni2+ ions:
where N is the Avogadro constant, μB is the Bohr magne
ton, k is the Boltzmann constant, J is the exchange inte
gral, P is the proportion of noninteracting paramagnetic
Ni2+ centers, C is the Curie constant, and θ is the Weiss
constant.
The bestfit parameters are g = 2.35±0.03, J =
= –30.0±0.4 cm–1 for 1 and g = 2.25±0.03, J =
= –23.6±0.1 cm–1 for 2. The proportion of noninteracting
paramagnetic centers (P) is at most 1% for 1 and 5% for 2.
Emphasize that only a few studies on the magnetic
behavior of nickel complexes with four carboxylate bridges
[Ni2(RCO2)4L2] are available.18,20,21,23,24,33—39 Quantita
tive interpretation of exchange interactions was performed
for fourteen compounds only18,20,21,23,33,36—39 (Table 3).
However, an analysis of these data reveals no reliable cor
relations between the efficiency of exchange interactions
of nickel(II) ions and the Ni...Ni distance, geometry of the
metal carboxylate core, parameters of substituents at carb
oxylate groups, etc.
According to our density functional calculations car
ried out by the UB3LYP/631G(d,p) method, the opti
mized geometries of the compounds synthesized corre
spond to a known structure with four carboxylate bridges,
typical of this type of compounds20—39 (Fig. 3). This is in
good agreement with the results of Xray study of com
pound 1. The largest deviation for the bond lengths (at
most 0.02 Å) was predicted for the Ni...Ni distance. Energy
minima located on the quintet potential energy surface
(PES) of the complexes in the highspin (HS) state, 1HS
and 2HS, possess similar characteristics of the coordina
tion units.
The J values calculated for the optimized geometries
of 1 and 2 are respectively –34 and –37 cm–1, which
indicates a weak antiferromagnetic coupling of the un
paired electrons of nickel(II) ions and is in agreement with
the values obtained using the results of magnetochemical
studies (–30 and –24 cm–1, respectively). An analysis of
the magnetic orbitals (αSOMO+βSOMO) of com
pounds 1 and 2 in the "broken symmetry" (BS) state shows
Nikolaevskii et al.2816 Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016
(Fig. 4, a) that the observed magnetic properties are due to
channels of antiferromagnetic exchange involving carbox
ylate bridges. According to calculations, the spin density
in complex 1 (Fig. 4, b) is localized on the metal and
oxygen atoms. This confirms the conclusions about the
role of carboxylate ligands in antiferromagnetic coupling
of nickel atoms.18
An analysis of the results of studies of the binuclear
NiII carboxylates (see Table 3) shows a record high J value
of –537 cm–1 for [Ni2(atc)4(Py)2].36 The results of single
point calculations of the complex in different approxima
tions disclose a strong antiferromagnetic exchange between
unpaired electrons of nickel ions (about –390 cm–1). Hav
ing analyzed our results and the available published data
Fig. 3. Optimized geometries of complexes 1 and 2 obtained from DFT UB3LYP/631g(d,p) calculations (hydrogen atoms are
omitted).
2.064
2.023
99°
2.741
2.125
153°
1
2.069
2.022
99°
2.732
2.125
152°
2
Fig. 4. Magnetic orbitals (αSOMO+βSOMO) of complex 1 in the BS state (a) and typical spin density distribution for compounds 1
and 2 (b).
ab
Synthesis and structure of binuclear Ni complexes Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016 2817
and based on the assumption that oxygen atoms occupy
vertices of a rectangular parallelepiped, one can assume
improved efficiency of spinspin exchange between NiII
magnetic ions in the undistorted metal carboxylate core
{Ni2(O2CR)4}.
Summing up, we synthesized two novel binuclear com
plexes [Ni2(O2CR)4(2,3lut)2] (O2CR = bzo (1), hbzo (2)).
The structure of 1 was determined by Xray analysis.
Structural distortion of the tetracarboxylate moiety
{Ni2(O2CR)4} in molecule 1 is due to steric effects caused
by the αsubstituent in the coordinated 2,3lutidine mole
cule. An analysis of magnetic data for 1 and 2 revealed
antiferromagnetic interactions between nickel(II) magnetic
ions (S = 1) with close values of gfactors and exchange
integrals (g = 2.35±0.03, J = –30.0±0.4 cm–1 for 1;
g = 2.25±0.03, J = –23.6±0.1 cm–1 for 2). According to
quantum chemical calculations, the magnetic behavior of
the complexes in question is governed by the antiferro
magnetic exchange channel formed as a result of the over
lap of the magnetic orbitals including four carboxylate
ligands. Based on these results and published data (see
Table 3), one can assume that the parameter J of the
binuclear nickel(II) complexes with four carboxylate bridges
correlates with the geometric parameters of the magneto
active fragment {Ni(μO2CR)4Ni}. It seems quite probable
that steric effects can be used as an important tool for
controlling the magnetic properties of the magnetically
active dinickel unit with four carboxylate bridges taking
into account structural features of the apical ligand.
Experimental
The novel complexes were synthesized in air from commer
cially available reactants, namely, ethanol (96%), 3,5di(tert
butyl)benzoic acid (>99%), 4hydroxy3,5di(tertbutyl)benzoic
acid (98%), 2,3lutidine (>99%), NiCl2•6H2O (>99.8%), and
KOH (>99%). IR spectra of the compounds were recorded on
a Perkin Elmer Spectrum 65 spectrophotometer equipped with
a Quest ATR Accessory (Specac) by the attenuated total reflec
tance (ATR) in the range of 400—4000 cm–1. Elemental analysis
was performed on a Euro EA3000 (Euro Vektor) automated
C,H,N,Sanalyzer. Powder Xray diffraction study was done on
a Bruker D8 Advance diffractometer (CuKα, Ni filter, LYNXEYE
detector, reflection geometry).
The magnetic properties of powders of compounds 1 and 2
were measured on a Quantum Design PPMS9 automated phys
ical property measurement system. Temperature dependences
of the magnetization were measured in the temperature range
from 2 to 300 K in an external magnetic field (H) of 5 kOe.
A correction for paramagnetic properties of the sample holder
was applied. The diamagnetic correction was made using Pascal´s
constants.46
Quantum chemical calculations were carried out within the
framework of the density functional theory (DFT) using the
Gaussian 09 program47 and the UB3LYP functional,48 which
correctly reproduces the parameters of openshell coordination
compounds,49—51 and the 631g(d,p) basis set. Stationary points
on the PES were located by full geometry optimization of mo
lecular structures followed by stability tests for the DFT wave
function. Exchange interactions between unpaired electrons of
paramagnetic centers were evaluated using the "broken symme
try" (BS) approach.52 The exchange parameters (J/cm–1) were
calculated using the Yamaguchi formula.53 Graphic images of
the molecular structures shown in Figs 3 and 4 were drawn using
the ChemCraft program54 for which corresponding Cartesian
atomic coordinates obtained from quantum chemical calcula
tions served as the input parameters.
Bis(2,3dimethylpyridineκκ
κκ
κNtetrakis[μμ
μμ
μO,O´3,5di(tert
butyl)benzoato]dinickel(II), [Ni2(bzo)4(2,3lut)2] (1). To a solu
tion of NiCl2•6H2O (0.238 g, 1 mmol) in ethanol (15 mL), a hot
solution of potassium salts of 3,5di(tertbutyl)benzoic acid, ob
tained by reaction of 3,5di(tertbutyl)benzoic acid (1.17 g,
5 mmol) with potassium hydroxide (0.28 g, 5 mmol) in ethanol
(30 mL), was added. The reaction mixture was refluxed for 5 min,
cooled to 60 °C, and kept at this temperature for additional
15 min. Potassium chloride precipitate was filtered off. 2.3Luti
dine (0.1072 g, 1 mmol) was added to the filtrate. The mixture
was stirred at 60 °C for 1 h, transferred to a Schlenk vessel, and
the solvent was gradually (over a period of 4 h) concentrated to
20 mL. A week later, a lightgreen residue formed. The residue
was filtered and washed with hot ethanol (3×5 mL). The yield of
complex 1 was 71% (calculated with respect to the initial amount
of NiCl2•6H2O). Darkgreen crystals suitable for Xray study
were grown within two weeks by slow evaporation of mother
liquor at a reduced pressure. The identity of the single crystals
and the residue isolated earlier was confirmed by powder
Xray diffraction. Found (%): C, 70.48; H, 8.42; N, 2.02.
C74H102N2Ni2O8. Calculated (%): C, 70.26; H, 8.13; N, 2.21.
IR, ν/cm–1: 2962 (m), 2903 (vw), 2865 (vw), 1620 (s), 1583 (vs),
1475 (vw), 1439 (s), 1392 (vs), 1361 (w), 1287 (m), 1247 (m),
1194 (w), 1162 (vw), 1133 (w), 1026 (vw), 995 (vw), 892 (m),
822 (m), 788 (s), 741 (vs), 723 (m), 704 (s), 604 (w), 535 (m),
492 (m), 424 (m), 413 (m).
Bis(2,3dimethylpyridineκκ
κκ
κNtetrakis[μμ
μμ
μO,O´4hydroxy
3,5di(tertbutyl)benzoato]dinickel(II), [Ni2(hbzo)4(2,3lut)2] (2)
was synthesized analogously using 4hydroxy3,5di(tertbutyl)
benzoic acid (1.25 g, 5 mmol) instead of 3,5di(tertbutyl)benzoic
acid. Transfer of the reaction mixture to the Schlenk vessel and
concentration of the solution to 20 mL was followed by precipi
tation of lightgreen residue of 2. The yield of complex 2 was 89%
(calculated with respect to the initial amount of NiCl2•6H2O).
We failed to grow single crystals suitable for Xray study due to low
solubility of the reaction product in common organic solvents.
Recrystallization of the complex from DMF afforded bright
red single crystals of 3.3´,5.5´tetra(tertbutyl)1.1´biphenyl
idene4.4´quinone.55 Found (%): C, 66.68; H, 7.97; N, 2.14.
C74H102N2Ni2O12. Calculated (%): C, 66.88; H, 7.74; N 2.11.
IR, ν/cm–1: 3603 (s), 2957 (m), 2903 (vw), 2865 (vw), 1618 (s),
1597 (m), 1574 (s), 1472 (m), 1449 (m), 1384 (vs), 1318 (s), 1281 (m),
1233 (s), 1202 (m), 1152 (s), 1133 (m), 1116 (s), 1024 (w),
616 (w), 890 (m), 821 (w), 782 (s), 787 (s), 750 (w), 722 (m), 701 (vs),
648 (m), 604 (w), 552 (m), 516 (m), 460 (s), 451 (s), 438 (s), 412 (m).
Singlecrystal Xray study of complex 1 was performed on
a Bruker Apex II diffractometer (CCD detector, MoKα,
λ = 0.71073 Å, graphite monochromator).56 A semiempirical
absorption correction57 was applied. The structure was solved by
the direct methods and refined in the fullmatrix anisotropic
approximation for all nonhydrogen atoms. Hydrogen atoms at
Nikolaevskii et al.2818 Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016
carbon atoms of organic ligands were located geometrically and
refined in the riding model. Calculations were carried out using
the SHELX97 software.58 Crystallographic parameters of com
plex 1: M = 1265.00, crystal dimensions 0.08×0.06×0.06 mm,
green, cubic, T = 184(2) K, triclinic, P1
–, a = 11.203(5),
b = 12.548(5), c = 12.662(5) Å, α = 88.946(7)°, β = 84.820(7)°,
γ = 78.346(7)°, V = 1736.1(12) Å3, Z = 1, ρ = 1.210 g cm–3,
μ = 0.596 mm–1, θ = 1.61—28.38°, –14 ≤ h ≤ 14, –16 ≤ k ≤ 16,
–16 ≤ l ≤ 16; a total of 18102 reflections, 8553 unique reflec
tions, 4388 reflections with I > 2σ(I), Rint = 0.0901, Tmin/Tmax =
= 0.9538/0.9651, S = 1.171, R1 = 0.0915, wR2 = 0.2574 (for the
whole data array), R1 = 0.0915, wR2 = 0.2161 (for I ≥ 2σ(I)),
Δρmin/Δρmax = –0.984/2.153 e Å–3. Full Xray data array was
deposited at the Cambridge Structural Database (CCDC No.
1499784; deposit@ccdc.cam.ac.uk or http://www.ccdc.cam.
ac.uk/data_request/cif).
Singlecrystal and powder Xray diffraction studies and
C,H,Nanalysis were performed at the Center of Collective use
of the Kurnakov Institute of General and Inorganic Chemistry,
Russian Academy of Sciences.
This work was financially supported by the Presidium
of the Russian Academy of Sciences and by the Federal
Agency for Scientific Organizations. S. A. Nikolaevskii,
M. A. Kiskin, and I. L. Eremenko express their gratitude
to the Russian Science Foundation for financial support
of Xray studies carried out in this work (Project No. 14
2300176).
References
1. J. S. Kanady, J. L. MendozaCortes, E. Y. Tsui, R. J. Niels
en, W. A. Goddard, T. Agapie, J. Am. Chem. Soc., 2013,
135, 1073.
2. J. Jeschke, C. Gabler, M. Korb, T. Ruffer, H. Lang, Eur. J.
Inorg. Chem., 2015, 2015, 2939.
3. D. Gatteschi, R. Sessoli, Angew. Chem., Int. Ed., 2003,
42, 268.
4. K. S. Gavrilenko, S. V. Punin, O. Cador, S. Golhen,
L. Ouahab, V. V. Pavlishchuk, Inorg. Chem., 2005, 44, 5903.
5. C. Papatriantafyllopoulou, S. Zartilas, M. J. Manos, C. Pi
chon, R. Clerac, A. J. Tasiopoulos, Chem. Commun., 2014,
50, 14873.
6. J. J. Perry IV, J. A. Perman, M. J. Zaworotko, Chem. Soc.
Rev., 2009, 38, 1400.
7. S. Wang, M.L. Hu, S. W. Ng, Acta Crystallogr., Sect. E:
Struct. Rep. Online, 2002, 58, m242.
8. S. W. Lee, H. J. Kim, Y. K. Lee, K. Park, J.H. Son, Y.U.
Kwon, Inorg. Chim. Acta, 2003, 353, 151.
9. L.P. Hsu, J.Y. Wu, K.L. Lu, J. Inorg. Organomet. Polym.
Mater., 2007, 17, 259.
10. P. Maniam, N. Stock, Inorg. Chem., 2011, 50, 5085.
11. N. Klein, I. Senkovska, I.A. Baburin, R. Grunker, U. Stoeck,
M. Schlichtenmayer, B. Streppel, U. Mueller, S. Leoni,
M. Hirscher, S. Kaskel, Chem. Eur. J., 2011, 17, 13007.
12. H. C. Hoffmann, B. Assfour, F. Epperlein, N. Klein,
S. Paasch, I. Senkovska, S. Kaskel, G. Seifert, E. Brunner,
J. Am. Chem. Soc., 2011, 133, 8681.
13. Q. Shi, Y. T. Sun, Z. S. Li, K. F. Ma, X. Q. Cai, D. S. Liu,
Inorg. Chim. Acta, 2009, 362, 4167.
14. Y. Pang, D. Tian, X.F. Zhu, Y.H. Luo, X. Zheng,
H. Zhang, Cryst. Eng. Comm., 2011, 13, 5142.
15. M. P. Yutkin, D. N. Dybtsev, V. P. Fedin, Russ. Chem. Rev.,
2011, 80, 1009 [Usp. Khim., 2011, 80, 1061].
16. V. V. Butova, M. A. Soldatov, A. A. Guda, K. A. Lomachen
ko, C. Lamberti, Russ. Chem. Rev., 2016, 85, 280 [Usp. Khim.,
2016, 85, 280].
17. M. Kato, Y. Muto, Coord. Chem. Rev., 1988, 29, 45.
18. V. M. Novotortsev, Yu. V. Rakitin, S. E. Nefedov, I. L.
Eremenko, Izv. Akad. Nauk. Ser. Khim., 2000, 437 [V. M.
Novotortsev, Yu. V. Rakitin, S. E. Nefedov, I. L. Eremenko,
Russ. Chem. Bull. (Int. Ed), 2000, 49, 438].
19. M. Cortijo, S. Herrero, B. Jerez, R. JimenezAparicio,
J. Perles, J. L. Priego, J. Torroba, J. Tortajada, ChemPlus
Chem, 2014, 79, 951.
20. N. I. Kirillova, Yu. T. Struchkov, M. A. PoraiKoshits, A. A.
Pasynskii, A. S. Antsyshkina, L. Kh. Minacheva, G. G.
Sadikov, T. C. Idrisov, V. T. Kalinnikov, Inorg. Chim. Acta,
1980, 40, 115.
21. N. Hirashima, S. Husebye, M. kato, K. MaartmannMoe,
Y. Muto, M. Nakashima, T. Tokii, Acta Chem. Scand., 1990,
44, 984.
22. M. Morooka, S. Ohba, M. Nakashima, T. Tokii, Y. Muto,
M. Kato, O.W. Steward, Acta Crystallogr., Sect. C: Cryst.
Struct. Commun., 1992, 48, 1888.
23. S. Husebye, M. Kato, K. MaartmannMoe, Y. Muto,
M. Nakashima, T. Tokii, Acta Chem. Scand., 1994, 48, 628.
24. I. L. Eremenko, S. E. Nefedov, A. A. Sidorov, M. A. Golubni
chaya, P. V. Danilov, V. N. Ikorskii, Y. G. Shvedenkov, V. M.
Novotortsev, I. I. Moiseev, Inorg. Chem., 1999, 38, 3764.
25. A. A. Sidorov, I. G. Fomina, A. E. Malkov, A. V. Reshetnik
ov, G. G. Aleksandrov, V. M. Novotortsev, S. E. Nefedov,
I. L. Eremenko, Izv. Akad. Nauk. Ser. Khim., 2000, 1915
[A. A. Sidorov, I. G. Fomina, A. E. Malkov, A. V. Reshetni
kov, G. G. Aleksandrov, V. M. Novotortsev, S. E. Nefedov,
I. L. Eremenko, Russ. Chem. Bull. (Int. Ed.), 2000, 49, 1887].
26. D. Lee, P.L. Hung, B. Spingler, S.J. Lippard, Inorg. Chem.,
2002, 41, 521.
27. T. O. Denisova, G. G. Aleksandrov, O. P. Fialkovskii, S. E.
Nefedov, Zh. Neorgan. Khim., 2003, 48, 1476 [T. O. Deniso
va, G. G. Aleksandrov, O. P. Fialkovskii, S. E. Nefedov,
Russ. J. Inorg. Chem. (Engl. Transl.), 2003, 48, 1340].
28. M. Affronte, I. Casson, M. Evangelisti, A. Candini, S. Car
retta, C. A. Muryn, S. J. Teat, G. A. Timco, W. Wernsdorfer,
R. E. P. Winpenny, Angew. Chem., Int. Ed., 2005, 44, 6496.
29. T. O. Denisova, E. V. Amel´chenkova, I. V. Pruss, Zh. V.
Dobrokhotova, O. P. Fialkovskii, S. E. Nefedov, Zh. Neor
gan. Khim., 2006, 51, 1098 [T. O. Denisova, E. V. Amel´
chenkova, I. V. Pruss, Zh. V. Dobrokhotova, O. P. Fialk
ovskii, S. E. Nifedov, Russ. J. Inorg. Chem. (Engl. Transl.),
2006, 51, 1020].
30. M. Dan, C. N. R. Rao, Angew. Chem., Int. Ed., 2006, 45, 281.
31. J.H. Deng, Y.P. Yi, Z.X. Xiong, L. Yuan, G.Q. Mei,
Acta Crystallogr., Sect. E: Struct. Rep.Online, 2009, 65, m1484.
32. K. A. Kounavi, M. J. Manos, A. J. Tasiopoulos, S. P. Per
lepes, V. Nastopoulos, Bioinorg. Chem. Appl., 2010, 2010,
178034.
33. L. Zhu, X. Chen, Q. Zhao, Z. Li, X. Zhang, B. Sun, Z. Anorg.
Allg. Chem., 2010, 636, 1441.
34. A. A. Pasynskii, S. S. Shapovalov, A. V. Gordienko, I. V.
Skabitskii, Koord. Khim., 2011, 37, 129 [A. A. Pasynskii,
Synthesis and structure of binuclear Ni complexes Russ.Chem.Bull., Int.Ed., Vol. 65, No. 12, December, 2016 2819
S. S. Shapovalov, A. V. Gordienko, I. V. Skabitskii, Russ. J.
Coord. Chem. (Engl. Transl.), 2011, 37, 127].
35. D. A. Kose, O. Yurdakul, J. Chin. Chem. Soc. (Taipei), 2014,
61, 1326.
36. M. Cortijo, P. DelgadoMartinez, R. GonzalezPrieto,
S. Herrero, R. JimenezAparicio, J. Perles, J. L. Priego, M. R.
Torres, Inorg. Chim. Acta, 2015, 424, 176.
37. Y. Pang, D. Tian, X.F. Zhu, Y.H. Luo, X. Zheng,
H. Zhang, CrystEngComm, 2011, 13, 5142.
38. Q. Shi, Y. Sun, L. Sheng, K. Ma, X. Cai, D. Liu, Inorg.
Chim. Acta, 2009, 362, 4167.
39. J. Zhao, Y. Wang, W. Dong, Y. Wu, D. Li, B. Liu, Q. Zhang,
Chem.Commun., 2015, 51, 9479.
40. M. A. Kiskin, I. L. Eremenko, Russ. Chem. Rev., 2006, 75,
559 [Usp. Khim., 2006, 75, 627].
41. Y. Wang, Z. Zhou, J. Solid State Chem., 2015, 228, 117.
42. E. M. Cheprakova, E. V. Verbitskiya, M. A. Kiskin, G. G.
Aleksandrov, P. A. Slepukhin, A. A. Sidorov, D. V. Star
ichenko, Y. N. Shvachko, I. L. Eremenko, G. L. Rusinov,
V. N. Charushin, Polyhedron, 2015, 100, 89.
43. S. Rowland, R. Taylor, J. Phys. Chem., 1996, 100, 7384.
44. Z. B. Han, X. N. Cheng, X. M. Chen, Cryst. Growth Des.,
2005, 5, 695.
45. L. Liu, G.M. Zhang, R.G. Zhu, Y.H. Liu, H.M. Yao,
Z.B. Han, RSC Adv., 2014, 4, 46639.
46. Yu. V. Rakitin, V. T. Kalinnikov, Sovremennaya magne
tokhimiya [Modern Magnetochemistry], Nauka, SanktPeter
burg, 1994, 276 pp. (in Russian).
47. M. J. Frisch, G. W. Trucks, H. B. Schlegel, G. E. Scuseria,
M. A. Robb, J. R. Cheeseman, G. Scalmani, V. Barone,
B. Mennucci, G. A. Petersson, H. Nakatsuji, M. Caricato,
X. Li, H. P. Hratchian, A. F. Izmaylov, J. Bloino, G. Zheng,
J. L. Sonnenberg, M. Hada, M. Ehara, K. Toyota, R. Fuku
da, J. Hasegawa, M. Ishida, T. Nakajima, Y. Honda,
O. Kitao, H. Nakai, T. Vreven, J. A. Montgomery, Jr., J. E.
Peralta, F. Ogliaro, M. Bearpark, J. J. Heyd, E. Brothers,
K. N. Kudin, V. N. Staroverov, T. Keith, R. Kobayashi,
J. Normand, K. Raghavachari, A. Rendell, J. C. Burant, S. S.
Iyengar, J. Tomasi, M. Cossi, N. Rega, J. M. Millam,
M. Klene, J. E. Knox, J. B. Cross, V. Bakken, C. Adamo,
J. Jaramillo, R. Gomperts, R. E. Stratmann, O. Yazyev, A. J.
Austin, R. Cammi, C. Pomelli, J. W. Ochterski, R. L. Martin,
K. Morokuma, V. G. Zakrzewski, G. A. Voth, P. Salvador,
J. J. Dannenberg, S. Dapprich, A. D. Daniels, O. Farkas, J. B.
Foresman, J. V. Ortiz, J. Cioslowski, D. J. Fox, GAUSSIAN
09, Revision D.01, Gaussian, Inc., Wallingford, CT, 2013.
48. W. Kohn, L. J. Sham, Phys. Rev., 1965, 140, A1133.
49. A. G. Starikov, Russ. J. Gen. Chem. (Engl. Transl.), 2009, 79,
2792 [Ross. Khim. Zh., 2009, 53, 115].
50. A. G. Starikov, R. M. Minyaev, V. I. Minkin, J. Mol. Struct.:
THEOCHEM, 2009, 895, 138.
51. A. A. Starikova, A. G. Starikov, V. I. Minkin, Russ. J. Coord.
Chem. (Engl. Transl.), 2015, 41, 487 [Koord. Khim., 2015,
41, 451].
52. L. Noodleman, J. Chem. Phys., 1981, 74, 5737.
53. Y. Kitagawa, T. Saito, Y. Nakanishi, Y. Kataoka, T. Matsui,
T. Kawakami, M. Okumura, K. Yamaguchi, J. Phys. Chem.
A., 2009, 113, 15041.
54. Chemcraft, version 1.7, 2013: http://www.chemcraftprog.com.
55. M. A. Khan, A. Osman, D. G. Tuck, Acta Crystallogr, Sect.
C, 1986, 42, 1399.
56. SMART (Control) and SAINT (Integration) Software, Ver
sion 5.0, Bruker AXS Inc., Madison, WI, 1997.
57. G. M. Sheldrick, SADABS, Program for Scanning and Cor
rection of Area Detector Data, Göttinngen University,
Göttinngen, Germany, 2004.
58. G. M. Sheldrick, Acta Crystallogr., Sect. A, 2008, 64, 112.
Received August 31, 2016;
in revised form October 26, 2016