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ORIGINAL PAPER
Hydrothermal Synthesis, Crystal Structure and Propertiesof Two Organic Amine Templated Lanthanide Sulfates
Jie Fu • Lei Zheng • Yan Yuan • You Song •
Yan Xu
Received: 4 November 2010 / Accepted: 29 June 2011 / Published online: 15 July 2011
� Springer Science+Business Media, LLC 2011
Abstract Two new lanthanide sulfates [C6H14N2]2[Ln2
(SO4)4(H2O)4][SO4]�6H2O (Ln = Pr 1, Nd 2) have been
hydrothermally synthesized and structurally characterized
by single-crystal X-ray diffraction, IR and TGA. Single
crystal X-ray diffraction illuminates that both 1 and 2
crystallize in orthorhombic crystal system, space group
Pbna with cell dimensions: a = 10.1362(13) A,
b = 13.4782(17) A, c = 25.565(3) A, V = 3492.6(8) A3,
Z = 4 for 1; a = 10.1243(12) A, b = 13.4438(16) A,
c = 25.550(3) A, V = 3477.6(7) A3, Z = 4 for 2. Structure
analysis indicates that both 1 and 2 are layered structures
and the sulfate ions as well as the organic templates reside
among the layers. Magnetic property of compound 1 was
investigated further.
Keywords Hydrothermal synthesis � Lanthanide
sulfates � Crystal structures � Magnetic property
Introduction
Great efforts have been made to synthesize non alumino-
silicate solid state materials due to their diverse structural
flexibility and superior catalysis, ion exchange and magnetic
properties [1–3]. Recently, one of the important advances in
the solid state chemistry has been the study of open-frame-
work architectures containing organic amine templated
sulfates [4–10]. Compared with other transition metals, rare-
earth elements’ ability to adopt a large range of coordination
numbers allows them to obtain new topologies, basing on the
variation of the polyhedra [11–23]. One of the strategies
used in the synthesis of solid state materials is to employ a
special organic amine as the structure-directing agent (SDA)
under hydrothermal (solvothermal) conditions. Successful
examples with organic amine templated lanthanide sulfates
materials have been reported. In the previous literatures,
there are a lot of 2D layered lanthanide sulfates have been
reported. For examples, [C2N2H10][La2(H2O)4(SO4)4]
�2H2O is the first example of organic templates 2D layered
lanthanum sulfate constructed by the fusion of 4-membered
ring ladders [22]; [Ln2(SO4)4(H2O)4][C6N2H14]2[C2N2H8]
[SO4][H2O]3 (Ln = La, Pr or Nd) is a layered structure
wherein the SO4 tetrahedra and the LnO9 polyhedra join
together to form (4, 4) net sheets, with two different amines
as well as the sulfate ions residing in the interlamellar space
[13]; [C2N2H10]1.5[Nd(SO4)3(H2O)]�2H2O is the first neo-
dymium sulfate exhibits of a novel two-dimensional zigzag
layer structure with 8-membered rings window [23] and
La2(H2O)2(C2H10N2)3(SO4)6�4H2O is built from inorganic
anionic sheets of lanthanum sulfates between which are
located the ethylenediammonium cations and water mole-
cules [10]. In this work, we used a new method to synthesize
two new 2-D layered lanthanide sulfates of [C6H14N2]2
[Ln2(SO4)4(H2O)4][SO4]�6H2O (Ln = Pr 1, Nd 2) in
Electronic supplementary material The online version of thisarticle (doi:10.1007/s10870-011-0166-8) contains supplementarymaterial, which is available to authorized users.
J. Fu � L. Zheng � Y. Yuan � Y. Xu (&)
State Key Laboratory of Materials-Oriented Chemical
Engineering, College of Chemistry and Chemical Engineering,
Nanjing University of Technology, Nanjing 210009,
People’s Republic of China
e-mail: [email protected]
Y. Song
State Key Laboratory of Coordination Chemistry,
Coordination Chemistry Institute, Nanjing University,
Nanjing 210093, People’s Republic of China
123
J Chem Crystallogr (2011) 41:1737–1741
DOI 10.1007/s10870-011-0166-8
hydrothermal by using 1,4-diazabicyclo[2.2.2]octane
(DABCO) as template. Although the inorganic framework is
similar with the reported literature, the guest molecules are
different. In the synthesis of 1 and 2, we used isonicotinic
acid and water as solvent to prevent the decomposed of
DABCO.
Experimental
General Remarks
Compounds 1 and 2 were prepared under hydrothermal
conditions. All chemicals purchased were of reagent grade
and used without further purification. The crystalline
product was characterized by thermogravimetric analysis,
single crystal XRD and IR spectrum. The element analyses
for C, H, and N analyses were performed on a Perkin-
Elmer 2400 elemental analyzer. IR spectra were recorded
on a Nicolet Impact 410 FTIR spectrometer using KBr
pellets. Thermogravimetric analyses were carried out in N2
atmosphere on a Diamond thermogravimetric analyzer
from 50 to 1,000 �C at a heating rate of 10 �C min-1.
X-ray Crystallographic Study
The single crystals of the 1 and 2 were affixed onto a thin
glass fiber by epoxy glue in air for data collection. And the
diffraction data were collected on a Bruker Apex 2 CCD
with Mo Ka radiation (k = 0.71073 A) at 296 K using
x - 2h scan method. An empirical absorption correction
was applied. All the non-hydrogen atoms were refined
anisotropically, while the hydrogen atoms of organic
molecule were refined in calculated positions, assigned
isotropic thermal parameters, and allowed to ride on their
parent atoms. All calculations were performed using the
SHELX97 program package [24]. Further details of the
X-ray structural analyses for compound 1 are given in
Table 1 and the selected bond lengths and angles are listed
in Table 2. CCDC 788161 and 788162.
Synthesis of Compounds 1 and 2
All the two compounds were prepared by a hydrothermal
method from a mixture of Ln2O3 (99.9%), HNO3
(65–68%), H2SO4 (95–98%) and DABCO (99.0%). In a
typical synthesis of 1, a solution was prepared by dis-
solving 0.0842 g Pr2O3 into 10.0 mL diluted nitric acid
(0.1596 g HNO3/10.0 mL H2O) under constant stirring for
an hour. Then 0.1205 g isonicotinic acid and 0.2233 g
DABCO was added into the solution under constant stirring
for 30 min. At last 0.2045 g H2SO4 was dropped into the
solution under stirring for 30 min, the final pH was 2.5.
The resulting mixture was transferred into a 25 mL Teflon-
lined stainless-steel autoclave and heated at 433 K for
3 days. The autoclave was slowly cooled to the room
temperature, and the product was washed with water and
dried in air for 1 day to give the green tabular crystals
(yield 30%, with respect to Pr). Elemental analyses for 1,
Anal. Calcd. (%): C, 12.30; H, 4.10; N, 4.78. Found: C,
12.44; H, 4.18; N, 4.54. IR (KBr pellet, cm-1): 3417 (m),
3191 (s), 1653 (m), 1635 (m), 1472 (m), 1095 (s), 604 (m).
The violet tabular crystals of 2 were prepared in the
same way as 1 by using Nd2O3 (0.0914 g) instead of Pr2O3.
The final yield was 46% (with respect to Nd). Elemental
analyses for 2, Anal. Calcd. (%): C, 12.25; H, 4.10; N,
4.76. Found: C, 12.06; H, 4.15; N, 4.68. IR (KBr pellet,
cm-1): 3417 (m), 3176 (s), 1653 (m), 1635 (m), 1473 (m),
1097 (s), 603 (m). The IR spectra of compounds 1 and 2
show the characteristic bands for DABCO in the region
1,400–1,600 cm-1. The strong bands around 1,097 cm-1
Table 1 Crystal data and structure refinement for 1
Compounds 1
Empirical formula C12H48N4O30Pr2S5
Formula weight 1170.66
Temperature 296(2) K
Wavelength 0.71073 A
Crystal system Orthorhombic
Space group Pbna
Unit cell dimensions a = 10.1362(13) A
b = 13.4782(17) A
c = 25.565(3) A
a = b = c = 90.00�Volume 3492.6(8) A3
Z 4
Calculated density 2.226 mg/m3
Absorption coefficient 3.170 mm-1
F(000) 2344
Crystal size 0.17 9 0.16 9 0.10 mm
h range for data collection 1.59–25.50�Limiting indices -12 B h B 12
16 B k B 14
Reflections collected unique 20470/3254 [Rint = 0.0376]
Absorption correction Semi-empirical from
equivalents
Refinement method Full-matrix least-squares on
F2
Data restraints parameters 3254/6/250
Goodness-of-fit on F2 1.322
Final R indices [I [ 2r(I)]R indices
(all data)
R1 = 0.0489,
wR2 = 0.1467
R1 = 0.0524,
wR2 = 0.1562
Largest diff. peak and hole 2.121 and -0.845 e A-3
1738 J Chem Crystallogr (2011) 41:1737–1741
123
can be attributed to the sulfate ion. Absorption at 603 cm-1
is due to Ln–O vibration. A band around 3,417 cm-1 can
be attributed to the presence of water and hydrogen bands.
Results and Discussion
Structural Description
Compounds 1 and 2 are isostructural and crystallize in
orthorhombic space group Pbna, and structures of both
compounds are similar to the reported layered lanthanide
sulfates. Take 1 as an example, the asymmetric unit of 1
contains 27 non-hydrogen atoms and of which 13 belong to
the inorganic layers, 8 to two organic moieties, 3 to the
interstitial sulfate ion with a � occupied S and two crystal-
lized water molecules, as shown in Fig. 1. In the layer of 1, Pr
is nine-coordinated by seven O atoms from four sulfates and
two O atoms from coordination water, forming a distorted
tricapped trigonal-prismatic geometry. The bond distances of
Pr–O vary from 2.464(4) to 2.604(4) A, whereas the angles of
O–Pr–O are between 54.09(12) and 156.15(14)�, which are in
accordance to other reported Pr compounds [13]. There are
two crystallographic independent S atoms: S(1) makes four
S–O–Pr linkages and links two adjacent Pr atoms through four
l2-O atoms (Pr–O–S bridges) to generate a zigzag [Ln–O–S–O]n
chain (Fig. 2a); S(2) makes three S–O–Pr linkages and
connects adjacent zigzag [Ln–O–S–O]n chains by using a
8-membered ring (Fig. 2b) to form an inorganic zigzag layer
of 1 along [0 0 1] plan as shown in Fig. 3. The inorganic
layer can be viewed as being built up of eight-membered
rings [–Pr–S(1)–Pr–S(2)–Pr–S(1)–Pr–S(2)–] forming of
four PrO9 polyhedra and four SO4 tetrahedra linked through
vertices, zigzag [Ln–O–S–O]n chains. All the S atoms are
tetrahedrally coordinated by four O atoms with the S–O
distances 1.449(8) to 1.498(6) A, which is similar to the
reported lanthanide sulfates [9, 11–13]. The layers are held
together by the N–H���O, C–H���O and O–H���O hydrogen
bonding assembly by diprotonated DABCO cations, water
molecules and free sulfate moieties, which of them are
located in the interlamellar space. The lanthanide sulfate
structure possesses a large number of hydrogen bond
Table 2 Selected bond lengths (A) and angles (�) for 1
Pr(1)–O(2W) 2.464(4) O(5)–Pr(1)–O(2) 75.66(13)
Pr(1)–O(1W) 2.470(4) O(5)–Pr(1)–O(4) 116.03(13)
Pr(1)–O(5) 2.538(4) O(2)–Pr(1)–O(4) 54.88(13)
Pr(1)–O(2) 2.543(4) O(5)–Pr(1)–O(8) 55.09(13)
Pr(1)–O(4) 2.551(4) O(2)–Pr(1)–O(8) 70.70(13)
Pr(1)–O(8) 2.557(4) O(4)–Pr(1)–O(8) 123.81(12)
S(1)–O(6) 1.470(4) O(6)–S(1)–O(8) 112.1(2)
S(1)–O(8) 1.491(4) O(5)–S(1)–O(8) 105.0(2)
S(2)–O(1) 1.466(4) O(1)–S(2)–O(2) 111.7(2)
S(2)–O(4) 1.483(4) O(2)–S(2)–O(4) 104.8(2)
S(3)–O(9) 1.449(8) O(9)–S(3)–O(10) 107.7(4)
S(3)–O(10) 1.498(6) C(2)–C(1)–N(1) 107.7(5)
C(1)–C(2) 1.501(9) N(2)–C(2)–C(1) 108.5(5)
C(1)–N(1) 1.521(9) N(1)–C(3)–C(4) 108.0(5)
C(2)–N(2) 1.496(8) N(2)–C(4)–C(3) 108.3(5)
C(3)–N(1) 1.484(8) N(1)–C(5)–C(6) 107.4(5)
C(3)–C(4) 1.512(9) N(2)–C(6)–C(5) 108.0(5)
C(4)–N(2) 1.504(8) C(3)–N(1)–C(5) 110.9(5)
C(5)–N(1) 1.487(9) C(5)–N(1)–C(1) 109.0(5)
C(5)–C(6) 1.533(10) C(6)–N(2)–C(2) 109.3(5)
C(6)–N(2) 1.495(9) C(6)–N(2)–C(4) 109.4(5)
O(2W)–Pr(1)–O(1W) 75.20(16)
Fig. 1 Molecular structure of the [C6H14N2]2[Pr2(SO4)4(H2O)4]
[SO4]�6H2O 1
Fig. 2 The SBUs of 1: zigzag Pr–O–S chain (a) and 8-membered
ring (b)
J Chem Crystallogr (2011) 41:1737–1741 1739
123
interactions involving the hydrogen atoms attached to the
protonated organic amine and free water molecule with
framework oxygen atoms (Fig. 4).
It is interesting to compare the structure of 1 with that of
b-(NH4)La(SO4)2 [25], (N2H5)Nd(H2O)(SO4)2 [26], and [Ln2
(SO4)4(H2O)4][C6H14N2]2[SO4][C2H8N2][H2O]3 (Ln = La,
Pr or Nd) [13]. In all these compounds, the interlamellar space
depends on the size and orientation of the guest species and
the distance increasing from 4.50 A for ammonium ion to 7.88
A for hydrazinium ion and 12.8–13.4 A for diprotonated
DABCO ion. According to the reported [Ln2(SO4)4(H2O)4]
[C6H14N2]2[SO4][C2H8N2][H2O]3 [13] the diprotonated
DABCO decomposed into ethylene and ethylenediamine,
whereas the same thing didn’t happen during the synthesis of
1. It is may be attributed to the mixed solvent of isonicotinic
acid and water.
The TGA curves of 1 and 2 given in Fig. 5 show distinct
mass losses. The total weight loss of 1 is 66.9%, which is in
agreement with the calculated value (68.5%). The weight
loss of 8.6% in the range of 40–150 �C corresponds to the
removal of three free water (the calculated value is 9.2%),
while the weight loss of 25.3% in the range of 150–480 �C
can be attributed to the loss of two coordination water and
DABCO molecules (the calculated value is 24.9%). The
last loss of 32.7% in the range of 480–980 �C can be
attributed to the loss of SO3 (the calculated value is
34.1%). The final product is Pr2O3. The weight loss of 2 is
similar to 1 and the final product is Nd2O3.
The magnetic susceptibility of compound 1 was measured
in the temperature ranging from 2 to 300 K and under 100 Oe
field. The vM value (Fig. 6) increases from 0.01
03 cm3 mol-1 at 300 K to a maximum of 0.0877 cm3 mol-1
at about 2 K. The vMT value of compound 1 is equal to
3.09 cm3 mol-1 K at room temperature, which is smaller
than the calculated value (3.20 cm3 mol-1 K) of one
uncoupled S = 1 spins of Pr(III) atoms. As the temperature
decreases, the value of vMT decreases continuously and
Fig. 3 The structure of inorganic layer in 1 along [0 0 1] plane
Fig. 4 Water, organic amine cations and sulfates are involved
hydrogen bonding interactions with inorganic layers. Yellow dottedlines represent the hydrogen bond interactions
Fig. 5 TG curves of 1 and 2
1740 J Chem Crystallogr (2011) 41:1737–1741
123
reaches 0.175 cm3 mol-1 K at 2 K, resulting from the
occurrence of intermolecular antiferromagnetic interaction
among neighbor Pr(III) ions. The 1/vM versus T plot for 1
could fit with Curie–Weiss equation from 90 to 300 K, giving
C = 3.557 cm3 mol-1 K and h = -44.4 K. The negative
Weiss constant indicates the existence of antiferromagnetic
interaction among the nearest magnetic centers.
Conclusions
In summary, we have successfully synthesized two lan-
thanide sulfates under hydrothermal conditions. Structure
analysis indicates that the inorganic frameworks of 1 and 2
are layered structure, while the free sulfate ions and the
organic template are resided among the layers. The for-
mation both compounds 1 and 2 indicates that the mixture
of isonicotinic acid and water as solvent plays an important
role to prevent the decomposed of DABCO during the
synthesis.
Acknowledgments We thank the National Natural Science Foundation
of China (20971068) for financial support.
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Fig. 6 The plots of vMT and 1/vM (inset) versus T for 1
J Chem Crystallogr (2011) 41:1737–1741 1741
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