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ORI GIN AL PA PER
Synthesis and Characterization of a NewNoncentrosymmetric Dihydrogenmonophosphate[C12H13N2O]H2PO4
Sami Soukrata • Mohamed Belhouchet • Tahar Mhiri
Received: 17 June 2014
� Springer Science+Business Media New York 2014
Abstract The organic–inorganic hybrid material [C12H13N2O]H2PO4 has been
synthesized at room temperature by slow evaporation. The compound crystallizes in
the noncentrosymmetric orthorhombic space group P212121 with the lattice
parameters a = 4.75 (5) A, b = 10.26 (5) A, c = 27.09 (3) A, Z = 4 and
V = 1323.3 (2) A3. The crystal structure has been determined and refined to
R1 = 0.047 and wR2 = 0.120 using 2870 independent reflections. The atomic
arrangement can be described by infinite anionic chains running parallel to the
a axis. The organic cations are linked to the inorganic chains by hydrogen bonds so
as to build a two-dimensional network. The infrared spectroscopy confirms the
presence of the organic group and the anionic entities. Concerning the differential
scanning calorimetry, it revealed one phase transition at 71 �C. Thermal analysis
was performed to study its thermal stability. Besides, the impedance spectroscopy
study, reported in the sample, reveals that the conduction in the material is due to a
Grotthus mechanism.
Keywords Inorganic compounds � Chemical synthesis � Infrared and NMR
spectroscopy � Thermal analysis � Electrical conductivity
Introduction
The prospect of creating new functional materials with tunable properties gives a
strong motivation on the research of organic–inorganic hybrid materials [1]. Interest
in these compounds with noncentrosymmetric structures has grown due to their
application in various fields such as e.g. quadratic non- linear optical research [2].
S. Soukrata (&) � M. Belhouchet � T. Mhiri
Laboratoire Physico-Chimie de l’Etat Solide. Departement de Chimie. Faculte des Sciences de Sfax,
Universite de Sfax, 3018 Sfax, Tunisie
e-mail: [email protected]
123
J Clust Sci
DOI 10.1007/s10876-014-0771-8
The synthesis of low-dimensional mixed organic–inorganic materials enables both
inorganic and organic components on the molecular scale to be optimized and thus
to exhibit specific properties, such as electronic, catalytic, optical, and second-order
non-linear optical to name just a few [3–6]. Among these hybrid compounds,
organic phosphates are particularly significant and their anions are interconnected
by strong hydrogen bonds so as to build infinite networks with various geometries
such as ribbons [6], chains [7], or layers [8, 9]. Considering the attractive properties
of organic phosphates and the new promising opportunities they may open with
regard to the development of useful organic–inorganic hybrids materials. In fact, the
current paper reports the synthesis, crystal structure, thermal behavior, vibrational
study and the dielectric measurements are combined to provide a good description
of this compound.
Experimental
Materials and Measurements
Infrared spectrum was diluted at room temperature on a Perkin-Elmer FT-IR
Spectrometer as KBr pellets in the region 4000–400 cm-1 region. All NMR spectra
were obtained on a Bruker DSX-300 spectrometer operating at 75.49 MHz for 13C
and 121.51 MHz for 31P, with classical 4-mm probehead allowing spinning rates up
to 10 kHz. 13C NMR chemical shifts are given relative to tetramethylsilane, while
the 31P ones are relative to 85 % H3PO4 (external reference precision 0.5 ppm). The
phosphorus spectrum was recorded under classical MAS conditions, while the
carbon ones was recorded by the use of crosspolarization from protons (contact time
5 ms) and MAS. In all cases, it was checked that there was a sufficient delay
between the scans, allowing a full relaxation of the nuclei. Simultaneous
thermogravimetry (TG) and differential thermal analyses (DTA) of a powdered
sample were performed in the temperature range of 25–450 �C, using a Setaram
TG–DTA92 thermo analyser, at a heating rate of 5 �C min-1. Differential scanning
calorimetry (DSC) measurements were measured in the temperature range of
25–300 �C using a Mettler Toledo DSC model DSC30 with samples placed inside
platinum crucibles at heating rate of 10 �C/min. Regarding the electrical conduc-
tivity, they were performed by means of a two-electrode configuration. Besides, the
polycrystalline [C12H13N2O]H2PO4 sample was pressed into pellets of 8 mm in
diameter and 1.1 mm in thickness using 3 tons/cm2 uniaxial pressures. The ac
conductivity measurements were performed with a Tegam 3550 impedance analyser
(209–4.63 MHz) which was also interfaced with a computer and a temperature
controller. Measurements were taken at temperatures from 291 to 393 K.
Chemical Preparation
Transparent plates of compound were synthesized in good yields by an alcoholic
reaction of phosphoric acid (0.098 g, 1 mmol Aldrich 85 %) with 2-amino-3-
S. Soukrata
123
benzyloxy pyridine (0.2 g, 0.99 mmol Aldrich 99 %) followed by slow evaporation
at room temperature.
X-ray Crystallography
Intensity data of the compound were collected using a Kappa CCD diffractometer
(Bruker-Nonius) using graphite monochromated MoKa radiation (k = 0.71073 A).
The structure was solved with a direct method from the SHELXS-97 program
[11].Which permitted the location of the PO4 groups. The remaining non-hydrogen
atoms, were deduced from difference Fourier maps during the refinement. All
hydrogen atoms were geometrically fixed by appropriate instructions of the
SHELXL-97 program [11] and held in the riding mode. The successive refinements
lead to a reliability factors of R1 = 0.047 and wR2 = 0.120. The crystal data and
details of data collection and refinement are summarized in Table 1.
Results and Discussion
Structure Description
The X-ray analysis of the title compound revealed that the asymmetric unit is
composed of one [C12H13N2O]? cation and one [H2PO4]- anionic unit (Fig. 1).
Figure 2 shows that the [H2PO4]- entities are connected by strong hydrogen
bonds, O(1)–H(O1)…O(4) and O(3)–H(O3)…O(2), to form double infinite chains
running parallel to the a axis. The detailed geometry of the H2PO4- groups,
gathered in Table 2, shows two types of P–O distances depending on whether the
oxygen atoms are hydrogen donors or acceptors. As expected, the P–OH distances
ranging from 1.566 (2) A to 1.568 (2) A, is significantly longer than the P–O
distances ranging from 1.501 (2) A to 1.508 (2) A. The average values of the P–O
distances and the O–P–O angles are 1.535 (2) A and 109.37 (2)�, respectively.
These values are generally in excellent agreement with other phosphates [13–15]. It
is worth noting that the O…O distances involved in the hydrogen bonds [2.587 (3)
and 2.591 (3) A] are of the same order of magnitude as in the H2PO4 tetrahedron
[between 2.446 (4) and 2.536 (4) A]. Such distances along with the short P…P
distance of 4.449 (2) A allow us to consider the [H4P2O8]n2n- network as a
polyanion. This result has also been noticed in other crystal structures [16–18]. With
regards to the organic-cation arrangement, the main features measured are similar to
intramolecular bond distances and angles usually reported for such species [18, 19].
The calculated average values of distortion indices [20], correspond to the different
angles and distances in the PO4 tetrahedra [DI(OPO) = 0.0206, DI(PO) = 0.0203,
DI(OO) = 0.0078] exhibit a pronounced distortion of the O–P–O angles and P–O
distances if compared to O–O distances. So, the PO4 group can be considered as a
rigid regular arrangement of oxygen atoms, with the phosphorus atom slightly
displaced from the gravity center. The perspective view display in the Fig. 3 shows
that the organic entities, are lodged between the anionic chains through N–H…O
hydrogen bonds to form a two dimensional network. An examination of the organic
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
moiety geometrical features shows that the dihedral angle between the pyridine ring
and benzene plane is 80.17�. Furthermore, the mean value of the C–C bond lengths
is equal to 1.391 (5) A, being the distance between single bond and double bond,
which agrees well with that in benzene [21]. Besides, the C–N, C–C bond lengths
vary from 1.314 (4) to 1.506 (4) A, the C–C–N, C–C–C angles are included between
Table 1 Crystal data and structure refinement of the title compound
Empirical formula [C12H13N2O]H2PO4
Formula weight 298.23
Crystal system / space group Orthorhombic / P212121
a /A 4.75 (5)
b /A 10.26 (5)
c /A 27.09 (3)
V /A3 1323.3 (2)
Z 4
D calc (g/cm3) 1.497
l (mm-1) 0.23
Crystal size (mm) 0.3 9 0.2 9 0.1
Color / shape Transparent / plate
Temp (K) 293
Theta range for collection 1.5–27
Reflections collected 9068
Independent reflections 2870
Data/restraints/parameters 2466/0/168
Goodness of fit on F2 1.00
Final R indices [I [ 2r(I)] 0.047
R indices (all data) 0.120
Largest difference peak/hole -0.34 / 0.66
Fig. 1 Asymmetric unit of [C12H13N2O]H2PO4
S. Soukrata
123
117.7 (3) and 123.5 (3)�, and C–C–O, C–O–C angles spread from 112.2 (3) to 128.0
(3)� Table 2. The crystal structure exhibits two types of hydrogen bonds, the first of
which, O–H…O, involve one short contact with H…A distances ranging from 1.78
to 1.79 A. The second one, N–H…O bonds, with H…A distances ranging from 1.76
to 2.05 A with D–H…A angles spread from 169 to 176� establishes the contact of
organic cation with the anionic chains (Table 3). This atomic arrangement includes
four hydrogen bond donors (two N and two O atoms) and two hydrogen bond
acceptors (O(2) and O(4) atoms).
NMR Spectroscopy
The solid state 31P MAS-NMR spectrum of the title compound is show on Fig. 4.
The spectrum exhibits a single resonance peak at 0.98 ppm. This value agrees with
those corresponding to monophosphate (between -10 and 5 ppm) [21–23] and is in
agreement with only one phosphorus crystallographic site in the structure. The 13C
CP-MAS NMR spectrum is show on Fig. 5. It displays ten different signals,
corresponding to twelve carbon atoms of the organic cation. The first one, whose
chemical shift peak is 68.5 ppm, is attributed to the methylene group substituted
found in the compound under study. The most shifted NMR components, whose
chemical shifts range from 111.8 to 147.3 ppm, are attributed to the aromatic carbon
atoms. To assign NMR components to different carbon atoms, the chemical shifts
have been calculated by means of the Chem Draw Ultra 6.0 software. The carbon
atoms are labeled in Fig. 1. The obtained results are gathered in Table 4, prove the
presence of only one organic moiety in the asymmetric unit of the compound which
agrees with the X-ray diffraction data.
IR Spectroscopy
To gain more information on the crystal structure, we have undertaken a vibrational
study using infrared spectroscopy. The infrared spectrum of the studied compound
at room temperature is show in Fig. 6. The assignments of the observed bands are
realized by comparison with similar compounds [19, 24]. Besides, the wavenumbers
of the observed peaks are quoted in Table 5. The isolated [PO4]3- tetrahedron with
an ideal Td symmetry has four vibrational modes; two stretching modes, m3 and m1
and two deformation modes, m4 and m2. These modes are observed at 1017, 938, 567
and 420 cm-1, respectively [25]. The three strong bands at 1090, 1062 and
1038 cm-1 are assigned to m3[PO4]3-. The stretching mode m1 appears as one strong
band at 980 cm-1. The bending vibrations arising from the m4[PO4]3-of the
phosphate anions are observed as three bands at 622, 580, and 496 cm-1. Next, the
medium band observed at 412 cm-1 is proposed as originating from m2[PO4]3-
bending vibrations. The broad bands with frequencies in the range of 3500 and
2700 cm-1 are attributed to the stretching of the organic and hydroxyl groups
(m(N–H), m(C–H)), and m(O–H) of P-OH groups. The ABC type bands characteristic
of the OH modes in the H2PO4 groups are barely perceived between 2500 and
1700 cm-1. The observed bands at 1628, 1584 and 1526 cm-1 are assigned to the
bending modes of the NH2 moiety (das(NH2) and ds(NH2), respectively). The
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
intense band around 1386 cm-1 is assigned to the m(C = C) vibration mode. The
bands which appear from 1494 to 1412 cm-1 are attributed to the bending mode
d(CH2). The observed bands at 1284-1158 cm-1 are assigned to m(C–N), m(C–C),
d(C–H), d(N–H) and d(OH).
Thermal Analysis
The thermal behavior of [C12H13N2O]H2PO4 has been studied by TG-DTA and
DSC from room temperature to 400 �C. Figure 7 shows the TG and DTA
thermograms of the anhydrous compound in which thermal behavior occurs in three
stages. The first one represented by an endothermic peak at 73 �C corresponds to the
phase transition. The second stage related to the endothermic peak at 168 �C is
attributed to the anhydrous compound. The third stage representing a set of
endothermic peaks in the range of 170–350 �C is assigned to the degradation of the
compound. This phase transition is confirmed by differential scanning calorimetry
(DSC) at 71 �C (Fig. 8).
Electrical Conductivity
The study of the dielectric properties is an important source for valuable
information about conduction processes [26]. Some complex impedance diagrams
Z00 versus Z0 cole–cole plots recorded at various temperatures are given in Fig. 9a
and b. The difference between the cole–cole and Debye law is determined by a (p/2)
Fig. 2 Projection along the b-axis of the inorganic entities of the title compound
S. Soukrata
123
dispersion angle when a = 0.122. The intercept on the real axis of the zero phases
angle extrapolation of the highest-frequency curve determines the bulk ohmic
resistance relative to experimental temperature and it is used to show the evolution
of the conductivity versus inverse temperature. The curves show the temperature
dependence on the resistance proving the protonic-conduction properties. Thermal
evolution of conductivity for the title compound is presented in Fig. 10. The plot in
this figure shows the evolution of the conductivity Log (rT) versus 103/T for the
compound under study. The conductivity to this compound is significant and
increases from r = 2.38 10-8 X-1 cm-1 at 291 K to r = 6.26 10-4 X-1 cm-1 at
393 K. We point out that the break in this curve observed around 348 K,
is accompanied by an increase of the activation energy (Ea1 = 0.2 eV,
Ea2 = 1.306 eV). It can be noted that this compound presents in the range of
temperature from 291 K to 338 K a behavior capacitive. Also, this compound
presents from the temperature 348 K a behavior resistive. This important evolution
Table 2 Interatomic distances (A) and angles (�) of [C12H13N2O]H2PO4
Tetrahedron PO4
P O1 O2 O3 O4
O1 1.566 (2) 110.03 (2) 102.6 (2) 109.6 (2)
O2 2.518 (3) 1.508 (2) 109.8 (2) 112.8 (2)
O3 2.446 (4) 2.517 (3) 1.568 (2) 111.4 (2)
O4 2.507 (4) 2.506 (3) 2.536 (4) 1.501 (2)
O1—H(O1) = 0.820 P—O1—H(O1) = 109.5
O3—H(O3) = 0.820 P—O3—H(O3) = 109.5
Organic cation
C1—N1 1.314 (4) O5—C6 1.450 (4)
C1—N2 1.332 (4) C6—C7 1.506 (4)
C1—C5 1.427 (4) C7—C8 1.378 (4)
N2—C2 1.361 (4) C7—C12 1.390 (4)
C2—C3 1.359 (4) C8—C9 1.361 (5)
C3—C4 1.403 (4) C9—C10 1.342 (5)
C4—C5 1.371 (4) C10—C11 1.356 (5)
C5—O5 1.361 (4) C11—C12 1.409 (5)
N1—C1—N2 120.3 (3) C5—O5—C6 118.8 (3)
N1—C1—C5 121.9 (3) O5—C6—C7 112.2 (3)
N2—C1—C5 117.7 (3) C8—C7—C12 118.3 (3)
C1—N2—C2 123.5 (3) C8—C7—C6 120.8 (3)
C3—C2—N2 120.1 (3) C12—C7—C6 120.9 (3)
C2—C3—C4 119.0 (3) C7—C8—C9 121.4 (3)
C5—C4—C3 120.0 (3) C10—C9—C8 120.6 (4)
O5—C5—C4 128.0 (3) C9—C10—C11 120.6 (4)
O5—C5—C1 112.4 (3) C10—C11—C12 120.1 (4)
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
confirms the protonic conductor character of our material. The sudden variation of
the conductivity at 348 K marks the transition already observed by the DSC analysis
at 346 K. This phase transition can be explained by a more disordered state, which
might be correlated with changes in the orientation of molecular entities as
[C12H13N2O]? or [H2PO4]- and to the high dynamical disorder of NH2 groups in
the hydrogen N–H…O bonds. Dielectric relaxation studies have been undertaken at
temperature between 348 and 393 K, in the formalism of the complex electric
modulus M*. For a given temperature and frequency, the real part M0 and the
imaginary part M00 of the M* complex modulus (M* = M0 ? j M00) have been
calculated from the complex data (Z* = Z0 - jZ00) by the relations M0 = xC0Z00
and M00 = xC0Z0. The plots of log M0 and the normalized M00/M00max imaginary part
of the complex modulus of [C12H13N2O]H2PO4 versus log (f) are given in Figs. 11
and 12 at various temperatures. Whatever the temperature, the value of M0 reaches,
at high frequencies, a constant value (M0 = 1/e?) at high frequencies and at low
Fig. 3 Perspective view of [C12H13N2O]H2PO4 compound. (H-bonds are represented by dashed lines)
Table 3 Hydrogen bond geometry of [C12H13N2O]H2PO4
D—H���A D—H H���A D���A D—H���A
O1—H(O1)���O4i 0.82 1.79 2.591 (4) 165
O3—H(O3)���O2ii 0.82 1.78 2.587 (3) 167
N2—H2A���O2 0.86 1.76 2.609 (3) 169
N1—H1A���O4 0.86 2.05 2.910 (4) 176
Symmetry codes: (i) x-1, y, z; (ii) x?1, y, z?1; (iii) -x?1, y-1/2, -z?1
S. Soukrata
123
frequencies it approaches zero, which indicates that the electrode polarization
phenomenon make a negligible contribution to M* and maybe ignored when the
electric data are analyzed in this form [27]. The M00/M00max spectrum relative to a
Fig. 4 31P MAS-NMRspectrum of [C12H13N2O]H2PO4
Fig. 5 13C MAS-NMR spectrum of [C12H13N2O]H2PO4 compound
Table 4 Calculated and experimental chemical shifts of the carbon atoms of the organic entity
Carbon atoms C6 C3 C4 C8 and
C12
C10 C9 and
C11
C2 C7 C5 C1
dcal. (ppm) 70.9 113.5 122.3 127.2 127.7 129.0 139.8 141.2 141.6 148.6
dexp. (ppm) 68.5 111.5 119.6 126.4 130.3 133.9 136.2 141.1 147.2 147.8
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
given temperature shows an asymmetrical peak. The modulus peak maximum shifts
to higher frequencies as temperature increases. The region to the left of the peak is
where the H? protons are mobile over long distances, whereas the region to the right
Fig. 6 IR spectrum of [C12H13N2O]H2PO4
Table 5 Spectral data and band assignments of the title compound
IR wavenumbers (cm-1) Assignment
3470 vs m(OH)
3288 vs ms(NH)
3144-2690 s mas(NH) ? m(C–H)
2440 -1970 m m(OH) ‘‘A ? B ? C’’
1628 vs das(NH2)
1584 m -1526 s ds(NH2)
1494 vs -1412 vs d(CH2)
1386 s m(C=C)
1346 s w(CH2)
1284 vs -1158 m m(C–N) ?m(C–C) ? d(C–H) ? d(N–H) and d(OH)
1090 s -1038 s m3(PO4)
980 s m1(PO4)
882 m
812 s
746 vs -700 s r(CH2)
622 m
580 m
540 s -496 s m4(PO4)
412 m m2(PO4)
S. Soukrata
123
is where the ions are spatially confined to their potential wells. The frequency range
where the peak occurs is indicative of the transition from short-range to long-range
mobility at decreasing frequency and is defined by the condition xsr = 1, where
sr is the most probable proton relaxation time [28]. In summary, the electric
properties of this hybrid compound may be interpreted by the following way: The
rise of temperature can favor the vibration of the inorganic chains, which induce a
rapid reorientation H2PO4- and fast H? moving [30]. The fact that the OH groups
Fig. 7 TG-DTA thermogram of [C12H13N2O]H2PO4 compound
Fig. 8 DSC curve of [C12H13N2O]H2PO4
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
Fig. 9 a Complex impedance diagrams (-Z00 versus Z0) for [C12H13N2O]H2PO4 at T = [291–363 K],b Complex impedance diagrams (-Z00 versus Z0) for [C12H13N2O]H2PO4 at T = [368–393 K]
S. Soukrata
123
belonging to the phosphate anions form infinite chains is strongly in favor of a
protonic mobility between the oxygens of the phosphate anions. Indeed, the H2PO4-
anion performs both as proton donor and acceptor, by its four oxygen atoms, thus
producing an extended intermolecular H- bonds network, through which structural
migration of proton may occur via Grotthus mechanism [30]. The literature provides
many examples of this type of situation [14, 15].
Fig. 10 Arrhenius plot of the electrical conductivity of the compound
Fig. 11 A plot of log M0 versus log (f) at various temperature for [C12H13N2O]H2PO4
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123
Conclusion
The present study reports on the synthesis and subsequent characterization of a
novel hybrid compound [C12H13N2O]H2PO4. This compound has been character-
ized by various physico-chemical methods. On the structural level, the atomic
arrangement of the title compound can be described by infinite anionic chains
running parallel to the a axis. The organic cations are linked to the inorganic chains
by hydrogen bonds so as to build a two-dimensional network. The number of solid-
state 13C and 31P MAS NMR components agrees perfectly with the ones of
crystallographically in dependent sites. Indeed, the thermal analysis results allow us
to show clearly that the compound presents an anhydrous character. The vibrational
properties of this compound were studied by Raman scattering and infrared
spectroscopy. The assignment of the vibrational bands was based on comparisons
with vibrational mode frequencies of homologous compounds. Finally, the
impedance spectroscopy study, reported in the sample, reveals that the conduction
in the material is due to a Grotthus mechanism.
References
1. D. B. Mitzi and P. Brock (2001). Inorg Chem 40, 2096–2104.
2. R. Masse, M. Bagieu-Beucher, J. Pecaut, J. P. Levy, and J. Zyss (1993). Nonlinear Opt 5, 413–423.
3. N. Kimizuka and T. Kunitake (1996). Adv. Mater 8, 89–91.
4. D. B. Mitzi, K. Chondroudis, and C. R. Kagan (2001). IBM J. Res. Dev 45, 29–45.
5. H. Suzuki, K. Notsu, Y. Takeda, W. Sugimoto, and Y. Sugahara (2003). Chem Mater 15, 636–641.
6. A. M. Guloy, Z. J. Tang, P. B. Miranda, and V. I. Srdanov (2001). Adv. Mater 13, 833–837.
Fig. 12 A plot of normalized modulus (M00/M00max) versus log (f) at various temperature for[C12H13N2O]H2PO4
S. Soukrata
123
7. L. Baoub and A. Jouini (1998). J Solid State Chem 141, 343–351.
8. A. Rayes, C. Ben Nasr, and M. Rzaigui (2004). Mater. Res. Bull 39, 1113–1121.
9. K. Kaabi, C. Ben Nasr, and M. Rzaigui (2004). J. Phys. Chem. Solids 65, 1759–1764.
10. K. Kaabi, A. Rayes, C. Ben Nasr, M. Rzaigui, and F. Lefebvre (2003). Mater Res Bull 38, 741–747.
11. G. M. Sheldrick SHELXS-97 Program for the Solution of Crystal Structures (University of Gottingen,
Germany, 1997).
12. G. M. Sheldrick SHELXL-97 Program for Crystal Structure Refinement (University of Gottingen,
Germany, 1997).
13. A. Rayes, C. Ben Nasr, and M. Rzaigui (2004). Mat. Res. Bull 39, 1113–1121.
14. I. Ben Djema, Z. Elaoud, T. Mhiri, R. Abdelhedi, and J. M. Savariault (2007). Solid State Commun
142, 610–615.
15. Z. Elaoud, S. AL-Juaid, T. Mhiri, and A. Daoud (2007). J. Alloy. Compd 442, 306–309.
16. F. Berrah, S. Bouacida, and T. Roisnel (2011). Acta Crystallogr E67, o1409–o1410.
17. S. Akriche and M. Rzaigui (2007). Acta Crystallogr. E63, o3460.
18. R. Ittyachan, P. Sagayaraj, and B. Kothandapani (2003). Acta Crystallogr. E59, o886–o888.
19. L. Guelmami, A. Gharbi, and A. Jouini (2012). J. Chem. Crystallogr 42, 549–554.
20. H. Dhaouadi, H. Marouani, M. Rzaigui, and A. Madani (2006). Phosphorus, Sulfur Silicon Relat.
Elem 181, 1801–1814.
21. W. H. Baur (1974). Acta Crystallogr. B30, 1195–1215.
22. Z. J. Li, X. M. Chem, Z. X. Ren, Y. Li, X. A. Chem, and Z. T. Huang (1997). Chinese. J. Struct.
Chem 16, 311–314.
23. S. Prabhakar, K. J. Rao, and C. N. R. Rao (1987). Chem. Phys. Letters 139, 96–102.
24. P. Hartmann, J. Vogel, and B. Schnabel (1994). J. Magn. Reson. 111, 110–114.
25. A. Oueslati, A. Touati, C. Ben Nasr, and F. Lefebvre (2006). Phosphorus, Sulfur Silicon Relat. Elem
181, 2117–2133.
26. K. Nakamoto (1986). Infrared and Raman Spectra of Inorganic and Coordination Compounds, Part
A: theory and Applications in Inorganic Chemistry (Wiley. New York 1986, 202.
27. R. Ayouchi, D. Leien, F. Martin, M. Gabas, E. Dalchiele, and J. R. Ramos (2003). Barrodo. Thin
Solid Films 426, 68–77.
28. F. S. Howell, R. A. Bose, P. B. Macedo, and C. T. Moynihan (1974). J. Phys. Chem 78, 639–648.
29. H. K. Palet and S. W. Martin (1992). Phys. Rev B.45, 10292–10300.
30. A. Schechter and R. F. Savinell (2002). Solid State Ionics 147, 181–187.
31. O. Labidi, P. Roussel, M. Huve, M. Drache, P. Conflant, and J. P. Wignacourt (2005). J. Solid State
Chem 178, 2247–2255.
Noncentrosymmetric Dihydrogenmonophosphate [C12H13N2O]H2PO4
123