106
N. Fridman et al. / Journal of Molecular Structure 917 (2009) 101–109
for 17 is observed at kmax(em) = 392 nm and kmax(em) = 383 nm at
very acidic solution, respectively, whereas at kmax(em) = 383 and
kmax(em) = 479 nm at very basic solution, respectively. One isos-
bestic point observed at 276 nm for 10 and two isosbestic point
at 286 and 314 nm found for 17. Fig. 5 represents the maxima of
that crystallize without solvent molecules (4–6, 10, 24, 17), and
those that crystallize with solvent molecules (2, 9, 16, 19, 20, 22).
In the first group, compounds 4–6 are identical except for the
substituent at the para position of the phenyl rings at 4 and 5 posi-
tions (Scheme 1) (H, Me, or OMe). The three compounds are iso-
morphous; having the same space group and very similar unit
cell dimensions. The five compounds (4–6, 10, 24) have similar
hydrogen bonding scheme (Fig. 6, Figures S4–S6). The molecules
are linked to each other through hydrogen bonds (Table 3) of the
type NH. . .N between the imidazole rings of neighbor molecules
forming infinite one-dimensional chain. It should be noted that
in the crystal structures of the five compounds there are no other
hydrogen bonds and the packing is therefore determined by the
formation of chains with van der Waals intermolecular interac-
tions. There are two crystallographic independent molecules of
24, one of them is disordered. The two molecules are also differing
significantly by the rotation angle of the bithiophene moiety rela-
tived to the plane of the imidazole ring (6.0° and 26.8°). The best
molecular fit is shown in Fig. 7. The crystal structure of compound
17 is different due to the presence of hydroxyl group at an ortho
position of the phenyl of position 2 of the imidazole ring. As a re-
sult, there are intramolecular hydrogen bonds between the hydro-
gen atom of the hydroxyl group and N atom of the imidazole ring
(Fig. 8). The hydroxyl group is also serving as a connector between
neighbor molecules via hydrogen bond. There are two crystallo-
graphic independent molecules in the asymmetric unit. The intra-
molecular hydrogen bond distances are given in Table 3.
the absorption (ma) and emission (mf) transitions of 10 and 17 in
acetonitrile as a function of pH. These spectra are indicative of sev-
eral acid–base equilibria that are possible in these systems (See
also Scheme 2). Moving from acidic to basic environment 17 exists
as the neutral species in the ground state at the range 0 6 pH 6 13,
forming [17–H+]ꢀ as revealed from its absorption spectra at
pH P 13. In contrast, in the excited state, 17 acts as a photoacid
that protonates at pH < 1, forming [17 +;H]+, and deprotonates at
pH P 13, forming [17ꢀH+]ꢀ as revealed from its emission spec-
trum. Comparing systems 17 with 10, a system that lacks the phe-
nolic proton, one can clearly see that the deprotonation step of 10
at around pH = 4 is almost identical to the deprotonation step of
17. This process is attributed to the formation of the neutral spe-
cies 10 out of the protonated system [10 + H+]+. Scheme 2 depicts
the proposed acid-base processes for 10 and 17. All the above phe-
nomena are similar to other proton transfer driven systems [21].
3.2. Crystallography
The molecular conformations of the various lophine derivatives
are very similar. The conformation may be defined by three rota-
tion angles marked as
at 4 and 5 positions are rotated in the same sense (the rotation
of angles and b ranges from 21.2 to 57.1°). The rotation angle
a, b, c in Scheme 1. The two phenyl rings
The second group consists of compounds that crystallize with
solvent molecules and form solvates. The number of acceptors
and donors for hydrogens in the solvent molecules determines
the crystal structures. The six solvates can be divided into two
a
c
is varied from 5.1 to 27.7° (Overlay of molecular structures is given
in Figures S1–S3 of the supplement materials). Although the differ-
ences are significant, the barrier to rotation is small and the rota-
tion can easily be a result of substituent or as a result of packing.
The crystal structure of the 12 compounds 2, 4–6, 9, 10, 16,17,
19, 20, 22, 24 may be divided into two classes; those compounds
Table 4
Crystallographic data and parameters for compounds 2, 4, 5 and 6
Parameters
2
4
5
6
Formula
Mr
C22H16N2Oꢀ2C2H6O C22H15N3
C24H19N3
349.42
Colorless
plate
C24H19N3O2
381.42
Yellow plate
Table 3
Geometry of hydrogen bonds
386.44
321.37
colorless
plate
Crystal color, habit Colorless prism
Compounds D–Hꢂ ꢂ ꢂA
d(D–H) d(Hꢂ ꢂ ꢂA) d(Dꢂ ꢂ ꢂA)
h(D–Hꢂ ꢂ ꢂ A)
(°)
(Å)
(Å)
(Å)
Crystal system Monoclinic
Orthorhombic Orthorhombic Orthorhombic
Crystal size (mm) 0.54 ꢃ 0.36
ꢃ 0.24
0.30 ꢃ 0.15
ꢃ 0.06
Pbca
8.875(2)
16.811(3)
23.825(5)
90
0.48 ꢃ 0.38
ꢃ 0.06
Pbca
9.042(2)
16.722(3)
25.791(5)
90
0.30 ꢃ 0.27
ꢃ 0.06
Pbca
9.806(2)
15.588(3)
26.201(5)
90
2
4
N1–H1N1ꢂ ꢂ ꢂ O2
0.86
0.82
0.82
0.86
1.95
2.04
1.77
2.13
2.784(2)
2.856(2)
2.580(2)
2.877(3)
163
177
169
144
O3–H3ꢂ ꢂ ꢂ N2
O1–H1ꢂ ꢂ ꢂ O3
N1–H1N1ꢂ ꢂ ꢂ N2
Space group
a (Å)
P21/c
11.470(2)
12.450(2)
15.720(3)
90
b (Å)
c (Å)
5
6
9
10
N1–H1N1ꢂ ꢂ ꢂ N2
N1–H1N1ꢂ ꢂ ꢂ N2
N1–H1N1ꢂ ꢂ ꢂ N2
N1–H1N1ꢂ ꢂ ꢂ O1
N1–H1N1ꢂ ꢂ ꢂ N2
N1–H1ꢂ ꢂ ꢂ O1S
N2–H2ꢂ ꢂ ꢂ O1W
O1W–H1W. . . O2S
N1A–H1NAꢂ ꢂ ꢂ O1B
0.92
0.86
0.86
0.86
0.82
0.86
0.86
0.91
0.86
2.05
2.48
2.10
2.29
2.49
2.04
2.06
2.36
1.95
2.881(2)
3.102(3)
2.958(16) 172
2.737(2)
3.314(2)
2.817(3)
2.923(3)
2.922(3)
2.809(2)
149
149
a
(°)
b (°)
113.32(2)
90
2061.5(7)
4
1.245
0.083
816
90
90
90
90
90
90
112
162
149
175
120
176
c
(°)
V (Å3)
3554.6(13)
8
1.201
0.072
1344
3899.61(14) 4005.0(14)
8
16
17
Z
8
Dcalcd. (g cmꢀ3
)
1.190
0.071
1472
50.1
6442
1.265
0.082
1600
50.1
5880
l
(MoK ) (cmꢀ1
)
a
F(000)
2hmax (°)
50.1
47.7
9333
N1B–H1NBꢂ ꢂ ꢂ O1A
O1B–H1OBꢂ ꢂ ꢂ N2B
0.86
0.82
1.97
2.832(2)
174
Reflections
collected
Independent
reflections
6842
1.78
1.76
2.08
2.530(2)
2.516(2)
2.931(3)
151
152
172
3637
2734
3448
3358
O1A–H1OAꢂ ꢂ ꢂ N1B 0.82
19
20
N1–H1N1ꢂ ꢂ ꢂ O1S
0.86
Largest difference 0.287
peak (e Åꢀ3
Largest difference ꢀ0.205
hole (e Åꢀ3
0.086
ꢀ0.086
0.128
ꢀ0.163
0.188
ꢀ0.168
)
O1–H1O1ꢂ ꢂ ꢂ N2
N2–H2N2ꢂ ꢂ ꢂ O1S
0.82
0.86
1.96
2.04
2.780(3)
2.889(2)
174
160
)
No. of parameters 276
228
337
277
O1S–H1Sꢂ ꢂ ꢂ O1
O3–H3O3ꢂ ꢂ ꢂ N1
N2–H2N2ꢂ ꢂ ꢂ O2
O1–H1O1ꢂ ꢂ ꢂ N1
0.96
0.82
0.86
0.82
1.88
1.89
2.04
1.90
2.11
2.830(2)
2.618(2)
2.897(5)
2.719(5)
2.908(3)
171
148
175
171
154
Ra
0.0455
0.1335
0.935
0.0448
0.1310
0.953
0.0443
0.1196
0.921
0.0470
0.1010
0.794
wRa
GOFb
22
24
N2A–H2NAꢂ ꢂ ꢂ N1B 0.86
P
P
P
P
2
2 1=2
a
R ¼
j Fo j ꢀ j Fc j = j Fo j; wR ¼ ½ wðj Fo j ꢀ j Fc j Þ = w j Foj ꢄ
.
P
GOF ¼ ½ wðj Fo j ꢀ j Fc j Þ =ðNO ꢀ NVÞꢄ1=2, where NO is the number of obser-
2
b
N2B–H2NBꢂ ꢂ ꢂ N1A 0.86
2.08
2.919(3)
166
vations and NV is the number of variables.