supporting information · 2018. 4. 9. · s9 x-ray diffraction analysis the crystal of 2a (c 94 h...
TRANSCRIPT
Supporting Information
Optical Readout of Controlled Monomer-Dimer Self-Assembly
P. A. Tarakanov,*ab
E. N. Tarakanova,a P. V. Dorovatovskii,
c Y. V. Zubavichus,
c V. N. Khrustalev,
d
S. A. Trashin,ae
K. De Wael,e M. E. Neganova,
a D. V. Mischenko,
b J. L. Sessler,
f P. A. Stuzhin,
g
V. E. Pushkarev*ah
and L. G. Tomilovaah
a Institute of Physiologically Active Compounds, Russian Academy of Sciences, 1 Severny Proezd, 142432
Chernogolovka, Moscow Region, Russian Federation. E-mails: [email protected];
[email protected] b Institute of Problems of Chemical Physics, Russian Academy of Sciences, 1 Academician Semenov Avenue,
142432 Chernogolovka, Moscow Region, Russian Federation c National Research Centre “Kurchatov Institute”, 1 Akad. Kurchatov Sq., Moscow 123182, Russia
d Inorganic Chemistry Department, Peoples’ Friendship University of Russia (RUDN University), 6
Miklukho-Maklay St., Moscow 117198, Russian Federation e AXES Research Group, Department of Chemistry, University of Antwerp, Groenenborgerlaan 171, 2020
Antwerpen, Belgium f Department of Chemistry, Shanghai University, Shanghai 200444, China
g Research Institute of Macroheterocycles, Ivanovo State University of Chemistry and Technology, 153000
Ivanovo, Russia h Department of Chemistry, M.V. Lomonosov Moscow State University, 1 Leninskie Gory, 119991 Moscow,
Russian Federation
Table of Contents
General Information S2
Synthesis S2
NMR Spectra S3
X-ray Diffraction Analysis S9
Studies of the Extent of Dissociation S11
Studies of the Influence of Fluoride Ion Concentration on the Dimer-Monomer Equilibria S12
Electrochemistry S19
In Vitro and in Vivo Toxicity Tests S21
References S21
Electronic Supplementary Material (ESI) for Dalton Transactions.This journal is © The Royal Society of Chemistry 2018
S2
General Information
UV-vis spectra were recorded on a Hitachi U-2900 spectrophotometer using quartz cuvettes (10 × 10 mm)
with the samples dissolved in pyridine, DMSO, o-DCB, unless otherwise specified. 1H and
13C NMR spectra
were recorded on Bruker Avance 500 (500 and 125 MHz, respectively) with the samples dissolved in
pyridine-d5 or DMSO-d6. Chemical shifts are given in parts per million (ppm) relative to TMS. Matrix-
assisted laser desorption/ionization time-of-flight (MALDI-TOF) mass spectra were acquired on a VISION-
2000 mass spectrometer with α-cyano-4-hydroxycinnamic acid (CHCA) as the matrix. Size exclusion column
chromatography was carried out using Bio-Beads S-X1 resin (BIORAD) eluted with pyridine. All other
reagents and solvents were obtained or distilled according to standard procedures. All reactions were
controlled by TLC and UV-vis until complete disappearance of the starting materials, unless otherwise
specified.
Electrochemical measurements were carried out in pyridine using a conventional three-electrode cell and
Autolab/PGSTAT101 (Metrohm Autolab B.V., the Netherlands). A double junction Ag/AgCl reference
electrode (Metrohm, Switzerland) was filled with 2 M LiCl in ethanol as the reference (inner) electrolyte and
0.1 M [TBA][BF4] in pyridine as the bridge electrolyte. Before making any measurements, a platinum disk
working electrode (2 mm in diameter, BASi, USA) was regenerated by polishing with an abrasive paper (grit
400), washed with ultrapure water and drying. Blank voltammograms were recorded in pure pyridine
containing 0.1 M [TBA][BF4] and then approximately 1 mM of a sample was introduced into the cell. After a
series of measurements, ferrocene was added as internal reference, and additional voltammograms were
recorded. Before the measurements the solutions were purged with N2 for at least 30 min. All measurements
were performed at room temperature (22 ± 2°C).
Synthesis
General procedure for the preparation of complexes 2a,b. Mg metal (50 mg) was boiled in isoamyl
alcohol (50 mL) in the presence of a catalytic amount of I2 until complete dissolution was observed (ca. 3 h).
The solution of the resulting Mg alkoxide was cooled to room temperature, 1,4-diazepine-2,3-dicarbonitrile
1a or 1b (1 mmol) was added, and the mixture was heated at reflux for 16 h. The course of the reaction was
monitored by UV-vis spectroscopy. Then, the reaction mixture was cooled to room temperature and the
solvent was evaporated under reduced pressure. The resulting dry residue was successively washed with 50%
aqueous acetic acid (4 × 50 mL), a 5% aqueous solution of sodium bicarbonate (2 × 50 mL), distilled water (4
× 50 mL) and finally with MeOH (50 mL) followed by drying in vacuo at 50 °C. The resulting solid was
subjected to gel permeation chromatography (Bio-Beads S-X1, pyridine). This yielded 2a and 2b in the form
of dark-green solids.
Tetrakis{5,7-bis[2’-(4-bromophenyl)ethenyl]-6H-1,4-diazepino}[2,3-b,g,l,q]porphyrazinato magnesium
(II) (2a). Yield 0.44 g (86%). UV-vis (DMSO) λmax/nm (log ε): 387 (4.77), 659 (4.59), 700 (4.41). 1H NMR
(500 MHz; DMSO-d6) δ/ppm: 8.20 (8H, d, 3J = 15.9 Hz, 2'-H), 7.7–7.65 (24H, br m, 1'-H; H
o-Ar), 7.47 (16H,
br s, Hm-Ar
), 6.11 (4H, br s, Heq
), 4.77 (4H, br s, Hax
). 13
C NMR (125 MHz; Py-d5) δ/ppm: 154.99, 149.19,
143.05, 137.46, 132.50, 131.68, 129.82, 37.75. MS (MALDI-TOF; HCCA): m/z 2050.87 [M+H]+, 4101.46
[M2+H]+; calculated for C92H57Br8MgN16: 2050.82.
Tetrakis{5,7-bis[2’-(4-methoxyphenyl)ethenyl]-6H-1,4-diazepino}[2,3-b,g,l,q]porphyrazinato
magnesium(II) (2b). Yield 0.39 g (94%). UV-vis (DMSO) λmax/nm (log ε): 386 (5.05), 661 (4.87), 698
(4.78). 1H NMR (500 MHz; pyridine-d5) δ/ppm: 8.49 (8H, d,
3J = 16.53 Hz, 2'-H), 8.13 (8H, d,
3J = 16.06 Hz,
1'-H), 7.69 (16H, d, 3J = 7.79 Hz, H
o-Ar), 6.89 (16H, d,
3J = 8.15 Hz, H
m-Ar), 6.67 (4H, br s, H
eq), 5.94 (4H, d,
2J = 12.64 Hz, H
ax), 3.81 (24H, s, -OMe).
13C NMR (125 MHz; Py-d5) δ/ppm: 161.12, 154.86, 143.05, 138.65,
130.15, 130.03, 128.95, 114.99, 55.62, 38.48. MS (MALDI-TOF/TOF; HCCA): m/z 1658.60 [M+H]+,
3317.07 [M2+H]+; calculated for C100H81MgN16O8: 1658.63.
Tetrakis(5,7-bis(4-tert-butylphenyl)-6H-1,4-diazepino)[2,3-b,g,l,q]porphyrazinato magnesium(II) (2c)
was synthesized according to a previously published procedure.1
S3
NMR Spectra
9 8 7 6 5 4 3 2 1 0Chemical Shift (ppm)
4.0
9
4.0
4
15
.98
7.9
68
.20
7.7
07
.66
7.6
57
.47
6.1
1
4.7
7
23.9
9
2'-H (d) 3J=15.9 Hz
1'-H; Ho-Ar
(br m) Hm-Ar (br s)
Hax (br s)Heq (br s)
H2O
*
Figure S1.
1H NMR spectrum of 2a (DMSO-d6, 293 K).
8 6 4 2F2 Chemical Shift (ppm)
2
3
4
5
6
7
8
F1
Ch
em
ica
l S
hift
(pp
m)
2'-H
1'-H;
Ho-Ar Hm-Ar
HaxHeq
H2O*
Figure S2.
1H-
1H COSY NMR spectrum of 2a (DMSO-d6, 293 K).
S4
170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 0 -10
Chemical Shift (ppm)
154
.99
149
.19
143
.05
137
.46
132
.50
131
.68
129
.82
37.7
5
***
Figure S3.
13C NMR spectrum of 2a (pyridine-d5, 293 K).
8 6 4 2 0F2 Chemical Shift (ppm)
0
20
40
60
80
100
120
140
160
F1
Ch
em
ica
l S
hift
(pp
m)
7.70-7.65; 129.82; 131.68
7.47; 132.50
8.20; 137.46
2'-H
1'-H;
Ho-Ar Hm-Ar
HaxHeq
H2O*
Figure S4.
1H-
13C HSQC spectrum of 2a (DMSO-d6, 293 K).
S5
8 6 4 2 0F2 Chemical Shift (ppm)
1
2
3
4
5
6
7
8
F1
Ch
em
ica
l S
hift
(pp
m)
2'-H
1'-H;
Ho-Ar Hm-Ar
HaxHeq
H2O*
Figure S5.
1H-
1H NOESY spectrum of 2a (DMSO-d6, 293 K).
16.15
8 7 6 5 4 3Chemical Shift (ppm)
24.113.944.0216.178.018.00
8.5
0
8.1
4
7.7
0
6.9
0
6.6
7
5.9
5
3.8
1
Ho-Ar (d) 3J=7.79 Hz
1'-H (d) 3J=16.06 Hz
Hm-Ar (d) 3J=8.15 Hz
2'-H (d) 3J=16.06 Hz
Hax (d) 2J=12.64 HzHeq (br s)
HOMe (s)
* * *H2O
Figure S6.
1H NMR spectrum of 2b (pyridine-d5, 293 K).
S6
8 7 6 5 4 3F2 Chemical Shift (ppm)
4
5
6
7
8
F1
Ch
em
ica
l S
hift
(pp
m)
2'-H
Ho-Ar
Hm-Ar
1'-H
HOMe
Hax
Heq
H2O
* * *
Figure S7.
1H-
1H COSY NMR spectrum of 2b (pyridine-d5, 293 K).
180 160 140 120 100 80 60 40 20 0Chemical Shift (ppm)
16
1.1
21
54
.86
14
3.0
51
38
.65
13
0.1
51
30
.03
12
8.9
51
14
.99
55
.62
38
.48
* * *
Figure S8.
13C NMR spectrum of 2b (pyridine-d5, 293 K).
S7
8 7 6 5 4F2 Chemical Shift (ppm)
0
20
40
60
80
100
120
140
160
F1
Ch
em
ica
l S
hift
(pp
m)
2'-H
Ho-ArHm-Ar
1'-H
HOMe
Hax
Heq
3.81; 55.62
5.95; 38.48
6.67; 38.48
7.70; 130.03 6.90; 114.99
8.50; 138.65
8.14; 128.95
H2O* * *
Figure S9.
1H-
13C HSQC spectrum of 2b (pyridine-d5, 293 K).
S8
8 7 6 5 4 3F2 Chemical Shift (ppm)
4
5
6
7
8
F1
Ch
em
ica
l S
hift
(pp
m)
2'-H
Ho-ArHm-Ar
1'-H
HOMe
Hax
Heq
H2O* * *
Figure S10.
1H-
1H NOESY spectrum of 2b (pyridine-d5, 293 K).
S9
X-ray Diffraction Analysis
The crystal of 2a (C94H62N16OSMgBr8, M = 2127.16) used for study was triclinic, space group P-1, at T = 100
K: a = 15.325(3) Å, b = 27.895(6) Å, c = 33.306(7) Å, = 113.35(3)°, = 100.91(3)°, = 95.58(3)°, V =
12599(6) Å3, Z = 4, dcalc = 1.121 g/cm
3, F(000) = 4216, μ = 0.973 mm
–1. The X-ray diffraction study was
carried out on the ‘Belok’ beamline ( = 0.96990 Å) of the National Research Center “Kurchatov Institute”
(Moscow, Russian Federation) using a Rayonix SX-165 CCD detector. A total of 720 images (117852
reflections, 40519 independent reflections, Rint = 0.0851) were collected using an oscillation range of 1.0° (
scan mode, 2θmax = 76.44°) and corrected for absorption using the Scala program (Tmin = 0.848; Tmax =
0.898).2 The data were indexed, integrated and scaled using the utility iMOSFLM in CCP4 program.
3 The
structure was determined by direct methods and refined by full-matrix least squares technique on F2 with
anisotropic displacement parameters for non-hydrogen atoms. Twelve of the sixteen para-bromophenyl
substituents were disordered over two sites each with equal occupancies. The independent part of the unit cell
of 2a contained several dimethylsulfoxide and water solvate molecules, which were strongly disordered. All
attempts to model and refine their positions were unsuccessful. Therefore, the contribution to the scattering by
the solvent molecules was removed by use of the utility SQUEEZE in PLATON06.4 The hydrogen atoms were
placed in calculated positions and refined within a riding model with fixed isotropic displacement parameters
[Uiso(H) = 1.5Ueq(C) for the methyl groups and 1.2Ueq(C) for the other groups]. The final divergence factors
were R1 = 0.1361 for 15689 independent reflections with I > 2(I) and wR2 = 0.2672 for all independent
reflections, S = 1.080. The calculations were performed using the SHELXTL program.5 Full crystallographic
data for the investigated compounds have been deposited with the Cambridge Crystallographic Data Center,
CCDC 1489687. Copies of this information may be obtained free of charge from the Director, CCDC, 12
Union Road, Cambridge CB2 1EZ, UK (fax: +44 1223 336033; e-mail: [email protected] or
www.ccdc.cam.ac.uk).
Figure S11. X-ray analysis data for 2a. Show packing of 2a in the crystal cell (hydrogen atoms are omitted
for clarity).
S10
Figure S12. Views of the X-ray structure of 2a. Ellipsoid (left) and space filling (right) representations,
respectively (hydrogen atoms and (aryl)ethenyl substituents are omitted for clarity).
S11
Studies of the Extent of Dissociation
0.0 2.0x10-6
4.0x10-6
6.0x10-6
8.0x10-6
1.0x10-5
0.0
0.2
0.4
0.6
0.8
1.0
CM
(tBuPh
Dz4PzMg)
Figure S13. The extent of dissociation () as function of concentration (mol L-1
) of 2c in DMSO (red line)
and in pyridine (black line).
0.0 2.0x10-6
4.0x10-6
6.0x10-6
8.0x10-6
1.0x10-5
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
CM
(MeStyr
Dz4PzMg)
Figure S14. The extent of dissociation () as function of concentration of 2b (mol L
-1) in DMSO (red line)
and in pyridine (black line).
S12
Studies of the Influence of Fluoride Ion Concentration on the Dimer-Monomer Equilibria
Complex 2c in DMSO
400 600 800
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
677
640
Figure S15. UV-vis spectroscopic changes seen upon addition of tetrabutylammonium fluoride to a solution
of 2c in DMSO.
0.0 2.0x10-4
4.0x10-4
6.0x10-4
0.18
0.20
0.22
0.24
A640
Abso
rban
ce (
a.u.)
CM
(F-)
Figure S16. Change in absorbance at 640 nm seen upon titration of 2c with tetrabutylammonium fluoride in
DMSO. Concentrations are in mol L-1
.
3.2 3.4 3.6 3.8 4.0 4.2
-1.0
-0.5
0.0
0.5
1.0
1.5
tg () = 4
R2 = 97
Lg
(I6
40
)
pCM
(F-)
Figure S17. Plot of the indicator concentration ratio for 2c at 640 nm vs. the negative log of the
tetrabutylammonium fluoride concentration.
S13
Complex 2c in pyridine
400 600 800
0.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
641
679
Figure S18. UV-vis spectroscopic changes seen upon addition of tetrabutylammonium fluoride to a solution
of 2c in pyridine.
0.0 2.0x10-5
4.0x10-5
6.0x10-5
0.2
0.4
0.6
0.8
1.0
1.2
A679
A641
Ab
sorb
ance
(a.
u.)
CM
(F-)
Figure S19. Change in absorbance at 679 and 641 nm seen upon titration of 2c with tetrabutylammonium
fluoride in pyridine. Concentrations are in mol L-1
.
4.2 4.4 4.6 4.8 5.0 5.2 5.4 5.6 5.8
-3
-2
-1
0
1
2 pCM
(F-) - Lg(I641); tg()=2.6; R2=93
pCM
(F-) - Lg(I679); tg()=2.9; R2=96
Lg(I)
pCM(F
-)
Figure S20. Plots of the indicator concentration ratio for 2с at 679 and 641 nm vs. the negative log of the
tetrabutylammonium fluoride concentration.
S14
400 600 8000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
642
680A
400 600 8000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
642
680B
Figure S21. UV-vis spectroscopic changes during dissociation of dimeric form of 2c in pyridine seen upon
addition of tetrabutylammonium fluoride (A) and the following reverse dimerization process upon addition of
FeBr3 (B).
0.0 2.0x10-5
4.0x10-5
6.0x10-5
8.0x10-5
1.0x10-4
0.2
0.4
0.6
0.8
1.0
1.2
CM
(F-) - A
680
CM
(F-) - A
642
CM
(Fe3+
) - A680
CM
(Fe3+
) - A642
Ab
sorb
ance
(a.
u.)
CM
(F-;Fe
3+)
Figure S22. Change in absorbance at 680 and 642 nm seen upon titration of 2c with tetrabutylammonium
fluoride in pyridine and upon titration of the resulting solution with FeBr3. Concentrations are in mol L-1
.
4.4 4.5 4.6 4.7 4.8 4.9 5.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5 pCM
(F-) - Lg(I
680); tg()=14; R
2
pCM
(F-) - Lg(I
642); tg()=14; R
2
pCM
(Fe3+
) - Lg(I680
); tg()=13; R2
pCM
(Fe3+
) - Lg(I642
); tg()=14; R2
Lg
(I
)
pCM
(F-; Fe
3+)
Figure S23. Plots of the indicator concentration ratio for 2c at 680 and 642 nm vs. the negative log of the
tetrabutylammonium fluoride or FeBr3 concentration.
S15
Complex 2b in DMSO
400 600 800 1000
0.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
1.0
1.1
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
660
702
Figure S24. UV-vis spectroscopic changes seen upon addition of tetrabutylammonium fluoride to a solution
of 2b in DMSO.
0.0 2.0x10-4
4.0x10-4
6.0x10-4
0.3
0.4
0.5
0.6
0.7
0.8
0.9 A702
A660
Abso
rban
ce (
nm
)
CM
(F-)
Figure S25. Change in absorbance at 702 and 660 nm seen upon titration of 2b with tetrabutylammonium
fluoride in DMSO. Concentrations are in mol L-1
.
3.80 3.85 3.90 3.95 4.00 4.05 4.10
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5
2.0 pC
M(F-) - Lg(I702); tg()=9; R
2=96
pCM(F-) - Lg(I660); tg()=8; R
2=96
Lg
(I)
pCM
(F-)
Figure S26. Plots of the indicator concentration ratio for 2b at 702 and 660 nm vs. the negative log of the
tetrabutylammonium fluoride concentration.
S16
300 400 500 600 700 800 9000.0
0.2
0.4
0.6
0.8
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
660
702
A
300 400 500 600 700 800 9000.0
0.2
0.4
0.6
0.8
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
660
702B
Figure S27. UV-vis spectroscopic changes during dissociation of dimeric form of 2b in DMSO seen upon
addition of tetrabutylammonium fluoride (A) and the following reverse dimerization process upon addition of
FeBr3 (B).
0.0 5.0x10-5
1.0x10-4
1.5x10-4
2.0x10-4
2.5x10-4
0.2
0.3
0.4
0.5
0.6
0.7
CM
(F-) - A
702
CM
(F-) - A
660
CM
(Fe3+
) - A702
CM
(Fe3+
) - A660
Ab
sorb
ance
(a.
u.)
CM
(F-;Fe
3+)
Figure S28. Change in absorbance at 702 and 660 nm seen upon titration of 2b with tetrabutylammonium
fluoride in DMSO and upon titration of the resulting solution with FeBr3. Concentrations are in mol L-1
.
3.8 4.0 4.2 4.4 4.6 4.8 5.0
-2
-1
0
1
2
pCM(F
-) - Lg(I
702); tg()=7; R
2
pCM(F
-) - Lg(I
660); tg()=6; R
2
pCM(Fe
3+) - Lg(I
702); tg()=4; R
2
pCM(Fe
3+) - Lg(I
660); tg()=4; R
2
Lg
(I
)
pCM(F
-; Fe
3+)
Figure S29. Plots of the indicator concentration ratio for 2b at 702 and 660 nm vs. the negative log of the
tetrabutylammonium fluoride or FeBr3 concentration.
S17
Complex 2b in pyridine
400 600 800
0.0
0.2
0.4
0.6
0.8
1.0
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
666
706
Figure S30. UV-vis spectroscopic changes seen upon addition of tetrabutylammonium fluoride to a solution
of 2b in pyridine.
0 1x10-5
2x10-5
3x10-5
4x10-5
5x10-5
6x10-5
7x10-5
0.3
0.4
0.5
0.6
0.7
0.8
A706
A666
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
Figure S31. Change in absorbance at 706 and 666 nm seen upon titration of 2b with tetrabutylammonium
fluoride in pyridine. Concentrations are in mol L-1
.
4.2 4.4 4.6 4.8 5.0 5.2 5.4 5.6 5.8 6.0 6.2
-2.0
-1.5
-1.0
-0.5
0.0
0.5
1.0
1.5 pCM
(F-) - Lg(I
706); tg() = 2.5; R
2 = 99.7
pCM
(F-) - Lg(I
666); tg() = 2; R
2 = 98
Lg
(I)
pCM
(F-)
Figure S32. Plots of the indicator concentration ratio for 2b at 706 and 666 nm vs. the negative log of the
tetrabutylammonium fluoride concentration.
S18
400 600 8000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
Absorb
ance (
a.u
.)
Wavelength (nm)
666
706
A
400 600 8000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
Ab
sorb
ance
(a.
u.)
Wavelength (nm)
666
706
B
Figure S33. UV-vis spectroscopic changes during dissociation of dimeric form of 2b in pyridine seen upon
addition of tetrabutylammonium fluoride (A) and the following reverse dimerization process upon addition of
FeBr3 (B).
0.0 4.0x10-5
8.0x10-5
1.2x10-4
1.6x10-4
0.4
0.5
0.6
0.7
0.8
0.9
1.0
CM
(F-) - A
706
CM
(F-) - A
666
CM
(Fe3+
) - A706
CM
(Fe3+
) - A666
Ab
sorb
ance
(a.
u.)
CM
(F-;Fe
3+)
Figure S34. Change in absorbance at 706 and 666 nm seen upon titration of 2b with tetrabutylammonium
fluoride in pyridine and upon titration of the resulting solution with FeBr3. Concentrations are in mol L-1
.
4.2 4.4 4.6 4.8 5.0 5.2 5.4 5.6 5.8
-2
-1
0
1
2
pCM
(F-) - Lg(I
706); tg()=7; R
2
pCM
(F-) - Lg(I
666); tg()=6; R
2
pCM
(Fe3+
) - Lg(I706
); tg()=9; R2
pCM
(Fe3+
) - Lg(I666
); tg()=8; R2
Lg
(I
)
pCM
(F-; Fe
3+)
Figure S35. Plots of the indicator concentration ratio for 2b at 706 and 666 nm vs. the negative log of the
tetrabutylammonium fluoride or FeBr3 concentration.
S19
Electrochemistry
Electrochemical analyses of 2a and 2b were carried out in pyridine containing 0.1 M [TBA][BF4] as the
supporting electrolyte. Under these conditions the complexes exist in their dimeric forms as illustrated in
Figure S36. One broad irreversible oxidation peak was observed at a potential of 0.804 and 0.777 V (vs. SCE)
for 2a and 2b, respectively. Reductive scans revealed more complex electrochemistry; up to five reversible
redox processes were observed (Table S1, Figure S37). Such behavior is consistent with the proposed dimeric
nature of the complexes, which can lead to a splitting of redox transitions similar to what is seen in the case of
double-decker sandwich complexes stabilized by a central lanthanide cation.6-8
The single broad oxidation
peak could result from two closely located irreversible redox transitions. Complexes 2a and 2b appear to be
noticeably more stable towards oxidation than monomeric phthalocyanine complexes9 and sandwich-type
double-decker systems.7, 8
The ΔR21 (R2 − R1) and ΔR43 (R4 – R3) values are larger for 2a than for 2b, which is
as expected given the greater Q-band splitting seen in the UV-vis spectrum (cf. Figures 2 and S36). The
reduction potentials R1, R2, and R3 for 2b were slightly shifted to more negative values relative to 2a,
meaning that the reduction of complex 2b is more difficult. Such a finding is as expected given the stronger
electron-donating effect of the substituents present in 2b.
300 400 500 600 700 800
0,5
1,0
1,5
2,0
2,5
3,0
704
700667
Absorb
ance
Wavelength (nm)
2a
2b
662
385
Figure S36. UV-vis spectra recorded for samples of 2a and 2b in pyridine in the presence of supporting
electrolyte. The concentrations of 2a and 2b were both ca. 0.1 mM; the cuvette path length was 1 mm.
-2,0 -1,5 -1,0 -0,5 0,0
-15
-10
-5
0
5
10
15
Curr
ent
/ A
Potential / V
2a
0,0 0,5 1,0 1,5 2,0 2,5
-15
-10
-5
0
5
10
Curr
ent
/ A
Potential / V
2a
S20
-2,0 -1,5 -1,0 -0,5 0,0
-10
-5
0
5
10
Curr
ent
/ A
Potential / V
2b
0,0 0,5 1,0 1,5 2,0 2,5
-10
-5
0
5
10
Curr
ent
/ A
Potential / V
2b
Figure S37. SWVA of complexes 2a and 2b in pyridine containing 0.1 M [TBA][BF4]. Amplitude, 50 mV;
frequency, 10 Hz; step potential, 5 mV; E1/2(ferrocene+/ ferrocene) = 0.49 V under these experimental
conditions.
Table S1. Reduction potentials for 2a and 2b in pyridine (values vs. SCEa)
Ox1b Red1 Red2 Red3 Red4 Red5
2a 1.294 -0.790 -1.016 -1.356 -1.646 -
2b 1.267 -0.883 -1.073 -1.433 -1.593 -1.793
a E1/2 (Fc
+/Fc) = 0.49 V.
b Irreversible process; the value of the peak potential is given.
S21
In Vitro and in Vivo Toxicity Tests
Compounds 2a,b were converted into water-soluble forms by co-solvation with polyvinylpyrrolidone (PVP)
for biological testing.
Cell viability was recorded as dehydrogenase activity as inferred from 3-(4,5-dimethylthiazol-2-yl)-2,5-
diphenyltetrazolium bromide (MTT) assays.10
Briefly, the SH-SY5Y cells or primary culture of rat cerebellar
granule cells were incubated with the test compounds or equivalent volume of vehicle (less than 1% of the
whole volume of medium under the layer of cells) for 24 h. Then, 20 μL of MTT (2 mg mol L–1
in PBS) were
added to each well and the cells were incubated at 37°C for 2 h. The supernatants were aspirated carefully,
200 μL of DMSO were added to each well to dissolve the precipitate, and the absorbance was measured at
570 nm using a microplate reader Victor (Perkin Elmer).
Acute intraperitoneal toxicity of complexes 2a and 2b was determined using male hybrid mice BDF1
(weighing 20−22 g) by injection of single doses of 25, 50, 100, and 150 mg kg–1
body weight, respectively.
Mice were kept under specific pathogen-free conditions; water and food were provided ad libitum. All
animals were observed for clinical signs of toxicity within the first 30 min following dose administration, and
then – with an interval of 1–4 h and further – once daily for 14 days. No deaths were registered during the 14
day study periods associated with either complex. The data obtained were plotted as a dose–effect curve, from
which the acute toxicity values (MTD, LD50 and LD100) of complexes 2a and 2b were determined.
Table S2. Acute toxicity studies of compounds 2a and 2b as determined using mal hybrid mice BDF1.
Compound Injected dose, mg
kg–1
Number of animals
per group
Number of deaths at
day 14 after injection
PVP
100 6 0
250 6 0
500 6 0
750 6 0
1500 6 0
3750 6 0
7500 6 0
2a
10 6 0
50 6 0
100 6 0
150 6 0
2b
10 6 0
50 6 0
100 6 0
150 6 0
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S22
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