Investigation of the electronic, photosubstitution, redox, and surface properties of new ruthenium (II)-containing amphiphiles

Article abstract of DOI:10.1021/ic1015934

A series of pyridine-and phenol-based ruthenium(II)-containing amphiphiles with bidentate ligands of the following types are reported: [(Lpy1)RuII(bpy) _2](PF₆ (1), [(py1)RuII(bpy)_2](PF₆ )(3), and [(LPhCII)RuII(bpy)₂](PF₆)(4). Species 1 and 2 are obtained by treatment of [Ru(bpy)₂Cl₂] with the ligands L Pyl (N-(pyridine-2-ylmethylene)octadecan-1-amine) and LPyA (N-(pyridine-2-ylmethyl)octadecan-1-amine). The imine species 3 and 4 are synthesized by reaction of [Ru(bpy)₂(CF₃SO ₃)₂] with the amine ligands HLPhBuA (2,4-di-ferf-butyl-6- ((octadecylamino)methyl)phenol), and HL A (2,4-dichloro-6-((octadecylamino) methyl)phenol). Compounds 1-4 are characterized by means of electrospray ionization (ESI+) mass spectrometry, elemental analyses, as well as electrochemical methods, infrared and UV-visible absorption and emission spectroscopies. The cyclic voltammograms (CVs) of 1-2 are marked by two successive processes around-1.78 and-2.27 V versus Fc+/ Fc attributed to bipyridine reduction. A further ligand-centered reductive process is seen for 1. The RuII/RuII couple appears at 0.93 V versus Fc+/Fc. The phenolato-containing 3 and 4 species present relatively lower reduction potentials and more reversible redox behavior, along with RuII/III and phenolate/phenoxyl oxidations. The interpretation of observed redox behavior is supported by density functional theory (DFT) calculations. Complexes 1-4 are surface-active as characterized by compression isotherms and Brewster angle microscopy. Species 1 and 2 show collapse pressures of about 29-32 mN · m-1, and are strong candidates for the formation of redox-responsive monolayer films.

Full text of DOI:10.1021/ic1015934

Inorg. Chem. 2011, 50, 969–977 969
DOI: 10.1021/ic1015934
Investigation of the Electronic, Photosubstitution, Redox, and Surface Properties
of New Ruthenium(II)-Containing Amphiphiles
Frank D. Lesh, Marco M. Allard, Rama Shanmugam, Lew M. Hryhorczuk, John F. Endicott, H. Bernhard Schlegel,
ꢀ
and Claudio N. Verani*
Department of Chemistry, Wayne State University, 5101 Cass Avenue, Detroit, Michigan 48202, United States
Received August 6, 2010
A series of pyridine- and phenol-based ruthenium(II)-containing amphiphiles with bidentate ligands of the following
types are reported: [(LPyI)RuII(bpy)2](PF6)2 (1), [(LPyA)RuII(bpy)2](PF6)2 (2), [(LPhBuI)RuII(bpy)2](PF6) (3), and
[(LPhClI)RuII(bpy)2](PF6) (4). Species 1 and 2 are obtained by treatment of [Ru(bpy)2Cl2] with the ligands LPyI
(N-(pyridine-2-ylmethylene)octadecan-1-amine) and LPyA (N-(pyridine-2-ylmethyl)octadecan-1-amine). The imine
species 3 and 4 are synthesized by reaction of [Ru(bpy)2(CF3SO3)2] with the amine ligands HLPhBuA (2,4-di-tert-butyl-
6-((octadecylamino)methyl)phenol), and HLPhClA (2,4-dichloro-6-((octadecylamino)methyl)phenol). Compounds
1-4 are characterized by means of electrospray ionization (ESIþ) mass spectrometry, elemental analyses, as well
as electrochemical methods, infrared and UV-visible absorption and emission spectroscopies. The cyclic
voltammograms (CVs) of 1-2 are marked by two successive processes around -1.78 and -2.27 V versus Fcþ/
Fc attributed to bipyridine reduction. A further ligand-centered reductive process is seen for 1. The RuII/RuIII couple
appears at 0.93 V versus Fcþ/Fc. The phenolato-containing 3and 4species present relatively lower reduction potentials and
more reversible redox behavior, along with RuII/III and phenolate/phenoxyl oxidations. The interpretation of observed
redox behavior is supported by density functional theory (DFT) calculations. Complexes 1-4 are surface-active as
characterized by compression isotherms and Brewster angle microscopy. Species 1 and 2 show collapse pressures of
about 29-32 mN m-1, and are strong candidates for the formation of redox-responsive monolayer films.
3
Introduction
photosensitizing properties and consequent relevance toward
water oxidation.
Metallosurfactants comprise a new class of coordination
compounds that combine metal properties such as geometric
control, redox, optical, and magnetic behavior1,2 with amphi-
philicity.3 These materials are increasingly relevant for high-end
applications involving optoelectronics,4 logic and memory
operations,5,6 and micellar luminescence and electron
transfer.7,8 Therefore, the integration of amphiphilic properties
to antennae constituents is a relevant step toward the develop-
ment of metallosurfactant precursors for photoresponsive
modular films for artificial photosynthesis. In this regard,
ruthenium bipyridyl complexes such as the [RuII(bpy)2]2þ have
received considerable attention because of their superior
In recent years, our group has spearheaded a com-
prehensive effort toward redox active precursors for
Langmuir-Blodgett films. We have established a wide
range of differentiated scaffold designs,9,10 studied redox
and collapse mechanisms,11 and demonstrated how coordi-
nation and protonation preferences dictate amphiphilic
behavior.12
We have envisioned the integration of the photore-
sponsive [RuII(bpy)2]2þ to bidentate amphiphilic ligands
containing aminomethyl-pyridine and -phenol head-
groups, and in this article, we evaluate a new family
of asymmetric [LRu(bpy)2]þ/2þ metalloamphiphiles, namely,
[(LPyI)RuII(bpy)2](PF6)2 (1), [(LPyA)RuII(bpy)2](PF6)2
(2), [(LPhBuI)RuII(bpy)2](PF6) (3), and [(LPhClI)RuII(bpy)2]-
(PF6) (4) (Scheme 1), where Py = pyridine and
*To whom correspondence should be addressed. Phone: 313 577 1076.
Fax: 313 577 8022. E-mail: cnverani@chem.wayne.edu.
(1) Bodenthin, Y.; Pietsch, U.; Mohwald, H.; Kurth, D. G. J. Am. Chem.
Soc. 2005, 127, 3110–3114.
(2) Talham, D. R. Chem. Rev. 2004, 104, 5479–5502.
(3) Hoogenboom, R.; Fournier, D.; Schubert, U. S. Chem. Commun.
2008, 155–162.
(4) Zhang, J.; Chu, B. W. K.; Zhu, N.; Yam, V. W. W. Organometallics
2007, 26, 5423–5429.
(5) Low, P. J. Dalton Trans. 2005, 2821–2824.
(6) Wassel, R. A.; Gorman, C. B. Angew. Chem. 2004, 43, 5120–5123.
(7) Guerrero-Martinez, A.; Vida, Y.; Dominguez-Gutierrez, D.;
Albuquerque, R. Q.; De Cola, L. Inorg. Chem. 2008, 47, 9131–9133.
(8) Wang, K.; Haga, M.; Monjushiro, H.; Akiba, M.; Sasaki, Y. Inorg.
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da Rocha, S. R.; Yee, G. T.; Hratchian, H. P.; Verani, C. N. Chem.;Eur.
J. 2007, 13, 9948–9956.
(10) Shakya, R.; Keyes, P. H.; Heeg, M. J.; Moussawel, A.; Heiney, P. A.;
Verani, C. N. Inorg. Chem. 2006, 45, 7587–7589.
(11) Shakya, R.; Hindo, S. S.; Wu, L.; Allard, M. M.; Heeg, M. J.;
Hratchian, H. P.; McGarvey, B. R.; da Rocha, S. R.; Verani, C. N. Inorg.
Chem. 2007, 46, 9808–9818.
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B.; Hryhorczuk, L.; Verani, C. N. Eur. J. Inorg. Chem. 2009, 345–356.
r
2011 American Chemical Society
Published on Web 01/07/2011
pubs.acs.org/IC

970 Inorganic Chemistry, Vol. 50, No. 3, 2011
Lesh et al.
Scheme 1. Series of Pyridine- and Phenolate-Based Ruthenium(II)-
Containing Amphiphiles 1-4
dication and bears resemblance to some of the work by
Yam et al.4,17,18 and Keyes et al.19,20 We aim at extending
efforts toward the relatively more inert bivalent Ru2þ ion,
targeting the electrochemical redox behavior of species
1-4, while preserving their amphiphilic and photore-
sponsive character. Along with the ligands LPyI and LPyA
present in 1 and 2, we recognized phenolato-based com-
plexes as less prevalent. This prompted us to merge
well-established amphiphilic ligands such as HLPhBuA
and HLPhClA with [Ru(bpy)2]2þ to yield the imines 3
and 4 with extended spectroscopic and electrochemical
features.19
Ligands. Condensation of 1-octadecylamine with 2-
pyridinecarboxyaldehyde in methanol gave the imine
surfactant ligand precursor LPyI which was subsequently
reduced in the presence of sodium borohydride to yield
the amine ligand precursor L .
PyA 15 The phenol-containing
surfactant ligands HLPhBuA and HLPhClA were generated
from 1-octadecylamine in reaction with 3,5-di-tert-butyl-
2-hydroxybenzaldehyde or 3,5-dichloro-2-hydroxyben-
zaldehyde, respectively, followed by reduction to generate
the amine precursors.16 These ligands were characterized
by means of H NMR and infrared (IR) spectroscopies
and electrospray ionization (ESI-MS) mass spectrometry
with generally 80-85% overall yields.
Ph = phenolate, I = imine and A = amine, and Bu or Cl
indicates the ortho- and para-substituted tert-butyl or
chloro groups in the phenolate complexes. We interro-
gate the electrochemical properties of these systems to
evaluate the nature of the redox processes, the optical
and electronic properties to evaluate the photostability
and excitability (emission) of these species, and the
amphiphilic properties to evaluate the potential for
formation of ordered LB films. In particular, we evalu-
ate (a) how the presence of C18 alkyl groups allow for
formation of high-quality Langmuir films at the air/
water interface, (b) the difference in related species
(imino versus amino) for LPy and (tert-butyl versus
chloro) for LPh, and (c) whether density functional
theory (DFT) calculations can model and account for
the observed redox responses. These concerns are ad-
dressed using a host of synthetic, spectrometric, spectros-
copic, and computational- and surface-dedicated methods,
and we attempt to correlate these properties to assess the
viability of these species as precursors for photoresponsive
LB films.
1
Complexes. The Ru(II) pyridine complexes 1-2 were
obtained by adapting general synthetic approaches for
analogous compounds by treatment of equimolar ratios
of cis-[Ru(bpy)2Cl2] 2H2O with the ligands LPyI and
3
L
PyA inabsoluteethanol.4,17 The Ru(II) phenol-containing
metallosurfactantsz 3-4 were achieved upon complexa-
tion of the ligands HLPhBuA and HLPhClA with Ru(bpy)2-
(CF3SO3)2 in isopropanol or acetone, respectively, using
triethylamine as a base for phenol deprotonation. Because
previous attempts using cis-[Ru(bpy)2Cl2] 2H2O led to
3
undesirable side products, Ru(bpy)2(CF3SO3)2 was chosen
for complexation with the phenolate-containing ligands.
This route took advantage of the excellent leaving group
properties of the triflate ion. It should be pointed out that
compounds 3 and 4 encompass imine ligands formed from
in situ oxidation of the parent amine ligands. Such conver-
sion has been reported in similar systems.21
All complexes were precipitated with ammonium hexa-
fluorophosphate and purified by column chromato-
graphy to yield microcrystalline powders which were
characterized by IR, elemental analyses, ESIþ mass spec-
trometry, and electrochemical methods. Elemental ana-
lyses for 1-4 were in excellent agreement with theoretical
percentages. The ESIþ mass analyses of 1 and 2 in
methanol indicate the presence of signature peak clusters
with general formulas [(LPyX)RuII(bpy)2]2þ and [(LPyX)-
RuII(bpy)2PF6]þ. The phenolate species 3 and 4, being
composed of a charged ligand, showed single mass pat-
terns corresponding to the monovalent [(LPhBuI)RuII-
(bpy)2]þ ion species. A differential isotopic distribution
was observed for 4 due to the contributing chloride
isotopes. The pertinent m/z peak clusters are shown in
Results and Discussion
Syntheses and Characterizations. Design Rationale.
The rationale behind our design strategy involves the
combination of distinct donor sets built into photore-
sponsive [RuII(bpy)2]2þ moieties by means of bidentate
chelating ligands containing hydrophobic alkyl tails. This
design is based on our previously described pyridyl-13-15
and phenol-based16 ligands coordinated to the Cu(II)
(13) Driscoll, J. A.; Allard, M. M.; Wu, L. B.; Heeg, M. J.; da Rocha,
S. R. P.; Verani, C. N. Chem.;Eur. J. 2008, 14, 9665–9674.
(14) Driscoll, J. A.; Keyes, P. H.; Heeg, M. J.; Heiney, P. A.; Verani, C. N.
Inorg. Chem. 2008, 47, 7225–7232.
(15) Jayathilake, H. D.; Driscoll, J. A.; Bordenyuk, A. N.; Wu, L. B.;
da Rocha, S. R. P.; Verani, C. N.; Benderskii, A. V. Langmuir 2009, 25, 6880–
6886.
(16) Hindo, S. S.; Shakya, R.; Rannulu, N. S.; Allard, M. M.; Heeg, M. J.;
Rodgers, M. T.; da Rocha, S. R.; Verani, C. N. Inorg. Chem. 2008, 47, 3119–
3127.
(17) Chu, B. W.; Yam, V. W. W. Inorg. Chem. 2001, 40, 3324–3329.
(18) Yam, V. W. W.; Lee, V. W. M. J. Chem. Soc., Dalton Trans. 1997,
3005–3010.
(19) Keyes, T. E.; Leane, D.; Forster, R. J.; Coates, C. G.; McGarvey,
J. J.; Nieuwenhuyzen, M. N.; Figgemeier, E.; Vos, J. G. Inorg. Chem. 2002,
41, 5721–5732.
(20) Leane, D.; Keyes, T. E. Inorg. Chim. Acta 2006, 359, 1627–1636.
(21) Lanznaster, M.; Heeg, M. J.; Yee, G. T.; McGarvey, B. R.; Verani,
C. N. Inorg. Chem. 2007, 46, 72–78.

Article
Inorganic Chemistry, Vol. 50, No. 3, 2011 971
Table 1. Photophysical Parameters for Complexes 1-4
complex
absorption λabs (nm)/ε (L mol-1 cm-1 a
)
emission λem/nm; cm-1 b,c
lifetime τo (ns)c
1
239 (17,330); 243 (17,530); 255 (16,030); 287 (44,120); 345 sh (4,460);
432 sh (8,940); 462 (11,080)
715; 13,986
77
2
3
4
245 (18,120); 291 (43,850); 342 (7,450); 424 sh (4,540); 472 (7,070)
248 (50,260); 294 (59,200); 377 (13,870); 476 sh (7,950); 521 (8,550)
247 (37,910); 295 (60,860); 363 (10,570); 519 (8,380)
641; 15,601
193
a Spectra measured in 1.0 ꢀ 10-5 M acetonitrile solution. b Emission maxima are corrected values. c Excitation wavelength at 460 nm for 1 and 470 nm
for 2.
Figure 1. UV-visible spectra of pyridyl complexes 1 and 2 (top) and
phenolate complexes 3 and 4 (bottom) in acetonitrile, 1.0 ꢀ 10-5 M.
Figure 2. Emission spectra of pyridyl complexes 1 and 2.
and 2 exhibit an ill-defined shoulder at 425 nm, absent in
the pyridyl-imine 1, where this corresponding shoulder is
slightly shifted to 432 nm. On the basis of other related
compounds,4,17,18,22 we tentatively ascribe this band to a
composite of allowed intraligand π f π* and dπ(RuII) f
π*(bpy) metal-to-ligand charge transfer transitions. The
second feature of importance in the visible region is a
broad band transition at 462 nm for 1. This transition
band is attributed to the dπ(RuII) f π*(iminomethylpyri-
dine) metal-to-ligand charge transfer transition,4,17,18,22
which in the pyridyl-amine 2 is red-shifted to 472 nm
with distinctly lower absorptivity. The overall smaller
ligand-field strengths of the σ-donating phenolato
ligands present comparatively red-shifted, markedly broad
low-energy metal-to-ligand charge-transfer (MLCT) or in-
traligand CT bands for complexes 3and 4, relativeto1and 2
containing the π-acceptor pyridyl ligands. These charge
transfer transitions are observed at 519-521 nm (ε =
8380-8550 L mol-1 cm-1) for both 3 and 4, thus consistent
with the behavior observed for other RuN5O chromophores
in similar ligand-donor environments.23,24
Emission Spectroscopy. Room temperature (RT) excita-
tion of 1 and 2 in acetonitrile at λ > 460 nm induces emission
at 715 and 641 nm, respectively (Figure 2). The pseudo-
Stokes shift for 1 (ca. 7700 cm-1) is about 2100 cm-1 larger
than that observed for 2 (ca. 5600 cm-1). Species 2 showed a
room-temperature lifetime 2.5 times longer than that of 1.
These observations lead to the inference that the lowest
energy triplet MLCT states originate from different chromo-
phores, as will be supported by the electrochemical data and
the Supporting Information, Figures S1-S4 and were
simulated in good agreement with their patterns, posi-
tions, and isotopic distributions.
Complex formation was further observed by the pres-
ence of vibrational modes attributed to the ligand,
particularly the characteristic strong C-H stretching
contribution of the alkyl chain appearing at 2851-2924
cm-1, and the strong stretch at 840-846 cm-1 (νP-F) due
to the totally symmetric vibration frequency of hexafluoro-
phosphate counterion.
Electronic Absorption Spectroscopy. Electronic absorp-
tion spectral data for complexes 1-4 were measured
in 10-3 to 10-5 M acetonitrile solutions. Table 1 lists
relevant absorption maxima and molar extinction coeffi-
cients, and spectra are displayed in Figure 1. Intense
intraligand σ f π* and π f π* processes dominate the
ultraviolet region of the spectrum for 1-4 with two
maxima centered about 245 and 290 nm. Appreciably
larger absorptivities have been observed for the phenolato-
based 3 and 4. Additionally, a third less intense
intraligand absorption band is positioned near 342 nm
for the pyridyl-based ligand compounds. A shoulder is
seen for 1; the equivalent band for compounds 3 and 4
is red-shifted to the vicinity of 370 nm. Previously
Meyer et al.22 have isolated and investigated the
related [Ru(bipy)2(AMPy)](ClO4)2, where (AMPy) is 2-
(aminomethyl)-pyridine, analogous to 1-2. A matching
absorption profile can be drawn between that species and
2, allowing to infer that the alkyl chain plays a negligible
electronic role to the overall spectroscopic properties of
these species. Both the complex [Ru(bipy)2(AMPy)](ClO4)2
(23) Chakraborty, S.; Walawalkar, M. G.; Lahiri, G. K. J. Chem. Soc.,
Dalton Trans. 2000, 2875–2883.
(24) Holligan, B. M.; Jeffery, J. C.; Norgett, M. K.; Schatz, E.; Ward,
M. D. J. Chem. Soc., Dalton Trans. 1992, 3345–3351.
(22) Brown, G. M.; Weaver, T. R.; Keene, F. R.; Meyer, T. J.; Kenan,
W. R., Jr. Inorg. Chem. 1976, 15, 190–196.

972 Inorganic Chemistry, Vol. 50, No. 3, 2011
Lesh et al.
Figure 4. CVs of 1-4 in acetonitrile, TBAPF6, versus Fcþ/Fc.
been proposed by Matsuo et al.25 using online electro-
spray MS, and seems to involve formation of monoden-
tate intermediates of 2 before the ligand LPyA is fully
exchanged by coordinating acetonitrile molecules.
When the non-coordinating dichloromethane was
used, no significant changes in the UV-visible and ESIþ
features of 2 were observed (Supporting Information,
Figure S6). Furthermore, both 1 and 3 revealed excellent
photostability in acetonitrile and dichloromethane. The
stability of 3 is tentatively associated to the strong
σ-donor nature of the phenolate moiety.20
Figure 3. UV-visible spectra recorded for photodissociation of 2 in
MeCN.
density functional theory (DFT) calculations. Further studies
are necessary for a definitive assignment. The phenolate-
based 3 and 4 seem non-emissive in the UV-visible range
accessible to the detector at room-temperature in acetonitrile.
The [Ru(bpy)2(AMPy)](PF6)2 compound was prepared ac-
cording to the protocol published by Meyer.22 This species is
analogous to the above-mentioned pyridyl-amine complex 2
but lacks the octadecyl chain. The response for both com-
pounds is identical in position and intensity.
Photolability Studies. Owing to the commonly ob-
served photoactive nature of ruthenium-containing com-
plexes, we examined the relative photolability of 1-3.
Samples were prepared in dry acetonitrile or dichloro-
methane to distinguish between the effects of coordinat-
ing versus non-coordinating solvents on the apparent
photolability of theruthenium complex. Clear photochem-
ical conversion was observed in complex 2 by the disap-
pearance of peaks at 342 and 472 nm, along with the
appearance of a new peak at 427 nm. The observations
indicate that 2 was converted into the [(MeCN)2-
RuII(bpy)2]2þ species in acetonitrile (Figure 3).
Electrochemistry. The cyclic voltammograms (CVs) of
1-4 demonstrate two successive cathodic waves, ranging
between E1/2=-1.78 and -2.27 V, for the one-electron
processes attributed to the classical bipyridine reduction
couples (Figure 4). Complex 1 reveals a third ligand-
centered reductive process at E1/2 = -2.22 V versus Fcþ/
Fc. The process observed at E1/2 = -1.63 V versus Fcþ/
Fc is tentatively ascribed to the reduction of the LPyI
imine-based ligand, which appears at the least negative
potential of all complexes. A single quasi-reversible one-
electron metal-centered RuII/RuIII couple appears at
E1/2 = 0.93 V (ΔEp = 0.08 V; |Ipc/Ipa | = 1.31) versus
Fcþ/Fc. The pyridyl-amine based complex 2 displays an
irreversible metal-centered oxidative process credited
to the RuII/RuIII couple, as an anodic wave observed at
E1/2 = 0.68 V versus Fcþ/Fc, where ΔEp = 0.12 V.
Additionally, this complex shows a ligand-based process
due to the oxidation of the ligand from aminomethylpyr-
idine to its imine counterpart. This oxidative dehydro-
genation mechanism was investigated by Keene et al.22,26,27
The conversion of an amine into an imine is catalyzed by the
coordination to the ruthenium ion, and its reversibility
seems highly dependent on the scan rate.
Complexes 3 and 4 present more negative potentials
for the reductive bipyridine couples, in contrast to the
pyridyl-based complexes 1 and 2. The averaged reduction
potentials are E1/2 = -1.94 and -2.25 V versus Fcþ/Fc,
and are comparable in reversibility to those containing
aminomethylpyridine ligands. The metal-based RuII/III
oxidation couple and the phenolate/phenoxyl radical
ligand oxidative processes are associated with the anodic
waves observed for complexes 3 and 4. These waves have
not been assigned conclusively and heavy orbital-interaction
between redox centers is most likely a major complicating
ESIþ mass spectrometry supports these results with the
appearance of a new peak at m/z = 248.2 associated with
the dicationic species [(MeCN)2RuII(bpy)2]2þ. Peaks of
interest for 2 and [(MeCN)2RuII(bpy)2]2þ were moni-
tored at different cone voltages (5, 20, and 40 V) and
times (0, 3, 20, 40 min). At low cone voltages (5 V), the
peak at m/z = 248.2 increased over time to 100%
intensity. Other relevant peaks appeared after 20 min
irradiation at m/z = 641.2 for [(MeCN)2RuII(bpy)2 þ
PF6]þ and m/z=361.6 for [LPyA þ Hþ], concomitant to
a decreased intensity for m/z = 919.7 associated with [2 -
PF6]þ and m/z = 387 from [2 - (PF6)2]2þ. The [2 -
(PF6)]þ ion disappears after 40 min of photoirradiation.
The observed isotopic fingerprint clusters were in good
agreement with the nature and charge of the ions present.
The mass spectroscopic results from the photosubstitu-
tion experiments for 1-2 in acetonitrile were plotted as
percentage intensity counts versus time (minutes). For 2,
the decrease in percentage abundance of the [(LPyA)-
RuII(bpy)2 þ (PF6)]þ species at a cone voltage of 5 V
followed concurrent increase in formation for the [(MeCN)2-
RuII(bpy)2]2þ photoproduct (Supporting Information,
Figure S5). A viable photodissociative mechanism has
(25) Arakawa, R.; Tachiyashiki, S.; Matsuo, T. Anal. Chem. 1995, 67,
4133–4138.
(26) Keene, F. R.; Ridd, M. J.; Snow, M. R. J. Am. Chem. Soc. 1983, 105,
7075–7081.
(27) Ridd, M. J.; Keene, F. R. J. Am. Chem. Soc. 1981, 103, 5733–5740.

Article
Inorganic Chemistry, Vol. 50, No. 3, 2011 973
Table 2. Cyclic Voltammetry Data for 1-4a
E1/2 (ΔEp) [V], |Ipc/Ipa
|
complex
reductionsb
oxidationsc
0.93 (0.08), |1.31|
0.68 (0.12); 0.93 (0.08)
1
2
3
4
-1.63 (0.09), |1.57|; -1.94 (0.09), |1.56|; -2.22 (0.1)
-1.78 (0.06), |0.66|; -2.03 (0.06), |0.91|
-1.95 (0.09), |1.34|; -2.27 (0.08), |2.02|
-1.93 (0.09), |1.65|; -2.23 (0.09), |1.51|
-0.01 (0.08); 0.28 (0.10); 0.71 (0.18), |1.44|
∼ 0.18 (0.20); 0.25ox
a CVs of 1-4 at 1.0 ꢀ 10 -3 mol L-1 in MeCN with 0.1 M TBAPF6 supporting electrolyte using 150 mV s-1 scan rate at RT in an inert atmosphere.
b Potentials listed as the cathodic peak potential Epc versus Fcþ/Fc. c Potentials listed as the anodic peak potential Epa versus Fcþ/Fc. ox = oxidation only
factor for these oxidative type processes. The chloro-
substituted complex 4 displays narrowly overlapping
oxidative processes. This indicates some destabilization
effects on the phenolate-to-phenoxyl oxidation when
compared to the tert-butyl-substituted complex 3. Table 2
summarizes the results with potentials reported versus the
Fcþ/Fc couple. The correlation of the observed spectros-
copic and electrochemical data to the frontier orbitals was
explored by means of DFT calculations to understand the
origin of these processes.
Electronic Structure Calculations. Representative mod-
els 10, 20, 30, and 40 composed of shortened propyl chains
were designed to offer insight into the electronic and
structural properties of 1-4 (Supporting Information,
Figure S7). The models are in good agreement with cor-
responding structural data of pyridyl- and phenol-based
[RuII(bpy)2] complexes previously reported.24,26,28-30 Similar
Figure 5. Relative molecular orbital energies.
approaches in our group9,11,12,14,16,31 have been instruc-
tive to provide information of the binding modes of
metal-containing amphiphilic compounds.
contrast, the LUMO and LUMOþ1 for 20 are ascribed
to the conventional antisymmetric and symmetric combi-
Nature of the HOMOs and LUMOs. Frontier orbitals
nations of the bipyridine orbitals. The model complexes
for 10-40 were calculated for correlation to and probing of
the origin of the observed electrochemical (redox) and
spectroscopic (optical) properties.28 Relative Molecular
Orbital (MO) energies are displayed in Figure 5, Support-
ing Information, Table S1 and Figure S8.
containing phenolato-based ligands (30 and 40) behave in a
generally comparable manner to one another. However,
these complexes consist of different occupied orbital
compositions relative to 10 and 20. The HOMO for 30 is
63% localized on the phenolate-imine based ligand and
31% contribution is coming from a ruthenium-based
orbital. The result is a largely mixed metal-ligand orbit-
al. Moreover, the HOMO-1 and HOMO-2 are chiefly
Rudπ-based orbitals with 76% and 69% contributions,
respectively, possessing unsuited spatial orientation for
overlap with the phenolate pπ-type orbital. Percent com-
positions of representative MOs are shown in Figure 6
and the Supporting Information, Figure S9.
As ordinarily observed for polypyridyl complexes, the
contributions from the first three occupied orbitals for the
pyridyl-imine based model 10 can be assigned to the Rudπ
orbitals. More specifically, the highest occupied molecu-
lar orbital (HOMO), HOMO-1, and HOMO-2 are com-
paratively similar in energy with 74-83% localization on
the metal ion. Although the orientation of HOMO-2 is
slightly different, the HOMO, HOMO-1, and HOMO-2
orbitals for 20 are quite consistent to the arrangement
observed for 10. Interestingly, the three lowest unoccupied
molecular orbitals (LUMOs) for 10 are distinctly unique
among the presented series. These three orbitals display
similar energy, rather than the typical set of symmetrical
and unsymmetrical combinations for bipyridines. The
LUMO is dominated by 70% localized contribution
of the pyridine-imine ligand, while the LUMOþ1
and LUMOþ2 are, respectively, the antisymmetric and
symmetric combinations of the bipyridine orbitals. In
The HOMO and HOMO-3 appear to be the result of π
interactions where the HOMO-3 (45: 46% phenolate-to-
metal) is the bonding orbital and the HOMO is described
by an antibonding arrangement (Scheme 2).
Correlations to Spectroscopic and Electrochemical
Data. Considerable differences in the behavior of 1-4
have been observed experimentally. Frontier orbital ar-
guments invoking 10-40 can be helpful to infer which
MOs are related to redox and spectroscopic processes.
This approach should be used with caution, considering
that orbitals are determined without nuclear relaxation
while electrochemistry is an equilibrium measurement.
Further complexity is brought to this picture when multi-
ple redox centers are involved. The electrochemical and
the DFT-calculated HOMO-LUMO gap are tabulated
in Table 3 and plotted in the Supporting Information,
Figure S10. The experimental data agrees well with the
theoretically calculated trend where 30 < 40 < 20 ≈ 10.
(28) Allard, M. M.; Odongo, O. S.; Lee, M. M.; Chen, Y.-J.; Endicott,
J. F.; Schlegel, H. B. Inorg. Chem. 2010, 49, 6840–6852.
(29) Cai, P.; Li, M. X.; Duan, C. Y.; Lu, F.; Guo, D.; Meng, Q. J. New J.
Chem. 2005, 29, 1011–1016.
(30) Chakraborty, S.; Walawalkar, M. G.; Lahiri, G. K. Polyhedron 2001,
20, 1851–1858.
(31) Shakya, R.; Imbert, C.; Hratchian, H. P.; Lanznaster, M.; Heeg,
M. J.; McGarvey, B. R.; Allard, M.; Schlegel, H. B.; Verani, C. N. Dalton
Trans. 2006, 2517–2525.

974 Inorganic Chemistry, Vol. 50, No. 3, 2011
Lesh et al.
Figure 6. Orbital composition for 10 and 30.
Scheme 2. Ru/Phenolate Orbital Interactions for 30 and 40
Figure 7. Compression isotherms of the metallosurfactants.
mixed
Ru-phenolato processes, rather than as formal RuII/RuIII or
phenolate/phenoxyl redox couples. This interpretation is
supported by the MLCT bands of 3 and 4 between 500 and
550 nm, where a similar trend is observed as a consequence of
a small HOMO-LUMO energy difference.
Amphiphilic Properties. The amphiphilic behavior of the
metallosurfactants 1-4 was analyzed by means of compres-
sion isotherms32 (Figure 7) and Brewster angle microscopy
(BAM).33,34 Langmuir film formation is monitored following
the spreading of solutions of the amphiphiles, dissolved in an
immiscible organic solvent, onto the aqueous subphase of a
minitrough with moveable barriers. As these barriers move
Table 3. Experimental and Calculated HOMO-LUMO Gaps
experimental
redox gap (V)a
calculated HOMO-LUMO
complex
model
gap (eV)b
closer to each other, compression isotherms plotting surface
2
pressure (Π, mN m-1) versus average molecular area (A,A )
1
2
3
4
2.56
2.46
1.94
2.11
10
20
30
40
3.3
3.3
2.5
2.8
˚
3
grant fundamental information concerning the two-
dimensional molecular organization of the monolayer at the
air/water interface, collapse pressures (πc), limiting areas per
molecule (Alim), and monolayer collapse areas (Ac). Simulta-
neously Brewster angle microscopy evaluates film homoge-
neity, domain and agglomerate formation upon passing
vertically polarized light through media possessing different
refractive indexes.
a Difference between half-wave potentials for oxidation and reduc-
tion. b B3LYP/LANL2DZ with IEF-PCM MeCN.
The tert-butyl-phenolate species presents the lowest
HOMO-LUMO gap (ΔEcalc=2.5 eV, ΔEexp=1.94 V),
and both of the pyridyl-based complexes demonstrate
comparable energy values. The differences observed can
be directly attributed to the HOMO orbital associated
with the anodic oxidation potential. Thus, the oxida-
tive processes must be described as involving heavily
(32) Petty, M. C. Langmuir-Blodgett Films: An Introduction; Cambridge
University Press: Cambridge, 1996.
(33) Mobius, D. Curr. Opin. Colloid Interface Sci. 1998, 3, 137–142.
(34) Vollhardt, D. Adv. Colloid Interface Sci. 1996, 64, 143–171.

Article
Given that the pyridyl-containing ruthenium amphi-
Inorganic Chemistry, Vol. 50, No. 3, 2011 975
philes 1 and 2 showed some solubility in water, complex
dissolution was prevented by using a 0.1 M NaCl aqueous
subphase with increased ionic strength. The compression
isotherms measured for 1 and 2 indicate the formation of
well-defined condensed phase regions and distinct col-
lapse pressures; properties characteristic of the formation
of stable monolayer films. The individual molecules of
both pyridyl-containing amphiphiles start interacting
at the air/water interface at an area of about 235
2
-1
˚
A molecule to form an expanded phase. No phase
3
transitions were observed, and 1 presents a collapse
pressure of about 29 mN m-1, while 2 shows a collapse
3
pressure of about 32 mN m-1. Amphiphiles 1 and 2 both
3
demonstrate a sudden decrease in surface pressures,
which is a trait typical of constant-area collapse
mechanisms.35,36 Collapse areas for these species were
obtained by extrapolating the steepest portion of the
isotherm to zero pressure, which have been determined
to be 125 and 120 A molecule-1 for 1 and 2, respec-
tively. Close structural resemblances can be attributed to
the similar interactions observed by the molecules of
both complexes at the air/water interface.
2
˚
3
Figure 8. BAM images of complexes 1 and 2.
Isothermal compressions for the phenolato-containing
ruthenium amphiphiles 3 and 4 were recorded in a 0.1 M
NaCl aqueous subphase. Although these species are
insoluble in water, this subphase was selected to keep
consistency. Single molecules of the tert-butyl-substituted
3 start interacting at the air/water interface at about 170
2
A molecule-1, whereas the molecules of the chloro-
˚
3
substituted 4 interact at a lower area of about 107
2
A molecule-1. These species do not show distinct phase
˚
3
transitions and display well-defined condensed phase regions
until the collapse pressure is reached. Similar surface collapse
pressures of about 39 mN m-1were observed for 3 and 4.
3
However, the tert-butyl-substituted 3 shows an isothermal
profile akin to a constant-pressure collapse mechanism, and
the chloro-substituted counterpart 4 presents a constant-
area collapse mechanism. Both mechanisms follow the Ries
sequence37,38 of folding, bending, and breaking into multi-
layers. Amphiphile 4 confers a moderately sharp area of
interaction relative to the other complexes in this series. The
Figure 9. BAM images of complexes 3 and 4.
limiting areas per molecule for 3 and 4 reach about 120
sion data. Likewise, the pyridyl-amine complex 2 shows a
homogeneous monolayer until collapse is reached at about
2
and 100 A molecule-1, respectively. The similar limiting
˚
3
32 mN m-1. The molecules of the phenolate-containing 3
and 4 form random domains before compression and
evolve to smooth, non-corrugated films. At a pressure of
areas per molecule for 1-4 are greater than the expected
3
values and can be accounted for by the increased ionic
strength of the subphase, suggesting some tilting of the alkyl-
chains.13
about 35 mN m-1 collapse is evident via the formation of
several spots interpreted as either Newton rings or vesicles
3
Representative Brewster angle micrographs have been
recorded simultaneously along with the isothermal com-
pressions for 1-4(Figures 8 and 9). Complexes 1and 2reveal
multiple domains before compression and at pressures lower
suggestive of thermodynamic film instability.39
Overview and Conclusions
than 4 mN m-1. The pyridyl-imine complex 1 exhibits a
3
In this article we have described the synthesis and char-
acterization of the new family of pyridyl- and phenolato-
containing amphiphiles described as [(LPyI)RuII(bpy)2](PF6)2
(1), [(LPyA)RuII(bpy)2](PF6)2 (2), [(LPhBuI)RuII(bpy)2](PF6)
(3), and [(LPhClI)RuII(bpy)2](PF6) (4). The viability of these
species as precursors for photoresponsive Langmuir-Blodgett
films was evaluated by addressing (i) the electronic properties
to assess the photostability and excitability (emission), (ii) the
smooth and homogeneous film throughout compression.
Formationof minordomains atabout 29mN m-1 suggest
collapse, directly correlating to the isothermal compres-
3
(35) Kundu, S.; Datta, A.; Hazra, S. Phys. Rev. E 2006, 73, 051608/
1–051608/7.
(36) Vaknin, D.; Bu, W.; Satija, S. K.; Travesset, A. Langmuir 2007, 23,
1888–1897.
(37) Ries, H. E., Jr. Nature 1979, 281, 287–289.
(38) Ybert, C.; Lu, W.; Moller, G.; Knobler, C. M. J. Phys.: Condens.
Matter 2002, 14, 4753–4762.
(39) Galvan-Miyoshi, J.; Ramos, S.; Ruiz-Garcia, J.; Castillo, R. J. Chem.
Phys. 2001, 115, 8178–8184.

976 Inorganic Chemistry, Vol. 50, No. 3, 2011
Lesh et al.
electrochemical properties to evaluate the nature of the redox
processes, and (iii) the amphiphilic properties to investigate the
potential for formation of ordered Langmuir-Blodgett films.
(i). Electronic Properties. Absorption spectral data
show the visible region dominated by dπ(RuII) f π*(bpy)
MLCT transitions for 1 and 2, along with dπ(RuII) f
π*(iminomethylpyridine) processes for 1. The pyridyl-
amine 2 shows a red-shifted band at 472 nm. The pheno-
lato complexes 3 and 4 present less intense and red-shifted
MLCT observed between 519-521 nm. Emission spectral
data show that species 1 and 2 emit at 715 and 641 nm,
respectively, with the second species having a lifetime 2.5
times longer than the first. The relative photolability of
these species was examined. Clear photochemical conver-
sion was observed for 2 in acetonitrile, but not in dichloro-
methane. On the basis of ESIþ mass spectrometric
methods, we suggested that 2 was converted into
[(MeCN)2RuII(bpy)2]2þ. The imines 1, 3, and 4 do not
show evidence of photodissociation.
(ii). Electrochemical Properties. Species 1-4 showed rich
redox chemistry, where two successive cathodic waves were
attributed to bipyridine reduction. More negative potentials
for these processes were observed for 3 and 4, whereas an
additional process was observed for 1 and ascribed to the
reduction of the imine-based LPyI ligand. Anodic waves were
associated to metal oxidation in 1-4 and the formation of
phenoxyl radicals for 3 and 4. DFT calculations based on
models 10-40 with shortened propyl chains have helped in the
interpretation of the experimental electronic and redox be-
havior of 1-4. The calculated HOMO-LUMO energy
differences correlate well with the observed electrochemical
potentials as follows: (a) the energy differences observed
for 1 and 2 when compared to 3 and 4, are directly
attributed to the HOMO orbital associated with the
oxidation processes, (b) the distinctive three low-lying
unoccupied LUMO orbitals for 10 seem consistent with
the electrochemical and emission spectroscopy results,
and (c) for 3 and 4, the oxidative processes are based on
heavily mixed Ru-phenolate based MOs that correlate to
broad low energy MLCT bands.
columns using an Innovative Technologies solvent purification
system. Infrared spectra were measured from 4000 to 400 cm-1 on
a Tensor 27 FTIR spectrophotometer in KBr pellets. H NMR
1
spectra were measured with Varian 300 and 400 MHz instruments.
ESI(positive) spectra were measured in a triple quadrupole Micro-
mass QuattroLC mass spectrometer with ESCi source. Elemental
analyses were performed by Midwest Microlab, Indianapolis, IN.
Absorption UV-visible spectroscopy from 1.0 ꢀ 10-3 to 1.0 ꢀ 10-5
M acetonitrile solutions were performed using a Cary 50 spectrom-
eter within the 250 to 1100 nm range. Fluorescence excitation and
emission spectra were measured on a Cary Eclipse fluorescence
spectrophotometer. Lifetime measurements were recorded using a
Hamamatsu R9220 type photomultiplier tube and decay traces were
collected using a National Instruments PCI-5154 digitizer. Samples
were excited using a Photochemical Research Associates Inc. nitro-
gen/dye laser combination LN1000 and LN107, respectively. Life-
times were determined by single exponential fitting of the
luminescence decay traces. Cyclic voltammetry experiments were
performed in 1.0 ꢀ 10-3 M dry acetonitrile analyte solutions
containing 0.1 M TBAPF6 supporting electrolyte using a BAS
50W voltammetric analyzer at a scan rate of 150 mV s-1. Astandard
three-electrode cell was employed with a carbon working electrode, a
Pt-wire auxiliary electrode, and an Ag/AgCl reference electrode
under an inert atmosphere at RT. All potentials are reported versus
the Fcþ/Fc internal standard reference couple.40
Computational Methods. Electronic structure calculations
were carried out with the Gaussian 09 suite of programs41
using DFT. Calculations with the B3LYP42-44 functional
employed the LANL2DZ45 basis set and pseudopotential.
Since all of the ground states were closed shell singlets,
calculations were carried out with spin restricted methods.
Tight self-consistent field (SCF) convergence (10-8 rms for
the density) was used throughout. Geometries were fully
optimized without symmetry constraints, and stationary
points were verified via frequency analysis. Solvent effects
in acetonitrile were estimated using the IEF-PCM polarizable
continuum model.46-48 Molecular orbitals were plotted with
GaussView.49
Photolability Studies. Irradiation of dissolved samples 1-3
was performed with a highly intense T-type halogen source (500
W) without use of an UV cutoff filter. Photoirradiation of each
sample at 1.0 ꢀ 10-3 M concentrations occurred in a 25 mL
round-bottom flask, fitted with a reflux condenser, under argon
(40) Gagne, R. R.; Koval, C. A.; Lisensky, G. C. Inorg. Chem. 1980, 19,
2854–2855.
(iii). Amphiphilic Properties. Species 1-4 are surface-
active and are strong candidates for the formation of
monolayer films, as characterized by compression iso-
therms and Brewster angle microscopy. The collapse
(41) Frisch, M. J.; Trucks, G. W.; Schlegel, H. B.; Scuseria, G. E.; Robb,
M. A.; Cheeseman, J. R.; Scalmani, G.; Barone, V.; Mennucci, B.; Petersson,
G. A.; Nakatsuji, H.; Caricato, M.; Li, X.; Hratchian, H. P.; Izmaylov, A. F.;
Bloino, J.; Zheng, G.; Sonnenberg, J. L.; Hada, M.; Ehara, M.; Toyota, K.;
Fukuda, R.; Hasegawa, J.; Ishida, M.; Nakajima, T.; Honda, Y.; Kitao, O.;
Nakai, H.; Vreven, T.; Montgomery, J. A.; Peralta, J. E.; Ogliaro, F.;
Bearpark, M.; Heyd, J.; Brothers, J. E.; Kudin, K. N.; Staroverov, V. N.;
Kobayashi, R.; Normand, J.; Raghavachari, K.; Rendell, A.; Burant, J. C.;
Iyengar, S. S.; Tomasi, J.; Cossi, M.; Rega, N.; Millam, J. M.; Klene, M.;
Knox, J. E.; Cross, J. B.; Bakken, V.; Adamo, C.; Jaramillo, J.; Gomperts,
R.; Stratmann, R. E.; Yazyev, O.; Austin, A. J.; Cammi, R.; Pomelli, C.;
Ochterski, J. W.; Martin, R. L.; Morokuma, K.; Zakrzewski, V. G.; Voth,
G. A.; Salvador, P.; Dannenberg, J. J.; Dapprich, S.; Parandekar, P. V.;
Mayhall, N. J.; Daniels, A. D.; Farkas, O.; Foresman, J. B.; Ortiz, J. V.;
Cioslowski, J.; Fox, D. J. Gaussian G09; Gaussian,Inc.: Wallingford, CT, 2009.
(42) Becke, A. D. J. Chem. Phys. 1993, 98, 5648–5652.
(43) Lee, C.; Yang, W.; Parr, R. G. Phys. Rev. B 1988, 37, 785–789.
(44) Miehlich, B.; Savin, A.; Stoll, H.; Preuss, H. Chem. Phys. Lett. 1989,
157, 200–206.
(45) Dunning, T. H.; Hay, P. J. In Modern Theoretical Chemistry; Plenum:
New York, 1976; Vol. 3, pp 1-28.
(46) Cossi, M.; Rega, N.; Scalmani, G.; Barone, V. J. Comput. Chem.
2003, 24, 669–681.
pressures are fairly high at about 29-32 mN m-1 for 1
3
and 2 and about 39 mN m-1 for 3 and 4. Relative
3
solubility in water for 1 and 2 requires the presence of a
NaCl aqueous subphase for proper film formation.
Knowledge gained from this effort provides relevant
insight toward the integration of amphiphilic prop-
erties in the design of photoresponsive precursors
for modular films aimed at artificial photosynthetic
processes. Our laboratories are currently working on
the deposition of Langmuir-Blodgett (LB) films and
their photophysical characterization. Integration of
[catalytic centers/antennae] into LB films is also under
development.
Experimental Section
(47) Miertus, S.; Scrocco, E.; Tomasi, J. Chem. Phys. 1981, 55, 117–129.
(48) Miertus, S.; Tomasi, J. Chem. Phys. 1982, 65, 239–245.
(49) Whangbo, M.-H.; Schlegel, H. B.; Wolfe, S. J. Am. Chem. Soc. 1977,
99, 1296–1304.
Materials and Methods. Reagents and solvents were used as
received from commercial sources. Methanol was distilled over
CaH2, and dichloromethane was doubly purified on alumina

Article
Inorganic Chemistry, Vol. 50, No. 3, 2011 977
blanketing and stirring for a time period of 40 min while keeping
constant the exposure intensity of irradiation. During this time
period aliquots were analyzed at times t = 0, 3, 20, and 40 min by
UV-visible spectroscopy and mass spectrometry.
2. Yield: 79%. Elemental anal. calcd for [C44H60F12N6P2-
Ru1]: C, 49.67, H, 5.68, N, 7.90%. Found: C, 49.21, H, 5.68, N,
7.95%. IR data (KBr, cm-1): 3670(w), 3287(w) (N-H); 3086(w)
(C-Harom); 2924(s), 2853(s) (alkyl chain C-H stretches);
1604(m) (CdNpyr); 1467(s), 1446(s) (CdCarom); 1162(m) (-C-
N-); 840(s) (PF6-). UV-visible data (ACN, 1.0 ꢀ 10-5 M): 245
(18 120), 291 (43 850), 342 (7450), 424 sh (4540), 472 (7070). 1H
NMR (400 MHz, CDCl3): δ 9.06 (d, 4H), 8.50-8.42 (m, 5H),
8.35 (m, 5H), 8.06 (d, 1H), 7.52 (t, 1H), 7.40 (t, 4H), 4.44 (s, 2H),
1.97 (t, 2H), 1.74 (s, 1H), 1.24 (m, 32H), 0.88 (t, 3H). MS data
(ESIþ in MeOH): m/z=387(100%) for([(LPyA)RuII(bpy)2]2þ)/þ2,
m/z = 919 for [(LPyA)RuII(bpy)2 þ (PF6-)]þ, and m/z = 773 for
[(LPyA)RuII(bpy)2]2þ - Hþ.
Isothermal Compression and Brewster Angle Microscopy. Mono-
layer studies were carried out using an automated KSV 200 mini
trough at a temperature of 18 (0.5 °C. Since compounds 1and 2are
found to be partially soluble in the pure water subphase, a 0.1 M
NaCl solution (pH ≈ 5.0) was prepared using ultrapure water
(Barnstead NANOpure) with a resistivity of about 18.2 MΩ cm-1
3
and was used as the subphase in each of the experiments. The surface
of the subphase was cleaned by vacuum suction after barrier
compression. Spreading solutions of a known concentration (1.0
mg mL-1) and a known quantity (30 μL),preparedinspectragrade
Preparation of the Metallosurfactants [(LPhBuI)RuII(bpy)2]-
(PF6) (3) and [(LPhClI)RuII(bpy)2](PF6) (4). A 10 mL isopropanol
or acetone solution of Ru(bpy)2(CF3SO3)2 (0.356 g, 0.5 mmol)
was added dropwise to a 30 mL isopropanol or acetone solution
containing either HLPhBuA (0.244 g, 0.5 mmol) or HLPhClA
(0.222 g, 0.5 mmol), respectively, and Et3N as base (0.076 g,
0.75 mmol) for deprotonation. Isolation and purification pro-
cedures were similar to those of 1 and 2.
3
chloroform, were then introduced on the clean aqueous subphase.
The system was then allowed to equilibrate for 15 min before
monolayer compression. The compression isotherms were obtained
at a compression rate of 10 mm min-1. The surface pressure was
3
measured using the Wilhelmy plate (paper plates 20 mm ꢀ 10 mm)
method. The selected isotherms represent the average of at least
three independent measurements with excellent reproducibility.
Brewster angle micrographs were taken simultaneously with the
compression isotherm using a KSV-Optrel BAM 300 equipped with
a HeNe laser (10 mW, 632.8 mm) and a CCD detector. The field of
view was 800 ꢀ 600 μm and the lateral resolution was about 1 μm.
3. Yield: 72%. Elemental anal. calcd for [C53H74F6N5O1P1-
Ru1]: C, 61.02, H, 7.15, N, 6.71%. Found: C, 61.25, H, 7.35, N,
6.69%. IR data (KBr, cm-1): 3120(w), 3078(w) (C-Harom);
2922(s), 2857(s) (alkyl chain and tert-butyl C-H stretches);
1602(m) (CdNpyr); 1465(s), 1442(s), 1423(s) (CdCarom); 1260(m),
1234(m) (C-O); 1161(m) (-C-N-); 841(s) (PF6-). UV-visible
data (ACN, 1.0 ꢀ 10-5 M): 248 (50 260), 294 (59 200), 377 (13
Syntheses. Preparation of the Ligands LPyI, LPyA, HLPhBuA
,
and HLPhClA. The ligands were synthesized according to the
literature or used as purchased from the commercial source.15,16
General synthetic approaches for complexes 1-4 followed
modifications of previously published procedures.4,14,17 The
starting complex Ru(bpy)2(CF3SO3)2 was prepared according
to the reported procedure.50
1
870), 476 sh (7950), 521 (8550). H NMR (400 MHz, CDCl3):
δ 8.71 (d, 4H), 8.22 (d, 4H), 8.05 (s, 1H), 7.83 (t, 4H), 7.75-
7.73 (s, 2H), 7.41 (t, 4H), 3.15 (t, 2H), 1.24 (m, 50H), 0.88
(t, 3H). MS data (ESIþ in MeOH): m/z = 898 (100%) for
[(LPhBuI)RuII(bpy)2]þ.
Preparation of the Metallosurfactants [(LPyI)RuII(bpy)2]-
(PF6)2 (1) and [(LPyA)RuII(bpy)2](PF6)2 (2). A 10 mL EtOH
4. Yield: 70%. Elemental anal. calcd for [C48H64Cl2F6N5O2-
P1Ru1]: C, 54.39, H, 6.09, N, 6.61%. Found: C, 54.60, H, 6.05,
N, 6.25%. IR data (KBr, cm-1): 3121(w), 3077(w) (C-Harom);
2923(s), 2852(s) (alkyl chain C-H stretches); 1602(w) (CdNpyr);
1459(s), 1442(s), 1418(s) (CdCarom); 1262(m) (C-O); 1172(m)
(-C-N-); 842(s) (PF6-). UV-visible data (ACN, 1.0 ꢀ 10-5 M):
solution of cis-[Ru(bpy)2Cl2] 2H2O (0.520 g, 1.0 mmol) was added
3
dropwise to a 30 mL EtOH solution containing either LPyI (0.394 g,
1.1 mmol) or LPyA (0.397 g, 1.1 mmol). In each instance, the
resulting mixtures were stirred under mild reflux overnight (24 h)
under an argon blanketing atmosphere and protected from light.
The solution was filtered while warm to eliminate unreacted solids,
and the filtrate was concentrated to half of the original volume by
rotary evaporation. Slow solvent evaporation after the addition of a
saturated solution of NH4PF6 in MeOH precipitated the crude
product which was filtered and washed with cold distilled water.
The compound was purified by column chromatography using a
neutral alumina column with toluene-acetonitrile (2:1) as eluent.
The solvent was removed, and the product was dissolved in acetone.
Slow solvent evaporation yielded an isolable dark red crystalline
powder after drying under vacuum.
1
247 (37 910), 295 (60 860), 363 (10 570), 519 (8380). H NMR
(400 MHz, CDCl3): δ 8.62 (d, 4H), 8.36 (d, 4H), 8.19 (s, 1H), 8.11
(t, 4H), 7.92-7.84 (s, 2H), 7.45 (t, 4H), 3.67 (t, 2H), 1.25 (m,
32H), 0.88 (t, 3H). MS data (ESIþ in MeOH): m/z = 856 (100%)
for [(LPhClI)RuII(bpy)2]þ.
Acknowledgment. This research was made possible by the
Division of Chemical Sciences, Geosciences, and Biosciences,
Office of Basic Energy Sciences of the U.S. Department of
Energy (DOE-BES) through the SISGR-Solar Energy Program
Grant DE-FG02-09ER16120 to C.N.V., J.F.E., and H.B.S.
Support to F.D.L., M.M.A., and R.S. is acknowledged. Com-
puter time allocated at the WSU-Grid System for the DFT
calculations is also acknowledged.
1. Yield: 76%. Elemental anal. calcd for [C44H58F12N6P2-
Ru1]: C, 49.76, H, 5.50, N, 7.91%. Found: C, 49.83, H, 5.44, N,
7.89%. IR data (KBr, cm-1): 3084(w) (C-Harom); 2920(s),
2851(s) (alkyl chain C-H stretches); 1606(m) (CdNpyr);
1466(s) (CdCarom); 1162(m) (-C-N-); 846(s) (PF6-). UV-visible
data (ACN, 1.0 ꢀ 10-5 M): 239 (17 330), 243 (17 530), 255 (16
030), 287 (44 120), 345 sh (4460), 432 sh (8940), 462 (11 080). 1H
NMR (400 MHz, CDCl3): δ 8.97 (d, 4H), 8.42 (d, 1H), 8.34 (d,
4H), 7.96 (d, 1H), 7.71-7.63 (m, 6H), 7.58 (s, 1H), 7.41 (t, 4H),
1.25 (m, 34H), 0.88 (t, 3H). MS data (ESIþ in MeOH): m/z = 386
(100%) for ([(LPyI)RuII(bpy)2]2þ)/þ2, m/z = 917 for [(LPyI)RuII-
(bpy)2 þ (PF6-)]þ, and m/z = 771 for [(LPyI)RuII(bpy)2]2þ - Hþ.
Supporting Information Available: Experimental and simu-
lated ESIþ peak cluster profiles for 1-4, and for the photosub-
stitution products in acetonitrile, UV-visible spectra for the
recorded photostability of 2 in DCM, schematics for represen-
tative DFT models, calculated orbital compositions and
energies, the correlation between experimental and calculated
half-wave potentials, and the Cartesian coordinates for the
optimized structures. This material is available free of charge
via the Internet at http://pubs.acs.org.
(50) Greaney, M. A.; Coyle, C. L.; Harmer, M. A.; Jordan, A.; Stiefel,
E. I. Inorg. Chem. 1989, 28, 912–920.