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Influence of nitrosyl coordination on the binding mode of quinaldate inselective ruthenium frameworks. Electronic structure and reactivity aspects{
Abhishek Dutta Chowdhury, Prinaka De, Shaikh M. Mobin and Goutam Kumar Lahiri*
Received 24th October 2011, Accepted 18th January 2012
DOI: 10.1039/c2ra00953f
The nitrosyl complexes, [RuII(trpy)(L)(NO+)Cl]BF4, [1]BF4, and [RuII(trpy)(L)(NO+)](BF4)2,
[2](BF4)2, (trpy = 2,29:69,299-terpyridine, L2 = deprotonated form of unsymmetrical quinaldic acid)
have been synthesized. Single crystal X-ray structures of [1]BF4 and [2](BF4)2 reveal that in the
former L2 binds to the ruthenium ion selectively in a monodentate fashion through the O2 donor
whereas the usual bidentate mode of L2 (O2, N donors) has been retained in [2](BF4)2 with the same
meridional configuration of trpy being seen in both. The Ru–NO group in [1]BF4 or [2](BF4)2,
exhibits almost linear (sp-hybridized form of NO+) geometry. The difference in bonding mode of the
unsymmetrical quinaldate in [1]BF4 and [2](BF4)2 has been reflected in their corresponding n(NO)/
n(CLO) frequencies as well as in their NO based two-step reduction processes, {RuII–NO+} A{RuII–NON} and {RuII–NON}A{RuII–NO2}. The close to bent geometry (sp2-hybridized form of
NON) of the one-electron reduced 1 or [2]+ is been reflected in their DFT optimized structures. The
spin density plot of the reduced species reveals that NO is the primary spin-bearing center with slight
delocalization onto the metal ion which has been reflected in its radical EPR spectrum. [1]+
and [2]2+ undergo facile photorelease of NO with significantly different kNO (s21) and t1/2 (s) values
which eventually lead to the concomitant formation of the corresponding solvent species. The
photoreleased NON can be trapped as an Mb–NO adduct. The reduced species 1 selectively reacts with
the molecular oxygen (O2) at pH y 1 to yield the corresponding nitro species,
[RuII(trpy)(L)(NO2)Cl]2.
Introduction
The important role of nitric oxide (NON) in various biological
and physiological processes, such as blood pressure regulation,
inflammatory response, and apoptosis has drawn renewed
research interest on nitrosyl chemistry in recent years.1–7 NON
is generated in biological processes by nitric oxide synthase
(NOS) during the oxidation of L-arginine to citrulline which
plays important roles in neurotransmission, smooth muscle
vasodilation and platelet disaggregation in mammals.6 The
interaction of NO with the metal ions is important from the
broader perspective of inorganic chemistry including in bioinor-
ganic chemistry.4,5 For example, the reactions of NON with
oxygenated heme-protein have considerable biological signifi-
cance.5 Though some organic nitrites, nitrates and S-nitrsothiols
have medicinal application as vasodilators,2 they are not suitable
for site specific NON delivery processes. However, transition
metal–nitrosyl complexes have shown potential application for
site-specific NON-delivery primarily due to photolabile nature of
the metal–nitrosyl bond.8–10 Among them, ruthenium nitrosyl
complexes have been emerged as a promising class of NO-donor
due to their reduced activity towards oxygen and stability in
water.8,9,11 Besides that, the non-innocent feature of NO
facilitates its accessibility in three different redox states, strongly
electrophilic NO+, neutral NON and anionic NO2, in transition
metal complexes depending on the electronic environment
around the metal center which in turn makes the nitrosyl
function as a versatile ligand in co-ordination chemistry.8,11
Further, ruthenium–nitrosyl complexes have shown considerable
applications in pharmaceuticals, catalysis, molecular electronics
and photochemical devices.12
In this context the present article describes the various aspects
of the coordinated nitrosyl function in the newly designed
selective molecular frameworks of [RuII(trpy)(L)(NO)Cl]n, [1]n,
and [RuII(trpy)(L)(NO)]n, [2]n, (trpy = 2,29:69,299-terpyridine, L2
= deprotonated form of unsymmetrical quinaldic acid). Herein
we report the synthesis and structural characterization of [1]BF4
and [2](BF4)2. Furthermore, the effect of structural diversity of
the co-ligand, L2 (monodentate versus bidentate) on the
electronic structures of [1]n and [2]n with special reference to
electrophilicity, redox potential and reactivity of the coordinated
nitosyl function have been investigated by experimental studies
Department of Chemistry, IIT Bombay, Powai, Mumbai, 400076, India.E-mail: [email protected]; Fax: 91-022-2572-3480{ Electronic supplementary information (ESI) available: Characterizationdetails of the complexes, crystallographic material and DFT results (TableS1–S7 and Fig. S1–S9). CCDC reference numbers 838835 and 838836. ForESI and crystallographic data in CIF or other electronic format see DOI:10.1039/c2ra00953f
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and DFT calculations.
Results and discussion
Synthesis, characterization and structural aspects
The complexes with Enemark–Feltham notation13 of {Ru(NO)}6
in [RuII(trpy)(L)(NO+)Cl](BF4), [1]BF4, and [RuII(trpy)(L)
(NO+)](BF4)2, [2](BF4)2, have been synthesized via the direct
reaction of NOBF4 with the previously structurally characterized
precursor complex [RuII(trpy)(L)Cl] (A)14 and the reaction of
NOBF4 with the in situ generated [RuII(trpy)(L)(C2H5OH)]+,
respectively, as shown in Scheme 1 (trpy = 2,29:69,299-terpyridine,
L2 = deprotonated form of unsymmetrical quinaldic acid,
HL).15,16
[1]BF4 and [2](BF4)2 exhibit satisfactory microanalytical and mass
spectral data (Fig. S1{) and show 1 : 1 and 1 : 2 molar conductivities
in acetonitrile solution, respectively (see Experimental Section).
The formation of [1]BF4 and [2](BF4)2 have been authenti-
cated by their single crystal X-ray structures (Fig. 1 and Table 1).
The five-membered chelate ring of L2 (through the O12 and N1
donors of L2) in the precursor A has been retained in [2](BF4)2
along with the usual meridional configuration of trpy.14
However, the direct nitrosylation of A (Scheme 1) surprisingly
leads to the concomitant transformation of the bidentate (O2, N
donors) mode of L2 to the monodentate (O2 donor) in [1]BF4
retaining the same meridional configuration of trpy.
The bond distances and bond angles in [1]BF4 and [2](BF4)2
(Table 2) are in good agreement with the reported data of
analogous complexes.8,9,11 The geometrical constraint due to the
meridional mode of trpy has been reflected in the appreciably
smaller trans angles involving the trpy ligand, N2–Ru–N4 of
156.5(3)u and 159.35(12)u in [1]BF4 and [2](BF4)2, respectively.
The central Ru–N3(trpy) bond lengths of 2.015(6) A in [1]BF4
and 1.981(3) A in [2](BF4)2 are significantly shorter than the
corresponding distances involving the terminal pyridine rings of
trpy, Ru–N2(trpy), 2.083(6) A and 2.075(3) A, and Ru–N4(trpy),
2.079(6) A and 2.079(3) A, respectively. The central Ru–N3(trpy)
distance in [1]BF4 is 0.034 A longer than that in [2](BF4)2 due to
the effect of the strongly p-accepting NO+ trans to the Ru–
N3(trpy). The Ru–O2(monodentate L2) bond distance in [1]BF4
(2.044(5) A) is appreciably longer relative to Ru–O2(chelated
L2) in [2](BF4)2 (1.990(2) A) due to the effect of oppositely
directed s/p-donor Cl2 versus the strongly p-accepting NO+
trans to the Ru–O2(L2) bond. The impact of varying coordina-
tion situations in the complexes has been reflected in their trans
angles: O1–Ru–Cl, 171.85(15)u and N3–Ru–N5, 175.6(3)u in
[1]BF4 versus O1–Ru–N5, 176.43(12)u and N(3)–Ru–N(1),
163.12(12)u in [2](BF4)2. The almost linear mode of Ru–N5–O3Scheme 1 The synthetic outline for [1]BF4 and [2](BF4)2.
Fig. 1 ORTEP diagrams of (a) [1]BF4?5H2O and (b) [2](BF4)2. Thermal
ellipsoids are drawn at 50% probability. The solvents of crystallization,
counter anions and hydrogen atoms are omitted for clarity.
3438 | RSC Adv., 2012, 2, 3437–3446 This journal is � The Royal Society of Chemistry 2012
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(NO), 173.0(8)u in [1]BF4 and 175.9(3)u [2](BF4)2 as well as the
triple bond feature of N5MO3 (NO) (1.141(9) A in [1]BF4 and
1.130(4) A in [2](BF4)2) establish the sp-hybridized state of the
nitrogen atom of the NO+ group as expected from the
coordinated p-accepting nitrosonium ion. However, the presence
of the p-accepting trpy ligand (N3) trans to Ru–N5–O3 in [1]BF4
makes the Ru–N–O angle (173.0(8)u) relatively more tilted
compared to that in [2](BF4)2 (175.9(3)u) where the Ru–N–O
group is trans to the s-donating O2 of the chelated L2. The
pendant quinaldate ring in [1]BF4 is slightly tilted (about 96u)with respect to the equatorial plane. The Ru–O1–C1 angle of
118.9(5)u implies that the bound oxygen (O1) is close to the sp2-
hybridized state which in turn introduces a resonating feature of
the carboxylate group (O1–C1, 1.276(9) A and C1–O2, 1.242(10)
A) in [1]BF4 (Table 2).
The DFT calculated bond parameters (Table 2) based on the
optimized structures of [1]+ and [2]2+ (Fig. S2{) are in general
agreement with the X-ray data.
The corresponding one-electron reduced species with
{Ru(NO)}7 configuration in [RuII(trpy)(L)(NON)Cl] (1) and
[RuII(trpy)(L)(NON)]+ ([2]+) can be generated electrochemi-
cally.8,11 The DFT calculated structural parameters of [1]+/1
and [2]2+/[2]+ (Fig. 2 and Table S1{) reveal similar structural
differences between the two sets of complexes based on the
electronic environment around the {Ru–NO} groups. The
s-donating ability of the carboxylate oxygen (O1) of L2 makes
the Ru–N5–O3 angle relatively more bent in [2]+ (139.6u) than in
1 (141.85u) where the Ru–NO group is situated trans to the
p-accepting trpy (N3) ligand (Fig. 3). The difference in calculated
Ru–N5–O3 angles between [2]2+ and [2]+ of y35u is reasonably
larger than that between [1]+ and 1 (y29u) implying greater
electron density on N(5) in [2]+ as has also been revealed by the
NBO studies (Table 3). The double bond feature of N5–O3
(NO), 1.176 A and 1.18 A in 1 and [2]+, respectively, suggests the
sp2 character of the nitrogen atom. The lengthening of the Ru–
N5 bond upon NO based reduction, 0.14 A for [1]+/1 and 0.12 A
for [2]2+/[2]+ due to increasing electron–electron repulsion upon
addition of an electron is in agreement with the established
concept of labilization of the Ru–NO bond on reduction.11h
Spectral and redox aspects
The 1H NMR spectra of [1]+ and [2]2+ in (CD3)2SO exhibit the
calculated number of seventeen partially overlapping aromatic
proton resonances in each case (Fig. S3{). The extent of overlap
of the proton signals is appreciably larger in [2]2+ as compared
to [1]+. The maximum downfield shifted signals in [2]2+ and [1]+
appear at 10.2 ppm and 9.2 ppm, respectively. This can be
attributed to the proton trans to the quinoline nitrogen N(1)
of the chelated L2 opposite to the central pyridine ring of
the p-acceptor trpy in [2]2+ whereas the same atom in the
monodentate quinoline ring in [1]+ exists away from the
coordination sphere.
Table 1 Selected crystallographic parameters
[1]BF4?5H2O [2](BF4)2
Empirical formula C25H17B1Cl1F4N5O8Ru C25H17B2F8N5O3RuMr 738.77 710.13Crystal system Triclinic TriclinicSpace group P1 P1a/A 8.5160(3) 8.4478(2)b/A 10.1858(4) 8.9532(2)c/A 16.7736(6) 17.6431(4)a (u) 92.631(3) 94.079(2)b (u) 102.713(3) 91.367(2)c (u) 93.147(3) 98.405(2)V/A3 1414.66(9) 1315.96(5)Z 2 2m/mm21 0.733 0.693T/K 150(2) K 120(2)Dc/g cm23 1.734 1.792F(000) 736 7042h range (u) 6.54 to 50 6.58 to 50data/restraints/parameters
4952/0/434 4622/0/397
R1, wR2 [I . 2s] 0.0698, 0.2092 0.0396, 0.1046R1, wR2 (all data) 0.0795, 0.2136 0.0435, 0.1067GOF 1.136 1.061largest diff. peak,hole/e A23
2.399 and 20.755 1.307 and 20.889
Table 2 Selected bond distances and bond angles in [1]BF4 and[2](BF4)2
Bond distance (A)/Bond angle (u)
[1]+ [2]2+
X-Ray DFT X-Ray DFT
Ru–N1 — — 2.116(3) 2.19Ru–N2 2.083(6) 2.11 2.075(3) 2.14Ru–N3 2.015(6) 2.03 1.981(3) 2.02Ru–N4 2.079(6) 2.11 2.079(3) 2.13Ru–N5 1.754(7) 1.79 1.758(3) 1.80Ru–O1 2.044(5) 2.05 1.990(2) 1.97Ru–Cl 2.361(2) 2.44 — —O(1)–C1 1.276(9) 1.30 1.317(4) 1.34O(2)–C1 1.242(10) 1.24 1.202(5) 1.21N(5)–O3 1.141(9) 1.14 1.130(4) 1.15N1–Ru–N3 — — 163.12(12) 160.82N2–Ru–N4 156.5(3) 156.32 159.35(12) 158.22O1–Ru–N5 98.3(3) 97.80 176.43(12) 175.03N3–Ru–N5 175.6(3) 175.95 94.83(13) 94.98Cl–Ru–O1 171.85(15) 171.59 — —N5–Ru–N2 100.1(3) 100.80 96.49(13) 90.86N5–Ru–N3 175.6(3) 175.95 94.83(13) 94.98N5–Ru–N4 103.4(3) 102.88 91.29(13) 95.83N5–Ru–N1 — — 101.82(12) 104.18N1–Ru–N4 — — 96.52(11) 99.17N3–Ru–O1 85.8(2) 86.11 84.26(11) 81.61Ru–N5–O3 173.0(8) 170.25 175.9(3) 174.02Ru-1-C1 118.9(5) 117.21 116.6(2) 119.15
Fig. 2 The DFT optimized geometry of (a) 1 and (b) [2]+. The hydrogen
atoms are omitted for clarity.
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The MOs of [1]+ and [2]2+ (Tables S2 and S4{) predict that in
both cases the HOMOs are primarily composed of L2 based
orbitals. The LUMO and LUMO + 1 are however dominated by
NO based orbitals which in effect make them susceptible towards
reduction (Tables S2 and S4{). Accordingly, [1]+ and [2]2+ exhibit
two successive reductions, Eu298,V (DEp, mV) at 0.31(70),
20.34(80) and 0.05(60), 20.64(90) in CH3CN versus SCE
corresponding to the {RuII–NO+} A {RuII–NON} (I) and
{RuII–NON} A {RuII–NO2} (II) couples, respectively (Fig. 4).8,11
The selective trans orientation of two p-accepting groups, trpy and
NO+ in [1]+ makes the reduction processes relatively easier than
that in [2]2+ where the NO+ is trans to the electron rich
O2 donor of L2. This has also been reflected in the greater
natural charge on N(5) (NO) in [1]+ than [2]2+ (Table 3). The
significant contribution of trpy based orbitals in higher UMOs
results in trpy based quasi-reversible reductions at further negative
potentials, Eu298,V (DEp, mV) of 20.84(100), 21.65(110) and
20.7(110), 21.15(110) for [1]+ and [2]2+, respectively.8a–c,11a,h–m,14
[1]+ and [2]2+ exhibit moderately intense transitions in the
near-UV region, 326 nm and 348 nm, respectively, followed by
several intense higher energy intraligand transitions in the UV
region in CH3CN (Fig. 5).8,11 The bands in the near-UV region
are assigned on the basis of the TD-DFT calculations on the
optimized structures of [1]+ and [2]2+ as the RuII(dp)/L(p) ANO+(p*) transition (Tables S5 and S6{). The slight difference in
electronic spectra in the complexes can be attributed to the
mixing of chloride ion orbitals in the HOMOs of [1]+ and the
denticity of L2. Upon one-electron reduction to [1] and [2]+ the
near UV region bands shift to the lower energy region at 556 nm
and 493 nm, respectively, which are assigned to the RuII(dp)/
NON(p) A p*(trpy) and RuII(dp)/NON(p) A L(p*) transitions,
respectively, based on the TD-DFT calculations.
The n(CLO) frequency of the coordinated L2 in the precursor
[(RuII(trpy)(L)(Cl)] (A) at 1635 cm21.14 has been appreciably
shifted to 1667 cm21 and 1696 cm21 in [1]BF4 and [2](BF4)2,
respectively (Fig. S4{) due to their different electronic environ-
ments. The characteristic vibrations of the BF42 counter anion
appear near 1600 cm21 and 1080 cm21. The reasonably high
n(NO) frequencies of [1]BF4 and [2](BF4)2 of 1895 cm21 (DFT:
1906 cm21) and 1926 cm21 (DFT: 1939 cm21), respectively,
imply their moderately electrophilic character. Upon one-
electron reduction to 1 and [2]+, the NO bands at 1895 cm21
and 1926 cm21 disappear. However, the n(NON) frequency of the
reduced state in the expected SWIR region of 1600–1700 cm21
did not resolve properly due to the presence of other
characteristic vibrations of the CLO of coordinated L2, BF42
counter anion as well as aryl ring vibrations.
The EPR spectrum of the representative one-electron reduced
paramagnetic [2]+ in frozen CH3CN/0.1 M Bu4N(PF6) solution
yields g-components at 2.012 (g1), 1.988 (g2) and 1.869 (g3) (Fig.
S5{) with a g-anisotropy (g1 2 g3) of 0.143, which is about twice
a large as that observed for the related {Fe(NO)}7 species due to
f(Ru) # 2f(Fe) (f = spin–orbit coupling constant).10b,11h
However, the value of ,g. = [1/3(g12 + g2
2 + g32)]1/2 = 1.957
implies that the spin is primarily localized on the N(5) of
NO.17,18 The overall negative shift of the g value (Dg = 45.0 ppt)
Fig. 3 Schematic representation of 1 and [2]+.
Table 3 The detailed NBO results of {Ru(NO)}n, (n = 6,7)
Total atomic charge Natural charge
Ru N(5) O(3) Cl Ru N(5) O(3) Cl
[1]+ 0.733 0.135 20.068 20.226 0.737 0.383 20.065 20.491[1] 0.617 0.026 20.182 20.349 0.635 0.184 20.194 20.576[2]2+ 1.013 0.054 20.070 — 0.802 0.317 20.072 —[2]+ 0.840 20.022 20.189 — 0.687 0.139 20.196 —
Fig. 4 Cyclic voltammograms of (a) [1]+ and (b) [2]2+ in CH3CN/0.1 M
[Et4N](ClO4) versus SCE, scan rate:100 mV s21.
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with respect to the free electron value of 2.0023 arises due to the
admixture of higher excited states with nonzero angular
momentum (eqn (1)).18 The radical EPR feature of [2]+ (Fig.
S5{) has been reflected in the significant bending of Ru–N(5)–
O(3) angle (139.69u) and lengthening of the N(5)–O(3) bond
(1.181 A).
g~ge{2
3
X
i
X
n
X
kj
SY0 jkLdkj jYnTSYn Lijdj
�� ��Y0TEn{E0
~gezDg (1)
j: spin orbit coupling constant
L: angular momentum operator
E0: energy of the SOMO
The SOMO of [2]+ indicates s-donation from the NO(p*)
orbital to the Ru(dz2) center which reveals {RuII–NON} as the
predominant oxidation state formulation along with consider-
able mixing of the {RuI–NO+} state due to the presence of 23%
metal contribution. The presence of y10% spin on the metal in
spin density analysis also reveals that spin is mainly concentrated
on NO (Fig. 6). Moreover, s-interaction between Ru and NO
results in spin density at the axial position (Fig. 6) which leads to
a significant hyperfine splitting in the EPR spectrum due to the
N(5) of NO.
Electronic features: theoretical insights
Molecular orbital analysis reveals that the LUMOs of [1]+ and
[2]2+ originate from the interaction of the p*-orbital of NO+ with
the metal’s t2g(dxy) and eg(dz2) orbitals, respectively, (Tables S2
and S4{).10b,11c–h,17 This is attributed to stronger back-bonding
in [1]+ between the metal t2g(dp) orbital and the p*-orbital of
trpy in the filled MOs. The presence of 10–25% metal
contribution in the LUMOs lowers the energy of the metal
t2g(dp) orbitals and thus the HOMOs are mainly composed of
the orbitals of the co-ligands (trpy, L or Cl).10b The significant
metal contribution (y58%) in [2]2+ has been predicted in the
HOMO 2 5 state whereas around 40% metal contribution in [1]+
has been detected in HOMO 2 11 which also provides evidence
for the lesser extent of back-bonding in [2]2+. The presence of a
s/p-donating chloride ion plays a crucial role for the stronger
back-bonding in [1]+. This is reflected in a greater natural charge
on the metal ion in [2]2+ than [1]+ (Table 3). The observed more
linearity of the {Ru–N(5)–O(3)} bond in [2]2+ (175.9(3)u) as
compared to [1]+ (171.0(8)u) suggests relatively larger degeneracy
of the p*-orbitals (LUMO and LUMO + 1) in [2]2+.
The addition of one-electron to the p*-orbital of {RuNO}6 in
[1]+ or [2]2+ leads to the formation of a {RuNO}7 species, 1 or [2]+
and hence lifts the said degeneracy of the p*-orbitals (LUMO and
LUMO + 1) (Tables S3–S4{).10b,17a Such a splitting can be viewed
as a Jahn–Teller splitting due to the lowering of symmetry and the
spin–orbit interaction which is reflected in the bending mode of
Ru–NO with Ru–N(5)–O(3) angles of 141.85u and 139.69 in 1 and
[2]+, respectively, as revealed in their DFT optimized structures.
The SOMO of 1 or [2]+ is primarily composed of the 2p(p)-atomic
orbitals of N5 and O3 (p*(NON)) along with a lesser extent of
4dxy(RuII) orbital of 1 and dz2(RuII) orbital of [2]+. The
appreciable extent of metal contribution in the SOMO suggests
{RuII–NON} as the predominant oxidation state along with partial
mixing of the {RuI–NO+} state.11c–i,l The SOMO of 1 suggests the
presence of a 4dxy(RuII) A pp*(NON) back-bonding interaction
while the SOMO of [2]+ reveals the s-charge donation from the
low-lying singly-occupied pp*(NON) to the metal eg-orbitals. This
can be attributed to the different coordination environment of the
NO function in the complexes: NO is trans to the p-accepting trpy
Fig. 5 Electronic spectra in CH3CN of (a) [1]+ (black), 1 (red) and (b)
[2]2+ (black), [2]+ (red).
Fig. 6 Mulliken atomic spin density plot for [2]+ (N(5): 0.514, O(3):
0.329, Ru: 0.096).
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ligand in the equatorial plane in [1]+ whereas in [2]2+ the NO is
trans to the s-donating O2 of L2 in an axial orientation.
The approximate bent geometry of {Ru–NO}7 in 1 and [2]+
introduces the possibility of a pair of conformational isomers
based on the dihedral angle (h) of Ltrans–Ru–N5–O3, with the
idealized eclipsed and staggered angles of h = 0u and h = 45u,respectively.11b–d,h The geometry optimization at the G03/
(U)B3LYP level reveals that the eclipsed conformation is more
stable by 0.01 eV in [2]+. However, neither eclipsed nor staggered
conformation is found to be perfectly suitable for 1 where the
dihedral angle (h) of Ltrans(N3)–Ru–N5–O3 is 28.3u (Fig. S6{).
Such a pseudo-staggered (h = 28.3u) conformation in 1 is more
stable by 0.05 eV and 0.12 eV with respect to the eclipsed (h = 0u)and staggered (h = 45u) forms, respectively. Another theoretically
possible staggered conformation with the dihedral angle of h =
245u is destabilized under the same level of DFT presumably
due to the repulsive interaction between O3 and O2. The
stereoelectronic effect of the chloride and O2 from bulky L in 1
collectively prevent it exhibiting either the eclipsed (h = 0u) or
staggered (h = 45u) conformation, leading to an energetically
favored pseudo-staggered (h = 28.3u) conformation.
Photo-lability of the {Ru–NO} bond
The facile photo-labilization of the {RuII–NON} bond maintain-
ing the integrity of the remaining part of the molecule is believed
to be significant particularly from the perspective of the
biochemically desired target oriented NON delivery process.8,9
In this context both the nitrosyl complexes, [RuII(trpy)(L)
(NO+)Cl]+, [1]+, and [RuII(trpy)(L)(NO+)]2+, [2]2+, are found
to undergo the facile photocleavage of the {Ru–NO} bond under
the exposure of light in CH3CN as evidenced by their spec-
troscopic signatures (Fig. 7).19 The photolabilization of the
{Ru–NO} bond is accompanied by the formation of the corre-
sponding solvent bound ruthenium(II)-photoadducts, [RuII(trpy)
(L)(Cl)(CH3CN)] and [RuII(trpy)(L))(CH3CN)]+, respectively,
and the transformation proceeds through several isosbestic
points (Fig. 7). The formation of an Mb–NO adduct on passing
the liberated ‘‘NO’’ through the aqueous solution of reduced Mb
under deoxygenated conditions has been evidenced by its
characteristic absorption band at lmax = 420 nm (Fig. S7{).
The estimated first-order rate constant (k/s21) and t1/2/s values of
the photocleavage process are 2.6 6 1021, 2.66 and 2.9 6 1022,
23.8 for [1]+ and [2]2+, respectively. The ten-fold faster
photolability of the {RuII–NON} bond in [1]+ as compared to
[2]2+ can be rationalized based on their structural differences
including the trans influence of co-ligands. The cleavage of the
{RuII–NO+} bond via the photo-irradiation process is known to
proceed through the formation of the intermediate excited S = 1
state in {RuIII–NON}* as shown below.8f
[RuII–NO+] + hn A [RuIII–NON]* A [RuII–solvent] + NON
The formation of a solvated Ru(II) species instead of Ru(III)–
solvate as a photoproduct has been attributed to the absence of
the otherwise expected EPR signal of Ru(III) as has also been
established earlier.8 The electronic effect of p-accepting ligands
certainly facilitates the formation of {RuII–CH3CN} in the
ground state of the photo-product, as has also been established
recently by us.8g It should be noted that the selective
photocleavage of the M–NO bond, maintaining the integrity of
the rest of the molecule is biologically significant.9 The
competition between the pp-orbitals of NO and N3(trpy) for
the same dp-orbital of the metal ion (observed in HOMO 2 4)
makes the {Ru–NO} bond in [1]+ more photolabile. On the other
hand, the greater extent of dp(Ru) A pp(NO) back-bonding as
well as trans-influence of the s-donating carboxylate group (O1
of L2) are the likely factors for the relatively slower photo-
dissociation process in [2]2+.
Reactivity of {Ru–NO} towards molecular oxygen: dioxygenase
activity
The reaction of NO with the oxygenated heme-proteins has
immense biological importance.5 Though nitrogen monoxide
plays crucial roles in various physiological processes, over-
production of NO can also lead to several toxicological
processes, such as cell death and DNA damage, primarily due
to the formation of highly reactive peroxynitrite (2OONLO).20
Nitric oxide dioxygenase (NODs) catalyzes the reaction of NO
Fig. 7 Time evolution of the electronic spectra of (a) [1]+, concentra-
tion: 0.57 6 1024 M in CH3CN, time intervals: 2 s, and (b) [2]2+,
concentration: 0.21 6 1025 M in CH3CN, time intervals: 5 s under the
exposure of light (Xe lamp, 350 W). Insets show the absorbance versus
time plots at (a) 326 nm and (b) 482 nm corresponding to the solvent
species in each case.
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with dioxygen to yield the environmentally and physiologically
benign nitrate anion (NO32) in mammals.21 Highly reactive
peroxynitrite (2OONLO or oxoperoxonitrate) is known to be the
powerful oxidant/nitrating agent in nitric oxide biochemistry and
has an influential role in stress injury.21 The selective conversion
of peroxynitrite (2OONLO) to biologically benign nitrate takes
place in oxygenated heme-proteins to control the overproduction
of NON22,23 but in synthetic model systems, peroxynitrite usually
transforms to nitrite.24a–b,d
Although the reduced [2]+ remains inactive towards molecular
oxygen (O2), 1 (in situ generated via the addition of N2H4 in the
CH3CN solution of [1]+ or [2]2+) is found to activate molecular
oxygen at 298 K. Upon bubbling dioxygen (O2) in an acetonitrile
solution of 1 at pH y 1, the intensity of the peaks at 525 nm and
376 nm corresponding to 1 periodically decreases with the
concomitant growth of a new peak at 476 nm (Fig. S8{). The
transformation proceeds through several isosbestic points at
501 nm, 399 nm and 355 nm, implying a clean process with the
selective involvement of two species, [RuII(trpy)(L)(NON)Cl] (1)
and [RuII(trpy)(L)(NO2)Cl]2 ([1a]2). The formation of [1a]2 is
evidenced from its ESI-MS(+) peak at 554.88 corresponding to
{([1a]–Cl) + H+} (calcd. mass: 554.03) (Scheme 2 and Fig. S9{).
The transformation of 1 to [1a]2 is likely to occur via the
intermediate transient peroxynitrite species {Ru–(OONLO)}
([1a9]2). Consequently, the oxygenation reaction of 1 in the
presence of tyrosine-mimic 2,4-di-tert-butylphenol at pH y 1
results in the nitrated product, 2,4-di-tert-butyl-6-nitrophenol
(NO2–DTBP) and oxidative coupling product, 2,29-dihydroxy-
3,39,5,59-tetra-tert-butyl-1,19-biphenyl as depicted in Scheme 2.24
Conclusions
The present article highlights the following points:
- The unprecedented hemilabile feature of the chelated
quinaldate ligand (L2) in the presence of NO+ in the molecular
framework of [1]+ comprising of selective co-ligands, p-acepting
trpy and s/p-donating chloride.
- The electronic aspects of the coordinated nitrosyl function in
[1]BF4 and [2](BF4)2 differ appreciably based on their specific
structural features as evidenced by their n(NO) frequencies and
Eu(RuII–NO+/RuII–NON) potentials.
- The built in electronic structural differences in [1]+ and
[2]2+ have further been reflected in the rate of light induced
{RuII–NO+} bond cleavage.
- Reduced 1 has been selectively transformed to the
corresponding {RuII–NO2} species through contact with mole-
cular oxygen, although the corresponding [2]+ failed to exhibit
any such activity with O2.
Experimental section
Materials
The precursor complexes Ru(trpy)Cl325a and [RuII(trpy)(L)(Cl)]
14 (trpy = 2,29:69,299-terpyridine) were prepared according to
literature procedures. The ligand quinaldic acid (HL) and other
reagents and chemicals were obtained from Aldrich and used as
received. For spectroscopic and electrochemical studies HPLC-
grade solvents were used.
Physical measurements
1H NMR spectra were recorded in (CD3)2SO on a 400 MHz
Bruker spectrometer. Chemical shift data are quoted as d in ppm
and as s, d, dd, t, q and m representing singlet, doublet, doublet of
doublet, triplet, quartet, sextet and multiplet peaks, respectively.
IR and UV-vis spectra were recorded using Thermo Nicolet 320
and Perkin Elmer Lambda 950 spectrophotometers, respectively.
ESI-mass spectra were recorded using micromass Q-TOF. Cyclic
voltammetric studies were carried out using a PAR model 273A
electrochemistry system. Platinum wire working and auxiliary
electrodes and an aqueous SCE were used in a three-electrode
configuration. The supporting electrolyte was 0.1 mol dm23
[NEt4](ClO4), and the solute concentration was y1023 mol dm23.
The half-wave potential Eu298 was set equal to 0.5(Epa + Epc),
where Epa and Epc are the anodic and cathodic cyclic voltammetric
peak potentials, respectively. Elemental analyses were carried out
on Perkin-Elmer 240C elemental analyzer. The 2,4-di-tert-butyl
phenol (DTBP) reactions were monitored by gas chromatographic
technique with a FID detector (Shimadzu GC-2014 gas chroma-
tograph) as well as GCMS (Hewlett-Packard GCD-HP1800A).
The EPR measurement was made in a two-electrode capillary tube
with a X-band Bruker system ESP300.25b
Scheme 2 Dioxygenase activity of 1 at pH y 1.
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Synthesis of [RuII(trpy)(L)(NO+)Cl]BF4 ([1]BF4). 50 mg of
[RuII(trpy)(L)(Cl)] (A, 0.09 mmol) and 4 equivalent of NOBF4
(42 mg, 0.36 mmol) were taken in 20 cm3 dichloromethane. The
mixture was stirred initially at 0 uC for 30 min followed by at
298 K for another 2 h. During the course of the reaction the
initially blue solution of [RuII(trpy)(L)(Cl)] (A) changed to red
and a dark yellow precipitate was formed. The precipitate was
allowed to settle inside the refrigerator for 1 h and then filtered
off under reduced pressure and washed thoroughly with
dichloromethane and diethyl ether and dried in vacuo. The solid
mass was recrystallized from 1 : 1 acetonitrile–benzene solution.
Yield: 45 mg (75%). Anal. calcd. for C25H17N5ClO3BF4Ru (Mol.
wt.: 659.01): C, 45.52; H, 2.60; N, 10.62. Found: C, 45.35; H,
2.58; N, 10.53%. Molar conductivity (LM [V21 cm2 M21],
CH3CN): 105. ESI(+)-MS (m/z, CH3CN): 572.05 ([1]+), 543.04
([1–NO + H]+), 537.08 ([1–NO–Cl]+). 1H NMR (400 MHz,
(CD3)2SO): d (ppm) (J/Hz): 9.25 (1H, d, 8.4), 9.09 (2H, d, 8.4),
9.02 (2H, d, 8.0), 8.97 (1H, d, 7.2), 8.70 (1H, d, 8.8), 8.67 (3H,
m), 8.34 (2H, m), 8.15 (1H, t, 7.84, 7.20), 8.02 (2H, d, 7.3), 7.79
(2H, m). IR (KBr) n(BF42): 1083, 1601; n(NO+):1895; n(CLO):
1667 cm21. l/nm (CH3CN) (e/dm3 mol21 cm21): 455(sh),
349(10 380), 326(15 120), 315(14 120), 283(16 540).
Synthesis of [RuII(trpy)(L)(NO+)](BF4)2 ([2](BF4)2). A mixture
of [RuII(trpy)(L)(Cl)] (50 mg, 0.09 mmol) and AgNO3 (153 mg,
0.9 mmol) were taken in 25 cm3 of ethanol and heated to reflux
with constant stirring for 1 h. The solution was cooled to room-
temperature and filtered through Celite to remove the white
precipitate of AgCl. Nitrosonium tetrafluoroborate (NOBF4,
16 mg, 0.14 mmol) was then added to the above filtrate and the
resulting solution was stirred for 6 h. Partial removal of the
solvent under reduced pressure resulted in dark solid which was
collected through filtration. The solid mass thus obtained was
washed several times with diethyl ether and dried in vacuo. The
product was recrystallized from 1 : 1 benzene–acetonitrile. Yield:
26 mg (55%). Anal. calcd. for C25H17N5O3B2F8Ru (Mol. wt.
711.04): C, 42.19; H, 2.41; N, 9.85. Found: C, 42.25; H, 2.45; N,
9.89%. Molar conductivity (LM [V21 cm2 M21], CH3CN): 190.
ESI(+)-MS (m/z, CH3CN): 624.31 ([2](BF4)2–BF4]+). 1H NMR
(400 MHz, (CD3)2SO): d (ppm) (J/Hz): 10.25 (1H, d, 8.5), 9.18
(2H, m), 8.92 (5H, m), 8.49 (2H, m), 8.28 (1H, d, 8.4), 7.94 (3H,
m), 7.75 (1H, m), 7.61 (2H, m). IR (KBr), n(BF42): 1083, 1599;
n(NO+):1927; n(CLO): 1696 cm21. l/nm (CH3CN) (e/dm3 mol21
cm21): 346(20 920), 325(20 360), 289(24 380), 279(26 770).
Trapping of photoreleased ‘‘NO’’ by myoglobin
3.0 cm3 acetonitrile solution of the nitroso species ([1]+ or [2]2+)
was initially taken in a quartz cuvette of optical path length of
1 cm. The cuvette was sealed with a rubber septum and the
solution was deoxygenated by purging nitrogen gas. The
photolyis was carried out for 10 min using a Xe 350 W lamp.
The photoreleased free ‘‘NO’’ was allowed to pass through the
reduced myoglobin solution in water using a cannula and the
UV-vis. spectrum was recorded.
Dioxygenase activity
The conversion process of [RuII(trpy)(L)(NON)Cl] (1) A[RuII(trpy)(L)(NO2)Cl]2 ([1a]2) in acetonitrile at pH y 1 and
in presence of bubbling O2 was monitored by following the
increase in absorbance of the new band at 476 nm corresponding
to lmax of the nitro species [1a]2 till the changes of intensity
completely levelled off. The above experiment was then repeated
in presence of 2,4-di-tert-butylphenol (DTBP) at 298 K and the
formation of corresponding products, 2,4-di-tert-butyl-6-nitro-
phenol (NO2-DTBP) and oxidative coupling product, 2,29-dihy-
droxy-3,39,5,59-tetra-tert-butyl-1,19-biphenyl were confirmed by
GC and GCMS.
Crystallography
Single crystals of [1]BF4 and [2](BF4)2 were grown by slow
evaporation of their 1 : 1 acetonitrile–benzene solutions. Single
crystal X-ray diffraction data were collected using an OXFORD
XCALIBUR-S CCD single crystal X-ray diffractometer at
150 K. The structures were solved and refined by full-matrix
least-squares techniques on F2 using the SHELX-97 program.26
All data were corrected for Lorentz polarization and absorption
effects, and the non-hydrogen atoms were refined anisotropi-
cally. Hydrogen atoms were included in the refinement process
as per the riding model. The complex [1]BF4 was crystallized
with five water molecules. CCDC-838835 and CCDC-838836
contain the supplementary crystallographic data for [1]+ and
[2]2+, respectively. These data can be obtained free of charge
from The Cambridge Crystallographic Data Centre via
www.ccdc.cam.ac.uk/data_request/cif
Computational details
Full geometry optimizations were carried out at the (R)B3LYP
and (U)B3LYP levels27,28 using density functional theory
method with Gaussian 03 (revision C.02).29 All elements except
ruthenium were assigned the 6-31G(d) basis set during geometry
optimizations and 6-31G(d,p) during single point and property
calculations. The LanL2DZ basis set with effective core potential
was employed for the ruthenium atom.30,31 Vertical electronic
excitations based on (R)/(U)-B3LYP optimized geometries were
computed for the time-dependent density functional theory (TD-
DFT)32 in acetonitrile using the Polarizable continuum model
(PCM) of Tomasi and co-workers,33 specifically, the conductor
like PCM (CPCM) in conjugation with the united atom
topological model (UAO radii, implemented in Gaussian 03)
was applied.33–35 GaussSum was used to calculate the fractional
contributions of various groups to each molecular orbital.36 No
symmetry constraints were imposed during structural optimiza-
tions, and the nature of the optimized structures and energy
minima were defined by subsequent frequency calculations.
Natural bond orbital analyses were performed using the NBO
3.1 module of Gaussian 03 on optimized geometry.37 All the
calculated structures were visualized with ChemCraft.38
Acknowledgements
The financial support received from Department of Science and
Technology (DST), New Delhi and Council of Scientific and
Industrial Research (CSIR), New Delhi (fellowship to A.D.C.)
and University Grant Commission (UGC) (fellowship to P.D.),
New Delhi is gratefully acknowledged. X-Ray and GCMS
studies were carried out at the National Single-Crystal X-ray
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Diffraction Facility and Sophisticated Analytical
Instrumentation Facilities (SAIF), IIT Bombay, respectively.
Computational facilities from the Department of Chemistry, IIT
Bombay are gratefully acknowledged. We thank Mr. Thomas
Scherer, Institut fur Anorganische Chemie, Universitat Stuttgart
for EPR measurement.
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