# Patent

## Title
Self-regenerating antioxidant catalysts and methods of using the same

## Abstract

The present invention relates to self-regenerating antioxidant catalysts and methods of using the same.

## Background
RELATED APPLICATION DATA
This application claims the benefit of U.S. Provisional Patent Application Ser. No. 62/085,862, filed Dec. 1, 2014, the disclosure of which is incorporated herein by reference in its entirety.


FIELD OF THE INVENTION
The present invention relates to self-regenerating antioxidant catalysts and methods of using the same.
BACKGROUND OF THE INVENTION
Artificial implant materials (AIMs) in contact with biological tissues induce the formation of reactive oxygen species (ROS), which then trigger an aseptic immune response (termed the foreign body reaction, FBR) that causes chemical and mechanical degradation of AIMs. Judicious selection of AIM type does not prevent this outcome, as even robust materials such as stainless steel and fluoropolymer plastics are attacked by corrosion and mechanical stress/strain forces. Immunosuppressive drugs protect AIMs against degradation by preventing the onset of FBR, but also impede essential healing processes and increase the risk of infection. Incorporating traditional organic antioxidants into AIMs enables them to halt or reduce ROS buildup and thus prevent FBR onset, but the prolonged nature of oxidative stress and the irreversible reactivity of traditional antioxidants with ROS eventually depletes the protective capacity.
SUMMARY OF THE INVENTION
A first aspect of the invention is a compound represented by one of the following structures:







wherein
each R is independently a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof;
X is a non-coordinating anion;
n is an integer from 1 to 30; and
m is an integer from 1 to 30;
and/or a derivative thereof.
A further aspect of the invention is a biomedical implant material comprising a compound and/or self-regenerating antioxidant catalyst of the present invention, wherein the compound is present on at least a portion of a surface of the biomedical implant material.
Another aspect of the invention is method of decreasing and/or preventing damage to a biomedical implant material, the method comprising providing the biomedical implant material, the biomedical implant material comprising a self-regenerating antioxidant catalyst of the present invention on at least a portion of a surface of the biomedical implant material, thereby decreasing and/or preventing damage to the biomedical implant material.
Another aspect of the invention is a compound represented by one of the following structures:




wherein each R independently is a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof. In some embodiments, R is hydrogen. In some embodiments, R is a substituted aryl group. In some embodiments, R is 3,5-dimethylphenyl or 4-methylphenyl.
A further aspect of the invention is a method of preparing a self-regenerating antioxidant catalyst of the present invention. In some embodiments, the method comprises preparing the self-regenerating antioxidant catalyst from a compound represented by one of the following structures:




wherein each R independently is a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof.



BRIEF DESCRIPTION OF THE FIGURES
FIG. 1 shows compounds analogous to [1H2][Br], 2 and Ru1 previously reported in the literature. Mes=2,4,6-trimethylphenyl; Dipp=2,6-diisopropylphenyl.
FIG. 2 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for [1H2][Br]. Hydrogen atoms and counterions have been omitted for clarity. Selected distances (Å) and angles (°): N1-C1, 1.327(4); N2-C1, 1.328(4); O1-C17, 1.306(4); O2-C17, 1.199(4); N1-C1-N2, 110.3(3); C1-N1-C16-C17, 99.5(3); C1-N2-C8-C9, 44.0(4).
FIG. 3A shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for the dodecametallic cyclic structure of 2. All atoms not in the Ag12 ring have been omitted for clarity.
FIG. 3B shows a simplified representation of Ag—NHC connectivity for the dodecametallic cyclic structure of 2.
FIG. 4 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for 2Ag1. Hydrogen atoms and solvent molecules have been omitted for clarity. Selected distances (Å) and angles (°): Ag1-C1, 2.038(11); Ag1-O3, 2.111(8); Ag2-O1, 2.094(9); N1-C1, 1.363(15); N2-C1, 1.416(16); O1-C17, 1.324(17); O2-C17, 1.194(17); C1-Ag1-O3, 175.5(5); N1-C1-N2, 101.8(10); C1-N1-C16-C17, 106(2); C1-N2-C8-C9, 41(2).
FIG. 5 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for 2Ag2. Hydrogen atoms and solvent molecules have been omitted for clarity. Selected distances (Å) and angles (°): Ag2 . . . Ag3, 2.967(2); Ag2-C20, 2.120(14); Ag2-O1, 2.094(9); Ag2-O10, 2.702(2); Ag3-C35, 2.097(14); Ag3-O9, 2.125(9); N4-aryl(centroid)-Ag3-NHC(centroid), 3.989; N3-C20, 1.309(16); N4-C20, 1.317(15); N5-C35, 1.404(18); N6-C35, 1.366(16); O5-C34, 1.271(17); O6-C34, 1.330(19); O7-C49, 1.259(16); O8-C49, 1.219(15); N3-C20-N4, 106.6(12); N5-C35-N6, 107.5(12); O1-Ag2-C20, 165.8(5); O10-Ag2-C20, 109.3(5); O9-Ag3-C35, 165.4(5); C20-Ag2-Ag3-C35, 75.4(6); C20-N3-C33-C34, 98(2); C20-N4-C27-C32, 37(2); C35-N5-C48-C49, 114(2); O9-Ag3-Ag2-O10, 4.0(4).
FIG. 6 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for Ru1. Hydrogen atoms and solvent molecules have been omitted for clarity. Selected distances (Å) and angles (°): Ru1-C1, 2.020(5); Ru-cymene(centroid), 1.696; Ru1-C11, 2.4152(15); Ru1-O1, 2.111(4); N1-C1, 1.363(6); N2-C1, 1.369(7); O1-C17, 1.281(7); O2-C17, 1.235(7); C1-Ru1-C11, 90.65(14); C1-Ru1-O1, 84.49(18); C11-Ru1-O1, 83.06(11); N1-C1-N2, 105.1(4); C1-N1-C16-C17, 45.7(7); C1-N2-C8-C9, 104.7(7).
FIG. 7 shows examples of NHC-supported cymene-Ru transfer hydrogenation catalysts. R=iPr or sBu.
FIG. 8 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for 2. Hydrogen atoms, solvent molecules and N-aryl substituents have been omitted for clarity. Selected distances (Å) and angles (°): Ru1-O1, 2.111(5); R1-O3, 2.113(4); Ru1-N5, 2.008(5); Ru1-N6, 2.021(5); Ru1-C1, 2.057(7); Ru1-C18, 2.062(7); O1-Ru1-O3, 90.48(19); N5-Ru1-N6, 80.3(2); O1-Ru1-C1, 84.6(2); O3-Ru1-C18, 85.8(2); C1-Ru1-C18, 166.1(3).
FIG. 9 shows an ORTEP diagram rendered using the POV-Ray engine, shown with 50% probability thermal ellipsoids and selected atom labels for 5. Hydrogen atoms, solvent molecules, counterions and N-aryl substituents have been omitted for clarity. Selected distances (Å) and angles (°): Ru1-O1, 2.139(5); R1-O3, 2.141(4); Ru1-N5, 2.011(5); Ru1-N6, 2.017(5); Ru1-C1, 2.089(6); Ru1-C19, 2.052(6); O1-Ru1-O3, 86.47(18); N5-Ru1-N6, 79.2(2); O1-Ru1-C1, 86.4(2); O3-Ru1-C19, 85.3(2); C1-Ru1-C19, 171.6(2).
FIG. 10A shows a cyclic voltammogram of 2 (black line) and 5 (grey line) in CH2Cl2 containing 1.0 mM analyte and 0.10 M [Bu4N][PF6] at 100 mV s−1 scan-rate.
FIG. 10B shows a cyclic voltammogram of 4 (black line) and 6 (grey line) in CH2Cl2 containing 1.0 mM analyte and 0.10 M [Bu4N][PF6] at 100 mV s−1 scan-rate.
FIG. 11A shows UV-visible spectra of 2 (black line) and 5 (grey line) in CH2Cl2 containing 1.0 mM analyte and 0.10 M [Bu4N][PF6] at 100 mV s−1 scan-rate.
FIG. 11B shows UV-visible spectra of 4 (black line) and 6 (grey line) in CH2Cl2 containing 1.0 mM analyte and 0.10 M [Bu4N][PF6] at 100 mV s−1 scan-rate.
FIG. 12A shows a graph of ABTS•− reduction after adding 5 μM Ru1 (black line) or 5 μM Trolox (straight black line), vs. initial ABTS•− absorbance (dashed grey line).
FIG. 12B shows a graph of ABTS•− reduction after adding 5 μM Ru1 (black line) then 5 additional 50 μM ABTS•− aliquots (*, grey line). Conditions: [ABTS•−]0=50 μM in EtOH at 25° C.; absorbance measured at 750 nm.
FIG. 12C shows a graph of ABTS•− reduction after adding 5 μM Trolox (black line) then 5 additional 10 μM ABTS•− aliquots (*, grey line). Conditions: [ABTS•−]0=50 μM in EtOH at 25° C.; absorbance measured at 750 nm.
FIG. 13 shows a graph illustrating the catalytic reduction of ABTS•− by Ru1 in PBS. (i) By itself, ABTS•− is stable in PBS. (ii) Addition of Ru1 from a CH3CN stock solution did not cause ABTS•− degradation. (iii) Subsequent addition of EtOH caused the absorbance to decrease, which indicated that EtOH functioned as a terminal reductant. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, 50 mM EtOH, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm.
FIG. 14A shows a graph illustrating the dependence of initial rate (v0) of reduction of ABTS•− catalyzed by Ru1 on [ABTS•−]0=5, 10, 25, 50 or 75 μM. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 14B shows a graph illustrating the dependence of observed rate constant (kobs) for Ru1-catalyzed ABTS•− reduction on [ABTS2−]0=50, 100, 150 or 200 μM. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 14C shows a graph illustrating the dependence of observed rate constant (kobs) for Ru1-catalyzed ABTS•− reduction on [EtOH]0=10, 30, 50 or 70 mM. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 14D shows a graph illustrating the dependence of observed rate constant (kobs) for Ru1-catalyzed ABTS•− reduction on [Ru1]0=1, 2, 3, 4 or 5 μM. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 14E shows a graph illustrating the dependence of observed rate constant (kobs) for Ru1-catalyzed ABTS•− reduction on pH=7.4, 7.9, 8.4 or 8.9. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 14F shows a graph illustrating the dependence of observed rate constant (kobs) for Ru1-catalyzed ABTS•− reduction on T=15, 25, 35 or 45° C. Each data point (⋄) is the average of 4 experiments performed on 4 different days and the error bars represent the standard deviation. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, [EtOH]0=50 mM, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm (unless specified otherwise).
FIG. 15 shows a schematic of a proposed mechanism for Ru1-catalyzed conversion of ABTS•− to ABTS2− with EtOH as the terminal reductant. Text and arrows outside the cyclic scheme correspond to forward reactions (clockwise), whereas text and arrows inside the cyclic scheme correspond to reverse reactions (counter-clockwise). Each Kn corresponds to the equilibrium constant for step “n” (i.e., K1 for step 1, etc.).
FIG. 16 shows a graph from a terminal reductant assay for ABTS•− reduction by Ru1. For each experiment, a PBS solution containing 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS•− at 25° C. was treated with 50 mM of the terminal reductant candidate and the decay in absorbance at 734 nm was measured. Observed rate constants (kobs) were extracted from slope of the plot of ln(A/A0) vs. time for the first 60 s following addition of the alcohol or ether. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, 50 mM alcohol, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm.
FIG. 17 shows a graph illustrating the necessity of having a non-tertiary alcohol for the catalytic reduction of ABTS•− by Ru1 in PBS. (i) By itself, ABTS•− is stable in the presence of Ru1 in PBS. (ii) Addition of t-BuOH did not afford ABTS•− degradation. (iii) Subsequent addition of EtOH caused the absorbance to decrease, which indicated that the lack of reactivity observed with t-BuOH was not due to catalyst deactivation but rather the fact that t-BuOH was not a competent terminal reductant. Conditions: [Ru1]0=5 μM, [ABTS•−]0=50 μM, [ABTS2−]0=100 μM, 50 mM ROH, PBS (pH 7.4), 25° C.; absorbance measured at 734 nm.
FIG. 18A shows a graph of in situ oxidation of ABTS2− to ABTS•− via HRP and H2O2 in the presence of 5 μM Ru1 (grey line) or 5 μM Trolox (black line). Conditions: [ABTS2−]0=20 μM, [Ru1]0=5 μM, [HRP]0=10 μM, [H2O2]0=10 μM, 1% DMSO in PBS (pH 7.4) at 25° C.; absorbance measured at 734 nm.
FIG. 18B shows a graph of ABTS•− formation by HRP in the presence of 5 μM Ru1, followed by two additional aliquots of 10 μM H2O2(grey lines). Conditions: [ABTS2−]0=20 μM, [Ru1]0=5 μM, [HRP]0=10 nM, [H2O2]0=10 μM, 1% DMSO in PBS (pH 7.4) at 25° C.; absorbance measured at 734 nm.
FIG. 18C shows a graph of ABTS•− formation by HRP in the presence of 5 μM Ru1, followed by two additional aliquots of 10 μM chemically synthesized ABTS•− (grey lines). Conditions: [ABTS2−]0=20 μM, [Ru1]0=5 μM, [HRP]0=10 nM, [H2O2]0=10 μM, 1% DMSO in PBS (pH 7.4) at 25° C.; absorbance measured at 734 nm.
FIG. 19A shows the synthesis of Ru7-SiO2. Conditions: (i) 10 equiv. NaOH, MeOH, Δ, 16 h; (ii) 3 equiv. N,N′-dicyclohexyl-carbodiimide, 3 equiv. N-hydroxysuccinimide, CH2Cl2, r.t., 16 h, then 3 equiv. APTES, 3 equiv. Et3N, r.t., 16 h; (iii) SiO2, toluene, 50° C., 2 h, then r.t., 15 h; (iv) 2.2 equiv. R—C≡C—H, 10 mol % [Pd(PPh3)4], 5 mol % CuI, THF/Et3N, 90° C., 48 h; (v) 25 equiv. MMA, 1 mol % (PhCO2)2, THF, 50° C., 20 h.
FIG. 19B shows the synthesis of Ru9-PMMA. Conditions: (i) 10 equiv. NaOH, MeOH, Δ, 16 h; (ii) 3 equiv. N,N′-dicyclohexyl-carbodiimide, 3 equiv. N-hydroxysuccinimide, CH2Cl2, r.t., 16 h, then 3 equiv. APTES, 3 equiv. Et3N, r.t., 16 h; (iii) SiO2, toluene, 50° C., 2 h, then r.t., 15 h; (iv) 2.2 equiv. R—C≡C—H, 10 mol % [Pd(PPh3)4], 5 mol % CuI, THF/Et3N, 90° C., 48 h; (v) 25 equiv. MMA, 1 mol % (PhCO2)2, THF, 50° C., 20 h.
FIG. 19C shows the structure of the abbreviated structure for the ligand 1−.
FIG. 20 shows the synthesis of SRAC with C≡C—H and coupling to N3-functionalized AIM. Conditions: (i) same as for Ru7, (ii) 1:1 alkyne/azide, 10 mol % CuSO4.5H2O, 3 equiv. sodium ascorbate, r.t., 48 h.



DETAILED DESCRIPTION
The present invention will now be described more fully hereinafter. This invention may be embodied in different forms and should not be construed as limited to the embodiments set forth herein. Rather, these embodiments are provided so that this disclosure will be thorough and complete, and will fully convey the scope of the invention to those skilled in the art.
The terminology used in the description herein is for the purpose of describing particular embodiments only and is not intended to be limiting of the invention. As used in the description and the appended claims, the singular forms “a”, “an” and “the” are intended to include the plural forms as well, unless the context clearly indicates otherwise.
Unless otherwise defined, all terms (including technical and scientific terms) used herein have the same meaning as commonly understood by one of ordinary skill in the art to which this invention belongs. It will be further understood that terms, such as those defined in commonly used dictionaries, should be interpreted as having a meaning that is consistent with their meaning in the context of the present application and relevant art and should not be interpreted in an idealized or overly formal sense unless expressly so defined herein. The terminology used in the description herein is for the purpose of describing particular embodiments only and is not intended to be limiting of the invention.
All patents, patent applications and publications referred to herein are incorporated by reference in their entirety. In case of a conflict in terminology, the present specification is controlling.
Also as used herein, “and/or” refers to and encompasses any and all possible combinations of one or more of the associated listed items, as well as the lack of combinations when interpreted in the alternative (“or”).
Unless the context indicates otherwise, it is specifically intended that the various features of the embodiments of the invention described herein may be used in any combination. For example, features described in relation to one embodiment may also be applicable to and combinable with other embodiments and aspects of the invention.
Moreover, the embodiments of the present invention also contemplate that in some embodiments, any feature or combination of features set forth herein may be excluded or omitted. To illustrate, if the specification states that a complex comprises components A, B and C, in some embodiments, any of A, B or C, or a combination thereof, may be omitted and disclaimed.
As used herein, the transitional phrase “consisting essentially of” (and grammatical variants) is to be interpreted as encompassing the recited materials or steps “and those that do not materially affect the basic and novel characteristic(s)” of the claimed invention. See, In re Herz, 537 F.2d 549, 551-52, 190 U.S.P.Q. 461, 463 (CCPA 1976) (emphasis in the original); see also MPEP §2111.03. Thus, the term “consisting essentially of” as used herein should not be interpreted as equivalent to “comprising.”
The term “about,” as used herein when referring to a measurable value such as an amount or concentration (e.g., the amount of a self-regenerating antioxidant catalyst) and the like, is meant to encompass variations of ±10%, ±5%, ±1%, ±0.5%, or even ±0.1% of the specified amount.
“Substituted” as used herein to describe chemical structures, groups, or moieties, refers to the structure, group, or moiety comprising one or more substituents. As used herein, in cases in which a first group is “substituted with” a second group, the second group is attached to the first group whereby a moiety of the first group (typically a hydrogen) is replaced by the second group. The substituted group may contain one or more substituents that may be the same or different.
“Substituent” as used herein references a group that replaces another group in a chemical structure. Typical substituents include nonhydrogen atoms (e.g., halogens), functional groups (such as, but not limited to, amino, sulfhydryl, carbonyl, hydroxyl, alkoxy, carboxyl, silyl, silyloxy, phosphate and the like), hydrocarbyl groups, and hydrocarbyl groups substituted with one or more heteroatoms. Exemplary substituents include, but are not limited to, alkyl, lower alkyl, halo, haloalkyl, alkenyl, alkynyl, cycloalkyl, cycloalkylalkyl, heterocyclo, heterocycloalkyl, aryl, arylalkyl, lower alkoxy, thioalkyl, hydroxyl, thio, mercapto, amino, imino, halo, cyano, nitro, nitroso, azido, carboxy, sulfide, sulfone, sulfoxy, phosphoryl, silyl, silylalkyl, silyloxy, boronyl, and modified lower alkyl.
“Alkyl” as used herein alone or as part of another group, refers to a straight (i.e., unbranched), branched, or cyclic hydrocarbon chain containing from 1 to 30 carbon atoms that is completely saturated. In some embodiments, the alkyl group may contain 1, 2, or 3 up to 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28, 29, or 30 carbon atoms. In some embodiments, the term “alkyl” or “alkyl group” refers to a cycloalkyl group, also known as carbocycle. Representative examples of alkyl include, but are not limited to, methyl, ethyl, n-propyl, iso-propyl, n-butyl, sec-butyl, iso-butyl, tert-butyl, n-pentyl, isopentyl, neopentyl, n-hexyl, 3-methylhexyl, 2,2-dimethylpentyl, 2,3-dimethylpentyl, n-heptyl, n-octyl, n-nonyl, n-decyl, cyclopropyl, cyclohexyl and the like. “Lower alkyl” as used herein, is a subset of alkyl and refers to a straight or branched chain hydrocarbon group containing from 1 to 4 carbon atoms. Representative examples of lower alkyl include, but are not limited to, methyl, ethyl, n-propyl, iso-propyl, n-butyl, iso-butyl, tert-butyl, and the like. The term “alkyl” or “loweralkyl” is intended to include both substituted and unsubstituted alkyl or loweralkyl unless otherwise indicated and these groups may be substituted with groups such as, but not limited to, polyalkylene oxides (such as PEG), halo (e.g., haloalkyl), alkyl, haloalkyl, alkenyl, alkynyl, cycloalkyl, cycloalkylalkyl, aryl, arylalkyl, heterocyclo, heterocycloalkyl, hydroxyl, alkoxy (thereby creating a polyalkoxy such as polyethylene glycol), alkenyloxy, alkynyloxy, haloalkoxy, cycloalkoxy, cycloalkylalkyloxy, aryloxy, arylalkyloxy, heterocyclooxy, heterocyclolalkyloxy, mercapto, alkyl-S(O)m, haloalkyl-S(O)m, alkenyl-S(O)m, alkynyl-S(O)m, cycloalkyl-S(O)m, cycloalkylalkyl-S(O)m, aryl-S(O)m, arylalkyl-S(O)m, heterocyclo-S(O)m, heterocycloalkyl-S(O)m, amino, carboxy, alkylamino, alkenylamino, alkynylamino, haloalkylamino, cycloalkylamino, cycloalkylalkylamino, arylamino, arylalkylamino, heterocycloamino, heterocycloalkylamino, disubstituted-amino, acylamino, acyloxy, ester, amide, sulfonamide, urea, alkoxyacylamino, aminoacyloxy, nitro or cyano, where m=0, 1, 2 or 3.
“Alkenyl” as used herein alone or as part of another group, refers to a straight (i.e., unbranched), branched, or cyclic hydrocarbon chain containing from 1 to 30 carbon atoms (or in loweralkenyl 1 to 4 carbon atoms) and has one or more double bonds (e.g., 1 to 10 double bonds in the hydrocarbon chain). In some embodiments, the alkenyl group may contain 1, 2, or 3 up to 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28, 29, or 30 carbon atoms. According to another aspect, the term alkenyl refers to a straight chain hydrocarbon having two double bonds, also referred to as “diene.” In some embodiments, the term “alkenyl” or “alkenyl group” refers to a cycloalkenyl group. Representative examples of alkenyl include, but are not limited to, methylene (═CH2), vinyl (—CH═CH2), allyl (—CH2CH═CH2), 2-butenyl, 3-butenyl, 4-pentenyl, 3-pentenyl, 2-hexenyl, 3-hexenyl, 2,4-heptadiene, cyclobutenyl, and the like. The term “alkenyl” or “loweralkenyl” is intended to include both substituted and unsubstituted alkenyl or loweralkenyl unless otherwise indicated and these groups may be substituted with groups such as those described in connection with alkyl and loweralkyl above.
“Alkynyl” as used herein alone or as part of another group, refers to a straight or branched chain hydrocarbon containing from 1 to 30 carbon atoms (or in loweralkynyl 1 to 4 carbon atoms) which include at least one triple bond in the hydrocarbon chain. In some embodiments, the alkynyl group may contain 2, or 3 up to 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28, 29, or 30 carbon atoms. Representative examples of alkynyl include, but are not limited to, 2-propynyl, 3-butynyl, 2-butynyl, 4-pentynyl, 3-pentynyl, and the like. The term “alkynyl” or “loweralkynyl” is intended to include both substituted and unsubstituted alkynyl or loweralkynyl unless otherwise indicated and these groups may be substituted with the same groups as set forth in connection with alkyl and loweralkyl above.
“Aryl” as used herein alone or as part of another group, refers to a monocyclic carbocyclic ring system or a bicyclic carbocyclic fused ring system or higher having one or more aromatic rings. Representative examples of aryl include, azulenyl, indanyl, indenyl, naphthyl, phenyl, tetrahydronaphthyl, and the like. The term “aryl” is intended to include both substituted and unsubstituted aryl unless otherwise indicated and these groups may be substituted with the same groups as set forth in connection with alkyl and loweralkyl above.
“Arylalkyl” as used herein alone or as part of another group, refers to an aryl group, as defined herein, appended to the parent molecular moiety through an alkyl group, as defined herein. Representative examples of arylalkyl include, but are not limited to, benzyl, 2-phenylethyl, 3-phenylpropyl, 2-naphth-2-ylethyl, and the like.
“Heterocycle” refers to a cyclic moiety having one or more closed rings with one or more heteroatoms (for example, oxygen, nitrogen or sulfur) in at least one of the rings, wherein the ring or rings may independently be fused, and/or bridged. In some embodiments, a heterocycle may be a heteroaryl. “Heteroaryl” refers to a cyclic moiety having one or more closed rings with one or more heteroatoms (for example, oxygen, nitrogen or sulfur) in at least one of the rings, wherein at least one of the rings is aromatic, and wherein the ring or rings may independently be fused, and/or bridged. Examples include without limitation phenyl, thiophenyl, triazolyl, pyridinyl, pyrimidinyl, pyridazinyl, pyrazinyl, quinolinyl, isoquinolinyl, indolyl, furyl, thienyl, pyrazolyl, quinoxalinyl, pyrrolyl, indazolyl, thieno[2,3-c]pyrazolyl, benzofuryl, pyrazolo[1,5-a]pyridyl, thiophenylpyrazolyl, benzothienyl, benzothiazolyl, thiazolyl, 2-phenylthiazolyl, and isoxazolyl.
“Halogen” or “halo” as used herein refer to fluoro, chloro, bromo or iodo.
An “amine” as used herein refers to an organic compound having a basic nitrogen atom (R—NR′R′′), and may be a primary (R—NH2), secondary (R—NHR′) or tertiary (R—NR′R′′) amine.
The term “carbonyl” refers to a —(C═O)— group.
The term “azide” refers to a —N3 group.
Provided according to embodiments of the present invention are self-regenerating antioxidant catalysts. “Self-regenerating” as used herein refers to a self-regenerating antioxidant catalyst's ability to be regenerated as an integral consequence of performing a reaction (e.g., without requiring a subsequent reaction in order to regenerate), such as, e.g., a degradation reaction, and used in a subsequent reaction (e.g., a degradation reaction). Thus, “self-regenerating” as used herein refers to the ability of a self-regenerating antioxidant catalyst to return to a state in which it can be reused in another reaction.
In some embodiments, the self-regenerating antioxidant catalyst may be stable in that a metal present in the self-regenerating antioxidant catalyst is not removed in the presence of a chelating molecule that may cause demetallation (e.g., such as ones that may be present in a biological system in which the self-regenerating antioxidant catalyst is present). The self-regenerating antioxidant catalyst may be stable and thus retain its activity. In some embodiments, the self-regenerating antioxidant catalyst may retain at least 50%, 55%, 60%, 65%, 70%, 75%, 80%, 85%, 90%, 95%, or 100% of its activity after at least 1, 2, 3, 4, 5, or 6 day(s), or 1, 2, 3, or 4 week(s), or 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12 or more month(s).
A self-regenerating antioxidant catalyst of the present invention may degrade, such as, for example, reduce, a radical catalytically. The radical may be an oxidizing radical (e.g., a compound that includes an unpaired electron). In some embodiments, the self-regenerating antioxidant catalyst reduces oxidizing radicals catalytically. In some embodiments, the self-regenerating antioxidant catalyst may be regenerated after a radical degradation reaction.
A self-regenerating antioxidant catalyst of the present invention may degrade (e.g., reduce) reactive oxygen species (ROS). “Reactive oxygen species” or “ROS” as used herein refer to oxygen containing compounds that can cause oxidation of another molecule. In some embodiments, a ROS may trigger an aseptic immune response and/or a foreign body reaction (FBR). “Oxidizing radicals” as used herein refer to compounds with unpaired electrons that can cause oxidation of another molecule. Although there is overlap between ROS and oxidizing radicals, the former may not necessarily contain unpaired electrons (e.g., ONOO−) and the latter may not necessarily contain oxygen (e.g., thiyl radicals). In some embodiments, the self-regenerating antioxidant catalyst may catalytically degrade a ROS and/or radical under physiologically relevant conditions, such as, for example, at physiological pH, a pH in a range of about 6 to about 8, and/or when in contact with a biological subject (e.g., when in, on, and/or in contact with a biological tissue and/or fluid)
In some embodiments, a self-regenerating antioxidant catalyst of the present invention may catalytically degrade a ROS and/or radical and after one or more degradation reaction(s) the self-regenerating antioxidant catalyst may be regenerated. In some embodiments, the self-regenerating antioxidant catalyst may be regenerated 2, 5, 10, 20, 30, 40, 50, 60, 70, 80, 90, 100, 150, 200, 250, 300, or more times. Some embodiments include that the self-regenerating antioxidant catalyst may be regenerated after 1, 2, 5, 10, 20, 30, 40, 50, 60, 70, 80, 90, 100, 150, 200, or more degradation reaction(s) (e.g., after 1 or more reaction(s) in which the self-regenerating antioxidant catalytically degrades a radical and/or ROS). In some embodiments, the self-regenerating antioxidant catalyst may provide at least tens or hundreds of turnovers or regeneratiions of the self-regenerating antioxidant catalyst compared to a stoichiometric antioxidant reaction. The self-regenerating antioxidant catalyst may provide greater protection against radicals and/or ROS to a material (e.g., an artificial implant material) in which the self-regenerating antioxidant catalyst is present on, in, and/or adjacent to. The self-regenerating antioxidant catalyst may catalytically degrade a ROS and/or radical under aerobic conditions and/or under conditions in which oxygen may or may not be present.
In some embodiments, a self-regenerating antioxidant catalyst of the present invention may slow the formation of a ROS and/or radical. The self-regenerating antioxidant catalyst may slow the formation of a ROS and/or radical under aerobic conditions and/or under conditions in which oxygen may or may not be present. The self-regenerating antioxidant catalyst may slow the formation of the ROS and/or radical under physiologically relevant conditions. In some embodiments, a self-regenerating antioxidant catalyst of the present invention may catalyze the degradation and/or slow the formation of radicals and/or ROS in aqueous buffer at physiologically-relevant pH (e.g., at a pH in a range of about 6 to about 8, about 7 to about 8, or at a pH of about 7.4). Some embodiments include that a self-regenerating antioxidant catalyst of the present invention may reduce or slow the formation of a radical and/or ROS by at least 10%, 20%, 30%, 40%, 50%, 60%, 70%, 80%, 90%, 100%, 150%, 200%, or more compared to the rate of formation of radicals and/or ROS in the absence of the self-regenerating antioxidant catalyst.
In some embodiments, a self-regenerating antioxidant catalyst of the present invention may reduce and/or prevent material damage by a ROS and/or radical. The self-regenerating antioxidant catalyst may reduce and/or prevent material damage by the ROS and/or radical under physiologically relevant conditions. The self-regenerating antioxidant catalyst may reduce and/or prevent material damage by the ROS and/or radical under aerobic conditions and/or under conditions in which oxygen may or may not be present. In some embodiments, a self-regenerating antioxidant catalyst of the present invention may reduce and/or prevent material damage by radicals and/or ROS in aqueous buffer, which may be at a physiologically-relevant pH. Some embodiments include that a self-regenerating antioxidant catalyst of the present invention may reduce and/or prevent material damage by a ROS and/or radical by at least 10%, 20%, 30%, 40%, 50%, 60%, 70%, 80%, 90%, 100%, 150%, 200%, or more compared to the amount and/or rate of material damage by radicals and/or ROS in the absence of the self-regenerating antioxidant catalyst.
In some embodiments, the self-regenerating antioxidant catalyst may be attached to an implant material and/or may catalytically reduce oxidative stress in tissue(s) (e.g., biological tissue(s)) in contact with and/or adjacent to the self-regenerating antioxidant catalyst and/or implant material. The self-regenerating antioxidant catalyst and/or implant material may reduce and/or prevent artificial implant failure caused by FBR. In some embodiments, the self-regenerating antioxidant catalyst may reduce and/or prevent immune response-mediated material degradation and/or loss of function. Chemical and/or mechanical degradation of a material (e.g., an artificial implant material) in which the self-regenerating antioxidant catalyst is in, on, and/or adjacent to may be reduced and/or prevented. In some embodiments, the self-regenerating antioxidant catalyst may reduce and/or prevent corrosion and/or mechanical stress/strain forces in a material in which the self-regenerating antioxidant catalyst is in, on, and/or adjacent to.
In some embodiments, the self-regenerating antioxidant catalyst may be integrated (e.g., covalently integrated) into a polymer, such as, e.g., an organic polymer, that retains the catalytic activity of the self-regenerating antioxidant catalyst. For example, the self-regenerating antioxidant catalyst may be integrated (e.g., covalently integrated) into a polymer, such as, but not limited to, polyethylene, polypropylene, poly(methyl methacrylate), poly(dimethyl siloxane), and any combination thereof.
According to some embodiments of the present invention, the self-regenerating antioxidant catalyst comprises a benzimidazole and/or a derivative thereof. A “derivative” as used herein refers to a compound and/or group that has a common structure with the compound referred to (e.g., a parent compound and/or group), but is substituted with one or more substituents. For example, a self-regenerating antioxidant catalyst may comprise and/or be derived from a benzimidazole, but the benzimidazole of the self-regenerating antioxidant catalyst may be substituted with one or more substituents, such as, e.g., shown in Ru1 and Ru2. In some embodiments, the self-regenerating antioxidant catalyst comprises a chelating, anionic benzimidazole-based N-heterocyclic carbene (NHC) ligand. In some embodiments, the self-regenerating antioxidant catalyst comprises a bipyridine, a phosphine, an amine and/or a derivative thereof. In some embodiments, the self-regenerating antioxidant catalyst may comprise ruthenium (e.g., Ru(II)) and/or a ruthenium complex.
In some embodiments, a self-regenerating antioxidant catalyst of the present invention may include a substituent that allows and/or provides for the attachment (e.g., covalent attachment) of the self-regenerating antioxidant catalyst to an implant material (e.g., an artificial and/or biological implant material). Example substituents that may be used to attach a self-regenerating antioxidant catalyst to an implant material include, but are not limited to, methacrylamide, diethylphosphonate, and/or derivatives thereof. In some embodiments, a self-regenerating antioxidant catalyst may be attached (e.g., covalently attached) to (e.g., into and/or onto) an organic and/or inorganic material. Example materials include, but are not limited to, poly(methyl methacrylate) (PMMA) (e.g. a PMMA films) or TiO2 (e.g., a TiO2 nanoparticles).
The self-regenerating antioxidant catalyst may have a structure represented by one of the following structures:







wherein
each R is independently a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof;
X is a non-coordinating anion;
n is an integer from 1 to 30; and
m is an integer from 1 to 30;
and/or a derivative thereof.
In some embodiments, each R is hydrogen. In some embodiments, at least one R is a substituted or unsubstituted alkyl group or a substituted or unsubstituted aryl group. In some embodiments, “n” and/or “m” may each independently be any integer from 1 to 30, such as 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17, 18, 19, 20, 21, 22, 23, 24, 25, 26, 27, 28, 29, or 30.
Example non-coordinating anions include, but are not limited to, tetrafluoroborate, hexafluorophosphate, tetraphenylborate, triflate, triflamide, methylsulfate, and any combination thereof.
In some embodiments, the self-regenerating antioxidant catalyst may retain the ability to degrade (e.g., reduce) radicals and/or ROS catalytically for a period of time. The self-regenerating antioxidant catalyst may retain the ability to degrade radicals and/or ROS catalytically for a given period of time, such as, e.g., 1, 2, 3, 4, 5, or 6 days, or 1, 2, 3, 3, 4, 5, or more weeks in aerobic, buffered (e.g., at a pH in a range of about 6 to about 8) aqueous solutions and/or under physiologically relevant conditions (e.g., at a pH in a range of about 6 to about 8). In some embodiments, the self-regenerating antioxidant catalyst may retain the ability to degrade radicals and/or ROS catalytically for at least 2 weeks in aerobic, buffered aqueous solutions and/or under physiologically relevant conditions.
In some embodiments, the self-regenerating antioxidant catalyst may utilize non-tertiary alcohols present in the environment in which the self-regenerating antioxidant catalyst is present, such as, for example, a biological system, to degrade radicals and/or ROS catalytically. In some embodiments, the self-regenerating antioxidant catalyst may use a sugar present in the environment in which the self-regenerating antioxidant catalyst is present, such as, for example, a biological system, to degrade radicals and/or ROS catalytically. In some embodiments, the self-regenerating antioxidant catalyst may utilize an oxidizing radical, such as, but not limited to hydrogen peroxide, present in the environment in which the self-regenerating antioxidant catalyst is present, such as, for example, a biological system, to degrade radicals (including the oxidizing radical, e.g., hydrogen peroxide) and/or ROS catalytically.
The self-regenerating antioxidant catalyst may be in, on, and/or in contact with at least a portion of a subject and/or a biological system. In some embodiments, the self-regenerating antioxidant catalyst may be in contact with a biological tissue and/or a biological fluid, such as, but not limited to, extracellular fluid, blood, lymph, pus, exudate, aqueous humour, vitreous humour, saliva, sweat, urine, etc. of a subject. Subjects suitable that may be in contact with a self-regenerating antioxidant catalyst of the present invention and/or treated with a method of the present invention include, but are not limited to, avian and mammalian subjects. Mammals of the present invention include, but are not limited to, canines, felines, bovines, caprines, equines, ovines, porcines, rodents (e.g. rats and mice), lagomorphs, primates, humans, and the like, and mammals in utero. Any mammalian subject in need of being treated according to the present invention is suitable. Human subjects of both genders and at any stage of development (i.e., neonate, infant, juvenile, adolescent, adult) may be treated according to the present invention. The invention may also be carried out on animal subjects, particularly mammalian subjects such as mice, rats, dogs, cats, livestock and horses for veterinary purposes, and for development purposes.
The self-regenerating antioxidant catalyst may be non-cytotoxic. In some embodiments, the self-regenerating antioxidant catalyst may be present in, on, and/or in contact with at least a portion of a material, subject and/or biological system in a therapeutically effective amount. In some embodiments, the therapeutically effective amount for a self-regenerating antioxidant catalyst of the present invention may be about 0.1 μM, 0.5 μM, 1 μM, 5 μM, 10 μM, 25 μM, 50 μM, 100 μM, 150 μM, 200 μM or more. The self-regenerating antioxidant catalyst may be present in a non-cytotoxic amount and/or at a concentration in a range of about 0.5 μM to about 100 μM and/or any range therein. In some embodiments, the therapeutically effective amount for a self-regenerating antioxidant catalyst of the present invention may be at least about 100 μM, such as, for example, for Ru1.
As used herein, the term “therapeutically effective amount” refers to an amount of a self-regenerating antioxidant catalyst of the present invention that elicits a therapeutically useful response in a subject and/or with regard to a material. Those skilled in the art will appreciate that the therapeutic effects need not be complete or curative, as long as some benefit is provided to the subject and/or material. In particular embodiments of the present invention, a therapeutically effective amount of a self-regenerating antioxidant catalyst results in the catalytic degradation of a ROS and/or radical, reduction in the rate of formation of a ROS and/or radical, and/or the reduction and/or prevention of material damage by a ROS and/or radical.
A self-regenerating antioxidant catalyst of the present invention may be attached to, such as, for example, covalently attached, to an implant material, such as, for example, an artificial and/or biomedical implant material. A surface (e.g., interior and/or exterior) of an implant material to which a self-regenerating antioxidant catalyst of the present invention may be attached include, but are not limited to, a metal, such as, for example, stainless steel, titanium, etc.; a polymer and/or plastic, such as, for example, fluoropolymer plastics, polyethylene, polypropylene, poly(methyl methacrylate), etc.; silicon dioxide; titanium dioxide; and any combination thereof. In some embodiments, the self-regenerating antioxidant catalyst may be attached to an existing, FDA-approved biomedical implant material. In some embodiments, the biomedical implant material may be functionalized with the self-regenerating antioxidant catalyst, thereby attaching the self-regenerating antioxidant catalyst to the biomedical implant material.
In some embodiments, a self-regenerating antioxidant catalyst of the present invention may be prepared from a compound represented by one of the following structures:




wherein each R is independently a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof.
In some embodiments, R is a substituted aryl group. In some embodiments, R is 3,5-dimethylphenyl or 4-methylphenyl.
According to some embodiments of the present invention, provided are methods of using a self-regenerating antioxidant catalyst of the present invention. In some embodiments, a method of decreasing and/or preventing damage to a material (e.g., an articifial and/or biomedical implant material) may be provided, the method comprising providing the material, the material comprising a self-regenerating antioxidant catalyst of the present invention on at least a portion of a surface of the material, thereby decreasing and/or preventing damage to the material. The self-regenerating antioxidant catalyst may be present on an interior and/or exterior surface of the material. In some embodiments, degradation of the material may be decreased and/or prevented. Some embodiments include that the self-regenerating antioxidant catalyst decreases and/or prevents damage to the material. In some embodiments, the self-regenerating antioxidant catalyst and/or method of decreasing and/or preventing damage to a material may decrease and/or prevent damage to the material when the material and/or self-regenerating antioxidant catalyst are exposed to and/or in contact with a biological system (e.g., when the material is implanted in a subject).
In some embodiments, a self-regenerating antioxidant catalyst and/or method of the present invention may reduce and/or prevent chemical and/or mechanical degradation of a material (e.g., an articifial and/or biomedical implant material). The self-regenerating antioxidant catalyst may reduce and/or prevent immune response-mediated material degradation in a biological system in which it is present. In some embodiments, the self-regenerating antioxidant catalyst may reduce and/or prevent loss of function of a material on which it is present.
The self-regenerating antioxidant catalyst may decrease the amount and/or rate of damage to a material by at least 5% or more, such as, for example, at least 10%, 15%, 20%, 25%, 30%, 35%, 40%, 45%, 50%, 55%, 60%, 65%, 70%, 75%, 80%, 85%, 90%, 95%, or 100% compared to a material without the self-regenerating antioxidant catalyst. In some embodiments, the self-regenerating antioxidant catalyst may decrease the amount and/or rate of damage to the implant material by at least 5% for a period of time of at least 1, 2, 3, 4, 5, 6 day(s), or 1, 2, 3, 4 or more week(s) compared to a material without the self-regenerating antioxidant catalyst under similar conditions.
In some embodiments, the self-regenerating antioxidant catalyst may decrease and/or prevent damage to a material (e.g., an articifial and/or biomedical implant material) by decreasing and/or preventing damage to the implant from oxidizing radicals, such as, for example, those produced by a sterile immune response and/or ROS. In some embodiments, the self-regenerating antioxidant may reduce and/or prevent the triggering of an immune response. The self-regenerating antioxidant catalyst may decrease the severity and/or duration of a sterile immune response. In some embodiments, the self-regenerating antioxidant catalyst may decrease and/or prevent triggering of a foreign body reaction. In some embodiments, the self-regenerating antioxidant catalyst may decrease and/or prevent severity and/or duration of the adverse effects of acute phase foreign body reaction.
The present invention is explained in greater detail in the following non-limiting Examples.
EXAMPLES
Example 1
A benzimidazolylidene with a chelating carboxylate side-chain (1−) was synthesized and its transition metal coordination chemistry and reactivity were studied (Scheme 1). To construct the framework for a chelating, anionic benzimidazole-based N-heterocyclic carbene (NHC) ligand (1−), N-(3,5-dimethylphenyl)benzimidazole was reacted with 2-bromoacetic acid to yield the corresponding benzimidazolium [1H2][Br]. Double deprotonation followed by metallation of [1H2][Br] with Ag2O produced the Ag—NHC complex [Ag(1)]n (2), which exhibited good solubility in organic solvents despite its multinuclear nature. Crystallographic analysis of 2 revealed a dodecametallic structure (n=12) comprising mononuclear [Ag(1)] and dinuclear [Ag2(1)2] subunits, the latter of which featured Ag—Ag bonds. Transmetallation of 1− from Ag to Ru via the reaction of [RuCl(η6-cymene)(μ-Cl)]2 with 2 afforded the Ru—NHC complex [RuCl(1)(η6-cymene)](Ru1), which demonstrated catalytic activity for transfer hydrogenation of C═O, C═N and C═C bonds using isopropanol as the H2 source.




Experimental:

Materials and Methods

N-(3,5-dimethylphenyl)benzimidazole was prepared as previously described (Hanan, et al., Lyssikatos, Synlett (2010) 2759). All other materials and solvents were of reagent quality and used as received. 1H and 13C{1H}NMR spectra were recorded using a Bruker 500 MHz spectrometer. Chemical shifts δ (in ppm) for 1H and 13C NMR are referenced to SiMe4 using the residual protio-solvent as an internal standard. For 1H NMR: CDCl3, 7.26 ppm; DMSO-d6, 2.50 ppm. For 13C NMR: CDCl3, 77.16 ppm; DMSO-d6, 39.52 ppm. Coupling constants (J) are expressed in hertz (Hz). Infrared spectra were recorded on a Thermo Nicolet IR200 spectrometer with 4 cm−1 resolution. Elemental analyses were performed at Atlantic Microlab, Inc. (Norcross, Ga.). All syntheses and purifications were performed under ambient conditions unless specified otherwise. Syntheses requiring an inert atmosphere were performed under an N2 atmosphere using standard Schlenk or glovebox techniques. When required, solvents were dried and deoxygenated using an Innovative Technologies solvent purification system, and then stored over molecular sieves (3 Å) in a drybox.
Crystal Structure Data Acquisition and Structure Determination
Single crystals of [1H2][Br] and Ru1 were immersed in Paratone-N oil at room temperature and mounted on glass fibers using epoxy glue. To protect crystals of 2 from rapid desolvation, those crystals were transferred from the solvent into cold, viscous Paratone-N oil, mounted on a glass fiber, and immediately cooled to 200 K under a stream of cold nitrogen. Intensity data on all crystals were collected under nitrogen at 200 K with Mo Kα radiation (λ=0.71073 Å) on a Rigaku AFC8S diffractometer equipped with a Mercury CCD area detector and controlled using the CrystalClear software package [23]. A crystal-to-detector distance of 27 mm was used for [1H2][Br] and Ru1, whereas the data collection for 2 required a crystal-to-detector distance of 42 mm accompanied by a detector swing of 12 degrees to resolve the diffraction profile and retain appropriate resolution limits. Data were corrected for absorption as well as Lorentz and polarization effects using the REQAB subroutine of CrystalClear [24]. The structures were solved by direct methods and subsequently refined using the SHELXTL software package [25] and checked for higher symmetry using the PLATON program suite [26]. All non-hydrogen atoms were refined anisotropically. Hydrogen atoms were placed at calculated positions using a riding model and assigned thermal parameters equal to either 1.5 (methyl hydrogen atoms) or 1.2 (non-methyl hydrogen atoms) times the thermal parameters of the atoms to which they were attached. For Ru1, a partially-occupied solvent molecule was identified from the difference electron density map and included in the refinement. In the case of 2, several solvent molecules could be identified from the difference map, and other highly disordered solvent molecules were modeled using the SQUEEZE tool of PLATON.
Syntheses
Synthesis of 2-(3-{3,5-dimethylphenyl}-benzimidazol-1-ium-1-yl)acetate hydrobromide [1H2][Br]
2-Bromoacetic acid (947 mg, 6.82 mmol) and N-(3,5-dimethylphenyl)benzimidazole (1.50 g, 6.75 mmol) were dissolved with 20 mL of toluene in a heavy-walled flask equipped with a stir bar. The flask was then sealed and the clear, dark orange-brown solution was heated to 110° C. After 16 h, a white precipitate had formed, at which point the reaction mixture was allowed to cool to room temperature and the precipitate was collected by filtration. The resulting solid was washed successively with Et2O, CH2Cl2 and acetone, and then dried in vacuo to afford 1.95 g (5.40 mmol, 80% yield) of the desired product as a white powder. 1H NMR (500 MHz, DMSO-d6): δ=13.93 (s, 1H), 10.25 (s, 1H), 8.19 (d, J=8.5, 1H), 7.91 (d, J=8.0, 1H), 7.81-7.71 (m, 2H), 7.50 (s, 2H), 7.36 (s, 1H), 5.60 (s, 2H), 2.43 (s, 6H). 13C NMR (125 MHz, DMSO-d6): δ 167.5, 143.3, 140.1, 132.8, 131.8, 131.5, 130.5, 127.4, 127.2, 122.4, 114.3, 113.7, 47.8, 20.7. IR (KBr): 3116 (w), 3024 (m), 2902 (m), 2761 (m), 2566 (w), 2511 (w), 2428 (w), 1742 (vs), 1731 (vs), 1620 (s), 1598 (m), 1557 (vs), 1487 (s), 1435 (m), 1401 (s), 1384 (s), 1366 (m), 1351 (m), 1326 (m), 1265 (m), 1232 (vs), 1221 (vs), 1202 (vs), 1149 (m), 1138 (w), 1030 (w), 999 (w), 879 (m), 856 (s), 779 (s), 746 (s), 692(s), 679 (m), 607 (m), 424 (w) cm−1. Anal. Calcd for C17H17BrN2O2: C, 56.52; H, 4.74; N, 7.75. Found: C, 56.62; H, 4.79; N, 7.67.
Synthesis of [Ag(1)]n (2)
To a solution of [1H2][Br](100 mg, 277 μmol) in anhydrous CH2Cl2 (10 mL) under nitrogen was added Ag2O (96.2 mg, 415 μmol), and the resulting white suspension was allowed to stir at room temperature in the absence of light. After 24 h, the reaction mixture was filtered through a 0.2 μm PTFE filter with the aid of CH2Cl2 (2 mL). The filtrate solvent was removed under reduced pressure and the resulting solids were then dried in vacuo to afford 104 mg (269 μmol, 97% yield) of the desired product as an off-white powder. 1H NMR (500 MHz, CDCl3): δ 7.52 (d, J=8.0, 1H), 7.37-7.32 (m, 2H), 7.31-7.27 (m, 1H), 7.21 (s, 2H), 7.10 (s, 1H), 5.17 (s, 2H), 2.39 (s, 6H). 13C NMR (125 MHz, CDCl3): δ 188.7, 171.9, 139.9, 138.1, 134.6, 134.5, 130.9, 124.3, 124.01, 123.99, 112.4, 112.1, 53.0, 21.4. IR (KBr): 3055 (m), 2976 (w), 2920 (m), 1614 (vs), 1483 (s), 1435 (m), 1383 (vs), 1308 (s), 1248 (m), 1184 (w), 1103 (vw), 1030 (w), 997 (vw), 914 (vw), 856 (m), 837 (w), 748 (s), 652 (m), 625 (m), 550 (vw), 432 (vw) cm−1. Anal. Calcd for C17H16N2O2.5Ag (2.0.5H2O): C, 51.54; H, 4.07; N, 7.07. Found: C, 51.86; H, 4.00; N, 7.05.
Synthesis of [RuCl(1) (η6-cymene)](Ru1)
To a stirred solution of 2 (100 mg, 258 μmol) in anhydrous CH2Cl2 (10 mL) under nitrogen was added [RuCl(η6-cymene)(μ-Cl)]2 (79.1 mg, 258 μmol) dissolved in 10 mL of CH2Cl2. During the course of the addition, the mixture changed first to a clear red and then to a clear orange solution with concomitant formation of a white precipitate, and the reaction was allowed to stir at room temperature. After 24 h, the reaction mixture was filtered through a 0.2 μm PTFE filter (to remove AgCl) with the aid of CH2Cl2 (4 mL). The filtrate solvent was removed under reduced pressure and the resulting solids were then dried in vacuo to afford 138 mg (251 μmol, 97% yield) of the desired product as a light red-orange powder. 1H NMR (500 MHz, CDCl3): δ 7.65 (s, 1H), 7.37-7.32 (m, 2H), 7.27-7.23 (m, 3H), 7.08 (d, J=8.0, 1H), 5.49 (d, J=6.0, 1H), 5.18 (d, J=6.0, 1H), 5.10 (d, J=6.0, 1H), 4.90 (d, J=16.5, 1H), 4.71 (d, J=17.0, 1H), 3.84 (d, J=5.5, 1H), 2.62 (sep, 1H), 2.51 (s, 3H), 2.42 (s, 3H), 2.01 (s, 3H), 1.11 (d, J=10.8, 3H), 1.09 (d, J=10.8, 3H). 13C NMR (125 MHz, CDCl3): δ 186.0, 169.3, 140.6, 139.2, 138.6, 136.6, 134.0, 131.5, 128.9, 125.1, 124.2, 124.1, 111.4, 110.2, 104.0, 102.1, 90.5, 90.3, 83.3, 80.8, 49.9, 30.8, 23.3, 21.9, 21.4, 21.3, 18.9. IR (KBr): 3049 (w), 3026 (vw), 2961 (w), 2923 (w), 2871 (w), 1634 (vs), 1506 (vw), 1483 (w), 1470 (w), 1450 (m), 1395 (s), 1359 (m), 1306 (w), 1252 (w), 1205 (w), 944 (vw), 866 (w), 758 (m), 733 (w), 700 (w), 675 (vw), 634 (vw), 559 (vw), 436 (vw) cm−1. Anal. Calcd for C27H29ClN2O2Ru: C, 58.96; H, 5.31; N, 5.09. Found: C, 58.77; H, 5.40; N, 5.02.
General Procedure for Transfer Hydrogenation Experiments
Unsaturated substrate (0.91 mmol), base (46 μmol) and Ru1 (9.1 μmol) were dissolved in dry iPrOH under nitrogen and the resulting solution was heated to 83° C. After 24 h, the reaction mixture was allowed to cool to room temperature, diluted with 20 mL of CH2Cl2, washed with water (3×20 mL), dried with Na2SO4, and the solvent was removed under reduced pressure. This crude material was then purified via flash column chromatography (SiO2, CH2Cl2). Product identity was confirmed by 1H NMR analysis. Reported yields are averages of two or more runs.
Results and Discussion:
Synthesis
3,5-dimethylphenyl was selected as a suitable benzimidazole N-substituent given its 1H NMR spectroscopic features: singlets for both alkyl and aryl protons, and the two methyl groups would readily reveal diastereotopic inequivalence within metal complexes. As the first step towards a carboxylate-functionalized NHC ligand, alkylation of the benzimidazole scaffold with ω-haloalkanoic acid, was pursued given that this reactivity has been demonstrated for N-substituted imidazoles [17c, 27]. Nucleophilic substitution of 2-bromoacetic acid by N-(3,5-dimethylphenyl)benzimidazole in toluene at 110° C. produced the benzimidazolium carboxylic acid [1H2][Br] as an air- and moisture-stable white powder in 80% yield (Scheme 2). Although benzimidazole protonation could be competitive with alkylation under these reaction conditions, it is not the major product. Incomplete reactions do exhibit 1H NMR peaks consistent with a benzimidazolium species other than [1H2][Br] that lacks an acetyl moiety. Continuing these reactions affords [1H2][Br] as the predominant product, suggesting that benzimidazole protonation is reversible and does not preclude N-alkylation.




Silver-NHC complexes are versatile transmetallating agents which can transfer NHC ligands to other metals without requiring synthesis and isolation of free NHCs [28]. Therefore, to access the corresponding silver-NHC complex of 1−, deprotonation and metallation at the carboxylic acid and benzimidazolium 2-position were pursued via treatment of [1H2][Br] with Ag2O in CH2Cl2 which afforded [Ag(1)]n (2) as an air- and moisture-stable off-white powder in near-quantitative yield (97%). Despite its multinuclear nature, complex 2 has good solubility in organic solvents such as CH2Cl2, CHCl3 and DMSO, and its 1H NMR spectra exhibit sharp, well-resolved peaks.
Precipitation of AgX generated upon dissociation from an NHC—AgX species is often the kinetic driving force for the transfer of a neutral NHC ligand to another metal. However, complex 2 contains no halides due to the nature of 1− as an L,X-type ligand and can thus transfer an NHC to another metal complex with concomitant halide abstraction. Indeed, treatment of 2 with [RuCl(η6-cymene)(μ-Cl)]2 in CH2Cl2 led to formation of a precipitate (AgCl), affording the Ru—NHC complex [RuCl(1)(η6-cymene)]2 (Ru1) as an air- and moisture-stable orange powder in near-quantitative yield (97%). This reaction afforded analytically pure material without the need for chromatography, crystallization or other purification techniques.
Spectroscopy
Conversion of N-(3,5-dimethylphenyl)benz-imidazole to [1H2][Br] generates a formal positive charge in the benzimidazole core, which is reflected by the 1H NMR signal at 10.27 ppm (DMSO-d6) for the C-2 proton (vs. 8.09 ppm in CDCl3 for the benzimidazole precursor) [29]. This downfield shift is accompanied by the appearance of new peaks at 13.94 and 5.60 ppm, corresponding to the CO2H and the N—CH2 protons, respectively (Table 1). N-Aryl imidazolium carboxylic acids Ia [27] and Ib [17c] (FIG. 1) bear closest structural resemblance to [1H2][Br], but the chemical shifts for the N—CH2 signals (5.32 ppm for both) and C-2 protons (9.63 and 9.62, respectively) were more upfield, reflecting the greater electron richness of the imidazole- vs. benzimidazole-based aromatic systems.







TABLE 1







Selected NMR spectroscopic features a













δH(NCH2)
δH(3,5-Me2)
δC(NCN)







[1H2][Br] b
5.60
2.43
143.3



2
5.17
2.39
188.7



Ru1
4.90 (d), 4.71 (d) 
2.51, 2.42
186.0







a Spectra acquired in CDCl3 or b DMSO-d6.



Chemical shifts (δ) in ppm.






Situated between the NHC and carboxylate moieties, the N—CH2 protons will be diagnostic for the stereoelectronic environment of 1− in metal complexes. Cationic benzimidazolium and neutral CO2H groups in [1H2][Br] are formally converted to their respective neutral NHC and anionic CO2− groups in 2, and this increase in electron-richness is accompanied by an upfield shift in the N—CH2 signals from 5.60 ppm (DMSO-d6) to 5.17 ppm (CDCl3). Conversely, the 13C NMR signal for the 2-position is shifted significantly downfield to 188.7 ppm (vs. 143.3 ppm for [1H2][Br]) and considerably broadened, consistent with (i) the carbenoid nature of the carbon and (ii) coordination to silver. The shift for 2 is also consistent with the range of values (175.7-206.9 ppm) observed for NHC-supported silver complexes with ancillary κ1O-carboxylate ligands [30]. No exact analog of 2 comprising Ag coordinated to a carboxylate-functionalized NHC in a 1:1 ratio has been previously reported, but there are examples of silver complexes with anionic NHC ligands in 1:2 ratios (e.g. IIa and IIb, FIG. 1) [31]. The 1H NMR signals for the N—CH2 protons in IIa and IIb (4.30 and 4.08 ppm, respectively) are significantly upfield of the corresponding signal in 2 (5.17 ppm), where the more electron rich character of the ligands in IIa and IIb could be due to the negative overall charge on these complexes.
Transmetallation from 2 to Ru1 is accompanied by a change in the N—CH2 resonance from one singlet at 5.17 ppm to two doublets at 4.90 and 4.71 ppm (J=16.5 and 17 Hz, respectively). Additionally, the methyl groups on the N-aryl substituent that in 2 afford a single peak (2.39 ppm) instead afford two peaks in Ru1 (2.51 and 2.42 ppm). Collectively, the splitting of the N—CH2 and 3,5-Me2 signals in Ru1 reflects their diastereotopic nature, which suggests that 1− binds to Ru with the NHC and carboxylate moieties in a chelate ring. Similar diastereotopically inequivalent features are observed in analogous cymene-ruthenium complexes supported by carboxylate-functionalized imidazole-based NHCs (e.g. IIIa and IIIb, FIG. 1) [17a, 32]. Complex IIIa, for example, exhibits two doublets for the N—CH2 protons (5.00 and 4.23 ppm, J=15.5 Hz) and two singlets for the 2,6-Me2 protons (2.29 and 2.05 ppm) [17a]. Another notable spectral change upon conversion of 2 to Ru1 is the sharpening of the 13C NMR signal for the 2-position (186.0 ppm). This peak in Ru1 is upfield of the corresponding signals in IIIa and IIIb (171.0 and 174.9 ppm, respectively) [17a, 32], but it is within the range of values observed for benzimidazolylidene-supported arene-ruthenium complexes (184.1-191.7 ppm) [33]. On average, the 13C NMR shifts for the 2-position in the benzimidazolylidene-supported complexes (186.7 ppm) are higher than in the non-benzimidazolylidene complexes (178.6 ppm), thus the downfield shift of Ru1 vs. IIIa and IIIb is consistent with this trend.
Crystallography
Diffraction-quality single crystals of [1H2][Br] were obtained from a saturated EtOH solution via vapor diffusion of Et2O at room temperature (FIG. 2). Crystallographic analysis revealed the carboxylic acid to be oriented nearly perpendicular to the benzimidazolium core (99.5(3)°), a feature consistent with the structure reported for Ib (73.8(3)°) [17c]. In contrast, the N-aryl substituent was more coplanar with the benzimidazolium core in [1H2][Br] than the imidazolium core in Ib (44.0(4°) vs. 82.8(3)°, respectively), due to the greater steric influence of the 2,6-diisopropyl substituents in the latter. A feature of [1H2][Br] is that the bond distance for the C═O functionality (1.199(4) Å) is among the shortest observed for this class of molecules (1.201-1.2398 Å) [17c, 34].
Silver(I) commonly adopts a 2-coordinate geometry with ligands oriented nearly 180° apart, but given that 1− cannot trans-chelate, it was expected that 2 would exhibit a multinuclear structure. Crystallographic analysis revealed that 2 exists in the solid state as a dodecametallic cyclic species (FIGS. 3A and 3B), comprising four distinct [Ag(1)] and [Ag2(1)2] subunits (2Ag1 and 2Ag2, respectively, FIGS. 4 and 5, respectively). The organic framework in 2Ag1 (FIG. 4) is largely unchanged from the ligand precursor, with the N-aryl and carboxylate substituents in 2Ag1 rotated 50±11° and 101±6° relative to the benzimidazole core (vs. 44.0(4)° and 99.5(3)° in [1H2][Br], respectively). No significant difference in the ratio of C—O to C═O bond distances was observed for 2Ag1 relative to [1H2][Br] (1.10 vs. 1.09, respectively), suggesting that the bonding within the carboxylate is relatively unchanged upon replacement of the H+ in [1H2][Br] with the Ag+ in the 2Ag1. Unlike [1H2][Br], the C═O in 2Ag1 is directed towards the benzimidazole core, presumably due to steric effects from the 2Ag2 bound to the C—O.







TABLE 2







Selected bond lengths and angles a












d(M—C)
d(M—O)
∠(CMO)
∠(CNCC)





2Ag1
2.064 ± 0.027
2.114 ± 0.015 
175.5 ± 2.4 
101 ± 6


2Ag2
2.060 ± 0.026
2.125 ± 0.027 
167.0 ± 2.9 
108 ± 4



2.112 ± 0.006
2.664 ± 0.055 
111.4 ± 2.0 
 94 ± 8


IIb b
2.069 (3)
—
—
90.5 (3)


NHC—Ag—O2C c
 2.052-2.0896 
2.085-2.25 
153.14-178.76 
—


NHC—Ag . . . Ag—NHC d
 2.06-2.096
—
—
—


Ru1
2.020 (5)
2.111 (4)
84.49 (18)
45.7 (7)


IIIa e
2.033 (9)
2.079 (8)
86.7 (3)
  40 (1)


IIIb f
2.032 (3)
2.083 (2)
86.0 (1)
38.9 (4)


Ru—O2C in 6-membered 
—
2.065-2.115
82.4-92.8
—


chelate ring g






arene-Ru—NHC h
2.003-2.089
—
—
—





a Values listed for 2Ag1 and 2Ag2 are the average ± standard deviation of the four comparable subunits. The top and bottom rows for 2Ag2 are for the 2- and 3-coordinate metal centers, respectively. Distances (d) in angstroms (Å) and angles (∠) in degrees (°). Literature data obtained from reference b 31, c 30, d 35, e 17a, f 32, g 39, and h 33 and 40.






Mononuclear silver-NHC complexes with κ1O-carboxylate ligands have been previously reported [30], with carbon-silver and oxygen-silver bond distances of 2.052-2.0896 Å and 2.085-2.25 Å, respectively. Although the Ag—O distances in 2Ag1 (2.114±0.015 Å, Table 2) are near the middle of the range observed for related complexes, the Ag—C distances (2.064±0.027 Å) are among the shortest. Similarly, the C—Ag—O angle of 175.5±2.4° for 2Ag1 is one of the most linear measured for these complexes (153.14-178.76°). Compared to the corresponding values in IIb (Ag—C=2.069(3) Å and C—Ag—C′=180.0(1)°) [31], however, 2Ag1 appears consistent with the motif for Ag complexes with anionic NHCs.
One prominent feature of the bimetallic 2Ag2 subunits is the presence of a close silver-silver contact (FIG. 5), with an Ag . . . Ag distance of 2.945±0.019 Å that is consistent with the values determined for other NHC-supported Ag . . . Ag complexes (2.782-3.124 Å) [35]. Because the Ag . . . Ag distance in 2Ag2 is less than twice the van der Waals radius for Ag (3.44 Å), some degree of closed-shell d10-d10 metallophilic interactions can be inferred [36]. Interestingly, the two metal centers in 2Ag2 have different coordination environments: one Ag is bound by two carboxylates (e.g. Ag2) and the other is bound by one (e.g. Ag3), where the former exhibits a longer Ag—C distance than the latter (2.112±0.006 Å vs. 2.060±0.026 Å, respectively). Silver-carbon bond lengths measured in other NHC-supported Ag . . . Ag complexes range from 2.06(2) to 2.096(5) Å [35], which places the Ag—C distances in 2Ag2 among the shortest and longest. The NHC—Ag bond vectors in these previously-reported bimetallic complexes were observed to be orthogonal with each other (77.2-96.71°), and the corresponding C—Ag . . . Ag—C dihedral angle in 2Ag2 of 73.5±1.8° followed this trend.
Excluding the closed-shell d10-d10 interaction, the silver bound by two carboxylates displays a 3-coordinate, distorted T-shape geometry (C—Ag-Ocis=111.4±2.00, C—Ag—Otrans=165.0±1.4°), whereas the silver bound by one carboxylate displays a 2-coordinate, distorted linear geometry (C—Ag—O=169.1±2.5°). Moreover, the metric parameters for the 2-coordinate silver in 2Ag2 are highly conserved with those for the silver in 2Ag1. For the 3-coordinate silver in 2Ag2, the bond to the cis carboxylate was significantly longer than the trans (2.664±0.055 Å vs. 2.138±0.034 Å), suggesting the former can be viewed as a neutral carbonyl interacting with a Lewis acid via its lone pair and the latter as an anionic oxygen coordinated to a metal. In support of this interpretation, the C—O distance in the carboxylate bound cis to the NHC (1.22 Å) is shorter than the trans (1.26 Å), indicating greater carbon-oxygen double bond character in the former.
In addition to the close Ag . . . Ag contact, the two [Ag(1)] constituents in 2Ag2 also exhibit an interaction between the π-systems of the N-aryl substituent of the ligand bound to the 3-coordinate silver and the NHC core of the ligand bound to the 2-coordinate silver. Given the centroid-centroid distance of 3.939±0.04 Å and high degree of coplanarity between the ring planes (6.37±1.68°), this π-π interaction is most appropriately classified as offset π-π stacking [37]. For comparison, π-π stacking has been observed in other NHC-supported metal complexes with centroid-centroid distances ranging from 3.307 Å to 4.725 Å [38], thus the value measured in 2Ag2 is consistent with this type of interaction.
Chelation of 1− to Ru in complex Ru1, inferred by 1H NMR spectroscopy from the diastereotopic nature of the N—CH2 protons, was confirmed by single crystal X-ray diffraction analysis (FIG. 6). The C1-Ru1-O1 angle of 84.49(18)° and Ru1-O1 distance of 2.111(4) Å in Ru1 were consistent with other complexes comprising 6-membered Ru-carboxylate chelate rings (82.4-92.8° and 2.065-2.115 Å, respectively) [39]. Previously reported NHC-supported cymene-ruthenium complexes exhibited Ru-arene centroid and Ru—NHC bond distances of 1.677-1.731 Å and 2.003-2.089 Å, respectively, and the corresponding values measured in Ru1 (Ru-cymene centroid=1.696 Å; Ru1-C1=2.020(5) Å) fall within these ranges [40]. These cymene complexes do not contain benzimidazole-based NHCs, but the relatively few crystallographically characterized benzimidazolylidene-ruthenium complexes bearing any kind of arene ligand exhibit Ru-centroid and Ru—NHC distances (1.658-1.721 Å and 2.016-2.089 Å) that are highly conserved with those for cymene-ruthenium-imidazolylidene complexes [33]. Collectively, the structural features observed in Ru1 suggest that coordination chemistry of the individual benzimid-azolylidene and carboxylate components in 1− are not significantly perturbed by the chelating linker.
Catalysis
Homogenous hydrogenation catalysis was first demonstrated with a cymene-ruthenium complex in 1978, with the dicationic metallocene IIIc producing cyclohexane from cyclohexene under 50 bar of H2(g) (FIG. 7) [41]. Noyori demonstrated that arene-ruthenium complexes could catalyze the transfer hydrogenation of achiral ketones, using iPrOH as the H2 source, into chiral alcohols with excellent enantioselectivity (e.g. IIId) [42]. Considering the other chelating carboxylate NHC-supported complexes, IIIa achieved near-quantitative hydrogenation of styrene to ethylbenzene in iPrOH, but the reactions required 60 bar of H2(g) to proceed and exhibited no conversion at lower pressures (e.g. 1 bar) [17a]. Complex IIIb, on the other hand, could convert acetophenone to 1-phenylethanol using iPrOH as the solvent and H2 source, but the authors noted the catalyst displayed inconsistent activity and IIIb was only obtained as a byproduct from the synthesis of a different complex. The closest analog of Ru1 with a chelating benzimidazolylidene that catalyzes transfer hydrogenation of acetophenone using iPrOH as the H2 source is IIIe, which comprises a neutral chelating benzimidazolylidene that can be deprotonated in situ to afford a complex with an anionic chelating NHC ligand (IIIf) under the basic conditions employed for transfer hydrogenation catalysis [43]. Although complex IIIe exhibited modest activity (19% yield after 20 h) and enantiomeric excess (33%) of (S)-1-phenylethanol, independently prepared and isolated IIIf showed no catalytic activity, even though the reactions with IIIe were performed in the presence of excess base (7.5 equiv.) to deprotonate the ligand.
The ability of Ru1 to catalyze transfer hydrogenation reactions and the factors influencing its activity using the conversion of acetophenone (4a) to 1-phenylethanol (5a) in iPrOH as the benchmark reaction was explored. Near-quantitative isolated yield (96%) of 5a was obtained after 24 h at 83° C. using 1 mol % Ru1 with 5 mol % KOtBu, corresponding to a turnover number (TON) of 96 (entry 1, Table 3). 1 mol % catalyst and 5 mol % KOtBu were selected as the standardized conditions for all subsequent transfer hydrogenation reactions using Ru1 as the catalyst. Analysis of the 4a→5a reaction mixture after 1 h by 1H NMR spectroscopy revealed a turnover frequency (TOF) of 31 h−1. Product formation was observed to be linear with respect to time for the first 2 h of all substrate hydrogenation reactions investigated. Repeating the 4a→5a reaction without Ru1 afforded only 6% of 5a. Conversely, when 5a was treated with 1 mol % Ru1 and 5 mol % KOtBu in toluene at 83° C. for 24 h, the dehydrogenation product 4a was formed in 50% isolated yield.







TABLE 3







Summary of transfer hydrogenation reactions catalyzed by 3 a












Entry
Substrate
Product
Yield (%) b
TON c
TOF (h−1) d





1








96
96
31


 



4a
5a





 


2








95
95
25


 



4b
5b





 


3








98
98
59


 



4c
5c





 


4








86
86
27, e 8.2 f


 



4d
5d





 


5








82
82
 8.1


 



4e
5e





a Reaction conditions:


0.91 mmol substrate, 9.1 μmol Ru1, 45 μmol KOtBu, 5 mL iPrOH, 83° C., 24 h.


b Isolated yield of pure product, averaged over 2 runs.


c Turnover number (TON) = (mmol of 5)/(mmol of Ru1).


d Turnover frequency (TOF) determined by 1H NMR spectroscopic analysis of reaction mixture after 1 h.


e Values correspond to TOF for hydrogenation of the C═C bond in 4d followed by


f the C═O bond in 1,3-diphenylpropan-1-one.






Transfer hydrogenation catalysis has been investigated with the 4a→5a reaction for other NHC-supported arene-ruthenium complexes under conditions comparable to those used for Ru1 (≦1 mol % catalyst, substoichiometric base, iPrOH solvent, temperatures ≧75° C.) from which a wide range of TON (34-1056) and TOF (4.1-1012 h−1) values [44] have been observed [31, 37a, 42]. Although the TON and TOF values for Ru1 (96 and 31 h−1, respectively) are at the lower ends of the ranges measured for all reported cymene-Ru—NHC transfer hydrogenation catalysts, they compare favorably to IIIa (no activity with H2(g)<60 bar) [17a], IIIb (inconsistent activity) [32], and IIIe (TON=4.8, TOF=0.24 h−1) [43]. Thus, despite the fact that replacing the imidazolylidene scaffold in IIIa and IIIb with the benzimidazolylidene scaffold in Ru1 does not produce significant variation in metric parameters, Ru1 achieves catalytic transfer hydrogenation with reproducible TON and TOF values using iPrOH as the sole H2 source, but IIIa and IIIb do not. Markedly different chemical reactivity between complexes supported by benzimidazolylidene- vs imidazolylidene ligands has been observed with Grubbs' catalysts, in which benzimidazolylidene-supported complexes were unstable with respect to ligand decomposition under conditions in which the imidazolylidene-supported complexes would be stable [45].
The scope of substrates which could undergo transfer hydrogenation by Ru1 using the standardized conditions was examined. Similar to 4a→5a, 2-nonanone (4b) and cyclohexanone (4c) were converted to 2-nonanol (5b) and cyclohexanol (5c) in near-quantitative isolated yields (TON=95 and 98, respectively; entries 2 and 3, Table 3). In contrast, the TOF for 4b→5b (25 h−1) was slightly slower than for 4a→5a and the TOF for 4c→5c (59 h−1) was significantly faster. Steric effects between the substrate and catalyst could affect the transition state energy and produce variation in TOF values. For example, 4a and 4b differ by the replacement of a phenyl with an n-heptyl group, a flexible n-alkyl chain that occupies a greater volume due to free rotation than a rigid aryl ring and will thus cause greater substrate-catalyst steric repulsion than 4a. Flexibility is significantly reduced if alkyl substituents are tied together in a cycloalkane ring, and diminished steric congestion likely contributes to the faster reactivity of 4c vs. 4b.
Using chalcone (4d; entry 4, Table 3) as an α,β-unsaturated ketone substrate with Ru1, the fully-saturated product 1,3-diphenyl-propan-1-ol (5d) was obtained in good yield (TON=86), wherein 1H NMR analysis revealed hydrogenation occurred at the alkene moiety before the ketone. For the first 2 h, the only observable product was 1,3-diphenylpropan-1-one (from hydrogenation of the C═C bond in 4d), and its formation was linear with respect to time over the first 2 h (TOF=27 h−1). After 2 h, 5d began to appear (from hydrogenation of the C═O bond in 1,3-diphenylpropan-1-one), and its formation was linear with respect to time over the next 2 h (TOF=8.2 h−1). After 24 h, the only observable product was 5d, which was isolated and used to determine TON. No formation of 1,3-diphenylprop-2-en-1-ol (from hydrogenation of the C═O bond in 4d) was observed during the course of the reaction. Other NHC-supported arene-ruthenium transfer hydrogenation catalysts have exhibited similar preferential reactivity at the carbon-carbon double bonds in α,β-unsaturated ketones [40e, 40k, 46], which has been proposed as evidence for an inner-sphere mechanism being operative in these systems [47]. No hydrogenation of stilbene was observed with Ru1, which suggests that polarization of the C═C bond (e.g. by the adjacent carbonyl in 4d) is necessary for reactivity. Substituting a ketone with an imine substrate (4e, entry 5) resulted in a lower yield of hydrogenated product 5e (TON=82) and significantly slower formation (TOF=8.1 h−1), behavior which is consistent with the slower overall reactivity observed for NHC-supported arene-ruthenium complexes with similar imine substrates (e.g., for 4e, TOF=2.0-33 h−1) [40e, 48]. Presumably, the trend of lower TOF values for imines vs. ketones arises from the less polar character of a C═N bond relative to a C═O bond.
We have reported a chelating benzimidazolylidene carboxylate ligand (1−) that can be accessed via the benzimidazolium hydrobromide precursor [1H2][Br]. Deprotonation and metallation with Ag2O produced the silver-NHC complex 2, which was revealed by X-ray crystallography to exist in the solid state as a dodecametallic cyclic species comprising mononuclear [Ag(1)] and dinuclear [Ag2(1)2] subunits. Despite this multinuclear structure, transmetallation of 1− from 2 to [RuCl(cymene)(μ-Cl)]2 proceeded smoothly with precipitation of AgCl to afford analytically pure ruthenium-NHC complex Ru1 in near-quantitative yield.
Complex Ru1 functions as a precatalyst in the transfer hydrogenation of unsaturated substrates using iPrOH as the H2 source. Benzylic, alkyl and cycloalkyl ketones were converted to their corresponding alcohols in excellent yields (TON=95-98) and at modest rates (TOF=25-59 h−1). Chalcone, an α,β-unsaturated ketone, underwent reduction faster at the alkene moiety (TOF=27 h−1) than at the carbonyl (TOF=8.2 h−1), ultimately affording the fully-saturated 1,3-diphenylpropan-1-ol in high yield (TON=86). Similarly, Ru1 was catalytically competent for the hydrogenation of an imine substrate, albeit with diminished reactivity (TON=82, TOF=8.1 h−1) relative to the ketone substrates.
1− can substitute an X-type ligand on a transition metal as well as coordinate in a bidentate manner with both the NHC and carboxylate moieties. Due to the anionic nature of 1−, this ligand exchange can be accomplished without altering the overall charge of the complex. Given that the transfer of 1− from 2 to another transition metal can afford analytically pure Ru1 in near-quantitative yields without the need for purification, this may serve as a general strategy to access diverse families of transition metal complexes for a wide variety of applications.
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Example 2
A chelating benzimidazolylidene-carboxylate ligand (1−) was transferred from 2 to [RuCl2(dmso)4] to afford trans(C)—[Ru(1)2(bpy)] (Ru3), but all attempts to incorporate 1 into cis(Cl)—[RuCl2(bpy)2] were unsuccessful. Alternatively, reaction of [RuCl(1)(η6-cymene)] (Ru1) with bpy and AgOTf successfully produced [Ru(1)(bpy)2][OTf] (Ru4). Methylation of Ru3 and Ru4 with MeOTf yielded trans(C)—[Ru(1-Me)2(bpy)][OTf]2 (Ru3.2MeOTf) and [Ru(1-Me)(bpy)2][OTf]2 (Ru4.MeOTf), accompanied by a +2 and +1 increase in net charge, respectively. Cyclic voltammetry indicated that the increase in Ru(II)/Ru(III) oxidation potential from Ru3 to Ru3.2MeOTf was twice the increase from 4 to Ru4.MeOTf. UV-visible spectroscopy also revealed that transitions in Ru3.2MeOTf occurred at higher energy than in 2 by double the difference between Ru4.MeOTf and 4. Crystallographic analysis demonstrated that the coordination environment of Ru did not differ significantly between 2 and Ru3.2MeOTf, suggesting that the observed shifts in oxidation potentials and absorption wavelengths are not due to changes in coordination chemistry or formal oxidation state. Collectively, these results show that Ru3.2MeOTf and Ru4.MeOTf feature Ru centers more electron deficient than those in 2 and 4, respectively, by amounts proportional to the difference in net charge.
The strategy was to prepare octahedral ruthenium complexes [RuLn(NHC)]m+ (A) comprising one or more benzimidazolylidene-carboxylate ligands (Scheme 3). Coordinative saturation was desired to minimize any variation in electron density at the metal due to changes in coordination number or ligand substitution. Conversion of A to [RuLn(NHC-Me)](m+1)+ (B) via methylation was expected to transform the L,X-type NHC-carboxylate into an L2-type chelating NHC-ester. Although this reaction at the ligand would be accompanied a +1 increase in net charge for the complex, the formal oxidation state of Ru in B would not change. Spectroscopic, crystallographic and electrochemical analysis and comparison of complexes A and B would then elucidate the impact of increasing the net charge on a complex separately from any increase in oxidation state of the metal center.




Materials and Methods

Complex 2, Ru1 and [RuCl2(bpy)(dmso)2] were prepared as previously described [6, 8]. All other materials and solvents were of reagent quality and used as received. 1H and 13C{1H} NMR spectra were recorded using a Bruker 500 MHz spectrometer. Chemical shifts δ (in ppm) for 1H and 13C NMR are referenced to SiMe4 using the residual protio-solvent as an internal standard [9]. For 1H NMR: CDCl3, 7.26 ppm; acetone-d6, 2.05 ppm. For 13C NMR: CDCl3, 77.16 ppm. Coupling constants (J) are expressed in hertz (Hz). Infrared spectra were recorded with 4 cm−1 resolution on a Shimadzu IRAffinity-1S spectrometer equipped with a Pike Technologies MIRacle ATR sampling accessory (diamond crystal). Elemental analyses were performed at Atlantic Microlab, Inc. (Norcross, Ga.). All reactions were performed under an inert atmosphere were performed under an N2 atmosphere using standard Schlenk or glovebox techniques with the exclusion of light. All workups and purifications were performed under ambient conditions using standard benchtop techniques without requiring exclusion of light. When required, solvents were dried and deoxygenated using an Innovative Technologies solvent purification system, and then stored over molecular sieves (3 Å) in a drybox.
General Spectroscopic Considerations
UV-visible absorption spectra were acquired on a Varian Cary 50 Bio spectrometer equipped with a Quantum Northwest TC-125 temperature controller. Room temperature solutions measurements were performed in matched gas-tight quartz cuvettes (Precision Scientific) with 1 cm path lengths and 3.0 mL analyte solution volumes thermostatted at 25° C. Absorption spectra were acquired in CH2Cl2 under an N2 atmosphere for all analytes. Extinction coefficients (ε) were calculated from Beer's law measurements using 10, 20, 30 and 40 μM analyte concentrations.
Electrochemistry
Electrochemical experiments were conducted on CH Instruments Electrochemical Workstations (series 660D) using a gastight, three-electrode cell under an atmosphere of dry nitrogen. The cell was equipped with gold working and tungsten counter electrodes, as well as a silver wire quasi-reference electrode. Unless specified otherwise, measurements were performed using 1.0 mM solutions of analyte in dry CH2Cl2 with 0.10 M [tetra-n-butyl-ammonium][PF6] as the electrolyte and 1.0 mM ferrocene (Fc) as the internal standard. All potentials reported were determined by cyclic voltammetry at 100 mV s−1 scan rates and referenced to ferrocene by shifting (Fc)0/+ to 0.00 V (CH2Cl2).
X-Ray Crystallographic Studies
Single crystals of Ru3 and Ru4 were immersed in Paratone-N oil at room temperature and mounted on glass fibers using epoxy glue. The samples were then mounted on the goniometer for data collection at 200 K under a stream of cold nitrogen. Intensity data were collected using Mo Kα radiation (λ=0.71073 Å) and a Mercury CCD detector with a Rigaku AFC8S diffractometer controlled using the CrystalClear software package [10]. The crystal-to-detector distance was 27 mm. Data were collected using ω-scans (0.5° oscillations) using 65 s exposures for Ru3 and 20 s exposures for Ru4. Data were corrected for absorption, Lorentz, and polarization effects using the REQAB subroutine of CrystalClear [11]. The structures were solved by direct methods and subsequently refined using the SHELXTL software package [12]. Further evaluation for higher symmetry and solvent occupancy was done using the PLATON program suite [13]. All non-hydrogen atoms were refined anisotropically. Hydrogen atoms were placed at calculated positions using a riding model and assigned thermal parameters equal to either 1.5 (methyl hydrogen atoms) or 1.2 (non-methyl hydrogen atoms) times the thermal parameters of the atoms to which they were attached. For Ru3, the ethanol and water solvent molecules were identified from the difference map and modeled by the judicious use of restraints. For Ru4, several partially-occupied acetone solvent molecules could initially be identified from the difference map, but their refinement proved problematic, even when heavily restrained. These disordered solvent molecules were instead modeled using the SQUEEZE tool of PLATON.
Synthesis of trans(C)—[Ru(1)2(bpy)] (Ru3)
Complex 2 (323 mg, 0.83 mmol) was dissolved in CHCl3 (10 mL) and to this solution was added dropwise a solution of [RuCl2(bpy)(dmso)2] (200 mg, 0.41 mmol, 0.5 equiv.) in CHCl3 (10 mL) and the mixture was then heated to reflux. After 24 h, the reaction mixture was allowed to cool to room temperature and was then filtered through a 0.2 μm PTFE filter (to remove AgCl) with the aid of CHCl3 (4 mL). The filtrate solvent was removed under reduced pressure and the resulting solids were then dissolved in minimum CH2Cl2 and added to 10 mL of hexanes resulting in the formation of a precipitate. The solids were collected via centrifugation, washed with Et2O (3×10 mL) and MeOH (3×10 mL), and then dried in vacuo to afford 262 mg (0.32 mmol, 78% yield) of the desired product as a dark red-purple solid. 1H NMR (500 MHz, CDCl3): δ=8.98 (d, J=5.5, 2H), 7.37 (d, J=8.5, 2H), 7.26-7.24 (m, 2H), 7.18 (t, J1=8.0, J2=15.5, 2H), 6.99-6.92 (m, 4H), 6.76 (d, J=8.0, 2H), 6.70 (s, 2H), 6.28 (d, J=8.0, 2H), 6.17 (s, 2H), 5.44 (s, 2H), 5.28 (d, J=16.0, 2H), 5.08 (d, J=15.5, 2H), 1.99 (s, 6H), 1.90 (s, 6H). 13C NMR (125 MHz, CDCl3): δ 198.3, 174.7, 160.0, 152.2, 138.9, 137.6, 137.4, 136.7, 134.6, 130.2, 129.2, 126.1, 125.4, 122.9, 122.8, 122.3, 120.8, 109.7, 109.2, 50.5, 21.2, 21.2. FT-IR (ATR, diamond): UV-vis (CH2Cl2), λ (ε) in nm (M−1 cm−1): 293 (sh, 2.05×104), 302 (2.59×104), 386 (3.57×104), 499 (4.07×103), 530 (5.46×103). Anal. Calc. for C44H39N6O4.5Ru (2.0.5H2O): C, 64.07; H, 4.77; N, 10.19. Found: C, 63.94; H, 4.84; N, 10.18.
Synthesis of [Ru(1)(bpy)2][OTf] (Ru4)
Complex Ru1 (100 mg, 0.18 mmol) and 2,2′-bipyridine (57 mg, 0.36 mmol, 2.0 equiv.) were dissolved in DMSO (1.5 mL) and stirred at room temperature for 5 min. To this solution was added dropwise a solution of AgOTf (49 mg, 0.19 mmol, 1.1 equiv.) in DMSO (1.5 mL) and the reaction mixture was heated to 170° C. After 24 h, the reaction mixture was allowed to cool to room temperature and then added to 10 mL of Et2O resulting in the formation of a precipitate. The solids were collected via centrifugation, washed with Et2O (3×5 mL), and then purified via column chromatography (Al2O3, 99:1 CH2Cl2/MeOH, Rf=0.4) to afford 130 mg (0.15 mmol, 83% yield) of the desired product as a dark red-purple solid. 1H NMR (500 MHz, CDCl3): δ=8.95 (d, J=9.5, 1H), 8.88 (d, J=8.0, 1H), 8.36 (d, J=8.0, 1H), 8.29 (d, J=8.0, 1H), 8.23 (d, J=8.0, 1H), 8.09 (td, J1=8.0, J2=1.3, 1H), 8.03 (td, J1=7.9, J2=1.2, 1H), 7.87 (d, J=8.5, 1H), 7.79 (td, J1=7.9, J2=1.2, 1H), 7.63 (td, J1=6.8, J2=1.0, 1H), 7.54-7.45 (m, 3H), 7.40 (d, J=8.0, 1H), 7.29 (td, J1=7.8, J2=0.7, 1H), 7.16 (td, J1=6.5, J2=1.0, 1H), 7.12 (t, J=7.8, 1H), 7.04 (dd, J1=5.5, J2=0.5, 1H), 7.00 (td, J1=6.6, J2=1.3, 1H), 6.79 (s, 1H), 6.53 (d, J=8.0, 1H), 6.37 (s, 1H), 5.54 (s, 1H), 5.08 (d, J=16.5, 1H), 4.57 (d, J=16.5, 1H), 2.03 (s, 3H), 1.91 (s, 3H). 13C NMR (125 MHz, CDCl3): δ 197.8, 172.5, 158.9, 158.1, 157.6, 155.6, 154.5, 151.6, 150.8, 148.8, 139.7, 138.7, 138.1, 137.5, 136.9, 136.3, 135.9, 134.9, 134.6, 131.4, 127.7, 126.8, 126.5, 125.7, 125.6, 124.8, 124.1, 123.9, 123.5, 123.4, 123.3, 122.8, 110.4, 108.8, 50.8, 21.3, 21.1. UV-vis (CH2Cl2), λ (ε) in nm (M−1 cm−1): 290 (sh, 1.49×105), 296 (1.68×105), 360 (4.92×104), 460 (sh, 2.43×104), 496 (2.93×104). Anal. Calc. for C38H31F3N6O5S1Ru (4.H2O): C, 53.08; H, 3.87; N, 9.77. Found: C, 53.14; H, 3.99; N, 9.75.
Synthesis of trans(C)—[Ru(1-Me)2(bpy)][OTf]2 (Ru3.2MeOTf)
Complex Ru3 (50 mg, 61 μmol) was dissolved in CH2Cl2 (2 mL) and then cooled to −30° C. After 30 min, 0.20 mL of a 0.77 M solution of MeOTf in CH2Cl2 (0.15 mmol, 2.5 equiv.) was added dropwise and the reaction was allowed to warm to room temperature and stirred for 2 h. The solution was then concentrated to 1 mL and added to 10 mL of hexanes resulting in the formation of a precipitate. The solids were collected via centrifugation, washed with EtOAc (3×5 mL) and Et2O (3×5 mL), and then dried in vacuo to afford 65 mg (57 μmol, 93% yield) of the desired product as a light orange-red solid. 1H NMR (500 MHz, acetone-d6): δ=8.58 (d, J=5.5, 2H), 7.88-7.80 (m, 4H), 7.78 (t, J=7.8, 4H), 7.37 (t, J=7.8, 2H), 7.19 (t, J=7.5, 2H), 7.15 (t, J=5.8, 2H), 6.94 (s, 2H), 6.77 (s, 2H), 6.56 (d, J=8.0, 2H), 5.80 (d, J=4.5, 4H), 5.72 (s, 2H), 4.27 (s, 6H), 2.13 (s, 6H), 2.05 (s, 6H, overlaps acetone-ds). UV-vis (CH2Cl2), λ (ε) in nm (M−1 cm−1): 296 (8.59×104), 329 (5.06×104), 445 (1.10×104). Anal. Calc. for C48H45F6N6O10.5S2Ru (5.0.5H2O): C, 50.00; H, 3.93; N, 7.29. Found: C, 49.91; H, 3.94; N, 7.20.
Synthesis of Ru(1-Me)(bpy)2][OTf]2 (Ru4.MeOTf)
Complex Ru4 (50 mg, 59 μmol) was dissolved in CH2Cl2 (2 mL) and then cooled to −30° C. After 30 min, 0.10 mL of a 0.77 M solution of MeOTf in CH2Cl2 (77 μmol, 1.3 equiv.) was added dropwise and the reaction was allowed to warm to room temperature and stirred for 2 h. The solution was then concentrated to 1 mL and added to 10 mL of hexanes resulting in the formation of a precipitate. The solids were collected via centrifugation, washed with Et2O (3×5 mL), and then dried in vacuo to afford 57 mg (57 μmol, 97% yield) of the desired product as a light orange-red solid. 1H NMR (500 MHz, acetone-d6): δ=9.52 (d, J=5.0, 1H), 8.93 (d, J=5.0, 1H), 8.79 (d, J=8.3, 1H), 8.71 (d, J=8.3, 1H), 8.57 (d, J=8.2, 1H), 8.35 (t, J=7.4, 1H), 8.28 (t, J=7.4, 1H), 8.18-8.10 (m, 2H), 7.88 (d, J=8.3, 1H), 7.80-7.75 (m, 2H), 7.74-7.68 (m, 2H), 7.59-7.51 (m, 2H), 7.39 (t, J=7.6, 1H), 7.25-7.17 (m, 2H), 6.87 (s, 1H), 6.68 (s, 1H), 6.59 (d, J=8.3, 1H), 5.85 (d, J=18.3, 1H), 5.69 (s, 1H), 5.44 (d, J=18.4, 1H), 3.81 (s, 3H), 2.07 (s, 3H), 1.86 (s, 3H). UV-vis (CH2Cl2), λ (ε) in nm (M−1 cm−1): 291 (1.43×105), 330 (6.28×104), 429 (2.03×104), 454 (2.30×104). Anal. Calc. for C40H34F6N6O8S2Ru: C, 47.76; H, 3.41; N, 8.35. Found: C, 47.32; H, 3.77; N, 7.96.
Results and Discussion
Each benzimidazolylidene-carboxylate ligand will occupy two coordination sites, thus any Ru-containing starting material must have two (or a multiple of two) vacant coordination sites or easily-displaceable ligands. Furthermore, coordinative saturation at Ru and resistance of the methylated product to substitution reactions can be achieved with an octahedral geometry and chelating ligands, respectively. Based on these considerations, it was sought to incorporate the benzimidazolylidene-carboxylate ligand into Ru complexes bearing one or two bpy ligands (bpy=2,2′-bipyridyl).
Silver-NHC complexes are useful for the synthesis of other transition metal-NHC complexes because they supply an NHC without requiring the synthesis and isolation of the free carbene[14]. Complex 2 is particularly versatile because it can abstract a halide from as well as transfer its NHC to another transition metal center. We have previously reported that the NHC in 2, a carboxylate-functionalized benzimidazolylidene, can function as a bidentate L,X type ligand for Ru [6].
The complex [RuCl2(bpy)(dmso)2] has been used to prepare coordinately-saturated octahedral Ru complexes [8] and, upon reaction with 2 equiv. of 2, afforded the desired Ru—NHC complex trans(C)—[Ru(1)2(bpy)] (2), featuring two carboxylates available for methylation (reaction a, Scheme 4). 1H NMR spectroscopic analysis revealed that both NHC ligands in Ru3 were equivalent, presumably due to the C2 axis bisecting N—Ru—N. Additionally, the signal for the N—CH2 protons shifted from the singlet at 5.17 ppm in [Ag(1)] to two doublets at 5.28 and 5.08 ppm in Ru3, indicating the protons had become inequivalent (i.e. two protons were oriented towards the bpy ligand and two away from it). The fact that the N—CH2 protons became diastereotopic was diagnostic for the formation of a C—Ru—O chelate ring, and has previously been observed with Ru1. Remarkably, one of the 3,5-dimethylphenyl aromatic proton signals in Ru3 was observed at 5.04 ppm, significantly upfield of any of the corresponding signals in [Ag(1)] (7.21 and 7.10 ppm).




Having prepared a complex that could increase in net charge by +2, it was next sought to prepare a complex that could increase in net charge by +1. Because complex Ru3 had the formula [Ru(1)2(bpy)], it was reasoned that a suitable target would have the formula [Ru(1)(bpy)2][A] (A=non-coordinating anion). Initial efforts were directed towards the reaction of 2 with cis-[RuCl2(bpy)2] [15], in conjunction with a variety of halide abstracting reagents, but only complicated mixtures were obtained, containing trace amounts of the desired product along with starting materials, intermediate byproducts, and ligand decomposition products. Given that installing the NHC onto a [Ru(bpy)2] complex was unsuccessful, an alternate route was pursued in which two bpy ligands would be installed onto a pre-formed [Ru(NHC)] complex [16]. Reaction of complex Ru1 with 2 equiv. of bpy in the presence of AgOTf afforded [Ru(1)(bpy)2][OTf] (Ru4) in good yield (reaction c, Scheme 4).
No C2 symmetry was present in complex Ru4 and its 1H NMR spectrum revealed all the protons in bpy ligands were inequivalent. Whereas Ru4 had a +1 net charge and Ru3 was overall neutral, the 1H NMR spectroscopic data indicated no straightforward trend that the ligands in Ru4 were significantly more electron deficient, and therefore more deshielded, than those in Ru3. Similar to Ru3, the N—CH2 protons in Ru4 were diastereotopic, but the doublets in Ru4 (5.08 and 4.57 ppm) were located upfield of the corresponding signals in Ru3. Conversely, the 3,5-dimethylphenyl aromatic protons in Ru4 (6.79, 6.37 and 5.54 ppm) resonated slightly downfield of those in Ru3 (6.70, 6.17 and 5.44 ppm). Furthermore, the most downfield bpy 1H NMR signals occurred at nearly identical chemical shifts (8.95 ppm for Ru4 vs. 8.98 ppm for Ru3). Although no trend was discernible from the individual proton resonances, the aromatic protons in Ru4 were collectively more downfield than those in Ru3. Of the 23 aromatic protons in complex Ru4, 15 were located downfield of the residual CHCl3 peak, compared to only 4 of the 22 aromatic protons in complex Ru3.
Reaction of Ru3 with 2.5 equiv. of MeOTf afforded the dimethylated complex trans(C)—[Ru(1-Me)2(bpy)][OTf]2 (Ru3.2MeOTf) in excellent yield (93%, reaction a, Scheme 5). Similar to complex Ru3, the 1H NMR spectrum of Ru3.2MeOTf revealed that the NHC ligands were equivalent. Methylation of the carboxylate moiety of the NHC ligand was inferred from the presence of a peak at 4.27 ppm and relative integration of 6, consistent with the formation of two methyl ester functional groups. In addition, the N—CH2 signal shifted significantly downfield to 5.80 ppm (vs. 5.28 ppm in Ru3) and 10 of the 22 aromatic protons were downfield of 7.26 ppm (vs. 4 protons in Ru3).




Similarly, reaction of complex Ru4 with 1.3 equiv of MeOTf afforded monomethylated complex [Ru(1-Me)(bpy)2][OTf]2 (Ru4.MeOTf) in near-quantitative yield (97%, reaction b, Scheme 5). A new singlet at 3.81 ppm was present in the 1H NMR spectrum of Ru4.MeOTf that was attributed to the formation of a methyl ester. Additionally, the doublets for the N—CH2 protons in Ru4.MeOTf (5.85 and 5.44 ppm) were significantly downfield of the corresponding peaks in the 1H NMR spectrum of Ru4 (5.08 and 4.57 ppm), consistent with a +1 increase in net charge on the complex rendering the metal (and thus also the ligands attached to it) more electron deficient. In support of this conclusion, the most downfield peak in the 1H NMR spectrum of Ru4.MeOTf was at 9.52 ppm, compared to 8.95 ppm for Ru4.
All attempts to isolate the monomethylated analog of Ru3.2MeOTf, comprising one methyl ester and one carboxylate, were unsuccessful. Reaction of Ru3 with 0.1 equiv. of MeOTf at −78° C., quenching via precipitation at this temperature, and immediate 1H NMR analysis of the crude precipitate revealed one additional methyl ester peak (4.20 ppm) and four aryl-CH3 (2.18, 2.07, 1.95 and 1.93 ppm) singlets distinct from the resonances arising from Ru3 or Ru3.2MeOTf. Despite the low temperature and low stoichiometry employed in this reaction, complex Ru3.2MeOTf was also observed in this 1H NMR spectrum in a 1:2 ratio with the supposed monomethylated complex. All complexes isolated from the reactions of Ru3 or Ru4 with MeOTf, including analytically-pure samples of Ru3.2MeOTf and Ru4.MeOTf, were unstable in solution (e.g. CDCl3, CD2Cl2, THF-ds, acetone-d6), which precluded more detailed NMR spectroscopic analysis.
Coordination Chemistry
Single crystals of Ru3 suitable for X-ray diffraction were grown via diffusion of Et2O vapor into a solution of Ru3 in EtOH at room temperature. Crystallographic analysis revealed the two NHC moieties in Ru3 were oriented trans relative to each other (FIG. 8), a configuration that minimized negative steric interactions between the two N-aryl substituents. Overall, the metric parameters determined for Ru3 were consistent with similar complexes that have been previously reported. More specifically, the Ru—C distances (2.057(7) and 2.062(7) Å) and the Ru—O distances (2.111(5) and 2.113(4) Å) in Ru3 fell within the range of values observed for comparable Ru—NHC (2.003-2.089 Å) [12] and Ru-carboxylate (2.065-2.115 Å) [18] complexes. Interestingly, the average C—O bond distances to the terminal oxygen (1.255(9) Å) and the oxygen coordinated to Ru (1.260(9) Å) were nearly identical in Ru3, suggesting a significant degree of charge delocalization within the carboxylate moieties.
Methylation of the terminal carboxylate oxygen atoms upon reaction of Ru3 with MeOTf, inferred by the presence of a methyl ester OCH3 peak in the 1H NMR spectrum of Ru3.2MeOTf, was confirmed by crystallographic analysis (FIG. 9). Although Ru3.2MeOTf had a +2 net charge and Ru3 was overall neutral, the Ru—C distances (2.052(6) and 2.089(6) Å) and the Ru—N distances (2.011(5) and 2.017(5) Å) in Ru3*2MeOTf were not significantly different from those in 2. Methylation of the ligand in Ru3 should convert the charge-delocalized carboxylate moieties to neutral esters that bind Ru via their carbonyl oxygen atoms. The average C—O bond distance to the methylated oxygen (1.317(8) Å) was substantially greater than to the Ru-bound oxygen (1.221(8) Å) in Ru3.2MeOTf, consistent with significant differentiation into single- and double-bond character, respectively. The Ru—O distances (2.139(5) and 2.141(4) Å) in Ru3.2MeOTf were only 2.8 picometers longer than the corresponding distances in Ru3, despite the fact that Ru3.2MeOTf featured a Ru bound to the carbonyl oxygen of a neutral ester ligand, whereas Ru3 featured a Ru bound to the carboxylate oxygen of an anionic carboxylate ligand. Compared to Ru3, the C—Ru—C angle in Ru3.2MeOTf (171.6(2)°) was slightly more obtuse and the O—Ru—O angle (86.47(18)°) was slightly more acute, which could be due to steric repulsion between the two OMe moieties in Ru3.2MeOTf.
Electrochemistry
Cyclic voltammetry of Ru3 revealed a quasireversible peak at −0.14 V (vs. Fc) that was attributed to the Ru(II)/Ru(III) redox couple (black line, FIG. 10A). Similar analysis of Ru3.2MeOTf indicated that the analogous oxidation process occurred at a potential 0.81 V higher in Ru3.2MeOTf (E1/2=0.67 V, grey line, FIG. 10A) than in Ru3, despite the fact that both Ru3 and Ru3.2MeOTf comprised Ru centers in the same oxidation state coordinated to ligand atoms with nearly identical bond distances. Presumably, the +2 net charge in Ru3.2MeOTf that formally resided on Ru significantly lowered the energy of the metal-centered orbitals and, in doing so, raised the energy required to remove electrons from them.
Complex 4 exhibited a Ru(II)/Ru(III) redox couple at 0.45 V (black line, FIG. 10B), a potential significantly higher than the corresponding value in Ru3, which could be attributed to Ru4 having a +1 net charge and Ru3 being overall neutral. Unlike Ru3, however, complex Ru4 also exhibited a quasireversible reduction at −1.95 V. The oxidation potential measured for Ru4.MeOTf (E1/2=0.82 V, grey line, FIG. 10B) was higher than in Ru4, but the difference between the Ru(II)/Ru(III) oxidation potential in Ru4 and Ru4.MeOTf (ΔE4→6=0.37 V) was substantially lower than between Ru3 and Ru3.2MeOTf (ΔE2→5=0.81 V). Similar to Ru4, complex Ru4.MeOTf displayed reduction peaks, albeit irreversible ones, at −1.02 and −1.81 V. Both Ru3.2MeOTf and Ru4.MeOTf decomposed under all cyclic voltammetry experimental conditions after 2-3 scans, which precluded more detailed analyses.
The increase in Ru(II)/Ru(III) oxidation potential showed a linear correlation with the increase in the net charge on the complex. More specifically, the increase in oxidation potential going from 2 to Ru3.2MeOTf was 2.2 times greater than the increase from Ru4 to Ru4.MeOTf (0.81 V/0.37 V), and the increase in net charge from Ru3 to Ru3.2MeOTf was twice that from Ru4 to Ru4.MeOTf. Examination of the oxidation onset potentials, instead of the half-wave potentials, revealed a closer correlation with net charge. The onset for the Ru(II)/Ru(III) oxidation in Ru3.2MeOTf occurred at a potential 0.77 V higher in energy than in Ru3 (0.58 vs. −0.19 V, respectively), and the corresponding process in Ru4.MeOTf was 0.38 V higher than in Ru4 (0.73 vs. 0.35 V, respectively). Therefore, the increase in oxidation onset potential going from Ru3 to Ru3.2MeOTf was twice the increase from Ru4 to Ru4.MeOTf (0.77 V/0.38 V).
Spectroscopy
The Ru—NHC complexes were then analyzed by UV-visible spectroscopy to elucidate any correlation between net charge and optical properties. Because the electrochemistry experiments revealed the Ru(II)/Ru(III) oxidation potentials were strongly affected by net charge, the lowest-energy optical transitions were examined, given that they likely involved transitions to or from metal-centered orbitals. The longest-wavelength peaks in Ru3 and Ru3.2MeOTf occurred at 530 nm (2.34 eV) and 445 nm (2.79 eV), respectively (FIG. 11A). Similar analysis of Ru4 and Ru4.MeOTf revealed their longest-wavelength peaks occurred at 496 nm (2.50 eV) and 454 nm (2.73 eV), respectively (FIG. 11B). The difference in longest-wavelength optical transition energy (ΔEopt) between Ru3.2MeOTf and Ru3 was 0.45 eV, whereas ΔEopt was 0.23 eV between Ru4.MeOTf and Ru4. Considering the ratio of these ΔEopt values, the increase in energy going from Ru3 to Ru3.2MeOTf was double the increase from Ru4 to Ru4.MeOTf (0.45 eV/0.23 eV).
A similar trend was observed with the second-lowest energy peaks. After the transition at 530 nm, the next longest wavelength peak for Ru3 was located at 386 nm (3.21 eV). Conversion to Ru3.2MeOTf shifted this peak to 329 nm (3.77 eV), a 0.56 eV increase in energy. Analogous peaks in Ru4 and Ru4.MeOTf were observed at 360 nm (3.44 eV) and 330 nm (3.75 eV), respectively, corresponding to an energy difference of 0.31 eV. Based on this second set of peaks, the increase in energy going from Ru3 to Ru3.2MeOTf was 1.8 times the increase from Ru4 to Ru4.MeOTf (0.56 eV/0.31 eV). Although the ratios determined from UV/vis spectroscopy were in good agreement with those obtained via electrochemistry, the possibility that the similarity of these ratio values was coincidental could not be definitively excluded. The UV/vis spectra of Ru3, Ru4, Ru3.2MeOTf and Ru4.MeOTf all displayed multiple transitions, some overlapping, which complicated peak assignments and consequently any interpretation of shifts in energy due to changes in net charge.
A chelating benzimidazolylidene-carboxylate ligand was used to prepare the complexes trans(C)—[Ru(1)2(bpy)] (Ru3) and [Ru(1)(bpy)2][OTf] (Ru4). With two NHC-carboxylate ligands, the net charge on Ru3 was increased by +2 upon methylation to give trans(C)—[Ru(1-Me)2(bpy)][OTf]2 (Ru3.2MeOTf). Similarly, the one NHC-carboxylate ligand in Ru4 reacted with MeOTf to afford [Ru(1-Me)(bpy)2][OTf]2 (Ru4.MeOTf), accompanied by a +1 increase in net charge. Cyclic voltammetry revealed the increase in Ru(II)/Ru(III) oxidation half-wave and onset potentials was 2.2 and 2.0 times greater, respectively, when accompanied by a +2 increase in net charge vs. a +1 increase. UV-visible spectroscopic analysis suggested the first and second longest-wavelength peaks in Ru3 were shifted to higher energy in Ru3.2MeOTf by a factor of 2.0 and 1.8, respectively, greater than the corresponding shift from Ru4 to Ru4.MeOTf. Despite these substantial changes in oxidation potentials and absorption wavelengths, the X-ray crystal structures of Ru3 and Ru4 showed that there were no significant changes in metal-ligand bond distances.
Collectively, these results demonstrate that the Ru centers in Ru3.2MeOTf and Ru4.MeOTf were rendered more electron deficient than those in Ru3 and Ru4, respectively, by amounts linearly proportional to the increase in the net charge of the complexes. Furthermore, the high degree of similarity of the metric parameters in Ru3 and Ru3.2MeOTf suggested that the changes in electron density at the metal centers observed by electrochemistry and UV/vis spectroscopy were not caused by significant changes in coordination chemistry. Because 2 can install the benzimidazolylidene-carboxylate ligand onto a variety of transition metal complexes and methylation of the carboxylate moiety with MeOTf can increase net charge without changing the formal oxidation state or coordination chemistry of the metal center, this represents a general strategy for studying the effects of net charge on the electronic and optical properties of organotransition metal complexes.
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Example 3
Transfer hydrogenation catalysis has been used for decades in chemical synthesis to transfer H2 to unsaturated organic substrates, which is analogous to proton-coupled electron transfer. Despite this parallel with biological reductions and these catalysts' widespread use, this report is the first instance of catalytic radical reduction in aqueous solution by a transfer hydrogenation-like process. An organoruthenium complex (Ru1) catalytically reduced 2,2′-azino-bis(3-ethylbenzo-thiazoline-6-sulfonate) radical monoanion (ABTS•−) using a non-tertiary alcohol terminal reductant (i.e., R1—CHOH—R2). Both the C—H and O—H groups of the —CHOH— moiety were necessary to function as a terminal reductant. Comparison of ethanol and isopropanol reaction rates to ethanol-d6 and isopropanol-dg yielded primary kinetic isotope effect values indicating H2 transfer from the CH—OH moiety in the rate-determining step. Furthermore, Ru1 slowed oxidative formation of ABTS•− by HO•, then reduced all ABTS•− formed, and remained catalytically active over multiple cycles. Collectively, these results demonstrate that Ru1 inhibits the oxidative formation of and catalyzes the reduction of radicals in aqueous solution by a transfer hydrogenation-like process.
Results and Discussion
It was sought to determine if Ru1 could catalyze the reduction of radicals in aqueous solution via a transfer hydrogenation-like process. Alkylation of N-(p-tolyl)-benzimidazole19 with bromoacetic acid20 afforded the NHC ligand precursor [1H2][Br] (Scheme 6). The desired Ag—NHC complex [Ag(1)]n (2) was obtained upon treatment of [1H2][Br] with Ag2O. Transfer of the NHC ligand from 2 to Ru was achieved upon reaction with [{RuCl(η6-cymene)}2(μ-Cl)2] to afford the Ru—NHC complex [RuCl(1)(η6-cymene)](Ru1).




Consistent with the loss of positive charge in the benzimidazole ring following deprotonation, the 1H NMR signal for the N—CH2—CO2 protons in 2 was upfield of the signal in [1H2][Br]. Whereas the N—CH2—CO2 protons in 2 displayed a singlet in the 1H NMR spectrum, the corresponding signal in Ru1 was an AB doublet, indicating that the two protons of the N—CH2—CO2 group were oriented in non-exchanging inequivalent magnetic environments due to the ligand chelate ring. Cyclic voltammetry of 1.0 mM Ru1 in CH2Cl2 containing 0.10 M [Bu4N][PF6] revealed no oxidation or reduction processes within the solvent window.
To probe the potential antioxidant activity of Ru1, 2,2′-azino-bis(3-ethylbenzothiazoline-6-sulfonate) radical monoanion (ABTS•−), which is stable in aerobic, protic media and undergoes reversible one-electron reduction to ABTS2−, was selected as the substrate for studies of catalytic radical reduction (Scheme 7). Investigations of potential radical degrading ability in biological environments often employ ABTS•− as the initial model substrate because its concentration can be readily measured by UV/visible spectroscopy at long wavelengths (λmax=750 nm in ethanol or 734 nm in phosphate buffered saline),23 but the non-radical dianion ABTS2−, formed upon one-electron reduction of ABTS•−, does not absorb above 400 nm. In addition, the large extinction coefficient for ABTS•− (ε750=1.6×104 M−1 cm−1 in EtOH and ε734=1.5×104 M−1 cm−1 in PBS) enables kinetic studies of radical-degrading and radical-forming reactions at concentrations more relevant to those encountered during oxidative stress. Furthermore, the oxidation of ABTS2− to ABTS•− occurs at a similar potential (0.67 V vs. Fc0/+) to the oxidation of H2O2 to O2 (E0′=0.70 V), thus, from a thermodynamic standpoint, ABTS•− will exhibit similar oxidizing radical reactivity to ROS encountered in biological systems.




As a non-catalytic control, Trolox (Scheme 8) was employed given its use as a benchmark in a variety of radical degradation and antioxidant studies.24 Trolox can serve as a 1e− or 2e− reductant, whereby the first 1e− oxidation is accompanied by rapid H+ loss to form a phenoxyl radical (TrO•), which can then undergo a second 1e− oxidation to form a phenoxonium cation (TrO+). In methanol (MeOH) or ethanol (EtOH) solutions, however, these processes converge into a single 2e− oxidation.25 Subsequent hydrolysis of TrO+ can then cleave the tertiary carbon-oxonium bond and thus render the 2e− oxidation of Trolox irreversible.




Because its electrochemistry and chemical reactivity have been thoroughly investigated, Trolox is routinely used as the baseline for the evaluation of other antioxidants. One comparison is the Trolox equivalent antioxidant capacity (TEAC) assay, in which the percent of ABTS•− degradation is plotted vs. antioxidant concentration and the slope of the linear fit for the antioxidant is divided by the slope similarly obtained for Trolox. However, the TEAC assay presupposes the antioxidant being studied degrades ABTS•− (i) in a dose-dependent or stoichiometric manner, (ii) by serving as the ultimate source of reducing equivalents, and (iii) reacting on a timescale similar to Trolox, presuppositions that would not be satisfied by some catalytic systems. For example, a compound that degrades ABTS•− catalytically could degrade 100% of the ABTS•− at all concentrations (i.e., is dose-independent). A linear fit of this data would have zero slope and thus afford a TEAC value of zero, leading to the contradictory determination that this catalyst had zero antioxidant capacity relative to Trolox despite the fact that it degraded 100% of the ABTS•− at all concentrations and Trolox did not. Because the TEAC assay may be unable to quantify the antioxidant capacity of some catalytic systems, traditional catalyst kinetic analyses are thus required.
Catalytic Reduction of ABTS•− to ABTS2− in EtOH
Addition of 5 μM Ru1 (DMSO stock) to 50 μM ABTS•− in EtOH caused a 100% decay in radical absorbance at 750 nm within 30 s (FIG. 12A, black line). Accompanying this degradation of 50 μM ABTS•− was an increase in absorbance at 340 nm corresponding to the formation of 50 μM ABTS2−, indicating 1:1 conversion of ABTS•− to ABTS2− by Ru1. Collectively, these results demonstrated that 5 μM Ru1 could achieve complete reduction of 50 μM ABTS•− (i.e., 10 turnovers). In the absence of Ru1, no ABTS•− degradation was observed in EtOH alone (FIG. 12A, dashed grey line), indicating that Ru1 catalyzed the reduction of ABTS•− to ABTS2− and was essential for reactivity. No ABTS•− formation was observed in an EtOH solution containing 5 μM Ru1 (DMSO stock) and 50 μM ABTS2−, even after extended periods of time, indicating that Ru1 does not oxidize ABTS2− to ABTS•− under these conditions and thus is unlikely to exert any pro-oxidant effects. The radical reducing activity of Ru1 was not limited to ABTS•−, and catalytic reduction of 2,2-diphenyl-1-picrylhydrazyl radical (DPPH•) to 1,1-diphenyl-2-picrylhydrazine (DPPH-H) in EtOH was also observed. In contrast to Ru1, the addition of 5 μM Trolox caused a rapid (within mixing time) decrease in the absorbance at 750 nm, but only by 20% (FIG. 12A, straight black line), corresponding to the reduction of 10 μM ABTS•− (2 equiv. vs Trolox) and consistent with the ability of Trolox to serve as a non-catalytic 2e− reductant in EtOH solution.25 
To assess its catalytic potential and corresponding regeneration, the reactivity of Ru1 with multiple sequential aliquots of excess ABTS•− was examined. After the reduction of 50 μM ABTS•− by 5 μM Ru1 (DMSO stock) was complete (FIG. 12B, black line), 5 additional 50 μM aliquots of ABTS•− were introduced, whereupon complete ABTS•− reduction occurred each time (FIG. 12B, grey line, 60 turnovers). Although the time required for complete degradation increased with each successive ABTS•− aliquot, 5 μM Ru1 nonetheless remained catalytically competent for the complete reduction of 500 μM ABTS•−. Rate law studies demonstrated that ABTS2− is an inhibitor for the Ru1-catalyzed reduction of ABTS•− (vide infra), thus the increase in time needed for complete degradation is caused by the fact that each successive ABTS•− aliquot is in the presence of a higher concentration of ABTS2− than the previous ABTS•− aliquot. Unlike Ru1, adding successive 10 μM aliquotst of ABTS•− after the initial reaction with 5 μM Trolox (FIG. 12C, black line) caused the absorbance at 750 nm to in increase (FIG. 12C, grey line) by amounts proportional to the concentration of ABTS•− added (i.e., 10 μM×1.6×104 M−1 cm−1), indicating that the antioxidant capacity of Trolox was exhausted upon reduction of 2 equiv. of ABTS•−. Together, these data demonstrate that Ru1 catalytically reduces radicals and, because it is regenerated after each reaction cycle, can degrade significantly more radicals than a non-catalytic antioxidant.
Although ABTS•− degradation has been previously observed with other ruthenium complexes,26-28 Ru1 is, to the best of our knowledge, the first with demonstrated catalytic activity. It is important to note that these previous studies measured the percentage of ABTS•− degradation as a function of Ru complex concentration (i.e., the TEAC assay approach). Interestingly, some reported absorbance vs. time plots displayed significantly slower ABTS•− degradation compared to Trolox and, notably, 100% ABTS•− degradation at multiple different Ru concentrations. Thus, it is entirely possible that one or more of the previously reported Ru complexes may have, in fact, degraded ABTS•− catalytically. Significantly slower reactivity compared to Trolox may have created the appearance that the total percentage of ABTS•− degraded by a Ru complex was dependent on the initial concentration of that complex and therefore led to the conclusion that radical degradation was non-catalytic.
As a catalyst for the 1e− reduction of ABTS•− to ABTS2−, Ru1 itself cannot serve as the terminal reductant for this reaction. Because the H2 for the transfer hydrogenation of C═O, C═N, and C═C bonds catalyzed by an organoruthenium complex is ultimately supplied by the non-tertiary alcohol solvent (e.g., Ru1 and i-PrOH),18 the electrons for the ABTS•− reduction experiments displayed in FIG. 12 most likely came from the EtOH solvent. To test this hypothesis and identify the chemical features required for terminal reductant function, it was first necessary to determine experimental conditions under which no ABTS•− degradation occurred in the presence of Ru1 alone.
Phosphate-buffered saline (PBS, pH 7.4) was selected as a suitable reaction medium because neither the solvent (H2O) nor the buffer components (Na2HPO4, KH2PO4, NaCl, KCl) were likely to undergo oxidation to supply the electrons necessary for the reduction of ABTS•− to ABTS2−. However, addition of 5 μM Ru1 (DMSO stock) to ABTS•− in PBS caused a gradual decay in radical absorbance at 734 nm, which indicated a suitable terminal reductant was present. Given that other radical scavenging assays have demonstrated that DMSO can function as a reductant,29 we concluded that the DMSO from the Ru1 stock solution was the most likely source of the reducing equivalents necessary for the reactivity. Addition of DMSO alone to ABTS•− in PBS produced no change in absorbance at 734 nm, again demonstrating that the reduction of ABTS•− to ABTS2− cannot occur without the catalyst Ru1.
To avoid the complications associated with redox active solvents, Ru1 stock solutions were thus prepared in CH3CN. No degradation of ABTS•− in PBS was observed after treatment with 5 μM Ru1 from a CH3CN stock (FIG. 13), indicating this solution lacked a suitable terminal reductant and confirming the prior determination that DMSO could provide reducing equivalents. Addition of 50 mM EtOH to 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− in PBS caused the absorbance at 734 nm to decrease (FIG. 13), thus confirming the hypothesis that the electrons necessary for the ABTS•− reduction observed in FIG. 12 were ultimately supplied by the EtOH solvent. Establishing experimental conditions under which no reaction occurred between the catalyst (Ru1) and substrate (ABTS•−) alone but did occur after the addition of EtOH provided the baseline necessary to study the catalyst kinetics and to gain insight into the mechanism for the reduction of ABTS•− to ABTS2−.
The synthesis of ABTS•− from ABTS2− does not proceed to 100% completion, thus any ABTS•− solution prepared will also inevitably contain a smaller amount of ABTS2−, the latter of which inhibits the Ru1-catalyzed reduction of ABTS•− to ABTS2− (vide infra). Furthermore, because the ratio of ABTS•− to ABTS2− is not constant from one synthetic batch to the next, the amount of inhibitor relative to catalyst will vary among the different experiments and thus cause significant variations in observed rates. Consequently, the standard protocol for the rate law studies entailed the addition of 100 μM ABTS2− (i.e., 20 equiv. relative to the typical 5 μM Ru1 concentration) to each experiment (with the exception of FIG. 4B) to minimize variations caused by inconstant ABTS2− to Ru1 ratios.
To PBS solutions containing 5 μM Ru1 (CH3CN stock), 100 μM ABTS2− and various initial concentrations of ABTS•− (5, 10, 25, 50 or 75 μM) was added 50 mM EtOH and the initial rates of ABTS•− degradation (v0) were measured for each experiment. The plot of v0 vs. [ABTS•−]0 revealed a linear correlation (FIG. 14A), which indicated that the Ru1-catalyzed reduction of ABTS•− was first-order in [ABTS•−] and that observed rate constants (kobs) could be obtained by plotting ln(A/A0) vs. t and performing linear regression.
Previous studies by others have shown that when a LnRu—Cl complex is added to H2O, the Cl− ligand is rapidly displaced to form the cationic aquo complex [LnRu(OH2)]1+. However, in a PBS solution containing ABTS•− and ABTS2−, there are multiple anionic species present that could conceivably have a higher affinity for [LnRu]1+ than H2O. During the initial studies of the Ru-catalyzed reduction of ABTS•− in PBS solutions (which did not contain the additional 100 μM ABTS2−), experiments performed under identical conditions yielded significantly different v0 values that could not be attributed to any known variable or impurity. Eventually, we hypothesized that, because each stock solution of ABTS•− unavoidably contained slightly different amounts of unoxidized ABTS2−, it was the attendant variation in the ABTS2−:Ru1 ratios among the different experiments that caused the variation in v0 values.
To test this hypothesis, 50 mM EtOH was added to solutions of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and various initial concentrations of extra ABTS2− (50, 100, 150 or 200 μM) in PBS and kobs values were measured for each experiment. Notably, kobs decreased as [ABTS2−]0 increased, which indicated that ABTS2− functioned as an inhibitor for the reaction. A linear correlation was observed in the plot of kobs vs. 1/[ABTS2−]0 (FIG. 14B), which suggested that ABTS2− dissociation from the Ru center was necessary for the catalytic reaction to proceed and confirmed our hypothesis that the minor differences in ABTS2− concentrations in the ABTS•− stock solutions caused significant variation in v0 values. Therefore, an extra 100 μM ABTS2− was added to each experiment performed in PBS, to ensure that the ABTS2−:Ru1 ratios were always ≧20 and relatively constant.
Because EtOH was essential for the Ru1-catalyzed reduction of ABTS•− to ABTS2−, it was next sought to determine the dependence of the reaction on EtOH concentration. To solutions of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− in PBS were added various initial concentrations of EtOH (10, 30, 50 or 70 mM), and the plot of kobs vs. [EtOH]0 revealed that the rate constant increased linearly with initial EtOH concentration (FIG. 14C). Because the addition of EtOH does not cause ABTS•− degradation in the absence of Ru1, the linear dependence of kobs on [EtOH]0 suggested that the coordination of EtOH to Ru was a necessary step to generating the catalytic intermediate that was competent for ABTS•− reduction.
Some [LnRu(OH2)]n+ complexes have been reported to undergo loss of H+ and conversion to hydroxo-bridged dimers of the form [(LnRu)2(μ-OH)](n−1)+, therefore it is conceivable that a similar transformation occurs upon addition of Ru1 to aqueous buffer. To elucidate the nuclearity of the catalytically-active species derived from Ru1, it was then analyzed the relationship between Ru1 concentration and ABTS•− reduction. To PBS solutions containing 50 μM ABTS•−, 100 μM ABTS2, and various initial concentrations of Ru1 (1, 2, 3, 4 or 5 μM; CH3CN stocks) was added 50 mM EtOH, and the kobs values measured increased linearly with increasing [Ru1]0 (FIG. 14D). If the predominant Ru-containing species in solution were multinuclear, such as [(LnRu)2(μ-OH)]1+ or [(LnRu)2(μ-O)], this species would need to dissociate an [LnRu]n+ subunit to generate a free coordination site to allow EtOH to bind, and kobs would thus depend on [Ru1]01/2 (if dimeric) or [Ru1]01/m (if a multinuclear species derived from m Ru1 subunits). However, because the observed rate constant depended linearly on [Ru1], the predominant Ru-containing species in solution leading up to the rate-determining step was most likely mononuclear. Furthermore, given that each experiment contained ≧20 equiv. ABTS2− for each molecule of Ru1 added and that ABTS2− dissociation was necessary for ABTS•− reduction to occur, it was concluded that the predominant Ru-containing species was a Ru-ABTS2− complex.
In a transfer hydrogenation catalytic cycle, the intermediate complex responsible for adding H2 to the unsaturated substrate (e.g., H2Rucat) is formed via removal of H+ and H− from the OH and CH groups, respectively, in the CH—OH moiety of a non-tertiary alcohol. Unlike transfer hydrogenation, however, the reduction of ABTS•− to ABTS2− will not be accompanied by H+ transfer to ABTS2−, therefore the buffer must absorb the 2 equiv. of H+ generated during each turnover. Therefore, the reaction rate for the Ru1-catalyzed reduction of ABTS•− to ABTS2− was expected to depend on the concentration of H+ in solution. To elucidate the relationship between [H+] and reaction rate, 50 mM EtOH was added to 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− in PBS solutions at various pH values (7.4, 7.9, 8.4 or 8.9), and ABTS•− reduction was faster at higher pH values. Notably, the linear correlation observed in the plot of kobs vs. 1/[H+] (FIG. 14E) indicated that a deprotonation reaction, in which H+ was transferred to the buffered aqueous solution, occurred before or during the rate-determining step of the catalytic cycle.
Given the results from the concentration studies, the Ru1-catalyzed reduction appeared to involve dissociation of H+ and ABTS2− from as well as association of EtOH to Ru, although not necessarily in that order, leading up to or during the rate-determining step. To gain greater insight into the nature of the transition state for the rate-determining step, it was next examined the temperature dependence of Ru1-catalyzed ABTS•− reduction. To PBS solutions of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− at various temperatures (15, 25, 35 or 45° C.) was added 50 mM EtOH, and the values of ln(kobs/T) were plotted against 1/T, which revealed a linear relationship (FIG. 14F). Using the linear form of the Eyring-Polanyi equation, the slope obtained from linear regression is equal to −ΔH‡/R and the y-intercept corresponds to ΔS‡/R+ln(kb/h). For the reduction of ABTS•− to ABTS2− catalyzed by Ru1, the values determined for ΔH‡ and ΔS‡ were 30.3±0.5 kcal mol−1 and 28.9±1.7 cal mo−1 K−1, respectively. The positive value for ΔS‡ revealed that the disorder in the system was increasing and thus suggested that dissociation of a ligand was occurring during the rate-determining step. In the transfer hydrogenation mechanism, the catalytically active metal-hydride species is formed when an alkoxide ligand undergoes β-hydride elimination and then the resulting aldehyde or ketone ligand dissociates from the metal, a process which increases the entropy of the system. Therefore, the positive value of ΔS‡ observed for the reduction of ABTS•− to ABTS2− catalyzed by Ru1 was consistent with the generation of a ruthenium-hydride species during the rate-determining step.
Based on the results from the rate law studies, it was concluded that a ruthenium-hydride complex derived from Ru1 was the species that reduced ABTS•−, and, without wishing to be bound to any particular theory, it is proposed that the catalytically active ruthenium-hydride complex is formed via a transfer hydrogenation-like mechanism. Addition of Ru1 to a PBS solution containing ABTS•− and ABTS2− results in rapid (with respect to turnover) substitution of the chloride ligand with ABTS2− to afford [LnRu-Ared]1− and begin the catalytic cycle (FIG. 15). In step 1, ABTS2− exchanges with H2O ligand to yield a cationic aquo complex [LnRu—OH2]1+, and the necessity of ABTS2− dissociation is demonstrated by the linear relationship between kobs and 1/[ABTS2−](i.e., FIG. 14B). Dissociation of H+ from [LnRu—OH2]+ to the buffer occurs in step 2 to produce a neutral hydroxo complex [LnRu—OH], which is supported by the inverse dependence of kobs on H+ concentration (i.e., FIG. 14E). The linear correlation between kobs and concentration of EtOH (i.e., FIG. 14C) suggests that EtOH coordinates to [LnRu—OH] in step 3 to afford [(LnRu—OH).EtOH]. Breakage of the O—H bond in the EtOH ligand then occurs via intramolecular H+ transfer to the hydroxo ligand and yields [(LnRu-OEt).H2O] in step 4. In step 5, the aquo ligand in [(LnRu-OEt).H2O] dissociates to form the alkoxide complex [LnRu-OEt]. Breakage of the carbinol C—H bond in the EtOH ligand then occurs via β-hydride elimination in step 6 to produce [(LnRu—H).MeC(═O)H], a ruthenium-hydride complex with an O-bound acetaldehyde. Subsequent dissociation of acetaldehyde in step 7 then affords the catalytically active ruthenium-hydride species [LnRu—H], which upon formation reacts with ABTS•− in 1:1 stoichiometry with rate constant kred, given that the rate of Ru1-catalyzed ABTS•− reduction is first-order in ABTS•− (i.e., FIG. 14A). Without wishing to be bound to any particular theory, it is proposed that [LnRu—H] undergoes one-electron oxidation upon reaction with 1 equiv. of ABTS•−, and the resulting Ru(III) species [LnRu—H]1+ undergoes deprotonation, accompanied by one-electron oxidation with a second equiv. of ABTS•−, and binding by the resulting ABTS2− to regenerate [LnRu-Ared]1− and restart the cycle.
An alternative pathway could be invoked in which [LnRu—H] transfers a hydride (H−) to an imine moiety in ABTS•− to afford H-ABTS•2− but the experimental data do not support this pathway. Inner-sphere H− transfer, for example, would first require ABTS•− to coordinate to [LnRu—H], but the rate law studies suggest that ABTS•− binding is not competitive with ABTS2−, which is also present in greater abundance (i.e., FIG. 14B). Any mechanism that involved H− transfer to an imine moiety in ABTS•− would create a charge-separated species with decreased radical delocalization, features that would render H-ABTS•2− significantly higher in energy than either ABTS•− or ABTS2−. Because such an endergonic reaction would likely be slower than the formation of [LnRu—H], subsequent H− transfer to ABTS•− would therefore be the rate-determining step. Once formed, H-ABTS•2− would then need to be oxidized by one equiv. of ABTS•−, and the rate of Ru1-catalyzed ABTS•− reduction would thus appear to be second-order in ABTS•− concentration: the rate-limiting formation of H-ABTS•2− would depend on [ABTS•−], and the reaction of H-ABTS•2− with ABTS•− would also depend on [ABTS•−]. Because the observed rate of Ru1-catalyzed ABTS•− reduction is instead first-order in [ABTS•−] (i.e., FIG. 14A), we can exclude hydride transfer to ABTS•− as a possible step in the catalytic cycle.
Compared to H− transfer from [LnRu—H] to ABTS•−, one-electron oxidation of [LnRu—H] by ABTS•− will likely have a lower activation energy and will thus occur before any hydride transfer could. Because the oxidation of [LnRu—H] by ABTS•− occurs after the rate-determining step, direct observation of the subsequent intermediates is not possible, but the steps proposed to complete the catalytic cycle are consistent with the known properties of organoruthenium-hydride complexes. One-electron oxidation of [LnRu—H] by ABTS•− will produce a cationic 17-electron Ru(III) complex, [LnRu—H]1+, that will function as an H+ source, not H−, and will be deprotonated in the pH 7.4 PBS. The resulting coordinatively unsaturated, neutral 17-electron Ru(I) species, [LnRu], will then be trapped by an additional ligand L′ from solution (e.g., H2O) to generate [LnRu-L′]. This 19-electron Ru(I) complex will be rapidly oxidized by ABTS•− to afford a cationic Ru(II) complex and ABTS2−, which will then combine to produce [LnRu-Ared]1− and complete the proposed catalytic cycle. Both the deprotonation of a ruthenium-hydride complex and generation of a radical, 19-electron Ru(I) species have significant literature precedent.
Tilset and Norton have shown that [RuH(η5-C5H5)(PPh3)2](M1red) undergoes one-electron oxidation at −0.34 V (vs. Fc0/+) to form M1ox, which has a pKa lower than M1red by 20-25 log units.30,31 Because the ABTS•−/ABTS2− redox couple occurs at +0.28 V,32 oxidation of M1red to M1ox by ABTS•− would be thermodynamically favorable. Tilset and Norton also noted that deprotonation of M1ox thermodynamically uphill by 4 pKa units would proceed if the resulting neutral, Ru(I) conjugate base (M2red) could subsequently be irreversibly oxidized. Because one-electron reduction of M2ox to M2red occurs at −2.42 V,30 even a weak oxidant, such as [Co(η5-C5Me5)2]1+ (E1/2=−1.91 V),33 would be able to convert M2red to M2ox and thus facilitate the deprotonation of M1ox.
Compared to an (η5-C5H5)1− ligand, μ6-cymene is less electron-donating, thus the oxidation of [LnRu—H] will likely occur at a higher potential than M1red. Similar to [LnRu—H], M3red is a Ru-hydride complex containing an η6-cymene ligand, and electrochemical analysis revealed M3red underwent irreversible oxidation to M3ox at −0.24 V.34 Although the oxidation of M3red occurred at a potential 100 mV higher than M1red, the value was still well below the ABTS•−/ABTS2− redox couple. Because the difference in oxidation potentials between [LnRu—H] and M3red is likely smaller than the difference between M3red and M1red, ABTS•− should be a sufficiently strong oxidant to be reduced by [LnRu—H] and afford ABTS2− and [LnRu—H]1+.
An extensive compendium of pKa values for Ru-hydride complexes have been measured, but there are fewer values available for cationic arene-Ru-hydride complexes. The complex most similar to [LnRu—H]1+ for which a pKa value has been reported is [RuH(bpy)(η6-C6Me6)]1+ (M4red, pKa=22.5±0.1 in CH3CN)35 and, using the method developed by Morris to estimate acidity in different solvents,36 the pKa for M4red in H2O can be estimated at 15.9. Little deprotonation of M4red would occur in pH 7.4 buffer, but the pKa for [LnRu—H]1+ will be significantly lower than M4red given that the former contains Ru(III), whereas the latter contains Ru(II). A more relevant insight into the acidity of [LnRu—H]1+ would be the pKa for the one-electron oxidized Ru(III) species M4ox. Using the observations of Tilset and Norton that one-electron oxidation lowers the pKa of a Ru-hydride complex by 20-25 units,30,31 the pKa for M4ox in H2O can be estimated in the range of −4.1 to −9.1. Similarly drastic increases in acidity occur upon one-electron oxidation of [RuH(μ5-C5H5)(CO)(PPh3)] (pKa decreases to 4-5 from 27-28)37 and [WH(η5-C5H5)(CO)2] (pKa decreases to −3 from 16).38 
Collectively, the results from the rate law studies suggested that [LnRu—H] was the catalytically active species for the reduction of ABTS•− to ABTS2− and was formed via rate-determining β-hydride elimination from a Ru-ethoxide species. Based on the oxidation potentials for similar Ru-hydride complexes in the literature, ABTS•− will be a sufficiently potent oxidant to oxidize [LnRu—H] to [LnRu—H]1+. Similarly, the pKa values for previously-reported neutral and cationic Ru(II) and Ru(III) hydrides suggested that pH 7.4 buffer will be sufficiently basic to deprotonate [LnRu—H]1+ and yield a neutral Ru(I) species. Subsequent oxidation by ABTS•− will be even more favorable than [LnRu—H] for this Ru(I) intermediate, and the resulting Ru(II) complex and ABTS2− formed then combine to regenerate [LnRu-Ared]1− and complete the catalytic cycle.
In the proposed mechanism, the key reducing species [LnRu—H] is generated via β-hydride elimination from an alkoxide ligand, therefore both the O—H and C—H groups in the CH—OH moiety may be a factor for reactivity. To test this hypothesis, a series of other molecules comprising (or lacking) these groups were then assayed to confirm the necessity of both for terminal reductant functionality. Addition of 50 mM i-PrOH, which comprises a CH—OH moiety, to a solution of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− in PBS caused the absorbance at 734 nm to decay with an observed rate constant statistically similar to that measured with EtOH (kiPrOH=8.92±1.96×10−4 s−1 vs. kEtOH=8.21±1.14×10−4 s−1; FIG. 16). When 50 mM MeOH was added instead, the radical absorbance decreased significantly more slowly (kMeOH=2.49±0.29×10−4 s−1) than with either EtOH or i-PrOH, but nonetheless faster than uncatalyzed ABTS•− thermal decomposition.
The addition of varying concentrations of acetone (25, 50, 75, 100 mM) before the addition of 50 mM i-PrOH had no effect on the reaction rate. Because β-hydride elimination from a Ru-isopropoxide species (i.e., step 6, FIG. 15) would generate a Ru—H complex with an O-bound acetone ligand, and acetone dissociation must occur to form the catalytically active reducing species [LnRu—H] (i.e., step 7, FIG. 15), the concentration of acetone could have an impact on the reaction rate. However, because no change in reaction rate was observed when acetone was added before i-PrOH, it would appear that the dissociation of O-bound acetone occurs after the rate-determining step. It is therefore concluded that β-hydride elimination (i.e., step 6, FIG. 15) is the rate-determining step.
Unlike the non-tertiary alcohols MeOH, EtOH and i-PrOH, t-BuOH lacks the C—H group of a CH—OH moiety and should therefore be unable to generate the Ru—H intermediate essential for ABTS•− reduction (i.e., step 6, FIG. 15). In confirmation of this expectation, the addition of 50 mM t-BuOH to a PBS solution containing 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− afforded no change in radical absorbance (FIG. 17, i). Subsequent addition of 50 mM EtOH (FIG. 17, ii) caused ABTS•− reduction to occur with the same rate constant as with EtOH alone (i.e., FIG. 16), which demonstrated that the absence of reactivity observed with t-BuOH was not due to catalyst deactivation but rather the inability of t-BuOH to undergo β-hydride elimination (i.e., step 6, FIG. 15) and form [LnRu—H].
Ethylene glycol (EG) and 1,2-dimethoxyethane (DME) were then assayed to elucidate the importance of the O—H group in the CH—OH moiety in Ru1-catalyzed ABTS•− reduction. Consistent with the results using EtOH and i-PrOH, addition of 50 mM EG to a solution of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− in PBS caused the absorbance at 734 nm to decrease, with an observed rate constant (kEG=5.61±0.73×10−4 s−1) slower than EtOH or i-PrOH, but not significantly so given the standard deviations (FIG. 16). In contrast, the addition of 50 mM DME to a PBS solution of 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− did not afford any radical degradation, which indicated that the O—H group in the CH—OH moiety was essential for terminal reductant functionality. Without this O—H group, DME cannot form the Ru-alkoxide species (i.e., step 4, FIG. 15) that precedes β-hydride elimination (i.e., step 6, FIG. 15) and, furthermore, renders β-hydride elimination energetically inaccessible as it would result in the formation of an O-methylated aldehyde with a formal positive charge on the oxygen that would also be coordinated to Ru with its last remaining electron pair. Clearly, both the C—H and O—H groups of a CH—OH moiety are necessary for terminal reductant function.







TABLE 4







Activation parameters for Ru1-catalyzed ABTS•− reduction with 


various terminal reductants












ΔH†
ΔS‡
Ea
ln(A)





EtOH
30.3 ± 0.5
28.9 ± 1.7
30.9 ± 0.5
45.0 ± 0.9


i-PrOH
31.2 ± 0.7
32.2 ± 2.3
31.8 ± 0.7
46.7 ± 1.1


EG
31.7 ± 0.6
32.8 ± 2.1
32.3 ± 0.6 
47.0 ± 1.0


MeOH
25.8 ± 0.9
11.4 ± 2.9
26.4 ± 0.9
36.2 ± 1.5





Values reported as the average ± standard deviation of 4 experiments performed on 4 different days with units of 10−5 s−1. Protio and deutero alcohol stock solutions (5M) were prepared in H2O and D2O to match the buffered solution for the experiment.






For the alcohols that did enable Ru1-catalyzed ABTS•− reduction (i.e., EtOH, i-PrOH, MeOH, and EG), potential origins of their differing observed rate constants were explored. Therefore, values of kobs were obtained via addition of 50 mM alcohol (EtOH, i-PrOH, MeOH, or EG) to PBS solutions containing 5 μM Ru1 (CH3CN stock), 50 μM ABTS•− and 100 μM ABTS2− at various temperatures (15, 25, 35 or 45° C.). Plotting ln(kobs/T) and ln(kobs) vs. 1/T enabled use of the linear forms of the Eyring-Polanyi and Arrhenius equations, respectively, to determine the values of ΔH‡, ΔS‡, Ea and ln(A) (where Ea and A correspond to the activation energy and pre-exponential factor in units of kcal mol−1 and s−1, respectively), which are listed in Table 4.
The Ru1-catalyzed reduction of ABTS•− in the presence of each non-tertiary alcohol exhibited a positive value for ΔS‡, which would be expected if β-hydride elimination were occurring from a Ru-alkoxide species via a process similar to EtOH (i.e., step 6, FIG. 15). Consistent with the nearly identical values of kobs measured for EtOH and i-PrOH, each of the parameters (ΔH‡, ΔS‡, Ea and ln(A)) calculated for EtOH and i-PrOH were statistically indistinguishable. Similarly, the slightly (but still statistically significant) slower reactivity observed with EG vs. EtOH was reflected by the slightly higher ΔH‡ (31.7±0.6 kcal mol−1) and Ea (32.3±0.6 kcal mol−1) values for EG compared to EtOH (ΔH‡=30.5±0.6 kcal mol−1 and Ea=30.9±0.5 kcal mol−1). Although MeOH afforded exhibited the lowest ΔH‡ and Ea values of all the non-tertiary alcohols tested, it afforded the slowest ABTS•− reduction, possibly because ΔS‡ and Ea were the least favorable. Ultimately, the usefulness of comparing the different transition state or activation parameters is limited by the fact that substitution of one non-tertiary alcohol for another will impact multiple steps in the catalytic cycle and in multiple ways, particularly steps 4 and 6.







TABLE 5







Activation parameters for Ru1-catalyzed ABTS•− reduction with 


various terminal reductants













pKa
Ka
ΔGr°
Kr
Ka × Kr





EtOH
15.9 
1.26 × 10−16
7.27
4.71 × 10−6 
5.93 × 10−22


i-PrOH
16.5 
3.16 × 10−17
4.96
2.33 × 10−4 
7.37 × 10−21


EG
14.22
6.03 × 10−15
12.8
4.30 × 10−10
2.59 × 10−24


MeOH
15.5 
3.16 × 10−16
14.3
3.57 × 10−11
1.13 × 10−26





Units for Ka, Kr, Ka × Kr are M, M, M2 and kcal mol−1, respectively. Values for ΔGr° calculated using the formula ΔGr° = ΔHr° − TΔSr° for the dehydrogenation of R1—CHOH—R2 to R1—C(═O)—R2) + 1⁄2 H2. Values for ΔHr° and ΔSr° estimated from the equations ΔHr° = ΔHf°(R1—C(═O)—R2) − ΔHr°(R1—CHOH—R2) and ΔSr° = 1⁄2 S°(H2) + S°(R1—C(═O)—R2) − S°(R1—CHOH—R2) for reported as the average ± standard deviation of 4 experiments performed on 4 different days with units of 10−s s−1. Protio and deutero alcohol stock solutions (5M) were prepared in H2O and D2O to match the buffered solution for the experiment.






Increasing the acidity of the O—H proton in a non-tertiary alcohol will render the intramolecular deprotonation in step 4 more thermodynamically favorable and thus the corresponding equilibrium constant in step 4 (K4) will be larger. Conversely, a thermodynamically more favorable alcohol dehydrogenation will make the corresponding equilibrium constant in step 6 (K6) larger. Based on the published pKa and ΔGr∘ values for the non-tertiary alcohols, the product of the corresponding Ka and Kr values gives a relative ordering that is consistent with the observed rate constants presented in FIG. 16 (Table 5).
Intramolecular proton transfer from the OH Considering only Ea, MeOH would be expected to afford the fastest reactivity, but the ln(A) for MeOH is nearly 10 units lower than the other alcohols investigated, which indicated that the pre-exponential factor was dominant, similar to the behavior observed with i-PrOH. The relative ordering of the ΔH‡ and Ea values for MeOH<EtOH<i-PrOH matches the trend for the enthalpy of dehydrogenation,39 in which the formation of formaldehyde is more unfavorable than the formation of acetaldehyde, which is in turn more unfavorable than the formation of acetone.
Collectively, the results from the terminal reductant assay demonstrate that both the OH and CH groups of the CH—OH moiety in a non-tertiary alcohol are necessary for the conversion of ABTS•− to ABTS2− by Ru1. These factors reflect the fact that the catalytically active reducing species [LnRu—H] must be formed via β-hydride elimination from the carbinol position of a metal-bound alkoxide ligand. An alcohol lacking a carbinol C—H group cannot undergo β-hydride elimination because it lacks a β-hydrogen, and a molecule lacking an O—H group cannot form the necessary alkoxide precursor for β-hydride elimination to occur.
To confirm that breakage of the C—H and O—H bonds in the CH—OH moiety of a non-tertiary alcohol was occurring during or before the rate-determining step of the catalytic reduction of ABTS•− by Ru1, rate constants were measured using a combination of protio and deutero EtOH and i-PrOH in protio and deutero PBS, the results of which are listed in Table 6. By performing measurements using protio alcohols in deutero PBS and deutero alcohols in protio PBS, it was possible to generate the mixed isotope CH—OD and CD-OH alcohols, respectively. With both EtOH and i-PrOH, significantly slower ABTS•− reduction was observed upon substitution of either the C—H or O—H group with C-D or O-D, and the doubly substituted CD-OD alcohols afforded the slowest reactivity.







TABLE 6







Observed rate constants for Ru1-catalyzed ABTS•− reduction with 


protio and deutero alcohols in protio and deutero PBS










PBS (H2O)
PBS (D2O)





EtOH
6.69 ± 0.73
1.31 ± 0.11


EtOH-d6
1.33 ± 0.22
0.454 ± 0.020


i-PrOH
9.43 ± 1.26
1.31 ± 0.12


i-PrOH-d8
1.92 ± 0.26
0.457 ± 0.024





Values reported as the average ± standard deviation of 4 experiments performed on 4 different days with units of 10−5 s−1. Protio and deutero alcohol stock solutions (5M) were prepared in H2O and D2O to match the buffered solution for the experiment.






Quantifying the effect of the C—H/C-D and O—H/O-D bond substitutions could be achieved by examining the ratios of the observed rate constants (Table 7). Although these ratios would normally correspond to the kinetic isotope effects of the deuterium substitution, it will be shown that an additional factor is present that must be abstracted to obtain the true values. Replacing the C—H (but not the O—H) bond with C-D results in a reaction that is 5.05±1.02 times slower with EtOH and 4.93±0.93 times slower with i-PrOH in protio PBS. However, when the same substitution was performed in deutero PBS, the kobs values for EtOH and i-PrOH were 2.88±0.27 and 2.86±0.31 times slower, respectively, for the C-D compared to C—H alcohols. Because these two sets of experiments involved the same C—H for C-D bond substitution, without changing the O—H or O-D groups, their results should have been statistically similar.







TABLE 7







Ratio of observed rate constants based on C—H/C—D and 


O—H/O—D isotopic substitution in protio and deutero PBS.










X = H
X = D





CH3CH2OX/
5.05 ± 1.02
2.88 ± 0.27


CD3CD2OX




(C—H/C—D for




EtOH)




(CH3)2CHOX/
4.93 ± 0.93
2.86 ± 0.31


(CD3)2CDOX




(C—H/C—D for 




i-PrOH)




CX3CX2OH/
5.13 ± 0.71
2.92 ± 0.51


CX3CX2OD




(O—H/O—D for




EtOH)




(CX3)2CXOH/
7.21 ± 1.18
4.18 ± 0.60


(CX3)2CXOD




(O—H/O—D for 




i-PrOH)





Values reported as the average ± standard deviation.






Similar behavior was observed in the O—H/O-D substitution results. Replacing the O—H bond in the all-protio EtOH and i-PrOH with O-D caused ABTS•− reduction to occur 5.13±0.71 and 7.21±1.18 times more slowly, respectively. However, replacing the O-D bond in EtOH-d6 or i-PrOH-d8 with O—H increased the respective kobs values by a factor of 2.92±0.51 or 4.18±0.60. These two sets of experiments should have given statistically similar results, given that they involved the same O—H for O-D bond substitution without changing the C—H or C-D groups. Notably, the C—H/C-D and O—H/O-D ratios were greater when comparing a value obtained in protio PBS to a value obtained in deutero PBS, which indicated that the solvent played an important role in the reaction mechanism. Many of the steps in the proposed mechanism (FIG. 15) involve H2O: displacement of ABTS2− by H2O in step 1, deprotonation of the H2O coordinated to Ru in step 2, intramolecular H+ transfer from the Ru-bound EtOH to hydroxide in step 4, and dissociation of H2O to generate an open coordination site necessary for β-hydride elimination in step 5. Replacing H2O with D2O would affect the equilibrium constants for each of these steps, thus it is unsurprising that a substantial solvent isotope effect would be observed for Ru1-catalayzed reduction of ABTS•− with non-tertiary alcohols.







TABLE 8







Kinetic isotope effects.









KIE
EtOH
i-PrOH





solvent
1.76 ± 0.39
1.72 ± 0.37


C—H
2.88 ± 0.27 
2.86 ± 0.31


O—H
2.92 ± 0.51
4.18 ± 0.60


C—H × O—H
8.41 ± 1.67
11.98 ± 2.14 


CH—OH in H2O/
14.7 ± 1.7 
20.6 ± 3.0 


CD—OD in D2O









Dividing each C—H/C-D ratio obtained in protio PBS by the corresponding ratio obtained in deutero PBS enabled calculation of the solvent isotope effects, which were 1.76±0.39 in the EtOH experiments and 1.72±0.37 in the i-PrOH experiments (Table 8). The fact that these numbers were similar for the independently performed EtOH and i-PrOH experiments supported their assignment as solvent isotope effects rather than some other unidentified experimental phenomenon. Having calculated the solvent isotope effect values, it was then possible to determine the kinetic isotope effects for deuterium substitution of the individual C—H and O—H groups in the CH—OH moieties in EtOH (2.88±0.27 and 2.92±0.51, respectively) and i-PrOH (2.86±0.31 and 4.18±0.60, respectively), values which were unambiguous for primary kinetic isotope effects,40 which indicated that C—H or O—H bond breakage occurred before or during the rate determining step.
The C—H/C-D kinetic isotope effect value determined for i-PrOH in the Ru1-catalyzed reduction of ABTS•− (2.86±0.31) was identical to the corresponding C—H/C-D value reported by Casey (2.86±0.20) for H2 transfer from i-PrOH to [Ru(S,S-TsDPEN)(η6-cymene)].41 A comparable C—H/C-D value (2.57±0.26) was observed by Bäckvall for the transfer of H2 from 1-(4-fluorophenyl)ethanol to another organoruthenium complex similar to Ru1 and [Ru(S,S-TsDPEN)(η6-cymene)].42 The C—H/C-D kinetic isotope effect value for EtOH in Ru1-catalyzed reduction of ABTS•− (2.88±0.27) was statistically indistinguishable from i-PrOH and consistent with the findings by Casey and Bäckvall.
The catalytic reduction of ABTS•− by Ru1 exhibited significantly larger O—H/O-D kinetic isotope effect values for i-PrOH (4.18±0.60) and EtOH (2.92±0.51) than O—H/O-D kinetic isotope effect values reported by Casey (1.79±0.07) and Bäckvall (1.87±0.17) with transfer hydrogenation reactions catalyzed by organoruthenium complexes. One possible explanation for such a large difference is that ABTS•− reduction by Ru1 and a non-tertiary alcohol formally involved ionic H+ transfer from the O—H group to the Ru-bound hydroxide in a distinct step, whereas the systems studied by Casey and Bäckvall proceeded via concerted H2 transfer from the non-tertiary alcohol CH—OH moiety to the catalyst. The difference between the O—H/O-D values for EtOH and i-PrOH during Ru1-catalyzed ABTS•− reduction (2.92±0.51 vs. 4.18±0.60, respectively) could be a consequence of the greater acidity of EtOH compared to i-PrOH (pKa=15.9 vs. 16.5, respectively), and the lower activation barrier this would produce for EtOH would render the ionic O—H bond breakage less sensitive to substitution with deuterium.
Having obtained unambiguous evidence that Ru1 catalyzes radical degradation, it was then sought to ascertain if Ru1 could also inhibit radical formation. Horseradish peroxidase (HRP) converts H2O2 to 2 equiv. of H2O via HO•, with concomitant consumption of 2e− and 2H+ in each turnover. Because ABTS2− can serve as a 1e− reductant in this reaction, the rate of radical formation can be quantified by measuring the absorbance of ABTS•− vs. time.43 Addition of 10 μM H2O2 to a PBS solution of 5 μM Ru1 (DMSO stock), 10 nM HRP and 50 μM ABTS2− caused the absorbance at 734 nm to increase, with an initial rate of ABTS•− formation (v0) of 2.17±0.35×10−8 M s−1 (FIG. 18A, grey line), but significantly more slowly than with HRP alone (v0=3.69±0.14×10−8 M s−1). After 12.8±0.7 min, the concentration of ABTS•− peaked at 8.71±0.55 μM and then began to decrease, indicating that radical degradation overtook radical formation, at an initial rate of decay (v0′) of 5.06±0.26×10−9 M s−1, which led to complete radical degradation within 60 min. To determine if the decreased rate of ABTS•− formation observed with Ru1 was caused by DMSO from the stock solution, 10 M H2O2 was added to 10 nM HRP and 50 μM ABTS2− in PBS containing 1% DMSO (same as 30 μL aliquot from Ru1 stock solution), resulting in a slightly slower rate of ABTS•− formation (v0=3.24±0.11×10−8 M s−1) than HRP alone. Because DMSO only slightly inhibited the rate of ABTS•− formation and nonetheless permitted complete oxidation of ABTS2−, the significantly lower value of v0 and the final ABTS•− concentration of zero observed in the presence of Ru1 can be attributed to the radical reducing ability of Ru1 and not DMSO from the stock solution.
In contrast to the experiments with Ru1, the addition of 10 μM H2O2 to a PBS solution of 5 μM Trolox (DMSO stock), 10 nM HRP and 50 μM ABTS2− resulted in no change in absorbance at 734 nm for the first 4.2±0.4 min, indicating that Trolox completely halted ABTS•− formation (FIG. 18A, black line). After 4.2±0.4 min, however, the absorbance at 734 nm began to increase with v0=3.44±0.11×10−8 M s−1 and ABTS•−=concentration reached a maximum of 15.06±0.04 μM at t=22.0±0.5 min (i.e., 75% net oxidation of ABTS2−; the subsequent decline is due to normal ABTS•− thermal decay). The fact that only 75% of the initial 20 μM ABTS2− was oxidized in the presence of 5 μM Trolox indicates that Trolox is consuming 5 μM HO• formed by HRP. Although Trolox functions as a 2e− reductant in EtOH solution (c.f. FIG. 13), it is because the first and second 1e− oxidations occur effectively in one step.25 In basic solutions (e.g., buffered aqueous media), TrO• is thermodynamically stable44 and the second 1e− oxidation to TrO+ is well-separated from the first.25 Interestingly, the initial rate of ABTS•− formation in the presence of Trolox is not statistically significantly different from the rate measured in the presence of DMSO or HRP alone, indicating that no inhibition of ABTS•− formation occurred after 4.2 min and demonstrating that the antioxidant capacity of Trolox had been exhausted.
To determine if Ru1 remained catalytically competent after the complete reduction of ABTS•− formed by 10 nM HRP and 10 μM H2O2 (FIG. 18B), two additional 10 μM aliquots of H2O2 were introduced. Addition of the second 10 μM aliquot of H2O2 caused the absorbance at 734 nm to increase (v0=2.06×10−8 M s−1; FIG. 18B) to a maximum ABTS•− concentration of 7.73 μM at 14.8 min, followed by a decrease (v0′=4.85×10−9 M s−1) that led to complete radical reduction 66.7 min after the peak. Similarly, the third 10 μM aliquot of H2O2 resulted in ABTS•− formation (v0=1.83×10−8 M s−1; FIG. 18B) that reached a maximum at 17.3 min (7.73 μM) before decreasing (v0′=4.26×10−9 M s−1) and resulting in complete reduction 66.5 min later.
Because the values measured for the initial rate of ABTS•− formation, time to peak absorbance, maximum ABTS•− concentration, initial rate of ABTS•− reduction and final ABTS•− concentration (i.e., zero) were highly conserved among the three sequential 10 μM H2O2 aliquots, it is evident that the ability of Ru1 to inhibit the formation of and catalyze the degradation of radicals is retained throughout the course of the experiment. Moreover, adding multiple sequential H2O2 aliquots confirmed the hypothesis that the decrease in absorbance at 734 nm was due to the reduction of ABTS•− to ABTS2− rather than some other chemical reaction.
Chemically synthesized ABTS•− aliquots were added in a similar manner to obtain greater insight into the ability of Ru1 to degrade vs. inhibit the formation of radicals. After the ABTS•− formed by 10 nM HRP and 10 μM H2O2 was completely reduced by Ru1 (FIG. 18C), a 10 μM aliquot of chemically synthesized ABTS•− was added (immediately increasing absorbance at 734 nm) that began to decay (v0′=3.41×10−9 M s−1) and complete reduction was attained within 95.7 min (FIG. 18C). Similarly, the second 10 μM aliquot of ABTS•− underwent reduction (v0′=3.55×10−9 M s−1) that was complete 96.5 min later (FIG. 18C). Initial rates of decay and times to complete reduction with chemically synthesized ABTS•− were slower than with H2O2, possibly because the ABTS2− concentration increased with each added aliquot in the former experiment but was constant throughout the latter.
An organoruthenium complex supported by a chelating anionic N-heterocyclic carbene ligand, Ru1, catalyzed the reduction of ABTS•− to ABTS2− in EtOH with 100 turnovers. No reduction of ABTS•− was observed in PBS, providing evidence that Ru1 itself cannot provide the necessary reducing equivalents. Subsequent addition of a non-tertiary alcohol (R1—CHOH—R2), however, caused ABTS•− reduction, with both the C—H and the O—H groups of the —CHOH— moiety being necessary to function as a terminal reductant.
Substitution of R1—CHOH—R2 with R1—CDOD-R2 significantly decreased the observed reaction rate constants, with corresponding primary kinetic isotope effect values consistent with concerted H2 transfer from the non-tertiary alcohol to the Ru complex in the rate-determining step. Furthermore, the values obtained with Ru1 closely match those previously reported from mechanistic studies of transfer hydrogenation reactions catalyzed by other organoruthenium complexes. In addition, Ru1 inhibited the oxidation of ABTS2− to ABTS•− by HO• and then reduced all of the ABTS•− formed, demonstrating that Ru1 can inhibit the formation of radicals as well as catalyze their degradation. Collectively, our findings unambiguously demonstrate that transfer hydrogenation catalytic activity can be harnessed for the reduction of radicals in aqueous solution using a variety of non-tertiary alcohols as the terminal electron sources.
Example 4
Experiments were performed to determine if covalent incorporation of an AIM into an organic polymer or inorganic material would endow that AIM with the ability to catalytically degrade radicals. Complexes Ru5 and Ru8 were thus prepared, using the procedure developed for Ru2,19 to obtain suitable starting materials that could be derivatized with the functional groups necessary for covalent incorporation into SiO2 and PMMA, respectively (FIG. 19). Hydrolysis of the CO2Me groups in Ru5 to produce Ru6 was followed by amide coupling with 3-aminopropyltriethoxysilane (APTES)48 to yield Ru7, which was then affixed49 to the surface of SiO2 microspheres (1.5 μm, Corpuscular Inc.) to afford Ru7-SiO2, the desired SRAC-functionalized inorganic material. Scanning electron microscopy (SEM) revealed that the average diameter and surface roughness of Ru7-SiO2 were not significantly different from the unfunctionalized microspheres, demonstrating that the material properties of SiO2 were not adversely affected by incorporation of Ru7. Sonogashira coupling of N-methacroyl-4-ethynylaniline50 to Ru8 yielded Ru9, which was then polymerized with methylmethacrylate (MMA)51 to produce Ru9-PMMA (Mn=24.2 kDa, PDI=2.6), the desired SRAC-functionalized organic polymer. Atomic force microscopy (AFM) of thin films (spin-cast from 10 mg mL−1 solutions in THF) of Ru9-PMMA and PMMA (prepared in the absence of Ru9) revealed nearly identical film thickness and surface roughness values, indicating that Ru9 did not interfere with the polymerization of MMA. Diffuse reflectance and film transmission UV/vis spectra of Ru7-SiO2 and Ru9-PMMA displayed peaks at 523 nm and 565 nm, respectively, which were similar to the values observed with Ru7 and Ru9. These observations provided evidence that the Ru—NHC complexes had been incorporated into SiO2 and PMMA without significant changes in electronic properties or coordination chemistry, consistent with other studies involving the covalent incorporation of Ru—NHC complexes into SiO2 and PMMA.52,53 No degradation of chemically-synthesized ABTS•− in PBS solutions containing Ru7-SiO2 or Ru9-PMMA, but subsequent addition of EtOH did cause the absorbance at 734 nm to decrease linearly (kobs=5.7 and 4.9×10−8 M s−1 for Ru7-SiO2 and Ru9-PMMA, respectively), indicating that these materials gained the ability to catalytically reduce ABTS•− via the covalent incorporation of SRACs.
After determining the general strategy of endowing an AIM with the ability to catalytically degrade radicals by covalently incorporating an SRAC was feasible, we then sought to obtain preliminary evidence that SRAC activity could be retained on an AIM exposed to RAW 264.7 macrophage cell culture (DMEM, 10% FBS, 1% penicillin/streptomycin, 5% humidified CO2, 37° C.) in collaboration with Dr. Nilofer Qureshi (UMKC, letter provided). Because ABTS•− itself was unstable in DMEM and all other cell culture media tested, direct measurement of the ABTS•− degrading activity of SRAC-AIMs in cellular environments was impossible. Thus, a method was needed to physically separate SRAC-AIMs from cellular environments to enable transfer to PBS. Reaction of Ru7 with SiO2-coated magnetic microspheres (SiO2@MM, 1.5 μm, Corpuscular Inc.) afforded Ru7-SiO2@MM, an SRAC-AIM which could be separated from cell cultures by using a magnet. Next, Ru7-SiO2@MM was added to RAW 264.7 cell culture, magnetically separated after 24 h, then washed with DMEM and PBS. The ability of Ru7-SiO2@MM to catalyze ABTS•− reduction in PBS (using EtOH as the terminal reductant) was retained after the 24 h exposure to the RAW 264.7 cell culture (5.2 and 4.8×10−8 M s−1 before and after, respectively).
The results demonstrate that our Ru—NHC complexes catalyze radical reduction and inhibit their formation by ROS through a transfer hydrogenation-like process. Other Ru complexes have been reported to be cytotoxic or cause ROS formation,54-56 but neither behavior was observed with our Ru—NHC complexes. No ABTS•− formation was observed upon addition of H2O2 to Ru1 or Ru2 and ABTS2−, providing evidence that Ru1 and Ru2 do not generate ROS. Treatment of RAW 264.7 cells with up to 100 μM Ru1 or Ru2 for 24 h resulted in no loss of cell viability (measured via the MTT assay), indicating that Ru1 and Ru2 are not cytotoxic. A recent study suggested that Ru—NHC complexes may be selectively cytotoxic to some cell types, which could explain the different behaviors reported in the literature.57 Collectively, the results confirm the feasibility of our proposed approach.
Example 5
Triethoxysilane groups such as those found in Ru7 readily react with surface hydroxyl groups on inorganic oxides to eliminate EtOH and form new Si—O bonds, therefore Ru7 will be covalently incorporated into TiO2 and hydroxyapatite,61,62 similar to Ru7-SiO2 (see Example 4). Surface functionalization of titanium63 and stainless steel64 with oxide and hydroxide groups will thus enable covalent incorporation of Ru7 by this approach as well. Although SRAC-functionalized PMMA (e.g. Ru9-PMMA) can be prepared by building a Ru—NHC complex into a monomer (e.g. Ru9) and then polymerizing MMA in its presence, this approach may be impractical for some polymers. Alternatively, amide coupling48 of propargyl amine to Ru6 will produce an SRAC with a C≡C—H group, which can then undergo Cu-catalyzed alkyne-azide coupling65 with azide-functionalized polyethylene (PE), polypropylene (PP) or PTFE to afford an AIM with a triazole linked SRAC (FIG. 20). Hydroxy-functionalized PE, PP and PTFE will be reacted with MeSO3Cl followed by NaN3 to access the desired azide-functionalized polymers.66 
The foregoing is illustrative of the present invention, and is not to be construed as limiting thereof. The invention is defined by the following claims, with equivalents of the claims to be included therein. All publications, patent applications, patents, patent publications, and other references cited herein are incorporated by reference in their entireties for the teachings relevant to the sentence and/or paragraph in which the reference is presented.

## Claims

1. A compound represented by one of the following structures:






each R is independently a hydrogen, substituted or unsubstituted alkyl group, or a substituted or unsubstituted aryl group, wherein the substituted alkyl group or the substituted aryl group are substituted with a substituent selected from the group consisting of an alkyl group, alkenyl group, alkynyl group, halogen atom, carbonyl-containing functional group, aryl group, heterocyle, alcohol, thiol, amine, ether, thioether, azide, and any combination thereof;
X is a non-coordinating anion;
n is an integer from 1 to 30; and
m is an integer from 1 to 30;
and/or a derivative thereof.

2. The compound of claim 1, wherein R in each occurrence is hydrogen.

3. A biomedical implant material comprising the compound of claim 1, wherein the compound is present on at least a portion of a surface of the biomedical implant material.

4. The biomedical implant material of claim 3, wherein the compound degrades a radical and/or reactive oxygen species (ROS) catalytically.

5. The biomedical implant material of claim 4, wherein the compound reduces the radical and/or ROS catalytically.

6. The biomedical implant material of claim 3, wherein the compound is regenerated after a radical degradation reaction and, after regeneration, the compound can catalytically degrade a radical and/or ROS.

7. The biomedical implant material of claim 3, wherein the compound is not consumed after a radical degradation reaction.

8. The biomedical implant material of claim 3, wherein the compound is covalently attached to the biomedical implant material.

9. A method of decreasing and/or preventing damage to a biomedical implant material, the method comprising:
providing the biomedical implant material, the biomedical implant material
comprising a self-regenerating antioxidant catalyst on at least a portion of a surface of the biomedical implant material, thereby decreasing and/or preventing damage to the biomedical implant material.

10. The method of claim 9, wherein the self-regenerating antioxidant catalyst decreases and/or prevents damage to the biomedical implant material by decreasing and/or preventing damage to the biomedical implant from a radical and/or reactive oxygen species (ROS).

11. The method of claim 9, wherein the self-regenerating antioxidant catalyst decreases severity and/or duration of a sterile immune response in a subject.

12. The method of claim 9, wherein the self-regenerating antioxidant catalyst decreases severity and/or duration of adverse effects of acute phase foreign body reaction in a subject.

13. The method of claim 9, wherein the self-regenerating antioxidant catalyst reduces a radical and/or reactive oxygen species (ROS) catalytically.

14. The method of claim 9, wherein the self-regenerating antioxidant catalyst is regenerated after a radical degradation reaction and, after regeneration, the self-regenerating antioxidant catalyst can catalytically degrade a radical and/or reactive oxygen species (ROS).

15. The method of claim 9, wherein the self-regenerating antioxidant catalyst is not consumed after a radical degradation reaction.

16. The method of claim 9, wherein the self-regenerating antioxidant catalyst comprises a chelating, anionic benzimidazole-based N-heterocyclic carbene (NHC) ligand.

17. The method of claim 9, wherein the self-regenerating antioxidant catalyst comprises a bipyridine, phosphine, and/or amine ligand.

18. The method of claim 9, wherein the self-regenerating antioxidant catalyst comprises at least one compound of claim 1.

19. The method of claim 9, wherein the biomedical implant material is covalently functionalized with the self-regenerating antioxidant catalyst.

20. The method of claim 9, wherein the self-regenerating antioxidant catalyst is present on the biomedical implant material in a therapeutically effective amount.