# NMR Studies into the Potential Interactions of FullereneC60 with Tetraphenylporphyrin and Some of Its Derivatives

Authors: C. Obondi; A. A. Rodriguez
Journal: Advances in Physical Chemistry
 (2010)

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## Abstract

1H NMR relaxation studies were employed to investigate potential interactions between C60 and tetraphenylporphyrin, H2[TPP], and parasubstituted tetraphenylporphyrins, H2[(p-X)4TPP], where X = CN and OCH3 in solution. The substituted porphyrins provided a means by which to investigate the role that electronic effects play in the interaction process. A comparison of the relaxation rates, R1, and correlation times, τC, of the pyrrole and phenyl hydrogens in these complexes, without and with the presence of C60, revealed that the introduction of C60 into solution did not have a noticeable effect on R1 and τC of these protons in H2[TPP], indicating the absence of long-term intermolecular interaction at either of these two sites. A similar analysis of the two protons in the other two substituted tetraphenylporphyrin analogs revealed slower molecular dynamics indicating the presence of intermolecular interactions. Stronger interactions were observed in H2[(p-OCH3)4TPP]  indicating that  the electron-donating abilities of the -OCH3 group promote the interaction process. Our results indicate that it is very likely that enhanced selectivity in the chemical purifications of fullerenes and metallofullerenes can be achieved by employing tetraphenylporphyrin-silica stationary phases which have been modified with electron-donating groups.


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## Body

## 1. Introduction

Because of their distinctive properties, fullerenes have experienced a tremendous amount of research interest. Pharmaceutically, fullerenes’ unique properties have been exploited to develop a variety of applications including being used as conduits for drug delivery, functionalized to serve as antibacterial agents, and tested as HIV inhibitors [1–3]. Porphyrins and fullerenes have been found to spontaneously be attracted to each other [4]. This newly recognized supramolecular recognition element, the attraction of the curved π-surface of the fullerene to the center of the flat π-surface of a porphyrin, is possibly due to π-π and n-π electron interactions. This phenomenon is in contrast to the traditional paradigm which requires the matching of a concave host with a convex guest [5].During the past few years, the intermolecular interaction of porphyrins and fullerenes has been studied extensively. Due to their potential applications in processes of molecular recognition [6–11], photosynthesis [12–16], photovoltaics [17–23], energy transfer [24–32], and electron transfer [33–45], porphyrin-fullerene complexes have attracted a great deal of attention. Of particular interest is the development of tetraphenylporphyrin-appended silica stationary phases for the chromatographic separation of fullerenes. Meyerhoff and coworkers have developed columns with selectivity superior to the commercially available “Buckyclutcher” and “Buckyprep” columns [46, 47]. Their work showed that columns packed with (p-carboxyl)triphenylporphyrin-silica gel generated the best fullerene separation. The underlying  rationale for the enhanced selectivity is believed to be π-π interactions between tetraphenylporphyrin and the  fullerene. The close association of a fullerene and a porphyrin was first recognized in the molecular packing of a crystal structure of porphyrin-fullerene assembly containing a covalent fullerene-porphyrin conjugate [48]. In the crystal structure of this species, C60 was found to be centered over the porphyrin with its electron-rich 6 : 6 ring-juncture in close proximity to the plane of the porphyrin. The phenyl carbon atoms of the porphyrin were all at distances greater than 4.0 Å from fullerene carbon atoms, indicating that the ortho C-H bonds did not contribute significantly to the association.In this study,1H NMR relaxation studies have been performed to investigate the nature and precise interaction site of fullerene, C60, with tetraphenylporphyrin, H2[TPP], and parasubstituted tetraphenylporphyrins, H2[(p-X)4TPP], where X = CN and OCH3 in deuterated chlorobenzene-d5 (CBZ). The porphyrin derivatives were selected to investigate possible interactions changes due to electronic donating or withdrawing capabilities of the substituent group. The pyrrole hydrogen, on the porphyrin ring, and the ortho hydrogen, on the phenyl group, were selected since these hydrogens are strategically located at sites which will allow the determination of the molecular dynamics at the porphyrin and phenyl sites. Relaxation rates of the pyrrole and phenyl hydrogens in the porphyrins, as shown in Figure 1, were determined at several temperatures in the presence and absence of fullerene. In addition, correlation times, τC, for these hydrogens were calculated. Possible interaction sites were determined by looking at the difference in relaxation rate, R1, and correlation time, τC, due to the presence and absence of the C60 molecule.Figure 1
Display of parasubstituted tetraphenylporphyrin showing the pyrrole and phenyl hydrogens studied.


## 2. Theoretical Background

1H spin-lattice relaxation in the tetraphenylporphyrin H2[TPP] system is due primarily to the magnetic dipole-dipole interactions. The relaxation rate, R1, can be expressed as the sum of intra- and interrelaxation. This relationship is demonstrated below by (1) [49–52]: (1)1T1=R1=R1DD(intra)+R1DD(inter).T1 is the measured relaxation time and R1 is simply the inverse of T1. The intermolecular contribution, R1DD(inter), can be eliminated experimentally by working with very low mole fractions of a solute and by working in deuterated solvents. These two conditions were met in our measurements: mole fractions of 1.299 × 10-5 and deuterated chlorobenzene-d5. In the absence of the intermolecular interaction, (1) reduces to the following [49–52]:(2)R1=R1DD(intra)=[(23)γH4ℏ2rAB6]nsτC,
where γH is the hydrogen gyromagnetic ratio, ℏ is the h/2π, rAB is the proton-to-proton distance of the interacting nuclei, ns is the number of interacting nuclei, and τc is the rotational correlation time which can be equated to the period of time necessary for a specific nuclear site to undergo reorientation (i.e., movement) to a new position which is different by about 54°. Once relaxation rates, R1, have been acquired experimentally, the rotational dynamics at a specific molecular site can be determined by solving (2) for τc.


## 3. Experimental Methods

The solvent chlorobenzene-d5 was selected for these measurements since it provided the best solubility parameters for all tetraphenylporphyrin derivatives and C60. Fullerene C60 and chlorobenzene-d5 (99.5+ at. %D) were purchased from Acros Organics [53]. Tetraphenylporphyrin H2[TPP] was purchased from the Aldrich Chemical Company [54]. Para-substituted tetraphenylporphyrin derivatives, H2[(p-X)4TPP] (X = CN and OCH3), of H2[TPP] were synthesized by adapting and slightly modifying the method reported by Adler et al. [55]. The purity of the H2[TPP] derivatives was accomplished by several recrystallizations and established by HPLC and NMR methods. Several tetraphenylporphyrin solutions, with  decreasing mole fractions, were initially prepared, and relaxation measurements were taken, to establish the solute mole fraction at which porphyrin-porphyrin interactions were absent. Solutions with solute mole fraction of 1.299 × 10-5 were found to eliminate possible porphyrin-porphyrin interactions as evidence by the constant relaxation rates. This information was used to ensure that subsequent samples were prepared consistently with this solute mole fraction. In solutions containing both host and guest, a 1 : 1 mole ratio in porphyrin : C60 was maintained. Approximately 0.5 mL of the sample was transferred into a 5-mm NMR tube, connected to a vacuum line, and thoroughly degassed by several freeze-pump-thaw cycles to eliminate molecular oxygen. The tubes were then sealed under vacuum.1H spin-lattice relaxation times were performed on a Varian 300 MHz instrument by using the standard inversion-recovery pulse sequence (i.e., D1-π-τ-π/2), where π is a 180° pulse, π/2 is a 90° pulse, and τ is a delay between pulses. Nine delay times were used in the pulse sequence with values, depending on the estimated T1, ranging from 0.0625 s to 16 s. A delay time (D1) of approximately 14 s was used between the transients. Each experiment used a minimum of 76 transients resulting in an acquisition time of approximately 4 hours. Experiments were conducted at five different temperatures. Typical 1H NMR spectra of the H2[TPP] and some of the derivatives were obtained and are shown in Figures 2, 3, and 4. The disappearance (i.e., broadening) of the N-H proton resonance into the baseline noise, due to the very rapid exchange rate of these porphyrin protons at the higher temperatures, prevented their use in this study. Therefore, the pyrrole and ortho hydrogens of the porphyrin and phenyl ring were utilized to monitor the molecular dynamics of the two molecular sites in these tetraphenylporphyrin complexes.Figure 2
1H NMR of H2[TPP] in chlorobenzene-d5. Peak (1), at about 8.90 ppm, corresponds to the pyrrole hydrogen while the multiplet (2), at about 8.25 ppm, corresponds to the orthohydrogen of the phenyl group.Figure 3
1H NMR of H2[(p-CN)4TPP] in chlorobenzene-d5. Peak (1), at about 8.90 ppm, corresponds to the pyrrole hydrogen while the multiplet (2), at about 8.28 ppm, corresponds to the orthohydrogen of the phenyl group.Figure 4
1H NMR of H2[(–OCH3)4TPP] in chlorobenzene-d5. Peak (1), at about 8.90 ppm, corresponds to the pyrrole hydrogen while the multiplet (2), at about 8.28 ppm, corresponds to the orthohydrogen of the phenyl group.


## 4. Results and Discussion

### 4.1.1H Relaxation Rates and Correlation Times of the Pyrrole and Phenyl Hydrogens in H2[TPP] with and without C60 in Chlorobenzene-d5

Shown in columns 2 and 4 of Table1 are the variable temperature relaxation rates, R1, of the pyrrole hydrogen in the absence and presence of C60, respectively. As expected, these rates are seen to decrease with rising temperature indicating a decrease in the effectiveness of the dipolar mechanism. Columns 3 and 5, of the same table, contain the values of the correlation times obtained via the respective relaxation rates and (2). The correlation times, τC, are also decreasing with rising temperature indicating faster molecular dynamics with increasing temperature [52].Table 1
1H relaxation Rates of pyrrole Hydrogen in H2[TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[TPP] in CBZH2[TPP] with C60 in CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.651 (0.005)3220.645 (0.012)3192830.581 (0.006)2880.571 (0.013)2832980.496 (0.016)2460.515 (0.010)2553130.434 (0.002)2150.432 (0.011)2143280.357 (0.002)1770.367 (0.012)182Values in parentheses represent error limits at the 90% confidence level.A comparison of the relaxation rates, without and with the presence of C60, reveals that the introduction of C60 to the solution does not affect the relaxation rate of this proton appreciatively. One notices that the change in relaxation rate is within experimental error indicating that the presence of C60 does not lead to noticeable intermolecular interaction at the pyrrole site of H2[TPP]. This observation is further illustrated graphically in Figure 5. An Arrhenius fit of τC versus T-1 yielded energies of activation of 7.23 and 6.80 kJ/mole for H2[TPP] without and with C60, respectively, suggesting that the energies of activation for molecular motion in the presence and absence of C60 are very similar and within the range of experimental error for these types of measurements.Figure 5
Relaxation rates of the pyrrole hydrogen ofH2[TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Shown in columns 2 and 4 of Table2 are the relaxation rates of the phenyl hydrogen in the absence and presence of C60. The corresponding correlation times are given in columns 3 and 5. Both R1 and τC for this hydrogen follow the same temperature dependence as was observed for the pyrrole hydrogen indicating the dipolar pathway becoming less efficient with faster molecular motion. As was the case for the pyrrole hydrogen, a comparison of the relaxation rates of the phenyl hydrogen, with and without C60 in the solution, shows that the changes in relaxation rates are within the experimental error indicating that the presence of C60 does not lead to noticeable intermolecular interaction at the phenyl site of H2[TPP]. The relaxation rates are also illustrated graphically in Figure 6. The Arrhenius fit of τC versus T-1 yielded energies of activation of 6.76 and 6.69 kJ/mole for H2[TPP] without and with C60, respectively. An interesting sidenote is a comparison of the reorientational dynamics at the pyrrole (i.e., overall molecular motion) and phenyl sites. The reorientational motion of the phenyl ring is higher an average of 36% than that at the pyrrole site, indicating significant internal motion being present in this complex.Table 2
1H relaxation Rates of phenyl Hydrogen in H2 [TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[TPP] in CBZH2[TPP] with C60 in CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.821 (0.004)2320.821 (0.008)2322830.752 (0.006)2130.729 (0.009)2062980.606 (0.012)1710.660 (0.019)1873130.576 (0.008)1630.557 (0.010)1583280.469 (0.009)1320.470 (0.011)132Values in parentheses represent error limits at the 90% confidence level.Figure 6
Relaxation rates of the pyrrole hydrogen ofH2[TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.


### 4.2.1H Relaxation Rates and Correlation Times of the Pyrrole and Phenyl Hydrogens in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5

The temperature behaviors of the relaxation rates and correlation times of the pyrrole and phenyl hydrogens in H2[(p-CN)4TPP], with and without C60, are shown in Tables 3 and 4, respectively. The relaxation rates and correlation times of both hydrogens show the expected temperature behavior, decreasing in magnitude with rising temperature indicating that the molecule is undergoing faster dynamics with an increase in temperature. The temperature behaviors of the relaxation rates for these hydrogens are also illustrated in Figures 7 and 8.Table 3
1H relaxation Rates of Pyrrole Hydrogen in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5.
T (K)H2[(p-CN)4TPP]H2[(p-CN)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.825 (0.014)4080.921 (0.016)4562830.820 (0.016)4060.878 (0.018)4352980.813 (0.024)4020.781 (0.009)3973130.809 (0.013)4000.765 (0.020)3793280.803 (0.014)3970.695 (0.020)344Values in parentheses represent error limits at the 90% confidence level.Table 4
1H relaxation Rates of Phenyl Hydrogen in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5..
T (K)H2[(p-CN)4TPP]H2[(p-CN)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2681.01 (0.012)2861.04 (0.015)2942830.968 (0.015)2740.986 (0.020)2792980.913 (0.015)2580.838 (0.020)2373130.879 (0.061)2490.832 (0.021)2353280.831 (0.017)2350.731 (0.023)207Values in parentheses represent error limits at the 90% confidence level.Figure 7
Relaxation rates of the pyrrole hydrogen ofH2[(p-CN)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Figure 8
Relaxation rates of the phenyl hydrogen ofH2[(p-CN)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.In the absence of C60, the relaxation rate for the pyrrole hydrogen gradually decreases in magnitude with increasing temperature indicating less sensitivity to temperature variations. It is interesting to note that, at both the pyrrole and phenyl hydrogen sites, the relaxation rate is enhanced at the two lower temperatures of 268 and 283 K when C60 is introduced into the solution. This improved relaxation results in longer correlation times at these two temperatures indicating that the slower rotational motion is enhancing the relaxation mechanism (dipole-dipole) at these temperatures. This observation suggests the presence of noticeable intermolecular interactions of C60 at the porphyrin and phenyl sites. While interactions are seen at both sites, a comparison of the data, and also illustrated in Figures 7 and 8, shows a slight interaction preference for the pyrrole site. This observation indicates that electrons withdrawing groups on the phenyl group may enhance intermolecular interactions, at least at reduced temperatures. However, as the temperature rises, the correlation times in the H2[(p-CN)4TPP]/C60 solution decrease, which has the effect of reducing the efficiency of the relaxation mechanism. This observation indicates that a rise in thermal energy prevents long-lasting H2[(p-CN)4TPP]-C60 interactions from occurring at both molecular sites. As was the case in the H2[TPP] sample, the reorientational motion of the phenyl ring is much higher than that at the pyrrole site, ranging from 43% at the lower temperature and increasing to nearly 66% at the highest temperature indicating the presence of a significant amount of internal motion.


### 4.3.1H Relaxation Rates and Correlation Times of Pyrrole and Phenyl Hydrogens in H2[(p-OCH3)4TPP] with and without C60 in Chlorobenzene-d5.

The data for the pyrrole and phenyl hydrogens for the electron-donating, para-OCH3-substituted porphyrin are given in Tables 5 and 6. The temperature behaviors of the relaxation rates are also illustrated in Figures 9 and 10. As was observed previously in H2[TPP] and H2[(p-CN)4TPP] complexes, both R1 and τC decrease in value with rising temperature indicating the reduced effectiveness of the dipole-dipole mechanism with increased reorientational motion.Table 5
1H relaxation rates of phenyl hydrogen in H2[(p-OCN3)4TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[(p-OCH3)4TPP]H2[(p-OCH3)4TPP] with C60in CBZin CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.699 (0.012)3460.725 (0.009)3592830.660 (0.014)3270.688 (0.015)3412980.624 (0.016)3080.659 (0.012)3263130.584 (0.015)2890.618 (0.018)3063280.547 (0.019)2700.585 (0.019)290Values in parentheses represent error limits at the 90% confidence level.Table 6
1H relaxation rates of phenyl hydrogen in H2[(p-OCN3)4TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[(p-OCH3)4TPP]H2[(p-OCH3)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.857 (0.011)2421.00 (0.01)2832830.834 (0.012)2360.956 (0.013)2702980.790 (0.016)2230.875 (0.015)2473130.778 (0.014)2200.847 (0.017)2403280.745 (0.015)2110.784 (0.019)222Values in parentheses represent error limits at the 90% confidence level.Figure 9
Relaxation rates of the pyrrole hydrogen ofH2[(p-OCH3)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Figure 10
Relaxation rates of the phenyl hydrogen ofH2[(p-OCH3)4TPP] with C60 (dashed line) and without C60 (solid line) in chlorobenzene-d5.A comparison of the pyrrole relaxation rate, as well asτC, with and without C60 shows that the introduction of C60 into solution enhances the relaxation rate of this pyrrole hydrogen by slowing the molecular dynamics (i.e., longer τC) at this site. This indicates that H2[(p-OCH3)4TPP] is experiencing intermolecular interaction with C60 at the pyrrole hydrogen site. This enhanced relaxation is also illustrated in Figure 9. While the error bars in the measurements are somewhat large, the effects of these interactions on the molecular dynamics at this hydrogen site are experimentally observable.A review of the relaxation rates and correlation times of the phenyl hydrogen, with and without the presence of C60, reveals higher relaxation rates and longer correlation times when C60 is present. This observation indicates the presence of phenyl/C60 interactions at this site. A comparison of the pyrrole and phenyl data indicates that, while C60 is interacting with H2[(p-OCH3)4TPP]/C60 at both the pyrrole and phenyl sites, there is a noticeable preference for the phenyl site. An illustration of the two types of interactions is given in Figure 11. We attribute this preference to the electron-donating abilities of the -OCH3 group which allows two potential points of interaction with C60. Gung and  Amicangelo analyzed the effects of substituents on π- π interactions and found that electron-donating groups increase interaction energies by promoting two types of electronic interactions: the normal π- π parallel stacking and the offset stacking of the substituent group over the guest molecule which can give rise to electrostatic interactions [56]. In some cases, this second type of interaction can lead to charge transfer with significant interaction energies.Illustration of possible interaction sites of tetraphenylporphyrin withC60.
(a)(b)


## 4.1.1H Relaxation Rates and Correlation Times of the Pyrrole and Phenyl Hydrogens in H2[TPP] with and without C60 in Chlorobenzene-d5

Shown in columns 2 and 4 of Table1 are the variable temperature relaxation rates, R1, of the pyrrole hydrogen in the absence and presence of C60, respectively. As expected, these rates are seen to decrease with rising temperature indicating a decrease in the effectiveness of the dipolar mechanism. Columns 3 and 5, of the same table, contain the values of the correlation times obtained via the respective relaxation rates and (2). The correlation times, τC, are also decreasing with rising temperature indicating faster molecular dynamics with increasing temperature [52].Table 1
1H relaxation Rates of pyrrole Hydrogen in H2[TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[TPP] in CBZH2[TPP] with C60 in CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.651 (0.005)3220.645 (0.012)3192830.581 (0.006)2880.571 (0.013)2832980.496 (0.016)2460.515 (0.010)2553130.434 (0.002)2150.432 (0.011)2143280.357 (0.002)1770.367 (0.012)182Values in parentheses represent error limits at the 90% confidence level.A comparison of the relaxation rates, without and with the presence of C60, reveals that the introduction of C60 to the solution does not affect the relaxation rate of this proton appreciatively. One notices that the change in relaxation rate is within experimental error indicating that the presence of C60 does not lead to noticeable intermolecular interaction at the pyrrole site of H2[TPP]. This observation is further illustrated graphically in Figure 5. An Arrhenius fit of τC versus T-1 yielded energies of activation of 7.23 and 6.80 kJ/mole for H2[TPP] without and with C60, respectively, suggesting that the energies of activation for molecular motion in the presence and absence of C60 are very similar and within the range of experimental error for these types of measurements.Figure 5
Relaxation rates of the pyrrole hydrogen ofH2[TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Shown in columns 2 and 4 of Table2 are the relaxation rates of the phenyl hydrogen in the absence and presence of C60. The corresponding correlation times are given in columns 3 and 5. Both R1 and τC for this hydrogen follow the same temperature dependence as was observed for the pyrrole hydrogen indicating the dipolar pathway becoming less efficient with faster molecular motion. As was the case for the pyrrole hydrogen, a comparison of the relaxation rates of the phenyl hydrogen, with and without C60 in the solution, shows that the changes in relaxation rates are within the experimental error indicating that the presence of C60 does not lead to noticeable intermolecular interaction at the phenyl site of H2[TPP]. The relaxation rates are also illustrated graphically in Figure 6. The Arrhenius fit of τC versus T-1 yielded energies of activation of 6.76 and 6.69 kJ/mole for H2[TPP] without and with C60, respectively. An interesting sidenote is a comparison of the reorientational dynamics at the pyrrole (i.e., overall molecular motion) and phenyl sites. The reorientational motion of the phenyl ring is higher an average of 36% than that at the pyrrole site, indicating significant internal motion being present in this complex.Table 2
1H relaxation Rates of phenyl Hydrogen in H2 [TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[TPP] in CBZH2[TPP] with C60 in CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.821 (0.004)2320.821 (0.008)2322830.752 (0.006)2130.729 (0.009)2062980.606 (0.012)1710.660 (0.019)1873130.576 (0.008)1630.557 (0.010)1583280.469 (0.009)1320.470 (0.011)132Values in parentheses represent error limits at the 90% confidence level.Figure 6
Relaxation rates of the pyrrole hydrogen ofH2[TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.


## 4.2.1H Relaxation Rates and Correlation Times of the Pyrrole and Phenyl Hydrogens in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5

The temperature behaviors of the relaxation rates and correlation times of the pyrrole and phenyl hydrogens in H2[(p-CN)4TPP], with and without C60, are shown in Tables 3 and 4, respectively. The relaxation rates and correlation times of both hydrogens show the expected temperature behavior, decreasing in magnitude with rising temperature indicating that the molecule is undergoing faster dynamics with an increase in temperature. The temperature behaviors of the relaxation rates for these hydrogens are also illustrated in Figures 7 and 8.Table 3
1H relaxation Rates of Pyrrole Hydrogen in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5.
T (K)H2[(p-CN)4TPP]H2[(p-CN)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.825 (0.014)4080.921 (0.016)4562830.820 (0.016)4060.878 (0.018)4352980.813 (0.024)4020.781 (0.009)3973130.809 (0.013)4000.765 (0.020)3793280.803 (0.014)3970.695 (0.020)344Values in parentheses represent error limits at the 90% confidence level.Table 4
1H relaxation Rates of Phenyl Hydrogen in H2[(p-CN)4TPP] with and without C60 in Chlorobenzene-d5..
T (K)H2[(p-CN)4TPP]H2[(p-CN)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2681.01 (0.012)2861.04 (0.015)2942830.968 (0.015)2740.986 (0.020)2792980.913 (0.015)2580.838 (0.020)2373130.879 (0.061)2490.832 (0.021)2353280.831 (0.017)2350.731 (0.023)207Values in parentheses represent error limits at the 90% confidence level.Figure 7
Relaxation rates of the pyrrole hydrogen ofH2[(p-CN)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Figure 8
Relaxation rates of the phenyl hydrogen ofH2[(p-CN)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.In the absence of C60, the relaxation rate for the pyrrole hydrogen gradually decreases in magnitude with increasing temperature indicating less sensitivity to temperature variations. It is interesting to note that, at both the pyrrole and phenyl hydrogen sites, the relaxation rate is enhanced at the two lower temperatures of 268 and 283 K when C60 is introduced into the solution. This improved relaxation results in longer correlation times at these two temperatures indicating that the slower rotational motion is enhancing the relaxation mechanism (dipole-dipole) at these temperatures. This observation suggests the presence of noticeable intermolecular interactions of C60 at the porphyrin and phenyl sites. While interactions are seen at both sites, a comparison of the data, and also illustrated in Figures 7 and 8, shows a slight interaction preference for the pyrrole site. This observation indicates that electrons withdrawing groups on the phenyl group may enhance intermolecular interactions, at least at reduced temperatures. However, as the temperature rises, the correlation times in the H2[(p-CN)4TPP]/C60 solution decrease, which has the effect of reducing the efficiency of the relaxation mechanism. This observation indicates that a rise in thermal energy prevents long-lasting H2[(p-CN)4TPP]-C60 interactions from occurring at both molecular sites. As was the case in the H2[TPP] sample, the reorientational motion of the phenyl ring is much higher than that at the pyrrole site, ranging from 43% at the lower temperature and increasing to nearly 66% at the highest temperature indicating the presence of a significant amount of internal motion.


## 4.3.1H Relaxation Rates and Correlation Times of Pyrrole and Phenyl Hydrogens in H2[(p-OCH3)4TPP] with and without C60 in Chlorobenzene-d5.

The data for the pyrrole and phenyl hydrogens for the electron-donating, para-OCH3-substituted porphyrin are given in Tables 5 and 6. The temperature behaviors of the relaxation rates are also illustrated in Figures 9 and 10. As was observed previously in H2[TPP] and H2[(p-CN)4TPP] complexes, both R1 and τC decrease in value with rising temperature indicating the reduced effectiveness of the dipole-dipole mechanism with increased reorientational motion.Table 5
1H relaxation rates of phenyl hydrogen in H2[(p-OCN3)4TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[(p-OCH3)4TPP]H2[(p-OCH3)4TPP] with C60in CBZin CBZR1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.699 (0.012)3460.725 (0.009)3592830.660 (0.014)3270.688 (0.015)3412980.624 (0.016)3080.659 (0.012)3263130.584 (0.015)2890.618 (0.018)3063280.547 (0.019)2700.585 (0.019)290Values in parentheses represent error limits at the 90% confidence level.Table 6
1H relaxation rates of phenyl hydrogen in H2[(p-OCN3)4TPP] with and without C60 in chlorobenzene-d5.
T (K)H2[(p-OCH3)4TPP]H2[(p-OCH3)4TPP] with C60R1 (1/s)τC (ps)R1 (1/s)τC (ps)2680.857 (0.011)2421.00 (0.01)2832830.834 (0.012)2360.956 (0.013)2702980.790 (0.016)2230.875 (0.015)2473130.778 (0.014)2200.847 (0.017)2403280.745 (0.015)2110.784 (0.019)222Values in parentheses represent error limits at the 90% confidence level.Figure 9
Relaxation rates of the pyrrole hydrogen ofH2[(p-OCH3)4TPP] with C60 (dash line) and without C60 (solided line) in chlorobenzene-d5.Figure 10
Relaxation rates of the phenyl hydrogen ofH2[(p-OCH3)4TPP] with C60 (dashed line) and without C60 (solid line) in chlorobenzene-d5.A comparison of the pyrrole relaxation rate, as well asτC, with and without C60 shows that the introduction of C60 into solution enhances the relaxation rate of this pyrrole hydrogen by slowing the molecular dynamics (i.e., longer τC) at this site. This indicates that H2[(p-OCH3)4TPP] is experiencing intermolecular interaction with C60 at the pyrrole hydrogen site. This enhanced relaxation is also illustrated in Figure 9. While the error bars in the measurements are somewhat large, the effects of these interactions on the molecular dynamics at this hydrogen site are experimentally observable.A review of the relaxation rates and correlation times of the phenyl hydrogen, with and without the presence of C60, reveals higher relaxation rates and longer correlation times when C60 is present. This observation indicates the presence of phenyl/C60 interactions at this site. A comparison of the pyrrole and phenyl data indicates that, while C60 is interacting with H2[(p-OCH3)4TPP]/C60 at both the pyrrole and phenyl sites, there is a noticeable preference for the phenyl site. An illustration of the two types of interactions is given in Figure 11. We attribute this preference to the electron-donating abilities of the -OCH3 group which allows two potential points of interaction with C60. Gung and  Amicangelo analyzed the effects of substituents on π- π interactions and found that electron-donating groups increase interaction energies by promoting two types of electronic interactions: the normal π- π parallel stacking and the offset stacking of the substituent group over the guest molecule which can give rise to electrostatic interactions [56]. In some cases, this second type of interaction can lead to charge transfer with significant interaction energies.Illustration of possible interaction sites of tetraphenylporphyrin withC60.
(a)(b)


## 5. Conclusion

1H NMR relaxation studies were employed to investigate potential interactions between C60 and tetraphenylporphyrin, H2[TPP], and parasubstituted tetraphenylporphyrins, H2[(p-X)4TPP], where X = CN and OCH3 in solution. The substituted porphyrins provided a means by which to investigate the role that electronic effects play in the interaction process. A comparison of the relaxation rates, R1, and correlation times, τC, of the pyrrole and phenyl hydrogens in H2[TPP], without and with the presence of C60, revealed that the introduction of C60 into solution did not have a noticeable effect on R1 and τC of these protons indicating the absence of long-term intermolecular interaction at either of these two sites. A similar analysis of the two protons in the electron-withdrawing substituted tetraphenylporphyrin analog, H2[(p-CN)4TPP], revealed slower molecular dynamics at the two lowest temperatures indicating the presence of intermolecular interactions. However, these interactions were absent at higher temperatures suggesting that the rise in thermal energy prevents long-lasting interactions from occurring at both molecular sites. A comparison of the pyrrole and phenyl hydrogens data in H2[(p-OCH3)4TPP] indicated that, while C60 is interacting at both the pyrrole and phenyl sites, there is a clear preference for the phenyl site. A graphical illustration of these interactions is given in Figure 11. We believe that this preference is due to the electron-donating abilities of the -OCH3 group which allows two potential points of interaction of C60 on the phenyl group. This observation is consistent with the results observed by Gung and Amicangelo [56].Our results indicate that it is very likely that enhanced selectivity in the chemical purifications of fullerenes and metallofullerenes can be achieved by employing tetraphenylporphyrin-silica stationary phases which have been modified with electron-donating groups.



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*Source: 102167-2010-09-20.xml*