Free energies, kinetics, and photoelectron-transfer properties, and theoretical and quantitative structural relationship studies of [SWCNT(5,5)-armchair-CnH20][R] (R = η2-CmPd(dppf), η2-CmPd(dppr), and η2-CmPd(dppcym)2, n = 20 to 300 and m = 60 and 70) nanostructure complexes

Metal complexes containing one or several bis(triorganylphosphine)palladium fragments attached to the C60 core and coordinated in olefinic η2 mode have been previously described. The number of carbon atoms of the single-walled carbon nanotubes (SWCNTs) is the useful numerical and structural electrochemical properties contributing to the relationship between the structures of the η2_CmPd(dppf), η2_CmPd(dppr), and η2_CmPd(dppcym)2 (m = 60 and 70) ligands (A to E) and [SWCNT(5,5)-armchair-CnH20] (n = 20 to 190) 1 to 18 and the production of the [SWCNT(5,5)-armchair-CnH20][R] (R = η2-CmPd(dppf), η2-CmPd(dppr), and η2-CmPd(dppcym)2, n = 20 to 300 and m = 60 and 70) complexes 30 to 174. In this study, the relationship between the number of carbon atoms index and the first and second free energies of electron transfer (ΔGet(n), n = 1,2) using the Rehm-Weller equation based on the first and second oxidation potentials (oxE1 and oxE2) of A to E for the predicted complexes 30 to 174 between 1 and 29 with exohedral metallofullerenes A to E, as [SWCNT(5,5)-armchair-CnH20][R] (R = η2-CmPd(dppf), η2-CmPd(dppr), and η2-CmPd(dppcym)2, n = 20 to 300 and m = 60 and 70) 30 to 174 was assessed. Here, the first and second free activation energies of electron transfer and the wavelengths of the electromagnetic photons in the photoelectron transfer process, ΔG#et(n) and λ(n) (nm), respectively, for 30 to 174 in accordance with the Marcus theory and Planck's equation were also calculated.


Background
The first metal complexes containing one or several bis (triorganylphosphine)platinum fragments attached to the C 60 core and coordinated in the olefinic η 2 mode were described in 1991 [1][2][3], revealing that fullerenes, at least buckminsterfullerene C 60 , can function as ligands in reactions with transition metals. Electronic structures of exohedral palladium complexes of [60] and [70] fullerenes with diphenylphosphinoferrocenyl, diphenylphosphinoru thenocenyl, and diphenylphosphinocymantrenyl ligands were studied by cyclic voltammetry and semi-empirical quantum chemical calculations in 2004 [1]. The probable sites of the electronic changes in these complexes under electrochemical oxidation and reduction have also been determined [1][2][3][4].
The bulk of fullerene metal complexes consist of heteroligand complexes. The only exceptions known to date are polymeric homoligand complexes of C 60 with palladium or platinum, which are prepared by the direct reaction of fullerene with zero-valent complexes of these

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metals with a weakly bound ligand, dibenzylideneacetone [1][2][3][4][5][6][7][8]. The platinum and palladium complexes (C 60 )M x (M = Pt and Pd) can also be prepared from the Pt(0) and Pd cyclooctadiene complexes. Two C 60 molecules are bound to the metal atom in η 2 mode. However, instead of separate (C 60 ) 2 M molecules, a polymeric chain is formed, which is probably indicative of enhanced reactivity (with respect to ligand-free palladium) of the other fullerene double bonds upon coordination of one bond. If an excess of the M(0) compound is present, the specific content of the metal increases [1][2][3][4][5][6][7][8].
According to elemental analysis, the insoluble precipitates have compositions of (C 60 )Pd x , where x = 1, 2, 3, and more. Some free metal is always present. C 60 molecules are presumably linked by metal atoms into onedimensional chains or two-and three-dimensional frameworks. The palladium (platinum) fullerene polymer reacts heterogeneously with P ligands (tertiary phosphines or tertiary phosphites) in solution to give the C 60 ML 2 complexes, which can also be synthesized by other methods [1][2][3][4][5][6][7][8]. The electrochemical synthesis of the (η 2 -C 60 M(PPh 3 ) 2 (M = Pt, Pd) complexes was performed by reacting the dianion of C 60 2− prepared by electrochemical reduction (at a Pt electrode in a toluene-acetonitrile solution in the presence of Bu 4 NBF 4 as the supporting electrolyte) with the ML 2 Cl 2 complex or with a divalent metal chloride in the presence of triphenylphosphine [1][2][3][4]. The palladium derivatives of C 60 and C 70 with cymantrenyldiphenylphosphine ligand were prepared in a similar way [7,8]. A series of new exohedral Pd(0) complexes with C 60 and C 70 fullerenes containing bisdiphenylphosphinoferrocene (dppf), bisdiphenylphosphinoruthenocene (dppr), or two diphenylphosphinocymantrene (dppcym) molecules as stabilizing ligands have been synthesized. These complexes contain a strongly electron-withdrawing fullerene cage and a metallocene group, which can be either electron releasing (ruthenocene) or electron withdrawing (cymantrene) and is linked with the cage through a bisdiphenylphosphine palladium bridge. The electrochemical pattern is impeded because the bisdiphenylphosphine palladium fragment linking these terminal groups is also redox active [1][2][3][4][5][6][7][8].
Metal complexes with fullerenes have attracted attention due to the prospects of their application in catalysis, in materials for nonlinear optics, for designing artificial photosynthesis systems, and in the development of supraand nanomaterials [4]. More specifically, metal-fullerene interactions are of particular importance. Platinum was the first metal found to form π-complexes with fullerenes. However, evidence for the existence of similar complexes for palladium was obtained soon thereafter. The most practical preparation of palladium η 2 complexes appeared to be by direct synthesis using Pd 2 (dba) 3 , fullerene, and a free phosphine ligand. Almost all known complexes of fullerenes with an undisturbed electronic system involve only η 2 coordination, which is typical of an isolated olefinic double bond. The η 2 coordination is probably due to the nonplanar surface geometry, which makes the axes of the pseudo-π-orbitals nonparallel and, thus, hampers their bonding to metal orbitals [1][2][3][4][5][6][7][8].
Nanotubes of type (n,n) are called armchair nanotubes because of their 'W' shape perpendicular to the tube axis. They are symmetrical along the tube axis, with a short unit cell (0.25 nm or 2.5 Å) that is repeated along the entire section of a long nanotube. All other nanotubes are called chiral nanotubes and have longer unit cell sizes along the tube axis [9][10][11]. The simplest type of nanotube is a cylindrical structure, which conceptually could be formed by folding and gluing a pair of opposite sides of a rectangular graphite sheet [9][10][11][12][13][14][15][16][17][18][19][20][21][22][23][24]. If both ends are capped, it will have at least two pentagons and be a type of fullerene. Nanotubes are large, linear fullerenes with aspect ratios as large as 103 to 105 [11]. The walls of such tubes can have various sizes of polygons [25]. Although many nanoscale fullerene materials occur regularly in applications, controlled production of numerous fullerenes and nanotubes with well-defined characteristics has not yet been achieved [16][17][18][19]25].
Carbon nanotubes possess many special properties, such as an open mesoporous structure, high electrical conductivity and chemical stability, and extremely high mechanical strength and modulus [11,[19][20][21]. These properties not only help in the transportation of ions but also facilitate the charging of the double layer and confer advantages in the development of electrochemical capacitors [22]. Single-walled carbon nanotubes have been recognized as potential electrode materials for electrochemical capacitors [23,24].
One of the most widely recognized structures of nanotubes is the (5,5) tube, which can be built by successively adjoining sections of ten C atoms. In the infinite tube, the periodic unit cell has two sections, each consisting of 20 C atoms [9]. The electronic structures and electrical properties of single-walled nanotubes can be simulated from those of a graphite layer (graphene sheet) [19][20][21][22][23][24]. Figure 1 shows the (5,5) armchair form with the imaginary structures of the η 2_ C m Pd(dppf), η 2_ C m Pd(dppr), and η 2_ C m Pd(dppcym) 2 (m = 60 and 70) ligands (A to E) and 1 to 174 as [SWCNT(5,5)-armchair-C n H 20 ][R] (R = η 2 -C m Pd(dppf), η 2 -C m Pd(dppr), and η 2 -C m Pd(dppcym) 2 , n = 20 to 300 and m = 60 and 70) 30 to 174. The nanotubes may not contain any hydrogen atoms (there is no hydrogen in the electric arc technique), and the nanotubes can be easily closed at both ends.
Electronic structures of tubular aromatic molecules derived from the metallic (5,5) armchair SWCNT for C 20 H 20 up to C 210 H 20 (see Figure 1) were reported by Zhou et al. in 2004 [9]. The authors considered how the electronic structures of short molecular sections of the (5,5) tube relate to, differ from, and asymptotically approach those of an infinite metallic tube [9]. Some of the structural and electronic properties were investigated, such as the ionization potential, electron affinity, Fermi energy, chemical hardness, and relative energetic stability. All of these metrics show the length periodicity in the frontier orbital (i.e., highest occupied molecular orbitallowest unoccupied molecular orbital) gap, in contrast to the optical 'charge transfer' transition and the static axial polarizability [9]. The (5,5) nanotubes have two types of symmetry. For nanotubes with odd identification numbers (1 to 17), the point group is D 5d , whereas nanotubes with even identification numbers (2 to 18) have a point group of D 5h . Static and time-dependent density function theory calculations were used to independently optimize the structure for neutral, cationic, and anionic complexes [9]. The hybrid nonlocal Becke, three-parameter, Lee-Yang-Parr (B3LYP) function was applied [9].
Infinite-length SWCNTs are π-bonded aromatic structures that can be either semi-conducting or metallic, depending upon the diameter and helical angle of the SWCNTs. In a pioneering 1992 DFT calculation, Mintmire et al. predicted that the infinite length (5,5) armchair SWCNT (6.70 Å diameter) would be metallic with a very low transition temperature separating the uniform (high-temperature) structure from the Peierls bond alternating (low-temperature) structure [23,26]. This specific SWCNT is the elongated tube of the C 60 , C 70 , etc. molecular family [9]. Most of the previous studies have dealt with C 60 @SWCNT and C 70 @SWCNT structures [18,[27][28][29][30].
Any extrapolation of results from one compound to other compounds must take into account considerations based on a Quantitative Structural Analysis Relationship Study, which mostly depends on the similarity of the physical and chemical properties of the compounds in question. Numerous studies in the above areas have also used topological indices [31][32][33][34][35]. In previous studies, the relationship between the D U index and electron affinity, reduction potential ( Red. E 1 ) of [SWCNT(5,5)-armchair-C n H 20 ] as well as the free energy of electron transfer (ΔG et ) between [SWCNT(5,5)-armchair-C n H 20 ] structures and fullerene C 60 in C 60 @[SWCNT(5,5)-armchair-C n H 20 ] complexes was investigated [28]. In some studies, the relationship between the D U index and the free energy of electron transfer (ΔG et ) using the Rehm-Weller equation based on the first oxidation potential ( ox E 1 ) of Sc 2 @C 84 and Er 2 @C 82 for the predicted supramolecular complexes between SWCNT(5,5)-armchair-C n H 20 and the endohe dral metallofullerenes Sc 2 @C 84 and Er 2 @C 82 as [M 2 @Cx] @[SWCNT(5,5)-armchair-C n H 20 ] (M = Er and Sc, x = 82 and 84) [28][29][30]36] was assessed.
To characterize the structural properties of the π-bonds, we investigated the relationship between the number of carbon atoms of the SWCNT (C n ) index and electron affinity, Red. E 1 of [SWCNT(5,5)-armchair-C n H 20 ] 1 to 18 (and extension of the results to 19 to 29) as well as the first and second free energies of electron transfer (ΔG et(n) , n = 1,2) using the Rehm-Weller equation [36] based on the first and second oxidation potential ( ox E 1 and ox E 2 ) of the η 2_ C m Pd(dppf)), η 2_ C m Pd(dppr), and η 2_ C m Pd (dppcym) 2 (m = 60 and 70) ligands (A to E) for the predicted [SWCNT(5,5)-armchair-C n H 20 ][R] (R = η 2 -C m Pd (dppf), η 2 -C m Pd(dppr), and η 2 -C m Pd(dppcym) 2 , n = 20 to 300 and m = 60 and 70) supramolecular complexes 30 to 174. We also calculated the first and second activation free energies of electron transfer and the wavelengths of the electromagnetic photons in the photoelectron transfer process, ΔG # et(n) , and λ (n) (nm) using the Marcus theory, Planck's equation, and the equations based on the first and second oxidation potentials ( ox E 1 and ox E 2 ) of A-E for the predicted supramolecular complexes 30 to 174. The Marcus theory is based on the traditional Arrhenius equation for the rates of chemical reactions in two ways. First, it provides a formula for the pre-exponential factor in the Arrhenius equation, based on the electronic coupling between the initial and final states of the electron-transfer reaction (i.e., the overlap of the electronic wave functions of the two states). Second, it provides a formula for the activation energy, based on a parameter called the reorganization energy, as well as the Gibbs free energy. The reorganization energy is defined as the energy required to reorganize the structure of the system from initial to final coordinates without changing the electronic state [37][38][39][40][41][42].
Although electrons are commonly described as residing in electron bands in bulk materials and electron orbitals in molecules, the following description will be described in molecular terms. When a photon excites a molecule, an electron in a ground state orbital can be excited to a higher energy orbital. This excited state leaves a vacancy in a ground state orbital that can be filled by an electron donor. An electron is produced in a high-energy orbital and can be donated to an electron acceptor. Photoinduced electron transfer is an electron transfer that occurs when certain photoactive materials interact with light, including semiconductors that can be photo-activated, such as many solar cells, biological systems like those used in photosynthesis, and small molecules with suitable absorptions and redox states [36][37][38][39][40][41][42].

Methods
The number of carbon atoms of the SWCNTs (C n ) was used as a structural index (1 to 29). All mathematical and graphing operations were performed using MATLAB-7.4.0 (R2007a) and Microsoft Office Excel 2003 programs. The number of carbon atoms in the SWCNTs (C n ) is a useful numerical and structural value in characterizing the empty fullerenes. However, we used other selected indices and the best results and equations for extending the physicochemical and electrochemical data.
The Rehm-Weller equation estimates the free energy change between an electron donor (D) and an acceptor (A) as where e is the unit electrical charge, E D°a nd E A°a re the reduction potentials of the electron donor and acceptor, respectively, ΔE * is the energy of the singlet or triplet excited state, and ω 1 is the work required to bring the donor and acceptor within the electron transfer (ET) distance. The work term in this expression can be considered to be '0' in so far as an electrostatic complex exists before the electron transfer [36]. The Marcus theory of electron transfer implies rather weak (<0.05 eV) electronic coupling between the initial (locally excited (LE)) and final (ET) states, and presumes that the transition state is close to the crossing point of the LE and CT terms. The value of the electron transfer rate constant k et is controlled by the activation free energy ΔG # et , which is a function of the reorganization energy (l/4) and the electron transfer driving force ΔG et :

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The reorganization energy of organic molecules ranges from 0.1 to 0.3 eV. In this study, we used the minimum amount of reorganization energy [37][38][39][40][41][42].
To calculate the maximum wavelengths (λ (n) ; n = 1 to 2 of the electromagnetic photon for the electron transfer process in the nanostructure supramolecular complexes, we used Planck's formula: In this study, this formula was also used to calculate the activation free energy of the electron transfer process [43].

Results and discussion
The electronic structures of the exohedral palladium complexes of [60]_ and [70]_fullerenes with diphenylphos phinoferrocenyl, diphenylphosphinoruthenocenyl, and diphenylphosphinocymantrenyl ligands (η 2_ C m Pd(dppf), η 2_ C m Pd(dppr), and η 2_ C m Pd(dppcym) 2 (m = 60 and 70) (A to E), respectively) were studied by cyclic voltammetry and semi-empirical quantum chemical calculations. The C 60 Pd(dppf), C 60 Pd(dppcym) 2 , C 60 Pd(dppr), C 70 Pd(dppr), and C 70 Pd(dppcym) 2 complexes were synthesized using the Schlenk technique by a previously described method [1,2,5,6]. The reaction required equivalent amounts of the respective fullerene, Pd 2 (dba) 3 complex (where dba is dibenzylideneacetone) and phosphine ligand under argon. Measurements of Ox E and Red E have been previously reported [1,2]. Voltammograms were recorded with 0.15 МBu n 4 NBF 4 as a supporting electrolyte in ortho-dichlorobenzene at 20°C in a 10-mL electrochemical cell vs. Ag/AgCl/KCl. Oxygen was removed by passing dry argon through the cell [1,2]. The CV curves were recorded on a stationary graphite electrode with sweep rates of 100 and 200 mV s −1 . The potentials of the peaks, which were often poorly pronounced in the CV curves, were determined [1,2]. The first and second reported oxidation potential ( ox E 1 and ox E 2 in volt) states of A to E are as follows [1,2]: The energy (E a ) is released upon the attachment of an electron to an atom or a molecule (A), resulting in the formation of the negative ion A − , i.e., A + e − → A − + E a . As in the case of the ionization potential, the adiabatic electron affinity (E aa ) and vertical electron affinity can be defined. The adiabatic E a is equal to the difference between the total energies of a neutral system (A) and the corresponding anion (A − ). The vertical A X is equal to the difference between the total energies of A and the anion A − in the equilibrium geometry of A [44]. The free energy of this reaction (ΔE s (A→A − )) corresponds to the absolute redox energy for the above process. The free energy of an electron (e − ) at rest in the gas phase is set to zero [45,46]. The redox energy of the reaction (A + e − → A − + E a ) can be calculated using a thermodynamic equation (see Equation 5). In this equation, ΔG s (A) and ΔG s (A − ) are the solvation energies of molecule A and its anion A − , respectively, and ΔE g (A→A − ) is the energy difference between molecule A and its anion (which is defined as the redox energy in the gas phase). Based on this thermodynamic cycle, we can obtain ΔE s (A→A − ), the absolute redox energy [45,46]: By calculating the gas phase energies and solvation energies of molecule A and its anion A − , the absolute redox potential (scaled) of molecule A in solution can be derived. A scaling coefficient that translates electron affinity into standard redox potentials can be extracted [44][45][46]. As seen in the results of [16], the static TD-DFT and independently optimized structure were used to calculate the physicochemical and electronic structure of tubular aromatic molecules derived from the metallic (5,5) armchair single-walled carbon nanotubes using the hybrid nonlocal B3LYP function [8,47,48].
The reduction potential ( Red E) of 1 to 18 can be calculated using the Gibbs equation (ΔG = −nFE) and the definition of adiabatic electron affinity. In this equation, ΔG is equal to the adiabatic electron affinity (the free energy of electron transfer, ΔG et in J mol  Table 1. The amount of Red E (in V) = −E aa (in eV), where E aa is the adiabatic electron affinity (see Table 1 for more details).
The values of the relative structural coefficients of the (5,5) armchair SWCNT for C 20 H 20 up to C 190 H 20 ([SWCNT(5,5)-armchair-C n H 20 ], 1 to 18), the adiabatic electron affinity (E aa in eV) and the reduction potentials ( Red E in V) of 1 to 18 are shown in Table 1. The absolute value of E aa or Red E increases with the number of carbon atoms in 1 to 18. From C 20 H 20 up to C 190 H 20 , the point groups alternate between D 5d and D 5h [9]. Using the equations 8 to 16 in Table 2, the values in Table 1, and the Rehm-Weller equation, we extended our results to compounds 19 to 29.

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Red E ¼ 0:9721 Ln n ð Þ-2:6088: ð7Þ Using these equations, we derived a good approximation for extending the formulas for the E aa and the Red E to [SWCNT(5,5)-armchair-C n H 20 ] (n = 200 to 300) 19 to 29.
The relative structural coefficients, the E aa (in eV), and the Red E (in V) of [SWCNT(5,5)-armchair-C n H 20 ] (n = 20 to 190) 1 to 18 are found in Table 1. The relationship between this index and the first and second free energies of electron transfer (ΔG et(n) , n = 1,2), as assessed using the Rehm-Weller equation based on the first and second oxidation potentials ( ox E 1 and ox E 2 ) of A to E for the predicted supramolecular complexes between 1 to 18 with the η 2_ C m Pd(dppf), η 2_ C m Pd(dppr), and η 2_ C m Pd  Figure 2 shows the relationship between the number (n) of carbon atoms in the [SWCNT(5,5)-armchair] 1 to 18 and the first and second free energies of electron transfer (ΔG et(n) , n = 1,2 kcal mol −1 ) of the ligands η 2_ C 60 Pd(dppf ) (A). These data were fit using a regression with a second-order polynomial. The R 2 values for these graphs were 0.9461. We calculated the values of  (Tables 1 and 3).
The Marcus theory is currently the dominant theory of electron transfer in chemistry. This theory is widely accepted because it accurately predicts electron transfer rates. The most significant prediction is that the rate of electron transfer will increase as the electron transfer reaction becomes more exergonic, but only to a point [37][38][39][40][41][42].
ET is one of the most important chemical processes in nature and plays a central role in many biological, physical, and chemical (both organic and inorganic) systems. Solid-state electronics depends on controlling ET in semiconductors. Current molecular electronics depends critically on understanding and controlling the transfer of electrons in and between molecules and nanostructures. Electron transfer is a very simple chemical reaction, which  can be used to gain insight into other kinds of chemistry and biochemistry. Electron transfer is fundamental in chemistry [37][38][39][40][41][42]. The free energy of electron transfer ΔG et is the difference between the reactants and the products, and ΔG et # is the activation energy. The reorganization energy is the energy required to force the reactants to have the same nuclear configuration as the products without permitting the electron transfer. If the entropy changes are ignored, the free energy becomes energy or potential energy [37][38][39][40][41][42].
Using Equation 2, we calculated the first and second activation free energies of electron transfer, ΔG # et(n) , for 30 to 174 in accordance with the Marcus theory; see Table 4. Figure 3 shows the surfaces of the free energies of electron transfer ΔG et(n) and ΔG et(n) # (n = 1,2) between [SWCNT (5,5)-armchair-C n H 20 ] (n = 20 to 300) 1 to 29 and the ligands η 2_ C m Pd(dppf), η 2_ C m Pd(dppr), and η 2_ C m Pd (dppcym) 2 Table 3. As shown in Figure 2, the periodicity of the plotted points is 3, which is common among benzenoids. Using  Figure 3 shows the free energy surfaces of electron transfer ΔG et(n) and ΔG et(n) # (n = 1,2) between 1 to 29 and the ligands A to E in the structures of 30 to 174, which were calculated using equations 1 to 17 and are shown in Tables 1, 2, 3, 4, and 5. With the appropriate equations, we calculated the E aa , the Red E in 1 to 18 and 19 to 29, the first and second free energies of electron transfer (ΔG et in kcal mol −1 ), and the first and second activation free energies of electron transfer ΔG # et(n) for 30 to 174 in accordance with the Marcus theory.
We determined the values of the maximum wavelengths (λ (n) ; n = 1 or2, in nm) for each stage of the electron transfer process in the nanostructure supramolecular complexes 30 to 174 with Planck's formula. Using this formula, we also determined the activation free energy of the electron transfer process. Most of the values were found in the UV-vis (190 to 800 nm) range of the (1) G et (2) Ligands 2_ C m Pd(dppf), 2_ C m Pd(dppr) and 2_ C m Pd(dppcym) 2 Table 5).

Conclusions
The complexes η 2_ C m Pd(dppf ), η 2_ C m Pd(dppr), and η 2_ C m Pd(dppcym) 2 (m = 60 and 70) (A to E) contain a strongly electron-withdrawing fullerene cage and a metallocene group, which can be either electron releasing (ruthenocene) or electron withdrawing (cymantrene) and is linked with the cage through a bisdiphenyl phosphinepalladium bridge. The oxidation potentials Table 5 Values of the first and the maximum wave lengths for each stage of the ET process ( ox E 1 and ox E 2 ) of η 2_ C m Pd(dppf ), η 2_ C m Pd(dppr), and η 2_ C m Pd(dppcym) 2 (m = 60 and 70) (A to E) have been reported. In this study, we identified structural relationships between the number of carbon atoms and the E aa , the values of the Red E of [SWCNT(5,5)-armchair-C n H 20 ] (n = 20 to 300) 1 to 18 and 19 to 29, the ΔG et (n) , and the ΔG # et(n) for the complexes 30 to 174. The number of carbon atoms is strongly correlated with the values of E aa and Red E in the (5,5) armchair SWCNT 1 to 18 and 19 to 29, which are important factors in characterizing these materials. The values of ΔG et(n) and ΔG # et(n) (n = 1,2) were calculated using the Rehm-Weller equation and Equations 2 and 3 for 30 to 119 and 120 to 174 supramolecular nanostructure complexes, respectively. The maximum wavelengths of the electromagnetic photons in the photoelectron transfer process for each stage (λ (n) ; n = 1 to 2, in nm) of the nanostructure complexes 30 to 174 were calculated with Planck's equation. The novel supramolecular complexes and the calculated values have neither been synthesized nor reported previously. Using this model and the associated equations, we can easily calculate the E aa , Red E, ΔG et(n) , ΔG # et(n) (kcal mol −1 ), and λ (n) (n = 1,2; in nm) of this family of compounds 30 to 174 with good approximation.