Chromium tricarbonyl η6-Complexes of (R)-[6]helicene -A DFT Study

Research Article 

Chromium tricarbonyl η6-Complexes of (R)-[6]helicene -A DFT Study

Corresponding author:  Dr. Lemi Türker, Middle East Technical University Department of Chemistry, Ankara-Turkey, Fax: +90-312 2103200; E-mail.
Isomeric chromium tricarbonyl η6-complexes of (R)-[6]helicene have been considered theoretically at the level of DFT ( as B3LYP/ 6-31G(d,p), B3LYP/LANL2DZ, B3LYP/SBKJC and B3LYP/6-31G(d,p)// B3LYP/SBKJC) in order to investigate some molecular orbital, electronic and thermodynamic properties. The chromium tricarbonyl η6-complex is formed each time on different ring of (R)-[6]helicene molecule ( on the same side of the molecular surface) to get the isomeric complexes and the effect of complexation on the stability and aromaticity of (R)-[6]helicene has been investigated by means of energy and NICS calculations results. Some geometrical and quantum chemical properties were obtained. Additionally, the calculated vibrational and UV/VIS spectra of the complexes were produced.Keywords: Hexahelicene; Chromium Tricarbonyl Complexes; DFT Calculations; Nics(0) Calculations

Helicenes are screw-shaped chiral molecules consisting of ortho-fused aromatic rings [1,2]. A striking physical property of helicenes is their optical activity to rotate plane-polarized light with an extraordinarily high specific rotation [3]. The property of super chirality enables helicenes to be used in many applications such as photo-optical switches [4] and enantioselective fluorescence detectors [5]. Hexahelicene ([6]helicene) was the first example of the helicene family that was synthesized and then optically resolved [6].

On the other hand, various η6-arene transition metal complexes are known. Of these, the arene-chromium tricarbonyl derivatives have been the most extensively studied ones [7-17]. The linkage of a metal tricarbonyl moiety to an aromatic compound can induce several consequences including, activation of the aromatic ring to nucleophilic attack, steric inhibition of attack on functional groups from the same side as the metal carbonyl group, enhancement of aryl-H acidities, stabilization of any charge on carbons α and β to the arene-metal moiety , etc. [7]. The attachment of Cr(CO)3 groups to an aromatic system leads to an activated attack of nucleophiles because the metal group acts as a kind of electron sink [7]. Moreover, in some cases, complex formation stabilizes the system which is otherwise unstable.

One of the first striking features of π-coordinated metal complexes, such as the chromium tricarbonyl complex coordinated to polycyclic aromatic hydrocarbons (PAHs), is their ability to undergo thermal η66-inter-ring haptotropic rearrangements (IRHR). That is the π-coordinated metal migrates between different rings of the PAH [18-26]. Haptotropic shifts can be of the σ–σ (sigmatropic rearrangement), σ–π, or π–π type. The haptotropic shift in organometallic species of π-ligands has been extensively studied in cyclic polyenes, such as cyclopentadienyl, indenyl, and anthracenyl ligands [20]. A reversible haptotropic shift has been applied to molecular switches [20].

The simplest system is to be mentioned where a haptotropic shift of ligand takes place is the (η6-naphthalene)-Cr(- CO)3 complex and their derivatives. On these species, various mechanistic studies have been performed to investigate the nature of η6-coordinated metal binding [27-29]. It has been found that the interactions between low-lying unoccupied orbitals (LUMO) of the Cr(CO)3 and high-lying occupied π-orbitals (HOMO) of naphthalene represent the dominant bonding mechanism. It has been observed that the chromium tricarbonyl moiety acting in these complexes as a powerful electron withdrawing group [30]. Moreover, some DFT calculations appeared in the literature recently on the Cr(CO)3 complexes of some polycyclic hydrocarbons [31-35]. The η6-hexahelicene complexes of iridium and ruthenium have been prepared. The results of final thermodynamic products have indicated that the η6-coordination of the metal fragment occurs to the helicene terminal ring [36].

Also, some DFT calculations have been performed on hexahelicene derivatives [37-40]. Abbate et al., studied the vibrational circular dichroism (VCD) and IR absorption spectra of the (-)-enantiomer of 2-Br-hexahelicene. They have measured and interpreted the results by use of density functional theory (DFT) calculations [37].

In the present treatise, chromium tricarbonyl η6-complexes of R-[6]helicene have been considered within the constraints of density functional theory (DFT).


The initial geometry optimizations of all the considered structures leading to energy minima have been achieved by using first MM2 (molecular mechanics) method followed by semi-empirical PM3 self-consistent fields molecular orbital (SCF MO) method [41,42] at the restricted level [43]. Subsequent geometry optimizations have been achieved by using various restricted Hartree-Fock (RHF) methods successively and finally optimizing within the framework of density functional theory (DFT, B3LYP) [44,45] using LANL2DZ [46,47] and SBKJC [48] and 6-31G(d,p) basis sets. It has to be noted that the exchange term of B3LYP consists of hybrid Hartree–Fock and local spin density (LSD) exchange functions with Becke’s gradient correlation to LSD exchange [45,49]. The correlation term of B3LYP consists of the Vosko, Wilk, Nusair (VWN3) local correlation functional [50] and Lee, Yang, Parr (LYP) correlation correction functional [51].

In the present study, for each set of calculations, also vibrational analyses have been done (using the same basis set employed in the corresponding geometry optimization). The normal mode analysis for each structure yielded no imaginary frequencies for the 3N−6 vibrational degrees of freedom, where N is the number of atoms in the system. This result indicates that the structure of each molecule corresponds to at least one local minimum on the potential energy surface. All these computations were performed by using the Spartan 06 [52] package program.

Absolute NMR shielding values [53] were calculated using the Gauge-Independent Atomic Orbital method [54] with the restricted closed shell formalism employing B3LYP/6-31G(d,p) type NICS calculations over the B3LYP/SBKJC optimized geometries and LANL2DZ basis set over B3LYP/ LANL2DZ optimized geometries as well as. The NICS values have been obtained by calculating absolute NMR shielding at the ring centers, NICS (0). The NICS calculations of the present systems have been performed by the use of Gaussian 03 package program [55].

Results and Discussion

The present study considers isomeric chromium tricarbonyl η6-complexes of (R)- [6]helicene. The chromium tricarbonyl moiety has been η6-complexed with each benzenoid ring of (R)-[6]helicene at a time. The [6]helicene under investigation was constructed in R-stereochemistry ((R)-[6]helicene) and the complexation was achieved in each case on the same surface (upper surface) of the (R)-[6]helicene.

For the calculations, LANL2DZ , SBKJC and also 6-31G(d,p) (as B3LYP/6-31G(d,p) and B3LYP/6-31G(d,p)//B3LYP/SBKJC) basis sets have been employed with the B3LYP functional at the restricted level. Note that these bases sets are suitable for transition metals [46-48,56].


Figure 1 shows the numbering and some bond lengths of ((R)-[6]helicene [57] and its calculated bond lengths at the levels of B3LYP/ LANL2DZ , B3LYP/ SBKJC and B3LYP/6-31G(d,p). As seen in the figure B3LYP/ LANL2DZ and B3LYP/6-31G(d,p) type calculation yields much closer bond lengths to the experimental values indicated in the figure.
The bond lengths obtained using SBKJC basis set are a little bit longer than the other calculated bond length values. However, LANL2DZ basis set cannot predict the direction of the dipole moments correctly. The attachment of Cr(CO)3 moiety to an aromatic ring attracts electrons acting as a kind of electron sink [7]. Therefore, the tip point of the dipole moment is expected to be somewhere nearby the ligand, whereas LANL2DZ type calculations locate the positive end on the ligand. The other basis sets presently employed with B3LYP functional correctly estimates the dipole moment direction. However, the magnitudes of all the dipole moments are obviously basis set dependent and quite different from each other (just as two examples see Tables 1 and 2).

Table 1 shows some bonding distances and the magnitudes of the dipole moments calculated at the level of B3LYP/SBKJC. The dipole moment values are quite high. The LANL2DZ basis set yields even much greater dipole moment values (106-130 Debye, see Table 2). The high values for dipole moments must be due to the opposite charge centers being far away from each other and also different magnitudes of the charges estimated by different methods for the same centers. The dipole moment orders are as follows; 6>1>2>5>3>4 (B3LYP/SBKJC); 1>2>5>6>3>4 (B3LYP/LANL2DZ); 1>3>5>4>6>2 (B3LYP-6- 31G(d,p)); and 5>4>3>2>1>6 (B3LYP-6-31G(d,p)// B3LYP/SBKJC).


Figure 1. Numbering and some bond lengths of hexahelicene [57] and its calculated bond lengths at various levels.

Figure 2. Optimized structures of the complexes considered (B3LYP/SBKJC).

All the complexes studied presently possess C1 symmetry. Figure 2 shows the optimized geometries of the complexes presently concerned (B3LYP/SBKJC). Note that dipole moment vector in each case originate somewhere in the helicene structure and aiming to the chromium ligand.

Note that the Cr-CO bond vectors have a staggered arrangement with respect to the carbon atoms of the ring where the complex formation occurred. Tables 1 and 2 show also Cr-CO and η6-bond lengths and of the complexes considered (B3LYP/
SBKJC and B3LYP/LANL2DZ, respectively).

Generally, Cr-CO bond lengths are comparable. The η6-bond is the longest for structure-5 followed by structure-4. Whereas 1 is characterized with the shortest η6-bond (Tables 1 and 2). The order is 1<6<2=3<4<5. The same order is produced by B3LYP/LANL2DZ type calculations (Table 2).

Electronic Energies

Table 3 shows the total electronic energy values for complexes 1-6, calculated at various levels. The corrected total electronic energy (Ecorr) includes the zero points vibrational energy term (ZPE). The B3LYP/SBKJC and B3LYP/LANL2DZ level of energy calculations (although the magnitudes are very different) produce the same order of stabilities, that is 1>3>2>4>6>5. Whereas B3LYP/6-31G(d,p) and B3LYP/6-31G(d,p)//B3LYP/ SBKJC stability orders are 2>4>5>6>3>1 and 2>1>3>6>4>5, respectively.

The stabilities of these complexes should be the implicit functions of their gross and fine topologies including curvature of the skeleton, the degree of π-conjugation between the adjacent rings etc. The most stable structure-1 is expected ( as produced by B3LYP/SBKJC and B3LYP/LANL2DZ level of calculations) if one considers the number of Clar’s sextets [58] in these isomeric structures. In structure-1, the Clar’s sextet can shift over five rings which contributes to the stability. Whereas in the other isomers less number of Clar’s sextets exists along the ribbon of hexagons. In that respect, the order of stability estimation by B3LYP/6-31G(d,p) type calculations should be unlikely. The B3LYP/6-31G(d,p)// B3LYP/SBKJC calculations also yield somewhat unexpected order. However, isomer-5 in all the cases, except B3LYP/6-31G(d,p) is expected to be the least stable one among the isomeric series.

The energy differences between structures 2 and 3 in one hand and 3 and 4 in the other are rather small. Then, if the activation energies for the haptotropic shift of the ligand are favorable, these structures should be pair wise interconvertible.

In general, shifts of the π–π type have relative low activation energies. At room temperature, complexes that present haptotropic phenomena are very fluxional, and it is common to find them in equilibrium[59]. The fluxionality of these complexes gives the possibility to use them as molecular switches. There is at least one example with aromatic polycyclic ligands in which it was possible to control the direction of the equilibrium by changing the conditions of the system [20]. There are several studies of haptotropic shifts in complexes with aromatic polycyclic ligands, like naphthalene or anthracene, where the metal moves across the rings [31,60-62]. Note that the larger the ring, and the larger its π system, the easier the slippage becomes [24]. This behavior is explained by the fact that larger rings bind more weakly to the metal centers when they are η5 coordinated. With cyclopentadienyl ligand, η3-Cp rings have not often been observed [63]. On the other hand, heterocycles exhibit a marked tendency to coordinate η1. Clear η3 coordination has never been observed (and was predicted to be unfavored relative to η1 ), although η5 coordination has been achieved when adequate substituents are. Also, a large number of haptotropic rearrangements in aromatic ligands were disclosed and qualitatively studied for many transition metals including Mo, W, Rh, Pd, Ir, Ni, Mn, Fe, Zr, Ru, and Os [61]. There are two kinds of haptotropic rearrangements: intra- ring haptotropic (when the metal fragment changes its p-coordination to the organic ligand within the same ring) and inter-ring haptotropic (involving migration of organometallic group from one of the aromatic ring to the other) [61]. The dynamic behavior of fluxional organometallic systems was tried to be theoretically investigated and all were revised [59]. In the present case, the chromium moiety should undergo 1,2-shift sequentially somewhat parallel to the shift of Clar’s sextet. Since strongly aromatic rings will be less willingly to donate electrons and the metal atom acts as an electron sink [7] then the metallic moiety should shift to the comparatively less aromatic ring.


The simplest criterion for aromatic compounds is that the presence of cyclic conjugated π-systems containing the proper number of π-electrons (i.e., the Hückel rule). While this criterion is enough to predict the aromaticity of a neutral and charged monocyclic ring systems, it is not always a clear indicator of aromaticity for more complex systems.

Aromaticity is expressed by a combination of various properties in cyclic delocalized systems. In general, aromaticity is discussed in terms of energetic, structural and magnetic criteria [64-69]. In 1996, Schleyer has introduced a simple and efficient probe for aromaticity: Nucleus-independent chemical shift (NICS) [70], which is the computed value of the negative magnetic shielding at some selected point in space, generally, in a ring or cage center. It is known in the literature that negative NICS values denote aromaticity (-11.5 for benzene, -11.4 for naphthalene) and positive NICS values denote antiaromaticity (28.8 for cyclobutadiene) while small NICS values indicate non-aromaticity (-2.1 for cyclohexane, -1.1 for adamantane). NICS may be a useful indicator of aromaticity that usually correlates well with the other energetic, structural and magnetic criteria for aromaticity [71-74]. Resonance energies and magnetic susceptibilities are measures of the overall aromaticity of a polycycle but do not provide information about the individual rings. In contrast, NICS has been proved to be an effective probe for local aromaticity of individual rings of polycyclic systems.

Table 4 shows the NICS(0) values of the (R)-[6]hexahelicene rings of structures 1 (the most stable complex expected by B3LYP/SBKJC and B3LYP/LANL2DZ type calculations) and 5 (the least stable complex estimated by all except B3LYP/ 6-31G(d,p) level of calculations).

In Table 4, the NICS(0) values are the crop of B3LYP/6-31G(d,p) level of calculations based on B3LYP/SBKJC geometry optimization. Note that the SBKJC and 6-31G(d,p) basis sets predict the direction of dipole moment correctly in contrast to the LANL2DZ basis set. Thus, B3LYP/SBKJC and B3LYP/6-31G(d,p) level of calculations should estimate the charge distribution in the complexes considered better than the B3LYP/ LANL2DZ level. The aromaticity order for the rings (A-F) based on NICS(0) values for complexes 1 and 5 are F>C>D>E>B and A>F>C>B>D, respectively. The common point between the aromaticity order of rings of structures 1 and 5 is that the ring occupying the position farthest away from the complex formed ring is the most aromatic one (namely F and A rings in 1 and 5, respectively).

The NICS(0) values of the other rings should be dictated by some subtle factors, such as the bond lengths of the ring, the curvature of the helix at the ring of interest etc. Note that the η6-bond in structure 5 is notably longer than the respective
bond in other complexes (see Tables 1 and 2).

The NICS(0) values calculated by using B3LYP/LANL2DZ level (Table 5) fall into the decreasing order of aromaticity as F>B>C>E>D and A>F>C>D>B for structures 1 and 5, respectively. Note that the both level of calculations predicts ring-F as the most aromatic in structure-1. For structure-5 the aromaticity order of A>F>C is predicted by the both levels of calculation.

In Table 5, due to the fastness of computations, LANL2DZ basis set has been employed for comparison purpose of local aromaticity of the rings in the presence and absence of the ligand. In the table, decomposed means the ligand (Cr(CO)3) moiety has been removed from the complex keeping the geometry of helicene as it was in the complex. The results reveal that the complexation increases the aromaticity of rings so that B>C>E and decreases the aromaticity in rings D and F in structure-1. Whereas in 5, by complexation the aromaticity of rings A,B and C increases but the respective property of rings D and F decreases (F>D). It seems that the complexation increases the aromaticity of the adjacent ring(s) in structure-1 but decreases in structure-5. It might be due to the variations in local electron density (caused by the complexation) which is contributed to the π-electron delocalization in each individual ring.

IR Spectra

Table 6 shows some characteristic IR bands for the most stable and least stable isomers (B3LYP/SBKJC), namely 1 and 5, respectively. Figure 3 shows the IR spectra of (R)- [6]helicene and its complexes 1 and 5 considered presently. Note that they have been the calculated spectra at the same level. The strongest bands in the figure for the complexes stand for the carbonyl stretching.

UV-VIS Spectra

All the calculated UV-VIS spectra presently obtained within DFT approach are actually the product of time-dependent density functional (TD-DFT) treatment. B3LYP/LANL2DZ and B3LYP/SBKJC level of calculations for the UV-VIS spectra yield similar spectra. Figure 4 shows B3LYP/SBKJC spectra for the complexes. The spectrum of complex-1 spans from 300 nm to 600 nm. As the complexation site moves from ring B to E the spectra exhibit bathochromic shift, eg., spans from 350 nm to 650 nm. For complex-5 the range covers 375- 750 nm. Note that complex-5 has the longest η6-Cr bonding, less electron withdrawing by the ligand and better π-electron delocalization over the helix, thus causing a bathochromic shift. As the complexation occurs at ring-6, the range of absorption wavelengths confines back to 300-640 nm.

Table 7 shows the main strong absorption peaks of the complexes. The starred ones are the strongest among the sets. The table also contains the HOMO-LUMO energy gaps (Δε) of the complexes calculated at the level of B3LYP/SBKJC (see Table 8).

Figure 3. IR spectra of (R)-[6]helicene and structures 1 and 5 (B3LYP/SBKJC).

Figure 4. UV-VIS spectra of some of the complexes (B3LYP/SBKJC).

In the case of polycyclic benzenoid hydrocarbons, α-bands are often the longest wavelength bands in their spectra [75]. The p-bands are moderately strong whereas mostly β-bands are very intense. The p-bands are generally more sensitive to structural changes than the α-bands. When the order of Δε values in Table 7 ( see also Table 8) are compared with the order of the strongest bands of the complexes, one finds not a direct parallelism comprising all the complexes considered. However, the strongest peak of structures 1,2,5 and 6 exhibit some correlation with Δε, the interfrontier molecular orbital energy gap. Their longest wavelengths also show bathochromic shift as Δε values decreases, thus they should be the p-bands, originating from the HOMO-LUMO transition.

Figure 5 shows some of the molecular orbital energies of (R)- [6]helixcene and its considered complexes 1 and 5. Note that the HOMO and LUMO energy levels are closer to each other in complex-5 than the complex-1 and (R)-[6]helicene (see Figure 5 ).

Figure 5. Some of the molecular orbital energy levels of hexahelicene and structures-1 and 5 (B3LYP/SBKJC).

Note also that the η6-bond in structure-5 has the longest one. Thus the ligand attracts the electrons less effectively. Consequently, perturbation in the electron population in other rings is less which means relative to structure-1, better conjugation exists in structure-5. The other factor might be the curvature of the helix in each complex. Depending on it, the π-electron conjugation between the rings might vary. Note that the increased conjugation causes the narrowing of the interfrontier molecular orbital energy gap, resulting in a bathochromic shift [76].

The Δε order is estimated as 4>3>1>6>5>2 by B3LYP/SBKJC type calculations.

The isomeric chromium tricarbonyl η6-complexes of (R )-[6] helicene have been subjected to DFT treatment at the different
level of calculations. Except for LANL2DZ basis set, the others presently employed predict the direction of dipole moments correctly. However, SBKJC and LANL2DZ basis sets predict the same stability order which seems in accord with some of the literature data of other types of complexes of helicene. Of the present complexes, the most stable and least stable ones are considered for NICS(0) calculations that the values show variation depending on the site of complexation. The order of NICS(0) values of the rings are basis set dependent, however, both the methods used for that purpose indicate that F-ring in structure-1 and A-ring in structure-5 are the most aromatic ones, respectively.

The calculated UV-VIS spectra, generally exhibit some slight bathochromic effect as the complexation site varies from ring-A to ring-D, gets the maximum value for ring-E and then the domain of wavelengths shrinks almost to the range of structure-3.

All these observations show that not only the gross but also the fine topology of these complexes are important factors dictating various properties of them.


1. Balaban AT. Chemical graphs. Part 50. Symmetry and enumeration of fibonacenes   (unbranched catacondensed benzenoids isoarithmic with helicenes and zigzag catafusenes).  Match Commun Math Comput Chem. 1989, 24: 29-38.

2. Martin RH. The Helicenes. Angew Chem Int Ed Engl. 1974, 13(10): 649-660.

3. Martin RH, Libert V. Helicenes. The Use of Resolved Hexahelicene-2-carboxylic Acid as a Common Precursor for the Photochemical Synthesis of Optically Pure Octa-, Nona-, Deca-, Undeca-, and Tridecahelicenes. Thermal Racemization of Deca- and Undecahelicenes. J Chem Res Synop. 1980, 4: 130-131.

4. Chen CT, Chou YC. C2-Symmetric dibenzosuberane-based helicenes as potential  chirochromic optical switches. J Am Chem Soc. 2000, 122(32): 7662-7672.

5. Reetz MT, Sostmann S. 2,15-Dihydroxy-hexahelicene (HELIXOL): Synthesis and use as an enantioselective fluorescent sensor. Tetrahedron. 2001, 57(13): 2515-2520.

6. Newman MS, Lednicer D. The synthesis and resolution of hexahelicene. J. Am. Chem.    Soc. 1956, 78(18): 4765-4770.

7. Pearson AJ: Metallo-Organic Chemistry. New York: Wiley; 1985.

8. Maity BC, Swamy VM, Sarkar A.Assembling monocyclic, spirocyclic and fused  carbocycles by ring-closing metathesis on an arene-chromium template. Tetrahedron Lett.  2001, 42(26): 4373-4376.

9. Bolm C, Muñiz K. Planar chiral arene chromium(0) complexes: Potential ligands for asymmetric catalysis. Chem Soc Rev. 1999, 28(1): 51-59.

10. Kalpana A, Akilandeswari L. The effect of fluorine substitution on the conformation and  aromaticity of η6-fluoro arene chromium tricarbonyl complexes – Density functional insights. Computational and Theoretical Chemistry. 2015,1069: 125-131.       

11. Mandal SK, Sarkar A.Engineering endo-selectivity in arene-chromium functionalizations   : out-of-plane coordination of TiCl4 to ketones leads to stereodivergence. J Org Chem.  1999, 64 (7): 2454-2458.

12. Jimenez-H JOC, Robles J, Sola M. Coordination and haptotropic migration of Cr(CO)3 in polycyclic aromatic hydrocarbons: The effect of the size and the curvature of the substrate.J. Phys. Chem. A. 2008, 112(6): 1202-1213.

13. Dunbar RC.Binding of transition metal ions to curved pi surfaces: Corannulene vs. coronene.J Phys Chem. A. 2002,106(42): 9809-9819.
14. F Nunzi, F Mercuri, A Sgamellotti, N Re .The coordination chemistry of carbon  nanotubes: A density functional study through a cluster model approach. J Phys Chem.  B.2002106(41):10622-10633.

15. Shapiro PJ, Zehnder R, Foo DM, Perrotin P, Budzelaar PHM,  Leitch S,  Twamley B. ansa-chromocene complexes. 2. isocyanide derivatives of Cr(II) and Cr(III), Their  syntheses, X-ray crystal structures, and physical properties, Organometallics. 2006, 25(3): 719–732.

16. Schaper F, Rentzsch M, Prosenc MH, Rief U, Schmidt K, Brintzinger HH .ansa-Metallocene derivatives XXXVI. Dimethylsilyl-bridged permethyl chromocene  carbonyl complexes – syntheses, crystal structures and interconversion reactions. J of  Organometallic Chemistry. 1997, 534: 67-79.

17. Shapiro PJ. The elusive chemistry of bent-sandwich chromocene. Current Organic   Chemistry. 2007, 11(17): 1482-1490.

18. B Deubzer, HP Fritz, CG Kreiter, K Ofele. Spektroskopische untersuchungen an etallorganischen verbindungen XLV.1H-NMR-spektren von naphthalin-chrom(0)- tricarbonyl und seinen derivaten. J. Organomet Chem. 1967, 7(2): 289-299.

19 Muller J, Goser P, Elian M. Dibenzo[a,e]cycloocten-komplexe des chroms und  molybdäns. Angew Chem Int. Edit. 1969, 8: 374-375. 

20.  Dötz KH, Jahr HC. Tunable haptotropic metal migration in fused arenes: towards  organometallic switches. Chem Rec. 2004, 4(2): 61-71.

21. Suzuki N, Hashizume D, Yoshida H, Tezuka M, Ida K, Nagashima S, Chihara T.  Reversible haptotropic shift in zirconocene-hexapentaene complexes. J Am Chem Soc.  2009, 131(6): 2050–2051.

22. Veiros LF. Haptotropic shifts in cyclopentadienyl organometallic complexes: Ring  folding vs ring slippageOrganometallics. 2000,19(26): 5549-5558.

23. Veiros LF. Haptotropic shifts in organometallic complexes with η5-coordinated π ligands. Journal of Organometallic Chemistry. 1999, 587(2): 221–232.

24. Calhorda MJ,Veıros LF. Haptotropic shifts of indenyl and other related πligands.  Commems Inorg Chem2001. MI. 22. No. 6. pp. 375-391.

25. Huidobro-Meezs IL, Segovia-Poncelis M, Barquera-Lozada JE.The role of  bulkiness in haptotropic shifts of metal–cumulene complexesEur. J Inorg Chem2016, 26: 4226-4233.

26. Tanabe M, Bourke SC, Herbert DE, Lough AJ, Manners I. Reversible, strain-controlled haptotropic shifts of cyclopentadienyl ligands in [1]- and  [2] metallocenophanes, Angew Chem Int Ed. 2005, 44(36): 5886 –5890.

27. TA Albright, P Hofmann, R Hoffmann, CP Lillya, PA Dobosh. Haptotropic   rearrangements of polyene-MLn complexes. II. Bicyclic polyene- MCp- M(CO)3 systems.JAm Chem Soc. 1983, 105: 3396-3411 .

28. KH Dötz, C Stinner, M Nieger. Reactions of complex ligands .67. Optically-active  naphthalene-Cr(CO)3 complexes via diastereoselective carbene annulation and  haptotropic metal migration.J Chem Soc Chem Commun.1995: 2535- 2536.

29. Merlic CA, Hietbrink BN, Houk KN. Donor and acceptor properties of the chromium  tricarbonyl substituent in benzylic and homobenzylic anions, cations, and radicals. J Org Chem. 2001, 66(20): 6738-6744.

30. CA Merlic, AL Zechman, M Miller. Reactivity of (h6-Arene)tricarbonylchromium complexes with carbenoids: Arene activation or protection? J Am Chem Soc.2001, 123(44): 11101-11102. 

31. A Arrais, E Diana, G Gervasio, R Gobetto, D Marabello et al, Stanghellini PL. Synthesis, structural and spectroscopic characterization of four [(η6‐PAH) Cr(CO)3] complexes (PAH= Pyrene, Perylene, Chrysene, 1, 2‐Benzanthracene). Eur J Inorg Chem.2004:  7: 1505-1513.

32. Ketrat S, Muller S, Dolg M.  A quantum chemical study of the haptotropic rearrangements of Cr(CO)3 on naphthalene
nd phenanthrene systems. J Phys Chem. A. 2007, 111(27): 6094-6102.

33. Türker L, Gümüş S. DFT studies on η6 -coronene-Cr(CO)complexes. Acta Chim.Slovenica. 2009, 56: 246-253.

34. Türker L, Gümüş S. Ab ınitio and DFT studies on certain η6-anthraquinone –Cr(CO)complexes. Polycyclic Arom Comp. 2008, 28(3): 181-192.

35. Türker L. Chromium tricarbonyl η-complexes of [3]cyclacens – A DFT study.2014, 640:1378-1384.

36. Álvarez CM,Barbero H, García-Escudero LA, Martín-Alvarez JM, Martínez-Pérez C, Miguel D. η6-Hexahelicene complexes of ıridium and ruthenium: Running along the helixInorg Chem. 201251(15): 8103–8111.

37. Abbate S, Lebon F, Longhi G, Fontana F, Caronna T,  Lightner DA. Experimental and  calculated vibrational and electronic circular dichroism spectra of 2-Br-hexahelicene.  Phys Chem Chem Phys. 2009,11(40): 9039-9043.

38. Thomsen C, Machón M, Bahrs S. Raman spectra and DFT calculations of the   vibrational modes of hexaheliceneSolid State Communications. 2010, 150(13–14): 628– 631.

39. Johannessen C, Blanch EW, Villani C, Abbate S, Longhi G et al. Raman and ROA spectra of (-)- and (+)-2-Br-hexahelicene: experimental and DFT studies of a π-conjugated chiral system. J Phys Chem. B. 2013,117(7): 2221-2230.

40. Liégeois V, Champagne B. Vibrational Raman optical activity of π-conjugated helical systems: Hexahelicene and heterohelicenes. Journal of Computational Chemistry. 2009, 30(8): 1261–1278.

41. Stewart JJP. Optimization of parameters for semi empirical methods I, Method. J    Comput Chem. 1989, 10(2): 209–220.

42. Stewart JJP. Optimization of parameters for semi empirical methods II, Appl J Comput  Chem. 1989, 10(2): 221–264.

43. Leach AR: Molecular Modeling. Essex: Longman; 1997.

44. Kohn W, Sham LJ. Self-consistent equations including exchange and correlation effects. Phys Rev. 1965, 140 : 1133–1138.

45. Parr RG, Yang W: Density   Functional   Theory of Atoms and Molecules. London:  Oxford University Press; 1989.

46. Bytheway I, Wong MW. The prediction of vibrational frequencies of inorganic   molecules using density functional theory. Chemical Physics Letters. 1998, 282, (3–4) : 219–226.

47. Chiodo S, Russo N, Sicilia E.LANL2DZ basis sets recontracted in the framework of density functional theory. J Chem Phys. 2006,125(10): 104107.

48. Vidal LN, Vazquez PAM. Electrically polarized valence basis sets for the SBKJC effective core potential developed for calculations of dynamic polarizabilities and Raman  intensities. Theoretical Chemistry Accounts. 2012, 131(2): 1111-1114.

49. Becke AD. Density-functional exchange-energy approximation with correct asymptotic behavior. Phys Rev. 1988, A 38 : 3098–3100.

50. Vosko SH, Vilk L, Nusair M. Accurate spin-dependent electron liquid correlationenergies for local spin density calculations: A critical analysis. Can J Phys. 1980, 58(8):  1200–1211.

51. Lee C, Yang W, Parr RG. Development of the Colle–Salvetti correlation energy formula   into a functional of the electron density. Phys Rev. 1988, B 37(2): 785–789.

52. SPARTAN 06. Wavefunction Inc., Irvine CA, USA, 2006.

53. Pulay PJ, Hinton F, Wolinski K: Nuclear magnetic shieldings and molecular tructure.Eds. Tossel, J.A. NATO ASI Series C, vol. 386, Netherlands: Kluwer, 1993, 243.

54. Hehre WJ, Radom L, Schleyer PR, Pople JA: Ab Initio Molecular Orbital Theory. New      York: Wiley; 1986.

55. Frisch MJ, Trucks GW, Schlegel, HB, Scuseria GE, Robb MA, Cheeseman JR,      Montgomery, Jr., JA, Vreven T, Kudin KN, Burant JC, Millam JM, Iyengar SS, Tomasi J,      Barone V, Mennucci B, Cossi M, Scalmani G, Rega N, Petersson GA, Nakatsuji H, Hada       M, Ehara M, Toyota K, Fukuda R, Hasegawa J, Ishida M, Nakajima T, Honda Y, Kitao O,      Nakai H, Klene M, Li X, Knox JE, Hratchian HP, Cross JB, Bakken V, Adamo C,       Jaramillo J, Gomperts R, Stratmann RE, Yazyev O, Austin AJ, Cammi R, Pomelli C,      Ochterski JW, Ayala PY, Morokuma K, Voth GA, Salvador P, Dannenberg JJ,      Zakrzewski VG, Dapprich S, Daniels AD, Strain MC, Farkas O, Malick DK, Rabuck AD,       Raghavachari K, Foresman JB, Ortiz JV, Cui Q, Baboul AG, Clifford S, Cioslowski J,       Stefanov BB, Liu G, Liashenko A, Piskorz P, Komaromi I, Martin RL, Fox DJ, Keith T,  Al-Laham MA, Peng CY, Nanayakkara A, Challacombe M, Gill PMW, Johnson B, Chen      W, Wong MW, Gonzalez C, Pople JA, Wallingford CT : Gaussian, Inc., 2004.

56. Young DC. Computational Chemistry. New York: Wiley; 2001.

57. Aloui F, El Abed R, Guerfel T, Hassine BB. Synthesis and X-ray analysis of a new [6]helicene. Synthetic Communications. 2006, 36(11): 1557-1567.

58. Clar E. The Aromatic Sextet. London : Wiley; 1972.

59. Mann BE. Fluxionality of polyene and polyenyl metal complexes. Chem Soc Rev. 1986, 15: 167–187.

60. Stanger A. Is the haptotropic rearrangement in bis(tributylphosphine) (anthracene)  nickel inter-or intramolecular? Determination of the molecularity by a spin saturation    transfer. Organometallics.1991, 10(8): 2979–2982.

61. Oprunenko YFInter-ring haptotropic rearrangements in π complexes of transition  metals with polycyclic aromatic ligands. Russ Chem Rev. 2000, 69: 683–704.
62.  Dotz KH, Stendel J, Muller S, Nieger M, Ketrat S, Dolg M, Haptotropic meta  migration in densely substituted hydroquinoid phenanthrene Cr (CO) 3 complexes.   Organometallics 2005, 24(13): 3219–3228.

63. Huttner G, Brintzinger HH, Bell LG, Frieddrich P, Bejenkc V et al. The structure of (C5H5)2W(CO)2a compound containing a benttrihapto-cyclopentadienyl ligand. J Organomet Chem1978, 141: 329-333.

64. Minkin VI, Glukhovtsev MN, Simkin BY: Aromaticity and Antiaromaticity: Electronic  and Structural Aspects. New York: Wiley; 1994.

65. Schleyer PR, Jiao H. What is aromaticity? Pure Appl Chem. 1996, 68(2), 209-218.
66. Glukhovtsev MN. Aromaticity today: Energetic and structural criteria. J Chem Educ. 1997, 74(1):132-136.

67. Krygowski TM, Cyranski MK, Czarnocki Z, Hafelinger G, Katritzky AR. Aromaticity: A  theoretical concept of immense practical importance. Tetrahedron. 2000, 56, 1783- 1796.

68. Schleyer PR. Introduction: Aromaticity. Chem Rev. 2001, 101(5), 1115-1118.

69. Cyranski MK, Krygowski TM, Katritzky AR, Schleyer PR. To what extent can  aromaticity be defined uniquely? J Org Chem. 2002, 67, 1333-1338.

70. Schleyer PR, Maerker C, Dransfeld A, Jiao H, Hommes NJRE. Nucleus-  independent chemical shifts: a simple and efficient aromaticity probe. J Am Chem Soc. 1996, 118(26), 6317-6318.            

71. Jiao H, Schleyer PR. Aromaticity of pericyclic reaction transition structures: Magnetic  evidence. J Phys Org Chem. 1998, 11(8-9), 655-662.

72. Schleyer PR, Kiran B, Simion DV, Sorensen TS. Does Cr (CO)3 complexation reduce  the aromaticity of benzene? J Am Chem Soc. 2000, 122(3), 510–513.

73. Quinonero D, Garau C, Frontera A, Ballaster P, Costa A et al. Quantification of  aromaticity in oxocarbons: the problem of the fictitious “nonaromatic” reference   system. Chem Eur J. 2002, 8(2), 433-438.

74. Patchkovskii S, Thiel W. Nucleus-independent chemical shifts from semiempirical   Calculations. J Mol Model. 2000, 6, 67-75 .

75. Streitwieser A, Jr: Molecular orbital Theory for Organic Chemists. New York: Wiley;  1961.

76. Fleming I. Frontier Orbitals and Organic Chemical Reactions. London: Wiley; 1976.

Be the first to comment on "Chromium tricarbonyl η6-Complexes of (R)-[6]helicene -A DFT Study"

Leave a comment

Your email address will not be published.