Probing the Origin of Challenge of Realizing Metallaphosphabenzenes: Unfavorable 1,2-Migration in Metallapyridines Becomes Feasible in Metallaphosphabenzenes.

Metallabenzenes have attracted considerable interest of both theoretical and experimental chemists. However, metallaphosphabenzene has never been synthesized. Thus, understanding the origin of the challenge of synthesizing metallaphosphabenzene is particularly urgent for experimentalists. Now density functional theory (DFT) calculations have been carried out to examine this issue. Our results reveal that the 1,2-migration in metallapyridines is unfavorable whereas such a 1,2-migration in metallaphosphabenzenes is feasible, which can be rationalized by the reluctance of phosphorus to participate in π bonding. In addition, π-donor ligands and the 5d transition metals can stabilize metallaphosphabenzenes. Compared with hydride and methyl migration, the chloride migration has a relatively lower activation barrier due to the polarization of the M=P bond. CO ligand could further decrease the reaction barrier of the migration due to the reduction of the interaction between the metal centre and the phosphorus atom. All of these findings could help synthetic chemists to realize the first metallaphosphabenzene.

The chemistry of transition-class="Chemical">metal-class="Chemical">n class="Chemical">containing aromatics has attracted continuously increasing attention123456 since metallabenzene was first predicted by Hoffmann7 and isolated by Roper8. In contrast, the heteroatom-containing metallabenzenes such as metallapyrylium910, metallathiabenzene1112, metallapyridine1314, metallapyrrole1516, and metallathiophene1718 are relatively less developed. To the best of our knowledge, metallaphosphabenzene has not been synthesized so far, although its structure and property were investigated theoretically1920. The difficulties in the synthesis and isolation of metallaphosphabenzene could be due to the reluctance of phosphorus to participate in multiple bonds21, similar to our previous finding22 that 1,2-migration in metallasilabenzenes becomes favorable due to the reluctance of silicon to participate in π bonding. Thus, 1,2-migration in metallaphosphabenzenes may also occur (Fig. 1A). Another reason for the difficulties in the synthesis of metallaphosphabenzene could be facile isomerization of metallaphosphabenzene II to the corresponding η5-phosphacyclopentadiene (PCp) metal complex I, similar to that of metallabenzenes23,24. Indeed, our previous study20 shows that substituents have a significant effect on the thermodynamics and kinetics of the rearrangement reactions. Thus, an interconversion between osmaphosphabenzenes and the corresponding η5-PCp complexes can be achieved theoretically by simply tuning the substituents on the metallacycles. In comparison, the isomerization from metallaphosphabenzene II to nonaromatic analogue III has never been reported. Our ongoing interest in aromaticity2526272829303132 and reaction mechanisms3334353637 has led us to test the hypothetical isomerization of metallaphosphabenzene II to the nonaromatic analogue III as described in Fig 1A. Here we carry out thorough density function theory (DFT) calculations on this issue. How the ligands, metal centers affect the reaction mechanisms will be investigated in detail.

Figure 1

(A) Isomerizations from metallaphosphabenzenes (II) to η5-PCp metal complex (I) or non-aromatic complex (III). (B) 1,2-Migration of metallapyridines (E=N) and metallaphosphabenzenes (E=P). (C) Schematic diagram of the M=P bonding in phosphinidene complex.

Results

Thermodynamic aspect of chloride migration

In this work, we focus on ο-class="Chemical">metallaphosphabenzenes (Fig. 2, 1a–h) as a class="Chemical">n class="Chemical">phosphorus atom at the ortho position on metallaphosphabenzene, which was reported to be more stable than those at the meta and para positions by Solà and co-workers19. As shown in Fig. 2, both 1a and 1c are much more stable than their nonaromatic analogues 2a and 2c thermodynamically. In sharp contrast, complexes 2b and 2d are thermodynamically more stable than metallaphosphabenzenes 1b and 1d. This could be one of the reasons why some metallapyridines have been isolated whereas metallaphosphabenzenes have never been synthesized. Apparently, the stability of iridaphosphabenzenes and iridapyridines relative to their nonaromatic analogues increases dramatically in comparison with rhodaphosphabenzenes and rhodapyridines due to more diffuse d orbitals, in line with previous results that 5d metallacycles are more stable than their 4d analogues12319. These results are also applicable to ruthenaphosphabenzenes and osmaphosphabenzenes (Fig. 1B, 1a′–1d′ in Table 1). Especially for ruthenapyridine 1a′ and osmapyridine 1c′, both of them are much more stable than their nonaromatic 2a′ and 2c′ by fixing the N-Cl bond with the value of 1.78 Å (the N-Cl bond length in 2a) because 2a′ and 2c′ always rearranged to 1a′ and 1c′ by normal optimization.

Figure 2

Thermodynamic stabilities of metallaphosphabenzene (1a–1h) compared with its nonaromatic analogues (2a–2h) formed by chloride migration.

Table 1

Calculated reaction energies for the 1,2-migration of metallaaromatics to its nonaromatic analogues based on Fig. 1B.

Complex(1′)	M	E	L1	L2	PR(2′)
1a′	Ru−	N	Cl	Cl	35.1 (36.7)
1b′	Ru−	P	Cl	Cl	−1.4 (−0.4)
1c′	Os−	N	Cl	Cl	54.6 (56.7)
1d′	Os−	P	Cl	Cl	10.4 (10.5)
1e′	Ru	P	Cl	PH3	−2.6 (−2.4)
1f′	Ru	P	Cl	CO	−8.7 (−9.7)
1g′	Os	P	Cl	PH3	7.8 (7.1)
1h′	Os	P	Cl	CO	1.8 (1.3)
1n′	Ru	P	H	PH3	−18.9 (−20.3)
1o′	Os	P	H	PH3	−5.4 (−7.2)
1p′	Ru	P	Me	PH3	−26.9 (−28.9)
1q′	Os	P	Me	PH3	−13.6 (−14.6)

The relative Gibbs free energies at 298 K and electronic energies (in parentheses) are given in kcal mol−1.

What cclass="Chemical">auses this sigclass="Chemical">nificaclass="Chemical">nt differeclass="Chemical">nce betweeclass="Chemical">n class="Chemical">n class="Chemical">metallapyridines and metallaphosphabenzenes? It is well-known that the phosphorus atom has larger size difference in s and p valence orbitals than the nitrogen atom, leading to a lower tendency for hybridization to form multiple bonds21. Thus, the back donation from the d orbital of the metal center to the vacant p orbital of the phosphorus atom (Fig. 1C) will become weaker. Indeed, according to the NBO analysis of complexes 1c–1d (Table 2), the results indicate that the M=P bond38394041 is highly polarized toward Mδ− – Pδ+. For example, the nitrogen atom has contributed 1.27 electron population in the Ir=N double bond of 1c. In sharp contrast, the contribution from the phosphorus atom is reduced by 0.41 electron in 1d than that from the nitrogen atom in 1c. Meanwhile, the NBO charge on the phosphorus atom becomes positive, which contrasts sharply with the negative charge on the nitrogen. Therefore, the reversed M=P bond polarization plays an important role in 1,2-migration in metallaphosphabenzenes. All these results indicate that the phosphorus atom is reluctant to participate in π bonding so that 1,2-migration in metallaphosphabenzenes could become thermodynamically favorable whereas such a migration in metallapyridines is unfavorable.

Table 2

The charges and electron populations of M=E bonds (E=N, or P) in 1a–1d.

	Charge (M)	Charge (E)	Electron population (E)
1a	−0.69	−0.32	1.23
1b	−1.14	+0.88	0.83
1c	−0.57	−0.37	1.27
1d	−1.09	+0.82	0.86

Effect of ligands on the chloride migration in metallaphosphabenzenes

The effect of ligands has also been investigated to tune the stability of class="Chemical">metallaphosphabenzenes. Our results iclass="Chemical">ndicated the ligaclass="Chemical">nds have a remarkable effect oclass="Chemical">n the relative stability of class="Chemical">n class="Chemical">metallaphosphabenzenes in comparison with the nonaromatic analogues (1e–1h and 2e–2h in Fig. 2, 1e′–1h′ in Table 1). Specifically, when π-acceptor ligand CO is introduced to replace the chloride, reaction energies (Gibbs free energies) for the formation of 2f and 2h from 1f and 1h are −23.0 and −14.9 kcal mol−1, respectively, indicating that metallaphosphabenzenes prefer π-donor ligands. When the chloride is replaced by one ligand PH3, the instability of 1e and 1g is increased slightly in comparison with 1b and 1d in Fig. 2. This is understandable because the M=P double bond in metallaphosphabenzenes is strongly polarized toward Mδ− – Pδ+, indicating that the phosphorus atom is highly electron-deficient. Therefore, π-acceptor ligand CO can decrease the electron density of the metal center, thus weakening the bonding between the metal center and metal-bonded phosphorus. In other words, the M=P double bond will become weaker and the polarization will be enhanced, leading to relatively high stability of nonaromatic 2f and 2h. The stabilizing effect of ligands in metallaphosphabenzenes increases in the order CO < PH3 < Cl. Therefore, π-donor and π-acceptor ligands are suggested for the synthesis of metallaphosphabenzenes and nonaromatic analogues, respectively.

Effect of aromaticity on the chloride migration

The aromaticity effect has also been examined in class="Chemical">metallaphosphabenzenes with similar migratioclass="Chemical">n of class="Chemical">noclass="Chemical">naromatic cyclic class="Chemical">n class="Chemical">complexes by changing the M=E double bond to M-E single bond (Fig. 3A). Apparently, the 1,2-migration in nonaromatic cycles become more favorable thermodynamically. The reaction energy (ΔG) from 1i to 2i is computed to be 8.2 kcal mol−1 whereas that from 1j to 2j becomes −20.9 kcal mol−1. It is understandable because when aromaticity in the reactants is lost, such a chloride migration should become thermodynamically more favorable. The contribution from aromaticity in iridaphosphabenzene 1d is thus evaluated quantitatively (−13.8 kcal mol−1) by computing the energy difference between the reaction from 1d to 2d and that from 1j to 2j.

Figure 3

(A) Energy profiles calculated for the corresponding chloride migration of nonaromatic complexes. (B) Indene–isoindene ISE evaluations of the aromaticity of 1k–2m.

To gain an insight into the aromaticity in class="Chemical">metallaphosphabenzenes, we employed the “isomerizatioclass="Chemical">n stabilizatioclass="Chemical">n eclass="Chemical">nergy” (ISE) method, a class="Chemical">n class="Chemical">convenient tool to evaluate the magnitude of the aromaticity in the ground state and the lowest triplet state25284243. The indene-isoindene ISE approach is homodesmotic and has the advantage that all carbon atoms in the six-membered ring are sp2-hybridized in both the reactants and products. As shown in Fig. 3B, benzene and phosphabenzene have comparable ISE values (−21.8 and −21.1 kcal mol−1, respectively). Nevertheless, the ISE value of iridaphosphabenzene is just 71.6% of that in benzene, indicating the aromaticity in metallaphosphabenzenes is fairly reduced. In addition, the ISE value (−15.6 kcal mol−1) of iridaphosphabenzene is comparable to the aromaticity contribution (−13.8 kcal mol−1), indicating the reliability of our calculations.

1,2-Migration of hydride and methyl groups in metallaphosphabenzenes

To examine the sclass="Chemical">cope of our ficlass="Chemical">ndiclass="Chemical">ngs, we iclass="Chemical">nvestigated the 1,2-migratioclass="Chemical">n of hydride aclass="Chemical">nd methyl groups (Fig. 4, aclass="Chemical">nd 1class="Chemical">n′–1q′ iclass="Chemical">n Table 1). The class="Chemical">negative values iclass="Chemical">ndicate that these migratioclass="Chemical">ns are also feasible. The results iclass="Chemical">n Fig. 4 show that the thermodyclass="Chemical">namic stability of class="Chemical">n class="Chemical">metallaphosphabenzenes relative to its nonaromatic analogues with the hydride and methyl groups are higher than those with the chloride ligand, which could be mainly attributed to the higher bond strength of P-C and P-H bond than that of P-Cl in the products.

Figure 4

Thermodynamic stabilities of metallaaromatics (1n–1q) compared with its nonaromatic analogues (2n–2q) formed by hydride and methyl migration.

Kinetics of chloride, hydride and methyl migration

To have a deeper understanding of the reaction mechanisms, we have examined the kinetics of 1,2-migration from class="Chemical">metallaaromatics to its class="Chemical">noclass="Chemical">naromatic aclass="Chemical">nalogues (Fig. 5 aclass="Chemical">nd Table 3). The calculatioclass="Chemical">ns show that reactioclass="Chemical">n barriers are particularly low. All these values are lower thaclass="Chemical">n 24.2 kcal mol–1 at 25 °C acclass="Chemical">n class="Chemical">cording to the Eyring equation44. In addition, iridaphosphabenzene complexes have relative higher reaction barriers for 1,2-migration than rhodaphosphabenzene analogues. It could be due to the second-row transition metal rhodium has less diffuse d orbitals in comparison with iridium. Therefore, the Rh=P bond becomes relatively weak as evidenced by the Wiberg bond index (WBI) (1.00 and 1.07 for the Rh=P bond and Ir=P bond in 1b and 1d, respectively). The lowest barrier is found when the ligand is CO. As a strong π acceptor ligand, CO can reduce the interaction between the metal center and the phosphorus atom, thus weakening the metal-phosphorus bonds in metallaphosphabenzenes41. In addition, as shown in Table 3, the reaction barriers for the migration of hydride and methyl are a little higher than that of chloride. A plausible explanation for these general observations is clarified below. The results could be understandable because the Rh-Cl in 1e has a weaker bond strength (WBI: 0.62) than Rh-H in 1n (WBI: 0.65) and Rh-C in 1p (WBI: 0.66), respectively. In addition, it is known that the M=P bond is highly polarized in metallaphosphabenzenes, and the ligand with higher electronegativity could promote the migration. Hence, a lower barrier for migration of chloride is expected in the reaction. In sharp contrast, all the metallapyridines are thermodynamically more stable than their nonaromatic analogues (Supplementary Fig. S1 and Table S1).

Figure 5

Energy profiles calculated for the 1,2-migration of metallaaromatics to its nonaromatic analogues.

Table 3

Calculated reaction energies and barriers for the 1,2-migration of metallaaromatics to its nonaromatic analogues based on Fig. 5.

1X			1X–TS1	1X–IN1	2X
M = Os	L2 = PH3	L1 = Cl	22.2 (20.8)	18.7 (18.6)	7.8 (7.1)
M = Os	L2 = CO	L1 = Cl	14.0 (12.5)	12.8 (11.5)	1.8 (1.3)
M = Os	L2 = PH3	L1 = H	17.3 (16.7)	0.7 (−0.7)	−5.4 (−7.2)
M = Ru	L2 = PH3	L1 = Cl	14.6 (14.0)	5.9 (6.3)	−2.6 (−2.4)
M = Ru	L2 = CO	L1 = Cl	9.5 (7.8)	−1.5 (−1.3)	−8.7 (−9.7)
M = Ru	L2 = PH3	L1 = H	10.9 (11.3)	−14.6 (−14.6)	−18.9 (−20.3)
M = Rh+	L2 = PH3	L1 = Cl	6.5 (6.1)	−11.2 (−9.0)	−19.2 (−20.8)
M = Rh+	L2 = CO	L1 = Cl	5.9 (4.7)	−11.1 (−10.6)	−23.0 (−25.0)
M = Rh+	L2 = PH3	L1 = H	8.8 (8.2)	−22.3 (−23.2)	−29.4 (−32.5)
M = Rh+	L2 = PH3	L1 = Me	8.4 (8.9)	−33.1(−32.4)	−41.9(−43.0)
M = Ir+	L2 = PH3	L1 = Cl	12.3 (10.5)	4.2 (4.2)	−8.3 (−10.2)
M = Ir+	L2 = CO	L1 = Cl	8.1 (6.5)	0.9 (0.4)	−14.9 (−16.4)
M = Ir+	L2 = PH3	L1 = H	14.2 (14.6)	−9.1 (−8.9)	−18.7 (−19.7)
M = Ir+	L2 = PH3	L1 = Me	14.5 (14.6)	−17.2 (−15.9)	−27.8 (−29.1)

The relative Gibbs free energies at 298 K and electronic energies (in parentheses) are given in kcal mol−1.

Discussion

The 1,2-migration on a series of class="Chemical">metallaphosphabenzenes aclass="Chemical">nd class="Chemical">n class="Chemical">metallapyridines have been studied thoroughly by DFT calculations. The effects of metal centers, ligands, aromaticity, and migration groups were examined systematically. Our results reveal that due to the reluctance of phosphorus to participate in π bonding, such a migration in metallapyridines is thermodynamically unfavorable whereas it becomes feasible in metallaphosphabenzenes, which could be the origin of challenge of realizing metallaphosphabenzenes. The 4d transition metals and π-acceptor ligands have the tendency to form nonaromatic analogues rather than metallaphosphabenzenes whereas π-donor ligands and the 5d transition metals can stabilize metallaphosphabenzenes. In addition, the chloride migration has relatively lower reaction barrier due to the weaker bond strength of M-L1 in metallaphosphabenzene in comparison with hydride and methyl migrations. All these findings could be useful for synthetic chemists to realize the first metallaphosphabenzene.

Methods

Computational details

The M0545 level of density functional theory was applied to optimize all of the stclass="Chemical">ructures studied iclass="Chemical">n the gas phase. Frequeclass="Chemical">ncy calculatioclass="Chemical">ns at the same level of theory have also beeclass="Chemical">n performed to ideclass="Chemical">ntify all statioclass="Chemical">nary poiclass="Chemical">nts as miclass="Chemical">nima (zero imagiclass="Chemical">nary frequeclass="Chemical">ncy) or traclass="Chemical">nsitioclass="Chemical">n states (oclass="Chemical">ne imagiclass="Chemical">nary frequeclass="Chemical">ncy). Calculatioclass="Chemical">ns of iclass="Chemical">ntriclass="Chemical">nsic reactioclass="Chemical">n class="Chemical">n class="Chemical">coordinates (IRC)4647 were also carried out on transition states to ensure that such structures are indeed connecting two minima. The LanL2DZ basis set48 was employed to describe Ru, Os, Rh, Ir, P and Cl whereas the 6–31G(d) basis set49 was used for all other atoms. Polarization functions were added for P (ξ(d) = 0.340), Cl (ξ(d) = 0.514), Ru (ξ(f) = 1.235), Os (ξ(f) = 0.886), Rh (ξ(f) = 1.350), and Ir (ξ (f) = 0.938)5051. In order to examine the effect of function for these complexes, the density functional M06L52 has been used with basis sets unchanged. The relative Gibbs free energies of 2b to 1b, 2d to 1d are −13.1 and −4.1 kcal mol−1, respectively, which are comparable to those (−18.9 and −7.1 kcal mol−1) at the M05/6–31G(d) level, indicating that the functional dependence is small. To examine the effect of basis sets, we employed a larger 6-311 + G(d) basis set53 to optimize the complexes 1a–1d, 2a–2d (Fig. 2). The additional calculations show that the basis set dependence is small. For example, using the 6–31G(d) basis set in the gas phase, the relative free energies of 2a–2d to 1a–b are 0.0, 11.4, −18.9, 26.7 and −7.1 kcal mol−1, respectively. Using the larger 6-311 + G(d) basis set, the relative free energies are 0.0, 9.6, −20.1, 24.6 and −8.3 kcal mol−1, respectively. To examine the solvent effect5455, we optimized the structures (1b, 1d, 2b and 2d) using the PCM model56 with benzene as the solvent. The additional calculations show that the solvent effect is small. For example, the relative free energies of 2b to 1b, 2d to 1d are −16.1 and −5.0 kcal mol−1 (−18.9 and −7.1 kcal mol−1 in Fig. 2) when the solvent effect is included. Moreover, the solvent effect is also small for the transition states. For instance, when the solvent effect is included, the reaction barriers of 1e–TS1 and 1f–TS1 become 8.7 and 5.8 kcal mol−1, which are close to those in Table 3 (6.5 and 5.9 kcal mol−1, respectively). In addition, the polar solvents (ethanol and DMSO) are also been taken into account (see Supplementary Table S2), and the results for the polar solvents suggest that the solvent effect is also small. In order to examine the ligand effect of the simplified PH3, we use PMe3 to replace PH3. The results show that the ligand effect is small. For instance, using the ligand PMe3, the relative free energy of 2b to 1b is −14.0 kcal mol−1, which is close to −18.9 kcal mol−1 with the PH3 ligand in Fig. 2. Calculations on complexes 1a–1h indicate that all of them in the singlet ground state are lower in energy than those in the lowest triplet state (Supplementary Table S3), indicating all of them have the close-shell singlet ground state. In addition, the thermodynamics of 1,2 migration on complexes 1a–1h in the lowest triplet state are also examined and the results are similar to those in Fig. 2. Specifically, the relative Gibbs free energies of 2a–2h to 1a–1h are 14.6, −17.1, 40.8, −5.0, −19.3, −30.2, −10.1 and −16.3 kcal mol−1, respectively. The natural bond orbital (NBO, Version 3.1) was also used to obtain Wiberg bond indices (bond orders)57. All calculations were carried out with the Gaussian 03 package58 except the M06L calculations, which were performed by Gaussian 09 package59. All the relative Gibbs free energies calculated at 298 K and electronic energies (in parentheses) are given in kcal mol−1.

Additional Information

How to cite this article: Wu, J. et al. Probing the Origin of Challenge of Realizing class="Chemical">Metallaphosphabenzenes: Uclass="Chemical">nfavorable 1,2-Migratioclass="Chemical">n iclass="Chemical">n class="Chemical">n class="Chemical">Metallapyridines Becomes Feasible in Metallaphosphabenzenes. Sci. Rep. 6, 28543; doi: 10.1038/srep28543 (2016).