Journal of Theoretical Chemistry

Volume 2013 (2013), Article ID 734354, 4 pages

http://dx.doi.org/10.1155/2013/734354

Research Article

A Computational Determination of the Lowest Energy Electronic and Geometric States of First Row Transition Metal Dioxygen Dications

Jillian Lennartz,¹ Eric Dumas,² Lennie Ramirez,² and John Morrison Galbraith²

¹Environmental Resource Management, 1 Beacon Street, 5th Floor, Boston, MA 02108, USA

²Department of Chemistry, Biochemistry, and Physics, Marist College, 3399 North Road, Poughkeepsie, NY 12601, USA

Received 28 March 2013; Accepted 13 August 2013

Academic Editors: G. Borosky, P. Derosa, G. Pacchioni, A. Stavrakoudis, A. Tilocca, and B. M. Wong

Copyright © 2013 Jillian Lennartz et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

The lowest energy geometric structures and electronic spin states of first row transition metal (TM) dioxygen dication molecules ([TM–O₂]²⁺; TM = Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, and Zn) have been determined at the B3LYP/LANL2DZ level of theory (along with an extra -type polarization function added to the O atoms). In order to further verify the spin states, CASSCF(6 + , 9) energy points were determined ( = number of TM electrons). It has been found that with the exception of [Sc–O₂]²⁺, [V–O₂]²⁺, [Co–O₂]²⁺, and [Ni–O₂]²⁺, all [TM–O₂]²⁺ molecules take on a high-spin state. [Sc–O₂]²⁺ adopts a trigonal structure, while [Ti–O₂]²⁺-[Mn–O₂]²⁺ are essentially linear and [Fe–O₂]²⁺-[Zn–O₂]²⁺ are bent. It is further noted that the O–O bond decreases from 130.0 pm to 118.1 pm as the TM changes from Sc to Zn. However, the TM–O₂ bond lengths fluctuate between values of 182.2 pm for [Ni–O₂]²⁺ and 232.2 pm for [Zn–O₂]²⁺.

1. Introduction

Transition metals (TMs) bound to an O₂ molecule are the chemically active site in many industrial [1–5] and biological [1, 2, 6–10] molecules. Considering the TM–O₂ bond to lie along the -axis of a Cartesian coordinate system, in TM–O₂ complexes, bonds can form by the interactions of TM , , and atomic orbitals with suitable orbitals on the O₂ ligand in order to make () or ( and ) bonds (Scheme 1). While there have been numerous studies of neutral TM–O₂ [11, 12] complexes, in many TM–O₂ containing molecules of biological and industrial importance, the TM is bound to a porphyrin ring in the 2⁻ oxidation state. Therefore, [TM–O₂]²⁺ molecules are the simplest approximations to this important class of TM–O₂ containing molecules.

Scheme 1

Probably the most studied TM–O₂ bond is the Fe–O₂ bond due to its role in heme-containing proteins [13–16]. This bond has been described as low-spin Fe(II) accepting an electron pair from excited singlet-state O₂ forming the bond, while donating an electron pair to oxygen to form a bond. An alternative view involves Fe(III) interacting with O²⁻. In a third possibility, triplet Fe(II) couples with triplet O₂ to form a closed shell singlet. Computational results vary depending on the extent of electron correlation and basis set size. It is clear, however, that the overall bonding scheme involves some degree of both O₂Fe and FeO₂   and electron transfer.

Further complicating matters, the number of near degenerate TM -orbitals leads to the possibility of many low lying spin states. In addition, there are a number of different ways that the O₂ unit can be arranged relative to the TM. Herein, we seek to determine the lowest energy electronic and geometric states of [TM–O₂]²⁺ molecules (TM = Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, and Zn) as a precursor to a more in-depth study of the TM–O₂ bond.

2. Theoretical Methods

In order to locate the lowest energy geometrical configuration, B3LYP [17–19] geometry optimizations were performed using the LANL2DZ [20–22] effective core potential basis set with an additional -type polarization function () on the O atoms [23]. Optimizations began with trigonal, linear, and bent starting structures as shown in Scheme 2. Optimizations at all three starting geometries were performed for singlet, triplet, and quintet spin states for [TM–O₂]²⁺ molecules with an even number of electrons (TM = Ti, Cr, Fe, Ni, and Zn) and doublet, quartet, and sextet spin states for molecules with an odd number of electrons (TM = Sc, V, Mn, Co, and Cu).

Scheme 2

In order to further verify the spin state of each molecule, CASSCF [24–29] energy point calculations were performed for the various different spin states at the lowest energy B3LYP conformation. The CASSCF active space consisted of nine orbitals: the 5 TM -type orbitals along with the and O₂ combinations (Scheme 3). Six electrons were placed into this active space from the O₂ and orbitals, along with the TM electrons (i.e., 1 for Sc, 2 for Ti, etc.).

Scheme 3

All calculations were carried out with the Gaussian 03 [30] suite of programs.

3. Results and Discussion

The geometric parameters and spin states of the lowest energy structures of all [TM–O₂]²⁺ molecules studied herein are reported in Table 1.

Table 1: Lowest energy spin states and geometric parameters of [TM–O₂]²⁺ molecules. Bond lengths in pm and bond angles in degree.

Spin state
O–O
TM–O₂
TMOO

ScO₂²⁺
Doublet
130.0
195.4
70.6

TiO₂²⁺
Triplet
124.2
176.5
180.0

VO₂²⁺
Doublet
121.0
197.1
180.0

CrO₂²⁺
Triplet
120.9
193.4
180.0

MnO₂²⁺
Quartet
120.7
200.6
175.4

FeO₂²⁺
Triplet
120.2
196.3
161.9

CoO₂²⁺
Doublet
120.0
198.3
144.4

NiO₂²⁺
Singlet
116.3
182.2
127.7

CuO₂²⁺
Quartet
124.4
196.7
137.5

ZnO₂²⁺
Triplet
118.1
232.2
126.0

[Sc–O₂]²⁺ adopts a trigonal structure as in 1 of Scheme 2. This can be thought of as the Sc²⁺ atom bonding to the system of O₂. The single electron of Sc²⁺ spin pairs with the single electron in the MO of O₂ as depicted in Scheme 3 (MO , 1), while one electron remains in the MO of O₂ (MO , 1) resulting in a doublet ground state.

[Ti–O₂]²⁺, [V–O₂]²⁺, [Cr–O₂]²⁺, and [Mn–O₂]²⁺ are essentially linear with the O₂ binding end-on to the TM²⁺. The slight bending in [Ti–O₂]²⁺ breaks the degeneracy of the and MOs. The observed triplet is the result of the subtle balance between orbital energies and favorable electron exchange. Doublet [V–O₂]²⁺ has one electron in the MO, and triplet [CrO₂]²⁺ has one electron in each of the degenerate MOs (Scheme 3, 2). In order for the high spin quartet to be the lowest energy state of [Mn–O₂]²⁺, one electron must remain in each of the MOs, while another single electron occupies the MO (Scheme 3, 2). This situation is only possible if the and MOs are close enough in energy that exchange stabilization outweighs the destabilization introduced by placing an electron in the higher energy MO.

Upon examination of Scheme 3, it would appear that [Fe–O₂]²⁺ should continue the trend of linearity by completely filling the MO thus forming a stable singlet. Indeed, a stable linear singlet was found; however, it was 18.2 kJ/mol above the bent triplet ground state. Upon bending, the linear MO (Scheme 3, 2) splits into the bent and MOs (Scheme 3, 3). This results in a stabilization of the MO due to increased bonding interaction, while the MO experiences little change energetically. The triplet is then formed by placing a single electron in the and MOs. The bent triplet is favored over the bent singlet due to favorable exchange between electrons in these energetically close orbitals.

Adding more electrons causes [Co–O₂]²⁺, [Ni–O₂]²⁺, [Cu–O₂]²⁺, and [Zn–O₂]²⁺ to become increasingly more bent. For [Co–O₂]²⁺ and [Ni–O₂]²⁺, the and MOs are filled one at a time resulting in doublet and singlet ground states, respectively. On the other hand, [Cu–O₂]²⁺ and [Zn–O₂]²⁺ adopt high spin quartet and triplet ground states, respectively, indicating that the , , and MOs (Scheme 3, 3) are close in energy.

It is interesting to note that the O–O bond length decreases from a value of 130.0 pm in [Sc–O₂]²⁺ to 118.1 pm in [Zn–O₂]²⁺ (Table 1). Such a decrease could be caused by increasing the electron density in O–O bonding MOs or decreasing electron density in O–O antibonding MOs. This range is both above and below the O–O bond distance in O₂ (121 pm [31]), but within the limits of O²⁻ (135 pm [31], an extra electron in the antibonding MO) and O²⁺ (112 pm [31], one less electron in the antibonding MO). However, the TM–O₂ bond lengths are not so consistent and fluctuate between values of 182.2 pm in [Ni–O₂]²⁺ and 232.2 pm in [Zn–O₂]²⁺ (Table 1).

4. Conclusions

In the current study, we present the lowest energy geometrical conformations and spin states of first row [TM–O₂]²⁺ molecules. [Sc–O₂]²⁺ is trigonal, while [Ti–O₂]²⁺-[Mn–O₂]²⁺ are linear and [Fe–O₂]²⁺-[Zn–O₂]²⁺ are bent. The O–O bond length decreases as the TM goes from Sc to Zn, whereas the TM–O₂ bond length fluctuates. For [Mn–O₂]²⁺, [Fe–O₂]²⁺, [Cu–O₂]²⁺, and [Zn–O₂]²⁺ molecules, high spin states are lowest in energy indicating degenerate or near-degenerate orbitals.

Although it is clear that there is some level of electron transfer from the O₂ to the TM as well as some degree of TM to O₂ back donation, a more detailed analysis is required in order to fully understand the bonding in these unique molecules and how that extends to larger molecules of biological and industrial importance. Furthermore, we have shown that while the current results can be used as a starting point for studies of TM–O₂ containing molecules with donor and acceptor ligands, caution must be exercised as both high- and low-spin ground states are possible.

Acknowledgments

This work was supported by the Research Corporation Cottrell College Science Award CC6519. The authors thank the School of Science and the office of the Academic Vice President of Academic Affairs at Marist College for continued support of research.

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