A multi-scale approach to spin crossover in Fe(ii) compounds
Transcript of A multi-scale approach to spin crossover in Fe(ii) compounds
This journal is c the Owner Societies 2011 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 10449
Cite this: Phys. Chem. Chem. Phys., 2011, 13, 10449–10456
A multi-scale approach to spin crossover in Fe(II) compoundsw
Marcel Swart,*ab
Mireia Guellaand Miquel Sola
a
Received 7th March 2011, Accepted 22nd March 2011
DOI: 10.1039/c1cp20646j
We report here for the first time a multi-scale study on the concept of spin-crossover compounds,
which integrates improved density functionals, a polarizable force field and hybrid QM/MM
calculations. This multi-scale setup is applied to the temperature dependence of spin states of a
Fe(II) compound with trispyrazolylborate ligands that exhibits spin-crossover. Our study shows a
transition temperature of around 290 K, which is in perfect agreement with experimental results.
Moreover, based on our data we provide the origin of why spin transition occurs in this
iron-compound: it results directly from spin-state changes in the iron-compound that lead to
more favourable electrostatic interactions for the high-spin state.
I. Introduction
Molecular switching due to thermally induced spin crossover
(SCO) in transition metal (TM) compounds has raised much
interest,1–38 in part because of the potential applications in
technology and biomedicine. Many of these studies involve
Fe(II) compounds that switch from low spin at low temperatures
to high spin at high(er) temperatures, although also other
transition metals such as cobalt may be involved.29,32 The
switch from low to high spin is usually accompanied by a
change in metal–ligand bond-lengths, but without further
changes in the molecular geometry; for instance for the
TM-compound under study here both spin-state geometries
have the same symmetry (D3d). Moreover, for d6 systems
(e.g. Fe(II)-compounds) changes in Mossbauer parameters
and magnetic properties are observed, resulting from the
change from a diamagnetic compound in the low-spin to a
paramagnetic compound with four unpaired electrons in the
high-spin state. The thermal transition temperature where this
switching takes place varies for different compounds, and is
observed with a temperature range for the switching that is
between a few degrees (sudden switch) to hundreds (gradual
process). Multiple spin-crossovers are also possible within one
compound, and may involve between 6 and 30 (un)paired
electrons.39
The origin of (sudden) SCO is often described as resulting from
the cooperative effect of a large number of TM compounds,1,30
e.g. through long-range interactions within the solid state
(crystal). Although indeed the ‘‘sudden switch’’ takes place in
the solid state, this viewpoint is too limited: isolated TM
compounds in solution also show SCO behavior,26,40,41 albeit of
the gradual kind. Therefore, in the general sense (valid for both
the sudden switch and the gradual process) the SCO phenomenon
is associated with spin-state preferences of the isolated TM
compounds. Several studies have in the past tried to analyze
SCO by computations,17,18,38 but these were hampered because of
inherent problems42–44 of the computational methodologies
used for the correct description of spin ground-states of TM
complexes. For instance, early density functionals using the
generalized gradient approximation (GGA) overestimate the
stability of low spin states, while hybrid functionals (containing
a portion of Hartree–Fock exchange) overestimate the stability of
high spin states.42,45 Also the basis set used can have a profound
influence.46,47 More recently, other studies have highlighted the
appropriateness of more recent and improved density functionals,
such as OPBE,42,43,48–50 SSB-D,44,51 TPSSh52–54 or M06-L.44,55
In a recent study,30 we investigated the spin-state preferences
of isolated Fe(II) compounds, with either trispyrazolylborate
(Tb) or trispyrazolylmethane (Tc) ligands. For these compounds,
we studied how substitution patterns on the ligands altered the
spin ground-states and Mossbauer parameters, which in
turn were compared with experimentally observed magnetic
susceptibility data and/or Mossbauer spectra.30 Because of the
use of OPBE,48–50 good results had been obtained for the spin
ground-state42,44 and the Mossbauer parameters. However, no
attempt was made to study the SCO patterns, which would
involve a study of the system at different temperatures.
Here, we report a multi-scale study on SCO in the iron
compound Fe(II)(Tb)2, using a sequential molecular dynamics
(MD) scheme. In this scheme, trajectories at different temperatures
are obtained from MD simulations employing a polarizable
force field, which is then followed by hybrid QM/MM
calculations on snapshots from these trajectories. Both the
force field parameterization as the QM/MM calculations
a Institut de Quımica Computacional and Departament de Quımica,Universitat de Girona, Campus Montilivi, 17071 Girona, Spain
b Institucio Catalana de Recerca i Estudis Avancats (ICREA),Pg. Lluıs Companys 23, 08010 Barcelona, Spain.E-mail: [email protected]
w Electronic supplementary information (ESI) available: Force fieldparameters for iron compound, radius of spherical box at differenttemperatures, and vibrational frequencies of analytical and IntraFFHessian. See DOI: 10.1039/c1cp20646j
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10450 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 This journal is c the Owner Societies 2011
involve improved density functionals for SCO studies in TM
complexes.
II. Computational methods
All of the density functional calculations were carried out with
the Amsterdam Density Functional (ADF) program, version
2010.01.56,57 Uncontracted basis sets of Slater-type orbitals
(STOs) of triple-B quality plus polarization (TZP) were used,
in some cases using the frozen-core (fc) approach.57 The
hybrid QM/MM calculations were performed always using
all-electron basis sets.
The molecular dynamics simulations with the polarizable force
field used the Discrete Reaction Field (DRF) approach58–68
within the DRF90 program.69 The parameters needed for
these simulations were specific for the systems under study,
which have been obtained in DFT calculations on the isolated
solvent and solutes (see below). The dichloromethane solvent
was in these MD simulations treated as a rigid body,
i.e. without internal (vibrational) degrees of freedom.
A. Polarizable force field setup
For the DRF approach, we need for each atom in the solvent
and the solutes (Fe(II)-compound in low and high spin
state), an atomic charge, an atomic radius and an atomic
polarizability. Details about the energy expressions, the setup
of the (QM/MM) DRF approach and how these result from
second-order perturbation theory are given in ref. 61 and 66.
For the dichloromethane solvent, we simply use standard
atomic polarizabilities60 that give a good representation of its
molecular value. This is different for the iron compound, for
which no standard polarizabilities are available. We therefore
computed first the molecular polarizability of Fe(II)(Tb)2 with
the ADF program,70 for both the low (singlet) and high
(quintet) spin-state. Because ADF allows the calculation of
molecular polarizability only for spin-restricted systems,
and not yet for unrestricted ones, these calculations were
performed using the finite field approach. Similar to a recent
study,71 we used electric field strengths of �1.0e–3, �2.0e–3,�3.0e–3 a.u. along the X-, Y- or Z-direction and measured the
change in dipole moments. The linear response then gives the
usual 3 � 3 polarizability tensor (see Table 1).
Although the tensor components are somewhat different
between the high and low spin states, the mean molecular
polarizability is virtually the same with values of 345.50 a.u.
for the low spin, and 345.55 a.u. for the high spin state. With
the standard value for the a-factor (2.1304) within the DRF
approach, we then used the polar60 program to obtain atomic
polarizabilities (a.u.) for the iron compounds: 2.1537 (H),
11.2741 (B), 10.0051 (C), 4.5261 (N) and 61.6579 (Fe).
With these atomic parameters the molecular tensors could be
perfectly reproduced.
The atomic charges and radii were taken directly from
calculations at OPBE/TZP,48 using the multipole derived
charge (MDC) analysis72 for the charges, and QCosmo radii.73,74
Indicated in Fig. 1 are the (D3d) symmetry-unique atoms with
their labels, and given in Table 2 are their charges and radii.
B. Molecular mechanics parameters for Fe(II)-compounds
Apart from the parameters for the polarizable force field, we
also need molecular mechanics parameters for the bonded
interactions (bonds, angles, dihedrals). For this we use the
IntraFF method75 that takes these parameters from the
computed Hessian. The basic philosophy behind IntraFF75
is that the force constant gives an estimate for the curvature
around the minimum, just as the Hessian matrix (a 3N � 3N
matrix with second derivatives of the energy with respect to
atomic coordinates) does. Therefore, by choosing appropriate
direction vectors for the different internal coordinates (bonds,
angles, dihedrals), reliable and consistent force constant values
can be obtained directly from the computed QM Hessian.
Here we use the analytical76 Hessian matrix obtained at
OPBE/TZP, from which the force field parameters for the
bonded interactions were obtained (see Supplementary Infor-
mation).w As an example, the Fe-N bonds had force constant
values (using the Amber77 convention) of 146.96 kcal mol�1
A�2 (low spin) and 120.01 kcal mol�1 A�2 (high spin).
C. Molecular dynamics setup
The MD simulations were performed with the DRF90
program,69 using a timestep of 1 fs. At each temperature
between 200 K and 450 K (with steps of 10 K) an initial
equilibration run was done of 100 ps, which was followed by a
production run of 100 ps. A Nose–Hoover thermostat78 within
the NVT-ensemble79 was used for obtaining the desired
temperature, and a soft wall-force potential69 was used to
keep the solvent molecules from evaporating from the
spherical box. The centre of mass of the solute was fixed at
Table 1 Molecular polarizability tensors (a.u.) of Fe(II)(Tb)2
Low spin High spin
320.61 0.0 0.0 317.25 0.0 0.00.0 320.61 0.0 0.0 317.25 0.00.0 0.0 395.27 0.0 0.0 402.16
Fig. 1 Fe(II)(Tb)2 with symmetry-unique atomlabels.
This journal is c the Owner Societies 2011 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 10451
the center of the box at all times. The size of the box was
adapted at the different temperatures in such a way as to retain
the macroscopic density of the solvent at these different
temperatures (see Supplementary information).w Quaternions
were used to treat the rigid body motions of the solvents.79
D. Hybrid QM/MM setup with polarizable force field
The hybrid QM/MM calculations using the DRF approach61,66,68
for the polarizable force field were performed with a locally
modified version of ADF2010.01. The major difference with
the implementation by Jensen and co-workers66 was the input
handling, which is now merged into the general QM/MM
setup of ADF.80,81 Moreover, the interaction between the QM
and MM systems, and within the MM systems were modified
at two places: (i) the electric field of the QM electrons at the
polarizable (MM) particles is now screened for overlapping
charge densities (using the error function);82 (ii) the dipole field
tensor between the induced MM dipoles is now screened for
overlapping charge densities (using Thole’s model).83 These
changes were needed to make the interactions consistent with
the DRF approach,61 where all of them are screened for
overlapping densities. More details of these changes in the
DRF-QM/MM setup within ADF will be given elsewhere.81
Note that because we have studied the spin-states at temperatures
between 200 and 450 K, and have selected 100 snapshots from
the MD trajectories, in total we have been running over 5000
single-point QM/MM calculations.
III. Results and discussion
We have studied the low-spin singlet and high-spin quintet
state of the Fe(II)(Tb)2 compound in a multi-scale approach
that closely integrates quantum-chemistry84 with molecular
dynamics simulations79 with a polarizable force field.61,69 The
iron compound studied here has at 0 K a low-spin singlet
ground-state, as identified before by us30 and others17 with
computational studies. Unlike other SCO-compounds in the
solid state, in a solution of dichloromethane it does not
show a sudden switch from low to high spin within a short
temperature range, but instead shows a gradual process of
switching.26 The transition temperature is therefore not as well
defined as in the solid state, but is roughly estimated to be
around 285–290 K for the Fe(II)(Tb)2 compound in a solution
of dichloromethane.26
In the current contribution, we attempt to analyze the SCO
phenomenon from a computational point of view using a
multi-scale approach where a density functional method
(OPBE) is used that is appropriate43,44,51 for the description
of spin-state preferences of transition-metal complexes.
Because our previous study30 used the OPBE functional, and
to be able to compare directly with that study, we have used
the OPBE functional in this study as well. This notwithstanding,
we have checked that SSB-D51 provides similar results. Thus,
for instance, the spin-state splitting at 0 K is almost the same
for the two functionals, with a value of 5.9 kcal mol�1 at
OPBE/TZP(fc), and 6.0 kcal mol�1 at SSB-D/TZP(fc).
A. Force field parameterization
The gas-phase D3d-symmetric structures of the Fe(II)(Tb)2compound in the low and high spin state were taken directly
from our previous study,30 where these were optimized
already. Here we have calculated the analytical Hessian for
obtaining the molecular mechanics (MM) parameters of the
bonded interactions, which were obtained with the IntraFF
program.75 The vibrational frequencies from these Hessians
showed positive values only, and were adequately reproduced
by our IntraFF parameters (with mean absolute deviations of
30 and 41 cm�1, see Supplementary information).
The force constants for the Fe–N bonds were some 20%
larger for the low spin-state (147 kcal mol�1 A�2) than for the
high spin-state (120 kcal mol�1 A�2), which is probably mainly
related to the larger Fe–N distance in the latter. For Cu–N
bonds in a blue-copper protein, an exponential decay of the
force constant was observed with increasing equilibrium
distance.85 For the copper systems, these values could be fitted
nicely by the anharmonic bond potential by Frost,86,87 which
only has two parameters (A, B). With only one set of
parameters for Cu–His bonds, the force constants for several
azurin mutants with varying copper-nitrogen distances could
be matched perfectly.85 However, one set was needed for the
reduced state of the copper proteins, and one for the oxidized
state. A similar situation is observed here, where we find
different A/B parameters for the low and high spin state
(see Table 3). Note that in the MD simulations the harmonic
bond potential was used in all cases.
The atomic charges72 and radii73,74 needed for the force field
were taken directly from single-point calculations on the
isolated iron compounds and a solvent molecule, and are
derived directly from the charge-density (de)localization in
Table 2 Atomic charges (a.u.) and radii (a.u.)a
Charges radii
SolventC �0.1472 3.2358H 0.4180 2.0593Cl �0.3444 3.5289Solute Low High Low HighB0 1.4520 1.4794 3.4859 3.4741H0 �0.4762 �0.4801 2.1535 2.1550N1 �0.3912 �0.3859 2.8269 2.8317N2 �0.3565 �0.4001 2.7562 2.8005C3 0.0771 0.0809 3.2787 3.2959H3 0.1573 0.1464 2.0599 2.0674C4 �0.2488 �0.2371 3.3434 3.3414H4 0.1434 0.1409 2.0646 2.0700C5 0.0417 0.0568 3.3410 3.3386H5 0.1227 0.1266 2.0660 2.0611Fe 0.7870 0.8301 3.8458 3.8506
a for atomlabels of solute see Fig. 1.
Table 3 Anharmonic Frost parametersa (a.u.) for Fe–N and Cu–Nbonds
A B Z1 Z2
Fe–N, low spin 1.43 58.4 26 7Fe–N, high spin 1.22 52.1 26 7Cu–N, reducedb 1.61 � 0.01 65.3 29 7Cu–N, oxidizedb 1.52 � 0.01 65.3 � 0.3 29 7
a UFrost(R) = e�A�R(Z1�Z2/R � B), see ref. 86 and 75. b from ref. 85.
10452 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 This journal is c the Owner Societies 2011
these. The multipole derived charge analysis72 was designed to
give the best possible description for the electrostatic potential
and field inside and outside the molecule, when using atomic
fractional charges as the sources for them. Therefore, the
atomic multipole moments (up to the dipole moment) that
result directly from the charge density distribution were
distributed into fractional atomic MDC-d charges.72 Likewise,
the radii were taken from the QCosmo model,74 which
determines the atomic radii for use within a dielectric continuum
model based on the distribution of charge density around the
nuclei. i.e., they are based on the second-order moments ri�Ria2,
where ri is the charge density at a grid point i, and Ria is the
distance between grid point i and nucleus a. Since the
(de)localization of charge density is governed by the total
molecular charge and/or total molecular spin, these radii
should be adequate representations of the atomic sizes for
either anionic, neutral or cationic species. This was indeed
found to be the case for the solvation energy (within the
QCosmo approach)74 of a series of ions and molecules. For
the neutral molecules we study here, we do indeed find atomic
radii that are quite close to ‘‘normal’’ van der Waals radii, of
ca. 1.5 A for nitrogen, 1.7 A for carbon, 1.9 A for chloride and
ca. 2.0 A for iron (see Table 2).
The atomic polarizabilities for the polarizable part of the
force field were determined from fitting to the molecular
polarizability of the iron complex in the low and high
spin-state (see section II.A). These atomic values are within
the DRF approach used not only for the interaction of the
induced dipole moments with the source field (induction
energy), but also for screening61 the other energy components69
(dispersion, repulsion, electrostatics, soft wall-force) for
overlapping charge densities (Thole’s model).83
B. Molecular dynamics simulations
We have surrounded the iron-complexes within a spherical
box with 160 dichloromethane solvent molecules, in order to
have at least two solvent layers surrounding it (see Fig. 2). The
size of the box was adapted at each temperature (between 200 K
and 450 K in steps of 10 K) according to the macroscopic
density of the solvent at that temperature. These were estimated
from the experimental values within a temperature range of
0 1C to 100 1C,88 with a second order polynomial fitted to
them. This gave the following relationship: rmacro = 1.361685�0.001732�T � 2.331e�6�T2. This relationship then gave the
total solvent volume at a certain temperature, which together
with the solute volume (estimated with the rangenconf
program69) gave the total volume, from which the radius of
the spherical box was obtained (ranging from 29.48 to 33.62
Bohr, see Supplementary information).wThe initial configuration of the solvent molecules around the
solute was done with the rangenconf program,69 and a pre-
equilibration run of 10 ps at a temperature of 200 K was
performed for both the low and high spin state separately.
Afterwards, at each temperature an equilibration run was
performed for 100 ps, followed by a production run of another
100 ps, again for both spin states separately. The length of the
equilibration run was deliberately chosen to be long, in order
to let the system adjust itself to the new temperature and
spherical box size. From the trajectory of the production run,
at every 1000 steps (i.e. every ps) the configuration was kept
for subsequent snapshots with hybrid QM/MM (see below).
During the MD simulations the iron compound moved
freely, apart from its center of mass that was fixed at the
center of the spherical box at all times. The IntraFF75 parameters
for the bonded parameters worked well with e.g. average
Fe–N2 distances of e.g. 1.96 � 0.03 A at 200 K and 1.96 �0.04 at 400 K for the low spin, and 2.20 � 0.03 A at 200 K and
2.21 � 0.04 at 400 K for the high spin state. At the same time,
the temperature was recovered correctly, e.g. at 289.8� 13.0 K
for the target of 290 K, because of the use of the Nose-Hoover
thermostat.78 The total dipole moment of the system varied
from 12 Debye at 200 K to ca. 21 Debye at 450 K, which is
coming mainly from the expansion of the box. i.e. the ‘‘static’’
dipole moment resulting from the (re)orientation of the
fractional charges increases synchronously with the increase
of the temperature (and hence box size), while the total
‘‘induced’’ dipole moment (i.e. the sum of all induced dipoles
at the polarizable particles) oscillates between 3.5 and 6.0
Debye, but without a clear correlation with the temperature.
The average of the purely classical total energy (Utot =Upot +
Ukinetic, where Upot = Uelst + Udisp + Urep + Uinduct + UMM
+Ucavit, see ref. 69) from the MD simulations goes up steadily
with temperature (because of both an increase of the kinetic
energy and a reduction of the interaction energy), for both
spin states (see Fig. 3). At low temperatures (250 K and
below), the low-spin singlet state has the lowest energy. On
the other hand, at more elevated temperatures (350 K and
above) there is a clear preference (20 kcal mol�1 or more) for
the high-spin quintet state. Most interestingly, the transition
temperature where the quintet state energy profile crosses with
the singlet state profile, is found in the region of 280–290 K
(see Fig. 3), exactly where it was also observed experimentally.26
Of course, in Fig. 3 we have not yet taken into account the
Fig. 2 Solvated Fe(II)(Tb)2 complex.
This journal is c the Owner Societies 2011 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 10453
contribution of the electronic energy, which could shift the
quintet state upwards by ca. 6 kcal mol�1 (vide supra). However,
at 290 K the MM energy difference (9.8 kcal mol�1) is already
larger than this shift, so the transition temperature would not
change much. This electronic effect we will take into account in
the QM/MM snapshots below. Furthermore, note that we report
here the energies U, not the Helmholtz free energies A or Gibbs
free energies G. In principle, these latter might be obtained
using e.g. free energy perturbation techniques, thermodynamic
integration, meta-dynamics, etc.However, neither one of these is
implemented yet in the programs we use (with polarizable force
fields). Moreover, this would lead to an enormous increase of the
computational effort, easily leading up to 100.000 single-point
QM/MM calculations, which is clearly outside our current
possibilities. Nevertheless, we have looked at the Helmholtz
free energies as coming directly from the partition function Z
(keeping in mind that our simulation times of 100 ps are
obviously too short to get reliable quantitative results), which
gave qualitatively similar results as the energies U: the low-spin
state was favored at low temperatures, the high-spin state at high
temperatures, and the transition between the two takes place
around 280–300 K.
C. Single-point hybrid QM/MM snapshots
From the production run MD simulations, we have kept at
every ps the configuration of solvent molecules and iron
complexes. With these coordinates, we then performed 100
single-point QM/MM calculations using the adapted DRF
implementation in the ADF program. All interactions between
QM and MM systems, and within the MM system, were
consistently61 treated and screened for overlapping charge
densities (see section II.D).
Before discussing the results that we obtained, we focus first
on the similarities between the MM and QM/MM interactions.
We have monitored the electrostatic and induction energies for
the interaction between the QM and MM regions, both within
the purely classical calculations with the DRF90 program and
within the hybrid QM/MM calculations with ADF. These
interactions are obtained in a significantly different manner.
i.e., within the DRF90 program69 the interactions are obtained
based on empirical atomic interactions, while in the polarizable
hybrid QM/MM calculations66,68 it is the electrons of the QM
system that ‘‘feel’’ and ‘‘feed’’ the interactions. i.e., it is not just
that the electrons ‘‘feel’’ the (screened) electrostatic potential
from the classical charges, they also ‘‘feed’’ back the interactions
through their electrostatic field to the polarizable particles,
and induce dipoles in these. These latter lead to an additional
electrostatic potential for the electrons, and therefore leads to
an iterative scheme that has to be solved self-consistently on
top of the usual SCF scheme within QM calculations.66
This however does not lead to problems, as the QM/MM
calculations converge normally within 15–30 SCF cycles.
Interestingly enough, for the sum of the electrostatic and
induction energies between the QM and MM systems, the
difference between either a purely classical description or a
polarizable QM/MM description is quite small (of typically
2–7 kcal mol�1). And this despite the fact that because of the
dynamic behavior of both the solute and the solvent
molecules, there is a large variation in this sum (taken from
those of the 100 snapshots) of some 40 kcal mol�1. The
screening for overlapping charge densities is done in
completely different ways, e.g. with Thole’s model60,67,69,73,83
for the purely classical MD simulations, and within the MM
system in hybrid QM/MM. However, the potential of the
electrostatic field in the QM region, and its feeding back, is
screened using the error function, i.e. following Jensen’s
model.82 Given the large similarity between MM and QM/MM
interactions, it is therefore again61,67,73 proof that the polarizable
DRF approach gives a consistent picture at both the polarizable
MM and QM/MM level.
The (averaged) QM/MM energy profile for both the low
and high spin- state is given in Fig. 4. Similar to the situation
in the MD simulations, the transition between low and high
spin takes place in the region around 280–300 K. The energy
profile and the transition region are not as clear as in the
profile from the MD simulations, probably due to the much
smaller number of points taken into account (100 vs. 100,000).
Therefore, also with the QM/MM calculations do we
reproduce the experimentally observed transition temperature
very well. This is not that surprising, since we already saw this
emerging in the MD simulations with the polarizable force
field. Moreover, we also saw that describing these systems with
either polarizable MM, or with polarizable QM/MM gives
basically the same results.
D. Spin crossover patterns
The SCO from low to high spin of the Fe(II)(Tb)2 complex in a
solution of dichloromethane takes place around 290 K, both
Fig. 3 Energy profile (Utot, kcal mol�1) from MD simulations.
Fig. 4 Hybrid QM/MM energy profile.
10454 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 This journal is c the Owner Societies 2011
experimentally26 and with our current computational study.
There are many different ways to probe the spin-state of
a system at a certain temperature,1 such as e.g. magnetic
susceptibility, Mossbauer spectroscopy, Raman spectroscopy,
Fourier Transform Infrared spectroscopy, UV–vis, etc. And
many focus on stimulating the system with either thermal
perturbations, pressure,89 or light. Indeed, one of main
characteristics of the transition is the change in metal-ligand
bond distances,30 that gives quite different spectroscopic
features (see e.g. ref. 90). But so far, not much attention has
been paid as to the origin of the transition with thermal
perturbations. It is often assumed that because some (but
not all!) of the vibrational frequencies are lower for the
high spin-state than for the low spin, it is merely the entropy
that causes the spin transition. However, this is not what is
coming out of our calculations. The electronic contribution
to the entropy for multiplet states (3.2 cal mol�1 K�1, e.g. ca.
1.0 kcal mol�1 at 300 K) is negligible compared to the
differences shown in Fig. 3 and 4. Furthermore, the entropy
of the total simulated system, when obtained from the parti-
tion function Z, is similar for both spin states with sometimes a
larger value for the singlet, and sometimes for the quintet.
Although we directly admit that the time-scale of our simulation
is much too short to get an accurate estimate of the entropy, it
is clear from our simulations that the driving force for the
transition is not entropy.
Our simulations reveal a different cause for the spin transition,
which is directly connected to the spin-state and changes related
with it. As the temperature goes up, the kinetic energy increases
and this has a direct effect on the system size, e.g. macroscopic
density (vide supra). Not only that, also the interaction energy
(Upot) between the solute and the solvent molecules, and between
the solvent molecules themselves, decreases drastically from e.g.
around �4100 kcal mol�1 at 200 K (low spin-state) to around
�3700 kcal mol�1 at 450 K. This is again a direct result from the
increasing kinetic energy, leading to larger distances between
solute and solvent molecules, and between solvent molecules
themselves. The reduction of the interaction energy takes place
for both spin states, but it does so more slowly for the high spin-
state. e.g. at 200 K, the total interaction energy (electrostatics,
dispersion, repulsion and induction) is ca. 20 kcal mol�1 more
favorable for the singlet than for the quintet; at 450 K it is
reversed, and the interaction of the quintet is more favorable by
ca. 20 kcal mol�1. This change results almost entirely from
electrostatics that is some 15–20 kcal mol�1 more favorable for
the singlet at low temperatures, and some 10 kcal mol�1 more
favorable for the quintet at higher temperatures.
The origin of this change in electrostatics can be attributed
to the nitrogens of the pyrazolyls and the hydrogens of the
solvent molecules. The hydrogens are at lower temperature
closer to the pyrazolyl rings (as measured by the Npyrazolyl–
Hsolvent distances) in the low spin than in the high spin-state. In
contrast, at higher temperatures they are closer in the high
spin-state than in the low spin-state. In itself, this should have
no effect on the electrostatics, but because the fractional
charge on nitrogen N2 is significantly larger (see Table 2) for
the high-spin (�0.40) than for the low-spin state (�0.35),the electrostatic interaction with these hydrogens is more
favorable for the high-spin state. At low temperatures this is
not allowed to happen because of the reduction of volume,
which makes that the bulkier chlorines of the solvent are
‘‘pushed’’ inwards. Only at elevated temperatures, when this
inwards pressure is released, can the solvent adapt itself to its
more favored orientation. i.e., the hydrogens will then be
found closer to the solute, which favors the high-spin state
over the low-spin state.
IV. Conclusions
We have investigated spin-crossover (SCO) behavior in a
iron(II) compound that is experimentally known to show
SCO in a solution of dichloromethane. The structures of
the Fe(II)(Tb)2 compound were already obtained in our
previous study, where we looked at spin ground-states and
Mossbauer parameters of a number of Fe(II) complexes with
trispyrazolylborate and trispyrazolylmethane ligands, and
how these are affected by substitution patterns. In that study,
we showed that the OPBE functional works very well for
predicting the spin-state of these complexes.
Here, we extend that study by taking into account the
temperature effects through the use of molecular dynamics
simulations using a polarizable force field. All of the
parameters for both the polarizable part, as for the bonded
molecular mechanics part were obtained in single-point
calculations on the isolated solutes and solvent. We have
studied the energy profile for both the low and high spin-state
from 200 K to 450 K, and find that the transition from low to
high spin takes place around 290 K, which is in excellent
agreement with experimental data that places it around
285–290 K.
Based on our data, we find that the transition from low to
high spin is not governed by entropy, but a much simpler
picture emerges. Because of the larger iron-nitrogen distances
in the high spin-state, there is a subtle but significant change in
the charge distribution in which the N2 nitrogen atom ‘‘gains’’
charge density (its fractional charge increases from �0.35 for
the low spin-state to �0.40 for the high spin-state). This is
logical because of the reduction of covalent interactions with
iron at these larger Fe–N distance. At the same time, the
solvent reorients itself at elevated temperatures whereby
the protons are on average closer to these nitrogens in the
high-spin state than in the low-spin state. This makes that the
electrostatic interactions between the solute and solvent is more
favorable for the high-spin state at elevated temperatures. At
lower temperatures, the kinetic energy is smaller and the total
volume available for the solvent reduces as well. This makes
that the bulkier chlorines are ‘‘pushed’’ inwards, and hence this
subtle effect favorable for the high-spin state is reduced. Future
studies will clarify if this ‘‘electrostatics’’ argument is limited to
the transition-metal compounds in solution, or if it is generally
applicable also in the ‘‘sudden’’ switch within the solid state.
Acknowledgements
The following organizations are thanked for financial
support: the Ministerio de Ciencia e Innovacion (MICINN,
project numbers CTQ2008-03077/BQU and CTQ2008-06532/
BQU) and the DIUE of the Generalitat de Catalunya
This journal is c the Owner Societies 2011 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 10455
(project numbers 2009SGR637 and 2009SGR528). Excellent
service by the Centre de Supercomputacio de Catalunya
(CESCA) is gratefully acknowledged. Support for the research
of M. Sola was received through the ICREA Academia 2009
prize for excellence in research funded by the DIUE of the
Generalitat de Catalunya. Part of this study (the adaptation of
the QM/MM implementation) was financially supported by
the HPC-Europa Transnational Access program.
References
1 P. Gutlich and H. Goodwin, Spin Crossover in Transition MetalCompounds I–III, Springer-Verlag, Berlin, 2004.
2 S. Trofimenko, J. Am. Chem. Soc., 1966, 88, 1842–1844.3 S. Trofimenko, J. Am. Chem. Soc., 1967, 89, 3170–3177.4 S. Trofimenko, J. Am. Chem. Soc., 1967, 89, 6288–6294.5 S. Trofimenko, Prog. Inorg. Chem., 1986, 34, 115–210.6 S. Trofimenko, J. C. Calabrese, P. J. Domaille and J. S. Thompson,Inorg. Chem., 1989, 28, 1091–1101.
7 S. Trofimenko, Chem. Rev., 1993, 93, 943–980.8 S. Trofimenko, Scorpionates. The Coordination Chemistry of Poly-pyrazolylborate Ligands, Imperial College Press, London, 1999.
9 A. L. Rheingold, G. Yap and S. Trofimenko, Inorg. Chem., 1995,34, 759–760.
10 D. L. Reger, Comments Inorg. Chem., 1999, 21, 1–28.11 D. L. Reger, T. C. Grattan, K. J. Brown, C. A. Little, J. J.
S. Lamba, A. L. Rheingold and R. D. Sommer, J. Organomet.Chem., 2000, 607, 120–128.
12 D. L. Reger, C. A. Little, A. L. Rheingold, M. Lam,L. M. Liable-Sands, B. Rhagitan, T. Concolino, A. Mohan,G. J. Long, V. Briois and F. Grandjean, Inorg. Chem., 2001, 40,1508–1520.
13 D. L. Reger, C. A. Little, V. G. Young and P. Maren, Inorg.Chem., 2001, 40, 2870–2874.
14 D. L. Reger, C. A. Little, M. D. Smith, A. L. Rheingold,K. C. Lam, T. L. Concolino, G. J. Long, R. P. Hermann andF. Grandjean, Eur. J. Inorg. Chem., 2002, 1190–1197.
15 D. L. Reger, J. D. Elgin, M. D. Smith, F. Grandjean, L. Rebbouhand G. J. Long, Eur. J. Inorg. Chem., 2004, 3345–3352.
16 D. L. Reger, J. R. Gardinier, J. D. Elgin, M. D. Smith, D. Hautot,G. J. Long and F. Grandjean, Inorg. Chem., 2006, 45, 8862–8875.
17 H. Paulsen, L. Duelund, H. Winkler, H. Toftlund andA. X. Trautwein, Inorg. Chem., 2001, 40, 2201–2203.
18 H. Paulsen, L. Duelund, A. Zimmermann, F. Averseng,M. Gerdan, H. Winkler, H. Toftlund and A. X. Trautwein,Monatsh. Chemie, 2003, 134, 295–306.
19 J. D. Oliver, D. F. Mullica, B. B. Hutchinson and W. O. Milligan,Inorg. Chem., 1980, 19, 165–169.
20 J. J. McGarvey, H. Toftlund, A. H. R. Alobaidi, K. P. Taylor andS. E. J. Bell, Inorg. Chem., 1993, 32, 2469–2472.
21 A. Looney, R. Han, K. McNeill and G. Parkin, J. Am. Chem. Soc.,1993, 115, 4690–4697.
22 G. J. Long and B. B. Hutchinson, Inorg. Chem., 1987, 26, 608–613.23 G. G. Lobbia, B. Bovio, C. Santini, P. Cecchi, C. Pettinari and
F. Marchetti, Polyhedron, 1998, 17, 17–26.24 M. C. Keyes, B. M. Chamberlain, S. A. Caltagirone, J. A. Halfen
and W. B. Tolman, Organometallics, 1998, 17, 1984–1992.25 J. P. Jesson, J. F. Weiher and S. Trofimenko, J. Chem. Phys., 1968,
48, 2058–2066.26 J. P. Jesson, S. Trofimenko and D. R. Eaton, J. Am. Chem. Soc.,
1967, 89, 3158–3164.27 C. Janiak, T. G. Scharmann, T. Brauniger, J. Holubova and
M. Nadvornik, Z. Anorg. Allg. Chem., 1998, 624, 769–774.28 C. Janiak, T. G. Scharmann, J. C. Green, R. P. G. Parkin,
M. J. Kolm, E. Riedel, W. Mickler, J. Elguero,R. M. Claramunt and D. Sanz, Chem.–Eur. J., 1996, 2, 992–1000.
29 C. Hannay, M. J. HubinFranskin, F. Grandjean, V. Briois,J. P. Itie, A. Polian, S. Trofimenko and G. J. Long, Inorg. Chem.,1997, 36, 5580–5588.
30 M. Guell, M. Sola and M. Swart, Polyhedron, 2010, 29, 84–93.31 F. Grandjean, G. J. Long, B. B. Hutchinson, L. Ohlhausen,
P. Neill and J. D. Holcomb, Inorg. Chem., 1989, 28, 4406–4414.
32 E. V. Dose, M. A. Hoselton, N. Sutin, M. F. Tweedle andL. J. Wilson, J. Am. Chem. Soc., 1978, 100, 1141–1147.
33 G. Bruno, G. Centineo, E. Ciliberto, S. Dibella and I. Fragala,Inorg. Chem., 1984, 23, 1832–1836.
34 J. C. Calabrese, P. J. Domaille, J. S. Thompson and S. Trofimenko,Inorg. Chem., 1990, 29, 4429–4437.
35 H. R. Bigmore, S. C. Lawrence, P. Mountford and C. S. Tredget,Dalton Trans., 2005, 635–651.
36 J. K. Beattie, R. A. Binstead and R. J. West, J. Am. Chem. Soc.,1978, 100, 3044–3050.
37 P. A. Anderson, T. Astley, M. A. Hitchman, F. R. Keene,B. Moubaraki, K. S. Murray, B. W. Skelton, E. R. T. Tiekink,H. Toftlund and A. H. White, J. Chem. Soc., Dalton Trans., 2000,3505–3512.
38 J. A. Wolny, H. Paulsen, A. X. Trautwein and V. Schunemann,Coord. Chem. Rev., 2009, 253, 2423–2431.
39 F. Renz, J. Hefner, D. Hill and M. Klein, Polyhedron, 2007, 26,2330–2334.
40 T. Buchen and P. Gutlich, Inorg. Chim. Acta, 1995, 231, 221–223.41 J. W. Turner and F. A. Schultz, J. Phys. Chem. B, 2002, 106,
2009–2017.42 M. Swart, A. R. Groenhof, A. W. Ehlers and K. Lammertsma,
J. Phys. Chem. A, 2004, 108, 5479–5483.43 M. Swart, J. Chem. Theory Comput., 2008, 4, 2057–2066.44 M. Swart, M. Guell and M. Sola, in Quantum Biochemistry:
Electronic structure and biological activity, ed. C. F. Matta,Wiley-VCH, Weinheim-Germany, 2010, vol. 2, pp. 551–583.
45 M. Swart, Inorg. Chim. Acta, 2007, 360, 179–189.46 M. Guell, J. M. Luis, M. Sola and M. Swart, J. Phys. Chem. A,
2008, 112, 6384–6391.47 M. Swart, M. Guell, J. M. Luis and M. Sola, J. Phys. Chem. A,
2010, 114, 7191–7197.48 M. Swart, A. W. Ehlers and K. Lammertsma, Mol. Phys., 2004,
102, 2467–2474.49 N. C. Handy and A. J. Cohen, Mol. Phys., 2001, 99, 403–412.50 J. P. Perdew, K. Burke and M. Ernzerhof, Phys. Rev. Lett., 1996,
77, 3865–3868.51 M. Swart, M. Sola and F. M. Bickelhaupt, J. Chem. Phys., 2009,
131, 094103.52 J. M. Tao, J. P. Perdew, V. N. Staroverov and G. E. Scuseria,
Phys. Rev. Lett., 2003, 91, 146401.53 K. P. Jensen, Inorg. Chem., 2008, 47, 10357–10365.54 V. N. Staroverov, G. E. Scuseria, J. Tao and J. P. Perdew, J. Chem.
Phys., 2003, 119, 12129–12137.55 Y. Zhao and D. G. Truhlar, J. Chem. Phys., 2006, 125, 194101.56 E. J. Baerends, T. Ziegler, J. Autschbach, D. Bashford,
J. A. Berger, A. Berces, F. M. Bickelhaupt, C. Bo, P. L. de Boeij,P. M. Boerrigter, L. Cavallo, D. P. Chong, L. Deng,R. M. Dickson, D. E. Ellis, M. van Faassen, L. Fan,T. H. Fischer, A. Giammona, A. Ghysels, C. Fonseca Guerra,S. J. A. van Gisbergen, A. W. Gotz, J. A. Groeneveld,O. V. Gritsenko, M. Gruning, S. Gusarov, F. E. Harris, P. vanden Hoek, C. R. Jacob, H. Jacobsen, L. Jensen, E. S. Kadantsev,J. K. Kaminski, G. van Kessel, R. Klooster, F. Kootstra,A. Kovalenko, M. V. Krykunov, E. van Lenthe, J. N. Louwen,D. A. McCormack, A. Michalak, M. Mitoraj, J. Neugebauer,V. P. Nicu, L. Noodleman, V. P. Osinga, S. Patchkovskii, P. H.T. Philipsen, D. Post, C. C. Pye, W. Ravenek, J. I. Rodrıguez,P. Romaniello, P. Ros, P. R. T. Schipper, G. Schreckenbach,J. S. Seldenthuis, M. Seth, D. G. Skachkov, J. G. Snijders,M. Sola, M. Swart, D. Swerhone, G. te Velde, P. Vernooijs,L. Versluis, L. Visscher, O. Visser, F. Wang, T. A. Wesolowski,E. M. van Wezenbeek, G. Wiesenekker, S. K. Wolff, T. K. Wooand A. L. Yakovlev, ADF 2010.01, SCM, Amsterdam, TheNetherlands, 2010.
57 G. te Velde, F. M. Bickelhaupt, E. J. Baerends, C. Fonseca Guerra,S. J. A. van Gisbergen, J. G. Snijders and T. Ziegler, J. Comput.Chem., 2001, 22, 931–967.
58 P. Th. van Duijnen, A. H. Juffer and J. P. Dijkman, THEOCHEM,1992, 260, 195–205.
59 P. Th. van Duijnen, in New challenges in computional quantumchemistry, ed. R. Broer, P. J. C. Aerts and P. S. Bagus, Dept. ofChemical Physics and Material Science, Groningen, 1994,pp. 71–84.
10456 Phys. Chem. Chem. Phys., 2011, 13, 10449–10456 This journal is c the Owner Societies 2011
60 P. Th. van Duijnen and M. Swart, J. Phys. Chem. A, 1998, 102,2399–2407.
61 P. Th. van Duijnen, M. Swart and L. Jensen, in Solvation effectson molecules and biomolecules: Computational methods andapplications, ed. S. Canuto, Springer, Dordrecht, The Netherlands,2008, pp. 39–102.
62 A. H. de Vries, ‘‘Modelling condensed-phase systems. From quantumchemistry to molecular models’’, PhD thesis, Groningen, TheNetherlands, 1995.
63 A. H. de Vries, P. Th. van Duijnen, A. H. Juffer, J. A.C. Rullmann, J. P. Dijkman, H. Merenga and B. T. Thole,J. Comput. Chem., 1995, 16, 37–55; 1445–1446.
64 A. H. de Vries, P. Th. van Duijnen, R. W. J. Zijlstra and M. Swart,J. Electron Spectrosc. Relat. Phenom., 1997, 86(1–3), 49–56.
65 B. T. Thole, P. Th. van Duijnen and J. C. d. Jager, in Structure anddynamics: Nucleic Acids and Proteins, ed. E. Clementi andR. H. Sarma, Adenine Press, Guilderland N. Y., 1983, pp. 95–105.
66 L. Jensen, P. Th. van Duijnen and J. G. Snijders, J. Chem. Phys.,2003, 118, 514–521.
67 P. Th. van Duijnen and M. Swart, J. Phys. Chem. C, 2010, 114,20547–20555.
68 F. C. Grozema, M. Swart, R. W. J. Zijlstra, J. J. Piet, L. D.A. Siebbeles and P. Th. van Duijnen, J. Am. Chem. Soc., 2005, 127,11019–11028.
69 M. Swart and P. Th. van Duijnen, Mol. Simul., 2006, 32, 471–484.70 S. J. A. van Gisbergen, V. P. Osinga, O. V. Gritsenko, R. van
Leeuwen, J. G. Snijders and E. J. Baerends, J. Chem. Phys., 1996,105, 3142–3151.
71 M. Swart, J. Comp. Meth. Sci. Engin., 2010, 10, 609–614.72 M. Swart, P. Th. van Duijnen and J. G. Snijders, J. Comput.
Chem., 2001, 22, 79–88.73 M. Swart and P. Th. van Duijnen, Int. J. Quantum Chem., 2011,
111, 1763–1772.74 M. Swart, QCosmo, 2011, in preparation.75 M. Swart, inDensity Functional Theory Applied to Copper Proteins,
PhD thesis, RuG University, Groningen, The Netherlands, 2002,pp. 40–57.
76 S. K. Wolff, Int. J. Quantum Chem., 2005, 104, 645–659.77 W. D. Cornell, P. Cieplak, C. I. Bayly, I. R. Gould, K. M. Merz
Jr., D. M. Ferguson, D. C. Spellmeyer, T. Fox, J. W. Caldwell andP. A. Kollman, J. Am. Chem. Soc., 1995, 117, 5179–5197.
78 S. Toxvaerd, Mol. Phys., 1991, 72, 159–168.79 M. P. Allen and D. J. Tildesley, Computer Simulation of Liquids,
Clarendon Press, Oxford, 1987.80 T. K. Woo, L. Cavallo and T. Ziegler, Theor. Chem. Acc., 1998,
100, 307–313.81 M. Swart, F. M. Bickelhaupt and P. Th. van Duijnen, New QM/
MM implementation in ADF, 2011, in preparation.82 L. Jensen, P. O. Astrand, A. Osted, J. Kongsted and
K. V. Mikkelsen, J. Chem. Phys., 2002, 116, 4001–4010.83 B. T. Thole, Chem. Phys., 1981, 59, 341–350.84 F. Jensen, Introduction to computational chemistry, Wiley & Sons,
New York, 1998.85 M. Swart, inDensity Functional Theory Applied to Copper Proteins,
PhD thesis, RuG University, Groningen, The Netherlands, 2002,pp. 124–127.
86 A. A. Frost and B. Musulin, J. Chem. Phys., 1954, 22, 1017–1020.87 A. A. Frost and B. Musulin, J. Am. Chem. Soc., 1954, 76,
2045–2048.88 D. R. Lide, L. I. Berger, A. K. Covington, K. Fischer,
J.-C. Fontaine, H. P. R. Frederikse, J. R. Fuhr, J. Gmehling,R. N. Goldberg, C. R. Hammond, N. E. Holden, H. D. BrookeJenkins, H. V. Kehiaian, J. A. Kerr, J. Krafczyk, F. J. Lovas,W. C. Martin, J. Menke, T. M. Miller, P. J. Mohr, J. Reader,L. E. Snyder, B. N. Taylor, T. G. Trippe, P. Vanysek, W. L. Wiese,C. Wohlfarth and D. Zwillinger, CRC Handbook of Chemistry andPhysics, CRC Press, Boca Raton (FL), USA, 2004–2005.
89 D. Antonangeli, J. Siebert, C. M. Aracne, D. L. Farber, A. Bosak,M. Hoesch, M. Krisch, F. J. Ryerson, G. Fiquet and J. Badro,Science, 2011, 331, 64–67.
90 A. Bousseksou, J. J. McGarvey, F. Varret, J. A. Real,J.-P. Tuchagues, A. C. Dennis and M. L. Boillot, Chem. Phys.Lett., 2000, 318, 409–416.