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On the identity of the radiation-induced stable alanine radicalw
Ewald Pauwels,*aHendrik De Cooman,
aMichel Waroquier,
aEli O. Hole
band
Einar Sagstuenb
Received 17th March 2010, Accepted 27th May 2010
DOI: 10.1039/c004380j
Using periodic DFT calculations, it is concluded that the stable
radiation-induced alanine radical most probably is the result of
reductive deamination and protonation of the detached amino
group, yielding an NH4+ ammonium ion and a negatively
charged radical.
Alanine dosimetry is an established technique for measuring
absorbed doses of ionizing radiation.1 When crystals or
powders of the amino acid L-a-alanine are exposed to ionizing
radiation, free radicals are formed and stably trapped in the
matrix. The number of stable radicals is proportional to the
absorbed dose, radiation dose read-out being enabled by
Electron Paramagnetic Resonance (EPR) spectroscopy.
Several radicals have been found to contribute to the overall
EPR spectrum of alanine, although a well-defined resonance
pattern due to one of the radiation-induced radical species,
often called the ‘Stable Alanine Radical’ (SAR), dominates the
spectrum.2 The structure of this radical is commonly assumed
to be that of B (Scheme 1), the stable end product of several
radiation-induced reductive processes including deamination
and protonation.3 This structure was proposed on the basis of
careful analysis of the g- and hyperfine couplings in several
EPR and ENDOR studies. In Table 1, the results of ref. 2 are
reproduced. The a- and b-proton hyperfine interactions clearly
indicate a p-type carbon-centred radical, with one hydrogen
atom and one methyl group directly bound to the radical
centre. The protonation of the carboxyl group in structure B
was first (indirectly) suggested by Kuroda and Miyagawa4
who found an additional weak hyperfine coupling (indicated
by the shorthand H(N) in Table 1) and attributed this to a
proton located close to one of the oxygens of the –COO�
group of the radical. This is consistent with chemical intuition,
as the proton compensates for the net negative charge induced
by the radiation-induced reduction event.
Since the advent of Density Functional Theory (DFT),
several theoretical studies have been performed for the
purpose of reproducing the EPR properties of alanine
radicals5,6 and the SAR in particular.7–9 However, only the
isotropic parts of the hyperfine couplings were calculated and
the radicals were considered being in the gas phase or in a very
rudimentary solution model. In the present work, a complete
theoretical determination of the g- and hyperfine coupling
tensors of the SAR using periodic DFT calculations is
reported. The application of periodic boundary conditions to
simulate the solid-state environment of a radical has proven
particularly successful in the reproduction of these EPR
properties.10,11 In addition, periodic calculations allow an
evaluation of the stability of a radical structure within its
solid-state environment and can also give insight into its
formation mechanism.12,13 The calculations strongly suggest
that B is not the correct structure of the SAR. Instead,
convincing evidence is presented in support of structure C, a
radical structure in which the abstracted amino group is
protonated, instead of the carboxyl group of the radical.
All DFT calculations were performed with the CP2K
software14 and the BLYP functional.15,16 The basic unit for
the periodic calculations was chosen to be the crystallographic
unit cell of alanine,17 duplicated along all directions [2a2b2c].
In this way, the interaction of a radical with its periodic images
is prevented. The Gaussian and plane waves (GPW) dual basis
set method18 was used in all geometry optimizations, employing
a TZVP triple-z Gaussian basis set19 and plane waves (300 Ry
density cut-off) with GTH pseudopotentials.20,21 For the
subsequent g- and hyperfine coupling tensor calculations, we
relied on recent implementations10,11 in the CP2K code,
employing the all-electron Gaussian and augmented plane
wave (GAPW) method.22 The density cut-off for the auxiliary
plane wave basis set was 200 Ry and the all-electron TZVP
basis23 was used. This methodology has proven successful in
other studies.24
Since the SAR presumably is an end product of reductive
radiation damage to the alanine crystal, we started by
simulating a periodic box with a net negative charge. One of
the 16 alanine molecules in this box was altered in accordance
with structure A (Scheme 1) by elongating the C–N bond.
Subsequent optimization proved this structure to be stable,
with an absolute energy of �1010.16267 a.u. for the entire
periodic box. Only deamination took place during the
optimization of this structure, yielding a separate NH3
molecule. Intriguingly, the carboxyl group of this radical
Scheme 1 The chemical structure of L-a-alanine and several suggested
structures for the Stable Alanine Radical.
a Center for Molecular Modeling, Ghent University, Technologiepark903, B-9052 Zwijnaarde, Belgium, QCMM-alliance Ghent-BrusselsBelgium. E-mail: [email protected]
bDepartment of Physics, University of Oslo, P.O. Box 1048 Blindern,N-0316 Oslo, Norway
w Electronic supplementary information (ESI) available: CalculatedEPR properties for B-like structures. See DOI: 10.1039/c004380j
This journal is �c the Owner Societies 2010 Phys. Chem. Chem. Phys., 2010, 12, 8733–8736 | 8733
COMMUNICATION www.rsc.org/pccp | Physical Chemistry Chemical Physics
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remained not protonated, thus maintaining a net negative
charge on the radical. Yet, Kuroda and Miyagawa4 argued
in their experimental paper that the carboxyl group is proto-
nated, and that this COOH proton is transferred from the
NH3 group of a nearby, hydrogen-bound molecule. In the
alanine crystal, the carboxyl group of each molecule is
involved in three hydrogen bonds with the amino groups of
three separate neighbouring molecules. In structure A (Fig. 1),
the radical participates in the same three hydrogen bonds.
Proton transfer along each of these three routes was explored.
Starting from structure A, the O–H distance between the
carboxyl oxygen of the radical and the amino proton of a
nearby molecule was constrained to a value of 0.9 A and the
geometry was optimized. This resulted in three structures,
similar to structure B, in which the negative charge of the
radical was effectively transferred to the neighbouring
molecule. However, these constrained species proved to be
severely less stable than structure A (with energy differences of
about 600 kJ mol�1), and they all reverted back to structure A
in a second, unconstrained optimization.
The instability of these structures suggests that structure B
is not valid. However, comparison of the calculated EPR
properties for structure A with the experimental values gives
no convincing evidence that A is the true structure of the SAR
either. As is evident from Table 1, two major hyperfine
interactions are present in this structure. Their anisotropic
couplings are characteristic for the typical patterns of a- andb-type hyperfine interactions. The corresponding isotropic
couplings, on the other hand, are largely underestimated with
respect to the experimental data. Even though this particular
EPR property depends significantly on the chosen density
functional or basis set,25 a difference of 30 MHz altogether
for the Hb interaction is unrealistically large. In addition, the
eigenvectors of the anisotropic hyperfine interactions do not
agree well with their experimental counterparts: the angles
between corresponding eigenvector directions are at least 251.
The calculated g-tensor is somewhat better: the g-values are
quite comparable and the eigenvector corresponding to the
maximum g-value deviates only 131 from the corresponding
experimental direction. Nevertheless, previous studies with a
similar methodology13,24,26,27 have clearly shown that valid
radical structures give rise to calculated EPR properties that
are in much better accordance with experimental data. Here,
the overall agreement of all EPR parameters is disappointing
and strongly suggests that structure A is not the appropriate
structure of the SAR. Structure B is also rejected, from
stability considerations.
In the previous simulations, the net negative charge of the
periodic cell (induced by the reductive radiation event) was not
counteracted. Proton transfers were considered, but only
between the radical and one of its surrounding molecules. In
that situation, the negative charge is still localized in the direct
vicinity of the radical and, in addition, the hydrogen-bonding
network of the radical is modified. Proton transfer between the
radical and an alanine molecule further away in the crystal
would leave this network intact and would also restore the
local charge neutrality. Such long-range proton transfers do
Table 1 Isotropic and anisotropic hyperfine couplings (in MHz) andg-tensor values of the stable alanine radical (experiment) and twomodel structures. The last column indicates the angle (in degrees)between corresponding experimental and calculated eigenvectordirections.
Aiso/giso Aaniso/ganiso Angle
Experiment Hb 69.9 �2.6 Ref. 2�2.34.8
Ha �56.1 �31.83.927.9
g 2.0033 2.00242.00342.0041
H(N) 0.2 �4.0 Ref. 4�1.75.7
A Hb 37.4 �2.8 47�2.2 475.0 25
Ha �36.1 �26.2 81�2.4 9028.6 33
g 2.0036 2.0023 262.0039 232.0047 13
C Hb 71.5 �2.7 3�2.0 34.7 2
Ha �42.6 �30.1 1�2.6 432.6 4
g 2.0041 2.0023 32.0045 42.0056 5
H(N) 0.0 �4.2 3�1.0 35.2 6
Fig. 1 Three-dimensional view of the periodic cell of alanine with the
optimized structures A and C. The radical centres are represented by
balls and sticks, and are additionally expanded at the bottom of the
Figure. Green lines indicate hydrogen bonds between the radical
carboxyl group and amino groups of neighbouring alanine molecules.
8734 | Phys. Chem. Chem. Phys., 2010, 12, 8733–8736 This journal is �c the Owner Societies 2010
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occur in irradiated biomolecular crystals. Not only are protons
formed as side products of oxidative radiation damage,
‘hopping’ of protons along hydrogen-bond chains has been
observed in both experimental28–30 and theoretical studies.31
The effects of such a process can most easily be simulated by
just adding one proton to the periodic cell, neutralizing the net
negative charge. Reconsidering structure A, there are two
likely sites for this proton: the –COO� group and the detached
NH3 group. Addition to either oxygens of the radical carboxyl
group resulted in stable structures similar to B (with the
difference that the COOH proton was now simply added
and not transferred from a neighbouring molecule). Proton
addition on the detached amino group resulted in the
formation of an NH4+ ammonium ion next to the negatively
charged radical (structure C in Scheme 1). This species proved
significantly more stable than the other two, with an absolute
energy of �1010.8671 a.u. at least 100 kJ mol�1 lower than the
others.
The calculated EPR properties for the B-like structures
(presented in the ESI as B-1 and B-2w) are in poor corres-
pondence with the experimental values for the SAR. Those of
structure C, on the other hand, are in near perfect agreement
with experiment (Table 1). The isotropic Hb coupling differs
by less than 2 MHz, whereas the difference between the
calculated and experimental Ha isotropic coupling is reduced
to 13 MHz. Most strikingly, however, is that all experimental
eigenvector directions are reproduced to within 61. In previous
works, these directional parameters proved to be particularly
useful to gauge the accuracy of a proposed radical model.32
The g-tensor is also nicely reproduced. Even though the actual
g-values differ somewhat more from their experimental
counterparts than for structure A, the eigenvector directions
are almost perfectly aligned with experiment. Comparing the
radical structures A and C in the lower part of Fig. 1, it is clear
that the additional amino proton has induced a reorientation
of the Ca–Ha bond in structure C. This feature is clearly
responsible for the improved agreement of calculated EPR
properties for structure C.
In view of its stability and the overall exceptional agreement
between calculated and experimental EPR properties, there is
little doubt that structure C to date represents the most
probable candidate for the structure of the stable alanine
radical. Since this structure has both a positively and
negatively charged part (illustrated in Scheme 1), it closely
resembles the zwitterionic form of undamaged alanine
molecules, which might explain the observed stability of this
radical. Finally, the additional H(N) dipolar hyperfine inter-
action that was observed by Kuroda et al.4 is clearly not due to
a proton attached to the carboxyl group. Rather, the proton is
bound to the amino group but still is in close proximity to the
radical (Fig. 1). The calculated hyperfine tensor for this
additional amino proton in structure C (also shown in
Table 1) is in perfect agreement with the experimental H(N)
tensor.
It is quite likely that the additional proton in structure C
actually originates from the other half of the radiation-
induced ionization process. A reduction site is generated for
every oxidation site. In alanine, oxidative radical formation
invariably involves deprotonation, giving rise to excess
protons.3 It is conceivable that these protons eventually
migrate towards the reduction sites, where they protonate
the detached NH3 group, effectively restoring charge
neutrality in both the oxidation and reduction site.
In conclusion, we have convincingly determined the true
structure of the stable alanine radical using periodic DFT
calculations. In structure C, the amino group of alanine
is detached and is further protonated, yielding an NH4+
ammonium ion trapped next to the negatively charged
radical.
Acknowledgements
This work is supported by the Fund for Scientific Research—
Flanders (FWO), the Research Board of the Ghent University
and BELSPO in the frame of IAP 6/27. The authors E. P. and
H. D. C. acknowledge a Postdoctoral Fellowship with the
FWO. Part of the computational resources and services used
in this work were provided by Ghent University.
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8736 | Phys. Chem. Chem. Phys., 2010, 12, 8733–8736 This journal is �c the Owner Societies 2010
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