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ISSN 1359-7345
Chemical Communications
www.rsc.org/chemcomm Volume 49 | Number 30 | 18 April 2013 | Pages 3061–3160
COMMUNICATION
Akira Ikezaki, Mikio Nakamura et al.
Equilibrium between Fe(
IV) porphyrin and Fe(III) porphyrin radical cation: new insight into the
electronic structure of high-valent iron porphyrin complexes
3098 Chem. Commun., 2013, 49, 3098--3100 This journal is
c
The Royal Society of Chemistry 2013
Cite this: Chem. Commun., 2013,
49, 3098
Equilibrium between Fe(IV) porphyrin and Fe(III)
porphyrin radical cation: new insight into the
electronic structure of high-valent iron porphyrin
complexes†
Akira Ikezaki,*
a
Masashi Takahashi
bc
and Mikio Nakamura*
bc
UV-Vis,NMR,andMo
¨
ssbauer studies have revealed that [Fe(TMP)(N
3
)
2
],
showing the Mo
¨
ssbauer parameters quite similar to those of the fe rryl
species of MauG, CytP450
BM3
,CytP450
CAM
, and CPO, exists as equili-
brium mixtur es of Fe(
IV) porphyrin and Fe(III) porphyrin radical cation.
It is now well established that there are two types of electronic
ground states in low-spin Fe(
III) porphyrins depending on which d
orbital has unpaired electron, i.e. (d
xy
)
2
(d
xz
,d
yz
)
3
(d
p
-type) and
(d
xz
,d
yz
)
4
(d
xy
)
1
(d
xy
-type).
1,2
One electron oxidation of Fe(III)
porphyrins usually produces Fe(
III)porphyrinradicalcations,
whereanelectronisremovedfromtheporphyrina
2u
HOMO i n
thecaseofmeso-substituted complexes.
3–5
Because the Fe(III)ion
has various spin-states and electron configurations, the Fe(
III)
porphyrin radical cations should have a wide variety of electronic
ground states. If the Fe(
III) ion is a low-spin ion, two types of
electronic ground states are expected, i.e. (d
xy
)
2
(d
xz
,d
yz
)
3
(a
2u
)
1
and
(d
xz
,d
yz
)
4
(d
xy
)
1
(a
2u
)
1
states.Wehaverecentlyreportedthat,while
[Fe
III
(TMP
)(HIm)
2
]
2+
(1)‡ adopts the (d
xy
)
2
(d
xz
,d
yz
)
3
(a
2u
)
1
ground
state with total spin S =1,[Fe
III
(TMP
)(
t
BuNC)
2
]
2+
exhibits the
diamagnetic S =0(d
xz
,d
yz
)
4
(d
xy
,a
2u
)
2
ground state because of the
strong interaction between half-occupied a
2u
and half-occupied
d
xy
orbitals probably in the ruffled porphyrin framework.
5–8
Furthermore, [Fe
III
(TMP
)(4,5-Cl
2
Im)
2
]
2+
has exhibited the
1
H NMR spectroscopic properties which are just between those
of 1 and [Fe
III
(TMP
)(
t
BuNC)
2
]
2+
.Thus,[Fe
III
(TMP
)(4,5-Cl
2
Im)
2
]
2+
exists as an equilibrium mixture of the two electron configura-
tional isomers as shown in eqn (1), which is a general description
to express the electronic structure of all the low-spin Fe(
III)
porphyrin radical cations.
5,6
The idea has led us to expect
(d
xy
)
2
(d
xz
,d
yz
)
3
(a
2u
)
1
$ (d
xz
,d
yz
)
4
(d
xy
,a
2u
)
2
(1)
that there should also be an equilibrium between two kinds of
one-electron oxidation products of Fe(
III) porphyrin, i.e. Fe(IV)
porphyrin and Fe(
III) porphyrin radical cation. Thus, some
complexes should exhibit the spectroscopic properties that
are just between those of pure Fe(
IV) porphyrin and Fe(III)
porphyrin radical cation. In this communication, we will report
a rare example showing the equilibrium mentioned above.
The complex in question is [Fe(TMP)(N
3
)
2
](2), which has
been prepared by the addition of the CH
3
OH solution of NaN
3
to the CH
2
Cl
2
solution of [Fe
III
(TMP
)(ClO
4
)
2
] at 193 K.
9
Fig. S1
of ESI† shows the UV-Vis spectra observed by the stepwise
addition of NaN
3
. The absence of the isosbestic point supports
the stepwise formation of 2. It should be noted that a very broad
band ascribed to the porphyrin radical is still observable
between 650 and 750 nm even after the addition of 20 equiv.
of N
3
, suggesting that 2 maintains some radical character.
1
H NMR spectra shown in Fig. S2 of ESI† were obtained by the
addition of 2.0 equiv. of NaN
3
(CD
3
OD solution) to the CD
2
Cl
2
solution of [Fe
III
(TMP
)(ClO
4
)
2
] at 195 K. Two characteristic
signals are observed at 42.1 and +34.3 ppm assigned to the
pyrrole-H(py-H) and meta-H signals, respectively, on the basis
of the spectral comparison with the pyrrole-d
8
complex. The
large isotropic shifts of these signals clearly indicate that 2 is
expressed as the low-spin Fe(
III) porphyrin radical cation as 1.
4,5
Table 1 lists the
1
H NMR chemical shifts (CD
2
Cl
2
, 195 K) of one-
electron oxidation products of Fe(
III) porphyrin complexes.
Close inspection of the data in Table 1 reveals that the meta-H
signal shifts upfield from +58.2 to +34.3, and then to +7.7 ppm as the
axial ligand changes from HIm( 1)toN
3
(2), and then to CH
3
O
(3);
3 is well characterized as an Fe(
IV)complexwithS =1.
9
Thus, the
spin densitie s at the meso -C atoms decrease on going from 1 to 2,
and then to 3, which in turn indicates that the radical character
decreases in the same order. In contrast, the py-H signal shifts
downfield from 61.2 to 42.1 ppm as the axial HIm ligand
is replaced by N
3
. The result also supports the decrease in
radical c haracter; the downfield shift of the py-H signal is 22 ppm
at 217 K when radical cationic [Fe
III
(TDP
)(HIm)
2
]
2+
is reduced to
[Fe
III
(TDP)(HIm)
2
]
+
.
5
The downfield shift is, however, only 4.5 ppm,
when the axial N
3
ligand is replaced by CH
3
O
, which is in sharp
a
Department of Chemistry, School of Medicine, Toho University, Otaku, Tokyo 143-
8540, Japan. E-mail: ikezaki@med.toho-u.ac.jp
b
Department of Chemistry, Faculty of Science, Toho University, Funabashi, Chiba
274-8510, Japan. E-mail: mnakamu@med.toho-u.ac.jp
c
Research Center for Materials with Integrated Properties, Toho University,
Funabashi, 274-8510, Japan
† Electronic supplementary information (ESI) available. See DOI: 10.1039/
c3cc40319j
Received 14th January 2013,
Accepted 11th February 2013
DOI: 10.1039/c3cc40319j
www.rsc.org/chemcomm
ChemComm
COMMUNICATION
This journal is
c
The Royal Society of Chemistry 2013 Chem. Commun., 2013, 49, 3098--3100 3099
contrast to the case of the meta-Hsignal.Thisisbecausetheelectronic
structure of iron changes from (d
xy
)
2
(d
xz
,d
yz
)
3
in 1 to (d
xy
)
2
(d
xz
,d
yz
)
2
in
3.Because3 has two unpaired electrons in the d
p
orbitals, the py-H
signal appears quite upfield, 37.5 ppm, in spite of the absence of the
radical spin on the porphyrin ring. As mentioned, the chemical shift
of the meta-H signal of 2 is just between the corresponding signals of
1 and 3. The result suggests that 2 should best be expressed as an
equilibrium mixture of Fe(
III) porphyrin radical cation and Fe(IV)
porphyrin as shown by eqn (2). The equilibrium constant is supposed
to be close to 1 on the basis of the chemical shifts of the meta-H
signals in 1–3.The
1
H NMR result is consistent with the UV-Vis result
showing the presence of radical species.
(d
xy
)
2
(d
xz
,d
yz
)
3
(a
2u
)
1
$ (d
xy
)
2
(d
xz
,d
yz
)
2
(a
2u
)
2
(2)
In order to reveal the factors that can affect the equilibrium given
ineqn(2),wehavepreparedaseriesofpara-substituted complexes
[Fe(p-X-TPP)(N
3
)
2
], where X is OCH
3
,H,F,andCF
3
group. The
chemical shifts of these complexes determined at 193 K are also
listed in Table 1 together with the Hammett s
p
values. The plots of the
ortho-andmeta-H chemical shifts against Hammett s
p
values have
yielded a good linearity as shown in Fig. 1 with the slopes +28.8 and
17.1 ppm, respectively. This is because the a
2u
orbital is stabilized by
the electron withdrawing para-substituent, which in turn destabilizes
the radical cationic state, resulting in the increases in population
of the Fe(
IV) isomer. The chemical shifts of the meta-H and py-H
signals of [Fe(p-CF
3
-TPP)(N
3
)
2
]are16.5and40.1 ppm, respectively,
both of which are much closer to the corresponding signals of 3, i.e.
7.7 and 37.5 ppm, respectively, as compared with those of other
complexes. These results support that [Fe(p-CF
3
-TPP)(N
3
)
2
]exists
mainly as the Fe(
IV) isomer though the population of the Fe(III)
porphyrin radical cation is not negligibly small.
One can argue that the electron withdrawing meso-substituents
make the a
2u
orbital stabilize so that the HOMO could be changed
from the a
2u
to the a
1u
orbital. In such a case, the decrease in
isotropic shift observed for the meta-H signal can be explained in
terms of the increase in population of the a
1u
radical cation because
the a
1u
orbital has zero coefficient at the meso-C atoms.
10,11
However,
if [Fe(p-CF
3
-TPP)(N
3
)
2
]isactuallyexpressedasthea
1u
radical cation,
then the py-H signal should appear extremely upfield because the
a
1u
orbital has large coefficient on the b-pyrrole positions.
10,11
The
data in Table 1 indicate that the py-H signals of these complexes are
observed in a relatively narrow region, i.e. 32.1 to 40.1 ppm.
Therefore, we have considered that [Fe(p-CF
3
-TPP)(N
3
)
2
]existsnotas
the low-spin Fe(
III)witha
1u
porphyrin radical cation but mainly as
the Fe(
IV)porphyrin.
The above-mentioned hypothesis has further been confirmed by
the Mo
¨
ssbauer spectroscopy.
12–15
Fig. 2 shows the Mo
¨
ssbauer
spectra of
57
Fe(95%) enriched 1 and 2 takeninfrozenmethanol
solution at 77 K. In each spectrum, there are at least two minor
components considered to be the decomposed and/or reduced
products. Table 2 lists the Mo
¨
ssbauer parameters together with
those of 3.
9
While the isomer shift (d per mm s
1
)andquadrupole
Table 1 NMR chemical shifts and electronic structures of oxidized complexes
Complexes
1
H NMR chemical shifts
a
s
p
b
Electronic structure
c
Ref.o-CH
3
(o-H) m-H p-CH
3
(p-H) py-H
[Fe(TMP)(
t
BuNC)
2
]
2+
2.5 6.6 2.2 4.7 — A 6
[Fe(TMP)(4,5-Cl
2
Im)
2
]
2+ d
24.8
e
4.0
e
25.6
e
—A$ B6
[Fe(TMP)(HIm)
2
]
2+
(1) 23.0 58.2 7.1 61.2 — B 6
[Fe(TMP)(N
3
)
2
](2) 11.6 34.3 5.4 42.1 — B $ C This work
[Fe(p-X-TPP)(N
3
)
2
]
f
X=CH
3
O(22.9) 30.4 — 36.3 0.28 B $ C This work
X=H (15.4) 25.9 (7.5) 32.1 0.00 B $ C This work
X=F (10.6) 21.5 — 34.8 0.06 B $ C This work
X=CF
3
(0.4) 16.5 — 40.1 0.53 B $ C This work
[Fe(TMP)(CH
3
O)
2
](3)
g
2.4 7.7 2.9 37.5 — C 9
a
Chemical shifts (d p pm) determined in CD
2
Cl
2
at 193 K.
b
Hammett s
p
values.
c
Electronic structure of isomer: A, (d
xz
,d
yz
)
4
(d
xy
,a
2u
)
2
;B,(d
xy
)
2
(d
xz
,d
yz
)
3
(a
2u
)
1
;
and C, (d
xy
)
2
(d
xz
,d
yz
)
2
(a
2u
)
2
.
d
Each signal splits into several signals due to the slow rotation about the Fe–N
axial
bond.
e
Data at 213 K.
f
p-X-TPP is a
dianion of meso-tetrakis(p-substituted phenyl)porphyrin.
g
Data at 195 K.
Fig. 1 Plots of the chemical shifts against Hammett s
p
values in a series of
[Fe(p-X-TPP)(N
3
)
2
]: (a) ortho-H and (b) meta-H.
Fig. 2 Mo
¨
ssbauer spectra of
57
Fe(95%) enriched (a) 1 and (b) 2 taken in frozen
methanol solution at 77 K.
Communication ChemComm
3100 Chem. Commun., 2013, 49, 3098--3100 This journal is
c
The Royal Society of Chemistry 2013
splitting (DE
q
per mm s
1
)valuesof1 are in the region of low-spin
d
p
-type Fe(III) complexes, those of 2 are outside of this region as
showninFig.S3ofESI.†Thus,theobservedd and DE
q
values of 2,
0.12 and 2.27 mm s
1
, respectively, suggest that 2 exists as an
equilibrium mixture of Fe(
III)porphyrinradicalandFe(IV)porphyrin.
It is interesting to compare the Mo
¨
ssbauer parameters of 2
with those of heme proteins adopting the Fe(
IV) oxidation state.
MauG is a naturally occurring diheme protein that catalyzes the
final step in the biosynthesis of the protein-derived tryptophan
tryptophylquinone (TTQ) prosthetic group of methylamine
dehydrogenase (MADH).
16,17
The reactive intermediates of
MauG consist of two distinct Fe(
IV) species, heme 1 and heme
2.
18
Heme 1 is considered to be the Fe
IV
QO species with the d
and DE
q
values to be 0.06 and 1.70 mm s
1
, respectively. Heme
2, having a His–Tyr axial ligation, is quite unusual as a c-type
heme protein.
19
It shows the d and DE
q
values to be 0.17 and
2.54 mm s
1
, respectively, which are larger than the corres-
ponding values of any other Fe(
IV) species reported previously.
18
A quantum chemical calculation has revealed that the coordina-
tion structure should be Fe
IV
(His)(Tyr
).
20
Chloroperoxidase compound II exists as two distinct ferryl
species. The major species has d and DE
q
values to be 0.10 and
2.06 mm s
1
, respectively, and is considered to have a protonated
ferryl group, i.e. Fe
IV
(Cys
)(OH
).
21,22
The minor species showing
a much smaller DE
q
value, 1.59 mm s
1
, has tentatively been
assigned as Fe
IV
QO(Cys
). The Mo
¨
ssbauer parameters of the
compound II in cytochrome P450
BM3
and P450
CAM
have been
reported as follows: 0.13 (d) and 2.16 (DE
q
)mms
1
for th e former,
and 0.14 (d)and2.06(DE
q
)mms
1
for the latter at physiological
pH.
22
These intermediates are also known to have a protonated
ferryl unit, i.e.,Fe
IV
(Cys
)(HO
).
23
The data in Table 2 indicate
that the Mo
¨
ssbauer parameters of these intermediates are quite
close to the corresponding values of 2. Thus, it might be reason-
able to assume that the reaction intermediates of these heme
proteins, which commonly have a Fe
IV
(Cys
)(HO
) structure also
exist as an equilibrium either between Fe(
IV)porphyrinandFe(III)
porphyrin radical cation or between Fe(
IV)porphyrinandFe(III)
porphyrin with radical center on the protein. In fact, Li and
co-workers have pointed out the possibility of the equilibrium
between MauG based diheme and protein radical cation.
18
In conclusion, we have found on the basis of the UV-Vis,
1
H NMR, and Mo
¨
ssbauer spectroscopy that [Fe(TMP)(N
3
)
2
]existsas
an equilibrium mixture of Fe(
IV) porphyrin and Fe(III)porphyrin
radical cation, and that the population of the isomers can be
controlledbythenatureofaxialligands and peripheral substituents.
The synthesis and characte rization of a wide variety of high-va lent
complexes having HO a s one of the axial ligands such as
[Fe(Por)(X)(HO
)]
+
and [Fe(Por)(Y
)(HO
)] are quite important since
they can be good models for the reactive intermediates involved in
the catalytic cycles of cytochrome P450 and peroxidase. Such a study
is now in progress in this group.
This work was supported by Grant-in-Aid for Scientific
Research (No. 21750175 to A.I. and 22550157 to M.N.) from
MEXT, Japan. This work was partly supported by the Research
Center for Materials with Integrated Properties, Toho University.
A.I. is grateful for Toho University Joint Research Fund.
Notes and references
‡ Abbreviations: TMP, TDP, and p-CF
3
-TPP are the dianions of
5,10,15,20-tetramesitylporphyrin, 5,10,15,20-tetradurylporphyrin, and
5,10,15,20-tetrakis(4-trifluoromethylphenyl)porphyrin, respectively. Por is
thedianionofporphyriningeneral.HIm,imidazole;4,5-Cl
2
Im, 4,5-dichloro-
imidazole;
t
BuNC, tert-butylisocyanide.
1 F. A. Walker, in The Porphyrin Handbook, ed. K. M. Kadish,
K. M. Smith and R. Guilard, Academic Press, San Diego, 2000,
vol. 5, ch. 36.
2 M. Nakamura, Coord. Chem. Rev., 2006, 250, 2271.
3 M. A. Phillippi, E. T. Shimomura and H. M. Goff, Inorg. Chem., 1981,
20, 1322.
4 H. M. Goff and M. A. Phillippi, J. Am. Chem. Soc., 1983, 105, 7567.
5 A. Ikezaki, Y. Ohgo and M. Nakamura, Coord. Chem. Rev., 2009,
253, 2056.
6 A. Ikezaki, H. Tukada and M. Nakamura, Chem. Commun., 2008, 2257.
7 A. C. Chamberlin, A. Ikezaki, M. Nakamura and A. Ghosh, J. Phys.
Chem. B, 2011, 115, 3642.
8 J. Conradie and A. Ghosh, J. Phys. Chem. B, 2003, 107, 6486.
9 J. T. Groves, R. Quinn, T. J. McMurry, M. Nakamura, G. Lang and
B. Boso, J. Am. Chem. Soc., 1985, 107, 354.
10 H. Fujii, J. Am. Chem. Soc., 1993, 115, 4641.
11 H. Fujii, T. Yoshimura and H. Kamada, Inorg. Chem., 1997, 36, 6142.
12 P. G. Debrunner, Mo
¨
ssbauer Spectroscopy of Fe Porphyrins,inIron
Porphyrin Part III: Physical Bioinorganic Chemistry, ed. A. B. P. Lever
and H. B. Gray, VCH, New York, 1989, vol. 4, pp. 139–234.
13 P. Gu
¨
tlich, E. Eckhard and A. X. Trautwein, Mo
¨
ssbauer Spectroscopy
and Transition Metal Chemistry, Springer-Verlag, Berlin, 2011, p. 568.
14 E. V. Kudrik, P. Afanasiev, L. X. Alvarez, P. Dubourdeaux,
M. Cle
´
mancey, J.-M. Latour, G. Blondin, D. Bouchu, F. Albrieux,
S. E. Nefedov and A. B. Sorokin, Nat. Chem., 2012, 4, 1024.
15 The isomer shift values are given relative to a-iron foil at room
temperature.
16 Y. Wang, M. E. Graichen, A. Liu, A. R. Pearson, C. M. Wilmot and
V. L. Davidson, Biochemistry, 2003, 42, 7318.
17 C. M. Wilmot and E. T. Yukl, Dalton Trans., 2013, 42, 3127.
18 X. Li, R. Fu, S. Lee, C. Krebs, V. L. Davidson and A. Liu, Proc. Natl.
Acad. Sci. U. S. A.
, 2008, 105, 8597.
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Science, 2010, 327, 1392.
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21 M. T. Green, J. H. Dawson and H. B. Gray, Science, 2004, 304, 1653.
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J. Am. Chem. Soc., 2006, 128, 11471.
Table 2 Mo
¨
ssbauer parameters and coordination structures of high-valent
hemes
Complexes
d
(mm s
1
)
DE
q
(mm s
1
)
Coordinating
atoms Ref.
[Fe(TMP)(HIm)
2
]
2+
(1)
a
0.15 1.87 N, N This work
[Fe(TMP)(N
3
)
2
](2)
a
0.12 2.27 N
,N
This work
[Fe(TMP)(CH
3
O)
2
](3)
b
0.025 2.104 O
,O
9
[Fe(TMP)(CH
3
O)
2
](3)
c
0.022 2.117 O
,O
9
Reaction intermediates of MauG
d
Heme 1, MauG 0.06 1.70 N, O
2
18
Heme 2, MauG 0.17 2.54 N, O
18
Ferryl form of CPO
d
0.10 2.06 S
,O
22
0.11 1.59 S
,O
2
22
Ferryl form of P450
BM3
d
0.13 2.16 S
,O
23
Ferryl form of P450
CAM
d
0.14 2.06 S
,O
23
a
Frozen methanol solution at 77 K.
b
Frozen toluene–methanol
solution at 77 K.
c
Frozen toluene–methanol solution at 4.2 K.
d
Frozen
water solution at 4.2 K.
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