Cp? Noninnocence Leads to a Remarkably Weak C-H Bond via Metallocene Protonation

Article abstract of DOI:10.1021/jacs.9b00193

Metallocenes, including their permethylated variants, are extremely important in organometallic chemistry. In particular, many are synthetically useful either as oxidants (e.g., Cp₂Fe⁺) or as reductants (e.g., Cp₂Co, Cp?₂Co, and Cp?₂Cr). The latter have proven to be useful reagents in the reductive protonation of small-molecule substrates, including N₂. As such, understanding the behavior of these metallocenes in the presence of acids is paramount. In the present study, we undertake the rigorous characterization of the protonation products of Cp?₂Co using pulse electron paramagnetic resonance (EPR) techniques at low temperature. We provide unequivocal evidence for the formation of the ring-protonated isomers Cp?(exo/endo-η⁴-C₅Me₅H)Co⁺. Variable temperature Q-band (34 GHz) pulse EPR spectroscopy, in conjunction with density functional theory (DFT) predictions, are key to reliably assigning the Cp?(exo/endo-η⁴-C₅Me₅H)Co⁺ species. We also demonstrate that exo-protonation selectivity can be favored by using a bulkier acid and suggest this species is thus likely a relevant intermediate during catalytic nitrogen fixation given the bulky anilinium acids employed. Of further interest, we provide physical data to experimentally assess the C-H bond dissociation free energy (BDFE_C-H) for Cp?(exo-η⁴-C₅Me₅H)Co⁺. These experimental data support our prior DFT predictions of an exceptionally weak C-H bond (<29 kcal mol^-1), making this system among the most reactive (with respect to C-H bond strength) to be thoroughly characterized. These data also point to the propensity of Cp?(exo-η⁴-C₅Me₅H)Co to mediate hydride (H^-) transfer. Our findings are not limited to the present protonated metallocene system. Accordingly, we outline an approach to rationalizing the reactivity of arene-protonated metal species, using decamethylnickelocene as an additional example.

Full text of DOI:10.1021/jacs.9b00193

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Article
Cp* Non-innocence Leads to a Remarkably
Weak C-H Bond via Metallocene Protonation
Matthew J. Chalkley, Paul H. Oyala, and Jonas C. Peters
J. Am. Chem. Soc., Just Accepted Manuscript • DOI: 10.1021/jacs.9b00193 • Publication Date (Web): 21 Feb 2019
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Cp* Non-innocence Leads to a Remarkably Weak C–H Bond via Me-
tallocene Protonation
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Matthew J. Chalkley, Paul H. Oyala,* and Jonas C. Peters*
Division of Chemistry and Chemical Engineering, California Institute of Technology (Caltech), Pasadena, California 91125,
United States
ABSTRACT Metallocenes, including their permethylated variants, are extremely important in organometallic chemistry. In partic-
ular, many are synthetically useful either as oxidants (e.g., Cp2Fe+) or as reductants (e.g., Cp2Co, Cp*2Co and Cp*2Cr). The latter
have proven to be useful reagents in the reductive protonation of small molecule substrates, including N2. As such, understanding
the behavior of these metallocenes in the presence of acids is paramount. In the present study, we undertake the rigorous characteri-
zation of the protonation products of Cp*2Co using pulse EPR techniques at low temperature. We provide unequivocal evidence for
the formation of the ring protonated isomers Cp*(exo/endo-η4-C5Me5H)Co+. Variable temperature Q-Band (34 GHz) pulse EPR
spectroscopy, in conjunction with DFT predictions, are key to reliably assigning the Cp*(exo/endo-η4-C5Me5H)Co+ species. We
also demonstrate that exo-protonation selectivity can be favored by using a bulkier acid and suggest this species is thus likely a
relevant intermediate during catalytic nitrogen fixation given the bulky anilinium acids employed. Of further interest, we provide
physical data to experimentally assess the C−H bond dissociation free energy (BDFEC−H) for Cp*(exo-η4-C5Me5H)Co+. These ex-
perimental data support our prior DFT predictions of an exceptionally weak C–H bond (<29 kcal mol−1), making this system among
the most reactive (with respect to C–H bond strength) to be thoroughly characterized. These data also point to the propensity of
Cp*(exo-η4-C5Me5H)Co to mediate hydride (H−) transfer. Our findings are not limited to the present protonated metallocene sys-
tem. Accordingly, we outline an approach to rationalizing the reactivity of arene-protonated metal species, using decamethylnickel-
ocene as an additional example.
1. INTRODUCTION
ates have not been reliably identified and characterized. It has
been presumed that the direct reactions of acids with reducing
metallocenes are deleterious to selectivity for N2RR versus H2
generation.4,15
Metallocenes such as ferrocene, chromocene, and cobaltocene
have enjoyed a privileged role in the development of organo-
metallic chemistry and serve as useful reagents owing to their
high compositional stabilities and accessible redox couples.1,2
Indeed, many chemists first encounter metallocenes in the
context of their one-electron redox chemistry, with the
Our lab became interested in metallocenes following the ob-
servation that Cp*2Co could serve as the electron source for
Fe-mediated N2RR in the presence of anilinium acids and an
Cp2Fe+/0 Cp2Cr+/0, and Cp2Co+/0 couples, and those of their
iron catalyst, P3 Fe (P3B = tris(o-diisopropylphosphinophenyl)-
B
,
related permethylated variants, being some of the most com-
borane).8,9 Indeed, the selectivity for N2RR under these condi-
tions proved far more efficient for NH3 formation (up to 78%)
than our originally published conditions using KC8 and
monly exploited in all of synthetic chemistry.3
An area where divalent metallocene reductants (e.g., Cp2*Cr,
Cp2*Co) have been proven particularly effective is catalytic
N2-to-NH3 conversion (N2RR).4,5,6 Schrock first identified their
utility in this context via the discovery of a molybdenum
tris(amido)amine ([HIPTN3N]Mo, HIPTN3N = [(3,5-(2,4,6-
iPr3C6H2)2C6H3NCH2CH2)3N]3−) N2RR catalyst system em-
ploying lutidinium as the acid and Cp2*Cr as the reductant.4
Since that discovery, other labs have exploited related cock-
tails that pair a metallocene reductant with an acid to drive
N2RR using a range of metal catalysts, with selectivities and
turnover numbers that continue to improve.5,6,7,8,9
[H(OEt2)2][BArF ]
(HBArF ,
BArF
4
=
tetrakis(3,5-
4
4
bis(trifluoromethyl)phenyl)borate)).16,17 However, contrary to
our mechanistic experiments with HBArF , reaction of
4
B
−
P3 FeN2 with anilinium acids led neither to the observation of
relevant intermediates (e.g., P3 Fe(NNH2)+) in freeze-quench
B
spectroscopic methods, nor to the observation of fixed-N
products upon annealing.9,18,19
The apparent need for both acid and reductant to be present to
achieve productive N–H bond formation is reminiscent of
Schrock and coworkers’ observations when attempting to
functionalize [HIPTN3N]Mo–N2 with catalytically relevant
reagents.20 In both cases, we have hypothesized that metallo-
cene-mediated proton-coupled electron transfer reactions may
play a key role in N–H bond-forming steps.7,9,21 Furthermore,
given the ubiquity of these metallocene reagents in N2RR, we
wondered whether metallocene-mediated N–H bond forming
steps might provide a contributing, or even dominant, mecha-
nistic pathway.
The protonation chemistry of metallocenes is well studied,
especially among Group 810,11 and 1012,13 metallocenes. Relat-
ed studies on more reducing Group 6 and 9 metallocenes (e.g.,
Cp*2Cr, Cp2Co, Cp*2Co), which are relevant to the aforemen-
tioned proton-coupled reduction of N2, have been much more
limited. While studies have shown that the release of H2 is
highly favorable on both thermodynamic and kinetic
grounds,14 protonated Group 6 and 9 metallocene intermedi-
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Density functional theory (DFT) studies by our group support-
Page 2 of 9
2.1 Pulse Electron Paramagnetic Resonance Spectros-
copy on Protonated Cp*2Co. To interrogate the reaction of
Cp*2Co with HOTf, we employed Q-band pulse EPR experi-
ments at very low temperatures. Electron spin-echo (ESE)
detected, field-swept spectra at Q-band, performed at 6 K and
10 K, clearly identify the presence of two different species
with dramatically different g-anisotropy in the precipitated
solid (Figure 2). Fortuitously, measurement of the approxi-
mate spin-lattice relaxation rates via inversion recovery (see
SI) reveals that the two species have significantly different T1’
times. The species with higher g-anisotropy (g = [2.625, 2.349,
1.984]) exhibits a much shorter T1’ than the species exhibiting
a narrower spectrum (g = [2.170, 2.085, 2.005]), even at 6 K.
This difference in relaxation rates becomes more dramatic
upon warming the sample to 10 K; at this temperature, T1’ for
the species with high g-anisotropy is short enough to greatly
diminish its electron-nuclear double resonance (ENDOR) re-
sponse relative to the other species, even at magnetic fields
with significant spectral overlap. Thus, the signals arising
from these two species in pulse EPR experiments can be large-
ly isolated by recording spectra at these two different tempera-
tures (6 K and 10 K; Figure 2).
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ed the notion that protonation of metallocenes such as Cp2*Co
or Cp2*Cr by catalytically relevant acids is thermodynamically
favorable. To our surprise, these DFT studies also predicted
that ring protonation is thermodyamically favored versus pro-
tonation at the metal (to form a hydride).8 Such selectivity
would contrast with the classic case of ferrocene, where proto-
nation at iron has been firmly established.10,22 The Cp2*Co and
Cp*2Cr ring-protonated species are predicted to have remarka-
bly weak C–H bond dissociation enthalpies (BDE <37 kcal
9
1
mol− ), which should in turn make them excellent PCET do-
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nors.7,9 These observations intimate that protonated metallo-
cene intermediates might thereby offer viable pathways for N–
H bond formation via PCET (or even hydride transfer; vide
infra), in addition to the more commonly presumed pathway
for deleterious H2 evolution (Figure 1).
Figure 1: Reaction pathways to consider for protonated Cp*2Co species,
illustrating both undesired HER and possible N–H bond forming steps
relevant to N2RR.
Figure 2: Pseudomodulated23 Q-band ESE-detected EPR spectra of the
reaction of Cp*2Co with HOTf (black traces), and DOTf (blue traces)
measured at 10 K (top traces) and 6 K (bottom traces). See SI for acquisi-
tion parameters. Simulations for each species are displayed in red (See SI
for simulation details). The sharp signals with asterisks above them are
due to a background signal arising from a component of the EPR cavity
(See SI for more detail).
We previously reported preliminary investigations into the
protonation of Cp*2Co. In brief, slow addition of a toluene
solution of Cp*2Co to a vigorously stirred suspension of tri-
fluoromethanesulfonic acid (HOTf) in toluene at −78 °C led to
precipitation of a purple solid that could be isolated via filtra-
tion. On the basis of the X-band continuous wave (CW) elec-
tron paramagnetic resonance (EPR) spectrum (77 K, Figure 4)
of the solid, we speculated that it was a protonated Cp*2Co
species.8 Herein, we undertake the rigorous characterization of
the protonation products of Cp*2Co using pulse EPR tech-
niques, and provide unequivocal evidence for the assignment
of the ring protonated isomers Cp*(exo/endo-η4-C5Me5H)Co+.
Variable temperature Q-Band (34 GHz) pulse EPR spectros-
copy, in conjunction with DFT predictions, are key to enabling
the assignment. We also demonstrate that exo-protonation can
be favored when using a bulkier acid. Of further interest, we
provide physical data to experimentally assess the C−H bond
For the narrower, more slowly relaxing species, a comparison
of the Q-band ESE-detected EPR spectra from the reaction of
Cp*2Co with HOTf and DOTf shows a clear change, from 16
resolved splittings centered at 1270 mT, to the 8 lines ex-
pected for a large hyperfine coupling to an I = 7/2 59Co nucle-
us (A(59Co)10 K = [15, 15, 225] MHz). This observation indi-
cates that, at least at the orientation corresponding to g3, there
1
is a single H nucleus with a hyperfine coupling of approxi-
mately ½ of the magnitude of the 59Co hyperfine coupling.
1
Analysis of the field-dependent H ENDOR (Figure 3a-b) at
2
10 K, with corroboration from H hyperfine sub-level correla-
tion (HYSCORE) spectra (see SI) of each respective species,
allows determination of the full hyperfine tensor of this acid-
derived proton: A(1H)10 K = [106.5, 112.5, 108.2] MHz, with
aiso = 109.1 MHz. Comparing this value to that known for the
hydrogen atom (1420 MHz) indicates that approximately 0.08
e− are localized on this proton.24 The amount of spin density
localized on this proton is unusually large, even when com-
pared with highly reactive, paramagnetic transition metal hy-
drides.25
dissociation free energy (BDFEC−H
)
for Cp*(exo-η4-
C5Me5H)Co+, which support our earlier DFT predictions that it
has an exceptionally weak C–H bond (Figure 1). This behavior
should not be limited to the present protonated metallocene,
and we thus outline a general approach to understanding the
reactivity of arene-protonated metal species.
Characterization of the species with greater g-anisotropy was
targeted by performing analogous experiments at 6 K. In this
2. RESULTS
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nents (T(1H)10 K = [−2.6, 3.4, −0.9] MHz; T(1H)6 K = [1.2, −2.8,
1.7] MHz). To evaluate possible chemical assignments for
these observations, DFT calculations were performed to opti-
mize the structure of the three plausible protonation isomers
(i.e., Co–H, exo-C–H, and endo-C–H) and then single point
calculations were performed to predict the relevant hyperfine
tensors (Figure 5a).27 Consistent with previous experimental
observations for paramagnetic transition metal hydrides, DFT
predicts the Co–H isomer to have a large, roughly axial dipo-
lar coupling tensor (T(1H)Co–H = [34.1, −20.7, −12.9]).28,29 Fur-
thermore, the predicted aiso value for the Co–H of −50 MHz is
inconsistent with our experimental EPR data for the protonat-
ed species. In contrast, the hyperfine coupling tensor for both
exo- and endo-isomers are predicted to be far more isotropic
(T(1H)exo-C−H = [−2.4, 3.8, −1.4] and T(1H)endo-C−H = [−3.1, 8.7,
−5.6]), consistent with the EPR data available. Importantly,
our DFT calculations also predict that the two ring-protonated
isomers have very different aiso values, with the exo-isomer
predicted to have aiso = 119 MHz and the endo-isomer predict-
ed to have aiso = 31 MHz. Thus, we assign the species with
small g-anisotropy to be the exo-isomer and that with large g-
anisotropy to be the endo-isomer.
case, the Q-band ESE-detected EPR spectra for this species in
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samples generated with HOTf and DOTf are indistinguishable,
1
indicating that the H hyperfine coupling to the acid-derived
proton is small in comparison to the 59Co hyperfine and the
inhomogeneous line broadening. This was confirmed via field-
dependent ENDOR (Figure 3c-d) and HYSCORE (see SI)
spectra acquired at 6 K, which reveal a single acid-derived
proton coupling of A(1H)6 K = [19.0, 15.0, 19.5] MHz, aiso
=
17.8 MHz.
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Assuming this assignment is correct then, on the basis of the
recorded CW EPR spectra, the endo-isomer is formed in high-
er yield with HOTf (Figure 4, top). We wondered whether it
might be possible to achieve preferential exo-functionalization
by using a bulkier acid. Indeed, we have found that slow addi-
tion of a toluene solution of Cp*2Co at −78 °C to a rapidly
stirred suspension of the more sterically encumbered
bis(trifluoromethane)sulfonimide (HNTf2) in toluene also pre-
cipitates a purple solid (Figure 4, bottom). Analysis of this
solid by CW X-Band EPR at 77 K reveals a near complete
Figure 3: a) Q-band Davies ENDOR spectra at 10 K and b) narrow Q-
band Davies ENDOR spectra at 10 K. c) Q-band Davies ENDOR spectra
at 6 K and d) narrow Q-band Davies ENDOR spectra at 6 K. Data from
the reaction with HOTf (black) and DOTf (blue) are shown. A simulation
(red) is given and in the spectra at 6 K the simulation is further decom-
posed into the components for the 1H simulation (green) and the 59Co
simulation (light blue). See SI for full acquisition parameters and simula-
tion details.
Additionally, features from 59Co (A(59Co)6 K = [245, 160, 187]
MHz) are observable in the ENDOR spectra at all fields,
which is likely due to the more isotropic nature of the coupling
symmetry of this species in comparison to the species with
smaller g-anisotropy. In the ENDOR acquired at 1230 mT,
additional splittings due to the 59Co nuclear quadrupole inter-
action are resolved. Simulations of these ENDOR spectra in-
dicate a quadrupole coupling constant of e2qQ/h = 170 MHz,
with negligible electric field gradient rhombicity (η). These
values are very similar to those reported for Cp2Co+ (e2qQ/h =
171.5 MHz and η = 0), as determined by nuclear quadrupole
resonance. This suggests that protonation results in only a
relatively minor perturbation of the environment around Co.26
Figure 4: (top) X-Band CW EPR spectrum of the reaction of Cp*2Co with
HOTf (black) and its simulation (red). (bottom) X-Band CW EPR spec-
trum of the reaction of Cp*2Co with HNTf2 (black) and its simulation
(red). The simulations are generated using the same parameters (see SI)
except for the weighting of the two species. For the top simulation it is
10:1 endo:exo and in the bottom simulation it is 3:10 endo:exo.
2.2 Stereochemical Assignment of Cp*2Co Protonation.
Notably, both of the proton hyperfine coupling tensors are
highly isotropic in nature, with only small anisotropic compo-
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Figure 5: a) DFT optimized structures for the protonated form of Cp*2Co. The predicted A(1H) values are for the proton circled in red. b) X-ray crystal
1
structure of Cp*(exo-η4-C5Me5H)Co. Thermal ellipsoids are shown at 50% probability. c) Experimentally derived H hyperfine parameters for the endo- and
exo-isomers of protonated Cp*2Co.
Scheme 1. Proposed Mechanism for the Oxidation of
Cp*(exo-η4-C5Me5D)Co with HBArF
4
inversion of the protonation-site selectivity. Both of the proto-
nation reactions are under kinetic control due to the rapid pre-
cipitation upon proton transfer. With the smaller HOTf, endo-
protonation is preferred (Figure 5a), but with the bulkier
HNTf2, steric clash with the opposite Cp* ring leads to exo-
protonation being favored (Figure 5b).
Further chemical confirmation of the protonation site was ob-
tained by pre-functionalization of the Cp* ring. Taking a cue
from classic literature, we noted that Wilkinson et al. previ-
ously characterized
a far more stable, neutral ring-
functionalized species, Cp(η4-C5H6)Co.30 By analogy to their
approach, we generated Cp*(exo-η4-C5Me5H)Co in moderate
yield via the reaction of Cp*2Co+ with excess tetrabu-
tylammonium borohydride in refluxing THF. The stereospeci-
ficity of exo-functionalization could be confirmed in the solid
state by XRD analysis (Figure 5b) and in solution via NMR
spectroscopy.
Although our efforts to use common oxidants (i.e., Fc+, Ag+)
to affect the electron transfer were unsuccessful, we found that
Cp*(exo-η4-C5Me5H)Co could be oxidized by reaction with
turned to the neutral species Cp*(exo-η4-C5Me5H)Co as a
means to indirectly measure pertinent thermochemical proper-
ties for Cp*(exo-η4-C5Me5H)Co+.
HBArF at −78 °C in pentane. The purple precipitate was ana-
4
lyzed by X-Band CW EPR and, as expected, demonstrated
only the signal that we had assigned to the exo-isomer. To
confirm that the strongly coupled proton observed derived
from our pre-functionalized ring and not the acid, Cp*(exo-η4-
One important parameter in this regard is the Cp*(exo-η4-
C5Me5H)Co+/0 redox couple. In cyclic voltammograms (CVs)
of Cp*(exo-η4-C5Me5H)Co, obtained at typical scan rates (0.01
to 1.0 V s−1) at room temperature in butyronitrile,31 only an
irreversible oxidation is observed. Continuing to scan these
voltammograms further in the cathodic direction leads to the
observation of the fully reversible Cp*2Co+/0 couple (Figure 6,
top), consistent with the loss of 0.5 equivalents of H2, as ex-
pected from Cp*(exo-η4-C5Me5H)Co+ in solution. By scanning
rapidly (>10 V s−1) at room temperature (Figure 6, bottom), or
alternatively by cooling the reaction mixture to −78 °C (see
SI), voltammograms with appreciable reversibility could be
C5Me5D)Co was reacted with HBArF . Only the formation of
4
Cp*(exo-η4-C5Me5D)Co+ was detected by EPR (Scheme 1, see
SI).
2.3 Thermochemical Measurements. We were also interest-
ed in experimentally validating the DFT-predicted thermo-
chemical properties of these species. The high kinetic instabil-
ity of Cp*(exo/endo-η4-C5Me5H)Co+ in solution precludes
direct measurement of the thermochemical properties that we
have predicted by DFT. Of particular interest is experimental
validation of a remarkably weak BDFEC-H. We therefore
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Cp*(exo-η4-C5Me5H)Co and Cp*2Co (53 and 62 kcal mol−1,
obtained, from which E0 could be determined to be −0.62 V vs
Fc+/0 (Figure 7).
respectively).
1
Cp*(exo-η4-C5Me5H)Co + 4MeOTEMPO• →
2
3
4
5
Cp*2Co + 4MeOTEMPO–H
Cp*2Co + 4MeOTEMPO• →
Cp*(η4-C5Me4CH2)Co + 4MeOTEMPO–H
(1)
(2)
6
With this thermochemical data for Cp*(exo-η4-C5Me5H)Co in
hand, it is possible to constrain the BDFEC−H for Cp*(exo-η4-
C5Me5H)Co+. Using the bound established for the BDFEC−H
for neutral Cp*(exo-η4-C5Me5H)Co, we can establish an upper
limit for the BDFEC–H of Cp*(exo-η4-C5Me5H)Co+ of 34 kcal
mol−1. But using the upper limit determined for the ΔG(H−) of
Cp*(exo-η4-C5Me5H)Co allows us to place an even lower up-
per limit for BDFE(Cp*(exo-η4-C5Me5H)Co+) of <29 kcal
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1
mol– . This experimental upper limit predicted from the solu-
tion phase data is in reasonable agreement with our gas-phase
DFT prediction of 23 kcal mol−1.36 The C–H bond of Cp*(exo-
η4-C5Me5H)Co+ is extremely weak.
Figure 6: Cyclic voltammograms of the Cp*(exo-η4-C5Me5H)Co+/0 couple
at room temperature in a 0.4 M [TBA][PF6] solution of butyronitrile. (top)
Scan showing that the oxidation of Cp*(exo-η4-C5Me5H)Co0 leads to the
emergence of the Cp*2Co+/0 couple. (bottom) Variable scan rate measure-
ments on the Cp*(exo-η4-C5Me5H)Co+/0 feature.
To further confirm this value, the methylated derivative,
Cp*(η4-C5Me6)Co, was prepared.13 The oxidation event for
this species is reversible.32 This result is consistent with the
significantly higher kinetic barrier anticipated for Me•
loss/transfer compared to H• loss/transfer. In acetonitrile, the
E0 we measure for Cp*(η4-C5Me6)Co+/0 is −0.61 V vs Fc+/0, in
good agreement with our experimental data for the Cp*(exo-
η4-C5Me5H)Co+/0 couple.
Figure 7: Thermochemistry of neutral and cationic Cp*(exo-η4-
An estimate of the hydricity (ΔG(H−)) of Cp*(exo-η4-
C5Me5H)Co provides another useful parameter. Dissolution of
Cp*(exo-η4-C5Me5H)Co in MeCN-d3 and reaction with 1 atm
C5Me5H)Co. Computational values are shown in parentheses. Thermody-
namic quantities are in kcal mol–1 and potentials are against Fc+/0
.
3. DISCUSSION
of CO2 or with excess [Pt(dmpe)2]2+ (dmpe
= 1,2-
It is well established that group 8 metallocenes form metal
hydrides upon protonation.10,11,22 In the case of ferrocene,
computational trajectories have been used to argue that there is
fast exchange between a terminal hydride and a hydride that
forms an agostic interaction with the Cp ring.37,38 In contrast,
neutral group 10 metallocenes (Cp2Ni and Cp*2Ni), and the
isoelectronic Cp2Co−, are known to undergo exo-
protonation.12,13,39 Here we find that, consistent with the near
isoenergetic energies predicted by DFT, Cp*2Co undergoes
both exo- and endo-protonation on the ring. This result pro-
vides a distinct example of a metallocene that undergoes non-
specific protonation. Furthermore, the protonation selectivity
can be altered by changing the steric profile of the acid.
dimethylphosphinoethane), leads in both cases to quantitative
hydride transfer. From this observation we can determine a
lower bound for the hydricity of Cp*(exo-η4-C5Me5H)Co
(ΔG(H−) <41 kcal mol−1; Figure 7).33 This is in good agree-
1
ment with our DFT prediction of ∆G(H−) = 37 kcal mol− for
this species. The C–H bond of Cp*(exo-η4-C5Me5H)Co is thus
about 15 kcal mol−1 more hydridic than the C–H bonds in the
common biological hydride donors NADH and NADPH.34
These observations hint at the possibility that, at least in prin-
ciple, species such as Cp*(exo-η4-C5Me5H)Co could mediate
hydride transfer steps relevant to N2RR, such as that shown in
Figure 1.
In an attempt to estimate the homolytic C−H bond strength
We suspect that formation of the exo-isomer is likely critical
(BDFE) of Cp*(exo-η4-C5Me5H)Co, it was reacted with excess
to observing productive PCET reactions in N2RR mediated by
4-
B
4-methoxy-2,2,6,6-tetramethyl-1-piperidinyloxy
(
the P3 Fe-system, as this isomer provides significantly less
4-
MeOTEMPO⦁). To our surprise, two equivalents of
steric shielding for the reactive H•. Given the steric profile of
the catalytically relevant acids that we and others have used
(e.g., anilinium and pyridinium),4,5,6,7,8,9 we expect that exo-
protonation is far more likely under N2RR conditions. Indeed,
we have calculated only small barriers (∆G‡ <5 kcal mol−1) for
the exo-protonation of Cp*2Co by substituted anilinium triflate
acids.9 Facile endo-protonation by these acids is inconsistent
with simple space-filling models.
MeOTEMPO−H were formed. The first equivalent derives from
the expected H-atom abstraction to form Cp*2Co, providing an
upper limit to the BDFEexo-C–H: <65 kcal mol−1 (eq 1, Figure
7).24 The second 4-MeOTEMPO−H equiv is derived from a sec-
ond H-atom abstraction step between 4-MeOTEMPO⦁ and
Cp*2Co (eq 2). This generates the known fulvene species,
Cp*(η4-C5Me4CH2)Co.35 These observations are consistent
with our BDFEC–H predictions for the C–H bond in both
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Although Cp* is most typically considered to be an innocent
ligand, evidence continues to emerge that it can be involved in
the management of protons. In addition to the well-established
protonation of Cp*2Ni,13,40 several half-sandwich Rh complex-
es have recently been reported to form Cp*–H linkages fol-
lowing reductive elimination of a Rh–H. 41,42,43 In these cases,
the Cp*–H bond has been directly implicated in H– transfer,
either to H+ or to NAD+.
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The present study illustrates that Cp*–H linkages are not lim-
ited to H– transfer pathways. Rather, the type of reactivity can
be predicted by the tendency of the metal center to achieve a
closed-shell, 18e− d6 configuration. Thus, the d7 Co center in
Cp*(exo-η4-C5Me5H)Co+ should favor a one electron process
(H• transfer), while the d8 Co center in Cp*(exo-η4-
C5Me5H)Co should favor a two electron process (H− transfer),
akin to those observed for the aforementioned d8 Rh centers.
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In this work, we have derived a BDFE for three different C–H
bonds relevant to decamethylcobaltocene (Cp*(exo-η4-
C5Me5H)Co+,
Cp*(exo-η4-C5Me5H)Co,
and
Cp*(η5-
C5Me4CH2H)Co) (Figure 8). All of these bonds are weak, but
that in Cp*(exo-η4-C5Me5H)Co+ is significantly weaker than
the other two. This can be readily explained in terms of the
two primary factors affecting the stability of the starting and
product complexes: aromaticity and electron count. In the case
of H-atom abstraction from Cp*(exo-η4-C5Me5H)Co or from a
methyl substituent in Cp*2Co, these factors offset one another
to provide a weak, but not an exceptionally weak, C–H BDFE.
For Cp*(exo-η4-C5Me5H)Co, H-atom abstraction aromatizes
the Cp* ring, offset by the formation of a 19e− center. On the
other hand, in Cp*2Co, H-atom abstraction transforms the 19e−
center to an 18e− center, but the Cp* ring is dearomatized.
Only in the case of Cp*(exo-η4-C5Me5H)Co+ are both stabiliz-
ing factors driving formation of the product. H-atom abstrac-
tion affords aromatic, 18e− Cp*2Co+, and correspondingly the
C–H bond is remarkably weak (BDFE <29 kcal mol−1).
Reagents with such weak X−H bonds have been sought due to
their utility in organic synthesis for the stepwise reduction of
unsaturated substrates, such as olefins, ketones, aldehydes,
esters, and enamines via H• transfer.44,45 Traditional strategies
for developing such reagents have focused on reactive metal
hydrides, for which the M• product of an overall hydrogen
atom transfer is stabilized by dimerization via M–M bond
formation, and/or the formation of bridging carbonyl prod-
ucts.46 Another strategy has involved the coordination of sub-
strates that contain otherwise strong X–H bonds to a highly
reducing, but nonetheless oxophilic/azaphilic, metal centers,
resulting in remarkable weakening of the X–H bond.47 One
system where this phenomenon has proven particularly effec-
tive for engendering synthetically useful PCET reactions is
SmI2-H2O, in which coordination of H2O to SmII has been
estimated to result in an O–H bond weakening of almost 100
kcal mol–1.48,49,50,51
The present study presents the protonation of Cp*2Co to form
Cp*(η5-C5Me5H)Co+ as a distinct and promising strategy for
developing extremely strong PCET donors. In general, this
strategy involves coupling a d7 (or d4) metal ion to a dearoma-
tized arene ligand. Given the prevalence of sandwich and half-
sandwich complexes in organometallic chemistry, it is likely
that as yet unrecognized examples of such PCET reagents
already exist, or are readily accessible.
Cp*(exo-η4-C5Me5H)Ni2+ provides one such example. Electro-
chemical oxidation of the stable Cp*(exo-η4-C5Me5H)Ni+ to
Cp*(exo-η4-C5Me5H)Ni2+ leads to rapid generation of
Figure 8: (top) A comparison of the experimental BDFEC–H for a variety
of related Cp*Co-species, demonstrating the importance of aromaticity
and electron count in predicting the stability of the indicated C–H bond.
(bottom) A comparison of computational BDFEC values for a redox
–
H
series of [Cp*(exo-η4-C5Me5H)Ni]n+.
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Cp*2Ni2+ on the CV time scale. This transformation was origi-
Paul H. Oyala: 0000-0002-8761-4667
Jonas C. Peters: 0000-0002-6610-4414
Notes
nally proposed to occur via H+ loss followed by e− loss.52 Al-
ternatively, we suspect that, in analogy to Cp*(exo-η4-
C5Me5H)Co+, this transformation may occur via rapid H• loss.
In contrast, electrochemical reduction of the cation Cp*(exo-
η4-C5Me5H)Ni+ to Cp*(exo-η4-C5Me5H)Ni is fully reversible
on the CV time scale.52
1
2
3
4
5
6
7
8
The authors declare no competing financial interest.
Author Contributions
The manuscript was written through contributions of all authors.
All authors have given approval to the final version of the manu-
script.
These results emphasize that the electron count of the metal
center, instead of its reducing power, can be a good predictor
of the reactivity. Indeed, our DFT calculations and the relative
experimental stability of Cp*(exo-η4-C5Me5H)Ni and
Cp*(exo-η4-C5Me5H)Ni+ suggest that even though H• loss
involves formal oxidation of the metal center the d9 NiI and d8
NiII species are less prone to PCET reactivity. However, upon
oxidation to the d7 NiIII species the C–H bond is weakened by
9
ACKNOWLEDGMENTS
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This work was supported by Department of Energy (DOE-
0235032). MJC acknowledges support from the Center for
Environmental Microbial Interactions (CEMI) and the Resnick
Sustainability Institute at Caltech. The Caltech EPR facility
was supported by the National Science Foundation (NSF MRI-
153194) and the Dow Next Generation Educator Fund.
1
approximately 20 kcal mol− . This weakening is due to the
high stability of the 18e−, d6 Cp*2Ni2+ product resulting from
net hydrogen atom transfer.
4. CONCLUSION
We have demonstrated using pulse EPR spectroscopy, sup-
ported by DFT calculations, that for Cp*2Co the Cp* ring is
the site of protonation. Both ring-protonated isomers (endo
and exo) can be formed and observed, with the selectivity be-
ing determined by the bulk of the acid. For the exo-species, we
were able to use the one-electron reduced, neutral congener,
Cp*(exo-η4-C5Me5H)Co, to verify our DFT prediction that the
protonated species, Cp*(exo-η4-C5Me5H)Co+, has a remarka-
REFERENCES
1
Wilkinson, G.; Rosenblum, M.; Whiting, M. C.; Woodward, R. B. The
structure of iron bis-cyclopentadienyl. J. Am. Chem. Soc. 1952, 74, 2125-
2126.
2
Ferrocenes; Štěpnička, P., Ed.; John Wiley and Sons, Ltd: Chichester,
England, 2008; pp 641.
3
Geiger, W. E. Organometallic electrochemistry:ꢀ origins, development,
1
bly weak C−H bond (<29 kcal mol− ). This is consistent with
and future. Organometallics 2007, 26, 5738-5765.
4
the suggestion that it may serve as a PCET donor in catalytic
N2RR in which it is generated in situ.
Yandulov, D. V.; Schrock, R. R. Catalytic reduction of dinitrogen to
ammonia at a single molybdenum center. Science 2003, 301, 76-78.
5
The facile protonation of Cp*2Co to generate Cp*(exo-η4-
C5Me5H)Co+ points to a more general strategy for developing
conceptually related, strong PCET donors. Such strategies
would complement current approaches for the development of
PCET reagents, which rely on creating weak M–H bonds or
coordination-induced weakening of O–H or N–H bonds.
We have also shown that Cp*(exo-η4-C5Me5H)Co+ can be
converted from a PCET donor to a strong hydride donor by
one electron reduction, as demonstrated by the capacity of
Cp*(exo-η4-C5Me5H)Co to convert CO2 to formate. This ob-
servation highlights the dual potential for metallocenes to me-
diate both hydride transfer and PCET steps during the proton-
coupled reduction of small molecule substrates (Figure 1).
Both types of reactivity differ from the canonical role associ-
ated with metallocenes as electron transfer reagents.
Arashiba, K.; Miyake, Y.; Nishibayashi, Y. A molybdenum complex
bearing PNP-type pincer ligands leads to the catalytic reduction of dini-
trogen into ammonia. Nat. Chem. 2010, 3, 120-125.
6
Hill, P. J.; Doyle, L. R.; Crawford, A. D.; Myers, W. K.; Ashley, A. E.
Selective catalytic reduction of N2 to N2H4 by a simple Fe complex. J. Am.
Chem. Soc. 2016, 138, 13521-13524.
7
Arashiba, K.; Eizawa, A.; Tanaka, H.; Nakajima, K.; Yoshizawa, K.;
Nishibayashi, Y. Catalytic nitrogen fixation via direct cleavage of nitro-
gen-nitrogen triple bond of molecular dinitrogen under ambient reaction
conditions. Bull. Chem. Soc. Jap. 2017, 90, 1111-1118.
8
Chalkley, M. J.; Del Castillo, T. J.; Matson, B. D.; Roddy, J. P.; Peters,
J. C. Catalytic N2-to-NH3 conversion by Fe at lower driving force: a pro-
posed role for metallocene-mediated PCET. ACS Cent. Sci. 2017, 3, 217-
223.
9
Chalkley, M. J.; Del Castillo, T. J.; Matson, B. D.; Peters, J. C. Fe-
mediated nitrogen fixation with a metallocene mediator: exploring pKa
effects and demonstrating electrocatalysis. J. Am. Chem. Soc. 2018, 140,
6122-6129.
10
Curphey, T. J.; Santer, J. O.; Rosenblum, M.; Richards, J. H. Protona-
ASSOCIATED CONTENT
tion of metallocenes by strong acids. Structure of the cation. J. Am. Chem.
Soc. 1960, 82, 5249-5250.
Supporting Information
11
Liles, D. C.; Shaver, A.; Singleton, E.; Wiege, M. B. New high yield
The Supporting Information is available free of charge on the
ACS Publications website at DOI: xxxxxx.
syntheses of ruthenocene and osmocene and their decamethyl derivatives.
The crystal structure of [Ru(η5-C5Me5)2]. J. Organomet. Chem. 1985, 288,
c33-c36.
Computational models (MOL)
X-ray data (CIF)
12 Court, T. L.; Werner, H. Studies on the reactivity of metal π-complexes:
X. Concerning the mechanism of formation of the cationic triple decker
sandwich complex [Ni2(C5H5)3]+, and the isolation of [NiC5H5]BF4. J.
Organomet. Chem. 1974, 65, 245-251.
Experimental procedures and compound characterization data
(PDF)
13
Koelle, U.; Khouzami, F. Permethylated electron-excess metallocenes.
AUTHOR INFORMATION
Corresponding Author
*phoyala@caltech.edu
Angew. Chem. Int. Ed. 1980, 19, 640-641.
14
Koelle, U.; Infelta, P. P.; Graetzel, M. Kinetics and mechanism of the
reduction of protons to hydrogen by cobaltocene. Inorg. Chem. 1988, 27,
879-883.
*jpeters@caltech.edu
15
Kuriyama, S.; Arashiba, K.; Nakajima, K.; Tanaka, H.; Kamaru, N.;
ORCID
Yoshizawa, K.; Nishibayashi, Y. Catalytic formation of ammonia from
Matthew J. Chalkley: 0000-0002-0484-7335
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Page 8 of 9
1
2
3
4
5
6
7
8
9
36
molecular dinitrogen by use of dinitrogen-bridged dimolybdenum–
Gas-phase BDFE values are consistently lower than those of solution
species. However, complications arising from differential hydrogen bond-
ing behavior precludes simple application of a correction factor that would
better correlate the gas phase DFT-predicted value with the solution phase
values inferred from experimental data.
dinitrogen complexes bearing PNP-pincer Ligands: remarkable effect of
substituent at PNP-pincer ligand. J. Am. Chem. Soc. 2014, 136, 9719-
9731.
16 Anderson, J. S.; Rittle, J.; Peters, J. C. Catalytic conversion of nitrogen
37
to ammonia by an iron model complex. Nature 2013, 501, 84-87.
Bühl, M.; Grigoleit, S. Molecular dynamics of neutral and protonated
17
Del Castillo, T. J.; Thompson, N. B.; Peters, J. C. A synthetic single-
ferrocene. Organometallics 2005, 24, 1516-1527.
site Fe nitrogenase: high turnover, freeze-quench 57Fe Mössbauer data,
38
Sharma, N.; Ajay, J. K.; Venkatasubbaiah, K.; Lourderaj, U. Mecha-
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
37
38
39
40
41
42
43
44
45
46
47
48
49
50
51
52
53
54
55
56
57
58
59
60
and a hydride resting state. J. Am. Chem. Soc. 2016, 138, 5341-5350.
nisms and dynamics of protonation and lithiation of ferrocene. Phys.
Chem. Chem. Phys. 2015, 17, 22204-22209.
18 Anderson, J. S.; Cutsail, G. E. III; Rittle, J.; Connor, B. A.; Gunderson,
W. A.; Zhang, L.; Hoffman, B. M.; Peters, J. C. Characterization of an
Fe≡N–NH2 intermediate relevant to catalytic N2 reduction to NH3. J. Am.
Chem. Soc. 2015, 137, 7803-7809.
39 Geiger, W. E.; Bowden, W. L.; El Murr, N. An electrochemical study of
the protonation site of the cobaltocene anion and of cyclopentadienylco-
balt(I) dicarbollides. Inorg. Chem. 1979, 18, 2358-2361.
19
40 Werner, H.; Dernberger, T. Untersuchungen zur Reaktivität von Metall-
π-Komplexen: XXXIII. Synthese und Reaktivität von Decamethyl- und
Pentamethylnickellocen. J. Organomet. Chem. 1980, 198, 97-103.
Thompson, N. B.; Green, M. T.; Peters, J. C. Nitrogen fixation via a
terminal Fe(IV) nitride. J. Am. Chem. Soc. 2017, 139, 15312-15315.
20
Yandulov, D. V.; Schrock, R. R. Studies relevant to catalytic reduction
41
of dinitrogen to ammonia by molybdenum triamidoamine complexes.
Pitman, C. L.; Finster, O. N. L.; Miller, A. J. M. Cyclopentadiene-
Inorg. Chem. 2005, 44, 1103-1117.
mediated hydride transfer from rhodium complexes. Chem. Commun.
2016, 52, 9105-9108.
21
Wickramasinghe, L. A.; Schrock, R. R.; Tsay, C.; Müller, P. Molyb-
42
denum complexes that contain a calix[6]azacryptand ligand as catalysts
Quintana, L. M. A.; Johnson, S. I.; Corona, S. L.; Villatoro, W.; God-
for reduction of N2 to ammonia. Inorg. Chem. 2018, 57, 15566-15574.
dard, W. A.; Takase, M. K.; VanderVelde, D. G.; Winkler, J. R.; Gray, H.
B.; Blakemore, J. D. Proton–hydride tautomerism in hydrogen evolution
catalysis. Proc. Natl. Acad. Sci. U. S. A. 2016, 113, 6409-6414.
22
Malischewski, M.; Seppelt, K.; Sutter, J.; Heinemann, F. W.; Dittrich,
B.; Meyer, K. Protonation of ferrocene: a low-temperature X-ray diffrac-
tion study of [Cp2FeH](PF6) reveals an iron-bound hydrido ligand. Angew.
Chem. Int. Ed. 2017, 56, 13372-13376.
43
Johnson, S. I.; Gray, H. B.; Blakemore, J. D.; Goddard, W. A. Role of
ligand protonation in dihydrogen evolution from a pentamethylcyclopen-
23 Hyde, J. S.; Pasenkiewicz-Gierula, M.; Jesmanowicz, A.; Antholine, W.
E. Pseudo field modulation in EPR spectroscopy. Appl. Magn. Reson.
1990, 1, 483-496.
tadienyl rhodium catalyst. Inorg. Chem. 2017, 56, 11375-11386.
44
Crossley, S. W. M.; Obradors, C.; Martinez, R. M.; Shenvi, R. A. Mn-,
Fe-, and Co-catalyzed radical hydrofunctionalizations of olefins. Chem.
Rev. 2016, 116, 8912-9000.
24 Wittke, J. P.; Dicke, R. H. Redetermination of the hyperfine splitting in
the ground state of atomic hydrogen. Phys. Rev. 1956, 103, 620-631.
45
Gentry, E. C.; Knowles, R. R. Synthetic applications of proton-coupled
25
Hu, Y.; Shaw, A. P.; Estes, D. P.; Norton, J. R. Transition-metal hy-
electron transfer. Acc. Chem. Res. 2016, 49, 1546-1556.
dride radical cations. Chem. Rev. 2016, 116, 8427-8462.
46
Hartung, J.; Norton, J. R. Catalysis involving the H• transfer reactions
26
Brown, T. L. Cobalt-59 nuclear quadrupole resonance spectroscopy.
of first-row transition metals. In Catalysis without Precious Metals; Bull-
ock, R. M., Ed.; Wiley: 2010, p 1-21.
Acc. Chem. Res. 1974, 7, 408-415.
27
47 Cuerva, J. M.; Campaña, A. G.; Justicia, J.; Rosales, A.; Oller-López, J.
L.; Robles, R.; Cárdenas, D. J.; Buñuel, E.; Oltra, J. E. Water: the ideal
hydrogen-atom source in free-radical chemistry mediated by TiIII and
other single-electron-transfer metals? Angew. Chem. Int. Ed. 2006, 45,
5522-5526.
Different functionals (TPSS, TPSSH, BP86, B3LYP) were used for
both the optimization and also the single point calculation to determine the
hyperfine coupling. In all cases, similar T-tensors and the highly disparate
magnitude of the aiso for the endo- and exo-functionalized species were
observed (See SI for full details).
28 Harmer, J.; Finazzo, C.; Piskorski, R.; Ebner, S.; Duin, E. C.; Goenrich,
M.; Thauer, R. K.; Reiher, M.; Schweiger, A.; Hinderberger, D.; Jaun, B.
A nickel hydride complex in the active site of methyl-coenzyme M reduc-
tase: implications for the catalytic cycle. J. Am. Chem. Soc. 2008, 130,
10907-10920.
48
Chciuk, T. V.; Flowers, R. A. Proton-coupled electron transfer in the
reduction of arenes by SmI2–water complexes. J. Am. Chem. Soc. 2015,
137, 11526-11531.
49
Chciuk, T. V.; Anderson, W. R.; Flowers, R. A. Proton-coupled elec-
tron transfer in the reduction of carbonyls by samarium diiodide–water
complexes. J. Am. Chem. Soc. 2016, 138, 8738-8741.
29
Kinney, R. A.; Saouma, C. T.; Peters, J. C.; Hoffman, B. M. Modeling
the signatures of hydrides in metalloenzymes: ENDOR analysis of a di-
iron Fe(μ-NH)(μ-H)Fe Core. J. Am. Chem. Soc. 2012, 134, 12637-12647.
30 Green, M. L. H.; Pratt, L.; Wilkinson, G. 760. A new type of transition
50
Chciuk, T. V.; Anderson, W. R.; Flowers, R. A. Interplay between
substrate and proton donor coordination in reductions of carbonyls by
SmI2–water through proton-coupled electron-transfer. J. Am. Chem. Soc.
2018, 140, 15342-15352.
metal–cyclopentadiene compound. J. Chem. Soc. 1959, 3753-3767.
31 Potentials in butyronitrile have been shown to be very good estimates of
those in acetonitrile. Butyronitrile also enables low temperature electro-
chemistry to be performed, which is beneficial for this study: Izutsu, K.
Reference electrodes for use in nonaqueous solutions In Handbook of
Reference Electrodes; Inzelt, G., Lewenstam, A., Scholz, F., Eds.; Spring-
er Berlin Heidelberg: Berlin, Heidelberg, 2013, p 145-187.
51
Kolmar, S. S.; Mayer, J. M. SmI2(H2O)n reduction of electron rich
enamines by proton-coupled electron transfer. J. Am. Chem. Soc. 2017,
139, 10687-10692.
52
Koelle, U.; Khouzami, F.; Lueken, H. Permethylmetallocenes, III.
Decamethylnickelocene: the neutral sandwich complex, the monocation,
the dication, and their addition reactions. Chem. Ber. 1982, 115, 1178-
1196.
32
Koelle, U. Electrochemistry of transition metal π-complexes. IV. Oxi-
dation of cyclopentadienyl diolefine and cyclobutadiene cobalt complexes.
Inorg. Chim. Acta 1981, 47, 13-18.
33 Wiedner, E. S.; Chambers, M. B.; Pitman, C. L.; Bullock, R. M.; Miller,
A. J. M.; Appel, A. M. Thermodynamic hydricity of transition metal hy-
drides. Chem. Rev. 2016, 116, 8655-8692.
34 Ilic, S.; Alherz, A.; Musgrave, C. B.; Glusac, K. D. Thermodynamic and
kinetic hydricities of metal-free hydrides. Chem. Soc. Rev. 2018, 47, 2809-
2836.
35 Ohki, Y.; Murata, A.; Imada, M.; Tatsumi, K. C−H bond activation of
decamethylcobaltocene mediated by a nitrogenase Fe8S7 P-cluster model.
Inorg. Chem. 2009, 48, 4271-4273.
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