Synthesis and structure of six-coordinate iron borohydride complexes supported by PNP ligands

Article abstract of DOI:10.1021/ic402762v

The preparation of a number of iron complexes supported by ligands of the type HN{CH₂CH₂(PR₂)}₂ [R = isopropyl (ⁱPrPNP) or cyclohexyl (^CyPNP)] is reported. This is the first time this important bifunctional ligand has been coordinated to iron. The iron(II) complexes (ⁱPrPNP)FeCl₂(CO) (1a) and ( ^CyPNP)FeCl₂(CO) (1b) were synthesized through the reaction of the appropriate free ligand and FeCl₂ in the presence of CO. The iron(0) complex (ⁱPrPNP)Fe(CO)₂ (2a) was prepared through the reaction of Fe(CO)₅ with ⁱPrPNP, while irradiating with UV light. Compound 2a is unstable in CH₂Cl₂ and is oxidized to 1a via the intermediate iron(II) complex [(ⁱPrPNP) FeCl(CO)₂]Cl (3a). The reaction of 2a with HCl generated the related complex [(ⁱPrPNP)FeH(CO)₂]Cl (4a), while the neutral iron hydrides (ⁱPrPNP)FeHCl(CO) (5a) and (^CyPNP)FeHCl(CO) (5b) were synthesized through the reaction of 1a or 1b with 1 equiv of ⁿBu₄NBH₄. The related reaction between 1a and excess NaBH₄ generated the unusual η¹-HBH₃ complex (ⁱPrPNP)FeH(η¹-HBH₃)(CO) (6a). This complex features a bifurcated intramolecular dihydrogen bond between two of the hydrogen atoms associated with the η¹-HBH₃ ligand and the N-H proton of the pincer ligand, as well as intermolecular dihydrogen bonding. The protonation of 6a with 2,6-lutidinium tetraphenylborate resulted in the formation of the dimeric complex [{(ⁱPrPNP)FeH(CO)} ₂(μ₂,η¹:η¹-H ₂BH₂)][BPh₄] (7a), which features a rare example of a μ₂,η¹:η¹-H ₂BH₂ ligand. Unlike all previous examples of complexes with a μ₂,η¹:η¹-H₂BH ₂ ligand, there is no metal-metal bond and additional bridging ligand supporting the borohydride ligand in 7a; however, it is proposed that two dihydrogen-bonding interactions stabilize the complex. Complexes 1a, 2a, 3a, 4a, 5a, 6a, and 7a were characterized by X-ray crystallography.

Full text of DOI:10.1021/ic402762v

Article
pubs.acs.org/IC
Synthesis and Structure of Six-Coordinate Iron Borohydride
Complexes Supported by PNP Ligands
Ingo Koehne,†,‡ Timothy J. Schmeier,‡,§ Elizabeth A. Bielinski,§ Cassie J. Pan,§ Paraskevi O. Lagaditis,†
Wesley H. Bernskoetter,⊥ Michael K. Takase,§ Christian Wurtele,† Nilay Hazari,*,§ and Sven Schneider*,†
̈
†Institut fur Anorganische Chemie, Georg-August-Universitat Gottingen, Tammannstrasse 4, 37077 Gottingen, Germany
̈
̈
̈
̈
§Department of Chemistry, Yale University, P.O. Box 208107, New Haven, Connecticut 06520, United States
⊥Department of Chemistry, Brown University, Providence, Rhode Island 02912, United States
S
* Supporting Information
ABSTRACT: The preparation of a number of iron complexes supported by ligands of the type HN{CH2CH2(PR2)}2 [R =
isopropyl (iPrPNP) or cyclohexyl (CyPNP)] is reported. This is the first time this important bifunctional ligand has been
coordinated to iron. The iron(II) complexes (iPrPNP)FeCl2(CO) (1a) and (CyPNP)FeCl2(CO) (1b) were synthesized through
the reaction of the appropriate free ligand and FeCl2 in the presence of CO. The iron(0) complex (iPrPNP)Fe(CO)2 (2a) was
iPr
prepared through the reaction of Fe(CO)5 with PNP, while irradiating with UV light. Compound 2a is unstable in CH2Cl2 and
is oxidized to 1a via the intermediate iron(II) complex [(iPrPNP)FeCl(CO)2]Cl (3a). The reaction of 2a with HCl generated the
related complex [(iPrPNP)FeH(CO)2]Cl (4a), while the neutral iron hydrides (iPrPNP)FeHCl(CO) (5a) and (CyPNP)FeHCl-
(CO) (5b) were synthesized through the reaction of 1a or 1b with 1 equiv of nBu4NBH4. The related reaction between 1a and
excess NaBH4 generated the unusual η1-HBH3 complex (iPrPNP)FeH(η1-HBH3)(CO) (6a). This complex features a bifurcated
intramolecular dihydrogen bond between two of the hydrogen atoms associated with the η1-HBH3 ligand and the N−H proton
of the pincer ligand, as well as intermolecular dihydrogen bonding. The protonation of 6a with 2,6-lutidinium tetraphenylborate
resulted in the formation of the dimeric complex [{(iPrPNP)FeH(CO)}2(μ2,η1:η1-H2BH2)][BPh4] (7a), which features a rare
example of a μ2,η1:η1-H2BH2 ligand. Unlike all previous examples of complexes with a μ2,η1:η1-H2BH2 ligand, there is no metal−
metal bond and additional bridging ligand supporting the borohydride ligand in 7a; however, it is proposed that two dihydrogen-
bonding interactions stabilize the complex. Complexes 1a, 2a, 3a, 4a, 5a, 6a, and 7a were characterized by X-ray crystallography.
years, bifunctional pincer-type ligands, such as the tridentate
chelating PNP ligand HN(CH2CH2PR2)2 (RPNP; R = alkyl or
aryl), have received significant attention and have been
coordinated to a variety of different transition metals.3 These
ligands have been used both to stabilize transition-metal
catalysts and to support complexes in unusual geometries. For
example, Beller and co-workers3ad have catalytically dehydro-
genated methanol to H2 and CO2 using a ruthenium complex
INTRODUCTION
■
Since Shaw and co-workers1 described the first examples of
pincer-supported transition-metal complexes in the 1970s,
these ligands have become ubiquitous in modern coordination
and organometallic chemistry.2 There are two major reasons
why pincer ligands are commonly used: (i) They often have
relatively easy and modular syntheses, which allow facile tuning
of the steric and electronic properties of the resulting
transition-metal complexes. (ii) The rigid binding of the ligand
to three coplanar sites of the metal frequently generates
complexes with extremely high thermal stability. In recent
Received: November 4, 2013
© XXXX American Chemical Society
A
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R
supported by a PNP ligand, while some of us utilized ligands
bond or a bridging hydride ligand. All of our borohydride-
containing species contain interesting examples of dihydrogen
bonds, which stabilize the complexes.12
of this type to stabilize electron-rich nitrido complexes of
ruthenium, rhodium, and iridium.3x,z,ac A particularly striking
feature of RPNP ligands is that they can participate in reactions
that involve metal−ligand cooperativity.3e,o−q,s,w In fact, both
the N−H bond and one of the C−H bonds of the ethylene
linker can be reversibly activated.3p,w As a result, these types of
ligands have been utilized to support transition-metal catalysts,
which operate via a bifunctional mechanism, for both the
hydrogenation and transfer hydrogenation of polar double
bonds and the dehydrogenation of boraneamines.3e,o−q,s,w,ab
Despite the many examples of bifunctional catalysis with
ruthenium species supported by RPNP pincer ligands,3i,q,s,w,ab,ad
analogous iron chemistry has been neglected. In fact, to date,
there have been no reports of iron complexes stabilized by
RPNP ligands.4 This is even more surprising given that related
ligands have been successfully utilized in iron-catalyzed
transformations. For example, Morris and co-workers employed
iron complexes supported by bifunctional tetradentate PNNP-
type ligands as highly efficient catalysts for the transfer
hydrogenation of ketones,5 while Milstein and co-workers
reported that pincer complexes such as {2,6-C5H3N-
(CH2PiPr2)2}FeH(η1-HBH3)(CO) are active catalysts for the
base-free hydrogenation of ketones.6 It should be noted that
apart from its catalytic applications, Milstein’s borohydride
complex is also important because it represents a rare example
RESULTS AND DISCUSSION
■
Metalation of the Ligand. Two routes were evaluated for
the preparation of Fe(PNP) complexes, starting from iron(0)
(Fe(CO)5) and iron(II) (FeCl2) precursors, respectively. The
i
treatment of FeCl2 with either PrPNP or CyPNP, followed by
the addition of CO, results in the formation of the six-
coordinate iron(II) complexes (iPrPNP)FeCl2(CO) (1a) and
(CyPNP)FeCl2(CO) (1b), respectively, in yields of at least 70%
(eq 1). This is a synthetic route analogous to that described by
Milstein et al. for the coordination of the pyridine-based ligand
2,6-C5H3N(CH2PiPr2)2 to FeBr2.6a The reaction is considerably
slower for the CyPNP ligand (4 h at 50 °C) compared to the
i
PrPNP ligand (2 h at room temperature), presumably because
of the increased steric bulk of the cyclohexyl ligand. The strong-
field ligand CO was introduced to ensure a low-spin ground-
state configuration.13 Accordingly, the new complexes are
diamagnetic, and a single sharp resonance is observed at 67.9
ppm in the 31P{1H} NMR spectrum of 1a while the
corresponding peak in the spectrum of 1b is observed at 58.9
ppm. The IR spectra of 1a and 1b contain strong CO stretching
vibrations at 1926 and 1944 cm−1, respectively, while the N−H
stretches are located at 3203 and 3188 cm−1, respectively.
of an iron species with an η1-borohydride (BH4 ) ligand.6b,7 In
−
general, of the three coordination modes (η1, η2, and η3; Figure
1a) that have been described for mononuclear borohydride
complexes,8 the η2-binding mode is the most commonly
found,8 while η1-coordination is relatively unusual, especially for
d6 metal ions.6b,7,9 Even in the few reported examples of
dinuclear complexes with bridging borohydride ligands, the
μ2,η2:η2-H2BH2-coordination mode (Figure 1b) is by far the
most common,10 and there are only two examples of complexes
with bridging μ2,η1:η1-H2BH2 ligands.11 In both of these cases,
the complexes also contain a supporting metal−metal bond and
bridging hydride ligand.
Surprisingly, when FeCl2 was treated with the even more
t
sterically bulky BuPNP ligand, followed by the addition of CO,
there was no evidence for the formation of a diamagnetic
species equivalent to 1a or 1b. Given the similar electronic
properties of the isopropyl, tert-butyl, and cyclohexyl
substituents, we propose that this is due to steric factors. The
molecular structure of 1a, which was elucidated by X-ray
diffraction, is shown in Figure 2, and important bond distances
and angles are summarized in Table 1. The iron atom is located
within a distorted octahedral coordination geometry, and the
i
chloride ligands occupy mutually trans positions. The PrPNP
Given our interest in the coordination chemistry of
complexes with bifunctional ligands, here we report the
ligand is coordinated meridionally with the CO ligand trans to
R
i
synthesis of iron complexes with PNP ligands [R = isopropyl
the PrPNP nitrogen donor. There are two independent
(iPr) or cyclohexyl (Cy)]. In particular, we have prepared a
number of complexes that feature unusual binding modes of
borohydride ligands, including a dimeric species with a bridging
μ2,η1:η1-H2BH2 ligand, which does not contain a metal−metal
molecules in the unit cell, and the P(1)−Fe(1)−P(2) and
Cl(1)−Fe(1)−Cl(2) bond angles of 168.96(4) and 168.82(4)°
and 173.44(3) and 172.68(11)°, respectively, are indicative of
the distorted octahedral geometry around the iron center. The
Fe(1)−N(1) bond distances in the two independent molecules
[2.065(2) and 2.071(3) Å] are consistent with other Fe−amine
bonds.6a,14 Overall, the bond distances and angles of 1a are
similar to those observed in the related compounds trans-
(iPrPNP)RuCl2(PMe3)3w and {2,6-C5H3N(CH2PiPr2)2}-
FeBr2(CO).6a For example, the (iPrPNP)Ru complex exhibits
a comparable Cl−Ru−Cl bond angle [171.04(2)°], yet a
slightly smaller P−Ru−P bite angle [163.04(3)°] as a
consequence of the longer Ru−N bond length [2.113(4) Å].
Figure 1. Reported coordination modes of borohydride ligands in (a)
monomeric and (b) dimeric complexes.
B
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high spectroscopic yields of 1a were detected, this complex
could only be isolated in approximately 25% yield, presumably
because of loss during purification by column chromatography.
When the reaction was monitored by 31P{1H} NMR spectros-
copy, several reaction intermediates, which could not be
characterized, were observed. However, a crystallization
attempt after partial conversion resulted in the isolation of a
crystal of the iron(II) dicarbonyl complex [(iPrPNP)FeCl-
(CO)2]Cl (3a), which was only characterized by X-ray
crystallography.15 This suggests that oxidation of 2a by the
solvent proceeds through the dicarbonyl intermediate 3a, which
loses CO over time to form 1a (Scheme 1). Nevertheless, the
Figure 2. ORTEP of 1a at 50% probability. Selected hydrogen atoms
have been omitted for clarity, and only one of the two independent
molecules in the unit cell is shown.
considerably lower overall yield renders direct synthesis of 1a
i
from FeCl2, PrPNP, and CO our preferred route.
Preparation of Hydride-Containing Complexes. The
reaction of 2a with HCl results in the protonation of the
iron(0) complex and the formation of the six-coordinate
An alternative preparative route to 1a starts from Fe(CO)5.
Irradiation in the presence of PrPNP in acetone results in the
formation of the diamagnetic five-coordinate iron(0) complex
i
iron(II) cation [(iPrPNP)FeH(CO)2]Cl (4a), with a chloride
counterion (eq 2). 4a exists as a mixture of two isomers, as
evidenced by two sets of signals in the NMR spectra (for
example, in the 31P{1H} NMR spectrum, two signals are
observed at 99.5 and 102.1 ppm). The ratio of these signals is
always 3:1 at room temperature and does not vary between
(iPrPNP)Fe(CO)2 (2a; Scheme 1), which was isolated and fully
characterized. A single resonance at 109.8 ppm is observed in
the 31P{1H} NMR spectrum of 2a. The two separate peaks at
222.4 and 226.2 ppm in the 13C{1H} NNR spectrum of 2a can
be assigned to chemically inequivalent CO ligands, which is in
agreement with the two CO stretching vibrations observed by
IR spectroscopy (1838 and 1767 cm−1). The significant
decrease in the average CO stretching frequency in the
iron(0) complex 2a, compared with the iron(II) complexes 1a
and 1b, is consistent with an increase in the back-donation to
the CO ligands from the more electron-rich metal center in the
lower oxidation state. The molecular structure of 2a, obtained
by X-ray diffraction (Figure 3), reveals a square-pyramidal
geometry around the iron atom. The PNP ligand is bound
meridionally and occupies three positions of the base of the
square pyramid, while the two CO ligands occupy the
remaining basal position and the apical position. This is
consistent with two different resonances being observed for the
carbonyl ligands in the 13C NMR spectrum, with slow or no
exchange of these ligands on the NMR time scale at room
temperature. The P(1)−Fe(1)−P(2) bond angle in 2a
[158.58(2)°] is smaller than that in 1a, presumably as a
consequence of the change in the geometry of the complex
from octahedral in 1a to square-pyramidal in 2a. As a result, the
Fe(1)−N(1) bond distance is longer in 2a [2.1281(12) Å] than
in 1a.
independent preparations of 4. Both sets of signals are
i
consistent with meridional coordination of the PrPNP ligand
and the hydride in a trans position to a CO ligand, as judged by
1
their H NMR chemical shifts (−7.38 and −8.22 ppm). Given
the similar NMR chemical shifts between the two isomers, we
propose that the two structures have either cis- or trans-
coplanar arrangements of the N−H and Fe−H moieties,
respectively, as shown in eq 2. Further confirmation of this
assignment was obtained through X-ray crystallography because
the structure of 4aTrans was elucidated.15 NMR spectroscopy on
the single crystals used for X-ray crystallography allowed us to
determine that 4aTrans is the main product of the reaction. The
CO stretching vibrations are observed at 1998 and 1943 cm−1
for 4aTrans and at 1987 and 1932 cm−1 for 4aCis in the IR
spectrum, consistent with the stretching frequencies observed
in the other iron(II) complexes synthesized as part of this work.
Presumably, a geometry with the hydride trans to the CO
ligand, as opposed to trans to the nitrogen atom of the PNP
ligand, is favored because it leads to less competition between
the two CO ligands for the electron density from the iron
center for back-donation.The neutral iron(II) hydridochloride
complexes 5a and 5b were obtained through the reaction of 1a
or 1b with 1 equiv of nBu4NBH4 in acetonitrile (ACN) at room
temperature, followed by recrystallization at −30 °C (Scheme
2). The related reactions between 1a and 1b and 1 equiv of
Complex 2a is oxidized upon dissolution in dichloromethane
(Scheme 1). The solution initially changes from dark green to
pale yellow, and after 12 h, a reddish-brown solution is
observed. NMR spectroscopy indicates that the purple
dichloride complex 1a is the major product. Although relatively
Table 1. Selected Bond Distances (Å) and Angles (deg) for the (iPrPNP)Fe Complexes 1a, 2a, 5a, 6a, and 7a
compound
Fe(1)−N(1)
Fe(1)−C(1)
Fe(1)−X(1)
Fe(1)−X(2)
C(1)−O(1)
P(1)−Fe(1)−P(2)
a
1a
2.065(2) and
2.071(3)
1.743(4) and
2.3201(9) and 2.322(2);
X = Cl
2.3417(10) and 2.331(1);
X = Cl
1.133(4) and
168.96(4) and
168.82(4)
1.753(4)
1.1458(5)
b
2a
2.1281(12)
1.7188(15)ba,
1.1809(19)ba,
158.58(2)
1.7449(15)ax
1.1848(17)ax
5a
6a
7a
2.070(3)
2.0715(13)
2.074(2)
1.713(4)
1.723(6)
1.720(3)
2.4125(10); X = Cl
1.43(3); X = H
1.45(2); X = H
1.47(2); X = H
1.161(4)
1.170(6)
1.169(3)
165.01(4)
165.920(18)
163.74(3)
1.707(18); X = η1-HBH3
1.74(2); X = μ2, η1:η1-
HBH3
a
b
There are two independent molecules in the unit cell. 2a has two CO ligands: ba refers to the CO that is part of the base of the square pyramid,
and ax refers to the CO that is in the axial position.
C
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Scheme 1
ppm, respectively, in the 1H NMR spectrum. The N−H
stretching frequencies for the PNP ligands in the solid-state IR
spectra of 5a and 5b were located at 3183 and 3134 cm−1,
respectively. This shift to lower frequency compared to the
dichloride complexes 1a and 1b is consistent with the
formation of a hydrogen bond involving the N−H bond of
the ligand. For example, the observed stretching frequency in
5a is quite similar to the N−H stretching frequency in a
(iPrPNP)IrIII formate complex that we have reported previously,
which contains an N−H···(O)CHOIr hydrogen bond.3o The
CO stretching frequencies of both 5a (1895 cm−1) and 5b
(1895 cm−1) are significantly lower than those in 1a and 1b,
which is consistent with the hydride ligand being a better σ
donor than the chloride ligand.17 In the case of complexes 5a
and 5b, no nuclear Overhasuer effect (NOE) was observed
1
between the N−H proton and Fe−H by H NMR spectros-
Figure 3. ORTEP of 2a at 50% probability. Selected hydrogen atoms
have been omitted for clarity.
copy, and on that basis, we propose that the N−H proton is
located in the trans position with respect to the hydride ligand.
When the reaction of 1a and Bu4NBH4 was monitored by
n
1H and 31P NMR spectroscopy the formation of two products
in a 6:1 ratio was initially observed, with 5a being the minor
species (Scheme 3). This product mixture eventually converted
exclusively to 5a upon standing in solution, with no
intermediates detected. The initially formed major product
showed a clear triplet at −18.6 ppm in the 1H NMR spectrum,
which integrated to one proton. This is consistent with the
presence of a single Fe−H bond. A singlet was observed at 96.3
ppm in the 31P{1H} NMR spectrum, which is quite close to the
31P{1H} NMR chemical shift observed for 5a (95.4 ppm). At
this stage, we propose that the initially formed product is an
isomer of 5a in which the N−H and Fe−H moieties are
oriented cis with respect to each other (5aCis). Our hypothesis
is that the ligand substitution of 1a with nBu4NBH4 is
kinetically controlled and a diastereomeric product mixture is
initially obtained because the hydride can attack either of the
two faces containing the chloride ligands in 1a. However,
instead of an initial statistical 1:1 ratio of the isomers 5aCis and
5a, a 6:1 ratio of 5aCis and 5a is observed because of the
directing ability of the N−H moiety. Intermolecular dihydrogen
bonding12 between nBu4NBH4 and the N−H bond of the PNP
ligand in 1a would favor hydride delivery to form 5aCis.
Subsequent isomerization of 5aCis to 5a gives exclusively one
product, although at this stage, the pathway for isomerization is
NaBH4 give a mixture of products, while the reaction of 1a with
LiHBEt3 also gave clean conversion to 5a (in higher yield than
the corresponding Bu4NBH4 reaction; see the Experimental
n
Section). This indicates that the choice of the hydride source is
crucial and Kemp, Goldberg, and co-workers have previously
made similar observations while preparing Ni−H species
supported by pincer ligands.16 Complex 5a could also be
prepared by photodecarbonylation of 4a with UV light
(Scheme 2); however, isolated yields were lower than those
of the direct synthesis from 1a because of the need for
purification using column chromatography. The metal hydride
resonances of 5a and 5b appear as triplets at −19.1 and −19.4
Scheme 2
D
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Scheme 3
Figure 4. (a) ORTEP of 5a at 50% probability. (b) Dimeric packing of 5a at 50% probability. Selected hydrogen atoms have been omitted for clarity,
and the disorder in some of the isopropyl groups of the ligand is not shown.
unclear. It is likely that 5a is thermodynamically preferred
because it maximizes the opposing dipole interactions between
the partially negatively charged chlorine atom in the Fe−Cl
bond and the adjacent partially positively charged hydrogen
atom in the N−H bond. Density functional theory (DFT)
calculations on the structures of 5a and 5aCis indicate that 5a is
thermodynamically more favorable.15 Similar behavior in
solution was observed during the synthesis of 5b.
formed between the chloride ligand and the N−H proton on
adjacent molecules (Figure 4b). The two hydrogen bonds have
identical intermolecular Cl(1)−H(1N*) and Cl(1*)−H(1N)
bond distances of 2.78(3) Å, which is significantly shorter than
the combined van der Waals radii of hydrogen and chlorine.19
The hydrogen bonds result in the formation of an essentially
planar eight-membered ring and are consistent with the low
N−H stretching frequency in the IR spectrum.
The molecular structure of 5a in the solid state is shown in
Figure 4 and reveals a distorted octahedral geometry around
the central iron atom, similar to those found for 1a and 3a. The
data were of sufficient quality that the hydrogen atoms involved
in the Fe−H and N−H bonds were located in the Fourier map
and their positions refined without restraint. As suggested by
1H NMR spectroscopy, the N−H bond is trans to the Fe−H
bond. The Fe−H bond distance of 1.43(3) Å is comparable to
that observed by Milstein and co-workers in {2,6-C5H3N-
(CH2PiPr2)2}FeHBr(CO).6a The substitution of a chloride
ligand on 1a for a hydride ligand on 5a results in significant C−
O bond lengthening in the CO ligand, presumably because of
the increased σ donation from the hydride ligand, which is
consistent with the IR data. The C−O bond distance increases
from 1.130(5) Å in 1a to 1.168(2) Å in 5a, while the Fe(1)−
C(1) bond distance contracts from 1.736(4) Å in 1a to
1.718(3) Å in 5a. The Fe−Cl bond length increases from
2.3384(11) Å in 1a to 2.4155(5) Å in 5a, which is consistent
with the increased trans influence of the hydride ligand.18 The
intramolecular Cl(1)−H(1N) distance is 2.58(3) Å. In the solid
state, 5a packs into dimers, with a pair of hydrogen bonds
Preparation of Borohydride-Containing Complexes.
The treatment of 1a with 10 equiv of NaBH4 in a 1:1 ACN/
EtOH mixture results in the formation of the iron(II)
borohydride complex (iPrPNP)FeH(η1-HBH3)(CO) (6a),
with no evidence for the formation of a dihydride species (eq
3). Complex 6a is a rare example of a monomeric group 8 η1-
E
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Figure 5. (a) ORTEP of 6a at 50% probability. (b) Dimeric packing of 6a at 50% probability. Selected hydrogen atoms have been omitted for clarity,
and the disorder in the CO ligand is not shown.
HBH3 complex.6b,7,9a,b,d,f,g The same product is obtained when
excess nBu4NBH4 is used as the hydride and borohydride
source, but in this case, longer reaction times (approximately 27
h) are required. In contrast, the treatment of the cyclohexyl-
substituted complex 1b with excess NaBH4 or nBu4NBH4
resulted in the formation of a mixture of products, and it was
not possible to isolate the analogous η1-HBH3 species to 6a.
consistent with the participation of the coordinated amine in
hydrogen bonding.
In a fashion analogous to the synthesis of 5a, the reaction of
1a with NaBH4 results in an initial product mixture containing
two species, one of which is 6a. Upon standing at room
temperature, the mixture converts entirely to 6a. Again, we
postulate that the other initial product is an isomer of 6a in
which the N−H bond is trans to the η1-HBH3 ligand and cis to
1
The H NMR spectrum of 6a at room temperature contains a
1
the Fe−H bond (6aCis). In the room temperature H NMR
resonance corresponding to the proton of the terminal Fe−H
at −19.5 ppm, similar to that of 5a, and also a broad resonance
centered at −2.5 ppm, which integrates to four protons and is
assigned as the η1-HBH3 protons. When the 1H NMR spectrum
is recorded at −40 °C, the broad resonance at −2.5 ppm is
decoalesced into two new signals at 0.9 and −14.8 ppm,
respectively. The signal at −14.8 ppm integrates to one proton,
spectrum of the mixture, a clear signal at −22.0 ppm is assigned
as the hydride of 6aCis. At −40 °C, there are two different
1
resonances in the H NMR spectrum that are consistent with
bridging Fe−H−B protons, supporting our hypothesis that
both 6a and 6aCis are present. The 31P{1H} NMR chemical shift
of 6aCis (100.2 ppm) is also close to that of 6a (99.1 ppm). In
this case, we propose that dihydrogen bonding12 between the
N−H proton and the η1-HBH3 ligand (vide infra) results in 6a
being thermodynamically preferred over 6aCis. DFT calculations
also indicate that 6a is the more stable isomer.15
while the signal at 0.9 ppm, which is partially obscured under
i
resonances associated with the PrPNP ligand, presumably
integrates to three protons. These results are consistent with
reduced η1-HBH3 fluxionality at low temperature, resulting in
separate signals for the bridging Fe−H−B and terminal B−H
protons, respectively. Indeed, 2D NOESY NMR experiments
(−40 °C, mixing time = 400 ms) do exhibit exchange
correlations between the protons associated with the resonance
at 0.9 ppm and the proton corresponding to the resonance at
−14.8 ppm, suggesting that interchange is still occurring at this
temperature but at a slower rate.15 Similar fluxional behavior in
complexes containing an η1-HBH3 ligand has been previously
observed by Baker and Field.20 The NMR experiments also
indicated an NOE correlation between the N−H resonances at
3.89 ppm and the terminal B−H protons at 0.9 ppm,
establishing that the N−H bond is cis to the η1-HBH3 ligand
and trans to the Fe−H bond.15The IR spectrum of 6a is also
consistent with an η1-HBH3 ligand. Well-defined stretches,
which have been assigned based on previous literature
The high-quality structure of 6a from X-ray diffraction, which
allowed for the location and refinement of the Fe−H, N−H,
and B−H hydrogen atoms, is shown in Figure 5. To the best of
our knowledge, there are only two previous examples of
structurally characterized iron complexes containing an η1-
HBH3 ligand.6b,7 The molecular structure in the solid state
confirms that the η1-HBH3 ligand and N−H bond are in a cis
arrangement. Overall, the bond angles and lengths around the
iron center in 6a are very similar to those observed in 5a. In
particular, the C−O bond length in the CO ligand and the Fe−
C bond length are almost identical in 5a and 6a, which provides
further support that η1-HBH3 is electronically similar to the
chloride ligand. The Fe(1)−H(20)−B(1) bond angle is bent
[141.8(15)°] and is in the typical range for η1-HBH3 metal
complexes.6b,7 The Fe−B distance [2.745(2) Å] is also
consistent with the two other iron complexes with η1-HBH3
ligands.6b,7 The bridging Fe(1)−H(20) bond length [1.70(2)
Å] is elongated compared to the terminal Fe−H bond length
[1.45(2) Å]. Similarly, the bridging borohydride B(1)−H(20)
bond distance [1.18(2) Å] is lengthened compared to the
terminal B−H bonds [for example, the B(1)−H(22) bond
distance is 1.09(2) Å].
precedent, are observed at 2352 (νBH ), 2030 (νFe−H−B), and
3
1069 (νBH ) cm−1.20b The CO stretching frequency at 1896
3
cm−1 is almost identical with the corresponding band in 5a,
indicating that the η1-HBH3 ligand donates an amount of
electron density similar to the chloride ligand in 5a. The N−H
stretching frequency in 6a is located at 3197 cm−1, which is
F
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Article
The structure of 6a features a bifurcated intramolecular
dihydrogen bond12 between the η1-HBH3 ligand and the N−H
bond of the PNP ligand. A close contact of 2.16(2) Å is
observed within N(1)−H(19)···H(21)−B(1), and a second
weaker contact of 2.43(3) Å is present within N(1)−H(19)···
H(23)−B(1). Although 2.43(3) Å is slightly larger than the van
der Waals radii (2.4 Å) of two hydrogen atoms,19 considering
the systematic underestimation of X−H bond distances
inherent in X-ray crystallography,21 we believe that this
interaction is significant. Furthermore, Crabtree and co-workers
report that in systems where a B−H···N−H dihydrogen bond is
present, the B−H···H−N bond angle is bent to maximize the
columbic interaction between the electropositive donor hydro-
gen atom and the electronegative acceptor boron atom.12b−d
Indeed in 6a, the angles of both proposed dihydrogen bonds
are bent (the B(1)−H(21)−H(19) bond angle is 93(1)°, while
the B(1)−H(23)−H(19) bond angle is 80(1)°), which
provides further support for two dihydrogen bonds. Related
examples of dihydrogen bonding have previously been observed
in ruthenium complexes by Noyori and co-workers9f and
Morris and co-workers9g and are believed to be important in
the catalytic activity of these species.
Along with the bifurcated intramolecular dihydrogen bond, a
bifurcated intermolecular dihydrogen bond is also present,
which causes a dimeric packing of molecules in 6a similar to
that in 5a (Figure 5b). However, unlike the planar bridging
eight-membered ring formed by connecting the molecules in
5a, a bridging distorted octahedron with hydrogen atoms
occupying the six vertices is formed in 6a. The intermolecular
dihydrogen bond is formed between the B−H bonds of the η1-
HBH3 ligand and the N−H bond of a neighboring molecule.
The same B−H bonds that form the intramolecular dihydrogen
bond also form the intermolecular dihydrogen bond, and
similar geometrical parameters are observed in the intra- and
intermolecular cases. In principle, dihydrogen bonding should
result in increased B−H bond distances.12b−d However, in 6a,
the B−H bond lengths of the two bonds that are involved in
dihydrogen bonds with the N−H moieties (B(1)−H(21)
1.12(2) and B(1)−H(23) 1.12(2) Å) are the same within error
as the terminal B−H bond distance (B(1)−H(22) 1.09(2) Å).
In an attempt to synthesize a dihydrogen complex, 6a was
treated with 1 equiv of 2,6-lutidinium tetraphenylborate in
tetrahydrofuran (THF). Upon the addition of the acid, the
solution rapidly changed from red to yellow, and the evolution
of a gas was observed. The dimeric complex [{(iPrPNP)FeH-
(CO)}2(μ2,η1:η1-H2BH2)][BPh4] (7a) was isolated in 75%
yield, along with 0.5 equiv of 2,6-lutidinium tetraphenylborate,
indicating that the reaction does not proceed further in the
presence of excess acid (eq 4). When the reaction was repeated
with 0.5 equiv of 2,6-lutidinium tetraphenylborate, 7a was
formed with full conversion of the starting material and H2
1
evolution was observed by H NMR spectroscopy. Compound
7a is particularly noteworthy because it is the first dimeric
group 8 species with a μ2,η1:η1-H2BH2 ligand and the only
example of a transition-metal complex that contains a μ2,η1:η1-
H2BH2 ligand, which does not also contain a bridging hydride
and a metal−metal bond.11 Therefore, the μ2,η1:η1-H2BH2
ligand in 7a could be described as the first example of an
“unsupported” bridging borohydride ligand, although because
of dihydrogen bonding (vide infra), this is almost certainly not
the case. In a fashion similar to that of the monomeric η1-HBH3
1
complex 6a, 7a exhibits fluxional behavior. In the H NMR
spectrum at room temperature, a single resonance is observed
for the two terminal Fe−H protons at −21.9 ppm, while all of
the protons associated with the μ2,η1:η1-H2BH2 ligand are
equivalent and appear as a broad resonance at −5.7 ppm. When
the spectrum is recorded at −80 °C, the broad peak at −5.7
ppm is no longer present, and two new resonances at 0.0 and
−14.5 ppm, which integrate to two protons each, are observed.
This is consistent with either no or slow exchange on the NMR
time scale of the protons associated with μ2,η1:η1-H2BH2 at low
temperature. It should be noted that complex 7a is insoluble in
most common NMR solvents and NMR data could only be
recorded in CD2Cl2. In this solvent, 7a is unstable at room
temperature and decomposes in minutes. As a result, minor
unidentified impurities are always present in the NMR
spectrum. In the IR spectrum, the CO stretching frequency
in 7a (1901 cm−1) is similar to that observed in 6a, suggesting a
similar electronic environment at the metal center. The
molecular structure of 7a from single-crystal X-ray diffraction
is shown in Figure 6. It should be noted that the key hydrogen
atoms associated with the Fe−H, B−H, and N−H bonds were
all located and refined. The dimeric core of 7a features a
Figure 6. ORTEP of the cation of 7a at 50% probability. Selected
hydrogen atoms, the counterion, and the solvent of crystallization have
been omitted for clarity.
G
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bridging borohydride ligand that coordinates to each iron
center through a single B−H bond. Although the bond lengths
and angles around the two iron centers are almost identical, the
molecule does not possess any symmetry elements and the
orientation of the ligands around the two iron centers differs by
approximately 90°. The bond angles and distances around the
iron and boron centers are consistent with those observed in
the monomeric complex 6a (Table 2). The two Fe−H(B)
bridging bond distances in 7a are 1.74(2) and 1.79(2) Å, while
the two Fe−B bond lengths are 2.734(4) and 2.781(4) Å,
consistent with the assigned μ2,η1:η1-H2BH2 coordination
mode. The Fe(1)−Fe(2) bond distance is >5.2 Å, indicating
that no metal−metal bond is present.
In a manner similar to that of 6a, dihydrogen bonding is also
featured in the core of 7a. Unlike the bifurcated dihydrogen
bonds seen in 6a, each N−H bond in 7a forms a single
dihydrogen bond to the borohydride ligand, which creates two
chelating six-membered rings. The N(1)−H(65)···H(68)−
B(1) dihydrogen bond length is 2.06(4) Å, and the N(2)−
H(70)···H(67)−B(1) bond length is 2.22(4) Å. As expected,
the B−H···H−N angles of the atoms involved in both proposed
dihydrogen bonds are bent [the B(1)−H(68)−H(65) bond
angle is 112(2)°, and the B(1)−H(67)−H(70) bond angle is
95(2)°]. The B−H bonds that bridge to the iron atoms are
longer than the B−H bonds that are involved in the dihydrogen
interactions; B(1)−H(66) is 1.17(2) Å and B(1)−H(69) is
1.18(2) Å, whereas B(1)−H(67) is 1.11(2) Å and B(1)−H(68)
is 1.11(2) Å. Overall, the dihydrogen-bonding interactions in
7a presumably stabilize the μ2,η1:η1-H2BH2 ligand and make it
more favorable for dimerization to occur. In fact, we suggest
that these dihydrogen bonds play a role similar to that of the
metal−metal bond and additional bridging hydride ligand
observed in other examples of complexes with μ2,η1:η1-H2BH2
ligands and serve to “support” the μ2,η1:η1-H2BH2 ligand.11
bonds between protons of the N−H groups and the bridging
borohydride ligands stabilize the complex. It is conceivable that
this type of intramolecular dihydrogen bonding will influence
the stoichiometric and catalytic reactivity of complexes with
PNP ligands, and further studies toward this end are being
conducted in our laboratories.
EXPERIMENTAL SECTION
■
General Methods. Experiments were performed under a
dinitrogen or an argon atmosphere in an M-Braun drybox or using
standard Schlenk techniques unless otherwise noted. Under standard
glovebox conditions, purging was not performed between uses of
pentane, diethyl ether, benzene, toluene, and THF; thus, when any of
these solvents were used, traces of all of these solvents were in the
atmosphere. Moisture- and air-sensitive liquids were transferred by a
stainless steel cannula on a Schlenk line or in a drybox. The solvents
for air- and moisture-sensitive reactions were dried by passage through
a column of activated alumina followed by storage under dinitrogen or
argon. All commercial chemicals were used as received except where
i
t
noted. PrPNP,3d CyPNP,22 BuPNP3u and 2,6-lutidinium tetraphenylbo-
rate23 were prepared using literature procedures. Anhydrous FeCl2,
Fe(CO)5, HCl in Et2O (2 M), LiHBEt3 in THF (1 M), NaBH4,
nBu4NBH4, and sodium tetraphenylborate were purchased from
Aldrich and used as received. Deuterated solvents were obtained
from Cambridge Isotope Laboratories. C6D6 was dried over sodium
metal, CD2Cl2 was dried over calcium hydride, and acetone-d6 was
dried by stirring for 24 h over molecular sieves (3 Å) and for 24 h over
activated B2O3. All deuterated solvents were distilled prior to use.
NMR spectra were recorded on Bruker AMX-400, AMX-500, Avance
300, or Avance 500 spectrometers or on a Varian 300 MHz
spectrometer at ambient probe temperatures unless noted. Chemical
shifts are reported in ppm, with respect to a residual internal protio
1
solvent for H and 13C NMR spectra and to an external standard for
31P NMR spectra (85% H3PO4 at 0.0 ppm). IR spectra were measured
using a diamond smart orbit ATR on a Nicolet 6700 FT-IR instrument
or a Nujol mull between KBr plates on a Bruker Vertex 70
spectrometer. UV−vis spectra were measured using a Cary 50
spectrophotometer. Robertson Microlit Laboratories, Inc., and the
CONCLUSIONS
■
analytical laboratory of the Institut fur Anorganische Chemie
̈
The synthesis of a variety of iron complexes supported by
i
PrPNP and CyPNP ligands is reported. A particularly interesting
feature of these complexes is the ability of the proton on the
N−H moiety of the PNP ligand to participate in both intra- and
intermolecular hydrogen bonding and dihydrogen bonding
with ligands that are coordinated to the iron center. For
example, we have prepared a rare example of an iron complex
with an η1-HBH3 ligand. In this species, two of the B−H bonds
of the ligands participate in bifurcated dihydrogen bonds with
the proton associated with the N−H group. Furthermore, we
have prepared the first example of a dimeric iron complex with
a μ2,η1:η1-H2BH2 ligand. In the previous examples of transition-
metal complexes with a μ2,η1:η1-H2BH2 ligand, a metal−metal
bond and another bridging ligand support the bridging
borohydride ligand. In our case, there is no additional bridging
ligand or Fe−Fe bond; however, we believe that dihydrogen
(Universitat Gottingen) performed the elemental analyses (inert
atmosphere).
̈
̈
X-ray Crystallography. Crystal samples were mounted in
MiTeGen polyimide loops with immersion oil. The diffraction
experiments were carried out on a Rigaku SCXMini diffractometer
with a Rigaku CCD detector using filtered Mo Kα radiation (λ =
0.71073 Å) for 1a, a Bruker Nonius FR591 rotating-anode
diffractometer with a Bruker Nonius Kappa CCD using Mo Kα
radiation (λ = 0.71073 Å) for 2a and 3a, a STOE IPDS II
diffractometer using Mo Kα radiation (λ = 0.71073 Å) for 4aTrans, a
Rigaku MicroMax-007HF diffractometer coupled to a Saturn994 +
CCD detector with Cu Kα radiation (λ = 1.54178 Å) for 5a, or a
Rigaku R-AXIS RAPID diffractometer coupled to a R-AXIS RAPID
imaging plate detector with Mo Kα radiation (λ = 0.71073 Å) for 6a
and 7a. For 1a, 5a, 6a, and 7a, the data frames were processed using
Rigaku CrystalClear24 and corrected for Lorentz and polarization
effects. The structures were solved by direct methods25 and expanded
using Fourier techniques.26 For 2a and 3a, the PLATON MULABS
semiempirical absorption correction using multiple scanned reflections
was applied. The structures were solved by direct methods, and the
full-matrix least-squares refinement was carried out on F2 using
SHELXTL NT 6.12.27 In all structures, non-hydrogen atoms were
refined anisotropically and hydrogen atoms were treated as idealized
contributions except where noted. Details of the crystal and refinement
data for 1a, 2a, 3a, 4aTrans, 5a, 6a, and 7a are described in the
Supporting Information.
Table 2. Selected Bond Distances (Å) for the (iPrPNP)Fe
Complexes 6a and 7a
bond distance
6a
2.745(2)
7a
Fe−B
2.734(4), 2.781(4)
1.17(2), 1.18(2)
1.11(2), 1.11(2)
FeH−B
BH···HN
B−H(t)
BH−HN
1.18(2)
1.12(2), 1.12(2)
1.09(2)
Synthetic Procedures and Characterization Data for New
Compounds. (iPrPNP)FeCl2(CO) (1a). Route A. A suspension of 10
2.16(2), 2.43(3)
2.06(4), 2.22(4)
H
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Article
iPr
mg of anhydrous FeCl2 (1 equiv, 0.080 mmol) and 25 mg of PNP (1
equiv, 0.080 mmol) in 5 mL of THF was degassed using three freeze−
pump−thaw cycles. CO (1 atm) was then introduced at room
temperature using a dual-manifold Schlenk line. The resulting pale-
purple suspension was stirred at room temperature for 2 h to give a
deep-purple solution, the solvent was removed, and the solid was
washed with 3 × 5 mL pentane to give 1a as a purple solid. Crystals
suitable for X-ray diffraction were grown from a saturated CH2Cl2
solution at −30 °C. Yield: 30 mg (0.065 mmol, 81%).
6.56 mg of HCl (1.5 equiv, 0.180 mmol) in Et2O (2 M) was added. A
color change to pale yellow and precipitation of a colorless solid were
observed. The solution was stirred for 10 min at room temperature,
the solvent was evaporated under vacuum, and the beige residue was
lyophilized from benzene to give 4a as a beige solid. Yield: 50 mg
(0.11 mmol, 93%). The spectroscopic characterization is in agreement
with a mixture of two isomers as described in the text (A (trans) and B
(cis)) in a 3:1 ratio with the trans and cis arrangements of the N−H
and Fe−H moieties.
Route B. Complex 2a (65 mg, 0.156 mmol) was dissolved in 20 mL
of CH2Cl2 and stirred at room temperature for 12 h. The solution
gradually changed from dark green to reddish brown. The solvent was
evaporated to dryness and the residue washed with pentanes. The
crude product was dissolved in THF and purified by column
chromatography as a purple band from silanized silica (eluent:
pentanes). The purple compound was dissolved in benzene and
filtered, and the solvent was evaporated to obtain 1a as a purple
microcrystalline solid. Yield: 17 mg (0.037 mmol, 24%).
Anal. Found (calcd) for C17H37Cl2FeNOP2: C, 44.16 (44.37); H,
8.07 (8.10); N, 2.95 (3.04). H NMR (400 MHz, CD2Cl2): 5.23 (br,
1H, NH), 3.62 (m, 2H, CH2), 3.31 (dd, J = 25.0 Hz, JHP = 12.5 Hz,
2H, CH2), 2.53 (m, 6H, CH2, CH), 2.11 (m, 2H, CH), 1.45 (m, 12H,
CH3), 1.38 (m, 12H, CH3). 13C{1H} NMR (125 MHz, CD2Cl2): 50.1
(vt, JCP = 4.5 Hz), 26.8 (vt, JCP = 6.7 Hz), 23.8 (vt, JCP = 10.7 Hz),
21.9 (vt, JCP = 9.2 Hz), 20.2, 19.9, 19.0, 18.8; CO resonance was not
detected. 31P{1H} NMR (162 MHz, CD2Cl2): 67.9. IR (cm−1): 3204
(νNH), 1926 (νCO). UV−vis [THF; λmax, nm (ε, L mol−1 cm−1)]: 226
(12929), 261 (10070), 322 (27724), 560 (117).
Anal. Found (calcd) for C18H38ClFeNO2P2: C, 47.30 (47.65); H,
8.56 (8.44); N, 2.99 (3.09). 1H NMR (500 MHz, CD2Cl2): 6.48 (s br,
A
1H, NHA), 5.91 (s br, 1H, NHB), 2.71 (br, 2H, CH2 ), 2.41 (m, 4H,
A
A
A
CHA), 2.05 (br, 2H, CH2 ), 1.93 (br, 2H, CH2A), 1.82 (br, 2H, CH2 ),
1.46 (dd, J = 7.2 Hz, 3JHP = 15.7 Hz, 6H, CH3 ), 1.38 (dd, J = 6.9 Hz,
A
B
3JHP = 13.8 Hz, 6H, CH3 ), 1.33 (m, 12H, CH3 ), 1.23 (m, 12H,
CH3 ), −7.38 (t, 2JHP = 48.8 Hz, 1H, FeHB), −8.22 (t, 2JHP = 44.8 Hz,
A
1H, FeHA); not all resonances for isomer B (cis) were identified.
13C{1H} NMR (75 MHz, CD2Cl2): 54.7 (vt, JCP = 3.5 Hz, NCAH2),
32.2 (vt, JCP = 11.9 Hz, CAH), 30.2 (vt, JCP = 10.5 Hz, CAH2), 28.4 (vt,
JCP = 10.1 Hz, CBH2), 26.5 (vt, JCP = 14.0 Hz, CAH), 21.1 (s, CBH3),
20.5 (s, CBH3), 20.2 (s, CAH3), 20.1 (s, CAH3), 19.2 (s, CAH3), 19.1 (s,
CBH3), 18.9 (s, CAH3), 18.7 (s, CBH3); CO resonances were not
detected. 31P{1H} NMR (120 MHz, CD2Cl2): 102.1 (s, PB), 99.5 (s,
PA). IR (Nujol, cm−1): 1998 (νCO), 1987 (νCO), 1943 (νCO), 1932
(νCO).
1
3
(iPrPNP)FeHCl(CO) (5a). Route A. To a solution of 200 mg of 1a (1
equiv, 0.434 mmol) in 1 mL of ACN was added 110 mg of nBu4NBH4
(1 equiv, 0.428 mmol) at room temperature. The solution changed
(CyPNP)FeCl2(CO) (1b). A suspension of 7 mg of anhydrous FeCl2 (1
equiv, 0.053 mmol) and 25 mg of CyPNP (1 equiv, 0.053 mmol) in 5
mL of THF was degassed using three freeze−pump−thaw cycles. CO
(1 atm) was then introduced at room temperature using a dual-
manifold Schlenk line. The resulting pale-purple suspension was
stirred at 50 °C for 4 h to give a deep-purple solution, the solvent was
removed, and the solid was washed with 3 × 5 mL pentane to give 3b
as a purple solid. Yield: 23 mg (0.037 mmol, 70%).
n
from purple to orange upon the addition of Bu4NBH4. The reaction
mixture was stirred for 48 h at ambient temperature, after which time
the volatiles were removed in vacuo. The residue was extracted with 3
× 5 mL of 2:1 Et2O/benzene and then cooled to −30 °C. Compound
5a was isolated as orange crystals. Crystals suitable for X-ray diffraction
were grown from a saturated Et2O solution at −30 °C. Yield: 70 mg
(0.16 mmol, 38%).
Route B. Compound 1a (100 mg, 0.217 mmol) was dissolved in 12
mL of THF and cooled to −50 °C. A cold solution (−50 °C) of
LiHBEt3 (0.240 mmol) in THF (1 M) was slowly added, and the
solution was allowed to warm to room temperature over 150 min. The
reaction mixture slowly changed from dark red to reddish yellow. After
evaporation of the solvent, the residue was washed with 6 mL of
pentanes, extracted with Et2O/benzene (3:1), and crystallized at −38
°C. Compound 5a was isolated as orange crystals. Yield: 45 mg (0.11
mmol, 51%).
Anal. Found (calcd) for C29H53Cl2FeNOP2: C, 56.95 (56.14); H,
8.74 (8.61); N, 2.16 (2.26). H NMR (400 MHz, CD2Cl2): 5.21 (br,
1H, NH), 3.56 (m, 2H, CH2), 3.27 (m, 2H, CH2), 2.47 (br, 2H), 2.24
(br, 5H) 2.09 (t, J = 13.3 Hz, 4H), 1.95−1.62 (m, 22H), 1.26 (t, J =
10.4 Hz, 6H), 1.13 (t, J = 9.7 Hz, 4H). 13C{1H} NMR (C6D6, 75
1
MHz): 49.4 (vt, JCP = 5.4 Hz), 34.5 (vt, JCP = 10.1 Hz), 32.7 (vt, JCP
=
8.5 Hz), 30.6, 29.7, 29.1 (d, JCP = 18.4 Hz), 28.79 (m), 27.2 (m), 26.7
(d, JCP = 4.6 Hz), 24.6 (vt, JCP = 6.2 Hz); CO resonance was not
detected. 31P{1H} NMR (162 MHz, CD2Cl2): 58.9. IR (cm−1): 3188
(νNH), 1944 (νCO). UV−vis [THF; λmax, nm (ε, L mol−1 cm−1)]: 212
(16891), 263 (10123), 325 (3246), 475 (177).
Anal. Found (calcd) for C17H38ClFeNOP2: C, 47.69 (47.96); H,
1
9.01 (9.00) N, 3.24 (3.29). H NMR (500 MHz, CD2Cl2): 3.69 (br,
(iPrPNP)Fe(CO)2 (2a). A total of 100 mg of Fe(CO)5 (1 equiv, 0.510
1H, NH), 2.93 (m, 2H, CH2), 2.76 (m, 2H, CH2), 2.02 (m, 2H, CH),
1.70 (m, 10H, CH3 and CH2), 1.55 (m, 2H, CH), 1.24 (m, 6H, CH3),
1.18 (m, 6H, CH3), 0.92 (m, 6H, CH3), −19.1 (t, 2JHP = 52.7 Hz, 1H,
FeH). 13C{1H} NMR (125 MHz, CD2Cl2): 53.6 (vt, JCP = 5.7 Hz),
29.3 (vt, JCP = 6.6 Hz), 27.0 (vt, JCP = 9.1 Hz), 25.0 (vt, JCP = 12.0
Hz), 20.7, 20.6 (vt, JCP = 2.4 Hz), 19.1, 18.0 (vt, JCP = 2.1 Hz); CO
resonance was not detected. 31P{1H} NMR (162 MHz, CD2Cl2): 95.4.
IR (cm−1): 3183 (νNH), 1895 (νCO), 1849. UV−vis [THF; λmax, nm (ε,
L mol−1 cm−1)]: 223 (12890), 336 (472), 438 (475).
i
mmol) was dissolved in 5 mL of acetone, and 156 mg of PrPNP (1
equiv, 0.510 mmol) in 5 mL of acetone was added. The pale-yellow
solution was stirred and irradiated with a 150 W xenon short arc lamp
for 150 min at room temperature. The deep-red solution was
evaporated to dryness and the residue washed with 4 × 8 mL pentanes.
The remaining red product was lyophilized from a benzene solution to
obtain 2a as an orange powder. Crystals suitable for X-ray diffraction
were grown by diffusion of pentanes into a saturated THF solution at
room temperature. Yield: 120 mg (0.288 mmol, 56%).
(CyPNP)FeHCl(CO) (5b). To a solution of 87 mg of 1b (1 equiv, 0.14
mmol) in 6 mL of ACN was added 36 mg of nBu4NBH4 (1 equiv, 0.14
mmol) at room temperature. The solution changed from purple to
yellow upon the addition of nBu4NBH4. The reaction mixture was
stirred for 48 h at ambient temperature, after which time the volatiles
were removed in vacuo. The residue was extracted with 3 × 5 mL of
3:1 Et2O/benzene and then cooled to −30 °C. The precipitate was
isolated and washed with pentane to yield 1b as a yellow-orange
powder. Yield: 66 mg (0.11 mmol, 80%).
Anal. Found (calcd) for C18H37FeNO2P2: C, 51.79 (51.81); H, 8.85
(8.94); N, 3.36 (3.36). 1H NMR (500 MHz, acetone-d6): 3.18 (m, 2H,
CH2), 2.35 (m, 2H, CH), 2.23 (m, 2H, CH), 1.98 (m, 4H, CH2), 1.68
(m, 2H, CH2), 1.31 (m, 12H, CH3), 1.21 (m, 12H, CH3); the NH
proton was not detected presumably because of H/D exchange with
the solvent. 13C{1H} NMR (125 MHz, acetone-d6): 226.2 (t, JCP
=
34.4 Hz), 222.4 (t, JCP = 19.5 Hz), 54.7 (vt, JCP = 5.3 Hz), 27.9 (vt, JCP
= 10.5 Hz), 26.4 (vt, JCP = 11.8 Hz), 25.0 (vt, JCP = 5.6 Hz), 19.2, 18.2,
17.0. 31P{1H} NMR (200 MHz, acetone-d6): 109.8. IR (Nujol, cm−1):
3263 (νNH), 1838 (νCO), 1767 (νCO).
Anal. Found (calcd) for C17H38ClFeNOP2: C, 59.52 (59.44), H,
9.34 (9.29); N, 2.44 (2.39). 1H NMR (300 MHz, C6D6): 3.74 (t, 3JHP
= 13.5 Hz, 1H, NH), 3.10 (m, 2H, CH2), 2.71 (m, 4H, CH2), 2.18 (m,
cis- and trans-[(iPrPNP)FeH(CO)2]Cl (4a). A total of 50 mg of 2a (1
2H, CH2), 1.66 (m, 30H, Cy), 1.20 (m, 14H, Cy), −23.64 (t, JHP
=
=
2
equiv, 0.120 mmol) was dissolved in 8 mL of THF, and a solution of
51.9 Hz, 1H, FeH). 13C{1H} NMR (75 MHz, C6D6): 53.8 (vt, JCP
I
dx.doi.org/10.1021/ic402762v | Inorg. Chem. XXXX, XXX, XXX−XXX

Inorganic Chemistry
Article
5.6 Hz), 37.9 (vt, JCP = 9.0 Hz), 36.4 (vt, JCP = 11.1 Hz), 31.1, 30.7,
28.8 (vt, JCP = 3.7 Hz), 27.4 (vt, JCP = 5.3 Hz), 27.2, 26.9, 26.6; CO
resonance was not detected. 31P{1H} NMR (162 MHz, C6D6): 88.6.
IR (cm−1): 3134 (νNH), 1895 (νCO), 1892. UV−vis [THF; λmax, nm (ε,
L mol−1 cm−1)]: 227 (10244), 329 (725), 447 (395).
ACKNOWLEDGMENTS
■
We thank Professor Gary Brudvig for access to his UV−vis
spectrometer and Professor Siegfried Schindler and Jonathan
Becker for access to the Bruker Nonius Kappa CCD
iPr
̈
diffractomer at Justus-Liebig-Universitat Giessen. We gratefully
( PNP)FeH(η1-HBH3)(CO) (6a). To a suspension of 846 mg of 1a (1
acknowledge support from the National Science Foundation
through the Centre for Chemical Innovation “CO2 as a
Sustainable Feedstock for Chemical Commodities” (Grant
CHE-1240020) and from the Deutsche Forschungsgemein-
schaft (Grant SCHN 950/4-1). This work was supported in
part by the facilities and staff of the Yale University Faculty of
Arts and Sciences High Performance Computing Center and by
the National Science Foundation under Grant CNS 08-21132,
which partially funded acquisition of the facilities.
equiv, 1.83 mmol) and 690 mg of NaBH4 (10 equiv, 18.4 mmol) in 5
mL of ACN was added 5 mL of EtOH at room temperature. The
solution changed from purple to yellow upon the addition of EtOH,
and gas evolution was observed. The reaction mixture was stirred for 2
h at ambient temperature, after which time the volatiles were removed
in vacuo. The solid was extracted with 5 × 10 mL of toluene, and the
volatiles were removed under reduced pressure. A total of 5 mL of
benzene was introduced, and the mixture was stirred for 48 h. The
benzene was removed under vacuum, providing 6a as a yellow powder.
Crystals suitable for X-ray diffraction were grown from a saturated
pentane/Et2O solution at −30 °C. Yield: 360 mg (0.888 mmol, 55%).
Anal. Found (calcd) for C17H42BFeNOP2: C, 50.28 (50.40); H,
REFERENCES
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6H, CH3), 1.11 (m, 6H, CH3), 0.90 (m, 6H, CH3), −2.58 (br, 4H,
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3
(2581), 400 (302), 468 (131).
[{(iPrPNP)FeH(CO)}2(μ2,η1:η1-H2BH2)][BPh4] (7a). To 22 mg of 6a (1
equiv, 5.4 μmol) and 24 mg of 2,6-lutidinium tetraphenylborate (1
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Yield: 6.0 mg (4.1 μmol, 75%).
Anal. Found (calcd): C, 62.12 (62.50); H, 8.78 (9.04); N, 2.39
1
(2.51). H NMR (500 MHz, CD2Cl2): 7.38 (br, 8H, BPh4), 7.02 (br,
8H, BPh4), 6.85 (br, 4H, BPh4), 3.85 (br, 4H, CH2), 3.17 (br, 4H,
CH2), 2.74 (br, 2H, NH), 2.38 (br, 4H, CH2), 2.28 (br, 4H, CH), 2.04
(br, 4H, CH2), 1.90 (br, 6H, CH3), 1.58 (br, 4H, CH), 1.49 (br, 6H,
CH3), 1.32 (br, 12H, CH3), 1.21 (br, 12H, CH3), 1.11 (br, 12H, CH3),
2
−6.90 (br, 4H, BH4), −22.0 (t, JHP = 54.5 Hz, 2H, FeH). 31P{1H}
NMR (162 MHz, CD2Cl2): 93.9. IR (cm−1): 3219 (νNH), 2004
(νFe−H−B), 1901 (νCO), 1062 (νBH ). UV−vis [THF; λmax, nm (ε, L
4
(p) Friedrich, A.; Drees, M.; auf der Gunne, J. S.; Schneider, S. J. Am.
̈
mol−1 cm−1)]: 210 (85880), 277 (4101), 446 (641). No 13C NMR
data were collected on this compound because of its low solubility in
all common solvents, except for CD2Cl2, in which it was unstable.
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̈
ASSOCIATED CONTENT
Ed. 2009, 48, 905. (t) Marziale, A. N.; Herdtweck, E.; Eppinger, J.;
Schneider, S. Inorg. Chem. 2009, 48, 3699. (u) Meiners, J.; Friedrich,
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■
S
* Supporting Information
1
Selected H, 31P{1H}, and 2D NMR spectra, X-ray crystallo-
graphic information in CIF format for 1a, 2a, 3a, 4aTrans, 5a, 6a,
and 7a, and details of DFT calculations. This material is
available free of charge via the Internet at http://pubs.acs.org.
Drees, M.; Kass, M.; Herdtweck, E.; Schneider, S. Inorg. Chem. 2010,
̈
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Herdtweck, E.; Holthausen, M.; Schneider, S. Nat. Chem. 2011, 3, 532.
(y) Meiners, J.; Scheibel, M. G.; Lemee-Cailleau, M.-H.; Mason, S. A.;
Boeddinghaus, M. B.; Faessler, T. F.; Herdtweck, E.; Khusniyarov, M.
M.; Schneider, S. Angew. Chem., Int. Ed. 2011, 50, 8184. (z) Scheibel,
M. G.; Askevold, B.; Heinemann, F. W.; Reijerse, E. J.; de Bruin, B.;
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AUTHOR INFORMATION
Corresponding Authors
*E-mail: nilay.hazari@yale.edu.
*E-mail:sven.schneider@chemie.uni-goettingen.de.
■
Author Contributions
‡These authors made equal contributions.
Friedrich, A.; Klopsch, I.; Drees, M.; Celinski, V. R.; auf der Gunne, J.
̈
Notes
S.; Schneider, S. J. Am. Chem. Soc. 2013, 135, 13342. (ac) Scheibel, M.
The authors declare no competing financial interest.
G.; Wu, Y.; Stuckl, A. C.; Krause, L.; Carl, E.; Stalke, D.; de Bruin, B.;
̈
J
dx.doi.org/10.1021/ic402762v | Inorg. Chem. XXXX, XXX, XXX−XXX

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