Trialkylborane-assisted CO2 reduction by late transition metal hydrides

Article abstract of DOI:10.1021/om200364w

Trialkylborane additives promote reduction of CO₂ to formate by bis(diphosphine) Ni(II) and Rh(III) hydride complexes. The late transition metal hydrides, which can be formed from dihydrogen, transfer hydride to CO ₂ to give a formate-borane adduct. The borane must be of appropriate Lewis acidity: weaker acids do not show significant hydride transfer enhancement, while stronger acids abstract hydride without CO₂ reduction. The mechanism likely involves a pre-equilibrium hydride transfer followed by formation of a stabilizing formate-borane adduct.

Full text of DOI:10.1021/om200364w

ARTICLE
pubs.acs.org/Organometallics
Trialkylborane-Assisted CO2 Reduction by Late Transition
Metal Hydrides
Alexander J. M. Miller, Jay A. Labinger,* and John E. Bercaw*
Arnold and Mabel Beckman Laboratories of Chemical Synthesis, California Institute of Technology, Pasadena, California 91125,
United States
S Supporting Information
b
ABSTRACT: Trialkylborane additives promote reduction of CO2
to formate by bis(diphosphine) Ni(II) and Rh(III) hydride com-
plexes. The late transition metal hydrides, which can be formed from
dihydrogen, transfer hydride to CO2 to give a formateÀborane
adduct. The borane must be of appropriate Lewis acidity: weaker
acids do not show significant hydride transfer enhancement, while
stronger acids abstract hydride without CO2 reduction. The mechanism likely involves a pre-equilibrium hydride transfer followed by
formation of a stabilizing formateÀborane adduct.
’ INTRODUCTION
We report here that the late transition metal hydrides, as well
as the partially reduced metal carbonyl components of our CO
reductive coupling system, are able to reduce CO2 to formate,
with Lewis acidic trialkylboranes playing a key role. Although no
catalysis has yet been achieved, the formateÀborane adducts
obtained appear to be considerably less strongly bound than in
the above-discussed systems, suggesting that this may be a prom-
ising new approach to CO2 reduction.
Efficient catalytic conversion of CO2 to fuels and chemicals
could be a major contributor toward achieving carbon neutrality.1
We have recently reported (stoichiometric) reactions relevant to
conversion of syngas to organic products, making use of a com-
bination of a metal carbonyl complex, a nucleophilic late transition
metal hydride, and an intramolecularly appended Lewis acid.2 Be-
cause some syngas conversion catalysts are known to convert CO2
as well—for example, the common CuO/ZnO/Al2O3 catalyst can
effectively convert a mixture of H2, CO2, and CO to methanol3—
we thought it might be worthwhile to examine the chemistry of our
CO-reducing systems with CO2.
The two main approaches to CO2 reduction currently under
consideration are electrocatalytic reduction,1a in which protons
and electrons are added sequentially (and/or concertedly), and
direct hydrogenation.1b,c Most of the electrocatalytic systems
operate at quite reducing potentials to generate CO and H2O,
while hydrogenation (under forcing pressures) more commonly
produces formic acid (Scheme 1). Lewis (particularly those based
on alkali and alkaline earth metals) and Brønsted acids have shown
promise in improving electrocatalytic CO2 reduction, notably
with low-valent Fe porphyrins.4 Bimetallic catalysts, including
the active site of the enzyme [NiFe] CO dehydrogenase, appear
to function by having one metal bound to C while the other acts
as a Lewis acid to bind O.5 Lewis acids such as AlOx and TiOx
appear to play an important role in heterogeneous catalysts that
convert CO2 (and CO) to CH4.6
’ RESULTS AND DISCUSSION
The Re carbonyl cation [(Ph2P(CH2)2B(C8H14))2Re(CO)4]-
[BF4] ([1][BF4]), bearing pendent alkylboranes in the secondary
coordination sphere of the metal, reacts with [HPt(dmpe)2][PF6]
(dmpe = 1,2-bis(dimethylphosphino)ethane), but not with the
analogous Ni hydride, to give boroxycarbene 2 (Scheme 2).2a
(Complex 2 can also be prepared by reduction of 1 with Na-
HBEt3.) Similarly, DuBois has found that CO2 is reduced to
[HCO2]À by [HPt(dmpe)2][PF6], whereas [Bu4N][HCO2]
transfers hydride to [Ni(dmpe)2]2+ to yield [HNi(dmpe)2]+
(Scheme 3).11 The hydride donor strengths (ΔGHÀ; smaller
values correspond to stronger hydride donors) of [HPt(dmpe)2]+,
[HNi(dmpe)2]+, and [HCO2]À have been determined to be
42.5, 50.9, and 44.2 kcal molÀ1 respectively12 (the last value is
3
estimated from the observation that [HCO2]À has a ΔGHÀ
similar to that of [HPt(depe)2]+ (depe = 1,2-bis(diethylphos-
phino)ethane),11 the ΔGHÀ of which was recalculated from the
originally published value12a using DuBois’ more recent pKa
value12c).
Several examples involving boron compounds have also been
reported. The conversion of a diboronyl BÀB7 or secondary
borane BÀH8 bond to a BÀO bond helps drive CO2 reduction
by homogeneous Cu- and Ni-based catalysts, respectively. Acti-
vation of dihydrogen by “frustrated Lewis pairs” can also lead to
reduction of CO2; products include methanol (after hydrolysis).9
All of these reactions are stoichiometric in boron; catalysis is
precluded by the difficulty of cleaving the strong BÀO bonds,
unless strong SiÀO bonds are formed using silane additives.10
Boroxycarbene 2 can serve as a hydride source, releasing H2
upon treatment with water or weak acids,2d but the above results
show that it is intermediate in hydride strength between
[HNi(dmpe)2][PF6] and [HPt(dmpe)2][PF6]; is it strong en-
ough to reduce CO2? Admission of 1 atm of CO2 to a thoroughly
Received: May 2, 2011
Published: July 18, 2011
r
2011 American Chemical Society
4308
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ARTICLE
Scheme 1
Scheme 4
Scheme 2
this is due to formation of an oligomeric species [1 (HCO2)]n,
3
with ÀBÀOC(H)OÀBÀ linkages. Similar behavior has been
observed for some of the CO reduction products studied pre-
viously.2d
The observation that 2 reacts with CO2 to yield [1 (HCO2)]
3
does not necessarily indicate that 2 is a stronger hydride donor
than [HCO2]À, since the BÀO interaction in 1 (HCO2) (and
3
the two BÀO interactions in [1 (HCO2)]n) presumably afford-
3
(s) additional stabilization. Similarly, although transfer of hydride
from [HNi(dmpe)2]+ to CO2 should be uphill by ∼7 kcal molÀ1
,
3
Scheme 3
addition of CO2 to a mixture of [HNi(dmpe)2][PF6] and [1]-
[BF4] produced significant amounts of 1 (HCO2) over 24 h at
3
room temperature. This reaction did not proceed to completion,
as evidenced by the presence of unreacted [HNi(dmpe)2]+; the
chemical shifts for the (single) remaining Re-containing species
were intermediate between those for [1]+ and 1 (HCO2), sug-
3
gesting an equilibrium between these species. (No boroxycar-
bene 2 was observed.) The precipitate that again formed over
time could be partially dissolved by addition of pyridine; the
degassed solution of 2 (formed in situ from [1][BF4] and Na-
1
1
HBEt3 in C6D5Cl) led after a few minutes to a new H NMR
resulting solution showed a slightly shifted H NMR signal for
resonance at δ 8.44. 31P NMR showed complete consumption of
2 and formation of a new species with a single signal whose
chemical shift was similar to that for [1]+; IR spectroscopy in-
dicated a [trans-L2Re(CO)4]+ substructure (a single strong stretch at
1993 cmÀ1) as well as a reduced CdO functionality (1620 cmÀ1).
These data are consistent with hydride transfer from 2 to CO2,
the formate group (δ 8.88) and two 31P NMR signals (δ 1.95 d,
2.98 d, JPP = 77 Hz), consistent with formation of the asymmetric
pyridine adduct 1 (HCO2)(C5H5N) (Scheme 5).
3
Similar chemistry is promoted by a simple trialkylborane, which
could imply that Re may simply be a spectator in the reaction
involving [1]+: when [HNi(dmpe)2][PF6] was allowed to react
t
giving 1 (HCO2) (Scheme 4); the same species could be ob-
with CO2 (1 atm) in the presence of Bu(CH2)2B(C8H14) in
3
tained by addition of [Bu4N][HCO2] to [1][BF4] in C6D5Cl.
The apparent symmetry exhibited by the NMR spectra suggests
the operation of a fluxional process that exchanges formate between
boranes, likely via reversible oligomerization (Scheme 4). After
about an hour, large amounts of precipitate formed along with
C6D5Cl, over a few hours a new 1H NMR resonance at δ 8.73
grew in, the hydride resonance of [HNi(dmpe)2]+ diminished,
and [Ni(dmpe)2][PF6]2 precipitated. The reaction did not go to
completion; the ultimate yield of formate (assessed by integra-
tion of NMR spectra) was about 50%. As the reaction proceeded,
the 1H NMR peak attributed to formate gradually shifted upfield
disappearance of the NMR signals assigned to 1 (HCO2); probably
3
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Scheme 5
Scheme 6
less robust, as might be expected for less acidic or more sterically
crowded Lewis acids. Triphenylborane did give substantial con-
version to formate, but the NMR spectral data indicated forma-
tion of unidentified side products as well. The much stronger acid
B(C6F5)3 exhibited only hydride transfer from Ni to B and no
CO2 reduction.
The results for the trialkylborane, above, clearly indicate for-
mation of a formateÀborane adduct (Scheme 6). To further probe
t
this interaction, aliquots of Bu(CH2)2B(C8H14) were added se-
quentially to a C6D5Cl solution of formate. Upon addition of borane,
a second [HCO2]À signal appeared upfield of the original signal
for free formate; the new signal increased in intensity, while the
first decreased correspondingly, and both signals broadened and
shifted upfield as more borane was added, up to one equivalent.
At and beyond one equivalent of borane, only a single sharp re-
sonance was observed, which shifted still further upfield as more
borane was added. Addition of 10 equivalents of pyridine caused
the peak to shift back to approximately the same position observed
after addition of one equivalent of borane, along with substantial
broadening. (Spectra are shown in the SI, Figure S15.) These
observations appear most consistent with formation of a strong
monoborane adduct, [HCO2BR3]À, which does not exchange with
free [HCO2]À on the NMR time scale, and a weaker bis(borane)
adduct, [HCO2(BR3)2]À, which does rapidly exchange with the
mono adduct; only the latter interaction is cleaved by addition of
pyridine. This model does not fully explain the NMR behavior,
particularly the changing peak shifts below one equivalent of
added borane, but we have observed that other factors (such as
counterion speciation and precipitation) can have an effect on
NMR shifts (the [Bu4N]+ resonances also shift with added borane
in the above experiment), which could account for these details.
In the absence of any borane, the reaction of [HNi(dmpe)2]-
[PF6] with 1 atm of CO2 gave only about 2% formate product;
with borane and the addition of tetraheptylammonium bromide
it proceeded to completion, accompanied by precipitation of [Ni-
(dmpe)2][Br]2. Under the latter conditions the formate 1H NMR
signal (δ 8.79) is close to the shift observed for the stoichiometric
combination of formate and borane (δ 8.89).
Figure 1. 11B NMR spectra of a mixture of [HNi(dmpe)2][PF6] and
tBu(CH2)2B(C8H14) in C6D5Cl before CO2 addition (red), 2 h after
addition of CO2 (1 atm) (green), and after 18 h (blue).
(δ 8.73 at 2 h, 8.66 at 18 h), while that for the tert-butyl group of
the borane shifted downfield (δ 0.89 before reaction, 0.95 at 2 h,
0.97 at 18 h). Concurrently the 11B NMR signal shifted upfield
(δ 88.2 before reaction, 65 at 2 h, 51 at 18 h) and broadened con-
siderably (Figure 1). Addition of one equivalent of tBu(CH2)2-
1
B(C8H14) to [Bu4N][HCO2] in C6D5Cl shifted the H NMR
resonance for [HCO2]À from δ 9.58 to δ 8.89, consistent with
some formateÀborane interaction.
In an attempt to eliminate some of these complications, we
investigated CO2 reduction in acetonitrile, in which all of the
constituents are soluble (although there was a concern that MeCN
would bind the borane too tightly to permit any acid assistance).
Reaction of [HNi(dmpe)2][PF6] with CO2 and no added borane
led to ∼5% conversion to [Ni(dmpe)2]2+ and [HCO2]À (δ 8.40;
cf. [Bu4N][HCO2] δ 8.68), while addition of a single equivalent
of tBu(CH2)2B(C8H14) gave 60% conversion to [HCO2(BR3)n]À
(δ 8.29), and 10 equivalents of borane effected essentially com-
plete conversion (δ 8.22). Addition of one equivalent of [Bu4N]-
[HCO2] at the end of the last reaction resulted in approximately
Several other boranes, of varying Lewis acidity, were also ex-
amined. Addition of CO2 to a mixture of isopropyl pinacol borane
and [HNi(dmpe)2]+ did not significantly increase the amount of
formate produced relative to the reaction in the absence of any
Lewis acid, although the small 1H NMR signal for [HCO2]À was
shifted upfield (δ 8.74 vs 8.84 without borane). Trimesitylborane
also failed to effect significant CO2 reduction, but produced a larger
upfield shift (δ 8.63), quite similar to that in the trialkylborane reac-
tions. It appears that these formateÀborane adducts are considerably
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doubling the peak intensity with a negligible change in position;
strong adduct formation with the borane and/or nucleophilic
attack at CO2. When a mixture of [Ni(dmpe)2]2+, 5 equiv of
NEt3, and 5 equiv of Bu(CH2)2B(C8H14) in CD3CN was ex-
when the reaction was carried out with one equivalent of 13CO2,
1
the H NMR signal at δ 8.21 appeared as a doublet (1JCH
=
t
202 Hz) and a new intense 13C{1H} NMR signal appeared at
δ 174.16. These findings establish conclusively that the signal
around δ 8.2 is indeed due to formate generated by reduction of
CO2. The 11B NMR resonance of the free borane in CD3CN is
far upfield from that in C6D5Cl, consistent with formation of a
CD3CN adduct; that must be weaker than the formateÀborane
adduct, however, since the 11B NMR resonance shifts further
upfield (by ∼3 ppm) as formate is produced.
posed to H2/CO2 (1 atm of a 1:1 mixture), slow conversion to
small amounts of formate (∼8% relative to Ni) was observed
over 3 days. The slow reaction is due (at least in part) to slow
formation of [HNi(dmpe)2]+ under these conditions: a solution
of [Ni(dmpe)2][PF6]2 and NEt3 (4 equiv) in CD3CN under 1
atm of H2 was only 30% converted to [HNi(dmpe)2][PF6] after
3 days.
In contrast, the reaction of [Ni(dmpe)2][BArF ] (BArF
=
4 2
4
In principle reduction of CO2 by H2 could be made catalytic in
nickel, by employing a suitable base in concert with [Ni(dm-
pe)2]2+ to cleave H2,12c followed by hydride delivery to CO2
(Scheme 7). The base must be of sufficient steric bulk to inhibit
tetrakis(3,5-trifluoromethylphenyl)borate) and NEt3 with H2
proceeded far faster in C6D5Cl, with high conversion to [HNi-
(dmpe)2]+ in 3 h and full conversion after 18 h. We ascribe the
difference to coordination of solvent (Scheme 8): the adduct
[Ni(dmpe)2(MeCN)]2+ has been structurally characterized, and
its formation constant was estimated by electrochemical techni-
ques as Keq = 0.3, whereas in chlorobenzene [Ni(dmpe)2]2+
would be present as the four-coordinate square-planar complex
(whose structure has also been determined).12a Counteranion
Scheme 7
effects appear to be unimportant: [Ni(dmpe)2][BArF ] reacts at
4 2
roughly the same rate as [Ni(dmpe)2][PF6]2 with NEt3 under
H2 in CD3CN.
Disappointingly, a solution of [Ni(dmpe)2][BArF4]2,
tBu(CH2)2B(C8H14), and NEt3 under H2/CO2 in C6D5Cl did
not produce any detectable formate, despite the steady growth of
[HNi(dmpe)2]+ over a few days. It is unclear why no formate is
generated. Reactions in CD2Cl2 led to formation of CD2HCl,
indicating a hydride transfer side reaction.
Reduction of CO2 with H2 could, however, be achieved with
the rhodium cation [Rh(dmpe)2][OTf], without the need for an
added base, since its H2 oxidative addition product, [H2Rh-
(dmpe)2][OTf], is a hydride donor of strength (ΔGHÀ = 50.4
Scheme 8
kcal mol )
À1 13 similar to that of [HNi(dmpe)2]+. Treatment of
[Rh(dmpe)2][OTf] with H2/CO2 (1 atm of a 1:1 mixture) in
CD3CN led to formation of some [H2Rh(dmpe)2][OTf] but no
formate over 4 days; however, inclusion of tBu(CH2)2B(C8H14)
in the reaction led to the generation of formate (1H NMR signal
at δ 8.24) along with the Rh product of hydride transfer, [HRh-
(dmpe)2(MeCN)]2+, over a few hours (Scheme 9). With one
equivalent of trialkylborane, the yield of formate was ∼25%
(by NMR integration). Some [Rh(dmpe)2]+ remained uncon-
verted during the course of the reaction, consistent with the
unfavorable thermodynamics of H2 oxidative addition (uphill
by 0.44 kcal molÀ1 13
1 atm of H2 is required for complete conversion.
)
and the low (∼0.5 atm) H2 pressure;
Scheme 9
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’ CONCLUSIONS
Reaction of [1][BF4] with [Bu4N][HCO2]. A J-Young NMR tube
was charged with 29.1 mg (0.0276 mmol) of [1][BF4], 7.9 mg
(0.0276 mmol) of [Bu4N][HCO2], and ∼0.6 mL of C6D5Cl. After 15
min, 1H and 31P{1H} NMR spectroscopy showed essentially complete
The late transition metal bis(diphosphine) hydride complexes
[HNi(dmpe)2]+ and [H2Rh(dmpe)2]+ (as well as a rheniumÀ
boroxycarbene complex) are able to reduce carbon dioxide to
formate, with the assistance of a trialkylborane that shifts the
otherwise unfavorable equilibrium by forming a formateÀborane
adduct. Furthermore, H2 can be used directly in these systems to
reduce CO2. As judged by NMR spectroscopy, the formateÀ
borane adduct is relatively weak (in comparison to those generated
in the CO reductions studied previously) and hence might be
broken sufficiently easily to close a catalytic cycle. While overall
catalysis has so far eluded us, the prospects for developing catalytic
systems based on this chemistry appear promising.
conversion to 1 (HCO2). After about 30 min some precipitates were
3
observed, and precipitation of white solids continued over the next 3 h.
At this time, the solution was decanted, and IR spectroscopy showed
resonances that matched the preparation of 1 (HCO2) from CO2; an
3
additional peak at 1660 cmÀ1 is unidentified, however. 1H NMR
(C6D5Cl, 400 MHz): [Bu4N]+ peaks omitted; δ 0.68 (br, 4H), 0.95
(br, 4H), 1.58 (br, 4H), 1.83 (br, 16H), 2.03 (br, 4H), 2.75 (br, 4H),
7.1À7.2 (m, 12H), 7.4 (m, 8H), 8.49 (s, 1H, [HCO2]À). 31P{1H} NMR
(C6D5Cl, 162 MHz): δ 2.4. IR (C6D5Cl): νCO 1993, 1660, 1621 cmÀ1
.
Reaction of [1][BF4] and [HNi(dmpe)2][PF6] with CO2 in C6D5Cl. A
J-Young NMR tube was charged with 24.3 mg (0.0231 mmol) of [1]-
[BF4], 11.6 mg (0.0231 mmol) of [HNi(dmpe)2][PF6], and ∼0.6 mL of
C6D5Cl. The tube was sealed, and initial NMR spectroscopic measure-
ments showed no reaction. One atmosphere of CO2 was added; after
∼20 min some formate was observed, which grew in over a few hours.
During this time precipitates formed, and after about 12 h there was
essentially no formate-containing product in solution. The solids were
collected, washed with CD3CN (to extract [Ni(dmpe)2][PF6]2) and
C6D5Cl, and treated with C6D5Cl containing 3.8 μL (0.0462 mmol,
2 equiv) of pyridine, which dissolved most of the solids. An asymmetric
product was observed by NMR spectroscopy that was assigned as
’ EXPERIMENTAL SECTION
General Considerations. All air- and moisture-sensitive com-
pounds were manipulated using standard vacuum line or Schlenk tech-
niques or in a glovebox under a nitrogen atmosphere. All reactions were
carried out in an inert atmosphere, unless otherwise noted. Under standard
glovebox conditions, petroleum ether, diethyl ether, benzene, toluene,
and tetrahydrofuran were used without purging, such that traces of those
solvents were in the atmosphere, and could be found intermixed in the
solvent bottles. The solvents for air- and moisture-sensitive reactions
were dried over sodium benzophenone ketyl or calcium hydride or
by the method of Grubbs.14 All NMR solvents were purchased from
Cambridge Isotopes Laboratories, Inc. Chlorobenzene-d5 (C6D5Cl) and
dichloromethane-d2 (CD2Cl2) were freezeÀpumpÀthaw degassed three
times before being run through a small column of activated alumina. Tetra-
hydrofuran-d8 (THF-d8) was purchased in a sealed ampule and dried by
passage through activated alumina. Unless noted, other materials were used
as received. [1][BF4],2a 2, [Pt(dmpe)2][PF6]2,15 [HPt(dmpe)2][PF6],15
[Ni(dmpe)2][BF4]2,12a [HNi(dmpe)2][PF6],15 tBu(CH2)2B(C8H14),16
1 (HCO2)(pyridine). 1H NMR (C6D5Cl, 300 MHz): δ 0.44 (br, 2H, Ph2-
3
PCH2CH2BR2), 0.68 (br, 2H, Ph2PCH2CH2BR2), 0.95 (2H, Ph2PCH2-
CH2BR2), 1.09 (2H, Ph2PCH2CH2BR2), 1.34 (6H, Ph2PCH2CH2BR2),
1.5À2.0 (m, 18H, Ph2PCH2CH2BR2), 2.1 (br, 4H, Ph2PCH2CH2BR2),
2.47 (br, 2H, Ph2PCH2CH2BR2), 2.93 (m, 2H, Ph2PCH2CH2BR2), 6.5À
7.5 (m, mixture of Ph2PR, free and bound C6H5N), 8.41 (m, 2H, C6H5N),
8.88 (1H, HCO2). 31P{1H} NMR (C6D5Cl, 121 MHz): δ 1.95 (d, JPP
77 Hz), 2.98 (d, JPP = 76 Hz).
=
CO2 Reduction by Nickel and Boranes in Chlorobenzene.
Reaction of [HNi(dmpe)2][PF6] with CO2. A J-Young NMR tube was
charged with 12.2 mg (0.0242 mmol) of [HNi(dmpe)2][PF6] and
∼0.6 mL of C6D5Cl. The tube was degassed by exposure to vacuum
briefly with gentle shaking, and 1 atm of CO2 was admitted to the tube.
The tube was sealed, shaken well, and monitored by NMR spectroscopy.
A small resonance assigned to formate was observed at δ 8.84, integrat-
ing 1À2% relative to the Ni hydride. No increase in the formate
resonance was observed over 48 h.
[Bu4N][HCO2],17 [Ni(dmpe)2][BArF ] ,2c and [Rh(dmpe)2][OTf]13,18
4 2
were synthesized by literature methods. All other materials were readily
commercially available, and used as received. H and 13C NMR spectra
1
were recorded on Varian Mercury 300 MHz, 400-MR 400 MHz, INOVA
500MHz, orINOVA600MHz spectrometersat roomtemperature, unless
indicated otherwise. Chemical shifts are reported with respect to residual
internal protio solvent for H and 13C{1H} spectra. Other nuclei were
1
referenced to an external standard: H3PO4 (31P), 15% BF3 Et2O/CDCl3
3
(11B), CFCl3 (19F), all at 0 ppm.
t
Reaction of [HNi(dmpe)2][PF6] with Bu(CH2)2B(C8H14) and CO2.
A solution of 6.7 mg (0.0327 mmol) of tBu(CH2)2B(C8H14) in ∼0.6 mL
of C6D5Cl was added to 16.5 mg (0.0327 mmol) of solid [HNi(dm-
pe)2][PF6]. Thereaction mixture was transferredtoa J-Young NMR tube,
and initial spectroscopic measurements were made. After two free-
zeÀpumpÀthaw cycles, 1 atm of CO2 was admitted to the tube, and
the reaction was monitored by NMR spectroscopy. After 24 h the re-
action had reached partial conversion (with the formate resonance shifting
from δ 8.73 to 8.66), which did not change over 4 days. Addition of
∼16.0 mg (0.0327 mmol, 1 equiv nominal; about 2 equiv by NMR
integration) of [hept4N][Br] led to significant further growth of
[hept4N][HCO2(BR3)n], which (along with excess [hept4N][Br]) was
the only soluble product (all hydride was consumed). The spectra agreed
well with independently synthesized [Bu4N][HCO2(BR3)n] (see below).
1H NMR (C6D5Cl, 400 MHz): δ 0.78 (m, 2H, tBuCH2CH2B(C8H14)),
0.88 (t, J = 6.8 Hz, [hept4N]+), 1.04 (s, 9H, tBuCH2CH2B(C8H14)), 1.1
(br, 2H, tBuCH2CH2B(C8H14)), 1.2À1.3 (br m, [hept4N]+), 1.39 (m,
’ EXPERIMENTAL PROCEDURES
CO2 Reduction Involving Rhenium Carbonyl Com-
plexes. Reaction of 2 with CO2. A 10 mL vial was charged with
26.4 mg (0.0251 mmol) of [1][BF4] and ∼0.6 mL of C6D5Cl. With
stirring, 25.1 μL (0.0251 mmol) of NaHBEt3 (1.0 M in toluene) was
added dropwise to provide a pale yellow solution. The reaction mixture
was transferred to a J-Young NMR tube, and initial spectroscopic mea-
surements showed clean conversion to boroxycarbene 2. The tube was
placed under vacuum for 1 min with gentle shaking to degas, and 1 atm
of CO2 was then admitted to the tube. NMR spectroscopy after 5 min
showed complete conversion to 1 (HCO2), most of which precipitated
3
overnight. 1H NMR (C6D5Cl, 500 MHz): toluene and BEt3 are omitted,
but overlap with some aliphatic peaks, preventing good integration;
δ 0.69 (br s, 4H), 1.59 (br s, overlapping), 1.84 (br, overlapping), 2.05
(br m, overlapping), 2.73 (br, 4H), 7.41 (br, 12H), 8.45 (s, 1H,
HCO2À). 31P{1H} NMR (C6D5Cl, 121 MHz): δ 2.2. IR (C6D5Cl):
t
t
2H, BuCH2CH2B(C8H14)), 1.5 (br, [hept4N]+), 1.76 (br, 2H, Bu-
CH2CH2B(C8H14)), 1.94 (br, 4H, tBuCH2CH2B(C8H14)), 2.2 (br, 6H,
tBuCH2CH2B(C8H14)),3.11(m,[hept4N]+),8.83(1H,[HCO2(BR3)n]À).
No discernible signals were observed by 11B NMR spectroscopy, presumably
νCO 1993, 1620 cm
of the low solubility of the product.
.
À1 13C NMR spectra could not be acquired because
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Organometallics
ARTICLE
due to broadening and overlapping with the borosilicate glass in the
probe construction.
freezeÀpumpÀthaw degassing twice). The reactions were monitored pe-
riodically by multinuclear NMR spectroscopy until equilibrium was reached
(under 24 h), with conversion at equilibrium estimated by integration.
CO2 without borane. In the absence of trialkylborane, only about 5%
hydride transfer was observed. The only two species observed in solution
were unreacted [HNi(dmpe)2]+ and small amounts of [Ni(dmpe)2]2+.
Reaction of [Bu4N][HCO2] with tBu(CH2)2B(C8H14) in C6D5Cl.
A J-Young NMR tube was charged with 15.8 mg (0.0549 mmol) of
[Bu4N][HCO2], 11.3 mg (0.0549 mmol) of tBu(CH2)2B(C8H14), and
∼0.6 mL of C6D5Cl. NMR spectroscopy revealed a formate resonance
at δ 8.89, well upfield of [Bu4N][HCO2] in the absence of borane
t
One equivalent of Bu(CH2)2B(C8H14) and CO2. When 1 equiv of
1
t
trialkylborane was added, about 65% hydride transfer was observed.
Ten equivalents of tBu(CH2)2B(C8H14) and CO2. When excess trialk-
ylborane was added, nearly quantitative hydride transfer was observed.
Only a trace of unreacted [HNi(dmpe)2]+ was observed.
Reaction of [Ni(dmpe)2][PF6]2 with [Bu4N][HCO2]. A small vial was
charged with 19.7 mg (0.0359 mmol) of [Ni(dmpe)2][PF6]2, and 10.3 mg
(0.0359 mmol), and ∼0.6 mL of CD3CN. As the mixture was stirred, a
color change from yellow to dark orange was observed. The mixture was
transferred to a J-Young NMR tube and monitored. The color faded to a
lighter orange over a few minutes. After 15 min, almost complete con-
version (∼95%) to [HNi(dmpe)2][PF6] was observed, although a slight
excess of [HCO2]À (δ 8.58) was still present.
(δ 9.58). H NMR (C6D5Cl, 500 MHz): δ 0.76 (m, BuCH2CH2B-
(C8tH14), 2H), 0.86 (t, J = 7.3 Hz, N(CH2CH2CH2CH3)4, 12H), 1.04
(s, BuCH2CH2B(C8H14), 9H), 1.25 (q, J = 7.2 Hz, N(CH2CH2-
CH2CH3)4, 8H), 1.4 (m, 10H, N(CH2CH2CH2CH3)4 and tBuCH2C-
H2B(C8H14) overlapping), 1.83 (br, tBuCH2CH2B(C8H14), 2H), 1.97
(br, tBuCH2CH2B(C8H14), 4H), 2.28 (br, tBuCH2CH2B(C8H14), 6H),
3.00 (m, N(CH2CH2CH2CH3)4), 8.89 (s, [HCO2(BR3)n]À, 1H). 13C-
{1H} NMR (C6D5Cl, 126 MHz): δ 13.66, 19.87, 23.91, 26.80, 30.05,
31.35, 33.0 (br), 40.75, 58.66, 168.48. 11B NMR (C6D5Cl, 160 MHz):
δ 2.7.
Titration of [Bu4N][HCO2] with tBu(CH2)2B(C8H14) in C6D5Cl.
A J-Young NMR tube was charged with 22.1 mg (0.0769 mmol) of
[Bu4N][HCO2] and 0.600 mL of C6D5Cl. Initial NMR spectra were
Addition of [Bu4N][HCO2] after Reduction. A 1:10 mixture of [HNi-
(dmpe)2][PF6] and tBu(CH2)2B(C8H14) was treated with CO2 accord-
ing to the general procedure. After the reaction was complete the tube
was brought into a glovebox and 1 equiv of [Bu4N][HCO2] was added
to the tube. The resonance at δ 8.210 roughly doubled in intensity (and
shifted by only 0.003 ppm), thereby confirming that formate is the pro-
duct of CO2 reduction.
t
collected. A 1.0 M solution of Bu(CH2)2B(C8H14) in C6D5Cl was
prepared, and ∼19 μL (∼0.25 equiv) was added by syringe, followed by
collection of NMR spectra. Integration showed that 0.20 equiv was
added. This procedure was repeated so that spectra with 0, 0.2, 0.75, 1.5,
2.4, 3.4, 5.1, and 7.0 equiv of borane (by NMR integration) were
obtained. Spectra are shown in the SI as Figure S15.
General Procedure for Reactions of [HNi(dmpe)2][PF6] with CO2
and Other Boranes. A solution of borane (∼0.03 mmol) in ∼0.6 mL of
C6D5Cl was added to an equimolar amount of solid [HNi(dmpe)2]-
[PF6]. The reaction mixture was transferred to a J-Young NMR tube,
and initial spectroscopic measurements were made. After two freezeÀ
pumpÀthaw cycles, 1 atm of CO2 was admitted to the tube, and the
reaction was monitored by NMR spectroscopy.
t
Reaction of [HNi(dmpe)2]+ and Bu(CH2)2B(C8H14) with 13CO2.
A J-Young NMR tube was charged with 18.9 mg (0.0374 mmol) of
t
[HNi(dmpe)2][PF6], 38.6 mg (0.187 mmol, 5 equiv) of Bu(CH2)2-
B(C8H14), and ∼0.6 mL of CD3CN. After initial NMR spectroscopic
measurements, the tube was subjected to two freezeÀpumpÀthaw
cycles, and 0.0187 mmol (0.5 equiv) of 13CO2 was condensed from a
2.87 mL calibrated gas bulb (11.8 mmHg). About 5% conversion to
[Ni(dmpe)2][PF6]2 had occurred after 30 min, and a small doublet
could be seen by 1H NMR. After 12 h, a large doublet at δ 8.21 (202 Hz)
was visible, consistent with formation of [H13CO2(BR3)n]À.
Attempted Catalytic Reactions. Attempted Catalysis in Acet-
onitrile. A J-Young NMR tube was charged with 5.0 mg (0.0102 mmol,
1 equiv) of [Ni(dmpe)2][BF4]2, 7.1 μL (0.0511 mmol, 5 equiv) of NEt3,
10.5 mg (0.0511 mmol, 5 equiv) of tBu(CH2)2B(C8H14), and ∼0.6 mL
of CD3CN. The tube was subjected to two freezeÀpumpÀthaw cycles,
and 1 atm of a 1:1 H2/CO2 mixture (mixed in a large round bulb on a
vacuum line) was admitted. The reaction was monitored by NMR
spectroscopy, and a small formate peak gradually grew in over 3 days,
along with another product, δ ∼6.8. Heating the tube to 60 °C for ∼24 h
generated visible amounts of [HNi(dmpe)2]+, but also several uniden-
tified products.
Isopropyl Pinacol Borate. The reaction proceeded essentially the
same as that with no borane added. The formate resonance appears be-
tween δ 8.70 and 8.74 during the reaction.
Triphenylborane. Complete disappearance of [HNi(dmpe)2]+ was
observed, along with the appearance of a presumed formate resonance at
δ 8.8 and some unidentified peaks (δ 5À6).
Trimesitylborane. No change in conversion was observed as com-
pared to the reaction without borane. A minor formate resonance was
observed at δ 8.63.
B(C6F5)3. Shortly after mixing B(C6F5)3 and [HNi(dmpe)2][PF6], a
1
mixture of [Ni(dmpe)2]2+ and [HNi(dmpe)2]+ was observed by H
NMR spectroscopy. 19F and 11B NMR showed complete consumption
of B(C6F5)3 and were consistent with formation of a four-coordinate
borate. The observed 11B NMR resonance is slightly downfield from the
expected chemical shift of [HB(C6F5)3]À, and the resonance is broa-
dened beyond being able to observe coupling (probably due to exchange
with some free borane). Even after CO2 addition, no formate was ob-
served after ∼12 h at room temperature. 1H NMR (C6D5Cl, 500 MHz):
δ À14.40 ([HNi(dmpe)2]+), 1.0 (m, [Ni(Me2PCH2CH2PMe2)2]2+),
1.18 (m, [HNi(Me2PCH2CH2PMe2)2]+), 1.28 (m, [Ni(Me2PCH2CH2-
PMe2)2]2+), 1.55 (m, [HNi(Me2PCH2CH2PMe2)2]+). 31P{1H} NMR
(C6D5Cl, 121 MHz): δ 24.3 ([HNi(dmpe)2]+), 43.0 ([Ni(dmpe)2]2+).
Attempted Catalysis in Chlorobenzene. A J-Young NMR tube was
4 2
charged with 35.5 mg (0.0174 mmol, 1 equiv) of [Ni(dmpe)2][BArF ] ,
10.0 μL (0.0695 mmol, 4 equiv) of NEt3, 3.6 mg (0.0174, 1 equiv) of
tBu(CH2)2B(C8H14), and ∼0.6 mL of C6D5Cl. The Ni2+ formed a
yellow oil at the bottom of the tube if it was allowed to settle. The tube
was subjected to two freezeÀpumpÀthaw cycles, and 1 atm of a 1:1
mixture of H2/CO2 (mixed in a large round bulb on a vacuum line) was
admitted to the tube. NMR spectroscopic monitoring showed steady
19F NMR (C6D5Cl, 282 MHz): δ À165.35 (m, 6F), À160.38 (t, JFF
=
generation of [HNi(dmpe)2][BArF ], but no evidence of formate was
4
20.6 Hz, 3F), À134.64 (m, 6F). 11B NMR (C6D5Cl, 160 MHz):
δ À0.48 (br).
observed.
Hydrogen Cleavage Reactions. Hydrogen Cleavage in Acet-
onitrile. A J-Young NMR tube was charged with 32.6 mg (0.0159 mmol)
4 2
CO2 Reductions by Nickel and Boranes in Acetonitrile.
General Procedure for Reactions of [HNi(dmpe)2][PF6] in Acetonitrile. A
J-Young NMR tube was charged with [HNi(dmpe)2][PF6] (∼0.03 mmol),
of [Ni(dmpe)2][BArF ] , 8.9 μL (0.0639 mmol, 4 equiv) of NEt3, and
∼0.6 mL of CD3CN. The tube was subjected to two freezeÀpumpÀ
thaw cycles, and 1 atm of H2 was admitted. The reaction was monitored
by NMR spectroscopy, revealing about 30% conversion to [HNi(dm-
pe)2]+ over 3 days.
t
the appropriate amount of Bu(CH2)2B(C8H14) (0, 1, 10 equiv), and
∼0.6 mL of CD3CN. The tube was sealed, initial NMR measurements
were taken, and the atmosphere was replaced with 1 atm of CO2 (after
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ARTICLE
Hydrogen Cleavage in Chlorobenzene. A J-Young NMR tube was
4 2
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charged with 29.0 mg (0.0140 mmol) of [Ni(dmpe)2][BArF ] , 7.9 μL
(0.0568 mmol, 4 equiv) of NEt3, and ∼0.6 mL of C6D5Cl. The Ni
dication was insoluble and formed an oil at the bottom of the tube. Initial
NMR measurements detected no Ni species. The tube was subjected to
two freezeÀpumpÀthaw cycles, and 1 atm of H2 was admitted. The tube
was sealed and monitored by NMR, which revealed relatively rapid
growth of [HNi(dmpe)2][BArF ]. After 18 h, no insolubles were visible,
4
and a large amount of Ni hydride was present. The two-phase reaction
prevented precise yields or equilibrium measurements.
(7) Laitar, D. S.; Muller, P.; Sadighi, J. P. J. Am. Chem. Soc. 2005,
CO2 Reduction by Rhodium and Boranes in Acetonitrile.
Reaction of [Rh(dmpe)2][OTf] with H2/CO2. A J-Young NMR tube was
charged with 19 mg (0.0344 mmol) of [Rh(dmpe)2][OTf] and ∼0.6 mL
of CD3CN. The tube was placed under 1 atm of a 1:1 mixture of H2 and
CO2, mixed by diffusion in a large round bulb on a vacuum manifold.
The reaction was monitored by multinuclear NMR, which showed
formation of [H2Rh(dmpe)2][OTf], but no more than a trace of for-
mate was observed.
127, 17196.
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Reaction of [Rh(dmpe)2][OTf] with tBu(CH2)2B(C8H14) and H2/CO2.
A J-Young NMR tube was charged with 15.9 mg (0.0288 mmol) of
t
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14, 860.
[Rh(dmpe)2][OTf], 5.9 mg (0.0288 mmol) of Bu(CH2)2B(C8H14),
and ∼0.6 mL of CD3CN. The tube was placed under 1 atm of a 1:1
mixture of H2 and CO2, mixed by diffusion in a large round bulb on a
vacuum manifold. The reaction was monitored by NMR spectroscopy,
which showed growth of signals attributable to [H2Rh(dmpe)2]+ (δÀ10.25,
br d, JPH = 146.4) and eventually [HCO2(BR3)n]À (δ 8.25) and [HRh-
(dmpe)2(MeCN)]2+ (δ À18.57, m).
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’ ASSOCIATED CONTENT
S
Supporting Information. Accompanying NMR spectra
b
Organometallics 1993, 12, 299.
for reactions described in the Experimental Section. This material is
available free of charge via the Internet at http://pubs.acs.org.
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’ AUTHOR INFORMATION
Corresponding Author
*E-mail: jal@caltech.edu; bercaw@caltech.edu.
’ ACKNOWLEDGMENT
This research was generously funded by BP through the
Methane Conversion Cooperative (MC2) Program and by the
Moore Foundation. The Varian 400-MR spectrometer was pur-
chased through NIH grant RR027690.
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