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Ligand-induced substrate steering and reshaping of [Ag2(H)]+ scaffold for selective CO2 extrusion from formic acid


Metalloenzymes preorganize the reaction environment to steer substrate(s) along the required reaction coordinate. Here, we show that phosphine ligands selectively facilitate protonation of binuclear silver hydride cations, [LAg2(H)]+ by optimizing the geometry of the active site. This is a key step in the selective, catalysed extrusion of carbon dioxide from formic acid, HO2CH, with important applications (for example, hydrogen storage). Gas-phase ion-molecule reactions, collision-induced dissociation (CID), infrared and ultraviolet action spectroscopy and computational chemistry link structure to reactivity and mechanism. [Ag2(H)]+ and [Ph3PAg2(H)]+ react with formic acid yielding Lewis adducts, while [(Ph3P)2Ag2(H)]+ is unreactive. Using bis(diphenylphosphino)methane (dppm) reshapes the geometry of the binuclear Ag2(H)+ scaffold, triggering reactivity towards formic acid, to produce [dppmAg2(O2CH)]+ and H2. Decarboxylation of [dppmAg2(O2CH)]+ via CID regenerates [dppmAg2(H)]+. These gas-phase insights inspired variable temperature NMR studies that show CO2 and H2 production at 70 °C from solutions containing dppm, AgBF4, NaO2CH and HO2CH.


Nature uses a number of design principles to create different classes of enzyme catalysts capable of a wide range of chemical transformations of substrates1. A metal ion or metal cluster often has a critical role as a co-factor2. A key concept in enzyme catalysis is the preorganization of the reaction environment by the enzyme, directing the substrate to the reaction site, which provides a favourable geometry for the transition state required for bond activation. In essence, the enzyme steers the substrate along the required reaction coordinate to allow the desired transformation to product(s)3.

The concept of changing the environment at a metal centre to switch on reactivity has also been recently exploited in gold chemistry. Au(I) complexes prefer to be linear, which is why they are unreactive toward oxidative addition of iodobenzene (Fig. 1a). To promote reactivity, ligand-induced preorganization of the metal centre has been shown to accommodate the geometry of the ensuing oxidative addition of aryl halides (Fig. 1b)4. Embedding the metal centre within a ligated nanocluster also facilitates reactivity, which can be further tuned by the choice of ligand (Fig. 1c)5.

Figure 1: Key concepts for switching on reactivity at coinage metal centres.

(a) Linear diphosphine Au(I) complexes do not undergo oxidative addition of iodobenzene. Oxidative addition of iodobenzene does occur for: (b) bisphosphine Au(I) complexes with P–Au–P bond angles of ≈90°; and (c) bisphosphine ligated gold cluster. Switching on desired protonation of binuclear silver hydride cations, [LAg2(H)]+ by formic acid: (d) undesired Lewis adduct formation occurs when silver centres have vacant coordination sites; (e) formic acid is steered to active site by phosphine ligands; (f) bisphosphine ligands reshape geometry of active site to switch on desired protonation reaction.

Here, we use gas-phase experiments and density functional theory (DFT) calculations to examine how the binuclear silver hydride cation, [Ag2(H)]+ (Fig. 1d,f), can be structurally manipulated by the appropriate choice of phosphine ligands6 to switch on the protonation of the hydride by formic acid to liberate hydrogen, which is a key step in the selective, catalysed decomposition of formic acid that does not occur in absence of ligands. We chose [Ag2(H)]+ since it has been spectroscopically characterized7 and ligated variants can readily be formed8,9,10. Formic acid was chosen as a substrate since its decomposition is one of the most widely studied topics in chemistry, with a rich history spanning more than a century11,12,13,14. Apart from the academic interest in establishing the mechanism(s) of decomposition, the selective, catalysed decomposition of formic acid has potentially important applications in areas ranging from hydrogen storage15,16,17 through to the generation of in situ hydrogenation sources for reduction of organic substrates18,19.

In the absence of a catalyst, pyrolysis of formic acid proceeds via two primary pathways: decarboxylation (equation (1)) and dehydration (equation (2)). These reactions are coupled by the water–gas shift reaction (Equation (3))20,21 and have been widely studied experimentally22 and theoretically23. In the gas-phase, the dehydration channel (Equation (2)) is the dominant reaction22, consistent with a lower activation energy, as predicted by DFT calculations23.

The concept of using metal catalysts to selectively decompose formic acid dates back over 100 years to Sabatier’s work on the role of metal and metal oxide catalysts11, and the substantial early literature has been reviewed12,13,14. Over the past century, a wide range of metal catalysts have been surveyed for their potential to selectively decarboxylate formic acid (Equation (1)). The types of metal catalysts examined include metal and metal oxide surfaces14, mononuclear metal complexes24, metal clusters25 and metal nanoparticles26.

The powerful combination of gas-phase ion–molecule reactions (IMRs), collision-induced dissociation (CID), infrared and ultraviolet action spectroscopy and computational chemistry allows us to examine the role of the ligand (L) in promoting decomposition of formic acid catalysed by the binuclear silver hydride cations, [LAg2(H)]+. Guided by the right choice of ligand, we have translated our gas-phase results to achieve the selective condensed-phase decarboxylation of formic acid.


Catalyst systems

The six systems that we have studied to examine the catalytic cycle (Fig. 2a) for decomposition of formic acid are designated by the letters, which identify the ligands as: 1a=no ligand; 1b L=PPh3; 1c L=2 × PPh3; 1d L=bis(diphenylphosphino)methane (dppm); 1e L=1,2-bis(diphenylphosphino)benzene (dppbz); and 1f L=bis(diphenylphosphino)ethane (dppe)). DFT calculations reveal that the ligand(s) can induce changes to the geometry of the Ag2(H)+ scaffold (Fig. 2b).

Figure 2: Role of the ligand in the selective decarboxylation of formic acid catalysed by [LAg2(H)]+.

(a) catalytic cycle, with following steps: (i), decarboxylation of [LAg2(O2CH)]+ via CID to generate [LAg2(H)]+. (ii), IMR of [LAg2(H)]+ to regenerate [LAg2(O2CH)]+. (iii), IMR of [LAg2(H)]+. (iv), CID of [LAg2(H)(HO2CH)]+ to regenerate [LAg2(H)]+. (v), IMR of [LAg2(H)(HO2CH)]+ with HO2CH to yield [LAg2(H)(HO2CH)2]+. (vi), CID of [LAg2(H)(HO2CH)2]+ to regenerate [LAg2(H)(HO2CH)]+. Most stable DFT-calculated structures of systems examined: (b) 1a, 1b, 1c, 1d, 1e and 1f. DFT calculations used the hybrid functional B3LYP53 with def2-TZVP AO basis set54 for all atoms and corresponding relativistic effective core potential for Ag atoms55. Bond distances are given in Å (black) and P–Ag–H bond angles in degrees (red).

Reactions of 1a–1f with formic acid

[Ag2(H)]+ and its ligated variants, [LAg2(H)]+, were prepared in the gas-phase via well-established ligand fragmentation reactions (Supplementary Figs 1–6; Supplementary equations 1 and 2), including decarboxylation of coordinated formates, equation (4) (refs 27, 28). The precursor ions were formed via electrospray ionization (ESI).

1a m/z 215, reacts via sequential addition of formic acid (Supplementary Fig.7a,b; equations (5) and (6); Fig. 2a (iii) and (v)), as confirmed via mass selection of [Ag2(H)(HCOH)]+ m/z 261, and subsequent reaction with formic acid, which yields [Ag2(H)(HO2CH)2]+ m/z 307. CID of [Ag2(H)(HCOH)]+ regenerates 1a via loss of formic acid (Fig. 2b and Supplementary Fig. 7c). These results confirm the concept that formic acid is trapped down the wrong reaction pathway (Fig. 2a (iii)).

We next tested whether ligation could steer the substrate away from coordination to form a Lewis adduct and toward the hydride site. Blocking one Ag site in 1b results in the formation of a mono adduct (equation (5), L=Ph3P, Supplementary Fig. 8b). Kinetic modelling of the temporal profiles of [(Ph3P)nAg2(H)]+ and [(Ph3P)nAg2(H)(HO2CH)2−n]+ (Supplementary Table 1) reveals that: (i) the addition of formic acid for n=0 and 1 is at ≈1% of the collision rate; (ii) in the case of n=0, addition of formic acid is reversible. Blocking both Ag sites makes 1c unreactive toward formic acid (Supplementary Fig. 8a). By replacing both Ph3P ligands with the dppm ligand, the Ag2(H)+ scaffold of 1e is compressed, with the P–Ag–H angle deviating substantially away from linearity. As a consequence [dppmAg2(H)]+ 1d (m/z 601) reacts with formic acid to form [dppmAg2(O2CH)]+ and H2 (equation (7), Fig. 3a), a reaction that proceeds at ≈ 1% of the collision rate (Supplementary Table 1). When [dppmAg2(D)]+ m/z 602, formed via fragmentation of the cluster cation [Ag33-D)dppm3]2+,8 was allowed to react with formic acid, the unlabelled formate [dppmAg2(O2CH)]+ and HD are formed (equation (8) and Supplementary Fig. 9b), which is consistent with a mechanism in which the hydride is protonated by formic acid to release H2. The reactions given by equations (4) and (7) represent those associated with the catalytic cycle (Fig. 2a) for the selective decarboxylation of formic acid (equation (1)). Indeed, sequential reactions of CID of [dppmAg2(O2CH)]+ to form [dppmAg2(H)]+ followed by ion-molecule reaction (IMR) with formic acid, allows completion of the cycle multiple times with no significant loss of signal (Supplementary Fig. 9). The other binuclear silver hydride cations, [LAg2(H)]+, containing bisphosphine ligands also reacted with formic acid to reform the [LAg2(O2CH)]+ and H2 (equation (7) and Fig. 3b,c), although the nature of the ligand influences the reaction efficiencies, which follow the order 1d1e>>1f (Supplementary Table 1).

Figure 3: Ion–molecule reaction of formic acid with mass-selected hydrides, [LAg2(H)]+.

(a) L= dppm, 1d, [HO2CH]ion trap=7.19 × 109 molecules cm−3. (b) L= dppbz, 1e, [HO2CH]ion trap=7.30 × 109 molecules cm−3. (c) L=dppe, 1f, [HO2CH]ion trap=7.09 × 109 molecules cm−3. The most intense peak of the isotope cluster is represented by the m/z value. * Represents the mass selected precursor ion.

IR and UV spectroscopy of reactive intermediates

In order to relate the structure of the proposed reactive intermediates 1d and [dppmAg2(O2CH)]+ to their observed reactivity (Fig. 2a), we next turned our attention to their gas-phase characterization29 using infrared multiple photon dissociation (IRMPD) spectroscopy (Fig. 4a,b)30 and ultraviolet action-spectroscopy (Fig. 4c,d)7,31. For each complex, the experimental IRMPD spectrum is compared against the theoretically predicted infrared absorption spectrum of the lowest energy isomer. In the case of [dppmAg2(H)]+ (m/z 601), infrared features could only be observed if mass-selected ions were irradiated on resonance with the infrared free electron laser (FEL) and in conjunction with an auxiliary CO2 laser32. The enhancement of the spectroscopic resolution was such that relatively weak IRMPD features could be observed (Fig. 4a). In the case of [dppmAg2(O2CH)]+ (m/z 645), however, infrared-induced fragmentation was more easily achieved using the infrared FEL only, and the auxiliary CO2 laser was thus not used.

Figure 4: Experimental (red line) and DFT-calculated (blue line) IRMPD and UV spectra

(hybrid functional B3LYP with Stuttgart relativistic effective core potential for Ag atoms with corresponding def2-TZVP AO basis set, same AO basis set for all other atoms) of (a) [dppmAg2(H)]+, 1d. (b) [dppmAg2(O2CH)]+. A scaling factor of 0.98 was applied to the calculated harmonic frequencies. UV action spectrum (red line) and calculated TDDFT spectrum with dispersion correction D3 (using CAM-B3LYP functional with Stuttgart relativistic effective core potential for Ag atoms with corresponding def2-TZVP AO basis set for all atoms, the black vertical lines correspond to values of oscillator strength frequency fe) for the lowest energy structure of: (c) [dppmAg2(H)]+. (d) [dppmAg2(O2CH)]+. The analysis of leading excitations is in Supplementary Fig. 10.

For both [dppmAg2(H)]+ and [dppmAg2(O2CH)]+, a good match was observed between the experimental and theoretically predicted infrared spectrum for the lowest energy structure. A detailed assignment of the main observed infrared features is provided (Supplementary Table 2). As expected, infrared bands associated with the auxiliary dppm ligand are observed. This is particularly true in the case of the [dppmAg2(H)]+ spectrum where four bands can be assigned to phenyl in plane ring deformation (998 cm−1), CH2 twist and P–C6H5 stretch (1,097 cm−1), phenyl in plane CH bending (1,438 cm−1), and phenyl CH bending and ring deformation (1,478 cm−1).

More importantly, diagnostic bands of the coordination mode of the hydride and formate ligands are also observed. In the case of [dppmAg2(H)]+ (Fig. 4a), the μ2 bridging coordination mode of the hydride is well characterized by two bands associated with the asymmetric and symmetric Ag–H stretching bands observed at 900 and 1,250 cm−1, respectively, in excellent agreement with the theoretical prediction (916 and 1,236 cm−1, respectively). In the case of [dppmAg2(O2CH)]+ (Fig. 4b), it was expected that the positions of the asymmetric and symmetric formate CO stretching bands were sensitive to the formate coordination modes. These two bands are strongly infrared active, and could thus be revealed through IRMPD without the use of the auxiliary CO2 laser. As can be seen in Supplementary Table 2, the observed position of these two bands (1,360 and 1,547 cm−1, respectively) is in excellent agreement with their predicted positions (1,345 and 1,564 cm−1, respectively) for the lowest energy structure of the [dppmAg2(O2CH)]+ complex. It can thus be concluded that IRMPD spectroscopy of [dppmAg2(H)]+ and [dppmAg2(O2CH)]+, in conjunction with electronic structure calculations, provide clear structural diagnostic of the coordination mode within the Ag2H+ or Ag2(O2CH)+ scaffolds.

Comparison of the ultravoilet action spectra and calculated time dependent density functional method (TDDFT) spectra using dispersion correction D3 (ref. 33) for the lowest energy structures for [dppmAg2(H)]+ and [dppmAg2(O2CH)]+ are shown in Fig. 4c,d. Introduction of dispersion correction into TDDFT reduces the distance between two parallel aromatic rings, thus preventing their mobility. In the case of [dppmAg2(H)]+, the experimental spectrum shows an increase in fragmentation yield as the wavelength decreases, with two superimposed bands at 270 and 235 nm (Fig. 4c). The corresponding TDDFT transitions with dominant oscillator strengths are due to leading excitations from HOMO-1 and HOMO to LUMO+2 (Supplementary Fig. 10), respectively. They involve the Ag2H subunit as well as the ligand. In contrast, the S1 and S2 states located close to 300 nm are characterized by HOMO to LUMO and HOMO-1 to LUMO excitations, respectively, in which Ag2 or Ag2HP2 are more involved than ring subunits of the ligand.

In the case of [dppmAg2(O2CH)]+, a similar action spectrum was obtained. The main difference is a pronounced shoulder at 250 nm resulting from an intense S1 transition involving mainly the Ag2HP2 subunit (Supplementary Fig. 10). The formate has little role in the excitations leading to absorption in this spectral region, which explains the similarity between the two optical spectra. Absorption spectra obtained with TDDFT-D3 are in good agreement with the experimental ultraviolet photodissociation (UVPD) spectra, thus confirming the calculated structural properties. Altogether, on the basis of UVPD and IRMPD spectra, the structural assignments of [dppmAg2H]+ and [dppmAg2(O2CH)]+ are unambiguous.

DFT-calculated mechanism of steps associated with the catalytic cycle

The catalytic cycle for the selective decomposition of formic acid involves two distinct types of reactions (Fig. 2a for 1d, Supplementary Fig. 11 for 1e and 1f, Supplementary Table 3 for all systems). The ion–molecule reaction of formic acid with [LAg2(H)]+ to produce [LAg2(O2CH)]+, and H2 must be an exothermic process with barriers that lie below the separated reactants in order for it to occur under the near thermal conditions of the ion-trap34. Indeed, DFT calculations reveal this to be the case, for 1d (Fig. 5 and Supplementary Table 3). The binding energy of cis-formic acid to [dppmAg2(H)]+ is 0.24 eV, and subsequent reaction via H2 formation proceeds via a transition state with barrier of 0.18 eV leading to the formation of [dppmAg2(O2CH)]+, which is exothermic by 0.95 eV. Throughout this reaction, the dppm ligand keeps the Ag2 subunit intact, while allowing the Ag–Ag bond length to relax. The overall exothermicities for this first reaction (step 1) for the other [LAg2(H)]+ complexes examined follow the order L=dppm, (0.95 eV)>L=dppe (0.76 eV)>L=dppbz (0.71 eV)>L=2 × Ph3P (0.68 eV)>L=Ph3P (0.51 eV), which is in qualitative agreement with experimental findings that dihydrogen release (equation (7)) occurs for L=dppm, dppbz and dppe, but not for the other ligands. The corresponding heights of barriers are 1d (0.18 eV)<1f (0.25 eV)<1e (0.36 eV) indicate that all three barriers can overcome under experimental conditions, although the efficiency of the reaction will depend on the height of the barrier. Only in these three cases do the Ag2HP2 subunits remain intact as can be seen from Fig. 1. Analysis of the charge distributions in these [LAg2(H)]+ complexes reveals delocalization of positive charge in this subunit (Supplementary Fig. 12).

Figure 5: DFT-calculated energy profile for the two reaction steps in the catalytic cycle of Fig. 1a.

(Step 1) ion-molecule reaction of formic acid with [dppmAg2(H)]+; (step 2) CID decarboxylation of [dppmAg2(O2CH)]+. Relative energies are in eV.

In contrast, decarboxylation of [LAg2(O2CH)]+ is endothermic as it requires energization through multiple collisions with the helium bath gas during the CID process in order to occur. The mechanism for CO2 release involves two steps. First, the formate needs to change from an O,O-bridging ligand to an O-bound ligand. This involves breaking one of the Ag-O bonds via a barrier of 1.7 eV. The next step involves decarboxylation28, which proceeds over a barrier of 1.86 eV to release of CO2. Altogether, a catalytic cycle involving the selective decomposition of formic acid via the release of H2 and CO2 (Equation (1)) can occur according to calculated energy profile for [dppmAg2(H)]+ (Fig. 5), under experimental conditions involving IMR for the spontaneous release of H2 and activation via CID for the release of CO2. It is to be expected that this is also the case for [dppbzAg2(H)]+ and [dppeAg2(H)]+ since that Ag2H(X)P2 subunit remains intact, although the energetics are slightly less favourable than in the case of [dppmAg2(H)]+ (Supplementary Table 3).

Solution-phase selective decarboxylation of formic acid

The fact that [dppmAg2(O2CH)]+ is both readily decarboxylated in the gas-phase and reformed via the reaction of [dppmAg2(H)]+ with formic acid prompted us to prepare stoichiometrically well-defined solutions in order to use variable temperature 1H and 13C NMR spectroscopy to examine the evolution of the two gaseous products formed in the selective decarboxylation of formic acid (equation (1)). No H2 evolution was observed by 1H NMR when a solution of AgBF4, 13C-labelled formic acid and dppm was heated from 25 to 70 °C (Supplementary Fig. 13). When the experiment was repeated with the addition of sodium formate, no evolution of H2 was observed from 25 to 55 °C (Supplementary Fig. 14). When the temperature was raised to 70 °C, H2 evolution was observed almost instantly (Supplementary Fig. 15). The evolution of both H2 and CO2 were observed to increase over time at 70 °C, and both H2 and CO2 reached a steady-state concentration after 11.5 min (Supplementary Figs 15 and 16).


While concepts of steric and electronic effects are well established in guiding the choice of ligand to modulate the reactivity of mononuclear catalysts in homogenous catalysis35,36, related concepts for choosing ligands to modulate the reactivity of binuclear and cluster catalysts are yet to be fully developed5. The value of gas-phase studies employing mass spectrometry (MS)-based methods37,38 is that they allow a systematic exploration of the factors that control reactivity for all steps in a catalytic cycle39,40. When used in conjunction with DFT calculations, where mechanistic pathways can be explored, different types of catalysts that vary in the metal, ligand and/or nuclearity that catalyse the same transformation41 or which transform the same substrate in different ways42 can be directly compared43.

Here, we have shown that ligand choice is a crucial factor in designing a binuclear silver hydride cluster that catalyses the selective decarboxylation of formic acid. Ligation of the Ag2(H)+ scaffold clearly has an influence on its geometry by shortening the Ag–Ag distance and increasing the Ag–H distance (Fig. 1). In the absence of bidentate bridging ligands, the reactivity pattern of 1a, 1b and 1c towards formic acid is consistent with simple Lewis acid/base interactions in which the number of vacant coordination sites in [(Ph3P)nAg2(H)]+ dictates how many formic acid molecules can coordinate via the O atom of the C=O to form the adducts [(Ph3P)nAg2(H)(HO2CH)2−n]+. Indeed DFT calculations reveal that this coordination mode yields the most stable adducts for n=0 and 1, while in the case of n=2 only a weakly bound ion–molecule complex is formed (Supplementary Fig. 17) and this is likely to simply dissociate back to separated reactants, which is why no adduct is observed experimentally. In contrast, the tight-bite angles of the bidentate bridging ligands dppm, dppbz and dppe switch on the protonation of the silver hydride in step 1 (Fig. 5) by providing an appropriate geometry to weaken the Ag–H bonds and bend the P–Ag–H away from linearity, thereby allowing coordination of formic acid and subsequent reaction between the coordinated moieties Ag(OCH(OH) and Ag(H). The ligand further tunes the reactivity as highlighted by both the experimentally determined reaction efficiencies, which follow the order 1d1e>>1f and the DFT-calculated barrier heights for reaction with cis-formic acid (Supplementary Fig. 18) to release H2, which follow the order 1d (0.18 eV)<1f (0. 25 eV)<1e (0.36 eV). The ligand also exerts an effect in step 2, with energy resolved CID experiments (Supplementary Fig. 5) providing reactivity orders for the ease of decarboxylation that are in agreement with the DFT-calculated barrier heights: [dppeAg2(O2CH)]+ (1.64 eV)≈[dppbzAg2(O2CH)]+ (1.65 eV)<[dppmAg2(O2CH)]+ (1.86 eV).

Finally, the gas-phase results encouraged us to examine related selective decarboxylation reactions in solution44,45. We found that both H2 and 13CO2 are evolved when a stoichiometrically well-defined solution containing dppm, AgBF4, 13C-labelled formic acid and sodium formate was warmed to 70 °C. While the precise nature of the reactive species in solution is unknown, previous studies have shown that: (i) related dppm complexes of silver carboxylates exist as dimers in solution46,47; (ii) the related silver hydride [(NHC)2Ag2(H)]+ (where, NHC=1,3-bis(2,6-diisopropylphenyl)imidazolin-2-ylidene) exists in solution and reacts with CO2 to form [(NHC)2Ag2(O2CH)]+, a reaction that is the reverse of decarboxylation of a coordinated formate ligand (equation (4)) studied here48.

Two key concepts have emerged from this work: (i) that ligands can have a vital role in reshaping the scaffold of a metal cluster to activate its reactivity towards a substrate; and (ii) that fundamental gas-phase studies can be used to direct the search for new types of metal complexes that promote related reactivity in solution49. Together these concepts have allowed us to achieve the selective extrusion of carbon dioxide from formic acid, an important process for applications in hydrogen storage15,16,17.



Chemicals listed in the Supplementary information were used as received.

Preparation of silver complexes for MS analysis

In situ silver precursor complexes for ESI/MS were typically generated by adding 20 mmol AgX (X=NO3 or BF4) followed by 10 mmol of phosphine ligand, L (L=PPh3, dppm, dppbz or dppe), to 20 ml of freshly prepared solvent mixtures in a 50 ml Quickfit round-bottom flask covered in foil and equipped with a glass stopper and magnetic stir bar. The solution was stirred for at least 5 min and 10 mmol of sodium formate was added. MS experiments were conducted immediately after the addition of sodium formate.

Gas-phase studies using CID and IMR

Gas-phase experiments on phosphine ligated silver formate clusters were carried out using a Finnigan hybrid linear quadrupole Fourier transform ion-cyclotron resonance mass spectrometer. The silver complexes prepared above were typically diluted in methanol or acetonitrile to a final silver(I) concentration of 50 μM and at least 1.0 ml. The diluted solution was drawn into a 500 μl gas tight borosilicate glass syringe with polytetrafluoroethylene (PTFE) plunger tips and injected into the Finnigan ESI source at a flow rate of 3–5 μl min−1. ESI source conditions to yield a stable current of 0.5 μA were: needle potential (3.5–5.0 kV); nitrogen sheath gas pressure (5–10 a.u.). The ion transfer capillary temperature was set to 250 °C. Voltages were: tube lens (≈20.0 V) and capillary voltage (10.0 V). The unimolecular fragmentation/dissociation of mass-selected precursor silver complexes occurred via CID using a normalized collision energy typically between 20 and 25%, and an activation time of 30 ms. IMR were carried by injecting formic acid into the helium bath gas5. The stoichiometry of all ions was confirmed by high-resolution MS experiments (Supplementary Table 4).

Energy-resolved CID experiments

Energy-resolved CID experiments were carried out using a Finnigan 3D ion trap (LCQ) mass spectrometer. The method of Brodbelt was adapted and details are given in the Supplementary methods (see text associated with Supplementary Fig. 4)50. The activation voltage was determined by Supplementary equation 3.

MS for IR action spectroscopy

Infrared spectroscopy of mass-selected ions in the 800–1,600 cm−1 range was performed using a 7 Tesla Fourier transform ion cyclotron resonance tandem mass spectrometer (Bruker Apex IV Qe)51 equipped with an ESI source and coupled to the infrared FEL beam line of CLIO52. This IR FEL delivers 10 μs long trains of picosecond pulses at 25 Hz. Ions of interest were accumulated and trapped in a 5 cm long hexapole ion-trap pressurized with argon. The trapping delay (500 ms) allows for an efficient collisional cooling of the ions. Ions are then pulse extracted to the ICR cell where they are mass-selected, and then irradiated for 1 s. Upon resonant vibrational excitation, dissociation of the selected ion can be monitored via its fragment peaks.

A significant enhancement of the photofragmentation yield can be observed using an auxiliary CO2 laser (10 W continuous wave, BFi OPTiLAS, France)32. For this purpose, a train of CO2 pulses at 25 Hz is generated and synchronized with the IR FEL laser with a retarding delay being on the order of 1 μs. This auxiliary CO2 laser was used in the case of [dppmAg2(H)]+ (m/z 601), and the CO2 laser pulse length (25 ms) was adjusted to avoid CO2 induced dissociation.

The experimental IRMPD bandwidth (fwhm) for both [dppmAg2(H)]+ and [dppmAg2(O2CH)]+ is on the order of 20 cm−1, as generally observed for IRMPD spectra of other systems obtained using the CLIO FEL.

MS for ultravoilet action spectroscopy

For ultravoilet action spectroscopy, a dual linear ion trap (LTQ-VELOS, ThermoScientific) was used to generate, mass select and trap ions in a first, high-pressure ion trap, for a controlled duration. During ion trapping, ions can be activated and fragmented by photons or CID. Fragment ions are transmitted to a second ion trap, with low pressure, where they are mass analyzed. A fused-silica window is positioned at the back end of the instrument allowing for the introduction of laser beams in the ultravoilet-visible range along the ion trap axis. Ultravoilet light was generated by doubling the output of an optical parametric oscillator (Horizon optical parametric oscillator pumped by the third harmonic of a Surelite II Nd:YAG laser, Continuum). A mechanical shutter, synchronized with the mass spectrometer, is used to stop the beam at all times except the ‘ion activation window’—that is the time after ion accumulation and before the mass analysis. A single laser pulse was used for the irradiation of the trapped ions and when irradiating ions the normalized collision energy is kept at zero. The fragmentation yield (FY) is given by equation (9).

P and F are the intensities on the mass spectrum for respectively the parent ion and the ensemble of photo-fragment ions. λ and Pw are respectively the wavelength and measured average power of the incoming ultravoilet laser beam.

DFT calculations

The extensive search for lowest energy structures and transitions states were performed by the hybrid B3LYP53 functional with def2-TZVP atomic basis set54, which has been used for all atoms. Silver atoms have been treated by Stuttgart relativistic effective core potential with corresponding atomic orbital (AO) basis set55. The same combination of functional and basis set was used for calculation of the infrared spectra, which were scaled by 0.98 to match experimental data. The IR spectrum for neutral monomeric cis-formic acid calculated at this level of DFT theory is also in good agreement with experimental data (Supplementary Fig. 19). For calculations of the absorption spectra TDDFT with the long-range corrected version of the hybrid B3LYP functional, the Coulomb-attenuated CAM-B3LYP functional and TZVP AO basis set has been employed.

Potential interactions between the aromatic rings of dppm, raises the question of whether the dispersion correction within DFT are required. We have tested the influence of dispersion correction on the structural and spectroscopic properties of [dppmAg2H]+ and [dppmAg2(O2CH)]+ complexes by introducing D3 into DFT and TDDFT33. Comparison of the measured and calculated infrared spectra suggest that dispersion corrections has no influence. In contrast, the absorption transitions calculated using the D3 correction in which aromatic rings are involved are only slightly blue shifted, thus improving agreement with the experimental UVPD spectra. Finally, the energy profile shown in Fig. 5 is almost unchanged when single point B3LYP-D3 energy calculations are carried out for each reaction step of the catalytic cycle (Supplementary Table 3).

NMR spectroscopy experiments

The NMR experiments were performed on a Bruker Avance Av500 NMR spectrometer (500.13 MHz 1H frequency) equipped with a 5 mm triple resonance CryoProbe Prodigy probe (1H/19F–2H/13C/15N). Solutions for analysis by NMR were prepared by dissolving: (1) solution A: AgBF4 (195 mg, 1 mmol), dppm (192 mg, 0.5 mmol), 13C formic acid (24 mg, 0.5 mmol) and sodium formate (34 mg, 0.5 mmol) in 1 ml of deuteroacetonitrile; (2) solution B: same as solution A, but without sodium formate added. NMR experiments were performed with the sample held at temperatures between +25 °C and +70 °C (±0.1 °C). Chemical shifts for 1H experiments are referenced to the residual protonated solvent signal (CD2HCN, δ 1.94 ppm); 13C referenced to the solvent signal (CD3CN, δ 1.39 ppm). One-dimensional NMR experiments were acquired using standard Bruker library pulse sequences.

Data availability

The data that support the findings of this study are available from the corresponding author upon request.

Additional information

How to cite this article: Zavras, A. et al. Ligand-induced substrate steering and reshaping of [Ag2(H)]+ scaffold for selective CO2 extrusion from formic acid. Nat. Commun. 7:11746 doi: 10.1038/ncomms11746 (2016).


  1. 1

    Menger, F. M. An alternative view of enzyme catalysis. Pure Appl. Chem. 77, 1873–1886 (2005).

    CAS  Article  Google Scholar 

  2. 2

    Valdez, C. E., Smith, Q. A., Nechay, M. R. & Alexandrova, A. N. Mysteries of metals in metalloenzymes. Acc. Chem. Res. 47, 3110–3117 (2014).

    CAS  Article  Google Scholar 

  3. 3

    Cannon, W. R., Singleton, S. F. & Benkovic, S. J. A perspective on biological catalysis. Nat. Struct. Biol. 3, 821–833 (1996).

    CAS  Article  Google Scholar 

  4. 4

    Joost, M. et al. Facile Oxidative addition of aryl iodides to gold(I) by ligand design: bending turns on reactivity. J. Am. Chem. Soc. 136, 14654–14657 (2014).

    CAS  Article  Google Scholar 

  5. 5

    Robinson, P. S. D., Khairallah, G. N., da Silva, G., Lioe, H. & O’Hair, R. A. J. Gold mediated C–I bond activation of iodobenzene. Angew Chem. Int. Ed. 51, 3812–3817 (2012).

    CAS  Article  Google Scholar 

  6. 6

    Meijboom, R., Bowen, R. J. & Berners-Price, S. J. Coordination complexes of silver(I) with tertiary phosphine and related ligands. Coord. Chem. Rev. 253, 325–342 (2009).

    CAS  Article  Google Scholar 

  7. 7

    Mitric, R. et al. Gas-phase synthesis and vibronic action spectroscopy of Ag2H+. J. Phys. Chem. Lett. 2, 548–552 (2011).

    CAS  Article  Google Scholar 

  8. 8

    Zavras, A. et al. Synthesis, Structural characterisation and gas-phase unimolecular reactivity of the silver hydride nanocluster [Ag3((PPh2)2CH2)3(μ 3-H)](BF4)2 . Inorg. Chem. 53, 7429–7437 (2014).

    CAS  Article  Google Scholar 

  9. 9

    Girod, M. et al. Formation and characterisation of the silver hydride nanocluster cation [Ag3H2((Ph2P)2CH2)]+ and its release of hydrogen. Chem. Eur. J. 20, 16626–16633 (2014).

    CAS  Article  Google Scholar 

  10. 10

    Khairallah, G. N., O’Hair, R. A. J. & Bruce, M. I. Gas-phase synthesis and reactivity studies of binuclear gold hydride cations, (R3PAu)2H+ (R=Me and Ph). Dalton Trans. 30, 3699–3707 (2006).

    Article  Google Scholar 

  11. 11

    Sabatier, P. & Mailhe, A. Catalytic decomposition of formic acid. Compt. Rend. 152, 1212–1215 (1912).

    CAS  Google Scholar 

  12. 12

    Sabatier, P. Catalysis in Organic Chemistry 538–539 (Library Press, 1923).

  13. 13

    Mars, P., Scholten, J. J. F. & Zwietering, P. The catalytic decomposition of formic acid. Adv. Catal. 14, 35–113 (1963).

    CAS  Google Scholar 

  14. 14

    Trillo, J. M., Munuera, G. & Criado, J. M. Catalytic decomposition of formic acid on metal oxides. Catal. Rev. 7, 51 (1972).

    CAS  Article  Google Scholar 

  15. 15

    Grasemann, M. & Laurenczy, G. Formic acid as a hydrogen source—recent developments and future trends. Energy Environ. Sci. 5, 8171–8181 (2012).

    CAS  Article  Google Scholar 

  16. 16

    Boddien, A. et al. CO2-“Neutral” hydrogen storage based on bicarbonates and formates. Angew Chem. Int. Ed. 50, 6411–6414 (2011).

    CAS  Article  Google Scholar 

  17. 17

    Enthaler, S., von Langermann, J. & Schmidt, T. Carbon dioxide and formic acid–the couple for environmental-friendly hydrogen storage? Energy Environ. Sci. 3, 1207–1217 (2010).

    CAS  Article  Google Scholar 

  18. 18

    Wienhöfer, G. et al. General and selective iron-catalyzed transfer hydrogenation of nitroarenes without base. J. Am. Chem. Soc. 133, 12875–12879 (2011).

    Article  Google Scholar 

  19. 19

    Braden, D. J., Henao, C. A., Heltzel, J., Maravelias, C. T. & Dumesic, J. A. Production of liquid hydrocarbon fuels by catalytic conversion of biomass-derived levulinic acid. Green Chem. 13, 1755–1765 (2011).

    CAS  Article  Google Scholar 

  20. 20

    Herrmann, W. A. & Muehlhofer, M. in Applied Homogeneous Catalysis with Organometallic Compounds, 2nd edn, Vol. 3 (eds Cornils, B. and Herrmann, W. A.), 1086 (Wiley-VCH, 2002).

  21. 21

    Odabasi, C., Gunay, M. E. & Yildirim, R. Knowledge extraction for water gas shift reaction over noble metal catalysts from publications in the literature between 2002 and 2012. Int. J. Hydrogen Energy 39, 5733–5746 (2014).

    CAS  Article  Google Scholar 

  22. 22

    Saito, K. et al. Unimolecular decomposition of formic acid in the gas phases on the ratio of the competing reaction channels. J. Phys. Chem. A 109, 5352–5357 (2005).

    CAS  Article  Google Scholar 

  23. 23

    Chang, J.-G., Chen, H.-T., Xu, S. & Lin, M. C. Computational study on the kinetics and mechanisms for the unimolecular decomposition of formic and oxalic acids. J. Phys. Chem. A 111, 6789–6797 (2007).

    CAS  Article  Google Scholar 

  24. 24

    Loges, B., Boddien, A., Gärtner, F., Junge, H. & Beller, M. Catalytic generation of hydrogen from formic acid and its derivatives: useful hydrogen storage materials. Topics Catal. 53, 902–914 (2010).

    CAS  Article  Google Scholar 

  25. 25

    Bi, Q.-Y. et al. Efficient subnanometric gold-catalyzed hydrogen generation via formic acid decomposition under ambient conditions. J. Am. Chem. Soc. 134, 8926–8933 (2012).

    CAS  Article  Google Scholar 

  26. 26

    Tedsree, K. et al. Hydrogen production from formic acid decomposition at room temperature using a Ag–Pd core–shell nanocatalyst. Nat. Nanotechnol. 6, 302–307 (2011).

    CAS  ADS  Article  Google Scholar 

  27. 27

    O’Hair, R. A. J. in Reactive Intermediates. MS Investigations in Solution (ed Santos, L.S.) Ch. 6, 199–227 (Wiley-VCH, 2010).

  28. 28

    O’Hair, R. A. J. & Rijs, N. J. Gas phase studies of the Pesci decarboxylation reaction: synthesis, structure, and unimolecular and bimolecular reactivity of organometallic ions. Acc. Chem. Res. 48, 329–340 (2015).

    Article  Google Scholar 

  29. 29

    Duncan, M. A. Spectroscopy of metal ion complexes: gas-phase models for solvation. Ann. Rev. Phys. Chem. 48, 69–93 (1997).

    CAS  ADS  Article  Google Scholar 

  30. 30

    MacAleese, L. & Maître, P. Infrared spectroscopy of organometallic ions in the gas phase: from model to real world complexes. Mass Spectrom. Rev. 26, 583–605 (2007).

    CAS  ADS  Article  Google Scholar 

  31. 31

    Antoine, R. & Dugourd, P. Visible and ultraviolet spectroscopy of gas phase protein ions. Phys. Chem. Chem. Phys. 13, 16494–16509 (2011).

    CAS  Article  Google Scholar 

  32. 32

    Lanucara, F. et al. Naked five-coordinate Fe(III)(NO) porphyrin complexes: vibrational and reactivity features. Inorg. Chem. 50, 4445–4452 (2011).

    CAS  Article  Google Scholar 

  33. 33

    Grimme, S., Antony, J., Ehrlich, S. & Krieg, H. A consistent and accurate ab initio parameterization of density functional dispersion correction (DFT-D) for the 94 elements H-Pu. J. Chem. Phys. 132, 154104 (2010).

    ADS  Article  Google Scholar 

  34. 34

    Donald, W. A., Khairallah, G. N. & O’Hair, R. A. J. The effective temperature of ions stored in a linear quadrupole ion trap mass spectrometer. J. Am. Soc. Mass Spectrom. 24, 811–815 (2013).

    CAS  ADS  Article  Google Scholar 

  35. 35

    Kamer, P. & van Leeuwen, P. W. N. M. Phosphorus(III) Ligands in Homogeneous Catalysis: Design and Synthesis Wiley (2012).

  36. 36

    Gorin, D. J., Sherry, B. D. & Toste, F. D. Ligand effects in homogeneous au catalysis. Chem. Rev. 108, 3351–3378 (2008).

    CAS  Article  Google Scholar 

  37. 37

    Eller, K. & Schwarz, H. Organometallic chemistry in the gas phase. Chem. Rev. 91, 1121–1177 (1991).

    CAS  Article  Google Scholar 

  38. 38

    Jena, P. & Castleman, A. W. Jr Cluster chemistry and dynamics special feature introductory perspective clusters: a bridge across the disciplines of physics and chemistry. Proc. Natl Acad. Sci. USA 103, 10560–10569 (2006).

    CAS  ADS  Article  Google Scholar 

  39. 39

    Waters, T., O’Hair, R. A. J. & Wedd, A. G. Catalytic gas phase oxidation of methanol to formaldehyde. J. Am. Chem. Soc. 125, 3384–3396 (2003).

    CAS  Article  Google Scholar 

  40. 40

    O’Hair, R. A. J. The 3D quadrupole ion trap mass spectrometer as a complete chemical laboratory for fundamental gas phase studies of metal mediated chemistry. Chem. Commun. 14, 1469–1481 (2006).

    Article  Google Scholar 

  41. 41

    O’Hair, R. A. J. Gas-phase studies of metal catalyzed decarboxylative cross-coupling reactions of esters. Pure. Appl. Chem. 87, 391–404 (2015).

    Article  Google Scholar 

  42. 42

    Schwarz, H. Chemistry with methane: concepts rather than recipes. Angew Chem. Int. Ed. 50, 10096–10115 (2011).

    CAS  Article  Google Scholar 

  43. 43

    Schwarz, H. How and why do cluster size, charge state, and ligands affect the course of metal-mediated gas-phase activation of methane? Isr. J. Chem. 54, 1413–1431 (2014).

    CAS  Article  Google Scholar 

  44. 44

    Agrawal, D. & Schröder, D. Insight into solution chemistry from gas-phase experiments. Organometallics 30, 32–35 (2011).

    CAS  Article  Google Scholar 

  45. 45

    Schröder, D. Applications of electrospray ionization mass spectrometry in mechanistic studies and catalysis research. Acc. Chem. Res. 45, 1521–1532 (2012).

    Article  Google Scholar 

  46. 46

    Neo, S. P., Zhou, Z. Y., Mak, T. C. W. & Hor, T. S. A. Solid-state tetramer vs. solution-state dimer reinvestigation of [Ag2(OAc)2(dppm)]2 and its dppm addition product [Ag(OAc)(dppm)]2 (dppm=Ph2PCH2PPh2). Inorg. Chem. 34, 520–523 (1995).

    CAS  Article  Google Scholar 

  47. 47

    Szłyk, E. et al. X-ray crystal structure of [Ag4(μ-dppm)2(μ-C2F5COO)4]. Synthesis and spectroscopy of silver(I) perfluorinated carboxylate complexes with bis(diphenylphosphino)methane. Dalton Trans. 17, 3404–3410 (2003).

    Article  Google Scholar 

  48. 48

    Tate, B. K. et al. A dinuclear silver hydride and an umpolung reaction of CO2 . Chem. Sci. 4, 3068–3074 (2013).

    CAS  Article  Google Scholar 

  49. 49

    Chen, P. Electrospray ionization tandem mass spectrometry in high-throughput screening of homogeneous catalysts. Angew Chem. Int. Ed. 42, 2832–2847 (2003).

    CAS  ADS  Article  Google Scholar 

  50. 50

    Colorado, A. & Brodbelt, J. An empirical approach to estimation of critical energies by using a quadrupole ion trap. J. Am. Soc. Mass Spectrom. 7, 1116–1125 (1996).

    CAS  Article  Google Scholar 

  51. 51

    Bakker, J. M., Besson, T., Lemaire, J., Scuderi, D. & Maitre, P. Gas-phase structure of a π-allyl-palladium complex: efficient infrared spectroscopy in a 7 T Fourier transform mass spectrometer. J. Phys. Chem. A 111, 13415–13424 (2007).

    CAS  Article  Google Scholar 

  52. 52

    Prazeres, R., Glotin, F., Insa, C., Jaroszynski, D. A. & Ortega, J. M. Two-colour operation of a free-electron laser and applications in the mid-infrared. Eur. Phys. J. D 3, 87–93 (1998).

    CAS  ADS  Article  Google Scholar 

  53. 53

    Becke, A. D. Density functional thermochemistry. III. The role of exact exchange. J. Chem. Phys. 98, 5648–5652 (1993).

    CAS  ADS  Article  Google Scholar 

  54. 54

    Schäfer, A., Huber, H. & Ahlrichs, R. Fully optimized contracted Gaussian basis sets of triple zeta valence quality for atoms Li to Kr. J. Chem. Phys. 100, 5829–5835 (1994).

    ADS  Article  Google Scholar 

  55. 55

    Andrae, D., Haeussermann, U., Dolg, M., Stoll, H. & Preuss, H. Energy-adjusted ab initio pseudopotentials for the second and third row transition elements. Theor. Chim. Acta 77, 123–141 (1990).

    CAS  Article  Google Scholar 

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We thank the ARC for financial support via grant DP150101388 (to R.A.J.O. and P.D.). A.Z. acknowledges the award of an Australian Postgraduate PhD Scholarship. The research leading to these results has received funding from the European Research Council under the European Union's Seventh Framework Programme (FP7/2007-2013 Grant Agreement No. 320659). Financial support from the French FT-ICR network (FR 3624 CNRS) for conducting the research is gratefully acknowledged. V.B.-K. and M.K. acknowledge Prof. Miroslav Radman at MedILS and Split-Dalmatia County for kind support.

Author information




A.Z. identified and optimized routes to the gas-phase formation of the silver hydride and silver formate complexes, carried out the CID, IMR and UVPD experiments and contributed to manuscript preparation. G.N.K carried out the IRMPD experiments and contributed to manuscript preparation. M.K. carried out all the DFT calculations and contributed to manuscript preparation; M.G., S.D., R.A., P.M., R.J.M., S.-A.A. performed experiments and/or analyzed data and/or provided intellectual input; V.B.-K. and P.D. contributed to the project design, interpretation of data and writing of the manuscript; R.A.J.O. devised the project, contributed to the design of experiments and interpretation of data, project management and writing of the manuscript.

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Correspondence to Vlasta Bonačić-Koutecký or Philippe Dugourd or Richard A. J. O’Hair.

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Supplementary Figures 1-19, Supplementary Tables 1-4, Supplementary Methods and Supplementary References (PDF 1324 kb)

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Zavras, A., Khairallah, G., Krstić, M. et al. Ligand-induced substrate steering and reshaping of [Ag2(H)]+ scaffold for selective CO2 extrusion from formic acid. Nat Commun 7, 11746 (2016).

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