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Size-Dependent Association of Cobalt Deuteride Cluster Anions Co3Dn (n = 0–4) with Dinitrogen


Dinitrogen (N2) activation by metal hydride species is of fundamental interest and practical importance while the role of hydrogen in N2 activation is not well studied. Herein, the structures of Co3Dn (n = 0–4) clusters and their reactions with N2 have been studied by using a combined experimental and computational approach. The mass spectrometry experiments identified that the Co3Dn (n = 2–4) clusters could adsorb N2 while the Co3Dn (n = 0 and 1) clusters were inert. The photoelectron imaging spectroscopy indicated that the electron detachment energies of Co3D2–4 are smaller than those of Co3D0,1, which characterized that it is easier to transfer electrons from Co3D2–4 than from Co3D0,1 to activate N2. The density functional theory calculations generally supported the experimental observations. Further analysis revealed that the H atoms in the Co3Hn (n = 2–4) clusters generally result in higher energies of the Co 3d orbitals in comparison with the Co3Hn (n = 0 and 1) systems. By forming chemical bonds with H atoms, the Co atoms of Co3H2–4 are less negatively charged with respect to the naked Co3 system, which leads to higher N2 binding energies of Co3H2–4N2 than that of Co3N2.


Mild, energy-saving approaches for conversion of N2 into available nitrogenous species are highly desirable in view of enormous energy consumption and greenhouse gas production in industrial Harber–Bosch process [1, 2]. Although the thermodynamically stable and kinetically inert N≡N bond renders its utilization a typically challengeable issue [3], some remarkable progress has been made on the daunting road of N2 fixation in different research areas [4,5,6,7,8]. One thing in common is that the N2 molecule should interact with a metal system [4, 8], in most cases, with multiple metal sites [5,6,7]. Recently, the transition metal hydride complexes have attracted extensive attentions owing to the potential in direct reduction of N2 avoiding the use of extra strong reducing agents and proton sources [9,10,11,12]. For example, a trinuclear titanium polyhydride complex found by Hou et al. can induce N2 cleavage and hydrogenation at ambient conditions [10]. Besides, it is significant to study N2 activation by hydride species because they are related to the Harber–Bosch process and biological nitrogen fixation [9, 13].

Gas-phase clusters are ideal models to mimic the active sites of related condensed-phase systems [14,15,16,17,18]. Homonuclear metal clusters such as M3–9 (M=Ni, Pd, Pt) [19], Nbn (n = 2–7) [20], Wn (n = 4–26) [21], Con (n = 4–28) [22], Con+(n = 1–18) [23, 24], and Ta2+ [25] have been reported to adsorb N2 in either a molecular or a dissociative way. The size-dependent reactivity and donation/back-donation of electrons in N2 activation were uncovered. There have been some reports and knowledge of N2 activation by metal clusters doped with ancillary main group atoms (C, S, etc.) in gas-phase investigations [26, 27]. However, to the best of our knowledge, there has been no report about the N2 activation by gas-phase metal hydride species that have already been studied to activate other very stable molecules such as CO2 [28,29,30,31] and CH4 [32,33,34,35].

In this work, we studied the gas-phase reactions between polynuclear cobalt deuteride clusters anions Co3Dn (n = 0–4) and N2 via mass spectrometry, photoelectron imaging spectroscopy, and quantum chemical calculations. Cobalt is a cheap, abundant, and monoisotopic (beneficial for mass spectrometry) late transition metal. Pure cobalt is less competitive than the early transition metals in N2 activation due to the energetically lower d orbitals that can be inefficient in π-back-donation [36]. It can be intriguing and instructive to use hydrogen atoms to promote the reactivity of cobalt clusters in N2 activation in terms of fundamental and practical aspects. The cobalt deuteride/hydride species (CoD+, CoH1,2) [37] have been generated in the gas phase while we are not aware of them being utilized in N2 reactivity studies. It is noteworthy that a lot of effort has been devoted to studying the reactions of small molecules (H2, N2, CH4, C2H2,4, and/or CO) with cobalt cluster systems Con (n = 4–28) [22], Con+ (n = 1–18) [23, 24], and ConN (n = 7–9)[38]. The photoelectron spectroscopy of Con (n = 1–108) has also been investigated by Wang and his coworkers [39].

Experimental and Computational Methods

Experimental Methods

Details of the experimental setup can be found in our previous studies [40, 41], and only a brief outline of the experiments is given below. In the reactivity experiments, the Co3Dn (n = 0–4) cluster anions were generated by laser ablation of a rotating and translating cobalt metal disk in the presence of 10% D2 seeded in a He carrier gas with a backing pressure of about 4 atm. The cluster anions of interest were mass-selected by a quadrupole mass filter (QMF) [40] and then entered into a linear ion trap (LIT) reactor [41], in which they were confined and thermalized by collisions with a pulse of He gas for about 1.4 ms. The thermalized cluster anions subsequently reacted with a pulse of N2 for about 8.6 ms. The pressures of N2 were in the range of 1–2 Pa. The reactant and product ions ejected from the LIT were transferred into a reflectron time-of-flight mass spectrometer (TOF-MS) for mass and intensity measurements [41].

The photoelectron imaging spectroscopy (PEIS) experiments were carried out with a separate apparatus of tandem TOF-MS coupled with an optical parametric oscillator (OPO) laser source and a PEIS system [42]. The Co3Dn (n = 0–4) clusters were generated according to the procedure described in the reactivity experiments with 5% D2 (for n = 3 and 4) and 0.6% D2 (for n = 0–2) seeded in He. The temperature of the cluster source was 298 K. The generated cluster anions from the supersonic expansion were skimmed into the tandem TOF-MS and were mass-selected by the primary TOF-MS with a mass gate to interact with a 550 nm laser beam delivered from the OPO system. The photodetached electrons were accelerated to the PEIS detector where the electron velocities were imaged. The two-dimensional images were transformed into three-dimensional electron velocity distributions. The photoelectron kinetic energies and angular distribution were obtained [43, 44]. The resolution of the photoelectron spectrometer was found to be around 30 meV for electrons with 1 eV kinetic energy in the test experiment with the gold anions [42].

Computational Methods

Density functional theory (DFT) calculations using Gaussian 09 program [45] were carried out to investigate the structures of Co3Hn (n = 0–4) as well as the mechanistic details for the size-dependent reactivity with N2. There is a long-standing controversy on the most stable geometry of Co3. The reported DFT calculations predicted either a linear or a triangular structure, depending on the functionals and basis sets adopted [46,47,48,49,50,51]. To find an appropriate functional for the polynuclear cobalt hydrides, the experimental values of electron detachment energies of Co3 [39], bond length of Co–Co [52], and bond dissociation energy of Co–H [53] were used to test various functionals (Table S1). It turned out that the TPSS functional [54] is the best overall with the def2-TZVP basis set [55]. The low-lying structure isomers for each of Co3Hn (n = 0–4) were determined by the TPSS calculations for different spin multiplicities. The electron adiabatic detachment energies (ADEs) and vertical detachment energies (VDEs) were calculated. Based on the structures of Co3Hn (n = 0–4), the structures and N2 adsorption energies of Co3Hn(N2)x (x = 1, 2, or 3) were calculated. The reported relative energies of the cluster isomers were corrected with zero-point vibrations. The molecular orbital (MO) analysis and natural bond orbital (NBO) analysis were performed to further interpret the experimental results.


Reactivity of Co3Dn (n = 0–4) with N2

The TOF mass spectra for the interactions of Co3Dn (n = 0–4) with N2 are shown in Figure 1. It is obvious that in the reactions of Co3 (Figure 1a) and Co3D (Figure 1b) with N2, no product peaks were generated. In contrast, under similar experimental conditions, the interactions of Co3D2 (Figure 1c), Co3D3 (Figure 1d), and Co3D4 (Figure 1e) with N2 generated product peaks that can be assigned as Co3D2–4N2, suggesting the following reaction channels:

$$ {\mathrm{Co}}_3{{\mathrm{D}}_{2-4}}^{-}+{\mathrm{N}}_2\to {\mathrm{Co}}_3{\mathrm{D}}_{2-4}{{\mathrm{N}}_2}^{-} $$
Figure 1

Time-of-flight mass spectra for the reactions of mass-selected (a) Co3, (b) Co3D, (c) Co3D2, (d) Co3D3, and (e) Co3D4 with 1.3–1.6 Pa N2 for about 8.6 ms. Peaks marked with asterisks are due to the residual water in the gas handling system

In addition to the adsorption of one N2 molecule, the adsorption of the second N2 molecules on Co3D3,4N2 appeared, indicating the following reaction channels:

$$ {\mathrm{Co}}_3{\mathrm{D}}_{3,4}{{\mathrm{N}}_2}^{-}+{\mathrm{N}}_2\to {\mathrm{Co}}_3{\mathrm{D}}_{3,4}{{\left({\mathrm{N}}_2\right)}_2}^{-} $$

The adsorption of the third N2 molecule on Co3D4(N2)2 was also observed, corresponding to the following reaction channel:

$$ {\mathrm{Co}}_3{\mathrm{D}}_4{{\left({\mathrm{N}}_2\right)}_2}^{-}+{\mathrm{N}}_2\to {\mathrm{Co}}_3{\mathrm{D}}_4{{\left({\mathrm{N}}_2\right)}_3}^{-} $$

The pseudo-first-order rate constants (k1) of the reactions between Co3Dn (n = 0–4) clusters and N2 were determined by Eq. (4) [56], in which IR is the intensity of the reactant cluster ions after the reaction, IT is the total ion intensity including product ion contribution, P is the effective pressure of the reactant gas, kB is the Boltzmann constant, T is the temperature (298 K) of the reactant gas, and tR is the reaction time (8.6 ms).

$$ \ln \frac{I_{\mathrm{R}}}{I_{\mathrm{T}}}=-{k}_1\frac{P}{k_{\mathrm{B}}T}{t}_{\mathrm{R}} $$

When estimating the k1 value in Eq. (4), the systematic deviations of tR (± 3%), T (± 1%), and P (± 20%) were considered. As shown in Figure 2, the k1 values for the reactions of Co3D2–4 with N2 were determined to be (3.4 ± 0.7) × 10−13, (5.9 ± 1.2) × 10−14, and (9.3 ± 1.9) × 10−14 cm3 molecule−1 s−1, respectively. The k1 value of Co3D2 with N2 is about six and four times larger than those of Co3D3 and Co3D4 systems, respectively.

Figure 2

The pseudo-first-order rate constants (k1) for the reactions of Co3Dn (n = 0–4) with N2

DFT Calculated Structures and N2 Adsorption Energies

The DFT calculated structures of the Co3Hn (n = 0–4) clusters and the N2 adsorption products are presented in Figure 3 (see Figures S1 and S2 for more details). For clarity, the ith isomer of Co3Hn is denoted as n-i. For example, 0–1 denotes the most stable structure of Co3. Similarly, N2 adsorption complex Co3Hn(N2)x is denoted as n-Cx-i. The DFT calculated lowest-lying isomer of Co3 (0–1) has an equilateral triangular structure with the bond length of 226 pm and the nonet spin state, while the linear structure of Co3 (0–2) has the septet state that is 0.38 eV higher in energy than the triangular one. For Co3H, the lowest-lying isomer (1–1) has the octet spin state and the Cs symmetry. The H atom in isomer 1–1 is bridgingly bonded with two Co atoms. The isomer 1–2 with a terminal H atom and the isomer 1–3 with the C2v symmetry were calculated to be 0.11 and 0.19 eV higher in energy than the 1–1 structure, respectively. All of the H atoms in the lowest-lying isomers of Co3H2 (2–1) and Co3H3 (3–1) are bridgingly bonded. One of the four H atoms in Co3H4 (4–1) is terminally bonded. Each of the Co3Hn (n = 1–4) clusters has one or two isomers that are very close in energy (within 0.2 eV) to the lowest-lying isomers. These isomers are possible candidates that could be populated in the cluster source. It is noteworthy that test calculations indicated that the cluster structures with an unbroken HH bond such as (H2)Co3H and (H2)Co3H2 are all high in energy (isomers 3–6 and 4–6 in Figure S1).

Figure 3

DFT calculated low-lying isomers of Co3Hn (n = 0–4) and their N2 adsorption products. The relative energies with respect to the lowest-lying isomers (n-1) for isomers (n-i) and the N2 binding energies for adsorption products (n-Cx-i) are in units of eV. Some selected bond lengths are given in pm. The superscripts indicate the spin multiplicities. The calculated ADE/VDE values of Co3HnN2 (n-C1-1, n = 2–4) are listed in the brackets. The bond orders of Co–N are listed in the square brackets

For the N2 adsorption complexes, several N2 binding modes were considered and it turned out that the end-on coordination is the most favorable mode. The most stable structures of the adsorption products Co3H2–4N2 remain the same spin multiplicities as the reactant clusters while that of Co3H0,1N2 have different spin multiplicities with respect to the reactants. As shown in Figure 3, the most stable structure of Co3N2 (0-C1-1) has the septet spin state and the N2 adsorption energy (1.15 eV) is larger than that of the isomer (0-C1-4) with nonet spin state by 0.61 eV. For Co3H, the low-lying isomers (1-1, 1-2, and 1-3) can bind N2 to generate the most stable adsorption structure (1-C1-1) with the sextet spin state which has a larger adsorption (1.30 eV) energy than the isomer in the octet spin state (1.16 eV). For Co3H2, the low-lying isomers (2-1, 2-2, and 2-3) can adsorb N2 to form the most stable adsorption structure (2-C1-1). For Co3H3, the N2 adsorption onto 3-1 and 3-3 can produce the most stable complex 3-C1-1 while the complex formed from 3-2 with N2 is higher in energy by 0.70 eV (3-C1-3, Figure S2). The most stable adsorption complex of Co3H4N2 (4-C1-1) can be formed from 4-1 and 4-2 with N2. In the adsorption complexes Co3H2N2 (2-C1-1), Co3H3N2 (3-C1-1), and Co3H4N2 (4-C1-1), the bond orders (Figure 3, square brackets) between N2 and the related Co atoms are around 0.83–0.87, which indicates that there is significant chemical bonding between N and Co atoms. Meanwhile the N-N bond order is decreased from 3.0 in free N2 to about 2.5 in the association complexes. Therefore, the N-N bond was significantly activated in the adsorption complexes. The structures of the complexes with two and three N2 molecules were also determined and all of the N2 units are end-on coordinated (Figure 3, bottom right). The N2 adsorption energy of Co3HnN2 (n-C1-1) generally increases as the increase of the number (n) of H atoms, which is qualitatively consistent with the experimental result that Co3H2–4 absorbed N2 while Co3H0,1 did not (Figure 1).

Photoelectron Spectra and Structure Assignments

For most of the Co3Hn (n = 0–4) clusters, the DFT calculations predicted more than one isomeric structure that are close in energy (Figure 3, left). The PEIS experiment can be helpful to assign the cluster structures. The photoelectron spectra of Co3D0–4 are presented in Figure 4, and the experimental and DFT calculated ADE/VDE values are listed in Table 1. The simulated photoelectron spectra of the low-lying isomers of Co3Hn (n = 0–4) based on the generalized Koopmans’ theorem [57], named as density of states (DOS) spectra, are presented in Figures S4–S8.

Figure 4

Photoelectron spectra of (a) Co3, (b) Co3D, (c) Co3D2, (d) Co3D3, and (e) Co3D4 taken with 550 nm (2.254 eV) photons. The structures shown are the most probable isomers in the experiments

Table 1 Experimental and DFT calculated ADE/VDE values of Co3Dn (n = 0–4)

For Co3 (Figure 4a), the spectrum is dominated by a band ranging from about 1.40 to 1.80 eV, with a band center at the electron binding energy (EBE) of 1.62 eV, which determines the VDE value. The ADE value of Co3 was estimated to be 1.41 eV by extrapolating the lower EBE side of the band to zero photoelectron intensity. The ADE and VDE values (1.41/1.62 eV) of Co3 are in line with those (1.40/1.60 eV) of Wang and his coworkers in a previous study [39]. The DFT calculations predicted that the isomers 0-1 and 0-2 of Co3 have ADE/VDE values of 1.26/1.45 eV and 1.18/1.20 eV, respectively, and the former (1.26/1.45 eV) better matches the experiment (1.41/1.62 eV). Moreover, the DOS spectrum of isomer 0-1 can reproduce the experimental band position and pattern better than that of isomer 0-2 (Figure S4). Thus, the isomer 0-1 is assigned to be the most probable structure generated in the experiment. For Co3D, the experimental ADE/VDE values are 1.57/1.69 eV (Figure 4b), which are slightly blue-shifted with respect to that of Co3 (1.41/1.62 eV). The theoretical ADE/VDE values of isomers 1-1, 1-2, and 1-3 are 1.22/1.23, 1.34/1.41, and 1.03/1.16 eV, respectively. Though isomer 1-1 was calculated to be the lowest-lying structure, its theoretical ADE/VDE values and DOS spectrum cannot fit the experiments well, while those of isomer 1-2 are closer to the experimental results (Figure S5). Isomer 1-3 is unlikely to be detected in the experiment because its theoretical ADE/VDE (1.03/1.16 eV) deviate largely from the experimental values (1.57/1.69 eV). Therefore, the isomer 1-2 is suggested to be the most probable structure contributing to the photoelectron spectrum of Co3D.

In contrast to narrow spectral band of Co3D and blue-shifted ADE of Co3D with respect to that of Co3, the spectral bands of Co3D2–4 (Figure 4c–e) are all broad and the ADE values of those clusters are all red-shifted (Table 1). For Co3D2, the isomers 2-1 and 2-2 are almost degenerate in energy (Figure 3). The combination of the DOS spectra of isomers 2-1 and 2-2 can fit most of the experimental features (Figure S6). Thus, isomers 2-1 and 2-2 are suggested to be coexist in the cluster source. Notably, the isomer 2-3 may have minor contribution because its DOS spectrum resembles the high EBE peaks in the experimental spectrum. Similarly, the broad spectral bands of Co3D3 by the experiment and the DOS spectra of several low-lying isomers (Figure S7) suggest that isomers 3-1 and 3-3 may be the major structures contributing to the experimental spectrum and isomer 3-2 may have the minor contribution. For Co3D4, the combination of the DOS spectra of isomers 4-1 and 4-2 (Figure S8) can match the experimental spectrum. The isomer 4-3 was unlikely to be touched in the PEIS experiments because the ADE/VDE values (2.72/3.06 eV) deviate largely from the experimental values (1.00/1.76 eV).


Size-Dependent Reactivity of Co3Dn (n = 0–4) with N2

The relaxed potential energy surface scans revealed that the processes of N2 adsorption onto Co3D2–4 are exothermic and barrier-free and the N2 adsorption energies of Co3D2–4 N2 are generally larger (1.31–1.55 eV, Figure 3) than those of Co3N2 and Co3DN2. In addition, the spin conversions [58] have to take place in order to form the most stable structures of Co3N2 (0-C1-1) and Co3DN2 (1-C1-1). The relatively low N2 binding energies of 0-C1-4 (0.54 eV) and 1-C1-2 (1.16 eV) and the possibly low-spin conversion efficiencies can lead to relatively weak N2 adsorption, which is in agreement with no observation of Co3N2 and Co3DN2 in the experiment (Figure 1). Interestingly, the rate constant for the reaction of Co3D3 with N2 is the smallest among Co3D2–4 reaction systems while Co3D3N2 has a larger N2 adsorption energy (1.55 eV) than Co3D2N2 (1.38 eV) and Co3D4N2 (1.31 eV). The DFT calculations indicated that the ADE (1.40 eV) and VDE (1.49 eV) values (Figure 3, in brackets) of Co3D3N2 are smaller than the N2 adsorption energy (1.55 eV), which means that associative electron detachment (AED) could take place in the experiment Co3D3 + N2 → (Co3D3N2)* → Co3D3N2 + e. Note that the AED process was often observed in the reactions of small molecules with negative ions [59, 60]. In contrast, the AED process for the Co3D2 and Co3D4 reaction systems would not take place because the ADE values of Co3D2N2 and Co3D4N2 are significantly higher than the corresponding N2 adsorption energies. In other words, Co3D3 could be the most reactive cluster towards N2 but exhibited the smallest reaction rate among Co3D2–4 due to the undetectable adsorption products (the IT value in Eq. (4) could be underestimated for Co3D3 + N2).

The size-dependent reactivity of the Co3Dn (n = 0–4) clusters with N2 is also supported by the PEIS experiment. The increased ADE of Co3D (1.57 eV) with respect to that of Co3 (1.41 eV) indicates that it is more difficult for Co3D to lose electrons to activate and then absorb N2. In contrast, the decreased ADEs of Co3D2–4 (1.00–1.18 eV) mean that Co3D2–4 can lose electrons more easily to activate and then absorb N2 than Co3 and Co3D. Therefore, the different ADEs by the PEIS can generally interpret the size-dependent reactivity of the Co3Dn (n = 0–4) clusters with N2 in the mass spectrometry experiment.

MO Analysis

To further understand the differences in electron detachment and N2 adsorption energies of the Co3Dn (n = 0–4) clusters, the MO analysis has been performed. The highest occupied MOs (HOMOs) were considered to lose electrons in the electron detachment. The HOMOs of selected isomers of Co3H0–4 (note that the electronic structures of Co3H0–4 and Co3D0–4 are identical) are given in Figure 5. Note that both isomers 1-1 and 1-2 are listed for a comparison although the isomer 1-2 is assigned as the experimental species. It can be seen that both the number and the bonding mode of H atoms can influence the energies of HOMOs that are primarily composed of the Co 3d orbitals. A terminally bonded H atom (denoted as Ht) of Co3H (1-2) lowers down the HOMO energy with respect to that of Co3, which leads to a larger ADE of Co3H (1.57 eV) than Co3 (1.41 eV). In contrast, the HOMO energy increases if the H atom is bridgingly bonded (denoted as Hb) in Co3H (1-1). For Co3H2–4, the HOMO energies are all higher than that of Co3, leading to smaller ADEs (1.00–1.18 eV) of Co3D2–4 than that of Co3. The increased HOMO levels of Co3H2–4 can also facilitate back-donation bonding with the π* orbitals of N2 due to the decreased energy gap. Interestingly, for each of the Co3Hn (n = 1–4) clusters, the isomers with more Hb atoms tend to have higher HOMO levels.

Figure 5

HOMO levels of selected Co3Hn (n = 0–4) cluster isomers that lose electrons to form the corresponding neutral counterparts. The up and down arrows denote the α and β electrons, respectively

NBO Analysis

The NBO analysis was performed to further interpret the bonding between N2 and Co3Hn (n = 0–4) clusters, and the results are presented in Table 2. It turned out that the less negatively charged Co atom functions as the preferred trapping site to anchor N2 molecule (hereafter called active-Co), while the other two Co atoms and the H atoms serve as indirect electron donors for the active-Co atom and N2 molecule. The active-Co atoms in Co3H0,1 (0-1 and 1-2) have relatively large negative charges (− 0.333 and − 0.290 e, respectively) and more 4s electron occupancies (4s1.32 and 4s1.31, respectively), which give rise to an unfavorable approach and relatively high σ-repulsion to the N2 molecule. Upon bonding of two H atoms on the Co3 cluster to form Co3H2 (2-1), the natural charge on the active-Co increases to − 0.099 e; meanwhile, more 3d and less 4s electron occupancies are located, which can result in an easier approach of N2 to the cluster and a larger adsorption energy (1.38 eV). The above changes of charge on the active-Co and the electron occupancies in 3d and 4s orbitals are further enhanced when three H atoms are bonded with Co3 to form Co3H3 (3-1), which leads to a further larger N2 adsorption energy (1.55 eV). For Co3H4, the natural charges on the active-Co and the four H atoms are + 0.134 e and − 1.225 e, respectively, and electron configuration of the 3d orbital reduces to 3d7.83. Such a positive Co site tends to compete with N2 for electron densities. It turns out that the active-Co of Co3H4 (4-1) gains − 0.250 e while the N2 unit only gains − 0.212 e which becomes smaller than the corresponding value (− 0.259 e) of Co3H3 (3-1) reaction system. As a result, the N2 is less activated in Co3H4N2 (4-C1-1) than in Co3H3N2 (3-C1-1), which is consistent with the larger N2 adsorption energy of the latter (1.55 eV) versus the former (1.31 eV). One can conclude that the H atoms on the metal cluster (Co3) significantly manipulate the charge/electron distribution (and the electronic structure), and an appropriate number of H atoms can enhance and maximize the cluster reactivity in N2 activation.

Table 2 Natural charge and electron occupancy analysis


The structures of Co3Dn (n = 0–4) clusters and their reactions with N2 have been studied by mass spectrometry, photoelectron imaging spectroscopy, and density functional theory calculations. The Co3D2–4 clusters were observed to adsorb N2 molecules in an ion trap reactor while Co3 and Co3D were inert. The photoelectron spectra indicated that Co3D and Co3D2–4 have blue- and red-shifted adiabatic electron detachment energies with respect to Co3, which interprets the size-dependent abilities to transfer electrons from the cluster anions to activate and then absorb N2 molecules. The density functional theory calculations revealed that (i) the disagreement of the largest N2 adsorption energy and the smallest reaction rate of Co3D3 among Co3D2–4 reaction systems may be resulted from the exothermic process of the associative electron detachment, leading to the undetectable neutral product in the mass spectrometry experiment and the underestimate of the rate constant; (ii) the highest occupied molecular orbitals of Co3H2–4 (primarily Co 3d orbitals) are pushed higher in energy upon the bonding of H atoms on the Co3 cluster, which facilitates electron detachment as well as N2 adsorption; and (iii) the bonding of H atoms on the Co3 cluster can also lead to less negatively charged Co sites with more 3d electron occupancies that are more effective to make π-back-donation bonding with N2 molecules. An appropriate number of H (or D) atoms on a metal cluster such as Co3 can enhance and maximize the cluster reactivity in N2 activation.


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This work was supported by the National Natural Science Foundation of China (Nos. 21833011, 21773253, and 21603237).

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Correspondence to Zi-Yu Li or Sheng-Gui He.

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Mou, LH., Li, ZY., Liu, QY. et al. Size-Dependent Association of Cobalt Deuteride Cluster Anions Co3Dn (n = 0–4) with Dinitrogen. J. Am. Soc. Mass Spectrom. 30, 1956–1963 (2019). https://doi.org/10.1007/s13361-019-02226-2

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  • Ion-molecule reactions
  • Mass spectrometry
  • Photoelectron imaging spectroscopy
  • N2 activation
  • Cobalt
  • Density functional theory