Chinese Journal of Chemical Physics  2018, Vol. 31 Issue (5): 641-648

The article information

Hong Wu, Qi-quan Luo, Rui-qi Zhang, Wen-hua Zhang, Jin-long Yang
吴红, 罗其全, 张瑞奇, 张文华, 杨金龙
Single Pt Atoms Supported on Oxidized Graphene as a Promising Catalyst for Hydrolysis of Ammonia Borane
氧化石墨烯负载的Pt单原子催化硼胺烷水解机理的理论研究
Chinese Journal of Chemical Physics, 2018, 31(5): 641-648
化学物理学报, 2018, 31(5): 641-648
http://dx.doi.org/10.1063/1674-0068/31/cjcp1804063

Article history

Received on: April 11, 2018
Accepted on: April 25, 2018
Single Pt Atoms Supported on Oxidized Graphene as a Promising Catalyst for Hydrolysis of Ammonia Borane
Hong Wua, Qi-quan Luoa, Rui-qi Zhanga, Wen-hua Zhangb,c,d, Jin-long Yanga,c     
Dated: Received on April 11, 2018; Accepted on April 25, 2018
a. Hefei National Laboratory for Physical Sciences at the Microscale, University of Science and Technology of China, Hefei 230026, China;
b. Key Laboratory of Materials for Energy Conversion, Chinese Academy of Sciences, University of Science and Technology of China, Hefei 230026, China;
c. Synergetic Innovation Center of Quantum Information & Quantum Physics, University of Science and Technology of China, Hefei 230026, China;
d. Department of Applied Mathematics, School of Physics and Engineering, Australian National University, Canberra, ACT 2600, Australia
*Author to whom correspondence should be addressed. Wen-hua Zhang, E-mail: whhzhang@ustc.edu.cn; Jin-long Yang, E-mail: jlyang@ustc.edu.cn
Abstract: Based on density functional theory calculations, the full hydrolysis of per N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule to produce three hydrogen molecules on single Pt atoms supported on oxidized graphene (P$\rm{t}_{1}$/Gr-O) is investigated. It is suggested that the first hydrogen molecule is produced by the combination of two hydrogen atoms from two successive B-H bonds breaking. Then one $\rm{H}_\rm{2}$O molecule attacks the left $^*$BHN$\rm{H}_\rm{3}$ group ($^*$ represents adsorbed state) to form $^*$BH($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ and the elongated O-H bond is easily broken to produce $^*$BH(OH)N$\rm{H}_\rm{3}$. The second $\rm{H}_\rm{2}$O molecule attacks $^*$BH(OH)N$\rm{H}_\rm{3}$ to form $^*$BH(OH)($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ and the breaking of O-H bond pointing to the plane of P$\rm{t}_{1}$/Gr-O results in the desorption of BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$. The second hydrogen molecule is produced from two hydrogen atoms coming from two $\rm{H}_\rm{2}$O molecules and P$\rm{t}_{1}$/Gr-O is recovered after the releasing of hydrogen molecule. The third hydrogen molecule is generated by the further hydrolysis of BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$ in water solution. The rate-limiting step of the whole process is the combination of one $\rm{H}_\rm{2}$O molecule and $^*$BHN$\rm{H}_\rm{3}$ with an energy barrier of 16.1 kcal/mol. Thus, P$\rm{t}_{1}$/Gr-O is suggested to be a promising catalyst for hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ at room temperature.
Key words: Density functional theory    Single atom catalysis    Platinum    Oxidized graphene    Ammonia borane hydrolysis    
Ⅰ. INTRODUCTION

Hydrogen is considered as one of the most potential clean and renewable energy carriers in future. Safe storage and transport of hydrogen is important for its real application [1]. It is expected that hydrogen is stored in types of stable materials under mild condition and can be released steadily by the trigger of catalysts [1-5]. Ammonia borane (N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$) is regarded as a promising candidate molecule for hydrogen storage due to its nontoxicity, high hydrogen content (19.6wt% H), and high thermal stability even in water solvent at ambient temperature [6-9]. The best scenario is that per N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule can completely release three hydrogen molecules and can be recovered easily [3, 5-8]. Respect to direct dissociation of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ at high temperature, hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ on catalysts is more promising for room temperature hydrogen generation.

Pt-based catalysts, such as small Pt nanoparticles supported on Si$\rm{O}_\rm{2}$ [10], $\gamma-\rm{Al}_\rm{2}$$\rm{O}_\rm{3}$ [10], porous chromium terephthalate (MIL-101) [11], carbon nanotubes (CNT) [12, 13], and reduced graphene oxide [14], exhibit superior catalytic activity for hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$. Transition non-noble metals such as Co [15-18], Ni [19-22], and Cu [23-25] are also widely studied to explore the possibility to replace noble metals for their low price. Both experimental and theoretical work were performed to better understand the hydrolysis mechanism of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ and get clues for catalysts improvement. In early stage, it was proposed that the hydrolysis starts from the B-N bond breaking by the attacking of water molecule [10] or the dissociation of $\rm{H}_\rm{2}$O in the hydroxylation process of the adsorbed N$\rm{H}_\rm{3}$B${\rm{H}}_x$ from B-H breaking [26]. Recently, the O-H bond cleavage of water is experimentally suggested as the rate-limiting step of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis on the Pt/CNT [27], PtRu/CNT [28], Co/CTF [17], Ni/ZIF-8 [21], and atomically dispersed Pt on the surface of Ni particle [29], etc. by kinetic isotope effect (KIE) method. Theoretically, it is suggested that the rate-limiting step could be water assisted B-N bond breaking [19], attacking of surfaced adsorbed OH group to break B-N bond [30], and even the dissociation of an O-H bond in $\rm{H}_\rm{2}$O [29] for the production of the first hydrogen molecule. Moreover, the whole picture of the full hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ with catalysts has not been provided yet.

Till now, the lack of abundance of Pt limits its practical use as catalysts and the catalytic performance of non-noble transition metals is relatively lower than that of Pt [31]. Searching for new types of catalysts is still demanding. An alternative way is to maximize the utilization of noble metal by downsizing the size of nanoparticles even to single atoms on designed substrates [32-34]. Reduced graphene oxide is a good candidate for substrates to anchor single metal atoms [35] for its large surface area, rich and controllable surface structures. Recently, the isolated Pt and Pd atoms supported on reduced graphene oxide have been successfully prepared and exhibited excellent catalytic activity for methanol oxidation [36] and selective hydrogenation of 1, 3-butadiene at mild reaction conditions [37], respectively. Also, the isolated Pt anchored by two interfacial oxygen at the edge of reduced graphene oxide was active for the partial hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ with about one hydrogen molecule released by per N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule [38]. Considering the rich structure configurations on reduced graphene oxide, it is anticipated to design a configuration of single Pt atoms supported on reduced graphene oxide with high catalytic activity for the full hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$.

Herein, in this work we design a single Pt atom supported on trivacancy structure terminated by an oxygen adatom to form an ether group in graphene nanosheet (P$\rm{t}_{1}$/Gr-O). P$\rm{t}_{1}$/Gr-O catalyzed full hydrolysis process of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ is studied, and it is found the rate limiting step is the hydratation of $^*$BHN$\rm{H}_\rm{3}$ with an energy barrier of 16.1 kcal/mol. The low activation energy indicates that on P$\rm{t}_{1}$/Gr-O the full hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ can proceed at room temperature. Thus P$\rm{t}_{1}$/Gr-O may be a promising catalyst for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis.

Ⅱ. COMPUTATIONAL DETAILS

All the calculations were performed by using spin-polarized density functional theory (DFT) method. The DFT semi-core pseudopotentials method (DSPP) [39] with a single effective potential replacing core electrons and the double numerical basis set together with polarization functions (DNP) were adopted to form the Perdew-Burke-Ernzerhof (PBE) exchange-correlation functional within the generalized gradient approximation (GGA) [40], implemented in D$\rm{Mol}^\rm{3}$ package [41, 42]. A smearing of 0.005 Ha (1 Ha$=$27.21 eV) to the orbital occupation was applied to achieve electronic convergence in geometric optimization and transition state search program. The real-space global cutoff radius was set to be 4.5 Å. A hexagonal supercell containing (6×6) unit cells of graphene monolayer with 20 Å vacuum layer was used as a support for a single Pt atom. The convergence tolerances of energy, force, and displacement for the geometry optimization were 1×$10^{-5}$ Ha, 0.002 Ha/Å, and 0.005 Å, respectively. In self-consistent-field (SCF) procedures a convergence criterion of 1×$10^{-6}$ Ha and fermi occupation were adopted. 3×3×1 k-points grid was used to describe the Brillouin zone for geometric optimization and self-consistent calculations. The transition state for each elementary step was determined by LST/QST method and confirmed via frequency calculations. The $\rm{H}_\rm{2}$O solvent environment was simulated by using a conductor-like screening model (COSMO) [43] in all calculations. The dielectric constant was set to 78.54 for $\rm{H}_\rm{2}$O. To verify the accuracy of our calculation method, we calculated the B-N bond breakage of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ attacked by one $\rm{H}_\rm{2}$O molecule in aqueous phase. The calculated energy barrier of 38.0 kcal/mol is close to that of 32.9 kcal/mol calculated at CCSD(T)//M06-2X/6-311$+$G(d, p) level [44]. The adsorption energies of surface species are defined as:

$ E_{\rm{ads}} = E_{{\rm{X}}/{\rm{catalyst}}} - (E_{\rm{catalyst}} + E_{\rm{X}}) $

where $E_{{\rm{X}}/{\rm{catalyst}}}$, $E_{\rm{catalyst}}$, and $E_{\rm{X}}$ represent the energies of adsorbed systems, catalyst itself, and surface species, respectively. This hydrogen bond (H-bond) energy is calculated by the following formula:

$ {E_\rm{H}{\textrm{-bond}}}={E_{{^*}\rm{X}\cdots{\rm{H}_2}O}}-({E_{{^*}\rm{X}}}+{E_{{\rm{H}_2}\rm{O(l)}}}) $

where $E_{{^*}\rm{X}\cdots{\rm{H}_2}O}$, $E_{{^*}\rm{X}}$, and $E_{{\rm{H}_2}\rm{O(l)}}$ represent the energies of the total systems, the adsorbed X species on P$\rm{t}_{1}$/Gr-O, and a liquid phase $\rm{H}_2$O molecule ($\rm{H}_2$O(l)), respectively. $^*$X denotes the adsorbed intermediates in the process of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis. The total energy of P$\rm{t}_{1}$/Gr-O with one N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ and three $\rm{H}_2$O molecules in water solvent is set as zero point for the relative energy for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis.

Ⅲ. RESULTS AND DISCUSSION A. Adsorption on the P$\rm{t}_{1}$/Gr-O Surface

A trivacancy with an edge ether on graphene basal plane (Gr-O) is designed to anchor a single Pt atom (denoted as P$\rm{t}_{1}$/Gr-O). In the most stable configuration of P$\rm{t}_{1}$/Gr-O as shown in FIG. 1(a), the three Pt-C bond lengths are 1.92, 1.95, and 2.00 Å, respectively, which are shorter than the Pt-O bond length of 2.14 Å. The binding energy of a single Pt atom respecting to Pt bulk is calculated as -46.7 kcal/mol, which can effectively prevent the aggregation of single Pt atoms.

FIG. 1 Top and side views of the most stable configuration of a single Pt atom adsorbed on the Gr-O sheet (a), the optimized structures of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ (b), $\rm{H}_\rm{2}$O (c), and $\rm{H}_\rm{2}$ (d) adsorbed on the P$\rm{t}_{1}$/Gr-O surface, respectively. The black, red, celadon, pink, blue, and white spheres represent C, O, Pt, B, N, and H atoms, respectively. Critical bond lengths are labeled (in unit of Å).

In the most stable adsorption configuration of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ on $\rm{Pt}_1$/Gr-O, a N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule binds with Pt atom through two hydrogen atoms of B$\rm{H}_\rm{3}$ group as shown in FIG. 1(b). The adsorption energy of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ on $\rm{Pt}_1$/Gr-O is calculated as -9.8 kcal/mol. The bond distances between Pt and two hydrogen atoms are 1.96 and 1.97 Å, respectively. For the interaction between Pt and H, the two B-H bonds are elongated to 1.26 and 1.27 Å from 1.21 Å in isolated solvated N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$. Meanwhile, the B-N bond is shortened by 0.03 Å. The changes in the B-H and B-N bond lengths agree with the results of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ adsorbed on P$\rm{d}_\rm{2}$/MgO and P$\rm{d}_\rm{4}$/MgO [45].

The adsorption energy of one $\rm{H}_\rm{2}$O molecule on P$\rm{t}_{1}$/Gr-O is calculated as 0.2 kcal/mol, which is much lower than that of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$. The distance between the oxygen atom in the $\rm{H}_\rm{2}$O molecule and Pt atom is 2.37 Å, as shown in FIG. 1(c), which also suggests a weak interaction between water and P$\rm{t}_{1}$/Gr-O. The adsorption of one hydrogen molecule is also investigated. With molecularly adsorbed configuration as shown in FIG. 1(d), the adsorption energy is calculated as 2.8 kcal/mol, which indicates the molecularly adsorbed hydrogen is ready to desorb from the catalyst. The bond length of H-H is elongated to 0.81 Å and two Pt-H bond lengths are 1.94 and 1.97 Å, respectively.

B. The elementary reactions of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis on the P$\rm{t}_{1}$/Gr-O surface 1. The B-H bond activation pathways

Two possible mechanisms have been proposed to initiate the hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$. One is the bond breakage of B-N bonds attacked by $\rm{H}_\rm{2}$O molecules [10] and the other is the dehydrogenation of B$\rm{H}_\rm{3}$ group [26]. On P$\rm{t}_{1}$/Gr-O, the energy barrier of B-N bond breakage with the help of one water molecule is calculated as high as 37.7 kcal/mol (FIG. S1(a) in supplementary materials), which is similar to the result over $\rm{Ni}_\rm{2}$P nanoparticles (38.1 kcal/mol) [19]. While the energy barrier of B-H bond breaking is only 11.3 kcal/mol, which indicates the adsorbed N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule prefers B-H bond breaking rather than B-N bond breaking. At transition state TS1, a Pt-H-B three-membered ring configuration is formed, and the Pt-H, B-H, and Pt-B distances are 1.64, 1.84, and 2.41 Å as shown in FIG. 2, respectively. After the breaking of B-H bond, the hydrogen atom locates at the bridge site of Pt-C and the $^*$B$\rm{H}_\rm{2}$N$\rm{H}_\rm{3}$ group binds to Pt site with the Pt-B bond length of 2.21 Å (I2). The carbon atom near the Pt atom is also active for trapping hydrogen atom, which resembles the Fe-C bridge site for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ dehydrogenation on prototype iron pincer catalyst [46].

FIG. 2 The relative energy profiles of the releasing of the first hydrogen molecule from N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ catalyzed by P$\rm{t_{1}}$/Gr-O. Critical bond lengths are labeled (in unit of Å).

For the next step, four possible reaction pathways (i.e., N-H bond breaking to form B$\rm{H}_\rm{2}$N$\rm{H}_\rm{2}$, directly producing a gas phase hydrogen molecule, hydrolysis of $^*$B$\rm{H}_\rm{2}$N$\rm{H}_\rm{3}$, and the second B-H bond breaking to form a molecularly adsorbed hydrogen) are investigated as shown in FIG. S1 (b)-(d) in supplementary materials and FIG. 2. The energy barriers of these four possible elementary steps are calculated as 33.9, 21.4, 21.4, and 10.0 kcal/mol, respectively. The formation of a molecularly adsorbed hydrogen via bond breaking of the second B-H bond has the lowest energy barrier. At transition state (TS2), the C-H and Pt-B bond lengths elongate by 0.76 and 0.12 Å, respectively. The formed molecular hydrogen weakly adsorbs on P$\rm{t}_{1}$/Gr-O and easily desorbs from catalyst with an energy barrier of 0.9 kcal/mol via transition state (TS3). The production of the first hydrogen releases 1.8 kcal/mol relative to the adsorbed N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ system.

2. Hydroxylation pathways of B atom in N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$

After desorption of the first hydrogen molecule, the left $^*$BHN$\rm{H}_\rm{3}$ adsorbs at bridge site of Pt-C. Four possible ways of the evolution of $^*$BHN$\rm{H}_\rm{3}$ including the breaking of B-H bond, the breaking of N-H bond and also the attachment of water molecule to form Pt (or C) bound $^*$BH($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ are considered as shown in FIG. S2 (a)-(c) in supplementary materials and FIG. 3. The energy barriers are calculated as 42.7, 32.1, 23.0, and 16.1 kcal/mol for the four possible reaction ways, respectively. The combination of a $\rm{H}_\rm{2}$O molecule with $^*$BHN$\rm{H}_\rm{3}$ to form C-BH($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ is the most kinetically favorable way. At initial state, a $\rm{H}_\rm{2}$O molecule interacts with the $^*$BHN$\rm{H_\rm{3}}$ group through the weak O$\cdots$H-N hydrogen bond with bond energy of -6.0 kcal/mol as the intermediate I5 and the geometric parameters are shown in FIG. 3. At transition state (TS4) the distance between O and B is shortened to 2.19 Å from 3.32 Å in I5. The formed $^*$BH($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ group locates on the C atom neighboring to Pt atom (I6). The O-H bond pointing to Pt atom is 0.04 Å longer than the other one. The elongated O-H bond easily breaks with an energy barrier of 8.9 kcal/mol, the released reaction energy is 11.7 kcal/mol. At transition state (TS5), the O-H bond length is 1.98 Å. The detached hydrogen atom adsorbs on the Pt-C bridge site and the $^*$BH(OH)N$\rm{H}_\rm{3}$ group binds to Pt atom (I7).

FIG. 3 The relative energy profiles of the hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ by the first and second $\rm{H}_\rm{2}$O molecules on P$\rm{t_{1}}$/Gr-O. Critical bond lengths are labeled (in unit of Å).

Then for the evolution of I7, the most favorable way is the attachment of the second $\rm{H}_\rm{2}$O molecule to $^*$BH(OH)N$\rm{H}_\rm{3}$, which is shown in FIG. 3 as the formation of I9 from I8 via TS6. The formation of $^*$BH(OH)($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ by combination of a $\rm{H}_\rm{2}$O molecule and $^*$BH(OH)N$\rm{H}_\rm{3}$ is an exothermic step (7.1 kcal/mol) with a relatively low energy barrier of 7.3 kcal/mol. At transition state (TS6), $^*$BH(OH)N$\rm{H}_\rm{3}$ leaves from the Pt atom with the Pt-B distance of 4.12 Å and the bond distance of O-B is 2.91 Å. At I9, $^*$BH(OH)($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$ adsorbs on the catalyst through one hydrogen atom in ($\rm{H}_\rm{2}$O) fragment and the O-H bond length is elongated to 1.04 Å. The breaking of the elongated O-H bond needs to conquer an energy barrier of 9.7 kcal/mol and it is an endothermic process with a reaction energy of 4.8 kcal/mol. The formed BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$ physically adsorbs on the P$\rm{t}_{1}$/Gr-O surface and the second isolated H atom adsorbs on the C atom (I10). The adsorption energy of BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$ is only 0.3 kcal/mol and it is supposed that the formed BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$ can easily dissolve in water solution.

FIG. 4 The relative energy (with I11$''$ included) profiles of the recovery of P$\rm{t}_{1}$/Gr-O catalyst. Critical bond lengths are labeled (in unit of Å).
3. Recovery of P$\rm{t}_{1}$/Gr-O catalyst

After the releasing of BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$, two hydrogen atoms present on P$\rm{t}_{1}$/Gr-O (I11$'$). By removing hydrogen atoms, the P$\rm{t}_{1}$/Gr-O catalyst can be recovered. The release of molecular hydrogen can be separated as the transfer of C bonded atomic hydrogen, the formation of chemically adsorbed molecular hydrogen and the desorption of hydrogen molecule. H transfers from I11$'$ to I12 via TS8 with an energy barrier of 11.6 kcal/mol. The distance between two hydrogen atoms are 3.71, 2.51, and 2.04 Å in I11$'$, TS8, and I12, respectively. Then the two hydrogen atoms combine with each other to form chemically adsorbed dihydrogen with an energy barrier of 8.8 kcal/mol. At transition state (TS9), the H-H bond length is 1.17 Å. The adsorption energy of chemically adsorbed hydrogen molecule is 2.8 kcal/mol, which indicates that the formed dihydrogen is ready to desorb from the catalyst. After the releasing of gas phase hydrogen molecule, the P$\rm{t}_{1}$/Gr-O catalyst recovers. The recovery of catalyst is an endothermic process with energy of 8.3 kcal/mol, which is easy to be conquered at room temperature if the entropy increasing is considered for the releasing of gas phase hydrogen molecule.

4. The release of the third hydrogen

Now, only two hydrogen molecules are released from one B$\rm{H}_\rm{3}$N$\rm{H}_\rm{3}$ molecule. The third molecular hydrogen comes from further hydrolysis of formed solvated BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$. In solvated BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$, the B-N bond length is 1.67 Å, which is 0.05 Å longer than that of the solvated isolated B$\rm{H}_\rm{3}$N$\rm{H}_\rm{3}$. The B-N bond is easy to be broken with the attack of one water molecule with an energy barrier of 10.6 kcal/mol, which is close to the reported B-N bond dissociation energy of 10.0 kcal/mol in N$\rm{H}_\rm{3}$B$\rm{H}_\rm{2}$OH [47] and much lower than that of the B-N bond breaking in B$\rm{H}_\rm{3}$N$\rm{H}_\rm{3}$ (38.0 kcal/mol). After the cleavage of B-N bond, the resulted BH$\rm{(OH)}_\rm{2}$, $\rm{H}_\rm{2}$O and N$\rm{H}_\rm{3}$ molecules form a cluster (I15) by HO$\cdots$HO-H and NH$\cdots$O$\rm{H}_\rm{2}$ hydrogen bonds. Then a complex BH$\rm{(OH)}_\rm{3}$$\cdots$N$\rm{H}_\rm{4}$ (I16) is formed by the dissociation of water with an energy barrier of 2.8 kcal/mol. The hydrogen bond length in I16 is 1.49 Å and the distance between the left H(-B) and the nearest H(-N) is 3.22 Å. The combination of the two hydrogen atoms conquers an energy barrier of 11.6 kcal/mol and releases energy of 8.6 kcal/mol. At transition state (TS13), the bond lengths of B-H and N-H are elongated to 1.52 and 1.39 Å, respectively, while the H-H distance is shortened to 0.95 Å. The generated products also include N$\rm{H}_\rm{3}$ and B$\rm{(OH)}_\rm{3}$. The species of products have not been definitely determined yet. Banu et al. used B$\rm{(OH)}_\rm{3}$, $\rm{H}_\rm{2}$ and N$\rm{H}_\rm{3}$ as the products for hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ without catalysts in gas phase and aqueous phase [44]. Chen et al. proposed that a N$\rm{H}_\rm{4}$B$\rm{(OH)}_\rm{4}$-B$\rm{(OH)}_\rm{3}$ mixture rather than N$\rm{H}_\rm{4}$B$\rm{O}_\rm{2}$ is the main B-containing byproducts after hydrolysis of B$\rm{H}_\rm{3}$N$\rm{H}_\rm{3}$ catalyzed by a Pt/CNT catalyst [27]. But this may be the evolution of hydrolysis species, which are not critical for the production of hydrogen.

FIG. 5 The relative energy (with I11$'$ included) profiles of hydrolysis of the resulted BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$ group in water solution. Critical bond lengths are labeled (in unit of Å).

The hydrolysis of the resulted BH$\rm{(OH)}_\rm{2}$ group in I15 over P$\rm{t}_{1}$/Gr-O surface is also considered. It is found a BH$\rm{(OH)}_\rm{2}$ molecule adsorbs weakly on P$\rm{t}_{1}$/Gr-O catalyst with the adsorption energy of -0.04 kcal/mol, which is much lower than that of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ (-9.8 kcal/mol). The hydrolysis of BH$\rm{(OH)}_\rm{2}$ groups can also proceed on P$\rm{t}_{1}$/Gr-O (as shown in FIG. S3 in supplementary materials) without the precover with N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ or atomic hydrogen. The energy barrier of BH$\rm{(OH)}_\rm{2}$ hydrolysis on P$\rm{t}_{1}$/Gr-O is significantly reduced to 4.8 kcal/mol compared to that (39.5 kcal/mol) of BH$\rm{(OH)}_\rm{2}$ hydrolysis without catalysts reported by Banu et al. [44].

Based on the aforementioned reaction pathways, the optimal reaction processes of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis on P$\rm{t}_{1}$/Gr-O are depicted in FIG. 6 as: (ⅰ) the preferential adsorption of one N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ molecule on P$\rm{t}_{1}$/Gr-O and the activation of B-H bonds, (ⅱ) the first B-H bond breaking, (ⅲ) the formation of molecularly adsorbed dihydrogen from the second B-H bond breaking, (ⅳ) the desorption of the first gas phase hydrogen molecule; (ⅴ) the attacking of the first water molecule, (ⅵ) the attacking of the second water molecule, (ⅶ) the desorption of BH$\rm{(OH)}_\rm{2}$N$\rm{H}_\rm{3}$, (ⅷ) the desorption of the second gas phase hydrogen molecule and the recovery of catalyst, (ⅸ) the attacking of the third water molecule, (ⅹ) the releasing of the third hydrogen molecule and the formation of final products.

FIG. 6 Proposed mechanism for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis over P$\rm{t}_{1}$/Gr-O surface.

Through the whole reaction pathways for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis, it is found that the attacking of first $\rm{H}_\rm{2}$O molecule to $^*$BHN$\rm{H}_\rm{3}$ ($^*$BHN$\rm{H}_\rm{3}$ $+$$\rm{H}_\rm{2}$O$\rightarrow$ $^*$B($\rm{H}_\rm{2}$O)HN$\rm{H}_\rm{3}$) is the rate-limiting step on P$\rm{t}_{1}$/Gr-O with an energy barrier of 16.1 kcal/mol. To gain more insight into the origin of the reaction activity of $\rm{H}_\rm{2}$O molecules reacting with the $^*$BN$\rm{H}_3$ group, the local density of states (LDOS) projected onto B atom and $\rm{H}_\rm{2}$O molecule in the I5, TS4, and I6 over P$\rm{t}_{1}$/Gr-O has been split as shown in FIG. 7. The highest occupied molecular orbital (HOMO) of water, 1$\rm{b}_\rm{1}$ state, is contributed by the lone pair electrons of oxygen atom. B atom has empty orbitals which can accept electrons from donation atom. At TS4, the density states of 1$\rm{b}_\rm{1}$ expanded and slightly overlapped with the orbitals of B atom. For the interaction between water and $^*$BHN$\rm{H}_\rm{3}$ group, the empty orbitals shift towards low energy direction. At I6, the orbitals of water molecule effectively overlap with that of B atom, which indicates the chemical bonding between water molecule and B atom. For the donation of lone pair electrons, the density of states of water molecule decreases and that of B atom increases below fermi level. The orbitals above fermi level shift towards low energy direction for the formation of chemical bond, which makes the hydrolysis of $^*$BHN$\rm{H}_\rm{3}$ group proceed.

FIG. 7 Left panels are structures of I5, TS4, and I6 in FIG. 3, right panel is the local density of states (LDOS) projected onto B atom and $\rm{H}_\rm{2}$O molecule in the I5, TS4, and I6 over P$\rm{t}_{1}$/Gr-O surface. $E_\rm{f}$ denotes the Fermi level. The dot dashed line shows the density states (energy levels) of isolated water molecule with solvent effect included. The energy levels are shifted according to the O 1s orbitals of water molecule in I5 and $\rm{H}_\rm{2}$O(l).
Ⅳ. CONCLUSION

In conclusion, the N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis mechanisms on single Pt atom anchored to the plane of graphene with a defective carbon atom replaced by an oxygen atom were examined by using first-principles calculations. The P$\rm{t}_{1}$/Gr-O catalyst prefers to activate the B-H bonds, and first hydrogen molecule is released by two detached H atoms from B-H bonds. The left $^*$BHN$\rm{H}_\rm{3}$ combines with two $\rm{H}_\rm{2}$O molecules to proceed the hydrolysis process. The combination of left $^*$BHN$\rm{H}_\rm{3}$ with the first $\rm{H}_\rm{2}$O molecule is the rate-limiting step with an energy barrier of 16.1 kcal/mol. Both attached water molecules detach one hydrogen atom to form N$\rm{H}_\rm{3}$BH$\rm{(OH)}_\rm{2}$, which can be easily hydrolyzed in water solvent to release one hydrogen molecule without catalyst. By combination and releasing of the two surface left hydrogen atoms, P$\rm{t}_{1}$/Gr-O can be recovered. A whole mechanism of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis over solid catalysts is presented for the first time. Based on the calculated results the P$\rm{t}_{1}$/Gr-O catalyst exhibits high catalytic activity for N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ hydrolysis at room temperature. Thus Pt single atoms anchored at a designed configuration on graphene nanosheet can perform high activity for hydrolysis of N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ at room temperature.

Supplementary materials:The bond breakage of B-N bond in N$\rm{H}_\rm{3}$B$\rm{H}_\rm{3}$ attacked by one $\rm{H}_\rm{2}$O molecule; the three possible reaction pathways of the $^*$B$\rm{H}_\rm{2}$N$\rm{H}_\rm{3}$ including N-H bond breaking to form B$\rm{H}_\rm{2}$N$\rm{H}_\rm{2}$, direct production of a gas phase hydrogen molecule, and hydrolysis of $^*$B$\rm{H}_\rm{2}$N$\rm{H}_\rm{3}$; the three possible reaction pathways of the $^*$BHN$\rm{H}_\rm{3}$ including the B-H bond breaking, the N-H bond breaking, and the attachment of one water molecule to form Pt bound BH($\rm{H}_\rm{2}$O)N$\rm{H}_\rm{3}$; and the hydroxylation pathways of BH$\rm{(OH)}_\rm{2}$ on P$\rm{t}_{1}$/Gr-O are shown in FIG. S1-S3.

Ⅴ. ACKNOWLEDGMENTS

This work is supported by the National Natural Science Foundation of China (No.21473167 and No.21688102) and the National Key Research and Development Program of China (No.2016YFA0200604), and the Fundamental Research Funds for the Central Universities (WK3430000005, WK2340000065), and the China Scholarship Council (CSC) (No.201706345015). We used computational resources of Super-computing Center of University of Science and Technology of China, Guangzhou and Shanghai Supercomputer Centers.

Reference
[1] U. Eberle, M. Felderhoff, and F. Schüth, Angew. Chem. Int. Ed. 48 , 6608 (2009). DOI:10.1002/anie.v48:36
[2] T. B. Marder, Angew. Chem. Int. Ed. 46 , 8116 (2007). DOI:10.1002/(ISSN)1521-3773
[3] C. W. Hamilton, R. T. Baker, A. Staubitz, and I. Manners, Chem. Soc. Rev. 38 , 279 (2009). DOI:10.1039/B800312M
[4] J. Yang, A. Sudik, C. Wolverton, and D. J. Siegel, Chem. Soc. Rev. 39 , 656 (2010).
[5] M. Yadav, and Q. Xu, Energy Environ. Sci. 5 , 9698 (2012). DOI:10.1039/c2ee22937d
[6] F. H. Stephens, V. Pons, and R. Tom Baker, Dalton Trans. 2 , 2613 (2007).
[7] B. Peng, and J. Chen, Energy Environ. Sci. 1 , 479 (2008).
[8] A. Staubitz, A. P. M. Robertson, and I. Manners, Chem. Rev. 110 , 4079 (2010). DOI:10.1021/cr100088b
[9] A. Karkamkar, C. Aardahl, and T. Autrey, Mater. Sci. 10 , 6 (2007).
[10] M. Chandra, and Q. Xu, J. Power Sources 168 , 135 (2007). DOI:10.1016/j.jpowsour.2007.03.015
[11] H. Shioyama, and Q. Xu, J. Am. Chem. Soc. 134 , 13926 (2012). DOI:10.1021/ja3043905
[12] W. Chen, J. Ji, X. Feng, X. Duan, G. Qian, P. Li, X. Zhou, D. Chen, and W. Yuan, J. Am. Chem. Soc. 136 , 16736 (2014). DOI:10.1021/ja509778y
[13] W. Chen, J. Ji, X. Duan, G. Qian, P. Li, X. Zhou, D. Chen, and W. Yuan, Chem. Commun. 50 , 2142 (2014). DOI:10.1039/c3cc48027e
[14] Y. Chen, X. Yang, M. Kitta, and Q. Xu, Nano Res. 10 , 3811 (2017). DOI:10.1007/s12274-017-1593-4
[15] K. Aranishi, Q. L. Zhu, and Q. Xu, ChemCatChem. 6 , 1375 (2014).
[16] J. Hu, Z. Chen, M. Li, X. Zhou, and H. Lu, ACS Appl. Mater. Interfaces 6 , 13191 (2014). DOI:10.1021/am503037k
[17] Z. Li, T. He, L. Liu, W. Chen, M. Zhang, G. Wu, and P. Chen, Chem. Sci. 8 , 781 (2017). DOI:10.1039/C6SC02456D
[18] P. Liu, X. Gu, K. Kang, H. Zhang, J. Cheng, and H. Su, ACS Appl. Mater. Interfaces 9 , 10759 (2017). DOI:10.1021/acsami.7b01161
[19] C.Y. Peng, L. Kang, S. Cao, Y. Chen, Z. S. Lin, and W. F. Fu, Angew. Chem. Int. Ed. 54 , 15725 (2015). DOI:10.1002/anie.201508113
[20] G. Zhao, J. Zhong, J. Wang, T. K. Sham, X. Sun, and S. T. Lee, Nanoscale 7 , 9715 (2015). DOI:10.1039/C5NR01168J
[21] C. Wang, J. Tuninetti, Z. Wang, C. Zhang, R. Ciganda, L. Salmon, S. Moya, J. Ruiz, and D. Astruc, J. Am. Chem. Soc. 139 , 11610 (2017). DOI:10.1021/jacs.7b06859
[22] K. Guo, H. Li, and Z. Yu, ACS Appl. Mater. Interfaces 10 , 517 (2018). DOI:10.1021/acsami.7b14166
[23] Q. Xu, and M. Chandra, J. Power Sources 163 , 364 (2006). DOI:10.1016/j.jpowsour.2006.09.043
[24] M. Kaya, M. Zahmakiran, S. Özkar, and M. Volkan, ACS Appl. Mater. Interfaces 4 , 3866 (2012). DOI:10.1021/am3005994
[25] D. Zhang, P. Liu, S. Xiao, X. Qian, H. Zhang, M. Wen, Y. Kuwahara, K. Mori, H. Li, and H. Yamashita, Nanoscale 8 , 7749 (2016). DOI:10.1039/C5NR07505J
[26] H. Ma, and C. Na, ACS Catal. 5 , 1726 (2015). DOI:10.1021/cs5019524
[27] W. Chen, D. Li, Z. Wang, G. Qian, Z. Sui, X. Duan, X. Zhou, I. Yeboah, and D. Chen, AIChE J. 63 , 60 (2017). DOI:10.1002/aic.v63.1
[28] W. Chen, D. Li, C. Peng, G. Qian, X. Duan, D. Chen, and X. Zhou, J. Catal. 356 , 186 (2017). DOI:10.1016/j.jcat.2017.10.016
[29] Z. Li, T. He, D. Matsumura, S. Miao, A. Wu, L. Liu, G. Wu, and P. Chen, ACS Catal. 7 , 6762 (2017). DOI:10.1021/acscatal.7b01790
[30] C. C. Hou, Q. Li, C. J. Wang, C. Y. Peng, Q. Q. Chen, H. F. Ye, W. F. Fu, C. M. Che, N. López, and Y. Chen, Energy Environ. Sci. 10 , 1770 (2017). DOI:10.1039/C7EE01553D
[31] W. W. Zhan, Q. L. Zhu, and Q. Xu, ACS Catal. 6 , 6892 (2016). DOI:10.1021/acscatal.6b02209
[32] B. Qiao, A. Wang, X. Yang, L. F. Allard, Z. Jiang, Y. Cui, J. Liu, J. Li, and T. Zhang, Nat. Chem. 3 , 634 (2011). DOI:10.1038/nchem.1095
[33] H. Zhang, T. Watanabe, M. Okumura, M. Haruta, and N. Toshima, Nat. Mater. 11 , 49 (2012). DOI:10.1038/nmat3143
[34] X. Yang, A. Wang, B. Qiao, and J. Li, Acc. Chem. Res. 46 , 1740 (2013). DOI:10.1021/ar300361m
[35] Y. Tang, X. Dai, Z. Yang, L. Pan, W. Chen, D. Ma, and Z. Lu, Phys. Chem. Chem. Phys. 16 , 7887 (2014). DOI:10.1039/C4CP00149D
[36] S. Sun, G. Zhang, N. Gauquelin, N. Chen, J. Zhou, S. Yang, W. Chen, X. Meng, D. Geng, M. N. Banis, R. Li, S. Ye, S. Knights, G. A. Botton, T. K. Sham, and X. Sun, Sci. Rep. 3 , 1775 (2013). DOI:10.1038/srep01775
[37] H. Yan, H. Cheng, H. Yi, Y. Lin, T. Yao, C. Wang, J. Li, S. Wei, and J. Lu, J. Am. Chem. Soc. 137 , 10484 (2015). DOI:10.1021/jacs.5b06485
[38] H. Yan, Y. Lin, H. Wu, W. Zhang, Z. Sun, H. Cheng, W. Liu, C. Wang, J. Li, X. Huang, T. Yao, J. Yang, S. Wei, and J. Lu, Nat. Commun. 8 , 1 (2017). DOI:10.1038/s41467-016-0009-6
[39] B. Delley, Phys. Rev. 66 , 155125 (2002). DOI:10.1103/PhysRevB.66.155125
[40] J. P. Perdew, K. Burke, and M. Ernzerhof, Phys. Rev. Lett. 77 , 3865 (1996). DOI:10.1103/PhysRevLett.77.3865
[41] B. Delley, J. Chem. Phys. 92 , 508 (1990). DOI:10.1063/1.458452
[42] B. Delley, J. Chem. Phys. 113 , 7756 (2000). DOI:10.1063/1.1316015
[43] A. Klamt, and G. Schüürmann, J. Chem. Soc. Perkin Trans. 2 , 799 (1993).
[44] T. Banu, T. Debnath, T. Ash, and A. K. Das, J. Chem. Phys. 143 , 194305 (2015). DOI:10.1063/1.4935933
[45] M. Tong, Z. Yin, Y. Wang, and G. Chen, Int. J. Hydrogen Energy 38 , 15285 (2013). DOI:10.1016/j.ijhydene.2013.09.097
[46] Y. Zhang, Y. Zhang, Z. H. Qi, Y. Gao, W. Liu, and Y. Wang, Int. J. Hydrogen Energy 41 , 17208 (2016). DOI:10.1016/j.ijhydene.2016.07.209
[47] H. A. LeTourneau, R. E. Birsch, G. Korbeck, and J. L. Radkiewicz-Poutsma, J. Phys. Chem. A 109 , 12014 (2005).
氧化石墨烯负载的Pt单原子催化硼胺烷水解机理的理论研究
吴红a, 罗其全a, 张瑞奇a, 张文华b,c,d, 杨金龙a,c     
a. 中国科学技术大学合肥微尺度物质科学国家研究中心,合肥 230026;
b. 中国科学技术大学,中国科学院能量转换材料重点实验室,合肥 230026;
c. 中国科学技术大学量子信息与量子科技前沿协同创新中心,合肥 230026;
d. 澳洲国立大学物理与工程研究学院应用数学系,堪培拉 2600
摘要: 本文研究了氧化石墨烯负载Pt单原子(Pt$_1$/Gr-O)催化硼胺烷(NH$_3$BH$_3$)全水解反应机理,即一分子的NH$_3$BH$_3$生成三分子的氢气(H$_2$)的过程.在水解路径中,首先吸附的硼胺烷连续断裂两个B$-$H键生成第一分子的H$_2$.接着,一个H$_2$O分子与$^*$BHNH$_3$基团($^*$表示吸附态)反应生成$^*$BH(H$_2$O)NH$_3$,其中伸长的O$-$H键断裂后形成$^*$BH(OH)NH$_3$.然后,第二个H$_2$O与$^*$BH(OH)NH$_3$反应生成$^*$BH(OH)(H$_2$O)NH$_3$,在指向Pt$_1$/Gr-O表面的O$-$H断裂后,生成BH(OH)$_2$NH$_3$并脱附到水溶液中.两个水分子脱氢产生的两个H原子脱附生成第二个H$_2$分子,且Pt$_1$/Gr-O催化剂恢复.脱附后的BH(OH)$_2$NH$_3$在水溶液中水解生成第三个H$_2$分子.纵观整个水解反应,H$_2$O分子和$^*$BHNH$_3$基团的结合是反应速控步,其反应能垒是16.1 kcal/mol.因此,Pt$_1$/Gr-O有希望成为室温催化NH$_3$BH$_3$全水解催化剂.
关键词: 密度泛函理论    单原子催化    Pt    氧化石墨烯    硼胺烷水解