Abstract
Industrial catalysts, consisting of metal species dispersed on a porous surface, are typically prepared by hydrogen treatment at high temperatures, and the migration of hydrogen constitutes the key elementary reaction that mediates the metal-support interactions and the generation of active catalytic sites. A detailed modeling of these processes is challenging especially for systems involving disordered surfaces. A debated issue is the role of the support “reducibility” on the mechanism of H-spillover processes. Transition-metal oxides such as titania significantly improve the activity and selectivity of catalysts supported on “non-reducible” oxides, such as silica, particularly in hydrogenation and dehydrogenation processes. To gain insight into the mechanism of H-migration in disordered catalysts and nano-particles, a comprehensive DFT-analysis of the potential energy surfaces is carried out for the transfer of H-atoms from a palladium-tetramer catalyst to a silica-support, represented by a substituted siloxane ring, doped with “reducible” titania. The H-migration to non-stoichiometric supports occurs via both a direct and H 2 -assisted transfer of H-atoms when the metal-catalyst is anchored to the non-bonding oxygen atoms of the support (defect sites). The calculations revealed that the transfer to different types of supports proceeds through identical pathways but significantly different barriers. The titania-promotion, as well as the addition of dihydrogen ligands to the catalyst, decreases the direct and H 2 -assisted H-migration barriers. Due to the extended transition state structures, the H2-assisted mechanism provides access to more distant and hindered active centers, and thus can account for the “bottleneck” particle-to-particle (along grain boundaries) transport of hydrogen atoms. The H-migration to titania-promoted stoichiometric (defect-free) supports generates intermetallic Pd-Ti bonds, in contrast to the pristine silica-based catalysts, which do not form analogous bonds between palladium and silicon centers of the support.
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Khoobiar S (1964) J Phys Chem 68:411
Benson JE, Kohn HW, Boudart M (1966) J Catal 5:307
Levy RB, Boudart M (1974) J Catal 32:304
Somorjai GA (1994) Introduction to surface chemistry and catalysis. Wiley-Interscience, New York, p 450
Ruckenstein E, Sushumna I (1988) In: Paál Z, Menon PG (eds) Hydrogen effects in catalysis. Marcel Dekker, New York, p 259
Conner WC, Falconer JL (1995) Chem Rev 95:759
Roessner F, Roland U (1996) J Mol Catal A 112:401
Rozanov VV, Krylov OV (1997) Russ Chem Rev 66:107
Pajonk GM (2000) Appl Catal A 202:157
Pajonk GM (1994) Heterog Chem Rev 1:329
Prins R (2012) Chem Rev 112:2714
Chen L, Cooper AC, Pez GP, Cheng H (2008) J Phys Chem C 112:1755
Sha X, Chen L, Cooper AC, Pez GP, Cheng H (2009) J Phys Chem C 113:11399
Hao S, Sholl DS (2013) J Phys Chem C 117:1217
Niklasson C (1988) Ind Eng Chem Res 27:1984
Xi Y, Zhang Q, Cheng H (2014) J Phys Chem C 118:494
Lykhach Y, Staudt T, Vorohkta M, Skala T, Johanek V, Prince KC, Matolin V, Libuda J (2012) J Catal 285:6
Nakano K, Kusunoki K (1985) Chem Eng Commun 34:99
Lu J, Aydin C, Browning ND, Gates BC (2012) J Am Chem Soc 134:5022
Cremer PS, Somorjai GA (1995) J Chem Soc, Faraday Trans 91:3671
Li Y, Yang RT (2006) J Am Chem Soc 128:726
Li Y, Yang FH, Yang RT (2007) J Phys Chem C 111:3405
Jung JH, Rim JA, Lee SJ, Cho SJ, Kim SY, Kang JK, Kim YM, Kim YJ (2007) J Phys Chem C 111:2679
Huizinga T, Prins R (1981) J Phys Chem 85:2156
Panayotov DA, Yates JT Jr (2007) J Phys Chem C 111:2959
Eriksson M, Petersson L-G (1994) Surf Sci 311:139
Gates BC (1995) Chem Rev 95:511
Polshettiwar V, Len C, Fihri A (2009) Coord Chem Rev 253:2599
Corti G, Zhan Y, Wang L, Hare B, Cantrell T, Beaux M II, Prakash T, Ytreberg FM, Miller MA, McIlroy DN (2013) J Phys D 46:505307
Chen H-W, White JM (1986) J Mol Catal 35:355
Vannice MA, Neikam WC (1971) J Catal 20:260
Roland U, Braunschweig T, Roessner F (1997) J Mol Catal A 127:61
Zolotarev YuA, Dorokhova EM, Nezavibatko VN, Borisov YuA, Rosenberg SG, Velikodvorskaia GA, Neumivakin LV, Zverlov VV, Myasoedov NF (1995) Amino Acids 8:353
Shishido T, Hattori H (1996) Appl Catal A 146:157
Hattori H (1993) Studies in surface science and catalysis. Elsevier, Kyoto
Lenz DH, Conner WC (1988) J Catal 112:116
Chiaranussati P, Gladden LF, Grifiths RW, Jackson SD, Webb G (1993) Trans Inst Chem Eng 71:267
Carley AF, Edwards HA, Mile B, Roberts MW, Rowlands CC (1994) J Chem Soc Faraday Trans 90:3341
Nasluzov VA, Rivanenkov VV, Shor AM, Neyman KM, Birkenheuer U, Rosch N (2002) Int J Quant Chem 90:386
Wu H-Y, Fan X, Kuo J-L, Deng W-Q (2011) J Phys Chem C 115:9241
Singh AK, Ribas MA, Yakobson BI (2009) ACS Nano 3:1657
Psofogiannakis GM, Froudakis GE (2009) J Am Chem Soc 131:15133
Choi S, Jeong K, Park JY, Lee YS (2015) Bull Korean Chem Soc 36:777
Im J, Shin H, Jang H, Kim H, Choi M (2014) Nature Commun 5:3370
Juarez-Mosqueda R, Mavrandonakis A, Kuc AB, Pettersson LGM, Heine T (2015) Front Chem 3:1
Cheng H, Chen L, Cooper AC, Sha X, Pez GP (2008) Energy Environ Sci 1:338
Psofogiannakisa GM, Froudakis GE (2011) Chem Commun 47:7933
Gates BC, Gucz, L, Knözinger H (eds) (1986) Metal clusters in catalysis. Elsevier, Amsterdam
Estiu GL, Zerner MC (1994) J Phys Chem 98:4793
Gomes JRB, Lodziana Z, Illas F (2003) J Phys Chem B 107:6411
Godet J, Pasquarello A (2005) Macroelectron Eng 80:288
Yokozawa A, Miyamoto Y (1997) Phys Rev B 55:13783
Cui Q, Musaev DG, Morokuma K (1998) J Chem Phys 108:8418
Cui Q, Musaev DG, Morokuma KJ (1998) Phys Chem 102:6373
Dai D, Liao DW, Balasubramanian K (1995) J Chem Phys 102:7530
Dai D, Balasubramanian K (1995) J Chem Phys 103:648
Balasubramanian K (1989) J Chem Phys 91:307
Efremenko I, German ED, Sheintuch M (2000) J Phys Chem A 104:8089
Zacarias AG, Castro M, Tour JM, Seminario JM (1999) J Phys Chem A 103:7692
Pereira JCG, Catlow CRA, Price GD (1999) J Phys Chem A 103:3252
Pereira JCG, Catlow CRA, Price GD (1999) J Phys Chem A 103:3268
Valerio G, Toulhout H (1996) J Phys Chem 100:10827
Blöchl PE (2000) Phys Rev B 62:6158
Ruckenstein E, Dadyburjor DB (1983) Rev Chem Eng 1:251
Che M, Bennett CO (1989) Adv Catal 36:55
Bell AT (2003) Science 299:1688
Somorjai GA, Borodko YG (2001) Catal Lett 76:1
Witham CA, Huang W, Tsung C-K, Kuhn JN, Somorjai GA, Toste FD (2010) Nature Chem 2:36
Dixon DA, Katz A, Arslan I, Gates BC (2014) Catal Let 144:1785
Catlow CRA, French SA, Sokol AA, Thomas JM (2005) Phil Trans R Soc A 363:913
Krylov OV, Kiselev VF (1989) Adsorption and catalysis on transition metals and their oxides. Springer, Berlin
Sauer J, Ugliengo P, Garrone E, Saunders VR (1994) Chem Rev 94:2095
Peri JB (1966) J Phys Chem 70:2937
Hockey JA, Pethica BA (1971) Trans Farad Soc 57:2247
Conner WC, Pajonk GM, Teichner SJ (1986) Adv Catal 34:1
Fuchs PL (ed) (2013) Handbook of reagents for organic synthesis, reagents for silicon-mediated organic synthesis. Wiley, New York, p 310
Maiti A, Gee RH, Maxwell R, Saab AP (2007) Chem Phys Lett 440:244
Goursot A, Papai I, Salahub DR (1992) J Am Chem Soc 114:7452
de Carneiro JWM, de Cruz MTM (2008) J Phys Chem A 112:8929
Fogelberg J, Eriksson M, Dannetun H, Petersson LG (1995) J Appl Phys 78:988
Nava P (2005) Density functional theory calculations on palladium clusters and on an AgInS semiconductor compound. Cuvillier Verlag, Gottingen
Asatryan R, Ruckenstein E (2014) Catal Rev Sci Eng 56:403
Kang JH, Shin EW, Kim WJ, Park JD, Moon SH (2000) Catal Today 63:183
Rieck JS, Bell AT (1985) J Catal 96:88
Chenakin SP, Melaet G, Szukiewicz R, Kruse N (2014) J Catal 312:1
Ruckenstein E (1987) The role of interactions and surface phenomena in sintering and redispersion of supported metal catalysts. In: Stevenson SA, Dumesic JA, Baker RTK, Ruckenstein E (eds) Metal-support interactions in catalysis, sintering and redispersion. van Nostrand Reinhold Company, New York, p 139
Bracey JD, Burch R (1984) J Catal 86:384
Wang S-Y, Moon SH, Albert VM (1981) J Catal 71:167
Venezia AM, Di Carlo G, Pantaleo G, Liotta LF, Melaet G, Kruse N (2009) Appl Catal B 88:430
Buijink JFK, Lange JP, Bos ANR, Horton AD, Nielein FGM (2008) In: Oyama ST (ed) Mechanisms in homogeneous and heterogeneous epoxidation catalysis. Elsevier, Amsterdam, p 355
Castillo R, Koch B, Ruiz P, Delmon B (1996) J Catal 161:524
Dadyburjor DB, Jewur SS, Ruckenstein E (1979) Catal Rev Sci Eng 19:293
Sankar G, Thomas JM, Catlow CRA, Barker CM, Gleeson D, Kaltsoyannis N (2001) J Phys Chem B 105:9028
Gao X, Wachs IE (1999) Catal Today 51:233
Dutoit DCM, Schneider M, Baiker A (1995) J Catal 153:165
Kumar D, Ali A (2012) Energy Fuels 26:2953
Chen J, Halin SJA, Schouten JC, Nijhuis TA (2011) Faraday Discuss 152:321
Li Y, Xu B, Fan Y, Feng N, Qiu A, He JMJ, Yang H, Chena Y (2004) J Mol Catal A 216:107
Dropsch H (1997) Baerns M Appl Catal A 158:163
Bowker M, Stone P, Bennett RA, Perkins N (2002) Surf Sci 497:155
Wells DH Jr, Delgass WN, Thomson KT (2004) J Am Chem Soc 126:2956
Oldroyd RD, Sankar G, Thomas JM, Ozkaya D (1998) J Phys Chem B 102:1849
Hu S, Willey RJ, Notari B (2003) J Catal 220:240
Liu T, Hacarlioglu P, Oyama ST, Luoa M-F, Pan X-R, Lu J-Q (2009) J Catal 267:202
Adams BD, Chen A (2011) Materialstoday 14:282
Moc J, Musaev DG, Morokuma K (2000) J Phys Chem A 104:11606
Wang Y, Cao Z, Zhang Q (2003) Chem Phys Lett 376:96
Asatryan R, Bozzelli JW, Ruckenstein E (2012) J Phys Chem A 116:11618
Asatryan R (2010) Chem Phys Lett 498:263
Asatryan R, Bozzelli JW, da Silva G, Swinnen S, Nguyen MT (2010) J Phys Chem A 114:6235
Asatryan R, Ruckenstein E (2012) Dihydrogen Catalysis Relevant to the Fixation of Nitrogen, 38th Northeast Regional ACS Meeting. Rochester, NY
Bianchi D, Lacroix M, Pajonk GM, Teichner SJ (1981) J Catal 68:411
Spencer MS, Burch R (1990) Golunski SE J Catal 126:311
Rößner F (2008) Handbook of heterogeneous catalysis, Part 5, spillover effects. Wiley, New York
Becke AD (1992) J Chem Phys 96:2155
Lee C, Yang W, Parr RG (1988) Phys Rev B 37:785
Dunning Jr TH, Hay PJ (1976). In Schaefer III HF (ed) Modern theoretical chemistry, vol 3, p 1. Plenum, New York
Frenking G, Deubel DV (2005) Theoretical aspects of transition metal catalysis. Springer, Berlin
Limtrakul J, Tantanak D (1995) J Mol Struct Theochem 358:179
Hay PJ, Wadt WR (1985) J Chem Phys 82:270
Barone G, Duca D, Ferrante F, LaManna G (2010) Int J Quant Chem 110:558
Tauster SJ (1987) Acc Chem Res 20:389
Roy LE, Hay PJ, Martin RL (2008) J Chem Theory Comput 4:1029
Asatryan R, Ruckenstein E (2013) J Phys Chem A 117:10912
Fayet P, Kaldor A, Cox DM (1990) J Chem Phys 92:254
Pelzer AW, Jellenek J, Jackson KA (2013) J Phys Chem A 117:10407
Ni M, Zeng Z (2009) J Mol Structure: Theochem 910:14
Minaev BF, Ågren H (2001) Adv Quant Chem 40:191
Efremenko I (2001) J Mol Catal A 173:19
German ED, Efremenko I, Sheintuch MJ (2001) Phys Chem A 105:11312
Frisch MJ et al (2003) Gaussian 03, revision B04. Gaussian Inc, Pittsburgh
Glendening ED, Reed AE, Carpenter JE, Weinhold F (1998) NBO Version 3.1 TCI, University of Wisconsin, Madison
Johansson A, Forsth M, Rosen A (2003) Surf Sci 529:247
Dashevskii VG, Asatryan R, Baranov AP (1978) J Struct Chem 19:404
Dashevskii VG, Asatryan R, Baranov AP (1978) J Struct Chem 19:678
Chen B, Falconer JL (1992) J Catal 134:737
Kramer R, Andre M (1979) J Catal 58:287
Zuegg H, Kramer R (1986) Effect of H2 on the catalytic activity of Pt-SiO2 catalysts. In: Baker R, Tauster S, Dumesic J (eds), ACS Symp Series, vol 298, Washington DC, p 145
Merte LR, Peng G, Bechstein R, Rieboldt F, Farberow CA, Grabow LC, Kudernatsch W, Wendt S, Lægsgaard E, Mavrikakis M, Besenbacher F (2012) Science 336:889
Zhang Q, Tang S, Wallace RM (2001) Appl Surf Sci 172:41
Zhou C, Wu J, Nie A, Forrey RC, Tachibana A, Cheng H (2007) J Phys Chem C 111:12773
Mori T, Masuda H, Imai H, Miyamoto A, Hasebe R, Murakami Y (1983) J Phys Chem 87:3648
\(\varDelta {\text{H}}^{\text{o}}_{\text{f}}\) (298 K) = 57.79 kcal mol−1, NIST Chemistry Webbook (2011)
Yamabe T, Yamashita K, Kaminoyama M, Koizumi M, Tachibana A, Fukui K (1984) J Phys Chem 88:1459
Woolley M, Khairallah GN, da Silva G, Donnelly PS, O’Hair RAJ (2014) Organometallics 33:5185
Buszeka RJ, Francisco JS, Anglada JM (2011) Int Rev Phys Chem 30:335
Iuga C, Alvarez-Idaboy R, Vivier-Bunge A (2011) J Phys Chem A 115:5138
Kebede MA, Varner ME, Scharko NK, Gerber RB, Raff JD (2013) J Am Chem Soc 135:8606
Shi F-Q, Li X, Xia Y, Zhang L, Yu Z-X (2007) J Am Chem Soc 129:15503
Blanco-Rey M, Wales DJ, Jenkins SJ (2009) J Phys Chem C 113:16757
Fu Q, Wagner T, Olliges S, Carstanjen H-D (2005) J Phys Chem B 109:944
Ruckenstein E (1986) Interactions and surface phenomena in supported metal catalysts. In: Baker R, Tauster S, Dumesic J (Eds.), ACS Symposium Series, vol 298, Washington DC, p 153
Haller GL, Resasco DE (1989) Adv Catal 36:173
Juszczyk W, Karpiński Z, Łomot D, Pielaszek J (2003) J Catal 220:299
Meng JH, He ShGJ (2014) Phys Chem Lett 5:3890
Wass DF, Chapman AM (2013) Top Curr Chem 334:261
Petkov PS, Petrova GP, Vayssilov GN, Rösch N (2010) J Phys Chem C 114:8500
Acknowledgments
This work was supported in part by the Ruckenstein fund and the National Science Foundation under grant CBET-1330311. We would like to thank the reviewers for valuable comments. We acknowledge also the CCR SUNY at Buffalo for providing High Performance Computing resources.
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Appendix
Appendix
1.1 Appendix 1: Transfer of the Second H-atom in Primary Radicals
The removal of the first H-atom from the molecular intermediates II or III, representing the H-atom diffusion over the support, generates the primary radicals IV (Scheme 1). It is important to examine also the H-spillover of the remaining second H-atom of the Pd4 cluster onto the support.
Table 6 presents two secondary H-spillover processes for 2H2-capped radicals IV. The results indicate that the kinetic barriers are fairly high, compared to the first H-migration. Again, the promotion by titania decreases the barrier.
1.2 Appendix 2: The Role of Spin-Multiplicity
The current calculations, in accord with literature data, show that the ground state spin multiplicity of the bare Pd4 is a triplet, whereas the hydrogenated complex Pd42H is a singlet (cf. [58, 106, 127]). Therefore, a spin-crossing is expected to occur in the dissociative chemisorption of H2 on the bare Pd4, even though the product formation half-reaction, starting from TS in a singlet state, could well characterize the reaction probability. However, it is not expected any nonadiabatic transition between PESs corresponding to different spins for the activation and hydrogen migration in reactions over the palladium tetramer supported on pristine silica and doped by titania catalysts, which are all ground state singlets. The calculations confirmed that there is no intersystem crossing along the reaction pathways for the metabolism of hydrogen in supported systems. In addition, the triplet state reactions are more energy demanding than the singlet ones. Note also that no changes in the ground state spin multiplicity of Pd4 and of some other small Pdn clusters (n = 2–4, 7, 13) have been found as a result of molecular adsorption [126].
To evaluate the possible role of the high-spin states on H-migration to a defect-free surface, the singlet –state pathway involving the 2H2-capped catalyst (Fig. 8) was recalculated for the triplet state PES. The singlet–triplet splitting (ΔEST = 12.38 kcal mol−1) evaluated at B3LYP level is expected to be somewhat underestimated because of the over-stabilization of the high-spin state energies by this functional [82, 108]. Additional calculations based on the pure GGA-BP86 functional, indeed, provide the somewhat higher value of 15.81 kcal mol−1. However, this insignificant difference cannot alter the general conclusions involving the high-spin states at the B3LYP level.
The triplet pathway is also not significant because of the presence of the barrier of 23.7 kcal mol−1 height on the triplet route leading to the coordination of palladium cluster to a bridged O-atom. The triplet pathway could play a role only if the triplet state population is sufficiently high. However, lower by ca. 16 kcal mol−1 the singlet state reagent generates H-migration, and produces an intermetallic Pd-Ti bond and a H2O-moiety, at almost the same barrier of 23.5 kcal mol−1 (Fig. 7).
1.3 Appendix 3: Hydrogenolysis and Activation of the Second H2 Molecule
As noted in Table 4, in some titania-promoted systems, the nascent H2 molecule (co-catalyst HAHB) undergoes an interface heterolytic cleavage (hydrogenolysis) instead of H 2 -assisted transfer, or ligates molecularly to the metal. This can be explained by the lower coordination of Pd4 (fewer bonds to other Pd and H-atoms, as well as dihydrogen ligands), examined in Appendix 1.
Table 4 involves two hydrogenolysis reactions of the low-coordinated catalysts containing none- or one-H2 ligand. In both cases, the interfacial Pd–O bonds activate heterolytically the dihydrogen to form hydridic and protic H-atoms via almost equal barriers (ca. 15 kcal mol−1), almost independent of the number of adsorbed H2 ligands. Such a small effect of the H2-ligation constitutes an interesting issue which provides evidence for the dominance of interfacial forces in these reactions, as it occurs during H2 activation by the closed-shell AuCeO2 + catalyst [155]. By analogy, the covalently bound Pd ion can be considered as a strong Lewis acid, with the O2− ion viewed as a Lewis base. This provides a synergistic effect of the two separated sites with counter polarity, called intermolecular frustrated Lewis pairs [156].
Thus, the H2-assisted reactions generally occur when a basic coordination-sphere of the metal cluster (Pd4) is saturated by H-atoms and/or H2-ligands. The coordination deficiency concerns not only the defective systems described in Table 4 (palladium cluster residing on two NBOs), but also the stoichiometric-supported catalysts, where palladium is linked to the valence-saturated oxygen atoms of the support (OH-groups with H-cover atoms noted in parentheses in Figs. 1, 2). The stoichiometric-supported catalysts favor the SMSI interactions, as noted in Sect. 4.2.
It should be emphasized that all hydrogenolysis reactions of titania-promoted systems are thermodynamically unfavorable (all are endothermic), in contrast to the alternative exothermic DHC-reactions (cf. Table 4). Importantly, all extended models included in Table 4 result in H-migration reactions via DHC pathways. The hydrogenolysis does not occur even if the absorbed and adsorbed hydrogen species are completely absent. Perhaps, this is due to the saturation of Pd4 through strong bonding with the third oxygen atom as another anchorage point of the siloxane ring (tripodally anchored to silica via covalent bonds with oxygen atoms).
For comparison, the barriers for the interfacial hydrogenolysis (heterolytic splitting) of the first dihydrogen molecule along the Pd–O covalent bond of the silica-supported catalyst (initially being NBO), was found to be 12.83 kcal mol−1, which is close to the hydrogenolysis barrier for the second H2 molecule mentioned above (ca. 15 kcal mol−1, Table 4).
The hydrogenolysis on supported systems can also be compared with the second H2-activation results on bare metallic palladium clusters present in the literature. As shown by Morokuma and co-workers [106], the activation of the second H2-molecule by Pd4 cluster is thermodynamically and kinetically unfavorable because of the instability of the products [106]. However, the process can well occur when a support is involved, as shown in this study (vide supra). Notably, Wang et al. found that the second molecular hydrogen can be fragmented over the Pd6 cluster of distorted Oh-symmetry through an overall barrier of ca. 9 kcal mol−1 height [107]. This barrier has a value in the range of those found in this paper for supported systems.
1.4 Appendix 4: Atomic and Molecular Hydrogen Coverages and H2-Intercalation
The saturation of a support and a catalyst can alter the H-migration barriers, as particularly discussed by Singh et al. [41] while considering the H-spillover for Pd4 catalyst on graphene. However, even at the saturation limit of the Pd4 catalyst, only one out of the 9H2 molecules has been found to be dissociated to form two hydridic atoms, which rationalizes the model employed in the current paper. Whereas, the GGA-PBE barrier for H-migration has been found to be too high for pristine graphene, the H-saturation of graphene reduced the barrier to ca. 16 kcal mol−1, accessible even at ambient temperatures [41].
In order to get an idea on the H-atom accommodation features and the coverage limits on the silica support, a fully saturated symmetric complex was designed containing 18H atoms. The three axial positions were connected to the three off-ring surface oxygen atoms in a “tripod” configuration. The remaining 15 hydridic atoms were placed at all possible ligand positions of the four octahedral Pd-centers. A relaxed full optimization of this structure led to the spontaneous recombination of the eight hydridic atoms to form four Kubas type dihydrogen ligands bound to the basic Pd-centers. Only two H2 molecules remain activated at the proximity of the reactive (basic) palladium centers at bridging positions, in addition to the three isolated H-atoms located at the top(non-reactive) sites of Pd4-cluster. Since the bare Pd4H18 complex accommodates only two hydridic H-atoms and 8H2 molecules (see also [41]), this result suggests a specific role of the oxidic support in activating the nascent H2-molecules. Furthermore, the defective sites introduce additional activation features. For illustration, the two extra hydridic atoms were added to the TS structure of the direct H-migration that initially contained only two hydridic atoms (with a barrier of 24.49 kcal mol−1 shown in Table 1). The full TS-search (gradient-norm optimization) led to the restoration of the H2-ligand in a product-like structure. Thus, the interplay between the different types of support centers can vary the oxidation states of the Pd-atoms, and thus control the amount of the retained H2-ligands. This seems to be in contrast with platinum which is prone to dissociate most of the nascent dihydrogen molecules [157]. A detailed study of this problem is beyond the scope of current paper, and constitutes an interesting open issue.
Another specific role of the dihydrogen is its “intercalation” between the catalyst and the support at the interface regions. Figure 9 compares a full-contact “tripod” structure of Pd4 located over the hexahydroxytrioxatrisilinane ring, with an actual reagent of the H-spillover in 2H2-capped systems involving a double-contact “dipod” structure where the reactive Pd-atom is moved away (separated) from the surface by an “intercalated” dihydrogen ligand.
The somewhat higher energy of the “dipod” structures provides lower H-spillover barriers for all considered systems: 6.45, 4.78, and 0.84 kcal mol−1, respectively, for pure silica, the binary oxide, and replaced by titania supports (Table 1). The spillover barrier onto the replaced by titania support is exceedingly low due to the interface location (“intercalation”) of the H2-ligand. These results strongly suggest a specific role of the dihydrogen as a ligand to a Pd nanoparticle at the interface regions. This constitutes an important new aspect in H-spillover phenomenon, albeit a partial contact of the catalyst nanoparticle with a support is known in literature. For instance, Pt4-cluster is known to be residing on a carbon nanotube only through one vertex, independent of hydrogen saturation [41, 45].
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Asatryan, R., Ruckenstein, E. Effect of “Reducible” Titania Promotion on the Mechanism of H-Migration in Pd/SiO2 Clusters. Catal Lett 146, 398–423 (2016). https://doi.org/10.1007/s10562-015-1642-0
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DOI: https://doi.org/10.1007/s10562-015-1642-0