N,N‐Dialkylcarbamato Complexes of the d10 cations of copper, silver, and gold

Alessio, Rocco; Dell’Amico, Daniela Belli; Calderazzo, Fausto; Englert, Ulli; Guarini, Alessandro; Labella, Luca; Strasser, Peter

doi:10.1002/hlca.19980810204

Cited by 52 publications

(35 citation statements)

References 44 publications

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“…A ZnO 2 -precursor, zinc(II) isobutylcarbamate (Zn(IBC)) 2 , was prepared by reacting zinc powder with isobutylammonium isobutylcarbamate. 23,24 Polyvinylpyrrolidone (PVP K15, Mw = 6,000-15,000) and PVP K30 (Mw = 40,000-80,000) were purchased from Daejung Chem. Metals Co. Ltd. and poly(ethylene glycol) (PEG 6000) was purchased from Yakuri Pure Chem.…”

Section: Methodsmentioning

confidence: 99%

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Kim¹,

Cha²,

Gong³

et al. 2014

Bulletin of the Korean Chemical Society

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Zinc peroxide nanoparticles (ZnO 2 NPs) were prepared by reacting zinc(II) isobutylcarbamate, as an organometallic precursor, with hydrogen peroxide (H 2 O 2 ) at 60°C. Polyethylene glycol and polyvinylpyrrolidone were used as stabilizers, which suppressed aggregation of the ZnO 2 NPs. Conditions such as concentrations of H 2 O 2 and the stabilizer were systemically controlled to determine their effect on the formation of nano-sized ZnO 2 NPs. The formation of stable ZnO 2 NPs was confirmed by UV-vis, Raman spectroscopy, X-ray photoelectron spectroscopy, transmission electron microscopy (TEM), scanning electron microscopy (SEM), and X-ray diffraction. The TEM images revealed that polyvinylpyrrolidone-stabilized ZnO 2 NPs (diameter, 10-30 nm) were well dispersed in the organic solvent. Quite pure ZnO NPs were obtained from the peroxide powder by simple heat treatment of ZnO 2 . The transition temperature of 170 o C was determined by differential scanning calorimetry.

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Section: Methodsmentioning

confidence: 99%

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Kim¹,

Cha²,

Gong³

et al. 2014

Bulletin of the Korean Chemical Society

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“…† X-ray diffraction X-ray powder diffraction was conducted on the as-prepared powders with Cu K a radiation in reection mode using a Bruker D8 Advance equipped with 2.3 soller slits and a positionsensitive detector (PSD). 44 Powder diffraction patterns were collected between 10 and 75 using a step size of 0.02 and a counting time of 7 s. Divergence and antiscattering slit were adjusted for a constant illuminated area.…”

Section: Synthesesmentioning

confidence: 99%

Electrochemical water splitting by layered and 3D cross-linked manganese oxides: correlating structural motifs and catalytic activity

Bergmann

Zaharieva

Dau

et al. 2013

Energy Environ. Sci.

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263

252

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a Manganese based precious metal-free electrocatalysts for the oxygen evolution reaction (OER) are promising materials for energy storage systems based on dark or photo-coupled water electrolysis, because they are active, inexpensive and of low toxicity. In this work, atomic scale structure-activity relationships of two different nano-structured manganese oxides, MnO x , are established using a combination of X-ray absorption, diffraction and electrochemistry. Prepared by chemical symproportionation (s-MnO x ) and impregnation (i-MnO x ), the s-MnO x catalyst consisted of a layered structure similar to d-MnO 2 while the i-MnO x catalyst displayed a mixture of tunnelled, 3D cross-linked b-and defective g-MnO 2 structures. During electrocatalytic oxygen evolution the structural motifs of both MnO x remain largely unchanged, but the oxidation state of Mn increases from 3.5 to 3.9-4.Kinetic parameters of the electrocatalytic oxygen evolution reaction were extracted using Tafel slope analysis and pH titration experiment, and the role of the protons abstracted was analyzed. The study reveals fundamental differences of general importance in the catalytic activity between layered and cross-linked structures. The exclusive presence of di-m-oxo-bridged Mn ions in the layered structure is coupled to a pronounced redox and charge capacity behaviour. This ensured efficient use of surface and bulk active sites, and resulted in a relatively large Tafel slope. Consequently, the intrinsic OER activity is especially high in s-MnO x . In contrast, 3D cross-linked structures with both mono-and di-m-oxo-bridged Mn ions resulted in lower intrinsic activity but smaller Tafel slope, and thus favourable activity at technological water-splitting rates. The insights from this comparative study will provide guidance in the structural design and optimization of other non precious metal oxide OER catalysts. Broader contextThe intermittency of the electrical output power of renewable solar and wind energy devices makes efficient, cost-effective, grid-scale energy storage mandatory. Electrical power storage using molecular bonds (synthesis of fuel molecules) offers a number of advantages over storage in solid state material lattices. As electrolytic synthesis of chemical fuels is a reductive chemical process, a corresponding electrooxidation process at the grid-scale level is essential. Electrochemical water oxidation to molecular oxygen is perhaps the only feasible oxidation process that can provide electrons and protons at the required grid-scale. However, inexpensive, efficient and stable water oxidation catalysts are rare, if non-existent. This is why the development of non-precious water oxidation catalysts has become a scientic priority. Manganese oxides attract special attention as water splitters, as they form the basis for Nature's oxygen evolving complex in the Photosystem II complex. Detailed insight into structure-activity relationships of inorganic Mn containing water splitting materials is still scarce.

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“…59,60 All potentials here are referenced to this reference electrode. Electrochemical catalyst pretreatments are illustrated in Fig.…”

Section: Electrochemical Pretreatmentsmentioning

confidence: 99%

Shape-selected bimetallic nanoparticle electrocatalysts: evolution of their atomic-scale structure, chemical composition, and electrochemical reactivity under various chemical environments

et al. 2013

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Dieser Beitrag ist mit Zustimmung des Rechteinhabers aufgrund einer (DFG geförderten) Allianz- bzw. Nationallizenz frei zugänglich.This publication is with permission of the rights owner freely accessible due to an Alliance licence and a national licence (funded by the DFG, German Research Foundation) respectively.Solid surfaces generally respond sensitively to their environment. Gas phase or liquid phase species may adsorb and react with individual surface atoms altering the solid-gas and solid-liquid electronic and chemical properties of the interface. A comprehensive understanding of chemical and electrochemical interfaces with respect to their responses to external stimuli is still missing. The evolution of the structure and composition of shape-selected octahedral PtNi nanoparticles (NPs) in response to chemical (gas-phase) and electrochemical (liquid-phase) environments was studied, and contrasted to that of pure Pt and spherical PtNi NPs. The NPs were exposed to thermal annealing in hydrogen, oxygen, and vacuum, and the resulting NP surface composition was analyzed using X-ray photoelectron spectroscopy (XPS). In gaseous environments, the presence of O2 during annealing (300 °C) lead to a strong segregation of Ni species to the NP surface, the formation of NiO, and a Pt-rich NP core, while a similar treatment in H2 lead to a more homogenous Pt-Ni alloy core, and a thinner NiO shell. Further, the initial presence of NiO species on the as-prepared samples was found to influence the atomic segregation trends upon low temperature annealing (300 °C). This is due to the fact that at this temperature nickel is only partially reduced, and NiO favors surface segregation. The effect of electrochemical cycling in acid and alkaline electrolytes on the structure and composition of the octahedral PtNi NPs was monitored using image-corrected high resolution transmission electron microscopy (TEM) and high-angle annular dark field scanning TEM (HAADF-STEM). Sample pretreatments in surface active oxygenates, such as oxygen and hydroxide anions, resulted in oxygen-enriched Ni surfaces (Ni oxides and/or hydroxides). Acid treatments were found to strongly reduce the content of Ni species on the NP surface, via its dissolution in the electrolyte, leading to a Pt-skeleton structure, with a thick Pt shell and a Pt-Ni core. The presence of Ni hydroxides on the NP surface was shown to improve the kinetics of the electrooxidation of CO and the electrocatalytic hydrogen evolution reactions. The affinity to water and the oxophilicity of Ni hydroxides are proposed as likely origin of the observed effects.DFG, EXC 314, Unifying Concepts in Catalysi

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N,N‐Dialkylcarbamato Complexes of the d¹⁰ cations of copper, silver, and gold

Cited by 52 publications

References 44 publications

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Electrochemical water splitting by layered and 3D cross-linked manganese oxides: correlating structural motifs and catalytic activity

Shape-selected bimetallic nanoparticle electrocatalysts: evolution of their atomic-scale structure, chemical composition, and electrochemical reactivity under various chemical environments

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N,N‐Dialkylcarbamato Complexes of the d10 cations of copper, silver, and gold

Cited by 52 publications

References 44 publications

Preparation of ZnO2Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Preparation of ZnO2Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Electrochemical water splitting by layered and 3D cross-linked manganese oxides: correlating structural motifs and catalytic activity

Shape-selected bimetallic nanoparticle electrocatalysts: evolution of their atomic-scale structure, chemical composition, and electrochemical reactivity under various chemical environments

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Product

Resources

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N,N‐Dialkylcarbamato Complexes of the d¹⁰ cations of copper, silver, and gold

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent

Preparation of ZnO₂Nanoparticles Using Organometallic Zinc(II) Isobutylcarbamate in Organic Solvent