Metal hydroxide mechanism

Salvaga and Cavallotti [43], and Randin and Hintermann [44] advanced a metal hydroxide mechanism which involved hydrolyzed nickel ions as the actual nickel reactant in Ni-P deposition ... 

As it is already established in the published literature, both of the above categories have their advantages and disadvantages.1,3 Furthermore, as it was suggested by Djokic6 in the example of electroless deposition of cobalt with hydrazine, the contribution from both electrochemical and metal hydroxide mechanisms is quite possible. 

For the review of all these mechanisms, the reader is referred to the Ref. [1]. In summary of the proposed listed mechanisms, it is, based on the experimental observations and the present knowledge, quite unlikely that the atomic hydrogen and hydride ion mechanisms are applicable in the description of the autocatalytic deposition. The universal mechanism is not applicable, since every single autocatalytic deposition (e.g., Ni, Co, Pd, Pt, Ag, An, Cu, Bi, etc.) must have a specific mechanism, and a generalization is quite difficult to achieve. It seems that the metal hydroxide and up to some extent the electrochemical mechanisms are the only mechanisms that can explain most of the characteristics of the autocatalytic deposition of metals and alloys. The discussions of the mechanistic aspects of autocatalytic deposition in details is out of the scope of the present book however, the metal hydroxide mechanism [1, 16-18] seems as the most acceptable way to explain the properties including the surface morphology of the deposits produced via the autocatalytic deposition. The metal hydroxide mechanism is based on the fact that under the conditions of autocatalytic deposition there is an unavoidable pH rise at the surface where the reaction in question takes place. Due to hydrolysis, hydrolyzed species can form and further be absorbed and/or reduced at the surface. This mechanism explains quite well the bath instability and formation of powders within the bulk electrolyte. When other parameters are constant, in general terms, an increase in pH of the solution leads to an increase in the rate of deposition, as schematically presented in Fig. 9.24. 

In order for a soHd to bum it must be volatilized, because combustion is almost exclusively a gas-phase phenomenon. In the case of a polymer, this means that decomposition must occur. The decomposition begins in the soHd phase and may continue in the Hquid (melt) and gas phases. Decomposition produces low molecular weight chemical compounds that eventually enter the gas phase. Heat from combustion causes further decomposition and volatilization and, therefore, further combustion. Thus the burning of a soHd is like a chain reaction. For a compound to function as a flame retardant it must intermpt this cycle in some way. There are several mechanistic descriptions by which flame retardants modify flammabiUty. Each flame retardant actually functions by a combination of mechanisms. For example, metal hydroxides such as Al(OH)2 decompose endothermically (thermal quenching) to give water (inert gas dilution). In addition, in cases where up to 60 wt % of Al(OH)2 may be used, such as in polyolefins, the physical dilution effect cannot be ignored. 

A fourth mechanism is called sweep flocculation. It is used primarily in very low soflds systems such as raw water clarification. Addition of an inorganic salt produces a metal hydroxide precipitate which entrains fine particles of other suspended soflds as it settles. A variation of this mechanism is sometimes employed for suspensions that do not respond to polymeric flocculants. A soHd material such as clay is deUberately added to the suspension and then flocculated with a high molecular weight polymer. The original suspended matter is entrained in the clay floes formed by the bridging mechanism and is removed with the clay. 

Inorganic salts of metals work by two mechanisms in water clarification. The positive charge of the metals serves to neutralize the negative charges on the turbidity particles. The metal salts also form insoluble metal hydroxides which are gelatinous and tend to agglomerate the neutralized particles. The most common coagulation reactions are as follows ... 

The type of catalyst influences the rate and reaction mechanism. Reactions catalyzed with both monovalent and divalent metal hydroxides, KOH, NaOH, LiOH and Ba(OH)2, Ca(OH)2, and Mg(OH)2, showed that both valence and ionic radius of hydrated cations affect the formation rate and final concentrations of various reaction intermediates and products.61 For the same valence, a linear relationship was observed between the formaldehyde disappearance rate and ionic radius of hydrated cations where larger cation radii gave rise to higher rate constants. In addition, irrespective of the ionic radii, divalent cations lead to faster formaldehyde disappearance rates titan monovalent cations. For the proposed mechanism where an intermediate chelate participates in the reaction (Fig. 7.30), an increase in positive charge density in smaller cations was suggested to improve the stability of the chelate complex and, therefore, decrease the rate of the reaction. The radii and valence also affect the formation and disappearance of various hydrox-ymethylated phenolic compounds which dictate the composition of final products. 

An interesting feature of the ring opening polymerization of siloxanes is their ability to proceed via either anionic or cationic mechanisms depending on the type of the catalyst employed. In the anionic polymerization alkali metal hydroxides, quaternary ammonium (I NOH) and phosphonium (R POH) bases and siloxanolates (Si—Oe M ) are the most widely used catalysts 1,2-4). They are usually employed at a level of 10 2 to KT4 weight percent depending on their activities and the reaction conditions. The activity of alkali metal hydroxides and siloxanolates decrease in the following order 76 79,126). 

Although organosilanes appear to react slowly (if at all) with water alone, in the presence of acids or bases (e.g., alkali metal hydroxides), reactions to give a silanol and H2 are rapid, with bases being particularly powerful catalysts. The evolution of H2 in this type of reaction may be used as both a qualitative and a quantitative test for Si-H bonds, and the mechanism of the acid and the base hydrolysis has been discussed in detail (30,31). This hydrolytic method is not very common for the preparation of silanols that are to be isolated, because both acids and bases catalyze the condensation of silanols to siloxanes, and therefore, only compounds containing large substituents are conveniently made in this way. If an anhydrous alkali metal salt is used, a metal siloxide may be isolated and subsequently hydrolyzed to give the silanol [Eq. (10)] (32). 

Before our work [39], only one catalytic mechanism for zinc dependent HDACs has been proposed in the literature, which was originated from the crystallographic study of HDLP [47], a histone-deacetylase-like protein that is widely used as a model for class-I HDACs. In the enzyme active site, the catalytic metal zinc is penta-coordinated by two asp residues, one histidine residues as well as the inhibitor [47], Based on their crystal structures, Finnin et al. [47] postulated a catalytic mechanism for HDACs in which the first reaction step is analogous to the hydroxide mechanism for zinc proteases zinc-bound water is a nucleophile and Zn2+ is five-fold coordinated during the reaction process. However, recent experimental studies by Kapustin et al. suggested that the transition state of HDACs may not be analogous to zinc-proteases [48], which cast some doubts on this mechanism. 

Proposed intermediates in the above reaction include atomic hydrogen [27, 28], hydride ions [29, 30], metal hydroxides [31], metaphosphites [32, 33], and excitons [34]. In general, the postulated mechanisms are not supported by direct independent evidence for these intermediates. Some authors [35] maintain that the mechanism is entirely electrochemical (i.e. it is controlled by electron transfer across the metal-electrolyte interface), but others [26] advocate a process involving a surface-catalyzed redox reaction without interfacial electron transfer. 

The hammerhead ribozyme and leadzyme belong to the second class of ribozymes. The short extra sequences of the ribozymes form the so-called catalytic loop which acts as the enzyme. There are two likely functions for metal ions in the mechanism of action of hammerhead ribozymes formation of metal hydroxide groups or direct coordination to phosphoryl oxygens. 

Fig. 6.10 shows idealized isotherms (at constant pH) for cation binding to an oxide surface. In the case of cation binding, onto a solid hydrous oxide, a metal hydroxide may precipitate and may form at the surface prior to their formation in bulk solution and thus contribute to the total apparent "sorption". The contribution of surface precipitation to the overall sorption increases as the sorbate/sorbent ratio is increased. At very high ratios, surface precipitation may become the dominant "apparent" sorption mechanism. Isotherms showing reversals as shown by e have been observed in studies of phosphate sorption by calcite (Freeman and Rowell, 1981). 

A novel finding related to the mechanism of catalysis by the genomic HDV ribozyme is that the pKa of C75 is perturbed to neutrality in the ri-bozyme-substrate complex and, more importantly, that C75 acts as a general acid catalyst in combination with a metal hydroxide which acts as a general base catalyst (Fig. 9A) [105]. The discovery of this phenomenon provided the first direct proof that a nucleobase can act as an acid/base catalyst in RNA. As a result, as shown by the solid curve in Fig. 9B, the curve that represents the dependence on the pH of the self-cleavage of the precursor genomic HDV ribozyme has a slope of unity at pH values that are below 7 (the activity increases linearly as the pH increases, with a slope of +1). Then, at higher pH values, the observed rate constant is not affected by the pH. 

Kinetic Scheme. Generally, metal ions in a solution for electroless metal deposition have to be complexed with a ligand. Complexing is necessary to prevent formation of metal hydroxide, such as Cu(OH)2, in electroless copper deposition. One of the fundamental problems in electrochemical deposition of metals from complexed ions is the presence of electroactive (charged) species. The electroactive species may be complexed or noncomplexed metal ion. In the first case, the kinetic scheme for the process of metal deposition is one of simple charge transfer. In the second case the kinetic scheme is that of charge transfer preceded by dissociation of the complex. The mechanism of the second case involves a sequence of at least two basic elementary steps ... 

The mechanisms of CD processes can be divided into two different processes formation of the required compound by ionic reactions involving free anions, and decomposition of metal complexes. These two categories can be further divided in two formation of isolated single molecules that cluster and eventually form a crystal or particle, and mediation of a solid phase, usually the metal hydroxide. We consider first the pathways involving free anions and defer to later those where a metal complex decomposes. 

It should be borne in mind that the mechanism may change in the course of the deposition. As the metal is depleted from solution, the complexmetal ratio will increase and may pass the point where no solid hydroxide phase is present in the solution. In this case, the ion-by-ion process will occur (initially in parallel with the hydroxide mechanism, later maybe exclusively) if the conditions are suitable. 

These processes have been shown for free metal ions. However, if a cluster mechanism based on metal hydroxide colloids is involved, they are equally applicable to the formation of the solid hydroxide species. The degree of conversion of... 

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