Oxidation-reduction reactions reducing agents

Define the following terms half-reaction, oxidation reaction, reduction reaction, reducing agent, oxidizing agent, redox reaction. 

The reaction of an alkyl halide with lithium is an oxidation-reduction reaction. Group I metals are powerful reducing agents. 

In the majority of cases both the primary and the induced reactions are oxidation-reduction reactions. In such reactions the actor can have either reducing or oxidizing properties. The chemical characteristics of the inductor and acceptor are always identical and opposite to that of the actor. When the latter is a reducing agent the acceptor and inductor are oxidants and vice versa. 

The reactions discussed above show that arsenic(fV) is of redox amphoteric character and a stronger reducing agent than arsenic(in), but at the same time it is a stronger oxidant than arsenic(V). Partners of the oxidation-reduction reactions of arsenic(fV) known so far can be seen in Table 13. It follows from the redox amphoteric character that the oxidation potentials of couples involving arsenic species are in the order... 

Carbon is a reducing agent the oxidised forms of carbon are carbon oxides. The dangerous reactions of these will therefore mainly be oxidation-reduction reactions. 

Silicon is generally considered to be a congener of carbon and this is also reflected in the evolution of silicon as a reducing agent for metal oxides. Silicon forms a fairly stable solid oxide silica or silicon dioxide (Si02) and also a stable gaseous oxide silicon monoxide (SiO), both of which can be useful in oxide reduction reactions. 

Metabolism of trimethylamine oxide in fish muscle involves an enzyme-catalyzed oxidation-reduction reaction. The enzyme responsible for the conversion of trimethylamine oxide to trimethylamine is known as trimethylamine-W-oxide reductase. This enzyme acts on nicotinamide adenine dinucleotide (NADH) and TMAO to produce NAD+, trimethylamine and water (Fig. 13.13.1). TMAO acts as the oxidizing agent and is reduced, while NADH undergoes oxidation as the reducing agent. 

The critical reaction in electroless deposition from the viewpoint of catalysis is oxidation of the reducing agent. The ability to catalyze oxidation of the reductant determines whether a metal or alloy can sustain electroless deposition in an otherwise properly formulated electroless solution. 

V to +0.7 V vs. RHE for a Pd surface. Normally, this is anodic, or positive, with respect to the Em value of the electroless reaction (Fig. 1). Following removal of the oxide species from the catalyst surface, whether deposition subsequently initiates or not depends on the interplay between the kinetics of the parallel metal ion and O2 reduction reactions, and oxidation of the reducing agent. Once an appropriate Em value is reached, metal deposition will occur. 

In solution, NaOCl dissociates into sodium ions (Na+) and hypochlorite ions (OC1). Bleaching involves an oxidation-reduction reaction in which the Cl in the OC1 ion (oxidizing agent) is reduced to the chloride ion (Cl ). The reducing agent is either a dye, which fades, or the stain being removed. 

Oxidation-reduction reactions represent yet another type of reaction that titrimetric analysis can utilize. In other words, a solution of an oxidizing agent can be in the buret, and a solution of a reducing agent can be in the reaction flask (and vice versa). In this section, we review the fundamentals of oxidization-reduction chemistry and discuss the titrimetric analysis applications. 

A reducing agent is the reactant that loses electrons in an oxidation-reduction reaction ... 

As an oxidizing agent, it undergoes oxidation-reduction reactions with reducing agents at ambient and elevated temperatures. 

Consequently, reduction of cobalt(III) ammines in basic solution is not favorable. A variety of reducing agents has been used to effect reaction (11). The fortunate coincidences that cobalt(III) complexes are substitution inert while cobalt(II) systems are labile and that cobalt(II) is resistant to oxidation or further reduction in acid solution offer many advantages in the study of redox processes. Not surprisingly, work with cobalt(III) complexes forms the basis for much of the present understanding of oxidation-reduction reactions. 

The reduction potential increases moving up the table. This means that substances near the top of the table are more likely to be reduced (are better oxidizing agents) and substances near the bottom are more likely to be oxidized (are better reducing agents). The substances in Table 14.2 correspond to the previous listing of how easily substances are oxidized. When two substances in Table 14.2 take part in a redox reaction, the one higher in the table is the substance that is reduced. 

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