Oxidation-reduction reactions general principles

The majority of potentiometric titrations involve chemical reactions which can be classified as (a) neutralisation reactions, (b) oxidation-reduction reactions, (c) precipitation reactions or (d) complexation reactions, and for each of these different types of reaction, certain general principles can be enunciated. 

Basic Principles of the Nernst Eqnation. Consider the following generalized oxidation/reduction reaction... 

Chapters 15 through 24 explore intermediary metabolism. Chapter 15 opens the topic with chemical principles that provide some unifying themes. Thermodynamic concepts learned earlier in general chemistry and in Chapter 1 are applied specifically to biochemical topics such as coupled reactions. In addition, this chapter explic-idy makes the connection between metabolism and electron transfer (oxidation-reduction) reactions. 

Distinguish between an electrolyte and a nonelectrolyte, and provide examples of each. 5.2 Use the solubility guidelines tor common ionic solids to determine whether 5-4 Oxidation-Reduction Reactions Some General Principles 5-7 Stoichiometry of Reactions in Aqueous Solutions Titrations... 

Oxidation-Reduction Reactions Some General Principles 167... 

Oxidation-Reduction Reactions Some General Principles— In an oxidation-reduction (redox) reaction certain atoms undergo an increase in oxidation state, a process called oxidation. Other atoms undergo a decrease in oxidation state, or reduction. Another useful view of redox reactions is as the combination of separate half-reactions for the oxidation and the reduction. 

Many of the reactions of oxoacids and oxoanions involve oxidation and reduction. There are certain general principles that apply, regardless of the particular species involved. 

To show how these general principles of nucleophilic substitution and addition apply to carbonyl compounds, we are going to discuss oxidation and reduction reactions, and reactions with organometallic reagents—compounds that contain carbon-metal bonds. We begin with reduction to build on what you learned previously in Chapter 12. 

Another type of reaction may be mentioned here, which, while not oxidation-reduction, shows some of the possibilities in the way of relative oxidizing potentials of different atoms, or the relative aflSnities of the atoms for valence electrons. Silver nitrite ind sodiuiii nitrite when treated with an alkyl halide give different products. With the former, a nitro compound is obtained mainly with the latter a nitrite predominates. While according to the older views, this would point to different structures for the two nitrites, according to the principles developed in this book, the explanation of these differences involves tautomerism and several chemical equilibria. The reaction may be given in general terms as follows ... 

You ve heard electrochemistry of corrosion as a lecture I shouldn t spend much time on it but I d like to describe some electrochemical effects for film formers. First the general principles. If you put a good electronic conductor (a metal) in an aqueous solution, you will typically find that an electrical potential is developed between the piece of conductor and the solution. When ions of the metal enter the solution and leave extra electrons behind a negative potential is developed. All oxidation reactions occurring on the surface are expected to produce this result. Similarly, reduction reactions that use electrons from the metal are expected to produce a more positive potential in the metal. The solution potential of the metal influences the rate of an electrochemical half-cell reaction in accordance with Le Chatelier s Principle, so it is possible to predict through the use of the Nernst Equation the potential that will exist when the only significantly rapid reactions are the oxidation and reduction parts of a reversible reaction. When more than one potentially reversible process occurs, the rate of oxidation will be expected to exceed the rate of reduction for at least one and the converse for at least one. At... 

The generally accepted mechanistic alternatives (other than direct reductive elimination) are illustrated in Figure 4.12. In principle, the dimer could lose the acetate group and the corresponding cationic Pd(III) dimer would then lead to ArCl via reductive elimination. Alternatively, the dimer could disproportionate to Pd(IV) and Pd(II). Canty, Ritter, Sanford et al. demonstrated previously for oxidative trifluoromethylation reactions that dinuclear Pd and mononuclear Pd pathways are connected [48]. The Pd(IV) complex could then either directly eliminate ArCl or dissociate the acetate ion and reductively eliminate ArCl from the cation (see Figure 4.12). Using computational means, it is not trivial to answer whether the pathways via the cationic Pd complexes (Pd(III) dimer or Pd(IV) monomer) are favored over alternative pathways. It is possible to reproduce the... 

---