Malika Ammam, PhD
Consultant - Freelancer
A Better Way to Learn Redox Chemistry Part 1: Summarized Principles and Over 250 Answered Questions and Problems
This short book (part 1) summarizes some basics of redox chemistry (electrochemistry) in solution. Each section of the book contains concise and clear referenced summaries of redox concepts. Over 250 answered questions and problems are provided to further clarify the discussed principles.
Mini Mixer
Mini Mixer
Some Basics of Chemistry
Useful in Redox Processes
A better understanding of redox (or electrochemical) processes in solution requires the
knowledge of some basics related to chemistry. These include, what solvents and electrolytes are
used in redox chemistry, the influence of parameters like conductivity, acidity, basicity, pH, and
some thermodynamics and kinetics associated with these processes. This Section 1 summarizes
some of these basics. Remember that all redox are chemical processes but not all chemical
reactions are redox and only those involving the transfer of electrons are characterized as redox.
Mini Mixer
Electrons in Matter and Link
to Redox Chemistry
Keep in mind that redox reactions are chemical processes but not all chemical reactions are redox.
Redox chemistry, also known as electrochemistry, involves the loss or gain of electrons and could track
the movement of consumed or released electrons during the process. Electrons are believed to exist since the early stages of formation of the Universe during the Big Bang. These subatomic particles, called electrons, are part of atoms, molecules, and matter in general. To better understand electrochemical processes discussed in later sections, some basics related to electrons are given here, including the structure of atoms, periodic table, main electronic models, electronic configuration, and the energy levels of electrons.
Principles of Redox Reactions
After reading Section 2, students should be able to identify the electronic structure of any
element of the periodic table and be able to visualize the electrons of the outer shell, which could
be involved in redox processes. This section 3 summarizes the basics of redox (or
electrochemical) processes by focusing on the species that might lose or gain electrons,
determination of the oxidation numbers (or states) of atoms in species involved in redox
processes, and easy ways of balancing redox reactions.
The previous section provided a short concise definition of redox reactions and proposed
ways to determine the oxidation states of elements, as well as how to balance redox reactions.
This section discusses the importance of reference systems (or electrodes) in electrochemistry for
determining the potentials of redox reactions at conditions different from the standard. The
variation trends of redox potentials across the periodic table are also summarized.
After highlighting the importance of reference systems (or electrodes) in the
determination of redox potentials (Section 4), further details regarding their measurements are
given in this section. These include the cell composition in terms of electrode and electrolyte and
the main mathematical quantities governing the redox reactions at equilibrium states.
Reference Systems and
Electrochemical Cells
Applications of Nernst
Equation
Redox equilibria are previously explained by the Nernst equation (Section 5), which
could be applied in many electrochemical systems to estimate quantities, such as potentials and
concentrations of redox species in solution. This section 6 is devoted to applications of the
Nernst equation in electrochemical systems, including energy (consumption or generation),
corrosion, redox titration, as well as study of solubility, precipitation, and complexation
reactions.
Une Meilleure Façon d'Apprendre
l’Oxydoréduction Partie 1: Résumés des Principes et Plus de 250 Questions et Problèmes Résolus
Ce petit livre (Partie 1) résume quelques principes de chimie d’oxydoréduction (électrochimie) en solution. Chaque section du livre contient des résumés référencés, concis et clairs des concepts d’oxydoréduction. Plus de 250 questions et problèmes avec solution sont fournis afin de clarifier davantage les principes discutés.
Quelques Principes de Chimie Utiles en Oxydoréduction
Une meilleure compréhension des processus d’oxydoréduction (ou électrochimiques) en solution nécessite la connaissance de quelques notions de base liées à la chimie générale. Ceux-ci comprennent, les solvants et électrolytes utilisés en chimie d’oxydoréduction, l'influence de paramètres tels que la conductivité, l'acidité, la basicité ou le pH, ainsi que les thermodynamiques et cinétiques de ces processus. Cette section résume certaines de ces bases. Rappelez-vous que tous les processus d’oxydoréduction sont des processus chimiques, mais pas toutes les réactions chimiques sont redox et seules celles impliquant le transfert d'électrons sont caractérisées comme redox.
Électrons dans la Matière et Lien avec l’Oxydoréduction
Il faut garder à l'esprit que toutes les réactions d'oxydoréduction sont des processus chimiques, mais pas toutes les réactions chimiques sont redox. L’oxydoréduction, également connue sous le nom d'électrochimie, implique la perte ou gain d'électrons, et également peut suivre le mouvement d’électrons consommés ou libérés au cours de processus. Les électrons existent depuis les premiers stades de la formation de l'Univers pendant le Big Bang. Ces particules subatomiques, appelées électrons, font partie des atomes, des molécules et de la matière en général. Pour mieux comprendre les processus électrochimiques, certaines notions de base concernant les électrons sont discutées dans cette section, y compris la structure des atomes, le tableau périodique, les principaux modèles électroniques, la configuration électronique et les niveaux d'énergie des électrons.
Principes des Réactions d’Oxydoréduction
À ce stade, les élèves devraient être capables d'identifier la structure électronique de n'importe quel élément et d'être en mesure de visualiser les électrons de la couche externe, qui pourraient être impliqués dans des processus d’oxydoréduction. Cette section résume les principes des processus d’oxydoréduction (ou électrochimiques) en se concentrant sur les espèces qui pourraient perdre ou gagner des électrons, détermination des nombres (ou états) d'oxydation des espèces impliquées dans ces processus redox et les moyens faciles d'équilibrer des réactions d’oxydoréduction.
Systèmes de Déférences et Cellules Électrochimiques
La section précédente décrivait les réactions d'oxydoréduction et proposait des moyens de déterminer les états d'oxydation des éléments, ainsi que les moyens d’équilibrer les réactions d'oxydoréduction. Cette section discute l'importance des systèmes de références (ou électrodes) en électrochimie en détermination des potentiels des réactions redox aux conditions différentes des standards. Les tendances des potentiels redox à travers le tableau périodique sont également résumées.
Après avoir souligné l'importance des systèmes de références (ou électrodes) pour déterminer les potentiels d'oxydo-réduction, d'autres détails concernant leurs mesures sont donnés dans cette section. Ceux-ci comprennent la composition des cellules électrochimiques en termes d'électrode et électrolyte, ainsi que les principales quantités mathématiques régissant les réactions redox à l'état d'équilibre.
Applications de l’Équation de
Nernst
Les équilibres redox sont expliqués précédemment par l'équation de Nernst, qui pourrait être
appliquée dans de nombreux systèmes électrochimiques pour estimer ses quantités, telles que les
potentiels et concentrations des espèces redox en solution. Cette section est consacrée aux
applications de l'équation de Nernst dans les systèmes électrochimiques, y compris les cellules
énergétiques (consommation ou génération), corrosion, titrages redox, ainsi que l'étude des
réactions de solubilité, précipitation et complexation.
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