Essential Information & explanations, latest texts & monographs on
Electrochemistry.
Electrochemical Methods : Fundamentals and Applications by Allen J. Bard
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Electrochemistry
Electrochemistry is the study of the electronic and electrical aspects of chemical reactions.
The elements involved in an electrochemical reaction are
characterized by the number of electrons each has. The oxidation state of an ion is the number of electrons it has accepted or donated compared to its neutral state (which is defined as having an oxidation state of 0). If an atom or ion donates an electron in a reaction its oxidation state is increased, if an element accepts an electron its oxidation state is decreased.
For example when sodium reacts with chlorine, sodium donates one electron and gains an oxidation state of +1. Chlorine accepts the electron and gains an oxidation state of -1. The sign of the oxidation state (positive/negative) actually corresponds to the value of each ion's electronic charge. The attraction of the differently charged sodium and chlorine ions is the reason they then ionicly bond to each other.
The loss of electrons of a substance is called oxidation, and the gain of electrons is reduction. This can be easily remembered through the use of the mnemonic, OIL RIG: Oxidation Is Loss Reduction Is Gain. The substance which loses electrons is also known as the reducing agent, or reductant, and the substance which accepts the electrons is called the oxidising agent, or oxidant.
A reaction in which both oxidation and reduction is occurring is called a redox reaction. These are very common; as one substance loses electrons the other substance accepts them. Redox reactions are the basis for ionic bonding.
Oxidation requires an oxidant. Oxygen is an oxidant, but not the only one. Despite the name, an oxidation reaction does not necessarily need to involve oxygen. In fact, even fire can be fed by an oxidant other than oxygen:
Fluorine fires are often unquenchable, as fluorine is an even stronger oxidant
(it has a higher electronegativity) than oxygen.
Table of contents showTocToggle("show","hide")
1 Oxidizing agent
2 Reducing agent
3 Techniques
4 See also
Oxidizing agent
An oxidizing agent is a substance used in electrochemistry that oxidizes another substance. In doing so, it becomes reduced.
Reducing agent
A reducing agent is a substance used in electrochemistry that reduces another substance. In doing so, it becomes oxidized.
A spontaneous electrochemical reaction can be used to generate an
electrical current, in electrochemical cells. This is the basis of all batteries and fuel cells. For example, gaseous oxygen (O2) and
hydrogen (H2) can be combined in a fuel cell to form water and
energy (a combination of heat and current, typically).
Conversely, non-spontaneous electrochemical reactions can be driven forward by the application of a current at sufficient voltage. The
electrolysis of water into gaseous oxygen and hydrogen is a typical example.
Techniques
Electrochemistry uses techniques that can be found in diverse applications.
See also
Chemistry
Analytical chemistry | Organic chemistry | Inorganic chemistry | Physical chemistry | Polymer chemistry | Biochemistry | Materials science | Environmental chemistry | Pharmacy | Thermochemistry | Electrochemistry | Nuclear chemistry
Periodic table | List of compounds
The above article is adapted from from Wikipedia All Wikipedia article text is available under the terms of the GNU Free Documentation License
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