CHEM 1A03 Lecture Notes - Lecture 10: Iron(Iii) Oxide, Aluminium Oxide, Oxidation State

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CHEM 1A03 Full Course Notes

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When the oxidation number is -3, the species has an abundance of electrons and can lose them more readily than species with a more positive oxidation number. For example, for the oxidation number of +5, the species is electron deficient making it want to gin electrons. The oxidation numbers of atoms may change over the course of a reaction from reactants to products, there is an exchange of electrons, we call this a redox reaction (reduction-oxidation), Oxidized - loses electrons (leo, loss of electrons is oxidation) Reduction - gains electrons (ger, gain of electrons is reduction) Reducing agent - causes something to be reduced, the reducing agent gets oxidized. Oxidizing agent - causes something to be oxidized, the oxidizing agent gets reduced. The species getting oxidized and reduced, (the reducing and oxidizing agent) are always on the reactants side of the equation).

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Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. Oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. In general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number.

An oxidizing agent is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction.

A reducing agent is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction.

As a summary, keep in mind the following:

CHEM 1A03 Lecture Notes - Lecture 10: Iron(Iii) Oxide, Aluminium Oxide, Oxidation State

CHEM 1A03 Full Course Notes

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