While acid-base reactions are proton-transfer events, oxidation-reduction reactions, or redox reactions, are electron-transfer reactions.
A half-reaction that illustrates the electrons involved in a redox reaction in detail.
The half-reaction that involves the loss of electrons is referred to as an oxidation reaction.
A reduction reaction is a half-reaction in which electrons are gained.
Magnesium is oxidized during the production of magnesium oxide. It's called a reducing agent because it transfers electrons to oxygen, causing it to be reduced.
Because it receives electrons from magnesium, oxygen is reduced and functions as an oxidizing agent, causing magnesium to be oxidized.
It's helpful to give oxidation numbers to the reactants and products to keep track of electrons in redox processes.
The oxidation number, commonly known as the oxidation state, of an atom, indicates how many charges it would have in a molecule if electrons were transported.
Combination, decomposition, combustion, and displacement reactions are some of the most prevalent oxidation-reduction reactions.
A combination reaction occurs when two or more chemicals react to produce a single result.
The reaction of decomposition is the polar opposite of the reaction of combination.
A decomposition reaction occurs when a chemical is broken down into two or more components.
A combustion reaction occurs when a chemical combines with oxygen, usually releasing heat and light in the form of a flame.
An ion of a compound is replaced by an ion of another element in a displacement reaction
In a disproportionation process, an element in one oxidation state gets oxidized and reduced at the same time.