Combustion: a kind of redox reaction in which any combustible substance combines with an oxidizing element, usually oxygen, to generate heat and form oxidized products. The term combustion is usually used for only large-scale oxidation of whole molecules, i.e. a controlled oxidation of a single functional group is not combustion.
C10H8+ 12 O2 → 10 CO2 + 4 H2O CH2S + 6 F2 → CF4 + 2 HF + SF6
Redox reactions
Redox reactions: in which changes in oxidation numbers of atoms in involved species occur.
Those reactions can often be interpreted as transferences of electrons between different molecular sites or species.
An example of a redox reaction is:
2 S2O32−(aq) + I2(aq) → S4O62−(aq) + 2 I−(aq)
In which I2 is reduced to I- and S2O32- (thiosulfate anion) is oxidized to S4O62-.
Acid-base reaction
Acid-base reactions: broadly characterized as reactions between an acid and a base, can have different definitions depending on the acid-base concept employed.
Some of the most common are:
Arrhenius definition: Acids dissociate in water releasing H3O+ ions; bases dissociate in water releasing OH- ions.
Bronsted-Lowry definition: Acids are proton (H+) donors; bases are proton acceptors. Includes the Arrhenius definition.
Lewis definition: Acids are electron-pair acceptors; bases are electron-pair donors. Includes the Brønsted-Lowry definition.
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