A chemical response is a process that always results in the conversion of reactants into product or products. The substance or substances initially concerned in a chemical reaction are called reactants. A type of a chemical response is normally characterised by the type of chemical change, and it yields one or more products which are, on the whole, totally different from the reactants.

Generally speaking, chemical reactions encompass changes that strictly contain the motion of electrons in the forming and breaking of chemical bonds. Chemical equations are often used to describe the chemical transformations of elementary particles that occur through the reaction.

Chemical adjustments are a result of chemical reactions. All chemical reactions contain a change in substances and a change in energy. However, neither matter nor energy is created or destroyed in a chemical reaction. There are such a lot of chemical reactions that it is useful to categorise them into totally different types including the widely used terms for describing frequent reactions.

Mixture response or synthesis response: it is a reaction in which 2 or more chemical elements or compounds unite to form a more advanced product.

Example: N2 + three H2 ' 2 NH3

Isomerisation reaction: is a response in which a chemical compound undergoes a structural rearrangement without any change in its net atomic composition.

Example: trans-2-butene and cis-2-butene are isomers.

Chemical decomposition response or analysis: is a response in which a compound is decomposed into smaller compounds or components:

Example: 2 H2O ' 2 H2 + O2

Single displacement or substitution: this type of reaction is characterized by an element being displaced out of a compound by a more reactive element.

Example: 2 Na(s) + 2 HCl(aq) ' 2 NaCl(aq) + H2(g)

Metathesis or Double displacement response: represents a response in which two compounds exchange ions or bonds to form different compounds

Examples: NaCl(aq) + AgNO3(aq) ' NaNO3(aq) + AgCl(s)

Acid-base reactions: broadly these reactions are characterized as reactions between an acid and a base, can have completely different definitions depending on the acid-base concept employed. Some of the commonest are:

Arrhenius definition: Acids dissociate in water releasing H3O+ ions; bases dissociate in water releasing OH- ions.

Brønsted-Lowry definition: Acids are proton (H+) donors; bases are proton acceptors.

Lewis definition: Acids are electron-pair acceptors; bases are electron-pair donors.
Instance: HCl(aq) + NaOH(aq) ' NaCl(aq) + H2O(l)

Redox reactions: are reactions in which modifications in oxidation numbers of atoms in involved species occur. Those reactions can often be interpreted as transfer of electrons between completely different molecular sites or species.

Example: 2 S2O32(aq) + I2(aq) ' S4O62(aq) + 2 I(aq)
In this case, I2 is reduced to I- and S2O32- (thiosulfate anion) is oxidized to S4O62-.

Combustion reaction: it is a kind of redox response in which any combustible substance combines with an oxidizing factor, normally oxygen, to generate heat and form oxidized products.

Example: C3H8 + 5 O2 ' 3 CO2 + 4 H2O

Different types of chemical reactions embrace natural reactions which are present in natural chemistry.
Organic reactions compose a wide variety of reactions involving compounds which have carbon as the principle factor in their molecular structure. In opposition to inorganic reactions, natural chemistry reactions are categorized in massive part by the types of the functional groups that exist within each compound. In this case the reactions are described by showing the mechanisms through which the modifications take place.

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