Types of Chemical Reactions

Types of Chemical Reactions

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 often characterized by the type of chemical change, and it yields one or more products which are, basically, different from the reactants.

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

Chemical adjustments are a results of chemical reactions. All chemical reactions involve 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 helpful to classify them into completely different types together with the widely used phrases for describing frequent reactions.

Mixture reaction or synthesis response: it is a reaction in which 2 or more chemical components or compounds unite to form a more complicated 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 reaction or evaluation: 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 a component being displaced out of a compound by a more reactive element.

Instance: 2 Na(s) + 2 HCl(aq) ‘ 2 NaCl(aq) + H2(g)

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

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

Acid-base reactions: broadly these reactions are characterised as reactions between an acid and a base, can have completely different definitions relying 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.

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 changes in oxidation numbers of atoms in involved species occur. Those reactions can often be interpreted as switch of electrons between completely different molecular sites or species.

Instance: 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 flamable substance combines with an oxidizing ingredient, normally oxygen, to generate heat and form oxidized products.

Instance: C3H8 + 5 O2 ‘ 3 CO2 + four H2O

Other types of chemical reactions include natural reactions which are present in natural chemistry.

Natural reactions compose a wide variety of reactions involving compounds which have carbon as the primary component in their molecular structure. In opposition to inorganic reactions, natural chemistry reactions are labeled in massive part by the types of the functional groups that exist within every compound. In this case the reactions are described by showing the mechanisms by means of which the changes take place.

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