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Typical of inorganic chemical reactions

There is no universally accepted list of the typical, important inorganic reactions. Although there are numerous available sources (books, journal and Internet websites) that include such lists, they all differ to some extent from each other. The inorganic reaction types listed and explained below were drawn from many of the available sources:

Synthesis reaction: (also referred to as combination or composition reaction)

This is a reaction in which two or more reactants combine to form a single product, where each reactant is a chemical element or compound and the reaction product consist of the two reactants. Examples include:

• sodium + chlorine → sodium chloride

2Na + Cl ₂ → 2NaCl

• carbon dioxide + water → carbonic acid

CO₂ + H₂O → H₂CO₃

• hydrogen + sulfur → hydrogen sulfide

2H₂ + S → H₂S

Decomposition reaction: (may be thermal, electrolytic or catalytic decomposition reaction)

This is a reaction in which a chemical compound is separated into elements or simpler compounds. It is often defined as the exact opposite of a synthesis reaction. Examples include:

• hydrogen peroxide → water + oxygen

2H₂O₂ → 2H₂O + O₂

• calcium carbonate → calcium oxide + carbon dioxide

CaCO₃ → CaO + CO₂

Single displacement reaction: (also referred to as substitution or single replacement reaction)

This is a reaction characterized by one element being displaced from a compound by another element. Examples include:

• zinc + hydrochloric acid → zinc chloride + hydrogen

Zn + 2HCl → ZnCl₂ + H₂

• copper +silver nitrate → silver + copper nitrate

Cu + 2AgNO₃ → 2Ag + Cu(NO₃)₂

Double replacement reaction: (also referred to as metathesis or exchange reaction)

Acid-base reaction: (also referred to as neutralization)

Redox reaction: (also referred to as oxidation-reduction reaction)

Precipitation reaction: (also referred to as aqueous metathesis reaction)