Combination reaction

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A combination reaction (also known as a synthesis reaction) is a reaction where two or more elements or compounds (reactants) combine to form a single compound (product). Such reactions may be represented by equations of the following form: X + Y -> XY. The combination of two or more elements and form one compound is called combination reaction. Combination reactions can involve different types of reactants:

There is no specific number of reactants in a combination reaction.

Combination reactions are usually exothermic because when the bond forms between the reactants, heat is released. For example, barium metal and fluorine gas will combine in a highly exothermic reaction to form the salt barium fluoride:

                                Ba + F2 -> BaF2  

Another example is magnesium oxide combining with carbon dioxide to produce magnesium carbonate.

                                MgO + CO2 -> MgCO3  

Another example is iron combining with sulphur to produce iron(II) sulfide.

                                Fe + S -> FeS  

When a combination reaction occurs between a metal and a non-metal the product is an ionic solid. An example could be lithium reacting with sulphur to give lithium sulphide. When magnesium burns in air, the atoms of the metal combine with the gas oxygen to produce magnesium oxide. This specific combination reaction produces the bright flame generated by flares.

Combination reactions can also occur in other situations when the two products do not have the same ionic charge. In such a situation, different quantities of each reactant must be used. To denote this in a chemical equation, a coefficient is added to one or more of the reactants so that the total ionic charge of each reactant is the same. For example, Iron (III) Oxide is formed by the following equation: ${\displaystyle {\ce {4 Fe + 3 O2 -> 2Fe2O3}}}$. This is because in this case, Iron has a charge of 3+ while each Oxygen atom in ${\displaystyle {\ce {O2}}}$ has a charge of 2-. Oxygen Gas (${\displaystyle {\ce {O2}}}$) must be used instead of elemental oxygen (${\displaystyle {{\ce {O}}}}$) because elemental oxygen is a free radical that is unstable and combines with other oxygen atoms to form ${\displaystyle {\ce {O2}}}$.

Another example example: ${\displaystyle {\ce {2 H2 + O2 -> 2H2O}}}$. In this case, two ${\displaystyle {\ce {H2}}}$ molecules must be used elemental oxygen (${\displaystyle {{\ce {O}}}}$) is an unstable radical not commonly found in nature; the equation ${\displaystyle {\ce {H2 + O -> H2O}}}$ is generally impossible under natural conditions. Likewise, the Hydrogen atoms should be in the form ${\displaystyle {\ce {H2}}}$ because ${\displaystyle {\ce {H}}}$ is an unstable free radical not commonly found in nature; the chemical equation ${\displaystyle {\ce {2H + O -> H2O}}}$ is also generally impossible under natural conditions.

Source of the article : Wikipedia