The two types of chemical reactions—double displacement and double decomposition—are fundamentally different from one another because one or more of the reactants in the former do not dissolve in the latter’s solvent. Double displacement reactions are chemical reactions in which the components of two reactants replace one another.
The same type of chemical reactions are explained by both “double displacement” and “double decomposition” reactions, but “double decomposition” is a much older term. As a result, the new term “double displacement” has largely replaced the earlier one because it better captures the reaction’s fundamental idea of a displacement. Additionally, when one or more reactants do not dissolve in the solvent, we used the earlier term.
Chemical reactions known as “double displacement reactions” occur when the components of two reactants swap places to create new products. The cation and anions typically go through this displacement in these reactions. Typically, the end product of these reactions is a precipitate. Therefore, the end product is entirely different from the reactants.
The A and C components of each reactant have been switched around in the equation above. Generally, these reactions occur in aqueous solutions. Furthermore, we can categorize these reactions as follows;.
One or more of the reactants in a double decomposition reaction are insoluble in the solvent, which is a type of double displacement reaction. However, this phrase is frequently used as an alternative to double displacement reactions. For instance, zinc sulfide and hydrochloric acid react to produce zinc chloride and hydrogen sulfide gas. There, the aqueous medium’s undissolved solid zinc sulfide is present.
Q. What is the difference between single displacement reaction and double displacement reaction?
When one reactant is partially replaced by another, the reaction is referred to as a displacement reaction. Replacement or metathesis reactions are other names for displacement reactions. Displacement reactions are divided into two categories:
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Single displacement reaction |
Double displacement reaction |
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1. A single displacement reaction is a chemical reaction in a more reactive element that replaces a less reactive element. |
1. A double displacement reaction is a chemical reaction in which two ionic species are exchanged between two molecules. |
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2. In single displacement reactions, a reactive species that can replace a functional group is required |
2. In double displacement reactions, exchangeable ions are required. |
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3. General Formula: A-B+C→A+B-C |
3. General Formula: A-B+C-D→A-C+B-D |
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4. The reactivity series can be used to anticipate the outcome of a displacement reaction since the chemical components at the top of the series can replace the chemical elements at the bottom. |
4. It could be ionic or covalent bonds that break and form during this reaction. |
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5. No precipitate formed as a result of the colour change. |
5. Precipitate is formed, hence one of the examples of displacement reaction is precipitation reaction. |
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6. Metals react with another metal’s salt solution. |
6. Two different metal salt solutions react with each other. |
What is the Difference Between Double Displacement and Double Decomposition Reaction?
Chemical reactions known as “double displacement reactions” occur when the components of two reactants swap places to create new products. We refer to double displacement reactions by their previous name, double decomposition reactions. Nevertheless, we refer to displacement reactions involving one or more reactants that are insoluble in the solvent by this term. The distinction between double displacement and double decomposition reaction is presented in tabular form in the infographic below.
Example of single displacement reaction:
The reaction of zinc metal with hydrochloric acid to produce zinc chloride and hydrogen gas is an illustration of a single displacement reaction:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)
Because zinc has a higher reactivity than hydrogen in this instance, there was only one displacement of hydrogen.