Author
Home > Science > What is the Difference Between Synthesis Reaction and Substitution Reaction?

Guilherme Mazui

•4 minutes to read

What is the Difference Between Synthesis Reaction and Substitution Reaction?

🆚 Go to Comparative Table 🆚

The main difference between a synthesis reaction and a substitution reaction lies in the process and the resulting products.

Synthesis Reaction:

  • A synthesis reaction occurs when two or more elements or compounds combine to form a new compound.
  • The general equation for a synthesis reaction is: $$\ce{A + B -> C}$$, where A and B are the reactants, and C is the product.
  • The reactants in these reactions are either chemical elements or molecules, and the final product is always a compound or a complex.
  • An example of a synthesis reaction is the combination of hydrogen gas and oxygen gas to form water: $$\ce{2H2 + O2 -> 2H2O}$$.

Substitution Reaction:

  • A substitution reaction takes place when an element or radical (more reactive) replaces another element in a compound.
  • The general equation for a substitution reaction is: $$\ce{A + BC -> B + AC}$$, where A is the element or radical that replaces the element in compound B.
  • This type of reaction produces a new compound and a new element.
  • An example of a substitution reaction is the reaction between magnesium and copper(II) sulfate, resulting in the formation of magnesium sulfate and copper: $$\ce{Mg + CuSO4 -> Cu + MgSO4}$$.

In summary, a synthesis reaction involves the combination of two or more elements or compounds to form a new compound, while a substitution reaction occurs when an element or radical replaces another element in a compound, producing a new compound and a new element.

On this page
  • What is the Difference Between Synthesis Reaction and Substitution Reaction?
  • Comparative Table: Synthesis Reaction vs Substitution Reaction

    • Comparative Table: Synthesis Reaction vs Substitution Reaction

    Here is a table comparing synthesis reactions and substitution reactions:

    Feature Synthesis Reaction Substitution Reaction
    Definition A chemical reaction in which two or more elements or compounds combine to form a new compound or complex. A chemical reaction where an element or radical (more reactive) replaces another element in a compound.
    General Form $$\ce{A} + \ce{B} \rightarrow \ce{AB}$$. $$\ce{A} + \ce{BC} \rightarrow \ce{B} + \ce{AC}$$.
    Example The combination of hydrogen gas and oxygen gas to form water molecules: $$\ce{2H2 + O2 \rightarrow 2H2O}$$. The replacement of hydrogen in water by a more reactive element, such as sodium: $$\ce{2Na + 2H2O \rightarrow 2NaOH + H2}$$.
    Energy Change Synthesis reactions are exothermic, meaning they release energy during bond formation. Substitution reactions may be exothermic or endothermic, depending on the specific reaction and the reactivity of the substituent.
    Reactants Synthesis reactions involve chemical elements or molecules. Substitution reactions involve an element or radical (more reactive) reacting with a compound.
    Products Synthesis reactions always produce a compound or complex as the final product. Substitution reactions may produce a new compound or a molecule with a substituted atom or group.
    Read more:

    Guilherme Mazui

    Guilherme Mazui is graduated in journalism from the Federal University of Minas Gerais (UFMG) and a master's degree in Communication from the University of São Paulo (USP). In addition, he has experience in advertising writing and has worked as a content editor in several companies.