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Understanding Chemical Reaction Types: Synthesis, Decomposition, Replacement, and Combustion

This guide explores the four primary types of chemical reactions: synthesis, decomposition, single replacement, and double replacement. Synthesis involves two or more reactants combining to form a complex product, while decomposition reactions occur when compounds break down into simpler substances. In single replacement reactions, a more reactive element displaces a less reactive one, and double replacement reactions feature the exchange of ion partners, often resulting in gas or precipitate formation. Learn the fundamentals with example reactions for each type.

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Understanding Chemical Reaction Types: Synthesis, Decomposition, Replacement, and Combustion

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  1. Reaction Types

  2. Synthesis Synthesis reactions involve 2 or more reactants combining to form a more complex product. 2Mg(s) + O2(g) → 2MgO(s)

  3. Decomposition Decomposition reactions occur when complex reactants divide and form into simpler products. 2H2O2(l) → O2(g) + 2H2O (l)

  4. Single Replacement One more reactive element replaces a less reactive ion in solution. Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)

  5. Double Replacement Two compounds exchange ion partners. Usually evidenced by gas or precipitate formation. Pb(NO3)2(aq) + 2KI(aq) → 2KNO3 (aq) + PbI2(s)

  6. Combustion When one substance burns to combine with oxygen. Organic compounds often produce CO2 and H2O. 2C3H8O(g) + 9O2(g)→ 6CO2(g) + 8H2O(g)

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