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Types of Chemical Reactions

Learn about addition or synthesis, decomposition, single replacement, double replacement, and combustion reactions. Explore patterns, energy release, and phase designations in reactions. Get ready for lab work and worksheet practice.

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Types of Chemical Reactions

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  1. Types of Chemical Reactions

  2. Addition or Synthesis Reactions • The formation of a compound from elements or simpler compounds • Follows the pattern A + B → AB • 2H2 + O2 → 2H2O • Accompanied by a release of energy • 2H2 + O2 → 2H2O + energy

  3. Decomposition Reactions • Opposite of synthesis reactions • Pattern: AB → A + B • 2H2O → 2H2 + O2 • Usually requires input of energy to proceed • 2H2O + energy → 2H2 + O2

  4. Single Replacement Reactions • Involves the “switching” of one component of a compound with another single element • Pattern: A + BC →AC + B • Zn + 2HCl → ZnCl2 + H2 • Energy is released • Zn + 2HCl → ZnCl2 + H2 + energy

  5. Double Replacement Reactions • Involves the “switching” of components of two compounds involved in a reaction. • Pattern: AB + CD → CB + AD • HCl + NaOH → NaCl + HOH (aka H2O) • Energy is usually released in these reactions • HCl + NaOH → NaCl + HOH (aka H2O) + energy

  6. Combustion Reactions • Involves the burning or rapid oxidation of compounds with oxygen • CH4 + 2O2 → CO2 + 2H2O • Look for the O2 on the reactant side • Look for CO2 and H2O on product side

  7. Phase designations • Use the following designations to indicate state or phase of each reactant and product • (g) = gas • (l) = liquid • (s) = solid • (aq) = aqueous solution (used in ionic equations)

  8. Assignment • Worksheet on equations • Prepare for Types of Reactions Lab

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