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Types of Reactions

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Synthesis

  • 2 reactants form 1 product
  • 2 🡪 1
  • 2H2(g) + O2(g) 🡪 2H2O(g)

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Decomposition

  • 1 reactant forms 2 products
  • 1 🡪 2
  • 2Ag2O(s) 🡪 4Ag(s) + O2(g)

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Single Replacement

  • 1 element switches places with another

(has a single element on each side)

  • Mr. Steal Your Girl
  • Zn(s) + H2SO4(aq) 🡪 ZnSO4(aq) + H2(g)

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Double Replacement

  • two compounds react, the positive ions and the negative ions of the two reactants switch places, forming two new compounds or products. All reactants and products are compounds.

  • HOCO, more than one big letter in all reactants and products

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  • BaCl​2​​(aq) + Na​2SO​4​​(aq) → BaSO​4​​(s) + 2NaCl(aq)

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Combustion

  • reaction with O2 to form heat, CO2 and H­2O
  • CO2 and H2O in products
  • CH4(g) + 2O2(g) 🡪 2H2O(g) + CO2(g)

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Neutralization

  • an acid and a base are placed together, and react to, producing a salt. The H+ of the acid combines with the OH- of the base to form water.

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  • H____ and ____OH in reactants
  • HCl(aq) + NaOH(aq) 🡪 H2O(l) + NaCl(aq)

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Precipitation

  • two aqueous solutions react to form an insoluble solid, called a precipitate

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  • Look at solubility chart. If a substance involved is not soluble, the reaction will form a precipitate.

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  • LiBr (aq) + AgNO3 (aq) 🡪 LiNO3 (aq) + AgBr (s)

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