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Types of Chemical Reactions –Part I

Types of Chemical Reactions –Part I. Mrs. Coyle Chemistry. Types of Chemical Reactions. Composition Decomposition Single Replacement (Displacement) Double Replacement (Displacement) Combustion Oxidation-Reduction. Composition (Combination, Synthesis).

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Types of Chemical Reactions –Part I

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  1. Types of Chemical Reactions –Part I Mrs. Coyle Chemistry

  2. Types of Chemical Reactions • Composition • Decomposition • Single Replacement (Displacement) • Double Replacement (Displacement) • Combustion • Oxidation-Reduction

  3. Composition(Combination, Synthesis) • Two or more substances combine to form a single substance. • General equation: A + B  AB example: 2Na + Cl2  2NaCl http://jchemed.chem.wisc.edu/jcesoft/cca/cca0/Movies/NACL1.html

  4. Decomposition • A compound is broken into two or more products. • General equation: AB  A + B example: 2H2O 2H2 + O2

  5. Single Replacement A + BC AC +B

  6. Activity Series • For an element to replace another the lone element must be more active than the element it is replacing in the substance. • See the reference chart behind your periodic table.

  7. Example: Zn+ 2 HCl ZnCl2 + H2

  8. Example: Thermite Reaction 2 Al + Fe2O3 Al2O3 + 2 Fe

  9. Example: 2NaBr (aq) + Cl2 (g) 2NaCl (aq) + Br2 (g)

  10. Examples: Ca + Al(NO3)3  K + Na2SO4 

  11. Double Replacement(Double Displacement) AB + CD  AD + CB

  12. Double Replacement Reactions • Occur in aqueous solutions • For a DR reaction to occur one of the following must happen: • A precipitate is formed (an insoluble or slightly soluble solid). • A molecular compound (usually water is formed). • A gas is formed.

  13. Example: Production of a PrecipitateSilver Nitrate + Sodium Chloride • Precipitate AgCl (s)

  14. Solubility Rules • See the reference chart behind your periodic table.

  15. Example: Production of H2O H2SO4(aq)+2NaOH(aq)2H2O(l) +Na2 SO4(aq)

  16. 3 Ways to Write Equations Involving Reactions in Solutions • Formula Equation ex: Zn(s) +2HCl(aq) ZnCl2(aq) + H2(g) • Complete Ionic Equation Zn(s) +2H+(aq)+2Cl-(aq)  Zn+2(aq)+ 2Cl -(aq) + H2(g) • Net Ionic Equation Zn(s) +2H+(aq)  Zn+2(aq)+H2(g)

  17. Note: • Spectator ions are ions that do not undergo chemical change during the reaction. • In a net ionic equation the charge and the atoms must balance.

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