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Synthesis and Decomposition Reactions

Synthesis and Decomposition Reactions. Synthesis reactions. Synthesis reactions occur when two substances (generally elements ) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product A + B  AB

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Synthesis and Decomposition Reactions

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  1. Synthesis and Decomposition Reactions

  2. Synthesis reactions • Synthesis reactions occur when two substances (generallyelements) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product A + B  AB Example: 2H2 + O2  2H2O Example: C+ O2  CO2

  3. Synthesis Reactions

  4. Practice • Predict the products. Write and balance the following synthesis reaction equations. • Sodium metal reacts with chlorine to form sodium chloride Na(s) + Cl2(g)  • Solid Magnesium reacts with fluorine to form magnesium fluoride Mg(s) + F2(g)  • Aluminum metal reacts with fluorine to form aluminum fluoride Al(s) + F2(g) 

  5. Answers • Sodium metal reacts with chlorine to form sodium chloride 2 Na(s) + Cl2(g)  2 NaCl(s) • Solid Magnesium reacts with fluorine to form magnesium fluoride Mg(s) + F2(g)  MgF2(s) • Aluminum metal reacts with fluorine to form aluminum fluoride 2 Al(s) + 3 F2(g)  2 AlF3(s)

  6. Decomposition Reactions • Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds • 1 Reactant  Product + Product In general: AB  A + B • Example: 2 H2O  2H2 + O2 • Example: 2 HgO  2Hg + O2

  7. Decomposition Reactions

  8. Decomposition Exceptions • Carbonates and chlorates are special case decomposition reactions that do not go to the elements. • Carbonates (CO32-) decompose to carbon dioxide and a metal oxide • Example: CaCO3  CO2 + CaO • Chlorates (ClO3-) decompose to oxygen gas and a metal chloride • Example: 2 Al(ClO3)3  2 AlCl3 + 9 O2

  9. Practice • Predict the products. Then, write and balance the following decomposition reaction equations: • Solid Lead (IV) oxide decomposes PbO2(s)  • Aluminum nitride decomposes AlN(s) 

  10. Answers: • Solid Lead (IV) oxide  lead + oxygen PbO2(s)  Pb(s) + O2(g) • Aluminum nitride  aluminum and nitrogen 2 AlN(s)  2 Al(s) + N2(g)

  11. Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N2(g) + O2(g) BaCO3(s)  (hint: make barium oxide and carbon dioxide) Co(s)+ S(s)  SO3(g) + H2O(l)  (Hint: make sulfuric acid) NI3(s)  Nitrogen monoxide (make Co be +3)

  12. Answers: N2(g) + O2(g) 2 NO(g) BaCO3(s)  BaO(s) + CO2(g) Co(s)+ S(s)  Co2S3(s) SO3(g) + H2O(l)  H2SO4 2 NI3(s)  N2(g) + 3 I2(s)

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