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Monday 4/2/12

This document serves as a comprehensive overview of chemical reactions and their types, including synthesis, combustion, decomposition, single replacement, and double replacement reactions. It emphasizes the importance of balancing chemical equations, showcasing examples such as the reaction of aluminum with copper(II) chloride and various other compounds. Additionally, it provides practice equations to help students enhance their balancing skills. Aimed at chemistry students, this guide is essential for mastering the fundamentals of chemical reactions.

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Monday 4/2/12

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  1. Monday4/2/12 • Get out your chemical reaction notes you have been taking and your balancing equations practice sheet. Try to balance the equations on the back.

  2. C. Balancing Example Al + CuCl2 Cu + AlCl3 Al Cu Cl Aluminum and copper(II) chloride react to form copper and aluminum chloride. 2 3 3 2  2  6 1 1 1 1 2 3 2  3  6   3

  3. __NaNO3 + __PbO __Pb(NO3)2 +__Na2O

  4. __AgI + __Fe2(CO3)3__ FeI3+__Ag2CO3

  5. __C2H4O2+__O2__CO2+__H2O

  6. __ZnSO4+__Li2CO3__ZnCO3+__Li2SO4

  7. __V2O5+__CaS__CaO+__V2S5

  8. __Mn(NO2)2+__BeCl2__Be(NO2)2 +__MnCl2

  9. __AgBr+__GaPO4__Ag3PO4+__GaBr3

  10. __H2SO4+__B(OH)3__B2(SO4)3+__H2O

  11. __S8+__O2__SO2

  12. __Fe+__AgNO3__Fe(NO3)2+__Ag

  13. Wednesday 4/18/12 • 1. Make sure you turned in your rxn rate vocab, 11.2 vocab, & 11.2 Guided reading to class tray. • 2. Get out paper for notes and answer the following question: • What are the different types of reac tions?

  14. Chemical Reactions Types of Chemical Reactions

  15. A. Synthesis • the combination of 2 or more substances to form a compound • only one product A + B  AB

  16. A. Synthesis H2(g) + Cl2(g)  2 HCl(g)

  17. B. Combustion • the burning of any substance in O2 to produce heat A + O2 B CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) EX: Burning of natural gas, wood and gasoline

  18. C. Decomposition • a compound breaks down into 2 or more simpler substances • only one reactant AB  A + B

  19. C. Decomposition 2 H2O(l)  2 H2(g) + O2(g)

  20. D. Single Replacement • one element replaces another in a compound • metal replaces metal (+) • nonmetal replaces nonmetal (-) • Halogens are replaced by a more reactive halogen A + BC  B + AC

  21. D. Single Replacement Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

  22. E. Double Replacement • ions in two compounds “change partners” • cation of one compound combines with anion of the other AB + CD  AD + CB

  23. E. Double Replacement Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)

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