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Understanding Single Replacement Reactions in Chemistry

Learn about single replacement reactions where metals and nonmetals replace elements in compounds. Use activity series tables to predict reactivity and occurrence of reactions. Practice with examples and rules to determine reaction outcomes.

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Understanding Single Replacement Reactions in Chemistry

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  1. A word about ….

  2. Single Replacement Reactions A + BX  AX + B Element + Compound  New Element + New Compound

  3. Single Replacement Rxns 2 Li(s) + 2 H2O(l)  2 LiOH(aq) + H2(g) Type #1:metal replaces a hydrogen in water molecule

  4. Single Replacement Rxns Type #2: one metal replaces another metal in a compound Cu(s) + 2 AgNO3(aq)  2 Ag(s) + Cu(NO3)2(aq)

  5. Single Replacement Reactions Metals have different reactivities must predict if given metal and given compound will react or not

  6. Single Replacement Rxns • Table J is an activity series • more reactive a metal is, the easier it loses its valence electrons • most active metal at top • least active metal at bottom • use Table J to determine if reaction will occur

  7. Single Replacement Rxns rule: metal CAN replace any metal listed BELOW itself on table J - CANNOT replace metal listed above itself on table J

  8. Ag(s) + Cu(NO3)2(aq)  ? • What is the metal and the metal cation it wants to replace? Ag and Cu+2 • Locate Ag and Cu on Table J • Ag below Cu so reaction will NOT go • Ag is less reactive than Cu

  9. Cu(s) + 2 AgNO3(aq)  ? • What is the metal and the metal cation? Cu and Ag+1 Locate Cu and Ag in Table J • Cu is above Ag • Cu more reactive than Ag so reaction WILL go  2 Ag(s) + Cu(NO3)2(aq)

  10. Single Replacement Reactions Type #3: nonmetal replaces another nonmetal in compound • Nonmetal often is halogen • Halogens have different reactivities (Table J) • Most active halogen = F (top) • Least active halogen = I (bottom)

  11. This reaction occurs because F2 is above Br2 Single Replacement Reactions rule: more active halogen replaces less active halogen in compound in aqueous solution F2(g) + 2 NaBr(aq)  2 NaF(aq) + Br2(l)

  12. NR Single Replacement Reaction Br2(g) + 2 NaF(aq)  ? Br2 below F2 in Table J - reaction does NOT occur

  13. KCl(aq) + Zn(s) <not balanced> No No AlCl3(aq) + Sn(s) <not balanced> No Ti(NO3)2(aq) + Pb(s) No CaF2(aq) + I2(g) Use Table J to predict if these reactions occur • K(s) + ZnCl2(aq)  • Fe(s) + Na3PO4(aq)  • Cu(s) + Mg(NO3)2(aq)  • Al(s) + SnCl2(aq)  • Ca(s) + KBr(aq)  • Ti(s) + Pb(NO3)2(aq)  • Cl2(g) + HF(aq)  • F2(g) + CaI2(aq) 

  14. Determining if a compound is soluble (aq) or NOT • LOOK AT TABLE F • LiOH • Cu(NO3)2 • AgCl2 • MgS • NaS2 • KOH • aq • aq • insoluble = precipitate = s • insoluble = precipitate = s • aq • aq

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