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Net Ionic Equations (8-4)

Net Ionic Equations (8-4). Show only the species (atoms/ions) participating in a reaction Single displacement reaction – exchange electrons Double displacement reaction – form new bonds (ionic or covalent) Steps From formula equation write complete ionic equation

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Net Ionic Equations (8-4)

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  1. Net Ionic Equations (8-4) • Show only the species (atoms/ions) participating in a reaction • Single displacement reaction – exchange electrons • Double displacement reaction – form new bonds (ionic or covalent) • Steps • From formula equation write complete ionic equation • use ion symbols for aqueous species • use element, formula symbols for (g), (l), (s) • Cancel spectator ions (ions not forming new bonds)

  2. Can be written for: • Single Displacement Reactions (electron transfer reactions) • One spectator ion • Charges must balance • Double Displacement Reactions (bond forming reactions) • Two spectator ions • Charges on reactants side must sum up to zero

  3. To predict the products of single-replacement reactions. Refer to the activity series (page 281 or appendix A, page 832) • Is the free element above the element to be replaced in the compound? • If yes, the reaction will occur • Is the free element below the element to be replaced in the compound? • If yes, then a reaction will NOT occur The more active an element is, the more likely it will form compounds!

  4. Simple Activity Series of Metals Activity Series of Halogens K Ca Na Mg Al Zn Fe Ni Pb H2 Cu Ag Au F2 Cl2 Br2 I2 Decreasing Reactivity Increasing Reactivity Increasing Reactivity Decreasing Reactivity 

  5. Example – Single DisplacementCheck Activity Series first! Formula Equation: Cu (s) + 2 AgNO3 (aq)  Cu(NO3)2 (aq) + 2 Ag (s)  Complete Ionic Equation: Cu (s) + 2 Ag1+ (aq) + 2 NO31- (aq)  Cu2+ (aq) + 2 NO31- (aq) + 2 Ag (s) Identify Spectator Ion: NO31-is found on both sides of the yields sign and will cancel out. Net Ionic Equation: Cu (s) + 2 Ag1+ (aq)  Cu2+ (aq) + 2 Ag (s) Note that charges balance. There are 2(+) charges on the reactants side and 2(+) charges on the products side.

  6. A Precipitation Reaction must produce a new solid substance. Use solubility rules (p. 284) to decide whether a precipitation will take place: • Reactants are usually all soluble ionic compounds (will dissolve easily in water). • If one of the ions from reactant #1 will form an insoluble compound with an ion from reactant #2, a precipitation reaction will take place. (Insoluble means will not dissolve in water.)

  7. Some Simple Solubility Rules  • All compounds of Group 1 and NH4+ are soluble. • All nitrates are soluble. • All halides, except those of Ag+ and Pb2+, are soluble. • All sulfates, except Ca2+, Sr2+, Ba2+, Hg22+, and Pb2+ are soluble. • All carbonates, except those of Group 1 and NH4+, are insoluble. • Most hydroxides, except those of Group 1 and NH4+, are insoluble.

  8. Example – Double Replacement Formula Equation: AgNO3 (aq) + NaCl (aq)  AgCl + NaNO3 Complete Ionic Equation: Ag1+ (aq) + NO31- (aq) + Na1+ (aq) + Cl1- (aq)  AgCl (s) + Na1+ (aq) + NO31- (aq) Identify Spectator Ions: Na1+ and NO31-are found on both sides of the yields sign and will cancel out. Net Ionic Equation: Ag1+ (aq) + Cl1- (aq)  AgCl (s) Note that charges balance. There is a net zero charge [(1+) + (1-)] on the reactants side and zero charge on the products side. (s) (aq)

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