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Reactions

Reactions. Part 2: Net Ionic Equations. Homework Review. #1 Which of the following will dissociate in water?. AgNO 3 Yes, Rule #1 NaOH Yes, Rule #2 and Rule #5 PbSO 4 No, Rule #4. #1 Which of the following will dissociate in water?. CaS No, Rule #6 LiCl Yes, Rule #3 Ba(OH) 2

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  1. Reactions Part 2: Net Ionic Equations

  2. Homework Review

  3. #1 Which of the following will dissociate in water? AgNO3 Yes, Rule #1 NaOH Yes, Rule #2 and Rule #5 PbSO4 No, Rule #4

  4. #1 Which of the following will dissociate in water? CaS No, Rule #6 LiCl Yes, Rule #3 Ba(OH)2 Yes, Rule #5

  5. #1 Which of the following will dissociate in water? BaCl2 Yes, Rule #3 KOH Yes, Rule #2 and Rule #5 Li3PO4 No, Rule #6 CaCO3 No, Rule #6

  6. #2. What is the precipitate formed? BaCl2(aq) + Na2SO4(aq) ?? BaCl2(aq) + Na2SO4(aq) 2Na+(aq) + 2Cl-(aq) + BaSO4(s) BaSO4 is the precipitate.

  7. Trick to guessing products BaCl2(aq) + Na2SO4(aq) ?? Swap the positive ions. (Double Displacement Reaction) • 2 NaCl + BaSO4 Check if products are soluble. If one is not, it is a precipitate.

  8. Key to Chemistry Alert

  9. There is more than one way to write an equation. NaCl(aq) + AgNO3(aq)  NaNO3(aq) + AgCl(s) Complete Molecular Equation uses the complete formulas of all reactants and products. Na+(aq) + Cl-(aq) + Ag+(aq) + NO3- (aq)  Na+(aq) + NO3- (aq) + AgCl(S) Complete Ionic Equation uses ions for all strong electrolytes and formulas for compounds that do not dissociate.

  10. Spectators Na+(aq) + Cl-(aq) + Ag+(aq) + NO3- (aq)  Na+(aq) + NO3- (aq) + AgCl(S) When an ion is an ion on both sides of the complete ionic equation, it is called a spectator ion. Na+(aq)and NO3-(aq) are on both sides and are therefore “spectators.”

  11. Net Ionic Equation To write a net ionic equation, start with the complete ionic equation. Na+(aq) + Cl-(aq) + Ag+(aq) + NO3- (aq)  Na+(aq) + NO3-(aq) + AgCl(S) Remove the spectator ions. Na+(aq) + Cl-(aq) + Ag+(aq) + NO3(aq) Na+(aq) + NO3-(aq) +AgCl(S) What remains is referred to as the Net Ionic Equation. Cl-(aq) + Ag+(aq)  AgCl(S)

  12. Example 2 Molecular Equation: K2CrO4(aq) + Ba(NO3)2(aq)  BaCrO4(s) + 2KNO3(aq) Complete Ionic Equation: 2K+(aq) + CrO4-2(aq) + Ba+2(aq) + 2NO3-(aq)  BaCrO4(s) + 2K+(aq) + 2NO3-(aq) Net Ionic Equation: Spectators are K+ and NO3-. CrO4-2(aq) + Ba+2(aq)  BaCrO4(s)

  13. Classwork (due tomorrow) Write molecular, complete ionic, and net ionic equations for the reactions of: AgNO3 and KCl CaCl2 and Na2CO3 PbCl2 and Ba(OH)2 Review Tomorrow Test is Wednesday

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